| 词条 | Chlorine pentafluoride |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 446239416 | Name = Chlorine pentafluoride | ImageFileL1 = Chlorine-pentafluoride-2D-dimensions.png | ImageFileR1 = Chlorine-pentafluoride-3D-balls.png | ImageFile2 = Chlorine-pentafluoride-3D-vdW.png | ImageSize2 = 135px | Section1 = {{Chembox Identifiers | CASNo_Ref = {{cascite|correct|??}} | CASNo = 13637-63-3 | PubChem = 61654 | RTECS = FO2975000 | ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} | ChemSpiderID = 55559 | StdInChI_Ref = {{stdinchicite|changed|chemspider}} | StdInChI = 1S/ClF5/c2-1(3,4,5)6 | StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} | StdInChIKey = KNSWNNXPAWSACI-UHFFFAOYSA-N | SMILES = FCl(F)(F)(F)F | Section2 = {{Chembox Properties | Formula = ClF5 | MolarMass = 130.445 g mol−1 | Appearance = colorless gas | MeltingPtC = −103 | BoilingPtC = −13.1 | Density = 4.5 kg/m3 (g/L) | Solubility = Hydrolyzes | Section3 = {{Chembox Structure | MolShape = Square pyramidal | Dipole = | Section4 = {{Chembox Thermochemistry | DeltaHf = −238.49 kJ mol−1 | Entropy = 310.73 J K−1 mol−1 }}Chlorine pentafluoride is an interhalogen compound with formula ClF5. This colourless gas is a strong oxidant that was once a candidate oxidizer for rockets. The molecule adopts a square pyramidal structure with C4v symmetry,[1] as confirmed by its high-resolution 19F NMR spectrum.[2] PreparationSome of the earliest research on the preparation was classified.[3][4] It was first prepared by fluorination of chlorine trifluoride at high temperatures and high pressures:[3] ClF3 + F2 → ClF5 ClF + 2F2 → ClF5 Cl2 + 5F2 → 2ClF5 CsClF4 + F2 → CsF + ClF5 NiF2 catalyzes this reaction.[5] Certain metal fluorides, MClF4 (i.e. KClF4, RbClF4, CsClF4), react with F2 to produce ClF5 and the corresponding alkali metal fluoride.[4] ReactionsIn a highly exothermic reaction, ClF5 reacts with water to produce chloryl fluoride and hydrogen fluoride:[6] {{chem|Cl|F|5}} + 2 {{chem|H|2|O}} → {{chem|Cl|O|2|F}} + 4 {{chem|H|F}} It is also a strong fluorinating agent. At room temperature it reacts readily with all elements (including otherwise "inert" elements like platinum and gold) except noble gases, nitrogen, oxygen and fluorine.[2] See also
References1. ^{{Greenwood&Earnshaw2nd|page=833}} 2. ^1 {{cite journal|author1=Pilipovich, D. |author2=Maya, W. |author3=Lawton, E.A. |author4=Bauer, H.F. |author5=Sheehan, D. F. |author6=Ogimachi, N. N. |author7=Wilson, R. D. |author8=Gunderloy, F. C. |author9=Bedwell, V. E. | title = Chlorine pentafluoride. Preparation and Properties| journal = Inorganic Chemistry| year = 1967| volume = 6| issue = 10| pages = 1918| doi = 10.1021/ic50056a036}} 3. ^1 {{Cite book| title = Ignition! An Informal History of Liquid Rocket Propellants| url = http://www.sciencemadness.org/library/books/ignition.pdf| last = Clark| first = John D.| authorlink = John Drury Clark| publisher = Rutgers University Press| year = 1972| pages = 87–88| isbn = 0-8135-0725-1 }} 4. ^1 {{cite journal|author = Smith D. F.| title = Chlorine Pentafluoride| journal = Science| year = 1963| volume = 141| issue = 3585| pages = 1039–1040| doi = 10.1126/science.141.3585.1039| pmid = 17739492}} 5. ^{{cite journal| vauthors = Šmalc A, Žemva B, Slivnik J, Lutar K| title = On the Synthesis of Chlorine Pentafluoride| journal = Journal of Fluorine Chemistry| year = 1981| volume = 17| pages = 381–383| doi = 10.1016/S0022-1139(00)81783-2| issue = 4}} 6. ^{{Greenwood&Earnshaw2nd|page=834}} External links
6 : Fluorides|Inorganic chlorine compounds|Interhalogen compounds|Rocket oxidizers|Fluorinating agents|Oxidizing agents |
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