Identify the correct statement about ClF3 from the following options:

To determine the shape of chlorine trifluoride (ClF₃), we use the VSEPR (Valence Shell Electron Pair Repulsion) model.

1. Count the valence electrons on the central atom (Cl).
• Chlorine is in group 17, so it has 7 valence electrons.
• Each fluorine atom contributes one electron to the bond.
• Total electrons = 7 (Cl) + 3 × 1 (F) = 10 electrons.

2. Convert the total electrons to electron pairs.
10 electrons ÷ 2 = 5 electron pairs.

3. Classify the electron pairs.
• There are three bonding pairs (Cl–F bonds).
• The remaining two pairs are lone (non‑bonding) pairs on chlorine.

4. Predict the arrangement of five electron pairs.
Five pairs adopt a trigonal‑bipyramidal electron‑pair geometry.

5. Place the lone pairs in positions that minimise repulsion.
Lone pairs preferentially occupy the equatorial positions because they experience less 90° repulsion compared with axial positions.

6. Determine the molecular geometry.
With the two equatorial positions taken by lone pairs, the three remaining positions (one axial and the two remaining equatorial) contain the Cl–F bonds. This results in a T‑shaped arrangement of the atoms.

Therefore, chlorine trifluoride has a T‑shaped molecular geometry with two lone pairs on the chlorine atom.