Kinetic Studies and Mechanism of Hydrogen Peroxide Catalytic Decomposition by Cu(II) Complexes with Polyelectrolytes Derived from L-Alanine and Glycylglycine

Skounas, Spyridon; Methenitis, Constantinos; Pneumatikakis, George; Morcellet, Michel

doi:https://doi.org/10.1155/2010/643120

Bioinorganic Chemistry and Applications

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Volume 2010 | Article ID 643120 | https://doi.org/10.1155/2010/643120

Kinetic Studies and Mechanism of Hydrogen Peroxide Catalytic Decomposition by Cu(II) Complexes with Polyelectrolytes Derived from L-Alanine and Glycylglycine

Spyridon Skounas,¹Constantinos Methenitis,¹George Pneumatikakis,¹and Michel Morcellet²

Academic Editor: Spyros Perlepes

Received23 Mar 2010

Accepted30 May 2010

Published18 Jul 2010

Abstract

The catalytic decomposition of hydrogen peroxide by Cu(II) complexes with polymers bearing L-alanine (PAla) and glycylglycine (PGlygly) in their side chain was studied in alkaline aqueous media. The reactions were of pseudo-first order with respect to [] and [L-Cu(II)] (L stands for PAla or PGlygly) and the reaction rate was increased with pH increase. The energies of activation for the reactions were determined at pH 8.8, in a temperature range of 293–308 K. A suitable mechanism is proposed to account for the kinetic data, which involves the Cu(II)/Cu(I) redox pair, as has been demonstrated by ESR spectroscopy. The trend in catalytic efficiency is in the order PGlyglyPAla, due to differences in modes of complexation and in the conformation of the macromolecular ligands.

1. Introduction

The formation of complexes between macromolecular ligands and transition metal ions has been widely investigated [1–6]. Synthetic macromolecular systems, offer the possibility of modelling the complexation and reactivity of metal ions with biological ligands [7]. The systems especially that are made up of synthetic polyelectrolytes could be considered as simple but representative models for studying biological ligand-metal interactions [7–9]. The thermodynamic and structural characterization of these metal ions complexes would help in understanding the mechanism and the binding mode of the metals both to proteins and to substrate molecules.

The decomposition of hydrogen peroxide has been used as a model reaction for the investigation of the catalytic activity of various metal complexes and has also been studied as a catalase model, although the catalytic mechanism has not been thoroughly elucidated [1, 2, 10–21]. It has been known for about a century that the decomposition of H₂O₂ to H₂O and O₂ is drastically accelerated by many metal ions [14–19]. Complexes of copper (II) especially with various ligands acting as catalysts have been investigated in depth and disagreements over mechanistic details, involving intermediate radicals or complexes, have lasted for decades. The formation of copper peroxide complexes both in acidic and alkaline solutions has been confirmed and a mechanism not involving any radicals has been suggested [17, 18]. On the other hand, the existence of O radicals in the decomposition of H₂O₂, catalyzed by Cu(II), in alkaline media in the presence of biological reductants has been, convincingly, demonstrated [20–22]. The difference in reactivity of Cu(II) complexes towards H₂O₂ is due to the change in the redox potential of Cu(II) ions as a result of ligation with different ligands [23]. It was supposed that a superoxide-copper (I) complex is formed [HO₂-Cu(I)(Ligand)] from the complex [HO₂-Cu(II)(Ligand)] in which an instantaneous electron transfer occurs [21]. Other investigators suggested the formation of a Cu(III)-peroxo complex, as a consequence of the interaction of Cu(II) ions with H₂O₂, this species producing highly reactive OH^. radicals [24–30]. Recently, a mechanism involving both Cu(I)/Cu(II) and Cu(II)/Cu(III) redox pairs has been reported [31]. It has also been proposed that in slight alkaline and neutral pH region, the decomposition of H₂O₂ by copper complexes may proceed by a combination of a molecular mechanism, in which a presumed intermediate species [CuL], reacts with [], a free-radical mechanism involving reversible oxidation reduction of a cupric-cuprous couple, and the formation of free radicals, for example, and H, leading to a chain reaction [32]. Other researchers have mentioned the formation of a peroxo-copper complex (brown compound) in the homogeneous and heterogeneous H₂O₂ decomposition with different Cu(II) complex ions that are by themselves active catalysts for H₂O₂ decomposition [33].

A series of polymers that are referred to as “nonpeptide amino acid-based polymers” or as “amino acid-derived polymers with modified backbones” [34] was previously synthesized and shown to exhibit polyelectrolyte and metal complexation behavior [35–40]. In previous works it has been shown that the complexes of Cu(II) with polyelectrolytes derived from glutamic and aspartic acids exhibit substantial catalytic activity in the decomposition of H₂O₂ in alkaline media [41, 42]. Key feature in these systems is the coordination of the ligands to Cu(II) through two amidic N^- from adjacent amino acids [41, 42]. In the present work, we investigate the catalytic activity of Cu(II) complexes with polyelectrolytes derived from alanine, PAla, and diglycine, PGlygly, (Scheme 1) towards the H₂O₂ decomposition in alkaline solutions. A suitable mechanism is proposed to account for the kinetic and ESR spectroscopic studies.

2. Experimental Section

2.1. Materials and Methods

All chemicals were of analytical reagent grade and were employed without further purification. The poly(N-methacryloyl-L-alanine) (PAla) and poly(N-methacryloyl-diglycine) (PGlygly) were prepared by polymerization of the corresponding monomers, carried out in dioxane (p.a Merck) at 60C with AIBN (azobisisobutyronitrile) as initiator. The monomers N-methacryloyl-L-alanine and N-methacryloyl-diglycine were prepared from methacryloyl chloride (tech. 90%, with 150 ppm phenothiazine, Aldrich Chem.Co) and L-alanine (optical purity 99, 5% NT, Fluca) and glycinoglycine (99, 5% NT, Fluka), respectively, according to the method of Kulkarni and Morawetz [43]. Full experimental details of the synthesis of these compounds have been published earlier [35, 37]. Cu· (Fluca) was used as the metal ion source. Water was obtained from a Milli-Q purification system (Millipore), which was feeded with doubly distilled water. The concentration of Cu(II) solutions was determined by complexometric titrations with EDTA. Working solutions of hydrogen peroxide were prepared weekly by volumetric dilution of 30% (v/v) H₂O₂ (AR. grade, Merck) and were standardized daily by titration with potassium permanganate. It was found that the natural decomposition rate of aqueous H₂O₂ solution was less than 1% in 24 h.

The decomposition of H₂O₂ catalyzed by Cu(II) complexes can be kinetically monitored by removing aliquots of the reaction mixture at predetermined intervals and titrating the undecomposed H₂O₂ with standard KMnO₄ solutions (0.04-0.05 N), standardized with (COONa)₂ (primary standard). The decomposition of hydrogen peroxide was carried out in a thermostated cell at four different temperatures between 293 and 308 K (0.1 K). The pH of the solutions was adjusted between 7 and 11 with buffer solution of H₃BO₃-NaClO₄ and the appropriate quantities of NaOH 0.1 M and between 6-7 with buffer solution of phosphate. The pH measurements were performed using a digital Xenon pHmeter and a RUSSEL CMAWL/3.7/180 combined electrode. Standardization was done at 25C with Russel buffers (potassium hydrogen phthalate at pH 4, potassium dihydrogen orthophosphate-disodium hydrogen orthophosphate at pH 7 and sodium hydrogen carbonate/sodium carbonate at pH 10). The chosen concentration range of H₂O₂ was to M. The analytical concentration of Cu(II) ranged from to M and the [ligand]/[metal] ratio (R) was chosen to be 4 and 8. The decomposition of H₂O₂ was halted with the addition of H₂SO₄. Acidification effectively halted the alkaline decomposition at the desired time and titrations with potassium permanganate in acidic media could be carried out even 1 h later without significant discrepancy.

2.2. EPR Measurements

The measurements were made in frozen (77 K) aliquots of the solutions of the reactions between the systems L-Cu(II) (L stands for PAla and PGlygly) (, [) and H₂O₂ at pH between 8.0 and 9.0 at 298 K, taken out at different times and carried out on a Bruker ESP-300 spectrometer (X-band) with 100 kHz field modulation, 9.3 GHz microwave frequency and equipped with a standard low-temperature apparatus. The hyperfine coupling constants and g-factors were calibrated by comparison with DPPH (2,2-diphenyl-1-picrylhydrazyl) ()

3. Results and Discussion

3.1. Solution Structure of the Complexes

The presence of both the carboxyl and the amidic groups in the ligands (Scheme 1) gives the possibility of different complex type formation. Although the exact geometry of the formed complexes cannot be reached because of the complexity of the macromolecular structures, the atoms of the ligands which interact with the Cu(II) ions and the stoichiometry of the formed complexes can be determined. Based on the potentiometric and spectroscopic results, molecular structures for the dominant copper(II)-PAla species existing in aqueous solutions were previously proposed in [35, 36]. At the complex formation involves two carboxylates and water molecules (type (I) complex); at another complex, a chelate with the participation of a deprotonated N atom of the amide function, starts to form (type (II) complex), that gradually becomes the main species. At complexes which involve two deprotonated amide N are also detected (type (III) complexes). For PGlygly-Cu(II) systems, at different complexes involving carboxylates, water molecules and/or hydroxyls are detected (type (I) complexes) [39]. At complexes with the participation of deprotonated N atoms of the amide functions are, as previously, also formed (type (III) complexes, unpublished results). It must be mentioned that at hydrolysis, in some extent, of the above copper complexes occurs and the formed copper hydroxides do not precipitate but could be firmly bounded to the soluble polyelectrolytes [44, 45].

3.2. Catalytic Properties

A number of experiments were performed to study the effect of pH, H₂O₂, and Cu(II) concentrations and temperature on the initial rate of the catalytic decomposition of H₂O₂ from the PAla-Cu(II) and PGlygly-Cu(II) systems. The reaction velocities at () were determined graphically from the tangential slopes of the curves, at zero time, which represent the concentration of hydrogen peroxide in respect to the elapsed reaction time. Thus the initial rate, , was expressed as .

Characteristic changes in the colour of the reaction solutions take place during the course of the reactions. The clear sky blue solutions of Cu(II) complexes turn into blurred blue-green after the addition of H₂O₂. Gradually, they become yellow-green and when concentrations of hydrogen peroxide higher than M are used, a yellow-brown solid precipitates from the solutions with . No attempt was made to investigate the nature of this precipitate. Small bubbles of oxygen are formed during the reaction. Within a week the reaction solutions did not get the initial colour. Blank experiments were performed and no catalytic activity was observed when solutions containing only the polymers in the absence of Cu(II) were used, in the whole pH range. At the pH range under investigation copper hydroxide is precipitated in the absence of the polyelectrolytes.

The reactions are found to be of pseudo-first order with respect to H₂O₂ (Figure 1) for all the studied pH and [H₂O₂]/catalyst ratios. The order of the reactions was not found to decrease with the increase of the initial H₂O₂ concentration. The reactions were, also, found to be of pseudo-first order with respect to the total concentration of Cu(II) (Figure 2) for all the studied pH and [H₂O₂]/catalyst ratios.

(a)

(b)

(a)

(b)

The dependence of the reaction rates on pH is given in Figure 3. The rates of H₂O₂ decomposition are pH-dependent. The observed rates are very low below pH:8 and strongly increase in the alkaline region. The order was found to be between 0.4 and 0.8 with respect to [], depending on the [H₂O₂]. A possible explanation is discussed forward in the text.

3.2.1. Effect of Temperature Activation Parameters

Using Arrhenius plots (Figure 4) and the Arrhenius equation the activation energies, , were calculated at pH 8.8 (Table 1).

(a)

(b)

The difference in the activation energy values between the PGlygly-Cu(II) system and the PAla-Cu(II) system should reflect not only the different microenvironment of the Cu(II) ions, but also the differences of the macromolecular ligands. In these two systems, key feature is the coordination of the ligand derived from alanine to each Cu(II) through deprotonated amide nitrogens and carboxylates [35, 36] and of the ligand derived from diglycine to each Cu(II) through carboxylates [39, 46]. (Indeed, in the first coordination sphere of Cu(II) ions amidic nitrogen(s) and oxygens are involved in the PAla system, while only oxygens are involved in the case of the Pglygly.) Furthermore, the distance of the copper centers from the polymeric backbone is smaller in the PAla than in the PGlygly system. As this distance increases, not only the approach of small molecules to the metal centers is more favorable, but also any structural changes around the metals are made more easily. The different mode of complexation of the two systems is, also, reflected on the differences in the variations of the enthalpies of activation, Δ, for the two systems, as Δ is a measure of the height of the energy barrier that should be overcome to reach the transition state and is related to the strengths of the intra- and intermolecular bonds which participate in the reaction leading to the transition state.

3.2.2. ESR Measurements

To verify the above assumptions, the catalytic reactions that take place in solutions with pH in the range 8-9 were, also, followed with ESR spectroscopy, in order to gain some insight of the mechanism and to deduce evidence for the participating intermediates. The change of the intensity of the axial ESR signal of paramagnetic Cu(II) during the course of the reactions was monitored and the existence of any new signal, due to any newly formed paramagnetic Cu(II) species, was investigated.

The two systems exhibited a completely different behavior. For the PAla-Cu(II) system we can detect three stages of the reaction (Figure 5). In the first, very short stage, a slight increase in the intensity of the signal is observed. In the second stage a rapid decrease in the intensity occurs until it reaches about 20% of the starting intensity without entire disappearance. In the final stage the signal starts building up again in a slow rate without ever reaching the original intensity. From our results it was not easy to assign any new EPR absorbing Cu(II) species, formed during the reaction. Furthermore, as any additional spectral lines in the area of were not detected, any Cu(II)-Cu(II) strong antiferromagnetic coupling was precluded to be the reason for the decrease in the intensity of the signal [47, 48]. Finally, as the formation of a diamagnetic Cu(III) complex (d⁸ low-spin complex) can also be ruled out, since it requires ligands able to give strong fields as tetrapeptides or ligands able to give a four-nitrogen in plane coordination [49], and no evidence of ESR lines due to paramagnetic Cu(III) complexes could be found, the reduction of EPR-silent Cu(I) complex is strongly suggested. The small initial increase in the intensity of the signal could be explained as the result of the adoption from the negatively charged macromolecular catalyst of a more extended structure that enables the approach of the, also, negatively charged peroxo anion that comes from the dissociation of H₂O₂ that occurs at this pH. In this structure, the metallic centers are further apart from each other and any small spin exchange between them is diminished.

(a)

(b)

The system PGlygly-Cu(II) shows a signal with an initial intensity of 20% of the initial intensity of the signal of the system PAla-Cu(II), for the same total Cu(II) concentration. The signal does not decrease in intensity as the reaction proceeds, but instead constantly increases. It finally reaches a plateau when the intensity equals the initial intensity of the signal of the PAla-Cu(II) system. This striking difference could not be explained only by the different nature of the catalytic sites (Cu(II) complexes), without taking into account that these sites are a part of a three-dimensional macromolecule. As the experimental conditions (pH, ionic strength, Cu(II) and polymer concentrations, temperature) of the formation of the complexes as well as the anchoring groups (amides and carboxylates) are exactly the same, the difference in the modes of complexation must be related to conformational effects. Indeed the complex formation between a polyelectrolyte and a metal ion causes many effects, mainly arising from changes in the net charge of the polymer and changes in the electrostatic interactions [2, 50, 51]. In previous works we have reported the effect of the complexation of Cu(II) ions on the hydrodynamic behavior of the PAla and PGlygly [39, 52]. In these works viscosimetric studies clearly demonstrated the formation of intramolecular Cu(II)-carboxylates complexes, which lead to the folding of the macromolecules. At higher pH values, when amide nitrogens replace carboxylates on the coordination sphere of Cu(II), only neighboring side chains are involved in complex formation, resulting in the unfolding of the macromolecules.

As a result of the differences in the complexation modes and the macromolecular ligand conformations of the two systems at the pH range under investigation, the mutual approach of the copper centers is feasible for PGlygly-Cu(II) complex but not for PAla-Cu(II). Consequently extensive Cu(II)-Cu(II) spin interactions may arise only in the PGlygly-Cu(II) system. These spin interactions explain the much smaller intensity of the initial signal in the PGlygly-Cu(II) system, as has been observed in other systems where copper-copper dipole interactions are promoted by the ligands [53, 54]. No signals were observed near and is greater than 4, indicating negligible exchange interactions [48, 55]. The approach of H₂O₂ and complexation to Cu(II) cause the unfolding of the macromolecule, as has been observed elsewhere [56], breaking the existing intra- and inter-crossings between the chains of the polymer. This results in the reduction of the spin interactions between copper centers and consequently the increase of the intensity of the paramagnetic signal. Obviously, the magnitude of the increase is bigger than the magnitude of the simultaneous decrease due to the reduction of Cu(II) to Cu(I). Furthermore, it seems that the reoxidation step is much quicker for the PGlygly polymer, as after 3 hrs from the beginning of the reaction all the copper is in the Cu(II) state, while for the PAla polymer only 20% of the copper is in the Cu(II) state at the same time.

We did not detect any new signals due to different from the initial Cu(II) species, for the period of a week. Thus, our experimental data cannot support the degradation process that has been reported for other systems [57].

3.2.3. Kinetics and Mechanism

Kinetic studies in the conditions mentioned above showed that the initial rate of the decomposition of H₂O₂ is proportional to [H₂O₂], [CuL₂]. For a given pH stands ( depends on the pH of the solution).

The following reactions are consistent with the above-mentioned observed rate law and the thermodynamic and spectroscopic measurements

It is assumed that step (4) is the rate determining step of the reaction, as the reduction of Cu(II) requires geometrical changes around the metal center. According to the Franck-Condon principle, before the electron-transfer the coordinate bonds between the cupric ion and the ligands must be stretched and the cupric complex must be rearranged to a structure which can accept one electron. This mechanism is in agreement with the suggestion for other macromolecular systems [21] and can explain the change in rate in going to more alkaline conditions, as the dependence of the redox potential of the couple ()/H₂O₂ () on pH is very well known. The redox potential drops from 1.4 to 0.18 V over the pH range 0–14 [21]. It is obvious that the oxidation of H₂O₂ to or by Cu(II) is more favorable in more alkaline conditions. This kind of mechanism does not involve any diffusible radical species in accordance to previous proposed mechanism [10, 18], but several very rapid intermediate steps between (4) and (5) may exist which include the participation of radicals. This should explain the nonlinear dependence of the initial rate of the reaction from [] as well as the formation of the brown peroxo-copper precipitate at high H₂O₂ concentrations, but from our data no conclusion can be drawn about the possible structures of these intermediate species

4. Conclusions

The complexes of copper (II) with the functional polymers PAla and PGlygly act as catalysts in the decomposition of H₂O₂ at alkaline conditions. The trend in catalytic efficiency is in the order , due to differences in the modes of complexation and the adopted conformations of the macromolecules upon complexation. The catalytic decomposition depends upon the concentration of H₂O₂, the concentration of the catalyst, temperature, and pH of the reacting solutions. The rate of the reaction is of pseudo-first order with respect to the concentration of H₂O₂ and the concentration of the catalyst at the pH range 7–10. The proposed mechanism involves reduction of Cu(II) to Cu(I), during the slow rate determining step.

Acknowledgments

The authors thank the General Secretariat of Research and Technology (GSRT), Project 91EΔ831 and the University of Athens for financial support.

References

M. Kaneko and E. Tsuchida, “Formation, characterization, and catalytic activities of polymer-metal complexes,” Journal of Polymer Science, Macromolecular Reviews, vol. 16, pp. 397–522, 1981.
View at: Google Scholar
E. Tsuchida and H. Nishide, “Polymer-metal complexes and their catalytic activity,” Advances in Polymer Science, no. 24, pp. 1–87, 1977.
View at: Google Scholar
Y. Kurimura, “Macromolecule metal complexes–reactios and molecular recognition,” Advances in Polymer Science, vol. 90, pp. 105–138, 1989.
View at: Google Scholar
J. François, C. Heitz, and M. M. Mestdagh, “Spectroscopic study (u.v.-visible and electron paramagnetic resonance) of the interactions between synthetic polycarboxylates and copper ions,” Polymer, vol. 38, no. 21, pp. 5321–5332, 1997.
View at: Google Scholar
M. Palumbo, A. Cosani, M. Terbojevich, and E. Peggion, “Metal complexes of poly(α-amino acids). Interaction of Cu (II) ions with poly(L-lysine) in the 0-Structure,” Biopolymers, vol. 17, pp. 243–246, 1978.
View at: Google Scholar
W. Bal, M. Dyba, F. Kasprzykowski et al., “How non-bonding amino acid side-chains may enormously increase the stability of a Cu(II)—peptide complex,” Inorganica Chimica Acta, vol. 283, no. 1, pp. 1–11, 1998.
View at: Google Scholar
H. J. van den Berg and G. Challa, “Polymeric models of reactive biological systems,” in Syntheses and Separations Using Functional Polymers, D. C. Sherrington and P. Hodge, Eds., pp. 227–264, Wiley, New York, NY, USA, 1988.
View at: Google Scholar
J. J. Grodzinski, “Biomedical application of functional polymers,” Reactive and Functional Polymers, vol. 39, no. 2, pp. 99–138, 1999.
View at: Google Scholar
E. A. Bekturov, S. E. Kudaibergenov, and V. B. Sigitov, “Complexation of amphoteric copolymer of 2-methyl-5-vinylpyridine-acrylic acid with copper(II) ions and catalase-like activity of polyampholyte-metal complexes,” Polymer, vol. 27, no. 8, pp. 1269–1272, 1986.
View at: Google Scholar
H. Sigel, K. Wyss, B. E. Fischer, and B. Prijs, “Metal ions and hydrogen peroxide. Catalase-like activity of ${Cu}^{2 +}$ in aqueous solution and its promotion by the coordination of 2, $2^{'}$ -bipyridyl,” Inorganic Chemistry, vol. 18, no. 5, pp. 1354–1358, 1979.
View at: Google Scholar
G. S. Vinodkumar and B. Mathew, “Polymer-metal complexes of glycine functions supported on N,N′-methylene-bis-acrylamide (NNMBA)-crosslinked polyacrylamides: synthesis, characterisation and catalytic activity,” European Polymer Journal, vol. 34, no. 8, pp. 1185–1190, 1998.
View at: Google Scholar
L. Jose and V. N. R. Pillai, “Catalase-like activity of divinylbenzene (DVB)-crosslinked polyacrylamide supported amino metal complexes,” European Polymer Journal, vol. 32, no. 12, pp. 1431–1435, 1996.
View at: Publisher Site | Google Scholar
L. Jose and V. N. R. Pillai, “Catalase-like activity of triethyleneglycol dimethacrylate-crosslinked polyacrylamide supported metal complexes,” Polymer, vol. 39, no. 1, pp. 229–233, 1998.
View at: Google Scholar
F. Haber and J. Weiss, “The catalytic decomposition of hydrogen peroxide by iron salts,” Proceedings of the Royal Society A, vol. 147, pp. 332–351, 1934.
View at: Google Scholar
W. G. Barb, J. H. Baxendale, P. George, and K. R. Hargrave, “Reactions of ferrous and ferric ions with hydrogen peroxide. Part II. The ferric ion reaction,” Transactions of the Faraday Society, vol. 47, pp. 591–616, 1951.
View at: Google Scholar
M. L. Kremer and G. Stein, “The catalytic decomposition of hydrogen peroxide by ferric perchlorate,” Transactions of the Faraday Society, vol. 55, pp. 959–973, 1959.
View at: Google Scholar
A. Glasner, “203. The constitution of copper peroxide and the catalytic decomposition of hydrogen peroxide,” Journal of the Chemical Society, pp. 2464–2467, 1959.
View at: Google Scholar
H. Sigel, C. Flierl, and R. Griesser, “On the kinetics and mechanism of the decomposition of hydrogen peroxide, catalyzed by the ${Cu}^{2 +}$ -2, $2^{'}$ -bipyridyl complex,” Journal of the American Chemical Society, vol. 91, no. 5, pp. 1061–1064, 1969.
View at: Google Scholar
M. L. Kremer, “Complex versus free radical mechanism for the catalytic decomposition of $H_{2} O_{2}$ by ferric ions,” International Journal of Chemical Kinetics, vol. 17, pp. 1299–1314, 1985.
View at: Google Scholar
G. Vierke, “Electron spin resonance spectra of the reaction products of copper(II) hydroxide suspensions in methanol with hydrogen peroxide and of polycrystalline copper(II) hydroxide and copper(II) peroxide,” Journal of the Chemical Society, Faraday Transactions 1, vol. 69, pp. 1523–1531, 1973.
View at: Publisher Site | Google Scholar
Y. Luo, K. Kustin, and I. R. Epstein, “Systematic design of chemical oscillators. 44. Kinetics and mechanism of hydrogen peroxide decomposition catalyzed by copper(2+) in alkaline solution,” Inorganic Chemistry, vol. 27, pp. 2489–2496, 1988.
View at: Google Scholar
T. Ozawa and A. Hanaki, “The first ESR spin-trapping evidence for the formation of hydroxyl radical from the reaction of copper(II) complex with hydrogen peroxide in aqueous solution,” Journal of the Chemical Society, Chemical Communications, no. 5, pp. 330–332, 1991.
View at: Publisher Site | Google Scholar
T. Ozawa, A. Hanaki, K. Onodera, M. Kasai, and Y. Matsushima, “Can copper(II) complexes activate hydrogen peroxide? : ESR-spin trapping studies,” Journal of Pharmacobio-Dynamics, vol. 13, supplement 2, 1991.
View at: Google Scholar
K. Hayakawa and S. Nakamura, “The decomposition of hydrogen peroxide with metal complexes. I. The catalytic decomposition of hydrogen peroxide by the ammine-copper(II) complex ions in an aqueous solution,” Bulletin of the Chemical Society of Japan, vol. 47, pp. 1162–1167, 1974.
View at: Google Scholar
P. Tachon, “Ferric and cupric ions requirement for DNA single-strand breakage by $H_{2} O_{2}$ ,” Free Radical Research Communications, vol. 7, no. 1, pp. 1–10, 1989.
View at: Google Scholar
G. R. A. Johnson, N. B. Nazhat, and R. A. Saadalla-Nazhat, “Reaction of the aquocopper(I) ion with hydrogen peroxide: evidence against hydroxyl free radical formation,” Journal of the Chemical Society, Chemical Communications, no. 7, pp. 407–408, 1985.
View at: Google Scholar
H. C. Sutton and C. C. Winterbourn, “On the participation of higher oxidation states of iron and copper in Fenton reactions,” Free Radical Biology and Medicine, vol. 6, no. 1, pp. 53–60, 1989.
View at: Google Scholar
M. Masarwa, H. Cohen, D. Meyerstein, D. L. Hickman, A. Bakac, and J. H. Espenson, “Reactions of low-valent transition-metal complexes with hydrogen peroxide. Are they “fenton-like” or not? 1. The case of ${Cu}^{+}$ aq and ${Cr}^{2 +}$ aq,” Journal of the Chemical Society, vol. 110, no. 13, pp. 4293–4297, 1988.
View at: Google Scholar
G. Czapski, S. Goldstein, and D. Meyerstein, “What is unique about superoxide toxicity as compared to other biological reductants? A hypothesis,” Free Radical Research Communications, vol. 4, no. 4, pp. 231–236, 1988.
View at: Google Scholar
G. R. A. Johnson and N. B. Nazhat, “Kinetics and mechanism of the reaction of the bis(1,10-phenanthroline)copper(I) ion with hydrogen peroxide in aqueous solution,” Journal of the American Chemical Society, vol. 109, no. 7, pp. 1990–1994, 1987.
View at: Google Scholar
M. Jezowska-Bojczuk, W. Leśniak, W. Bal et al., “Molecular mechanism of hydrogen peroxide conversion and activation by Cu(II)-amikacin complexes,” Chemical Research in Toxicology, vol. 14, no. 10, pp. 1353–1362, 2001.
View at: Publisher Site | Google Scholar
J. Schubert, V. S. Sharma, E. R. White, and L. S. Bergelson, “Catalytic decomposition of hydrogen peroxide by copper chelates and mixed ligand complexes of histamine in the presence of phosphate buffer in the neutral pH region,” Journal of the American Chemical Society, vol. 90, no. 16, pp. 4476–4478, 1968.
View at: Google Scholar
M. Y. El-Sheikh, F. M. Ashmawy, I. A. Salem, and A. B. Zaki, “Heterogeneous decomposition of hydrogen peroxide with transition metal-ammine complexes I. Kinetics of catalytic decomposition of hydrogen peroxide in presence of resins in the form of ammine- Cu (II) complex ions in aqueous medium,” Zeitschrift für Physikalische Chemie, vol. 268, pp. 595–606, 1987.
View at: Google Scholar
S. L. Bourke and J. Kohn, “Polymers derived from the amino acid L-tyrosine: polycarbonates, polyarylates and copolymers with poly(ethylene glycol),” Advanced Drug Delivery Reviews, vol. 55, no. 4, pp. 447–466, 2003.
View at: Publisher Site | Google Scholar
C. Methenitis, J. Morcellet-Sauvage, and M. Morcellet, “The interaction of poly(N-methacryloyl-L-alanine) with copper (II) 1. Potentiometric study,” Polymer Bulletin, vol. 12, no. 2, pp. 133–139, 1984.
View at: Publisher Site | Google Scholar
C. Methenitis, J. Morcellet-Sauvage, and M. Morcellet, “The interaction of poly(N-methacryloyl-L-alanine) with copper (II) 2. Spectroscopic study,” Polymer Bulletin, vol. 12, no. 2, pp. 141–147, 1984.
View at: Publisher Site | Google Scholar
C. Methenitis, J. Morcellet, G. Pneumatikakis, and M. Morcellet, “Polymers with amino acids in their side chain: conformation of polymers derived from glycylglycine and phenylalanine,” Macromolecules, vol. 27, no. 6, pp. 1455–1460, 1994.
View at: Google Scholar
C. Methenitis, G. Pneumatikakis, M. Pitsikalis, J. Morcellet, and M. Morcellet, “Polymers with amino-acids in their side-chain. Conformation of poly(N-methecryloyl-L-methionine,” Journal of Polymer Science Part A, vol. 33, pp. 2233–2239, 1995.
View at: Google Scholar
C. Methenitis, J. Morcellet, G. Pneumatikakis, and M. Morcellet, “Copper coordination by polymers with glycylglycine, phenylalanine or methionine in the side chain: potentiometric and viscosimetric study,” European Polymer Journal, vol. 39, no. 4, pp. 687–696, 2003.
View at: Publisher Site | Google Scholar
A. Lekchiri, J. Morcellet, and M. Morcellet, “Complex formation between copper (II) and poly(N-methacryloyl-L-asparagine),” Macromolecules, vol. 20, no. 1, pp. 49–53, 1987.
View at: Google Scholar
A. Lekchiri, M. Brighli, C. Methenitis, J. Morcellet, and M. Morcellet, “Complexation of a polyelectrolyte derived from glutamic acid with copper(II). Catalase-like activity of the complexes,” Journal of Inorganic Biochemistry, vol. 44, no. 4, pp. 229–238, 1991.
View at: Publisher Site | Google Scholar
A. Lekchiri, A. Castellano, J. Morcellet, and M. Morcellet, “Copper complexes and catalase-like activity of a polyelectrolyte derived from aspartic acid,” European Polymer Journal, vol. 27, no. 11, pp. 1271–1278, 1991.
View at: Google Scholar
R. K. Kulkarni and H. Morawetz, “Effect of asymmetric centers on free radical polymerization and the properties of polymers: methacrylyl alanine, methacrylyl glutamic acid, acrylyl glutamic acid, and their polymers,” Journal of Polymer Science, vol. 54, no. 160, pp. 491–503, 1961.
View at: Google Scholar
H. Yokoi, S. Kawata, and M. Iwaizumi, “Interaction modes between heavy metal ions and water-soluble polymers. 1. Spectroscopic and magnetic reexamination of the aqueous solutions of cupric ions and poly(vinyl alcohol),” Journal of the American Chemical Society, vol. 108, no. 12, pp. 3358–3361, 1986.
View at: Google Scholar
H. Yokoi, Y. Mori, and Y. Fujise, “Studies on the complex formation between iron(III) or copper(II) and poly(vinyl alcohol) in terms of inclusion of the Metal Hydroxide-Like Clusters,” Bulletin of the Chemical Society of Japan, vol. 68, pp. 2061–2065, 1995.
View at: Google Scholar
S. Skounas, C. Methenitis, and M. Morcellet, “Copper coordination by polymers with glycylglycine, phenylalanine or methionine in the side chain: Spectroscopic studies,” Unpublished results.
View at: Google Scholar
M. González-Álvarez, G. Alzuet, J. Borrás, S. García-Granda, and J. M. Montejo-Bernardo, “Structural and functional models for the dinuclear copper active site in catechol oxidases: synthesis, X-ray crystal structures, magnetic and spectroscopic properties of μ-methoxo-bridged dinuclear copper(II) complexes with N-substituted sulfonamide ligands,” Journal of Inorganic Biochemistry, vol. 96, no. 4, pp. 443–451, 2003.
View at: Publisher Site | Google Scholar
A. Pezeshk, F. T. Greenaway, and J. R. J. Sorenson, “Barbiturate copper complexes: preparation and spectral studies,” Inorganica Chimica Acta, vol. 80, pp. 191–195, 1983.
View at: Google Scholar
S. T. Kirksey Jr., T. A. Neubecker, and D. W. Margerum, “Thermally stable copper(III)- and nickel(III)-tripeptide complexes and their photochemical decomposition in acid solution,” Journal of the American Chemical Society, vol. 101, no. 6, pp. 1631–1633, 1979.
View at: Google Scholar
Y. Ikeda, M. Beer, M. Schmidt, and K. Huber, “ ${Ca}^{2 +}$ and ${Cu}^{2 +}$ induced conformational changes of sodium polymethacrylate in dilute aqueous solution,” Macromolecules, vol. 31, no. 3, pp. 728–733, 1998.
View at: Google Scholar
E. Tsuchida, H. Nishide, and T. Nishiyama, “Kinetic discussion on the catalysis of copper-partially-quaternized poly-(vinylpyridine) complexes,” Journal of Polymer Science Part A, no. 47, pp. 35–46, 1974.
View at: Google Scholar
A. Lekchiri, C. Methenitis, J. Morcellet, and M. Morcellet, “Effect of the complexation with copper(II) on the hydrodynamic behaviour of some polyelectrolytes,” Polymer Bulletin, vol. 17, no. 2, pp. 119–125, 1987.
View at: Publisher Site | Google Scholar
V. Malatesta, A. Gervasini, and F. Morazzoni, “Chelation of copper(II) ions by doxorubicin and $4^{'}$ ;-epidoxorubicin: ESR evidence for a new complex at high anthracycline/copper molar ratios,” Inorganica Chimica Acta, vol. 136, no. 2, pp. 81–85, 1987.
View at: Google Scholar
T. Breyer, F. W. Breitbarth, and W. Vogelsberger, “EPR spectroscopic investigation of the sol-gel transition in modified tetraethylorthosilicate gels,” Journal of Colloid and Interface Science, vol. 266, no. 1, pp. 153–159, 2003.
View at: Publisher Site | Google Scholar
B. J. Hathaway, “Copper,” Coordination Chemistry Reviews, vol. 52, pp. 87–169, 1983.
View at: Google Scholar
G. Multhaup, T. Ruppert, A. Schlicksupp et al., “Copper-binding amyloid precursor protein undergoes a site-specific fragmentation in the reduction of hydrogen peroxide,” Biochemistry, vol. 37, no. 20, pp. 7224–7230, 1998.
View at: Publisher Site | Google Scholar
R. P. Bonomo, R. Marchelli, and G. Tabbi, “Study of $H_{2} O_{2}$ interaction with copper(II) complexes with diamino- diamide type ligands, diastereoisomeric dipeptides, and tripeptides,” Journal of Inorganic Biochemistry, vol. 60, no. 3, pp. 205–218, 1995.
View at: Publisher Site | Google Scholar

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Copyright © 2010 Spyridon Skounas et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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