For a long time, Noble gases were called 'inert'. However, Xenon ($Xe$) can form stable compounds (like $Xe{F}_2,Xe{F}_4$) for several reasons:

1. Ionization Energy: Xe has the lowest I.E. among noble gases (comparable to Oxygen), allowing it to lose/share electrons with highly electronegative atoms ($F$ or $O$).
2. Atomic Size: Large size means valence electrons are less tightly held by the nucleus.
3. d-Orbitals: The availability of empty $5d$ orbitals allows Xenon to promote its electrons and expand its octet to accommodate more than 8 valence electrons.