Answer: The correct answer is Option D.
Explanation:
To calculate the hybridization of [tex]SO_2[/tex], we use the equation:
[tex]\text{Number of electron pair}=\frac{1}{2}[V+N-C+A][/tex]
where,
V = number of valence electrons present in central atom (S) = 6
N = number of monovalent atoms bonded to central atom = 0
C = charge of cation = 0
A = charge of anion = 0
Putting values in above equation, we get:
[tex]\text{Number of electron pair}=\frac{1}{2}[6]=3[/tex]
The number of electron pair around the central metal atom are 3. This means that the hybridization will be [tex]sp^2[/tex] and the electronic geometry of the molecule will be trigonal planar.
Hence, the correct answer is Option D.
