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Fluorine azide
Names
	Other names triazadienyl fluoride
Identifiers
CAS Number	14986-60-8 ;
3D model (JSmol)	Interactive image;
ChemSpider	10328964;
PubChem CID	23235952;
CompTox Dashboard (EPA)	DTXSID40631418 ;
	InChI InChI=1S/FN3/c1-3-4-2 Key: AJXWEJAGUZJGRI-UHFFFAOYSA-N;
	SMILES [N-]=[N+]=NF;
Properties
Chemical formula	FN3
Molar mass	61.019 g/mol
Appearance	Yellow-green gas
Melting point	−139 °C (−218 °F; 134 K)
Boiling point	−30 °C (−22 °F; 243 K)
Explosive data
Shock sensitivity	Extreme
Friction sensitivity	Extreme
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Extremely sensitive explosive
NFPA 704 (fire diamond)	[citation needed] 0 4
Related compounds
Other cations	Hydrazoic acid; Chlorine azide; Bromine azide; Iodine azide
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Fluorine azide or triazadienyl fluoride is a yellow green gas composed of nitrogen and fluorine with formula FN₃.^[1] Its properties resemble those of ClN₃, BrN₃, and IN₃.^[2] The bond between the fluorine atom and the nitrogen is very weak, leading to this substance being very unstable and prone to explosion.^[3] Calculations show the F–N–N angle to be around 102° with a straight line of 3 nitrogen atoms.^[4]

The gas boils at –30° and melts at –139 °C.^[5]

It was first made by John F. Haller in 1942.^[6]

Reactions

Fluorine azide can be made by reacting hydrazoic acid or sodium azide, with fluorine gas.^[5]^[7]

HN₃ + F₂ → N₃F + HF

NaN₃ + F₂ → N₃F + NaF

Fluorine azide decomposes without explosion at normal temperatures to make dinitrogen difluoride:

2 FN₃ → N₂F₂ + 2 N₂.^[1]

At higher temperatures such as 1000 °C fluorine azide breaks up into nitrogen monofluoride radical:^[7]

FN₃ → NF + N₂

The FN itself dimerizes on cooling.

2 NF → N₂F₂

Solid or liquid FN₃ can explode, releasing a large amount of energy. A thin film burns at the rate of 1.6 km/s.^[8] Due to the explosion hazard, only very small quantities of this substance should be handled at a time.^[9]

FN₃ adducts can be formed with the Lewis acids boron trifluoride (BF₃) and arsenic pentafluoride (AsF₅) at -196 °C. These molecules bond with the first nitrogen atom from the fluorine.^[10]

Properties

Spectroscopy

Parameter	Value^[9]	Unit
A	48131.448	MHz
B	5713.266	MHz
C	5095.276	MHz
μ_a	1.1
μ_b	0.7

Shape

Distances between atoms are F–N 0.1444 nm, FN=NN 0.1253 nm and FNN=N 0.1132 nm.^[9]

Physical

FN₃ has a density of 1.3 g/cm³.^[11]

FN₃ adsorbs on to solid surfaces of potassium fluoride, but not onto lithium fluoride or sodium fluoride. This property was being investigated so that FN₃ could boost the energy of solid propellants.^[11]

The ultraviolet photoelectric spectrum shows ionisation peaks at 11.01, 13,72, 15.6, 15.9, 16.67, 18.2, and 19.7 eV. Respectively these are assigned to the orbitals: π, n_N or n_F, n_F, π_F, n_N or σ, π and σ.^[3]

References

^ ^a ^b Gipstein, Edward; John F. Haller (1966). "Absorption Spectrum of Fluorine Azide". Applied Spectroscopy. 20 (6): 417–418. Bibcode:1966ApSpe..20..417G. doi:10.1366/000370266774386470. ISSN 0003-7028. S2CID 96337253.
^ Saxena, P. B. (2007-01-01). Chemistry of Interhalogen Compounds. Discovery Publishing House. p. 96. ISBN 9788183562430. Retrieved 16 June 2014.
^ ^a ^b Rademacher, Paul; Andreas J. Bittner; Gabriele Schatte; Helge Willner (1988). "Photoelectron Spectrum and Electronic Structure of Triazadienyl Fluoride, N3F". Chemische Berichte. 121 (3): 555–557. doi:10.1002/cber.19881210325. ISSN 0009-2940.
^ Peters, Nancy J. S.; Leland C. Allen; Raymond A. Firestone (1988). "Fluorine azide and fluorine nitrate: structure and bonding". Inorganic Chemistry. 27 (4): 755–758. doi:10.1021/ic00277a035. ISSN 0020-1669.
^ ^a ^b Gholivand, Khodayar; Gabriele Schatte; Helge Willner (1987). "Properties of triazadienyl fluoride, N3F". Inorganic Chemistry. 26 (13): 2137–2140. doi:10.1021/ic00260a025. ISSN 0020-1669.
^ Lowe, Derek (21 October 2008). "Things I Won't Work With: Triazadienyl Fluoride". In the Pipeline. Retrieved 15 June 2014.
^ ^a ^b Benard, D. J.; B. K. Winker; T. A. Seder; R. H. Cohn (1989). "Production of nitrogen monofluoride (a1Δ) by dissociation of fluorine azide". The Journal of Physical Chemistry. 93 (12): 4790–4796. doi:10.1021/j100349a022. ISSN 0022-3654.
^ Seder, T.A.; D.J. Benard (1991). "The decomposition of condensed phase fluorine azide". Combustion and Flame. 85 (3–4): 353–362. Bibcode:1991CoFl...85..353S. doi:10.1016/0010-2180(91)90139-3. ISSN 0010-2180.
^ ^a ^b ^c Christen, Dines.; H. G. Mack; G. Schatte; H. Willner (1988). "Structure of triazadienyl fluoride, FN₃, by microwave, infrared, and ab initio methods". Journal of the American Chemical Society. 110 (3): 707–712. Bibcode:1988JAChS.110..707C. doi:10.1021/ja00211a007. ISSN 0002-7863.
^ Schatte, G.; H. Willner (1991). "Die Wechselwirkung von N₃F mit Lewis-Säuren und HF. N₃F als möglicher Vorläufer für die Synthese von N₃+-Salzen = The interaction of N₃F with Lewis acids and HF•N₃F as possible precursor for the synthesis of N₃+ salts". Zeitschrift für Naturforschung B (in German). 46 (4): 483–489. doi:10.1515/znb-1991-0410. ISSN 0932-0776. S2CID 97045269.
^ ^a ^b Brener, Nathan E.; Kestner, Neil R.; Callaway, Joseph (December 1990). Theoretical Studies of Highly Energetic CBES Materials: Final Report for the Period 2 March 1987 to 31 May 1987 (PDF). Louisiana State University, Department of Physics and Astronomy. pp. 21–27. Archived (PDF) from the original on March 3, 2016. Retrieved 25 June 2014.