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In chromium and copper, the are the configuration fill up like $$\mathrm{3d^5 4s^1}$$ but not $\mathrm{4s}$ first as it has lower energy level. and why only these 2 elements.

Wildcat
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cjh
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  • Copper doesn't have $3d^5$ in its base state, but a completely filled $d$ orbital. – M.A.R. Jul 26 '15 at 16:16
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    If you've just only been recently introduced to the electron configurations, then an appropriate answer would be: "the half-filled 3d orbital in Cr and the completely filled 3d orbital in Cu are particularly stable". For a more detailed but also potentially very technical answer, look up exchange energy. – orthocresol Jul 26 '15 at 16:23
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    This is a very popular question in the chemistry world, and it has been asked and answered before: http://chemistry.stackexchange.com/questions/151/why-do-elements-in-columns-6-and-11-assume-abnormal-electron-configurations – Ben Norris Jul 27 '15 at 01:06

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In any element after Argon [1s22s22p63s23p6], the repulsion force between the elctrons increase at a great extent and also the atom becomes very stable. So the elctrons tend to move in far 4s orbital first and after filling it completely , fill the 3d orbital. About chromium and copper, they are exceptions. Any half filled or fully-filled orbitals are more stable then rest of the configurations, so in Chromium one electron of 4s comes to 3d orbital and a stable 3d5 is obtained, similarly in Copper one electron from 4s comes to 3d orbital and forms stable 3d10.

I hope this answers your question, If you have any further doubts you can ask me :)

Mann Bilimoria
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