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Although odorless, lithium fluoride has a bitter-saline taste.  Lithium fluorides structure is analogous to that of sodium chloride, but it is much less soluble in water.

Lithium fluoride is the least soluble of the alkali metal fluorides.  This characteristic likens Lithium fluoride to the alkaline earth fluorides.

Lithium Fluoride, LiF, is typically a white inorganic compound, although it may appear colorless until ground into finer particles.  Lithium fluoride is soluble in acid and slightly soluble in water, while insoluble in ethanol and acetone.

White cubic crystals; refractive index 1.3915; density 2.635 g/cm3; melts at 845°C; vaporizes at 1,676°C; very slightly soluble in water 0.27 g/100g at 18°C; soluble in hydrofluoric acid; insoluble in alcohol.

The latter phosphor has superior characteristics compared to its long serving counterpart, which has been the most widely used TL personnel dosimeter for the past 30 years.  Lithium fluoride (LiF) is used chiefly as a fluxing agent in enamels and glasses.

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Lithium Fluoride is a water insoluble Lithium source for use in oxygen-sensitive applications, such as metal production.  Lithium fluorides have diverse applications in current technologies and science, from oil refining and etching to synthetic organic chemistry and the manufacture of pharmaceuticals.

Lithium fluoride is exceptionally chemically stable and LiF/BeF2 mixtures (FLiBe) have low melting points (360 to 459 °C or 680 to 858 °F) and the best neutronic properties of fluoride salt combinations appropriate for reactor use.  Lithium fluoride is used two different mixtures in the two cooling circuits.

Lithium fluoride is produced by the electrolysis of molten potassium bifluoride.  This electrolysis proceeds more efficiently when the electrolyte contains a few percent of LiF, possibly because it facilitates formation of an Li-C-F interface on the carbon electrodes.

Lithium Fluoride (LiF) is a colourless crystalline material grown by vacuum Stockbarger technique.  Lithium fluoride has a wide transmission spectrum from the VUV to IR, but it is most commonly used for specialised UV optics due to its deep UV transmission.

The material can be cleaved along (100) and less commonly (110).  Although the optical characteristics are good the structure is not perfect and cleavage is difficult.

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Because of the large band gap for Lithium fluoride, its crystals are transparent to short wavelength ultraviolet radiation, more so than any other material.  Lithium fluoride is therefore used in specialized optics for the vacuum ultraviolet spectrum. Lithium fluoride is used also as a diffracting crystal in X-ray spectrometry.

In the ceramic industry, lithium fluoride is sometimes used for manufacturing enamels and glazes, reducing kiln mild improvement in thermal shock resistance, abrasion resistance and acid resistance.

Lithium fluoride is also used as a means to record ionizing radiation exposure from gamma rays, beta particles, and neutrons (indirectly, using the 63Li (n,alpha) nuclear reaction) in thermoluminescent dosimeters. Lithium fluoride nanopowder enriched to 96% has been used as the neutron reactive backfill material for microstructured semiconductor neutron detectors.

-Used in the preparation of hypersensitive thermoluminescent materials, dosimeters, and in the room-temperature oxidation of noble metals using fluorine in anhydrous HF.

A useful molten salt, consists of a mixture of LiF, together with sodium fluoride and potassium fluoride.  The primary coolant for the Molten-Salt Reactor Experiment was FLiBe; LiF-BeF2 (66-33 mol%).

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However, Lithium fluoride can be cleaned with alcohol. Lithium fluoride is widely available in the forms LiF : Mg,Ti and LiF : Mg,Cu,P.

Modest precautions should be taken against moisture and high energy radiation damage. Lithium fluoride is sensitive to thermal shock. Irradiation produces color centers.

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Lithium fluoride is most widely used as a flux in the production of ceramics, such as enamels, glasses and glazes.  Similarly Lithium fluoride is also used in brazing and welding fluxes and molten salt chemistry in metallurgy.

Lithium fluoride is most widely used as a flux in the production of ceramics, such as enamels, glasses and glazes.  Similarly Lithium fluoride is also used in brazing and welding fluxes and molten salt chemistry in metallurgy.

Lithium fluorides are also commonly used to alloy metals and for optical deposition.  Lithium Fluoride is generally immediately available in most volumes.

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One of its main uses is as a component of molten salts and it is evaporated under vacuum to form anti-reflective layers for optical coatings. Lithium fluoride (LiF) single crystal as well as doped with proper activators is a highly sensitive phosphor used in several applications such as integrated optics, color center laser, and radiation dosimetry.

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Lithium fluoride (highly enriched in the common isotope lithium-7) forms the basic constituent of the preferred fluoride salt mixture used in liquid-fluoride nuclear reactors.  Typically lithium fluoride is mixed with beryllium fluoride to form a base solvent (FLiBe), into which fluorides of uranium and thorium are introduced.

Lithium fluoride also possesses the highest UV transmission of any material, being able to transmit significantly into the VUV region at the hydrogen Lyman-alpha line (121nm). Lithium fluoride is slightly soluble in water, while being soluble in HDF and other acids.

In its high-temperature molten state, Lithium fluoride functions in batteries as an electrolyte component. Lithium Fluoride (LiF) has the lowest refractive index of all common infrared materials.

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Lithium fluoride is involved to record ionizing radiation exposure from gamma rays, beta particles and neutrons in thermoluminescent dosimeters.  In nuclear reactors, lithium fluoride is mixed with beryllium fluoride to form a base solvent, which is used in molten-salt reactor experiment.

Due to lithium generally being a harder material to come by, lithium fluoride is also less readily accessible.  Naturally occurring lithium fluoride exists as the rare mineral gricite.

Lithium fluoride is an inorganic compound with the chemical formula LiF.  Lithium fluoride is a colorless solid, that transitions to white with decreasing crystal size.

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Lithium fluoride finds the most use in ceramic, chemical (especially molten salt), and optical applications. Lithium fluoride is an essential component of fluorine electrolyte cell.

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Lithium fluoride is reacted with hydrogen fluoride-HF and phosphorus pentachloride to make lithium hexafluorophosphate, an ingredient in lithium ion battery electrolyte.

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Lithium fluoride is a white crystalline. Lithium fluoride is not hygroscopic as are the other lithium halides and is not affected by exposure to the air.

Lithium fluoride is mainly used as a component of molten salts. Formation of Lithium fluoride from the elements releases one of the highest energy per mass of reactants, second only to that of BeO.

Lithium fluoride transmits well into the VUV region at the hydrogen Lyman-alpha line (121nm) and beyond. Lithium fluoride is also used for X-ray monochromator plates where its lattice spacing makes it the most useful analysis crystal. Lithium Fluoride is an electrolyte salt used in various industrial applications and contains a minimum 98.5% wt% of active ingredient.

7789-24-4 Fluorolithium Lithium fluoride (LiF) Lithium monofluoride Trilithium trifluoride Lithium fluoride (Li3F3) lithium;fluoride Lithium fluorure NTL 50 TLD 100 TLD 700 Lithium fluoride (6LiF) Lithium fluoride (7LiF) Lithium fluorure [French] UNII-1485XST65B MFCD00011090 1485XST65B NSC12957 Lithium fluorure (FRENCH) 17409-87-9 LiF Lithium fluoride, 97%, for analysis Lithium bifluoride Lithium fluoride, 99.98%, extra pure Lithium fluoride (Li(HF2)) HSDB 651 (6L)Lithium fluoride (7L)Lithium fluoride EINECS 232-152-0 NSC 12957 Lithium fluorure [French] EINECS 235-292-0 EINECS 238-958-9 EINECS 241-438-4 ACMC-20akmp WLN: LI F Lithium fluoride, ultra dry 12159-92-1 Lithium fluoride, Optical Grade DTXSID10894119 TLD-100 s228 AMY37018 NSC-12957 AKOS015833195 AKOS015902703 Lithium fluoride, 99.99% (metals basis) FT-0627899 A839270 Q409319 Hydrofluoric acid, ion(1-), with lithanylium (1:1)

Lithium fluoride is sensitive to ionization radiation, especially when doped with proper activators.  Lithium fluoride doped with Mg, Cu, and P is found to be the most sensitive material for ionizing radiations using thermoluminescence (TL) technique.

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Lithium Fluoride is used for windows, lenses and prisms in the Vacuum UV, UV, visible and infrared where transmission in the range 0.104µm to 7µm is desired.  Transmission is about 40% at 121nm, this is one of the most popular material for deep UV spectrum.

Lithium fluoride has a density of 2.64 g/cc, a melting point of 845°C, and a vapor pressure of 10-4 Torr at 1,180°C.  Lithium fluoride is crystalline in appearance and white in color.

Lithium fluoride is widely used in many fields.  Lithium fluoride is used in the soldering progress for glass lining as a cosolvent.

VUV grade Lithium fluoride windows are available. This is the best VUV transmitter available. Lithium fluoride is an inorganic compound with a formula of LiF.

Lithium fluoride possesses the highest UV transmission of any material, being able to transmit significantly into the VUV region at the hydrogen Lyman-alpha line (121nm).  Lithium fluoride can be applied in rechargeable Li batteries, in radiation dosimeter for personnel monitoring as well as radiation research, as an optical material, as a heat sink material, to produce ceramics, and to dissolve fluid fuel for molten salt reactors. lithium fluoride is a strong irritant to the eyes and skin; potassium bromide is toxic by ingestion and inhalation; sodium chloride is table salt, a medical concern when ingested in excess, but certainly of no significant hazard to emergency responders.

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Lithium fluoride is widely used in PLED and OLED as a coupling layer to enhance electron injection.  The thickness of the LiF layer is usually around 1 nm.  The dielectric constant (or relative permittivity) of Lithium fluoride is 9.0.

High purity, submicron and nanopowder forms may be considered. Lithium fluoride is the material with the most extreme UV transmission of all and is used for special UV optics.

Lithium fluoride finds application as an additive of aluminum electrolysis and rare earth electrolysis as a crystal in X-ray spectrometry.  Lithium fluoride is also used in specialized UV optics due to its large band gap and transparency to short wave length ultraviolet radiation.

Lithium fluoride is prepared from lithium hydroxide or lithium carbonate with hydrogen fluoride. Lithium Fluoride (LiF) has the lowest refractive index of all common infrared materials.

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Lithium fluoride has the highest UV transmission of all materials and is used for X-ray monochromator plates where its lattice spacing makes it the most suitable analysis crystal.  Lithium fluoride has low effective atomic number (8.14), which is sufficiently close to that of the biological tissue (7.4).

Lithium fluoride has a large bandgap which causes it to have an extreme UV transmission.  This results in lithium fluoride having the most transparent crystals to short wavelength UV radiation, and makes this material especially useful to special UV optics.  Lithium fluoride is capable of transmitting beyond the VUV range and is also used in X-ray spectrometry.

Lithium fluoride is different from the other lithium halides in that it does not form hydrates which can be isolated from solution. Lithium fluoride does show an increase in solubility as hydrofluoric acid is added to an aqueous solution.  Under these conditions the Lithium fluoride ion is converted to the bifluoride ion, HF-2, allowing further dissolving of the solid lithium fluoride.

In metallurgy processes, lithium fluoride is sometimes used as welding/soldering flux, and is a particularly popular choice for aluminum and magnesium metals.  Lithium fluoride is also used in the aluminum industry to improve the electrical efficiency of the additive, as a neutron shielding material in the atomic energy industry, and in molten salt reactors as a solvent.