Polycarbonyl

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Polycarbonyl, (also known as polymeric-CO, p-CO or poly-CO) is a solid, metastable, and explosive polymer of carbon monoxide.[1] The polymer is produced by exposing carbon monoxide to high pressures. The structure of the solid appears amorphous, but may include a zigzag of equally-spaced CO groups.[2]

Formation[edit]

Poly-CO can be produced at pressures of 5.2 GPa; it is amorphous and yellow to dark red in color.[3] Polymerisation is catalysed by blue light at slightly lower pressures in the δでるた-phase of solid CO.[4] Another white, crystalline phase can be made at higher temperatures at 6 or 7 GPa.[1]

R. J. Mills discovered this solid, which was first produced in a tungsten carbide anvil in 1947. Originally this was thought to be polymeric carbon suboxide, but the formation does not yield any gas byproduct such as carbon dioxide.[5] The yield of the solid can be up to 95%.[6]

Properties[edit]

The polymer is stable above about 80 K. Below this temperature the εいぷしろん form of solid molecular CO is formed instead. When the pressure is released the polymer remains stable at atmospheric pressure. The solid dissolves in water, alcohol and acetone.[5] When exposed to the atmosphere it is hygroscopic, becomes gluey, and changes colour, becoming darker.[6] The reaction with water produces carboxylic groups.[7][8]

The solid stores a high energy. It can decompose explosively forming glassy carbon and carbon dioxide.[6] The energy density stored can be up to 8 kJ/g. During the decomposition the temperature can be 2500 K.[6] The density is 1.65 g/cm3, however most of the solid produced is porous, so the true density is likely to be higher.[6]

Infrared spectroscopy shows bands at 650, 1210, 1440, 1650 and 1760 cm−1. The 1760 band is likely to be due to the -C-(C=O)-C- structure.[4] The 1600 is due to vibration of a C=C double bond.[6]

The solid is electrically insulating with an electronic gap energy of 1.9 eV.[4]

Nuclear magnetic resonance for the material made from 13CO shows sharp resonance at 223 ppm due to ester or lactone attached carbon, and 151 ppm due to C=C double bonds. There is also broad resonance at 109 and 189 ppm. Over time of a few days, the 223 ppm peak reduces and all the other features increase in strength.[6]

Structure[edit]

Ideas of the structure include a zigzag chain of CO pointing in opposite directions, or five atom rings connected by CO and C−C bonds. The rings are lactones of tetronic acid: −C:−(C=O)−(C−O−)−(C=O)−O−. Interconnections between the rings are zigzags of CO.[4]

Other ideas of the structure of the solid, include graphitic carbon with carbon dioxide under pressure, and a polymer with this C3O2 monomer: −(C=O)−O−(C−)=C<. Yet other ideas are that the solid is the same as the polymer of carbon suboxide with oxalic anhydride.[9]

References[edit]

  1. ^ a b Rademacher, N.; L. Bayarjargal; W. Morgenroth; B. Winkler; J. Ciezak-Jenkins (2011). "Preparation and characterization of solid carbon monoxide at high pressure in the diamond anvil cell" (PDF). Retrieved 30 May 2013.
  2. ^ Podeszwa, Rafał; Rodney J. Bartlett (2003). "Crystal orbital study of polycarbonyl". International Journal of Quantum Chemistry. 95 (4–5): 638–642. doi:10.1002/qua.10655. ISSN 0020-7608.
  3. ^ Rademacher, Nadine; Lkhamsuren Bayarjargal; Wolfgang Morgenroth; Jennifer Ciezak-Jenkins; Sasha Batyrev; Björn Winkler. "High Pressure Investigations of Liquid and Polymerized CO up to 20 GPa Using Pair Distribution Function Analysis" (PDF). Retrieved 30 May 2013.
  4. ^ a b c d Bernard, Stephane (Feb 1998). "DECOMPOSITION AND POLYMERIZATION OF SOLID CARBON MONOXIDE UNDER PRESSURE" (PDF). Trieste. Retrieved 30 May 2013.
  5. ^ a b Mills, R. L.; D. Schiferl; A. I. Katz; B. W. Olinger (1984). "New Phases and Chemical Reactions in Solid Co Under Pressure" (PDF). Le Journal de Physique Colloques. 45 (C8): C8–187–C8–190. doi:10.1051/jphyscol:1984833. ISSN 0449-1947.
  6. ^ a b c d e f g Lipp, Magnus J.; William J. Evans, Bruce J. Baer, Choong-Shik Yoo; Baer, Bruce J.; Yoo, Choong-Shik (2005). "High-energy-density extended CO solid" (PDF). Nature Materials. 4 (3): 211–215. Bibcode:2005NatMa...4..211L. doi:10.1038/nmat1321. ISSN 1476-1122. PMID 15711555. S2CID 25779399.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  7. ^ Ceppatelli, Matteo; Anton Serdyukov; Roberto Bini; Hans J. Jodl (2009). "Pressure Induced Reactivity of Solid CO by FTIR Studies". The Journal of Physical Chemistry B. 113 (19): 6652–6660. doi:10.1021/jp900586a. ISSN 1520-6106. PMID 19368397.
  8. ^ Katz, Allen I.; David Schiferl; Robert L. Mills (1984). "New phases and chemical reactions in solid carbon monoxide under pressure". The Journal of Physical Chemistry. 88 (15): 3176–3179. doi:10.1021/j150659a007. ISSN 0022-3654.
  9. ^ Lipp, M.; W. J. Evans; V. Garcia-Baonza; H. E. Lorenzana (1998). "Carbon Monoxide: Spectroscopic Characterization of the High–Pressure Polymerized Phase". Journal of Low Temperature Physics. 111 (3/4): 247–256. Bibcode:1998JLTP..111..247L. doi:10.1023/A:1022267115640. ISSN 0022-2291. S2CID 116687814.

Other reading[edit]

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