Centre Number
Candidate
Number
Candidate Name
UNIVERSITY OF CAMBRIDGE LOCAL EXAMINATIONS SYNDICATE
General Certificate of Education Ordinary Level
COMBINED SCIENCE
5129/2
PAPER 2
OCTOBER/NOVEMBER SESSION 2001
2 hours 15 minutes
Candidates answer on the question paper.
No additional materials are required.
TIME
2 hours 15 minutes
INSTRUCTIONS TO CANDIDATES
Write your name, Centre number and candidate number in the spaces at the top of this page.
Answer all questions.
Write your answers in the spaces provided on the question paper.
INFORMATION FOR CANDIDATES
The number of marks is given in brackets [ ] at the end of each question or part question.
A copy of the Periodic Table is printed on page 16.
FOR EXAMINER’S USE
TOTAL
This question paper consists of 14 printed pages and 2 blank pages.
SB (SLC/SLC) QK11417/2
© UCLES 2001
http://www.xtremepapers.net
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Examiner’s
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2
1
(a) Complete the table in Fig. 1.1.
nucleon
number
chlorine atom
35
magnesium atom
24
sodium ion
23
proton
number
protons
neutrons
electrons
17
12
12
Fig. 1.1
[4]
(b) (i)
What is the formula of the compound formed between magnesium and chlorine?
...............................................................................................................................[1]
(ii)
2
What type of bonding occurs in this compound? ..................................................[1]
The following is a list of gases.
acetylene
ethene
carbon dioxide
nitrogen
oxygen
carbon monoxide
sulphur dioxide
Use the list to complete the following sentences.
(a) The gas that undergoes polymerisation is ........................................................ .
[1]
(b) The gases that are used in welding are ........................................................
and ........................................................ .
[2]
(c) The gas that is a pollutant in the air and damages buildings is
........................................................ .
[1]
(d) The gas that is produced by incomplete combustion of petrol is
........................................................ .
[1]
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3
3
Ammonia is manufactured according to the following equation.
N2 + 3H2 → 2NH3
(a) (i)
Calculate the relative molecular mass, Mr, of nitrogen and of ammonia.
[Ar : H, 1; N, 14]
Mr of nitrogen ............................................................................................................
Mr of ammonia ......................................................................................................[2]
(ii)
Calculate the mass of nitrogen required to manufacture 8.5 kg of ammonia.
Show your working.
...................................................................................................................................
...................................................................................................................................
...............................................................................................................................[3]
(b) Ammonia is used to manufacture ammonium sulphate.
Explain why ammonium sulphate is used as a fertiliser.
..........................................................................................................................................
......................................................................................................................................[1]
4
Carbon is an element. Methane is a compound.
(a) Explain the difference between an element and a compound using carbon and methane
as examples.
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
......................................................................................................................................[3]
(b) Name the homologous series to which methane belongs.
......................................................................................................................................[1]
(c) Draw the structure of methane.
[1]
5129/2/O/N/01
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4
5
Study the following reaction scheme.
metal A
water
sodium hydroxide
hydrochloric acid
salt C + water
+
gas B
warm with ammonium chloride
sodium chloride + gas D + water
(a) Identify substances A, B, C and D.
metal A .......................................................
gas B
.......................................................
salt C
.......................................................
gas D
.......................................................
(b) (i)
[4]
What type of reaction occurs between sodium hydroxide and hydrochloric acid?
...............................................................................................................................[1]
(ii)
Construct an equation for this reaction.
...............................................................................................................................[1]
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5
6
Fig. 6.1 describes some properties of five substances.
substance
conducts
electricity
when solid
conducts
electricity
when melted
melting
point
/ °C
soluble in
water
A
no
no
–114
yes
B
yes
yes
961
no
C
no
yes
714
yes
D
no
no
114
no
E
yes
yes
1917
no
Fig. 6.1
(a) (i)
(ii)
Give the letter of one metal in the table. ...............................................................[1]
Give two reasons for your choice.
...................................................................................................................................
...................................................................................................................................
...............................................................................................................................[2]
(b) (i)
Give the letter of one covalent compound in the table.
...............................................................................................................................[1]
(ii)
Give two reasons for your choice.
...................................................................................................................................
...................................................................................................................................
...............................................................................................................................[2]
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6
7
Fig. 7.1 shows a lighting circuit.
switch A
live
switch B
switch C
lamp P
lamp Q
230
volts
neutral
Fig. 7.1
(a) Which switches must be closed to light lamp Q only? .................................................[1]
(b) Draw a fuse in the correct position in the circuit to protect all the wiring.
[2]
(c) Explain how a fuse makes the circuit safer.
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
......................................................................................................................................[3]
(d) Each lamp in the circuit has a resistance of 920 Ω. The potential difference across the
circuit is 230 V.
Calculate the current through switch A when all the switches are closed.
.................................................[3]
(e) What energy changes take place inside the lamp?
......................................................................................................................................[2]
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7
8
Fig. 8.1 shows the electromagnetic spectrum.
radio
microwaves
infra-red
visible light
ultraviolet
S
gamma-rays
Fig. 8.1
(a) Which part of the spectrum has the lowest frequency? ...............................................[1]
(b) Name part S. ................................................................................................................[1]
(c) State two properties of all types of radiation in the spectrum.
1. ......................................................................................................................................
2. ..................................................................................................................................[2]
(d) Yellow light from the Sun has a wavelength of 5.0 x 10–7 m and travels at a speed of
3 x 108 m / s. The light takes 500 s to reach the Earth.
Calculate
(i)
the distance between the Earth and the Sun;
.................................................[2]
(ii)
the frequency of the yellow light.
.................................................[2]
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8
9
Radium, Ra, emits alpha-particles and decays to radon, Rn.
226 Ra
88
→
XRn
Y
+
4He
2
(a) Deduce
(i)
the value X, ...........................................................................................................[1]
(ii)
the value Y, ...........................................................................................................[1]
(iii)
the number of neutrons in the radium nucleus. ....................................................[1]
(b) Radium has a half-life of 1600 years. 4800 years ago, a sample of radium emitted
alpha-particles at a rate of 24 000 per second.
At what rate does this sample emit alpha-particles now?
[3]
(c) In paper mills, the thickness of the paper is controlled by measuring how many
beta-particles pass through the paper each second.
(i)
Name a suitable detector for beta-particles. .........................................................[1]
(ii)
Explain why alpha-particles are not used.
...............................................................................................................................[1]
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9
10 (a) A magnet is placed near two pieces of iron, as shown in Fig. 10.1.
N
iron
S
magnet
iron
Fig. 10.1
The pieces of iron become magnetised.
On the diagram, mark the north and south poles of both pieces of iron.
[2]
(b) Electromagnets are often used instead of permanent magnets.
State one advantage of an electromagnet that a permanent magnet does not have.
..........................................................................................................................................
......................................................................................................................................[1]
(c) Why is the core of an electromagnet made of iron rather than steel?
..........................................................................................................................................
......................................................................................................................................[1]
(d) State two ways in which the strength of an electromagnet can be increased.
1. ......................................................................................................................................
2. ..................................................................................................................................[2]
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10
11 In a fermentation experiment, water is boiled for 30 minutes, cooled and mixed with yeast
and glucose. The mixture is left as shown in Fig. 11.1, for two hours.
mixture
of yeast
and
glucose
in boiled
water
tube
A
tube
B
limewater
Fig. 11.1
(a) (i)
Which type of respiration takes place?
...............................................................................................................................[1]
(ii)
What change is seen in tube B?
...............................................................................................................................[1]
(iii)
Write a word equation for this respiration reaction.
...............................................................................................................................[1]
(iv)
What is the advantage, to the yeast, of this reaction?
...............................................................................................................................[1]
(b) The type of respiration you have named in (a)(i) can take place in human muscle.
(i)
Name the product formed.
...............................................................................................................................[1]
(ii)
What type of activity can cause this product to form?
...............................................................................................................................[1]
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For
Examiner’s
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11
12 Fig. 12.1 shows an ecosystem diagram.
(a) Draw no more than five arrows to show the direction of the flow of energy in the
ecosystem.
snail
songbird
grass
Sun
rabbit
hawk
[4]
Fig. 12.1
(b) There are no decomposers shown in this ecosystem.
(i)
Name a group of organisms that are decomposers.
...............................................................................................................................[1]
(ii)
Explain the function of decomposers in an ecosystem.
...................................................................................................................................
...................................................................................................................................
...............................................................................................................................[2]
(c) Explain why green plants are called producers, but animals are called consumers.
..........................................................................................................................................
..........................................................................................................................................
..........................................................................................................................................
......................................................................................................................................[3]
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12
13 (a) (i)
Define excretion.
...................................................................................................................................
...................................................................................................................................
...............................................................................................................................[2]
(ii)
Name two substances which are excreted by a human.
1. ...............................................................................................................................
2. ...........................................................................................................................[2]
(iii)
For each substance named in (ii), state where it is produced and name the organ
which excretes it.
1
where produced .................................................................................................
excreted by ........................................................................................................
2
where produced .................................................................................................
excreted by ....................................................................................................[4]
(b) (i)
What is meant by egestion (defaecation)?
...................................................................................................................................
...............................................................................................................................[1]
(ii)
Suggest reasons why egestion should not be considered an example of excretion.
...................................................................................................................................
...............................................................................................................................[1]
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13
14 (a) Define osmosis.
..........................................................................................................................................
..........................................................................................................................................
......................................................................................................................................[2]
(b) Fig. 14.1 shows a plant cell into which water passes by osmosis.
Fig. 14.1
(i)
What is the name for this type of cell?
...............................................................................................................................[1]
(ii)
Which is the more concentrated solution, the plant cell sap or the water in the soil?
...............................................................................................................................[1]
(c) Plant roots absorb ions from the soil.
Name one ion which is absorbed by plants.
......................................................................................................................................[1]
(d) Water absorbed by the roots passes upwards through the plant to the leaves.
(i)
Through which structures is the water lost from the leaves to the air?
...............................................................................................................................[1]
(ii)
Name this process.
...............................................................................................................................[1]
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14
BLANK PAGE
5129/2/O/N/01
15
BLANK PAGE
5129/2/O/N/01
Magnesium
Sodium
Calcium
5129/2/O/N/01
Strontium
45
89
Key
b
X
a
*
89
227
Actinium
Ac
b = proton (atomic) number
X = atomic symbol
a = relative atomic mass
†
72
Hafnium
Lanthanum
57
178
Hf
40
Zirconium
Zr
91
Titanium
139
Yttrium
Y
22
48
Ti
La
39
21
Scandium
Sc
*58-71 Lanthanoid series
†90-103 Actinoid series
88
Radium
87
Francium
226
Ra
56
Barium
Caesium
Fr
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
150
Sm
Pu
94
Plutonium
62
152
Eu
Am
95
Americium
63
Europium
78
Platinum
Pt
Iridium
195
Ir
46
Palladium
Pd
106
Nickel
Ni
192
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
Sulphur
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