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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Bjc51192 on April 03, 2011, 09:49:57 PM

Title: Electron configuration of Cu+
Post by: Bjc51192 on April 03, 2011, 09:49:57 PM

Hey everyone,
Im not quite understanding the concept of electron configuration.

Cu+ is a transition metal which means it loses its highest n value since it is +

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d ^ 9 or

[Ar] 4s^2 3d^9

since its losing its highest n value it will be [Ar] 4s^1 3d^9

However, the answer is [Ar] 3d^10

can someone explain why?

ty

Title: Re: Electron configuration of Cu+
Post by: opti384 on April 04, 2011, 12:14:34 AM

Quote

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d ^ 9

Is this correct?

Title: Re: Electron configuration of Cu+
Post by: Bjc51192 on April 04, 2011, 08:12:19 AM

Thats just what I think it is. The answer was 3d10

Title: Re: Electron configuration of Cu+
Post by: tamim83 on April 04, 2011, 08:50:25 AM

The electron configuration for Cu is [Ar] 4s¹ 3d¹⁰.