Ionic equations: reactions of Group 1 and Group 7
I can write balanced ionic equations and half equations for the reactions of Group 1 and 7 elements.
Ionic equations: reactions of Group 1 and Group 7
I can write balanced ionic equations and half equations for the reactions of Group 1 and 7 elements.
These resources will be removed by end of Summer Term 2025.
Lesson details
Key learning points
- Reduction is the gain of electrons, and oxidation is the loss of electrons.
- Displacement reactions are often examples of redox reactions.
- Half equations show which elements are oxidised, and which are reduced.
Keywords
Oxidation - A type of reaction in which a substance gains oxygen or loses electrons.
Half equation - A chemical equation used to show the electrons lost in oxidation or the electrons gained in reduction.
Reduction - A type of reaction in which a substance loses oxygen or gains electrons.
Redox - A redox reaction is one in which a substance is oxidised and another is reduced.
Ionic equation - A chemical equation in which reacting ions are shown; unreacting ions (spectator ions) are not included.
Common misconception
Pupils can confuse oxidation and reduction when involving electrons. They often mistake a positive charge on an ion as meaning electrons have been added and vice versa for negative ions.
It is very important to teach from first principles what causes the charges and then work up to half equations where the pupils can see the electrons in the equations, finally combining these to form ionic equations.
Equipment
None required.
Licence
This content is © Oak National Academy Limited (2024), licensed on Open Government Licence version 3.0 except where otherwise stated. See Oak's terms & conditions (Collection 2).
Lesson video
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Starter quiz
6 Questions
when an element replaces a less reactive element in a compound
name of the salts formed from halogens
non-metallic elements in Group 7 that react with metals to form salt
ionic compounds made of positive and negative ions