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s er UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
International General Certificate of Secondary Education

0620/12

CHEMISTRY
Paper 1 Multiple Choice

May/June 2010
45 Minutes

Additional Materials:

*8778752636*

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, highlighters, 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.
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.
You may use a calculator.

This document consists of 15 printed pages and 1 blank page.
IB10 06_0620_12/RP
© UCLES 2010

[Turn over

2
1

The diagram shows a cup of tea.

Which row describes the water particles in the air above the cup compared with the water particles in the cup? moving faster
A





B





C





D
2

closer together





Which row shows the change that takes place when element X gains the new particle shown? particle gained

change

A

an isotope of element X is formed

B

electron

the element one place to the right of X in the Periodic Table is formed

C

proton

an isotope of element X is formed

D
3

electron

proton

the element one place to the right of X in the Periodic Table is formed

The symbols of two atoms may be written as shown.
52
23

X

52
24 Y

Which statement about these atoms is correct?
A

They are different elements because they have different numbers of neutrons.

B

They are different elements because they have different numbers of protons.

C

They are isotopes of the same element because they have the same nucleon number.

D

They are isotopes of the same element because they have the same proton number.

© UCLES 2010

0620/12/M/J/10

3
4

The diagram shows an atom. e e

key e electron nucleus containing nine particles

e e

What is the proton number and neutron number of the atom? proton number
A

4

5

B

4

9

C

5

4

D
5

neutron number 5

9

A fruit drink coloured orange contains a dissolved mixture of red and yellow colouring agents.
One of these colouring agents is suspected of being illegal.
Which method could be used to show the presence of this illegal colouring agent?
A
B

distillation

C

evaporation

D
6

chromatography

filtration

A student carries out an experiment to find how fast 3 cm pieces of magnesium ribbon dissolve in
10 cm3 samples of sulfuric acid at different temperatures.
Which piece of apparatus does the student not need?
A

balance

B

measuring cylinder

C

stop-clock

D

thermometer

© UCLES 2010

0620/12/M/J/10

[Turn over

4
7

Three electrolysis cells are set up. Each cell has inert electrodes.
The electrolytes are listed below. cell 1

aqueous sodium chloride

cell 2

concentrated hydrochloric acid

cell 3

molten lead(II) bromide

In which cells is a gas formed at both electrodes?
A
8

1 and 2

B

1 and 3

C

D

2 only

3 only

The diagram shows apparatus for plating a spoon with silver.

spoon

metal electrode

electrolyte

Which statement is not correct?
A
B

The electrolyte would be a silver salt dissolved in water.

C

The metal electrode would be made from silver.

D
9

Silver would stick to the spoon because it is a very reactive metal.

The spoon would be connected to the negative of the power supply.

Aqueous copper(II) sulfate solution is electrolysed using inert electrodes.
Copper(II) ions (Cu2+), hydrogen ions (H+), hydroxide ions (OH–) and sulfate ions ( SO 42 − ) are present in the solution.
To which electrodes are the ions attracted during this electrolysis? attracted to anode

attracted to cathode

A

Cu2+ and H+

OH– and SO 4 2 −

B

Cu2+ and SO 42 −

H+ and OH–

C

H+ and OH–

Cu2+ and SO 42 −

D

OH– and SO 42 −

Cu2+ and H+

© UCLES 2010

0620/12/M/J/10

5
10 In which compounds are pairs of electrons shared between atoms?
1
2

methane

3
A

sodium chloride

lead bromide

1 only

B

C

2 only

1 and 3

D

1, 2 and 3

11 Element X has six electrons in its outer shell. e e

key e = electron

e e e e

How could the element react?
A

by gaining two electrons to form a positive ion

B

by losing six electrons to form a negative ion

C

by sharing two electrons with two electrons from another element to form two covalent bonds

D

by sharing two electrons with two electrons from another element to form four covalent bonds

12 Hydrogen and chlorine react as shown.
1 molecule of hydrogen

+

1 molecule
2 molecules

of chlorine of hydrogen chloride

What is the equation for this reaction?
A

2H + 2Cl → 2HCl

B

2H + 2Cl → H2Cl 2

C

H2 + Cl 2 → 2HCl

D

H2 + Cl 2 → H2Cl 2

13 Which name is given to mixtures of metals?
A

alloys

B

compounds

C

ores

D

salts

© UCLES 2010

0620/12/M/J/10

[Turn over

6
14 Iron is extracted from iron oxide using carbon monoxide as shown in the equation. iron oxide + carbon monoxide → iron + carbon dioxide
What does the equation show?
A

Carbon monoxide is oxidised to carbon dioxide.

B

Carbon monoxide is reduced to carbon dioxide.

C

Iron is oxidised to iron oxide.

D

Iron oxide is oxidised to iron.

15 A student investigates the rate of reaction between marble chips and hydrochloric acid.
The loss in 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 2010

0620/12/M/J/10

7
16 Clouds are formed when water vapour evaporates from the sea.

clouds

water vapour

sea

What is the energy change and what name is given to the type of change when water evaporates? energy change

type of change

A

energy given out

endothermic

B

energy given out

exothermic

C

energy taken in

endothermic

D

energy taken in

exothermic

17 Which process is not exothermic?
A

burning a fossil fuel

B

obtaining lime from limestone

C

radioactive decay of 235U

D

reacting hydrogen with oxygen

18 When pink cobalt(II) sulfate crystals are heated, they form steam and a blue solid.
When water is added to the blue solid, it turns pink and becomes hot.
Which terms describe the pink cobalt(II) sulfate crystals and the reactions? pink cobalt sulfate

reactions

A

aqueous

irreversible

B

aqueous

reversible

C

hydrated

irreversible

D

hydrated

reversible

© UCLES 2010

0620/12/M/J/10

[Turn over

8
19 An element melts at 1455 °C, has a density of 8.90 g / cm3 and forms a green chloride.
Where in the Periodic Table is this element found?
A
B

C
D

20 An excess of copper(II) oxide is added to dilute sulfuric acid to make crystals of hydrated copper(II) sulfate.
The processes listed may be used to obtain crystals of hydrated copper(II) sulfate.
1

concentrate the resulting solution

2

filter

3

heat the crystals

4

wash the crystals

Which processes are needed and in which order?
A

1, 2, 3 and 4

B

1, 2, 4 and 3

C

2, 1, 2 and 3

D

2, 1, 2 and 4

21 Which is not a property of Group I metals?
A

They are soft and can be cut with a knife.

B

They corrode rapidly when exposed to oxygen in the air.

C

They produce an acidic solution when they react with water.

D

They react rapidly with water producing hydrogen gas.

© UCLES 2010

0620/12/M/J/10

9
22 Aqueous sodium hydroxide is added to a solid, X, and the mixture is heated.
A green precipitate is formed and an alkaline gas is given off.
Which ions are present in X?
A

NH4+ and Fe2+

B

NH4+ and Fe3+

C

OH– and Fe2+

D

OH– and Fe3+

23 An aqueous solution of the organic compound methylamine has a pH greater than 7.
Which statement about methylamine is correct?
A

It neutralises an aqueous solution of sodium hydroxide.

B

It reacts with copper(II) carbonate to give carbon dioxide.

C

It reacts with hydrochloric acid to form a salt.

D

It turns blue litmus red.

24 The positions in the Periodic Table of four elements are shown.
Which element is most likely to form an acidic oxide?

A
B
C
D

© UCLES 2010

0620/12/M/J/10

[Turn over

10
25 The diagram shows the manufacture of steel. gas X

waste gases

molten iron

What is gas X?
A

carbon dioxide

B

chlorine

C

hydrogen

D

oxygen

26 A student added dilute hydrochloric acid to four metals and recorded the results.
Not all of the results are correct. results metal

gas given off

1

copper

yes

2

iron

yes

3

magnesium

no

4

zinc

yes

Which two results are correct?
A

1 and 3

© UCLES 2010

B

1 and 4

C

2 and 3

0620/12/M/J/10

D

2 and 4

11
27 An element does not conduct electricity and exists as diatomic molecules.
In which area of the Periodic Table is the element to be found?

C D

A
B

28 Copper, iron and zinc are all used as pure metals.
Which of these three metals are also used in alloys? copper iron

zinc

A







B







C







D







29 Solutions of a halogen and a sodium halide are mixed.
Which mixture darkens in colour because a reaction occurs?
A

bromine and sodium chloride

B

bromine and sodium fluoride

C

chlorine and sodium fluoride

D

chlorine and sodium iodide

30 Some properties of four elements are shown in the table.
Which element is a metal? melting point / °C

electrical conductivity when liquid

electrical conductivity when solid

A

–7

low

low

B

801

high

low

C

1535

high

high

D

3550

low

low

© UCLES 2010

0620/12/M/J/10

[Turn over

12
31 The diagram shows three types of item.

cutlery

cooking pan

instruments used in hospitals

Which method of rust prevention can be used for all three types of item?
A

coating with plastic

B

covering with grease

C

galvanising

D

using stainless steel

32 Aluminium is an important metal with many uses.
Some of its properties are listed.
1

It is a good conductor of heat.

2

It is a reactive metal.

3

It has a low density.

4

It has an oxide layer that prevents corrosion.

Which set of properties help to explain the use of aluminium for cooking and storing food?
A

B

1, 2 and 3

1, 2 and 4

C

1, 3 and 4

D

2, 3 and 4

33 To grow roses, a fertiliser containing nitrogen, phosphorus and potassium is needed.
For the best flowers, the fertiliser should contain a high proportion of potassium.
Which fertiliser is best for roses?

fertiliser

proportion by mass
N

P

K

A

9

0

25

B

13

13

20

C

29

5

0

D

29

15

5

© UCLES 2010

0620/12/M/J/10

13
34 Which statements about water are correct?
1
2

Household water may contain salts in solution.

3

Water is used in industry for cooling.

4
A

Water is treated with chlorine to kill bacteria.

Water for household use is filtered to remove soluble impurities.

1, 2 and 3

B

1 and 4

C

2, 3 and 4

D

1, 2, 3 and 4

35 Which statement about methane is not correct?
A

It is a liquid produced by distilling petroleum.

B

It is produced as vegetation decomposes.

C

It is produced by animals such as cows.

D

It is used as a fuel.

36 Which compound in polluted air can damage stonework and kill trees?
A

carbon dioxide

B

carbon monoxide

C

lead compounds

D

sulfur dioxide

37 Diesel, petrol and bitumen are all
A

fuels.

B

hydrocarbons.

C

lubricants.

D

waxes.

© UCLES 2010

0620/12/M/J/10

[Turn over

14
38 A macromolecule is a very large molecule.
Macromolecules can be made by joining smaller molecules together. This is called polymerisation. Which row in the table describes the formation of a polymer? monomer polymer

A

ethane

poly(ethane)

B

ethene

poly(ethene)

C

ethane

poly(ethene)

D

ethene

poly(ethane)

39 Which structure shows a compound that belongs to a different homologous series to propane?
A

B
H

H
H

C

C

H
H

H

H

H

C

C

C

C

H

C

H

H

H

H
C

H

D

H

H

H

H

H

H

H

H

H

C

C

C

C

H

H

H
H

H

H

H

H

40 Which structure is incorrect?
A

B

H
C

C

H

H

H

H

© UCLES 2010

H
H

H

C

H
O

H

H

H

0620/12/M/J/10

H

C

C

H

O

C

D

C

H

H
H

H

H

C

C

H

H

O

H

15
BLANK PAGE

© UCLES 2010

0620/12/M/J/10

© UCLES 2010

24

40

Sodium

Calcium

88

0620/12/M/J/10

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

88

Radium

Fr

Francium

87

*

Hafnium

72

Lanthanum

57

Hf

La

40

Zirconium

Zr

91

Titanium

178

Yttrium

22

48

Ti

139

39

Y

89

Scandium

21

227

Barium

Caesium

56

Cs

45

Sc

226

55

137

Ba

133

Strontium

Rubidium

38

Rb

37

Sr

85

20

Potassium

19

Ca

39

Magnesium

Na

12

Mg

23

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

141

Pa

Thorium

55

Tc
186

Re

144

Nd

92

60

Uranium

U

238

Neodymium

75

Rhenium

43

Technetium

25

Manganese

Mn
29

30

65

8

9

VII

2

0

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

Eu

152

Platinum

Am
95

Americium

63

Europium

78

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

70

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

In

32

Germanium

Ge

73

Silicon

115

Gallium

Ga

Dysprosium

81

49

31

13

Aluminium

Si

Al
14

28

Carbon

27

Boron

12

C

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

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

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

Hydrogen

B

4

28

64

7

VI

He

27

59

6

V

H

59

5

IV

The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).

91

Protactinium

Th

232

Praseodymium

Cerium

59

Pr

Ce

74

Tungsten

42

Molybdenum

24

Chromium

Cr

140

Tantalum

41

23

Vanadium

V

51

1

III
1

Group

DATA SHEET
The Periodic Table of the Elements

16

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.

University of 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.

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