PRISMANE
650-42-0 cas
Tetracyclo[2.2.0.02,6.03,5]hexane
Prismane is a polycyclic hydrocarbon with the formula C6H6. It is an isomer of benzene, specifically a valence isomer. Prismane is far less stable than benzene. The carbon (and hydrogen) atoms of the prismane molecule are arranged in the shape of a six-atomtriangular prism. Albert Ladenburg proposed this structure for the compound now known as benzene.[1] The compound was not synthesized until 1973.[2]
| Prismane | |||
|---|---|---|---|
| |||
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| Identifiers | |||
| CAS number | 650-42-0  | ||
| ChemSpider | 16736515  | ||
| Jmol-3D images | Image 1 | ||
| Properties | |||
| Molecular formula | C6H6 | ||
| Molar mass | 78.11 g mol−1 | ||
History
In the mid 19th century, investigators proposed several possible structures for benzene which were consistent with its empirical formula, C6H6, which had been determined by combustion analysis. The first, which was proposed by Kekulé in 1867, later proved to be closest to the true structure of benzene. This structure inspired several others to propose structures that were consistent with benzene's empirical formula; for example, Ladenburg proposed prismane, Dewar proposed Dewar benzene, and Koerner and Claus proposedClaus' benzene. Some of these structures would be synthesized in the following years. Prismane, like the other proposed structures for benzene, is still often cited in the literature, because it is part of the historical struggle toward understanding the mesomeric structures and resonance of benzene. Some computational chemists still research the differences between the possible isomers of C6H6.[3]
Properties
Prismane is a colourless liquid at room temperature. The deviation of the carbon-carbon bond angle from 109° to 60° in a triangle leads to a high ring strain, reminiscent of that of cyclopropane but greater. The compound is explosive, which is unusual for a hydrocarbon. Due to this ring strain, the bonds have a low bond energy and break at a low activation energy, which makes synthesis of the molecule difficult; Woodward and Hoffmann noted that prismane's thermal rearrangement to benzene is symmetry-forbidden, comparing it to "an angry tiger unable to break out of a paper cage."[4]
The substituted derivative hexamethylprismane (in which all six hydrogens are substituted by methyl groups) has a higher stability, and was synthesized by rearrangement reactionsin 1966.[5]
Synthesis
The synthesis starts from benzvalene (1) and 4-phenyltriazolidone, which is a strong dienophile. The reaction is a stepwise Diels-Alder like reaction, forming a carbocation as intermediate. The adduct (2) is then hydrolyzed under basic conditions and afterwards transformed into a copper(II) chloride derivative with acidic copper(II) chloride. Neutralized with a strong base, the azo compound (3) could be crystallized with 65% yield. The last step is a photolysis of the azo compound. This photolysis leads to a biradical which forms prismane (4) and nitrogen with a yield of less than 10%. The compound was isolated by preparative gas chromatography.
SYNTHESIS
MeLi, CH2Cl2,
Et2O
-45 °C, 45 %
Et2O
-45 °C, 45 %
+
Et2O, Dioxane
0 °C to RT, 60 min, 50-60 %
0 °C to RT, 60 min, 50-60 %
KOH,
MeOH, H2O
Reflux, 24 h
MeOH, H2O
Reflux, 24 h
CuCl2, HCl,
H2O
65 % (2 steps)
H2O
65 % (2 steps)
hν,
PhMe
30 °C, 5 h, 8 %
PhMe
30 °C, 5 h, 8 %
| References |
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http://chemistry.stackexchange.com/questions/8898/does-benzene-have-isomers-and-resonance-structures
References
- Ladenburg A. (1869). "Bemerkungen zur aromatischen Theorie". Chemische Berichte 2: 140–2. doi:10.1002/cber.18690020171.
- Katz T. J., Acton N. (1973). "Synthesis of Prismane". Journal of the American Chemical Society 95 (8): 2738–2739. doi:10.1021/ja00789a084.
- UD Priyakumar, TC Dinadayalane, GN Sastry (2002). "A computational study of the valence isomers of benzene and their group V hetero analogs". New J. Chem. 26 (3): 347–353.doi:10.1039/b109067d.
- R. B. Woodward and R. Hoffmann, Angew. Chem., Int. Ed. Engl., 8, 789, (1969)
- Lemal D. M., Lokensgard J. P. (1966). "Hexamethylprismane". Journal of the American Chemical Society 88 (24): pp 5934–5935. doi:10.1021/ja00976a046.
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