Ionisation Energies | A Level Chemistry | OCR, AQA, Edexcel
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This week we are revising Ionisation Energies
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Ionisation is the process by which an electron is removed from an atom or a molecule. The process is endothermic, because energy is required to break the force of attraction between the electron and the central positive nucleus.
The first ionisation energy is the energy needed to remove 1 electron from each atom of an element in 1 mole of gaseous atoms, to form 1 mole of gaseous ions with a +1 charge.
The second ionisation energy is the energy needed to remove 1 electron from each ion of an element in 1 mole of gaseous +1 ions to form 1 mole of gaseous ions with a +2 charge.
The successive ionisation energy is the energy each time you remove an electron. When talking about successive ionisation energies, we often draw a graph for a particular element of the first ionisation energy, second ionisation energy, third ionisation energy, and so on.
Gas state symbol (g) is used because gaseous atoms are used when ionisation energies are recorded.
A period in a periodic table is a horizontal row. All the elements in a period have the same number of electron shells.
A group in a periodic table is a vertical column. All the elements in a group have the same number of outermost electrons.
The shielding effect is the effect of inner electrons which reduces the pull of the nucleus on the electrons in the outer shell.
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