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| Names | |
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| Other names
Lead difluoride
plumbous fluoride | |
| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.029.089 |
PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| 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] | |
Solubility product (Ksp)
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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): | |
LD50 (median dose)
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3031 mg/kg (oral, rat) |
| Related compounds | |
Other anions
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Lead(II) chloride Lead(II) bromide Lead(II) iodide |
Other cations
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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
[edit]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
[edit]
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]
References
[edit]- ^ NIST-data review 1980
- ^ 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.
- ^ 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.
- ^ Arnold Hollemann, Egon Wiberg, 101st ed., de Gruyter 1995 Berlin; ISBN 3-11-012641-9
- ^ "Fluorocronite".
- ^ "List of Minerals". 21 March 2011.
- ^ Grange, J.; et al. (Muon g−2 Collaboration) (Jan 27, 2015). "Muon (g−2) Technical Design Report". arXiv:1501.06858. Bibcode:2015arXiv150106858G.
((cite journal)): Cite journal requires|journal=(help) Via inSPIRE
| Pb(II) | |
|---|---|
| Pb(II,IV) | |
| Pb(IV) | |