Question

(c) Which element of the 3d series has the lowest enthalpy of atomisation and why?

Hint:

Elements with stable electron configurations, such as copper’s \( 3d^{10} \), have lower enthalpies of atomisation because less energy is needed to break the bonds.

Answer 1

The element in the 3d series with the lowest enthalpy of atomisation is copper (Cu). Copper has a completely filled \( 3d^{10} \) configuration, which contributes to its high stability. This stable electron configuration reduces the energy required to break the metallic bonds during atomisation, resulting in a lower enthalpy of atomisation. In comparison, elements like zinc (Zn) and manganese (Mn) have less stable electron configurations, requiring more energy to break the metallic bonds during atomisation. \bigskip Step 2: Therefore, copper (Cu) has the lowest enthalpy of atomisation due to the stability provided by its filled \( 3d^{10} \) configuration. \bigskip