How is the molecule bonded?
The Lewis structures of ozone indicate that the central atom has three electron domains with a triangular planar geometry. As only two of the domains are bonding, the molecular geometry is bent or V-shaped. The greater repulsion of the lone pair gives a bond angle of about 177°. The double bond is composed of a sigma bond from the overlap of hybrid orbitals, and a pi bond from the overlap of unhybridized p orbitals. The electrons of the pi bond are less tightly held so become delocalized through the structure. As there are three pairs of electrons in two bonding positions, the bond order is 1.5. This means that the bonds are intermediate in length and strength between single and double bonds. The only bonded atoms in ozone are oxygen, therefore it should not be polar. The fact that is it polar is surprising, but it can be explained by the unequal distribution of electrons throughout the structure.