Which of the following pairs of compounds is | vedclass

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(D) To be isoelectronic,the total number of valence electrons must be the same.For $IBr_{2}^{-}$: $7 (I) + 2 	imes 7 (Br) + 1 (	ext{charge}) = 22$ v

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$IBr_{2}^{-}, XeF_2$

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(D) To be isoelectronic,the total number of valence electrons must be the same.For $IBr_{2}^{-}$: $7 (I) + 2 	imes 7 (Br) + 1 (	ext{charge}) = 22$ valence electrons.For $XeF_{2}$: $8 (Xe) + 2 	imes 7 (F) = 22$ valence electrons.Both species have $22$ valence electrons,so they are isoelectronic.Both $IBr_{2}^{-}$ and $XeF_{2}$ have $3$ lone pairs and $2$ bond pairs around the central atom,resulting in a linear geometry ($sp^3d$ hybridization),making them isostructural.

Which of the following pairs of compounds is isoelectronic and isostructural?

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