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.
Thank you so much
Dear Abdur Raheem ,
In the following link you will find the explanation why:
https://terpconnect.umd.edu/~wbreslyn/chemistry/electron-configurations/configurationCopper-Cu.html
Think this will solve the ‘mystery’ for you.
Best regards.
Dear Abdur Raheem, the electronic configuration of Cu is [Ar]3d10 4s1 because, completely filled subshell exhibit extra stability. The electronic configuration of Cu2+ is [Ar]3d9.
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