Find the number of lone pairs in ${\mathrm{XeO}}_2{\mathrm{F}}_2.$

Xenon basically belongs to the noble gas family. ${\mathrm{XeO}}_2{\mathrm{ }\mathrm{F}}_2$ molecular geometry is originally said to be trigonal bipyramidal but due to the presence of lone pair on equatorial position, the actual shape will be see-saw.

The repulsion between bond pair and lone pair of electrons will be more. Here, fluorine will be axial atoms and oxygen will be equatorial atoms.

In ${\mathrm{XeO}}_2{\mathrm{F}}_2$, $\mathrm{Xe}$ is ${\mathrm{sp}}^3{\mathrm{d}}^2$ hybridized with $11$ lone pairs.