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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.5 São Paulo Sept./Oct. 2003

http://dx.doi.org/10.1590/S0103-50532003000500013 

ARTICLE

 

Inorganic self-assembly through sequential complexation in the formation of bimetallic and trimetallic architectures from multisite ligands based on 5,5'-disubstituted 2,2'-bipyridines

 

 

Vanderlei G. MachadoI, II, #; Antonio S. MangrichII; Jean-Marie LehnI*

IISIS, Université Louis Pasteur, 4, rue Blaise Pascal F-67000, Strasbourg, France
IIDepartamento de Química, Universidade Federal do Paraná, UFPR, 81531-970, Curitiba-PR, Brazil

 

 


ABSTRACT

Two multisite 5,5'-disubstituted 2,2'-bipyridine ligands containing N-methyl hydroxamic acids as substituents [5,5'-bis(N-methylhydroxamic)-2,2'-bipyridine (4) and 5-methyl-5'-(N-methylhydroxamic)-2,2-bipyridine (10)] were synthesized. These ligands were used in order to illustrate the strategy of self-assembly through sequential complexation. According to this concept, the first metal added organizes the ligands disposed in 5,5'-positions to accomodate the second metal ion that is sequentially added. Thus, addition of Fe2+ to a solution of 4 led to a Fe2+-tris(bipyridine) complex. Addition of Fe3+ to this solution yielded a trimetallic architecture, which was characterized. Ligand 10 yielded a mixture of bimetallic architectures through complexation with Fe2+ followed by Fe3+ ions. However, if the order of metal addition is changed, only one bimetallic complex is obtained. This is due to the fact that the first metal ion added (Fe3+) acts as a template, organizing the bipyridine ligands and preforming an adequate cavity for the Fe2+ ion.

Keywords: inorganic self-assembly, sequential ligands, sequential complexation, metallo-exoreceptors


RESUMO

Dois pré-ligantes 2,2'-bipiridínicos 5,5'-dissubstituídos apresentando em sua estrutura dois ou três sítios de coordenação [5,5'-bis(ácido N-metil-hidroxâmico)-2,2'-bipiridina (4) e 5-metil-5'-(ácido N-metil-hidroxâmico)-2,2-bipiridina (10)] foram sintetizados. Estes ligantes foram empregados no estudo de uma estratégia de automontagem por complexação seqüencial. De acordo com este conceito, o primeiro metal adicionado organiza os substituintes-ligantes das posições 5,5' para a complexação do segundo íon metálico adicionado seqüencialmente. A adição de Fe2+ a uma solução contendo 4 levou à formação do complexo Fe2+-tris(bipiridil). A adição de Fe3+ a este complexo rendeu uma arquitetura trimetálica. O ligante 10 levou à formação de uma mistura de arquiteturas bimetálicas pela adição seqüencial de íons Fe2+ e Fe3+. No entanto, quando a ordem de adição foi alterada, somente um complexo bimetálico foi obtido. Isto se deve ao fato de que o primeiro metal adicionado (Fe3+) age como um molde, organizando os ligantes bipiridínicos e pré-formando uma cavidade adequada para o íon Fe2+.


 

 

Introduction

Self-assembly of inorganic architectures from programmed components has been an extensively investigated field of supramolecular chemistry in recent years.1-6 Such processes involve the design of programmed supramolecular species, which are spontaneously formed from carefully constructed ligands and metal ions able to read the binding sites according to their coordination algorithm.1,2,6 This strategy has allowed the synthesis of a great variety of inorganic architectures,1-6 such as double-7 and triple-helical8 complexes, rack-,9 grid-10 and cage-type11 arrays of metal ions synthesized by our own group. The design of ligands containing different coordination sites has spontaneously yielded structures having different metal ions at specific locations, as in heterometallic helicates12 and in large multicomponent arrays.13

Exoreceptors are receptor molecules where the substrate fixation sites are divergent, in opposition to the convergent chemistry of the endoreceptors.1,6,14,15 The different kinds of exoreceptors include organic as well as inorganic entities. For instance, linear koilands, are rigid and compact exoreceptors with two diametrically opposing cavities, and connector molecules with two extremities complementary to the cavities of the exoreceptor.14 In the metallo-exoreceptors,15 the ligands bearing the groups responsible for the fixation of the substrate, are assembled by the central metal ion, which has a double function: it disposes the recognition units according to the coordination geometry of the ion, and it also introduces strong electrostatic interactions due to the charge of the ion.

Recently, we have discussed the potential presented by self-assembled metallo-exoreceptors generated by complexation of 5,5'-disubstituted 2,2'-bipyridines (bipys) with a suitable metal ion.6 Thus, the octahedral coordination of 5,5'-disubstituted 2,2'-bipyridines by a metal ion such as Fe2+ will enable the substituents to acquire a proper spatial orientation, leading to the formation of a ditopic metallo-exoreceptor presenting two potential substrate binding subunits. These receptors may be of importance in many areas of supramolecular chemistry, such as enzyme modelling, anionic recognition and in the development of molecular devices. Their use depends in principle only on the design of the 2,2'-bipyridine ligand, more specifically on the nature of the substituents in 5,5'-positions. If the resultant metallo-exoreceptor possesses potential binding units as substituents, the complexation at these sites with other metal ions or with other substrates occurs in a defined sequence. Thus, transition metal complexes of aminoacid16 and amide17-5,5'-disubstituted-bipy ligands have been shown to form receptor pockets along the (pseudo)-threefold axis, to which chloride counteranions may bind. Three iron (II) complexes of 5,5'-bis(ethoxycarbonylamino)-2,2'-bipyridine have been shown to be able to encapsulate sulfate, perchlorate, or nitrate anions.18 This strategy of self-assembly through sequential complexation may involve, in a first step, the synthesis of specially designed sequential ligands16-19 capable of presenting hierarchical assembly features.

Hydroxamic acids are hard ligands capable of complexing hard ions such as Fe3+, while the soft bipy ligands bind soft metal ions such as Fe2+, Co2+ and Ru2+. These features allowed the synthesis of molecular redox switches possessing these two types of ligands anchored on a triple-stranded ligand20 or on a calix[4]arene ring.21 Chemical oxidation and reduction leads to the reversible translocation of the metal ion between the soft and the hard sites, and these changes can be easily monitored spectroscopically. Here, we report the synthesis and properties of two sequential ligands 4 and 10 that bear either a single, or two, hydroxamic acid groups anchored on a bipy moiety with a view to illustrating the concept of sequential complexation through the formation of bimetallic and trimetallic architectures.

 

Experimental

General

All chemicals used were high-purity commercial reagents. Deionized water was used in all measurements. This solvent was boiled and bubbled with nitrogen and kept in a nitrogen atmosphere to avoid the presence of carbon dioxide. THF was distilled from sodium using benzophenone as an indicator.22 Dichloromethane was distilled from calcium hydride.22 All other solvents employed in the reactions were used as received. Tetrakis(triphenylphosphine)palladium (0), [Pd(PPh3)4], was prepared according to the procedure described in the literature.23 N-methyl acetohydroxamic acid was prepared by reacting N-methylhydroxylamine with acetyl chloride in basic methanol.24 The stock FeCl3 solutions were standardized with a standard solution of triply recrystallized K2Cr2O7, after reduction with stannous ions, according to normal procedures.25

Instrumentation and physical measurements

Melting points (mp) were obtained on a Kofler hot stage and were uncorrected. TLC was performed on HF-254 (Merck) plates, visualizing with a 254 nm UV lamp. UV-Vis experiments were made with Cary 13 and HP-8453 spectrophotometers equipped with a thermostated bath and all measurements were performed at 25oC. The pH-meter titrations were performed with a Metrohm-636 titrimeter. Nuclear magnetic resonance spectra were recorded on Bruker AC 200 (200 MHz) or Bruker AM 400 spectrometers. Chemical shifts were recorded in ppm with the solvent resonance as the internal standard. Data are reported as follows: chemical shift, multiplicity (s = singlet, d = doublet, t = triplet, m = multiplet, dd = doublet of doublet, bs = broad singlet), integration and coupling constants (Hz). Electronic paramagnetic resonance (EPR) experiments were carried out at 77K on a Bruker ESP 300E spectrometer operating at X-band frequency (~9.5 GHz) with 100 kHz field modulations, modulation amplitude equal to 2.024 G and microwave power approximately equal to 20 mW. The spectra were recorded in first and second derivative mode for the powdered and frozen solution (77 K) samples in quartz tubes. WINEPR® software was also used to treat the spectra. Infrared spectra were measured on a Bomen FTIR spectrophotometer, with KBr pellets. Electron impact (EI+) mass spectra were obtained with a Fisons Instruments TRIO 2000 (Manchester) spectrometer. Fast-atom bombardment (FAB+) mass spectra were recorded on a Micromass AUTOSPEC-M-HF (Manchester) instrument and electron spray (ESI+) mass spectra were obtained on a VG BIOQ triple quadrupole Quattro II (Micromass, Altrincham) spectrometer. Microanalyses were determined by a Perkin Elmer 2400 elemental analyzer.

Synthesis of the ligands and their metal complexes

Compounds 1, 2, 3 and 5 were prepared according to the procedures described in the literature (1,26,27 2,28 329 and 530).

5,5'-Bis(N-methylhydroxamic)-2,2'-bipyridine (4)

A mixture of N-methyl hydroxylammonium hydrochloride (14.1 mL of an aqueous solution 4 mol L-1; 56.4 mmol) with NaOH (14.1 mL of an aqueous solution 3.5 mol L-1) was added to the 5,5'-bis(chlorocarbonyl)-2,2'-bipyridine (2.30 g; 8.20 mmol) at room temperature, while stirring. The mixture was then stirred overnight. The suspension was adjusted to pH 7, and the white solid was collected, and washed with water and acetone. The product was dried (2.1 g ; 85% yield); 1H NMR (200 MHz, DMSO-d6): d 3.31 (6H, s), 8.18 (2H, dd, J 2.1 and 8.2 Hz), 8.46 (2H, d, J 8.3 Hz), 8.93 (2H, d, J 2.1 Hz), 10.31 (2H, s); IR (KBr) nmax/cm-1: 3553, 3490, 3145, 2822, 1734, 1655, 1600, 1500, 1423, 1385, 1221, 1174, 1082, 1024, 951, 910, 849, 753, 644; MS (FAB+): 303.1 (100); Anal. calcd. for C14H14N4O4 : C, 55.63; H, 4.64; N, 18.54. Found: C, 55.85; H, 4.60; N, 18.80.

5-Methyl-2-trimethyltinpyridine (6)

To a closed flask, protected from moisture by argon flow, n-butyl lithium 1.6 mol L-1 solution in hexane (35.8 mL, 57.2 mmol) was added. The temperature in the flask was lowered to -78 oC. 2-Bromo-5-methylpyridine (9.36 g, 54.4 mmol) was added drop by drop as a dried THF solution, while stirring. The color of the solution changed to dark brown. Trimethyltinchloride 1 mol L-1 solution in THF (54.4 mL, 54.4 mmol) was added drop by drop while stirring. At the end of the addition, the color of the solution changed to yellow. The reaction mixture was filtered and the solvent was rotary-evaporated. The oily pale yellow product obtained was distilled under vacuum and the first fraction was collected (75 oC, 3.5 mm Hg) (11.34 g, 81.5%). This product is unstable and must be used immediately in the next reaction. 1H NMR (200 MHz, CDCl3): d 2.29 (3 H, s, CH3), 7.32 (1 H, d, J 7.8 Hz), 7.36 (1 H, d, J 8.6 Hz), 8.59 (1 H, s).

5-Carboxyethyl-5'-methyl-2,2'-bipyridine (7)

A solution of 2-chloro-5-ethylnicotinate (4.0 g, 21.6 mmol), 5-methyl-2-trimethyltinpyridine (5.79 g, 22.6 mmol) and [Pd(PPh3)4] (2.9 g, 2.51 mmol) in dry toluene (96 mL) was refluxed for 72 h. The solvent was removed and dichloromethane was added to the black oil. The black solid separated was filtered off and the liquid, after removal of the solvent, was chromatographied (Al2O3 II-III activity, dichloromethane as eluent). The fractions were collected and the solvent was rotary-evaporated. The yield obtained was 4.09 g (78%) of a pale yellow solid. 1H NMR (200 MHz, CDCl3): d 1.43 (3H, t, J 7.1 Hz), 2.42 (3H, s), 4.43 (2H, q, J 7.1 Hz), 7.66 (1H, dd, J 1.7 and 8.0 Hz), 8.37 (1H, dd, J 1.5 and 8.4 Hz), 8.39 (1H, d, J 8.3 Hz), 8.46 (1H, d, J 8.0 Hz), 8.53 (1H, d, J 1.7 Hz), 9.25 (1H, d, J 1.5 Hz); IR (KBr) nmax/cm-1: 3052, 2985, 1719, 1591, 1552, 1461, 1387,1367, 1295, 1279, 1238, 1135, 1028, 851, 788, 747; MS (EI+): 197.1 (100), 242.2 (60).

5-Carboxy-5'-methyl-2,2'-bipyridine (8)

5-Carboxyethyl-5'-methyl -2,2'-bipyridine (1.0 g; 4.13 mmol) was taken up in methanol (5 mL) to which NaOH 1 mol L-1 (5 mL) was added and the solution stirred at room temperature for about 5 h. The solvent was evaporated and the residue dissolved in a minimum amount of water. The solution was extracted with dichloromethane (2×15 mL) and the aqueous layer acidified to pH~3 with concentrated HCl. The product precipitated as an almost white solid. After filtration and washing with water, the solid was dried (0.85 g, 97%). 1H NMR (200 MHz, DMSO-d6): d 2.39 (3H, s), 7.83 (1H, dd, J 2.3 and 8.2 Hz), 8.37 (1H, d, J 8.0 Hz), 8.39 (1H, dd, J 2.1 and 8.3 Hz), 8.48 (1H, d, J 8.3 Hz), 8.58 (1H, d, J 2.3 Hz), 9.14 (1H, d, J 2.1 Hz); IR (KBr) nmax/cm-1: 3432, 1875, 1702, 1593, 1556, 1468, 1370, 1262, 1220, 1138, 1049, 839, 790, 742, 714; MS (EI+): 142.1 (25), 169.1 (27), 214.2 (100).

5-(Chlorocarbonyl)-5'-methyl-2,2-bipyridine (9)

Compound 8 (0.83 g; 3.88 mmol) and 20 mL of thionyl chloride were refluxed for 3.5 h. The excess thionyl chloride was distilled off and the pale yellow solid was dried under vacuum for two hours. The yield was quantitative and the product was used immediately in the subsequent reaction. IR (KBr) nmax/cm-1: 1717, 1594, 1546, 1378, 1220, 1128, 847, 786.

5-Methyl-5'-(N-methylhydroxamic)-2,2-bipyridine (10)

A mixture of N-methyl hydroxylammonium hydrochoride (3.5 mL of an aqueous solution 4 mol L-1; 14.1 mmol) with NaOH (3.5 mL of an aqueous solution 3.5 mol L-1; 12.3 mmol) was added to compound 9 (0.9 g, 3.88 mmol) at room temperature, while stirring. The mixture was stirred overnight. The suspension was adjusted until pH 7, the white solid obtained was collected, and washed with water and diethyl ether. The product was dried (0.78 g, 74%). 1H NMR (200 MHz, CDCl3): d 2.42 (3H, s), 3.48 (3H, s), 7.66 (1H, dd, J 2.1 and 8.2 Hz), 7.99 (1H, dd, J 2.2 and 8.3 Hz), 8.30 (1H, d, J 8.1 Hz), 8.38 (1H, d, J 8.3 Hz), 8.52 (1H, d, J 2.1 Hz), 8.82 (1H, d, J 2.2 Hz); IR (KBr) nmax/cm-1: 3358, 2829, 1604, 1455, 1423, 1386, 1220, 1025, 908, 836, 781, 739, 650; MS (EI+): 169.1 (62), 197.1 (100), 227.2 (12), 243.2 (5); Anal. calcd. for C13H13N3O2 : C, 64.20; H, 5.35; N, 17.28. Found: C, 63.94; H, 5.34; N, 17.37.

Synthesis of the complex [Fe2+(4)3](Cl-)2 (11)

Ligand 4 (1.0 g; 3.31 mmol) was added to a degassed (with a stream of nitrogen) aqueous solution of FeCl2 (0.219 g; 1.10 mmol) while stirring at room temperature. The color of the reactional mixture changed immediately to purple. The mixture was stirred for one hour at room temperature under nitrogen. After that, the mixture was filtered and the purple solution was rotary-evaporated. The microcrystalline solid was dissolved in a minimum amount of water and precipitated by addition of hot acetone. The solid was filtered, washed with small volumes of acetone (5´20mL) and dried to give dark violet crystals (1.03 g; 90% yield). This complex is only soluble in water and methanol with very small amount of water.31 1H NMR (200 MHz, D2O): d 3.09 (18H, s), 7.60 (6H, s), 8.22 (6H, d, J 7.84 Hz), 8.54 (6H, d, J 7.84 Hz); IR (KBr) nmax/cm-1: 3339, 3060, 2853, 1721, 1632, 1384, 1223, 1184, 1136, 1083, 1045, 913, 851, 741, 565; MS (FAB+): 997.1 (50%), 961.1 (100%); MS (ESI+): 997.2 (5%), 481.4 (100%); Anal. calcd. for C42H42N12O12 FeCl2: C, 48.80; H, 4.07; N, 16.27. Found: C, 48.92; H, 4.05; N, 16.34.

Synthesis of the complex [Fe2+(Fe3+)2(42-) 3](Cl-)2 (12)

A solution of FeCl3 (66.5 mg, 0.246 mmol) in methanol (9 mL) was added while stirring to a solution of 11 (127 mg, 0.123 mmol) in water (15 mL). The color of the solution immediately changed from purple to brownish red. The mixture was stirred at room temperature for one hour. The resultant solution was chromatographied on a Sephadex column. The fraction corresponding to the product was collected and was rotary-evaporated. The resultant solid was dried (black solid; 112 mg; 80%). The EPR spectrum for the solution (methanol:water 4:1; pH 6.2) at liquid N2 temperature (77 K), as also for a solid sample of 12, showed a line having g = 4.3. IR (KBr) nmax/cm-1: 3405, 1719, 1607, 1435, 1384, 1202, 1135, 1089, 961, 848, 752, 704; Anal. calcd. for C42H36N12O12 Fe3Cl2: C, 44.27; H, 3.16; N, 14.76. Found: C, 44.36; H, 3.19; N, 14.85.

Synthesis of the complex [(Fe3+)2(42-)3] (13)

A suspension of 4 (0.0401 g; 0.133 mmol) in 10 mL of water was stirred. After that, FeCl3 (0.0144 g; 0.0885 mmol) was added drop by drop as a solution 9.94´10-3 mol L-1 in methanol. The solid dissolved immediately and a wine solution was observed. The reactional mixture was stirred for one hour and it was then chromatographied on a Sephadex column. The solvent was removed and the solid was dried (0.0327g; 73%). EPR spectrum for the frozen solution (methanol:water 4:1; pH 6.2; 77 K) showed a line having g= 4.3. IR (KBr) nmax/cm-1: 3421, 2360, 1719, 1610, 1435, 1384, 1205, 1087, 1040, 962, 851, 702, 672; Anal. calcd. for C42H36N12O12 Fe2: C, 49.82; H, 3.56; N, 16.61. Found: C, 50.02; H, 3.54; N, 16.68.

Synthesis of the complexes [Fe2+(10)3](Cl-)2 (14a,b)

Ligand 10 (0.100 g; 0.411 mmol) was suspended in degassed water (10 mL) and FeCl2 (0.0174 g; 0.137 mmol) was added while stirring at room temperature. The solid was solubilized and the color of the reactional mixture immediately changed to purple. The solution was stirred for one hour, filtered and the solvent was rotary-evaporated. The resultant dark purple microcrystalline solid was dried (0.101 g; 86% yield). The 1H NMR spectrum revealed the presence of two isomers, 14a and 14b. 1H NMR (400 MHz, CD3OD: D2O 4:1): d 2.23 (s), 2.49 (s), 3.26 (s), 3.27 (s), 3.43 (s), 7.32 (3H, m), 7.75 (3H, m); 8.06 (3H, m), 8.43 (3H, m), 8.61-8.68 (6H, m). The COSY H-H spectrum showed the following correlations: methyl group bonded to aromatic system with H-3', H-4' and H-6', H-3'/H-4', H3'/H-6', H-4'/H-6', H-3/H-4, H-3/H-6 and H-4/H-6. Anal. calcd. for C39H39N9O6 FeCl2: C, 54.69; H, 4.56; N, 14.72. Found: C, 54.40; H, 4.58; N, 14.78.

Synthesis of the complexes [Fe2+Fe3+(10-)3](Cl-)2 (15a,b)

These complexes were only prepared in solution. The EPR spectrum for the frozen solution (methanol:water 4:1; pH 6.2) of 15a,b (77 K) showed a broad line having g = 4.3.

Synthesis of the complex [Fe3+(10)3](Cl-)2 (16)

This complex was only prepared in solution. Ligand 10 (0.00292 g; 0.012 mmol) was added to a solution of FeCl3 5.24´10-4 mol L-1 in 16 mL methanol and 4 mL buffer MES (pH=6.20, 50 mmol L-1). An orange solution was immediately formed. lmax=424 nm; emax=3106 L mol-1 cm-1; the EPR spectrum of this frozen solution (77 K) showed a very sharp line having g= 4.3.

Synthesis of the complex [Fe2+(10)3](Cl-)2 (14a)

This complex was prepared only in solution for NMR measurements. Ligand 10 (0.00237 g; 9.7´10-6 mol) was dissolved in 0.5 mL of a CD3OD:D2O (4:1) mixture. After that, FeCl3 was added (5.45´10-4 g; 3.36´10-6 mol) and an orange color appeared. FeCl2 was then added (36.5 mL from a D2O stock solution 0.092 mol L-1). Finally, after 10 minutes, 2 mg (1.13´10-5 mol) of ascorbic acid was added to the NMR tube. 1H NMR (400 MHz): d 2.23 (9H, s), 3.24 (9H, s), 7.32 (3H, m), 7.75 (3H, m); 8.06 (3H, m), 8.43 (3H, m), 8.61-8.68 (6H, m). The COSY H-H spectrum showed the following correlations: methyl group bonded to aromatic system with H-3', H-4' and H-6', H-3'/H-4', H3'/H-6', H-4'/H-6', H-3/H-4, H-3/H-6 and H-4/H-6.

pKa determinations

The pKa titrations were performed in aqueous 0.1 mol L-1 tetramethylammonium chloride with magnetic stirring, using a water-jacket equipped sealed cell in which a strong argon stream was maintained. The medium was thermostated at 25.0 ± 0.1 °C with circulating water through the outer jacket. Standard 0.1 mol L-1 CO2-free NaOH was delivered from a microburette. Potential measurements were performed in millivolt mode with the use of a glass electrode. The potential versus volume data were analysed with Superquad.32

Stoichiometry determinations

The experiments for stoichiometry determinations were performed with the mole-ratio method33 and with the method of continuous variations (Job's method).34

The mole-ratio determinations were made as follows: a solution of complex 11 (2.5´10-4 mol L-1) was prepared in a 4:1 (v:v) methanol:buffer MES (30´10-3 mol L-1; pH 6.2) mixture. A volume of 1 mL was transferred from this solution to a quartz cuvette sealed with a rubber septum. This sealed solution was bubbled with argon and the sample was placed in the UV-Vis apparatus, with the cell-compartment thermostated at 25 oC. A baseline was made with this initial solution in order to verify the appearance of the band at ca. 420 nm. Small aliquots of a FeCl3 stock solution (8.43´10-3 mol L-1) in methanol were then transferred to the cuvette with a microsyringe with intervals of five minutes between each addition. The mixture was stirred after each addition and the maximum in absorbance at 426 nm was read. The same experiment was performed with the titrations of 11 with FeCl3 in the mixture having pH 4.5 (buffer pyridine-HCl 30´10-3 mol L-1). The titrations of ligand 4 with FeCl3 were also made in a similar manner.

Job plots were performed for the complex formed with 11 and Fe3+. These studies were performed at 25 °C in 4:1 (v:v) methanol:buffer (30´10-3 mol L-1) mixture. The stock solutions of 11 and Fe3+ in the experiments at pH 6.2 had concentrations of 2.5 ´10-4 mol L-1. Two sets of experiments were made at pH 4.5, with stock solutions of 3.6´10-4 mol L-1 and 4.9´10-4 mol L-1. The absorbances were read at lmax equal to 426 nm.

EDTA competition experiments

Buffered stock solutions of FeCl3 (1.85´10-3 mol L-1), 11 (6.01´10-4 mol L-1) and EDTA (7.17´10-4 mol L-1) were prepared in a 4:1 (v:v) methanol:water mixture and the pH 4.5 was kept constant with pyridine (30´10-3 mol L-1). Ionic strength was also kept constant with the use of tetrabutylammonium tetrafluoroborate 0.1 mol L-1 (the use of KNO3 provoked the precipitation of the solutions after some hours of experiment). Other solutions were prepared having [Fe3+]=3.06´10-4 mol L-1; [EDTA]=0.58-3.48´10-4 mol L-1; [11]=2.11-4.23´10-4 mol L-1. These solutions were kept for one week at 25 °C in a thermostated bath to allow equilibration and their UV-Vis spectra were then taken. The molar absorptivities for complexes 11 and 12 at 426 nm and pH 4.5 were calculated as 1997 and 4012 L mol-1 cm-1 per Fe3+, respectively. Competition experiments took into account the following equilibrium (1),

whose equilibrium constant (Keq) can be calculated by means of equation (2).

Since 11 and 12 are the only iron-containing and only absorbing species, a, the fraction of the iron present as 12 complex, is given by equation (3),

A being the absorbance of the solution at 426 nm, c and e the molar concentration and molar absorptivity respectively at 426 nm for the species present in equilibrium. The subscripts 11 and 12 are related with complexes 11 and 12, respectively while Fe(EDTA)- refers to the complex formed with Fe3+ and EDTA. Since the solutions of Fe(EDTA)- are colorless at 426 nm, we considered eFe(EDTA-) equal to zero in the calculations. With the use of 1025.0 as the formation constant of Fe(EDTA)-,35 b1 could be averaged for the reaction represented by equation (4).

 

Results and Discussion

Synthesis of the ligands and the complexes

The 5,5'-disubstituted-2,2'-bipyridines were synthesized according to the synthetic routes described in Schemes 1 and 2. Ligands 4 and 6-10 are new compounds and were fully characterized.

The first reaction involved the coupling of b-picoline with the use of Raney-nickel, resulting in 5,5'-dimethyl-bipy (1).26,27 This compound was oxidized with potassium permanganate in aqueous solution (reflux for 16 h), resulting in the diacid 2 in good yield.28 The latter was transformed into the corresponding bis-acid chloride (3) with thionyl chloride during reflux29 in quantitative yield. Reaction of 3 with N-methylhydroxylamine yielded ligand 4 (85%).

 

 

The synthetic pathway shown in Scheme 2 gives access in good yield to non-symmetrical 5,5'-disubstituted 2,2'-bipys. Diazotation of 2-amino-5-methylpyridine and subsequent reaction with bromine in the presence of a concentrated solution of hydrobromic acid resulted in 5.30 Stannylation with n-butyl lithium and trimethyltin chloride36 yielded compound 6, which was then coupled in very good yield with ethyl 6-chloronicotinate in toluene through a modification of the literature procedure37 using [Pd(PPh3)4] as a catalyst23 to give the monoester 7. Hydrolysis of 7 with NaOH aqueous methanol gave the corresponding acid 8 almost quantitatively. The acid was refluxed with thionyl chloride to yield quantitatively the acyl chloride 9, which was reacted with N-methyl hydroxylamine to give ligand 10 in good yield (74%).

 

 

The Fe2+ complexes 11 and 14 of the bipy ligands 4 and 10 were obtained by stirring the ligand with FeCl2 in degassed water in the proportion metal:ligand 1:3.38

pKa values

A first question that emerges is whether the complexation of ligands 4 and 10 with Fe2+ affects the physicochemical properties of the N-methyl hydroxamic acid groups. If the metal ion causes, for instance, changes in the ionization constants of these groups, it will influence the capability of the complex formed to act as a metallo-exoreceptor. Therefore, pKa values of ligands 4 and 10 and their respective Fe2+ complexes 11 and 14a,b were obtained by potentiometric titrations (Table 1). For comparison, the pKa value for the N-methyl acetohydroxamic acid was determined under the same conditions, giving a value close to those obtained for the bipy ligands 4 and 10. The values determined for the corresponding Fe2+ complexes 11 and 14a,b show that the binding of the metal ion induces a significant change in the pKa of the hydroxamic acid group. Thus, the pKa values of 8.2 and 9.1 for ligand 4 decrease by about two units to 6.2 and 7.1, indicating the important role of the metal ion.

Self-assembly of a trimetallic complex

Along the lines presented in the Introduction, ligand 4 was first complexed by FeCl2 and the Fe2+-tris(bipyridine) complex formed (11) was titrated with a FeCl3 solution, according to Scheme 3, to yield complex 12. The formation of this trinuclear structure was followed by UV-Vis and EPR spectroscopies.

Complex 11 presents an absorption band at 550 nm due to metal to ligand charge transfer (MLCT). Addition of FeCl3 into a buffered solution (pH 6.2) of this complex leads to the appearance of a new band in the visible region of the spectrum. The color change is complete within a few minutes (ca. 4 minutes). This band, at 426 nm, is characteristic of the ligand to metal charge transfer in tris(hydroxamato)Fe3+ complexes.39 The molar absorptivity of 2864 L mol-1 cm-1 per Fe3+ at this pH agrees with the data from the literature20,39 and for the tris(hydroxamato)Fe3+ complex prepared under the same conditions from ligand 10 (lmax = 424 nm; emax = 3106 L mol-1 cm-1). A plot of absorbance at 426 nm as a function of added Fe3+ equivalents indicates a 1:2 11:Fe3+ ratio (Figure 1a).

 

 

According to the literature, the complexation of hydroxamic acids with Fe3+ in more acid pH values leads to the formation of mono- and bis(hydroxamato)Fe3+ complexes.39 This was confirmed when the complexation of 4 with Fe3+ was performed at pH 4.5 (methanol/water 4:1). The appearance of a band at 465 nm was observed (emax = 1882 L mol-1 cm-1), corresponding to the formation of bis(hydroxamato)Fe3+, in agreement with the literature.21,39 The addition of Fe3+ to a solution of complex 11 under the same conditions led also to the appearance of a band at ca. 420 nm (emax = 4012 L mol-1 cm-1 per Fe3+) and to the same stoichiometry 1:2 11:Fe3+ (Figure 1b).

Job plots of absorbance values at 426 nm both at pH 4.5 (pyridine buffer) and 6.2 (MES buffer) showed also a maximum absorbance for a 1:2 11:Fe3+ ratio (Figure 2). The data indicate the formation of tris(hydroxamato)Fe3+ under these conditions, in agreement with the fact that the complexation decreases the pKa values for the hydroxamic acid groups, making them available to form the tris(hydroxamato)Fe3+ complex after the first complexation with the Fe2+ ion. This result highlights the double role of the Fe2+ ion in the process, not only organizing the hydroxamic acid groups for the second complexation with the Fe3+ ion, but also inducing favorable conditions for this sequential binding in a hierarchical fashion.

 

 

 

 

The experiments also demonstrated that complex 11 is not stable at pH above 5.8 in the presence of oxygen. Under these conditions, the band at 550 decreases as a band develops at 426 nm, characteristic of tris(hydroxamato)Fe3+ species. The final spectrum presents the same pattern for complex 12 above. The addition of ascorbic acid to these solutions, in order to reduce the Fe3+ ion, caused the reappearance of the original band at 550 nm in complex 11. The addition of Fe3+ to the starting complex 11 in the ratio 1:2 11:Fe3+, however, prevents the oxidation of Fe2+ bound to the bipy units. These results agree with data from literature,40 since it has been well established that Fe2+ can be easily oxidized to Fe3+ in the presence of atmospheric oxygen, and that the rates of oxidation are highly dependent on pH and on the nature of the coordinating ligands.

These same conditions were also used to perform direct complexation of the hydroxamic acid groups of ligand 4 with Fe3+ (Scheme 4). Only a band in the visible region was observed (lmax = 426 nm; emax = 3046 L mol -1cm-1). Subsequent addition of Fe2+ led to the appearance of the band at 550 nm, corresponding to the formation of (bipy)3Fe2+, in agreement with the formation of the same trinuclear structure 12, independent of the sequence of metal ion addition.

 

 

Ligand competition experiments involving EDTA, complex 11, and Fe3+ were performed at pH 4.5 (according to equation 1). The equilibrium constant (Keq) for equation 1 was calculated from spectra of solutions in which EDTA competed with 11 for Fe3+. This value, Keq=8.31´10-9, represents the average of 6 values calculated at pH 4.5. The competition constant (Keq) and the formation constant of FeEDTA- were used35 to calculate of the formation constant of complex 11, giving a value of log b = 16.9.

Complex 12 was also studied by EPR spectroscopy. EPR spectra for this complex in solid state (second derivative mode) and in frozen solution (4:1 methanol:water; buffer MES 30´10-3 mol L-1, pH 6.2; 77 K) in first derivative mode provided further evidence for the proposed structure (Figure 3). A line showing g = 4.3, characteristic for high spin Fe3+ in a rhombic site with oxygenated ligands around the metal ion, was obtained. The spectrum for the second derivative mode suggests that there is only one type of coordination site for Fe3+ in the complex.

 

 

Figure 4 depicts the EPR spectrum for an experiment of sequential complexation using first Fe3+ and then Fe2+ ions, in a 4:1 methanol:water frozen mixture (buffer MES 30´10-3 mol L-1, pH 6.2). The shape of the spectrum is similar to that observed for complex 12. Figure 4 shows also the spectrum for the reaction between ligand 4 with only Fe3+ ions, which displays the same pattern as the other two spectra. The similarities among the three spectra suggest that the complexation of 4 with Fe3+ leads to a structure reminiscent of 12, i.e., the suggested structure 13. The same experiments were performed with solutions at pH 4.5 and gave the same results as those at pH 6.2, since this technique does not allow us to distinguish between bis- and tris(hydroxamate)Fe3+ complexes. Other considerations about the EPR spectra will be made below.

 

 

Self-assembly of bimetallic architectures

Ligand 10 is interesting as it explores the strategy of sequential complexation, since the complexation with Fe2+ and Fe3+ ions may yield in principle bimetallic architectures, with the added feature that a mixture of two isomers is expected if the complexation is performed with Fe2+ ions only. A 1H NMR study, in CD3OD-D2O (4:1), demonstrated the presence of signals corresponding to the methyl protons on the pyridine ring (d 2.23 and 2.49) and for the methyl protons from the hydroxamic acid groups (d 3.26, 3.27 and 3.43). The proportion of the two isomers, obtained by integration of the methyl signals, was 73% for 14a and 27% for 14b (Scheme 5).

If Fe3+ is added to the mixture of 14a and 14b, UV-Vis studies suggest the formation of a mixture containing tris(hydroxamato)Fe3+ (15a) and bis(hydroxamato)Fe3+ (15b), according to Scheme 5. A broad band in the visible region of the spectrum between 420 and 460 nm gives evidence for the mixture. No changes in the spectrum could be observed by heating at 40°C for several hours. It was not possible to follow complexation by 1H NMR because of signal broadening (due to the presence of complexed paramagnetic Fe3+), but no changes occurred in the region of methyl protons under complexation (the disappearance of the protons at d 2.49 and 3.43, that would characterize the transformation of the isomer 15b in 15a, was not observed). In addition, complexed Fe3+ was reduced with ascorbic acid on heating and the resulting 1H NMR spectrum was found to be the same as that of complex 14a,b, with no change in the proportion of the two isomers.

Sequential complexation performed by changing the order of addition of the metal ions (Scheme 6) should yield only one of the two possible isomers. With initial addition of Fe3+ followed by the complexation with Fe2+, the first metal ion would organize the ligands, acting as a template and forming an adequate cavity for Fe2+. Thereafter, reduction of complexed Fe3+ by ascorbic acid should lead to decomplexation from its site. This strategy was verified by UV-Vis, 1H NMR and EPR.

 

 

 

The UV-Vis results are depicted in Figure 5. When Fe3+ was added to the ligand solution (pH 6.2) in metal:ligand 1:3 ratio, the visible band at 424 nm, characteristic of the tris(hydroxamato)Fe3+ complex, was observed. Addition of Fe2+ in the same proportion led to the formation of the (bipy) Fe2+ complex, with increase in absorbance at 530 nm. Thereafter, reaction with ascorbic acid gave a decrease in the absorbance at 424 nm.

 

 

The same process was also followed by 1H NMR measurements (Figure 6) and revealed the transformation of the five signals from the methyl groups into only two signals, at d 2.21 and at 3.24. This is consistent with the structure of isomer 14a and corroborates the UV-Vis data and the strategy displayed in Scheme 6. The 1H NMR spectrum of the same sample taken 15 days after the first experiment, did not give any indication of isomerization.

Figure 7 depicts EPR spectra for sequential experiments with ligand 10. A sharp line was obtained for the entity involving only this ligand and Fe3+ (complex 16) in contrast to the broad lines observed for the Fe3+ complexes with ligand 4 (Figure 4). This line, with g = 4.3, is characteristic for high spin Fe3+ in a rhombic site, corresponding to the structure of a tris(hydroxamato)Fe3+ complex. Addition of Fe2+ into a solution containing 16 led to the broadening of the line in the EPR spectrum, similar in shape to that observed for complexes 12 and 13. A similar EPR spectrum was obtained for the mixture with complexes 15a and 15b (Scheme 5). Since these experiments are expected to yield complexes related to 12 and 13, they provide further evidence for the latter's structures. The broadening observed may be due to a distortion of the Fe3+ sites, which would not occur in complex 16. Efforts are being made to crystallize the complexes in order to compare their solid state structures to the proposed structures in solution.

 

 

Conclusions

The data described above illustrate the process of self-assembly through sequential complexation in the synthesis of bimetallic and trimetallic structures from the reaction of 2,2'-bipyridine ligands bearing hydroxamic acid groups in 5,5' positions with Fe2+ and Fe3+. In addition, the studies performed in this work allow the visualization of three important aspects: the free ligand by itself is not capable of performing functions such as recognition of substrates. On complexation around the metallic ion, the ligands are organized so as to generate two secondary complexation sites capable of binding metal ions or other substrates. Furthermore, binding of the metal ion also results in a lowering of the pKa values of the hydroxamic acids units. This interesting feature amounts to an activation of potential catalytic groups in a substrate binding pocket. It could make complexes 11 and 14a attractive as mimics of the enzymatic hydrolysis of compounds of biological interest, in mild conditions of pH. In addition, complexes such as 11 and 14a display features of siderophores reminiscent of those of iron carriers in living systems.41

Finally, from a broader point of view, the stepwise, hierarchical self-assembly through sequential binding of specific substrates allows the induction and control of growth processes leading to the generation of structurally organized and functionally integrated supramolecular devices.

 

Acknowledgments

A.S.M. thanks CNPq and V.G.M. is grateful for financial support from Capes, CNPq, PRONEX/Química/UFSC and UNISUL.

 

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Received: March 17, 2003
Published on the web: August 15, 2003

 

 

* email: lehn@isis.u-strasbg.fr
# Present address: Centro Tecnológico, GRUCENSO, Pró-Reitoria Acadêmica, Universidade do Sul de Santa Catarina, CP 370, 88704-900, Tubarão-SC, Brazil

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