Peroxidase-catalyzed halide ion oxidation

Abstract

The first complete mechanistic analysis of halide ion oxidation by a peroxidase was that of iodide oxidation by horseradish peroxidase. It was shown conclusively that a two-electron oxidation of iodide by compound I was occurring. This implied that oxygen atom transfer was occurring from compound I to iodide, forming hypoiodous acid, HOI. Searches were conducted for other two-electron oxidations. It was found that sulfite was oxidized by a two-electron mechanism. Nitrite and sulfoxides were not. If a competing substrate reduces some compound I to compound II by the usual one-electron route, then compound II will compete for available halide. Thus compound II oxidizes iodide to an iodine atom, I^·, although at a slower rate than oxidation of I^- by compound I. An early hint that mammalian peroxidases were designed for halide ion oxidation was obtained in the reaction of lactoperoxidase compound II with iodide. The reaction was accelerated by excess iodide, indicating a co-operative effect. Among the heme peroxidases, only chloroperoxidase (for example from Caldariomyces fumago) and mammalian myeloperoxidase are able to oxidize chloride ion. There is not yet a consensus as to whether the chlorinating agent produced in a peroxidase-catalyzed reaction is hypochlorous acid (HOCl), enzyme-bound hypochlorous acid (either Fe–HOCl or X–HOCl where X is an amino acid residue), or molecular chlorine Cl₂. A study of the non-enzymatic iodination of tyrosine showed that the iodinating reagent was either HOI or I₂. It was impossible to tell which species because of the equilibria:

I₂+H₂O=HOI+I^-+H⁺</ p>

I^-+I₂=I₃^-

The same considerations apply to product analysis of an enzyme-catalyzed reaction. Detection of molecular chlorine Cl₂ does not prove it is the chlorinating species. If Cl₂ is in equilibrium with HOCl then one cannot tell which (if either) is the chlorinating reagent. Examples will be shown of evidence that peroxidase-bound hypochlorous acid is the chlorinating agent. Also a recent clarification of the mechanism of reaction of myeloperoxidase with hydrogen peroxide and chloride along with accurate determination of the elementary rate constants will be discussed.     

Myeloperoxidase-catalyzed taurine chlorination: initial versus equilibrium rate

Myeloperoxidase (MPO) catalyzes the two-electron oxidation of chloride, thereby producing hypochlorous acid (HOCl). Taurine (2-aminoethane-sulfonic acid, Tau) is thought to act as a trap of HOCl forming the long-lived oxidant monochlorotaurine [(N-Cl)-Tau], which participates in pathogen defense. Here, we amend and extend previous studies by following initial and equilibrium rate of formation of (N-Cl)-Tau mediated by MPO at pH 4.0-7.0, varying H(2)O(2) concentration. Initial rate studies show no saturation of the active site under assay conditions (i.e. [H(2)O(2)] > or = 2000 [MPO]). Deceleration of Tau chlorination under equilibrium is quantitatively described by the redox equilibrium established by H(2)O(2)-mediated reduction of compound I to compound II. At equilibrium regime the maximum chlorination rate is obtained at [H(2)O(2)] and pH values around 0.4mM and pH 5. The proposed mechanism includes known acid-base and binding equilibria taking place at the working conditions. Kinetic data ruled out the currently accepted mechanism in which a proton participates in the molecular step (MPO-I+Cl(-)) leading to the formation of the chlorinating agent. Results support the formation of a chlorinating compound I-Cl(-) complex (MPO-I-Cl) and/or of ClO(-), through the former or even independently of it. ClO(-) diffuses away and rapidly protonates to HOCl outside the heme pocket. Smaller substrates will be chlorinated inside the enzyme by MPO-I-Cl and outside by HOCl, whereas bulkier ones can only react with the latter.     

On the mechanism of chlorination by chloroperoxidase

Spectral-scan results obtained on the millisecond time scale are reported for reactions of chloroperoxidase with peracetic acid and chloride ion in both the presence and the absence of monochlorodimedone. A multimixing experiment is performed in which stoichiometric amounts of chloroperoxidase and peracetic acid are premixed for 0.7 s before the resultant compound I is reacted with chloride ion. The combined results show that the only detectable enzyme intermediate species is compound I (except in very late stages of the reaction), that the disappearance of compound I is accelerated by the presence of chloride ion, and that it is further accelerated if both chloride and monochlorodimedone are present. It is concluded that compound I is an obligate intermediate species in the reaction. Experiments are performed on the reaction of monochlorodimedone with hypochlorous acid in both the presence and the absence of added chloride ion, but in the absence of chloroperoxidase. The presence of chloride ion greatly accelerates the reaction rate apparently by setting off a chlorine chain reaction. This reaction would be important in the enzyme-catalyzed reaction if hypochlorous acid were liberated into the solution. A careful analysis of steady-state kinetic results shows that in the chlorination of monochlorodimedone at least, liberation of free hypochlorous acid is not important in the enzyme-catalyzed pathway. Rather the reaction proceeds from compound I to formation of iron(III)-OCl by chloride ion addition to the ferryl oxygen atom. This obligate intermediate species then chlorinates the substrate. It is well described as enzyme-activated hypochlorous acid, in which replacement of the proton in HOCl by the heme iron ion produces a Cl+ species of great potency. Thus the enzyme controls chlorination of monochlorodimedone rather than unleashing an uncontrolled chain reaction in which it would be rapidly destroyed.     

Myeloperoxidase-catalyzed chlorination: the quest for the active species

Myeloperoxidase (MPO) is a dominating enzyme of circulating polymorphonuclear neutrophils that catalyzes the two-electron oxidation of chloride, thereby producing the strong halogenating agent hypochlorous acid (ClO⁻/HOCl). In absence of MPO the tripeptide Pro-Gly-Gly reacts with HOCl faster than the amino acid taurine (2-aminoethanesulfonic acid, Tau), while the MPO-mediated chlorination shows reverse order. A comparative study of the enzymatic oxidation of both substrates at pH 4.0–6.0, varying H₂O₂ concentration is presented. Initial and equilibrium rates studies have been carried on, reaction rates in the latter being slower due to the chemical equilibrium between MPO-I and MPO-II–HO₂. A maximum of chlorination rate is observed for Pro-Gly-Gly and Tau when [H₂O₂] ≈ 0.3–0.7 mM and pH ≈ 4.5–5.0. Several mechanistic possibilities are considered, the proposed one implies that chlorination takes place via two pathways. One, for bulkier substrates, involves chlorination by free HOCl outside the heme cavity; ClO⁻ is released from the active center, diffuses away the heme cavity, and undergoes protonation to HOCl. The other implies the existence of compound I–Cl⁻ complex (MPO-I–Cl), capable of chlorinating smaller substrates in the heme pocket. Electronic structure calculations show the size of Pro-Gly-Gly comparable to the available gap in the substrate channel, this tripeptide being unable to reach the active site, and its chlorination is only possible by free HOCl outside the enzyme.     

Molecular chlorine generated by the myeloperoxidase-hydrogen peroxide-chloride system of phagocytes produces 5-chlorocytosine in bacterial RNA

Myeloperoxidase, a heme enzyme secreted by activated phagocytes, uses H(2)O(2) and Cl(-) to generate the chlorinating intermediate hypochlorous acid (HOCl). This potent cytotoxic oxidant plays a critical role in host defenses against invading pathogens. In this study, we explore the possibility that myeloperoxidase-derived HOCl might oxidize nucleic acids. When we exposed 2'-deoxycytidine to the myeloperoxidase-H(2)O(2)-Cl(-) system, we obtained a single major product that was identified as 5-chloro-2'-deoxycytidine using mass spectrometry, high performance liquid chromatography, UV-visible spectroscopy, and NMR spectroscopy. 5-Chloro-2'-deoxycytidine production by myeloperoxidase required H(2)O(2) and Cl(-), suggesting that HOCl is an intermediate in the reaction. However, reagent HOCl failed to generate 5-chloro-2'-deoxycytidine in the absence of Cl(-). Moreover, chlorination of 2'-deoxycytidine was optimal under acidic conditions in the presence of Cl(-). These results implicate molecular chlorine (Cl(2)), which is in equilibrium with HOCl through a reaction requiring Cl(-) and H(+), in the generation of 5-chloro-2'-deoxycytidine. Activated human neutrophils were able to generate 5-chloro-2'-deoxycytidine. Cellular chlorination was blocked by catalase and heme poisons, consistent with a myeloperoxidase-catalyzed reaction. The myeloperoxidase-H(2)O(2)-Cl(-) system generated similar levels of 5-chlorocytosine in RNA and DNA in vitro. In striking contrast, only cell-associated RNA acquired detectable levels of 5-chlorocytosine when intact Escherichia coli was exposed to the myeloperoxidase system. This observation suggests that oxidizing intermediates generated by myeloperoxidase selectively target intracellular RNA for chlorination. Collectively, these results indicate that Cl(2) derived from HOCl generates 5-chloro-2'-deoxycytidine during the myeloperoxidase-catalyzed oxidation of 2'-deoxycytidine. Phagocytic generation of Cl(2) therefore may constitute one mechanism for oxidizing nucleic acids at sites of inflammation.     

On the irreversible destruction of reduced nicotinamide nucleotides by hypohalous acids

Degradation of the reduced pyridine nucleotides NMNH and NADH by HOCl involves two distinct stages: a fast reaction, k = 4.2 x 10(5) M(-1) s(-1), leads to generation of stable pyridine products (Py/Cl) with a strong absorption band at 275 nm (epsilon = 12.4 x 10(3) M(-1) cm(-1) in the case of NMNH); secondarily, a subsequent reaction of HOCl, k = 3.9 x 10(3) M(-1) s(-1), leads to a complete loss of the aromatic absorption band of the pyridine ring. HOBr and HOI(I(2)) react similarly. Apparent rate constants of the primary reactions of HOX species with NMNH at pH 7.2 increase in the order HOCl (3 x 10(5) M(-1) s(-1)) < HOBr( approximately 4 x 10(6) M(-1) s(-1)) < HOI(I(2))( approximately 6.5 x 10(7) M(-1) s(-1)). HOBr reacts fast also with the primary product Py/Br, k approximately 9 x 10(5) M(-1) s(-1), while the reactions of HOI and I(2) with Py/I are slower, approximately 1.4 x 10(3) M(-1) s(-1) and >6 x 10(3) M(-1) s(-1), respectively. Halogenation of the amide group of NMN(+) by HOX species is many orders of magnitude slower than oxidation of NMNH. Taurine inhibits HOCl-induced oxidation of NADH, but HOBr-induced oxidation is not inhibited because the taurine monobromamine rapidly oxidizes NADH, and oxidation by HOI(I(2)) is not inhibited because taurine is inert toward HOI(I(2)). Also sulfur compounds (GSH, GSSG, and methionine) are less efficient in protecting NADH against oxidation by HOBr and HOI(I(2)) than against oxidation by HOCl. The results suggest that reactions of HOBr and HOI(I(2)) in a cellular environment are much more selectively directed toward irreversible oxidation of NADH than reactions of HOCl. It is noteworthy that the rather inert N-chloramines react with iodide to generate HOI(I(2)), i.e., the most reactive and selective oxidant of reduced pyridine nucleotides. NMR investigations show that the primary stable products of the reaction between NMNH and HOCl are various isomeric chlorohydrins originating from a nonstereospecific electrophilic addition of HOCl to the C5&dbond;C6 double bond of the pyridine ring. The primary products (Py/X) of NMNH all exhibit similar absorption bands around 275 nm and are hence likely to result from analogous addition of HOX to the C5&dbond;C6 bond of the pyridine ring. Since the Py/X species are stable and inert toward endogeneous reductants like ascorbate and GSH, they may generally be useful markers for assessing the contribution of hypohalous acids to inflammatory injury.     

Mechanism of reaction of horseradish peroxidase with chlorite and chlorine dioxide

It is demonstrated that horseradish peroxidase (HRP) mixed with chlorite follows the whole peroxidase cycle. Chlorite mediates the two-electron oxidation of ferric HRP to compound I (k(1)) thereby releasing hypochlorous acid. Furthermore, chlorite acts as one-electron reductant of both compound I (k(2)) and compound II (k(3)) forming chlorine dioxide. The strong pH-dependence of all three reactions clearly suggests that chlorous acid is the reactive species. Typical apparent bimolecular rate constants at pH 5.6 are 1.4 x 10(5)M(-1)s(-1) (k(1)), 2.25 x 10(5)M(-1)s(-1) (k(2)), and 2.4 x 10(4)M(-1)s(-1) (k(3)), respectively. Moreover, the reaction products hypochlorous acid and chlorine dioxide, which are known to induce heme bleaching and amino acid modification upon longer incubation times, also mediate the oxidation of ferric HRP to compound I (2.4 x 10(7)M(-1)s(-1) and 2.7 x 10(4)M(-1)s(-1), respectively, pH 5.6) but do not react with compounds I and II. A reaction scheme is presented and discussed from both a mechanistic and thermodynamic point of view. It helps to explain the origin of contradictory data so far found in the literature on this topic.     

The free amino acid tyrosine enhances the chlorinating activity of human myeloperoxidase

A key function of neutrophil myeloperoxidase (MPO) is the synthesis of hypochlorous acid (HOCl), a potent oxidizing agent that plays a cytotoxic role against invading bacteria and viruses at inflammatory sites and in phagosomes. MPO displayed a chlorinating activity preferably at acidic pH but at neutral pH MPO catalyzes mainly reactions of the peroxidase cycle. In the present work effects of tyrosine on the chlorinating activity of MPO were studied. At pH 7.4 we detected an increased HOCl production in the presence of tyrosine not only by the MPO-H₂O₂-Cl^- system but also in suspensions of zymosan-activated neutrophils. An excess of H₂O₂ is known to cause an accumulation of compound II of MPO blocking the generation of HOCl at neutral pH. As evidenced by spectral changes, tyrosine-induced activation of MPO to synthesize HOCl was due to the ability of tyrosine to reduce compound II back to the native state, thus accelerating the enzyme turnover. MPO-induced oxidation of tyrosine is relevant to what can be in vivo; we detected MPO-catalyzed formation of dityrosine in the presence of plasma under experimental conditions when tyrosine concentration was about three magnitudes of order less than the Cl⁻ concentration. At acidic pH formation of compound II was impaired in the presence of chloride and dityrosine couldn't be detected in plasma. In conclusion, the ability of tyrosine to increase the chlorinating activity of MPO at neutral pH and enhanced values of H₂O₂ may be very effective for the specific enhancement of HOCl production under acute inflammation.     

Reactions of pholasin with peroxidases and hypochlorous acid

The ability of myeloperoxidase (MPO) and horseradish peroxidase (HRP) to induce chemiluminescence (CL) in Pholasin (Knight Scientific, Plymouth, UK), the photoprotein of the Common Piddock Pholas dactylus, was studied. The oxidation of Pholasin by compound I or II of HRP induced an intense light emission, whereas native HRP showed only a small effect. The luminescence observed upon incubation of Pholasin with native MPO was diminished by preincubation with catalase. Considering the high instability of diluted MPO, it is concluded that traces of hydrogen peroxide in water converted MPO to its active forms, compound I and/or II, which are able to oxidize Pholasin. Indeed, the addition of hydrogen peroxide to a mixture of MPO and Pholasin induced an intense burst of light. This emission was enhanced in degree and duration in the absence of chloride. Hypochlorous acid, the reaction product of Cl(-) and compound I of MPO, was itself able to elicit a luminescent response in Pholasin and this luminescence was strongly inhibited by methionine and taurine. However, both of these HOCl scavengers only slightly reduced the light emission induced by MPO/H(2)O(2) in both the presence or absence of chloride. Thus, hypochlorous acid produced by the MPO/H(2)O(2)/Cl(-) system, under the conditions described in this study, did not contribute to Pholasin luminescence. The Pholasin luminescence elicited by formyl-leucyl-methionyl-phenylalanine (fMLP)-stimulated neutrophils depends both on superoxide anion radicals and higher oxidation states of myeloperoxidase (but not on hypochlorous acid). This is shown by the inhibition of luminescence with superoxide dismutase and potassium cyanide, together with the lack of effect of both methionine and taurine. The luminescence response is about eight times greater in cells stimulated with fMLP/cytochalasin B than with fMLP alone.     

The mechanism of myeloperoxidase-dependent chlorination of monochlorodimedon

Chlorination of monochlorodimedon is routinely used to measure the production of hypochlorous acid catalysed by myeloperoxidase from H2O2 and Cl-. We have found that the myeloperoxidase/H2O2/Cl- system, at pH 7.8, catalysed the loss of monochlorodimedon with a rapid burst phase followed by a much slower steady-state phase. The loss of monochlorodimedon in the absence of Cl- was only 10% of the steady-state rate in the presence of Cl-, which indicates that the major reaction of monochlorodimedon was with hypochlorous acid. During the steady-state reaction, myeloperoxidase was present as 100% compound II, which cannot participate directly in hypochlorous acid formation. Monochlorodimedon was necessary for formation of compound II, since it was not formed in the presence of methionine. Both the amount of hypochlorous acid formed during the burst phase, and the steady-state rate of hypochlorous acid production, increased with increasing concentrations of myeloperoxidase and with decreasing concentrations of monochlorodimedon. Inhibition by monochlorodimedon was competitive with Cl-. From these results, and the ability of myeloperoxidase to slowly peroxidase monochlorodimedon in the absence of Cl-, we propose that the reaction of monochlorodimedon with the myeloperoxidase/H2O2/Cl- system involves a major pathway due to hypochlorous acid-dependent chlorination and a minor peroxidative pathway. Only a small fraction of compound I needs to react with monochlorodimedon instead of Cl- at each enzyme cycle, for compound II to rapidly accumulate. Monochlorodimedon, therefore, cannot be regarded as an inert detector of hypochlorous acid production by myeloperoxidase, but acts to limit the chlorinating activity of the enzyme. In the presence of reducing species that act like monochlorodimedon, the activity of myeloperoxidase would depend on the rate of turnover of compound II. Components of human serum promoted the conversion of ferric-myeloperoxidase to compound II in the presence of H2O2. We suggest, therefore, that in vivo the rate of turnover of compound II may determine the rate of myeloperoxidase-dependent production of hypochlorous acid by stimulated neutrophils.     

Oxidation of NADH by chloramines and chloramides and its activation by iodide and by tertiary amines

Irreversible oxidation of reduced nicotinamide nucleotides by neutrophil-derived halogen oxidants (HOCl, chloramines, HOBr, etc.) is likely to be a highly lethal process, because of the essential role of NAD(P)H in important cell functions such as mitochondrial electron transport, and control of the cellular thiol redox state by NADPH-dependent glutathione reductase. Chloramines (chloramine-T, NH(2)Cl, etc.) and N-chloramides (N-chlorinated cyclopeptides) react with NADH to generate the same products as HOCl, i.e., pyridine chlorohydrins, as judged from characteristic changes in the NADH absorption spectrum. Compared with the fast oxidation of NADH by HOCl, k approximately 3 x 10(5) M(-1) s(-1) at pH 7.2, the oxidation by chloramines is about five orders of magnitude slower; that by chloramides is about four orders of magnitude slower. Apparent rate constants for oxidation of NADH by chloramines increase with increasing proton or buffer concentration, consistent with general acid catalysis, but oxidation by chloramides proceeds with pH-independent kinetics. In presence of iodide the oxidation of NADH by chloramines or chloramides is faster by at least two orders of magnitude; this is due to reaction of iodide with the N-halogen to give HOI/I(2), the most reactive and selective oxidant for NADH among HOX species. Quinuclidine derivatives (QN) like 3-chloroquinuclidine and quinine are capable of catalyzing the irreversible degradation of NADH by HOCl and by chloramines; QN(+)Cl, the chain carrier of the catalytic cycle, is even more reactive toward NADH than HOCl/ClO(-) at physiological pH. Oxidation of NADH by NH(2)Br proceeds by fast, but complex, biphasic kinetics. A compilation of rate constants for interactions of reactive halogen species with various substrates is presented and the concept of selective reactivity of N-halogens is discussed.     

Role of monochloramine in the oxidation of erythrocyte hemoglobin by stimulated neutrophils

Stimulation of the oxygen (O2) metabolism of isolated human neutrophilic leukocytes resulted in oxidation of hemoglobin of autologous erythrocytes without erythrocyte lysis. Hb oxidation could be accounted for by reduction of O2 to superoxide (O-2) by the neutrophils, dismutation of O-2 to yield hydrogen peroxide (H2O2), myeloperoxidase-catalyzed oxidation of chloride (Cl-) by H2O2 to yield hypochlorous acid (HOCl), the reaction of HOCl with endogenous ammonia (NH+4) to yield monochloramine ( NH2Cl ), and the oxidative attack of NH2Cl on erythrocytes. NH2Cl was detected when HOCl reacted with the NH+4 and other substances released into the medium by neutrophils. The amount of NH+4 released was sufficient to form the amount of NH2Cl required for the observed Hb oxidation. Oxidation was increased by adding myeloperoxidase or NH+4 to increase NH2Cl formation. Due to the volatility of NH2Cl , Hb was oxidized when neutrophils and erythrocytes were incubated separately in a closed container. Oxidation was decreased by adding catalase to eliminate H2O2, dithiothreitol to reduce HOCl and NH2Cl , or taurine to react with HOCl or NH2Cl to yield taurine monochloramine . NH2Cl was up to 50 times more effective than H2O2, HOCl, or taurine monochloramine as an oxidant for erythrocyte Hb, whereas HOCl was up to 10 times more effective than NH2Cl as a lytic agent. NH2Cl contributes to oxidation of erythrocyte components by stimulated neutrophils and may contribute to other forms of neutrophil oxidative cytotoxicity.     

(-)-Epicatechin enhances the chlorinating activity of human myeloperoxidase

The heme-containing enzyme myeloperoxidase (MPO) accumulates at inflammatory sites and is able to catalyse one- and two-electron oxidation reactions. Here it is shown that (-)-epicatechin, which is known to have numerous beneficial health effects, in low micromolar concentration enhances the degradation of monochlorodimedon (MCD) or the chlorination of taurine in a concentration-dependent bell-shaped manner whereas at higher concentrations it sufficiently suppresses the release of hypochlorous acid. Presented reaction mechanisms demonstrate the efficiency of micromolar concentrations of the flavan-3-ol in overcoming the accumulation of compound II that does not participate in the chlorination cycle. In case of MCD the mechanism is more complicated since it also acts as peroxidase substrate with very different reactivity towards compound I (3 × 10⁵ M⁻¹ s⁻¹) and compound II (8.8 M⁻¹ s⁻¹) at pH 7. By affecting the chlorinating activity of myeloperoxidase (-)-epicatechin may participate in regulation of immune responses at inflammatory sites.     

Hypochlorous acid-induced DNA base modification: potentiation by nitrite: biomarkers of DNA damage by reactive oxygen species

Chronic inflammation results in increased nitric oxide formation and nitrite (NO-2) accumulation. Activated phagocytes release myeloperoxidase generating the cytotoxic agent hypochlorous acid (HOCl). Reaction of HOCl with NO-2 results in the formation of nitryl chloride (NO2Cl), a potent oxidising, nitrating and chlorinating species. Exposure of DNA to NO-2 alone (up to 250 microM) at pH 7.4 did not induce oxidative DNA base damage. However, incubation of DNA with NO-2 in the presence of HOCl led to increases in thymine glycol, 5-hydroxyhydantoin, 8-hydroxyadenine and 5-chlorouracil to levels higher than those achieved by HOCl alone. No significant increases in 8-hydroxyguanine, xanthine, hypoxanthine, 2-hydroxyadenine, FAPy guanine, FAPy adenine and 8-chloroadenine were observed. HOCl-induced depletion of FAPy guanine and 8-hydroxyguanine was reduced in the presence of NO-2. Modification of DNA by HOCl/NO-2 (presumably generating NO2Cl) produces a pattern of DNA base damage products in isolated DNA that is similar to the pattern produced by HOCl but not other reactive species.     

On the oxidation of cytochrome c by hypohalous acids

Oxidation of cytochrome c, a key protein in mitochondrial electron transport and a mediator of apoptotic cell death, by reactive halogen species (HOX, X2), i.e., metabolites of activated neutrophils, was investigated by stopped-flow. The fast initial reactions between FeIIIcytc and HOX species, with rate constants (at pH 7.6) of k > 3 x 10(6) M(-1) s(-1) for HOBr, k > 3 x 10(5) M(-1) s(-1) for HOCl, and k = (6.1+/-0.3) x 10(2) M(-1) s(-1) for HOI, are followed by slower intramolecular processes. All HOX species lead to a blue shift of the Soret absorption band and loss of the 695-nm absorption band, which is an indicator for the intact iron to Met-80 bond, and of the reducibility of FeIIIcytc. All HOX species do, in fact, persistently impair the ability of FeIIIcytc to act as electron acceptor, e.g., in reaction with ascorbate or O2*-. I2 selectively oxidizes the iron center of FeIIcytc, with a stoichiometry of 2 per I2, and with k(FeIIcytc + I2) approximately 4.6 x 10(4) M(-1) s(-1) and k(FeIIcytc + I2*-) = (2.9+/-0.4) x 10(8) M(-1) s(-1). Oxidation of FeIIcytc by HOX species is not selectively directed toward the iron center; HOBr and HOCl are considered to react primarily by N-halogenation of side chain amino groups, and HOI mainly by sulfoxidation. There is some evidence for the generation of HO* radicals upon reaction of HOCl with FeIIcytc. Chloramines (e.g., NH2Cl), bromamine (NH2Br), and cyclo-Gly2 chloramide oxidize FeIIcytc slowly and unselectively, but iodide efficiently catalyzes reactions of these N-halogens to yield fast selective oxidation of the iron center; this is due to generation of I2 by reaction of I- with the N-halogen and recycling of I- by reaction of I2 with FeIIcytc. Iodide also catalyzes methionine sulfoxidation and thiol oxidation by NH2Cl. The possible biological relevance of these findings is discussed.     

Investigation of the reaction of peroxynitrite with propofol at acid pH: predominant production of oxidized, nitrated, and halogenated derivatives.

We reported here the reaction, in acidic conditions, of peroxynitrite (ONOO(-)) with the anaesthetic agent propofol (2,6-diisopropylphenol, PPF). The most interesting finding is that peroxynitrite is able to nitrate and to oxidize propofol leading to 4-nitropropofol, quinone, and diphenylquinone as the major products. More surprisingly, we also found that peroxynitrite is capable of halogenating propofol in the presence of halide ions, suggesting the formation of nitrosyl chloride (NOCl) or nitryl chloride (NO(2)Cl) from the reaction of peroxynitrite with chloride ions. A significant enhancement of the halogenation yield is observed with a simultaneous decrease of the yields of the other products in the presence of methanol or hydrogen peroxide. Increased halogenation of PPF probably results from the formation of peroxynitrate (O(2)NOO(-)), that further oxidizes chloride ions in hypochlorous acid (HOCl) or molecular chlorine (Cl(2)). Spontaneous decay of peroxynitrate is relatively slow in acidic medium, thus explaining the decrease of the yields of the other products. By direct EPR techniques, we also observed that this reaction occurs via a radical pathway.     

A kinetic analysis of the catalase activity of myeloperoxidase

The predominant physiological activity of myeloperoxidase is to convert hydrogen peroxide and chloride to hypochlorous acid. However, this neutrophil enzyme also degrades hydrogen peroxide to oxygen and water. We have undertaken a kinetic analysis of this reaction to clarify its mechanism. When myeloperoxidase was added to hydrogen peroxide in the absence of reducing substrates, there was an initial burst phase of hydrogen peroxide consumption followed by a slow steady state loss. The kinetics of hydrogen peroxide loss were precisely mirrored by the kinetics of oxygen production. Two mols of hydrogen peroxide gave rise to 1 mol of oxygen. With 100 microM hydrogen peroxide and 6 mM chloride, half of the hydrogen peroxide was converted to hypochlorous acid and the remainder to oxygen. Superoxide and tyrosine enhanced the steady-state loss of hydrogen peroxide in the absence of chloride. We propose that hydrogen peroxide reacts with the ferric enzyme to form compound I, which in turn reacts with another molecule of hydrogen peroxide to regenerate the native enzyme and liberate oxygen. The rate constant for the two-electron reduction of compound I by hydrogen peroxide was determined to be 2 x 10(6) M(-1) s(-1). The burst phase occurs because hydrogen peroxide and endogenous donors are able to slowly reduce compound I to compound II, which accumulates and retards the loss of hydrogen peroxide. Superoxide and tyrosine drive the catalase activity because they reduce compound II back to the native enzyme. The two-electron oxidation of hydrogen peroxide by compound I should be considered when interpreting mechanistic studies of myeloperoxidase and may influence the physiological activity of the enzyme.     

Human hemi-myeloperoxidase. Initial chlorinating activity at neutral pH, compound II and III formation, and stability towards hypochlorous acid and high temperature.

Human neutrophilic myeloperoxidase (MPO) is involved in the defence mechanism of the body against micro-organisms. The enzyme catalyses the generation of the strong oxidant hypochlorous acid (HOCl) from hydrogen peroxide and chloride ions. In normal neutrophils MPO is present in the dimeric form (140 kDa). The disulphide-linked protomers each consist of a heavy subunit and a light one. Reductive alkylation converts the dimeric enzyme into two promoters, 'hemi-myeloperoxidase'. We studied the initial activities of human dimeric MPO and hemi-MPO at the physiological pH of 7.2 and found no significant differences in chlorinating activity. These results indicate that, at least at neutral pH, the protomers of MPO function independently. The absorption spectra of MPO compounds II and III, both inactive forms concerning HOCl generation, and the rate constants of their formation were the same for dimeric MPO and hemi-MPO, but hemi-MPO required a slightly larger excess of H2O2 for complete conversion. Hemi-MPO was less stable at a high temperature (80 degrees C) as compared to the dimeric enzyme. Furthermore, the resistance of the chlorinating activity of hemi-MPO against its oxidative product hypochlorous acid was somewhat lower (IC50 = 32 microM HOCl) compared to dimeric MPO (IC50 = 50 microM HOCl). The higher stability of dimeric MPO in the presence of its oxidative product compared to that of monomeric MPO might be the reason for the occurrence of MPO as a dimer.     

The reactivity of myeloperoxidase compound I formed with hypochlorous acid

The reaction of human myeloperoxidase (MPO) with hypochlorous acid (HOCl) was investigated by conventional stopped-flow spectroscopy at pH 5, 7, and 9. In the reaction of MPO with HOCl, compound I is formed. Its formation is strongly dependent on pH. HOCl (rather than OCl-) reacts with the unprotonated enzyme in its ferric state. Apparent second-order rate constants were determined to be 8.1 x 10(7) M(-1)s(-1) (pH 5), 2.0 x 10(8) M(-1)s(-1) (pH 7) and 2.0 x 10(6) M(-1)s(-1) (pH 9) at 15 degrees C. Furthermore, the kinetics and spectra of the reactions of halides and thiocyanate and of physiologically relevant one-electron donors (ascorbate, nitrite, tyrosine and hydrogen peroxide) with this compound I were investigated using the sequential-mixing technique. The results show conclusively that the redox intermediates formed upon addition of either hydrogen peroxide or hypochlorous acid to native MPO exhibit the same spectral features and reactivities and thus are identical. In stopped-flow investigations, the MPO/HOCl system has some advantage since: (i) in contrast to H2O2, HOCl cannot function as a one-electron donor of compound I; and (ii) MPO can easily be prevented from cycling by addition of methionine as HOCl scavenger. As a consequence, the observed absorbance changes are bigger and errors in data analysis are smaller.     

Chlorination of pyridinium compounds. Possible role of hypochlorite, N-chloramines, and chlorine in the oxidation of pyridinoline cross-links of articular cartilage collagen type II during acute inflammation

Reactive oxygen species produced by activated neutrophils and monocytes are thought to be involved in mediating the loss of collagen and other matrix proteins at sites of inflammation. To evaluate their potential to oxidize the pyridinoline (Pyd) cross-links found in collagen types I and II, we reacted hydrogen peroxide (H(2)O(2)), hypochlorous acid/hypochlorite (HOCl/OCl(-)), and singlet oxygen (O(2)((1)delta g)) with the Pyd substitutes, pyridoxamine dihydrochloride and vitamin B(6), which share the same chemical structure and spectral properties of Pyd cross-links. Neither H(2)O(2) (125-500 microm) nor O(2)((1)delta g) (10-25 microm) significantly changed the spectral properties of pyridoxamine or vitamin B(6). Reaction of HOCl/OCl(-) (12.5-50 microm) with pyridoxamine at pH 7.2 resulted in a concentration-dependent appearance of two new absorbance peaks and a decrease in fluorescence at 400 nm (excitation 325 nm). The new absorbance peaks correlated with the formation of an N-chloramine and the product of its subsequent reaction with pyridoxamine. In contrast, the extent to which HOCl reacted with vitamin B(6), which lacks a primary amine group, was variable at this pH. At lysosomal pH 5.5, Cl(2)/HOCl/OCl(-) reacted with both pyridoxamine and vitamin B(6). Four of the chlorinated products of this reaction were identified by gas chromatography-mass spectrometry and included 3-chloropyridinium, an aldehyde, and several chlorinated products with disrupted rings. To evaluate the effects of Cl(2)/HOCl/OCl(-) on Pyd cross-links in collagen, we exposed bone collagen type I and articular cartilage type II to HOCl. Treatment of either collagen type with HOCl at pH 5. 0 or 7.2 resulted in the oxidation of amine groups and, for collagen type II, the specific decrease in Pyd cross-link fluorescence, suggesting that during inflammation both oxidations may be used by neutrophils and monocytes to promote the loss of matrix integrity.