Jump to content

Trisulfur

From Wikipedia, the free encyclopedia

Trisulfur
Trisulfur.png
Trisulfur.png
Ball-and-stick model of trisulfur
Ball-and-stick model of trisulfur
Names
IUPAC name
Trisulfur
Other names
Thiozone
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
  • InChI=1S/S3/c1-3-2
    Key: NVSDADJBGGUCLP-UHFFFAOYSA-N
  • trisulfanidylo S3−: InChI=1S/HS3/c1-3-2/h1H/p-1
    Key: WMXWXNVGXOWZRJ-UHFFFAOYSA-M
  • [S-][S+]=S
  • trisulfanidylo S3−: [S-]S[S]
Properties
S3
Molar mass 96.198 g/mol
Appearance Cherry-red
Structure
bent
Related compounds
Related compounds
 Ozone
Disulfur monoxide
Sulfur dioxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

The S3 molecule, known as trisulfur, sulfur trimer, thiozone, or triatomic sulfur, is a cherry-red allotrope of sulfur. It comprises about 10% of vaporised sulfur at 713 K (440 °C; 824 °F) and 1,333 Pa (10.00 mmHg; 0.1933 psi). It has been observed at cryogenic temperatures as a solid. Under ordinary conditions it converts to cyclooctasulfur.

8 S3 → 3 S8

Structure and bonding

[edit]

In terms of structure and bonding S3 and ozone (O3) are similar. Both adopt bent structures and are diamagnetic. Although represented with S=S double bonds, the bonding situation is more complex.[1]

The S–S distances are equivalent and are 191.70±0.01 pm, and with an angle at the central atom of 117.36°±0.006°.[2] However, cyclic S3, where the sulfur atoms are arranged in an equilateral triangle with three single bonds (similar to cyclic ozone and cyclopropane), is calculated to be lower in energy than the bent structure experimentally observed.[3] A similar structure has been predicted for ozone, but has not been observed.

The name thiozone was invented by Hugo Erdmann in 1908 who hypothesized that S3 comprises a large proportion of liquid sulfur.[4] However its existence was unproven until the experiments of J. Berkowitz in 1964.[5] Using mass spectrometry, he showed that sulfur vapour contains the S3 molecule. Above 1,200 °C (2,190 °F) S3 is the second most common molecule after S2 in gaseous sulfur.[5] In liquid sulfur the molecule is not common until the temperature is high, such as 500 °C (932 °F). However, small molecules like this contribute to most of the reactivity of liquid sulfur.[5] S3 has an absorption peak of 425 nm (violet) with a tail extending into blue light.[5]

S3 can also be generated by photolysis of S3Cl2 embedded in a glass or matrix of solid noble gas.[5]

Natural occurrence

[edit]

S3 occurs naturally on Io in volcanic emissions. S3 is also likely to appear in the atmosphere of Venus at heights of 20 to 30 km, where it is in thermal equilibrium with S2 and S4.[6]: 546  The reddish colour of Venus' atmosphere at lower levels is likely to be due to S3.[6]: 539 

Reactions

[edit]

S3 reacts with carbon monoxide to make carbonyl sulfide and S2.

Formation of compounds with a defined number of sulfur atoms is possible:

S3 + S2O → S5O (cyclic)[7]

Radical anion

[edit]
Lazurite contains S−3.

Although S3 is elusive under ordinary conditions, the intensely blue radical anion S−3 is abundant.[8] The anion is sometimes called thiozonide,[9] by analogy with the ozonide anion, O−3, to which it is valence isoelectronic. The preferred IUPAC name is trisulfanidylo. The gemstone lapis lazuli and the mineral lazurite (from which the pigment ultramarine is derived) contain S−3. International Klein Blue, developed by Yves Klein, also contains the S−3 radical anion.[10] The blue colour is due to the C2A2 transition to the X2B1 electronic state in the ion,[9] causing a strong absorption band at 610–620 nm or 2.07 eV (in the orange region of the visible spectrum).[11] The Raman frequency is 523 cm−1 and another infrared absorption is at 580 cm−1.[5]

The S−3 ion has been shown to be stable in aqueous solution under a pressure of 0.5 GPa (73,000 psi), and is expected to occur naturally at depth in the Earth's crust where subduction or high pressure metamorphism occurs.[12] This ion is probably important in movement of copper and gold in hydrothermal fluids.[13]

Lithium hexasulfide (which contains S−6, another polysulfide radical anion) with tetramethylenediamine solvation dissociates acetone and related donor solvents to S−3.[14]

The S−3 radical anion was also made by reducing gaseous sulfur with Zn2+ in a matrix. The material is strongly blue-coloured when dry and changes colour to green and yellow in the presence of trace amounts of water.[15] Another way to make it is with polysulfide dissolved in hexamethylphosphoramide where it gives a blue colour.[16]

Other methods of production of S−3 include reacting sulfur with partially hydroxylated magnesium oxide at 400 °C.[17]

Raman spectroscopy can be used to identify S−3, and it can be used non-destructively in paintings. The bands are 549 cm−1 for symmetric stretch, 585 cm−1 for asymmetric stretch, and 259 cm−1 for bending.[18] Natural materials can also contain S−2 which has an optical absorption at 390 nm and Raman band at 590 cm−1.[18]

Trisulfide ion

[edit]

The trisulfide ion, S2−3 is part of the polysulfide series. The sulfur chain is bent at an angle of 107.88°.[5] Strontium trisulfide (SrS3) has a S–S bond length of 205 pm.[5] The bonds are single. It is isoelectronic to sulfur dichloride.

References

[edit]
  1. ^ Greenwood NN, Earnshaw A (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 645–662. ISBN 978-0-08-037941-8.
  2. ^ McCarthy MC, Thorwirth S, Gottlieb CA, Patrick T (11 March 2004). "The rotational spectrum and geometrical structure of thiozone, S3". Journal of the American Chemical Society. 126 (13): 4096–4097. Bibcode:2004JAChS.126.4096M. doi:10.1021/ja049645f. PMID 15053585.
  3. ^ Flemmig B, Wolczanski PT, Hoffmann R (1 June 2005). "Transition metal complexes of cyclic and open ozone and thiozone" (PDF). Journal of the American Chemical Society. 127 (4): 1278–1285. doi:10.1021/ja044809d. PMID 15669867.
  4. ^ Erdmann H (1908). "Ueber Thiozonide, ein Beitrag zur Kenntniss des Schwefels und seiner ringförmigen Verbindungen" [On thiozonide, an article on the knowledge of sulfur and its ring-forming compounds]. Justus Liebigs Annalen der Chemie. 362 (2): 133–173. doi:10.1002/jlac.19083620202.
  5. ^ a b c d e f g h Meyer B (March 1975). "Elemental sulfur" (PDF). Chemical Reviews. 76 (3): 367–388. doi:10.1021/cr60301a003.
  6. ^ a b Lewis JS (2004). Physics and Chemistry of the Solar System. Academic Press. ISBN 978-0-12-446744-6.
  7. ^ Steudel R, Steudel Y (2 November 2004). "The thermal decomposition of S2O forming SO2, S3, S4 and S5O — an ab initio MO study". ChemInform. 35 (44). doi:10.1002/chin.200444022.
  8. ^ Chivers T, Elder PJ (2013). "Ubiquitous trisulfur radical anion: fundamentals and applications in materials science, electrochemistry, analytical chemistry and geochemistry". Chem. Soc. Rev. 42 (14): 5996–6005. doi:10.1039/C3CS60119F. PMID 23628896.
  9. ^ a b Linguerri R, Komiha N, Fabian J, Rosmus P (2008). "Electronic states of the ultramarine chromophore S–
    3    ". Zeitschrift für Physikalische Chemie. 222 (1): 163–176. doi:10.1524/zpch.2008.222.1.163. S2CID 95495454.
  10. ^ Manning CE (25 February 2011). "Sulfur surprises in deep geological fluids". Science. 331 (6020): 1018–1019. Bibcode:2011Sci...331.1018M. doi:10.1126/science.1202468. PMID 21350156. S2CID 206532249.
  11. ^ Steudel R (2003). "Cluster anions S−
    n     and S2−
    n    ". Elemental Sulfur and Sulfur-Rich Compounds. Vol. 2. Springer. p. 16. ISBN 978-3-540-40378-4.
  12. ^ Pokrovski GS, Dubrovinsky LS (25 February 2011). "The S–
    3     ion is stable in geological fluids at elevated temperatures and pressures". Science. 331 (6020): 1052–1054. Bibcode:2011Sci...331.1052P. doi:10.1126/science.1199911. PMID 21350173. S2CID 206530875.
  13. ^ Pokrovsky GS, Kokh MA, Guillaume D, et al. (3 November 2015) [12 October 2015]. "Sulfur radical species form gold deposits on Earth". Proceedings of the National Academy of Sciences. 112 (44): 13484–13489. Bibcode:2015PNAS..11213484P. doi:10.1073/pnas.1506378112. PMC 4640777. PMID 26460040.
  14. ^ Chivers T, Manners I (2009). Inorganic Rings and Polymers of the p-Block Elements: From Fundamentals to Applications. Royal Society of Chemistry. pp. 295–296. ISBN 978-1-84755-906-7.
  15. ^ Gao Q, Xiu Y, Li Gd, Chen Js (2010). "Sensor material based on occluded trisulfur anionic radicals for convenient detection of trace amounts of water molecules". Journal of Materials Chemistry. 20 (16): 3307–3312. doi:10.1039/B925233A.
  16. ^ Chivers T, Drummond I (October 1972). "Characterization of the trisulfur radical anion S−
    3     in blue solutions of alkali polysulfides in hexamethylphosphoramide". Inorganic Chemistry. 11 (10): 2525–2527. doi:10.1021/ic50116a047.
  17. ^ Lunsford JH, Johnson DP (1973). "Electron paramagnetic resonance study of S–
    3     formed on magnesium oxide". The Journal of Chemical Physics. 58 (5): 2079–2083. doi:10.1063/1.1679473.
  18. ^ a b Hark RR, Clark RJ. "Raman microscopy of diverse samples of lapis lazuli at multiple excitation wavelengths" (PDF). Archived from the original (PDF) on 2011-07-26.
[edit]
  • Media related to Trisulfur at Wikimedia Commons
Retrieved from "https://en.wikipedia.org/w/index.php?title=Trisulfur&oldid=1259226709"