Selenium oxybromide

Selenium oxybromide
Selenium oxybromide
Selenium oxybromide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.247 Edit this at Wikidata
UNII
  • InChI=1S/Br2OSe/c1-4(2)3 checkY
    Key: ZWTYAOCEBBZVQQ-UHFFFAOYSA-N checkY
  • InChI=1/Br2OSe/c1-4(2)3
    Key: ZWTYAOCEBBZVQQ-UHFFFAOYAF
  • Br[Se](Br)=O
Properties
SeOBr2
Molar mass 254.77 g/mol
Appearance red-yellow solid
Density 3.38 g/cm3, solid
Melting point 41.6 °C (106.9 °F; 314.8 K)
Boiling point decomposes at 220 °C (428 °F; 493 K)
reacts
Solubility soluble in carbon disulfide, benzene, carbon tetrachloride[1]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Selenium oxybromide (SeOBr2) is a selenium oxohalide chemical compound.[2]

Preparation

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.[3]

2 Se + Br2 → Se2Br2
Se2Br2 + 3 Br2 → 2 SeBr4
SeBr4 + SeO2 → 2 SeOBr2

Structure

Evidence from infrared and polarized Raman spectroscopy suggests that selenium oxybromide adopts a pyramidal molecular geometry with Cs symmetry,[4] like other chalcogen(IV) oxohalides such as thionyl bromide (SOBr2) and selenium oxydichloride (SeOCl2).[2]

Properties

Selenium oxybromide is a reddish-brown solid with a low melting point (41.6 °C) and chemical properties similar to selenium oxychloride. It boils at 220 °C 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 6×10−5 S/m. SeOBr2 is hydrolyzed by water to form H2SeO3 and HBr.

SeOBr2 is highly reactive, with most reactions taking place in the liquid state. Selenium will dissolve in it, forming Se2Br2. Iron, copper, gold, platinum, and zinc are all attacked by SeOBr2.[3]

References

  1. ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–81. ISBN 0-8493-0594-2.
  2. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 777. ISBN 978-0-08-037941-8.
  3. ^ a b Lenher, Victor (1 August 1922). "Selenium oxybromide". Journal of the American Chemical Society. 44 (8): 1668–1673. doi:10.1021/ja01429a008.
  4. ^ Wilson, William W. (1972). Vibrational spectroscopic studies of some simple and mixed selenium(iv) oxy-halides and pseudohalides (MSc). University of British Columbia. doi:10.14288/1.0061859.

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