In the organic compound $\mathrm{CH}_2=\mathrm{CH}-\mathrm{CH}_2-\mathrm{CH}_2-$ $\mathrm{C} \equiv \mathrm{CH}$, the $\mathrm{C}_2-\mathrm{C}_3$ bond is the pair of hybridised orbitals involved in the formation of (a) $s p-s p^2$ (b) $s p-s p^3$ (c) $s p^2-s p^3$ (d) $s p^3-s p^3$

Question

In the organic compound $\mathrm{CH}_2=\mathrm{CH}-\mathrm{CH}_2-\mathrm{CH}_2-$ $\mathrm{C} \equiv \mathrm{CH}$, the $\mathrm{C}_2-\mathrm{C}_3$ bond is the pair of hybridised orbitals involved in the formation of (a) $s p-s p^2$ (b) $s p-s p^3$ (c) $s p^2-s p^3$ (d) $s p^3-s p^3$,

MARKS App · Accepted Answer

(c) When both double and triple bonds are present, double bond is given preference while numbering the carbon chain. Thus, $\therefore \quad \mathrm{C}_2-\mathrm{C}_3$ bond is formed by overlap of $s p^2-s p^3$ orbital. Thus, option (c) is correct.

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