chemistry 12 - weebly

Contents: 19 pages Examination: 2 hours 50 multiple-choice questions Additional Time Permitted: 60 minutes © Province of British Columbia

Chemistry 12 Examination Booklet

2009/10 Released Exam January 2010 Form A

DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO.

FOR FURTHER INSTRUCTIONS REFER TO THE RESPONSE BOOKLET.

Chemistry 12 – 1001 Form A Page 1

PART A: MULTIPLE CHOICE Value: 62.5% of the examination

Suggested Time: 80 minutes

INSTRUCTIONS: For each question, select the best answer and record your choice on the Answer Sheet provided. Using an HB pencil, completely fill in the bubble that has the letter corresponding to your answer.

You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,

fill in the bubble as follows.

FA B C D E HGExam Booklet Form/Cahier d’examen

1. Which of the following reactions would you expect to proceed most rapidly

at room temperature? A. Ca s( ) +S s( ) → CaS s( )

B. H2 g( ) + Cl2 g( ) → 2HCl g( )

C. Pb2+ aq( ) + CO32− aq( ) → PbCO3 s( )

D. Br2 ( ) + H2O ( ) → 2Br− aq( ) + 1

2 O2 g( ) + 2H+ aq( )

2. Solid sodium metal reacts rapidly with water in an open beaker to produce aqueous

sodium hydroxide and hydrogen gas. A change in which of the following could be used to measure the rate of this reaction?

A. the volume of the solution B. the pressure of the hydrogen gas C. the concentration of the solid sodium D. the mass of the beaker and its contents

Chemistry 12 – 1001 Form A

3. Consider the following PE diagram:

Progress of reaction

PE(kJ)

500

300

100

400

200

Which of the following is correct for the activated complex?

PE (kJ) Stability

A. 200 low

B. 200 high

C. 500 low

D. 500 high

4. When carbon disulphide reacts with chlorine gas, 238 kJ is released.

Which of the following correctly represent this reaction?

I CS2 g( ) + 3Cl2 g( ) → CCl4 g( ) + S2Cl2 g( ) + 238 kJ

II CS2 g( ) + 3Cl2 g( ) + 238 kJ → CCl4 g( ) + S2Cl2 g( )

III CS2 g( ) + 3Cl2 g( ) → CCl4 g( ) + S2Cl2 g( ) ΔH = +238 kJ

IV CS2 g( ) + 3Cl2 g( ) → CCl4 g( ) + S2Cl2 g( ) ΔH = −238 kJ

A. I and III only B. I and IV only C. II and III only D. II and IV only


5. Consider the following reaction mechanism:

Step 1: 2NO → N2O2

Step 2: N2O2 + H2 → N2O + H2O

Step 3: N2O + H2 → N2 + H2O

Which of the following is correct?

Activated Complex Reaction Intermediate

A. N2O N2O2

B. N2O2 H2O

C. N2OH2 N2O

D. N2O2H2 N2


6. A student places some HI g( ) into a closed reaction container and the following equilibrium is established:

2HI g( ) →← I2 g( ) + H2 g( )

Which of the following describes the forward and reverse reaction rates? A.

reverse

forward

Time

ReactionRate

B.

forward

reverse

Time

ReactionRate

C.

reverse

forward

Time

ReactionRate

D.

forward

reverse

Time

ReactionRate


7. Consider the equilibrium:

H2 g( ) + FeO s( ) →← H2O g( ) + Fe s( )

The following chemicals are placed in separate 1.0 L containers.

Container I H2, H2O

Container II Fe, FeO

Container III H2O, Fe

Container IV H2, H2O, FeO

In which container(s) will the equilibrium be established? A. Container III only B. Container IV only C. Containers I and II only D. Containers III and IV only 8. Consider the following:

energy + 6CO2 g( ) + 6H2O( )

?→← C6H12O6 s( ) + 6O2 g( )

Which of the following describes how enthalpy and entropy change in the forward direction?

Enthalpy Entropy

A. increases decreases

B. increases increases

C. decreases increases

D. decreases decreases


9. Consider the following system at equilibrium:

energy + N2H6CO2 s( ) →← 2NH3 g( ) + CO2 g( )

Which of the following is correct when the volume of the system is increased?

Equilibrium Shift Amount of N2H6CO2

A. left increases

B. left no change

C. right decreases

D. right no change

10. Consider the following system at equilibrium:

2NO g( ) + O2 g( ) →← 2NO2 g( )

Some O2 is added to the equilibrium. Which of the following describes how the

forward and reverse reaction rates change as a new equilibrium is being established?

Forward Rate Reverse Rate

A. increases decreases

B. increases increases

C. decreases increases

D. decreases decreases


11. Consider the following equilibrium:

NH4NO2 s( ) →← N2 g( ) + 2H2O g( )

Which of the following correctly represents the H2O[ ] at equilibrium?

A. H2O[ ] =Keq

N2[ ]

B. H2O[ ] = 12

Keq

N2[ ]⎛⎝⎜

⎞⎠⎟

C. H2O[ ] =Keq NH4NO2[ ]

N2[ ]

D. H2O[ ] =Keq NH4NO2[ ]

N2[ ]

12. Consider the following:

I COCl2 g( ) →← CO g( ) + Cl2 g( ) Keq = 2.2 × 10−10

II 2NO g( ) →← N2 g( ) + O2 g( ) Keq = 2.4 × 103

III 2SO3 g( ) →← 2SO2 g( ) + O2 g( ) Keq = 4.1 × 10−3

Which of the following correctly lists the equilibria in order from most favouring

products to least favouring products? A. I, III, II B. II, I, III C. II, III, I D. III, II, I


13. Consider the equilibrium system:

N2 g( ) + 3Cl2 g( ) →← 2NCl3 g( ) ΔH = +460 kJ

Which of the following describes what happens when some NCl3 is added?

Equilibrium Shift Value of Keq

A. right remains constant

B. right increases

C. left remains constant

D. left decreases

14. Consider the following equilibrium:

2BN s( ) + 3Cl2 g( ) →← 2BCl3 g( ) + N2 g( ) Keq = 1.6 × 10−3

At equilibrium, there were 0.30 mol BN , 0.20 mol BCl3 and 0.10 mol N2 in a 2.0 L container.

How many moles of Cl2 were present? A. 0.31mol

B. 1.4 mol

C. 2.7mol

D. 4.8mol

15. Which solute will result in a molecular solution? A. HCN B. Ba OH( )2

C. CH 3COOH

D. CH 3CH2OH


16. Which best describes the equilibrium in a saturated solution? A. The rate of crystallization determines the solubility. B. The rate of crystallization equals the rate of dissolving. C. There is no solid solute on the bottom of the container. D. The solute is completely dissolved and the equilibrium favours the products. 17. Which compound will have a solubility greater than 0.1M at 25°C ? A. SrS

B. CoS

C. BaSO4

D. Ag2SO4 18. What is the net ionic equation for the reaction between 0.10 M Na2S and 0.10 M Zn NO3( )2 ? A. Zn2+ aq( ) + S2− aq( ) → ZnS s( )

B. Na+ aq( ) + NO3−

aq( ) → NaNO3 s( ) C. Na2S aq( ) + Zn NO3( )2 aq( ) → ZnS s( ) + 2NaNO3 aq( )

D. 2Na+ aq( ) + S2− aq( ) + Zn2+ aq( ) + 2NO3−

aq( ) → ZnS s( ) + 2Na+ aq( ) + 2NO3−

aq( ) 19. Which of the following correctly represents a K sp expression?

A. Ksp = Ag+⎡⎣ ⎤⎦2

S2−⎡⎣ ⎤⎦

B. Ksp =Ba2+⎡⎣ ⎤⎦ NO3

−⎡⎣ ⎤⎦2

Ba NO3( )2⎡⎣

⎤⎦

C. Ksp =CaCO3⎡⎣ ⎤⎦

CO2⎡⎣ ⎤⎦ CaO⎡⎣ ⎤⎦

D. Ksp = 1

Cu2+⎡⎣ ⎤⎦ Cl−⎡⎣ ⎤⎦2


20. What is the solubility of the salt PbSO4 ?

A. 3.2 ×10−16 M

B. 9.0 ×10−9 M

C. 1.8 ×10−8 M

D. 1.3 ×10− 4 M 21. What is the maximum I −[ ] that can exist in a solution with Pb2+[ ] = 8.5 × 10−3 M ? A. 2.0 × 10−6 M

B. 1.0 × 10−6 M

C. 5.0 × 10−4 M

D. 1.0 × 10−3 M

22. Which of the following occurs when a sample of 0.1M HNO3 is tested? A. phenolphthalein turns pink

B. bromthymol blue turns yellow

C. Ca s( ) reacts and produces CO2 g( ) D. Na s( ) reacts and produces NO2 g( ) 23. Given the equilibrium:

HCO3− + NH4

+ →← H2CO3 + NH3

Which species is the Brønsted-Lowry base for the forward reaction? A. NH3

B. NH4+

C. HCO3−

D. H2CO3


24. What is the conjugate acid for NH2− in water?

A. H 3O+

B. NH4+

C. NH3

D. NH2− 25. What is a characteristic common to all strong acids? A. They ionize 100%. B. They are concentrated. C. They only react with strong bases. D. They have strong conjugate bases. 26. Which equation represents the behaviour of a strong Arrhenius base? A. CaO s( ) + H2O( ) → Ca OH( )2 s( )

B. RbOH aq( ) → Rb+ aq( ) + OH− aq( )

C. Co OH( )2

s( ) →← Co2+ aq( ) + 2OH − aq( ) D. Al H2O( )

6

3+aq( ) + H2O( ) →← Al H2O( )

5OH( )2+

aq( ) + H 3O+ aq( )

27. Which of the following equations represents the ionization of water?

A. H2O( ) →← H2 aq( ) + 1

2 O2 aq( )

B. H2O( ) →← H+ aq( ) + OH− aq( )

C. 2H2O( ) →← H3O

+ aq( ) + O2− aq( )

D. H2O( ) + H2O( ) →← H+ aq( ) + OH− aq( )


28. The ionization of water is endothermic. Which of the following is a reasonable value of Kw

if the temperature of water is greater than 25º C ? A. 1.2 × 10−15

B. 0.81 × 10−14

C. 1.0 × 10−14

D. 2.0 × 10−14

29. What is the pOH of 0.25M HNO3 ?

A. 4.0 × 10−14

B. − 0.60

C. 0.60

D. 13.40

30. What is the equilibrium constant expression for the predominant equilibrium in HPO42− aq( )?

A. H3O

+⎡⎣

⎤⎦ PO4

3−⎡⎣ ⎤⎦HPO4

2−⎡⎣ ⎤⎦

B. H2PO4

−⎡⎣ ⎤⎦ OH−⎡⎣ ⎤⎦HPO4

2−⎡⎣ ⎤⎦

C. HPO4

2− aq( ) + H2O( ) →← H2PO4− aq( ) + OH− aq( )

D. HPO4

2− aq( ) + H2O( ) →← H3O+ aq( ) + PO4

3− aq( )


31. Which of the following 0.10 M solutions would have the highest pH? A. H2S

B. HIO3

C. HNO2

D. CH3COOH

32. Which of the following describes the predominant hydrolysis reaction that occurs in KHCO3 aq( ) ?

A. KHCO3 aq( ) →← K+ aq( ) + HCO3− aq( )

B. HCO3

− aq( ) + H2O ( ) →← H3O+ aq( ) + CO32− aq( )

C. CO3

2− aq( ) + H2O ( ) →← HCO3− aq( ) + OH− aq( )

D. HCO3

− aq( ) + H2O ( ) →← H2CO3 aq( ) + OH− aq( )

33. Which of the following represents an acidic salt solution? A. NH3 aq( )

B. NH4Cl aq( )

C. NaNO3 aq( )

D. K2CO3 aq( )

34. A chemical indicator changes colour at its A. titration point. B. transition point. C. equivalence point. D. stoichiometric point.


35. A solution was tested with two indicators and the following results were obtained.

Indicator Colour

chlorophenol red red

phenolphthalein pink

Which of the following could be the approximate pH of the solution? A. 6.0 B. 7.0 C. 9.2 D. 11.7 36. What is the complete ionic equation for the reaction of hydrochloric acid with NaOH aq( )?

A. H+ aq( ) + OH− aq( ) → H2O ( )

B. HCl aq( ) + NaOH aq( ) → NaCl aq( ) + H2O ( )

C. HCl aq( ) + NaOH aq( ) + H2O ( ) → NaCl aq( ) + H3O+ aq( ) + OH− aq( )

D. H+ aq( ) + Cl− aq( ) + Na+ aq( ) + OH− aq( ) → Na+ aq( ) + Cl− aq( ) + H2O ( )

37. Consider the following buffer equilibrium system:

HCN aq( ) + H2O ( ) →← H3O+ aq( ) + CN− aq( )

What is the net result of adding a small amount of HNO3 ? A. The pH increases slightly.

B. The pH decreases slightly.

C. The CN−⎡⎣ ⎤⎦ increases slightly.

D. The HCN⎡⎣ ⎤⎦ decreases slightly.


38. An oxide of which of the following elements will form a solution that acts only as a base? A. P B. N C. Li D. Zn 39. The reduced substance in a chemical reaction can best be described as a substance that A. is the reducing agent and loses electrons. B. is the reducing agent and gains electrons. C. is the oxidizing agent and loses electrons. D. is the oxidizing agent and gains electrons. 40. Consider the following redox equation:

3C3H8O + K2Cr2O7 + 4H2SO4 → 3C3H6O + Cr2 SO4( )3 + K2SO4 + 7H2O

Which species is the oxidizing agent? A. C in C3H8O

B. H in C3H8O

C. O in C3H8O

D. Cr in K2Cr2O7

41. How does the oxidation number of arsenic As( ) change as As4 reacts to form H3AsO4 ? A. It decreases by 5.

B. It increases by 5 4 .

C. It increases by 5.

D. It increases by 20.


42. Tests between metals X, Y and Z and their ions produced the following results:

X + Y+ → no reaction

Y+ + Z → Y + Z+

Which of the following describes the relative strengths of the oxidizing agents? A. X > Y > Z

B. Z > Y > X

C. X+ > Y+ > Z+

D. Z+ > Y+ > X+ 43. The following skeletal equation can be balanced in acidic solution:

As2O3 → AsH3 Which of the following appear in the balanced equation?

Electrons Water

A. 3e− 32

H2O

B. 6e− 3H2O

C. 9e− 32

H2O

D. 12e− 3H2O

44. A solution of H2O2 is titrated with KMnO4 aq( ) according to the redox equation shown below:

5H2O2 + 2MnO4− + 6H+ → 5O2 + 2Mn2+ + 8H2O

A 10.00 mL sample of H2O2 is reacted with 13.5mL of 0.0241M KMnO4 .

What is the molarity of the H2O2 solution? A. 0.0130 M

B. 0.0325 M

C. 0.0346 M

D. 0.0813 M


45. Consider the following diagram of a standard electrochemical cell:

1.

0 M KNO

3

Metal ZMetal X

1.0 M X(NO3)2 1.0 M Z(NO3)2

Voltse–e–

Which of the following is correct as the cell operates?

Metal Z Anion Migration

A. anode towards Metal X

B. anode towards Metal Z

C. cathode towards Metal X

D. cathode towards Metal Z


Use the following diagram to answer questions 46, 47 and 48.

1.0 M HCl 1.0 M AgNO3

Ag

H2(g)

Pt (inert)

Volts

PorousBarrier

46. What is the cathode half-cell reaction?

A. Ag → Ag+ + e−

B. Ag+ + e− → Ag

C. 2H+ + 2e− → H2

D. 2Cl− + 2e− → Cl2

47. Which of the following is correct as the cell operates?

Direction of Ag+ Migration

pH Near the Pt Electrode

A. towards Pt increases

B. towards Pt decreases

C. towards Ag increases

D. towards Ag decreases


48. Which of the following is correct as the cell operates?

Direction of Electron Flow Mass of Pt Electrode

A. from Ag to Pt increases

B. from Ag to Pt decreases

C. from Pt to Ag decreases

D. from Pt to Ag does not change

49. An iron pipeline can be protected from rusting by connecting it to A. a zinc nitrate solution. B. a silver nitrate solution. C. the positive terminal of a direct current power supply. D. the negative terminal of a direct current power supply. 50. Which of the following is the anode half-cell reaction for molten KBr ?

A. K → K+ + e−

B. K+ + e− → K

C. 2Br− → Br2 + 2e−

D. H2O → 2e− + 2H+ + 12 O2

You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,

ensure that you have filled in the bubble as follows.

FA B C D E HGExam Booklet Form/Cahier d’examen

This is the end of the multiple-choice section. Answer the remaining questions in the Response Booklet.

Chemistry 12 Data Page 1

Bas

ed o

n m

ass

of C

12 a

t 12.

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Valu

es in

par

enth

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able

or

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isot

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for

elem

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whi

ch d

o no

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ally

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PER

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AB

LE

OF

TH

E E

LE

ME

NT

S

12

34

56

78

910

1112

1314

1516

1718

4 Be

Bery

llium

9.0

11 Na

Sodi

um

23.0

12 Mg

Mag

nesi

um

24.3

19 KPo

tass

ium

39.1

20 Ca

Cal

cium

40.1

37 Rb

Rub

idiu

m

85.5

55 Cs

Ces

ium

132.

9

56 Ba

Bariu

m

137.

3

87 Fr

Fran

cium

(223

)

88 Ra

Rad

ium

(226

)

21 Sc

S can

dium

45.0

2 2 Ti

Tita

n ium

47.9

39 YYt

trium

88.9

40 Zr

Zirc

o niu

m

91.2

57 La

L ant

hanu

m

1 38.

9

7 2 Hf

Haf

n ium

178.

5

89 Ac

Actin

ium

(227

)

104

Rf

Rut

her fo

rdiu

m

(26 1

)

23 VVa

nadi

um

50.9

24 Cr

Chr

omiu

m

52.0

41 Nb

Nio

bium

92.9

42 Mo

Mol

ybde

num

95.9

73 TaTa

ntal

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180.

9

74 WTu

ngst

en

183.

8

105

Db

Dub

nium

(262

)

106

Sg

Seab

orgi

um

(263

)

25 Mn

Man

gane

se

54.9

26 Fe

Iron

55.8

43 Tc

Tech

netiu

m

(98)

44 Ru

Rut

heni

um

101.

1

75 Re

Rhe

nium

186.

2

76 Os

Osm

ium

190.

2

107

Bh

Bohr

ium

(262

)

108

Hs

Has

sium

(265

)

27 Co

Cob

alt

5 8.9

45 Rh

Rh o

dium

1 02.

9

77 IrIr i

dium

1 92.

2

1 09

Mt

Me i

tner

ium

(266

)

28 Ni

Nick

e l

58. 7

78 Pt

Plat

inu m

195 .

1

29 Cu

Cop

per

63.5

47 Ag

Silve

r

107.

9

79 Au

Gol

d

197.

0

30 Zn

Zinc

65.4

48 Cd

Cad

miu

m

112.

4

80 Hg

Mer

cury

200.

6

5 B Boro

n

10.8

13 Al

Alum

inum

27.0

31 Ga

Gal

lium

69.7

49 In Indi

um

114.

8

81 Tl

Thal

lium

204.

4

6 CC

arbo

n

12.0

14 Si

Silic

on

28.1

32 Ge

Ger

man

ium

72.6

50 Sn

Tin

118.

7

82 Pb

Lead

207.

2

7 NN

itrog

en

14. 0

1 5 PPh

osp h

orus

31.0

3 3 As

Ars e

nic

74.9

5 1 Sb

Antim

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121.

8

8 3 Bi

Bism

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209.

0

8 OO

xyge

n

16.0

16 SSu

lphu

r

32.1

34 Se

Sele

nium

79.0

52 TeTe

lluri u

m

127.

6

84 Po

Polo

nium

(209

)

9 FFl

uorin

e

19.0

17 Cl

Chl

orin

e

35.5

35 Br

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ine

79.9

53 IIo

dine

126.

9

85 At

Asta

tine

(210

)

10 Ne

Neo

n

20.2

18 Ar

Argo

n

39.9

36 Kr

Kryp

ton

83.8

54 Xe

Xeno

n

131.

3

86 Rn

Rad

on

(222

)

2 He

Hel

ium

4.0

58 Ce

Cer

i um

140.

1

90 Th

Thor

ium

232.

0

59 Pr

Pras

eody

miu

m

140.

9

91 Pa

Prot

actin

ium

231.

0

60 Nd

Neo

dym

ium

144.

2

92 UU

rani

um

238.

0

61 Pm

Prom

ethi

um

(145

)

93 Np

Nep

tuni

um

(237

)

62 Sm

Sam

ariu

m

1 50.

4

94 Pu

Plu t

oniu

m

(244

)

63 Eu

Euro

pium

152.

0

95 Am

Amer

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m

(243

)

64 Gd

Gad

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157.

3

96 Cm

Cur

ium

(247

)

65 Tb

Terb

ium

158.

9

97 Bk

Berk

eliu

m

(247

)

66 Dy

Dys

pros

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162.

5

98 Cf

Cal

iforn

ium

(251

)

67 Ho

Hol

miu

m

164.

9

99 Es

E ins

tein

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(252

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6 8 Er

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3

100

Fm

Ferm

ium

(25 7

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69 Tm

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168.

9

101

Md

Men

dele

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(258

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70 Yb

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173.

0

102

No

Nob

eliu

m

(259

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71 Lu

Lute

tium

175.

0

103

Lr

Law

renc

ium

(262

)

1 HH

ydro

gen

1.0

46 Pd

Palla

dium

106 .

4

38 Sr

Stro

ntiu

m

87.6

3 Li

Lith

ium

6.9

14

Si

Si

li

co

n

28.1

Ato

mic

Num

ber

Sym

bol

Nam

eA

tom

ic M

ass

14 Si

Silic

on

28.1

Data Page 2 Chemistry 12

ATOMIC MASSES OF THE ELEMENTSBased on mass of C12 at 12.00.

Values in parentheses are the mass number of the most stable or bestknown isotopes for elements that do not occur naturally.

ActiniumAluminumAmericiumAntimonyArgonArsenicAstatineBariumBerkeliumBerylliumBismuthBoronBromineCadmiumCalciumCaliforniumCarbonCeriumCesiumChlorineChromiumCobaltCopperCuriumDubniumDysprosiumEinsteiniumErbiumEuropiumFermiumFluorineFranciumGadoliniumGalliumGermaniumGoldHafniumHeliumHolmiumHydrogenIndiumIodineIridiumIronKryptonLanthanumLawrenciumLeadLithiumLutetiumMagnesiumManganeseMendelevium

AcAlAmSbArAsAtBaBkBeBiBBrCdCaCfCCeCsClCrCoCuCmDbDyEsErEuFmFFrGdGaGeAuHfHeHoHInIIrFeKrLaLrPbLiLuMgMnMd

89 13 95 51 18 33 85 56 97 4 83 5 35 48 20 98 6 58 55 17 24 27 29 96 105 66 99 68 63 100 9 87 64 31 32 79 72 2 67 1 49 53 77 26 36 57 103 82 3 71 12 25 101

(227) 27.0 (243) 121.8 39.9 74.9 (210) 137.3 (247) 9.0 209.0 10.8 79.9 112.4 40.1 (251) 12.0 140.1 132.9 35.5 52.0 58.9 63.5 (247) (262) 162.5 (252) 167.3 152.0 (257) 19.0 (223) 157.3 69.7 72.6 197.0 178.5 4.0 164.9 1.0 114.8 126.9 192.2 55.8 83.8 138.9 (262) 207.2 6.9 175.0 24.3 54.9 (258)

MercuryMolybdenumNeodymiumNeonNeptuniumNickelNiobiumNitrogenNobeliumOsmiumOxygenPalladiumPhosphorusPlatinumPlutoniumPoloniumPotassiumPraseodymiumPromethiumProtactiniumRadiumRadonRheniumRhodiumRubidiumRutheniumRutherfordiumSamariumScandiumSeleniumSiliconSilverSodiumStrontiumSulphurTantalumTechnetiumTelluriumTerbiumThalliumThoriumThuliumTinTitaniumTungstenUraniumVanadiumXenonYtterbiumYttriumZincZirconium

HgMoNdNeNpNiNbNNoOsOPdPPtPuPoKPrPmPaRaRnReRhRbRuRfSmScSeSiAgNaSrSTaTcTeTbTlThTmSnTiWUVXeYbYZnZr

804260109328417

102768

461578948419596191888675453744

10462213414471138167343526581906950227492235470393040

200.6 95.9 144.2 20.2 (237) 58.7 92.9 14.0 (259) 190.2 16.0 106.4 31.0 195.1 (244) (209) 39.1 140.9 (145) 231.0 (226) (222) 186.2 102.9 85.5 101.1 (261) 150.4 45.0 79.0 28.1 107.9 23.0 87.6 32.1 180.9 (98) 127.6 158.9 204.4 232.0 168.9 118.7 47.9 183.8 238.0 50.9 131.3 173.0 88.9 65.4 91.2

Element Symbol Atomic Number

AtomicMass Element Symbol Atomic

NumberAtomicMass

Chemistry 12 Data Page �

NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air.** Not stable in aqueous solutions.

Negative Ions(Anions)

Po s i t i v e I o n s( C a t i o n s )

Aluminum

Ammonium

Barium

Calcium

Chromium(II), chromous

Chromium(III), chromic

Copper(I)*, cuprous

Copper(II), cupric

Hydrogen

Hydronium

Iron(II)*, ferrous

Iron(III), ferric

Lead(II), plumbous

Al3+

NH4+

Ba2+

Ca2+

Cr2+

Cr3+

Cu+

Cu2+

H+

H3O+

Fe2+

Fe3+

Pb2+

Hydroxide

Hypochlorite

Iodide

Monohydrogen phosphate

Nitrate

Nitrite

Oxalate

Oxide**

Perchlorate

Permanganate

Phosphate

Sulphate

Sulphide

Sulphite

Thiocyanate

OH–

ClO–

I–

HPO42–

NO3–

NO2–

C2O42–

O2–

ClO4–

MnO4–

PO4?–

SO42–

S2–

SO32–

SCN–

Bromide

Carbonate

Chlorate

Chloride

Chlorite

Chromate

Cyanide

Dichromate

Dihydrogen phosphate

Ethanoate, acetate

Fluoride

Hydrogen carbonate, bicarbonate

Hydrogen oxalate, binoxalate

Hydrogen sulphate, bisulphate

Hydrogen sulphide, bisulphide

Hydrogen sulphite, bisulphite

Br–

CO32–

ClO3–

Cl–

ClO2–

CrO42–

CN–

Cr2O72–

H2PO4–

CH3COO–

F–

HCO3–

HC2O4–

HSO4–

HS–

HSO3–

Lead(IV), plumbic

Lithium

Magnesium

Manganese(II), manganous

Manganese(IV)

Mercury(I)*, mercurous

Mercury(II), mercuric

Potassium

Silver

Sodium

Tin(II)*, stannous

Tin(IV), stannic

Zinc

Pb4+

Li+

Mg2+

Mn2+

Mn4+

Hg22+

Hg2+

K+

Ag+

Na+

Sn2+

Sn4+

Zn2+

Data Page � Chemistry 12

SOLUBILITY OF COMMON COMPOUNDS IN WATER

The term soluble here means > 0.1 mol/L at 25°C.

Negative Ions(Anions)

Positive Ions(Cations)

Solubility ofCompounds

All

All

All

Soluble

Soluble

Soluble

All Soluble

Soluble

Low Solubility

All others

Soluble

Low Solubility

Soluble

Low Solubility

Soluble

Low Solubility

Soluble

Low Solubility

All others

All others

All others

All others

or

or

or

or

14243

14253

123

123

123

Alkali ions: Li+, Na+, K+, Rb+, Cs+, Fr+

Ammonium ion: NH4+

Chloride, Cl–

Bromide, Br–

Iodide, I–

Nitrate, NO3–

Hydrogen ion: H+

Ag+, Pb2+, Cu+

Sulphide, S2–Alkali ions, H+, NH4

+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+

Sulphate, SO42–

Hydroxide, OH–Alkali ions, H+, NH4

+, Sr2+ ?

Sulphite, SO32–

Phosphate, PO43–

Carbonate, CO32–

Alkali ions, H+, NH4+

Ag+, Ca2+, Sr2+, Ba2+, Pb2+


SOLUBILITY PRODUCT CONSTANTS AT 25°C

Name Formula

Barium carbonate

Barium chromate

Barium sulphate

Calcium carbonate

Calcium oxalate

Calcium sulphate

Copper(I) iodide

Copper(II) iodate

Copper(II) sulphide

Iron(II) hydroxide

Iron(II) sulphide

Iron(III) hydroxide

Lead(II) bromide

Lead(II) chloride

Lead(II) iodate

Lead(II) iodide

Lead(II) sulphate

Magnesium carbonate

Magnesium hydroxide

Silver bromate

Silver bromide

Silver carbonate

Silver chloride

Silver chromate

Silver iodate

Silver iodide

Strontium carbonate

Strontium fluoride

Strontium sulphate

Zinc sulphide

BaCO3

BaCrO4

BaSO4

CaCO3

CaC2O4

CaSO4

CuI

Cu(IO3)2

CuS

Fe(OH)2

FeS

Fe(OH)3

PbBr2

PbCl2

Pb(IO3)2

PbI2

PbSO4

MgCO3

Mg(OH)2

AgBrO3

AgBr

Ag2CO3

AgCl

Ag2CrO4

AgIO3

AgI

SrCO3

SrF2

SrSO4

ZnS

2.6 10–9

1.2 10–10

1.1 10–10

5.0 10–9

2.3 10–9

7.1 10–5

1.3 10–12

6.9 10–8

6.0 10–37

4.9 10–17

6.0 10–19

2.6 10–39

6.6 10–6

1.2 10–5

3.7 10–13

8.5 10–9

1.8 10–8

6.8 10–6

5.6 10–12

5.3 10–5

5.4 10–13

8.5 10–12

1.8 10–10

1.1 10–12

3.2 10–8

8.5 10–17

5.6 10–10

4.3 10–9

3.4 10–7

2.0 10–25

K sp


Perchloric HClO H ClO

Hydriodic HI H I

Hydrobromic HBr H Br

Hydrochloric HCl H Cl

Nitric HNO H NO

Sulphuric H SO H HSO

4 4

3 3

2 4 4

→ +

→ +

→ +

→ +

→ +

→ +

+ −

+ −

+ −

+ −

+ −

+ −

very large

very large

very large

very large

very large

very large

Hydronium Ion H O H H O

Iodic HIO H IO

Oxalic H C O H HC O

Sulphurous SO H O H SO H HSO

Hydrogen sulphate ion HSO H SO

3 2

3 31

2 2 4 2 42

2 2 2 3 32

4 42 2

1 0

1 7 10

5 9 10

1 5 10

1 2 10

+ +

+ − −

+ − −

+ − −

− + − −

→← +→← + ×→← + ×

+( ) →← + ×→← + ×

.

.

.

.

.

Phosphoric H PO H H PO

Hexaaquoiron ion iron ion Fe H O H Fe H O OH

Citric H C H O H H C H O

Nitrous HNO H NO

Hydrofluoric HF

III

3 4 2 43

2 63

2 52 3

3 6 5 7 2 6 5 74

2 24

7 5 10

6 0 10

7 1 10

4 6 10

→← + ×

( ) →← + ( ) ( ) ×→← + ×→← + ×

+ − −

+ + + −

+ − −

+ − −

.

, .

.

.

( )

→→← + ×+ − −H F 3 5 10 4.

Methanoic formic HCOOH H HCOO

Hexaaquochromium ion chromium ion Cr H O H Cr H O OH

Benzoic C H COOH H C H COO

Hydrogen oxalate ion HC O H C O

Ethanoic acetic

III

, .

, .

.

.

,

( )

→← + ×

( ) →← + ( ) ( ) ×→← + ×→← + ×

+ − −

+ + + −

+ − −

− + − −

1 8 10

1 5 10

6 5 10

6 4 10

4

2 63

2 52 4

6 5 6 55

2 4 2 42 5

CHCH COOH H CH COO3 351 8 10→← + ×+ − −.

Dihydrogen citrate ion H C H O H HC H O

Al H O H Al H O OH

Carbonic CO H O H CO H HCO

Monohydrogen citrate ion HC H O H

2 6 5 7 6 5 72 5

2 63

2 52 5

2 2 2 3 37

6 5 72

1 7 10

1 4 10

4 3 10

− + − −

+ + + −

+ − −

− +

→← + ×

( ) →← + ( ) ( ) ×

+( ) →← + ×→←

.

.

.

Hexaaquoaluminum ion, aluminum ion

++ ×→← + ×

− −

− + − −

C H O

Hydrogen sulphite ion HSO H SO

6 5 73 7

3 32 7

4 1 10

1 0 10

.

.

Hydrogen sulphide H S H HS

Dihydrogen phosphate ion H PO H HPO

Boric H BO H H BO

Ammonium ion NH H NH

Hydrocyanic HCN H CN

28

2 4 42 8

3 3 2 310

4 310

10

9 1 10

6 2 10

7 3 10

5 6 10

4 9 10

→← + ×→← + ×→← + ×→← + ×→← + ×

+ − −

− + − −

+ − −

+ + −

+ − −

.

.

.

.

.

Phenol C H OH H C H O

Hydrogen carbonate ion HCO H CO

Hydrogen peroxide H O H HO

Monohydrogen phosphate ion HPO H PO

Water H O H OH

Hydroxide ion OH

6 5 6 510

3 32 11

2 2 212

42

43 13

214

1 3 10

5 6 10

2 4 10

2 2 10

1 0 10

→← + ×→← + ×→← + ×→← + ×→← + ×

+ − −

− + − −

+ − −

− + − −

+ − −

−

.

.

.

.

.

←← +

← +

+ −

+ −

H O very small

Ammonia NH H NH very small

2

3 2

RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASESin aqueous solution at room temperature.

Name of Acid Base Acid Ka

ST

RO

NG

WE

AK

ST

RO

NG

WE

AK

ST

RE

NG

TH

OF

AC

IDS

TR

EN

GT

H O

F B

AS

E


ACID-BASE INDICATORS

Indicator

yellow to blue

red to yellow

red to yellow

red to yellow

yellow to blue

red to yellow

yellow to red

yellow to blue

yellow to red

red to amber

yellow to blue

colourless to pink

colourless to blue

yellow to red

blue to yellow

Methyl violet

Thymol blue

Orange IV

Methyl orange

Bromcresol green

Methyl red

Chlorophenol red

Bromthymol blue

Phenol red

Neutral red

Thymol blue

Phenolphthalein

Thymolphthalein

Alizarin yellow

Indigo carmine

pH Range in WhichColour Change Occurs

Colour Changeas pH Increases

0.0 – 1.6

1.2 – 2.8

1.4 – 2.8

3.2 – 4.4

3.8 – 5.4

4.8 – 6.0

5.2 – 6.8

6.0 – 7.6

6.6 – 8.0

6.8 – 8.0

8.0 – 9.6

8.2 – 10.0

9.4 – 10.6

10.1 – 12.0

11.4 – 13.0


F g e F

S O e SO

H O H e H O

MnO H e Mn H O

Au e Au s

2

2 82

42

2 2 2

42

23

2 2 2 87

2 2 2 01

2 2 2 1 78

8 5 4 1 51

3 1 50

( ) + →← +

+ →← +

+ + →← +

+ + →← + +

+ →← ( ) +

− −

− − −

+ −

− + − +

+ −

.

.

.

.

.

BrO H e Br H O

ClO H e Cl H O

Cl g e Cl

Cr O H e Cr H O

O g H e

312 2 2

4 2

2

2 72 3

2

12 2

6 5 3 1 48

8 8 4 1 39

2 2 1 36

14 6 2 7 1 23

2 2

− + −

− + − −

− −

− + − +

+ −

+ + →← ( ) + +

+ + →← + +

( ) + →← +

+ + →← + +

( ) + + →

l .

.

.

.

←← +H O2 1 23.

MnO s H e Mn H O

IO H e I s H O

Br e Br

AuCl e Au s Cl

NO H e NO g H

22

2

312 2 2

2

4

3 2

4 2 2 1 22

6 5 3 1 20

2 2 1 09

3 4 1 00

4 3 2

( ) + + →← + +

+ + →← ( ) + +

( ) + →← +

+ →← ( ) + +

+ + →← ( ) +

+ − +

− + −

− −

− − −

− + −

.

.

.

.

l

OO +0 96.

Fe e Fe

O g H e H O

MnO H O e MnO s OH

I s e I

Cu e Cu s

3 2

2 2 2

4 2 2

2

0 77

2 2 0 70

2 3 4 0 60

2 2 0 54

0 52

+ − +

+ −

− − −

− −

+ −

+ →← +

( ) + + →← +

+ + →← ( ) + +

( ) + →← +

+ →← ( ) +

.

.

.

.

.

H SO H e S s H O

Cu e Cu s

SO H e H SO H O

Cu e Cu

Sn e Sn

2 3 22

42

2 3 22

4 2

4 4 3 0 45

2 0 34

4 2 0 17

0 15

2 0 15

+ + →← ( ) + +

+ →← ( ) +

+ + →← + +

+ →← +

+ →← +

+ −

+ −

− + −

+ − +

+ − +

.

.

.

.

.

S s H e H S g

H e H g

Pb e Pb s

Sn e Sn s

Ni e Ni s

( ) + + →← ( ) +

+ →← ( ) +

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

+ −

+ −

+ −

+ −

+ −

2 2 0 14

2 2 0 00

2 0 13

2 0 14

2 0 26

2

22

2

2

.

.

.

.

.

H PO H e H PO H O

Co e Co s

Se s H e H Se

Cr e Cr

H O e H OH M

3 4 3 3 22

23 2

2 27

2 2 0 28

2 0 28

2 2 0 40

0 41

2 2 2 10 0 41

+ + →← + −

+ →← ( ) −

( ) + + →← −

+ →← −

+ →← + ( ) −

+ −

+ −

+ −

+ − +

− − −

.

.

.

.

.

Fe e Fe s

Ag S s e Ag s S

Cr e Cr s

Zn e Zn s

Te s H e H Te

2

22

3

2

2

2 0 45

2 2 0 69

3 0 74

2 0 76

2 2 0 79

+ −

− −

+ −

+ −

+ −

+ →← ( ) −

( ) + →← ( ) + −

+ →← ( ) −

+ →← ( ) −

( ) + + →← −

.

.

.

.

.

2 2 2 0 83

2 1 19

3 1 66

2 2 37

2 71

2 22

3

2

H O e H g OH

Mn e Mn s

Al e Al s

Mg e Mg s

Na e Na s

+ →← ( ) + −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

− −

+ −

+ −

+ −

+ −

.

.

.

.

.

Ca e Ca s

Sr e Sr s

Ba e Ba s

K e K s

Rb e Rb s

2

2

2

2 2 87

2 2 89

2 2 91

2 93

2 98

+ −

+ −

+ −

+ −

+ −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

.

.

.

.

.

Cs e Cs s

Li e Li s

+ −

+ −

+ →← ( ) −

+ →← ( ) −

3 03

3 04

.

.

Hg e Hg

O g H M e H O

NO H e N O H O

Ag e Ag s

Hg e Hg

2

12 2

72

3 2 4 2

12 2

2

2 0 85

2 10 2 0 82

2 4 2 2 0 80

0 80

0 80

+ −

+ − −

− + −

+ −

+ −

+ →← ( ) +

( ) + ( ) + →← +

+ + →← + +

+ →← ( ) +

+ →← ( ) +

l

l

.

.

.

.

.

STANDARD REDUCTION POTENTIALS OF HALF-CELLSIonic concentrations are at 1M in water at 25°C.

Reducing AgentsOxidizing AgentsS

TR

ON

GW

EA

KS

TR

ON

GW

EA

K

Overpotential Effect

Overpotential Effect

ST

RE

NG

TH

OF

OX

IDIZ

ING

AG

EN

TS

TR

EN

GT

H O

F R

ED

UC

ING

AG

EN

TE° Volts( )

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Instructions:

AnswerthefollowingquestionsinthespaceprovidedinthisResponse Booklet.Youareexpectedtocommunicateyourknowledgeandunderstandingofchemicalprinciplesinaclearandlogicalmanner.YourstepsandassumptionsleadingtoasolutionmustbewritteninthisResponse Booklet.Answersmustincludeunitswhereappropriateandbegiventothecorrectnumberofsignificantfigures.For questions involving calculations, full marks will NOT be given for providing only an answer.

Chemistry 12 – 1001 Response Booklet Page 1

PART B: WRITTEN RESPONSE Value: 37.5% of the examination

Suggested Time: 40 minutes

1. (4 marks)

Consider the following reaction mechanism:

Step 1 HBr + O2 → HOOBr slow

Step 2 HOOBr + HBr → 2HOBr fast

Step 3 2 HOBr + HBr → H2O + Br2( ) fast

Overall Reaction

Write the equation for the overall reaction. Given that the overall reaction is exothermic,

sketch a PE diagram for the mechanism on the axis provided.

Reaction time

PE(kJ)

Chemistry 12 – 1001 Response Booklet

2. (4 marks)

Consider the following equilibrium:

2H2 g( ) + S2 g( ) →← 2H2S g( )

Initially, 9.0 × 10−4 mol S2 and 1.1 × 10−2mol H2S are placed in a 1.0 L container.

At equilibrium, there is 8.6 × 10−3mol H2S present. Calculate Keq .


3. (4 marks)

Will a precipitate form when 10.0 mL of 1.0 M Pb NO3( )2 is mixed with 40.0 mL of

2.0 × 10−2M NaCl ? Justify your answer.


4. (3 marks)

For the reactant pair KHC 2O4 and Na2HPO4 , write the net ionic equation for the predominant

equilibrium that will be established. Predict whether the equilibrium will favour reactants or

products and explain why.


5. (5 marks)

Calculate the initial concentration of an NH4NO3 salt solution that has a pH = 4.70 .

Begin by writing the equation for the predominant equilibrium reaction.


6. (3 marks)

A 10.00 mL sample of H 2SO4 is titrated with 0.50 M KOH in three separate trials

and the results are tabulated below.

Trial Volume of 0.50 M KOH

1 20.30 mL

2 19.10 mL

3 18.90 mL

Calculate the concentration of the H 2SO4 .


7. (4 marks)

Balance the following redox equation in acidic solution:

ClO4− + I2 + H2PO4

− → Cl2 + IPO4 (acidic)


8. (3 marks)

Consider the electrolysis of an ionic solution as shown in the diagram.

Pt(inert)

Ionic Solution

DC Power Source

Cu

e–e–

Bubbles appear around the inert electrode and a shiny metal coating appears on the copper electrode. Give an example of one of the possible ionic solutions that could be used. Provide a set of corresponding half reactions which would explain these results.

Ionic Solution: Half-reaction at the Pt electrode: Half-reaction at the Cu electrode:

Version 0601.1


A B C,

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Question 1


1. PlaceyourPersonalEducationNumber(PEN)labelatthetopofthisBookletANDfillinthebubble(FormA,B,C,D,E,F,GorH)thatcorrespondstotheletteronyourExaminationBooklet.

2. UseapenciltofillinbubbleswhenansweringquestionsonyourAnswerSheet.

3. Useapencilorblue-orblack-inkpenwhenansweringwritten-responsequestionsinthisBooklet.

4. ReadtheExaminationRulesonthebackofthisBooklet.

Course Code = CH 12

Chemistry 122009/10 Released Exam

JANUARY 2010

Response Booklet



12

MINISTRY USE ONLY

Examination Rules

1.Thetimeallottedforthisexaminationistwohours.Youmay,however,takeupto60minutesofadditionaltimetofinish.

2.AnswersenteredintheExaminationBookletwillnotbemarked.

3.Cheatingonanexaminationwillresultinamarkofzero.TheMinistryofEducationconsiderscheatingtohaveoccurredifstudentsbreakanyofthefollowingrules:

• Studentsmustnotbeinpossessionoforhaveusedanysecureexaminationmaterialspriortotheexaminationsession.


• Studentsmustnotgiveorreceiveassistanceofanykindinansweringanexaminationquestionduringanexamination,includingallowingtheirpaperstobeviewedbyothersorcopyinganswersfromanotherstudent’spaper.

• Studentsmustnotpossessanybook,paperoritemthatmightassistinwritinganexamination,includingadictionaryorpieceofelectronicequipment,thatisnotspecificallyauthorizedfortheexaminationbyministrypolicy.

• Studentsmustnotcopy,plagiarizeorpresentastheirown,workdonebyanyotherperson.

• Studentsmustimmediatelyfollowtheinvigilator’sordertostopwritingattheendoftheexaminationtimeandmustnotalteranExaminationBooklet,ResponseBookletorAnswerSheetaftertheinvigilatorhasaskedstudentstohandinexaminationpapers.

• Studentsmustnotremoveanypieceoftheexaminationmaterialsfromtheexaminationroom,includingworkpages.

4.Theuseofinappropriatelanguageorcontentmayresultinamarkofzerobeingawarded.

5.Uponcompletionoftheexamination,returnallexaminationmaterialstothesupervisinginvigilator.


PlacePersonalEducationNumber(PEN)here. PlacePersonalEducationNumber(PEN)here.

Instructions:

AnswerthefollowingquestionsinthespaceprovidedinthisResponse Booklet.Youareexpectedtocommunicateyourknowledgeandunderstandingofchemicalprinciplesinaclearandlogicalmanner.YourstepsandassumptionsleadingtoasolutionmustbewritteninthisResponse Booklet.Answersmustincludeunitswhereappropriateandbegiventothecorrectnumberofsignificantfigures.For questions involving calculations, full marks will NOT be given for providing only an answer.

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