| 词条 | Fluorine perchlorate |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 448917315 | ImageFileL1 = fluorine-perchlorate-2D.png | ImageSizeL1 = 120 | ImageAltL1 = Full structural formula of fluorine perchlorate | ImageFileR1 = Fluorine perchlorate molecule ball.png | ImageSizeR1 = 120 | ImageName1 = Ball-and-stick model of the fluorine perchlorate molecule | IUPACName = Perchloryl hypofluorite | OtherNames = Fluorine perchlorate |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|??}} | CASNo = 10049-03-3 | UNII_Ref = {{fdacite|changed|FDA}} | UNII = M5BON9S68S | ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} | ChemSpiderID = 10326178 | PubChem = 13022374 | InChI = 1/ClFO4/c2-6-1(3,4)5 | InChIKey = DRFVFUCINMEBEQ-UHFFFAOYAO | StdInChI_Ref = {{stdinchicite|changed|chemspider}} | StdInChI = 1S/ClFO4/c2-6-1(3,4)5 | StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} | StdInChIKey = DRFVFUCINMEBEQ-UHFFFAOYSA-N | SMILES = FOCl(O)(O)O }} |Section2={{Chembox Properties | Formula = {{chem|FClO|4}} | MolarMass = | Appearance = | Density = | MeltingPtC = -167.3 | BoilingPtC = -16 | Solubility = }} |Section3={{Chembox Thermochemistry | DeltaHf = 9 kcal/mol[1]}} |Section4={{Chembox Hazards | MainHazards = Highly explosive gas | FlashPt = | AutoignitionPt = }}Perchloryl Hypofluorite is the rarely encountered chemical compound of fluorine, chlorine, and oxygen with the chemical formula {{chem|ClO|4F}} or {{chem|FOClO|3}}. It is an extremely unstable gas that explodes spontaneously[2] and has a penetrating odor.[3] SynthesisOne synthesis uses fluorine and perchloric acid,[4] though the action of ClF5 on water is another method{{Citation needed|date=July 2013}}.
Another method of synthesis involves the thermal decomposition of tetrafluoroammonium perchlorate, {{chem|NF|4|ClO|4}}, which yields very pure {{chem|FClO|4}} that may be manipulated and frozen without explosions.[5]
StructureFluorine perchlorate is not analogous to perchloric acid because the fluorine atom does not exist as a positive ion. It contains an oxygen atom in a rare oxidation state of 0, due to the electronegativity of oxygen, which is higher than that of chlorine but lower than that of fluorine. SafetyFClO4 has a very dangerous and unpredictable series of reactions associated with it, as a covalent perchlorate (chlorine in the +7 oxidation state) and a compound featuring a very sensitive O-F single bond. Small amounts of reducing agent, such as organic compounds, can trigger explosive detonation. Products of these decomposition reactions could include oxygen halides, interhalogen compounds, and other hazardous substances. Accidental synthesis is possible if precursors are carelessly mixed. Like similar covalent fluorides and perchlorates, it needs to be handled with extreme caution. ReactionFClO4 is a strong oxidant and it reacts with iodide ion:
FClO4 can also react with tetrafluoroethylene:[6] CF2=CF2 + FOClO3 → CF3CF2OClO3 It may be a radical addition reaction. [7]References1. ^Breazeale, J. D.; MacLaren, R. O.. Thermochemistry of oxygen-fluorine bonding, United Technology Center, Sunnyvale, CA, 1963. Accession Number: AD0402889. Retrieved online from on 2009-05-21. 2. ^Pradyot Patnaik. A comprehensive guide to the hazardous properties of chemical substances, 3rd ed., Wiley-Interscience, 2007. {{ISBN|0-471-71458-5}} 3. ^Robert Alan Lewis. Lewis' dictionary of toxicology, CRC Press, 1998, p. 508. {{ISBN|1-56670-223-2}} 4. ^{{Cite journal| first1 = G. H.| first2 = G. H.| title = The Preparation of Fluorine Perchlorate from Fluorine and Perchloric Acid| journal = Journal of the American Chemical Society| volume = 69| issue = 3| last1 = Rohrback| pages = 677–678| year = 1947| doi = 10.1021/ja01195a063| last2 = Cady}} 5. ^{{Cite journal| first1 = C. J.| first2 = K. O.| title = Reactions of fluorine perchlorate with fluorocarbons and the polarity of the oxygen-fluorine bond in covalent hypofluorites| journal = Inorganic Chemistry| volume = 18| issue = 9| last1 = Schack| pages = 2619–2620| year = 1979| doi = 10.1021/ic50199a056| last2 = Christe}} 6. ^{{Greenwood&Earnshaw}} 7. ^{{cite journal|doi=10.1021/ic50199a056|title=Reactions of fluorine perchlorate with fluorocarbons and the polarity of the oxygen-fluorine bond in covalent hypofluorites|year=1979|last1=Schack|first1=Carl J.|last2=Christe|first2=Karl O.|journal=Inorganic Chemistry|volume=18|issue=9|pages=2619}} External links
4 : Explosive chemicals|Perchlorates|Oxidizing agents|Hypofluorites |
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