Selenium tetrabromide

From Wikipedia, the free encyclopedia
Names
IUPAC name
Tetrabromo-λ4-selane
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.256 Edit this at Wikidata
EC Number
  • 232-181-9
UNII
  • InChI=1S/Br4Se/c1-5(2,3)4
    Key: VTQZBGAODFEJOW-UHFFFAOYSA-N
  • InChI=1/Br4Se/c1-5(2,3)4
    Key: VTQZBGAODFEJOW-UHFFFAOYAY
  • Br[Se](Br)(Br)Br
Properties
SeBr4
Molar mass 398.576
Density 4.029 g/cm3
Melting point 75 °C (167 °F; 348 K) (dissolves)
Boiling point 115 °C (239 °F; 388 K) (sublimes)
Structure[1]
trigonal (α)
monoclinic (β)
P31c, No. 159 (α)
C2/c, No.15 (β)
16
Hazards
GHS labelling:
GHS05: CorrosiveGHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard
Signal word
 Danger
H301, H311, H314, H331, H351, H373, H410
P201, P202, P260, P261, P264, P270, P271, P273, P280, P281, P301+P310, P301+P330+P331, P302+P352, P303+P361+P353, P304+P340, P305+P351+P338, P308+P313, P310, P311, P312, P314, P321, P322, P330, P361, P363, P391, P403+P233, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Selenium tetrabromide is an inorganic compound with a chemical formula SeBr4.

Preparation[]

Selenium tetrabromide could be produced by mixing elemental bromine and selenium:[2][3]

Properties[]

Selenium tetrabromide exists in two polymorphs, the trigonal, black α-SeBr4 and the monoclinic, orange-reddish β-SeBr4, both of which feature tetrameric cubane-like Se4Br16 units but differ in how they are arranged.[1] It dissolves in carbon disulfide, chloroform and ethyl bromide, but decomposes in water,[4] so that it produces selenous acid in wet air.

The compound is only stable under a bromine-saturated atmosphere; gas phase measurements of the gas density indicate that the compound decomposes into selenium monobromide and bromine.[3]

References[]

  1. ^ a b Born, Ref. P.; Kniep, R.; Mootz, D. (1979). "Phasenbeziehungen im System Se-Br und die Kristallstrukturen des dimorphen SeBr4". Z. Anorg. Allg. Chem. 451 (1): 12–24. doi:10.1002/zaac.19794510103.
  2. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 772–774. ISBN 978-0-08-037941-8.
  3. ^ a b Tideswell, N. W.; McCullough, J. D. (1956). "Selenium Bromides. I. A Spectrophotometric Study of the Dissociation of Selenium Tetrabromide and Selenium Dibromide in Carbon Tetrachloride Solution1,2". Journal of the American Chemical Society. 78 (13): 3026–3029. doi:10.1021/ja01594a025.
  4. ^ Perry, Dale L. (2011). Handbook of Inorganic Compounds. CRC Press. p. 360. ISBN 978-1-4398-1461-1.
Stub icon

This inorganic compound–related article is a stub. You can help Wikipedia by .

  • v
  • t
Retrieved from ""