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Scandium bromide

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Scandium(III) bromide
Names
IUPAC name
Tribromoscandium
Other names
Scandium tribromide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.349 Edit this at Wikidata
EC Number
  • 236-699-6
  • InChI=1S/3BrH.Sc/h3*1H;/q;;;+3/p-3
    Key: APPHYFNIXVIIJR-UHFFFAOYSA-K
  • Br[Sc](Br)Br
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
−2.455 kJ/g
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chlorideFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
0
0
Related compounds
Other anions
 Scandium fluoride
Scandium chloride
Scandium triiodide
Other cations
 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).

Scandium bromide refers to inorganic compounds with the formula ScBr3(H2O)n. The anhydrous trihalide is hygroscopic. Both anhydrous and the hydrate are water soluble, diamagnetic, and colorless.[4]

Preparation and properties

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ScBr3 can be produced by "burning" scandium in bromine gas.[5]

2 Sc + 3 Br2 → 2 ScBr3

Scandium bromide can also be prepared by treating excess hydrobromic acid with scandium oxide. The heptahydrate can be crystallized from the solution. According to X-ray crystallogrphy, [Sc(H2O)7]Br3 featureseven-coordinate Sc3+.[4] The thermal decomposition of the hydrate yields scandium oxybromide (ScOBr) and scandium oxide.[6] The anhydrous form can be produced by the reaction of bromine, scandium oxide and graphite in nitrogen gas.[7]

Heating reaction between ammonium bromide and scandium oxide or scandium bromide hexahydrate, through (NH4)3ScBr6 intermediate, decomposes to obtain anhydrous scandium bromide.[8]

Uses

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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.[9]

References

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  1. ↑ Steinwand, S.J. et al. Inorg. Chem. 36, 6413, (1997)
  2. ↑ "Scandium tribromide".
  3. ↑ "Scandium Bromide".
  4. 1 2 Lim, Kevin C.; Skelton, Brian W.; White, Allan H. (2001). "Crystal Structures of the ('Maximally') Hydrated Scandium Halides, ScX3.nH2O (X = Cl, Br, I)". Australian Journal of Chemistry. 53 (10): 875–878. doi:10.1071/CH00120.
  5. ↑ "WebElements Periodic Table » Scandium » reactions of elements".
  6. ↑ Petrů, F.; Kůtek, F. (1960). "Beiträge zur Chemie seltener Elemente X. Basische Scandiumhalogenide". Collection of Czechoslovak Chemical Communications. 25 (4): 1143–1147. doi:10.1135/cccc19601143. ISSN 1212-6950.
  7. ↑ 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.
  8. ↑ 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.
  9. ↑ "Scandium(III) bromide | CAS 13465-59-3".
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