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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.

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.

Boron sulfide is obtained by placing fine powdered iron boride into a reaction tube and reacting it with hydrogen sulfide gas.?

Boron sulfide is very flammable under air and immediately reacts with water to give boric acid and hydrogen sulfide.