See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Solution **Analyzing each option:** **(A) C-C in benzene vs C=C in ethene** - Benzene: C-C bond is aromatic with resonance stabilization (partial double bond character ~1.5) - Ethene: C=C is a pure double bond - The aromatic C-C bond has **less π-character** than a true double bond, so it requires **less energy to break** - **Benzene C-C bond has LOWER dissociation energy** ✓ **(B) C≡C in propyne vs C≡H in ethyne** - Both contain triple bonds - Triple bonds (C≡C and C≡H) have similar very high bond dissociation energies - C≡H might be slightly higher, but the difference is minimal - Both are strong bonds, not a clear distinction **(C) C=C in cyclopropene vs C=C in allene derivative** - Cyclopropene has ring strain that destabilizes the double bond - The allene structure shown has extended conjugation/stability - Cyclopropene C=C might be weaker, but the comparison is complex **(D) C=O in $COCl_2$ vs C=O in $CH_3COCl$** - Both contain carbonyl groups with similar C=O bond strengths - The electron-withdrawing Cl atoms in both make them comparable - No significant difference in the marked C=O bonds **Answer: (A)** — The aromatic C-C bond in benzene has less dissociation energy than the C=C double bond in ethene because aromatic bonds have reduced π-character compared to pure double bonds.