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.

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

Similar Questions

In which of the following compounds is the underlined carbon atom $sp^3$ hybridized?

Number of $sp$ hybridised carbon atoms in the given compound is:
$CH_2 = CH - C \equiv C - CH_2 - CN$

$CH_3-CH_2-CH=CH_2$ has hybridisation

The total number of $\pi-$bond electrons in the following structure is

The hybridisation of each carbon in the following compound respectively is:
$CH_3-C(=O)-CH_2-CN$

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