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PubMed1996

Rapid oxidation of DL-selenomethionine by peroxynitrite.

Peroxynitrite, the reaction product of nitric oxide and superoxide, rapidly oxidizes DL-selenomethionine (MetSe) with overall second-order kinetics, first-order in peroxynitrite and first-order in MetSe. The oxidation of MetSe by peroxynitrite goes by two competing mechanism. The first produces ethylene by what we propose to be a one-electron oxidation of MetSe. In the second mechanism, MetSe undergoes a two-electron oxidation that gives methionine selenoxide (MetSe = O); the apparent second-order rate constant, k2(app), for this process is (2.4 +/- 0.1) x 10(3) M-1s-1 at pH 7.4 and 25 degrees C. The kinetic modeling of the experimental data suggests that both peroxynitrous acid (k2 = 20,460 +/- 440 M-1s-1 at 25 degrees C) and the peroxynitrite anion (k3 = 200 +/- 170 M-1s-1 at 25 degrees C) are involved in the second-order reaction leading to selenoxide. These rate constants are 10- to 1,000-fold higher than those for the reactions of methionine (Met) with peroxynitrite. With increasing concentrations of MetSe at pH 7.4, the yield of ethylene decreases, while that of MetSe = O increases, suggesting that the reactions leading to ethylene and selenoxide have different kinetic orders. These results are analogous to those we previously reported for methionine and 2-keto-4-thiomethylbutanoic acid (KTBA),where ethylene is produced in a first-order reaction and sulfoxide in a second-order reaction. Therefore, we suggest that the reaction of peryoxynitrite with MetSe involves a mechanism similar to that we proposed for Met, in which an activated intermediate of peroxynitrous acid (HOONO) is the one-electron oxidant and reacts with first-order kinetics and ground-state peroxynitrite is the two-electron oxidant and reacts with second-order kinetics.

Chromatography, Gas↗

PubMed1996

Peroxynitrite-dependent tryptophan nitration.

Peroxynitrite (ONOO-), the reaction product of superoxide (O2.-) and nitric oxide (.NO), nitrates tyrosine and other phenolics. We report herein that tryptophan is also nitrated by peroxynitrite in the absence of transition metals to one predominant isomer of nitrotryptophan, as determined from spectral characteristics and liquid chromatography-mass spectrometry analysis. At high peroxynitrite to tryptophan ratios, other oxidation products were detected as well. The amount of nitrotryptophan formed from peroxynitrite increased at acidic pH, with an apparent pKa of 7.8. High concentrations of Fe(3+)-EDTA were required to enhance peroxynitrite-induced nitrotryptophan formation, while addition of up to 15 microM Cu/Zn superoxide dismutase had a minimal effect on tryptophan nitration. Cysteine, ascorbate, and methionine decreased nitrotryptophan yield to an extent similar to that predicted by their reaction rates with ground-state peroxynitrite, and typical hydroxyl radical scavengers partially inhibited nitration. Plots of the observed rate constant of nitrotryptophan formation vs tryptophan concentration presented downward curvatures. Thus, the kinetics of metal-independent nitration reactions were interpreted in terms of two parallel mechanisms. In the first one, ground-state peroxynitrous acid nitrated tryptophan with a second-order rate constant of 184 +/- 11 M-1 s-1 at 37 degrees C. The activation enthalpy was 9.1 +/- 0.3 kcal mol-1, and the activation entropy was -19 +/- 1 cal mol-1 K-1. In the second mechanism, ONOOH*, an activated intermediate derived from trans-peroxynitrous acid formed in a steady state, was the nitrating agent.

Deferoxamine↗

PubMed1993

Interaction of myeloperoxidase with peroxynitrite. A comparison with lactoperoxidase, horseradish peroxidase and catalase.

Polymorphonuclear neutrophils generate both nitric oxide and superoxide and these molecules can combine to form peroxynitrite. Neutrophils also contain myeloperoxidase which reacts with peroxynitrous acid (HOONO). On mixing myeloperoxidase with HOONO compound II was formed. Compound I could not be detected as an intermediate. The apparent second-order rate constant of formation of compound II was strongly pH-dependent (2.5 x 10(5) M-1 x s-1 at pH 8.9 and 6.2 x 10(6) M-1 x s-1 at pH 7.2). The pKa of this effect is 6.9 and it was concluded that the enzyme reacts with the protonated form of the peroxide, that is peroxynitrous acid, with a pH-independent second-order rate constant of 2.0 x 10(7) M-1 x s-1 at 12 degrees C. The interaction of HOONO with lactoperoxidase was studied for comparison. As was observed for myeloperoxidase, compound I could not be detected as an intermediate. The apparent second-order rate constant of compound II formation is pH-dependent and is 3.3 x 10(5) M-1 x s-1 at pH 7.4 and 8.4 x 10(4) M-1 x s-1 at pH 9.0. In contrast, horseradish peroxidase reacts with HOONO to form compound I, which is subsequently followed by the formation of compound II. The second-order rate constant for the formation of compound I is 3.2 x 10(6) M-1 x s-1 and is pH-dependent, the pKa for this effect is 6.8. Catalase (up to 3 microM) does not affect the rate of decomposition of peroxynitrite and no compound I formation is observed. Since nitrite may be present in the peroxynitrite preparation and to discriminate between the reaction of the enzyme with nitrite or peroxynitrite, the effect of nitrite on myeloperoxidase was studied. The dissociation constant for the myeloperoxidase-nitrite complex is pH-dependent and has values of 580 microM at pH 6.0 and 55 mM at pH 8.5.

Catalase↗

PubMed1996

Peroxynitrite mediated oxidation of purine bases of nucleosides and isolated DNA.

Reaction of nitric oxide with superoxide anion produces the highly reactive species peroxynitrite (ONOO-). This compound has been shown to be a strong oxidant of lipids and proteins. However, no data are available on its effect on DNA, with the exception of the induction of strand breaks. We report the result of studies on the reactions of peroxynitrite with the adenine and guanine moieties of nucleosides and isolated DNA. The samples were analyzed for 8-oxo-7,8-dihydro-2'-deoxyguanosine (8-oxo-dGuo),2,2-diamino-4-[(2-deoxy-beta-D-erythro-pentofuranosyl) amino]-5-(2H)-oxazolone (oxazolone) and 8-oxo-7,8-dihydro-2'-deoxyadenosine (8-oxo-dAdo). The effects of peroxynitrite treatment were compared with those of ionizing radiation in aerated aqueous solution, chosen as a source of hydroxyl radicals. At the nucleoside level, both oxidizing conditions led to the formation of oxazolone and 8-oxo-dAdo. In addition, evidence was provided for the formation of the 4R* and 4S* diastereoisomers of 4-hydroxy-8-oxo-4, 8-dihydro-2'-deoxyguanosine. The latter dGuo oxidation products were chosen as markers of the release of singlet oxygen (1O2) upon reaction of peroxynitrous acid with hydrogen peroxide. Oxidation of purine bases was then studied within isolated DNA. A significant increase in the level of 8-oxo-dGuo, oxazolone and 8-oxo-dAdo was observed within double stranded DNA upon exposure to gamma-radiation. Oxazolone and 8-oxo-dAdo were formed upon peroxynitrite treatment but no significant increase in the amount of 8-oxo-dGuo was detected. These results showed that peroxynitrite exhibits oxidizing properties toward purine moieties both in nucleosides and isolated DNA. However, the significant differences in the oxidative damage distribution within DNA observed after exposure to gamma radiation by comparison with peroxynitrite treatment questions the involvement of hydroxyl radicals as the main oxidizing species released by decomposition of peroxynitrous acid.

DNA↗

PubMed1997

Thermodynamics of peroxynitrite and its CO2 adduct.

The equilibrium constant, K3, of aqueous homolysis of peroxynitrous acid into hydroxyl and nitrogen dioxide free radicals was estimated to be 5 x 10(-10) M. This value was derived from a thermodynamic cycle by use of the experimentally known delta fH degree(ONOO-,aq) = -10.8 kcal/mol and the enthalpy of ionic dissociation of ONOOH(aq), delta H degree 1 = 0 kcal/mol, as well as of the entropy of gaseous ONOOH, S degree(ONOOH,g) = 72 eu. Furthermore we assumed the entropy of hydration of ONOOH, delta S degree 2, to be -25 eu, a value closely bracketed by the hydration entropies of analogous substances. The rate constant of radical recombination of OH. with NO2. to yield ONOOH, k-3, was resimulated from experimental data and found to be ca. 5 x 10(9) M-1 s-1. Together with the estimated K3, this yields the homolysis rate constant k3 = 2.5 s-1. This value is close to 0.5 s-1, the rate constant of formation of a reactive intermediate during the isomerization of peroxynitrous acid to nitrate. Our thermodynamic estimate is therefore consistent with substantial amounts of OH. and NO2. free radicals being formed in this process. The thermodynamic implications for the carbon dioxide/peroxynitrite system are also discussed.

Carbon Dioxide↗

PubMed2002

Reactive oxygen and nitrogen species and cellular and organismal decline: amelioration with melatonin.

Cellular and organismal decline is, in part, believed to be a consequence of oxygen and nitrogen-based reactants which persistently damage macromolecules throughout a lifetime. The resulting accumulation of damaged molecules eventually seriously compromises essential functions of cells leading to their death. Excessive cellular loss causes deterioration of organ function and inevitably to the demise of the organism. The sequence of events, known as the free radical theory of aging, is widely espoused by biological gerontologists. Antioxidants are commonly employed to combat molecular damage mediated by oxygen and nitrogen-based reactants. One of these protective agents is melatonin. Melatonin has several distinct advantages as a preserver of organelle structure and function. It is widely distributed in organisms and within cells. It works via a number of mechanisms to reduce oxidative damage. Thus, melatonin scavenges a number of reactants including the hydroxyl radical (*OH), hydrogen peroxide (H(2)O(2)), nitric acid (NO*), peroxynitrite (ONOO(-)) and peroxynitrous acid (ONOOH). One of the products of melatonin's interaction with H(2)O(2), i.e., N(1)-acetyl-N(2)-formyl-5-methoxykynuramine (AFMK), is also a highly efficient radical scavenger. The cascade of reactions where the secondary metabolites are also effective scavenges is believed to contribute to melatonin's high efficacy in reducing oxidative damage. Besides its direct scavenging actions, melatonin stimulates several antioxidative enzymes including superoxide dismutase, glutathione peroxidase and glutathione reductase in addition to inhibiting a proxidative enzyme, nitric oxide synthase. This combination of actions assists melatonin in protecting cells from the degenerative changes normally associated with aging and age-related diseases.

Aging↗

PubMed2001

Biochemical reactivity of melatonin with reactive oxygen and nitrogen species: a review of the evidence.

Melatonin (N-acetyl-5-methoxytryptamine), an endogenously produced indole found throughout the animal kingdom, was recently reported, using a variety of techniques, to be a scavenger of a number of reactive oxygen and reactive nitrogen species both in vitro and in vivo. Initially, melatonin was discovered to directly scavenge the high toxic hydroxyl radical (*OH). The methods used to prove the interaction of melatonin with the *OH included the generation of the radical using Fenton reagents or the ultraviolet photolysis of hydrogen peroxide (H202) with the use of spin-trapping agents, followed by electron spin resonance (ESR) spectroscopy, pulse radiolysis followed by ESR, and several spectrofluorometric and chemical (salicylate trapping in vivo) methodologies. One product of the reaction of melatonin with the *OH was identified as cyclic 3-hydroxymelatonin (3-OHM) using high-performance liquid chromatography with electrochemical (HPLC-EC) detection, electron ionization mass spectrometry (EIMS), proton nuclear magnetic resonance (1H NMR) and COSY 1H NMR. Cyclic 3-OHM appears in the urine of humans and other mammals and in rat urine its concentration increases when melatonin is given exogenously or after an imposed oxidative stress (exposure to ionizing radiation). Urinary cyclic 3-OHM levels are believed to be a biomarker (footprint molecule) of in vivo *OH production and its scavenging by melatonin. Although the data are less complete, besides the *OH, melatonin in cell-free systems has been shown to directly scavenge H2O2, singlet oxygen (1O2) and nitric oxide (NO*), with little or no ability to scavenge the superoxide anion radical (O2*-) In vitro, melatonin also directly detoxifies the peroxynitrite anion (ONOO-) and/or peroxynitrous acid (ONOOH), or the activated form of this molecule, ONOOH*; the product of the latter interaction is proposed to be 6-OHM. How these in vitro findings relate to the in vivo antioxidant actions of melatonin remains to be established. The ability of melatonin to scavenge the lipid peroxyl radical (LOO*) is debated. The weight of the evidence is that melatonin is probably not a classic chain-breaking antioxidant, since its ability to scavenge the LOO* seems weak. Its ability to reduce lipid peroxidation may stem from its function as a preventive antioxidant (scavenging initiating radicals), or yet unidentified actions. In sum, in vitro melatonin acts as a direct free radical scavenger with the ability to detoxify both reactive oxygen and reactive nitrogen species; in vivo, it is an effective pharmacological agent in reducing oxidative damage under conditions in which excessive free radical generation is believed to be involved.

Animals↗

PubMed2002

Peroxynitrite reaction with the reduced and the oxidized forms of lipoic acid: new insights into the reaction of peroxynitrite with thiols.

Thiols represent preferential targets of peroxynitrite in biological systems. In this work, we investigated the mechanisms and kinetics of the reaction of peroxynitrite with the dithiol dihydrolipoic acid (DHLA) and its oxidized form, lipoic acid (LA). Peroxynitrite reacted with DHLA being oxidation yields higher at alkaline pH. The stoichiometry for the reaction was two thiols oxidized per peroxynitrite. LA formation accounted for approximately 50% DHLA consumption at pH 7.4, probably reflecting secondary reactions between LA and peroxynitrite. Indeed, peroxynitrous acid reacted with LA with an apparent second-order rate constant (k(2app)) of 1400 M(-1) s(-1) at pH 7.4 and 37 degrees C. Nitrite and LA-thiosufinate were formed as reaction products. Surprisingly, the k(2app) for peroxynitrite-dependent DHLA oxidation was only 250 M(-1) s(-1) per thiol, at pH 7.4 and 37 degrees C. Testing various low-molecular-weight thiols, we found that an increase in the thiol pK (pK(SH)) value correlated with a decrease of k(2app) for the reaction with peroxynitrite at pH 7.4. The pK(SH) for DHLA is 10.7, in agreement with its modest reactivity with peroxynitrite.

8,11,14-Eicosatrienoic Acid↗

PubMed1999

Uric acid oxidation by peroxynitrite: multiple reactions, free radical formation, and amplification of lipid oxidation.

Uric acid has been considered to be an efficient scavenger of peroxynitrite but the reaction between urate and peroxynitrite has been only partially characterized. Also, previous studies have indicated that urate may increase peroxynitrite-mediated oxidation of low density lipoprotein (LDL). Here, we examined the reaction between urate and peroxynitrite by combining kinetic, oxygen consumption, spin trapping, and product identification studies; in parallel, we tested the effect of urate upon peroxynitrite-mediated lipid oxidation. Our results demonstrated that urate reacts with peroxynitrite with an apparent second order rate constant of 4.8 x 10(2) M(-1). s(-1) in a complex process, which is accompanied by oxygen consumption and formation of allantoin, alloxan, and urate-derived radicals. The main radical was identified as the aminocarbonyl radical by the electrospray mass spectra of its 5, 5-dimethyl-l-pyrroline N-oxide adduct. Mechanistic studies suggested that urate reacts with peroxynitrous acid and with the radicals generated from its decomposition to form products that can further react with peroxynitrite anion. These many reactions may explain the reported efficiency of urate in inhibiting some peroxynitrite-mediated processes. Production of the aminocarbonyl radical, however, may propagate oxidative reactions. We demonstrated that this radical is likely to be the species responsible for the effects of urate in amplifying peroxynitrite-mediated oxidation of liposomes and LDL, which was monitored by the formation of lipid peroxides and thiobarbituric acid-reactive substances. The aminocarbonyl radical was not detectable during urate attack by other oxidants and consequently it is unlikely to be responsible for all previously described prooxidant effects of uric acid.

Allantoin↗

PubMed1993

Nitric oxide interaction with lactoferrin and its production by macrophage cells studied by EPR and spin trapping.

The production of nitrate (NO3-) and nitrite (NO2-) from macrophage-derived NO was studied using EPR and spin trapping. The formation of NO3- was determined via EPR in reactions involving the iron-binding protein, lactoferrin. The formation of NO2- was determined via EPR/spin trapping in the reaction between NO2- and H2O2. Dissolved nitric oxide (NO.) was reacted with lactoferrin yielding an EPR spectrum (77 degrees K) different from the normal EPR spectrum obtained for lactoferrin, suggesting that NO. interacts with the ferric ions bound to lactoferrin forming a ferric-nitrosyl type complex. The EPR spectrum (77 degrees K) of this ferric-nitrosyl type complex was also observed in the supernatant fluid of macrophage cell suspensions following their stimulation with lipopolysaccharide (LPS). During LPS stimulation of macrophages, these cells generate NO. which in turn produces NO3- and NO2-. The ferric-nitrosyl type complex is formed in a reaction mixture containing apolactoferrin and bicarbonate following the reaction of Fe+2 with NO3-, generated from macrophage-derived NO(.), to produce Fe+3 and NO(.). Furthermore, in an acidic medium, NO2- reacts with H2O2 forming peroxynitrous acid (HOONO) which rapidly decomposes into hydroxyl radicals (.OH) and the nitrogen dioxide (NO2.) radical. In the supernatant fluid of LPS-stimulated macrophage suspensions, the production of .OH was verified by spin trapping using 5,5-dimethyl-1-pyrroline-1-oxide (DMPO) as the spin trap and ethanol as the .OH scavenger. The EPR spectra corresponding to the DMPO-OH and the DMPO-hydroxyethyl adducts were identified.(ABSTRACT TRUNCATED AT 250 WORDS)

Animals↗

PubMed2005

Oxidation of hypotaurine and cysteine sulphinic acid by peroxynitrite.

Peroxynitrite mediates the oxidation of the sulphinic group of both HTAU (hypotaurine) and CSA (cysteine sulphinic acid), producing the respective sulphonates, TAU (taurine) and CA (cysteic acid). The reaction is associated with extensive oxygen uptake, suggesting that HTAU and CSA are oxidized by the one-electron transfer mechanism to sulphonyl radicals, which may initiate an oxygen-dependent radical chain reaction with the sulphonates as final products. Besides the one-electron mechanism, HTAU and CSA can be oxidized by the two-electron pathway, leading directly to sulphonate formation without oxygen consumption. The apparent second-order rate constants for the direct reaction of peroxynitrite with HTAU and CSA at pH 7.4 and 25 degrees C are 77.4+/-5 and 76.4+/-9 M(-1).s(-1) respectively. For both sulphinates, the apparent second-order rate constants increase sharply with decrease in pH, and the sigmoidal curves obtained are consistent with peroxynitrous acid as the species responsible for sulphinate oxidation. The kinetic data, together with changes in oxygen uptake, sulphinate depletion, sulphonate production, and product distribution of nitrite and nitrate, suggest that oxidation of sulphinates by peroxynitrite may take place by the two reaction pathways whose relative importance depends on reagent concentrations and pH value. In the presence of bicarbonate, the direct reaction of sulphinates with peroxynitrite is inhibited and the oxidative reaction probably involves only the radicals *NO2 and CO3*-, generated by decomposition of the peroxynitrite-CO2 adduct.

Bicarbonates↗

PubMed1997

Mercaptoethylguanidine and guanidine inhibitors of nitric-oxide synthase react with peroxynitrite and protect against peroxynitrite-induced oxidative damage.

Nitric oxide (NO) produced by the inducible nitric-oxide synthase (iNOS) is responsible for some of the pathophysiological alterations during inflammation. Part of NO-related cytotoxicity is mediated by peroxynitrite, an oxidant species produced from NO and superoxide. Aminoguanidine and mercaptoethylguanidine (MEG) are inhibitors of iNOS and have anti-inflammatory properties. Here we demonstrate that MEG and related compounds are scavengers of peroxynitrite. MEG caused a dose-dependent inhibition of the peroxynitrite-induced oxidation of cytochrome c2+, hydroxylation of benzoate, and nitration of 4-hydroxyphenylacetic acid. MEG reacts with peroxynitrite with a second-order rate constant of 1900 +/- 64 M-1 s-1 at 37 degrees C. In cultured macrophages, MEG reduced the suppression of mitochondrial respiration and DNA single strand breakage in response to peroxynitrite. MEG also reduced the degree of vascular hyporeactivity in rat thoracic aortic rings exposed to peroxynitrite. The free thiol plays an important role in the scavenging effect of MEG. Aminoguanidine neither affected the oxidation of cytochrome c2+ nor reacted with ground state peroxynitrite, but inhibited the peroxynitrite-induced benzoate hydroxylation and 4-hydroxyphenylacetic acid nitration, indicating that it reacts with activated peroxynitrous acid or nitrogen dioxide. Compounds that act both as iNOS inhibitors and peroxynitrite scavengers may be useful anti-inflammatory agents.

Animals↗

PubMed2003

Melatonin: detoxification of oxygen and nitrogen-based toxic reactants.

In the last decade, melatonin has been found to be highly protective against damage to macromolecules resulting from oxygen and nitrogen-based reactants. Considering this, numerous studies have examined the mechanisms whereby this indoleamine directly detoxifies these damaging agents. The evidence is compelling that melatonin scavenges several oxygen-derived reactive agents including the hydroxyl radical (OH), hydrogen peroxide (H2O2), singlet oxygen (1O2) and hypochlorous acid (HOCl). Additionally, melatonin reportedly reacts with nitric oxide (NO), the peroxynitrite anion (ONOO-) and/or peroxynitrous acid (ONOOH) to detoxify them. In some cases the products that are formed as a consequence of melatonin's scavenging actions have been identified. Whereas the ability of melatonin to neutralize these toxic agents likely accounts, in part, for the antioxidant activity of melatonin, it is not the only means by which melatonin serves to protect molecules from oxygen and nitrogen-based reactive metabolites.

Animals↗

PubMed1995

Stopped-flow kinetic study of the reaction of ascorbic acid with peroxynitrite.

A new mechanism is presented for the oxidation of ascorbate by peroxynitrite. Our mechanism involves the reaction of ascorbate both with ground-state peroxynitrous acid (HOONO) and with a reactive intermediate (HOONO*); the reactive intermediate is postulated to be formed in the decay of HOONO to form nitrate. At physiological pH, the ascorbate monoanion (AH-) is the predominant ascorbate species. The plot of the observed rate constant for peroxynitrite decay (kobs) vs AH- for the reaction of peroxynitrite with AH- shows two regions, one linear and one curved. In the linear region, which involves high AH- concentrations, the reaction is dominated by the bimolecular reaction between HOONO and AH-. At lower AH- concentrations, this bimolecular reaction slows and reactions with both HOONO and HOONO* produce the observed curvature. Analysis of the data leads to the estimation of the ratio of rate constants for the reaction of AH- with HOONO* (k2*) and the decay of HOONO to nitrate (kN), giving the value of k2*/kN = 3158 +/- 505 M-1; and of the rate constant (k2) for the reaction between AH- and HOONO, k2 = 236 +/- 14 M-1 s-1. Ascorbate displays higher selectivity for HOONO* than does methionine or 2-keto-4-thiomethylbutanoic acid, two substrates whose reactivity toward HOONO and HOONO* has previously been reported. The biological relevance of the reaction of ascorbate with peroxynitrite is discussed in terms of the rate constants and the concentrations of AH- typically found in biological systems; ascorbate may react with HOONO*, although the reaction with ground-state HOONO probably is too slow to occur in vivo.

Ascorbic Acid↗

PubMed1996

Modulatory role of nitric oxide on superoxide-dependent luminol chemiluminescence.

Reactive oxygen species are involved in luminol chemiexcitation induced in biological systems, but the contribution of nitrogen-derived oxidants in the process still remains unclear. Herein, we report that luminol chemiluminescence (LCL) induced by a superoxide (O2.-)- and hydrogen peroxide (H2O2)-generating system (2-25 mU/ml xanthine oxidase plus acetaldehyde and oxygen) was markedly inhibited by nitric oxide (.NO) added either as bolus (0-10 microM) or a continuous flow (0-10 microM/min). However, the inhibition of LCL was followed by an overshoot in light emission after most .NO was consumed or the infusion stopped and was due to reactions of remaining peroxynitrite, the product of the reaction between O2.- and .NO, with luminol. Nitric oxide also inhibited peroxynitrite- and glucose oxidase-induced LCL, but no overshoot was observed. On the other hand, a continuous flux of pure peroxynitrite, at 2 to 10 microM/min, induced LCL with quantum yields close to those obtained by identical micromolar fluxes of O2.-, while peroxynitrite formed from the decomposition of the sydnonimine SIN-1 yielded 76% of the chemiluminescence obtained with authentic peroxynitrite. Peroxynitrite-induced LCL was 80 and 55% inhibitable by SOD and catalase, respectively, showing that there were O2.- and H2O2-dependent routes of chemiexcitation. The hydroxyl radical scavengers dimethyl sulfoxide, mannitol, and ethanol and the metal chelator diethylenetriaminepentaacetic acid did not inhibit peroxynitrite-induced LCL while desferrioxamine was an efficient inhibitor of light emission by reaction with an activated state of peroxynitrous acid which is responsible of performing the initial one-electron oxidation of luminol. Our results are consistent with a dual role of .NO in O2.(-)-induced LCL: (I) formation of peroxynitrite which in turn promotes the light-emitting route and (II) reaction with luminol radical intermediates directing the system toward a dark pathway. These considerations are of critical importance when analyzing cell- and tissue-derived LCL in .NO-, O2.(-)-, and peroxynitrite-producing systems.

Acridines↗

PubMed2002

Role of reactive oxygen and nitrogen species in acute respiratory distress syndrome.

Reactive oxygen species are reactive, partially reduced derivatives of molecular oxygen (O 2 ). Important reactive oxygen species in biologic systems include superoxide radical anion, hydrogen peroxide, and hydroxyl radical. Closely related species include the hypohalous acids, particularly hypochlorous acid; chloramine and substituted chloramines; and singlet oxygen. Reactive nitrogen species are derived from the simple diatomic gas, nitric oxide. Peroxynitrite and its protonated form, peroxynitrous acid, are the most significant reactive nitrogen species in biologic systems. A variety of enzymatic and nonenzymatic processes can generate reactive oxygen species and reactive nitrogen species in mammalian cells. An extensive body of experimental evidence from studies using animal models supports the view that reactive oxygen species and reactive nitrogen species are important in the pathogenesis of acute respiratory distress syndrome. This view is further supported by data from clinical studies that correlate biochemical evidence of reactive oxygen species-mediated or reactive nitrogen species-mediated stress with the development of acute respiratory distress syndrome. Despite these data, pharmacologic strategies directed at minimizing reactive oxygen species-mediated or reactive nitrogen species-mediated damage have yet to be successfully introduced into clinical practice. The most extensively studied compound in this regard is N -acetylcysteine; unfortunately, clinical trials with this compound in patients with acute respiratory distress syndrome have yielded disappointing results.

Animals↗

PubMed1996

Peroxynitrite-mediated formation of free radicals in human plasma: EPR detection of ascorbyl, albumin-thiyl and uric acid-derived free radicals.

Formation of peroxynitrite by the fast reaction between nitric oxide and superoxide anion may represent a critical control point in cells producing both species, leading to either down-regulation of the physiological effects of superoxide anion and nitric oxide by forming an inert product, nitrate, or to potentiation of their toxic effects by oxidation of nearby molecules by peroxynitrite. (The term peroxynitrite is used to refer to the sum of all possible forms of peroxynitrite anion and peroxynitrous acid unless otherwise specified.) In this report we demonstrate that, in spite of all the antioxidant defences present in human plasma, its interaction with peroxynitrite leads to generation of free radical intermediates such as (i) the ascorbyl radical, detected by direct EPR, (ii) the albumin-thiyl radical, detected by spin-trapping experiments with both N-tert-butyl-alpha-phenylnitrone and 5,5-dimethyl-1-pyrroline N-oxide (DMPO), and (iii) a uric acid-derived free radical, detected as the DMPO radical adduct in plasma whose thiol groups were previously blocked with 5,5-dithiobis-(2-nitrobenzoic acid). The identity of the latter adduct was confirmed by parallel experiments demonstrating that it is not detectable in plasma pretreated with uricase, whereas it is formed in incubations of peroxynitrite with uric acid. Peroxynitrite-mediated oxidations were also followed by oxygen consumption and ascorbate and plasma-thiol depletion. Our results support the view that peroxynitrite-mediated one-electron oxidation of biomolecules may be an important event in its cytotoxic mechanism. In addition, the data have methodological implications by providing support for the use of EPR methodologies for monitoring both free radical reactions and ascorbate concentrations in biological fluids.

Ascorbic Acid↗

PubMed1995

Reaction between peroxynitrite and hydrogen peroxide: formation of oxygen and slowing of peroxynitrite decomposition.

Peroxynitrite, the reaction product of nitric oxide and superoxide, is a potent and versatile oxidant that can attack a wide range of targets. In this work, we studied the oxidation of hydrogen peroxide by peroxynitrite, which led to oxygen evolution. Oxygen yields increased at alkaline pH with an apparent pKa of 7.05 +/- 0.04. The maximum yields were 16% and 32% of added peroxynitrite at pH 5.9 and 7.4, respectively, assuming that two molecules of peroxynitrite are needed to produce one of oxygen. Hydroxyl radical scavengers (dimethyl sulfoxide, mannitol, ethanol, formate, and acetate) inhibited oxygen evolution to a similar extent to that predicted from their rate constants with hydroxyl radical. The apparent rate constant of peroxynitrite decomposition was zero-order in hydrogen peroxide at acidic pH. At neutral and alkaline pH, the rate of peroxynitrite disappearance decreased in the presence of millimolar concentrations of hydrogen peroxide by up to 50%. The apparent activation enthalpy and entropy for peroxynitrite decomposition increased by 1.7 kcal mol-1 and 4.7 cal mol-1 K-1, respectively, in the presence of hydrogen peroxide. We propose that an activated intermediate of peroxynitrous acid is responsible for hydrogen peroxide oxidation at acidic pH, while at more alkaline pH the formation of a stabilizing complex between hydrogen peroxide and transperoxynitrite anion is involved.

Hydrogen Peroxide↗