Cambridge IGCSE™
*6193842897*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
February/March 2020
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working and use appropriate units.
INFORMATION
●● The total mark for this paper is 40.
●● The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Blank pages are indicated.
IB20 03_0620_62/2RP
© UCLES 2020
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2
1The table gives the boiling points of four alcohols.
alcohol
boiling point / °C
methanol
65
ethanol
79
propan-1-ol
97
butan-1-ol
117
The apparatus shown can be used to separate a mixture of the four alcohols shown in the table.
A
condenser
B
mixture
of alcohols
alcohol collected
heat
(a)Name the apparatus labelled A and B.
A .................................................................................................................................................
B .................................................................................................................................................
[2]
(b)Add to the diagram one arrow to show where water enters the condenser.
[1]
(c) (i)Why is it not safe to heat the mixture of alcohols with a Bunsen burner?
........................................................................................................................................ [1]
(ii)Suggest how the mixture of alcohols can be heated safely?
........................................................................................................................................ [1]
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3
(d)Describe how the condenser allows the alcohol to be collected as a liquid.
.....................................................................................................................................................
............................................................................................................................................... [1]
(e) Which alcohol would be collected first?
Explain your answer.
alcohol collected first ..................................................................................................................
explanation .................................................................................................................................
.....................................................................................................................................................
[2]
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BLANK PAGE
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2A student investigated the time taken to collect 40 cm3 of hydrogen gas when magnesium reacts
with dilute sulfuric acid.
Five experiments were done using the apparatus shown.
inverted 50 cm3
measuring cylinder
dilute sulfuric acid
and distilled water
water
Experiment 1
●● Using a measuring cylinder, 8 cm3 of dilute sulfuric acid was poured into the boiling tube.
●● Using a second measuring cylinder, 12 cm3 of distilled water was added to the acid in the
boiling tube.
●● The apparatus was set up as shown in the diagram, ensuring the inverted measuring cylinder
was full of water.
●● The bung was removed from the boiling tube.
●● A coiled length of magnesium ribbon was added to the boiling tube, the bung was immediately
replaced and a timer started.
●● The time taken for 40 cm3 of gas to be collected was measured.
●● The student felt the outside of the boiling tube.
(a) (i)The student noticed that the boiling tube was warm.
What does this tell you about the type of reaction?
........................................................................................................................................ [1]
(ii)Describe one change that could be made to the apparatus to help keep the temperature
of the contents of the boiling tube constant during the reaction.
........................................................................................................................................ [1]
Experiment 2
●● The boiling tube was rinsed out with distilled water.
●● Experiment 1 was repeated using 10 cm3 of dilute sulfuric acid and 10 cm3 of distilled water.
Experiment 3
●● Experiment 2 was repeated using 12 cm3 of dilute sulfuric acid and 8 cm3 of distilled water.
Experiment 4
●● Experiment 2 was repeated using 16 cm3 of dilute sulfuric acid and 4 cm3 of distilled water.
Experiment 5
●● Experiment 2 was repeated using 20 cm3 of dilute sulfuric acid and no distilled water.
© UCLES 2020
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6
(b)Use the information in the description of the experiments and the timer diagrams to complete
the table. Record the time in seconds.
experiment
volume of
dilute sulfuric
acid / cm3
volume of
distilled water
/ cm3
0
seconds
0
1
8
time to collect
40 cm3 of gas / s
timer diagram
45 15
5
10
15
minutes
30
0
0
2
10
45 15
5
15
5
15
5
15
5
15
10
30
0
0
3
12
45 15
10
30
0
0
4
16
45 15
10
30
0
0
5
20
45 15
10
30
[4]
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7
(c)Add a suitable scale to the y-axis and plot the results from Experiments 1 to 5 on the grid.
Draw a smooth line graph.
time to collect
40 cm3 of gas / s
6
8
10
12
14
16
18
20
volume of dilute sulfuric acid / cm
3
[4]
(d) (i)
From your graph, deduce the time taken to collect 40 cm3 of gas if the experiment was
repeated using 9 cm3 of dilute sulfuric acid.
Show clearly on the grid how you worked out your answer.
.............................. s
[2]
(ii)
What volume of distilled water would be needed if the experiment was repeated
using 9 cm3 of dilute sulfuric acid?
.............................. cm3 [1]
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(e)The rate of reaction can be calculated using the equation shown.
rate of reaction =
volume of gas collected
time taken to collect the gas
(i)Use this equation to calculate the rate of reaction in Experiment 1. Give the units for the
rate of reaction you have calculated.
rate of reaction = .............................. units = ..............................
[2]
(ii)In which Experiment, 1, 2, 3, 4 or 5, was the rate of reaction greatest?
........................................................................................................................................ [1]
(f)Why would measuring the volume of dilute sulfuric acid with a burette rather than a measuring
cylinder be an improvement?
.....................................................................................................................................................
............................................................................................................................................... [1]
(g)The magnesium starts to react with the dilute sulfuric acid as soon as it is added.
(i)Why does this decrease the accuracy of the investigation?
........................................................................................................................................ [1]
(ii)Describe one improvement that you could make to overcome this problem.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [1]
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9
3Solution J and solid K were analysed.
tests on solution J
tests
observations
Solution J was colourless. Solution J was
divided into three portions in three test‑tubes.
test 1
Universal indicator paper was dipped into the
first portion of solution J.
test 2
the universal indicator paper turned red
A spatula measure of sodium carbonate was
added to the second portion of solution J. The
gas given off was tested.
test 3
effervescence was seen, the gas produced
turned limewater milky
1 cm3 of dilute nitric acid and a few drops of
aqueous silver nitrate were added to the third
portion of solution J.
a white precipitate formed
(a)Use the observation from test 1 to suggest the pH of solution J.
pH = .............................. [1]
(b)Name the gas given off in test 2.
............................................................................................................................................... [1]
(c)Identify solution J.
.....................................................................................................................................................
............................................................................................................................................... [2]
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tests on solid K
Solid K was ammonium nitrate.
Complete the expected observations.
Solid K was dissolved in water to produce solution K. Solution K was divided into two equal portions.
(d)About 1 cm3 of dilute nitric acid and a few drops of aqueous barium nitrate were added to the
first portion of solution K.
observations ......................................................................................................................... [1]
(e)2 cm3 of aqueous sodium hydroxide was added to the second portion of solution K. The mixture
was warmed and the gas given off was tested.
observations ...............................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
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4A black dye can be obtained from some plant roots.
Plan an investigation to determine how many different coloured substances are contained in a
black dye obtained from plant roots.
You must include how the results you obtain will tell you how many different coloured substances
are contained in the black dye.
You have access to plant roots and all normal laboratory apparatus.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
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BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/62/F/M/20
Cambridge IGCSE™
*1792185691*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
February/March 2020
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working and use appropriate units.
INFORMATION
●● The total mark for this paper is 80.
●● The number of marks for each question or part question is shown in brackets [ ].
●● The Periodic Table is printed in the question paper.
This document has 12 pages. Blank pages are indicated.
IB20 03_0620_42/2RP
© UCLES 2020
[Turn over
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1Petroleum is a useful natural resource.
The diagram shows how petroleum can be separated into useful substances.
refinery gas
gasoline fraction
A
kerosene fraction
diesel oil
fuel oil fraction
lubricating oil fraction
petroleum
B
(a)What is the name of the separation process shown in the diagram?
............................................................................................................................................... [2]
(b)Name the fraction leaving at:
A .................................................................................................................................................
B .................................................................................................................................................
[2]
(c) Refinery gas is a mixture of hydrocarbons.
One refinery gas is butane, C4H10.
(i)Suggest the names of two other refinery gases.
............................................................... and ............................................................... [2]
(ii)Write the chemical equation for the complete combustion of butane.
........................................................................................................................................ [2]
(iii)
Name the toxic gas produced by the incomplete combustion of butane.
........................................................................................................................................ [1]
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3
(d) Gasoline and kerosene are both fuels. They have different properties.
(i)Describe the differences in the properties given.
viscosity of the fuel ..............................................................................................................
..............................................................................................................................................
flammability of the fuel .........................................................................................................
..............................................................................................................................................
[2]
(ii)What difference in the molecules of gasoline and kerosene causes these differences in
properties?
........................................................................................................................................ [1]
(e) Hydrogen fuel cells can be used to power vehicles.
Write the word equation for the overall reaction that takes place in a hydrogen fuel cell.
............................................................................................................................................... [1]
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[Total: 13]
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2
luminium is extracted from its ore. The ore is converted into pure aluminium oxide, which then
A
undergoes electrolysis as shown.
+ power –
supply
anodes
+
+
electrolyte
wires
cathode
molten aluminium
(a) (i)Name an ore of aluminium.
........................................................................................................................................ [1]
(ii)
What is meant by the term electrolysis?
..............................................................................................................................................
........................................................................................................................................ [2]
(b) Aluminium oxide has a melting point of about 2000 °C, but the electrolysis process operates at
about 900 °C.
(i)
Name the compound added to aluminium oxide to reduce the operating temperature.
........................................................................................................................................ [1]
(ii)Suggest one benefit to the environment of reducing the operating temperature.
..............................................................................................................................................
........................................................................................................................................ [1]
(iii)Write the ionic half-equation for the reaction taking place at:
the negative electrode (cathode) .........................................................................................
the positive electrode (anode) .............................................................................................
[4]
(iv)
Explain why the anodes need frequent replacement.
..............................................................................................................................................
......................................................................................................................................... [2]
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5
(c) Aluminium oxide reacts with acids and with alkalis.
(i)
What term is used to describe an oxide that reacts with acids and with alkalis?
........................................................................................................................................ [1]
(ii)
Aluminium oxide reacts with dilute sulfuric acid to form a salt.
State the name and write the formula of the salt formed.
name ....................................................................................................................................
formula .................................................................................................................................
[2]
(iii)
Aluminium oxide reacts with dilute sodium hydroxide to form a salt and one other product.
Name the other product.
........................................................................................................................................ [1]
(iv)
luminium hydroxide, Al (OH)3, decomposes when heated to form aluminium oxide and
A
water.
Write the chemical equation for this reaction.
........................................................................................................................................ [2]
(v)Suggest the names of two other aluminium compounds that decompose when heated to
form aluminium oxide.
..............................................................................................................................................
........................................................................................................................................ [2]
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3
The Periodic Table is a method of classifying elements.
(a) Identify the element which is in Group VI and Period 4.
............................................................................................................................................... [1]
(b) Calcium is in Group II and chlorine is in Group VII of the Periodic Table.
xplain, in terms of number of outer shell electrons and electron transfer, how calcium atoms
E
and chlorine atoms form ions. Give the formulae of the ions formed.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [5]
(c) G
roup V chlorides are covalent molecules. The boiling points of some Group V chlorides are
shown.
chloride
boiling point / °C
NCl 3
71
PCl 3
(i)
AsCl 3
130
SbCl 3
283
Suggest the approximate boiling point of PCl 3.
........................................................................................................................................ [1]
(ii)
Explain the trend in boiling points in terms of attractive forces between particles.
..............................................................................................................................................
........................................................................................................................................ [2]
© UCLES 2020
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7
(iii)
omplete the dot-and-cross diagram to show the electron arrangement in a molecule of
C
PCl 3.
Show outer electrons only.
Cl
Cl
P
Cl
[3]
(d) PCl 3 reacts with chlorine, Cl 2, to form PCl 5. This reaction is exothermic and reaches an
equilibrium.
PCl 3(g) + Cl 2(g)
PCl 5(g)
(i)Describe two features of an equilibrium.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)
tate the effect, if any, on the position of this equilibrium when the following changes are
S
made.
Explain your answers.
temperature is increased .....................................................................................................
..............................................................................................................................................
pressure is increased ..........................................................................................................
..............................................................................................................................................
[4]
(iii)
Explain, in terms of particles, what happens to the rate of the forward reaction when the
reaction mixture is heated.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
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(e) PCl 5 reacts with lithium fluoride, LiF, to form LiPF6.
PCl 5 + 6LiF → LiPF6 + 5LiCl
Calculate the mass of LiF needed to form 3.04 g of LiPF6 using the following steps.
●● Calculate the number of moles of LiPF6 formed.
[Mr: LiPF6, 152]
number of moles = ..............................
●●
Deduce the number of moles of LiF needed.
number of moles = ..............................
●●
Calculate the mass of LiF needed.
mass = .............................. g
[3]
(f) Lithium fluoride has ionic bonding.
(i)What is an ionic bond?
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Give two physical properties of ionic compounds.
..............................................................................................................................................
........................................................................................................................................ [2]
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9
4
Iron is a typical transition element.
Iron:
●● acts as a catalyst
●● forms coloured compounds
●● has more than one oxidation state.
(a)Name one major industrial process that uses iron as a catalyst and name the product made in
this process.
process .......................................................................................................................................
product made ..............................................................................................................................
[2]
(b) When aqueous sodium hydroxide is added to aqueous iron(II) sulfate, a precipitate forms.
(i)What colour is this precipitate?
........................................................................................................................................ [1]
(ii)
Write the ionic equation for this reaction. Include state symbols.
........................................................................................................................................ [3]
(c)Iron(II) sulfate can be converted to iron(III) sulfate by potassium manganate(VII) at room
temperature.
(i)What is the role of potassium manganate(VII) in this reaction?
........................................................................................................................................ [1]
(ii)What condition must be used for this reaction to occur?
........................................................................................................................................ [1]
(iii)
In terms of electron transfer, what happens to the iron(II) ions in this reaction?
........................................................................................................................................ [1]
(iv)State the colour change seen during this reaction.
from purple to ................................................................................................................ [1]
(d)Deduce the charge on the iron ion in each of these compounds.
FeF3 ............................................................................................................................................
Fe(NO3)3 .....................................................................................................................................
[2]
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5
There are two types of polymers.
(a) Addition polymers are made from many identical small units.
(i)What is the term used to describe these small units?
........................................................................................................................................ [1]
(ii)
A section of an addition polymer is shown.
H
CH3 H
CH3 H
CH3
C
C
C
C
H
CH3 H
C
C
CH3 H
CH3
Draw the structure of the small unit used to make this addition polymer.
Show all of the atoms and all of the bonds.
[2]
(b) Polyamides are condensation polymers.
What does the term condensation mean when used to describe this type of polymer?
............................................................................................................................................... [1]
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(c) A polyamide can be made from two different molecules.
A simplified structure of octanedioic acid is shown.
H
O
O
O
C
C
O
H
A simplified structure of 1,6-diaminohexane is shown.
(i)
H
H
N
N
H
H
omplete the diagram to show a section of polyamide manufactured from octanedioic acid
C
and 1,6-diaminohexane. Include all of the atoms and all of the bonds in the linkages.
[3]
(ii)
State the name of a synthetic polyamide.
........................................................................................................................................ [1]
[Total: 8]
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/42/F/M/20
© UCLES 2020
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/F/M/20
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
12
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
February/March 2020
45 minutes
You must answer on the multiple choice answer sheet.
*0772987719*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
• There are forty questions on this paper. Answer all questions.
• For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
• Follow the instructions on the multiple choice answer sheet.
• Write in soft pencil.
• Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
• Do not use correction fluid.
• Do not write on any bar codes.
• You may use a calculator.
INFORMATION
• The total mark for this paper is 40.
• Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
• Any rough working should be done on this question paper.
• The Periodic Table is printed in the question paper.
This document has 16 pages. Blank pages are indicated.
IB20 03_0620_22/5RP
© UCLES 2020
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2
1
The formula of methane is CH4 and the formula of ethane is C2H6.
Which row describes diffusion and the relative rates of diffusion of methane and ethane?
2
3
description of diffusion
relative rate of diffusion
A
particles move from
a high concentration
to a low concentration
ethane diffuses more
quickly than methane
B
particles move from
a high concentration
to a low concentration
methane diffuses more
quickly than ethane
C
particles move from
a low concentration
to a high concentration
ethane diffuses more
quickly than methane
D
particles move from
a low concentration
to a high concentration
methane diffuses more
quickly than ethane
Which test is used to show that a sample of water is pure?
A
Evaporate the water to see if any solids remain.
B
Heat the water to check its boiling point.
C
Test with anhydrous cobalt(II) chloride.
D
Use universal indicator paper to check its pH.
Chromatography is used to separate and identify the components in both coloured and colourless
mixtures.
For colourless mixtures the chromatogram has to be treated with another chemical.
What is the name of this type of chemical?
A
colouring agent
B
display agent
C
finding agent
D
locating agent
© UCLES 2020
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3
4
Lithium reacts with fluorine to form the compound lithium fluoride.
Which statement about this reaction is correct?
5
A
Each fluorine atom gains one electron.
B
Each fluorine atom gains two or more electrons.
C
Each fluorine atom loses one electron.
D
Each fluorine atom loses two or more electrons.
14
12
6 C and 6 C are isotopes of carbon.
Which statement about these isotopes is correct?
6
A
12
14
6 C is more reactive than 6 C because the atoms have less mass.
B
12
14
6 C is more reactive than 6 C because the atoms have different numbers of neutrons.
C
The reactions of 126 C are similar to 146 C because they have the same number of outer shell
electrons.
D
The reactions of 126 C are similar to 146 C because they have the same number of protons in
the nucleus.
The molecular structure of hydrazine, N2H4, is shown.
H
H
N
H
N
H
Which description of the bonding in hydrazine is not correct?
A
Each nitrogen atom has a non-bonding pair of electrons.
B
Each nitrogen atom has four bonding pairs of electrons.
C
Each nitrogen atom shares one of its electrons with a nitrogen atom.
D
Each nitrogen atom shares two of its electrons with hydrogen atoms.
© UCLES 2020
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4
7
Solid X has a high boiling point.
Its structure has positive ions surrounded by a sea of electrons.
Which other properties does solid X have?
8
A
brittle and an electrical conductor
B
brittle and an insulator
C
malleable and an electrical conductor
D
malleable and an insulator
The formulae of some ions are shown.
positive ions
negative ions
Al 3+
Cl –
Fe2+
N3–
Mg2+
NO3–
Na+
O2–
Zn2+
SO42–
In which row is the formula not correct?
9
compound
formula
A
aluminium oxide
Al 2O3
B
iron(II) nitride
Fe2N3
C
sodium sulfate
Na2SO4
D
zinc nitrate
Zn(NO3)2
The equation for the decomposition of magnesium nitrate is shown.
2Mg(NO3)2(s) → 2MgO(s) + 4NO2(g) + O2(g)
Which volume of gas is produced when 0.1 moles of magnesium nitrate is decomposed
completely?
A
1.2 dm3
© UCLES 2020
B
4.8 dm3
C
6.0 dm3
0620/22/F/M/20
D
8.4 dm3
5
10 Which statements about the electrolysis of molten lead(II) bromide are correct?
A
1
Lead ions move to the anode and are oxidised.
2
Lead ions move to the cathode and are reduced.
3
Bromide ions move to the anode and are oxidised.
4
Bromide ions move to the cathode and are reduced.
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
11 Aqueous copper(II) sulfate is electrolysed using carbon electrodes.
Which statement is correct?
A
Bubbles of hydrogen are formed at the anode.
B
Bubbles of oxygen gas are formed at the cathode.
C
Copper is deposited at the anode.
D
The blue colour of the solution fades.
12 Nitrogen trifluoride, NF3, is used in the manufacture of certain types of solar panels. The equation
for the formation of nitrogen trifluoride is shown.
N2 + 3F2 → 2NF3
type of bond
bond energy (kJ mol–1)
N≡N
+950
F–F
+150
N–F
+280
Using the table of bond energies, what is the energy change for this reaction?
A
–560 kJ mol–1
B
–280 kJ mol–1
C
+280 kJ mol–1
D
+3080 kJ mol–1
© UCLES 2020
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6
13 Which statements about hydrogen fuel cells are correct?
A
1
The reaction between hydrogen and oxygen is endothermic.
2
The waste product in a hydrogen fuel cell is water.
3
A chemical reaction in the cell produces hydrogen which is used as the fuel.
4
A hydrogen fuel cell is used to generate electricity.
1 and 2
B
1 and 3
C
2 and 4
D
3 and 4
14 Which change is a physical change?
A
Copper(II) carbonate changes colour from green to black when it is heated, and stays black
when it cools.
B
Ethanol reacts with oxygen to form carbon dioxide and water.
C
Hydrogen peroxide decomposes into water and oxygen when it is boiled.
D
Ice forms liquid water when it is heated.
15 A student adds excess magnesium ribbon to 10 cm3 of 0.5 mol / dm3 sulfuric acid.
The hydrogen gas is collected and its volume measured every 10 seconds.
The experiment is repeated using the same mass of magnesium ribbon with 5 cm3 of 0.5 mol / dm3
sulfuric acid added to 5 cm3 of water.
Which graph shows the results of the second experiment?
250
A
200
original experiment
150
volume of
hydrogen / cm3
B
100
C
50
D
0
0
50
100
150
time / seconds
© UCLES 2020
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200
250
7
16 An equilibrium reaction is shown.
N2O4(g)
2NO2(g)
The forward reaction is endothermic.
What is the effect of changing the temperature and pressure on the equilibrium position?
increasing temperature
increasing pressure
A
moves to the left
moves to the left
B
moves to the left
moves to the right
C
moves to the right
moves to the left
D
moves to the right
moves to the right
17 In which reaction is the underlined compound acting as a reducing agent?
A
CO2 + C → 2CO
B
2CuO + C → 2Cu + CO2
C
Fe2O3 + 3CO → 2Fe + 3CO2
D
CaCO3 + 2HCl → CaCl 2 + H2O + CO2
18 X, Y and Z are oxides of elements in the same row of the Periodic Table.
Some information about each oxide is shown.
oxide
solubility
in water
ability to
neutralise
an acid
ability to
neutralise
an alkali
X
soluble
key
Y
insoluble
= able
Z
slightly soluble
= not able
Which types of oxides are X, Y and Z?
X
Y
Z
A
acidic
amphoteric
basic
B
amphoteric
basic
basic
C
basic
amphoteric
acidic
D
basic
acidic
amphoteric
© UCLES 2020
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19 Four different acids are dissolved in water.
Which beaker contains the most concentrated strong acid solution?
A
B
Z–
HY
Z–
HY
Y–
H+
H+
–
Z
Z–
H+
HY
H+
Z–
H+
H+
HY
Y–
H+
HY
Z–
H
HY
+
C
D
X–
HX
H+
H+
W–
H+
HX
HX
X–
HX
X
HX
HX
H+
HX
H
W–
W–
–
H+
+
H+
HX
W–
20 The following substances can be reacted together to prepare salts.
1
copper(II) oxide and excess hydrochloric acid
2
hydrochloric acid and excess sodium hydroxide
3
hydrochloric acid and excess zinc carbonate
In which reactions can the excess reactant be separated from the solution by filtration?
A
1 and 2
© UCLES 2020
B
1 and 3
C
2 and 3
0620/22/F/M/20
D
3 only
9
21 Salt S is dissolved in water and three tests are carried out on the solution.
test
result
1
aqueous sodium
hydroxide is added
green precipitate formed,
insoluble in excess sodium
hydroxide
2
dilute nitric acid is added
no reaction
3
aqueous barium nitrate is added
to the acidified solution from test 2
white precipitate formed
What is the identity of S?
A
copper(II) chloride
B
copper(II) sulfate
C
iron(II) chloride
D
iron(II) sulfate
22 Which statement about the Periodic Table is correct?
A
Most metallic elements are on the left.
B
Elements in the same period have the same number of outer electrons.
C
Elements on the left are usually gases.
D
The relative atomic mass of the elements increases from right to left.
23 The diagram shows elements W, X, Y and Z in a section of the Periodic Table.
W
X
Z
Y
Which statement about the reactivity of the elements is correct?
A
X is more reactive than Y, and W is more reactive than Z.
B
X is more reactive than Y, and Z is more reactive than W.
C
Y is more reactive than X, and W is more reactive than Z.
D
Y is more reactive than X, and Z is more reactive than W.
© UCLES 2020
0620/22/F/M/20
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10
24 Some properties of substances are listed.
1
They conduct electricity.
2
They have low densities.
3
They have high melting points.
4
They are malleable.
Which properties are shown by transition metals?
A
1 and 3 only
B
1 and 4 only
C
1, 2 and 3
D
1, 3 and 4
25 Sodium is a Group I metal.
Which property, that is typical of most metals, is not shown by sodium?
A
conductor of heat
B
high melting point
C
malleable
D
shiny
26 Four metals, iron, copper, magnesium and Y, are heated separately with their oxides.
The results are shown.
metal
magnesium
oxide
Y
oxide
copper
oxide
iron
oxide
Y
key
magnesium
= reacts
copper
= no reaction
iron
What is the order of reactivity of the metals, least reactive first?
least reactive
most reactive
A
copper
iron
Y
magnesium
B
copper
Y
iron
magnesium
C
magnesium
iron
Y
copper
D
magnesium
Y
iron
copper
© UCLES 2020
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11
27 Aluminium is extracted from bauxite by electrolysis.
Which statement is correct?
A
Aluminium ions are oxidised to form aluminium.
B
The cathode has to be replaced regularly because it reacts with the oxygen which is formed.
C
Cryolite is added to remove impurities.
D
Carbon dioxide is produced at the anode.
28 Some properties of aluminium are listed.
1
It conducts heat.
2
It has a low density.
3
It is strong.
4
It is resistant to corrosion.
Which of these properties make aluminium suitable for making food containers for chilled food
products?
A
1, 2 and 4
B
1, 3 and 4
C
1 only
D
4 only
29 Water is treated at a waterworks to make it fit to drink.
What is present in the water when it leaves the waterworks?
A
bacteria only
B
bacteria and insoluble substances
C
chlorine compounds only
D
chlorine compounds and soluble substances
30 Sulfur dioxide, carbon monoxide and oxides of nitrogen are common gaseous pollutants found in
the air.
Which pollutants contribute to acid rain?
A
carbon monoxide and sulfur dioxide
B
oxides of nitrogen and sulfur dioxide
C
oxides of nitrogen only
D
sulfur dioxide only
© UCLES 2020
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12
31 Oxides of nitrogen, such as NO and NO2, are formed in the petrol engines of cars.
They are removed from the exhaust gases by reactions in the car’s catalytic converter.
Which row describes how oxides of nitrogen are formed in a petrol engine, and a reaction that
happens in the catalytic converter?
how oxides of nitrogen are formed
a reaction that happens
in the catalytic convertor
A
by the reaction between
nitrogen and oxygen from the air
2NO + 2CO → N2 + 2CO2
B
by the reaction between
nitrogen and oxygen from the air
2NO + 2H2 → N2 + 2H2O
C
by the reaction between nitrogen
compounds in petrol and oxygen from the air
2NO + 2CO → N2 + 2CO2
D
by the reaction between nitrogen
compounds in petrol and oxygen from the air
2NO + 2H2 → N2 + 2H2O
32 Zinc is used to cover iron to prevent it from rusting.
Why is zinc a suitable metal to use?
A
Iron is more reactive than zinc.
B
Iron atoms are bigger than zinc atoms.
C
Zinc is more reactive than iron.
D
Zinc atoms are bigger than iron atoms.
33 Fertilisers are mixtures of different compounds used to increase the growth of crops.
Which pair of substances contain the three essential elements for plant growth?
A
ammonium nitrate and calcium phosphate
B
ammonium nitrate and potassium chloride
C
ammonium phosphate and potassium chloride
D
potassium nitrate and calcium carbonate
© UCLES 2020
0620/22/F/M/20
13
34 Which row describes the conditions used in the manufacture of sulfuric acid by the Contact
process?
catalyst
pressure
temperature
A
iron
high
high
B
iron
low
low
C
vanadium(V) oxide
high
low
D
vanadium(V) oxide
low
high
35 Petroleum is an important raw material that is separated into useful products.
Which terms describe petroleum and the method used to separate it?
description
separation method
A
compound
cracking
B
compound
fractional distillation
C
mixture
cracking
D
mixture
fractional distillation
36 Which statements about propene are correct?
A
1
Propene contains only single bonds.
2
Propene decolourises bromine water.
3
Propene is obtained by cracking.
4
Propene is a hydrocarbon.
1 and 4
B
2, 3 and 4
C
2 and 4 only
D
4 only
37 Which row describes the production of ethanol and its properties?
can be made
from glucose
can be made
from ethene
is used as a
fuel
is used as a
solvent
A
key
B
= yes
C
= no
D
© UCLES 2020
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14
38 Ethanoic acid is a typical carboxylic acid.
Which statement about ethanoic acid is correct?
A
It can be oxidised to produce ethanol.
B
It is a proton acceptor.
C
It is fully dissociated in water.
D
It reacts with ethanol to produce ethyl ethanoate and water.
39 Which structure represents the ester made from ethanoic acid and propanol?
B
A
H
H
H
H
C
C
C
H
H
H
O
O
H
C
C
H
H
H
H
H
O
C
C
C
H
H
O
H
H
O
C
C
C
H
H
O
H
H
C
C
H
H
H
H
H
O
C
C
O
H
40 The structure of a polymer is shown.
H
O
N
C
N
C
H
O
H
O
N
C
Which statements about the polymer are correct?
A
1
The polymer is nylon.
2
The polymer is formed by condensation polymerisation.
3
There are ester linkages between the monomers.
1 and 2
© UCLES 2020
H
H
C
C
C
H
H
H
H
H
C
C
H
H
D
C
H
H
B
2 and 3
C
2 only
0620/22/F/M/20
D
3 only
H
H
15
BLANK PAGE
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reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/22/F/M/20
© UCLES 2020
21
0620/22/F/M/20
calcium
40
38
Sr
strontium
88
56
Ba
barium
137
88
potassium
39
37
Rb
rubidium
85
55
Cs
caesium
133
87
22
cerium
140
90
Th
thorium
232
lanthanum
139
89
Ac
actinium
–
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
Ce
57
–
dubnium
Db
105
181
tantalum
Ta
73
93
niobium
Nb
41
51
vanadium
V
–
rutherfordium
Rf
104
178
hafnium
Hf
72
91
zirconium
Zr
40
48
titanium
La
lanthanoids
57–71
89
yttrium
Y
39
45
scandium
Ti
23
Cr
24
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
relative atomic mass
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Pt
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
49
70
gallium
Ga
31
27
aluminium
Al
13
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ca
K
–
actinoids
20
19
Ra
24
23
radium
magnesium
sodium
Fr
Mg
Na
francium
89–103
12
11
Sc
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
Group
The Periodic Table of Elements
16
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
October/November 2020
45 minutes
You must answer on the multiple choice answer sheet.
*4506129529*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
 There are forty questions on this paper. Answer all questions.
 For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
 Follow the instructions on the multiple choice answer sheet.
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
 Do not use correction fluid.
 Do not write on any bar codes.
 You may use a calculator.
INFORMATION
 The total mark for this paper is 40.
 Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
 Any rough working should be done on this question paper.
 The Periodic Table is printed in the question paper.
This document has 16 pages. Blank pages are indicated.
IB20 11_0620_22/4RP
© UCLES 2020
[Turn over
2
1
Which gas has the slowest rate of diffusion?
A
2
H2
B
NH3
C
CH4
D
A chromatography experiment is carried out to analyse the pigments present in four different
types of leaf. The student carrying out the experiment forgot to complete his table of results,
which is shown.
plant
leaf
number of
pigments
identified
colour of
identified
pigments
distance
travelled by
the solvent
front (cm)
distance travelled
from the origin by
each pigment (cm)
Rf value
maple
F
green
/ yellow
3.7
green: 3.0
yellow: 3.1
green: 0.81
yellow: 0.83
laurel
2
green
/ yellow
G
green: 2.5
yellow: 2.5
green: 0.78
yellow: 0.78
lime
3
green
/ yellow
/ orange
3.5
green: 2.9
yellow: 3.0
orange: 2.7
green: 0.83
yellow: 0.86
yellow: 0.77
3
green
/ yellow
/ orange
3.5
green: 2.8
yellow: 3.0
orange: 2.7
green: 0.80
yellow: H
orange: 0.77
ash
Which row identifies the values of F, G and H?
3
CO2
F
G
H
A
2
3.2
0.80
B
3
3.5
0.83
C
2
3.2
0.86
D
3
3.5
0.78
Which statement about isotopes is correct?
A
They have different proton numbers.
B
They have different chemical properties.
C
They have the same nucleon number.
D
They have the same number of electrons in their outer shell.
© UCLES 2020
0620/22/O/N/20
3
4
In the chromatography experiment shown, which label represents the solvent front?
A
B
D
C
5
Different methods of separation rely on substances having different properties.
Which property does distillation make use of?
6
A
boiling point
B
colour
C
particle size
D
solubility in different solvents
The arrangements of the electrons in two ions formed from elements X and Y are shown.
X
Y
n = 20
p = 19
n = 20
p = 17
Which equation represents the reaction between elements X and Y?
A
X2 + 2Y  2X+ + 2Y–
B
X2 + 2Y  2X– + 2Y+
C
2X + Y2  2X+ + 2Y–
D
2X + Y2  2X– + 2Y+
© UCLES 2020
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7
8
Which row identifies compounds that contain single covalent bonds only, double covalent bonds
only or both single and double covalent bonds?
single covalent bonds
only
double covalent bonds
only
both single and
double covalent bonds
A
C2H4
CH3OH
CO2
B
CH3OH
C2H4
CO2
C
CH3OH
CO2
C2H4
D
CO2
C2H4
CH3OH
Ethyl methanoate, HCOOC2H5, burns in excess oxygen to produce carbon dioxide and water.
The equation is shown.
2HCOOC2H5 + xO2  6CO2 + 6H2O
What is the value of x?
A
9
2
B
7
C
9
D
18
Rubidium is in Group I of the Periodic Table and bromine is in Group VII.
Rubidium reacts with bromine to form an ionic compound.
Which row shows the electron change taking place for rubidium and the correct formula of the
rubidium ion?
electron change
formula of ion formed
A
electron gained
Rb+
B
electron gained
Rb–
C
electron lost
Rb+
D
electron lost
Rb–
10 Which statement explains why graphite is used as a lubricant?
A
All bonds between the atoms are weak.
B
It conducts electricity.
C
It has a low melting point.
D
Layers in the structure can slide over each other.
© UCLES 2020
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11 The relative atomic mass of chlorine is 35.5.
When calculating relative atomic mass, which particle is the mass of a chlorine atom compared
to?
A
a neutron
B
a proton
C
an atom of carbon-12
D
an atom of hydrogen-1
12 Universal indicator solution is added to a neutral solution of concentrated aqueous sodium
chloride.
The solution, which contains H+ (hydrogen), Na+ (sodium), Cl – (chloride) and OH– (hydroxide)
ions, is electrolysed.
The product at the cathode is hydrogen gas and the product at the anode is chlorine gas.
What happens to the colour of the indicator in the solution during electrolysis?
A
The colour changes from blue to green.
B
The colour changes from blue to red.
C
The colour changes from green to blue.
D
The colour changes from green to red.
13 What is the empirical formula of an oxide of iron, formed by reacting 2.24 g of iron with 0.96 g of
oxygen?
A
FeO
B
Fe2O
C
Fe2O3
D
Fe3O4
14 The combustion of methane is exothermic.
CH4 + 2O2  CO2 + 2H2O
Which statement about this reaction is correct?
A
The energy needed to break the bonds in methane and oxygen is greater than the energy
released in making new bonds in carbon dioxide and water.
B
The energy needed to break the bonds in methane and oxygen is less than the energy
released in making new bonds in carbon dioxide and water.
C
The energy released in breaking bonds in methane and oxygen is greater than the energy
needed to make new bonds in carbon dioxide and water.
D
The energy released in breaking bonds in methane and oxygen is less than the energy
needed to make new bonds in carbon dioxide and water.
© UCLES 2020
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15 Hydrogen reacts with oxygen in a fuel cell.
2H2 + O2  2H2O
The reaction is exothermic.
286 kJ of energy is released for every mole of water formed.
Which volume of hydrogen gas, measured at room temperature and pressure, would react with
oxygen with the release of 7000 J of energy?
A
587 cm3
B
1175 cm3
C
587 dm3
D
1175 dm3
16 Which substance does not require oxygen in order to produce energy?
A
coal
B
hydrogen
C
natural gas
D
235
U
17 Nitrogen, N2, and hydrogen, H2, can be converted into ammonia, NH3, using a catalyst.
What is the purpose of the catalyst?
A
to increase the amount of ammonia produced
B
to increase the rate of reaction
C
to reduce the amount of reactants needed
D
to reduce the rate of reaction
18 Ammonia is produced by the Haber process. The equation is shown.
N2(g) + 3H2(g)
2NH3(g)
The forward reaction is exothermic.
Which statement is correct?
A
Increasing pressure decreases the yield of ammonia, but speeds up the reaction.
B
Increasing temperature decreases the yield of ammonia, but speeds up the reaction.
C
Increasing the concentration of hydrogen and nitrogen results in a lower yield of ammonia.
D
Increasing the temperature increases the yield of ammonia and speeds up the reaction.
© UCLES 2020
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19 During the manufacture of sulfuric acid, sulfur dioxide is converted to sulfur trioxide.
2SO2 + O2  2SO3
Which type of reaction is this?
A
displacement
B
neutralisation
C
oxidation
D
thermal decomposition
20 The equation for a redox reaction is shown.
2FeSO4 + Cl 2 + H2SO4  Fe2(SO4)3 + 2HCl
Which element is reduced?
A
chlorine
B
iron
C
oxygen
D
sulfur
21 The equation shows a reaction between aqueous hydrogen bromide and aqueous ammonia.
HBr(aq) + NH3(aq)  NH4+(aq) + Br–(aq)
Which statement describes the role of aqueous hydrogen bromide?
A
It is a catalyst.
B
It is a reducing agent.
C
It is a proton acceptor.
D
It is a proton donor.
22 The equations for three reactions are shown.
1
Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq)
2
2AgNO3(aq) + CuI2(aq)  Cu(NO3)2(aq) + 2AgI(s)
3
CuO(s) + H2SO4(aq)  CuSO4(aq) + H2O(l)
Which reactions are suitable for making a salt by precipitation?
A
1 and 2 only
© UCLES 2020
B
1 and 3 only
C
2 and 3 only
0620/22/O/N/20
D
1, 2 and 3
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23 Zinc oxide is an amphoteric oxide.
Which row describes the reactions of zinc oxide?
reaction
with alkalis
reaction
with acids
A
B
C
D
24 A student carries out an experiment to prepare pure magnesium sulfate crystals.
The diagram shows the first stage of the preparation.
stirrer
magnesium
carbonate
dilute sulfuric acid
He adds magnesium carbonate until no more reacts.
Which process should he use for the next stage?
A
crystallisation
B
evaporation
C
filtration
D
neutralisation
25 Which row about elements in the Periodic Table is correct?
statement 1
statement 2
A
two elements in the same group
have similar chemical properties
metals are on the
left of the table
B
two elements in the same group
have similar chemical properties
metals are on the
right of the table
C
two elements in the same period
have similar chemical properties
metals are on the
left of the table
D
two elements in the same period
have similar chemical properties
metals are on the
right of the table
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26 A new element oxfordium, Ox, was discovered with the following properties.
solubility
electrical
conduction
formula
of element
insoluble in water
doesn’t conduct
Ox2
bonding in a
molecule of Ox2
Ox
Ox
In which group of the Periodic Table should the new element be placed?
A
Group III
B
Group V
C
Group VII
D
Group VIII
27 A flammable gas needs to be removed from a tank at an industrial plant.
For safety reasons, an inert gas is used.
Which gas is suitable?
A
argon
B
hydrogen
C
methane
D
oxygen
28 Transition elements can have variable oxidation states.
Which pair of compounds shows a transition element in two different oxidation states?
A
Cr2O3 and Cr2(SO4)3
B
Cu2O and CuCO3
C
ZnS and ZnSO4
D
NiO and Ni(NO3)2
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29 Which diagram best represents the structure of a substance that is a good conductor of electricity
at 25 C?
A
B
C
D
– + – +
+ – + –
– + – +
30 Why is aluminium metal unreactive with air?
A
It is covered with a layer of oxide.
B
It is low in the reactivity series.
C
It is produced by electrolysis of its oxide.
D
It melts at a high temperature.
31 The apparatus used for the extraction of aluminium oxide by electrolysis is shown.
carbon
anodes
–
+
carbon lining
as cathode
solution of
aluminium oxide
in molten cryolite
molten aluminium
collects at the bottom
Which equation represents a reaction taking place at the anode?
A
O + 2e–  O2–
B
2O2–  O2 + 4e–
C
Al 3–  Al + 3e–
D
Al 3+ + 3e–  Al
© UCLES 2020
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32 The results of tests on solid S and its aqueous solution are shown.
tests on solid S
tests on aqueous solution of S
effect of heat
effect of aqueous
sodium hydroxide
effect of
aqueous ammonia
brown gas given off,
together with a gas which
relights a glowing splint
white ppt., soluble in
excess, giving a
colourless solution
white ppt., soluble in
excess, giving a
colourless solution
What is S?
A
aluminium nitrate
B
aluminium sulfate
C
zinc sulfate
D
zinc nitrate
33 Part of the carbon cycle is shown.
combustion
glucose
CO2
Q
R
plant
CH4
P
What are processes P, Q and R?
P
Q
R
A
decomposition
respiration
photosynthesis
B
respiration
photosynthesis
decomposition
C
respiration
decomposition
photosynthesis
D
photosynthesis
respiration
decomposition
34 The element sulfur is found in a number of different minerals.
Which mineral contains the greatest percentage by mass of sulfur?
A
barite, BaSO4
B
galena, PbS
C
gypsum, CaSO4
D
pyrite, FeS2
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35 Which structure represents a molecule of ethanol?
A
H
B
H
H
C
C
H
H
C
H
H
H
C
C
H
H
H
H
H
C
C
H
H
D
H
O
H
H
H
36 Which structures are structural isomers of each other?
2
1
H
H
H
H
H
C
C
C
C
H
H
H
H
H
H
H
H
H
C
C
C
H
H
H
H
C
H
H
3
H
4
H
H
H
C
C
C
H
H
C
H
H
H
H
H
H
H
C
C
C
C
H
H
H
H
H
A
1, 2, 3 and 4
B
1, 2 and 4 only
C
1 and 3 only
D
2 and 4 only
H
H
37 Which molecule is not produced by an addition reaction of ethene?
A
CH3CH3
© UCLES 2020
B
CH2BrCH2Br
C
CH3CH2OH
0620/22/O/N/20
C
D
CH3CH2CH3
O
C
O
H
13
38 The flow chart shows the preparation of ethanol and some important chemistry of ethanol.
fermentation
substance X
process Y
ethanol
carbon dioxide + substance Z
What are X, Y and Z?
X
Y
Z
A
yeast
combustion
oxygen
B
glucose
combustion
steam
C
glucose
polymerisation
water
D
yeast
fermentation
glucose
39 Which statement about nylon and Terylene is correct?
A
Nylon and Terylene are made from monomers with C=C bonds.
B
Nylon and Terylene contain the same linkage.
C
Nylon is a polyester.
D
Terylene is made from two different monomers.
40 Which diagram represents the structure of a protein?
A
O
O
C
C
O
O
B
C
C
C
O
O
H
O
N
C
D
© UCLES 2020
N
N
H
H
O
O
O
O
C
C
O
O
C
C
H
O
N
C
O
N
C
H
O
0620/22/O/N/20
14
BLANK PAGE
© UCLES 2020
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15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/22/O/N/20
© UCLES 2020
21
39
Y
12
Mg
magnesium
24
20
Ca
calcium
40
38
11
Na
sodium
23
19
K
potassium
39
37
22
73
Ta
72
Hf
89
57–71
lanthanoids
88
56
0620/22/O/N/20
Th
thorium
232
–
90
89
Ac
140
139
actinium
Ce
cerium
La
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
57
lanthanum
–
dubnium
Db
105
181
tantalum
–
rutherfordium
Rf
104
178
hafnium
93
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
Cr
24
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
Pt
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
49
70
gallium
Ga
31
27
aluminium
Si
14
13
Al
12
carbon
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
Group
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
–
actinoids
Ra
radium
88
87
Fr
137
133
francium
89–103
Ba
barium
Cs
caesium
91
Nb
niobium
55
Zr
zirconium
85
yttrium
Sr
strontium
41
51
vanadium
V
Rb
40
48
titanium
Ti
23
relative atomic mass
rubidium
45
scandium
Sc
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
*7179838283*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
October/November 2020
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working and use appropriate units.
INFORMATION
●● The total mark for this paper is 80.
●● The number of marks for each question or part question is shown in brackets [ ].
●● The Periodic Table is printed in the question paper.
This document has 12 pages. Blank pages are indicated.
IB20 11_0620_42/4RP
© UCLES 2020
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2
1The electronic structures of some atoms and ions are shown.
A
B
C
D
2+
+
E
F
H
G
–
3–
–
(a)Write the letters, A, B, C, D, E, F, G or H, of the electronic structures which show:
(i)atoms of two different noble gases ....................................... and ��������������������������������������
[2]
(ii)an ion of a Group I element ........................................................................................... [1]
(iii)an ion of a Group V element .......................................................................................... [1]
(iv)a pair of ions that could form a compound with the formula XY2. ............ and .............. [1]
(b)State which electronic structure, A, B, C, D, E, F, G or H, is incorrect.
Explain why.
incorrect electronic structure �����������������������������������������������������������������������������������������������������
explanation .................................................................................................................................
.....................................................................................................................................................
[2]
(c)State how many protons are found in the nucleus of ion C. ................................................. [1]
(d)Use the Periodic Table to deduce:
(i)the chemical symbol for ion G ....................................................................................... [1]
(ii)the element which forms an ion with a 3+ charge and the same electronic structure as H.
........................................................................................................................................ [1]
© UCLES 2020
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2Soluble salts can be made by adding a metal carbonate to a dilute acid.
(a)Give the formula of the dilute acid which reacts with a metal carbonate to form a nitrate salt.
............................................................................................................................................... [1]
(b)A student wanted to make hydrated iron(II) sulfate crystals, FeSO4•xH2O, by adding excess
iron(II) carbonate to dilute sulfuric acid. The student followed the procedure shown.
step 1Add dilute sulfuric acid to a beaker.
step 2Add small amounts of iron(II) carbonate to the dilute sulfuric acid in the beaker until
the iron(II) carbonate is in excess.
step 3Filter the mixture formed in step 2.
step 4
Heat the filtrate until it is a saturated solution. Allow to cool.
step 5
Once cold, pour away the remaining solution. Dry the crystals between filter papers.
(i)Why must the iron(II) carbonate be added in excess in step 2?
........................................................................................................................................ [1]
(ii)State two observations in step 2 that would show that iron(II) carbonate was in excess.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(iii)Describe what should be done during step 3 to ensure there is a maximum yield of crystals.
........................................................................................................................................ [1]
(iv)A saturated solution is formed in step 4.
Describe what a saturated solution is.
..............................................................................................................................................
........................................................................................................................................ [2]
(v)Name a different compound that could be used instead of iron(II) carbonate to produce
hydrated iron(II) sulfate crystals from dilute sulfuric acid.
........................................................................................................................................ [1]
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(c)On analysing the crystals, the student found that one mole of the hydrated iron(II) sulfate
crystals, FeSO4•xH2O, had a mass of 278 g.
Determine the value of x using the following steps:
●●
calculate the mass of one mole of FeSO4
mass = .............................. g
●●
calculate the mass of H2O present in one mole of FeSO4•xH2O
mass of H2O = .............................. g
●●
determine the value of x.
x = ..............................
[3]
(d)Insoluble salts can be made by mixing solutions of two soluble salts.
A student followed the procedure shown to make silver bromide, an insoluble salt.
step 1
dd aqueous silver nitrate to a beaker. Then add aqueous potassium bromide and
A
stir.
step 2Filter the mixture formed in step 1.
step 3Dry the residue.
(i)State the term used to describe this method of making salts.
........................................................................................................................................ [1]
(ii)Give the observation the student would make during step 1.
........................................................................................................................................ [1]
(iii)Write the ionic equation for the reaction between aqueous silver nitrate and aqueous
potassium bromide.
Include state symbols.
........................................................................................................................................ [3]
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(e)Sodium chloride is an ionic salt. It can be made by reacting sodium with chlorine gas.
The equation for this reaction is shown.
2Na(s) + Cl 2(g) → 2NaCl (s)
Calculate the volume of chlorine gas, in cm3, that reacts to form 2.34 g of NaCl .
The reaction takes place at room temperature and pressure.
volume of chlorine gas = .............................. cm3 [3]
(f)Sodium chloride does not conduct electricity when solid, but does conduct electricity when
molten.
(i)Explain why, in terms of structure and bonding.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(ii)Name the product formed at the positive electrode when electricity is passed through
molten sodium chloride.
........................................................................................................................................ [1]
(iii)State the type of change that occurs at the positive electrode in (ii).
Explain your answer in terms of electron transfer.
type of change .....................................................................................................................
explanation ..........................................................................................................................
[2]
(iv)Describe what else can be done to sodium chloride to allow it to conduct electricity.
........................................................................................................................................ [1]
© UCLES 2020
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6
3Group I metals are very reactive. Transition elements are also metals but are less reactive than
Group I metals.
(a)State two physical properties of Group I metals which are similar to those of transition metals.
1 ..................................................................................................................................................
2 ..................................................................................................................................................
[2]
(b)Describe two ways in which the physical properties of Group I metals are different from those
of transition metals.
1 ..................................................................................................................................................
.....................................................................................................................................................
2 ..................................................................................................................................................
.....................................................................................................................................................
[2]
(c) When Group I metals are added to water they fizz and an alkaline solution forms.
(i)Name the gas given off.
........................................................................................................................................ [1]
(ii)Identify the ion present in the solution which makes the solution alkaline.
........................................................................................................................................ [1]
(iii)Write the chemical equation for the reaction between sodium and water.
........................................................................................................................................ [2]
(d)When the transition element iron is added to water the iron rusts.
When an iron object is coated with a layer of zinc, rusting is prevented.
(i)
Name this process of coating iron objects with a layer of zinc.
........................................................................................................................................ [1]
(ii)
Explain how completely coating an iron object with a layer of zinc prevents rusting.
........................................................................................................................................ [1]
(iii)
Rusting of iron ships can be prevented by attaching zinc blocks to the hull of the ship.
Explain how this prevents rusting.
..............................................................................................................................................
........................................................................................................................................ [2]
© UCLES 2020
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7
4Alkenes and alkanes are homologous series of compounds containing carbon and hydrogen atoms.
(a)State the name of the type of compound made from carbon and hydrogen atoms only.
............................................................................................................................................... [1]
(b)Alkenes take part in addition reactions.
(i)Describe what is meant by the term addition reaction.
........................................................................................................................................ [1]
(ii)Draw the structure of the product made in the addition reaction between propene and
bromine. Show all of the atoms and all of the bonds.
[2]
(iii)Describe the colour change seen when propene is added to aqueous bromine.
from ............................................................ to ............................................................. [2]
(iv)Draw the structures of molecules of two different alkenes which both undergo an addition
reaction with steam to form butan-2-ol. Show all of the atoms and all of the bonds.
[2]
(c)Propane undergoes a substitution reaction with chlorine.
Write the chemical equation for the reaction between one molecule of propane and one
molecule of chlorine.
............................................................................................................................................... [2]
© UCLES 2020
[Total: 10]
0620/42/O/N/20
[Turn over
8
5This question is about alcohols, carboxylic acids and esters.
(a)Ethanol will react with hot aqueous potassium manganate(VII) to form ethanoic acid.
(i)State the other condition needed for this reaction to take place.
........................................................................................................................................ [1]
(ii)State the type of chemical change that happens to the ethanol during this reaction.
........................................................................................................................................ [1]
(iii)The structure of ethanoic acid is shown.
H
H
C
H
O
C
O
H
Complete the dot-and-cross diagram to show the electron arrangement in a molecule of
ethanoic acid.
O
H
H
C
C
H
O
H
[3]
© UCLES 2020
0620/42/O/N/20
9
(b)Ethanoic acid is a weak acid and hydrochloric acid is a strong acid.
Complete the table to show the similarities and differences in the properties of samples of
these two acids of equal concentration.
dilute ethanoic acid
dilute hydrochloric acid
extent of dissociation
colour after adding
universal indicator solution
observation when
magnesium ribbon is added
[6]
(c)Ethanoic acid will react with an alcohol to form the ester shown.
H
H
H
O
H
C
H
C
C
O
C
H
H
C
H
H
H
(i)Name the other product formed when ethanoic acid reacts with an alcohol to make this
ester.
........................................................................................................................................ [1]
(ii)Give one condition needed when ethanoic acid reacts with the alcohol to make this ester.
........................................................................................................................................ [1]
(iii)Draw the structure of the alcohol which was added to ethanoic acid to make this ester.
Show all of the atoms and all of the bonds.
[2]
© UCLES 2020
0620/42/O/N/20
[Turn over
10
(d)Polyesters can be manufactured from carboxylic acids and alcohols.
Hexanedioic acid has the structure: HOOC–CH2–CH2–CH2–CH2–COOH.
This structure can be simplified as shown.
H
O
O
O
C
C
O
H
Ethanediol has the structure: HO–CH2–CH2–OH.
This structure can be simplified as shown.
H
O
O
H
The functional groups are found at the end of each molecule.
(i)State what is meant by the term functional group.
........................................................................................................................................ [1]
(ii)Determine the empirical formula of hexanedioic acid.
........................................................................................................................................ [1]
(iii)Calculate the percentage by mass of oxygen present in ethanediol.
Give your answer to the nearest whole number.
.............................. % [2]
(iv)Complete the diagram to show a section of polyester manufactured from hexanedioic acid
and ethanediol. Include all of the atoms and all of the bonds in the linkages.
[2]
(v)State the name of a polyester.
........................................................................................................................................ [1]
© UCLES 2020
[Total: 22]
0620/42/O/N/20
11
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/42/O/N/20
© UCLES 2020
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/O/N/20
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
12
Cambridge IGCSE™
*8955238231*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
October/November 2020
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working and use appropriate units.
INFORMATION
●● The total mark for this paper is 40.
●● The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Blank pages are indicated.
IB20 11_0620_62/RP
© UCLES 2020
[Turn over
2
1
The diagram shows the apparatus used to pass an electric current
concentrated hydrochloric acid. Hydrogen and chlorine were formed at the electrodes.
through
+ power –
supply
switch
A
(a)Name the item of apparatus labelled A.
............................................................................................................................................... [1]
(b)The electrodes were made of platinum.
(i)Give two reasons why platinum is a suitable material for the electrodes.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(ii)Suggest another material suitable to use as electrodes in this experiment.
........................................................................................................................................ [1]
(c)The teacher doing this experiment wore safety glasses, gloves, had their hair tied back and
stood up throughout the experiment.
State one other safety precaution that should be taken when doing this experiment.
Explain your answer.
safety precaution ........................................................................................................................
explanation .................................................................................................................................
[2]
© UCLES 2020
[Total: 6]
0620/62/O/N/20
3
2
student investigated the rate of a reaction between sodium metabisulfite and potassium iodate.
A
In the reaction, starch was used as an indicator. At first the reacting mixture remained colourless
but then suddenly changed to a blue-black colour.
Five experiments were done. In each experiment the total volume of liquid was 45 cm3.
Experiment 1
●● Using a 10 cm3 measuring cylinder, 5 cm3 of aqueous sodium metabisulfite was poured into a
beaker.
●● Using another 10 cm3 measuring cylinder, 5 cm3 of aqueous starch was poured into the beaker.
●● Using a 25 cm3 measuring cylinder, 15 cm3 of distilled water was poured into the beaker.
●● Using another 25 cm3 measuring cylinder, 20 cm3 of aqueous potassium iodate was poured into
the beaker. At the same time a stop‑clock was started.
●● The mixture in the beaker was stirred until a sudden colour change was seen.
●● The stop‑clock was immediately stopped and the time recorded.
●● The beaker was rinsed with water.
Experiment 2
●● Experiment 1 was repeated
aqueous potassium iodate.
using
17 cm3
of
distilled
water
and
18 cm3
of
Experiment 3
●● Experiment 1 was repeated
aqueous potassium iodate.
using
21 cm3
of
distilled
water
and
14 cm3
of
Experiment 4
●● Experiment 1 was repeated
aqueous potassium iodate.
using
23 cm3
of
distilled
water
and
12 cm3
of
Experiment 5
●● Experiment 1 was repeated
aqueous potassium iodate.
using
25 cm3
of
distilled
water
and
10 cm3
of
© UCLES 2020
0620/62/O/N/20
[Turn over
4
(a)Use the information in the description of the experiments and the stop‑clock diagrams to
complete the table. Record the times in seconds.
experiment
volume of
aqueous sodium
metabisulfite
/ cm3
volume
of distilled
water
/ cm3
volume of
aqueous
potassium
iodate / cm3
stop‑clock diagram
0
seconds
0
1
20
45 15
time to
change
colour
/s
5
10
15
minutes
30
0
0
2
18
45 15
5
15
5
15
5
15
5
15
10
30
0
0
3
14
45 15
10
30
0
0
4
12
45 15
10
30
0
0
5
10
45 15
10
30
[5]
© UCLES 2020
0620/62/O/N/20
5
(b)Plot the results from Experiments 1 to 5 on the grid.
Draw a smooth curve of best fit.
80
70
60
time to change
colour / s
50
40
30
10
12
14
16
18
20
22
volume of aqueous potassium iodate / cm3
[3]
(c) (i)
From your graph, predict the time to change colour if 16 cm3 of aqueous potassium iodate
was used.
Show clearly on the grid how you worked out your answer.
time to change colour = .............................. s [2]
(ii)Calculate the volume of distilled water required if 16 cm3 of aqueous potassium iodate was
used.
volume of distilled water = .............................. cm3 [1]
(d)Sketch on the grid the graph you would expect if Experiments 1 to 5 were repeated at a higher
temperature.[1]
© UCLES 2020
0620/62/O/N/20
[Turn over
6
(e)The concentration of potassium iodate in the reaction mixture in each experiment can be
calculated using the equation shown.
concentration =
0.05 × volume of aqueous potassium iodate
45
(i)Calculate the concentration of potassium iodate in the reaction mixture in Experiment 2.
concentration = .............................. mol / dm3 [1]
(ii)State which experiment, 1, 2, 3, 4 or 5, had the fastest rate of reaction.
........................................................................................................................................ [1]
(f)Suggest why the volume of distilled water added to each experiment was increased as the
volume of aqueous potassium iodate was decreased.
.....................................................................................................................................................
............................................................................................................................................... [1]
(g)Give one change you could make to the apparatus used which would improve the results.
Explain your answer.
change to apparatus ...................................................................................................................
.....................................................................................................................................................
explanation .................................................................................................................................
.....................................................................................................................................................
[2]
(h)How could the reliability of the results of this investigation be checked?
.....................................................................................................................................................
............................................................................................................................................... [1]
© UCLES 2020
[Total: 18]
0620/62/O/N/20
7
3Solid Q and solid R were analysed. Solid Q was zinc carbonate.
Tests were done on each solid.
tests on solid Q
Complete the expected observations.
(a)Solid Q was placed in a boiling tube. About 10 cm3 of dilute sulfuric acid was added to the
boiling tube. Any gas produced was tested.
The contents of the boiling tube were kept for (c).
observations ...............................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(b)Identify the gas given off in (a).
............................................................................................................................................... [1]
(c)The reaction mixture from (a) was filtered.
The filtrate was solution S. 1 cm depth of solution S was poured into a boiling tube.
(i)Aqueous sodium hydroxide was added dropwise and then in excess to solution S in the
boiling tube.
observations ........................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Explain why it is not possible to identify the cation contained in solution S from your
observations in (c)(i).
..............................................................................................................................................
....................................................................................................................................... [1]
(iii)Suggest an additional test that can be done on solution S to confirm the cation was Zn2+.
..............................................................................................................................................
........................................................................................................................................ [1]
© UCLES 2020
0620/62/O/N/20
[Turn over
8
tests on solid R
Tests were done and the following observations were made.
tests on solid R
observations
test 1
A flame test was done on solid R.
yellow flame
Solid R was dissolved in distilled water to
produce solution R. The solution was divided
into two equal portions in two test‑tubes.
test 2
About 1 cm3 of dilute nitric acid followed by a
few drops of aqueous silver nitrate were added
to the first portion of solution R.
yellow precipitate formed
test 3
The second portion of solution R was added to
1 cm3 of aqueous bromine in a test‑tube.
the solution changed colour
from orange to brown
(d) Identify solid R.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2020
[Total: 10]
0620/62/O/N/20
9
4Brass is a mixture of two metals, copper and zinc.
opper does not react with dilute sulfuric acid. Zinc reacts with hot dilute sulfuric acid to form the
C
soluble salt zinc sulfate.
Plan an investigation to find the percentage by mass of zinc in a sample of brass.
In your answer you should include how to calculate the percentage by mass of zinc.
You have access to normal laboratory apparatus.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
© UCLES 2020
0620/62/O/N/20
[Turn over
10
BLANK PAGE
© UCLES 2020
0620/62/O/N/20
11
BLANK PAGE
© UCLES 2020
0620/62/O/N/20
12
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/62/O/N/20
Cambridge IGCSE™
*7932494915*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
May/June 2020
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working and use appropriate units.
INFORMATION
●● The total mark for this paper is 40.
●● The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Blank pages are indicated.
IB20 06_0620_62/3RP
© UCLES 2020
[Turn over
2
BLANK PAGE
© UCLES 2020
0620/62/M/J/20
3
1Hot copper(II) oxide reacts with hydrogen. The products are copper and steam.
The apparatus used to react copper(II) oxide with hydrogen is shown.
copper(II) oxide
U-tube
unreacted
hydrogen
hydrogen
colourless
liquid
collected
ice
(a)Draw an arrow on the diagram to show where the apparatus should be heated.
[1]
(b)During the reaction the colour of the copper(II) oxide changes.
State the colour change.
from ................................................................... to ....................................................................
[1]
(c)Identify the colourless liquid collected.
............................................................................................................................................... [1]
(d)Explain why the U-tube is in ice.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2020
0620/62/M/J/20
[Turn over
4
(e) (i)Large amounts of unreacted hydrogen should not be allowed to escape into the laboratory.
State why.
........................................................................................................................................ [1]
(ii)Complete the diagram to show how the unreacted hydrogen could be collected and its
volume measured.
Label any apparatus that you draw.
U-tube
unreacted
hydrogen
ice
colourless liquid
collected
[2]
© UCLES 2020
[Total: 8]
0620/62/M/J/20
5
2
A student investigated the temperature change when magnesium ribbon reacts with
dilute sulfuric acid.
Five experiments were done.
Experiment 1
●● Using a measuring cylinder, 20 cm3 of dilute sulfuric acid were poured into a boiling tube.
●● A thermometer was used to measure the initial temperature of the acid.
●● A 1 cm length of magnesium ribbon was added to the acid in the boiling tube.
●● The acid and magnesium ribbon in the boiling tube were stirred continuously using a
thermometer.
●● The highest temperature reached by the mixture was measured.
●● The boiling tube was rinsed out with distilled water.
Experiment 2
●● E
xperiment 1 was repeated using a 2 cm length of magnesium ribbon instead of the 1 cm length.
Experiment 3
●● E
xperiment 1 was repeated using a 3 cm length of magnesium ribbon instead of the 1 cm length.
Experiment 4
●● E
xperiment 1 was repeated using a 5 cm length of magnesium ribbon instead of the 1 cm length.
Experiment 5
●● E
xperiment 1 was repeated using a 6 cm length of magnesium ribbon instead of the 1 cm length.
© UCLES 2020
0620/62/M/J/20
[Turn over
6
(a)Use the information in the description of the experiments and the thermometer diagrams to
complete the table.
experiment
1
2
3
4
5
length of
magnesium
ribbon / cm
initial temperature
highest temperature
initial
highest
thermometer
thermometer
temperature
temperature
diagram
diagram
of acid / °C
of acid / °C
30
30
25
25
20
20
30
30
25
25
20
20
30
30
25
25
20
20
30
40
25
35
20
30
30
40
25
35
20
30
temperature
increase
/ °C
[4]
(b)In which experiment, 1, 2, 3, 4 or 5, was the temperature increase the largest?
............................................................................................................................................... [1]
© UCLES 2020
0620/62/M/J/20
7
(c)Add a suitable scale to the y-axis and plot the results from Experiments 1 to 5 on the grid.
Draw a smooth line graph, making sure that your line passes through (0,0).
temperature
increase / °C
0
0
1
2
3
4
length of magnesium ribbon / cm
5
6
[5]
(d)Explain why the graph line must pass through (0,0).
.....................................................................................................................................................
............................................................................................................................................... [1]
(e)From your graph, deduce the temperature increase if Experiment 1 is repeated using a 4 cm
length of magnesium ribbon.
Show clearly on the grid how you worked out your answer.
..............................
[3]
(f) (i)Why would carrying out the experiment in a polystyrene cup rather than a boiling tube
improve the accuracy of the results?
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Sketch on the grid the graph you would expect if the experiment was repeated using a
polystyrene cup instead of a boiling tube.
[1]
© UCLES 2020
0620/62/M/J/20
[Turn over
8
(g)The volume of dilute sulfuric acid could be measured with a 20 cm3 pipette.
(i)State one advantage of using a pipette rather than a measuring cylinder.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)State one disadvantage of using a pipette rather than a measuring cylinder.
..............................................................................................................................................
........................................................................................................................................ [1]
© UCLES 2020
[Total: 18]
0620/62/M/J/20
9
3Two solids, solid L and solid M, were analysed. Solid L was chromium(III) chloride.
Tests were done on each solid.
tests on solid L
Complete the expected observations.
Solid L was dissolved in distilled water to produce solution L. Solution L was divided into four
portions in three test-tubes and a boiling tube.
(a) T
o the first portion of solution L in the boiling tube, about 1 cm depth of dilute hydrochloric acid
was added. The boiling tube was warmed gently.
strip of filter paper was dipped in acidified potassium manganate(VII) solution and held at
A
the mouth of the boiling tube.
observations ......................................................................................................................... [1]
(b)To the second portion of solution L aqueous sodium hydroxide was added slowly until it was in
excess and no further changes were seen.
observations ...............................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(c)To the third portion of solution L aqueous ammonia was added slowly until it was in excess and
no further changes were seen.
observations ...............................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(d)To the fourth portion of solution L about 1 cm depth of dilute nitric acid was added followed by
about 1 cm depth of aqueous silver nitrate.
observations ...............................................................................................................................
............................................................................................................................................... [1]
© UCLES 2020
0620/62/M/J/20
[Turn over
10
tests on solid M
Tests were done and the following observations made.
tests on solid M
observations
test 1
Flame test
yellow flame seen
test 2
About 10 cm3 of dilute nitric acid was added to
solid M.
Any gas produced was tested.
effervescence
limewater turned milky
test 3
About 1 cm depth of aqueous barium nitrate
was added to the solution formed by adding
dilute nitric acid to solid M in test 2.
no change
(e)Identify solid M.
............................................................................................................................................... [2]
© UCLES 2020
[Total: 8]
0620/62/M/J/20
11
4Many window-cleaning products contain aqueous ammonia. Aqueous ammonia is an alkali that
reacts with dilute acids.
Plan an investigation to find which of two window-cleaning products contains the most concentrated
aqueous ammonia. Include in your plan:
●● the method you will use
●● how your results will be used to determine which window-cleaning product contains the most
concentrated aqueous ammonia.
You are provided with an aqueous solution of the two window‑cleaning products,
dilute hydrochloric acid of known concentration and common laboratory apparatus.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
© UCLES 2020
0620/62/M/J/20
[Turn over
12
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/62/M/J/20
Cambridge IGCSE™
*7336615318*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
May/June 2020
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working and use appropriate units.
INFORMATION
●● The total mark for this paper is 80.
●● The number of marks for each question or part question is shown in brackets [ ].
●● The Periodic Table is printed in the question paper.
This document has 16 pages. Blank pages are indicated.
IB20 06_0620_42/4RP
© UCLES 2020
[Turn over
2
1
(a)Give the name of the process that:
(i)occurs when a gas turns into a liquid
........................................................................................................................................ [1]
(ii)
occurs when a solid turns into a gas without first forming a liquid
........................................................................................................................................ [1]
(iii)is used to separate a mixture of liquids with different boiling points
........................................................................................................................................ [1]
(iv)is used to extract aluminium from aluminium oxide
........................................................................................................................................ [1]
(v)is used to separate a mixture of amino acids.
........................................................................................................................................ [1]
(b)The symbols of the elements in Period 2 of the Periodic Table are shown.
Li
Be
B
C
N
O
F
Ne
For each of the following, give the symbol of an element from Period 2 which matches the
description.
Each element may be used once, more than once or not at all.
Which element:
(i)combines with hydrogen to produce ammonia
........................................................................................................................................ [1]
(ii)makes up approximately 21% of clean, dry air
........................................................................................................................................ [1]
(iii)has atoms with only two electrons in the outer shell
........................................................................................................................................ [1]
(iv)has atoms with only seven protons
........................................................................................................................................ [1]
(v)is a monoatomic gas
........................................................................................................................................ [1]
(vi)is a soft metal stored in oil?
........................................................................................................................................ [1]
© UCLES 2020
[Total: 11]
0620/42/M/J/20
3
2Fluorine forms both ionic and covalent compounds.
(a) Magnesium reacts with fluorine to form the ionic compound magnesium fluoride.
The electronic structures of an atom of magnesium and an atom of fluorine are shown.
Mg
F
(i)Complete the dot-and-cross diagrams to show the electronic structures of one magnesium
ion and one fluoride ion. Show the charges on the ions.
.........
.........
Mg
F
[3]
(ii)
What is the formula of magnesium fluoride?
........................................................................................................................................ [1]
(iii)
Magnesium fluoride does not conduct electricity when it is solid.
What can be done to solid magnesium fluoride to make it conduct electricity?
In your answer explain why magnesium fluoride conducts electricity when this change is
made.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
© UCLES 2020
0620/42/M/J/20
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4
(b) Carbonyl fluoride, COF2, is a covalent compound. The structure of a molecule of COF2 is
shown.
F
C
F
O
Complete the dot-and-cross diagram to show the electron arrangement in a molecule of
carbonyl fluoride. Show outer shell electrons only.
F
F
C
O
[3]
(c) The melting points of magnesium fluoride and carbonyl fluoride are shown.
melting point / °C
(i)
magnesium fluoride
1263
carbonyl fluoride
–111
xplain, using your knowledge of structure and bonding, why magnesium fluoride has a
E
high melting point.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)
Explain, using your knowledge of structure and bonding, why carbonyl fluoride has a low
melting point.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
© UCLES 2020
[Total: 13]
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5
3
(a) Sulfuric acid is made from sulfur in a four-stage process.
stage 1
Sulfur is converted into sulfur dioxide.
stage 2
Sulfur dioxide is converted into sulfur trioxide.
stage 3
Sulfur trioxide is converted into oleum.
stage 4
Oleum is converted into sulfuric acid.
(i)How is sulfur converted into sulfur dioxide in stage 1?
........................................................................................................................................ [1]
(ii)Describe how sulfur dioxide is converted into sulfur trioxide in stage 2.
Your answer should include:
●●
●●
●●
n equation for the reaction
a
the temperature used
the name of the catalyst used.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(iii)The reaction in stage 2 can reach equilibrium.
What is meant by the term equilibrium?
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(b) Sulfur trioxide is converted into oleum, H2S2O7, in stage 3.
What is sulfur trioxide reacted with to convert it into oleum?
............................................................................................................................................... [1]
(c) Oleum is converted into sulfuric acid in stage 4.
Write a chemical equation for the conversion of oleum, H2S2O7, into sulfuric acid.
............................................................................................................................................... [2]
© UCLES 2020
0620/42/M/J/20
[Turn over
6
(d)When copper is reacted with hot concentrated sulfuric acid, sulfur dioxide gas is formed.
Balance the chemical equation for this reaction.
Cu + .......H2SO4 → CuSO4 + SO2 + .......H2O
[1]
(e) Sulfur dioxide is a reducing agent.
ive the colour change that occurs when excess sulfur dioxide is bubbled into acidified aqueous
G
potassium manganate(VII).
starting colour of the solution ......................................................................................................
final colour of the solution ...........................................................................................................
[1]
(f)When sulfuric acid reacts with ammonia the salt produced is ammonium sulfate.
Write the chemical equation for this reaction.
............................................................................................................................................... [2]
(g)Barium sulfate is an insoluble salt.
Barium sulfate can be made from aqueous ammonium sulfate using a precipitation reaction.
(i)Name a solution that can be added to aqueous ammonium sulfate to produce a precipitate
of barium sulfate.
........................................................................................................................................ [1]
(ii)Write an ionic equation for this precipitation reaction. Include state symbols.
........................................................................................................................................ [2]
© UCLES 2020
[Total: 16]
0620/42/M/J/20
7
4
Oxygen is produced by the decomposition of hydrogen peroxide. Manganese(IV) oxide is the
catalyst for this reaction.
(a)What is meant by the term catalyst ?
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(b)
A student measures the volume of oxygen produced at regular time intervals using the
apparatus shown. Large lumps of manganese(IV) oxide are used.
gas syringe
manganese(IV) oxide
catalyst
aqueous hydrogen peroxide
A graph of the results is shown.
volume
of oxygen
produced
/ cm3
0
0
time / s
What happens to the rate of this reaction as time increases?
In your answer, explain why the rate changes in this way.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [4]
(c)
The experiment is repeated using the same mass of manganese(IV) oxide. Powdered
manganese(IV) oxide is used instead of large lumps. All other conditions stay the same.
Sketch a graph on the axes in (b) to show how the volume of oxygen changes with time. [2]
© UCLES 2020
0620/42/M/J/20
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8
(d)In terms of particles, explain what happens to the rate of this reaction when the temperature is
increased.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(e)The equation for the decomposition of hydrogen peroxide is shown.
2H2O2(aq) → 2H2O(l) + O2(g)
25.0 cm3 of aqueous hydrogen peroxide forms 48.0 cm3 of oxygen at room temperature and
pressure (r.t.p.).
Calculate the concentration of aqueous hydrogen peroxide at the start of the experiment using
the following steps.
●●
Calculate the number of moles of oxygen formed.
.............................. mol
●●
Deduce the number of moles of hydrogen peroxide that decomposed.
.............................. mol
●●
Calculate the concentration of hydrogen peroxide in mol / dm3.
.............................. mol / dm3
[3]
(f) Oxygen can also be produced by the decomposition of potassium chlorate(V), KCl O3.
The only products of this decomposition are potassium chloride and oxygen.
Write a chemical equation for this decomposition.
............................................................................................................................................... [2]
© UCLES 2020
[Total: 16]
0620/42/M/J/20
9
5
Electrolysis of concentrated aqueous sodium chloride using inert electrodes forms chlorine,
hydrogen and sodium hydroxide.
(a)What is meant by the term electrolysis?
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(b)Name a substance that can be used as the inert electrodes.
............................................................................................................................................... [1]
(c)Write an ionic half-equation for the formation of hydrogen during this electrolysis.
............................................................................................................................................... [1]
(d)Give the formulae of the four ions present in concentrated aqueous sodium chloride.
............................................................................................................................................... [2]
(e)Explain how sodium hydroxide is formed during this electrolysis.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2020
[Total: 8]
0620/42/M/J/20
[Turn over
10
6
(a)Propane reacts with chlorine in a photochemical reaction as shown.
C3H8 + Cl 2 → C3H7Cl + HCl
(i)What type of reaction is this?
........................................................................................................................................ [1]
(ii)What condition is needed for this photochemical reaction to occur?
........................................................................................................................................ [1]
(iii)Draw two structural isomers of compounds with the formula C3H7Cl.
Show all of the atoms and all of the bonds.
[2]
(b)Propene reacts with chlorine in an addition reaction as shown.
C3H6 + Cl 2 → C3H6Cl 2
(i)
State why this is an addition reaction.
........................................................................................................................................ [1]
© UCLES 2020
0620/42/M/J/20
11
(ii)The structures of the reactants and products of this reaction are shown.
H
H
H
H
C
C
C
H
+
Cl
Cl
→
H
H
H
H
H
C
C
C
H
Cl
Cl
H
Some bond energies are shown in the table.
bond
bond energy
in kJ / mol
C–C
347
C=C
612
C–H
413
C–Cl
339
Cl –Cl
242
Calculate the energy change for the reaction between propene and chlorine using the
following steps.
●●
Calculate the energy needed to break the bonds.
.............................. kJ
●●
Calculate the energy released when bonds are formed.
.............................. kJ
●●
Calculate the energy change for the reaction between propene and chlorine.
.............................. kJ / mol
[3]
© UCLES 2020
0620/42/M/J/20
[Turn over
12
(c)There are three functional groups in compound A.
compound A
COOH CH2OH
C
C
H
H
(i)Name the homologous series of compounds that contains the following structures.
C=C .....................................................................................................................................
–OH .....................................................................................................................................
–COOH ................................................................................................................................
[3]
(ii)What would you observe when compound A is added to:
aqueous bromine .................................................................................................................
aqueous sodium carbonate? ...............................................................................................
[2]
(d)Compound A can be used as a single monomer to produce two different polymers.
(i)Draw one repeat unit of the addition polymer formed from compound A.
[2]
(ii)What type of condensation polymer is formed from compound A?
........................................................................................................................................ [1]
© UCLES 2020
[Total: 16]
0620/42/M/J/20
13
BLANK PAGE
© UCLES 2020
0620/42/M/J/20
14
BLANK PAGE
© UCLES 2020
0620/42/M/J/20
15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/42/M/J/20
© UCLES 2020
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/M/J/20
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
May/June 2020
45 minutes
You must answer on the multiple choice answer sheet.
*8601179553*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
• There are forty questions on this paper. Answer all questions.
• For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
• Follow the instructions on the multiple choice answer sheet.
• Write in soft pencil.
• Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
• Do not use correction fluid.
• Do not write on any bar codes.
• You may use a calculator.
INFORMATION
• The total mark for this paper is 40.
• Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
• Any rough working should be done on this question paper.
• The Periodic Table is printed in the question paper.
This document has 16 pages. Blank pages are indicated.
IB20 06_0620_22/2RP
© UCLES 2020
[Turn over
2
1
A mixture of ice and water is left to stand and the ice melts.
Which row describes what happens as the ice is melting?
2
temperature of mixture
energy changes
A
increases
average kinetic energy of particles increases
B
increases
energy is used to overcome attractive forces
C
stays the same
average kinetic energy of particles increases
D
stays the same
energy is used to overcome attractive forces
Which piece of apparatus is used to measure 25.0 cm3 of aqueous sodium hydroxide?
A
3
B
C
D
Paper chromatography is used to determine the Rf values for four different food colourings.
Which food colouring has an Rf value of 0.6?
solvent front
25
20
distance
/ cm
15
10
5
baseline
0
A
© UCLES 2020
B
C
0620/22/M/J/20
D
3
4
The diagram shows the electronic structure of a particle with a nucleon number (mass number) of
40.
e e
e e
e
e e
e e
e e
e e
40
e
e e
e e
The table shows the suggestions that three students, 1, 2 and 3, made to identify the particle.
student
particle
1
2
3
Ar
Cl
Ca2+
Which students are correct?
A
5
1 and 2 only
B
1 and 3 only
C
2 and 3 only
D
1, 2 and 3
The electronic structures of two atoms, P and Q, are shown.
P
Q
P and Q combine together to form a compound.
What is the type of bonding in the compound and what is the formula of the compound?
type of bonding
formula
A
ionic
PQ
B
ionic
PQ2
C
covalent
PQ2
D
covalent
PQ
© UCLES 2020
0620/22/M/J/20
[Turn over
4
6
7
Which statement about the structure of a metal explains why metals are malleable?
A
The electrons can move freely throughout the lattice.
B
The layers of metal ions can slide over each other.
C
The metal ions are positively charged.
D
There is a strong force of attraction between the metal ions and the electrons.
The bonding, structure and melting point of sodium chloride and sulfur dichloride are shown.
compound
bonding
structure
melting point / °C
sodium chloride
ionic
giant lattice
801
sulfur dichloride
covalent
simple molecular
–121
Why does sulfur dichloride have a lower melting point than sodium chloride?
8
A
The covalent bonds in sulfur dichloride are weaker than the attractive forces between
molecules in sodium chloride.
B
The covalent bonds in sulfur dichloride are weaker than the ionic bonds in sodium chloride.
C
The attractive forces between molecules in sulfur dichloride are weaker than the attractive
forces between molecules in sodium chloride.
D
The attractive forces between molecules in sulfur dichloride are weaker than the ionic bonds
in sodium chloride.
Lead(II) nitrate, Pb(NO3)2, reacts with potassium iodide, KI, to form a yellow precipitate, PbI2,
and a soluble salt, KNO3.
What is the equation for the reaction?
9
A
Pb(NO3)2 + KI → PbI2 + KNO3
B
Pb(NO3)2 + 2KI → PbI2 + KNO3
C
2Pb(NO3)2 + 2KI → PbI2 + 2KNO3
D
Pb(NO3)2 + 2KI → PbI2 + 2KNO3
The Haber process is a reversible reaction.
N2(g) + 3H2(g)
2NH3(g)
The reaction has a 30% yield of ammonia.
Which volume of ammonia gas, NH3, measured at room temperature and pressure, is obtained
by reacting 0.75 moles of hydrogen with excess nitrogen?
A
3600 cm3
© UCLES 2020
B
5400 cm3
C
12 000 cm3
0620/22/M/J/20
D
18 000 cm3
5
10 Electrolytes can be broken down by electrolysis.
Which rows are correct for each electrolyte?
1
2
A
electrolyte
reaction
at cathode
product
at anode
dilute aqueous sodium chloride
2H+ + 2e– → H2
oxygen
+
2H + 2e → H2
concentrated hydrochloric acid
3
molten aluminium oxide
4
concentrated aqueous sodium bromide
1 and 2
B
1 and 4
C
–
2O
2–
→ O2 + 4e
–
chlorine
aluminium
Na+ + e– → Na
2 and 3
D
bromine
3 and 4
11 The electrolysis of aqueous copper(II) sulfate, using inert electrodes, is shown.
+
–
aqueous copper(II) sulfate
Which statement about a reaction at an electrode is correct?
A
Copper ions gain electrons at the negative electrode.
B
Copper ions gain electrons at the positive electrode.
C
Hydrogen ions gain electrons at the negative electrode.
D
Hydrogen ions gain electrons at the positive electrode.
© UCLES 2020
0620/22/M/J/20
[Turn over
6
12 Methane burns in excess oxygen.
The equation is shown.
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
Bond energies are shown.
bond
bond energy
/ kJ mol–1
C=O
805
C–H
410
O=O
496
O–H
460
What is the energy change for the reaction?
A
(4 × 410 + 2 × 496) – (2 × 805 + 4 × 460)
B
(2 × 805 + 2 × 460) – (410 + 2 × 496)
C
(410 + 2 × 496) – (805 + 2 × 460)
D
(410 + 496) – (805 + 460)
13 Which statements about hydrogen fuel cells are correct?
A
1
Water is formed as the only waste product.
2
Both water and carbon dioxide are formed as waste products.
3
The overall reaction is 2H2 + O2 → 2H2O.
4
The overall reaction is endothermic.
1 and 3
B
1 and 4
C
2 and 3
14 Which list contains only chemical changes?
A
melting, evaporating, dissolving
B
rusting, freezing, subliming
C
neutralisation, polymerisation, combustion
D
boiling, condensing, distillation
© UCLES 2020
0620/22/M/J/20
D
2 and 4
7
15 The results of adding excess marble chips (calcium carbonate) to hydrochloric acid at 50 °C and
at 30 °C are shown. Only the temperature is changed.
50 °C
volume of
carbon dioxide
given off / cm3
30 °C
0
0
time / s
Which row describes the reacting particles at 30 °C compared to those at 50 °C?
collision rate
collision energy
A
higher
higher
B
higher
lower
C
lower
higher
D
lower
lower
16 Methane reacts with steam and an equilibrium is reached.
CH4(g) + H2O(g)
CO(g) + 3H2(g)
The forward reaction is endothermic.
Which row shows how the amount of hydrogen at equilibrium changes when the pressure or
temperature is changed as indicated?
change in
temperature
change in
pressure
amount of
hydrogen
A
decrease
no change
increase
B
increase
no change
decrease
C
no change
increase
decrease
D
no change
decrease
decrease
© UCLES 2020
0620/22/M/J/20
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8
17 When aqueous iron(III) chloride is added to aqueous potassium iodide a chemical reaction
occurs and iodine is formed.
Which statement is correct?
A
Iodide ions are oxidised, they gain electrons in this reaction.
B
Iodide ions are oxidised, they lose electrons in this reaction.
C
Iron(III) chloride is oxidised in this reaction.
D
Neither iodide ions nor iron(III) chloride is oxidised in this reaction.
18 The graph shows how the pH of a solution changes as an acid is added to an alkali.
acid + alkali → salt + water
Which letter represents the area of the graph where both acid and salt are present?
14
pH
A
B
C
7
D
0
volume of acid added
19 Which statement describes a weak acid?
A
It is a proton acceptor and is fully ionised in aqueous solution.
B
It is a proton acceptor and is partially ionised in aqueous solution.
C
It is a proton donor and is fully ionised in aqueous solution.
D
It is a proton donor and is partially ionised in aqueous solution.
© UCLES 2020
0620/22/M/J/20
9
20 The apparatus shown is used to prepare aqueous copper(II) sulfate.
filter paper
stirrer
excess of solid X
solid X
aqueous
copper(II) sulfate
Y
heat
What are X and Y?
X
Y
A
copper
aqueous iron(II) sulfate
B
copper(II) chloride
dilute sulfuric acid
C
copper(II) oxide
dilute sulfuric acid
D
sulfur
aqueous copper(II) chloride
21 Which process is not used in the preparation of an insoluble salt?
A
filtration
B
washing
C
crystallisation
D
drying
22 Which statement about Group I and Group VII elements is correct?
A
Group VII elements are monoatomic non-metals.
B
Lithium is more reactive with water than caesium.
C
The melting points of Group I metals increase down the group.
D
Potassium bromide reacts with chlorine to produce an orange solution.
© UCLES 2020
0620/22/M/J/20
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10
23 The properties of the element titanium, Ti, can be predicted from its position in the Periodic Table.
Which row identifies the properties of titanium?
can be used
as a catalyst
conducts electricity
when solid
has low density
forms coloured
compounds
A
B
C
D
24 Which diagram shows a mixture of noble gases?
A
B
C
D
25 Which property is shown by all metals?
A
They are extracted from their ores by heating with carbon.
B
They conduct electricity.
C
They form acidic oxides.
D
They react with hydrochloric acid to form hydrogen.
26 Many metal carbonates decompose when they are heated.
Which row describes what happens when potassium carbonate, calcium carbonate and
copper(II) carbonate are heated using a Bunsen burner?
decomposes easily
decomposes
with difficulty
does not decompose at
Bunsen temperatures
A
calcium carbonate
copper(II) carbonate
potassium carbonate
B
copper(II) carbonate
calcium carbonate
potassium carbonate
C
copper(II) carbonate
potassium carbonate
calcium carbonate
D
potassium carbonate
calcium carbonate
copper(II) carbonate
© UCLES 2020
0620/22/M/J/20
11
27 Molten iron from the blast furnace contains impurities.
The process of turning the impure iron into steel involves blowing oxygen into the molten iron and
adding calcium oxide.
What are the reasons for blowing in oxygen and adding calcium oxide?
blowing in oxygen
adding calcium oxide
A
carbon is removed by reacting with oxygen
reacts with acidic impurities making slag
B
carbon is removed by reacting with oxygen
reacts with slag and so removes it
C
iron reacts with the oxygen
reacts with acidic impurities making slag
D
iron reacts with the oxygen
reacts with slag and so removes it
28 Four iron nails are added to four different metal sulfate solutions.
In which solution does a displacement reaction occur?
A
copper(II) sulfate
B
magnesium sulfate
C
sodium sulfate
D
zinc sulfate
29 Which statement about pure water is not correct?
A
It condenses at 100 °C.
B
It freezes at 0 °C.
C
It turns cobalt(II) chloride paper blue.
D
It turns anhydrous copper(II) sulfate blue.
© UCLES 2020
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12
30 Three processes in the carbon cycle are shown.
1
Methane reacts with oxygen producing carbon dioxide and water.
2
Carbon dioxide and water are absorbed and used by plants to make oxygen.
3
Oxygen is used by living things to release energy.
Which processes have taken place?
1
2
3
A
combustion
photosynthesis
respiration
B
combustion
respiration
photosynthesis
C
photosynthesis
combustion
respiration
D
respiration
photosynthesis
combustion
31 In the Haber process, nitrogen and hydrogen are reacted to make ammonia.
N2(g) + 3H2(g)
2NH3(g)
The forward reaction is exothermic.
Which conditions produce the maximum yield of ammonia?
pressure
temperature
A
high
high
B
high
low
C
low
high
D
low
low
32 Which process, used to prevent iron from rusting, involves sacrificial protection?
A
alloying
B
electroplating
C
galvanising
D
painting
© UCLES 2020
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13
33 A student suggests three uses of calcium carbonate (limestone).
1
manufacture of cement
2
manufacture of iron
3
treating alkaline soils
Which suggestions are correct?
A
1 and 2 only
B
1 and 3 only
C
2 and 3 only
D
1, 2 and 3
34 One of the reactions used in the manufacture of sulfuric acid is shown.
2SO2 + O2
2SO3
Which catalyst is used to increase the rate of this reaction?
A
iron
B
manganese(IV) oxide
C
vanadium(V) oxide
D
nickel
35 Ethanol is made on an industrial scale by the fermentation of sugars or by the reaction of ethene
with steam in the presence of a suitable catalyst.
What is a disadvantage of making ethanol from ethene rather than by fermentation?
A
A continuous production process is used.
B
A non-renewable raw material is used.
C
The product is very pure.
D
The rate of reaction is very high.
36 Which statement about compounds in the same homologous series is correct?
A
They have the same chemical properties because they have the same number of carbon
atoms.
B
They have the same physical properties because they have the same number of carbon
atoms.
C
They have different chemical properties because they have different numbers of carbon
atoms.
D
They have different physical properties because they have different numbers of carbon
atoms.
© UCLES 2020
0620/22/M/J/20
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14
37 Increasing the number of atoms in one molecule of a hydrocarbon increases the amount of
energy released when it burns.
What is the correct order?
more energy
released
less energy
released
A
ethene
ethane
methane
B
ethene
methane
ethane
C
methane
ethane
ethene
D
methane
ethene
ethane
38 An organic compound, P, reacts with zinc to produce a gas, Q.
What are P and Q?
P
Q
A
ethanoic acid
carbon dioxide
B
ethanoic acid
hydrogen
C
ethanol
carbon dioxide
D
ethanol
hydrogen
39 Alkanes undergo substitution reactions in the presence of UV light.
Which equation represents a substitution reaction of ethane?
A
C2H6 + Cl 2 → C2H4 + 2HCl
B
C2H6 + Cl 2 → C2H5Cl + HCl
C
C2H6 + Cl 2 → C2H4Cl 2 + H2
D
C2H6 + HCl → C2H5Cl + H2
40 Which substances are natural polymers?
A
1
proteins
2
carbohydrates
3
nylon
4
poly(ethene)
1 and 2
© UCLES 2020
B
1 and 3
C
2 and 3
0620/22/M/J/20
D
3 and 4
15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/22/M/J/20
© UCLES 2020
21
39
Y
12
Mg
magnesium
24
20
Ca
calcium
40
38
11
Na
sodium
23
19
K
potassium
39
37
22
73
Ta
72
Hf
89
57–71
lanthanoids
88
56
0620/22/M/J/20
Th
thorium
232
–
90
89
Ac
140
139
actinium
Ce
cerium
La
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
57
lanthanum
–
dubnium
Db
105
181
tantalum
–
rutherfordium
Rf
104
178
hafnium
93
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
Cr
24
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
Pt
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
49
70
gallium
Ga
31
27
aluminium
Si
14
13
Al
12
carbon
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
Group
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
–
actinoids
Ra
radium
88
87
Fr
137
133
francium
89–103
Ba
barium
Cs
caesium
91
Nb
niobium
55
Zr
zirconium
85
yttrium
Sr
strontium
41
51
vanadium
V
Rb
40
48
titanium
Ti
23
relative atomic mass
rubidium
45
scandium
Sc
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
*2018500414*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
May/June 2021
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working and use appropriate units.
INFORMATION
●● The total mark for this paper is 40.
●● The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Any blank pages are indicated.
IB21 06_0620_62/RP
© UCLES 2021
[Turn over
2
1Barium sulfate is an insoluble salt. Barium sulfate can be made by reacting excess aqueous
sodium sulfate with aqueous barium chloride.
sodium sulfate + barium chloride → sodium chloride + barium sulfate
A student made a sample of barium sulfate using the following steps.
step 1
aqueous
sodium sulfate
step 2
step 3
residue of solid
barium sulfate
A
stir
B
aqueous
barium chloride
excess aqueous
sodium sulfate was added
to aqueous barium chloride
the mixture
was stirred
the solid barium sulfate was
removed from the mixture
(a)Name the items of apparatus labelled A and B.
A .................................................................................................................................................
B .................................................................................................................................................
[2]
(b)Name the process shown in step 3.
............................................................................................................................................... [1]
(c)The general name for the solid in step 3 is residue.
State the general name for the solution obtained from the process in step 3.
............................................................................................................................................... [1]
© UCLES 2021
0620/62/M/J/21
3
(d)Two more steps, step 4 and step 5, are needed to obtain a pure sample of barium sulfate. In
each of these steps something is removed from the residue.
State what is done in each of step 4 and step 5 and identify the substance removed from the
barium sulfate.
step 4 .........................................................................................................................................
.....................................................................................................................................................
substance removed ....................................................................................................................
step 5 .........................................................................................................................................
.....................................................................................................................................................
substance removed ....................................................................................................................
[4]
© UCLES 2021
[Total: 8]
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[Turn over
4
BLANK PAGE
© UCLES 2021
0620/62/M/J/21
5
2
A student investigated the volume of gas made when sodium carbonate reacts with dilute
hydrochloric acid.
Five experiments were carried out using the apparatus shown.
rubber delivery tube
clamp
bung
inverted 100 cm3
measuring cylinder
boiling tube
trough
water
Experiment 1
●● Using a measuring cylinder, 16 cm3 of dilute hydrochloric acid was poured into a boiling tube.
●● The apparatus was set up as shown in the diagram.
●● The bung was removed from the boiling tube.
●● 2.5 g of sodium carbonate was added to the boiling tube and the bung was immediately
replaced.
●● When no more gas was being collected, the volume of gas in the measuring cylinder was
measured.
Experiment 2
●● Experiment 1 was repeated using 14 cm3 of dilute hydrochloric acid instead of 16 cm3.
Experiment 3
●● Experiment 2 was repeated using 12 cm3 of dilute hydrochloric acid instead of 14 cm3.
Experiment 4
●● Experiment 3 was repeated using 10 cm3 of dilute hydrochloric acid instead of 12 cm3.
Experiment 5
●● Experiment 4 was repeated using 6 cm3 of dilute hydrochloric acid instead of 10 cm3.
© UCLES 2021
0620/62/M/J/21
[Turn over
6
(a)Use the information in the description of the experiments and the inverted measuring cylinder
diagrams to complete the table.
experiment
volume of dilute
hydrochloric acid / cm3
inverted measuring
cylinder diagram
volume of gas
collected / cm3
40
50
1
60
40
50
2
60
40
50
3
60
30
40
4
50
20
30
5
40
[3]
© UCLES 2021
0620/62/M/J/21
7
(b)Write a suitable scale on the y-axis and plot the results from Experiments 1 to 5 on the grid.
Draw a straight line of best fit.
volume of
gas collected
/ cm3
4
6
8
10
12
14
16
volume of dilute hydrochloric acid / cm3
[4]
(c) (i)
From your graph, deduce the volume of gas that would be collected if 7 cm3 of dilute
hydrochloric acid was used.
Show clearly on the grid how you worked out your answer.
.............................. cm3
[2]
(ii)The volume of gas made per cm3 of dilute hydrochloric acid can be calculated using the
equation shown.
volume of gas per cm3 of acid =
volume of gas collected in cm3
volume of acid in cm3
Use this equation and your answer to (c)(i) to calculate the volume of gas made per cm3
of dilute hydrochloric acid.
© UCLES 2021
.............................. [1]
0620/62/M/J/21
[Turn over
8
(d)The bung was removed and then replaced immediately after the sodium carbonate was added
to the boiling tube.
(i)Explain why the bung must be replaced immediately after the sodium carbonate is added
to the boiling tube.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Explain how the apparatus could be altered so that the bung does not have to be removed.
You may draw a diagram to explain your answer.
..............................................................................................................................................
........................................................................................................................................ [2]
(e)State one advantage of using a burette rather than a measuring cylinder to measure the
volume of the dilute hydrochloric acid.
............................................................................................................................................... [1]
(f)In Experiments 1 to 5, the sodium carbonate was in excess.
Sketch on the grid the graph you would expect if all of the experiments were repeated using
dilute hydrochloric acid of half the concentration.
Label your line F.[2]
© UCLES 2021
[Total: 16]
0620/62/M/J/21
9
3Solution G and solid H were analysed.
tests on solution G
tests
observations
Solution G was divided into three equal portions
in three test‑tubes.
test 1
Sodium hydroxide was added dropwise and
then in excess to the first portion of solution G.
white precipitate which did not
dissolve in excess
test 2
About 1 cm3 of dilute nitric acid followed by a
few drops of aqueous silver nitrate were added
to the second portion of solution G.
yellow precipitate
test 3
About 10 cm3 of aqueous hydrogen peroxide
was added to the third portion of solution G.
The gas produced was tested.
the mixture became brown and bubbled;
the gas relit a glowing splint
(a)Identify the gas produced in test 3.
............................................................................................................................................... [1]
(b)Use the results of test 1 and test 2 to identify solution G.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2021
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10
tests on solid H
Solid H was hydrated copper(II) sulfate.
Complete the expected observations.
(c)About half of solid H was placed in a boiling tube and heated using a Bunsen burner.
observations ...............................................................................................................................
............................................................................................................................................... [2]
(d)A flame test was carried out on solid H.
observations ......................................................................................................................... [1]
The remaining solid H was placed in a boiling tube. About 10 cm3 of distilled water was added to the
boiling tube. The tube was shaken to dissolve solid H and form solution H.
Solution H was divided into two approximately equal portions in two test‑tubes.
(e)Aqueous ammonia was added dropwise and then in excess to the first portion of solution H.
observations ...............................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(f)Approximately 1 cm3 of dilute nitric acid followed by a few drops of aqueous barium nitrate were
added to the second portion of solution H.
observations ......................................................................................................................... [1]
© UCLES 2021
[Total: 10]
0620/62/M/J/21
11
4The mineral epsomite contains hydrated magnesium sulfate. When epsomite is heated strongly, it
loses water and eventually becomes anhydrous magnesium sulfate.
Plan an investigation to find the percentage by mass of water in a sample of epsomite. Your plan
should include how you would calculate the percentage by mass of water in epsomite.
You have access to common laboratory apparatus.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
© UCLES 2021
0620/62/M/J/21
[Turn over
12
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/62/M/J/21
Cambridge IGCSE™
*9904169354*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
May/June 2021
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 80.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB21 06_0620_42/2RP
© UCLES 2021
[Turn over
2
1The symbols of the elements of Period 3 of the Periodic Table are shown.
Na
Mg
Al
Si
P
S
Cl
Ar
Answer the following questions about these elements.
Each element may be used once, more than once or not at all.
Write the symbol of an element which:
(a)is malleable
............................................................................................................................................... [1]
(b)has only two electrons in its outermost shell
............................................................................................................................................... [1]
(c)forms an oxide which leads to acid rain
............................................................................................................................................... [1]
(d)forms an ion with a 2– charge
............................................................................................................................................... [1]
(e)is extracted from an ore called bauxite
............................................................................................................................................... [1]
(f)does not form an oxide
............................................................................................................................................... [1]
(g)forms an oxide with a macromolecular structure
............................................................................................................................................... [1]
(h)forms an amphoteric oxide
............................................................................................................................................... [1]
(i) exists as diatomic molecules
............................................................................................................................................... [1]
(j)forms a binary compound with hydrogen that is a strong acid.
............................................................................................................................................... [1]
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2Silver has an atomic number of 47.
(a)Naturally occurring atoms of silver are 107Ag and 109Ag.
(i)
State the name given to atoms of the same element with different nucleon numbers.
........................................................................................................................................ [1]
(ii)Complete the table to show the number of protons, neutrons and electrons in each atom
and ion of silver shown.
107
47Ag
109
+
47Ag
protons
neutrons
electrons
[3]
(iii)
Complete this definition of relative atomic mass.
Relative atomic mass is the ............................... mass of naturally occurring atoms
of an element on a scale where the ............................... atom has a mass of exactly
............................... units.
[3]
(iv)A sample of silver has a relative atomic mass of 108.0.
Deduce the percentage of 107Ag present in this sample of silver.
........................................................................................................................................ [1]
(b)Silver nitrate is a salt of silver made by reacting silver oxide with an acid.
Write the formula of the acid which reacts with silver oxide to form silver nitrate.
............................................................................................................................................... [1]
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4
(c)Aqueous silver nitrate is a colourless solution containing Ag+(aq) ions.
(i)Describe what is seen when aqueous silver nitrate is added to aqueous sodium iodide,
NaI(aq).
........................................................................................................................................ [1]
(ii)Write the ionic equation for the reaction between aqueous silver nitrate and aqueous
sodium iodide.
Include state symbols.
........................................................................................................................................ [3]
(d)In the positive test for aqueous nitrate ions, aqueous sodium hydroxide and one other substance
are warmed with the nitrate ions.
Name this other substance and the gas formed.
name of substance .....................................................................................................................
name of gas ................................................................................................................................
[2]
(e)When silver nitrate is exposed to sunlight, silver is formed.
Name the type of reaction which needs light to make it happen.
............................................................................................................................................... [1]
(f)Members of one homologous series only react with chlorine in the presence of sunlight.
(i)Name a member of this homologous series.
........................................................................................................................................ [1]
(ii)Name two products that form when the compound in (i) reacts with chlorine.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
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3Sodium hydrogencarbonate is found in baking powder.
When sodium hydrogencarbonate is heated it forms three products.
2NaHCO3 → Na2CO3 + H2O + CO2
(a)Name the type of reaction that takes place when sodium hydrogencarbonate reacts in this way.
............................................................................................................................................... [1]
(b)Calculate the volume of carbon dioxide formed at room temperature and pressure when 12.6 g
of NaHCO3 is heated using the following steps:
●
determine the mass of one mole of NaHCO3
.............................. g
●
calculate the number of moles of NaHCO3 used
.............................. moles
●
determine the number of moles of carbon dioxide formed
.............................. moles
●
calculate the volume of carbon dioxide formed at room temperature and pressure.
.............................. dm3
[4]
(c)Limewater is aqueous calcium hydroxide. Carbon dioxide turns limewater milky because a
white precipitate forms.
Write the formula of:
●
calcium hydroxide ................................................................................................................
● the white precipitate that forms when limewater turns milky. ...............................................
[2]
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4A student carries out an electrolysis experiment using the apparatus shown.
wire
+
–
carbon electrodes
dilute aqueous
sodium chloride
The student uses dilute aqueous sodium chloride.
(a)State the name given to any solution which undergoes electrolysis.
............................................................................................................................................... [1]
(b)Hydroxide ions are discharged at the anode.
(i)Complete the ionic half-equation for this reaction.
..........OH–(aq) → ........................... + O2(g) + 4e–[2]
(ii)Explain how the ionic half-equation shows the hydroxide ions are being oxidised.
........................................................................................................................................ [1]
(c)Describe what the student observes at the cathode.
............................................................................................................................................... [1]
(d)Write the ionic half-equation for the reaction at the cathode.
............................................................................................................................................... [2]
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(e)The student repeats the experiment using concentrated aqueous sodium chloride.
(i)Describe what the student observes at:
●
the cathode ...................................................................................................................
● the anode. .....................................................................................................................
[2]
(ii)The student added litmus to the solution after the electrolysis of concentrated aqueous
sodium chloride.
State the colour seen in the solution. Give a reason for your answer.
colour of solution .................................................................................................................
reason ..................................................................................................................................
[2]
(f)Carbon electrodes are used because they are inert.
State another element that can be used instead of carbon.
............................................................................................................................................... [1]
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8
5This question is about compounds of nitrogen.
(a)Nitrogen reacts with lithium to form lithium nitride, Li3N.
(i)Write the chemical equation for the reaction between lithium and nitrogen.
........................................................................................................................................ [2]
(ii)Lithium nitride is ionically bonded.
Complete the diagram to show the electronic structure of the nitride ion.
Show the charge on the nitride ion.
........
N
[2]
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9
(b) Nitrogen reacts with fluorine to form nitrogen trifluoride, NF3.
(i)The chemical equation can be represented as shown.
N≡N + 3 F–F 2 F–N–F
F
Some bond energies are shown in the table.
bond
bond energy in kJ / mol
N≡N
945
F–F
160
N–F
300
alculate the energy change for the reaction between nitrogen and fluorine, using the
C
following steps:
●
energy taken in to break bonds
.............................. kJ
●
energy released when bonds are formed
.............................. kJ
●
energy change during the reaction.
.............................. kJ / mol
[3]
(ii)
se your answer to (i) to deduce whether this reaction is endothermic or exothermic.
U
Explain your answer.
..............................................................................................................................................
........................................................................................................................................ [1]
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(iii)Complete the dot-and-cross diagram to show the electron arrangement in a molecule of
NF3.
Use dots for nitrogen electrons and crosses for fluorine electrons.
Show outer electrons only.
F
N
F
F
[3]
(c)Lithium nitride melts at 813 °C. Nitrogen trifluoride melts at –206 °C.
Explain in terms of attractive forces why lithium nitride has a much higher melting point than
nitrogen trifluoride.
In your answer refer to the types of attractive forces between particles and their relative
strengths.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(d)Ammonium nitrate, NH4NO3, is a compound of nitrogen.
(i)Calculate the percentage by mass of nitrogen in ammonium nitrate.
percentage by mass of nitrogen = .............................. [2]
(ii)State a use of ammonium nitrate in agriculture.
........................................................................................................................................ [1]
(iii)State the name of a compound that will displace ammonia from ammonium nitrate.
........................................................................................................................................ [1]
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11
(e)Ammonia is a base which forms a weakly alkaline solution when dissolved in water.
(i)
Define the term base.
........................................................................................................................................ [1]
(ii)Suggest the pH of aqueous ammonia.
........................................................................................................................................ [1]
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6Molecules A and B can form condensation polymers.
A
HO
B
OH
HOOC
COOH
(a)Each molecule has two identical functional groups.
(i)Name the functional group in B.
........................................................................................................................................ [1]
(ii)Draw the part of the structure of the synthetic polymer that would form when two molecules
of A and two molecules of B combine. Show all of the bonds in the linkages.
[3]
(iii)Name the other product formed when molecules of A and B undergo polymerisation.
........................................................................................................................................ [1]
(b)Molecule A is a simple sugar unit which can be made by hydrolysis of complex carbohydrates.
(i)Draw part of the complex carbohydrate that could be hydrolysed to make molecules of A.
Include one linkage and show all of the bonds in the linkage.
[1]
(ii)State two sets of conditions which could be used to hydrolyse the complex carbohydrate
to form A.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(iii)Name the technique used to identify the individual sugar units made by the hydrolysis of a
complex carbohydrate.
........................................................................................................................................ [1]
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13
(c)Ethanol can be made from the simple sugar glucose, C6H12O6.
(i)State the name of this process.
........................................................................................................................................ [1]
(ii)Complete the chemical equation for this reaction.
C6H12O6 →[2]
© UCLES 2021
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14
BLANK PAGE
© UCLES 2021
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15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/42/M/J/21
© UCLES 2021
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/M/J/21
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
May/June 2021
45 minutes
You must answer on the multiple choice answer sheet.
*4675923471*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
• There are forty questions on this paper. Answer all questions.
• For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
• Follow the instructions on the multiple choice answer sheet.
• Write in soft pencil.
• Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
• Do not use correction fluid.
• Do not write on any bar codes.
• You may use a calculator.
INFORMATION
• The total mark for this paper is 40.
• Each correct answer will score one mark.
• Any rough working should be done on this question paper.
• The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB21 06_0620_22/3RP
© UCLES 2021
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1
A gas is released at point P in the apparatus shown.
P
damp universal indicator paper
Which gas turns the damp universal indicator paper red most quickly?
2
A
ammonia, NH3
B
chlorine, Cl 2
C
hydrogen chloride, HCl
D
sulfur dioxide, SO2
A mixture of colourless compounds is separated using chromatography.
Which type of reagent is used to detect these compounds after separation?
3
4
A
a dehydrating agent
B
a locating agent
C
an oxidising agent
D
a reducing agent
Which statement about paper chromatography is correct?
A
A solvent is needed to dissolve the paper.
B
Paper chromatography separates mixtures of solvents.
C
The solvent should cover the baseline.
D
The baseline should be drawn in pencil.
Element X has 7 protons.
Element Y has 8 more protons than X.
Which statement about element Y is correct?
A
Y has more electron shells than X.
B
Y has more electrons in its outer shell than X.
C
Y is in a different group of the Periodic Table from X.
D
Y is in the same period of the Periodic Table as X.
© UCLES 2021
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3
5
A covalent molecule Q contains only six shared electrons.
What is Q?
6
A
ammonia, NH3
B
chlorine, Cl 2
C
methane, CH4
D
water, H2O
Information about four substances E, F, G and H is shown.
melting point / °C
electrical conductivity
E
1710
does not conduct when solid
F
3500
conducts when solid
G
120
does not conduct
H
801
conducts when molten
E, F, G and H are graphite, poly(ethene), sodium chloride and silicon(IV) oxide but not in that
order.
What are E, F, G and H?
7
E
F
G
H
A
graphite
poly(ethene)
silicon(IV) oxide
sodium chloride
B
sodium chloride
graphite
poly(ethene)
silicon(IV) oxide
C
poly(ethene)
sodium chloride
graphite
silicon(IV) oxide
D
silicon(IV) oxide
graphite
poly(ethene)
sodium chloride
Chemical compounds formed from a Group I element and a Group VII element contain ionic
bonds.
How are the ionic bonds formed?
A
Electrons are transferred from Group VII atoms to Group I atoms.
B
Electrons are shared between Group I atoms and Group VII atoms.
C
Electrons are lost by Group I atoms and Group VII atoms.
D
Electrons are transferred from Group I atoms to Group VII atoms.
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8
Some information about particles P, Q, R and S is shown.
nucleon
number
number of
neutrons
number of
electrons
P
12
6
6
Q
24
12
10
R
16
8
10
S
14
8
6
Which two particles are isotopes of the same element?
A
9
P and Q
B
P and S
C
Q and R
D
R and S
D
30
Chlorine gas will react with iron metal.
Exactly 21.3 g of chlorine reacts with 11.2 g of iron.
How many iron atoms react with 30 molecules of chlorine?
A
10
B
15
C
20
10 In separate experiments, electricity was passed through concentrated aqueous sodium chloride
and molten lead(II) bromide.
What would happen in both experiments?
A
A halogen would be formed at the anode.
B
A metal would be formed at the cathode.
C
Hydrogen would be formed at the anode.
D
Hydrogen would be formed at the cathode.
11 A reaction involving aluminium is shown.
xAl + yO2 + 6H2O → xAl (OH)3
Which values of x and y balance the equation?
x
y
A
2
3
B
3
2
C
3
4
D
4
3
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5
12 Four different fuels are used to heat a beaker of water, for the same amount of time, using the
apparatus shown.
thermometer
stirrer
screen to
reduce draughts
200 g of water
spirit burner
fuel
The initial temperature of the water and the temperature after heating by the fuel are recorded.
Which fuel releases the most heat energy?
initial temperature
/ °C
temperature after
heating / °C
A
17
46
B
24
52
C
26
61
D
30
62
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13 An excess of calcium carbonate reacts with dilute hydrochloric acid. The volume of
carbon dioxide produced is measured at regular time intervals. The results are shown as
experiment 1.
The experiment is repeated with only one change to the reaction conditions.
The results are shown as experiment 2.
experiment 2
experiment 1
volume
of CO2
time
Which change is made in experiment 2?
A
The concentration of the acid is increased.
B
The volume of acid is increased.
C
The mass of calcium carbonate is increased.
D
The calcium carbonate is powdered.
14 When sulfur is heated it undergoes a ......1...... change as it melts.
Further heating causes the sulfur to undergo a ......2...... change and form sulfur dioxide.
Which words complete gaps 1 and 2?
1
2
A
chemical
chemical
B
chemical
physical
C
physical
chemical
D
physical
physical
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7
15 Four statements about the effect of increasing temperature on a reaction are shown.
1
The activation energy becomes lower.
2
The particles move faster.
3
There are more collisions between reacting particles per second.
4
There are more collisions which have energy greater than the activation energy.
Which statements are correct?
A
1, 2 and 3
B
1, 3 and 4
C
2, 3 and 4
D
2 and 3 only
16 An example of a redox reaction is shown.
Zn + Cu2+ → Zn2+ + Cu
Which statement about the reaction is correct?
A
Zn is the oxidising agent and it oxidises Cu2+.
B
Zn is the oxidising agent and it reduces Cu2+.
C
Zn is the reducing agent and it oxidises Cu2+.
D
Zn is the reducing agent and it reduces Cu2+.
17 When bismuth(III) chloride, BiCl 3, reacts with water, a white precipitate of bismuth(III)
oxychloride, BiOCl, is formed. The equation for the reaction is shown.
BiOCl (s) + 2H+(aq) + 2Cl –(aq)
BiCl 3(aq) + H2O(l)
The reaction is in equilibrium.
Which changes cause the white precipitate to dissolve?
A
1
adding acid
2
adding water
3
adding sodium chloride solution
1 and 2 only
© UCLES 2021
B
1 and 3 only
C
2 and 3 only
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D
1, 2 and 3
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18 Element X forms an oxide, XO, that neutralises sulfuric acid.
Which row describes X and XO?
element X
nature of oxide, XO
A
metal
acidic
B
metal
basic
C
non-metal
acidic
D
non-metal
basic
19 Information about the solubility of salts is shown.
salt
solubility
chlorides
soluble (except for lead(II) chloride and silver chloride)
nitrates
soluble
sulfates
soluble (except for barium sulfate and lead(II) sulfate)
Aqueous solutions of which two compounds would produce a precipitate when added together?
A
Ba(NO3)2 and CaCl 2
B
CuSO4 and Zn(NO3)2
C
KCl and Na2SO4
D
Pb(NO3)2 and MgSO4
© UCLES 2021
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9
20 The equation shows the reaction between hydrogen and oxygen.
2 H–H + O=O → 2 H–O–H
The bond energies are shown.
bond energy
in kJ / mol
H–H
436
O=O
495
O–H
463
Which row shows the energy change and the type of reaction?
energy change
in kJ / mol
type of reaction
A
441
exothermic
B
441
endothermic
C
485
exothermic
D
485
endothermic
21 Burning fossil fuels releases sulfur dioxide which leads to acid rain.
Which ion in the rain water causes it to be acidic?
A
H+
B
OH–
C
O2–
D
SO42–
22 Which statement about the trends shown by the elements of Period 3 in the Periodic Table is not
correct?
A
The elements become less metallic across the period.
B
The group number increases across the period.
C
The number of electron shells increases across the period.
D
The number of outer electrons increases across the period.
© UCLES 2021
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23 The diagram shows the positions of elements E, F, G and H in the Periodic Table.
G
H
E
F
Which statements about elements E, F, G and H are correct?
A
1
E has a higher density than F.
2
E has a higher melting point than F.
3
G has a darker colour than H.
4
G has a lower melting point than H.
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
24 When aqueous iodine is added to a solution of vanadium ions, V2+, the V2+ ions each lose one
electron.
Which property of transition elements is shown by this reaction?
A
Transition elements have variable oxidation states.
B
Transition elements form a stable 1+ ion.
C
Transition elements are oxidising agents.
D
Transition elements can act as catalysts.
25 A piece of aluminium is dropped into dilute hydrochloric acid.
No immediate reaction is observed.
Which statement explains this observation?
A
Aluminium does not neutralise acids.
B
Aluminium is a non-metal so does not react with acids.
C
Aluminium is below hydrogen in the reactivity series.
D
Aluminium is covered in an unreactive oxide layer.
© UCLES 2021
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11
26 Some metal nitrates and carbonates decompose when heated strongly.
Metal Q has a nitrate that decomposes to give a salt and a colourless gas only.
The carbonate of metal Q does not decompose when heated with a Bunsen burner.
What is metal Q?
A
calcium
B
copper
C
sodium
D
zinc
27 Aluminium is extracted from its ore by electrolysis.
Which equation represents the reaction that occurs at the anode during the electrolysis?
A
Al 3+ + 3e– → Al
B
Al 3+ → Al + 3e–
C
2O2– → O2 + 4e–
D
2O2– + 2e– → O2
28 Mild steel consists mostly of iron. Mild steel can be prevented from rusting by a process called
galvanising.
Copper is not a very strong metal. However, if it is mixed with a suitable metal a strong alloy
called brass is produced.
Which statement is correct?
A
Copper corrodes very quickly when wet and brass does not.
B
Copper is mixed with zinc to produce brass.
C
Galvanising mild steel changes it from a pure metal into an alloy.
D
When a steel object is galvanised this means it is coated with a thin layer of tin.
29 Water is used for the irrigation of crops and for drinking water.
For which uses must water be chlorinated?
irrigation
drinking
A
B
C
D
© UCLES 2021
0620/22/M/J/21
[Turn over
12
30 Which natural resource cannot provide a raw material for the manufacture of ammonia?
A
air
B
limestone
C
petroleum
D
water
31 Ammonia is made in the Haber process.
Which conditions are used in the Haber process?
temperature
/ °C
pressure
/ atmospheres
catalyst used
A
450
200
iron
B
450
5
vanadium(V) oxide
C
200
450
iron
D
200
5
vanadium(V) oxide
32 Which process in the carbon cycle is responsible for removing carbon dioxide from the
atmosphere?
A
combustion
B
decomposition
C
photosynthesis
D
respiration
33 The equations represent two reactions, P and Q, of lime (calcium oxide).
P
CaO + SiO2 → CaSiO3
Q
CaO + SO2 → CaSO3
In which processes do the reactions occur?
P
Q
A
extraction of iron
extraction of iron
B
extraction of iron
flue gas desulfurisation
C
flue gas desulfurisation
extraction of iron
D
flue gas desulfurisation
flue gas desulfurisation
© UCLES 2021
0620/22/M/J/21
13
34 Which statement about ethanol is not correct?
A
Ethanol can be made by fermentation.
B
Ethanol is oxidised to make ethanoic acid.
C
Ethanol reacts with oxygen exothermically, making it a good fuel.
D
Ethanol reacts with propanoic acid to make propyl ethanoate.
35 Which pair of formulae represents two alkanes?
A
CH4 and C8H18
B
C2H6 and C5H8
C
C3H6 and C5H12
D
C10H8 and C4H8
36 Which statement about alkanes is correct?
A
They burn in oxygen.
B
They contain carbon, hydrogen and oxygen atoms.
C
They contain double bonds.
D
They contain ionic bonds.
37 Which statements about ethanoic acid are correct?
A
1
It is a strong acid.
2
It reacts with ethanol to form an ester.
3
It has the formula CH3COOH.
1 and 2 only
© UCLES 2021
B
1 and 3 only
C
2 and 3 only
0620/22/M/J/21
D
1, 2 and 3
[Turn over
14
38 The flow chart shows how petroleum may be turned into a plastic.
process
1
petroleum
saturated
hydrocarbon
process
2
unsaturated
hydrocarbon
process
3
plastic
What are processes 1, 2 and 3?
process 1
process 2
process 3
A
cracking
fractional distillation
polymerisation
B
cracking
polymerisation
fractional distillation
C
fractional distillation
cracking
polymerisation
D
fractional distillation
polymerisation
cracking
39 The structure of a synthetic polymer is shown.
O
O
C
C
N
N
H
H
O
O
C
C
O
N
N
H
H
C
The structure shows that it is a ......1...... . It is formed by ......2...... polymerisation.
Which words complete gaps 1 and 2?
1
2
A
polyamide
addition
B
polyamide
condensation
C
polyester
addition
D
polyester
condensation
40 Which substance is a natural polymer?
A
ethene
B
Terylene
C
nylon
D
protein
© UCLES 2021
0620/22/M/J/21
15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/22/M/J/21
© UCLES 2021
21
0620/22/M/J/21
calcium
40
38
Sr
strontium
88
56
Ba
barium
137
88
potassium
39
37
Rb
rubidium
85
55
Cs
caesium
133
87
22
cerium
140
90
Th
thorium
232
lanthanum
139
89
Ac
actinium
–
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
Ce
57
–
dubnium
Db
105
181
tantalum
Ta
73
93
niobium
Nb
41
51
vanadium
V
–
rutherfordium
Rf
104
178
hafnium
Hf
72
91
zirconium
Zr
40
48
titanium
La
lanthanoids
57–71
89
yttrium
Y
39
45
scandium
Ti
23
Cr
24
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
relative atomic mass
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Pt
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
49
70
gallium
Ga
31
27
aluminium
Al
13
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ca
K
–
actinoids
20
19
Ra
24
23
radium
magnesium
sodium
Fr
Mg
Na
francium
89–103
12
11
Sc
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
Group
The Periodic Table of Elements
16
Cambridge IGCSE™
*8853844180*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
October/November 2021
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 40.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Any blank pages are indicated.
IB21 11_0620_62/2RP
© UCLES 2021
[Turn over
2
1Carbon dioxide is a colourless gas that is denser than air.
Carbon dioxide can be made by reacting marble chips with dilute hydrochloric acid.
A student tried to make and collect carbon dioxide gas using the apparatus shown.
A
gas jar
C
B
(a) (i)Name the substances labelled A and B.
A ..........................................................................................................................................
B ..........................................................................................................................................
[1]
(ii)Name the item of apparatus labelled C.
........................................................................................................................................ [1]
(b)Explain why very little carbon dioxide gas would be collected using the apparatus shown.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2021
0620/62/O/N/21
3
(c)Complete the diagram to show how carbon dioxide gas could be collected and the volume
measured.
[2]
(d)At the end of the experiment there were unreacted marble chips and aqueous calcium chloride
in the item of apparatus labelled C.
Describe how you would find the mass of unreacted marble chips in apparatus C.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
© UCLES 2021
[Total: 9]
0620/62/O/N/21
[Turn over
4
2
student investigated the reaction between two different solutions of aqueous sodium carbonate,
A
solution K and solution L, and two different solutions of dilute hydrochloric acid, acid M and acid N.
Three experiments were done.
(a) Experiment 1
●
●
●
●
●
burette was filled with solution K. Some of solution K was run out of the burette so that
A
the level of solution K was on the burette scale.
Using a measuring cylinder 25 cm3 of acid M was poured into a conical flask.
Five drops of methyl orange indicator were added to the conical flask.
The conical flask was placed on a white tile.
Solution K was added slowly from the burette to the conical flask, while the flask was
swirled, until the solution just changed colour.
Use the burette diagrams to complete the table for Experiment 1.
7
31
8
32
9
33
initial reading
final reading
Experiment 1
final burette reading / cm3
initial burette reading / cm3
volume of solution K added / cm3
Experiment 2
●
●
●
●
●
●
© UCLES 2021
he conical flask was emptied and rinsed with distilled water.
T
The burette was refilled with solution K. Some of solution K was run out of the burette so
that the level of solution K was on the burette scale.
Using a measuring cylinder 25 cm3 of acid N was poured into the conical flask.
Five drops of methyl orange indicator were added to the conical flask.
The conical flask was placed on a white tile.
Solution K was added slowly from the burette to the conical flask, while the flask was
swirled, until the solution just changed colour.
0620/62/O/N/21
5
Use the burette diagrams to complete the table for Experiment 2.
3
15
4
16
5
17
initial reading
final reading
Experiment 2
final burette reading / cm3
initial burette reading / cm3
volume of solution K added / cm3
Experiment 3
●
●
●
●
●
●
●
he burette was emptied and rinsed with distilled water.
T
The conical flask was emptied and rinsed with distilled water.
The burette was filled with solution L. Some of solution L was run out of the burette so that
the level of solution L was on the burette scale.
Using a measuring cylinder 25 cm3 of acid N was poured into the conical flask.
Five drops of methyl orange indicator were added to the conical flask.
The conical flask was placed on a white tile.
Solution L was added slowly from the burette to the conical flask, while the flask was
swirled, until the solution just changed colour.
Use the burette diagrams to complete the table for Experiment 3.
2
26
3
27
4
28
initial reading
final reading
Experiment 3
final burette reading / cm3
initial burette reading / cm3
volume of solution L added / cm3
[5]
© UCLES 2021
0620/62/O/N/21
[Turn over
6
(b) State the colour change observed at the end-point in the conical flask in Experiment 1.
from ................................................................ to ���������������������������������������������������������������� [1]
(c)Describe one other observation made when solution K was added to acid M in Experiment 1.
............................................................................................................................................... [1]
(d) (i)Compare the volumes of solution K used in Experiment 1 and Experiment 2.
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)
Suggest why different volumes of solution K were needed in Experiment 1 and Experiment 2.
........................................................................................................................................ [1]
(e)Deduce the volume of solution L required to reach the end-point if Experiment 3 is repeated
using acid M in place of acid N.
volume of solution L = .............................. cm3 [1]
(f) Explain why the conical flask was rinsed with water at the start of Experiment 2 and Experiment 3.
............................................................................................................................................... [1]
(g)At the start of Experiment 3 the burette was rinsed with water.
Describe an additional step that should have been done after rinsing the burette with water but
before filling the burette with solution L. Explain your answer.
.....................................................................................................................................................
............................................................................................................................................... [2]
(h) Explain why the conical flask is placed on a white tile.
............................................................................................................................................... [1]
(i) Describe how the reliability of the results can be confirmed.
.....................................................................................................................................................
............................................................................................................................................... [1]
© UCLES 2021
0620/62/O/N/21
7
(j)State one source of error in Experiment 1. Suggest an improvement to reduce this error.
source of error ............................................................................................................................
improvement ...............................................................................................................................
[2]
© UCLES 2021
[Total: 18]
0620/62/O/N/21
[Turn over
8
3Solid O and liquid P were analysed. Solid O was ammonium bromide.
Tests were done on each substance.
tests on solid O
Complete the expected observations.
Solid O was dissolved in water to form solution O. Solution O was divided into four approximately
equal portions in four test‑tubes.
(a) To the first portion of solution O, approximately 2 cm3 of aqueous ammonia was added.
observations ......................................................................................................................... [1]
(b)To the second portion of solution O, approximately 2 cm3 of aqueous sodium hydroxide was
added. The mixture formed was warmed. A gas was given off.
(i)
The gas given off was tested with damp red litmus paper.
observations .................................................................................................................. [1]
(ii)
Identify the gas given off.
........................................................................................................................................ [1]
(c)To the third portion of solution O, approximately 1 cm3 of dilute nitric acid followed by a few
drops of aqueous silver nitrate were added.
observations ......................................................................................................................... [1]
(d)To the fourth portion of solution O, approximately 1 cm3 of aqueous chlorine was added.
observations ......................................................................................................................... [1]
© UCLES 2021
0620/62/O/N/21
9
tests on liquid P
tests
observations
A few drops of liquid P were placed in a
crucible. A lighted splint was applied to the
surface of liquid P in the crucible.
burned with an orange flame and lots of smoke;
soot was left around the top of the crucible
test 1
test 2
A few drops of liquid P were added to a
test‑tube containing 1 cm3 of aqueous
bromine.
colour changed from orange to colourless
(e)State what conclusions can be made about liquid P.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2021
[Total: 7]
0620/62/O/N/21
[Turn over
10
4
Cobalt is a metal. Cobalt is between copper and iron in the reactivity series. The mineral
spherocobaltite contains the compound cobalt(II) carbonate and no other metal ions.
Cobalt(II) carbonate is insoluble in water and reacts with dilute acids to form an aqueous solution
of a salt.
Describe how you would obtain a sample of cobalt metal starting with a large lump of spherocobaltite.
You have access to all normal laboratory apparatus and chemicals.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
© UCLES 2021
0620/62/O/N/21
11
BLANK PAGE
© UCLES 2021
0620/62/O/N/21
12
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/62/O/N/21
Cambridge IGCSE™
*8417627571*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
October/November 2021
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 80.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB21 11_0620_42/3RP
© UCLES 2021
[Turn over
2
1This question is about states of matter.
(a)Complete the table, using ticks ( ) and crosses ( ), to describe the properties of gases, liquids
and solids.
state of matter
particles
are touching
particles have
random movement
particles are
regularly arranged
gas
liquid
solid
[3]
(b)Substances can change state.
(i)Boiling and evaporation are two ways in which a liquid changes into a gas.
Describe two differences between boiling and evaporation.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(ii)Name the change of state when:
●
a gas becomes a liquid .................................................................................................
● a solid becomes a gas. .................................................................................................
[2]
© UCLES 2021
0620/42/O/N/21
3
(c)A substance boils at temperature X and melts at temperature Y.
Complete the graph to show the change in temperature over time as the substance cools from
temperature A to temperature B.
A
X
temperature
Y
B
time
[2]
(d)A solution is a mixture of a solute and a solvent.
(i)Name the process when a solid substance mixes with a solvent to form a solution.
........................................................................................................................................ [1]
(ii)Name the type of reaction when two solutions react to form an insoluble substance.
........................................................................................................................................ [1]
© UCLES 2021
[Total: 11]
0620/42/O/N/21
[Turn over
4
2Acids are important laboratory chemicals.
(a)Some acids completely dissociate in water to form ions.
(i)State the term applied to acids that completely dissociate in water.
........................................................................................................................................ [1]
(ii)Complete the equation to show the complete dissociation of sulfuric acid in water.
H2SO4 → .....................................................................................
[2]
(iii)State the colour of methyl orange in sulfuric acid.
........................................................................................................................................ [1]
(b)The equation for the reaction between powdered zinc carbonate and dilute nitric acid is shown.
ZnCO3....... + 2HNO3....... → Zn(NO3)2....... + H2O....... + CO2.......
(i)Complete the equation by adding state symbols.
[2]
(ii)A student found that 2.5 g of zinc carbonate required 20 cm3 of dilute nitric acid to react
completely.
Calculate the concentration of dilute nitric acid using the following steps:
●
calculate the mass of 1 mole of ZnCO3
.............................. g
●
calculate the number of moles of ZnCO3 reacting
.............................. moles
●
determine the number of moles of HNO3 reacting
.............................. moles
●
calculate the concentration of HNO3.
.............................. mol / dm3
[4]
© UCLES 2021
[Total: 10]
0620/42/O/N/21
5
3Atoms contain protons, neutrons and electrons.
(a)Complete the table to show the relative mass and the relative charge of a proton, a neutron
and an electron.
relative mass
relative charge
proton
neutron
1
1840
electron
[3]
(b)The table shows the number of protons, neutrons and electrons in some atoms and ions.
Complete the table.
atom
or ion
number of
protons
number of
neutrons
number of
electrons
35
44
36
32
16S
39 +
19K
[5]
© UCLES 2021
[Total: 8]
0620/42/O/N/21
[Turn over
6
4Chlorine reacts with carbon monoxide to produce phosgene gas, COCl 2(g). A catalyst is used.
Cl 2(g) + CO(g)
COCl 2(g)
The reaction is exothermic.
(a)Explain why the reaction is exothermic in terms of the energy changes of bond breaking and
bond making.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(b) (i)Complete the energy level diagram for this reaction.
On your diagram show:
●
●
●
the product of the reaction
an arrow representing the energy change, labelled ∆H
an arrow representing the activation energy, labelled A.
energy
Cl 2(g) + CO(g)
progress of reaction
[3]
(ii)State why a catalyst is used.
........................................................................................................................................ [1]
© UCLES 2021
0620/42/O/N/21
7
(c)Describe and explain the effect, if any, on the position of equilibrium when:
(i)the pressure is increased
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)the temperature is increased.
..............................................................................................................................................
........................................................................................................................................ [2]
(d)The reaction between chlorine and carbon monoxide can be represented as shown.
O
Cl
Cl
+
CO
Cl
C
Cl
When one mole of chlorine reacts with one mole of carbon monoxide, 230 kJ of energy is
released.
Some bond energies are shown in the table.
bond
bond energy in kJ / mol
Cl –Cl
240
C=O
745
C–Cl
400
Use the information to calculate the energy of the bond between the C and the O in
carbon monoxide, CO.
© UCLES 2021
bond energy in carbon monoxide, CO = .............................. kJ / mol [3]
0620/42/O/N/21
[Turn over
8
(e)Complete the dot-and-cross diagram to show the electron arrangement in a molecule of COCl 2.
O
Cl
C
Cl
Show outer electrons only.
O
C
Cl
Cl
[3]
© UCLES 2021
[Total: 17]
0620/42/O/N/21
9
5Iron is a transition element. Potassium is a Group I element.
(a)Iron and potassium have the same type of bonding.
Name and describe the type of bonding in these two elements.
name ...........................................................................................................................................
description ..................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
[4]
(b)Transition elements and Group I elements have some similar physical properties.
They can both:
●
●
●
e hammered into a shape
b
conduct electricity
be stretched into wires.
(i)Name the term used to describe the ability of elements to be hammered into a shape.
........................................................................................................................................ [1]
(ii)Describe what happens to the particles in iron when it is hammered into a shape.
..............................................................................................................................................
........................................................................................................................................ [1]
(iii)Suggest why copper, rather than other transition elements, is used for wires which conduct
electricity.
........................................................................................................................................ [1]
(c)Transition elements are harder and stronger than Group I elements.
Describe how two other physical properties of transition elements are different from those of
Group I elements.
1 ..................................................................................................................................................
2 ..................................................................................................................................................
[2]
© UCLES 2021
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10
(d)Chemical properties of some Group I elements are shown in the table.
element
reaction with cold water
reaction with oxygen
flame test
colour
red
lithium
●
●
steadily effervesces
forms a colourless solution
very slowly forms an oxide layer
sodium
●
●
strongly effervesces
forms a colourless solution
slowly forms an oxide layer
potassium
●
●
v ery strongly effervesces
forms a colourless solution
quickly forms an oxide layer
rubidium
ruby red
(i)Add to the table:
● the flame test colours for sodium and potassium
● the predicted reactions of rubidium with water and with oxygen.
[4]
(ii)Name the gas produced when Group I elements react with water.
........................................................................................................................................ [1]
(iii)Name the solution formed when potassium reacts with water.
........................................................................................................................................ [1]
(iv)Predict the pH of the colourless solution formed when potassium reacts with water.
........................................................................................................................................ [1]
(v)Write the chemical equation for the reaction of sodium with oxygen.
........................................................................................................................................ [2]
(e)Iron is a typical transition element. It is the catalyst used in the Haber process.
(i)Write the equation for the reaction that occurs in the Haber process.
........................................................................................................................................ [2]
(ii)State the temperature and pressure used in the Haber process. Include units.
temperature .........................................................................................................................
pressure ...............................................................................................................................
[2]
© UCLES 2021
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11
6Ethanol, C2H5OH, belongs to the homologous series called alcohols.
(a)Write the general formula of alcohols.
............................................................................................................................................... [1]
(b)Explain why ethanol cannot be described as a hydrocarbon.
............................................................................................................................................... [1]
(c)Ethanol can be manufactured from different substances by reaction with steam or by
fermentation.
(i)Give the formula of the substance which reacts with steam to form ethanol.
........................................................................................................................................ [1]
(ii)Name a substance which will undergo fermentation to form ethanol.
........................................................................................................................................ [1]
(d)Ethanol is a fuel.
Write the chemical equation for the complete combustion of ethanol.
............................................................................................................................................... [2]
© UCLES 2021
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12
(e)Ethane-1,2-diol has two alcohol functional groups.
H
O
H
H
C
C
H
H
O
H
One molecule of ethane-1,2-diol will react with two molecules of ethanoic acid to form
molecule X.
X has two ester functional groups and a molecular formula of C6H10O4.
(i)State the empirical formula of X.
........................................................................................................................................ [1]
(ii)Draw the structure of X.
Show all of the atoms and all of the bonds.
[2]
(iii)Name the other substance formed in this reaction.
........................................................................................................................................ [1]
(f)Each alcohol functional group in ethane-1,2-diol reacts with acidified potassium manganate(VII)
to form a different organic compound, Y.
(i)Name the functional groups formed in Y.
........................................................................................................................................ [1]
(ii)Draw the structure of Y.
Show all of the atoms and all of the bonds.
[1]
© UCLES 2021
[Total: 12]
0620/42/O/N/21
13
BLANK PAGE
© UCLES 2021
0620/42/O/N/21
14
BLANK PAGE
© UCLES 2021
0620/42/O/N/21
15
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Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/42/O/N/21
© UCLES 2021
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/O/N/21
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
October/November 2021
45 minutes
You must answer on the multiple choice answer sheet.
*8181221372*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
 There are forty questions on this paper. Answer all questions.
 For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
 Follow the instructions on the multiple choice answer sheet.
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
 Do not use correction fluid.
 Do not write on any bar codes.
 You may use a calculator.
INFORMATION
 The total mark for this paper is 40.
 Each correct answer will score one mark.
 Any rough working should be done on this question paper.
 The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB21 11_0620_22/3RP
© UCLES 2021
[Turn over
2
1
An experiment is set up as shown.
cotton wool soaked
in ammonia
cotton wool soaked
in hydrochloric acid
After several minutes, a white ring of ammonium chloride appears as shown.
ammonium chloride
Which statement explains the observation after several minutes?
2
A
Ammonia gas diffuses faster than hydrogen chloride gas because its molecules have a lower
molecular mass.
B
Ammonia gas diffuses faster than hydrogen chloride gas because its molecules have a
higher molecular mass.
C
Ammonia gas diffuses slower than hydrogen chloride gas because its molecules have a
lower molecular mass.
D
Ammonia gas diffuses slower than hydrogen chloride gas because its molecules have a
higher molecular mass.
A student put exactly 25.00 cm3 of dilute hydrochloric acid into a conical flask.
The student added 2.5 g of solid sodium carbonate and measured the change in temperature of
the mixture.
Which apparatus does the student need to use?
A
balance, measuring cylinder, thermometer
B
balance, pipette, stopwatch
C
balance, pipette, thermometer
D
burette, pipette, thermometer
© UCLES 2021
0620/22/O/N/21
3
3
A student separates sugar from pieces of broken glass by dissolving the sugar in water and
filtering off the broken glass.
filtrate
What is the filtrate?
4
5
A
broken glass only
B
broken glass and sugar solution
C
pure water
D
sugar solution
How many protons, neutrons and electrons are there in one atom of the isotope 27
13 Al ?
protons
neutrons
electrons
A
13
13
13
B
13
14
13
C
14
13
13
D
14
14
13
Which description of brass is correct?
A
alloy
B
compound
C
element
D
non-metal
© UCLES 2021
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4
6
Some properties of diamond are shown.
1
It is very hard.
2
Every atom forms four bonds.
3
It does not conduct electricity.
Which properties are also shown by silicon(IV) oxide?
A
7
8
9
1 only
B
1 and 2
C
1 and 3
D
2 and 3
Which statement describes the attractive forces between molecules?
A
They are strong covalent bonds which hold molecules together.
B
They are strong ionic bonds which hold molecules together.
C
They are weak forces formed between covalently-bonded molecules.
D
They are weak forces which hold ions together in a lattice.
Which substance is described as a macromolecule?
A
ammonia
B
graphite
C
iron
D
sodium chloride
The equation for the reaction of sodium with water is shown.
2Na + 2H2O  2NaOH + H2
What is the volume of hydrogen gas, measured at r.t.p., produced when 18.4 g of sodium reacts
with excess water?
9.6 dm3
A
B
15.0 dm3
C
19.2 dm3
D
30.0 dm3
10 Iron can be electroplated with zinc to make it resistant to corrosion.
Which row about electroplating iron with zinc is correct?
positive electrode
(anode)
negative electrode
(cathode)
electrolyte
A
iron
zinc
iron nitrate
B
iron
zinc
zinc nitrate
C
zinc
iron
iron nitrate
D
zinc
iron
zinc nitrate
© UCLES 2021
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5
11 Chlorine reacts with ethane to produce chloroethane and hydrogen chloride.
H
H
H
C
C
H
H
H
+
Cl
Cl
H
H
H
C
C
H
H
Cl
+
H
Cl
The reaction is exothermic.
The bond energies are shown in the table.
bond
bond energy
in kJ / mol
C–Cl
+340
C–C
+350
C–H
+410
Cl –Cl
+240
H–Cl
+430
What is the energy change for the reaction?
A
–1420 kJ / mol
B
–120 kJ / mol
C
+120 kJ / mol
D
+1420 kJ / mol
12 Chlorine gas is bubbled into aqueous potassium iodide.
What is the ionic equation for the reaction that takes place?
A
Cl + I–  Cl – + I
B
Cl 2 + 2I–  Cl 2– + I2
C
Cl 2 + 2I–  2Cl – + I2
D
Cl 2 + 2I–  2Cl – + 2I
13 Concentrated aqueous sodium chloride is electrolysed.
Which equation represents the reaction at the cathode?
A
Na+ + e–  Na
B
2O2–  O2 + 4e–
C
2H+ + 2e–  H2
D
2Cl –  Cl 2 + 2e–
© UCLES 2021
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6
14 Which statements about hydrogen are correct?
A
1
When hydrogen is burned, heat energy is released.
2
When hydrogen is used in a fuel cell, electrical energy is generated.
3
When hydrogen is used as a fuel, water is the only product.
1, 2 and 3
B
1 and 2 only
C
1 only
D
3 only
15 Solid X is heated strongly.
The colour of the solid changes from blue to white.
What is solid X?
A
anhydrous cobalt(II) chloride
B
calcium carbonate
C
hydrated copper(II) sulfate
D
lead(II) bromide
16 Iron(II) chloride solution reacts with chlorine gas.
The equation is shown.
2FeCl 2(aq) + Cl 2(g)  2FeCl 3(aq)
Which statements about this reaction are correct?
A
1
Fe2+ ions are reduced to Fe3+ ions.
2
Chlorine acts as a reducing agent.
3
Fe2+ ions each lose an electron.
4
Cl 2 molecules are reduced to Cl – ions.
1 and 2
B
2 and 3
C
2 and 4
D
3 and 4
17 Which statements about acids and bases are correct?
A
1
An acid reacts with a metal to give off hydrogen.
2
A base reacts with an ammonium salt to give off ammonia.
3
An acid reacts with a carbonate to give off carbon dioxide.
4
Alkaline solutions are orange in methyl orange.
1, 2 and 3
© UCLES 2021
B
1, 2 and 4
C
1, 3 and 4
0620/22/O/N/21
D
2, 3 and 4
7
18 Oxide 1 is a solid that reacts with dilute hydrochloric acid.
Oxide 2 is a gas that reacts with sodium hydroxide solution.
What are the formulae of the oxides?
oxide 1
oxide 2
A
CaO
MgO
B
MgO
NO2
C
NO2
SO2
D
SO2
CaO
19 Which reaction is a photochemical reaction?
A
addition of bromine to propene
B
esterification of ethanol and ethanoic acid
C
oxidation of ethanol
D
substitution of methane with chlorine
20 The equation shown represents a reaction at equilibrium.
m and n represent the balancing numbers for the reactant and product respectively.
mP(g)
nQ(g)
A high temperature increases the concentration of Q.
A high pressure increases the concentration of Q.
Which statement about the reaction is correct?
A
The forward reaction is exothermic and m is greater than n.
B
The forward reaction is exothermic and m is less than n.
C
The forward reaction is endothermic and m is greater than n.
D
The forward reaction is endothermic and m is less than n.
© UCLES 2021
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8
21 A period of the Periodic Table is shown.
group
I
II
III
IV
V
VI
VII
VIII
element
R
S
T
V
W
X
Y
Z
The letters are not their chemical symbols.
Which statement is correct?
A
Element R does not conduct electricity.
B
Elements R and Y react together to form an ionic compound.
C
Element Z exists as a diatomic molecule.
D
Element Z reacts with element T.
22 All metal nitrates are soluble in water.
All metal chlorides are soluble except silver and lead.
All metal carbonates are insoluble except sodium and potassium.
Which aqueous solutions produce a precipitate when mixed together?
A
1
silver nitrate + sodium carbonate
2
silver nitrate + sodium chloride
3
barium nitrate + potassium chloride
1 and 2 only
B
1 and 3 only
C
2 and 3 only
D
1, 2 and 3
23 Which row describes properties of transition elements?
property 1
property 2
property 3
A
coloured compounds
high density
variable oxidation states
B
high density
high melting point
one oxidation state
C
high melting point
coloured compounds
one oxidation state
D
low melting point
high density
variable oxidation states
© UCLES 2021
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9
24 The noble gases are in Group VIII of the Periodic Table.
Which statement explains why noble gases are unreactive?
A
They all have eight electrons in their outer shells.
B
They all have full outer shells.
C
They are all gases.
D
They are all monoatomic.
25 Which statement is correct for all metals?
A
They conduct electricity when molten.
B
They gain electrons when they form ions.
C
They have a low density.
D
They have a low melting point.
26 Carbon dioxide is produced during the extraction of aluminium from bauxite.
Which statement describes how this carbon dioxide is made?
A
Carbon monoxide reduces aluminium oxide forming carbon dioxide and aluminium.
B
Carbon is burned in the blast furnace to release heat energy.
C
Oxygen made in the process reacts with the carbon electrode.
D
The ore of aluminium undergoes thermal decomposition.
27 Aluminium objects do not need protection from corrosion.
Iron objects must be protected from corrosion.
Which statement explains why aluminium resists corrosion?
A
Aluminium does not form ions easily.
B
Aluminium does not react with water or air.
C
Aluminium has a protective oxide layer.
D
Aluminium is below iron in the reactivity series.
© UCLES 2021
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10
28 Which statements explain why zinc is used to protect iron from rusting?
A
1
Zinc is more reactive than iron.
2
Zinc is less reactive than iron.
3
Zinc can form alloys with iron.
4
Zinc acts as a sacrificial metal.
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
29 Which conditions are used in the Haber process?
temperature
/ C
pressure
/ atmospheres
A
100
10
B
450
10
C
450
200
D
1000
500
30 Which process does not produce a greenhouse gas?
A
acid rain on limestone buildings
B
combustion of wood
C
digestion in cows
D
zinc reacting with sulfuric acid
31 Which reaction involving sulfur dioxide is correct?
A
It is produced during the extraction of zinc from zinc blende.
B
It reacts with concentrated sulfuric acid to form oleum.
C
It reacts with sulfur to form sulfur trioxide.
D
It turns an acidified solution of potassium manganate(VII) purple.
32 Lime (calcium oxide) is used to treat waste water from a factory.
Which substance is removed by the lime?
A
ammonia
B
sodium chloride
C
sodium hydroxide
D
sulfuric acid
© UCLES 2021
0620/22/O/N/21
11
33 What is the structure of the ester formed from ethanoic acid and propanol?
A
H
H
H
C
C
H
H
B
O
C
H
H
C
C
H
H
H
H
H
C
C
H
H
O
C
H
O
H
C
H
H
H
C
O
H
D
C
H
H
C
H
O
C
H
C
O
C
H
H
H
C
C
C
H
H
H
H
H
C
H
H
H
C
H
H
H
O
H
C
O
H
34 Fuel X produces carbon dioxide and water when it is burned in air. So does fuel Y.
What could X and Y be?
X
Y
A
C
H2
B
C
C8H18
C
CH4
H2
D
CH4
C8H18
© UCLES 2021
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12
35 The structures of four organic molecules are shown.
H
H
H
O
C
Cl
H
C
O
H
H
H
H
H
C
C
H
H
O
O
H
H
H
How many different homologous series are represented by these molecules?
A
1
B
2
C
3
D
4
36 Which statement about ethene is correct?
A
It has the chemical formula C2H6.
B
It burns in excess oxygen producing carbon dioxide and water.
C
It reacts with Br2 to produce an orange solution.
D
It reacts with oxygen to form ethanol.
37 Ethanol is manufactured by fermentation of sugars or by catalytic hydration of ethene.
Which row states an advantage of each method?
fermentation
hydration
A
produces purer ethanol
is a batch process
B
produces purer ethanol
is a continuous process
C
uses a renewable resource
is a batch process
D
uses a renewable resource
is a continuous process
38 Which statements about unsaturated hydrocarbons are correct?
A
1
They contain both single and double bonds.
2
They turn aqueous bromine from colourless to brown.
3
They can be manufactured by cracking.
1 and 2 only
© UCLES 2021
B
1 and 3 only
C
2 and 3 only
0620/22/O/N/21
D
C
1, 2 and 3
H
13
39 Which polymers have the same linkage between monomer units?
A
carbohydrate and polyamide
B
carbohydrate and polyester
C
protein and polyamide
D
protein and polyester
40 The diagram shows the partial structure of Terylene.
O
C
O
O
O
O
C
C
O
From which pair of compounds is it made?
A
HO
O
O
C
C
OH
+
HO
OH
O
B
C
D
HO
C
HO
HO
© UCLES 2021
O
OH
+
OH
+
O
O
C
C
OH
+
HO
HO
HO
C
OH
O
O
C
C
O
O
C
C
0620/22/O/N/21
OH
OH
14
BLANK PAGE
© UCLES 2021
0620/22/O/N/21
15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/22/O/N/21
© UCLES 2021
21
0620/22/O/N/21
22
cerium
140
90
Th
thorium
232
lanthanum
139
89
Ac
actinium
–
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
Ce
57
La
–
dubnium
Db
105
181
tantalum
Ta
73
93
niobium
Nb
41
51
vanadium
V
–
rutherfordium
Rf
104
178
hafnium
Hf
72
91
zirconium
Zr
40
48
titanium
Ti
23
Cr
24
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
relative atomic mass
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Pt
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
49
70
gallium
Ga
31
27
aluminium
Al
13
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
–
actinoids
Ra
radium
88
87
Fr
137
francium
89–103
barium
133
lanthanoids
57–71
89
yttrium
caesium
Y
39
Ba
38
37
45
scandium
Cs
40
39
56
calcium
potassium
Sc
55
Ca
K
88
20
19
strontium
24
23
85
magnesium
sodium
rubidium
Mg
Na
Sr
12
11
Rb
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
Group
The Periodic Table of Elements
16
Cambridge IGCSE™
*9457558127*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
May/June 2022
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 40.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Any blank pages are indicated.
IB22 06_0620_62/3RP
© UCLES 2022
[Turn over
2
1Sodium hydrogencarbonate decomposes when heated. The products are solid sodium carbonate,
water and carbon dioxide.
A student decomposed a sample of sodium hydrogencarbonate using the apparatus shown.
A
X
delivery tube
sodium
hydrogencarbonate
B
water
(a)Name the items of apparatus labelled A and B.
A .................................................................................................................................................
B ................................................................................................................................................
[2]
(b)When the sodium hydrogencarbonate was heated, a colourless liquid collected at the point
marked X.
Suggest the identity of the colourless liquid.
............................................................................................................................................... [1]
(c)
On the diagram draw one arrow to show where the apparatus should be heated during the
experiment.[1]
(d)State an observation that would indicate the sodium hydrogencarbonate had stopped reacting.
.....................................................................................................................................................
............................................................................................................................................... [1]
(e)Explain why it is important to remove the delivery tube from the water as soon as heating is
stopped.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
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2
student investigated the reaction between two different solutions of aqueous sodium carbonate,
A
solution K and solution L, and dilute hydrochloric acid using two different indicators.
Two experiments were done.
Experiment 1
● A burette was rinsed with water and then with the dilute hydrochloric acid.
● The burette was filled with dilute hydrochloric acid. Some of the dilute hydrochloric acid was
run out of the burette so that the level of the dilute hydrochloric acid was on the burette scale.
● Using a measuring cylinder, 25 cm3 of solution K was poured into a conical flask.
● Five drops of methyl orange indicator and five drops of thymolphthalein indicator were added
to the conical flask.
● The conical flask was placed on a white tile.
● Dilute hydrochloric acid was added slowly from the burette to the conical flask, while the flask
was swirled, until the solution turned yellow. This is the first colour change.
● More dilute hydrochloric acid from the burette was added to the conical flask, while swirling the
flask, until the solution changed colour again. This is the second colour change.
(a)Use the burette diagrams to complete the table for Experiment 1.
1
11
22
2
12
23
3
13
24
initial burette reading
burette reading at
first colour change
burette reading at
second colour change
Experiment 1
burette reading at first colour change / cm3
final burette reading at second colour change / cm3
initial burette reading / cm3
volume of dilute hydrochloric acid added for first
colour change / cm3
total volume of dilute hydrochloric acid added for
second colour change / cm3
[3]
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4
(b)
Experiment 2
● The conical flask was emptied and rinsed with distilled water.
● Experiment 1 was repeated using solution L instead of solution K.
Use the burette diagrams to complete the table for Experiment 2.
3
19
35
4
20
36
5
21
37
initial burette reading
burette reading at
first colour change
burette reading at
second colour change
Experiment 2
burette reading at first colour change / cm3
final burette reading at second colour change / cm3
initial burette reading / cm3
volume of dilute hydrochloric acid added for first
colour change / cm3
total volume of dilute hydrochloric acid added for
second colour change / cm3
[3]
(c)State the colour change observed at the end-point when dilute hydrochloric acid is added to
methyl orange in an alkaline solution.
from ................................................................ to ................................................................. [1]
(d) For Experiment 1, compare the volume of dilute hydrochloric acid needed for the first colour
change with the volume of dilute hydrochloric acid for the second colour change.
.....................................................................................................................................................
............................................................................................................................................... [2]
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5
(e)Compare the concentration of solution K used in Experiment 1 to the concentration of solution L
used in Experiment 2.
Explain your answer.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(f) (i)Deduce the volume of dilute hydrochloric acid needed for the second colour change when
Experiment 2 is repeated using 50 cm3 of solution L.
........................................................................................................................................ [2]
(ii)State why using 50 cm3 of solution L would cause a problem.
..............................................................................................................................................
........................................................................................................................................ [1]
(g)State the advantage of using a pipette instead of the measuring cylinder in these experiments.
............................................................................................................................................... [1]
(h) Explain why the conical flask was swirled as the dilute hydrochloric acid was added from the
burette.
.....................................................................................................................................................
............................................................................................................................................... [1]
(i)
At the start of Experiment 1, the burette was rinsed with water and then with dilute
hydrochloric acid.
At the start of Experiment 2, the conical flask was rinsed with water but not with solution L.
(i)
Explain why the conical flask was rinsed with water.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)
Explain why the conical flask was not rinsed with solution L in Experiment 2.
..............................................................................................................................................
........................................................................................................................................ [1]
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6
3Solid M and solid N were analysed. Solid M was iron(III) nitrate.
Tests were done on each substance.
tests on solid M
Complete the expected observations.
Solid M was dissolved in water to form solution M. Solution M was divided into two approximately
equal portions in two test-tubes.
(a) T
o the first portion of solution M, aqueous sodium hydroxide was added gradually until in
excess. The product was kept for (b).
observations ...............................................................................................................................
............................................................................................................................................... [2]
(b) (i)The product from (a) was transferred to a boiling tube. A piece of aluminium foil was added
and the mixture warmed gently. Any gas produced was tested.
observations ........................................................................................................................
........................................................................................................................................ [1]
(ii)Identify the gas made in (i).
........................................................................................................................................ [1]
(c)To the second portion of solution M, about 1 cm depth of dilute nitric acid followed by a few
drops of aqueous barium nitrate were added.
observations ......................................................................................................................... [1]
© UCLES 2022
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7
tests on solid N
tests
observations
test 1
A flame test was carried out on solid N.
the flame became red
Solid N was dissolved in water to form
solution N. Solution N was divided equally into
one test-tube and one boiling tube.
test 2
About 1 cm depth of dilute nitric acid followed
by a few drops of aqueous silver nitrate were
added to the first portion of solution N in a
test‑tube.
no visible change
test 3
About 2 cm depth of dilute hydrochloric acid
was added to the second portion of solution N.
The mixture was warmed and any gas
produced was tested.
acidified aqueous potassium manganate(VII)
changed from purple to colourless
(d) Identify the gas produced in test 3.
............................................................................................................................................... [1]
(e)Identify solid N.
.....................................................................................................................................................
............................................................................................................................................... [2]
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8
4
The diagram shows some coffee beans.
Caffeine occurs naturally in coffee beans. Caffeine is a white crystalline solid. It is very soluble in
hot water but much less soluble in cold water.
Plan an investigation to obtain a pure crystalline sample of caffeine from coffee beans.
Assume that all other soluble substances in coffee beans are very soluble in both hot and cold
water.
You are provided with coffee beans and common laboratory apparatus.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
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Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/62/M/J/22
Cambridge IGCSE™
*6148594183*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
May/June 2022
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 80.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB22 06_0620_42/3RP
© UCLES 2022
[Turn over
2
1The symbols of the elements of Period 3 of the Periodic Table are shown.
Na
Mg
Al
Si
P
S
Cl
Ar
Answer the following questions about these elements.
Each symbol may be used once, more than once or not at all.
Write the symbol of the element which:
(a)forms a stable ion with a 2+ charge ������������������������������������������������������������������������������������� [1]
(b)is the least reactive in the period ����������������������������������������������������������������������������������������� [1]
(c)is used in water treatment ��������������������������������������������������������������������������������������������������� [1]
(d)forms an oxide which is the main impurity in iron ore ���������������������������������������������������������� [1]
(e)is an important component of fertilisers ������������������������������������������������������������������������������� [1]
(f)is stored under oil ���������������������������������������������������������������������������������������������������������������� [1]
(g)is used in food containers ���������������������������������������������������������������������������������������������������� [1]
(h)is found in the ore zinc blende. �������������������������������������������������������������������������������������������� [1]
© UCLES 2022
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3
Question 2 starts on the next page.
© UCLES 2022
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4
2Calcium hydroxide, Ca(OH)2, is slightly soluble in water.
(a)Calcium hydroxide can be made by the reaction of calcium with water.
(i)Write the chemical equation for this reaction.
........................................................................................................................................ [2]
(ii)Name another substance that reacts with water to form calcium hydroxide.
........................................................................................................................................ [1]
(b)When calcium hydroxide dissolves in water, it dissociates into ions and forms a weakly alkaline
solution.
(i)Suggest the pH of aqueous calcium hydroxide.
........................................................................................................................................ [1]
(ii)Give the formula of the ion responsible for making the solution alkaline.
........................................................................................................................................ [1]
(c)Limewater is a saturated solution of calcium hydroxide, Ca(OH)2(aq).
(i)Name the gas limewater is used to test for.
........................................................................................................................................ [1]
(ii)Suggest what is meant by the term saturated solution.
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)Describe how you would make a sample of limewater starting with solid calcium hydroxide.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iv)Describe how you would test for the presence of calcium ions in a sample of limewater.
test .......................................................................................................................................
observations ........................................................................................................................
..............................................................................................................................................
[3]
© UCLES 2022
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5
(d)A 25.0 cm3 sample of limewater is placed in a conical flask. The concentration of Ca(OH)2 in the
limewater is determined by titration with dilute hydrochloric acid, HCl.
(i)Name the item of apparatus used to measure the volume of acid in this titration.
........................................................................................................................................ [1]
(ii)State the type of reaction which takes place.
........................................................................................................................................ [1]
(iii)As well as limewater and dilute hydrochloric acid, state what other type of substance must
be added to the conical flask.
........................................................................................................................................ [1]
(iv)The equation for the reaction is shown.
Ca(OH)2 + 2HCl → CaCl 2 + 2H2O
20.0 cm3 of 0.0500 mol / dm3 HCl reacts with the 25.0 cm3 of Ca(OH)2.
Determine the concentration of Ca(OH)2 in g / dm3. Use the following steps.
●
Calculate the number of moles in 20.0 cm3 of 0.0500 mol / dm3 HCl.
.............................. mol
●
Determine the number of moles of Ca(OH)2 in 25.0 cm3 of the limewater.
.............................. mol
●
Calculate the concentration of Ca(OH)2 in mol / dm3.
.............................. mol / dm3
●
Determine the concentration of Ca(OH)2 in g / dm3.
.............................. g / dm3
[5]
© UCLES 2022
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3Transition elements are found in the middle block of the Periodic Table.
(a)Chromium has several isotopes. Manganese has only one isotope.
(i)State what is meant by the term isotopes.
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)State the nucleon number of manganese.
........................................................................................................................................ [1]
52
Cr3+ ion.
(iii)Complete the table to show the number of protons, neutrons and electrons in a 24
protons
neutrons
electrons
[3]
(b)One chemical property of transition elements is that they form coloured compounds.
(i)Give the colours of the following hydrated salts.
●
hydrated copper(II) sulfate ������������������������������������������������������������������������������������������
● hydrated cobalt(II) chloride �����������������������������������������������������������������������������������������
[2]
(ii)State two other chemical properties of transition elements.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(c) T
ransition elements and Group I elements are metals. They share many physical properties
including the ability to:
● conduct electricity
● be hammered into shape.
(i)Explain why transition elements and Group I elements conduct electricity.
........................................................................................................................................ [1]
(ii)State the property that describes a material which can be hammered into shape.
........................................................................................................................................ [1]
© UCLES 2022
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7
(d)Transition elements and Group I elements differ in other physical properties. Transition
elements are harder and stronger than Group I elements.
Describe two other ways in which the physical properties of transition elements differ from
Group I elements.
1 ..................................................................................................................................................
2 ..................................................................................................................................................
[2]
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4Fluorine and chlorine are halogens.
(a)Suggest the appearance of fluorine.
............................................................................................................................................... [1]
(b)Fluorine reacts with sulfur to form a compound which has 25.2% sulfur by mass and a relative
molecular mass of 254.
Determine the molecular formula of this compound.
molecular formula = .............................. [3]
(c)Nitrogen trichloride, NCl 3, is a covalent compound.
Complete the dot-and-cross diagram to show the electron arrangement in a molecule of NCl 3.
Show outer electrons only.
Cl
N
Cl
Cl
[3]
© UCLES 2022
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9
(d)Lithium chloride, LiCl, is an ionic compound.
Complete the dot-and-cross diagram to show the electron arrangement and charges of the
ions in lithium chloride.
.....
Li
.....
Cl
[3]
(e)Explain, in terms of attractive forces between particles, why LiCl is a solid at room temperature
but NCl 3 is a liquid with a relatively low boiling point.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
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5The reaction scheme shows five organic reactions, numbered 1 to 5.
carbon dioxide + water
2
sugar
1
3
ethanol
alkene A
4
alkane B
5
compound C
(a)Name reaction 1.
............................................................................................................................................... [1]
(b)Name reaction 2 and write the chemical equation for this reaction.
name ...........................................................................................................................................
equation ......................................................................................................................................
[3]
(c)Reaction 3 forms ethanol from alkene A.
(i)Identify alkene A.
........................................................................................................................................ [1]
(ii)State the type of reaction that occurs during reaction 3.
........................................................................................................................................ [1]
(iii)State the reagents and conditions needed for reaction 3.
..............................................................................................................................................
........................................................................................................................................ [2]
(d)Alkene A is converted into alkane B in reaction 4.
(i)State the reagent and conditions for reaction 4.
..............................................................................................................................................
........................................................................................................................................ [3]
(ii)State the general formula of alkanes.
........................................................................................................................................ [1]
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11
(e) Ethanol is oxidised in reaction 5 by heating it with dilute sulfuric acid and one other reagent.
(i)Identify the other reagent in reaction 5.
........................................................................................................................................ [1]
(ii)Name the homologous series compound C belongs to.
........................................................................................................................................ [1]
(iii)Draw the structure of compound C.
Show all of the atoms and all of the bonds.
[1]
© UCLES 2022
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6This question is about polymers.
(a)Polymer X is a condensation polymer.
Part of the structure of polymer X is shown.
O
C
O
O
O
O
C
C
O
(i)How many molecules of water are produced when this part of polymer X is formed from its
monomers?
........................................................................................................................................ [1]
(ii)Complete the structures of the two monomers used to make polymer X.
Show all of the atoms and all of the bonds in the functional groups.
and
[2]
(iii)What type of condensation polymer is X?
........................................................................................................................................ [1]
(b)Part of polymer Y has the structure shown.
O
C
O
O
C
O
O
C
O
State the number of different types of monomer needed to make polymer Y.
............................................................................................................................................... [1]
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13
(c)Part of polymer Z has the structure shown.
CH3 H
CH3 H
CH3 H
C
C
C
C
H
CH3 H
C
CH3 H
C
CH3
(i)Draw and name the structure of the monomer which forms polymer Z.
Show all of the atoms and all of the bonds.
name ...............................................
[3]
(ii)Name the chemical process used to make the monomer that forms polymer Z.
........................................................................................................................................ [1]
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© UCLES 2022
0620/42/M/J/22
15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/42/M/J/22
© UCLES 2022
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/M/J/22
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
May/June 2022
45 minutes
You must answer on the multiple choice answer sheet.
*2772444271*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
 There are forty questions on this paper. Answer all questions.
 For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
 Follow the instructions on the multiple choice answer sheet.
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
 Do not use correction fluid.
 Do not write on any bar codes.
 You may use a calculator.
INFORMATION
 The total mark for this paper is 40.
 Each correct answer will score one mark.
 Any rough working should be done on this question paper.
 The Periodic Table is printed in the question paper.
This document has 16 pages.
IB22 06_0620_22/2RP
© UCLES 2022
[Turn over
2
1
2
Which two gases will diffuse at the same rate, at the same temperature?
A
carbon monoxide and carbon dioxide
B
carbon monoxide and nitrogen
C
chlorine and fluorine
D
nitrogen and oxygen
A student measures the time taken for 2.0 g of magnesium to dissolve in 50 cm3 of dilute
sulfuric acid.
Which apparatus is essential to complete the experiment?
A
3
1
stop-clock
2
measuring cylinder
3
thermometer
4
balance
1, 2 and 4
B
1 and 2 only
C
1 and 4 only
D
2, 3 and 4
A chromatogram of a single substance T is shown.
solvent front
3
4
1
2
baseline
Which measurements are used to find the Rf value of T?
A
4
1 and 2
B
1 and 4
C
2 and 3
X and Y are two different elements.
X and Y have the same number of nucleons.
Which statement about X and Y is correct?
A
They have the same physical properties.
B
Their atoms have the same number of electrons.
C
They are in different groups of the Periodic Table.
D
They have different relative masses.
© UCLES 2022
0620/22/M/J/22
D
3 and 4
3
5
The diagrams show the structures of three macromolecules P, Q and R.
P
Q
R
What are P, Q and R?
6
P
Q
R
A
diamond
silicon(IV) oxide
graphite
B
graphite
diamond
silicon(IV) oxide
C
silicon(IV) oxide
diamond
graphite
D
silicon(IV) oxide
graphite
diamond
Which dot-and-cross diagram shows the arrangement of outer shell electrons in a molecule of
hydrogen chloride?
A
H
7
B
Cl
H
C
Cl
H
D
Cl
H
Cl
The equation for the reaction between barium chloride and dilute sulfuric acid is shown.
BaCl 2 + H2SO4  BaSO4 + 2HCl
Which row shows the state symbols for this equation?
BaCl 2
H2SO4
BaSO4
2HCl
A
(aq)
(aq)
(s)
(aq)
B
(aq)
(l)
(s)
(aq)
C
(l)
(aq)
(s)
(l)
D
(aq)
(l)
(aq)
(l)
© UCLES 2022
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4
8
Methane and steam react in the presence of a catalyst.
CH4(g) + H2O(g)  CO(g) + 3H2(g)
0.5 mol of methane reacts completely with 0.5 mol of steam.
What is the volume of carbon monoxide and hydrogen produced, measured at room temperature
and pressure?
9
volume
of CO / dm3
volume
of H2 / dm3
A
0.5
1.5
B
1.0
3.0
C
12.0
12.0
D
12.0
36.0
A compound of element X has the formula X2O and a relative formula mass of 144.
What is element X?
A
copper, Cu
B
gadolinium, Gd
C
sulfur, S
D
tellurium, Te
© UCLES 2022
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5
10 The diagram shows the electrolysis of concentrated hydrochloric acid and concentrated aqueous
sodium chloride using carbon electrodes.
electrode 1
+
–
electrode 2
electrode 3
concentrated
hydrochloric acid
+
–
electrode 4
concentrated aqueous
sodium chloride
At which electrodes is hydrogen produced?
A
electrode 1 only
B
electrodes 1 and 3
C
electrode 2 only
D
electrodes 2 and 4
11 The diagram shows the electrolysis of aqueous copper(II) sulfate using inert electrodes.
Which arrow shows the movement of electrons in the circuit?
power
supply
A
B
anode
cathode
C
D
© UCLES 2022
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6
12 Which row identifies a chemical change and a physical change?
chemical change
physical change
A
boiling ethanol
burning ethanol
B
burning ethanol
evaporating ethanol
C
dissolving ethanol in water
burning ethanol
D
evaporating ethanol
dissolving ethanol in water
13 Which statements explain why increasing the concentration of a reactant increases the rate of
reaction?
A
1
It increases the collision rate of particles.
2
It lowers the activation energy.
3
A greater proportion of the colliding molecules have the required activation energy.
4
There are more particles per unit volume.
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
14 When the colourless gas N2O4 is heated, it forms the brown gas NO2.
When the reaction mixture is cooled, the brown colour fades and turns back to colourless.
Which type of reaction is described by these observations?
A
decomposition
B
displacement
C
reduction
D
reversible
15 Water is added to anhydrous copper(II) sulfate.
What happens during the reaction?
A
The copper(II) sulfate turns blue and the solution formed gets colder.
B
The copper(II) sulfate turns blue and the solution formed gets hotter.
C
The copper(II) sulfate turns white and the solution formed gets colder.
D
The copper(II) sulfate turns white and the solution formed gets hotter.
© UCLES 2022
0620/22/M/J/22
7
16 Which arrow on the energy level diagram shows the overall energy change for an endothermic
reaction?
C
products
A
energy
D
B
reactants
progress of reaction
17 When a hydrogen–oxygen fuel cell is in operation, a different reaction happens at each electrode.
at the hydrogen electrode
H2  2H+ + 2e–
at the oxygen electrode
O2 + 2H2O + 4e–  4OH–
The electrons that are lost at the hydrogen electrode travel through the external circuit to the
oxygen electrode, where they are gained by the oxygen and water.
A hydrogen–oxygen fuel cell is operated for a period of time and four moles of oxygen molecules
are consumed.
Which mass of hydrogen is consumed?
A
2.0 g
B
4.0 g
C
8.0 g
D
16.0 g
18 The oxides of two elements, X and Y, are separately dissolved in water and the pH of each
solution tested.
oxide tested
pH of solution
X
1
Y
13
Which information about X and Y is correct?
oxide is
acidic
oxide is
basic
metal
non-metal
A
X
Y
X
Y
B
X
Y
Y
X
C
Y
X
X
Y
D
Y
X
Y
X
© UCLES 2022
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8
19 An acid is neutralised by adding an excess of an insoluble solid base.
A soluble salt is formed.
How is the pure salt obtained from the reaction mixture?
A
crystallisation  evaporation  filtration
B
evaporation  crystallisation  filtration
C
filtration  crystallisation  evaporation
D
filtration  evaporation  crystallisation
20 Substance J takes part in a redox reaction.
In the reaction, J gains electrons.
Which statement is correct?
A
J is the oxidising agent and it is oxidised in the reaction.
B
J is the oxidising agent and it is reduced in the reaction.
C
J is the reducing agent and it is oxidised in the reaction.
D
J is the reducing agent and it is reduced in the reaction.
21 Elements in Group IV of the Periodic Table are shown.
carbon
silicon
germanium
tin
lead
What does not occur in Group IV as it is descended?
A
The proton number of the elements increases.
B
The elements become more metallic.
C
The elements have more electrons in their outer shell.
D
The elements have more electron shells.
© UCLES 2022
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9
22 Which statement about acids is correct?
A
Acids are proton acceptors.
B
Acids transfer electrons to bases in aqueous solution.
C
Hydrochloric acid reacts with ammonium hydroxide to produce ammonia.
D
Ethanoic acid partially ionises in aqueous solution.
23 Which elements have both a high melting point and variable oxidation states?
A
alkali metals
B
transition elements
C
halogens
D
noble gases
24 Lithium, sodium and potassium are elements in Group I of the Periodic Table.
Chlorine, bromine and iodine are elements in Group VII of the Periodic Table.
Which row identifies the least dense of these elements in each group?
Group I
Group VII
A
lithium
chlorine
B
lithium
iodine
C
potassium
chlorine
D
potassium
iodine
© UCLES 2022
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10
25 The reactions of metals P, Q, R and S are shown.
metal
reaction
with water
reaction with
hydrochloric acid
reduction of the
metal oxide with carbon
P
no reaction
no reaction
reduced
Q
slow
vigorous
no reaction
R
vigorous
vigorous
no reaction
S
very slow
vigorous
reduced
What is the order of reactivity of the metals?
least
reactive
most
reactive
A
P
S
Q
R
B
P
Q
S
R
C
R
S
Q
P
D
R
Q
S
P
26 The number of protons and the number of neutrons in the atoms of elements X, Y and Z are
shown.
number of
protons
number of
neutrons
X
6
6
Y
7
6
Z
8
10
Which statement about the elements is correct?
A
X and Y are isotopes of the same element.
B
Z forms an ion with a +2 charge.
C
X and Z react together to form an ionic compound.
D
X, Y and Z are non-metals.
© UCLES 2022
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11
27 Which diagram represents the arrangement of atoms in an alloy?
A
B
C
D
28 Three metal compounds, J, K and L, are heated using a Bunsen burner.
The results are shown.
J
colourless gas produced, which relights a glowing splint
K
colourless gas produced, which turns limewater milky
L
no reaction
Which row identifies J, K and L?
J
K
L
A
magnesium carbonate
potassium carbonate
potassium nitrate
B
magnesium carbonate
potassium nitrate
potassium carbonate
C
potassium nitrate
magnesium carbonate
potassium carbonate
D
potassium nitrate
potassium carbonate
magnesium carbonate
29 Processes involved in the extraction of zinc are listed.
1
Heat zinc oxide with carbon.
2
Condense zinc vapour.
3
Vaporise the zinc.
4
Roast zinc ore in air.
In which order are the processes carried out?
A
1234
B
4312
C
4132
D
1432
© UCLES 2022
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12
30 Which process uses sacrificial protection to prevent steel from rusting?
A
galvanising
B
oiling
C
copper plating
D
painting
31 Fertilisers are used to provide three of the elements needed for plant growth.
Which two compounds would give a fertiliser containing all three of these elements?
A
Ca(NO3)2 and (NH4)2SO4
B
Ca(NO3)2 and (NH4)3PO4
C
KNO3 and (NH4)2SO4
D
KNO3 and (NH4)3PO4
32 Which processes produce carbon dioxide?
A
1
respiration
2
photosynthesis
3
fermentation
4
combustion of hydrogen
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
33 Which reaction in the Contact process requires the use of a catalyst?
A
S + O2  SO2
B
2SO2 + O2  2SO3
C
SO3 + H2SO4  H2S2O7
D
H2S2O7 + H2O  2H2SO4
34 What are the products when limestone (calcium carbonate) is heated strongly?
A
calcium hydroxide and carbon dioxide
B
calcium hydroxide and carbon monoxide
C
calcium oxide and carbon dioxide
D
calcium oxide and carbon monoxide
© UCLES 2022
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13
35 The structure of ester W is shown.
H
H
C
H
O
H
C
O
C
H
H
Which row gives the names of ester W and the carboxylic acid and alcohol from which it is made?
name of ester W
carboxylic acid
alcohol
A
ethyl methanoate
ethanoic acid
methanol
B
ethyl methanoate
methanoic acid
ethanol
C
methyl ethanoate
ethanoic acid
methanol
D
methyl ethanoate
methanoic acid
ethanol
36 Ethene reacts with substance X to form ethanol.
What is X?
A
ethanoic acid
B
glucose
C
hydrogen
D
steam
37 Alkenes can be produced by cracking large hydrocarbon molecules to form smaller hydrocarbon
molecules.
Which equations represent possible reactions when tetradecane, C14H30, is cracked?
A
1
C14H30  C2H6 + C3H6 + C4H8 + C5H10
2
C14H30  H2 + C2H4 + C3H6 + C4H8 + C5H10
3
C14H30  C2H6 + 4C3H6
4
C14H30  C2H6 + C3H8 + C9H18
1 only
© UCLES 2022
B
1 and 4
C
1, 2 and 3
0620/22/M/J/22
D
3 and 4
[Turn over
14
38 The structures of some hydrocarbons are shown.
1
2
H
H
H
C
C
C
3
H
H
H
H
C
C
C
C
H
H
H
H
H
H
H
H
H
H
H
H
H
H
C
C
H
H
4
H
H
H
C
H
H
H
H
C
C
C
H
H
H
Which statement about the hydrocarbons is correct?
A
1 and 2 have a different general formula.
B
1 and 4 are in different homologous series.
C
2 and 3 are structural isomers.
D
3 and 4 have the same empirical formula.
39 Ethane reacts with chlorine in the presence of ultraviolet light.
Which substances are produced in the reaction?
1
H
A
2
H
1, 2 and 3
© UCLES 2022
H
B
3
H
H
C
C
H
H
1 and 3 only
Cl
C
H
H
C
C
Cl
Cl
2, 3 and 4
0620/22/M/J/22
4
H
H
D
H
2 and 4 only
H
H
H
H
C
C
Cl
H
15
40 Which polymer structure has the same linkages as Terylene?
A
B
CH3
CH3
C
C
C
H
O
CH3 CH3 O
O
n
OH
C
C
C
H
H
C
n
D
H
CH3 CH3 O
CH3 CH3
N
C
C
C
C
H
H
H
H
C
n
O
n
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/22/M/J/22
© UCLES 2022
21
0620/22/M/J/22
calcium
40
38
Sr
strontium
88
56
Ba
barium
137
88
potassium
39
37
Rb
rubidium
85
55
Cs
caesium
133
87
22
cerium
140
90
Th
thorium
232
lanthanum
139
89
Ac
actinium
–
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
Ce
57
–
dubnium
Db
105
181
tantalum
Ta
73
93
niobium
Nb
41
51
vanadium
V
–
rutherfordium
Rf
104
178
hafnium
Hf
72
91
zirconium
Zr
40
48
titanium
La
lanthanoids
57–71
89
yttrium
Y
39
45
scandium
Ti
23
Cr
24
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
relative atomic mass
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Pt
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
49
70
gallium
Ga
31
27
aluminium
Al
13
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ca
K
–
actinoids
20
19
Ra
24
23
radium
magnesium
sodium
Fr
Mg
Na
francium
89–103
12
11
Sc
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
Group
The Periodic Table of Elements
16
Cambridge IGCSE™
*8853844180*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
October/November 2021
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 40.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Any blank pages are indicated.
IB21 11_0620_62/2RP
© UCLES 2021
[Turn over
2
1Carbon dioxide is a colourless gas that is denser than air.
Carbon dioxide can be made by reacting marble chips with dilute hydrochloric acid.
A student tried to make and collect carbon dioxide gas using the apparatus shown.
A
gas jar
C
B
(a) (i)Name the substances labelled A and B.
A ..........................................................................................................................................
B ..........................................................................................................................................
[1]
(ii)Name the item of apparatus labelled C.
........................................................................................................................................ [1]
(b)Explain why very little carbon dioxide gas would be collected using the apparatus shown.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2021
0620/62/O/N/21
3
(c)Complete the diagram to show how carbon dioxide gas could be collected and the volume
measured.
[2]
(d)At the end of the experiment there were unreacted marble chips and aqueous calcium chloride
in the item of apparatus labelled C.
Describe how you would find the mass of unreacted marble chips in apparatus C.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
© UCLES 2021
[Total: 9]
0620/62/O/N/21
[Turn over
4
2
student investigated the reaction between two different solutions of aqueous sodium carbonate,
A
solution K and solution L, and two different solutions of dilute hydrochloric acid, acid M and acid N.
Three experiments were done.
(a) Experiment 1
●
●
●
●
●
burette was filled with solution K. Some of solution K was run out of the burette so that
A
the level of solution K was on the burette scale.
Using a measuring cylinder 25 cm3 of acid M was poured into a conical flask.
Five drops of methyl orange indicator were added to the conical flask.
The conical flask was placed on a white tile.
Solution K was added slowly from the burette to the conical flask, while the flask was
swirled, until the solution just changed colour.
Use the burette diagrams to complete the table for Experiment 1.
7
31
8
32
9
33
initial reading
final reading
Experiment 1
final burette reading / cm3
initial burette reading / cm3
volume of solution K added / cm3
Experiment 2
●
●
●
●
●
●
© UCLES 2021
he conical flask was emptied and rinsed with distilled water.
T
The burette was refilled with solution K. Some of solution K was run out of the burette so
that the level of solution K was on the burette scale.
Using a measuring cylinder 25 cm3 of acid N was poured into the conical flask.
Five drops of methyl orange indicator were added to the conical flask.
The conical flask was placed on a white tile.
Solution K was added slowly from the burette to the conical flask, while the flask was
swirled, until the solution just changed colour.
0620/62/O/N/21
5
Use the burette diagrams to complete the table for Experiment 2.
3
15
4
16
5
17
initial reading
final reading
Experiment 2
final burette reading / cm3
initial burette reading / cm3
volume of solution K added / cm3
Experiment 3
●
●
●
●
●
●
●
he burette was emptied and rinsed with distilled water.
T
The conical flask was emptied and rinsed with distilled water.
The burette was filled with solution L. Some of solution L was run out of the burette so that
the level of solution L was on the burette scale.
Using a measuring cylinder 25 cm3 of acid N was poured into the conical flask.
Five drops of methyl orange indicator were added to the conical flask.
The conical flask was placed on a white tile.
Solution L was added slowly from the burette to the conical flask, while the flask was
swirled, until the solution just changed colour.
Use the burette diagrams to complete the table for Experiment 3.
2
26
3
27
4
28
initial reading
final reading
Experiment 3
final burette reading / cm3
initial burette reading / cm3
volume of solution L added / cm3
[5]
© UCLES 2021
0620/62/O/N/21
[Turn over
6
(b) State the colour change observed at the end-point in the conical flask in Experiment 1.
from ................................................................ to ���������������������������������������������������������������� [1]
(c)Describe one other observation made when solution K was added to acid M in Experiment 1.
............................................................................................................................................... [1]
(d) (i)Compare the volumes of solution K used in Experiment 1 and Experiment 2.
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)
Suggest why different volumes of solution K were needed in Experiment 1 and Experiment 2.
........................................................................................................................................ [1]
(e)Deduce the volume of solution L required to reach the end-point if Experiment 3 is repeated
using acid M in place of acid N.
volume of solution L = .............................. cm3 [1]
(f) Explain why the conical flask was rinsed with water at the start of Experiment 2 and Experiment 3.
............................................................................................................................................... [1]
(g)At the start of Experiment 3 the burette was rinsed with water.
Describe an additional step that should have been done after rinsing the burette with water but
before filling the burette with solution L. Explain your answer.
.....................................................................................................................................................
............................................................................................................................................... [2]
(h) Explain why the conical flask is placed on a white tile.
............................................................................................................................................... [1]
(i) Describe how the reliability of the results can be confirmed.
.....................................................................................................................................................
............................................................................................................................................... [1]
© UCLES 2021
0620/62/O/N/21
7
(j)State one source of error in Experiment 1. Suggest an improvement to reduce this error.
source of error ............................................................................................................................
improvement ...............................................................................................................................
[2]
© UCLES 2021
[Total: 18]
0620/62/O/N/21
[Turn over
8
3Solid O and liquid P were analysed. Solid O was ammonium bromide.
Tests were done on each substance.
tests on solid O
Complete the expected observations.
Solid O was dissolved in water to form solution O. Solution O was divided into four approximately
equal portions in four test‑tubes.
(a) To the first portion of solution O, approximately 2 cm3 of aqueous ammonia was added.
observations ......................................................................................................................... [1]
(b)To the second portion of solution O, approximately 2 cm3 of aqueous sodium hydroxide was
added. The mixture formed was warmed. A gas was given off.
(i)
The gas given off was tested with damp red litmus paper.
observations .................................................................................................................. [1]
(ii)
Identify the gas given off.
........................................................................................................................................ [1]
(c)To the third portion of solution O, approximately 1 cm3 of dilute nitric acid followed by a few
drops of aqueous silver nitrate were added.
observations ......................................................................................................................... [1]
(d)To the fourth portion of solution O, approximately 1 cm3 of aqueous chlorine was added.
observations ......................................................................................................................... [1]
© UCLES 2021
0620/62/O/N/21
9
tests on liquid P
tests
observations
A few drops of liquid P were placed in a
crucible. A lighted splint was applied to the
surface of liquid P in the crucible.
burned with an orange flame and lots of smoke;
soot was left around the top of the crucible
test 1
test 2
A few drops of liquid P were added to a
test‑tube containing 1 cm3 of aqueous
bromine.
colour changed from orange to colourless
(e)State what conclusions can be made about liquid P.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2021
[Total: 7]
0620/62/O/N/21
[Turn over
10
4
Cobalt is a metal. Cobalt is between copper and iron in the reactivity series. The mineral
spherocobaltite contains the compound cobalt(II) carbonate and no other metal ions.
Cobalt(II) carbonate is insoluble in water and reacts with dilute acids to form an aqueous solution
of a salt.
Describe how you would obtain a sample of cobalt metal starting with a large lump of spherocobaltite.
You have access to all normal laboratory apparatus and chemicals.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
© UCLES 2021
0620/62/O/N/21
11
BLANK PAGE
© UCLES 2021
0620/62/O/N/21
12
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/62/O/N/21
Cambridge IGCSE™
*8417627571*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
October/November 2021
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 80.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB21 11_0620_42/3RP
© UCLES 2021
[Turn over
2
1This question is about states of matter.
(a)Complete the table, using ticks ( ) and crosses ( ), to describe the properties of gases, liquids
and solids.
state of matter
particles
are touching
particles have
random movement
particles are
regularly arranged
gas
liquid
solid
[3]
(b)Substances can change state.
(i)Boiling and evaporation are two ways in which a liquid changes into a gas.
Describe two differences between boiling and evaporation.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(ii)Name the change of state when:
●
a gas becomes a liquid .................................................................................................
● a solid becomes a gas. .................................................................................................
[2]
© UCLES 2021
0620/42/O/N/21
3
(c)A substance boils at temperature X and melts at temperature Y.
Complete the graph to show the change in temperature over time as the substance cools from
temperature A to temperature B.
A
X
temperature
Y
B
time
[2]
(d)A solution is a mixture of a solute and a solvent.
(i)Name the process when a solid substance mixes with a solvent to form a solution.
........................................................................................................................................ [1]
(ii)Name the type of reaction when two solutions react to form an insoluble substance.
........................................................................................................................................ [1]
© UCLES 2021
[Total: 11]
0620/42/O/N/21
[Turn over
4
2Acids are important laboratory chemicals.
(a)Some acids completely dissociate in water to form ions.
(i)State the term applied to acids that completely dissociate in water.
........................................................................................................................................ [1]
(ii)Complete the equation to show the complete dissociation of sulfuric acid in water.
H2SO4 → .....................................................................................
[2]
(iii)State the colour of methyl orange in sulfuric acid.
........................................................................................................................................ [1]
(b)The equation for the reaction between powdered zinc carbonate and dilute nitric acid is shown.
ZnCO3....... + 2HNO3....... → Zn(NO3)2....... + H2O....... + CO2.......
(i)Complete the equation by adding state symbols.
[2]
(ii)A student found that 2.5 g of zinc carbonate required 20 cm3 of dilute nitric acid to react
completely.
Calculate the concentration of dilute nitric acid using the following steps:
●
calculate the mass of 1 mole of ZnCO3
.............................. g
●
calculate the number of moles of ZnCO3 reacting
.............................. moles
●
determine the number of moles of HNO3 reacting
.............................. moles
●
calculate the concentration of HNO3.
.............................. mol / dm3
[4]
© UCLES 2021
[Total: 10]
0620/42/O/N/21
5
3Atoms contain protons, neutrons and electrons.
(a)Complete the table to show the relative mass and the relative charge of a proton, a neutron
and an electron.
relative mass
relative charge
proton
neutron
1
1840
electron
[3]
(b)The table shows the number of protons, neutrons and electrons in some atoms and ions.
Complete the table.
atom
or ion
number of
protons
number of
neutrons
number of
electrons
35
44
36
32
16S
39 +
19K
[5]
© UCLES 2021
[Total: 8]
0620/42/O/N/21
[Turn over
6
4Chlorine reacts with carbon monoxide to produce phosgene gas, COCl 2(g). A catalyst is used.
Cl 2(g) + CO(g)
COCl 2(g)
The reaction is exothermic.
(a)Explain why the reaction is exothermic in terms of the energy changes of bond breaking and
bond making.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(b) (i)Complete the energy level diagram for this reaction.
On your diagram show:
●
●
●
the product of the reaction
an arrow representing the energy change, labelled ∆H
an arrow representing the activation energy, labelled A.
energy
Cl 2(g) + CO(g)
progress of reaction
[3]
(ii)State why a catalyst is used.
........................................................................................................................................ [1]
© UCLES 2021
0620/42/O/N/21
7
(c)Describe and explain the effect, if any, on the position of equilibrium when:
(i)the pressure is increased
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)the temperature is increased.
..............................................................................................................................................
........................................................................................................................................ [2]
(d)The reaction between chlorine and carbon monoxide can be represented as shown.
O
Cl
Cl
+
CO
Cl
C
Cl
When one mole of chlorine reacts with one mole of carbon monoxide, 230 kJ of energy is
released.
Some bond energies are shown in the table.
bond
bond energy in kJ / mol
Cl –Cl
240
C=O
745
C–Cl
400
Use the information to calculate the energy of the bond between the C and the O in
carbon monoxide, CO.
© UCLES 2021
bond energy in carbon monoxide, CO = .............................. kJ / mol [3]
0620/42/O/N/21
[Turn over
8
(e)Complete the dot-and-cross diagram to show the electron arrangement in a molecule of COCl 2.
O
Cl
C
Cl
Show outer electrons only.
O
C
Cl
Cl
[3]
© UCLES 2021
[Total: 17]
0620/42/O/N/21
9
5Iron is a transition element. Potassium is a Group I element.
(a)Iron and potassium have the same type of bonding.
Name and describe the type of bonding in these two elements.
name ...........................................................................................................................................
description ..................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
[4]
(b)Transition elements and Group I elements have some similar physical properties.
They can both:
●
●
●
e hammered into a shape
b
conduct electricity
be stretched into wires.
(i)Name the term used to describe the ability of elements to be hammered into a shape.
........................................................................................................................................ [1]
(ii)Describe what happens to the particles in iron when it is hammered into a shape.
..............................................................................................................................................
........................................................................................................................................ [1]
(iii)Suggest why copper, rather than other transition elements, is used for wires which conduct
electricity.
........................................................................................................................................ [1]
(c)Transition elements are harder and stronger than Group I elements.
Describe how two other physical properties of transition elements are different from those of
Group I elements.
1 ..................................................................................................................................................
2 ..................................................................................................................................................
[2]
© UCLES 2021
0620/42/O/N/21
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10
(d)Chemical properties of some Group I elements are shown in the table.
element
reaction with cold water
reaction with oxygen
flame test
colour
red
lithium
●
●
steadily effervesces
forms a colourless solution
very slowly forms an oxide layer
sodium
●
●
strongly effervesces
forms a colourless solution
slowly forms an oxide layer
potassium
●
●
v ery strongly effervesces
forms a colourless solution
quickly forms an oxide layer
rubidium
ruby red
(i)Add to the table:
● the flame test colours for sodium and potassium
● the predicted reactions of rubidium with water and with oxygen.
[4]
(ii)Name the gas produced when Group I elements react with water.
........................................................................................................................................ [1]
(iii)Name the solution formed when potassium reacts with water.
........................................................................................................................................ [1]
(iv)Predict the pH of the colourless solution formed when potassium reacts with water.
........................................................................................................................................ [1]
(v)Write the chemical equation for the reaction of sodium with oxygen.
........................................................................................................................................ [2]
(e)Iron is a typical transition element. It is the catalyst used in the Haber process.
(i)Write the equation for the reaction that occurs in the Haber process.
........................................................................................................................................ [2]
(ii)State the temperature and pressure used in the Haber process. Include units.
temperature .........................................................................................................................
pressure ...............................................................................................................................
[2]
© UCLES 2021
[Total: 22]
0620/42/O/N/21
11
6Ethanol, C2H5OH, belongs to the homologous series called alcohols.
(a)Write the general formula of alcohols.
............................................................................................................................................... [1]
(b)Explain why ethanol cannot be described as a hydrocarbon.
............................................................................................................................................... [1]
(c)Ethanol can be manufactured from different substances by reaction with steam or by
fermentation.
(i)Give the formula of the substance which reacts with steam to form ethanol.
........................................................................................................................................ [1]
(ii)Name a substance which will undergo fermentation to form ethanol.
........................................................................................................................................ [1]
(d)Ethanol is a fuel.
Write the chemical equation for the complete combustion of ethanol.
............................................................................................................................................... [2]
© UCLES 2021
0620/42/O/N/21
[Turn over
12
(e)Ethane-1,2-diol has two alcohol functional groups.
H
O
H
H
C
C
H
H
O
H
One molecule of ethane-1,2-diol will react with two molecules of ethanoic acid to form
molecule X.
X has two ester functional groups and a molecular formula of C6H10O4.
(i)State the empirical formula of X.
........................................................................................................................................ [1]
(ii)Draw the structure of X.
Show all of the atoms and all of the bonds.
[2]
(iii)Name the other substance formed in this reaction.
........................................................................................................................................ [1]
(f)Each alcohol functional group in ethane-1,2-diol reacts with acidified potassium manganate(VII)
to form a different organic compound, Y.
(i)Name the functional groups formed in Y.
........................................................................................................................................ [1]
(ii)Draw the structure of Y.
Show all of the atoms and all of the bonds.
[1]
© UCLES 2021
[Total: 12]
0620/42/O/N/21
13
BLANK PAGE
© UCLES 2021
0620/42/O/N/21
14
BLANK PAGE
© UCLES 2021
0620/42/O/N/21
15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/42/O/N/21
© UCLES 2021
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/O/N/21
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
October/November 2021
45 minutes
You must answer on the multiple choice answer sheet.
*8181221372*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
 There are forty questions on this paper. Answer all questions.
 For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
 Follow the instructions on the multiple choice answer sheet.
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
 Do not use correction fluid.
 Do not write on any bar codes.
 You may use a calculator.
INFORMATION
 The total mark for this paper is 40.
 Each correct answer will score one mark.
 Any rough working should be done on this question paper.
 The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB21 11_0620_22/3RP
© UCLES 2021
[Turn over
2
1
An experiment is set up as shown.
cotton wool soaked
in ammonia
cotton wool soaked
in hydrochloric acid
After several minutes, a white ring of ammonium chloride appears as shown.
ammonium chloride
Which statement explains the observation after several minutes?
2
A
Ammonia gas diffuses faster than hydrogen chloride gas because its molecules have a lower
molecular mass.
B
Ammonia gas diffuses faster than hydrogen chloride gas because its molecules have a
higher molecular mass.
C
Ammonia gas diffuses slower than hydrogen chloride gas because its molecules have a
lower molecular mass.
D
Ammonia gas diffuses slower than hydrogen chloride gas because its molecules have a
higher molecular mass.
A student put exactly 25.00 cm3 of dilute hydrochloric acid into a conical flask.
The student added 2.5 g of solid sodium carbonate and measured the change in temperature of
the mixture.
Which apparatus does the student need to use?
A
balance, measuring cylinder, thermometer
B
balance, pipette, stopwatch
C
balance, pipette, thermometer
D
burette, pipette, thermometer
© UCLES 2021
0620/22/O/N/21
3
3
A student separates sugar from pieces of broken glass by dissolving the sugar in water and
filtering off the broken glass.
filtrate
What is the filtrate?
4
5
A
broken glass only
B
broken glass and sugar solution
C
pure water
D
sugar solution
How many protons, neutrons and electrons are there in one atom of the isotope 27
13 Al ?
protons
neutrons
electrons
A
13
13
13
B
13
14
13
C
14
13
13
D
14
14
13
Which description of brass is correct?
A
alloy
B
compound
C
element
D
non-metal
© UCLES 2021
0620/22/O/N/21
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4
6
Some properties of diamond are shown.
1
It is very hard.
2
Every atom forms four bonds.
3
It does not conduct electricity.
Which properties are also shown by silicon(IV) oxide?
A
7
8
9
1 only
B
1 and 2
C
1 and 3
D
2 and 3
Which statement describes the attractive forces between molecules?
A
They are strong covalent bonds which hold molecules together.
B
They are strong ionic bonds which hold molecules together.
C
They are weak forces formed between covalently-bonded molecules.
D
They are weak forces which hold ions together in a lattice.
Which substance is described as a macromolecule?
A
ammonia
B
graphite
C
iron
D
sodium chloride
The equation for the reaction of sodium with water is shown.
2Na + 2H2O  2NaOH + H2
What is the volume of hydrogen gas, measured at r.t.p., produced when 18.4 g of sodium reacts
with excess water?
9.6 dm3
A
B
15.0 dm3
C
19.2 dm3
D
30.0 dm3
10 Iron can be electroplated with zinc to make it resistant to corrosion.
Which row about electroplating iron with zinc is correct?
positive electrode
(anode)
negative electrode
(cathode)
electrolyte
A
iron
zinc
iron nitrate
B
iron
zinc
zinc nitrate
C
zinc
iron
iron nitrate
D
zinc
iron
zinc nitrate
© UCLES 2021
0620/22/O/N/21
5
11 Chlorine reacts with ethane to produce chloroethane and hydrogen chloride.
H
H
H
C
C
H
H
H
+
Cl
Cl
H
H
H
C
C
H
H
Cl
+
H
Cl
The reaction is exothermic.
The bond energies are shown in the table.
bond
bond energy
in kJ / mol
C–Cl
+340
C–C
+350
C–H
+410
Cl –Cl
+240
H–Cl
+430
What is the energy change for the reaction?
A
–1420 kJ / mol
B
–120 kJ / mol
C
+120 kJ / mol
D
+1420 kJ / mol
12 Chlorine gas is bubbled into aqueous potassium iodide.
What is the ionic equation for the reaction that takes place?
A
Cl + I–  Cl – + I
B
Cl 2 + 2I–  Cl 2– + I2
C
Cl 2 + 2I–  2Cl – + I2
D
Cl 2 + 2I–  2Cl – + 2I
13 Concentrated aqueous sodium chloride is electrolysed.
Which equation represents the reaction at the cathode?
A
Na+ + e–  Na
B
2O2–  O2 + 4e–
C
2H+ + 2e–  H2
D
2Cl –  Cl 2 + 2e–
© UCLES 2021
0620/22/O/N/21
[Turn over
6
14 Which statements about hydrogen are correct?
A
1
When hydrogen is burned, heat energy is released.
2
When hydrogen is used in a fuel cell, electrical energy is generated.
3
When hydrogen is used as a fuel, water is the only product.
1, 2 and 3
B
1 and 2 only
C
1 only
D
3 only
15 Solid X is heated strongly.
The colour of the solid changes from blue to white.
What is solid X?
A
anhydrous cobalt(II) chloride
B
calcium carbonate
C
hydrated copper(II) sulfate
D
lead(II) bromide
16 Iron(II) chloride solution reacts with chlorine gas.
The equation is shown.
2FeCl 2(aq) + Cl 2(g)  2FeCl 3(aq)
Which statements about this reaction are correct?
A
1
Fe2+ ions are reduced to Fe3+ ions.
2
Chlorine acts as a reducing agent.
3
Fe2+ ions each lose an electron.
4
Cl 2 molecules are reduced to Cl – ions.
1 and 2
B
2 and 3
C
2 and 4
D
3 and 4
17 Which statements about acids and bases are correct?
A
1
An acid reacts with a metal to give off hydrogen.
2
A base reacts with an ammonium salt to give off ammonia.
3
An acid reacts with a carbonate to give off carbon dioxide.
4
Alkaline solutions are orange in methyl orange.
1, 2 and 3
© UCLES 2021
B
1, 2 and 4
C
1, 3 and 4
0620/22/O/N/21
D
2, 3 and 4
7
18 Oxide 1 is a solid that reacts with dilute hydrochloric acid.
Oxide 2 is a gas that reacts with sodium hydroxide solution.
What are the formulae of the oxides?
oxide 1
oxide 2
A
CaO
MgO
B
MgO
NO2
C
NO2
SO2
D
SO2
CaO
19 Which reaction is a photochemical reaction?
A
addition of bromine to propene
B
esterification of ethanol and ethanoic acid
C
oxidation of ethanol
D
substitution of methane with chlorine
20 The equation shown represents a reaction at equilibrium.
m and n represent the balancing numbers for the reactant and product respectively.
mP(g)
nQ(g)
A high temperature increases the concentration of Q.
A high pressure increases the concentration of Q.
Which statement about the reaction is correct?
A
The forward reaction is exothermic and m is greater than n.
B
The forward reaction is exothermic and m is less than n.
C
The forward reaction is endothermic and m is greater than n.
D
The forward reaction is endothermic and m is less than n.
© UCLES 2021
0620/22/O/N/21
[Turn over
8
21 A period of the Periodic Table is shown.
group
I
II
III
IV
V
VI
VII
VIII
element
R
S
T
V
W
X
Y
Z
The letters are not their chemical symbols.
Which statement is correct?
A
Element R does not conduct electricity.
B
Elements R and Y react together to form an ionic compound.
C
Element Z exists as a diatomic molecule.
D
Element Z reacts with element T.
22 All metal nitrates are soluble in water.
All metal chlorides are soluble except silver and lead.
All metal carbonates are insoluble except sodium and potassium.
Which aqueous solutions produce a precipitate when mixed together?
A
1
silver nitrate + sodium carbonate
2
silver nitrate + sodium chloride
3
barium nitrate + potassium chloride
1 and 2 only
B
1 and 3 only
C
2 and 3 only
D
1, 2 and 3
23 Which row describes properties of transition elements?
property 1
property 2
property 3
A
coloured compounds
high density
variable oxidation states
B
high density
high melting point
one oxidation state
C
high melting point
coloured compounds
one oxidation state
D
low melting point
high density
variable oxidation states
© UCLES 2021
0620/22/O/N/21
9
24 The noble gases are in Group VIII of the Periodic Table.
Which statement explains why noble gases are unreactive?
A
They all have eight electrons in their outer shells.
B
They all have full outer shells.
C
They are all gases.
D
They are all monoatomic.
25 Which statement is correct for all metals?
A
They conduct electricity when molten.
B
They gain electrons when they form ions.
C
They have a low density.
D
They have a low melting point.
26 Carbon dioxide is produced during the extraction of aluminium from bauxite.
Which statement describes how this carbon dioxide is made?
A
Carbon monoxide reduces aluminium oxide forming carbon dioxide and aluminium.
B
Carbon is burned in the blast furnace to release heat energy.
C
Oxygen made in the process reacts with the carbon electrode.
D
The ore of aluminium undergoes thermal decomposition.
27 Aluminium objects do not need protection from corrosion.
Iron objects must be protected from corrosion.
Which statement explains why aluminium resists corrosion?
A
Aluminium does not form ions easily.
B
Aluminium does not react with water or air.
C
Aluminium has a protective oxide layer.
D
Aluminium is below iron in the reactivity series.
© UCLES 2021
0620/22/O/N/21
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10
28 Which statements explain why zinc is used to protect iron from rusting?
A
1
Zinc is more reactive than iron.
2
Zinc is less reactive than iron.
3
Zinc can form alloys with iron.
4
Zinc acts as a sacrificial metal.
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
29 Which conditions are used in the Haber process?
temperature
/ C
pressure
/ atmospheres
A
100
10
B
450
10
C
450
200
D
1000
500
30 Which process does not produce a greenhouse gas?
A
acid rain on limestone buildings
B
combustion of wood
C
digestion in cows
D
zinc reacting with sulfuric acid
31 Which reaction involving sulfur dioxide is correct?
A
It is produced during the extraction of zinc from zinc blende.
B
It reacts with concentrated sulfuric acid to form oleum.
C
It reacts with sulfur to form sulfur trioxide.
D
It turns an acidified solution of potassium manganate(VII) purple.
32 Lime (calcium oxide) is used to treat waste water from a factory.
Which substance is removed by the lime?
A
ammonia
B
sodium chloride
C
sodium hydroxide
D
sulfuric acid
© UCLES 2021
0620/22/O/N/21
11
33 What is the structure of the ester formed from ethanoic acid and propanol?
A
H
H
H
C
C
H
H
B
O
C
H
H
C
C
H
H
H
H
H
C
C
H
H
O
C
H
O
H
C
H
H
H
C
O
H
D
C
H
H
C
H
O
C
H
C
O
C
H
H
H
C
C
C
H
H
H
H
H
C
H
H
H
C
H
H
H
O
H
C
O
H
34 Fuel X produces carbon dioxide and water when it is burned in air. So does fuel Y.
What could X and Y be?
X
Y
A
C
H2
B
C
C8H18
C
CH4
H2
D
CH4
C8H18
© UCLES 2021
0620/22/O/N/21
[Turn over
12
35 The structures of four organic molecules are shown.
H
H
H
O
C
Cl
H
C
O
H
H
H
H
H
C
C
H
H
O
O
H
H
H
How many different homologous series are represented by these molecules?
A
1
B
2
C
3
D
4
36 Which statement about ethene is correct?
A
It has the chemical formula C2H6.
B
It burns in excess oxygen producing carbon dioxide and water.
C
It reacts with Br2 to produce an orange solution.
D
It reacts with oxygen to form ethanol.
37 Ethanol is manufactured by fermentation of sugars or by catalytic hydration of ethene.
Which row states an advantage of each method?
fermentation
hydration
A
produces purer ethanol
is a batch process
B
produces purer ethanol
is a continuous process
C
uses a renewable resource
is a batch process
D
uses a renewable resource
is a continuous process
38 Which statements about unsaturated hydrocarbons are correct?
A
1
They contain both single and double bonds.
2
They turn aqueous bromine from colourless to brown.
3
They can be manufactured by cracking.
1 and 2 only
© UCLES 2021
B
1 and 3 only
C
2 and 3 only
0620/22/O/N/21
D
C
1, 2 and 3
H
13
39 Which polymers have the same linkage between monomer units?
A
carbohydrate and polyamide
B
carbohydrate and polyester
C
protein and polyamide
D
protein and polyester
40 The diagram shows the partial structure of Terylene.
O
C
O
O
O
O
C
C
O
From which pair of compounds is it made?
A
HO
O
O
C
C
OH
+
HO
OH
O
B
C
D
HO
C
HO
HO
© UCLES 2021
O
OH
+
OH
+
O
O
C
C
OH
+
HO
HO
HO
C
OH
O
O
C
C
O
O
C
C
0620/22/O/N/21
OH
OH
14
BLANK PAGE
© UCLES 2021
0620/22/O/N/21
15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
0620/22/O/N/21
© UCLES 2021
21
0620/22/O/N/21
22
cerium
140
90
Th
thorium
232
lanthanum
139
89
Ac
actinium
–
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
Ce
57
La
–
dubnium
Db
105
181
tantalum
Ta
73
93
niobium
Nb
41
51
vanadium
V
–
rutherfordium
Rf
104
178
hafnium
Hf
72
91
zirconium
Zr
40
48
titanium
Ti
23
Cr
24
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
relative atomic mass
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Pt
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
49
70
gallium
Ga
31
27
aluminium
Al
13
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
–
actinoids
Ra
radium
88
87
Fr
137
francium
89–103
barium
133
lanthanoids
57–71
89
yttrium
caesium
Y
39
Ba
38
37
45
scandium
Cs
40
39
56
calcium
potassium
Sc
55
Ca
K
88
20
19
strontium
24
23
85
magnesium
sodium
rubidium
Mg
Na
Sr
12
11
Rb
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
Group
The Periodic Table of Elements
16
Cambridge IGCSE™
*9457558127*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
May/June 2022
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 40.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Any blank pages are indicated.
IB22 06_0620_62/3RP
© UCLES 2022
[Turn over
2
1Sodium hydrogencarbonate decomposes when heated. The products are solid sodium carbonate,
water and carbon dioxide.
A student decomposed a sample of sodium hydrogencarbonate using the apparatus shown.
A
X
delivery tube
sodium
hydrogencarbonate
B
water
(a)Name the items of apparatus labelled A and B.
A .................................................................................................................................................
B ................................................................................................................................................
[2]
(b)When the sodium hydrogencarbonate was heated, a colourless liquid collected at the point
marked X.
Suggest the identity of the colourless liquid.
............................................................................................................................................... [1]
(c)
On the diagram draw one arrow to show where the apparatus should be heated during the
experiment.[1]
(d)State an observation that would indicate the sodium hydrogencarbonate had stopped reacting.
.....................................................................................................................................................
............................................................................................................................................... [1]
(e)Explain why it is important to remove the delivery tube from the water as soon as heating is
stopped.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2022
[Total: 7]
0620/62/M/J/22
3
2
student investigated the reaction between two different solutions of aqueous sodium carbonate,
A
solution K and solution L, and dilute hydrochloric acid using two different indicators.
Two experiments were done.
Experiment 1
● A burette was rinsed with water and then with the dilute hydrochloric acid.
● The burette was filled with dilute hydrochloric acid. Some of the dilute hydrochloric acid was
run out of the burette so that the level of the dilute hydrochloric acid was on the burette scale.
● Using a measuring cylinder, 25 cm3 of solution K was poured into a conical flask.
● Five drops of methyl orange indicator and five drops of thymolphthalein indicator were added
to the conical flask.
● The conical flask was placed on a white tile.
● Dilute hydrochloric acid was added slowly from the burette to the conical flask, while the flask
was swirled, until the solution turned yellow. This is the first colour change.
● More dilute hydrochloric acid from the burette was added to the conical flask, while swirling the
flask, until the solution changed colour again. This is the second colour change.
(a)Use the burette diagrams to complete the table for Experiment 1.
1
11
22
2
12
23
3
13
24
initial burette reading
burette reading at
first colour change
burette reading at
second colour change
Experiment 1
burette reading at first colour change / cm3
final burette reading at second colour change / cm3
initial burette reading / cm3
volume of dilute hydrochloric acid added for first
colour change / cm3
total volume of dilute hydrochloric acid added for
second colour change / cm3
[3]
© UCLES 2022
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4
(b)
Experiment 2
● The conical flask was emptied and rinsed with distilled water.
● Experiment 1 was repeated using solution L instead of solution K.
Use the burette diagrams to complete the table for Experiment 2.
3
19
35
4
20
36
5
21
37
initial burette reading
burette reading at
first colour change
burette reading at
second colour change
Experiment 2
burette reading at first colour change / cm3
final burette reading at second colour change / cm3
initial burette reading / cm3
volume of dilute hydrochloric acid added for first
colour change / cm3
total volume of dilute hydrochloric acid added for
second colour change / cm3
[3]
(c)State the colour change observed at the end-point when dilute hydrochloric acid is added to
methyl orange in an alkaline solution.
from ................................................................ to ................................................................. [1]
(d) For Experiment 1, compare the volume of dilute hydrochloric acid needed for the first colour
change with the volume of dilute hydrochloric acid for the second colour change.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2022
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5
(e)Compare the concentration of solution K used in Experiment 1 to the concentration of solution L
used in Experiment 2.
Explain your answer.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
(f) (i)Deduce the volume of dilute hydrochloric acid needed for the second colour change when
Experiment 2 is repeated using 50 cm3 of solution L.
........................................................................................................................................ [2]
(ii)State why using 50 cm3 of solution L would cause a problem.
..............................................................................................................................................
........................................................................................................................................ [1]
(g)State the advantage of using a pipette instead of the measuring cylinder in these experiments.
............................................................................................................................................... [1]
(h) Explain why the conical flask was swirled as the dilute hydrochloric acid was added from the
burette.
.....................................................................................................................................................
............................................................................................................................................... [1]
(i)
At the start of Experiment 1, the burette was rinsed with water and then with dilute
hydrochloric acid.
At the start of Experiment 2, the conical flask was rinsed with water but not with solution L.
(i)
Explain why the conical flask was rinsed with water.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)
Explain why the conical flask was not rinsed with solution L in Experiment 2.
..............................................................................................................................................
........................................................................................................................................ [1]
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6
3Solid M and solid N were analysed. Solid M was iron(III) nitrate.
Tests were done on each substance.
tests on solid M
Complete the expected observations.
Solid M was dissolved in water to form solution M. Solution M was divided into two approximately
equal portions in two test-tubes.
(a) T
o the first portion of solution M, aqueous sodium hydroxide was added gradually until in
excess. The product was kept for (b).
observations ...............................................................................................................................
............................................................................................................................................... [2]
(b) (i)The product from (a) was transferred to a boiling tube. A piece of aluminium foil was added
and the mixture warmed gently. Any gas produced was tested.
observations ........................................................................................................................
........................................................................................................................................ [1]
(ii)Identify the gas made in (i).
........................................................................................................................................ [1]
(c)To the second portion of solution M, about 1 cm depth of dilute nitric acid followed by a few
drops of aqueous barium nitrate were added.
observations ......................................................................................................................... [1]
© UCLES 2022
0620/62/M/J/22
7
tests on solid N
tests
observations
test 1
A flame test was carried out on solid N.
the flame became red
Solid N was dissolved in water to form
solution N. Solution N was divided equally into
one test-tube and one boiling tube.
test 2
About 1 cm depth of dilute nitric acid followed
by a few drops of aqueous silver nitrate were
added to the first portion of solution N in a
test‑tube.
no visible change
test 3
About 2 cm depth of dilute hydrochloric acid
was added to the second portion of solution N.
The mixture was warmed and any gas
produced was tested.
acidified aqueous potassium manganate(VII)
changed from purple to colourless
(d) Identify the gas produced in test 3.
............................................................................................................................................... [1]
(e)Identify solid N.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2022
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8
4
The diagram shows some coffee beans.
Caffeine occurs naturally in coffee beans. Caffeine is a white crystalline solid. It is very soluble in
hot water but much less soluble in cold water.
Plan an investigation to obtain a pure crystalline sample of caffeine from coffee beans.
Assume that all other soluble substances in coffee beans are very soluble in both hot and cold
water.
You are provided with coffee beans and common laboratory apparatus.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
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10
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© UCLES 2022
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11
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© UCLES 2022
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Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/62/M/J/22
Cambridge IGCSE™
*6148594183*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
May/June 2022
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 80.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB22 06_0620_42/3RP
© UCLES 2022
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2
1The symbols of the elements of Period 3 of the Periodic Table are shown.
Na
Mg
Al
Si
P
S
Cl
Ar
Answer the following questions about these elements.
Each symbol may be used once, more than once or not at all.
Write the symbol of the element which:
(a)forms a stable ion with a 2+ charge ������������������������������������������������������������������������������������� [1]
(b)is the least reactive in the period ����������������������������������������������������������������������������������������� [1]
(c)is used in water treatment ��������������������������������������������������������������������������������������������������� [1]
(d)forms an oxide which is the main impurity in iron ore ���������������������������������������������������������� [1]
(e)is an important component of fertilisers ������������������������������������������������������������������������������� [1]
(f)is stored under oil ���������������������������������������������������������������������������������������������������������������� [1]
(g)is used in food containers ���������������������������������������������������������������������������������������������������� [1]
(h)is found in the ore zinc blende. �������������������������������������������������������������������������������������������� [1]
© UCLES 2022
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3
Question 2 starts on the next page.
© UCLES 2022
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4
2Calcium hydroxide, Ca(OH)2, is slightly soluble in water.
(a)Calcium hydroxide can be made by the reaction of calcium with water.
(i)Write the chemical equation for this reaction.
........................................................................................................................................ [2]
(ii)Name another substance that reacts with water to form calcium hydroxide.
........................................................................................................................................ [1]
(b)When calcium hydroxide dissolves in water, it dissociates into ions and forms a weakly alkaline
solution.
(i)Suggest the pH of aqueous calcium hydroxide.
........................................................................................................................................ [1]
(ii)Give the formula of the ion responsible for making the solution alkaline.
........................................................................................................................................ [1]
(c)Limewater is a saturated solution of calcium hydroxide, Ca(OH)2(aq).
(i)Name the gas limewater is used to test for.
........................................................................................................................................ [1]
(ii)Suggest what is meant by the term saturated solution.
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)Describe how you would make a sample of limewater starting with solid calcium hydroxide.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iv)Describe how you would test for the presence of calcium ions in a sample of limewater.
test .......................................................................................................................................
observations ........................................................................................................................
..............................................................................................................................................
[3]
© UCLES 2022
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5
(d)A 25.0 cm3 sample of limewater is placed in a conical flask. The concentration of Ca(OH)2 in the
limewater is determined by titration with dilute hydrochloric acid, HCl.
(i)Name the item of apparatus used to measure the volume of acid in this titration.
........................................................................................................................................ [1]
(ii)State the type of reaction which takes place.
........................................................................................................................................ [1]
(iii)As well as limewater and dilute hydrochloric acid, state what other type of substance must
be added to the conical flask.
........................................................................................................................................ [1]
(iv)The equation for the reaction is shown.
Ca(OH)2 + 2HCl → CaCl 2 + 2H2O
20.0 cm3 of 0.0500 mol / dm3 HCl reacts with the 25.0 cm3 of Ca(OH)2.
Determine the concentration of Ca(OH)2 in g / dm3. Use the following steps.
●
Calculate the number of moles in 20.0 cm3 of 0.0500 mol / dm3 HCl.
.............................. mol
●
Determine the number of moles of Ca(OH)2 in 25.0 cm3 of the limewater.
.............................. mol
●
Calculate the concentration of Ca(OH)2 in mol / dm3.
.............................. mol / dm3
●
Determine the concentration of Ca(OH)2 in g / dm3.
.............................. g / dm3
[5]
© UCLES 2022
[Total: 21]
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6
3Transition elements are found in the middle block of the Periodic Table.
(a)Chromium has several isotopes. Manganese has only one isotope.
(i)State what is meant by the term isotopes.
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)State the nucleon number of manganese.
........................................................................................................................................ [1]
52
Cr3+ ion.
(iii)Complete the table to show the number of protons, neutrons and electrons in a 24
protons
neutrons
electrons
[3]
(b)One chemical property of transition elements is that they form coloured compounds.
(i)Give the colours of the following hydrated salts.
●
hydrated copper(II) sulfate ������������������������������������������������������������������������������������������
● hydrated cobalt(II) chloride �����������������������������������������������������������������������������������������
[2]
(ii)State two other chemical properties of transition elements.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(c) T
ransition elements and Group I elements are metals. They share many physical properties
including the ability to:
● conduct electricity
● be hammered into shape.
(i)Explain why transition elements and Group I elements conduct electricity.
........................................................................................................................................ [1]
(ii)State the property that describes a material which can be hammered into shape.
........................................................................................................................................ [1]
© UCLES 2022
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7
(d)Transition elements and Group I elements differ in other physical properties. Transition
elements are harder and stronger than Group I elements.
Describe two other ways in which the physical properties of transition elements differ from
Group I elements.
1 ..................................................................................................................................................
2 ..................................................................................................................................................
[2]
© UCLES 2022
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8
4Fluorine and chlorine are halogens.
(a)Suggest the appearance of fluorine.
............................................................................................................................................... [1]
(b)Fluorine reacts with sulfur to form a compound which has 25.2% sulfur by mass and a relative
molecular mass of 254.
Determine the molecular formula of this compound.
molecular formula = .............................. [3]
(c)Nitrogen trichloride, NCl 3, is a covalent compound.
Complete the dot-and-cross diagram to show the electron arrangement in a molecule of NCl 3.
Show outer electrons only.
Cl
N
Cl
Cl
[3]
© UCLES 2022
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9
(d)Lithium chloride, LiCl, is an ionic compound.
Complete the dot-and-cross diagram to show the electron arrangement and charges of the
ions in lithium chloride.
.....
Li
.....
Cl
[3]
(e)Explain, in terms of attractive forces between particles, why LiCl is a solid at room temperature
but NCl 3 is a liquid with a relatively low boiling point.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
© UCLES 2022
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10
5The reaction scheme shows five organic reactions, numbered 1 to 5.
carbon dioxide + water
2
sugar
1
3
ethanol
alkene A
4
alkane B
5
compound C
(a)Name reaction 1.
............................................................................................................................................... [1]
(b)Name reaction 2 and write the chemical equation for this reaction.
name ...........................................................................................................................................
equation ......................................................................................................................................
[3]
(c)Reaction 3 forms ethanol from alkene A.
(i)Identify alkene A.
........................................................................................................................................ [1]
(ii)State the type of reaction that occurs during reaction 3.
........................................................................................................................................ [1]
(iii)State the reagents and conditions needed for reaction 3.
..............................................................................................................................................
........................................................................................................................................ [2]
(d)Alkene A is converted into alkane B in reaction 4.
(i)State the reagent and conditions for reaction 4.
..............................................................................................................................................
........................................................................................................................................ [3]
(ii)State the general formula of alkanes.
........................................................................................................................................ [1]
© UCLES 2022
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11
(e) Ethanol is oxidised in reaction 5 by heating it with dilute sulfuric acid and one other reagent.
(i)Identify the other reagent in reaction 5.
........................................................................................................................................ [1]
(ii)Name the homologous series compound C belongs to.
........................................................................................................................................ [1]
(iii)Draw the structure of compound C.
Show all of the atoms and all of the bonds.
[1]
© UCLES 2022
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12
6This question is about polymers.
(a)Polymer X is a condensation polymer.
Part of the structure of polymer X is shown.
O
C
O
O
O
O
C
C
O
(i)How many molecules of water are produced when this part of polymer X is formed from its
monomers?
........................................................................................................................................ [1]
(ii)Complete the structures of the two monomers used to make polymer X.
Show all of the atoms and all of the bonds in the functional groups.
and
[2]
(iii)What type of condensation polymer is X?
........................................................................................................................................ [1]
(b)Part of polymer Y has the structure shown.
O
C
O
O
C
O
O
C
O
State the number of different types of monomer needed to make polymer Y.
............................................................................................................................................... [1]
© UCLES 2022
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13
(c)Part of polymer Z has the structure shown.
CH3 H
CH3 H
CH3 H
C
C
C
C
H
CH3 H
C
CH3 H
C
CH3
(i)Draw and name the structure of the monomer which forms polymer Z.
Show all of the atoms and all of the bonds.
name ...............................................
[3]
(ii)Name the chemical process used to make the monomer that forms polymer Z.
........................................................................................................................................ [1]
© UCLES 2022
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14
BLANK PAGE
© UCLES 2022
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15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/42/M/J/22
© UCLES 2022
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/M/J/22
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
May/June 2022
45 minutes
You must answer on the multiple choice answer sheet.
*2772444271*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
 There are forty questions on this paper. Answer all questions.
 For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
 Follow the instructions on the multiple choice answer sheet.
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
 Do not use correction fluid.
 Do not write on any bar codes.
 You may use a calculator.
INFORMATION
 The total mark for this paper is 40.
 Each correct answer will score one mark.
 Any rough working should be done on this question paper.
 The Periodic Table is printed in the question paper.
This document has 16 pages.
IB22 06_0620_22/2RP
© UCLES 2022
[Turn over
2
1
2
Which two gases will diffuse at the same rate, at the same temperature?
A
carbon monoxide and carbon dioxide
B
carbon monoxide and nitrogen
C
chlorine and fluorine
D
nitrogen and oxygen
A student measures the time taken for 2.0 g of magnesium to dissolve in 50 cm3 of dilute
sulfuric acid.
Which apparatus is essential to complete the experiment?
A
3
1
stop-clock
2
measuring cylinder
3
thermometer
4
balance
1, 2 and 4
B
1 and 2 only
C
1 and 4 only
D
2, 3 and 4
A chromatogram of a single substance T is shown.
solvent front
3
4
1
2
baseline
Which measurements are used to find the Rf value of T?
A
4
1 and 2
B
1 and 4
C
2 and 3
X and Y are two different elements.
X and Y have the same number of nucleons.
Which statement about X and Y is correct?
A
They have the same physical properties.
B
Their atoms have the same number of electrons.
C
They are in different groups of the Periodic Table.
D
They have different relative masses.
© UCLES 2022
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D
3 and 4
3
5
The diagrams show the structures of three macromolecules P, Q and R.
P
Q
R
What are P, Q and R?
6
P
Q
R
A
diamond
silicon(IV) oxide
graphite
B
graphite
diamond
silicon(IV) oxide
C
silicon(IV) oxide
diamond
graphite
D
silicon(IV) oxide
graphite
diamond
Which dot-and-cross diagram shows the arrangement of outer shell electrons in a molecule of
hydrogen chloride?
A
H
7
B
Cl
H
C
Cl
H
D
Cl
H
Cl
The equation for the reaction between barium chloride and dilute sulfuric acid is shown.
BaCl 2 + H2SO4  BaSO4 + 2HCl
Which row shows the state symbols for this equation?
BaCl 2
H2SO4
BaSO4
2HCl
A
(aq)
(aq)
(s)
(aq)
B
(aq)
(l)
(s)
(aq)
C
(l)
(aq)
(s)
(l)
D
(aq)
(l)
(aq)
(l)
© UCLES 2022
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4
8
Methane and steam react in the presence of a catalyst.
CH4(g) + H2O(g)  CO(g) + 3H2(g)
0.5 mol of methane reacts completely with 0.5 mol of steam.
What is the volume of carbon monoxide and hydrogen produced, measured at room temperature
and pressure?
9
volume
of CO / dm3
volume
of H2 / dm3
A
0.5
1.5
B
1.0
3.0
C
12.0
12.0
D
12.0
36.0
A compound of element X has the formula X2O and a relative formula mass of 144.
What is element X?
A
copper, Cu
B
gadolinium, Gd
C
sulfur, S
D
tellurium, Te
© UCLES 2022
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5
10 The diagram shows the electrolysis of concentrated hydrochloric acid and concentrated aqueous
sodium chloride using carbon electrodes.
electrode 1
+
–
electrode 2
electrode 3
concentrated
hydrochloric acid
+
–
electrode 4
concentrated aqueous
sodium chloride
At which electrodes is hydrogen produced?
A
electrode 1 only
B
electrodes 1 and 3
C
electrode 2 only
D
electrodes 2 and 4
11 The diagram shows the electrolysis of aqueous copper(II) sulfate using inert electrodes.
Which arrow shows the movement of electrons in the circuit?
power
supply
A
B
anode
cathode
C
D
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6
12 Which row identifies a chemical change and a physical change?
chemical change
physical change
A
boiling ethanol
burning ethanol
B
burning ethanol
evaporating ethanol
C
dissolving ethanol in water
burning ethanol
D
evaporating ethanol
dissolving ethanol in water
13 Which statements explain why increasing the concentration of a reactant increases the rate of
reaction?
A
1
It increases the collision rate of particles.
2
It lowers the activation energy.
3
A greater proportion of the colliding molecules have the required activation energy.
4
There are more particles per unit volume.
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
14 When the colourless gas N2O4 is heated, it forms the brown gas NO2.
When the reaction mixture is cooled, the brown colour fades and turns back to colourless.
Which type of reaction is described by these observations?
A
decomposition
B
displacement
C
reduction
D
reversible
15 Water is added to anhydrous copper(II) sulfate.
What happens during the reaction?
A
The copper(II) sulfate turns blue and the solution formed gets colder.
B
The copper(II) sulfate turns blue and the solution formed gets hotter.
C
The copper(II) sulfate turns white and the solution formed gets colder.
D
The copper(II) sulfate turns white and the solution formed gets hotter.
© UCLES 2022
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7
16 Which arrow on the energy level diagram shows the overall energy change for an endothermic
reaction?
C
products
A
energy
D
B
reactants
progress of reaction
17 When a hydrogen–oxygen fuel cell is in operation, a different reaction happens at each electrode.
at the hydrogen electrode
H2  2H+ + 2e–
at the oxygen electrode
O2 + 2H2O + 4e–  4OH–
The electrons that are lost at the hydrogen electrode travel through the external circuit to the
oxygen electrode, where they are gained by the oxygen and water.
A hydrogen–oxygen fuel cell is operated for a period of time and four moles of oxygen molecules
are consumed.
Which mass of hydrogen is consumed?
A
2.0 g
B
4.0 g
C
8.0 g
D
16.0 g
18 The oxides of two elements, X and Y, are separately dissolved in water and the pH of each
solution tested.
oxide tested
pH of solution
X
1
Y
13
Which information about X and Y is correct?
oxide is
acidic
oxide is
basic
metal
non-metal
A
X
Y
X
Y
B
X
Y
Y
X
C
Y
X
X
Y
D
Y
X
Y
X
© UCLES 2022
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8
19 An acid is neutralised by adding an excess of an insoluble solid base.
A soluble salt is formed.
How is the pure salt obtained from the reaction mixture?
A
crystallisation  evaporation  filtration
B
evaporation  crystallisation  filtration
C
filtration  crystallisation  evaporation
D
filtration  evaporation  crystallisation
20 Substance J takes part in a redox reaction.
In the reaction, J gains electrons.
Which statement is correct?
A
J is the oxidising agent and it is oxidised in the reaction.
B
J is the oxidising agent and it is reduced in the reaction.
C
J is the reducing agent and it is oxidised in the reaction.
D
J is the reducing agent and it is reduced in the reaction.
21 Elements in Group IV of the Periodic Table are shown.
carbon
silicon
germanium
tin
lead
What does not occur in Group IV as it is descended?
A
The proton number of the elements increases.
B
The elements become more metallic.
C
The elements have more electrons in their outer shell.
D
The elements have more electron shells.
© UCLES 2022
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9
22 Which statement about acids is correct?
A
Acids are proton acceptors.
B
Acids transfer electrons to bases in aqueous solution.
C
Hydrochloric acid reacts with ammonium hydroxide to produce ammonia.
D
Ethanoic acid partially ionises in aqueous solution.
23 Which elements have both a high melting point and variable oxidation states?
A
alkali metals
B
transition elements
C
halogens
D
noble gases
24 Lithium, sodium and potassium are elements in Group I of the Periodic Table.
Chlorine, bromine and iodine are elements in Group VII of the Periodic Table.
Which row identifies the least dense of these elements in each group?
Group I
Group VII
A
lithium
chlorine
B
lithium
iodine
C
potassium
chlorine
D
potassium
iodine
© UCLES 2022
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10
25 The reactions of metals P, Q, R and S are shown.
metal
reaction
with water
reaction with
hydrochloric acid
reduction of the
metal oxide with carbon
P
no reaction
no reaction
reduced
Q
slow
vigorous
no reaction
R
vigorous
vigorous
no reaction
S
very slow
vigorous
reduced
What is the order of reactivity of the metals?
least
reactive
most
reactive
A
P
S
Q
R
B
P
Q
S
R
C
R
S
Q
P
D
R
Q
S
P
26 The number of protons and the number of neutrons in the atoms of elements X, Y and Z are
shown.
number of
protons
number of
neutrons
X
6
6
Y
7
6
Z
8
10
Which statement about the elements is correct?
A
X and Y are isotopes of the same element.
B
Z forms an ion with a +2 charge.
C
X and Z react together to form an ionic compound.
D
X, Y and Z are non-metals.
© UCLES 2022
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11
27 Which diagram represents the arrangement of atoms in an alloy?
A
B
C
D
28 Three metal compounds, J, K and L, are heated using a Bunsen burner.
The results are shown.
J
colourless gas produced, which relights a glowing splint
K
colourless gas produced, which turns limewater milky
L
no reaction
Which row identifies J, K and L?
J
K
L
A
magnesium carbonate
potassium carbonate
potassium nitrate
B
magnesium carbonate
potassium nitrate
potassium carbonate
C
potassium nitrate
magnesium carbonate
potassium carbonate
D
potassium nitrate
potassium carbonate
magnesium carbonate
29 Processes involved in the extraction of zinc are listed.
1
Heat zinc oxide with carbon.
2
Condense zinc vapour.
3
Vaporise the zinc.
4
Roast zinc ore in air.
In which order are the processes carried out?
A
1234
B
4312
C
4132
D
1432
© UCLES 2022
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12
30 Which process uses sacrificial protection to prevent steel from rusting?
A
galvanising
B
oiling
C
copper plating
D
painting
31 Fertilisers are used to provide three of the elements needed for plant growth.
Which two compounds would give a fertiliser containing all three of these elements?
A
Ca(NO3)2 and (NH4)2SO4
B
Ca(NO3)2 and (NH4)3PO4
C
KNO3 and (NH4)2SO4
D
KNO3 and (NH4)3PO4
32 Which processes produce carbon dioxide?
A
1
respiration
2
photosynthesis
3
fermentation
4
combustion of hydrogen
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
33 Which reaction in the Contact process requires the use of a catalyst?
A
S + O2  SO2
B
2SO2 + O2  2SO3
C
SO3 + H2SO4  H2S2O7
D
H2S2O7 + H2O  2H2SO4
34 What are the products when limestone (calcium carbonate) is heated strongly?
A
calcium hydroxide and carbon dioxide
B
calcium hydroxide and carbon monoxide
C
calcium oxide and carbon dioxide
D
calcium oxide and carbon monoxide
© UCLES 2022
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13
35 The structure of ester W is shown.
H
H
C
H
O
H
C
O
C
H
H
Which row gives the names of ester W and the carboxylic acid and alcohol from which it is made?
name of ester W
carboxylic acid
alcohol
A
ethyl methanoate
ethanoic acid
methanol
B
ethyl methanoate
methanoic acid
ethanol
C
methyl ethanoate
ethanoic acid
methanol
D
methyl ethanoate
methanoic acid
ethanol
36 Ethene reacts with substance X to form ethanol.
What is X?
A
ethanoic acid
B
glucose
C
hydrogen
D
steam
37 Alkenes can be produced by cracking large hydrocarbon molecules to form smaller hydrocarbon
molecules.
Which equations represent possible reactions when tetradecane, C14H30, is cracked?
A
1
C14H30  C2H6 + C3H6 + C4H8 + C5H10
2
C14H30  H2 + C2H4 + C3H6 + C4H8 + C5H10
3
C14H30  C2H6 + 4C3H6
4
C14H30  C2H6 + C3H8 + C9H18
1 only
© UCLES 2022
B
1 and 4
C
1, 2 and 3
0620/22/M/J/22
D
3 and 4
[Turn over
14
38 The structures of some hydrocarbons are shown.
1
2
H
H
H
C
C
C
3
H
H
H
H
C
C
C
C
H
H
H
H
H
H
H
H
H
H
H
H
H
H
C
C
H
H
4
H
H
H
C
H
H
H
H
C
C
C
H
H
H
Which statement about the hydrocarbons is correct?
A
1 and 2 have a different general formula.
B
1 and 4 are in different homologous series.
C
2 and 3 are structural isomers.
D
3 and 4 have the same empirical formula.
39 Ethane reacts with chlorine in the presence of ultraviolet light.
Which substances are produced in the reaction?
1
H
A
2
H
1, 2 and 3
© UCLES 2022
H
B
3
H
H
C
C
H
H
1 and 3 only
Cl
C
H
H
C
C
Cl
Cl
2, 3 and 4
0620/22/M/J/22
4
H
H
D
H
2 and 4 only
H
H
H
H
C
C
Cl
H
15
40 Which polymer structure has the same linkages as Terylene?
A
B
CH3
CH3
C
C
C
H
O
CH3 CH3 O
O
n
OH
C
C
C
H
H
C
n
D
H
CH3 CH3 O
CH3 CH3
N
C
C
C
C
H
H
H
H
C
n
O
n
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/22/M/J/22
© UCLES 2022
21
0620/22/M/J/22
calcium
40
38
Sr
strontium
88
56
Ba
barium
137
88
potassium
39
37
Rb
rubidium
85
55
Cs
caesium
133
87
22
cerium
140
90
Th
thorium
232
lanthanum
139
89
Ac
actinium
–
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
Ce
57
–
dubnium
Db
105
181
tantalum
Ta
73
93
niobium
Nb
41
51
vanadium
V
–
rutherfordium
Rf
104
178
hafnium
Hf
72
91
zirconium
Zr
40
48
titanium
La
lanthanoids
57–71
89
yttrium
Y
39
45
scandium
Ti
23
Cr
24
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
relative atomic mass
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Pt
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
49
70
gallium
Ga
31
27
aluminium
Al
13
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ca
K
–
actinoids
20
19
Ra
24
23
radium
magnesium
sodium
Fr
Mg
Na
francium
89–103
12
11
Sc
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
Group
The Periodic Table of Elements
16
Cambridge IGCSE™
*2244180806*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
October/November 2022
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 40.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Any blank pages are indicated.
IB22 11_0620_62/2RP
© UCLES 2022
[Turn over
2
1A mixture of three coloured compounds was separated using the apparatus shown in the diagram.
lid
paper
A
baseline
(a)Give the name of the item of apparatus labelled A.
............................................................................................................................................... [1]
(b)One drop of the mixture of coloured compounds was placed on the paper and some solvent
was poured into A.
Draw on the diagram:
●
spot (●) to show where the drop of the mixture of coloured compounds should be placed
a
on the paper at the start of the experiment
● a line to show the level of the solvent in A at the start of the experiment.
[2]
(c)Name an item of apparatus that should be used to place a drop of the mixture of coloured
compounds onto the paper.
............................................................................................................................................... [1]
(d)State when the paper should be removed from the solvent in A.
............................................................................................................................................... [1]
(e)Name this method of separation of coloured compounds.
............................................................................................................................................... [1]
© UCLES 2022
[Total: 6]
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3
2
A student investigated the temperature change when two different aqueous solutions of
sodium hydroxide, solution G and solution H, reacted with dilute hydrochloric acid.
Two experiments were done.
(a) Experiment 1
● A burette was rinsed with distilled water and then with dilute hydrochloric acid.
● The burette was filled with the dilute hydrochloric acid. The hydrochloric acid was then run
out through the tap until the level was on the 0.00 cm3 mark.
● A 50 cm3 measuring cylinder was used to pour 20 cm3 of solution G into a beaker.
● A thermometer was used to measure the initial temperature of solution G.
● 5 cm3 of dilute hydrochloric acid was added from the burette into the beaker.
● The mixture in the beaker was stirred using the thermometer and the temperature of the
mixture was measured.
● Another 5 cm3 of dilute hydrochloric acid was added from the burette into the beaker.
● The mixture in the beaker was stirred using the thermometer and the temperature of the
mixture was measured.
● 5 cm3 portions of dilute hydrochloric acid continued to be added and the temperature
measured until a total of 35 cm3 of dilute hydrochloric acid had been added.
Experiment 2
● Experiment 1 was repeated using solution H instead of solution G.
© UCLES 2022
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4
Use the thermometer diagrams to complete the table.
Experiment 1 using solution G
Experiment 2 using solution H
total volume
temperature
temperature
of dilute
thermometer temperature
thermometer temperature
change
change
hydrochloric
diagram
/ C
diagram
/ C
since start
since start
acid added
/ C
/ C
/ cm3
0
5
10
15
20
25
30
35
30
30
25
25
20
20
30
30
25
25
20
20
30
30
25
25
20
20
30
30
25
25
20
20
30
30
25
25
20
20
30
30
25
25
20
20
30
30
25
25
20
20
30
30
25
25
20
20
[5]
© UCLES 2022
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5
(b)Complete a suitable scale on the y-axis and plot the results from Experiments 1 and 2 on the
grid.
Draw two smooth line graphs. Both curves must start at (0,0). Clearly label your lines.
temperature
change / C
0
0
5
10
15
20
25
35
30
total volume of dilute hydrochloric acid added / cm3
[5]
(c)
From your graph, deduce the temperature change obtained when a total volume of 13 cm3 of
dilute hydrochloric acid is added in Experiment 1.
Show clearly on the grid how you worked out your answer.
temperature change = .............................. °C [2]
(d)Explain why the temperature change decreases towards the end of each experiment.
.....................................................................................................................................................
............................................................................................................................................... [1]
© UCLES 2022
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6
(e)Explain what conclusion about the concentrations of solution G and solution H can be made
from the results of Experiments 1 and 2.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(f) E
xplain how the results obtained would be different if a polystyrene cup is used instead of the
beaker.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(g)Give an advantage and a disadvantage of using a burette rather than a measuring cylinder to
add the dilute hydrochloric acid to solution G and solution H.
advantage ...................................................................................................................................
.....................................................................................................................................................
disadvantage ..............................................................................................................................
.....................................................................................................................................................
[2]
© UCLES 2022
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7
3Solid I and solid J were analysed.
Tests were done on each substance.
tests on solid I
tests
observations
test 1
Dilute hydrochloric acid was added to a
boiling tube containing solid I.
effervescence was seen, the solid dissolved
to form a colourless solution
Any gas produced was tested.
the gas turned limewater milky
test 2
A flame test was carried out on the solution
formed in test 1.
a red flame was seen
(a)Identify the gas made in test 1.
............................................................................................................................................... [1]
(b)Identify solid I.
.....................................................................................................................................................
............................................................................................................................................... [2]
© UCLES 2022
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8
tests on solid J
Solid J was aluminium chloride.
Solid J was dissolved in water to form solution J. Solution J was divided into four approximately
equal portions in four test-tubes.
(c) A
queous sodium hydroxide was added dropwise and then in excess to the first portion of
solution J.
observations ...............................................................................................................................
............................................................................................................................................... [2]
(d) Aqueous ammonia was added dropwise and then in excess to the second portion of solution J.
observations ...............................................................................................................................
............................................................................................................................................... [2]
(e) A
bout 1 cm depth of dilute nitric acid followed by a few drops of aqueous barium nitrate were
added to the third portion of solution J.
observations ......................................................................................................................... [1]
(f) A
bout 1 cm depth of dilute nitric acid followed by a few drops of aqueous silver nitrate were
added to the fourth portion of solution J.
observations ......................................................................................................................... [1]
© UCLES 2022
[Total: 9]
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9
4Hydrogels are powders that absorb water to form hydrated solids. Hydrogels and the hydrated
solids formed are insoluble in water.
Plan an investigation to find which hydrogel, hydrogel A or hydrogel B, is able to absorb the
greater mass of water.
You are provided with samples of hydrogel A, hydrogel B, water and common laboratory apparatus.
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
............................................................................................................................................................
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............................................................................................................................................................
............................................................................................................................................................
...................................................................................................................................................... [6]
© UCLES 2022
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BLANK PAGE
© UCLES 2022
0620/62/O/N/22
11
BLANK PAGE
© UCLES 2022
0620/62/O/N/22
12
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/62/O/N/22
Cambridge IGCSE™
*4909270147*
CHEMISTRY0620/42
Paper 4 Theory (Extended)
October/November 2022
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 80.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB22 11_0620_42/3RP
© UCLES 2022
[Turn over
2
1
Diamond and graphite are different solid forms of carbon. The carbon atoms in diamond and
graphite are arranged in different ways.
(a) State the number of covalent bonds each carbon atom has in diamond.
.............................................................................................................................................. [1]
(b) State the term used to describe the structure of diamond.
.............................................................................................................................................. [1]
(c) Name an oxide that has a similar structure to diamond.
.............................................................................................................................................. [1]
(d) Describe the arrangement of atoms in graphite.
....................................................................................................................................................
.............................................................................................................................................. [2]
(e) Explain how graphite conducts electricity.
.............................................................................................................................................. [1]
(f) Buckminsterfullerene is a simple molecular form of carbon.
The relative molecular mass of Buckminsterfullerene is 720.
Determine the number of carbon atoms in one molecule of Buckminsterfullerene.
.............................................................................................................................................. [1]
(g) All forms of carbon burn to produce carbon dioxide.
Name the substance used to test for carbon dioxide.
.............................................................................................................................................. [1]
© UCLES 2022
[Total: 8]
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3
2
Sodium is a reactive metal.
(a) Suggest why sodium is stored under oil.
.............................................................................................................................................. [1]
(b) Sodium burns in air to form sodium oxide, Na2O.
(i)
State the term given to a reaction in which a substance burns.
. ...................................................................................................................................... [1]
(ii)
State the colour of the flame seen when sodium burns.
. ...................................................................................................................................... [1]
(iii)
rite a chemical equation for the reaction which takes place when sodium burns in air to
W
form sodium oxide.
. ...................................................................................................................................... [2]
(iv)
Complete the dot-and-cross diagram to show the electron arrangement and charges of
the ions in sodium oxide.
.......
Na
.......
O
.......
Na
[3]
© UCLES 2022
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4
(c) S
odium reacts vigorously with water to form aqueous sodium hydroxide, NaOH, which is a
strong base.
(i)
Explain in terms of proton transfer what is meant by a base.
. ...................................................................................................................................... [1]
(ii)
State a pH number that indicates the presence of a strong alkali.
. ...................................................................................................................................... [1]
(iii)
State the colour of methyl orange in aqueous sodium hydroxide.
. ...................................................................................................................................... [1]
(iv)
The equation for the reaction is shown.
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
alculate the concentration of NaOH(aq) formed, in g / dm3, when 0.345 g of sodium is
C
added to 50.0 cm3 of distilled water. Assume there is no change in volume.
Use the following steps.
●
Calculate the number of moles of Na added.
= .............................. mol
●
Determine the number of moles of NaOH formed.
= .............................. mol
●
concentration of NaOH = .............................. mol / dm3
●
© UCLES 2022
Calculate the concentration of NaOH in mol / dm3.
Determine the Mr of NaOH and calculate the concentration of NaOH in g / dm3.
concentration of NaOH = .............................. g / dm3
[5]
0620/42/O/N/22
5
(d) When NaOH(aq) is added to aqueous iron(III) chloride, FeCl 3(aq), a solid product is formed.
(i)
Name the type of reaction where a solid is formed from two solutions.
. ...................................................................................................................................... [1]
(ii)
State the colour of this solid product.
. ...................................................................................................................................... [1]
(iii)
Name this solid product.
. ...................................................................................................................................... [1]
(iv)
Write the ionic equation for the reaction. Include state symbols.
. ...................................................................................................................................... [3]
© UCLES 2022
[Total: 22]
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6
3
ulfuric acid is manufactured by an industrial process. Sulfur is obtained from sulfur-containing
S
metal ores.
The sulfur in the metal ore is converted to sulfur dioxide which is then oxidised to sulfur trioxide as
shown.
2SO2(g) + O2(g) 2SO3(g)
(a) Name a metal ore which contains sulfur.
.............................................................................................................................................. [1]
(b) Describe the process which converts metal ores to sulfur dioxide.
.............................................................................................................................................. [1]
(c) Name the industrial process used to manufacture sulfuric acid.
.............................................................................................................................................. [1]
(d) The reaction that produces sulfur trioxide is an equilibrium. The forward reaction is exothermic.
(i)
State the temperature and pressure used to make sulfur trioxide.
temperature = .............................. °C
pressure = .............................. atm
[2]
(ii)
Name the catalyst used.
. ...................................................................................................................................... [1]
(iii)
Describe two features of an equilibrium.
1 . .........................................................................................................................................
2 . .........................................................................................................................................
[2]
(iv)
State the effect, if any, on the position of equilibrium when the following changes are
made.
Explain your answers.
temperature is increased .....................................................................................................
. ............................................................................................................................................
pressure is increased ..........................................................................................................
© UCLES 2022
. ............................................................................................................................................
[4]
0620/42/O/N/22
7
(v)
xplain, in terms of particles, what happens to the rate of reaction when the temperature
E
is increased.
. ............................................................................................................................................
. ............................................................................................................................................
. ............................................................................................................................................
. ............................................................................................................................................
. ...................................................................................................................................... [3]
(e) Name the compound formed when sulfuric acid reacts with ammonia.
.............................................................................................................................................. [1]
© UCLES 2022
[Total: 16]
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8
4
A student prepares magnesium sulfate crystals, MgSO4, by adding excess magnesium to dilute
sulfuric acid.
(a) Write the chemical equation for this reaction.
.............................................................................................................................................. [1]
(b) Describe two observations which show the reaction has finished.
1 .................................................................................................................................................
2 .................................................................................................................................................
[2]
(c) The excess magnesium is removed by filtration.
State the general name given to a solid separated from a solution by filtration.
.............................................................................................................................................. [1]
(d) The aqueous magnesium sulfate is heated until crystals begin to appear.
(i)
Suggest the name for a solution in which no more solute can dissolve.
. ...................................................................................................................................... [1]
(ii)
Suggest why more crystals of magnesium sulfate appear on cooling.
. ...................................................................................................................................... [1]
(e) M
agnesium sulfate crystals have the formula, MgSO4•xH2O, where x is a whole number of
molecules of water.
The student heats the crystals to remove the molecules of water.
MgSO4•xH2O(s) → MgSO4(s) + xH2O(g)
(i)
Name the term given to crystals containing molecules of water.
. ...................................................................................................................................... [1]
© UCLES 2022
0620/42/O/N/22
9
(ii)
The student heats a sample of MgSO4•xH2O and finds it has lost 0.140 moles of H2O and
has 2.40 g of MgSO4 remaining.
Determine the value of x. Use the following steps.
●
Calculate the Mr of MgSO4.
Mr = ..............................
●
Determine the number of moles of MgSO4 formed.
moles of MgSO4 formed = ..............................
●
Determine the value of x in MgSO4•xH2O.
x = ..............................
[3]
(f) If the student uses dilute nitric acid instead of dilute sulfuric acid, the salt formed is
magnesium nitrate, Mg(NO3)2.
Write the chemical equation for the reaction when solid magnesium nitrate is heated.
.............................................................................................................................................. [2]
© UCLES 2022
[Total: 12]
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10
5
Ethane is an alkane which undergoes a photochemical reaction with chlorine as shown.
C2H6(g) + Cl 2(g) → C2H5Cl (l) + HCl (g)
(a) Write the general formula of alkanes.
.............................................................................................................................................. [1]
(b) State why this reaction is described as a photochemical reaction.
.............................................................................................................................................. [1]
(c) In this reaction, an atom of hydrogen is replaced with a chlorine atom.
State the name of this type of organic reaction.
.............................................................................................................................................. [1]
(d) In this reaction, one of the products is chloroethane.
Name the other product.
.............................................................................................................................................. [1]
(e) The energy profile diagram of this reaction is shown.
energy
C2H6 + Cl 2
A
B
C2H5Cl + HCl
progress of reaction
(i)
Name the energy change labelled A.
. ...................................................................................................................................... [1]
(ii)
Name the energy change labelled B.
. ...................................................................................................................................... [1]
(iii)
State how the energy profile diagram shows this is an exothermic reaction.
. ...................................................................................................................................... [1]
© UCLES 2022
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11
(f) The equation for the reaction can be represented as shown.
H
H
H
C
C
H
H
H
+
Cl
Cl
H
H
H
C
C
H
H
Cl
+
H
Cl
Some bond energies are given.
bond
bond energy
/ kJ mol
C–H
410
C–C
350
Cl –Cl
240
C–Cl
340
H–Cl
430
Use the bond energies in the table to calculate the energy change in this reaction.
Use the following steps.
●
Calculate the energy needed to break bonds.
●
Calculate the energy released in making bonds.
energy = .............................. kJ
energy = .............................. kJ
●
Determine the energy change in this reaction.
energy change in this reaction = .............................. kJ / mol
[3]
© UCLES 2022
[Total: 10]
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12
6
A carboxylic acid Y has the structure shown.
O
H
C
O
H
(a) State the general formula of carboxylic acids.
.............................................................................................................................................. [1]
(b) Name carboxylic acid Y.
.............................................................................................................................................. [1]
(c) Write the molecular formula of carboxylic acid Y.
.............................................................................................................................................. [1]
(d) Complete the dot-and-cross diagram to show the arrangement of electrons in a molecule of
carboxylic acid Y.
O
H
C
O
H
[3]
© UCLES 2022
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13
(e) Carboxylic acid Y will react with propan-1-ol, C3H7OH, to form ester Z and one other product.
(i)
Name and draw the structure of ester Z.
Show all of the atoms and all of the bonds.
name ..........................................................
structure
[3]
(ii)
Name the other product formed when carboxylic acid Y reacts with propan-1-ol.
. ...................................................................................................................................... [1]
(iii)
Name:
●
an ester which is a structural isomer of ester Z
. ............................................................................................................................................
●
a carboxylic acid which is a structural isomer of ester Z.
. ............................................................................................................................................
[2]
© UCLES 2022
[Total: 12]
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14
BLANK PAGE
© UCLES 2022
0620/42/O/N/22
15
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/42/O/N/22
© UCLES 2022
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/O/N/22
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
rutherfordium
104
178
La
57
actinoids
89–103
Hf
hafnium
72
91
zirconium
Zr
40
48
titanium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
137
87
133
Ba
barium
Cs
caesium
lanthanoids
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
16
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
October/November 2022
45 minutes
You must answer on the multiple choice answer sheet.
*7173935082*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
 There are forty questions on this paper. Answer all questions.
 For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
 Follow the instructions on the multiple choice answer sheet.
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
 Do not use correction fluid.
 Do not write on any bar codes.
 You may use a calculator.
INFORMATION
 The total mark for this paper is 40.
 Each correct answer will score one mark.
 Any rough working should be done on this question paper.
 The Periodic Table is printed in the question paper.
This document has 16 pages.
IB22 11_0620_22/4RP
© UCLES 2022
[Turn over
2
1
The rate of diffusion of three gases, ammonia, carbon dioxide and methane, is measured.
What is the order of the rate of diffusion of the gases from slowest to fastest?
2
3
A
CO2  NH3  CH4
B
CO2  CH4  NH3
C
CH4  NH3  CO2
D
NH3  CH4  CO2
Which description of Brownian motion is correct?
A
random movement of particles due to bombardment by larger particles
B
random movement of particles due to bombardment by smaller particles
C
random movement of particles from a high concentration to a low concentration
D
random movement of particles from a low concentration to a high concentration
The chromatogram obtained using four substances, J, K, L and M, is shown.
solvent front
baseline
J
K
L
M
Which statement about M is correct?
A
It is a mixture of J and K only.
B
It is a pure substance.
C
It is a mixture of J, K and L.
D
It is a mixture of J, K and an unknown substance.
© UCLES 2022
0620/22/O/N/22
3
4
Which statements about isotopes of the same element are correct?
A
5
6
They are atoms which have the same chemical properties because they have the
same number of electrons in their outer shell.
2
They are atoms which have the same number of electrons and neutrons but
different numbers of protons.
3
They are atoms which have the same number of electrons and protons but different
numbers of neutrons.
1 and 2
B
1 and 3
C
2 only
D
3 only
Which statement about solid magnesium oxide is correct?
A
It is a giant structure made up of magnesium and oxygen atoms bonded covalently.
B
It is an electrical conductor with mobile magnesium ions and oxygen ions.
C
Magnesium loses electrons and these electrons move freely through a lattice.
D
Oxygen ions and magnesium ions are attracted to each other in a giant lattice.
Which molecule contains only three shared pairs of electrons?
A
7
1
CH3OH
B
Cl 2
C
H2O
D
N2
D
2 and 4
Which particles are present in the structure of metals?
A
1
positive ions
2
negative ions
3
shared pairs of electrons
4
mobile electrons
1 and 2
B
© UCLES 2022
1 and 4
C
2 and 3
0620/22/O/N/22
[Turn over
4
8
Caffeine is a stimulant found in coffee.
O
CH3
C
H 3C
N
C
N
C
C
O
C
N
H
N
CH3
caffeine
Which formula represents caffeine?
A
9
C7H10N4O2
B
C8H10N3O2
C
C8H10N4O2
D
C8H11N4O2
Which sample does not contain a number of atoms equal to the Avogadro constant?
A
14 g of nitrogen, N2
B
6 g of water, H2O
C
4 g of helium, He
D
28 g of carbon monoxide, CO
© UCLES 2022
0620/22/O/N/22
5
10 The electrolysis of concentrated aqueous sodium chloride and molten sodium chloride is shown.
electrode 1
+
+
–
–
+
concentrated aqueous
sodium chloride
–
electrode 2
molten
sodium chloride
What are the products at electrodes 1 and 2?
electrode 1
electrode 2
A
chlorine
chlorine
B
hydrogen
chlorine
C
hydrogen
sodium
D
sodium
sodium
11 When an acid is added to an alkali, the temperature of the reaction mixture rises.
Which words describe this reaction?
A
decomposition and endothermic
B
decomposition and exothermic
C
neutralisation and endothermic
D
neutralisation and exothermic
© UCLES 2022
0620/22/O/N/22
[Turn over
6
12 Some properties of four fuels are shown.
Which fuel is a gas at room temperature and makes two products when it burns in a plentiful
supply of air?
fuel
formula
melting point
/ C
boiling point
/ C
A
hydrogen
H2
–259
–253
B
methane
CH4
–182
–164
C
octane
C8H18
–57
126
D
wax
C31H64
60
400
13 The electrical energy, or voltage, of two simple cells is measured.
V
V
zinc
magnesium
magnesium
copper
electrolyte
electrolyte
cell 1
cell 2
statement 1
The voltage of cell 1 is greater than cell 2.
statement 2
Zinc is more reactive than copper.
statement 3
Magnesium is oxidised in both cells.
statement 4
Magnesium atoms lose electrons to form magnesium ions.
Which option is correct?
A
All the statements are correct.
B
Only statements 1 and 3 are correct.
C
Statement 2 is correct and explains statement 1.
D
Statement 4 is correct and explains statement 3.
© UCLES 2022
0620/22/O/N/22
7
14 Dilute aqueous sodium chloride is electrolysed using carbon electrodes.
What is the product at the anode?
A
carbon dioxide
B
hydrogen
C
oxygen
D
sodium
15 The volume of gas given off in a chemical reaction is measured over time.
The results are shown.
100
90
80
70
volume 60
of gas
50
/ cm3
40
30
20
10
0
0
2
4
6
8
10
time / s
At which time is the rate of reaction greatest?
0s
A
B
4s
C
6s
D
10 s
16 Dinitrogen tetroxide, N2O4, is converted into nitrogen dioxide, NO2, in a reversible reaction.
N2O4(g)
2NO2(g)
The forward reaction is endothermic.
Which conditions give the highest equilibrium yield of nitrogen dioxide?
pressure
/ atmospheres
temperature
A
2
high
B
2
low
C
50
high
D
50
low
© UCLES 2022
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8
17 When magnesium is heated with zinc oxide a reaction occurs.
The equation is shown.
Mg + ZnO  MgO + Zn
Which substance is oxidised?
A
magnesium
B
magnesium oxide
C
zinc
D
zinc oxide
18 X and Y are oxides of two different elements.
●
X reacts with water to produce aqueous solution Z.
●
Z turns universal indicator paper blue.
●
An aqueous solution of Y reacts with sodium carbonate to produce carbon dioxide
gas.
Which statement is correct?
A
X and Y are both the oxides of metals.
B
X and Y are both the oxides of non-metals.
C
X is the oxide of a metal and Y is the oxide of a non-metal.
D
X is the oxide of a non-metal and Y is the oxide of a metal.
19 Ethanoic acid reacts with water to produce an acidic solution.
Which row describes the roles of ethanoic acid and water in this reaction?
ethanoic acid
water
A
accepts a proton
donates a proton
B
accepts an electron
donates an electron
C
donates a proton
accepts a proton
D
donates an electron
accepts an electron
© UCLES 2022
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9
20 Copper(II) sulfate is a soluble salt.
Calcium sulfate is an insoluble salt.
Which row shows suitable reactants for preparing a pure sample of the named salt?
salt
reactants
A
calcium sulfate
calcium carbonate + dilute sulfuric acid
B
calcium sulfate
aqueous calcium chloride and aqueous sodium sulfate
C
copper(II) sulfate
copper + dilute sulfuric acid
D
copper(II) sulfate
aqueous copper(II) chloride and aqueous sodium sulfate
21 Strontium displaces magnesium from molten magnesium chloride.
Bromine displaces iodine from aqueous potassium iodide.
Which row describes the change in reactivity down both Group II and Group VII of the Periodic
Table?
reactivity down the group
Group II
Group VII
A
decreases
decreases
B
decreases
increases
C
increases
decreases
D
increases
increases
22 Elements J and K are in the same period in the Periodic Table.
J reacts with acids to produce a salt and hydrogen.
K reacts with sodium to form an ionic compound.
Which statement about J and K is correct?
A
An atom of J has more electrons than an atom of K.
B
J and K are both metals.
C
J and K are both non-metals.
D
J is to the left of K in the Periodic Table.
© UCLES 2022
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10
23 Part of the Periodic Table is shown.
Which element has a high density, a high melting point and forms a brown oxide?
A
D
B
C
24 The reactions of four metals, W, X, Y and Z, are listed.
●
Metal W displaces metal X from the oxide of metal X.
●
Metal Y has a greater tendency to form positive ions than metal W.
●
Aqueous ions of metal Z are reduced by metal X.
What is the order of reactivity of the metals?
least
reactive
most
reactive
A
Y
W
X
Z
B
Y
X
W
Z
C
Z
W
X
Y
D
Z
X
W
Y
25 Three experiments, J, K and L, are set up to investigate rusting.
J
K
water
water
water
mild steel
painted iron
In which experiments does rusting occur?
J
K
L
A
key
B
= yes
C
= no
D
© UCLES 2022
L
0620/22/O/N/22
stainless steel
11
26 Silver is below copper in the reactivity series.
Which row describes the reactions of silver?
reaction with steam
reaction with dilute hydrochloric acid
A
no reaction
no reaction
B
no reaction
reacts to produce hydrogen gas
C
reacts to produce hydrogen gas
no reaction
D
reacts to produce hydrogen gas
reacts to produce hydrogen gas
27 Iron is galvanised by coating it in zinc.
Brass is made by mixing copper with zinc.
Which row gives the reasons for each of these uses of zinc?
reason for galvanising iron
reason for making brass
A
prevents corrosion
produces a softer metal
B
prevents corrosion
produces a harder metal
C
produces a harder metal
produces a softer metal
D
produces a harder metal
produces a harder metal
28 The diagram shows a stage in the purification of dirty water.
dirty water
sand
pot with holes
in bottom
fine gravel
coarse gravel
Which process does this apparatus show?
A
chlorination
B
condensation
C
distillation
D
filtration
© UCLES 2022
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12
29 Which substance in polluted air damages stonework and kills trees?
A
carbon dioxide
B
carbon monoxide
C
lead compounds
D
sulfur dioxide
30 Ammonium nitrate, NH4NO3, is a fertiliser and is added to fields to help crops grow.
Slaked lime, Ca(OH)2, is an alkali and is added to fields to reduce the acidity of the soil.
Ammonium nitrate and slaked lime should not be added to a field at the same time because they
react with each other to form a gas, Z.
What is Z?
A
ammonia
B
hydrogen
C
nitrogen
D
oxygen
31 The scheme shows four stages in the conversion of sulfur to sulfuric acid.
In which stage is a catalyst used?
sulfur
stage A
air
sulfur
dioxide
stage B
sulfur
trioxide
air
stage C
concentrated
sulfuric acid
stage D
water
32 Which element has an oxide that is used as a food preservative?
A
helium
B
hydrogen
C
iron
D
sulfur
© UCLES 2022
0620/22/O/N/22
concentrated
sulfuric acid
oleum
13
33 Which substance gives off carbon dioxide on heating?
A
lime
B
limestone
C
limewater
D
slaked lime
34 Which compound has the most –CH2– groups in one molecule?
A
butane
B
butanoic acid
C
butan-1-ol
D
but-1-ene
35 Methane reacts with chlorine in the presence of ultraviolet light.
Which substance is not produced in this reaction?
A
H
B
H
H
H
Cl
C
D
H
Cl
C
Cl
H
H
C
Cl
H
36 Ethene reacts with both hydrogen and steam.
Which row about these reactions is correct?
reactant
with ethene
type of reaction
catalyst used
A
hydrogen
substitution
phosphoric acid
B
hydrogen
addition
nickel
C
steam
substitution
phosphoric acid
D
steam
addition
nickel
37 Which type of reaction occurs when ethanol is converted to ethanoic acid?
A
combustion
B
decomposition
C
neutralisation
D
oxidation
© UCLES 2022
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14
38 Hydrolysis of polymer P produces the three compounds shown.
H
N
C
H
O
O
H
H
N
C
H
O
O
H
H
N
C
H
O
What is the structure of polymer P?
A
H
O
N
C
N
C
H
O
O
H
B
N
N
C
H
C
H
O
N
C
O
D
C
C
H
O
N
C
H
O
N
C
H
H
N
N
H
H
N
N
O
N
C
H
O
O
N
H
C
C
O
39 Which statement about unsaturated hydrocarbons is correct?
A
CH3CH2CH=CHCH3 is an unsaturated hydrocarbon.
B
Ethene has more hydrogen atoms per molecule than ethane.
C
Unsaturated hydrocarbons have double bonds between carbon and hydrogen atoms.
D
Unsaturated hydrocarbons turn aqueous bromine from colourless to brown.
© UCLES 2022
0620/22/O/N/22
O
H
15
40 The equation shows the formation of a polymer called Kevlar.
n HOOC
COOH
+
n H 2N
NH2
– H2 O
O
O
C
C
N
N
H
H n
Which row describes Kevlar?
how the polymer is formed
type of polymer
A
addition polymerisation
polyamide
B
addition polymerisation
polyester
C
condensation polymerisation
polyamide
D
condensation polymerisation
polyester
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2022
0620/22/O/N/22
© UCLES 2022
21
0620/22/O/N/22
22
cerium
140
90
Th
thorium
232
lanthanum
139
89
Ac
actinium
–
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
Ce
57
La
–
dubnium
Db
105
181
tantalum
Ta
73
93
niobium
Nb
41
51
vanadium
V
–
rutherfordium
Rf
104
178
hafnium
Hf
72
91
zirconium
Zr
40
48
titanium
Ti
23
Cr
24
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
relative atomic mass
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Pt
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
49
70
gallium
Ga
31
27
aluminium
Al
13
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
–
actinoids
Ra
radium
88
87
Fr
137
francium
89–103
barium
133
lanthanoids
57–71
89
yttrium
caesium
Y
39
Ba
38
37
45
scandium
Cs
40
39
56
calcium
potassium
Sc
55
Ca
K
88
20
19
strontium
24
23
85
magnesium
sodium
rubidium
Mg
Na
Sr
12
11
Rb
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
Group
The Periodic Table of Elements
16
Cambridge IGCSE™
*6847411147*
CHEMISTRY0620/62
Paper 6 Alternative to Practical
May/June 2023
1 hour
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 40.
●
The number of marks for each question or part question is shown in brackets [ ].
●
Notes for use in qualitative analysis are provided in the question paper.
This document has 12 pages. Any blank pages are indicated.
IB23 06_0620_62/3RP
© UCLES 2023
[Turn over
2
1Hot powdered lead(II) oxide is reduced by methane, a flammable gas. The products are lead,
steam and carbon dioxide gas.
Fig. 1.1 shows the apparatus used to reduce lead(II) oxide using excess methane.
powdered lead(II) oxide
methane
waste gases
A
B
ice
Fig. 1.1
(a)Name the item of apparatus labelled A.
.............................................................................................................................................. [1]
(b)Draw an arrow on Fig. 1.1 to show where the apparatus should be heated.
[1]
(c)Explain why powdered lead(II) oxide is used and not a large lump of lead(II) oxide.
....................................................................................................................................................
.............................................................................................................................................. [1]
(d)Explain what happens at the point labelled B, on Fig. 1.1.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
(e)The waste gases contain methane.
State why the waste gases should not be released into the laboratory.
....................................................................................................................................................
.............................................................................................................................................. [1]
© UCLES 2023
[Total: 6]
0620/62/M/J/23
3
2A student investigates how the rate of the reaction between aqueous iron(III) nitrate and aqueous
sodium thiosulfate changes with temperature.
The student does five experiments using the apparatus shown in Fig. 2.1.
eye
5 cm3 of aqueous sodium thiosulfate
100 cm3 beaker
50 cm3 of aqueous iron(III) nitrate
printed sheet
printed text
Fig. 2.1
(a) Experiment 1
●
●
●
●
●
●
●
se a 50 cm3 measuring cylinder to pour 50 cm3 of aqueous iron(III) nitrate into a 100 cm3
U
beaker.
Stand the beaker on a printed sheet as shown in Fig. 2.1.
Use a 10 cm3 measuring cylinder to pour 5 cm3 of aqueous sodium thiosulfate into the
beaker and at the same time start a stop-clock.
Use a thermometer to stir the contents of the beaker.
Look down from above the beaker and when the text on the printed sheet becomes visible,
stop the stop-clock.
Use the thermometer to measure the temperature of the solution when the text becomes
visible.
Rinse the beaker and thermometer with water.
Experiment 2
●
●
●
●
●
●
●
●
se the 50 cm3 measuring cylinder to pour 50 cm3 of aqueous iron(III) nitrate into the
U
100 cm3 beaker.
Heat the beaker on a gauze over a Bunsen burner until the temperature of the iron(III) nitrate
has increased by about 5 °C.
Stand the beaker on the printed sheet as shown in Fig. 2.1.
Use the 10 cm3 measuring cylinder to pour 5 cm3 of aqueous sodium thiosulfate into the
beaker and at the same time start a stop-clock.
Use the thermometer to stir the contents of the beaker.
Look down from above the beaker and when the text on the printed sheet becomes visible,
stop the stop-clock.
Use the thermometer to measure the temperature of the solution when the text becomes
visible.
Rinse the beaker and thermometer with water.
Experiment 3
●
epeat Experiment 2, this time heating the aqueous iron(III) nitrate until the temperature
R
has increased by about 10 °C.
Experiment 4
●
© UCLES 2023
epeat Experiment 2, this time heating the aqueous iron(III) nitrate until the temperature
R
has increased by about 15 °C.
0620/62/M/J/23
[Turn over
4
Experiment 5
●
epeat Experiment 2, this time heating the aqueous iron(III) nitrate until the temperature
R
has increased by about 25 °C.
Use the thermometer diagrams and stop-clock diagrams to complete Table 2.1.
Table 2.1
experiment
stop-clock diagram
0
seconds
0
1
time taken for
the text to
become visible
/s
45 15
5
10
temperature of the
solution when the
text becomes
visible / C
30
25
15
minutes
30
thermometer
diagram
20
0
30
0
2
45 15
5
25
15
10
20
30
0
30
0
3
45 15
5
25
15
10
20
30
0
40
0
4
45 15
5
35
15
10
30
30
0
50
0
5
45 15
5
45
15
10
40
30
© UCLES 2023
[4]
0620/62/M/J/23
5
(b)Write a suitable scale on the y-axis and plot your results from Experiments 1 to 5 on Fig. 2.2.
Draw a smooth curve of best fit.
time taken for the
text to become
visible / s
10
20
30
40
50
60
temperature of the solution
when the text becomes visible / C
Fig. 2.2
[4]
(c)Deduce the experiment in which the rate of reaction is fastest.
.............................................................................................................................................. [1]
(d)Use your graph to predict the temperature of the solution when the text becomes visible after
55 seconds.
Show your working on Fig. 2.2.
© UCLES 2023
temperature = .............................. °C [2]
0620/62/M/J/23
[Turn over
6
(e)Explain why wrapping the beaker in cotton wool after it has been heated will improve the
accuracy of the results obtained.
....................................................................................................................................................
.............................................................................................................................................. [2]
(f) (i)Explain why it would be an improvement to measure the volume of aqueous iron(III) nitrate
in a burette rather than a measuring cylinder.
. ............................................................................................................................................
. ...................................................................................................................................... [1]
(ii)Suggest why it would not be an improvement to add the aqueous sodium thiosulfate using
a pipette.
. ............................................................................................................................................
. ...................................................................................................................................... [1]
(g)Suggest why the aqueous sodium thiosulfate must be added after the aqueous iron(III) nitrate
has been heated and not before it is heated.
....................................................................................................................................................
.............................................................................................................................................. [1]
(h)Describe how the results of the experiment would change when the experiment is repeated
using a 250 cm3 beaker in place of the 100 cm3 beaker.
Explain your answer.
change in results ........................................................................................................................
explanation .................................................................................................................................
....................................................................................................................................................
[2]
[Total: 18]
© UCLES 2023
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7
3A student tests two substances: solution F and solid G.
Tests on solution F
Table 3.1 shows the tests and the student’s observations for solution F. The student divides
solution F into three portions.
Table 3.1
tests
observations
Do a flame test on the first portion of solution F.
light green colour
test 1
test 2
To the second portion of solution F, add a
1 cm depth of aqueous sodium hydroxide and
a piece of aluminium foil. Warm the mixture
gently and test any gas produced.
effervescence was seen;
the gas turned damp red litmus paper blue
test 3
To the third portion of solution F, add a 1 cm
depth of dilute nitric acid followed by a few
drops of aqueous silver nitrate.
no change
(a)Describe how to do the flame test used in test 1.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
(b)Identify the gas given off in test 2.
.............................................................................................................................................. [1]
(c)Identify solution F.
....................................................................................................................................................
.............................................................................................................................................. [2]
(d)State what would be observed if the student adds dilute sulfuric acid to another portion of
solution F.
observations ...............................................................................................................................
.............................................................................................................................................. [1]
© UCLES 2023
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[Turn over
8
Tests on solid G
Solid G is iron(II) carbonate.
(e)About 10 cm3 of dilute sulfuric acid is added to solid G.
Any gas given off is tested.
observations ...............................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
(f)To the product from (e), aqueous sodium hydroxide is added dropwise until in excess.
observations adding dropwise ....................................................................................................
observations in excess ...............................................................................................................
[2]
[Total: 10]
© UCLES 2023
0620/62/M/J/23
9
4A metal polish is a mixture of four substances.
The properties of these substances are shown in Table 4.1.
Table 4.1
name of substance
solubility in water
reaction with dilute nitric acid
propanol
soluble
dissolves
ethanoic acid
soluble
dissolves
iron(III) oxide
insoluble
reacts when warmed to form a soluble salt
silicon(IV) oxide
insoluble
no reaction
Plan an experiment to find the percentage by mass of silicon(IV) oxide in the mixture. Your plan
should include how you will calculate the percentage of silicon(IV) oxide in the mixture.
You are provided with a sample of the metal polish, dilute nitric acid and common laboratory
apparatus.
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
..................................................................................................................................................... [6]
© UCLES 2023
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[Turn over
10
BLANK PAGE
© UCLES 2023
0620/62/M/J/23
11
Notes for use in qualitative analysis
Tests for anions
anion
test
test result
carbonate, CO32–
add dilute acid, then test for carbon
dioxide gas
effervescence, carbon dioxide
produced
chloride, Cl –
[in solution]
acidify with dilute nitric acid, then
add aqueous silver nitrate
white ppt.
bromide, Br –
[in solution]
acidify with dilute nitric acid, then
add aqueous silver nitrate
cream ppt.
iodide, I–
[in solution]
acidify with dilute nitric acid, then
add aqueous silver nitrate
yellow ppt.
nitrate, NO3–
[in solution]
add aqueous sodium hydroxide,
then aluminium foil; warm carefully
ammonia produced
sulfate, SO42–
[in solution]
acidify with dilute nitric acid, then
add aqueous barium nitrate
white ppt.
sulfite, SO32–
add a small volume of acidified
aqueous potassium manganate(VII)
the acidified aqueous potassium
manganate(VII) changes colour
from purple to colourless
Tests for aqueous cations
cation
effect of aqueous sodium hydroxide
aluminium, Al 3+
white ppt., soluble in excess, giving
a colourless solution
ammonium, NH4+
ammonia produced on warming
calcium, Ca2+
white ppt., insoluble in excess
no ppt. or very slight white ppt.
chromium(III), Cr3+
green ppt., soluble in excess
green ppt., insoluble in excess
copper(II), Cu2+
light blue ppt., insoluble in excess
light blue ppt., soluble in excess,
giving a dark blue solution
iron(II), Fe2+
green ppt., insoluble in excess,
ppt. turns brown near surface on
standing
green ppt., insoluble in excess,
ppt. turns brown near surface on
standing
iron(III), Fe3+
red-brown ppt., insoluble in excess
red-brown ppt., insoluble in excess
zinc, Zn2+
white ppt., soluble in excess, giving
a colourless solution
white ppt., soluble in excess, giving
a colourless solution
© UCLES 2023
0620/62/M/J/23
effect of aqueous ammonia
white ppt., insoluble in excess
–
12
Tests for gases
gas
test and test result
ammonia, NH3
turns damp red litmus paper blue
carbon dioxide, CO2
turns limewater milky
chlorine, Cl 2
bleaches damp litmus paper
hydrogen, H2
‘pops’ with a lighted splint
oxygen, O2
relights a glowing splint
sulfur dioxide, SO2
turns acidified aqueous potassium manganate(VII) from purple to colourless
Flame tests for metal ions
metal ion
flame colour
lithium, Li+
red
sodium, Na+
yellow
potassium, K+
lilac
calcium, Ca2+
orange-red
barium, Ba2+
light green
copper(II), Cu2+
blue-green
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2023
0620/62/M/J/23
Cambridge IGCSE™
*7052172409*
CHEMISTRY0620/42
May/June 2023
Paper 4 Theory (Extended)
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 80.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
This document has 12 pages.
IB23 06_0620_42/3RP
© UCLES 2023
[Turn over
2
1A list of oxides, A to H, is shown.
A
calcium oxide
B
aluminium oxide
C
silicon(IV) oxide
D
sulfur dioxide
E
carbon dioxide
F
iron(III) oxide
G
silver oxide
H
carbon monoxide
Answer the following questions about the oxides, A to H.
Each letter may be used once, more than once or not at all.
State which of the oxides, A to H:
(a)is responsible for acid rain
���������������������������������������������������������������������������������������������������������������������������������������������� [1]
(b)has a giant covalent structure
���������������������������������������������������������������������������������������������������������������������������������������������� [1]
(c)is a reducing agent in the blast furnace
���������������������������������������������������������������������������������������������������������������������������������������������� [1]
(d)is the main constituent of bauxite
���������������������������������������������������������������������������������������������������������������������������������������������� [1]
(e)is the main impurity in iron ore
���������������������������������������������������������������������������������������������������������������������������������������������� [1]
(f)can be reduced by heating with copper.
���������������������������������������������������������������������������������������������������������������������������������������������� [1]
© UCLES 2023
[Total: 6]
0620/42/M/J/23
3
2Fluorine, chlorine and bromine are in Group VII of the Periodic Table.
(a)State the name given to Group VII elements.
............................................................................................................................................... [1]
(b)Explain why Group VII elements have similar chemical properties.
............................................................................................................................................... [1]
(c)Complete Table 2.1 to show the colour and state at r.t.p. of some Group VII elements.
Table 2.1
element
colour
state at r.t.p.
fluorine
pale yellow
chlorine
bromine
liquid
[3]
(d)Bromine has two naturally occurring isotopes, 79Br and 81Br.
(i)State the term given to the numbers 79 and 81 in these isotopes of bromine.
........................................................................................................................................ [1]
(ii)Complete Table 2.2 to show the number of protons, neutrons and electrons in the atom
and ion of bromine shown.
Table 2.2
79
Br
81
Br –
protons
neutrons
electrons
[3]
© UCLES 2023
0620/42/M/J/23
[Turn over
4
(iii)Table 2.3 shows the relative abundances of the two naturally occurring isotopes of bromine.
Table 2.3
isotope
79
Br
relative abundance
55%
81
Br
45%
Calculate the relative atomic mass of bromine to one decimal place.
relative atomic mass = .............................. [2]
(e)Chlorine displaces bromine from aqueous potassium bromide but does not displace fluorine
from aqueous sodium fluoride.
(i)Write the symbol equation for the reaction between chlorine and aqueous potassium
bromide.
........................................................................................................................................ [2]
(ii)State why chlorine does not displace fluorine from aqueous sodium fluoride.
........................................................................................................................................ [1]
(f)Aqueous silver nitrate is a colourless solution containing Ag+(aq) ions.
(i)Describe what is seen when aqueous silver nitrate is added to aqueous sodium chloride.
........................................................................................................................................ [1]
(ii)Write the ionic equation for the reaction between aqueous silver nitrate and aqueous
sodium chloride.
Include state symbols.
........................................................................................................................................ [3]
© UCLES 2023
[Total: 18]
0620/42/M/J/23
5
3Over 200 million tonnes of sulfuric acid are manufactured every year.
(a)State the name of the process used to manufacture sulfuric acid.
............................................................................................................................................... [1]
(b)Part of the manufacture of sulfuric acid involves converting sulfur dioxide to sulfur trioxide.
(i)Describe two methods by which sulfur dioxide is obtained.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
The conversion of sulfur dioxide to sulfur trioxide is a reversible reaction which can reach
equilibrium.
2SO2(g) + O2(g)
2SO3(g)
(ii)State two features of an equilibrium.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(iii)State the typical conditions and name the catalyst used in the conversion of sulfur dioxide
to sulfur trioxide.
temperature ........................................... °C
pressure ................................................. kPa
catalyst ..................................................
[3]
© UCLES 2023
0620/42/M/J/23
[Turn over
6
(iv)Complete Table 3.1 to show the effect, if any, when the following changes are applied to
the conversion of sulfur dioxide to sulfur trioxide.
2SO2(g) + O2(g)
2SO3(g)
The forward reaction is exothermic.
Only use the words increases, decreases or no change.
Table 3.1
change
effect on the rate of
the forward reaction
temperature decreases
decreases
effect on the concentration
of SO3(g) at equilibrium
pressure increases
no catalyst
decreases
[4]
(v)Explain in terms of collision theory why reducing the temperature decreases the rate of the
forward reaction.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(c)Sulfuric acid contains SO42– ions.
The oxidation number of O atoms in SO42– ions is –2.
Determine the oxidation number of S atoms in SO42– ions. Show your working.
oxidation number = .............................. [2]
[Total: 17]
© UCLES 2023
0620/42/M/J/23
7
4Solid sodium hydroxide is a base which dissolves to form an aqueous solution, NaOH(aq).
(a)State what is meant by the term base.
............................................................................................................................................... [1]
(b)State the term given to a base which dissolves to form an aqueous solution.
............................................................................................................................................... [1]
(c)State the colour of thymolphthalein in NaOH(aq).
............................................................................................................................................... [1]
(d)Complete the word equation for the reaction of NaOH(aq) with ammonium chloride.
sodium
hydroxide
+
ammonium
chloride
→
........................
+
........................
+
........................
........................
[3]
(e)Some metal oxides react with NaOH(aq).
(i)State the term given to metal oxides which react with bases such as NaOH(aq).
........................................................................................................................................ [1]
(ii)Name a metal oxide which reacts with NaOH(aq).
........................................................................................................................................ [1]
© UCLES 2023
0620/42/M/J/23
[Turn over
8
(f)Ethanoic acid, CH3COOH, is a weak acid.
(i)Complete the dot-and-cross diagram in Fig. 4.1 of a molecule of ethanoic acid.
O
H
H
C
C
H
O
H
Fig. 4.1
[3]
(ii)Suggest the pH of dilute ethanoic acid.
........................................................................................................................................ [1]
(iii)Complete the symbol equation to show the dissociation of ethanoic acid.
CH3COOH ..................................................................................................................... [3]
(iv)Write the ionic equation for the reaction when an acid neutralises a soluble base.
........................................................................................................................................ [1]
© UCLES 2023
0620/42/M/J/23
9
(g)In a titration, 25.0 cm3 of 0.0800 mol / dm3 aqueous potassium hydroxide, KOH(aq), is neutralised
by 20.0 cm3 of dilute sulfuric acid, H2SO4(aq).
2KOH(aq) + H2SO4(aq) → K2SO4(aq) + 2H2O(l)
Calculate the concentration of H2SO4, in g / dm3 using the following steps.
●
Calculate the number of moles of KOH used.
.............................. mol
●
Determine the number of moles of H2SO4 which react with the KOH.
.............................. mol
●
Calculate the concentration of H2SO4 in mol / dm3.
.............................. mol / dm3
●
Calculate the concentration of H2SO4 in g / dm3.
.............................. g / dm3
[5]
© UCLES 2023
[Total: 21]
0620/42/M/J/23
[Turn over
10
5Propane and propene both react with chlorine.
(a)When a molecule of propane, C3H8, reacts with chlorine in the presence of ultraviolet light, one
atom of hydrogen is replaced by one atom of chlorine.
(i)State the term given to reactions in which one atom in an alkane is replaced by another
atom.
........................................................................................................................................ [1]
(ii)
State the purpose of ultraviolet light in this reaction.
........................................................................................................................................ [1]
(iii)State the term given to any reaction which requires ultraviolet light.
........................................................................................................................................ [1]
(iv)Write the symbol equation for the reaction between propane and chlorine.
........................................................................................................................................ [2]
(b)A molecule of propene, C3H6, is unsaturated and will react with chlorine at room temperature.
(i)State why propene is an unsaturated molecule.
........................................................................................................................................ [1]
(ii)Give the structural formula of the product of this reaction.
........................................................................................................................................ [1]
(c)Propene undergoes addition reactions with steam.
There are two possible products, A and B.
Draw the displayed formula and name each product.
displayed formula of product A
name of product A ......................................................................................................................
displayed formula of product B
name of product B ......................................................................................................................
[4]
© UCLES 2023
[Total: 11]
0620/42/M/J/23
11
6Carboxylic acids can be converted to esters.
(a)Name the ester formed when butanoic acid, CH3CH2CH2COOH, reacts with ethanol, CH3CH2OH.
............................................................................................................................................... [1]
(b)Identify the other product formed in this reaction.
............................................................................................................................................... [1]
(c)Deduce the empirical formula of the ester formed.
............................................................................................................................................... [1]
(d)PET is a polyester. Part of the structure of PET is shown in Fig. 6.1.
O
O
C
C
O
O
O
O
C
C
O
O
Fig. 6.1
(i)Circle one repeat unit of this polymer.
[1]
(ii)Draw the structures of the monomers which make up PET. Draw the functional groups
using displayed formulae.
[2]
(iii)State the type of polymerisation used in making PET.
........................................................................................................................................ [1]
[Total: 7]
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2023
0620/42/M/J/23
© UCLES 2023
12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/M/J/23
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
rutherfordium
La
57
actinoids
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
89–103
178
104
137
88
133
87
Hf
hafnium
Ba
barium
lanthanoids
Cs
72
91
zirconium
Zr
40
48
titanium
caesium
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
–
Nh
nihonium
113
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
–
Mc
moscovium
115
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
Ts
tennessine
117
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Og
oganesson
118
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
12
Cambridge IGCSE™
CHEMISTRY
0620/22
Paper 2 Multiple Choice (Extended)
May/June 2023
45 minutes
You must answer on the multiple choice answer sheet.
*1398337971*
You will need: Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
 There are forty questions on this paper. Answer all questions.
 For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
 Follow the instructions on the multiple choice answer sheet.
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
 Do not use correction fluid.
 Do not write on any bar codes.
 You may use a calculator.
INFORMATION
 The total mark for this paper is 40.
 Each correct answer will score one mark.
 Any rough working should be done on this question paper.
 The Periodic Table is printed in the question paper.
This document has 16 pages.
IB23 06_0620_22/6RP
© UCLES 2023
[Turn over
2
1
Four physical changes of ethanol are listed.
1
condensation
2
evaporation
3
freezing
4
boiling
In which changes do the particles move further apart?
A
2
1 and 2
B
1 and 3
C
2 and 4
D
3 and 4
D
2 and 4
An atom of element X contains:
●
5 protons
●
6 neutrons
●
5 electrons.
Which statements about element X are correct?
A
1
X has an atomic number of 6.
2
X has a nucleon number of 11.
3
X is in Group II of the Periodic Table.
4
X is in the second period of the Periodic Table.
1 and 3
© UCLES 2023
B
1 and 4
C
2 and 3
0620/22/M/J/23
3
3
Ammonia, NH3, is a covalent molecule.
Which diagram shows the outer-shell electron arrangement in a molecule of ammonia?
A
H
N
H
B
H
H
N
H
H
C
D
N
H
H
N
H
4
5
H
H
H
Which structure does silicon(IV) oxide most closely resemble?
A
carbon dioxide
B
diamond
C
graphite
D
sodium chloride
Substance P conducts electricity when solid.
Which particles move in solid P so that it can conduct electricity?
A
1
anions
2
cations
3
electrons
1 and 2
© UCLES 2023
B
1 only
C
2 and 3
0620/22/M/J/23
D
3 only
[Turn over
4
6
7
Which equation represents a chemical change?
A
BaCl 2(s)  BaCl 2(l)
B
Ca2+(aq) + SO42–(aq)  CaSO4(s)
C
KCl (s) + H2O(l)  K+(aq) + Cl –(aq)
D
Na+(aq) + NO3–(aq)  NaNO3(aq)
Which sample contains the largest number of molecules?
A
16 g of methane, CH4(g)
B
16 g of oxygen, O2(g)
C
16 g of phosphorus, P4(s)
D
16 dm3 of methane at r.t.p., CH4(g)
© UCLES 2023
0620/22/M/J/23
5
8
The concentration of a sample of dilute aqueous sodium hydroxide is found by titration.
The apparatus used is shown.
dilute aqueous
hydrochloric acid,
HCl (aq)
dilute aqueous
sodium hydroxide,
NaOH(aq)
Which information is needed to calculate the concentration of the dilute aqueous
sodium hydroxide in mol / dm3?
concentration
of HCl
volume of
HCl used
molar mass
of HCl
volume of
NaOH used
molar mass
of NaOH
A
B
C
D
key
= needed
= not needed
9
In experiment 1, aqueous copper(II) sulfate is electrolysed using graphite electrodes.
In experiment 2, aqueous copper(II) sulfate is electrolysed using copper electrodes.
Which statement identifies a half-equation for a reaction at one of the electrodes?
A
In experiment 1, the half-equation for the anode reaction is 4OH–  2H2O + O2 + 4e–.
B
In experiment 1, the half-equation for the cathode reaction is 2H+ + 2e–  H2.
C
In experiment 2, the half-equation for the anode reaction is Cu2+ + 2e–  Cu.
D
In experiment 2, the half-equation for the cathode reaction is 4OH–  2H2O + O2 + 4e–.
© UCLES 2023
0620/22/M/J/23
[Turn over
6
10 Which substance is not produced during the electrolysis of concentrated aqueous
sodium chloride?
A
chlorine
B
hydrogen
C
sodium
D
sodium hydroxide
11 Methane burns in excess oxygen.
The equation is shown.
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)
Bond energies are shown.
bond
bond energy
in kJ / mol
C=O
805
C–H
410
O=O
496
O–H
460
What is the energy change for the reaction?
A
(4  410 + 2  496) – (2  805 + 4  460)
B
(2  805 + 4  460) – (4  410 + 2  496)
C
(410 + 2  496) – (805 + 2  460)
D
(410 + 496) – (805 + 460)
12 Which change increases the rate of reaction by decreasing the activation energy, Ea?
A
addition of a catalyst
B
decrease in size of solid reactants
C
increase in concentration of solutions
D
increase in temperature
© UCLES 2023
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7
13 In the Contact process, sulfur dioxide is reacted with oxygen to form sulfur trioxide.
Which conditions are used in this reaction?
temperature
/ C
pressure
/ kPa
catalyst
A
300
200
iron
B
300
20 000
vanadium(V) oxide
C
450
200
vanadium(V) oxide
D
450
20 000
iron
14 Which reaction is reversible?
A
an iron nail rusting when left in moist air
B
limestone reacting with an acid to form carbon dioxide gas
C
magnesium burning in air to produce a white ash
D
white anhydrous copper(II) sulfate turning blue when water is added
15 The equation for the reaction of sulfur dioxide with acidified potassium dichromate(VI) is shown.
3SO2 + Cr2O72– + 2H+  3SO42– + 2Cr3+ + H2O
What is oxidised and what is the oxidising agent?
oxidised
oxidising agent
A
SO2
Cr2O72–
B
SO2
H+
C
Cr2O72–
H+
D
Cr2O72–
Cr2O72–
16 What is the definition of a strong acid?
A
a proton acceptor that is completely dissociated in aqueous solution
B
a proton acceptor that is partially dissociated in aqueous solution
C
a proton donor that is completely dissociated in aqueous solution
D
a proton donor that is partially dissociated in aqueous solution
© UCLES 2023
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8
17 Which statement about amphoteric oxides is correct?
A
They are made by combining an acidic oxide with a basic oxide.
B
They react with water to give a solution of pH 7.
C
They react with both acids and bases.
D
They do not react with acids or bases.
18 Copper(II) carbonate is formed when aqueous sodium carbonate is added to aqueous
copper(II) nitrate.
The ionic equation for the reaction is shown.
CO32–(aq) + Cu2+(aq)  CuCO3(s)
How is pure copper(II) carbonate obtained from the reaction mixture?
A
evaporate  filter  dry
B
evaporate  wash  crystallise
C
filter  evaporate  crystallise
D
filter  wash  dry
19 Q and R are elements in the same period of the Periodic Table.
Q has 7 electrons in its outer shell and R has 2 electrons in its outer shell.
Which statement about Q and R is correct?
A
Q is a metal and R is a non-metal.
B
Q and R have different numbers of electron shells.
C
R is found to the right of Q in the Periodic Table.
D
The proton number of R is less than the proton number of Q.
20 Lead(II) sulfate is an insoluble salt.
Which reaction produces a mixture from which lead(II) sulfate is obtained by filtration?
A
adding solid lead(II) carbonate to dilute sulfuric acid
B
adding solid lead(II) hydroxide to dilute sulfuric acid
C
adding metallic lead to dilute sulfuric acid
D
adding aqueous lead(II) nitrate to dilute sulfuric acid
© UCLES 2023
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9
21 Which statement about alkali metals is correct?
A
Lithium is more dense than sodium.
B
Sodium is more reactive than potassium.
C
Sodium has a higher melting point than potassium.
D
They are in Group II of the Periodic Table.
22 Which row describes the properties of a transition element?
melting
point
density
forms coloured
compounds
A
high
low
no
B
high
high
yes
C
low
low
no
D
low
low
yes
23 Which row identifies the properties of zinc?
thermal
conductivity
reacts with
dilute acid
A
good
yes
B
good
no
C
poor
yes
D
poor
no
24 Uses of metals depend on their properties.
Which property is necessary for the use given?
use of the metal
property of the metal
A
car bodies
ductile
B
cutlery
conducts heat
C
food containers
resists corrosion
D
overhead electrical cables
high density
© UCLES 2023
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10
25 Which compounds both contribute to acid rain?
A
carbon monoxide and carbon dioxide
B
carbon monoxide and oxides of nitrogen
C
oxides of nitrogen and sulfur dioxide
D
sulfur dioxide and carbon dioxide
26 P, Q, R and S are metals.
P reacts with dilute hydrochloric acid, forming hydrogen.
Q reacts violently with water.
R reacts with water to give hydrogen.
S is formed by heating its oxide with carbon.
Which row identifies the metals?
P
Q
R
S
A
copper
sodium
potassium
iron
B
zinc
magnesium
calcium
iron
C
zinc
sodium
calcium
magnesium
D
iron
potassium
sodium
zinc
27 Which compound is formed when iron rusts?
A
anhydrous iron(II) oxide
B
anhydrous iron(III) oxide
C
hydrated iron(III) hydroxide
D
hydrated iron(III) oxide
28 Why is cryolite used in the extraction of aluminium by electrolysis?
A
It dissolves the aluminium oxide.
B
It protects the anodes from corrosion.
C
It changes bauxite to aluminium oxide.
D
It decreases the melting point of the aluminium.
© UCLES 2023
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11
29 A wax candle is made from a mixture of hydrocarbons.
The candle is lit and placed in a gas jar along with a strip of cobalt(II) chloride test paper as
shown.
cobalt(II) chloride paper
gas jar
combustion products
wax candle
After a short time, the oxygen in the jar is used up and the candle flame goes out.
Which substance does the cobalt(II) chloride paper identify?
A
carbon dioxide
B
carbon monoxide
C
sulfur dioxide
D
water
30 The hydrocarbon C4H8 has two structural isomers, but-1-ene and but-2-ene.
Which statement is correct?
A
But-2-ene has the structural formula CH3CH=CHCH3 and the same general formula as
butane.
B
But-2-ene has the structural formula CH3CH=CHCH3 and the same empirical formula as
ethene.
C
But-1-ene has the structural formula CH3CH2CH=CH2 and the same general formula as
butane.
D
But-1-ene has the structural formula CH3CHCH2=CH and the same empirical formula as
ethene.
31 Which compound rapidly decolourises aqueous bromine?
A
propane
B
propanoic acid
C
propanol
D
propene
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32 What are the products of the addition reactions of ethene with bromine and hydrogen?
bromine
hydrogen
A
CH2BrCH2Br
CH3CH3
B
CH2BrCH2Br
CH2CH2
C
CH3CH2Br
CH3CH3
D
CH3CH2Br
CH2CH2
33 Ethanol is manufactured by fermentation and the catalytic addition of steam to ethene.
Which row describes an advantage of both methods?
from sugar by fermentation
from ethene and steam
A
ethanol needs to be purified
the process is continuous
B
it is a batch process
ethene comes from petroleum
C
the process is slow
the process is rapid
D
renewable resources are used
the ethanol produced is pure
34 Methanoic acid and propan-1-ol react to form an ester.
What is the structural formula of the ester?
A
HCOOCH2CH2CH3
B
CH3CH2COOCH3
C
CH3COOCH2CH3
D
CH3CH2CH2COOH
© UCLES 2023
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13
35 What is the correct structure of PET?
A
O
O
H
C
C
N
N
O
O
C
C
H
B
C
O
O
C
C
O
O
O
H
C
C
N
O
N
N
N
H
H
O
O
O
C
C
O
O
O
H
C
C
N
N
H
D
O
O
C
C
H
O
O
O
O
C
O
C
36 Alkanes undergo substitution reactions in the presence of UV light.
Which equation represents a substitution reaction of ethane?
A
C2H6 + Cl 2  C2H4 + 2HCl
B
C2H6 + Cl 2  C2H5Cl + HCl
C
C2H6 + Cl 2  C2H4Cl 2 + H2
D
C2H6 + HCl  C2H5Cl + H2
37 Methane reacts with chlorine in substitution reactions.
How many different products, containing a single carbon atom, can be made during the
reactions?
A
2
© UCLES 2023
B
3
C
4
0620/22/M/J/23
D
5
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14
38 Rock salt is a mixture of salt and sand.
The method used to separate the sand from the salt is listed.
step 1
Crush the rock salt, add to warm water and stir.
step 2
Pour the mixture through a filter paper held in a funnel.
step 3
Evaporate the water to crystallise the salt.
Which statement about the method is correct?
A
The filtrate in step 2 is pure water.
B
The residue in step 2 is pure crystals of salt.
C
The solute is salt.
D
The solvent is a mixture of salt and water.
39 Two compounds, M and N, are dissolved in water and separated by chromatography.
The results are shown.
solvent front
N
10 cm
M
2 cm
baseline
What is the Rf value of M and which compound is most soluble in water?
Rf value of M
most soluble
compound
A
0.2
M
B
0.2
N
C
5.0
M
D
5.0
N
© UCLES 2023
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15
40 When acid is added to salt X, a gas is produced which turns limewater milky.
When sodium hydroxide is added to salt X, a gas is produced which turns litmus paper blue.
What is X?
A
CaCO3
B
(NH4)2CO3
C
NH4NO3
D
ZnCO3
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.
© UCLES 2023
0620/22/M/J/23
© UCLES 2023
21
45
39
Y
12
Mg
magnesium
24
20
Ca
calcium
40
38
11
Na
sodium
23
19
K
potassium
39
37
22
73
Ta
72
Hf
89
57–71
lanthanoids
88
56
0620/22/M/J/23
Rf
Db
Th
thorium
232
–
90
89
Ac
140
139
actinium
Ce
cerium
La
231
protactinium
Pa
91
141
praseodymium
Pr
59
58
57
lanthanum
–
dubnium
–
rutherfordium
105
181
tantalum
93
238
uranium
U
92
144
neodymium
Nd
60
–
seaborgium
Sg
106
184
tungsten
W
74
96
molybdenum
Mo
42
52
chromium
Cr
24
–
neptunium
Np
93
–
promethium
Pm
61
–
bohrium
Bh
107
186
rhenium
Re
75
–
technetium
Tc
43
55
manganese
Mn
25
–
plutonium
Pu
94
150
samarium
Sm
62
–
hassium
Hs
108
190
osmium
Os
76
101
ruthenium
Ru
44
56
iron
Fe
26
27
28
29
30
Pt
–
americium
Am
95
152
europium
Eu
63
–
meitnerium
Mt
109
192
–
curium
Cm
96
157
gadolinium
Gd
64
–
darmstadtium
Ds
110
195
platinum
Ir
iridium
78
106
palladium
Pd
46
59
nickel
Ni
77
103
rhodium
Rh
45
59
cobalt
Co
–
berkelium
Bk
97
159
terbium
Tb
65
–
roentgenium
Rg
111
197
gold
Au
79
108
silver
Ag
47
64
copper
Cu
–
californium
Cf
98
163
dysprosium
Dy
66
–
copernicium
Cn
112
201
mercury
Hg
80
112
cadmium
Cd
48
65
zinc
Zn
B
C
–
einsteinium
Es
99
165
holmium
Ho
67
–
nihonium
Nh
113
204
thallium
Tl
81
115
–
fermium
Fm
100
167
erbium
Er
68
–
flerovium
Fl
114
207
lead
Pb
82
119
tin
Sn
In
indium
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
49
70
gallium
Ga
31
27
aluminium
Al
13
11
boron
6
–
mendelevium
Md
101
169
thulium
Tm
69
–
moscovium
Mc
115
209
bismuth
Bi
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
N
7
–
nobelium
No
102
173
ytterbium
Yb
70
–
livermorium
Lv
116
–
polonium
Po
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
O
8
–
lawrencium
Lr
103
175
lutetium
Lu
71
–
tennessine
Ts
117
–
astatine
At
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
F
9
–
oganesson
Og
118
–
radon
Rn
86
131
xenon
Xe
54
84
krypton
Kr
36
40
argon
Ar
18
20
neon
Ne
10
4
5
helium
VIII
1
VII
hydrogen
VI
2
V
He
IV
1
III
H
Group
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
–
actinoids
Ra
radium
Fr
104
88
87
francium
178
89–103
137
133
hafnium
Ba
barium
Cs
caesium
91
Nb
niobium
55
Zr
zirconium
85
yttrium
Sr
strontium
41
51
vanadium
V
Rb
40
48
titanium
Ti
23
relative atomic mass
rubidium
scandium
Sc
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
The Periodic Table of Elements
16
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education
*7994315301*
CHEMISTRY
0620/22
Paper 2
October/November 2015
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name in the spaces at the top of this page.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
A copy of the Periodic Table is printed on page 16.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certificate.
This document consists of 14 printed pages and 2 blank pages.
IB15 11_0620_22/2RP
© UCLES 2015
[Turn over
2
1
The structures of six substances are shown below.
A
B
Ag Ag Ag Ag
Fe Fe Fe Ni
Ag Ag Ag
Fe Ni Fe Fe
Ag Ag Ag Ag
Ni Fe Fe Fe
D
F
Na+
I–
Na+
I–
I–
Na+
I–
Na+
Na+
I–
Na+
I–
E
F
N
F
F
N
F
F
C
O
O
O
Xe
O
Xe
N
F
F
O
F
Xe
O
Xe
Xe
Answer the following questions about these substances.
Each substance may be used once, more than once or not at all.
(a) Which substance, A, B, C, D, E or F,
(i)
is a simple molecular compound,
.......................... [1]
(ii)
is an alloy,
.......................... [1]
(iii)
is a compound, whose aqueous solution gives a yellow
precipitate on addition of aqueous silver nitrate,
.......................... [1]
is an atmospheric pollutant arising from reactions taking
place in car engines,
.......................... [1]
(v)
is a diatomic molecule,
.......................... [1]
(vi)
conducts electricity when molten but not when solid?
.......................... [1]
(iv)
(b) Substance A is an element.
What is meant by the term element ?
....................................................................................................................................................
.............................................................................................................................................. [1]
(c) Substance D oxidises water to oxygen.
Complete the symbol equation for this reaction.
2F2 + 2H2O → .......HF + ...............
[2]
[Total: 9]
© UCLES 2015
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3
2
A student measured the highest temperature reached when four different fuels were burned. He
used the apparatus shown below.
thermometer
clamp
copper can
water
spirit burner
fuel
(a) The same amount of each fuel was burned.
Suggest two other things which the student should keep constant to make the experiment a
fair test.
1. ................................................................................................................................................
2. ................................................................................................................................................
[2]
(b) Is burning an exothermic or an endothermic reaction?
Give a reason for your answer.
.............................................................................................................................................. [1]
(c) The table below shows the results.
(i)
fuel
molecular
formula
initial
temperature / °C
final
temperature / °C
ethanol
C 2 H 6O
23
44
hexane
C6H14
17
46
pentane
C5H12
22
48
propanol
C 3 H 8O
21
45
Which fuel gave the highest temperature change?
....................................................................................................................................... [1]
(ii)
Which fuel has the highest relative molecular mass?
You are not expected to do any calculations.
....................................................................................................................................... [1]
© UCLES 2015
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4
(d) Methane is a fuel.
(i)
Draw the structure of methane showing all atoms and all bonds.
[1]
(ii)
Which one of the following fuels is largely methane?
Tick one box.
coal
fuel oil
gasoline
natural gas
[1]
(e) Pentane and hexane belong to the same homologous series.
(i)
How can you tell this from their names?
....................................................................................................................................... [1]
(ii)
Complete the following sentence about a homologous series using words from the list
below.
acidic
alcohol
compounds
density
different
elements
functional
masses
properties
solid
A homologous series is a family of similar ........................... with similar ...........................
due to the presence of the same ........................... group.
[3]
[Total: 11]
© UCLES 2015
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3
The order of reactivity of zinc, magnesium, calcium and barium is shown below.
zinc → magnesium → calcium → barium
least reactive
most reactive
(a) Equal-sized pieces of zinc, magnesium, calcium and barium are placed in water.
Some observations from these reactions are shown in the table.
(i)
Complete the box for barium.
metal
observations
zinc
no reaction with cold water
magnesium
gives a few bubbles with hot water, does not disappear
calcium
gives off bubbles steadily with cold water, gets smaller slowly
barium
[2]
(ii)
Give the name of a metal in the above table which is extracted by heating with carbon.
....................................................................................................................................... [1]
(iii)
Suggest why barium cannot be extracted using carbon.
....................................................................................................................................... [1]
(b) Barium can be extracted by heating barium oxide with aluminium.
4BaO + 2Al → 3Ba + BaAl 2O4
How does this equation show that barium oxide gets reduced?
.............................................................................................................................................. [1]
(c) A solution of barium hydroxide is alkaline.
(i)
Describe how you would show that barium hydroxide solution is alkaline.
....................................................................................................................................... [1]
(ii)
Complete the word equation for the reaction of barium hydroxide with hydrochloric acid.
barium
hydrochloric
→
+
hydroxide
acid
.........................
+ .........................
.........................
[2]
© UCLES 2015
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6
(d) A student used the apparatus shown below to calculate the concentration of barium hydroxide
solution.
hydrochloric acid
A
barium hydroxide solution
(i)
Give the name of the piece of apparatus labelled A.
....................................................................................................................................... [1]
(ii)
The hydrochloric acid is added to the barium hydroxide solution in the flask until the acid
is in excess.
Describe how the pH of the solution changes as the acid is added.
.............................................................................................................................................
....................................................................................................................................... [2]
(e) Complete the diagram below for the electrolysis of molten zinc chloride.
Label the electrodes and the power source.
molten
zinc chloride
[3]
[Total: 14]
© UCLES 2015
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4
A student investigated the reaction of lumps of iron with sulfuric acid.
Fe(s) + H2SO4(aq) → FeSO4(aq) + H2(g)
She used the apparatus shown below.
water
sulfuric acid
(a) (i)
lumps of
iron
Describe how this apparatus can be used to investigate the rate of this reaction.
.............................................................................................................................................
.............................................................................................................................................
....................................................................................................................................... [3]
(ii)
Describe how the rate of reaction would differ if smaller lumps of iron were used.
All other conditions remain the same.
....................................................................................................................................... [1]
(b) The student investigated the effect of temperature on the reaction rate.
(i)
State three factors which the student should keep the same in each experiment.
1. .........................................................................................................................................
2. .........................................................................................................................................
3. .........................................................................................................................................
[3]
© UCLES 2015
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8
(ii)
The table shows how the rate of reaction changed with temperature.
temperature
/ °C
rate of reaction
in cm3 / s
20
2.2
30
4.4
40
8.8
50
17.6
Use the information in the table to describe how the rate of reaction changed with
temperature.
.............................................................................................................................................
....................................................................................................................................... [2]
(c) Iron(II) sulfate can be prepared by adding excess iron to sulfuric acid.
Describe how you could obtain pure dry crystals of iron(II) sulfate from the reaction mixture in
the conical flask.
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
[Total: 12]
© UCLES 2015
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5
A crystal of sulfur melts when heated.
(a) Explain, using the kinetic particle theory, the differences between the arrangement and motion
of the particles in sulfur crystals and liquid sulfur.
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [4]
(b) Sulfur dioxide is an atmospheric pollutant.
(i)
Describe how sulfur dioxide is formed and how it gets into the atmosphere.
.............................................................................................................................................
.............................................................................................................................................
....................................................................................................................................... [2]
(ii)
What type of oxide is sulfur dioxide?
....................................................................................................................................... [1]
(iii)
Flue gas desulfurisation removes sulfur dioxide from exhaust gases in factories.
Describe the process of flue gas desulfurisation.
.............................................................................................................................................
....................................................................................................................................... [2]
(iv)
Sulfur dioxide is also formed when copper is reduced by hot concentrated sulfuric acid.
Complete the symbol equation for this reaction.
Cu + ......H2SO4 → CuSO4 + SO2 + ......H2O
[2]
(c) Copper is a metal.
Give two physical properties which are characteristic of all metals.
1. ................................................................................................................................................
2. ................................................................................................................................................
[2]
© UCLES 2015
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10
(d) The table below gives some properties of some metals that are used to make electrical cables
and wires.
metal
strength
electrical
conductivity
melting point
/ °C
price
$ / kg
aluminium
comparatively weak
good
660
1.5
copper
strong
very good
1093
29
steel
strong
fairly good
1535
2.1
silver
fairly strong
very good
962
635
(i)
Suggest why aluminium with a steel core is used for overhead power cables.
.............................................................................................................................................
....................................................................................................................................... [2]
(ii)
Copper is used in electrical wiring in the home rather than silver.
Suggest why.
....................................................................................................................................... [1]
[Total: 16]
© UCLES 2015
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6
Geraniol is a chemical found in rose petals.
The structure of geraniol is shown below.
CH3
H
C
C
CH3
CH2
CH2
C
CH3
(a) (i)
(ii)
C
CH2
OH
H
On the structure above, put a ring around the alcohol functional group.
[1]
Is geraniol a saturated or an unsaturated compound?
Give a reason for your answer.
....................................................................................................................................... [1]
(b) Geraniol can be extracted from rose petals by steam distillation using the apparatus shown
below. The geraniol is carried off in small droplets with the steam.
A
rose petals
and water
X
geraniol
water
heat
(i)
Give the name of the piece of apparatus labelled A.
....................................................................................................................................... [1]
(ii)
The vapour at point X is a mixture of geraniol and steam.
Give one property of a mixture which distinguishes it from a compound.
.............................................................................................................................................
....................................................................................................................................... [1]
(iii)
The geraniol and water are collected in the beaker.
What information in the diagram above shows that geraniol is less dense than water?
....................................................................................................................................... [1]
© UCLES 2015
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12
(c) Geraniol can also be extracted from rose petals by grinding the petals in ethanol.
(i)
Draw the structure of ethanol showing all atoms and all bonds.
[1]
(ii)
Complete the word equation for the complete combustion of ethanol.
ethanol + oxygen → .................................................. + ........................
[2]
(d) What is the percentage by volume of oxygen in the air?
.............................................................................................................................................. [1]
[Total: 9]
© UCLES 2015
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13
7
Beryllium is in Group II and Period 2 of the Periodic Table.
(a) Describe the structure of a beryllium atom.
In your answer, refer to
•
•
•
the type and number of each subatomic particle present,
the charges on each type of subatomic particle,
the position of each type of subatomic particle in the atom.
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [5]
(b) Part of the structure of beryllium chloride is shown below.
Cl
Be
Cl
Cl
Be
Cl
Cl
Be
Cl
Deduce the simplest formula for beryllium chloride.
.............................................................................................................................................. [1]
(c) Beryllium carbide, Be2C, reacts with water. Beryllium hydroxide and methane are formed.
Be2C + 4H2O → 2Be(OH)2 + CH4
(i)
Calculate the relative formula mass of beryllium hydroxide.
[2]
(ii)
Describe one adverse effect of methane on the environment.
....................................................................................................................................... [1]
[Total: 9]
© UCLES 2015
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14
BLANK PAGE
© UCLES 2015
0620/22/O/N/15
15
BLANK PAGE
© UCLES 2015
0620/22/O/N/15
© UCLES 2015
Magnesium
Sodium
Calcium
0620/22/O/N/15
Strontium
89
Key
b
X
a
72
b = proton (atomic) number
X = atomic symbol
a = relative atomic mass
*58-71 Lanthanoid series
90-103 Actinoid series
88
Ac
Actinium
Ra
Radium
Fr
Francium
87
*
Hafnium
Lanthanum
57
178
Hf
40
Zirconium
Zr
91
Titanium
139
Yttrium
22
48
Ti
La
39
Y
89
Scandium
21
227
56
Barium
Caesium
45
Sc
226
55
137
Ba
133
Cs
38
Rubidium
37
88
Sr
85
Rb
20
Potassium
19
40
Ca
39
12
24
Mg
23
Na
Beryllium
4
Lithium
K
11
3
9
Be
7
II
Li
I
51
93
Ta
181
Niobium
Nb
90
58
73
52
96
Mo
W
184
Protactinium
Thorium
55
Tc
186
Re
144
Nd
92
60
Uranium
U
238
Neodymium
75
Rhenium
43
Technetium
25
Manganese
Mn
27
59
28
59
29
64
30
65
5
Ru
101
Iron
190
Pm
Osmium
Os
Np
93
Neptunium
61
Promethium
76
44
Ruthenium
26
56
Fe
Sm
150
Iridium
Pu
94
Plutonium
62
152
Eu
Am
95
Americium
63
Europium
78
Platinum
195
Pt
192
46
Palladium
Pd
106
Nickel
Ni
Ir
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
Gd
157
Gold
Au
197
Silver
96
64
Curium
Cm
Gadolinium
79
47
Ag
108
Copper
Cu
201
Bk
Terbium
Tb
159
Mercury
Hg
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
11
6
Dy
162
Thallium
Tl
204
Indium
Cf
98
Californium
66
Es
Holmium
Ho
165
Lead
Pb
207
Tin
99
Einsteinium
67
82
50
119
Sn
115
32
Germanium
Ge
73
Silicon
In
Gallium
Dysprosium
81
49
31
70
Ga
14
28
Si
Carbon
27
Aluminium
13
12
C
Al
Boron
B
7
14
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
8
Se
79
Sulfur
S
32
Oxygen
Po
169
Md
Thulium
Tm
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
16
O
9
Yb
173
Astatine
At
Iodine
I
127
Bromine
Br
80
Chlorine
No
102
Nobelium
70
Ytterbium
85
53
35
17
Cl
35.5
Fluorine
F
19
Lr
Lutetium
Lu
175
Radon
Rn
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
Helium
2
0
Hydrogen
VII
4
VI
He
V
1
IV
H
III
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
91
Pa
Th
232
Praseodymium
Cerium
59
141
Pr
140
74
Tungsten
42
Molybdenum
24
Chromium
Cr
Ce
Tantalum
41
23
Vanadium
V
1
Group
DATA SHEET
The Periodic Table of the Elements
16
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education
*7234333226*
CHEMISTRY
0620/32
Paper 3 (Extended)
October/November 2015
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
A copy of the Periodic Table is printed on page 12.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certificate.
This document consists of 12 printed pages.
IB15 11_0620_32/FP
© UCLES 2015
[Turn over
2
1
Use your copy of the Periodic Table to help you answer some of these questions.
(a) Predict the formulae of the following compounds.
(i)
nitrogen fluoride ..................................................................................................................
(ii)
phosphorus sulfide .............................................................................................................
[2]
(b) Deduce the formulae of the following ions.
(i)
selenide ..............................................................................................................................
(ii)
gallium ................................................................................................................................
[2]
(c) Use the following ions to determine the formulae of the compounds.
ions
OH–
Cr3+
Ba2+
SO42–
compounds
(i)
chromium(III) sulfate ..........................................................................................................
(ii)
barium hydroxide ................................................................................................................
[2]
[Total: 6]
© UCLES 2015
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3
2
(a) Polluted air contains two oxides of carbon and two oxides of nitrogen. A major source of these
pollutants is motor vehicles.
(i)
Describe how carbon dioxide and carbon monoxide are formed in motor vehicle engines.
.............................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
....................................................................................................................................... [3]
(ii)
State one adverse effect of each of these gases.
.............................................................................................................................................
....................................................................................................................................... [2]
(iii)
Nitrogen monoxide, NO, is released by motor vehicle exhausts.
Explain how nitrogen monoxide is formed in motor vehicle engines.
.............................................................................................................................................
....................................................................................................................................... [2]
(iv)
When nitrogen monoxide is released into the atmosphere, nitrogen dioxide, NO2, is formed.
Suggest an explanation why this happens.
....................................................................................................................................... [1]
(b) Predict the possible adverse effect on the environment when this non-metal oxide, NO2, reacts
with water and oxygen.
....................................................................................................................................................
.............................................................................................................................................. [2]
(c) How are the amounts of carbon monoxide and nitrogen monoxide emitted by modern motor
vehicles reduced? Include an equation in your answer.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
[Total: 13]
© UCLES 2015
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4
3
Two of the main uses of zinc are for galvanising and for making alloys.
One of the main ores of zinc is zinc blende, ZnS. There are two stages in the extraction of zinc from
this ore.
(a) Stage 1 Zinc oxide is made from zinc blende.
Describe how this is done and write a word equation for the reaction.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
(b) Stage 2 Zinc oxide is reduced to zinc.
Write a word equation for the reduction of zinc oxide by coke.
.............................................................................................................................................. [1]
(c) The zinc produced by this process is impure. It can be purified by electrolysis using a method
which is similar to the purification of copper. Under the conditions used in the process, zinc is
the product at the negative electrode (cathode).
Complete the following description of this purification.
The electrolyte is aqueous ................................................................................................. . [1]
The negative electrode (cathode) is made of .................................................................... . [1]
The positive electrode (anode) is impure zinc.
The equation for the reaction at the cathode is ................................................................. . [1]
The equation for the reaction at the anode is .................................................................... . [1]
Explain why the concentration of the electrolyte does not change.
....................................................................................................................................................
.............................................................................................................................................. [2]
© UCLES 2015
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5
(d) Brass is an alloy which contains zinc.
(i)
Name the other metal in brass.
....................................................................................................................................... [1]
(ii)
Suggest two reasons why an alloy such as brass is preferred to either of its constituent
metals.
.............................................................................................................................................
....................................................................................................................................... [2]
(e) In an experiment to investigate the rate of rusting of steel, three pieces of steel were used. One
piece of steel was completely coated with copper, one piece completely coated with zinc and
the third piece was left uncoated. All three pieces were left exposed to the atmosphere.
(i)
Explain why the uncoated piece started to rust.
.............................................................................................................................................
....................................................................................................................................... [1]
(ii)
The coating on both of the other two pieces was scratched, exposing the steel.
exposed steel
does not rust
thin layer
of zinc
steel
The piece of steel coated with zinc still did not rust but the copper-coated piece of steel
rusted very rapidly.
Explain these observations in terms of the formation of ions and the transfer of electrons.
.............................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
....................................................................................................................................... [4]
[Total: 17]
© UCLES 2015
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6
4
(a) Propane reacts with chlorine to form a mixture of chloropropanes. This is a photochemical
reaction.
(i)
What is meant by the phrase photochemical reaction?
.............................................................................................................................................
....................................................................................................................................... [1]
(ii)
The products of this reaction include two isomers, one of which has the following structural
formula.
H
H
H
H
C
C
C
H
H
H
Cl
Draw the structural formula of the other isomer.
[1]
(iii)
Explain why these two different compounds are isomers.
.............................................................................................................................................
....................................................................................................................................... [2]
© UCLES 2015
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7
(b) Bond breaking is an endothermic change and bond forming is an exothermic change.
Bond energy is the amount of energy in kJ / mol needed to break one mole of the specified
bond.
H
H
H
H
C
C
C
H
H
H
H
+
Cl
Cl
→
H
H
H
H
C
C
C
H
H
H
Cl
+
H
Cl
Use the following bond energies to determine whether this reaction is exothermic or
endothermic. You must show your reasoning.
bond
bond energies
in kJ / mol
C–Cl
338
C–H
412
Cl –Cl
242
H–Cl
431
C–C
348
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
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8
(c) (i)
Chloropropane can be hydrolysed to propanol, CH3CH2CH2OH, by sodium hydroxide.
Write the equation for this reaction.
....................................................................................................................................... [2]
(ii)
Propanol can be dehydrated. It loses a water molecule to form a hydrocarbon.
Give the name and structural formula of this hydrocarbon.
name .................................................
structural formula
[2]
(iii)
Propanol is oxidised to a carboxylic acid by acidified potassium manganate(VII).
Deduce the name of this acid.
....................................................................................................................................... [1]
(d) Propanol reacts with methanoic acid to form the ester propyl methanoate.
CH3CH2CH2OH + HCOOH → HCOOCH2CH2CH3 + H2O
4.0 g of methanoic acid was reacted with 6.0 g of propanol.
(i)
Calculate the Mr of methanoic acid = ........................................
[1]
(ii)
Calculate the Mr of propanol = ........................................
[1]
(iii)
Determine which one is the limiting reagent. Show your reasoning.
.............................................................................................................................................
.............................................................................................................................................
....................................................................................................................................... [2]
(iv)
Calculate the maximum yield in grams of propyl methanoate, Mr = 88.
....................................................................................................................................... [1]
[Total: 17]
© UCLES 2015
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9
5
Iron is extracted from its ore, hematite, in a blast furnace.
Substances added to the furnace are:
• iron ore, hematite, containing impurities such as silica, SiO2
• air
• coke, C
• limestone, CaCO3
Substances formed in the blast furnace are:
• molten iron
• molten slag
• waste gases such as carbon dioxide
(a) State the two functions of the coke used in the blast furnace.
....................................................................................................................................................
.............................................................................................................................................. [2]
(b) Write an equation for the conversion of hematite, Fe2O3, to iron.
.............................................................................................................................................. [2]
(c) Explain how the silica impurity is removed and separated from the molten iron.
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
(d) The molten iron from the furnace is impure.
It contains impurities which include the element carbon.
Explain how the carbon is removed. Include an equation in your answer.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
[Total: 10]
© UCLES 2015
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10
6
The table below shows the elements in the third period of the Periodic Table, the number of
electrons in their outer energy level, their oxidation state in their common compounds and their
melting points.
element
Na
Mg
Al
Si
P
S
Cl
Ar
number of outer electrons
1
2
3
4
5
6
7
8
oxidation state
+1
+2
+3
+4 / –4
–3
–2
–1
0
melting point / °C
98
650
660
1414
317
115
–101
–189
(a) Describe and explain the variation in oxidation state across the period.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
(b) The first three elements, Na, Mg and Al, are metals.
Describe the structure of a typical metal.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
(c) Explain why Na, Mg and Al are good conductors of electricity.
.............................................................................................................................................. [1]
(d) Which element exists as diatomic molecules of the type X2?
.............................................................................................................................................. [1]
(e) Silicon has a similar structure to diamond.
Explain why silicon has the highest melting point in the period.
....................................................................................................................................................
.............................................................................................................................................. [2]
© UCLES 2015
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11
(f) Sodium chloride is a crystalline solid with a high melting point. It dissolves in water to give a
neutral solution. Phosphorus trichloride is a liquid at room temperature. It reacts with water to
form an acidic solution.
Suggest an explanation for these differences in properties.
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
(g) Describe how you could show that magnesium oxide is a basic oxide and not an amphoteric
oxide.
....................................................................................................................................................
.............................................................................................................................................. [2]
(h) Draw a dot-and-cross diagram showing the bonding in magnesium oxide. Show outer electrons
only.
[3]
[Total: 17]
© UCLES 2015
0620/32/O/N/15
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© UCLES 2015
4
Magnesium
Sodium
45
0620/32/O/N/15
88
89
Key
b
X
a
Ta
181
b = proton (atomic) number
90
92
27
59
28
59
29
64
30
65
5
6
7
14
8
16
9
19
VII
2
4
0
56
Pm
Osmium
Os
190
Np
93
Neptunium
61
Promethium
76
44
Ruthenium
Ru
101
Iron
Fe
Sm
150
Pu
94
Plutonium
62
Eu
152
Am
95
Americium
63
Europium
78
Pt
Platinum
Ir
Iridium
195
46
Palladium
Pd
106
Nickel
Ni
192
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
Gd
157
Gold
Au
197
96
64
Curium
Cm
Gadolinium
79
47
Silver
Ag
108
Copper
Cu
Bk
Terbium
Tb
159
Mercury
Hg
201
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
70
Dy
162
Thallium
Tl
204
Cf
98
Es
Holmium
Ho
165
Lead
Pb
207
99
Einsteinium
67
82
50
Tin
Sn
Indium
In
32
119
Californium
66
73
Ge
Germanium
14
Silicon
115
Gallium
Ga
Dysprosium
81
49
31
13
Aluminium
28
Si
27
Carbon
C
Al
Boron
B
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
79
Se
Po
Md
Thulium
Tm
169
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
Sulfur
S
32
Oxygen
O
80
Yb
173
Astatine
At
Iodine
I
127
Bromine
Br
No
102
Nobelium
70
Ytterbium
85
53
35
17
Chlorine
Cl
35.5
Fluorine
F
Lr
Lutetium
Lu
175
Radon
Rn
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
He
12
VI
Helium
11
V
H
26
1
IV
Hydrogen
1
III
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
91
U
Uranium
Pa
Protactinium
Th
Thorium
60
238
59
Nd
Neodymium
Pr
Praseodymium
Ce
Cerium
75
144
74
Re
186
Rhenium
43
Technetium
Tc
Manganese
25
141
140
W
184
Tungsten
42
Molybdenum
Mo
96
Chromium
24
55
Mn
232
58
73
Tantalum
41
Niobium
Nb
93
Vanadium
23
52
Cr
X = atomic symbol
72
51
V
a = relative atomic mass
*58-71 Lanthanoid series
90-103 Actinoid series
87
Ac
Ra
Radium
Fr
Francium
Actinium
227
57
Hf
Hafnium
La
Lanthanum
Ba
Barium
Cs
Caesium
56
178
40
139
*
Zr
91
Titanium
Zirconium
22
48
Ti
137
133
38
226
55
37
Y
Sr
Strontium
Rb
Rubidium
Yttrium
89
39
21
Scandium
Sc
88
85
Calcium
20
Potassium
19
40
Ca
39
12
24
Mg
23
Na
Beryllium
Lithium
K
11
3
9
Be
7
II
Li
I
Group
DATA SHEET
The Periodic Table of the Elements
12
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education
*7362226526*
CHEMISTRY
0620/62
Paper 6 Alternative to Practical
October/November 2015
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certificate.
This document consists of 12 printed pages.
IB15 11_0620_62/FP
© UCLES 2015
[Turn over
2
1
The volume of hydrochloric acid that reacts with 25.0 cm3 of aqueous sodium hydroxide can be
found using the apparatus below.
hydrochloric acid
25.0 cm3 of aqueous
sodium hydroxide
+ indicator
(a) Complete the boxes to identify the pieces of apparatus labelled.
[2]
(b) Name a suitable indicator that could be used.
.............................................................................................................................................. [1]
© UCLES 2015
0620/62/O/N/15
3
(c) A student did the experiment four times and the volume of hydrochloric acid added each time
was measured.
Use the burette diagrams in the table to record the volumes of hydrochloric acid added.
experiment
burette diagram
volume of acid
added / cm3
16
1
17
18
16
2
17
18
16
3
17
18
16
4
17
18
[2]
(d) (i)
What type of chemical reaction occurs when hydrochloric acid reacts with sodium
hydroxide?
....................................................................................................................................... [1]
(ii)
How did the student know when all of the sodium hydroxide had reacted?
....................................................................................................................................... [1]
© UCLES 2015
0620/62/O/N/15
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4
(e) (i)
Which one of the results is anomalous?
....................................................................................................................................... [1]
(ii)
Suggest what may have caused this result to be anomalous.
....................................................................................................................................... [1]
(iii)
Use the other results to calculate the average amount of hydrochloric acid that reacted
with the sodium hydroxide solution.
.............................................................................................................................................
....................................................................................................................................... [2]
(f) Which of the solutions was more concentrated? Explain your answer.
....................................................................................................................................................
.............................................................................................................................................. [2]
[Total: 13]
© UCLES 2015
0620/62/O/N/15
5
2
A mixture of three compounds, P, Q and R, was separated using a piece of paper.
solvent front
R
P
baseline
Q
(a) Name this method of separation.
.............................................................................................................................................. [1]
(b) What could have been used to apply the mixture onto the paper?
.............................................................................................................................................. [1]
(c) Suggest a possible solvent that could be used for this separation.
.............................................................................................................................................. [1]
(d) Suggest why compound Q remained on the baseline.
....................................................................................................................................................
.............................................................................................................................................. [1]
(e) Rf values are used to identify compounds.
Rf =
distance travelled by compound
distance travelled by the solvent
Use the diagram to work out the Rf value of compound R.
....................................................................................................................................................
.............................................................................................................................................. [2]
[Total: 6]
© UCLES 2015
0620/62/O/N/15
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6
3
A teacher demonstrated the rate of reaction of dilute nitric acid with powdered calcium carbonate
at different temperatures.
50 cm3 of dilute nitric acid was heated to a known temperature and placed on a balance.
cotton wool
powdered
calcium carbonate
50 cm3 of dilute
nitric acid
balance
Excess powdered calcium carbonate was added to the nitric acid and the mass of the beaker and
contents recorded. The time taken for the mass to decrease by 1 g was measured. The experiment
was repeated at different temperatures.
(a) Using the thermometer diagrams, record the temperatures in the table.
thermometer
diagram
temperature of
nitric acid / °C
time for mass to
decrease by 1 g
in seconds
30
139
25
20
40
102
35
30
50
99
45
40
60
60
55
50
75
45
70
65
85
38
80
75
[3]
© UCLES 2015
0620/62/O/N/15
7
(b) Plot the results on the grid and draw a smooth line graph.
160
140
120
100
time
80
/s
60
40
20
0
0
10
20
30
40
50
60
70
80
temperature of acid / °C
[3]
(c) Which point is inaccurate? Explain why you chose this point.
....................................................................................................................................................
.............................................................................................................................................. [2]
(d) Use your graph to find out the time of reaction at a temperature of 30 °C. Show clearly on the
grid how you obtained your answer.
.............................................................................................................................................. [3]
© UCLES 2015
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8
(e) (i)
How does the rate of this reaction vary with the change in temperature?
....................................................................................................................................... [1]
(ii)
Explain why.
.............................................................................................................................................
.............................................................................................................................................
....................................................................................................................................... [2]
(f) (i)
What would be the effect of repeating the experiments using lumps of calcium carbonate
instead of powdered calcium carbonate? Explain your answer.
.............................................................................................................................................
....................................................................................................................................... [2]
(ii)
Sketch on the grid the curve you would expect.
[1]
(g) Explain why cotton wool was used in the neck of the conical flask.
....................................................................................................................................................
.............................................................................................................................................. [2]
[Total: 19]
© UCLES 2015
0620/62/O/N/15
9
4
Three jars of gas have lost their labels. The gases are known to be
•
ethene,
•
ammonia,
•
oxygen.
Complete the table to show the chemical tests that could be used to identify each of these gases.
gas
chemical test
result of test
................................................
................................................
................................................
.......................................... [2]
................................................
................................................
................................................
.......................................... [2]
................................................
................................................
................................................
.......................................... [2]
ethene
ammonia
oxygen
[Total: 6]
© UCLES 2015
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10
5
Two aqueous solutions, K and L, were analysed. Solution L was aqueous calcium iodide.
Tests on the solutions and some of the observations are in the following tables.
Complete the observations in the second table.
tests
observations
tests on solution K
green / blue
(a) Colour of solution K.
(b) The solution was divided into four
equal portions.
(i)
(ii)
(iii)
(iv)
Aqueous sodium hydroxide
was added to the first portion
drop by drop and shaken.
pale blue precipitate
An excess of aqueous sodium
hydroxide was then added to
the mixture.
the precipitate was insoluble
Aqueous ammonia was added
to the second portion drop by
drop and shaken.
blue precipitate
An excess of aqueous
ammonia was then added to
the mixture.
the precipitate dissolved to form a deep blue solution
Dilute nitric acid and barium
nitrate solution were added to
the third portion.
no visible change
Dilute nitric acid and silver
nitrate solution were added to
the fourth portion.
white precipitate formed
(c) Identify solution K.
.............................................................................................................................................. [2]
© UCLES 2015
0620/62/O/N/15
11
tests
observations
tests on solution L
(d) Colour of solution L.
...................................................................................... [1]
(e) The solution was divided into three
equal portions.
(i)
(ii)
(iii)
Aqueous sodium hydroxide
was added to the first portion
of the solution drop by drop
and shaken.
...................................................................................... [2]
An excess of aqueous sodium
hydroxide was then added to
the mixture.
...................................................................................... [1]
Aqueous ammonia was added
to the second portion of the
solution drop by drop and
shaken.
...................................................................................... [1]
An excess of aqueous
ammonia was then added to
the mixture and shaken.
...................................................................................... [1]
Dilute nitric acid and silver
nitrate solution were added to
the third portion of the solution.
...................................................................................... [2]
[Total: 10]
© UCLES 2015
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12
6
You are provided with samples of three metals, tin, zinc and silver.
Plan an investigation to show the order of reactivity of these three metals.
You are provided with common laboratory apparatus and dilute acids.
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
..................................................................................................................................................... [6]
[Total: 6]
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable
effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will
be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2015
0620/62/O/N/15
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education
*7492298954*
CHEMISTRY
0620/62
Paper 6 Alternative to Practical
February/March 2015
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certificate.
This document consists of 12 printed pages.
IB15 03_0620_62/3RP
© UCLES 2015
[Turn over
2
1
A teacher separated a mixture of two liquids using the apparatus shown. The liquids were:
•
ethanoic acid, boiling point 118 °C,
•
chloroethanoic acid, boiling point 190 °C.
cold water out
fractionating column
small
glass beads
cold water in
mixture of liquids
heat
(a) Complete the boxes to label the pieces of apparatus used.
(b) (i)
[2]
Which liquid would be collected first? Explain why.
.............................................................................................................................................
....................................................................................................................................... [2]
(ii)
How would the teacher know when all of this liquid had been collected?
....................................................................................................................................... [1]
(c) Suggest why small glass beads are used in the fractionating column instead of large glass
beads.
....................................................................................................................................................
.............................................................................................................................................. [1]
(d) Give a test to show that the liquids are acidic.
test .............................................................................................................................................
result .................................................................................................................................... [2]
[Total: 8]
© UCLES 2015
0620/62/F/M/15
3
2
The rate of reaction between excess calcium carbonate and dilute hydrochloric acid was investigated
using the apparatus shown below. The temperature of the hydrochloric acid was 25 °C.
gas syringe
hydrochloric acid
excess calcium carbonate
The volume of carbon dioxide evolved was measured every minute for six minutes.
(a) Use the gas syringe diagrams to complete the table of results.
time
/ minutes
0
1
2
3
4
5
6
total volume of
carbon dioxide evolved / cm3
gas syringe diagram
0
10
20
30
40
50
60
0
10
20
30
40
50
60
0
10
20
30
40
50
60
30
40
50
60
70
80
90
30
40
50
60
70
80
90
30
40
50
60
70
80
90
30
40
50
60
70
80
90
[3]
© UCLES 2015
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4
(b) Plot the results on the grid below and draw a smooth line graph.
100
80
60
volume of
carbon dioxide
evolved / cm3
40
20
0
0
1
2
3
4
5
6
time / minutes
[4]
(c) (i)
Which point appears to be inaccurate? Explain why.
.............................................................................................................................................
....................................................................................................................................... [2]
(ii)
Use your graph to work out the volume of gas expected at that time. Show clearly on the
grid how you worked out your answer.
....................................................................................................................................... [2]
(d) Sketch, on the grid, the graph you would expect if the experiment was repeated using
hydrochloric acid at a temperature of 50 °C.
[2]
[Total: 13]
© UCLES 2015
0620/62/F/M/15
5
3
Electricity was passed through concentrated hydrochloric acid using the apparatus shown.
battery
+
–
positive
electrode
negative
electrode
concentrated
hydrochloric acid and
Universal Indicator
Effervescence was observed at both electrodes.
(a) Name this process used to break down concentrated hydrochloric acid.
.............................................................................................................................................. [1]
(b) Suggest why the electrodes are made of platinum and not aluminium.
.............................................................................................................................................. [1]
(c) (i)
Name the gas given off at the positive electrode.
.............................................................................................................................................
(ii)
What would be the colour of the Universal Indicator around the positive electrode at the
end of the experiment?
.............................................................................................................................................
[2]
[Total: 4]
© UCLES 2015
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6
4
A student investigated the solubility of salt D in water at various temperatures.
Four experiments were carried out.
(a) Experiment 1
4 g of salt D was added to a boiling tube. A burette was filled with distilled water and 10.0 cm3 of
water added to the boiling tube. The mixture of salt D and water was heated carefully until all of
the solid had dissolved. The boiling tube was removed from the heat and the solution allowed
to cool. The solution was stirred gently with a thermometer.
The temperature at which crystals first appeared was noted.
The boiling tube and its contents were kept for the remaining three experiments.
(b) Experiment 2
From the burette another 2.0 cm3 of water was added to the boiling tube and contents from
Experiment 1.
The mixture was heated to dissolve the crystals and allowed to cool as in Experiment 1. The
temperature at which crystals first appeared was noted.
Record, in the table, the total volume of water in the boiling tube.
(c) Experiment 3
From the burette another 2.0 cm3 of water was added to the boiling tube and contents from
Experiment 2. The experiment was repeated exactly as before.
Record, in the table, the total volume of water in the boiling tube.
© UCLES 2015
0620/62/F/M/15
7
(d) Experiment 4
From the burette another 4.0 cm3 of water was added to the boiling tube and contents from
Experiment 3. The experiment was repeated exactly as before.
Record in the table the total volume of water in the boiling tube.
Use the thermometer diagrams in the table to record the temperatures at which crystals first
appeared in the four experiments.
Experiment
number
total volume
of water / cm3
thermometer diagram
temperature at which
crystals first appeared / °C
95
1
10.0
90
85
80
2
75
70
70
3
65
60
60
4
55
50
[3]
© UCLES 2015
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8
(e) Plot the results on the grid below and draw a smooth line graph.
temperature
at which crystals
first appeared / °C
8.0
10.0
12.0
14.0
16.0
18.0
20.0
total volume of water / cm3
[5]
(f) From your graph, find the temperature at which crystals of D would first appear if the total
volume of water in the solution was 20.0 cm3.
Show clearly on the grid how you worked out your answer.
...............................
[3]
(g) How would the student know when salt D was completely dissolved in the water?
.............................................................................................................................................. [1]
© UCLES 2015
0620/62/F/M/15
9
(h) The solubility of salt D at 100 °C is 57 g in 100 cm3 of water.
Suggest, with a reason, the effect of using 8 g of salt D instead of 4 g in these experiments.
....................................................................................................................................................
.............................................................................................................................................. [2]
(i) Salt C is less soluble in water than salt D.
Sketch on the grid the graph you would expect for salt C. Label this graph.
[2]
(j) Describe and explain one improvement that could be made to the experimental method to
obtain more reliable results in this investigation.
improvement ..............................................................................................................................
explanation ................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
[Total: 18]
© UCLES 2015
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10
5
Two metal salt solutions, E and F, were analysed.
E was a mixture of iron(II) sulfate and ammonium sulfate.
The tests on the solutions and some of the observations are in the following table.
Complete the observations in the table.
tests
observations
tests on solution E
(a) Appearance of solution E.
................................................................ [1]
The solution was divided into three equal
portions in separate test-tubes.
(b) Dilute nitric acid and aqueous barium
nitrate were added to the first portion of the
solution.
................................................................ [1]
(c) (i) Excess aqueous sodium hydroxide
was added to the second portion of
the solution.
................................................................ [2]
(ii) The mixture was filtered and the filtrate
heated.
The gas given off was tested with
damp litmus paper.
(d) Dilute sulfuric acid and aqueous potassium
manganate(VII), an oxidising agent, were
added to the third portion of the solution.
Aqueous sodium hydroxide was then
added to the mixture.
......................................................................
................................................................ [2]
................................................................ [1]
tests on solution F
(e) Appearance of solution F.
(f)
yellow liquid
Zinc powder was added to solution F.
rapid effervescence
The solution was observed for five minutes.
turned blue, then green and finally light purple
The gas given off was tested with a splint.
lighted splint popped
© UCLES 2015
0620/62/F/M/15
11
(g) Identify the gas given off in test (f).
.............................................................................................................................................. [1]
(h) What conclusions can you draw about solution F?
....................................................................................................................................................
.............................................................................................................................................. [2]
[Total: 10]
© UCLES 2015
0620/62/F/M/15
[Turn over
12
6
Rhubarb Leaves
Ethanedioic acid dihydrate, H2C2O4.2H2O, is a white crystalline solid. This acid is water-soluble and
is found in rhubarb leaves.
Plan an investigation to obtain crystals of ethanedioic acid dihydrate from some rhubarb leaves.
You are provided with common laboratory apparatus, water and sand.
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
..................................................................................................................................................... [7]
[Total: 7]
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable
effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will
be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2015
0620/62/F/M/15
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education
*7492298954*
CHEMISTRY
0620/62
Paper 6 Alternative to Practical
February/March 2015
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certificate.
This document consists of 12 printed pages.
IB15 03_0620_62/3RP
© UCLES 2015
[Turn over
2
1
A teacher separated a mixture of two liquids using the apparatus shown. The liquids were:
•
ethanoic acid, boiling point 118 °C,
•
chloroethanoic acid, boiling point 190 °C.
cold water out
fractionating column
small
glass beads
cold water in
mixture of liquids
heat
(a) Complete the boxes to label the pieces of apparatus used.
(b) (i)
[2]
Which liquid would be collected first? Explain why.
.............................................................................................................................................
....................................................................................................................................... [2]
(ii)
How would the teacher know when all of this liquid had been collected?
....................................................................................................................................... [1]
(c) Suggest why small glass beads are used in the fractionating column instead of large glass
beads.
....................................................................................................................................................
.............................................................................................................................................. [1]
(d) Give a test to show that the liquids are acidic.
test .............................................................................................................................................
result .................................................................................................................................... [2]
[Total: 8]
© UCLES 2015
0620/62/F/M/15
3
2
The rate of reaction between excess calcium carbonate and dilute hydrochloric acid was investigated
using the apparatus shown below. The temperature of the hydrochloric acid was 25 °C.
gas syringe
hydrochloric acid
excess calcium carbonate
The volume of carbon dioxide evolved was measured every minute for six minutes.
(a) Use the gas syringe diagrams to complete the table of results.
time
/ minutes
0
1
2
3
4
5
6
total volume of
carbon dioxide evolved / cm3
gas syringe diagram
0
10
20
30
40
50
60
0
10
20
30
40
50
60
0
10
20
30
40
50
60
30
40
50
60
70
80
90
30
40
50
60
70
80
90
30
40
50
60
70
80
90
30
40
50
60
70
80
90
[3]
© UCLES 2015
0620/62/F/M/15
[Turn over
4
(b) Plot the results on the grid below and draw a smooth line graph.
100
80
60
volume of
carbon dioxide
evolved / cm3
40
20
0
0
1
2
3
4
5
6
time / minutes
[4]
(c) (i)
Which point appears to be inaccurate? Explain why.
.............................................................................................................................................
....................................................................................................................................... [2]
(ii)
Use your graph to work out the volume of gas expected at that time. Show clearly on the
grid how you worked out your answer.
....................................................................................................................................... [2]
(d) Sketch, on the grid, the graph you would expect if the experiment was repeated using
hydrochloric acid at a temperature of 50 °C.
[2]
[Total: 13]
© UCLES 2015
0620/62/F/M/15
5
3
Electricity was passed through concentrated hydrochloric acid using the apparatus shown.
battery
+
–
positive
electrode
negative
electrode
concentrated
hydrochloric acid and
Universal Indicator
Effervescence was observed at both electrodes.
(a) Name this process used to break down concentrated hydrochloric acid.
.............................................................................................................................................. [1]
(b) Suggest why the electrodes are made of platinum and not aluminium.
.............................................................................................................................................. [1]
(c) (i)
Name the gas given off at the positive electrode.
.............................................................................................................................................
(ii)
What would be the colour of the Universal Indicator around the positive electrode at the
end of the experiment?
.............................................................................................................................................
[2]
[Total: 4]
© UCLES 2015
0620/62/F/M/15
[Turn over
6
4
A student investigated the solubility of salt D in water at various temperatures.
Four experiments were carried out.
(a) Experiment 1
4 g of salt D was added to a boiling tube. A burette was filled with distilled water and 10.0 cm3 of
water added to the boiling tube. The mixture of salt D and water was heated carefully until all of
the solid had dissolved. The boiling tube was removed from the heat and the solution allowed
to cool. The solution was stirred gently with a thermometer.
The temperature at which crystals first appeared was noted.
The boiling tube and its contents were kept for the remaining three experiments.
(b) Experiment 2
From the burette another 2.0 cm3 of water was added to the boiling tube and contents from
Experiment 1.
The mixture was heated to dissolve the crystals and allowed to cool as in Experiment 1. The
temperature at which crystals first appeared was noted.
Record, in the table, the total volume of water in the boiling tube.
(c) Experiment 3
From the burette another 2.0 cm3 of water was added to the boiling tube and contents from
Experiment 2. The experiment was repeated exactly as before.
Record, in the table, the total volume of water in the boiling tube.
© UCLES 2015
0620/62/F/M/15
7
(d) Experiment 4
From the burette another 4.0 cm3 of water was added to the boiling tube and contents from
Experiment 3. The experiment was repeated exactly as before.
Record in the table the total volume of water in the boiling tube.
Use the thermometer diagrams in the table to record the temperatures at which crystals first
appeared in the four experiments.
Experiment
number
total volume
of water / cm3
thermometer diagram
temperature at which
crystals first appeared / °C
95
1
10.0
90
85
80
2
75
70
70
3
65
60
60
4
55
50
[3]
© UCLES 2015
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[Turn over
8
(e) Plot the results on the grid below and draw a smooth line graph.
temperature
at which crystals
first appeared / °C
8.0
10.0
12.0
14.0
16.0
18.0
20.0
total volume of water / cm3
[5]
(f) From your graph, find the temperature at which crystals of D would first appear if the total
volume of water in the solution was 20.0 cm3.
Show clearly on the grid how you worked out your answer.
...............................
[3]
(g) How would the student know when salt D was completely dissolved in the water?
.............................................................................................................................................. [1]
© UCLES 2015
0620/62/F/M/15
9
(h) The solubility of salt D at 100 °C is 57 g in 100 cm3 of water.
Suggest, with a reason, the effect of using 8 g of salt D instead of 4 g in these experiments.
....................................................................................................................................................
.............................................................................................................................................. [2]
(i) Salt C is less soluble in water than salt D.
Sketch on the grid the graph you would expect for salt C. Label this graph.
[2]
(j) Describe and explain one improvement that could be made to the experimental method to
obtain more reliable results in this investigation.
improvement ..............................................................................................................................
explanation ................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [2]
[Total: 18]
© UCLES 2015
0620/62/F/M/15
[Turn over
10
5
Two metal salt solutions, E and F, were analysed.
E was a mixture of iron(II) sulfate and ammonium sulfate.
The tests on the solutions and some of the observations are in the following table.
Complete the observations in the table.
tests
observations
tests on solution E
(a) Appearance of solution E.
................................................................ [1]
The solution was divided into three equal
portions in separate test-tubes.
(b) Dilute nitric acid and aqueous barium
nitrate were added to the first portion of the
solution.
................................................................ [1]
(c) (i) Excess aqueous sodium hydroxide
was added to the second portion of
the solution.
................................................................ [2]
(ii) The mixture was filtered and the filtrate
heated.
The gas given off was tested with
damp litmus paper.
(d) Dilute sulfuric acid and aqueous potassium
manganate(VII), an oxidising agent, were
added to the third portion of the solution.
Aqueous sodium hydroxide was then
added to the mixture.
......................................................................
................................................................ [2]
................................................................ [1]
tests on solution F
(e) Appearance of solution F.
(f)
yellow liquid
Zinc powder was added to solution F.
rapid effervescence
The solution was observed for five minutes.
turned blue, then green and finally light purple
The gas given off was tested with a splint.
lighted splint popped
© UCLES 2015
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11
(g) Identify the gas given off in test (f).
.............................................................................................................................................. [1]
(h) What conclusions can you draw about solution F?
....................................................................................................................................................
.............................................................................................................................................. [2]
[Total: 10]
© UCLES 2015
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6
Rhubarb Leaves
Ethanedioic acid dihydrate, H2C2O4.2H2O, is a white crystalline solid. This acid is water-soluble and
is found in rhubarb leaves.
Plan an investigation to obtain crystals of ethanedioic acid dihydrate from some rhubarb leaves.
You are provided with common laboratory apparatus, water and sand.
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
...........................................................................................................................................................
..................................................................................................................................................... [7]
[Total: 7]
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable
effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will
be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local
Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2015
0620/62/F/M/15
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education
*6533820761*
CHEMISTRY
0620/22
Paper 2
February/March 2015
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name in the spaces at the top of this page.
Write in dark blue or black pen.
You may use an HB pencil for any diagrams or graphs.
Do not use staples, paper clips, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
A copy of the Periodic Table is printed on page 16.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certificate.
This document consists of 14 printed pages and 2 blank pages.
IB15 03_0620_22/3RP
© UCLES 2015
[Turn over
2
1
The diagram shows the structures of some substances containing carbon.
A
B
C
Ca2+ CO32– Ca2+ CO32–
O
CO32– Ca2+ CO32– Ca2+
C
O
H
Ca2+ CO32– Ca2+ CO32–
H
H
C
C
H
H
H
CO32– Ca2+ CO32– Ca2+
D
E
F
Cl
H
H
C
C
C
C
H
Cl
H
H
H
Cl
Cl
Answer the following questions about these substances.
Each substance may be used once, more than once or not at all.
(a) Which substance, A, B, C, D, E or F
(i)
is a saturated hydrocarbon, ................................................................................................
(ii)
has an ionic structure, ........................................................................................................
(iii)
is a product of respiration, ..................................................................................................
(iv)
is in the same homologous series as methane, .................................................................
(v)
is used for cutting? .............................................................................................................
[5]
(b) Substance D is an element.
Explain why substance D is an element.
.............................................................................................................................................. [1]
[Total: 6]
© UCLES 2015
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3
2
Some properties of the halogens are shown in the table.
halogen
boiling point
/ °C
state at room temperature
and pressure
fluorine
–188
chlorine
–35
gas
bromine
+59
liquid
iodine
+184
solid
astatine
solid
(a) Use the information in the table to deduce
(i)
the boiling point of astatine,
....................................................................................................................................... [1]
(ii)
the state of fluorine at room temperature and pressure.
....................................................................................................................................... [1]
(b) When chlorine reacts with aqueous potassium iodide, the solution turns brown.
(i)
Write a word equation for this reaction.
....................................................................................................................................... [2]
(ii)
Explain why iodine does not react with aqueous potassium chloride.
.............................................................................................................................................
....................................................................................................................................... [1]
(c) When sodium reacts with iodine, energy is released.
(i)
What is the name given to a reaction which releases energy?
....................................................................................................................................... [1]
(ii)
Explain what happens in terms of electron transfer when a sodium atom reacts with an
iodine atom.
.............................................................................................................................................
....................................................................................................................................... [2]
[Total: 8]
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3
The diagram shows a limestone column in an industrial town. Limestone is largely calcium
carbonate.
iron pins
column when first built
the same column
after 40 years
(a) Describe and explain the changes to the column over 40 years.
In your answer refer to
•
•
•
the change to the limestone,
the name of a pollutant causing this change,
the chemistry involved in this change.
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [4]
(b) The sections of the column are joined with iron pins which rust when exposed to the atmosphere.
Describe two methods of rust prevention and explain how they prevent rusting.
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
© UCLES 2015
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5
(c) Iron is a transition element.
Give two properties of transition elements that make them different from non-transition metals
such as magnesium.
....................................................................................................................................................
.............................................................................................................................................. [2]
(d) An isotope of iron has 58 nucleons.
Complete the table to show
•
•
the number of electrons and neutrons in this isotope of iron,
the relative charges on each particle.
particle
number of each
particle present
relative charge
on the particle
electron
neutron
proton
no charge
26
[4]
(e) Iron reacts with hydrochloric acid to form iron(II) chloride and a gas which ‘pops’ with a lighted
splint.
Complete the symbol equation for this reaction.
Fe + ....... HCl → FeCl 2 + ............
[2]
[Total: 15]
© UCLES 2015
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4
Ammonium phosphate, (NH4)3PO4, is a fertiliser.
(a) Which two elements in ammonium phosphate are important for plant growth?
............................................................. and ......................................................................... [1]
(b) Aqueous ammonium phosphate can be made in the laboratory by reacting aqueous ammonia
with aqueous phosphoric acid.
aqueous
phosphoric acid
A
flask
aqueous
ammonia
(i)
State the name of the piece of apparatus labelled A.
....................................................................................................................................... [1]
(ii)
Suggest the pH value of aqueous phosphoric acid.
....................................................................................................................................... [1]
(iii)
Describe how the pH of the mixture in the flask changes as the acid is added.
....................................................................................................................................... [1]
(iv)
Which one of the following best describes the reaction of aqueous ammonia with aqueous
phosphoric acid?
Put a ring around the correct answer.
combustion
decomposition
neutralisation
reduction
[1]
(c) When sodium hydroxide is added to ammonium phosphate, ammonia is released.
Complete the symbol equation for this reaction.
(NH4)3PO4 + 3NaOH → Na3PO4 + .......NH3 + 3 ...............
[2]
[Total: 7]
© UCLES 2015
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7
5
The table shows the concentration of some ions present in a sample of seawater.
formula of ion
concentration
in g / dm3
bromide
Br –
0.06
calcium
Ca2+
0.30
chloride
Cl –
20.00
I–
0.04
magnesium
Mg2+
1.00
potassium
K+
0.50
sodium
Na+
11.00
sulfate
SO42–
0.80
name of ion
(a) (i)
Which positive ion in the table has the lowest concentration?
....................................................................................................................................... [1]
(ii)
Give the name of the ion with the formula I–.
....................................................................................................................................... [1]
(iii)
Which two ions in the table are formed from elements in Group II of the Periodic Table?
............................................................ and ................................................................... [1]
(iv)
Give the names of two ions in the table which move towards the anode (positive electrode)
when a sample of this seawater is electrolysed.
............................................................ and ................................................................... [2]
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8
(b) Sodium chloride can be extracted from seawater.
Concentrated aqueous sodium chloride is electrolysed using the apparatus shown.
battery
+
–
graphite
anode
graphite
cathode
concentrated aqueous
sodium chloride
(i)
Suggest why the anode and cathode are made of graphite.
....................................................................................................................................... [1]
(ii)
Give the name of the product formed at the cathode (negative electrode).
....................................................................................................................................... [1]
(iii)
Chlorine is formed at the anode.
Complete the electronic structure of a chlorine molecule. Show only the outer shell
electrons.
Cl
Cl
[2]
(c) Molten magnesium bromide is electrolysed.
Predict the products at the anode (positive electrode) and cathode (negative electrode).
anode .........................................................................................................................................
cathode ......................................................................................................................................
[2]
[Total: 11]
© UCLES 2015
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9
6
Zinc oxide is used for making baby soap and cream for treating sunburn.
(a) Suggest why the zinc oxide used for these purposes needs to be pure.
.............................................................................................................................................. [1]
(b) Zinc oxide can be reduced by carbon. Carbon monoxide is one of the products.
(i)
What is the meaning of the term reduction?
....................................................................................................................................... [1]
(ii)
Write a word equation for the reaction of zinc oxide with carbon.
....................................................................................................................................... [1]
(iii)
Explain why, in the laboratory, the reaction should be carried out in a fume cupboard.
....................................................................................................................................... [1]
(c) The table shows how easy it is to reduce various metal oxides by heating with carbon.
metal oxide
ease of reduction with carbon
lead oxide
easily reduced at 300 °C
magnesium oxide
not reduced at 900 °C
nickel oxide
easily reduced at 500 °C
zinc oxide
fairly easily reduced at 900 °C
Use the information in the table to put the metals in order of their reactivity.
least reactive
most reactive
[2]
(d) Zinc oxide reacts with sulfuric acid.
Complete the word equation for this reaction.
zinc oxide + sulfuric acid → zinc sulfate + ............................
[1]
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10
(e) Pure dry crystals of zinc sulfate can be made by the reaction of dilute sulfuric acid with excess
zinc.
(i)
How is excess zinc removed from the reaction mixture?
....................................................................................................................................... [1]
(ii)
Describe how you would obtain pure dry crystals of zinc sulfate from an aqueous solution
of zinc sulfate.
.............................................................................................................................................
.............................................................................................................................................
.............................................................................................................................................
....................................................................................................................................... [3]
(iii)
Zinc sulfate can be made from the reaction of sulfuric acid with zinc oxide or zinc.
Give the name of another compound that reacts with sulfuric acid to produce zinc sulfate.
....................................................................................................................................... [1]
(f) A student reacts zinc with excess sulfuric acid.
She obtains 16.1 g of zinc sulfate from 6.5 g of zinc.
(i)
Calculate the mass of zinc sulfate she would obtain from 26.0 g of zinc.
[1]
(ii)
Calculate the relative formula mass of zinc sulfate, ZnSO4.
[2]
[Total: 15]
© UCLES 2015
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11
7
Petroleum is separated into useful fractions by fractional distillation.
fractions
refinery gas
gasoline fraction
T
kerosene fraction
diesel oil
fuel oil
lubricating fraction
petroleum
bitumen
(a) (i)
(ii)
Put an X on the diagram to show where the temperature in the column is the highest. [1]
Give the name of the fraction labelled T.
....................................................................................................................................... [1]
(iii)
The lubricating fraction is used to make lubricants.
Give one other use of this fraction.
....................................................................................................................................... [1]
(b) Each fraction contains alkanes.
Which two of the following statements are correct?
Tick two boxes.
Alkanes burn to form carbon dioxide and hydrogen.
Ethene is an alkane with two carbon atoms.
Alkanes polymerise to form poly(alkanes).
Alkanes are generally unreactive apart from burning.
Methane is an alkane present in natural gas.
[2]
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12
(c) Hydrogen can be made by cracking.
(i)
What is meant by the term cracking?
.............................................................................................................................................
....................................................................................................................................... [2]
(ii)
Complete the equation for the cracking of propane.
C3H8 → ................ + H2
[1]
(d) Ethanol is formed by the catalytic addition of steam to ethene.
(i)
Complete the structures of ethene and ethanol in the equation below, showing all atoms
and bonds.
H
H
C
+
O
H
H
H
H
C
H
ethene
ethanol
[2]
(ii)
What does the symbol
mean?
....................................................................................................................................... [1]
[Total: 11]
© UCLES 2015
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8
A student placed a crystal of purple potassium manganate(VII) on a filter paper which had been
soaked in water.
After 5 minutes, a purple colour had spread out from the crystal.
After 30 minutes, the purple colour had spread further out.
crystal of
potassium
manganate(VII)
wet filter paper
at the start
after 5 minutes
after 30 minutes
(a) Use the kinetic particle theory to explain these observations.
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
....................................................................................................................................................
.............................................................................................................................................. [3]
(b) Describe the closeness and motion of the particles in a crystal of potassium manganate(VII).
closeness ...................................................................................................................................
motion ........................................................................................................................................
[2]
(c) Mixtures of dyes can be separated by paper chromatography using the apparatus shown
below.
base line
On the diagram above
•
•
draw a line to show the solvent level at the beginning of the experiment,
put a cross to show where the spot of dye mixture is placed at the beginning of the
experiment.
[2]
[Total: 7]
© UCLES 2015
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14
BLANK PAGE
© UCLES 2015
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15
BLANK PAGE
© UCLES 2015
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© UCLES 2015
Magnesium
Sodium
Calcium
0620/22/F/M/15
Strontium
89
Key
b
X
a
72
b = proton (atomic) number
X = atomic symbol
a = relative atomic mass
*58-71 Lanthanoid series
90-103 Actinoid series
88
Ac
Actinium
Ra
Radium
Fr
Francium
87
*
Hafnium
Lanthanum
57
178
Hf
40
Zirconium
Zr
91
Titanium
139
Yttrium
22
48
Ti
La
39
Y
89
Scandium
21
227
56
Barium
Caesium
45
Sc
226
55
137
Ba
133
Cs
38
Rubidium
37
88
Sr
85
Rb
20
Potassium
19
40
Ca
39
12
24
Mg
23
Na
Beryllium
4
Lithium
K
11
3
9
Be
7
II
Li
I
51
93
Ta
181
Niobium
Nb
90
58
73
52
96
Mo
W
184
Protactinium
Thorium
55
Tc
186
Re
144
Nd
92
60
Uranium
U
238
Neodymium
75
Rhenium
43
Technetium
25
Manganese
Mn
27
59
28
59
29
64
30
65
5
6
Ru
101
Iron
190
Pm
Osmium
Os
93
Np
Neptunium
61
Promethium
76
44
Ruthenium
26
56
Fe
Sm
150
Iridium
94
Pu
Plutonium
62
152
Eu
95
Am
Americium
63
Europium
78
Platinum
195
Pt
192
46
Palladium
Pd
106
Nickel
Ni
Ir
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
Gd
157
Gold
Au
197
Silver
96
64
Curium
Cm
Gadolinium
79
47
Ag
108
Copper
Cu
201
Bk
Terbium
Tb
159
Mercury
Hg
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
Dy
162
Thallium
Tl
204
Indium
98
Cf
Californium
66
Es
Holmium
Ho
165
Lead
Pb
207
Tin
99
Einsteinium
67
82
50
119
Sn
115
32
Germanium
Ge
73
Silicon
In
Gallium
Dysprosium
81
49
31
70
Ga
14
28
Si
Carbon
27
Aluminium
13
12
C
Al
Boron
B
11
7
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
14
8
Se
79
Sulfur
Po
169
Md
Thulium
Tm
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
S
32
Oxygen
O
16
9
Yb
173
Astatine
At
Iodine
I
127
Bromine
Br
80
Chlorine
No
102
Nobelium
70
Ytterbium
85
53
35
17
Cl
35.5
Fluorine
F
19
2
0
Lr
Lutetium
Lu
175
Radon
Rn
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
Helium
VII
Hydrogen
VI
4
V
He
IV
H
III
1
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
91
Pa
Th
232
Praseodymium
Cerium
59
141
Pr
140
74
Tungsten
42
Molybdenum
24
Chromium
Cr
Ce
Tantalum
41
23
Vanadium
V
1
Group
DATA SHEET
The Periodic Table of the Elements
16
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International
Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after
the live examination series.
Cambridge International Examinations
Cambridge International General Certificate of Secondary Education
0620/12
CHEMISTRY
Paper 1 Multiple Choice
February/March 2015
45 Minutes
Additional Materials:
*8505533334*
Multiple Choice Answer Sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
READ THESE INSTRUCTIONS FIRST
Write in soft pencil.
Do not use staples, paper clips, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.
There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
Read the instructions on the Answer Sheet very carefully.
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.
The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level1/Level 2 Certificate.
This document consists of 15 printed pages and 1 blank page.
IB15 03_0620_12/2RP
© UCLES 2015
[Turn over
2
1
A crystal of purple potassium manganate(VII) was added to each of the beakers shown in the
diagram.
hot water
cold water
crystal of potassium
manganate(VII)
One beaker contained hot water and the other beaker contained cold water.
In both beakers the purple colour of the potassium manganate(VII) spreads out.
Which result and explanation are correct?
2
result
explanation
A
colour spreads faster in cold water
particles move faster at a higher temperature
B
colour spreads faster in cold water
particles move slower at a higher temperature
C
colour spreads faster in hot water
particles move faster at a higher temperature
D
colour spreads faster in hot water
particles move slower at a higher temperature
During a reaction, the following changes take place.
1
The temperature rises.
2
A gas is given off.
Which apparatus is required to measure the rate of this reaction?
3
A
balance and burette
B
balance and gas syringe
C
gas syringe and burette
D
gas syringe and stopclock
Which statement about bonding is not correct?
A
Carbon can form four single covalent bonds.
B
Chlorine atoms react to gain a noble gas electronic structure.
C
Covalent bonding involves losing and gaining electrons.
D
Hydrogen molecules have the formula H2.
© UCLES 2015
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3
4
The table shows the numbers of particles present in the nuclei of four atoms or ions.
protons
neutrons
electronic structure
1
18
22
2,8,8
2
19
20
2,8,8
3
19
21
2,8,8,1
4
20
20
2,8,8,2
Which two particles belong to the same element?
A
5
6
B
1 and 2
C
1 and 4
D
2 and 3
2 and 4
Which substance is an ionic compound?
volatility
electrical conductivity
when molten
solubility in water
A
high
good
soluble
B
high
poor
insoluble
C
low
good
soluble
D
low
poor
insoluble
Covalent bonds are formed when electrons are ……1…… .
Most covalent compounds have ……2…… electrical conductivity.
Which words correctly complete gaps 1 and 2?
7
1
2
A
shared
high
B
shared
low
C
transferred
high
D
transferred
low
Which equation for the reaction between sodium carbonate and dilute hydrochloric acid is
correct?
A
Na2CO3(s) + HCl (aq) → NaCl (aq) + CO2(g) + H2O(I)
B
Na2CO3(s) + HCl (aq) → Na2Cl (aq) + CO2(g) + H2O(I)
C
Na2CO3(s) + 2HCl (aq) → NaCl (aq) + CO2(g) + H2O(I)
D
Na2CO3(s) + 2HCl (aq) → 2NaCl (aq) + CO2(g) + H2O(I)
© UCLES 2015
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4
8
The diagram shows an electrolysis experiment.
electrode Q
electrode P
X
During the electrolysis, sodium was formed at electrode P and chlorine at electrode Q.
Which row correctly identifies P, Q and X?
9
P
Q
X
A
anode
cathode
concentrated solution of
sodium chloride in water
B
anode
cathode
molten sodium chloride
C
cathode
anode
concentrated solution of
sodium chloride in water
D
cathode
anode
molten sodium chloride
The diagram shows apparatus for plating a spoon with silver.
spoon
metal electrode
electrolyte
Which statement is not correct?
A
Silver would stick to the spoon because it is a very reactive metal.
B
The electrolyte would be a silver salt dissolved in water.
C
The metal electrode would be made from silver.
D
The spoon would be connected to the negative terminal of the power supply.
© UCLES 2015
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5
10 Limestone can be changed into slaked lime in two chemical reactions.
1
When limestone, CaCO3, is heated it decomposes into lime, CaO.
2
Water is slowly dripped onto the cooled lime. The lime appears to expand and
steam is produced. Slaked lime, Ca(OH)2, is formed.
Which row shows the correct description of each of the chemical reactions?
reaction 1
reaction 2
A
endothermic
endothermic
B
endothermic
exothermic
C
exothermic
endothermic
D
exothermic
exothermic
11 A student investigates the rate of reaction between marble chips and hydrochloric acid.
The mass of the reaction flask is measured.
The graph shows the results of two experiments, P and Q.
mass of
reaction flask
P
Q
0
time
Which change explains the difference between P and Q?
A
A catalyst is added in P.
B
A higher temperature is used in P.
C
Bigger marble chips are used in Q.
D
Hydrochloric acid is more concentrated in Q.
© UCLES 2015
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6
12 Hydrated cobalt(II) chloride decomposes on heating.
The equation for the reaction is
CoCl 2.6H2O
CoCl 2 + 6H2O
The reaction is reversed by adding water.
Which row describes the colour change and the type of reaction for the reverse reaction?
colour change
type of reaction
A
blue to pink
endothermic
B
blue to pink
exothermic
C
pink to blue
endothermic
D
pink to blue
exothermic
13 When copper is heated in air a black coating forms on the copper.
What happens to the copper in this reaction?
A
The copper catches fire.
B
The copper decomposes.
C
The copper gains oxygen.
D
The copper loses oxygen.
14 Three chemicals, P, Q and R, were each dissolved in water. The table shows some of the
reactions of these solutions.
solution
reaction when solid sodium
carbonate is added
reaction when heated with
solid ammonium chloride
P
gas evolved
no reaction
Q
no reaction
gas evolved
R
no reaction
no reaction
The pH of the three solutions was also measured.
What are the correct pH values of these solutions?
P
Q
R
A
2
7
13
B
2
13
7
C
7
2
13
D
13
7
2
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15 The oxide of element X forms a solution with pH 4.
The oxide of element Y forms a solution that turns Universal Indicator blue.
Which row correctly classifies elements X and Y?
element X
element Y
A
metal
metal
B
metal
non-metal
C
non-metal
metal
D
non-metal
non-metal
16 Which two processes are involved in the preparation of magnesium sulfate from dilute sulfuric
acid and an excess of magnesium oxide?
A
neutralisation and filtration
B
neutralisation and oxidation
C
thermal decomposition and filtration
D
thermal decomposition and oxidation
17 Which statement about aqueous sodium hydroxide is correct?
A
When it is added to a solution containing sulfate ions, a white precipitate is formed.
B
When it is added to a solution of copper(II) ions, a blue precipitate is formed which dissolves
in excess to give deep blue solution.
C
When it is added to a solution of iron(II) ions, a green precipitate is formed which does not
dissolve in excess.
D
When it is added to ammonium chloride, a gas is produced which turns blue litmus red.
18 Which pair of elements will react together most violently?
A
chlorine and lithium
B
chlorine and potassium
C
iodine and lithium
D
iodine and potassium
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19 The table shows some information about elements in Group VII of the Periodic Table.
name
state at room
temperature
colour
chlorine
gas
yellow-green
bromine
liquid
brown
iodine
?
?
astatine
solid
black
Which information about iodine completes the table?
state
colour
A
liquid
black
B
liquid
green
C
solid
grey
D
solid
yellow
20 The diagram shows a section of the Periodic Table.
Which element is described below?
‘A colourless, unreactive gas that is denser than air.’
A
B
C
D
21 Which is not a characteristic property of transition metals?
A
act as catalysts
B
form coloured compounds
C
high melting point
D
low density
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22 Which statement is correct for all metals?
A
conduct electricity when molten
B
gain electrons when they form ions
C
have a low density
D
have a low melting point
23 Metal X lies between zinc and iron in the reactivity series.
Which statements about metal X are correct?
A
1
It reacts with steam to produce hydrogen gas.
2
It does not react with steam but will produce hydrogen with dilute acid.
3
The metal can be obtained from its oxide by heating strongly with charcoal.
4
The metal oxide cannot be reduced using carbon.
1 and 3
B
1 and 4
C
2 and 3
D
2 and 4
D
1, 2 and 3
24 Which of these gases is an atmospheric pollutant?
A
1
carbon monoxide
2
nitrogen dioxide
3
sulfur dioxide
1 only
B
2 only
C
3 only
25 Molten iron from the blast furnace contains impurities.
The process of turning the impure iron into steel involves blowing oxygen into the molten iron and
adding calcium oxide.
What are the reasons for blowing in oxygen and adding calcium oxide?
blowing in oxygen
adding calcium oxide
A
carbon is removed by reacting with oxygen
reacts with acidic impurities making slag
B
carbon is removed by reacting with oxygen
reacts with slag and so removes it
C
iron reacts with the oxygen
reacts with acidic impurities making slag
D
iron reacts with the oxygen
reacts with slag and so removes it
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26 Some properties of aluminium are listed.
1
It has mechanical strength.
2
It is resistant to corrosion.
3
It has a low density.
4
It conducts heat.
Which three properties make aluminium useful for making the bodies of aircraft?
A
1, 2 and 3
B
1, 2 and 4
C
1, 3 and 4
D
2, 3 and 4
27 The table describes three types of water.
water
type
source of
water
appearance before
treatment
treatment
appearance after
treatment
P
river
muddy
none
muddy
Q
river
muddy
filtration and chlorination
clear
R
well
clear
chlorination only
clear
Which statement is correct?
A
Only Q and R are suitable for drinking, while P could be used for irrigation.
B
Only Q and R are suitable for drinking, while P is unsuitable for any purpose.
C
Only Q is suitable for drinking. R could be used for washing cars and P for irrigation.
D
P, Q and R are suitable for irrigation and washing cars, but are not suitable for drinking.
28 A sample of air from a town centre was analysed and found to contain mainly nitrogen and
oxygen, but also traces of the four gases below.
Which of these gases is a pollutant?
A
argon
B
carbon dioxide
C
sulfur dioxide
D
water vapour
29 Which elements does an NPK fertiliser contain?
A
nickel, phosphorus, potassium
B
nickel, potassium, calcium
C
nitrogen, phosphorus, potassium
D
nitrogen, potassium, calcium
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30 The diagram shows experiments involving the rusting of iron.
tube P
tube Q
tube R
oil
iron nails
water
water boiled
to remove air
anhydrous calcium
chloride to dry the air
The following results were suggested.
1
In tube P, the iron nails rust.
2
In tube Q, the iron nails do not rust.
3
In tube R, the iron nails do not rust.
Which results are correct?
A
1 and 2 only
B
1 and 3 only
C
2 and 3 only
D
1, 2 and 3
31 Gas X is a waste gas from digestion in animals.
Gas Y is formed when gas X is burnt with a small amount of oxygen.
Gas Z is formed when gas X is burnt with an excess of oxygen.
What are X, Y and Z?
X
Y
Z
A
carbon dioxide
methane
carbon monoxide
B
carbon monoxide
methane
carbon dioxide
C
methane
carbon dioxide
carbon monoxide
D
methane
carbon monoxide
carbon dioxide
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32 The list gives four experiments carried out with calcium carbonate.
1
acid added
2
alkali added
3
heated strongly
4
water added
Which experiments produce carbon dioxide?
A
B
1 and 2
C
1 and 3
D
2 and 3
2 and 4
33 The diagram shows the soil pH range over which a vegetable grows well.
The pH of the soil to be used is 5.5.
5.0
6.0
7.0
8.0
pH
vegetable
grows well
Why is lime added to the soil before planting the vegetable?
A
The lime acts as a catalyst.
B
The lime changes the soil acidity.
C
The lime is an indicator.
D
The lime supplies nitrogen.
34 The diagram shows the structure of a compound.
H
H
H
H
C
C
C
C
H
H
H
Which functional groups does this molecule contain?
carboxylic
acid
alkene
alcohol
A
no
no
no
B
no
yes
yes
C
yes
no
yes
D
yes
yes
yes
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35 Petroleum is separated into useful fractions by fractional distillation.
Separation occurs in a fractionating column.
Some properties of three of these fractions are shown.
boiling point
range / °C
fraction
number of
carbon atoms in
the molecules
1
5–10
2
320–350
3
120–210
16–24
Which statement is correct?
A
Fraction 1 has a higher boiling point range than fraction 2.
B
Fraction 2 is removed from a higher point in the fractioning tower than fraction 1.
C
Molecules in fraction 3 have shorter chains than those in fraction 2.
D
None of the fractions is liquid at room temperature.
36 The structures of four molecules are shown.
1
H
2
H
H
H
C
C
C
H
H
OH
H
H
3
H
H
C
C
H
H
OH
H
4
H
H
C
C
H
H
H
H
H
C
C
H
H
Which molecules belong to the same homologous series?
A
1 and 2
B
1 and 3
C
2 and 4
D
3 and 4
37 Which statement about alkanes is correct?
A
Ethane has one more carbon atom and one more hydrogen atom than methane.
B
They are converted to alcohols by reaction with steam.
C
They contain carbon-carbon double bonds.
D
They form carbon dioxide and water on combustion.
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38 Which statement about alkenes is not correct?
A
They are hydrocarbons.
B
They are saturated.
C
They contain a C=C bond.
D
They form polymers.
39 Ethene reacts with Y to produce ethanol.
ethene + Y → ethanol
What is Y?
A
hydrogen
B
oxygen
C
steam
D
yeast
40 Which description of ethanoic acid is correct?
A
a clear, colourless and odourless liquid
B
a colourless liquid with a distinctive odour
C
a soft white solid with a distinctive odour
D
a transparent solid with a low melting point
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BLANK PAGE
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Magnesium
Sodium
Calcium
0620/12/F/M/15
Strontium
Key
b
X
a
b = proton (atomic) number
X = atomic symbol
a = relative atomic mass
*58-71 Lanthanoid series
90-103 Actinoid series
Actinium
Ac
89
Ra
Radium
88
Fr
Francium
87
*
Hafnium
72
Lanthanum
57
178
Hf
40
Zirconium
Zr
91
Titanium
139
Yttrium
22
48
Ti
La
39
Y
89
Scandium
21
227
Barium
56
Caesium
45
Sc
226
55
137
Ba
133
Cs
38
Rubidium
37
88
Sr
85
Rb
20
Potassium
19
40
Ca
39
12
24
Mg
23
Na
Beryllium
4
Lithium
K
11
3
9
Be
7
II
Li
I
93
Ta
181
Niobium
Nb
90
58
73
52
96
Mo
W
184
Protactinium
Thorium
55
Tc
186
Re
144
Nd
92
60
Uranium
U
238
Neodymium
75
Rhenium
43
Technetium
25
Manganese
Mn
27
59
28
59
29
64
30
65
5
6
Ru
101
Iron
190
Pm
Osmium
Os
Np
93
Neptunium
61
Promethium
76
44
Ruthenium
26
56
Fe
150
Sm
Pu
94
Plutonium
62
Eu
152
Platinum
Am
95
Americium
63
Europium
78
Pt
Iridium
195
192
46
Palladium
Pd
106
Nickel
Ni
Ir
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
Gd
157
Gold
Au
197
Silver
96
64
Curium
Cm
Gadolinium
79
47
Ag
108
Copper
Cu
201
Bk
Terbium
Tb
159
Mercury
Hg
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
Dy
162
Thallium
Tl
204
Indium
Cf
98
Californium
66
Es
Holmium
Ho
165
Lead
Pb
207
Tin
99
Einsteinium
67
82
50
119
Sn
115
32
Germanium
Ge
73
Silicon
In
Gallium
Dysprosium
81
49
31
70
Ga
14
28
Si
Carbon
27
Aluminium
13
12
C
Al
Boron
B
11
7
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
14
8
Se
79
Sulfur
Po
169
Md
Thulium
Tm
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
S
32
Oxygen
O
16
9
Yb
173
Astatine
At
Iodine
I
127
Bromine
Br
80
Chlorine
No
102
Nobelium
70
Ytterbium
85
53
35
17
Cl
35.5
Fluorine
F
19
2
0
Lr
Lutetium
Lu
175
Radon
Rn
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
Helium
VII
Hydrogen
VI
4
V
He
IV
H
III
1
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
91
Pa
Th
232
Praseodymium
Cerium
59
141
Pr
140
74
Tungsten
42
Molybdenum
24
Chromium
Cr
Ce
Tantalum
41
23
Vanadium
V
51
1
Group
DATA SHEET
The Periodic Table of the Elements
16
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at
www.cie.org.uk after the live examination series.