Chemistry – Atoms, elements and compounds - Metallic bonding | e-Consult

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.