Which is/are correct statement(s) for `XeF_(2)`?

Options

A. It has bent structure
B. It is hydrolysed rapidly in aqueous solution of a base
C. It oxidizes `Cl^(-)` and `I^(-)` to `Cl_(2)` and `I_(2)` respectively
D. Both B and C

Answer

To determine the correct statements regarding \( \text{XeF}_2 \), we will analyze each statement step by step.

### Step 1: Analyze the Structure of \( \text{XeF}_2 \)

1. **Valence Electrons**: Xenon (Xe) has 8 valence electrons. Fluorine (F) has 7 valence electrons, and since there are 2 fluorine atoms, they contribute a total of 14 valence electrons.
2. **Total Valence Electrons**: The total number of valence electrons in \( \text{XeF}_2 \) is \( 8 + 14 = 22 \) electrons.
3. **Bonding and Lone Pairs**: In \( \text{XeF}_2 \), xenon forms 2 bonds with fluorine atoms, using 2 of its electrons. This leaves \( 22 - 4 = 18 \) electrons, which will be in the form of lone pairs.
4. **Lone Pairs on Xenon**: Xenon will have 3 lone pairs (6 electrons) remaining after forming 2 bonds with fluorine.
5. **Steric Number**: The steric number is calculated as the sum of bond pairs and lone pairs. Here, it is \( 2 \) (bond pairs) + \( 3 \) (lone pairs) = \( 5 \).
6. **Hybridization**: The hybridization corresponding to a steric number of 5 is \( sp^3d \).
7. **Molecular Geometry**: The molecular geometry of \( \text{XeF}_2 \) is trigonal bipyramidal, but the shape considering only the atoms (bonding pairs) is linear due to the arrangement of lone pairs.

**Conclusion for Step 1**: The statement that \( \text{XeF}_2 \) has a bent structure is **incorrect**; it has a linear structure.

### Step 2: Hydrolysis of \( \text{XeF}_2 \)

1. **Reaction with Base**: When \( \text{XeF}_2 \) is treated with a base like NaOH, it undergoes hydrolysis.
2. **Balanced Reaction**: The reaction can be represented as:
\[ 2 \text{XeF}_2 + 4 \text{NaOH} \rightarrow 2 \text{Xe} + 4 \text{NaF} + O_2 + 2 H_2O \]
3. **Conclusion for Step 2**: This statement is **correct**; \( \text{XeF}_2 \) hydrolyzes rapidly in an aqueous solution of a base.

### Step 3: Oxidizing Ability of \( \text{XeF}_2 \)

1. **Reaction with Halides**: \( \text{XeF}_2 \) can oxidize halides like \( \text{Cl}^- \) and \( \text{I}^- \).
2. **Balanced Reactions**:
- For \( \text{Cl}^- \):
\[ \text{XeF}_2 + 2 \text{HCl} \rightarrow \text{Xe} + \text{HF} + \text{Cl}_2 \]
- For \( \text{I}^- \):
\[ \text{XeF}_2 + 2 \text{KI} \rightarrow \text{Xe} + 2 \text{KF} + \text{I}_2 \]
3. **Conclusion for Step 3**: This statement is also **correct**; \( \text{XeF}_2 \) oxidizes \( \text{Cl}^- \) to \( \text{Cl}_2 \) and \( \text{I}^- \) to \( \text{I}_2 \).

### Final Conclusion

The correct statements regarding \( \text{XeF}_2 \) are:
- It hydrolyzes rapidly in an aqueous solution of a base.
- It oxidizes \( \text{Cl}^- \) and \( \text{I}^- \) to \( \text{Cl}_2 \) and \( \text{I}_2 \) respectively.

Thus, the correct answer is that both statements B and C are correct.