Hexanitroethane
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| Preferred IUPAC name
Hexanitroethane | |
| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.011.857 |
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| C2N6O12 | |
| Molar mass | 300.0544 |
| Melting point | 135 °C (275 °F; 408 K) |
| Related compounds | |
Related compounds
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Nitroethane Tetranitromethane Trinitromethane Hexanitrobenzene Octanitrocubane |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Hexanitroethane (HNE) is an organic compound with chemical formula C2N6O12 or (O2N)3C-C(NO2)3. It is a solid matter with a melting point of 135 °C.
Hexanitroethane is used in some pyrotechnic compositions as a nitrogen-rich oxidizer, e.g. in some decoy flare compositions and some propellants. Like hexanitrobenzene, HNE is investigated as a gas source for explosively pumped gas dynamic laser.
A composition of HNE as oxidizer with boron as fuel is being investigated as a new explosive.[1]
Preparation
[edit]The first synthesis was described by Wilhelm Will in 1914, using the reaction between the potassium salt of tetranitroethane with nitric acid.[2]
- C2(NO2)4K2 4 HNO3 → C2(NO2)6 2 KNO3 2 H2O
A practicable method for industrial use starts with furfural,[3] which first undergoes oxidative ring-opening by bromine to mucobromic acid.[4] In the following step, mucobromic acid is reacted with potassium nitrite at just below room temperature to form the dipotassium salt of 2,3,3-trinitropropanal. The final product is obtained by nitration with nitric acid and sulfuric acid at −60 °C.
Properties
[edit]The thermal decomposition of hexanitroethane has been detected at 60 °C upwards in both the solid and solution phases.[5] Above 140 °C, this can occur explosively.[6] The decomposition is first order and is significantly faster in solution than in the solid. For the solid, the following reaction can be formulated:[5]
- C2(NO2)6 → 3 NO2 NO N2O 2 CO2
For the decomposition in solution, tetranitroethylene is first formed and can be trapped and detected as a Diels–Alder adduct, for example with anthracene or cyclopentadiene.[7][8]
References
[edit]- ^ Compatibility Testing of Hexanitroethane with Boron Archived September 30, 2007, at the Wayback Machine
- ^ Will, W. (1914). "Über das Hexanitro-äthan". Berichte der Deutschen Chemischen Gesellschaft (in German). 47 (1): 961–965. doi:10.1002/cber.191404701154.
- ^ US 3101379, "Synthesis of hexanitroethane", issued 1961-01-04
- ^ Taylor, G. (2015). "MUCOBROMIC ACID". Organic Syntheses: 11–12. doi:10.15227/orgsyn.000.0011.
- ^ a b Marshall, Henry P.; Borgardt, Frank G.; Noble, Paul (1965). "Thermal Decomposition of Hexanitroethane 1a,b". The Journal of Physical Chemistry. 69 (1): 25–29. doi:10.1021/j100885a007. ISSN 0022-3654.
- ^ Bretherick, L. (18 March 2017). Bretherick's Handbook of Reactive Chemical hazards. Urben, P. G. (8th ed.). Amsterdam. pp. 240–241. ISBN 978-0-08-101059-4. OCLC 982005430.
{{cite book}}: CS1 maint: location missing publisher (link) - ^ Griffin, T. Scott; Baum, Kurt (1980). "Tetranitroethylene. In situ formation and Diels-Alder reactions". The Journal of Organic Chemistry. 45 (14): 2880–2883. doi:10.1021/jo01302a024. ISSN 0022-3263.
- ^ Tzeng, Dongjaw; Baum, Kurt (1983). "Reactions of hexanitroethane with alcohols". The Journal of Organic Chemistry. 48 (26): 5384–5385. doi:10.1021/jo00174a053. ISSN 0022-3263.