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

1 Answer
anor277
Jan 1, 2017

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?

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