3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||78.075 g·mol−1|
|Appearance||White crystalline solid (single crystals are transparent)|
|Melting point||1,418 °C (2,584 °F; 1,691 K)|
|Boiling point||2,533 °C (4,591 °F; 2,806 K)|
|0.015 g/L (18 °C)|
0.016 g/L (20 °C)
Solubility product (Ksp)
|3.9 × 10−11 |
|Solubility||insoluble in acetone|
slightly soluble in acid
Refractive index (nD)
|cubic crystal system, cF12|
a = 5.451 Å, b = 5.451 Å, c = 5.451 Å
α = 90°, β = 90°, γ = 90°
|Ca, 8, cubic|
F, 4, tetrahedral
|Occupational safety and health (OHS/OSH):|
|Reacts with concentrated sulfuric acid to produce hydrofluoric acid|
|NFPA 704 (fire diamond)|
|Lethal dose or concentration (LD, LC):|
LDLo (lowest published)
|>5000 mg/kg (oral, guinea pig)|
4250 mg/kg (oral, rat)
|Safety data sheet (SDS)||ICSC 1323|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
what is ?)(
Calcium fluoride is the inorganic compound of the elements calcium and fluorine with the formula CaF2. It is a white insoluble solid. It occurs as the mineral fluorite (also called fluorspar), which is often deeply coloured owing to impurities.
The compound crystallizes in a cubic motif called the fluorite structure.
Ca2+ centres are eight-coordinate, being centered in a cube of eight F− centres. Each F− centre is coordinated to four Ca2+ centres in the shape of a tetrahedron. Although perfectly packed crystalline samples are colorless, the mineral is often deeply colored due to the presence of F-centers. The same crystal structure is found in numerous ionic compounds with formula AB2, such as CeO2, cubic ZrO2, UO2, ThO2, and PuO2. In the corresponding anti-structure, called the antifluorite structure, anions and cations are swapped, such as Be2C.
The gas phase is noteworthy for failing the predictions of VSEPR theory; the CaF2 molecule is not linear like MgF2, but bent with a bond angle of approximately 145°; the strontium and barium dihalides also have a bent geometry. It has been proposed that this is due to the fluoride ligands interacting with the electron core or the d-subshell of the calcium atom.
The mineral fluorite is abundant, widespread, and mainly of interest as a precursor to HF. Thus, little motivation exists for the industrial production of CaF2. High purity CaF2 is produced by treating calcium carbonate with hydrofluoric acid:
- CaCO3 + 2 HF → CaF2 + CO2 + H2O
Naturally occurring CaF2 is the principal source of hydrogen fluoride,[clarification needed] a commodity chemical used to produce a wide range of materials. Calcium fluoride in the fluorite state is of significant commercial importance as a fluoride source. Hydrogen fluoride is liberated from the mineral by the action of concentrated sulfuric acid:
- CaF2 + H2SO4 → CaSO4(solid) + 2 HF
Calcium fluoride is used to manufacture optical components such as windows and lenses, used in thermal imaging systems, spectroscopy, telescopes, and excimer lasers (used for photolithography in the form of a fused lense). It is transparent over a broad range from ultraviolet (UV) to infrared (IR) frequencies. Its low refractive index reduces the need for anti-reflection coatings. Its insolubility in water is convenient as well. It also allows much smaller wavelenthes to pass through.
CaF2 is classified as "not dangerous", although reacting it with sulfuric acid produces very toxic hydrofluoric acid. With regards to inhalation, the NIOSH-recommended concentration of fluorine-containing dusts is 2.5 mg/m3 in air.
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- Aigueperse, Jean; Mollard, Paul; Devilliers, Didier; Chemla, Marius; Faron, Robert; Romano, Renée; Cuer, Jean Pierre (2005), "Fluorine Compounds, Inorganic", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, p. 307, doi:10.1002/14356007.a11_307.
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- NIST webbook thermochemistry data
- Charles Townes on the history of lasers
- National Pollutant Inventory - Fluoride and compounds fact sheet
- Crystran Material Data
- MSDS (University of Oxford)