Electron Configuration clarification

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sfoksn

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Okay, so as far as I remember, only Cr, Mo, Au, Ag, Cu only follow the weird distribution of electrons (half filled s or half filled d) in the ground state. When things are ionized, however, do every element follow the irregular pattern?

Because, Zn, when it becomes Zn2+, it seems to lose electrons from 4s shell instead of 3d shell to maintain fully filled 3d orbital.. Nickel, which has same electron configuration with the Zn2+, has 4s2 3d8.

So what is it? Is there a rule I can follow to determine this?

Thanks in advance.
 
Okay, so as far as I remember, only Cr, Mo, Au, Ag, Cu only follow the weird distribution of electrons (half filled s or half filled d) in the ground state. When things are ionized, however, do every element follow the irregular pattern?

Because, Zn, when it becomes Zn2+, it seems to lose electrons from 4s shell instead of 3d shell to maintain fully filled 3d orbital.. Nickel, which has same electron configuration with the Zn2+, has 4s2 3d8.

So what is it? Is there a rule I can follow to determine this?

Thanks in advance.

Normally, when there are no electrons, 4s is lower in energy than the 3d. That is why we fill it in 4s then 3d. But, once the 3d gets electrons, it drops in energy below 4s. So when you remove electrons, the electrons come from the higher energy 4s shell.

There is some rule where you add the n+l numbers or something and the one with the highest number is the one you remove the electrons from. I don't exactly remember it, but it was posted here before.

Link http://forums.studentdoctor.net/showthread.php?p=9345141#post9345141

And it is not only Cr and Cu luv8724. It is the ones sfoksn listed.
 
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