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 simple diatomic molecule (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]

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 (1,450,377 psi), 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