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Fluorine

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Products Intro: Product Name:Fluorine
CAS:7782-41-4
Purity:99.00% Package:100g,500g,1KG,10KG,100KG
Company Name: Henan Tianfu Chemical Co.,Ltd.
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Products Intro: CAS:7782-41-4
Purity:99% Package:500G;1KG;5KG;25KG
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Products Intro: Product Name:Fluorine
CAS:7782-41-4
Company Name: HuBei ZhuoXi Fluorochemical Co., Ltd.,   Gold
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Products Intro: Product Name:Fluorine
CAS:7782-41-4
Purity:99%
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Products Intro: Product Name:Fluorine
CAS:7782-41-4
Purity:99.9+ Package:2KG/5000.00;
Fluorine Basic information
Product Name:Fluorine
Synonyms:Fluoride in Water;Fluoride samples;Fluoride solution;Anti-THRB antibody produced in rabbit;Coagulation factor II;THRB;Anti-THRB (AP2, Cleaved-Arg327) antibody produced in rabbit;FLUORINE
CAS:7782-41-4
MF:F2
MW:38
EINECS:231-954-8
Product Categories:Fluoro;Inorganics;Organic Fluorides
Mol File:7782-41-4.mol
Fluorine Structure
Fluorine Chemical Properties
Melting point -220°C
Boiling point -188°C
density 1.695(15℃)
vapor pressure >760 mmHg at 20 °C
refractive index 1.000195
storage temp. -20°C
form pale yellow gas
OdorStrong ozone-like odor detectable at 0.1 to 0.2 ppm
Water Solubility reacts
Stability:Stable. Extremely strong oxidant which may react violently with combustible materials, including plastics, reducing agents and organic material. Reacts with water to form corrosive acids.
CAS DataBase Reference7782-41-4(CAS DataBase Reference)
NIST Chemistry ReferenceFluorine(7782-41-4)
EPA Substance Registry SystemFluorine(7782-41-4)
Safety Information
Hazard Codes T+,C
Risk Statements 7-26-35
Safety Statements 9-26-36/37/39-45
RIDADR UN 1045/9192
HazardClass 2.3
Hazardous Substances Data7782-41-4(Hazardous Substances Data)
ToxicityLC50 (1 hr) inhalation by rats, mice, guinea pigs: 185, 150, 170 ppm (by vol) (Keplinger, Suissa)
MSDS Information
ProviderLanguage
Fluorine English
Fluorine Usage And Synthesis
Chemical PropertiesFluorine (F) is a chemical element(group VIla, halogens).It is a pale yellow,highly toxic, corrosive, flammable gas. It is a stable, extremely strong oxidant, which may react violently with combustible materials, including plastics, reducing agents, and organic material. It reacts with water to form corrosive acids. Fluorine is very toxic and may be fatal if inhaled. Fluorine reacts violently with many oxidising agents (e.g. perchlorates, peroxides, permanganates, chlorates, nitrates, chlorine, bromine, and fluorine), strong acids (hydrochloric, sulphuric, and nitric), organic compounds, combustible materials like oil and paper, hydrogen, bromine, iodine, and chemically active metals like, potassium, sodium, magnesium, and zinc.
Fluorine is the most electro negative of all elements and the most chemically energetic of all nonmetallic elements. Fluorine is a high-tonnage chemical that is used in production of fluorides, in synthesis of fluorocarbons,and as an oxidizer for rocket fuels. Because of its severe oxidizing characteristics, special permits are required for shipping of fluorine,and all containers,piping,and processing equipment used for fluorine service must be passivated prior to use. Thereafter, they must be designated for exclusive fluorine service.
Chemical PropertiesFluorine is a yellow compressed, gas. Commonly shipped as a cryogenic gas. It has a characteris tic pungent odor; the odor threshold is 0.035 ppm.
HistoryFluorine was finally isolated in 1886 by Moisson. Fluorine occurs chiefly in fluorspar (CaF2) and cryolite (Na2AlF6), and is in topaz and other minerals. It is a member of the halogen family of elements, and is obtained by electrolyzing a solution of potassium hydrogen fluoride in anhydrous hydrogen fluoride in a vessel of metal or transparent fluorspar. Modern commercial production methods are essentially variations on the procedures first used by Moisson. Fluorine is the most electronegative and reactive of all elements. It is a pale yellow, corrosive gas, which reacts with practically all organic and inorganic substances. Finely divided metals, glass, ceramics, carbon, and even water burn in fluorine with a bright flame. Until World War II, there was no commercial production of elemental fluorine. The atom bomb project and nuclear energy applications, however, made it necessary to produce large quantities. Safe handling techniques have now been developed and it is possible at present to transport liquid fluorine by the ton. Fluorine and its compounds are used in producing uranium (from the hexafluoride) and more than 100 commercial fluorochemicals, including many well-known high-temperature plastics. Hydrofluoric acid is extensively used for etching the glass of light bulbs, etc. Fluorochlorohydrocarbons have been extensively used in airconditioning and refrigeration. However, in recent years the U.S. and other countries have been phasing out ozone-depleting substances, such as the fluorochlorohydrocarbons that have been used in these applications. It has been suggested that fluorine might be substituted for hydrogen wherever it occurs in organic compounds, which could lead to an astronomical number of new fluorine compounds. The presence of fluorine as a soluble fluoride in drinking water to the extent of 2 ppm may cause mottled enamel in teeth, when used by children acquiring permanent teeth; in smaller amounts, however, fluorides are said to be beneficial and used in water supplies to prevent dental cavities. Elemental fluorine has been studied as a rocket propellant as it has an exceptionally high specific impulse value. Compounds of fluorine with rare gases have now been confirmed. Fluorides of xenon, radon, and krypton are among those known. Elemental fluorine and the fluoride ion are highly toxic. The free element has a characteristic pungent odor, detectable in concentrations as low as 20 ppb, which is below the safe working level. The recommended maximum allowable concentration for a daily 8-hour time-weighted exposure is 1 ppm. Fluorine is known to have fourteen isotopes.
UsesIn manufacture of UF6 for nuclear power generation, of SF6 for dielectrics, of fluorinating and metal fluoride compounds.
DefinitionNonmetallic halogen element in group 17 of the periodic table. An 9, aw 18.99840, valence of 1, no other stable isotopes, the most electronegative element and most powerful oxidizing agent known.
General DescriptionFluorine is a pale yellow gas with a pungent odor. Fluorine is commonly shipped as a cryogenic liquid. Fluorine is toxic by inhalation and skin absorption. Contact with skin in lower than lethal concentrations causes chemical burns. Fluorine reacts with water to form hydrofluoric acid and oxygen. Fluorine is corrosive to most common materials. Fluorine reacts with most combustible materials to the point that ignition occurs. Under prolonged exposure to fire or intense heat the containers may violently rupture and rocket.
Air & Water ReactionsWater vapor will react combustibly with Fluorine; an explosive reaction occurs between liquid Fluorine and ice, after an intermediate induction period, [NASA SP-3037: 52(1967)]: If liquid air, which has stood for some time is treated with Fluorine, a precipitate is formed which is likely to explode. Explosive material is thought to be Fluorine Hydrate, [Mellor 2:11(1946-1947)].
Reactivity ProfilePropellant; ignites upon contact with alcohols, amines, ammonia, beryllium alkyls, boranes, dicyanogen, hydrazines, hydrocarbons, hydrogen, nitroalkanes, powdered metals, silanes, or thiols [Bretherick, 1979 p.174]; Aluminum powder and iodine in close contact will ignite spontaneously, Fluorine with metals requires added heat for ignition, [NFPA 491M]. Antimony is spontaneously flammable in Fluorine, chlorine, and bromine. With iodine, the reaction produces heat, which can cause flame or even an explosion if the quantities are great enough, [Mellor 9:379(1946-1947)]. The oxides of the alkalis and alkaline earths are vigorously attacked by Fluorine gas with incandescence, [Mellor 2:13(1946-1947)]. Fluorine causes aromatic hydrocarbons and unsaturated alkanes to ignite spontaneously, [Mellor 2, Supp. 1:55(1956)]. Fluorine vigorously reacts with arsenic and arsenic trioxide at ordinary temperatures, [Mellor 9:34(1946-1947)]. Bromine mixed with Fluorine at ordinary temperatures yields bromine trifluoride, with a luminous flame, [Mellor 2:12(1946-1947)]. Calcium silicide burns readily in Fluorine, [Mellor 6:663(1946-1947)]. The carbonates of sodium, lithium, calcium, and lead in contact with Fluorine are decomposed at ordinary temperatures with incandescence, [Mellor 2:13(1946-1947)]. A mixture of Fluorine and carbon disulfide ignites at ordinary temperatures, [Mellor 2:13(1946-1947)]. The reaction between Fluorine and carbon tetrachloride is violent and sometimes explosive, [Mellor 2, Supp. 1, 198(1956)]. The uncontrolled reaction between Fluorine and chlorine dioxide is explosive, [Mellor 2, Supp. 1, 532(1956)]. Fluorine and silver cyanide react with explosive violence at ordinary temperatures, [Mellor 2, Supp. 1:63(1956)]. Fluorine and sodium acetate produce an explosive reaction involving the formation of diacetyl peroxide, [Mellor 2, Supp. 1:56(1956)]. Selenium, silicon, or sulfur ignites in Fluorine gas at ordinary temperatures, [Mellor 2:11-13(1946-1947)]. Each bubble of sulfur dioxide gas led into a container of Fluorine produces an explosion, [Mellor 2:1(1946-1947)]. Fluorine and thallous chloride react violently, melting the product, [Mellor, Supp. 1:63(1956)].
HazardPowerful oxidizing agent; though nonflammable, it reacts violently with a wide range of both organic and inorganic compounds and thus is a dangerous fire and explosion risk in contact with such materials. Toxic by inhalation, extremely strong irritant to
Health HazardPoisonous; may be fatal if inhaled. Vapor extremely irritating. Contact may cause burns to skin and eyes. Chronic absorption may cause osteosclerosis and calcification of ligaments.
Health Hazardreactions; highly irritating and corrosive to the eyes, skin, and mucous membranes. Toxicity The acute toxicity of fluorine is high. Even very low concentrations irritate the respiratory tract, and brief exposure to 50 ppm can be intolerable. High concentrations can cause severe damage to the respiratory system and can result in the delayed onset of pulmonary edema, which may be fatal. Fluorine is highly irritating to the eyes, and high concentrations cause severe injury and can lead to permanent damage and blindness. Fluorine is extremely corrosive to the skin, causing damage similar to second-degree thermal bums. Fluorine is not considered to have adequate warning properties. Chronic toxicity is unlikely to occur due to the corrosive effects of fluorine exposure. Fluorine has not been found to be carcinogenic or to show reproductive or developmental toxicity in humans.
Health HazardThe acute toxicity of fluorine is high. Even very low concentrations irritate the respiratory tract, and brief exposure to 50 ppm can be intolerable. High concentrations can cause severe damage to the respiratory system and can result in the delayed onset of pulmonary edema, which may be fatal. Fluorine is highly irritating to the eyes, and high concentrations cause severe injury and can lead to permanent damage and blindness. Fluorine is extremely corrosive to the skin, causing damage similar to second-degree thermal bums. Fluorine is not considered to have adequate warning properties. Chronic toxicity is unlikely to occur due to the corrosive effects of fluorine exposure. Fluorine has not been found to be carcinogenic or to show reproductive or developmental toxicity in humans.
Fire HazardFluorine is not flammable, but is a very strong oxidizer, reacting vigorously with most oxidizable materials at room temperature, frequently with ignition. Water should not be used to fight fires involving fluorine
Fire HazardFluorine is not flammable, but is a very strong oxidizer, reacting vigorously with most oxidizable materials at room temperature, frequently with ignition. Water should not be used to fight fires involving fluorine.
Fire HazardMay ignite other combustible materials (wood, paper, oil, etc.) Mixture with fuels may explode. Container may explode in heat of fire. Vapor explosion and poison hazard indoors, outdoors, or in sewers. Poisonous gas is produced in fire. Avoid contact with all oxidizable materials, including organic materials. Will react violently with water and most organic materials to produce heat and toxic fumes. Keep gas in tank, avoid exposure to all other materials.
Safety ProfileA poison gas. A skin, eye, and mucous membrane irritant. A most powerful caustic irritant to tissue. Mutation data reported. A very dangerous fire and explosion hazard. A powerful oxidizer. Reacts violently with many materials. with ammonia, cesium fluoride + fluorocarboxylic acids, cesium heptafluoropropoxide, 1or 2 fluoriminoperfluoropropane, graphite, halocarbons (e.g., carbon tetrachloride, chloroform, perfluorocyclobutane, iodo form, 1,2-d~hlorotetrafluoroethane), liquid hydrocarbons (e.g., anthracene, turpentine), hydrogen, hydrogen + oxygen, hydrogen fluoride + seleninyl fluoride + heat, nitric acid, silver cyanide, sulfur dioxide, carbon monoxide, sodium acetate, sodium bromate, stainless steel, water. Reacts to form explosive products with alkanes + oxygen (forms peroxides), cyano guanidine, perchloric acid (forms fluorine perchlorate gas), potassium chlorate (forms fluorine perchlorate gas), potassium hydroxide (forms potassium trioxide). Forms explosive mixtures with acetonitrile + chlorine fluoride, ice. Ignition or violent reaction on contact with acetylene, ceramic materials, covalent halides (e.g., chromyl chloride, phosphorus pentachloride, phosphorus trichloride, phosphorus trifluoride, boron trichloride, silicon tetrachloride), halogens (e.g., bromine, iodine, chlorine + spark or heating to 100°C), dcyanogen, gaseous hydrocarbons (e.g., town gas, methane, benzene), hydrogen halide gases or concentrated solutions (e.g., hydrogen bromide, hydrogen chloride, hydrogen iodide, hydrogen fluoride), metal acetylides and carbides (e.g., monocesium acetylide, cesium acetylide, lithium acetylide, rubidium acetylide, tungsten carbide, ditungsten carbide, zirconium dicarbide, uranium dicarbide), metal cyano complexes [e.g., potassium hexacyanoferrate(II), lead hexacyanoferrate(lII), potassium hexa cyanoferrate(III)], metal hydrides (e.g., copper hydride, potassium hydride, sodum hydride), metal iodides (e.g., lead iodide, calcium iodde, mercury iodide, potassium iodde), metals, metal salts, metal shcides (e.g., calcium disihcide, lithium hexasilicide), nickel(IV) oxide, nonmetals (e.g., boron, yellow or red phosphorus, selenium, tellurium, sdicon, carbon, charcoal, sulfur), oxygenated organic compounds (e.g., methanol, ethanol, 3-methyl butanol, acetaldehyde, trichloroacetaldehyde, acetone, lactic acid, benzoic acid, salicylic acid, ethyl acetate, methyl borate), nonmetal oxides (e.g., arsenic trioxide, nitrogen oxide, dinitrogen tetroxide), oxygen + polymers [e.g., phenol-formaldehyde resins (bakelite), polpacrylonitrile-butadiene (Buna N), polyamides (nylons), polychloropene (neoprene), polyethylene, polytrifluoroprop ylmethylsiloxane, poljrvin~7lchloride-vinyl acetate (Tygon), poljrvinylidene fluoride-hexafluoropropylene (Won), polyurethane foam, polymethyl methacrylate (Perspex), polytetrafluooethylene (Teflon)], sulfides (e.g., antimony trisulfide, carbon disulfide vapor, chromium (II) sulfide, hydrogen sulfide, barium sulfide, potassium sulfide, zinc sulfide, molybdenum sulfide), xenon + catalysts (e.g., nickel fluoride, silver difluoride, nickel(IⅡ) oxide, silver (I) oxide). Incandescent reaction with boron nitride, hexalithium dshcide + heat, metal borides, metal oxides (e.g., nickel(Ⅱ) oxide, alkali metal oxides, alkaline earth oxides), nitrogenous bases (e.g., aniline, dmethylamine, pyridne), gahc acid. Incompatible with cesium heptafluoro propoxide, cyanoguanid~ne, halocarbons,hexalithmm dishcide, seleninyl fluoride, hydrogen sulfide, oxygen, sodium acetate, sodium bromate, sodium dicyanamides, most organic matter, H-containing molecules, oxides of S, N, P, alkali metals,and alkaline earths. It reacts violently with halogen acids, hydrazine, ClO2, coke, cyanamide, cyanides, KNO3, (PbO + glycerol), CCl4, shcides, skates, trinitromethane, alkenes, alkyl benzenes, CS2, Cr(OCl)2, Al, T1, Sn, Sb, As, natural gas, liquid air, perfluoropropionyl fluoride, polyvinyl chloride acetate. Many reactions go on even at <-160°. Reacts with water or steam to produce heat and toxic and corrosive fumes. Used as one component of liquid rocket fuel and in chemical lasers. See also FLUORIDES.
Potential ExposureElemental fluorine is used in the con version of uranium tetrafluoride to uranium hexafluoride; in the synthesis of organic and inorganic fluorine com pounds; and as an oxidizer in rocket fuel.
First aidIf this chemical gets into the eyes, remove any contact lenses at once and irrigate immediately for at least 15 minutes, occasionally lifting upper and lower lids. Seek medical attention immediately. If this chemical contacts the skin, remove contaminated clothing and wash immediately with soap and water. Seek medical attention immediately. If this chemical has been inhaled, remove from exposure, begin rescue breathing (using universal precautions, includ ing resuscitation mask) if breathing has stopped and CPR if heart action has stopped. Transfer promptly to a medical facility. When this chemical has been swallowed, get medi cal attention. Give large quantities of water and induce vomiting. Do not make an unconscious person vomit. If frostbite has occurred, seek medical attention immediately; do NOT rub the affected areas or flush them with water. In order to prevent further tissue damage, do NOT attempt to remove frozen clothing from frostbitten areas. If frostbite has NOT occurred, immediately and thoroughly wash con taminated skin with soap and water.
storageWork with fluorine requires special precautions and protective equipment and should be carried out only by specially trained personnel. Fluorine will react with many materials normally recommended for handling compressed gases.
ShippingUN1045 Fluorine, compressed, Hazard Class: 2.3; Labels: 2.3-Poisonous gas, 5.1-Oxidizer, 8-Corrosive material, Inhalation Hazard Zone A. Cylinders must be transported in a secure upright position, in a well-ventilated truck. Protect cylinder and labels from physical damage. The owner of the compressed gas cylinder is the only entity allowed by federal law (49CFR) to transport and refill them. It is a violation of transportation regulations to refill compressed gas cylinders without the express written per mission of the owner.
Purification MethodsPass the gas through a bed of NaF at 100o to remove HF and SiF4. [For description of stills used in fractional distillation, see Greenberg et al. J Phys Chem 65 1168 1961; Stein et al. Purification of Fluorine by Distillation, Argonne National Laboratory, ANL-6364 1961 (from Office of Technical Services, US Dept of Commerce, Washington 25).] HIGHLY TOXIC.
IncompatibilitiesFluorine is an extremely powerful oxi dizing gas. Keep away from heat, water, nitric acid, oxidi zers, organic compounds. Containers may explode if heated. Reacts violently with reducing agents; ammonia, all combustible materials, metals (except the metal containers in which it is shipped). Reacts violently with H2O to form hydrofluoric acid, oxygen and ozone. The most potent oxidizer.
Flammability and ExplosibilityFluorine is not flammable, but is a very strong oxidizer, reacting vigorously with most oxidizable materials at room temperature, frequently with ignition. Water should not be used to fight fires involving fluorine.
Waste DisposalReturn refillable compressed gas cylinders to supplier. Fluorine may be combusted by means of a fluorine-hydrocarbon air burner followed by a caustic scrubber and stack. Consult with environmental regulatory agencies for guidance on acceptable disposal practices. Generators of waste containing this contaminant (≥100 kg/mo) must conform with EPA regulations gov erning storage, transportation, treatment, and waste disposal.
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