Why are metals good conductors of electricity?

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Metals conduct electricity because their atoms form a lattice with a sea of delocalized electrons that are not bound to any single atom. Each metal atom contributes electrons to this shared electron cloud, so there are free charge carriers that can move throughout the structure. When a voltage is applied, these mobile electrons drift and carry current quickly, which is why metals are such good conductors. The crucial point is having at least one free electron per atom to supply that continuous flow of charge. Factors like large atomic radius or dense packing describe the arrangement of atoms but don’t by themselves ensure conductivity, and a high melting point reflects bond strength rather than the presence of free carriers.