Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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Which
of the following statements concerning intermolecular forces are CORRECT?
1. | London dispersion forces exist in all molecular
solids. | 2. | Dipole-dipole
attractions occur in all molecules that contain polar bonds. | 3. | Hydrogen bonding only occurs for molecules containing OH
bonds. | | |
a. | 1
only | b. | 2
only | c. | 3
only | d. | 1 and
2 | e. | 1, 2, and
3 | | |
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2.
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Which
one of the following substances will exhibit dipole-dipole intermolecular forces?
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3.
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What
intermolecular force or bond is primarily responsible for the solubility of H2S in
water? a. | ion-dipole
force | b. | dipole-dipole force | c. | ionic
bonding | d. | covalent bonding | e. | hydrogen
bonding | | |
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4.
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What
intermolecular force or bond is primarily responsible for the solubility of chlorine (Cl2)
in water? a. | dipole/dipole
force | b. | hydrogen bonding | c. | dipole/induced
dipole force | d. | ion-dipole force | e. | ion-induced
dipole force | | |
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5.
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As
molecular solids, which of the following will exhibit dipole-dipole intermolecular forces:
PH3, SO3, Br2, and SiCl4? a. | PH3
only | b. | PH3
and SO3 | c. | SO3 and SiCl4 | d. | Br2
and SiCl4 | e. | PH3, SO3, and
SiCl4 | | |
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6.
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Which
of the following molecules will have the highest boiling point?
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7.
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Which
one of the following molecules will have the lowest boiling point? a. | CCl4 | b. | CHCl3 | c. | CH2Cl2 | d. | CH3Cl | e. | CH4 | | |
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8.
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Which
is the dominant intermolecular force present in formic acid, HCO2H(l)? a. | London
dispersion | b. | ionic bonding | c. | hydrogen
bonding | d. | dipole-dipole | e. | dipole/induced
dipole | | |
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9.
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Arrange H2O, H2S, and H2Se in order from lowest to
highest boiling point. a. | H2O < H2S <
H2Se | b. | H2O < H2Se <
H2S | c. | H2S < H2Se <
H2O | d. | H2S < H2O <
H2Se | e. | H2Se < H2O <
H2S | | |
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10.
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Hydrogen bonding is present in all of the following molecular solids EXCEPT ____
. a. | CH3OCH3 | b. | H2O | c. | NH3 | d. | HF | e. | H2O2 | | |
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11.
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Which
of the following is NOT a network solid? a. | graphite | b. | diamond | c. | buckminster fullerene
(C60) | d. | silicon dioxide | e. | elemental
silicon | | |
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12.
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Arrange NaCl, HCl, CCl4, and GeCl4 in order of increasing
boiling point. a. | HCl <
CCl4 < GeCl4 < NaCl | b. | HCl <
GeCl4 < CCl4 < NaCl | c. | CCl4
< NaCl < HCl < GeCl4 | d. | GeCl4 < NaCl < HCl <
CCl4 | e. | NaCl < GeCl4 < CCl4 <
HCl | | |
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13.
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Which
of the following properties of water can be attributed to hydrogen
bonding?
1. | high melting point | 2. | high heat of vaporization | 3. | low vapor pressure | 4. | high surface tension | | |
a. | 1 and 3 | b. | 2 and
3 | c. | 2, 3, and
4 | d. | 1, 3, and
4 | e. | 1, 2, 3, and
4 | | |
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14.
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The
tendency of a liquid that tends to minimize its surface area is called a. | capillary
action | b. | viscosity | c. | surface
tension | d. | vaporization | e. | none of the
above | | |
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15.
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The
measure of the resistance to the flow of a liquid is called a. | vapor pressure
| b. | viscosity | c. | sublimation | d. | condensation | e. | none of the above | | |
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16.
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Liquids that
have high vapor pressure and low boiling points are called a. | abnormal liquids
| b. | volatile liquids
| c. | non-volatile liquids
| d. | viscous liquids
| e. | none of the
above | | |
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17.
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How
many joules of heat are needed to completely vaporize 24.40 grams of water at its boiling
point? Given ΔHvap = 40.6 kJ/mol a. | 54.97 | b. | 5.5 x
104 | c. | 29.98 | d. | 3.00 x
104 | e. | none of the above | | |
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18.
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How many
kilojoules of heat are needed to completely vaporize 42.8 grams of C4H10C at
its boiling point? Given ΔHvap = 26.5kJ/mol a. | 74.12
kJ | b. | 9.49
kJ | c. | 15.3
kJ | d. | 16.3
kJ | e. | none of the
above | | |
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19.
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When
sufficient quantity of heat has been added to reach the boiling point of a solution, what happens to
any additional heat added? a. | Additional heat raises the temperature of the liquid which in turn
increases the rate at which boiling occurs. | b. | Additional heat lowers
the intermolecular forces of the liquid which in turn increases the volatility of the liquid.
| c. | Additional heat alters
the viscosity and the surface tension of the liquid which raises the vapor pressure and increases the
boiling point which is why you must continually heat the solution. | d. | Additional heat is used
to maintain the boiling of the liquid as the process is endothermic and requires continued input of
energy. | e. | None of the above are correct
statements. | | |
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20.
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How much
energy does it take to melt a 16.87 g ice cube?
ΔHfus = 6.02
kJ/mol a. | 102 kJ
| b. | 108
kJ | c. | 936 J
| d. | 5.64 kJ
| e. | None of the
above | | |
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