The type of hybrid orbitals used by the chlor | vedclass

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(A) The hybridization of the central atom is calculated using the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is the number of valence electro

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$sp^3$

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(A) The hybridization of the central atom is calculated using the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is the number of valence electrons,$M$ is the number of monovalent atoms,$C$ is the cationic charge,and $A$ is the anionic charge.For $ClO_2^-$,$V = 7$ (for $Cl$),$M = 0$ (oxygen is divalent),$C = 0$,and $A = 1$.$H = \frac{1}{2}(7 + 0 - 0 + 1) = \frac{8}{2} = 4$.$A$ value of $4$ corresponds to $sp^3$ hybridization.Therefore,the chlorine atom in $ClO_2^-$ is $sp^3$ hybridized,resulting in an angular (bent) shape due to the presence of two lone pairs.

The type of hybrid orbitals used by the chlorine atom in $ClO_2^-$ is

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