What Is Bromide Used For
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| Names | |||
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| Systematic IUPAC proper name Bromide[ane] | |||
| Identifiers | |||
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| 3D model (JSmol) |
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| Beilstein Reference | 3587179 | ||
| ChEBI |
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| ChEMBL |
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| ChemSpider |
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| Gmelin Reference | 14908 | ||
| KEGG |
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| PubChem CID |
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| Properties | |||
| Chemic formula | Br− | ||
| Molar mass | 79.904 g·mol−ane | ||
| Cohabit acrid | Hydrogen bromide | ||
| Thermochemistry | |||
| Std molar | 82 J·mol−one·K−1 [two] | ||
| Std enthalpy of | −121 kJ·mol−1 [two] | ||
| Pharmacology | |||
| ATC code | N05CM11 (WHO) | ||
| Pharmacokinetics: | |||
| Biological one-half-life | 12 d | ||
| Related compounds | |||
| Other anions | Fluoride Chloride | ||
| Except where otherwise noted, data are given for materials in their standard land (at 25 °C [77 °F], 100 kPa). Infobox references | |||
A bromide ion is the negatively charged grade (Br− ) of the element bromine, a fellow member of the halogens group on the periodic table. Most bromides are colorless. Bromides accept many practical roles, existence found in anticonvulsants, flame-retardant materials, and cell stains.[3] Although uncommon, chronic toxicity from bromide tin can result in bromism, a syndrome with multiple neurological symptoms. Bromide toxicity tin also crusade a type of pare eruption. See potassium bromide. The bromide ion has an ionic radius of 196 pm.[4]
Natural occurrence [edit]
Bromide is present in typical seawater (35 PSU) with a concentration of around 65 mg/L, which is near 0.2% of all dissolved salts. Seafood and deep sea plants mostly accept higher levels than land-derived foods. Bromargyrite—natural, crystalline silverish bromide—is the virtually common bromide mineral known but is still very rare. In addition to silver, bromine is also in minerals combined with mercury and copper.[5]
Formation and reactions of bromide [edit]
Dissociation of bromide salts [edit]
Bromide salts of alkali metal, alkaline earth metals, and many other metals dissolve in water (and even some alcohols and a few ethers) to requite bromide ions. The classic instance is sodium bromide, which fully dissociates in water:
- NaBr → Na+ + Br−
Hydrogen bromide, which is a diatomic molecule, takes on salt-like backdrop upon contact with h2o to requite an ionic solution called hydrobromic acrid. The process is ofttimes described simplistically as involving formation of the hydronium table salt of bromide:
- HBr + H2O → H3O+ + Br−
Hydrolysis of bromine [edit]
Bromine readily reacts with water, i.e. information technology undergoes hydrolysis:
- Brii + HtwoO → HOBr + HBr
This forms hypobromous acid (HOBr), and hydrobromic acid (HBr in h2o). The solution is called "bromine water". The hydrolysis of bromine is more favorable in the presence of base, for case sodium hydroxide:
- Brii + NaOH → NaOBr + NaBr
This reaction is analogous to the production of bleach, where chlorine is dissolved in the presence of sodium hydroxide.[half-dozen]
Oxidation of bromide [edit]
One can test for a bromide ion by adding an oxidizer. One method uses dilute HNO3.
Balard and Löwig's method can be used to extract bromine from seawater and sure brines. For samples testing for sufficient bromide concentration, improver of chlorine produces bromine (Br2):[vii]
- Cl2 + two Br− → 2 Cl− + Brii
Applications [edit]
Bromide's main commercial value based on value and quantity is its use in producing organobromine compounds, which themselves are rather specialized. Organobromine compounds are mainly used equally burn retardants, and fifty-fifty these applications are controversial. Many metal bromides are produced commercially, including LiBr, NaBr, NHfourBr, CuBr, ZnBrtwo and AlBriii. Some applications are for silver-based photography, which is fading in value, and drilling fluid, which calls for generic, dense compounds and thus is of niggling value.[8]
Medicinal and veterinary uses [edit]
Folk and passé medicine [edit]
Lithium bromide was used as a sedative beginning in the early 1900s. However, it roughshod into disfavour in the 1940s due to the ascension popularity of safer and more than efficient sedatives (specifically, barbiturates) and when some heart patients died after using a salt substitute (see lithium chloride).[9] Like lithium carbonate and lithium chloride, information technology was used as a treatment for bipolar disorder.
Bromide compounds, especially potassium bromide, were oftentimes used every bit sedatives in the 19th and early 20th centuries. Their utilize in over-the-counter sedatives and headache remedies (such as Bromo-Seltzer) in the U.s.a. extended to 1975 when bromides were withdrawn as ingredients due to chronic toxicity.[10] This utilise gave the discussion "bromide" its colloquial connotation of a comforting cliche.[11]
It has been said that during World War I, British soldiers were given bromide to adjourn their sexual urges.[12] Lord Dunsany mentions a soldier being given bromide every bit a allaying for nervous burnout and overwork in his play Fame and the Poet (1919).[13]
Bromide salts are used in hot tubs equally mild germicidal agents to generate in situ hypobromite
The bromide ion is antiepileptic and every bit bromide salt, is used in veterinary medicine in the Usa. The kidneys excrete bromide ions. The half-life of bromide in the human torso (12 days) is long compared with many pharmaceuticals, making dosing challenging to adjust. (A new dose may require several months to achieve equilibrium.) Bromide ion concentrations in the cerebrospinal fluid are nearly 30% of those in blood and are strongly influenced past the body'south chloride intake and metabolism.[14]
Since bromide is still used in veterinary medicine in the United states, veterinary diagnostic labs can routinely measure out blood bromide levels. Yet, this is not a conventional exam in human medicine in the US since there are no FDA-approved uses for the bromide. Therapeutic bromide levels are measured in European countries similar Frg, where bromide is still used therapeutically in homo epilepsy.
Biochemistry [edit]
Bromide is rarely mentioned in the biochemical context. Some enzymes employ bromide as substrate or as a cofactor.
Substrate [edit]
Bromoperoxidase enzymes use bromide (typically in seawater) to generate electrophilic brominating agents. Hundreds of organobromine compounds are generated past this process. Notable examples are bromoform, thousands of tons of which are produced annually in this style. The historical dye Tyrian purple is produced by like enzymatic reactions.[15]
Cofactor [edit]
In ane specialized report, bromideis an essential cofactor in the peroxidising catalysis of sulfonimine crosslinks in collagen IV. This mail-translational modification occurs in all animals and bromine is an essential trace element for humans.[16]
Eosinophils need bromide for fighting multicellular parasites. Hypobromite is produced via eosinophil peroxidase, an enzyme that can use chloride just preferentially uses bromide.[17]
The average concentration of bromide in human claret in Queensland, Australia, is 5.3±1.4mg/L and varies with age and gender.[18] Much higher levels may bespeak exposure to brominated chemicals. It is likewise establish in seafood.
Further reading [edit]
Encyclopedia articles and books [edit]
- Christe, Grand., and Southward. Schneider (2020), Bromine, Encyclopædia Britannica.
- Emerson, S., and J. Hedges (2011), Chemical Oceanography and the Marine Carbon Bike, Cambridge Academy Press, Cambridge.
- Glasow, R. von, and C. Hughes (2014), Biogeochemical Cycles: Bromine, Encyclopedia of Atmospheric Sciences (Second Edition).
- Knight, J., and N. Schlager (2002), Real-life chemistry, Gale Group, Detroit, MI.
- Millero, F. J. (2013), Chemic oceanography, Taylor & Francis, Boca Raton.
- Newton D. E. (2010), Bromine (Revised), Chemical Elements: From Carbon to Krypton.
- Riley, J. P., G. Skirrow, and R. Chester (1975), Chemical Oceanography, Academic Press, London
- Ross, R. (2017), Facts Most Bromine, LiveScience.
- Steele, J. H., S. A. Thorpe, and K. Thou. Turekian (2001), Encyclopedia of Ocean Sciences, Academic Press, San Diego.
- Steele, J. H., South. A. Thorpe, and Thou. Chiliad. Turekian (2009), Encyclopedia of Bounding main Sciences, Academic Press, Boston.
- Watkins, T. (2011), Bromine, Environmental Encyclopedia.
Peer-reviewed journal articles for bromine (Br) [edit]
- Wisniak, J. (2002), The history of bromine from discovery to commodity, NOPR.
Peer-reviewed periodical articles for bromide (Br−) [edit]
- Anbar, A. D., Y. L. Yung, and F. P. Chavez (1996), Methyl bromide: Bounding main sources, body of water sinks, and climate sensitivity, AGU Journals.
- Foti, Southward. C., and Naval Ordnance Lab White Oak Md (1972), Concentration of Bromide Ions in Seawater by Isotopic Exchange with Mercurous Bromide, DTIC.
- Gribble, G. W. (2000), The natural product of organobromine compounds, Environmental Science and Pollution Enquiry, seven(one), 37–49, doi:x.1065/espr199910.002.
- Leri A. (2012), The Chemistry of Bromine in Terrestrial and Marine Environments, Science Highlight.
- Magazinovic, R. S., B. C. Nicholson, D. E. Mulcahy, and D. E. Davey (2004), Bromide levels in natural waters: its relationship to levels of both chloride and total dissolved solids and the implications for water treatment, Chemosphere, 57(four), 329–335, doi:10.1016/j.chemosphere.2004.04.056.
- Pilinis, C., D. B. Male monarch, and Due east. South. Saltzman (1996), The oceans: A source or a sink of methyl bromide?, Geophysical Inquiry Letters, 23(8), 817–820, doi:10.1029/96gl00424.
- Stemmler, I., I. Hense, and B. Quack (2015), Marine sources of bromoform in the global open up sea – global patterns and emissions, Biogeosciences, 12(half-dozen), 1967–1981, doi:x.5194/bg-12-1967-2015.
- Suzuki, A., Lim, L., Hiroi, T., & Takeuchi, T. (2006, March 20). Rapid decision of bromide in seawater samples past capillary ion chromatography using monolithic silica columns modified with cetyltrimethylammonium ion.
References [edit]
- ^ "Bromide – PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Data. Archived from the original on 2012-11-03.
- ^ a b Zumdahl, Steven South. (2009). Chemical Principles (6th ed.). Houghton Mifflin. ISBN978-0-618-94690-7.
- ^ Rattley, Matt (2012). "Ambiguous bromine". Nature Chemistry. iv (half dozen): 512. Bibcode:2012NatCh...4..512R. doi:10.1038/nchem.1361. PMID 22614389.
- ^ "Revised effective ionic radii and systematic studies of interatomic distances in halides and chalcogenides". Acta Crystallographica A. 32: 751–767. 1976. doi:10.1107/s0567739476001551.
- ^ "Mindat.org - Mines, Minerals and More". world wide web.mindat.org. Archived from the original on two March 2001. Retrieved 29 April 2018.
- ^ Chemistry of the Elements, North. Northward. Greenwood, A. Earnshaw, Elsevier, 2012, pp 789
- ^ Magazinovic, Rodney S; Nicholson, Brenton C; Mulcahy, Dennis E; Davey, David East (2004). "Bromide levels in natural waters: its human relationship to levels of both chloride and total dissolved solids and the implications for water handling". Chemosphere. 57 (4): 329–335. Bibcode:2004Chmsp..57..329M. doi:10.1016/j.chemosphere.2004.04.056. PMID 15312731. Archived from the original on 2021-05-25. Retrieved 2021-03-07 .
- ^ Dagani, Michael J.; Barda, Henry J.; Benya, Theodore J.; Sanders, David C. "Bromine Compounds". Ullmann'south Encyclopedia of Industrial Chemical science. Weinheim: Wiley-VCH. doi:x.1002/14356007.a04_405.
- ^ Bipolar disorder Archived 2022-02-24 at the Wayback Machine. webmd.com
- ^ Adams, Samuel Hopkins (1905). The Great American fraud. Printing of the American Medical Association. .
- ^ "the definition of bromide". Dictionary.com. Archived from the original on 24 Dec 2016. Retrieved 21 December 2016.
- ^ Tanaka, Yuki (2002) Japan'due south Comfort Women: Sexual slavery and prostitution during World War II and the U.s.a. Occupation, Routledge, p. 175. ISBN 0415194008.
- ^ Lord Dunsany (August 1919). "Fame and the Poet". The Atlantic Monthly: 175–183.
- ^ Goodman, Fifty. S.; Gilman, A., eds. (1970). "10. Hypnotics and Sedatives". The Biological Ground of Therapeutics (4th ed.). London: Macmillan. p. 121.
- ^ Gribble, Gordon West. (1999). "The diversity of naturally occurring organobromine compounds". Chemical Society Reviews. 28: 335–346. doi:10.1039/a900201d.
- ^ McCall, A. Scott; Cummings, Christopher F.; Bhave, Gautam; Vanacore, Roberto; Page-McCaw, Andrea; Hudson, Billy G. (2014). "Bromine Is an Essential Trace Element for Assembly of Collagen IV Scaffolds in Tissue Development and Architecture". Cell. 157 (6): 1380–1392. doi:x.1016/j.cell.2014.05.009. PMC4144415. PMID 24906154.
- ^ Mayeno, Arthur N.; Curran, A. Jane; Roberts, Robert L.; Foote, Christopher S. (1989-04-05). "Eosinophils Preferentially Use Bromide to Generate Halogenating Agents". Periodical of Biological Chemistry. 264 (10): 5660–5668. doi:10.1016/s0021-9258(18)83599-two. ISSN 0021-9258. PMID 2538427.
- ^ Olszowy, HA; Rossiter, J; Hegarty, J; Geoghegan, P (1998). "Background levels of bromide in human blood". Journal of Analytical Toxicology. 22 (three): 225–xxx. doi:x.1093/jat/22.iii.225. PMID 9602940.
What Is Bromide Used For,
Source: https://en.wikipedia.org/wiki/Bromide
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