Chemistry:Rubidium bromide
From HandWiki
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| 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 | |
PubChem CID
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| UNII | |
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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 [77 °F], 100 kPa). | |
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| Infobox references | |
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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