Chemistry Higher level Paper 1 - IB Documents
[Pages:17]M17/4/CHEMI/HPM/ENG/TZ2/XX
Chemistry Higher level Paper 1
Thursday 11 May 2017 (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. ? The periodic table is provided for reference on page 2 of this examination paper. ? The maximum mark for this examination paper is [40 marks].
17 pages
2217?6113 ? International Baccalaureate Organization 2017
1
2
3
4
5
The Periodic Table
6
7
8
9
10
11
12
13
14
15
16
17
18
1
1H 1.01
3
4
2 Li
Be
6.94 9.01
Atomic number Element
Relative atomic mass
2
He 4.00
5
B 10.81
6
C 12.01
7
N 14.01
8
O 16.00
9
F 19.00
10
Ne 20.18
11
12
3 Na Mg
22.99 24.31
13
Al 26.98
14
Si 28.09
15
P 30.97
16
S 32.07
17
Cl 35.45
18
Ar 39.95
19
20
21
22
4K
Ca
Sc
Ti
39.10 40.08 44.96 47.87
23 V 50.94
24 Cr 52.00
25
Mn 54.94
26
Fe 55.85
27 Co 58.93
28 Ni 58.69
29 Cu 63.55
30 Zn 65.38
31
Ga 69.72
32
Ge 72.63
33 As 74.92
34 Se 78.96
35 Br 79.90
36
Kr 83.90
37
38
39
40
5 Rb
Sr
Y
Zr
85.47 87.62 88.91 91.22
41
Nb 92.91
42
Mo 95.96
43
44
45
46
47
48
49
50
51
52
53
54
Tc
Ru Rh
Pd
Ag Cd
In
Sn
Sb
Te
I
Xe
(98) 101.07 102.91 106.42 107.87 112.41 114.82 118.71 121.76 127.60 126.90 131.29
55
56 57 72
73
6 Cs
Ba
La
Hf
Ta
132.91 137.33 138.91 178.49 180.95
74
75
76
77
78
79
80
81
82
83
84
W
Re
Os
Ir
Pt
Au Hg
Tl
Pb
Bi
Po
183.84 186.21 190.23 192.22 195.08 196.97 200.59 204.38 207.2 208.98 (209)
85 At (210)
86 Rn (222)
87
88 89 104
7 Fr
Ra
Ac
Rf
(223) (226) (227) (267)
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 ?
M17/4/CHEMI/HPM/ENG/TZ2/XX
58
59
Ce
Pr
140.12 140.91
60
Nd 144.24
61
Pm (145)
62
63
64
65
66
67
68
69
70
71
Sm Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
150.36 151.96 157.25 158.93 162.50 164.93 167.26 168.93 173.05 174.97
90
91
Th
Pa
232.04 231.04
92
U 238.03
93
Np (237)
94
Pu (244)
95
Am (243)
96
Cm (247)
97
Bk (247)
98
Cf (251)
99
Es (252)
100
Fm (257)
101
Md (258)
102
No (259)
103
Lr (262)
? 3 ?
M17/4/CHEMI/HPM/ENG/TZ2/XX
1. What is the sum of the coefficients when the equation is balanced with whole numbers?
A. 26.5
--C8H18(g) + --O2(g) --CO(g) + --H2O(l)
B. 30
C. 53
D. 61
2. What is the maximum volume, in dm3, of CO2(g) produced when 1.00g of CaCO3(s) reacts with 20.0cm3 of 2.00moldm-3 HCl(aq)?
CaCO3(s) + 2HCl(aq) CaCl2(aq) + H2O(l) + CO2(g) Molar volume of gas = 22.7dm3mol-1; Mr(CaCO3) = 100.00
A. 1 ? 20.0 ? 2.00 ? 22.7
2
1000
B. 20.0 ? 2.00 ? 22.7 1000
C.
1.00 ? 22.7
100.00
D.
1.00 ? 2 ? 22.7
100.00
3. Which factors affect the molar volume of an ideal gas?
I. Pressure II. Temperature III. Empirical formula
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
Turn over
? 4 ?
M17/4/CHEMI/HPM/ENG/TZ2/XX
4. Which electron transition emits radiation of the longest wavelength?
n = 5 n = 4
n = 3
D C
n = 2
B A
n = 1
5. X, Y and Z represent the successive elements, Ne, Na and Mg, but not necessarily in that order.
First ionization energy / kJmol-1
X
2081
Y
496
Z
738
What is the order of increasing atomic number?
A. X < Y < Z
B. X < Z < Y
C. Y < Z < X
D. Y < X < Z
6. Which property increases down Group 1, the alkali metals? A. Atomic radius B. Electronegativity C. First ionization energy D. Melting point
7. Which element is a lanthanide? A. Hf B. Tb C. U D. Y
? 5 ?
M17/4/CHEMI/HPM/ENG/TZ2/XX
8. Ammonia is a stronger ligand than water. Which is correct when concentrated aqueous ammonia solution is added to dilute aqueous copper(II) sulfate solution? A. The d-orbitals in the copper ion split. B. There is a smaller splitting of the d-orbitals. C. Ammonia replaces water as a ligand. D. The colour of the solution fades.
9. How many bonding electrons are there in the urea molecule? H2N CO H2N
A. 8 B. 16 C. 20 D. 24
10. Which does not show resonance? A. PO43B. C6H6 C. C6H12 D. O3
Turn over
? 6 ? 11. Which metal has the strongest metallic bond?
A. Li B. Na C. K D. Rb
M17/4/CHEMI/HPM/ENG/TZ2/XX
12. Which is the first step in the CFC-catalysed destruction of ozone in UV light? A. CCl2F2 CClF2+ + ClB. CCl2F2 CClF2 + Cl C. CCl2F2 CCl2F+ + FD. CCl2F2 CCl2F + F
13. Which statement is correct? A. Sigma bonds are formed only by the combination of s atomic orbitals. B. Pi bonds can be formed in the absence of sigma bonds. C. Pi bonds are formed parallel to the axis between atoms. D. Pi bonds are formed only by the combination of hybrid orbitals.
? 7 ? 14. What can be deduced from this reaction profile?
M17/4/CHEMI/HPM/ENG/TZ2/XX
Reactants
Enthalpy
Products
Reaction coordinate A. The reactants are less stable than the products and the reaction is exothermic. B. The reactants are less stable than the products and the reaction is endothermic. C. The reactants are more stable than the products and the reaction is exothermic. D. The reactants are more stable than the products and the reaction is endothermic.
15. What can be deduced from the facts that ozone absorbs UV radiation in the region of 340nm and molecular oxygen in the region of 242nm? A. The bond between atoms in molecular oxygen is a double bond. B. The bonds in ozone are delocalized. C. The bonds between atoms in ozone are stronger than those in molecular oxygen. D. The bonds between atoms in molecular oxygen need more energy to break.
Turn over
? 8 ?
M17/4/CHEMI/HPM/ENG/TZ2/XX
16. The Born-Haber cycle for potassium oxide is shown below: 2K+(g) + O2-(g)
+612kJ 2K+(g) + 2e- + O(g)
+838kJ 2K(g) + O(g)
+428kJ
2K(s) +
1 2
O2(g)
lattice enthalpy
-361kJ
K2O(s)
Which expression represents the lattice enthalpy in kJmol-1? A. -361 + 428 + 838 + 612 B. -(-361) + 428 + 838 + 612 C. -361 + 428 + 838 - 612 D. -(-361) + 428 + 838 - 612
17. Which ion's hydration energy is the most exothermic? A. Li+ B. Na+ C. BrD. I-
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