The C-H bond distance is the longest in | vedclass

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(C) The $C-H$ bond length depends on the hybridization of the carbon atom. As the $s$-character in the hybrid orbital increases,the bond length decrea

Vedclass · Accepted Answer

$C_2H_4Br_2$

Vedclass · Answer

(C) The $C-H$ bond length depends on the hybridization of the carbon atom. As the $s$-character in the hybrid orbital increases,the bond length decreases. $C_2H_2$ ($sp$ hybridization,$50\% \ s$-character),$C_2H_4$ ($sp^2$ hybridization,$33.3\% \ s$-character),and $C_6H_6$ ($sp^2$ hybridization) have shorter $C-H$ bonds. In $C_2H_4Br_2$ ($1$,$2$-dibromoethane),the carbon atoms are $sp^3$ hybridized ($25\% \ s$-character). Since $sp^3$ hybridized carbon has the least $s$-character,the $C-H$ bond is the longest. Therefore,the correct option is $C$.

The $C-H$ bond distance is the longest in

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