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. 2017 Oct 30;7:14347. doi: 10.1038/s41598-017-14728-8

DHPA-Containing Cobalt-Based Redox Metal-Organic Cyclohelicates as Enzymatic Molecular Flasks for Light-Driven H2 Production

Liang Zhao 1, Jian Wang 1, Pengyan Wu 1, Cheng He 1, Xiangyang Guo 1, Chunying Duan 1,✉
PMCID: PMC5662590  PMID: 29085048

Abstract

The supramolecular assembly of predesigned organic and inorganic building blocks is an excellent tool for constructing well-defined nanosized molecular cavities that catalyse specific chemical transformations. By incorporating a reduced nicotinamide adenine dinucleotide (NADH) mimic within the ligand backbone, a redox-active cobalt-based macrocycle was developed as a redox vehicle for the construction of an artificial photosynthesis (AP) system. The cyclohelicate can encapsulate fluorescein within its cavity for light-driven H2 evolution, with the turnover number (TON) and turnover frequency (TOF) reaching 400 and 100 moles H2 per mole redox catalyst per hour, respectively. Control experiments demonstrated that the reactions were potentially occurred within the cavity of the cyclohelicates which were inhibited in the presence of adenosine triphosphate (ATP), and the redox-active NADH mimic dihydropyridine amido moieties within the ligands played an important role in photocatalytic proton reduction process.

Introduction

Metal-organic macrocycles represent a unique class of functional molecular containers that display interesting recognition properties and fascinating reactivity similar to natural enzymes1,2. The architectures generating well-defined cavities provided specific inner environments for the selective bonding of guest molecules and catalysing their reactions3,4. Inspired by the pocket feature of natural enzymes, functional coordination cages with various structures and catalytic activities have been developed to achieve the excellent catalytic ability of natural enzymes5–7. However, few Werner-type capsules have been used as mimics of highly evolved and finely tuned molecular photosynthetic systems8,9, despite their importance in living systems and sustainable solar energy conversion10–12. As artificial photosynthesis (AP) systems always involve a photosensitizer for light absorption, a catalyst for H2 generation, and an electron donor13,14, the intrinsic difficulties in mimicking photosynthetic systems include the feasibility of processing in an aqueous solution and a well-defined cavity to bring the proton reduction centre and photosensitizer closer together15,16. Most importantly, metal-organic nanocages should comprise at least one of the two basic functional units that exhibit redox activity and/or light-harvesting ability for the possible construction of highly efficient and easily operated supramolecular AP systems17,18.

Reduced nicotinamide adenine dinucleotide (NADH) plays an important role in the reduction-oxidation metabolism of some most important coenzymes found in living cells19–21. The dihydropyridine amido (DHPA) group is described as the key structure in NADH models22 and an important part in electron transfer. Therefore, the incorporation of a DHPA group into the ligand backbone as the active site should be a powerful approach to mimic the activity of these enzymes i.e., the cofactor in [FeFe]-hydrogenase that controls the redox levels by sharing the effect of electron gain, loss and distribution23–25.

Through modulation of tridentate N2O units containing amide groups on a central dihydropyridine ring at the meta sites (Fig. 1), we developed new cobalt-based redox-active helical triangles to encapsulate a photosensitizer for light-driven H2 production. We reasoned that the amide groups in the positively charged cages matched the functional requirements and could offer hydrogen bonding interactions for the recognition of fluorescein (Fl). The confinement of the cavity possibly enforced the proximity between the redox-active cobalt(II) centres and Fl, enhancing the PET efficiency to avoid unwanted energy transfer or reverse-ET reactions26,27. The mild redox couple of DHPA close to the H2/H+ couple and the geometric position of DHPA close to the redox catalyst centre made this supramolecular system a more complete working model of AP systems28,29. Control experiments based on the reference compound that has the similar structural feature and almost same coordination geometries, as well as redox potential with that of the original, but without the DHPA fragments were also carried out for a comparison.

Figure 1.

Figure 1

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Perspective view of the supramolecular structure of the AP system for light-driven H2 production, showing the construction of the nanocage host as a proton reductive catalyst and the encapsulation of Fl guest as a photocatalyst.

Results and Discussion

The ligand H2 ZPB contianing two tridentate coordinated units was obtained from the reaction of 2-pyridyl aldehyde with malono-hydrazide in an ethanol solution. Evaporating a solution containing equivalent molar ratios of H2 ZPB and Co(NO3)2·6H2O in the presence of NaClO4 for several days led to the formation of the compound Co–ZPB. ESI-MS spectrum of the formed Co–ZPB solid exhibited intense peaks at m/z = 947.19 and m/z = 996.66, with the isotopic distribution patterns separated by 0.50 ± 0.01 Da, and a comparison with the simulation results based on natural isotopic abundances suggested that these peaks are assigned to [Co3(HZPB)3·ClO4]2+ and [Co3(HZPB)2(H2 ZPB) ·2ClO4]2+, respectively, indicating the successful assembly of a Co-based M3L3 molecular macrocycle (Fig. 2a). Tridentate (N2O) coordinated units sharing two five-membered chelating rings are one kind of efficient building blocks that have been widely used to construct stable and functional discrete architectures with regular structure and high symmetry30,31. According to our previous work, each of three cobalt centres typically coordinated with two planar tridentate N2O chelators to form a mer configuration molecular macrocycle with considerable stabilities. In the presence of Fl, the ESI-MS spectrum of Co–ZPB exhibited a new peak at m/z = 1112.22 that was assigned to [Co3(HZPB)3·ClO4 ⊃ Fl]2+ through comparison with the simulation results obtained based on natural isotopic abundances (Fig. 2b), which indicates the ability of Co–ZPB to encapsulate Fl within its cavity.

Figure 2.

Figure 2

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ESI-MS of (a) Co–ZPB (0.1 mM) and (b) Co–ZPB (0.1 mM) after the addition of 1 equiv. of Fl in CH3CN solution. ESI-MS of (c) Co–ZPB (0.1 mM) after the addition of 1 equiv. of ATP in CH3CN/H2O solution. Insets show the measured and simulated isotopic patterns at 947.19, 996.66 (a), 1112.22 (b) and 1149.69 (c).

1H NMR spectrum of Co–ZPB recorded after the addition of a 1.0 molar ratio of Fl exhibited significant upfield shifts of protons H3,6 (δ = 0.15 ppm) and other protons, suggesting that Fl was encapsulated within the electron-rich cavity of Co–ZPB (Figure S5 in supporting information). UV-Vis titration of Co–ZPB upon addition of Fl caused a significant absorption enhancement at 510 nm. The titration curve of this band reflected the formation of 1:1 stoichiometric ratio of the host-guest complexation, with a calculated association constant of 2.19 × 105 M−1 (Figure S9 in supporting information)32. It is postulated that the amide groups located within the positively charged macrocycle introduced geometric and functional properties that are beneficial to the recognition of the organic dye33,34.

The cyclic voltammogram of Co–ZPB in CH3CN exhibited broad peak at −0.88 V (vs. Ag/AgCl). Because redox potentials of the cobalt centers with same coordination environment in compound Co–QDB (vide infra) and of the DHPA moiety are very close to this value (Figures S20 and S21 in supporting information), the peak was assigned to the overlap of CoII/CoI reduction reaction with the reduction reaction of the DHPA moiety. Clearly, Co–ZPB is well suited to explore the redox-induced reactions that occur near the H2/H+ couple (Fig. 3a). When the addition of increasing amounts of Et3NH+ triggered the appearance of a new irreversible cathodic wave near the CoII/CoI response. Increasing the acid concentration raised the height of the new wave with a linear relationship and shifted it to more negative potentials. The new wave was assigned to proton reduction, suggesting that Co–ZPB can reduce protons in a catalytic reaction35,36. Moreover, as the oxidation potential of Fl in its photoexcited state (FI* → FI+ + e−) and ground state (Fl → Fl + + e−) are −1.55 V and 0.87 V (vs SCE)37, respectively, the photoexcited state of Fl (Fl*) has sufficient capability to reduce Co(II) to Co(I) directly. In the meantime, Co–ZPB was also an efficient quencher of the photosensitizer Fl (Fig. 4a and Figure S12 in supporting information). The addition of Co–ZPB to the solution of Fl (10 μM) in 1:1 CH3CN/H2O caused significant emission quenching. The quenching behaviour is considered a photoinduced electron transfer process from the excited state of Fl (Fl*) to Co–ZPB, enabling the activation of Co–ZPB by Fl for H2 production in solution38,39.

Figure 3.

Figure 3

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(a) Cyclic voltammograms of Co–ZPB (0.1 mM) containing n-Bu4NClO4 (0.1 M) in a CH3CN solution and upon the addition of Et3NHCl with concentrations of 0.04 mM (red line) and 0.08 mM (blue line), respectively. Scan Rate: 100 mV/s. The inset showing the i c vs. [HNEt3]. (b) H2 production after irradiation of the system containing TEA (5%), Co–ZPB (0.1 mM) and different concentrations of Fl.

Figure 4.

Figure 4

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(a) Normalized fluorescence of Fl (0.01 mM) (red bar) in CH3CN/H2O (1:1) at pH 11.0 in the presence of Co–ZPB (0.015 mM) (blue bar) and in the presence of Co–ZPB (0.015 mM) and ATP (0.15 mM) (green bar). The intensities were recorded at 520 nm, with excitation at 460 nm. (b) TON of photocatalytic H2 evolution after 6 hours of irradiation in CH3CN/H2O (1:1) at pH 11.0 with 5% TEA for the system containing Co–ZPB (0.1 mM)/Fl (0.1 mM) (red bar) in the presence of 0.2 mM ATP (green bar) or 0.2 mM ATP (blue bar).

The photocatalytic activities of Co–ZPB (0.1 mM) assembled with Fl (0.1 mM) towards evolution of molecular hydrogen were evaluated in an acetonitrile/water solution at room temperature in the presence of 5% triethylamine (TEA) as the sacrificial electron donor40,41. The volume of H2 was quantified at the end of the photolysis by GC of the headspace gases. Our system could work at pH range from 10.5 to 12.5, with maximal H2 evolution at pH 11.0 (Figure S15 in supporting information). The initial calculated turnover frequency (TOF) was approximately 100 moles H2 per mole catalyst per hour, with a turnover number (TON) of approximately 400 moles H2 per mole of catalyst (Fig. 3b). Notably, the TON for Fl and the redox catalyst was obtained in a stoichiometric catalyst/photosensitizer ratio. Compared to the intermolecular systems in which the TON value of one component is optimized with the other component in greater excess, the TON in the stoichiometric system reflects the true activity of the AP system. Meantime, ESI-MS spectrum of the Co−ZPB after reaction exhibited intense peaks at m/z = 947.21, 1062.71 and 1112.20, with the isotopic distribution patterns separated by 0.50 ± 0.01 Da. The peaks were assigned to host and host-guest complex, respectively, indicating the Co−ZPB/Fl system has sufficient structural stabilities during the reaction (Figure S2 in supporting information).

At a fixed Fl concentration (0.1 mM), the initial rates of H2 generation increased with the [Co–ZPB] at lower concentrations (<0.1 mM) (Figure S19 in supporting information). When [Co–ZPB] was fixed 0.1 mM and the Fl concentration was varied, the TOF plateaued at 0.1 mM; further addition of Fl did not increase the lifetime or TON of Co–ZPB. In all cases, the optimal conditions consisted of a constant molar ratio of Co–ZPB/Fl. An increase in the Co–ZPB/Fl ratio decreased the TON, and a decrease in the Co–ZPB/Fl ratio hardly increased the TONs of Fl or Co–ZPB. A 1:1 stoichiometric ratio of Co–ZPB/Fl complexation species apparently dominated the photosynthetic system. Control experiments demonstrated that Fl, Co–ZPB and light are essential for H2 generation.

To confirm whether the photoinduced H2 production occurred within the cavity of Co–ZPB or through a normal homogeneous system, the photocatalytic reaction was inhibited by the addition of a non-reactive species, adenosine triphosphate (ATP), to the reaction mixture because previous work showed that a cobalt-based cyclohelicate recognized ATP42. As expected, the presence of the molecular host Co–ZPB led to obvious upfield shifts of the aromatic protons on the adenosine ring, suggesting that ATP was encapsulated within the cavity of the macrocyclic complex (Figure S6 in supporting information). The ESI-MS spectrum of Co–ZPB in the presence of ATP exhibited an intense peak at m/z = 1149.69, with the isotopic distribution patterns separated by 0.50 ± 0.02 Da. This peak was assigned to [Co3(HZPB)2(H2 ZPB) ⊃ ATP]2+, indicating the stable existence of Co–ZPB in solution and the successful encapsulation of ATP within the cavity of Co–ZPB (Fig. 2c).

Importantly, the addition of ATP to replace the photosensitizer or redox catalyst Co–ZPB did not result in any H2 production, but the presence of 0.3 mM ATP effectively stopped the photocatalytic H2 production of the Co–ZPB (0.1 mM)/Fl (0.1 mM) system (Fig. 4b). This competitive inhibition behaviour was described as enzymatic-like and suggested that the H2 production possibly occurred within the cavity of Co–ZPB. The UV-Vis titration of Co–ZPB after the addition of ATP caused a significant decrease in absorption at 510 nm. The titration curve confirmed the 1:1 stoichiometric host-guest behaviour with an association constant of 3.64 × 106 M−1 (Figure S17 in supporting information). This value was thirty fold larger than that of the encapsulation of Fl, demonstrating the possibility of ATP to substitute for Fl to encapsulate the cavity of the metallohelicate. The H2 production likely occurred within the cavity of Co–ZPB, rather than in a normal homogeneous system2,43.

The incorporation of a DHPA group into the ligand backbone as the active site seemed being a powerful approach to adjust the overpotential of the metal sites for proton reduction by sharing the effect of electron gain, loss and distribution. To further investigate the important role of the NADH model in the proton reduction process, a new metallohelicate Co–QDB that has the similar molecular structural features and coordination geometries of cobalt centers with that of Co–ZPB, but without fragment of the DHPA group was synthesized and structurally characterized for comparison. The ligand H2 QDB was synthesized through the reaction of 2-quiolinecarboxaldehyde with 5-(dibenzylamino)isophthalohydrazide according to the literature method (Fig. 5)44. Co–QDB was prepared in a yield of 75% by layering a methanol solution of Co(NO3)2·6H2O onto a dichloromethane solution of H2 QDB in the presence of NH4PF6. The ESI-MS spectrum of Co–QDB exhibited intense peaks at m/z = 1088.05, 1119.55 and 1161.03, with the isotopic distribution patterns separated by 0.5 ± 0.01 Da, and a comparison with the simulation results based on natural isotopic abundances suggested that the peaks are assigned to [Co3(QDB) (HQDB)2]2+, [Co3(HQDB)3(NO3)]2+ and [Co3(HQDB)3(PF6)]2+, respectively, revealing the same structure and stability of the Co–QDB in solution (Figure S3 in supporting information). Single-crystal X-ray analysis confirmed the formation of a pseudo-C 3 symmetric macrocyclic helicate with three cobalt ions and three deprotonated HQDB ligands connected in an alternating pattern (Figure S1 in supporting information). Each cobalt centre was coordinated by two tridentate N2O chelating groups in a mer geometry with pairs of O atoms and amide N atoms each bearing a cis relationship, whereas the acetohydrazide N atoms were trans to each other that further indicate the mer configuration of the Co–ZPB. The measured C–O, C–N and N–N bond distances were all within the normal range of single and double bonds, pointing to the extensive electron delocalization over the entire molecular skeleton (Table S1 in supporting information)45,46. The separations between cobalt ions were 9.58 Å on average, and the average separation between the tertiary amine N atoms was 11.36 Å. The presence of four counter anions revealed that only two of the amide groups lost their protons during the coordination. These amide groups provided geometric and functional properties beneficial to the recognition of organic dyes, as observed in our previous works.

Figure 5.

Figure 5

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Procedure for the synthesis and crystal structure of the cobalt-based cyclohelicate showing the coordinated geometry of the redox-active metal centre. Solvent molecules and anions are omitted for clarity. The metal, oxygen, nitrogen and carbon atoms are drawn in green, red, blue and grey respectively.

The cyclic voltammogram of Co–QDB recorded in DMF exhibited one reversible reduction of CoII/CoI at −1.08 V (vs. Ag/AgCl). This potential falls well within the redox range of reducing a proton in aqueous media47, enabling the host to be a redox catalyst for proton reduction (Figure S21 in supporting information). Co–QDB was also demonstrated to be an efficient quencher of the excited state of Fl through photoinduced electron transfer (Fig. 6a and Figure S14 in supporting information). Photolysis of a solution of 0.04 mM Fl and 0.08 mM Co–QDB in a solvent mixture containing TEA (5% v:v) in DMF/CH3CN/H2O resulted in H2 generation, with optimal photocatalysis at pH 10.0 (Figure S16 in supporting information). As shown in Fig. 6b, the initial TOF was approximately 40 moles H2 per mole catalyst per hour, with a TON of approximately 250 moles H2 per mole of catalyst. The TON and TOF of the Co–QDB/Fl system is obviously lower than those of the Co–ZPB/Fl system.

Figure 6.

Figure 6

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(a) Family of the emission spectra of Fl (0.01 mM) in the presence of TEA in 1:1 CH3CN/H2O at pH 11.0 after the addition of different concentrations of Co–QDB. (b) H2 production after irradiation the system containing TEA (5%), Co–QDB (80 μM) and different concentrations of Fl.

Interestingly, the Co–QDB/Fl ratio is crucial: the TON plateaus at a 2:1 stoichiometric ratio of Co–QDB/Fl under the optimal conditions. At a fixed Co–QDB concentration (0.08 mM), the decrease in the Co–QDB/Fl ratio decreased the TON, and the increase in the Co–QDB/Fl ratio hardly increased the TON of Fl or Co–QDB, suggesting that a potential 2:1 stoichiometric ratio of the Co–QDB/Fl complexation species dominated the photosynthetic system (Fig. 6b). Additionally, glutathione (GSH), an important compound in natural systems that is inactive toward hydrogenation, was chosen as an inhibitor because our previous work showed that an isostructural cyclohelicate could recognize GSH well44. When the addition of 0.2 mM GSH to the 2:1 Co–QDB (0.08 mM)/Fl (0.04 mM) system directly stopped the photocatalytic H2 production. Since GSH does not exhibit any suitable redox potential for H2 production, this competitive inhibition suggested demonstrated that the H2 production occurred within the cavity of Co–QDB.

The ESI-MS spectrum of Co–QDB in the presence of Fl exhibited intense peaks at m/z ~2360.27 assigned to {K[Co3(HQDB)(QDB)2]2 ⊃ Fl}2+, providing additional proof for the 2:1 stoichiometric complexation behaviour (Figure S3 in supporting information). After irradiating the system for 6 hours, ESI-MS spectrum of the Co−QDB also exhibited intense peaks at m/z = 1088.05, 1161.03, and 2341.27, with the isotopic distribution patterns separated by 0.50 ± 0.01 Da. The peaks are assigned to host and host-guest complex, respectively, indicating the Co−QDB system also has sufficient structural stabilities in the reaction process (Figure S4 in supporting information). UV-Vis titration of Co–QDB after addition of Fl supported the 2:1 stoichiometry of the host-guest complexation, with an association constant of 8.32 × 109 M−2 (Figure S10 in supporting information). The 1H NMR spectrum of Co–QDB after the addition of a 0.5 molar ratio of Fl exhibited significant upfield shifts of protons H3,6 (δ = 0.13 ppm) and other protons, reflecting the encapsulation of Fl within the cavity of the macrocycle Co–QDB (Figure S7 in supporting information). Of course Co–QDB was able to recognize GSH in similar aqueous media (Figure S8 in supporting information). UV-Vis absorption titration of Co–QDB after the addition of GSH also induced quenching and suggested the formation of a 1:1 stoichiometry of the host–guest complexation with an association constant of 5.05 × 105 M−1 (Figure S18 in supporting information). At a fixed Co–QDB concentration of 0.08 mM, the presence of GSH could substitute for Fl to occupy the cavity of Co–QDB. It is hypothesized that Co–ZPB and Co–QDB are true molecular flasks48,49, within which AP systems are assembled through encapsulation of an organic dye as a photosensitizer.

Conclusion

In summary, we have reported the preparation of a redox-active cobalt-based macrocycle through the incorporation of an NADH mimic within the ligand backbone and a new strategy for the construction of AP systems. The metal-organic cyclohelicate is an enzymatic molecular flask and encapsulated Fl within its cavity for light-driven H2 evolution with a TON and TOF that reached 400 and 100 moles H2 per mole redox catalyst per hour, respectively. The reaction was inhibited by the presence of ATP and occurred within the cavity of the cyclohelicate. The control experiments indicated that the redox-active dihydropyridine amido group of the NADH mimic was helpful for the photocatalytic proton reduction process. By incorporating other redox-active or photoactive functional groups, this strategy can be extended to highly active AP systems.

Materials and Methods

Materials

All chemicals were reagent grade, obtained from commercial sources and used without further purification. The elemental analyses of C, H and N were performed on a Vario EL III elemental analyser. 1H NMR spectra were measured on a Varian INOVA 400 M spectrometer. ESI mass spectra were obtained on an HPLC-Q-TOFMS instrument using methanol as the mobile phase. UV-Vis spectra were measured on an HP 8453 spectrometer. The solution fluorescence spectra were obtained using an FLS920 spectrometer (Edinburgh Instruments). Both the excitation and emission slit widths were 2 nm. The solutions of Co–ZPB (1.0 × 10−3 M) and Co–QDB (4.0 × 10−3 M) were prepared in CH3CN and DMF, respectively. Stock solutions of Fl (1.0 × 10−3 M) were prepared directly in CH3CN and were excited at 460 nm.

All electrochemical measurements were carried under nitrogen at room temperature on a CHI 1130 (CH Instrument Co., Shanghai) electrochemical analyser with a conventional three-electrode system consisting of a homemade Ag/AgCl electrode as the reference electrode, a platinum silk electrode with a 0.5 mM diameter as the counter electrode, and a glassy carbon electrode as the working electrode. Cyclic voltammograms were recorded at solution concentrations of 0.1 mM and 1.0 mM for Co–ZPB and Co–QDB, respectively, and 0.1 M for the supporting electrolyte, (n-Bu4N)ClO4. The electrodes were polished on an MD-Nap polishing pad. A 0.2 M solution of Et3NHCl was added via a syringe.

General Procedure for Hydrogen Production

For photoinduced hydrogen evolution, varying amounts of the catalyst and the 1:1 CH3CN/H2O solution containing Fl and TEA were added in a total volume of 5.0 mL for Co–ZPB, and varying amounts of catalyst, Fl and TEA in DMF/CH3CN/H2O (1/4/4) were added to a total volume of 5.0 mL for Co–QDB. The pH of this solution was adjusted by adding HCl or NaOH and measured with a pH metre50,51. Typically, the Co–ZPB sample contained Co–ZPB (1 × 10−4 M), Fl (1 × 10−4 M) and 5% TEA as the sacrificial electron donor at pH 11.0, and the Co–QDB sample contained Co–QDB (8 × 10−5 M), Fl (4 × 10−5 M) and 5% TEA as the sacrificial electron donor at pH 10.0. The flask was sealed with a septum, protected from light, and degassed by bubbling nitrogen for 15 min under atmospheric pressure at room temperature. Next, the samples were irradiated by a 500 W xenon lamp; the reaction temperature was maintained at 293 K using a water filter to absorb heat. The generated photoproduct of H2 was characterized on a 7890 T GC instrument with a 5 Å molecular sieve column (0.6 m × 3 mm), a thermal conductivity detector, and nitrogen as the carrier gas. The amount of hydrogen generated was determined by the external standard method. The hydrogen in the resulting solution was not measured, and the slight effect of the hydrogen gas generated on the pressure of the Schlenk bottle was neglected in the calculation of the volume of hydrogen gas.

Synthesis of Co–ZPB

Dimethyl 1-benzyl-4-phenyl-1,4-dihydropyridine-3,5-dicarboxylate

Methyl propiolate (1.68 g, 20 mmol), benzaldehyde (1.06 g, 10 mmol), and benzylamine (1.07 g, 10 mmol) in glacial acetic acid (2.0 mL) were heated at 80 °C for 30 min52. After cooling, the mixture was poured into water (20 mL) and stirred for 1 h. The solid product was filtered and washed with Et2O (3 × 30 mL) to give pure dimethyl 1-benzyl-4-phenyl-1,4-dihydropyridine-3,5-dicarboxylate, which was recrystallized by ethanol (Figure S23 in supporting information). Yield: 1.91 g, 52.3%. 1H NMR (400 MHz, DMSO-d 6, ppm): δ 7.51 (s, 2H), 7.45–7.41 (m, 2H), 7.37–7.34 (m, 3H), 7.20–7.16 (m, 2H), 7.13–7.08 (m, 3H), 4.82 (s, 2H), 4.70 (s, 1H), 3.53 (s, 6H).

1-benzyl-4-phenyl-1,4-dihydropyridine-3,5-dicarbohydrazide

A mixture solution of 80% hydrazine hydrate (50 ml) and dimethyl 1-benzyl-4-phenyl-1,4-dihydropyridine-3,5-dicarboxylate (3.63 g, 10 mmol) was stirred at 85 °C over 12 h. The white precipitate was formed, which was collected by filtration, washed with methanol and dried in vacuum. Yield: 1.72 g, 47.3%. 1H NMR (400 MHz, DMSO-d 6, ppm): δ 8.67 (s, 2H), 7.42–7.39 (m, 2H), 7.35–7.32 (m, 3H), 7.20 (s, 2H), 7.17–7.12 (m, 4H), 7.09–7.05 (m, 1H), 5.00 (s,1H), 4.60 (s, 2H), 4.12 (s, 4H).

Synthesis of H2ZPB

1-benzyl-4-phenyl-1,4-dihydropyridine-3,5-dicarbohydrazide (3.63 g, 10 mmol) was added to a ethanol solution (50 mL) containing 2-pyridylaldehyde (2.35 g, 22 mmol). After 5 drops of acetic acid was added, the mixture was heated at 85 °C under magnetic stirring for 12 h according to the ref.53. The yellow solid was collected by filtration, washed with methanol and dried in vacuum. Yield: 4.33 g, 79.9%. 1H NMR (400 MHz, DMSO-d 6, ppm): δ 11.36 (s, 2H6), 8.57 (d, 2H1), 8.21 (s, 2H5), 7.83–7.78 (m, 4H3,4), 7.51–7.47 (m, 2H2), 7.46–7.41 (m, 4H8,11), 7.39–7.35 (m, 3H10,12), 7.27–7.20 (m, 4Hβ,γ), 7.14–7.09 (m, 1Hα), 5.35 (s, 1H7), 4.77 (s, 2H9). Anal calc. for C32H27N7O2·H2O: H 5.22, C 68.68, N 17.52%. Found: H 5.50, C 68.27, N 17.18%. ESI-MS calcd for C32H27N7O2 541.22, found 542.23 [M + H]+, 564.21 [M + Na]+.

Synthesis of Co–ZPB

Co(NO3)2·6H2O (29.1 mg, 0.10 mmol) and H2 ZPB (54.2 mg, 0.10 mmol) were dissolved in CH3OH/CH2Cl3 (1/1,v/v) to give a red solution. After addition of NaClO4, red precipitates formed were isolated and dried under vacuum. Yield: 68%. 1H NMR (400 MHz, DMSO-d 6, ppm): δ 11.39 (s, 2H6), 8.58 (d, 2H1), 8.22 (s, 2H5), 7.83 (m, 4H3,4), 7.50 (m, 2H2), 7.45–7.33 (m, 7H8,10,11,12), 7.25 (m, 4Hβ,γ), 7.12 (m, 1Hα), 5.34 (s, 1H7), 4.78 (s, 2H9). Anal calc. for Co3(C96H79N21O6)·3ClO4·NO3: H 3.69, C 53.38, N 14.27%. Found: H 3.89, C 52.05, N 13.95%. ESI-MS: m/z: 947.19 [Co3(HZPB)3·ClO4]2+, 996.66 [Co3(HZPB)2(H2 ZPB)·2ClO4]2+.

Synthesis of Co–QDB

Co(NO3)2·6H2O (30 mg, 0.10 mmol) and H2 QDB (70 mg, 0.10 mmol) were dissolved in DMF and then stirred for 2 h. The solution was left for several days at room temperature to give X-ray quality black block crystals. Yield: 65%. 1H NMR (400 MHz, DMSO-d 6, ppm): δ 12.24 (s, 2H), 8.61 (s, 2H), 8.46 (m, 2H), 8.12 (m, 2H), 8.05 (m, 4H), 7.79 (m, 2H), 7.76 (s, 1H), 7.66 (m, 2H), 7.46 (s, 2H), 7.40–7.27 (m, 10H), 4.85 (s, 4H). Anal calc. for Co3(C126H95N21O6)·2PF6: H 3.88, C 61.37, N 11.93%. Found: H 4.08, C 60.06, N 11.69%. ESI-MS: m/z: 1088.05 [Co3(QDB)(HQDB)2]2+, 1119.55[Co3(HQDB)3·NO3]2+, 1161.03 [Co3(HQDB)3 PF6]2+.

Electronic supplementary material

Supplementary Information (1.2MB, pdf)

Acknowledgements

We gratefully acknowledge the financial support from the Natural Science Foundation of China (21501019, 21531001, and 21421005).

Author Contributions

C.D. and C.H. designed the project; L.Z. and J.W. synthesized the compounds and carried out the experiments; P.W. and X.G. synthesized part of the compounds. L.Z. and C.D. wrote the manuscript. All authors discussed the results and commented on the manuscript.

Competing Interests

The authors declare that they have no competing interests.

Footnotes

Electronic supplementary material

Supplementary information accompanies this paper at 10.1038/s41598-017-14728-8.

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