Carbon monoxide

Carbon monoxide (CO) is a colorless, odorless, and tasteless gas that is slightly less dense than air. It is toxic to hemoglobic animals (including humans) when encountered in concentrations above about 35 ppm, although it is also produced in normal animal metabolism in low quantities, and is thought to have some normal biological functions. In the atmosphere, it is spatially variable and short lived, having a role in the formation of ground-level ozone.

Carbon monoxide consists of one carbon atom and one oxygen atom, connected by a triple bond that consists of two covalent bonds as well as one dative covalent bond. It is the simplest oxocarbon and is isoelectronic with the cyanide anion, the nitrosonium cation and molecular nitrogen. In coordination complexes the carbon monoxide ligand is called carbonyl.

Carbon monoxide is produced from the partial oxidation of carbon-containing compounds; it forms when there is not enough oxygen to produce carbon dioxide (CO₂), such as when operating a stove or an internal combustion engine in an enclosed space. In the presence of oxygen, including atmospheric concentrations, carbon monoxide burns with a blue flame, producing carbon dioxide.^[4] Coal gas, which was widely used before the 1960s for domestic lighting, cooking, and heating, had carbon monoxide as a significant fuel constituent. Some processes in modern technology, such as iron smelting, still produce carbon monoxide as a byproduct.^[5]

Worldwide, the largest source of carbon monoxide is natural in origin, due to photochemical reactions in the troposphere that generate about 5×10¹² kilograms per year.^[6] Other natural sources of CO include volcanoes, forest fires, and other forms of combustion.

In biology, carbon monoxide is naturally produced by the action of heme oxygenase 1 and 2 on the heme from hemoglobin breakdown. This process produces a certain amount of carboxyhemoglobin in normal persons, even if they do not breathe any carbon monoxide. Following the first report that carbon monoxide is a normal neurotransmitter in 1993,^[7]^[8] as well as one of three gases that naturally modulate inflammatory responses in the body (the other two being nitric oxide and hydrogen sulfide), carbon monoxide has received a great deal of clinical attention as a biological regulator. In many tissues, all three gases are known to act as anti-inflammatories, vasodilators, and promoters of neovascular growth.^[9] Clinical trials of small amounts of carbon monoxide as a drug are ongoing.^[10] Nonetheless, too much carbon monoxide causes carbon monoxide poisoning.

History

Aristotle (384–322 BC) first recorded that burning coals produced toxic fumes. An ancient method of execution was to shut the criminal in a bathing room with smouldering coals. What was not known was the mechanism of death. Greek physician Galen (129–199 AD) speculated that there was a change in the composition of the air that caused harm when inhaled.^[11] In 1776, the French chemist de Lassone produced CO by heating zinc oxide with coke, but mistakenly concluded that the gaseous product was hydrogen, as it burned with a blue flame. The gas was identified as a compound containing carbon and oxygen by the Scottish chemist William Cumberland Cruikshank in the year 1800.^[12]^[13] Its toxic properties on dogs were thoroughly investigated by Claude Bernard around 1846.^[14]

During World War II, a gas mixture including carbon monoxide was used to keep motor vehicles running in parts of the world where gasoline and diesel fuel were scarce. External (with a few exceptions) charcoal or wood gas generators were fitted, and the mixture of atmospheric nitrogen, carbon monoxide, and small amounts of other gases produced by gasification was piped to a gas mixer. The gas mixture produced by this process is known as wood gas. Carbon monoxide was also used on a large scale during the Holocaust at some Nazi German extermination camps, the most notable by gas vans in Chelmno, and in the Action T4 "euthanasia" program.^[15]

Molecular properties

Carbon monoxide has a molar mass of 28.0, which makes it slightly lighter than air, whose average molar mass is 28.8. According to the ideal gas law, CO is therefore less dense than air.

The bond length between the carbon atom and the oxygen atom is 112.8 pm.^[16]^[17] This bond length is consistent with a triple bond, as in molecular nitrogen (N₂), which has a similar bond length and nearly the same molecular mass. Carbon–oxygen double bonds are significantly longer, 120.8 pm in formaldehyde, for example.^[18] The boiling point (82 K) and melting point (68 K) are very similar to those of N₂ (77 K and 63 K, respectively). The bond dissociation energy of 1072 kJ/mol is stronger than that of N₂ (942 kJ/mol) and represents the strongest chemical bond known.^[19]

The ground electronic state of carbon monoxide is a singlet state^[20] since there are no unpaired electrons.

Bonding and dipole moment

Carbon and oxygen together have a total of 10 electrons in the valence shell. Following the octet rule for both carbon and oxygen, the two atoms form a triple bond, with six shared electrons in three bonding molecular orbitals, rather than the usual double bond found in organic carbonyl compounds. Since four of the shared electrons come from the oxygen atom and only two from carbon, one bonding orbital is occupied by two electrons from oxygen, forming a dative or dipolar bond. This causes a C ← O polarization of the molecule, with a small negative charge on carbon and a small positive charge on oxygen. The other two bonding orbitals are each occupied by one electron from carbon and one from oxygen, forming (polar) covalent bonds with a reverse C → O polarization, since oxygen is more electronegative than carbon. In the free carbon monoxide, a net negative charge δ- remains at the carbon end and the molecule has a small dipole moment of 0.122 D.^[21]

The molecule is therefore asymmetric: oxygen has more electron density than carbon, and is also slightly positively charged compared to carbon being negative. By contrast, the isoelectronic dinitrogen molecule has no dipole moment.

If carbon monoxide acts as a ligand, the polarity of the dipole may reverse with a net negative charge on the oxygen end, depending on the structure of the coordination complex.^[22] See also the section "Coordination chemistry" below.

Bond polarity and oxidation state

Theoretical and experimental studies show that, despite the greater electronegativity of oxygen, the dipole moment points from the more-negative carbon end to the more-positive oxygen end.^[23]^[24] The three bonds are in fact polar covalent bonds that are strongly polarized. The calculated polarization toward the oxygen atom is 71% for the σ-bond and 77% for both π-bonds.^[25]

The oxidation state of carbon in carbon monoxide is +2 in each of these structures. It is calculated by counting all the bonding electrons as belonging to the more electronegative oxygen. Only the two non-bonding electrons on carbon are assigned to carbon. In this count, carbon then has only two valence electrons in the molecule compared to four in the free atom.

Biological and physiological properties

Toxicity

Main article: Carbon monoxide poisoning

Carbon monoxide poisoning is the most common type of fatal air poisoning in many countries.^[26] Carbon monoxide is colorless, odorless, and tasteless, but highly toxic. It combines with hemoglobin to produce carboxyhemoglobin, which usurps the space in hemoglobin that normally carries oxygen, but is ineffective for delivering oxygen to bodily tissues. Concentrations as low as 667 ppm may cause up to 50% of the body's hemoglobin to convert to carboxyhemoglobin.^[27] A level of 50% carboxyhemoglobin may result in seizure, coma, and fatality. In the United States, the OSHA limits long-term workplace exposure levels above 50 ppm.^[28] Within short time scales, carbon monoxide absorption is cumulative, since the half-life is about 5 hours in fresh air.

The most common symptoms of carbon monoxide poisoning may resemble other types of poisonings and infections, including symptoms such as headache, nausea, vomiting, dizziness, fatigue, and a feeling of weakness. Affected families often believe they are victims of food poisoning. Infants may be irritable and feed poorly. Neurological signs include confusion, disorientation, visual disturbance, syncope (fainting), and seizures.^[29]

Some descriptions of carbon monoxide poisoning include retinal hemorrhages, and an abnormal cherry-red blood hue.^[30] In most clinical diagnoses these signs are seldom noticed.^[29] One difficulty with the usefulness of this cherry-red effect is that it corrects, or masks, what would otherwise be an unhealthy appearance, since the chief effect of removing deoxygenated hemoglobin is to make an asphyxiated person appear more normal, or a dead person appear more lifelike, similar to the effect of red colorants in embalming fluid. The "false" or unphysiologic red-coloring effect in anoxic CO-poisoned tissue is related to the meat-coloring commercial use of carbon monoxide, discussed below.

Carbon monoxide also binds to other molecules such as myoglobin and mitochondrial cytochrome oxidase. Exposures to carbon monoxide may cause significant damage to the heart and central nervous system, especially to the globus pallidus,^[31] often with long-term chronic pathological conditions. Carbon monoxide may have severe adverse effects on the fetus of a pregnant woman.^[32]

Normal human physiology

Carbon monoxide is produced naturally by the human body as a signaling molecule. Thus, carbon monoxide may have a physiological role in the body, such as a neurotransmitter or a blood vessel relaxant.^[33] Because of carbon monoxide's role in the body, abnormalities in its metabolism have been linked to a variety of diseases, including neurodegenerations, hypertension, heart failure, and inflammation.^[33]

Functional Summary^[34]

CO functions as an endogenous signaling molecule.
CO modulates functions of the cardiovascular system.
CO inhibits blood platelet aggregation and adhesion.
CO may play a role as potential therapeutic agent.

Microbiology

Carbon monoxide is a nutrient for methanogenic archaea,^[35] a building-block for acetyl coenzyme A. This is the theme for the emerging field of bioorganometallic chemistry. Extremophile micro-organisms can, thus, metabolise carbon monoxide in such locations as the thermal vents of volcanoes.^[36]

In bacteria, carbon monoxide is produced via the reduction of carbon dioxide by the enzyme carbon monoxide dehydrogenase, an Fe-Ni-S-containing protein.^[37]

CooA is a carbon monoxide sensor protein.^[38] The scope of its biological role is still unknown; it may be part of a signaling pathway in bacteria and archaea. Its occurrence in mammals is not established.

Occurrence

Monthly averages of global concentrations of tropospheric carbon monoxide at an altitude of about 12,000 feet. Data were collected by the MOPITT (Measurements Of Pollution In The Troposphere) sensor on NASA’s Terra satellite.^[39]

Carbon monoxide occurs in various natural and artificial environments. Typical concentrations in parts per million are as follows:

**Composition of dry atmosphere, by volume**^[40]
Concentration	Source
ppmv: parts per million by volume (note: volume fraction is equal to mole fraction for ideal gas only, see volume (thermodynamics))
0.1 ppmv	Natural atmosphere level (MOPITT)^[41]
0.5–5 ppmv	Average level in homes^[42]
5–15 ppmv	Near-properly adjusted gas stoves in homes, modern vehicle exhaust emissions^[43]
17 ppmv	Atmosphere of Venus
100–200 ppmv	Exhaust from automobiles in the Mexico City central area in 1975^[44]
700 ppmv	Atmosphere of Mars
5,000 ppmv	Exhaust from a home wood fire^[45]
7,000 ppmv	Undiluted warm car exhaust without a catalytic converter^[43]

Atmospheric presence

The streak of red, orange, and yellow across South America, Africa, and the Atlantic Ocean in this animation points to high levels of carbon monoxide on September 30, 2005.

Carbon Monoxide concentrations in Northern Hemisphere spring as measured with the MOPITT instrument.

Carbon monoxide is present in small amounts in the atmosphere, chiefly as a product of volcanic activity but also from natural and man-made fires (such as forest and bushfires, burning of crop residues, and sugarcane fire-cleaning). The burning of fossil fuels also contributes to carbon monoxide production. Carbon monoxide occurs dissolved in molten volcanic rock at high pressures in the Earth's mantle.^[46] Because natural sources of carbon monoxide are so variable from year to year, it is extremely difficult to accurately measure natural emissions of the gas.

Carbon monoxide is a short-lived greenhouse gas and also has an indirect radiative forcing effect by elevating concentrations of methane and tropospheric ozone through chemical reactions with other atmospheric constituents (e.g., the hydroxyl radical, OH^.) that would otherwise destroy them.^[47] Through natural processes in the atmosphere, it is eventually oxidized to carbon dioxide. Carbon monoxide is both short-lived in the atmosphere (on average about two months) and spatially variable in concentration.

In the atmosphere of Venus carbon monoxide occurs as a result of the photodissociation of carbon dioxide by electromagnetic radiation of wavelengths shorter than 169 nm.

Due to its long lifetime in the mid-troposphere, carbon monoxide is also used as tracer of transport for pollutant plumes.^[48]

Urban pollution

Carbon monoxide is a temporary atmospheric pollutant in some urban areas, chiefly from the exhaust of internal combustion engines (including vehicles, portable and back-up generators, lawn mowers, power washers, etc.), but also from incomplete combustion of various other fuels (including wood, coal, charcoal, oil, paraffin, propane, natural gas, and trash).

Large CO pollution events can be observed from space over cities.^[49]

Role in ground-level ozone formation

Main article: Tropospheric ozone

Carbon monoxide is, along with aldehydes, part of the series of cycles of chemical reactions that form photochemical smog. It reacts with hydroxyl radical (^•OH) to produce a radical intermediate ^•HOCO, which transfers rapidly its radical hydrogen to O₂ to form peroxy radical (HO₂^•) and carbon dioxide (CO₂).^[50] Peroxy radical subsequently reacts with nitrogen oxide (NO) to form nitrogen dioxide (NO₂) and hydroxyl radical. NO₂ gives O(³P) via photolysis, thereby forming O₃ following reaction with O₂. Since hydroxyl radical is formed during the formation of NO₂, the balance of the sequence of chemical reactions starting with carbon monoxide and leading to the formation of ozone is:

CO + 2O₂ + hν → CO₂ + O₃

(where hν refers to the photon of light absorbed by the NO₂ molecule in the sequence)

Although the creation of NO₂ is the critical step leading to low level ozone formation, it also increases this ozone in another, somewhat mutually exclusive way, by reducing the quantity of NO that is available to react with ozone.^[51]

Indoor pollution

In closed environments, the concentration of carbon monoxide can easily rise to lethal levels. On average, 170 people in the United States die every year from carbon monoxide produced by non-automotive consumer products.^[52] However, according to the Florida Department of Health, "every year more than 500 Americans die from accidental exposure to carbon monoxide and thousands more across the U.S. require emergency medical care for non-fatal carbon monoxide poisoning"^[53] These products include malfunctioning fuel-burning appliances such as furnaces, ranges, water heaters, and gas and kerosene room heaters; engine-powered equipment such as portable generators; fireplaces; and charcoal that is burned in homes and other enclosed areas. The American Association of Poison Control Centers (AAPCC) reported 15,769 cases of carbon monoxide poisoning resulting in 39 deaths in 2007.^[54] In 2005, the CPSC reported 94 generator-related carbon monoxide poisoning deaths.^[52] Forty-seven of these deaths were known to have occurred during power outages due to severe weather, including Hurricane Katrina.^[52] Still others die from carbon monoxide produced by non-consumer products, such as cars left running in attached garages. The Centers for Disease Control and Prevention estimates that several thousand people go to hospital emergency rooms every year to be treated for carbon monoxide poisoning.^[55]

Presence in blood

Carbon monoxide is absorbed through breathing and enters the blood stream through gas exchange in the lungs. It is also produced in hemoglobin metabolism and enters the blood from the tissues, and thus is present in all normal tissues, even if not inhaled.

Normal circulating levels in the blood are 0% to 3%, and are higher in smokers. Carbon monoxide levels cannot be assessed through a physical exam. Laboratory testing requires a blood sample (arterial or venous) and laboratory analysis on a CO-Oximeter. Additionally, a noninvasive carboxyhemoglobin (SpCO) test method from Pulse CO-Oximetry exists and has been validated compared to invasive methods.^[56]

Astrophysics

Outside of Earth, carbon monoxide is the second-most common molecule in the interstellar medium, after molecular hydrogen. Because of its asymmetry, the carbon monoxide molecule produces far brighter spectral lines than the hydrogen molecule, making CO much easier to detect. Interstellar CO was first detected with radio telescopes in 1970. It is now the most commonly used tracer of molecular gas in general in the interstellar medium of galaxies, as molecular hydrogen can only be detected using ultraviolet light, which requires space telescopes. Carbon monoxide observations provide much of the information about the molecular clouds in which most stars form.^[57]

Beta Pictoris, the second brightest star in the constellation Pictor, shows an excess of infrared emission compared to normal stars of its type, which is caused by large quantities of dust and gas (including carbon monoxide)^[58]^[59] near the star.

Production

Many methods have been developed for carbon monoxide's production.^[60]

Industrial production

A major industrial source of CO is producer gas, a mixture containing mostly carbon monoxide and nitrogen, formed by combustion of carbon in air at high temperature when there is an excess of carbon. In an oven, air is passed through a bed of coke. The initially produced CO₂ equilibrates with the remaining hot carbon to give CO. The reaction of CO₂ with carbon to give CO is described as the Boudouard reaction.^[61] Above 800 °C, CO is the predominant product:

CO₂ + C → 2 CO (ΔH = 170 kJ/mol)

Another source is "water gas", a mixture of hydrogen and carbon monoxide produced via the endothermic reaction of steam and carbon:

H₂O + C → H₂ + CO (ΔH = +131 kJ/mol)

Other similar "synthesis gases" can be obtained from natural gas and other fuels.

Carbon monoxide is also a byproduct of the reduction of metal oxide ores with carbon, shown in a simplified form as follows:

MO + C → M + CO

Carbon monoxide is also produced by the direct oxidation of carbon in a limited supply of oxygen or air.

2C(s) + O₂ → 2CO(g)

Since CO is a gas, the reduction process can be driven by heating, exploiting the positive (favorable) entropy of reaction. The Ellingham diagram shows that CO formation is favored over CO₂ in high temperatures.

Laboratory preparation

Carbon monoxide is conveniently produced in the laboratory by the dehydration of formic acid or oxalic acid, for example with concentrated sulfuric acid.^[62]^[63]^[64] Another method is heating an intimate mixture of powdered zinc metal and calcium carbonate, which releases CO and leaves behind zinc oxide and calcium oxide:

Zn + CaCO₃ → ZnO + CaO + CO

Silver nitrate and iodoform also afford carbon monoxide:

CHI₃ + 3AgNO₃ + H₂O → 3HNO₃ + CO + 3AgI

Coordination chemistry

Main article: metal carbonyl

Energy level scheme of the σ and π orbitals of carbon monoxide

The HOMO of CO is a σ MO.

The LUMO of CO is a π*antibonding MO.

Most metals form coordination complexes containing covalently attached carbon monoxide. Only metals in lower oxidation states will complex with carbon monoxide ligands. This is because there must be sufficient electron density to facilitate back-donation from the metal d_xz-orbital, to the π*molecular orbital from CO. The lone pair on the carbon atom in CO, also donates electron density to the d_x²−y² on the metal to form a sigma bond. This electron donation is also exhibited with the cis effect, or the labilization of CO ligands in the cis position. Nickel carbonyl, for example, forms by the direct combination of carbon monoxide and nickel metal:

Ni + 4 CO → Ni(CO)₄ (1 bar, 55 °C)

For this reason, nickel in any tubing or part must not come into prolonged contact with carbon monoxide. Nickel carbonyl decomposes readily back to Ni and CO upon contact with hot surfaces, and this method is used for the industrial purification of nickel in the Mond process.^[65]

In nickel carbonyl and other carbonyls, the electron pair on the carbon interacts with the metal; the carbon monoxide donates the electron pair to the metal. In these situations, carbon monoxide is called the carbonyl ligand. One of the most important metal carbonyls is iron pentacarbonyl, Fe(CO)₅:

Many metal-CO complexes are prepared by decarbonylation of organic solvents, not from CO. For instance, iridium trichloride and triphenylphosphine react in boiling 2-methoxyethanol or DMF to afford IrCl(CO)(PPh₃)₂.

Metal carbonyls in coordination chemistry are usually studied using infrared spectroscopy.

Organic and main group chemistry

In the presence of strong acids and water, carbon monoxide reacts with alkenes to form carboxylic acids in a process known as the Koch–Haaf reaction.^[62] In the Gattermann–Koch reaction, arenes are converted to benzaldehyde derivatives in the presence of AlCl₃ and HCl.^[63] Organolithium compounds (e.g. butyl lithium) react with carbon monoxide, but these reactions have little scientific use.

Although CO reacts with carbocations and carbanions, it is relatively nonreactive toward organic compounds without the intervention of metal catalysts.^[66]

With main group reagents, CO undergoes several noteworthy reactions. Chlorination of CO is the industrial route to the important compound phosgene. With borane CO forms an adduct, H₃BCO, which is isoelectronic with the acylium cation [H₃CCO]⁺. CO reacts with sodium to give products resulting from C-C coupling such as sodium acetylenediolate 2Na+
·C
2O2−
2. It reacts with molten potassium to give a mixture of an organometallic compound, potassium acetylenediolate 2K+
·C
2O2−
2, potassium benzenehexolate 6K+
C
6O6−
6,^[67] and potassium rhodizonate 2K+
·C
6O2−
6.^[68]

The compounds cyclohexanehexone or triquinoyl (C₆O₆) and cyclopentanepentone or leuconic acid (C₅O₅), which so far have been obtained only in trace amounts, can be regarded as polymers of carbon monoxide.

At pressures of over 5 gigapascals, carbon monoxide converts into a solid polymer of carbon and oxygen. This is metastable at atmospheric pressure but is a powerful explosive.^[69]^[70]

Uses

Chemical industry

Carbon monoxide is an industrial gas that has many applications in bulk chemicals manufacturing.^[71] Large quantities of aldehydes are produced by the hydroformylation reaction of alkenes, carbon monoxide, and H₂. Hydroformylation is coupled to the Shell higher olefin process to give precursors to detergents.

Phosgene, useful for preparing isocyanates, polycarbonates, and polyurethanes, is produced by passing purified carbon monoxide and chlorine gas through a bed of porous activated carbon, which serves as a catalyst. World production of this compound was estimated to be 2.74 million tonnes in 1989.^[72]

CO + Cl₂ → COCl₂

Methanol is produced by the hydrogenation of carbon monoxide. In a related reaction, the hydrogenation of carbon monoxide is coupled to C-C bond formation, as in the Fischer-Tropsch process where carbon monoxide is hydrogenated to liquid hydrocarbon fuels. This technology allows coal or biomass to be converted to diesel.

In the Monsanto process, carbon monoxide and methanol react in the presence of a homogeneous rhodium catalyst and hydroiodic acid to give acetic acid. This process is responsible for most of the industrial production of acetic acid.

An industrial scale use for pure carbon monoxide is purifying nickel in the Mond process.

Meat coloring

Carbon monoxide is used in modified atmosphere packaging systems in the US, mainly with fresh meat products such as beef, pork, and fish to keep them looking fresh. The carbon monoxide combines with myoglobin to form carboxymyoglobin, a bright-cherry-red pigment. Carboxymyoglobin is more stable than the oxygenated form of myoglobin, oxymyoglobin, which can become oxidized to the brown pigment metmyoglobin. This stable red color can persist much longer than in normally packaged meat.^[73] Typical levels of carbon monoxide used in the facilities that use this process are between 0.4% to 0.5%.

The technology was first given "generally recognized as safe" (GRAS) status by the U.S. Food and Drug Administration (FDA) in 2002 for use as a secondary packaging system, and does not require labeling. In 2004, the FDA approved CO as primary packaging method, declaring that CO does not mask spoilage odor.^[74] Despite this ruling, the process remains controversial for fears that it masks spoilage.^[75]^[76] In 2007, a bill^[77] was introduced to the United States House of Representatives to label modified atmosphere carbon monoxide packaging as a color additive, but the bill died in subcommittee. The process is banned in many other countries, including Japan, Singapore, and the European Union.^[78]^[79]^[80]

Medicine

Following the first report that carbon monoxide is a normal neurotransmitter in 1993,^[7]^[8] as well as one of three gases that naturally modulate inflammatory responses in the body (the other two being nitric oxide and hydrogen sulfide), carbon monoxide has received a great deal of clinical attention as a biological regulator. In many tissues, all three gases are known to act as anti-inflammatories, vasodilators, and encouragers of neovascular growth.^[9] However, the issues are complex, as neovascular growth is not always beneficial, since it plays a role in tumor growth, and also the damage from wet macular degeneration, a disease for which smoking (a major source of carbon monoxide in the blood, several times more than natural production) increases the risk from 4 to 6 times.

There is a theory that, in some nerve cell synapses, when long-term memories are being laid down, the receiving cell makes carbon monoxide, which back-transmits to the transmitting cell, telling it to transmit more readily in future. Some such nerve cells have been shown to contain guanylate cyclase, an enzyme that is activated by carbon monoxide.^[8]

Studies involving carbon monoxide have been conducted in many laboratories throughout the world for its anti-inflammatory and cytoprotective properties. These properties have potential to be used to prevent the development of a series of pathological conditions including ischemia reperfusion injury, transplant rejection, atherosclerosis, severe sepsis, severe malaria, or autoimmunity. Clinical tests involving humans have been performed, however the results have not yet been released.^[10]

Lasers

Carbon monoxide has also been used as a lasing medium in high-powered infrared lasers.^[81]

Gas lasers

Carbon dioxide Carbon monoxide Helium–neon Nitrogen TEA laser Asterix IV laser ISKRA4,5

Distinct subtypes:	Chemical laser Excimer lasers Ion laser Metal-vapor laser

Laser types: Solid-state Semiconductor Dye Gas Chemical Excimer Ion Metal Vapor

Niche uses

Carbon monoxide has been proposed for use as a fuel on Mars. Carbon monoxide/oxygen engines have been suggested for early surface transportation use as both carbon monoxide and oxygen can be straightforwardly produced from the atmosphere of Mars by zirconia electrolysis, without using any Martian water resources to obtain hydrogen, which would be needed to make methane or any hydrogen-based fuel.^[82]

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1 2 Blumenthal, Ivan (1 June 2001). "Carbon monoxide poisoning". J R Soc Med (The Royal Society of Medicine) 94 (6): 270–272. PMC 1281520. PMID 11387414.
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↑ Thauer, R. K. (1998). "Biochemistry of methanogenesis: a tribute to Marjory Stephenson. 1998 Marjory Stephenson Prize Lecture" (Free). Microbiology 144 (9): 2377–2406. doi:10.1099/00221287-144-9-2377. PMID 9782487.
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↑ Global Maps. Carbon Monoxide. earthobservatory.nasa.gov
↑ Source for figures: Carbon dioxide, NOAA Earth System Research Laboratory, (updated 2010.06). Methane, IPCC TAR table 6.1, (updated to 1998). The NASA total was 17 ppmv over 100%, and CO₂ was increased here by 15 ppmv. To normalize, N₂ should be reduced by about 25 ppmv and O₂ by about 7 ppmv.
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↑ Singer, Siegfried Fred (1975). The Changing Global Environment. Springer. p. 90. ISBN 9027704023.
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↑ White, James Carrick; et al. (1989). Global climate change linkages: acid rain, air quality, and stratospheric ozone. Springer. p. 106. ISBN 0-444-01515-9.
↑ Pommier, M.; Law, K. S.; Clerbaux, C.; Turquety, S.; Hurtmans, D.; Hadji-Lazaro, J.; Coheur, P.-F.; Schlager, H.; Ancellet, G.; Paris, J.-D.; Nédélec, P.; Diskin, G. S.; Podolske, J. R.; Holloway, J. S.; Bernath, P. (2010). "IASI carbon monoxide validation over the Arctic during POLARCAT spring and summer campaigns". Atmospheric Chemistry and Physics 10 (21): 10655–10678. Bibcode:2010ACP....1010655P. doi:10.5194/acp-10-10655-2010.
↑ Pommier, M.; McLinden, C. A.; Deeter, M. (2013). "Relative changes in CO emissions over megacities based on observations from space". Geophysical Research Letters 40 (14): 3766. Bibcode:2013GeoRL..40.3766P. doi:10.1002/grl.50704.
↑ Reeves, Claire E.; Penkett, Stuart A.; Bauguitte, Stephane; Law, Kathy S.; Evans, Mathew J.; Bandy, Brian J.; Monks, Paul S.; Edwards, Gavin D.; Phillips, Gavin; Barjat, Hannah; Kent, Joss; Dewey, Ken; Schmitgen, Sandra; Kley, Dieter (2002). "Potential for photochemical ozone formation in the troposphere over the North Atlantic as derived from aircraft observationsduring ACSOE". Journal of Geophysical Research 107 (D23): 4707. Bibcode:2002JGRD..107.4707R. doi:10.1029/2002JD002415.
↑ Ozone and other photochemical oxidants. National Academies. 1977. p. 23. ISBN 0-309-02531-1.
1 2 3 U.S Consumer Product Safety Commission, Carbon Monoxide Questions and Answers, accessed 2009-12-04
↑ "Tracking Carbon Monoxide". Environmental Public Health Tracking – Florida Dept. of Health.
↑ "AAPCC Annual Data Reports 2007". American Association of Poison Control Centers.
↑ Centers for Disease Control and Prevention, National Environmental Public Health Tracking Network, Carbon Monoxide Poisoning, accessed 2009-12-04
↑ Roth D., Herkner H., Schreiber W., Hubmann N., Gamper G., Laggner A.N., Havel C. (2011). "Accuracy of Noninvasive Multiwave Pulse Oximetry Compared With Carboxyhemoglobin From Blood Gas Analysis in Unselected Emergency Department Patients" (PDF). Annals of Emergency Medicine 58 (1): 74–9. doi:10.1016/j.annemergmed.2010.12.024. PMID 21459480.
↑ Combes, Françoise (1991). "Distribution of CO in the Milky Way". Annual Review of Astronomy & Astrophysics 29: 195–237. Bibcode:1991ARA&A..29..195C. doi:10.1146/annurev.aa.29.090191.001211.
↑ Khan, Amina. "Did two planets around nearby star collide? Toxic gas holds hints". Los Angeles Times. Retrieved March 9, 2014.
↑ Dent, W.R.F.; Wyatt, M.C.;Roberge, A.; Augereau,J.-C.; Casassus, S.;Corder, S.; Greaves, J.S.; de Gregorio-Monsalvo, I; Hales, A.; Jackson, A.P.; Hughes, A. Meredith; Lagrange, A.-M; Matthews, B.; Wilner, D. (March 6, 2014). "Molecular Gas Clumps from the Destruction of Icy Bodies in the β Pictoris Debris Disk". Science 343: 1490–1492. arXiv:1404.1380. Bibcode:2014Sci...343.1490D. doi:10.1126/science.1248726. Retrieved March 9, 2014.
↑ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 200. ISBN 0-12-352651-5.
↑ Higman, C; van der Burgt, M (2003). Gasification. Gulf Professional Publishing. p. 12. ISBN 0-7506-7707-4.
1 2 Koch, H.; Haaf, W. (1973). "1-Adamantanecarboxylic Acid". Org. Synth. ; Coll. Vol. 5, p. 20
1 2 Coleman, G. H. and Craig, David (1943). "p-Tolualdehyde". Org. Synth. ; Coll. Vol. 2, p. 583
↑ Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. Newyork: Academic Press. p. 646. ISBN 978-0121266011.
↑ Mond L, Langer K, Quincke F (1890). "Action of carbon monoxide on nickel". Journal of the Chemical Society 57: 749–753. doi:10.1039/CT8905700749.
↑ Chatani, N.; Murai, S. "Carbon Monoxide" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. doi:10.1002/047084289
↑ Büchner, W.; Weiss, E. (1964). "Zur Kenntnis der sogenannten "Alkalicarbonyle" IV[1] Über die Reaktion von geschmolzenem Kalium mit Kohlenmonoxid". Helvetica Chimica Acta 47 (6): 1415–1423. doi:10.1002/hlca.19640470604.
↑ Fownes, George (1869). A Manual of elementary chemistry. H.C. Lea. p. 678.
↑ Katz, Allen I.; Schiferl, David; Mills, Robert L. (1984). "New phases and chemical reactions in solid carbon monoxide under pressure". The Journal of Physical Chemistry 88 (15): 3176–3179. doi:10.1021/j150659a007.
↑ Evans, W. J.; Lipp, M. J.; Yoo, C.-S.; Cynn, H.; Herberg, J. L.; Maxwell, R. S.; Nicol, M. F. (2006). "Pressure-Induced Polymerization of Carbon Monoxide: Disproportionation and Synthesis of an Energetic Lactonic Polymer". Chemistry of Materials 18 (10): 2520–2531. doi:10.1021/cm0524446.
↑ Elschenbroich, C.; Salzer, A. (2006). Organometallics: A Concise Introduction (2nd ed.). Weinheim: Wiley-VCH. ISBN 3-527-28165-7.
↑ Wolfgang Schneider; Werner Diller (2005), "Phosgene", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a19_411
↑ Sorheim, S, Nissena, H, Nesbakken, T (1999). "The storage life of beef and pork packaged in an atmosphere with low carbon monoxide and high carbon dioxide". Journal of Meat Science 52 (2): 157–164. doi:10.1016/S0309-1740(98)00163-6.
↑ Eilert EJ (2005). "New packaging technologies for the 21st century". Journal of Meat Science 71 (1): 122–127. doi:10.1016/j.meatsci.2005.04.003.
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↑ Landis (2001). "Mars Rocket Vehicle Using In Situ Propellants". Journal of Spacecraft and Rockets 38 (5): 730–735. Bibcode:2001JSpRo..38..730L. doi:10.2514/2.3739.

External links

Wikimedia Commons has media related to Carbon monoxide.

Explanation of the structure
Carbon Monoxide Safety Association
International Chemical Safety Card 0023
NIOSH Pocket Guide to Chemical Hazards
CDC – Carbon Monoxide – NIOSH Workplace Safety and Health Topic
External MSDS data sheet
Carbon Monoxide Detector Placement
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Carbon Monoxide Hazards with Backpacking Stoves
Microscale Gas Chemistry Experiments with Carbon Monoxide
Instant insight outlining the physiology of carbon monoxide from the Royal Society of Chemistry
Pictures of CO Poisoning Radiology and Pathology Images from MedPix.
The Silent Killer - Everything You Need To Know About Carbon Monoxide Poisoning

Oxides

Mixed oxidation states	Antimony tetroxide (Sb₂O₄) Cobalt(II,III) oxide (Co₃O₄) Iron(II,III) oxide (Fe₃O₄) Lead(II,IV) oxide (Pb₃O₄) Manganese(II,III) oxide (Mn₃O₄) Silver(I,III) oxide (Ag₂O₂) Triuranium octoxide (U₃O₈)

+1 oxidation state	Copper(I) oxide (Cu₂O) Dicarbon monoxide (C₂O) Dichlorine monoxide (Cl₂O) Lithium oxide (Li₂O) Potassium oxide (K₂O) Rubidium oxide (Rb₂O) Silver oxide (Ag₂O) Thallium(I) oxide (Tl₂O) Sodium oxide (Na₂O) Water (hydrogen oxide) (H₂O)

+2 oxidation state	Aluminium(II) oxide (Al O) Barium oxide (Ba O) Beryllium oxide (Be O) Cadmium oxide (Cd O) Calcium oxide (Ca O) Carbon monoxide (C O) Chromium(II) oxide (Cr O) Cobalt(II) oxide (Co O) Copper(II) oxide (Cu O) Iron(II) oxide (Fe O) Lead(II) oxide (Pb O) Magnesium oxide (Mg O) Mercury(II) oxide (Hg O) Nickel(II) oxide (Ni O) Nitric oxide (N O) Palladium(II) oxide (Pd O) Strontium oxide (Sr O) Sulfur monoxide (S O) Disulfur dioxide (S₂O₂) Tin(II) oxide (Sn O) Titanium(II) oxide (Ti O) Vanadium(II) oxide (V O) Zinc oxide (Zn O)

+3 oxidation state	Aluminium oxide (Al₂O₃) Antimony trioxide (Sb₂O₃) Arsenic trioxide (As₂O₃) Bismuth(III) oxide (Bi₂O₃) Boron trioxide (B₂O₃) Chromium(III) oxide (Cr₂O₃) Dinitrogen trioxide (N₂O₃) Erbium(III) oxide (Er₂O₃) Gadolinium(III) oxide (Gd₂O₃) Gallium(III) oxide (Ga₂O₃) Holmium(III) oxide (Ho₂O₃) Indium(III) oxide (In₂O₃) Iron(III) oxide (Fe₂O₃) Lanthanum oxide (La₂O₃) Lutetium(III) oxide (Lu₂O₃) Nickel(III) oxide (Ni₂O₃) Phosphorus trioxide (P₄O₆) Promethium(III) oxide (Pm₂O₃) Rhodium(III) oxide (Rh₂O₃) Samarium(III) oxide (Sm₂O₃) Scandium oxide (Sc₂O₃) Terbium(III) oxide (Tb₂O₃) Thallium(III) oxide (Tl₂O₃) Thulium(III) oxide (Tm₂O₃) Titanium(III) oxide (Ti₂O₃) Tungsten(III) oxide (W₂O₃) Vanadium(III) oxide (V₂O₃) Ytterbium(III) oxide (Yb₂O₃) Yttrium(III) oxide (Y₂O₃)

+4 oxidation state	Carbon dioxide (C O₂) Carbon trioxide (C O₃) Cerium(IV) oxide (Ce O₂) Chlorine dioxide (Cl O₂) Chromium(IV) oxide (Cr O₂) Dinitrogen tetroxide (N₂O₄) Germanium dioxide (Ge O₂) Hafnium(IV) oxide (Hf O₂) Lead dioxide (Pb O₂) Manganese dioxide (Mn O₂) Nitrogen dioxide (N O₂) Plutonium(IV) oxide (Pu O₂) Rhodium(IV) oxide (Rh O₂) Ruthenium(IV) oxide (Ru O₂) Selenium dioxide (Se O₂) Silicon dioxide (Si O₂) Sulfur dioxide (S O₂) Tellurium dioxide (Te O₂) Thorium dioxide (Th O₂) Tin dioxide (Sn O₂) Titanium dioxide (Ti O₂) Tungsten(IV) oxide (W O₂) Uranium dioxide (U O₂) Vanadium(IV) oxide (V O₂) Zirconium dioxide (Zr O₂)

+5 oxidation state	Antimony pentoxide (Sb₂O₅) Arsenic pentoxide (As₂O₅) Dinitrogen pentoxide (N₂O₅) Niobium pentoxide (Nb₂O₅) Phosphorus pentoxide (P₂O₅) Tantalum pentoxide (Ta₂O₅) Vanadium(V) oxide (V₂O₅)

+6 oxidation state	Chromium trioxide (Cr O₃) Molybdenum trioxide (Mo O₃) Rhenium trioxide (Re O₃) Selenium trioxide (Se O₃) Sulfur trioxide (S O₃) Tellurium trioxide (Te O₃) Tungsten trioxide (W O₃) Uranium trioxide (U O₃) Xenon trioxide (Xe O₃)

+7 oxidation state	Dichlorine heptoxide (Cl₂O₇) Manganese heptoxide (Mn₂O₇) Rhenium(VII) oxide (Re₂O₇) Technetium(VII) oxide (Tc₂O₇)

+8 oxidation state	Osmium tetroxide (Os O₄) Ruthenium tetroxide (Ru O₄) Xenon tetroxide (Xe O₄) Iridium tetroxide (Ir O₄) Hassium tetroxide (Hs O₄)

Related	Oxocarbon Suboxide Oxyanion Ozonide

Oxides are sorted by oxidation state. Category:Oxides

Oxocarbons

Common oxides	CO 2 CO

Exotic oxides	CO 3 CO 4 CO 5 CO 6 C 2O C 2O 2 C 2O 3 C 2O 4 C 2O 4 C 3O 2 C 3O 3 C 3O 6 C 4O 2 C 4O 4 C 4O 6 C 5O 2 C 5O 5 C 6O 6 C 6O 6 C 8O 8 C 9O 9 C 10O 8 C 10O 10 C 12O 6 C 12O 9 C 12O 12

Polymers	Graphite oxide C₃O₂ CO CO₂

Compounds derived from oxides	Metal carbonyls Carbonic acid Bicarbonates Carbonates Dicarbonates Tricarbonates

Neurotransmitters

Amino acid-derived	Major excitatory/inhibitory systems: Glutamate system: Agmatine Aspartic acid (aspartate) Cycloserine Glutamic acid (glutamate) Glutathione Glycine GSNO GSSG Kynurenic acid NAA NAAG Proline Serine; GABA system: GABA GABOB GHB; Glycine system: α-Alanine β-Alanine Glycine Hypotaurine Proline Sarcosine Serine Taurine; GHB system: GHB T-HCA (GHC) Biogenic amines: Monoamines: 6-OHM Dopamine Epinephrine (adrenaline) Melatonin NAS (normelatonin) Norepinephrine (noradrenaline) Serotonin (5-HT); Trace amines: 3-Iodothyronamine N-Methylphenethylamine N-Methyltryptamine m-Octopamine p-Octopamine Phenylethanolamine Phenethylamine Synephrine Tryptamine m-Tyramine p-Tyramine; Others: Histamine Neuropeptides: See here instead.

Lipid-derived	Endocannabinoids: 2-AG 2-AGE (noladin ether) 2-ALPI 2-OG AA-5-HT Anandamide (AEA) DEA LPI NADA NAGly OEA Oleamide PEA RVD-Hpα SEA Virodhamine (O-AEA) Neurosteroids: See here instead.

Nucleobase-derived	Nucleosides: Adenosine system: Adenosine ADP AMP ATP

Vitamin-derived	Cholinergic system: Acetylcholine

Miscellaneous	Gasotransmitters: Carbon monoxide (CO) Hydrogen sulfide (H₂S) Nitric oxide (NO); Candidates: Acetaldehyde Ammonia (NH₃) Carbonyl sulfide (COS) Nitrous oxide (N₂O) Sulfur dioxide (SO₂)

Molecules detected in outer space

Molecules

Diatomic	Aluminium monochloride Aluminium monofluoride Aluminium monoxide Argon hydride Carbon monophosphide Carbon monosulfide Carbon monoxide Carborundum Cyanogen radical Diatomic carbon Fluoromethylidynium Hydrogen chloride Hydrogen fluoride Hydrogen (molecular) Hydroxyl radical Iron(II) oxide Magnesium monohydride cation Methylidyne radical Nitric oxide Nitrogen (molecular) Nitrogen monohydride Nitrogen sulfide Oxygen (molecular) Phosphorus monoxide Phosphorus mononitride Potassium chloride Silicon carbide Silicon mononitride Silicon monoxide Silicon monosulfide Sodium chloride Sodium iodide Sulfur monohydride Sulfur monoxide Titanium oxide

Triatomic	Aluminium hydroxide Aluminium isocyanide Amino radical Carbon dioxide Carbonyl sulfide CCP radical Chloronium Diazenylium Dicarbon monoxide Disilicon carbide Ethynyl radical Formyl radical Hydrogen cyanide Hydrogen isocyanide (HCN) Hydrogen isocyanide (HNC) Hydrogen sulfide Hydroperoxyl Iron cyanide Isoformyl Magnesium cyanide Magnesium isocyanide Methylene radical N₂H⁺ Nitrous oxide Nitroxyl Ozone Phosphaethyne Potassium cyanide Protonated molecular hydrogen Sodium cyanide Sodium hydroxide Silicon carbonitride c-Silicon dicarbide Silicon naphthalocyanine Sulfur dioxide Thioformyl Thioxoethenylidene Titanium dioxide Tricarbon Water

Four atoms	Acetylene Ammonia Cyanic acid Cyanoethynyl Cyclopropynylidyne Formaldehyde Fulminic acid HCCN Hydrogen peroxide Hydromagnesium isocyanide Isocyanic acid Isothiocyanic acid Ketenyl Methylene amidogen Methyl radical Propynylidyne Protonated carbon dioxide Protonated hydrogen cyanide Silicon tricarbide Thioformaldehyde Tricarbon monoxide Tricarbon sulfide Thiocyanic acid

Five atoms	Ammonium Ion Butadiynyl Carbodiimide Cyanamide Cyanoacetylene Cyanoformaldehyde Cyanomethyl Cyclopropenylidene Formic acid Isocyanoacetylene Ketene Methane Methoxy radical Methylenimine Propadienylidene Protonated formaldehyde Protonated formaldehyde Silane Silicon-carbide cluster

Six atoms	Acetonitrile Cyanobutadiynyl radical E-Cyanomethanimine Cyclopropenone Diacetylene Ethylene Formamide HC₄N Ketenimine Methanethiol Methanol Methyl isocyanide Pentynylidyne Propynal Protonated cyanoacetylene

Seven atoms	Acetaldehyde Acrylonitrile Cyanodiacetylene Ethylene oxide Hexatriynyl radical Methylacetylene Methylamine Methyl isocyanate Vinyl alcohol

Eight atoms	Acetic acid Aminoacetonitrile Cyanoallene Ethanimine Glycolaldehyde Heptatrienyl radical Hexapentaenylidene Methylcyanoacetylene Methyl formate Propenal

Nine atoms	Acetamide Cyanohexatriyne Cyanotriacetylene Dimethyl ether Ethanol Methyldiacetylene Octatetraynyl radical Propene Propionitrile

Ten atoms or more	Acetone Benzene Buckminsterfullerene (C₆₀ fullerene) ("bucky-ball") C₇₀ fullerene Cyanodecapentayne Cyanopentaacetylene Cyanotetra-acetylene Ethylene glycol Ethyl formate Methyl acetate Methyl-cyano-diacetylene Methyltriacetylene Propanal n-Propyl cyanide Pyrimidine

Deuterated
molecules

Unconfirmed

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Category:Astrochemistry
Category:Molecules
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Inorganic compounds of carbon and related ions

Compounds	CBr₄ CCl₄ CF CF₄ CI₄ CO CO₂ CO₃ COS CS CS₂ CSe₂ C₃O₂ C₃S₂ CH₄ C₂H₆ C₃H₈ C₄H₁₀ C₅H₁₂ C₆H₁₄ C₇H₁₆ C₈H₁₈ C₆H₆ SiC

Carbon ions	Carbides [:C≡C:]^2–, [::C::]^4–, [:C=C=C:]^4– Cyanides [:C≡N:]^– Cyanates [:O-C≡N:]^– Thiocyanates [:S-C≡N:]^– Fulminates [:C≡N-O:]^– Thiofulminates [:C≡N-S:]^–

Oxides and related	Oxides Metal carbonyls Carbonic acid Bicarbonates Carbonates

Oxygen compounds

AgO Al₂O₃ AmO₂ Am₂O₃ As₂O₃ As₂O₅ Au₂O₃ B₂O₃ BaO BeO Bi₂O₃ BiO₂ Bi₂O₅ BrO₂ Br₂O₃ Br₂O₅ CO CO₂ C₂O₃ CaO CaO₂ CdO CeO₂ Ce₂O₃ ClO₂ Cl₂O Cl₂O₃ Cl₂O₄ Cl₂O₆ Cl₂O₇ CoO Co₂O₃ Co₃O₄ CrO₃ Cr₂O₃ Cr₂O₅ Cr₅O₁₂ CsO₂ Cs₂O₃ CuO D₂O Dy₂O₃ Er₂O₃ Eu₂O₃ F₂O F₂O₂ F₂O₄ FeO Fe₂O₃ Fe₃O₄ Ga₂O Ga₂O₃ GeO GeO₂ H₂O H₂¹⁸O H₂O₂ HfO₂ HgO Hg₂O Ho₂O₃ I₂O₄ I₂O₅ I₂O₆ I₄O₉ In₂O₃ InO₂ KO₂ K₂O₂ La₂O₃ Li₂O Li₂O₂ Lu₂O₃ MgO Mg₂O₃ MnO MnO₂ Mn₂O₃ Mn₂O₇ MoO₂ MoO₃ Mo₂O₃ NO NO₂ N₂O N₂O₃ N₂O₄ N₂O₅ NaO₂ Na₂O Na₂O₂ NbO NbO₂ Nd₂O₃

Chemical formulas

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