anthracene

Anthracene[1]
IUPAC name Anthracene
Identifiers
CAS number	120-12-7 Y
PubChem	8418
ChemSpider	8111 Y
UNII	EH46A1TLD7 Y
DrugBank	DB07372
KEGG	C14315 Y
ChEBI	CHEBI:35298 Y
ChEMBL	CHEMBL333179 Y
Jmol-3D images	Image 1 Image 2
SMILES c3ccc2cc1ccccc1cc2c3 c1ccc2cc3ccccc3cc2c1
InChI InChI=1S/C14H10/c1-2-6-12-10-14-8-4-3-7-13(14)9-11(12)5-1/h1-10H Y Key: MWPLVEDNUUSJAV-UHFFFAOYSA-N Y InChI=1/C14H10/c1-2-6-12-10-14-8-4-3-7-13(14)9-11(12)5-1/h1-10H Key: MWPLVEDNUUSJAV-UHFFFAOYAK
Properties
Molecular formula	C14H10
Molar mass	178.23 g mol−1
Appearance	Colorless
Density	1.25 g/cm³ at 19.85 °C, Solid 0.969 g/cm³ at 220 °C, liquid
Melting point	218 °C, 491 K, 424 °F
Boiling point	340 °C, 613 K, 644 °F
Solubility in other solvents	Water: none Methanol: 0.908g per liter Hexane: 1.64g per liter
Hazards
EU classification	Dangerous for the Environment
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Anthracene is a solid polycyclic aromatic hydrocarbon 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 light.

In 2010, a strong absorption band of anthracene was observed along a line of sight to a star in the open cluster IC 348, and this may be associated with an intervening molecular cloud.^[2]

Production

Commercial anthracene is obtained from coal tar, common impurities being phenanthrene and carbazole. 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.

Reactions

Anthracene photodimerizes by the action of UV light:

The dimer is connected by a pair of new carbon-carbon bonds, the result of the [4+4] cycloaddition. The dimer reverts to anthracene thermally or with UV irradiation below 300 nm. The reversible dimerization and the photochromic properties of anthracenes are the basis of potential applications. Substituted anthracene derivatives behave similarly. The reaction is affected by the presence of oxygen.

In general, reduction of anthracene yields 9,10-dihydroanthracene (destroying the aromaticity of the center ring) rather than 1,4-dihydroanthracene (which would destroy the aromaticity of one of the terminal rings). This preference for reduction at the 9 and 10 positions is explained by the fact that aromatic stabilization energy is directly correlated with the number of conjugated pi bonds in an aromatic system. Since 9,10-dihydroanthracene in essence preserves two "benzene" rings (a total of 6 conjugated pi bonds), whereas the 1,4-isomer preserves only one and a half such rings (a total of 5 pi bonds); the latter is not the thermodynamically favorable product. Likewise, electrophilic substitution occurs at the "9" and "10" positions of the center ring.

Oxidation occurs readily, giving anthraquinone, C₁₄H₈O₂ (below), for example using hydrogen peroxide and vanadyl acetylacetonate. ^[3]

Uses

Anthracene is converted mainly to anthroquinone, a precursor to dyes.^[4]

Anthracene is an organic semiconductor. It 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.

It is also used in wood preservatives, insecticides, and coating materials.^{[citation needed]}

Derivatives

A variety of anthracene derivatives find niche uses. Derivatives having a hydroxyl group are 1-hydroxyanthracene and 2-hydroxyanthracene, homologous to phenol and naphthols, and hydroxyanthracene (also called anthrol, and anthracenol)^[5][6] are pharmacologically active. Anthracene may also be found with multiple hydroxyl groups, as in 9,10-dihydroxyanthracene.

Toxicology

Like many other polycyclic aromatic hydrocarbons (PAH), anthracene is carcinogenic as listed by OSHA^[7]. Anthracene, as many other PAHs, is generated during combustion processes: Exposure to humans happens mainly through tobacco smoke and ingestion of food contaminated with combustion products [2].

See also

• Phenanthrene
• Tetracene
• 9,10-Dithioanthracene, which migrates in a straight line when adsorbed on a flat copper surface.

References

External links

• International Chemical Safety Card 0825
• IARC - Monograph 32
• National Pollutant Inventory - Polycyclic Aromatic Hydrocarbon Fact Sheet
• European Chemicals Agency - ECHA