Question

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

Answer 1

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?