Interaction between iron(II) and hydroxamic acids: oxidation of iron(II) to iron(III) by desferrioxamine B under anaerobic conditions

Interaction between iron(II) and acetohydroxamic acid (Aha), alpha-alaninehydroxamic acid (alpha-Alaha), beta-alaninehydroxamic acid (beta-Alaha), hexanedioic acid bis(3-hydroxycarbamoyl-methyl)amide (Dha) or desferrioxamine B (DFB) under anaerobic conditions was studied by pH-metric and UV-Visible spectrophotometric methods. The stability constants of complexes formed with Aha, alpha-Alaha, beta-Alaha and Dha were calculated and turned out to be much lower than those of the corresponding iron(II) complexes. Stability constants of the iron(II)-hydroxamate complexes are compared with those of other divalent 3d-block metal ions and the Irving-Williams series of stabilities was found to be observed. Above pH 4, in the reactions between iron(II) and desferrioxamine B, the oxidation of the metal ion to iron(III) by the ligand was found. The overall reaction that resulted in the formation of the tris-hydroxamato complex [Fe(HDFB)]+ and monoamide derivative of DFB at pH 6 is: 2Fe2+ + 3H4DFB+ = 2[Fe(HDFB)]+ + H3DFB-monoamide+ + H2O + 4H+. Based on these results, the conclusion is that desferrioxamine B can uptake iron in iron(III) form under anaerobic conditions.     

Kinetics and mechanism of iron exchange in hydroxamate siderophores: Catalysis of the iron(III) transfer from ferrioxamine B to ethylenediaminetetraacetic acid

The oxalate catalyzed iron(III) transfer from a trihydroxamate siderophore ferrioxamine B, [Fe(Hdfb)⁺], to ethylenediaminetetraacetic acid (H₄edta) has been studied spectro-photometrically in weakly acidic aqueous solutions at 298 K and a constant 2.0 M ionic strength maintained by NaClO₄. The results reveal that oxalate is a more efficient catalyst than the so far studied synthetic monohydroxamic acids. Any role of reduction of Fe(Hdfb)⁺ by oxalate in the catalysis has been rejected by the experimentally observed preservation of the oxalate concentration during the reaction time. Therefore, catalysis has been proposed to be a substitution based process. Under our experimental conditions Fe(Hdfb)⁺ is hexacoordinated and addition of oxalate results in the formation of Fe(H₂dfb)(C₂O₄), Fe(H₃dfb)(C₂O₄)⁻₂ and Fe(C₂O₄)³⁻₃. Therefore, catalysis was proposed to be accomplished by the intermediate formation of the ternary and tris(oxalato) complexes. All three complexes react with H₂edta²⁻ to form thermodynamically stable Fe(edta)⁻ as a final reaction product. Whereas the formation of the ternary complexes is fast enough to feature a pre-equilibrium process to the iron exchange reaction, the formation of Fe(C₂O₄)³⁻₃ is slow and is directly involved in the rate determining step of the Fe(edta)⁻ formation. Nonlinear dependencies of the rate constant on the oxalate and the proton concentrations have been observed and a four parallel path mechanism is proposed for the exchange reaction. The rate and equilibrium constants for the various reaction paths were determined from the kinetic and equilibrium study involving the desferrioxamine B- (H₄dfb⁺), oxalate- and proton-concentration variations. The observed proton catalysis was attributed to the fast monoprotonation of ferrioxamine B as well as of the oxalate ligand. The observed catalysis of iron dissociation from the siderophore has been discussed in view of its significance with respect to in vivo microbial iron transport.     

Fluorescence quenching and bonding properties of some hydroxamic acid derivatives by iron(III) and manganese(II)

Spectrophotometric investigations of highly fluorescent metal chelating molecules are of relevance due to their potential application in novel, selective fluorescence‐based sensors. Benzene and naphthalene chromophores are highly fluorescent while hydroxamic acids are widely used as ligands for complexation of transition metals. In order to develop fluorescence probes, several phenyl derivatives of N‐phenylbenzohydroxamic acid and an aminodihydroxamic acid linked with a naphthalene chromophore were synthesized and their selective ionophoric properties towards iron(III) and manganese(II) ions were investigated using fluorescence and absorption spectroscopy. Both methods confirm the formation of 1:1 and 1:2 complexes for iron(III) and a 1:1 complex for manganese(II). The complex that is formed depends on the concentration of the ligand and pH of the medium. The amino dihydroxamic acid exhibits a prominent selectivity towards iron(III) with a two‐step 1:1 and 1:2 quenching mechanism at pH 3 and towards manganese(II) with a 1:1 quenching mechanism at a probe concentration of 1 × 10^?5 mol dm^?3 at pH 9.5 The logarithm of overall formation constants of 1:1 and 1:2 complexes of iron(III) were estimated as 3.30 and 9.05, respectively. Copyright © 2008 John Wiley & Sons, Ltd.     

Kinetics and mechanism of electron transfer between meso-tetra sulphonated phenyl porphyrin iron(III)-apomyoglobin and Fe(EDTA)2- complexes

The kinetics of electron transfer between Fe(EDTA)2- and meso-tetra sulphonated phenyl porphyrin iron(III)-apomyoglobin have been studied by applying stopped-flow mixing and monitoring photometric changes at soret band (429 nm). The studies were carried out at pH's 6, 6.5, 7, 7.5, and 8 and at temperature between 10 and 40 degrees C. The mechanism proposed on the basis of the dependence of kobsd on Fe(EDTA)2- concentrations at various pH's, followed the rate equation: kobsd = ka[H+] + Kakb/[H+] + Ka.[Fe(EDTA)2-] The values of rate parameters calculated using a weighted non-linear least-squares analysis were: ka, 528 +/- 2 sec-1; kb, 25 +/- 1 sec-1; and Ka, 2.0 +/- 0.1 microM at 25 degrees C and 0.5 M sodium phosphate, and those of thermodynamic parameters calculated by the Eyring equation were: delta H*, 8.1 +/- 0.3 kcal mole-1 and delta S*, -23.4 +/- 1.1 eu at pH 7 and 0.5 M sodium phosphate.     

Towards bioreductively activated prodrugs: Fe(III) complexes of hydroxamic acids and the MMP inhibitor marimastat

Fe(III)-salen (N,N-bis(salicylidene)-ethane-1,2-diimine) complexes of simple hydroxamic acids and the MMP (matrix metalloproteinase) inhibitor marimastat have been evaluated as hypoxia activated drug carriers. The aceto- (aha), propion- (pha), benzohydroxamato (bha), and marimastat complexes were prepared and characterised by single crystal X-ray diffraction and electrochemical analysis. The hydroxamato ligands form a bidentate chelate to Fe(III) with the remaining octahedral coordination sites occupied by the tetradentate salen ligand. Bonding of the hydroxamato ligands is in the typical motif of the majority of Fe(III) complexes in the literature. The reduction potentials of the complexes are of the order of -1300 mV (vs ferrocene/ferrocenium) and show partial reversibility in the re-oxidation waveforms of the cyclic voltammetry scans. This suggests that the Fe-salen carrier system would provide a suitably redox inert framework yet would release the ligands at hypoxic tumour sites upon reduction to the more labile Fe(II) oxidation state. Furthermore, biological testing of the marimastat complex established that these carriers are stable in non-reducing biological environments and would serve to deliver MMP inhibitors to tumour sites intact.     

Reversion by Fe(III) of the inhibition by hydroxamic acids of the cyanide-Insensitive respiration in the yeast Saccharomycopsis lipolytica

The specific inhibitory effect of benzhydroxamic acid on the cyanide-insensitive respiration could be reversed in whole cells of the yeast Saccharomycopsis lipolytica, by addition of Fe(III), in a way suggesting a competition between the added iron and an enzyme-bound metallic ion, both central atoms for the ligand benzhydroxamic acid. The possibility that added metal ions modify the penetration of BHAM into the cells was ruled out. Co(II), Cu(II) and Al(III) could substitute for Fe(III). A linear relation between the concentration in added Fe(III) and the reversed respiration rate was observed. At a given cell concentration. the reversion by added Fe(III) of the inhibitory effect of benzhydroxamic acid on the alternative respiration appeared more related to the degree of inhibition rather than to the concentration in added inhibitor. Increasing cell concentrations required increasing amounts of Fe(III) to reach the same level of reversion. No reversal occurred at concentrations in added Fe(III) lower than 0.1 mM, whatever the benzhydroxamic concentration, the cell concentration or the yeast batch.     

Characterization of Mn(II) and Mn(III) binding capability of natural siderophores desferrioxamine B and desferricoprogen as well as model hydroxamic acids

Complexes formed between Mn(II) ion and acetohydroxamic acid (HAha), benzohydroxamic acid (HBha), N-methyl-acetohydroxamic acid (HMeAha), DFB model dihydroxamic acids (H₂(3,4-DIHA), H₂(3,3-DIHA), H₂(2,5-DIHA), H₂(2,5-H,H-DIHA), H₂(2,4-DIHA), H₂(2,3-DIHA)) and two trihydroxamate based natural siderophores, desferrioxamine B (H₄DFB) and desferricoprogen (H₃DFC) have been investigated under anaerobic condition (and some of them also under aerobic condition). The pH-potentiometric results showed the formation of well-defined complexes with moderate stability. Monohydroxamic acids not, but all of the dihydroxamic acids and trihydroxamic acids were able to hinder the hydrolysis of the metal ion up to pH ca. 11. Maximum three hydroxamates were found to coordinate to the Mn(II) ion, but presence of water molecule in the inner-sphere was also indicated by the corresponding relaxivity values even in the tris-chelated complexes. Moreover, prototropic exchange processes were found to increase the relaxation rate of the solvent water proton over the value of [Mn_aqua]²⁺ in the protonated Mn(II)-siderophore complexes at physiological pH. The much higher stability of Mn(III)-hydroxamate (especially tris-chelated) complexes compared to the corresponding Mn(II)-containing species results in a significantly decreased formal potential compared to the Mn(III)_aqua/Mn(II)_aqua system. As a result, air oxygen becomes an oxidizing agent for these manganese(II)-hydroxamate complexes above pH 7.5. The oxidation processes, followed by UV-Vis spectrophotometry, were found to be stoichiometric only in the case of the tris-chelated complexes of siderophores, which predominate above pH 9. ESI-MS provided support about the stoichiometry and cyclic-voltammetry was used to determine the stability constants for the tris-chelated complexes, [Mn(HDFB)]⁺ and [MnDFC].     

The reduction of hydroxamic acids with titanium(III) chloride: a tool for the characterization of siderophores

Hydroxamic acid siderophores were observed to be inactivated by exposure to titanium(III) chloride. To study the reaction, a series of eight model hydroxamic acids were prepared and reacted with titanium(III) chloride. The products were shown by ir and NMR comparisons with authentic compounds to be the corresponding amides. The reduction was found to require 2 mol of titanium(III) per mol of hydroxamic acid.     

A mechanistic study of ferrioxamine B reduction by the biological reducing agent ascorbate in the presence of an iron(II) chelator

The iron overload drug desferal (desferrioxamine B) forms the stable iron complex ferrioxamine B. The reduction potential of ferrioxamine B (E^o = −482 mV versus NHE pH 7) prohibits its reduction by biological reducing agents such as ascorbate, but it was found that the iron(II) chelator 2,2′-bipyridine (bipy) facilitates this reduction. Evidence is given to support the formation of a ternary complex between iron, bipy, and desferrioxamine B as the key step in facilitating the reduction. The equilibrium constant for the formation of the ternary complex was found to be 8.9 × 10⁷ and ternary complex formation is explained in terms of a three step mechanism. The mechanism for the reduction of ferrioxamine B is discussed in terms of rapidly established pre-equilibria which include ternary complex formation, ascorbic acid deprotonation, and encounter complex formation between ascorbate and the ternary complex. These equilibria are followed by rate limiting reduction of the ternary complex. Bipy was found to be a similar facilitator to sulfonated bathophenanthroline for the reduction of ferrioxamine B by ascorbate.     

Synthesis and characterization of a triazine dendrimer that sequesters iron(III) using 12 desferrioxamine B groups

The synthesis of a third generation triazine dendrimer, 1, containing multiple, iron-sequestering desferrioxamine B (DFO) groups is described. Benzoylation of the hydroxamic acid groups of DFO and formation of a reactive dichlorotriazine provide the intermediate for reaction with the second generation dendrimer displaying twelve amines. This strategy further generalizes the ‘functional monomer’ approach to generate biologically active triazine dendrimers. Dendrimer 1 is prepared in seven steps in 35% overall yield and displays 12 DFO groups making it 56% drug by weight. Spectrophotometric titrations (UV–vis) show that 1 sequesters iron(III) atoms with neither cooperativity nor significant interference from the dendrimer backbone. Evidence from NMR spectroscopy and mass spectrometry reveals a limitation to this functional monomer approach: trace amounts of O-to-N acyl migration from the protected hydroxamic acids to the amine-terminated dendrimer occurs during the coupling step leading to N-benzoylated dendrimers displaying fewer than 12 DFO groups.     

Stimulatory effect of phosphate, ATP and ADP on iron transfer from Fe(III)-bleomycin to apotransferrin

1. The rate of ferric ion transfer from Fe(III)-bleomycin to apotransferrin was increased in the presence of orthophosphate, ATP and ADP, while AMP was without effect. 2. Ortho phosphate activation probably involves formation of a Fe(III)-bleomycin-phosphate complex. The optical absorption of Fe(III)-bleomycin at 450 nm is enhanced in the presence of phosphate. 3. ATP and ADP remove the ferric ion from the iron-drug complex; thus making the ferric ion readily available for uptake by apotransferrin. 4. Low concentrations of ATP, ADP and AMP, also enhance the 450 nm absorption of the iron-drug complex. Higher ATP and ADP concentrations reduce both the 450 and 384 nm absorption of Fe(III)-bleomycin.     

Electron transfer. Part 165: Oxidations of Ti(II)(aq) with ligated iron(III) and ruthenium(III)

Titanium(II) solutions, prepared by dissolving titanium wire in triflic acid + HF, contain equimolar quantities of Ti(IV). Treatment of such solutions with excess Fe(III) or Ru(III) complexes yield Ti(IV), but reactions with Ti(II) in excess give Ti(III). Oxidations by (NH₃)₅Ru(III) complexes, but not by Fe(III) species, are catalyzed by titanium(IV) and by fluoride. Stoichiometry is unchanged. The observed rate law for the Ru(III)-Ti(II)-Ti(IV) reactions in fluoride media points to competing reaction paths differing by a single F⁻, with both routes involving a Ti(II)-Ti(IV) complex which is activated by deprotonation. It is suggested that coordination of Ti(IV) to Ti^II(aq) minimizes the mismatch of Jahn-Teller distortions which would be expected to lower the Ti(II,III) self-exchange rate.     

Complexation of iron(III) by catecholate-type polyphenols

We report here a complete physico-chemical study of the chelation of iron(III) by catechin (L¹), an abundant polyphenol in green tea. Using a fruitful combination of electrospray mass spectrometry, absorption spectrophotometry and potentiometry, we have characterized three ferric complexes of catechin (L¹Fe, and (L¹)₃Fe) as well as a ternary complex L¹FeNTA when an exogenous ligand (nitrilotriacetic acid) is added to the medium. Thanks to this study, we discuss the influence of an exogenous tetradentate ligand in the ferric recognition processes by catecholate-type polyphenols.     

Aminosuberoyl hydroxamic acids (ASHAs): a potent new class of HDAC inhibitors

Histone deacetylase (HDAC) inhibitors that target Class I and Class II HDACs are currently in advanced clinical trials for the treatment of cancer. Vorinostat (Zolinza, SAHA) is a hydroxamic acid approved for the treatment of patients with cutaneous T-cell lymphoma who have progressive, persistent or recurrent disease on or following two systemic therapies. As part of an on-going effort to better understand the nature of the HDAC enzyme/inhibitor interaction and design highly effective HDAC inhibitors, we herein report the design, synthesis and HDAC inhibitory activity of a vorinostat-derived series of substrate-based HDAC inhibitors.     

Iron transfer from urate-Fe(III) to citrate and ATP.

1. Urate, citrate and ATP, which form stable complexes with ferric ions, are proposed to function as low mol. wt iron binding agents in humans. 2. Citrate and ATP were found to readily take up iron from the urate-Fe(III) complex; the study suggests that citrate and ATP may be physiologically more important iron binding agents than urate.     

Heavy-atom effects on energy transfer from polynucleotides to terbium (III)

Energy transfer in nucleic acids or polynucleotides at room temperature can be studied by using the fluorescence of complexed terbium (III) as a tool. Complexing the heavy atom thallium (I) enhances energy transfer from poly(G) to terbium (III). Thallium has no effect on transfer from GMP to terbium and a small negative effect on the transfer from single-stranded DNA to terbium. Use of the Medinger-Wilkinson model to analyze the poly(G) results provides an estimate of the room-temperature intersystem crossing constant.     

Complexes of hydroxamates III.: Equilibrium and kinetic studies on the reactions of iron(III) with monohydroxamic acids

Spectral analysis of iron(III) complexes with acetohydroxamate (AX) and histidinehydroxamate (HX) in the UV-visible region revealed that many species may exist in pH range 1.0–7.5. The solution spectra were unstable in pH range ~2.7–4.0. Different species were obtained from fresh solutions and overnight solutions. The difference was rationalized due to hydrolysis and/or polymerization of complexes in solution, especially in pH range 2.7–4.0. The kinetics of the reactions of Fe(III) with AX and HX were accomplished, and mechanisms were suggested for both systems. In both cases, Fe³⁺ and FeOH²⁺ species were found to be the active species in the complex formation of 1:1 complex.     

Evidence that two enzyme-derived histidine ligands are sufficient for iron binding and catalysis by factor inhibiting HIF (FIH)

A 2-His-1-carboxylate triad of iron binding residues is present in many non-heme iron oxygenases including the Fe(II) and 2-oxoglutarate (2OG)-dependent dioxygenases. Three variants (D201A, D201E, and D201G) of the iron binding Asp-201 residue of an asparaginyl hydroxylase, factor inhibiting HIF (FIH), were made and analyzed. FIH-D201A and FIH-D201E did not catalyze asparaginyl hydroxylation, but in the presence of a reducing agent, they displayed enhanced 2OG turnover when compared with wild-type FIH. Turnover of 2OG by FIH-D201A was significantly stimulated by the addition of HIF-1alpha(786-826) peptide. Like FIH-D201A and D201E, the D201G variant enhanced 2OG turnover but rather unexpectedly catalyzed asparaginyl hydroxylation. Crystal structures of the FIH-D201A and D201G variants in complex with Fe(II)/Zn(II), 2OG, and HIF-1alpha(786-826/788-806) implied that only two FIH-based residues (His-199 and His-279) are required for metal binding. The results indicate that variation of 2OG-dependent dioxygenase iron-ligating residues as a means of functional assignment should be treated with caution. The results are of mechanistic interest in the light of recent biochemical and structural analyses of non-heme iron and 2OG-dependent halogenases that are similar to the FIH-D201A/G variants in that they use only two His-residues to ligate iron.