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IUPAC name
Other names
bismuth trihydride
hydrogen bismuthide
18288-22-7 YesY
ChemSpider 8886 N
Jmol interactive 3D Image
PubChem 9242
Molar mass 212.00 g/mol
Appearance colourless gas
Density 0.008665 g/mL (20 °C)
Boiling point 16.8 °C (62.2 °F; 289.9 K) (extrapolated)
trigonal pyramidal
Related compounds
Related hydrides
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Infobox references

Bismuthine (IUPAC name: bismuthane) is the chemical compound with the formula BiH3. As the heaviest analogue of ammonia, BiH3 is unstable, decomposing to bismuth metal well below 0 °C. This compound adopts the expected pyramidal structure with H-Bi-H angles of around 90°.[1]

The term bismuthine may also refer to a member of the family of organobismuth(III) species having the general formula BiR
, where R is an organic substituent. For example, Bi(CH3)3 is trimethylbismuthine.

Preparation and properties[edit]

BiH3 is prepared by the redistribution of methylbismuthine (BiH2Me):[2]

3 BiH2Me → 2 BiH3 + BiMe3

The required BiH2Me, which is also thermally unstable, is generated by reduction of methylbismuth dichloride, BiCl2Me with LiAlH4.[1]

As suggested by the behavior of SbH3, BiH3 is unstable and decomposes to its constituent elements according to the following equation:

2 BiH3 → 3 H2 + 2 Bi (ΔHf'ogas = −278 kJ/mol)

The methodology used for detection of arsenic ("Marsh test") can also be used to detect BiH3. This test relies on the thermal decomposition of these trihydrides to the metallic mirrors of reduced As, Sb, and Bi. These deposits can be further distinguished by their distinctive solubility characteristics: arsenic dissolves in NaOCl, antimony dissolves in ammonium polysulfide, and bismuth resists both reagents.[2]

Uses and safety considerations[edit]

The low stability of BiH3 poses significant hazards and precludes technical applications, except as an intermediary product.


  1. ^ a b W. Jerzembeck, H. Bürger, L. Constantin, L. Margulès, J. Demaison, J. Breidung, W. Thiel (2002). "Bismuthine BiH3: Fact or Fiction? High-Resolution Infrared, Millimeter-Wave, and Ab Initio Studies". Angew. Chem. Int. Ed. 41 (14): 2550–2552. doi:10.1002/1521-3773(20020715)41:14<2550::AID-ANIE2550>3.0.CO;2-B. 
  2. ^ a b Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001.ISBN 0-12-352651-5.

External links[edit]