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Electrolysis 1
The substance broken down by electrolysis is called the electrolyte.

Electrolysis 1

Electrolysis is a process you need to be familiar with in GCSE Chemistry and this is the first of two quizzes on the subject. In electrolysis ionic compounds are broken down. It is essential for your exam that you know at least the basic definitions (electrolyte, electrode, anode, cathode, ionic compound, anion, cation) and can recognise diagrams showing electrolysis. You should be able to work out what is produced at each electrode from the starting material - you don't need to learn each and every electrolysis, knowing a few simple principles such as the reactivity series will help you work things out from 'scratch'.

Electrolysis is carried out by dipping two electrodes connected to a DC supply into a solution of an electrolyte or a molten electrolyte. One electrode is attached to the negative side of the power source and the other to the positive side.

In industry, electrolysis is used in many ways. One of the favourites of the examiners is the production of aluminium so learn the Hall-Heroult process well. Other examples of real life electrolysis are the production of sodium hydroxide and chlorine by the electrolysis of brine, and the refining of the metal copper. If you know the principles of electrolysis plus these examples, you should cope easily with any questions that you come across.

The key to understanding what is happening during electrolysis is to remember two basic facts - one is about electricity, the other is about chemical bonding. Firstly, keep in mind that electricity is a flow of electrons pumped round a circuit in one direction by a power supply (e.g. power pack, battery) and secondly, ionic bonding involves the loss and gain of electrons.

Opposite electrical charges attract one another so the positive ions in the electrolyte move towards the negative electrode and vice-versa. Positive ions are called cations and so the negative electrode is called the cathode because it attracts the cations. The positive electrode attracts the anions and is therefore called the anode. During electrolysis in solution, oxygen is usually produced at the anode as anions are very stable.

When a cation reaches the cathode, one or more electrons are transferred to the cation, cancelling out its positive charge. Most cations are metals so when they gain an electron, they become metal atoms and are deposited on the cathode. What happens then depends on the reactivity of the metal and whether the electrolysis is being carried out in solution or using a molten electrolyte.

If the electrolysis is being carried out in solution, hydrogen will be produced if the metal in solution is higher in the reactivity series e.g. sodium, potassium. Less reactive metals will form a deposit on the cathode and, as the thickness of the deposit increases, some of the deposit will flake off and be seen on the bottom of the electrolysis vessel. In a molten solution, where water is not present, the metal atoms are always produced - this is how reactive metals like sodium and potassium are extracted from their ores.

Have a go at this quiz and see how well you understand the electrolysis of ionic compounds

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Pick the correct combination for the names of the positive and negative electrodes.
+ve anode -ve negode
+ve cathode -ve anode
+ve posode -ve cathode
+ve anode -ve cathode
Electrodes get their names from the type of ion they attract
What do we call the substance broken down by electrolysis?
This word is reasonably easy to remember being so close to electrolysis. An electrolyte must separate into positive and negative ions when it is molten or dissolved in water
When lead bromide is electrolysed...
Pb 2+ is reduced at the cathode, Br- is oxidised at the anode
Pb2+ is oxidised at the cathode, Br- is reduced at the anode
Pb2+ is reduced at the anode, Br- is oxidised at the cathode
Pb3+ is reduced at the cathode, Br- is oxidised at the anode
Reduction is a gain of electrons and oxidation is a loss of electrons. Metals are produced from their ores by reduction of their ions
When a negatively charged ion reaches the positively charged electrode...
It can lose an electron to become a neutral atom
It can lose an electron to become a positive ion
It gains an electron to become a neutral atom
It gains an electron to become a negative ion
Many anions (e.g sulfate - SO42-) are too stable to lose their electron and in those cases oxygen is released from the small quantity of hydroxide ions that are always present in water. Substances containing the stable anions are therefore only electrolytes when in solution
Why does an electrolyte need to be either molten or in solution?
To ensure the atoms can move
To enable the ions to move
So that water ions can be involved in the reaction
So that the electrodes can be put in the electrolyte
If the electrolyte is solid, the ions are unable to move and so electricity cannot flow. You should have discarded the first option the second you read the word 'atoms' - atoms have no overall charge and therfore are unaffected by electrolysis
Pick the correct combination to show what is collected at each electrode when molten copper bromide is electrolysed.
Copper ions at the cathode, Bromine gas at the anode
Copper metal at the anode, Bromide ions at the cathode
Copper metal at the cathode, Bromine gas at the anode
Copper metal at the anode, Bromine gas at the cathode
Bromine has a red-brown colour and its molecules are diatomic (contain 2 atoms bonded covalently so its formula is Br2)
During electrolysis...
+ve ions move to cathode and -ve ions move to anode
+ve ions move to anode and -ve ions move to cathode
+ve ions and -ve ions move to cathode
+ve ions and -ve ions move to anode
Remember: opposite charges attract
Pick the correct half equations to show what happens when PbBr2 is electrolysed.
Cathode: Pb+ + e- → Pb
Anode: 2Br- → Br2 + 2e-
Anode: Pb2+ + 2e- → Pb
Cathode: 2Br- → Br2 + 2e-
Cathode: Pb2+ + 2e- → Pb
Anode: Br- → Br  + 2e-
Cathode: Pb2+ +2e- → Pb
Anode: 2Br- → Br2 + 2e-
This is only going to come up in the higher tier of the exam
Pick the correct half equations to show what happens when an aqueous solution of KCL is electrolysed.
Cathode: K+ + e- → K
Anode: 2Cl- → Cl2 +2e-
Cathode: 2H+ + 2e- → H2
Anode: 2Cl- → Cl2 + 2e-
Cathode: H+ + e- → H
Anode: 2Cl- → Cl2 +2e-
Cathode: K+ + e- → K
Anode: Cl- → Cl + e-
Hydrogen gas is produced because it is less reactive than potassium
Electrolysis means which of the following?
Splitting up substances using heat
Splitting up substances using electrons
Splitting up substances using electricity
Joining up substances using electricity
It is a chemical decomposition
Author:  Kate Gardiner

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