Metals as Conductors (AQA GCSE Chemistry: Combined Science)

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How do metals conduct electricity?

  • Metals consist of giant structures
  • Within the metal lattice, the atoms lose their outer electrons and become positively charged metal ions
    • The outer electrons no longer belong to any specific metal atom and are said to be delocalised
  • Metals can conduct electricity because the delocalised electrons are able to move through the structure and carry a charge 
  • The metallic bond is the strong force of attraction between the positive metal ions and the delocalised electrons
  • This type of bonding occurs in metals and metal alloys, which are mixtures of metal

Diagram to show metallic bonding

Metallic bonding in a metal

There is attraction between positive metal ions and delocalised electron

Examiner Tip

When explaining why metals conduct electricity in an exam, be careful that you don't write electrons move 'throughout' the structure, but say 'through' the structure.

How do metals conduct heat?

  • Metals are also good conductors of heat
  • The delocalised electrons are free to move and transfer thermal energy through the structure
  • Some metals are better conductors of heat energy than others

Table of different conductivities of metals

Metal Thermal conductivity*
Silver 406
Copper 385
Gold 314
Brass 109
Aluminium 205
Iron 79.5
Steel 50.2
Lead  34.7

*W/mK = Watts per metre Kelvin is a unit of thermal conductivity

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Alexandra

Author: Alexandra

Expertise: Chemistry

Alex studied Biochemistry at Newcastle University before embarking upon a career in teaching. With nearly 10 years of teaching experience, Alex has had several roles including Chemistry/Science Teacher, Head of Science and Examiner for AQA and Edexcel. Alex’s passion for creating engaging content that enables students to succeed in exams drove her to pursue a career outside of the classroom at SME.