(40) GCSE Chemistry Revision "Extraction of Metals"

Introduction

• Overview: Metal extraction using carbon

• Learning objectives:

  • Describe how certain metals can be extracted using carbon.

  • Identify oxidized or reduced substances in relation to oxygen gain or loss.

Extraction of Metals

Unreactive Metals

• Example: Gold

  • Gold is found in the Earth as a metal.

  • Gold is unreactive, allowing the presence of gold nuggets.

Reactive Metals

• Examples: Iron Oxide and Copper Oxide

  • These metals form compounds with oxygen in the Earth’s crust.

  • They need extraction methods to separate the metals from these compounds.

Reactivity Series

• Key Fact:

  • A more reactive metal can displace a less reactive metal from its compound.

• Illustration of the Reactivity Series:

  • Lists metals from most reactive to least reactive (e.g., magnesium is above iron).

Displacement Reaction Example

• Magnesium reacting with Iron Oxide:

  • Reaction: Magnesium reacts with iron oxide to produce magnesium oxide and iron.

  • Reduction: Iron is reduced (loses oxygen).

  • Oxidation: Magnesium is oxidized (gains oxygen).

Role of Carbon in Metal Extraction

• Carbon is used for extraction due to its low cost.

• Carbon and Iron Oxide Reaction:

  • Reaction: Carbon + Iron Oxide → Carbon Dioxide + Iron.

  • Oxidation and Reduction:

    • Iron is reduced (loses oxygen).

    • Carbon is oxidized (gains oxygen).

Blast Furnace

• Iron is extracted in a blast furnace.

• Note: Reactions in the blast furnace are more complex than shown.

Displacement Reactions

• Examples of Reactions:

  • Identify one impossible reaction using the reactivity series.

• Reaction Analysis:

  • First Reaction:

    • Magnesium (loses oxygen) = Reduced

    • Lithium (gains oxygen) = Oxidized

  • Third Reaction:

    • Copper (loses oxygen) = Reduced

    • Carbon (gains oxygen) = Oxidized

Conclusion

• Learning recap: Ability to describe metal extraction with carbon and identify oxidation/reduction processes.