Encyclopedia of Metalloproteins

2013 Edition
| Editors: Robert H. Kretsinger, Vladimir N. Uversky, Eugene A. Permyakov

Strontium, Physical and Chemical Properties

  • Timothy P. Hanusa
Reference work entry
DOI: https://doi.org/10.1007/978-1-4614-1533-6_174

Synonyms

Definition

A heavy member of the alkaline-earth elements (atomic number 38), strontium is a soft, silvery, highly reactive metal. Its compounds have various uses, particularly in pyrotechnics, as phosphors, and in sugar refining. Strontium salts are generally nontoxic, and the human body treats strontium much as it does calcium; strontium supplementation can be used to increase bone density and growth.

Background

Strontium is a member of the alkaline-earth family of metals (Group 2 in the periodic table). It is a relatively common element, ranking approximately 15th in natural abundance in the Earth’s crust; it is more plentiful than, for example, sulfur or chromium. The free metal does not occur in nature, but is found combined in minerals such as celestite (strontium sulfate, SrSO 4) (Fig. 1), or less commonly, in strontianite (strontium carbonate, SrCO 3). A mineral from a lead mine near the village of Strontian, in Scotland, was...
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References

  1. Braithwaite N, Weaver G (1990) Electronic materials. Butterworth, LondonGoogle Scholar
  2. De Deckker P (2004) On the celestite-secreting Acantharia and their effect on seawater strontium to calcium ratios. Hydrobiologia 517:1–13CrossRefGoogle Scholar
  3. Hanusa TP et al (2007) Alkaline-earth metals: beryllium, magnesium, calcium, strontium, and barium. In: Crabtree RH, Mingos DMP (eds) Comprehensive organometallic chemistry-III, vol 2. Elsevier, Oxford, pp 67–152CrossRefGoogle Scholar
  4. Hargittai M (2000) Molecular structure of metal halides. Chem Rev 100:2233–2301CrossRefPubMedGoogle Scholar
  5. Haeckel E (1904) Kunstformen der Natur. Bibliographisches Institut, Leipzig, plate 21Google Scholar
  6. Kaupp M, Schleyer PvR (1992) The structural variations of monomeric alkaline earth MX2 compounds (M = Ca, Sr, Ba; X = Li, BeH, BH2, CH3, NH2, OH, F). An ab initio pseudopotential study. J Am Chem Soc 114:491–497CrossRefGoogle Scholar
  7. Lin X, Doble DMJ et al (2003) Cationic assembly of metal complex aggregates: structural diversity, solution stability, and magnetic properties. J Am Chem Soc 125:9476–9483CrossRefPubMedGoogle Scholar
  8. Panthöfer M, Wedig U et al (2004) Geometric and electronic structure of polymeric C70-fullerides: the case of \( {}_{\infty }^1 \)[C703−]. Solid State Sci 6:619–624CrossRefGoogle Scholar
  9. Pierson HO (1999) Handbook of chemical vapor deposition: principles, technology, and applications. Noyes, NorwichGoogle Scholar
  10. Rodriguez-Cruz SE, Williams ER (2001) Gas-phase reactions of hydrated alkaline earth metal ions, M2+(H2O)n (M = Mg, Ca, Sr, Ba and n = 4-7), with benzene. J Am Soc Mass Spectrom 12:250–257CrossRefPubMedGoogle Scholar
  11. Westerhausen M (1998) Synthesis, properties, and reactivity of alkaline earth metal bis[bis(trialkylsilyl)amides]. Coord Chem Rev 176:157–210CrossRefGoogle Scholar

Copyright information

© Springer Science+Business Media New York 2013

Authors and Affiliations

  1. 1.Department of ChemistryVanderbilt UniversityNashvilleUSA