In the series Sc (Z=21) to Zn (Z=30),the enth | vedclass

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(N/A) The enthalpy of atomization depends on the strength of metallic bonding between atoms. Greater the number of unpaired electrons,stronger is the

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(N/A) The enthalpy of atomization depends on the strength of metallic bonding between atoms.
Greater the number of unpaired electrons,stronger is the metallic bonding,and higher is the enthalpy of atomization.
In the $3d$ series,all elements except $Zn$ $(3d^{10} 4s^2)$ have at least one unpaired electron in their $d$-orbitals,which contributes to strong inter-atomic metallic bonding.
Since $Zn$ has a completely filled $d$-subshell $(3d^{10})$ and no unpaired electrons,the metallic bonding is the weakest,leading to the lowest enthalpy of atomization.

In the series $Sc (Z=21)$ to $Zn (Z=30)$,the enthalpy of atomisation of zinc is the lowest,i.e.,$126 \ kJ \ mol^{-1}$. Why?

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