The angle between the covalent bonds is maximum in :

Options

A. `CH_(4)`
B. `BF_(3)`
C. `PF_(3)`
D. `NH_(3)`

Explanation

To determine the molecule with the maximum angle between covalent bonds, we need to analyze the molecular geometry of the given compounds: CH4, BF3, PF3, and NH3.

### Step-by-Step Solution:

1. **Identify the Molecular Geometry of Each Compound:**
- **CH4 (Methane):** The molecular geometry is tetrahedral. The bond angle in a tetrahedral structure is approximately 109.5°.
- **BF3 (Boron Trifluoride):** The molecular geometry is trigonal planar. The bond angle in a trigonal planar structure is approximately 120°.
- **PF3 (Phosphorus Trifluoride):** The molecular geometry is trigonal pyramidal (similar to NH3). The bond angle is approximately 107° due to the presence of a lone pair on phosphorus.
- **NH3 (Ammonia):** The molecular geometry is also trigonal pyramidal, with a bond angle of approximately 107°.

2. **Compare the Bond Angles:**
- CH4: 109.5°
- BF3: 120°
- PF3: 107°
- NH3: 107°

3. **Determine the Maximum Bond Angle:**
- Among the bond angles calculated, BF3 has the largest bond angle of 120°.

4. **Conclusion:**
- The angle between the covalent bonds is maximum in BF3.

### Final Answer:
The angle between the covalent bonds is maximum in BF3.

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