To write the configuration for the Copper ions, first we need to write the electron configuration for just Copper (Cu). We first need to find the number of electrons for the Cu atom (there are 29 electrons) using the Periodic Table. When we write the configuration, we'll put all 29 electrons in orbitals around the nucleus of the Copper atom.
In this video we'll start with using the Periodic Table to help us write the notation for Copper. Alternatively you can use a chart showing how the orbitals fill ( • Using the Electron Con... ).
This would give us the (incorrect) Copper electron configuration of
1s2 2s2 2p6 3s2 3p6 3d9 4s2
--Copper is an exception! --
Half-filled and fully filled subshell have got extra stability.
Therefore, one of the 4s2 electrons jumps to the 3d9. This give us the (correct) configuration of:
1s2 2s2 2p6 3s2 3p6 3d10 4s1
Note that when writing the electron configuration for an atom like Cu, the 3d is usually written before the 4s. Both of the configurations have the correct numbers of electrons in each orbital, it is just a matter of how the electronic configuration notation is written (see below for link to an explanation why).
For the Cu+ ion we remove one electron from 4s1 leaving us with:
1s2 2s2 2p6 3s2 3p6 3d10
For the Cu2+ ion we remove a total of three electrons (two from the 4s1 and one form the 3d10) leaving us with
1s2 2s2 2p6 3s2 3p6 3d9
• Introduction to Writing Electron Configurations: • Introduction to Electr...
• Electron Configurations Chart: • Using the Electron Con...
• Writing Electron Configs Using only the Periodic Table: • Writing Electron Confi...
• Order of d and s Orbital Filling: eic.rsc.org/Coature/the-troub...
The configuration notation provides an easy way for scientists to write and communicate how electrons are arranged around the nucleus of an atom. This makes it easier to understand and predict how atoms will interact to form chemical bonds.