Octasulfur

Last updated • 1 min readFrom Wikipedia, The Free Encyclopedia
Octasulfur
Stereo, skeletal formula of octathiocane Molecular Sulfur (S8) V.1.svg
Stereo, skeletal formula of octathiocane
Spacefill model of octathiocane Cyclooctasulfur-above-3D-vdW.png
Spacefill model of octathiocane
Ball and stick model of octathiocane Cyclooctasulfur-above-3D-balls.png
Ball and stick model of octathiocane
Sample of pulverised octasulfur Sulfur2.jpg
Sample of pulverised octasulfur
Names
Systematic IUPAC name
  • cyclo-Octasulfur [1]
  • Octathiocane [2]
  • Cyclooctasulfane
Other names
Octasulfur
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
2973
MeSH Cyclooctasulfur
PubChem CID
UNII
  • InChI=1S/S8/c1-2-4-6-8-7-5-3-1 Yes check.svgY
    Key: JLQNHALFVCURHW-UHFFFAOYSA-N Yes check.svgY
  • S1SSSSSSS1
Properties
S8
Molar mass 256.48 g·mol−1
AppearanceVivid, yellow, translucent crystals
Density 2.07 g/cm3
Melting point 119 °C; 246 °F; 392 K
Boiling point 444.6 °C; 832.4 °F; 717.8 K
log P 6.117
Thermochemistry
Std molar
entropy (S⦵298)
32 J·mol−1·K−1 [3]
0 kJ/mol [3]
Related compounds
Related compounds
 Hexathiane
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Octasulfur is an inorganic substance with the chemical formula S8. It is an odourless and tasteless yellow solid, and is a major industrial chemical. It is the most common allotrope of sulfur and occurs widely in nature. [4]

Contents

Nomenclature

The name octasulfur is the most commonly used for this chemical. It is systematically named cyclo-octasulfur (which is the preferred IUPAC name) and cyclooctasulfane. It is also the final member of the thiocane heterocylic series, where every carbon atom is substituted with a sulfur atom, thus this sulfur allotrope is systematically named octathiocane as well.

Structure

The chemical consists of rings of 8 sulfur atoms. It adopts a crown conformation with D4d point group symmetry. The S–S bond lengths are equal, at about 2.05 Å. Octasulfur crystallizes in three distinct polymorphs: rhombohedral, and two monoclinic forms, of which only two are stable at standard conditions. The rhombohedral crystal form is the accepted standard state. The remaining polymorph is only stable between 96 and 115 °C at 100 kPa. Octasulfur forms several allotropes: α-sulfur, β-sulfur, γ-sulfur, and λ-sulfur.

λ-Sulfur is the liquid form of octasulfur, from which γ-sulfur can be crystallised by quenching. If λ-sulfur is crystallised slowly, it will revert to β-sulfur. Since it must have been heated over 115 °C, neither crystallised β-sulfur or γ-sulfur will be pure. The only known method of obtaining pure γ-sulfur is by crystallising from solution.

Octasulfur easily forms large crystals, which are typically yellow and are somewhat translucent.

Production and reactions

Octasulfur is not typically produced as S8 per se. It is the main (99%) component of elemental sulfur, which is recovered from volcanic sources and is a major product of the Claus process, associated with petroleum refineries.

See also

References

  1. ↑ International Union of Pure and Applied Chemistry (2005). Nomenclature of Inorganic Chemistry (IUPAC Recommendations 2005). Cambridge (UK): RSC–IUPAC. ISBN   0-85404-438-8. p. 49. Electronic version.
  2. ↑ "cyclooctasulfur (CHEBI:29385)". Chemical Entities of Biological Interest. UK: European Bioinformatics Institute. Main.
  3. 1 2 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN   978-0-618-94690-7.
  4. ↑ Steudel, R., "Homocyclic Sulfur Molecules", Topics Curr. Chem. 1982, 102, 149.
This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.