Lithium fluoride

Lithium fluoride
Lithium fluoride boule
Lithium fluoride
__ Li+     __ F

__ Li+     __ F
Names
IUPAC name
Lithium fluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.229 Edit this at Wikidata
EC Number
  • 232-152-0
RTECS number
  • OJ6125000
UNII
  • InChI=1S/FH.Li/h1H;/q;+1/p-1 checkY
    Key: PQXKHYXIUOZZFA-UHFFFAOYSA-M checkY
  • InChI=1/FH.Li/h1H;/q;+1/p-1
    Key: PQXKHYXIUOZZFA-REWHXWOFAG
  • [Li+].[F-]
Properties
LiF
Molar mass 25.939(2) g/mol
Appearance White powder or colorless hygroscopic crystals
Density 2.635 g/cm3
Melting point 845 °C (1,553 °F; 1,118 K)
Boiling point 1,676 °C (3,049 °F; 1,949 K)
0.127 g/(100 mL) (18 °C)
0.134 g/(100 mL) (25 °C)
1.84×10−3[1]
Solubility soluble in HF
insoluble in alcohol
−10.1·10−6 cm3/mol
1.3915
Structure
Face-centered cubic
a = 403.51 pm
Linear
Thermochemistry
1.507 J/(g·K)
35.73 J/(mol·K)
-616 kJ/mol
Hazards
GHS labelling:
GHS06: Toxic
Danger
H301, H315, H319, H335[2]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Lethal dose or concentration (LD, LC):
143 mg/kg (oral, rat)[3]
Related compounds
Other anions
Lithium chloride
Lithium bromide
Lithium iodide
Lithium astatide
Other cations
Sodium fluoride
Potassium fluoride
Rubidium fluoride
Caesium fluoride
Francium fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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.[4] Partly because Li and F are both light elements, and partly because F2 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.

  1. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
  2. ^ "Lithium fluoride - Product Specification Sheet". Sigma-Aldrich. Merck KGaA. Retrieved 1 Sep 2019.
  3. ^ "Lithium fluoride". Toxnet. NLM. Archived from the original on 12 August 2014. Retrieved 10 Aug 2014.
  4. ^ Aigueperse J, Mollard P, Devilliers D, et al. (2005). "Fluorine Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a11_307. ISBN 9783527303854.