Barium bromide

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title: "Barium bromide" type: doc version: 1 created: 2026-02-28 author: "Wikipedia contributors" status: active scope: public tags: ["bromides", "alkaline-earth-metal-halides", "barium-compounds"] topic_path: "general/bromides" source: "https://en.wikipedia.org/wiki/Barium_bromide" license: "CC BY-SA 4.0" wikipedia_page_id: 0 wikipedia_revision_id: 0

| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 476999120 | ImageFile = Barium-bromide-xtal-packing-3x3x3-3D-sf.png | ImageCaption = Space-filling model of the crystal structure | ImageSize = | ImageName = Barium bromide |Section1={{Chembox Identifiers | ChemSpiderID_Ref = | ChemSpiderID = 59728 | InChI = 1/Ba.2BrH/h;21H/q+2;;/p-2 | InChIKey = NKQIMNKPSDEDMO-NUQVWONBAE | SMILES = Br[Ba]Br | SMILES2 = [Ba+2].[Br-].[Br-] | StdInChI_Ref = | StdInChI = 1S/Ba.2BrH/h;21H/q+2;;/p-2 | StdInChIKey_Ref = | StdInChIKey = NKQIMNKPSDEDMO-UHFFFAOYSA-L | CASNo_Ref = | CASNo = 10553-31-8 | CASNo_Comment = (anhydrous) | CASNo2_Ref = | CASNo2 = 7791-28-8 | CASNo2_Comment = (dihydrate) | PubChem = 5462743 | PubChem_Comment = (anhydrous) | PubChem2 = 44537612 | PubChem2_Comment = (dihydrate) | UNII_Ref = | UNII = TI8NM689HW | EC_number = 234-140-0 |Section2={{Chembox Properties | Formula = Ba Br2 (anhydrous)

BaBr2·2H2O (dihydrate) | MolarMass = 297.14 g/mol | Appearance = White solid | Density = 4.78 g/cm3 (anhydrous) 3.58 g/cm3 (dihydrate) | Solubility = 92.2 g/100 mL (0°C) | MeltingPtC = 857 | MeltingPt_notes = | BoilingPtC = 1835 | BoilingPt_notes = | MagSus = -92.0·10−6 cm3/mol |Section3={{Chembox Structure | Coordination = | CrystalStruct = PbCl2-type (orthorhombic, oP12) | SpaceGroup = Pnma (No. 62) |Section4={{Chembox Thermochemistry | DeltaHf = −181.1 kcal/mol |Section7={{Chembox Hazards |ExternalSDS = NIH BaBr |MainHazards = Toxic |NFPA-H = 3 |NFPA-F = 0 |NFPA-R = 0 | GHSPictograms = | GHSSignalWord = Warning | HPhrases = | PPhrases = |Section8={{Chembox Related | OtherAnions = Barium fluoride Barium chloride Barium iodide | OtherCations = Beryllium bromide Magnesium bromide Calcium bromide Strontium bromide Radium bromide Lead bromide

Barium bromide is the chemical compound with the formula BaBr2. It is ionic and hygroscopic in nature.

Structure and properties

BaBr2 crystallizes in the lead chloride (cotunnite) motif, giving white orthorhombic crystals that are deliquescent.

::data[format=table title="Coordination geometry of ions in barium bromide{{ cite web | url = http://www.crystallography.net/cod/1527183.html | title = Information card for entry 1527183 | author = | website = [[Crystallography Open Database]] | year = 1963 | publisher = | access-date = 2021-03-26 }}{{ cite web | url = https://www.ccdc.cam.ac.uk/structures/Search?Ccdcid=1596411&DatabaseToSearch=Published | title = ICSD 15706 : ICSD Structure : Ba Br₂ | author = | website = [[Cambridge Structural Database]]: Access Structures | publisher = [[Cambridge Crystallographic Data Centre]] | access-date = 2021-03-26 }}"]

Ion	Ba2+	Br− (tetrahedral)	Br− (trigonal)	Coordination sphere	Ball-and-stick model
{BaBr9}	{BrBa4}	{BrBa3}
[[File:Barium-bromide-xtal-Ba-coordination-3D-bs-17.png	150px]]	[[File:Barium-bromide-xtal-Br1-coordination-3D-bs-17.png	150px]]	[[File:Barium-bromide-xtal-Br2-coordination-3D-bs-17.png	150px]]
9	4	3
(7+2) coordination
distorted tricapped trigonal prismatic	distorted tetrahedral	trigonal pyramidal
::

In aqueous solution BaBr2 behaves as a simple salt.

Solutions of barium bromide reacts with the sulfate salts to produce a solid precipitate of barium sulfate. :BaBr2 + → BaSO4 + 2 Br− Similar reactions occur with oxalic acid, hydrofluoric acid, and phosphoric acid, giving solid precipitates of barium oxalate, fluoride, and phosphate, respectively.

Preparation

Barium bromide can be prepared by treating barium sulfide or barium carbonate with hydrobromic acid: :BaS + 2 HBr → BaBr2 + H2S :BaCO3 + 2 HBr → BaBr2 + CO2 + H2O Barium bromide crystallizes from concentrated aqueous solution in its dihydrate, BaBr2·2H2O. Heating this dihydrate to 120 °C gives the anhydrous salt. | last =Patnaik | first =Pradyot | year = 2003 | title =Handbook of Inorganic Chemical Compounds | publisher = McGraw-Hill Professional | pages = 81–82 | isbn =978-0-07-049439-8 | url= https://books.google.com/books?id=Xqj-TTzkvTEC&q=%22barium+bromide%22+subject:%22Chemistry,+Inorganic%22&pg=RA1-PA81 | access-date = 2007-12-03

Uses

Barium bromide is a precursor to chemicals used in photography and to other bromides. Historically, barium bromide was used to purify radium in a process of fractional crystallization devised by Marie Curie. Since radium precipitates preferentially in a solution of barium bromide, the ratio of radium to barium in the precipitate would be higher than the ratio in the solution. | last =Sime | first =Ruth Lewin | author-link =Ruth Lewin Sime | year = 1996 | title =Lise Meitner: A Life in Physics | publisher = University of California Press | page = 233 | isbn =978-0-520-20860-5 | url= https://books.google.com/books?id=uPzZQzx-mkcC&q=%22barium+bromide%22+radium&pg=PA233 | access-date = 2007-12-03

Safety

Barium bromide, along with other water-soluble barium salts (e.g. barium chloride), is toxic. However, there is no conclusive data available on its hazards.https://www.sigmaaldrich.com/MSDS/MSDS/DisplayMSDSPage.do?country=US&language=en&productNumber=413607&brand=ALDRICH |

In popular culture

The compound appears in the intro title card of Breaking Bad, where the first pairs of letters are replaced with Br35 and Ba56, the symbols and atomic numbers of bromine and barium respectively.

References

(1963). "The Crystal Structures of Barium Chloride, Barium Bromide, and Barium Iodide". [[Journal of Physical Chemistry.
{{Greenwood&Earnshaw
. (1963). ["Information card for entry 1527183"](http://www.crystallography.net/cod/1527183.html). **.
. ["ICSD 15706 : ICSD Structure : Ba Br₂"](https://www.ccdc.cam.ac.uk/structures/Search?Ccdcid=1596411&DatabaseToSearch=Published). *[[Cambridge Crystallographic Data Centre]]*.
{{Greenwood&Earnshaw

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