Question

what is the molecular geometry of clf₄ (cl has 2 lone pairs)?
a square pyramidal
b seesaw
c octahedral
d trigonal bipyramidal
e square planar

Explanation:

Step1: Determine the electron - pair geometry

The central atom \(Cl\) in \(ClF_4\) has \(4\) bonding pairs and \(2\) lone pairs. The total number of electron pairs is \(4 + 2=6\). The electron - pair geometry for \(6\) electron pairs is octahedral.

Step2: Determine the molecular geometry

When there are \(2\) lone pairs in an octahedral electron - pair geometry, the molecular geometry is square planar. The lone pairs are placed opposite to each other to minimize repulsion.

Answer:

e Square planar