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

💡 Solution & Explanation

# Ozone Structure Analysis **Ozone ($O_3$) Lewis Structure:** - Central oxygen atom is bonded to two terminal oxygen atoms - Structure: O=O-O (with resonance to O-O=O) **Hybridization of Central Oxygen:** 1. **Count electron groups around central O:** - 1 double bond to one O atom = 1 electron group - 1 single bond to other O atom = 1 electron group - 1 lone pair = 1 electron group - **Total = 3 electron groups** 2. **Hybridization determination:** - 3 electron groups → **$sp^2$ hybridization** 3. **Orbital arrangement:** - 3 $sp^2$ hybrid orbitals arranged trigonally - Geometry around central O: **bent/angular** (bent molecular shape, trigonal planar electron geometry) - 1 unhybridized p-orbital perpendicular to the plane participates in resonance **Answer: A** — The central oxygen atom uses **$sp^2$ hybridization** This allows the formation of one σ-bond and one π-bond with adjacent oxygens, plus accommodation of a lone pair, with the structure stabilized by resonance.