Hydrogen polyoxides (also known as oxidanes, oxohydrogens, or oxyhydrogens) are chemical compounds that consist only of hydrogen and oxygen atoms, are bonded exclusively by single bonds (i.e., they are saturated), and are acyclic (have molecular structures containing no cycles or loops). They can therefore be classed as hydrogen chalcogenides.
The simplest possible stable hydrogen polyoxide (the parent molecule) is water, H2O. The general structure of the class of molecules is some number of oxygen atoms single-bonded to each other in a chain. The oxygen atom at each end of this oxygen skeleton is attached to a hydrogen atom. Thus, these compounds form a homologous series with chemical formula H
2O
n in which the members differ by a constant relative molecular mass of 16 (the mass of each additional oxygen atom). The number of oxygen atoms is used to define the size of the hydrogen polyoxide (e.g., hydrogen pentoxide contains a five-oxygen backbone).
An oxidanyl group is a functional group or side-chain analog of hydrogen polyoxide that is attached to some structure other than just a hydrogen atom. Examples include the hydroxy (oxidyl) and hydroperoxy (dioxidanyl) groups.
Specific examples
editHOn
editSeveral molecules are known where one end of the polyoxide chain is protonated and the other is an unprotonated radical:
- Hydroxyl (HO•)
- Hydroperoxyl (HOO•), the protonated form of superoxide
- Hydrogen ozonide (HOOO•), the protonated form of ozonide
H2On
editNeutral dihydrogen polyoxides containing up to five oxygen atoms have been produced experimentally.
- Water (H2O) is the most common hydrogen polyoxide, occurring widely on Earth's surface.
- Hydrogen peroxide (H2O2) is a common disinfectant and readily decomposes to form water and oxygen.
- Trioxidane (H2O3) is rare and readily decomposes into water and singlet oxygen.
- Tetraoxidane (H2O4) has been synthesized by reaction among peroxy radicals at low temperature.[1]
- Pentaoxidane (H2O5) is a byproduct of trioxidane production[2] and has also been synthesized by reaction among peroxy radicals at low temperature.[1]
Hydrogen polyoxides containing up to 10 oxygen atoms have been studied theoretically, but those containing more than five oxygens are expected to be extremely unstable.[3]
H3On
edit- Trihydrogen oxide (H3O), which has been studied theoretically and is expected to be stable at pressures over a few hundred gigapascals.[4]
Ionization
editAll the hydrogen polyoxides are known or expected to autoionise when in liquid form, with the acidic hydrogen being solvated by other of the neutral polyoxide molecules.
- H2On ⇌ H+ + HO–
n - 2 H2On ⇌ H
3O+
n + HO–
n
The ions can also be formed by protonation or deprotonation of various neutral hydrogen polyoxide by suitably strong other acids or bases. Specific ions include:
- Hydroxide (HO–)
- Hydronium (H3O+)
- Protonated ozone (HO3+)
See also
editReferences
edit- ^ a b Levanov, Alexander V.; Sakharov, Dmitri V.; Dashkova, Anna V.; Antipenko, Ewald E.; Lunin, Valeri V. (2011). "Synthesis of Hydrogen Polyoxides H2O4 and H2O3 and Their Characterization by Raman Spectroscopy". European Journal of Inorganic Chemistry. 2011 (33): 5144–5150. doi:10.1002/ejic.201100767.
- ^ Xu, Xin; Goddard, William A. III (November 2002). "Peroxone chemistry: Formation of H2O3 and ring-(HO2)(HO3) from O3/H2O2". Proceedings of the National Academy of Sciences. 99 (24): 15308–15312. Bibcode:2002PNAS...9915308X. doi:10.1073/pnas.202596799. PMC 137712. PMID 12438699.
- ^ Martins-Costa, Marilia; Anglada, Josep M.; Ruiz-Lopez, Manuel F. (2011). "Structure, stability, and dynamics of hydrogen polyoxides". International Journal of Quantum Chemistry. 111 (7–8): 1543–1554. doi:10.1002/qua.22695.
- ^ Huang, Peihao; Liu, Hanyu; Lv, Jian; Li, Quan; Long, Chunhong; Wang, Yanchao; Chen, Changfeng; Ma, Yanming (16 August 2019). "Metallic liquid H3O in a thin-shell zone inside Uranus and Neptune". arXiv:1908.05821 [physics.comp-ph].