GCE Chemistry Unit 2 - Chemistry In Action Question Paper … · 1 2 3 4 5 6 7 8 9 10 11 Chemistry...

(JUN09CHEM201)APW/Jun09/CHEM2 CHEM2

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For Examiner’s Use

Examiner’s Initial

Centre Number

Surname

Other Names

Candidate Signature

Candidate Number

General Certificate of EducationAdvanced Subsidiary ExaminationJune 2009

Time allowed� 1 hour 45 minutes

Instructions� Use black ink or black ball-point pen.� Fill in the boxes at the top of this page.� Answer all questions.� You must answer the questions in the spaces provided. Answers written

in margins or on blank pages will not be marked.� All working must be shown.� Do all rough work in this book. Cross through any work you do not

want to be marked.� The Periodic Table/Data Sheet is provided as an insert.

Information� The marks for questions are shown in brackets.� The maximum mark for this paper is 100.� Your answers to the questions in Section B should be written in

continuous prose, where appropriate.� You will be marked on your ability to:

– use good English– organise information clearly– use specialist vocabulary where appropriate.

Advice� You are advised to spend about 1 hour 15 minutes on Section A and

about 30 minutes on Section B.

For this paper you must have:� Periodic Table/Data Sheet provided as an insert (enclosed).� a calculator.

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Chemistry CHEM2

Unit 2 Chemistry In Action

Thursday 11 June 2009 1.30 pm to 3.15 pm

APW/Jun09/CHEM2

2 Areas outsidethe box will

not be scannedfor marking

1 Sodium thiosulfate solution (Na2S2O3) reacts slowly with dilute hydrochloric acid to form aprecipitate. The rate of this reaction can be studied by measuring the time (t) that it takes fora small fixed amount of precipitate to form under different conditions. The fixed amount ofprecipitate is taken as the amount needed to obscure a cross on paper.

The equation for this reaction is shown below.

Na2S2O3 + 2HCl → 2NaCl + S + SO2 + H2O

1 (a) Identify the insoluble product of this reaction which forms the precipitate.

.............................................................................................................................................(1 mark)

1 (b) When this reaction takes place, the collision between the reacting particles requires anactivation energy. State what is meant by the term activation energy.

.............................................................................................................................................

.............................................................................................................................................(2 marks)

1 (c) In terms of particles, explain why, at a fixed temperature, you might expect the rate ofthis reaction to double when the concentration of sodium thiosulfate is doubled and theconcentration of hydrochloric acid remains the same.

.............................................................................................................................................

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.............................................................................................................................................(2 marks)

1 (d) (i) State what is meant by the term rate of reaction.

...................................................................................................................................

...................................................................................................................................(1 mark)

(02)

Section A

Answer all the questions in the spaces provided.

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1 (d) (ii) Consider the description of the way in which this experiment is carried out.Use your understanding of the term rate of reaction to explain why it is possibleto use a simplified formula as a measure of the rate of this reaction.

...................................................................................................................................

...................................................................................................................................(1 mark)

Turn over for the next question

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1t

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2 Barium can be extracted from barium oxide (BaO) in a process using aluminium.A mixture of powdered barium oxide and powdered aluminium is heated strongly.The equation for this extraction process is shown below.

3BaO(s) + 2Al(s) → 3Ba(s) + Al2O3(s)

Some standard enthalpies of formation are given in the table below.

Substance BaO(s) Al2O3(s)

∆H / kJ mol–1 –558 –1669

2 (a) (i) State what is meant by the term standard enthalpy of formation.

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................(3 marks)

2 (a) (ii) State why the standard enthalpy of formation of barium and that of aluminiumare both zero.

...................................................................................................................................(1 mark)

2 (a) (iii) Use the data to calculate the standard enthalpy change for the reaction shown bythe equation above.

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................

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...................................................................................................................................(3 marks)

f



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2 (b) (i) Suggest the major reason why this method of extracting barium is expensive.

...................................................................................................................................(1 mark)

2 (b) (ii) Using barium oxide and aluminium powders increases the surface area of thereactants. Suggest one reason why this increases the rate of reaction.

...................................................................................................................................(1 mark)

2 (c) (i) Write an equation for the reaction of barium with water.

...................................................................................................................................(1 mark)

2 (c) (ii) A solution containing barium ions can be used to test for the presence of sulfateions in an aqueous solution of sodium sulfate.

Write the simplest ionic equation for the reaction which occurs and state what isobserved.

Simplest ionic equation

...................................................................................................................................

Observation ..............................................................................................................(2 marks)

2 (c) (iii) State how barium sulfate can be used in medicine. Explain why this use ispossible, given that solutions containing barium ions are poisonous.

Use ............................................................................................................................

Explanation ...............................................................................................................

...................................................................................................................................(2 marks)

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3 A group of students devised an experiment which they believed would enable them toinvestigate the strength of the intermolecular forces between ethyl ethanoate molecules(CH3COOCH2CH3) and trichloromethane molecules (CHCl3).

They mixed exactly 0.10 mol of each of the two liquids in a copper calorimeter and recordedthe following results. The starting temperature of both liquids was the same.

Mass of 0.10 mol of ethyl ethanoate / g 8.80

Mass of 0.10 mol of trichloromethane / g 11.95

Increase in temperature (∆T) on mixing / K 9.5

3 (a) (i) Write an expression for the heat change (q) which relates mass (m), specific heatcapacity (c) and change in temperature (∆T).

...................................................................................................................................(1 mark)

3 (a) (ii) Calculate the amount of heat required to increase the temperature of 8.80 g ofethyl ethanoate by 9.5 K during the mixing process. (You should assume that c for ethyl ethanoate = 1.92 J g–1K–1)

...................................................................................................................................(1 mark)

3 (a) (iii) Calculate the amount of heat required to increase the temperature of 11.95 g oftrichloromethane by 9.5 K during the mixing process. (You should assume that c for trichloromethane = 0.96 J g–1K–1)

...................................................................................................................................(1 mark)

3 (a) (iv) Using the values from parts (a) (ii) and (a) (iii), calculate the molar enthalpychange in kJ mol–1 for the mixing process.

...................................................................................................................................

...................................................................................................................................(2 marks)



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3 (b) The students deduced that the heat change was due only to the formation ofintermolecular forces between ethyl ethanoate molecules and trichloromethanemolecules.

Ignoring all experimental errors, give one reason why the students may have made anincorrect deduction.

.............................................................................................................................................

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4 Carbon monoxide and hydrogen are used in the manufacture of methanol. An equilibrium isestablished according to the following equation.

Cu catalystCO(g) + 2H2(g) CH3OH(g) ∆H = –9l kJ mol–1

4 (a) Give two features of a reaction at equilibrium.

Feature 1 .............................................................................................................................

.............................................................................................................................................

Feature 2 .............................................................................................................................

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4 (b) Explain why an increase in temperature causes a decrease in the equilibrium yield ofmethanol.

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4 (c) (i) State what is meant by the term catalyst.

...................................................................................................................................

...................................................................................................................................(1 mark)

4 (c) (ii) State the effect, if any, of the copper catalyst on the position of this equilibriumat a fixed temperature.

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4 (d) Two methods are used to produce carbon monoxide from natural gas. Equations forthese two methods are shown below.

Method 1 CH4 + H2O → 2CO + 3H2

Method 2 CH4 + CO2 → 2CO + 2H2

The manufacture of methanol from these sources of carbon monoxide has beendescribed as carbon neutral.

4 (d) (i) State what is meant by the term carbon neutral.

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................(1 mark)

4 (d) (ii) Show how combining the equations from these two methods can lead to the 1:2 mol ratio of carbon monoxide to hydrogen required for this synthesis ofmethanol.

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5 This question is about the extraction of metals.

5 (a) Coke is mainly carbon and is a raw material used in the extraction of iron fromiron(III) oxide.

5 (a) (i) Write an equation for the formation of carbon monoxide from carbon.

...................................................................................................................................(1 mark)

5 (a) (ii) Write an equation for the reduction of iron(III) oxide to iron by carbonmonoxide.

...................................................................................................................................(1 mark)

5 (a) (iii) The Earth’s resources of iron(III) oxide are very large and commercial ores havea high iron content. Give one economic and one environmental reason forrecycling scrap iron and steel.

Economic reason ......................................................................................................

...................................................................................................................................

Environmental reason ...............................................................................................

...................................................................................................................................(2 marks)

5 (b) Pure titanium is extracted by the reduction of titanium(IV) chloride, but not by thedirect reduction of titanium(IV) oxide using carbon.

5 (b) (i) Write an equation for the conversion of titanium(IV) oxide into titanium(IV)chloride.

...................................................................................................................................(2 marks)

5 (b) (ii) Write an equation for the extraction of titanium from titanium(IV) chloride.

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5 (b) (iii) State why titanium is not extracted directly from titanium(IV) oxide usingcarbon.

...................................................................................................................................(1 mark)

5 (c) Aluminium is extracted by the electrolysis of a molten mixture containing aluminiumoxide.

5 (c) (i) State why the electrolysis needs to be of a molten mixture.

...................................................................................................................................(1 mark)

5 (c) (ii) Write an equation for the reaction of oxide ions at the positive electrode duringthe electrolysis.

...................................................................................................................................(1 mark)

5 (c) (iii) State why the positive electrodes need frequent replacement.

...................................................................................................................................(1 mark)

5 (c) (iv) Give the major reason why it is less expensive to recycle aluminium than toextract it from aluminium oxide by electrolysis.

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6 Acidified silver nitrate solution can be used to identify and distinguish between halide ionsin solution.

6 (a) Explain why hydrochloric acid should not be used to acidify the silver nitrate.

.............................................................................................................................................

.............................................................................................................................................(1 mark)

6 (b) State and explain what would be observed when acidified silver nitrate solution isadded to a solution of sodium fluoride.

Observation ........................................................................................................................

Explanation ........................................................................................................................(2 marks)

6 (c) State what would be observed when acidified silver nitrate solution is added to asolution containing iodide ions. Write the simplest ionic equation for the reaction thatoccurs.

Observation ........................................................................................................................

Equation .............................................................................................................................(2 marks)

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7 The reaction of bromine with an alkene is used in a test to show that the alkene isunsaturated.

7 (a) State what is meant by the term unsaturated as applied to an alkene.

.............................................................................................................................................(1 mark)

7 (b) Name and outline a mechanism for the reaction of bromine with but-2-ene.

Name of mechanism ..........................................................................................................

Mechanism

(5 marks)

7 (c) But-2-ene can exist as a pair of stereoisomers.

7 (c) (i) State what is meant by the term stereoisomers.

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................(2 marks)

7 (c) (ii) Draw the structure of (E)-but-2-ene.

...................................................................................................................................(1 mark)

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(14)

8 Nucleophiles react with bromoethane in substitution reactions. This type of reaction isillustrated in the following scheme.

8 (a) State what is meant by the term nucleophile.

.............................................................................................................................................(1 mark)

8 (b) Outline a mechanism for the reaction of potassium cyanide with bromoethane(Reaction 1).

(2 marks)

8 (c) Explain why an excess of ammonia is needed in Reaction 2 to produce a high yield ofethylamine.

.............................................................................................................................................

.............................................................................................................................................(1 mark)

CH3CH2CNpropanenitrile

CH3CH2Br

CH3CH2NH2ethylamine

CH3CH2OHethanol

Reaction 1

KCN KOH

Reaction 3

Reaction 2NH3

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8 (d) When potassium hydroxide reacts with bromoethane, ethene can also be formed.Name and outline a mechanism for this reaction.

Name of mechanism ...........................................................................................................

Mechanism

(4 marks)


8





9 Butan-2-ol can be oxidised by acidified potassium dichromate(VI) to form butanone asshown by the following equation.

CH3CH2CH(OH)CH3 + [O] → CH3CH2COCH3 + H2O

9 (a) State the class of alcohol to which butan-2-ol belongs.

.............................................................................................................................................(1 mark)

9 (b) The infrared spectrum shown below is either that of butan-2-ol or that of butanone.

Identify the compound to which this infrared spectrum refers.

Explain your answer.

You may find it helpful to refer to the table of infrared absorption data on the back ofthe Periodic Table (Table 1).

Identity of the compound ...................................................................................................

Explanation ........................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(3 marks)

APW/Jun09/CHEM2(16)

4000 3000 2000Wavenumber / cm–1

1500 1000 500

Transmittance /%

100

50

0

Areas outsidethe box will


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17

9 (c) Draw the displayed formula of the alcohol C4H9OH which is resistant to oxidation byacidified potassium dichromate(VI).

.............................................................................................................................................(1 mark)


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18

10 In the past 150 years, three different processes have been used to extract bromine frompotassium bromide. These processes are illustrated below.

Extraction Process 1

2KBr + MnO2 + 2H2SO4 → MnSO4 + K2SO4 + 2H2O + Br2


The reaction of solid potassium bromide with concentrated sulfuric acid.


The reaction of aqueous potassium bromide with chlorine gas.

10 (a) Write a half-equation for the conversion of MnO2 in acid solution into Mn2+ ions andwater. In terms of electrons, state what is meant by the term oxidising agent andidentify the oxidising agent in the overall reaction.

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APW/Jun09/CHEM2(18)

Section B

Answer both questions in the spaces provided.



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10 (b) Write an equation for Extraction Process 2 and an equation for Extraction Process 3.Calculate the percentage atom economy for the extraction of bromine from potassiumbromide by Extraction Process 3. Suggest why Extraction Process 3 is the method inlarge-scale use today.

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Question 10 continues on the next page

APW/Jun09/CHEM2



10 (c) Bromine has been used for more than 70 years to treat the water in swimming pools.The following equilibrium is established when bromine is added to water.

Br2 + H2O HBrO + HBr

Give the oxidation state of bromine in HBr and in HBrO

Deduce what will happen to this equilibrium as the HBrO reacts with micro-organismsin the swimming pool water. Explain your answer.

.............................................................................................................................................

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.............................................................................................................................................(4 marks)

(20)

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11 One of the first substances used as an anaesthetic in medicine was chloroform(trichloromethane, CHCl3). By 1950, halothane was in common use but by 1990 this hadbeen replaced by more acceptable anaesthetics such as desflurane.

CF3CHBrCl CF3CHFOCHF2halothane desflurane

One reason for replacing halothane was that it is an organic compound that containschlorine. Chlorine-containing organic compounds are thought to cause damage to the ozonelayer in the upper atmosphere.

11 (a) Name and outline a mechanism for the reaction of chlorine with methane to formchloromethane (CH3Cl).

Write an overall equation for the reaction of chlorine with methane to formtrichloromethane (CHCl3).

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Question 11 continues on the next page

APW/Jun09/CHEM2



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11 (b) Explain how chlorine atoms are formed from chlorine-containing organic compoundsin the upper atmosphere.

Explain, with the aid of equations, how chlorine atoms act as a catalyst in thedecomposition of ozone into oxygen.

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(22)



11 (c) Use the formulae of the two anaesthetics, halothane and desflurane, to help to explainwhy desflurane is considered to be a more environmentally acceptable anaestheticthan halothane.

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END OF QUESTIONS

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APW/Jun09/CHEM2

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INSERT TO/APW/Jun09/CHEM2

Tabl

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1 H n

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che

mic

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hift

dat

a

Typ

e of

pro

ton

δ/pp

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RO

H0.

5 –

5.0

RC

H3

0.7

– 1.

2

RN

H2

1.0

– 4.

5

R2C

H2

1.2

– 1.

4

R3C

H1.

4 –

1.6

RC

H2C

l or

Br

3.1

– 4.

2

RC

C2.

1– 2

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HO

RO

C3.

1 –

3.9

H

R4.

5 –

6.0

CH

C

O

RC

O3.

7 –

4.1

C H

9.0

– 10

.0R

OC

H

10.0

– 1

2.0

RO O

C

H

RC

C20

– 5

0

O

CC

5 –

40

OC

50 –

90

alco

hols

,et

hers

or

este

rs

RC O

160

– 18

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ters

or

acid

s

RC O

190

– 22

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dehy

des

or k

eton

es

Cl o

r B

rR

C10

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0

NR

C25

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0

90 –

150

CC

Tabl

e 3

13C

n.m

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hem

ical

shi

ft d

ata

Typ

e of

car

bon

δ

/ppm

CR

N11

0 –

125

110

– 16

0

Tabl

e 1

Infr

ared

abs

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ion

data

Bon

dW

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umbe

r/c

m–1

N

H33

00 –

350

0(a

min

es)

O

H32

30 –

355

0(a

lcoh

ols)

C

H28

50 –

330

0

O

H25

00 –

300

0(a

cids

)

C

N22

20 –

226

0

C

O16

80 –

175

0

C

C16

20 –

168

0

C

O10

00 –

130

0

C

C 7

50 –

110

0

GC

E C

hem

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1

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5

12

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6

14

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7

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8

19

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27

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28

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31

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sp

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32

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35

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39

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103

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nu

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The

Per

iod

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able

of

the

Ele

men

ts

23

.0N

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diu

m

11

39

.1 Kp

ota

ssiu

m

19

40

.1C

acalc

ium

20

45

.0S

cscand

ium

21

47

.9 Ti

tita

niu

m

22

50

.9 Vvanad

ium

23

52

.0C

rchro

miu

m

24

54

.9M

nm

an

gan

ese

25

55

.8Fe iro

n

26

58

.9C

oco

balt

27

58

.7N

inic

kel

28

63

.5C

uco

pp

er

29

65

.4Z

nzin

c

30

69

.7G

ag

alli

um

31

72

.6G

eg

erm

an

ium

32

74

.9A

sars

enic

33

79

.0S

esele

niu

m

34

79

.9B

rb

rom

ine

35

83

.8K

rkry

pto

n

36

85

.5R

bru

bid

ium

37

87

.6S

rstr

ontium

38

88

.9 Yytt

rium

39

91

.2Z

rzirco

niu

m

40

92

.9N

bnio

biu

m

41

96

.0M

om

oly

bd

enu

m

42

[98

]Tc

tech

netiu

m

43

10

1.1

Ru

ruth

eniu

m

44

10

2.9

Rh

rho

diu

m

45

10

6.4

Pd

palla

diu

m

46

10

7.9

Ag

silv

er

47

11

2.4

Cd

cad

miu

m

48

11

4.8

Inin

diu

m

49

11

8.7

Sn

tin

50

12

1.8

Sb

antim

ony

51

12

7.6

Tete

llurium

52

12

6.9 I

iod

ine

53

13

1.3

Xe

xeno

n

54

13

2.9

Cs

caesiu

m

55

13

7.3

Ba

barium

56

13

8.9

La *

lanth

anum

57

17

8.5

Hf

hafn

ium

72

18

0.9

Tata

nta

lum

73

18

3.8

Wtu

ng

ste

n

74

18

6.2

Re

rheniu

m

75

19

0.2

Os

osm

ium

76

19

2.2

Iririd

ium

77

19

5.1

Pt

pla

tinum

78

19

7.0

Au

go

ld

79

20

0.6

Hg

merc

ury

80

20

4.4

Tl

thalli

um

81

20

7.2

Pb

lead

82

20

9.0

Bi

bis

muth

83

[20

9]

Po

po

loniu

m

84

[21

0]

At

asta

tine

85

[22

2]

Rn

rad

on

86

[22

3]

Frfr

anciu

m

87

[22

6]

Ra

rad

ium

88

[22

7]

Ac

†actiniu

m

89

14

0.1

Ce

cerium

58

14

0.9

Pr

pras

eody

miu

m

59

14

4.2

Nd

neo

dym

ium

60

[14

5]

Pm

pro

meth

ium

61

15

0.4

Sm

sam

arium

62

15

2.0

Eu

euro

piu

m

63

15

7.3

Gd

gad

olin

ium

64

15

8.9

Tb

terb

ium

65

16

2.5

Dy

dysp

rosiu

m

66

16

4.9

Ho

ho

lmiu

m

67

16

7.3

Er

erb

ium

68

16

8.9

Tm

thuliu

m

69

17

3.1

Yb

ytt

erb

ium

70

17

5.0

Lulu

tetium

71

23

2.0

Th

tho

rium

90

23

1.0

Pa

pro

tactiniu

m

91

23

8.0

Uura

niu

m

92

[23

7]

Np

nep

tuniu

m

93

[24

4]

Pu

plu

toniu

m

94

[24

3]

Am

am

ericiu

m

95

[24

7]

Cm

curium

96

[24

7]

Bk

berk

eliu

m

97

[25

1]

Cf

calif

orn

ium

98

[25

2]

Es

ein

ste

iniu

m

99

[25

7]

Fmfe

rmiu

m

10

0

[25

8]

Md

men

del

eviu

m

10

1

[25

9]

No

no

beliu

m

10

2

[26

2]

Lrla

wre

nciu

m

10

3

24

.3M

gm

ag

nesiu

m

12

(1)

(2)

(3)

(4)

(5)

(6)

(7)

(8)

(9)

(10)

(11)

(12)

(13)

(14)

(15)

(16)

(17)

(18)

Key

[26

7]

Rf

ruth

erfo

rdiu

m

10

4

[26

8]

Db

dub

niu

m

10

5

[27

1]

Sg

seab

org

ium

10

6

[27

2]

Bh

bo

hrium

10

7

[27

0]

Hs

hassiu

m

10

8

[27

6]

Mt

meitnerium

10

9

[28

1]

Ds

darm

stad

tium

11

0

[28

0]

Rg

roentg

eniu

m

11

1

Ele

men

ts w

ith a

tom

ic n

umb

ers

112-

116

have

bee

n re

por

ted

but

not

fully

aut

hent

icat

ed

GCE Chemistry Unit 2 - Chemistry In Action Question Paper … · 1 2 3 4 5 6 7 8 9 10 11 Chemistry...

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Transcript of GCE Chemistry Unit 2 - Chemistry In Action Question Paper … · 1 2 3 4 5 6 7 8 9 10 11 Chemistry...