Question

Which element of the 3d transition series has the lowest enthalpy of atomisation and why?

Hint:

Greater the number of unpaired \(d\)-electrons, stronger is the metallic bonding and higher is the enthalpy of atomisation.

Answer 1

Step 1: Enthalpy of atomisation depends on the strength of metal–metal bonding in the solid state.
Step 2: Strong metallic bonding in transition metals is due to the presence of unpaired \(d\)-electrons.
Step 3: Zinc has a completely filled \(3d^{10}\) electronic configuration, resulting in no unpaired \(d\)-electrons.
Step 4: Due to weaker metallic bonding, zinc has the lowest enthalpy of atomisation among 3d transition elements.