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Oxidation and Reduction

How would you...

Question

How would you account for the increasing oxidising power in the series $V O_{2}^{+} < M n O_{4}^{-}$ ?

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Solution

1)The oxidation state of $V$ in $V O_{2}^{+}$ is $+ 5$ .
2)The oxidation state of $M n$ is $+ 7$ in $M n O_{4}^{-}$ .
3) Thus, due to the increased stability of the lower species to which they are reduced.

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Q. How would you account for the increasing oxidising power in the series

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

Q. How would you account for the following ?

The oxidising power of the following three oxoions in the series follows the order :

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

Q. 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 -}

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Q. Following order is observed in oxidizing power of certain ions:

V O_{2}^{+}

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M n O_{4}^{2 -}

The reason for this increasing order of oxidizing power is:

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