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Article

Pentadentate and Hexadentate Pyridinophane Ligands Support Reversible Cu(II)/Cu(I) Redox Couples

by
Glenn Blade
1,
Andrew J. Wessel
2,
Karna Terpstra
1 and
Liviu M. Mirica
1,*
1
Department of Chemistry, University of Illinois Urbana-Champaign, 600 S. Matthews Ave, Urbana, IL 61801, USA
2
Department of Chemistry, Washington University, One Brookings Drive, St. Louis, MO 63130, USA
*
Author to whom correspondence should be addressed.
Inorganics 2023, 11(11), 446; https://doi.org/10.3390/inorganics11110446
Submission received: 5 October 2023 / Revised: 31 October 2023 / Accepted: 17 November 2023 / Published: 20 November 2023
(This article belongs to the Special Issue Editorial Board Members’ Collection Series in “Bioinorganic Chemistry of Copper”)
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Abstract

:
Two new ligands were synthesized with the goal of copper stabilization, N,N′-(2-methylpyridine)-2,11-diaza[3,3](2,6)pyridinophane (PicN4) and N-(methyl),N′-(2-methylpyridine)-2,11-diaza[3,3](2,6)pyridinophane (PicMeN4), by selective functionalization of HN4 and TsHN4. These two ligands, when reacted with various copper salts, generated both Cu(II) and Cu(I) complexes. These ligands and Cu complexes were characterized by various methods, such as NMR, UV-Vis, MS, and EA. Each compound was also examined electrochemically, and each revealed reversible Cu(II)/Cu(I) redox couples. Additionally, stability constants were determined via spectrophotometric titrations, and radiolabeling and cytotoxicity experiments were performed to assess the chelators relevance to their potential use in vivo as 64Cu PET imaging agents.

Graphical Abstract

1. Introduction

Mononuclear copper complexes have been extensively utilized throughout various areas of inorganic chemistry: synthesis of structural or functional biomimetic inorganic complexes of Cu-containing enzymes [1,2,3,4], cation detection or sequestration [5,6], development of metal-based therapeutic or diagnostic compounds [7,8,9,10], and many others. In particular, the development of 64Cu-based positron emission tomography (PET) agents has garnered significant attention in recent years as an alternative to shorter-lived radionuclides 11C and 18F, which are commonly used in PET imaging [11,12,13]. However, these 64Cu PET agents still face challenges presented by the possibility of in vivo decomplexation. Ideally, a suitable chelator should demonstrate high thermodynamic stability and kinetic inertness in order to avoid this problem, which has been the focus of many studies in recent years [14]. However, a problem faced by some of the most common 64Cu chelators is the issue of reduction-induced demetallation. Given the reducing environment of cells and the presence of in vivo bioreductants, the ideal chelator should be able to avoid this issue by remaining stable even upon reduction to CuI [15]. As such, ligands with flexible donor arms that have the ability to stabilize both CuII and CuI are good candidates for chelating 64Cu [16]. Several studies have been published in recent years focused on the coordination chemistry of 64Cu complexes with macrocyclic ligands substituted with pendant arms like 2-pyridylmethyl, picolinate, thiazolyl, and others [17,18,19,20,21].
In that vein, two new pyridinophane ligand systems, inspired by previous macrocyclic polydentate ligands, have been synthesized [22,23,24]. By substituting non-interacting groups (i.e. Me or tBu) for groups that can interact with the metal center, greater binding modes than usual for RN4 ligands can be achieved with altered characteristics of the resultant complexes. Interacting groups like 2-methylpyridyl, picolyl—“Pic”, could bind directly with the metal center while being easily synthetically attached to the N4 backbone. When both alkyl groups are chosen to be the picolyl fragment, the resultant hexadentate ligand N,N′-(2-methylpyridine)-2,11-diaza[3,3](2,6)pyridinophane, PicN4, offers the possibility of a distorted octahedral environment around the metal center while simultaneously shielding from inner sphere interactions. An asymmetric version could also be synthesized using previously reported methods to make N-(methyl),N′-(2-methylpyridine)-2,11-diaza[3,3](2,6)pyridinophane, PicMeN4, which could act as a pentadentate ligand and leave one coordination site available for an exogenous ligand. This flexible pentadentate ligand could more easily adapt to geometries other than a distorted octahedral arrangement. When this ligand was bound to copper, both PicN4 and PicMeN4 were able to stabilize both CuII and CuI oxidation states, with each complex being crystallographically characterized. Each of these four complexes was spectroscopically scrutinized by various techniques, including NMR, EPR, ESI-MS, and UV-Vis. Cyclic voltammetry experiments were able to show that the conversion between CuII and CuI was remarkably reversible for both systems, as a consequence of the flexible nature of the picolyl arms being able to come off the Cu center. The PicN4CuII/I couple was also low at E1/2 = −1.1 V vs. Fc/Fc+. Calculation of CuII stability constants using spectrophotometric titrations also revealed the moderate ability of the complexes to stabilize both CuII and CuI complexes. Finally, preliminary radiolabeling studies showed that both PicN4 and PicMeN4 can quickly and efficiently be radiolabeled with 64Cu, making these ligands potentially relevant chelators for use in 64Cu PET imaging studies.

2. Results and Discussion

2.1. Synthesis

The ligand synthesis of PicN4 was a two-step development. The first attempt at the synthesis of PicN4 involved an SN2-based mechanism utilizing 2-chloromethyl pyridine under basic conditions at a roughly 80% yield [25]. Multiple bases were tested for this synthesis; between sodium carbonate, potassium carbonate, and Hünig’s base (diisopropylethylamine), Hünig’s base gave the highest yield of 81%, while the carbonates gave smaller yields of around 40%. Additional synthetic attempts using reductive amination have given inconsistent results and a maximum yield of 46%. Full synthetic details and product descriptions can be found in the Supporting Information.
Ligand synthesis for PicMeN4 was achieved by two different methods, as depicted in Scheme 1. In the first pathway, the direct functionalization of MeHN4 by placing the 2-methylpyridyl on the secondary amine was performed to make the product. This pathway requires making MeHN4, a product synthesized by previously discussed methods [23]. The second pathway utilized TsHN4 for functionalization to yield PicTsN4. The tosyl deprotection reaction using concentrated sulfuric acid did not degrade the ligand significantly, providing a good yield of PicHN4. The penultimate product, PicHN4, was then methylated to yield the final product, PicMeN4. Since both pathways showed that the products TsMeN4 and TsPicN4 could survive the harsh sulfuric acid conditions of the detosylation reaction, the second pathway was chosen. Functionalization of the secondary amines occurred by one of two methods: reductive amination or SN2. Both methods achieved high yields (75% and 81%, respectively), but the SN2 was much more consistent and less reliant on the purity of reagents.
The syntheses of the 1·(OTf)2 and 2·OTf complexes was achieved by mixing the appropriate triflate salt with the ligand in MeCN (Scheme 2). CuII(OTf)2 and PicN4 were mixed overnight and either crashed out of solution by trituration with diethyl ether or recrystallized via diethyl ether diffusion, with an 88% yield of 1·(OTf)2. While most studies in this paper utilize the triflate complex, other salts like CuII(ClO4)2 or CuII(PF6)2 were also employed with similar yields. Similarly, [(MeCN)4CuI]OTf and PicN4 were mixed in MeCN for one hour and recrystallized via ether diffusion for a 55% yield of 2·OTf.
The synthesis of complexes 3·(OTf)2 and 4·OTf were similarly completed: the relevant copper triflate salt and the ligand were mixed in MeCN (Scheme 2). While crystals for the CuII salt were not easily obtained, a green solid was crashed out from MeCN with toluene and rinsing with pentane (55% isolated yield). When attempting to get crystals of 3·(OTf)2, the use of sodium tetraphenylborate, NaBPh4, generated orange crystals of 4·OTf in low yield. A more acceptable approach to preparing 4·OTf was PicMeN4 and [(MeCN)4CuI]OTf mixed in MeCN for one hour in the dark and recrystallized via diethyl ether diffusion at −35 °C (77% yield).

2.2. Structural Characterization of Metal Complexes

X-ray diffraction-quality crystals of the copper complexes were obtained by diethyl ether diffusion into MeCN solutions at room temperature or –35 °C (Figure 1 and Table 1). Full crystallographic details are provided in the Supplemental Information. The crystal structure of 12+ had a similar distorted octahedral environment to the one observed for the analogous tBuN4 complex [22,26,27]. The inclusion of the two pyridine moieties on the metal center preclude the need of additional exogenous ligands, such as solvent or triflates directly bound to the metal center. The CuII center exhibits a Jahn-Teller like distortion, with the four pyridine nitrogens having relatively short bond lengths to copper (2.00–2.06 Å), while the amine nitrogens form much longer bonds (2.28, 2.35 Å).
Upon reduction to 2+, the coordination environment changes to a pentadentate distorted square pyramid geometry with a structural parameter τ5 = 0.13.[28] As expected for CuI structures, the Cu-Neq bond lengths averaged a shorter value of 2.00 Å, while the Cu-Nax bond lengths were much longer at 2.34 Å. The non-coordinating picolyl nitrogen was sufficiently far away to not interact with the Cu center at 3.32 Å [4,22].
Supposing that crystals of 4+ was more stable than 32+, the ligand was mixed with CuIOTf in MeCN and recrystallized with ether diffusion at room temperature to yield large orange crystals. The cation of 4+ adopts a distorted square pyramid pentadentate geometry with a structural parameter τ5 = 0.12, similar to 2+ [28]. It has a similar delineation of Cu-N bonds around the Cu: Cu-Neq bond lengths averaged 2.00 Å, while Cu-Nax bond lengths averaged 2.33 Å. Unlike in 2, the methylamine on the PicMeN4 backbone was less sterically restricted than the picolyl functionalized amines.
In an attempt to obtain crystals of 3·(PF6)2, the blue solid was dissolved in MeCN with two equivalents of NaBPh4 and subjected to diethyl ether diffusion at room temperature. When isolated, there were primarily orange crystals of 4·PF6 present with a blue solution. Crystals of 3·(BPh4)2 were eventually recovered under these conditions as a mixture of CuII and CuI crystals. Although it was unknown exactly how the CuII complex was reduced in the solution, it was suspected that the NaBPh4 and the BPh3 impurity promoted the reduction of the CuII center. Regardless, 32+ displays a Jahn-Teller like distorted octahedral geometry with one exogenous MeCN bound to the CuII center. Interestingly, the CuII species seemed to exhibit Jahn-Teller like compression along the N1-Cu-N3 axis where the Cu-N bond lengths are around 1.95 Å, while the other four Cu-N bonds are longer at an average of 2.20 Å.

2.3. Complex Characterization

To better understand the solution state characteristics of these complexes, several techniques were utilized, including electron paramagnetic resonance (EPR), NMR, and electrochemical studies. The paramagnetic d9 CuII complexes 12+ and 32+ were characterized by EPR in a fashion similar to previous CuII species, and the EPR spectra are shown in Figure 2 and the EPR parameters are summarized in Table 2. Analysis by Evan’s method measured in CD3CN yielded the expected values for these d9 CuII centers: 1.80 µB and 1.71 µB for 12+ and 32+, respectively [29]. The EPR spectrum for 1·(OTf)2 exhibited values of gx = 2.070, gy = 2.055, and gz = 2.259 (Az = 144.5 G) and gx = 2.067, gy = 2.056, and gz = 2.264 (Az = 152.5 G) for 3·(OTf)2, which is consistent with what is expected of a distorted octahedral CuII center, and in line with the solid state structural data [22,29,30].
While the paramagnetic 1H NMR spectrum of 12+ did not afford much information (Figure S14), the spectra of the d10 CuI species could generally be assigned with the help of a gCOSY 2D spectrum (Figures S9–S13). The assignment of the 2·OTf spectrum gathered in CD3CN was assigned as so: the four most downfield aromatic peaks corresponded to the different pyridine hydrogens on the picolyl arm, while the two upfield sets of aromatic multiplets corresponded to the pyridine hydrogens on the N4 backbone [31]. The methylene region contained five total peaks: a singlet (4.62 ppm) matched to the two picolyl methylene hydrogens and a pair of doublets matched to the N4 methylene hydrogens. Further assignment of the N4 methylene hydrogens could not be easily discerned due to the symmetry and structure of the molecule. The integration and the 2D NMR corroborated this assignment (Figure S11). Since the methylene on the picolyl arm appears as a singlet, this implies there was rapid exchange between the bound arm and the unbound arm which was faster than the NMR time-scale.
The assignment of the 4·OTf spectrum followed in a similar way. The three most downfield aromatic peaks matched the four pyridine hydrogens on the picolyl arm, while the two down-field aromatic multiplets corresponded with the para- and meta-hydrogens on the N4 pyridine backbone. The two singlet peaks in the aliphatic region corresponded to the two methylamines: the methylene moiety on the picolyl arm (4.469 ppm) and the methyl group (3.313 ppm). In a similar fashion to the PicN4 complex, the methylene on the picolyl arm was not fixed in spaced which allowed resolution into a singlet. The remaining four sets of doublets (Javg ≈ 15 Hz, geminal) corresponded to the methylene protons fixed in place on the N4 backbone. Based on the gCOSY crossover peaks (Figure S13), the doublet pairs 4.248 and 3.668 ppm correspond to interaction protons, while 4.177 and 4.040 ppm are also coupled.
Cyclic voltammetry (CV) for 1·(OTf)2 featured a couple at −0.752 V vs. Fc0/+ (Figure 3), corresponding to the CuII/I couple with a quasi-reversible nature (ΔEp = 97 mV) as well as an irreversible oxidation at + 1.047 V (Figure S15). In order to confirm the reversibility of the CuII/I couple, 2·OTf was also scrutinized to yield a similar couple at −0.716 V vs. Fc0/+ (ΔEp = 176 mV). A similar analysis for 3·(OTf)2 found a quasi-reversible CuII/I couple at −0.468 V vs. Fc0/+ (ΔEp = 105 mV) along with an irreversible CuIII oxidation at 1.552 V (Figure S16). Confirming the reversibility of this quasi-reversible CuII/I couple, a CV of 4·OTf showed the couple at −0.441 V vs. Fc0/+ (ΔEp = 96 mV).
Notably, all four copper complexes exhibit larger ΔEp values than the values expected for fully reversible redox processes (Table 3). However, the measured ΔEp values for the Fc0/+ couple in both sets of experimental conditions, 129 mV and 176 mV, are also larger than standard values, indicating that the large peak-to-peak separation may not necessarily imply redox irreversibility of the copper complexes. Furthermore, the discrepancies between the ΔEp values of the complexes can be explained by the different sets of experimental conditions for each: CuII complexes are air stable and can be analyzed on the bench top, while CuI complexes are very air sensitive and required rigorous anaerobic conditions of a glovebox.
Additionally, both complexes were subjected to conditions with increasing concentrations of water in MeCN. The CuII/I couple for PicN4 was only shifted slightly to −0.800 V vs. Fc0/+ even in a 70% water to MeCN solution (with 0.2 M TBAP). The reversibility of the couple remained stable throughout the course of the experiment (Figure S17). The CuII/I couple of PicMeN4 shifted less drastically to −0.600V vs. Fc0/+ after adding up to 70% water to an MeCN solution (with 0.2 M TBAP). The system was overall reversible but at higher concentrations of water, and additional oxidation and reduction peaks appeared probably due to water binding to the metal center over MeCN (Figure S18).

2.4. Ligand Acidity Constants and Complex Stability Constants

To determine the acidity constants (pKa) of PicN4 and PicMeN4, UV-Vis spectrophotometric titrations were performed and the changes in the spectra were monitored. To a solution of either PicN4 or PicMeN4 in 0.1 M KCl, aliquots of 0.15 M KOH were added and the UV-Vis spectra were recorded at each pH. For the PicN4 ligand, the increase of the solution’s pH results in the steady decrease of the π—π* transition band at 264 nm, until around pH 7, at which point the absorbance begins to increase (Figure 4). The data was then simulated in the HypSpec 2014 program (Protonic Software, UK) [32], which afforded the species distribution plot (Figure 4) and three pKa values: 8.94, 5.32, and 3.60. These values are tentatively assigned to the tertiary amine nitrogen, pyridine on the N4 backbone, and picolyl nitrogen, respectively. Despite containing six potential sites for protonation, only three pKa values were determined. This is likely due to the increased electrostatic repulsion that occurs upon sequential protonation steps, making it difficult to observe higher charged species in the pH range of the titration [33].
For the PicMeN4 ligand, a similar decrease in the peak at 261 nm occurred upon the increase in pH, until the lowest absorbance was observed at approximately pH 4 (Figure S25). Thereafter, the absorbance was observed to increase until a plateau at pH 7. Analysis using HypSpec provided four pKa values, the highest of which, 11.13, is assigned to the deprotonation of the methyl amine nitrogen (Table 4). The next highest value, 9.16, is assigned to the deprotonation of the tertiary amine amended with the 2-methylpyridine arm, which has previously been shown to lower the basicity of amine nitrogens attached to it [34,35,36]. This assignment also aligns with the highest pKa observed in PicN4, which contains two similar amine sites.
To obtain the CuII stability constants for the complexes, similar spectrophotometric pH titrations were performed for a 1:1 mixture of Cu2+ and ligand in 0.1M KCl (Figure 5). Analysis of the spectral changes occurring in the UV for each complex gave a series of stability constants, as summarized in Table 5. The log(KCu(II)L) values reveal that PicN4 is able to form slightly more stable copper complexes than PicMeN4. In the case of PicMeN4, a value corresponding to the deprotonation of water was also obtained (7.75), but this was not observed for PicN4. This could likely be attributed to the open coordination site available for PicMeN4, as evidenced in the crystal structure, which would allow for the binding and subsequent deprotonation of a water molecule.
The determination of the CuI stability constants for each complex relied on the CuII stability constant and the E1/2 values determined in the aqueous CV experiments. CVs of the complexes in aqueous conditions with 0.1 M NaOAc as a supporting electrolyte revealed E1/2 values of −0.415 V and −0.220 V vs. Ag/AgCl for 12+ and 32+, respectively (Figures S19 and S20). It is worth noting that the aqueous CV data of 12+ showed an additional reversible redox couple at −0.245 V vs. Ag/AgCl, which could be attributed to an alternative coordination mode, perhaps from the binding of an acetate ion present in solution. Another possible explanation for the observation of two species in solution could be two protonation states, as the species distribution for this complex shows nearly equal amounts of CuL and CuLH species at pH 7. Nevertheless, for the purpose of determining CuI stability constants, the more negative reduction potential was used in the Nernst equation. Stability constants for CuI could then be obtained by applying a Nernstian relationship using the reduction potentials, which results in log(KCu(I)L) values of 7.05 and 9.46 for PicN4 and PicMeN4, respectively.
Another important consideration for 64Cu chelators is the possibility of transmetalation with biogenic metals in vivo. Therefore, the stability constants of the ligands PicN4 and PicMeN4 towards Zn2+ were also determined. Both ligands have significantly lower Zn stability constants as compared to those for Cu, and the affinity towards Zn is also markedly lower at biological pH. This data indicates that the copper complexes of PicN4 and PicMeN4 are unlikely to undergo transmetalation with zinc, a promising trait for potential 64Cu chelators.
When comparing the log(KCu(II)L) to other commonly used 64Cu chelators, it is observed that PicN4 and PicMeN4 have moderately lower stability constants than the other chelators (Table 6). Many of these chelators have N,O-based donor sets, but notably also have irreversible reduction potentials (e.g. DOTA, TETA). The chelators described in this work have the added benefit of reversible CuII/I redox couples, allowing for the ability to form stable CuI complexes.

2.5. Radiolabeling Studies

The radiolabeling capabilities of PicN4 and PicMeN4 were also evaluated. Using a stock solution of 64CuCl2 diluted in ammonium acetate buffer (pH 5.5), mixtures of the ligands and 64CuCl2 were incubated at 45 °C for 30 min. These relatively mild conditions are comparable to those used for the common 64Cu chelators like NOTA and DOTA [38]. The radiolabeled compounds were then analyzed by radio-HPLC using water (0.1% TFA) and acetonitrile (0.1% TFA) as the mobile phase with a gradient of 0–100% acetonitrile over 15 min (Figure 6). A control of only 64CuCl2 in ammonium acetate was also analyzed to compare the retention times. Both ligands showed complete conversion to 64Cu complexes, with no remaining free 64Cu being observed in either radio-HPLC trace. While PicMeN4 shows one peak in the chromatogram, PicN4 shows two peaks close to one another. One possible explanation for this observation is an alternative coordination environment around the copper center, such as a different counterion (e.g. chloride, acetate) bound to the metal center. This observation is consistent with the aqueous CV studies that show PicN4 also having two species present in solution (Figure S19).
After confirming that the ligands were able to be radiolabeled with 64Cu, the lipophilicity of the complexes was determined by measuring the octanol/PBS partition coefficient (logDoct, Table 7). Both dicationic complexes are particularly hydrophilic, with 64Cu-PicMeN4 having a more negative partition coefficient than 64Cu-PicN4.

2.6. Cytotoxicity Studies

In order to test the plausibility of in vivo applications for these two chelators, cytotoxicity studies were performed using an Alamar blue assay on mouse neuroblastoma Neuro2a (N2a) cells. Cells were treated with each compound of their CuII complexes and cell viability was evaluated after a 48 h incubation period. The percentage of cell viability, as summarized in Figure 7, revealed that both ligands PicN4 and PicMeN4 are toxic at higher concentrations, but PicMeN4 is significantly less toxic than PicN4. Notably, the addition of Cu greatly reduces the toxicity of these ligands, with both complexes showing extremely high cell viability across the board, even at concentrations of 20 µM.

3. Conclusions

Inspired by previous pyridinophane ligands, herein we report two new ligand systems, PicN4 and PicMeN4. The 2-methylpyridyl arms of these ligands bind to the Cu center in place of exogenous ligands and allow for a polydentate binding mode greater than tBuN4. The hexadentate PicN4 ligand offers the metal center a fully bound, distorted octahedral geometry, which can shield the metal center from side reactions. The asymmetric PicMeN4 ligand offers five coordinating atom donors with the option of binding one exogenous ligand. This flexible pentadentate ligand can adopt geometries other than distorted octahedral and could be used to probe electrocatalytic transformations.
When bound to copper, PicN4 and PicMeN4 both stabilized CuII and CuI centers, which were characterized by various spectroscopic means. Crystal structures were also obtained for all four compounds, showing a preferred geometry of distorted octahedral for the CuII complexes and a distorted square pyramidal geometry for the CuI complexes. Electrochemically, PicN4 exhibits a reversible CuII/I couple at a low potential of −0.1 V vs. SHE. Conversely, the PicMeN4 CuII/I couple was also reversible, but the ability to bind an exogenous ligand caused other redox features to appear. Both CuI and CuII stability constants for each ligand were also determined, as were their affinities for CuII at biologically relevant pHs.

Supplementary Materials

The following supporting information can be downloaded at https://www.mdpi.com/article/10.3390/inorganics11110446/s1, Figures S1-S33, Tables S1–S11, References [43,44,45,46,47,48,49] are cited in the Supplementary Materials.

Author Contributions

Conceptualization, L.M.M.; methodology, G.B., A.J.W. and K.T.; validation, G.B., A.J.W. and K.T.; formal analysis, G.B., A.J.W. and K.T.; investigation, G.B., A.J.W. and K.T.; writing—original draft preparation, A.J.W. and G.B.; writing—review and editing, G.B., A.J.W., K.T. and L.M.M.; visualization, G.B., A.J.W. and K.T.; supervision, L.M.M.; project administration, L.M.M.; funding acquisition, L.M.M. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the US National Institutes of Health (R01GM114588 and RF1AG083937 to L.M.M.).

Data Availability Statement

All research data can be found in the Supplementary Materials or can be requested from the corresponding author.

Acknowledgments

We would like to thank the National Institutes of Health (R01GM114588 and RF1AG083937 to L.M.M.) for financial support for this project. We would also like to thank Nigam P. Rath (Univ. of Missouri—St. Louis, USA) for assistance with X-ray structure analysis.

Conflicts of Interest

The authors declare no competing financial interest.

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Inorganics 11 00446 sch001
Scheme 1. Synthesis of PicN4 and PicMeN4. (i) 90% H2SO4, reflux 2.5 h; 88% (ii) 2-(methylchloro)pyridine HCl, iPr2EtN, MeCN, 48 h; 81% (iii) TsCl, DCM, 0 C, 3 h; 44% (iv) 2-(methylchloro)pyridine HCl, iPr2EtN, MeCN, 48 h; 82% (v) 90% H2SO4, reflux, overnight; 89% (vi) formic acid, formaldehyde, reflux, overnight; 82%.
Scheme 1. Synthesis of PicN4 and PicMeN4. (i) 90% H2SO4, reflux 2.5 h; 88% (ii) 2-(methylchloro)pyridine HCl, iPr2EtN, MeCN, 48 h; 81% (iii) TsCl, DCM, 0 C, 3 h; 44% (iv) 2-(methylchloro)pyridine HCl, iPr2EtN, MeCN, 48 h; 82% (v) 90% H2SO4, reflux, overnight; 89% (vi) formic acid, formaldehyde, reflux, overnight; 82%.
Inorganics 11 00446 sch001
Inorganics 11 00446 sch002
Scheme 2. Preparation of Copper Complexes.
Scheme 2. Preparation of Copper Complexes.
Inorganics 11 00446 sch002
Inorganics 11 00446 g001
Figure 1. ORTEP plots (50% probability ellipsoids) of cations 12+ , 2+, 32+, and 4+. Counterions and H atoms are omitted for clarity. The crystallographic datasets for 1·(OTf)2, 2·OTf, 3·(OTf)2, and 3·OTf have been deposited at CCDC under the record numbers 2049802, 2049803, 2049804, and 2049805.
Figure 1. ORTEP plots (50% probability ellipsoids) of cations 12+ , 2+, 32+, and 4+. Counterions and H atoms are omitted for clarity. The crystallographic datasets for 1·(OTf)2, 2·OTf, 3·(OTf)2, and 3·OTf have been deposited at CCDC under the record numbers 2049802, 2049803, 2049804, and 2049805.
Inorganics 11 00446 g001
Inorganics 11 00446 g002
Figure 2. EPR spectrum (black) and simulation (red) of 1·(OTf)2 (left) and 3·(OTf)2 (right) in MeCN:PrCN (1:3) at 77K.
Figure 2. EPR spectrum (black) and simulation (red) of 1·(OTf)2 (left) and 3·(OTf)2 (right) in MeCN:PrCN (1:3) at 77K.
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Inorganics 11 00446 g003
Figure 3. Cyclic voltammetry of the copper complexes 1·(Otf)2 (a), 2·Otf (b), 3·(Otf)2 (c), and 4·Otf (d) (0.1 M Bu4NclO4/CH3CN; arrow indicates the initial scan direction). The asterisk (*) corresponds to a trace amount of PicMeN4CuII(H2O) complex.
Figure 3. Cyclic voltammetry of the copper complexes 1·(Otf)2 (a), 2·Otf (b), 3·(Otf)2 (c), and 4·Otf (d) (0.1 M Bu4NclO4/CH3CN; arrow indicates the initial scan direction). The asterisk (*) corresponds to a trace amount of PicMeN4CuII(H2O) complex.
Inorganics 11 00446 g003
Inorganics 11 00446 g004
Figure 4. Variable pH (2.28–11.03) UV-Vis spectra of PicN4 in 0.1 M KCl at 25 °C (left) and its species distribution plot (right). [PicN4]tot = 60 µM.
Figure 4. Variable pH (2.28–11.03) UV-Vis spectra of PicN4 in 0.1 M KCl at 25 °C (left) and its species distribution plot (right). [PicN4]tot = 60 µM.
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Inorganics 11 00446 g005
Figure 5. Variable pH (2.29–11.03) UV-Vis spectra of the PicN4 + Cu2+ system in 0.1 M KCl at 25 °C (left) and its species distribution plot (right). [Cu2+]tot = [PicN4]tot = 50 µM.
Figure 5. Variable pH (2.29–11.03) UV-Vis spectra of the PicN4 + Cu2+ system in 0.1 M KCl at 25 °C (left) and its species distribution plot (right). [Cu2+]tot = [PicN4]tot = 50 µM.
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Inorganics 11 00446 g006
Figure 6. Radio-HPLC chromatograms for the 64Cu labeled complexes of PicN4 and PicMeN4.
Figure 6. Radio-HPLC chromatograms for the 64Cu labeled complexes of PicN4 and PicMeN4.
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Inorganics 11 00446 g007
Figure 7. Cell viability (% of control) of Neuro2A cells upon incubation with PicMeN4, PicN4, and their CuII complexes at 2, 5, 10, and 20 µM concentrations.
Figure 7. Cell viability (% of control) of Neuro2A cells upon incubation with PicMeN4, PicN4, and their CuII complexes at 2, 5, 10, and 20 µM concentrations.
Inorganics 11 00446 g007
Table 1. Selected bond distances (Å) and angles (°) of cations 1–4.
Table 1. Selected bond distances (Å) and angles (°) of cations 1–4.
12+2+32+4+
Cu-N12.056(4)2.1341(1)1.944(9)2.1286(1)
Cu-N22.028(4)2.0817(1)2.173(7)2.0768(2)
Cu-N32.003(4)1.9640(1)1.967(8)1.9461(1)
Cu-N42.276(4)2.3983(1)2.258(7)2.3957(2)
Cu-N52.348(4)2.3456(1)2.165(8)2.262(2)
Cu-N62.017(4)3.3232.219(9)---
N2-Cu-N184.4381.3682.983.07
N4-Cu-N5148.38146.78152.1147.85
φ(°) a86.60, 84.1986.91, 87.9388.07, 89.2888.19, 87.00
θ(°) b36.1928.9220.3931.80
a φ (°) designates the angles between the average plane of two pyridine rings and a mean equatorial plane; b θ (°) designates the angle between the equatorial plane made between atoms N1, N2, and Cu and the plane made between atoms N3, Cu, and N6 for CuII complexes and N3, Cu, and para-carbon on picolyl arm for CuI.
Table 2. Selected EPR Data for Paramagnetic Complexes.
Table 2. Selected EPR Data for Paramagnetic Complexes.
gxgygzAz (G)
1·(OTf)22.0702.0552.259145
3·(OTf)22.0672.0562.264152
Table 3. Selected Physical Parameters of Complexes 1–4.
Table 3. Selected Physical Parameters of Complexes 1–4.
12+2+32+4+
E, V (ΔEp, mV) a,b,c
E1/2 = −0.752 (97)
Eox = 1.047		E1/2 = −0.716 (176)E1/2 = −0.468 (105)
Eox = 1.552		E1/2 = −0.441 (96)
UV-Vis, λmax, nm (ε, M−1 cm−1), MeCN
257 (22,775),
340 (446),
717 (146)		250 (8395),
362 (2438),
444 (893)		258 (12,251),
322 (671),
687 (91)		246 (11,731),
332 (3331),
370 (3854),
435 (1611)
μeff (μB) at 293 K, Evans’ Method, CD3CN
1.80N/A1.71N/A
a Redox Potentials (vs. Fc/Fc+), 0.1 M tBAP/MeCN, 0.01 M Ag/AgNO3 or Ag wire reference, Δep is the separation between anodic and cathodic waves in mV, measured at 100 mV/s. b 12+ & 32+ had 3-segment sweep. c 2+ & 4+ had 5-segment sweep. N/A: not applicable.
Table 4. Acidity constants (pKa) of ligands.
Table 4. Acidity constants (pKa) of ligands.
PicN4PicMeN4
[H4L]4+ = [H3L]3+ + H+-2.47(9)
[H3L]3+ = [H2L]2+ + H+3.60(3)5.46(9)
[H2L]2+ = [HL]+ + H+5.32(0)9.16(9)
[HL] = [L] + H+8.94(6)11.13(8)
Table 5. Stability constants (logK values) and calculated pM values for Cu and Zn complexes. Errors reported for the last digit.
Table 5. Stability constants (logK values) and calculated pM values for Cu and Zn complexes. Errors reported for the last digit.
PicN4 + Cu2+PicMeN4 + Cu2+PicN4 + Zn2+PicMeN4 + Zn2+
M2+ + H2L+ = [MH2L]4+4.13(3)---
M2+ + HL+ = [MHL]3+7.40(1)4.54(1)2.67(2)9.28(7)
M2+ + L = [ML]2+17.96(3)17.07(1)11.45(4)10.41(7)
[ML(H2O)]2+ = [ML(OH)]+ + H+-7.75(2)--
pM2+ (pH 7.4)a16.8112.908.878.02
log(KCu(II)L)17.9617.07--
log(KCu(I)L)7.059.46--
a Values calculated as −log[M]free, where [M2+] = 10−6 M, [L] = 10−5 M.
Table 6. Comparison of log(KCu(II)L) values of commonly used 64Cu chelators.
Table 6. Comparison of log(KCu(II)L) values of commonly used 64Cu chelators.
ChelatorLog(KCu(II)L)Ref.
PicN417.96This work
PicMeN417.07This work
YW-15-Me14.7[7]
DO4S19.6[16]
PCTA19.1[37,38]
EDTA19.2[37,39,40]
TETA21.1[39,40,41,42]
DOTA22.2[39,40,41]
cyclen24.6[39,40]
Table 7. Molecular weight and measured LogD values of the 64Cu complexes.
Table 7. Molecular weight and measured LogD values of the 64Cu complexes.
64Cu ComplexMW (g/mol)log Doct
64Cu-PicN4556.98−1.564 ± 0.26
64Cu-PicMeN4479.90−2.171 ± 0.09
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Blade, G.; Wessel, A.J.; Terpstra, K.; Mirica, L.M. Pentadentate and Hexadentate Pyridinophane Ligands Support Reversible Cu(II)/Cu(I) Redox Couples. Inorganics 2023, 11, 446. https://doi.org/10.3390/inorganics11110446

AMA Style

Blade G, Wessel AJ, Terpstra K, Mirica LM. Pentadentate and Hexadentate Pyridinophane Ligands Support Reversible Cu(II)/Cu(I) Redox Couples. Inorganics. 2023; 11(11):446. https://doi.org/10.3390/inorganics11110446

Chicago/Turabian Style

Blade, Glenn, Andrew J. Wessel, Karna Terpstra, and Liviu M. Mirica. 2023. "Pentadentate and Hexadentate Pyridinophane Ligands Support Reversible Cu(II)/Cu(I) Redox Couples" Inorganics 11, no. 11: 446. https://doi.org/10.3390/inorganics11110446

APA Style

Blade, G., Wessel, A. J., Terpstra, K., & Mirica, L. M. (2023). Pentadentate and Hexadentate Pyridinophane Ligands Support Reversible Cu(II)/Cu(I) Redox Couples. Inorganics, 11(11), 446. https://doi.org/10.3390/inorganics11110446

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