What is the electron configuration for copper?

Answer 1

Copper's atomic number is 29. Filling in the first 29 orbitals gives the configuration of 1s2 2s2 2p6 3s2 3p6 4s1 3d10. Seeing as how there is only one electron in the 4 shell, coppers valence electron configuration is thus 4s1.

Answer 2

The valence electron configuration of copper is 4s1 3d10 because copper doesn't have a valence electron total of 11 (a D orbital cannot hold more than 10 electrons). Therefore, everything is moved up 1, so there is only 1 valence electron in the s orbital.

Answer 3

Cu 1+:

[Ar] 3d10 4s1

Cu 2+:

[Ar] 3d10 4s2

Although this is apparently contradictory to the usual rule, Cu 2+ really IS more stable than Cu 1+. This anomaly has been attributed to the Jahn-Teller effect which is the lengthening of the axial ligand bonds in a transition metal complex. I'm not sure what that means, but that's the answer.

It may not be the answer to this question but the answer to this one: What is the electron configuration for ion copper 1 and 2

Answer 4

1s2 2s2 2p6 3s2 3p6 3d10 4s1.

See the Related Questions links for more information about copper.

Answer 5

1s2 2s2 2p6 3s2 3p6 4s2 3d9

because you have to fill 4s first because it is lower in energy and following the aufbau principle lower energy levels are filled first

Answer 6

The electron configuration for copper is: 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1

Answer 7

[Ar]4s^13d^10

A filled or half-filled d shell is more stable. So, in the most stable configuration the 3p shell takes an electron from the 4s orbital

Answer 8

The electron configuration for copper is [Ar] 3d10 4s1. Despite copper being in Group 11 of the Periodic Table, it fills its 3d orbital before its 4s orbital due to stability reasons.

Answer 9

[Ar]4s1,3d10