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(C) The oxidation state of transition metals depends on the number of electrons available for bonding in the $(n-1)d$ and $ns$ orbitals. Transition me

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

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(C) The oxidation state of transition metals depends on the number of electrons available for bonding in the $(n-1)d$ and $ns$ orbitals. Transition metals with the configuration $(n-1)d^5 ns^2$ (such as $Mn$,$Z=25$) have the maximum number of unpaired electrons (seven in total),allowing them to exhibit the highest oxidation states (e.g.,$+7$ in $KMnO_4$). Therefore,the configuration $(n-1)d^5 ns^2$ corresponds to the highest oxidation state.

Which transition metal configuration exhibits the highest oxidation state?

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