Name: 
 

Chapter 11 Online Practice


Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 
Hydrogen bonding is present in all of the following molecular solids EXCEPT ____ .
a.
CH3OCH3
b.
H2O
c.
NH3
d.
HF
e.
H2O2
 

 2. 
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
 

 3. 
Which intermolecular forces are present in PCl3(s)?

1.
London dispersion
2.
dipole-dipole
3.
hydrogen bonding
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
1 and 3
 

 4. 
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
 

 5. 
Which one of the following molecules will have the lowest boiling point?
a.
CCl4
b.
CHCl3
c.
CH2Cl2
d.
CH3Cl
e.
CH4
 

 6. 
For which of the following pure solids is it necessary to break covalent bonds to make a liquid or gas?
a.
NaCl
b.
NH3
c.
CH3CO2H
d.
Kr
e.
SiO2
 

 7. 
The toughness of the skin of a liquid is a measure of its ____.
a.
meniscus quality
b.
adhesive forces
c.
dispersion forces
d.
viscosity
e.
surface tension
 

 8. 
Which of the following liquids will have the largest enthalpy of vaporization?
a.
C3H8
b.
C4H10
c.
C4H8
d.
C5H12
e.
C6H14
 

 9. 
Which of the following molecules would be expected to form hydrogen bonds in the liquid or solid state: ethylene glycol (HOCH2CH2OH), methanol (CH3OH), and formaldehyde (H2CO)?
a.
ethylene glycol only
b.
methanol only
c.
formaldehyde only
d.
ethylene glycol and methanol
e.
ethylene glycol, methanol, and formaldehyde
 

 10. 
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
 

 11. 
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
 

 12. 
Which of the following statements concerning the phase diagram below are CORRECT?

chapter_11_online_p_files/i0130000.jpg

1.
Moving from point B to A results in a phase transition from liquid to gas.
2.
Point D lies at the critical point.
3.
At point C, liquid and gas phases coexist at equilibrium.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 3
e.
2 and 3
 

 13. 
The normal boiling point is defined as
a.
the temperature at which the vapor pressure of a liquid equals 1 atm.
b.
the pressure at which any liquid boils at 273.15 K.
c.
the temperature at which water always boils.
d.
the pressure of a gas when its temperature reaches 373.15 K.
e.
the temperature at which the enthalpy of vaporization equals 40.7 kJ/mol.
 

 14. 
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
 

 15. 
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
 

 16. 
Which one of the following substances will exhibit dipole-dipole intermolecular forces?
a.
C2H4
b.
SO2
c.
CO2
d.
F2
e.
Ar
 

 17. 
Which of the following gases can be liquefied at 25 °C?

Gas
boiling pt.
critical temp.
CH 4
-161.5 ° C
-82.6 ° C
C 3 H 8
-42.1 ° C
+96.7 ° C
O 2
-183 ° C
-119 ° C
a.
CH4 only
b.
C3H8 only
c.
O2 only
d.
CH4 and O2
e.
C3H8 and O2
 

 18. 
Which of the following statements are correct?

1.
Above the critical pressure, only the solid phase of a pure substance can exist.
2.
Above the critical temperature, a gas may not be condensed to a liquid.
3.
At the critical point, three phases (gas, liquid, and solid) may coexist at equilibrium.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
1 and 3
 

 19. 
Which of the following molecules will have the highest boiling point?
a.
H2
b.
CH4
c.
Ne
d.
Cl2
e.
O2
 

 20. 
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
 

 21. 
Which of the following statements concerning the attraction of ions to polar molecules are CORRECT?

1.
The energy of attraction between an ion and a polar molecule is inversely proportional to the distance between the center of the ion and the oppositely charged pole of the dipole.
2.
The higher the ion charge, the greater the attraction between the ion and a polar molecule.
3.
The greater the dipole moment, the greater the attraction between the ion and a polar molecule.
a.
1 only
b.
2 only
c.
3 only
d.
2 and 3
e.
1, 2, and 3
 

 22. 
Which intermolecular force or bond is responsible for the density of H2O(s) being less than that of H2O(l)?
a.
London dispersion forces
b.
hydrogen bonding
c.
ionic bonding
d.
covalent bonding
e.
dipole/induced dipole forces
 

 23. 
Ammonia, NH3, is used as a refrigerant. At its boiling point of -33 °C, the enthalpy of vaporization of ammonia is 23.3 kJ/mol. How much heat is required to vaporize 355 g of ammonia at -33 °C?
a.
1.12 kJ
b.
152 kJ
c.
251 kJ
d.
486 kJ
e.
8.27 ´ 103 kJ
 

 24. 
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
 

 25. 
Which of the following phase transitions is endothermic?
a.
gas to solid
b.
liquid to gas
c.
liquid to solid
d.
gas to liquid
e.
none of the above
 

 26. 
Which process requires the greatest endothermic change in enthalpy for water?
a.
freezing
b.
condensation
c.
vaporization
d.
melting
e.
sublimation
 



 
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