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) $O_{2}$ and $F_{2}$ both stabilize higher oxidation states of metals due to there strong non metallic nature but $O_{2}$ exceeds $F_{2}$ in doing so because $O_{2}$ has tendency to form multiple bonds with metal as it forms $O^{2 -}$ ion which has stronger attraction for higher oxidation states as compared to $F^{-}$ .
(ii) According to the Valance bond theory completely filled orbitals do not take part in the bond formation. Xenon has a complete octet. There is no unpaired electrons in any of its orbitals. Therefore the structure of xenon fluorides can not be explained in terms of VB theory but requires VSEPR theory to explain the involvement of lone pairs in bonding.

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