Question

what is the molecular geometry of clf5?
a square pyramidal
b seesaw
c octahedral
d trigonal bipyramidal
e square planar

Explanation:

Step1: Determine the central atom and its valence electrons

The central atom in \(ClF_5\) is \(Cl\). Chlorine has 7 valence electrons.

Step2: Calculate the number of bonding pairs and lone pairs

\(Cl\) forms 5 bonds with \(F\) atoms (5 bonding pairs). Using the formula \(V = BP+LP\) (where \(V\) is the total number of electron pairs around the central atom, \(BP\) is the number of bonding pairs, and \(LP\) is the number of lone pairs), and \(V=\frac{7 + 5}{2}=6\) (since each \(F\) donates 1 electron). So, \(LP=V - BP=6 - 5 = 1\)

Step3: Use VSEPR theory

According to VSEPR theory, for a molecule with 6 electron pairs (5 bonding and 1 lone pair) around the central atom, the electron - pair geometry is octahedral. But the molecular geometry (which ignores lone pairs in terms of the shape description for the atoms) is square pyramidal.

Answer:

a. Square pyramidal