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

$sp^2$ carbon is not present in

Amongst the given options,the compound$(s)$ in which all the atoms are in one plane in all the possible conformations (if any),is (are):
$(A)$ $CH_2=CH-CH=CH_2$
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$(C)$ $H_2C=C=O$
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The hybridisations of carbon-$2$ in $P$ and $Q$ are respectively:

Which of the following bonds is most acidic?

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