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The dihydrogen cation is of great historical, theoretical, and experimental interest. Historically it is of interest because, having only one electron, the equations of quantum mechanics that describe its structure can be solved approximately in a relatively straightforward way, as long as the motion of the nuclei and relativistic and quantum ...
Zundel cation. A hydrogen atom is made up of a nucleus with charge +1, and a single electron. Therefore, the only positively charged ion possible has charge +1. It is noted H +. Depending on the isotope in question, the hydrogen cation has different names: Hydron: general name referring to the positive ion of any hydrogen isotope (H +)
It is a triangular species, like the aforementioned dihydrogen complexes. It is known as protonated molecular hydrogen or the trihydrogen cation. [85] Hydrogen directly reacts with chlorine, fluorine and bromine to give HF, HCl, and HBr, respectively. The conversion involves a radical chain mechanism.
An often studied dihydrogen complex of iron, [HFe(H 2)(dppe) 2] +.. The usual method for characterization is 1 H NMR spectroscopy.The magnitude of spin–spin coupling, J HD, is a useful indicator of the strength of the bond between the hydrogen and deuterium in HD complexes.
The trihydrogen cation or protonated molecular hydrogen (IUPAC name: hydrogenonium ion) is a cation (positive ion) with formula H + 3, consisting of three hydrogen nuclei sharing two electrons. The trihydrogen cation is one of the most abundant ions in the universe.
Øyvind Burrau (or Øjvind Burrau [1] [2]), born 24 March 1896 [3] in Copenhagen, died 31 March 1979, [4] was a Danish scientist who is best known for his early quantum mechanical description of the dihydrogen cation [1] [2] which he made while at the Niels Bohr Institute. [2] Burrau worked as a geodesist at the Geodætisk Institut from 1928 to ...
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In chemistry, a dihydrogen bond is a kind of hydrogen bond, an interaction between a metal hydride bond and an OH or NH group or other proton donor. With a van der Waals radius of 1.2 Å, hydrogen atoms do not usually approach other hydrogen atoms closer than 2.4 Å. Close approaches near 1.8 Å, are, however, characteristic of dihydrogen ...