Mg: 1s2- 2s2 - 2p6 - 3s2
1s2 2s2 2p6 3s2 3p6 3d10 4s1
[Xe]4f145d106s26p2
4s2 3d6
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.
Cu+3 reported formally in 2007. Cu 1 e's in 4S and 10 e's in 3D Cu+3 0 e's in 4S and 8 e's in 3D LFSE suggets the existence of Cu+3.
The element that has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 is Bromine
the electronic configuration of cu is4s1 ,3d10 and ofcr is 4s1 3d5,cu prefers to filled d shell and in cu s d both are half filled.as there bis very short energy difference therefore electron used to jumps within d and s sub shell causing irregular valency of the elements
In the case of chromium (Cr), the electron configuration of 3d54s1 is more stable than 3d44s2. A half-filled sublevel is more stable than a sublevel that is less than half full. In the case of copper (Cu), the electron configuration of 3d104s1 is more stable than 3d94s2, again because a full sublevel and a half-filled sublevel is more stable.
The electron configuration of Cu2+ is [Ar]3d94s0.
There is 1 unpaired electron in Copper (Cu)
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 electronic configuration od Cu is [Ar] 3d10 4s1 This is an exception to the aufbau principle which would predict [Ar] 3d9 4s2.
The electron configuration of copper is 1s22s22p63s23p63d104s1.
Cu+3 reported formally in 2007. Cu 1 e's in 4S and 10 e's in 3D Cu+3 0 e's in 4S and 8 e's in 3D LFSE suggets the existence of Cu+3.
Because copper loose electron from its penultimate outer shell
The element that has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 is Bromine
yes, Cu+ has a pseudo-noble-gas electron configuration
the electronic configuration of cu is4s1 ,3d10 and ofcr is 4s1 3d5,cu prefers to filled d shell and in cu s d both are half filled.as there bis very short energy difference therefore electron used to jumps within d and s sub shell causing irregular valency of the elements
The atom always stays in maximum stability.. The orbital with full electrons , no electron or half electrons is maximum stable ... In the case of Cu the electron moves in 3d orbital because in that case the 3d orbital is going to be filled with maximum 10 electrons hence the 4s orbital is going to be filled with half number of electrons - 1 electron ..... So the last electron goes in the 3d orbital except going into 4s orbital..... therefore the electron configuration of Cu is [Ar]3d10 4s1 .....The reason is same for the atom of Silver.....
In the case of chromium (Cr), the electron configuration of 3d54s1 is more stable than 3d44s2. A half-filled sublevel is more stable than a sublevel that is less than half full. In the case of copper (Cu), the electron configuration of 3d104s1 is more stable than 3d94s2, again because a full sublevel and a half-filled sublevel is more stable.