Chemistry:Pyrene

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Short description: Chemical compound
Pyrene
Structural formula of pyrene
Ball-and-stick model of the pyrene molecule
Pyrene crystal 1.jpg
Names
Preferred IUPAC name
Pyrene[1]
Other names
Benzo[def]phenanthrene
Identifiers
3D model (JSmol)
1307225
ChEBI
ChEMBL
ChemSpider
84203
KEGG
RTECS number
  • UR2450000
UNII
Properties
C16H10
Molar mass 202.256 g·mol−1
Appearance colorless solid

(yellow impurities are often found at trace levels in many samples).

Density 1.271 g/cm3[2]
Melting point 150.62 °C (303.12 °F; 423.77 K)[2]
Boiling point 394 °C (741 °F; 667 K)[2]
0.049 mg/L (0 °C)
0.139 mg/L (25 °C)
2.31 mg/L (75 °C)[3]
log P 5.08[4]
Band gap 2.02 eV[5]
-147·10−6 cm3/mol[6]
Structure[7]
Monoclinic
P21/a
a = 13.64 Å, b = 9.25 Å, c = 8.47 Å
α = 90°, β = 100.28°, γ = 90°
4
Thermochemistry[8]
229.7 J/(K·mol)
224.9 J·mol−1·K−1
125.5 kJ·mol−1
Enthalpy of fusion (ΔfH⦵fus)
 17.36 kJ·mol−1
Hazards
Main hazards irritant
GHS pictograms GHS07: HarmfulGHS09: Environmental hazard
GHS Signal word Warning
NFPA 704 (fire diamond)
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
1
2
0
Flash point non-flammable
Related compounds
Related PAHs
 benzopyrene
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
Tracking categories (test):

Pyrene is a polycyclic aromatic hydrocarbon (PAH) consisting of four fused benzene rings, resulting in a flat aromatic system. The chemical formula is C
16H
10. This yellow-green solid is the smallest peri-fused PAH (one where the rings are fused through more than one face). Pyrene forms during incomplete combustion of organic compounds.[10]

Occurrence and properties

Pyrene was first isolated from coal tar, where it occurs up to 2% by weight. As a peri-fused PAH, pyrene is much more resonance-stabilized than its five-member-ring containing isomer fluoranthene. Therefore, it is produced in a wide range of combustion conditions. For example, automobiles produce about 1 μg/km.[11]

Reactions

Oxidation with chromate affords perinaphthenone and then naphthalene-1,4,5,8-tetracarboxylic acid. Pyrene undergoes a series of hydrogenation reactions and is susceptible to halogenation, Diels-Alder additions, and nitration, all with varying degrees of selectivity.[11] Bromination occurs at one of the 3-positions.[12]

Reduction with sodium affords the radical anion. From this anion, a variety of pi-arene complexes can be prepared.[13]

Photophysics

Pyrene and its derivatives are used commercially to make dyes and dye precursors, for example pyranine and naphthalene-1,4,5,8-tetracarboxylic acid. It has strong absorbance in UV-Vis in three sharp bands at 330 nm in DCM. The emission is close to the absorption, but moving at 375 nm.[14] The morphology of the signals change with the solvent. Its derivatives are also valuable molecular probes via fluorescence spectroscopy, having a high quantum yield and lifetime (0.65 and 410 nanoseconds, respectively, in ethanol at 293 K). Pyrene was the first molecule for which excimer behavior was discovered.[15] Such excimer appears around 450 nm. Theodor Förster reported this in 1954.[16]

Applications

STM image of self-assembled Br4Py molecules on Au(111) surface (top) and its model (bottom; pink spheres are Br atoms).[17]

Pyrene's fluorescence emission spectrum is very sensitive to solvent polarity, so pyrene has been used as a probe to determine solvent environments. This is due to its excited state having a different, non-planar structure than the ground state. Certain emission bands are unaffected, but others vary in intensity due to the strength of interaction with a solvent.

Diagram showing the numbering and ring fusion locations of pyrene according to IUPAC nomenclature of organic chemistry.

Pyrenes are strong electron donor materials and can be combined with several materials in order to make electron donor-acceptor systems which can be used in energy conversion and light harvesting applications.[14]

Safety and environmental factors

Although it is not as problematic as benzopyrene, animal studies have shown pyrene is toxic to the kidneys and liver. It is now known that pyrene affects several living functions in fish and algae.[18][19][20][21]

Its biodegradation has been heavily examined. The process commences with dihydroxylation at each of two kinds of CH=CH linkages.[22] Experiments in pigs show that urinary 1-hydroxypyrene is a metabolite of pyrene, when given orally.[23]

See also

References

  1. ↑ International Union of Pure and Applied Chemistry (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. The Royal Society of Chemistry. pp. 206. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4. 
  2. ↑ 2.0 2.1 2.2 Haynes, p. 3.472
  3. ↑ Haynes, p. 5.162
  4. ↑ Haynes, p. 5.176
  5. ↑ Haynes, p. 12.96
  6. ↑ Haynes, p. 3.579
  7. ↑ Camerman, A.; Trotter, J. (1965). "The crystal and molecular structure of pyrene". Acta Crystallographica 18 (4): 636–643. doi:10.1107/S0365110X65001494. 
  8. ↑ Haynes, pp. 5.34, 6.161
  9. ↑ GHS: PubChem
  10. ↑ Figueira-Duarte, Teresa M.; Müllen, Klaus (2011). "Pyrene-Based Materials for Organic Electronics". Chemical Reviews 111 (11): 7260–7314. doi:10.1021/cr100428a. PMID 21740071. 
  11. ↑ 11.0 11.1 Senkan, Selim and Castaldi, Marco (2003) "Combustion" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim.
  12. ↑ Gumprecht, W. H. (1968). "3-Bromopyrene". Org. Synth. 48: 30. doi:10.15227/orgsyn.048.0030. 
  13. ↑ Kucera, Benjamin E.; Jilek, Robert E.; Brennessel, William W.; Ellis, John E. (2014). "Bis(pyrene)metal complexes of vanadium, niobium and titanium: Isolable homoleptic pyrene complexes of transition metals". Acta Crystallographica Section C: Structural Chemistry 70 (8): 749–753. doi:10.1107/S2053229614015290. PMID 25093352. 
  14. ↑ 14.0 14.1 Tagmatarchis, Nikos; Ewels, Christopher P.; Bittencourt, Carla; Arenal, Raul; Pelaez-Fernandez, Mario; Sayed-Ahmad-Baraza, Yuman; Canton-Vitoria, Ruben (2017-06-05). "Functionalization of MoS 2 with 1,2-dithiolanes: toward donor-acceptor nanohybrids for energy conversion" (in en). npj 2D Materials and Applications 1 (1): 13. doi:10.1038/s41699-017-0012-8. ISSN 2397-7132. 
  15. ↑ Van Dyke, David A.; Pryor, Brian A.; Smith, Philip G.; Topp, Michael R. (May 1998). "Nanosecond Time-Resolved Fluorescence Spectroscopy in the Physical Chemistry Laboratory: Formation of the Pyrene Excimer in Solution". Journal of Chemical Education 75 (5): 615. doi:10.1021/ed075p615. Bibcode: 1998JChEd..75..615V. 
  16. ↑ Förster, Th.; Kasper, K. (June 1954). "Ein Konzentrationsumschlag der Fluoreszenz.". Zeitschrift für Physikalische Chemie 1 (5_6): 275–277. doi:10.1524/zpch.1954.1.5_6.275. 
  17. ↑ Pham, Tuan Anh; Song, Fei; Nguyen, Manh-Thuong; Stöhr, Meike (2014). "Self-assembly of pyrene derivatives on Au(111): Substituent effects on intermolecular interactions". Chem. Commun. 50 (91): 14089–92. doi:10.1039/C4CC02753A. PMID 24905327. 
  18. ↑ Oliveira, M.; Ribeiro, A.; Hylland, K.; Guilhermino, L. (2013). "Single and combined effects of microplastics and pyrene on juveniles (0+ group) of the common goby Pomatoschistus microps (Teleostei, Gobiidae)". Ecological Indicators 34: 641–647. doi:10.1016/j.ecolind.2013.06.019. 
  19. ↑ Oliveira, M.; Gravato, C.; Guilhermino, L. (2012). "Acute toxic effects of pyrene on Pomatoschistus microps (Teleostei, Gobiidae): Mortality, biomarkers and swimming performance". Ecological Indicators 19: 206–214. doi:10.1016/j.ecolind.2011.08.006. 
  20. ↑ Oliveira, M.; Ribeiro, A.; Guilhermino, L. (2012). "Effects of exposure to microplastics and PAHs on microalgae Rhodomonas baltica and Tetraselmis chuii". Comparative Biochemistry and Physiology Part A: Molecular & Integrative Physiology 163: S19–S20. doi:10.1016/j.cbpa.2012.05.062. 
  21. ↑ Oliveira, M.; Ribeiro, A.; Guilhermino, L. (2012). "Effects of short-term exposure to microplastics and pyrene on Pomatoschistus microps (Teleostei, Gobiidae)". Comparative Biochemistry and Physiology Part A: Molecular & Integrative Physiology 163: S20. doi:10.1016/j.cbpa.2012.05.063. 
  22. ↑ Seo, Jong-Su; Keum, Young-Soo; Li, Qing (2009). "Bacterial Degradation of Aromatic Compounds". International Journal of Environmental Research and Public Health 6 (1): 278–309. doi:10.3390/ijerph6010278. PMID 19440284. 
  23. ↑ Keimig, S. D.; Kirby, K. W.; Morgan, D. P.; Keiser, J. E.; Hubert, T. D. (1983). "Identification of 1-hydroxypyrene as a major metabolite of pyrene in pig urine". Xenobiotica 13 (7): 415–20. doi:10.3109/00498258309052279. PMID 6659544. 

Cited sources

Further reading

  • Birks, J. B. (1969). Photophysics of Aromatic Molecules. London: Wiley. 
  • Valeur, B. (2002). Molecular Fluorescence: Principles and Applications. New York: Wiley-VCH. 
  • Birks, J. B. (1975). "Excimers" (in en). Reports on Progress in Physics 38 (8): 903–974. doi:10.1088/0034-4885/38/8/001. ISSN 0034-4885. Bibcode: 1975RPPh...38..903B. 
  • Fetzer, J. C. (2000). The Chemistry and Analysis of the Large Polycyclic Aromatic Hydrocarbons. New York: Wiley. 



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