2
1
A mixture of sand and sodium chloride can be separated in three steps.
Step 1 is to add water to the mixture.
The diagram shows step 2 and step 3.
Where is pure sodium chloride collected?
A
filter paper
and funnel
B
evaporating
dish
D
C
heat
step 2
2
step 3
The results of two tests on solution X are shown.
reagent added
observation on adding
a few drops of reagent
observation on adding
an excess of reagent
aqueous sodium hydroxide
white precipitate
precipitate dissolves
aqueous ammonia
white precipitate
precipitate remains
Which ion is present in solution X?
A
3
Al 3+
B
Ca2+
C
Cu2+
D
Zn2+
Which diagram shows the arrangement of particles inside a balloon containing a mixture of the
gases nitrogen and oxygen?
A
B
C
D
key
nitrogen atom
oxygen atom
3
4
A student follows the rate of the reaction between marble chips, CaCO3, and dilute
hydrochloric acid.
CaCO3 + 2HCl → CaCl 2 + CO2 + H2O
Which diagrams show apparatus that is suitable for this experiment?
1
2
measuring
cylinder
hydrochloric
acid
loose
plug
marble chips
hydrochloric
acid
balance
water
marble chips
3
4
hydrochloric
acid
hydrochloric
acid
burette
burette
gas syringe
marble chips
marble chips
A
1 and 2 only
B
1 and 3
C
1 and 4 only
D
1, 2 and 4
4
5
A chemist wishes to separate and identify a mixture of substances using paper chromatography.
The diagram shows the apparatus used. The solvent is water.
solvent
The solvent front is allowed to reach the top of the paper before the chemist removes the paper
from the solvent.
Which problem does this cause?
6
A
This causes the spot nearest the bottom of the paper to catch up with the spot above it.
B
This makes it impossible to calculate Rf values.
C
This makes it impossible to use a locating agent.
D
This results in a safety hazard caused by solvent fumes.
Which particle contains the same number of both neutrons and electrons?
A
7
40
2+
20 Ca
B
2+
24
12 Mg
C
19 −
9F
D
Which statement is correct for all metals?
A
They are hard and brittle.
B
They are made up of a lattice of positive and negative ions.
C
They conduct electricity by movement of electrons.
D
They conduct electricity by movement of ions.
32 2 −
16 S
5
8
X represents the element of atomic number 8 and Y represents the element of atomic number 19.
The two elements react together to form a compound.
Which row is correct for the compound formed?
9
formula
type of bonding
A
Y2X
covalent
B
Y2X
ionic
C
X2Y
covalent
D
X2Y
ionic
The empirical formula of a liquid compound is C2H4O.
To find the empirical formula, it is necessary to know
A
the density of the compound.
B
the percentage composition by mass of the compound.
C
the relative molecular mass of the compound.
D
the volume occupied by 1 mole of the compound.
10 25.0 g of hydrated copper(II) sulfate crystals are heated to produce anhydrous copper(II) sulfate
and water vapour.
CuSO4.5H2O(s) → CuSO4(s) + 5H2O(g)
What is the mass of anhydrous copper(II) sulfate formed?
[Mr: CuSO4, 160; H2O, 18]
A
9.0 g
B
16.0 g
C
22.5 g
D
25.0 g
71 g
D
142 g
11 Which sample contains the most atoms?
A
0.5 moles of water
B
1.0 moles of carbon dioxide
C
1.0 moles of methane
D
2.0 moles of hydrogen chloride
12 The relative atomic mass of chlorine is 35.5.
What is the mass of 2 moles of chlorine gas?
A
17.75 g
B
35.5 g
C
6
13 One mole of an organic compound, Q, is completely burnt in oxygen and produces exactly three
moles of water.
Which compound is Q?
A
butane, C4H10
B
ethanol, C2H5OH
C
propane, C3H8
D
propanol, C3H7OH
14 In an experiment, 1 mol of powdered copper and 1 mol of powdered zinc are placed in a flask.
Dilute acid, containing 1 mol of acid, is added to the flask.
The flask is left until all the reactions, if any, are complete.
Which diagram shows the result of the experiment?
A
B
colourless
neutral
solution
blue
neutral
solution
1 mol of copper
C
0.5 mol of copper +
0.5 mol of zinc
D
blue
neutral
solution
1 mol of zinc
colourless
acidic
solution
1 mol of copper +
1 mol of zinc
7
15 A simple cell can be made using two different metals as the electrodes and an aqueous solution
as the electrolyte.
Which statements about simple cells are correct?
A
1
A greater voltage is produced using magnesium and silver than using magnesium
and copper.
2
The electrolyte is an aqueous solution containing both positive and negative ions.
3
The more reactive metal will release electrons.
1, 2 and 3
B
1 and 3 only
C
1 only
D
2 and 3 only
16 Magnesium can be produced by electrolysis of molten magnesium chloride, MgCl 2.
What are the equations for the reactions that occur at the positive electrode and at the negative
electrode?
positive electrode
negative electrode
A
2Cl – → Cl 2 + 2e–
2H+ + 2e– → H2
B
Cl 2 + 2e– → 2Cl –
Mg2+ + 2e– → Mg
C
2Cl – → Cl 2 + 2e–
Mg2+ + 2e– → Mg
D
2Cl – → Cl 2 + 2e–
Mg2+ + 2e– → 2Mg
17 Three different solutions were electrolysed using inert electrodes.
solution 1
aqueous sodium chloride
solution 2
concentrated hydrochloric acid
solution 3
dilute sulfuric acid
Which solutions produce hydrogen at the negative electrode?
A
1, 2 and 3
B
1 and 2 only
C
1 only
D
2 and 3 only
18 Compound Y reacts with oxygen. This reaction has a positive enthalpy change of reaction, ∆H.
What information can be deduced about Y and its reaction with oxygen?
A
Compound Y can be used as a fuel.
B
Compound Y could be a hydrocarbon.
C
In the reaction the energy needed to break bonds is greater than the energy released when
bonds are made.
D
In the reaction the products are at a lower energy level than the reactants.
8
19 The formation of liquid water from hydrogen and oxygen may occur in three stages.
1
2H2(g) + O2(g) → 4H(g) + 2O(g)
2
4H(g) + 2O(g) → 2H2O(g)
3
2H2O(g) → 2H2O(I)
Which stages are endothermic?
A
1, 2 and 3
B
1 only
C
2 only
D
3 only
20 Which statement is correct for both aluminium and iron?
A
Both form 2+ ions.
B
Both have amphoteric oxides.
C
The manufacture of both metals involves the reduction of the metal ions.
D
They are both normally manufactured by electrolysis.
21 A household cleaning compound is used to remove calcium carbonate from bathroom surfaces.
The compound reacts with the calcium carbonate to form a soluble salt, carbon dioxide and
water.
What is the pH of this cleaning compound?
A
pH 2
B
pH 7
C
pH 10
D
pH 14
22 Dilute hydrochloric acid is added separately to samples of copper, copper(II) oxide and
copper(II) carbonate.
Which row correctly shows whether copper(II) chloride is produced?
Cu
CuO
CuCO3
A
key
B
= copper(II) chloride produced
C
= copper(II) chloride not produced
D
23 Which ions are present when hydrochloric acid has exactly neutralised aqueous sodium
hydroxide?
A
Na+, Cl –, H+ and OH–
B
Na+, Cl – and H+ only
C
Na+ and Cl – only
D
H+ and OH– only
24 Which experiment will result in the formation of a white precipitate?
A
aqueous barium nitrate added to aqueous sodium chloride
B
aqueous sodium carbonate added to aqueous calcium chloride
C
carbon dioxide passed through aqueous potassium chloride
D
dilute hydrochloric acid added to aqueous ammonia
25 Which statement about both the Group I and Group VII elements is correct?
A
They conduct electricity when molten.
B
They form covalent compounds when bonded to non-metals.
C
They exist as diatomic molecules.
D
When Group I elements combine with Group VII elements, ionic compounds form.
26 The elements helium, argon and neon are noble gases.
Which statement is correct?
A
All these elements have eight electrons in their outer shell.
B
Argon is used to react with impurities in the manufacture of steel.
C
Helium is used in balloons as it is more dense than air.
D
Neon is used in light bulbs to give an inert atmosphere.
27 The diagram shows four pieces of apparatus that are used to measure the volume of a gas or
liquid.
Which piece of apparatus should always be filled to the same level?
A
B
C
D
burette
gas syringe
measuring cylinder
pipette
28 Aqueous sodium thiosulfate reacts with acid to make a precipitate of sulfur.
Na2S2O3(aq) + 2HCl (aq) → 2NaCl (aq) + H2O(l) + SO2(g) + S(s)
A student investigates the effect of temperature on the rate of this reaction.
The student:
●
places a piece of paper with a cross on it below the reaction mixture as shown in the
diagram
●
measures the time taken for the cross to no longer be seen
●
repeats the reaction at different temperatures.
paper with cross
50 cm3 aqueous
sodium thiosulfate
+ acid
Which apparatus is needed for this investigation?
A
balance, pipette, stop-clock
B
balance, stop-clock, thermometer
C
burette, gas syringe, thermometer
D
measuring cylinder, stop-clock, thermometer
[Turn over
29 A paper chromatography experiment is carried out to find an
shown.
Rf value for Fe3+(aq). The result is
solvent front
Fe3+
y
x
starting line
To make the spot containing Fe3+(aq) more visible, the paper is sprayed with aqueous sodium
hydroxide so that a precipitate of iron(III) hydroxide forms.
Under the conditions of the experiment, the Rf of Fe3+(aq) is given by ......1...... and the colour of
the precipitate is ......2...... .
Which row correctly completes gaps 1 and 2?
gap 1
gap 2
A
x
y
red-brown
B
x
y
green
C
D
y
x
y
x
red-brown
green
5
30 The diagram shows two experiments.
experiment 1
add a few drops
add an excess
of NaOH(aq)
of NaOH(aq)
Al 3+(aq)
no precipitate
experiment 2
precipitate formed
add a few drops
add an excess
of NaOH(aq)
of NaOH(aq)
Cu2+(aq)
?
no precipitate
?
precipitate formed
What are the results of adding an excess of NaOH(aq) in each experiment?
experiment 1
experiment 2
A
key
B
= precipitate remains
C
= precipitate dissolves
D
31 Which methods of separation require a change of state from liquid to gas?
A
1
paper chromatography
2
crystallisation
3
distillation
4
filtration
1 and 2
B
1 and 3
C
2 and 3
D
3 and 4
[Turn over
6
32 Hydrogen sulfide, H2S, and hydrogen chloride, HCl, are both gases at temperatures above
–50 °C.
Which gas will diffuse most rapidly at the temperature given?
A
hydrogen chloride at –40 °C
B
hydrogen chloride at –20 °C
C
hydrogen sulfide at –40 °C
D
hydrogen sulfide at –20 °C
33 The diagram shows the relative mass and the relative charge of two particles,
atoms and ions.
2000
relative
mass
1
–1
0
relative charge
Which of these particles are present in a hydrogen atom and in a hydrogen ion?
H+
H
A
both
and
B
both
and
C
but not
D
but not
both
and
but not
neither
nor
but not
34 Which ion has the most shells that contain electrons?
A
Al 3+
B
Be2+
C
N3–
D
S2–
35 Which substance conducts electricity both when solid and when molten?
A
an alloy
B
a hydrocarbon
C
a metal oxide
D
a salt
and
, present in
7
35 When they react together, which pair of elements form an ionic compound?
A
carbon and hydrogen
B
hydrogen and chlorine
C
lithium and oxygen
D
sulfur and oxygen
36 How many shared electrons are in one carbon dioxide molecule?
A
2
B
4
C
8
D
12
37 Element X has a lattice of positive ions and a ‘sea of electrons’.
e–
e–
e–
e–
e–
e
e–
e–
e
–
–
e–
e–
e–
e–
e–
e–
Which property will X have?
A
It conducts electricity by the movement of ions and electrons.
B
It has a high melting point.
C
It is decomposed by an electric current.
D
It is not malleable.
39 Which row shows the correct state symbols for the reaction between calcium carbonate and
dilute hydrochloric acid? (The conditions are room temperature and pressure.)
CaCO3 +
2HCl → CaCl 2 +
H2O
+
CO2
A
s
aq
aq
aq
g
B
s
l
aq
l
g
C
s
l
l
aq
g
D
s
aq
aq
l
g
[Turn over
8
40 The expression shown for the value of Ar for fluorine is incomplete.
Ar (fluorine) =
average mass of one ......1...... of fluorine
......2...... of the mass of one atom of
How should the gaps in the expression be correctly completed?
gap 1
gap 2
A
atom
1
6
B
atom
1
12
C
molecule
1
6
D
molecule
1
12
12
6C
EXTRA QUESTIONS
41 The chloride of metal X is dissolved in water.
A concentrated solution of this chloride is electrolysed using inert electrodes.
inert anode
inert cathode
concentrated aqueous solution
of chloride of metal X
X is above sodium in the reactivity series.
In addition to chlorine, which gas is liberated and at which electrode?
gas
liberated at
electrode
A
hydrogen
anode
B
hydrogen
cathode
C
oxygen
anode
D
oxygen
cathode
42 Many reactions can be classified as redox reactions.
Which equations show redox reactions?
A
1
Mg + 2HCl → MgCl 2 + H2
2
2FeCl 2 + Cl 2 → 2FeCl 3
3
2Na + Br2 → 2NaBr
1, 2 and 3
B
1 and 2 only
C
2 and 3 only
D
3 only
43 Which aqueous reagent liberates ammonia from ammonium nitrate on warming?
A
calcium nitrate
B
potassium hydroxide
C
sodium chloride
D
sulfuric acid
39
Y
Mg
magnesium
24
20
Ca
calcium
40
38
Na
sodium
23
19
K
potassium
39
37
73
Ta
72
Hf
89
57–71
lanthanoids
88
56
Rf
Th
thorium
232
–
90
89
Ac
140
139
actinium
Ce
cerium
La
lanthanum
58
57
–
rutherfordium
231
protactinium
Pa
91
141
praseodymium
Pr
59
–
dubnium
Db
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
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
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
23
Rb
40
48
titanium
Ti
22
relative atomic mass
rubidium
45
scandium
Sc
12
11
21
9
7
name
atomic symbol
Be
beryllium
Li
lithium
atomic number
4
3
Key
II
I
The Periodic Table of Elements