Mg + Cl2 redox reaction explain?

The metal loses electrons, and in forming `Mg^(2+)` it loses 2 electrons and is oxidized:

`Mg(s) rarr Mg^(2+) + 2e^-` `(i)`

And on the other hand chlorine is reduced to chloride ion by accepting electrons:

`Cl_2(g) +2e^(-) rarr 2Cl^(-)` `(ii)`

E `(i) + (ii)=` `Mg(s) + Cl_2(g) rarr MgCl_2(s)`

Both charge and mass are balanced, as required.