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CHM115 Final Exam Review
CHM115 Final Exam Review
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1
Chemical reactions between nonmetals and nonmetals primarily involve:
interactions between protons and electrons
interactions between protons
transfer of electrons
sharing of electrons
2
Argon atoms do not combine to form Ar
2
molecules, yet Ar atoms do attract to one another weakly through:
Dipole-dipole forces
Ion-dipole forces
Hydrogen bonding
Dispersion forces
3
The BF
6
molecule is:
Polar
Nonpolar
4
A reaction is carried out where the solid dissolves in water causing the flask to be hot to the touch. Which is correct?
ΔH < 0, process is exothermic
ΔH > 0, process is endothermic
ΔH < 0, process is endothermic
ΔH > 0, process is exothermic
5
For an ideal gas, increasing the temperature at constant amount and volume results in:
no change in the pressure
a decrease in the pressure
cannot determine
an increase in the pressure
6
Which is the full electron configuration for Cobalt?
[Ar]
1s22s22p63s23p64s23d7
1s22s22p63s23p63d24s7
1s22s22p63s23p63d74s2
7
What is the density of Cl
2
at 315 K and 0.75 atm?
2.03 x 10-2 g/L
2.44 x 103 g/L
1.03 g/L
2.05 g/L
8
Using the phase diagram below, melting occurs along the:
above point D
AC line
BC line
CD line
9
Using the phase diagram below, a supercritical fluid is found:
at BC line
at AC line
above point D
at CD line
10
Which is the correct formula for iron (III) sulfate?
Fe2SO4
Fe2SO3
Fe2(SO4)3
Fe3(SO4)2
11
Which of the following has the lowest vapor pressure?
HBr
H2O
N2
CCl4
12
How many grams of NH
3
can be produced if 3.90g of H
2
reacts with 4.50g of NO? 2NO + 5H
2
--> 2NH
3
+ 2H
2
O.
2.56 g
33.0 g
5.11 g
13.2 g
13
What is the charge of the anion that sulfur is most likely to form?
2
1
-2
-1
14
What orbital does the image below represent?
s
px
py
dyz
15
Chemical reactions between metals and nonmetals primarily involve:
interactions between protons and electrons
transfer of electrons
sharing of electrons
interactions between protons
16
What orbital does the image below represent?
py
px
dyz
s
17
How many d electrons are there in a Ti
3+
atom?
3
1
2
0
18
Using the phase diagram below, deposition occurs along the:
CD line
above point D
AC line
BC line
19
C
6
H
14
will be:
more soluble in a nonpolar solvent
more soluble in a polar solvent
20
What is the maximum number of orbitals in an atom that can have the quantum numbers n=4, l=1
3
0
1
2
21
The CHCl
3
molecule is:
Nonpolar
Polar
22
Which of the following is a chemical change?
Iron rusting to form Fe2O3
Salt dissolving
Alcohol Evaporating
Butter melting in a frying pan
23
How many total resonance structures are there for SO
2
?
4
1
3
2
24
Which one of these compounds can hydrogen bond with water?
BH3
NH3
CH4
MgBr2
25
How many electrons are in one atom of Fe
3+
?
23
20
21
22
26
What is the maximum number of electrons in an atom that can have the quantum numbers n=3, m
s
=1/2
6
9
3
0
27
Are the molecules below isomers, identical molecules, or neither
isomers
neither
identical
28
If we took 7.5 liters of gas at 1.00 atm and compressed it to 2.0 liters, what would the pressure of that gas be?
1.20 atm
15.0 atm
0.267 atm
3.75 atm
29
Using the phase diagram below, the triple point is found at point:
D
C
B
A
30
What is the volume of 5.0 M AgCl
2
solution required to make 250 mL of a 2.4 M AgCl
2
solution?
0.048 mL
20.8 mL
120 mL
76.9 mL
31
The physical change H
2
O(l) --> H
2
O(g) is called:
Deposition
Condensation
Vaporization
Fusion
32
Which one of the following is an alkaline earth metal in the fifth period?
Rhubidium
Calcium
Strontium
Potassium
33
Which of the following is a compound?
Water
Sugar
Carbon (C)
Magnesium (Mg)
34
Which element will exhibit chemical behavior similar to that of calcium (Ca)?
Potassium
Zirconium
Barium
Carbon
35
The CCl
4
molecule is:
Nonpolar
Polar
36
Which of the following most easily formas an anion?
Al
Au
O
Mg
37
A tank with pressure of 200.0 atm has 2 moles of Ar, 1 mole of Ne and 3 moles of CO
2
. What is the partial pressure Ne?
60.0 atm
66.7 atm
33.3 atm
100 atm
38
Are the molecules below isomers, identical molecules, or neither
isomers
neither
identical
39
Which is the most reasonable prediction for the H-B-H bond angle in BH
3
?
90o
109.5o
120o
107o
40
According to the VSEPR model, the predicted molecular geometry of carbon tetrachloride is:
Bent
Tetrahedral
Linear
Trigonal planar
41
Which of the following is an example of an extensive property?
Weight
Temperature
Boiling point
Concentration
42
Which of the following species has nonpolar covalent bonds?
F2
CO
NaCl
He
43
Using the phase diagram below, at 200
o
C and 1 atm, this substance is most likely a
gas
supercritical fluid
solid
liquid
44
The physical change H
2
O(s) --> H
2
O(l) is called:
Deposition
Fusion
Vaporization
Condensation
45
Using the phase diagram below, at 50
o
C and 1 atm, this substance is most likely a
supercritical fluid
liquid
solid
gas
46
Which element has the following ground state electron configuration? [Kr] 5s
2
4d
10
5p
2
Sn
Sb
Bi
Pb
47
Pi bonds have their e
-
density concentrated above and below the plane of the nuclei of the bonding atoms
False
True
48
After carrying out the operation (19.22+0.027)/3.8188, to how many significant figures must the answer be shown?
1
1
3
4
49
At its ground-state, an atom of Calcium is:
Paramagnetic
Diamagnetic
50
Use the table of bond energies below to calculate an estimate of ΔH for the reaction CH
4
+ 2O
2
→ CO
2
+ 2H
2
O
-349 KJ/mol
-794 KJ/mol
923 KJ/mol
-624 KJ/mol
51
Determine which of the following ions has the smallest atomic radius
Mg2+
O2-
F-
Na+
52
KCl is a ______ electrolyte
Non
Strong
Weak
53
If you heat some liquids & each has only one of the IMFs listed below, which liquid would have the lowest boiling point?
dipole-dipole forces
a, b, and c would all have the same boiling point
dispersion forces
ionic forces
54
What is the charge of the calcium ion in CaCl
2
?
-2
-1
2
1
55
The mass of a sample is 365 milligrams. Which of the following expresses that mass in kilograms?
3.65 x 10-6 kg
3.65 x 104 kg
3.65 x 10-4 kg
3.65 x10-1 kg
56
What quantum number is the most important in determining the shape of an atomic orbital?
The Principle QN, n
They are all equally important
The Magnetic AN, ml
The Angular Momentum QN, l
57
CH
3
COOH is a ______ electrolyte
Strong
Non
Weak
58
What is the term for the total number of protons in the nucleus?
Atomic number
Isotope number
Mass to charge ratio
Mass number
59
How many L of CO
2
will be produced at 32°C and 2.50 bar if 10.0 mL of 2.0 M NaHCO
3
reacts with an excess of 1.5 M H
2
SO
4
0.0213 L
20.3 L
0.406 L
0.203 L
60
Which of the following is evidence of a physical change?
State of matter change
Particle size change
Temperature change
All of the above
61
Which of the following gases would have the largest van der Waals 'b' parameter?
NH3
PH3
H2
He
62
According to kinetic molecular theory, gas particles are:
Neither a nor b
Both a and b
In constant random motion
Small compared to the distanced between them
63
C
6
H
14
is a ______ electrolyte
Non
Strong
Weak
64
What quantum number is the most important in determining the orientation of an atomic orbital?
The Principle QN, n
They are all equally important
The Angular Momentum QN, l
The Magnetic AN, ml
65
Which of the following has the lowest boiling point?
HBr
HF
HCl
HI
66
The H
2
O molecule is:
Polar
Nonpolar
67
Using the phase diagram below, vaporization occurs along the:
BC line
above point D
AC line
CD line
68
Are the molecules below isomers, identical molecules, or neither
identical
neither
isomers
69
Sigma bonds are covalent bonds in which the e
-
density is concentrated between the nuclei of the bonding atoms
True
False
70
How much energy (in Joules) is carried by a photon of light with a wavelength of 405 nm?
4.90 x 10-22 J
4.90 x 10-19 J
2.68 x 10-40 J
4.90 x 10-28 J
71
Which of the following gases would have the largest van der Waals 'a' parameter?
H2
PH3
He
NH3
72
List all possible values of m
l
for orbitals in the 3d subshell
-3,-2,-1,0,1,2,3
0,1,2,3
-2,-1,0,1,2
0,1,2
73
Express 923,820 g using 3 significant figures
9.24 x 105 g
9.20 x 105 g
920 g
9.2 x 105 g
74
Based on their positions in the periodic table, predict which has the largest first ionization energy
F
Cs
N
Li
75
What quantum number is the most important in determining the size of an atomic orbital?
They are all equally important
The Angular Momentum QN, l
The Magnetic AN, ml
The Principle QN, n
76
A sample of gold foil contains 6.20 x 10
23
atoms. What is the mass of the foil?
111 g
0.00523 g
3.17 x 10-22 g
203 g
77
What is the concentration of a solution made by dissolving 0.750 moles of glucose in 150 mL of water?
12.5 M
0.00500 M
0.250 M
5.00 M
78
What type of electron configuration of sulfur is: 1s
2
2s
2
2p
6
3s
2
3p
6
4s
1
Ground state
Excited state
79
What is the charge of the iron ion in FeCl
3
?
-3
-2
3
2
80
Which of the following ions is isoelectronic with Ar?
Mg2+
Ca2+
Na+
Cl2-
81
Which of the following compounds could not exist?
XeI6
CBr5
SF5
IF5
82
Are the molecules below isomers, identical molecules, or neither
isomers
identical
neither
83
“Matter is neither created nor destroyed." This is the:
Law of difinite proportions
Law of multiple proportions
Law of conservation of mass
Dalton's atomic theory
84
Typically, the solubility of a gas in a liquid increases with:
An increase in P and an increase in T
An increase in P and a decrease in T
A decrease in P and a decrease in T
A decrease in P and an increase in T
85
The physical change H
2
O(g) --> H
2
O(l) is called:
Fusion
Condensation
Deposition
Vaporization
86
NaCl will be:
more soluble in a polar solvent
more soluble in a nonpolar solvent
87
Which of the following compounds has the lowest lattice energy?
LiF
RbI
NaCl
KBr
88
Which of the following bonds would be the most polar?
F-I
F-Br
F-Cl
F-F
89
Which of the following has a variable shape but a fixed volume?
Solid
Gas
Liquid
All of the above
90
What is the maximum number of electrons in an atom that can have the quantum numbers n=3, l=2, m
l
=0
4
6
0
2
91
Which one of the following is an alkali metal in the fourth period?
Strontium
Potassium
Calcium
Rhubidium
92
Ascorbic acid has the following percent composition: 40.92% C, 4.58% H, and 54.50% O by mass. MM=176.14g/mol.
C6H8O3
C6H8O6
C3H4O6
C3H4O3
93
Ionic compounds are always represented by ________ formulas?
Molecular
Structural
Orbital
Empirical
94
How many moles of benzoic acid, C
7
H
6
O
2
, are in 40.0 grams of benzoic acid?
4,880 moles
1.38 moles
74.3 moles
0.328 moles
95
List all the possible values of l for orbitals with n = 4
-4,-3,-2,-1,0,1,2,3,4
0,1,2,3
0,1,2,3,4
1,2,3,4
96
Using the phase diagram below, at 200
o
C and 0.25 atm, this substance is most likely a
supercritical fluid
solid
liquid
gas
