Glyoxal

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Glyoxal
Skeletal formula of glyoxal
Space-filling model of glyox
Names
Preferred IUPAC name
Oxaldehyde
Systematic IUPAC name
Ethanedial
Other names
Glyoxal
Oxalaldehyde
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.003.160
KEGG
UNII
Properties
C2H2O2
Molar mass 58.04 g·mol−1
Density 1.27 g/cm3
Melting point 15 °C (59 °F; 288 K)
Boiling point 51 °C (124 °F; 324 K)
Thermochemistry
1.044 J/(K·g)
Hazards
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oilHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroformReactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calciumSpecial hazards (white): no codeNFPA 704 four-colored diamond
1
2
1
Flash point −4 °C (25 °F; 269 K)
285 °C (545 °F; 558 K)
Related compounds
Related aldehydes
acetaldehyde
glycolaldehyde
propanedial
methylglyoxal
Related compounds
glyoxylic acid
glycolic acid
oxalic acid
pyruvic acid
diacetyl
acetylacetone
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

Glyoxal is an organic compound with the chemical formula OCHCHO. It is the smallest dialdehyde (a compound with two aldehyde groups). It is a crystalline solid, white at low temperatures and yellow near the melting point (15 °C). The liquid is yellow, and the vapor is green.[1]

Pure glyoxal is not commonly encountered because it forms hydrates, which oligomerize. For many purposes, these hydrated oligomers behave equivalently to glyoxal. It is produced industrially as a precursor to many products.[2]

Production[edit]

Glyoxal was first prepared and named by the German-British chemist Heinrich Debus (1824–1915) by reacting ethanol with nitric acid.[3][4]

Commercial glyoxal is prepared either by the gas-phase oxidation of ethylene glycol in the presence of a silver or copper catalyst (the Laporte process) or by the liquid-phase oxidation of acetaldehyde with nitric acid.[2]

The first commercial glyoxal source was in Lamotte, France, started in 1960. The single largest commercial source is BASF in Ludwigshafen, Germany, at around 60,000 tons per year. Other production sites exist also in the US and China. Commercial bulk glyoxal is made and reported as a 40%-strength solution in water.

Glyoxal may be synthesized in the laboratory by oxidation of acetaldehyde with selenious acid.[5]

Anhydrous glyoxal is prepared by heating solid glyoxal hydrate(s) with phosphorus pentoxide and condensing the vapors in a cold trap.[6]

The experimentally determined Henry's law constant of glyoxal is:

KH = 4.19 × 105 × exp[62.2 × 103/R × (1/T1/298)].[7][clarification needed]

Applications[edit]

Coated paper and textile finishes use large amounts of glyoxal as a crosslinker for starch-based formulations. It condenses with urea to afford 4,5-dihydroxy-2-imidazolidinone, which further reacts with formaldehyde to give the bis(hydroxymethyl) derivative dimethylol ethylene urea, which is used for wrinkle-resistant chemical treatments of clothing, i.e. permanent press.

Glyoxal is used as a solubilizer and cross-linking agent in polymer chemistry.

Glyoxal is a valuable building block in organic synthesis, especially in the synthesis of heterocycles such as imidazoles.[8] A convenient form of the reagent for use in the laboratory is its bis(hemiacetal) with ethylene glycol, 1,4-dioxane-2,3-diol. This compound is commercially available.

Glyoxal solutions can also be used as a fixative for histology, that is, a method of preserving cells for examining them under a microscope.

Speciation in solution[edit]

Hydrated glyoxal (top) and derived oligomers, called dimers and trimers. The middle and lower species exist as mixtures of isomers.

Glyoxal is supplied typically as a 40% aqueous solution.[2] Like other small aldehydes, glyoxal forms hydrates. Furthermore, the hydrates condense to give a series of oligomers, some of which remain of uncertain structure. For most applications, the exact nature of the species in solution is inconsequential. At least one hydrate of glyoxal is sold commercially, glyoxal trimer dihydrate: [(CHO)2]3(H2O)2 (CAS 4405-13-4). Other glyoxal equivalents are available, such as the ethylene glycol hemiacetal 1,4-dioxane-trans-2,3-diol (CAS 4845-50-5, m.p. 91–95 °C),

It is estimated that, at concentrations less than 1 M, glyoxal exists predominantly as the monomer or hydrates thereof, i.e., OCHCHO, OCHCH(OH)2, or (HO)2CHCH(OH)2. At concentrations above 1 M, dimers predominate. These dimers are probably dioxolanes, with the formula [(HO)CH]2O2CHCHO.[9] Dimer and trimers precipitate as solids from cold solutions.

Other occurrences[edit]

Glyoxal has been observed as a trace gas in the atmosphere, e.g. as an oxidation product of hydrocarbons.[10] Tropospheric concentrations of 0–200 ppt by volume have been reported, in polluted regions up to 1 ppb by volume.[11]

Safety[edit]

The LD50 (oral, rats) is 3300 mg/kg, which is very low.[2]

References[edit]

  1. ^ O'Neil, M.J. (2001): The Merck Index, 13th Edition, page 803.
  2. ^ a b c d Mattioda, Georges; Blanc, Alain, "Glyoxal", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a12_491.pub2 
  3. ^ See:
  4. ^ Henry Enfield Roscoe and Carl Schorlemmer, A Treatise on Chemistry, vol. 3 (New York, New York: D. Appleton and Co., 1890), pp. 101-102.
  5. ^ Ronzio, A. R.; Waugh, T. D. (1944). "Glyoxal Bisulfite". Organic Syntheses. 24: 61. ; Collective Volume, 3, p. 438 
  6. ^ Harries, C.; Temme, F. (1907). "Über monomolekulares und trimolekulares Glyoxal" [On monomoleular and trimoecular glyoxal]. Berichte. 40 (1): 165–172. doi:10.1002/cber.19070400124. Man erhitzt nun das Glyoxal-Phosphorpentoxyd-Gemisch mit freier Flamme und beobachtet bald, dass sich unter Schwarzfärbung des Kolbeninhalte ein flüchtiges grünes Gas bildet, welches sich in der gekühlten Vorlage zu schönen Krystallen von gelber Farbe kondensiert. [One heats the mixture of (crude) glyoxal and P4O10 with an open flame and soon observes, upon blackening of the contents, a mobile green gas which condenses in the cooled flask as beautiful yellow crystals.] 
  7. ^ Ip, H. S.; Huang, X. H.; Yu, J. Z. (2009). "Effective Henry's law constants of glyoxal, glyoxylic acid, and glycolic acid". Geophys. Res. Lett. 36 (1): L01802. Bibcode:2009GeoRL..36.1802I. doi:10.1029/2008GL036212. 
  8. ^ Snyder, H. R.; Handrick, R. G.; Brooks, L. A. (1942). "Imidazole". Organic Syntheses. 22: 65. ; Collective Volume, 3, p. 471 
  9. ^ Whipple, E. B. (1970). "Structure of Glyoxal in Water". J. Am. Chem. Soc. 92 (24): 7183–7186. doi:10.1021/ja00727a027. 
  10. ^ Vrekoussis, M.; Wittrock, F.; Richter, A.; Burrows, J. P. (2009). "Temporal and spatial variability of glyoxal as observed from space". Atmos. Chem. Phys. 9: 4485–4504. doi:10.5194/acp-9-4485-2009. 
  11. ^ Volkamer, Rainer; et al. (2007). "A missing sink for gas‐phase glyoxal in Mexico City: Formation of secondary organic aerosol". Geophys. Res. Lett. 34: 19. Bibcode:2007GeoRL..3419807V. doi:10.1029/2007gl030752. 

External links[edit]