Metals conduct electricity because they have “free electrons.” Unlike most other forms of matter, metallic bonding is unique because the electrons are not bound to a particular atom. This allows the delocalized electrons to flow in response to a potential difference.
And since metals don't tightly hold on to electrons during metallic bonding, they are easily replaced. In metallic bonding, electrons are delocalized and move freely among nuclei. When a force is exerted n the metal, the nuclei shift, but the bonds do not break, giving metals their characteristic malleability.
Oxidation half reaction is written as follows when using using reduction potential chart example when using copper it is written as follows CU2+ +2e- --> c(s) +0.34v oxidasation is the loos of electron hence copper oxidation potential is as follows cu (s) --> CU2+ +2e -0.34v
