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![Page 1: I'IHI'ITIBIR UNIVERSITYexampapers.nust.na/greenstone3/sites/localsite/collect... · · 2018-03-01What is the hybridisation of the carbon atoms in ethyne, CZHZ? A. Sp B. spz C](https://reader034.vdocuments.mx/reader034/viewer/2022051802/5afc53da7f8b9a814d8bf1fb/html5/thumbnails/1.jpg)
I'IHI'ITIBIR UNIVERSITY
OF SCIENCE nnD TECHFIOLOGY
FACULTY OF HEALTH AND APPLIED SCIENCES
DEPARTMENT OF NATURAL AND APPLIED SCIENCES
QUALIFICATION: BACHELOR OF SCIENCE
QUALIFICATION CODE: O7BOSC LEVEL: 7
COURSE CODE: ICH6OZS COURSE NAME: INORGANIC CHEMISTRY
SESSION: NOVEMBER 2017 PAPER: THEORY
DURATION: 3 HOURS MARKS: 100
FIRST OPPORTUNITY EXAMINATION QUESTION PAPER
EXAMINER(S) DR. EUODIA HESS
MODERATOR:P ROF HABAU KA KWAAM BWA
INSTRUCTIONS
Answer ALL the questions.
Write clearly and neatly.
Number the answers clearly
All written work must be done in blue or black ink and sketches can
be done in pencil
PWI‘JE"5. No books, notes and other additional aids are allowed
THIS QUESTION PAPER CONSISTS 0F 9 PAGES (Including this front page, list of useful constants
and Periodic Table)
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SECTION A [40]
QUESTION 1: Multiple Choice Questions [40]
0 There are 20 multiple choice questions in this section. Each question carries
2 marks.
0 Answer ALL questions by selecting the letter of the correct answer.
0 Choose the best possible answer for each question, even ifyou think there is
another possible answer that is not given.
1. Which of the following conditions favours the existence of a substance in the solid state?
A. High temperature
B. Low temperature
C. High thermal energy
D. Weak cohesive forces
2. Which of the following is not a characteristic of a crystalline solid?
A. Definite characteristic heat of fusion
B. Isotropic nature
C. A regular periodically repeated pattern of arrangement of constituent particles in the entire
crystal
D. A true crystal
3. Which of the following is an amorphous solid?
A. Graphite
B. Quartz Glass
C. Chrome alum
D. Silicon carbide
4. Iodine molecules are held in the crystal lattice by ?
A. London forces
B. Dipole-dipole interactions
C. Covalent bonds
D. Coulombic forces
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5. Which of the following is a network solid?
A. 502 (solid)
B. 12
C. Diamond
D. H20 (ice)
6. What is the hybridisation of the carbon atoms in ethyne, CZHZ?
A. Sp
B. spz
C. 3193
D. 31336!
E. 5193612
7. What is the electronic geometry for 5 regions of high electron density on a central atom?
A. octahedral
B. square planar
C. tetrahedral
D. trigonal bipyramidal
E. trigonal planar
8. What angle(s) are associated with a central atom that has tetrahedral electronic geometry?
A. 109.5
B. 120
C. 120 and 180
D. 90 and 120
E. 90 and 180
9. Which one of the following molecules is polar?
A. N2
B. R,
c. C12
D. CO2
E. H20
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10.
11.
12.
13.
What kind of hybrid orbitals is utilised by the carbon atom in CR; molecules?
A. Sp
B. 5p2
C. 5103
D. sp3d
E. sp3d2
The electronic geometry of the central atom in PC13 is
A. pyramidal
B. trigonal planar
C. tetrahedral
D. octahedral
E. trigonal bipyramidal
The molecular geometry of PC13 is__
A. pyramidal
B. trigonal planar
C. tetrahedral
D. octahedral
E. trigonal bipyramidal
Choose the false statement from the following:
A. A sigma bond is a bond resulting from head-on overlap of atomic orbitals.
B. A pi bond is a bond resulting from side-on overlap of atomic orbitals.
C. A double bond consists of one sigma bond and one pi bond
D. A triple bond may consist of one sigma bond and two pi bonds or of two sigma bonds and
one pi bond.
E. A carbon atom involved in a double bond may not be sp3 hybridized.
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14. How many lone pairs of electrons does the Lewis dot structure of H25 have around its central
atom and what is the shape of the molecule?
A. 0, linear
B. 0, bent
C. 1, trigonal planar
D. 2, tetrahedral
E. 2, bent
15. Number of dative bonds to central metal ion is its
A. oxidation number
B. compound number
C. dative number
D. coordination number
16. ions which are produced from ligands are
A. Cation
B. Anion
C. Complex ion
D. All of them
17. In a face centred cubic lattice the number of nearest neighbours for a given lattice point is
A. 6
B. 4
C. 8
D. 12
18. Use VSEPR theory to predict the molecular geometry of 5032—.
A. bent
B. tetrahedral
C. square planar
D. triangular planar
E. triangular pyramidal
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19. In a comparison with s-block elements, melting points of transition elements are
A. Higher
B. Lower
C. Same
D. Constant
20. Due to ligands' action of splitting colour of transition metal compound, this change occurs at
A. s-orbital
B. p-orbital
C. d -orbital
D. f-orbital
SECTION B:
QUESTION 1:
1.1 What is the coordination number of the metal in each of the following complexes?
a) [HgClalZ'
b) [ZrF8]4'
C) [Cl‘(H20)4Cl2]+
d) [Mo(CO)sBr]‘
e) [Au(CN)2]‘
1.2 What is the oxidation state of the metal in each of the following complexes?
a) ”180412"
b) [Zng]4‘
C) [Cl’(H20)4C|2]Jr
d) [MO(CO)sBr]'
e) [AU(CN)2]'
1.3 What are the geometries for complexes with coordination number 2, 4, and 6?
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[60]
[39]
(10)
(10)
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1.4 What is the name for each of the following coordination compounds?
a) K3[Cr(C204)2CI2]
b) [Ag(NH3)2]N03
c) [Cu(en)2]504
d) Cs[FeCI4]
e) (NH4)3[RhCI6]
1.5 For each of the following complex ions give the oxidation number of metal ion,
depict low-spin or high-spin configurations, give the number of unpaired
electrons in each state and tell whether or not its paramagnetic or diamagnetic.
a) [RUIHZOI6I2+
bl [NiUVihld2+
QUESTION 2:
2.1 What are the shapes of the ions H30+ and CW}? Draw the Lewis structure for each
ion.
2.2 Deduce whether nitrogen trifluoride, dichloromethane and sulfur tetrafluoride polaror non-polar. if polar, indicate the negative and positive sides of the molecule.
2.3 Identify the hybridization of the central atom in following inorganic species:
a) 3H4—
b) SF;
c) SOF4
QUESTION 3:
Calculate the amount of energy (in kJ) needed to heat 346 g of liquid water from 0°C to 182 °C.
Assume that the specific heat of water is 4.184 J/g- °C over the entire liquid range
and that the specific heat of steam is 1.99 J/g- °C ( AHvap = 40.79 kJ/mol for water).
END OF EXAMINATION
(10)
I11]
(2)
(3)
(6)
[10]
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USEFUL CONSTANTS:
Gas constant, R = 8.3145 J' mol‘l' K'1 = 0.083145 dm3' bar
- mol'l' K'1 = 0.08206 L atm mol'l' K“1
1Pa‘m3=1kPa.L =1N-m =1]
1 atm = 101 325 Pa = 760 mmHg = 760 torr
Avogadro's Number, NA = 6.022 x 1023 mol'1
Planck’s constant, h = 6.626 x 10‘34 J5
Speed of light, c = 2.998 x 108 ms‘1
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Page 9 of 9
PERIODICTABLEOF
THEELEMENTS
1
18
1
2
H
He
1.00794
2
‘3
14
‘5
1"
'7
4.00260
3
4
5
6
7
8
9
10
Li
Be
B
C
N
0
F
Ne
6.941
9.01218
10.81
12.011
14.0067
15999418998420.179
11
12
13
14
15
16
17
18
Na
Mg
Al
Si
P
S
Cl
Ar
22.989824.305
3
4
5
6
7
8
9
10
11
12
26.981528.0855
30.9738
32.06
35.453
39.948
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
39.0983
40.08
44.9559
47.88
50.941551.996
54.9380
55.847
58.9332
58.69
63.546
6538
69.72
72.59
74.9216
78.96
79.904
83.8
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
85.4678
87.62
88.9059
91.22
92.9064
95.94
(98)
101.07
102.906
106.42
107.868
112.41
114.82
118.69
121.75
127.6
126.9
131.29
55
56
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Lu
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
132905
137.33
174.967
178.49
180.948
183.85
186207
1902
19222
195.08
196.967200.59
204.383
2072
208.908
(209)
(210)
(222)
87
88
103
104
105
106
107
108
109
110
111
112
114
116
118
Fr
Ra
Lr
Rf
Db
Sg
Bh
HS
Mt
Uun
Uuu
Uub
Uuq
Uuh
Uuo
(223)
226.025
(260)
(261)
(262)
(263)
(264)
(265)
(268)
(269)
(272)
(269)
Lanthlnidw:
57
58
59
60
61
62
63
64
65
66
67
68
69
70
La
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
138.906140.12140.90814424(145)
150.36
151.96
15725158925162.50161.930167.26166.934173.04
Actinidefl
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
PuAmCm
Bk
Cf
Es
Fde
No
227.028232.038231.036238.029237.048
(244)
(243)
(247)
(247)
(251)
(252)
(257)
(258)
(259)