Which of the following order of oxidising power is correct for the following species?
$V O_{2}^{+}, M n O_{4}^{-}, C r_{2} O_{7}^{2 -}$

V O_{2}^{+} < C r_{2} O_{7}^{2 -} < M n O_{4}^{-}

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V O_{2}^{+} < M n O_{4}^{-} < C r_{2} O_{7}^{2 -}

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C r_{2} O_{7}^{2 -} < V O_{2}^{+} < M n O_{4}^{-}

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C r_{2} O_{7}^{2 -} < M n O_{4}^{-} < V O_{2}^{+}

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Solution

The correct option is A $V O_{2}^{+} < C r_{2} O_{7}^{2 -} < M n O_{4}^{-}$
Here all the central metal ions of $V O_{2}^{+}, M n O_{4}^{-}, C r_{2} O_{7}^{2 -}$ are in $d^{0}$ configuration.
Here the oxidising power is in the order of $V O_{2}^{+} < C r_{2} O_{7}^{2 -} < M n O_{4}^{-}$ .
It is due to the increasing stability of the lower species to which they are reduced.

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