Among the following molecules,

a) ${\mathrm{XeO}}_3$

b) ${\mathrm{XeOF}}_4$

c) ${\mathrm{XeF}}_6$

Those having same number of lone pairs on $\mathrm{Xe}$ are

a) ${\mathrm{XeO}}_3$ has xenon as the central atom and three oxygen atoms are doubly bonded to it. Its hybridization is ${\mathrm{sp}}^3$ and the structure is pyramidal. It contains 3 bond pairs and 1 lone pair.

b) ${\mathrm{XeOF}}_4$ has xenon as the central atom, one oxygen atom is doubly bonded and 4 fluorine single bonds. So, it has 5 bond pairs and 1 lone pair. Its hybridization is ${\mathrm{sp}}^3\mathrm{d}$ and the structure is square pyramidal.

c) ${\mathrm{XeF}}_{6^{\text{'}}}$, has 6 bond pairs and 1 lone pair. Its hybridization is ${\mathrm{sp}}^3{\mathrm{d}}^3$ and the structure is square distorted octahedral.