Ferric ion sequestering agents: kinetics of iron release from ferritin to catechoylamides

Ascorbate and ferritin interactions: Consequences for iron release in vitro and in vivo and implications for inflammation

This review discusses the chemical mechanisms of ascorbate-dependent reduction and solubilization of ferritin's ferric iron core and subsequent release of ferrous iron. The process is accelerated by low concentrations of Fe(II) that increase ferritin's intrinsic ascorbate oxidase activity, hence increasing the rate of ascorbate radical formation. These increased rates of ascorbate oxidation provide reducing equivalents (electrons) to ferritin's core and speed the core reduction rates with subsequent solubilization and release of Fe(II). Ascorbate-dependent solubilization of ferritin's iron core has consequences relating to the interpretation of ⁵⁹Fe uptake sourced from ⁵⁹Fe-lebelled holotransferrin into ferritin. Ascorbate-dependent reduction of the ferritin core iron solubility increases the size of ferritin's iron exchangeable pool and hence the rate and amount of exchange uptake of ⁵⁹Fe into ferritin, whilst simultaneously increasing net iron release rate from ferritin. This may rationalize the inconsistency that ascorbate apparently stabilizes ⁵⁹Fe ferritin and retards lysosomal ferritinolysis and whole cell ⁵⁹Fe release, whilst paradoxically increasing the rate of net iron release from ferritin. This capacity of ascorbate and iron to synergise ferritin iron release has pathological significance, as it lowers the concentration at which ascorbate activates ferritin's iron release to within the physiological range (50-250 μM). These effects have relevance to inflammatory pathology and to the pro-oxidant effects of ascorbate in cancer therapy and cell death by ferroptosis.

Decorporation of Iron Metal Using Dialdehyde Cellulose-Deferoxamine Microcarrier

Deferoxamine iron chelator has a limited therapeutic index due to rapid clearance from blood and possesses dose-limiting toxicity. Therefore, an intravenous deferoxamine delivery system based on dialdehyde cellulose (DAC) polymer was developed and its efficacy and toxicity were tested in iron-overloaded animals. The amino groups of deferoxamine were conjugated to free aldehyde moieties of dialdehyde cellulose via Schiff base reaction to form dialdehyde cellulose-deferoxamine (DAC-DFO) conjugate and characterized by Fourier transform infrared spectrophotometer, scanning electron microscope, and X-ray diffraction. The toxicity of prepared formulation was analyzed by XTT cell viability assay and LD50 study in mice. The change in serum iron levels, after intravenous administration of formulation, was observed in iron-overloaded rats. The DAC-DFO conjugate was tagged with Tc-99m to study the blood kinetics and observe change in blood circulation time. DAC-DFO conjugate was dispersible in water at concentration ∼75 mg/ml. In vitro cytotoxicity assay and LD₅₀ study in mice indicated significantly enhanced safety of covalently bound deferoxamine (at >1000 mg/kg body weight compared to free drug at ∼270 mg/kg dose). A preliminary scintigraphy imaging and blood clearance study, with technetium-99m, indicated prolonged circulation of conjugated DFO in rabbit blood. A single dose of formulation injected into iron overloaded animals was found to maintain the normal serum iron levels until 10 days. The polymeric conjugate was effective in maintaining normal serum iron levels until 10 days at a dose of 100 mg/kg body weight.

Iron Binding and Iron Removal Efficiency of Desferrioxamine Based Polymeric Iron Chelators: Influence of Molecular Size and Chelator Density

Desferrioxamine (DFO) is a clinically approved, high affinity iron chelator used for the treatment of iron overload. Due to its short half-life and toxicity, DFO is administered for 8-12 h per day, 5-7 d per week. In this manuscript, the influence of molecular properties of hyperbranched polyglycerol (HPG)-DFO conjugates on their iron binding by isothermal titration calorimetry, iron removal efficiency from ferritin in presence and absence of a low molecular weight (MW) iron chelator, and protection against iron mediated oxidation of proteins is reported. The iron binding properties of HPG-DFO are slightly altered with size and DFO density of conjugates. The lower MW conjugate shows greater iron removal efficiency at room temperature, however, the efficacy of high MW conjugates increases at physiological temperature. The iron removal from ferritin by HPG-DFO conjugates increases significantly in presence of a low MW chelator, suggesting the potential of combination therapy. The molecular properties of the polymer scaffold also have influence on the prevention of iron mediated oxidation of proteins by the conjugates. The results therefore help to define the iron binding thermodynamics of HPG-DFO and their dependence on MW, and can be extended to improve the general understanding of polymeric chelator-iron interactions in situ.

Identification and characterization of a novel-type ferric siderophore reductase from a gram-positive extremophile

Iron limitation is one major constraint of microbial life, and a plethora of microbes use siderophores for high affinity iron acquisition. Because specific enzymes for reductive iron release in gram-positives are not known, we searched Firmicute genomes and found a novel association pattern of putative ferric siderophore reductases and uptake genes. The reductase from the schizokinen-producing alkaliphile Bacillus halodurans was found to cluster with a ferric citrate-hydroxamate uptake system and to catalyze iron release efficiently from Fe[III]-dicitrate, Fe[III]-schizokinen, Fe[III]-aerobactin, and ferrichrome. The gene was hence named fchR for ferric citrate and hydroxamate reductase. The tightly bound [2Fe-2S] cofactor of FchR was identified by UV-visible, EPR, CD spectroscopy, and mass spectrometry. Iron release kinetics were determined with several substrates by using ferredoxin as electron donor. Catalytic efficiencies were strongly enhanced in the presence of an iron-sulfur scaffold protein scavenging the released ferrous iron. Competitive inhibition of FchR was observed with Ga(III)-charged siderophores with K(i) values in the micromolar range. The principal catalytic mechanism was found to couple increasing K(m) and K(D) values of substrate binding with increasing k(cat) values, resulting in high catalytic efficiencies over a wide redox range. Physiologically, a chromosomal fchR deletion led to strongly impaired growth during iron limitation even in the presence of ferric siderophores. Inductively coupled plasma-MS analysis of ΔfchR revealed intracellular iron accumulation, indicating that the ferric substrates were not efficiently metabolized. We further show that FchR can be efficiently inhibited by redox-inert siderophore mimics in vivo, suggesting that substrate-specific ferric siderophore reductases may present future targets for microbial pathogen control.

The power plant of the cell is also a smithy: the emerging role of mitochondria in cellular iron homeostasis

Iron is required for a barrage of essential biochemical functions in virtually every species of life. Perturbation of the availability or utilization of iron in these functions or disruption of other components along iron-requiring pathways can not only lead to cellular/organismal insufficiency of respective biochemical end-products but also result in a broad derangement of iron homeostasis. This is largely because of the elaborate regulatory mechanisms that connect cellular iron utilization with uptake and distribution. Such mechanisms are necessitated by the 'double-edged' nature of the metal, whose very property as a useful biological catalyst also makes it able to generate highly toxic compounds. Since the majority of iron is dispatched onto a functional course by mitochondria-localized pathways, these organelles are in an ideal position within the cellular iron anabolic pathways to be a central site for regulation of iron homeostasis. The goal of this article is to provide an overview of how mitochondria acquire and use iron and examine the ramifications of disturbances in these processes on overall cellular iron homeostasis.

Determination of the chelatable iron pool of single intact cells by laser scanning microscopy

We have previously established a method of detecting intracellular chelatable iron in viable cells based on digital fluorescence microscopy. To quantify cellular chelatable iron, it was crucial to determine the intracellular indicator concentration. In the present study, we therefore adapted the method to confocal laser scanning microscopy, which should allow the determination of the indicator concentration on the single-cell level. The fluorescent heavy-metal indicator phen green SK (PG SK), the fluorescence of which is quenched by iron, was loaded into cultured rat hepatocytes. The hepatocellular fluorescence increased when cellular chelatable iron available to PG SK was removed from the probe by an excess of the membrane-permeable transition metal chelator 2,2'-dipyridyl (2, 2'-DPD, 5 mM). We optimized the scanning parameters for quantitatively recording changes in fluorescence and determined individual intracellular PG SK concentrations from the unquenched cellular fluorescence (after 2,2'-DPD) compared with PG SK standards in a "cytosolic" medium. An ex situ calibration method based on laser scanning microscopy was set up to determine the concentration of cellular chelatable iron from the increase of PG SK fluorescence after addition of 2,2'-DPD (5 mM). As the stoichiometry of the PG SK:Fe(2+) complex was 3:1 as long as PG SK was not limiting, cellular chelatable iron was calculated directly from absolute changes in cellular fluorescence. Using this method, we found 2.5 +/- 2.2 microM chelatable iron in hepatocytes. This method makes it possible to determine the pool of chelatable iron in single vital cells independently of cellular differences (e.g., dye loading, cell volume) in heterogeneous cell populations.

Mechanism of testicular atrophy induced by di-n-butyl phthalate in rats. Part 4. Changes in the activity of succinate dehydrogenase and the levels of transferrin and ferritin in the Sertoli and germ cells

A single oral dose of di-n-butyl phthalate (DBP) to male rats caused a sloughing of the germ cells at 6 h both with a decrease in the activity of succinate dehydrogenase (SDH) in the Sertoli cells and in the Sertoli-germ connection and with an increase in the activity of lactate dehydrogenase (LDH) in the germ cells. Increases in transferrin (Tf) concentrations were observed in the Sertoli cells, Sertoli-germ connection, epididymis-ductus deferens and liver of rats. Decreases in Tf and ferritin (Ft) levels were observed in the seminal vesicle and seminiferous lumen, respectively. An increase in favin adenine dinucleotide (FAD) level was found in the interstitial cells.

Monitoring of iron(III) removal from biological sources using a fluorescent siderophore

We present here the physicochemical and biochemical properties of NBD-DFO, the 7-nitrobenz-2-oxa-1,3-diazole (NBD) derivative of the siderophore, desferrioxamine B (DFO) (Lytton et al., Mol. Pharmacol. 40, 584, 1991). Modification of DFO at its terminal amine renders it more lipophilic, imparts to it fluorescent properties, and is conservative of the high-affinity iron(III) binding capacity. NBD-DFO partitions readily from aqueous solution into n-octanol (Pcoeff = 5) and displays solvent-induced shifts in absorption and fluorescence spectra. The relative quantum yield of the probe's fluorescence increases over a 10-fold range with decreasing dielectric constant of the solvent. Fluorescence is quenched upon binding of iron(III) to the probe. We demonstrate here the application of NBD-DFO for the specific detection and monitoring of iron (III) in solutions and iron(III) mobilization from cells. Interactions between fluorescent siderophore and the ferriproteins ferritin and transferrin were monitored under physiological conditions. Iron removal from ferritin was evident by the demonstrable quenching of NBD-DFO fluorescence by scavenged iron(III). Quantitation of iron sequestered from cells by NBD-DFO or from other siderophore-iron(III) complexes was accomplished by dissociation of NBD-DFO-Fe complex by acidification and addition of excess ethylenediamin-etetraacetic acid. The sensitivity of the method and the iron specificity indicate its potential for monitoring chelatable iron under conditions of iron-mediated cell damage, iron overload, and diseases of iron imbalance such as malaria.

Haem binding to horse spleen ferritin and its effect on the rate of iron release

Horse spleen ferritin is shown to bind haem to generate a haemoprotein, named herein haemoferritin. A total of 14-16 haem molecules are bound per 24 subunits of ferritin. The molecular mass of the non-haem-iron-free haemoferritin has been determined to be 420 +/- 40 kDa, indicating that haem binding does not lead to dissociation of the 24 subunits that comprise the ferritin molecule. The functional role of the bound haem has been investigated with respect to the release of iron from the non-haem iron core. The bound haem is shown to increase the rate of iron release in a reductive assay system. In the absence of haem the rate of iron release depends on the redox potential of the reductant, but in the presence of haem the rate is largely independent of the reductant and is faster than the rate for the haem-free ferritin. These data haem, but in the presence of haem electron transfer is not rate-limiting.

The mobilization of ferritin iron by liver cytosol. A comparison of xanthine and NADH as reducing substrates

Considerable evidence suggests that the release of iron from ferritin is a reductive process. A role in this process has been proposed for two hepatic enzymes, namely xanthine oxidoreductase and an NADH oxidoreductase. The abilities of xanthine and NADH to serve as a source of reducing power for the enzyme-mediated release of ferritin iron (ferrireductase activity) were compared with turkey liver and rat liver homogenates. The maximal velocity (Vmax.) for the reaction with NADH was 50 times greater than with xanthine; however, the substrate concentration required to achieve half-maximal velocity (Km) was 1000 times less with xanthine than with NADH. NADPH could be substituted for NADH with little loss in activity. Dicoumarol did not inhibit the reaction with NADH or NADPH, demonstrating that the ferrireductase activity with those substrates was not the result of the liver enzyme 'DT-diaphorase' [NAD(P)H dehydrogenase (quinone)]. A flavin nucleotide was required for ferrireductase activity with rat and turkey liver cytosol when xanthine, NADH or NADPH was used as the reducing substrate. FMN yielded twice the activity with NADH or NADPH, whereas FAD was twice as effective with xanthine as substrate. Kinetic comparisons, differences in lability and partial chromatographic resolution of the ferrireductase activities with the two types of reducing substrates strongly indicate that the ferrireductase activities with xanthine and NADH are catalysed by separate enzyme systems contained in liver cytosol. Complete inhibition by allopurinol of the ferrireductase activity endogenous to undialysed liver cytosol preparations and the ability of xanthine to restore equivalent activity to dialysed preparations indicate that the source of reducing power for the endogenous activity is xanthine. These studies suggest that xanthine, NADH or NADPH can serve as a source of reducing power for the enzyme-mediated reduction of ferritin iron, with a flavin nucleotide serving as the shuttle of electrons from the enzymes to the ferritin iron.

Molecular aspects of the removal of ferritin-bound iron by DL-dihydrolipoate

The removal of ferritin-bound iron by the physiologic dithiol DL-dihydrolipoate was studied over the pH range 5.5-9.0. A novel method was devised for the determination of iron removal, making it possible to study the actual release of iron from ferritin, regardless of the oxidation state or complexation form. The overall iron-removal process appears to depend upon a balance between the deprotonation of the dithiol and the protolytic dissolution of the iron core inside the ferritin molecule. The amount of iron removed at equilibrium increases with the pH, at any of the dihydrolipoate/ferritin iron ratios tested. The formation of the binuclear iron-dithiol complex [Fe2(dihydrolipoate)3]-3 is not strictly required for iron mobilization, but it seems to affect the efficiency of the dithiol in iron mobilization by providing a stable complexation form for the released iron outside the ferritin protein shell. Comparison of the release of ferritin-bound iron by free and immobilized dihydrolipoate indicates that mobility of the dithiol is mandatory for the removal process to take place.

Reductive release of ferritin iron: a kinetic assay

Ferritin iron release, a process of considerable interest in biology and medicine, occurs most readily in the presence of reducing agents. Here is described a kinetic assay for measuring the rate of ferritin iron removal promoted by various reductants. The new procedure uses ferrozine as a chromophoric, high-affinity chelator for the product, Fe(II). The initial rate of iron release is quantified by continuous spectrophotometric measurement of the Fe(ferrozine)2/3+ complex which absorbs maximally at 562 nm. The initial rate of iron mobilization is dependent on reductant concentration, but not on the concentration of the chelating agent, ferrozine. Saturation kinetics are observed for all reductants, including dihydroxyfumarate, cysteine, caffeic acid, ascorbate, and glutathione. Superoxide dismutase greatly inhibits ferritin iron release by ascorbate, but has little or no effect on the reducing action of dihydroxyfumarate, cysteine, caffeic acid, or glutathione. Ferritin iron removal by dihydroxyfumarate was inhibited by various metal ions. This new assay may be used for rapid screening of test compounds for treatment of iron overload and for investigation of the mechanistic aspects of ferritin iron reduction.

Reduction and release of ferritin iron by plant phenolics

The reductive release of ferritin iron by several naturally occurring o-diphenols was studied. The initial rate of iron release was quantified by spectrophotometric measurement of the Fe(ferrozine)3(2+) complex, which absorbs maximally at 562 nm. The initial rate of iron release was dependent upon o-diphenol concentration, but not on the concentration of the chromophoric chelating agent, ferrozine, Stoichiometric measurements resulted in a ratio of 2Fe(II) released per molecule of o-diphenol. The series of o-diphenols studied included, caffeic acid, chlorogenic acid, dihydrocaffeic acid, 3,4-dihydroxybenzoic acid, and several analogs. These reductants represent an oxidation reduction potential range of 0.38 volts. A direct correlation between reducing power of the o-diphenols and rate of ferritin iron release was observed. Superoxide dismutase, catalase, mannitol, or general radical traps had no effect on the rate of iron removal; however, EDTA and oxalate inhibited iron release. A mechanism for ferritin iron reduction and release by o-diphenols consistent with the experimental observations is discussed.

Superoxide ion as a primary reductant in ascorbate-mediated ferritin iron release

The mechanism of ascorbate-promoted ferritin iron reduction under aerobic conditions was studied. The initial rate of ferritin iron release was determined by spectrophotometric measurement of the Fe(ferrozine)3(2+) complex which absorbs at 562 nm. Variation of the initial ferrozine concentration had no influence on the rate of iron release suggesting that ferrozine does not participate in the rate-determining step. Experimental measurements of the initial rate of iron release as a function of ascorbate concentration resulted in saturation kinetics with Vmax = 2.0 X 10(-7) M.min-1 and KM = 1.3 X 10(-3) M. The effect of pH was quite pronounced with a maximal rate of iron release at pH 7.0. Stoichiometric measurements on the reaction mixture, with added catalase, resulted in a ratio of 2 Fe(II) released per ascorbate. Ascorbate-mediated iron release was inhibited 85% by superoxide dismutase, but 0% inhibition was noted with aposuperoxide dismutase. It is proposed that superoxide ion, generated during the iron-promoted oxidation of ascorbate, acts as a reductant of ferritin iron. A mechanism of ferritin iron release consistent with these experimental observations is discussed.

Comparative study of iron mobilization from haemosiderin, ferritin and iron(III) precipitates by chelators

The heteroaromatic chelators 1,2-dimethyl-3-hydroxypyrid-4-one, maltol, mimosine and 2,4-dihydroxypyridine-N-oxide, have been shown to mobilize iron from human spleen haemosiderin, ferritin and also from iron(III) precipitates, all containing equal amounts of iron, at physiological pH. In the case of almost every chelator, the least-solubilized polynuclear iron form was ferritin, whereas haemosiderin was more soluble and the iron(III) precipitate the most soluble of all. Most of the chelators were more efficient than desferrioxamine at releasing iron from ferritin, but less efficient in the removal of iron from the other two polynuclear iron forms. It is suggested that the chelator differences in iron mobilization may be related to variations in the chelator molecular structure, the protein structure, iron forms and in the mechanism of iron release.

Removal of ferritin-bound iron by DL-dihydrolipoate and DL-dihydrolipoamide

The naturally occurring dithiols DL-dihydrolipoate and DL-dihydrolipoamide were tested for their ability in the removal of ferritin-bound iron. Both compounds remove the iron stored inside the protein by complexing it in the ferric form. The iron can be reduced to the ferrous form by excess dithiol, but this is not necessary for complete removal. Reaction is complete in few hours and, at molar ratios of chelator to metal higher than 10, more than 60% of the ferritin-bound iron was removed. The amount of iron stored in the ferritin molecule does not affect the rate and the yield of the removal reaction. The iron-removing ability of DL-dihydrolipoate was found to be identical to that of an equimolar solution of sodium dithionite, and to be pH-dependent. Results are discussed in terms of the molecular architecture of ferritin and of the chelators, and their possible physiological relevance is pointed out.

Iron mobilization from ferritin using alpha-oxohydroxy heteroaromatic chelators

Several alpha-oxohydroxy heteroaromatic chelators have been shown to mobilize iron from horse spleen ferritin. Although the reactions were slow, taking up to 3 days to reach completion, the amounts of iron mobilized were higher than those reported for other chelators. These results increase the prospects for the clinical use of alpha-oxohydroxy chelators in the treatment of iron overload.

Reductive mobilisation of ferritin iron

The reductive mobilisation of iron from ferritin, the principal protein of iron storage, was studied. The kinetic characteristics of iron release by dithionite, thioglycollate, and dihydroriboflavin 5'-phosphate (FMNH2) were found to differ widely. The dependence on pH is most pronounced for the dithionite reduction which proceeds 100 times faster at pH 4 than at pH 7. The experimental data can be consistently explained in terms of specific interactions of products or educts with interfacial iron(III) hydroxide of the ferritin core. Surface complexes with the product sulfite are postulated in the dithionite reaction, and with the educt in the thioglycollate reaction. Iron(II) complexes with the radical anion FMN-. are suggested to be involved in the iron release by FMNH2. The mobilisation of iron by a series of thiols of different size and coordinative properties confirmed the importance of surface complex formation. No evidence was found for predominant effects of hindered shell penetration.

Transfer of ferritin-bound iron to adriamycin

Interactions of adriamycin with ferritin-bound iron have been investigated. It is demonstrated (i) that adriamycin stimulates an iron-dependent lipid peroxidation in submitochondrial particles in the presence of ferritin, and (ii) that incubation of adriamycin with ferritin results in a slow transfer of iron to adriamycin with formation of an adriamycin-iron complex. The results are discussed in relation to the possible role for intracellular iron in adriamycin toxicity.

Fate of oxygen during ferritin iron incorporation

The deposition of Fe(II) into ferritin using 18O2 as the oxidant was investigated. Only 3-4% of the oxygen atoms in the FeOOH core of ferritin were derived from the oxidant. This was true whether large (1200-1900 Fe/molecule) or small (220-240 Fe/molecule) amounts of iron were added to apoferritin or when iron was added to ferritin already containing 1000 Fe/molecule. Experiments using H218O in the solvent showed that nearly all of the oxygen atoms in the core were derived from solvent. The stoichiometry of the reaction was close to 2 Fe(II)/O2, instead of the expected value of 4 Fe(II)/O2. Reactions of 18O2 with Fe(II) in the absence of apoferritin had a similar 18O distribution and stoichiometry. Our results are most consistent with the crystal growth model of ferritin iron deposition.