World Library  
Flag as Inappropriate
Email this Article

Solid oxygen

Article Id: WHEBN0002814939
Reproduction Date:

Title: Solid oxygen  
Author: World Heritage Encyclopedia
Language: English
Subject: Oxygen, Tetraoxygen, Allotropes of oxygen, A Pail of Air, Cryogenics
Collection: Cryogenics, Oxygen
Publisher: World Heritage Encyclopedia
Publication
Date:
 

Solid oxygen

Solid oxygen forms at normal atmospheric pressure at a temperature below 54.36 K (−218.79 °C, −361.82 °F). Solid oxygen O2, like liquid oxygen, is a clear substance with a light sky-blue color caused by absorption in the red part of the visible light spectrum.

Oxygen molecules have attracted attention because of the relationship between the molecular magnetization and crystal structures, electronic structures, and superconductivity. Oxygen is the only one of the simple diatomic molecules (and one of the few molecules in general) to carry a magnetic moment.[1] This makes solid oxygen particularly interesting, as it is considered a 'spin-controlled' crystal[1] that displays antiferromagnetic magnetic order in the low temperature phases. For papers dealing with the magnetic properties of solid oxygen we refer to magnetisation of condensed oxygen under high pressures and in strong magnetic fields by R.J. Meier, C.J. Schinkel and A. de Visser, J. Phys. C15 (1982) 1015-1024, far infrared absorption dealing with the magnetic excitations or spinwaves in Meier R J, Colpa J H P and Sigg H 1984 J. Phys. C: Solid State Phys. 17 4501. At very high pressures, solid oxygen changes from an insulating to a metallic state;[2] and at very low temperatures, it even transforms to a superconducting state.[3] Structural investigations of solid oxygen began in the 1920s and, at present, six distinct crystallographic phases are established unambiguously.

The density of solid oxygen ranges from 21 cm3/mol in the α-phase, to 23.5 cm3/mol in the γ-phase.[4]

Contents

  • Phases 1
    • Red oxygen 1.1
    • Metallic oxygen 1.2
  • References 2

Phases

A total of six different phases of solid oxygen are known to exist:[1][5]

  1. α-phase: light blue — forms at 1 atm below 23.8 K, monoclinic crystal structure.
  2. β-phase: faint blue to pink — forms at 1 atm below 43.8 K, rhombohedral crystal structure, (at room temperature and high pressure begins transformation to tetraoxygen).
  3. γ-phase: faint blue - forms at 1 atm below 54.36 K, cubic crystal structure.
  4. δ-phase: orange — forms at room temperature by applying a pressure of 9 GPa
  5. ε-phase: dark-red to black — forms at room temperature at pressures greater than 10 GPa
  6. ζ-phase: metallic — forms at pressures greater than 96 GPa

It has been known that oxygen is solidified into a state called the β-phase at room temperature by applying pressure, and with further increasing pressure, the β-phase undergoes phase transitions to the δ-phase at 9 GPa and the ε-phase at 10 GPa; and, due to the increase in molecular interactions, the color of the β-phase changes to pink, orange, then red (the stable octaoxygen phase), and the red color further darkens to black with increasing pressure. It was found that a metallic ζ-phase appears at 96 GPa when ε-phase oxygen is further compressed.[5]

Red oxygen

As the pressure of oxygen at room temperature is increased through 10 GPa, it undergoes a dramatic phase transition to a different allotrope. Its volume decreases significantly,[6] and it changes color from blue to deep red.[7] This ε-phase was discovered in 1979, but the structure has been unclear. Based on its infrared absorption spectrum, researchers assumed in 1999 that this phase consists of O
4
molecules in a crystal lattice.[8] However, in 2006, it was shown by X-ray crystallography that this stable phase known as ε oxygen or red oxygen is in fact O
8
.[9][10] No one predicted the structure theoretically:[5] a rhomboid O
8
cluster[11] consisting of four O
2
molecules.

Ball-and-stick model of O8
Part of the crystal structure of ε-oxygen

In this phase it exhibits a dark-red color, very strong infrared absorption, and a magnetic collapse.[1] It is also stable over a very large pressure domain and has been the subject of numerous X-ray diffraction, spectroscopic and theoretical studies. It has been shown to have a monoclinic C2/m symmetry and its infrared absorption behaviour was attributed to the association of oxygen molecules into larger units.

  • Liquid oxygen is already used as an oxidant in rockets, and it has been speculated that red oxygen could make an even better oxidant, because of its higher energy density.[12]
  • Researchers think that this structure may greatly influence the structural investigation of elements.[5]
  • It is the phase that forms above 600 K at pressures greater than 17 GPa.[5]
  • At 11 GPa, the intra-cluster bond length of the O
    8
    cluster is 0.234 nm, and the inter-cluster distance is 0.266 nm. (For comparison, the intra-molecular bond length of the oxygen molecule O
    2
    is 0.120 nm.)[5]
  • The formation mechanism of the O
    8
    cluster found in the work is not clear yet, and the researchers think that the charge transfer between oxygen molecules or the magnetic moment of oxygen molecules has a significant role in the formation.[5]

Metallic oxygen

A ζ-phase appears at 96 GPa when ε-phase oxygen is further compressed.[6] This phase was discovered in 1990 by pressurizing oxygen to 132 GPa.[2] The ζ-phase with metallic cluster[13] has been known to exhibit superconductivity at low temperature.[3][5]

References

  1. ^ a b c d Freiman, Y. A. & Jodl, H. J. (2004). "Solid oxygen". Phys. Rep. 401: 1–228.  
  2. ^ a b Desgreniers, S., Vohra, Y. K. & Ruoff, A. L. (1990). "Optical response of very high density solid oxygen to 132 GPa". J. Phys. Chem. 94 (3): 1117–1122.  
  3. ^ a b Shimizu, K., Suhara, K., Ikumo, M., Eremets, M. I. & Amaya, K. (1998). "Superconductivity in oxygen". Nature 393 (6687): 767–769.  
  4. ^ Roder, H. M. (1978). "The molar volume (density) of solid oxygen in equilibrium with vapor" (reprint). Journal of Physical and Chemical Reference Data 7 (3): 949.  
  5. ^ a b c d e f g h "Solid Oxygen ε-Phase Crystal Structure Determined Along With The Discovery of a Red Oxygen O8 Cluster". Retrieved 2008-01-10. 
  6. ^ a b Akahama, Yuichi; Haruki Kawamura, Daniel Häusermann, Michael Hanfland, and Osamu Shimomura (June 1995). "New High-Pressure Structural Transition of Oxygen at 96 GPa Associated with Metallization in a Molecular Solid". Physical Review Letters 74 (23): 4690–4694.  
  7. ^ Nicol, Malcolm; K. R. Hirsch; Wilfried B. Holzapfel (December 1979). "Oxygen Phase Equilibria near 298 K". Chemical Physics Letters 68 (1): 49–52.  
  8. ^ Gorelli, Federico A.; Lorenzo Ulivi; Mario Santoro; Roberto Bini (November 1999). "The ε Phase of Solid Oxygen: Evidence of an O4 Molecule Lattice". Physical Review Letters 83 (20): 4093–4096.  
  9. ^ Hiroshi Fujihisa, Yuichi Akahama, Haruki Kawamura, Yasuo Ohishi, Osamu Shimomura, Hiroshi Yamawaki, Mami Sakashita, Yoshito Gotoh, Satoshi Takeya, and Kazumasa Honda (2006-08-26). "O8 Cluster Structure of the Epsilon Phase of Solid Oxygen". Phys. Rev. Lett. 97 (8): 085503.  
  10. ^ Lars F. Lundegaard, Gunnar Weck, Malcolm I. McMahon, Serge Desgreniers and Paul Loubeyre (2006-09-14). "Observation of an O8 molecular lattice in the phase of solid oxygen". Nature 443 (7108): 201–204.  
  11. ^ Steudel, Ralf; Wong, MW (2007). "Dark-Red O8 Molecules in Solid Oxygen: Rhomboid Clusters, Not S8-Like Rings".  
  12. ^ Ball, Phillip (16 November 2001). "New form of oxygen found". Nature News.  
  13. ^ Peter P. Edwards, Friedrich Hensel (2002-01-14). "Metallic Oxygen". ChemPhysChem (Weinheim, Germany: WILEY-VCH-Verlag) 3 (1): 53–56.  
This article was sourced from Creative Commons Attribution-ShareAlike License; additional terms may apply. World Heritage Encyclopedia content is assembled from numerous content providers, Open Access Publishing, and in compliance with The Fair Access to Science and Technology Research Act (FASTR), Wikimedia Foundation, Inc., Public Library of Science, The Encyclopedia of Life, Open Book Publishers (OBP), PubMed, U.S. National Library of Medicine, National Center for Biotechnology Information, U.S. National Library of Medicine, National Institutes of Health (NIH), U.S. Department of Health & Human Services, and USA.gov, which sources content from all federal, state, local, tribal, and territorial government publication portals (.gov, .mil, .edu). Funding for USA.gov and content contributors is made possible from the U.S. Congress, E-Government Act of 2002.
 
Crowd sourced content that is contributed to World Heritage Encyclopedia is peer reviewed and edited by our editorial staff to ensure quality scholarly research articles.
 
By using this site, you agree to the Terms of Use and Privacy Policy. World Heritage Encyclopedia™ is a registered trademark of the World Public Library Association, a non-profit organization.
 


Copyright © World Library Foundation. All rights reserved. eBooks from Project Gutenberg are sponsored by the World Library Foundation,
a 501c(4) Member's Support Non-Profit Organization, and is NOT affiliated with any governmental agency or department.