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How to Identify the Oxides of Iron

Iron readily forms oxides when in the presence of oxygen. Iron is a transition metal found in group VIII B of the periodic table. Unlike traditional metals, such as the alkaline and alkali earth metals, transition metals are noted for their ability to exist in a multitude of oxidation states. The extensive range of oxidation states is directly related to the fact that transition metals possess a d - orbital in their electron configuration. The determination of the specific oxide of iron present is made by examining the non-metal portion of the oxide.

Instructions

- 1
  Determine the overall oxidation state of the iron oxide compound present. This information is most commonly presented in the upper right corner of the compound, similar to where an exponent is displayed.
- 2
  Multiply the oxidation charge of the oxygen by the number of oxygen atoms present. For reference, the oxidation charge of oxygen is -2.
- 3
  Subtract the total charge value of the oxygen atoms present from the overall charge of the compound. It is important to remember that a negative quantity is being subtracted from the overall charge. This operation yields the overall charge of the iron atoms present in the compound.
- 4
  Divide the overall charge of the iron atoms present in the compound by the number of iron atoms. The result of this operation yields the oxidation state of each iron atom.
- 5
  Rewrite the compound to express the oxidation state of the iron. For example if the oxidation state of the iron was determined to be +3 the compound would be written as iron (III) oxide, to reflect the charge on the iron.

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