XeF_2 is isostructural with | vedclass

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(D) To determine the isostructural species,we calculate the hybridization and geometry of the molecules:$1$. $XeF_2$: The central atom $Xe$ has $8$ va

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$ICl_2^-$

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(D) To determine the isostructural species,we calculate the hybridization and geometry of the molecules:$1$. $XeF_2$: The central atom $Xe$ has $8$ valence electrons. It forms $2$ bonds with $F$ atoms and has $3$ lone pairs. The steric number is $2 + 3 = 5$,corresponding to $sp^3d$ hybridization. Due to $3$ lone pairs in the equatorial positions,the geometry is linear.$2$. $ICl_2^-$: The central atom $I$ has $7$ valence electrons. Including the negative charge,it has $8$ electrons. It forms $2$ bonds with $Cl$ atoms and has $3$ lone pairs. The steric number is $2 + 3 = 5$,corresponding to $sp^3d$ hybridization. Like $XeF_2$,it has a linear geometry.$3$. $SbCl_3$: The central atom $Sb$ has $5$ valence electrons. It forms $3$ bonds with $Cl$ atoms and has $1$ lone pair. The steric number is $3 + 1 = 4$,corresponding to $sp^3$ hybridization and a pyramidal geometry.$4$. $TeF_2$: The central atom $Te$ has $6$ valence electrons. It forms $2$ bonds with $F$ atoms and has $2$ lone pairs. The steric number is $2 + 2 = 4$,corresponding to $sp^3$ hybridization and a $V$-shaped (bent) geometry.Therefore,$XeF_2$ and $ICl_2^-$ are isostructural.

$XeF_2$ is isostructural with

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