Question

Among the interhalide species
$IF _{2}^{\ominus}, IF _{3}, IF _{4}^{\ominus}$, and $IF _{7}$

• A. All iodine centers are either $s p^{3} d$ or $s p^{3} d^{2}$ hybridized
• B. The minimum angular separation between fluorine atoms is $60^{\circ}$
• C. The anionic species are both isoelectronic and isostructural to $XeF _{2}$ and $XeF _{4}$
• D. There is no species having a single lone pair of electrons

Answer 1

Answer: (C)

Hybridization and structure of $IF^- _{2} \rightarrow sp { }^{3} d$ and linear Hybridization and structure of $XeF _{2} \rightarrow s p^{3} d$ and linear
So Both $XeF _{2}$ and $IF _{2}^{-}$are isostructural and isoelectronic Hybridization and structure of $IF _{4}^{-} \rightarrow s p^{3} d^{2}$ and square planar Hybridization and structure of $XeF _{4} \rightarrow s p^{3} d^{2}$ and square planar Hence, both $XeF _{4}$ and $IF _{4}^{-}$are isoelectronic and isostructural.