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An example of this irregularity would be that that the electron configuration of Copper(Cu) would be [Ar]3d^10, 4s^1. Instead of having 9 electrons in the d subshell, the elements would be at a lower potential energy with 10 electrons, taking one away from the s subshell.
AustinGrove3B wrote:Having full or half full subshells is less potential energy than having semi full subshells. For that reason, sometimes electrons will be taken from the s subshell to fill the d subshell.
Thanks, I was confused about this too, and this example was so helpful!
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