What makes metals good conductors of electricity?

Metals are good conductors of electricity due to their structure, which contains free-moving electrons that carry electrical charge.

In more detail, metals are made up of 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. The ease with which these electrons can move makes metals excellent conductors of electricity.

Furthermore, the more free electrons a metal has, the better it conducts electricity. For example, copper and silver have more free electrons and are therefore better conductors than other metals.

It's also worth noting that the structure of metals allows them to conduct heat well, too. This is because the free electrons can also carry thermal energy, or heat, through the metal. So, when you're using a metal object and it gets hot quickly, that's due to the same free-moving electrons that make metals good electrical conductors.

In summary, the key to metals' ability to conduct electricity lies in their unique structure, with their 'sea' of free electrons that can carry electrical charge. This is why metals are commonly used in electrical wiring and other applications where the conduction of electricity is required.