Bismuth(III) sulfide

Bismuth(III) sulfide (Bi2S3) is a chemical compound of bismuth and sulfur. It occurs in nature as the mineral bismuthinite.

Bismuth(III) sulfide
Names
IUPAC name
Bismuth(III) sulfide
Other names
Bismuth sulfide
Dibismuth trisulfide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.014.287
EC Number
  • 215-716-0
UNII
  • InChI=1S/2Bi.3S/q2*+3;3*-2 checkY
    Key: YNRGZHRFBQOYPP-UHFFFAOYSA-N checkY
  • InChI=1/2Bi.3S/q2*+3;3*-2
    Key: YNRGZHRFBQOYPP-UHFFFAOYAA
  • [BiH3+3].[BiH3+3].[S-2].[S-2].[S-2]
Properties
Bi2S3
Molar mass 514.14 g·mol−1
Appearance brown powder
Density 6.78 g/cm3[1]
Melting point 850 ˚C[1]
insoluble
Solubility soluble in acids
-123.0·10−6 cm3/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Irritant
GHS labelling:
GHS07: Exclamation mark
Warning
H315, H319, H335
P261, P264, P271, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P332+P313, P337+P313, P362, P403+P233, P405, P501
Related compounds
Other anions
 Bismuth(III) oxide
Bismuth selenide
Bismuth telluride
Other cations
 Arsenic trisulfide
Antimony trisulfide
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

Synthesis

Bismuth(III) sulfide can be prepared by reacting a bismuth(III) salt with hydrogen sulfide:

2 Bi3+ + 3 H2S → Bi2S3 + 6 H+

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.

2 Bi + 3 S → Bi2S3

Properties

Bismuth(III) sulfide is isostructural with stibnite (stibnite is one of the forms of antimony(III) sulfide). 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. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  2. Wells A.F. (1984) Structural Inorganic Chemistry, 5th edition Oxford Science Publications, ISBN 0-19-855370-6
  3. Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
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