`XeF_2` is isostructural with

Options

A. `TeF_(2)`
B. `ICl_(2)^(-)`
C. `SbCl_(3)`
D. `BaCl_(2)`

Explanation

To determine which compound is isostructural with \( \text{XeF}_2 \), we need to analyze the structure of \( \text{XeF}_2 \) and compare it with the given options: \( \text{TeF}_2 \), \( \text{YCl}_2^- \), \( \text{SbCl}_3 \), and \( \text{BaCl}_2 \).

### Step-by-Step Solution:

1. **Identify the Structure of \( \text{XeF}_2 \)**:
- \( \text{XeF}_2 \) has a central xenon (Xe) atom surrounded by two fluorine (F) atoms.
- The molecular geometry of \( \text{XeF}_2 \) is linear due to the presence of three lone pairs of electrons on the xenon atom.

2. **Determine the Valence Electrons**:
- Xenon (Xe) has 8 valence electrons.
- Each fluorine (F) contributes 1 electron, but we focus on the central atom for isostructural comparison.

3. **Analyze Given Compounds**:
- **\( \text{TeF}_2 \)**: Tellurium (Te) has 6 valence electrons. With 2 fluorine atoms, it does not match the electron count of xenon.
- **\( \text{YCl}_2^- \)**: Yttrium (Y) has 3 valence electrons. With 2 chlorine atoms and a negative charge, it totals 8 electrons (3 from Y + 2 from each Cl + 1 from the charge). The structure is linear with 3 lone pairs on Y, similar to \( \text{XeF}_2 \).
- **\( \text{SbCl}_3 \)**: Antimony (Sb) has 5 valence electrons. With 3 chlorine atoms, it totals 8 electrons, but the geometry is trigonal pyramidal, not linear.
- **\( \text{BaCl}_2 \)**: Barium (Ba) has 2 valence electrons. With 2 chlorine atoms, it totals 4 electrons, which does not match.

4. **Conclusion**:
- The only compound that has the same number of valence electrons and a linear structure is \( \text{YCl}_2^- \).

### Final Answer:
The compound that is isostructural with \( \text{XeF}_2 \) is \( \text{YCl}_2^- \).