Study Notes
The reactivity of metals involves their ability to react with other substances, such as oxygen, water, and acids, forming new compounds. More reactive metals displace less reactive ones in compounds, a process known as displacement reactions.
- Chemical Reaction — a process where substances (reactants) change to form new substances (products). Example: Copper reacting with oxygen to form copper oxide.
- Oxidation — a reaction where oxygen is added to a substance. Example: Magnesium burning in air to form magnesium oxide.
- Reduction — a reaction where oxygen is removed from a substance. Example: Zinc oxide reacting with carbon to form zinc.
- Reactivity Series — a list of metals arranged in order of their reactivity. Example: Potassium is more reactive than copper.
- Displacement Reaction — a reaction where a more reactive metal displaces a less reactive metal from its compound. Example: Magnesium displacing copper from copper sulfate.
Exam Tips
Key Definitions to Remember
- Chemical Reaction: A process that changes reactants into products.
- Oxidation: Addition of oxygen to a substance.
- Reduction: Removal of oxygen from a substance.
- Displacement Reaction: A more reactive metal displaces a less reactive one from its compound.
Common Confusions
- Confusing oxidation with reduction.
- Misunderstanding the reactivity series order.
Typical Exam Questions
- What is a displacement reaction? A reaction where a more reactive metal displaces a less reactive metal from its compound.
- What happens when magnesium burns in air? It reacts with oxygen to form magnesium oxide.
- Write a word equation for zinc reacting with hydrochloric acid. Zinc + hydrochloric acid → zinc chloride + hydrogen
What Examiners Usually Test
- Understanding of oxidation and reduction.
- Ability to write and balance chemical equations.
- Knowledge of the reactivity series and its implications.