In the series ethane,ethylene and acetylene,t | vedclass

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(D) The $C-H$ bond energy depends on the hybridization of the carbon atom.In ethane $(C_2H_6)$,carbon is $sp^3$ hybridized ($25\% \ s$-character).In e

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Greatest in acetylene

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(D) The $C-H$ bond energy depends on the hybridization of the carbon atom.In ethane $(C_2H_6)$,carbon is $sp^3$ hybridized ($25\% \ s$-character).In ethylene $(C_2H_4)$,carbon is $sp^2$ hybridized ($33.3\% \ s$-character).In acetylene $(C_2H_2)$,carbon is $sp$ hybridized ($50\% \ s$-character).As the $s$-character increases,the electronegativity of the carbon atom increases,which pulls the bonding electrons closer to the nucleus,resulting in a shorter and stronger $C-H$ bond.Therefore,the $C-H$ bond energy is greatest in acetylene.

In the series ethane,ethylene and acetylene,the $C-H$ bond energy is

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