Question

draw the lewis structure of brf₃ and then determine the ideal bonding angle(s) of the central atom.

Explanation:

Step1: Determine valence - electrons

Bromine (Br) has 7 valence electrons and each fluorine (F) has 7 valence electrons. For \(BrF_3\), the total number of valence electrons is \(7 + 3\times7=28\).

Step2: Draw the Lewis structure

Place Br in the center and connect it to 3 F atoms with single bonds. Then, distribute the remaining electrons as lone - pairs. Br has 2 lone - pairs and 3 bonding pairs.

Step3: Determine the electron - pair geometry

The electron - pair geometry of \(BrF_3\) is trigonal bipyramidal due to 5 electron - pairs (3 bonding and 2 non - bonding) around the central Br atom.

Step4: Determine the molecular geometry and bond angles

The molecular geometry is T - shaped. In a trigonal bipyramidal electron - pair geometry, the bond angles between the equatorial positions are \(120^{\circ}\) and the bond angles between the axial and equatorial positions are \(90^{\circ}\).

Answer:

D. \(90^{\circ}\) and \(120^{\circ}\)