Summary
The extraction of metals from their ores involves using chemical reactions to obtain the metal. Metals less reactive than carbon can be extracted by heating with carbon, while more reactive metals require electrolysis.
- Metallic Bonding — a lattice of positive ions in a sea of delocalised electrons Example: Explains why metals are malleable and good conductors of electricity.
- Alloys — mixtures of a metal with other elements Example: Brass is an alloy of copper and zinc.
- Reactivity Series — a list of metals arranged in order of decreasing reactivity Example: Potassium is more reactive than iron.
- Blast Furnace — a method to extract iron from its ore using carbon Example: Iron is extracted from hematite using a blast furnace.
- Electrolysis — a process to extract metals more reactive than carbon Example: Aluminum is extracted from bauxite using electrolysis.
Exam Tips
Key Definitions to Remember
- Metallic Bonding
- Alloys
- Reactivity Series
- Blast Furnace
- Electrolysis
Common Confusions
- Confusing alloys with compounds
- Misunderstanding the reactivity series order
Typical Exam Questions
- What is the role of carbon in the extraction of iron? Carbon reduces iron oxide to iron.
- How is aluminum extracted from its ore? By electrolysis of aluminum oxide dissolved in molten cryolite.
- Why are alloys harder than pure metals? Different sized atoms in alloys prevent layers from sliding easily.
What Examiners Usually Test
- Understanding of the reactivity series
- Differences between extraction methods for different metals
- The role of carbon in metal extraction