Lithium fluoride

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Lithium fluoride

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Template:Longitem	LiF
Molar mass	25.939(2) g/mol
Appearance	White powder or colorless hygroscopic crystals
Density	2.635 g/cm3
Melting point	Template:Chembox CalcTemperatures
Boiling point	Template:Chembox CalcTemperatures
Template:Longitem	1.84Template:E
Solubility	soluble in HF insoluble in alcohol
Template:Longitem	−10.1·10−6 cm3/mol
Template:Longitem	1.3915
Template:Longitem	Face-centered cubic
Template:Longitem	a = 403.51 pm
Template:Longitem	Linear
Template:Longitem	1.507 J/(g·K)
Template:Longitem	35.73 J/(mol·K)
Template:Longitem	−616 kJ/mol
NFPA 704 (fire diamond)	Template:NFPA 704 diamond
Template:Longitem	Lithium chloride Lithium bromide Lithium iodide Lithium astatide
Template:Longitem	Sodium fluoride Potassium fluoride Rubidium fluoride Caesium fluoride Francium fluoride

Lithium fluoride is an inorganic compound with the chemical formula LiF. It is a colorless solid that transitions to white with decreasing crystal size. Its structure is analogous to that of sodium chloride, but it is much less soluble in water. It is mainly used as a component of molten salts. Partly because Li and F are both light elements, and partly because Template:Chem2 is highly reactive, formation of LiF from the elements releases one of the highest energies per mass of reactants, second only to that of BeO.

Manufacturing

LiF is prepared from lithium hydroxide or lithium carbonate with hydrogen fluoride.

Applications

Precursor to lithium hexafluorophosphate for batteries

Lithium fluoride is reacted with hydrogen fluoride (HF) and phosphorus pentachloride to make lithium hexafluorophosphate Template:Chem2, an ingredient in lithium ion battery electrolyte.

The lithium fluoride alone does not absorb hydrogen fluoride to form a bifluoride salt.

In molten salts

Fluorine 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. A useful molten salt, FLiNaK, consists of a mixture of LiF, together with sodium fluoride and potassium fluoride. The primary coolant for the Molten-Salt Reactor Experiment was FLiBe; Template:Chem2 (66 mol% of LiF, 33 mol% of Template:Chem2).

Optics

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

Radiation detectors

It is also used as a means to record ionizing radiation exposure from gamma rays, beta particles, and neutrons (indirectly, using the [[Lithium-6|Template:Nuclide]] (n,alpha) nuclear reaction) in thermoluminescent dosimeters. ⁶LiF nanopowder enriched to 96% has been used as the neutron reactive backfill material for microstructured semiconductor neutron detectors (MSND).

Nuclear reactors

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 is exceptionally chemically stable and LiF/Template:Chem2 mixtures (FLiBe) have low melting points () and the best neutronic properties of fluoride salt combinations appropriate for reactor use. MSRE used two different mixtures in the two cooling circuits.

Cathode for PLED and OLEDs

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, ε) of LiF is 9.0.

Natural occurrence

Naturally occurring lithium fluoride is known as the extremely rare mineral griceite.