key: cord-0977741-mfe4dfne
authors: Ivoilova, Alexandra; Mikhalchenko, Ludmila V.; Tsmokalyuk, Anton; Leonova, Marina; Lalov, Andrey; Mozharovskaia, Polina; Kozitsina, Alisa N.; Ivanova, Alla V.; Rusinov, Vladimir L.
title: Redox Conversions of 5-Methyl-6-nitro-7-oxo-4,7-dihydro-1,2,4triazolo[1,5-a]pyrimidinide L-Arginine Monohydrate as a Promising Antiviral Drug
date: 2021-08-22
journal: Molecules
DOI: 10.3390/molecules26165087
sha: f335b874c57d8c1b1241bf160e76f4eb0120f8e7
doc_id: 977741
cord_uid: mfe4dfne

This article presents the results of a study of electrochemical transformations in aqueous and aprotic media of 5-methyl-6-nitro-7-oxo-4,7-dihydro-1,2,4-triazolo[1,5-a]pyrimidinide l-arginine monohydrate (1a, Triazid) obtained by electrochemical methods and ESR spectroscopy. The effect of pH on the current and the reduction potential of 1a in an aqueous Britton–Robinson buffer solution was studied. It was found that 1a is irreversibly reduced in aqueous acidic media on a glassy carbon electrode in one stage with the participation of six electrons and the formation of 5-methyl-6-amino-7-oxo-1,2,4-triazolo[1,5-a]pyrimidin. The electroreduction of 1a in DMF on a background of tetrabutylammonium salts proceeds in two stages, controlled by the kinetics of second-order reactions. In the first stage, the reduction of 1a is accompanied by protonation by the initial compound of the basic intermediate products formed in the electrode reaction (self-protonation mechanism). The second quasi-reversible stage of the electroreduction 1a corresponds to the formation of a dianion radical upon the reduction of the heterocyclic anion 5-methyl-6-nitro-7-oxo-4,7-dihydro-1,2,4-triazolo[1,5-a]pyrimidin, which is formed upon the potentials of the first peak. The ESR spectrum of the radical dianion was recorded upon electroreduction of Triazid in the presence of Bu(4)NOH. The effect of the formation of ion pairs on the reversibility of the second peak of the 1a transformation is shown. A change in the rate and regioselectivity of the protonation of the dianion radical in the presence of Na(+) and Li(+) ions is assumed. The results of studying the electroreduction of 1a by ESR spectroscopy with a TEMPO trap make it possible to assume the simultaneous formation of both a nitroxyl radical and a radical with the spin density localized on the nitrogen at the 4 position of the six-membered ring.

It is known that influenza viruses, because of their mutation, are one of the most common and widely spread illnesses. This leads to some difficulties in dealing with influenza. In this regard, the creation of new, more active, and safe medicinal antiviral drugs does not lose its relevance [1] [2] [3] [4] .

Currently, there is a certain pharmacological niche of drugs based on nitro compounds that are effective against various types of influenza. In recent decades, nitro compounds of an aromatic and heterocyclic nature have attracted considerable attention since they are its maintenance in aqueous solutions [21] . Therefore, the goal of this work was to study the possible pathways of the redox transformation of the molecule 5-methyl-6-nitro-7-oxo-4,7-dihydro-1,2,4-triazolo [1,5-a] pyrimidinide l-arginine monohydrate (Triazid), the comparison of its reactivity with the sodium salt of 2-methylthio-6-nitro-7-oxo-1,2,4-triazolo [5,1-c] [1, 2, 4] triazin, dihydrate (Triazavirin ® ), and the identification of possible intermediate products of the electroreduction of Triazid using electrochemical methods and ESR spectroscopy.

5-Methyl-6-nitro-7-oxo-4,7-dihydro-1,2,4-triazolo[1,5-a]pyrimidinide l-arginine monohydrate (1a, Triazid), sodium salt of 5-methyl-6-nitro-7-oxo-4,7-dihydro-1,2,4-triazolo [1,5-a] pyrimidine (1b), sodium salt of 2-methylthio-6-nitro-7-oxo-1,2,4-triazolo- [5,1c] [1, 2, 4] triazin, dihydrate (2a, Triazavirin ® ), and 2-methylthio-6-nitro-7-oxo-1,2,4-triazolo- [5,1-c] [1, 2, 4] triazin (2b) were synthesized at the Department of Organic and Biomolecular Chemistry, Ural Federal University. The structure of the compounds (Scheme 1) was determined using NMR spectroscopy, IR and UV spectroscopy, and elemental analysis [22] [23] [24] . To conduct a study of the electroreduction of substances, aqueous solutions of 0.1 M nitric acid of the puriss grade from the USA manufacturer Sigma-Aldrich ® , St. Louis and Britton-Robinson (BR) buffers were used. The solutions were prepared in distilled water. Britton-Robinson solutions were prepared by mixing orthophosphoric, acetic, and boric acids and adjusting to the required pH with sodium hydroxide according to [25] . We used acids and salts of the puriss grade from the Spain Barcelona manufacturer PanReac without additional purification. To prepare solutions, we used deionized water obtained on a DVS-M/1NA (18)-N unit from Mediana-Filter, Moscow,Russia.

To carry out the study in aprotic solutions, acetonitrile of the puriss. spec. grade from the USA manufacturer PanReac was used without additional purification. In addition, DMF and DMSO of the puriss. spec. grade from the USA manufacturer Sigma-Aldrich ® with preliminary distillation [26] in the presence of a molecular sieve were used. We used To conduct a study of the electroreduction of substances, aqueous solutions of 0.1 M nitric acid of the puriss grade from the USA manufacturer Sigma-Aldrich ® , St. Louis and Britton-Robinson (BR) buffers were used. The solutions were prepared in distilled water. Britton-Robinson solutions were prepared by mixing orthophosphoric, acetic, and boric acids and adjusting to the required pH with sodium hydroxide according to [25] . We used acids and salts of the puriss grade from the Spain Barcelona manufacturer PanReac without additional purification. To prepare solutions, we used deionized water obtained on a DVS-M/1NA (18)-N unit from Mediana-Filter, Moscow,Russia.

To carry out the study in aprotic solutions, acetonitrile of the puriss. spec. grade from the USA manufacturer PanReac was used without additional purification. In addition, DMF and DMSO of the puriss. spec. grade from the USA manufacturer Sigma-Aldrich ® with preliminary distillation [26] in the presence of a molecular sieve were used. We used lithium perchlorate and tetrabutylammonium tetrafluoroborate of the puriss. spec. grade from the USA manufacturer Sigma-Aldrich ® .

To detect the radical, N-(1-hydroxy-2,2,6,6-tetramethylpiperidin-4-yl-)-2-methylpropanamide hydrochloride (TMTH) (Novosibirsk Institute of Organic Chemistry, Russia) was used as a spin probe [27, 28] . As a spin trap, 3,3,5,5-tetramethyl-1-pyrroline N-oxide (TEMPO) (Sigma-Aldrich ® , St. Louis, MI, USA, CAS No. 244007) was used [29, 30] .

Cyclic voltammograms (CVs) and chronoamperograms (CAs) were carried out using a µAutolab Type III potentiostat/galvanostat (Metrohm, Switzerland). Glassy carbon disks (Ø 2 and 5 mm stationary or rotating, respectively) were used as a working electrode. The surface of the working electrode was mechanically cleaned before each measurement. A saturated Ag/AgCl/KClsat electrode acted as a reference electrode in an aqueous medium, and a graphite electrode was used as the auxiliary electrode (Metrohm, Switzerland). The potentials of the working electrode in aprotic solutions were measured relative to a silver chloride reference electrode with two Ag/AgCl/KClsat/DMF membranes or a saturated calomel electrode (SCE). The CA was recorded at the potentials of the limiting current of electroreduction of compounds in the time interval of 0 < t < 5 s, and the logarithmic analysis of the chronoamperograms was performed in the interval of 1 < t < 2 s. The working solutions were purged with argon with a purity of 99.9% for 15 min before each measurement. Aqueous buffer solutions of Britton-Robinson (BR) or 0.1 M nitric acid were used as supporting electrolytes. The pH measurements were carried out on an Expert-pH ion meter (Econiks-Expert, Russia) and an EV-74 universal ion meter.

Each voltammogram was recorded three times. The mean peak current and the confidence interval were calculated (p = 0.95.)

ESR spectra were registered using a Bruker Elexsys E 500 spectrometer (Germany, Rheinstetten) with an ER4122SHQE resonator and Bruker EMX 6/1 (Germany Rheinstetten) spectrometer equipped with ER4102ST rectangular cavity equipped with two electrode convex Pt/Pt electrolytic cells controlled by a Zahner IM-6 potentiostat.

The generation of Triazid reduction products with a concentration of 0.01 M was carried out with the addition of a 0.01 M spin probe TMTH over 1/5/10/15 min. After the indicated time intervals, an aliquot of the solution was taken, and the ESR spectrum was recorded. To control the number of probes appearing in the background solution, the products were generated in a similar way and at the same potential without adding Triazid. Aliquots were taken after 1/5/10/15 min of generation, and the ESR spectra were recorded.

Before each experiment, the working solution was purged with argon. Simultaneous Electrochemical Experiment ESR (SEESR) was used to detect paramagnetic particles during 1a reduction. The spectra of the radical anion were recorded at a potential of −2 V in a two-electrode Pt/Pt electrochemical cell placed in the resonator of an ESR spectrometer. The half-life of the species detected was less than 0.01 s.

All quantum chemical calculations in the field of ESR were performed by the ORCA [31] [32] [33] ver. 5.0.0 program package using a hybrid PBE0 [34] density functional in a triple-zeta basis set with two polarization functions def2-TZVPP [35] and atom-pairwise dispersion correction with the Becke-Johnson damping scheme (D3BJ) [36] , and respect to the effects of solvation in the SMD continuum [37] were included in all calculations. TightSCF convergence criteria were applied throughout. Full geometry optimization with TightOpt convergence criteria was carried out to find stationary points on the potential energy surfaces. Numerical harmonic frequency calculations were used to obtain thermodynamic quantities and verify that all stationary points found were local minima. Visualization of molecular orbitals were produced using the Avogadro program [38, 39] .

ESR spectra were recorded with a TEMPO spin trap [29, 30] after preliminary generation of Triazid 1a reduction products with a concentration of 0.1 M in DMSO in a conventional electrochemical cell for 15 min in the presence of a spin trap. An aliquot of the resulting solution was taken, and the ESR spectrum was recorded. The simulation and visualization of the calculated ESR spectra with traps were performed using the EasySpin 5.3 software package [40] .

3.1. Electrochemical Behavior of Compounds 1a and 1b in Aqueous Media Figure 1 shows the CV of the first stages of the electroreduction of the studied compounds in an aqueous acidic medium.

ESR spectra were recorded with a TEMPO spin trap [29, 30] after preliminary generation of Triazid 1a reduction products with a concentration of 0.1 M in DMSO in a conventional electrochemical cell for 15 min in the presence of a spin trap. An aliquot of the resulting solution was taken, and the ESR spectrum was recorded.

The simulation and visualization of the calculated ESR spectra with traps were performed using the EasySpin 5.3 software package [40] . Figure 1 shows the CV of the first stages of the electroreduction of the studied compounds in an aqueous acidic medium. The investigated compounds 1a and 1b in 0.1 M HNO3 were irreversibly reduced at the potential values -0.71 and -0.56 V, respectively. These potentials are comparable to the potentials of heterocyclic nitro compounds with a nitro group in their structure [6, 17, 19, 41, 42] . The value of the potential of the electroreduction of 1a in a buffer solution at a pH of 2 is −0.63 V. Previously, we studied the electroreduction of compound 1a in a buffer solution with a pH value of 2 [20] . A comparison of the CV of compounds 1a and 2a showed that under the same conditions (BR pH = 2), the latter undergoes reduction processes at potential values 250 mV higher than the former. The difference in the ER potentials is probably due to the presence of an additional electronegative nitrogen atom in the six-membered ring of the condensed heterocyclic system 2a. Another difference in the electrochemical behavior of these nitro compounds is the fact that in acidic and neutral media, 2a is reduced in two subsequent, irreversible stages, while the irreversible peak of the ER of 1a is the only one up to the background discharge potential (Figure S1 Supplementary Materials).

As shown in Figure 1 , irreversible peaks of the ER products 1a and 1b are observed in nitric acid at potentials +0.68 and +0.67 V, respectively, on the anodic part of the voltammograms after changing the direction of the potential sweep. The anion of the corresponding hydroxylamino derivative is probably oxidized at these potentials. The closeness of the values of these oxidation potentials indicates the formation of electroreduction products similar in structure to compounds 1a and 1b.

To determine the effective number of electrons ne involved in the electrochemical reduction reaction, the current of the first stage of the reduction of compound 1a at a pH of The investigated compounds 1a and 1b in 0.1 M HNO 3 were irreversibly reduced at the potential values -0.71 and -0.56 V, respectively. These potentials are comparable to the potentials of heterocyclic nitro compounds with a nitro group in their structure [6, 17, 19, 41, 42] . The value of the potential of the electroreduction of 1a in a buffer solution at a pH of 2 is −0.63 V. Previously, we studied the electroreduction of compound 1a in a buffer solution with a pH value of 2 [20] . A comparison of the CV of compounds 1a and 2a showed that under the same conditions (BR pH = 2), the latter undergoes reduction processes at potential values 250 mV higher than the former. The difference in the ER potentials is probably due to the presence of an additional electronegative nitrogen atom in the six-membered ring of the condensed heterocyclic system 2a. Another difference in the electrochemical behavior of these nitro compounds is the fact that in acidic and neutral media, 2a is reduced in two subsequent, irreversible stages, while the irreversible peak of the ER of 1a is the only one up to the background discharge potential (Figure S1 Supplementary Materials).

As shown in Figure 1 , irreversible peaks of the ER products 1a and 1b are observed in nitric acid at potentials +0.68 and +0.67 V, respectively, on the anodic part of the voltammograms after changing the direction of the potential sweep. The anion of the corresponding hydroxylamino derivative is probably oxidized at these potentials. The closeness of the values of these oxidation potentials indicates the formation of electroreduction products similar in structure to compounds 1a and 1b.

To determine the effective number of electrons n e involved in the electrochemical reduction reaction, the current of the first stage of the reduction of compound 1a at a pH of 2 in the CV was compared with the current calculated using the Rendles-Shevchik equation for irreversible electrochemical reactions [43] and the current of the standard reversible redox system Fe(CN) 6 3− /Fe(CN) 6 4− under the same conditions (Table 1 ). In addition, the number of electrons participating in the ER of compound 1a was determined from the value of the limiting current at the rotating disk electrode (n e RDE), the value of the chronoamperogram current at t = 1 s (n e CA), and the amount of electricity in the interval t from 1 to 2 s, in comparison with the amount of electricity passing under the same conditions at the potential of the limiting recovery current of the model compound (n e CC). The results are presented in Table 1 , and similar values for 2a are given for comparison. The value of the effective number of electrons n e of the first stage of the electroreduction of compound 2a was equal to 4e, which suggests the reduction of the nitro group to hydroxylamine [20] . Under the same conditions, the value of n e during the electroreduction of compound 1a is approximately the value 6e. That is, it can be assumed that the intermediate electroreduction products of compound 1a are electrochemically active at the same potentials, in contrast to the electroreduction products of compound 2a, which are reduced at more negative potentials.

The graph of changes in the limiting current ER of compound 1a (I lim ) at a pH of 2 on voltammograms obtained at different speeds of rotation of the disk electrode (ω) in the coordinates I lim from ω 0.5 is linear but does not pass through the origin of the coordinates ( Figure S2 in Supplementary Materials). The current of the ER peak in the CV curves versus υ 0.5 also grows nonlinearly (Figure 2 ), and the degree of deviation from the straight line depends on the acidity of the medium. As shown in Figure 2 , the value of the peak current of the ER of 1a deviated from that theoretically calculated by the Rendls-Shevchik equation for irreversible processes [43] at high values of v ≥ 0.75 V·s −1 in the acidic region. At pH 7, the peak current was close to the theoretically calculated one only at low v. The decrease in the peak current for the ER of As shown in Figure 2 , the value of the peak current of the ER of 1a deviated from that theoretically calculated by the Rendls-Shevchik equation for irreversible processes [43] at high values of v ≥ 0.75 V·s −1 in the acidic region. At pH 7, the peak current was close to the theoretically calculated one only at low v. The decrease in the peak current for the ER of 1a in alkaline media (pH > 10) at all values of the potential v is explained [17] by the insufficient protonation rate of the RA due to the low proton concentration. It follows from these data that the electrochemical reaction of the ER of 1a is controlled by kinetics.

The reduction current in the CV of compound 1a ( Figure 3B ) in an acidic medium, within the measurement errors, had a maximum current value close to the value of the transfer of 6e to the 1a molecule. At a pH above 4 and in the neutral pH range, the current gradually decreased. At pH values of 10-12, the value of current the ER of compound 1a practically did not change and was only approximately 20% of the maximum value of the ER current of 1a. Such a decrease in the current of the ER of 1a is probably associated with a decrease in the rate of protonation of intermediate anionic species due to the low concentration of protons. However, the electroreduction of compound 1a remained irreversible under these conditions. Preparative electrolysis of compound 1a was carried out in an acidic medium (for electrolysis conditions of 1a, see Supplementary Materials). The obtained data from the electrochemical studies of both NMR and mass spectroscopy ( Figures S3 and S4 in Supplementary Materials) suggest that the ER of 1a in aqueous acidic media proceeds at the nitro group of the compound with the participation of 6 electrons per molecule and leads to the formation of the corresponding heterocyclic amine:

The end product of electroreduction, 5-Methyl-6-amino-7-oxo-4,7-dihydro-1,2,4-triazolo[1,5-a]pyrimidine, was isolated at a yield of 82% after electrolysis of the solution of 1a in a BR buffer solution at a pH of 2.

The product was obtained as a precipitate upon cooling the catholyte and was not associated with l-arginine ( Figures S3 and S4 in Supplementary Materials) It is known [19, 44, 45] that in some cases, when an organic solvent is added to aqueous buffer solutions, the six-electron peak of the nitro group reduction can be divided into two stages. In the CV data of compound 1a, two stages of electroreduction were observed (5 mM) when 40% DMF was added to the Britton-Robinson buffer solution in the range of 9 > pH > 12, but both stages remained irreversible. In acidic and neutral media, the addition of 40% DMF or more did not lead to a separation of the ER peak of compound 1a ( Figure S5 in Supplementary Materials) These results indicate a high rate of protonation of the formed intermediate particles, which results in the formation of compounds electrochemically active at these potentials.

A comparison of the CV data for compounds 1a and 1b ( Figure 1 ) indicated another interesting detail: the currents of the ER of 1a and 1b were practically equal, while the ER potentials of these compounds in 0.1 M HNO3 differed noticeably by approximately 150 mV. However, it would seem that because both compounds were in an acidic medium, they should be protonated and reduced in the same protonated form. The difference in With an increase in the pH of the background electrolyte solution of 3 < pH < 6, the maximum of the reduction peak 1a shifted toward negative potential values ( Figure 3A) , with ∆E/∆pH = 30 mV, and at a pH > 6, it remained almost unchanged.

Preparative electrolysis of compound 1a was carried out in an acidic medium (for electrolysis conditions of 1a, see Supplementary Materials). The obtained data from the electrochemical studies of both NMR and mass spectroscopy ( Figures S3 and S4 in Supplementary Materials) suggest that the ER of 1a in aqueous acidic media proceeds at the nitro group of the compound with the participation of 6 electrons per molecule and leads to the formation of the corresponding heterocyclic amine: -HetNO 2 NH 3 + -R-COOH + 6e + 6H + → HHetNH 2 + NH 3 + -R-COO − +2H 2 O The end product of electroreduction, 5-Methyl-6-amino-7-oxo-4,7-dihydro-1,2,4-triazolo [1,5-a]pyrimidine, was isolated at a yield of 82% after electrolysis of the solution of 1a in a BR buffer solution at a pH of 2.

The product was obtained as a precipitate upon cooling the catholyte and was not associated with l-arginine ( Figures S3 and S4 in Supplementary Materials).

It is known [19, 44, 45] that in some cases, when an organic solvent is added to aqueous buffer solutions, the six-electron peak of the nitro group reduction can be divided into two stages. In the CV data of compound 1a, two stages of electroreduction were observed (5 mM) when 40% DMF was added to the Britton-Robinson buffer solution in the range of 9 > pH > 12, but both stages remained irreversible. In acidic and neutral media, the addition of 40% DMF or more did not lead to a separation of the ER peak of compound 1a ( Figure S5 in Supplementary Materials) These results indicate a high rate of protonation of the formed A comparison of the CV data for compounds 1a and 1b (Figure 1 ) indicated another interesting detail: the currents of the ER of 1a and 1b were practically equal, while the ER potentials of these compounds in 0.1 M HNO 3 differed noticeably by approximately 150 mV. However, it would seem that because both compounds were in an acidic medium, they should be protonated and reduced in the same protonated form. The difference in ER potentials is probably determined by the influence of counterions. The formation of ion pairs of alkali metal ions and small organic cations with anionic particles has been the subject of previous studies [46, 47] . They showed that the formation of ion pairs leads to a change in the distribution of electron density in the radical anion (RA), which affects the reduction potential of compounds. The difference in the ER potentials of compounds 1a and 1b is probably related to the effect of Na + ions; 5 mM Na + is added to the solution together with 1b, and in the case of the ER of 1a, the bulky amino acid cation should have little effect on the electron density distribution in RA 1a. In a BR solution at a pH of 2, a slight decrease in the peak current and a slight shift in the potential of the ER of 1a to the positive region (−0.63 V) compared with the HNO 3 solution are possibly related to the presence of Na + ions.

In an aprotic medium, anionic intermediate particles formed during reduction are protonated more slowly than they are in an aqueous medium. Therefore, a study of 1a in DMF and acetonitrile was carried out with the aim of registering intermediate electroreduction particles. The electrochemical behavior of 1a in aprotic solvents was found to be similar. In the CV results 1a in DMF, two ER peaks were observed (Figure 4 ). The first of them was an irreversible flat ER peak at −1.22 V, with the next stage at −1.63 V. According to the CV and CA data, the current value of the first stage of the ER of 1a was noticeably lower than the current of the peak of the one-electron oxidation of ferrocene under the same conditions and varied nonlinearly in the concentration range of 0.6 to 8 mM ( Figure 5A ). In the range of working concentrations of 1-3 mM, the current of the first peak is was approximately half the current of a one-electron transfer. As shown by the results of the CV of l-arginine hydrochloride, neither the l-arginine cation nor its anion obtained by adding alkali were not reduced under these conditions. No paramagnetic activity was recorded in l-arginine solutions when the potential was applied under CV conditions. This indicates that, most likely, an electron is transferred to the heterocyclic part of salt 1a. According to the results of quantum-chemical calculations of the energies of the lowest vacant molecular orbital of the heterocyclic anion (LUMO) and the energy of the single-occupied molecular orbital (SOMO) of the dianion radical (DAR) formed during its ER (Figure 6 ), the most likely explanation that the transfer of electrons to the nitro group and a double bond of a six-membered ring. Since 1a is a salt formed by a heterocyclic anion and an amino acid, it can be assumed that the transfer of the first electron at the potentials of the first stage is accompanied by rapid protonation of the formed ER product by the initial depolarizer-so-called self-protonation [48, 49] . The amino acid l-arginine, which is part of compound 1a, is a good proton donor. The pKa value of the first stage in the aqueous medium is 2.17 [50] . The pKa value of compound 1a in water was determined potentiometrically to be 3.45. Therefore, in an aprotic medium, 1a can act as a proton donor.

The dependence of the current of the first peak I1 of the reduction of 1a on v 0.5 in an aprotic medium (Figure 7) is linear and passes through the origin only in the region of As shown by the results of the CV of l-arginine hydrochloride, neither the l-arginine cation nor its anion obtained by adding alkali were not reduced under these conditions. No paramagnetic activity was recorded in l-arginine solutions when the potential was applied under CV conditions. This indicates that, most likely, an electron is transferred to the heterocyclic part of salt 1a. According to the results of quantum-chemical calculations of the energies of the lowest vacant molecular orbital of the heterocyclic anion (LUMO) and the energy of the single-occupied molecular orbital (SOMO) of the dianion radical (DAR) formed during its ER (Figure 6 ), the most likely explanation that the transfer of electrons to the nitro group and a double bond of a six-membered ring. As shown by the results of the CV of l-arginine hydrochloride, neither the l-arginine cation nor its anion obtained by adding alkali were not reduced under these conditions. No paramagnetic activity was recorded in l-arginine solutions when the potential was applied under CV conditions. This indicates that, most likely, an electron is transferred to the heterocyclic part of salt 1a. According to the results of quantum-chemical calculations of the energies of the lowest vacant molecular orbital of the heterocyclic anion (LUMO) and the energy of the single-occupied molecular orbital (SOMO) of the dianion radical (DAR) formed during its ER (Figure 6 ), the most likely explanation that the transfer of electrons to the nitro group and a double bond of a six-membered ring. Since 1a is a salt formed by a heterocyclic anion and an amino acid, it can be assumed that the transfer of the first electron at the potentials of the first stage is accompanied by rapid protonation of the formed ER product by the initial depolarizer-so-called self-protonation [48, 49] . The amino acid l-arginine, which is part of compound 1a, is a good proton donor. The pKa value of the first stage in the aqueous medium is 2.17 [50] . The pKa value of compound 1a in water was determined potentiometrically to be 3.45. Therefore, in an aprotic medium, 1a can act as a proton donor. Since 1a is a salt formed by a heterocyclic anion and an amino acid, it can be assumed that the transfer of the first electron at the potentials of the first stage is accompanied by rapid protonation of the formed ER product by the initial depolarizer-so-called selfprotonation [48, 49] . The amino acid l-arginine, which is part of compound 1a, is a good proton donor. The pKa value of the first stage in the aqueous medium is 2.17 [50] . The pKa value of compound 1a in water was determined potentiometrically to be 3.45. Therefore, in an aprotic medium, 1a can act as a proton donor.

The dependence of the current of the first peak I 1 of the reduction of 1a on v 0.5 in an aprotic medium (Figure 7) is linear and passes through the origin only in the region of low rates of potential application <2 Vs −1 . The obtained data allow us to assume that at the potentials of the first stage, E1, the most rapid reaction is self-protonation leading to the formation of an electrochemically inactive heterocyclic anion Het − at E1:

Proton transfer can probably proceed not only intermolecularly, but also intramolecularly, as well as through several reaction centers. As a result, the formation of radicals with different positions of the spin density of the unpaired electron and, consequently, different reactivity is possible (Supplementary Materials Scheme S1).

The second stage of the electroreduction of compound 1a is quasi-reversible. On the reverse curve after the second peak in the concentration range of 1.6-3.0 mM, an anodic peak was recorded at E = −1.54 V and ΔEp was approximately 90 mV. The value of the current at the potentials of the second stage of the ER I2 increased with increasing concentration ( Figure 5A ), but the linear plot of the dependence of I2 in the C1a 0.6-3.0 mM interval does not pass through the origin. With an increase in the concentration of 1a, the ratio of the currents at the potentials of the second I2 and the first I1 stages I2/I1 also increased ( Figure 5B ), which suggests reduction at the potentials of the second stage of the secondorder chemical reaction product. The potentials of the second peak, mainly the heterocyclic anion formed at the potentials of the first stage of the ER of 1a, are probably reduced.

Het -+ e → [Het] = E2 The obtained data allow us to assume that at the potentials of the first stage, E 1 , the most rapid reaction is self-protonation leading to the formation of an electrochemically inactive heterocyclic anion Het − at E 1 :

+ -R-COO − Proton transfer can probably proceed not only intermolecularly, but also intramolecularly, as well as through several reaction centers. As a result, the formation of radicals with different positions of the spin density of the unpaired electron and, consequently, different reactivity is possible (Supplementary Materials Scheme S1).

The second stage of the electroreduction of compound 1a is quasi-reversible. On the reverse curve after the second peak in the concentration range of 1.6-3.0 mM, an anodic peak was recorded at E = −1.54 V and ∆Ep was approximately 90 mV. The value of the current at the potentials of the second stage of the ER I 2 increased with increasing concentration ( Figure 5A ), but the linear plot of the dependence of I 2 in the C 1a 0.6-3.0 mM interval does not pass through the origin. With an increase in the concentration of 1a, the ratio of the currents at the potentials of the second I 2 and the first I 1 stages I 2 /I 1 also increased ( Figure 5B ), which suggests reduction at the potentials of the second stage of the second-order chemical reaction product. The potentials of the second peak, mainly the heterocyclic anion formed at the potentials of the first stage of the ER of 1a, are probably reduced.

Het -+ e → [Het] = E 2 The oxidation peak of the dianion radical (DAR) on the reverse at a potential of −1.54 V was approximately half of the second cathodic peak at v = 0.1 Vs −1 (Figure 4) , and with an increase in v to 5 Vs −1 , the value of I a /I c increased to 0.74.

The peak current of the second stage of electroreduction of compound 1a from v 0.5 in an aprotic medium changed nonlinearly (Figure 7 ). An increase in the v led to a relative decrease in the currents of both cathodic peaks. Moreover, the I 2 /I 1 ratio at a high v (above 2 Vs −1 ) remained constant and approximately equal to 2, while at v = 50 mV s −1 , it exceeded 4. It can be assumed that the protonation reaction of DAR (with the initial compound and/or donor impurities in the solution) has time to proceed at low values v, which leads to an increase in the second cathodic peak and a decrease in the anodic peak at −1.54 V in the CV of compound 1a.

The gradual addition of Bu 4 NOH alkali caused a decrease and complete disappearance of the current of the first stage ( Figure 8A ) at an equivalent alkali content, while the current value of the second stage remained practically unchanged. leads to an increase in the second cathodic peak and a decrease in the anodic peak at −1.54 V in the CV of compound 1a.

The gradual addition of Bu4NOH alkali caused a decrease and complete disappearance of the current of the first stage ( Figure 8A ) at an equivalent alkali content, while the current value of the second stage remained practically unchanged. It is interesting to note that the anodic peak of −1.54V increased under these conditions, and the Ia/Ic value was 0.7 when the Bu4NOH content was two times higher than the 1a concentration. This result can be considered a confirmation of the assumption that the DAR formed at the potentials of the second stage of the ER of compound 1a disappears as a result of the protonation reaction. An increase in the rate of potential deposition or a decrease in the content of proton donors due to the addition of alkali makes it possible to register a higher current of its oxidation at a potential of −1.54 V:

Het -NH3 + -R-COOH + OH − → Het -+ NH3 + -R-COO − +H2O Het -+ e → [Het] = The formation of dianion radicals was also shown for a number of 1,2,4-nitrotriazoles [51] .

It is important to note that the addition of an aqueous NaOH solution to a solution of 1a had a different effect on the cathodic peaks of the CVs of the compound ( Figure 8B ). The addition of NaOH to a solution of 1a in DMF also led to the disappearance of the first stage of the ER. The second stage became irreversible, while the potential of the ER shifted to more positive potentials, and the current increased. Apparently, these changes can be associated with the formation of ion pairs between the heterocyclic anion 1a and Na + ions, in which the electron density at the reaction center increases under the influence of the cation, and the protonation of DAR proceeds at a higher rate. When Bu4NOH was added to the solution instead of NaOH ( Figure 8A ), ion pairs with the heterocyclic anion were not formed since the charge density in the bulk cation Bu4N + is significantly lower than that in the Na + ion. As a result, the reversible ER of the 1a anion was observed on the CVs. Figure 9 shows the cyclic voltammograms of the solution of 1a in the presence of added LiClO4. These were made in order to exclude the effect of the water added with alkali to the DMF solution and to study the effect of a cation even smaller than Na + . It is interesting to note that the anodic peak of −1.54V increased under these conditions, and the I a /I c value was 0.7 when the Bu 4 NOH content was two times higher than the 1a concentration. This result can be considered a confirmation of the assumption that the DAR formed at the potentials of the second stage of the ER of compound 1a disappears as a result of the protonation reaction. An increase in the rate of potential deposition or a decrease in the content of proton donors due to the addition of alkali makes it possible to register a higher current of its oxidation at a potential of −1.54 V:

Het -NH 3 + -R-COOH + OH − → Het -+ NH 3 + -R-COO − +H 2 O Het -+ e → [Het] = The formation of dianion radicals was also shown for a number of 1,2,4-nitrotriazoles [51] . It is important to note that the addition of an aqueous NaOH solution to a solution of 1a had a different effect on the cathodic peaks of the CVs of the compound ( Figure 8B ). The addition of NaOH to a solution of 1a in DMF also led to the disappearance of the first stage of the ER. The second stage became irreversible, while the potential of the ER shifted to more positive potentials, and the current increased. Apparently, these changes can be associated with the formation of ion pairs between the heterocyclic anion 1a and Na + ions, in which the electron density at the reaction center increases under the influence of the cation, and the protonation of DAR proceeds at a higher rate. When Bu 4 NOH was added to the solution instead of NaOH ( Figure 8A ), ion pairs with the heterocyclic anion were not formed since the charge density in the bulk cation Bu 4 N + is significantly lower than that in the Na + ion. As a result, the reversible ER of the 1a anion was observed on the CVs. Figure 9 shows the cyclic voltammograms of the solution of 1a in the presence of added LiClO 4 . These were made in order to exclude the effect of the water added with alkali to the DMF solution and to study the effect of a cation even smaller than Na + . By comparing the influences of LiClO4 and NaOH, it can be noted that the presence of LiClO4, in contrast to that of NaOH, does not affect the first stage of the ER of 1a, but the second stage of ER in the presence of both compounds becomes irreversible and the reduction current increases, probably due to the protonation of the resulting products. In addition, in both cases, oxidation peaks appear on the anodic reversal curve at close potentials in the range of −0.5 to −0.3V. It is possible that in the presence of alkali metals, not only does the rate of protonation of 1a dianion radicals change, but the regioselectivity of the chemical reaction also changes. It should be emphasized that the ESR signal could not be detected in the presence of Li + ions when LiOH was added to a solution of 1a in DMF.

The electron density of the lowest free molecular orbital (LUMO) of the heterocyclic anion 1a was theoretically calculated to determine the possible reduction centers ( Figure  6 ). From these calculations, two possible pathways for the formation of radicals were suggested. The first, which is the most probable, is the reduction of the nitro group with the formation of a nitroxyl radical, and the second is the formation of a radical on the nitrogen at the 4 position of the six-membered ring of the heterocycle.

Preliminary reduction of 1a was carried out at a peak potential of E = −1.7 V in a DMSO solution in the presence of a TMTH spin probe to detect the formation of radical products during the ER of 1a. The obtained experimental data indicate the appearance of radicals in the solution of the electrochemical cell during electrolysis. A significant increase in the number of paramagnetic centers in the solution of the electrochemical cell during the entire electrolysis process for 1a ( Figure S6 in Supplementary Materials) was observed. In addition, a linear relationship between the number of spins and the time spent on the electroreduction of the products of 1a was observed ( Figure S6 tab in Supplementary Materials).

The high reactivity of the anionic particles formed during the ER of 1a, primarily in the protonation reactions, makes it difficult to obtain high-intensity ESR spectra. Therefore, the ER of 1a c was carried out in an SEESR experiment in the presence of Bu4NOH.

The SEESR experiment was used for the detection of paramagnetic species during the reduction of 1a. Figure 10 gives examples of the experimental and simulated spectra By comparing the influences of LiClO 4 and NaOH, it can be noted that the presence of LiClO 4 , in contrast to that of NaOH, does not affect the first stage of the ER of 1a, but the second stage of ER in the presence of both compounds becomes irreversible and the reduction current increases, probably due to the protonation of the resulting products. In addition, in both cases, oxidation peaks appear on the anodic reversal curve at close potentials in the range of −0.5 to −0.3V. It is possible that in the presence of alkali metals, not only does the rate of protonation of 1a dianion radicals change, but the regioselectivity of the chemical reaction also changes. It should be emphasized that the ESR signal could not be detected in the presence of Li + ions when LiOH was added to a solution of 1a in DMF.

The electron density of the lowest free molecular orbital (LUMO) of the heterocyclic anion 1a was theoretically calculated to determine the possible reduction centers ( Figure 6 ). From these calculations, two possible pathways for the formation of radicals were suggested. The first, which is the most probable, is the reduction of the nitro group with the formation of a nitroxyl radical, and the second is the formation of a radical on the nitrogen at the 4 position of the six-membered ring of the heterocycle.

Preliminary reduction of 1a was carried out at a peak potential of E = −1.7 V in a DMSO solution in the presence of a TMTH spin probe to detect the formation of radical products during the ER of 1a. The obtained experimental data indicate the appearance of radicals in the solution of the electrochemical cell during electrolysis. A significant increase in the number of paramagnetic centers in the solution of the electrochemical cell during the entire electrolysis process for 1a ( Figure S6 in Supplementary Materials) was observed. In addition, a linear relationship between the number of spins and the time spent on the electroreduction of the products of 1a was observed ( Figure S6 tab in Supplementary Materials).

The high reactivity of the anionic particles formed during the ER of 1a, primarily in the protonation reactions, makes it difficult to obtain high-intensity ESR spectra. Therefore, the ER of 1a c was carried out in an SEESR experiment in the presence of Bu 4 NOH.

The SEESR experiment was used for the detection of paramagnetic species during the reduction of 1a. Figure 10 gives examples of the experimental and simulated spectra of the radical anion generation recorded at a potential of −2 V in a two-electrode Pt/Pt electrochemical cell placed in the resonator of an ESR spectrometer. The half-life of the detected species was less than 0.01 s. The isotropic spectrum of the radical dianion recorded at room temperature was a triplet of triplets-three equidistant lines by splitting on the nitrogen (spin = 1) of the NO 2 group (a N 1 = 2.12 mT), with each of them split by a small constant (a N 2 = 0.7 mT) on the nitrogen (spin = 1) in position 4 of the heterocycle.

Calculated using the DFT level of theory (PBE0/def2-TZVPP), the hyperfine coupling constants for the dianion radical of 1A-g i = 2.0057, a N 1 (NO 2 group) = 2.28 mT, and a N 2 (N in the 4 position of the heterocycle) = 0.44 mT-were in agreement with the experiment.

The ESR spectra of the adducts of the TEMPO spin trap with the reduction product 1a are additional evidence of the structure of the radicals formed during the ER of 1a ( Figure S7 in the Supplementary Materials). The obtained ESR spectrum can be described as a superposition of the ESR spectra of two adducts; in one adduct, the center of the interaction of the spin trap with the supposed radical is the nitro group, and in the second, the center is the nitrogen atom in position 4 of the six-membered heterocycle.

The results of this study of the electrochemical behavior of compound 1a (5-methyl-6nitro-7-oxo-4,7-dihydro-1,2,4-triazolo[1,5-a]pyrimidinide l-arginine monohydrate) in an acidic aqueous medium showed that the electroreduction of the nitro group of this compound proceeds irreversibly in one six-electron step with the formation of the corresponding heterocyclic amine. The ER of 1a proceeds at more negative potentials in comparison with that of the previously studied 2a in both aqueous and aprotic media. Compound 1a is reduced in two stages in aprotic media. The transfer of the first electron is accompanied by the competition of protonation reactions with the participation of the starting compound 1a. At the potentials of the second stage, the heterocyclic anion 1a is reversibly reduced to form the dianion radical. The ESR spectrum of this particle was recorded upon the ER of compound 1a in the presence of Bu 4 NOH.

The effect of Na + and Li + ions added to the DMF solution was considered. In the presence of these ions, not only does the rate of protonation of the dianion radicals of the investigated compound change, but the regioselectivity of this reaction also changes. The results of ESR spectroscopy make it possible to assume the formation of both a nitroxyl radical and a radical with spin density localization on nitrogen in the 4 position of the six-membered ring during the ER of 1a. The obtained ESR spectrum of adducts of radical particles with a TEMPO spin trap can be described as a superposition of the ESR spectra of these radicals.

Supplementary Materials: The following are available online. Figure S1 : CVs obtained in BR solution and compound 1a before background discharge. Figure S2 : The dependence of the limiting current of the electroreduction of compound 1a (C = 5·10 −3 mM) on ω 0.5 in a BR solution with pH = 2. Figure S3 : NMR spectrum of the product after electrolysis of 1a. Figure S4 : Mass spectra of products after electrolysis of 1a. Electrolysis of compound 1a in an acidic medium. Figure S5 : CVs of 1a in a 60% Britton-Robinson buffer with 40% DMF. Sweep scan 50 mVs −1 : 1-pH = 2; 2-pH = 9; 3-pH = 12. Scheme S1: Possible further ways of reducing 1a. Figure S6 : ESR spectra of the products of the reduction reaction of compound 1a with the TMTH probe and the relative number of paramagnetic centers after 0, 1, 5, 10, and 15 min of electroreduction at −1.7 V. Figure S7 : ESR spectra of TMPO spin trap adducts with a reduction product 1a. 

The data presented in this study are available on request from the corresponding author.

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The authors declare no conflict of interest.Sample Availability: Samples of the compounds 5-Methyl-6-nitro-7-oxo-4,7-dihydro-1,2,4-triazolo [1,5-a]pyrimidinide l-arginine monohydrate (1a, Triazid), sodium salt of 5-methyl-6-nitro-7-oxo-4,7dihydro-1,2,4-triazolo[1,5-a]pyrimidine (1b), sodium salt of 2-methylthio-6-nitro-7-oxo-1,2,4-triazolo- [5,1-c] [1, 2, 4] triazin, dihydrate (2a, Triazavirin ® ), and 2-methylthio-6-nitro-7-oxo-1,2,4-triazolo-[5,1c] [1, 2, 4] triazin (2b) are available from the authors.