Ionisation energy

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8 Terms

1
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First ionisation energy

Energy required to remove 1 mole of electrons from 1 mole of a gaseous atom, to form 1 mole of gaseous 1+ ions. (Measured in kj/mol)

2
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Second ionisation energy

Energy required to remove 1 mole of electrons from 1 mole of gaseous 1+ ions to ore 1 mole of gaseous 2+ ions

3
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Factors affecting ionisation energy

  1. Nuclear charge (number of protons)

  2. Distance from nucleus to outer electrons

  3. Electron shielding


4
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Ionisation energy across a period exceptions (Group 5 and 6 dip)

  1. Sulfur has lower first ionisation energy

  2. Because its paired electrons together in 3p orbital, whereas Phosphorus has unpaired electrons in each 3p orbital

  3. So paired electrons in sulfur cause electron-electron repulsion

  4. The repulsion makes it easier to remove an electron

  5. While shielding remains similar

  6. So less energy required to remove an electron


5
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Ionisation energy across a period

Increases, because atoms have more nuclear charge, so there is more attraction between the outer electrons and positive protons, so atomic radius decreases, with similar amount of shielding. So more energy is required to remove an electron,

6
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Ionisation energy across a period exceptions (Group 2 and 3 dip)

  1. Aluminium has lower first ionisation energy than magnesium

  2. Because aluminiums outer electron is in 3p1 orbital

  3. Since 3p1 orbital is higher in energy, it’s then slightly further away from nucleus than magnesium’s 3s orbital.

  4. So aluminium 3p1 electron experiences more shielding from 3s electrons

  5. So less attraction between nucleus and outer electron

  6. So less energy is required to remove that electron.


7
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Ionisation energy down a group

  1. Decreases

  2. Because atomic radius increases, so outer electrons are further away from nucleus

  3. The number of shells also increases, so more shielding

  4. So less electrostatic attraction between nucleus and outer electrons

  5. So less energy required to remove an electron


8
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Successive ionisation energy

Continuously removing electrons from an atom