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Revision as of 10:04, 1 November 2011 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Script assisted update of identifiers for the Chem/Drugbox validation project (updated: 'KEGG', 'CASNo').← Previous edit		Latest revision as of 02:18, 14 October 2024 edit undoDrmies (talk | contribs)Autopatrolled, Checkusers, Oversighters, Administrators406,746 edits there is no point in citing a playTags: Mobile edit Mobile app edit iOS app edit App section source
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			{{Short description|Chemical compound or ion}}
			{{Other uses}}
			<!-- sometimes excessively wordy or uses weird phrasing -->
	{{Chembox		{{Chembox
			|ImageFileL1 = Br-.svg
	| Verifiedfields = changed
			|ImageSizeL1 = 50px
	| Watchedfields = changed
			|ImageFileR1 = Bromide ion.svg
	| verifiedrevid = 406458537
			|ImageSizeR1 = 60px
	| SystematicName = Bromide<ref>{{Cite web|title = Bromide - PubChem Public Chemical Database|url = http://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=259|work = The PubChem Project|location = USA|publisher = National Center for Biotechnology Information}}</ref>
			|Verifiedfields = changed
	| Section1 = {{Chembox Identifiers
	| CASNo_Ref = {{cascite|changed|??}}		|Watchedfields = changed
			|verifiedrevid = 458436846
	| CASNo = <!-- blanked - oldvalue: 24959-67-9 -->
			|SystematicName = Bromide<ref>{{Cite web|title = Bromide – PubChem Public Chemical Database|url = https://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=259|work = The PubChem Project|location = USA|publisher = National Center for Biotechnology Information|url-status = live|archive-url = https://web.archive.org/web/20121103072332/https://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=259|archive-date = 2012-11-03}}</ref>
	| PubChem = 259
			|Section1={{Chembox Identifiers
	| PubChem_Ref = {{Pubchemcite|correcyt|pubchem}}
			|CASNo_Ref = {{cascite|correct|CAS}}
	| ChemSpiderID = 254
			|CASNo = 24959-67-9
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
			|UNII_Ref = {{fdacite|correct|FDA}}
	| KEGG = <!-- blanked - oldvalue: C01324 -->
			|UNII = 952902IX06
	| KEGG_Ref = {{keggcite|changed|kegg}}
			|PubChem = 259
	| ChEBI_Ref = {{ebicite|changed|EBI}}
			|ChemSpiderID = 254
	| ChEBI = 15858
			|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChEMBL = 11685
			|KEGG = C01324
	| ChEMBL_Ref = {{ebicite|correct|EBI}}
			|KEGG_Ref = {{keggcite|changed|kegg}}
	| Beilstein = 3587179
			|ChEBI_Ref = {{ebicite|correct|EBI}}
	| Gmelin = 14908
	| SMILES =		|ChEBI = 15858
			|ChEMBL = 11685
	| StdInChI = 1S/BrH/h1H/p-1
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}		|ChEMBL_Ref = {{ebicite|correct|EBI}}
			|Beilstein = 3587179
	| StdInChIKey = CPELXLSAUQHCOX-UHFFFAOYSA-M
			|Gmelin = 14908
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
			|SMILES =
			|StdInChI = 1S/BrH/h1H/p-1
			|StdInChI_Ref = {{stdinchicite|correct|chemspider}}
			|StdInChIKey = CPELXLSAUQHCOX-UHFFFAOYSA-M
			|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	}}		}}
	| Section2 = {{Chembox Properties		|Section2={{Chembox Properties
	| Formula = Br<sup>-</sup>		|Formula = Br<sup>−</sup>
	| MolarMass = 79.904 g mol<sup>-1</sup>		|MolarMass = 79.904&nbsp;g·mol<sup>−1</sup>
			|ConjugateAcid = ]
	| ExactMass = 78.918337647 g mol<sup>-1</sup>
			}}
			|Section6={{Chembox Pharmacology
			|ATCCode_prefix = N05
			|ATCCode_suffix = CM11
			|HalfLife = 12 d}}
			|Section5={{Chembox Thermochemistry
			|DeltaHf = −121&nbsp;kJ·mol<sup>−1</sup><ref name=b1>{{cite book| last= Zumdahl |first=Steven S.|title =Chemical Principles |edition=6th | publisher = Houghton Mifflin | year = 2009| isbn = 978-0-618-94690-7}}</ref>
			|Entropy = 82&nbsp;J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=b1/>
			}}
			|Section8={{Chembox Related
			|OtherAnions = ]<br />
			]<br />
			]
	}}		}}
	| Section3 = {{Chembox Pharmacology
	| HalfLife = 12 d}}
	}}		}}
			A '''bromide''' ] is the negatively charged form ('''Br<sup>−</sup>''') of the element ], a member of the ] on the ]. Most bromides are colorless. Bromides have many practical roles, being found in anticonvulsants, flame-retardant materials, and cell stains.<ref>{{cite journal |doi=10.1038/nchem.1361|title=Ambiguous bromine|year=2012|last1=Rattley|first1=Matt|journal=Nature Chemistry|volume=4|issue=6|page=512|pmid=22614389|bibcode=2012NatCh...4..512R|doi-access=free}}</ref> Although uncommon, chronic toxicity from bromide can result in ], a syndrome with multiple neurological symptoms. Bromide toxicity can also cause a type of skin eruption, see ]. The bromide ion has an ] of 196&nbsp;pm.<ref>{{cite journal|title=Revised effective ionic radii and systematic studies of interatomic distances in halides and chalcogenides |journal=Acta Crystallographica A |date=1976 |volume=32 |pages=751–767 |doi=10.1107/s0567739476001551|last1=Shannon |first1=R. D. |issue=5 |bibcode=1976AcCrA..32..751S }}</ref>
	{{Other uses2|bromide}}
	A '''bromide''' is a chemical compound containing bromide ], that is ] atom with effective ] of −1. The class name can include ]ic compounds such as ] or ] compounds such as ].
	==Natural occurrence==		==Natural occurrence==
	Bromide is present in typical ] (35 ]) with a concentration of around 65&nbsp;mg/L, which is around 0.2% of all dissolved ]s. Seafoods generally have high levels of bromide, while foods derived from land have variable amounts.		Bromide is present in typical ] (35&nbsp;]) with a concentration of around 65&nbsp;mg/L, which is about 0.2% of all dissolved ]s. Seafood and deep sea plants generally have higher levels than land-derived foods. ]—natural, crystalline silver bromide—is the most common bromide mineral known but is still very rare. In addition to silver, bromine is also in minerals combined with mercury and copper.<ref>{{cite web|url=https://www.mindat.org|title=Mindat.org - Mines, Minerals and More|website=www.mindat.org|access-date=29 April 2018|url-status=live|archive-url=https://web.archive.org/web/20010302042623/https://www.mindat.org/|archive-date=2 March 2001}}</ref>
			==Formation and reactions of bromide==
	==Chemistry==
			===Dissociation of bromide salts===
	One can test for a bromide ion by adding dilute ] (HNO<sub>3</sub>), then ] (AgNO<sub>3</sub>). A cream precipitate forms.
			Bromide salts of ], ]s, and many other metals dissolve in water (and even some alcohols and a few ethers) to give bromide ions. The classic case is sodium bromide, which fully dissociates in water:
			:NaBr → Na<sup>+</sup> + Br<sup>−</sup>
			Hydrogen bromide, which is a ], takes on salt-like properties upon contact with water to give an ionic solution called ]. The process is often described simplistically as involving formation of the hydronium salt of bromide:
	==Medical uses==
			:HBr + H<sub>2</sub>O → H<sub>3</sub>O<sup>+</sup> + Br<sup>−</sup>
	{{Main|potassium bromide}}
			===Hydrolysis of bromine===
	Bromide compounds, especially ], were frequently used as sedatives in the 19th and early 20th century. Their use in over the counter sedatives and headache remedies (such as ]) in the United States extended to 1975, when these bromides were withdrawn as ingredients, due to ].<ref>{{citation | url =http://books.google.com/books?id=fd_S2Van52EC&dq=%22The+Great+American+Fraud%22&printsec=frontcover&source=bn&hl=en&ei=c0jPS5uZFYG0lQfBp-GgCw&sa=X&oi=book_result&ct=result&resnum=4&ved=0CBkQ6AEwAw#v=twopage&q&f=true | title = The Great American fraud}}.</ref>
			Bromine readily reacts with water, i.e. it undergoes hydrolysis:
			:Br<sub>2</sub> + H<sub>2</sub>O → HOBr + HBr
			This forms ] (HOBr), and ] (HBr in water). The solution is called "]". The hydrolysis of bromine is more favorable in the presence of base, for example ]:
	This use gave the word "bromide" its colloquial connotation of a boring ], a bit of ] overused as a calming phrase, or verbal ].
			:Br<sub>2</sub> + NaOH → NaOBr + NaBr
	The bromide ion is antiepileptic, and bromide salts are still used as such, particularly in veterinary medicine. Bromide ion is excreted by the kidneys. The half-life of bromide in the human body (12 days) is long compared with many pharmaceuticals, making dosing difficult to adjust (a new dose may require several months to reach equilibrium). Bromide ion concentrations in the cerebrospinal fluid are about 30% of those in blood, and are strongly influenced by the body's chloride intake and metabolism.<ref>Goodman and Gilman, ''The Biological Basis of Therapeutics'', Fourth Edition, Chapter 10 (''Hypnotics and Sedatives''), p. 121, The MacMillan Co., London, 1970.</ref>
			This reaction is analogous to the production of ], where chlorine is dissolved in the presence of sodium hydroxide.<ref>Chemistry of the Elements, N. N. Greenwood, A. Earnshaw, Elsevier, 2012, pp 789</ref>
			===Oxidation of bromide===
	Since bromide is still used in veterinary medicine (particularly to treat seizures in dogs) in the United States, veterinary diagnostic labs can routinely measure blood bromide levels. However, this is not a conventional test in human medicine in the U.S., since there are no FDA-approved uses for bromide, and it is no longer available in over-the-the-counter sedatives. Therapeutic bromide levels are measured in European countries like Germany, where bromide is still used therapeutically in human epilepsy.
			One can test for a bromide ion by adding an oxidizer. One method uses dilute ].
			Balard and Löwig's method can be used to extract bromine from seawater and certain brines. For samples testing for sufficient bromide concentration, addition of chlorine produces bromine (Br<sub>2</sub>):<ref>{{Cite journal |last1 = Magazinovic |first1 = Rodney S. |last2 = Nicholson |first2 = Brenton C. |last3 = Mulcahy |first3 = Dennis E. |last4 = Davey |first4 = David E. |date = 2004 |title = Bromide levels in natural waters: its relationship to levels of both chloride and total dissolved solids and the implications for water treatment |url = https://linkinghub.elsevier.com/retrieve/pii/S0045653504003935 |journal = Chemosphere |language = en |volume = 57 |issue = 4 |pages = 329–335 |doi = 10.1016/j.chemosphere.2004.04.056 |pmid = 15312731 |bibcode = 2004Chmsp..57..329M |access-date = 2021-03-07 |archive-date = 2021-05-25 |archive-url =https://web.archive.org/web/20210525180633/https://linkinghub.elsevier.com/retrieve/pii/S0045653504003935 |url-status = live}}</ref>
	Chronic toxicity from bromide can result in ], a syndrome with multiple neurological symptoms. Bromide toxicity can also cause a type of skin eruption. See ].
			:Cl<sub>2</sub> + 2&nbsp;Br<sup>−</sup> → 2&nbsp;Cl<sup>−</sup> + Br<sub>2</sub>
			==Applications==
	] was used as a ] beginning in the early 1900s, but it fell into disfavor in the 1940s when some heart patients died after using it as a salt substitute.<ref></ref> Like ] and ] it was used as treatment for ].
			Bromide's main commercial value is its use in producing ]s, which themselves are rather specialized. Organobromine compounds are commonly used as ].<ref>Michael J. Dagani, Henry J. Barda, Theodore J. Benya, David C. Sanders: ''Bromine Compounds'', Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. {{doi|10.1002/14356007.a04_405}}</ref> Some brominated flame retardants were identified as ] to both humans and the environment and were suspected of causing ] and ].<ref>{{cite web |url=http://www.epa.gov/oppt/existingchemicals/pubs/actionplans/pbde.html |title=Polybrominated Diphenyl Ethers (PBDEs) Action Plan Summary &#124; Existing Chemicals &#124; OPPT &#124; US EPA |access-date=2012-12-03 |url-status=live |archive-url=https://web.archive.org/web/20150901200633/http://www.epa.gov/oppt/existingchemicals/pubs/actionplans/pbde.html |archive-date=2015-09-01 }}</ref><ref>{{cite web |url=http://www.cerc.usgs.gov/pubs/center/pdfdocs/pbde.pdf |title=Brominated Flame Retardants in the Environment |publisher=Columbia Environmental Research Center |access-date=2012-12-03 |url-status=live |archive-url=https://web.archive.org/web/20160508170026/http://www.cerc.usgs.gov/pubs/center/pdfDocs/PBDE.pdf |archive-date=2016-05-08 }}</ref>
			Many metal bromides are produced commercially, including ], ], ], ], ] and ]. ] is used for the largely obsolete photographic ].<ref name=Weaver>{{cite web|last1=Weaver|first1=Gawain|title=A Guide to Fiber-Base Gelatin Silver Print Condition and Deterioration|url=http://gawainweaver.com/images/uploads/Weaver_Guide_to_Gelatin_Silver.pdf|publisher=George Eastman House, International Museum of Photography and Film|access-date=30 October 2009|date=2008}}</ref>
	==In biology==
	Bromide is needed by ] (white blood cells of the granulocyte class, specialized for dealing with multi-cellular parasites), which use it to generate antiparasitic ]s by the action of ], a ] enzyme which is able to use chloride, but preferentially uses bromide when available.<ref>{{cite journal|pmid=2538427|year=1989|last1=Mayeno|first1=AN|last2=Curran|first2=AJ|last3=Roberts|first3=RL|last4=Foote|first4=CS|title=Eosinophils preferentially use bromide to generate halogenating agents|volume=264|issue=10|pages=5660–8|journal=The Journal of biological chemistry}}</ref> Despite this use by the body, bromide is not known to be strictly necessary for life, as its functions may generally be replaced (though in some cases not as well) by chloride.
			==Medicinal and veterinary uses==
	Bromide salts are also sometimes used in ]s and spas as mild germicidal agents, using the action of an added oxidizing agent to generate ''in situ'' ], in a similar fashion to the peroxidase in eosinophils.
			] reactions to bromide, all except lower right]]
			===Folk and passé medicine===
			] was used as a ] beginning in the early 1900s. However, it fell into disfavour in the 1940s due to the rising popularity of safer and more efficient sedatives (specifically, ]) and when some heart patients died after using a salt substitute (see ]).<ref> {{Webarchive|url=https://web.archive.org/web/20220224085437/https://www.webmd.com/bipolar-disorder/guide/bipolar-disorder-treatment-care?pagenumber=1 |date=2022-02-24}}. webmd.com</ref> Like ] and ], it was used as a treatment for ].
			From 1954 - 1977, the Australian ] ] was researching safe ways to use ] for the treatment of ] while working at the Royal Park Psychiatric Hospital in ]. While conducting this research she discovered that bromide caused symptoms of mental illness, leading to a major reduction in its usage.<ref>{{Cite web |title=Papers of Shirley Andrews |url=https://nla.gov.au/nla.obj-233797980 |access-date=2022-10-26 |website=Trove |language=en}}</ref>
	The average concentration of bromide in human blood is 5.3±1.4&nbsp;mg/L and varies with age and gender.<ref>{{cite journal|pmid=9602940|year=1998|last1=Olszowy|first1=HA|last2=Rossiter|first2=J|last3=Hegarty|first3=J|last4=Geoghegan|first4=P|title=Background levels of bromide in human blood|volume=22|issue=3|pages=225–30|journal=Journal of analytical toxicology}}</ref> Much higher levels may indicate exposure to brominated chemicals (e.g. ]). However, bromide occurs in relatively high concentration in seawater and many types of seafood, and bromide concentrations in the blood are heavily influenced by seafood contributions to the diet.
			{{Further|Potassium bromide}}
			Bromide compounds, especially ], were frequently used as sedatives in the 19th and early 20th centuries. Their use in over-the-counter sedatives and headache remedies (such as ]) in the United States extended to 1975 when bromides were withdrawn as ingredients due to ].<ref>{{Cite book | url =https://archive.org/details/greatamericanfr03adamgoog | title = The Great American fraud | publisher =Press of the American Medical Association | last1 =Adams | first1 =Samuel Hopkins | year =1905}}.</ref> This use gave the word "bromide" its colloquial connotation of a comforting ].<ref name="Dictionary">{{cite web|title=the definition of bromide|url=https://www.dictionary.com/browse/bromide|website=Dictionary.com|access-date=21 December 2016|url-status=live|archive-url=https://web.archive.org/web/20161224192445/https://www.dictionary.com/browse/bromide|archive-date=24 December 2016}}</ref>
	==History==
	{{Unreferenced section|date=December 2010}}
			It has been said that during ], British soldiers were given bromide to curb their sexual urges.<ref>Tanaka, Yuki (2002) ''Japan's Comfort Women: Sexual slavery and prostitution during World War II and the US Occupation'', Routledge, p. 175. {{ISBN|0415194008}}.</ref>
	In some countries, bromide salts remain available in a liquid form at pharmacies{{Citation needed|date=August 2009}}, although since the 1970s they have been removed as over-the-counter sedatives in most countries in the West.
			Bromide salts are used in ]s as mild ] agents to generate ''in situ'' ].
			The bromide ion is ] and as bromide salt, is used in veterinary medicine in the US. The kidneys excrete bromide ions. The half-life of bromide in the human body (12 days) is long compared with many pharmaceuticals, making dosing challenging to adjust. (A new dose may require several months to reach equilibrium.) Bromide ion concentrations in the ] are about 30% of those in blood and are strongly influenced by the body's chloride intake and metabolism.<ref>{{cite book|editor1-last=Goodman |editor1-first=L. S. |editor2-last=Gilman |editor2-first=A. |date=1970 |chapter=10. Hypnotics and Sedatives |page=121 |title=The Biological Basis of Therapeutics |edition=4th |publisher=Macmillan |location=London}}</ref>
			Since bromide is still used in veterinary medicine in the United States, veterinary diagnostic labs can routinely measure blood bromide levels. However, this is not a conventional test in human medicine in the US since there are no FDA-approved uses for the bromide. Therapeutic bromide levels are measured in European countries like ], where bromide is still used therapeutically in human epilepsy.
			==Biochemistry==
			Bromide is rarely mentioned in the biochemical context. Some enzymes use bromide as substrate or as a ].
			===Substrate===
			] enzymes use bromide (typically in seawater) to generate electrophilic brominating agents. Hundreds of ]s are generated by this process. Notable examples are bromoform, thousands of tons of which are produced annually in this way. The historical dye ] is produced by similar enzymatic reactions.<ref>{{cite journal|first=Gordon W. |last=Gribble |title=The diversity of naturally occurring organobromine compounds |journal=Chemical Society Reviews |date=1999 |volume=28 |issue=5 |pages=335–346 |doi=10.1039/a900201d}}</ref>
			===Cofactor===
			In one specialized report, bromide is an essential cofactor in the peroxidising catalysis of sulfonimine crosslinks in collagen IV. This ] occurs in all animals and bromine is an essential trace element for humans.<ref name="pmid24906154">{{Cite journal |last1 = McCall |first1 = A. Scott |last2 = Cummings |first2 = Christopher F. |last3 = Bhave |first3 = Gautam |last4 = Vanacore |first4 = Roberto |last5 = Page-McCaw |first5 = Andrea |last6 = Hudson |first6 = Billy G. |title = Bromine Is an Essential Trace Element for Assembly of Collagen IV Scaffolds in Tissue Development and Architecture |url= |journal = Cell |language = en |volume = 157 |issue = 6 |pages = 1380–1392 |year = 2014 |doi = 10.1016/j.cell.2014.05.009 |pmc = 4144415 |pmid = 24906154}}</ref>
			] need bromide for fighting multicellular parasites. ] is produced via ], an enzyme that can use chloride but preferentially uses bromide.<ref>
			{{Cite journal |last1 = Mayeno |first1 = Arthur N. |last2 = Curran |first2 = A. Jane |last3 = Roberts |first3 = Robert L. |last4 = Foote |first4 = Christopher S. |date = 1989-04-05 |title = Eosinophils Preferentially Use Bromide to Generate Halogenating Agents |journal = Journal of Biological Chemistry |volume = 264 |issue = 10 |pages = 5660–5668 |doi = 10.1016/s0021-9258(18)83599-2 |issn = 0021-9258 |pmid = 2538427|doi-access = free}}</ref>
			The average concentration of bromide in human blood in Queensland, Australia, is {{val|5.3|1.4|u=mg/L}} and varies with age and gender.<ref>{{cite journal|pmid=9602940|year=1998|last1=Olszowy|first1=HA|last2=Rossiter|first2=J|last3=Hegarty|first3=J|last4=Geoghegan|first4=P|title=Background levels of bromide in human blood|volume=22|issue=3|pages=225–30|journal=Journal of Analytical Toxicology|doi=10.1093/jat/22.3.225|doi-access=free}}</ref> Much higher levels may indicate exposure to brominated chemicals. It is also found in seafood.
			==Further reading==
			===Encyclopedia articles and books===
			* Christe, K., and S. Schneider (2020), Bromine, Encyclopædia Britannica.
			* Emerson, S., and J. Hedges (2011), Chemical Oceanography and the Marine Carbon Cycle, Cambridge University 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), Chemical 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 About Bromine, LiveScience.
			* Steele, J. H., S. A. Thorpe, and K. K. Turekian (2001), Encyclopedia of Ocean Sciences, Academic Press, San Diego.
			* Steele, J. H., S. A. Thorpe, and K. K. Turekian (2009), Encyclopedia of Ocean Sciences, Academic Press, Boston.
			* Watkins, T. (2011), Bromine, Environmental Encyclopedia.
			===Peer-reviewed journal articles for bromine (Br)===
			* Wisniak, J. (2002), The history of bromine from discovery to commodity, NOPR.
			===Peer-reviewed journal articles for bromide (Br<sup>−</sup>)===
			* Anbar, A. D., Y. L. Yung, and F. P. Chavez (1996), Methyl bromide: Ocean sources, ocean sinks, and climate sensitivity, AGU Journals.
			* Foti, S. 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 production of organobromine compounds, Environmental Science and Pollution Research, 7(1), 37–49, {{doi|10.1065/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(4), 329–335, {{doi|10.1016/j.chemosphere.2004.04.056}}.
			* Pilinis, C., D. B. King, and E. S. Saltzman (1996), The oceans: A source or a sink of methyl bromide?, Geophysical Research 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 ocean – global patterns and emissions, Biogeosciences, 12(6), 1967–1981, {{doi|10.5194/bg-12-1967-2015}}.
			* Suzuki, A., Lim, L., Hiroi, T., & Takeuchi, T. (2006, March 20). Rapid determination of bromide in seawater samples by capillary ion chromatography using monolithic silica columns modified with cetyltrimethylammonium ion.
	==References==		==References==
	{{Reflist}}		{{Reflist}}
			{{Bromides}}
			{{Monatomic anion compounds}}
			{{GABAAR PAMs}}
			{{Authority control}}
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