June 1999 - Paper 1

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

5070/1

CHEMISTRY PAPER 1 Multiple Choice Friday

18 JUNE 1999

Morning

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 16 printed pages. SB (KG) QF92362/3 © UCLES 1999

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2 1

In the Haber process, nitrogen and hydrogen react to form ammonia. Which set of diagrams represents the molecules of nitrogen, hydrogen and ammonia? nitrogen

hydrogen

ammonia

A

B

C

D

2

An ion X + has 23 nucleons and 10 electrons. What does the nucleus of the ion X + contain?

3

protons

neutrons

A

12

11

B

11

12

C

10

13

D

9

14

Which of the following has the highest electrical conductivity? A

aqueous sugar solution

B

solid graphite

C

solid sodium chloride

D

gaseous carbon dioxide

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3 4

A mixture of two liquids in equal proportions is fractionally distilled. When the thermometer first shows a steady reading, at which point will there be the greater proportion of the liquid with the higher boiling point?

thermometer A

B

C

mixture of liquids

D

heat

5

The apparatus shown is set up, using different gases in the beaker.

beaker porous pot oxygen

X water

Which gas, when present in the beaker, causes the water level at X to rise? A

carbon dioxide, CO2

B

chlorine, Cl2

C

nitrogen dioxide, NO2

D

methane, CH4

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4 6

A number for the elements from oxygen to aluminium changes as shown.

number for the element

O F Ne Na Mg Al element What is this number?

7

A

the Group number of the element in the Periodic Table

B

the number of electron shells in an atom

C

the number of electrons in the outer shell of an atom

D

the number of protons in an atom

In an experiment to find the formula of magnesium oxide, magnesium metal is heated in a covered crucible.

magnesium

heat Why is the crucible covered with a loose-fitting lid?

8

A

to prevent air escaping from the crucible

B

to prevent magnesium carbonate forming

C

to prevent magnesium oxide escaping from the crucible

D

to prevent water vapour entering the crucible

A solid element conducts electricity. The element burns in air to form a white solid. This white solid dissolves in water to give an alkaline solution. What is the element? A

aluminium

B

calcium

C

carbon

D

copper 5070/1 S99

5 9

Silver ions react with chloride ions. Ag+(aq) + Cl −(aq) → AgCl(s) It is found that 5 cm3 of a 0.1 mol/dm3 solution of the chloride of metal X needs 10 cm3 of 0.1 mol/dm3 silver nitrate for complete reaction. What is the formula of the chloride? A

XCl 4

B

XCl 2

C

XCl

D

X2Cl

10 Which equation represents the combustion of methane with the products collected at 120 °C? + 2O2(g) → CO2(g) + 2H2O(l)

A

CH4(l)

B

CH4(g) + 2O2(l)

C

CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

D

CH4(l)

+ 2O2(l)

→ CO2(s) + 2H2O(l) → CO2(l)

+ 2H2O(s)

11 Which change always takes place when aqueous copper(II) sulphate is electrolysed? A

Copper is deposited at the negative electrode.

B

Oxygen is evolved at the positive electrode.

C

Sulphate ions move towards the negative electrode.

D

The colour of the solution fades.

12 The electrolysis shown in the diagram is set up.

carbon electrodes

+

–

concentrated aqueous potassium iodide What is observed? at positive electrode

at negative electrode

A

solution turns brown

bubbles of colourless gas

B

solution turns brown

C

bubbles of colourless gas

D

bubbles of colourless gas

silvery droplets bubbles of colourless gas solution turns brown 5070/1 S99

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6 13 Hydrogen reacts with chlorine. H2(g) + Cl2(g) → 2HCl(g)

∆H = −184 kJ

Why does ∆H for this reaction have a negative sign? A

Hydrogen and chlorine are covalent, but hydrogen chloride is ionic.

B

More bonds are formed than are broken.

C

The total energy of bond breaking is less than that of bond forming.

D

The speed of the reaction increases as temperature increases.

14 Why is vanadium(V) oxide used in the oxidation of sulphur dioxide to sulphur trioxide? A

It acts as a reducing agent.

B

It prevents the decomposition of sulphur trioxide.

C

It removes impurities.

D

It speeds up the reaction.

15 In the graph, curve X represents the results of the reaction between 1.0 g of granulated zinc and an excess of acid at 30 °C. X

total volume of gas produced (measured at r.t.p.)

Y

time Which changes will produce curve Y? A

using 1.0 g of powdered zinc at 20 °C

B

using 1.0 g of granulated zinc at 20 °C

C

using 0.5 g of granulated zinc at 40 °C

D

using 0.5 g of granulated zinc at 20 °C

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7 16 Which element in the reaction below is oxidised? 2FeSO4 + Cl2 + H2SO4 → Fe2(SO4)3 + 2HCl A

chlorine

B

hydrogen

C

iron

D

sulphur

17 The word equation shows a chemical reaction. +

sulphuric acid

a salt

substance Y

+

water

+

carbon dioxide

What could substance Y be? A

copper(II) oxide

B

magnesium

C

sodium carbonate

D

sodium hydroxide

18 Solid R is gradually added to aqueous solution S. The changes in pH are shown on the graph. 14

pH

7

0 mass of solid R added What are R and S? R A B C D

insoluble metal oxide insoluble non-metal oxide soluble metal oxide soluble non-metal oxide

S hydrochloric acid sodium hydroxide hydrochloric acid sodium hydroxide

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8 19 A solution X forms a white precipitate with dilute sulphuric acid and also with aqueous silver nitrate. What could solution X contain? A

barium chloride

B

barium nitrate

C

magnesium chloride

D

magnesium sulphate

20 The diagram shows apparatus used to test the gases produced by burning coal. to pump

burning coal

R

Which substance is placed in tube R to show that sulphur dioxide is formed? A

aqueous potassium dichromate(VI)

B

aqueous potassium iodide

C

damp red litmus paper

D

limewater

21 Which of the following is a typical property of transition metals? A

They form coloured compounds.

B

They have low densities.

C

They have low melting points.

D

They react with cold water to give hydrogen.

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9 22 The structure of a compound containing an element Y and hydrogen is represented as shown. Only outer shell electrons are shown. key

H H x

x x

x = electron from Y = electron from H

x

x x

Y Y x

x x

x

H H To which group of the Periodic Table does element Y belong? A

III

B

IV

C

V

D

VI

23 The diagram shows the positions of four elements in the Periodic Table. Which element gains electrons to form negatively charged ions? I

II

III

IV

V

VI

VII

0 A

D

C

B

24 Which substance can be reduced by heating with carbon? A

aluminium oxide

B

calcium carbonate

C

iron(III) oxide

D

magnesium oxide

25 What happens when zinc is placed in aqueous copper(II) sulphate? A

Copper atoms are oxidised.

B

Zinc atoms are oxidised.

C

Copper ions are oxidised.

D

Zinc ions are oxidised.

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10 26 The table shows some typical properties of metals and non-metals. Which properties for a metal and for a non-metal are both correct? metals

non-metals

A

do not conduct electricity

usually have a low melting point

B

usually have a high melting point

good conductor of heat

C

shiny when polished

good conductor of electricity

D

good conductor of electricity

usually dull in appearance

27 The list shows four metals and hydrogen in order of reactivity. most reactive

rubidium potassium tin hydrogen

least reactive

gold

Which of the following do not give hydrogen as a product? A

The adding of rubidium to water.

B

The adding of tin to dilute hydrochloric acid.

C

The electrolysis of aqueous gold chloride.

D

The electrolysis of aqueous rubidium chloride.

28 Which substance does not need air as a raw material for its manufacture? A

ammonia

B

iron

C

sodium

D

sulphuric acid

29 Which of the following is a reaction of dilute hydrochloric acid? A

Ammonium chloride reacts to give ammonia.

B

Calcium carbonate reacts to give carbon dioxide.

C

Copper reacts to give hydrogen.

D

Universal Indicator paper turns blue.

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11 30 The diagram shows a reaction used to manufacture a fertilizer. ammonia

+

substance X

a fertilizer

What could substance X be? A

lime (calcium oxide)

B

nitrogen

C

potassium hydroxide

D

sulphuric acid

31 Which of the following is not a use of silicon or its compounds? A

making fire-resistant plastics

B

making glass

C

making polishes

D

making smokeless fuel

32 Which statement best confirms that two substances are allotropes of carbon? A

They both reduce heated iron(III) oxide to iron.

B

They have different crystalline structures.

C

Equal masses of the substances require equal masses of oxygen for complete combustion.

D

Equal masses of the substances give equal masses of carbon dioxide, and no other product, when completely burnt in oxygen.

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12 33 The structure of butan-1-ol is shown.

H

H

H

H

H

C

C

C

C

H

H

H

H

Which structure is an isomer of that shown above?

A

H

H

H

H

OH

C

C

C

C

H

H

H

H

H

H

H

H

C

C

H

H

C

C

H

B H H

H

H

OH

H

H

C

C

H H

H H

C

C

H

H

C

D

H

H

H

H

H

C

C

C

C

H

H

OH H

OH

H

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OH

13 34 The diagram shows the fractional distillation of petroleum.

fraction X

fraction Y heated petroleum

Which statements about fractions X and Y are correct? X burns more easily than Y

35

X has a higher boiling point than Y

A

yes

yes

B

yes

no

C

no

yes

D

no

no

Which set contains all the possible combustion products of methane, CH4? A

carbon, carbon dioxide, carbon monoxide and water

B

carbon, carbon monoxide and hydrogen

C

carbon dioxide, carbon monoxide, hydrogen and water

D

carbon monoxide and water

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14 36 The structures of two compounds are shown. H

H

H

H H

C

H H

H

C

C

C

C

H

H H

C

H H

H

H

H

H H

C

H

H

C

C

C

C

H

H

C

H H

H

H

Which statement about these two compounds is correct? A

They are both hydrocarbons.

B

They are both saturated compounds.

C

They are in the same homologous series.

D

They are isomers of each other.

37 Equal masses of coconut oil, butter, margarine and palm oil are separately dissolved in an organic solvent. A few drops of aqueous bromine are added to each solution and the mixtures are shaken. The table shows the results. Which sample contains the most unsaturation? sample A

colour of mixture

butter

orange

B

coconut oil

dark orange

C

margarine

yellow

D

palm oil

colourless

38 When an animal fat is boiled with aqueous sodium hydroxide, a soap and glycerol are formed. This reaction is an example of A

esterification.

B

fermentation.

C

hydrolysis.

D

polymerisation.

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15 39 The structure of the monomer of Perspex is shown. H

CH3 C

C

H

CO2CH3

Which description of Perspex is correct? type of polymer A B

carbohydrate ester

polymer formed by condensation polymerisation addition polymerisation

C

hydrocarbon

addition polymerisation

D

polyester

condensation polymerisation

40 The apparatus shown was set up to prepare ethanoic acid from ethanol.

water out

condenser

cold water in

ethanol and acidified potassium dichromate(VI) heat What was the purpose of the condenser? A

to make sure air does not react with ethanol

B

to stop ethanoic acid changing back to ethanol

C

to stop ethanol being converted into ethene

D

to stop ethanol vapour escaping

5070/1 S99

Magnesium

Sodium

5070/1 S99

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