Ana Denicola

Factors affecting protein thiol reactivity and specificity in peroxide reduction.

Protein thiol reactivity generally involves the nucleophilic attack of the thiolate on an electrophile. A low pK(a) means higher availability of the thiolate at neutral pH but often a lower nucleophilicity. Protein structural factors contribute to increasing the reactivity of the thiol in very specific reactions, but these factors do not provide an indiscriminate augmentation in general reactivity. Notably, reduction of hydroperoxides by the catalytic cysteine of peroxiredoxins can achieve extraordinary reaction rates relative to free cysteine. The discussion of this catalytic efficiency has centered in the stabilization of the thiolate as a way to increase nucleophilicity. Such stabilization originates from electrostatic and polar interactions of the catalytic cysteine with the protein environment. We propose that the set of interactions is better described as a means of stabilizing the anionic transition state of the reaction. The enhanced acidity of the critical cysteine is concurrent but not the cause of catalytic efficiency. Protein stabilization of the transition state is achieved by (a) a relatively static charge distribution around the cysteine that includes a conserved arginine and the N-terminus of an α-helix providing a cationic environment that stabilizes the reacting thiolate, the transition state, and also the anionic leaving group; (b) a dynamic set of polar interactions that stabilize the thiolate in the resting enzyme and contribute to restraining its reactivity in the absence of substrate; but upon peroxide binding these active/binding site groups switch interactions from thiolate to peroxide oxygens, simultaneously increasing the nucleophilicity of the attacking sulfur and facilitating the correct positioning of the substrate. The switching of polar interaction provides further acceleration and, importantly, confers specificity to the thiol reactivity. The extraordinary thiol reactivity and specificity toward H(2)O(2) combined with their ubiquity and abundance place peroxiredoxins, along with glutathione peroxidases, as obligate hydroperoxide cellular sensors.

The peroxidase and peroxynitrite reductase activity of human erythrocyte peroxiredoxin 2.

Peroxiredoxin 2 (Prx2) is a 2-Cys peroxiredoxin extremely abundant in the erythrocyte. The peroxidase activity was studied in a steady-state approach yielding an apparent K(M) of 2.4 microM for human thioredoxin and a very low K(M) for H2O2 (0.7 microM). Rate constants for the reaction of peroxidatic cysteine with the peroxide substrate, H2O2 or peroxynitrite, were determined by competition kinetics, k(2) = 1.0 x 10(8) and 1.4 x 10(7) M(-1) s(-1) at 25 degrees C and pH 7.4, respectively. Excess of both oxidants inactivated the enzyme by overoxidation and also tyrosine nitration and dityrosine were observed with peroxynitrite treatment. Prx2 associates into decamers (5 homodimers) and we estimated a dissociation constant K(d) < 10(-23) M(4) which confirms the enzyme exists as a decamer in vivo. Our kinetic results indicate Prx2 is a key antioxidant enzyme for the erythrocyte and reveal red blood cells as active oxidant scrubbers in the bloodstream.

Reactivity of hydrogen sulfide with peroxynitrite and other oxidants of biological interest

Hydrogen sulfide (H(2)S) is an endogenously generated gas that can also be administered exogenously. It modulates physiological functions and has reported cytoprotective effects. To evaluate a possible antioxidant role, we investigated the reactivity of hydrogen sulfide with several one- and two-electron oxidants. The rate constant of the direct reaction with peroxynitrite was (4.8±1.4)×10(3)M(-1) s(-1) (pH 7.4, 37°C). At low hydrogen sulfide concentrations, oxidation by peroxynitrite led to oxygen consumption, consistent with a one-electron oxidation that initiated a radical chain reaction. Accordingly, pulse radiolysis studies indicated that hydrogen sulfide reacted with nitrogen dioxide at (3.0±0.3)×10(6)M(-1) s(-1) at pH 6 and (1.2±0.1)×10(7)M(-1) s(-1) at pH 7.5 (25°C). The reactions of hydrogen sulfide with hydrogen peroxide, hypochlorite, and taurine chloramine had rate constants of 0.73±0.03, (8±3)×10(7), and 303±27M(-1) s(-1), respectively (pH 7.4, 37°C). The reactivity of hydrogen sulfide was compared to that of low-molecular-weight thiols such as cysteine and glutathione. Considering the low tissue concentrations of endogenous hydrogen sulfide, direct reactions with oxidants probably cannot completely account for its protective effects.

Desferrioxamine inhibition of the hydroxyl radical-like reactivity of peroxynitrite: Role of the hydroxamic groups

Nitric oxide reacts with superoxide to form peroxynitrite, a strong oxidizing species. Peroxynitrite can either directly oxidize molecules such as thiols or protonate to peroxynitrous acid, which can yield an oxidant with a reactivity similar to that of hydroxyl radical in a transition metal-independent mechanism. This oxidative chemistry of peroxynitrite, however, is inhibited by the metal chelator desferrioxamine. Indeed, desferrioxamine, was a potent inhibitor of dimethylsulfoxide, hydrogen peroxide, 5,5-dimethyl-1-pyrroline-N-oxide, and luminol oxidation, whereas the metal chelator diethylenetriaminepentaacetic acid, and ferrioxamine, the iron complex of desferioxamine, were not. Two other hydroxamates, acetohydroxamate and salicylhydroxamate, were also effective inhibitors. Stopped-flow experiments showed that there is no direct reaction between peroxynitrite anion or cis-peroxynitrous acid with desferrioxamine. Electron paramagnetic resonance (EPR) studies showed the formation of the desferrioxamine nitroxide radical in incubations containing desferrioxamine, but not ferrioxamine, indicating that the hydroxamic group acts as a one-electron donor to peroxynitrite-derived oxidants. Taken together, our results led us to propose that desferrioxamine can inhibit the oxidative chemistry of peroxynitrite by reaction of the hydroxamic acid moieties with trans-peroxynitrous acid.

Chapter 4 – The Biological Chemistry of Peroxynitrite

Publisher Summary This chapter provides a comprehensive overview of the physical and biological chemistry of peroxynitrite. A foundation is provided to rationalize the biological fate and actions of peroxynitrite and the strategies for preventing peroxynitrite-dependent biological damage and pathology. Peroxynitrite anion is formed in vivo as a result of the diffusion controlled reaction between nitric oxide (NO) and superoxide anion radicals. The anion and its conjugated acid, peroxynitrous acid, are strong oxidant species that cause molecular damage in a variety of pathophysiological conditions. Peroxynitrite reacts fast with a number of biological targets, including thiols, metalloproteins, and carbon dioxide, or more slowly decomposes to hydroxyl and nitrogen dioxide radicals by proton-catalyzed homolysis. Carbon dioxide accounts for a significant fraction of peroxynitrite consumption and leads to the secondary formation of carbonate and nitrogen dioxide radicals. At the molecular level, the predominant outcome of peroxynitrite reactions in vivo is one or two electron oxidations and nitrations. Peroxynitrite can diffuse through tissue compartments, being able to cross biomembranes by both passive diffusion and anion channels. Thus, although the biological half-life of peroxynitrite is short, it is sufficient for peroxynitrite to diffuse a couple of cell diameters and cause biological effects distant from its site of production.

Reaction of Human Hemoglobin with Peroxynitrite ISOMERIZATION TO NITRATE AND SECONDARY FORMATION OF PROTEIN RADICALS

Peroxynitrite, a strong oxidant formed intravascularly in vivo, can diffuse onto erythrocytes and be largely consumed via a fast reaction (2 × 104 m–1 s–1) with oxyhemoglobin. The reaction mechanism of peroxynitrite with oxyhemoglobin that results in the formation of methemoglobin remains to be elucidated. In this work, we studied the reaction under biologically relevant conditions using millimolar oxyhemoglobin concentrations and a stoichiometric excess of oxyhemoglobin over peroxynitrite. The results support a reaction mechanism that involves the net one-electron oxidation of the ferrous heme, isomerization of peroxynitrite to nitrate, and production of superoxide radical and hydrogen peroxide. Homolytic cleavage of peroxynitrite within the heme iron allows the formation of ferrylhemoglobin in ∼10% yields, which can decay to methemoglobin at the expense of reducing equivalents of the globin moiety. Indeed, spin-trapping studies using 2-methyl-2-nitroso propane and 5,5 dimethyl-1-pyrroline-N-oxide (DMPO) demonstrated the formation of tyrosyl- and cysteinyl-derived radicals. DMPO also inhibited covalently linked dimerization products and led to the formation of DMPO-hemoglobin adducts. Hemoglobin nitration was not observed unless an excess of peroxynitrite over oxyhemoglobin was used, in agreement with a marginal formation of nitrogen dioxide. The results obtained support a role of oxyhemoglobin as a relevant intravascular sink of peroxynitrite.

Peroxynitrite reactions with carbon dioxide-bicarbonate.

Publisher Summary This chapter discusses the peroxynitrite reactions with carbon dioxide-bicarbonate. The chemical reactivities and biological actions of peroxynitrite anion (ONOO - )—the product of the radical-radical reaction between superoxide (O 2 .- ) and nitric oxide ( . NO)—can be profoundly influenced by carbon dioxide (CO2)-bicarbonate (HCO3 - ). This modulation of ONOO - reactivity—a key component of oxidative stress and tissue inflammatory injury—is highly influenced by the formation of a reactive nitrosoperoxocarbonate intermediate (ONOOCO 2 - ) that alters both the chemical stability and reaction pathways of ONOO - . The importance of the CO2–HCO 3 - pair in modulating . NO and oxygen radical-dependent cell signaling and toxicity has been underestimated. Current evidence supports the idea that CO2–HCO 3 - can significantly participate in the biological reactivity and fate of not only ONOO - , but also other • NO-derived species and oxygen radicals. Thus, the CO2–HCO 3 - pair is a critical biological effector for ONOO - , via the formation ONOOCO2 - . This reactive species is notable in that it potently redirects the biological reactivity and diffusivity of ONOO - .

Synthesis and antitrypanosomal evaluation of E-isomers of 5-nitro-2-furaldehyde and 5-nitrothiophene-2-carboxaldehyde semicarbazone derivatives. Structure-activity relationships.

Several novel semicarbazone derivatives were prepared from 5-nitro-2-furaldehyde or 5-nitrothiophene-2-carboxaldehyde and semicarbazides bearing a spermidine-mimetic moiety. All derivatives presented the E-configuration, as determined by NMR-NOE experiments. These compounds were tested in vitro as potential antitrypanosomal agents, and some of them, together with the parent compounds, 5-nitro-2-furaldehyde and 5-nitrothiophene-2-carboxaldehyde semicarbazone derivatives, were also evaluated in vivo using infected mice. Structure-activity relationship studies were carried out using voltammetric response and lipophilic-hydrophilic balance as parameters. Two of the compounds (1 and 3) displayed the highest in vivo activity. A correlation was found between lipophilic-hydrophilic properties and trypanocidal activity, high R(M) values being associated with low in vivo effects.

Acceleration of nitric oxide autoxidation and nitrosation by membranes

The reaction between nitric oxide (•NO) and oxygen yields reactive species capable of oxidizing and nitrosating proteins, as well as deaminating DNA bases. Although this reaction is considered too slow to be biologically relevant, it has been shown that membranes, lipoproteins, mitochondria and possibly proteins can accelerate this reaction. This effect stems from the higher solubility of both •NO and O2in the hydrophobic phase of these biological particles, leading to a concentration of both reagents and so a higher rate of reaction. It has been determined that this reaction occurs from 30 to 300 times more rapidly within the membrane, while even higher values have been suggested for proteins. The autoxidation of •NO in membranes is not the main route for cellular •NO consumption but an important consequence of this phenomenon is to focus the generation of significant amounts of oxidizing and nitrosating molecules (nitrogen dioxide and dinitrogen trioxide) in the small volume comprised by cellular membranes. Even so, these reactive species are diffusible and their ultimate fate will depend on the reactivity towards available substrates rather than on physical barriers. The acceleration of •NO autoxidation by biological hydrophobic phases may thus be a general phenomenon that increases in importance in cases of •NO overproduction. IUBMB Life, 59: 243‐248, 2007

Platyhelminth Mitochondrial and Cytosolic Redox Homeostasis Is Controlled by a Single Thioredoxin Glutathione Reductase and Dependent on Selenium and Glutathione

Platyhelminth parasites are a major health problem in developing countries. In contrast to their mammalian hosts, platyhelminth thiol-disulfide redox homeostasis relies on linked thioredoxin-glutathione systems, which are fully dependent on thioredoxin-glutathione reductase (TGR), a promising drug target. TGR is a homodimeric enzyme comprising a glutaredoxin domain and thioredoxin reductase (TR) domains with a C-terminal redox center containing selenocysteine (Sec). In this study, we demonstrate the existence of functional linked thioredoxin-glutathione systems in the cytosolic and mitochondrial compartments of Echinococcus granulosus, the platyhelminth responsible for hydatid disease. The glutathione reductase (GR) activity of TGR exhibited hysteretic behavior regulated by the [GSSG]/[GSH] ratio. This behavior was associated with glutathionylation by GSSG and abolished by deglutathionylation. The Km and kcat values for mitochondrial and cytosolic thioredoxins (9.5 μm and 131 s–1, 34 μm and 197 s–1, respectively) were higher than those reported for mammalian TRs. Analysis of TGR mutants revealed that the glutaredoxin domain is required for the GR activity but did not affect the TR activity. In contrast, both GR and TR activities were dependent on the Sec-containing redox center. The activity loss caused by the Sec-to-Cys mutation could be partially compensated by a Cys-to-Sec mutation of the neighboring residue, indicating that Sec can support catalysis at this alternative position. Consistent with the essential role of TGR in redox control, 2.5 μm auranofin, a known TGR inhibitor, killed larval worms in vitro. These studies establish the selenium- and glutathione-dependent regulation of cytosolic and mitochondrial redox homeostasis through a single TGR enzyme in platyhelminths.