`XeF_2` is isostructural with

Options

A. `ICl_2^(-)`
B. `SbCl_3`
C. `BaCl_2`
D. `TeF_2`

Explanation

To determine which molecule is isostructural with \( \text{XeF}_2 \), we can follow these steps:

### Step 1: Understand the Structure of \( \text{XeF}_2 \)
- \( \text{XeF}_2 \) (Xenon Difluoride) has a linear structure. This is due to the presence of three lone pairs of electrons on the central xenon atom, which repel the bonding pairs of electrons (the fluorine atoms) and create a linear arrangement.

### Step 2: Determine the Steric Number of \( \text{XeF}_2 \)
- The steric number is calculated as the number of bonded atoms plus the number of lone pairs on the central atom. For \( \text{XeF}_2 \):
- Number of bonded atoms (F) = 2
- Number of lone pairs on Xe = 3
- Steric number = 2 (bonded atoms) + 3 (lone pairs) = 5

### Step 3: Identify Other Molecules with the Same Steric Number
- We need to find other molecules that also have a steric number of 5 and exhibit a similar linear structure. One such molecule is \( \text{RnF}_2 \) (Radon Difluoride), which has a similar arrangement due to its electron configuration and bonding characteristics.

### Step 4: Confirm the Valence Electrons
- \( \text{Xe} \) has 8 valence electrons, and each \( \text{F} \) contributes 1 electron. Thus, \( \text{XeF}_2 \) has a total of:
- 8 (from Xe) + 2 (from 2 F) = 10 valence electrons.
- Similarly, \( \text{RnF}_2 \) also has 8 valence electrons from Radon and 2 from the two Fluorine atoms, confirming that it has the same electron count.

### Conclusion
- Therefore, \( \text{XeF}_2 \) is isostructural with \( \text{RnF}_2 \) (Radon Difluoride).