To write the configuration for the Manganese ions, first we need to write the electron configuration for just Manganese (Mn). We first need to find the number of electrons for the Mn atom (there are 25 electrons) using the Periodic Table. When we write the configuration, we'll put all 25 electrons in orbitals around the nucleus of the Manganese atom.
In this video we'll use the Periodic Table to help us write the notation for Manganese. Alternatively you can use a chart showing how the orbitals fill ([ Ссылка ]).
Either way, the Manganese electron configuration will be 1s2 2s2 2p6 3s2 3p6 3d5 4s2
Note that when writing the electron configuration for an atom like Mn, 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 an explanation why).
For the Mn2+ ion we remove two electrons from 4s2 leaving us with:
1s2 2s2 2p6 3s2 3p6 3d5
For the Mn3+ ion we remove a total of three electrons (two from the 4s2 and one form the 3d5) leaving us with
1s2 2s2 2p6 3s2 3p6 3d4
• Introduction to Writing Electron Configurations: [ Ссылка ]
• Electron Configurations Chart: [ Ссылка ]
• Writing Electron Configs Using only the Periodic Table: [ Ссылка ]
• Order of d and s Orbital Filling: [ Ссылка ]
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.
