Comment on the nature of two S–O bonds formed in `SO_(2)` molecule. Are the two S–O bonds in this molecule equal ?

Explanation

The electronic configuration of S is `1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(4)`.
During the formation of `SO_(2)`, one electron from 3p orbital goes to the 3d orbital and S undergoes `sp_(2)` hybridization. Two of these orbitals form sigma bonds with two oxygen atoms and the third contains a lone pair. p-orbital and d-orbital contain an unpaired electron each. One of these electrons forms pπ- pπ bond with one oxygen atom and the other forms pπ- dπ bond with the other oxygen. This is the reason `SO_(2)` has a bent structure. Also, it is a resonance hybrid of structures I and II.

Both S−O bonds are equal in length (143 pm) and have a multiple bond character.