Explain the following giving an appropriate reason in each case:
(i) O2 and F2 both stabilize higher oxidation states of metals but O2 exceeds F2 in doing so.
(ii) Structures of xenon fluorides cannot be explained by valence bond approach.

(i) O2 and F2 both will stabilize the higher oxidation states. But the higher oxidation state of metal with O2 is more stable. Because oxygen will gain 2 electrons from the metal atom, but fluorine gains only 1 electron leading to the formation of O2⁻, F⁻. The bond between metal and non-metal will be strong when the metal is able to lose more electrons to the non-metal, so the higher oxidation state stabilizes the compound.
(ii) The compounds of xenon fluorides like XeF2, XeF4, XeF6 cannot be explained using valence bond theory because in valence bond theory we take valence electrons into consideration, but in compounds of xenon we have lone pair electrons which affect the shape of a molecule. So, the compounds of xenon are explained by valence shell electron pair repulsion theory.