In 3d series (Sc→Zn), the enthalpy of atomisation of Zn is low. Why?
The enthalpy of atomization is determined by the amount of metallic bonding that an element has. An element's enthalpy of atomization increases as its metallic bonding becomes more extensive. There are some unpaired electrons in all transition metals (except zinc, electronic configuration: 3d10, 4s23d10, 4s2 ), which explain for their stronger metallic bonding. The inter-atomic electrical bonding in zinc is the weakest due to the absence of these unpaired electrons, and as a result, it has the lowest enthalpy of atomization.
