Study Notes
The Reactivity Series is a list of metals arranged in order of their reactivity, from most to least reactive. Metals react differently with water, acids, and oxygen, which helps determine their position in the series.
- Reactivity Series — a list of metals ordered by their reactivity. Example: Potassium is more reactive than iron.
- Displacement Reaction — a reaction where a more reactive metal displaces a less reactive metal from a compound. Example: Magnesium displacing copper from copper sulfate.
- Oxide Layer — a protective layer formed on metals like aluminum, preventing further reaction. Example: Aluminum oxide layer prevents aluminum from reacting with air.
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 some metals do not react with acids
Typical Exam Questions
- What happens when magnesium is placed in copper(II) sulfate solution? Magnesium displaces copper, forming magnesium sulfate and copper.
- Why does aluminum appear unreactive? It forms a protective oxide layer that prevents further reaction.
- Which metals react with cold water? Potassium, sodium, and calcium react with cold water.
What Examiners Usually Test
- Ability to deduce the order of reactivity from experimental results
- Understanding of displacement reactions
- Explanation of the apparent unreactivity of aluminum