N00/420/H(1)
INTERNATIONAL BACCALAUREATE
BACCALAURÉAT INTERNATIONAL
BACHILLERATO INTERNACIONAL
CHEMISTRY
HIGHER LEVEL
PAPER 1
Tuesday 7 November 2000 (afternoon)
1 hour
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.
880-203 15 pages
Periodic Table
1 2
Atomic Number
H He
1.01 4.00
3 4 5 6 7 8 9 10
Li Be B C N O F Ne
6.94 9.01 Atomic Mass 10.81 12.01 14.01 16.00 19.00 20.18
11 12 13 14 15 16 17 18
Na Mg Al Si P S Cl Ar
22.99 24.31 26.98 28.09 30.97 32.06 35.45 39.95
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
39.10 40.08 44.96 47.90 50.94 52.00 54.94 55.85 58.93 58.71 63.55 65.37 69.72 72.59 74.92 78.96 79.90 83.80
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
85.47 87.62 88.91 91.22 92.91 95.94 98.91 101.07 102.91 106.42 107.87 112.40 114.82 118.69 121.75 127.60 126.90 131.30
55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
132.91 137.34 138.91 178.49 180.95 183.85 186.21 190.21 192.22 195.09 196.97 200.59 204.37 207.19 208.98 (210) (210) (222)
87 88 89 ! 104 105 106 107 108 109
Fr Ra Ac Rf Db Sg Bh Hs Mt
(223) (226) (227) (261) (262) (263) (262)

58 59 60 61 62 63 64 65 66 67 68 69 70 71
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
140.12 140.91 144.24 146.92 150.35 151.96 157.25 158.92 162.50 164.93 167.26 168.93 173.04 174.97
!
90 91 92 93 94 95 96 97 98 99 100 101 102 103
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
232.04 231.04 238.03 (237) (242) (243) (247) (247) (251) (254) (257) (258) (259) (260)
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1. Which compound has the highest percentage by mass of carbon?
A. C2H2
B. C2H4
C. C3H8
D. C4H10
2. A certain compound has a relative molar mass of 88. A possible empirical formula for this compound is
A. CH2
B. CH2O
C. CH3O
D. C2H4O
3. H2 + Cl2 Ć 2HCl
Hydrogen and chlorine react according to the equation above. What will be the result of the reaction of
H2 Cl2
2.0 moles of and 1.5 moles of ?
A. 3.5 mol of HCl
H2
B. 1.5 mol of HCl and 0.5 mol of
Cl2
C. 2.0 mol of HCl and 0.5 mol of
H2
D. 3.0 mol of HCl and 0.5 mol of
4. 25.0 cm3 of sulfuric acid solution reacts with 36.2 cm3 of 0.225 mol dm-3 sodium hydroxide solution.
The concentration of the acid is
36.2 × 0.225
A.
25.0
2 × 36.2 × 0.225
B.
25.0
36.2 × 0.225
C.
2 × 25.0
25.0
D.
2 × 36.2 × 0.225
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5. The electron transition between which two levels releases the most energy?
A. First to third
B. Fourth to ninth
C. Sixth to third
D. Second to first
XCl2
6. A solid element, X, contains unpaired electrons in its atoms and forms an ionic chloride, . Which
electron configuration is possible for element X?
A. [Ne] 3s2
B. [Ar] 3d24s2
C. [He] 2s2 2p2
D. [Ne] 3s2 3p4
7.
Abundance
60 61 62
Mass
The mass spectrum of an element is shown above. Which statement about this element is correct?
A. The three isotopes are separated after being converted to negative ions
B. The isotope with mass 62 will be deflected more than the isotopes with masses 60 or 61
C. The most abundant isotope contains 61 neutrons
D. Its atomic mass will be between 60 and 61
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8. Which pair of species is listed in increasing order of the property given?
A. Ionisation energy: O, F
B. Radius: Mg, Mg2+
C. Melting point: I2, Br2
D. Covalent character: HI, HBr
9. Most of the oxides of non-metallic elements are
A. ionic and basic.
B. ionic and acidic.
C. covalent and basic.
D. covalent and acidic.
10. Which aqueous complex ion will not be coloured?
A. Ni2+
B. Fe2+
C. Sc3+
D. Cr3+
11. Which compound contains both sp2 and sp3 hybridised carbon atoms?
COOH
CH3
A. C.
C N CH CH2
B. D.
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12. Which molecule has the largest bond angle?
A. BF3
CF4
B.
C. NF3
D. OF2
13. In which of the compounds below are the electrons in the carbon oxygen bonds delocalised?
CH3CH2ONa
I. Sodium ethoxide,
CH3COONa
II. Sodium ethanoate,
A. I only
B. II only
C. Both I and II
D. Neither I nor II
14. Which species does not contain at least one 90 bond angle?
A. CF4
B. PF5
C. SF6
2-
D. SiF6
15. Which compound has the greatest vapour pressure at 298 K?
A. C3H7OH
B. C2H5OCH3
C. C2H5COOH
D. C3H7NH2
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16. 125 cm3 of an unknown gas has a mass of 0.725 g at 25 C and 0.97 atmospheres. Which expression will
give the relative molar mass of the gas? (R = 82.05 cm3 atm K-1 mol-1)
0.725Ä„ 82.05Ä„ 25
A.
0.97 Ä„125
125× 0.97
B.
0.725× 82.05× 298
0.725× 82.05× 298
C.
0.97 × 0.125
0.725× 82.05× 298
D.
0.97 ×125
17. For which combination of properties will a gas behave most ideally?
A. Polar molecules at a low temperature and high pressure
B. Polar molecules at a high temperature and low pressure
C. Nonpolar molecules at a low temperature and high pressure
D. Nonpolar molecules at a high temperature and low pressure
18. "HÖ =-393 kJ
C(s) + O2(g) Ć CO2(g)
"HÖ =-588 kJ
2CO(g) + O2(g) Ć 2CO2 (g)
According to the data above, what is the enthalpy of formation of carbon monoxide in kJ mol-1?
A. -87
B. -99
C. -173
D. -220
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19. C2H4 (g) + H2 (g) C2H6(g) "HÖ = -137 kJ
Which statement about the information above is correct?
A. The total energy of the bonds broken in the reactants is greater than the total energy of the bonds
formed in the product
B. The bonds broken and the bonds made are of the same strength
C. The total energy of the bonds broken in the reactants is less than the total energy of the bonds
formed in the product
D. No conclusion can be made about the sums of the bond enthalpies in the product compared with the
reactants.
20. When 50 cm3 of 1 mol dm-3 HCl is mixed with 50 cm3 of 1 mol dm-3 NaOH, the temperature of the
resulting solution increases by 6 C. What will be the temperature change when 100 cm3 of each of these
solutions are mixed?
A. 3 C
B. 6 C
C. 12 C
D. 24 C
21. NH4Cl(s) Ć NH3(g) + HCl(g)
What are the signs of "H and "S for this reaction?
"H "S
" "
" "
" "
A. ++
B. - -
C. +-
D. -+
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22.
Volume
of CO2
Time
CaCO3
The curve above is obtained for the reaction of an excess of with hydrochloric acid. How and
why does the rate of reaction change with time?
Rate of reaction Reason
A. decreases the HCl becomes more dilute
CaCO3
B. decreases the pieces of become smaller
C. increases the temperature increases
D. increases the CO2 produced acts as a catalyst
O2
23. The rate equation for the reaction between and NO is
Rate = k[O2 ][NO]2
O2
By what factor would the rate of this reaction increase if the concentrations of and NO are both
doubled?
1
A.
8
B. 3
C. 4
D. 8
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24.
II
III
Energy
I
Progress of reaction
Which energy value(s) will change when a catalyst is added?
A. I only
B. II only
C. II and III only
D. I, II and III
25. 2H2 (g) + CO(g) lCH3OH(g)
Methanol is made in industry by means of the reaction above. The equilibrium expression for this
reaction is
[CH3OH]
A.
2[H2 ][CO]
[CH3OH]
B.
[H2]2[CO]
2[H2 ][CO]
C.
[CH3OH]
[H2]2[CO]
D.
[CH3OH]
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26. N2(g) + 3H2 (g) l2NH3(g) "H = -91.8 kJ
The industrial synthesis of ammonia is based on the reaction above. Which factor(s) will increase the
equilibrium concentration of ammonia?
I. Increase in pressure
II. Increase in temperature
A. I only
B. II only
C. Both I and II
D. Neither I nor II
27. Which is the correct combination?
Intermolecular forces Boiling point "Hvap
"
"
"
A. weak low low
B. weak low high
C. strong high low
D. strong low low
28. When the pH of a solution changes from 2.0 to 4.0, the hydrogen ion concentration
A. increases by a factor of 100.
B. increases by a factor of 2.
C. decreases by a factor of 2.
D. decreases by a factor of 100.
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29. Which will be the same for separate 1 mol dm-3 solutions of a strong acid and a weak acid?
I. Electrical conductivity
II. Concentration of H+ ions
A. I only
B. II only
C. Both I and II
D. Neither I nor II
[H+ ] = 20 Ä„10-3 mol dm-3?
30. What is the Ka of a 0.10 mol dm-3 solution of a weak monoprotic acid if the .
A. 20 Ä„10-2 mol dm-3
.
B. 2.0 Ä„10-4 mol dm-3
C. 4.0 Ä„10-5 mol dm-3
D. 4.0 Ä„10-7 mol dm-3
31. A buffer solution will be formed by combining equal volumes of 0.1 mol dm-3 solutions of
A. hydrochloric acid and sodium hydroxide.
B. hydrochloric acid and sodium ethanoate.
C. ethanoic acid and sodium hydroxide.
D. ethanoic acid and sodium ethanoate.
32. Which is not a redox reaction?
A. 3H2 + N2 Ć 2NH3
B. N2O4 Ć 2NO2
C. Cl2 + 2NaI Ć 2NaCl + I2
D. 2H2O2 Ć 2H2O + O2
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33. The same quantity of electricity was passed through separate molten samples of aluminium oxide and
sodium chloride. How many moles of sodium will be produced if 0.2 moles of oxygen gas were formed?
A. 0.1
B. 0.2
C. 0.4
D. 0.8
34. 2AgNO3(aq) + Zn(s) Ć 2Ag(s) + Zn(NO3)2(aq)
Zn(NO3)2 (aq) + Co(s) Ć No reaction
2AgNO3(aq) + Co(s) Ć Co(NO3)2(aq) + 2Ag(s)
Using the above information, the order of increasing activity of the metals is
A. Ag < Zn < Co
B. Co < Ag < Zn
C. Co < Zn < Ag
D. Ag < Co < Zn
35. Which compound gives two distinct peaks in its NMR spectrum?
A. C6H6
B. C2H5OH
CH3
C. CH3 C OH
CH3
D. CH3OCH3
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36. Which substance is most likely to react with hydroxide ions by means of a SN1 mechanism?
A. C6H5Cl
B. (CH3)3CCl
C. (CH3)2CHCH2Cl
D. CH3CH2CH2CH2Cl
37. When the compounds below are listed in order of decreasing boiling point (highest to lowest) what is the
correct order?
1. ethane 2. fluoroethane 3. ethanol 4. ethanoic acid
A. 4, 3, 1, 2
B. 4, 3, 2, 1
C. 3, 4, 1, 2
D. 2, 1, 3, 4
38. Which reagent reacts with CH3CH2COCH3?
I. LiAlH4
II. H+ / K2Cr2O7
A. I only
B. II only
C. Both I and II
D. Neither I nor II
39. Which compound can show optical activity?
A. CH3COOH
B. H2NCH2COOH
C. HOCH(CH3)COOH
D. (CH3)3CCOOH
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40. How many different structural isomers have the formula C4H9Cl?
A. 2
B. 3
C. 4
D. 5
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