Study Notes
The activity series of metals ranks metals by their reactivity with water, acids, and other substances. More reactive metals can displace less reactive metals from compounds.
- Reactivity Series — a list of metals arranged by 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(II) sulfate.
- Oxide Layer — a protective layer that forms on metals like aluminum, preventing further reaction. Example: Aluminum forms Al2O3, making it appear unreactive.
Exam Tips
Key Definitions to Remember
- Reactivity Series
- Displacement Reaction
- Oxide Layer
Common Confusions
- Confusing the order of metals in the reactivity series
- Misunderstanding why aluminum appears unreactive
Typical Exam Questions
- What is a displacement reaction? A more reactive metal displaces a less reactive metal from its compound.
- Why does aluminum appear unreactive? It forms a protective oxide layer that prevents further reaction.
- How can you determine the reactivity of a metal? By observing its reactions with water, acids, and other substances.
What Examiners Usually Test
- Ability to place metals in the correct order of reactivity
- Understanding of displacement reactions and their outcomes
- Explanation of the apparent unreactivity of aluminum