Hybridisation in SO₂ is:

Concept:

Hybridization:

• The atomic orbitals s, p, d, f of the central atom having compatible energies mix up. 
• This leads to the formation of new hybrid orbitals which have now different energies, shapes, and orientations than the component atomic orbitals.
• The number of hybrid orbitals is equal to atomic orbitals mixing.
•  After the formation of hybrid orbitals, they overlap with atomic orbitals of suitable side atoms and leads to the formation of covalent chemical bonds.
• The formula for calculating hybridization - H = ½ ( V + M - C + A )
• Where V = number of valence electrons on the central atom. M = No. Of monovalent atoms C = cationic charge A = anionic charge.

Few types of hybridization, their modes of mixing, and geometry of molecules are-

Explanation:

• SO₂ molecule, sulfur is the central atom.

H = ½ (V + M - C + A)

• Putting this in the formula, we get H = 3, which corresponds to sp² hybridization. The structure of the SO₂ molecule is

Thus, the hybridization in SO₂ is sp².

• In SO₂, the lone pair of electrons is housed on an sp² hybrid orbital.
• Due to this lone pair, there is electron-pair - bond pair repulsion and the bond angle deviates from the ideal bond angle 120.