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Explain the electron-sea model in metallic bonding.

The electron-sea model in metallic bonding describes metal atoms as a lattice of positive ions surrounded by a 'sea' of delocalised electrons.

The electron-sea model, also known as the free-electron model, is a fundamental concept in understanding the unique properties of metals. In this model, metal atoms are visualised as a closely packed, regular lattice of positive ions. These ions are formed when the metal atoms lose their valence electrons. These lost electrons do not attach themselves to any particular atom. Instead, they become delocalised, meaning they are free to move throughout the entire structure. This forms a 'sea' of electrons that surrounds the positive ions.

This model is particularly useful in explaining the properties of metals. For instance, the delocalised electrons allow metals to conduct electricity. When a voltage is applied, these free electrons can move and carry the electric charge. Similarly, metals are good conductors of heat because these electrons can also transfer thermal energy.

The electron-sea model also explains the malleability and ductility of metals. When a force is applied, the layers of positive ions can slide over each other. The 'sea' of electrons between these layers maintains the metallic bond and prevents the ions from repelling each other. This allows the metal to change shape without breaking.

Moreover, the model accounts for the shiny appearance of metals. When light hits the surface of a metal, the delocalised electrons absorb and re-emit the light, causing the metal to shine.

In summary, the electron-sea model provides a comprehensive explanation for the unique properties of metals. It visualises metals as a lattice of positive ions surrounded by a 'sea' of delocalised electrons, which are responsible for the conductivity, malleability, ductility, and lustre of metals.

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