Accordingly, the hybridization of Cl in ClF5 is sp3d2.
In a ClF5 molecule, chlorine is the central atom with five single bonds with fluorine atoms. Since chlorine has 7 electrons in the valence shell, the remaining two electrons form a lone pair of electrons. According to the VSEPR theory (valence shell electron pair repulsion theory), the shape of a ClF5 molecule is square pyramidal.
Electronic groups include lone pairs and atoms around the central atom. There are 5 atoms and 1 lone pair or a total of 6 electrons around the central atom Cl. This corresponds to AX6 or octahedral. The electronic geometry of ClF5 is AX6 or octahedral.
The number of lone pairs of electrons on chlorine in ClF5 is 1.
Each of the six atomic elements has 7 valence electrons. What is that? The total number of valence electrons in a ClF5 molecule = 7 + 7*5 = 7 + 35 = 42.
Since BrF3 and ClF5 do not obey the octet rule.