Why does zinc not exhibit variable oxidation | vedclass

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(B) The electronic configuration of zinc ($Zn$, atomic number $30$) is $[Ar] 3d^{10} 4s^2$.In $Zn^{2+}$ ion, the two electrons from the $4s$ orbital a

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Completely filled $3d$ subshell

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(B) The electronic configuration of zinc ($Zn$, atomic number $30$) is $[Ar] 3d^{10} 4s^2$.In $Zn^{2+}$ ion, the two electrons from the $4s$ orbital are removed, resulting in the configuration $[Ar] 3d^{10}$.Since the $3d$ subshell is completely filled, it is highly stable and does not allow for the loss of further electrons to show variable oxidation states.Therefore, zinc only exhibits a $+2$ oxidation state.

Why does zinc not exhibit variable oxidation states?

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