The type of hybrid orbitals used by the chlor | vedclass

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(A) To determine the hybridization of the chlorine atom in $ClO_2^-$,we use the formula: $H = \frac{1}{2} [V + M - C + A]$Where $V$ is the number of v

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$sp^3$

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(A) To determine the hybridization of the chlorine atom in $ClO_2^-$,we use the formula: $H = \frac{1}{2} [V + M - C + A]$Where $V$ is the number of valence electrons of the central atom $(Cl = 7)$,$M$ is the number of monovalent atoms attached ($0$ in this case,as oxygen is divalent),$C$ is the cationic charge $(0)$,$A$ is the anionic charge $(1)$.$H = \frac{1}{2} [7 + 0 - 0 + 1] = \frac{8}{2} = 4$.$A$ value of $4$ corresponds to $sp^3$ hybridization.$ClO_2^-$ has two lone pairs on the chlorine atom,which results in a $V$-shaped or bent structure.

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

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