In an organic compound,what is the effect of | vedclass

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(B) The hybridization of carbon atoms significantly influences the properties of the $C-H$ or $C-C$ bonds.$(I)$ As the $s$-character in a hybrid orbit

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Higher $s$-character leads to shorter bond length and higher bond enthalpy.

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(B) The hybridization of carbon atoms significantly influences the properties of the $C-H$ or $C-C$ bonds.$(I)$ As the $s$-character in a hybrid orbital increases (e.g.,$sp > sp^2 > sp^3$),the hybrid orbital becomes closer to the nucleus.$(II)$ This results in a shorter bond length because the electrons are held more tightly by the nucleus.$(III)$ Consequently,the bond becomes stronger,leading to a higher bond enthalpy.$(IV)$ Additionally,the electronegativity of the carbon atom increases with higher $s$-character.

List-$I$	List-$II$
$A$. Ethane	$1$. $2 \ sp$ carbons
$B$. Ethylene	$2$. $6 \ sp^2$ carbons
$C$. Acetylene	$3$. $2 \ sp^3$ carbons
$D$. Benzene	$4$. $2 \ sp^2$ carbons
	$5$. $1 \ sp$ and $1 \ sp^2$ carbons

In an organic compound,what is the effect of the hybridization of carbon on bond length and bond enthalpy?

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Match the following lists:
List-$I$ List-$II$
$A$. Ethane $1$. $2 \ sp$ carbons
$B$. Ethylene $2$. $6 \ sp^2$ carbons
$C$. Acetylene $3$. $2 \ sp^3$ carbons
$D$. Benzene $4$. $2 \ sp^2$ carbons
$5$. $1 \ sp$ and $1 \ sp^2$ carbons

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