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W A Pryor

Publications and source records attributed to W A Pryor.

At least 55 records · Page 3Linked to original sources
PubMed1997

Cigarette smoke radicals and the role of free radicals in chemical carcinogenicity.

This article consists of two parts: a brief overview of the ways in which free radicals can be involved in chemical carcinogenesis, and a review of cigarette smoke chemistry. Carcinogenesis is generally agreed to involve at least three stages: initiation, promotion, and progression. It is suggested that radicals sometimes are involved in the initiation step, either in the oxidative activation of a procarcinogen (such as benzo[a]pyrene) to its carcinogenic form or in the binding of the carcinogenic species to DNA, or both. The fraction of initiation events that involve radicals, as opposed to two-electron steps, is not known, but radicals probably are involved in a substantial number, although probably not a majority, of cancer initiation reactions. Promotion always involves radicals, at least to some extent. Progression probably does not normally involve radicals. The second part of this article reviews the molecular mechanisms involved in cigarette-induced tumors, particularly by aqueous cigarette tar (ACT) extracts and by a model of these solutions, aged solutions of catechol. ACT solutions as well as aged solutions of catechol contain a quinone-hydroquinone-semiquinone system that can reduce oxygen to produce superoxide and hence hydrogen peroxide and the hydroxyl radical. Both the cigarette tar radical and the catechol-derived radical can penetrate viable cells, bind to DNA, and cause nicks.

DNA Damage↗
PubMed1996

Carbon dioxide catalysis of the reaction of peroxynitrite with ethyl acetoacetate: an example of aliphatic nitration by peroxynitrite.

The reaction of peroxynitrite anion (O=N-OO-) with CO2 results in the formation of an unstable nitrosoperoxycarbonate anion adduct, O=N-OOCO-2 (1). Adduct 1 can serve as a source for several reactive intermediates, including the nitrocarbonate anion (O2N-OCO-2), the carbonate radical ion/nitrogen dioxide radical pair, and the nitronium ion/carbonate ion pair. One or more of these reactive intermediates mediate(s) electrophilic nitrations, for example of tyrosine residues in proteins, which is often observed in peroxynitrite-producing systems. We here report, for the first time, the nitration of an aliphatic substrate, ethyl acetoacetate, by peroxynitrite. The yield of nitration is markedly enhanced in the presence of added carbonate. The major product of this reaction is ethyl 2-nitroacetoacetate. The importance of this reaction is discussed in relation to the possible aliphatic nitrations of amines, sugars, thiols, and thioethers in peroxynitrite-producing biological systems.

Acetoacetates↗
PubMed1996

Trolox inhibits peroxynitrite-mediated oxidative stress and apoptosis in rat thymocytes.

Peroxynitrite is a strong oxidant that reacts with a variety of biomolecules in vivo and in vitro. When rat thymocytes in phosphate buffer are exposed to 25 microM peroxynitrite for 10 min, DNA single strand breaks (SSB) can be detected. These SSB are repaired if the cells are incubated in fresh media at 37 degrees C for 120 min. In addition, DNA protein cross-links and apoptosis are observed 1 and 6 h, respectively, after peroxynitrite exposure. Peroxynitrite mediates the formation of thiobarbituric acid-reactive substances (TBARS) that may be responsible for the DNA-protein crosslinks (DPXL). Both TBARS and DPXL formation are lowered by posttreating the cells immediately after the 10-min exposure to peroxynitrite with Trolox, a water-soluble vitamin E analog. These results suggest that oxidative stress mediated by peroxynitrite can trigger a critical sequence of events ending in programmed cell death and that intracellular oxidation is a component of the apoptosis of thymocytes, since both oxidative processes and apoptosis can be prevented by Trolox. In addition to Trolox, we obtained partial data on three other phenolic antioxidants (3-tert-butyl-4-hydroxyanisole, butylated hydroxytoluene, and 2,6-diisopropylphenol). We find that Trolox and these three phenols similarly protect rat thymocytes from apoptosis mediated by peroxynitrite.

Animals↗
PubMed1996

Synthesis of peroxynitrite in a two-phase system using isoamyl nitrite and hydrogen peroxide.

A new method for the preparation of high concentrations of peroxynitrite (up to 1 M) is described. The synthesis uses a two-phase system and involves a displacement reaction by the hydroperoxide anion (in the aqueous phase) on isoamyl nitrite (in the organic phase). The product peroxynitrite remains in the aqueous phase, whereas isoamyl alcohol forms a new organic phase along with the unreacted isoamyl nitrite. The aqueous phase contains some 0.15 M isoamyl alcohol and the unreacted hydrogen peroxide, but no isoamyl nitrite. Removal of isoamyl alcohol or traces of isoamyl nitrite is accomplished by washing the aqueous phase with dichloromethane, chloroform, or hexane. A near total removal of hydrogen peroxide is then achieved by passing the solutions through a short column of manganese dioxide. The peroxynitrite in these postprocessed solutions has broad absorption spectrum with a maximum around 302 nm, follows a characteristic first-order decomposition at pH 7.2 and 25 degrees C (k = 0.34 +/- 0.1 s-1), and reacts with organic compounds to give either nitrated or one-electron transfer products. When stored frozen at -20 degrees C, these peroxynitrite solutions decompose at a rate of about 1.7 % per day and should be used within 2-4 weeks. For short-term storage of about 1 week or less, these solutions can be stored at refrigerator temperatures (approximately 5 degrees C) where peroxynitrite has a half-life of about 7 days.

Amyl Nitrite↗
PubMed1996

Acceleration of peroxynitrite oxidations by carbon dioxide.

Stopped-flow kinetic studies of the isomerization of peroxynitrite to give nitrate have been performed in carbonate-enriched buffers using pH jump and carbonic anhydrase as probes. The data are consistent with the reaction of CO2 and the peroxynitrite anion rapidly forming an unstable nitrosoperoxy-carbonate anion adduct, O=N-OOCO2- (1). The CO2 catalysis of the isomerization of peroxynitrite is not accompanied by the formation of nitrite, hydrogen peroxide, or other hydroperoxidic material like peroxycarbonate. The reaction proceeds via the transient formation of an oxidant or oxidants that is (are) capable of promoting electrophilic nitration reactions. We propose that O=N-OOCO2- rearranges to give a nitrocarbonate anion, O2N-OCO2- (2) which in turn, may serve as the proximal oxidant in biological systems that produce peroxynitrite. At least four different mechanistic classes of reactions that have been ascribed to peroxynitrite can be envisioned to involve 2: (a) hydrolysis to nitrate, (b) one-electron or (c) two-electron oxidations, and (d) electrophilic nitration. Given the fast reaction of peroxynitrite with carbon dioxide and the ubiquitous presence of the latter, the role of CO2 cannot be neglected in complex peroxynitrite reactions in vitro and in vivo.

Carbon Dioxide↗
PubMed1996

Detection of aldehydes in bronchoalveolar lavage of rats exposed to ozone.

We report the detection of hexanal, heptanal, and nonanal in the bronchoalveolar lavage (BAL) of rats exposed to 0.5 to 10 ppm ozone with or without simultaneous 5% CO2. These three aldehydes primarily result from the Criegee ozonation of specific mono- or polyunsaturated fatty acids that are present in significant amounts in the rat lung; e.g., palmitoleic acid gives heptanal, oleic gives nonanal, and linoleic and arachidonic can give hexanal. Hexanal also is produced in the ozone-initiated autoxidation of any n-6 polyunsaturated fatty acid, and thus is a measure of generalized oxidative stress. (Monounsaturated fatty acids do not undergo appreciable autoxidation.) This detection and quantitation of aldehydes directly demonstrates for the first time that unsaturated fatty acids undergo Criegee ozonation in the lung when ozone is inhaled. Exposure to ozone alone produced smaller apparent yields of the three aldehydes than did exposure to ozone plus 5% CO2. Hexanal, heptanal, and nonanal can be detected in BAL of rats 5 hr after the end of the ozone exposure, but after more than 5 hr only hexanal can be found, probably from ozone-induced autoxidation of n-6 PUFA that continues after ozone exposure. The measured amounts of aldehydes are low, and that, coupled with inherent biovariability, suggests that aldehydes may not be useful as quantitative dosimeters. However, they can be useful biomarkers, since some of these aldehydes (e.g., nonanal) are produced in ozone-specific pathways and aldehydes are the most easily detected among the lipid ozonation products (LOP). Furthermore, our identification of these aldehydes by BAL, coupled with our recognition that ozone itself cannot penetrate far enough into the lung to cause many of the effects associated with the inhalation of ozone, suggests that these aldehydes, as well as other types of LOP (such as hydroxyhydroperoxides and Criegee ozonides), may act as signal transduction molecules, activating lipases and causing the release of inflammatory molecules by a variety of pathways not yet entirely elucidated.

Aldehydes↗
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

Competitive reactions of peroxynitrite with 2'-deoxyguanosine and 7,8-dihydro-8-oxo-2'-deoxyguanosine (8-oxodG): relevance to the formation of 8-oxodG in DNA exposed to peroxynitrite.

We have examined the formation of 7,8-dihydro-8-oxo-2'-deoxyguanosine (8-oxodG) in reactions of peroxynitrite with 2'-deoxyguanosine (dG) and calf-thymus DNA. Peroxynitrite reacts with dG at neutral pH, but this reaction does not result in the buildup of 8-oxodG. We also do not find any evidence for the formation of 8-oxodG in calf-thymus DNA upon exposure to peroxynitrite. When 8-oxodG is mixed with 1000-fold excess dG and then allowed to react with peroxynitrite, about 50% of the 8-oxodG is destroyed. The preferential reaction of 8-oxodG is also evident when dG in calf-thymus DNA is partially oxidized in an Udenfriend system and then allowed to react with peroxynitrite. We suggest that 8-oxodG is not produced in peroxynitrite-mediated oxidations of dG and DNA or that it is produced but then is rapidly consumed in further reactions with peroxynitrite. Oxidized DNA bases frequently can be more oxidation sensitive than their corresponding progenitors and, therefore, may be present at] low steady-state concentrations and not represent stable markers of oxidative stress status. The importance of the 8-oxodG/peroxynitrite reaction is discussed in relation to the formation of more stable, secondary oxidation products that might be more useful markers of DNA damage.

8-Hydroxy-2'-Deoxyguanosine↗
PubMed1996

Direct and indirect oxidations by peroxynitrite, neither involving the hydroxyl radical.

A new mechanism (Mechanism III) that combines features of mechanisms suggested earlier (Goldstein and Czapski, Inorg. Chem. 34:4041-4048; 1995; Pryor, Jin, and Squadrito Proc. Natl. Acad. Sci. USA 91:11173-11177; 1994) is proposed for oxidations by peroxynitrite. In Mechanism III, oxidations by peroxynitrite can take place either directly by ground-state peroxynitrous acid, ONOOH, or indirectly by ONOOH*, where ONOOH* is an activated form of peroxynitrous acid. In the direct oxidation pathway the reaction is first order in peroxynitrite and first order in substrate, and the oxidation yield approaches 100%. In the indirect oxidation pathway the reaction is first order in peroxynitrite and zero order in substrate. In the presence of sufficient concentrations of a substrate that reacts by the indirect oxidation pathway, about 50-60% of the ONOOH directly isomerizes to nitric acid, and about 40-50% of the ONOOH is converted into ONOOH*. Thus, the oxidation yields by the indirect pathway will not exceed 40-50%, and there will always be a residual yield of nitrate even in the presence of very high concentrations of the substrate. Competitive inhibition studies with various free radical scavengers showed that in some cases these scavengers have no effect on oxidation yields. In others, only partial inhibition was observed, far less than that predicted from to the known rate constants for the reactions of these scavengers with the hydroxyl radical. There are some cases where the extent of inhibition correlates well with the known rate constants of the reactions of these scavengers with hydroxyl radical; nevertheless, even in these cases, the involvement of hydroxyl radicals in indirect oxidations by peroxynitrite is ruled our on the basis of kinetics and oxidation yields. Thus, direct oxidations by peroxynitrite are explained in terms of ONOOH, and indirect oxidations in terms of ONOOH*, and substrates can react by one or both of these pathways.

Chemical Phenomena↗
PubMed1995

Peroxynitrite causes apoptosis in rat thymocytes.

Peroxynitrite is demonstrated to cause apoptosis in freshly harvested rat thymocytes suspended in phosphate buffer, as shown by the typical ladder pattern of DNA fragmentation. This evidence suggests a new function for peroxynitrite, already known to be a strong oxidant. Peroxynitrite can nick DNA, oxidize cellular thiols and initiate the apoptotic process responsible for genomic degradation.

Animals↗
PubMed1995

Peroxynitrite causes DNA damage and oxidation of thiols in rat thymocytes [corrected].

We report here the ability of peroxynitrite to cause DNA strand breaks and to oxidize cellular thiol groups in viable rat thymocytes. Peroxynitrite was added to rat thymocytes in a phosphate buffer and DNA damage was measured by the fluorescence analysis of DNA unwinding assay. Peroxynitrite causes DNA strand breaks in a dose-dependent fashion. Four hydroxyl radical scavengers, namely mannitol, dimethyl sulfoxide, sodium benzoate, and Trolox, were tested for their ability to protect DNA from oxidative damage by peroxynitrite. Mannitol failed to protect DNA at concentrations at which it would have conferred nearly complete protection from damage by the hydroxyl radical. Strikingly, dimethyl sulfoxide and benzoate, which are more efficient hydroxyl radical scavengers than mannitol, caused an increase in DNA damage. Trolox was the only scavenger, among the four tested here, that was able to protect DNA from oxidative damage by peroxynitrite. We have previously shown that, among the scavengers tested, Trolox is the most effective scavenger of HOONO*, where HOONO* is a reactive form of HOONO that is a more selective oxidant than is the hydroxyl radical (see W. A. Pryor, X. Jin, and G. L. Squadrito, 1994, Proc. Natl. Acad. Sci. USA 91, 11173-11177). Thus, these results are consistent with our earlier observations that oxidations by peroxynitrite involve a reactive intermediate, HOONO*, rather than hydroxyl radicals. Peroxynitrite also oxidized cellular thiols in a dose-dependent fashion. Greater than 90% of the cells exposed to peroxynitrite were still viable for up to 10 min after DNA damage and thiol oxidation had occurred. In conclusion, DNA damage caused by peroxynitrite can be rationalized as caused by a powerful oxidant, HOONO*, which is formed during the decomposition of peroxynitrite to nitrite.

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↗
PubMed1995

Spin trap studies on the decomposition of peroxynitrite.

The observation of the hydroxyl radical spin adduct of 5,5-dimethyl-1-pyrroline-N-oxide (DMPO) is evaluated as a probe for the production of hydroxyl radicals from the decomposition of peroxynitrite. Although a weak signal corresponding to the DMPO-hydroxyl radical spin adduct (.DMPO-OH) is observed when peroxynitrite is allowed to decompose in the presence of DMPO, it is concluded that this does not constitute proof of the presence of free hydroxyl radicals. The observed rate constant for the decay of peroxynitrite increases from 0.35 to 0.51 s-1 (46% increase) when the concentration of DMPO is increased from 0 to 75 mM. This strongly suggests there is a reaction between DMPO and HOONO, or between DMPO and an activated intermediate of HOONO, to produce the hydroxyl radical spin adduct. The addition of glutathione or cysteine produces a large increase in the intensity of the .DMPO-OH spin adduct signal; experiments employing superoxide dismutase suggest that the increases in the amounts of .DMPO-OH adduct are produced from the decomposition of the spin adduct of the superoxide radical (.DMPO-OOH). The superoxide adduct arises as a result of the autoxidation of thiols, a process known to produce superoxide. The results presented here are incompatible with the formation of free hydroxyl radicals but can be explained in terms of an intermediate of HOONO that is less reactive and more selective than the free hydroxyl radical.

Animals↗
PubMed1995

Peroxynitrite causes DNA nicks in plasmid pBR322.

Peroxynitrite causes single-strand breaks in pBR322 supercoiled DNA as evidenced by agarose gel electrophoresis analysis. The effect of three free radical scavengers, namely mannitol, benzoate and dimethylsulfoxide, were studied. Mannitol failed to protect DNA from damage by peroxynitrite while benzoate and dimethylsulfoxide amplified the damage. These results suggest the damage caused by peroxynitrite alone is not mediated by free radicals since typical free radical scavengers fail to prevent the damage.

Benzoates↗