Question

Identify the oxidized substance and the reduced substance in the redox reaction. Mg(s)+Cl2(g)⟶Mg2+(aq)+2Cl−(aq) Which substance gets oxidized? Mg Cl2 Cl− Mg2+ Which substance gets reduced?

Answer 1

Answer:

Mg (s) is the oxidized substance and $Cl_{2}$ (g) is the reduced substance

Explanation:

If oxidation number of a substance increases then that substance is being oxidized. This is due to release of electron from that substance.

If oxidation number of a substance decreases then that substance is being reduced. This is due to consumption of electrons by that substance.

                               Element                        oxidation number

                                  Mg(s)                                     0

                                $Cl_{2}$                       0 (Cl)

                                $Mg^{2+}$                    +2 (Mg)

                                $Cl^{-}$                          -1 (Cl)

So oxidation number of Mg increases by +2 which occurs due to release of two electrons from Mg (s). Hence Mg (s) is being oxidized.

And oxidation number of Cl decreases by -1 which occurs due to consumption of one electron by $Cl_{2}$ (g). Hence $Cl_{2}$ (g) is being reduced.