The highest value for Zn is attributed to the removal of an electron from the stable d¹⁰ configuration of Zn²⁺, emphasizing the significance of achieving a fully filled d orbital for stability.
Explain the reason behind the highest value for Zn in relation to its electron configuration and the stability of Zn²⁺.
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The highest value for zinc (Zn) in terms of second ionization enthalpy is attributed to the removal of an electron from its stable d¹⁰ configuration, resulting in Zn²⁺. Zn²⁺ possesses a completely filled d subshell, leading to enhanced stability. The ionization process involves the removal of the lone 4s electron, resulting in the formation of the stable d¹⁰ configuration characteristic of Zn²⁺. This unique stability accounts for the relatively high second ionization enthalpy of zinc, as the ionization involves the removal of an electron from a highly stable electronic configuration.