Chemistry:Scandium bromide
| Names | |
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| IUPAC name
Tribromoscandium
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| Other names
Scandium tribromide
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
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PubChem CID
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| Properties | |
| ScBr3 | |
| Molar mass | 284.67 g/mol |
| Appearance | anhydrous powder |
| Density | 3.914 g/cm3 |
| Melting point | 904 °C (1,659 °F; 1,177 K)[1][2][3] |
| soluble | |
| Solubility | soluble in ethanol |
| Thermochemistry | |
Std enthalpy of
formation (ΔfH⦵298) |
-2.455 kJ/g |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other anions
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Scandium fluoride Scandium chloride Scandium triiodide |
Other cations
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Yttrium(III) bromide Lutetium(III) bromide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Scandium bromide, or ScBr3, is a trihalide, hygroscopic, water-soluble chemical compound of scandium and bromine.
Preparation and properties
ScBr3 is produced through the burning of scandium in bromine gas.[4]
- 2 Sc(s) + 3 Br2(g) → 2 ScBr3(s)
Scandium bromide can also be prepared by reacting excess hydrobromic acid with scandium oxide, and the hexahydrate can be crystallized from the solution. The thermal decomposition of hexahydrate can only yield scandium oxybromide (ScOBr) and scandium oxide.[5] The anhydrous form can be produced by the reaction of bromine, scandium oxide and graphite in nitrogen gas.[6]
Heating reaction between ammonium bromide and scandium oxide or scandium bromide hexahydrate, through (NH4)3ScBr6 intermediate, decomposes to obtain anhydrous scandium bromide.[7]
Uses
Scandium bromide is used for solid state synthesis of unusual clusters such as Sc19Br28Z4, (Z=Mn, Fe, Os or Ru). These clusters are of interest for their structure and magnetic properties.[8]
References
- ↑ Steinwand, S.J. et al. Inorg. Chem. 36, 6413, (1997)
- ↑ "Scandium tribromide". https://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=83495.
- ↑ "Scandium Bromide". http://www.americanelements.com/scbr.html.
- ↑ "WebElements Periodic Table » Scandium » reactions of elements". http://www.webelements.com/scandium/chemistry.html.
- ↑ Petrů, F.; Kůtek, F. (1960). "Beiträge zur Chemie seltener Elemente X. Basische Scandiumhalogenide" (in en). Collection of Czechoslovak Chemical Communications 25 (4): 1143–1147. doi:10.1135/cccc19601143. ISSN 1212-6950. http://cccc.uochb.cas.cz/25/4/1143/.
- ↑ Reid, Allen Forrest; Wadsley, Arthur D.; Sienko, Michell J. (Jan 1968). "Crystal chemistry of sodium scandium titanate, NaScTiO4, and its isomorphs". Inorganic Chemistry 7 (1): 112–118. doi:10.1021/ic50059a024. ISSN 0020-1669. http://dx.doi.org/10.1021/ic50059a024.
- ↑ Meyer, Gerd; Dötsch, Siegfried; Staffel, Thomas (1987-01-01). "The ammonium-bromide route to anhydrous rare earth bromides MBr3". Journal of the Less Common Metals 127: 155–160. doi:10.1016/0022-5088(87)90372-9. ISSN 0022-5088. https://dx.doi.org/10.1016/0022-5088%2887%2990372-9.
- ↑ "Scandium(III) bromide | CAS 13465-59-3". https://www.scbt.com/scbt/product/scandium-iii-bromide-13465-59-3.
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