Which option correctly explains electrical conductivity of metals?
metals are poor conductors of electricity because the inner electrons in metallic crystals are not free to move.
metals are poor conductors of electricity because the valence electrons in metallic crystals are not free to move.
metals are good conductors of electricity because the valence electrons in metallic crystals are free to move.
metals are good conductors of electricity because the inner electrons in metallic crystals are free to move.

Metals are good conductors of electricity because the valence electrons in metallic crystals are free to move.

Explanation:

Metallic bonds joins atoms of metals and alloys together. The formation of this bond type is favoured by large atomic radius, low ionization energy and a large number of electrons in the valence shell.

The metallic bond is responsible for the bulk of the physical properties of metals we know such as malleablility, ductility, electrical and thermal conductivity e.t.c.

a non redox reaction occurs when there is not a transfer of electrons. for redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. elements that are reduced gain electrons, and elements that are oxidized lose electrons.

explanation: