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Metallic Bonding and Types of Solids: Flashcards

Revise metallic bonding, alloys and the properties of ionic, molecular, covalent network and metallic solids.

10 cardsBeginner

10 cards

  1. Question
    What is metallic bonding?
    Answer

    The attraction between positive metal ions in a lattice and a sea of delocalized electrons.

  2. Question
    Why do metals conduct electricity?
    Answer

    Their delocalized electrons are free to move through the structure.

  3. Question
    Why are metals malleable but ionic crystals brittle?
    Answer

    Metal layers slide without breaking the bonding; in an ionic crystal, sliding brings like charges together and it shatters.

  4. Question
    Why are alloys harder than pure metals?
    Answer

    Atoms of a different size disrupt the layers, so they slide less easily.

  5. Question
    Name the four types of solid.
    Answer

    Ionic, molecular, covalent network, metallic.

  6. Question
    Why do molecular solids have low melting points?
    Answer

    Only weak forces between molecules need to be overcome; the covalent bonds inside the molecules stay intact.

  7. Question
    When does an ionic compound conduct electricity?
    Answer

    When molten or dissolved, because the ions are then free to move.

  8. Question
    Give two examples of covalent network solids.
    Answer

    Diamond, graphite, silicon dioxide (quartz), silicon.

  9. Question
    Why does graphite conduct electricity but diamond does not?
    Answer

    In graphite each C bonds to 3 others, leaving one delocalized electron per atom; in diamond all 4 outer electrons are in bonds.

  10. Question
    A solid melts at 801 °C and conducts only when molten. What type is it?
    Answer

    Ionic (e.g. sodium chloride).