2.1.5

Electrolysis 2

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Electrolysis - Extracting Metals

Electrolysis is used to extract reactive metals from molten ores (melted materials containing metals). It is used to extract metals such as aluminium, which are more reactive than carbon.

Illustrative background for At the anode (positive electrode)Illustrative background for At the anode (positive electrode) ?? "content

At the anode (positive electrode)

  • Carbon dioxide is formed at the anode.
  • The anode is usually made of carbon because it is a good conductor and is cheap.
Illustrative background for At the cathode (negative electrode)Illustrative background for At the cathode (negative electrode) ?? "content

At the cathode (negative electrode)

  • The aluminium is formed at the cathode.
Illustrative background for DisadvantageIllustrative background for Disadvantage ?? "content

Disadvantage

  • Lots of energy is needed to:
    • Melt the solid ionic compound to allow the ions to flow.
    • To produce the electrical current.
  • All this energy costs money, and a lot of it!

Electrolysis of Aqueous Solutions

The products of the electrolysis of aqueous solutions are difficult to predict because the water molecules in the solution split up to form hydrogen (H+) and hydroxide (OH-) ions.

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At the anode (positive electrode)

  • What is formed at the anode depends on if halide ions are present:
    • If halide ions are present, the respective halogen forms.
    • If halide ions are absent, oxygen forms.
Illustrative background for At the cathode (negative electrode)Illustrative background for At the cathode (negative electrode) ?? "content

At the cathode (negative electrode)

  • What is formed at the cathode depends on the reactivity of the metal:
    • If the metal's more reactive than hydrogen, hydrogen is produced.
    • If the metal's less reactive than hydrogen, the metal is produced.

Half Equations

During electrolysis, different reactions take place at the different electrodes. Half equations show the reactions that happen at each electrode. The electrolysis of lead bromide is an example of this:

Illustrative background for At the anode (positive electrode)Illustrative background for At the anode (positive electrode) ?? "content

At the anode (positive electrode)

  • Oxidation reactions happen i.e. negatively charged ions lose electrons.
    • E.g. 2Br- → Br2 + 2e-
Illustrative background for At the cathode (negative electrode)Illustrative background for At the cathode (negative electrode) ?? "content

At the cathode (negative electrode)

  • Reduction reactions happen i.e. positively charged ions gain electrons.
    • E.g. Pb2+ + 2e- → Pb

Jump to other topics

1Biology

1.1Practicals

1.1.1Microscope & Bacteria

1.1.2Bacteria

1.1.3Osmosis Tests

1.1.4Osmosis & Food Tests

1.1.5Enzymes

1.1.6Enzymes 2

1.1.7Photosynthesis & Plant Responses

1.1.8Photosynthesis Experiments

1.1.9Reaction Time

1.1.10Quadrats

1.1.11Decay

2Chemistry

2.1Practicals

2.1.1Salts

2.1.2Neutralisation

2.1.3Titration

2.1.4Electrolysis

2.1.5Electrolysis 2

2.1.6Rate of Reaction

2.1.7Rate of Reaction 2

2.1.8Chromatography

2.1.9Identifying Gases

2.1.10Identifying Gases 2

2.1.11Identifying Ions

2.1.12Carbonates, Halides & Sulfates

2.1.13Flame Emission Spectroscopy

2.1.14Water Purification

2.1.15Water Purification 2

3Physics

3.1Practicals

3.1.1Specific Heat Capacity

3.1.2Thermal Capacity & Insulation

3.1.3Latent Heat

3.1.4Resistance & Current

3.1.5Resistance & Current 2

3.1.6Density

3.1.7Density 2

3.1.8Force & Extension - Springs

3.1.9Waves - Ripple Tank

3.1.10Light

3.1.11Light Reflection & Refraction

3.1.12Radiation

3.1.13Radiation 2

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Electrolysis

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