Two Synthetic Approaches to Coinage Metal(I) Mesocates: Electrochemical versus Chemical Synthesis.

We report two different approaches to isolate neutral and cationic mesocate-type metallosupramolecular architectures derived from coinage monovalent ions. For this purpose, we use a thiocarbohydrazone ligand, H2L (1), conveniently tuned with bulky phosphine groups to stabilize the MI ions and prevent ligand crossing to achieve the selective formation of mesocates. The neutral complexes [Cu2(HL)2] (2), [Ag2(HL)2] (3), and [Au2(HL)2] (4) were prepared by an electrochemical method, while the cationic complexes [Cu2(H2L)2](PF6)2 (5), [Cu2(H2L)2](BF4)2 (6), [Ag2(H2L)2](PF6)2 (7), [Ag4(HL)2](NO3)2 (8), and [Au2(H2L)2]Cl2 (9) were obtained by using a metal salt as the precursor. All of the complexes are neutral or cationic dinuclear mesocates, except the silver nitrate derivative, which exhibits a tetranuclear cluster mesocate architecture. The crystal structures of the neutral and cationic copper(I), silver(I), and gold(I) complexes allow us to analyze the influence of synthetic methodology or the counterion role on both the micro- and macrostructures of the mesocates.

Introduction

In the recent years, a wide variety of metallosupramolecular architectures obtained through self-assembly processes between organic ligands and metal ions have been published, among which helicates and mesocates can be highlighted.[1−7]

Mesocates or helicates are composed of at least two organic strands and two metal ions. If the ligands adopt a twisted arrangement around the metal ions, homochiral racemic helicates are formed, whereas if the ligands coordinate to metal ions without crossing each other,[8] achiral mesocates are obtained. In a same manner, mesocates are complexes that could be seen as the midpoint of two helicates of opposite hand.

To date, supramolecular research has mainly focused on helicates because their simplicity has facilitated the study of inherent factors directing the self-assembly process and their similarity to the DNA double helix has made new approaches to potential metallodrugs possible.[9−12] In spite of this, mesocates must be considered as fascinating as helicates because they also exhibit high potential in different fields such as magnetism,[13−17] luminescent molecular sensors,[18−20] or pharmacology,[21−23] among others. For that reason, the development of synthetic routes to obtain mesocates on selective processes is of great interest nowadays and deserves to be investigated.

Since Albrecht and Kotila reported the first mesocate case[8] and established the well-known “odd–even rule” referring to the length of the spacer in the ligand, we and other authors have highlighted the difficulty in controlling the factors that allow the selective formation of mesocates or helicates.[24] In this context, different aspects such as the ligand design,[8,25,26] the nature of the metal ion,[24,27] the experimental conditions (solvent, temperature, etc.),[24] or the inclusion of guest molecules[20] have been investigated. All of these studies have mainly been focused on the ligand design and/or divalent metal ions.[8,25,27] In contrast, studies with MI coinage metal ions are scarce, and no routes for the isolation of metal(I) mesocates/helicates have been reported. Thus, only a few examples of copper(I),[18,26,28] silver(I),[29−31] and gold(I)[22] mesocates have been published to date.

Thiosemicarbazone ligands can be considered as one of the most versatile kernels in chemistry.[32] Through decades of intensive research, thousands of different thiosemicarbazone compounds have been achieved. The exhaustive research performed in thiosemicarbazones may be attributed to their versatility on coordination, their utility to form diverse heterocycles, and their proven biological activities, like antitumor, metastatic, and antibacterial, among many others.[33] Over the past few years, an increased interest in thiocarbohydrazone ligands, which may be considered as extended thiosemicarbazones, has emerged.[34] Thus, thiocarbohydrazones possess two more donor atoms in their skeleton compared to thiosemicarbazones and therefore could potentially form a wider variety of metallosupramolecular structures. Surprisingly, a reduced number of thiocarbohydrazone metal complexes has been reported to date.[34] Among them, grids[35,36] and mononuclear[37] and dinuclear[38] species have been described. Also, examples of silver(I) clusters derived from these types of ligands have been found.[39,40] In addition, no examples of donor NSP-thiocarbohydrazone ligands have been found in the literature.

Our research group has pioneered the application of an electrochemical procedure for the isolation of neutral metal complexes with singular supramolecular arrangements. This methodology, combined with the use of thiosemicarbazones as ligands, allowed us to isolate cluster helicates with monovalent metal ions, whereas lineal helicates or mesocates were assembled with divalent metal ions.[24,27,41−44]

Taking all of these considerations in mind, herein we report a double and efficient route focused on the preparation of neutral and ionic mesocates with monovalent coinage metal ions (Scheme ).

Scheme 1

Selective Isolation of Mesocates Presented in This Work

Our strategy is based on a conveniently functionalized thiocarbohydrazone strand. In this sense, we have designed the thiocarbohydrazone ligand H2L (1), which incorporates two phosphine groups (Figure ) that fit with the proposed requirements for the isolation of metal(I) mesocates. In this sense, ligand 1 is equipped with (i) two bulky triphenylphosphine binding domains that each contain a phosphorus soft donor atom to stabilize MI coinage ions and hinder crossing of the organic strands and (ii) a spacer containing a soft donor atom that may coordinate to the metal ions and at the same time prevent ligand crossing to favor the selective formation of mesocates.

Figure 1

Representation of ligand 1.

Results and Discussion

In this work, we have carried out the synthesis of both neutral and cationic copper(I), silver(I), and gold(I) mesocates (Scheme ) derived from the thiocarbohydrazone ligand 1 by using two different methodologies. Neutral complexes were obtained using an electrochemical procedure (2–4), whereas cationic mesocates (5–9) were isolated from different metallic salts like [Cu(CH3CN)4]PF6, [Cu(CH3CN)4]BF4, AgPF6, AgNO3, and H[AuCl4] (see the Experimental Section). The main objective was to study the influence of different factors such as the synthetic procedure, the counterion, and the MI ion size on the final stoichiometry and/or architecture of the complexes.

Scheme 2

Complexes 2–9 Synthesized in This Work

Thiocarbohydrazone Ligand H2L

The phosphinethiocarbohydrazone ligand 1 (Figure ) can be described as bicompartmental and potentially pentadentate [N2SP2]. 1 was obtained by the reaction of 2-diphenylphosphinobenzaldehyde and thiocarbohydrazide in a 2:1 ratio and fully characterized using a wide variety of techniques, as detailed in the Experimental Section and shown in Figures S1–S6.

Self-Assembly of Neutral Mesocates by Electrochemical Synthesis

The electrochemical methodology is a simple, efficient, and inexpensive technique that allows metallosupramolecular architectures to be obtained directly from redox processes that involve the oxidation of a free metal plate and the reduction of the precursor organic ligand (section 1). In addition, it is carried out at room temperature with pure reagents instead of metal salts, avoiding in many cases a possible competition between the anion and ligand during coordination to the metal ion.[45,46]

Electrochemical monooxidation of a metal plate (copper, silver, and gold) in a conducting acetonitrile (CH3CN) solution of ligand 1 afforded orange (copper and silver) or yellow (gold) solids, which were readily characterized. The analytical data and mass spectrometry (MS) spectra (Figure S7) for these solids are consistent with the formation of the neutral metal(I) dimeric complexes [M2(HL)2] (2–4), which arise from the monodeprotonation of ligands in solution. These formulations agree with the molar conductivity values of 2–10 μS·cm–1, typical for nonelectrolyte compounds [10–3 M N,N-dimethylformamide (DMF) solutions].[47] The solids were also characterized by IR, 1H and 31P NMR, and UV–vis spectroscopy studies (Figures S8–S10 and Table S1).

The three neutral complexes share some similar features in the IR spectra. Thus, coordination of the ligand to the metal ions leads to a displacement on the vibrational bands to larger wavelengths compared to the free ligand (Figure S8), indicating coordination of the ligand through the imine nitrogen and sulfur atoms.

To study the properties of the neutral complexes in solution, we performed 1H and 31P NMR experiments at room temperature using DMSO-d6 as the solvent. The 1H NMR spectra of these compounds generally show a displacement of the signals to low field with respect to the free ligand and a broadening of the aromatic signals (Figure S9). This effect can be attributed to coordination of the ligand to the MI metal centers (M = Cu, Ag, and Au). The 31P NMR spectra of the complexes exhibit a displacement of the signals to low field with respect to the free ligand, which confirms coordination of the phosphorus atom to the metal ions (Figure S10). It should be highlighted that in the case of the silver(I) complex 3, a doublet appears at 6.19 ppm because of the 107Ag–31P coupling. The value of the coupling constant in this case (J = 364.1 Hz) indicates that two phosphorus atoms are coordinated to each metal ion.[48] Also, in gold(I) complex 4, a single singlet appears at 34.57 ppm, showing that in solution the four phosphorus atoms are equivalent.

X-ray Structures of Neutral Mesocates

Slow evaporation of the mother liquors from the syntheses of 2 and 3 or recrystallization in chloroform/hexane of solid 4 allowed us to obtain orange crystals suitable for X-ray diffraction studies. The structures revealed the formation of neutral dinuclear mesocates of [Cu2(HL)2]·3.5CH3CN (2*; Figure ), [Ag2(HL)2]·4CH3CN (3*; Figure ), and [Au2(HL)2]·8CHCl3 (4*; Figure ) stoichiometries. Selected crystal data are collected in the Supporting Information. Relevant bond lengths and angles for these structures are compiled in Tables S2–S4.

Figure 2

Crystal structure of the copper(I) mesocate 2*.

Figure 3

Crystal structure of the silver(I) mesocate 3*.

Figure 4

Crystal structure of the gold(I) mesocate 4*.

Every mesocate unit is composed of two monoanionic bridging ligands [HL]−. In the case of the copper and silver mesocates, the metal ions are coordinated to the imine nitrogen, phosphorus, and central thioamide sulfur atoms of one ligand strand, completing tetracoordination with the phosphorus atom of the second ligand unit, thus generating a [P2NS] tetrahedral distorted environment.

In the gold mesocate 4*, each gold ion is bound to the phosphorus and central thioamide sulfur atoms of one ligand strand and the phosphorus atom of the second ligand unit, exhibiting a [P2S] trigonal-planar distorted kernel. However, a weak interaction with the imine nitrogen atom (Au1–N1, 2.65 Å) cannot be ruled out.[49]

These coordination modes result in 18-membered metallomacrocyclic rings for each complex with dimensions of ca. 10.2 × 3.2 Å for copper, 9.1 × 3.1 Å for silver, and 10.0 × 3.6 Å for gold complexes (Figures S11–S13). The intradinuclear M–M distances are 8.475, 6.312, and 9.047 Å for copper, silver, and gold complexes, respectively, which precludes metal–metal interactions.

The assembly of neutral mesocates confirms that the two bulky phosphine groups in ligand 1 avoid crossing of the ligand threads and ensures the formation of mesocates instead of helicates. Moreover, the mesocate arrangement of the ligand maximizes the number of weak intramolecular interactions of the types of CH−π, hydrogen-bonding, and agostic contacts (Figures and S14–S16),[49,50] thus contributing to the mesocate assembly process.

Figure 5

Intramolecular agostic interactions (CH60···Cu1 3.02 Å, CH74···Cu1 2.89 Å, CH21···Cu2 2.89 Å, and CH33···Cu2 3.01 Å) in 2*.

In addition, the ligand incorporates the central sulfur donor atom in one of the PN binding domains, acting as PNS/PN for one of the metal ions and monodentate P for the second one. The behavior of the sulfur atom as a monodentate donor also favors the mesohelical arrangement because a M–S–M bridging behavior would lead to the formation of cluster metal(I) complexes, as was found before.[40,51]

On the other side, the electrochemical synthetic procedure plays a key role in mesocates formation because it allows precise control of the electrochemical conditions to achieve monodeprotonation of the ligand. This control refers to the reaction time that relates to the metal oxidation state and deprotonation degree in the ligand. In the herein-exposed case, bideprotonation of the ligand would presumably result in tetranuclear copper(I) cage assembly or oxidation to copper(II) complexes, as reported by Dragancea and coauthors.[52] In order to confirm this prediction, we performed electrochemical synthesis of the complexes in bideprotonation conditions. The compounds isolated correspond to M4L2 species, as indicated by elemental analysis, IR spectroscopy, and MS (the spectra of Cu4L2 are shown as examples in Figures S17 and S18).

Self-Assembly of the Cationic Mesocates

Complexes 5–9 were synthesized by the reaction of 1 with the corresponding metallic salt (in 1:1 ratio): 5 from [Cu(CH3CN)4]PF6, 6 from [Cu(CH3CN)4]BF4, 7 from AgFP6, 8 from AgNO3, and 9 from reduced [H(AuCl4)]. They were readily characterized by different techniques (see the Experimental Section and Figures S19–S27). Characterization data and MS spectra allowed us to propose dicationic dinuclear species [M2(H2L)2]2+ involving the neutral ligand in the case of compounds 5–7 and 9 and a dicationic tetranuclear stoichiometry [Ag4(HL)2]2+ for compound 8, being in this case the ligand acting in a monoanionic mode. These formulations are in agreement with the measured molar conductivity values, in the range of 133–156 mS cm–1, typical for 1:2 electrolyte compounds (10–3 M DMF solutions).[47] The solids were also characterized by IR, 1H NMR, and UV–vis, obtaining a pattern similar to that found in neutral mesocates. It should be highlighted that, in the IR spectra of complexes 5–8, the characteristic bands corresponding to the counterions (PF6–, BF4–, and NO3–) can be clearly identified (Figures S19–S22). It is also remarkable that in the MS spectra of the silver complexes a fragment containing the counterion {Ag2(H2L)2]PF6}+ can be observed for 7 (Figure S23) and the tetranuclear signal [Ag4(HL)2-H]+ for the cluster 8 (Figure S24).

X-ray Structures

Slow evaporation of the mother liquors resulting from the synthesis of compounds 5–9 allowed us to obtain suitable crystals from which the molecular structure was determined by X-ray crystallography. The main crystal data are collected in the Supporting Information. Selected bond lengths and angles for these structures are collected in Tables S5–S9. In all cases, the bond distances M–S, M–N, and M–P (M = CuI, AgI, and AuI) are in the range expected for complexes derived from thiocarbohydrazone ligands.[37,39]

The crystal structures revealed that [Cu2(H2L)2](PF6)2·CH3CN·2H2O (5*), [Cu2(H2L)2](BF4)2·5CH3CN (6*), [Ag2(H2L)2](PF6)2·6CH3CN (7*), and [Au2(H2L)2]Cl2·6.2CH3OH (9*) consist of discrete dicationic dinuclear mesocates [M2(H2L)2]2+ structurally similar to those obtained by electrochemical synthesis (2*–4*). In the case of the silver complex prepared with silver nitrate, a dicationic tetranuclear silver cluster mesocate [Ag4(HL)2](NO3)2·4CH3OH (8*) was isolated, thus confirming the singular stoichiometry found for the solid 8.

Analyzing the structures by metal ion, the copper complexes (5* and 6*; Figures S27 and S28) give rise to mesohelical architectures similar to those isolated by electrochemical synthesis (Figure ), where copper atoms are coordinated to a sulfur atom, an imine nitrogen atom, and a phosphorus atom of one ligand and a phosphorus atom of another ligand site, giving a [P2NS] tetrahedral distorted environment (Tables S5 and S6).

In the case of the cationic silver complexes, we have obtained two different architectures: 7* (Figure ) and 8* (Figure ). Compound 7* (Figure ) exhibits two silver atoms coordinated to the thioamide sulfur atom and the phosphorus atom of one ligand site and the phosphorus atom of another ligand site, giving a [P2S] distorted trigonal-planar environment (Table S7). We must highlight that the coordination mode is different compared to the neutral silver mesocate obtained by an electrochemical procedure, where we have observed a [P2NS] distorted tetrahedral environment (Figure ). Therefore, we can conclude that the methodology does not affect the global mesohelical structure but does affect the microstructure of both silver(I) mesocates.

Figure 6

Crystal structure of the dicationic silver(I) mesocate 7*.

Figure 7

Crystal structure of the tetranuclear silver(I) cluster 8* (above). Counterions and hydrogen atoms have been omitted for clarity. Cluster core representation in 8* (below).

Nevertheless, the structure of the silver nitrate compound 8* (Figure ) is a dicationic tetranuclear silver complex where the ligands are coordinated in its monoanionic form [HL]− to silver metal ions without crossing each other. Also, 8* exhibits Ag–Ag bonds, giving rise to a cluster mesocate structure.

In this structure, Ag1 and Ag3 atoms are bound to the imine and thioamide nitrogen atoms, to the phosphorus atom of one ligand thread, and to the sulfur atom of the second ligand site. Furthermore, each metal ion is bound to another metal ion, assuming a [PN2SAg] distorted square-pyramidal environment, whereas metal ions Ag2 and Ag4 assume a [PNSAg] tetrahedral distorted environment (Table S8).

Each sulfur atom acts as μ2-S–Ag. The distance between the pairs Ag1–Ag2 (3.325 Å) and Ag3–Ag4 (3.140 Å), although larger than the metallic silver bond (2.889 Å),[53] is lower than the sum of the van der Waals radii for both silver atoms (3.44 Å).[54] Thus, the existence of argentophilic interactions can be considered.[55,56] We must remark herein that two named cluster mesocates, M2(L4)3I2 (M = CuI and AuI), were published before.[28] However, after careful analysis of these examples, they did not show metal–metal interactions (M–M distances of 12.00–12.12 Å). For that reason, to the best of our knowledge, this is the first example of a real cluster mesocate with coinage metal ions.

Bond distances Ag–S are in the expected range, giving rise to an asymmetric bridge. Bond distances Ag–N are also in the expected range, being larger than those found in the literature.[24] The phosphorus atoms are oriented, avoiding unfavorable steric interactions (Figure ).

Analysis of the two silver(I) structures obtained from silver(I) salts demonstrates that the ability of the counterion to deprotonate the ligand determines the resulting nuclearity of the cationic silver mesocates: a dinuclear mesocate was obtained in the case of the PF6– salt, whereas a tetranuclear mesocate was assembled when the counterion was NO3–. In addition, in the case of dinuclear silver mesocates (neutral 3* and cationic 7*), we can establish that the methodology affects the microstructure because we observe two different coordination environments in these two complexes. In addition, the presence/absence of a counterion depending on the synthetic methodology employed is also relevant for the final nuclearity of the mesocate. Thus, we have observed that, although the ligand acts as monodeprotonated in the neutral silver complex 3* and the cationic silver complex 8*, 3* shows a dinuclear architecture, whereas 8* derived from nitrate salt presents a tetranuclear cluster structure.

In the case of gold, the chemical synthesis was performed with a chloride precursor, giving rise to the crystalline dinuclear mesocate 9* (Figure ), where each metal ion is coordinated to a thioamide sulfur and one phosphorus atom of the ligand site and a phosphorus atom of another ligand, giving a [P2S] trigonal-planar distorted environment (Table S9).

Figure 8

Crystal structure of the dicationic gold(I) mesocate 9*. Counterions and hydrogen atoms have been omitted for clarity.

Furthermore, similar to neutral mesocates (2*–4*), weak agostic interactions are established between the C–H protons of the phenyl phosphines and the MI ions (CH35···Cu1 2.72 Å in complex 5*; CH29···Cu1 2.86 Å in complex 6*; CH29···Ag1 2.99 Å in complex 7*; CH35···Au1 3.00 Å in complex 9*).

Similar to those mesocates obtained by electrochemical synthesis (2*–4*), phosphine groups exhibit an anti conformation to avoid unfavorable steric interactions, resulting in the formation of 20-membered metallomacrocycles in the case of copper(I) mesocates (5* and 6*), while in the case of the silver(I) mesocate 7* (Figure ) and gold(I) mesocate 9*, 28-membered metallomacrocycles were formed.

Figure 9

Metallomacrocycle ring featured in 7*.

The distance between metal ions is large for all ionic dinuclear mesocates [Cu1–Cu2 6.093 Å (5*); Cu1–Cu1i 6.389 Å (6*); Ag1–Ag1i 6.566 Å (7*); Au1–Au1i 6.704 Å (9*)] so that metallophilic interactions are excluded (∼2.8–3.4 Å).[54] These distances are significantly smaller than those found in neutral mesocates for the copper(I) and gold(I) derivatives and on the same order as the case of the silver(I) complex.

Conclusions

In this work, we have presented a feasible synthetic double approach to mesocates using a diphosphinethiocarbohydrazone ligand. The introduction of two phosphorus atoms in the ligand donor set ensures stabilization of the MI coinage metal ions. In parallel, the presence in the ligand of the two bulky phosphines avoids crossing of the ligand threads, giving rise to the assembly of mesocates instead of helicates.

The electrochemical methodology allowed us to obtain dinuclear neutral mesocates, [M2(HL)2], whereas cationic dinuclear mesocates [M2(H2L)2]X2 were obtained if we used coinage salts. In the case of silver(I), two different structures were isolated, a tetranuclear mesocate, [Ag4(HL)2]X2, with a NO3– counterion and a dinuclear mesocate, [Ag2(H2L)2]X2, with X = PF6–, thus demonstrating that the counterion influences the nuclearity of the cationic mesocates.

Analysis of the crystal structures shows that it is possible to isolate mesocate species independently of the monovalent metal ion used.

Overall, the reported results demonstrated once again the importance of the ligand design in the selective obtainment of metallosupramolecular architectures.

Experimental Section

Materials and Methods

Thiocarbohydrazide, 2-diphenylphosphinobenzaldehyde, tetrakis(acetonitrile)copper(I) hexafluorophosphate, tetrakis(acetonitrile)copper(I) tetrafluoroborate, silver hexafluorophosphate, silver nitrate, tetrachloroauric(III) acid salts, copper, silver, and gold plates, and all solvents were purchased from commercial sources and used without any purification. Melting points were determined using a Buchi 560 instrument. Elemental analysis of the compounds (C, H, N, and S) was performed with a Fisons EA model 1108 analyzer. Positive-ion electrospray ionization (ESI+) MS data were registered using a Bruker Microtof mass spectrometer. A Varian Mercury 300 spectrometer was employed to record the 1H NMR spectra operating at room temperature using DMSO-d6 or CD3CN as the deuterated solvent. Variable-temperature 1H NMR experiments in deuterated acetone and 13C and 31P NMR were performed on an Bruker Agilent AVIII-500. Chemical shifts are reported as δ (ppm). IR spectra were recorded from 400 to 4000 cm–1 on a Bruker FT-MIR VERTEX 70 V spectrophotometer using KBr pellets. A Crison micro CM 2200 conductivity meter was used to measure the conductivity values from 10–3 M solutions in DMF at room temperature. UV–vis absorption spectra were recorded from solutions of ca. 10–5 M in acetonitrile at room temperature using a Jasco UV–vis spectrophotometer.

Thiocarbohydrazone Ligand H2L (1)

A total of 0.93 g (3.2 mmol) of 2-diphenylphosphinobenzaldehyde and 0.17 g (1.6 mmol) of thiocarbohydrazide were mixed and dissolved in absolute ethanol (50 mL). Then a catalytic amount of p-toluensulfonic acid was added to promote iminic condensation. The reaction mixture was refluxed for 3 h using a Dean–Stark trap to remove the released water. The resulting solution was cooled to 4 °C until the formation of a yellow product was observed. This solid was filtered off and washed with diethyl ether. Yield: 0.96 g (92%). Mp: 195–200 °C. Elem anal. Found: C, 71.2; H, 5.0; N, 8.5; S, 4.6. Calcd for C39H32N4P2S: C, 71.9; H, 5.0; N, 8.6; S, 4.9. ESI+ MS: m/z 651.2 ([H2L + H]+), 667.2 ([H2L(O) + H]). 1H NMR (500 MHz, acetone-d6, 278 K): δ 11.52 (s, 1H, H1), 11.01 (s, 1H, H1), 9.21 (d, J = 3.5 Hz, 1H, H2), 8.65 (d, J = 3.5 Hz, 1H, H2), 8.26 (m, 1H, H3), 7.95 (m, 1H, H3), 7.22 (t, J = 7.0 Hz, 4H, H4 + H5), 7.49 (m, 14H, HAr), 7.18 (t, J = 7.0 Hz, 4H, HAr), 6.85 (m, 2H, H6). 13C/DEPT NMR (500 MHz, DMSO-d6): δ 175.35 (C=S), 136.11 (C=N), 136.04 (C=N), 133.98–129.34 (CHAr). 31P NMR (500 MHz, DMSO-d6): δ −10.15 (PIII), −14.69 (PIII). IR (KBr, cm–1): ν(N–H) 3138, ν(C–H) 2915, ν(C=N + C–N) 1585, 1522, 1477, 1432, ν(C=S) 1142, 745, 686. UV–vis (λmax, nm): 276, 332.

Neutral Metal Complexes

The copper(I), silver(I), and gold(I) neutral complexes were prepared by using an electrochemical procedure. The electrochemical cell can be summarized as . As an example, the synthetic procedure used for the isolated complex [Ag2(HL)2] 3 is as follows:

A total of 0.1 g of 1 (0.154 mmol) was dissolved in acetonitrile (75 mL), and a small amount of tetraethylammonium perchlorate was added to the media as a supporting electrolyte. The resulting solution was electrolyzed at 5 mA and 5 V at room temperature for 50 min, and the orange solid obtained was isolated by filtration, washed with diethyl ether, and dried under vacuum. Electronic efficiency Ef = 1.0 mol F–1. Orange crystals suitable for X-ray diffraction studies of [Ag2(HL)2]·2CH3CN (3*) were obtained from the mother liquors of the synthesis.

The same procedure was followed for the synthesis of copper(I) mesocate 2 (5 mA and 9.5 V for 50 min; Ef = 1.1 mol F–1) and gold(I) mesocate 4 (5 mA and 9.5 V for 50 min; Ef = 0.9 mol F–1).

The proposed mechanism for their formation involves one electron for each metal atom as follows:

[Cu2(HL)2] (2)

Yield: 0.092 g (84%) of orange solid. The mp decomposes at 225 °C. Elem anal. Found: C, 65.2; H, 4.5; N, 8.0; S, 4.2. Calcd for C78H62N8P4S2Cu2: C, 65.8; H, 4.2; N, 7.9; S, 4.5. MALDI-TOF MS: m/z 713.1 ([Cu(HL) + H]+). 1H NMR (300 MHz, DMSO-d6): δ 11.78 (s, 1H, H1), 9.76 (s, 1H, H1), 8.56 (s, 2H, H2), 8.32–6.19 (m, HAr). 31P NMR (300 MHz, DMSO-d6): δ 2.62, −1.71. IR (KBr, cm–1): ν(O–H + N–H) 3438 (f), ν(C–H) 3053 (d), ν(C=N + C–N) 1630 (d), 1500 (m), 1477 (f), 1435 (mf), ν(C=S) 1095 (m), 746 (m). ΛM (μS cm–1): 4.0. UV–vis (λmax, nm): 358. Orange X-ray-quality crystals of [Cu2(HL)2]·3.5CH3CN (2*) were collected after filtration of the initial precipitate obtained during the synthesis, followed by slow evaporation of the mother liquors.

[Ag2(HL)2] (3)

Yield: 0.090 g (75%) of orange solid. The mp decomposes at 228 °C. Elem anal. Found: C, 61.5; H, 3.8; N, 7.3; S, 4.0. Calcd for C78H62N8P4S2Ag2: C, 61.9; H, 4.0; N, 7.4; S, 4.2. MALDI-TOF MS: m/z 757.0 ([Ag(HL) + H]+), 865.0 ([Ag2(HL)]+), 1515.0 ([Ag2(HL)2 + H]+). 1H NMR (300 MHz, DMSO-d6): δ 10.45 (s, 1H, H1), 9.04 (s, 1H, H1), 8.29 (s, 2H, H2), 7.99–6.58 (m, HAr). 31P NMR (300 MHz, DMSO-d6): δ 6.19 (J = 364.1 Hz). IR (KBr, cm–1): ν(O–H + N–H) 3438 (mf), ν(C–H) 3053 (d), ν(C=N + C–N) 1631 (m), 1459 (d), 1435 (f), ν(C=S) 1095 (m), 746 (d). ΛM (μS cm–1): 2.4. UV–vis (λmax, nm): 338. Yellow crystals suitable for X-ray diffraction studies of [Ag2(HL)2]·4CH3CN (3*) were obtained from the mother liquors of the synthesis.

[Au2(HL)2] (4)

Yield: 0.106 g (81%) of yellow solid. The mp decomposes at 228 °C. Elem anal. Found: C, 54.9; N, 6.7; H, 3.6; S, 3.6. Calcd for C78H62N8P4S2Au2: C, 55.4; N, 6.6; H, 3.6; S, 3.8. ESI+ MS: m/z 847.1 ([Au(HL) + H]+), 1693.3 ([Au2(HL)2]+). 1H NMR (300 MHz, DMSO-d6): δ 9.70 (s, 2H, H1), 9.02 (s, 2H, H1), 8.31 (s, 2H, H2), 7.89–6.52 (m, HAr). 31P NMR (300 MHz, DMSO-d6): δ 34.57. IR (KBr, cm–1): ν(O–H + N–H) 3435 (mf), 3053 (d), ν(C–H) 2924 (d), ν(C=N + C–N) 1630 (m), 1510 (d), 1460 (f), 1435 (f), ν(C=S) 1097 (m), 748 (d). ΛM (μS cm–1): 9.9. UV–vis (λmax, nm): 358, 408. Yellow crystals suitable for X-ray diffraction studies of [Au2(HL)2]·8CHCl3·C6H14 (4*) were obtained from recrystallization of the solid in a mixture of chloroform/hexane.

Cationic Metal Complexes

Cationic metal complexes derived from copper(I), silver(I), and gold(I) salts were synthesized by the same procedure using acetonitrile as the solvent in PF6– and BF4– salts and methanol in the case of NO3– and Cl– salts. As an example, the synthetic procedure of complex [Cu2(H2L)2](PF6)2 (5) is summarized as follows: A total of 0.05 g of 1 (0.08 mmol) and 0.028 g of [Cu(CH3CN)4]PF6 (0.08 mmol) were mixed and dissolved in acetonitrile (50 mL). The resulting orange solution was refluxed for 3 h. Afterward, it was concentrated to a small volume (20 mL) and cooled overnight to 4 °C. The orange solid obtained was filtered off and washed with diethyl ether.

[Cu2(H2L)2](PF6)2 (5)

Yield: 0.106 g (78%) of orange solid. Mp: 265 °C. Elem anal. Found: C, 52.7; H, 3.9; N, 6.2; S, 3.6. Calcd for C78H64N8P6S2F12Cu2: C, 54.5; H, 3.8; N, 6.5; S, 3.7. ESI+ MS: m/z: 713.1 ([Cu(H2L)]+), 777.1 ([Cu2(H2L) – H]+), 1427.2 ([Cu2(H2L)2 – H]+). IR (KBr, cm–1): ν(NH) 3262, ν(C=N + C–N) 1585, 1545, 1479, ν(C=S) 1095, 748, ν(PF6) 845. ΛM (μS cm–1): 138. UV–vis (λmax, nm): 346. Yellow X-ray-quality crystals of [Cu2(H2L)2](PF6)2·CH3CN·2H2O (5*) were collected after filtration of the initial precipitate obtained during the synthesis, followed by slow evaporation of the mother liquors.

[Cu2(H2L)2](BF4)2 (6)

Yield: 0.092 g (81%) of orange solid. Mp: 205 °C. Elem anal. Found: C, 57.3; H, 3.9; N, 6.7; S, 3.9. Calcd for C78H64N8P4S2B2F8Cu2: C, 58.5; H, 4.0; N, 7.0; S, 4.0. ESI+ MS: m/z 713.1 ([Cu(H2L)]+), 777.0 ([Cu2(H2L) – H]+), 1427.2 ([Cu2(H2L)2 – H]+). 1H NMR (300 MHz, CD3CN): δ 10.41 (s, 2H), 8.52 (s, 2H), 6.93 (s, 2H), 7.6–6.2 (HAr). IR (KBr, cm–1): ν(NH) 3259, ν(C=N + C–N) 1631, 1541, 1435, ν(C=S) 1122, 750, ν(BF4) 1084. ΛM (μS cm–1): 134. UV–vis (λmax, nm): 338. Orange X-ray-quality crystals of [Cu2(H2L)2](BF4)2·5CH3CN (6*) were grown by slow evaporation of the mother liquors from the synthesis.

[Ag2(H2L)2](PF6)2 (7)

Yield: 0.114 g (79%) of yellow solid. Mp: 225 °C. Elem anal. Found: C, 48.3; H, 3.1; N, 5.8; S, 3.2. Calcd for C78H64N8P6S2F12Ag2: C, 46.3; H, 3.2; N, 5.5; S, 3.2. ESI+ MS: m/z: 759.1 ([Ag(H2L)]+), 865.0 ([Ag2(H2L) – H]+), 1515.2 ([Ag2(H2L)2 – H]+), 1661.1 ({[Ag2(H2L)2]PF6}+). 1H NMR (300 MHz, CD3CN-d3): δ 9.79 (s, 2H), 8.66 (s, 2H), 7.68 (s, 2H), 6.94 (s, 2H), 7.8–6.4 (HAr). IR (KBr, cm–1): ν(NH) 3258, ν(C=N + C–N) 1585, 1537, 1479, 1435, ν(C=S) 1095, 746, ν(PF6) 843. ΛM (μS cm–1): 133. UV–vis (λmax, nm): 344. Yellow X-ray-quality crystals of [Ag2(H2L)2](PF6)2·6CH3CN (7*) were grown by slow evaporation of the mother liquors from the synthesis.

[Ag4(HL)2](NO3)2 (8)

Yield: 0.059 g (87%) of yellow solid. Mp: 205–210 °C. Elem anal. Found: C, 50.6; H, 3.7; N, 7.9; S, 3.4. Calcd for C78H62O6N10P4S2Ag4: C, 50.5; H, 3.4; N, 7.6; S, 3.5. ESI+ MS: m/z 865.0 ([Ag2(HL)]+), 1728.0 ([Ag4(HL)2 – H]+). 1H NMR (300 MHz, CD3CN): δ 10.02 (s, 1H), 8.84 (s, 1H), 8.25 (s, 2H), 8.15 (s, 2H), 7.8–6.3 (HAr). IR (KBr, cm–1): ν(NH) 3262, ν(C=N + C–N) 1533, 1479, 1464, 1435, ν(N–O) 1385, ν(C=S) 1096, 748, ν(N–N) 1029. ΛM (μS cm–1): 156. UV–vis (λmax, nm): 342. Colorless crystals suitable for X-ray diffraction studies of [Ag4(HL)2](NO3)2·4CH3OH (8*) were obtained from the mother liquors of the synthesis.

[Au2(H2L)2]Cl2 (9)

Yield: 0.081 g (78%) of yellow solid. Mp: 212 °C. Elem anal. Found: C, 53.0; H, 3.4; N, 6.2; S, 3.5. Calcd for Au2C78H64N8P4S2Cl2: C, 53.0; H, 3.8; N, 6.3; S, 3.6. ESI+ MS: m/z 847.2 ([Au(H2L)]+), 1043.1 ([Au2(H2L)]+), 1693.9 ([Au2(H2L)2 – H]+). IR (KBr, cm–1): ν(NH) 3251, ν(C=N + C–N) 1608, 1531, 1432, ν(C=S) 1117, 748. ΛM (μS cm–1): 135. UV–vis (λmax, nm): 350. Yellow crystals suitable for X-ray diffraction studies of [Au2(H2L)2]Cl2·6.2CH3OH (9*) were obtained from the mother liquors of the synthesis.