Anions Containing Tripoid Conjugated N4- System: Salts of 5-(Substituted Amino)-[1,2,3]triazolo[4,5-c][1,2,5]oxadiazol-5-ium-4-ides, as well as Their Synthesis, Structure, and Thermal Stability.

A strategy for the synthesis of 5-((2-cyanoethyl)-X-amino)-[1,2,3]triazolo[4,5-c][1,2,5]oxadiazol-5-ium-4-ides (X = H; CH2CH2CN; NO2 (4a); CN (4b); CO2Et (4c)) starting from 3-amino-4-azido-1,2,5-oxadiazole was developed. The key step in this strategy is the intramolecular thermolytic cyclization of the azido group and the bis(2-cyanoethyl)triazene group. Removal of the 2-cyanoethyl protecting group from amides 4a-c gave potassium salt of the corresponding nitramide and sodium salts of cyano- and ethoxycarbonylamide. The structure and thermal stability of the synthesized compounds were studied experimentally using multinuclear NMR spectroscopy, X-ray crystallography, thermogravimetry, and differential scanning calorimetry.

1. Introduction

Nitrate anion A has a high thermal stability. Sodium and potassium nitrates begin to decompose at temperatures above 380 °C. Chemists are faced with the task of studying the changes in the thermal stability of compounds when oxygen atoms in the nitrate anion are replaced by nitrogen atoms (Figure 1).

Figure 1

Nitrate anion A, related isoelectronic structures B–E, and E-type anions 1 and 2.

The structure of the nitrate anion has the following features: (1) a flat Y-shaped (tripoid) topology; (2) the positive charge is localized on the central N-atom of the system, and the negative charges are distributed over three terminal O-atoms; and (3) six electrons take part in conjugation (the so-called Y-aromaticity [1]).

With the successive isoelectronic substitution of oxygen atoms in the nitrate anion A for nitrogen atoms, anions B, C, and D are formed, while the conjugated 6-π electron system is retained (Figure 1). In the case when substituents in the nitrogen atoms exhibit the –M effect (NO2, CN, etc.), negative charge delocalization is possible, which can lead to an elongation of the conjugation chain and a probable increase in the stability of the electron shell of the system.

Representative compounds of type B are the well-known anions of primary nitramines. Compounds of type C are represented in the literature as anions of unannulated and annulated 1,2,3-triazole 2-oxides and tetrazole 2-oxides. Type D acyclic anions are not described (for theoretical studies of such systems, see [2]), and type E anions are represented by compounds 1 [3] and 2 [4], in which three of the four atoms of the tripoid conjugated system are built into a five-membered heterocyclic ring (Figure 1).

Note that the thermal stability of compounds B–E may decrease compared with the nitrate anion, as the substituents may give rise to new pathways for the decomposition of the molecule, which were not present in the nitrate anion. An example of B compounds that are less thermally stable than the nitrate anion are dinitramide salts [5,6,7].

Previously, our group systematically studied the compounds of type B (dinitramide salts [8,9]) and C (4H-[1,2,3]triazolo[4,5-c][1,2,5]oxadiazole 5-oxide [10]). Now, we are starting to study the compounds of type E.

This article describes an approach to the synthesis of salts 3a–c and investigates their structure and thermal stability (Figure 2).

Figure 2

Compounds described in this paper.

2. Results and Discussion

2.1. Synthesis

We started our study with compound 3a. Typically, N-nitramides of heterocycles are prepared through nitration of the appropriate N-amino heterocycles (for review, see [11]). However, sometimes, these compounds are not available. We developed an alternative approach to the synthesis of target salts (Scheme 1). The main idea in this route is the synthesis of compound 6 bearing two cyanoethyl groups and the subsequent stepwise removal of these groups.

Scheme 1

Retrosynthetic analysis of salt 3a.

Choosing this synthetic route, we kept in mind a number of known reactions. The first one was thermolytic cyclization of 3-azido-4-azo-1,2,5-oxadiazoles leading to 5-Ar(Alk)-substituted 1,2,3-triazolo[4,5-c][1,2,5]oxadiazoles [12,13,14,1,2,5]oxadiazolo[3,4-. Russ. Chem. Bull.. 2008 ">15]. This reaction proceeded smoothly with a good yield when the starting 1,2,5-oxadiazoles (furazans) were heated in organic solvents (acetonitrile, benzene, etc.) at 80 °C for several hours. Related cyclization of the adjacent azido and triazene groups took place in more drastic conditions at temperatures ≥ 130 °C in order to give N-substituted 2-aminobenzotriazoles [16,17].

The 2-cyanoethyl group is a well-known protecting group. An example of the use of this group is the synthesis of dinitramide from 3-(dinitroamino)propanenitrile [8,18].

The key compound in our synthetic route, triazene 7, was obtained through a reaction of diazonium salt 8 with 3,3′-iminodipropionitrile in CH2Cl2 at –35 °C in a 53% yield (Scheme 2). This salt is a rather labile compound. It was obtained through a modified method that was recently described [19]. Our method involved the reaction of 3-amino-4-azido-1,2,5-oxadiazole 9 with NOBF4 in trifluoroacetic acid at 0–5 °C, followed by solvent removal at this temperature in vacuo and immediate cooling to −35 °C. Unlike previous methods for the in situ preparation of salt 8 (cf. lit. [14,20]), our method made it possible to isolate diazonium salt 8 in the solid state and to carry out the reaction of this salt with amine in organic solvents.

Scheme 2

Synthesis of compounds 5–7.

The key step in the synthesis of salts 3a–c (Scheme 3) includes an intramolecular reaction of the triazene group and the azido group (Scheme 2). In the 1,2,5-oxadiazole (furazan) series, such cyclization was not previously described. To find the conditions for cyclization, triazene 7 was analyzed by TG-DSC (for details see the “Thermal Behavior” section). As a result, the optimum reaction temperature was found. Refluxing triazene 7 in acetonitrile for 24 h afforded (bis(2-cyanoethyl)amino)triazolofurazan 6 in a quantitative yield. The next step involved the removal of the cyanoethyl group by treating triazolofurazan 6 with a solution of KOH in methanol to provide (cyanoethylamino)triazolofurazan 5 in a 93% yield (Scheme 2).

Scheme 3

Synthesis of amines 4a–c and amides 3a–c.

Scheme 3 shows the synthesis of nitramide 3a, cyanamide 3b, and ethoxycarbonylamide 3c. The nitration of amine 5 with NO2BF4 at −30 °C in MeCN gave nitro derivative 4a, which, without isolation, was treated with a solution of KOH (3.2 eq. excess) in MeOH to give K-salt of nitramide 3a. This salt formed a fairly strong complex with MeCN at a ratio of 1:1, which did not disintegrate during column chromatography (ethyl acetate/methanol, 5:1). The complex completely lost MeCN at 80 °C under reduced pressure within 2 h.

The cyanation of amine 5 with BrCN in the presence of Et3N in MeCN gave the N-cyano derivative 4b in an 82% yield. The following treatment of the latter with 1 eq. of sodium bis(trimethylsilyl)amide (NaHMDS, 2M THF solution) in dry THF resulted in the elimination of the cyanoethyl group to give Na-salt of cyanamide 3b. Purification (flash chromatography, ethyl acetate/methanol, 5:1) gave the dihydrate salt in an 85% yield.

Na-salt of ethoxycarbonylamide 3c was synthesized in a similar way. First, amine 5 was introduced into the reaction with ethyl chloroformate in the presence of Et3N in MeCN, yielding N-ethoxycarbonyl derivative 4c (81%). The latter was treated with 1 eq. of NaHMDS (2M THF solution) in dry THF, resulting in the desired Na-salt of cyanamide 3c in a 90% yield. Flash chromatography (ethyl acetate/methanol, 5:1) afforded monohydrate of the salt in a 90% yield.

2.2. Spectroscopy

All of the compounds obtained were fully characterized by IR (KBr) and multinuclear (1H, 13C, and 14N) NMR spectroscopy recorded in [D6]-acetone, [D6]-DMSO, or [D4]-methanol (for details, see Supplementary Materials).

The cyanoethyl substituents in triazene 7 are non-equivalent and appear in 1H NMR spectra as two sets of signals, δ = 3.03, 3.15 (t, J = 6.7 Hz), 4.29, 4.39 (t, J = 6.7 Hz) ppm, which is apparently due to hindered internal rotation about the single N–N bond in the triazene moiety [21]. This phenomenon disappears in the case of bis(2-cyanoethyl)amino)triazolofurazan 6 in the 1H NMR spectra, of which only one pair of triplets referring to both cyanoethyl substituents is observed: δ = 3.21 (t, J = 6.7 Hz), 4.62 (t, J = 6.7 Hz) ppm. The same is true for the 13C NMR spectra of this compounds. Because of the symmetry of the triazolofurazan moiety in compounds 3–6, atoms C-3a and C-6a are equivalent and appear in the 13C NMR spectra as one peak: δ = 163±1 ppm (regardless of the solvent). This is quite close to the 13C NMR spectra of compounds 11 (C-3a,6a: δ = 160.5 ppm) [22] and salts 12 (C-3a,6a: δ ~ 161 ppm) [10] (Figure 3).

Figure 3

Compounds 11–13.

In all 14N NMR [23] spectra of triazolofurazans 3–6, at least two signals related to the heterocyclic framework are observed. One narrow signal of the N-5 atom is in the range from −30 to −80 ppm (Δν½ = 60–200 Hz). The exception is the spectrum of compound 4c in [D6]-acetone, in which, unexpectedly, all signals are significantly widened, including the signal of the N-5 atom (δ = −77 ppm, Δν½ = 770 Hz). Interestingly, in the spectra of the covalent compounds 11 (in CDCl3) and 13 (in [D6]-acetone), similar signals appear in the same range (δ = −50 and −39 ppm, respectively [10,22]).

For compound 6, 1H–15N HSQC was performed in [D6]-acetone to determine definitely the N-5 signal (δ = −52 ppm). It is noteworthy that for compound 5, the N-5 peak is observed in the same place. Replacing hydrogen with a strong electron withdrawing group (CN, COOEt) in compounds 4b,c results in shifting of the N-5 signal to a stronger field (δ = −77 ppm). Similar signals in the case of Na-salts 3b,c, on the contrary, are shifted to a weaker field (δ = −31 ppm). At the same time, the N-5 peak of the K-salt of nitramide 3a is observed in the same range (δ = −47 ppm) as in compounds 5 and 6.

Another type of signal related to the heterocyclic framework is the broadened ones, which could be attributed to N-1 and N-3 of the furazan cycle (δ = 0–40 ppm, Δν½ = 900–2000 Hz). In the 15N NMR spectrum of the nitramide 3a complex with MeCN in [D6]-acetone, a full set of signals is observed: δ = 23 (N-1 and N-3), −8 (NO2), −49 (N-5), −87, −94 (N-4, N-6, N–NO2).

2.3. X-ray Structure Analysis

The structures of the salts 3a (in the form of acetonitrile solvate), 3b (in the form of dihydrate), and 3c (in the form of monohydrate), as well as molecules 4b, 6, and 7 were confirmed using single-crystal X-ray crystallography. As an example, the typical view of the anion 3a is provided in Figure 4.

Figure 4

General view of the anion 3a in crystal. Anisotropic displacement parameters are drawn at a 50% probability level.

In all of the molecules obtained, all atoms of the triazolofurazan framework, together with the exocyclic N7 atom, lie in the same plane. Both in anions 3a–c and in neutral molecules 4b and 6, the corresponding bond lengths of the furazan ring are almost the same (for details see Supplementary Materials).

The compounds studied by X-ray diffraction analysis can be divided into two groups. The first group includes anions 3b and 3c and (bis(2-cyanoethyl)amino)triazolofurazan 6. The second group includes nitro-substituted anion 3a and cyano-substituted compound 4b (Figure 5).

Figure 5

Resonance structures of compounds 3a–c, 4b, and 6.

In all of the compounds of the first group, an effective transfer of a negative charge from the N7 atom to the triazole ring is observed. As a result, the N5–N7 exocyclic bond, and the N4–N5 and N5–N6 endocyclic bonds of the tripoid system are aligned (ca. 1.35 Å) (Table 1). In terms of the resonance theory, this means a large contribution from the resonance structures 3b", 3c", and 6" (Figure 5). Note that the effect of the exocyclic oxygen atom in anion 12 on the bond lengths in the triazole ring is practically the same [10].

Table 1

Selected bond lengths of compounds 3a–c, 4b, and 6.

Compound	3a	3b	3c	4b	6	12 1
bond lengths, Å
N4–N5	1.337(2)	1.3420(18)	1.360(2)	1.328(2)	1.3465(8)	1.3545(16)
N5–N6	1.339(2)	1.3535(17)	1.347(2)	1.324(2)	1.3465(8)	1.3443(16)
N5–N7	1.382(2)	1.3368(18)	1.338(2)	1.379(2)	1.3320(14)	-

1 Lit. [10].

For compounds of the second group, the negative charge transfer from the N7 atom occurs not so much in the triazole ring as in the electron-withdrawing substituent, to the cyano group in compound 4b and to the nitro group in the anion 3a. As a result, the N5–N7 bond becomes longer (ca. 1.38 Å), while the N4–N5 and N5–N6 bonds are somewhat shorten (ca. 1.33 Å). In terms of the resonance theory, this means a small contribution from the resonance structures 3a" and 4b"(Figure 5).

It is important to note that in the case of amides 3b and 3c, the furazanotriazole ring is practically coplanar with the exocyclic substituents N–CN and N–COOEt, i.e., the substituents and the ring form a single conjugated system. In nitramide 3a, the furazanotriazole ring and the N–NO 2 fragment are not coplanar, with a dihedral angle of 58.2° to the ring plane. A similar situation was observed in the case of pyridine-1-nitramide, for which the dihedral angle between the N-NO 2 fragment and the pyridine ring is 71.7° [24]. Thus, in nitramide 3a, the furazanotriazole ring and the nitro group do not form a single conjugated system.

2.4. Thermal Behavior

The thermal stability of the investigated compounds was assessed by tracking the signals of the thermogravimetry (TG) and differential scanning calorimetry (DSC) (for detail see Supplementary Materials). As a first measure of the thermal stability, the extrapolated onset of the decomposition peak can be used. Note that a more precise conclusion can be drawn only after kinetic analysis of the decomposition process [25]. Through the extrapolated onsets of the decomposition peak, the thermal stability of the analyzed compounds increased in a row, as follows: 5 (127 °C) < 3a (152 °C) ≈ 3c (165 °C) < 4b (185 °C) ≈ 3b (190 °C) < 4c (233 °C) ≈ 6 (234 °C).

Nitramide 3a melts at 152 °C with the subsequent decomposition. Cyanamide 3b upon heating shows a series of weak endothermic events with the marked exotherm of the thermal decomposition with an extrapolated onset of 190 °C. Initial endotherms apparently correspond to the elimination of water, this conclusion is supported by nearly 16% of the mass loss prior to 150 °C. Ethoxycarbonylamide 3c shows a more complex picture, including an endothermic event that shifts to exothermic events consisting of two peaks: the first peak is 122 °C, the second one is 170 °C. As for 3b, initial endotherm probably corresponded to the elimination of water. The subsequent exothermic event with an extrapolated onset of 122 °C most likely was not related to the decomposition of the heterocyclic system. This is supported by nearly 10% of mass loss prior to 150 °C. Apparently, the second peak with an extrapolated onset of 170 °C refers to the decomposition of ethoxycarbonylamide 3c.

Covalent (2-cyanoethyl)amines 4b,c are thermostable but low-melting compounds. So, compound 4b melts at 76 °C with a thermal decomposition at further heating (extrapolated onset: 185 °C). Compound 4c reveals first endothermic event at 61 °C, and then decomposes above 200 °C in these experimental conditions. Bis(2-cyanoethyl)amine 6 melts at 139 °C with the decomposition at further heating (extrapolated onset: 234 °C). As expected, amine 5 bearing the NH proton has one of the lowest thermal stabilities, decomposing right after the endothermic event at 127 °C, as evidenced by the heat release and mass loss signals. The endotherm at 127 °C is preceded by two weaker endothermic events without noticeable mass loss. The tentative interpretation of these effects is a phase transition, and for endotherm at 127 °C, the melting of amine 5.

It can be seen that both covalent and ionic compounds have a relatively high thermal stability (>150 °C), except for the triazolofurazan 5 bearing NH proton. This suggests that 5-amino-[1,2,3]triazolo[4,5-c][1,2,5]oxadiazol-5-ium-4-ide is a promising scaffold for the design of various thermally stable systems.

Triazene 7 at heating first reveals the endotherm at 79 °C, followed by an exothermic event with a maximum at 133 °C, and after 200 °C, a sharp peak of the heat release is observed. The tentative assignment of the first effect on DSC trace (endotherm at 79 °C) is melting. The following exotherm shows the associated mass loss of 11 wt.%, which closely matches the elimination of one molecule of nitrogen from triazene 7. The last exotherm with an extrapolated onset of 221 °C is thus the thermal decomposition of the formed amine 6.

3. Conclusions

In conclusion, we developed a strategy for the synthesis of N-substituted 5-aminotriazolofurazans 3–6 starting from 3-amino-4-azido-1,2,5-oxadiazole 9. Previously unknown in the 1,2,5-oxadiazole series in the intramolecular thermolytic cyclization of the azido group and the bis(2-cyanoethyl)triazene group was investigated. This cyclization opens the door to compounds containing tripoid conjugated system consisting of four nitrogen atoms. The key compound in our synthetic route, triazene 7, was prepared through the the reaction of 3,3′-iminodipropionitrile with diazonium salt 8 in dichloromethane. The latter salt was synthesized by a method involving the reaction of 3-amino-4-azido-1,2,5-oxadiazole 9 with NOBF4 in trifluoroacetic acid, followed by solvent removal to give diazonium salt in the solid state. The structures of the salts 3a–c, as well as covalent compounds 4b, 6, and 7, were confirmed using single-crystal X-ray crystallography. According to the TG-DCS analysis, the extrapolated onset temperatures for the decomposition of compounds 3, 4, and 6 were between 152 and 234 °C. This indicates a relatively high stability for both covalent and ionic compounds of this type, and allows us to consider 5-amino-[1,2,3]triazolo[4,5-c][1,2,5]oxadiazol-5-ium-4-ide as a promising scaffold for creating various thermally stable systems.

4. Materials and Methods

CAUTION!!! Although we encountered no difficulties during the preparation and handling of the compounds described in this paper, they are potentially explosive energetic materials that are sensitive to impact and friction. Any manipulations must be carried out using the appropriate standard safety precautions.

General. All reactions were carried out in well-cleaned oven-dried glassware with magnetic stirring. 1H, 13C, 14N, and 15N NMR spectra were recorded with a Bruker DRX-500 (500.1, 125.8, and 36.1 MHz, respectively) and Bruker AV600 (600.1, 150.9, 43.4, and 60.8 MHz, respectively) spectrometers. Chemical shifts are reported in delta (δ) units, parts per million (ppm) downfield from internal TMS (1H, 13C) or external CH3NO2 (14N, 15N negative values of δN correspond to upfield shifts); multiplicities are indicated by s (singlet), d (doublet), t (triplet), q (quartet), m (multiplet), and br (broad). The IR spectra were recorded with a Bruker “ALPHA-T” spectrometer in the range of 400–4000 cm−1 (resolution 2 cm−1) as pellets with KBr or as a thin layer. Elemental analyses were performed with the CHN Analyzer Perkin-Elmer 2400 or EuroVector EA. High-resolution ESI mass spectra (HRMS) were recorded with a Bruker micrOTOF II instrument. All of the measurements were performed in positive (+MS) or negative (–MS) ion mode (interface capillary voltage: 4500 V) with a scan range of m/z 50–3000. External calibration of the mass spectrometer was performed with Electrospray Calibrant Solution (Fluka). A direct syringe injection was used for all of the analyzed solutions in MeCN (flow rate: 3 µL·min−1). Nitrogen was used as a nebulizer gas (0.4 bar) and dry gas (4.0 L·min−1); the interface temperature was set at 180 °C. All of the spectra were processed using the Bruker DataAnalysis 4.0 software package. Thermal analysis was performed with a Netzsch STA 449F1 instrument. Differential scanning calorimetry (DSC) and thermogravimetry (TG) signals were obtained for the sample of ca. 1 mg enclosed in an aluminum crucible with a pierced lid and heated linearly at 5 K·min−1 rate in argon flow. Analytical thin-layer chromatography (TLC) was carried out on Merck 25 TLC silica gel 60 F254 aluminum sheets. The visualization of the TLC plates was accomplished with a UV light. Silica gel 60 Merck (15–40 μm) was used for the preparative column chromatography. All of the reagents were purchased from Acros or Sigma-Aldrich. The solvents were purified before use, according to standard procedures. 3-Amino-4-azido-1,2,5-oxadiazole 9 was prepared according to a previously published procedure [20].

(. NOBF4 (760 mg, 6.5 mmol) was added to a vigorously stirred solution of 3-amino-4-azido-1,2,5-oxadiazole 9 (760 mg, 6 mmol) in TFA (4 mL) at 0–5 °C under an argon atmosphere. The reaction mixture was stirred for 3 h, after that it was concentrated under reduced pressure at 0–5 °C. The obtained slurry was cooled to −35 °C, then a cooled (−35 °C) 3,3′-iminodipropionitrile (3 g, 24.4 mmol) solution in CH2Cl2 (10 mL) was added. The reaction mixture was smoothly warmed to RT under vigorous stirring. The solvent was evaporated in vacuo and the residue was purified by flash chromatography (ethyl acetate/petroleum ether, 1:1) to give a white solid (825 mg, 53%). 1H NMR (500.1 MHz, [D6]-acetone): δ 3.03, 3.15 (t, 4 H, CH2CH2CN, J = 6.7 Hz), 4.29, 4.39 (t, 4 H, CH2CH2CN, J = 6.7 Hz) ppm. 13C NMR (125.8 MHz, [D6]-acetone): δ 13.1, 16.6 (CH2CH2CN), 43.7, 51.2 (CH2CH2CN), 117.0, 117.1 (CN), 148.1, 154.5 (C(3,4)) ppm. 14N NMR (36.1 MHz, [D6]-acetone): δ –130 (N3, ν½ = 670 Hz), –144 (N3, ν½ = 70 Hz). IR (KBr): ν˜ 592, 631, 748, 766, 889, 916, 943, 1014, 1146, 1173, 1190, 1279, 1307, 1340, 1349, 1382, 1404, 1438, 1470, 1495, 1561, 2140, 2166, 2254, 2935, 2963, 3012 cm−1. HRMS (ESI) m/z [M+NH4]+ calcd for C8H8N10O: 278.1221, found: 278.1221.

5-(Bis(2-cyanoethyl)amino)-[1,2,3]triazolo[4,5-. A solution of azidotriazene 7 (870 mg, 3.35 mmol) in MeCN (30 mL) was refluxed for 24 h, and finally allowed to cool to RT. The solvent was evaporated in vacuo and the residue was purified by flash chromatography (ethyl acetate/petroleum ether, 1:1) to give a pale beige solid in a quantitative yield (770 mg). 1H NMR (500.1 MHz, [D6]-acetone): δ 3.22 (t, 4 H, CH2CH2CN, J = 6.7 Hz), 4.62 (t, 4 H, CH2CH2CN, J = 6.7 Hz) ppm. 13C NMR (125.8 MHz, [D6]-acetone): δ 14.8 (CH2CH2CN), 50.4 (CH2CH2CN), 117.2 (CN), 162.2 (C(3a,6a)) ppm. 14N NMR (36.1 MHz, [D6]-acetone): δ –52 (N-5, ν½ = 140 Hz), –130 (N-4, N-6, ν½ = 590 Hz) ppm. IR (KBr): ν˜ 676, 771, 794, 811, 924, 967, 1014, 1041, 1120, 1192, 1330, 1363, 1392, 1421, 1436, 1480, 1540, 2251, 2938, 2971, 3021 cm−1. HRMS (ESI) m/z [M+Na]+ calcd for C8H8N8O: 255.0713, found: 255.0705.

5-((2-Cyanoethyl)amino)-[1,2,3]triazolo[4,5-. A solution of KOH (500 mg, 8.88 mmol) in MeOH (15 mL) was added dropwise to a vigorously stirred solution of triazolofurazan 6 (1030 mg, 4.44 mmol) in MeOH (70 mL). The reaction mixture was stirred for 30 min (TLC control), and then the solvent was evaporated in vacuo and the residue was purified by flash chromatography (ethyl acetate) to give a pale yellow solid (742 mg, 93%). 1H NMR (600.1 MHz, [D6]-acetone): δ 3.14 (t, 2 H, CH2CH2CN, J = 6.3 Hz), 4.26 (t, 2 H, CH2CH2CN, J = 6.3 Hz) ppm. 13C NMR (150.9 MHz, [D6]-acetone): δ 15.7 (CH2CH2CN), 43.6 (CH2CH2CN), 117.2 (CN), 162.4 (C(3a,6a)) ppm. 14N NMR (43.4 MHz, [D6]-acetone): δ –52 (N-5, ν½ = 70 Hz), –132 (N-4, N-6, ν½ = 620 Hz) ppm. IR (KBr): ν˜ 782, 795, 810, 938, 1028, 1051, 1138, 1339, 1360, 1432, 1458, 1548, 2270, 2966, 3015, 3201, 3468 cm–1. HRMS (ESI) m/z [M–H]– calcd for C5H5N7O: 178.0483, found: 178.0481.

5-(. To a stirred solution of triazolofurazan 5 (600 mg, 3.35 mmol) in dry MeCN (5 mL) at RT under an argon atmosphere, a solution of Et3N (327 mg, 0.51 mL, 3.69 mmol) in dry MeCN (2 mL) and BrCN (387 mg, 3.69 mmol) in dry MeCN (2 mL) were sequentially added. The reaction mixture was stirred at RT for 30 min (TLC control), then the solvent was evaporated in vacuo and the residue was purified by flash chromatography (ethyl acetate/petroleum ether, 1:1) to give a pale beige solid (563 mg, 82%). 1H NMR (500.1 MHz, [D6]-acetone): δ 3.40 (t, 2 H, CH2CH2CN, J = 7.0 Hz), 5.00 (t, 2 H, CH2CH2CN, J = 7.0 Hz) ppm. 13C NMR (125.8 MHz, [D6]-acetone): δ 15.5 (CH2CH2CN), 51.1 (CH2CH2CN), 105.1 (CN), 116.0 (CH2CH2CN), 162.2 (C(3a,6a)) ppm. 14N NMR (36.1 MHz, [D6]-acetone): δ –71 (N-5, ν½ = 170 Hz), –105 (N-4, N-6, ν½ = 500 Hz), –129 (ν½ = 480 Hz), –145 (ν½ = 600 Hz) ppm. IR (KBr): ν˜ 463, 633, 654, 810, 835, 907, 945, 1044, 1213, 1334, 1396, 1434, 1445, 1521, 2248, 2943, 2977, 2990, 3036, 3414 cm–1. HRMS (ESI) m/z [M+Na]+ calcd for C6H4N8O: 227.0400, found: 227.0406.

5-((2-Cyanoethyl)(ethoxycarbonyl)amino)-[1,2,3]triazolo[4,5-. To a stirred solution of triazolofurazan 5 (360 mg, 2 mmol) in dry MeCN (5 mL) at RT under an argon atmosphere, a solution of Et3N (327 mg, 0.41 mL, 2.6 mmol) in dry MeCN (2.5 mL) and ClCOOEt (284 mg, 0.25 mL, 2.6 mmol) in dry MeCN (2.5 mL) were sequentially added. The reaction mixture was stirred at RT for 24 h (TLC control), then the solvent was evaporated in vacuo and the residue was purified by flash chromatography (ethyl acetate/petroleum ether, 1:1) to give a pale yellow solid (409 mg, 81%). 1H NMR (500.1 MHz, [D6]-acetone): δ 1.31 (t, 3 H, CH3CH2, J = 7.0 Hz), 3.08 (t, 2 H, CH2CH2CN, J = 6.4 Hz), 4.39 (k, 2 H, CH3CH2, J = 7.0 Hz), 4.58 (t, 2 H, CH2CH2CN, J = 6.4 Hz) ppm. 13C NMR (125.8 MHz, [D6]-acetone): δ 13.0 (CH2CH3), 16.1 (CH2CH2CN), 47.5 (CH2CH2CN), 64.5 (CH2CH3), 116.5 (CN), 151.6 (C=O), 162.8 (C(3a,6a)) ppm. 14N NMR (36.1 MHz, [D6]-acetone): δ –77 (N-5, ν½ = 630 Hz), –130 (500 Hz) ppm. IR (KBr): ν˜ 598, 615, 714, 746, 767, 809, 834, 872, 1014, 1029, 1044, 1092, 1153, 1176, 1225, 1291, 1315, 1376, 1402, 1428, 1445, 1466, 1750, 2251, 2981, 3486 cm−1.

K-Salt of 5-(nitroamino)-[1,2,3]triazolo[4,5-. NO2BF4 (642 mg, 4.8 mmol) was added in one portion to a stirred solution of triazolofurazan 5 (720 mg, 4.0 mmol) in dry MeCN (10 mL) at −30 °C under an argon atmosphere. The reaction mixture was stirred at this temperature for 15 min (TLC control). Then, a cooled (−30 °C) solution of KOH (717 mg, 12.8 mmol) in MeOH (10 mL) was added to the reaction mixture. This was allowed to warm up to RT, then the reaction mixture was concentrated under a reduced pressure. The residue was purified by column chromatography (ethyl acetate/methanol, 5:1) to give a pale yellow solid (737 mg) as a MeCN–nitramide complex (1:1). This complex was dried at 80 °C under reduced pressure for 2 h, yielding K-salt of nitramide (614 mg, 89%) as a yellow solid. 13C NMR (125.8 MHz, [D6]-DMSO): δ 163.0 (C(3a,6a)) ppm. 14N NMR (36.1 MHz, [D6]-DMSO): δ –9 (NO2, ν½ = 40 Hz), –48 (N-5, ν½ = 180 Hz). 13C NMR of MeCN–nitramide complex (1:1) (150.9 MHz, [D6]-acetone): δ 163.2 (C(3a,6a)) ppm. 14N NMR of MeCN–nitramide complex (1:1) (43.4 MHz, [D6]-acetone): δ 23 (N-1 and N-3, ν½ = 555 Hz), –8 (NO2, ν½ = 40 Hz), –50 (N-5, ν½ = 200 Hz), –89 (N-4 and N-6 or N-NO2, ν½ = 440 Hz) ppm. 15N NMR of MeCN–nitramide complex (1:1) (60.8 MHz, [D6]-acetone): δ 23 (N-1 and N-3), –8 (NO2), –49 (N-5), –87, 94 (N-4, N-6, N-NO2) ppm. IR (KBr): ν˜ 656, 751, 829, 1029, 1054, 1178, 1241, 1311, 1446 cm−1. Elemental analysis calculated (%) for C2KN7O2: C 11.48, H 0.00, N 46.88; found C 11.59, H 0.00, N 46.61.

Na-Salt of 5-cyanamido-[1,2,3]triazolo[4,5-. To a stirred solution of triazolofurazan 4b (100 mg, 0.5 mmol) in dry THF (5 mL) at RT under an argon atmosphere, a 2M THF solution of NaHMDS (alternatively, 2 eq. of DBU with subsequent treatment with ion-exchange resins (Amberlite IR 120, Na-form) can be used) (0.25 mL, 0.5 mmol) was added. The reaction mixture was stirred at RT for 5 min (TLC control), then the reaction mixture was purified by flash chromatography (ethyl acetate/methanol, 5:1) to give Na-salt dihydrate as a yellow solid (87 mg, 85%). 13C NMR (150.9 MHz, [D4]-methanol): δ 117.6 (CN), 163.5 (C(3a,6a)) ppm. 14N NMR (43.4 MHz, [D4]-methanol): δ –31 (N-5, ν½ = 60 Hz), –125 (ν½ = 800 Hz), –176 (ν½ = 505 Hz) ppm. IR (KBr): ν˜ 532, 551, 805, 825, 883, 940, 1042, 1158, 1352, 1386, 1440, 1526, 1637, 2171, 2191, 2280, 2928, 3508 cm−1. Elemental analysis calcd (%) for C3H4N7NaO3: C 17.23, H 1.93, N 46.89; found C 17.11, H 2.01, N 46.45.

Na-Salt of [1,2,3]triazolo[4,5-. To a stirred solution of triazolofurazan 4c (190 mg, 0.757 mmol) in dry THF (5 mL) at RT under an argon atmosphere, a 2M THF solution of NaHMDS (0.38 mL, 0.76 mmol) was added. The reaction mixture was stirred at RT for 5 min (TLC control), then the reaction mixture was purified by flash chromatography (ethyl acetate/methanol, 5:1) to give Na-salt monohydrate as a deep yellow solid (162 mg, 90%). 1H NMR (600.1 MHz, [D6]-DMSO): δ 1.19 (t, 3 H, CH3CH2, J = 6.6 Hz), 4.03 (k, 2 H, CH3CH2, J = 6.6 Hz) ppm. 13C NMR (150.9 MHz, [D6]-DMSO): δ 14.6 (CH2CH3), 59.5 (CH2CH3), 158.9 (C=O), 162.6 (C(3a,6a)) ppm. 14N NMR (43.4 MHz, [D6]-DMSO): δ –29 (N-5, ν½ = 60 Hz) ppm. IR (KBr): ν˜ 510, 779, 819, 1094, 1147, 1288, 1360, 1380, 1450, 1639, 3176, 3269, 3437, 3635 cm–1. Elemental analysis calcd (%) for C5H7N6NaO4: C 25.22, H 2.96, N 35.29; found C 25.39, H 3.05, N 34.72.

X-ray crystallographic data and refinement details.

X-ray diffraction data for 3a, 3b, and 3b were collected on a Bruker Smart APEX II diffractometer equipped with a Photon II detector, for 4b on a Bruker Quest diffractometer equipped with a Photon III detector, and for 6 and 7 on a Bruker APEX DUO diffractometer equipped with a CCD area detector. For all of the experiments, MoKα radiation was used (λ = 0.71072 Å, graphite monochromator). A semiempirical absorption correction was applied with the SADABS program [26] using the intensity data of equivalent reflections. Structures were solved with the dual-space method using the SHELXT program [27] and refined by a full-matrix least squares technique on F2 with anisotropic displacement parameters for non-hydrogen atoms with the SHELXL program [28]. Hydrogen atoms of the coordinated water molecules in 3b and 3c were found from difference Fourier synthesis and were refined in isotropic approximation. All of the other hydrogen atoms were placed in calculated positions and refined in the riding model with isotropic displacement parameters Uiso(H) equal to 1.5Ueq(C) for methyl groups and 1.2Ueq(C) for the other groups. Detailed crystallographic information is provided in the Supplementary Materials. Full crystallographic data have been deposited with the Cambridge Crystallographic Data Center, CCDC 2183138–2183143. Copies of the data can be obtained free of charge via https://www.ccdc.cam.ac.uk/structures/ (accesses on 24 August 2022).