Ethylene | |
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General | |
Molecular formula | C2H4 |
SMILES | C=C |
Molar mass | 28.05 g/mol |
Appearance | colorless gas |
CAS number | [74-85-1] |
Properties | |
Density and phase | 1.178 kg/m³ at 15 °C, gas [1] |
Solubility in water | 3.5 mg/100 ml (17 °C) |
Melting point | −169.2 °C (104.0 K, -272.6 °F) |
Boiling point | −103.7 °C (169.5 K, -154.7 °F) |
pKa | 44 |
Critical point | 282.4 K (9.2 °C) at 5.04 MPa (50 atm) |
Std enthalpy of formation ΔfH°gas |
+52.47 kJ/mol |
Standard molar entropy S°gas |
219.32 J·K−1·mol−1 |
Structure | |
Symmetry group | D2h |
Dipole moment | Zero |
Hazards | |
MSDS | External MSDS |
EU classification | Extremely flammable (F+) |
NFPA 704 |
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Supplementary data page | |
Structure and properties |
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Thermodynamic data |
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Spectral data | UV, IR, NMR, MS |
Related compounds | |
Related compounds | Ethane Acetylene |
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
Ethylene (or IUPAC name ethene) is the chemical compound with the formula C2H4. It is the simplest alkene. Because it contains a carbon-carbon double bond, ethylene is called an unsaturated hydrocarbon or an olefin. It is extremely important in industry and also has a role in biology as a hormone.[2] Ethylene is the most produced organic compound in the world; global production of ethylene exceeded 75 million metric tonnes per year in 2005.[3] To meet the ever increasing demand for ethylene, sharp increases in production facilities have been added globally, particularly in the Gulf countries.
Contents |
This hydrocarbon has four hydrogen atoms bound to a pair of carbon atoms that are connected by a double bond. All six atoms that comprise ethylene are coplanar. The H-C-H angle is 117°, close to the 120° for ideal sp² hybridized carbon. The molecule is also relatively rigid: rotation about the C-C bond is a high energy process that requires breaking the π-bond, while retaining the σ-bond between the carbon atoms.
The double bond is a region of high electron density, and most reactions occur at this double bond position.
From 1795 on, ethylene was referred to as the olefiant gas (oil-making gas), because it combined with chlorine to produce the oil of the Dutch (1,2-dichloroethane). Ethylene was first synthesized in 1795 by a collaboration of four Dutch chemists.
In the mid-19th century, the suffix -ene (an Ancient Greek root added to the end of female names meaning "daughter of") was widely used to refer to a molecule or part thereof that contained one fewer hydrogen atoms than the molecule being modified. Thus, ethylene (C2H4) was the "daughter of ethyl" (C2H5). The name ethylene was used in this sense as early as 1852.
In 1866, the German chemist August Wilhelm von Hofmann proposed a system of hydrocarbon nomenclature in which the suffixes -ane, -ene, -ine, -one, and -une were used to denote the hydrocarbons with 0, 2, 4, 6, and 8 fewer hydrogens than their parent alkane.[4] In this system, ethylene became ethene. Hofmann's system eventually became the basis for the Geneva nomenclature approved by the International Congress of Chemists in 1892, which remains at the core of the IUPAC nomenclature. However, by that time, the name ethylene was deeply entrenched, and it remains in wide use today, especially in the chemical industry.
The 1979 IUPAC nomenclature rules made an exception for retaining the non-systematic name ethylene[5], however, this decision was reversed in the 1993 rules[6] so the correct name is now ethene.
Approximately 80% of ethylene used in the United States and Europe is used to create ethylene oxide, ethylene dichloride, and polyethylene.[7] In smaller quantities, ethylene is used as an anesthetic agent (in an 85% ethylene/15% oxygen ratio), to hasten fruit ripening, as well as a welding gas.[8][7]
Polyethylenes of various density and melt flow account for more than 50% of world ethylene demand. The primary use of polyethylene is in film applications for packaging, carrier bags and trash liners. Other applications include injection moulding, pipe extrusion, wire and cable sheathing and insulation, as well as extrusion coating of paper and cardboard.
Ethylene derivatives include: ethylene oxide, styrene monomer (via ethyl benzene) and linear higher olefins.[7]
Ethylene oxide is a key raw material in the production of surfactants and detergents. It is also used to manufacture ethylene glycols, which are in turn used in packaging and textiles, and to make glycol ether solvents.
Styrene monomer is used principally in polystyrene for packaging and insulation, as well as in styrene butadiene rubber for tires and footwear.
Linear higher olefins are used as base materials for the manufacture of detergents, plasticisers, synthetic lubricants and additives, but also as co-monomers in the production of polyethylenes. [7]
Ethylene is produced in the petrochemical industry by steam cracking. In this process, gaseous or light liquid hydrocarbons are heated to 750–950 °C, inducing numerous free radical reactions followed by immediate quench to freeze the reactions. This process converts large hydrocarbons into smaller ones and introduces unsaturation. Ethylene is separated from the resulting complex mixture by repeated compression and distillation. In a related process used in oil refineries, high molecular weight hydrocarbons are cracked over zeolite catalysts. Heavier feedstocks, such as naphtha and gas oils require at least two "quench towers" downstream of the cracking furnaces to recirculate pyrolysis-derived gasoline and process water. When cracking a mixture of ethane and propane, only one water quench tower is required.[9]
The areas of an ethylene plant are:
Since the production of ethylene is energy intensive, much effort has been dedicated recovering heat from the gas leaving the furnaces. Most of the energy recovered from the cracked gas is used to make high pressure (1200 psig) steam. This steam is in turn used to drive the turbines for compressing cracked gas, the propylene refrigeration compressor, and the ethylene refrigeration compressor. An ethylene plant, once running, does not need to import any steam to drive its steam turbines. A typical world scale ethylene plant (about 1.5 billion pounds of ethylene per year) uses a 45,000 horsepower (34,000 kW) cracked gas compressor, a 30,000 horsepower (22,000 kW) propylene compressor, and a 15,000 horsepower (11,000 kW) ethylene compressor.
When starting an ethylene plant it is important to start the cooling systems in the proper order. The cooling systems consist of Cooling Tower Water (CTW); propylene refrigeration with four or five different levels or stages. Each level corresponds to a particular pressure and temperature; and three or four stages of ethylene regfrigeration. The CTW must be started first because the propylene system needs it to condense propylene and the ethylene refrigeration systems needs it to desuperheat high pressure ethylene. The propylene system must start next because the ethylene system needs high pressure propylene for desuperheating the high pressure ethylene stage and the low pressure propylene stage for condensing the high pressure ethylene. While the ethylene plant is running, the plant can continue to run for a time if the ethylene refrigeration compressor shuts down. However, if the propylene compressor shuts down the whole plant must be shut down immediately.[9]
Ethylene can be conveniently produced in the laboratory by distilling absolute ethanol with an excess of concentrated sulfuric acid and washing the distillate vapor stream in an aqueous solution of sodium hydroxide to remove the sulfur dioxide contaminant.[10]
Although ethylene is a relatively simple molecule, its spectrum[11] is considered to be one of the most difficult to explain adequately from both a theoretical and practical perspective. For this reason, it is often used as a test case in computational chemistry. Of particular note is the difficulty in characterizing the ultraviolet absorption of the molecule. Interest in the subtleties and details of the ethylene spectrum can be dated back to at least the 1950s.
Ethylene is an extremely important building block in the petrochemical industry. It can undergo many types of reactions which leads to a plethora of major chemical products. A list of some major types of reactions includes, 1) Polymerization, 2) Oxidation, 3) Halogenation and Hydrohalogenation, 4) Alkylation, 5) Hydration, 6) Oligomerization, 7) Oxo-reaction, and 8) a ripening agent for fruits and vegetables (see Physiological responses of plants).[9]
Like most alkenes, ethylene reacts with halogens to produce halogenated hydrocarbons1,2-C2H4X2. It can also react with water to produce ethanol, but the rate at which this happens is very slow unless a suitable catalyst, such as phosphoric or sulfuric acid, is used. Under high pressure, and, in the presence of a catalytic metal (platinum, rhodium, nickel), hydrogen will react with ethylene to form ethane.
Ethylene is used primarily as an intermediate in the manufacture of other chemicals in the synthesis of monomers. Ethylene can be chlorinated to produce 1,2-dichloroethane (ethylene dichloride). This can be converted to vinyl chloride, the monomer precursor to plastic polyvinyl chloride, or combined with benzene to produce ethylbenzene, which is used in the manufacture of polystyrene, another important plastic.
Ethylene is more reactive than alkanes because of two reasons:
1. It has a double bond, one called the π-bond(pi) and one called the σ-bond (sigma), where the π-bond is weak and the σ-bond is strong. The presence of the π-bond makes it a high energy molecule. Thus bromine water decolourises readily when it is added to ethylene.
2. High electron density at the double bond makes it react readily. It is broken in an addition reaction to produce many useful products.
Ethylene polymerizes to produce polyethylene, also called polyethene or polythene, the world's most widely-used plastic.
Major polyethylene product groups are low density polyethylene, high density polyethylene, polyethylene copolymers, as well as ethylene-propylene co- & terpolymers.[9]
Ethylene is oxidized to produce ethylene oxide, which is hydrolysed to ethylene glycol. It is also a precursor to vinyl acetate.
Ethylene undergoes oxidation by palladium to give acetaldehyde. This conversion was at one time a major industrial process.[12] The process proceeds via the initial complexation of ethylene to a Pd(II) center.
Major intermediates of the oxidation of Ethylene are ethylene oxide, acetaldehyde, vinyl acetate and ethylene glycol. The list of products made from these intermediates is long. Some of them are: polyesters, polyurethane, morpholine, ethanolamines, aspirin and glycol ethers.[9]
Major intermediates from the halogenation and hydrohalogenation of ethylene include: ethylene dichloride, ethyl chloride and ethylene dibromide. Some products in this group are: polyvinyl chloride, trichloroethylene, perchloroethylene, methyl chloroform, polyvinylidiene chloride and copolymers, and ethyl bromide.[9]
Major chemical intermediates from the alkylation of ethylene include: ethylbenzene, ethyl toluene, ethyl anilines, 1,4-hexadiene and aluminium alkyls. Products of these intermediates include polystyrene, unsaturated polyesters and ethylene-propylene terpolymers.[9]
Ethanol is the primary intermediate of the hydration of ethylene. Important products from ethanol are: ethylamines, acetaldehyde, and ethyl acetate.[9]
The primary products of the Oligomerization of ethylene are alpha-olefins and linear primary alcohols. These are used as plasticizers and surfactants.[9]
The Oxo-reaction of ethylene results in propionaldehyde with its primary products of propionic acid and n-propyl alcohol.[9]
Ethylene is useful in organic synthesis.[13] Representative reactions include Diels-Alder additions, ene reaction, and arene alkylation.
Ethylene is found in many lip gloss products.
Production of ethylene in mineral oil-filled transformers is a key indicator of severe localized overheating (>750 degrees C).[14]
Ethylene acts physiologically as a hormone in plants.[15][16] It exists as a gas and acts at trace levels throughout the life of the plant by stimulating or regulating the ripening of fruit, the opening of flowers, and the abscission (or shedding) of leaves. Its biosynthesis starts from methionine with 1-aminocyclopropane-1-carboxylic acid (ACC) as a key intermediate.
Ethylene has been used in practice since the ancient Egyptians, who would gash figs in order to stimulate ripening (wounding stimulates ethylene production by plant tissues). The ancient Chinese would burn incense in closed rooms to enhance the ripening of pears. In 1864, it was discovered that gas leaks from street lights led to stunting of growth, twisting of plants, and abnormal thickening of stems (Arteca, 1996; Salisbury and Ross, 1992). In 1901, a Russian scientist named Dimitry Neljubow showed that the active component was ethylene [17] . Doubt discovered that ethylene stimulated abscission in 1917[18]. It wasn't until 1934 that Gane reported that plants synthesize ethylene (Gane, 1934). In 1935, Crocker proposed that ethylene was the plant hormone responsible for fruit ripening as well as senescence of vegetative tissues (Crocker, 1935).
It has been shown that ethylene is produced from essentially all parts of higher plants, including leaves, stems, roots, flowers, fruits, tubers, and seedlings.
"Ethylene production is regulated by a variety of developmental and environmental factors. During the life of the plant, ethylene production is induced during certain stages of growth such as germination, ripening of fruits, abscission of leaves, and senescence of flowers. Ethylene production can also be induced by a variety of external aspects such as mechanical wounding, environmental stresses, and certain chemicals including auxin and other regulators"[19]
The biosynsthesis of the hormone starts with conversion of the amino acid methionine to S-adenosyl-L-methionine (SAM, also called Adomet) by the enzyme Met Adenosyltransferase. SAM is then converted to 1-aminocyclopropane-1-carboxylic-acid (ACC) by the enzyme ACC synthase (ACS); the activity of ACS is the rate-limiting step in ethylene production, therefore regulation of this enzyme is key for the ethylene biosynthesis. The final step requires oxygen and involves the action of the enzyme ACC-oxidase (ACO), formerly known as the Ethylene Forming Enzyme (EFE). Ethylene biosynthesis can be induced by endogenous or exogenous ethylene. ACC synthesis increases with high levels of auxins, specially Indole Acetic Acid (IAA), and cytokinins. ACC synthase is inhibited by abscisic acid.
Ethylene could be perceived by a transmembrane protein dimer complex. The first gene encoding an ethylene receptor was first cloned from Arabidopsis thaliana by Caren Chang, Elliot Meyerowitz and colleagues at the California Institute of Technology[20] and then in tomato by Jack Wilkinson, Harry Klee and colleagues at the Monsanto Company[21]. Ethylene receptors are encoded by multiple genes in the Arabidopsis and tomato genomes. The gene family is comprised of five receptors in Arabidopsis and at least six in tomato, most of which have been shown to bind ethylene. DNA sequences for ethylene receptors have also been identified in many other plant species and an ethylene binding protein has even been identified in Cyanobacteria[22]
Environmental cues can induce the biosynthesis of the plant hormone. Flooding, drought, chilling, wounding, and pathogen attack can induce ethylene formation in the plant.
In flooding, root suffers from lack of oxygen, or anoxia, which leads to the synthesis of 1-Aminocyclopropane-1-carboxylic acid (ACC). ACC is transported upwards in the plant and then oxidized in leaves. The product, the ethylene causes epinasty of the leaves.
One speculation recently put forth for epinasty is the downard pointing leaves may act as pump handles in the wind. The ethylene may or may not additionally induce the growth of a valve in the xylem, but the idea would be that the plant would harness the power of the wind to pump out more water from the roots of the plants than would normally happen with transpiration.
Like the other plant hormones, ethylene is considered to have pleiotropic effects. This essentially means that it is thought that at least some of the effects of the hormone are unrelated. What is actually caused by the gas may depend on the tissue affected as well as environmental conditions. In the evolution of plants, ethylene would simply be a message that was coopted for unrelated uses by plants during different periods of the evolutionary development.
Ethylene shortens the shelf life of many fruits by hastening fruit ripening and floral senescence. Tomatoes, bananas, and apples will ripen faster in the presence of ethylene. Bananas placed next to other fruits will produce enough ethylene to cause accelerated fruit ripening. Ethylene will shorten the shelf life of cut flowers and potted plants by accelerating floral senescence and floral abscission. Flowers and plants which are subjected to stress during shipping, handling, or storage produce ethylene causing a significant reduction in floral display. Flowers affected by ethylene include carnation, geranium, petunia, rose, and many others[23].
Ethylene can cause significant economic losses for florists, markets, suppliers, and growers. Researchers have come up with several ways to inhibit ethylene, including inhibiting ethylene synthesis and inhibiting ethylene perception. Inhibiting ethylene synthesis is less effective for reducing post-harvest losses since ethylene from other sources can still have an effect. By inhibiting ethylene perception, fruits, plants and flowers don't respond to ethylene produced endogenously or from exogenous sources. Inhibitors of ethylene perception include compounds that have a similar shape to ethylene, but do not elicit the ethylene response. An example of an ethylene perception inhibitor is 1-methylcyclopropene (1-MCP).
Commercial growers of bromeliads, including pineapple plants, use ethylene to induce flowering. Plants can be induced to flower either by treatment with the gas in a chamber, or by placing a banana peel next to the plant in an enclosed area.
Depending on the concentration, ethylene gas can cause a pleasant odor, euphoria, nausea, hyperglycemia, a variety of psychological effects, blood pressure changes, hypoxia, loss of consciousness, or death.
Ethylene has a pleasant sweet faint odor, and has a slightly sweet taste, and as it enhances fruit ripening, assists in the development of odour-active aroma volatiles (especially esters), which are responsible for the specific smell of each kind of flower or fruit.
In mild doses, ethylene produces states of euphoria, associated with stimulus to the pleasure centers of the human brain.
Exposure at 37.5% for 15 minutes may result in marked memory disturbances. Humans exposed to as much as 50% ethylene in air, whereby the oxygen availability is decreased to 10%, experience a complete loss of consciousness and may subsequently die due to hypoxia.
Symptoms of ethylene exposure include the following.
Mild exposure in air
Moderate exposure in air
High concentration in air
Very high concentration in air
Severe oxygen deprivation
Very high concentrations in oxygen
Ethylene has long been in use as an inhalatory anaesthetic. When used as a surgical anaesthetic, it is always administered with oxygen with an increased risk of fire. In such cases, however, it acts as a simple, rapid anaesthetic having a quick recovery.
Many geologists and scholars believe that the famous Greek Oracle at Delphi (the Pythia) went into her trance-like state as an effect of ethylene rising from ground faults.[24]
There is no evidence to indicate that prolonged exposure to low concentrations of ethylene can result in chronic effects. Prolonged exposure to high concentrations may cause permanent effects because of oxygen deprivation. Prolonged inhalation of about 85% in oxygen (a relatively high concentration) is also slightly toxic, resulting in a slow fall in blood pressure. At about 94% in oxygen, ethylene is acutely fatal.
It shows little or no carcinogenic or mutagenic properties. Although there may be moderate hyperglycemia, post operative nausea - while higher than nitrous oxide - is less than in the use of cyclopropane. During the induction and early phases, blood pressure may rise a little, but this effect may be due to patient anxiety, as blood pressure quickly returns to normal. Cardiac arrythmias are infrequent and cardio-vascular effects are benign.
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