A | B | C | D | E | F | G | H | CH | I | J | K | L | M | N | O | P | Q | R | S | T | U | V | W | X | Y | Z | 0 | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9
Names | |
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IUPAC name
Rubidium bromide
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Other names
Rubidium(I) bromide
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Identifiers | |
3D model (JSmol)
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ChemSpider | |
ECHA InfoCard | 100.029.238 |
PubChem CID
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UNII | |
CompTox Dashboard (EPA)
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Properties | |
RbBr | |
Molar mass | 165.372 g/mol |
Appearance | white crystalline solid |
Density | 3.350 g/cm3 |
Melting point | 693 °C (1,279 °F; 966 K) |
Boiling point | 1,340 °C (2,440 °F; 1,610 K) |
98 g/100 mL | |
−56.4·10−6 cm3/mol | |
Hazards | |
Flash point | Non-flammable |
Related compounds | |
Other anions
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Rubidium fluoride Rubidium chloride Rubidium iodide Rubidium astatide |
Other cations
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Lithium bromide Sodium bromide Potassium bromide Caesium bromide Francium bromide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
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Rubidium bromide is an inorganic compound with the chemical formula RbBr. It is a salt of hydrogen bromide. It consists of bromide anions Br− and rubidium cations Rb+. It has a NaCl crystal structure, with a lattice constant of 685 picometres.[1]
There are several methods for synthesising rubidium bromide. One involves reacting rubidium hydroxide with hydrobromic acid:
- RbOH + HBr → RbBr + H2O
Another method is to neutralize rubidium carbonate with hydrobromic acid:
- Rb2CO3 + 2 HBr → 2 RbBr + H2O + CO2
Rubidium metal would react directly with bromine to form RbBr, but this is not a sensible production method, since rubidium metal is substantially more expensive than the carbonate or hydroxide; moreover, the reaction would be explosive.
References
- ^ G. Chern; J. G. Skofronick; W. P. Brug; S. A. Safron (1989). "Surface phonon modes of the RbBr(001) crystal surface by inelastic He-atom scattering". Phys. Rev. B. 39 (17): 12838–12844. doi:10.1103/PhysRevB.39.12838. PMID 9948158.
- WebElements. URL accessed March 1, 2006.
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