what is the correct electron configuration for Zn2+?

[Smooth Operater]

what is the correct electron configuration for Zn2+?

[Ar] 4s2,3d8
[Ar] 4s0,3d10

the right answer is [Ar] 4s0,3d10

but i thought 3d subshell has higher energy than 4s subshelll there electron should be removed first from 3d subshell.

Thanks!

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[souslepont]

You're right, but remember, the transition metals are special. They basically never follow the rules. That's what I tell myself when I don't know the answer, anyway.

 

[jackbauer!]

remember, atoms/molecules always want to be in their lowest, most stable state.

Zn2+ is in a lower state when it's d-subshell is filled (i.e. 4s0 3d10), rather than when it's s-subshell is filled and it's d-subshelled has unpaired electrons (i.e. 4s2 3d8)......

the first case is paramagnetic and the second, correct case, is diamagnetic.

hopefully that makes sense.

jb!

 

[Whimsique]

when it has a charge we first subtract it from the lowest energy orbital?

 

[Sea of ASH]

when it has a charge we first subtract it from the lowest energy orbital?

no the highest. 4 is higher than 3...

 

[dl9006]

memorize as fact

 

[klutzy1987]

4S has more energy than 3D so 4S will always lose electrons first.

 

[Phloem01]

I'm confuzed...Zn2+ would have the same configuration as nickel and my periodic table shows the nickel config. as [Ar]3d84s2

 

[HowAboutDAT]

so it fills the 4s orbital before the 3d, but empties the 4s before the 3d...right?