| Identification | Back Directory | [Name]
diboron trisulphide | [CAS]
12007-33-9 | [Synonyms]
diboron trisulphide | [EINECS(EC#)]
234-504-9 | [Molecular Formula]
B2S3 | [MDL Number]
MFCD00058743 | [MOL File]
12007-33-9.mol | [Molecular Weight]
117.817 |
| Chemical Properties | Back Directory | [Melting point ]
310℃ [AES93] | [density ]
1.550 | [solubility ]
sol ethanol, but decomposes | [form ]
yellow amorphous solid | [color ]
yellow amorphous solid | [crystal system]
Monoclinic | [Space group]
P21/c | [Lattice constant]
| a/nm | b/nm | c/nm | α/o | β/o | γ/o | V/nm3 | | 0.4039 | 1.0722 | 1.862 | 90 | 96.23 | 90 | 0.8016 |
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| Hazard Information | Back Directory | [Chemical Properties]
Boron trisulfide, also known as boron sulfide or diboron trisulphide, is a white crystal or amorphous powder with a relative density of 1.55 and a melting point of 310℃. When heated, it turns into a sticky paste. When exposed to humid air, it decomposes and is slightly soluble in phosphorus trichloride and sulfur dichloride. Furthermore, it readily undergoes hydrolysis, producing boric acid and hydrogen sulfide. Additionally, it decomposes upon contact with alcohol.
| [Uses]
Boron sulfide has been used in organic synthesis
to reduce sulfoxides to thiols, and to convert
ketones to thioketones. The sulfide
glasses, M2S→B2S3, where M is Li or Na, have
electrical conductivities 103 times greater than
the corresponding oxide glasses. Electrically conducting boron sulfide glasses have also
been made incorporating LiI and other
glass-forming sulfides. These glasses
have potential as electrolytes in batteries or fuel
cells. | [Preparation]
Boron sulfide is obtained by placing fine powdered iron boride into a reaction tube and reacting it with hydrogen sulfide gas.? | [Precautions]
Boron sulfide is very flammable under air and immediately reacts with water to give boric acid and hydrogen sulfide.
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