Chemistry – Atoms, elements and compounds - Metallic bonding | e-Consult
Atoms, elements and compounds - Metallic bonding (1 questions)
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Metals are excellent conductors of electricity due to their unique metallic bonding. The metallic bond arises from a "sea" of delocalised electrons.
- Metallic Bonding: In a metal, the valence electrons are not associated with individual atoms but are free to move throughout the entire metallic lattice. This creates a 'sea' of delocalised electrons.
- Electron Availability: These delocalised electrons are not bound to specific atoms and can easily move under the influence of an electric field.
- Charge Carriers: The delocalised electrons act as the charge carriers in an electric current. When a potential difference is applied, these electrons drift in a specific direction, constituting the electric current.
- Lattice Structure: The metallic lattice, composed of positively charged metal ions, provides a framework for the delocalised electrons to move through with minimal resistance. The regular arrangement of ions facilitates electron flow.
Therefore, the presence of a large number of delocalised electrons readily available for conduction is the primary reason for the good electrical conductivity of metals.