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 in Sulfur Species **Key Concept:** sp³ hybridization requires 4 electron groups (bonding + lone pairs) around the central atom. ## Analysis of 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 with O atoms - Steric number = 2 (2 bonding pairs, 1 lone pair) - Hybridization: **sp** ✗ **(III) $H_2S$:** - S forms 2 single bonds with H atoms - Steric number = 4 (2 bonding pairs, **2 lone pairs**) - Electron groups = 4 → Hybridization: **sp³** ✓ **(IV) $S_8$:** - Sulfur atoms form single bonds in a ring structure - Each S atom: 2 bonding pairs + 2 lone pairs - Steric number = 4 → Hybridization: **sp³** ✓ ## Conclusion: Both **(III) $H_2S$** and **(IV) $S_8$** have S atoms in sp³ hybridization state. Since answer **D** typically represents "both III and IV," this is the correct answer.