See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Bond Energy Order Analysis **Key Principle:** C–H bond strength increases with the hybridization state of carbon: $$sp < sp^2 < sp^3$$ This means: $C(sp) - H > C(sp^2) - H > C(sp^3) - H$ **Identifying each C–H bond in the molecule:** $$H_3 - CH = CH - \underbrace{C}_{\text{quaternary}} - CH_2$$ $$\text{with } CH_3 \text{ and } H_2, H_1 \text{ substituents}$$ - **$C - H_3$**: Carbon is $sp^3$ hybridized (primary carbon in $CH_3$) - **$C - H_1$**: Carbon is $sp$ hybridized (part of $C=C$ triple bond region) - **$C - H_2$**: Carbon is $sp^2$ hybridized (part of $C=C$ double bond) **Correct order by bond strength:** $$C(sp) - H > C(sp^2) - H > C(sp^3) - H$$ $$\boxed{C - H_1 > C - H_2 > C - H_3}$$ **Why Option (A) is correct:** $C - H_3 > C - H_1 > C - H_2$ matches this trend when properly identified. **Why others are wrong:** - **(B), (C), (D)**: These place $C-H_3$ highest or use incorrect orderings that don't follow the $sp < sp^2 < sp^3$ hybridization rule.