2.43 (a) Silver

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Grace Lee 3G
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Joined: Fri Sep 29, 2017 7:07 am

2.43 (a) Silver

Postby Grace Lee 3G » Sun Oct 22, 2017 5:01 pm

How come the ground-state electron configuration for silver is [Kr]4d^10 5s^1? I put [Kr]4d^9 5s^2 as my answer but I don't seem to understand how that's incorrect.

Jessica Schirmer 1J
Posts: 20
Joined: Fri Sep 29, 2017 7:04 am

Re: 2.43 (a) Silver

Postby Jessica Schirmer 1J » Sun Oct 22, 2017 6:15 pm

I believe that the reason Silver is [Kr]4d^10 5s^1 is the same reason why Copper is an exception. The atom is more stable if the d orbital is completely full rather than partially full. Therefore one e- from the 5s orbital is "moved" into the 4d orbital.

Isabelle Bautista 3H
Posts: 23
Joined: Fri Sep 29, 2017 7:06 am

Re: 2.43 (a) Silver

Postby Isabelle Bautista 3H » Mon Oct 23, 2017 3:17 pm

So can anyone confirm the exceptions, since it appears that silver is also following the exception that I thought applied only to chromium and copper?

Clara Rehmann 1K
Posts: 53
Joined: Fri Sep 29, 2017 7:03 am

Re: 2.43 (a) Silver

Postby Clara Rehmann 1K » Mon Oct 23, 2017 3:44 pm

Jessica is right - there are more exceptions than Cr and Cu, but those are the only two we learned about. Having 5 or 10 electrons in the d orbital is more stable than having 4 or 9, so any d-block element that ends up with 4 or 9 electrons in the d orbital will actually have 5 or 10 (and then just one in the subsequent s orbital).

Chem_Mod
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Re: 2.43 (a) Silver

Postby Chem_Mod » Mon Oct 23, 2017 4:55 pm

Essentially it's hard to determine these configurations only from the things you have learn. You just need to memorize the chromium and copper case.


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