Selenium oxybromide
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3D model (JSmol)
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| 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).
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Template:Chembox Footer/trackingTemplate:Short description
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 (Page Module:Chem2/styles.css has no content.SOBr2) and selenium oxydichloride (Page Module:Chem2/styles.css has no content.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
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- ^ Page Module:Citation/CS1/styles.css has no content.Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–81. ISBN 0-8493-0594-2.
- ^ a b Page Module:Citation/CS1/styles.css has no content.Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 777. doi:10.1016/C2009-0-30414-6. ISBN 978-0-08-037941-8.
- ^ a b Page Module:Citation/CS1/styles.css has no content.Lenher, Victor (1 August 1922). "Selenium oxybromide". Journal of the American Chemical Society. 44 (8): 1668–1673. doi:10.1021/ja01429a008.
- ^ Page Module:Citation/CS1/styles.css has no content.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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