Selenium oxybromide (SeOBr<sub>2</sub>) is a selenium oxohalide chemical compound.
Selenium oxybromide can be prepared through the reaction of selenium dioxide and selenium tetrabromide. Selenium and selenium dioxide are reacted with bromine to form selenium monobromide and selenium tetrabromide. Dissolving the selenium dioxide in the tetrabromide will produce the oxybromide.
Evidence from infrared and polarized Raman spectroscopy suggests that selenium oxybromide adopts a pyramidal molecular geometry with C<sub>s</sub> symmetry, like other chalcogen(IV) oxohalides such as thionyl bromide () and selenium oxydichloride ().
Selenium oxybromide is a reddish-brown solid with a low melting point (41.6 ðC) and chemical properties similar to selenium oxychloride. It boils at 220 ðC and decomposes near the boiling point, making distillation an ineffective purification method. Its electrical conductivity in the liquid state just above the melting temperature is 6ÃÂ10<sup>âÂÂ5</sup> S/m. SeOBr<sub>2</sub> is hydrolyzed by water to form H<sub>2</sub>SeO<sub>3</sub> and HBr.
SeOBr<sub>2</sub> is highly reactive, with most reactions taking place in the liquid state. Selenium will dissolve in it, forming Se<sub>2</sub>Br<sub>2</sub>. Iron, copper, gold, platinum, and zinc are all attacked by SeOBr<sub>2</sub>.