i) Write the electronic configuration of each of the following ions of copper: I. Cu++ II. Cu(2+)(2+) [29Cu29𝐶𝑢]

The electronic configuration of a neutral copper atom (Cu) is [Ar] 3d10 4s1. Copper has 29 electrons in its neutral state.

i) For Cu++, also written as Cu(2+), two electrons are removed. These electrons are removed first from the 4s orbital and then from the 3d orbital. So, the electronic configuration of Cu++ or Cu(2+) is [Ar] 3d9.

ii) For Cu(2+)(2+), it seems like there might be a mistake in the question. Cu(2+) already represents a copper ion with a charge of +2, so Cu(2+)(2+) would suggest a charge of +4, which is not commonly seen for copper. If we were to remove 4 electrons from a neutral copper atom, the electronic configuration would be [Ar] 3d7. However, this is not a common or stable state for copper.