| 词条 | Perfluorotributylamine | |
| 释义 |
| ImageFile = Perfluorobutylamine Structure V.1.svg | ImageSize = | ImageAlt = | IUPACName = 1,1,2,2,3,3,4,4,4-nonafluoro-N,N-bis(1,1,2,2,3,3,4,4,4-nonafluorobutyl)butan-1-amine | PIN = 1,1,2,2,3,3,4,4,4-nonafluoro-N,N-bis(nonafluorobutyl)butan-1-amine | OtherNames = Fluorinert |Section1={{Chembox Identifiers | Abbreviations = PFTBA | CASNo = 311-89-7 | PubChem = 9397 | ChemSpiderID = 13836523 | ChEBI = 38854 | SMILES = C(C(C(F)(F)F)(F)F)(C(N(C(C(C(C(F)(F)F)(F)F)(F)F)(F)F)C(C(C(C(F)(F)F)(F)F)(F)F)(F)F)(F)F)(F)F | InChI = 1/C12F27N/c13-1(14,7(25,26)27)4(19,20)10(34,35)40(11(36,37)5(21,22)2(15,16)8(28,29)30)12(38,39)6(23,24)3(17,18)9(31,32)33 | InChIKey = RVZRBWKZFJCCIB-UHFFFAOYAW | StdInChI = 1S/C12F27N/c13-1(14,7(25,26)27)4(19,20)10(34,35)40(11(36,37)5(21,22)2(15,16)8(28,29)30)12(38,39)6(23,24)3(17,18)9(31,32)33 | StdInChIKey = RVZRBWKZFJCCIB-UHFFFAOYSA-N }} |Section2={{Chembox Properties | C=12 | F=27 | N=1 | Appearance = | Density = 1.884 g/mL | MeltingPtC = -50 | BoilingPtC = 178 | Solubility = Insoluble | SolubleOther = Insoluble | Solvent = methanol and isopropyl alcohol}} |Section3={{Chembox Hazards | MainHazards = | FlashPt = | AutoignitionPt = }} }} Perfluorotributylamine (PFTBA), also referred to as FC43, is a colorless liquid with the formula N(C4F9)3. The compound consists of three butyl groups connected to an amine center, in which all of the hydrogen atoms have been replaced with fluorine. The compound is produced for the electronics industry, along with other perfluoroalkylamines. Unlike ordinary amines, perfluoroamines are nonbasic. PreparationIt is prepared by electrofluorination of tributylamine using hydrogen fluoride as solvent and source of fluorine:[1] N(C4H9)3 + 27 HF → N(C4F9)3 + 27 H2 UsesThe compound has two commercial uses. It is used as an ingredient in Fluosol, artificial blood. This application exploits the high solubility of oxygen and carbon dioxide in the solvent, as well as the low viscosity and toxicity.[1] It is also a component of Fluorinert coolant liquids. CPUs of some computers are immersed in this liquid to facilitate cooling.[1] NicheThe compound is used as a calibrant[2] in gas chromatography when the analytical technique uses mass spectrometry as a detector to identify and quantify chemical compounds in gases or liquids. When undergoing ionization in the mass spectrometer, the compound decomposes in a repeatable pattern to form fragments of specific masses, which can be used to tune the mass response and accuracy of the mass spectrometer. Most commonly used ions are those with approximate mass of 69, 131, 219, 414 and 502 atomic mass units. SafetyFluorofluids are generally of very low toxicity, so much that they have been evaluated as synthetic blood.[3] Environmental impactIt is a greenhouse gas with warming properties more than 7,000 times that of carbon dioxide over a 100 year period,[4][5] and, as such, is the most potent greenhouse gas ever discovered.[6] Its concentration in the atmosphere is approximately 0.18 parts per trillion. The compound can persist in the atmosphere for up to 500 years. Sulfur hexafluoride, however, has a GWP of 23,900,[7] which would make it much more powerful. See also
References1. ^{{Cite journal | last1 = Garrelts | first1 = J. C. | title = Fluosol: An oxygen-delivery fluid for use in percutaneous transluminal coronary angioplasty | journal = DICP : The Annals of Pharmacotherapy | volume = 24 | issue = 11 | pages = 1105–1112 | year = 1990 | pmid = 2275237}} 2. ^Dunnivant, Frank and Ginsbach, Jake. "GAS CHROMATOGRAPHY, LIQUID CHROMATOGRAPHY, CAPILLARY Electrophoresis - MASS SPECTROMETRY A BASIC INTRODUCTION", Chapter 7, {{ISBN|978-0-9882761-0-9}}, ., Nov. 2012. 3. ^1 2 {{cite encyclopedia|chapter=Fluoroethers and Fluoroamines|authors=Michael G. Costello, Richard M. Flynn, John G. Owens|year=2001|publisher=Wiley-VCH|place=Weinstein|encyclopedia=Kirk-Othmer Encyclopedia of Chemical Technology|doi=10.1002/0471238961.0612211506122514.a01.pub2|isbn=978-0471238966}} 4. ^{{Cite journal | last1 = Hong | first1 = A. C. | last2 = Young | first2 = C. J. | last3 = Hurley | first3 = M. D. | last4 = Wallington | first4 = T. J. | last5 = Mabury | first5 = S. A. | title = Perfluorotributylamine: A novel long-lived greenhouse gas | doi = 10.1002/2013GL058010 | journal = Geophysical Research Letters | pages = 6010–6015| year = 2013 | pmid = | pmc = | volume=40| issue = 22 | bibcode = 2013GeoRL..40.6010H }} 5. ^{{cite web | url=https://www.theguardian.com/environment/2013/dec/10/new-greenhouse-gas-powerful-chemical-perfluorotributylamine | title=Newly discovered greenhouse gas '7,000 times more powerful than CO2' | work=The Guardian | date=10 December 2013 | accessdate=11 December 2013 | author=Goldenberg, Suzanne}} 6. ^{{cite web | url=https://www.motherjones.com/environment/2013/12/discovered-greenhouse-gas-7000-powerful-carbon-dioxide | title=Newly Discovered Greenhouse Gas "7,000 Times More Powerful than CO2" | work=Mother Jones | date=11 December 2013 | accessdate=12 December 2013 | author=Goldenberg, Suzanne}} 7. ^{{cite web |url=http://www.ipcc.ch/publications_and_data/ar4/wg1/en/ch2s2-10-2.html |title=2.10.2 Direct Global Warming Potentials |year=2007 |publisher=Intergovernmental Panel on Climate Change |accessdate=22 February 2013 }} 4 : Greenhouse gases|Perfluorinated compounds|Amines|Coolants |
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