An isostructural compound with $XeF_2$ among the following is:

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1. **Analyze $XeF_2$:** 
   - Central atom Xenon (Xe) has 8 valence electrons.
   - It forms 2 sigma bonds with Fluorine.
   - Remaining electrons = $8 - 2 = 6$ (3 lone pairs).
   - Structure: 2 Bond Pairs + 3 Lone Pairs $\rightarrow$ **Linear** geometry (Lone pairs occupy equatorial positions in trigonal bipyramidal electron geometry).

2. **Analyze Option A ($ICl_2^-$):**
   - Central atom Iodine (I) has 7 valence electrons.
   - Negative charge adds 1 electron $\rightarrow$ Total 8 valence electrons on the central shell context.
   - It forms 2 sigma bonds with Chlorine.
   - Remaining electrons = $8 - 2 = 6$ (3 lone pairs).
   - Structure: 2 Bond Pairs + 3 Lone Pairs $\rightarrow$ **Linear** geometry.
   - Since both have the same structure (Linear) and hybridization ($sp^3d$), they are **isostructural**.

3. **Analyze other options:**
   - $SbCl_3$: 3 Bond Pairs + 1 Lone Pair $\rightarrow$ Trigonal Pyramidal.
   - $BaCl_2$: Ionic/Linear (but typically considered distinct from covalent VSEPR analogs in this context).
   - $TeF_2$: 2 Bond Pairs + 2 Lone Pairs $\rightarrow$ Bent/Angular.

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