See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Solution: Resonance Energy Comparison **Key Principle:** Resonance energy is the stabilization gained from delocalization of electrons across multiple resonance structures. Greater number of stable resonance structures = higher resonance energy. ## Analysis of Option (C): **Benzoate anion** ($C_6H_5COO^{\ominus}$): - The negative charge on oxygen is delocalized into the benzene ring - Generates **4 significant resonance structures**: - Charge on each ortho position (2 structures) - Charge on each para position (1 structure) - Original structure with charge on oxygen (1 structure) - All structures are relatively stable - **High resonance energy** **Phenoxide anion** ($C_6H_5O^{\ominus}$): - The negative charge on oxygen is delocalized directly into the benzene ring - Generates **4 resonance structures** (charge at ortho and para positions) - However, these structures have **lower stability** because they place negative charge on less electronegative carbon atoms - **Lower resonance energy** than benzoate ## Why other options fail: **(A)** $CH_3COOH$ vs $CH_3COONa$: No significant resonance; both have similar structure **(B)** Enol form is unstable; keto form dominates—minimal resonance contribution **(D)** Naphthalene vs indane: Naphthalene has extended conjugation but less resonance stabilization than benzoate **(E)** Benzene is already aromatic; 1,3,5-hexatriene has fewer resonance contributors **Benzoate anion (Option C) has the highest resonance energy** due to the optimal combination of multiple stable resonance structures and effective charge delocalization.