In general, the Pb2+ ion (lead(II) ion) is more stable than the Pb+ ion (lead(I) ion). This is due to the electronic configuration and the stability factors associated with the two ions.
The Pb2+ ion has a noble gas configuration of [Xe] for its 5s and 4f orbitals, meaning it has a completely filled 5s and 4f subshells. This stability arises from the filled orbitals, resulting in a more stable electronic configuration.
On the other hand, the Pb+ ion has an electronic configuration of [Xe]4f145d106s1, which means it has an incomplete 6s orbital. Having an incomplete orbital makes it more prone to losing an electron to achieve a stable configuration.
Moreover, the Pb2+ ion is more stable due to its higher ionic charge. The higher positive charge on the Pb2+ ion results in stronger electrostatic attractions between the ion and any surrounding negative charges, such as anions or electron pairs from ligands in coordination complexes. This stronger electrostatic attraction contributes to the stability of the Pb2+ ion.
Overall, the Pb2+ ion is more stable than the Pb+ ion due to its noble gas electronic configuration and higher positive charge.
