The kinetics and mechanisms of reactions of iron(III) with caffeic acid, chlorogenic acid, sinapic acid, ferulic acid and naringin

The kinetics and mechanisms of the reactions of iron(III) with the hydroxy cinnamic acid based ligands caffeic, chlorogenic, sinapic and ferulic acids and the flavonoid naringin have been investigated in aqueous solution. The mechanisms for caffeic and chlorogenic acid are generally consistent with the formation of a 1:1 complex that subsequently decays through an electron transfer reaction. On reaction with iron(III), ferulic and sinapic acids undergo an electron transfer without the prior formation of any complex. There was no evidence of electron transfer occurring in the complex formed when iron(III) is reacted with naringin. Rate constants for k1 (formation) and k(-1) (dissociation) have been evaluated for the complex formation reactions of [Fe(H2O)6(OH)]2+ with caffeic acid, chlorogenic acid and naringin. Analysis of the kinetic data yielded stability constants, equilibrium constants for protonation of the iron(III) chlorogenic acid complex initially formed, together with the rate constants for complex decomposition through intramolecular electron transfers and in the case of caffeic acid and chlorogenic acid, rate constants for the iron(III) assisted decomposition of the initial complex formed. Some of the suggested mechanisms and calculated rate constants are validated by calculations carried out using global analysis of time dependent spectra.     

The kinetics and mechanisms of the reactions of iron(III) with quercetin and morin

The kinetics and mechanisms of the reactions of a pseudo-first order excess of iron(III) with the flavonoids quercetin and morin have been investigated in aqueous solution at 25 degrees C and an ionic strength of 0.5M. Mechanisms have been proposed which account satisfactorily for the kinetic data. The data are consistent with a mechanism in which the metal:ligand complex formed initially on reaction of iron(III) with the ligand subsequently decomposes through an electron transfer step. Morin forms a 1:1 metal:ligand complex while quercetin forms a 2:1 metal:ligand complex. Both ligands showed evidence for the involvement of the iron hydroxo dimer Fe2(OH)2(4+) in the complex formation reaction at the hydroxy-carbonyl moiety. The iron(III) assisted decomposition of the initial iron(III) complex formed was also investigated and the rate constants evaluated. Both the complex formation and subsequent electron transfer reactions of iron(III) with these ligands were monitored using UV-visible spectrophotometry. All of the suggested mechanisms and calculated rate constants are supported by calculations carried out using global analysis of time dependant spectra.     

Release of iron from ferritin molecules and their iron-cores by 3-hydroxypyridinone chelators in vitro

Ferritin molecules contain 24 subunits forming a shell around an inorganic iron-core. Release of iron(III) from ferritin and its isolated iron-cores by a series of hydroxypyridinone chelators with high affinities for iron(III) has been compared. The results collectively suggest that the chelators act by penetrating the protein shell and interacting directly with the iron-core in ferritin. Iron(III) is probably removed bound to a single ligand, but once outside the protein shell, the trihydroxypyridinone iron(III) complex predominates. The order of effectiveness of a group of pyridinones found for iron removal from ferritin molecules in solution differs from that obtained with hepatocytes in culture or with whole animals, where membrane solubility and other factors may modulate the response.     

Synthesis of 2-amido-3-hydroxypyridin-4(1H)-ones: novel iron chelators with enhanced pFe3+ values

The synthesis of a range of 2-amido-3-hydroxypyridin-4-ones as bidentate iron(III) chelators with potential for oral administration is described. The pKa values of the ligands together with the stability constants of their iron(III) complexes have been determined. Results indicate that the introduction of an amido substituent at the 2-position leads to an appreciable enhancement of the pFe3+ values. The ability of these novel 3-hydroxypyridin-4-ones to facilitate the iron excretion in bile was investigated using a 59Fe-ferritin loaded rat model. The optimal effect was observed with the N-methyl amido derivative 15b, which has an associated pFe3+ value of 21.7, more than two orders of magnitude higher than that of deferiprone (1,2-dimethyl-3-hydroxypyridin-4-one) 1a (pFe3+ = 19.4). Dose response studies suggest that chelators with high pFe3+ values scavenge iron more effectively at lower doses when compared with simple dialkyl substituted hydroxypyridinones.     

The kinetics and mechanisms of the complex formation and antioxidant behaviour of the polyphenols EGCg and ECG with iron(III)

(-)-Epigallocatechin-gallate ((-)-EGCg) and (-)-epicatechin-gallate ((-)-ECG) are important antioxidants which are found in green tea. The kinetics and mechanisms of the reactions of a pseudo-first order excess of iron(III) with EGCg and ECG have been investigated in aqueous solution at 25 degrees C and an ionic strength of 0.5M NaClO(4). Mechanisms have been proposed which account satisfactorily for the kinetic data. These are consistent with a mechanism in which the 2:1 metal:ligand complex initially formed on reaction of iron(III) with the ligand subsequently decomposes in an electron transfer step. Complex formation takes place at two separate binding sites via coupled reactions. Rate constants of 4.28(+/-0.06) x 10(6) M(-2) s(-1) and 2.83(+/-0.04) x 10(6) M(-2) s(-1) have been evaluated for the reaction of monohydroxy Fe(OH)2+ species with EGCg and ECG, respectively while rate constants for of 2.94(+/-0.4) x 10(4) M(-2) s(-1) and 2.41(+/-0.25) x 10(4) M(-2) s(-1) have been evaluated for the reaction of Fe3+ species with EGCg and ECG, respectively. The iron(III) assisted decomposition of the initial iron(III) complex formed was also investigated and the rate constants evaluated. Both the complex formation and subsequent electron transfer reactions of iron(III) with EGCg and ECG were monitored using UV-visible spectrophotometry. All of the suggested mechanisms and calculated rate constants are supported by calculations carried out using global analysis of time dependant spectra. The results obtained show that one molecule of either EGCg or EGC is capable of reducing up to four iron(III) species, a fact which is consistent with the powerful antioxidant properties of the ligands.     

Partition coefficients of the iron(III) complexes of pyridoxal isonicotinoyl hydrazone and its analogs and the correlation to iron chelation efficacy

Pyridoxal isonicotinoyl hydrazone and its analogs are orally effective Fe(III) chelators which show potential as drugs to treat iron overload disease. The present investigation describes the measurement of the partition coefficient of the apochelator and Fe(III) complex of 20 of these ligands. These measurements have been done to investigate the relationship between lipophilicity and the efficacy of iron chelation in rabbit reticulocytes loaded with non-heme ⁵⁹Fe. The results demonstrate a linear relationship between the partition coefficient (P) of the apochelator and its Fe(III) complex, and a simple equation has been derived relating these two parameters. Experimental data in the literature are in agreement with the equation. The relationship of the partition coefficients of the iron chelators and of their Fe(III) complexes to the effectiveness of the ligands in mobilizing iron in vitro and in vivo is also discussed.     

Iron chelators inhibit human platelet aggregation, thromboxane A2 synthesis and lipoxygenase activity

The iron chelators desferrioxamine and 1,2-dimethyl-3-hydroxypyrid-4-one (L1) inhibited human platelet aggregation in vitro as well as thromboxane A2 synthesis and conversion of arachidonate to lipoxygenase-derived products. Non-chelating compounds related to L1 were without effect on cyclooxygenase or lipoxygenase activity. Since both cyclooxygenase and lipoxygenase are iron-containing enzymes, it is suggested that the inhibition of platelet function by these iron chelators may be related to the removal or binding of iron associated with these enzymes. These iron chelators may therefore be of potential therapeutic value as platelet antiaggregatory agents and of possible use in the treatment of atherosclerotic and inflammatory joint diseases.     

The kinetics and mechanisms of the reactions of aluminium(III) with gallic acid, gallic acid methyl ester and adrenaline

The kinetics and mechanisms of the reactions of gallic acid, gallic acid methyl ester and adrenaline with aluminium(III) have been investigated in aqueous solution at 25 degrees C and an ionic strength of 0.5 M. A mechanism has been proposed which accounts satisfactorily for the kinetic data. This is consistent with a mechanism in which complex formation takes place almost exclusively by reaction of [Al(H2O)5OH]2+ with the ligands. [Al(H2O)5OH]2+ reacts with gallic acid, gallic acid methyl ester and adrenaline with rate constants of 1145, 1330 and 316 M(-1) s(-1) respectively. These data together with the equilibrium data enable the rate constants for reaction of [Al(H2O)6]3+ with both gallic acid and gallic acid methyl ester to be calculated. In view of the dissociative nature of water exchange on [Al(H2O)6]3+ and [Al(H2O)5(OH)]2+ the complex formation rate constants are discussed in terms of the Eigen-Wilkins-Tamm mechanism. The overall mechanisms have been validated using global analysis. The results are compared with previously published data on the complex formation reactions of aluminium(III). In addition, the rate constants and mechanisms for replacement of maltol by gallic acid methyl ester and diethylenetriaminepentaacetic acid (dtpa) have been investigated.     

Effects of deferasirox and deferiprone on cellular iron load in the human hepatoma cell line HepaRG

Two oral chelators, CP20 (deferiprone) and ICL670 (deferasirox), have been synthesized for the purpose of treating iron overload diseases, especially thalassemias. Given their antiproliferative effects resulting from the essential role played by iron in cell processes, such compounds might also be useful as anticancer agents. In the present study, we tested the impact of these two iron chelators on iron metabolism, in the HepaRG cell line which allowed us to study proliferating and differentiated hepatocytes. ICL670 uptake was greater than the CP20 uptake. The iron depletion induced by ICL670 in differentiated cells increased soluble transferrin receptor expression, decreased intracellular ferritin expression, inhibited ⁵⁵Fe (III) uptake, and reduced the hepatocyte concentration of the labile iron pool. In contrast, CP20 induced an unexpected slight increase in intracellular ferritin, which was amplified by iron-treated chelator exposure. CP20 also promoted Fe(III) uptake in differentiated HepaRG cells, thus leading to an increase of both the labile pool and storage forms of iron evaluated by calcein fluorescence and Perls staining, respectively. In acellular conditions, compared to CP20, iron removing ability from the calcein-Fe(III) complex was 40 times higher for ICL670. On the whole, biological responses of HepaRG cells to ICL670 treatment were characteristic of expected iron depletion. In contrast, the effects of CP20 suggest the potential involvement of this compound in the iron uptake from the external medium into the hepatocytes from the HepaRG cell line, therefore acting like a siderophore in this cell model.     

Synthesis, siderophore activity and iron(III) chelation chemistry of a novel mono-hydroxamate, bis-catecholate siderophore mimic: N(alpha),-N(epsilon)-Bis[2,3-dihydroxybenzoyl]-l-lysyl-(gamma-N-methyl-N-hydroxyamido)-L-glutamic acid

The synthesis and characterization of a novel tripodal mono-hydroxamate, bis catecholate siderophore mimic, N(alpha),-N(epsilon)-bis[2,3-dihydroxybenzoyl]-l-lysyl-(gamma-N-methyl-N-hydroxyamido)-l-glutamic acid (H(6)L), is described. The structure of H(6)L was established by 2D NMR and mass spectrometry. The chelation chemistry of H(6)L with respect to iron(III) is characterized in aqueous solution through determination of ligand pK(a) values and iron(III) binding constants using spectrophotometric and potentiometric titration techniques. Proton dependent iron(III)-ligand equilibrium constants were determined using a model based on the sequential protonation of the iron(III)-siderophore complex. These results were used to calculate the pH dependent speciation, the overall formation constant logbeta(110) (31.4) and pM value (18.3) for H(6)L with iron(III). The ability of H(6)L to deliver the essential nutrient iron to living cells is determined through growth promotion assays using various bacterial strains.     

Synthesis and antiproliferating activity of iron chelators of hydroxyamino-1,3,5-triazine family

We synthesized and evaluated new specific tridentate iron(III) chelators of 2,6-bis[hydroxyamino]-1,3,5-triazine (BHT) family for use in iron deprivation cancer therapy. Physical properties of BHT chelators are easily customizable allowing easy penetration through cellular membranes. Antiproliferative activity of new BHT chelators was studied on MDA-MB-231 and MiaPaCa cells and compared to a clinically available new oral iron chelator, deferasirox (DFX). The antiproliferative activity of new chelators was found to correlate with iron(III) chelation ability and some of analogs showed substantially higher antiproliferative activity than DFX.     

Recent achievements on siderophore production and application

Iron is the most abundant chemical element on Earth but its most common oxidation state is Fe(III) which presents a very low solubility under physiological conditions. During evolution, micro-organisms have developed sound strategies to acquire iron from both the environment and superior organisms, including direct uptake of iron ions from exogenous iron/heme sources and the synthesis of specialized Fe(III) chelators called siderophores. The present review paper aims at presenting and discussing the latest achievements in siderophore isolation and production, as well as novel applications of these molecules in therapies against iron-related diseases and in vaccines, and their application as antimicrobial agents and biosensors.     

Lability of iron at the dinuclear centres of ferritin studied by competition with four chelators

Ferritin molecules contain 24 polypeptide chains folded as four-helix bundles and arranged as a hollow shell capable of storing up to 4500 Fe(III) atoms. H chains contain ferroxidase centres which lie within the bundle, about 12?Å (1.2?nm) from the outside surface and 8?Å from the inner surface of the protein shell. Catalysis of Fe(II) oxidation precedes storage of Fe(III) as ferrihydrite, with the formation of μ-oxo-bridged Fe(III) dimers as intermediates. Factors influencing the movement of μ-oxo-bridged Fe(III) from the ferroxidase centre to the ferritin cavity are uncertain. Assistance by small chelators is one possibility. The aim of this investigation was to determine whether iron at the dinuclear centres of three ferritins (human H chain homopolymer, HuHF, the non-haem ferritin of Escherichia coli, EcFTN, and horse spleen ferritin, HoSF) is accessible to chelators. Forty-eight Fe(II) atoms/molecule were added to the apoferritins followed, 2?min later, by the addition of chelator (1,10-phenanthroline, 2,2-bipyridine, desferrioxamine or 3,4-dihydroxybenzaldehyde). Iron species were analysed by Mössbauer spectroscopy or visible absorbance. Competition between chelators and apoferritin for Fe(II) was also investigated. The main conclusions of the study are that: (1) dinuclear iron and iron in small iron-cores in HuHF and EcFTN is mobilisable by all four chelators; (2) the chelators penetrate the shell; (3) 3,4-dihydroxybenzaldehyde is the most efficient in mobilising Fe(III) but the least successful in competing for Fe(II); (4) Fe(III) is more readily released from EcFTN than from HuHF; (5) 2,2′-bipyridine aids the movement of Fe(III) from ferroxidase centre to core.     

Iron chelators can protect against oxidative stress through ferryl heme reduction

Iron chelators such as desferrioxamine have been shown to ameliorate oxidative damage in vivo. The mechanism of this therapeutic action under non-iron-overload conditions is, however, complex, as desferrioxamine has properties that can impact on oxidative damage independent of its capacity to act as an iron chelator. Desferrioxamine can act as a reducing agent to remove cytotoxic ferryl myoglobin and hemoglobin and has recently been shown to prevent the formation of a highly cytotoxic heme-to-protein cross-linked derivative of myoglobin. In this study we have examined the effects of a wide range of iron chelators, including the clinically used hydroxypyridinone CP20 (deferriprone), on the stability of ferryl myoglobin and on the formation of heme-to-protein cross-linking. We show that all hydroxypyridinones, as well as many other iron chelators, are efficient reducing agents of ferryl myoglobin. These compounds are also effective at preventing the formation of cytotoxic derivatives of myoglobin such as heme-to-protein cross-linking. These results show that the use of iron chelators in vivo may ameliorate oxidative damage under conditions of non-iron overload by at least two mechanisms. The antioxidant effects of chelators in vivo cannot, therefore, be attributed solely to iron chelation.     

N-hydroxyguanidines as new heme ligands: UV-visible, EPR, and resonance Raman studies of the interaction of various compounds bearing a C=NOH function with microperoxidase-8

Interaction between microperoxidase-8 (MP8), a water-soluble hemeprotein model, and a wide range of N-aryl and N-alkyl N'-hydroxyguanidines and related compounds has been investigated using UV-visible, EPR, and resonance Raman spectroscopies. All the N-hydroxyguanidines studied bind to the ferric form of MP8 with formation of stable low-spin iron(III) complexes characterized by absorption maxima at 405, 535, and 560 nm. The complex obtained with N-(4-methoxyphenyl) N'-hydroxyguanidine exhibits EPR g-values at 2.55, 2.26, and 1.86. The resonance Raman (RR) spectrum of this complex is also in agreement with an hexacoordinated low-spin iron(III) structure. The dissociation constants (K(s)) of the MP8 complexes with mono- and disubstituted N-hydroxyguanidines vary between 15 and 160 microM at pH 7.4. Amidoximes also form low-spin iron(III) complexes of MP8, although with much larger dissociation constants. Under the same conditions, ketoximes, aldoximes, methoxyguanidines, and guanidines completely fail to form such complexes with MP8. The K(s) values of the MP8-N-hydroxyguanidine complexes decrease as the pH of the solution is increased, and the affinity of the N-hydroxyguanidines toward MP8 increases with the pK(a) of these ligands. Altogether these results show that compounds involving a -C(NHR)=NOH moiety act as good ligands of MP8-Fe(III) with an affinity that depends on the electron-richness of this moiety. The analysis of the EPR spectrum of the MP8-N-hydroxyguanidine complexes according to Taylor's equations shows a strong axial distortion of the iron, typical of those observed for hexacoordinated heme-Fe(III) complexes with at least one pi donor axial ligand (HO(-), RO(-), or RS(-)). These data strongly suggest that N-hydroxyguanidines bind to MP8 iron via their oxygen atom after deprotonation or weakening of their O-H bond. It thus seems that N-hydroxyguanidines could constitute a new class of strong ligands for hemeproteins and iron(III)-porphyrins.     

Effects of deferrioxamine on iron-catalyzed lipid peroxidation.

The kinetics of iron binding by deferrioxamine B mesylate and the ramifications of this process upon iron-catalyzed lipid peroxidation were assessed. The relative rates of Fe(III) binding by deferrioxamine varied for the chelators tested as follows: ADP greater than AMP greater than citrate greater than histidine greater than EDTA. The addition of a fivefold molar excess of deferrioxamine to that of Fe(III) did not result in complete binding (within 10 min) for any of the Fe(III) chelates tested except ADP:Fe(III). The rates of Fe(III) binding by deferrioxamine were greater at lower pH and when the competing chelator concentration was high in relationship to iron. The relatively slow binding of Fe(III) by deferrioxamine also affected lipid peroxidation, an iron-dependent process. The addition of deferrioxamine to an ascorbate- and ADP:Fe(III)-dependent lipid peroxidation system resulted in a time-dependent inhibition or stimulation of malondialdehyde formation (i.e., lipid peroxidation), depending on the ratio of deferrioxamine to iron. Converse to Fe(III), the rates of Fe(II) binding by deferrioxamine from the chelators tested above were rapid and complete (within 1 min), and resulted in the oxidation of Fe(II) to Fe(III). Lipid peroxidation dependent on Fe(II) autoxidation was stimulated by the addition of deferrioxamine. Malondialdehyde formation in this system was inhibited by the addition of catalase, and a similar extent of lipid peroxidation was achieved by substituting hydrogen peroxide for deferrioxamine. Collectively, these results suggest that the kinetics of Fe(III) binding by deferrioxamine is a slow, variable process, whereas Fe(II) binding is considerably faster. The binding of either valence of iron by deferrioxamine may result in variable effects on iron-catalyzed processes, such as lipid peroxidation, either via slow binding of Fe(III) or the rapid binding of Fe(II) with concomitant Fe(II) oxidation.     

Metal binding by pyridine-2,6-bis(monothiocarboxylic acid), a biochelator produced by Pseudomonas stutzeri and Pseudomonas putida

Pyridine-2,6-bis(monothiocarboxylic acid) (pdtc),a natural metal chelator produced by Pseudomonas stutzeri and Pseudomonas putidathat promotes the degradation of carbon tetrachloride, was synthesized and studiedby potentiometric and spectrophotometric techniques. The first two stepwise protonationconstants (pK) for successive proton addition to pdtc were found to be 5.48 and2.58. The third stepwise protonation constant was estimated to be 1.3. The stability (affinity)constants for iron(III), nickel(II), and cobalt(III) were determined by potentiometric orspectrophotometric titration. The results show that pdtc has strong affinity for Fe(III)and comparable affinities for various other metals. The stability constants (log K) are 33.93 for Co(pdtc)₂ ^1-; 33.36 for Fe(pdtc)₂ ^1-; and 33.28 for Ni(pdtc)₂ ^2-. These protonationconstants and high affinity constants show that over a physiological pH range theferric pdtc complex has one of the highest effective stability constants for ironbinding among known bacterial chelators.     

Characterization of Fe(III) sequestration by an analog of the cytotoxic siderophore brasilibactin A: implications for the iron transport mechanism in mycobacteria

Mycobacteria such as M. tuberculosis represent a significant health concern throughout much of the developing world. In mycobacteria and other pathogenic bacteria, an important virulence factor is the ability of the bacterium to obtain iron from its host. One means of obtaining iron is through the use of siderophores. Brasilibactin A is a membrane bound siderophore produced by Nocardia brasiliensis with structural similarity to the mycobactin class of siderophore in mycobacteria. A characterization of the protonation constants and Fe(III) affinity of a water soluble Brasilibactin A analog (Bbtan) has been performed. Using protonation constants and competition with EDTA, the stability constant of the 1?:?1 Fe(III)-Bbtan complex was found to be log β(110) = 26.96. The pFe of Bbtan is 22.73, somewhat low for a proposed siderophore molecule. The redox potential of the Fe-Bbtan complex was found to be -300 mV vs. NHE, very high for an iron-siderophore complex. The combination of relatively low complex stability and ease of iron reduction may play a crucial role in the mechanism of mycobactin siderophore-mediated iron uptake in mycobacteria and related organisms.     

Role of iron chelators in growth-promoting effect on mouse hybridoma cells in a chemically defined medium

Summary The role of various iron chelators on the multiplication of mouse hybridoma cells in an albumin-free, transferrin-deficient defined medium was investigated. Fe(III)-dihydroxyethylglycine, Fe(III)-glycylglycine, Fe(III)-ethylenediamine-N,N′-dipropionic acid, or Fe(III)-iminodiacetic acid supported the excellent growth of the cells. In addition, the growth of the iron-starved cells, which had been preincubated in a protein-, iron- and chelator-free defined medium, restored rapidly when the medium was supplemented with holotransfeerrin, ferric iron, and chelator compared to that when supplemented with holotransferin, but without iron and chelator. The results suggest that such chelators modulate a progression of transferrn cycle in the presence of transferin and ferric iron. An alternative explantation is that there is a decrease in generation of iron-catalyzed free radicals.     

The kinetics and mechanisms of the reaction of iron(III) with gallic acid, gallic acid methyl ester and catechin.

The kinetics and mechanisms of the reactions of a number of pyrogallol-based ligands with iron(III) have been investigated in aqueous solution at 25 degrees C and ionic strength 0.5 M NaClO(4). Mechanisms have been proposed which account satisfactorily for the kinetic data. These are generally consistent with a mechanism in which the 1:1 complex that is formed initially when the metal reacts with the ligand subsequently decays through an electron transfer reaction. There was also some evidence for the formation of a 1:2 ligand-to-metal complex at higher pH values. The kinetics of complex formation were investigated with either the ligand or metal in pseudo-first-order excess. Rate constants for k(1) of 2.83(+/-0.09)x10(3), 1.75(+/-0.045)x10(3) and 3300(+/-200) M(-1) s(-1) and k(-1) of 20(+/-6.0), 35(+/-13) and 25+/-7.6 M(-1) s(-1) have been evaluated for the reaction of Fe(OH)(2+) with gallic acid, gallic acid methyl ester and catechin, respectively. The stability constant of each [Fe(L)](+) complex has been calculated from the kinetic data. The iron(III) assisted decomposition of the initial iron(III) complex formed was investigated. Analysis of the kinetic data yielded both the equilibrium constants for protonation of the iron(III) complexes initially formed together with the rate constants for the intramolecular electron transfers for gallic acid and gallic acid methyl ester. All of the suggested mechanisms and calculated rate constants are supported by calculations carried out using global analysis of time-dependent spectra.