is a form of '''iron sulfide''' (others include
Iron Pyrite a.k.a. "Fool's Gold"), and can be obtained by reacting
Iron and
Sulfur under great heat.
The reaction can be explained by the following equation:
:S
8 (s) + 8Fe
(s) → 8FeS
(s)
Iron (II) sulfide exists in several distinct forms, where the
Stoichiometry and properties differ slightly:
- Pyrrhotite - Fe1-xS - a very complicated form observed in mineralogical settings, and also as the waste product of the '' Desulfovibrio '' bacteria, pyrrhotite displays Ferrimagnetism .
- Troilite - FeS - a very similar material to pyrrhotite, but does not possess Ferromagnetic properties.
- Mackinawite - Fe1+xS - the least stable from of iron sulfide, Mackinawite has a layered structure similar to Graphite .
Iron(II) sulfide itself doesn't have many real uses, but it is useful for demonstrating a certain number of chemical changes, especially
Exothermic Reactions in
Laboratories .
The methods of
Chemical Composition can be shown by the production of iron(II) sulfide from
Iron and
Sulfur :
:S
8 (s) + 8Fe
(s) → 8FeS
(s)
This reaction itself requires a heated environment to carry out, however it is exothermic and more energy is given out than taken in.
By reacting iron with sulfur into iron sulfide, teachers can show students that iron shows
Ferromagnetic Properties only in
Elemental form as iron sulfide is not ferromagnetic.
By reacting iron sulfide with
Hydrochloric Acid (HCl), the
Acidic Properties of hydrochloric acid and the
Toxic , pungent fume of
Hydrogen Sulfide can both be demonstrated:
:FeS
(s) + 2HCl
(aq) → FeCl
2 (aq) + H
2S
(g)
By this reaction, teachers can also show changes of state caused by chemical changes.
D. Vaughan, J. Craig, (1978) Mineral Chemistry of Metal Sulfides, Cambridge University Press. ISBN 0521214890
