| 词条 | Fluorine azide | ||||||||||||||||
| 释义 |
| Watchedfields = changed | verifiedrevid = | ImageFileL1 = Fluorine azide.svg | ImageSizeL1 = 120px | ImageFileR1 = Fluorine-azide-3D-balls.png | ImageSizeR1 = 100px | IUPACName = | OtherNames = triazadienyl fluoride |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|??}} | CASNo = 14986-60-8 | UNNumber = | PubChem = 23235952 | InChI=1S/FN3/c1-3-4-2 | InChIKey=AJXWEJAGUZJGRI-UHFFFAOYSA-N | SMILES = [N-]=[N+]=NF}} |Section2={{Chembox Properties | Formula = FN3 | MolarMass = 61.019 g/mol | Appearance = Yellow green gas | Density = | MeltingPtC = -152 | BoilingPtC = -82 | Solubility = | SolubleOther = }} |Section3={{Chembox Explosive | ShockSens = Extreme | FrictionSens = Extreme | DetonationV = | REFactor = }} |Section4={{Chembox Hazards | MainHazards = Extremely sensitive explosive | NFPA-H = | NFPA-F = 0 | NFPA-R = 4 | NFPA_ref = {{cn|date= August 2018}} | FlashPt = | AutoignitionPt = }} |Section8={{Chembox Related | OtherAnions = | OtherCations = Hydrazoic acid Chlorine azide | OtherFunction = | OtherFunction_label = | OtherCompounds = }} }}Fluorine azide or triazadienyl fluoride (FN3) is a yellow green gas composed of nitrogen and fluorine with formula FN3.[1] It is counted as an interhalogen compound, as the azide functional group is termed a pseudohalogen. It resembles ClN3, BrN3, and IN3 in this respect.[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.[2] The gas liquifies at –82° and can be turned to a solid at –152 °C.[1][3] It was first made by John F. Haller in 1942.[4] ReactionsFluorine azide can be made by reacting hydrazoic acid and fluorine gas.[5] Another way to form it is by reacting sodium azide with fluorine.[6] 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:[6] FN3 → FN{a1Δ} + N2. Solid or liquid FN3 explodes, releasing much heat. A thin film burns at the rate of 1.6 km/s.[7] Because the explosion hazard is great only very small quantities of this substance should be handled at a time. A 0.02 g limit is recommended for experiments.[13] N3F adducts can be formed with the Lewis acids boron trifluoride (BF3) and arsenic pentafluoride (AsF5) at -196 °C. These molecules bond with the Nα atom.[14] PropertiesSpectroscopy
ShapeThe nitrogen atoms in this molecule can be labelled with Greek letters: Nα for nitrogen attached to fluorine, Nβ for the intermediate nitrogen, and Nγ for the terminal nitrogen.[8] The terminal nitrogen can also be labelled Nω.[9] Distances between atoms are F-N 0.1444 nm, FN-NN 0.1253 nm and FNN-N 0.1132 nm.[10] PhysicalN3F has a density of 1.3 g/cm3.[11] N3F adsorbs on to solid surfaces of potassium fluoride, but not onto lithium fluoride or sodium fluoride. This property was being investigated so that N3F 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, nN or nF, nF, πF, nN or σ, π and σ.[9] References1. ^1 2 {{cite journal|last=Gipstein|first=Edward|author2=John F. Haller |year=1966|title=Absorption Spectrum of Fluorine Azide|journal=Applied Spectroscopy|volume=20|issue=6|pages=417–418|issn=0003-7028|doi=10.1366/000370266774386470|bibcode=1966ApSpe..20..417G}} 2. ^{{cite journal|last=Peters|first=Nancy J. S.|author2=Leland C. Allen |author3=Raymond A. Firestone |year=1988|title=Fluorine azide and fluorine nitrate: structure and bonding|journal=Inorganic Chemistry|volume=27|issue=4|pages=755–758|issn=0020-1669|doi=10.1021/ic00277a035}} 3. ^1 {{cite book|last=Saxena|first=P. B.|title=Chemistry of Interhalogen Compounds|url=https://books.google.com/books?id=nvatWdX1ZWcC&pg=PA96|accessdate=16 June 2014|date=2007-01-01|publisher=Discovery Publishing House|isbn=9788183562430|page=96}} 4. ^{{cite web|url=http://blogs.sciencemag.org/pipeline/archives/2008/10/21/things_i_wont_work_with_triazadienyl_fluoride|title=Things I Won't Work With: Triazadienyl Fluoride.|last=Lowe|first=Derek|authorlink=Derek Lowe (chemist)|date=21 October 2008|work=In the Pipeline|accessdate=15 June 2014}} 5. ^{{cite journal|last=Gholivand|first=Khodayar|author2=Gabriele Schatte |author3=Helge Willner |year=1987|title=Properties of triazadienyl fluoride, N3F|journal=Inorganic Chemistry|volume=26|issue=13|pages=2137–2140|issn=0020-1669|doi=10.1021/ic00260a025}} 6. ^1 {{cite journal|last=Benard|first=D. J.|author2=B. K. Winker |author3=T. A. Seder |author4=R. H. Cohn |year=1989|title=Production of nitrogen monofluoride (a1Δ) by dissociation of fluorine azide|journal=The Journal of Physical Chemistry|volume=93|issue=12|pages=4790–4796|issn=0022-3654|doi=10.1021/j100349a022}} 7. ^{{cite journal|last=Seder|first=T.A.|author2=D.J. Benard |year=1991|title=The decomposition of condensed phase fluorine azide|journal=Combustion and Flame|volume=85|issue=3–4|pages=353–362|issn=0010-2180|doi=10.1016/0010-2180(91)90139-3}} 8. ^1 {{cite journal|last=Schatte|first=G.|author2=H. WIllner |year=1991|title=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|journal=Zeitschrift für Naturforschung B|volume=46|issue=4|pages=483–489|issn=0932-0776|language=de}} 9. ^1 2 {{cite journal|last=Rademacher|first=Paul|author2=Andreas J. Bittner |author3=Gabriele Schatte |author4=Helge Willner |year=1988|title=Photoelectron Spectrum and Electronic Structure of Triazadienyl Fluoride, N3F|journal=Chemische Berichte|volume=121|issue=3|pages=555–557|issn=0009-2940|doi=10.1002/cber.19881210325}} 10. ^1 2 {{cite journal|last=Christen|first=Dines.|author2=H. G. Mack |author3=G. Schatte |author4=H. Willner |year=1988|title=Structure of triazadienyl fluoride, FN3, by microwave, infrared, and ab initio methods|journal=Journal of the American Chemical Society|volume=110|issue=3|pages=707–712|issn=0002-7863|doi=10.1021/ja00211a007}} 11. ^1 {{cite book|last1=Brener|first1=Nathan E.|last2=Kestner|first2=Neil R.|last3=Callaway|first3=Joseph|title=Theoretical Studies of Highly Energetic CBES Materials: Final Report for the Period 2 March 1987 to 31 May 1987|url=http://www.dtic.mil/dtic/tr/fulltext/u2/a231340.pdf|accessdate=25 June 2014|date=December 1990|publisher=Louisiana State University, Department of Physics and Astronomy|pages=21–27}} External links
3 : Nitrogen fluorides|Azides|Gases with color |
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