Bond length of ethane (I), ethene (II), acety | vedclass

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(C) The bond length depends on the hybridization of the carbon atoms involved in the bond.Ethane $(I)$ has $sp^3$ hybridized carbons, resulting in a $

Vedclass · Accepted Answer

$I > IV > II > III$

Vedclass · Answer

(C) The bond length depends on the hybridization of the carbon atoms involved in the bond.Ethane $(I)$ has $sp^3$ hybridized carbons, resulting in a $C-C$ single bond length of approximately $154 \ pm$.Ethene $(II)$ has $sp^2$ hybridized carbons, resulting in a $C=C$ double bond length of approximately $133 \ pm$.Acetylene $(III)$ has $sp$ hybridized carbons, resulting in a $C \equiv C$ triple bond length of approximately $120 \ pm$.Benzene $(IV)$ has $sp^2$ hybridized carbons with resonance, resulting in a $C-C$ bond length of approximately $139 \ pm$ (intermediate between single and double bonds).Therefore, the order of bond length is: Ethane $(154 \ pm) >$ Benzene $(139 \ pm) >$ Ethene $(133 \ pm) >$ Acetylene $(120 \ pm)$.This corresponds to the order: $I > IV > II > III$.

Bond length of ethane $(I)$, ethene $(II)$, acetylene $(III)$ and benzene $(IV)$ follows the order

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