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Ferrocyanide

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Title: Ferrocyanide  
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Collection: Anions, Coordination Compounds, Cyanides, Iron Compounds
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Ferrocyanide

Ferrocyanide is the name of the anion [Fe(CN)6]4−. Salts of this coordination complex give yellow solutions. It is usually available as the salt potassium ferrocyanide, which has the formula K4Fe(CN)6. [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] It is of commercial interest as a precursor to the pigment Prussian blue.

Contents

  • Reactions 1
    • Use in biochemical research 1.1
  • Nomenclature 2
  • See also 3
  • References 4

Reactions

Treatment of ferrocyanide with ferric-containing salts gives the intensely coloured pigment Prussian blue [1] (sometimes called ferric ferrocyanide and ferrous ferricyanide).

Ferrocyanide may undergo oxidation, resulting in ferricyanide:

[Fe(CN)6]4− [Fe(CN)6]3− + e

This conversion can be followed spectroscopically at 420 nm, since ferrocyanide has negligible absorption while ferricyanide has an extinction coefficient of 1040 M−1 cm−1.[2]

Use in biochemical research

Ferrocyanide and its oxidized product ferricyanide cannot freely pass through 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 transplasma membrane electron transport activity.

Nomenclature

According to the recommendations of IUPAC, ferrocyanide should be called "hexacyanoferrate(II)." Cyanides as a chemical class were named because they were discovered in ferrocyanide. Ferrocyanide in turn was named in Latin to mean "blue substance with iron." The dye Prussian blue had been first made in the early 18th century. The word "cyanide" used in the name is from kyanos, Greek for "(dark) blue."

See also

References

  1. ^ a b Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego: Academic Press.  
  2. ^ Appleby, C. A., and Morton, R. K., Lactic dehydrogenase and cytochrome b2 of baker's yeast: Purification and crystallization. Biochem. J., 71, 492-499 (1959).
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