Polyacetylene

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This article is about polymers with alternating double and single bonds. For compounds with multiple triple bonds, see polyyne.
Polyacetylene
trans-Polyacetylen
cis-Polyacetylen
Identifiers
CAS number 25067-58-7 N
Properties
Molecular formula [C2H2]n
Solubility in water insoluble
Hazards
R-phrases R10
S-phrases
Related compounds
Related compounds Ethyne (monomer)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Polyacetylene (IUPAC name: polyethyne) is an organic polymer with the repeating unit (C2H2)n. It is an important polymer, as the discovery of polyacetylene and its high conductivity upon doping helped to launch the field of organic conductive polymers. The high electrical conductivity discovered by Hideki Shirakawa, Alan Heeger, and Alan MacDiarmid for this polymer led to intense interest in the use of organic compounds in microelectronics (organic semiconductors). This discovery was recognized by the Nobel Prize in Chemistry in 2000.[1][2] Early work in the field of polyacetylene research was aimed at using doped polymers as easily processable and lightweight "plastic metals." [3] Despite the promise of this polymer in the field of conductive polymers, many of its properties such as instability to air and difficulty with processing have led to avoidance in its application to large scale use in many consumer goods.

Structure[edit]

A segment of trans-polyacetylene

Structural diagram
Ball-and-stick model

Polyacetylene consists of a long chain of carbon atoms with alternating single and double bonds between them, each with one hydrogen atom. The double bonds can have either cis or trans geometry. The controlled synthesis of each isomer of the polymer, cis-polyacetylene or trans-polyacetylene, can be achieved by changing the temperature at which the reaction is conducted. The cis form of the polymer is thermodynamically less stable than the trans isomer. Despite the conjugated nature of the polyacetylene backbone, not all of the carbon–carbon bonds in the material are equal: a distinct single/double alternation exists.[4] Each hydrogen atom can be replaced by a functional group. Substituted polyacetylenes tend to be more rigid than saturated polymers.[3] Furthermore, placing different functional groups as substituents on the polymer backbone leads to bending of the polymer chain out of conjugation.

History[edit]

Cuprene was one of the earliest reported acetylene polymers. Its highly cross-linked nature led to no further studies in the field for quite some time.[5] Linear polyacetylene was first prepared by Giulio Natta in 1958.[6] The resulting polyacetylene was linear, of high molecular weight, displayed high crystallinity, and had a regular structure. X-ray diffraction studies demonstrated that the resulting polyacetylene was trans-polyacetylene.[6] After this first reported synthesis, few chemists were interested in polyacetylene because the product of Natta’s preparation was an insoluble, air sensitive, and infusible black powder.

The next major development of polyacetylene polymerization was made by Hideki Shirakawa’s group who were able to prepare silvery films of polyacetylene. They discovered that the polymerization of polyacetylene could be achieved at the surface of a concentrated solution of the catalyst system of Et3Al and Ti(OBu)4 in an inert solvent such as toluene.[4] In parallel with Shirakawais studies, Alan Heeger, and Alan MacDiarmid were studying the metallic properties of polythiazyl [(SN)x], a related but inorganic polymer.[7] Polythiazyl caught his interest as a chain-like metallic material, and he collaborated with Alan MacDiarmid who had previous experience with this material. By the early 1970s, this polymer was known to be superconductive at low temperatures.[7] Shirakawa, Heeger, and MacDiarmid collaborated on further development of polyacetylene.[6]

Upon doping polyacetylene with I2, the conductivity increased seven orders of magnitude.[4] Similar results using Cl2 and Br2. These materials exhibited the largest room temperature conductivity observed for a covalent organic polymer, and this seminal report was key in furthering the development of organic conductive polymers.[8] Further studies led to improved control the cis/trans isomer ratio and demonstrated that cis-polyacetylene doping led to higher conductivity than doping of trans-polyacetylene.[4] Doping cis-polyacetylene with AsF5 further increased the conductivities, bringing them close to that of copper. Furthermore, it was found that heat treatment of the catalyst used for polymerization led to films with higher conductivities.[9]

Synthesis[edit]

From acetylene[edit]

Ziegler-Natta scheme

A variety of methods have been developed to synthesize polyacetylene, from pure acetylene as well as other monomers. One of the most common methods uses titanium and aluminum catalysts, known as Ziegler-Natta catalysts, with gaseous acetylene. This method allows control over the structure and properties of the final polymer by varying temperature and catalyst loading.[10] Mechanistic studies suggest that this polymerization involves metal-insertion into the triple bond of the monomer.[11]

Insertion mechanism for polyacetylene

By varying the apparatus and catalyst loading, Shirakawa and coworkers were able to synthesize polyacetylene as thin films, rather than insoluble black powders. They obtained these films by coating the walls of a reaction flask under inert conditions with a solution of the Ziegler-Natta catalyst and adding gaseous acetylene, resulting in immediate formation of a film.[12] Enkelmann and coworkers further improved polyacetylene synthesis by changing the catalyst to a CoNO3/NaBH4 system, which was stable to both oxygen and water.[5]

Polyacetylene can also be produced by radiation polymerization of acetylene. Glow discharge radiation, γ-radiation, and ultraviolet irradiation have been used. These methods avoid the use of catalysts and solvent, but they require low temperatures to produce regular polymers. Gas-phase polymerization typically produces irregular cuprene, whereas liquid-phase polymerization, conducted at −78 °C produces linear cis-polyacetylene and solid phase polymerization, conducted at still lower temperature produces trans-polyacetylene.[6]

Ring-opening metathesis polymerization[edit]

Polyacetylene can be synthesized by ring-opening metathesis polymerization (ROMP) from cyclooctatetraene, a material easier to handle than the acetylene monomer. This synthetic route also provides a facile method for adding solubilizing groups to the polymer while maintaining the conjugation.[3] Robert Grubbs and coworkers synthesized a variety of polyacetylene derivatives with linear and branched alkyl chains. Polymers with linear groups such as n-octyl had high conductivity but low solubility, while highly branched tert-butyl groups increased solubility but decreased conjugation due to polymer twisting to avoid steric crowding. They obtained soluble and conductive polymers with sec-butyl and neopentyl groups, because the methylene (CH2) unit directly connected to the polymer reduces steric crowding and prevents twisting.[3]

Grubbs route to polyacetylene

From precursor polymers[edit]

Dehydrohalogenation route to polyacetylene

Polyacetylene can also be synthesized from precursor polymers. This method enables processing of the polymer before conversion to insoluble polyacetylene. Short, irregular segments of polyacetylene can be obtained by dehydrohalogenation of poly(vinyl chloride).[13] Thermal conversion of precursor polymers is a more effective method for synthesizing long polyacetylene chains. In the Durham-precursor route, polymers are prepared via ring-opening metathesis polymerization, and a subsequent heat-induced reverse Diels-Alder reaction yields the final polymer, as well as a volatile side product.[5]

Durham precursor polymer route to polyacetylene

Doping[edit]

When polyacetylene films are exposed to vapors of electron-accepting compounds (p-type dopants), the electrical conductivity of the material increases by orders of magnitude over the undoped material.[14] p-type dopants include Br2, I2, Cl2, and AsF5. These dopants act by abstracting an electron from the polymer chain. The conductivity of these polymers is believed to be a result of the creation of charge-transfer complexes between the polymer and halogen.[8] Charge-transfer occurs from the polymer to the acceptor compound; the polyacetylene chain acts as a cation and the acceptor as an anion. The “hole” on the polymer backbone is weakly associated with the anionic acceptor by Coulomb potential.[14] Polyacetylene doped with (p-type) dopants retain their high conductivity even after exposure to air for several days.[6]

Electron-donating (n-type) dopants can also be used to create conductive polyacetylene. n-Type dopants for polyacetylene include lithium, sodium, and potassium.[6] As with p-type dopants, charge-transfer complexes are created, where the polymer backbone is anionic and the donor is cationic. The increase in conductivity upon treatment with an n-type dopant is not as significant as those achieved upon treatment with a p-type dopant. Polyacetylene chains doped with n-type dopants are extremely sensitive to air and moisture.[6]

The conductivity of polyacetylene varies depending on structure and doping. Undoped trans-polyacetylene films have a conductivity of 4.4×10−5 Ω−1cm−1, while cis-polyacetylene has a lower conductivity of 1.7×10−9 Ω−1cm−1 Doping with bromine causes an increase in conductivity to 0.5 Ω−1cm−1, while a higher conductivity of 38 Ω−1cm−1 is obtained through doping with iodine.[8] Doping of either cis- or trans-polyacetylene leads to an increase in their conductivities. Doped cis-polyacetylene films usually have conductivities two or three times greater than doped trans-polyacetylene even though the parent film has lower conductivity.[15]

Properties[edit]

The structure of polyacetylene films have been examined by both infrared[16] and Raman[17] spectroscopy, and found that structure depends on synthetic conditions. When the synthesis is performed below −78 °C, the cis form predominates, while above 150 °C the trans form is favored. At room temperature, the polymerization yields a ratio of 60:40 cis:trans.[15] Films containing the cis form appear coppery, while the trans form is silvery.[15] Films of cis-polyacetylene are very flexible and can be readily stretched, while trans-polyacetylene is much more brittle.

The synthesis and processing of polyacetylene films affects the properties. Increasing the catalyst ratio creates thicker films with a greater draw ratio, allowing them to be stretched further.[6] Lower catalyst loadings leads to the formation of dark red gels, which can be converted to films by cutting and pressing between glass plates.[15] A foam-like material can be obtained from the gel by displacing the solvent with benzene, then freezing and subliming the benzene.[6] Polyacetylene has a bulk density of 0.4 g/cm3, while density of the foam is significantly lower, at 0.02–0.04 g/cm3.[6] The morphology consists of fibrils, with an average width of 200 Ǻ. These fibrils form an irregular, web-like network, with some cross-linking between chains.[6] The insolubility of polyacetylene makes it difficult to characterize this material and to determine the extent of cross-linking in the material.

Products of oxidation of polyacetylene

Applications[edit]

Polyacetylene has no commercial applications, although the discovery of polyacetylene as a conductive organic polymer led to many developments in materials science. Conducting polymers are of interest for low-cost solution-processing for film-forming polymers.[4] Therefore, much attention in recent years has shifted to other conductive polymers for application purposes, e.g. polythiophene and polyaniline.

Polyacetylenes suffer from many drawbacks including instability in air and insolubility in solvents making it essentially impossible to process the material. While both cis and trans-polyacetylene show high thermal stability,[15] exposure to air causes a large decrease in the flexibility and conductivity.[6] When polyacetylene is exposed to air, oxidation of the backbone by O2 occurs. Infrared spectroscopy shows formation of carbonyl groups, epoxides, and peroxides.[6][18] Coating with polyethylene or wax can slow the oxidation temporarily, while coating with glass increases stability indefinitely.[6]

References[edit]

  1. ^ Heeger, Alan (2001). "Nobel Lecture: Semiconducting and metallic polymers: The fourth generation of polymeric materials". Reviews of Modern Physics (free download) 73 (3): 681. Bibcode:2001RvMP...73..681H. doi:10.1103/RevModPhys.73.681. 
  2. ^ "The Nobel Prize in Chemistry 2000". 
  3. ^ a b c d Gorman, C.B; Ginsburg, E.J.; Grubbs, R.H (1993). "Soluble, Highly Conjugated Derivatives of Polyacetylene from the Ring-Opening Metathesis Polymerization of Monosubstituted Cyclooctratetraenes: Synthesis and the Relationship between Polymer Structure and Physical Properties". Journal of the American Chemical Society 115 (4): 1397–1409. doi:10.1021/ja00057a024. 
  4. ^ a b c d e Norden, B; Krutmeijer, E. The Nobel Prize in Chemistry, 2000: Conductive Polymers. 
  5. ^ a b c Feast, W.J.; Tsibouklis, J.; Pouwer, K.L.; Groenendaal, L.; Meijer, E.W. (1996). "Synthesis, processing and material properties of conjugated polymers". Polymer 37 (22): 5017. doi:10.1016/0032-3861(96)00439-9. 
  6. ^ a b c d e f g h i j k l m n Saxon, A.M.; Liepins, F.; Aldissi, M. (1985). "Polyacetylene: Its Synthesis, Doping, and Structure". Prog. Polym. Sci. 11: 57. doi:10.1016/0079-6700(85)90008-5. 
  7. ^ a b Hall, N; McDiarmid, Alan; Heeger, Alan (2003). "Twenty-five years of conducting polymers". Chem. Comm.: 1–4. doi:10.1039/B210718J. 
  8. ^ a b c Shirakawa, H.; Louis, E.J.; MacDiarmid, A.G.; Chiang, C.K.; Heeger, A.J. (1977). "Synthesis of Electrically Conducting Organic Polymers: Halogen Derivatives of Polyacetylene, (CH)x". J.C.S. Chem. Comm. (16): 578–580. doi:10.1039/C39770000578. 
  9. ^ Shirakawa, Hideki (1995). "Synthesis and characterization of highly conducting polyacetylene". Synthetic Metals 69: 3. doi:10.1016/0379-6779(94)02340-5. 
  10. ^ Feast, W.J; Tsibouklis, J.; Pouwer, K.L.; Groenendaal, L.; Meijer, E.W (1996). "Synthesis, processing and material properties of conjugated polymers". Polymer 37 (22): 5017–5047. doi:10.1016/0032-3861(96)00439-9. 
  11. ^ Clarke, T.C.; Yannoni, T.S.; Katz, T.J (1983). "Mechanism of Ziegler-Natta Polymerization of Acetylene: A Nutation NMR Study". Journal of the American Chemical Society 105 (26): 7787–7789. doi:10.1021/ja00364a076. 
  12. ^ Ito, T; Shirakawa, H., S. Ikeda, S (1974). "Simultaneous Polymerization and Formation of Polyacetylene Film on the Surface of Concentrated Soluble Ziegler-Type Catalyst Solution". J. Polymer Science Part A 12 (13): 11–20. Bibcode:1996JPoSA..34.2533I. doi:10.1002/pola.1996.854. 
  13. ^ "Conducting Polymers". ch.ic.ac.uk. 
  14. ^ a b Chiang, C.K.; Gau, S.C.; Fincher, C.R.; Park, Y.W.; MacDiarmid, A.G.; Heeger, A.J. (1978). "Polyacetylene, (CH)x: n-type and p-type doping and compensation". Appl. Phys. Lett. 33: 18. Bibcode:1978ApPhL..33...18C. doi:10.1063/1.90166. 
  15. ^ a b c d e MacDiarmid, A; Heeger, A. (1979). "Organic Metals and Semiconductors: The Chemistry of Polyacetylene (CHx) and its Derivatives". Synthetic Metals 1 (101–118): 101. doi:10.1016/0379-6779(80)90002-8. 
  16. ^ Shirakawa, H.S.; Ito, T. S. Ikeda, S (1971). "Infrared Spectroscopy of Poly(acetylene)". Polymer J. 2 (2): 231–244. doi:10.1295/polymj.2.231. 
  17. ^ Shirakawa, H.S.; Ito, T. S. Ikeda, S. (1973). "Raman Scattering and Electronic Spectra of Poly(acetylene)". Polymer J 4 (4): 460–462. doi:10.1295/polymj.4.460. 
  18. ^ Will, F.G.; D.W. McKee (1983). "Thermal Oxidation of Polyacetylene". Journal of Polymer Science 21 (12): 3479–3492. Bibcode:1983JPoSA..21.3479W. doi:10.1002/pol.1983.170211210. 

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