Metal Crystal Structures

HKDSE Tip

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  Metallic bonding:

  Metallic bonding is the electrostatic attraction between metal cations and delocalized electrons.
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  Bond strength:

  Metallic bond strength increases with more delocalized electrons.
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  Cation charge:

  A higher charge on the cation (like $A{l}^{3+}$ vs $N{a}^{+}$) and more delocalized electrons lead to a stronger metallic bond.
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  Key properties:

  Metals have high electrical conductivity, malleability, and ductility due to metallic bonding.
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  Layer sliding:

  When a force is applied, layers of metal atoms/ions can slide over each other without breaking the metallic bond, because the sea of delocalized electrons holds the structure together continuously.