Xenon tetrafluoride, `XeF_(4)` is:

Options

A. tetrahedral annd acts as a fluoride donor with `SbF_(5)`
B. square planar and acts as a fluoride donor with `PF_(5)`
C. square planar and acts as fluoride donor with `NaF`
D. see-saw shape and acts as a fluoride donor with `AsF_(5)`

Answer

To determine the nature of xenon tetrafluoride, \( \text{XeF}_4 \), we will analyze its structure and reactivity step by step.

### Step 1: Determine the molecular geometry of \( \text{XeF}_4 \)

1. **Valence Electrons Calculation**:
- Xenon (Xe) has 8 valence electrons.
- Each fluorine (F) has 7 valence electrons, and there are 4 fluorine atoms.
- Total valence electrons = \( 8 + (4 \times 7) = 8 + 28 = 36 \) electrons.

2. **Lewis Structure**:
- Place xenon in the center and surround it with 4 fluorine atoms.
- Each fluorine atom forms a single bond with xenon, using 8 electrons (4 bonds).
- This leaves us with \( 36 - 8 = 28 \) electrons.
- Distribute the remaining electrons as lone pairs. Xenon will have 2 lone pairs.

3. **Geometry**:
- The presence of 4 bonded pairs (from F) and 2 lone pairs around the xenon atom leads to a square planar geometry.
- The 4 fluorine atoms occupy the corners of a square, while the 2 lone pairs are positioned opposite each other.

### Step 2: Analyze the options

- **Tetrahedral**: Incorrect, as the geometry is square planar.
- **Square Planar**: Correct, as derived from the Lewis structure.
- **Seesaw Shape**: Incorrect, as this shape corresponds to a different arrangement of lone pairs and bonded pairs.

### Step 3: Reactivity with \( \text{PF}_5 \)

1. **Reaction Analysis**:
- When \( \text{XeF}_4 \) reacts with \( \text{PF}_5 \), it forms \( \text{XeF}_3^+ \) and \( \text{PF}_6^- \).
- This indicates that \( \text{XeF}_4 \) donates a fluoride ion to \( \text{PF}_5 \).

2. **Conclusion**:
- Since \( \text{XeF}_4 \) acts as a fluoride donor, it confirms that it can participate in reactions as a Lewis acid.

### Final Answer
Xenon tetrafluoride, \( \text{XeF}_4 \), is **square planar** and acts as a fluoride donor in reactions.

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