Fluorine

Base Information

• Chemical Name: Fluorine
• CAS No.: 7782-41-4
• Deprecated CAS: 28077-97-6,719993-31-4,719993-31-4
• Molecular Formula: F2
• Molecular Weight: 37.9968
• Hs Code.: 2801301000
• European Community (EC) Number: 231-954-8
• ICSC Number: 0046
• UN Number: 1045,9192
• UNII: 284SYP0193
• DSSTox Substance ID: DTXSID3024106
• Nikkaji Number: J95.227C
• Wikipedia: Fluorine
• Wikidata: Q1963030
• NCI Thesaurus Code: C502
• Mol file: 7782-41-4.mol

Synonyms:Fluorine;Fluorine 19;Fluorine-19

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Chemical Property of Fluorine

Chemical Property:

• Appearance/Colour: pale yellow gas with a pungent odour
• Vapor Pressure: >760 mmHg at 20 °C
• Melting Point: -220 °C
• Refractive Index: 1.000195
• Boiling Point: -188 °C
• PSA: 0.00000
• Density: 0.963 g/cm³
• LogP: 0.84040
• Storage Temp.: -20°C
• Water Solubility.: reacts
• XLogP3: 1.1
• Hydrogen Bond Donor Count: 0
• Hydrogen Bond Acceptor Count: 2
• Rotatable Bond Count: 0
• Exact Mass: 37.99680632
• Heavy Atom Count: 2
• Complexity: 0
• Transport DOT Label: Poison Gas Oxidizer Corrosive

Purity/Quality:

Safty Information:

• Pictogram(s): C,T+
• Hazard Codes: T+,C
• Statements: 7-26-35
• Safety Statements: 9-26-36/37/39-45

MSDS Files:

SDS file from LookChem

Total 1 MSDS from other Authors

Useful:

• Chemical Classes: Toxic Gases & Vapors -> Oxidizers
• Canonical SMILES: FF
• Recent ClinicalTrials: Pre-procedural Mouthwash in Reducing Bacteria in Dental Aerosols
• Recent EU Clinical Trials: A Phase 3, Randomized, Double-blind Study to Evaluate the Safety and Efficacy of Emtricitabine and Tenofovir Alafenamide (F/TAF) Fixed-Dose Combination Once Daily for Pre-Exposure Prophylaxis in Men and Transgender Women Who Have Sex with Men and Are At Risk of HIV-1 Infection
• Recent NIPH Clinical Trials: The randomized controlled trial for the prevention of root caries.
• Inhalation Risk: A harmful concentration of this gas in the air will be reached very quickly on loss of containment.
• Effects of Short Term Exposure: The substance is very corrosive to the eyes, skin and respiratory tract. Inhalation of this gas may cause lung oedema. The liquid may cause frostbite. The effects may be delayed. Medical observation is indicated.
• Description: Fluorine is a highly toxic, pale yellow gas about 1.3 times as heavy as air at atmospheric temperature and pressure. When cooled below its boiling point (-306.8°F or -188.2°C), it is a liquid about 1.5 times as dense as water.
• Physical properties: Fluorine does not occur in a free state in nature, and because fluorine is one of the mostreactive elements, no chemical can free it from any of its many compounds. The reason forthis is that fluorine atoms are the smallest of the halogens, meaning the electron donated by ametal (or some nonmetals) are closer to fluorine’s nucleus and thus exert a great force betweenthe fluorine nuclei and the elements giving up one electron. The positive nuclei of fluorinehave a strong tendency to gain electrons to complete the outer shell, which makes it a strongoxidizer.Because the fluorine atom has only nine electrons, which are close to the nucleus, thepositive nucleus has a strong tendency to gain electrons to complete its outer shell. As a gasits density (specific gravity) is 1.695, and as a liquid, its density is 1.108. Its freezing point is–219.61°C, and its boiling point is –188°C. Fluorine, as a diatomic gas molecule (F2), is paleyellow in color. Fluorine is the most electronegative nonmetallic element known (wants togain electrons) and is, therefore, the strongest oxidizing agent known.
• Uses: In manufacture of UF6 for nuclear power generation, of SF6 for dielectrics, of fluorinating and metal fluoride compounds. Probably the most common use of fluorine is its addition to municipal water supplies tohelp prevent tooth decay. Stannous (II) fluoride (SnF2) is added to the water in proportionsof about one part per million (1 ppm). In addition, many brands of toothpaste add stannousfluoride or other fluoride compounds to their product to help prevent tooth decay. Toothenamel degenerates overtime. Fluorine promotes remineralization, essentially making a formof new enamel called “fluorapatite,” which is resistant to decay.Another popular use for the element fluorine is the plastic called Teflon. This is a fluoropolymerconsisting of long chainlike inert molecules of carbon linked chemically to fluorine.Teflon is useful as a coating for nonstick surfaces in cookware, ironing board covers, razorblades, and so forth.Of great importance are the inert fluorocarbons, such as dichlorodifluoromethane (CF2Cl2)and chlorofluorocarbon compounds (CFCs) and their usage as gas propellants in spray cans(e.g., hair spray, deodorants, and paint). They are also used as coolants in air conditioning andrefrigeration (freon). The use of fluorinated carbon gases, known as fluorocarbons, in aerosolcans and refrigerants has been banned in the United States since 1978 because these gases diffuseinto the upper atmosphere and react to destroy the ozone gases found in the ozone layer.A reduced ozonosphere layer allows more ultraviolet radiation to filter to the Earth’s surface.Excessive strong ultraviolet radiation from the sun can be harmful to both plants and animals.The ozone layer filters out most of the harmful ultraviolet radiation.When hydrogen and fluorine gases meet, they explode spontaneously and form hydrogenfluoride (HF), which, when dissolved in water, becomes hydrofluoric acid that is strongenough to dissolve glass. It is used to etch glass and to produce “frosted” light bulbs.The artificial radioactive fluorine isotope F-18 emits positrons (positive electrons) that,when injected into the body, interact with regular negative electrons, and they annihilate each other, producing X-ray-like radiation. This medical procedure is performed in PositronEmission Topography (PET), in which the produced radiation generates a picture of the bodypart being examined. Since F-18 has a short half-life of about 110 minutes, there is littlechance of radiation damage to the patient.Fluorine compounds are also used to reduce the viscosity of molten metals and slag byproductsso that they will flow more easily. In addition, fluorine is a component of therapeuticchemotherapy drugs used to treat a number of different types of cancer. Fluorine is used in the manufacture of vari ous fluorocarbons and fluorides, as a rocketpropellant, and in many inorganic and or ganic syntheses.

Technology Process of Fluorine

There total 181 articles about Fluorine which guide to synthetic route it. The literature collected by LookChem mainly comes from the sharing of users and the free literature resources found by Internet computing technology. We keep the original model of the professional version of literature to make it easier and faster for users to retrieve and use. At the same time, we analyze and calculate the most feasible synthesis route with the highest yield for your reference as below:

synthetic route:

Reference yield: 98.8%

uranium hexafluoride (7783-81-5) → uranium pentafluoride (13775-07-0) + fluorine (7782-41-4)

Guidance literature:

In gas; Irradiation (UV/VIS); photolysis by UV light at room temp.;

Reference yield: 92.1%

calcium fluoride + water (7732-18-5) → fluorine (7782-41-4)

Guidance literature:

In neat (no solvent); passing over 1.0 g/min water-steam in 120 ml air at 1300°C for 30 minutes;;

Reference yield: 75.0%

bismuth pentafluoride (7787-62-4) + K2NiF6 (17218-47-2) → fluorine (7782-41-4)

Guidance literature:

In solid; 1 equiv of K2NiF6 and ca. 3 equiv of BiF5 were premixed at ambient temp., F2 evolution started when the mixt. heated to about 60-70°C, peak pressure 990 Torr;

upstream raw materials:

bismuth pentafluoride

Cs₂CuF₆

Cs₂MnF₆

K₂NiF₆

Downstream raw materials:

caesium tetrafluoroborate

Carbonyl fluoride

difluoroether

iodine pentafluoride

Refernces

• 1、 Henne, A. L.. "". . p. 96 - 97. Retrieved 1938.
• 2、 Miller, W. T.,Bigelow, L. A.. "". . p. 1585 - 1589. Retrieved 1936.
• 3、 Dennis, L. M.,Veeder, J. M.,Rochov, E. G.. "". . p. 3263 - 3269. Retrieved 1931.
• 4、 Suchard, S. N.,Gross, R. W. F.,Whittier, J. S.. "". . p. 411 - 413. Retrieved 1971.
• 5、 Leskiv,Abramov,Oleinik,Kepman,Sukhoverkhov,Mazej,Rau,Chilingarov,Sidorov. "Vaporization products of transition-metal and rare-earth complex fluorides studied by high-temperature mass spectrometry". . p. 1327 - 1333. Retrieved 2008/10/09.