Which of the following shape are not possible for possible value of n in `XeF_(n)` molecule ?

Options

A. Linear
B. Square planar
C. Trigonal planar
D. Capped octahedral

Explanation

To determine which shapes are not possible for the molecule \( \text{XeF}_n \), we will analyze the shapes based on the value of \( n \) and the molecular geometry of xenon difluoride.

### Step-by-Step Solution:

1. **Understanding the Molecular Geometry**:
- Xenon (Xe) is a noble gas with 8 valence electrons. Each fluorine (F) atom contributes 1 electron, so for \( n \) fluorine atoms, the total number of valence electrons is \( 8 + n \).

2. **Case Analysis for Different Values of \( n \)**:
- **Case 1: \( n = 1 \)**
- The molecule is \( \text{XeF} \).
- With one fluorine atom, the shape is linear.
- **Shape: Linear** (Possible)

- **Case 2: \( n = 2 \)**
- The molecule is \( \text{XeF}_2 \).
- The geometry is linear due to the two bonding pairs and three lone pairs on xenon.
- **Shape: Linear** (Possible)

- **Case 3: \( n = 4 \)**
- The molecule is \( \text{XeF}_4 \).
- The geometry is square planar due to the four bonding pairs and two lone pairs on xenon.
- **Shape: Square Planar** (Possible)

- **Case 4: \( n = 6 \)**
- The molecule is \( \text{XeF}_6 \).
- The geometry is capped octahedral due to the six bonding pairs and one lone pair on xenon.
- **Shape: Capped Octahedral** (Possible)

3. **Identifying the Impossible Shape**:
- The options provided were: Linear, Square Planar, Trigonal Planar, and Capped Octahedral.
- From our analysis, we found that:
- Linear is possible for \( n = 1 \) and \( n = 2 \).
- Square planar is possible for \( n = 4 \).
- Capped octahedral is possible for \( n = 6 \).
- **Trigonal Planar** is not possible for any value of \( n \) in \( \text{XeF}_n \).

### Conclusion:
The shape that is **not possible** for any value of \( n \) in the \( \text{XeF}_n \) molecule is **Trigonal Planar**.

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