X and Y are two covalent molecules in which the hybridization of the central atoms is the same, but the…

${\mathrm{XeF}}_2 \text{and} {\mathrm{PF}}_5$ both have ${\mathrm{sp}}^3\mathrm{d}$ hybridisation. Howerver, their shapes will be different according to the VSEPR theory. 

Xenon fluoride structure has two covalent bonds between one xenon atom and two fluorine atoms. The xenon atom also holds 3 lone pairs of electrons. It has a linear structure.

In Phosphorous pentafluoride, phosphorous atom forms five $s{p}^{3}d$ hybrid orbitals and all the five hybrid orbitals will be used to form bonds with five fluorine atoms. There are no lone pairs. It has a trigonal bipyramidal shape.