NAME:

MODS:
IMF Practice
1.
Three heats of vaporization were measured and found to be 34.5 kJ/mol, 1.8 kJ/mol and
6.8 kJ/mol. Match these to the following substances: liquid O2, liquid Ne, and liquid
methanol, CH3OH.
2.
For each of the following substances, tell what type of Intermolecular Forces are expected:
Kr
NH3
HI
CH3CH2OH
C2H6
CH3F
3.
Arrange the following substances in order of increasing magnitude of London Dispersion
forces: SiF4, Xe, CF4, GeF4, CH4, Pb
4.
Methane, CH4, reacts with chlorine, Cl2, to produce the following chlorinated hydrocarbons:
methyl chloride (CH3Cl), methylene chloride (CH2Cl2), chloroform (CHCl3), and carbon
tetrachloride (CCl4). Which compound will have the lowest boiling point, and why?
5.
Why is the boiling point of CH4 significantly lower than the boiling point of HF?
6.
Which of the following would be expected to have the highest boiling point?
a)
C2H6
b)
C3H8
c)
C5H12
d)
C4H10
7.
Which of the following would be expected to have the highest boiling point?
a)
H2Te
b)
H2O
c)
H2S
d)
H2Se
8.
Both of the following molecules have a formula of C4H10. Which one will have the lower
boiling point, and why?
9.
Draw 8 liquid water molecules (bent, with lone pairs!) connected by Hydrogen bonds.