Summary
Electrolysis is the process of breaking down ionic compounds using electricity, where ions move to electrodes and undergo reactions.
- Inert Electrode — A metal that transfers electrons without exchanging ions with the solution. Example: Platinum
- Electrolyte — A substance that conducts electricity when dissolved in water. Example: Sodium chloride solution
- Anode — The positive electrode where oxidation occurs. Example: Chlorine gas is produced at the anode during electrolysis of sodium chloride.
- Cathode — The negative electrode where reduction occurs. Example: Hydrogen gas is produced at the cathode during electrolysis of water.
Exam Tips
Key Definitions to Remember
- Electrolysis: The breakdown of ionic compounds using electricity.
- Anode: Positive electrode where oxidation occurs.
- Cathode: Negative electrode where reduction occurs.
Common Confusions
- Confusing the anode and cathode; remember PANIC: Positive Anode, Negative Is Cathode.
- Misunderstanding the role of inert electrodes; they prevent side reactions.
Typical Exam Questions
- What is the positive electrode called? Anode
- What happens when molten NaCl is electrolyzed? Chlorine is produced at the positive electrode
- Which ions move to the cathode during electrolysis? Cations
What Examiners Usually Test
- Understanding of the movement and reactions of ions at electrodes.
- Ability to predict products of electrolysis based on reactivity.
- Knowledge of the role of inert electrodes in preventing side reactions.