What is the charge of iron (Fe?

Difference in oxidation of iron?

• I am aware that naturally occurring rust is iron oxide and the iron involved is a Fe(III) with a plus 3 charge. How are you able to produce ferrous oxide or Fe(II)O with the iron having a plus 2 charge? Is the iron(II) a low abundance isotope of iron and where could you possibly find this in nature or how could you experimentally produce that specific iron?

• Answer:

  Naturally occurring rust is actually hydrated iron(III) oxide, either Fe(OH)3 in water or FeO(OH) in temperate air. Fe2O3 is actually dehydrated rust. The formation of rust requies not only oxygen, but water, as well. 4Fe(s) + 3O2(g) + 2H2O(l) --> 4FeO(OH)(s) Iron can form various iron(II) oxides on the way to FeO(OH), but they would only be intermediate products. The isotope of iron will have little to no impact on the ultimate oxidation product. Iron-56 makes up almost 92% of stable Fe atoms. All of the isotopes of iron have the same electron arrangement, and therefore, the same chemistry.