XeF2 is isostructural with - DASH

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XeF₂ is isostructural with

SbCl₃

BaCl₂

TeF₂

ICl₂^$-$

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Step-by-Step Explanation Step 1: Identify the Central Atom and Its Valence Electrons In $XeF_2$, xenon (Xe) is the central atom. Xenon is a noble gas with 8 valence electrons. Each fluorine (F) contributes 1 bond with Xe. Step 2: Count Total Electron Pairs Around the Central Atom The xenon in $XeF_2$ forms two sigma bonds (each to a fluorine) and has three lone pairs (since xenon uses 2 electrons for bonding with fluorines out of a total of 8 valence electrons, leaving 6 electrons or 3 lone pairs). Thus, the total number of electron pairs around Xe is 5 (2 bonding pairs + 3 lone pairs). Step 3: Determine the Electron-Pair Geometry Using VSEPR Theory According to VSEPR Theory, 5 total electron pairs (bonding + lone pairs) around the central atom correspond to a trigonal bipyramidal electron-pair geometry. The three lone pairs occupy the equatorial positions to minimize repulsions, while the two bonding pairs are in the axial positions. Step 4: Determine the Molecular Shape When three lone pairs occupy equatorial positions, only the two bonding pairs in the axial positions remain visible in the geometric shape. This arrangement leads to a linear molecular shape for $XeF_2$. Step 5: Compare with $ICl_2^-$ In $ICl_2^-$, iodine (I) also ends up with 5 electron pairs (2 bonding pairs + 3 lone pairs) around it, leading to the same trigonal bipyramidal electron arrangement and a linear shape for the actual molecule. Therefore, $ICl_2^-$ is isostructural with $XeF_2$. Hence, $XeF_2$ is isostructural with $ICl_2^-$.

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