M03/420/H(1)+
IB DIPLOMA PROGRAMME
PROGRAMME DU DIPLÔME DU BI
PROGRAMA DEL DIPLOMA DEL BI
c
CHEMISTRY
HIGHER LEVEL
PAPER 1
Wednesday 14 May 2003 (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.
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The Periodic Table
Atomic Number
1 2
H He
1.01 4.00
Element
3 4 5 6 7 8 9 10
Li Be B C N O F Ne
6.94 9.01 10.81 12.01 14.01 16.00 19.00 20.18
Atomic Mass
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 !
Fr Ra Ac
(223) (226) (227)

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. What amount of oxygen, , (in moles) contains 1.8×1022 molecules?
O2
A. 0.0030
B. 0.030
C. 0.30
D. 3.0
2. 3.0 dm3 of sulfur dioxide are reacted with 2.0 dm3 of oxygen according to the equation:
2 SO2(g) + O2(g) 2 SO3(g)
What volume of sulfur trioxide (in dm3) is formed? (Assume the reaction goes to completion and all
gases are measured at the same temperature and pressure.)
A. 5.0
B. 4.0
C. 3.0
D. 2.0
dm-3
3. What volume (in dm3) of 0.30 mol NaCl solution can be prepared from 0.060 mol of solute?
A. 0.018
B. 0.20
C. 0.50
D. 5.0
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4. Consider the composition of the species W, X, Y and Z below. Which species is an anion?
Species Number of protons Number of neutrons Number of electrons
W 9 10 10
X 11 12 11
Y 12 12 12
Z 13 14 10
A. W
B. X
C. Y
D. Z
5. What is the electron configuration for an atom with Z = 22?
A. 1s22s22p63s23p63d4
B. 1s22s22p63s23p64s24p2
1s22s22p63s23p63d24p2
C.
D. 1s22s22p63s23p64s23d2
6. Which is related to the number of electrons in the outer main energy level of the elements from the alkali
metals to the halogens?
I. Group number
II. Period number
A. I only
B. II only
C. Both I and II
D. Neither I nor II
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7. Which of the following salts form coloured solutions when dissolved in water?
I. ScCl3
II. FeCl3
NiCl2
III.
IV.
ZnCl2
A. I and II only
B. II and III only
C. III and IV only
D. I, II, III and IV
8. The compounds Na2O, Al2O3 and SO2 respectively are
A. acidic, amphoteric and basic.
B. amphoteric, basic and acidic.
C. basic, acidic and amphoteric.
D. basic, amphoteric and acidic.
9. What is the formula for the compound formed by calcium and nitrogen?
CaN
A.
B. Ca2N
Ca2N3
C.
D. Ca3N2
2
10. What is the best description of the carbon-oxygen bond lengths in ?
CO3-
A. One short and two long bonds
B. One long and two short bonds
C. Three bonds of the same length
D. Three bonds of different lengths
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11. Which of the following is true for ?
CO2
C==O bond CO2 molecule
A. polar non-polar
B. non-polar polar
C. polar polar
D. non-polar non-polar
12. The molar masses of C2H, CHOH and CHF are very similar. How do their boiling points compare?
6 3 3
A. C2H6 < CHOH < CHF
3 3
B. CH3F < CH3OH < C2H6
C. CH3OH < CH3F < C2H6
D. C2H6 < CH3F < CH3OH
-
13. What is the distribution of electron pairs and the arrangement of atoms in the triiodide ion, I3 ?
Electron pairs Atom arrangement
A. tetrahedral bent
B. square planar linear
C. trigonal bipyramid linear
D. trigonal bipyramid bent
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(Ã ) (Ä„)
14. What is the number of sigma and pi bonds and the hybridization of the carbon atom in
O
H C O H
Sigma Pi Hybridization
sp2
A. 4 1
sp3
B. 4 1
sp3
C. 3 2
sp2
D. 3 1
0 °C
15. Solid, liquid and gaseous water are all present at very low pressure near . How do the distances
between the molecules in the three states compare under these conditions?
A. The distances are equal in all three states.
B. Distances are similar in the solid and liquid, which are smaller than that in the gas.
C. Distances are smallest in the solid, and similar in the liquid and gas.
D. Distances are smallest in the liquid, and similar in the solid and the gas.
16. In which gas sample do molecules have the greatest average kinetic energy?
H2
A. at 100 K
B. CH4 at 273 K
C. at 373 K
H2O
D. CH3OH at 353 K
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17. What energy changes occur when chemical bonds are formed and broken?
A. Energy is absorbed when bonds are formed and when they are broken.
B. Energy is released when bonds are formed and when they are broken.
C. Energy is absorbed when bonds are formed and released when they are broken.
D. Energy is released when bonds are formed and absorbed when they are broken.
18. Which combination of ionic charge and ionic radius give the largest lattice enthalpy for an ionic compound?
Ionic charge Ionic radius
A. high large
B. high small
C. low small
D. low large
19. Under what conditions is a reaction spontaneous at all temperatures?
Ö
"SÖ
"H
A. + +
B. + -
C. - -
D. - +
"H
20. What is for the reaction below in kJ?
CS2(g) + 3O2(g) CO2(g) + 2SO2(g)
["Hf / kJ mol-1: CS2(g) 110, CO2(g) - 390, SO2(g) - 290]
A. -570
B. -790
C. -860
D. -1080
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21. Which of the following is (are) important in determining whether a reaction occurs?
I. Energy of the molecules
II. Orientation of the molecules
A. I only
B. II only
C. Both I and II
D. Neither I nor II
22. The reaction between NO2 and F2 gives the following rate data at a certain temperature. What is the
order of reaction with respect to NO2 and F2 ?
[F2]
[NO2] dm-3 Rate / mol dm-3 min-1
/ mol
dm-3
/ mol
0.1 0.2 0.1
0.2 0.2 0.4
0.1 0.4 0.2
NO2 F2
order order
A. first first
B. first second
C. second first
D. second second
23. Which step in a multi-step reaction is the rate determining step?
A. The first step
B. The last step
C. The step with the lowest activation energy
D. The step with the highest activation energy
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24.
I2(g) + 3Cl2(g) 2ICl3(g)
What is the equilibrium constant expression for the reaction above?
[ICl3]
A. Kc =
[I2][Cl2]
2[ICl3]
Kc =
B.
3[I2][Cl2]
2[ICl3]
Kc =
C.
[I2] + 3[Cl2]
[ICl3]2
D. Kc =
[I2][Cl2]3
25. Which of the factors below affect the equilibrium vapour pressure of a liquid in a container?
I. Temperature
II. Surface of the liquid
III. Volume of the container
A. I only
B. I and II only
C. II and III only
D. I, II and III
26. How does the [H+] in an aqueous solution with pH = 4 compare with the [H+] in a solution with pH = 2?
The [H+] is
A. twice as great.
B. half as much.
1
C. of the value.
10
1
D. of the value.
100
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27. Which is a buffer solution?
I. 0.01 mol dm-3 HCl, 0.01 mol dm-3 NaCl
II. 0.01 mol dm-3 CH3COOH , 0.01 mol dm-3 CH3COONa
A. I only
B. II only
C. Both I and II
D. Neither I nor II
28. Which one of the following species can act as both a Brłnsted-Lowry acid and base in aqueous solution?
A. CH3COOH
-
B. NO3
H2PO-
C.
4
D. OH-
29. The Ka value for an acid is 1.0 ×10-2 . What is the value for its conjugate base?
Kb
A. 1.0 ×10-2
1.0 ×10-6
B.
C. 1.0 ×10-10
D. 1.0 ×10-12
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cm3
30. Separate 20.0 solutions of a weak acid and a strong acid of the same concentration are titrated with
NaOH solution. Which will be the same for these two titrations?
I. Initial pH
II. pH at equivalence point
III. Volume of NaOH required to reach the equivalence point
A. I only
B. III only
C. I and II only
D. II and III only
31. Which is the strongest reducing agent according to the spontaneous reactions below?
2Cr (s) + 3Fe2+(aq) 2Cr3+(aq) + 3Fe(s)
Fe(s) + Pb2+ (aq) Fe2+ (aq) + Pb(s)
A. Cr (s)
B. Cr3+(aq)
Pb2+(aq)
C.
D. Pb(s)
32. What occurs during the operation of a voltaic cell based on the reaction:
Ni(s) + Pb2+(aq) Ni2+(aq) + Pb(s)
External circuit Ion movement in solution
move away from Pb(s)
A. electrons move from Ni to Pb Pb2+ (aq)
B. electrons move from Ni to Pb Pb2+ (aq)
move toward Pb(s)
C. electrons move from Pb to Ni Ni2+(aq)
move away from Ni(s)
D. electrons move from Pb to Ni Ni2+(aq)
move toward Ni(s)
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-
33.
Ag (s) + NO3 (aq) + H+ (aq) Ag+ (aq) + NO(g) + H2O (l)
When the oxidation-reduction equation above is balanced, what is the coefficient for H+(aq) ?
A. 1
B. 2
C. 3
D. 4
34. Aqueous solutions of AgNO3 , Cu (NO3)2 and Cr (NO3)3 are electrolyzed using the same quantity of electricity.
How do the number of moles of metal formed compare?
A. Ag = Cu = Cr
B. Ag > Cu > Cr
C. Ag < Cu < Cr
D. Cu > Ag > Cr
35. Which of the substances below is least soluble in water?
A. CH2OHCHOHCH2OH
O
B. CH3CCH3
O
CH3CH2COH
C.
O
CH3COCH3
D.
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36. What product results from the reaction of ?
CH2 = CH2 with Br2
A. CHBrCHBr
B. CH2CHBr
CH3CH2Br
C.
D. CH2BrCH2Br
37. How many different tripeptides can be prepared from three amino acids?
(Each amino acid is used only once in a given tripeptide.)
A. 1
B. 3
C. 6
D. 9
38. The reaction of C6H6 with Br2 in the presence of a halogen carrier is expected to produce
C6HBr
A.
6
B. C6HBr2
6
C. C6HBr2 + H2
4
C6HBr + HBr
D.
5
39. Which compound reacts fastest with water?
A. (CH3)3CBr
(CH3)3CCl
B.
C. CH3CH2CH2CH2Br
CH3CH2CH2CH2Cl
D.
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HNMR
40. Which of the following compounds exhibits three lines in the 1 spectrum?
I. CH3CH2OCH3
II. (CH3)3 CCl
CH3CH2COOH
III.
A. I only
B. II only
C. I and III only
D. I, II and III
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