MHTCET 15 May 2024 Shift 1 Paper

Concept:Ozone shows resonance, so both $\mathrm{O}-\mathrm{O}$ bonds are equivalent with a bond order of about $1.5$.Explanation:The two resonance structures of ozone place the double bond on alternate oxygen atoms.The actual molecule is a resonance hybrid of these structures.Hence, neither bond is a pure single bond nor a pure double bond.A typical $\mathrm{O}-\mathrm{O}$ single bond is about $148\ \mathrm{pm}$, while a typical $\mathrm{O}=\mathrm{O}$ double bond is about $121\ \mathrm{pm}$.The resonance hybrid has a bond length intermediate between these two values.Experimentally, the $\mathrm{O}-\mathrm{O}$ bond length in ozone is $128\ \mathrm{pm}$.Answer:$\mathrm{O}-\mathrm{O}$ bond length in ozone is $128\ \mathrm{pm}$, which corresponds to option A.