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	FeC6H6O7
Molar mass	245.95644 g/mol
Appearance	slightly gray-green powder or white crystals unstable
Density	1.91 g/cm3
Melting point	decomposes
	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.^[3] Ferrous citrates are all paramagnetic, reflecting the weak crystal field of the carboxylate ligands.^[4]

Structure of the anionic coordination polymer {[Fe(C₆H₅O₇)(H₂O)]⁻}_n.^[3] (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.^[5]^[2] Ferrous citrates are all highly unstable in air, converting to ferric citrates.

References

^ Food Chemicals Codex (US Pharmacopeia Conv, 2010 - 1405 pages), page 396 – https://books.google.com.vn/books?id=zNr3YaoNZvQC&pg=PA396&hl=vi&sa=X&ved=0ahUKEwiZobTm0rbqAhXKc3AKHfxaDHQQ6AEIQjAE#v=onepage&q&f=false. Accessed July 6, 2020.
^ ^a ^b Perry, Dale L.; Phillips, Sidney L., eds. (1995). Handbook of Inorganic Compounds. Boca Raton, Florida: CRC Press. p. 167. ISBN 0-8493-8671-3.
^ ^a ^b 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 about an organic compound is a stub. You can help Wikipedia by expanding it.

[1] Food Chemicals Codex (US Pharmacopeia Conv, 2010 - 1405 pages), page 396 – https://books.google.com.vn/books?id=zNr3YaoNZvQC&pg=PA396&hl=vi&sa=X&ved=0ahUKEwiZobTm0rbqAhXKc3AKHfxaDHQQ6AEIQjAE#v=onepage&q&f=false. Accessed July 6, 2020.

[hpic-2] 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-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.

[4] 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-5] "CFR - Code of Federal Regulations Title 21". www.fda.gov. U.S. Food and Drug Administration. 2013-06-01. Retrieved 2014-08-02.

[1]

[2]

[3]

[4]

[5]