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

💡 Solution & Explanation

# Ozone Structure Analysis **Step 1: Identify the molecular structure of ozone ($O_3$)** Ozone has a bent/angular structure with three oxygen atoms. The central oxygen forms bonds with two terminal oxygen atoms. **Step 2: Determine bonding in the central oxygen** - The central O forms one single bond ($\sigma$) with one terminal O - The central O forms one double bond ($\pi + \sigma$) with the other terminal O - This requires **2 hybrid orbitals** for $\sigma$ bonding **Step 3: Account for lone pairs** The central oxygen has: - 2 bonding pairs (one with each terminal O) - 1 lone pair of electrons - Total: 3 electron pairs around the central atom **Step 4: Determine hybridization** With 3 electron pairs requiring 3 orbitals to accommodate them: - Hybridization = $sp^2$ **Step 5: Verify with geometry** $sp^2$ hybridization produces trigonal planar electron geometry with a bent molecular shape due to the lone pair, which matches ozone's structure. --- **Answer: A — The central oxygen atom uses $sp^2$ hybridization** The three electron pairs (2 bonding + 1 lone pair) around the central atom require $sp^2$ hybrid orbitals to accommodate them.