Chemistry:Anthrone
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| Preferred IUPAC name
Anthracen-9(10H)-one | |
Other names
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| Properties | |
| C14H10O | |
| Molar mass | 194.233 g·mol−1 |
| Appearance | White to light yellow needles |
| Melting point | 155 to 158 °C (311 to 316 °F; 428 to 431 K) |
| Boiling point | 721 °C (1,330 °F; 994 K) |
| Insoluble | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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Anthrone is a tricyclic aromatic ketone. It is used for a common cellulose assay and in the colorimetric determination of carbohydrates.[1]
Derivatives of anthrone are used in pharmacy as laxative. They stimulate the motion of the colon and reduce water reabsorption. Some anthrone derivatives can be extracted from a variety of plants, including Rhamnus frangula, Aloe ferox, Rheum officinale, and Cassia senna.[citation needed] Glycosides of anthrone are also found in high amounts in rhubarb leaves, and alongside concentrated amounts of oxalic acid are the reason for the leaves being inedible.
Synthesis and reactions
Anthrone can be prepared from anthraquinone by reduction with tin or copper.[2]
An alternative synthesis involves cyclization of o-benzylbenzoic acid induced with hydrogen fluoride.[3]
Anthrone condenses with glyoxal to give, following dehydrogenation, acedianthrone, a useful octacyclic pigment.[4]
Tautomer
thumb|center|314px|Tautomeric equilibrium for anthrone. Anthrone is the more stable tautomer relative to the anthrol. The tautomeric equilibrium is estimated at 100 in aqueous solution. For the two other isomeric anthrols, the tautomeric equilibrium is reversed.[5]
References
- ↑ Trevelyan, W. E.; Forrest, RS; Harrison, JS (1952). "Determination of Yeast Carbohydrates with the Anthrone Reagent". Nature 170 (4328): 626–627. doi:10.1038/170626a0. PMID 13002392. Bibcode: 1952Natur.170..626T.
- ↑ Macleod, L. C.; Allen, C. F. H. (1934). "Benzanthrone". Organic Syntheses 14: 4. doi:10.15227/orgsyn.014.0004.
- ↑ Fieser, Louis F.; Hershberg, E. B. (May 1939). "Inter- and Intramolecular Acylations with Hydrogen Fluoride". Journal of the American Chemical Society 61 (5): 1272–1281. doi:10.1021/ja01874a079.
- ↑ Bien, H.-S.; Stawitz, J.; Wunderlich, K. (2005). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a02_355.
- ↑ Ośmiałowski, Borys; Raczyńska, Ewa D.; Krygowski, Tadeusz M. (2006). "Tautomeric Equilibria and Pi Electron Delocalization for Some Monohydroxyarenes Quantum Chemical Studies". The Journal of Organic Chemistry 71 (10): 3727–3736. doi:10.1021/jo052615q. PMID 16674042.
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