thehipster

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Why is the electron configuration for Zn2+ [Ar]4s0 3d10 and not
[Ar]4s2 3d8? Does the d group not lose electrons? Will it always be taken from the s group or just in this case?

Thanks
 

dontbam

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thehipster said:
Why is the electron configuration for Zn2+ [Ar]4s0 3d10 and not
[Ar]4s2 3d8? Does the d group not lose electrons? Will it always be taken from the s group or just in this case?

Thanks
you always want to make the most stable electron configuration according to some law, i forget, so the 2 electrons in the 4s orbital will excite to the 3d8 to make 3d10

if you have 3d8 you have TWO unfilled orbitals, therefore if you fill them up to 10, then you'll have filled all the orbitals making Zn+2 more stable
 
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