Mercury sulfide
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| Names | |
|---|---|
| IUPAC name
Mercury sulfide
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| Other names | |
| Identifiers | |
| ECHA InfoCard | 100.014.270 |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| HgS | |
| Molar mass | 232.66 g/mol |
| Density | 8.10 g/cm3 |
| Melting point | 580 °C decomp. |
| insoluble | |
| Band gap | 2.1 eV (direct, α-HgS) [1] |
Refractive index (nD)
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w=2.905, e=3.256, bire=0.3510 (α-HgS) [2] |
| Thermochemistry | |
Std molar
entropy (S⦵298) |
78 J·mol−1·K−1[3] |
Std enthalpy of
formation (ΔfH⦵298) |
−58 kJ·mol−1[3] |
| Hazards | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
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Mercury oxide Mercury selenide Mercury telluride |
Other cations
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Zinc sulfide Cadmium 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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Mercury sulfide, mercuric sulfide, mercury sulphide, 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.[4]
Crystal structure
HgS is dimorphic with two crystal forms:
- red cinnabar (α-HgS, hexagonal, hP6, P3221), is the form in which mercury is most commonly found in nature.
- black, metacinnabar (β-HgS), is less common in nature and adopts the zinc blende (T2d-F43m) crystal structure.
Crystals of red, α-HgS, are optically active. This is caused by the Hg-S helices in the structure.[5]
Preparation and chemistry
β-HgS is precipitated as a black powder when H2S is bubbled through solutions of Hg(II) salts.[6] β-HgS is unreactive to all but concentrated acids.[4]
Mercury metal is produced from the cinnabar ore by roasting in air and condensing the vapour.[4]
Uses
α-HgS is used as a red pigment when it is known as vermilion. Vermilion is known to darken and this has been ascribed to conversion from red α-HgS to black β-HgS. Investigations at Pompeii where red walls when originally excavated have darkened has been ascribed to the formation of Hg-Cl compounds (e.g., corderoite, calomel, and terlinguaite) and calcium sulfate, gypsum, rather than β-HgS, which was not detected.[7]
See also
References
- ^ L. I. Berger, Semiconductor Materials (1997) CRC Press ISBN 0-8493-8912-7
- ^ Webminerals
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 0-618-94690-X.
- ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 1406. ISBN 978-0-08-022057-4.
- ^
Glazer, A. M. (1986). "On the origin of optical activity in crystal structures". J. Appl. Cryst. 19 (2): 108–122. doi:10.1107/S0021889886089823.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5
- ^
Cotte, M (2006). "Blackening of Pompeian Cinnabar Paintings: X-ray Microspectroscopy Analysis". Anal. Chem. 78 (21): 7484–7492. doi:10.1021/ac0612224. PMID 17073416.
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