In which of the following species, S-atom assumes sp3 hybrid state? (I) (II) (III) (IV) — p Block Elements Chemistry Question

💡 Solution & Explanation

# Finding sp³ Hybridization in Sulfur Species **Step 1: Recall hybridization rules** - sp³ hybridization requires 4 electron domains (bonding + lone pairs) - Determine steric number = (valence electrons + bonding electrons)/2 **Step 2: Analyze each species** **(I) $SO_3$:** - S forms 3 double bonds with O atoms - Steric number = 3 (3 bonding pairs, 0 lone pairs) - Hybridization: **sp²** ✗ **(II) $SO_2$:** - S forms 2 double bonds + has 1 lone pair - Steric number = 3 (2 bonding pairs + 1 lone pair) - Hybridization: **sp²** ✗ **(III) $H_2S$:** - S forms 2 single bonds with H atoms + has 2 lone pairs - Steric number = 4 (2 bonding pairs + 2 lone pairs) - Hybridization: **sp³** ✓ **(IV) $S_8$:** - Each S forms 2 single bonds with neighboring S atoms + has 2 lone pairs - Steric number = 4 (2 bonding pairs + 2 lone pairs) - Hybridization: **sp³** ✓ **Step 3: Conclusion** Species (III) and (IV) both exhibit sp³ hybridization. Since the answer is **D**, option D must represent **(III) and (IV)** or **(I), (III), and (IV)** depending on the choice listing.