Styrene

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Styrene
Styrene.svg
Styrene-from-xtal-2001-3D-balls.png
Styrene-from-xtal-2001-3D-sf.png
Styrene-elpot-3D-vdW.png
Names
IUPAC name
Styrene [1]
Systematic IUPAC name
Ethenylbenzene [2]
Other names
Styrene [2]
Vinylbenzene
Phenylethene
Phenylethylene
Cinnamene
Styrol
Diarex HF 77
Styrolene
Styropol
Identifiers
3D model (JSmol)
1071236
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.002.592 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 202-851-5
2991
KEGG
PubChem CID
RTECS number
  • WL3675000
UNII
UN number 2055
  • InChI=1S/C8H8/c1-2-8-6-4-3-5-7-8/h2-7H,1H2 Yes check.svgY
    Key: PPBRXRYQALVLMV-UHFFFAOYSA-N Yes check.svgY
  • c1ccccc1C=C
Properties
C8H8
Molar mass 104.15 g/mol
Appearancecolorless oily liquid
Odor sweet, floral [3]
Density 0.909 g/cm3
Melting point −30 °C (−22 °F; 243 K)
Boiling point 145 °C (293 °F; 418 K)
0.03% (20 °C) [3]
log P 2.70 [4]
Vapor pressure 5 mmHg (20 °C) [3]
−6.82×10−5 cm3/mol
1.5469
Viscosity 0.762 cP at 20 °C
Structure
0.13 D
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
flammable, toxic, probably carcinogenic
GHS labelling:
GHS-pictogram-flamme.svg GHS-pictogram-exclam.svg GHS-pictogram-silhouette.svg
Danger
H226, H315, H319, H332, H361, H372
P201, P202, P210, P233, P240, P241, P242, P243, P260, P261, P264, P270, P271, P280, P281, P302+P352, P303+P361+P353, P304+P312, P304+P340, P305+P351+P338, P308+P313, P312, P314, P321, P332+P313, P337+P313, P362, P370+P378, P403+P235, P405, P501
NFPA 704 (fire diamond)
NFPA 704.svgHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazards (white): no code
2
3
2
Flash point 31 °C (88 °F; 304 K)
Explosive limits 0.9–6.8% [3]
Lethal dose or concentration (LD, LC):
2194 ppm (mouse, 4  h)
5543 ppm (rat, 4 h) [5]
10,000 ppm (human, 30 min)
2771 ppm (rat, 4 h) [5]
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 100 ppm C 200 ppm 600 ppm (5-minute maximum peak in any 3 hours) [3]
REL (Recommended)
TWA 50 ppm (215 mg/m3)
ST 100 ppm (425 mg/m3) [3]
IDLH (Immediate danger)
700 ppm [3]
Safety data sheet (SDS) MSDS
Related compounds
Related styrenes;
related aromatic compounds
 polystyrene, stilbene;
ethylbenzene
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Styrene is an organic compound with the chemical formula C6H5CH=CH2. Its structure consists of a vinyl group as substituent on benzene. Styrene is a colorless, oily liquid, although aged samples can appear yellowish. The compound evaporates easily and has a sweet smell, although high concentrations have a less pleasant odor.[ vague ] Styrene is the precursor to polystyrene and several copolymers, and is typically made from benzene for this purpose. Approximately 25 million tonnes of styrene were produced in 2010, [6] increasing to around 35 million tonnes by 2018.

Natural occurrence

Styrene is named after storax balsam (often commercially sold as styrax), the resin of Liquidambar trees of the Altingiaceae plant family. Styrene occurs naturally in small quantities in some plants and foods (cinnamon, coffee beans, balsam trees and peanuts) [7] and is also found in coal tar.

History

In 1839, the German apothecary Eduard Simon isolated a volatile liquid from the resin (called storax or styrax (Latin)) of the American sweetgum tree ( Liquidambar styraciflua ). He called the liquid "styrol" (now called styrene). [8] [9] He also noticed that when styrol was exposed to air, light, or heat, it gradually transformed into a hard, rubber-like substance, which he called "styrol oxide". [10]

By 1845, the German chemist August Wilhelm von Hofmann and his student John Buddle Blyth had determined styrene's empirical formula: C8H8. [11] They had also determined that Simon's "styrol oxide" – which they renamed "metastyrol" – had the same empirical formula as styrene. [12] Furthermore, they could obtain styrene by dry-distilling "metastyrol". [13]

In 1865, the German chemist Emil Erlenmeyer found that styrene could form a dimer, [14] and in 1866 the French chemist Marcelin Berthelot stated that "metastyrol" was a polymer of styrene (i.e. polystyrene). [15] Meanwhile, other chemists had been investigating another component of storax, namely, cinnamic acid. They had found that cinnamic acid could be decarboxylated to form "cinnamene" (or "cinnamol"), which appeared to be styrene.

In 1845, French chemist Emil Kopp suggested that the two compounds were identical, [16] and in 1866, Erlenmeyer suggested that both "cinnamol" and styrene might be vinylbenzene. [17] However, the styrene that was obtained from cinnamic acid seemed different from the styrene that was obtained by distilling storax resin: the latter was optically active. [18] Eventually, in 1876, the Dutch chemist van 't Hoff resolved the ambiguity: the optical activity of the styrene that was obtained by distilling storax resin was due to a contaminant. [19]

Industrial production

From ethylbenzene

The vast majority of styrene is produced from ethylbenzene, [20] and almost all ethylbenzene produced worldwide is intended for styrene production. As such, the two production processes are often highly integrated. Ethylbenzene is produced via a Friedel–Crafts reaction between benzene and ethene; originally this used aluminum chloride as a catalyst, but in modern production this has been replaced by zeolites.

By dehydrogenation

Around 80% of styrene is produced by the dehydrogenation of ethylbenzene. This is achieved using superheated steam (up to 600 °C) over an iron(III) oxide catalyst. [21] The reaction is highly endothermic and reversible, with a typical yield of 88–94%.

StyreneProduction.svg

The crude ethylbenzene/styrene product is then purified by distillation. As the difference in boiling points between the two compounds is only 9 °C at ambient pressure this necessitates the use of a series of distillation columns. This is energy intensive and is further complicated by the tendency of styrene to undergo thermally induced polymerisation into polystyrene, [22] requiring the continuous addition of polymerization inhibitor to the system.

Via ethylbenzene hydroperoxide

Styrene is also co-produced commercially in a process known as POSM (Lyondell Chemical Company) or SM/PO (Shell) for styrene monomer / propylene oxide. In this process, ethylbenzene is treated with oxygen to form the ethylbenzene hydroperoxide. This hydroperoxide is then used to oxidize propylene to propylene oxide, which is also recovered as a co-product. The remaining 1-phenylethanol is dehydrated to give styrene:

Styrol synthesis.svg

Other industrial routes

Pyrolysis gasoline extraction

Extraction from pyrolysis gasoline is performed on a limited scale. [20]

From toluene and methanol

Styrene can be produced from toluene and methanol, which are cheaper raw materials than those in the conventional process. This process has suffered from low selectivity associated with the competing decomposition of methanol. [23] Exelus Inc. claims to have developed this process with commercially viable selectivities, at 400–425 °C and atmospheric pressure, by forcing these components through a proprietary zeolitic catalyst. It is reported [24] that an approximately 9:1 mixture of styrene and ethylbenzene is obtained, with a total styrene yield of over 60%. [25]

From benzene and ethane

Another route to styrene involves the reaction of benzene and ethane. This process is being developed by Snamprogetti and Dow. Ethane, along with ethylbenzene, is fed to a dehydrogenation reactor with a catalyst capable of simultaneously producing styrene and ethylene. The dehydrogenation effluent is cooled and separated and the ethylene stream is recycled to the alkylation unit. The process attempts to overcome previous shortcomings in earlier attempts to develop production of styrene from ethane and benzene, such as inefficient recovery of aromatics, production of high levels of heavies and tars, and inefficient separation of hydrogen and ethane. Development of the process is ongoing. [26]

Laboratory synthesis

A laboratory synthesis of styrene entails the decarboxylation of cinnamic acid: [27]

C6H5CH=CHCO2H → C6H5CH=CH2 + CO2

Styrene was first prepared by this method. [28]

Polymerization

The presence of the vinyl group allows styrene to polymerize. Commercially significant products include polystyrene, acrylonitrile butadiene styrene (ABS), styrene-butadiene (SBR) rubber, styrene-butadiene latex, SIS (styrene-isoprene-styrene), S-EB-S (styrene-ethylene/butylene-styrene), styrene-divinylbenzene (S-DVB), styrene-acrylonitrile resin (SAN), and unsaturated polyesters used in resins and thermosetting compounds. These materials are used in rubber, plastic, insulation, fiberglass, pipes, automobile and boat parts, food containers, and carpet backing.

Hazards

Autopolymerisation

As a liquid or a gas, pure styrene will polymerise spontaneously to polystyrene, without the need of external initiators. [29] This is known as autopolymerisation. At 100 °C it will autopolymerise at a rate of ~2% per hour, and more rapidly than this at higher temperatures. [22] As the autopolymerisation reaction is exothermic it can be self-accelerating, with a real risk of a thermal runaway, potentially leading to an explosion. Examples include the 2019 explosion of the tanker Stolt Groenland, [30] explosions at the Phillips Petroleum Company in 1999 and 2000 and overheating styrene tanks leading to the 2020 Visakhapatnam gas leak, which killed several people. [31] [32] The autopolymerisation reaction can only be kept in check by the continuous addition of polymerisation inhibitors.

Health effects

Styrene is regarded as a "known carcinogen", especially in case of eye contact, but also in case of skin contact, of ingestion and of inhalation, according to several sources. [20] [33] [34] [35] Styrene is largely metabolized into styrene oxide in humans, resulting from oxidation by cytochrome P450. Styrene oxide is considered toxic, mutagenic, and possibly carcinogenic. Styrene oxide is subsequently hydrolyzed in vivo to styrene glycol by the enzyme epoxide hydrolase. [36] The US Environmental Protection Agency (EPA) has described styrene to be "a suspected toxin to the gastrointestinal tract, kidney, and respiratory system, among others". [37] [38]

On 10 June 2011, the US National Toxicology Program has described styrene as "reasonably anticipated to be a human carcinogen". [39] [40] However, a STATS author describes [41] a review that was done on scientific literature and concluded that "The available epidemiologic evidence does not support a causal relationship between styrene exposure and any type of human cancer". [42] Despite this claim, work has been done by Danish researchers to investigate the relationship between occupational exposure to styrene and cancer. They concluded, "The findings have to be interpreted with caution, due to the company based exposure assessment, but the possible association between exposures in the reinforced plastics industry, mainly styrene, and degenerative disorders of the nervous system and pancreatic cancer, deserves attention". [43] In 2012, the Danish EPA concluded that the styrene data do not support a cancer concern for styrene. [44] The US EPA does not have a cancer classification for styrene, [45] but it has been the subject of their Integrated Risk Information System (IRIS) program. [46]

The National Toxicology Program of the US Department of Health and Human Services has determined that styrene is "reasonably anticipated to be a human carcinogen". [47] Various regulatory bodies refer to styrene, in various contexts, as a possible or potential human carcinogen. The International Agency for Research on Cancer considers styrene to be "probably carcinogenic to humans". [48] [49]

The neurotoxic [50] properties of styrene have also been studied and reported effects include effects on vision [51] (although unable to reproduce in a subsequent study [52] ) and on hearing functions. [53] [54] [55] [56] Studies on rats have yielded contradictory results, [54] [55] but epidemiologic studies have observed a synergistic interaction with noise in causing hearing difficulties. [57] [58] [59] [60]

Related Research Articles

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Toluene, also known as toluol, is a substituted aromatic hydrocarbon with the chemical formula C6H5CH3, often abbreviated as PhCH3, where Ph stands for phenyl group. It is a colorless, water-insoluble liquid with the odor associated with paint thinners. It is a mono-substituted benzene derivative, consisting of a methyl group (CH3) attached to a phenyl group by a single bond. As such, its systematic IUPAC name is methylbenzene. Toluene is predominantly used as an industrial feedstock and a solvent.

<span class="mw-page-title-main">Formaldehyde</span> Organic compound (H–CHO); simplest aldehyde

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<span class="mw-page-title-main">Petrochemical</span> Chemical product derived from petroleum

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<span class="mw-page-title-main">Acetophenone</span> Chemical compound

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<span class="mw-page-title-main">Naphthalene</span> Chemical compound

Naphthalene is an organic compound with formula C
10H
8. It is the simplest polycyclic aromatic hydrocarbon, and is a white crystalline solid with a characteristic odor that is detectable at concentrations as low as 0.08 ppm by mass. As an aromatic hydrocarbon, naphthalene's structure consists of a fused pair of benzene rings. It is the main ingredient of traditional mothballs.

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Polystyrene (PS) is a synthetic polymer made from monomers of the aromatic hydrocarbon styrene. Polystyrene can be solid or foamed. General-purpose polystyrene is clear, hard, and brittle. It is an inexpensive resin per unit weight. It is a poor barrier to air and water vapor and has a relatively low melting point. Polystyrene is one of the most widely used plastics, with the scale of its production being several million tonnes per year. Polystyrene is naturally transparent, but can be colored with colorants. Uses include protective packaging, containers, lids, bottles, trays, tumblers, disposable cutlery, in the making of models, and as an alternative material for phonograph records.

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References

  1. ↑ pubchem.ncbi.nlm.nih.gov/compound/7501#section=IUPAC-Name&fullscreen=true
  2. 1 2 "Front Matter". Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: Royal Society of Chemistry. 2014. pp. P001–P004. doi:10.1039/9781849733069-FP001. ISBN   978-0-85404-182-4.
  3. 1 2 3 4 5 6 7 NIOSH Pocket Guide to Chemical Hazards. "#0571". National Institute for Occupational Safety and Health (NIOSH).
  4. ↑ "Styrene". www.chemsrc.com.
  5. 1 2 "Styrene". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  6. ↑ "New Process for Producing Styrene Cuts Costs, Saves Energy, and Reduces Greenhouse Gas Emissions" (PDF). US Department of Energy. Archived from the original (PDF) on 21 April 2013.
  7. ↑ Steele, D.H.; M.J., Thornburg; J.S., Stanley; R.R., Miller; R., Brooke; J.R., Cushman; G., Cruzan (1994). "Determination of styrene in selected foods". Journal of Agricultural and Food Chemistry. 42 (8): 1661–1665. doi:10.1021/jf00044a015. ISSN   0021-8561. Archived from the original on 14 February 2018.
  8. ↑ Simon, E. (1839) "Ueber den flüssigen Storax (Styrax liquidus)" (On liquid storax (Styrax liquidus), Annalen der Chemie, 31 : 265–277. From p. 268: "Das flüchtige Oel, für welches ich den Namen Styrol vorschlage, … " (The volatile oil, for which I suggest the name "styrol", … )
  9. ↑ For further details of the history of styrene, see: F. W. Semmler, Die ätherischen Öle nach ihren chemischen Bestandteilen unter Berücksichtigung der geschichtlichen Entwicklung [The volatile liquids according to their chemical components with regard to historical development], vol. 4 (Leipzig, Germany, Veit & Co., 1907), § 327. Styrol, pp. 24-28. Archived 1 May 2018 at the Wayback Machine
  10. ↑ (Simon, 1839), p. 268. From p. 268: "Für den festen Rückstand würde der Name Styroloxyd passen." (For the solid residue, the name "styrol oxide" would fit.)
  11. ↑ See:
  12. ↑ (Blyth and Hofmann, 1845a), p. 348. From p. 348: "Analysis as well as synthesis has equally proved that styrol and the vitreous mass (for which we propose the name of metastyrol) possess the same constitution per cent."
  13. ↑ (Blyth and Hofmann, 1845a), p. 350
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  15. ↑ Berthelot, M. (1866) "Sur les caractères de la benzine et du styrolène, comparés avec ceux des autres carbures d'hydrogène" (On the characters of benzene and styrene, compared with those of other hydrocarbons), Bulletin de la Société Chimique de Paris, 2nd series, 6 : 289–298. From p. 294: "On sait que le styrolène chauffé en vase scellé à 200°, pendant quelques heures, se change en un polymère résineux (métastyrol), et que ce polymère, distillé brusquement, reproduit le styrolène." (One knows that styrene [when] heated in a sealed vessel at 200 °C, for several hours, is changed into a resinous polymer (metastyrol), and that this polymer, [when] distilled abruptly, reproduces styrene.)
  16. ↑ Kopp, E. (1845), "Recherches sur l'acide cinnamique et sur le cinnamène" Archived 8 November 2016 at the Wayback Machine (Investigations of cinnamic acid and cinnamen), Comptes rendus, 21 : 1376–1380. From p. 1380: "Je pense qu'il faudra désormais remplacer le mot de styrol par celui de cinnamène, et le métastyrol par le métacinnamène." (I think that henceforth one will have to replace the word "styrol" with that of "cinnamène", and "metastyrol" with "metacinnamène".)
  17. ↑ Erlenmeyer, Emil (1866) "Studien über die s.g. aromatischen Säuren" (Studies of the so-called aromatic acids), Annalen der Chemie, 137 : 327–359; see p. 353.
  18. ↑ Berthelot, Marcellin (1867). "Sur les états isomériques du styrolène" [On the isomeric states of styrene]. Annales de Chimie et de Physique. 4th series (in French). 12: 159–161. From p. 160: "1° Le carbure des cinnamates est privé de pouvoir rotatoire, tandis que le carbure du styrax dévie de 3 degrés la teinte de passage (l = 100 mm)." (1. The carbon [atom] of cinnamates is bereft of rotary power [i.e., the ability to rotate polarized light], whereas the carbon of styrax deflects by 3 degrees the neutral tint [i.e., the relative orientation of the polarized quartz plates at which the light through the polarimeter appears colorless] (length = 100 mm). [For further details about 19th century polarimeters, see: Spottiswode, William (1883). Polarisation of Light (4th ed.). London: Macmillan and Co. pp. 51–52. Archived from the original on 10 September 2010. Retrieved 15 September 2016.])
  19. ↑ van 't Hoff, J. H. (1876) "Die Identität von Styrol und Cinnamol, ein neuer Körper aus Styrax" (The identity of styrol and cinnamol, a new substance from styrax), Berichte der deutschen chemischen Gesellschaft, 9 : 5-6.
  20. 1 2 3 James, Denis H.; Castor, William M. (2007). "Styrene". Ullmann's Encyclopedia of Industrial Chemistry . Weinheim: Wiley-VCH. doi:10.1002/14356007.a25_329.pub2. ISBN   978-3527306732.
  21. ↑ Lee, Emerson H. (13 December 2006). "Iron Oxide Catalysts for Dehydrogenation of Ethylbenzene in the Presence of Steam". Catalysis Reviews. 8 (1): 285–305. doi:10.1080/01614947408071864.
  22. 1 2 Khuong, Kelli S.; Jones, Walter H.; Pryor, William A.; Houk, K.N. (February 2005). "The Mechanism of the Self-Initiated Thermal Polymerization of Styrene. Theoretical Solution of a Classic Problem". Journal of the American Chemical Society . 127 (4): 1265–1277. doi:10.1021/ja0448667. PMID   15669866.
  23. ↑ Yashima, Tatsuaki; Sato, Keiichi; Hayasaka, Tomoki; Hara, Nobuyoshi (1972). "Alkylation on synthetic zeolites: III. Alkylation of toluene with methanol and formaldehyde on alkali cation exchanged zeolites". Journal of Catalysis. 26 (3): 303–312. doi:10.1016/0021-9517(72)90088-7.
  24. ↑ "Welcome to ICIS". www.icis.com. Retrieved 1 May 2018.
  25. ↑ Stephen K. Ritter, Chemical & Engineering News, 19 March 2007, p.46.
  26. ↑ "CHEMSYSTEMS.COM" (PDF). www.chemsystems.com. Archived from the original (PDF) on 8 July 2011. Retrieved 1 May 2018.
  27. ↑ Abbott, T.W.; Johnson, J.R. (1941). "Phenylethylene (Styrene)". Organic Syntheses {{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 1, p. 440.
  28. ↑ R. Fittig und F. Binder "Ueber die Additionsproducte der Zimmtssaure" in "Untersuchungen über die ungesättigten Säuren. I. Weitere Beiträge zur Kenntniß der Fumarsäure und Maleïnsäure" Rudolph Fittig, Camille Petri, Justus Liebigs Annalen der Chemie 1879, volume 195, pp. 56–179. doi : 10.1002/jlac.18791950103
  29. ↑ Miller, A.A.; Mayo, F.R. (March 1956). "Oxidation of Unsaturated Compounds. I. The Oxidation of Styrene". Journal of the American Chemical Society. 78 (5): 1017–1023. doi:10.1021/ja01586a042.
  30. ↑ "Report on the investigation of the cargo tank explosion and fire on board the chemical tanker Stolt Groenland" (PDF). e UK Marine Accident Investigation Branch.
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