Properties of Metallic Substances (AQA AS Chemistry) : Revision Note

Stewart Hird

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Metallic Lattice Structures

  • Metals form giant metallic lattices in which the metal ions are surrounded by a ‘sea’ of delocalised electrons

  • The metal ions are often packed in hexagonal layers or in a cubic arrangement

  • This layered structure with the delocalised electrons gives a metal its key properties

States of Matter Metallic Lattice, downloadable AS & A Level Chemistry revision notes

Layers of copper ions (the delocalised electrons are not shown in the diagram)

  • If other atoms are added to the metal structure, such as carbon atoms, this creates an alloy

  • Alloys are much stronger than pure metals, because the other atoms stop the layers of metal ions sliding over each other easily

  • The strength of the metallic attraction can be increased by:

    • Increasing the number of delocalised electrons per metal atom

    • Increasing the positive charges on the metal centres in the lattice

    • Decreasing the size of the metal ions

  • Due to the delocalised ‘sea’ of electrons, metallic structures have some characteristic properties:

Malleability

  • Metallic compounds are malleable

  • When a force is applied, the metal layers can slide

  • The attractive forces between the metal ions and electrons act in all directions

  • So when the layers slide, the metallic bonds are re-formed

  • The lattice is not broken and has changed shape

How metals are malleable diagram

This diagram shows how the layers of positive metal ions slide over each other when a force is applied

Atoms are arranged in layers so the layers can slide when force is applied

Strength

  • Metallic compounds are strong and hard

    • Due to the strong attractive forces between the metal ions and delocalised electrons

Electrical conductivity

  • Metals can conduct electricity when in the solid or liquid state

    • In the solid and liquid states, there are mobile electrons which can freely move around and conduct electricity

  • When a potential difference is applied to a metallic lattice, the delocalised electrons repel away from the negative terminal and move towards the positive terminal

    • As the number of outer electrons increases across a period, the number of delocalised charges also increases:

      • Sodium = 1 outer electron

      • Magnesium = 2 outer electrons

      • Aluminium = 3 outer electrons

    • Therefore, the ability to conduct electricity also increases across a period

How metals conduct electricity diagram

Diagram showing how the delocalised electrons in a metal move towards the positive termninal when a potential difference is applied

The delocalised electrons move towards the positive terminal when a potential difference is applied

  • Since the bonding in metals is non-directional, it does not really matter how the cations are oriented relative to each other

Thermal conductivity

  • Metals are good thermal conductors due to the behaviour of their cations and their delocalised electrons

    • When metals are heated, the cations in the metal lattice vibrate more vigorously as their thermal energy increases

      • These vibrating cations transfer their kinetic energy as they collide with neighbouring cations, effectively conducting heat

    • The delocalised electrons are not bound to any specific atom within the metal lattice and are free to move throughout the material

      • When the cations vibrate, they transfer kinetic energy to the electrons

      • The delocalised electrons then carry this increased kinetic energy and transfer it rapidly throughout the metal, contributing to its high thermal conductivity.

Melting and boiling point

  • Metals have high melting and boiling points

    • This is due to the strong electrostatic forces of attraction between the cations and delocalised electrons in the metallic lattice

    • These require large amounts of energy to overcome 

    • As the number of mobile charges increases across a period, the melting and boiling points increase due to stronger electrostatic forces 

Examiner Tips and Tricks

You should be able to draw the structure of a metal with positive ions in layers and the delocalised electrons surrounding the ions

If drawing the structure of a metal in the exam, make sure to include labels for metal ions and delocalized electrons

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Stewart Hird

Author: Stewart Hird

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 Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.

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