How to write the electronic configuration of elements?
Writing electronic configuration of elements is a skill every student must learn if they have a smooth ride in their chemistry journey.
But don’t worry, writing electronic configuration is really simple and I will teach you all you need to do.
I want to emphasize that there are two forms of electronic configuration; shell electronic configuration and electronic configuration.
The orbital configuration can be written with the knowledge of the electronic configuration however this article is all about electronic configuration.
I will try and elucidate the configuration of the first few elements in the periodic table.
The electronic configuration follows a regular pattern according to AufBau’s principle.
Is 2s 2p 3s 3p 4s 3d ………..
Please remember that the sub-levels have different capacities of electrons. S orbitals contain 2 electrons, p orbital contains 6 electrons, d orbital contains 10 electrons while f orbital contains 14 electrons.
Electronic configuration of Hydrogen
To write the electronic configuration of hydrogen, you need to remember the atomic number of the element.
Hydrogen has atomic number 1.
Shell electronic configuration – 1
Electronic configuration – Is1
This is an s block element.
Electronic configuration of Carbon
To write the electronic configuration of Carbon, you need to remember the atomic number of the element.
Carbon has atomic number 6.
Shell electronic configuration – 2,4
Electronic configuration – Is2 2s2 2p2
This is a p block element
Electronic configuration of Neon
To write the electronic configuration of Neon, you need to remember the atomic number of the element.
Neon has the atomic number 10.
Shell electronic configuration – 2, 8
Electronic configuration – Is2 2s2 2p6
Electronic configuration of Sodium
To write the electronic configuration of Sodium, you need to remember the atomic number of the element.
Sodium has the atomic number 11.
Shell electronic configuration – 2,8,1
Electronic configuration – Is2 2s2 2p6 3s1
Electronic configuration of Alumnium
To write the electronic configuration of Aluminium, you need to remember the atomic number of the element.
Aluminium has atomic number 13.
Shell electronic configuration – 2, 8, 3
Electronic configuration – Is2 2s2 2p6 3s2 3p1
Electronic configuration of Silicon
To write the electronic configuration of Silicon, you need to remember the atomic number of the element.
Aluminium has atomic number 14.
Shell electronic configuration – 2, 8, 4
Electronic configuration – Is2 2s2 2p6 3s2 3p2
Electronic configuration of Argon
To write the electronic configuration of Argon, you need to remember the atomic number of the element.
Argon has atomic number 18.
Shell electronic configuration – 2, 8, 8
Electronic configuration – Is2 2s2 2p6 3s2 3p6
You will notice that the configuration of Nein and Argon are completely filled up.
Electronic configuration of Calcium
To write the electronic configuration of Calcium, you need to remember the atomic number of the element.
Calcium has atomic number (electron) of 20
Shell electronic configuration – 2, 8, 8,2
Electronic configuration – Is2 2s2 2p6 3s2 3p6 4s2
Electronic configuration of Scandium
To write the electronic configuration of Scandium, you need to remember the atomic number of the element.
Scandium has atomic number 21.
Electronic configuration – Is2 2s2 2p6 3s2 3p6 4s2 3d1
Electronic configuration of Manganesse
To write the electronic configuration of Manganese, you need to remember the atomic number of the element.
Manganese has atomic number 25.
Electronic configuration – Is2 2s2 2p6 3s2 3p6 4s2 3d5
Hint
It is important to note that the electronic configuration of elements is based on the electrons and not on the atomic number of the elements.
Let me illustrate with examples; the electronic configuration of sodium atom (Na) is different from the electronic configuration sodium ion (Na+)
Na has 11 electrons 1s2 2s2 2p6 3s1
Na+ has 10 electrons 1s2 2s2 2p6
This is a complete guide on how to write an electronic configuration of elements and deduce the number of orbitals.