To determine the hybridization of the central atom in \( \text{SO}_2 \), let's analyze the molecule step-by-step.
1. Identify the central atom: In \( \text{SO}_2 \), the central atom is sulfur (S).
2. Count the number of valence electrons:
- Sulfur has 6 valence electrons.
- Each oxygen atom has 6 valence electrons (2 oxygens contribute \( 6 \times 2 = 12 \) electrons).
3. Determine the bonding and lone pairs around the central atom:
- In \( \text{SO}_2 \), sulfur forms a double bond with each oxygen atom.
- Sulfur has one lone pair of electrons remaining.
4. Calculate the steric number (the number of regions of electron density):
- Sulfur has 2 double bonds + 1 lone pair = 3 regions of electron density.
5. Determine the hybridization based on the steric number:
- A steric number of 3 corresponds to \( sp^2 \) hybridization.
Therefore, the hybridization of the central atom in \( \text{SO}_2 \) is \( sp^2 \).
So, the correct answer is:
b) [tex]\( sp^2 \)[/tex]
