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Revision as of 12:35, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 473644809 of page Radium_bromide for the Chem/Drugbox validation project (updated: 'CASNo').		Latest revision as of 15:16, 25 July 2024 edit Starmakerthing (talk | contribs)36 edits added imageTag: Visual edit
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	{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}}
	{{Chembox		{{Chembox
	| Verifiedfields = changed		| Verifiedfields = changed
			| Watchedfields = changed
	| verifiedrevid = 464379716		| verifiedrevid = 476995008
	| ImageFile = Ra bromid.jpg		| ImageFile = Ra bromid.jpg
	| ImageSize = 150px
	| ImageCaption = Radium (II) bromide		| ImageFile1 = Radium Bromide.png
	| Reference = <ref name="hand">{{cite book | last = Lide | first = David R. | year = 1998		| ImageSize =
			| ImageCaption = Radium bromide
			| Reference = <ref name="hand">{{cite book | last = Lide | first = David R. | year = 1998
	| title = Handbook of Chemistry and Physics		| title = Handbook of Chemistry and Physics
	| edition = 87 | volume =		| edition = 87 | volume =
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	| publisher = CRC Press		| publisher = CRC Press
	| isbn = 0-8493-0594-2 | pages = 4–78}}</ref><ref name="Chemical">Chemical Compounds (Inorganic); B-Table, Record No. 2630. ''International Critical Tables of Numerical Data, Physics, Chemistry and Technology (1st Electronic Edition''). '''2000'''</ref>		| isbn = 0-8493-0594-2 | pages = 4–78}}</ref><ref name="Chemical">Chemical Compounds (Inorganic); B-Table, Record No. 2630. ''International Critical Tables of Numerical Data, Physics, Chemistry and Technology (1st Electronic Edition''). '''2000'''</ref>
	| IUPACName = radium bromide		| IUPACName = radium bromide
	| OtherNames = radium bromide		| OtherNames = radium bromide
	| Section1 = {{Chembox Identifiers		| Section1 = {{Chembox Identifiers
		⚫	| CASNo_Ref = {{cascite|correct|CAS}}
		⚫	| CASNo = 10031-23-9
			| EINECS = 233-086-5
			| UNII_Ref = {{fdacite|correct|FDA}}
			| UNII = R74O7T8569
		⚫	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
		⚫	| ChemSpiderID=20138062
		⚫	| PubChem =
		⚫	| SMILES = BrBr
	| InChI = 1/2BrH.Ra/h2*1H;/q;;+2/p-2		| InChI = 1/2BrH.Ra/h2*1H;/q;;+2/p-2
	| InChIKey = GIKWXTHTIQCTIH-NUQVWONBAJ		| InChIKey = GIKWXTHTIQCTIH-NUQVWONBAJ
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	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = GIKWXTHTIQCTIH-UHFFFAOYSA-L		| StdInChIKey = GIKWXTHTIQCTIH-UHFFFAOYSA-L
		⚫	}}
⚫	| CASNo_Ref = {{cascite|changed|??}}
		⚫	| Section2 = {{Chembox Properties
⚫	| CASNo = <!-- blanked - oldvalue: 10031-23-9 -->
⚫	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
⚫	| ChemSpiderID=20138062
⚫	| PubChem =
⚫	| SMILES = ..
⚫	}}
⚫	| Section2 = {{Chembox Properties
	| Formula = RaBr<sub>2</sub>		| Formula = RaBr<sub>2</sub>
	| Molar Mass = 385.782 g/mol		| MolarMass = 385.782 g/mol
	| Appearance = white ] crystals		| Appearance = white ] crystals
	| Density = 5.79 g/cm<sup>3</sup>		| Density = 5.79 g/cm<sup>3</sup>
	| Melting Pt = 728°C		| MeltingPtC = 728
	| Boiling Pt = subl 900		| BoilingPtC = 900
			| BoilingPt_notes = sublimes
	| Solubility = 70.6 g/100 g at 20°C		| Solubility = 70.6 g/100 g at 20°C
	}}		}}
	| Section3 = {{Chembox Hazards		| Section3 = {{Chembox Hazards
	| MainHazards =		| MainHazards =
	| FlashPt =		| FlashPt =
	| Autoignition =		| AutoignitionPt =
	}}		}}
	| Section4 = {{Chembox Thermochemistry		| Section4 = {{Chembox Thermochemistry
	| DeltaHf =		| DeltaHf =
	| DeltaHc =		| DeltaHc =
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	| HeatCapacity =		| HeatCapacity =
	}}		}}
	| Section8 = {{Chembox Related		| Section8 = {{Chembox Related
	| OtherAnions = ]		| OtherAnions = ]
			| OtherCations = ]<br />]<br />]<br />]<br />]
	| OtherCations =
	| OtherFunctn =		| OtherFunction =
	| Function =		| OtherFunction_label =
	| OtherCpds =		| OtherCompounds =
	}}		}}
			| Section9 = {{Chembox Hazards
			| MainHazards = Radioactive, highly toxic, explosive, dangerous for the environment
			| NFPA-H = 4
			| NFPA-F = 0
			| NFPA-R = 3
			| NFPA-S = RA
			| GHSPictograms = {{GHS01}}{{GHS06}}{{GHS08}}{{GHS09}}
			}}
	}}		}}
			'''Radium bromide''' is the ] ] of ], with the formula RaBr<sub>2</sub>. It is produced during the process of separating radium from ] ]. This inorganic compound was discovered by ] and ] in 1898, and the discovery sparked a huge interest in ] and ]. Since elemental radium oxidizes readily in air and water, radium salts are the preferred chemical form of radium to work with.<ref name="Babcock">Babcock, A.B., Jr. Survey of Processes for Radium Recovery from Pitchblende Ores. ''AEC Research and Development Report''. '''23 Feb 1950'''. No. NYO—112</ref> Even though it is more stable than elemental radium, radium bromide is still extremely toxic, and can explode under certain conditions.<ref name="Kirby">Kirby, H.W; Salutsky, Murrell L. The Radiochemistry of Radium. ''Energy Citations Database'' '''Dec 1964'''.</ref>
			==History==
			After the Curies discovered radium (in the form of ]) in 1898, scientists began to isolate radium on an industrial scale, with the intent of using it for ] treatments. Radium salts, including radium bromide, were most often used by placing the chemical in a tube that was then passed over or inserted into diseased tissue in the body. Many of the first scientists to try to determine ] were affected by their exposure to the radioactive material. Pierre Curie went so far as to self-inflict a severe chemical skin reaction by applying a radium source directly to his forearm, which ultimately created a skin lesion.<ref name="Dutreix">Dutreix, Jean; Pierquin, Bernard; Tubiana, Maurice. The Hazy Dawn of Brachytherapy. ''Radiotherapy and Oncology'' (49) '''1998''' 223-232</ref> All types of therapeutic tests were performed for different skin diseases including ], ] and ]. Later, it was hypothesized that radium could be used to treat cancerous diseases.
			However, during this time frame, radium also gained popularity among pseudoscientific "health remedy" industries, ] that could "heal" and "reinvigorate" cells in the human body and remove poisonous substances. As a result, radium gained popularity as a "health trend" in the 1920s and radium salts were added to food, drinks, clothing, toys, and even toothpaste.<ref name="Harvie">Harvie, David I. The Radium Century. ''Endeavor'' '''1999''' Vol. 23, Issue 3: 100-105</ref> Furthermore, many respectable journals and newspapers in the early 1900s published statements claiming that radium posed no health hazard.
			The main problem with the growth of interest in radium was the lack of radium on earth itself. In 1913, it was reported that the ] had four grams of radium total, which at the time was more than half the world supply.<ref name="Harvie"/> Numerous countries and institutions across the world set out to extract as much radium as possible, a time-consuming and expensive task. It was reported in ''Science'' magazine in 1919 that the United States had produced approximately 55 grams of radium since 1913, which was also more than half the radium produced in the world at the time.<ref name="Voil">Voil, Charles H. Radium Production. ''Science'' '''17 March 1919''' Vol. 49, No 1262: 227-228</ref> A principal source for radium is ], which holds a total of 257&nbsp;mg of radium per ton of U<sub>3</sub>O<sub>8</sub>.<ref name="Babcock"/> With so little product recovered from such a large amount of material, it was difficult to extract a large quantity of radium. This was the reason radium bromide became one of the most expensive materials on earth. In 1921, it was stated in ''Time'' magazine that one ton of radium cost 17,000,000,000 Euros, whereas one ton of gold cost 208,000 Euros and one ton of diamond cost 400,000,000 Euros.<ref name="Harvie"/>
			Radium bromide was also found to induce ] at normal temperatures.<ref name="Nature">100 and 50 years ago. ''Nature'' '''24 July 2003''' Vol. 424, Issue 6927: 381</ref> This led to the US army manufacturing and supplying ] watches and gun sights to soldiers. It also allowed for the invention of the ], which soon became a popular household item.<ref name="Schwarcz">Schwarcz, Joe. A Dazzling display in a little jar. ''The Gazette: Saturday Extra; The Right Chemistry'' pg B5</ref>
			==Properties==
			Radium bromide is a luminous salt that causes the air surrounding it, even when encased in a tube, to glow a brilliant green and demonstrate all bands of the nitrogen spectrum. It is possible that the effect of the ] on the ] in the air causes this ]. Radium bromide is highly reactive and crystals can sometimes explode, especially if heated. Helium gas evolved from alpha particles can accumulate within the crystals, which can cause them to weaken and rupture.
			Radium bromide will crystallize when separated from aqueous solution. It forms a ], very similar to ].<ref name="Kirby"/>
			==Production==
			Radium is obtained from uranium or ] ores by the "Curie method", which involves two major stages. In the first stage the ore is treated with sulfuric acid dissolves many components. The residue contains, barium, radium, and lead sulfates. The mixture will then be treated with ] and sodium carbonate to remove the lead. The second stage involves separation of the barium from the radium.<ref name="Babcock" /><ref name="Kirby" />
			Radium bromide can be obtained from radium chloride by reaction with a stream of ].<ref name="Kirby"/>
			==Hazards==
			Radium bromide, like all radium compounds, is highly radioactive and very toxic. Due to its chemical similarity to ], radium tends to accumulate in the bones, where it irradiates the ] and can cause ], ], ], ], genetic defects, ], ulcers, and ]. Symptoms of poisoning can take years to develop, by which time it is usually too late for any effective medical treatment. Radium bromide also poses a severe ], amplified due to its high ] in water, and it can ] and cause long-lasting damage to organisms.{{citation needed|date=September 2023}}
			Radium bromide is highly reactive, and crystals can explode if violently shocked or heated. This is, in part, due to self-damage of the crystals by alpha radiation, which weakens the lattice structure.{{dubious|date=September 2023}}
			==Uses==
			Radium and radium salts were commonly used for treating ]; however, these treatments have been mostly phased out in favor of less toxic chemicals such as ] or ].<ref name="Harvie" /> Radium bromide was also used in luminous paint on watches, but its use was ultimately phased out in the 1960-1970s in favor of less dangerous chemicals like ] and ].
			==See also==
			*]
			*]
			*]
			==References==
			{{Reflist}}
			{{Radium compounds}}
			{{Bromides}}
			{{DEFAULTSORT:Radium Bromide}}
			]
			]
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