In ozone, the central oxygen atom uses — p Block Elements Chemistry Question

💡 Solution & Explanation

# Ozone Structure and Central Oxygen Hybridization **Step 1: Identify the structure of ozone ($O_3$)** Ozone has a bent/angular structure with resonance forms: $$O=O^{+}-O^{-} \longleftrightarrow O^{-}-O^{+}=O$$ **Step 2: Analyze bonding around the central oxygen** The central oxygen atom forms: - One $\sigma$ bond with the left oxygen - One $\sigma$ bond with the right oxygen - One $\pi$ bond (delocalized in resonance) **Step 3: Count electron domains** - 2 bonding pairs (the two $\sigma$ bonds) - 1 lone pair on the central oxygen - **Total: 3 electron domains** **Step 4: Determine hybridization** 3 electron domains require **$sp^2$ hybridization** (3 hybrid orbitals to accommodate all electron domains). --- **Answer: A — The central oxygen atom uses $sp^2$ hybridization** This provides the correct geometry (bent molecular shape) and accounts for the resonance bonding with delocalized $\pi$ electrons characteristic of ozone.