Which of the following electronic configurati | vedclass

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

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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 available in the $(n-1)d$ and $ns$ orbitals. For $(n-1)d^3ns^2$,total electrons = $3 + 2 = 5$. For $(n-1)d^5ns^1$,total electrons = $5 + 1 = 6$. For $(n-1)d^8ns^2$,total electrons = $8 + 2 = 10$. For $(n-1)d^5ns^2$,total electrons = $5 + 2 = 7$. Comparing these,the configuration $(n-1)d^5ns^2$ has the highest number of electrons available for bonding,allowing it to exhibit the highest oxidation state.

Which of the following electronic configurations of a transition metal atom shows the highest oxidation state?

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