CHEMISTRY 102
HOUR EXAM I
1.
Fall 2014
Page 1
Draw the Lewis structure for ICl5. How many of the following four statements (I-IV)
is/are true regarding ICl5?
I. The central atom in ICl5 has one lone pair of electrons.
II. Some of the ClICl bond angles are approximately 90°.
III. ICl5 is polar.
IV. The shape of ICl5 is square pyramid.
a) 0 (None are true.)
b) 1
c) 2
d) 3
e) 4 (All are true.)
Use the figure below to answer the next two questions.
2.
What color is electromagnetic radiation having a frequency of 5.0  1014 sec 1?
a) red
3.
b) orange
c) yellow
d) blue
In the emission spectrum for hydrogen, what color is the n = 6 to n = 2 electronic
transition?
a) red
b) orange
c) yellow
d) blue
_______________________________________________
4.
5.
e) violet
e) violet
Consider the compound butane, which has a formula of C4H10. If a sample of butane
contains 2.59  1023 atoms of hydrogen, what mass of butane is present?
a) 25.0 g
b) 50. g
d) 1.25 g
e) 2.50 g
c) 5.00 g
An unknown element E forms a covalent compound with fluorine having the formula
EF4. The shape of the EF4 molecule is see-saw. Which of the following elements could
be E?
CHEMISTRY 102
Hour Exam I
6.
Fall 2014
Page 2
a) O
b) N
c) Se
d) P
e) I
Place the following atoms/ions in order of decreasing size (largest to smallest).
F, Te, I, Ne+
7.
8.
a) Te > I > F > Ne+
b) F > Te > I > Ne+
d) Te > F > Ne+ > I
e) Ne+ > F > I > Te
Which of the following ground state electron configurations is associated with the atom
having the largest ionization energy?
a) [Ne]3s23p2
b) [Ne]3s23p3
d) [He]2s22p3
e) [Ar]4s23d104p3
c) [He]2s22p4
The ground state electron configuration for an atom or ion has 2 electrons in the n = 1
orbital, 8 electrons in n = 2 orbitals, 18 electrons in n = 3 orbitals, and 12 electrons in
n = 4 orbitals. Which of the following could be this atom or ion?
a) Zr
9.
c) I > Ne+ > F > Te
b) Mo2+
c) Sr2
d) Cd
e) Pd2
Which of the following is not accounted for in the Bohr model?
a) Electrons follow circular orbits.
b) Electrons move between orbits by absorbing or emitting photons of electromagnetic
radiation.
c) Energy is quantized.
d) Electrons exhibit wave properties.
e) For the n =  state, the electron has been removed from the atom.
10.
Which of the following statements (a-d) is true regarding element 117 (symbolized as
X)?
a)
b)
c)
d)
e)
11.
Element 117 would form a stable compound with potassium having the formula K2X.
Element 117 has 2 unpaired electrons in the ground state.
Element 117 has one valence electron in the ground state.
Element 117 has 14 electrons in various f orbitals in the ground state.
None of the above statements (a-d) are true.
When l = 5, these are called h orbitals. How many different ml values are possible for
allowed h orbitals?
a) 25
b) 21
c) 18
d) 15
e) 11
CHEMISTRY 102
HOUR EXAM I
12.
Which of the following statements is false?
a)
b)
c)
d)
e)
13.
When a metal reacts with a nonmetal, an ionic compound is produced.
Nonmetals form anions when reacted with a metal to form a compound.
Alkaline earth metals form stable +2 charged ions when in ionic compounds.
Transition metals gain electrons to form stable ions when in ionic compounds.
When nonmetals form compounds with each other, a covalent compound usually
results.
The most stable ion of a certain isotope contains 15 protons and has a mass number of 33.
Which of the following statements (a-d) about this ion is true? Note: the most stable ion
is the ion that forms when this isotope is in an ionic compound.
a)
b)
c)
d)
e)
14.
Fall 2014
Page 3
The net charge of the ion is 3.
The ion contains 10 electrons.
The ion contains 33 neutrons.
The ion is sulfur.
All of the above statements (a-d) are false.
Which of the following statements is false?
a) The periodic table predicts that the 8s atomic orbital will be lower in energy that the
6d atomic orbitals.
b) The quantum mechanical model assumes that the electron has wave properties.
c) The Heisenberg uncertainty principle implies that we cannot know the exact location
of an electron as it moves around the nucleus.
d) DeBroglie hypothesized that all matter exhibits both particulate and wave properties.
e) The quantum mechanical model tells us that there are seven degenerate (same energy)
4f atomic orbitals.
15.
Which of the following statements (a-d) about the electromagnetic spectrum is true?
Note that wavelengths are given in units of cm.
Radiowave
, cm
Microwave
1
Infrared
10-2
Vis.
10-4
UV
x-ray
10-6
-ray
10-8
a) Ultraviolet (UV) radiation has a longer wavelength than visible (Vis.) radiation.
b) The frequency of microwave radiation is higher than the frequency of visible (Vis.)
radiation.
c) Gamma (γ) ray radiation travels faster than radiowaves because it has a shorter
wavelength.
d) A photon of x-ray radiation is more energetic than a photon of microwave radiation.
CHEMISTRY 102
Hour Exam I
16.
Fall 2014
Page 4
e) None of the above statements (a-d) are true.
Which two atomic orbitals are depicted in the figures below?
a) dxy, py
b) d z 2 , px
c) d x 2  y2 , p y
d) dxz, py
e) dxy, px
17.
The density of osmium (the densest metal) is 22.57 g/cm3. If a 1.00 kg rectangular block
of osmium has two dimensions of 4.00 cm  4.00 cm, calculate the third dimension of the
rectangular block. The volume of a rectangle is length  width  height.
a) 44.3 cm
18.
19.
20.
c) 16.0 cm
d) 1.41 cm
e) 3.97 cm
A certain molecule is linear and nonpolar. Which of the following could be this
molecule?
a) FKrF (KrF2)
b) OSO (SO2)
d) OCS (COS)
e)
c) OOO (O3)
FSF (SF2)
Which of the following molecules has the smallest bond angle?
a) FKrF (KrF2)
b) OSO (SO2)
d) OCS (COS)
e)
c) OOO (O3)
FSF (SF2)
When heated, baking soda (commonly called sodium bicarbonate) undergoes a
decomposition reaction to form solid sodium carbonate, carbon dioxide gas and water
vapor. How many moles of sodium carbonate are produced for every 2.0 moles of
sodium bicarbonate that are decomposed? (HCO3 is the bicarbonate ion formula.)
a)
b)
c)
d)
e)
21.
b) 2.77 cm
1.0 mol sodium carbonate
1.5 mol sodium carbonate
2.0 mol sodium carbonate
2.5 mol sodium carbonate
3.0 mol sodium carbonate
Which of the following statements (a-c) is/are true?
CHEMISTRY 102
HOUR EXAM I
a)
b)
c)
d)
e)
22.
Fall 2014
Page 5
The positive charge in an atom is uniformly distributed throughout the atom.
In a neutral atom, the atomic number equals the number of electrons in the atom.
Most of the mass of an atom is due to the electrons.
Statements b and c are both true.
None of the statements (a-c) are true.
Draw the Lewis structures for the following four compounds: BH3, PS2, BrF3, and OCl2.
How many of these four compounds satisfy the octet rule (duet rule for H) for all elements in the compound?
a) 0 (none)
b) 1
c) 2
d) 3
e) 4 [All satisfy the octet rule (duet rule for H)].
23.
When the following calculation is performed, how many significant figures are in the
correct answer?
(1.00866 – 1.00776)  6.022  1023
a) 1
b)
2
c) 3
d) 4
e) 6
__________________________________
Creatine is an organic compound important to the building of muscle tissue in the body. The
skeletal structure of creatine is below. Complete the Lewis structure and answer the next two
questions.
H
H
N
N
H
O
H
C
N
C
O
H
C
H
H
24.
How many of the carbon and nitrogen atoms exhibit approximately 109o?
a) 0
25.
b) 1
c) 2
d) 3
e) 4
How many double bonds are in the completed Lewis structure?
a) 0
b) 1
c) 2
d) 3
e) 4
CHEMISTRY 102
Hour Exam I
26.
Fall 2014
Page 6
Draw the Lewis structures for the following four diatomic ions: C22−, N22−, O22−, and
F22+. How many of these four diatomic ions must have a double or triple bond in order to
satisfy the octet rule?
a) 0 (none)
b) 1
c) 2
d) 3
e) 4 (All of these ions must have a double or triple bond in order to satisfy the
octet rule.)
27.
Which of the following statements is true concerning atoms of bromine?
a)
b)
c)
d)
e)
28.
Br should have a more negative electron affinity value than Kr.
Br should have a smaller ionization energy than Br2.
Br should have a smaller electronegativity value than Ba (element #56).
Br should have a smaller radius than Br2+.
Br should have a larger ionization energy than Ne.
Which of the following bonds to selenium should be the most pure (nonpolar) covalent
bond?
a) Se − Ga
29.
31.
c) Se − I
d) Se − In
A pure substance that can be broken down into other substances by chemical change is
classified as a(n):
a) compound
30.
b) Se − Cl
b) element
c) phase
d) solution
e) mixture
Sarin is a nerve gas whose chemical formula has 2 atoms of oxygen for each molecule of
sarin. If 50.0 g of sarin contains 11.4 g of oxygen, calculate the molar mass of sarin.
a) 280. g/mol
b) 35.0 g/mol
d) 210. g/mol
e) 140. g/mol
c) 70. g/mol
How many of the following four compounds is/are named correctly?
MgCO3, magnesium carbonate
P2O5, phosphorus oxide
Co(ClO2)3, cobalt(VI) perchlorate
HNO3, nitric acid
a) 0 (none)
b) 1
c) 2
d) 3
e) 4 (All are correctly named.)
CHEMISTRY 102
HOUR EXAM I
Fall 2014
Page 7
USEFUL CONSTANTS/EQUATIONS
RH = 2.178 × 1018 J
h = 6.626 × 1034 Js
c=
λν
En = RHZ2(1/n2), Z = atomic number
E = hν =
hc/λ
λ = h/mv (de Broglie equation)
N = 6.022 ×
1023
1 cm = 1 × 10−2 m; 1 nm = 1 × 10−9 m
c = 2.998 × 108 m/sec
Density = mass/volume
1 kHz = 1000 Hz = 1000 s−1
Mass % of A =
1 J = 1 kg m2/sec2
mass of A
× 100
totalmass
 1
1 
E = RHZ2  2  2 
 n2
1 mL = 1 cm3
n1 
PERIODIC TABLE OF THE ELEMENTS
1
1A
1
H
1.008
3
Li
6.941
11
Na
22.99
19
K
39.10
37
Rb
85.47
55
Cs
132.9
87
Fr
223
2
2A
4
Be
9.012
12
Mg
24.31
20
Ca
40.08
38
Sr
87.62
56
Ba
137.3
88
Ra
226
3
21
Sc
44.96
39
Y
88.91
57
La*
138.9
89
Ac†
227
*
Lanthanides
†
Actinides
26
Fe
55.85
Atomic number
Atomic mass
4
22
Ti
47.90
40
Zr
91.22
72
Hf
178.5
104
Rf
261
5
23
V
50.94
41
Nb
92.91
73
Ta
180.9
105
Db
262
6
24
Cr
52.00
42
Mo
95.94
74
W
183.9
106
Sg
266
7
25
Mn
54.94
43
Tc
98
75
Re
186.2
107
Bh
262
8
26
Fe
55.85
44
Ru
101.1
76
Os
190.2
108
Hs
265
9
27
Co
58.93
45
Rh
102.9
77
Ir
192.2
109
Mt
266
10
28
Ni
58.70
46
Pd
106.4
78
Pt
195.1
110
Ds
271
11
29
Cu
63.55
47
Ag
107.9
79
Au
197.0
111
12
30
Zn
65.39
48
Cd
112.4
80
Hg
200.6
112
58
Ce
140.1
90
Th
232.0
59
Pr
140.9
91
Pa
231
60
Nd
144.2
92
U
238
61
Pm
145
93
Np
244
62
Sm
150.4
94
Pu
242
63
Eu
152.0
95
Am
243
64
Gd
157.3
96
Cm
247
65
Tb
158.9
97
Bk
247
66
Dy
162.5
98
Cf
251
13
3A
5
B
10.81
13
Al
26.98
31
Ga
69.72
49
In
114.8
81
Tl
204.4
14
4A
6
C
12.01
14
Si
28.09
32
Ge
72.59
50
Sn
118.7
82
Pb
207.2
15
5A
7
N
14.01
15
P
30.97
33
As
74.92
51
Sb
121.8
83
Bi
209.0
16
6A
8
O
16.00
16
S
32.07
34
Se
78.96
52
Te
127.6
84
Po
209
67
Ho
164.9
99
Es
252
68
Er
167.3
100
Fm
257
69
Tm
168.9
101
Md
258
70
Yb
173.0
102
No
259
17
7A
9
F
19.00
17
Cl
35.45
35
Br
79.90
53
I
126.9
85
At
210
71
Lu
175.0
103
Lr
260
18
8A
2
He
4.003
10
Ne
20.18
18
Ar
39.95
36
Kr
83.80
54
Xe
131.3
86
Rn
222
CHEMISTRY 102
Hour Exam I
Fall 2014
Page 8