Ferrocyanide

Anion in which a Fe2+ ion is complexed by 6 CN− ions
Ferrocyanide ion
Identifiers
CAS Number
  • 13408-63-4 checkY
3D model (JSmol)
  • Interactive image
ChEBI
  • CHEBI:5032
ChemSpider
  • 10446887
KEGG
  • C01913
PubChem CID
  • 9552077
UNII
  • FLX0VIC39Y checkY
CompTox Dashboard (EPA)
  • DTXSID0065436 Edit this at Wikidata
InChI
  • InChI=1S/6CN.Fe/c6*1-2;/q6*-1;+2
    Key: UETZVSHORCDDTH-UHFFFAOYSA-N
  • [C-]#N.[C-]#N.[C-]#N.[C-]#N.[C-]#N.[C-]#N.[Fe+2]
Properties
Chemical formula
 C6FeN64−
Molar mass 211.955 g·mol−1
Related compounds
Related compounds
 Ferricyanide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
Chemical compound

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 and, as its potassium salt, an anticaking agent.[2]

Reactions

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

Ferrocyanide reversibly oxidized by one electron, giving ferricyanide:

[Fe(CN)6]4− ⇌ [Fe(CN)6]3− + e−

This conversion can be followed spectroscopically at 420 nm, since ferrocyanide has negligible absorption at this wavelength while ferricyanide has an extinction coefficient of 1040 M−1 cm−1.[3]

Applications

The dominant use of ferrocyanides is as precursors to the Prussian blue pigments. Sodium ferrocyanide is a common anti-caking agent. Specialized applications involves their use as precipitating agents for production of citric acid and wine.[2]

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 acceptor in the study of redox reactions in cells. Ferricyanide is consumed in the process, thus any increase in ferrocyanide can be attributed to secretions of reductants or transplasma membrane electron transport activity.

Nickel ferrocyanide (Ni2Fe(CN)6) is also used as catalyst in electro-oxidation (anodic oxidation) of urea.[4] Aspirational applications range from hydrogen production for cleaner energy with lower CO2 emission to wastewater treatment.

Ferrocyanide is also studied as an electrolyte in flow batteries.[5][6]

Nomenclature

According to the recommendations of IUPAC, ferrocyanide should be called "hexacyanidoferrate(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 κύανος kyanos, Greek for "(dark) blue."

Gallery

See also

References

  1. ^ a b Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 0-12-352651-5.
  2. ^ a b Gail, E.; Gos, S.; Kulzer, R.; Lorösch, J.; Rubo, A.; Sauer, M.; Kellens, R.; Reddy, J.; Steier, N. (2011). "Cyano Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a08_159.pub3. ISBN 978-3527306732.
  3. ^ Appleby, C. A.; Morton, R. K. (1959). "Lactic dehydrogenase and cytochrome b2 of baker's yeast: Purification and crystallization". Biochem. J. 71 (3): 492–499. doi:10.1042/bj0710492. PMC 1196822. PMID 13638255.
  4. ^ Geng, Shi-Kui; Zheng, Yao; Li, Shan-Qing; Zhao, Xu; Hu, Jun; Shu, Hai-Bo; Jaroniec, Mietek; Chen, Ping; Liu, Qinghua; Qiao, Shizhang (2020). "Nickel ferrocyanide as high-performance next generation electrocatalyst for urea oxidation". Nature Energy. doi:10.21203/rs.3.rs-67358/v1. S2CID 231949301.
  5. ^ Evans-Pritchard, Ambrose (2016-08-10). "Holy Grail of energy policy in sight as battery technology smashes the old order". The Telegraph. ISSN 0307-1235. Retrieved 2023-06-28.
  6. ^ Developing Organic Flow Batteries for Energy Storage (arpa-e.gov) http://arpa-e.energy.gov/sites/default/files/documents/files/HarvardFlowBattery_OPEN2012_ExternalProjectImpactSheet_FINAL.pdf
  • v
  • t
  • e
Salts and covalent derivatives of the cyanide ion
HCN He
LiCN Be(CN)2 B(CN)3 C(CN)4
C2(CN)2 		NH4CN
ONCN
O2NCN
N3CN 		OCN−
-NCO
O(CN)2 		FCN Ne
NaCN Mg(CN)2 Al(CN)3 Si(CN)4
(CH3)3SiCN 		P(CN)3 SCN−
-NCS
(SCN)2
S(CN)2 		ClCN Ar
KCN Ca(CN)2 Sc(CN)3 Ti V Cr(CN)63− Mn Fe(CN)2
Fe(CN)64−
Fe(CN)63− 		Co(CN)2
Co(CN)3−
5 		Ni(CN)2
Ni(CN)42−
Ni(CN)44− 		CuCN Zn(CN)2 Ga(CN)3 Ge(CN)2
Ge(CN)4 		As(CN)3
(CH3)2AsCN
(C6H5)2AsCN 		SeCN−
(SeCN)2
Se(CN)2 		BrCN Kr
RbCN Sr(CN)2 Y(CN)3 Zr Nb Mo(CN)84− Tc Ru Rh Pd(CN)2 AgCN Cd(CN)2 In(CN)3 Sn(CN)2 Sb(CN)3 Te(CN)2
Te(CN)4 		ICN Xe
CsCN Ba(CN)2 * Lu(CN)3 Hf Ta W(CN)84− Re Os Ir Pt(CN)42-
Pt(CN)64-
 AuCN
Au(CN)2- 		Hg2(CN)2
Hg(CN)2 		TlCN Pb(CN)2 Bi(CN)3 Po At Rn
Fr Ra ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
 
* La(CN)3 Ce(CN)3
Ce(CN)4 		Pr(CN)3 Nd Pm Sm(CN)3 Eu(CN)3 Gd(CN)3 Tb Dy(CN)3 Ho(CN)3 Er Tm Yb(CN)3
** Ac(CN)3 Th(CN)4 Pa UO2(CN)2 Np Pu Am Cm Bk Cf Es Fm Md No