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.
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 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 element that has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 is Bromine
The electron configuration is incomplete. Assuming that you mean [Ar]4s23dy, here are the possibilities: y=1 Sc y=2 Ti y=3 V y=4 Cr (Actually [Ar]4s13d5) y=5 Mn y=6 Fe y=7 Co y=8 Ni y=9 Cu (Actually [Ar]4s13d10) y=10 Zn Basically the first row of transition metals, since their outermost electron shell is the 3d shell.
Cu
The electron configuration of Cu2+ is [Ar]3d94s0.
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.
Ca 4s23d9
The electronic configuration od Cu is [Ar] 3d10 4s1 This is an exception to the aufbau principle which would predict [Ar] 3d9 4s2.
actually all the elements listed can exhibit.
Only the atomic radius is equivalent - 128 pm.
There is 1 unpaired electron in Copper (Cu)
Argon
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 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.
1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d10 or [Ar]3d10, 4s1