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4. Electrochemistry

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  1. 4.1 Electrolysis

    1. 4.1.1Electrolysis as the decomposition of

      • Define electrolysis as the decomposition of an ionic compound, when molten or in aqueous solution, by the passage of an electric current

    2. 4.1.2In simple electrolytic cells: (a) the

      • Identify in simple electrolytic cells: (a) the anode as the positive electrode (b) the cathode as the negative electrode (c) the electrolyte as the molten or aqueous substance that undergoes electrolysis

    3. 4.1.8Transfer of charge during electrolysis

      • Describe transfer of charge during electrolysis to include: (a) the movement of electrons in the external circuit (b) the loss or gain of electrons at the electrodes (c) the movement of ions in the electrolyte

    4. 4.1.3Products and observations during

      • Identify products and observations during electrolysis of: (a) molten lead(II) bromide (b) concentrated aqueous sodium chloride (c) dilute sulfuric acid with inert platinum/carbon electrodes

    5. 4.1.4Metals or hydrogen are formed at the

      • State: metals or hydrogen are formed at the cathode and that non-metals (other than hydrogen) are formed at the anode

    6. 4.1.5Predict the identity of the products

      • Predict the identity of the products at each electrode for the electrolysis of a binary compound in the molten state

    7. 4.1.6Metal objects are electroplated to

      • State: metal objects are electroplated to improve their appearance and resistance to corrosion

    8. 4.1.7Metals are electroplated

      • Describe how metals are electroplated

    9. 4.1.9Products formed at the electrodes and

      • Identify the products formed at the electrodes and describe the observations made during the electrolysis of aqueous copper(II) sulfate using inert carbon/graphite electrodes and when using copper electrodes

    10. 4.1.10Predict the identity of the products

      • Predict the identity of the products at each electrode for the electrolysis of a halide compound in dilute or concentrated aqueous solution

    11. 4.1.11Construct ionic half-equations for

      • Construct ionic half-equations for reactions at the anode (to show oxidation) and at the cathode (to show reduction)

  2. 4.2 Hydrogen–oxygen fuel cells

    1. 4.2.1Hydrogen–oxygen fuel cell uses

      • State: a hydrogen–oxygen fuel cell uses hydrogen and oxygen to produce electricity with water as the only chemical product

    2. 4.2.2Advantages and disadvantages of using

      • Describe advantages and disadvantages of using hydrogen–oxygen fuel cells in comparison with gasoline/petrol engines in vehicles