Electrolysis and Ionic Compounds

Front

Ionic compounds conduct electricity only when molten or in aqueous solution.

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Ions are able to move and carry charge when molten or in solution.

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Halide ions include Cl^-, Br^-, and I^-.

Back

These ions can lead to halogen production at the anode.

Front

Electrolysis of molten compounds uses inert electrodes.

Back

This process can include compounds like lead(II) bromide.

Front

Aqueous solutions in electrolysis can include sodium chloride.

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Other examples are dilute sulphuric acid and copper(II) sulphate.

Front

Electrolysis can predict the products formed at the electrodes.

Back

This depends on the ions present and their reactivity.

Front

Electrolysis of water acidified with sulphuric acid: H⁺ ions

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H⁺ ions go to the cathode, producing H₂ (g) as these are the other ions present in H₂SO₄.

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Oxidation definition

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Oxidation is the loss of electrons.

Front

Negative electrode half equation

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X⁺ + e⁻ → X, where electrons are gained and positive ions are reduced.

Front

Positive electrode half equation

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X⁻ → e⁻ + X, where electrons are lost and negative ions are oxidised.

Front

Example of electrolysis: Copper sulphate solution using copper electrodes

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Example of electrolysis using copper sulphate solution and copper electrodes.