Why is the electron configuration of chromium #"[Ar]3d"^5"4s"^1"# and not #"[Ar]3d"^4"4s"^2"#, and why is the #"3d"# sublevel written before the #"4s"# sublevel even though it is higher in energy?

Question

Luna Chen · Accepted Answer

The electron configurations of the elements are determined experimentally. Chromium is one of the approximately 20 transition metal exemptions to the Aufbau sequence of filling orbitals.

The experimentally determined electron configuration of chromium is #"[Ar]3d"^5"4"^1"# rather than #"[Ar]3d"^4"4s"^2"#. It may be that the electron configuration in which a sublevel is completely filled or half-filled is lower in energy and therefore more stable.

Avery Adams · Answer

Refer to the explanation.

When writing electron configurations using the Aufbau principle, there are two schools of thought. One is like the electron configuration of chromium in your question, in which the #"3d"# sublevel is written before the #"4s"# sublevel.

When written this way, all of the sublevels for #"n=3"# are written together in order of sublevels #3# s, p, and d, even though the #"4s"# sublevel fills before the #"3d"# sublevel according to the Aufbau principle. This has the advantage of writing the valence electrons (highest energy s and p sublevels) at the end of the electron configuration.

The other school of thought is that the electron configuration of an element should be written so that the sublevels are in order of increasing energy, which will place the #"4s"# sublevel before the #"3d"# sublevel as indicated by the Aufbau diagram. Using this method, the electron configuration for chromium would be written as #["Ar"]"4s"^1"3d"^5#.

Either way is acceptable, however placing the 3d sublevel before the 4s sublevel is more common. Ask your instructor which method he or she prefers.

Mateo Aguilar · Answer

undefined The electron configuration of chromium is [Ar]3d^54s^1 instead of [Ar]3d^44s^2 because it is more energetically favorable for chromium to have a half-filled d sublevel. This arrangement provides greater stability due to exchange energy and Hund's rule, which state that electrons prefer to occupy orbitals singly before pairing up. Despite the 4s sublevel being higher in energy than the 3d sublevel, the 3d sublevel is filled first because it is within the same principal energy level (n=3) and experiences greater effective nuclear charge, making it slightly lower in energy than the 4s sublevel.