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Summary Unit 1 Topic 3 - Electronic Configuration
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Study notes for Unit 1 Topic 3 - Electronic Configuration for Chemistry Edexcel A Level 2015. Focusing on Electronic configuration, electron shells and subshells, the different types of orbitals, energy levels and spd notation.

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  • December 1, 2022
  • December 1, 2022
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Chemistry Notes Topic 1.3 - Electron Configuration


Electron shells:
● Electron shells are made up of subshells and orbitals.
● Electrons move around the nucleus in quantum shells, and these are all given
numbers known as principal quantum numbers.
● These shells contain different types of subshell.
● These subshells have different numbers of orbitals which can each hold up to 2
electrons.

Subshells:
● S = 1 orbital = maximum 2 electrons
● P = 3 orbitals = maximum 6 electrons
● D = 5 orbitals = maximum 10 electrons
● F = 7 orbitals = maximum 14 electrons

First 4 quantum shells:
Shell Subshells Total electrons

1st 1s 2

2nd 2s 2p 2 + (3 x 2) = 8

3rd 3s 3p 3d 2 + (3 x 2) + (5 x 2) = 18

4th 4s 4p 4d 4f 2 + (3 x 2) + (5 x 2) + (7 x 2) = 32


Orbitals:
● An orbital is an area of space that an electron moves in.
● Orbitals in the same subshell have the same energy.
● The electrons in each orbital spin in opposite directions - spin-pairing.
● S-orbitals are spherical.
● P-orbitals are dumbbell shaped,
there are 3 at right angles to each
other.




● Orbitals are represented by arrows in boxes.
● Each box = one orbital. Each arrow = one electron.
● The arrows represent the electrons spinning in
opposite directions.

Energy levels of subshells:
● The 4s subshell has a lower energy level than the 3d
subshell even though its principal quantum number is
bigger.
● It is the same for the 5s and 4p shells, etc,

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