How Iron acts as both oxidant and reductant?
Answers
Explanation:
+2 and +3 are common oxidation states of iron. I don't think there's a reaction where Fe3+ in FeCl3 can be oxidised to Fe4+ although iron can take oxidation states upto +6 but they are very rare and very high energy is required to pull extra electrons from 3d orbital.
FeCl3 in normal reactions is reduced to FeCl2, so FeCl3 is an oxidizing agent.
FeCl3 + CuCl = FeCl2 + CuCl2
However FeCl2 can act as both oxidising and reducing agent depending on the reactant. [ +2 state lies between 0 and +3]
Answer:
Explanation:
Reaction of iron with air
Iron metal reacts in moist air by oxidation to give a hydrated iron oxide. This does not protect the iron surface to further reaction since it flakes off, exposing more iron metal to oxidation. ... On heating with oxygen, O2, the result is formation of the iron oxides Fe2O3 and Fe3O4.