Benzene


This article is about the chemical compound. For other uses, see Benzene (disambiguation).

Not to be confused with Benzine.




















































































































Benzene is an important organic chemical compound with the chemical formula C6H6. The benzene molecule is composed of six carbon atoms joined in a ring with one hydrogen atom attached to each. As it contains only carbon and hydrogen atoms, benzene is classed as a hydrocarbon.


Benzene is a natural constituent of crude oil and is one of the elementary petrochemicals. Due to the cyclic continuous pi bond between the carbon atoms, benzene is classed as an aromatic hydrocarbon, the second [n]-annulene ([6]-annulene). It is sometimes abbreviated PhH. Benzene is a colorless and highly flammable liquid with a sweet smell, and is responsible for the aroma around petrol stations. It is used primarily as a precursor to the manufacture of chemicals with more complex structure, such as ethylbenzene and cumene, of which billions of kilograms are produced annually. As benzene has a high octane number, it is an important component of gasoline.


As benzene is a human carcinogen, most non-industrial applications have been limited.




Contents





  • 1 History

    • 1.1 Discovery


    • 1.2 Ring formula


    • 1.3 Nomenclature


    • 1.4 Early applications


    • 1.5 Occurrence



  • 2 Structure


  • 3 Benzene derivatives


  • 4 Production

    • 4.1 Catalytic reforming


    • 4.2 Toluene hydrodealkylation


    • 4.3 Toluene disproportionation


    • 4.4 Steam cracking


    • 4.5 Other methods



  • 5 Uses

    • 5.1 Component of gasoline



  • 6 Reactions

    • 6.1 Sulfonation, chlorination, nitration


    • 6.2 Hydrogenation


    • 6.3 Metal complexes



  • 7 Health effects


  • 8 Exposure to benzene

    • 8.1 Benzene exposure limits


    • 8.2 Toxicology

      • 8.2.1 Biomarkers of exposure


      • 8.2.2 Biotransformations


      • 8.2.3 Molecular toxicology


      • 8.2.4 Biological oxidation and carcinogenic activity



    • 8.3 Routes of exposure

      • 8.3.1 Inhalation


      • 8.3.2 Exposure from soft drinks


      • 8.3.3 Contamination of water supply




  • 9 See also


  • 10 References


  • 11 External links




History



Discovery


The word "benzene" derives from "gum benzoin" (benzoin resin), an aromatic resin known to European pharmacists and perfumers since the 15th century as a product of southeast Asia.[12] An acidic material was derived from benzoin by sublimation, and named "flowers of benzoin", or benzoic acid. The hydrocarbon derived from benzoic acid thus acquired the name benzin, benzol, or benzene.[13]Michael Faraday first isolated and identified benzene in 1825 from the oily residue derived from the production of illuminating gas, giving it the name bicarburet of hydrogen.[14][15] In 1833, Eilhard Mitscherlich produced it by distilling benzoic acid (from gum benzoin) and lime. He gave the compound the name benzin.[16] In 1836, the French chemist Auguste Laurent named the substance "phène";[17] this word has become the root of the English word "phenol", which is hydroxylated benzene, and "phenyl", the radical formed by abstraction of a hydrogen atom (free radical H•) from benzene.




Kekulé's 1872 modification of his 1865 theory, illustrating rapid alternation of double bonds[18]


In 1845, Charles Mansfield, working under August Wilhelm von Hofmann, isolated benzene from coal tar.[19] Four years later, Mansfield began the first industrial-scale production of benzene, based on the coal-tar method.[20][21] Gradually, the sense developed among chemists that a number of substances were chemically related to benzene, comprising a diverse chemical family. In 1855, Hofmann used the word "aromatic" to designate this family relationship, after a characteristic property of many of its members.[22] In 1997, benzene was detected in deep space.[23]



Ring formula




Historic benzene structures (from left to right) by Claus (1867),[24]Dewar (1867),[25]Ladenburg (1869),[26]Armstrong (1887),[27]Thiele (1899)[28][29] and Kekulé (1865). Dewar benzene and prismane are different chemicals that have Dewar's and Ladenburg's structures. Thiele and Kekulé's structures are used today.


The empirical formula for benzene was long known, but its highly polyunsaturated structure, with just one hydrogen atom for each carbon atom, was challenging to determine. Archibald Scott Couper in 1858 and Joseph Loschmidt in 1861[30] suggested possible structures that contained multiple double bonds or multiple rings, but too little evidence was then available to help chemists decide on any particular structure.


In 1865, the German chemist Friedrich August Kekulé published a paper in French (for he was then teaching in Francophone Belgium) suggesting that the structure contained a ring of six carbon atoms with alternating single and double bonds. The next year he published a much longer paper in German on the same subject.[31][32] Kekulé used evidence that had accumulated in the intervening years—namely, that there always appeared to be only one isomer of any monoderivative of benzene, and that there always appeared to be exactly three isomers of every disubstituted derivative—now understood to correspond to the ortho, meta, and para patterns of arene substitution—to argue in support of his proposed structure.[33] Kekulé's symmetrical ring could explain these curious facts, as well as benzene's 1:1 carbon-hydrogen ratio.


The new understanding of benzene, and hence of all aromatic compounds, proved to be so important for both pure and applied chemistry that in 1890 the German Chemical Society organized an elaborate appreciation in Kekulé's honor, celebrating the twenty-fifth anniversary of his first benzene paper. Here Kekulé spoke of the creation of the theory. He said that he had discovered the ring shape of the benzene molecule after having a reverie or day-dream of a snake seizing its own tail (this is a common symbol in many ancient cultures known as the Ouroboros or Endless knot).[34] This vision, he said, came to him after years of studying the nature of carbon-carbon bonds. This was 7 years after he had solved the problem of how carbon atoms could bond to up to four other atoms at the same time. Curiously, a similar, humorous depiction of benzene had appeared in 1886 in a pamphlet entitled Berichte der Durstigen Chemischen Gesellschaft (Journal of the Thirsty Chemical Society), a parody of the Berichte der Deutschen Chemischen Gesellschaft, only the parody had monkeys seizing each other in a circle, rather than snakes as in Kekulé's anecdote.[35] Some historians have suggested that the parody was a lampoon of the snake anecdote, possibly already well known through oral transmission even if it had not yet appeared in print.[13] Kekulé's 1890 speech[36] in which this anecdote appeared has been translated into English.[37] If the anecdote is the memory of a real event, circumstances mentioned in the story suggest that it must have happened early in 1862.[38]


The cyclic nature of benzene was finally confirmed by the crystallographer Kathleen Lonsdale in 1929.[39][40]



Nomenclature


The German chemist Wilhelm Körner suggested the prefixes ortho-, meta-, para- to distinguish di-substituted benzene derivatives in 1867; however, he did not use the prefixes to distinguish the relative positions of the substituents on a benzene ring.[41] It was the German chemist Karl Gräbe who, in 1869, first used the prefixes ortho-, meta-, para- to denote specific relative locations of the substituents on a di-substituted aromatic ring (viz, naphthalene).[42] In 1870, the German chemist Viktor Meyer first applied Gräbe's nomenclature to benzene.[43]



Early applications


In the 19th and early 20th centuries, benzene was used as an after-shave lotion because of its pleasant smell. Prior to the 1920s, benzene was frequently used as an industrial solvent, especially for degreasing metal. As its toxicity became obvious, benzene was supplanted by other solvents, especially toluene (methylbenzene), which has similar physical properties but is not as carcinogenic.


In 1903, Ludwig Roselius popularized the use of benzene to decaffeinate coffee. This discovery led to the production of Sanka. This process was later discontinued. Benzene was historically used as a significant component in many consumer products such as Liquid Wrench, several paint strippers, rubber cements, spot removers, and other products. Manufacture of some of these benzene-containing formulations ceased in about 1950, although Liquid Wrench continued to contain significant amounts of benzene until the late 1970s.[citation needed]



Occurrence


Trace amounts of benzene are found in petroleum and coal. It is a byproduct of the incomplete combustion of many materials. For commercial use, until World War II, most benzene was obtained as a by-product of coke production (or "coke-oven light oil") for the steel industry. However, in the 1950s, increased demand for benzene, especially from the growing polymers industry, necessitated the production of benzene from petroleum. Today, most benzene comes from the petrochemical industry, with only a small fraction being produced from coal.[44]



Structure


Main article: Aromaticity



The various representations of benzene. (N.B.: There is an error in the label of the second figure; the word "isomer" should be replaced by "resonance forms" or "mesomers".)


X-ray diffraction shows that all six carbon-carbon bonds in benzene are of the same length, at 140 picometres (pm)[citation needed]. The C–C bond lengths are greater than a double bond (135 pm) but shorter than a single bond (147 pm). This intermediate distance is consistent with electron delocalization: the electrons for C–C bonding are distributed equally between each of the six carbon atoms. Benzene has 6 hydrogen atoms – fewer than the corresponding parent alkane, hexane. The molecule is planar.[45] The MO description involves the formation of three delocalized π orbitals spanning all six carbon atoms, while the VB description involves a superposition of resonance structures.[46][47][48][49] It is likely that this stability contributes to the peculiar molecular and chemical properties known as aromaticity. To accurately reflect the nature of the bonding, benzene is often depicted with a circle inside a hexagonal arrangement of carbon atoms.


Derivatives of benzene occur sufficiently often as a component of organic molecules that the Unicode Consortium has allocated a symbol in the Miscellaneous Technical block with the code U+232C (⌬) to represent it with three double bonds,[50] and U+23E3 (⏣) for a delocalized version.[51]



Benzene derivatives


Main articles: Aromatic hydrocarbons and Alkylbenzenes

Many important chemical compounds are derived from benzene by replacing one or more of its hydrogen atoms with another functional group. Examples of simple benzene derivatives are phenol, toluene, aniline, and tert-Butyl benzene, abbreviated PhOH, PhMe, and PhNH2, respectively. Linking benzene rings gives biphenyl, C6H5–C6H5. Further loss of hydrogen gives "fused" aromatic hydrocarbons, such as naphthalene and anthracene. The limit of the fusion process is the hydrogen-free allotrope of carbon, graphite.


In heterocycles, carbon atoms in the benzene ring are replaced with other elements. The most important variations contain nitrogen. Replacing one CH with N gives the compound pyridine, C5H5N. Although benzene and pyridine are structurally related, benzene cannot be converted into pyridine. Replacement of a second CH bond with N gives, depending on the location of the second N, pyridazine, pyrimidine, and pyrazine.[52]



Production


Four chemical processes contribute to industrial benzene production: catalytic reforming, toluene hydrodealkylation, toluene disproportionation, and steam cracking. According to the ATSDR Toxicological Profile for benzene, between 1978 and 1981, catalytic reformats accounted for approximately 44–50% of the total U.S benzene production.[44]



Catalytic reforming


In catalytic reforming, a mixture of hydrocarbons with boiling points between 60–200 °C is blended with hydrogen gas and then exposed to a bifunctional platinum chloride or rhenium chloride catalyst at 500–525 °C and pressures ranging from 8–50 atm. Under these conditions, aliphatic hydrocarbons form rings and lose hydrogen to become aromatic hydrocarbons. The aromatic products of the reaction are then separated from the reaction mixture (or reformate) by extraction with any one of a number of solvents, including diethylene glycol or sulfolane, and benzene is then separated from the other aromatics by distillation. The extraction step of aromatics from the reformate is designed to produce aromatics with lowest non-aromatic components. Recovery of the aromatics, commonly referred to as BTX (benzene, toluene and xylene isomers), involves such extraction and distillation steps. There are a good many licensed processes available for extraction of the aromatics.


In similar fashion to this catalytic reforming, UOP and BP commercialized a method from LPG (mainly propane and butane) to aromatics.



Toluene hydrodealkylation


Toluene hydrodealkylation converts toluene to benzene. In this hydrogen-intensive process, toluene is mixed with hydrogen, then passed over a chromium, molybdenum, or platinum oxide catalyst at 500–600 °C and 40–60 atm pressure. Sometimes, higher temperatures are used instead of a catalyst (at the similar reaction condition). Under these conditions, toluene undergoes dealkylation to benzene and methane:


C6H5CH3 + H2 → C6H6 + CH4

This irreversible reaction is accompanied by an equilibrium side reaction that produces
biphenyl (aka diphenyl) at higher temperature:


2 C
6H
6 ⇌ H
2 + C
6H
5–C
6H
5

If the raw material stream contains much non-aromatic components (paraffins or naphthenes), those are likely decomposed to lower hydrocarbons such as methane, which increases the consumption of hydrogen.


A typical reaction yield exceeds 95%. Sometimes, xylenes and heavier aromatics are used in place of toluene, with similar efficiency.


This is often called "on-purpose" methodology to produce benzene, compared to conventional BTX (benzene-toluene-xylene) extraction processes.



Toluene disproportionation


Where a chemical complex has similar demands for both benzene and xylene, then toluene disproportionation (TDP) may be an attractive alternative to the toluene hydrodealkylation. In the broad sense, 2 toluene molecules are reacted and the methyl groups rearranged from one toluene molecule to the other, yielding one benzene molecule and one xylene molecule.


Given that demand for para-xylene (p-xylene) substantially exceeds demand for other xylene isomers, a refinement of the TDP process called Selective TDP (STDP) may be used. In this process, the xylene stream exiting the TDP unit is approximately 90% paraxylene. In some current catalytic systems, even the benzene-to-xylenes ratio is decreased (more xylenes) when the demand of xylenes is higher.



Steam cracking


Steam cracking is the process for producing ethylene and other alkenes from aliphatic hydrocarbons. Depending on the feedstock used to produce the olefins, steam cracking can produce a benzene-rich liquid by-product called pyrolysis gasoline. Pyrolysis gasoline can be blended with other hydrocarbons as a gasoline additive, or routed through an extraction process to recover BTX aromatics (benzene, toluene and xylenes).



Other methods


Although of no commercial significance, many other routes to benzene exist. Phenol and halobenzenes can be reduced with metals. Benzoic acid and its salts undergo decarboxylation to benzene. Via the reaction the diazonium compound with hypophosphorus acid aniline gives benzene. Trimerization of acetylene gives benzene.



Uses


Benzene is used mainly as an intermediate to make other chemicals, above all ethylbenzene, cumene, cyclohexane, nitrobenzene, and alkylbenzene. More than half of the entire benzene production is processed into ethylbenzene, a precursor to styrene, which is used to make polymers and plastics like polystyrene and EPS. Some 20% of the benzene production is used to manufacture cumene, which is needed to produce phenol and acetone for resins and adhesives. Cyclohexane consumes c. 10% of the world's benzene production; it is primarily used in the manufacture of nylon fibers, which are processed into textiles and engineering plastics. Smaller amounts of benzene are used to make some types of rubbers, lubricants, dyes, detergents, drugs, explosives, and pesticides. In 2013, the biggest consumer country of benzene was China, followed by the USA. Benzene production is currently expanding in the Middle East and in Africa, whereas production capacities in Western Europe and North America are stagnating.[53]


Toluene is now often used as a substitute for benzene, for instance as a fuel additive. The solvent-properties of the two are similar, but toluene is less toxic and has a wider liquid range. Toluene is also processed into benzene.[54]




BenzeneEthylbenzeneCumeneCyclohexaneAnilineChlorobenzeneAcetonePhenolStyreneBisphenol AAdipic acidCaprolactamPolystyrenePolycarbonateEpoxy resinPhenolic resinNylon 6-6Nylon 6

Major commodity chemicals and polymers derived from benzene. Clicking on the image loads the appropriate article



Component of gasoline


As a gasoline (petrol) additive, benzene increases the octane rating and reduces knocking. As a consequence, gasoline often contained several percent benzene before the 1950s, when tetraethyl lead replaced it as the most widely used antiknock additive. With the global phaseout of leaded gasoline, benzene has made a comeback as a gasoline additive in some nations. In the United States, concern over its negative health effects and the possibility of benzene's entering the groundwater have led to stringent regulation of gasoline's benzene content, with limits typically around 1%.[55] European petrol specifications now contain the same 1% limit on benzene content. The United States Environmental Protection Agency introduced new regulations in 2011 that lowered the benzene content in gasoline to 0.62%.[56]



Reactions


The most common reactions of benzene involve substitution of a proton by other groups.[57]Electrophilic aromatic substitution is a general method of derivatizing benzene. Benzene is sufficiently nucleophilic that it undergoes substitution by acylium ions and alkyl carbocations to give substituted derivatives.




Electrophilic aromatic substitution of benzene

The most widely practiced example of this reaction is the ethylation of benzene.


EtC6H5route.png

Approximately 24,700,000 tons were produced in 1999.[58]
Highly instructive but of far less industrial significance is the Friedel-Crafts alkylation of benzene (and many other aromatic rings) using an alkyl halide in the presence of a strong Lewis acid catalyst. Similarly, the Friedel-Crafts acylation is a related example of electrophilic aromatic substitution. The reaction involves the acylation of benzene (or many other aromatic rings) with an acyl chloride using a strong Lewis acid catalyst such as aluminium chloride or Iron(III) chloride.




Friedel-Crafts acylation of benzene by acetyl chloride



Sulfonation, chlorination, nitration


Using electrophilic aromatic substitution, many functional groups are introduced onto the benzene framework. Sulfonation of benzene involves the use of oleum, a mixture of sulfuric acid with sulfur trioxide. Sulfonated benzene derivatives are useful detergents. In nitration, benzene reacts with nitronium ions (NO2+), which is a strong electrophile produced by combining sulfuric and nitric acids. Nitrobenzene is the precursor to aniline. Chlorination is achieved with chlorine to give chlorobenzene in the presence of a catalyst such as aluminium tri-chloride.



Hydrogenation


Via hydrogenation, benzene and its derivatives convert to cyclohexane and derivatives. This reaction is achieved by the use of high pressures of hydrogen in the presence of heterogeneous catalysts, such as finely divided nickel. Whereas alkenes can be hydrogenated near room temperatures, benzene and related compounds are more reluctant substrates, requiring temperatures >100 °C. This reaction is practiced on a large scale industrially. In the absence of the catalyst, benzene is impervious to hydrogen. Hydrogenation cannot be stopped to give cyclohexene or cyclohexadienes as these are superior substrates. Birch reduction, a non catalytic process, however selectively hydrogenates benzene to the diene.



Metal complexes


Benzene is an excellent ligand in the organometallic chemistry of low-valent metals. Important examples include the sandwich and half-sandwich complexes, respectively, Cr(C6H6)2 and [RuCl2(C6H6)]2.



Health effects




A bottle of benzene. The warnings show benzene is a toxic and flammable liquid.


Benzene is classified as a carcinogen, which increases the risk of cancer and other illnesses, and is also a notorious cause of bone marrow failure. Substantial quantities of epidemiologic, clinical, and laboratory data link benzene to aplastic anemia, acute leukemia, bone marrow abnormalities and cardiovascular disease.[59][60][61] The specific hematologic malignancies that benzene is associated with include: acute myeloid leukemia (AML), aplastic anemia, myelodysplastic syndrome (MDS), acute lymphoblastic leukemia (ALL), and chronic myeloid leukemia (CML).[62]


The American Petroleum Institute (API) stated in 1948 that "it is generally considered that the only absolutely safe concentration for benzene is zero".[63] There is no safe exposure level; even tiny amounts can cause harm.[64] The US Department of Health and Human Services (DHHS) classifies benzene as a human carcinogen. Long-term exposure to excessive levels of benzene in the air causes leukemia, a potentially fatal cancer of the blood-forming organs. In particular, acute myeloid leukemia or acute nonlymphocytic leukemia (AML & ANLL) is not disputed to be caused by benzene.[65] IARC rated benzene as "known to be carcinogenic to humans" (Group 1).


As benzene is ubiquitous in gasoline and hydrocarbon fuels are in use everywhere, human exposure to benzene is a global health problem. Benzene targets liver, kidney, lung, heart and the brain and can cause DNA strand breaks, chromosomal damage, etc. Benzene causes cancer in animals including humans. Benzene has been shown to cause cancer in both sexes of multiple species of laboratory animals exposed via various routes.[66][67]



Exposure to benzene


According to the Agency for Toxic Substances and Disease Registry (ATSDR) (2007), benzene is both an anthropogenically produced and naturally occurring chemical from processes that include: volcanic eruptions, wild fires, synthesis of chemicals such as phenol, production of synthetic fibers, and fabrication of rubbers, lubricants, pesticides, medications, and dyes. The major sources of benzene exposure are tobacco smoke, automobile service stations, exhaust from motor vehicles, and industrial emissions; however, ingestion and dermal absorption of benzene can also occur through contact with contaminated water. Benzene is hepatically metabolized and excreted in the urine. Measurement of air and water levels of benzene is accomplished through collection via activated charcoal tubes, which are then analyzed with a gas chromatograph. The measurement of benzene in humans can be accomplished via urine, blood, and breath tests; however, all of these have their limitations because benzene is rapidly metabolized in the human body.[68]


Exposure to benzene may lead progressively to aplastic anaemia, leukaemia, and multiple myeloma.[69]


OSHA regulates levels of benzene in the workplace.[70] The maximum allowable amount of benzene in workroom air during an 8-hour workday, 40-hour workweek is 1 ppm. As benzene can cause cancer, NIOSH recommends that all workers wear special breathing equipment when they are likely to be exposed to benzene at levels exceeding the recommended (8-hour) exposure limit of 0.1 ppm.[71]



Benzene exposure limits


The United States Environmental Protection Agency has set a maximum contaminant level (MCL) for benzene in drinking water at 0.005 mg/L (5 ppb), as promulgated via the U.S. National Primary Drinking Water Regulations.[72] This regulation is based on preventing benzene leukemogenesis. The maximum contaminant level goal (MCLG), a nonenforceable health goal that would allow an adequate margin of safety for the prevention of adverse effects, is zero benzene concentration in drinking water. The EPA requires that spills or accidental releases into the environment of 10 pounds (4.5 kg) or more of benzene be reported.


The U.S. Occupational Safety and Health Administration (OSHA) has set a permissible exposure limit of 1 part of benzene per million parts of air (1 ppm) in the workplace during an 8-hour workday, 40-hour workweek. The short term exposure limit for airborne benzene is 5 ppm for 15 minutes.[73] These legal limits were based on studies demonstrating compelling evidence of health risk to workers exposed to benzene. The risk from exposure to 1 ppm for a working lifetime has been estimated as 5 excess leukemia deaths per 1,000 employees exposed. (This estimate assumes no threshold for benzene's carcinogenic effects.) OSHA has also established an action level of 0.5 ppm to encourage even lower exposures in the workplace.[74]


The U.S. National Institute for Occupational Safety and Health (NIOSH) revised the Immediately Dangerous to Life and Health (IDLH) concentration for benzene to 500 ppm. The current NIOSH definition for an IDLH condition, as given in the NIOSH Respirator Selection Logic, is one that poses a threat of exposure to airborne contaminants when that exposure is likely to cause death or immediate or delayed permanent adverse health effects or prevent escape from such an environment [NIOSH 2004]. The purpose of establishing an IDLH value is (1) to ensure that the worker can escape from a given contaminated environment in the event of failure of the respiratory protection equipment and (2) is considered a maximum level above which only a highly reliable breathing apparatus providing maximum worker protection is permitted [NIOSH 2004[75]].[76] In September 1995, NIOSH issued a new policy for developing recommended exposure limits (RELs) for substances, including carcinogens. As benzene can cause cancer, NIOSH recommends that all workers wear special breathing equipment when they are likely to be exposed to benzene at levels exceeding the REL (10-hour) of 0.1 ppm.[77] The NIOSH short-term exposure limit (STEL – 15 min) is 1 ppm.


American Conference of Governmental Industrial Hygienists (ACGIH) adopted Threshold Limit Values (TLVs) for benzene at 0.5 ppm TWA and 2.5 ppm STEL.



Toxicology



Biomarkers of exposure


Several tests can determine exposure to benzene. Benzene itself can be measured in breath, blood or urine, but such testing is usually limited to the first 24 hours post-exposure due to the relatively rapid removal of the chemical by exhalation or biotransformation. Most people in developed countries have measureable baseline levels of benzene and other aromatic petroleum hydrocarbons in their blood. In the body, benzene is enzymatically converted to a series of oxidation products including muconic acid, phenylmercapturic acid, phenol, catechol, hydroquinone and 1,2,4-trihydroxybenzene. Most of these metabolites have some value as biomarkers of human exposure, since they accumulate in the urine in proportion to the extent and duration of exposure, and they may still be present for some days after exposure has ceased. The current ACGIH biological exposure limits for occupational exposure are 500 μg/g creatinine for muconic acid and 25 μg/g creatinine for phenylmercapturic acid in an end-of-shift urine specimen.[78][79][80][81]



Biotransformations


Even if it is not a common substrate for metabolism, benzene can be oxidized by both bacteria and eukaryotes. In bacteria, dioxygenase enzyme can add an oxygen to the ring, and the unstable product is immediately reduced (by NADH) to a cyclic diol with two double bonds, breaking the aromaticity. Next, the diol is newly reduced by NADH to catechol. The catechol is then metabolized to acetyl CoA and succinyl CoA, used by organisms mainly in the Krebs Cycle for energy production.


The pathway for the metabolism of benzene is complex and begins in the liver. Several enzymes are involved. These include cytochrome P450 2E1 (CYP2E1), quinine oxidoreductase (NQ01), GSH, and myeloperoxidase (MPO). CYP2E1 is involved at multiple steps: converting benzene to oxepin (benzene oxide), phenol to hydroquinone, and hydroquinone to both benzenetriol and catechol. Hydroquinone, benzenetriol and catechol are converted to polyphenols. In the bone marrow, MPO converts these polyphenols to benzoquinones. These intermediates and metabolites induce genotoxicity by multiple mechanisms including inhibition of topoisomerase II (which maintains chromosome structure), disruption of microtubules (which maintains cellular structure and organization), generation of oxygen free radicals (unstable species) that may lead to point mutations, increasing oxidative stress, inducing DNA strand breaks, and altering DNA methylation (which can affect gene expression). NQ01 and GSH shift metabolism away from toxicity. NQ01 metabolizes benzoquinone toward polyphenols (counteracting the effect of MPO). GSH is involved with the formation of phenylmercapturic acid.[62][82]


Genetic polymorphisms in these enzymes may induce loss of function or gain of function. For example, mutations in CYP2E1 increase activity and result in increased generation of toxic metabolites. NQ01 mutations result in loss of function and may result in decreased detoxification. Myeloperoxidase mutations result in loss of function and may result in decreased generation of toxic metabolites. GSH mutations or deletions result in loss of function and result in decreased detoxification. These genes may be targets for genetic screening for susceptibility to benzene toxicity.[83]



Molecular toxicology


The paradigm of toxicological assessment of benzene is shifting towards the domain of molecular toxicology as it allows understanding of fundamental biological mechanisms in a better way. Glutathione seems to play an important role by protecting against benzene-induced DNA breaks and it is being identified as a new biomarker for exposure and effect.[84] Benzene causes chromosomal aberrations in the peripheral blood leukocytes and bone marrow explaining the higher incidence of leukemia and multiple myeloma caused by chronic exposure. These aberrations can be monitored using fluorescent in situ hybridization (FISH) with DNA probes to assess the effects of benzene along with the hematological tests as markers of hematotoxicity.[85] Benzene metabolism involves enzymes coded for by polymorphic genes. Studies have shown that genotype at these loci may influence susceptibility to the toxic effects of benzene exposure. Individuals carrying variant of NAD(P)H:quinone oxidoreductase 1 (NQO1), microsomal epoxide hydrolase (EPHX) and deletion of the glutathione S-transferase T1 (GSTT1) showed a greater frequency of DNA single-stranded breaks.[86]



Biological oxidation and carcinogenic activity


One way of understanding the carcinogenic effects of benzene is by examining the products of biological oxidation. Pure benzene, for example, oxidizes in the body to produce an epoxide, benzene oxide, which is not excreted readily and can interact with DNA to produce harmful mutations.



Routes of exposure



Inhalation


Outdoor air may contain low levels of benzene from automobile service stations, wood smoke, tobacco smoke, the transfer of gasoline, exhaust from motor vehicles, and industrial emissions.[87] About 50% of the entire nationwide (United States) exposure to benzene results from smoking tobacco or from exposure to tobacco smoke.[88] After smoking 32 cigarettes per day, the smoker would take in about 1.8 milligrams (mg) of benzene. This amount is about 10 times the average daily intake of benzene by nonsmokers.[89]


Inhaled benzene is primarily expelled unchanged through exhalation. In a human study 16.4 to 41.6% of retained benzene was eliminated through the lungs within five to seven hours after a two- to three-hour exposure to 47 to 110 ppm and only 0.07 to 0.2% of the remaining benzene was excreted unchanged in the urine. After exposure to 63 to 405 mg/m3 of benzene for 1 to 5 hours, 51 to 87% was excreted in the urine as phenol over a period of 23 to 50 hours. In another human study, 30% of absorbed dermally applied benzene, which is primarily metabolized in the liver, was excreted as phenol in the urine.[90]



Exposure from soft drinks


Main article: Benzene in soft drinks

Under specific conditions and in the presence of other chemicals benzoic acid (a preservative) and ascorbic acid (Vitamin C) may interact to produce benzene. In March 2006, the official Food Standards Agency in Britain conducted a survey of 150 brands of soft drinks. It found that four contained benzene levels above World Health Organization limits. The affected batches were removed from sale. Similar problems were reported by the FDA in the United States.[91]



Contamination of water supply


In 2005, the water supply to the city of Harbin in China with a population of almost nine million people, was cut off because of a major benzene exposure. Benzene leaked into the Songhua River, which supplies drinking water to the city, after an explosion at a China National Petroleum Corporation (CNPC) factory in the city of Jilin on 13 November 2005.



See also


  • 6-membered aromatic rings with one carbon replaced by another group: borabenzene, benzene, silabenzene, germabenzene, stannabenzene, pyridine, phosphorine, arsabenzene, pyrylium salt

  • Industrial Union Department v. American Petroleum Institute

  • BTEX


References




  1. ^ Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. pp. 138, 577. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4. 


  2. ^ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5. 


  3. ^ Arnold, D.; Plank, C.; Erickson, E.; Pike, F. (1958). "Solubility of Benzene in Water". Industrial & Engineering Chemistry Chemical & Engineering Data Series. 3 (2): 253–256. doi:10.1021/i460004a016. 


  4. ^ Breslow, R.; Guo, T. (1990). "Surface tension measurements show that chaotropic salting-in denaturants are not just water-structure breakers". Proceedings of the National Academy of Sciences of the United States of America. 87 (1): 167–9. Bibcode:1990PNAS...87..167B. doi:10.1073/pnas.87.1.167. PMC 53221 Freely accessible. PMID 2153285. 


  5. ^ Coker, A. Kayode; Ludwig, Ernest E. (2007). Ludwig's Applied Process Design for Chemical And Petrochemical Plants. 1. Elsevier. p. 114. ISBN 0-7506-7766-X. Retrieved 2012-05-31. 


  6. ^ abcde http://chemister.ru/Database/properties-en.php?dbid=1&id=644


  7. ^ ab Atherton Seidell; William F. Linke (1952). Solubilities of Inorganic and Organic Compounds: A Compilation of Solubility Data from the Periodical Literature. Supplement. Van Nostrand. 


  8. ^ abc Benzene in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD), http://webbook.nist.gov (retrieved 2014-05-29)


  9. ^ abc Sigma-Aldrich Co., Benzene. Retrieved on 2014-05-29.


  10. ^ abc "NIOSH Pocket Guide to Chemical Hazards #0049". National Institute for Occupational Safety and Health (NIOSH). 


  11. ^ "Benzene". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). 


  12. ^ The word "benzoin" is derived from the Arabic expression "luban jawi", or "frankincense of Java". Morris, Edwin T. (1984). Fragrance: The Story of Perfume from Cleopatra to Chanel. Charles Scribner's Sons. p. 101. ISBN 0684181959. 


  13. ^ ab Rocke, A. J. (1985). "Hypothesis and Experiment in the Early Development of Kekule's Benzene Theory". Annals of Science. 42 (4): 355–81. doi:10.1080/00033798500200411. 


  14. ^ Faraday, M. (1825). "On new compounds of carbon and hydrogen, and on certain other products obtained during the decomposition of oil by heat". Philosophical Transactions of the Royal Society. 115: 440–466. doi:10.1098/rstl.1825.0022. JSTOR 107752.  On pages 443–450, Faraday discusses "bicarburet of hydrogen" (benzene). On pages 449–450, he shows that benzene's empirical formula is C6H6, although he doesn't realize it because he (like most chemists at that time) used the wrong atomic mass for carbon (6 instead of 12).


  15. ^ Kaiser, R. (1968). "Bicarburet of Hydrogen. Reappraisal of the Discovery of Benzene in 1825 with the Analytical Methods of 1968". Angewandte Chemie International Edition in English. 7 (5): 345–350. doi:10.1002/anie.196803451. 


  16. ^ Mitscherlich, E. (1834). "Über das Benzol und die Säuren der Oel- und Talgarten" [On benzol and oily and fatty types of acids]. Annalen der Pharmacie. 9 (1): 39–48. doi:10.1002/jlac.18340090103.  In a footnote on page 43, Liebig, the journal's editor, suggested changing Mitscherlich's original name for benzene (namely, "benzin") to "benzol", because the suffix "-in" suggested that it was an alkaloid (e.g., Chinin (quinine)), which benzene isn't, whereas the suffix "-ol" suggested that it was oily, which benzene is. Thus on page 44, Mitscherlich states: "Da diese Flüssigkeit aus der Benzoësäure gewonnen wird, und wahrscheinlich mit den Benzoylverbindungen im Zusammenhang steht, so gibt man ihr am besten den Namen Benzol, da der Name Benzoïn schon für die mit dem Bittermandelöl isomerische Verbindung von Liebig und Wöhler gewählt worden ist." (Since this liquid [benzene] is obtained from benzoic acid and probably is related to benzoyl compounds, the best name for it is "benzol", since the name "benzoïn" has already been chosen, by Liebig and Wöhler, for the compound that's isomeric with the oil of bitter almonds [benzaldehyde].)


  17. ^ Laurent, Auguste (1836) "Sur la chlorophénise et les acides chlorophénisique et chlorophénèsique," Annales de Chemie et de Physique, vol. 63, pp. 27–45, see p. 44: "Je donne le nom de phène au radical fondamental des acides précédens (φαινω, j'éclaire), puisque la benzine se trouve dans le gaz de l'éclairage." (I give the name of "phène" (φαινω, I illuminate) to the fundamental radical of the preceding acids, because benzene is found in illuminating gas.)


  18. ^ Critics pointed out a problem with Kekulé's original (1865) structure for benzene: Whenever benzene underwent substitution at the ortho position, two distinguishable isomers should have resulted, depending on whether a double bond or a single bond existed between the carbon atoms to which the substituents were attached; however, no such isomers were observed. In 1872, Kekulé suggested that benzene had two complementary structures and that these forms rapidly interconverted, so that if there were a double bond between any pair of carbon atoms at one instant, that double bond would become a single bond at the next instant (and vice versa). To provide a mechanism for the conversion process, Kekulé proposed that the valency of an atom is determined by the frequency with which it collided with its neighbors in a molecule. As the carbon atoms in the benzene ring collided with each other, each carbon atom would collide twice with one neighbor during a given interval and then twice with its other neighbor during the next interval. Thus, a double bond would exist with one neighbor during the first interval and the other neighbor during the next interval. See pages 86–89 of Auguste Kekulé (1872) "Ueber einige Condensationsprodukte des Aldehyds" (On some condensation products of aldehydes), Liebig's Annalen der Chemie und Pharmacie, 162(1): 77–124, 309–320.


  19. ^ Hofmann, A. W. (1845) "Ueber eine sichere Reaction auf Benzol" (On a reliable test for benzene), Annalen der Chemie und Pharmacie, vol. 55, pp. 200–205; on pp. 204–205, Hofmann found benzene in coal tar oil.


  20. ^ Mansfield Charles Blachford (1849). "Untersuchung des Steinkohlentheers". Annalen der Chemie und Pharmacie. 69: 162–180. doi:10.1002/jlac.18490690203. 


  21. ^ Charles Mansfield filed for (November 11, 1847) and received (May 1848) a patent (no. 11,960) for the fractional distillation of coal tar.


  22. ^ Hoffman, Augustus W. (1856). "On insolinic acid". Proceedings of the Royal Society. 8: 1–3. doi:10.1098/rspl.1856.0002. The existence and mode of formation of insolinic acid prove that to the series of monobasic aromatic acids, Cn2Hn2-8O4, the lowest known term of which is benzoic acid, … .  [Note: The empirical formulas of organic compounds that appear in Hofmann's article (p. 3) are based upon an atomic mass of carbon of 6 (instead of 12) and an atomic mass of oxygen of 8 (instead of 16).]


  23. ^ Cernicharo, José; et al. (1997), "Infrared Space Observatory's Discovery of C4H2, C6H2, and Benzene in CRL 618", Astrophysical Journal Letters, 546 (2): L123–L126, Bibcode:2001ApJ...546L.123C, doi:10.1086/318871 


  24. ^ Claus, Adolph K.L. (1867) "Theoretische Betrachtungen und deren Anwendungen zur Systematik der organischen Chemie" (Theoretical considerations and their applications to the classification scheme of organic chemistry), Berichte über die Verhandlungen der Naturforschenden Gesellschaft zu Freiburg im Breisgau (Reports of the Proceedings of the Scientific Society of Freiburg in Breisgau), 4 : 116-381. In the section Aromatischen Verbindungen (aromatic compounds), pp. 315-347, Claus presents Kekulé's hypothetical structure for benzene (p. 317), presents objections to it, presents an alternative geometry (p. 320), and concludes that his alternative is correct (p.326). See also figures on p. 354 or p. 379.


  25. ^ Dewar, James (1867) "On the oxidation of phenyl alcohol, and a mechanical arrangement adapted to illustrate structure in the non-saturated hydrocarbons," Proceedings of the Royal Society of Edinburgh 6: 82–86.


  26. ^ Ladenburg, Albert (1869) "Bemerkungen zur aromatischen Theorie" (Observations on the aromatic theory), Berichte der Deutschen Chemischen Gesellschaft 2: 140–142.


  27. ^ Armstrong, Henry E. (1887) "An explanation of the laws which govern substitution in the case of benzenoid compounds," Journal of the Chemical Society, 51, 258–268; see p. 264.


  28. ^ Thiele, Johannes (1899) "Zur Kenntnis der ungesättigten Verbindungen" (On our knowledge of unsaturated compounds), Justus Liebig’s Annalen der Chemie,306: 87–142; see: "VIII. Die aromatischen Verbindungen. Das Benzol." (VIII. The aromatic compounds. Benzene.), pp. 125–129. See further: Thiele (1901) "Zur Kenntnis der ungesättigen Verbindungen," Justus Liebig’s Annalen der Chemie, 319: 129–143.


  29. ^ In his 1890 paper, Armstrong represented benzene nuclei within polycyclic benzenoids by placing inside the benzene nuclei a letter "C", an abbreviation of the word "centric". Centric affinities (i.e., bonds) acted within a designated cycle of carbon atoms. From p. 102: " … benzene, according to this view, may be represented by a double ring, in fact." See:

    • Armstrong, H.E. (1890). "The structure of cycloid hydrocarbons". Proceedings of the Chemical Society. 6: 101–105. 

    The use of a circle to denote a benzene nucleus first appeared in:

    • Armit, James Wilson; Robinson, Robert (1925). "Polynuclear heterocyclic aromatic types. Part II. Some anhydronium bases". Journal of the Chemical Society, Transactions. 127: 1604–1618. doi:10.1039/ct9252701604. 

    A history of the determination of benzene's structure is recounted in:

    • Balaban, Alexandru T.; Schleyer, Paul v. R.; Rzepa, Henry S. (2005). "Crocker, Not Armit and Robinson, Begat the Six Aromatic Electrons". Chemical Reviews. 105 (10): 3436–3447. doi:10.1021/cr0300946. 



  30. ^ J. Loschmidt, Chemische Studien (Vienna, Austria-Hungary: Carl Gerold's Sohn, 1861),
    pp. 30, 65.


  31. ^ Kekulé, F. A. (1865). "Sur la constitution des substances aromatiques". Bulletin de la Societe Chimique de Paris. 3: 98–110.  On p. 100, Kekulé suggests that the carbon atoms of benzene could form a "chaîne fermée" (a closed chain, a loop).


  32. ^ Kekulé, F. A. (1866). "Untersuchungen über aromatische Verbindungen (Investigations of aromatic compounds)". Liebigs Annalen der Chemie und Pharmacie. 137 (2): 129–36. doi:10.1002/jlac.18661370202. 


  33. ^ Rocke, A. J. (2010) Image and Reality: Kekule, Kopp, and the Scientific Imagination, University of Chicago Press, pp. 186–227, ISBN 0226723356.


  34. ^ Read, John (1995). From alchemy to chemistry. New York: Dover Publications. pp. 179–180. ISBN 9780486286907. 


  35. ^ English translation Wilcox, David H.; Greenbaum, Frederick R. (1965). "Kekule's benzene ring theory: A subject for lighthearted banter". Journal of Chemical Education. 42 (5): 266–67. Bibcode:1965JChEd..42..266W. doi:10.1021/ed042p266. 


  36. ^ Kekulé, F. A. (1890). "Benzolfest: Rede". Berichte der Deutschen Chemischen Gesellschaft. 23: 1302–11. doi:10.1002/cber.189002301204. 


  37. ^ Benfey O. T. (1958). "August Kekulé and the Birth of the Structural Theory of Organic Chemistry in 1858". Journal of Chemical Education. 35: 21–23. Bibcode:1958JChEd..35...21B. doi:10.1021/ed035p21. 


  38. ^ Gillis Jean (1966). "Auguste Kekulé et son oeuvre, réalisée à Gand de 1858 à 1867". Mémoires de la classe des sciences - Académie royale des sciences, des lettres et des beaux-arts de Belgique. 37 (1): 1–40. 


  39. ^ Lonsdale, K. (1929). "The Structure of the Benzene Ring in Hexamethylbenzene". Proceedings of the Royal Society. 123A: 494. 


  40. ^ Lonsdale, K. (1931). "An X-Ray Analysis of the Structure of Hexachlorobenzene, Using the Fourier Method". Proceedings of the Royal Society. 133A (822): 536–553. Bibcode:1931RSPSA.133..536L. doi:10.1098/rspa.1931.0166. 


  41. ^ See:
    • Wilhelm Körner (1867) "Faits pour servir à la détermination du lieu chimique dans la série aromatique" (Facts to be used in determining chemical location in the aromatic series), Bulletins de l'Académie royale des sciences, des lettres et des beaux-arts de Belgique, 2nd series, 24 : 166–185 ; see especially p. 169. From p. 169: "On distingue facilement ces trois séries, dans lesquelles les dérivés bihydroxyliques ont leurs terms correspondants, par les préfixes ortho-, para- et mêta-." (One easily distinguishes these three series – in which the dihydroxy derivatives have their corresponding terms – by the prefixes ortho-, para- and meta-.)

    • Hermann von Fehling, ed., Neues Handwörterbuch der Chemie [New concise dictionary of chemistry] (Braunschweig, Germany: Friedrich Vieweg und Sohn, 1874), vol. 1, p. 1142.




  42. ^ Graebe (1869) "Ueber die Constitution des Naphthalins" (On the structure of naphthalene), Annalen der Chemie und Pharmacie, 149 : 20–28 ; see especially p. 26.


  43. ^ Victor Meyer (1870) "Untersuchungen über die Constitution der zweifach-substituirten Benzole" (Investigations into the structure of di-substituted benzenes), Annalen der Chemie und Pharmacie, 156 : 265–301 ; see especially pp. 299–300.


  44. ^ ab Hillis O. Folkins (2005). "Benzene". Ullmann’s Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_475. 


  45. ^ Moran D, Simmonett AC, Leach FE, Allen WD, Schleyer PV, Schaefer HF (2006). "Popular Theoretical Methods Predict Benzene and Arenes To Be Nonplanar". Journal of the American Chemical Society. 128 (29): 9342–3. doi:10.1021/ja0630285. PMID 16848464. 


  46. ^ Cooper, David L.; Gerratt, Joseph; Raimondi, Mario (1986). "The electronic structure of the benzene molecule". Nature. 323 (6090): 699–701. Bibcode:1986Natur.323..699C. doi:10.1038/323699a0. 


  47. ^ Pauling, Linus (1987). "Electronic structure of the benzene molecule". Nature. 325 (6103): 396. Bibcode:1987Natur.325..396P. doi:10.1038/325396d0. 


  48. ^ Messmer, Richard P.; Schultz, Peter A. (1987). "The electronic structure of the benzene molecule". Nature. 329 (6139): 492. Bibcode:1987Natur.329..492M. doi:10.1038/329492a0. 


  49. ^ Harcourt, Richard D. (1987). "The electronic structure of the benzene molecule". Nature. 329 (6139): 491–492. Bibcode:1987Natur.329..491H. doi:10.1038/329491b0. 


  50. ^ "Unicode Character 'BENZENE RING' (U+232C)". fileformat.info. Retrieved 2009-01-16. 


  51. ^ "Unicode Character 'BENZENE RING WITH CIRCLE' (U+23E3)". fileformat.info. Retrieved 2009-01-16. 


  52. ^ "Heterocyclic Chemistry: Heterocyclic Compounds". Michigan State University, Department of Chemistry. 


  53. ^ "Market Study: Benzene (2nd edition), Ceresana, August 2014". ceresana.com. Retrieved 2015-02-10. 


  54. ^ "Market Study: Toluene, Ceresana, January 2015". ceresana.com. Retrieved 2015-02-10. 


  55. ^ Kolmetz, Gentry, Guidelines for BTX Revamps, AIChE 2007 Spring Conference


  56. ^ "Control of Hazardous Air Pollutants From Mobile Sources". U.S. Environmental Protection Agency. 2006-03-29. p. 15853. Archived from the original on 2008-12-05. Retrieved 2008-06-27. 


  57. ^
    Stranks, D. R.; M. L. Heffernan; K. C. Lee Dow; P. T. McTigue; G. R. A. Withers (1970). Chemistry: A structural view. Carlton, Victoria: Melbourne University Press. p. 347. ISBN 0-522-83988-6. 


  58. ^ Welch, Vincent A.; Fallon, Kevin J. and Gelbke, Heinz-Peter (2005) "Ethylbenzene" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, doi:10.1002/14356007.a10_035.pub2


  59. ^ Kasper, Dennis L.et al. (2004) Harrison's Principles of Internal Medicine, 16th ed., McGraw-Hill Professional, p. 618, ISBN 0071402357.


  60. ^ Merck Manual, Home Edition, "Overview of Leukemia".


  61. ^ Bard, D (2014). "Traffic-related air pollution and the onset of myocardial infarction: disclosing benzene as a trigger? A small-area case-crossover study". PLOS ONE. 9: 6. Bibcode:2014PLoSO...9j0307B. doi:10.1371/journal.pone.0100307. PMC 4059738 Freely accessible. PMID 24932584. 


  62. ^ ab Smith, Martyn T. (2010). "Advances in understanding benzene health effects and susceptibility". Annu Rev Public Health. 31: 133–48. doi:10.1146/annurev.publhealth.012809.103646. PMC 4360999 Freely accessible. PMID 20070208. 


  63. ^ American Petroleum Institute, API Toxicological Review, Benzene, September 1948, Agency for Toxic Substances and Disease Registry, Department of Health and Human Services


  64. ^ Smith, Martyn T. (2010-01-01). "Advances in Understanding Benzene Health Effects and Susceptibility". Annual Review of Public Health. 31 (1): 133–148. doi:10.1146/annurev.publhealth.012809.103646. PMC 4360999 Freely accessible. PMID 20070208. 


  65. ^ WHO. International Agency for Research on Cancer, IARC Monographs on the Evaluation of Carcinogenic Risks to Humans, Overall Evaluations of Carcinogenicity: An Updating of IARC Monographs Archived 2008-03-06 at the Wayback Machine., Volumes 1 to 42, Supplement 7


  66. ^ Huff J (2007). "Benzene-induced cancers: abridged history and occupational health impact". Int J Occup Environ Health. 13 (2): 213–21. doi:10.1179/oeh.2007.13.2.213. PMC 3363002 Freely accessible. PMID 17718179. 


  67. ^ Rana SV; Verma Y (2005). "Biochemical toxicity of benzene". J Environ Biol. 26 (2): 157–68. PMID 16161967. 


  68. ^ Agency for Toxic Substances and Disease Registry. (2007). Benzene: Patient information sheet.


  69. ^ Br J Ind Med. 1991 Jul;48(7):437-44. The toxicity of benzene and its metabolism and molecular pathology in human risk assessment. Yardley-Jones A, Anderson D, Parke DV.


  70. ^ Occupational Safety and Health Standards, Toxic and Hazardous Substances, 1910.1028. Osha.gov. Retrieved on 2011-11-23.


  71. ^ Public Health Statement for Benzene, Agency for Toxic Substances and Disease Registry. (August 2007). Benzene: Patient information sheet. Atsdr.cdc.gov (2011-03-03). Retrieved on 2011-11-23.


  72. ^ Drinking Water Contaminants|Organic Chemicals|Benzene. Water.epa.gov. Retrieved on 2014-04-17.


  73. ^ Chemical Sampling Information Benzene. Osha.gov. Retrieved on 2011-11-23.


  74. ^ Benzene Toxicity: Standards and Regulations|ATSDR – Environmental Medicine & Environmental Health Education – CSEM. Atsdr.cdc.gov (2000-06-30). Retrieved on 2010-10-09.


  75. ^ NIOSH respirator selection logic (October 2004). Cincinnati, OH: U.S. Department of Health and Human Services, Public Health Service, Centers for Disease Control, National Institute for Occupational Safety and Health, DHHS (NIOSH). Publication No. 2005-100.


  76. ^ Documentation for Immediately Dangerous to Life or Health Concentrations (IDLH): Introduction. Cdc.gov. Retrieved on 2011-11-23.


  77. ^ "Public Health Statement for Benzene" U.S. Department of Health and Human Services, Public Health Service, Centers for Disease Control, National Institute for Occupational Safety and Health. Atsdr.cdc.gov (2011-03-03). Retrieved on 2011-11-23.


  78. ^ Ashley, DL; Bonin, MA; Cardinali, FL; McCraw, JM; Wooten, JV (1994). "Blood concentrations of volatile organic compounds in a nonoccupationally exposed US population and in groups with suspected exposure" (PDF). Clinical Chemistry. 40 (7 Pt 2): 1401–4. PMID 8013127. 


  79. ^ Fustinoni S, Buratti M, Campo L, Colombi A, Consonni D, Pesatori AC, Bonzini M, Farmer P, Garte S, Valerio F, Merlo DF, Bertazzi PA (2005). "Urinary t,t-muconic acid, S-phenylmercapturic acid and benzene as biomarkers of low benzene exposure". Chemico-biological interactions. 153–154: 253–6. doi:10.1016/j.cbi.2005.03.031. PMID 15935823. 


  80. ^ ACGIH (2009). 2009 TLVs and BEIs. American Conference of Governmental Industrial Hygienists, Cincinnati, Ohio.


  81. ^ Baselt, R. (2008) Disposition of Toxic Drugs and Chemicals in Man, 8th edition, Biomedical Publications, Foster City, CA, pp. 144–148, ISBN 0962652377.


  82. ^ Snyder, R; Hedli, C.C. (1996). "An overview of benzene metabolism". Environ Health Perspect. 104 (Suppl 6): 1165–1171. doi:10.1289/ehp.96104s61165. PMC 1469747 Freely accessible. PMID 9118888. 


  83. ^ Dougherty, D; Garte, S; Barchowsky, A; Zmuda, J; Taioli, E (2008). "NQO1, MPO, CYP2E1, GSTT1 and STM1 polymorphisms and biological effects of benzene exposure—a literature review". Toxicology Letters. 182 (1–3): 7–17. doi:10.1016/j.toxlet.2008.09.008. PMID 18848868. 


  84. ^ Fracasso ME, Doria D, Bartolucci GB, Carrieri M, Lovreglio P, Ballini A, Soleo L, Tranfo G, Manno M (2010). "Low air levels of benzene: Correlation between biomarkers of exposure and genotoxic effects". Toxicol Lett. 192 (1): 22–8. doi:10.1016/j.toxlet.2009.04.028. PMID 19427373. 


  85. ^ Eastmond, D.A.; Rupa, DS; Hasegawa, LS (2000). "Detection of hyperdiploidy and chromosome breakage in interphase human lymphocytes following exposure to the benzene metabolite hydroquinone using multicolor fluorescence in situ hybridization with DNA probes". Mutat Res. 322 (1): 9–20. PMID 7517507. 


  86. ^ Garte, S; Taioli, E; Popov, T; Bolognesi, C; Farmer, P; Merlo, F (2000). "Genetic susceptibility to benzene toxicity in humans". J Toxicol Environ Health A. 71 (22): 1482–1489. doi:10.1080/15287390802349974. PMID 18836923. 


  87. ^ ToxFAQs for Benzene, Agency for Toxic Substances and Disease Registry, Department of Health and Human Services[dead link]


  88. ^ ToxGuide for Benzene, Agency for Toxic Substances and Disease Registry, Department of Health and Human Services


  89. ^ Public Health Statement. Benzene, Division of Toxicology and Environmental Medicine, August 2007


  90. ^ Benzene, CASRN: 71-43-2. Hazardous Substances Data Bank, U.S. National Library of Medicine. National Institutes of Health.


  91. ^ "FDA: Too Much Benzene In Some Drinks", CBS News, May 19, 2006. Retrieved July 11, 2006.



External links


Benzene




Skeletal formula detail of benzene.

Geometry


Benzene ball-and-stick model

Ball and stick model


Benzene molecule
Space-filling model

Names

Preferred IUPAC name
Benzene

Other names
Benzol (historic/German)
[6]annulene (not recommended[1])

Identifiers

CAS Number



  • 71-43-2 ☑Y


3D model (JSmol)


  • Interactive image


ChEBI


  • CHEBI:16716 ☑Y


ChEMBL


  • ChEMBL277500 ☑Y


ChemSpider


  • 236 ☑Y


ECHA InfoCard

100.000.685

EC Number
200-753-7

KEGG


  • C01407 ☑Y



PubChem CID


  • 241


RTECS number
CY1400000

UNII


  • J64922108F ☑Y





Properties

Chemical formula


C6H6

Molar mass
78.11 g·mol−1
Appearance
Colorless liquid

Odor
Aromatic, gasoline-like

Density
0.8765(20) g/cm3[2]

Melting point
 5.53 °C (41.95 °F; 278.68 K)

Boiling point
 80.1 °C (176.2 °F; 353.2 K)

Solubility in water

1.53 g/L (0 °C)
1.81 g/L (9 °C)
1.79 g/L (15 °C)[3][4][5]
1.84 g/L (30 °C)
2.26 g/L (61 °C)
3.94 g/L (100 °C)
21.7 g/kg (200 °C, 6.5 MPa)
17.8 g/kg (200 °C, 40 MPa)[6]

Solubility
Soluble in alcohol, CHCl3, CCl4, diethyl ether, acetone, acetic acid[6]

Solubility in ethanediol
5.83 g/100 g (20 °C)
6.61 g/100 g (40 °C)
7.61 g/100 g (60 °C)[6]

Solubility in ethanol
20 °C, solution in water:
1.2 mL/L (20% v/v)[7]

Solubility in acetone
20 °C, solution in water:
7.69 mL/L (38.46% v/v)
49.4 mL/L (62.5% v/v)[7]

Solubility in diethylene glycol
52 g/100 g (20 °C)[6]

log P
2.13

Vapor pressure
12.7 kPa (25 °C)
24.4 kPa (40 °C)
181 kPa (100 °C)[8]

Conjugate acid

Benzenium

UV-vis (λmax)
255 nm


Magnetic susceptibility (χ)

−54.8·10−6 cm3/mol


Refractive index (nD)

1.5011 (20 °C)
1.4948 (30 °C)[6]

Viscosity
0.7528 cP (10 °C)
0.6076 cP (25 °C)
0.4965 cP (40 °C)
0.3075 cP (80 °C)
Structure

Molecular shape


Trigonal planar

Dipole moment

0 D
Thermochemistry


Heat capacity (C)

134.8 J/mol·K


Std molar
entropy (So298)

173.26 J/mol·K[8]


Std enthalpy of
formation (ΔfHo298)

48.7 kJ/mol


Std enthalpy of
combustion (ΔcHo298)

3267.6 kJ/mol[8]
Hazards
Main hazards
potential occupational carcinogen, flammable

Safety data sheet

See: data page
HMDB

GHS pictograms

The flame pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The skull-and-crossbones pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The exclamation-mark pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The health hazard pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)[9]

GHS signal word
Danger

GHS hazard statements


H225, H304, H315, H319, H340, H350, H372[9]

GHS precautionary statements


P201, P210, P301+310, P305+351+338, P308+313, P331[9]

NFPA 704



Flammability code 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., gasolineHealth code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gasReactivity 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

3


3


0




Flash point
 −11.63 °C (11.07 °F; 261.52 K)

Autoignition
temperature

 497.78 °C (928.00 °F; 770.93 K)

Explosive limits
1.2–7.8%
Lethal dose or concentration (LD, LC):


LD50 (median dose)

930 mg/kg (rat, oral)


LCLo (lowest published)

44,000 ppm (rabbit, 30 min)
44,923 ppm (dog)
52,308 ppm (cat)
20,000 ppm (human, 5 min)[11]
US health exposure limits (NIOSH):


PEL (Permissible)

TWA 1 ppm, ST 5 ppm[10]


REL (Recommended)

Ca TWA 0.1 ppm ST 1 ppm[10]


IDLH (Immediate danger)

500 ppm[10]
Related compounds

Related compounds


Toluene
Borazine

Supplementary data page

Structure and
properties


Refractive index (n),
Dielectric constant (εr), etc.

Thermodynamic
data


Phase behaviour
solid–liquid–gas

Spectral data


UV, IR, NMR, MS

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









  • Benzene at The Periodic Table of Videos (University of Nottingham)

  • International Chemical Safety Card 0015

  • USEPA Summary of Benzene Toxicity

  • NIOSH Pocket Guide to Chemical Hazards


  • CID 1 from PubChemEdit this at Wikidata

  • Dept. of Health and Human Services: TR-289: Toxicology and Carcinogenesis Studies of Benzene


  • Video Podcast of Sir John Cadogan giving a lecture on Benzene since Faraday, in 1991

  • Substance profile


  • Benzene in the ChemIDplus database

  • NLM Hazardous Substances Databank – Benzene












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