Number of lone pair(s) of electrons on central atom and the shape of BrF3 molecule respectively, are:

🧠 $\ce{BrF3}$: Br is in period 4 with 7 valence electrons. After forming 3 bonds to F, 4 electrons remain on Br → 2 lone pairs. Total steric number = 3 bonds + 2 LP = 5 → trigonal bipyramidal electron geometry. The 2 lone pairs occupy the equatorial positions (largest space) → T-shaped (bent T-shape) molecular geometry.

🗺️ Lone pairs occupy equatorial > axial in trigonal bipyramidal because equatorial lone pairs have only 2 axial neighbours at 90°, while axial lone pairs would have 3 equatorial neighbours at 90°.

⚠️ Trap: Option (d) says 1 lone pair → T-shape. That's wrong on the LP count. $\ce{BrF3}$ has 2 lone pairs, and still gives T-shape — option (c) is the only one correct on both counts.

$\boxed{\text{Answer: (c) 2 lone pairs, bent T-shape}}$