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`!Selenium oxybromide`! (`F33f`_`[Se`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Selenium]`_`f`F33f`_`[O`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Oxygen]`_`f`F33f`_`[Br2`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Bromine]`_`f) is a `F33f`_`[selenium`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Selenium]`_`f `F33f`_`[oxohalide`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Oxohalide]`_`f `F33f`_`[chemical compound`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Chemical_compound]`_`f.`:cite-ref-g-e-2-0[`F5bf`_`[2`#cite-note-g-e-2]`_`f]

>>Contents

• `F0af`_`[Preparation`#preparation]`_`f

• `F0af`_`[Structure`#structure]`_`f

• `F0af`_`[Properties`#properties]`_`f

• `F0af`_`[References`#references]`_`f

-─

>>Preparation

Selenium oxybromide can be prepared through the reaction of `F33f`_`[selenium dioxide`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Selenium_dioxide]`_`f and `F33f`_`[selenium tetrabromide`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Selenium_tetrabromide]`_`f. Selenium and selenium dioxide are reacted with `F33f`_`[bromine`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Bromine]`_`f to form selenium monobromide and selenium tetrabromide. Dissolving the selenium dioxide in the tetrabromide will produce the oxybromide.`:cite-ref-lenher-1922-3-0[`F5bf`_`[3`#cite-note-lenher-1922-3]`_`f]

2 Se + Br2 → Se2Br2

Se2Br2 + 3 Br2 → 2 SeBr4

SeBr4 + SeO2 → 2 SeOBr2

>>Structure

Evidence from `F33f`_`[infrared`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Infrared_spectroscopy]`_`f and `F33f`_`[polarized Raman`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Raman_spectroscopy]`_`f spectroscopy suggests that selenium oxybromide adopts a `F33f`_`[pyramidal molecular geometry`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Trigonal_pyramidal_molecular_geometry]`_`f with `F33f`_`[Cs symmetry`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Molecular_symmetry]`_`f,`:cite-ref-4[`F5bf`_`[4`#cite-note-4]`_`f] like other chalcogen(IV) oxohalides such as `F33f`_`[thionyl bromide`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Thionyl_bromide]`_`f (SOBr2) and `F33f`_`[selenium oxydichloride`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Selenium_oxydichloride]`_`f (SeOCl2).`:cite-ref-g-e-2-1[`F5bf`_`[2`#cite-note-g-e-2]`_`f]

>>Properties

Selenium oxybromide is a reddish-brown solid with a low melting point (41.6 °C) and chemical properties similar to `F33f`_`[selenium oxychloride`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Selenium_oxychloride]`_`f. It boils at 220 °C and decomposes near the boiling point, making distillation an ineffective purification method. Its `F33f`_`[electrical conductivity`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Electrical_conductivity]`_`f in the liquid state just above the melting temperature is 6×10−5 S/m. SeOBr2 is `F33f`_`[hydrolyzed`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Hydrolyzed]`_`f by water to form `F33f`_`[H2SeO3`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Selenous_acid]`_`f and `F33f`_`[HBr`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Hydrobromic_acid]`_`f.

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.`:cite-ref-lenher-1922-3-1[`F5bf`_`[3`#cite-note-lenher-1922-3]`_`f]

>>References

`:cite-note-hand-1`!1.`! `:citereflide1998`aLide, David R. (1998). `*Handbook of Chemistry and Physics`* (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–81. `F33f`_`[ISBN`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=ISBN_(identifier)]`_`f 0-8493-0594-2.

`:cite-note-g-e-2`!2.`! `F0af`_`[↑`#cite-ref-g-e-2-0]`_`f `:citerefgreenwoodearnshaw1997`a`F33f`_`[Greenwood, Norman N.`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Norman_Greenwood]`_`f; Earnshaw, Alan (1997). `*Chemistry of the Elements`* (2nd ed.). `F33f`_`[Butterworth-Heinemann`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Butterworth-Heinemann]`_`f. p. 777. `F33f`_`[doi`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Doi_(identifier)]`_`f:10.1016/C2009-0-30414-6. `F33f`_`[ISBN`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=ISBN_(identifier)]`_`f 978-0-08-037941-8.

`:cite-note-lenher-1922-3`!3.`! `F0af`_`[↑`#cite-ref-lenher-1922-3-0]`_`f `:citereflenher1922`aLenher, Victor (1 August 1922). "Selenium oxybromide". `*Journal of the American Chemical Society`*. `!44`! (8): 1668–1673. `F33f`_`[doi`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Doi_(identifier)]`_`f:10.1021/ja01429a008.

`:cite-note-4`!4.`! `F0af`_`[↑`#cite-ref-4]`_`f `:citerefwilson1972`aWilson, William W. (1972). `*Vibrational spectroscopic studies of some simple and mixed selenium(iv) oxy-halides and pseudohalides`* (MSc). University of British Columbia. `F33f`_`[doi`:/page/wikibook/entry.mu`zim=wikipedia_en_all_nopic_2025-08.zim|entry_path=Doi_(identifier)]`_`f:10.14288/1.0061859.

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