Iron(II) citrate

Iron(II) citrate
Names
	IUPAC name Iron(II) hydrogen 2-hydroxy-1,2,3-tricarboxylpropane
	Other names Iron(II) citrate, Ferrous citrate, Iron citrate
Identifiers
CAS Number	23383-11-1 ; 61918-28-3 (duplicate);
ECHA InfoCard	100.041.463
UNII	33KM3X4QQW ;
Properties
Chemical formula	C12H30Fe3O24
Molar mass	725.883 g·mol−1
Density	1.91 g/cm3
Melting point	decomposes[1]
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	Infobox references

Ferrous citrate, or iron(II) citrate, describes coordination complexes containing citrate anions with Fe²⁺ formed in aqueous solution. Although a number of complexes are possible (or even likely), only one complex has been crystallized. That complex is the coordination polymer with the formula [Fe(H₂O)₆]²⁺{[Fe(C₆H₅O₇)(H₂O)]^-}₂^.2H₂O, where C₆H₅O₇^3- is HOC(CH₂CO₂^-)₂(CO₂^-, i.e., the triple conjugate base of citric acid wherein the three carboxylic acid groups are ionized.[2] Ferrous citrates are all paramagnetic, reflecting the weak crystal field of the carboxylate ligands.[3]

Structure of the anionic coordination polymer {[Fe(C₆H₅O₇)(H₂O)]^-}_n.[2] (legend: red = O, gray = C, blue = Fe, white = H).

Ferrous citrates are produced by treating disodium citrate Na
₂C
₆H
₆O
₇ with sources of iron(II) aquo complexes, such as iron(II) sulfate.[4][1] Ferrous citrates are all highly unstable in air, converting to ferric citrates.

References

Perry, Dale L.; Phillips, Sidney L., eds. (1995). Handbook of Inorganic Compounds. Boca Raton, Florida: CRC Press. p. 167. ISBN 0-8493-8671-3.
Strouse, Jane; Layten, Steven W.; Strouse, Charles E. (1977). "Structural Studies of transition metal complexes of triionized and tetraionized citrate. Models for the coordination of the citrate ion to transition metal ions in solution and at the active site of aconitase". Journal of the American Chemical Society. 99 (2): 562–572. doi:10.1021/ja00444a041. PMID 830693.
Pierre, J. L.; Gautier-Luneau, I. (2000). "Iron and Citric Acid: A Fuzzy Chemistry of Ubiquitous Biological Relevance". Biometals. 13: 91–96. doi:10.1023/A:1009225701332.
"CFR - Code of Federal Regulations Title 21". www.fda.gov. U.S. Food and Drug Administration. 2013-06-01. Retrieved 2014-08-02.

This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.

[hpic-1] Perry, Dale L.; Phillips, Sidney L., eds. (1995). Handbook of Inorganic Compounds. Boca Raton, Florida: CRC Press. p. 167. ISBN 0-8493-8671-3.

[Strouse-2] Strouse, Jane; Layten, Steven W.; Strouse, Charles E. (1977). "Structural Studies of transition metal complexes of triionized and tetraionized citrate. Models for the coordination of the citrate ion to transition metal ions in solution and at the active site of aconitase". Journal of the American Chemical Society. 99 (2): 562–572. doi:10.1021/ja00444a041. PMID 830693.

[3] Pierre, J. L.; Gautier-Luneau, I. (2000). "Iron and Citric Acid: A Fuzzy Chemistry of Ubiquitous Biological Relevance". Biometals. 13: 91–96. doi:10.1023/A:1009225701332.

[fda-4] "CFR - Code of Federal Regulations Title 21". www.fda.gov. U.S. Food and Drug Administration. 2013-06-01. Retrieved 2014-08-02.