Understanding electronic structure is crucial for understanding the chemistry of reactions. Here, we will review how to deduce electronic configurations of atoms and explain what is meant by the terms shells, subshells and orbitals.
Electron shells
Electrons orbit the nucleus in electron shells, called quantum shells which are given principal quantum numbers. Each quantum shell contains different types of subshells. Each subshell contains a different number of orbitals. The four types of subshells and the number of electrons they can hold are summarised below.
subshell
number of orbitals
maximum electrons
s
1
1×2=2
p
3
3×2=6
d
5
5×2=10
f
7
7×2=14
And the subshells and electrons in the first four quantum shells are summarised below.
shell
subshells
number of electrons
1st
1s
2
2nd
2s2p
2+(3×2)=8
3rd
3s3p3d
2+(3×2)+(5×2)=18
4th
4s4p4d4f
2+(3×2)+(5×2)+(7×2)=32
Orbitals
Each subshell contains different numbers of orbitals, which can hold up to two electrons. Orbitals have characteristic shapes.
s orbitals are spherical.
p orbitals are shaped like dumbbells, of which there are three.
Below is an s-orbital.
Below is a p-orbital, of which there are three kinds; pz, py and px.
Note: Electrons in each orbital spin in opposite directions, this is called 'spin-pairing'.
Deducing electronic configuration
A simple set of rules must be followed to work out electronic configuration.
Rule
explanation
1. Arrows in boxes
Electrons in orbitals are represented by arrows in boxes. Each box represents one orbital and an arrow represents one electron.
2. Lowest energy subshells first
Electrons fill up the lowest energy subshells first. From low to high, the order is: 1s2s2p3s3p4s3d4p4d4f. Note, unusually, 4s is filled before 3d because it is lower in energy, even though it's principal quantum number is bigger; this is an exception you must remember.
Below is the electronic configuration of calcium.
3. Single before double
Electrons fill orbitals singularly before they start to pair up.
To represent electronic configuration, you can either draw out the energy levels (as in the image for Rule 2. above) or use subshell notation.
Example
For potassium, the subshell notation is:1s22s22p63s23p64s1. You can check this is correct by adding the total of the superscripts. Here, it equals 19, which tells you it is correct as that is the number of electrons in a K atom.
Note: Noble gas symbols (i.e Ar or Ne) are sometimes used for simplicity. For potassium, it is also correct to write the configuration as [Ar]4s1, since the [Ar] corresponds to 1s22s22p63s23p6.
Using the periodic table
The periodic table can be used as it is split into s-block, p-block and d-block elements.
s-block elements have an outer shell configuration of s1 or s2.
p-block elements have an outer shell configuration of p1 to p6.
d-block elements have an outer shell configuration of d1 to d10.
Remember: 4s must be filled to 4s2, and only afterwards 3d can be filled.
Exception to the rule
Cr and Cu don't fit the usual rule. Their 4s shell only ever fills to 4s1 as they donate the second electron to the 3d subshell as it's more stable.
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Unit 1
The history of the atom
Unit 2
Electronic configuration
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Electronic structure: shells and orbitals
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FAQs - Frequently Asked Questions
What is meant by 'spin-pairing'?
Spin-pairing explains that electrons in each orbital spin in opposite directions.
How do you work out electronic configuration?
To deduce electronic configuration:
1. Draw arrows in boxes,
2. Fill lower energy subshells first,
3. Fill electrons singularly before pairing up.
What shapes do orbitals have?
s orbitals are spherical. p orbitals are shaped like dumbbells, of which there are three.