Among the following molecules.

$$\begin{gathered} \left(P\right)Xe{O}_3 \\ \left(Q\right)XeO{F}_4 \\ \left(R\right)Xe{O}_2{F}_2 \\ \left(S\right)Xe{F}_6 \end{gathered}$$

Those having different molecular geometry but same number of lone pairs on Xe are :

In each case Xe has 1 l.p.

In ${\mathrm{XeO}}_3$, Xe has 8 electrons in its valence shell, 6 of which are used to link with 3 O atoms, while the remaining 2 electrons act as a lone pair that is not bonded to anything.

In the compound ${\mathrm{XeOF}}_4$, Xe has 8 electrons in its valence shell, 6 of which are utilised to form bonds with the atoms 1 O and 4 F, while the remaining 2 electrons form a lone pair.

In ${\mathrm{XeF}}_6$, of the 8 electrons in Xe's valence shell, 6 are utilised to form bonds with the 6 F atoms, leaving 2 electrons as a lone pair.