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Journal of the Brazilian Chemical Society

Print version ISSN 0103-5053On-line version ISSN 1678-4790

J. Braz. Chem. Soc. vol.14 no.6 São Paulo Nov./Dec. 2003

http://dx.doi.org/10.1590/S0103-50532003000600002 

REVIEW

 

Molecular materials and devices: developing new functional systems based on the coordination chemistry approach

 

 

Henrique E. Toma

Instituto de Química, Universidade de São Paulo, CP 26077, 05513-970 São Paulo - SP, Brazil

 

 


ABSTRACT

At the onset of the nanotechnology age, molecular designing of materials and single molecule studies are opening wide possibilities of using molecular systems in electronic and photonic devices, as well as in technological applications based on molecular switching or molecular recognition. In this sense, inorganic chemists are privileged by the possibility of using the basic strategies of coordination chemistry to build up functional supramolecular materials, conveying the remarkable chemical properties of the metal centers and the characteristics of the ancillary ligands. Coordination chemistry also provides effective self-assembly strategies based on specific metal-ligand affinity and stereochemistry. Several molecular based materials, derived from inorganic and metal-organic compounds are focused on this article, with emphasis on new supramolecular porphyrins and porphyrazines, metal-clusters and metal-polyimine complexes. Such systems are also discussed in terms of their applications in catalysis, sensors and molecular devices.

Keywords: molecular nanotechnology, supramolecular chemistry, molecular devices, molecular films, sensors


RESUMO

Neste limiar da era nanotecnológica, o planejamento molecular dos materiais e os estudos de moléculas isoladas estão abrindo imensas possibilidades no emprego de sistemas moleculares em dispositivos eletrônicos e fotônicos, bem como em aplicações tecnológicas baseadas em propriedades de chaveamento ou reconhecimento molecular. Com esse escopo, os químicos inorgânicos em particular, podem aplicar com vantagens as estratégias proporcionadas pela química de coordenação, para construir nanomateriais funcionais que permitam a exploração das propriedades dos centros metálicos e das características dos ligantes presentes. A química de coordenação também oferece recursos eficientes na auto-montagem de nanoestruturas, baseadas na especificidade da interação metal-ligante e nas características estereoquímicas dos complexos. Diversos materiais moleculares gerados a partir de compostos inorgânicos e metal-orgânicos são focalizados neste artigo, com ênfase em novas porfirinas e porfirazinas supramoleculares, clusters e complexos metálicos. Tais sistemas também são enfocados sob o ponto de vista de suas aplicações em catálise, sensores e dispositivos moleculares.


 

 

1. Introduction

Molecular nanotechnology is an important branch of the nanosciences, exhibiting strong chemical appeal, besides encompassing most of the exciting aspects of nanomaterials, nanobiology and nanoelectronics. In a historical perspective, it was Richard Feynman,1 in his 1959 talk "There's Plenty of Room at the Bottom" who first considered the possibility of processing the information at the atomic level, calling the attention for the new universe hidden in the nanodimensional space. In 1965, Arthur von Hippel2 proposed the bottom up approach to materials design, in his book "The Molecular Designing of Materials and Devices". In the following years, the molecular approach expanded considerably, from the development of chemical vapor deposition, sol-gel and related processes, leading to dramatic changes in electronics and materials design.

Nowadays, the future of the technology unquestionably bears on the progress of the materials science. Consequently, with the rise of molecular nanotechnology, molecular materials are becoming a major focus of interest for the design of nanostructures and devices.3-20 In fact, functional nanostructured molecular materials are being currently pursued in the academy and industries, relying on the bottom up approach, as envisaged by Erix Drexler,3 but using molecular building blocks and supramolecular chemistry as tools.5-20

Supramolecular chemistry provides, perhaps, the most important strategy toward molecular nanotechnology. It has been defined as the chemistry beyond the molecule.5 Its essence arises from the special way the different molecules interact, exchanging information and creating organized structures. In the supramolecular design, molecular building blocks incorporating suitable functional groups are specially devised in order to promote their effective coupling by means of hydrogen bonding, hydrophobic or/and electrostatic interactions, or metal ion coordination. The last point, here referred as the coordination chemistry approach, has been systematically exploited by our group since the last decade. It is increasingly being employed in the development of supramolecular systems, due to its many advantages, such as the self-assembly character of the metal-ligand complexation; the control of selectivity based on simple acid-base principles, and the introduction of a variety of structural, electronic, energetic and kinetic properties. Such important properties convey an exceptional functionality gain for the nanostructured materials containing metal complexes. Now, going back to an earlier expectation, reported in 1991 by the occasion of the National Meeting of the Brazilian Chemical Society,7 this article will focus mainly on the exciting perspectives of the coordination chemistry approach toward molecular nanotechnology.

 

2. A Chemical Route for Molecular Nanotechnology

Chemistry provides the starting point in the route for molecular nanotechnology shown in Figure 1, creating from atoms and molecules, the molecular building blocks (or synthons) for the construction of nanoscale structures, such as nanoparticles, nanolayers and nanotubes. By working out appropriately the assembled nanostructures, an unlimited number of nanostructured materials can be generated, allowing important applications, such as dispersions and coatings, high surface area materials, high performance materials and functional nanodevices.

 

 

The coordination chemistry approach has been successfully employed in the self assembly of highly organized structures, such as those resulting from the direct interaction between linear polypyridine polymers and copper(I) ions.5,19 Nanoporous materials have been generated from discrete molecular building blocks, as exemplified by the series of nanoscale cavity-containing coordination compounds, reported by Belanger et al..8 In this particular aspect, the coordination approach is very effective, circumventing two of the most conventional problems found in solid state chemistry. The first one is the collapse of the channels upon removal of the solvent from the porous solid. In the molecular nanostructured materials involving bridged coordination compounds, the interactions are usually strong enough to preclude the cavity and channel collapse. The second is the occurrence of multiple intersecting and interpenetrating structures replacing the vacancies in the solids. This is less prone to occur in such nanostructured materials, if intentionally substitution-inert coordination compounds are employed.

Because of their key role, molecular building blocks should be carefully planned in order to generate nanostructured materials. Most of the strategies rely upon the preprogramming of synthons, in order to allow a directed-assembly approach. For instance, in the assembly of square cavity structures (Figure 2), synthons have been employed8 consisting of octahedral complexes displaying rigid or semi-rigid bifunctional edges in cis-configuration, a detail which allows them to coordinate sequentially.

 

 

This type of molecular nanostructured material exhibits a selective size control response when deposited onto electrode surfaces, discriminating, by means of amperometric response, the small ferrocene type of ions from typically large redox active species.8

 

3. Nanoscale Technology

The development of nanoscale technology is a rather complex subject, which can be focused on, either in terms of a bottom-up (molecular approach) or a top-down (miniaturization) approach. The main reasons behind moving to smaller sizes are the superior physical properties of the nanostructured materials, including the improved mechanical, electronic and/or optical response in molecular timescales, the better efficiency of the precisely engineered micro/nano electronic devices, and more powerful processing and computing performance. Microelectromechanical (MEMS) and microelectronic devices have been designed based on the available lithography processes. Further reduction to the nanoscale dimension, however, will require the use of very short wavelengths, in the ultraviolet and X-ray spectral region, as provided by the Synchroton radiation, implying in the involvement of very sophisticated and expensive equipments.

Nanoparticles combined with polymers can generate a wide variety of nanocomposite materials. Although they are expected to be the first high-scale nanotechnology products to appear in the market, it should be noticed that the modification of the chemical and physical properties of the polymers by using fine particles is not a new fact. For instance, most of the plastic coatings employed in electrical cables already contain large amounts of finely divided inorganic oxides and clays; whereas rubber tires contain a high percentage of carbon black. However, it should be mentioned that the remarkable improvement of the mechanical properties of the plastics by the use of suitable inorganic nanoparticles is attracting more and more investiments in this area. Such nanocomposites are contributing for a better quality and low cost of the containers and recipients, specially for beverages and food. The resistance of the optical glasses is significantly improved by the incorporation of nanoparticles. Also, inorganic nanoparticles are being successfully employed in high quality photographic papers, preventing the diffusion and spreading of the images by concentrating the very small dots of ink at the impact region. The most impressive applications of nanoparticles will be found in cosmetics. Nanoparticles can be used to impart a much better performance for the cosmetic products, such as light scattering control, ultraviolet radiation protection, softness, and coverage.

Molecular machines and devices are being pursued as possible nanosize versions of the microscale components of MEMS and microelectronics.9-20 The development of this area has been very impressive, and is moving up to the top end of the miniaturization scale: the single molecule technology. With the aid of scanning probe microscopy (AFM, STM), single atoms and molecules can be precisely imaged and manipulated. Such a positional control allows to connect them to microelectrodes, or suitable circuits, and thus to perform single molecule conduction measurements.

A single molecule can efficiently capture light or electrons, as well as electric or magnetic impulses, and then, processing information. For instance, it can also undergo geometrical changes, such as cis-trans photo-isomerization, producing atomic movements under the action of light. Specialized molecules can conduct electron (molecular wires), or pump electrons/photons (photonic pumps). Molecules can also be effective probes for molecular recognition. Combining such many abilities and properties, molecules can be designed to communicate with each other, signalizing this by means of color changes, emission of light and/or sound, release or uptake of protons and ions, etc. They can also be interfaced to a metal wire or fiber optics, for transducing their response into measurable electrical or optical signals. The possibility of changing the molecular properties can be used to convert them into molecular optical or electrical switches. A very interesting case is the ability of some dichalcogenide carbamate esters to undergo reversible light induced tautomerism, generating two enantiomers. The reversible light induced conversion of the two quiral forms can be used to write and read information, in a binary language. This class of optoelectronic molecular materials has been patented as chiropticeneâ switch, and recently employed in supramolecular opto-electronic architectures, supporting a memory capacity of 2 terabytes, in a device of the size of a cubic inch.21 Therefore it is not surprising that smallest nanomachines can be really made up of single molecules, fitted in a suitable supramolecular environment.

 

4. Molecular Building Blocks and Supramolecular Chemistry

Coordination compounds such as those illustrated in Figure 3 have been systematically employed as versatile building blocks for the assembling of symmetric supramolecular structures.7,22,23 Such complexes are rather stable and inert, imparting convenient structural characteristics to the supramolecular species, and also a wide variety of functional aspects from their rich chemistry. As a matter of fact, ruthenium(II) polypyridine and polypyrazine complexes (Figure 3a) are among the most extensively investigated compounds in the last decades, because of their remarkable photochemical and photophysical properties.24,25 Triangular m-oxo-bridged ruthenium-acetate clusters (Figure 3b) provide another interesting class of complexes, displaying strong electronic delocalization, and a series of reversible monoelectronic redox processes in the range of -2.0 to 2.0 V. The behavior of the triangular center can be modulated by the application of potentials, as well as by the nature of the axial ligand. This aspect is particularly interesting, since at very negative potentials, the triangular clusters become strong p-donor agents, while at the opposite extreme they act as strong p-acceptor agents. A comprehensive review of the triangular ruthenium clusters has been recently reported.22 Iron(II) and ruthenium(II) polyimine complexes (Figure 3c) functionalized with pyridine bridging groups provide flexible building blocks for supramolecular structures and have also been exploited for molecular recognition purposes. Meso-tetra(4-pyridyl)porphyrins (Figure 3d) are particularly important because of the presence of the biomimetic porphyrin center, which can be further exploited in combination with the several metal complexes, through the bridging pyridine ligand. Finally, the tetrapyridylporphyrazine species (Figure 3e) differ from the corresponding porphyrin analogues, by the presence of the four nitrogen atoms at the meso-position and by the fused pyridine ring.

 

 

Combination of such molecular building blocks can be performed by using metal ions as linking elements, but the direct combination usually leads to insoluble, random polymeric materials. A better control can be achieved by employing suitable metal complexes displaying functional groups for selective molecular interactions or for carrying out electrochemical coupling, via electropolymeri- zation reactions, such as [Fe(CN)5]3-, [RuCl(bipy)2]+, [RuCl(phen-Cl)2]+ and [Ru3O(Ac)6(py)2]+. The use of such metal complexes attached to the peripheral bridging groups has been proved highly rewarding. In fact, by combining ruthenium(II)-polypyridine complexes and porphyrins or porphyrazines, novel types of supermolecules exhibiting enhanced chemical, electrochemical, photochemical and photophysical properties have been generated. A typical example is shown in Figure 4. Strong hydrophobic interactions allow the packing of the highly symmetric supermolecules into organized molecular layers. By making use of appropriate combinations of electrostatic and p-stacking effects, functional bilayered structures have been assembled, involving different types of porphyrins and porphyrazines supermolecules. The chemistry of such polymetallic porphyrins has been recently reviewed,25,26 and will not be dealt with here. Instead, we will concentrate on the recent progress in the characterization and properties of the molecular materials generated from the supramolecular approach, as well as on their applications in molecular devices.

 

 

5. Proton-Induced Molecular Switching

The development of molecular switching represents an important issue to be pursued in the design of molecular devices. In the coordination chemistry approach, molecular switching can be conveniently performed by polynuclear complexes containing suitable bridging ligands, capable of modulating the intermetallic electronic interactions. This control can be performed by exploiting two crucial factors: the molecular geometry and the electronic properties of the bridge. In this way, switches can be made by chemically or physically changing the molecular conformation or the metal-metal separation, as well as, by tuning the degree of the electronic coupling through the redox and/or acid-base properties of spacer.27-33 Another way of controlling metal-metal interactions is based on the differential solvent effects on the metal complexes.34,35

A simple and efficient pH-induced molecular "on/off" switching has been recently devised based on a symmetric bridged ruthenium dimer, [(edta)Ru(m-L)Ru(edta)]n- , where n = 3, or 4, and L = benzotriazolate ligand, by exploiting its unusual mixed-valence state behavior as a function of the pH.36 Benzotriazole is an N-heterocycle possessing three vicinal coordinating N-atoms, with the ability to form mono37-39 and binuclear complexes40-42 with transition metal ions. The chemistry of this type of ruthenium-benzotriazolate complex is characterized by a fluxional coordination model involving the bridging ligand.

Due to the strong metal-metal electronic coupling, the symmetric binuclear complex, [(edta)Ru(m-L)Ru(edta)]3_ is readily formed from the reaction of [RuIII(edta)(H2O)]_ with benzotriazole, even in the presence of an excess of the bridging ligand.36 The cyclic voltammograms in aqueous solutions at several pH, show two reversible wave couples, with identical current intensity at any potential scan rate and typical monoelectronic Nernstian behavior, as shown in Figure 5. The redox potentials E(1) and E(2) refer to the RuIIIRuIII/RuIIIRuII and RuIIIRuII/RuIIRuII couples. By decreasing the pH of the solution, the most evident transformation in the cyclic voltammograms is the progressive decrease of DE = E(1)-E(2), from 195 mV (at pH 8.0) to ca. 75 mV (at pH 2.5). The calculated pKa of the bridging benzotriazole ligand is 3.3. At pH 8.0, a very strong intervalence band appears at 1450 nm (e = 2200 mol-1  L cm-1), exhibiting a rather narrow bandwidth (2900 cm-1) as compared with the theoretical one (3990 cm-1) for a class III system in the Robin-Day categorization of mixed valence systems.43 All the data support a strongly coupled mixed-valence system. Below pH 3, the protonation of the bridging ligand decreases dramatically the electronic coupling between the two metal centers, leading to a rather weak and broad intervalence transfer band around 1410 nm (e = 185 mol-1  L cm-1).

 

 

The rather distinct strengths of electronic coupling for these protonated and deprotonated mixed-valence complexes has been rationalized from a molecular orbital energy/superexchange perspective.43 Apart from the structural factor (geometric intermetallic distance), the magnitude of the interaction between the metal ions depends essentially on the mixing between the redox levels of the ruthenium(II,III) ions and the frontier orbitals of the bridging ligand. Unlike pyridine and pyrazine ligands, which have low-lying p-orbitals, and therefore act as p-acceptor ligands, the triazolate derivatives are similar to imidazoles and behave as s/p-donors.44,45 This means that the metal-metal electronic communication is governed predominantly by a hole-transfer mechanism.46 As a consequence, protonation of the benzotriazolate ligand induces a decrease of its p-orbital energies, and the interaction between the dp(Ru) and p(btaH) orbitals decreases, leading to the lowering of the resonance energy.

In this way, the metal-metal electron coupling can be modulated as a function of the pH, from the protonation/deprotonation of the intervening benzotriazolate (bta-)/benzotriazole (btaH) ligand, providing a striking proton-induced molecular switching system as illustrated in Figure 6.

 

 

6. Molecular Recognition

Iron(II) polyimine complexes functionalized with bridging groups provide useful building blocks for the generation of supramolecular structures, as exemplified in Figure 7. Such complexes exhibit characteristic red-violet colors, and their low spin configuration results from the exceptional stability of the iron(II)-diimine bonding.47

 

 

An interesting multibinding complex has been obtained48 by attaching four aliphatic polyamine chains to a low spin, iron(II)-polyimine center, derived from 2,6-diacetylpyridine, as shown in Figure 8.

 

 

Molecular simulations for this complex corroborate the evidence from 1H NMR spectroscopy of a symmetric structure, with the four polyamines displaying a tetrahedral arrangement around the metal center. The protonated polyamine complex interacts specifically with hexacyanoferrate(II) ions, generating an inclusion compound which has been characterized by means of vibrational and Mössbauer spectroscopy, and cyclic voltammetry.48 The proposed binding modes involve hydrogen bonding of four cyanide groups of the hexacyanoferrate(II) ion with the protonated amines, leaving two cyanide ligands for intermolecular interactions, as shown in Figure 9.

 

 

7. Photoinduced Charge-Separation in Supramolecular Systems

Polynuclear metal complexes containing phophysically active centers are particularly interesting from the point of view of photoinduced electron transfer and energy transfer processes.49-54 The presence of a metal complex attached to the photoactive center via a bridging ligand provides additional pathways for the deactivation of the excited states, and in some cases can promote effective charge-separation, giving rise to molecular dyad and triad devices. In these systems, the geometry, intermetallic separation distance, and electronic properties of the bridging ligands are relevant factors to be considered, in addition to the photochemical and photophysical characteristics of the metal ions.

Recently dyads and triads based on the photoactive, multibridging tris(bipyrazine)ruthenium(II) complex directly bound to transition metal complexes, have been generated55 by following the coordination chemistry approach previously employed in the design of symmetric heptanuclear supermolecules, from [Ru(bpz)3]2+ (bpz = bipyrazine).56-58 Such new systems contain a tris(bipyrazine) ruthenium(II) ion attached to bis(bipyridine) chlororuthenium(II)/(III) or pentacyanoferrate(II)/(III) complexes via a bipyrazine bridging ligand, e.g., [Ru(bpz)3Ru(bipy)2Cl]3+/4+ or [Ru(bpz)3Fe(CN)5]-/0 , as shown in Figure 10(A,B) (bipy = 2,2'-bipyridine). By attaching both complexes to the [Ru(bpz)3]2+ center, the triad system [(CN)5FeIII(bpz)2RuII(bpz)Ru II(bipy)2Cl]+ (Figure 10C) has been obtained, after suitable oxidation of the iron(II) sites.

 

 

The electronic spectrum of the bimetallic complex in the visible region exhibits two strong, composite bands at 575 and 440 nm. According to the calculations, the electronic band at 575 nm arises from the excitation from MO 155 (HOMO), mainly localized on the [RuII(bipy)2Cl]+ moiety (71%), to MO 156 (LUMO), mainly localized on the bridging bpz ligand (61%); thus corresponding to a RupII®bpz(bridge) charge-transfer transition. Another related transition, from MO 155 to MO 159 (the last one exhibiting 82% bpz bridge character), is theoretically expected at 487 nm. It is however much less intense, being masked by the strong band at 575 nm. The second characteristic band at 440 nm corresponds to the MO 152 ® MO 157 transition centered on the [RuII(bpz)3]2+ chromophore. It is interesting to note that MO 152 involves 65% RucII + 29% non-bridging bpz character. There is only little contribution of the bridging bpz ligand (5.8%) to this level. Surprisingly, MO 157 exhibits 71% non-bridging bpz character, as compared with 16% for the bridging bpz one. Therefore, the absorption band at 440 nm involves preferential excitation of the RucII dp electrons to the non-bridging bpz p* levels, rather than to the bridging bpz ones. The high energy transition as a shoulder at 410 nm, corresponds to the MO 149 ® MO 156 excitation, where the first MO has 57% RuIIc character and the second one, 61% bridging bpz character. These results indicate that in the [RuII(bpz)3]2+ moiety, the excitation to the bridging bpz p* levels involves higher energies, as compared with the excitation to the corresponding non-bridging ligands.

At room temperature, the bimetallic complex exhibits only a weak asymmetric emission band at 608 nm, associated with the [Ru(bpz)3]2+ center, indicating substantial quenching from the [Ru(bipy)2Cl]+ moiety. The measured lifetime is 0.558 ms. The lack of emission from the [Ru(bipy)2Cl(bpz)]+ moiety is consistent with the fact that [Ru(bipy)2Cl(pz)]2+ and related [Ru(bipy)2XY] species are not good emitters at room temperature.59 This type of behavior has been ascribed to efficient mechanisms of deactivation of the 3MLCT excited state, associated with the existence of low energy ligand field states.49,60

The excitation process corresponds to:

In this system, electron transfer in the excited bimetallic complex is expected to predominate over energy transfer. The electron transfer mechanism seems to be reflected in the contrasting emission lifetimes observed at room temperature (0.558 ms) and at 77 K (9.4 ms). In general, electron transfer is less effective in solid glassy solvents at 77 K, because of the outer-sphere reorganization requirements involved,61-65 thus increasing the luminescence lifetimes. Time resolved, differential absorption spectrum of the transient species shows a transient absorption signal around 430 nm, reflecting the bleaching of the MLCT band in the starting [Ru(bpz)3]2+ chromophore, while the rise of the absorption bands at 380 and 750 nm is consistent with the formation of the bpz- radical species, as expected for the excited bimetallic complex, [(bpz)(bpz-)RuIII(bpz)RuII(bipy) 2Cl]3+* .

An interesting point is the observed bleaching of the absorption around 600 nm. This absorption coincides with the MLCT bands in the [RuII(bipy)2(bpz)Cl]+ moiety, and the observed changes can only be interpreted in terms of the occurrence of an intramolecular electron transfer process, generating the [(bpz)(bpz-)RuII(bpz)RuIII (bipy)2Cl]3+ species, in parallel with the radiative and non-radiative decay processes, e.g.:

The decay of the [(bpz)(bpz-)RuII(bpz)RuIII (bipy)2Cl]3+ transient species has been measured by means of flash-photolysis, proceeding according to a first order process with k = 1.3 x 106 s-1, regenerating the starting [(bpz)2RuII(bpz)RuII (bipy)2Cl]3+ complex.

The precursor trinuclear complex [(CN)5FeII(bpz) RuII(bpz)2RuII(bipy)2Cl] + displays the characteristic MLCT bands in the [Ru(bpz)3]2+, [Ru(bipy)2(bpz)Cl]+ and [Fe(CN)5(bpz)]3- moieties at 440, 600 and 700 nm, respectively. The three distinct moieties exhibit rather contrasting Eo values, i.e. 2.08, 1.14 and 0.70 V, respectively. In this way, one can carry out a selective oxidation of the [Fe(CN)5(bpz)]3- group. This results in the decay of the absorption band at 700 nm, so that the absorption spectrum of the mixed valence triad [(CN)5FeIII(bpz)RuII (bpz)2RuII(bipy)2Cl]- becomes very similar to that for the bimetallic [RuII(bpz)3RuII(bipy)2Cl] + complex.

Such mixed valence triad does not exhibit detectable luminescence properties. However, rather interesting time resolved, differential absorption profiles have been obtained from flash photolysis experiments. Initially, in a nanosecond time scale, there is a bleaching of the absorption at 440 nm, associated with the [RuII(bpz)3]2+ chromophore in the trinuclear complex, generating the [(CN)5FeIII(bpz)RuIII (bpz-) (bpz)RuII(bipy)2Cl]- * excited state.

The excited state decays according to a first order process, with k = 7.4 x 107 s-1, regenerating the absorption band at 440 nm. This process is accompanied by a partial bleaching of the absorption band at 600 nm associated with the [Ru(bipy)2Cl]+ chromophore, masking the rise of the absorption band of [FeII(CN)5(bpz)]3- at 700 nm, thus reflecting a sequence of steps which lead to long distance charge-separation, in the inverted mixed valence complex [(CN)5FeII(bpz)RuII (bpz)2RuIII(bipy)2 Cl]-.

The regeneration of the starting complex via charge-recombination is relatively slow, proceeding with a first-order rate constant k = 1.7 x 106 s-1

 

8. Vectorial Energy Transfer and Antenna Effect

One of the most important features responsible for the great efficiency of photosynthesis is the energy transfer process from the neighboring chromophores to the special pair, through the so called antenna effect.66-77 Because of their key role, energy transfer processes have been extensively studied for a number of systems. For instance, Lehn and co-workers.78 have shown that the luminescence from Eu2+ ion is enhanced by energy transfer from the criptate ligand containing three 2,2'-bipyridine subunits, especially when excited in the intraligand ppp* transition.

Recently, a new calix[4]arene receptor (Figure 11) modified with 8-hydroxyquinoline has been reported by our group.79 This species exhibits a characteristic emission band at 488 nm associated with the 8-oxyquinoline group, and has been designed to incorporate the luminescent Eu3+ and Tb3+ ions by coordination of the oxygen atoms of the quinoline and calixarene units. In the case of the Eu3+ complex, a less intense 8-oxyquinoline fluorescence emission is observed at 490 nm, accompanied by a series of narrow bands associated with the lanthanide 5D0,1 to 7Fj transitions. The strongest europium ion emission is observed at 619 nm, corresponding to the electric-dipole allowed 5D0®7F2 hypersensitive transition. The excitation profile for the 8-oxyquinoline emission in the corresponding Eu3+ complex practically coincides with its absorption bands. In the phosphorescence mode, only the emission of the europium ion has been observed, while the excitation profiles are consistent with the energy transfer from the calixarene ring, rather than from the 8-oxyquinoline one. According to the electronic spectra, the 1pp and 3pp levels of calixarene are higher in energy than those of the 8-oxyquinoline group. The efficient calixarene singlet-triplet conversion by the heavy metal effect promotes energy transfer to the 5D0 level of Eu3+, thus explaining the observed antenna effect. Presumably, since the 1pp* of 8-oxyquinoline occurs at 490 nm, the 3pp* level is lower than the 5D0 level of Eu3+.

 

 

Similar Eu(III) complexes containing three b-diketone and one 2,2'-bipyridine ligands have been reported by Gameiro et al.80-82 Those complexes exhibit the characteristic Eu(III) emission, under UV irradiation, promoted by efficient antenna effect, as in the case of the calix[4]arene complex. However, in the case of the 4,4,4-trifluoro-1-fenil-1,3-butadione (btfa) complex, i.e. [Eu(btfa)3(bipy)], the lanthanide emission is supressed, presumably by photodecomposition reactions. This property has been exploited for the design of rather promissing molecular dosimeters, for UV exposure.

The occurrence of vectorial energy transfer68,75,83 has also been reported for a zinc porphyrin species modified with four tris-(4,4'-dimethyl-2,2'-bipyridine)ruthenium(II) complexes covalently bound at the meso- positions,84 [ZnTBipyP{Ru(dmbipy)2}4]8+ (Figure 12).

 

 

Such species exhibited a characteristic metalloporphyrin spectrum, with absorption bands at 437 (Soret), 570 and 615 nm; in addition to the ruthenium complex bands at 295 (p®p*) and 490 nm (MLCT). It is interesting to note that the Soret band is broadened and less intense than in conventional or analogous supermolecular porphyrins.76,77 This behavior is similar to that previously ascribed85 to the coupling between the transition moment vectors of the Soret and RuII(dp)®bipy(p*) transitions. The coupling is favored when the difference between the transition energies tends to zero and the oscillator strengths are high. In the case of [ZnTBipyP{Ru(dmbipy)2}4]8+, the porphyrin transitions are sensitive to coordination effects, while the ruthenium complex transitions are virtually insensitive. This characteristic has been used to tune the electronic coupling between the central and peripheral subunits, by shifting the porphyrin energy levels.

The structure of [ZnTBipyP{Ru(dmbipy)2}4]8+ molecule has been especially designed for efficient vectorial energy transfer from the peripheral ruthenium complexes to the porphyrin moiety. In this system, the excited triplet MLCT states of the ruthenium complexes are energetically close to the lowest singlet excited state (S1) of the zinc porphyrin. It is known that the excited electron in the MLCT state of ruthenium bipyridine complexes is localized in the bipyridine ring with the lowest energy p* state. On the other hand, the p* energy level of the 4,4'-dimethyl-2,2'-bipyridine ligands in the [RuII(4,4'-dmbipy)3]2+ complexes is higher than of ruthenium complexes with non substituted bipyridine ligands,22,23 such that their emission bands occur at 633 nm and 613 nm, respectively. In the supramolecular complex all the bipyridine rings of the peripheral complexes have a methyl substituent, except for the bridging ring that is bound to the aromatic porphyrin ring. Thus, the excited electron should be preferentially localized on the bridging pyridyl ring, facilitating the vectorial energy transfer processes from the ruthenium complexes to the porphyrin ring.

When excited at 500 nm (ruthenium complex MLCT transition) [ZnTBipyP{Ru(dmbipy)2}4]8+ exhibits predominantly ruthenium complex emission pattern, but showing significant contribution of the zinc porphyrin emission. On the other hand, the spectrum obtained after excitation at the Q band at 570 nm is dominated by the S1 zinc porphyrin emission; however, a significant contribution from [Ru(dmbipy)3] complex emission can also be found. The observations show that the S1 and MLCT1 states are rather close in energy, supporting the hypothesis of thermally equilibrated excited MLCT1 and porphyrin singlet states. Selective perturbation of the energies of those excited states was carried out by coordinating an imidazole ligand to the zinc porphyrin center. As a result, the zinc porphyrin bands shifted from 450 (Soret), 570 and 614 nm to 457, 575 and 625 nm. Because of the lowering the energy of the corresponding excited state, the emission spectra of that supermolecule exhibit essentially a zinc porphyrin like pattern, when excited at both wavelengths 500 and 570 nm. Therefore, even such small energy decrease (290 cm_1) in the S1 state, has been enough to drive the energy transfer from the excited peripheral ruthenium complexes to the central zinc porphyrin moiety. This antenna effect has been confirmed by the excitation spectrum, which reproduced the zinc porphyrin and ruthenium complexes absorption bands.

 

9. Singlet Oxygen Generation and DNA Photocleavage

An important application of photosensitizing compounds is based on their ability to promote photoinduced damage to biological molecules including lipids, proteins and DNA, allowing the eradication of early localized tumors by the use of light. This type of medical treatment is known as photodynamic therapy (PDT). The sensitizing properties of various molecules, such as methylene blue, transition metal polypyridines and porphyrins have been extensively investigated in the last decades, aiming the development of efficient PDT drugs, imparting minima medical problems.86-97 It is well established that the activity of such drugs is closely related to their ability to interact with cellular membranes and macromolecules, such as double-stranded DNA. For this reason, the interaction between the photosensitizing agents and DNA represents a relevant issue for investigation.

Recent work from our laboratories has focused on the plasmid pBR322 and DNA interactions with a free-base tetraruthenated porphyrin species (TRP), revealing the occurrence of light induced single-strand breaks and 8-oxo-7,8-dihydro-2'-deoxyguanosine formation in the presence of molecular oxygen.86 The special sensitizer employed combines the remarkable redox and photochemical/photophysical properties of the porphyrins and ruthenium(II)-polypyridine compounds, in addition to their ability to strongly bind DNA via intercalation and outside association.87-91 Analogously to its molecular components, the TRP species exhibits a potential usefulness in photodynamic therapy (PDT) applications.92,93 From the supramolecular point of view, the peripheral ruthenium-polypyridine groups interact with the porphyrin center, promoting energy and electron transfer processes, and enhancing the photodynamic properties of the molecule.71

Two types of mechanisms have been associated with the photosensitized reactions involving DNA.94 The so called type I mechanism involves direct electron transfer or hydrogen abstraction of the 2'-deoxyguanosine (dGuo) bases by the excited sensitizer, while type II proceeds via their reaction with singlet oxygen, O2(1Dg), yielding 8-oxo-2'-deoxyguanosine (8-oxodGuo) and 4-hydroxy-8-oxo-4,8-dihydro-2'-deoxyguanosine. Recently, the photodynamic properties of TRP and its zinc metallated derivative, ZnTRP (Figure 4), have been evaluated95 in comparison with methylene blue and riboflavin, using 2'-deoxyguanosine as a model compound.96,97 Riboflavin is a characteristic type I photosensitizer, while methylene blue exhibits a type II behavior. The selectivity measured by the ratio of the amount of photoproducts generated by type II/type I mechanisms was 0.4 for riboflavin, and 2.3, 3.6 and 5.6 for TRP, methylene blue and ZnTRP, respectively, showing that ZnTRP is the most specific type II photosensitizer of the series.

The binding of ZnTRP to CT-DNA has been monitored from the corresponding DNA-induced changes on the uv-vis absorption and luminescence spectra in aqueous solution. The addition of increasing amounts of DNA (in the range of 0 to 17.9 mmol L-1) to the ZnTRP solution leads, initially, to a pronounced hypochromic effect on the Soret band at 426 nm (Figure 13). However, at higher concentrations of DNA the Soret band shifts to 438 nm and a systematic increase of the absorption is observed, evidencing a change in the interaction mode between those species. The binding constants for the low and high DNA concentration ranges, K1 = 5.0 x 107 and K2 = 1.0 x 105 mol  L-1 , respectively, can be compared with those found86 for TRP (K1 = 2.5 x 104 and K2 = 1.5 x 105 mol L-1). A stronger electrostatic interaction of ZnTRP with the DNA chain in the low DNA concentration range (Figure 2) is evidenced with respect to the TRP analogue.

 

 

The luminescence spectrum of ZnTRP exhibits a strong emission band at 621 nm and a side band at 660 nm assigned to the Q0-0 and Q0-1 porphyrin transitions, respectively, as shown in Figure 14. In the low DNA concentration range, e.g. below 15 mmol  L-1, the luminescence intensity at 621 nm decreases systematically to about 1/3 of the initial value and the resulting spectral profile becomes very broad. This type of behavior differs from that previously reported for the TRP-DNA system,86 in which case, only a systematic increase in the luminescence has been detected.

 

 

Presumably, the presence of the metal ion can play an important role, by promoting strong electrostatic interactions of the phosphate residues with the cationic ZnTRP species, in addition to their possible coordination to the Zn center. This would explain the observed increase in the electrostatic binding constant.

In the high DNA concentration range (up to 255 mmol  L-1), a systematic increase of the luminescence emission at 630 nm has been observed. This process is accompanied by an inversion in the spectral pattern, making the 660 nm band more intense. The luminescence spectra are coherent with the observed changes in the uv-vis spectra as a function of the DNA concentration, confirming the occurrence of two distinct binding modes in the ZnTRP - DNA system. This type of behavior has also been reported for a number of systems89,91 and interpreted in terms of a switch from electrostatic to intercalation mode as the concentration of DNA increases.

2'-Deoxyguanosine (dGuo) is the critical DNA target component in both type I and II photosensitization mechanisms, consisting in a good model compound for understanding the photoinduced oxidation of DNA. Type I mechanism is known to convert dGuo into oxazolone and imidazolone products through a mechanism that involves an electron transfer from the excited photosensitizer to DNA. Type II mechanism involves energy transfer from the excited sensitizer to dioxygen, yielding O2(1Dg) reactive species which convert dGuo into the oxidation products 8-oxodGuo and 4-hydroxy-8-oxo-4,8-dihydro-2'-deoxyguanosine.96-98 From the quantification of the different oxidation products, O2(1Dg) species has been postulated as the reactive species in dGuo photooxidation mechanisms mediated by the tetraruthenated porphyrins.96

Direct evidence of the formation of O2(1Dg) in photoexcitation of ZnTRP in air saturated acetonitrile solutions, has been obtained from its characteristic phosphorescence emission decay at 1270 nm98 (Figure 15). The calculated life time was t=(8.0±0.1) x 10_5 s. The efficiency of ZnTRP as a photosensitizer in the photooxidation of DNA has been investigated by monitoring the formation of 8-oxodGuo residues as a function of time and ZnTRP concentration. The amount of 8-oxodGuo increases linearly with the concentration of ZnTRP, when the time of exposure and irradiation intensity were kept constant, as expected for a photooxidation process promoted by the porphyrin sensitizer. The amount of 8-oxodGuo residues formed as a function of the irradiation time follows a single exponential behavior, (k = 0.019±0.005 min-1) and the following scheme has been proposed:

 

 

Photooxidation kinetics carried out using dGuo instead of CT-DNA have resulted in similar rate constant (0.018 min-1), confirming that deoxyguanosine is the preferential target for O2 (1Dg).

 

10. Oxidative Catalysis and Cytochrome P-450 Activity

Manganese and iron porphyrins have been extensively studied as models of cytochrome P-450 because they act as good oxygen atom transfer catalysts.99,100 The active species consist of high-valence metal-oxo porphyrins, which are very reactive and sensitive to substituent effects at the meso-aryl and b-pyrrol carbon atoms. The binding of selected metal complexes101-103 such as the trinuclear m3-oxo-ruthenium acetate clusters24,104-110 to the periphery of the metalloporphyrin ring provides an interesting strategy111 to improve the activity of the porphyrin catalyst, as in the MnTCP species112 (Figure 16), as a consequence of their electron withdrawing/donor and/or electron transfer properties, or by acting as cofactors, or by creating new pathways for the oxidation of organic substrates.

 

 

The catalytic activity of the supramolecular MnTCP and of the porphyrin species MnTPyP has been compared in the epoxidation of cyclooctene by iodosylbenzene in acetonitrile.112 Both compounds seem to catalyze efficiently and selectively the epoxidation of this substrate. However, in the oxidation of cyclohexane, a less reactive substrate, the results have been remarkably different. MnTPyP leads to the formation of cyclohexanone (13%) and cyclohexanol (27%) in about 1:2 molar ratio, but MnTCP generates exclusively cyclohexanol (45%) keeping the same total yield.

In this type of system, high-valent metal-oxo porphyrins such as O=MnVP have been proposed as the active species.99,100 Such species are very reactive and can not be detected under the conditions employed for catalysis. Its existence has been evidenced by Groves and Jin113 in a stopped-flow reaction of MnIIIT(4-MPyP) with chloroperoxybenzoic acid in aqueous solution. In this case, the formation of the O=MnVT(4-MPyP) species was found to be complete after 30 ms, and is followed by a slower first-order reaction which leads to the formation of the less reactive O=MnIVT(4-MPyP) species. More recently, a stable O=MnVT(2-MPyP) was characterized by 1H-NMR spectroscopy.114

The efficiency and high selectivity of MnTCP is consistent with the involvement of O=MnVTCP as catalyst rather than O=MnIVTCP. In fact, the related O=MnIVT(4-MPyP) species has been reported to be much less reactive than O=MnVT(4-MPyP) leading to reactions involving radical species, presumably responsible for the formation of cyclohexanone. Attempts to detect the O=MnVTCP species have been carried out by rapidly mixing MnTCP and iodosylbenzene solutions using a suitable flow-cell device, and measuring the UV-Vis spectra with a diode-array spectrophotometer. The final spectrum, however, corresponds to the O=MnIVTCP species,115,116 containing a mixture of RuIIIRuIIIRuIV/RuIIIRu IIIRuIII redox states (E0 = 1.17 V). From this observation, the redox potential O=MnVTCP species should be higher than 1.17 V and all peripheral clusters should be in the RuIVRuIIIRuIII form.

 

11. Electric Conductivity, Rectifying Effects and Photoaction Response of Supramolecular Films

An interesting supramolecular species (here denoted TRPz = tetraruthenated porphyrazine) is constituted by the free-base (3,4-pyridyl)porphyrazine coordinated to four peripheral [Ru(bipy)2Cl]+ groups71 (Figure 17). In this system, the pyridyl groups are fused to the macrocycle ring, in contrast with the related meso-tetra(4-pyridyl)porphyrins,117 TPyP, allowing a strong electronic interaction between the central and peripheral complexes, as reflected in an efficient antenna effect .

 

 

A typical electronic spectrum of the TRPz species in ethanol can be seen in Figure 18. The deconvoluted spectrum based on bigaussian functions exhibits the porphyrazine bands at 380 (B0-1), 406 (B0-0), 594 (Qy0-1), 638 (Qx0-1), 677 (Qy0-0) and 708 nm (Qx0-0). The remaining bands at 294, 344, 436 and 498 nm are attributed to the bipy (ppp*) and RuII (dp)®bipy(pp2*), RuII (dp)®py(pp*), and RuII(dp)®bipy(pp1* ), MLCT transitions, respectively.

 

 

The emission spectrum of the TRPz species is characterized by the porphyrazine luminescence, at 720 nm (Figure 18), while the excitation profile practically coincides with the absorption spectra, reproducing even the MLCT band at 500 nm, of the peripheral ruthenium complexes. Such coincidence corroborates the occurrence of efficient energy transfer processes from the ruthenium complexes to the porphyrazine center, in contrast to the related supramolecular tetrapyridyl derivatives.

Analogously to the supramolecular TPyP systems, the tetraruthenated porphyrazine species also form very homogeneous molecular films onto solid surfaces, by the slow evaporation of the solvent (e.g. methanol). Such films are suitable for the preparation of modified electrodes, displaying versatile electrochemical and photoelectrochemical properties. Another strategy is provided by the controlled electrostatic/stacking assembly of cationic TRPz and suitable anionic species, such as the tetrasulfonatephthalocyaninatecopper(II) complex, CuTSPc, yielding the corresponding TRPz/CuTSPc double layered films66,118 as illustrated in Figure 19. Both films exhibit electron hopping conductivity at the onset of the film oxidation wave; however, a remarkable aspect of the stacked ion pair film is the occurrence of an additional, fast electron transfer mechanism. This finding was associated with electronic conduction through the films, arising from the formation of porphyrazine/phthalocyanine columnar stacks with extended p interaction.

The spectrum of a TRPz film on ITO is analogous to the solution spectrum exhibiting the Soret band at 390 and a broad Q band at 705 nm, respectively; and the peripheral ruthenium complexes p-p* and charge transfer bands at 300 and 500 nm. When a TRPz solution in dimethylsulfoxide is titrated with CuTSPc in the same solvent, the Q band at 710 nm of TRPz decreases indicating stacked ion-pairing in solution. The plot of the absorbance at 710 nm as a function of the mole fraction of the interacting species shows a sharp end point at 1:1 mole ratio, as expected for a relatively strong interaction between those species. Suitable films of the TRPz/CuTSPC stacked ion-pairs have been generated in a controlled way, by alternating a dip-coating step, starting from methanolic TRPz followed by air drying, and another dip-coating step with aqueous CuTSPc, and rinsing with water. The films are similar to those obtained by mixing m-meso-tetra(4-pyridyl)porphyrin{tetrakis-chloro(bis -bipyridine)ruthenium(II)} and meso-tetrasulfonatophenylporphyrins,119 however a contrasting aspect in the case of TRPz/CuTSPc films is that the electronic spectra of the two components are strongly affected, exhibiting a hypochromic shift and broadening of the Q band, as a consequence of the extended p interaction throughout of the stacked TRPz/TSPc films.

Cyclic voltammetry of the TRPz species in solution exhibits four redox processes in the -1.6 to 1.2 range, as shown in Figure 20, ascribed to the RuIII/II redox pair at E1/2 = 0.94 V, and to the first and second reduction of the porphyrazine center at -0.63 and -0.99 V, followed by the bipy0/- couple around -1.5 V. However, based on spectroelectrochemical measurements for the TRPz species in solution (Figure 21), it has been shown that this wave is actually composite, involving the RuIII/II redox pair, preceded by the oxidation of the porphyrazine center, around 0.7 V.

 

 

 

 

The cyclic voltammograms of glassy carbon electrodes modified with TRPz alone or TRPz/CuTSPc layered films exhibit a pair of bell shaped waves at 0.9 V, in LiTFMS aqueous solution (Figure 22). The peak currents increase linearly as a function of the scan rate, as expected for an electroactive species immobilized on the electrode surface. Cyclic voltammetry has been carried out in the presence of penta- and hexacyanoferrate complexes in order to probe the homogeneity and conductivity of the TRPz and TRPz/CuTSPc films, as shown in Figure 21. When the potentials are scanned from 0.40 V to 1.2 V in the presence of [FeII(CN)6] and [FeII(CN)5(NH3)] complexes, no electrochemical response is observed at their normal redox potentials, i.e., 0.42 and 0.33 V, respectively. However, a rather a sharp and intense anodic peak appears at the onset of the broad oxidation wave, around 0.70 V. The current intensity of this electrochemical process is proportional to the square root of the scan rate, as expected for a diffusion controlled oxidation reaction at the modified electrode surface. The results are consistent with an electrochemical process mediated by the porphyrazine film, which act as a physical barrier for the approach of the cyanoferrate complexes from the glassy carbon electrode surface.

 

 

Since the modified films act as insulators below 0.70 V, there is no response when the redox potentials of the reduced species in solution are lower than this value. When this limiting potential is reached, the film becomes conducting via RuIII/II electron hopping, and the reduced species can be rapidly oxidized, leading to a sharp, unidirectional, electrochemical response. In this case, an electric rectifier response is observed.120 It is interesting to note that when the redox potentials of the reduced species match the limit conducting values, e. g. Eo > 0.70 V, the electric conduction becomes bidirectional, approaching a reversible type of electrochemical response. This expectation has been confirmed by using the (N-methylpyrazinium)pentacyanoferrate complex (E1/2 = 0.75 V vs SHE), as shown in Figure 22.

In the impedance spectroscopy measurements for the TRPz/CuTSPc films, at 0.6 V, the beginning of a semi-circle is observed in the high-frequency region, followed by a very short diffusion controlled region and finally saturation (Figure 23). This kind of response can be associated with a Randles type circuit modified with a low frequency capacitor. This is evidence that the electrons are moving mainly by hopping mechanism and that the limiting step is the electron transfer rate from one redox site to the next one. However, at 0.95 V, instead of one semicircle, the spectrum exhibited two, which can be associated with a capacitive and an inductive contribution at high frequencies. After these two kinetic controlled regions the system reaches a saturation regime, as can be seem by the almost vertical straight line in the low frequency region. The most important feature observed in that spectrum is the appearance of a second kinetic controlled region. The presence of capacitive and inductive components has been explained by considering that the electrons are moving in two different directions through the film and by distinct mechanisms. The fact that the film is constituted by strongly p interacting, stacked porphyrazine and phthalocyanine species, facilitates the formation of columnar structures oriented perpendiculary to the electrode surface. According to spectroelectrochemistry, the stacks are being oxidized near the onset of the insulator/conductor switching potential. These are characteristics of porphyrin molecular wires that have been long studied by Ibers and co-workers121-123 The two kinetic controlled processes have been associated with an electron transfer from the peripheral ruthenium complexes to the central p stack and then through the stack until reaching the electrode surface.

 

 

The modified electrodes of TRPz/CuTSPc films exhibited photoelectrochemical response in O2 saturated aqueous solution.118 The electrodes modified with bilayer films are active below -0.05 V generating a reproducible photoelectrochemical response at -0.4 V bias. The photoaction spectrum exhibits a broad band centered at 700 nm and a shoulder at 500, consistent with the Q and MLCT bands envelope. Its similarity with the absorption spectrum is a clear indication that the porphyrazine bilayer material is responsible for the observed photoelectrochemical activity. In fact, the electrodes modified with bilayer films are much more efficient, probably because of the faster electron transfer from the electrode to the film/solution interface. Presumably, the photocurrent response should be generated when the excited supramolecular system transfers electrons, reducing O2 to H2O2 or H2O and generating ruthenium(III) complexes, which are able to dope the -stacked system increasing its conductivity and enhancing its photoaction response.

 

12. Multielectron Transfer Catalysis by Supramolecular Films of Tetracluster-Cobaltporphyrins

The tetraelectronic reduction of O2 to water is a fundamental process carried out by the aerobic organisms, during the mitochondrial energy generation cycle. In general, the dioxygen reduction can proceed by bi- or tetraelectronic mechanisms, but the first one is by far more common. Typical cobalt porphyrins usually catalyze the dioxygen reduction yielding hydrogen peroxide instead to water.124 Outstanding research in this area has been carried out by Anson and co-workers along the last twenty years.125-127 Collman and co-workers128-131 have shown that the simultaneous interaction of the O2 molecule with two CoP centers is involved in the activation by a cofacial bis-cobaltporphyrin. However, more recently, they found out that the change of the electrode material from pyrolytic graphite to gold can switch the mechanism from tetraelectronic to bielectronic.131 Anson and co-workers,124-126,132-135 have studied cobalt meso-tetra(pyridyl) and meso-tetra(4-cyanophenyl) porphyrins bound to [Ru(NH3)5]2+ or [Os(NH3)5]2+ ions, showing that the back-bonding from the ruthenium(II) and osmium(II) complexes plays an important role in the activation of the cobalt porphyrin center.136 On the other hand, they also showed that the [Ru(NH3)5]2+ modified cobalt porphyrin becomes a bielectronic catalyst137 when in solution, revealing the importance of the electrode material or the arrangement of the molecules in the reaction pathway. Recently, however, a surprising efficiency has been reported for a rather simple molecule, such as the (5,10,15,20-tetramethylporphyrinato)cobalt(II) species.138

Previously, we have shown that the coordination of four [Ru(edta)]_ complexes to iron and cobalt meso-tetra(pyridyl)porphyrins enhances their catalytic activity toward O2 reduction in aqueous solution.102,103 This enhancement has been ascribed to the regeneration of the active CoIIP species by electron transfer from the reduced [RuII(edta)]2_ complexes. However, the cobalt porphyrin remained a bielectronic catalyst. Along this line, a highly efficient, tetraelectronic catalyst based on a supramolecular meso-tetra(4-pyridyl)porphynato cobalto(III) complex containing four [Ru3O(CH3COO)6(py)2] + clusters coordinated to the pyridyl substituents, CoTCP (Figure 16, M = Co) has been recently reported.139

The CoTCP supermolecule exhibits a characteristic electronic spectrum (Figure 25) composed by the characteristic porphyrin Soret and Q bands at 435, and 557, 611 nm, respectively; and the ruthenium clusters bands at 318 and 693 nm.

 

 

 

 

This supramolecular species forms stable films by dip coating, onto glassy carbon electrodes, exhibiting a reversible redox couple at E1/2 = 0.22 V in aqueous solution (Figure 26). The adherence and durability of the modified electrodes are noteworthy. Typical surface concentration of 3.9x10_10 mol cm2 has been obtained from coulometric measurements, being consistent with a multilayered film.

 

 

The spectrum of a film of CoTCP deposited onto a glassy carbon electrode surface is very similar to that of the molecular species in acetonitrile solution, but the Soret and Q bands are shifted respectively to 440, 555 and 610 nm, and the intracluster band to 705 nm. In comparison with the spectra of the films of supramolecular porphyrin coordinated to [Ru(bipy)2Cl]+ complexes,66,120,140 the CoTCP film spectrum is much less broadened. This is an evidence that in the films the cobalt porphyrin rings are too far to interact with each other, due to the bulkiness of the peripheral [Ru3O(OAc)6(py)2]+ groups.

According to the spectroelectrochemistry measurements (Figure 27), there is an inversion in the potential order of the cluster (RuIIIRuIIIRuIII/RuIIIRu IIIRuII) and cobalt porphyrin (CoIII/IIP) redox processes, in comparison with the spectroelectrochemistry in acetonitrile solution. The inversion has been ascribed to the axial ligand exchange, when the solvent is changed from ACN to water.141 In this system, the E0 values estimated using the spectroelectrochemistry data are 0.21 and 0.07 V for the RuIIIRuIIIRuIII/ RuIIIRuIIIRuII and CoIII/IIP redox pairs, respectively.

 

 

The cyclic voltammograms of O2 saturated aqueous solution, using a bare glassy carbon electrode exhibit a slow increase in the cathodic current below -0.0 V. In contrast, sharp and intense cathodic peaks around 0.2 V have been observed in the cyclic voltammograms of CoTCP modified glassy carbon electrodes, as shown in Figure 28. The catalytic wave is much more intense than the wave associated with the RuIIIRuIIIRuIII/ RuIIIRuIIIRuII and CoIII/IIP redox pairs. The current intensities match the calculated peak currents for the reduction of the dioxygen to water (n=4). In order to clarify the role of the ruthenium clusters on the catalytic activity, experiments with electrodes modified with ZnTCP, a zinc porphyrin derivative that lacks the cobalt porphyrin site, have been carried out in the same conditions. In this case the enhancement of the cathodic current in the 0.3 to -0.0 V range is rather small, approaching the bare glassy carbon electrode response.

 

 

Rotating disc voltammograms recorded from 100 to 3000 rpm are shown in Figure 29. All of them have a typical sigmoid shaped profile characteristic of a reversible electrochemical process. The Levich and Koutecky/Levich plots are linear up to 4000 rpm and pass through the origin within experimental error. These are good evidence that the reaction rate is not limited by mass transport or electron diffusion through the film. In other words, the reduction proceeds as rapidly as the O2 molecules reach the film as can be inferred by the smooth current decay after the catalytic wave on the CV's and the flat plateau on the RDE voltammograms. The high current density (2.8 mA/cm2 at 4000 rpm) achieved at the CoTCP modified electrodes is a good indication of the high efficiency of the catalytic reaction. Rotating ring disc electrochemical experiments carried under the same experimental conditions have also been performed. No significant ring current has been measured, confirming the tetraelectronic reduction of the O2 molecules.

 

 

14. Electropolymerized Films of Tetraruthenated Porphyrins as New Functional Electrochemical Materials

By means of electropolymerization,142-148 molecular films can be deposited just on the polarized electrode surface, allowing to control the amount of deposited material.149-151 These characteristics can be very conveniently exploited for the preparation of arrays of modified electrodes. The strategy based on the electropolymerization of halogen substituted aromatic compounds has already been reported in the case of the reductive dimerization of 5-chlorophenanthroline (5-ClPhen) by Fussarydel et al.152 Following this approach, the corresponding porphyrin supermolecular species by attaching four [Ru(5-ClPhen)2Cl]+ groups to the pyridine N-atoms of H2(TPyP) have also been developed. Such species have been called ETRP (electropolymerizable tetraruthenated porphyrins).153

The UV-Vis spectra of H2(ETRP) in methanol exhibits the characteristic porphyrin peaks at 419 nm, and the Q bands at 513, 552, 588 and 648 nm, in addition to an intense and narrow band at 295 nm and a broad band at 450 nm, ascribed to the 5-Clphen p-p* intraligand and RuII(dp)®5-Clphen (pp*) MLCT transitions, respectively.

Four waves have been observed in the cyclic voltammograms of the supramolecular porphyrin species in DMF solution. The reversible waves at E1/2 = 1.00 and -0.65V have been assigned to the Ru(III/II) redox pair and to the monoelectronic reduction of the porphyrin ring to the p-radical anion, respectively, while a shoulder at Epc = -1.04 V corresponds to the formation of the respective porphyrin dianion. The monoelectronic reduction of a 5-Clphen ligand of each peripheral ruthenium complexes occurrs at Epc = -1.11 V, as inferred by the higher current intensity and potential range of this wave. Its anodic wave seems to be broader, more intense and shifted to positive potentials because of the overlap with the anodic wave corresponding to the reoxidation of the porphyrin dianion.

A typical series of successive voltammograms in DMF (-1.3 to 1.2 V range) using platinum disk electrodes are shown in Figure 31. The stepwise increase of the Ru(III/II) wave current as a function of the number of successive scans, reflect the electropolymerization process.149,154,155 It leads to a film resistant to washing with DMF and acetonitrile.

 

 

 

 

The reduction of the 5-ClPhen ligand induces the elimination of the phenanthroline chloro group as chloride anion and the formation of a radical species152 which reacts promptly with another radical, forming a dimer in the case of the free ligand. The H2(ETRP) species has two of such ligand for each of the four peripheral ruthenium complexes. Consequently, just two of the eight 5-ClPhen ligands present in the porphyrin supermolecule are enough to form intramolecular C-C bonds by this process, in order to generate a polymer. In fact, it has been observed that H2(ETRP) can be directly electropolymerized from a DMF solution, but the deposition process is sluggish and the resultant films are rather unstable, due to the looseness of the polymeric chains in the structure.

Considering that the new supermolecular porphyrin is able to form quite homogeneous films by dip-coating25,66,140,156 and that such films are poorly soluble in acetonitrile, a new procedure has been devised by carrying out the electropolymerization reaction on the preformed films, instead of from the molecular species in solution.153 The advantage is the high concentration of the monomer in the electrode surface and orientation of the monomer molecules, leading to a more compact and highly reticulated structure. Such aspects increase the efficiency of the electropolymerization process, since only one or two scans in the 0.0 V to -1.3 range are enough to promote the completion of the electropolymerization reaction. Another advantage of this process is that it requires only a minimum amount of the monomer, in contrast with the conventional electrodeposition procedure from a concentrated solution.

A typical bell shaped voltammogram of a platinum electrode modified with a thin polymeric H2(ETRP) film in acetonitrile electrolyte solution is shown in Figure 31.B. The films deposited onto ITO by dip-coating solution has been examined by AFM microscopy, before and after the electropolymerization procedure. The AFM images (Figure 32) reveal that the dip-coated samples surface are formed by aggregates more or less uniformly distributed onto the ITO surface, while the electropolymerized films exhibit broad and regularly distributed features, reflecting the occurrence of structural changes and molecular reorganization, as depicted in Figure 33.

 

 

 

 

The conduction properties of the electropolymerized supermolecular porphyrin films (0.65 to 1.25 V range) have been probed by impedance spectroscopy. The Nyquist plots of the data obtained at different equilibrium potentials for G = 4 x 10-9 mol cm-2 show that the impedance of the films is very high at potentials far from the E1/2 of the Ru(III/II) redox pair. Only the activation controlled region (a fraction of a semicircle) is visible in that diagram. But, the charge transfer resistance decreases sharply as the applied potential approaches the Ru(III/II) redox potential, defining the activation controlled, diffusion controlled and saturation regions characteristic of electrodes modified with thin electroactive films.157 When the potential is increased further, the impedance increases again, such that the profile of the conductance vs potential plot reasonably matches the voltammetric wave profile. This behavior is typically explained by assuming a redox conduction mechanism.155,158 When the peripheral ruthenium complexes are totally reduced or oxidized, e.g. at 0.65 and 1.25 V, the charge transfer impedance is high because of the low concentration of charge carriers. It reaches the minimum at the E1/2 when the concentration of the oxidized and the reduced species are equal.

The high background impedance of the electropolymerized porphyrin films contrasts with the relatively high intrinsic conductivity observed for the electrostatic assembled Co(TRPyP)/Zn(TPPS) bilayer films.159 In this case, a quite low electric resistance (about a kW) has been observed, becoming very low close to the E1/2 of the Ru(III/II) redox pair. This difference arises from distinct molecular organization in those materials. In the case of the electrostatic assembled films, the porphyrin rings are forming stacks in which there is a considerable interaction between the extended p-clouds of that macrocycle, which should be responsible for the relatively high intrinsic conductivity. On the other hand, the C-C bonds in the electropolymerized porphyrin films make the stacking of the porphyrin rings termodynamically unfavorable because of the angular tension. Consequently, the porphyrin rings are more randomly oriented in this material and there is less p-p interaction between them, but the peripheral ruthenium complexes are sufficiently close to touch each other, allowing the occurrence of a fast and efficient electron hopping processes.

 

15. Amperometric Sensors

Sulfur dioxide and its source compounds, such as the sulfite salts, are widely used as preservatives in food industry. They are added to foods and beverages in order to inhibit bacterial growth, to prevent oxidation and inhibit discoloration, improving the final appearance of the products.160-162 In wine, sulfur dioxide is usually found either bound to unsaturated compounds and phenolic constituents, or as HSO3-, SO32- and SO2. Only SO2 exhibits antiseptic properties.163,164 In spite of its relevance, the control of its amounts in wine is essential, because at high levels it produces a disagreeable aroma and taste, besides of being hazardous to human health. The maximum allowed levels of SO2 in wines are regulated by each country's legislation. In Brazil, for instance, the addition of 50 and 200 ppm of free and bound SO2, respectively, is considered acceptable.165

In general, iodometric methods are preferred in industry for the determination of SO2. The results should be interpreted with caution because of the poor stability of the solutions and of the difficulties associated with the end point determination, particularly in the case of the red wines. Flow injection analysis (FIA) is becoming increasingly important in quality control because of its high sampling rate and simplicity, among other interesting features. Most of the FIA methods make use of a gas-diffusion cell to separate the sulfur dioxide released from the matrix compounds, through a semi-permeable membrane. The analyte can be determined with an optical detector, by monitoring its reaction with formaldehyde and p-rosaniline, in acidic solutions,166,167 or with electrochemical sensors.168,169.

Chemically modified electrodes constitute very attractive amperometric detectors for FIA, allowing the exploitation of the properties of the immobilized species and films. Recently, we reported a successful application of modified electrodes containing molecular films of tetraruthenated porphyrins, in flow injection analysis of NADH, dopamine, nitrite and sulfite ions.170,171 In those cases, in spite of the good performance of the modified electrodes as electrochemical detectors, a high concentration of trifluoromethanesulfonate or perchlorate counter ions is required to decrease the solubility and prevent the gradual leaching of the tetraruthenated porphyrins from the surface. This problem has been minimized by using electrodes modified with an alternating layers of cationic and anionic porphyrin films.172 The performance of this second generation of electrodes has been investigated in the analysis of free and total sulfur dioxide in wine, using a home made diffusion cell on line with the FIA amperometric detector. The gas diffusion cell is necessary for the transference of the gaseous compounds from the donor stream to the acceptor one, through a semipermeable membrane. For the build up of the amperometric detector, a glassy carbon electrode has been modified with alternating layers of CoTRP/ZnTPPS films.

It should be mentioned that the detection of sulfite ions using conventional electrodes is usually complicated by a high overpotential and a poor electrochemical response. We have shown that CoTRP modified electrodes provide a considerable enhancement of the sulphite response and decrease of the overpotential. As a consequence of the electrocatalytical properties of the modified electrodes, the oxidation wave was cathodically shifted, approaching the RuII/III redox couple potential (+0.70 V vs saturated Ag/AgClKCl). A similar behavior has been observed for the electrostatically assembled CoTRP/ZnTPPS films.140

Different types of wines (dry white, dry red and sweet white) have been analysed, including a home made red wine containing any preservative. The lack of detectable signal in this case indicates that the present analytical method is very reliable, excluding any interference from the natural constituents of wine. The agreement between the iodometric and FIA methods is quite good. However, the use of chemical sensors can be easily scaled up to a large number of samples and has all the advantages of the FIA methods. This is in contrast with the tedious and time consuming titration procedures.

Nitrite ion is another interesting analytical substrate because of its prevalence in industrialized meats as preserving agent and appearance builder. But, when ingested it can react with hemoglobin oxidizing it to metahemoglobin, and with amines converting them to nitrosamines, which are well-known carcinogenic substances.173,174 The environmental impact caused by the build-up of high nitrite and nitrate concentrations, owing to their use as fertilizers, and the problems caused by the contamination of water sources for human consumption are also big concerns.175

The capacity of being electropolymerized makes the H2(ETRP) films rather interesting for that kind of application, specially for the preparation of microelectrode arrays, and because of their expected higher stability. A linear increase of the anodic current around 1 V has been observed in the cyclic voltammograms, as the concentration of nitrite was increased from 1x10_4 to 8x10_3 mol L-1 , suggesting a quite a high activity, in spite of the higher electric impedance of the film. Consequently the oxidation of nitrite to nitrate is being mediated by the Ru(III) species electrochemically generated at the film.40,159,162,176 The kinetics of the mediated oxidation reaction of nitrite to nitrate has been studied by RDE voltammetry in the 200 to 8000 rpm rotation range, and 1x10_5 to 1x10_3 mol L-1 concentration range. The voltammograms exhibit a typical sigmoidal shaped profile characteristic of quite a rapid mediated reaction. The Levich plots presents a small but increasing curvature as the concentration of the substrate is increased at higher rotation rates. This is a clear indication that at these high mass transport conditions the current is no longer limited only by diffusion, but also by the kinetic of the heterogeneous electron transfer at the electrode surface. Accordingly, the corresponding rate constant has been obtained from the linear coefficients of the Koutech-Levich plots as kf = 3.7 x 104 mol L-1  s_1 That value is one order of magnitude higher than that previously obtained150,176 for the Co(TRP)/Zn(TPPS) electrostatic assembled bilayer films, suggesting that the new material can be even more active than the previously studied materials.

Another important application of the nanostructured films of the supramolecular porphyrins is in the determination of acetaminophen in pharmaceutical formulations. This work has been recently performed177 by means of batch injection analysis (BIA) utilizing amperometric detection with glassy carbon electrodes modified with [Co(TPyP){Ru(bipy)2Cl}4]5+ triflate films.

In fact, BIA is an interesting alternative for application of electrodes modified with tetraruthenated porphyrins. This sensor exhibits sharp current response peaks, rapid washout and excellent reproducibility for BIA-amperometric quantification of acetaminophen. Also, a wide linear working range (10-4 to 10-6 mol L-1) as well as high sensibility and sampling frequency rate (detection limit = 1.1 x 10-7 mol L-1, sampling frequency = 120 injections/h); and a small volume of analysis (100 mL/injection) has been achieved. The proposed method177 permits the direct and selective quantification of acetaminophen in many pharmaceutical products, avoiding cumbersome processes as previous separations, solvent extraction or sample filtration. Such new procedure has been applied to the analysis of commercial pharmaceutical products and the results were in excellent agreement with the ones obtained by standard spectrophotometric method.

 

16. Conclusion

By exploiting the strategies of coordination chemistry, versatile functional nanomaterials can be designed, conveying the remarkable characteristics of the metal centers, such as their electronic, optical and chemical properties, as well as all the characteristics of the ancillary ligands. Coordination chemistry also provides effective self-assembly strategies for molecular materials, based on specific metal-ligand affinity and stereochemistry. From the several molecular materials focused on this article, based on supramolecular porphyrins and porphyrazines, metal-clusters and metal-polyimine complexes, an exciting field of investigation has been presented, covering a wide range of applications in catalysis, sensors and molecular devices.

 

Acknowledgements

The support from FAPESP, CNPq, RENAMI and the "Instituto do Milênio de Materiais Complexos" is gratefully acknowledged.

 

References

1. Feynman, R. P.; Engineering Science 1960, 23, 22.        [ Links ]

2. Hipell, A.; The Molecular Designing of Materials and Devices, MIT Press: Cambridge, 1965, vol IV.        [ Links ]

3. Drexler, K.; Engines of Creation: Challenges and Choices of the Last Technological Revolution, Anchor Press: New York, 1986.        [ Links ]

4. Sheats, J. R.; Barbara, P. F.; Ac. Chem. Res. 1999, 32, 191.        [ Links ]

5. Lehn, J. M.; Supramolecular Chemistry, VCH: Weinheim, 1995.        [ Links ]

6. Atwood, J. R.; Davies, J. E. D; Macnicol, D. D.; Comprehensive Supramolecular Chemistry, Pergamon-Elsevier: New York, 1996.        [ Links ]

7. Toma, H. E.; Quim. Nova 1991, 14, 189;         [ Links ]Toma, H. E.; An. Acad. Brasil. Ci. 2000, 72, 1.        [ Links ]

8. Belanger, S.; Hupp, J. T.; Stern, C. L.; Stone, R. V.; Watson, D. F.; Carrell, T. G.; J. Am. Chem. Soc. 1999, 121, 557.        [ Links ]

9. Stoddart, J. F.; Acc. Chem. Res. 2001, 40, 2447.        [ Links ]

10. Balzani, V.; Credi, A.; Raymo, F. M.; Stoddart, J. F.; Angew. Chem., Int. Ed. 2000, 39, 3349.        [ Links ]

11. Cantrill, S. J.; Pease, A. R.; Stoddart, J. F.; J. Chem. Soc., Dalton 2000, 3715.        [ Links ]

12. Pease, A. R.; Stoddart, J. F.; Struc. Bond. 2001, 99, 189.        [ Links ]

13. Collier, C. P.; Jeppesen, J. O.; Luo, Y.; Perkins, J.; Wong, E. W.; Heath, R. J.; Stoddart, J.F.; J. Am. Chem. Soc, 2001, 123, 12632.        [ Links ]

14. Luo, Y.; Collier, C. P.; Jeppesen, J. O; Nielsen, K. A.; Delonno E.; Ho, G.; Perkins, J.; Tseng, H. R.; Yamamoto, T.; Stoddart, J. F.; Heath, J. R.; ChemPhysChem 2002, 3, 519.        [ Links ]

15. Balzani, V.; Credi, A.; Venturini, M.; Chem.-Eur. J. 2002, 8, 5524.        [ Links ]

16. Balzani, V. Credi.; Venturini, M.; Proc. Natl. Acad. Sci. USA 2002, 99, 4814.        [ Links ]

17. Whitesides, G. M.; Grzybowski, B.; Science 2002, 295, 2418.        [ Links ]

18. Whitesides, G. M.; Sci. Am. 2001, 285, 78.        [ Links ]

19. Lehn, J. M; Proc. Natl. Acad. Sci. USA 2002, 99, 4763;         [ Links ]Machado, V. G.; Baxter, P. N. W.; Lehn, J.-M.; J. Braz. Chem. Soc. 2001, 12, 431.        [ Links ]

20. Lehn, J. M.; Polym. Int. 2002, 51, 825.        [ Links ]

21. Schumaker, R. S.; US pat. 6,124,963, 2000.

22. Toma, H. E.; Araki, K.; Alexiou, A. D. P.; Nikolaou, S.; Dovidauskas, S.; Coord. Chem. Rev. 2001, 219, 187.        [ Links ]

23. Toma, H. E.; Araki, K.; Coord. Chem. Rev. 2000, 196, 307.        [ Links ]

24. Juris, A.; Balzani, V.; Barigelletti, F.; Campagna, S.; Belser, P.; Vonzelewsky, A.; Coord. Chem. Rev. 1988, 84, 85.        [ Links ]

25. Kalyanasundaram, K.; Photochemistry of Polypyridine and Porphyrin Complexes, Academic Press: London, 1992.        [ Links ]

26. Araki, K.; Toma, H. E.; Quim. Nova 2002, 25, 962.        [ Links ]

27. Ward, M. D.; Chem. Soc. Rev. 1995, 24, 121        [ Links ]

28. Fraysse, S.; Coudret, C.; Launay, J.-P.; Eur. J. Inorg. Chem. 2000, 1581.        [ Links ]

29. Masui, H.; Freda, A. L.; Zerner, M. C.; Lever, A. B. P.; Inorg. Chem. 2000, 39, 141.        [ Links ]

30. Hossain, M. D.; Ueno, R.; Haga, M.; Inorg. Chem. Commun. 2000, 3, 35.        [ Links ]

31. Chao, H.; Ye, B. H.; Zhang, Q. L.; Ji, L. N.; Inorg. Chem. Commun. 1999, 2, 338.        [ Links ]

32. Reimers, J. R.; Hush, N. S.; J. Phys. Chem. A 1999, 103, 3066.        [ Links ]

33. Ward, M. D.; Chem. Ind. 1997, 640.        [ Links ]

34. Neyhart, G. A.; Timpson, C. J.; Bates, W. D.; Meyer, T. J.; J. Am. Chem. Soc. 1996, 118, 3730.        [ Links ]

35. Neyhart, G. A.; Hupp, J. T.; Curtis, J. C.; Timpson, C. J.; Meyer, T. J.; J. Am. Chem. Soc. 1996, 118, 3724.        [ Links ]

36. Rocha, R. C.; Toma, H. E.; Inorg. Chem. Commun. 2001, 4, 230.        [ Links ]

37. Rocha, R. C.; Araki, K.; Toma, H. E.; Transition Met. Chem. 1998, 23, 13.        [ Links ]

38. Toma, H. E.; Giesbrecht, E.; Rojas, R. L. E.; Can. J. Chem. 1983, 61, 2520.        [ Links ]

39. Toma, H. E.; Giesbrecht, E.; Rojas, R. L. E.; J. Chem. Soc., Dalton 1985, 2469.        [ Links ]

40. Rocha, R. C.; Araki, K.; Toma, H. E.; Inorg. Chim. Acta 1999, 285, 197.        [ Links ]

41. Rocha, R. C.; Toma, H. E.; Inorg. Chim. Acta 2000, 310, 65.        [ Links ]

42. Rocha, R. C.; Toma, H. E.; Can. J. Chem. 2001, 79, 145.        [ Links ]

43. Robin, M. B.; Day, P.; Adv. Inorg. Chem. Radiochem. 1967, 10, 247.        [ Links ]

44. Haga, M. A.; Ali, M. M.; Koseki, S.; Fujimoto, K.; Yoshimura, K.; Nozaki, T.; Ohno, T.; Nakajima, K.; Stufkens, D. J.; Inorg. Chem. 1996, 35, 3335.        [ Links ]

45. Haga, M.; Ano, T.; Kano, K.; Yamabe, S.; Inorg. Chem. 1991, 30, 3843.        [ Links ]

46. Giuffrida, G.; Campagna, S.; Coord. Chem. Rev. 1994, 135, 517.        [ Links ]

47. Toma, H. E.; Chavez-Gil, T. E.; Inorg. Chim. Acta 1997, 257, 197.        [ Links ]

48. Toma, H. E.; Chavez-Gil, T. E.; Rocha, R. C.; Rechenberg, H. R.; J. Inclusion Phenom. 1999, 34, 57.        [ Links ]

49. Balzani, V.; Scandola, F.; Supramolecular Photochemistry, Harwood: West Sussex, 1991.        [ Links ]

50. Schlicke, B.; Belser, P.; Cola, L. De; Sabbioni, E.; Balzani, V; J. Am. Chem. Soc. 1999 121, 4207.        [ Links ]

51. Baudin, H. B.; Davidsson, J.; Serroni, S.; Juris, A.; Balzani, V.; Campagna, S.; Hammarstrom, L.; J. Phys. Chem. A 2002, 106, 4312.        [ Links ]

52. Vogtle, F.; Plevoets, M.; Nieger, M.; Azzellini, G. C.; Credi, A.; De Cola, L.; De Marchis, V.; Venturi, M.; Balzani, V.; J. Am. Chem. Soc. 1999, 121, 6290.        [ Links ]

53. Belser, P.; Bernhard, S.; Blum, C.; Beyeler, A.; Cola, L. De, Balzani, V.; Coord. Chem. Rev. 1999, 190, 155.        [ Links ]

54. Balzani, V.; Juris, A.; Coord. Chem. Rev. 2001, 211, 97.        [ Links ]

55. Barigelletti, F.; Flamigni, L.; Guardigli, M.; Juris, A.; Beley, M.; Chodorowski-Kimmes, S.; Collin, J.-P.; Sauvage, J.-P.; Inorg. Chem. 1996, 35, 136.        [ Links ]

56. Camera, S. G.; Toma, H. E.; J. Photochem. Photobiol. A 2002, 151, 57.        [ Links ]

57. Toma, H. E.; Lever, A. B. P; Inorg. Chem. 1986, 25, 176.        [ Links ]

58. Toma, H. E.; Alburn, P. A.; Dodsworth, E. S.; Golovin, M. N.; Lever, A. B. P.; Inorg. Chem. 1987, 26, 4257.        [ Links ]

59. Toma, H. E.; Santos, P. S.; Lever, A. B. P.; Inorg. Chem. 1988, 27, 3850.        [ Links ]

60. Berg-Brennan, C.; Subramanian, P.; Absi, M.; Stern, C.; Hupp, J. T.; Inorg. Chem., 1996, 35, 3719.        [ Links ]

61. Cola, L.; Belser, P.; Coord. Chem. Rev. 1998, 177, 301.        [ Links ]

62. Bergonzi, R.; Fabbrizzi, L.; Licchelli, M.; Mangano, C.; Coord. Chem. Rev. 1998, 170, 31.        [ Links ]

63. Indelli, M. T.; Scandola, F.; Collin, J. P.; Sauvage, J. P.; Inorg. Chem. 1996, 35, 303.        [ Links ]

64. Lee, J. D.; Vrana, L. M.; Bullock, E. R.; Brewer, K. J.; Inorg. Chem. 1998, 37, 3575.        [ Links ]

65. Indelli, M. T.; Bignozzi, C. A.; Harriman, A.; Schnoover, R. J.; Scandola, F.; J. Am. Chem. Soc. 1994, 116, 3768.        [ Links ]

66. Araki, K.; Toma, H. E.; J. Photochem. Photobiol. A 1994, 83, 245.        [ Links ]

67. Bensasson, R. V.; Land, E. J.; Moore, A. L.; Crouch, R. L.; Dirks, G.; Moore, T. A.; Gust, D.; Nature 1981, 290, 329.        [ Links ]

68. Bignozzi, C. A.; Argazzi, R.; Chiorboli, C.; Roffia, S.; Scandola, F.; Coord. Chem. Rev. 1991, 111, 261.        [ Links ]

69. Carbonera, D.; Valentin, M. Di; Agostini, G,; Giacometti, G.; Liddell, P. A.; Gust, D.; Moore, A. L.; Moore, T. A.; Appl. Magn. Reson. 1997, 13, 487.        [ Links ]

70. Plevoets, M.; Vogtle, F.; Cola, L. De; Balzani, V.; New J. Chem. 1999, 23, 63.        [ Links ]

71. Toyama, M. M.; Franco, M.; Catalani, L. H.; Araki, K.; Toma, H. E.; J. Photochem. Photobiol. A 1998, 118, 11.        [ Links ]

72. Wasielewski, M. R.; Liddell, P. A.; Barrett, D.; Moore, T. A.; Gust, D.; Nature 1986, 322, 570.        [ Links ]

73. Whitten, D. G.; Spooner, S. P.; Hsu, Y.; Penner, T. L.; React. Polym. 1991, 15, 37.        [ Links ]

74. Wasielewski, M. R.; Chem. Rev. 1992, 92, 435.        [ Links ]

75. Clayton, A. H. A.; Ghiggino, K. P.; Lawson, J. M.; Paddonrow, M. N.; J. Photochem. Photobiol. A 1994, 80, 323.        [ Links ]

76. Harriman, A.; Hissler, M.; Trompette, O.; Ziessel, R.; J. Am. Chem. Soc. 1999, 121, 2516.        [ Links ]

77. LeGourrierec, D.; Andersson, M.; Davidsson, J.; Mukhtar, E.; Sun, L. C.; Hammarstrom, L.; J. Phys. Chem. A 1999, 103, 557.        [ Links ]

78. Lehn, J. M.; Angew. Chem., Int. Ed. 1988, 27, 89;         [ Links ]B. Alpha; R. Ballardini; V. Balzani; J. M. Lehn; S. Perathoner; N. Sabbatini; Photochem. Photobiol. 1990, 146, 347;         [ Links ]B. Alpha; V. Balzani; J. M. Lehn; S. Perathoner; N. Sabbatini; Angew. Chem. Int. Ed. 1987, 26, 1266;         [ Links ]G. Blasse; G. J. Dirksen; N. Sabbatini; S. Perathoner; J. M. Lehn; B. Alpha; J. Phys. Chem. 1988, 92, 2419.        [ Links ]

79. Bagatin, I. A.; Toma, H. E.; New J. Chem. 2000, 24, 841.        [ Links ]

80. Gameiro, C. G.; Achete, C. A.; Simão, R. A.; Da Silva, E. F.; Santa-Cruz, P. A.; J. Alloy Compd. 2002, 344, 385.        [ Links ]

81. Gameiro, C. G.; Da Silva, E. F.; Alves, S.; De Sa, G. F.; Santa-Cruz, P. A.; J. Alloy Compd. 2001, 323, 820.        [ Links ]

82. Gameiro, C. G.; Da Silva, E. F.; Alves, S.; De Sa, G. F.; Santa-Cruz, P. A.; Mater. Sci Forum 1999, 315, 249.        [ Links ]

83. Hu, Y. Z.; Tsukiji, S.; Shinkai, S.; Oishi, S.; Hamachi, I.; J. Am. Chem. Soc. 2000, 122, 241.        [ Links ]

84. Araki, K.; Losco, P.; Engelmann, F. M.; Winnischofer, H.; Toma, H. E.; J. Photochem. Photobiol. A 2001, 142, 25.        [ Links ]

85. Flamini, L.; Barigelletti, F.; Armaroli, N.; Collin, J. P.; Dixon, I. M.; Sauvage, J. P.; Williams, J. A. G.; Coord. Chem. Rev. 1999, 192, 671.        [ Links ]

86. Onuki, J.; Ribas, A. V.; Medeiros, M. H. G.; Araki, K.; Toma, H. E.; Catalani, L. H.; Di Mascio, P.; Photochem. Photobiol. 1996, 63, 273.        [ Links ]

87. Vincendo, P., Mouysset, S.; Paillous, N.; Photochem. Photobiol. 1997,65, 647.        [ Links ]

88. Barton J. K.; Raphael, A. L.; J. Am. Chem. Soc. 1984, 106, 2466.        [ Links ]

89. Fiel, R. J.; J. Biomol. Struc.Dyn. 1989, 6 , 1259.        [ Links ]

90 Fiel, R. J.; Howard, J. C.; Mark, E. H.; Gupta, N. D.; Nucleic Acids Res. 1979, 6, 3093.        [ Links ]

91. Marzilli, L. G.; New J. Chem. 1990, 14, 409.        [ Links ]

92. Dougherty, T. J.; Gomer, C. J.; Henderson, B. W.; Jori, G.; Kessel, D.; Korbelik, M.; Moan, J.; Peng, Q.; J. Natl. Cancer Inst. 1998, 90, 889.        [ Links ]

93. Henderson, B. W.; Dougherty, T. J.; Photochem. Photobiol. 1992, 55, 145.        [ Links ]

94. Foote, C. S; Photochem. Photobiol. 1991, 54, 659.        [ Links ]

95. Araki, K.; Silva, C. A.; Toma, H. E.; Catalani, L. H.; Medeiros, M. H. G.; Di Mascio, P.; J. Inorg. Biochem. 2000, 78, 269.        [ Links ]

96. Ravanat, J.-L.; Berger, M.; Benard, F.; Langois, R.; Oullet, R.; van Lier, J. E.; Cadet, J.; Photochem. Photobiol. 1992, 55, 809.        [ Links ]

97. Adam, W.; Saha-Möller, C. R.; Schönberger, A.; J. Am. Chem. Soc. 1997, 119 , 719.        [ Links ]

98. Ravanat, J. L.; Cadet, J.; Araki, K.; Toma, H. E.; Medeiros, M. H. G.; Di Mascio, P.; Photochem. Photobiol. 1998, 68, 698.        [ Links ]

99. Gunter, M. J.; Turner, P.; Coord Chem. Rev. 1991, 108, 115.        [ Links ]

100. Meunier, B.; Chem. Rev. 1992, 92, 1411.        [ Links ]

101. Araki, K.; Toma, H. E.; J. Chem. Res. (M) 1994, 1501.        [ Links ]

102. Araki, K.; Toma, H. E.; Inorg. Chim. Acta 1991, 179, 293.        [ Links ]

103. Toma, H. E.; Araki, K.; J. Chem. Res. (S) 1990, 83.        [ Links ]

104. Alexiou, A. D. P.; Toma, H. E.; J. Chem. Res. (S) 1993, 464.        [ Links ]

105. Toma, H. E.; Cunha, C. J.; Cipriano, C.; Inorg. Chim. Acta 1988, 154, 63.        [ Links ]

106. Toma, H. E.; Alexiou, A. D. P.; Electrochim. Acta, 1993, 38, 975.        [ Links ]

107. Araujo, J. Jr.; Nikolaou, S.; Alexiou, A.D.P.; Toma, H.E.; Monatsh. Chem. 1997, 128 759        [ Links ]

108. Alexiou, A. D. P; Toma, H. E.; J. Chem. Res. (S) 1997, 338.        [ Links ]

109 Toma, H.E.; Cunha, C.J.; Can. J. Chem. 1989, 67, 1632.        [ Links ]

110. Toma, H.E.; Cipriano, C.; J. Electroanal. Chem. 1989, 263, 313.        [ Links ]

111. Toma, H. E.; Araki, K.; Silva, E. O.; Monatsh. Chem. 1998, 129, 975.        [ Links ]

112. Dovidauskas, S.; Toma, H. E.; Araki, K.; Sacco, H. C.; Iamamoto, Y.; Inorg. Chim. Acta 2000, 305, 206.        [ Links ]

113. Jin, N.; Groves, J.T.; J. Am. Chem. Soc. 1999, 121, 2923.        [ Links ]

114. Sorokin, A.; Robert, A.; Meunier, B.; J. Am. Chem. Soc. 1993, 115, 7293        [ Links ]

115. Czernuszewicz, R.S.; Su, Y.O.; Stern, M.K.; Macor, K.A.; Kim, D.; Groves, J.T.; Spiro, T.G; J. Am. Chem. Soc. 1988,110, 4158        [ Links ]

116. Smegal, J.A.; Hill, C.L.; J. Am. Chem. Soc. 1983, 105, 3515.        [ Links ]

117. Toyama, M.M.; Araki, K.; Toma, H.E.; Spectrosc. Lett. 1998, 31, 1065.        [ Links ]

118. Araki, K.; Wagner, M.J.; Wrighton, M.S.; Langmuir 1996, 12, 5393.        [ Links ]

119. Araki, K.; Toma, H.E.; Electrochim. Acta 1999, 44, 1577.        [ Links ]

120. Araki, K.; Angnes, L.; Toma, H.E.; Adv. Mater. 1995, 7, 554        [ Links ]

121. Palmer, S.M.; Stanton, J.L.; Jaggi, N.K.; Hoffman, B.M.; Ibers, J.A.; Schwartz, L.H.; Inorg. Chem. 1985, 24, 2040.        [ Links ]

122. Newcomb, T.M.; Godfrey, M.R.; Hoffman, B.M.; Ibers, J.A.; J. Am. Chem. Soc. 1989, 111, 7078        [ Links ]

123. Newcomb, T.P.; Godfrey, M.R.; Hoffman, B.M.; Ibers, J.A.; Inorg. Chem. 1990, 29, 223.        [ Links ]

124. Shi, C.N.; Anson, F. C.; Inorg. Chem. 1992, 31, 5078.        [ Links ]

125. Steiger, B.; Shi, C.N.; Anson, F. C.; Inorg. Chem. 1993, 32, 2107.        [ Links ]

126. Anson, F. C.; Shi, C.N.; Steiger, B.; Acc. Chem. Res. 1997, 30, 437.        [ Links ]

127. Song, E. H.; Shi, C. N.; Anson, F. C.; Langmuir 1998, 14, 4315.        [ Links ]

128. Collman, J. P.; Marrocco, M.; Denisevich, P.; Koval, C.; Anson, F. C.; J. Electronal. Chem. 1979, 101, 117.        [ Links ]

129. Collman, J. P.; Denisevich, P.; Konai, Y.; Marrocco, M.; Koval, C.; Anson, F. C.; J. Am. Chem. Soc. 1980, 102, 6027.        [ Links ]

130. Durand, R. R.; Bencosme, C. S.; Collman, J. P.; Anson, F. C.; J. Am. Chem. Soc. 1983, 105, 2710.        [ Links ]

131. Collman, J. P.; Inorg. Chem. 1997, 36, 5145.        [ Links ]

132. Shi, C. N.; Anson, F. C.; J. Am. Chem. Soc. 1991, 113, 9564.        [ Links ]

133. Shi, C. N.; Anson, F. C.; Inorg. Chim. Acta 1994, 225, 215.        [ Links ]

134. Steiger, B.; Anson, F. C.; Inorg. Chem. 1995, 34, 3355.        [ Links ]

135. Steiger, B.; Anson, F. C.; Inorg. Chem. 1997, 36, 4138.        [ Links ]

136. Steiger, B.; Anson, F. C.; J. Porphyrins Phtalocyanines 1999, 3, 159.        [ Links ]

137. Shi, C. N.; Anson, F. C.; Inorg. Chem. 1995, 34, 4554.        [ Links ]

138. Shi, C. N.; Anson, F. C.; Inorg. Chem. 1998, 37, 1037.        [ Links ]

139. Araki, K.; Dovidauskas, S.; Winnischofer, H.; Alexiou, A. D. P.; Toma, H. E.; J. Electroanal. Chem. 2001, 498, 152.        [ Links ]

140. Araki, K.; Angnes, L.; Azevedo, C. M. N.; Toma, H. E.; J. Electroanal. Chem. 1995, 397, 205.        [ Links ]

141. Truxillo, L.A.; Davis, D.G.; Anal. Chem. 1975, 47, 2260.        [ Links ]

142. VilchezAguado F.; GutierrezGranados, S.; SucarSuccar S.; BiedCharreton, C.; Bedioui, F.; New J. Chem. 1997, 21, 1009.        [ Links ]

143. Shimidzu, T.; Polym. Adv. Technol. 1997, 8, 275.        [ Links ]

144. Deronzier, A.; Devaux, R.; Limosin, D.; Latour, J.M.; J. Electroanal. Chem. 1992, 324, 325.        [ Links ]

145. Schaferling, M.; Bauerle, P.; Synth. Met. 2001, 119, 289.        [ Links ]

146. Diab, N.; Schuhmann, W.; Electrochim. Acta 2001, 47, 265.        [ Links ]

147. Bruti, E.M.; Giannetto, M.; Mori, G.; Seeber, R.; Electroanalysis 1999, 11, 565.        [ Links ]

148. Volf, R.; Shishkanova, T.V.; Kral, V.; J. Inclusion Phenom. Macrocyclic Chem. 1999, 35, 111.        [ Links ]

149. Takada, K.; Storrier, G.D.; Goldsmith, J.I.; Abruna, H.D.; J. Phys. Chem. B 2001, 105, 2404.        [ Links ]

150. Bommarito, S.L.; Lowerybretz, S.P.; Abruna, H.D.; Inorg. Chem. 1992, 31, 502.        [ Links ]

151. Takada, K.; Storrier, G.D.; Pariente, F.; Abruna, H.D.; J. Phys. Chem. B 1998, 102, 1387.        [ Links ]

152. Fussarydel, O.; Zhang, H.T.; Hupp, J.T.; Leidner, C.R.; Inorg. Chem. 1989, 28, 1533.        [ Links ]

153. Winnischofer, H.; Lima, S. S.; Araki, K.; Toma, H. E.; Anal. Chim. Acta 2003, 480, 97.        [ Links ]

154. Kuester, S.N.; McGuire,M.M.; Drew, S. M; J. Electroanal. Chem. 1998, 452, 13.        [ Links ]

155. Bommarito, S. L.; Lowerybretz, S.P.; Abruna, H.D.; Synlett 1993, 375.        [ Links ]

156. Araki, K.; Toma, H.E.; J. Coord. Chem. 1993, 30, 9.        [ Links ]

157. Armstrong, R.D.; Lindholm, B.; Sharp, M.; J. Electroanal. Chem. 1986, 202, 69.        [ Links ]

158. Andrieux, C.P.; Haas, O.; Saveant, J.M.; J. Am. Chem. Soc. 1986, 108 , 8175.        [ Links ]

159. Rocha, J.R.C.; Angnes, L.; Bertotti, M.; Araki, K.; Toma, H.E.; Anal. Chim. Acta 2002, 452, 23.        [ Links ]

160. Coker, L. E.; J. Assoc. Off. Anal. Chem. 1986, 69, 8.        [ Links ]

161. Moylan, J. G.; Bowes, F. W.; Pappin, W. J.; J. Assoc. Off. Anal. Chem., 1986, 69, 11.        [ Links ]

162. Ough, C. S.; Tratado Basico de Enología, Acribia: Zaragoza, 1996.        [ Links ]

163. Ough, C. S.; J. Assoc. Off. Anal. Chem, 1986, 69, 5-7.        [ Links ]

164. Gomes, M. T.; Rocha, T. A.; Duarte, A. C.; Oliveira, J. P.; Anal. Chem. 1996, 68, 1561.        [ Links ]

165. Normas de Qualidade para Alimento, Instituto Adolfo Lutz: São Paulo, 1976, vol. 6.        [ Links ]

166. Linares, P.; Luque de Castro, M. D.; Valcárcel, M.; Anal. Chim. Acta, 1989, 225, 443.        [ Links ]

167. Zhi, Z.; Ríos, A.; Valcárcel, M.; Analyst 1995, 120, 2013.        [ Links ]

168. Decnop-Weever, L. G.; Kraak, J. C.; Anal. Chim. Acta 1997, 337, 125.        [ Links ]

169. Cardwell, T. J.; Cattrall, R. W.; Chen, G. N.; Scollary, G. R.; Hamilton, I. C.; Analyst 1991, 116, 253.        [ Links ]

170. Granados, M.; Maspoch, S.; Blanco, M.; Anal. Chim. Acta 1986, 179, 445.        [ Links ]

171. Angnes, L.; Azevedo, C. M. N.; Araki, K.; Toma, H. E.; Anal. Chim. Acta 1996, 329, 91.        [ Links ]

172. Azevedo, C. M. N.; Araki, K.; Angnes, L.; Toma, H. E.; Electroanalysis 1998, 10, 467.        [ Links ]

173. Huang, Y. G.; Ji, J. D.; Hou, Q. N.; Mutat. Res. 1996, 358, 7.        [ Links ]

174. Wolff, I. A.; Wassema, A. E.; Science 1972, 177, 15.        [ Links ]

175. Williams, A. E.; Johnson, J. A.; Lund, I. J.; Kabala, Z. J.; J. Environ. Qual. 1998, 27, 1147.        [ Links ]

176. Rocha, J. R. C.; Demets, G. J. -F.; Bertotti, M.; Araki, K.; Toma, H. E.; J. Electroanal. Chem. 2002, 526, 69.        [ Links ]

177. Quintino, M. S.; Araki, K.; Toma, H. E.; Angnes, L.; Electroanalysis 2002, 14, 1236.        [ Links ]

 

 

Received: March 24, 2003
Published on the web: October 15, 2003
FAPESP helped in meeting the publication costs of this article.

 

 

* e-mail: henetoma@iq.usp.br

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