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| Names | |||
|---|---|---|---|
| Systematic IUPAC name
Bromide[1] | |||
| Identifiers | |||
3D model (JSmol)
|
|||
| 3587179 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| 14908 | |||
| KEGG | |||
PubChem CID
|
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| UNII | |||
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| |||
| Properties | |||
| Br− | |||
| Molar mass | 79.904 g·mol−1 | ||
| Conjugate acid | Hydrogen bromide | ||
| Thermochemistry | |||
Std molar
entropy (S⦵298) |
82 J·mol−1·K−1[2] | ||
Std enthalpy of
formation (ΔfH⦵298) |
−121 kJ·mol−1[2] | ||
| Pharmacology | |||
| N05CM11 (WHO) | |||
| Pharmacokinetics: | |||
| 12 d | |||
| Related compounds | |||
Other anions
|
Fluoride | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |||
A bromide ion is the negatively charged form (Br−) of the element bromine, a member of the halogens group on the periodic table. Most bromides are colorless. Bromides have many practical roles, being found in anticonvulsants, flame-retardant materials, and cell stains.[3] Although uncommon, chronic toxicity from bromide can result in bromism, a syndrome with multiple neurological symptoms. Bromide toxicity can also cause a type of skin eruption, see potassium bromide. The bromide ion has an ionic radius of 196 pm.[4]
- ^ "Bromide – PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information. Archived from the original on 2012-11-03.
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin. ISBN 978-0-618-94690-7.
- ^ Rattley, Matt (2012). "Ambiguous bromine". Nature Chemistry. 4 (6): 512. Bibcode:2012NatCh...4..512R. doi:10.1038/nchem.1361. PMID 22614389.
- ^ Shannon, R. D. (1976). "Revised effective ionic radii and systematic studies of interatomic distances in halides and chalcogenides". Acta Crystallographica A. 32 (5): 751–767. Bibcode:1976AcCrA..32..751S. doi:10.1107/s0567739476001551.