Maximum bond energy of C-H bonds is found in | vedclass

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

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Ethyne

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(C) The bond energy of a $C-H$ bond depends on the hybridization of the carbon atom. As the $s$-character in the hybrid orbital increases,the electronegativity of the carbon atom increases,making the $C-H$ bond shorter and stronger. In $Ethane$ $(C_2H_6)$,carbon is $sp^3$ hybridized ($25\% \ s$-character). In $Ethene$ $(C_2H_4)$,carbon is $sp^2$ hybridized ($33.3\% \ s$-character). In $Ethyne$ $(C_2H_2)$,carbon is $sp$ hybridized ($50\% \ s$-character). Since $Ethyne$ has the highest $s$-character,it has the strongest and shortest $C-H$ bond,resulting in the maximum bond energy.

Maximum bond energy of $C-H$ bonds is found in the compound:

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