Writing e- configurations of atoms

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Johana Jeon 1A
Posts: 30
Joined: Sun Feb 12, 2017 3:00 am

Writing e- configurations of atoms

Postby Johana Jeon 1A » Sun Jul 16, 2017 3:32 pm

In the course reader page 65, I'm still not 100% sure as to why e- configuration of chromium is, Cr: [Ar] 3d^5 4s^1 and copper is, Cu: [Ar] 3d^10 4s^1
Why is it not 3d^5 4s^2?
Also when writing e- configurations, what's the oder of orbitals? Is it f-orbital, d-orbital, p-orbital, and then s-orbital?

Davalanya 1F
Posts: 23
Joined: Fri Jun 23, 2017 11:39 am
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Re: Writing e- configurations of atoms

Postby Davalanya 1F » Sun Jul 16, 2017 4:08 pm

Cu and Cr are just the two e- configuration exceptions we have to know. They do not follow the normal guide of the periodic table. if you look at the e- configuration of zinc its 3d^10s^2. In the chemical principles book, when you open the textbook the periodic table has the e- configurations for all the elements.
The order is f,d,s,p.

Katherine Jordak 1H
Posts: 51
Joined: Fri Sep 29, 2017 7:05 am

Re: Writing e- configurations of atoms

Postby Katherine Jordak 1H » Sun Oct 22, 2017 4:44 pm

As Davalanya said, copper and chromium are exceptions to the electron configuration. This is because the predicted copper electron configuration has the d subshell at 1 electron less than it needs to be half full. Therefore, the d subshell snags an electron from the s subshell. This happens because the atom is more stable if the outer subshell is either half full or completely full.


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