1.55 - 1.60 Electrolysis

1.55 Using electrolysis

Electrolysis is often used to give metal objects a decorative coating. This is known as electroplating.

Electrolysis happens when an electric current is passed through an ionic compound which has been melted or dissolved.

Electrolysis has a wide range of uses including : electroplating, extraction of aluminium, production of chlorine and the purification of copper . This post helps you to understand and explain the various changes that can happen in electrolysis.

Assumed background knowledge

https://www.goldhilleducation.co.uk/index.php/private-tuition/formulae-of-compounds

How metals conduct an electric current:

The delocalised electrons in the metallic lattice are free to move through the material when a voltage is applied.

1.55 - 1.57 Activity 1. Know your anions

Students should:

1.55C understand why covalent compounds do not conduct electricity
1.56C understand why ionic compounds conduct electricity only when molten or in aqueous solution
1.57C know that anion and cation are terms used to refer to negative and positive ions respectively

A liquid substance containing ions which are mobile can conduct an electric current. When this happens chemical changes take place at the electrodes. Electrons are given off at the negative electrode ( cathode) and electrons are taken away from the positive electrode ( anode).

The ions ( which are mobile because they are molten or dissolved) will migrate as the electric field is applied. The positive ions (Anions) will migrate to the negative electrode and the negative ions (Cations) migrate to the positive electrode.

chemical changes then take place at the electrodes and a current flows.

Covalently bonded compounds do not contain ions so that even when molten ( so that the molecules are free to move) , there is no migration of particles and no conduction.

1.58 Activity 2. Electrolysis of molten ionic compounds

Students should:

1.58C describe experiments to investigate electrolysis, using inert electrodes, of molten compounds including lead(II) bromide and aqueous solutions including sodium chloride, dilute sulfuric acid and copper(II) sulfate and to predict the products

Q1. At what point does the salt start conducting? Open or Close

The salt begins to conduct an electric current once it has all become molten.
Q2. What changes can you see taking place in the sodium chloride whilst it is conducting? Open or Close

It looks like the salt is reacting and producing some gases
Q3. Why does the lamp go out again? Open or Close

The molten salt is allowed to cool and so it solidifies and stops being able to conduct

Use the animation to the right to see the migration of ions in a molten compound

ions start vibrating

ions become mobile

ions migrate to opposite electrode

electrons are transferred at electrodes

1.59 Activity 3. Half equations

Students should:

1.59C write ionic half-equations representing the reactions at the electrodes during electrolysis and understand why these reactions are classified as oxidation or reduction

1.60C practical: investigate the electrolysis of aqueous solutions

Questions
Answers

What is the half equation for the reduction of sodium ions at the cathode?
Why is it called "reduction" ?
What is the product?
What is the half equation for the oxidation of chloride ions at the anode?
Why is it called "oxidation" ?
What is the product?

Enter your text here ...

1.58 Activity 4. A toxic separation

The electrolysis of molten lead bromide is a popular electrolysis reaction and is often shown in schools. However it is dangerous and needs to be performed in controlled conditions. Watch the this video carefully to find out why.