Caesium 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]

Caesium bromide
Names
IUPAC name
Caesium bromide
Other names
Cesium bromide,
Caesium(I) bromide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.209
EC Number
  • 232-130-0
UNII
Properties
CsBr
Molar mass 212.809 g/mol[1]
Appearance White solid
Density 4.43 g/cm3[1]
Melting point 636 °C (1,177 °F; 909 K)[1]
Boiling point 1,300 °C (2,370 °F; 1,570 K)[1]
1230 g/L (25 °C)[1]
-67.2·10−6 cm3/mol[2]
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)[3]
Structure
CsCl, cP2
Pm3m, No. 221[4]
a = 0.4291 nm
0.0790 nm3
1
Cubic (Cs+)
Cubic (Br−)
Hazards
GHS pictograms
GHS Signal word Warning
GHS hazard statements
 H302, H315, H319, H335
P261, P264, P270, P271, P280, P301+312, P302+352, P304+340, P305+351+338, P312, P321, P330, P332+313, P337+313, P362, P403+233, P405, P501
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
2
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1400 mg/kg (oral, rat)[5]
Related compounds
Other anions
 Caesium fluoride
Caesium chloride
Caesium iodide
Caesium astatide
Other cations
 Sodium bromide
Potassium bromide
Rubidium bromide
Francium bromide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y verify (what is YN ?)
Infobox references

Synthesis

Caesium 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)
  • Direct synthesis:
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.

Uses

Caesium bromide is sometimes used in optics as a beamsplitter component in wide-band spectrophotometers.

gollark: Rust.
gollark: Well, that's more interesting than your idea.
gollark: Ever played (Sid Meier's) Civilization series?
gollark: Well, a small one, yes.
gollark: That's not a civilization. That is a small tribe.

References
  1. Haynes, p. 4.57
  2. Haynes, p. 4.132
  3. Haynes, p. 10.240
  4. Vallin, J.; Beckman, O.; Salama, K. (1964). "Elastic Constants of CsBr and CsI from 4.2°K to Room Temperature". Journal of Applied Physics. 35 (4): 1222. doi:10.1063/1.1713597.
  5. Caesium bromide. nlm.nih.gov
  6. Schulz, L. G. (1951). "Polymorphism of cesium and thallium halides". Acta Crystallographica. 4 (6): 487. doi:10.1107/S0365110X51001641.

Cited sources
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.