1

Name

Register Number Class

SCIENCE CHEMISTRY 5116/3

Paper 3

MAY 2010 1 hour 15 minutes

PRELIMINARY EXAMINATION

SECONDARY FOUR EXPRESS/SECONDARY FIVE NORMAL

READ THESE INSTRUCTIONS FIRST

Do not open this booklet until you are told to do so. Write your name, class and register number on top of this page and on any separate answer paper used. Section A Answer all questions. Write down your answers in the space provided in the answer sheet. Section B Answer 2 out of 3 questions. Write down your answers on the answer sheet provided. At the end of the examination: Hand in the Answer sheet only .

For Examiner’s Use Section A Section B TOTAL

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This question paper consists of 11 printed pages.

MACPHERSON SECONDARY SCHOOL

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Section A (45 Marks)

Answer all the questions in the answer booklet provided.

A1 The diagram below shows the structure of an atom of element Q.

(a) Complete the table below about the three different particles found in an atom of element Q.

Particle Name of particle Relative charge

X

(b) Is element Q a metal or non-metal? Give a reason for your answer.

(c) Element Q reacts with oxygen to form the compound Q2O.

(i) Draw a dot-and-cross diagram of the electronic structure of the compound. Show only the outer electrons. (ii) Would you expect the compound to have a high or low melting point ? Explain your answer.

[3] [1] [3] [2]

●

○

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A2 Carbon monoxide reacts with copper (II) oxide accordng to the following equation:

CO + CuO CO2 + Cu

(a) What volume of cabon monoxide is required to to convert 4.0 g of copper (II) oxide [2]

(b) Find the mass of copper metal obtained at the end of the reaction. [2]

(c) Find the number of moles of carbon dioxide molecules produced under room conditions.

[2]

A3 Given below is a list of substances.

Sodium hydroxide Silver Chloride Magnesium Lead (II) nitrate

Dilute nitric acid Calcium oxide Ammonium sulfate

Select from the list above, substance(s) that is suitable for the following descriptions.

(a)

A salt that is prepared by precipitation.

(b)

Two substances that are reacted to form magnesium nitrate.

(c)

A substance that is prepared by titration.

(d)

A substance that is added to neutralise the soil.

(e)

Two substances when reacted in the aqueous state forms a white preciptate that dissolves when one of the reactant is added in excess.

(f) A substance that can liberate a gas that turns damp red litmus blue

[6]

4

A4

(a) Deduce the identity of the substance lettered M, P, Q, R and S by giving their chemical name.

[5]

(b) Write down the equation for the reaction of metal M with dilute hydochloric acid. [2]

(c) Describe how you can identify the combustible gas. [2]

A5

Answer the following questions using the metals below:

copper zinc magnesium sodium iron

(a) Name the most reactive metal

(b) Write down the name of the metal which is likely to be found native (i.e. naturally occurring).

(c) Which metal does not react with water but reacts readily with dilute

hydrochloric acid.

(d) Which metal is used to galvanise iron sheets.

[1] [1] [1] [1]

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A6 The figure below shows an experiment to be carried out by a student to investigate the substances formed when methane burns in plentiful supply of air.

a) A liquid P collects in tube A. Name liquid P. [1]

b) What would you expect to see in tube B during the experiment? [1]

c) Write a balanced chemical equation for the complete combustion of

methane in air. [1]

d) However, if insufficient air is present, a different colourless gas is produced in the combustion. This gas could be harmful to the student.

i) Name this substance. [1]

ii) How might the gas be harmful to the student? [1]

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A7

An experiment was set up as shown in the diagram below. It investigated the reaction between granulated zinc and 2.0 mol/dm3 sulphuric acid. The results of the experiment are shown in the graph below.

granulated zinc

sulphuric acid

(i) On the same axes above, sketch what you would expect if the experiment was repeated at a lower temperature.Label the curve T.

(ii) On the same axes above, sketch what you would expect

if the experiment was repeated using zinc powder. Label the curve P .

(iii) In terms of the kinetic particle theory (the movement of

particles of matter), explain the effect of a higher temperature on the speed of reaction.

[2] [2] [2]

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SECTION B (10 marks each) Answer TWO essay questions only

B1 (a) Although sodium chloride and butane have approximately the same relative molecular mass, the boiling point of sodium chloride is more than 1000oC higher than that of butane. With the aid of suitable diagrams, explain why the boiling point of sodium chloride is much higher than that of butane.

[5]

B1(b) Uranium is between magnesium and zinc in the reactivity series.

Equal sized strips of magnesium, uranium and zinc were placed in hydrochloric acid.

The hydrochloric acid was of the same concentration. The results are shown in the table.

(i) Describe the observation of uranium with hydrochloric acid.

(ii) Uranium has several isotopes which are radioactive.

One of its isotopes is uranium–235. The other is Uranium –237.

What do you understand by the term isotopes?

How do these two isotopes differ?

[2] [3]

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B2(a) There are three main stages involved in the production of polythene bottles from crude oil. Polythene is also known as polyethene.

(i) State the processes involved in :

how heavy oil can be obtained from crude oil in stage I. how monomer X be obtained from heavy oil in stage II.

[2]

(ii) Draw the structure of monomer X.

[2]

(iii) Describe a test to confirm the nature of monomer X.

[2]

) B2(b)B2(b)

The macromolecule below is an addition polymer.

Polymer X

(i) Draw the structure of the monomer from which polymer X is formed.

(ii) Polymer X is used as an insulating cover for electrical wires. Explain why polymer X does not conduct electricity.

(iii) Polymer X is non-biodegradable. Describe one pollution problem that this causes.

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[2] [1] [1]

Crude oil Heavy oil Monomer X

Polythene bottles

Stage I Stage II Stage III

C C C C C C

H H H H H H

H H Cl H Cl Cl

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B3

An experiment was carried out to investigate the rate of decomposition of aqueous hydrogen peroxide at room temperature. The unbalanced equation and the total volume of oxygen gas given off every twenty seconds is given below.

H2O2 (aq) → H2O (l) + O2 (g)

Time / s 0 20 40 60 80 100 120 140 160 Total volume of oxygen /cm3

0

14

22

33

35

36

36

36

(a) Copy and balance the chemical equation above. [1]

(b) Plot the graph of total volume of oxygen against time on the graph paper provided in the answer sheet.

Use the graph that you have plotted , to

i) estimate the missing the volume of oxygen at 60 seconds.

ii) state the total volume of oxygen produced at the end of reaction.

[3] [1] [1]

(c) Describe how you can test for the gas evolved .

[2]

(d) The reaction was repeated at 800C. Sketch and label on the same graph paper, the graph for the reactions

carried out for this temperatures.

[2]

#### END OF PAPER THREE#####

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DATA SHEET The Periodic Table of Elements

Group I II III IV V VI VII 0

1

H Hydrogen

1

4

He Helium

2

7

Li Lithium

3

9

Be Beryllium

4

11

B Boron

5

12

C Carbon

6

14

N Nitrogen

7

16

O Oxygen

8

19

F Fluorine

9

20

Ne Neon

10

23

Na Sodium

11

24

Mg Magnesium 12

27

Al Aluminium

13

28

Si Silicon

14

31

P Phosphorus 15

32

S Sulphur

16

35.5

Cl Chlorine 17

40

Ar Argon

18

39

K Potassium 19

40

Ca Calcium

20

45

Sc Scandium

21

48

Ti Titanium 22

51

V Vanadium 23

52

Cr Chromium

24

55

Mn Manganese 25

56

Fe Iron

26

59

Co Cobalt

27

59

Ni Nickel

28

64

Cu Copper

29

65

Zn Zinc

30

70

Ga Gallium

31

73

Ge Germanium 32

75

As Arsenic

33

79

Se Selenium

34

80

Br Bromine

35

84

Kr Krypton

36

85

Rb Rubidium 37

88

Sr Strontium

38

89

Y Yttrium

39

91

Zr zirconium 40

93

Nb Niobium

41

96

Mo Molybdenum

42

Tc Technetium 43

101

Ru Ruthenium

44

103

Rh Rhodium

45

106

Pd Palladium 46

108

Ag Silver

47

112

Cd Cadmium 48

115

In Indium

49

119

Sn Tin

50

122

Sb Antimony

51

128

Te Tellurium

52

127

I Iodine

53

131

Xe Xenon

54

133

Cs Caesium

55

137

Ba Barium

56

139

La Lanthanum 57

178

Hf Hafnium

72

181

Ta Tantalum 73

184

W Tungsten

74

186

Re Rhenium

75

190

Os Osmium

76

192

Ir Iridium

77

195

Pt Platinum

78

197

Au Gold

79

201

Hg Mercury

80

204

Tl Thallium

81

207

Pb Lead

82

209

Bi Bismuth

83

Po Polonium

84

At Astatine

85

Rn Radon

86

Fr Francium 87

226

Ra Radium

88

227

Ac Actinium

89

*58-71 Lanthanoid series †90-103 Actinoid series

140

Ce Cerium

58

141

Pr Praseodymium 59

144

Nd Neodymium 60

Pm Promethium 61

150

Sm Samarium 62

152

Eu Europium 63

157

Gd Gadolinium 64

159

Tb Terbium

65

162

Dy Dysprosium 66

165

Ho Holmium

67

167

Er Erbium

68

169

Tm Thulium

69

173

Yb Ytterbium 70

175

Lu Lutetium

71

a

X b

A = relative atomic mass

X = atomic symbol

B = proton (atomic) number

232

Th Thorium

90

Pa Protactinium

91

238

U Uranium

92

Np Neptunium

93

Pu Plutonium 94

Am Americium 95

Cm Curium

96

Bk Berkelium 97

Cf Californium 98

Es Einsteinium 99

Fm Fermium

100

Md Mendelevium

101

No Nobelium 102

Lr Lawrencium 103

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

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Colours of Some Common Metal Hydroxides

Calcium hydroxide White Copper(II) hydroxide Light blue

Iron(II) hydroxide Green Iron(III) hydroxide Red-brown Lead(II) hydroxide White

Zinc hydroxide White