GetWiki

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider{edih}
| ChemSpiderID = 22994
| SMILES = [Cs+].[Br-]
| InChIKey = LYQFWZFBNBDLEO-REWHXWOFAA
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/BrH.Cs/h1H;/q;+1/p-1
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = LYQFWZFBNBDLEO-UHFFFAOYSA-M
| CASNo = 7787-69-1
| CASNo_Ref = {{cascite|correct|CAS}}
| EINECS = 232-130-0
| RTECS = FK9275000
| UNII = 06M25EDM3F
| PubChem = 24592
| InChI = 1/BrH.Cs/h1H;/q;+1/p-1
}}|Section2={{Chembox Properties
| Formula = CsBr
| MolarMass = 212.809 g/molHaynes, p. 4.57
| Appearance = White solid
| Density = 4.43 g/cm3
| MeltingPtC = 636| MeltingPt_ref =
| BoilingPtC = 1300| BoilingPt_ref =
| Solubility = 1230 g/L (25 °C) Disputed.

}}|Section3={hide}Chembox Structure

Caesium chloride>CsCl, cP2

3{edih}m, No. 22110.1063/1.1713597>TITLE=ELASTIC CONSTANTS OF CSBR AND CSI FROM 4.2K TO ROOM TEMPERATURE

VOLUME=35

PAGES=1222

LAST1=VALLIN

LAST2=BECKMAN

LAST3=SALAMA

BIBCODE=1964JAP....35.1222V, | LattConst_a = 0.4291 nm| UnitCellFormulas = 1| UnitCellVolume =0.0790 nm3| Coordination = Cubic (Cs+)Cubic (Br−) }}|Section4={{Chembox Hazards | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 0 | GHSSignalWord=Warning | GHSPictograms={{GHS07}} | HPhrases = {{H-phrases|302|315|319|335}} | PPhrases = {{P-phrases|261|264|270|271|280|301+312|302+352|304+340|305+351+338|312|321|330|332+313|337+313|362|403+233|405|501}} | FlashPt = Non-flammable | LD50 = 1400 mg/kg (oral, rat)Caesium bromide. nlm.nih.gov }}|Section8={{Chembox Related | OtherAnions = Caesium fluorideCaesium chlorideCaesium iodideCaesium astatide | OtherCations = Sodium bromidePotassium bromideRubidium bromideFrancium bromide }} }}Caesium bromide or cesium bromide is an ionic compound of caesium and bromine with the chemical formula CsBr. It is a white or transparent solid with melting point at 636 Â°C that readily dissolves in water. Its bulk crystals have the cubic CsCl structure, but the structure changes to the rocksalt type in nanometer-thin film grown on mica, LiF, KBr or NaCl substrates.JOURNAL, 10.1107/S0365110X51001641, Polymorphism of cesium and thallium halides, Acta Crystallographica, 4, 6, 487–489, 1951, Schulz, L. G., Synthesis Caesium bromide can be prepared via following reactions: Neutralization: CsOH (aq) + HBr (aq) → CsBr (aq) + H2O (l) Cs2(CO3) (aq) + 2 HBr (aq) → 2 CsBr (aq) + H2O (l) + CO2 (g) Direct synthesis: 2 Cs (s) + Br2 (g) → 2 CsBr (s) The direct synthesis is a vigorous reaction of caesium with bromine. Due to its high cost, it is not used for preparation. Uses Caesium bromide is sometimes used in optics as a beamsplitter component in wide-band spectrophotometers. References {{Reflist}}* Crystran Ltd experimental data July 2021 {{Webarchive|url=https://web.archive.org/web/20121218002818weblink |date=2012-12-18 }} Cited sources {{RubberBible92nd}} External links {{Commons category|Caesium bromide}} MSDS at Oxford University {{Webarchive|url=https://web.archive.org/web/20071017044744weblink |date=2007-10-17 }} Crystran Physical data {{Webarchive|url=https://web.archive.org/web/20121218002818weblink |date=2012-12-18 }}, weblink" title="web.archive.org/web/20070927230133weblink">IR transmission spectrum Ultra-violet photoabsorption measurements in alkali iodide and caesium bromide evaporated films {{Caesium compounds}}{{Bromides}}{{Authority control}}