Metals are excellent conductors of electricity due to the presence of a 'sea' of delocalised electrons. In a metallic lattice, the metal atoms are arranged in a regular, repeating pattern, forming a giant lattice of positive ions. These positive ions are held together by the electrostatic attraction to the delocalised electrons.

When an electric field is applied, the delocalised electrons are free to move throughout the entire metal structure. This movement of charge constitutes an electric current. Because there are many free electrons available, metals can conduct electricity very efficiently.

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Metals are malleable and ductile because of the nature of their metallic bonding.

• Metallic Bonding & Flexibility: The metallic bond is not a strong, directional bond like covalent bonds. The delocalised electrons allow the metal ions to slide past each other without breaking the bonds.
• Malleability: Malleability is the ability of a metal to be hammered or rolled into thin sheets. When a force is applied, the metallic lattice deforms without fracturing. The delocalised electrons facilitate this deformation by allowing the ions to rearrange themselves into new, stable positions.
• Ductility: Ductility is the ability of a metal to be drawn into wires. Similar to malleability, the delocalised electrons allow the metal ions to slide past each other without breaking the bonds. This continuous deformation allows the metal to be elongated into wires.
• Crystal Structure: The crystal structure of metals (e.g., face-centred cubic, body-centred cubic) also contributes to malleability and ductility. These structures allow for easier sliding of the metal ions.

In essence, the ability of the metallic lattice to deform under stress without breaking is a direct consequence of the delocalised electrons and the non-directional nature of the metallic bond.

In a solid metal, metal ions (positive ions) are arranged in a regular, repeating lattice structure. This lattice is surrounded by a "sea" of delocalised electrons that are free to move throughout the entire structure.

Electrical Conductivity: The delocalised electrons are the key to good electrical conductivity. When a voltage is applied, these electrons are easily displaced and flow in a specific direction, forming an electric current. The lattice provides a framework for these electrons to move through with minimal resistance.

Malleability and Ductility: The metallic bond, formed by the interaction between the positive metal ions and the delocalised electrons, is non-directional. This means that the metal ions can slide past each other without breaking the bonds. The delocalised electrons facilitate this movement by allowing the ions to rearrange themselves into new, stable positions under stress. This ability to deform without fracturing is what gives metals their malleability and ductility.