n.
A salt containing the negative tetravalent radical Fe(CN)6, used in making blue pigments, blueprint paper, and ferricyanide.
ferrocyanide
Dictionary:
fer·ro·cy·a·nide (fĕr'ō-sī'ə-nīd')  |
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The common name for hexacyanoferrate(II), a compound containing the complex ion [Fe(CN)6]4−. The oxidation state of iron is 2+ (Fe2+ or FeII) and is low spin (spin paired), consistent with the strong field nature of the cyanide (CN−) ligand.
The [Fe(CN)6]4− ion is very stable, with the CN− ligands adopting the octahedral geometry typical of FeII complexes. The free acid hydrogen hexacyanoferrate(II), H4[Fe(CN)6], is soluble in water and is isolated as a white powder by ether precipitation of the ion in strongly acidic solutions. The salts of sodium, Na4Fe(CN)6, and potassium, K4Fe(CN)6, are prepared by heating an aqueous mixture of sodium cyanide (NaCN), iron(II) sulfate (FeSO4), and other salts. The complexes are substitutionaly inert (in contrast to ferricyanide, [Fe(CN)6]3−, which dissociates rapidly) and are isolated as yellow crystalline decahydrate solids that are insoluble in most organic solvents. Hexacyanoferrate(II) may be converted to hexacyanoferrate(III) (ferricyanide) by strong oxidizing agents such as peroxides and permanganate ion. See also Ferricyanide.
Ferrocyanide is a commonly used as a reducing agent; and principal applications include the preparation of dyes, preparation of fixatives used in photography, and stabilization of synthetic and natural latex foams, and as an emulsion polymerization catalyst.
Nearly 300 years ago the mixed-valence compound Prussian blue (Fe4III[FeII(CN)6]3 · xH2O, where x = 14–16) was discovered to be a pigment. Prussian blue is prepared by the addition of FeIII to [Fe(CN)6]4− or of FeII to [Fe(CN)6]3−, and the structure has been determined by x-ray analysis and powder neutron diffraction studies. Uses of this complex, also known as Turnbull's blue, include artists' colors, carbon paper, typewriter ribbons, and printing inks. The reduction of Prussian blue results in the formation of Everitt's salt, K2[Fe IIFe II(CN6)]. See also Coordination chemistry;
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An organic compound used in industry that is reputed to be virtually harmless in spite of its cyanide content.
| Wikipedia: Ferrocyanide |
| Ferrocyanide | |
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| Identifiers | |
| CAS number | [] |
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| Properties | |
| Molecular formula | C6FeN6-4 |
| Molar mass | 211.9494 |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
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Ferrocyanide is the name of the anion Fe(CN)64−. In aqueous solutions, this coordination complex is relatively unreactive. It is usually available as the potassium salt potassium ferrocyanide, which has the formula K4Fe(CN)6.
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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−
[Fe(CN)6]3− + e−
This conversion can be followed spectroscopically at 535 nm with an absorption coefficient of 21600 M−1 cm−1.
Treatment of ferrocyanide with ferric-containing compounds affords Prussian Blue, an intensely blue compound 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.
Potassium ferricyanide is often used as a mediator in the test strips used with blood glucose meters by people suffering from 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)."
See also
References
- ^ a b Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
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 | Dictionary. The American Heritage® Dictionary of the English Language, Fourth Edition Copyright © 2007, 2000 by Houghton Mifflin Company. Updated in 2009. Published by Houghton Mifflin Company. All rights reserved. Read more |
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| Sci-Tech Encyclopedia. McGraw-Hill Encyclopedia of Science and Technology. Copyright © 2005 by The McGraw-Hill Companies, Inc. All rights reserved. Read more |
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Mentioned in
- Prussian blue
- ferrocyanate
- ferrocyanide process (chemical engineering)
- Huber's reagent (analytical chemistry)
- potash blue (inorganic chemistry)
- haloxyline
- ferric ferrocyanide (inorganic chemistry)
- sideroleukocyte
- iron blue (inorganic chemistry)
- nitroprussic
