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Cu electronic configuration is 1s2 2s2 …

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Cu electronic configuration is 1s2 2s2 2p6 3s2 3p6 4s1 3d10 When we convert it cu2+ then why electron go from 4s1 and 3d9.....why electron go from 4s1 Electron will always go from 3d10 to 3d8.direct from D orbital but why from 4s1

Posted by Abhishek Maurya 5 years, 5 months ago

CBSE > Class 12 > Chemistry

2 answers

Lucky Singh 5 years, 5 months ago

Electronic configuration of Cu is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d9 ([Ar] 4s2, 3d9), whereas for Cu2+ is [Ar], 3d9. I found some periodic tables and electronic configuration notes, there is [Ar] 4s1, 3d10 for Cu. Isn't electron should be fill first 4s (2 e) and then 3d9? and for the ionize state of Cu (Cu2+) electron shouldn't be escape from the 4s state? Also I'm looking for the reason of electronic configuration [Ar] 4s1, 3d10.

Maneesh Kumar 5 years, 5 months ago

It is so because as we know that 4s electrons are filled first as they have lower energy than 3d. Electronic configuration of Cu should be [Ar]4s2,3d9 but it is observed that actual electronic configuration of Cu is [Ar]4s1,3d10. As 4s orbital has only one electron so it is no longer low energy orbital. It has energy higher than 3d and it lose electron first because electron will be removed first from the orbital which is farther from nucleus.

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