A covalent bond will be formed by the overlapping of atomic orbitals having single electron of opposite spin, according to the overlapping of atomic orbitals the covalent bond may be of two types :
(i) Sigma bond `(sigma) " " (ii) ` Pi bond `(pi)`
Sigma bond is stronger bond than the Pi-bond. If atomic orbitals overlap about the nuclear axis then sigma bond is formed but when atomic orbitals overlap sideway then Pi-bond is formed.
Compound having maximum bond angle is :

Options

A. `BBr_(3)`
B. `BCl_(3)`
C. `BF_(3)`
D. none of these

Answer

To solve the question regarding which compound has the maximum bond angle among BBr3, BCl3, and BF3, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Covalent Bonds**:
- A covalent bond is formed by the overlapping of atomic orbitals that contain single electrons with opposite spins. There are two types of covalent bonds: sigma (σ) bonds and pi (π) bonds. Sigma bonds are formed by end-to-end overlapping of orbitals and are stronger than pi bonds, which are formed by side-to-side overlapping.

2. **Identifying the Compounds**:
- The compounds given are BBr3 (Boron Tribromide), BCl3 (Boron Trichloride), and BF3 (Boron Trifluoride).

3. **Determining Molecular Geometry**:
- All three compounds (BBr3, BCl3, and BF3) have a central boron atom and three surrounding halogen atoms. The geometry of these compounds is trigonal planar due to the presence of three bonding pairs and no lone pairs on the boron atom.

4. **Bond Angles in Trigonal Planar Geometry**:
- In a trigonal planar geometry, the bond angles between the atoms are ideally 120 degrees. This is a characteristic of the trigonal planar arrangement and does not change based on the type of halogen atom attached to the boron.

5. **Comparing Bond Angles**:
- Since all three compounds have the same trigonal planar geometry, the bond angles in BBr3, BCl3, and BF3 are all 120 degrees. Therefore, there is no compound that has a maximum bond angle compared to the others.

6. **Conclusion**:
- The answer to the question is that none of the compounds (BBr3, BCl3, BF3) has a maximum bond angle that differs from the others. All have the same bond angle of 120 degrees.

### Final Answer:
None of these compounds has a maximum bond angle; all have the same bond angle of 120 degrees.

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