{{Chembox new
| Name = Acetylene
| ImageFile = Acetylene-2D.png
| ImageSize = 150px
| ImageName = Acetylene
| ImageFile1 = Acetylene-3D-vdW.png
| ImageSize1 = 150px
| ImageName1 = Acetylene
| IUPACName = Ethyne
| Section1 = {{Chembox Identifiers
| CASNo = 74-86-2
| SMILES = C#C
}}
| Section2 = {{Chembox Properties
| Formula = C₂H₂
| MolarMass = 26.0373 g/mol
| Density = 1.09670 kg/m³ gas
| MeltingPt = -84 °C
| BoilingPt = -83.8 °C
| pKa = 25
}}
}}
'''Acetylene''' ([[IUPAC nomenclature|systematic]] name: '''ethyne''') is a [[hydrocarbon]] belonging to the group of [[alkyne]]s. It is considered to be the simplest of all alkynes as it consists of two [[hydrogen]] [[atoms]] and two [[carbon]] atoms. Acetylene is an [[Saturation (chemistry)|unsaturated]] [[organic compound]] because its four atoms are triple bonded through a [[covalent bond]].

The carbon-carbon triple bond leaves the carbon atoms with two sp hybrid orbitals for sigma bonding, placing all four atoms in the same straight line, with CCH bond angles of 180°.

Acetylene was discovered in 1836 by [[Edmund Davy]] who identified it as a "new carburet of hydrogen." It was rediscovered in 1860 by French chemist [[Marcellin Berthelot]], who coined the name "acetylene." The Nobel Laureate [[Gustaf Dalén]] was blinded by an acetylene explosion.

==Preparation==

The principal raw materials for acetylene manufacture are [[calcium carbonate]] ([[limestone]]) and [[coal]]. The calcium carbonate is first converted into calcium oxide and the coal into [[coke (fuel)|coke]], then the two are reacted with each other to form [[calcium carbide]] and [[carbon monoxide]]:

: CaO + 3C → CaC₂ + CO

Calcium [[carbide]] (or [[calcium acetylide]]) and water are then reacted by any of several methods to produce acetylene and [[calcium hydroxide]]. This reaction was discovered by [[Friedrich Wohler]] in 1862.

: CaC₂ + 2H₂O → Ca(OH)₂ + C₂H₂

Calcium carbide synthesis requires an extremely high temperature, ~2000 degrees Celsius, so the reaction is performed in an [[electric arc furnace]]. This reaction was an important part of the late-1800s revolution in chemistry enabled by the massive [[hydroelectric power]] project at [[Niagara Falls]].

Acetylene can also be manufactured by the partial [[combustion]] of [[methane]] with [[oxygen]], or by the [[Cracking (chemistry)|cracking]] of [[hydrocarbon]]s.

Berthelot was able to prepare acetylene from [[methyl alcohol]], [[ethyl alcohol]], [[ethylene]], or [[ether]], when he passed any one of these as a gas or vapour through a red-hot tube. Berthelot also found acetylene was formed by sparking electricity through mixed [[cyanogen]] and [[hydrogen]] gases. He was also able to form acetylene directly by combining pure hydrogen with [[carbon]] using electrical discharge of a [[carbon arc]].

==Reactions==

* Above {{nowrap|400 °C}} ({{nowrap|673 K}}) the [[pyrolysis]] of acetylene will start, which is relatively low for a hydrocarbon. The main products are the [[dimer]] [[vinylacetylene]] (C₄H₄) and [[benzene]]. At temperatures above {{nowrap|900 °C}} ({{nowrap|1173 K}}), the main product will be [[soot]].
*Using acetylene, [[Marcellin Berthelot|Berthelot]] was the first to show that an [[aliphatic]] compound could form an [[aromatic]] compound when he heated acetylene in a glass tube to produce [[benzene]] with some [[toluene]]. Berthelot oxidized acetylene to yield [[acetic acid]] and [[oxalic acid]]. He found acetylene could be reduced to form [[ethylene]] and [[ethane]].
*[[Polymerization]] of acetylene with [[Ziegler-Natta catalyst]]s produces [[polyacetylene]] films. Polyacetylene, a chain of carbon molecules with alternating single and double bonds, was the first [[organic semiconductor]] to be discovered; reaction with [[iodine]] produces an extremely conductive material.
* In the '''Kucherov reaction''' (invented in 1881 by the Russian chemist Mikhail Kucherov)<ref>Kutscheroff, M. Ber. Bunsenges. Phys. Chemie '''1881''', 1540–1542.</ref> acetylene is [[Hydration reaction|hydrated]] to [[acetaldehyde]] with a [[mercury (element)|mercury]] salt such as [[mercury(II) bromide]]. Before the advent of the Wacker process this reaction was conducted on an industrial scale.<ref>''Hydration of Acetylene: A 125th Anniversary''
Dmitry A. Ponomarev and Sergey M. Shevchenko [[Journal of Chemical Education]] Vol. 84 No. 10 October '''2007''' 1725</ref>

===Reppe chemistry===
[[Walter Reppe]] discovered that acetylene can react at high pressures with heavy metal [[catalyst]]s to give industrially significant chemicals:

* Acetylene reacting with [[alcohol]]s, [[hydrogen cyanide]], [[hydrogen chloride]], or [[carboxylic acid]]s to give [[vinyl]] compounds:

[[Image:Reppe-chemnistry-vinylization.png|300px]]

* With [[aldehydes]] to give ethynyl diols.

[[Image:Reppe-chemistry-endiol.png|300px]]

This is industrially used to produce [[1,4-butynediol]] from [[formaldehyde]] and acetylene:

:HCCH + CH₂O → CH₂(OH)CCCH₂OH

* With [[carbon monoxide]] to give [[acrylic acid]], or acrylic esters, which can be used to produce [[acrylic glass]].

[[Image:Reppe-chemistry-carbonmonoxide-01.png|400px]]
[[Image:Reppe-chemistry-carbonmonoxide-02.png|400px]]

* Cyclicization to give [[benzene]] and [[cyclooctatetraene]]:

[[Image:Reppe-chemistry-benzene.png|240px]]
[[Image:Reppe-chemistry-cyclooctatetraene.png|240px]]

==Uses==
Approximately 80 percent of the acetylene produced annually in the [[United States]] is used in chemical synthesis. The remaining 20 percent is used primarily for [[oxyacetylene]] [[gas welding]] and [[blowtorch|cutting]] due to the high temperature of the flame; combustion of acetylene with oxygen produces a flame of over {{nowrap|3300 °C}} ({{nowrap|6000 °F}}), releasing 11.8 [[Kilojoule|kJ]]/g. Oxyacetylene is the hottest burning common fuel gas.<ref name="BOC">http://www.boc.com/products_and_services/by_product/acetylene/index.asp</ref> [[Cyanogen]], a more exotic gas, produces a flame of over {{nowrap|4525 °C}} ({{nowrap|8180 °F}}) when it burns in oxygen.<ref>{{Citation
| last = Thomas
| first =N.
| author-link =
| last2 =Gaydon, A. G.; Brewer, L.
| first2 =
| author2-link =
| title = Cyanogen Flames and the Dissociation Energy of N2
| journal =The Journal of Chemical Physics
| volume =20
| issue =3
| pages =369-374
| date =March 1952
| year =
| url =http://scitation.aip.org/getabs/servlet/GetabsServlet?prog=normal&id=JCPSA6000020000003000369000001&idtype=cvips&gifs=yes
| doi =
| id = }}</ref>

Acetylene is also used in the [[carbide lamp|acetylene ('carbide') lamp]], once used by miners (not to be confused with the [[Davy lamp]]), on vintage [[automobile|cars]], and still sometimes used by [[caver]]s. In this context, the acetylene is generated by dripping [[water]] from the upper chamber of the lamp onto [[calcium carbide]] (CaC₂) pellets in the base of the lamp.

In former times a few towns used acetylene for lighting, including [[Tata (Hungary)|Tata]] in [[Hungary]] where it was installed on [[24 July]] [[1897]], and [[North Petherton]], [[England]] in 1898.

In modern times acetylene is sometimes used for [[carburization]] (that is, hardening) of [[steel]] when the object is too large to fit into a furnace.<ref name="BOC" />

Acetylene has been proposed as a carbon feedstock for [[molecular manufacturing]] using nanotechnology. Since it does not occur naturally, using acetylene could limit out-of-control self-replication.

Acetylene is used to volatilize carbon in [[radiocarbon dating]]. The carbonaceous material in the archeological sample reacted in a small specialized research furnace with [[lithium]] metal to form [[lithium carbide]] (also known as [[lithium acetylide]]). The carbide can then be reacted with water, as usual, to form acetylene gas to be fed into [[mass spectrometer]] to sort out the isotopic ratio of carbon 14 to carbon 12.

'''The Future'''

The use of acetylene is expected to continue a gradual increase in the future as new applications are developed. One new application is the conversion of acetylene to ethylene for use in making a variety of polyethylene plastics. In the past, a small amount of acetylene had been generated and wasted as part of the steam cracking process used to make ethylene. A new catalyst developed by Phillips Petroleum allows most of this acetylene to be converted into ethylene for increased yields at a reduced overall cost.<ref>[http://science.enotes.com/how-products-encyclopedia/acetylene Acetylene: How Products are Made]</ref>

==Safety and handling==
===Compression===
Due to the carbon-to-carbon triple bond, acetylene gas is fundamentally [[instability|unstable]], and will [[chemical decomposition|decompose]] in an [[exothermic]] [[chemical reaction|reaction]] if [[gas compressor|compressed]] to any great extent. Acetylene can explode with extreme violence if the pressure of the gas exceeds about {{nowrap|100 kPa}} (≈14.5 psi) as a gas or when in liquid or solid form, so it is shipped and stored dissolved in [[acetone]] or [[dimethylformamide]] (DMF), contained in a metal cylinder with porous filling ([[Agamassan]]), which renders it safe to transport and use.

There are strict regulations on the shipment of dangerous [[gas cylinder]]s throughout the world. The use of dissolved acetylene is decreasing rapidly, due to favourable flameless [[welding]] processes.

===Toxic effects===
Inhaling acetylene may cause dizziness, headache and nausea.<ref name="HitCL">Muir, GD (ed.) 1971, ''Hazards in the Chemical Laboratory'', The Royal Institute of Chemistry, London.</ref> It may also contain toxic impurities: the [http://www.cganet.com/publication_detail.asp?id=G-1.1 Compressed Gas Association Commodity Specification for acetylene] has established a grading system for identifying and quantifying [[phosphine]], [[arsine]], and [[hydrogen sulfide]] content in commercial grades of acetylene in order to limit exposure to these impurities. The sulfur, phosphorus and arsenic are carryovers from the synthesis ingredient coke, an impure form of carbon and different, organic impurities would be expected from the thermal cracking of hydrocarbons source.

While the impurities in acetylene can be toxic and even fatal, pure acetylene is of a very low toxicity (not counting the "narcotic" effects). Up to 80% percent, (''v''/''v'') acetylene has been administered to surgical patients as a [[general anaesthetic]]. The trade name for acetylene was "narcylene." It was used a fair amount experimentally in Germany in their impoverished 1920's, perhaps on several thousand patients. Medically, acetylene was considered to be nearly as safe as [[nitrous oxide]] and with a slightly higher potency, allowing for the use of higher percentages of oxygen in the blend; it is about 50% more potent. However, the use of acetylene and oxygen mixtures was dropped after several gas explosions inside patients' lungs. The energy of these explosions would be expected to exceed any of the flammable inhalation anesthetics due to the instability of the triple bond (cyclopropane would be nearly as bad). It was suggested that such an internal thorax explosion could not occur with air mixtures (without purified oxygen).

Acetylene has been infrequently abused in a manner akin to nitrous oxide abuse up through modern times, according to the literature. Such abuse can result in the death of the abuser due to toxicity of the above mentioned impurities [[phosphine]], [[arsine]], and [[hydrogen sulfide]]. Since the gas is charged (absorbed) into tanks soaked with acetone over a solid matrix, some acetone comes out with the gas, further contributing to the poisonings. The driver for this abusive behavior is better understood with the view of acetylene's anesthetic properties and addictive behaviors.

Impurities in acetylene are easily detectable by smell. Pure acetylene is a colorless and odorless gas. The characteristic [[garlic]]-like odor of technical grade acetylene is attributable to contamination by impurities. Impurities which may be present include: [[divinyl sulfide]], [[ammonia]], [[oxygen]], [[nitrogen]], [[phosphine]], [[arsine]], [[methane]], [[carbon dioxide]], [[carbon monoxide]], [[hydrogen sulfide]], [[vinyl acetylene]], [[divinyl acetylene]], [[diacetylene]], [[propadiene]], [[hexadiene]], [[butadienyl acetylene]], and [[methyl acetylene]].

===Fire hazard===
Mixtures with air containing between 3% and 82% acetylene are explosive on ignition. The minimum ignition temperature is {{nowrap|335 °C}}.<ref name="HitCL" /> The majority of acetylene's chemical energy is what is ''not'' contained in the carbon-carbon triple bond; that is, it is greater than that of three carbon-carbon bonds spread out, but is disallowed therefrom because of the spaces between its mate carbon and all other carbons likewise shielded in charge.

===Incompatibilities===
* [[bromine]], [[chlorine]], [[copper]], [[mercury (element)|mercury]], [[silver]].

==Other meanings==
Sometimes the plural "acetylenes" may refer to the class of organic chemical compounds known as [[alkyne]]s which contain the -C≡C- group.

==Natural occurrence==
Acetylene is a moderately common chemical in the universe, often associated with the atmospheres of [[gas giant]]s.<ref>{{cite press release | publisher = [[W. M. Keck Observatory]] | title = Precursor to Proteins and DNA found in Stellar Disk | date = 20 December 2005 | url = http://www.keckobservatory.org/article.php?id=39}}</ref> One curious discovery of acetylene is on [[Enceladus (moon)|Enceladus]], a moon of [[Saturn]]. Natural acetylene is believed to form from either [[catalytic]] decomposition of long chain hydrocarbons or at temperatures ≥ 1,770 [[kelvin]]. Since such temperatures are highly unlikely on such a small distant body, this discovery is potentially suggestive of catalytic reactions within the moon, making it a promising site to search for prebiotic chemistry.<ref>{{cite web | publisher = [[The Planetary Society]] | author = Emily Lakdawalla | title = LPSC: Wednesday afternoon: Cassini at Enceladus | date = 17 March 2006 | url = http://www.planetary.org/blog/article/00000498/}}</ref><ref>{{cite journal|journal=[[Nature (journal)|Nature]] | volume=445 | pages=376-377| date= 25 January 2007| doi = 10.1038/445376b| title= Planetary science: Inside Enceladus| author=John Spencer and David Grinspoon}}</ref>

==References==
{{reflist}}

==External links==
* [http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA5/MAIN/1ORGANIC/ORG07/MENU.HTM Acetylene at Chemistry Comes Alive!]
* {{gutenberg|name=Acetylene, the Principles of Its Generation and Use|no=8144}}

{{Template:Alkynes}}

[[Category:Alkynes]]

[[ar:أسيتلين]]
[[ca:Acetilè]]
[[cs:Ethyn]]
[[da:Acetylen]]
[[de:Ethin]]
[[et:Atsetüleen]]
[[el:Αιθίνιο]]
[[es:Acetileno]]
[[eo:Acetileno]]
[[fa:استیلن]]
[[fr:Acétylène]]
[[gl:Acetileno]]
[[hr:Acetilen]]
[[id:Asetilena]]
[[it:Acetilene]]
[[la:Ethinum]]
[[lv:Acetilēns]]
[[lt:Acetilenas]]
[[hu:Acetilén]]
[[nl:Ethyn]]
[[ja:アセチレン]]
[[no:Acetylen]]
[[pl:Etyn]]
[[pt:Acetileno]]
[[ro:Acetilenă]]
[[ru:Ацетилен]]
[[scn:Acitalena]]
[[simple:Acetylene]]
[[sk:Acetylén]]
[[sl:Acetilen]]
[[sr:Ацетилен]]
[[fi:Asetyleeni]]
[[sv:Etyn]]
[[uk:Ацетилен]]
[[zh:乙炔]]