In which of the following, ions are correctly | vedclass

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(B) The oxidation states of the transition elements in the given ions are $V$ in $VO_2^{+}$ is $+5$, $Cr$ in $Cr_2O_7^{2-}$ is $+6$, and $Mn$ in $MnO_

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$VO_2^{+} < Cr_2O_7^{2-} < MnO_4^{-}$

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(B) The oxidation states of the transition elements in the given ions are $V$ in $VO_2^{+}$ is $+5$, $Cr$ in $Cr_2O_7^{2-}$ is $+6$, and $Mn$ in $MnO_4^{-}$ is $+7$. Oxidizing power is directly related to the ease of reduction, which depends on the stability of the lower oxidation states formed. For these transition metals, the stability of the reduced products follows the trend $Mn^{2+} > Cr^{3+} > V^{3+}$. Consequently, the oxidizing power increases as the reduction potential increases, leading to the order $VO_2^{+} < Cr_2O_7^{2-} < MnO_4^{-}$.

In which of the following, ions are correctly arranged in the increasing order of oxidizing power?

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