5-(Fluorodinitromethyl)-2H-tetrazole and its tetrazolates – Preparation and Characterization of New High Energy Compounds

Abstract

5-(Fluorodinitromethyl)-2H-tetrazole (HFDNTz) has been prepared by the cycloaddition reaction of HN₃ with F(NO₂)₂CCN, which in turn was prepared by aqueous fluorination of sodium dinitrocyanomethanide. HFDNTz was converted into the ammonium, silver and tetraphenylphosphonium 5-(fluorodinitromethyl)tetrazolates. While the reaction of trinitroacetonitrile with HBr, followed by the treatment with NaOH, resulted in the formation of sodium dinitrocyanomethanide, the reaction of trinitroacetonitrile with aqueous ammonia produced ammonium dinitrocyanomethanide. Hydrazinium dinitromethanide was obtained from trinitroacetonitrile and hydrazine hydrate. All compounds were fully characterized by multinuclear NMR spectroscopy, IR spectroscopy and X-ray crystal structure determinations. Initial safety testing (impact and friction sensitivity) and thermal stability measurements (DTA) were also carried out.

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Introduction

Tetrazoles are a fascinating class of compounds. The parent compound 1H-tetrazole has a nitrogen content of 80%, resulting in a relatively high heat of formation of about 330 kJ mol⁻¹.^1–3 At the same time, tetrazoles can exhibit astonishing high thermal stabilities which results in a wide array of application in agriculture, medicine and biology.⁴ For energetic materials applications, tetrazole is usually further functionalized with explosophore groups such as nitro, N-nitro, azo, or azido.^5–15

In recent years, much effort in energetic materials research was dedicated to the synthesis of novel energetic highly over-oxidized compounds that can be used to replace ammonium perchlorate as high-oxygen carrier in solid rocket propellant formulations. An expression that is often being used in order to indicate the degree of oxidation of a compound is the oxygen balance (OB). In its original form, the OB was defined as percentage of oxygen required for complete conversion of a molecule to carbon dioxide, water and metal oxide.¹⁶ Because if the usually high combustion temperatures in rocket engines, it is more useful to calculate the OB of a rocket propellant based on combustion to carbon monoxide instead of carbon monoxide. While energetic, tetrazoles are usually notoriously under-oxidized. 5-Nitrotetrazolate¹² has an OB of 14.0% for combustion to CO but the recently investigated 5-(trinitromethyl)tetrazolate⁵ has an OB of 29.4%. The general disadvantage of most 5-(trinitromethyl)tetrazolates are their high impact (IS) and friction sensitivities (FS) (e.g. IS = 0.5 J and FS < 1 N for the rubidium and cesium salts).⁵

The instability of the trinitromethyl group toward catastrophic decomposition is well established. It has been found that the fluorodinitromethyl group –CF(NO₂)₂ is generally more stable than the trinitromethyl group –C(NO₂)₃ without incurring too much of a performance penalty. The 5-(fluorodinitromethyl)tetrazolate anion has an OB of 20.9% for combustion to N₂, CO and CF₄. Fluorine-containing compounds such as Teflon or Viton are common ingredients of metallized formulations for flares and pyrotechnics (e.g. MTV: Mg/Teflon/Viton). The highly exothermic formation of metal fluorides during combustion increases the flame temperature which in turn improves the performance of the formulation.

The synthesis of 5-(fluorodinitromethyl)-2H-tetrazole (HFDNTz) by reaction of fluorodinitroacetonitrile with sodium azide or trimethylsilyl azide has been reported but the obtained tetrazole was not isolated and directly converted into the sodium or ammonium salt. The tetrazole and the salts were identified only by IR and ¹⁹F NMR spectra and have not been well characterized.^17,18

In this manuscript we report the synthesis and full characterization of 5-(fluorodinitromethyl)-2H-tetrazole and three salts with the energetic 5-(fluorodinitromethyl)tetrazolate anion.

Experimental part

Caution! The compounds of this work are energetic materials that might explode under certain conditions (e.g. elevated temperatures, impact, friction or electric discharge). Appropriate safety precautions,¹⁹ such as the use of shields or barricades in a fume hood and personal protection equipment (safety glasses, face shields, ear plugs, as well as gloves and suits made from leather and/or Kevlar) should be taken all the time when handling these materials. Ignoring safety precautions may lead to serious injuries!

Materials and apparatus

All chemicals and solvents were obtained from Sigma-Aldrich or Alfa-Aesar and were used as supplied. NMR spectra were recorded at 298 K on Bruker AMX500 or Varian VNMRS-600s spectrometers using (CD₃)₂CO or D₂O solutions in standard 5 mm glass tubes. Chemical shifts are given relative to neat tetramethylsilane (¹H, ¹³C) or neat CH₃NO₂ (¹⁴N, ¹⁵N). Raman spectra were recorded at ambient temperatures in Pyrex glass tubes in the range of 4000–80 cm⁻¹ on a Bruker Equinox 55 FT-RA spectrometer using a Nd-YAG laser at 1064 nm or a Cary 83 spectrometer using an Ar laser at 488 nm. Infrared spectra were recorded in the range 4000–400 cm⁻¹ on Midac M Series or Bruker Optics Alpha ATR FT-IR spectrometers. Solid samples were recorded as KBr pellets or with an ATR attachment. The KBr pellets were prepared using an Econo mini-press (Barnes Engineering Co.). Gaseous samples were kept in a 5 cm Pyrex glass cell that was equipped with AgCl windows. Differential thermal analysis (DTA) curves were recorded using a purge of dry nitrogen gas and a heating rate of 5 °C min⁻¹ on an OZM Research DTA552-Ex instrument with the Meavy 2.2.0 software. The sample size was 3–15 mg. The impact and friction sensitivity data were determined on an OZM Research BAM Fall Hammer BFH-10 and an OZM Research BAM Friction apparatus FSKM-10, respectively, through five individual measurements that were averaged. Both instruments were calibrated using RDX. The samples were finely powdered materials that were not sifted.

X-ray crystal structure determination

The single crystal X-ray diffraction data were collected on a Bruker SMART APEX DUO diffractometer, equipped with an APEX II CCD detector, using Mo K_α radiation (TRIUMPH curved-crystal monochromator) from a fine-focus tube. The frames were integrated using the SAINT algorithm²⁰ to give the hkl files corrected for Lp/decay. The absorption correction was performed using the SADABS program.²¹ The structures were solved and refined on F² using the Bruker SHELXTL Software Package.^22–25 Non-hydrogen atoms were refined anisotropically. Unless noted otherwise, the positions of hydrogen atoms attached to heteroatoms have been located from the difference electron density map. ORTEP drawings were prepared using the ORTEP-III for Windows V2.02 program.²⁶

Synthesis of trinitroacetonitrile

Under an atmosphere of nitrogen, a mixture of cyanoacetamide (16.8 g, 0.2 mol) and dichloromethane (50 mL) was cooled to 0 °C. While stirring vigorously, 100% nitric acid (32 mL) was added through an addition funnel within a time period of 2 minutes. The cyanoacetamide dissolved and a yellow two-layer mixture was obtained. While maintaining a temperature of 0 °C, oleum (20% SO₃) (38 mL) was slowly added drop wise and the mixture then stirred vigorously at ambient temperature for an additional 8–10 hours until all gas-evolution stopped. The pale yellow two-phase mixture was transferred into a separatory funnel and the upper organic layer removed. The lower acid layer was extracted three times with dichloromethane (30 mL each). The combined organic layers were extracted twice with cold (−5 °C) concentrated sulphuric acid (15 mL each) and the obtained colourless solution kept over magnesium sulfate.

Neat trinitroacetonitrile was obtained as a colourless solid by removing the solvent from a cold dichloromethane solution (−40 °C) on a vacuum line.

NMR (CDCl₃) δ(ppm): ¹³C (100.54 MHz) 103.4 (s, CN), 112.1 (sept, ¹J(¹³C¹⁴N) = 9.5 Hz, C(NO₂)₃); ¹⁴N (36.14 MHz) −45.4 (s, ν_½ = 20 Hz, NO₂), −272 (s, ν_½ = 350 Hz, CN); Raman (25 °C, 50 mW): 2265 (7.8), 1628 (1.9), 1623 (2.1), 1350 (1.4), 1344 (1.4), 1276 (3.1), 1164 (1.5), 943 (4.6), 856 (6.8), 801 (0.8), 657 (0.9), 477 (2.2), 444 (2.5), 380 (6.6), 360 (10.0), 200 (3.8), 151 (6.5), 110 (7.6) cm⁻¹.

Synthesis of sodium dinitrocyanomethanide²⁷

The obtained solution of (NO₂)₃CCN in CH₂Cl₂ (100 mL) was added drop wise to a stirred solution of methanol (50 mL) and 48% aqueous HBr (100 mL). The mixture was stirred at ambient temperature for about 4 hours during which the solution gradually turned from colourless to reddish brown and evolved brown fumes of bromine. The pH of the mixture was then adjusted to pH 10 with 3 M NaOH in methanol. The now milky, yellow mixture was taken to dryness on a rotary evaporator. The yellow solid residue was extracted five times with ethyl acetate (70 mL each). The combined organic phases were carefully evaporated on a rotary evaporator without heating. Pumping on a vacuum line at ambient temperature for 12 hours resulted in the isolation of a yellow solid residue (yield: 18.2 g, 53.2% based on 0.2 mol cyanoacetamide). Single crystals of Na[(NO₂)₂CCN]·H₂O were obtained by recrystallization from an ethanol–water solution.

DTA: 150 °C (exotherm); NMR (acetone-d₆) δ(ppm): ¹³C (100.54 MHz) 109.1 (s, CN), 157.0 (s, C(NO₂)₂); ¹⁴N (36.14 MHz) −20.6 (s, ν_½ = 40 Hz, NO₂), −88 (s, ν_½ = 320 Hz, CN).

Raman (25 °C, 20 mW): 2244 (7.7), 2226 (4.4), 1493 (1.0), 1442 (1.5), 1433 (2.1), 1377 (8.8), 1295 (1.3), 1260 (5.7), 1250 (5.7), 1230 (10.0), 1159 (2.6), 1153 (1.8), 1070 (0.6), 1026 (0.2), 1004 (0.2), 921 (0.3), 883 (1.4), 865 (7.1), 858 (8.5), 778 (0.5), 769 (0.8), 753 (0.3), 731 (0.3), 577 (0.9), 515 (0.7), 505 (0.8), 469 (1.1), 440 (0.5), 408 (1.1), 273 (2.0), 217 (3.4), 212 (3.3), 151 (4.2), 117 (7.4), 98 (7.3) cm⁻¹; IR (ATR): 3583 (m), 3511 (m), 2230 (ms), 1631 (m), 1611 (m), 1498 (s), 1481 (s), 1424 (m), 1376 (w), 1224 (vs), 1150 (s), 861 (w), 855 (w), 792 (vw), 773 (w), 744 (m), 569 (vw), 497 (vw), 417 (vw) cm⁻¹.

Synthesis of ammonium dinitrocyanomethanide

A concentrated aqueous ammonia solution (5 mL) was added drop wise to a solution of (NO₂)₃CCN (400 mg, 2.28 mmol) in CH₂Cl₂ (5 mL). Immediately, a yellow reaction mixture was obtained that is weakly effervescent. After stirring for 12 hours at ambient temperature, the reaction mixture was taken to dryness on a vacuum line, resulting in a yellow solid (yield: 314 mg, 93%.) Single crystals were obtained from an aqueous solution by slow evaporation of the solvent.

DTA: 240 °C (exotherm); NMR (D₂O) δ(ppm): ¹H (599.80 MHz) 7.2 (s br, NH₄), δ(ppm): ¹³C (100.54 MHz) 111.8 (s, CN), 152.4 (s, C(NO₂)₂); ¹⁴N (36.14 MHz) −23.1 (s, ν_½ = 50 Hz, NO₂), −89 (s, ν_½ = 300 Hz, CN), −363.4 (quint, ¹J(¹H¹⁴N) = 56.9 Hz, NH₄); IR (ATR): 3500–2800 (br, s), 2224 (ms), 1791 (w), 1661 (m), 1610 (w sh), 1523 (w sh), 1477 (m sh), 1396 (s), 1341 (m sh), 1207 (vs), 1144 (s sh), 1110 (s), 852 (w), 827 (w), 788 (w), 772 (m), 744 (s), 566 (m), 501 (m), 433 (w) cm⁻¹.

Synthesis of tetraphenylphosphonium dinitrocyanomethanide

A solution of PPh₄Cl (0.400 g; 1.07 mmol) in water (5 mL) was added to a solution of Na[(NO₂)₂CCN] (0.153 g; 1.00 mmol) in water (5 mL). The precipitate was filtered off, washed with water (10 mL) and dried on a vacuum line resulting in a pale yellow solid (yield: 0.452 g; 96%). DTA: 180 °C (endotherm, melting), 240 °C (exotherm); IR (ATR): 3086 (vw), 3071 (vw), 2956 (vw), 2923 (vw), 2892 (vw), 1593 (s), 1480 (w), 1435 (s), 1395 (vw), 1358 (vw), 1314 (m), 1215 (m), 1185 (vw), 1161 (m), 1106 (s), 1073 (m), 1025 (m), 1025 (vw), 996 (m), 970 (m), 937 (vw), 835 (m), 795 (m), 754 (m), 721 (s), 688 (s), 615 (w), 523 (vs), 447 (w) cm⁻¹.

Synthesis of hydrazinium dinitromethanide

A solution of hydrazinium hydrate (1 mL) in water (1 mL) was added drop wise to a solution of trinitroacetonitrile (200 mg, 1.14 mmol) in water (5 mL). The reaction was exothermic and a colourless gas was evolved. The orange reaction mixture was allowed to evaporate under air, resulting in pale yellow [N₂H₅][(NO₂)₂CH].

DTA: 134 °C (exotherm); NMR (DMSO-d₆) δ(ppm): ¹H (599.80 MHz) 5.6 (s br, N₂H₅), 8.3 (s, (NO₂)₂CH); ¹³C (150.84 MHz) 165.6 (s, CH(NO₂)₂); ¹⁴N (36.14 MHz) −24.1 (s, ν_½ = 100 Hz, NO₂), −336 (s, ν_½ = 600 Hz, N₂H₅); IR (DTA): 3600–2800 (br, m), 1604 (w), 1585 (w), 1499 (vw), 1483 (w), 1459 (vw), 1436 (m), 1341 (w), 1298 (w), 1251 (vw sh), 1240 (vw sh), 1192 (m), 1105 (s), 1071 (m), 997 (m), 948 (w), 758 (m), 719 (s), 687 (s), 615 (vw), 568 (vw), 522 (vs), 503 (m sh), 470 (m sh), 436 (w sh), 411 (vw) cm⁻¹.

Synthesis of fluorodinitroacetonitrile²⁸

A solution of Na[(NO₂)₂CCN] (10.0 g, 65.5 mmol) in water (30 mL) was placed in a 1′′ o.d. FEP reactor equipped with a magnetic stirrer, a gas inlet and a gas outlet tube. After cooling the solution with an ice/water bath to 0 °C, a stream of 10% fluorine in nitrogen was introduced at a rate of approx. 10 l h⁻¹. The off-gas was swept through four traps at −78 °C and then vented through a bubbler that contained perfluorinated Krytox GPL107 oil. After about 3 hours, the fluorine stream was stopped and replaced by a pure nitrogen stream. This stream was maintained for an additional two hours in order to sweep all fluorinated products into the traps. The content of all four traps was combined and fluorodinitroacetonitrile was obtained as a colourless liquid. The crude product was purified by fractional condensation using cold traps at −31 °C, −78 °C and −196 °C. The −31 °C fraction consisted of water and (NO₂)₃CF, and the −196 °C trap contained CO₂, SiF₄, and some NO₂. The fluorodinitroacetonitrile (5.35 g, 55.2%) stopped in the −78 °C trap.

NMR (CDCl₃) δ(ppm): ¹³C (100.54 MHz) 104.8 (d, ²J(¹³C¹⁹F = 35.3 Hz, CN), 105.5 (d, quint, ¹J(¹³C¹⁹F) = 298.1 Hz, ¹J(¹³C¹⁴N) = 3.0 Hz, CF(NO₂)₂); ¹⁴N (36.14 MHz) −36.7 (d, ²J(¹⁴N¹⁹F) = 11.2 Hz, ν_½ = 5 Hz, NO₂), −95 (s, ν_½ = 320 Hz, CN); ¹⁹F (470.55 MHz) −90.8 (quint, ²J(¹⁴N¹⁹F) = 11.3 Hz, CF(NO₂)₂); IR (gas-phase, 10 Torr): 2914 (vw), 2261 (m), 1632 (vs), 1297 (s), 1093 (m), 1022 (vw), 842 (w), 801 (s), 794 (s sh), 655 (w) cm⁻¹.

Synthesis of HFDNTz

In a 250 mL round bottom flask, a mixture of NaN₃ (3.00 g, 46.0 mmol) and CCl₄ (50 mL) was cooled to 0 °C using an ice bath and acetic acid (15 mL) was added slowly. After 5 minutes, a solution of fluorodinitroacetonitrile (1.20 g, 8.76 mmol) in CCl₄ was added slowly through an addition funnel. When the addition was complete, the mixture was stirred for 10 hours at ambient temperature. The solvent was removed using a rotary evaporator. The gel-like, colourless residue was dissolved in CH₂Cl₂ (20 mL) and 2 M H₂SO₄ (10 mL). The organic phase was removed and the aqueous phase extracted three times with CH₂Cl₂ (15 mL each). The combined organic phases were dried over magnesium sulphate. The solvent was carefully evaporated on a rotary evaporator. The remaining colourless, oily liquid was dried by pumping for several hours on a vacuum line at ambient temperature, resulting in a colourless solid (yield: 1.42 g, 84.3%).

DTA: 110 °C (explosion); NMR (CDCl₃) δ(ppm): ¹H (599.80 MHz) 14.0 (s, CN₄H); ¹³C (150.84 MHz) 115.2 (d, ¹J(¹³C¹⁹F), = 290.1 Hz CF(NO₂)₂), 153.9 (d, ²J(¹³C¹⁹F = 25.9 Hz, CN₄); ¹⁴N (36.14 MHz) −27.3 (s, ν_½ = 70 Hz, NO₂), −50 (s, ν_½ = 350 Hz, CN₄); ¹⁹F (564.33 MHz) −98.1 (s, CF(NO₂)₂); Raman (25 °C, 20 mW): 3100–2900 (3.9), 1701 (2.1), 1693 (2.0), 1611 (2.4), 1482 (5.7), 1424 (2.4), 1359 (4.2), 1313 (2.2), 1239 (1.6), 1210 (2.7), 1188 (2.0), 1104 (2.9), 1081 (2.0), 1057 (1.6), 1034 (1.5), 982 (6.4), 956 (3.4), 837 (10.0), 801 (4.2), 544 (2.4), 539 (2.3), 425 (3.1), 397 (3.7), 371 (8.6), 300 (2.6), 282 (2.8), 196 (3.3) cm⁻¹; IR (KBr): 3072 (w), 3069 (vw), 3012 (w), 2911 (w), 2774 (w), 2682 (vw), 2593 (vw), 1694 (s), 1611 (vs), 1478 (w), 1422 (w), 1362 (m), 1307 (m), 1240 (s), 1211 (m), 1173 (m), 1093 (vw), 1078 (w), 1054 (m), 1031 (s), 980 (m), 883 (m), 849 (m), 836 (s), 800 (s), 745 (w), 695 (vw), 663 (vw), 594 (m), 582 (m), 549 (w), 459 (vw), 403 (vw) cm⁻¹.

Synthesis of [NH₄][FDNTz]

A solution of 20% NH₃ in water (5 mL) was added to a solution of HFDNTz (400 mg, 2.08 mmol). The resulting light yellow solution was allowed to evaporate, resulting in crystalline [NH₄][FDNTz] (yield: 992 mg, 93.4%).

DTA: 140 °C (explosion); NMR (D₂O) δ(ppm): ¹H (599.80 MHz) 7.04 (s, NH₄); ¹³C (150.84 MHz) 117.9 (d, ¹J(¹³C¹⁹F) = 290.1 Hz CF(NO₂)₂), 150.8 (d, ²J(¹³C¹⁹F) = 23.2 Hz, CN₄); ¹⁴N (36.14 MHz) −38.2 (s, ν_½ = 60 Hz, NO₂), −52 (s, ν_½ = 350 Hz, CN₄), −362.3 (quint, ¹J(¹H¹⁴N) = 58.7 Hz, NH₄); ¹⁹F (564.33 MHz) −98.5 (s, CF(NO₂)₂); Raman (25 °C, 40 mW): 3200–2800 (3.4), 1685 (1.3), 1609 (2.8), 1472 (8.9), 1364 (4.1), 1326 (1.8), 1320 (1.9), 1319 (1.9), 1313 (1.9), 1309 (1.8), 1191 (5.4), 1161 (1.7), 1153 (1.7), 1102 (4.4), 1071 (2.9), 1067 (3.0), 985 (6.9), 949 (7.8), 839 (9.1), 805 (1.7), 707 (1.3), 652 (2.2), 542 (1.9), 537 (2.1), 533 (2.2), 443 (3.6), 437 (3.3), 401 (3.7), 398 (3.7), 373 (10.0), 303 (3.2), 292 (2.9), 204 (5.8), 170 (6.3), 166 (6.3) cm⁻¹; IR (ATR): 3600–3050 (s), 2977 (m), 2931 (w), 2901 (w), 1655 (w sh), 1606 (m), 1455 (w sh), 1401 (vs), 1320 (w), 1275 (vw), 1184 (vw), 1089 (s), 1049 (vs), 980 (w), 880 (m), 836 (w), 801 (w), 643 (vw), 615 (vw), 452 (w) cm⁻¹.

Synthesis of Ag[FDNTz]

A solution of AgNO₃ (937 mg, 2.50 mmol) in water (5 mL) was added to a solution of HFDNTz (384 mg, 2.00 mmol). The resulting white precipitate was filtered off and washed with water. The white solid was dried in a vacuum in darkness (yield: 687 mg, 92.0%).

DTA: 185 °C (exotherm); IR (ATR): 1644 (s), 1604 (vs), 1467 (vw), 1375 (vw), 1305 (w), 1255 (w), 1201 (w), 1114 (vw), 1042 (vw), 1004 (vw), 973 (w), 833 (w), 796 (w) cm⁻¹.

Synthesis of Ag[FDNTz]·½NH₃

Single crystals of Ag[FDNTz]·½NH₃ were obtained by dissolving Ag[FDNTz] (0.243 g; 0.81 mmol) in 25% aqueous ammonia (5 mL) and letting the solution evaporate under air in darkness.

DTA: 165 °C (endotherm, loss of NH₃), 180 °C (exotherm); IR (ATR): 3363 (m), 3201 (m), 2339 (vw), 2261 (w), 2166 (m), 1665 (s), 1594 (vs), 1498 (vw), 1465 (w), 1356 (s), 1308 (m), 1243 (m), 1195 (w), 1112 (m), 1048 (vw), 979 (m), 834 (ms), 799 (ms), 617 (m), 538 (w) cm⁻¹.

Synthesis of [PPh₄][FDNTz]

A solution of PPh₄Cl (425 mg, 2.50 mmol) in water (5 mL) was added to a solution of HFDNTz (384 mg, 2.00 mmol). The resulting white precipitate was filtered off and washed with water. The white solid was dried in a vacuum (yield: 430 mg, 98.9%).

DTA: 175 °C (exotherm); NMR (CDCl₃) δ(ppm): ¹H (599.80 MHz) 7.5–7.9 (m, PPh₄); ¹³C (150.84 MHz) 117.9 (d, ¹J(¹³C¹⁹F), = 290.1 Hz CF(NO₂)₂), 117.5 (d, ¹J(¹³C³¹P = 88.0 Hz, PPh₄), 120.6 (d, ¹J(¹³C¹⁹F = 282.0 Hz, CF(NO₂)₂), 130.8 (d, ²J(¹³C³¹P = 15.6 Hz, PPh₄), 134.4 (d, ²J(¹³C³¹P = 10.5 Hz, PPh₄), 135.9 (d, ³J(¹³C³¹P = 3.2 Hz, PPh₄), 150.8 (d, ¹J(¹³C¹⁹F = 88.0 Hz, CN₄); 150.8 (d, ²J(¹³C¹⁹F = 23.2 Hz, CN₄); ¹⁴N (36.14 MHz) −39.1 (s, ν_½ = 50 Hz, NO₂), −52 (s, ν_½ = 380 Hz, CN₄); ¹⁹F (564.33 MHz) −94.0 (s, CF(NO₂)₂); ³¹P (242.82 MHz) 23.14 (s, PPh₄); IR (ATR): 3088 (vw), 3071 (vw), 2956 (vw), 2892 (vw), 1593 (s), 1480 (m), 1435 (s), 1395 (vw), 1358 (w), 1339 (vw), 1314 (m), 1215 (m), 1185 (w), 1161 (m), 1106 (s), 1073 (m), 1025 (w), 996 (m), 970 (m), 937 (vw), 835 (m), 795 (m), 754 (m), 721 (s), 688 (s), 645 (vw sh), 615 (w), 523 (vs), 447 (w), 436 (vw sh), 404 (vw) cm⁻¹.

Results and discussion

Synthesis

The synthetic route for the preparation of 5-(fluorodinitromethyl)-2H-tetrazole (HFDNTz) is shown in Scheme 1.

Scheme 1 Synthesis of 5-(fluorodinitromethyl)-2H-tetrazole.

Nitration of cyanoacetamide with fuming nitric acid in 20% oleum under anhydrous conditions resulted in the formation of trinitroacetonitrile.^5,29 Due to the compound's reported sensitivity and high reactivity, trinitroacetonitrile was recommended to be handled only in solution.²⁷ As a result, trinitroacetonitrile had not been fully characterized. We were able to isolate the compound by careful evaporation of the solvent from dichloromethane solutions in a vacuum at −40° C as a moisture sensitive, wax-like colourless solid. It is a very noxious lachrymator that slowly vaporizes in the air at ambient temperature.

Treatment of a trinitroacetonitrile solution in methanol with a 48% aqueous HBr solution resulted in gas evolution and the slow formation of elemental bromine. When the resulting reaction mixture was neutralized with sodium hydroxide, sodium dinitrocyanomethanide could be isolated in up to 53% yield. While this reaction had already been described in the literature, its mechanism is unknown but was assumed to involve the formation of N₂O.²⁷ Single crystals of Na[(NO₂)₂CCN]·H₂O were obtained from an aqueous solution by slow evaporation of the solvent.

When trinitroacetonitrile was reacted with N₂H₄·H₂O in water, a vigorous gas evolution was observed. However, no evidence for the formation of the dinitrocyanomethanide anion could be obtained. Instead, yellow crystals of [N₂H₅][(NO₂)₂CH] were formed when the resulting bright yellow solution was taken to dryness (Scheme 2). The mechanism for the formation of the dinitromethanide anion is unknown. However, it should be noted that a mixture of pure trinitroacetonitrile and neat N₂H₄ is hypergolic. The reaction of the two compounds is highly exothermic. On several occasions, flames and/or explosions were observed when neat hydrazine was mixed with solid trinitroacetonitrile.

Scheme 2 Reaction of trinitroacetonitrile with hydrazine hydrate.

When a clear colourless solution of trinitroacetonitrile in dichloromethane was treated with an aqueous ammonia solution at ambient temperature, a yellow effervescing mixture was obtained. Yellow crystals of [NH₄][(NO₂)₂CCN] were isolated in quantitative yield when the solvent was removed from the reaction mixture after 12 hours of stirring at ambient temperature. The evolved gas was identified by IR spectroscopy as N₂O (Scheme 3).

Scheme 3 Reaction of trinitroacetonitrile with aqueous ammonia.

Fluorodinitroacetonitrile, F(NO₂)₂CCN, was obtained by aqueous fluorination of sodium dinitrocyanomethanide with 10% F₂ in N₂ (Scheme 1). The off-gas of the fluorination reaction was passed trough a series of cold traps at −78 °C. Lower cold trap temperatures were not used to avoid trapping of fluorine nitrate, a possible fluorination side product. While Wiesboeck and Ruff reported only moderate yields of 29% of F(NO₂)₂CCN and the formation of the hydrolysis products acetonitrile and fluorodinitroacetamide when aqueous solutions with more than 3% Na[(NO₂)₂CCN] were fluorinated,²⁸ we did not observe the formation of appreciable amounts on hydrolysis products even in the case of reaction mixtures containing more than 10% of Na[(NO₂)₂CCN]. However, we did observe a contamination of the crude F(NO₂)₂CCN with up to 10% fluorotrinitromethane, FC(NO₂)₃, and also trace amounts of CO₂. Although not necessary for this work, crude F(NO₂)₂CCN could be purified by fractional condensation at −31 °C, −78 °C and −196 °C. The F(NO₂)₂CCN stopped in the −78 °C trap and was isolated as a colourless liquid with a vapour pressure of 56 Torr at 23 °C.

The 1,3-dipolar cycloaddition reaction of F(NO₂)₂CCN with HN₃, followed by extraction with dichloromethane resulted in the isolation of HFDNTz as a colourless, hygroscopic solid in approximately 85% yield. Single crystals suitable for an X-ray crystal structure determination were obtained from a dichloromethane solution by slow evaporation of the solvent in vacuo.

HFDNTz is acidic and forms ammonium 5-(fluorodinitromethyl)tetrazolate in quantitative yield when treated with aqueous ammonia (Scheme 4).

Scheme 4 Synthesis of 5-(fluorodinitromethyl)tetrazolate (FDNTz) salts.

Silver 5-(fluorodinitromethyl)tetrazolate was obtained as a white amorphous precipitate in quantitative yield when an aqueous solution of silver nitrate was added to a solution of HFDNTz in water. Colourless crystals of the ammonia adduct [Ag][FDNTz]·½NH₃ were obtained by recrystallization of the amorphous precipitate from an aqueous ammonia solution. While the nitrotetrazoles of this work are energetic and must be treated with great care, both silver salts are especially treacherous and can explode upon provocation (heat or mechanical shock). The tetraphenylphosphonium (PPh₄) salt of FDNTz was precipitated from an aqueous solution of HFDNTz by the addition of an aqueous PPh₄Cl solution. Crystalline [PPh₄][FDNTz] was obtained by recrystallization from acetone.

X-ray crystal structures

Single crystals suitable for X-ray crystal structure determinations were obtained for Na[(NO₂)₂CCN]·H₂O, NH₄[(NO₂)₂CCN], [PPh₄][(NO₂)₂CCN], [N₂H₅][(NO₂)₂CH], HFDNTz, [NH₄][FDNTz], [Ag][FDNTz]·½NH₃, and [PPh₄][FDNTz]. The relevant data and parameters for the X-ray measurements and refinements of the crystal structures are summarized in Tables 1 and 2. Further crystallographic data and representations of the unit cells for all crystal structures are given in the ESI.†

Table 1 Crystallographic data of the dinitromethanide salts

	Na[(NO2)2CCN]·H2O	[NH4][(NO2)2CCN]	[PPh4][(NO2)2CCN]	[N2H5][(NO2)2CH]
Formula	C2H2N3NaO5	C2H4N4O4	C26H20N3O4P	CH6N4O4
mol wt [g mol^−1]	171.06	148.09	469.42	138.10
Temp [K]	100(2)	100(2)	104(2)	100(2)
Crystal system	Orthorhombic	Monoclinic	Monoclinic	monoclinic
Space group	P212121	P21/n	P21/n	P21/n
a [Å]	7.5138(6)	8.1144(12)	11.6601(8)	3.6434(4)
b [Å]	8.1663(6)	4.8009(8)	14.2600(9)	13.7827(13)
c [Å]	19.9151(14)	14.218(2)	13.4402(9)	10.6457(10)
α [°]	90	90	90	90
β [°]	90	96.914(3)	90.099 (1)	98.230(2)
γ [°]	90	90	90	90
V [Å^3]	1221.99(16)	549.85(15)	2234.7(3)	529.08(9)
Z	8	4	4	4
λ [Å]	0.71073	0.71073	0.71073	0.71073
ρ calc [g cm^−3]	1.860	1.789	1.395	1.734
μ [mm^−1]	0.237	0.170	0.163	0.169
F(000)	688	304	976	288
Reflns collected	30 172	12 950	55 116	12 436
Ind reflns	3734	1681	6814	1614
R int	0.0355	0.0265	0.0385	0.2311
No. of parameters	201	103	307	100
R 1 [I > 2σ(I)]	0.0253	0.0292	0.0359	0.0255
wR2 [I > 2σ(I)]	0.0651	0.795	0.0922	0.0769
GOF	1.060	1.053	1.035	1.087

---

Table 2 Crystallographic data of the 5-(fluorodinitromethyl)tetrazoles

	HFDNTz	[NH4][FDNTz]	Ag[FDNTz]·½NH3	[PPh4][FDNTz]
Formula	C2HFN6O4	C2H4FN7O4	C24H18Ag12F12N78O48	C26H20FN6O4P
Mol wt [g mol^−1]	192.09	209.12	3689.60	530.45
Temp. [K]	100(2)	101(2)	100(2)	101(2)
Crystal system	Monoclinic	Monoclinic	Triclinic	Monoclinic
Space group	C2/c	P21/c	P1̄	P21
a [Å]	28.8030(7)	13.9642(7)	15.4270(10)	11.8077(14)
b [Å]	5.3703(1)	8.9672(5)	15.4526(10)	7.1276(8)
c [Å]	28.897(1)	13.9957(7)	20.5225(13)	14.7721(18)
α [°]	90	90	82.7270(10)	90
β [°]	119.723(2)	115.4716(1)	88.1560(10)	95.585(2)
γ [°]	90	90	82.6690(10)	90
V [Å^3]	3881.71(19)	1582.19(14)	4812.6(5)	1237.3(3)
Z	24	8	2	2
λ [Å]	0.71073	0.71073	0.71073	0.71073
ρ calc [g cm^−3]	1.972	1.756	2.546	1.424
μ [mm^−1]	0.200	0.174	2.540	0.165
F(000)	2304	848	3528	548
Reflns collected	46 406	37 464	22 050	26 729
Ind reflns	5932	4778	22 050	7495
R int	0.0774	0.0384	0.0939	0.0451
No. of parameters	361	277	1576	343
R 1 [I > 2σ(I)]	0.0414	0.0329	0.0584	0.0435
wR2 [I > 2σ(I)]	0.0830	0.0786	0.0977	0.0916
GOF	1.035	1.026	0.992	1.023

---

From an aqueous solution, sodium dinitrocyanomethanide crystallizes as a monohydrate in the orthorhombic space group P2₁2₁2₁ with the unit cell parameters a = 7.5138(6) Å, b = 8.1663(6) Å and c = 19.9151(14) Å. The solid-state structure of Na[(NO₂)₂CCN]·H₂O does not consist of isolated ions but is dominated by cation–anion interactions that result in a polymeric structure. The asymmetric unit of the structure contains two formula units (Z′ = 2). One CN nitrogen atom as well as several oxygen atoms of the anion coordinate each sodium ion, which in turn is bridged to another sodium ion through a water molecule (Fig. 1).

Fig. 1 The solid-state structure of Na[(NO₂)₂CCN]·H₂O. Thermal ellipsoids are shown at the 50% probability level. Hydrogen atom positions were determined from the electron density map and are depicted as spheres of arbitrary radius. Selected bond distances (Å): C1–C2 1.412(2), C1–N1 1.390(2), C1–N2 1.385(2), C2–N3 1.147(2), N1–O1 1.250(2), N1–O2 1.245(2), N2–O3 1.249(2), N2–O4 1.246(2), Na1–O1′ 2.418(1), Na1–O3 2.450(1), Na1–O6 2.475(1), Na1–N6 2.421(1), Na1–O1s 2.362(1), Na1–O2s 2.292(1), Na2–O2 2.575(1), Na2–O4 2.445(1), Na2–O2′ (1), Na2′–O4 2.508(1), Na2′–O4′ 2.445(1).

The ammonium salt of the dinitrocyanomethanide anion crystallizes with four formula units per unit cell (Z = 4) in the monoclinic space group P2₁/n. Not surprisingly, the solid-state structure of [NH₄][(NO₂)₂CCN] contains hydrogen bonds between the ammonium ions and the oxygen atoms as well as the CN nitrogen atom of the anions (Fig. 2). The observed C–N and C≡N bond distances of 1.385(2)/1.390(2) Å and 1.152(2) Å, respectively, in the anion in [NH₄][(NO₂)₂CCN] are virtually identical to the ones observed for Na[(NO₂)₂CCN]·H₂O (1.385(2)/1.390(2) Å and 1.147(2) Å).

Fig. 2 Hydrogen bonding in the solid-state structure of [NH₄][(NO₂)₂CCN]. Thermal ellipsoids are shown at the 50% probability level. Hydrogen atom positions were determined from the electron density map and are depicted as spheres of arbitrary radius. Selected distances (Å): C1–C2 1.412(2), C1–N1 1.385(2), C1–N2 1.402(2), C2–N3 1.152(2), N1–O1 1.240 (1), N1–O2 1.266(1), N2–O3 1.233(1), N2–O4 1.253(1), N3–N4 3.068(1) O1–N4 3.032(1), O2–N4 2.999(1)/3.130(1), O3–N4 2.841(1), O4–N4 2.920(1).

Single crystals of [PPh₄][(NO₂)₂CCN] suitable for structure determination were obtained from an acetone solution by slow evaporation of the solvent. The compound crystallizes in the monoclinic space group P2₁/n with four formula units in the unit cell (Z = 4). The solid state structure consists of isolated PPh₄⁺ cations and [(NO₂)₂CCN]⁻ anions (Fig. 3). The closest cation–anion interactions are 3.122(2) Å (O2⋯C19) and 3.187(2) Å (O1⋯C10). The observed C–N and C≡N bond distances of 1.3966(15)/1.4150(7) Å and 1.1513(17) Å, respectively, in the [(NO₂)₂CCN] anion are in good agreement with the ones observed for the Na⁺ and NH₄⁺ salts.

Fig. 3 The solid-state structure of Na[(NO₂)₂CCN]. Thermal ellipsoids are shown at the 50% probability level. Hydrogen atoms were omitted for clarity. Selected bond distances (Å): C1–C2 1.4150(17), C1–N1 1.3966(15), C1–N2 1.3994(16), C2–N3 1.1513(17), N1–O1 1.2571(14), N1–O2 1.2360(14), N2–O3 1.2518(15), N2–O4 1.2305(14).

Single crystals of [N₂H₅][(NO₂)₂CH] were obtained from an aqueous solution by slow evaporation. The compound crystallizes without crystal water in the monoclinic space group P2₁/n (Z = 4) with the unit cell parameters a = 3.6434(4) Å, b = 13.7827(13) Å, and c = 10.6457(10) Å. The solid-state structure consists of N₂H₅⁺ cations and [(NO₂)₂CH]⁻ anions (Fig. 4) that are linked through hydrogen bonds between the cation and the oxygen atoms of the anion. The observed C–N bond distances in the [(NO₂)₂CH]⁻ anion of 1.368(1) Å and 1.365(1) Å are noticeable shorter than the ones observed for the [(NO₂)₂CCN]⁻ anion in the PPh₄⁺ salt (1.3966(15) and 1.4150(7) Å).

Fig. 4 The crystal structure of [N₂H₅][(NO₂)₂CH]. Thermal ellipsoids are shown at the 50% probability level. Hydrogen atom positions were determined from the electron density map and are depicted as spheres of arbitrary radius. Selected bond distances (Å): C1–N1 1.368(1), C1–N2 1.3647(9), N1–O1 1.2648(8), N1–O2 1.2647(8), N2–O3 1.2621(8), N2–O4 1.2648(8).

Single crystals of 5-(fluorodinitromethyl)-2H-tetrazole (HFDNTz) were obtained by slow evaporation of a dichloromethane solution in vacuo at a temperature of −20 °C. The compound crystallizes in the monoclinic space group C2/c with a unit cell volume of 3881.71(19) ų (Z = 24). Further crystallographic details for the compound are listed in Table 2. The structure of HDNTz is depicted in Fig. 5, while the bond lengths and angles of the tetrazole ring in this compound are summarized in Table 3 together with the ones for the related tetrazolates of this work.

Fig. 5 The molecular structure of 5-(fluorodinitromethyl)-2H-tetrazole. Thermal ellipsoids are shown at the 50% probability level. The position of the hydrogen atom was determined from the electron density map. It is depicted as a sphere of arbitrary radius. Selected bond distances (Å) and bond angles (°): C1–C2 1.490(2), C1–N1 1.325(2), C1–N4 1.350(2), C2–N5 1.540(2), C2–N6 1.539(2), C2–F1 1.318(2), N1–N2 1.324(2), C1–C2–F1 113.0(1), C1–C2–N5 109.7(1), C1–C2–N6 113.0(1), N1–C1–C2 122.5(2).

Table 3 Selected bond lengths (Å) and angles (°) for the 5-(fluorodinitromethyl)tetrazoles

	HFDNTz^a	[NH4][FDNTz]^a	Ag[FDNTz]·½NH3 ^a	[PPh4][FDNTz]
a Values given for only one of the different molecules in the asymmetric unit.
C1–C2	1.490(2)	1.4850(14)	1.463(10)	1.476(4)
C1–N1	1.325(2)	1.3298(13)	1.324(9)	1.335(4)
C1–N4	1.350(2)	1.3357(13)	1.325(8)	1.319(4)
N1–N2	1.324(2)	1.3438(12)	1.343(8)	1.347(3)
N2–N3	1.319(2)	1.3224(13)	1.327(8)	1.311(4)
N3–N4	1.325(2)	1.3383(12)	1.348(7)	1.347(3)
C2–F	1.318(2)	1.3328(11)	1.313(8)	1.339(4)
C2–N5	1.540(2)	1.5466(14)	1.540(9)	1.543(4)
C2–N6	1.539(2)	1.5381(14)	1.545(9)	1.534(4)
C1–N1–N2	100.36(14)	103.48(8)	104.0(6)	102.9(2)
C1–N4–N3	105.48(14)	103.42(8)	104.4(5)	103.5(2)
N1–N2–N3	115.32(14)	109.64(8)	109.8(6)	110.0(2)
N2–N3–N4	105.32(13)	109.91(8)	108.6(6)	109.7(2)
N1–C1–N4	113.51(15)	113.55(9)	113.2(6)	113.9(2)
N1–C1–C2	122.49(15)	124.33(9)	125.0(7)	119.9(2)
C1–C2–N5	109.68(13)	113.60(8)	113.1(6)	114.7(2)
C1–C2–N6	113.00(13)	112.04(8)	108.7(6)	110.9(2)
N5–C2–N6	104.60(12)	103.55(8)	103.9(5)	102.7(2)

---

The geometry of the five-membered ring in HFDNTz is essentially identical to the one of 5-(trinitromethyl)-2H-tetrazole (HTNTz).⁵ Due to the strong electron withdrawing effect of the fluorodinitromethyl group, the hydrogen atom of the tetrazole moiety is exclusively located in the 2-position (N2) of the five-membered ring. Similar to HTNTz and atypical for alkyl-substituted tetrazoles, the distance between C1 and N1 (1.325(2) Å) is shorter than the one between C1 and N4 (1.350(2) Å). In addition, the three N–N distances in the five-membered ring of HFDNTz can be considered identical within their margins of error. This is in good agreement with the observed geometry of HTNTz but is unlike the distance pattern of a regular alkyl-substituted tetrazole.⁵ The asymmetric unit of the 5-(fluorodinitromethyl)-2H-tetrazole solid-state structure consists of three HFDNTz molecules (Z′ = 3) that are arranged in a triangular fashion with the fluorine atoms of the –CF(NO₂)₂ groups facing each other (Fig. 6). The three fluorine atoms form the corners of a slightly disordered regular triangle with F–F distances of 2.886(2) and 2.939(2) Å and F–F–F angles of 58.82(4) and 60.59(4)°. In addition, the HFDNTz molecules are associated through N(2)–H⋯N(4) hydrogen bonds.

Fig. 6 The asymmetric unit in the solid-state structure of 5-(fluorodinitromethyl)-2H-tetrazole. Thermal ellipsoids are shown at the 50% probability level. Selected distances (Å) and angles (°): F1–F2 2.886(2), F1–F3 2.939(1), F2–F3 2.939(2), F1–F2–F3 60.59(4), F2–F3–F1 58.82(4), F2–F1–F3 60.59(4).

The solid-state structure of ammonium 5-(fluorodinitromethyl)tetrazolate consists of ammonium cations and FDNTz anions that are associated through hydrogen bonding (Fig. 7). Further crystallographic details of the structure are listed in Table 2, the observed bond lengths and angles for the FDNTz⁻ anion are summarized in Table 3.

Fig. 7 Hydrogen bonding in the solid-state structure of [NH₄][FDNTz]. Hydrogen atom positions were determined from the electron density map and are depicted as spheres of arbitrary radius. Selected distances (Å): N1–N14 2.915(2), N2–N13 3.007(1), N7–N13′ 2.944(1), N8–N13, 2.982(2), N9–N14 2.965(1), N10–N13′’ 3.018(1).

All attempts to grow single crystals of silver 5-(fluorodinitromethyl)tetrazolate (AgFDNTz) suitable for X-ray structure determination were unsuccessful. The crystallization of an amorphous sample of AgFDNTz from an aqueous ammonia solution resulted in crystals of the ammonia adduct Ag[FDNTz]·½NH₃ instead. Selected crystallographic data of the compound are listed in Table 2. The solid-state structure of the silver salt contains [Ag(NH₃)₂]⁺ cations and polymeric anion chains. The anion chains are made up from [Ag₄(FDNTz)₄] units in which two silver atoms are linked in a 1,2-fashion by always two bridging FDNTz⁻ anions. Every tetrazolate anion is coordinated to three different Ag atoms. The units are linked together by Ag(NH₃) and Ag(NH₃)₂ units, resulting in a complex polymeric anion chain. The resulting overall structure can be described as [Ag(NH₃)₂]₃[Ag₂₁(NH₃)₆(FDNTz)₂₄]. Part of a polymeric anion chain of the structure is depicted in Fig. 8. Further crystallographic details of the structure are listed in Table 2, the observed bond lengths and angles for the FDNTz⁻ anion are summarized in Table 3.

Fig. 8 Part of the polymeric anion structure of Ag[FDNTz]·½NH₃. Hydrogen atoms have been omitted for clarity. Selected bond distances (Å): Ag1–N2, Ag1–N7, Ag1–N15, Ag2–N2, Ag2–N78, Ag2–N79, Ag3–N14, Ag3–N8, Ag3–N21.

The tetraphenylphosphonium salt [PPh₄][FDNTz] crystallizes in the monoclinic space group P2₁ with two formula units per unit cell (Z = 2). The solid-state structure consists of isolated and well-separated PPh₄⁺ cations and FDNTz⁻ anions (Fig. 9). The closest cation–anion distance is 2.989(3) Å (C18⋯O4). Further crystallographic details of the structure are listed in Table 2, the observed bond lengths and angles for the FDNTz⁻ anion are summarized in Table 3. In going from the neutral tetrazole HFDNTz to the weakly coordinated tetrazolate anion in [PPh₄][FDNTz], the geometry of the five-membered ring changes. While the C1–N1 distance increases only slightly (0.01 Å), the second C–N distance (C1–N4) shortens by over 0.03 Å).

Fig. 9 Molecular structure of [PPh₄][FDNTz]. Hydrogen atoms have been omitted for clarity. Selected bond distances (Å) and bond angles (°): C1–C2 1.476(4), C1–N1 1.335(4), C1–N4 1.319(4), C2–N5 1.543(4), C2–N6 1.534(4), C2–F1 1.339(4), N1–N2 1.347(4), C1–C2–F1 114.1(2), C1–C2–N5 114.7(2), C1–C2–N6 110.9(2), N1–C1–C2 119.9(3).

It is interesting to note that the N1–N2 and N3–N4 distances in the anion are longer by about 0.02 Å than the ones in the parent tetrazole. The third N–N distance (N2–N3) remains essentially unchanged within the error margins.

Stability of the compounds

The impact and friction sensitivities of most of the compounds of this study were determined using a BAM Fall Hammer and BAM Friction tester. In addition, decomposition temperatures were determined through DTA scans with heating rates of 5 °C min⁻¹. The obtained sensitivity and stability data is summarized in Table 4. The impact and friction sensitivities, and decomposition temperature of F(NO₂)₂CCN were not determined due to the volatility of the compound.

Table 4 Sensitivity and stability data for the compounds studied^a

Compound	T d  [°C]^b	FS [N]	IS [J]	OB [%]
a T d: decomposition temperature, FS: friction sensitivity, IS: impact sensitivity, OB: oxygen balance. b DTA onset. c Sample evaporates. d Endotherm at 180 °C (melting). e Explosion. f Endotherm at 165 °C (loss of NH3).
RDX	220	120	7.5	−21
(NO2)3CCN	—^c	112	12	17.4
Na[(NO2)2CCN]	150	>360	80	−5.2
[NH4][(NO2)2CCN]	240	>360	75	−21.6
[PPh4][(NO2)2CCN]	240^d	>360	>100	−206.2
[N2H5][(NO2)2CH]	134	230	90	−11.6
HFDNTz	110^e	40	3.5	−2.1
[NH4][FDNTz]	140^e	50	4	−13.4
[Ag][FDNTz]	185	<2	2	−1.3
[Ag][FDNTz]·½NH3	180^f	<2	2	−5.2
[PPh4][FDNTz]	175	>360	>100	−181.7

---

With the exception of trinitroacetonitrile, all investigated compounds are under-oxidized and have a negative oxygen balance. It is not surprising that based on the impact and friction sensitivities, the two most stable compounds, [PPh₄][(NO₂)₂CCN] and [PPh₄][FDNTz], are the ones with the lowest oxygen balances. Explosion upon heating were observed only in the case of the free tetrazole HFDNTz as well as the corresponding ammonium salt [NH₄][FDNTz]. All other investigated compounds showed smooth thermal decompositions. In the case of (NO₂)₃CCN, it was not possible to determine a decomposition temperature because the sample evaporated completely upon heating with a nitrogen purge before its decomposition. The thermally least stable compounds are HFDNTz, [N₂H₅][NO₂)₂CH], [NH₄][FDNTz], and Na[(NO₂)₂CCN] with decomposition temperatures of 110 °C, 134 °C, 140 °C, and 150 °C, respectively. It is interesting that [NH₄][(NO₂)₂CCN)] shows a much higher thermal stability of 240 °C than the closely related Na[(NO₂)₂CCN)] (150 °C). This might be related to the different oxygen balances as well as the presence of stabilizing hydrogen bonding in the case of the ammonium salt. With the exception of the PPh₄⁺ salt, all 5-(fluorodinitromethyl)tetrazolates and the parent 5-(fluorodinitromethyl)-2H-tetrazole are sensitive compounds. With impact sensitivities of less than 5 J and friction sensitivities of 50 Nm or less, these compounds must be considered explosion hazards that have to be handled with great care while using proper safety precautions. Both silver salts, [Ag][FDNTz] and [Ag][FDNTz]·½NH₃, are especially treacherous with friction sensitivities of fewer than 2 Nm and impact sensitivities of about 2 J.

Conclusions

5-(Fluorodinitromethyl)-2H-tetrazole was prepared by a four-step synthesis starting from cyanoacetamide. Nitration of cyanoacetamide with fuming nitric acid in oleum resulted in the formation of trinitroacetonitrile, which was converted into sodium dinitrocyanomethanide by reaction with HBr, followed by treatment with NaOH. Aqueous fluorination with 10% fluorine in nitrogen resulted in the formation of fluorodinitroacetonitrile and, after reaction with HN₃, in the isolation of 5-(fluorodinitromethyl)-2H-tetrazole. The tetrazole was converted into ammonium, silver and tetraphenylphosphonium 5-(fluorodinitromethyl)-2H-tetrazolate. While the treatment of trinitroacetonitrile with aqueous NH₃ resulted in the isolation of [NH₄][(NO₂)₂CCN], [N₂H₅][(NO₂)₂CH] is formed in the reaction of trinitroacetonitrile with hydrazine hydrate. Most compounds of this study have been fully characterized by their X-ray crystal structure, vibrational and multinuclear NMR spectra, their decomposition temperature, as well as friction and impact sensitivities.

Note added at Proof

During the peer-review process of this manuscript, M. A. Kettner and T. M. Klapötke coincidently reported the synthesis and characterization of ammonium 5-(fluorodinitromethyl)tetrazolate.³⁰

Acknowledgements

The Office of Naval Research (ONR) and the Defence Threat Reduction Agency (DTRA) financially supported this work. We acknowledge NSF CRIF grant 1048807 for the support of an X-ray diffractometer. We thank Professors G. K. S. Prakash and G. A. Olah for their help and stimulating discussions.

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Footnote

† Electronic supplementary information (ESI) available: Crystallographic reports including packing diagrams. CCDC 1044179–1044181. For ESI and crystallographic data in CIF or other electronic format see DOI: 10.1039/c5dt00291e

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