17084-02-5

Basic information

• Product Name: [N-[2-[bis(carboxymethyl)amino]ethyl]-N-(2-hydroxyethyl)glycinato(3-)]iron
• Synonyms: [N-[2-[bis(carboxymethyl)amino]ethyl]-N-(2-hydroxyethyl)glycinato(3-)]iron;Iron(2-), [N-[2-[bis(carboxy-.kappa.O)methyl]amino-.kappa.N]ethyl]-N-[2-(hydroxy-.kappa.O)ethyl}glycinate(3-)-.kappa.N,.kappa.O];iron, [n-[2-[bis(carboxymethyl)amino]ethyl]-n-(2-hydroxyethyl)glycinato(3-)];Iron, [N-[2-[bis[(carboxy-.kappa.O)methyl]amino-.kappa.N]ethyl]-N-[2-(hydroxy-.kappa.O)ethyl]glycinato(3-)-.kappa.N,.kappa.O];Ferric hedta;Iron, [[N-(carboxymethyl)-N'-(2-hydroxyethyl)-N,N'-ethylenediglycinato](3-)]-;Nsc97346
• CAS NO: 17084-02-5
• Molecular Formula: C₁₀H₁₅N₂O₇*Fe
• Molecular Weight: 334.103
• EINECS: 241-142-5
• Mol File: 17084-02-5.mol

Chemical Properties

• Boiling Point: 572.5 °C at 760 mmHg
• Flash Point: 300 °C
• Appearance: /
• Density: g/cm³
• Vapor Pressure: 1.72E-15mmHg at 25°C
• CAS DataBase Reference: [N-[2-[bis(carboxymethyl)amino]ethyl]-N-(2-hydroxyethyl)glycinato(3-)]iron(CAS DataBase Reference)
• NIST Chemistry Reference: [N-[2-[bis(carboxymethyl)amino]ethyl]-N-(2-hydroxyethyl)glycinato(3-)]iron(17084-02-5)
• EPA Substance Registry System: [N-[2-[bis(carboxymethyl)amino]ethyl]-N-(2-hydroxyethyl)glycinato(3-)]iron(17084-02-5)

Safety Data

• Hazardous Substances Data: 17084-02-5(Hazardous Substances Data)

Usage

Uses

Used in Pharmaceutical Industry:
Ferric glycine complex is used as an iron supplement for patients with iron-deficiency anemia. It provides a stable and bioavailable source of iron, helping to alleviate symptoms associated with iron deficiency and improve overall health.
Used in Food Industry:
As a food additive, ferric glycine complex is used to fortify products with iron, ensuring adequate iron intake for individuals who may not receive enough through their diet. This is particularly important for populations at risk of iron deficiency, such as children, pregnant women, and vegetarians.
Used in Treatment of Iron Overload Disorders:
Ferric glycine complex has been studied for its potential use in the treatment of iron overload disorders, such as hemochromatosis. Its high bioavailability and stability make it a promising candidate for managing and treating conditions where iron levels in the body are excessively high.
Overall, [N-[2-[bis(carboxymethyl)amino]ethyl]-N-(2-hydroxyethyl)glycinato(3-)]iron, or ferric glycine complex, serves as an important tool in addressing iron deficiencies and related health conditions across various industries, including pharmaceuticals and food production. Its unique properties make it a valuable asset in ensuring adequate iron intake and managing iron-related disorders.

InChI:InChI=1/C10H18N2O7.Fe/c13-4-3-11(5-8(14)15)1-2-12(6-9(16)17)7-10(18)19;/h13H,1-7H2,(H,14,15)(H,16,17)(H,18,19);/q;+2

Upstream product

• 43218-58-2 {Fe(II)(N-(hydroxyethyl)ethylenediaminetriacatate)}^(1-) 

Relevant articles and documents

Electron Spin Resonance Studies of Iron(III) Complexes of Ethylenediamine-tetra-acetate and N-(2-Hydroxyethyl)ethylenediamine-NN'N'-triacetate in Co-ordinating Solvents

Remarkable solvent dependence of the apparent peak-to-peak linewidth (ΔHpp) has been observed for the rhombic type of e.s.r. spectra of the high-spin FeIII(edta) (edta = ethylenediaminetetra-acetate) and FeIII(hedta) hedt

Influence of the polyamino carboxylate chelating ligand (L) on the kinetics and mechanism of the formation of FeII(L)NO in the system FeII(L)/NO/HONO/NO2- in aqueous solution

FeII(L) reacts with NO, HONO, and NO2- to produce FeII(L)NO for L = diethylenetriaminepentaacetate, ethylenediaminetetraacetate, N-(hydroxyethyl)ethylenediaminetriacetate, nitrilotriacetate, ethylenediaminediacetate, and water. The reaction with HONO and NO2- occurs in two parallel paths of different order with respect to the reaction components. The systematic variation of the nature of L enables an investigation of the role of labile coordination sites on the Fe(II) center during such reactions. The parallel reactions are characterized by the rate law -d[FeII(L)]/dt = kA[HONO]2 + kB[FeII(L)][HONO], and the contribution of each path depends on the nature of L, pH, and total nitrite concentration. The kinetic data support the formation of a reactive intermediate, most probably N2O3 (kA path), and the reduction of HONO by FeII(L) to NO (kB path). The observed reactions and reactivity patterns strongly depend on the availability of labile coordinated solvent molecules on FeII(L), as governed by the nature of the ligand L. The results of this study are discussed in reference to the available literture data and in comparison to the kinetics of oxidation of these complexes by molecular oxygen.

Kinetics and mechanism of the autoxidation of iron(II) induced through chelation by ethylenediaminetetraacetate and related ligands

The oxidation of FeII(L) complexes by molecular oxygen is significantly enhanced by the presence of a chelating ligand L. The kinetics of this reaction was studied for L = ethylenediaminetetraacetate, N-(hydroxyethyl)ethylenediaminetriacetate, and diethylenetriaminepentaacetate as a function of [FeII(L)], [O2], pH, temperature, and pressure. All the observed kinetic relationships can be accounted for in terms of a mechanism in which O2 rapidly reacts with FeII(L) to produce FeII(L)O2, followed by three parallel reaction steps. These include spontaneous and acid-catalyzed electron transfer, as well as a reaction with FeII(L) to produce (L)FeIII-O22--FeIII(L). The results are discussed in reference to the available literature data for these and related oxidation processes.