Why are metals typically good conductors of electricity?

Metals are typically good conductors of electricity because they have free electrons that can move easily.

In more detail, the structure of a metal atom can be thought of as a lattice of positive ions, surrounded by a 'sea' of delocalised electrons. These electrons are not attached to any particular atom and are free to move throughout the metal. This is often referred to as the 'sea of electrons' model.

When a voltage (or a 'push') is applied across a piece of metal, these free electrons can move easily through the metal, carrying the electrical charge with them. This movement of charge is what we know as an electric current. Therefore, the more free electrons a material has, the better it can conduct electricity.

Metals have a high number of free electrons because of their atomic structure. In the outer shell of a metal atom, there are typically one to three electrons. These outer electrons are not tightly bound to the nucleus and can be easily dislodged. Once dislodged, they become free electrons and contribute to the 'sea' of electrons.

This is why metals such as copper, silver, and aluminium are excellent conductors of electricity. They have a large number of free, delocalised electrons that can carry electrical charge efficiently. This property is not only important for the conduction of electricity but also for the conduction of heat, making metals good thermal conductors as well.

In summary, the good electrical conductivity of metals is due to their unique atomic structure, which results in a large number of free, delocalised electrons that can carry electrical charge easily when a voltage is applied.