Tetrafluorohydrazine

Tetrafluorohydrazine
Names
	IUPAC name 1,1,2,2-tetrafluorohydrazine
	Other names Tetrafluorohydrazine, perfluorohydrazine, UN 1955
Identifiers
CAS Number	10036-47-2 ;
3D model (JSmol)	Interactive image;
ChemSpider	23228 ;
ECHA InfoCard	100.030.091
PubChem CID	24845;
CompTox Dashboard (EPA)	DTXSID9064922 ;
	InChI InChI=1S/F4N2/c1-5(2)6(3)4 Key: GFADZIUESKAXAK-UHFFFAOYSA-N ; InChI=1/F4N2/c1; InChI=1/F4N2/c1-5(2)6(3)4 Key: GFADZIUESKAXAK-UHFFFAOYAX;
	SMILES FN(F)N(F)F;
Properties
Chemical formula	N2F4
Molar mass	104.01 g mol−1
Melting point	−164.5 °C (−264.1 °F; 108.6 K)
Boiling point	−73 °C (−99 °F; 200 K)
	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 (ΔH_f) 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.

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[Greenwood&Earnshaw-1] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[2] Tetrafluorohydrazine at DTIC.mil archived March 12, 2007

[3] 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.

[bohn67-4] 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

[5] "Nitrogen difluoride NF₂(g)". www.chem.msu.su.

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