Ozone: Greater dispersion forces and a bent structure (allowing polarity). Polar structure = hydrogen bonds allowing stronger bonds = greater melting and boiling point. Coordinate covalent bond in ozone allows greater reactivity than the covalent bond in oxygen. Oxygen= linear structure= only dispersion forces and that too weaker due to lower molecular weight= weaker intermolecular forces= lower melting and boiling points.
Mostly correct stuff but the setting out should be improved on. The question starts by asking about the differences in structure so that's what you should begin with.
Oxygen is a non-polar molecule with a linear structure, with one double O=O covalent bond.
Ozone is a polar molecule which gives it its bent structure. It contains a coordinate covalent bond (O=O-O you should draw the molecules).
Then it asks for two differences in their properties:
Ozone's higher molar mass (3 Oxygen molecules instead of 2), means it has increased dispersion forces acting on it which gives it higher boiling and melting points than Oxygen.
Since Ozone is polar, it also has strong dipole-dipole forces between molecules , which makes it more soluble in water (also a polar molecule) than oxygen which is non-polar.
Other properties you could include:
Ozone is more reactive and is a stronger oxidising agent, which is due to its unstable structure.
Ozone is more easily decomposed than oxygen which is very stable. This is also due to ozone's unstable structure.
Hope this helps
Someone please correct me if I made any mistakes.