Polycarbonyl
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-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 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]- ^ 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.
- ^ 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.
- ^ 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.
- ^ a b c d Bernard, Stephane (Feb 1998). "DECOMPOSITION AND POLYMERIZATION OF SOLID CARBON MONOXIDE UNDER PRESSURE" (PDF). Trieste. Retrieved 30 May 2013.
- ^ 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.
- ^ 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) - ^ 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.
- ^ 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.
- ^ 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]- Batyrev, I. G.; W. D. Mattson; B. M. Rice (2012). "Modeling of Early Stages of Formation of Poly-CO". MRS Proceedings. 1405. doi:10.1557/opl.2012.345. ISSN 1946-4274.
- Sun, Jian; Dennis D. Klug; Chris J. Pickard; Richard J. Needs (2011). "Controlling the Bonding and Band Gaps of Solid Carbon Monoxide with Pressure" (PDF). Physical Review Letters. 106 (14): 145502. Bibcode:2011PhRvL.106n5502S. doi:10.1103/PhysRevLett.106.145502. ISSN 0031-9007. PMID 21561202. S2CID 19591866.