| 词条 | Vanadium tetrafluoride |
| 释义 |
| verifiedrevid = 402871120 | Name = Vanadium(IV) fluoride | ImageFileL1 = VF4structure1.jpg | ImageSizeL1 = 100px | ImageNameL1 = 3D model of vanadium(IV) fluoride | ImageFileR1 = VF4structure2.jpg | ImageSizeR1 = 100px | ImageNameR1 = 3D model of vanadium(IV) fluoride | IUPACName = vanadium tetrafluoride |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 11226730 | InChI = 1/4FH.V/h4*1H;/q;;;;+4/p-4 | InChIKey = JTWLHYPUICYOLE-XBHQNQODAC | SMILES = [V+4].[F-].[F-].[F-].[F-] | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/4FH.V/h4*1H;/q;;;;+4/p-4 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = JTWLHYPUICYOLE-UHFFFAOYSA-J | CASNo = 10049-16-8 | UNII_Ref = {{fdacite|correct|FDA}} | UNII = M372NC1A3B | PubChem = 165641 | EINECS = 233-171-7 | UNNumber = UN2923 |Section2={{Chembox Properties | V=1 | F=4 | Appearance = Lime green powder, hygroscopic[1] | Odor = Odorless | Density = 3.15 g/cm3 (20 °C)[1] 2.975 g/cm3 (23 °C)[1] | Solubility = Very soluble[1] | SolubleOther = Soluble in acetone, acetic acid Very slightly soluble in SO2Cl2, alcohols, CHCl3[1] | MeltingPtC = 325 | MeltingPt_notes = at 760 mmHg decomposes[2] | BoilingPt = Sublimes[2] |Section3={{Chembox Structure | CrystalStruct = Monoclinic, mP10 | SpaceGroup = P21/c, No. 14 |Section4={{Chembox Thermochemistry | DeltaHf = −1412 kJ/mol[3] | DeltaGf = −1312 kJ/mol[3] | Entropy = 126 J/mol·K[3] |Section7={{Chembox Hazards | GHSPictograms = {{GHS05}}{{GHS06}}[4] | GHSSignalWord = Danger | HPhrases = {{H-phrases|300|330|314|318}}[4] | PPhrases = {{P-phrases|260|301+310|303+361+353|304+340|305+351+338|320|330|405|501}}[4] | SkinHazard = Causes burns | EyeHazard = Causes serious damage }} Vanadium(IV) fluoride (VF4) is an inorganic compound of vanadium and fluorine. It is paramagnetic yellow-brown solid that is very hygroscopic.[1] Unlike the corresponding vanadium tetrachloride, the tetrafluoride is not volatile because it adopts a polymeric structure. It decomposes before melting. Preparation and reactionsVF4 can be prepared by treating VCl4 with HF: VCl4 + 4 HF → VF4 + 4 HCl It was first prepared in this way.[5] It decomposes at 325 °C, undergoing disproportionation to the tri- and pentafluorides:[1] 2 VF4 → VF3 + VF5 StructureReferences1. ^1 2 3 {{cite book|last = Kwasnik|first = W.|editor-last = Brauer|editor-first = Georg|year = 1963|title = Handbook of Preparative Inorganic Chemistry|publisher = Academic Press|place = London|edition = UK|pages = 252–253}} 2. ^1 2 3 4 {{CRC90}} 3. ^1 2 {{cite web|last = Anatolievich|first = Kiper Ruslan|website = http://chemister.ru|url = http://chemister.ru/Database/properties-en.php?dbid=1&id=408|title = vanadium(IV) fluoride|accessdate = 2014-06-25}} 4. ^1 2 {{cite web|title = Vanadium(IV) fluoride, 95%|url = http://www.alfa.com/en/catalog/11543|website = http://www.alfa.com|publisher = Alfa Aesar|accessdate = 2014-06-25}} 5. ^Otto Ruff, Herbert Lickfett "Vanadinfluoride" Chemische Berichte 1911, vol. 44, pages 2539–2549. {{DOI|10.1002/cber.19110440379}} 6. ^Becker S., Muller B. G. Vanadium Tetrafluoride, Angew. Chem. Intnl. Ed. Engl. 1990, vol. 29, page 406
4 : Vanadium compounds|Fluorides|Metal halides|Inorganic compound stubs |
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