Of the following outer electronic configurati | vedclass

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(D) The maximum oxidation state of a transition metal is determined by the total number of electrons in the $(n-1)d$ and $ns$ orbitals.For $(n-1)d^3ns

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$(n - 1)d^5ns^2$

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(D) The maximum oxidation state of a transition metal is determined by the total number of electrons in the $(n-1)d$ and $ns$ orbitals.For $(n-1)d^3ns^2$,the total number of valence electrons is $3 + 2 = 5$.For $(n-1)d^5ns^1$,the total number of valence electrons is $5 + 1 = 6$.For $(n-1)d^8ns^2$,the total number of valence electrons is $8 + 2 = 10$,but only the unpaired electrons or those in the outer shell are typically involved in bonding,limiting the oxidation state.For $(n-1)d^5ns^2$,the total number of valence electrons is $5 + 2 = 7$.Therefore,the configuration $(n - 1)d^5ns^2$ can achieve the maximum oxidation state of $+7$ (e.g.,in $Mn$).

Of the following outer electronic configurations of atoms,the highest oxidation state is achieved by which one of them?

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