Lead(II) fluoride

Lead(II) fluoride
Names
Other names
Lead difluoride
plumbous fluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.089 Edit this at Wikidata
UNII
  • InChI=1S/2FH.Pb/h2*1H;/q;;+2/p-2
    Key: FPHIOHCCQGUGKU-UHFFFAOYSA-L
  • F[Pb]F
Properties
PbF2
Molar mass 245.20 g/mol
Appearance white powder
Odor odorless
Density 8.445 g/cm3 (orthorhombic)
7.750 g/cm3 (cubic)
Melting point 824 °C (1,515 °F; 1,097 K)
Boiling point 1,293 °C (2,359 °F; 1,566 K)
0.057 g/100 mL (0 °C)
0.0671 g/100 mL (20 °C)[1]
2.05 x 10−8 (20 °C)
Solubility soluble in nitric acid and hydrochloric acid;
insoluble in acetone and ammonia
−-58.1·10−6 cm3/mol
Structure
Fluorite (cubic), cF12
Fm3m, No. 225
Hazards
Lethal dose or concentration (LD, LC):
3031 mg/kg (oral, rat)
Related compounds
Other anions
 Lead(II) chloride
Lead(II) bromide
Lead(II) iodide
Other cations
 Difluorocarbene
Difluorosilylene
Difluorogermylene
Stannous 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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Lead(II) fluoride is the inorganic compound with the formula PbF2. It is a white solid. The compound is polymorphic, at ambient temperatures it exists in orthorhombic (PbCl2 type) form, while at high temperatures it is cubic (Fluorite type).[2]

Preparation

Lead(II) fluoride can be prepared by treating lead(II) hydroxide or lead(II) carbonate with hydrofluoric acid:[3]

Pb(OH)2 + 2 HF → PbF2 + 2 H2O

Alternatively, it is precipitated by adding hydrofluoric acid to a lead(II) salt solution, or by adding a fluoride salt to a lead salt, such as potassium fluoride to a lead(II) nitrate solution,[4]

2 KF + Pb(NO3)2 → PbF2 + 2 KNO3

or sodium fluoride to a lead(II) acetate solution.

2 NaF + Pb(CH3COO)2 → PbF2 + 2 NaCH3COO

It appears as the very rare mineral fluorocronite.[5][6]

Uses

Two 25 mm × 25 mm × 140 mm PbF
2 scintillator crystals used in the Muon g−2 experiment.

Lead(II) fluoride is used in low melting glasses, in glass coatings to reflect infrared rays, in phosphors for television-tube screens, and as a catalyst for the manufacture of picoline.[3] The Muon g−2 experiment uses PbF
2 scintillators in conjunction with silicon photomultipliers.[7]

It also serves as a oxygen scavenger in high-temperature fluorine chemistry, as plumbous oxide is relatively volatile.[8]

References

  1. ^ NIST-data review 1980
  2. ^ Haines, J.; Léger, J. M.; Schulte, O. (1998-04-01). "High-pressure isosymmetric phase transition in orthorhombic lead fluoride". Physical Review B. 57 (13). American Physical Society (APS): 7551–7555. Bibcode:1998PhRvB..57.7551H. doi:10.1103/physrevb.57.7551. ISSN 0163-1829.
  3. ^ a b Carr, Dodd S. "Lead Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_249. ISBN 978-3527306732.
  4. ^ Arnold Hollemann, Egon Wiberg, 101st ed., de Gruyter 1995 Berlin; ISBN 3-11-012641-9
  5. ^ "Fluorocronite".
  6. ^ "List of Minerals". 21 March 2011.
  7. ^ Grange, J.; et al. (Muon g−2 Collaboration) (Jan 27, 2015). Muon (g−2) Technical Design Report. Fermi National Accelerator Laboratory (Report). arXiv:1501.06858. Bibcode:2015arXiv150106858G. FERMILAB-FN-0992-E. Via inSPIRE
  8. ^ Beeks, Kjeld; Sikorsky, Tomas; Rosecker, Veronika; Pressler, Martin; Schaden, Fabian; Werban, David; Hosseini, Niyusha; Rudischer, Lukas; Schneider, Felix; Berwian, Patrick; Friedrich, Jochen; Hainz, Dieter; Welch, Jan; Sterba, Johannes H.; Kazakov, Georgy; Schumm, Thorsten (2023). "Growth and characterization of thorium‑doped calcium fluoride single crystals" (PDF). Scientific Reports. 13 (1): 3897–. Bibcode:2023NatSR..13.3897B. doi:10.1038/s41598-023-31045-5. PMC 9995343. PMID 36890210.

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