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The electronic structure of the two isoelectronic species $${\text{C}}_8$$ and $${\text{B}}_4{\text{N}}_4$$ has been studied at several ab initio levels (Hartree–Fock, CASSCF, CASPT2, and coupled cluster). For both systems, the total position spread tensor and the electron entropy have been computed and compared. These quantities are indicators that give insight into the electron mobility (and, in the case of the spread, the behavior of different-spin electrons), and are a measure of the multi-reference character of an electronic wavefunction. Our results indicate that the two systems are deeply different. In fact, the $${\text{C}}_8$$ cluster shows a pronounced multi-reference character. The $${\text{B}}_4{\text{N}}_4$$ system, on the other hand, is very well described by a single reference wave function. Analysis of ground-state electronic structure unveils different electron delocalization behavior in the studied systems.

In this study the spectrophotometric behaviour of gelatin-based hydrogels, in the presence and absence of dyes, was studied. The aim was to formulate equivalent-tissue phantoms to be used as 3D-dosimeter, suitable for Optical Computed Tomography (OCT). The hydrogels show good transparency and good stability of baseline optical density and, in the presence of dye, the response of optical density as a function of concentration was higher than in aqueous solution. The hydrogels were formulated in order to reduce the diffusion of the image of the irradiated field over time and to have stable fantoms as a function of time. To this purpose, the diffusion coefficients of two dyes, Bromophenol Blue (BPB) and Bromocresol Green (BCG), were determined as a function of the hydrogel chemical composition. As comparison, in some experiments Xylenol Orange (XO) was used. In particular, the presence of sucrose, as thickener, can reduce to almost half BPB mobility. In conclusion, it was shown that optical properties and controlled dye diffusion in gelatin-based hydrogels could allow using them as 3D-dosimeter for optical detection.

Reactions of Co(II) and Ni(II) salts with the monosodium salt of 3-hydroxy-4-nitrobenzoic acid (3) in aqueous solution resulted in isomorphous covalent complexes 3C and 3D, of centrosymmetric geometries. In similar conditions, 2-hydroxy-4-methoxybenzoic acid (5) led to the covalent Zn(II) complex 5A, exhibiting a marked dissymmetric geometry. The present crystallographic data with structural data for a series of closely related metal complexes previously reported allow a tentative rationalization of the solid-state architecture of such complexes. The dissymmetry in 5A was interpreted on the basis of a mixed (monodentate and bidentate) metal-ligation mode and a pyramidal coordination at the metal.

The purpose of this study was to investigate the complexes formed by copper(II) with potential non-steroidal anti-inflammatory agents (NSAIDs) under physiological conditions. A former study suggested that 2-benzylaminomethylpyrrolidine ligands could be good candidates as potential OIL ( OH-inactivating ligand) when complexed to copper(II). In order to assess the chemical behavior as OIL, [S]-2-[N-(2′-hydroxybenzyl)aminomethyl]pyrrolidine (OHbamp) was synthesized and bound to copper(II). Physico-chemical properties were determined at 37 °C in 0.15 M NaCl using glass electrode potentiometry, UV–Vis and circular dichroism spectroscopies, before and after copper(II) complexation. [Cu(OHbamp)(H2O)3]+ was the main complex found at both physiological and inflammatory pH values, showing appreciable stability at pathological pH compared to copper(II) complexes of histidine, the predominant low-molar-mass ligand of copper(II) in blood plasma. However, neutral species such as [Cu(OHbamp)2(H2O)2] and [Cu(OHbamp)(OH)(H2O)3] are predominant only above pH 8, preventing a significant amount of drug from diffusing through membranes at inflammatory pH. In conclusion, copper(II)-OHbamp system does not meet all the requirements to be an OIL. Nevertheless, these results allow us to better identify the chemical features needed for a good OIL candidate.

The crystal structures of two Mg(II) complexes of 3-hydroxy-4-nitrobenzoic acid have been reported. The first complex, 2 (C14H20N2O16Mg), consists of ionic entities comprising one hexaaquamagnesium cation and two organic carboxylate anions. The second complex, 3 (C7H15NO11Mg) consists of zwitterionic entities comprising one organic ligand per Mg atom. In both cases, the complexes are linked through an extensive hydrogen bonding network. The 3D supramolecular architectures of these complexes are also stabilized by two types of stacking interactions. An interesting interconversion between the two complexes was observed in aqueous solution.

As a nonessential element, aluminum is likely to be toxic both at low usual dietary levels in the long run (chronic toxicity) and at high therapeutic levels in shorter periods of time (acute toxicity). In both situations, aluminum toxicity is a direct function of aluminum bioavailability, which is itself dependent on Al(3+) solubility and charge neutralization. Dietary acids, by their intrinsic acidity and coordinating capacity, can extend the pH range, thus the section of the gastrointestinal tract, within which the Al(3+) ion remains soluble, and also help Al(3+) diffusion across the intestinal epithelium through the formation of neutral complex species. The present work examines the impact of glutamic acid, an essential amino acid also widely used in industrial food and drinks, on aluminum speciation in the gastrointestinal tract and blood plasma. Complex formation between the Al(3+) ion and glutamate has first been investigated through potentiometric titrations, complex stoichiometries being then checked by ESI mass spectrometry and NMR measurements. A series of mono- and polynuclear species has been characterized, whose influence on aluminum distribution in vivo has been assessed by computer simulation. The capacity of glutamate to maintain Al(3+) ions in solution under normal dietary conditions is predicted to be intermediate between glycine-like amino acids and succinate on the one hand, and tartrate and malate on the other hand, its Al(3+) neutralization effect being similar to that of succinate, tartrate and malate. These results, which point to a potential aggravating role of glutamate on aluminum gastrointestinal absorption, substantiate recent observations made on rats. In spite of the moderate effect expected from glutamate on aluminum bioavailability under most aluminum-based therapies investigated, attention is therefore called to the risk of glutamic acid ingestion simultaneously to any aluminum therapeutic form. Incidentally, the former implication of 'the' aluminum glutamate complex in the transfer of aluminum through the blood-brain barrier of aluminum loaded rats may effectively be attributed to one of the species characterized here, but is of no significance at all to aluminum contamination in humans, even at most extreme levels.

With a view to the possible use of copper(II)-*OH inactivating ligand (OIL) complexes as regulators of inflammation, the reactivity of the copper(II)-ascorbate system with hydrogen peroxide has been investigated in the presence of three key substances: histidine (the main copper(II) low molecular mass ligand in extracellular fluid), salicylic acid (the well-known nonsteroidal antiinflammatory drug, previously shown to be potentiated by copper(II) in animal models of inflammation), and anthranilic acid (an inactive substance by itself, known to be activated by copper(II) in the same models) at physiological pH (7.4) and inflammatory pH (5.5). Such substances may affect the amount of TBARS detected in solution following copper-mediated Fenton-like reactions through three distinct mechanisms: (i) by decreasing the Cu(II)/Cu(I) redox potential, i.e. at the expense of *OH radical production, (ii) by scavenging *OH radicals in the body of the solution, and/or (iii) by acting as a true OIL, i.e. at the expense of *OH detection. Redox potential measurements of initial solutions have been performed in parallel to TBARS determinations to help discriminate between different ligand influences. Computer-aided speciation has been used to understand the role of copper(II) distribution on the ligand effects characterised. Contrary to previous interpretations, histidine has been found to mainly affect *OH production by lowering the redox potential of the Cu(II)/Cu(I) couple. Salicylate, which has no effect on *OH production, has been confirmed to mainly scavenge *OH radicals in the body of the solution. Anthranilate, which both increases *OH production and decreases *OH detection, behaves as a potential OIL. These results tend to confirm our previous hypothesis that copper potentiation of antiinflammatory substances is indirect, i.e. independent of any interaction between metal and drug, whereas copper activation of substances that are inactive by themselves results from specific metal-substance interactions taking place at inflammatory sites.

It has long been established that copper complexes of inactive substances exert antiinflammatory activity and that copper complexes of nonsteroidal antiinflammatory drugs (NSAIDs) are more active than these drugs by themselves. Based on these observations, it was proposed that copper complexes of NAIDs are their active metabolites. This hypothesis was not confirmed for salicylic acid, however, as computer-aided speciation studies have shown that no copper-salicylate complex can reach significant levels in blood plasma. In view of this result, it was of interest to test with the same technique the influence on copper metabolism of an inactive substance known to be activated by copper. Anthranilic acid was chosen for this test in the present work. First, copper(II)-anthranilate interactions have been investigated by glass electrode potentiometry under physiological conditions. Given the key role of histidine as copper(II) ligand in blood plasma, copper(II)-histidine-anthranilate ternary equilibra have also been determined. Computer simulations of copper distribution have then been run relative to the two main biofluids in respect of global metabolism, i.e., gastrointestinal (g.i.) fluid and blood plasma. Like salicylic acid, anthranilic acid is expected to favor copper g.i. absorption, but cannot either exert any significant influence on plasma copper distribution. Clearly, the fact that anthranilate becomes antiinflammatory when administered with copper cannot originate in any effect of anthranilate on copper global metabolism. Speciation investigations have then been extended to the synovial fluid. Whereas salicylate does not appear to be a better ligand of copper in this medium than in blood plasma at any pH between 7.4 and 5.5, anthranilate on the contrary can mobilize increasing fractions of copper as the pH decreases, i.e., the more inflammation, the more copper is bound to anthranilate. This is in line with the recent observation that salicylate inactivates copper-induced .OH radicals through its bulk scavenging properties whereas .OH inactivation by anthranilate under the same conditions is a direct function of the copper-anthranilate binding. Anthranilate thus seems to correspond to the recently defined notion of .OH-inactivating ligand (OIL). More generally, these results provide a beginning of rationale for the antiinflammatory properties of copper complexes with substances that are active or inactive against inflammation by themselves. The extra antiinflammatory activity induced by copper on NSAIDs appears to be independent of any Cu(II)-NSAID association in vivo. On the contrary, the binding of inactive substances with copper(II) at inflammatory sites seems to be essential to their activation by copper.

Some years ago, the application of computer modeling to metal speciation in biofluids was questioned based on the discrepancy between the simulated distribution of copper(II) in blood plasma and related experimental results obtained by Neumann and Sass-Kortsak in reconstituted serum. A recent investigation of the relevant copper(II)-amino acid equilibria reconciled these conflicting data, confirming that the reliability of computer models crucially depends on the data on which they are based. Since then, however, some of the constants of the copper-serine system used in that study have been suspected to be overestimated. This work thus reports the redetermination of copper-serine and copper-histidine-serine formation constants under physiological conditions. In addition, serine being close to asparagine in Neumann and Sass-Kortsak's classification, copper-asparagine and copper-histidine-asparagine equilibria have also been reinvestigated. For asparagine complexes, former constants have been basically confirmed. In contrast, all constants relative to serine have effectively been found lower than the previous ones. The effects of these new data on the stimulated distribution of plasma copper are only minor, but a better agreement is observed relative to Neumann and Sass-Kortsak's models in reconstituted serum.

In the effort to improve the performance of hydroxylapatite (HA) in removing lead ions from aqueous solutions, millimeter-sized granules with 50 % porosity were synthesized. Such HA particles, after drying at 100°C, or heating at 800°C or 1100°C, exhibited the specific surface areas of 50 m2 g−1, 25 m2 g−1, and 5 m2 g−1, respectively. It was found that heavy metal sorption capacity of HAs can be related to their surface area. Non-calcined granules were difficult to handle and easy to crush. Hardened granules showed heavy metal absorption on their outer surfaces. Absorption capacity of sintered HA particles towards lead was lower but adsorbed lead ions were spread inside the porous structure of HA granules more evenly. Under flow conditions, lead ions were captured by HA at a rate of 0.5 mg g−1 min−1. Small lead phosphate aggregates were released from the HA sorbent together with calcium ions. Size of the aggregates depended on the lead concentration and ranged from 1–50 μm in diameter; the aggregates could be removed by ultrafiltration. Results show that porous hardened HA granules can be used as an efficient phosphate source for the immobilization of lead ions from aqueous media. Organic ligands tend to interfere with the water purification procedure.

Pharmacological activities of copper(II) complexes are a direct function of the nature of their ligands associated with the metal ion in vivo. Some of these, defined as *OH-inactivating ligands (G. Berthon, Agents Actions 39 (1993) 210-217), may act as specific "lures" for hydroxyl radicals at inflammatory sites and behave as pseudo-catalase-like agents. This property has been advanced for anthranilic acid (H. Miche, V. Brumas, G. Berthon, J. Inorg. Biochem. 68 (1997) 27-38). With a view to improve the chemical features required to render such inactive substances effective anti-inflammatory drugs through their association with copper(II), an in vitro investigation into copper(II) interactions with the anionic form of an anthranilic acid derivative, namely 3-methoxyanthranilate (Man), has been performed under experimental conditions pertaining in vivo. Copper(II)-Man complex equilibria have been determined using glass electrode potentiometry, then checked by UV-vis and mass spectrometries. Given the prime role of histidine as a copper(II) ligand in blood plasma, copper(II)-histidine-Man ternary equilibria have also been studied. Subsequent computer simulations of the distribution of copper(II) in the extracellular fluid revealed that Man can specifically mobilize Cu(II) ions under inflammatory conditions without affecting their distribution under normal physiological conditions. Thiobarbituric acid reactive substances (TBARS) tests conducted with respect to standardized copper-mediated Fenton-type reactions (P. Maestre, L. Lambs, J.P. Thouvenot, G. Berthon, Free Rad. Res. 20 (1994) 205-218) have shown that, like anthranilic acid, Man can effectively both increase the Fenton-like reactivity of copper and decrease the amount of TBARS detected in solution, i.e., act as a potential *OH-inactivating ligand.

Recently a growing body of evidence has accumulated on the beneficial effects of copper compounds toward various models of inflammation, and copper complexes of nonsteroidal antiinflammatory drugs (NSAIDs) have been shown to be more effective in this respect than the parent agents. However, the origin of this activity remains unclear: The ability of NSAIDs to influence copper metabolism is still questionable, and apart from the claimed SOD-like activity of copper salts in vivo, relatively little is known about how copper-NSAID interactions may help regulate the inflammatory process. Before the potential role of copper-NSAID complexes versus inflammation can be elucidated, speciation studies are necessary (i) to analyze the overall influence of these drugs on copper metabolism and (ii) to discriminate the individual complexes likely to represent the active form of the drug in vivo. In this paper, copper(II) complex equilibria with salicylic and acetylsalicylic acids--and benzoic acid used as a reference--as well as the mixed-ligand complex equilibria generated by these binary systems and L-histidine [main low-molar-mass ligand of copper(II) in blood plasma] have been investigated under physiological conditions (37 degrees C; 0.15-M NaCl). Confirming previous observations by others, resulting simulated plasma copper distributions virtually rule out any quantitative influence of salicylate on copper tissue diffusion at therapeutic levels. Even though, as is presently shown, both salicylate and acetylsalicylate may favor the gastrointestinal absorption of copper, it seems unlikely that salicylate can exert its antinflammatory activity predominantly through copper complexation. The assertion that copper-NSAID complexes represent the active forms of NSAIDs therefore seems to be of limited significance for salicylate.

S-carboxymethyl-L-cysteine (SCC) is a mucolytic agent extensively used in the treatment of respiratory tract disorders. Some of the undesirable side effects observed during SCC therapy being reminiscent of symptoms characteristic of copper and zinc imbalances, the objective of this paper was to test the possible interference of SCC with the metabolism of these two metals. Copper(II)- and zinc(II)-SCC complex equilibria have thus been investigated under physiological conditions by means of classical potentiometry combined with computer-assisted calculation techniques. Formation constants derived from these studies have then been used to simulate 1) the potential influence of SCC on the distribution of the above metals in blood plasma and 2) the extent to which gastrointestinal interactions between the drug and each metal ion in turn are likely to affect the bioavailability of each other. The results of these simulations show that 1) plasma therapeutic levels of SCC are not likely to induce dramatic changes in the distributions of copper(II) and zinc(II) low molecular weight fractions, 2) the gastrointestinal distribution of the drug is not affected by standard dietary doses of these metals, and 3) in contrast, therapeutic concentrations of SCC are capable of mobilizing significant fractions of both metals into tissue-diffusible electrically neutral complexes. In conclusion significant depletions of neither copper nor zinc are to be expected from oral administration of SCC. While the drug may to some extent facilitate the excretion of Cu2+ and Zn2+ ions from blood plasma, its gastrointestinal influence is, on the contrary, favorable to a better absorption of these two metals.