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

💡 Solution & Explanation

# Determining sp³ Hybridization of Sulfur To identify sp³ hybridization, we need: **4 electron groups around S** (bonds + lone pairs). ## 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 - Electron groups = 2 - Hybridization: **sp** ✗ **(III) $H_2S$:** - S forms 2 single bonds with H atoms - S has 2 lone pairs - Total electron groups = 2 + 2 = **4** - Hybridization: **sp³** ✓ **(IV) $S_8$:** - Each S forms 2 single bonds with neighboring S atoms (ring structure) - Each S has 2 lone pairs - Total electron groups = 2 + 2 = **4** - Hybridization: **sp³** ✓ ## Conclusion: Both **$H_2S$ and $S_8$** have sp³ hybridized S atoms. Since the correct answer is D (typically representing multiple correct options), **both (III) and (IV)** exhibit sp³ hybridization.