1.1.1-Propellane

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The correct title of this article is [1.1.1]Propellane. The omission of any brackets is due to technical restrictions.
[1.1.1]Propellane
1.1.1-propellane.svg
1.1.1-propellane.png
Names
Preferred IUPAC name
Tricyclo[1.1.1.01,3]pentane
Identifiers
3D model (JSmol)
ChemSpider
PubChem CID
  • InChI=1S/C5H6/c1-4-2-5(1,4)3-4/h1-3H2 Yes check.svgY
    Key: ZTXSPLGEGCABFL-UHFFFAOYSA-N Yes check.svgY
  • C1(C2)(C3)C23C1
Properties
C5H6
Molar mass 66.103 g·mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

[1.1.1]Propellane is an organic compound, the simplest member of the propellane family. It is a hydrocarbon with formula C5H6 or C2(CH2)3. The molecular structure consists of three rings of three carbon atoms each, sharing one C–C bond.

Contents

[1.1.1]Propellane is a highly strained molecule. The bonds of the two central carbon atoms have an inverted tetrahedral geometry, and the length of the central bond is 160 pm. The strength of that bond is disputed; estimates vary from 59–65  kcal/mol to no strength at all. The energy of the biradical state (with no central bond at all) is calculated to be 80 kcal/mol higher. At 114 °C it will spontaneously isomerize to 3-methylidenecyclobutene (5 below) with a half-life of 5 minutes. Its strain energy is estimated to be 102 kcal/mol (427  kJ/mol). Surprisingly, [1.1.1]propellane is persistent at room temperature and is somewhat less susceptible to thermal decomposition than the less strained (90 kcal/mol) [2.2.2]propellane system, which has an estimated half-life of only about 1 h at 25 °C. [1] This unusual stability is attributed to delocalisation of electron density from the bond between the central carbon atoms onto the bridging carbon atoms. [2]

The type of bonding in this molecule has been explained in terms of charge-shift bonding. [3]

Synthesis

[1.1.1]Propellane was first reported by Kenneth B. Wiberg and F. Walker in 1982. The synthesis commences with cyclopropanation of 1,1-bis(chloromethyl)ethylene, [4] according to the following scheme:

Scheme 1. Synthesis of [1.1.1]propellane 111propellaneSynthesis.png
Scheme 1. Synthesis of [1.1.1]propellane

Synthesis begins with conversion of the 1,3-di-carboxylic acid of bicyclo[1.1.1]pentane 1 in a Hunsdiecker reaction to the corresponding dibromide 2 followed by a coupling reaction with n-butyllithium. The final product 3 was isolated by column chromatography at −30 °C.

However, a much simplified synthesis was published by Szeimies. [5] It starts with dibromocarbene addition to the alkene bond of 3-chloro-2-(chloromethyl)propene 6 followed by deprotonation by methyllithium and nucleophilic displacements in 7. [6] The product was not isolated but kept in solution at −196 °C.

Reactions

Acetic acid addition

[1.1.1]Propellane spontaneously reacts with acetic acid to yield a methylidenecyclobutane ester (4 above).

Polymerization

[1.1.1]Propellane undergoes a polymerization reaction where the central C–C bond is split and connected to adjacent monomer units, resulting in staffanes. [7]

Scheme 2. Synthesis of [n]staffane Staffanes.png
Scheme 2. Synthesis of [n]staffane

A radical polymerization initiated by methyl formate and benzoyl peroxide results in a distribution of oligomers. An anionic addition polymerization with n-butyllithium results in a fully polymerized product. X-ray diffraction of the polymer shows that the connecting C–C bonds have bond lengths of only 1.48 Å, significantly shorter than the normal 1.54 Å.

The compound 1,3-dehydroadamantane, which can be viewed as a bridged [1.3.3]propellane, also polymerizes in a similar way.

See also

Related Research Articles

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References

  1. ↑ "Houben-Weyl Methods of Organic Chemistry Vol. E 17e, 4th Edition Supplement (E-Book PDF) - Thieme.de - Thieme Webshop - Armin de Meijere, Holger Butenschön, Hak-Fun Chow, Lutz Fitjer, Günter Haufe". Thieme Webshop (in German). Archived from the original on October 22, 2017. Retrieved 2017-10-21.
  2. ↑ Sterling, Alistair J.; Dürr, Alexander; Smith, Russell; Anderson, Edward Alexander; Duarte, Fernanda (2020-04-13). "Rationalizing the diverse reactivity of [1.1.1]propellane through sigma-pi-delocalization". Chemical Science. 11 (19): 4895–4903. doi: 10.1039/D0SC01386B . ISSN   2041-6539. PMC   8159217 . PMID   34122945.
  3. ↑ Wu, Wei; Gu, Junjing; Song, Jinshuai; Shaik, Sason; Hiberty, Philippe C. (2009). "The Inverted Bond in [1.1.1]Propellane is a Charge-Shift Bond". Angew. Chem. Int. Ed. 48 (8): 1407–1410. doi: 10.1002/anie.200804965 . PMID   19072971.
  4. ↑ Wiberg, K. B.; Walker, F. H. (1982). "[1.1.1]Propellane". J. Am. Chem. Soc. 104 (19): 5239–5240. doi:10.1021/ja00383a046.
  5. ↑ Belzner, Johannes; Bunz, Uwe; Semmler, Klaus; Szeimies, Günter; Opitz, Klaus; Schlüter, Arnulf-Dieter; et al. (1989). "Concerning the synthesis of [1.1.1]propellane". Chem. Ber. 122 (2): 397–398. doi:10.1002/cber.19891220233.
  6. ↑ Mondanaro, Kathleen R.; Dailey, William P. "[1.1.1]Propellane". Organic Syntheses . 75: 98; Collected Volumes, vol. 10.
  7. ↑ Kaszynski, Piotr; Michl, Josef (1988). "[n]Staffanes: a molecular-size "Tinkertoy" construction set for nanotechnology. Preparation of end-functionalized telomers and a polymer of [1.1.1]propellane". J. Am. Chem. Soc. 110 (15): 5225–5226. doi:10.1021/ja00223a070.
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