The shape of `BrF_3` molecule is slightly bent 'T' , because

Options

A. The lone pairs occupy the equatorial position to minimize lone pair- lone pair and the bond pair-lone pair repulsions
B. The axial fluroine atoms will be bent towards the equatorial fluorine in orer to minimize the lone pair-lonepair repulsions.
C. According to the VSEPR theory, one lone pair of Br occupies the equatorial position and the second one occupied the axial position in order to minimize the lone pair-lone pair repulsion
D. Both (1) and (2)

Answer

To determine why the shape of the BrF3 molecule is slightly bent 'T', we can follow these steps:

### Step 1: Identify the Central Atom and Valence Electrons
- The central atom in BrF3 is Bromine (Br).
- Bromine is a halogen and has 7 valence electrons.

### Step 2: Determine Bonding and Lone Pairs
- In BrF3, Bromine forms bonds with 3 Fluorine (F) atoms.
- Each bond uses one valence electron from Bromine, so 3 electrons are used for bonding.
- This leaves 4 valence electrons remaining for Bromine, which means there are 2 lone pairs (since each lone pair consists of 2 electrons).

### Step 3: Calculate the Steric Number
- The steric number is calculated as the number of bond pairs plus the number of lone pairs.
- In BrF3, there are 3 bond pairs and 2 lone pairs, so the steric number is 5 (3 + 2 = 5).

### Step 4: Determine Hybridization and Geometry
- For a steric number of 5, the hybridization is sp³d.
- The geometry corresponding to sp³d hybridization is trigonal bipyramidal.

### Step 5: Analyze the Arrangement of Lone Pairs and Bond Pairs
- In a trigonal bipyramidal arrangement, there are two positions: axial and equatorial.
- To minimize repulsions, the two lone pairs will occupy the equatorial positions, as lone pair-lone pair repulsion is greater than bond pair-bond pair repulsion.

### Step 6: Determine the Final Shape
- With two lone pairs in the equatorial positions, the three bond pairs (the fluorine atoms) will be arranged around the Bromine atom.
- The axial fluorine atoms will slightly bend towards the equatorial fluorine atom to further minimize repulsions.
- This results in a slightly bent 'T' shape for the BrF3 molecule.

### Conclusion
- The shape of the BrF3 molecule is slightly bent 'T' due to the arrangement of lone pairs and bond pairs in such a way as to minimize repulsions according to VSEPR theory.