Final answer:
The correct orbital diagram for a Cd2+ ion is represented by option D, which shows the electron configuration as 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 after two electrons are removed from the outermost 5s orbital.
Step-by-step explanation:
The question involves determining the correct orbital diagram for a Cd2+ ion. Cadmium (Cd) has an atomic number of 48 which means the neutral atom has 48 electrons. However, as we are considering a Cd2+ ion, two electrons are removed, leaving us with 46 electrons to distribute in the orbitals. The electron configuration of a neutral Cd atom is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10. When forming the Cd2+ ion, the two electrons from the outermost shell are removed, specifically from the 5s orbital, resulting in the configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10. The correct answer is, therefore, 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10, which corresponds to option D.