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(D) The electronic configuration of $Zn$ is $[Ar] 3d^{10} 4s^2$. Because the $3d$ subshell is completely filled,the $d$-electrons do not participate i

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both $(a)$ and $(c)$

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(D) The electronic configuration of $Zn$ is $[Ar] 3d^{10} 4s^2$. Because the $3d$ subshell is completely filled,the $d$-electrons do not participate in the formation of metallic bonds. Metallic bonding in transition elements depends on the number of unpaired electrons in the $d$-orbitals. Since $Zn$ has zero unpaired electrons $(U.P.E.)$,the metallic bonding is weak,resulting in a lower melting point compared to other $3d$ series elements.

The melting point of $Zn$ is lower compared to those of the other elements of the $3d$ series because $-$

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