To determine if species are isostructural, we need to compare their shapes using VSEPR theory.

• $\text{XeF}_2$: The central Xenon atom has 8 valence electrons. It forms 2 $\sigma$ bonds with Fluorine atoms and has 3 lone pairs. The steric number is 5 ($sp^3d$ hybridisation). To minimise repulsion, the 3 lone pairs occupy equatorial positions, resulting in a linear shape.
• $\text{TeF}_2$: Tellurium has 6 valence electrons, forms 2 bonds, and has 2 lone pairs ($sp^3$, bent shape).
• $\text{ICl}_2^-$: The central Iodine atom has 7 valence electrons plus 1 from the negative charge, totalling 8 valence electrons. It forms 2 $\sigma$ bonds with Chlorine atoms and has 3 lone pairs. The steric number is 5 ($sp^3d$ hybridisation). Similar to $\text{XeF}_2$, it has a linear shape.
• $\text{SbCl}_3$: Antimony has 5 valence electrons, forms 3 bonds, and has 1 lone pair ($sp^3$, trigonal pyramidal).
• $\text{BCl}_3$: Boron has 3 valence electrons, forms 3 bonds, and has 0 lone pairs ($sp^2$, trigonal planar). Therefore, $\text{XeF}_2$ is isostructural with $\text{ICl}_2^-$.