| Mercury(I) bromide | |
|---|---|
-bromide-xtal-3D-vdW.png) |
|
| IUPAC name |
|
| Other names | Mercurous bromide |
| Identifiers | |
| CAS number | [] |
| RTECS number | ? |
| Properties | |
| Molecular formula | Hg2Br2 |
| Molar mass | 560.99 g/mol |
| Appearance | white tetragonal crystals |
| Density | 7.307 g/cm³, solid |
| Melting point |
405°C |
| Boiling point | |
| Solubility in water | 3.9 x 10-5 g/100 mL |
| Structure | |
| Molecular shape | linear |
| Hazards | |
| EU classification | Very toxic (T+) Dangerous for the environment (N) |
| R-phrases | R26/27/28, R33, R50/53 |
| S-phrases | S13, S28, S45, S60, S61[2] |
| Flash point | non-flammable |
| Related compounds | |
| Other anions | Mercury(I) fluoride Mercury(I) chloride Mercury(I) iodide |
| Other cations | Zinc bromide Cadmium bromide Mercury(II) bromide |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
|
Mercury(I) bromide or mercurous bromide is the chemical compound composed of mercury and bromine with the formula Hg2Br2. It changes color from white to yellow when heated[1] and fluoresces orange when exposed to ultraviolet light. It has applications in acousto-optical devices[3].
A very rare mineralogical form is called kuzminite, Hg2(Br,Cl)2.
Reactions
Mercury(I) bromide is prepared by the oxidation of elemental mercury with elemental bromine or by adding sodium bromide to a solution of mercury(I) nitrate[1]. It decomposes to mercury(II) bromide and elemental mercury[3].
Structure
In common with other Hg(I) (mercurous) compounds which contain linear X-Hg-Hg-X units, Hg2Br2 contains linear BrHg2Br units with an Hg-Hg bond length of 249 pm (Hg-Hg in the metal is 300 pm) and an Hg-Br bond length of 271 pm.[4] The overall coordination of each Hg atom is octahedral as, in addition to the two nearest neighbours, there are four other Br atoms at 332 pm. [4]The compound is often formulated as Hg22+ 2Br−.[5]
References
- ^ a b c Perry, Dale L.; Phillips, Sidney L. (1995), Handbook of Inorganic Compounds, CRC Press, pp. 255, ISBN 0849386713, http://books.google.com/books?id=0fT4wfhF1AsC&pg=PA255&dq=%22Mercury(I)+bromide%22&as_brr=3&sig=9IOtdrqpdYj5BIUYqvEI9PxYFek, retrieved on 2008-05-30
- ^ "483230 Mercury(I) bromide 99.9+ %". Sigma-Aldrich. http://www.sigmaaldrich.com/catalog/search/ProductDetail/ALDRICH/483230. Retrieved on 2008-05-30.
- ^ a b Macintyre, Jane Elizabeth; Daniel, F. M.; Stirling, V. M. (1992), Dictionary of Inorganic Compounds, 1, CRC Press, pp. 314, ISBN 0412301202, http://books.google.com/books?id=YmBiXJ7qRtAC&pg=PA314&dq=Mercury(I)+bromide&sig=0njDGroae4vdeaiZ_abPpcm8No4, retrieved on 2008-05-30
- ^ a b Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
- ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5
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