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

Jan 1, 2017

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.

$\text{normal boiling point of dioxygen}$ $- 183$ ""^@C

$\text{normal boiling point of ozone}$ $- 112$ ""^@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?