Question

which molecule exhibits resonance? co₂ o₃ becl₂ nf₃

Explanation:

Step1: Recall resonance conditions

Resonance occurs when a molecule has delocalized electrons and can be represented by multiple valid Lewis structures.

Step2: Analyze each molecule

• \( \text{CO}_2 \): Linear, double bonds between C and O, no resonance (two equivalent but not delocalized in a way requiring resonance).
• \( \text{O}_3 \): Ozone has a central O bonded to two O atoms. It has a resonance structure due to delocalized π electrons (one single and one double bond, which can switch).
• \( \text{BeCl}_2 \): Linear, sp hybridization, no resonance (single bonds, electron distribution fixed).
• \( \text{NF}_3 \): Trigonal pyramidal, single bonds, no resonance (electron distribution fixed).

Answer:

\( \text{O}_3 \) (Ozone) exhibits resonance.