Redox reactions
Chemistry · Unit 3 — Equilibrium, acids and redox reactions · Oxidation and reduction
Learning objectives (33)
LO-1Analyse data to determine the relative amounts of product produced at each electrode in electrolysis. The following subject matter may be assessed in the internal assessments.LO-2Analyse data, including displacement reactions of metals, combustion, corrosion and electrochemical processes to determine redox reactions. Electrochemical cellsLO-3Analyse data, including standard electrode potentials, to make predictions about the spontaneity of a reaction and to compare electrochemical cells. Chem istry 2025 v1.3 Electrolytic cellsLO-4Apply half-equations and oxidation numbers to balance redox equations (acid conditions only) and to discriminate between the species oxidised and reduced, and the oxidising agent and reducing agent.LO-5Apply oxidation numbers (represented as roman numerals) to name transition metal compounds. Chem istry 2025 v1.3LO-6Apply standard electrode potentials to determine the relative strength of oxidising and reducing agents.LO-7Calculate cell potential, 𝐸cell o (Formula: 𝐸cell o = 𝐸reduction half−cell o − 𝐸oxidation half−cell o)LO-8Calculate moles of electrons, current, time, mass of substance or volume of gas produced or used during electrolysis. (Formula: q = 𝑛(e−) × F or q = I × t).LO-9Describe that electrolytic cells can be used in small-scale and industrial situations, including metal plating and the purification of copper.LO-10Describe the standard hydrogen electrode.LO-11Determine the oxidation state (represented with the sign given before the number) of an atom in an ion or compound, e.g. +2.LO-12Determine the products of the electrolysis of a molten salt.LO-13Determine the species oxidised and reduced, and the oxidising agent and reducing agent, in redox reactions.LO-14Discriminate between a galvanic and an electrolytic cell. Galvanic cellsLO-15displacement reactionsLO-16electroplating using an electrolytic cell.LO-17Explain that electrochemical cells, including galvanic and electrolytic cells, consist of oxidation and reduction half-reactions connected via an external circuit that allows electrons to move from the anode (oxidation reaction) to the cathode (reduction reaction).LO-18Explain that galvanic cells can be represented as cell diagrams, including anode and cathode half-equations.LO-19Explain 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).LO-20Explain that oxidation occurs at the negative electrode (anode) and reduction occurs at the positive electrode (cathode).LO-21Explain that two half-cells can be connected by a salt bridge to create a galvanic cell, e.g. Mg, Zn, Fe and Cu and solutions of their ions.LO-22Explain the products of the electrolysis of aqueous solutions, e.g. dilute and concentration sodium chloride(aq) and copper sulfate(aq).LO-23Explain the term standard electrode (reduction) potential, 𝐸o.LO-24factors that affect electrolysisLO-25galvanic cellsLO-26Identify 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.LO-27Identify that electrolytic cells use an external electrical potential difference to pr ovide the energy to allow a non-spontaneous redox reaction to occur.LO-28Identify that galvanic cells generate an electrical potential difference from a s pontaneous redox reaction.LO-29Identify the essential components of a galvanic cell, including the oxidation and reduction half- cells, the positive and negative electrodes and their solutions of their ions, the flow of electrons and the movement of ions, and the salt bridge.LO-30Identify the essential components of an electrolytic cell, including source of electric current and conductors, positive and negative electrodes, and the electrolyte.LO-31Identify the limitations associated with standard electrode (reduction) potentials, 𝐸o.LO-32Sketch a galvanic cell and label the essential components. Standard electrode potentialLO-33State the factors that affect the products in electrolysis.
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