What is the total number of unpaired electron | vedclass

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(A) The element located in period-$4$ and group-$12$ is Zinc $(Zn)$.$Zn$ has an atomic number of $30$.The electronic configuration of $Zn$ in the grou

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Zero

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(A) The element located in period-$4$ and group-$12$ is Zinc $(Zn)$.$Zn$ has an atomic number of $30$.The electronic configuration of $Zn$ in the ground state is $[Ar] \ 3d^{10} \ 4s^2$.In this configuration,all $3d$ and $4s$ orbitals are completely filled,meaning there are $0$ unpaired electrons.In the excited state (e.g.,$Zn^{2+}$ ion),the configuration is $[Ar] \ 3d^{10}$,which also contains $0$ unpaired electrons.Therefore,the total number of unpaired electrons is $0$.

What is the total number of unpaired electrons in an element placed at period-$4$ and group-$12$ either in excited or at ground state?

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