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_

Vedclass · Accepted Answer

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

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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?

Similar Questions

Which of the following metal oxides is not amphoteric?

The incorrect statement$(s)$ among $(a)-(c)$ is (are) :-
$(a)$ $W(VI)$ is more stable than $Cr(VI)$
$(b)$ In the presence of $HCl$,permanganate titrations provide satisfactory results.
$(c)$ Some lanthanoid oxides can be used as phosphors.

Which of the following pairs of oxides is amphoteric in nature?

The addition of dilute $NaOH$ to $Cr^{3+}$ salt solution will give:

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