The iodine atom in $I {C l}_{2}^{-}$ involves :

s p^{3} d

hybridisation

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s p^{3} d^{2}

hybridisation

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s p^{2}

hybridisation

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s p^{3}

hybridisation

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Solution

The correct option is B $s p^{3} d$ hybridisation
$I {C l}_{2}^{-}$ is formed by removing $C l^{+}$ from $I C l_{3}$ .
Hence, the hybridization of the central iodine atom is the same in both, i.e., ${s p}^{3} d$ .
Hence, option A is the correct answer.

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Similar questions

A l H_{3}

A l H_{4}^{-}

C 3 - C 4

The correct order of hybridisation of the central atom in the following species $N H_{3}$ , ${[P t C l_{4}]}^{2 -}$ , $P C l_{5}$ and $B C l_{3}$

C (1) H_{2} = C (2) H - C (3) \equiv C H

(i)	$X e F_{2}$	(a)	Central atom is $s p^{3}$ hybridised and has a bent shape.
(ii)	$N_{3}^{-}$	(b)	Central atom is $s p^{3} d^{2}$ hybridised and has an octahedral shape.
(iii)	$P C l_{6}^{-}$	(c)	Central atom is $s p$ hybridised and has a linear shape.
(iv)	$I C l_{2}^{+}$	(d)	Central atom is $s p^{3} d$ hybridised and has a linear shape.

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