Study Notes
The reactivity series is a list of metals arranged in order of their reactivity, from most to least reactive. It helps predict how metals will react with water, acids, and other substances.
- 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 a compound. Example: Magnesium displaces copper from copper(II) sulfate.
- Oxidation — a reaction in which a substance gains oxygen or loses electrons. Example: Iron rusting when exposed to oxygen and water.
- Reduction — a reaction in which a substance loses oxygen or gains electrons. Example: Copper(II) oxide being reduced by zinc.
- Redox Reaction — a reaction where both oxidation and reduction occur simultaneously. Example: Zinc reducing copper(II) oxide while being oxidized itself.
Exam Tips
Key Definitions to Remember
- Reactivity Series
- Displacement Reaction
- Oxidation
- Reduction
- Redox Reaction
Common Confusions
- Confusing the order of metals in the reactivity series
- Misunderstanding the difference between oxidation and reduction
Typical Exam Questions
- What is a displacement reaction? A more reactive metal displaces a less reactive metal from its compound.
- How does the reactivity series predict reactions with acids? More reactive metals will react more vigorously with acids.
- What conditions are required for rusting? Presence of water and oxygen.
What Examiners Usually Test
- Ability to recall the order of the reactivity series
- Understanding of displacement reactions
- Identification of oxidation and reduction in reactions