Chapter 11: Intermolecular Forces of Attraction
1. Using your decision matrix, determine the predominant intermolecular force of attraction that
is found in each of the following substances.
a. AgCl (s)
b. Ne (g)
c. CaBr2 (aq)
d. HBr (l)
e. O3 (g)
f.
XeF4 (s)
g. BCl3 (s)
h. H2O (l)
i.
2.
CH3NH
Look at each of the following PAIRS and determine which has the higher melting or boiling
temperature. To do this first determine what type of Intermolecular force is predominant in
each cpd or element. (The stronger the Intermolecular force the higher the temperature at
which it melts. If the two cpds/substances have the same type of IF then the one with the higher
mass/electron density will have the higher melting/boiling temperature)
a. SF4 (s) or NaCl (s)
b. SF4 (s) or XeF4 (s)
c. NH3 (g) or H2S (g)
d. BCl3 (s) or PCl3(s)
e. Sulfur (s) or Boron (s)
f.
3.
CH3CH3 (l) or CH3OH (l)
Look at each of the following PAIRS and determine which will evaporate faster. To do this
determine the predominant IF. (The higher the force, the slower it will evaporate. The lower
the force the faster it evaporates and the higher its vapor pressure will be.)
a. H2O (l) or K2O (s)
b.
CO2 or SeO2 (draw first)
c.
Kr (s) or I2(s)
d.
CH4
e.
NH3 or BH3
or CCl4