MODULE
6
Redox reactions
Introduction
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Redox reactions or reduction-oxidation reactions involve the transfer of electrons, and therefore their movement, from one chemical species to another. The movement of electrons can be used to generate an electrical current, making redox reactions one of the most important types of chemical reaction. Redox reactions convert chemical potential energy into electrical energy, so are used to generate a major source of energy in the world. Redox reactions can also be highly destructive. Some are responsible for killing bacteria and make excellent household cleaners. They can also sterilise unsanitary environments or hospitals and destroy certain metal structures and biomolecules. For example, the rusting of metals (especially cars) and the browning (or oxidation) of fruit are the result of redox reactions.
Prior knowledge
Check your understanding of concepts related to redox reactions before you start.
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Prior knowledge quiz
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Subject matter
Science understanding → Identify that displacement reactions of metals, combustion, corrosion and electrochemical processes, can be modelled as redox reactions involving oxidation of one substance and reduction of another substance. → Determine the species oxidised and reduced, and the oxidising agent and reducing agent, in redox reactions. → Explain that oxidation can be modelled as the loss of electrons from a chemical species, and reduction can be modelled as the gain of electrons by a chemical species; these processes can be represented using balanced half-equations and redox equations (acidic conditions only). → Determine the oxidation state (represented with the sign given before the number) of an atom in an ion or compound, e.g. +2.
200 CHEMISTRY FOR QUEENSLAND UNITS 3 & 4
06_BLO_CHE_QCE_U34_SB_44269_1PP.indd 200
OXFORD UNIVERSITY PRESS
14-Jun-25 14:22:55