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

💡 Solution & Explanation

# Ozone Structure and Bonding **Step 1: Identify ozone's molecular formula and structure** Ozone is $O_3$. Its structure is: $$O=\overset{..}{O}-O^-$$ The central oxygen atom forms one double bond with one terminal oxygen and one single bond with the other terminal oxygen (resonance structures exist). **Step 2: Determine hybridization of central oxygen** The central oxygen atom has: - 1 double bond (1 σ + 1 π bond) - 1 single bond (1 σ bond) - 1 lone pair This requires **3 electron groups** around the central atom. **Step 3: Apply hybridization rules** Three electron groups require $sp^2$ hybridization: - 3 $sp^2$ orbitals (for σ bonds and lone pair) - 1 unhybridized $p$ orbital (for π bond) **Answer: A is $sp^2$ hybridization** The central oxygen atom uses $sp^2$ hybrid orbitals to form σ bonds with both terminal oxygens and accommodate its lone pair, while an unhybridized $p$ orbital forms the π bond in the double bond.