Tetrafluorohydrazine
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IUPAC name
1,1,2,2-tetrafluorohydrazine
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Other names
Tetrafluorohydrazine, perfluorohydrazine, UN 1955
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Identifiers | |
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ChemSpider | |
ECHA InfoCard | 100.030.091 |
PubChem CID
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CompTox Dashboard (EPA)
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Properties | |
Chemical formula
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N2F4 |
Molar mass | 104.01 g mol−1 |
Melting point | −164.5 °C (−264.1 °F; 108.6 K) [1] |
Boiling point | −73 °C (−99 °F; 200 K)[1] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
what is ?) | (|
Infobox references | |
Tetrafluorohydrazine or perfluorohydrazine, N2F4, is a colourless, reactive inorganic gas. It is a fluorinated analog of hydrazine. It is a highly hazardous chemical that explodes in the presence of organic materials.
Tetrafluorohydrazine is manufactured from nitrogen trifluoride using an iron catalyst or iron(II) fluoride. It is used in some chemical syntheses, as a precursor or a catalyst.
Tetrafluorohydrazine was considered for use as a high-energy liquid oxidizer in some never-flown rocket fuel formulas in 1959.[2]
Properties[]
Tetrafluorohydrazine is in equilibrium with its radical monomer nitrogen difluoride.[3]
- N2F4 ⇌ 2 NF2•
At room temperature N2F4 is mostly associated with only 0.7% in the form of NF2 at 5mm Hg pressure. When the temperature rises to 225 °C, it mostly dissociates with 99% in the form of NF2.[4]
The energy needed to break the N-N bond in N2F4 is 20.8 kcal/mol, with an entropy change of 38.6 eu.[4] For comparison, the dissociation energy of the N-N bond is 14.6 kcal/mol in N2O4, 10.2 kcal/mol in N2O2, and 60 kcal/mol in N2H4. The enthalpy of formation of N2F4 (ΔHf) is 34.421 kJ/mol.[5]
References[]
- ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Tetrafluorohydrazine at DTIC.mil archived March 12, 2007
- ^ Jäger, Susanne; von Jouanne, Jörn; Keller-Rudek, Hannelore; Koschel, Dieter; Kuhn, Peter; Merlet, Peter; Rupecht, Sigrid; Vanecek, Hans; Wagner, Joachim (1986). Koschel, Dieter; Kuhn, Peter; Merlet, Peter; Ruprecht, Sigrid; Wagner, Joachim (eds.). F Fluorine: Compounds with Oxygen and Nitrogen. Gmelin Handbook of Inorganic Chemistry. 4. Berlin: Springer. p. 162. doi:10.1007/978-3-662-06339-2. ISBN 978-3-662-06341-5. Retrieved 29 August 2015.
- ^ a b Bohn, Robert K.; Bauer, Simon Harvey (February 1967). "An electron diffraction study of the structures of NF2 and N2F4". Inorganic Chemistry. 6 (2): 304–309. doi:10.1021/ic50048a024. molecule dimensions and angles
- ^ "Nitrogen difluoride NF2(g)". www.chem.msu.su.
- Nitrogen fluorides
- Rocket oxidizers
- Hydrazines
- Gases
- Fluorides