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.
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.
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
1s2 2s2 2p6 3s2 3p6 3d10 4s1.
See the Related Questions links for more information about copper.
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
The electron configuration for copper is: 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1
[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
[Ar]4s1,3d10
[Ar],4s2,3d9
copper
The electron configuration of sulfur (long) is: 1s22s22p63s23p4. The electron configuration of sulfur (short) is: [He]3s23p4.
The longhand electron configuration for sulfur is 1s2.2s2.2p6.3s2.3p4.
The electron configuration of aluminium is [Ne]3s2.3p1.
The electron configuration of copper(II) is [Ar] 3d9 . Copper is [Ar] 3d10 4s1
The electron configuration of copper is: [Ar]4s13d10. It isn't 4s23d9 because Cu is able to obtain a more stable electron configuration when it takes an electron from the 4s and adds it to 3d. A half filled 4s and a completely filled 3d is more stable.
The electron configuration of copper is 1s22s22p63s23p63d104s1.
The expected ground-state electron configuration of copper is ; however, the actual configuration is because a full dsubshell is particularly stable. There are 18 other anomalous elements for which the actual electron configuration is not what would be expected.
The electron configuration of a Copper(II)ion is [Ar]4s0 3d9.
The abbrieviated electron configuration of copper is [Ar] 4s23d9
[Ar],4s2,3d9
yes, Cu+ has a pseudo-noble-gas electron configuration
copper
1 valence electron. The electronic configuration of copper is 2, 8, 18, 1
only five filled sublevels
The electron configuration is the number of electrons in each energy level of an element. The electron configuration of Li is, 1s2 2s1. The electron configuration of F is, 1s2 2s2 2p5.