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

💡 Solution & Explanation

# Solution: Determining sp³ Hybridization in Sulfur Species **Concept:** Hybridization is determined by the number of electron groups (bonding + lone pairs) around the central atom. - sp³ hybridization requires **4 electron groups** --- ## Analysis of Each Species: **(I) $SO_3$:** - S forms 3 double bonds with O atoms - Electron groups = 3 - Hybridization: **sp²** ✗ **(II) $SO_2$:** - S forms 2 double bonds with O atoms + 1 lone pair - Electron groups = 3 - Hybridization: **sp²** ✗ **(III) $H_2S$:** - S forms 2 single bonds with H atoms + 2 lone pairs - Electron groups = 4 - Hybridization: **sp³** ✓ **(IV) $S_8$:** - Crown-shaped ring structure with S-S single bonds - Each S atom forms 2 single bonds to neighboring S atoms + 2 lone pairs - Electron groups = 4 - Hybridization: **sp³** ✓ --- **Species with sp³ hybridization: (III) and (IV)** Therefore, the answer is **D** (both III and IV show sp³ hybridization in sulfur).