Models for ferrous cytochrome b5: Sign inversions in the magnetic circular dichroism spectra of bis-imidazole ferrous porphyrin systems

The magnetic circular dichroism (MCD) spectrum of bis-imidazole ferrous tetraphenylporphyrin in the Soret region is nearly the mirror image of the spectrum of ferrous cytochrome b₅, a bis-imidazole (histidine)-ligated hemoprotein. Based on previous MCD studies of model and protein heme systems, a sign inversion in the spectra of two heme chromophores having essentially the same coordination structure is unexpected. To investigate whether the nature of the porphyrin itself could account for the observed spectral discrepancy, two additional model complexes, bis-imidazole ferrous protoporphyrin IX dimethylester and bis-imidazole ferrous octaethylporphyrin, whose peripheral porphyrin substituent patterns more closely match that of the protein- bound porphyrin, have been prepared and their MCD spectra measured. In these cases, the band pattern of the ferrous protein in the Soret region is successfully reproduced. It therefore appears that the anomalous MCD spectrum of the tetraphenylporphyrin complex can be attributed to the nature and positioning of the peripheral substituents on the porphyrin ring. Although iron tetraphenylporphyrin complexes are frequently used as models for protoporphyrin- containing hemoproteins, one should be aware that such differences in the peripheral porphyrin substituents may significantly affect the spectral properties of the model complex.     

Electrochemistry and spectroscopy of sulfate and thiosulfate complexes of iron porphyrins

The electrochemical and spectroscopic properties of the complex formed by the addition of thiosulfate to ferric porphyrins were examined. The NMR spectrum of the thiosulfate-ferric porphyrin complex was consistent with a high-spin ferric complex, while the EPR spectrum at liquid nitrogen temperatures indicated that the complex under these conditions was low-spin. Such behavior has been previously observed for other ferric porphyrin complexes. The visible spectra were characterized by a shift in the Soret band to higher energies, with smaller changes in the longer wavelength region. The complex was reasonably stable in DMF, but slowly reduced over several hours to Fe^II(TPP) and S₄O₆ ²⁻. The voltammetric behavior of the thiosulfate complex in DMF consists of two waves, the first of which was irreversible. The ferric/ferrous reduction in the presence of thiosulfate was shifted negatively about 400 mV, compared to the Fe(TPP)(Cl) reduction. The visible, NMR and EPR spectra were most consistent with a Fe-S bonded ferric porphyrin-thiosulfate complex, Fe(P)(SSO₃)⁻. The kinetics of the reduction of ferric porphyrin by thiosulfate in DMSO indicated an autocatalytic mechanism, where the first step is the formation of the catalyst. The identity of the catalyst could not be determined because it must be present at low concentrations, but it is formed from the reaction of the ferric complex with thiosulfate. Coordination of thiosulfate to the porphyrin was not necessary for the reduction to occur, and the reduction of Fe(TPP)(Cl) by thiosulfate was accelerated by the addition of sulfate. Under these conditions, sulfate had replaced thiosulfate as the axial ligand for the ferric porphyrin. In the presence of sulfate, the reduction occurred in a single kinetic pseudo-first order step.     

Electron paramagnetic resonance spectroscopy of lactoperoxidase complexes: clarification of hyperfine splitting for the NO adduct of lactoperoxidase

Electron paramagnetic resonance (EPR) studies of the nitrosyl adduct of ferrous lactoperoxidase (LPO) confirm that the fifth axial ligand in LPO is bound to the iron via a nitrogen atom. Complete reduction of the ferric LPO sample is required in order to observe the nine-line hyperfine splitting in the ferrous LPO/NO EPR spectrum. The ferrous LPO/NO complex does not exhibit a pH or buffer system dependence when examined by EPR. Interconversion of the ferrous LPO/NO complex and the ferric LPO/NO2- complex is achieved by addition of the appropriate oxidizing or reducing agent. Characterization of the low-spin LPO/NO2- complex by EPR and visible spectroscopy is reported. The pH dependence of the EPR spectra of ferric LPO and ferric LPO/CN- suggests that a high-spin anisotropic LPO complex is formed at high pH and an acid-alkaline transition of the protein conformation near the heme site does occur in LPO/CN-. The effect of tris(hydroxymethyl)aminomethane buffer on the LPO EPR spectrum is also examined.     

The coordination of imidazole and substituted pyridines by the hemeoctapeptide N-acetyl-ferromicroperoxidase-8 (FeIINAcMP8)

The N-terminus acetylated ferric hemeoctapeptide from cytochrome c, N-acetylmicroperoxidase-8 (Fe(III)-NAcMP8) can be reduced by dithionite in aqueous solution to produce Fe(II)-NAcMP8. The UV-Vis spectrum has a broad Soret band and relatively poorly defined Q bands which is consistent with a mixture of a five-coordinate high spin species with His as the axial ligand and a six-coordinate, predominantly high spin species with His/H(2)O as axial ligands. There are two spectroscopically observable pK(a)s at 8.7+/-0.1 and 10.9+/-0.2 which are attributed to ionization of a heme propionic acid group and coordinated H(2)O, respectively; a pK(a) > or = 14 is due to ionization of the proximal His ligand. Equilibrium constants were determined by UV-Vis spectrophotometry at 25.0+/-0.2 degrees C and 0.5 M ionic strength (NaClO(4)) for the coordination of imidazole and a number of substituted pyridines, and complement available data for the ferric hemepeptide, allowing a comparison to be made of the affinity of an iron porphyrin with Fe in the +2 and +3 oxidation states towards these ligands. Imidazole is coordinated more strongly by the ferric porphyrin (log K=4.08) than by the ferrous porphyrin (log K=3.40). The equilibrium constants for coordination of pyridines by the ferric and ferrous porphyrins increase and decrease, respectively, with increasing ligand basicity. Values determined by cyclic voltammetry show the same dependence on the identity of the ligand. In the ferric porphyrin, the stability of the complex increases with the basicity of the ligand and hence its ability to donate electron density onto the metal. In the case of the more electron rich ferrous porphyrin, greater stability occurs with pyridine ligands that have an electron withdrawing group and hence can accept electron density from the metal. This is consistent with the midpoint reduction potentials E(1/2) of the pyridine complexes determined by cyclic voltammetry; E(1/2) is linearly dependent on, and becomes more negative with an increase in, ligand basicity. Log K for coordination of pyridines by the ferrous hemepeptide correlates well with the energy of the ligand frontier orbital with pi symmetry, suggesting that pi-bonding effects are significant in determining the strength of binding of pyridines by a ferrous porphyrin.     

Nitric oxide binding to cationic and anionic ferric porphyrins in aqueous solution: reversible formation of ferrous NO species of the cationic porphyrin

Two water-soluble ferric porphyrins, sodium 5α,10β,15α,20β-tetrakis(2-(sulfonatoacetamido)phenyl)porphyrinatoiron(III) (Fe^IIITanP) and 5α,10β,15α,20β-tetrakis(2-(N,N,N-trimethylammoniumacetamido)phenyl)porphyrinatoiron(III) chloride (Fe^IIITcatP), were synthesized. The pK_a values of the coordinated H₂O of Fe^IIITanP and Fe^IIITcatP were evaluated to be 8.0 and 4.1, respectively. Reactions of NO with the ferric porphyrins were examined spectrophotometrically in aqueous solution. Porphyrin Fe^IIITanP binds NO reversibly to give the corresponding ferric NO species at pH 1.3 and pH 3.0, and Fe^IIITcatP reacts similarly with NO at pH 1.3. The thermodynamic data for the NO binding were estimated from van't Hoff plots. At pH 3.0, visible and ESR spectral data indicated that Fe^IIITcatP binds NO reversibly to produce ferrous NO species depending on NO partial pressures. These results were discussed based on through-space intramolecular interactions between the coordinated H₂O or NO and the ionic substituents of the porphyrins.     

Studies on ferrochelatase: The effects of thiols and other factors on the determination of activity

1. Haems are unstable under aerobic conditions in the presence of thiols, which are used to activate the ferrochelatase enzyme; catalase inhibits this degradation of haem. In addition, thiols interfere with the determination of protohaem as its pyridine haemochromogen derivative. 2. Three ferrochelatase assays are described that minimize interference by these two reactions. Two of these assays involve measurement of porphyrin utilization, one spectrophotometrically and the second spectrofluorimetrically. The third assay measures haem formation by a pyridine haemochromogen technique. Results obtained with these three methods were in close agreement at a GSH concentration of 4mm. 3. The stimulatory effect of GSH on ferrochelatase has been confirmed. The spectrum of the haem formed is dependent on GSH concentration; at high GSH concentrations (20mm) the haem is in the reduced state, but at low concentration (4mm) the spectrum of the product resembles that of an oxidized haemoprotein such as ferrihaemoglobin. 4. The inhibitory effect of oxygen on ferrochelatase activity has been confirmed by spectrophotometric assay of porphyrin disappearance.     

The effect on photohaemolysis of variation in the structure of the porphyrin photosensitizer.

A comparison of the photosensitizing ability of a variety of porphyrins for photohaemolysis gives the following order of activity: protoporphyrin greater than deuteroporphyrin, mesoporphyrin, haematoporphyrin dimethyl ester much greater than haematoporphyrin diacetate, haematoporphyrin greater than haematoporphyrin monoacetate, coproporphyrin III, haematoporphyrin derivative, coproporphyrin III tetramethyl ester greater than uroporphyrin I, meso-tetra-(N-methyl-4-pyridinium)porphyrin tetratoluene-p-sulphonate, meso-tetra-(p-carboxyphenyl)porphyrin, protoporphyrin dimethyl ester, meso-tetra-(p-hydroxy-sulphonylphenyl)porphyrin tetrasodium salt, uroporphyrin III, deuteroporphyrin-3,8-disulphonic acid and protohaemin. The results for the metal-free porphyrins are rationalized in terms of solubility and partition properties, and a model is proposed for the incorporation of amphipathic porphyrins into the membrane lipid bilayer. Experiments with erythrocytes from patients with erythropoeitic protoporphyria and with normal erythrocytes to which porphyrin was added in a deuterium oxide medium do not lead to an increase in the rate of photohaemolysis. A possible explanation for this somewhat surprising observation is outlined.     

Spectroscopic studies on bleomycin-iron complexes with carbon monoxide, nitric oxide, isocyanide, azide, and cyanide and comparison with iron-porphyrin complexes

The bleomycin-iron complexes with CO, NO, C2H5NC, OH-, N-3, CN-, and CH3NH2 were characterized by electronic, ESR, 1H-NMR, and M?ssbauer spectroscopies and the findings were compared with the corresponding hemoprotein complexes. The 1H-NMR and M?ssbauer features for the CO and C2H5NC adducts of the bleomycin-Fe(II) complex are consistent with an S = 0 ferrous assignment. The OH-, CH3NH2, and N-3 adducts of the bleomycin-Fe(III) complex show the ESR, 1H-NMR, and M?ssbauer spectra typical of a low-spin Fe(III). The unique M?ssbauer parameters of the bleomycin-Fe(II)-NO complex demonstrate mixing between the NO pi- and the Fe 3d-orbitals. The magnitude of the proton chemical shifts over +/- 50 ppm indicates a high-spin ferric type for the bleomycin-Fe(III)-CN complex. The M?ssbauer parameters (delta EQ = 0.89 and delta = 0.48 mm/s) of the CN- adduct differ substantially from those of typical low-spin hemoprotein-cyanide complexes. Except for the CN- adduct, the M?ssbauer and crystal field parameters of these bleomycin-iron complexes are similar to those of the corresponding hemoprotein complexes.     

The pH dependence of the resonance raman spectra and structural alterations at heme moieties of various c-type cytochromes.

The pH dependence of resonance Raman spectra were studied for ferrous and ferric cytochromes c, c2, c3, c-551, and c-555. The frequencies of the 1565 cm-1 (ferric) and 1539 cm-1 lines (ferrous) were sensitive to the replacement of the sixth ligand. The titration curve for the 1565 cm-1 line of cytochrome c was parallel with that for the 695 nm band. The pH dependence of the 1539 cm-1 line of ferrous cytochrome c3 suggested the stepwise replacement of the sixth ligand of its four hemes, although such pH dependence was not recognized for the Raman spectra of other ferrous cytochromes investigated. The relative intensities of three Raman lines at 1639, 1587, and 1561 cm-1 of ferric protoporphyrin bis-imidazole complex were changed clearly by the presence of detergents. The relative intensities of the corresponding three Raman lines of cytochromes b5 and c were close to those of the ferric porphyrin complex in the presence and absence of detergents, respectively, suggesting an appreciable difference in their heme environments. Reduced hemin in detergent solution, unexpectedly, gave the Raman spectrum of ferric low spin type.     

Parameters controlling the kinetics of ferric and ferrous hemeproteins reduction by hydrated electrons

To clarify the processes of hemeproteins reduction, three classes of these proteins (ferric, ferrous and desFe) were reduced by hydrated electrons generated by pulse radiolysis. Spectral and kinetic investigations were made on alpha hemoglobin chain and myoglobin. Human alpha chain has been chosen to avoid all ferric contaminations and horse ferric myoglobin to eliminate all ferrous protein fractions. We have successively studied the influences of: the iron presence, its oxidation state (II and III), the protein charge and the iron-ligand nature (H2O, OH-, N3- and CN-). For alpha human hemoglobin chain without metallic ion or with ferrous iron, the reduction rates are the same: 1.1 +/- 0.2.10(10) M-1.s-1. In the case of horse ferric myoglobin, the reduction rates depend principally on the protein charge (from pH 6.3 to pH 9.5, the reduction rate of Mb(FeIII)N3- decreases from 2.5 +/- 0.5.10(10) M-1.s-1 to 1.2 +/- 0.2.10(10) M-1.s-1) and are also modulated by the equilibrium constant of the hemeprotein-ligand association (1.2 +/- 0.2.10(10) M-1.s-1 for Mb(FeIII)N3- and 0.8 +/- 0.2.10(10) M-1.s-1 for Mb(FeIII)CN-, at pH 9.8).     

Dissociation rates of axially coordinated imidazoles and formation constants of low spin ferric complexes derived from tetraphenylporphyrin and tetramesitylporphyrin

The dissociation rates of axially coordinated imidazole in bis-ligated low spin ferric complexes of synthetic porphyrins such as tetraphenylporphyrin (TPP) and tetramesitylporphyrin (TMP) were measured by NMR method. In both TPP and TMP complexes, the axial lability of imidazoles increased in the order 1-methylimidazole < 2-methylirnidazole < 2-ethylimidazole ∼ 1,2-dimethylimidazole. The results were explained in terms of the steric repulsion between the 2-alkyl group of imidazole and the porphyrin ring. The dissociation rates of TPP complexes were then compared with those of TMP complexes carrying the same axial ligands. In every case examined, imidazole dissociated faster from the TPP complex than from the TMP complex. The results were ascribed to the stability of the bis-ligated TMP complex relative to the corresponding TPP complex; the formation constant of the TMP complex having 2-Melm as axial ligand was larger than that of the corresponding TPP complex by a factor of c. 600. A hypothesis has been proposed to explain the stability of the sterically hindered porphyrin complex relative to the less hindered complex.     

Intermediates in the ferrous oxidase cycle of bleomycin

We have previously shown that the bleomycin-induced autooxidation of ferrous iron follows Michaelis--Menten kinetics which are characteristic of enzymatic reactions [Caspary, W. J., Lanzo, D. A., Niziak, C., Friedman, R., & Bachur, N. R. (1979) Mol. Pharmacol. 16, 256]. In this paper, we identify the iron complexes formed during this reaction. The first is a ferrous iron--bleomycin complex which can be considered the catalyst substrate complex. The product of this reaction is a ferric iron--bleomycin complex which is found in a low-spin and a high-spin form. The relative concentrations of these two forms are a function of pH. Glutathione, a biologically relevant reducing agent, binds to the ferric iron--bleomycin complex, reduces it, and may serve as a model for the reduction of the ferric iron--bleomycin complex to the ferrous state during the catalytic cycle. Oxygen uptake induced by bleomycin and ferrous iron is not inhibited by superoxide dismutase (SOD) or catalase. In the absence of bleomycin, catalase strongly inhibits oxygen uptake. This suggests the presence of a relatively stable intermediate in which the superoxide radical is not readily accessible to superoxide dismutase. At pH 9.3, we are able to observe a transient species by electron spin resonance (ESR). When potassium superoxide is added to the ferric iron--bleomycin complex, the same ESR spectrum is produced. We suggest that a transient species composed of a ferric iron, the superoxide ion, and bleomycin is formed. The precise nature of the binding cannot be determined from the data presented.     

The crystal structures of the ferric and ferrous forms of the heme complex of HmuO, a heme oxygenase of Corynebacterium diphtheriae

Crystal structures of the ferric and ferrous heme complexes of HmuO, a 24-kDa heme oxygenase of Corynebacterium diphtheriae, have been refined to 1.4 and 1.5 A resolution, respectively. The HmuO structures show that the heme group is closely sandwiched between the proximal and distal helices. The imidazole group of His-20 is the proximal heme ligand, which closely eclipses the beta- and delta-meso axis of the porphyrin ring. A long range hydrogen bonding network is present, connecting the iron-bound water ligand to the solvent water molecule. This enables proton transfer from the solvent to the catalytic site, where the oxygen activation occurs. In comparison to the ferric complex, the proximal and distal helices move closer to the heme plane in the ferrous complex. Together with the kinked distal helix, this movement leaves only the alpha-meso carbon atom accessible to the iron-bound dioxygen. The heme pocket architecture is responsible for stabilization of the ferric hydroperoxo-active intermediate by preventing premature heterolytic O-O bond cleavage. This allows the enzyme to oxygenate selectively at the alpha-meso carbon in HmuO catalysis.     

A nuclear magnetic resonance study of axial ligation for the reduced states of chloroperoxidase,cytochrome P-450cam,and porphinatoiron(II) thiolate complexes

The reduced forms of cytochrome P-450_cam and chloroperoxidase were examined by proton NMR spectroscopy. The pH and temperature dependences of the proton NMR spectra of both ferrous enzymes are reported. A series of alkyl mercaptide complexes of both synthetic and natural-derivative iron(II) porphyrins was also examined. The proton NMR spectra of these complexes facilitated the assignment of resonances due to the axial ligand in the model compounds on the basis of their isotropic shifts and multiplicities. Comparison of model compound data with that for the reduced enzymes supports assignment of the methylene protons for the axial cysteinate of ferrous cytochrome P-450_cam and ferrous chloroperoxidase to proton NMR resonances at 279 and 200 ppm (pH 7.0, 298K), respectively. Differences in the active site structure of the two enzymes are further demonstrated by ¹⁵N-NMR spectroscopy of the cyanide complexes of the ferric forms.     

Heme ferrous-hydroperoxo complexes: some theoretical considerations

We report density functional calculations on complexes of ferrous hemes with hydroperoxide, where the axial ligand trans to OOH(-) is imidazole, thiolate, or phenoxide. The geometrical parameters and charge distributions within the Fe-O-O-H moiety are identical between the ferrous complexes reported here and their ferric counterparts previously described, even though the latter contain one unpaired electron on iron as opposed to the former, which are diamagnetic. The extra negative charge upon going from a formally ferric state to formally ferrous appears to be distributed essentially on the porphyrin. These findings support recent experimental data showing that the ferrous state of certain hemoproteins can interact with peroxides in a catalytically competent fashion, cleaving the O-O bond heterolytically in a manner reminiscent of the "canonical" ferric-peroxo complexes, and contrary to any expectations based on the Fenton concept commonly invoked in non-heme chemistry.     

Photophysical characterization and photodynamic activity of metallo 5-(4-(trimethylammonium)phenyl)-10,15,20-tris(2,4,6-trimethoxyphenyl)porphyrin in homogeneous and biomimetic media

The photophysical properties and photodynamic effect of Zn(ii), Pd(ii), Cu(ii) and free-base 5-(4-(trimethylammonium)phenyl)-10,15,20-tris(2,4,6-trimethoxy phenyl)porphyrin (H2P) iodide have been studied in N,N-dimethylformamide (DMF) and in different biomimetic systems. The absorption, fluorescence, triplet state and singlet molecular oxygen production of the metal complexes were all referred to H2P. The photodynamic activity was first analyzed using 9,10-dimethylanthracene and guanosine 5'-monophosphate in N,N-dimethylformamide. The photooxidation processes were also investigated in benzene/benzyl-n-hexadecyldimethyl ammonium chloride/water reverse micelles. Photosensitization efficiency of these porphyrins was H2P approximately ZnP > PdP in homogeneous solution and ZnP > H2P > PdP in micelles, whereas no photooxidation effect was detected using the Cu(ii) complex. Human erythrocytes were used as a biological membrane model. The photohemolytic activity depended on irradiation time, sensitizer and concentration of the agent. When cells were treated with 1 microM sensitizer, the hemolytic activity was H2P > ZnP > CuP. However, it was H2P > ZnP approximately CuP using 5 microM of the respective porphyrin. Although CuP could undergo a type I photoreaction, in all cases the photohemolytic effect considerably diminishes in anoxic conditions, indicating that an oxygen atmosphere is required for the mechanism of cellular membrane damage. The behavior of these amphiphilic metallo porphyrins provides information on the photodynamic activity of these agents in biomimetic microenvironments.     

Studies on the equilibria and kinetics of the reactions of ferrous catalase with ligands

The optical absorption spectrum of bovine liver catalase was found to change on light irradiation in the presence of proflavin and EDTA in a deaerated solution. Upon addition of CO to the photolyzed product, the spectrum changed to an another form, suggesting that the photolyzed product is the ferrous form of the enzyme and CO is bound to the ferrous enzyme. When O2 was introduced into the ferrous enzyme, the absorption spectrum returned to its original ferric state. An intermediate spectrum was obtained in this reaction at -20 degrees C in 33% v/v ethylene glycol. Judged from the spectral characteristics of this compound, it is probably an oxyferrous enzyme. It was converted into ferric enzyme gradually when the sample was left at room temperature. The ferrous enzyme, which was generated by flash photolysis of the CO complex of the enzyme in an air-saturated buffer, reacted with O2 to form the oxyferrous enzyme with a second order rate constant of 9.2 x 10(3) M-1.s-1 at pH 8.6 and 20 degrees C. The oxyferrous enzyme thus obtained autodecomposed into the ferric form with a rate constant of 0.1 s-1.     

Roles of porphyrins and host iron transport proteins in regulation of growth of Porphyromonas gingivalis W50.

Porphyromonas gingivalis (Bacteroides gingivalis) requires iron in the form of hemin for growth and virulence in vitro, but the contributions of the porphyrin ring structure, porphyrin-associated iron, host hemin-sequestering molecules, and host iron-withholding proteins to its survival are unknown. Therefore, the effects of various porphyrins, host iron transport proteins, and inorganic iron sources on the growth of P. gingivalis W50 were examined to delineate the various types of iron molecules used for cellular metabolism. Cell envelope-associated hemin and iron stores contributed to the growth of P. gingivalis in hemin-free culture, and depletion of these endogenous reserves required eight serial transfers into hemin-free medium for total suppression of growth. Comparable growth of P. gingivalis was observed with 7.7 microM equivalents of hemin as hemoglobin (HGB), methemoglobin, myoglobin, hemin-saturated serum albumin, lactoperoxidase, cytochrome c, and catalase. Unrestricted growth was recorded in the presence of haptoglobin-HGB and hemopexin-hemin complexes, indicating that these host defense proteins do not sequester HGB and hemin from P. gingivalis. The iron chelator 2,2'-bipyridyl functionally chelated hemin-associated iron, resulting in dose-dependent inhibition of growth in hemin-restricted cultures at 1 to 25 microM 2,2'-bipyridyl concentrations. In the absence of an exogenous iron source, protoporphyrin IX did not support P. gingivalis growth. These findings suggest that the iron atom in the hemin molecule is the critical constituent for growth and that the tetrapyrrole porphyrin ring structure may represent an important vehicle for delivery of iron into the P. gingivalis cell. P. gingivalis does not have a strict requirement for porphyrins, since growth occurred with nonhemin iron sources, including high concentrations (200 muM) of ferric, ferrous, and nitrogenous inorganic iron, and P. gingivalis exhibited unrestricted growth in the presence of host transferrin, lactoferrin, and serum albumin. The diversity of iron substrates utilized by P. gingivalis and the observation that growth was not affected by the bacteriostatic effects of host iron-withholding proteins, which it may encounter in the periodontal pocket, may explain why P. gingivalis is such a formidable pathogen in the periodontal disease process.     

Spectroscopic and equilibrium studies of ligand and organic substrate binding to indolamine 2,3-dioxygenase

The binding of a number of ligands to the heme protein indolamine 2,3-dioxygenase has been examined with UV-visible absorption and with natural and magnetic circular dichroism spectroscopy. Relatively large ligands (e.g., norharman) which do not readily form complexes with myoglobin and horseradish peroxidase (HRP) can bind to the dioxygenase. Except for only a few cases (e.g., 4-phenylimidazole) for the ferric dioxygenase, a direct competition for the enzyme rarely occurs between the substrate L-tryptophan (Trp) and the ligands examined. L-Trp and small heme ligands (CN-,N3-,F-) markedly enhance the affinity of each other for the ferric enzyme in a reciprocal manner, exhibiting positive cooperativity. For the ferrous enzyme, L-Trp exerts negative cooperativity with some ligands such as imidazoles, alkyl isocyanides, and CO binding to the enzyme. This likely reflects the proximity of the Trp binding site to the heme iron. Other indolamine substrates also exert similar but smaller cooperative effects on the binding of azide or ethyl isocyanide. The pH dependence of the ligand affinity of the dioxygenase is similar to that of myoglobin rather than that of HRP. These results suggest that indolamine 2,3-dioxygenase has the active-site heme pocket whose environmental structure is similar to, but whose size is considerably larger than, that of myoglobin, a typical O2-binding heme protein. Although the L-Trp affinity of the ferric cyanide and ferrous CO enzyme varies only slightly between pH 5.5 and 9.5, the unligated ferric and ferrous enzymes have considerably higher affinity for L-Trp at alkaline pH than at acidic pH. L-Trp binding to the ferrous dioxygenase is affected by an ionizable residue with a pKa value of 7.3.     

The kinetics of flavine oxidation-reduction. II. Metal ion interactions.

The oxidation-reduction reactions of tetraacetylriboflavine in the presence of various metal ions in dimethylformamide have been investigated using the stopped-flow technique under anaerobic conditions. Dismutation kinetics in the presence of redox-inactive dissociated divalent metal ions such as Cd2+, Zn2+, and Fe2+ are typically triphasic. Metal ions act primarily upon an intermediate flavine dimer formed by fast association of flavoquinone and flavohydroquinone, resulting in a parallel formation and neutral and chelated radicals. A competition between metal ions and proton donors, e.g. the neutral flavohydroquinone (FredH3), is observed at the level of this intermediate complex. Small spectral changes occur secondarily as an ill-defined intermediate phase which could correspond to the reorganization of the solvation of radical chelate. The neutral radical is finally chelated at a much slower rate, the yield of total radical formation remaining almost unchanged during this kinetic phase. The oxidation of flavohydroquinone by ferric ions, either dissociated or strongly coordinated within a porphyrin, is complete and proceeds through biphasic kinetics. The first phase (Fred leads to F) is much faster than the second one (F leads to Fox). Dismutation resulting from the transient accumulation of neutral flavosemiquinone competes with the direct oxidation with ferric ions for the completion of the second oxidation step. The relative rate of dismutation is essentially limited by acidic-basic reactions in the absence of an excess of ferrous ion. The kinetic analysis of the direct oxidation reactions favors an outer-sphere mechanism for the electron transfer to the ferric ion, either free or strongly coordinated. The formation of a ferrous radical chelate can result from the dismutation reactions only when the amount of ferric ion initially present is not sufficient for complete oxidation.