词条 | Nitryl fluoride |
释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 428847234 | Name = Nitryl fluoride | ImageFileL1 = Nitryl-fluoride-2D-dimensions.png | ImageNameL1 = Nitryl fluoride | ImageFileR1 = Nitryl-fluoride-3D-vdW.png | ImageNameR1 = Nitryl fluoride | OtherNames = |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|??}} | CASNo = 10022-50-1 | UNII_Ref = {{fdacite|changed|FDA}} | UNII = DAT2I9R64A | EINECS = 233-021-0 | PubChem = 66203 | ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} | ChemSpiderID = 59588 | SMILES = [N+](=O)([O-])F | InChI = 1/FNO2/c1-2(3)4 | InChIKey = JVJQPDTXIALXOG-UHFFFAOYAU | StdInChI_Ref = {{stdinchicite|changed|chemspider}} | StdInChI = 1S/FNO2/c1-2(3)4 | StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} | StdInChIKey = JVJQPDTXIALXOG-UHFFFAOYSA-N |Section2={{Chembox Properties | Formula = {{nitrogen}}{{oxygen|2}}{{fluorine}} | MolarMass = 65.0039 g/mol | Density = | Solvent = other solvents | SolubleOther = | MeltingPtC = -166 | BoilingPtC = -72 }} |Section8={{Chembox Related | OtherAnions = nitryl chloride, nitryl bromide | OtherCations = nitrosyl fluoride, sulfuryl fluoride }}Nitryl fluoride, NO2F, is a colourless gas and strong oxidizing agent, which is used as a fluorinating agent[1] and has been proposed as an oxidiser in rocket propellants (though never flown). It is a molecular species, not ionic, consistent with its low boiling point. The structure features planar nitrogen with a short N-F bond length of 135 pm.[2] PreparationHenri Moissan and Lebeau recorded the preparation of nitryl fluoride in 1905 by the fluorination of nitrogen dioxide. This reaction is highly exothermic, which leads to contaminated products. The simplest method avoids fluorine gas but uses cobalt(III) fluoride:[3]NO2 + CoF3 → NO2F + CoF2 The CoF2 can be regenerated to CoF3. Other methods have been described.[4] Thermodynamic propertiesThe thermodynamic properties of this gas were determined by IR and Raman spectroscopy[5] The standard heat of formation of FNO2 is -19 ± 2 kcal/mol.3
ReactionsNitryl fluoride can be used to prepare organic nitro compounds and nitrate esters. See also
References1. ^Merck Index, 13th edition (2001), p.1193 2. ^F. A. Cotton and G.Wilkinson, Advanced Inorganic Chemistry, 5th edition (1988), Wiley, p.333. 3. ^{{cite journal|last=Davis|first=Ralph A.|author2=Rausch, Douglas A. |title=Preparation of Nitryl Fluoride|journal=Inorganic Chemistry|volume=2|issue=6|pages=1300–1301|doi=10.1021/ic50010a048|year=1963}} 4. ^{{cite journal|last1=Faloon|first1=Albert V.|last2=Kenna|first2=William B.|title=The Preparation of Nitrosyl Fluoride and Nitryl Fluoride1|journal=Journal of the American Chemical Society|volume=73|issue=6|year=1951|pages=2937–2938|issn=0002-7863|doi=10.1021/ja01150a505}} 5. ^1 2 3 4 {{cite journal|last=Tschuikow-Roux|first=E.|title=THERMODYNAMIC PROPERTIES OF NITRYL FLUORIDE|journal=Journal of Physical Chemistry|volume=66|issue=9|pages=1636–1639|doi=10.1021/j100815a017|year=1962}} External links
4 : Oxohalides|Fluorinating agents|Fluorides|Nonmetal halides |
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