chemistry standard level paper 1 - ib documents past papers - subject... · 2019. 11. 7. ·...

ChemistryStandard levelPaper 1

13 pages

Wednesday 8 November 2017 (afternoon)

45 minutes

N17/4/CHEMI/SPM/ENG/TZ0/XX

© International Baccalaureate Organization 20178817 – 6104

Instructions to candidates

• Do not open this examination paper until instructed to do so.• Answer all the questions.• For each question, choose the answer you consider to be the best and indicate your choice on

the answer sheet provided.• The periodic table is provided for reference on page 2 of this examination paper.• The maximum mark for this examination paper is [30 marks].

88 Ra

(226

)

56 Ba

137.

33

38 Sr87

.62

20 Ca

40.0

8

12 Mg

24.3

1

4 Be

9.012

‡†

89 ‡

Ac

(227

)

57 †

La13

8.91

39 Y88

.91

21 Sc 44.9

6

90 Th23

2.04

58 Ce

140.

12

72 Hf

178.

49

40 Zr 91.2

2

22 Ti47

.87

91 Pa23

1.04

59 Pr14

0.91

73 Ta18

0.95

41 Nb

92.9

1

23 V50

.94

92 U23

8.03

60 Nd

144.

24

74 W18

3.84

42 Mo

95.9

6

24 Cr

52.0

0

55 Cs

132.

91

37 Rb

85.4

7

19 K39

.10

11 Na

22.9

9

3 Li 6.941 H 1.011 Fr87 (223

)

93 Np

(237

)

61 Pm (145

)

75 Re

186.

21

43 Tc (98)25 Mn

54.9

4

94 Pu (244

)

62 Sm15

0.36

76 Os

190.

23

44 Ru

101.

07

26 Fe 55.8

5

95 Am

(243

)

63 Eu15

1.96

77 Ir19

2.22

45 Rh

102.

91

27 Co

58.9

3

96 Cm

(247

)

64 Gd

157.

25

78 Pt19

5.08

46 Pd10

6.42

28 Ni

58.6

9

97 Bk

(247

)

65 Tb15

8.93

79 Au

196.

97

47 Ag

107.

87

29 Cu

63.5

5

The

Perio

dic

Tabl

e

Ato

mic

num

ber

Elem

ent

Rel

ativ

e at

omic

mas

s

98 Cf

(251

)

66 Dy

162.

50

80 Hg

200.

59

48 Cd

112.

41

30 Zn 65.3

8

99 Es (252

)

67 Ho

164.

93

81 Tl20

4.38

49 In11

4.82

31 Ga

69.7

2

13 Al

26.9

8

5 B10

.81

13

100

Fm (257

)

68 Er16

7.26

82 Pb 207.

2

50 Sn11

8.71

32 Ge

72.6

3

14 Si28

.09

6 C12

.01

14

101

Md

(258

)

69 Tm16

8.93

83 Bi

208.

98

51 Sb12

1.76

33 As

74.9

2

15 P30

.97

7 N14

.01

15

102

No

(259

)

70 Yb17

3.05

84 Po (209

)

52 Te12

7.60

34 Se78

.96

16 S32

.07

8 O16

.00

16

103

Lr (262

)

71 Lu17

4.97

85 At

(210

)

53 I12

6.90

35 Br

79.9

0

17 Cl

35.4

5

9 F19

.00

17

86 Rn

(222

)

54 Xe13

1.29

36 Kr

83.9

0

18 Ar

39.9

5

10 Ne

20.1

8

2 He

4.0018

34

56

78

910

1112

1 2 3 4 5 6 710

4 R

f(2

67)

105

Db

(268

)

106

Sg (269

)

107

Bh

(270

)

108

Hs

(269

)

109

Mt

(278

)

110

Ds

(281

)

111

Rg

(281

)

112

Cn

(285

)

113

Unt

(286

)

114

Uug

(289

)

115

Uup

(288

)

116

Uuh

(293

)

117

Uus

(294

)

118

Uuo

(294

)

– 2 – N17/4/CHEMI/SPM/ENG/TZ0/XX

1. How many atoms of nitrogen are there in 0.50 mol of (NH4)2CO3?

A. 1

B. 2

C. 3.01 × 1023

D. 6.02 × 1023

2. What is the value of x when 32.2 g of Na2SO4·xH2O are heated leaving 14.2 g of anhydrous Na2SO4? Mr (H2O) = 18; Mr (Na2SO4) = 142.

Na2SO4·xH2O (s) → Na2SO4 (s) + xH2O (g)

A. 0.1

B. 1

C. 5

D. 10

3. How many grams of sodium azide, NaN3, are needed to produce 68.1 dm3 of N2 (g) at STP?

Molar volume at STP = 22.7 dm3 mol-1; Mr (NaN3) = 65.0

2NaN3 (s) → 3N2 (g) + 2Na (s)

A. 32.5

B. 65.0

C. 130.0

D. 195.0

4. Whatisthesumofthecoefficientswhenthefollowingequationisbalancedusingthesmallestwholenumbers?

__C6H12O6(aq)→ __C2H5OH(aq)+ __CO2 (g)

A. 4

B. 5

C. 9

D. 10

Turn over


5. Whatisthenumberofprotonsandthenumberofneutronsin131I?

Protons Neutrons

A. 53 78

B. 53 131

C. 78 53

D. 131 53

6. Whichistheelectronconfigurationofachromiumatominthegroundstate?

A. [Ne]3s23p64s13d4

B. [Ar]3d3

C. 1s22s22p63s23p64s23d4

D. [Ar]4s13d5

7. Which trends are correct across period 3 (from Na to Cl)?

I. Atomic radius decreasesII. Melting point increasesIII. First ionization energy increases

A. I and II only

B. I and III only

C. II and III only

D. I, II and III


8. WhichoxidedissolvesinwatertogiveasolutionwithapHbelow7?

A. MgO

B. Li2O

C. CaO

D. P4O10

9. The electronegativity values of four elements are given.

C N O F2.6 3.0 3.4 4.0

What is the order of increasing polarity of the bonds in the following compounds?

A. CO < OF2 < NO < CF4

B. CF4 < CO < OF2 < NO

C. NO < OF2 < CO < CF4

D. CF4 < NO < OF2 < CO

10. WhichcompoundhastheshortestC–Nbond?

A. CH3NH2

B. (CH3)3CNH2

C. CH3CN

D. CH3CHNH

Turn over


11. Whichofthefollowingseriesshowsincreasinghydrogenbondingwithwater?

A. Propane < propanal < propanol < propanoic acid

B. Propane < propanol < propanal < propanoic acid

C. Propanal < propane < propanoic acid < propanol

D. Propanoic acid < propanol < propanal < propane

12. Which statements are correct for metals?

I. Theyconductelectricitybecausetheyhavefreemovingions.II. They consist of a close-packed lattice of positive ions with delocalized electrons.III. Theyaremalleablebecausethelayersofpositiveionscanslideovereachother.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

13. Which statement is correct for this reaction?

Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2(g)∆H = -26.6 kJ

A. 13.3 kJ are released for every mole of Fe produced.

B. 26.6kJareabsorbedforeverymoleofFeproduced.

C. 53.2 kJ are released for every mole of Fe produced.

D. 26.6 kJ are released for every mole of Fe produced.


14. The enthalpy changes for two reactions are given.

Br2 (l) + F2 (g) →2BrF(g)∆H = x kJBr2 (l) + 3F2 (g) → 2BrF3(g)∆H = y kJ

What is the enthalpy change for the following reaction?

BrF (g) + F2 (g) → BrF3 (g)

A. x - y

B. -x + y

C. 12

(-x + y)

D. 12

(x - y)

15. What is the enthalpy change, in kJ, of the following reaction?

3H2 (g) + N2 (g) � 2NH3 (g)

Bond Bond enthalpy / kJ mol-1

N≡N 945H-H 436N-H 391

A. (6 × 391) - [(3 × 436) + 945]

B. (3 × 391) - (436 + 945)

C. -[(3 × 436) + 945] + (3 × 391)

D. -(6 × 391) + [(3 × 436) + 945]

Turn over


16. Thediagramshowstheenergyprofileforacatalysedanduncatalysedreaction.Whichrepresentstheenthalpychange,∆H, and the activation energy, Ea, for the catalysed reaction?

x

y

zPote

ntia

l ene

rgy

Reaction coordinate

∆H Ea (catalysed reaction)

A. z x + z

B. z z + y

C. -z x

D. z + x x


17. Excessmagnesiumpowderwasaddedtoabeakercontaininghydrochloricacid,HCl(aq). Themassofthebeakeranditscontentswasrecordedandplottedagainsttime(lineI).

Mass

Time

I

II

Which change could give line II?

A. DoublingthemassofpowderedMg

B. UsingthesamemassofMgribbon

C. Increasing the temperature

D. Using the same volume of more concentrated HCl

18. Whatwillhappenifthepressureisincreasedinthefollowingreactionmixtureatequilibrium?

CO2 (g) + H2O (l) � H+(aq)+ HCO3-(aq)

A. TheequilibriumwillshifttotherightandpHwilldecrease.

B. TheequilibriumwillshifttotherightandpHwillincrease.

C. TheequilibriumwillshifttotheleftandpHwillincrease.

D. TheequilibriumwillshifttotheleftandpHwilldecrease.

Turn over


19. 10.0 cm3ofanaqueoussolutionofsodiumhydroxideofpH= 10 is mixed with 990.0 cm3 of distilled water. What is the pH of the resulting solution?

A. 8

B. 9

C. 11

D. 12

20. Which statement is incorrect for a 0.10 mol dm-3 HCOOH solution?

A. pH = 1

B. [H+ ] << 0.10 mol dm-3

C. [HCOO- ]isapproximatelyequalto[H+ ]

D. HCOOH is partially ionized

21. What are the oxidation states of chromium in (NH4)2Cr2O7 (s) and Cr2O3 (s)?

(NH4)2Cr2O7 (s) Cr2O3 (s)

A. +7 +3

B. +6 +3

C. +6 +6

D. +7 +6

22. Which of the following is a redox reaction?

A. 3Mg (s) + 2AlCl3(aq)→ 2Al (s) + 3MgCl2(aq)

B. SiO2 (s) +2NaOH(aq)→ Na2SiO3(aq)+ H2O (l)

C. KCl(aq)+ AgNO3(aq)→ AgCl (s) + KNO3(aq)

D. 2NaHCO3(aq)→ Na2CO3(aq)+ CO2 (g) + H2O (l)


23. What is the reaction type and major product at the anode (positive electrode) when molten sodium chloride is electrolysed using platinum electrodes?

Reaction type Product

A. reduction Cl2

B. oxidation Cl2

C. reduction Na

D. oxidation Na

24. WhatisthemajorproductofthereactionbetweenHClandbut-2-ene?

A. 1,2-dichlorobutane

B. 2,3-dichlorobutane

C. 1-chlorobutane

D. 2-chlorobutane

25. Whichcompoundcanbeoxidizedwhenheatedwithanacidifiedsolutionofpotassiumdichromate(VI)?

A. CH3C(O)CH2CH3

B. CH3CH2CH(OH)CH3

C. (CH3)3COH

D. CH3(CH2)2COOH

Turn over


26. What is the name of this compound, using IUPAC rules?

C

C

O

C

C

C HH

HH

HH

HHH

H

H H

A. 3-methylbutan-3-ol

B. 2-ethylpropan-2-ol

C. 2-methylbutan-2-ol

D. 3-methylbutan-2-ol

27. Whichtypeofreactionoccursbetweenanalcoholandacarboxylicacid?

A. Addition

B. Oxidation

C. Esterification

D. Polymerization

28. How many structural isomers of C6H14 exist?

A. 4

B. 5

C. 6

D. 7


29. Whatinformationisprovidedby1H NMR, MS and IR for an organic compound?

I. 1H NMR: chemical environment(s) of protonsII. MS: fragmentation patternIII. IR: types of functional group

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

30. Astudentperformsanacid-basetitrationusingapHmeter,butforgetstocalibrateit.Whichtypeoferrorwilloccurandhowwillitaffectthequalityofthemeasurements?

A. Random error and lower precision

B. Systematic error and lower accuracy

C. Systematic error and lower precision

D. Random error and lower accuracy


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