Rusting of Iron (Edexcel IGCSE Chemistry: Double Science)

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Rusting of iron

  • Rusting is the name given specifically to the corrosion of iron in the presence of water and oxygen from the air:

iron + water + oxygen  hydrated iron(III)oxide

  • Rust is a soft solid substance that flakes off the surface of iron easily, exposing fresh iron below which then undergoes rusting
  • This means that over time all of the iron rusts and its structure becomes weakened
  • Oxygen and water must be present for rust to occur
  • You can investigate the conditions needed for rusting by setting up a series of control test tubes as shown below
  • Boiled water removes any dissolved oxygen and calcium chloride is a drying agent 

Investigating rusting

Investigating the conditions for rusting

Diagram showing how the conditions for rusting can be investigated

  • The nail on the left rusts
    • It is in contact with both air (which contains oxygen) and water
  • The nail in the middle does not rust
    • It is not in contact with air because the oil provides a barrier to prevent oxygen diffusing into the boiled water
  • The nail on the right does not rust
    • It is not in contact with water because calcium chloride absorbs any water molecules present due to moisture
  • The results show that both air and water must be present for rusting to occur

Rust prevention

Barrier Methods

  • Rust can be prevented by coating iron with barriers that prevent the iron from coming into contact with water and oxygen
  • However, if the coatings are washed away or scratched, the iron is once again exposed to water and oxygen and will rust
  • Unlike some other metals, once iron begins to rust it will continue to corrode internally as rust is porous and allows both air and water to come into contact with fresh metal underneath any barrier surfaces that have been broken or scratched
  • Common barrier methods include: paint, oil, grease, and electroplating

Sacrificial Protection

  • Iron can be prevented from rusting using the reactivity series
  • A more reactive metal can be attached to a less reactive metal
  • The more reactive metal will oxidise and therefore corrode first, protecting the less reactive metal from corrosion
  • Zinc is more reactive than iron therefore will lose its electrons more easily than iron and is oxidised more easily
  • For continued protection, the zinc bars have to be replaced before they completely corrode

Zinc bars on the side of steel ships

VleRzCAu_9-2-4-sacrificial-protection

Diagram to show the use of zinc bars on the sides of steel ships as a method of sacrificial protection

Galvanising

  • Galvanising is a process where the iron to be protected is coated with a layer of zinc
  • This can be done by electroplating or dipping it into molten zinc
  • ZnCO3 is formed when zinc reacts with oxygen and carbon dioxide in the air and protects the iron by the barrier method
  • If the coating is damaged or scratched, the iron is still protected from rusting by sacrificial protection

Examiner Tip

Corrosion and rusting are not the same process. Corrosion is the general term used to describe the degradation of metal surfaces whereas rusting is the specific type of corrosion that happens to iron.

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Stewart

Author: Stewart

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Exam Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.