Metals conduct electricity because they have delocalized electrons. Delocalized electrons are electrons that are not bound to a single atom, but are instead free to move throughout the metal. This allows the electrons to carry electrical current when an electric field is applied.

In non-metals, the electrons are bound to the atoms and cannot move freely. This is why non-metals do not conduct electricity as well as metals.

The amount of electrical conductivity of a metal depends on the number of delocalized electrons it has. Metals with more delocalized electrons, such as copper and silver, are better conductors of electricity than metals with fewer delocalized electrons, such as iron and aluminum.

The electrical conductivity of a metal also depends on its temperature. As the temperature of a metal increases, the electrons become more energetic and can move more freely. This results in an increase in electrical conductivity.

The following are some of the metals that conduct electricity well:

• Copper
• Silver
• Gold
• Aluminum
• Platinum
• Tin
• Lead
• Mercury

These metals are often used in electrical applications, such as wires and cables.