Chemistry:1,3-Butadiene

From HandWiki
1,3-Butadiene
Full structural formula of 1,3-butadiene
Skeletal formula of 1,3-butadiene
Ball-and-stick model of 1,3-butadiene
Space-filling model of 1,3-butadiene
Names
Preferred IUPAC name
Buta-1,3-diene[1]
Other names
  • Biethylene
  • Erythrene
  • Divinyl
  • Vinylethylene
  • Bivinyl
  • Butadiene
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
EC Number
  • 271-039-0
KEGG
RTECS number
  • EI9275000
UNII
UN number 1010
Properties
C4H6
Molar mass 54.0916 g/mol
Appearance Colourless gas
or refrigerated liquid
Odor Mildly aromatic or gasoline-like
Density
  • 0.6149 g/cm3 at 25 °C, solid
  • 0.64 g/cm3 at −6 °C, liquid
Melting point −108.9 °C (−164.0 °F; 164.2 K)
Boiling point −4.4 °C (24.1 °F; 268.8 K)
1.3 g/L at 5 ℃, 735 mg/L at 20 ℃
Solubility
Vapor pressure 2.4 atm (20 °C)[2]
1.4292
Viscosity 0.25 cP at 0 °C
Hazards
Main hazards Flammable, irritative, carcinogen
Safety data sheet ECSC 0017
R-phrases (outdated) R45 R46 R12
S-phrases (outdated) S45 S53
NFPA 704 (fire diamond)
Flammability code 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 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 codeNFPA 704 four-colored diamond
4
3
2
Flash point −85 °C (−121 °F; 188 K) liquid flash point[2]
420 °C (788 °F; 693 K)
Explosive limits 2–12%
Lethal dose or concentration (LD, LC):
548 mg/kg (rat, oral)
  • 115,111 ppm (mouse)
  • 122,000 ppm (mouse, 2 h)
  • 126,667 ppm (rat, 4 h)
  • 130,000 ppm (rat, 4 h)[3]
250,000 ppm (rabbit, 30 min)[3]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 1 ppm ST 5 ppm[2]
REL (Recommended)
 Potential occupational carcinogen[2]
IDLH (Immediate danger)
 2000 ppm[2]
Related compounds
Related Alkenes
and dienes
 Isoprene
Chloroprene
Related compounds
 Butane
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references

1,3-Butadiene is the organic compound with the formula (CH2=CH)2. It is a colorless gas that is easily condensed to a liquid. It is important industrially as a monomer in the production of synthetic rubber. The molecule can be viewed as the union of two vinyl groups. It is the simplest conjugated diene.

Although butadiene breaks down quickly in the atmosphere, it is nevertheless found in ambient air in urban and suburban areas as a consequence of its constant emission from motor vehicles.[4]

The name butadiene can also refer to the isomer, 1,2-butadiene, which is a cumulated diene with structure H2C=C=CH−CH3. This allene has no industrial significance.

History

In 1863, the French chemist E. Caventou isolated butadiene from the pyrolysis of amyl alcohol.[5] This hydrocarbon was identified as butadiene in 1886, after Henry Edward Armstrong isolated it from among the pyrolysis products of petroleum.[6] In 1910, the Russian chemist Sergei Lebedev polymerized butadiene and obtained a material with rubber-like properties. This polymer was, however, found to be too soft to replace natural rubber in many applications, notably automobile tires.

The butadiene industry originated in the years leading up to World War II. Many of the belligerent nations realized that in the event of war, they could be cut off from rubber plantations controlled by the British Empire, and sought to reduce their dependence on natural rubber.[7] In 1929, Eduard Tschunker and Walter Bock, working for IG Farben in Germany, made a copolymer of styrene and butadiene that could be used in automobile tires. Worldwide production quickly ensued, with butadiene being produced from grain alcohol in the Soviet Union and the United States, and from coal-derived acetylene in Germany.

Production

Extraction from C4 hydrocarbons

In the United States, western Europe, and Japan, butadiene is produced as a byproduct of the steam cracking process used to produce ethylene and other alkenes. When mixed with steam and briefly heated to very high temperatures (often over 900 °C), aliphatic hydrocarbons give up hydrogen to produce a complex mixture of unsaturated hydrocarbons, including butadiene. The quantity of butadiene produced depends on the hydrocarbons used as feed. Light feeds, such as ethane, give primarily ethylene when cracked, but heavier feeds favor the formation of heavier olefins, butadiene, and aromatic hydrocarbons.

Butadiene is typically isolated from the other four-carbon hydrocarbons produced in steam cracking by extractive distillation using a polar aprotic solvent such as acetonitrile, N-methylpyrrolidone, furfural, or dimethylformamide, from which it is then stripped by distillation.[8]

From dehydrogenation of n-butane

Butadiene can also be produced by the catalytic dehydrogenation of normal butane (n-butane). The first such post-war commercial plant, producing 65,000 tons per year of butadiene, began operations in 1957 in Houston, Texas.[9] Prior to that, in the 1940s the Rubber Reserve Company, a part of the United States government, constructed several plants in Borger, TX, Toledo, OH, and El Segundo, CA to produce synthetic rubber for the war effort as part of the United States Synthetic Rubber Program.[10] Total capacity was 68 KMTA (Kilo Metric Tons per Annum).

Today, butadiene from n-butane is commercially practiced using the Houdry Catadiene process, which was developed during World War II. It entails treating butane over a alumina and chromia at high temperatures.[11]

From ethanol

In other parts of the world, including South America, Eastern Europe, China, and India, butadiene is also produced from ethanol. While not competitive with steam cracking for producing large volumes of butadiene, lower capital costs make production from ethanol a viable option for smaller-capacity plants. Two processes were in use.

In the single-step process developed by Sergei Lebedev, ethanol is converted to butadiene, hydrogen, and water at 400–450 °C over any of a variety of metal oxide catalysts:[12]

2 CH3CH2OH → CH2=CH−CH=CH2 + 2 H2O + H2

This process was the basis for the Soviet Union's synthetic rubber industry during and after World War II, and it remained in limited use in Russia and other parts of eastern Europe until the end of the 1970s. At the same time this type of manufacture was canceled in Brazil. As of 2017, no butadiene was produced industrially from ethanol.

In the other, two-step process, developed by the Russian emigree chemist Ivan Ostromislensky, ethanol is oxidized to acetaldehyde, which reacts with additional ethanol over a tantalum-promoted porous silica catalyst at 325–350 °C to yield butadiene:[12]

CH3CH2OH + CH3CHO → CH2=CH−CH=CH2 + 2 H2O

This process was one of the three used in the United States to produce "government rubber" during World War II, although it is less economical than the butane or butene routes for the large volumes. Still, three plants with a total capacity of 200 KMTA[when defined as?] were constructed in the US (Institute, WV; Louisville, KY; and Kobuta, PA ) with start-ups completed in 1943, the Louisville plant initially created butadiene from acetylene generated by an associated Calcium Carbide plant. The process remains in use today in China and India.

From butenes

1,3-Butadiene can also be produced by catalytic dehydrogenation of normal butenes. This method was also used by the United States Synthetic Rubber Program (USSRP) during World War II. The process was much more economical than the alcohol or n-butane route but competed with aviation gasoline for available butene molecules (butenes were plentiful thanks to catalytic cracking). The USSRP constructed several plants in Baton Rouge and Lake Charles, LA; Houston, Baytown, and Port Neches, TX; and Torrance, CA.[10] Total annual production was 275 KMTA.

In the 1960s, a Houston company known as "Petro-Tex" patented a process to produce butadiene from normal butenes by oxidative dehydrogenation using a proprietary catalyst. It is unclear if this technology is practiced commercially.

After World War II, the production from butenes became the major type of production in USSR.

For laboratory use

1,3-Butadiene is inconvenient for laboratory use because it is gas. Laboratory procedures have been optimized for its generation from nongaseous precursors. It can be produced by the retro-Diels-Alder reaction of cyclohexene.[13] Sulfolene is a convenient solid storable source for 1,3-butadiene in the laboratory. It releases the diene and sulfur dioxide upon heating.

Uses

Most butadiene is polymerized to produce synthetic rubber. Polybutadiene itself is a very soft, almost liquid material of commercial interest. The copolymers prepared from butadiene and styrene and/or acrylonitrile, such as acrylonitrile butadiene styrene (ABS), acrylonitrile butadiene (NBR) and styrene-butadiene (SBR) are tough and/or elastic. SBR is the material most commonly used for the production of automobile tires.[11]

Smaller amounts of butadiene are used to make the nylon intermediate, adiponitrile, by the addition of a molecule of hydrogen cyanide to each of the double bonds in a process called hydrocyanation developed by DuPont. Other synthetic rubber materials such as chloroprene, and the solvent sulfolane are also manufactured from butadiene. Butadiene is used in the industrial production of 4-vinylcyclohexene via a Diels Alder dimerization reaction.[14] Vinylcyclohexene is a common impurity found in butadiene upon storage due to dimerization. Cyclooctadiene and cyclododecatriene are produced via nickel- or titanium-catalyzed dimerization and trimerization reactions, respectively. Butadiene is also useful in the synthesis of cycloalkanes and cycloalkenes, as it reacts with double and triple carbon-carbon bonds through the Diels-Alder reaction.

Reactions

The industrial uses illustrate the tendency of butadiene to polymerize. Its susceptibility to 1,4-addition reactions is illustrated by it hydrocyanation. Like many dienes, it undergoes Pd-catalyzed reactions that proceed via allyl complexes.[15] It is a partner in Diels-Alder reactions, e.g. with maleic anhydride to give tetrahydrophthalic anhydride.[16]

Like other dienes, butadiene is a ligand for low-valent metal complexes, e.g. the derivatives Fe(butadiene)(CO)3 and Mo(butadiene)3.

The structure of (butadiene)iron tricarbonyl.[17]

Environmental health and safety

Butadiene is of low acute toxicity. LC50 is 12.5-11.5 vol% for inhalation by rats and mice.[11]

Long-term exposure has been associated with cardiovascular disease, there is a consistent association with leukemia, as well as a significant association with other cancers.[18]

1,3-Butadiene has been designated a Group 1 carcinogen ('carcinogenic to humans') by IARC,[19] and has also been listed as a carcinogen by the Agency for Toxic Substances Disease Registry and the US EPA.[20][21] The American Conference of Governmental Industrial Hygienists (ACGIH) lists the chemical as a suspected carcinogen.[21] The Natural Resource Defense Council (NRDC) lists some disease clusters that are suspected to be associated with this chemical.[22] Some researchers have concluded it is the most potent carcinogen in cigarette smoke, twice as potent as the runner up acrylonitrile[23]

1,3-Butadiene is also a suspected human teratogen.[24][25][26] Prolonged and excessive exposure can affect many areas in the human body; blood, brain, eye, heart, kidney, lung, nose and throat have all been shown to react to the presence of excessive 1,3-butadiene.[27] Animal data suggest that women have a higher sensitivity to possible carcinogenic effects of butadiene over men when exposed to the chemical. This may be due to estrogen receptor impacts. While these data reveal important implications to the risks of human exposure to butadiene, more data are necessary to draw conclusive risk assessments. There is also a lack of human data for the effects of butadiene on reproductive and development shown to occur in mice, but animal studies have shown breathing butadiene during pregnancy can increase the number of birth defects, and humans have the same hormone systems as animals.[28]

1,3-Butadiene is recognized as a Highly Reactive Volatile Organic Compound (HRVOC) for its potential to readily form ozone, and as such, emissions of the chemical are highly regulated by TCEQ in parts of the Houston-Brazoria-Galveston Ozone Non-Attainment Area.[1]

See also

References

  1. ↑ Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 374. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4. 
  2. ↑ 2.0 2.1 2.2 2.3 2.4 NIOSH Pocket Guide to Chemical Hazards. "#0067". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0067.html. 
  3. ↑ 3.0 3.1 "1,3-Butadiene". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/106990.html. 
  4. ↑ "1,3-Butadiene". US Environmental Protection Agency US EPA. http://www.epa.gov/ttn/atw/hlthef/butadien.html. Retrieved 2014-09-02. 
  5. ↑ Caventou, E. (1863). "Ueber eine mit dem zweifach-gebromten Brombutylen isomere Verbindung und über die bromhaltigen Derivate des Brombutylens". Justus Liebigs Annalen der Chemie 127: 93–97. doi:10.1002/jlac.18631270112. 
  6. ↑ Armstrong, H. E.; Miller, A. K. (1886). "The decomposition and genesis of hydrocarbons at high temperatures. I. The products of the manufacture of gas from petroleum". J. Chem. Soc. 49: 74–93. doi:10.1039/CT8864900074. 
  7. ↑ Simple Things Won't Save the Earth, J. Robert Hunter
  8. ↑ Sun, H.P. Wristers, J.P. (1992). Butadiene. In J.I. Kroschwitz (Ed.), Encyclopedia of Chemical Technology, 4th ed., vol. 4, pp. 663–690. New York: John Wiley & Sons.
  9. ↑ Beychok, M.R. and Brack, W.J., "First Postwar Butadiene Plant", Petroleum Refiner, June 1957.
  10. ↑ 10.0 10.1 Herbert, Vernon, "Synthetic Rubber: A Project That Had to Succeed", Greenwood Press, 1985, ISBN:0-313-24634-3
  11. ↑ 11.0 11.1 11.2 J. Grub, E. Löser (2012). "Butadiene". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a04_431.pub2. 
  12. ↑ 12.0 12.1 Kirshenbaum, I. (1978). Butadiene. In M. Grayson (Ed.), Encyclopedia of Chemical Technology, 3rd ed., vol. 4, pp. 313–337. New York: John Wiley & Sons.
  13. ↑ E. B. Hershberg, John R. Ruhoff (1937). "1,3-Butadiene". Org. Synth. 17: 25. doi:10.15227/orgsyn.017.0025. 
  14. ↑ "4-Vinylcyclohexene". IARC. http://monographs.iarc.fr/ENG/Monographs/vol60/mono60-13.pdf. Retrieved 2009-04-19. 
  15. ↑ J. E. Nyström, T. Rein, J. E. Bäckvall (1989). "1,4-Functionalization of 1,3-Dienes via Palladium-Catalyzed Chloroacetoxylation and Allylic Amination: 1-Acetoxy-4-diethylamino-2-butene and 1-Acetoxy-4-benzylamino-2-butene". Org. Synth. 67: 105. doi:10.15227/orgsyn.067.0105. 
  16. ↑ Arthur C. Cope, Elbert C. Herrick (1950). "cis-Δ4-Tetrahydrophthalic Anhydride". Org. Synth. 50: 93. doi:10.15227/orgsyn.030.0093. 
  17. ↑ Reiss, Guido J. (2010). "Redetermination of (η4-s-cis-1,3-butadiene)tricarbonyliron(0)". Acta Crystallographica Section E 66: m1369. doi:10.1107/S1600536810039218. 
  18. ↑ "NPI sheet". http://www.npi.gov.au/database/substance-info/profiles/16.html. 
  19. ↑ Grosse, Yann; Baan, Robert; Straif, Kurt; Secretan, Béatrice; El Ghissassi, Fatiha; Bouvard, Véronique; Altieri, Andrea; Cogliano, Vincent (2008). "Carcinogenicity of 1,3-butadiene, ethylene oxide, vinyl chloride, vinyl fluoride, and vinyl bromide" (in English). The Lancet Oncology 8 (8): 679–680. doi:10.1016/S1470-2045(07)70235-8. ISSN 1470-2045. https://www.thelancet.com/journals/lanonc/article/PIIS1470204507702358/fulltext. 
  20. ↑ http://www.atsdr.cdc.gov/substances/toxsubstance.asp?toxid=81
  21. ↑ 21.0 21.1 Health Effects https://www.osha.gov/SLTC/butadiene/index.html
  22. ↑ http://www.nrdc.org/health/diseaseclusters/
  23. ↑ Fowles, J; Dybing, E (4 September 2003). "Application of toxicological risk assessment principles to the chemical constituents of cigarette smoke". Institute of Environmental Science and Research (New Zealand: Centers for Disease Control and Prevention) 12 (4): 424–430. doi:10.1136/tc.12.4.424. PMID 14660781. PMC 1747794. http://tobaccocontrol.bmj.com/content/12/4/424. Retrieved 12 October 2014. 
  24. ↑ Landrigan, PJ (1990). "Critical assessment of epidemiologic studies on the human carcinogenicity of 1,3-butadiene". Environmental Health Perspectives 86: 143–147. doi:10.1289/ehp.9086143. PMID 2205484. 
  25. ↑ "1,3-Butadiene CAS No. 106-99-0". Report on Carcinogens. http://ntp.niehs.nih.gov/ntp/roc/eleventh/profiles/s025buta.pdf. 
  26. ↑ Melnick, Ronald L.; Kohn, Michael C. (1995). "Mechanistic data indicate that 1,3-butadiene is a human carcinogen". Carcinogenesis 16 (2): 157–63. doi:10.1093/carcin/16.2.157. PMID 7859343. 
  27. ↑ "Archived copy". http://www.environment-agency.gov.uk/business/topics/pollution/27.aspx. 
  28. ↑ EPA website

External links




Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:1,3-Butadiene&oldid=2423873"