Ferrocyanide



 

Ferrocyanide is the name of the anion coordination complex is relatively unreactive. It is usually available as the potassium salt potassium ferrocyanide, which has the formula K4Fe(CN)6.

Coordination chemistry

[Fe(CN)6]4− is a diamagnetic species, featuring low-spin iron(II) center in an octahedral ligand environment. Although many salts of cyanide are highly toxic, ferro- and ferricyanides are less toxic because they tend not to release free cyanide.[1] Its most important reaction is its oxidation to ferricyanide:

[Fe(CN)6]4− \overrightarrow{\leftarrow} [Fe(CN)6]3− + e−

This conversion can be followed absorption coefficient of 21600 M−1 cm−1.

Treatment of ferrocyanide with ferric-containing compounds affords Prussian Blue, an intensely blue polymer that is widely used as a pigment.[1]

Use in biochemistry

Ferrocyanide and its oxidized product ferricyanide, [Fe(CN)6]3−, are impermeable to the plasma membrane. For this reason ferrocyanide has been used as a probe of extracellular electron receptor in the study of redox reactions in cells. Ferricyanide is used thus any increase in ferrocyanide can be attributed to secretions of reductants or "Trans Plasma Membrane Electron Transport" (TPMET) activity.

diabetes. It is used in this application because it is easily reduced to potassium ferrocyanide.

Nomenclature

According to the recommendations of IUPAC, ferrocyanide should be called "hexacyanoferrate(II)."

References

  1. ^ a b Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
 
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