Which of the following is not square planar ? .

Options

A. `XeF_(4)`
B. `XeF_(2)`
C. `XeOF_(4)`
D. `CH_(3)CI`

Explanation

To determine which of the given compounds is not square planar, we will analyze each option based on the number of bond pairs and lone pairs, hybridization, and resulting molecular geometry.

### Step-by-Step Solution:

1. **Identify the Compounds**: We have four compounds to analyze:
- A: XeF4
- B: XeF2
- C: XeOF4
- D: CH3Cl

2. **Analyze Compound A: XeF4**
- **Bond Pairs**: 4 (from 4 Xe-F bonds)
- **Lone Pairs**: 2 (on xenon)
- **Total Electron Pairs**: 4 bond pairs + 2 lone pairs = 6
- **Hybridization**: sp³d²
- **Geometry**: Octahedral
- **Shape**: Square planar (due to the arrangement of lone pairs)
- **Conclusion**: This compound is square planar.

3. **Analyze Compound B: XeF2**
- **Bond Pairs**: 2 (from 2 Xe-F bonds)
- **Lone Pairs**: 3 (on xenon)
- **Total Electron Pairs**: 2 bond pairs + 3 lone pairs = 5
- **Hybridization**: sp³d
- **Geometry**: Trigonal bipyramidal
- **Shape**: Linear (due to the arrangement of lone pairs)
- **Conclusion**: This compound is not square planar.

4. **Analyze Compound C: XeOF4**
- **Bond Pairs**: 5 (4 Xe-F bonds and 1 Xe=O bond)
- **Lone Pairs**: 1 (on xenon)
- **Total Electron Pairs**: 5 bond pairs + 1 lone pair = 6
- **Hybridization**: sp³d²
- **Geometry**: Octahedral
- **Shape**: Square pyramidal (due to the presence of one lone pair)
- **Conclusion**: This compound is not square planar.

5. **Analyze Compound D: CH3Cl**
- **Bond Pairs**: 4 (3 C-H bonds and 1 C-Cl bond)
- **Lone Pairs**: 0
- **Total Electron Pairs**: 4 bond pairs + 0 lone pairs = 4
- **Hybridization**: sp³
- **Geometry**: Tetrahedral
- **Shape**: Tetrahedral
- **Conclusion**: This compound is not square planar.

### Final Conclusion:
The compound that is **not square planar** is **B: XeF2**.