Question 2.43 6th Edition

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Samantha Man 1L
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Joined: Fri Sep 28, 2018 12:22 am

Question 2.43 6th Edition

Postby Samantha Man 1L » Tue Oct 23, 2018 3:20 pm

For this problem they ask you to write out the ground-state electron configuration of different elements given. Does anyone know why silver is written as [Kr](4d^10)(5s^1) and not as [Kr](5s^2)(4d^9)?

Andonios Karas 4H
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Re: Question 2.43 6th Edition

Postby Andonios Karas 4H » Tue Oct 23, 2018 3:29 pm

Silver is one of the few exceptions to the common rule. While filling the s-orbital then filling the d-orbital typically achieves the lowest energy state for an atom, Silver, among other elements like Chromium and Copper, has a lower energy state with only 1 electron in the s-orbital and a full d-orbital. This is because Silver is a transition metal. However, because we only need to know the electron configurations of the elements in the 1st row of the d-block, you'll just to remember Chromium's and Copper's configuration.

Catherine Kim 3K
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Joined: Fri Sep 28, 2018 12:26 am

Re: Question 2.43 6th Edition

Postby Catherine Kim 3K » Tue Oct 23, 2018 10:30 pm

The rule is to write 5s e- after 4d e-. As for silver, d^10 has lower energy. A lower total energy may be achieved if an electron enters a 4d orbital instead of expected 5s orbital, if that arrangement completes a full subshell. You can find other exceptions to the building-up principle in Appendix 2C of the textbook [6th edition for me].


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