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Year 11 - Science

Ionic equations: reactions of Group 1 and Group 7

Groups of the periodic table

Unit Summary

This unit explores how elements' reactions are related to electron arrangement and atomic number. It covers the properties of Groups 1, 7, and 0 and explains how these depend on outer electrons. It also predicts element reactivity and reactions based on their positions in the periodic table.

Lesson Summary

You will learn to write balanced ionic equations and half equations for the reactions of Group 1 and 7 elements.

Key Notes

  • 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.

Vocabulary To Learn

  • 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 Mistakes To Avoid

  • 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.

3 Quick Questions (With Answers)

1. Explain the scientific idea in this lesson using two key points.

Reduction is the gain of electrons, and oxidation is the loss of electrons. Displacement reactions are often examples of redox reactions.

2. Define this scientific word and use it in context. 'oxidation'

A type of reaction in which a substance gains oxygen or loses electrons. Include the word in a full scientific explanation, not as a single label.

3. Correct this common scientific misunderstanding.

Mistake: 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. Correction: 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.

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