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Determining Electronic Configuration (CIE AS Chemistry)

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Determining Electronic Configurations

  • Writing out the electronic configuration tells us how the electrons in an atom or ion are arranged in their shells, sub-shells and orbitals
  • This can be done using the full electron configuration or the shorthand version
    • The full electron configuration describes the arrangement of all electrons from the 1s sub-shell up
    • The shorthand electron configuration includes using the symbol of the nearest preceding noble gas to account for however many electrons are in that noble gas
  • Ions are formed when atoms lose or gain electrons
    • Negative ions are formed by adding electrons to the outer sub-shell
    • Positive ions are formed by removing electrons from the outer sub-shell
    • The transition metals fill the 4s sub-shell before the 3d sub-shell but lose electrons from the 4s first and not from the 3d sub-shell
      • Remember: The 4s sub-shell is lower in energy
  • The Periodic Table is split up into four main blocks depending on their electronic configuration:
    • s block elements
      • Have their valence electron(s) in an s orbital
    • p block elements
      • Have their valence electron(s) in a p orbital
    • d block elements
      • Have their valence electron(s) in a d orbital
    • f block elements
      • Have their valence electron(s) in an f orbital

The blocks of the Periodic Table

Atomic Structure Electronic Configuration & Periodicity, downloadable AS & A Level Chemistry revision notes

The elements can be divided into the s, p, d or f block, according to their outer shell electron configuration

Exceptions

  • Chromium and copper have the following electron configurations, which are different to what you may expect:
    • Cr is [Ar] 4s1 3d5 not [Ar] 4s2 3d4 
    • Cu is [Ar] 4s1 3d10 not [Ar] 4s2 3d9 
  • This is because the [Ar] 4s1 3d5 and [Ar] 4s1 3d10 configurations are energetically stable

Worked example

Write down the full and shorthand electron configuration of the following:

  1. Potassium
  2. Calcium
  3. Gallium
  4. Ca2+ 

Answer 1:

  • Potassium has 19 electrons so the full electronic configuration is:
    • 1s2 2s2 2p6 3s2 3p6 4s1
  • The 4s orbital is lower in energy than the 3d subshell and is therefore filled first
  • The nearest preceding noble gas to potassium is argon which accounts for 18 electrons so the shorthand electron configuration is:
    • [Ar] 4s1

Answer 2:

  • Calcium has 20 electrons so the full electronic configuration is:
    • 1s2 2s2 2p6 3s2 3p6 4s2
  • The 4s orbital is lower in energy than the 3d subshell and is therefore filled first
  • The nearest preceding noble gas to potassium is argon which accounts for 18 electrons so the shorthand electron configuration is:
    • [Ar] 4s2

Answer 3:

  • Gallium has 31 electrons so the full electronic configuration is:
    • 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1 
  • Again, the nearest preceding noble gas to potassium is argon which accounts for 18 electrons so the shorthand electron configuration is:
    • [Ar] 4s2 3d10 4p1

Answer 4:

  • If you ionise calcium and remove its two outer electrons, the electronic configuration of the Ca2+ ion is identical to that of argon.
  • So, the full electronic configuration is:
    • 1s2 2s2 2p6 3s2 3p6
  • Since this is the electronic configuration of an argon atom, the shorthand electron configuration of Ca2+ is: 
    • [Ar]

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Richard

Author: Richard

Expertise: Chemistry

Richard has taught Chemistry for over 15 years as well as working as a science tutor, examiner, content creator and author. He wasn’t the greatest at exams and only discovered how to revise in his final year at university. That knowledge made him want to help students learn how to revise, challenge them to think about what they actually know and hopefully succeed; so here he is, happily, at SME.