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(D) The enthalpy of atomisation depends on the strength of metallic bonding,which is determined by the number of unpaired electrons in the $d$-orbital

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$Zn$

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(D) The enthalpy of atomisation depends on the strength of metallic bonding,which is determined by the number of unpaired electrons in the $d$-orbital. $Zn$ has a completely filled $d$-orbital $(3d^{10} 4s^2)$,meaning there are no unpaired electrons available for metallic bonding. Consequently,$Zn$ exhibits the weakest metallic bonding among the $3d$ transition series,resulting in the lowest enthalpy of atomisation.

The transition element that has the lowest enthalpy of atomisation is

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