Explanation:

Maximum bond angle:
The maximum bond angle refers to the angle between two adjacent bonds in a molecule. It is the largest angle that can be formed between the bonded atoms in a molecule.

Bond angles in BBr3, BCl3, and BF3:
- BBr3 (Boron tribromide): BBr3 is a trigonal planar molecule with the boron atom in the center and three bromine atoms surrounding it. The bond angle in BBr3 is approximately 120 degrees.
- BCl3 (Boron trichloride): BCl3 is also a trigonal planar molecule with the boron atom in the center and three chlorine atoms surrounding it. The bond angle in BCl3 is approximately 120 degrees.
- BF3 (Boron trifluoride): BF3 is a trigonal planar molecule with the boron atom in the center and three fluorine atoms surrounding it. The bond angle in BF3 is also approximately 120 degrees.

Explanation of the answer:
According to the given options, the maximum bond angle is not present in any of the given compounds (BBr3, BCl3, or BF3). This is because all three compounds have the same molecular geometry, which is trigonal planar, and the bond angles in a trigonal planar molecule are fixed at 120 degrees.

Reasoning:
The bond angles in a molecule are determined by the repulsion between electron pairs around the central atom. In a trigonal planar molecule, such as BBr3, BCl3, and BF3, the three bonding pairs of electrons are arranged as far apart as possible to minimize repulsion. This arrangement results in bond angles of 120 degrees.

Conclusion:
In conclusion, none of the given compounds (BBr3, BCl3, or BF3) have a maximum bond angle since all three compounds have the same bond angle of approximately 120 degrees.