7782-41-4

Usage

Uses

Used in Nuclear Power Generation:
Fluorine is used in the manufacture of UF6, which is utilized in nuclear power generation.
Used in Dielectrics:
Fluorine is used in the production of SF6, a gas that serves as a dielectric in electrical applications.
Used in Fluorinating and Metal Fluoride Compounds:
Fluorine is employed in the creation of fluorinating agents and metal fluoride compounds.
Used in Water Treatment:
Fluorine is added to municipal water supplies as stannous (II) fluoride (SnF2) to help prevent tooth decay. It promotes remineralization, creating a form of new enamel called "fluorapatite," which is resistant to decay.
Used in Dental Care:
Many brands of toothpaste include stannous fluoride or other fluoride compounds to prevent tooth decay.
Used in Plastics:
Fluorine is a component of Teflon, a fluoropolymer consisting of long chain-like inert molecules of carbon linked chemically to fluorine. Teflon is used as a coating for nonstick surfaces in cookware, ironing board covers, razor blades, and more.
Used in Gas Propellants:
Fluorine is present in inert fluorocarbons, such as dichlorodifluoromethane (CF2Cl2) and chlorofluorocarbon compounds (CFCs), which are used as gas propellants in spray cans (e.g., hair spray, deodorants, and paint) and as coolants in air conditioning and refrigeration (freon).
Used in Medical Imaging:
The artificial radioactive fluorine isotope F-18 is used in Positron Emission Tomography (PET), a medical procedure that generates images of the body part being examined. F-18 emits positrons that interact with regular negative electrons, producing X-ray-like radiation.
Used in Glass Etching:
Fluorine reacts with hydrogen to form hydrogen fluoride (HF), which, when dissolved in water, becomes hydrofluoric acid. This acid is strong enough to dissolve glass and is used to etch glass and produce "frosted" light bulbs.
Used in Metal Processing:
Fluorine compounds are used to reduce the viscosity of molten metals and slag byproducts, allowing them to flow more easily.
Used in Cancer Treatment:
Fluorine is a component of therapeutic chemotherapy drugs used to treat various types of cancer.
Used in Chemical Synthesis:
Fluorine is utilized in the manufacture of various fluorocarbons and fluorides, as a rocket propellant, and in many inorganic and organic syntheses.

Isotopes

There are a total of 16 isotopes of fluorine. Only one, F-19, is stable. It makesup 100% of the fluorine found on Earth. All the others are radioactive with half-livesranging from 2.5 milliseconds to 4.57100×10-22 years.

Origin of Name

From the Latin and French words for “flow,” fluere.

Characteristics

Fluorine reacts violently with hydrogen compounds, including water and ammonia. It alsoreacts with metals, such as aluminum, zinc, and magnesium, sometimes bursting into flames,and with all organic compounds, in some cases resulting in such complex fluoride compoundsas fluorocarbon molecules. It is an extremely active, gaseous element that combines spontaneouslyand explosively with hydrogen, producing hydrogen fluoride acid (HF), which is usedto etch glass. It reacts with most metals except helium, neon, and argon. It forms many differenttypes of “salts” when combining with a variety of metals. Fluorine, as a diatomic gas,is extremely poisonous and irritating to the skin and lungs, as are many fluoride compounds.Fluorine and its compounds are also corrosive.

History

Fluorine 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.

Air & Water Reactions

Water 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 Profile

Propellant; 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)].

Hazard

Powerful 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

Hazard

Many of the fluorine compounds, such as CFCs, are inert and nontoxic to humans. Butmany other types of compounds, particularly the salts and acids of fluorine, are very toxicwhen either inhaled or ingested. They are also strong irritants to the skin.There is also danger of fire and explosion when fluorine combines with several elementsand organic compounds.Poisonous fluoride salts are not toxic to the human body at the very low concentrationlevels used in drinking water and toothpaste to prevent dental decay.

Health Hazard

Fluorine is a severe irritant to the eyes, skin,and mucous membranes. In humans its irri tant effect on the eyes can be felt at a level of5 ppm in air. The acute toxicity of fluorine was found to be moderate in animals. Expo sure to this gas can cause respiratory distressand pulmonary edema. Chronic exposure canproduce mottled enamel of the teeth, calcifi-cation of ligaments, and injury to the lungs,liver, and kidney. The latter effects, however,were observed in animals at high concentra tions. The LC50 value in mice is 150 ppm foran exposure period of 1 hour. Human toxic ity data on fluorine are very limited.

Health Hazard

Poisonous; 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 Hazard

reactions; 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 Hazard

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.

Fire Hazard

May 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.

Fire Hazard

Fluorine 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

Flammability and Explosibility

Fluorine 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.

Safety Profile

A 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 Exposure

Elemental 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.

Physiological effects

Fluorine gas is a powerful corrosive irritant and is highly toxic [I]. In one series of animal experiments, inhalation of acute exposures of 10 000 ppm for 5 minutes, 1000 ppm for 30 minutes, and 500 ppm for I hour produced 100 percent mortality in rats, mice, guinea pigs, and rabbits. Inhalation of 100 ppm for 7 hours produced wide variation in species mortality, ranging from 0 percent in guinea pigs to 96 percent in mice.

Environmental Fate

Fluorine remains persistent in the environment. In water, fluorides attach to aluminum in freshwater and calcium and magnesium in seawater and settle into the sediment. Fluorides may be taken up from soil and accumulate in plants or they may be deposited on the upper parts of the plants. The amount of fluoride taken up by plants depends on the type of plant, the nature of the soil, and the amount and form of fluoride in the soil. Levels of fluorides in surface water average about 0.2 ppm, while well water levels range from 0.02 to 1.5 ppm. The 15 000 water systems serving about 162 million people in the USA are fluoridated in the range of 0.7–1.2 ppm.

storage

Work 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.

Shipping

UN1045 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 Methods

Pass 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.

Toxicity evaluation

Fluorine-containing compounds are diverse and the specifics of toxicity depend upon their reactivity, structure, and ability to release fluoride ions. Ingested fluoride initially acts locally on the intestinal mucosa, where it forms hydrofluoric acid. Once released, fluoride ions combined with blood calcium forming calcium fluoride producing hypocalcemia. Fluoride at high doses can stimulate osteoblasts and inhibit osteoclasts. Inorganic fluoride inhibits enzymes requiring metal ion cofactors which inhibit ATP production in the mitochondrial electron transport chain system of the cell. Although the exact mechanism of dental fluorosis is unknown, it is generally believed to be due to a fluorideinduced delay in the hydrolysis and removal of the enamel amelogenin matrix proteins during enamel maturation and subsequent effects on crystal growth. In one proposed mechanism, fluoride indirectly inhibits amelogeninase, a calciumdependent metalloenzyme, by binding to calcium thereby decreasing the calcium availability and the activation of amelogeninases.

Incompatibilities

Fluorine 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.

Waste Disposal

Return 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.

GRADES AVAILABLE

Fluorine is available at a minimum purity of 97 percent.

InChI:InChI=1/F

Synthetic route

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

Conditions	Yield
In gas Irradiation (UV/VIS); photolysis by UV light at room temp.;	A 98.8% B n/a
In neat (no solvent, gas phase) Irradiation (UV/VIS); photolysis by UV light at room temp.;	A 98.8% B n/a
In gas Irradiation (UV/VIS); photolysis at 1-10 Torr; nearly complete decompn. within some h;
In neat (no solvent, gas phase) Irradiation (UV/VIS); photolysis at 1-10 Torr; nearly complete decompn. within some h;

KH2F3 → fluorine (7782-41-4)

Conditions	Yield
In neat (no solvent) Electrolysis; melt of KH2F3; passing through column with granuled NaF;	95%

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

Conditions	Yield
In neat (no solvent) passing over 1.0 g/min water-steam in 120 ml air at 1300°C for 30 minutes;;	92.1%
In neat (no solvent) passing over 1.0 g/min water-steam in 120 ml air at 1300°C for 30 minutes;;	92.1%
With silica gel In neat (no solvent) passing 1.0 g/min water-steam in 120 ml air over a mixture of 2.38 g CaF2 and 2.62 g SiO2 at 1300°C for 30 minutes;;	90.5%

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

Conditions	Yield
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;	75%

calcium fluoride → fluorine (7782-41-4)

Conditions	Yield
With silica gel In neat (no solvent) passing dry air over a mixture of 2.38 g CaF2 and 2.62 g SiO2 at 1300°C for 30 minutes;;	52.9%
With SiO2 In neat (no solvent) passing dry air over a mixture of 2.38 g CaF2 and 2.62 g SiO2 at 1300°C for 30 minutes;;	52.9%
With silica gel In neat (no solvent) passing dry air over a mixture of 2.38 g CaF2 and 2.62 g SiO2 at 1200°C for 30 minutes;;	12.2%

bismuth pentafluoride (7787-62-4) + Cs2CuF6 (43070-30-0) → fluorine (7782-41-4)

Conditions	Yield
In solid 1 equiv of Cs2CuF6 and ca. 2 equiv of BiF5 were premixed at ambient temp., F2 evolution started when the mixt. heated to about 60-70°C, peak pressure 836 Torr;	46%

bismuth pentafluoride (7787-62-4) + K2NiF6 (17218-47-2) + titanium(IV) fluoride (7783-63-3) → fluorine (7782-41-4)

Conditions	Yield
In solid equimolar amts. of reactants were premixed at ambient temp., F2 evolution started when the mixt. heated to about 60-70°C, peak pressure 820 Torr;	45%

bismuth pentafluoride (7787-62-4) + Cs2MnF6 (16962-46-2) → fluorine (7782-41-4)

Conditions	Yield
In solid 1 equiv of Cs2MnF6 and 3 equiv of BiF5 were premixed at ambient temp., F2 evolution started when the mixt. heated to about 60-70°C, peak pressure 929 Torr;	41%

K2NiF6 (17218-47-2) + titanium(IV) fluoride (7783-63-3) → fluorine (7782-41-4)

Conditions	Yield
In solid equimolar amts. of reactants were premixed at ambient temp., F2 evolution started when the mixt. heated to about 60-70°C, peak pressure 810 Torr;	14%

cesium hydrogen fluoride → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis;
In melt Electrolysis;

KF*1.6HF + lithium fluoride → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; electrolysis of KF*1.6HF with 0.1-2,5% LiF at 100-110°C; current density: 0.097A/cm*cm; C-anode with 35-47% Cu, steel cathode;;

KF*3HF → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; KF*3HF (m.p.: 0-150°C); electrode: Fe, Ni, Cu or alloys of these metals; copper diaphragma;;
In melt Electrolysis; electrolysis of KF*3HF; open or closed system; crucible of Cu; various cathode and anode; with or without diaphragma; various temp.;;
In melt Electrolysis;

KF*1.8HF → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; closed crucible (cathode) and diaphragma of copper;;
In melt Electrolysis; closed crucible (cathode) and diaphragma of copper;;
In melt Electrolysis; electrolysis of KF*1.8HF in a closed crucible (cathode) of Cu at 160-250°C, 20 A and 8.5-9 V ; diaphragma of copper; graphite anode; current efficiency: 92-94%;;

KF*2HF → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; electrolysis of KF*2HF in a crucible (cathode) of monel metal at 73-75°C and 12 A; diaphragma of copper; Ni anode; current efficiency: 72%; sealed with Portland cement;;
In melt Electrolysis; electrolysis of KF*2HF in a crucible (cathode) of monel metal at 73-75°C and 12 A; diaphragma of copper; Ni anode; current efficiency: 72%; sealed with Portland cement;;

KF*2HF + sodium fluoride + lithium fluoride → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; electrolysis of KF*2HF with 1% LiF and 2% NaF at 100°C, 300 A and 11 V; coal anode, steel cathode;;

potassium hydrogenfluoride (1279123-63-5) → fluorine (7782-41-4)

Conditions	Yield
In hydrogen fluoride Electrochem. Process; laboratory fluorine cell (40 -42 % HF, 100 A, 80 - 100°C); passing through column with granulated NaF;
In melt Electrolysis; graphite anode; description and drawing of apparatus given;;
In melt Electrolysis; graphite anode; description and drawing of apparatus given;;

potassium hydrogenfluoride (1279123-63-5) + hydrogen fluoride (7664-39-3) → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; KHF2 presaturated with HF (40 - 42 wt. %); adsorption on column packed with NaF pellets;

KF*(2.9-6.7)HF → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; electrolysis of KF*(2.9-6.7)HF at 15-50°C; various material for vessel, cathode and anode;;
In melt Electrolysis;
In melt Electrolysis;

KF*(1.8-2.2)HF → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; at 80-110°C;;

rubidium hydrogenfluoride → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis;

potassium hydrogen bifluoride + sodium hydrogenfluoride → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; electrolysis of a mixt. of KF*HF (65%) and NaF*HF (35%); vessel and diaphragma of Mg or Monel metal;;
In melt Electrolysis; electrolysis of a mixt. of KF*HF (65%) and NaF*HF (35%); vessel and diaphragma of Mg or Monel metal;;
In melt Electrolysis; electrolysis of a mixt. of KF*HF (65%) and NaF*HF (35%); vessel and diaphragma of Mg or Monel metal;;

hydrogen fluoride (7664-39-3) + water (7732-18-5) → fluorine (7782-41-4) + ozone (10028-15-6)

Conditions	Yield
In water Electrolysis; reaction by use of aq. HF solns., mechanism discussed;;
In water Electrolysis; reaction by use of aq. HF solns., mechanism discussed;;

(x)FH*(x)FK → fluorine (7782-41-4)

Conditions	Yield
In melt byproducts: H2; Electrolysis; anode: 40% anthracite and 60% coke pressed at 1250-1300°C and 300-400 at; 70-85°C; 2000 A; pilot plant;;
In melt Electrolysis;
In melt Electrolysis;

rubidium fluoride → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; electrolysis of RbF; hollow C-anode (permeable to gas); current density: 0.0775 A/cm*cm; Cu-cathode;;

potassium fluoride → fluorine (7782-41-4)

Conditions	Yield
In melt Electrolysis; electrolysis of KF; hollow C-anode (permeable to gas); current density: 0.0775 A/cm*cm; Cu-cathode;;

potassium fluoride + hydrogen fluoride (7664-39-3) → fluorine (7782-41-4)

Conditions	Yield
In hydrogen fluoride Electrolysis; electrolysis of non-aq. HF and KF at -30 to -40°C;;
In hydrogen fluoride HF (liquid); Electrolysis; electrolysis of non-aq. HF and KF at -30 to -40°C;;

sodium fluoride → fluorine (7782-41-4)

Conditions	Yield
With oxygen In neat (no solvent) byproducts: Na4P2O7; heating of a mixt. of NaF and Na2P2O6 at 650-750°C in air;;
With Na2P2O6; O2 In neat (no solvent) byproducts: Na4P2O7; heating of a mixt. of NaF and Na2P2O6 at 650-750°C in air;;

sodium pyrophosphate (124-43-6) + sodium fluoride → fluorine (7782-41-4) + sodium phosphate

Conditions	Yield
With oxygen

hydrogen fluoride (7664-39-3) + sodium fluoride → fluorine (7782-41-4)

Conditions	Yield
In hydrogen fluoride byproducts: H2; HF (liquid); Electrolysis; photoelectrolysis of anhydrous HF/NaF at a TiO(2-x)F(x) or n-TiO(2-x) electrode under 365 nm illumination or in the dark;; F2 identified by volatility at -196 °C, IR inactivity, MS and chemical behaviour;;

sodium metaphposphate + sodium fluoride → sodium pyrophosphate (124-43-6) + fluorine (7782-41-4)

Conditions	Yield
With oxygen

fluorine (7782-41-4) + tin(IV) oxide → tin(IV) fluoride (7783-62-2)

Conditions	Yield
In neat (no solvent) formation at fluorination of SnO2 with F2 at 500-550°C;;	100%
In neat (no solvent) formation at fluorination of SnO2 with F2 at 400°C;;	80%
In neat (no solvent) reaction with fluorine at 500-550°C under formation of SnF4;;
In neat (no solvent) reaction with fluorine at 500-550°C under formation of SnF4;;

tantalum + niobium + fluorine (7782-41-4) → [Nb2Ta2F20]

Conditions	Yield
In neat (no solvent) High Pressure; all manipulations in metal vac. line; mixt. of calcd. amts. of metal powders reacted with 10% excess of F2 gas at 393 K for 3 h in steel autoclave, cooled to room temp.; excess F2 removed in dynamic vac., crystalline product scraped from upper surfaces of autoclave; elem. anal.;	100%

tantalum + niobium + fluorine (7782-41-4) → [NbTa3F20] (900794-96-9)

Conditions	Yield
In neat (no solvent) High Pressure; all manipulations in metal vac. line; mixt. of calcd. amts. of metal powders reacted with 10% excess of F2 gas at 393 K for 3 h in steel autoclave, cooled to room temp.; excess F2 removed in dynamic vac., crystalline product scraped from upper surfaces of autoclave; elem. anal.;	100%

tantalum + niobium + fluorine (7782-41-4) → [Nb3TaF20] (900794-98-1)

Conditions	Yield
In neat (no solvent) High Pressure; all manipulations in metal vac. line; mixt. of calcd. amts. of metal powders reacted with 10% excess of F2 gas at 393 K for 3 h in steel autoclave, cooled to room temp.; excess F2 removed in dynamic vac., crystalline product scraped from upper surfaces of autoclave; elem. anal.;	100%

chromium(III) fluoride (7788-97-8) + fluorine (7782-41-4) → chromium pentafluoride (14884-42-5)

Conditions	Yield
In neat (no solvent) anhydrous CrF3 and F2 shaked for 29 h at 270-303 ° C; remaining F2 removed at -196 ° C;	100%
addn. of F2 to CrF3 at -196°C, then 260°C for 65 h;	92.5%
In neat (no solvent) High Pressure; CrF3 was loaded into a Monel autoclave in a dry-box; after evacuation F2 was admitted (30 atm); heating at 350°C for 2 h;; cooling to room temp.; autoclave was evacuated to 1E-1 torr for severalhours and subsequently opened in a dry-box; elem. anal.;;

tantalum + fluorine (7782-41-4) → tantalum pentafluoride

Conditions	Yield
In neat (no solvent) High Pressure; all manipulations in metal vac. line; metal powder reacted with 10% excess of F2 gas at 393 K for 3 h in steel autoclave, cooled to room temp.; excess F2 removed in dynamic vac., crystalline product scraped from upper surfaces of autoclave; elem. anal.;	100%

ammonium hexachloridoplatinate(IV) + fluorine (7782-41-4) + sodium chloride (7647-14-5) → sodium hexafluoridoplatinate(IV)

Conditions	Yield
at 450℃; for 144h; Inert atmosphere; Milling;	100%

bismuth pentafluoride (7787-62-4) + hydrogen fluoride (7664-39-3) + silver fluoride + fluorine (7782-41-4) → Ag(2+)*2BiF6(1-)=Ag(BiF6)2

Conditions	Yield
In hydrogen fluoride HF (liquid); dry Ar-atmosphere; metal reactor lined with fluorinated plastic, prepassivated with F2; 2 atm F2,(pptn. of AgF2 in one part), mechanical transfer of excess BiF5 onto AgF2, stirring (15 h); evapn., repeated treatment with BF3 (dissoln. of AgF2) and decantation,drying (dynamic vac.);	99.7%

xenon + fluorine (7782-41-4) → xenon difluoride (13709-36-9)

Conditions	Yield
In neat (no solvent) Xe and F2 condensed into nickel can (-196°C), warmed (room temp., pressure 34 atm.), preheated electric furnace (400°C) placed around the nickel can (7 h, pressure 78 atm.), quenched to room temp. in water, cooled (-78°C); excess Xe condensed into a storage cylinder (-196°C), evapn. (through a cold trap, -78°C);	99.3%
In gas react. temp. of 400°C, Xe:F2 about 2.0, Monel vessel with volume between 95 and 1200 ml; cooling down with H2O;;	>95
Electric Arc; react. of F2 with an excess of Xe in an electrical discharge; sublimation in vac., discarding the leading fraction;

chlorine (7782-50-5) + fluorine (7782-41-4) → chlorine monofluoride (7790-89-8)

Conditions	Yield
In gas byproducts: ClO2, ClF3; Irradiation (UV/VIS); pulsed irradiation of gaseous stoichiometric mixt. of F2 and Cl2 in a closed space at room temp. (light pulses lasting 5E-6 to E-3 s with λ=200-450 nm); impurities detected by spectroscopic methods; presence of ;	99%
In neat (no solvent) equilibrium react. at 250°C;;
In neat (no solvent) Cl2 and an excess of F2;;

ammonium pertechnetate (34035-97-7) + fluorine (7782-41-4) → technetium hexafluoride

Conditions	Yield
In hydrogen fluoride byproducts: O2, N2; HF (liquid); High Pressure; at 600°C for 1 h in an autoclave; evapd. at -196°C, condensed, sealed, recrystd. by cooling from 0 to -78°C;	99%

iodine (7553-56-2) + fluorine (7782-41-4) → IF3 (22520-96-3)

Conditions	Yield
In trichlorofluoromethane Ar/F2 mixture bubbled into I2 in CFCl3 (at -45°C) until the I2 disappeared completely; solv. evapd., warmed (to -30°C), cooled (to -78°C);	99%

di(rhodium)tetracarbonyl dichloride + carbon monoxide (201230-82-2) + antimony pentafluoride (7783-70-2) + fluorine (7782-41-4) → chloropentacarbonylrhodium(III) undecafluorodiantimonate(V)

Conditions	Yield
In hydrogen fluoride HF (liquid); HF added to Rh complex under vac., kept at -196°C, F2 added, stirred for ca. 2 h, further addn. of F2, stirred at room temp. for 1 h, excess F2 removed at -196°C, HF and SbF5 added, warmed to room temp., stirred at 70°C, CO added,; stirred at -20°C for 20 h; removal of all volatiles under vac.;	99%

Carbonyl fluoride (353-50-4) + fluorine (7782-41-4) → hypofluorous acid trifluoromethyl ester (373-91-1)

Conditions	Yield
rubidium fluoride equimolar amt. of educts, steel vessel, -78°C, yield: 97 mol-%;	97%
potassium fluoride equimolar amt. of educts, steel vessel, -78°C, yield: 97 mol-%;	97%
cesium fluoride equimolar amt. of educts, steel vessel, -78°C, yield: 97 mol-%;	97%

xenon + fluorine (7782-41-4) → xenon tetrafluoride (13709-61-0)

Conditions	Yield
In gas Holloway's apparatus; continous working possible;; yields of 11gXeF4/h of very pure XeF4 are obtained;;	97%
on heating of a Xe-F2 mixture (1:5) in a closed, 1600ml Ni vessel at 400°C with following chilling of react. vessel in water;; on pumping off of excess fluorine at -78°C and removing of resting Xe with U tube (with temp. of -195°C); in 1 hour 10g XeF4 with a yield >99% are obtained;;	>99
Electrochem. Process; on electrical discharge at -78°C; detailed information about react. conditions and apparatus given;;

chromium(VI) oxide + chlorine monofluoride (7790-89-8) + fluorine (7782-41-4) → chloryl fluoride (13637-83-7) + CrF3O

Conditions	Yield
In neat (no solvent) byproducts: Cl2, O2; ClF added to CrO3, mixt. heated at 110°C for 4 h with periodic shaking, vessel evacuated at -196, -78°C, at room temp., vessel charged with F2, heated to 120°C for 12 h, removed F2 and ClO2F, repeated react. with F2 for 2 and 3 h; at -196°C removed excess F2, at room temp. removed ClO2F, elem. anal.;	A n/a B 97%

chromium oxyfluoride + chlorine monofluoride (7790-89-8) + fluorine (7782-41-4) → chloryl fluoride (13637-83-7) + CrF3O

Conditions	Yield
In neat (no solvent) byproducts: Cl2, O2; ClF added to CrO2F2, mixt. heated to 100°C for 12 h, vessel evacuated at -196, -78°C, at room temp., vessel charged with F2, heated to 120°C for 4 h; at -196°C removed excess F2, at room temp. removed ClO2F, elem. anal.;	A n/a B 97%

dodecacarbonyltetrairidium (117678-68-9) + fluorine (7782-41-4) → fac-iridiumtricarbonyltrifluoride (146168-99-2, 146237-54-9)

Conditions	Yield
In hydrogen fluoride HF (liquid); (Schlenk, N2) to a soln. of Ir-complex in HF 2 atm of F2 at -78°Cwas added, the soln. was allowed to warm to room temp., stirred for 16 h; the soln. was removed in vac.;	96%

Carbonyl fluoride (353-50-4) + fluorine (7782-41-4) → hypofluorous acid trifluoromethyl ester (373-91-1) + bis(trifluoromethyl)peroxide (927-84-4)

Conditions	Yield
yttrium(III) fluoride Kinetics; 150°C, 10 h;	A n/a B 95%
bismuth(III) fluoride Kinetics; 150°C, 12 h;	A n/a B 95%
terbium(III) fluoride Kinetics; 100°C, 30 h;	A n/a B 95%

chlorine trifluoride + fluorine (7782-41-4) → 18F-fluoride (27948-18-1) + chlorine trifluoride (7790-91-2)

Conditions	Yield
In gas at 119 - 232°C in Al-tubes about 30 - 45 min;;	A 95% B n/a
In gas at 170°C in Ni-tubes about 40 min;;	A 12% B n/a
nickel(II) fluoride In gas Kinetics; at 467, 497 and 530°K in Ni-tubes;;

fluorine (7782-41-4) → Perfluor-(polyacrylnitril)

Conditions	Yield
With polyacrylonitrile volume ratio of polyacrylnitrile:F2 = 1:60, at 20°C for 6 h then with F2 for 30 h; F2 dild. with He;	95%
With polyacrylonitrile volume ratio of polyacrylnitrile:F2 = 1:60, at 20°C for 6 h then with F2 for 30 h; F2 dild. with He;	95%

boron tris{pentafluoro-oxotellurate(VI)} (40934-88-1) + fluorine (7782-41-4) → TeF5OF (83314-21-0)

Conditions	Yield
In neat (no solvent) byproducts: BF3, TeF5OH, TeF6; under dry N2, B(OTeF5)3 in a Monel vessel evacd., cooled to -196°C, addn. of F2, closed vessel warmed to ambient temp., placed in an oven at 100°C, 67 h; cooled to -196°C, excess F2 pumped off, volatiles sepd. by fractional condensation during warming to room temp., TeF5OF retained in a trap cooled at -126°C;	95%
In neat (no solvent) byproducts: BF3, TeF5OH, TeF6; under dry N2; B(OTeF5)3 in a Monel vessel evacd., cooled to -196°C, addn. of F2, closed vessel warmed to ambient temp., placed in an oven at 115°C, 24 h;; cooled to -196°C, excess F2 pumped off, volatiles sepd. by fractional condensation during warming to room temp., TeF5OF retained in a trap cooled at -126°C;;	94%
In neat (no solvent) byproducts: BF3, TeF5OH, TeF6; under dry N2, B(OTeF5)3 in a stainless steel vessel evacd., cooled to -196°C, addn. of F2, closed vessel warmed to ambient temp., placed in an oven at 115°C, 51 h; cooled to -196°C, excess F2 pumped off, volatiles sepd. by fractional condensation during warming to room temp., TeF5OF retained in a trap cooled at -126°C;	81%

antimony pentafluoride (7783-70-2) + gold (7440-57-5, 457905-15-6) + fluorine (7782-41-4) → Au(SbF6)2Au(AuF4)2

Conditions	Yield
In hydrogen fluoride HF (liquid); Argon atmosphere, fluorocarbon polymer tube, addn. of fluorine (5 h, 800Torr), vigorous agitation (20°C, 21 h); decantation, washing (HF);	95%

deca-B-methyl-1,12-dicarba-closo-dodecaborane(12) (168098-42-8) + fluorine (7782-41-4) + sodium fluoride → perfluro-deca-B-methyl-para-carborane (356060-61-2)

Conditions	Yield
In further solvent(s) a soln. (perfluorononane) of B compd. pumped into reactor with N2/F2 bubbling, gradually heated to 110°C (24 h), held for 4 d; F2 turned off, allowed to purge for 4 h, filtered, solvent removed (vac.), sublimated (65°C/0.01 mm);	94%

sodium sulfamate + fluorine (7782-41-4) → sodium difluorosulfamate (911368-67-7)

Conditions	Yield
In water byproducts: HF; soln. NaSO3NH2 (H2O) placed into teflon-FEP ampule; cooling to 0°C, F2 (10% v/v in N2) introduced; 45 min of fluorination; mixt. pumped to dryness at 0°C;	94%

trinitromethane (517-25-9) + fluorine (7782-41-4) → fluorotrinitromethane (1840-42-2)

Conditions	Yield
With sodium hydroxide In water at 0-5°C 1.5 h;	92.3%
With NaOH In water at 0-5°C 1.5 h;	92.3%
In water 40% F2 in N2; velocity of flow 9l/h; at 0-5°C;	90%

potassium hydrogenfluoride (1279123-63-5) + diethyl ether (60-29-7) + 12-ammoniocarba-closo-dodecaborane + hydrogen fluoride (7664-39-3) + fluorine (7782-41-4) → 1-H-12-H3N-closo-1-CB11F10·0.1Et2O

Conditions	Yield
Stage #1: potassium hydrogenfluoride; 12-ammoniocarba-closo-dodecaborane; hydrogen fluoride; fluorine at -78 - 20℃; Stage #2: diethyl ether In hexane	92%

Upstream product

• 7787-62-4 bismuth pentafluoride 
• 43070-30-0 Cs₂CuF₆ 
• 16962-46-2 Cs₂MnF₆ 
• 17218-47-2 K₂NiF₆ 
• 7783-63-3 titanium(IV) fluoride 
• 7789-24-4 lithium fluoride 
• 7681-49-4 sodium fluoride 
• 1279123-63-5 potassium hydrogenfluoride 
• 7664-39-3 hydrogen fluoride 
• 7732-18-5 water 
• 7789-23-3 potassium fluoride 
• 124-43-6 sodium pyrophosphate 

Downstream Products

• 353-50-4 Carbonyl fluoride 
• 7783-41-7 difluoroether 
• 676353-70-1 iodine pentafluoride 
• 7664-39-3 hydrogen fluoride 
• 13760-83-3 ErF₃, orthorhombic 
• 7783-51-9 gallium trifluoride 
• 7784-18-1 aluminum(III) fluoride 
• 13709-38-1 lanthanum(III) fluoride 
• 13709-38-1 lanthanum trifluoride 
• 13709-38-1 lanthanum trifluoride 
• 13760-81-1 F₃Lu, orthorhombic 
• 14986-60-8 fluoroazide 
• 851363-60-5 zirconium(IV) fluoride 
• 19058-78-7 iodine(V) oxofluoride 

Relevant academic research and scientific papers

Structural Modification of the Cation-Ordered Ruddlesden-Popper Phase YSr2Mn2O7 by Cation Exchange and Anion Insertion

Calcium-for-strontium cation substitution of the a-b0c0/b0a-c0-distorted, cation-ordered, n = 2 Ruddlesden-Popper phase, YSr2Mn2O7, leads to separation into two phases, which both retain an a-b0c0/b0a-c0-distorted framework and have the same stoichiometry but exhibit different degrees of Y/Sr/Ca cation order. Increasing the calcium concentration to form YSr0.5Ca1.5Mn2O7 leads to a change in the cooperative tilting on the MnO6 units to a novel a-b-c-/b-a-c- arrangement described in space group P21/n11. Low-temperature, topochemical fluorination of YSr2Mn2O7 yields YSr2Mn2O5.5F3.5. In contrast to many other fluorinated n = 2 Ruddlesden-Popper oxide phases, YSr2Mn2O5.5F3.5 retains the a-b0c0/b0a-c0 lattice distortion and P42/mnm space group symmetry of the parent oxide phase. The resilience of the a-b0c0/b0a-c0-distorted framework of YSr2Mn2O7 to resist symmetry-changing deformations upon both cation substitution and anion insertion/exchange is discussed on the basis the A-site cation order of the lattice and the large change in the ionic radius of manganese upon oxidation from Mn3+ to Mn4+. The structure property relations observed in the Y-Sr-Ca-Mn-O-F system provide insight into assisting in the synthesis of n = 2 Ruddlesden-Popper phases, which adopt cooperative structural distortions that break the inversion symmetry of the extended lattice and therefore act as a route for the preparation of ferroelectric and multiferroic materials.

Production of fluorine by the electrolysis of calcium fluoride-containing tetrafluoroborate melts

Tetrafluoroborate melts have been shown to be viable electrolytes for the electrochemical production of fluorine from dissolved CaF2. The anode reaction at pyrolytic graphite electrodes apparently involves the oxidation of BF4-

Dinitrogen difluoride chemistry. Improved syntheses of cis- and trans-N2F2, Synthesis and characterization of N 2F+Sn2F9-, ordered crystal structure of N2F+Sb2F11 -, High-level electronic structure calculations of cis-N 2F2

N2F+ salts are important precursors in the synthesis of N5+ compounds, and better methods are reported for their larger scale production. A new, marginally stable N2F + salt, N2F+Sn2F9 -, was prepared and characterized. An ordered crystal structure was obtained for N2F+Sb2F11-, resulting in the first observation of individual N - N and N-F bond distances for N2F+ in the solid phase. The observed N - N and N-F bond distances of 1.089(9) and 1.257(8) A, respectively, are among the shortest experimentally observed N-N and N-F bonds. High-level electronic structure calculations at the CCSD(T) level with correlation-consistent basis sets extrapolated to the complete basis limit show that cis-N2F 2 is more stable than trans-N2F2 by 1.4 kcal/mol at 298 K. The calculations also demonstrate that the lowest uncatalyzed pathway for the trans-cis isomerization of N2F2 has a barrier of 60 kcal/mol and involves rotation about the N - N double bond. This barrier is substantially higher than the energy required for the dissociation of N2F2 to N2 and 2 F. Therefore, some of the N2F2 dissociates before undergoing an uncatalyzed isomerization, with some of the dissociation products probably catalyzing the isomerization. Furthermore, it is shown that the trans-cis isomerization of N2F2 is catalyzed by strong Lewis acids, involves a planar transition state of symmetry Cs, and yields a 9:1 equilibrium mixture of cis-N2F2 and trans-N2F2. Explanations are given for the increased reactivity of cis-N2F 2 with Lewis acids and the exclusive formation of cis-N 2F2 in the reaction of N2F+ with F-. The geometry and vibrational frequencies of the F2N - N isomer have also been calculated and imply strong contributions from ionic N2F+ F- resonance structures, similar to those in F3NO and FNO.

Vaporization products of transition-metal and rare-earth complex fluorides studied by high-temperature mass spectrometry

Gaseous products of the thermal decomposition of Ni(IV), Tb(IV), Mn(IV), and Pt(IV) complex fluorides were studied by high-temperature mass spectrometry. The results demonstrate that the decomposition of potassium hexafluoronickelate and potassium heptafl

Thermochemical reactions and equilibria between fluoromicas and silicate matrices: A petromimetic perspective on structural ceramic composites

A petromimetic (geological-analog) approach is applied to the design of alumina-fiber-reinforced glass-ceramic-matrix composites that use a refractory, trioctahedral fluoromica fiber-matrix interphase and feldspar matrixes. Studies of the solid-state reaction couples between these silicate phases are pursued to address the chemical tailorability of the interphase/matrix interface from an engineering perspective. The minimization of alumina and silica activities within polyphase, feldspar-based matrixes via MgO buffering is shown to be an effective route toward a stable fluoromica interphase. An anorthite-2-vol%-alumina (CaAl2Si2O8+α-Al2O3) substrate, chemically buffered with MgO, is shown to exhibit thermodynamic stability against fluorokinoshitalite (BaMg3[Al2Si2]O10F2), up to temperatures potentially as high as 1460 °C. The key to the approach is the reduction of alumina activity via the formation of MgAl2O4 spinel. Similarly, the formation of forsterite (Mg2SiO4) stabilizes the mica in contact with matrix compositions otherwise containing excess silica. The cationic interdiffusion between solid-solution feldspars and fluoromicas also is characterized. Coupled interdiffusion of K+ and Si4+ in exchange for Ba2+ and Al3+ was observed between K-Ba solid-solution celsian and the barium-rich solid-solution end-member fluorokinoshitalite at 1300 °C. A similar cationic exchange also is observed against the potassium-rich end-member fluorophlogopite (KMg3[AlSi3]O10F2), although in a reverse direction, at temperatures of 1280 °C. The interfacial compositions identified via electron microprobe analysis specify one set of local equilibrium conditions from which global ceramic composite equilibrium can be achieved.

Synthesis of Manganese Tetrafluoride at Atmospheric Pressure

The fluorination rate of powdery MnF3 is measured by the gravimetric method at 450-540°C, fluorine partial pressure 1.0-10.1 kPa, near-atmospheric total pressure, and the linear rate of (F2 + N2) gas mixture 2.0 cm/s. It is shown that the rate law of fluorination α = 10-0.14exp[-84.7 × 103/RT]ρF20.57τ. A new procedure of MnF4 synthesis from particulate MnF2 and MnF3 in a fluorine flow at atmospheric pressure and the design of a fluorination reactor are described. They are shown to afford relatively high reaction rates (up to 35 g/h based on MnF4) and high yields with respect to fluorine (up to 42%).

Thermal Decomposition and Pyrohydrolysis of Manganese Tetrafluoride

Thermal decomposition of MnF4 and its reaction with water vapor are studied by gravimetric, DTA, and TG analyses complemented by chemical and X-ray diffraction analyses of the solid products. The decomposition is found to begin at temperatures higher than 325 K and to proceed with the formation of MnF3 and partial evolution of MnF4. At temperatures below 473 K, the reaction does not reach completion because of kinetic hindrance. Pyrohydrolysis of MnF4 is accompanied by reduction and proceeds stepwise to form first MnF3 · 3H2O and then MnOF.

Kinetics of Fluorination of Manganese Compounds with Fluorine Gas

The kinetics of fluorination of MnO2, MnF2, and KMnF3 powders by fluorine in nitrogen carrier gas at atmospheric pressure was studied by gravimetry. The kinetic equations of fluorination were deduced. MnO2 converts to MnF3 markedly more rapidly than MnF2. The volatile product (MnF4) forms above 780 K.

Novel type of oxonium salts H3OM(AsF6)3 (M=Mn, Co, Ni): Syntheses, structures and some properties

H3OAsF6 reacts with M(AsF6)2 (M=Mn,Co,Ni) in anhydrous hydrogen fluoride (aHF) acidified with AsF5 at room temperature yielding novel oxonium salts H3OM(AsF6)3. If MF2 is used instead of M(AsF6)2 the aHF should be rich in AsF5 to synthesize M(AsF6)2 in situ. As source of the oxonium cation water or the transition metal oxide can be used. X-ray powder diffraction at variable temperatures revealed for H3OCo(AsF6)3 a phase transition at 120K. The high temperature (HT) form crystallizes in the orthorhombic space group Pnma (No.62) with a=1037.6(1), b=1372.6(1), c=932.8(1) pm, V=1.3285(2) nm3, Z=4 and dc=3.223 g/cm3 at 150 K. The low temperature (LT) form crystallizes in the monoclinic space group P21/c (No.14) with a=1032.6(1), b=1370.2(2), c=1867.1(2) pm, β=90.036(9)°, V=2.6416(5) nm3, Z=8, dc=3.242 g/cm3 at 90 K. The structure was solved by direct methods using diffractometer data sets and refined to conventional R1=0.039 for 2604 reflections (HT-form) and R1=0.053 for 9215 reflections (LT-form), respectively. One main feature of the H3OCo(AsF6)3 structure is a ring of four AsF6 octahedra which are connected by four cobalt atoms. This kind of ring system is continued infinitely in the plane and also perpendicular to the plane. In this arrangement open channels are created in which oxonium ions are placed below and above the plane. Gauthier-Villars.

Observation of the laser induced fluorescence spectra of C2(d3?g 3?u) from the infrared multiphoton dissociation of bis-trifluoromethyl peroxide

C2 has been produced by infrared multiphoton dissociation of bis-trifluoromethyl peroxide.The (0,0), (1,0), and (2,0) transition of the Swan system for C2 have been detected using laser induced fluorescence method.The (0,0), (2,0) laser excitation spectra