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Microscale chemistry: redox reactions

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Carry out two redox reactions and observe and interpret the results

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Introduction guide
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Level

16-18 years

Use

Category

Redox chemistry

Specification

Scotland
- National 5
  - SQA Chemistry
    - Chemistry in society
      - Metals
        Redox
        Reduction is a gain of electrons by a reactant in any reaction.
        Oxidation is a loss of electrons by a reactant in any reaction.
        In a redox reaction, reduction and oxidation take place at the same time.
        Reactions of metals
        Metals can be arranged in order of reactivity by comparing the rates at which they react.
- Higher
  - SQA Chemistry
    - 1. Chemical changes and structure
      - (c) Oxidising and reducing agents
        In a redox reaction, reduction and oxidation take place at the same time.
        An oxidising agent is a substance that accepts electrons.
        A reducing agent is a substance that donates electrons.
        Oxidising and reducing agents can be identified in redox reactions.
Northern Ireland
- A/AS level
  - CCEA Chemistry
    - Unit AS 1: Basic Concepts in Physical and Inorganic Chemistry
      - 1.7 Redox
        1.7.6 6 use Roman numerals to indicate the oxidation number when an element has compounds or ions with different oxidation numbers, for example chlorate(I) and chlorate(V);
Republic of Ireland
- Leaving Certificate
  - Chemistry
    - 1. Periodic table and atomic structure
      - 1.1 Periodic table
        Depth of treatment
        Brief statement of the principal resemblances of elements within each main group, in particular alkali metals, alkaline earth metals, halogens and noble gases.
      - 1.4 Electronic Structure of Atoms
        Depth of treatment
        Explanations in terms of atomic radius, screening effect and nuclear charge for general trends in proprties of elements in groups I and VII.
        Activities
        Mandatory experiment 1.2 - Redox reactions of group VII elements - halogens as oxidising agents (reactions with bromides, iodides, Fe²⁺ and sulfites). Displacement reactions of metals (Zn with Cu²⁺, Mg with Cu²⁺).

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