chemistry...chemistry 115 2002 higher school certificate examination – 2 – section i 75 marks...

General Instructions

• Reading time – 5 minutes

• Working time – 3 hours

• Write using black or blue pen

• Draw diagrams using pencil

• Board-approved calculators maybe used

• A data sheet and a Periodic Tableare provided at the back of thispaper

• Write your Centre Number andStudent Number at the top ofpages 9, 13, 17 and 21

Total marks – 100

Pages 2–23

75 marks

This section has two parts, Part A and Part B

Part A – 15 marks

• Attempt Questions 1–15

• Allow about 30 minutes for this part

Part B – 60 marks

• Attempt Questions 16–27

• Allow about 1 hour and 45 minutes for this part

Pages 25–30

25 marks

• Attempt ONE question from Questions 28–32

• Allow about 45 minutes for this section

Section II

Section I

Chemistry

115

2002H I G H E R S C H O O L C E R T I F I C AT E

E X A M I N AT I O N

– 2 –

Section I75 marks

Part A – 15 marksAttempt Questions 1–15Allow about 30 minutes for this part

Use the multiple-choice answer sheet.

Select the alternative A, B, C or D that best answers the question. Fill in the response ovalcompletely.

Sample: 2 + 4 = (A) 2 (B) 6 (C) 8 (D) 9

A B C D

If you think you have made a mistake, put a cross through the incorrect answer and fill in thenew answer.

A B C D

If you change your mind and have crossed out what you consider to be the correct answer, thenindicate the correct answer by writing the word correct and drawing an arrow as follows.

correct

A B C D

1 Which conditions would be best for the fermentation of sugars by yeast?

(A) Low oxygen concentration and a temperature between 25°C and 35°C

(B) High oxygen concentration and a temperature between 25°C and 35°C

(C) Low oxygen concentration and a temperature between 45°C and 60°C

(D) High oxygen concentration and a temperature between 45°C and 60°C

2 What is the catalyst for the conversion of ethanol to ethene?

(A) NaOH

(B) H2SO4

(C) HNO3

(D) Pt

3 Which explanation best describes why an understanding of electrolysis has made asignificant impact on the production of materials?

(A) Electrolysis reactions do not require an energy source.

(B) Electrolysis can be used to split water into hydrogen and oxygen.

(C) Electrolysis provides a way to make non-spontaneous reactions occur.

(D) Electrolysis can be used to produce aluminium.

4 Which statement concerning galvanic cells is correct?

(A) Oxidation occurs at the anode.

(B) They are also known as electrolytic cells.

(C) The cathode is assigned a negative charge.

(D) An external power source must be present.

5 What arrangement of an electrolytic cell would electroplate a silver coin with copper?

Electrolyte

copper sulfate

silver nitrate

silver nitrate

copper sulfate

Anode

silver coin

copper

silver coin

copper

Cathode

copper

silver coin

copper

silver coin

(A)

(B)

(C)

(D)

– 3 –

6 Which is amphiprotic?

(A) H2SO4

(B) NH4+

(C) HCO3–

(D) SO42–

7 What did the Brönsted–Lowry definition of acids identify that made it a significantimprovement over earlier definitions?

(A) Acids contain hydrogen.

(B) Acids are proton donors.

(C) Acids contain oxygen.

(D) Acids are electron-pair acceptors.

8 In a titration, an acid of known concentration is placed in a burette and reacted with abase that has been pipetted into a conical flask.

What should each piece of glassware be rinsed with immediately before the titration?

Conical flask

water

water

base

base

Pipette

base

water

base

water

Burette

acid

water

acid

water

(A)

(B)

(C)

(D)

Burette (acid)

Pipette (transfers base to conical flask)

Conical flask (base)

– 4 –

9 The following list of steps refers to an experimental plan for making an ester in a flask.Some of the steps in the list may NOT be required for this experiment. The steps are NOTin the correct sequence.

1. Heat the mixture under reflux.

2. Add three drops of concentrated sulfuric acid.

3. Add 1 mL of ethanol.

4. Add 1 mL of ethene.

5. Add 1 mL of ethanoic acid.

6. Distil the mixture.

7. Add three drops of phenolphthalein indicator.

Which alternative is the best sequence for making an ester?

(A) 3, 5, 7, 1

(B) 4, 3, 7, 6

(C) 5, 4, 2, 6

(D) 5, 3, 2, 1

10 Which equation represents esterification?

CH3—CH2—O—C—H + H2OCH3—OH + CH3—C—OH(C)

O

H—C—ONa + CH3—OH

O

CH3—O—C—H + NaOH(B)

CH3—OH + CH3—C—OH(D)

O O

CH3—O—C—CH3 + H2OH+

H+

(A)

O O

CH3—O—C—CH3 + H2O CH3—OH + CH3—C—OH

OOH+

– 5 –

11 A car engine burns fuel with insufficient air. Which substance would be emitted in theexhaust in higher levels than from an engine with a correct fuel to air ratio?

(A) Carbon dioxide

(B) Carbon monoxide

(C) Oxygen

(D) Water

12 Oxides of nitrogen are produced by the combustion of coal. The percentage of thesecompounds remaining in emissions can be reduced using the methods named in thegraph.

Which of the following is the most effective method for removing oxides of nitrogenproduced by the combustion of coal?

(A) Low nitrogen oxide burners

(B) Reburning technologies

(C) Ammonia-injecting scrubbers

(D) Selective catalytic scrubbers

0

10

20

30

40

50

60

70

80

90

100

Reburningtechnologies

Ammonia-injectingscrubbers

Low nitrogen

oxide burners

Selectivecatalyticscrubbers

Oxides of nitrogen

remaining in emissions

(%)

– 6 –

13 The Haber Process for producing ammonia was developed early in the twentieth century.What was the major advantage of its development?

(A) A government sold the process to other governments.

(B) The inventor sold the process for a great deal of money.

(C) It provided a source of nitrogen for farming and industry.

(D) It provided jobs for many who were unemployed.

14 Ammonia is produced from hydrogen and nitrogen, according to the equation:

N2(g) + 3H2(g) 2NH3(g)

The graph shows the yield of ammonia produced at 200°C and 100 kPa.

Which graph shows a correct comparison of the yield of ammonia produced at atemperature of 400°C and 100 kPa with the yield produced at 200°C and 100 kPa?

Yield ofammonia

Time

200°C

400°C

(A)

Yield ofammonia

Time

200°C

400°C

(B)

(C) (D)

Yield ofammonia

Time

200°C

400°C

Time

200°C

400°C

Yield ofammonia

200°CYield ofammonia

Time

– 7 –

15 The table gives the results of chemical tests for some cations and anions.

(ppt = precipitate)

When a group of students performed the above tests on an unknown solution theyobtained the following results:

Which conclusion is consistent with these results?

(A) The sample contained both CaCl2 and BaCl2.

(B) The sample contained both CaCl2 and PbCl2.

(C) The sample contained both FeCl3 and PbCl2.

(D) The sample contained both FeCl3 and BaCl2.

Add0.1 M AgNO3

white ppt

Add0.1 M Na2CO3

white ppt

Add0.1 M KSCN

no change

Add cold0.1 M HCl

no change

Add0.1 M AgNO3

no change

no change

no change

no change

white ppt

Add0.1 M Na2CO3

white ppt

brown ppt

white ppt

white ppt

no change

Add0.1 M KSCN

no change

red colour

no change

no change

no change

Add cold0.1 M HCl

no change

no change

no change

white ppt

no change

Ion

Ca2+

Fe3+

Ba2+

Pb2+

Cl–

– 8 –

© Board of Studies NSW 2002

Section I (continued)

Part B – 60 marksAttempt Questions 16–27Allow about 1 hour and 45 minutes for this part

Answer the questions in the spaces provided.

Show all relevant working in questions involving calculations.

MarksQuestion 16 (6 marks)

You have carried out a first-hand investigation to compare the reactivity of an alkenewith its corresponding alkane.

(a) State the name of the alkene.

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(b) Outline a procedure to compare the reactivity of this alkene with itscorresponding alkane.

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(c) Describe the results obtained from this first-hand investigation and includerelevant chemical equations.

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3

2

1

2002 HIGHER SCHOOL CERTIFICATE EXAMINATION

Chemistry

– 9 –116

Centre Number

Student Number

Question 17 (3 marks)

Explain why alkanes and their corresponding alkenes have similar physical properties,but very different chemical properties.

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3

– 10 –

Marks


(a) Name the type of polymerisation shown in the following reaction:

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(b) Assess current developments in the use of biopolymers.

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5

O OC

O

C

O

OCH2 CH2 + H2O

+ n HOHO OHC

O

C

O

CH2 CH2 OHn

n

1

– 11 –

Marks

BLANK PAGE


– 12 –

Section I – Part B (continued)


(a) Describe the conditions under which a nucleus is unstable.

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Question 19 continues on page 14

2


Chemistry

– 13 –117

Centre Number

Student Number

Question 19 (continued)

(b) The following is a flow diagram showing the sequence of products releasedduring the decay of uranium.

Use examples from the flow diagram to describe processes by which an unstableisotope undergoes radioactive decay.

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End of Question 19

82 84 86 88 90 92

206

214

222

230

238

Pb

Po

Rn

Ra

Th

PaTh U

U

Po

Po

Bi

BiPb

Pb

Mas

s nu

mbe

r

Atomic number

3

– 14 –

Marks


(a) Identify ONE common household base.

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

(b) A student used indicators to determine whether three colourless solutions wereacidic or basic. The indicators used are shown in the table.

Samples of each solution were tested with the indicators. The colours of theresulting solutions are shown in the table.

The student concluded that each of the three solutions tested was basic. Assessthe validity of this conclusion.

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Colour ofsolution C

yellow

yellow

yellow

red

Colour ofsolution B

yellow

yellow

blue

red

Colour ofsolution A

yellow

yellow

blue

purple

Indicator added

Methyl orange

Methyl red

Thymol blue

Alizarin

pH range

3.2–4.4

4.8–6.0

8.0–9.6

11.0–12.4

Colour change

red to yellow

red to yellow

yellow to blue

red to purple

Indicator

Methyl orange

Methyl red

Thymol blue

Alizarin

3

1

– 15 –

Marks


Evaluate the impact of industrial sources of sulfur dioxide and nitrogen oxides on theenvironment, making use of appropriate chemical equations.

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7

– 16 –

Marks




Solutions of hydrochloric acid, acetic acid and sulfuric acid were prepared. Each ofthe solutions had the same concentration (0.01 mol L–1). The pH of the acetic acidsolution was 3.4.

(a) Calculate the pH of the hydrochloric acid solution.

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(b) Compare the pH of the sulfuric acid solution to the pH of the hydrochloric acidsolution. Justify your answer. (No calculations are necessary.)

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(c) Explain why the acetic acid solution has a higher pH than the hydrochloric acidsolution.

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2

2

1

0.01 mol L−1

acetic acid

pH = 3.4

0.01 mol L−1

sulfuric acid0.01 mol L−1

hydrochloricacid


Chemistry

– 17 –118

Centre Number

Student Number


A bottle of soft drink was placed on an electronic balance and weighed. The cap wasremoved and placed next to the bottle on the balance. The mass of the cap, bottle andits contents was monitored. The results are shown in the graph. The experiment wasconducted at 25°C and 101.3 kPa. Assume that no evaporation has occurred.

(a) Identify the gas released.

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(b) Calculate the volume of the gas released.

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3

1

615

620

625

630

Time

Mass of cap, bottle and contents (g)

– 18 –

Marks


Assess the impact of atomic absorption spectroscopy (AAS) on the scientificunderstanding of the effects of trace elements.

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4

– 19 –

Marks

BLANK PAGE


– 20 –



(a) What is the systematic name of the CFC in the diagram?

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(b) Identify the bonding within ozone, using a Lewis electron-dot diagram.

(c) Discuss how CFCs damage the ozone layer, using relevant equations.

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3

2

C C FF

ClCl

FF

1


Chemistry

– 21 –119

Centre Number

Student Number


Water can be described as either ‘hard’ or ‘soft’.

(a) Describe a test you have used to determine whether a given sample of water is‘hard’ or ‘soft’.

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(b) A sample of hard water contains 6 × 10–4 mol L–1 of magnesium carbonate.

Calculate the mass, in mg, of magnesium carbonate in 150 mL of this sample.

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3

2

– 22 –

Marks


Describe the physical and chemical processes needed to purify and sanitise a townwater supply.

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5

– 23 –

Marks

BLANK PAGE


– 24 –

Section II

25 marksAttempt ONE question from Questions 28–32Allow about 45 minutes for this section

Answer the question in a writing booklet. Extra writing booklets are available.

Show all relevant working in questions involving calculations.

Page

Question 28 Industrial Chemistry ................................................................... 26

Question 29 Shipwrecks and Salvage ............................................................ 27

Question 30 The Biochemistry of Movement ................................................ 28

Question 31 The Chemistry of Art ................................................................. 29

Question 32 Forensic Chemistry .................................................................... 30


Chemistry

– 25 –120

Question 28 — Industrial Chemistry (25 marks)

(a) (i) Define saponification.

(ii) Account for the cleaning action of soap.

(b) One of the reactions used to form sulfuric acid is the reaction of oxygen withsulfur dioxide under equilibrium conditions to form sulfur trioxide.

Before the reaction, the concentration of sulfur dioxide was 0.06 mol L−1 andthe concentration of oxygen was 0.05 mol L−1. After equilibrium was reached,the concentration of sulfur trioxide was 0.04 mol L−1.

Calculate the equilibrium constant, K, for the reaction. Show relevant working.

(c) (i) Use a chemical equation to describe what happens when sulfuric acid isadded to water in a laboratory.

(ii) Describe the use of sulfuric acid as an oxidising agent, as a dehydratingagent and as a means of precipitating sulfates. Use chemical equations toillustrate your answer.

(d) During your practical work, you performed a first-hand investigation involvingan equilibrium reaction.

(i) Outline the procedure you used.

(ii) Explain how you analysed the equilibrium reaction qualitatively.

(e) Evaluate changes in industrial production methods for sodium hydroxide. 6

4

2

3

2

4

3

1

– 26 –

Marks

Question 29 — Shipwrecks and Salvage (25 marks)

(a) (i) Name the type of electrochemical cell that produces a spontaneousreaction.

(ii) Calculate the voltage required to operate the cell shown in the diagram asan electrolytic cell, showing relevant half-equations in your working.

(b) Describe how the work of early scientists increased our understanding ofelectron transfer reactions.

(c) (i) Name ONE method for removing salt from an artefact recovered from awreck.

(ii) Explain, using an example, chemical procedures used to clean andpreserve artefacts from wrecks.

(d) During your practical work you performed a first-hand investigation to compareand describe the rate of corrosion of materials in different acidic and neutralsolutions.

(i) Outline the procedure used.

(ii) It is hypothesised that acidic environments accelerate the corrosion ofshipwrecks.

Explain how data obtained from the procedure in part (d) (i) does or doesnot support this hypothesis.

(e) Analyse the effect of ocean depth on corrosion of metallic objects. 6

4

2

4

1

4

Fe2+

(1 mol L−1)Cu2+

(1 mol L−1)

CopperIron

Salt bridgeV

3

1

– 27 –

Marks

Question 30 — The Biochemistry of Movement (25 marks)

(a) (i) To what class of compounds do these molecules belong?

(ii) Using the two compounds in part (a) (i), describe the formation of apeptide bond, illustrating your answer with a chemical equation. Clearlyindicate the peptide bond.

(b) Explain why triacylglycerols (TAGs) are an important energy store for humans.

(c) (i) Name the acid that builds up in muscles in anaerobic respiration.

(ii) Discuss the characteristics of muscle cells used for light exercise andthose of muscle cells used for heavy exercise.

(d) During your practical work you performed a first-hand investigation todemonstrate the effect of various factors on the reaction of a named enzyme.

(i) Name the enzyme and outline the procedure used to demonstrate theeffect of ONE of these factors on the reaction.

(ii) Explain how the results obtained from the experiment in part (d) (i) canbe used to indicate changes in the structure of the enzyme investigated.

(e) Discuss the oxidation of fatty acids as an inhibitor of the conversion of pyruvateto acetyl CoA, with reference to the dietary needs of sprinting athletes.

6

4

2

4

1

4

3

H—N—C—C—O—H

H CH3

H

O

H—N—C—C—O—H

H H

H

O

1

– 28 –

Marks

Question 31 — The Chemistry of Art (25 marks)

(a) (i) Identify the metal ion that will produce a yellow colour in a flame test.

(ii) Explain how some metal ions produce a characteristic colour in a flame.

(b) Using an example from medicine or biological research, describe the bondingin a coordination complex.

(c) (i) Explain what is meant by a reflectance spectrum.

(ii) Outline how infrared light and ultraviolet light are used to determine thechemical composition of pigments.

(d) During your practical work you performed a first-hand investigation to determinethe oxidising strength of potassium permanganate.

(i) State the electronic configuration of manganese in terms of subshells.

(ii) Outline the procedure used to determine the oxidising strength ofpotassium permanganate.

(iii) Using your results from the procedure in part (d) (ii), justify a conclusionabout the oxidising strength of potassium permanganate. Usehalf-equations in your answer.

(e) Analyse trends in the physical properties of the first transition series. 6

3

2

1

3

2

4

3

1

– 29 –

Marks

Question 32 — Forensic Chemistry (25 marks)

(a) (i) Identify the functional group in glycerol.

(ii) Compare the reactions of both glycerol and 1-propanol when they reactwith cold dilute KMnO4.

(b) Discuss the value of electron spectroscopy and scanning tunnelling microscopyin the analysis of small samples in forensic chemistry.

(c) (i) What class of compounds is used to break proteins into fragments ofdifferent lengths?

(ii) Describe the processes of electrophoresis and chromatography inseparating organic compounds.

(d) During your practical work you performed a first-hand investigation to describethe emission spectrum of sodium.

(i) Name the piece of equipment you used to analyse the emission spectrumof sodium in the laboratory.

(ii) Outline the procedure that you used in this investigation.

(iii) Explain how the emission spectrum was produced.

(e) Discuss the uses of DNA analysis in forensic chemistry.

End of paper

6

3

2

1

4

1

4

3

1

– 30 –

Marks

BLANK PAGE

– 31 –

BLANK PAGE


– 32 –

– 33 –

DATA SHEET

K+ + e– K(s) –2.94 V

Ba2+ + 2e– Ba(s) –2.91 V

Ca2+ + 2e– Ca(s) –2.87 V

Na+ + e– Na(s) –2.71 V

Mg2+ + 2e– Mg(s) –2.36 V

Al3+ + 3e– Al(s) –1.68 V

Mn2+ + 2e– Mn(s) –1.18 V

H2O + e– 1–2 H2(g) + OH– –0.83 V

Zn2+ + 2e– Zn(s) –0.76 V

Fe2+ + 2e– Fe(s) –0.44 V

Ni2+ + 2e– Ni(s) –0.24 V

Sn2+ + 2e– Sn(s) –0.14 V

Pb2+ + 2e– Pb(s) –0.13 V

H+ + e– 1–2 H2(g) 0.00 V

SO42– + 4H+ + 2e– SO2(aq) + 2H2O 0.16 V

Cu2+ + 2e– Cu(s) 0.34 V

1–2 O2(g) + H2O + 2e– 2OH– 0.40 V

Cu+ + e– Cu(s) 0.52 V

1–2 I2(s) + e– I– 0.54 V

1–2 I2(aq) + e– I– 0.62 V

Fe3+ + e– Fe2+ 0.77 V

Ag+ + e– Ag(s) 0.80 V

1–2 Br2(l) + e– Br– 1.08 V

1–2 Br2(aq) + e– Br– 1.10 V

1–2 O2(g) + 2H+ + 2e– H2O 1.23 V

1–2 Cl2(g) + e– Cl– 1.36 V

1–2 Cr2O72– + 7H+ + 3e– Cr3+ + 7–2 H2O 1.36 V

1–2 Cl2(aq) + e– Cl– 1.40 V

MnO4– + 8H+ + 5e– Mn2+ + 4H2O 1.51 V

1–2 F2(g) + e– F– 2.89 V

Avogadro’s constant, NA ............................................................... 6.022 × 1023 mol–1

Volume of 1 mole ideal gas: at 101.3 kPa (1.00 atm) andat 273 K (0°C) ........................... 22.41 Lat 298 K (25°C) ......................... 24.47 L

Ionisation constant for water at 298 K (25°C), Kw ...................... 1.0 × 10–14

Specific heat capacity of water ..................................................... 4.18 × 103 J kg–1 K–1

Some useful formulaepH = –log10 [H+] ∆H = –m C ∆T

Some standard potentials


Chemistry

Aylward and Findlay, SI Chemical Data (4th Edition) is the principal source of data forthis examination paper. Some data may have been modified for examination purposes.120a

– 34 –

1179 F

19.0

0Fl

uori

ne

17 Cl

35.4

5C

hlor

ine

35 Br

79.9

0B

rom

ine

53 I12

6.9

Iodi

ne

85 At

[210

.0]

Ast

atin

e

1157 N

14.0

1N

itrog

en

15 P30

.97

Phos

phor

us

33 As

74.9

2A

rsen

ic

51 Sb12

1.8

Ant

imon

y

83 Bi

209.

0B

ism

uth

1135 B

10.8

1B

oron

13 Al

26.9

8A

lum

iniu

m

31 Ga

69.7

2G

alliu

m

49 In11

4.8

Indi

um

81 Tl

204.

4T

halli

um

107

Bh

[264

.1]

Boh

rium

108

Hs

[265

.1]

Has

sium

109

Mt

[268

]M

eitn

eriu

m

110

Uun —

Unu

nnili

um

111

Uuu —

Unu

nuni

um

112

Uub —

Unu

nbiu

m

114

Uuq —

Unu

nqua

dium

116

Uuh —

Unu

nhex

ium

118

Uuo —

Unu

noct

ium

87 Fr[2

23.0

]Fr

anci

um

88 Ra

[226

.0]

Rad

ium

89–1

03

Act

inid

es

104

Rf

[261

.1]

Rut

herf

ordi

um

105

Db

[262

.1]

Dub

nium

106

Sg[2

63.1

]Se

abor

gium

57 La

138.

9L

anth

anum

89 Ac

[227

.0]

Act

iniu

m

1 H1.

008

Hyd

roge

n

Sym

bol o

f el

emen

t

Nam

e of

ele

men

t

PE

RIO

DIC

TA

BL

E O

F T

HE

EL

EM

EN

TS

KE

Y

2 He

4.00

3H

eliu

m

3 Li

6.94

1L

ithiu

m

4 Be

9.01

2B

eryl

lium

Ato

mic

Num

ber

Ato

mic

Wei

ght

79 Au

197.

0G

old

6 C12

.01

Car

bon

8 O16

.00

Oxy

gen

10 Ne

20.1

8N

eon

11 Na

22.9

9So

dium

12 Mg

24.3

1M

agne

sium

14 Si28

.09

Silic

on

16 S32

.07

Sulf

ur

18 Ar

39.9

5A

rgon

19 K39

.10

Pota

ssiu

m

20 Ca

40.0

8C

alci

um

21 Sc44

.96

Scan

dium

22 Ti

47.8

7T

itani

um

23 V50

.94

Van

adiu

m

24 Cr

52.0

0C

hrom

ium

25 Mn

54.9

4M

anga

nese

26 Fe55

.85

Iron

27 Co

58.9

3C

obal

t

28 Ni

58.6

9N

icke

l

29 Cu

63.5

5C

oppe

r

30 Zn

65.3

9Z

inc

32 Ge

72.6

1G

erm

aniu

m

34 Se78

.96

Sele

nium

36 Kr

83.8

0K

rypt

on

37 Rb

85.4

7R

ubid

ium

38 Sr87

.62

Stro

ntiu

m

39 Y88

.91

Yttr

ium

40 Zr

91.2

2Z

irco

nium

41 Nb

92.9

1N

iobi

um

42 Mo

95.9

4M

olyb

denu

m

43 Tc

[98.

91]

Tech

netiu

m

44 Ru

101.

1R

uthe

nium

45 Rh

102.

9R

hodi

um

46 Pd10

6.4

Palla

dium

47 Ag

107.

9Si

lver

48 Cd

112.

4C

adm

ium

50 Sn11

8.7

Tin

52 Te12

7.6

Tellu

rium

54 Xe

131.

3X

enon

55 Cs

132.

9C

aesi

um

56 Ba

137.

3B

ariu

m

57–7

1

Lan

than

ides

72 Hf

178.

5H

afni

um

73 Ta18

0.9

Tant

alum

74 W18

3.8

Tun

gste

n

75 Re

186.

2R

heni

um

76 Os

190.

2O

smiu

m

77 Ir19

2.2

Irid

ium

78 Pt19

5.1

Plat

inum

79 Au

197.

0G

old

80 Hg

200.

6M

ercu

ry

82 Pb20

7.2

Lea

d

84 Po[2

10.0

]Po

loni

um

86 Rn

[222

.0]

Rad

on

58 Ce

140.

1C

eriu

m

59 Pr14

0.9

Pras

eody

miu

m

60 Nd

144.

2N

eody

miu

m

61 Pm[1

46.9

]Pr

omet

hium

62 Sm 150.

4Sa

mar

ium

63 Eu

152.

0E

urop

ium

64 Gd

157.

3G

adol

iniu

m

65 Tb

158.

9Te

rbiu

m

66 Dy

162.

5D

yspr

osiu

m

67 Ho

164.

9H

olm

ium

68 Er

167.

3E

rbiu

m

69 Tm

168.

9T

huliu

m

70 Yb

173.

0Y

tterb

ium

71 Lu

175.

0L

utet

ium

90 Th

232.

0T

hori

um

91 Pa23

1.0

Prot

actin

ium

92 U23

8.0

Ura

nium

93 Np

[237

.0]

Nep

tuni

um

94 Pu[2

39.1

]Pl

uton

ium

95 Am

[241

.1]

Am

eric

ium

96 Cm

[244

.1]

Cur

ium

97 Bk

[249

.1]

Ber

keliu

m

98 Cf

[252

.1]

Cal

ifor

nium

99 Es

[252

.1]

Ein

stei

nium

100

Fm[2

57.1

]Fe

rmiu

m

101

Md

[258

.1]

Men

dele

vium

102

No

[259

.1]

Nob

eliu

m

103

Lr

[262

.1]

Law

renc

ium

Act

inid

es

Lan

than

ides

Whe

re th

e at

omic

wei

ght i

s no

t kno

wn,

the

rela

tive

atom

ic m

ass

of th

e m

ost c

omm

on r

adio

activ

e is

otop

e is

sho

wn

in b

rack

ets.

The

ato

mic

wei

ghts

of

Np

and

Tc

are

give

n fo

r th

e is

otop

es 23

7 Np

and

99T

c.

chemistry...chemistry 115 2002 higher school certificate examination – 2 – section i 75 marks...

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