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(A) 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 decreas

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acetylene

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(A) 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.In acetylene $(HC \equiv CH)$,the carbon is $sp$ hybridized ($50\% \ s$-character).In ethylene $(CH_2=CH_2)$,the carbon is $sp^2$ hybridized ($33.3\% \ s$-character).In methane $(CH_4)$ and ethane $(CH_3-CH_3)$,the carbon is $sp^3$ hybridized ($25\% \ s$-character).Since $sp$ hybridization has the highest $s$-character,the $C-H$ bond length is the shortest in acetylene.

$C-H$ bond length is least in

Similar Questions

$X$ and $Y$ are two covalent molecules in which the hybridization of the central atoms is the same,but their shapes are different. $X$ and $Y$ are:

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