Anthracene
| Anthracene[1] | |
|---|---|
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| IUPAC name | Anthracene |
| Identifiers | |
| CAS number | |
| SMILES | C12=CC=CC=C1C=C3C(C=CC=C3)=C2 |
| Properties | |
| Molecular formula | C14H10 |
| Molar mass | 178.23 g/mol |
| Appearance | Light Brown |
| 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 | Irritant Dangerous for the Environment |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references | |
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Editor-In-Chief: C. Michael Gibson, M.S., M.D. [1]
Overview
Anthracene is a solid polycyclic aromatic hydrocarbon consisting of three fused benzene rings derived from coal-tar. Anthracene is used in the artificial production of the red dye alizarin. It is also used in wood preservatives, insecticides, and coating materials. Anthracene is colorless but exhibits a blue (400-500 nm peak) fluorescence under ultraviolet light.
Synthesis
A classic method for the preparation of anthracene in the laboratory is by cyclodehydration of o-methyl- or o-methylene-substituted diarylketones in the so-called Elbs reaction (named for the German chemist Karl Elbs).
Reactions
Anthracene has the ability to photodimerize with irradiation by UV light. This results in considerable changes in the physical properties of the material.
The dimer is connected by two covalent bonds resulting from the [4+4] cycloaddition. The dimer reverts to anthracene thermally or with UV irradiation below 300 nm. The reversible bonding and photochromic properties of anthracenes is the basis of many potential applications using poly and monosubstituted anthracene derivatives. The reaction is sensitive to oxygen.
In most other reactions of anthracene, the central ring is also targeted, as it is the most highly reactive. Electrophilic substitution occurs at the "9" and "10" positions of the center ring, and oxidation of anthracene occurs readily, giving anthraquinone, C14H8O2 (below).
Uses
Anthracene can also have a hydroxyl group to form 1-hydroxyanthracene and 2-hydroxyanthracene, homologous to phenol and napthol, and hydroxyanthracene is also called anthrol, and anthracenol.[2][3] Hydroxyanthracene derivatives are pharmacologically active, and are contained in aloe for example.[4][5]
Anthracene is an organic semiconductor.
Anthracene is used as a scintillator for detectors of high energy photons, electrons and alpha particles. Plastics such as polyvinyltolulene can be doped with Anthracene to produce a plastic scintillator that is approximately water equivalent for use in radiation therapy dosimetry. Anthracenes emission spectrum peaks at between 400 nm and 440 nm.
See also
References
- ↑ NIST Chemistry WebBook Anthracene
- ↑ 1-Hydroxyanthracene NIST datapage
- ↑ 2-Hydroxyanthracene NIST datapage
- ↑ TGA News
- ↑ Herbals and Breastfeeding
External links
- IARC Monograph "Anthracene."
- National Pollutant Inventory - Polycyclic Aromatic Hydrocarbon Fact Sheet
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