# What is the difference in the boiling points of O_2 and O_3 at standard pressure in terms of intermolecular forces?

This site lists the boiling point of ozone as $- 112$ ""^@C.
The normal boiling point of oxygen is $- 183$ ""^@C, so the difference in volatility is quite substantial. Of course, ozone is a heavier molecule, with a bigger electron cloud, and consequently greater dispersion forces to increase intermolecular forces. However, the large difference in boiling point probably also reflects the polarity of the ozone molecule, the which we draw with formal positive and negative charges.