Write down the electron configuration of the Cu(I) ion in the format 1s2_2s2_2p6_etc_etc.
To determine the electron configuration of the Cu(I) ion, we need to find the number of electrons in a neutral copper atom (Cu) and then remove one electron to account for the Cu(I) ion.
The atomic number of copper (Cu) is 29, which means that it has 29 electrons in its neutral state. The electron configuration of a neutral copper atom is:
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^9
To form the Cu(I) ion, one electron is removed. Therefore, subtract one electron from the 4s^2 orbital:
1s^2 2s^2 2p^6 3s^2 3p^6 3d^10
So the electron configuration of the Cu(I) ion is:
1s^2 2s^2 2p^6 3s^2 3p^6 3d^10