"Bromo" redirects here. For other uses, see Bromo (disambiguation). selenium ← bromine → krypton Cl ↑ Br ↓ I 35Br Periodic table Appearance gas/liquid: red-brown solid: metallic luster General properties Name, symbol, number bromine, Br, 35 Pronunciation /ˈbroʊmiːn/ BROH-meen or /ˈbroʊmɪn/ BROH-min Element category halogen Group, period, block 17, 4, p Standard atomic weight 79.904g·mol−1 Electron configuration Ar 4s2 3d10 4p5 Electrons per shell 2, 8, 18, 7 (Image) Physical properties Phase liquid Density (near r.t.) (Br2, liquid) 3.1028 g·cm−3 Melting point 265.8 K, -7.2 °C, 19 °F Boiling point 332.0 K, 58.8 °C, 137.8 °F Critical point 588 K, 10.34 MPa Heat of fusion (Br2) 10.571 kJ·mol−1 Heat of vaporization (Br2) 29.96 kJ·mol−1 Specific heat capacity (25 °C) (Br2) 75.69 J·mol−1·K−1 Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 185 201 220 244 276 332 Atomic properties Oxidation states 7, 5, 4, 3, 1, -1 (strongly acidic oxide) Electronegativity 2.96 (Pauling scale) Ionization energies 1st: 1139.9 kJ·mol−1 2nd: 2103 kJ·mol−1 3rd: 3470 kJ·mol−1 Atomic radius 120 pm Covalent radius 120±3 pm Van der Waals radius 185 pm Miscellanea Crystal structure orthorhombic Magnetic ordering diamagnetic1 Electrical resistivity (20 °C) 7.8×1010Ω·m Thermal conductivity (300 K) 0.122 W·m−1·K−1 Speed of sound (20°C) 206 m/s CAS registry number 7726-95-6 Most stable isotopes Main article: Isotopes of bromine iso NA half-life DM DE (MeV) DP 79Br 50.69% 79Br is stable with 44 neutrons 81Br 49.31% 81Br is stable with 46 neutrons v · d · e Bromine ( /ˈbroʊmiːn/ BROH-meen or /ˈbroʊmɪn/ BROH-min; from Greek: βρῶμος, brómos, meaning "stench (of he-goats)"),2 is a chemical element with the symbol Br, an atomic number of 35, and an atomic mass of 79.904. It is in the halogen element group. The element was isolated independently by two chemists in 1825-26. Elemental bromine is a fuming red-brown liquid at room temperature, corrosive and toxic, with properties between those of chlorine and iodine. Free bromine does not occur in nature, but occurs as colorless soluble crystalline mineral halide salts, analogous to table salt. Bromine is rarer than about three-quarters of elements in the Earth's crust, however the high solubility of bromide ion has caused its accumulation in the oceans, and commercially the element is easily extracted from brine pools, mostly in the United States, Israel, and China. About 556,000 metric tons were produced in 2007,3 an amount similar to the far more abundant element magnesium. At high temperatures, organobromine compounds are easily converted to free bromine atoms, a process which acts to terminate free radical chemical chain reactions. This makes such compounds useful fire retardants and this is bromine's primary industrial use, consuming more than half of world production of the element. The same property allows volatile organobromine compounds, under the action of sunlight, to form free bromine atoms in the atmosphere which are highly effective in ozone depletion. This unwanted side-effect has caused many common volatile brominated organics like methyl bromide, a pesticide that was formerly a large industrial bromine consumer, to be abandoned. Remaining uses of bromine compounds are in well-drilling fluids, as an intermediate in manufacture of organic chemicals, and in film photography.

Bromine has no essential function in mammals, though it is preferentially used over chloride by one antiparasitic enzyme in the human immune system. Organobromides are needed and produced enzymatically from bromide by some lower life forms in the sea, particularly algae. As a pharmaceutical, simple bromide ion, Br-, has inhibitory effects on the central nervous system, and bromide salts were once a major medical sedative, before being replaced by shorter-acting drugs. They retain niche uses as antiepileptics. Contents 1 Characteristics 1.1 Physical 1.2 Chemical characteristics 1.3 Occurrence 1.4 Isotopes 2 Compounds and chemistry 2.1 Organic chemistry 2.2 Inorganic chemistry 3 History 4 Production 4.1 Laboratory methods 5 Applications 5.1 Flame retardant 5.2 Gasoline additive 5.3 Pesticide 5.4 Medical and veterinary 5.5 Other uses 6 Biological role 7 Safety 8 References 9 External links Characteristics Physical Illustrative and secure bromine sample for teaching Elemental bromine exists as a diatomic molecule, Br2. It is a dense, mobile, slightly transparent reddish-brown liquid, that evaporates easily at standard temperature and pressures to give a red vapor (its color resembles nitrogen dioxide) that has a strongly disagreeable odor resembling that of chlorine. It is the only nonmetallic element that is a liquid at room temperature, and one of only two elements on the periodic table that are liquids at room temperature (mercury is the other). At a pressure of 55 GPa bromine converts to a metal. At 75 GPa it converts to a face centered orthorhombic structure. At 100 GPa it converts to a body centered orthorhombic monoatomic form.4 Chemical characteristics Being less reactive than chlorine but more reactive than iodine, bromine reacts vigorously with metals, especially in the presence of water, to give bromide salts. It is also reactive toward most organic compounds, especially upon illumination, conditions that favor the dissociation of the diatomic molecule into bromine radicals: Br2 2 Br· It bonds easily with many elements and has a strong bleaching action. Bromine is slightly soluble in water, but it is highly soluble in organic solvents such as carbon disulfide, aliphatic alcohols, and acetic acid. Occurrence See also: Category:Halide minerals and Halide mineral World bromine production trend View of salt evaporation pans on the Dead Sea, where Jordan (right) and Israel (left) produce salt and bromine 31°9′0″N 35°27′0″E / 31.15°N 35.45°E / 31.15; 35.45 The diatomic element Br2 does not occur naturally. Instead, bromine exists exclusively as bromide salts in diffuse amounts in crustal rock. Owing to leaching, bromide salts have accumulated in sea water (65 ppm),5 but at a lower concentration than chloride. Bromine may be economically recovered from bromide-rich brine wells and from the Dead Sea waters (up to 50000 ppm).67 It exists in the Earth's crust at 0.4 ppm, making it the 62nd most abundant element. The bromine concentration in soils varies normally between 5-40 ppm, but some volcanic soils can contain up to 500 ppm. The concentration of bromine in the atmosphere is extremely low, at only a few ppt.8 A large number of organobromine compounds are found in small amounts in nature. China's bromine reserves are located in the Shandong Province and Israel's bromine reserves are contained in the waters of the Dead Sea. The largest bromine reserve in the United States is located in Columbia County and Union County, Arkansas, U.S.9 Isotopes Main article: Isotopes of bromine

Bromine has two stable isotopes, 79Br (50.69 %) and 81Br (49.31%). At least another 23 radioisotopes are known to exist.10 Many of the bromine isotopes are fission products. Several of the heavier bromine isotopes from fission are delayed neutron emitters. All of the radioactive bromine isotopes are relatively short lived. The longest half life is the neutron deficient 77Br at 2.376 days. The longest half life on the neutron rich side is 82Br at 1.471 days. A number of the bromine isotopes exhibit metastable isomers. Stable 79Br exhibits a radioactive isomer, with a half life of 4.86 seconds. It decays by isomeric transition to the stable ground state.11 Compounds and chemistry This section needs additional citations for verification. Please help improve this article by adding reliable references. Unsourced material may be challenged and removed. (September 2010) Organic chemistry Main article: Organobromine compound N-Bromosuccinimide Organic compounds are brominated by either addition or substitution reactions. Bromine undergoes electrophilic addition to the double-bonds of alkenes, via a cyclic bromonium intermediate. In non-aqueous solvents such as carbon disulfide, this affords the di-bromo product. For example, reaction with ethylene will produce 1,2-dibromoethane. Bromine also undergoes electrophilic addition to phenols and anilines. When used as bromine water, a small amount of the corresponding bromohydrin is formed as well as the dibromo compound. So reliable is the reactivity of bromine that bromine water is employed as a reagent to test for the presence of alkenes, phenols, and anilines. Like the other halogens, bromine participates in free radical reactions. For example, hydrocarbons are brominated upon treatment with bromine in the presence of light. Bromine, sometimes with a catalytic amount of phosphorus, easily brominates carboxylic acids at the α-position. This method, the Hell-Volhard-Zelinsky reaction, is the basis of the commercial route to bromoacetic acid. N-Bromosuccinimide is commonly used as a substitute for elemental bromine, being easier to handle, and reacting more mildly and thus more selectively. Organic bromides are often preferable relative to the less reactive chlorides and more expensive iodide-containing reagents. Thus, Grignard and organolithium compound are most often generated from the corresponding bromides. Certain bromine-related compounds have been evaluated to have an ozone depletion potential or bioaccumulate in living organisms. As a result, many industrial bromine compounds are no longer manufactured, are being restricted, or scheduled for phasing out. The Montreal Protocol mentions several organobromine compounds for this phase out. Inorganic chemistry See also: Category:Bromine compounds Inorganic bromine compounds adopt a variety of oxidation states from -1 to +7.12 Oxidation states of bromine −1 HBr 0 Br2 +1 BrCl +3 BrF3 +5 BrF5 +5 BrO− 3 +7 BrO− 4 Bromine is an oxidizer, and it will oxidize iodide ions to iodine, being itself reduced to bromide: Br2 + 2 I− → 2 Br− + I2 Bromine will also oxidize metals and metalloids to the corresponding bromides. Anhydrous bromine is less reactive toward many metals than hydrated bromine, however. Dry bromine reacts vigorously with aluminium, titanium, mercury as well as alkaline earths and alkali metals. Dissolving bromine in alkaline solution gives a mixture of bromide and hypobromite: Br2 + 2 OH− → Br− + OBr− + H2O This hypobromite is responsible for the bleaching abilities of bromide solutions. Warming of these solutions causes the disproportion reaction of the hypobromite to give bromate, a strong oxidising agent very similar to chlorate. 3 BrO− → BrO− 3 + 2 Br−

In contrast to the route to perchlorates, perbromates are not accessible through electrolysis but only by reacting bromate solutions with fluorine or ozone. BrO3− + H2O + F2 → BrO− 4 + 2 HF BrO3− + O3 → BrO− 4 + O2 Bromine reacts violently and explosively with aluminium metal, forming aluminium bromide: 2 Al + 3 Br2 → 2 AlBr3 Bromine reacts with hydrogen in gaseous form and gives hydrogen bromide: H2 + Br2 → 2HBr Bromine reacts with alkali metal iodides in a displacement reaction. This reaction forms alkali metal bromides and produces elemental iodine: 2 NaI + Br2 → 2 NaBr + I2 2 KI + Br2 → 2 KBr + I2 History Bromine was discovered independently by two chemists Antoine Balard1314 and Carl Jacob Löwig1516171819 in 1825 and 1826.20 Balard found bromide chemicals in the ash of seaweed from the salt marshes of Montpellier in 1826. The seaweed was used to produce iodine, but also contained bromine. Balard distilled the bromine from a solution of seaweed ash saturated with chlorine. The properties of the resulting substance resembled that of an intermediate of chlorine and iodine; with those results he tried to prove that the substance was iodine monochloride (ICl), but after failing to do so he was sure that he had found a new element and named it muride, derived from the Latin word muria for brine.14 Carl Jacob Löwig isolated bromine from a mineral water spring from his hometown Bad Kreuznach in 1825. Löwig used a solution of the mineral salt saturated with chlorine and extracted the bromine with diethyl ether. After evaporation of the ether a brown liquid remained. With this liquid as a sample for his work he applied for a position in the laboratory of Leopold Gmelin in Heidelberg. The publication of the results was delayed and Balard published his results first.19 After the French chemists Louis Nicolas Vauquelin, Louis Jacques Thénard, and Joseph-Louis Gay-Lussac approved the experiments of the young pharmacist Balard, the results were presented at a lecture of the Académie des Sciences and published in Annales de Chimie et Physique.13 In his publication Balard states that he changed the name from muride to brôme on the proposal of M. Anglada. (Brôme (bromine) derives from the Greek βρωμος (stench).1321) Other sources claim that the French chemist and physicist Joseph-Louis Gay-Lussac suggested the name brôme for the characteristic smell of the vapors.2223 Bromine was not produced in large quantities until 1860. The first commercial use, besides some minor medical applications, was the use of bromine for the daguerreotype. In 1840 it was discovered that bromine had some advantages over the previously used iodine vapor to create the light sensitive silver halide layer used for daguerreotypy.24 Potassium bromide and sodium bromide were used as anticonvulsants and sedatives in the late 19th and early 20th centuries, until they were gradually superseded by chloral hydrate and then the barbiturates.25 Production Approximately 556,000 metric tons (worth around US $2.5 billion) of bromine is produced per year (2007) worldwide, with the United States, Israel, and China producing more than 80% of the world's supply, and Jordan and Japan producing much of the rest.26272829 Bromine production has increased sixfold since the 1960s. Bromide-rich brines are treated with chlorine gas, flushing through with air. In this treatment, bromide anions are oxidized to bromine by the chlorine gas. 2 Br− + Cl2 → 2 Cl− + Br2 Laboratory methods

In the laboratory, because of its commercial availability and long shelf-life, bromine is not typically prepared. Small amounts of bromine can however be generated through the reaction of solid sodium bromide with concentrated sulfuric acid (H2SO4). The first stage is formation of hydrogen bromide (HBr), which is a gas, but under the reaction conditions some of the HBr is oxidized further by the sulfuric acid to form bromine (Br2) and sulfur dioxide (SO2). NaBr (s) + H2SO4 (aq) → HBr (aq) + NaHSO4 (aq) 2 HBr (aq) + H2SO4 (aq) → Br2 (g) + SO2 (g) + 2 H2O (l) Similar alternatives, such as the use of dilute hydrochloric acid with sodium hypobromite, are also available. The most important thing is that the anion of the acid (in the above examples, sulfate and chloride, respectively) be more electronegative than bromine, allowing the substitution reaction to occur. Reactions involving a strong oxidizing agent, such as potassium permanganate, on bromide ions in the presence of an acid also gives bromine. An acidic solution of bromate ions and bromide ions will also comproportionate slowly to give bromine. Like iodine, bromine is soluble in chloroform but only slightly soluble in water. In water, the solubility can be increased by the presence of bromide ions. Concentrated solutions of bromine are rarely prepared in the lab because of hazards. Also as with iodine sodium thiosulphate (or any soluble thiosulfphate) is an effective reagent for reducing bromine to colorless odorless bromide, thus dealing with stains and odor from the element in unwanted places. For the same reason, thiosulfate is used in photography to deal with free bromine in emulsions. Applications A wide variety of organobromine compounds are used in industry. Some are prepared from bromine and others are prepared from hydrogen bromide, which is obtained by burning hydrogen in bromine.3 Illustrative of the addition reaction30 is the preparation of 1,2-dibromoethane, the organobromine compound produced in the largest amounts: C2H4 + Br2 → CH2BrCH2Br Flame retardant Tetrabromobisphenol A Brominated flame retardants represent a commodity of growing importance, and represent the largest use of bromine. When the brominated material burns, the flame retardant produces hydrobromic acid which interferes in the radical chain reaction of the oxidation reaction of the fire. The mechanism is that the highly reactive hydrogen oxygen and hydroxy radicals react with hydrobromic acid and form less reactive bromine radicals (free bromine atoms). These also react with radicals in the first to help terminate the reaction.3132 The bromine-containing compounds can be placed in the polymers either during polymerization if a small amount of brominated monomer is added or the bromine containing compound is added after polymerization. Tetrabromobisphenol A can be added to produce polyesters or epoxy resins. Epoxy used in printed circuit boards (PCB) are normally made from flame retardant resins, indicated by the FR in the abbreviation of the products (FR-4 and FR-2. Vinyl bromide can be used in the production of polyethylene, polyvinylchloride or polypropylene. Decabromodiphenyl ether can be added to the final polymers.33 Gasoline additive Ethylene bromide was an additive in gasolines containing lead anti-engine knocking agents. It scavenges lead by forming volatile lead bromide, which is exhausted from the engine. This application accounted for 77% of the bromine use in 1966 in the US. This application has declined since the 1970s due to environmental regulations (see below).34 Pesticide Methyl bromide (bromomethane)

Poisonous methyl bromide was widely used as pesticide to fumigate soil and to fumagate housing, by the tenting method. Ethylene bromide was similarly used.28 These volatile organobromine compounds are all now regulated as ozone depletion agents. The Montreal Protocol on Substances that Deplete the Ozone scheduled the phase out for the ozone depleting chemical by 2005, and organobromide pesticides are no longer used (in housing fumagation they have been replaced by such compounds as sulfuryl fluoride, which contain neither the chlorine or bromine organics which harm ozone). Prior to the Montreal protocol in 1991 (for example) an estimated 35,000 metric tons of the chemical were used to control nematodes, fungi, weeds and other soil-borne diseases.3536 Medical and veterinary Main article: potassium bromide Bromide compounds, especially potassium bromide, were frequently used as general sedatives in the 19th and early 20th century. Bromides in the form of simple salts are still used as anticonvulsants, in both veterinary and human medicine. Long-term use of potassium bromide can lead to bromism. Other uses Orange fluoresces of DNA Ethidium bromide intercalate The bromides of calcium, sodium, and zinc account for a sizable part of the bromine market. These salts form dense solutions in water that are used as drilling fluids sometimes called clear brine fluids.2837 Bromine is also used in the production of brominated vegetable oil, which is used as an emulsifier in many citrus-flavored soft drinks (e.g. Mountain Dew). After the introduction in the 1940s the compound was extensively used until the UK and the US limited its use in the mid 1970s and alternative emulsifiers were developed.38 Soft drinks containing brominated vegetable oil are still sold in the US (2011).39 Tralomethrin Several dyes, agrichemicals, and pharmaceuticals are organobromine compounds. 1-Bromo-3-chloropropane, 1-bromoethylbenzene, and 1-bromoalkanes are prepared by the antimarkovnikov addition of HBr to alkenes. Ethidium bromide, EtBr, is used as a DNA stain in gel electrophoresis. High refractive index compounds Bromine, like chlorine, is used in maintenance of swimming pools, especially spas (hot tubs), where it is generated in situ from a bromide plus hydrogen peroxide. In spas, the high water temperatures render chlorinated water purification and buffering compounds unstable, and bromine compounds may improve the life of the free-halogen antimicrobial. Water purification compounds, disinfectants and insecticides, such as tralomethrin (C22H19Br4NO3).28 Potassium bromide is used in some photographic developers to inhibit the formation of fog (undesired reduction of silver). Bromine vapor is used as the second step in sensitizing daguerreotype plates to be developed under mercury vapor. Bromine acts as an accelerator to the light sensitivity of the previously iodized plate. Bromine is also used to reduce mercury pollution from coal-fired power plants. This can be achieved either by treating activated carbon with bromine or by injecting bromine compounds onto the coal prior to combustion. Biological role Tyrian purple Bromine has no known essential role in human or mammalian health, but inorganic bromine and organobromine compounds do occur naturally, and some may be of use to higher organisms in dealing with parasites. For example, in the presence of H2O2 formed by the eosinophil, and either chloride or bromide ions, eosinophil peroxidase provides a potent mechanism by which eosinophils kill multicellular parasites (such as, for example, the nematode worms involved in filariasis); and also certain bacteria (such as tuberculosis bacteria). Eosinophil peroxidase is a haloperoxidase that preferentially uses bromide over chloride for this purpose, generating hypobromite (hypobromous acid).40

Marine organisms are the main source of organobromine compounds. Over 1600 compounds were identified by 1999. The most abundant one is methyl bromide (CH3Br) with an estimated 56,000 metric tonnes produced by marine algae each year.41 The essential oil of the Hawaiian alga Asparagopsis taxiformis consists of 80% methyl bromide.42 In fact, most organobromine compounds in nature arise in the sea, via the action of a unique algal enzyme, vanadium bromoperoxidase.43 Though this enzyme is the most prolific creator of organic bromides by living organisms, other bromoperoxidases exist in nature that do not use vandadium. A famous example of a bromine-containing organic compound that has been used by humans since ancient times is the fabric dye Tyrian purple.414445 The brominated indole indigo dye is produced by a medium-sized predatory sea snail, the marine gastropod Murex brandaris. The organobromine nature of the compound was not discovered until 1909 (see Paul Friedländer).46 Bromine can also be substituted for the methyl substituent in the nitrogenous base thymine of DNA, creating the base analog 5-bromouracil. When this base is incorporated into DNA its different hydrogen bonding properties may cause mutation at the site of that base pair.47 Safety See also: List of highly toxic gases Elemental bromine is toxic and causes burns. As an oxidizing agent, it is incompatible with most organic and inorganic compounds. Care needs to be taken when transporting bromine; it is commonly carried in steel tanks lined with lead, supported by strong metal frames. When certain ionic compounds containing bromine are mixed with potassium permanganate (KMnO4) and an acidic substance, they will form a pale brown cloud of bromine gas. This gas smells like bleach and is very irritating to the mucous membranes. Upon exposure, one should move to fresh air immediately. If symptoms of bromine poisoning arise, medical attention is needed. References ^ Magnetic susceptibility of the elements and inorganic compounds, in Handbook of Chemistry and Physics 81st edition, CRC press. ^ Gemoll W, Vretska K (1997). Griechisch-Deutsches Schul- und Handwörterbuch ("Greek-German dictionary"), 9th ed.. öbvhpt. ISBN 3-209-00108-1.  ^ a b Jack F. Mills (2002). Bromine: in Ullmann's Encyclopedia of Chemical Technology. Weinheim: Wiley-VCH Verlag. doi:10.1002/14356007.a04_391.  ^ Duan, Defang; Liu, Yanhui; Ma, Yanming; Liu, Zhiming; Cui, Tian; Liu, Bingbing; Zou, Guangtian (2007-09-26). "Ab initio studies of solid bromine under high pressure". Physical Review B 76: 104113. doi:10.1103/PhysRevB.76.104113.  ^ Tallmadge, John A.; Butt, John B.; Solomon Herman J. (1964). "Minerals From Sea Salt". Ind. Eng. Chem. 56: 44. doi:10.1021/ie50655a008.  ^ Oumeish, Oumeish Youssef (1996). "Climatotherapy at the Dead Sea in Jordan". Clinics in Dermatology 14: 659. doi:10.1016/S0738-081X(96)00101-0.  ^ Al-Weshah, Radwan A. (2008). "The water balance of the Dead Sea: an integrated approach". Hydrological Processes 14: 145. doi:10.1002/(SICI)1099-1085(200001)14:1<145::AID-HYP916>3.0.CO;2-N.  ^ John Emsley. "Bromine". Nature's Building Blocks - An A-Z Guide to the Elements. p. 71. ISBN 0198503407.  ^ "Bromine:An Important Arkansas Industry". Butler Center for Arkansas Studies. http://www.cals.lib.ar.us/butlercenter/lesson_plans/lesson%20plans/Lesson%20plans-retained/Bromine.pdf.  ^ GE (1989). Chart of the Nuclides, 14th Edition. Nuclear Energy.  ^ Audi, Georges (2003). "The NUBASE Evaluation of Nuclear and Decay Properties". Nuclear Physics A (Atomic Mass Data Center) 729: 3. doi:10.1016/j.nuclphysa.2003.11.001.  ^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4. ^ a b c Balard, A. J. (1826). "Mémoire sur une substance particulière contenue dans l'eau de la mer" (Memoir on a particular substance contained in seawater)". Annales de Chimie et de Physique 2nd series 32: 337–381. http://books.google.com/books?id=vBIAAAAAMAAJ&pg=PA337&lpg=PA337#v=onepage&q&f=false.  ^ a b Balard, Antoine (1826). "Memoire of a peculire Substance contained in Sea Water". Annals of Philosophy: 387– and 411–. http://books.google.com/?id=A-M4AAAAMAAJ.  ^ Löwig, Carl Jacob (1829). Das Brom und seine chemischen Verhältnisse (Bromine and its chemical relationships). Heidelberg: Carl Winter.  ^ Löwig, Carl (1827). "Über Brombereitung und eine auffallende Zersetzung des Aethers durch Chlor (On the preparation of bromine and a striking decomposition of ether by chlorine)". Magazine für Pharmacie 21: 31–36. http://books.google.com/books?id=bO43AAAAMAAJ&pg=PA31#v=onepage&q&f=false.  ^ Löwig, Carl (1828). "Über einige Bromverbindungen und über Bromdarstellung" (On some bromine compounds and on the production of bromine)". Poggendorff's Annalen der Physik und Chemie 14: 485–499. http://books.google.com/books?id=vG0EAAAAYAAJ&pg=PA485#v=onepage&q&f=false.  ^ Löwig, Carl (1828). "Ueber einige Bromverbindungen und über Bromdarstellung". Annalen der Physik 90 (11): 485–499. doi:10.1002/andp.18280901113.  ^ a b Landolt, Hans Heinrich (1890). "Nekrolog: Carl Löwig". Berichte der deutschen chemischen Gesellschaft 23: 905. doi:10.1002/cber.18900230395. http://gallica.bnf.fr/ark:/12148/bpt6k907222/f920.chemindefer.  ^ Weeks, Mary Elvira (1932). "The discovery of the elements: XVII. The halogen family.". Journal of Chemical Education 9: 1915. doi:10.1021/ed009p1915.  ^ Vauquelin, L.N.; Thenard, L.J.; Gay-Lussac, J.L. (1826). "Rapport sur la Mémoire de M. Balard relatif à une nouvelle Substance" (Report on a memoir by Mr. Balard regarding a new substance)". Annales de Chimie et de Physique 2nd series 32: 382–384. http://books.google.com/books?id=vBIAAAAAMAAJ&pg=PA382&lpg=PA382#v=onepage&q&f=false.  ^ On page 341 of his article -- A. J. Balard (1826) "Mémoire sur une substance particulière contenue dans l'eau de la mer" (Memoir on a particular substance contained in seawater), Annales de Chimie et de Physique, 2nd series, vol. 32, pages 337-381 -- Balard states that Mr. Anglada persuaded him to name his new element brôme. However, on page 382 of the same journal -- "Rapport sur la Mémoire de M. Balard relatif à une nouvelle Substance" (Report on a memoir by Mr. Balard regarding a new substance), Annales de Chimie et de Physique, series 2, vol. 32, pages 382-384. -- a committee of the French Academy of Sciences claimed that they had renamed the new element brôme. ^ Wisniak, Jaime (2004). "Antoine-Jerôme Balard. The discoverer of bromine". Revista CENIC Ciencias Químicas 35. http://revistas.mes.edu.cu:9900/EDUNIV/03-Revistas-Cientificas/Rev.CENIC-Ciencias-Quimicas/2004/1/09204109.pdf.  ^ Barger, M. Susan; White, William Blaine (2000). "Technological Practice of Daguerreotypy". The Daguerreotype: Nineteenth-century Technology and Modern Science. JHU Press. pp. 31–35. ISBN 9780801864582.  ^ Shorter, Edward (1997). A History of Psychiatry: From the Era of the Asylum to the Age of Prozac. John Wiley and Sons. p. 200. ISBN 9780471245315.  ^ Emsley, John (2001). "Bromine". Nature's Building Blocks: An A-Z Guide to the Elements. Oxford, England, UK: Oxford University Press. pp. 69–73. ISBN 0198503407.  ^ Lyday, Phyllis A.. "Commodity Report 2007: Bromine". United States Geological Survey. http://minerals.usgs.gov/minerals/pubs/commodity/bromine/bromimcs07.pdf. Retrieved 2008-09-03.  ^ a b c d Lyday, Phyllis A.. "Mineral Yearbook 2007: Bromine". United States Geological Survey. http://minerals.usgs.gov/minerals/pubs/commodity/bromine/myb1-2006-bromi.pdf. Retrieved 2008-09-03.  ^ http://minerals.usgs.gov/minerals/pubs/commodity/bromine/mcs-2009-bromi.pdf 2009 mineral commodities report ^ N. A. Khan, F. E. Deatherage, and J. B. Brown (1963), "Stearolic Acid", Org. Synth., http://www.orgsyn.org/orgsyn/orgsyn/prepContent.asp?prep=CV4P0851 ; Coll. Vol. 4: 851  ^ Green, Joseph (1996). "Mechanisms for Flame Retardancy and Smoke suppression - A Review". Journal of Fire Sciences 14: 426. doi:10.1177/073490419601400602.  ^ Kaspersma, Jelle; Doumena, Cindy; Munrob Sheilaand; Prinsa, Anne-Marie (2002). "Fire retardant mechanism of aliphatic bromine compounds in polystyrene and polypropylene". Polymer Degradation and Stability 77: 325. doi:10.1016/S0141-3910(02)00067-8.  ^ Weil, Edward D.; Levchik, Sergei (2004). "A Review of Current Flame Retardant Systems for Epoxy Resins". Journal of Fire Sciences 22: 25. doi:10.1177/0734904104038107.  ^ Alaeea, Mehran; Ariasb, Pedro; Sjödinc, Andreas; Bergman, Åke (2003). "An overview of commercially used brominated flame retardants, their applications, their use patterns in different countries/regions and possible modes of release". Environment International 29: 683. doi:10.1016/S0160-4120(03)00121-1.  ^ Messenger, Belinda; Braun, Adolf (2000). "Alternatives to Methyl Bromide for the Control of Soil-Borne Diseases and Pests in California". Pest Management Analysis and Planning Program. http://www.cdpr.ca.gov/docs/emon/methbrom/alt-anal/sept2000.pdf. Retrieved 2008-11-17.  ^ Decanio, Stephen J.; Norman, Catherine S. (2008). "Economics of the "Critical Use" of Methyl bromide under the Montreal Protocol". Contemporary Economic Policy 23: 376. doi:10.1093/cep/byi028.  ^ Darley, H. C. H.; Gray, George Robert (1988). Composition and Properties of Drilling and Completion Fluids. Gulf Professional Publishing. pp. 61–62. ISBN 9780872011472.  ^ Kaufman, Vered R.; Garti, Nissim (1984). "Effect of cloudy agents on the stability and opacity of cloudy emulsions for soft drinks". International Journal of Food Science & Technology 19: 255. doi:10.1111/j.1365-2621.1984.tb00348.x.  ^ Horowitz, B. Zane (1997). "Bromism from Excessive Cola Consumption',Clinical Toxicology". Clinical Toxicology 35: 315. doi:10.3109/15563659709001219. PMID 9140329.  ^ Mayeno AN, Curran AJ, Roberts RL, Foote CS (April 1989). "Eosinophils preferentially use bromide to generate halogenating agents". J. Biol. Chem. 264 (10): 5660–8. PMID 2538427.  ^ a b Gordon W. Gribble (1999). "The diversity of naturally occurring organobromine compounds". Chemical Society Reviews 28: 335. doi:10.1039/a900201d.  ^ Burreson, B. Jay; Moore, Richard E.; Roller, Peter P. (1976). "Volatile halogen compounds in the alga Asparagopsis taxiformis (Rhodophyta)". Journal of Agricultural snd Food Chemistry 24: 856. doi:10.1021/jf60206a040.  ^ Butler, Alison; Carter-Franklin, Jayme N. (2004). "The role of vanadium bromoperoxidase in the biosynthesis of halogenated marine natural products". Natural Product Reports 21 (1): 180. doi:10.1039/b302337k. PMID 15039842.  ^ Gordon W. Gribble (1998). "Naturally Occurring Organohalogen Compounds". Acc. Chem. Res. 31: 141. doi:10.1021/ar9701777.  ^ John Emsley. "Bromine". Nature's Building Blocks - An A-Z Guide to the Elements. p. 73. ISBN 0198503407.  ^ Friedländer, P. (1909). "Über den Farbstoff des antiken Purpurs aus murex brandaris". Berichte der deutschen chemischen Gesellschaft 42: 765. doi:10.1002/cber.190904201122.  ^ Microbiology A Human Perspective. McGraw-Hill Science Engineering, 2009. Print. External links Wikimedia Commons has media related to: Bromine Look up bromine in Wiktionary, the free dictionary. WebElements.com – Bromine Theodoregray.com – Bromine USGS Minerals Information: Bromine Bromine Science and Environmental Forum (BSEF) Chemistry in its element podcast (MP3) from the Royal Society of Chemistry's Chemistry World: Bromine v · d · eDiatomic chemical elements

Hydrogen H2 | Nitrogen N2 | Oxygen O2 | Fluorine F2 | Chlorine Cl2 | Bromine Br2 | Iodine I2 | Astatine At2 | v · d · e Periodic table H   He Li Be   B C N O F Ne Na Mg   Al Si P S Cl Ar K Ca   Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr   Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo Alkali metals Alkaline earth metals Lanthanides Actinides Transition metals Other metals Metalloids Other nonmetals Halogens Noble gases Unknown chem. properties Large version 

Hydrogen H2 | Nitrogen N2 | Oxygen O2 | Fluorine F2 | Chlorine Cl2 | Bromine Br2 | Iodine I2 | Astatine At2 | v · d · e Periodic table H   He Li Be   B C N O F Ne Na Mg   Al Si P S Cl Ar K Ca   Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr   Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo Alkali metals Alkaline earth metals Lanthanides Actinides Transition metals Other metals Metalloids Other nonmetals Halogens Noble gases Unknown chem. properties Large version 

Hydrogen H2 | Nitrogen N2 | Oxygen O2 | Fluorine F2 | Chlorine Cl2 | Bromine Br2 | Iodine I2 | Astatine At2 | v · d · e Periodic table H   He Li Be   B C N O F Ne Na Mg   Al Si P S Cl Ar K Ca   Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr   Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo Alkali metals Alkaline earth metals Lanthanides Actinides Transition metals Other metals Metalloids Other nonmetals Halogens Noble gases Unknown chem. properties Large version