Explain the following giving an appropriate reason in each case.
(i) $O_{2}$ and $F_{2}$ both stabilize higher oxidation states of metals but $O_{2}$ exceeds $F_{2}$ in doing so.
(ii) Structures of xenon fluorides cannot be explained by valence bond approach.

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Solution

(i) $O_{2}, F_{2}$ both will stabilize the higher oxidation states. But the higher oxidation state of metal with $O_{2}$ is more stable. Because oxygen will gain 2 electrons from metal atom but the fluorine gains only 1 electron leading to the formation of $O^{2 -}, F^{-}$ . The bond between metal and non-metal will be strong when the metal is able to lose more electrons to non metal so the higher oxidation state stabilizes the compound.
II) The compounds of xenon fluorides like $X e F_{2}, X e F_{4}, X e F_{6}$ can not be explained using valence band 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.

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