S3_Chemistry_EOY_08_P1

7/30/2019 S3_Chemistry_EOY_08_P1

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Group

I II III IV V VI VII 01

HHydrogen

1

4

HeHelium

2

7

LiLithium

3

9

BeBeryllium

4

11

BBoron

5

12

CCarbon

6

14

NNitrogen

7

16

OOxygen

8

19

FFluorine

9

20

NeNeon

10

23

NaSodium

11

24

MgMagnesium

12

27

AlAluminium

13

28

SiSilicon

14

31

PPhosphorus

15

32

SSulphur

16

35.5

ClChlorine

17

40

ArArgon

18

39

KPotassium

19

40

CaCalcium

20

45

ScScandium

21

48

TiTitanium

22

51

VVanadium

23

52

CrChromium

24

55

MnManganese

25

56

FeIron

26

59

CoCobalt

27

59

NiNickel

28

64

CuCopper

29

65

ZnZinc

30

70

GaGallium

31

73

GeGermanium

32

75

AsArsenic

33

79

SeSelenium

34

80

BrBromine

35

84

KrKrypton

36

85

RbRubidium

37

88

SrStrontium

38

89

YYttrium

39

91

ZrZirconium

40

93

NbNiobium

41

96

MoMolybdenum

42

TcTechnetium

43

101

RuRuthenium

44

103

RhRhodium

45

106

PdPalladium

46

108

AgSilver

47

112

CdCadmium

48

115

InIndium

49

119

SnTin

50

122

SbAntimony

51

128

TeTellurium

52

127

IIodine

53

131

XeXenon

54

133

CsCaesium

55

137

BaBarium

56

139

LaLanthanium

57

178

HfHafnium

72

181

TaTantalum

73

184

WTungsten

74

186

ReRhenium

75

190

OsOsmium

76

192

IrIridium

77

195

PtPlatinum

78

197

AuGold

79

201

HgMercury

80

204

TlThallium

81

207

PbLead

82

209

BiBismuth

83

PoPolonium

84

AtAstatine

85

RnRadon

86

FrFrancium

87

226

RaRadium

88

227

AcActinium

89 +

*58-71 Lanthanoid series

+90-103 Actinoid series

140Ce

Cerium

58

141Pr

Praseodymium

59

144Nd

Neodymium

60

PmPromethium

61

150Sm

Samarium

62

152Eu

Europium

63

157Gd

Gadolinium

64

159Tb

Terbium

65

162Dy

Dysprosium

66

165Ho

Holmium

67

167Er

Erbium

68

169TmThulium

69

173Yb

Ytterbium

70

175Lu

Lutetium

71

Key

a

X

b

a = relative atomic massX = atomic symbol

b = proton (atomic) number

232

ThThorium

90

PaProtactinium

91

238

UUranium

92

NpNeptunium

93

PuPlutonium

94

AmAmericium

95

CmCurium

96

BkBerkelium

97

CfCalifornium

98

EsEinsteinium

99

FmFermium

100

MdMendelevium

101

NoNobelium

102

LrLawrencium

103

The volume of one mole of any gas is 24 dm 3 at room temperature and pressure (r.t.p)

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Four possible answers labelled A, B, C and D are given for each question. Choose the one youconsider to be correct.

1 Fractional distillation is used to separate a mixture of two liquids with boiling points of 68 oCand 105 oC as shown in the diagram below.

Which graph would be obtained if the temperature at point X was plotted against the totalvolume of distillate produced?

A B

C D

4

60

70

8090

100

110

Total volume of distillate

Temperature/ oC

60

70

8090

100

110


Temperature/ oC

60

70

80

90

100

110


Temperature/ oC

60

70

80

90

100

110


Temperature/ oC

Point X


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2 What will be observed if aqueous bromine is added to aqueous sodium chloride?

A A brown solution is observed.

B A gas which bleaches moist litmus paper is observed.

C A white precipitate is observed.D No visible change.

3 Which pair of substances could be separated by mixing with water and filtering?

A NaNO3 and CuSO4B AgCl and CaSO4C MgCO3 and Fe(OH)3D KCl and CuO

4 Substance P contains one or more of the three substances X, Y or Z.

Two chromatograms of the four substances, using different solvents, are shown in the

diagrams below.

What does substance P contain?

A Y and Z

B X and Y

C X, Y and ZD Y only

5 Which oxide produces hydroxide ions when mixed with water?

A Al2O3B K2O

C CO2D SO3

5

Solvent I Solvent II

Solvent

front

Solvent

front

Start lineStart line


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6 What happens when solid citric acid is added to a piece of magnesium ribbon?

A Effervescence is observed

B Heat is liberatedC Citric acid crystals dissolve

D No visible change

7 The ionic equation for the reaction between an aqueous solution of a silver salt and an alkalito give a precipitate of silver hydroxide is:

Ag+ (aq) + OH- (aq) AgOH (s)

What can be deduced from this equation?

A The silver salt is silver nitrate.

B The equation represents a neutralisation reaction.C All silver salts are soluble in water.

D Any alkali can be used in the reaction

8 Which of the following equations best represents the reaction between hydrochloric acid andcopper(II) oxide?

A HCl + CuO CuCl2 + H2OB 2 H+ + CuO Cu2+ + H2O

C 2 H+ + O2- H2OD Cu2+ + 2 Cl- CuCl2

9 When a mixture of sample X and sodium hydroxide was heated, a colourless and pungent gasthat turned moist red litmus paper blue was released.

What can we say about sample X?

A Sample X contains a nitrate salt

B Sample X contains dilute acidC Sample X contains a sulphate salt

D Sample X contains an ammonium salt

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10 An aqueous solution of potassium carbonate was mixed with dilute hydrochloric acid in a

beaker. The mass of the beaker and contents was then recorded at various times. Which of thefollowing graphs depicts the result correctly?

A B

C D

11 There are two unlabelled test tubes. One contains sodium carbonate solution and the other

contains sodium chloride solution. Which test could identify the solutions?

A Add aqueous ammonia

B Add dilute hydrochloric acid

C Add lead(II) nitrate solution

D Add sodium hydroxide solution

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Add excess aqueous NaOH

12 Study the reaction scheme below for a white solid X

What could solid X be?

A lead(II) sulphate

B ammonium chloride

C zinc sulphate

D calcium chloride

13 The relative atomic mass of an element, which consists of two isotopes, 146X and 154X is 152.Find the ratio of the numbers of the lighter to heavier atoms.

A 3:1B 4:1

C 1:4

D 1:3

14 The table below shows the proton numbers of elements W, X, Y and Z.

Element Proton number

W 6

X 9Y 16

Z 19

Which of the following compounds has the highest melting point?

A Y2B WY2C WX4D ZX

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White solid X

Aqueous solution

White

precipitate

White precipitate formed

Colourless solution

add water

Add acidifiedbarium nitrate

solution

Add aqueous

NaOH


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15 X and Y represent symbols of 2 different elements. Which of the following is definitely true

about atom 14X and atom 14Y?

A They have the same number of electrons.

B They have the same number of neutronsC They are isotopes of one another.

D They have different number of proton and neutron

16 Which statement best explains why sodium chloride has a high melting point?

A There are delocalised electrons in the crystalline lattice of sodium chloride.

B The crystalline lattice of sodium chloride contains strong covalent bonds.

C The chemical reaction between elements sodium and chlorine is vigorous.

D There are strong electrostatic forces between sodium ions and chloride ions in thecrystalline lattice of sodium chloride.

17 What substance is represented by the structure shown in the diagram below?

A Diamond

B Silicon(IV) oxideC Graphite

D Solid iodine

18 Oxygen (16O), sulphur (32S), selenium (79Se), tellurium (128Te) are Group VI elements in the

Periodic Table. They form hydrides with different melting and boiling point.

Which of the following hydride molecules is most polar?

A H2OB H2S

C H2Se

D H2Te

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19 Which formula represents a non-polar molecule containing polar covalent bonds?

A HF

B Cl2C CCl4D H2

20 Based on intermolecular forces, which of these substances would have the highest boiling

point?

A He

B CH4C O2

D NH3

21 When copper (II) carbonate is heated strongly, it decomposes to give carbon dioxide and a

black solid, copper(II) oxide.

CuCO3 (s) CuO (s) + CO2 (g)

What is the volume of carbon dioxide produced at r.t.p. when 62.0 g of copper (II) carbonate

is heated?

A 12.0 dm3

B 1.2 dm3

C 24.0 dm3

D 36.0 dm3

22 What is the percentage by mass of water in hydrated copper(II) sulphate, CuSO4.5H2O?

A 7.2 %

B 64 %C 36 %

D 3.6 %

23 Which of the following has the largest number of atoms?

A 0.1 mole of carbon

B 0.2 mole of magnesium

C 0.3 mole of oxygen gasD 0.4 mole of neon gas

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24 A sample of ethane gas is shown below.

Ethane gas burns in oxygen as shown in the equation below:

2 C2H6 (g) + 7 O2 (g) 4 CO2 (g) + 6 H2O (l)

What is the mass of water produced from the combustion of the sample of gas?

A 0.36 g

B 0.72 g

C 1.80 gD 2.16 g

25 The reaction between aqueous copper(II) sulphate and aqueous sodium carbonate can berepresented by the equation

CuSO4 (aq) + Na2CO3 (aq) CuCO3 (s) + Na2SO4 (aq)

In an experiment, 8.0 cm3 of 1.0 mol/dm3 aqueous copper(II) sulphate was mixed with 6.0

cm3 of 1.0 mol/dm3 aqueous sodium carbonate in a beaker. What did the beaker contain whenthe reaction was complete?

A A colourless solution onlyB A green precipitate only

C A green precipitate and a colourless solutionD A green precipitate and a blue solution

26 The following shows some information about elements X and Y.

Atom X has 20 neutrons and nucleon number 39.

Atom Y has an electron arrangement of 2.8.18.18.8.1

Which of the following properties about element X and Y is true?

A Melting point of element Y is higher than that of element X.B Element Y is less dense than element X.

C The reaction between element Y and water is more vigorous than the reaction between

element X and water.D Element Y can conduct electricity, whereas element X cannot.

11

Ethane gas

960 cm3

(r.t.p)


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27 Elements X, Y and Z are located in Group VII of the Periodic Table.

Element Z is more electronegative than element X.

The reaction of red-hot iron wool with gas Y is more vigorous than the reaction of

red-hot iron wool with gas X.

The reactivity of the three elements in ascending order is

A X, Y, Z

B Y, Z, X

C Y, X, ZD Z, X, Y

28 The properties of four elements, AD, are given below. Which of these elements is mostlikely to be a transition element?

Element Property

A has a melting point of 800 oC.

B forms oxides with oxidation states (valencies) of +2 and +3.

C is a non-conductor of electricity in the molten state.

D reacts with water at room temperature to form hydrogen gas.

29 A sample of unpolluted rain water has a pH of about 6. What gas (or gases) cause(s) this pH?

A Sulphur dioxide

B Sulphur dioxide and nitrogen dioxide

C Carbon dioxideD Carbon monoxide

30 Which of the following gases cannot be removed by a catalytic converter?

A Carbon monoxideB Nitrogen dioxide

C Carbon dioxide

D Unburnt hydrocarbon

-- END OF PAPER 1 --

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S3_Chemistry_EOY_08_P1

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