Lead(II) sulfide

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Lead(II) sulfide
Galena-unit-cell-3D-ionic.png
Sulfid olovnaty.PNG
Names
Other names
Plumbous sulfide
Galena, Sulphuret of lead
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.861 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 215-246-6
PubChem CID
RTECS number
  • OG4550000
UNII
UN number 3077
  • InChI=1S/Pb.S X mark.svgN
    Key: XCAUINMIESBTBL-UHFFFAOYSA-N X mark.svgN
  • [Pb]=S
Properties
PbS
Molar mass 239.30 g/mol
AppearanceBlack
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]
3.91 [5]
Structure [6]
Halite (cubic), cF8
Fm3m, No. 225
a = 5.936 Å
4
Octahedral (Pb2+)
Octahedral (S2−)
3.59 D [7]
Thermochemistry [8]
49.5 J/mol⋅K
Std molar
entropy (S⦵298)
91.2 J/mol
−100.4 kJ/mol
−98.7 kJ/mol
Hazards
GHS labelling:
GHS-pictogram-exclam.svg GHS-pictogram-silhouette.svg GHS-pictogram-pollu.svg
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)
NFPA 704.svgHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 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
2
0
0
Flash point Non-flammable
Safety data sheet (SDS) External MSDS
Related compounds
Other anions
Lead(II) oxide
Lead selenide
Lead telluride
Other cations
Carbon monosulfide
Silicon monosulfide
Germanium(II) sulfide
Tin(II) sulfide
Related compounds
 Thallium sulfide
Lead(IV) sulfide
Bismuth sulfide
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 Pb S. Galena is the principal ore and the most important compound of lead. It is a semiconducting material with niche uses.

Contents

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

Galena-based cat's-whisker detector used in the early 1900s CatWhisker.jpg
Galena-based cat's-whisker detector used in the early 1900s
World War II German PbS infrared detector German WWII PbS IR detector.jpg
World War II German PbS infrared detector

Photodetector

PbS was one of the first materials used for electrical diodes that could detect electromagnetic radiation, including infrared light. [16] As an infrared sensor, PbS directly detects light, as opposed to thermal detectors, which respond to a change in detector element temperature caused by the radiation. A PbS element can be used to measure radiation in either of two ways: by measuring the tiny photocurrent the photons cause when they hit the PbS material, or by measuring the change in the material's electrical resistance that the photons cause. Measuring the resistance change is the more commonly used method. At room temperature, PbS is sensitive to radiation at wavelengths between approximately 1 and 2.5 μm. This range corresponds to the shorter wavelengths in the infra-red portion of the spectrum, the so-called short-wavelength infrared (SWIR). Only very hot objects emit radiation in these wavelengths.

Cooling the PbS elements, for example using liquid nitrogen or a Peltier element system, shifts its sensitivity range to between approximately 2 and 4 μm. Objects that emit radiation in these wavelengths still have to be quite hot—several hundred degrees Celsius—but not as hot as those detectable by uncooled sensors. (Other compounds used for this purpose include indium antimonide (InSb) and mercury-cadmium telluride (HgCdTe), which have somewhat better properties for detecting the longer IR wavelengths.) The high dielectric constant of PbS leads to relatively slow detectors (compared to silicon, germanium, InSb, or HgCdTe).

Planetary science

Elevations above 2.6 km (1.63 mi) on the planet Venus are coated with a shiny substance. Though the composition of this coat is not entirely certain, one theory is that Venus "snows" crystallized lead sulfide much as Earth snows frozen water. If this is the case, it would be the first time the substance was identified on a foreign planet. Other less likely candidates for Venus' "snow" are bismuth sulfide and tellurium. [17]

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.

Related Research Articles

Photoconductivity is an optical and electrical phenomenon in which a material becomes more electrically conductive due to the absorption of electromagnetic radiation such as visible light, ultraviolet light, infrared light, or gamma radiation.

Sulfide (British English also sulphide) is an inorganic anion of sulfur with the chemical formula S2− or a compound containing one or more S2− ions. Solutions of sulfide salts are corrosive. Sulfide also refers to large families of inorganic and organic compounds, e.g. lead sulfide and dimethyl sulfide. Hydrogen sulfide (H2S) and bisulfide (SH−) are the conjugate acids of sulfide.

<span class="mw-page-title-main">Zinc sulfide</span> Inorganic compound

Zinc sulfide is an inorganic compound with the chemical formula of ZnS. This is the main form of zinc found in nature, where it mainly occurs as the mineral sphalerite. Although this mineral is usually black because of various impurities, the pure material is white, and it is widely used as a pigment. In its dense synthetic form, zinc sulfide can be transparent, and it is used as a window for visible optics and infrared optics.

<span class="mw-page-title-main">Lead(II) iodide</span> Chemical compound

Lead(II) iodide is a chemical compound with the formula PbI
2. At room temperature, it is a bright yellow odorless crystalline solid, that becomes orange and red when heated. It was formerly called plumbous iodide.

<span class="mw-page-title-main">Cadmium sulfide</span> Chemical compound

Cadmium sulfide is the inorganic compound with the formula CdS. Cadmium sulfide is a yellow salt. It occurs in nature with two different crystal structures as the rare minerals greenockite and hawleyite, but is more prevalent as an impurity substituent in the similarly structured zinc ores sphalerite and wurtzite, which are the major economic sources of cadmium. As a compound that is easy to isolate and purify, it is the principal source of cadmium for all commercial applications. Its vivid yellow color led to its adoption as a pigment for the yellow paint "cadmium yellow" in the 18th century.

<span class="mw-page-title-main">Sulfur monoxide</span> Chemical compound

Sulfur monoxide is an inorganic compound with formula SO. It is only found as a dilute gas phase. When concentrated or condensed, it converts to S2O2 (disulfur dioxide). It has been detected in space but is rarely encountered intact otherwise.

<span class="mw-page-title-main">Indium antimonide</span> Chemical compound

Indium antimonide (InSb) is a crystalline compound made from the elements indium (In) and antimony (Sb). It is a narrow-gap semiconductor material from the III-V group used in infrared detectors, including thermal imaging cameras, FLIR systems, infrared homing missile guidance systems, and in infrared astronomy. Indium antimonide detectors are sensitive to infrared wavelengths between 1 and 5 μm.

<span class="mw-page-title-main">Mercury sulfide</span> Chemical compound

Mercury sulfide, or mercury(II) sulfide is a chemical compound composed of the chemical elements mercury and sulfur. It is represented by the chemical formula HgS. It is virtually insoluble in water.

<span class="mw-page-title-main">Cadmium selenide</span> Chemical compound

Cadmium selenide is an inorganic compound with the formula CdSe. It is a black to red-black solid that is classified as a II-VI semiconductor of the n-type. It is a pigment, but applications are declining because of environmental concerns.

<span class="mw-page-title-main">Magnesium sulfide</span> Inorganic compound generated in the production of metallic iron

Magnesium sulfide is an inorganic compound with the formula MgS. It is a white crystalline material but often is encountered in an impure form that is brown and non-crystalline powder. It is generated industrially in the production of metallic iron.

<span class="mw-page-title-main">Lithium fluoride</span> Chemical compound

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. 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.

<span class="mw-page-title-main">Infrared detector</span>

An infrared detector is a detector that reacts to infrared (IR) radiation. The two main types of detectors are thermal and photonic (photodetectors).

<span class="mw-page-title-main">Platinum silicide</span> Chemical compound

Platinum silicide, also known as platinum monosilicide, is the inorganic compound with the formula PtSi. It is a semiconductor that turns into a superconductor when cooled to 0.8 K.

<span class="mw-page-title-main">Indium arsenide</span> Chemical compound

Indium arsenide, InAs, or indium monoarsenide, is a narrow-bandgap semiconductor composed of indium and arsenic. It has the appearance of grey cubic crystals with a melting point of 942 °C.

Lead selenide (PbSe), or lead(II) selenide, a selenide of lead, is a semiconductor material. It forms cubic crystals of the NaCl structure; it has a direct bandgap of 0.27 eV at room temperature. A grey solid, it is used for manufacture of infrared detectors for thermal imaging. The mineral clausthalite is a naturally occurring lead selenide.

Indium(III) sulfide (Indium sesquisulfide, Indium sulfide (2:3), Indium (3+) sulfide) is the inorganic compound with the formula In2S3.

<span class="mw-page-title-main">Quantum dot solar cell</span> Type of solar cell based on quantum dot devices

A quantum dot solar cell (QDSC) is a solar cell design that uses quantum dots as the captivating photovoltaic material. It attempts to replace bulk materials such as silicon, copper indium gallium selenide (CIGS) or cadmium telluride (CdTe). Quantum dots have bandgaps that are adjustable across a wide range of energy levels by changing their size. In bulk materials, the bandgap is fixed by the choice of material(s). This property makes quantum dots attractive for multi-junction solar cells, where a variety of materials are used to improve efficiency by harvesting multiple portions of the solar spectrum.

<span class="mw-page-title-main">Lead(IV) sulfide</span> Chemical compound

Lead(IV) sulfide is a chemical compound with the formula PbS2. This material is generated by the reaction of the more common lead(II) sulfide, PbS, with sulfur at >600 °C and at high pressures. PbS2, like the related tin(IV) sulfide SnS2, crystallises in the cadmium iodide motif, which indicates that Pb should be assigned the formal oxidation state of 4+.

A gas detector is a device that detects the presence of gases in an area, often as part of a safety system. A gas detector can sound an alarm to operators in the area where the leak is occurring, giving them the opportunity to leave. This type of device is important because there are many gases that can be harmful to organic life, such as humans or animals.

Quantum dots (QDs) are semiconductor nanoparticles with a size less than 10 nm. They exhibited size-dependent properties especially in the optical absorption and the photoluminescence (PL). Typically, the fluorescence emission peak of the QDs can be tuned by changing their diameters. So far, QDs were consisted of different group elements such as CdTe, CdSe, CdS in the II-VI category, InP or InAs in the III-V category, CuInS2 or AgInS2 in the I–III–VI2 category, and PbSe/PbS in the IV-VI category. These QDs are promising candidates as fluorescent labels in various biological applications such as bioimaging, biosensing and drug delivery.

References

  1. 1 2 Haynes, p. 4.69
  2. ↑ Linke, W. (1965). Solubilities. Inorganic and Metal-Organic Compounds. Vol. 2. Washington, D.C.: American Chemical Society. p. 1318.
  3. ↑ Ronald Eisler (2000). Handbook of Chemical Risk Assessment. CRC Press. ISBN   978-1-56670-506-6.
  4. ↑ Haynes, p. 4.128
  5. ↑ Haynes, p. 4.135
  6. ↑ Haynes, p. 4.141
  7. ↑ Haynes, p. 9.63
  8. ↑ Haynes, p. 5.25
  9. ↑ Vaughan, D. J.; Craig, J. R. (1978). Mineral Chemistry of Metal Sulfides. Cambridge: Cambridge University Press. ISBN   978-0-521-21489-6.;
  10. ↑ 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
  11. ↑ Sutherland, Charles A.; Milner, Edward F.; Kerby, Robert C.; Teindl, Herbert; Melin, Albert; Bolt, Hermann M. (2005). "Lead". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_193.pub2. ISBN   978-3527306732.
  12. ↑ "The Quantum Mechanics of Larger Semiconductor Clusters ("Quantum Dots")". Annual Review of Physical Chemistry. 41 (1): 477–496. 1990-01-01. Bibcode:1990ARPC...41..477B. doi:10.1146/annurev.pc.41.100190.002401.
  13. ↑ Zhou, H. S.; Honma, I.; Komiyama, H.; Haus, Joseph W. (2002-05-01). "Coated semiconductor nanoparticles; the cadmium sulfide/lead sulfide system's synthesis and properties". The Journal of Physical Chemistry. 97 (4): 895–901. doi:10.1021/j100106a015.
  14. ↑ Wang, Wenzhong; Liu, Yingkai; Zhan, Yongjie; Zheng, Changlin; Wang, Guanghou (2001-09-15). "A novel and simple one-step solid-state reaction for the synthesis of PbS nanoparticles in the presence of a suitable surfactant". Materials Research Bulletin. 36 (11): 1977–1984. doi:10.1016/S0025-5408(01)00678-X.
  15. ↑ Lee, HyoJoong; Leventis, Henry C.; Moon, Soo-Jin; Chen, Peter; Ito, Seigo; Haque, Saif A.; Torres, Tomas; Nüesch, Frank; Geiger, Thomas (2009-09-09). "PbS and CdS Quantum Dot-Sensitized Solid-State Solar Cells: "Old Concepts, New Results"". Advanced Functional Materials. 19 (17): 2735–2742. doi: 10.1002/adfm.200900081 . ISSN   1616-3028. S2CID   98631978.
  16. ↑ Putley, E H; Arthur, J B (1951). "Lead Sulphide – An Intrinsic Semiconductor". Proceedings of the Physical Society. Series B. 64 (7): 616–618. doi:10.1088/0370-1301/64/7/110.
  17. ↑ "'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.
  18. ↑ "Lead sulfide MSDS" (PDF). Archived from the original (PDF) on 2006-11-11. Retrieved 2009-11-20.
  19. ↑ 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.

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