Copper can exist in non-ionic form (as Cu) or in one of two redox states: Cu (reduced) or Cu (oxidized). Each form of Cu has a specific distribution of electrons (i.e., electron configuration), tabulated below:
The electronic configurations of Cu control the number and types of bonds Cu can form with other atoms (e.g., see Copper Biology section). These diverse coordination chemistries are what enable Cu to participate in many different biological and chemical reactions.
Finally, due to its full d-orbital, Cu has diamagnetic resonance. In contrast, Cu has one unpaired electron in its d-orbital, giving it paramagnetic resonance. The different resonances of the Cu ions enable determination of Cu's redox state by techniques such as electron paramagnetic resonance (epr) spectroscopy, which can identify atoms with unpaired electrons by exciting electron spins.