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1.3Unit 2 · Bonding & Electrolysis

Metallic bonding — Edexcel IGCSE Chemistry Modular - UNIT 2 Revision Notes & Topical Questions

5 min read 5 parts Lesson 3 of 4 1 quiz

📚 Edexcel IGCSE Chemistry Modular - UNIT 2 Hub / Topical Revision
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Lesson summary

Metallic bonding — Edexcel IGCSE Chemistry: describe the giant metallic lattice and use its structure to explain melting point, electrical conductivity and malleability. Giant latticeIn a solid metal, atoms form a regular, repeating three-dimensional arrangement.

  • The metallic bond
  • Exam explanation
  • Compare with an ionic solid
  • Worked example

Section 1 of 5Structure of a metal

  1. Giant lattice

    In a solid metal, atoms form a regular, repeating three-dimensional arrangement.
    • Their outer electrons become delocalised: they are no longer attached to one particular atom and can move through the lattice.
    • The atoms left behind are positive metal ions.

  2. The metallic bond

    Metallic bonding is the strong electrostatic attraction between positive metal ions and the negatively charged delocalised electrons.
    • This attraction holds the giant lattice together.
    • A metal alloy also has metallic bonding, although it contains more than one type of atom.

Section 2 of 5Melting and boiling

  1. Most metals have relatively high melting and boiling points because a large amount of energy is needed to overcome the strong attraction between the positive ions and delocalised electrons throughout the lattice.
    • The exact temperature varies between metals because the strength of metallic bonding varies.

  2. Exam explanation

    When asked why a metal has a high melting point, name both the positive metal ions and the delocalised electrons, state that the attraction between them is strong, and link that strength to the large energy input needed.

Section 3 of 5Electrical conductivity

  1. Metals conduct electricity as solids because their delocalised electrons can move through the lattice.
    • When a potential difference is applied, the electrons carry electrical charge.
    • The ions stay in their lattice positions; they are not the mobile charge carriers in solid metal.

  2. Compare with an ionic solid

    An ionic solid does not conduct while solid because its charged ions cannot move freely. A metal can conduct while solid because it has mobile electrons. This distinction helps identify which particles carry the charge.

Section 4 of 5Malleability

  1. Most metals are malleable: they can be hammered or rolled into a new shape.
    • Metal ions are arranged in layers that can slide past one another when a force is applied.
    • The delocalised electrons continue to attract the positive ions, so the metal stays bonded as its shape changes.

  2. Worked example

    Explain why copper can be shaped into a sheet and still conduct electricity.
    • Its layers of positive ions can slide without the metallic bond breaking completely, while the delocalised electrons remain free to move and carry charge.

Section 5 of 5Check your understanding

  1. 1.
    • Define a delocalised electron.
    • 2.
    • Identify the two types of charged particle involved in metallic bonding.
    • 3.
    • Explain why a metal conducts electricity when solid.
    • 4.
    • Use the lattice model to explain malleability.
    • 5.
    • Explain a high melting point in terms of force and energy.

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