Lead(II) sulfide
Names | |
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Other names
Plumbous sulfide
Galena, Sulphuret of lead | |
Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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100.013.861 |
EC Number |
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PubChem CID
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RTECS number
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UNII | |
UN number | 3077 |
CompTox Dashboard (EPA)
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Properties | |
PbS | |
Molar mass | 239.30 g/mol |
Appearance | Black |
Density | 7.60 g/cm3[1] |
Melting point | 1,113[1] °C (2,035 °F; 1,386 K) |
Boiling point | 1,281 °C (2,338 °F; 1,554 K) |
2.6×10−11 kg/kg (calculated, at pH=7)[2] 8.6×10−7 kg/kg[3] | |
−83.6·10−6 cm3/mol[4] | |
Refractive index (nD)
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3.91[5] |
Structure[7] | |
Halite (cubic), cF8 | |
Fm3m, No. 225 | |
a = 5.936 Å
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Formula units (Z)
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4 |
Octahedral (Pb2+) Octahedral (S2−) | |
3.59 D[6] | |
Thermochemistry[8] | |
Heat capacity (C)
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49.5 J/mol⋅K |
Std molar
entropy (S⦵298) |
91.2 J/mol |
Std enthalpy of (ΔfH⦵298)formation |
−100.4 kJ/mol |
Gibbs free energy (ΔfG⦵)
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−98.7 kJ/mol |
Hazards | |
GHS labelling: | |
Danger | |
H302, H332, H360, H373, H410 | |
P201, P202, P260, P261, P264, P270, P271, P273, P281, P301+P312, P304+P312, P304+P340, P308+P313, P312, P314, P330, P391, P405, P501 | |
NFPA 704 (fire diamond) | |
Flash point | Non-flammable |
Safety data sheet (SDS) | External MSDS |
Related compounds | |
Other anions
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Lead(II) oxide Lead selenide Lead telluride |
Other cations
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Germanium(II) sulfide
Tin(II) sulfide |
Related compounds
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Bismuth sulfide
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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) sulfide (also spelled sulphide) is an inorganic compound with the formula PbS. Galena is the principal ore and the most important compound of lead. It is a semiconducting material with niche uses.
Addition of hydrogen sulfide or sulfide salts to a solution containing a lead salt, such as PbCl2, gives a black precipitate of lead sulfide.
- Pb2+ + H2S → PbS↓ + 2 H+
This reaction is used in qualitative inorganic analysis. The presence of hydrogen sulfide or sulfide ions may be tested using "lead acetate paper."
Like the related materials PbSe and PbTe, PbS is a semiconductor.[9] In fact, lead sulfide was one of the earliest materials to be used as a semiconductor.[10] Lead sulfide crystallizes in the sodium chloride motif, unlike many other IV-VI semiconductors.
Since PbS is the main ore of lead, much effort has focused on its conversion. A major process involves smelting of PbS followed by reduction of the resulting oxide. Idealized equations for these two steps are:[11]
- 2 PbS + 3 O2 → 2 PbO + 2 SO2
- PbO + C → Pb + CO
The sulfur dioxide is converted to sulfuric acid.
Nanoparticles
Lead sulfide-containing nanoparticle and quantum dots have been well studied.[12] Traditionally, such materials are produced by combining lead salts with a variety of sulfide sources.[13][14] In 2009, PbS nanoparticles have been examined for use in solar cells.[15]
Applications
Photodetector
PbS was one of the first materials used for electrical diodes that could detect electromagnetic radiation, including
Cooling the PbS elements, for example using liquid nitrogen or a
, InSb, or HgCdTe).Planetary science
Elevations above 2.6 km (1.63 mi) on the
Safety
Lead(II) sulfide is so insoluble that it is almost nontoxic, but pyrolysis of the material, as in smelting, gives dangerous toxic fumes of lead and oxides of sulfur.[18] Lead sulfide is insoluble and a stable compound in the pH of blood and so is probably one of the less toxic forms of lead.[19] A large safety risk occurs in the synthesis of PbS using lead carboxylates, as they are particularly soluble and can cause negative physiological conditions.
References
- ^ a b Haynes, p. 4.69
- ^ Linke, W. (1965). Solubilities. Inorganic and Metal-Organic Compounds. Vol. 2. Washington, D.C.: American Chemical Society. p. 1318.
- ISBN 978-1-56670-506-6.
- ^ Haynes, p. 4.128
- ^ Haynes, p. 4.135
- ^ Haynes, p. 9.63
- ^ Haynes, p. 4.141
- ^ Haynes, p. 5.25
- ISBN 978-0-521-21489-6.;
- ^ Hogan, C. Michael (2011). "Sulfur". in Encyclopedia of Earth, eds. A. Jorgensen and C.J. Cleveland, National Council for Science and the environment, Washington DC. Archived 2012-10-28 at the Wayback Machine
- ISBN 978-3527306732.
- .
- .
- .
- S2CID 98631978.
- .
- ^ "'Heavy metal' snow on Venus is lead sulfide". Washington University in St. Louis. Archived from the original on 2008-04-15. Retrieved 2009-07-07.
- ^ "Lead sulfide MSDS" (PDF). Archived from the original (PDF) on 2006-11-11. Retrieved 2009-11-20.
- ^ Bischoff, Fritz; Maxwell, L. C.; Evens, Richard D.; Nuzum, Franklin R. (1928). "Studies on the Toxicity of Various Lead Compounds Given Intravenously". Journal of Pharmacology and Experimental Therapeutics. 34 (1): 85–109.
Cited sources
- Haynes, William M., ed. (2016). ISBN 9781498754293.