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I understand why Chromium and Copper are exceptions using the symmetry argument. However, why isn't Vanadium an exception as well? The configuration for Vanadium is [Ar]3d^3 4s^2. Why don't the 2 electrons from 4s go to 3d to fill the d orbital?
I believe that the exceptions to electron configuration involve only moving one electron into the S orbital in order to make the d orbital stable. This is done when the d orbital is half full or full. In your example, Vanadium requires two electrons to be moved and not one.
It is just not energetically favorable enough to remove 2 electrons from the 4s and move them in parallel spins to 3d orbitals. Although the symmetry is achieved, it's just not energetically favorable.
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