What would be the shape of CIF₃ molecules which has three single bonds and two lone pairs?

Concept:

VSEPR Theory

• The shape of the molecule is determined by repulsions between all of the electrons present in the valence shell.
• Electron pairs in the valence shell of the central atom repel each other and align themselves to minimize this repulsion.
• Lone pairs of the electron on the central atom repeal the most. i.e., Lone pair -lone pair repulsion > lone pair-bond pair > bond pair-bond pair.
• The valence shell electron pairs arrange themselves in space as far as possible to minimize mutual repulsion.

Explanation:

ClF₃

• In ClF₃, there are 5 electron pairs around Cl. In which 3 are bonding pairs and 2 are non-bonding pairs.
• Here, Repulsion is minimized by placing the five electron groups at angles of 120° and 90° which is a trigonal bipyramidal arrangement.
• The two non-bonding pairs are on the trigonal plane. So, these two equatorial lone pairs making the final structure T-shaped.

According to VSEPR theory, ClF₃ molecules possess T-shape.