Final answer:
The electron configuration for a Pd2+ ion is [Kr]4d8, which is derived from the neutral palladium atom's electron configuration [Kr]4d105s0 after losing two electrons.
Step-by-step explanation:
The electron configuration for a Pd2+ ion involves first determining the configuration of a neutral palladium (Pd) atom and then accounting for the loss of two electrons due to the positive charge.
Palladium has an atomic number of 46, which gives it 46 electrons as a neutral atom. Its electron configuration is [Kr]4d105s0. As Palladium is in the d-block, it is known for its ability to achieve a filled or half-filled d subshell which makes it more stable. When Pd loses two electrons to form Pd2+, these electrons are removed from the 4d orbital, leaving us with the configuration [Kr]4d8. Thus, the electron configuration for Pd2+ is [Kr]4d8.