Ferricyanide

Ferricyanide

Names
IUPAC name iron(3+) hexacyanide
Systematic IUPAC name hexacyanidoferrate(III)
Other names ferric hexacyanide; hexacyanidoferrate(3-); hexacyanoferrate(III)
Identifiers
3D model (JSmol)	Interactive image
PubChem CID	439210
SMILES [C-]#N.[C-]#N.[C-]#N.[C-]#N.[C-]#N.[C-]#N.[Fe+3]
Properties
Chemical formula	[Fe(CN)6]3−
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Ferricyanide is the anion [Fe(CN)₆]³⁻.  It is also called hexacyanoferrate(III) and in rare, but systematic nomenclature, hexacyanidoferrate(III). The most common salt of this anion is potassium ferricyanide, a red crystalline material that is used as an oxidant in organic chemistry.^[1]

Properties

[Fe(CN)₆]³⁻ consists of a Fe³⁺ center bound in octahedral geometry to six cyanide ligands. The complex has O_h symmetry. The iron is low spin and easily reduced to the related ferrocyanide ion [Fe(CN)₆]⁴⁻, which is a ferrous (Fe²⁺) derivative. This redox couple is reversible and entails no making or breaking of Fe-C bonds:

[Fe(CN)₆]³⁻ + e⁻ → [Fe(CN)₆]⁴⁻

This redox couple is a standard in electrochemistry.

Compared to normal cyanides like potassium cyanide, ferricyanides are much less toxic because of the tight hold of the CN⁻ to the Fe³⁺. They do react with mineral acids, however, to release highly toxic hydrogen cyanide gas.

Uses

Treatment of ferricyanide with ferrous salts affords the brilliant, long-lasting pigment Prussian blue, the traditional color of blueprints.

References

1. ↑ Gail, E.; Gos, S.; Kulzer, R.; Lorösch, J.; Rubo, A.; Sauer, M.; Kellens, R.; Reddy, J.; Steier, N.; Hasenpusch, W. (October 2011). "Cyano Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a08_159.pub3. 

See also

• Potassium ferricyanide
• Ferrocyanide