Bismuth(III) sulfide
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| Names | |
|---|---|
| IUPAC name
Bismuth(III) sulfide | |
| Other names
Bismuth sulfide Dibismuth trisulfide | |
| Identifiers | |
1345-07-9  | |
| 3D model (Jmol) | Interactive image |
| ChemSpider | 141425 |
| ECHA InfoCard | 100.014.287 |
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| Properties | |
| Bi2S3 | |
| Molar mass | 514.16 g/mol |
| Appearance | brown powder |
| Density | 6.78 g/cm3[1] |
| Melting point | 850 ˚C[1] |
| insoluble | |
| Solubility | soluble in acids |
| Hazards | |
| Main hazards | Irritant |
| R-phrases | R36/37/38 |
| S-phrases | S26, S37 |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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| Infobox references | |
Bismuth(III) sulfide is a chemical compound of bismuth and sulfur. It occurs in nature as the mineral bismuthinite.
Synthesis
Bismuth(III) sulfide can be prepared by reacting a bismuth(III) salt with hydrogen sulfide:
- 2Bi3+ +3H2S → Bi2S3 + 6H+
Bismuth (III) sulfide can also be prepared by the reaction of elemental bismuth and elemental sulfur in an evacuated silica tube at 500 °C for 96 hours.
- 2Bi + 3S → Bi2S3
Properties
Bismuth(III) sulfide is isostructural with Sb2S3, stibnite. Bismuth atoms are in two different environments, both of which have 7 coordinate Bismuth atoms, 4 in a near planar rectangle and three more distant making an irregular 7-coordination group.[2]
It can react with acids to produce the odoriferous hydrogen sulfide gas.
Bismuth(III) sulfide may be produced in the body by the reaction of the common gastrointestinal drug bismuth subsalicylate with naturally-occurring sulfides; this causes temporary black tongue when the sulfides are in the mouth and black feces when the sulfides are in the colon.
Uses
It is used as a starting material to produce many other bismuth compounds. [3]
References
- 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
- ↑ Wells A.F. (1984) Structural Inorganic Chemistry, 5th edition Oxford Science Publications, ISBN 0-19-855370-6
- ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8