Electronic Structure (AQA GCSE Chemistry: Combined Science)

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Electronic structure

  • We can represent the structure of the atom in two ways: using diagrams called electron shell diagrams or by writing out a special notation called the electronic configuration (or electronic structure or electron distribution)

Electron shell diagrams

  • Electrons orbit the nucleus in shells (or energy levels) and each shell has a different amount of energy associated with it
  • The further away from the nucleus, the more energy a shell has
  • Electrons fill the shell closest to the nucleus 
  • When a shell becomes full of electrons, additional electrons have to be added to the next shell
    • The first shell can hold 2 electrons
    • The second shell can hold 8 electrons 
  • For this course, a simplified model is used that suggests that the third shell can hold 8 electrons
    • For the first 20 elements, once the third shell has 8 electrons, the fourth shell begins to fill
  • The outermost shell of an atom is called the valence shell and an atom is much more stable if it can manage to completely fill this shell with electrons 

Electron shell diagram

Diagram to show the rules of electron-shell filling

A simplified model showing the electron shells

  • The arrangement of electrons in shells can also be explained using numbers
  • Instead of drawing electron shell diagrams, the number of electrons in each electron shell can be written down, separated by commas
  • This notation is called the electronic configuration (or electronic structure)
    • The electronic structure of carbon is 6 electrons, 2 in the 1st shell and 4 in the 2nd shell
      • So its electronic configuration is 2,4
  • Electronic configurations can also be written for ions
    • E.g. A sodium atom has 11 electrons, a sodium ion has lost one electron, therefore has 10 electrons; 2 in the first shell and 8 in the 2nd shell
      • Its electronic configuration is 2,8

Examiner Tip

All of the shells up to the outer shell will be full. Electron transfer occurs with electrons from the outer shell only. You can use the term ‘shell’, 'orbital' or ‘energy level’ to describe the space that electrons occupy.

Electronic configuration: number notation

How does the electronic structure of an element relate to its location in the Periodic Table?

  • There is a clear relationship between the electronic configuration and how the Periodic Table is designed
  • The number of notations in the electronic configuration tells us the number of occupied shells
    • This tells us what period an element is in
  • The last notation shows the number of outer electrons the atom has
    • This tells us the group an element is in
  • Elements in the same group have the same number of outer shell electrons 

Diagram showing the relationship between the electronic configurations

Diagram to show the two ways to represent electronic structure of chlorine

The electronic configuration for chlorine

  • Period: The red numbers at the bottom show the number of notations 
    • The number of notations is 3
    • Therefore chlorine has 3 occupied shells 
  • Group: The last notation, in this case 7
    • This means that chlorine has 7 electrons in its outer shell 
    • Chlorine is therefore in Group 7

The Periodic Table showing the location of chlorine 

Position-of-Chlorine-in-Periodic-Table

Chlorine is in Group 7, Period 3

Examiner Tip

The group number will be labelled on the Periodic Table you are given in your exam, but the period number isn't so it is a good idea to write this on yourself at the beginning. 

Electronic configuration: First 20 elements

The Electronic Configuration of the First Twenty Elements

Element Atomic Number  Electronic Configuration
hydrogen 1 1
helium 2 2
lithium 3 2,1
berylium 4 2,2
boron 5 2,3
carbon 6 2,4
nitrogen 7 2,5
oxygen 8 2,6
fluorine 9 2,7
neon 10 2,8
sodium 11 2,8,1
magnesium 12 2,8,2
aluminium 13 2,8,3
silicon 14 2,8,4
phosphorus 15 2,8,5
sulfur 16 2,8,6
chlorine 17 2,8,7
argon 18 2,8,8
potassium 19 2,8,8,1
calcium 20 2,8,8,2

Note: although the third shell can hold up to 18 electrons, the filling of the shells follows a more complicated pattern after potassium and calcium. For these two elements, the third shell holds 8 and the remaining electrons (for reasons of stability) occupy the fourth shell first before filling the third shell.

Worked example

Draw and write the electronic structure of magnesium. 

Answer:

  • Magnesium has 12 electrons in total.
  • A maximum of two can fit in the first shell and eight in the second shell.
  • The remaining two will occupy the third shell. 

magnesium-atom

  • The written form of this electronic structure is 2,8,2 

Examiner Tip

You should be able to represent the first 20 elements using either electron shell diagrams or written electronic configuration.

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Stewart

Author: Stewart

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Exam Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.