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Metallic bonding is the third major type of bonding you need to understand. It is found in metals and alloys and explains their distinctive properties: high melting points, electrical and thermal conductivity, malleability, and ductility. The model of metallic bonding is fundamentally different from both ionic and covalent bonding.
In a metal, the atoms are packed closely together in a regular lattice arrangement. Each metal atom loses its outer shell electron(s), becoming a positive ion (cation). These electrons do not belong to any particular atom — they become delocalised, forming a "sea" of electrons that spreads throughout the entire structure.
The metallic bond is the strong electrostatic attraction between the positive metal ions and the delocalised electrons. This is the definition you need to learn precisely.
Notice the key features of this model:
The strength of metallic bonding depends on three interrelated factors:
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