Metallic Bonding

The video explains the unique properties of metals, which are attributed to metallic bonding. Metal atoms form a lattice structure, losing electrons to become positive ions. These electrons become delocalised, creating a 'sea' of electrons that allows metals to conduct electricity and heat. The metallic bond is the attraction between these electrons and the positive ions, giving metals their strength, malleability, and conductivity. Metals can be shaped without breaking and are shiny due to electron interaction with light.

What is meant by 'delocalised electrons' in the context of metallic bonding?

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How do the properties of metals, such as conductivity and malleability, relate to their electron structure?

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