This page uses content from Wikipedia and is licensed under CC BY-SA.

Bismuth(III) sulfide

Bismuth(III) sulfide
Bismuth(III) sulfide
IUPAC name
Bismuth(III) sulfide
Other names
Bismuth sulfide
Dibismuth trisulfide
3D model (JSmol)
ECHA InfoCard 100.014.287
EC Number
  • 215-716-0
Molar mass 514.16 g/mol
Appearance brown powder
Density 6.78 g/cm3[1]
Melting point 850 ˚C[1]
Solubility soluble in acids
-123.0·10−6 cm3/mol
Main hazards Irritant
GHS pictograms GHS07: Harmful
GHS Signal word Warning
H315, H319, H335
P261, P264, P271, P280, P302+352, P304+340, P305+351+338, P312, P321, P332+313, P337+313, P362, P403+233, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references

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


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


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.


It is used as a starting material to produce many other bismuth compounds.[3]


  1. ^ a b 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