Summary
The topic covers how metals are extracted and used, focusing on their reactivity and the processes involved in their extraction and recycling.
- 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 displacing copper from copper sulfate.
- Redox Reaction — a chemical reaction involving the transfer of electrons. Example: Zinc reducing copper(II) oxide.
- Oxidation — the gain of oxygen or loss of electrons. Example: Iron rusting.
- Reduction — the loss of oxygen or gain of electrons. Example: Copper ions gaining electrons to form copper metal.
- Galvanising — coating a metal with a more reactive metal to prevent rusting. Example: Iron coated with zinc.
- Phytoextraction — using plants to absorb metal compounds from the soil. Example: Plants absorbing metal compounds into their shoots.
- Dynamic Equilibrium — a state where the rate of the forward reaction equals the rate of the backward reaction. Example: The Haber process for ammonia production.
Exam Tips
Key Definitions to Remember
- Reactivity Series
- Displacement Reaction
- Redox Reaction
- Oxidation
- Reduction
Common Confusions
- Confusing oxidation with reduction
- Misunderstanding the reactivity series order
Typical Exam Questions
- What is the removal of oxygen from a substance called? Reduction
- Which series is used to predict the reactions of metals with carbon and other elements? Reactivity series
- How could you extract sodium from molten sodium chloride? Electrolysis
What Examiners Usually Test
- Understanding of the reactivity series
- Ability to identify redox reactions
- Knowledge of metal extraction methods