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Tetraoxygen

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The tetraoxygen molecule (O4), also called oxozone, was first predicted in 1924 by Gilbert N. Lewis, who proposed it as an explanation for the failure of liquid oxygen to obey Curie's law.[1] Today it seems Lewis was off, but not by much: computer simulations indicate that although there are no stable O4 molecules in liquid oxygen, O2 molecules do tend to associate in pairs with antiparallel spins, forming transient O4 units.[2] In 1999, researchers thought that solid oxygen existed in its ε-phase (at pressures above 10 GPa) as O4.[3] However, in 2006, it was shown by X-ray crystallography that this stable phase known as ε oxygen or red oxygen is in fact O8.[4] Nevertheless, tetraoxygen has been detected as a short-lived chemical speciesin mass spectrometry experiments.[5]

Absorption bands of the O4 molecule e.g. at 360, 477 and 577 nm are frequently used to do aerosol inversions in atmospheric optical absorption spectroscopy. Due to the known distribution of O2 and therefore also O4, O4 slant column densities can be used to retrieve aerosol profiles which can then be used again in radiative transfer models to model light paths.[6]

[edit]Free moleculeEdit

Theoretical calculations have predicted the existence of metastable O4 molecules with two different shapes: a "puckered" square like cyclobutane or S4,[7] and a "pinwheel" with three oxygen atoms surrounding a central one in a trigonal planar formation similar to boron trifluoride.[8][9] It was previously pointed out that the "pinwheel" O4 molecule should be the natural continuation of the isoelectronic series BO33-, CO32-, NO3-,[10] and analogous to SO3; that observation served as the basis for the mentioned theoretical calculations.

Theoretical structures of metastable O4.
[1] [2]
D2d structure D3h structure

In 2001, a team at the University of Rome La Sapienza conducted a neutralization-reionization mass spectrometry experiment to investigate the structure of free O4 molecules.[5] Their results did not agree with either of the two proposed molecular structures, but they did agree with a complex between two O2 molecules, one in the ground state and the other in a specific excited state.

[edit]Edit

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