Paper 1

UNIVERSITY OF CAMBRIDGE LOCAL EXAMINATIONS SYNDICATE General Certificate of Education Ordinary Level

5070/1

CHEMISTRY PAPER 1 Multiple Choice Tuesday

16 NOVEMBER 1999

1 hour

Additional materials: Electronic calculator and/or Mathematical tables Multiple choice answer sheet Soft clean eraser Soft pencil (type B or HB is recommended)

TIME

1 hour

INSTRUCTIONS TO CANDIDATES Do not open this booklet until you are told to do so. Write your name, Centre number and candidate number on the answer sheet in the spaces provided unless this has already been done for you. There are forty questions in 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 very carefully the instructions on the answer sheet. INFORMATION FOR CANDIDATES 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. Mathematical tables are available. You may use a calculator. A copy of the Periodic Table is printed on page 16.

This question paper consists of 15 printed pages and 1 blank page. SB (KG) QK94129/4 © UCLES 1999

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2 1

An atom of an element contains 17 protons, 18 neutrons and 17 electrons. What is the atomic structure of another isotope of this element? protons

2

neutrons

electrons

A

17

20

17

B

17

18

16

C

18

18

17

D

20

18

17

An inflated balloon goes down because gas molecules can diffuse through the rubber. Four balloons are filled with different gases at the same temperature and pressure. Which balloon would go down most quickly? A

carbon dioxide, CO2

3

4

B

C

methane, CH4

nitrogen, N2

D

oxygen, O2

Which statement explains why oxygen can be separated from nitrogen by the fractional distillation of liquid air? A

Oxygen is more dense than nitrogen.

B

Oxygen is more reactive than nitrogen.

C

The two elements have different boiling points.

D

The two gases are in different groups of the Periodic Table.

Which of the following is the best method of obtaining pure water from ink? A

chromatography

B

distillation

C

filtration

D

freezing

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3 5

Hydrogen chloride is very soluble in water, whereas chlorine is only slightly soluble in water. Both gases can be dried using concentrated sulphuric acid. Which diagram represents the correct method of obtaining dry chlorine from damp chlorine containing a small amount of hydrogen chloride? A

B

damp Cl 2 and HCl

damp Cl 2 and HCl

concentrated sulphuric acid

water

water

C

D

damp Cl 2 and HCl

concentrated sulphuric acid

6

concentrated sulphuric acid

damp Cl 2 and HCl

water

water

concentrated sulphuric acid

What do both an atom and an ion of the isotope of sodium, 23 11 Na, contain? A

11 electrons

B

12 neutrons

C

23 protons

D

23 neutrons

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4 7

The diagram represents an atom of an element. e

5n 4p

e

key e = electron n = neutron p = proton

e

e Which symbol gives this information? A

8

9

9 4 Be

B

9 5B

C

4 9F

D

13 8O

Which substance in the table is an ionic compound?

substance

state at room temperature

electrical conductivity at room temperature

electrical conductivity of aqueous solution

A

liquid

good

insoluble

B

liquid

poor

poor

C

solid

good

good

D

solid

poor

good

The bonding in sulphuric acid can be represented by the structure shown. H

O

O S

H

O

O

What is the total number of electrons in the covalent bonds surrounding the sulphur atom? A

4

B

6

C

8

D

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12

5 10 An excess of hydrochloric acid is added to 0.10 mol of magnesium in the apparatus shown.

100 cm3 syringe

dilute hydrochloric acid magnesium

Why is it impossible to measure the total volume of hydrogen produced using this apparatus? A

Hydrogen is less dense than air.

B

Hydrogen is soluble in hydrochloric acid.

C

There is air in the tube.

D

The volume of hydrogen formed is greater than 100 cm3.

11 20 cm3 of oxygen are reacted with 20 cm3 of carbon monoxide. What are the volumes of the gases remaining, at the original temperature and pressure? oxygen/cm3

carbon monoxide/cm3

carbon dioxide/cm3

A

0

0

20

B

0

0

40

C

10

0

20

D

10

10

20

12 Aqueous copper(II) sulphate is electrolysed using copper electrodes. Which equation represents the reaction taking place at the anode (positive electrode)? A

Cu(s) → Cu2+(aq) + 2e−

B

Cu2+(aq) + 2e− → Cu(s)

C

4OH−(aq) → 2H2O(l) + O2(g) + 4e−

D

2H+(aq) + 2e− → H2(g)

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6 13 Element X is extracted by the electrolysis of a molten compound of elements X and Y. The electrode reactions are as shown. at the cathode

at the anode

X 2+ + 2e− → X

2Y 2− − 4e− → Y2

Which of the following could be the compound? A

aluminium oxide

B

calcium chloride

C

magnesium oxide

D

potassium chloride

14 In which circuit does the bulb light up?

key A

Cu

B

CuSO4(aq)

Cu

Ag

NaCl(s)

= bulb

C

Zn

Cu

C2H5OH(I)

D

Zn

Ag

H2SO4(aq)

Cu

15 Nitrogen and hydrogen react in a closed vessel. N2(g) + 3H2(g)

2NH3(g)

How do the speeds of the forward and reverse reactions change, if the pressure in the vessel is increased but the temperature is kept constant? speed of forward reaction

speed of reverse reaction

A

increases

increases

B

does not change

does not change

C

decreases

increases

D

decreases

does not change

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7 16 Solution X turns acidified potassium dichromate(VI) from orange to green. What must solution X contain? A

an alkali

B

an ammonium salt

C

an oxidising agent

D

a reducing agent

17 The manufacture of sulphuric acid by the Contact process can be represented as follows. S → SO2 → SO3 → H2SO4 Which diagram shows the oxidation state (oxidation number) of sulphur at each stage of the process? A

B

8 7 6 oxidation 5 4 state 3 2 1 0

C

D 8 7 6 5 4 3 2 1 0

18 Which of the following compounds dissolves in water to give a solution with a pH greater than 7? A

calcium carbonate

B

copper(II) hydroxide

C

sodium hydroxide

D

sulphur dioxide

19 Which words in the table complete the following description of the preparation of copper(II) sulphate? An excess of copper(II) oxide was added to dilute sulphuric acid. The mixture was ——-1—— to remove the excess of oxide. The solution was ——2—— to half its volume and then cooled, so that it ——-3—— . 1

2

A

distilled

evaporated

B

distilled

C

filtered

condensed

crystallised

D

filtered

evaporated

crystallised

filtered

3 crystallised evaporated

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8 20 Which statement about groups in the Periodic Table is correct? A

All groups contain both metals and non-metals.

B

Atoms of elements in the same group have the same total number of electrons.

C

In Group l, reactivity decreases with increasing proton (atomic) number.

D

In Group VII, the melting point of the elements increases with proton (atomic) number.

21 Element Q has a melting point greater than 1000 °C. It has oxidation states (oxidation numbers) of +2 and +3 in its compounds. These compounds are coloured. In which position of the Periodic Table shown is Q found?

A D B

C

22 The table gives the formulae of the catalysts used in some industrial processes. process

catalyst

Haber process

Fe + Mo

Contact process

V2O5

cracking of alkanes

Al2O3 + SiO2

polymerisation of ethene

Al(C2H5)3 + TiCl4

manufacture of silicones

CuCl

How many different transition metals are included (as elements or as compounds) in the list of catalysts? A

3

B

4

C

5

D

6

23 Which oxide can be reduced to its metal by heating in a stream of hydrogen gas? A

aluminium oxide

B

copper(II) oxide

C

magnesium oxide

D

sodium oxide

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9 24 When heated, solid X gives off a gas which turns limewater milky. The residue reacts with dilute acid and also with aqueous alkali. What is X? A

copper(II) carbonate

B

magnesium carbonate

C

sodium carbonate

D

zinc carbonate

25 The table shows the results of adding weighed pieces of iron to solutions M and S. solution used

initial mass of iron /g

mass of iron after 15 minutes /g

M

5

4

S

5

4

What could the aqueous solutions M and S have been? M

S

A

copper(II) sulphate

B

iron(II) chloride

C

dilute hydrochloric acid

D

magnesium chloride

silver nitrate calcium chloride sodium chloride dilute sulphuric acid

26 Hydrogen can be manufactured from methane using a nickel catalyst. methane X

nickel catalyst

hydrogen Y

What are X and Y? X

Y

A

oxygen

oxides of carbon

B

nitrogen

C

steam

oxides of carbon

D

steam

ethene

ammonia

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10 27 An element is burned in an excess of oxygen. Which statement about the oxide formed is always correct? A

It is a crystalline solid.

B

It is greater in mass than the element.

C

It is soluble in water.

D

It is white in colour.

28 An element X, necessary for plant growth, can be added to the soil only in the form of compounds which contain the ion X +. What is X ? A

hydrogen

B

nitrogen

C

phosphorus

D

potassium

29 What is the concentration of hydrogen ions in 0.05 mol/dm3 sulphuric acid? A

0.025 g/dm3

B

0.05 g/dm3

C

0.10 g/dm3

D

2.0 g/dm3

30 Which ions are discharged when concentrated aqueous sodium chloride is electrolysed? A

chloride and hydroxide ions

B

chloride and hydrogen ions

C

hydrogen and sodium ions

D

hydroxide and sodium ions

31 Carbon and silicon are in the same group of the Periodic Table. What is the formula of sodium silicate? A

NaSiO2

B

NaSiO3

C

Na2SiO3

D

Na2SiO4

32 Which statement shows that diamond and graphite are allotropes of carbon? A

Both have giant molecular structures.

B

Complete combustion of equal masses of each produces equal masses of carbon dioxide as the only product.

C

Graphite conducts electricity, whereas diamond does not.

D

Under suitable conditions, graphite can be converted into diamond. 5070/1 W99

11 33 Which calcium compound does not increase the pH of acidic soils? A

calcium carbonate

B

calcium hydroxide

C

calcium oxide

D

calcium sulphate

34 Which compound, on combustion, never forms soot? A

carbon monoxide

B

ethanol

C

ethene

D

methane

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12 35 The molecular structure of a hydrocarbon is shown below. H H H

C

H

H

C

C

H

H

C

H H

H Which structure is an isomer of this hydrocarbon? A

B H

H H

H

H H

C

H

C

C

C

H

C

H H

H

H

H

H

C

C

C

H H

C

H H

H

H H

H

C

H

D

H

H

H

H

H

C

C

C

C

C

H

H

H

H

H

H H

H

C

H

H

C

C

H

H

C

H

H

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13 36 Octane is an alkane present in petrol. What are the products when octane is completely burned in air? A

carbon dioxide and hydrogen

B

carbon dioxide and water

C

carbon monoxide and water

D

carbon monoxide, carbon dioxide and water

37 Which type of reaction occurs when soap is formed from fats? A

hydrolysis

B

polymerisation

C

fermentation

D

substitution

38 Which of these equations does not represent an addition reaction? A

CH2Cl2 + Cl2 → CHCl3 + HCl

B

C2H4 + Br2 → C2H4Br2

C

n C2H4 → ( CH2 − CH2 ) n

D

C3H6 + H2O → C3H7OH

39 A polymer has the structure shown. CH2

CH

CH2

CH3

CH

CH2

CH3

CH CH3

What is the molecular formula of the monomer? A

C2H4

B

C2H6

C

C3H6

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D

C3H8

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14 40 What is the linkage between the units in fats and also in Terylene? O A

C

O

H B

C

O

H

C

D

O

H

C

N

H

H

C

C

H

H

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15 BLANK PAGE

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Magnesium

Sodium

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Strontium

45

Key

b

a

X

*

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

89

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

Calcium

Rb

19

20

40

Ca

39

K

12

24

Mg

23

Na

Beryllium

4

Lithium

Potassium

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

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

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

51

1

Group

DATA SHEET The Periodic Table of the Elements

16