|Preferred IUPAC name
|Systematic IUPAC name
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||178.234 g·mol−1|
|Density||1.28 g/cm3 (25 °C)|
0.969 g/cm3 (220 °C)
|Melting point||216 °C (421 °F; 489 K) at 760 mmHg|
|Boiling point||341.3 °C (646.3 °F; 614.5 K) at 760 mmHg|
|0.022 mg/L (0 °C)|
0.044 mg/L (25 °C)
0.29 mg/L (50 °C)
0.00045% w/w (100 °C, 3.9 MPa)
|Solubility||Soluble in alcohol, (C2H5)2O, acetone, C6H6, CHCl3, CS2|
|Solubility in ethanol||0.76 g/kg (16 °C)|
1.9 g/kg (19.5 °C)
3.28 g/kg (25 °C)
|Solubility in methanol||18 g/kg (19.5 °C)|
|Solubility in hexane||3.7 g/kg|
|Solubility in toluene||9.2 g/kg (16.5 °C)|
129.4 g/kg (100 °C)
|Solubility in carbon tetrachloride||7.32 g/kg|
|Vapor pressure||0.01 kPa (125.9 °C)|
0.1 kPa (151.5 °C)
13.4 kPa (250 °C)
|UV-vis (λmax)||345.6 nm, 363.2 nm|
|Thermal conductivity||0.1416 W/(m·K) (240 °C)|
0.1334 W/(m·K) (270 °C)
0.1259 W/(m·K) (300 °C)
|Viscosity||0.602 cP (240 °C)|
0.498 cP (270 °C)
0.429 cP (300 °C)
|Monoclinic (290 K)|
a = 8.562 Å, b = 6.038 Å, c = 11.184 Å
α = 90°, β = 124.7°, γ = 90°
Heat capacity (C)
Std enthalpy of
Std enthalpy of
|GHS Signal word||Warning|
|H302, H305, H315, H319, H335, H410|
|P261, P273, P305+P351+P338, P501|
|NFPA 704 (fire diamond)|
|Flash point||121 °C (250 °F; 394 K)|
|540 °C (1,004 °F; 813 K)|
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|100-149 mg/kg (rats, oral)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|(what is ?)|
Anthracene is a solid polycyclic aromatic hydrocarbon (PAH) of formula C14H10, consisting of three fused benzene rings. It is a component of coal tar. Anthracene is used in the production of the red dye alizarin and other dyes. Anthracene is colorless but exhibits a blue (400–500 nm peak) fluorescence under ultraviolet radiation.
Coal tar, which contains around 1.5% anthracene, remains a major source of this material. Common impurities are phenanthrene and carbazole. The mineral form of anthracene is called freitalite and is related to a coal deposit. A classic laboratory method for the preparation of anthracene is by cyclodehydration of o-methyl- or o-methylene-substituted diarylketones in the so-called Elbs reaction.
Reduction of anthracene with alkali metals yields the deeply colored radical anion salts M+[anthracene]− (M = Li, Na, K). Hydrogenation gives 9,10-dihydroanthracene, preserving the aromaticity of the two flanking rings.
The dimer, called dianthracene (or sometimes paranthracene), is connected by a pair of new carbon-carbon bonds, the result of the [4+4] cycloaddition. It reverts to anthracene thermally or with UV irradiation below 300 nm. Substituted anthracene derivatives behave similarly. The reaction is affected by the presence of oxygen.
Electrophilic substitution of anthracene occurs at the 9 position. For example, formylation affords 9-anthracenecarboxaldehyde. Substitution at other positions is effected indirectly, for example starting with anthroquinone. Bromination of anthracene gives 9,10-dibromoanthracene.
Anthracene, a wide band-gap organic semiconductor is used as a scintillator for detectors of high energy photons, electrons and alpha particles. Plastics, such as polyvinyltoluene, can be doped with anthracene to produce a plastic scintillator that is approximately water-equivalent for use in radiation therapy dosimetry. Anthracene's emission spectrum peaks at between 400 nm and 440 nm.
Anthracene is commonly used as a UV tracer in conformal coatings applied to printed wiring boards. The anthracene tracer allows the conformal coating to be inspected under UV light. Anthracene also used in manufacturing of anthraquinone.
A variety of anthracene derivatives find specialized uses. Derivatives having a hydroxyl group are 1-hydroxyanthracene and 2-hydroxyanthracene, homologous to phenol and naphthols, and hydroxyanthracene (also called anthrol, and anthracenol) are pharmacologically active. Anthracene may also be found with multiple hydroxyl groups, as in 9,10-dihydroxyanthracene.
Anthracene, as many other polycyclic aromatic hydrocarbons, is generated during combustion processes. Exposure to humans happens mainly through tobacco smoke and ingestion of food contaminated with combustion products.
Many investigations indicate that anthracene is noncarcinogenic: "consistently negative findings in numerous in vitro and in vivo genotoxicity tests". Early experiments suggested otherwise because crude samples were contaminated with other polycyclic aromatic compounds. Furthermore, it is readily biodegraded in soil. It is especially susceptible to degradation in the presence of light.
|Wikimedia Commons has media related to Anthracenes.|
|Wikisource has the text of the 1879 American Cyclopædia article Anthracene.|