fluorocarbon

Perfluorocarbons or PFCs, are organofluorine compounds with the formula C_xF_y, meaning they contain only carbon and fluorine.{{GoldBookRef |title= fluorocarbons |file= F02459}} The terminology is not strictly followed and many fluorine-containing organic compounds are also called fluorocarbons. Compounds with the prefix perfluoro- are hydrocarbons, including those with heteroatoms, wherein all C-H bonds have been replaced by C-F bonds.

{{cite journal

|author=Murphy WJ

|title=Fluorine Nomenclature... A statement by the Editors

|journal=Ind. Eng. Chem.

|volume=39

|issue=3

|pages=241–242

|date=March 1947

|doi=10.1021/ie50447a004

}}

Fluorocarbons includes perfluoroalkanes, fluoroalkenes, fluoroalkynes, and perfluoroaromatic compounds.

Perfluoroalkanes are very stable because of the strength of the carbon–fluorine bond, one of the strongest in organic chemistry.

{{cite journal

|author=O'Hagan D

|title=Understanding organofluorichemistry. An introduction to the C–F bond

|journal=Chem. Soc. Rev.

|date=February 2008

|volume=37

|issue=2

|pages=308–19

|pmid=18197347

|doi=10.1039/b711844a

}}

Its strength is a result of the electronegativity of fluorine imparting partial ionic character through partial charges on the carbon and fluorine atoms, which shorten and strengthen the bond (compared to carbon-hydrogen bonds) through favorable covalent interactions. Additionally, multiple carbon–fluorine bonds increase the strength and stability of other nearby carbon–fluorine bonds on the same geminal carbon, as the carbon has a higher positive partial charge. Furthermore, multiple carbon–fluorine bonds also strengthen the "skeletal" carbon–carbon bonds from the inductive effect. Therefore, saturated fluorocarbons are more chemically and thermally stable than their corresponding hydrocarbon counterparts, and indeed any other organic compound. They are susceptible to attack by very strong reductants, e.g. Birch reduction and very specialized organometallic complexes.

{{cite journal

|vauthors=Kiplinger JL, Richmond TG, Osterberg CE

|title=Activation of Carbon-Fluorine Bonds by Metal Complexes

|journal=Chem. Rev.

|volume=94

|issue=2

|pages=373–431

|year=1994

|doi=10.1021/cr00026a005

}}

Fluorocarbons are colorless and have high density, up to over twice that of water. They are not miscible with most organic solvents (e.g., ethanol, acetone, ethyl acetate, and chloroform), but are miscible with some hydrocarbons (e.g., hexane in some cases). They have very low solubility in water, and water has a very low solubility in them (on the order of 10 ppm). They have low refractive indices.

{{Image frame|content=\overset{\delta+}{C}-\overset{\delta-}{F}|caption=The partial charges in the polarized carbon–fluorine bond|width=150}}

As the high electronegativity of fluorine reduces the polarizability of the atom, fluorocarbons are only weakly susceptible to the fleeting dipoles that form the basis of the London dispersion force. As a result, fluorocarbons have low intermolecular attractive forces and are lipophobic in addition to being hydrophobic and non-polar. Reflecting the weak intermolecular forces these compounds exhibit low viscosities when compared to liquids of similar boiling points, low surface tension and low heats of vaporization. The low attractive forces in fluorocarbon liquids make them compressible (low bulk modulus) and able to dissolve gas relatively well. Smaller fluorocarbons are extremely volatile. There are five perfluoroalkane gases: tetrafluoromethane (bp −128 °C), hexafluoroethane (bp −78.2 °C), octafluoropropane (bp −36.5 °C), perfluoro-n-butane (bp −2.2 °C) and perfluoro-iso-butane (bp −1 °C). Nearly all other fluoroalkanes are liquids; the most notable exception is perfluorocyclohexane, which sublimes at 51 °C.{{cite web |url=http://www.ornl.gov/~webworks/cpr/v823/rpt/108771.pdf |title=Archived copy |access-date=2008-11-29 |url-status=dead |archive-url=https://web.archive.org/web/20081205213815/http://www.ornl.gov/~webworks/cpr/v823/rpt/108771.pdf |archive-date=2008-12-05 }} Fluorocarbons also have low surface energies and high dielectric strengths.

File:Tetrafluormethan.svg|Carbon tetrafluoride, the simplest perfluoroalkane

File:Perfluorooctane.png|Perfluorooctane, a linear perfluoroalkane

File:Perfluoro(2-methylpentane).svg|Perfluoro-2-methylpentane, a branched perfluoroalkane

File:Perfluoro-1,3-dimethylcyclohexane.svg|Perfluoro-1,3-dimethylcyclohexane, a cyclic perfluoroalkane

File:Perfluorodecaline.svg|Perfluorodecalin, a polycyclic perfluoroalkane

In the 1960s there was a lot of interest in fluorocarbons as anesthetics. The research did not produce any anesthetics, but the research included tests on the issue of flammability, and showed that the tested fluorocarbons were not flammable in air in any proportion, though most of the tests were in pure oxygen or pure nitrous oxide (gases of importance in anesthesiology).

{{cite journal

|author=Larsen ER

|title=Fluorine Compounds in Anesthesiology: VI Flammability

|journal=Fluorine Chem. Rev.

|volume=3

|year= 1969

|pages=22–27

}}

{{cite tech report

|title=Flutec

|year=1982

|institution=ISC Chemicals Limited

}}

In 1993, 3M considered fluorocarbons as fire extinguishants to replace CFCs.{{cite web|url=https://www.nist.gov/el/fire_research/upload/R9302960.pdf|title=Development of Perfluorocarbons As Clean Extinguishing Agents|author1=John A. Pignato, Jr.|author2=Paul E. Rivers|author3=Myron T. Pike|publisher=National Institute of Standards and Technology|url-status=dead|archive-url=https://web.archive.org/web/20140521123729/https://www.nist.gov/el/fire_research/upload/R9302960.pdf|archive-date=2014-05-21|access-date=2019-01-03}} This extinguishing effect has been attributed to their high heat capacity, which takes heat away from the fire. It has been suggested that an atmosphere containing a significant percentage of perfluorocarbons on a space station or similar would prevent fires altogether.{{cite journal

|author=McHale ET

|title=Life Support Without Combustion Hazards

|journal=Fire Technology

|volume=10 |issue=1 |pages=15–24 |year=1974 |doi=10.1007/bf02590509|s2cid=111161665

}}

{{cite journal

|author=Huggett C

|title=Habitable Atmospheres Which Do Not Support Combustion

|journal=Combustion and Flame

|volume=20 |pages=140–142 |year= 1973

|issue=1

|doi=10.1016/s0010-2180(73)81268-4|bibcode=1973CoFl...20..140H

}}

When combustion does occur, toxic fumes result, including carbonyl fluoride, carbon monoxide, and hydrogen fluoride.

Perfluorocarbons dissolve relatively high volumes of gases. The high solubility of gases is attributed to the weak intermolecular interactions in these fluorocarbon fluids.{{cite web |title=Dissolving gases in FLUTEC liquids |publisher=F2 Chemicals Ltd |date=2005-05-10 |url=http://www.f2chemicals.com/pdf/technical/Gas%20solubility.pdf}}

The table shows values for the mole fraction, {{mvar|x}}{{sub|1}}, of nitrogen dissolved, calculated from the Blood–gas partition coefficient, at 298.15 K (25 °C), 0.101325 MPa.{{cite journal |vauthors=Battino R, Rettich TR, Tominaga T |year=1984 |title=The solubility of nitrogen and air in liquids |journal=J. Phys. Chem. Ref. Data |volume=13 |issue=2 |pages=308–319 |doi=10.1063/1.555713 |bibcode=1984JPCRD..13..563B }}

The development of the fluorocarbon industry coincided with World War II.{{cite journal

|author=McBee ET

|title=Fluorine Chemistry

|journal=Ind. Eng. Chem.

|volume=39 |issue=3 |pages=236–237 |date=March 1947 |doi=10.1021/ie50447a002}} Prior to that, fluorocarbons were prepared by reaction of fluorine with the hydrocarbon, i.e., direct fluorination. Because C-C bonds are readily cleaved by fluorine, direct fluorination mainly affords smaller perfluorocarbons, such as tetrafluoromethane, hexafluoroethane, and octafluoropropane.{{Cite encyclopedia |title=Fluorine Compounds, Organic |encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry |date=2000 |doi=10.1002/14356007.a11_349 |isbn=978-3-527-30385-4 |last2=Schwertfeger |first2=Werner |last3=Feiring |first3=Andrew |last4=Smart |first4=Bruce |last5=Behr |first5=Fred |last6=Vogel |first6=Herward |last7=McKusick |first7=Blaine |last1=Siegemund |first1=Günter}}

A major breakthrough that allowed the large scale manufacture of fluorocarbons was the Fowler process. In this process, cobalt trifluoride is used as the source of fluorine. Illustrative is the synthesis of perfluorohexane:

:{{chem2|C6H14 + 28 CoF3 -> C6F14 + 14 HF + 28 CoF2}}

The resulting cobalt difluoride is then regenerated, sometimes in a separate reactor:

:{{chem2|2 CoF2 + F2 -> 2 CoF3}}

Industrially, both steps are combined, for example in the manufacture of the Flutec range of fluorocarbons by F2 chemicals Ltd, using a vertical stirred bed reactor, with hydrocarbon introduced at the bottom, and fluorine introduced halfway up the reactor. The fluorocarbon vapor is recovered from the top.

Electrochemical fluorination (ECF) (also known as the Simons' process) involves electrolysis of a substrate dissolved in hydrogen fluoride. As fluorine is itself manufactured by the electrolysis of hydrogen fluoride, ECF is a rather more direct route to fluorocarbons. The process proceeds at low voltage (5 – 6 V) so that free fluorine is not liberated. The choice of substrate is restricted as ideally it should be soluble in hydrogen fluoride. Ethers and tertiary amines are typically employed. To make perfluorohexane, trihexylamine is used, for example:

:{{chem2|N(C6H13)3 + 45 HF -> 3 C6F14 + NF3 + 42 H2}}

The perfluorinated amine will also be produced:

:{{chem2|N(C6H13)3 + 39 HF -> N(C6F13)3 + 39 H2}}

Fluoroalkanes are generally inert and non-toxic.{{cite web |url=http://www.fluorocarbons.org/chemical-families/pfcs/pfc-toxicological-profile |title=EFCTC - Toxicological profiles of PFCS Perfluorocarbons |access-date=2014-05-19 |url-status=dead |archive-url=https://web.archive.org/web/20150924013903/http://www.fluorocarbons.org/chemical-families/pfcs/pfc-toxicological-profile |archive-date=2015-09-24 }}{{cite web|url=https://www.epa.gov/HPV/pubs/summaries/perfluro/c13244tp.pdf|title=HPV Robust Summaries and Test Plan|url-status=dead|archive-url=https://web.archive.org/web/20121202022600/https://www.epa.gov/HPV/pubs/summaries/perfluro/c13244tp.pdf|publisher=Internet Archive|archive-date=2012-12-02|access-date=2019-01-03}}{{cite journal |author1=Yamanouchi K|author2=Yokoyama K|journal=Proceedings of the XTH International Congress for Nutrition, Kyoto |title=Symposium on Perfluorochemical Artificial Blood |pages=91 |year=1975}}

Fluoroalkanes are not ozone depleting, as they contain no chlorine or bromine atoms, and they are sometimes used as replacements for ozone-depleting chemicals.{{Cite web |url=http://www.expertglossary.com/climate-change/definition/perfluorocarbons-pfcs |title=Perfluorocarbons (PFCS) definition - ExpertGlossary |access-date=2022-12-14 |archive-date=2014-05-19 |archive-url=https://web.archive.org/web/20140519132431/http://www.expertglossary.com/climate-change/definition/perfluorocarbons-pfcs |url-status=dead }}

The term fluorocarbon is used rather loosely to include any chemical containing fluorine and carbon, including chlorofluorocarbons, which are ozone depleting.

Perfluoroalkanes used in medical procedures are rapidly excreted from the body, primarily via expiration with the rate of excretion as a function of the vapour pressure; the half-life for octafluoropropane is less than 2 minutes,{{cite journal | author1=Platts DG|author2=Fraser JF|title = Contrast Echocardiography in Critical Care: Echoes of the Future?: A Review of the Role of Microsphere Contrast Echocardiography|journal=Critical Care and Resuscitation |volume=13 |year= 2011 |issue=1 |pages= 44–55 |doi=10.1016/S1441-2772(23)01257-7 |pmid=21355829 }} compared to about a week for perfluorodecalin.{{cite journal |author=Geyer RP |journal=Proc. XTH Intern. Congress for Nutr., Kyoto |title=Symp on Perfluorochemical Artif. Blood |pages=3–19 |year=1975}}

Image:Halogenated gas concentrations 1978-present.png

Low-boiling perfluoroalkanes are potent greenhouse gases, in part due to their very long atmospheric lifetime, and their use is covered by the Kyoto Protocol.{{citation needed|date=May 2017}}{{Cite web|url=http://unfccc.int/kyoto_protocol/items/2830.php|title=Kyoto Protocol|last=Change|first=United Nations Framework Convention on Climate|website=unfccc.int|access-date=2017-09-27}} The global warming potential (compared to that of carbon dioxide) of many gases can be found in the IPCC 5th assessment report,Myhre, G., D. Shindell, F.-M. Bréon, W. Collins, J. Fuglestvedt, J. Huang, D. Koch, J.-F. Lamarque, D. Lee, B. Mendoza, T. Nakajima, A. Robock, G. Stephens, T. Takemura and H. Zhang (2013) [http://www.climatechange2013.org/images/report/WG1AR5_Chapter08_FINAL.pdf "Anthropogenic and Natural Radiative Forcing"] (see Table 8.A.1). In: Climate Change 2013: The Physical Science Basis. Contribution of Working Group I to the Fifth Assessment Report of the Intergovernmental Panel on Climate Change. Stocker, T.F., D. Qin, G.-K. Plattner, M. Tignor, S.K. Allen, J. Boschung, A. Nauels, Y. Xia, V. Bex and P.M. Midgley (eds.). Cambridge University Press, Cambridge, United Kingdom and New York, NY, USA. with an extract below for a few perfluoroalkanes.

The aluminium smelting industry has been a major source of atmospheric perfluorocarbons (tetrafluoromethane and hexafluoroethane especially), produced as by-product of the electrolysis process.{{cite web|url=http://www.aluminum-production.com/anode_effect.html|title=The Anode Effect|website=aluminum-production.com|access-date=2014-05-20|archive-date=2019-02-22|archive-url= https://web.archive.org/web/20190222083751/http://www.aluminum-production.com/anode_effect.html |url-status=dead}} However, the industry has been actively involved in reducing emissions in recent years.{{cite web |url=http://www.climatevision.gov/sectors/aluminum/pdfs/tmsfirst.pdf |title=Perfluorocarbon (PFC) Generation at Primary Aluminum Smelters |access-date=|vauthors = Leber BP, etal|url-status=dead |archive-url=https://web.archive.org/web/20130216164759/http://www.climatevision.gov/sectors/aluminum/pdfs/tmsfirst.pdf |archive-date=2013-02-16 }} climatevision.gov

As they are inert, perfluoroalkanes have essentially no chemical uses, but their physical properties have led to their use in many diverse applications. These include:

• Perfluorocarbon tracer
• Liquid dielectric
• Chemical vapor deposition
• Organic Rankine cycle
• Fluorous biphasic catalysis{{cite web |url=https://chemistry.illinois.edu/system/files/inline-files/Flannigan.pdf |title=Fluorous Biphasic Catalysis |access-date= |first = David J. |last=Flannigan |date = 21 November 2002|website = chemistry.illinois.edu}}
• Cosmetics
• Ski waxes

As well as several medical uses:

• Contrast-enhanced ultrasound
• Oxygen Therapeutics
• Blood substitute
• Liquid breathing
• Eye surgery {{cite journal

|author1=Imamura Y|author2=Minami M|author3=Ueki M|author4=Satoh B|author5=Ikeda T|title=Use of perfluorocarbon liquid during vitrectomy for severe proliferative diabetic retinopathy

|journal=Br J Ophthalmol |volume=87 |issue=5 |pages=563–566 |year=2003 |doi=10.1136/bjo.87.5.563|pmid=12714393|pmc=1771679}}

• Tattoo removal {{cite web |url=http://www.aslms.org/professional/documents/EditorsChoiceLSMFeb45.2.pdf |title=Archived copy |access-date=2014-05-19 |url-status=dead |archive-url=https://web.archive.org/web/20140519154936/http://www.aslms.org/professional/documents/EditorsChoiceLSMFeb45.2.pdf |archive-date=2014-05-19 }}

Unsaturated fluorocarbons are far more reactive than fluoroalkanes. Although difluoroacetylene is unstable (as is typical for related alkynes, see dichloroacetylene), hexafluoro-2-butyne and related fluorinated alkynes are well known.

File:Perfluoroisobutene.svg|Perfluoroisobutene, a reactive and highly toxic fluoroalkene gas

File:Tetrafluoroethylene.svg|Tetrafluoroethylene, an important perfluorinated monomer.

File:Hexafluoropropylene.svg|Hexafluoropropylene, another important perfluoroalkene.

File:Hexafluorobutyne.png|Hexafluoro-2-butyne, a perfluoroalkyne.

Fluoroalkenes polymerize more exothermically than normal alkenes. Unsaturated fluorocarbons have a driving force towards sp³ hybridization due to the electronegative fluorine atoms seeking a greater share of bonding electrons with reduced s character in orbitals. The most famous member of this class is tetrafluoroethylene, which is used to manufacture polytetrafluoroethylene (PTFE), better known under the trade name Teflon.

Fluoroalkenes and fluorinated alkynes are reactive and many are toxic for example perfluoroisobutene.{{Cite web|title=Schedule 2 of Chemical Weapons Convention|url=https://www.opcw.org/chemical-weapons-convention/annexes/annex-chemicals/schedule-2|access-date=2022-01-25|website=OPCW|language=en}}{{cite book |doi=10.1016/B978-008043405-6/50040-2|chapter=Highly-toxic fluorine compounds|title=Fluorine Chemistry at the Millennium|year=2000|last1=Timperley|first1=Christopher M.|pages=499–538|isbn=9780080434056}} To produce polytetrafluoroethylene various fluorinated surfactants are used, in the process known as Emulsion polymerization, and the surfactant included in the polymer can bioaccumulate.

Perfluoroaromatic compounds contain only carbon and fluorine, like other fluorocarbons, but also contain an aromatic ring. The three most important examples are hexafluorobenzene, octafluorotoluene, and octafluoronaphthalene.

File:hexafluorobenzene.svg|Hexafluorobenzene

Perfluoroaromatic compounds can be manufactured via the Fowler process, like fluoroalkanes, but the conditions must be adjusted to prevent full fluorination. They can also be made by heating the corresponding perchloroaromatic compound with potassium fluoride at high temperature (typically 500 °C), during which the chlorine atoms are replaced by fluorine atoms. A third route is defluorination of the fluoroalkane; for example, octafluorotoluene can be made from perfluoromethylcyclohexane by heating to 500 °C with a nickel or iron catalyst.{{cite book |last=Banks|first=RE|date=1970|title=Fluorocarbons and their Derivatives, Second Edition|location=London|publisher=MacDonald & Co. (Publishers) Ltd.|pages=203–207|isbn=978-0-356-02798-2}}

Perfluoroaromatic compounds are relatively volatile for their molecular weight, with melting and boiling points similar to the corresponding aromatic compound, as the table below shows. They have high density and are non-flammable. For the most part, they are colorless liquids. Unlike the perfluoralkanes, they tend to be miscible with common solvents.{{citation needed|date=May 2017}}

• :Category:Fluorocarbons
• Fluorochemical industry
• Hydrofluorocarbon
• Fluorographene
• Perfluorocycloalkene (PFCA)

{{Reflist|2}}

{{Commons category|Perfluorocarbons}}

• [http://www.fluorocarbons.org Fluorocarbons and Sulphur Hexafluoride, proposed by the European Fluorocarbons Technical Committee]
• [http://www.vega.org.uk/video/programme/119 CFCs and Ozone Depletion] Freeview video provided by the Vega Science Trust.
• [https://web.archive.org/web/20070926183553/http://fluoroconsultants.com/db4/00322/fluoroconsultants.com/_download/INTRODUCTIONTOFLUOROPOLYMERS.pdf Introduction to fluoropolymers]
• [http://www.journals.royalsoc.ac.uk/content/9jcptv5dak4nafm2/fulltext.pdf Organofluorine chemistry by Graham Sandford]{{dead link|date=October 2017 |bot=InternetArchiveBot |fix-attempted=yes }}

{{Fluorine compounds}}

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Category:Greenhouse gases