In terms of intermolecular forces, what are the difference in the boiling points of #O_2# and #O_3# at standard pressure?

1 Answer
Jan 1, 2017

Answer:

Liquid oxygen is bad enough.........

Explanation:

Liquid ozone would constitute an even greater risk. We would predict the #O_3# molecule should have a higher boiling point than dioxygen, on the basis that it is a bigger molecule that should have a greater degree of dispersion forces.

#"normal boiling point of dioxygen"# #-183# #""^@C#

#"normal boiling point of ozone"# #-112# #""^@C#

The boiling points are consistent with the presumed intermolecular forces. There is also some degree of polarity, of charge separation, present in the ozone molecule, i.e. #""^(-)O-^(+)O=O#.

What is the structure of the ozone molecule?