Final answer:
The electronic configuration of Cu(I) is 3d¹⁰, a fully filled d-subshell, typically leading to higher stability, while Cu(II) has a 3d⁹ configuration which is less stable due to an unpaired electron. However, the stability of these ions can vary with the specific ligands and coordination environment in different complexes.
Step-by-step explanation:
The question revolves around the electronic configuration and stability of Cu(I) and Cu(II) ions. Based on the given information, the electronic configuration of Cu(I) is 3d¹⁰, which means it has a completely filled d-subshell. This configuration generally leads to a higher level of stability due to the 'exchange energy' and fully paired electrons in the orbitals.
On the other hand, Cu(II) has an electronic configuration of 3d⁹, indicating an incomplete d-subshell with one unpaired electron, which usually results in less stability. However, the actual stability of copper ions in solution can depend on factors such as the ligands present and the overall coordination environment. For example, Cu(NO3)2.5H2O, a copper(II) complex, exhibits bright colors which are typical of d-electron transitions that can take place when the d-orbitals are not fully occupied.
In general, a fully occupied or a half-filled d-subshell is associated with higher stability due to symmetrical distribution of electrons and reduced repulsion among them. The stability of Cu(I) and Cu(II) can thus differ based on the geometry and nature of ligands in the complexes. Given these factors, the stability can also be context-dependent.