| 词条 | Caesium bromide |
| 释义 |
| Watchedfields = changed | verifiedrevid = 443321289 | ImageFile = CsCl polyhedra.png | ImageSize = | IUPACName = Caesium bromide | OtherNames = Cesium bromide, Caesium(I) bromide |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | 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 | UNII = 06M25EDM3F | PubChem = 24592 | InChI = 1/BrH.Cs/h1H;/q;+1/p-1 |Section2={{Chembox Properties | Formula = CsBr | MolarMass = 212.809 g/mol[1] | Appearance = White solid | Density = 4.43 g/cm3[1] | MeltingPtC = 636 | MeltingPt_ref = [1] | BoilingPtC = 1300 | BoilingPt_ref = [1] | Solubility = 1230 g/L (25 °C)[1] | RefractIndex = 1.8047 (0.3 µm) 1.6974 (0.59 µm) 1.6861 (0.75 µm) 1.6784 (1 µm) 1.6678 (5 µm) 1.6439 (20 µm)[2] | MagSus = -67.2·10−6 cm3/mol[3] |Section3={{Chembox Structure | CrystalStruct = CsCl, cP2 | SpaceGroup = Pm{{overline|3}}m, No. 221[4] | 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)[5] |Section8={{Chembox Related | OtherAnions = Caesium fluoride Caesium chloride Caesium iodide Caesium astatide | OtherCations = Sodium bromide Potassium bromide Rubidium bromide Francium 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 a melting point a 636 °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.[6] SynthesisCaesium bromide can be prepared via following reactions:
CsOH (aq) + HBr (aq) → CsBr (aq) + H2O (l) Cs2(CO3) (aq) + 2 HBr (aq) → 2 CsBr (aq) + H2O (l) + CO2 (g)
2 Cs (s) + Br2 (g) → 2 CsBr (s) The direct synthesis is a vigorous reaction of caesium with other halogens. Due to its high cost, it is not used for preparation. UsesCaesium bromide is sometimes used in optics as a beamsplitter component in wide-band spectrophotometers. References1. ^1 2 3 4 Haynes, p. 4.57 2. ^Haynes, p. 10.240 3. ^Haynes, p. 4.132 4. ^{{cite journal|doi=10.1063/1.1713597|title=Elastic Constants of CsBr and CsI from 4.2°K to Room Temperature|journal=Journal of Applied Physics|volume=35|issue=4|pages=1222|year=1964|last1=Vallin|first1=J.|last2=Beckman|first2=O.|last3=Salama|first3=K.}} 5. ^Caesium bromide. nlm.nih.gov 6. ^{{cite journal|doi=10.1107/S0365110X51001641|title=Polymorphism of cesium and thallium halides|journal=Acta Crystallographica|volume=4|issue=6|pages=487|year=1951|last1=Schulz|first1=L. G.}} Cited sources
External links{{Commons category|Caesium bromide}}
4 : Bromides|Metal halides|Caesium compounds|Alkali metal bromides |
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