Chemistry - CHEMICAL BONDING Question with Solution | TestHub

In ${\mathrm{XeOF}}_4$, the central $\mathrm{Xe}$ atom is bonded to $\mathrm{O}$ atom through a double bond and to $\mathrm{F}$ atoms through single bonds. So the total number of bonds formed by $\mathrm{Xe}$ atom in the molecule is six. Thus, out of the eight valence electrons in Xenon, two are left unused in bonding and will be present as one lone pair.

The total number of bond pairs is five (double bond is considered as a single super pair). The geometry of the molecules with four bond pairs and one lone pair is square pyramidal as shown below-