91Ó°ÊÓ

In both SO₂ and SO₃, sulfur is the central atom with trigonal planar electron domain geometry. In SO₂, sulfur undergoes sp² hybridization and forms two σ bonds with oxygen atoms, along with two π bonds created by overlapping p-orbitals. In SO₃, sulfur also undergoes sp² hybridization and forms three σ bonds with oxygen atoms, while the π electrons are delocalized over the entire molecule, resulting in resonance structures. In the molecular orbital model, the π bonding in SO₂ comprises one bonding π MO, one non-bonding MO, and one antibonding π* MO. In SO₃, the π bonding involves two bonding π MOs, one non-bonding MO, and one antibonding π* MO, accounting for delocalization and resonance.