Antimonides (sometimes called stibnides or stibinides) are compounds of antimony with more electropositive elements. The antimonide ion is Sb(3−) but the term refers also to any anionic derivative of antimony.[1]

Antimonides are often prepared by heating the elements.[2] Alternatively, sodium electride in ammonia dissolves antimony to give an antimonide upon evaporation.[3]

The reduction of antimony leads to alkali metal antimonides of various types, depending on stoichiometry.[4] Known antimonides include isolated Sb(3−) ions (in Li3Sb and Na3Sb). Other motifs include dumbbells Sb2(4−) in Cs4Sb2, discrete antimony chains, for example, Sb6(8−) in SrSb3, infinite spirals (Sb−)_{n} (in NaSb, RbSb), planar four-membered rings Sb4(2−), Sb7(3−) cages in Li3Sb7,[5] and net shaped anions Sb3(2−) in BaSb3.

Some antimonides are semiconductors, e.g. those of the boron group such as indium antimonide. Being reducing, many antimonides are decomposed by oxygen.

See also

References

  1. ^
  2. ^ E. Dönges (1963). "Phosphides, Arsenides, Antimonides and Bismuthides". Handbook of Preparative Inorganic Chemistry, 2nd Ed.. Vol. 2pages=985. G. Brauer (ed.). NY, NY: Academic Press.
  3. ^ Ellis, John E. (2006-04-17). "Adventures with Substances Containing Metals in Negative Oxidation States". Inorganic Chemistry. 45 (8): 3167–3186. doi:10.1021/ic052110i. ISSN 0020-1669
  4. ^ King, R. Bruce (2005). Encyclopedia of Inorganic Chemistry, Second Edition. 2nd ed. Wiley. p. 211. ISBN 9780470860786.
  5. ^ Beswick, Michael A.; Choi, Nick; Harmer, Christopher N.; Hopkins, Alexander D.; McPartlin, Mary; Wright, Dominic S. (1998). "Low-Temperature Synthesis of Zintl Compounds with a Single-Source Molecular Precursor". Science. 281 (5382): 1500–1501. doi:10.1126/science.281.5382.1500. PMID 9727974