Why are metals good conductors of electricity?

Answer 1

Because metals release negative ions which conduct electricity.

Because of the force of attraction between valence electron and also because the free electrons can move freely through the lattice carrying a charge.

Answer 2

Metals are elements with between one and three valence electrons, which therefore have a tendency to rid themselves of electrons in order to obtain a stable electron configuration, as opposed to nonmetals which (except for hydrogen, which is a special case) have between four and eight valence electrons and which have much less tendency to rid themselves of electrons. So a collection of metal atoms forms a metallic bond, in which a cloud of loosely shared electrons is created from the surplus electrons that the metals tend to shed. This electron cloud very readily conducts electricity.

ANOTHER ANSWER:According to electron sea theory the valence electrons of a metal atom are not firmly held by the nucleus due to large size and low ionization of metal atoms. These electrons form a sea of electrons and can move easily from one atom to the other. Therefore metals conduct heat are known as good conductors of electricity.
Metal atoms have free electrons which involve in metallic bonding which are responsible for the conductivity.

Answer 3

Metals are good conductors of electricity because they have a sea of free electrons that can move easily through the metal lattice when a voltage is applied. These free electrons are not bound to specific atoms, allowing them to carry electrical charge efficiently. The structure of metals also allows for a high density of mobile charge carriers, facilitating the flow of electric current.