| 词条 | Hydrogen anion |
| 释义 |
| SystematicName = Hydride[1] |Section1={{Chembox Identifiers | CASNo = 12184-88-2 | PubChem = 166653 | ChemSpiderID = 145831 | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChEBI = 29239 | Gmelin = 14911 | SMILES = [H-] | StdInChI = 1S/H/q-1 | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = KLGZELKXQMTEMM-UHFFFAOYSA-N | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} }} |Section2={{Chembox Properties | Formula = {{Chem|H|-}} | H=1 | ConjugateAcid = Dihydrogen }} |Section3={{Chembox Thermochemistry | Entropy = 108.96 J K−1 mol−1 }} }} The hydrogen anion, H−, is a negative ion of hydrogen, that is, a hydrogen atom that has captured an extra electron. The hydrogen anion is an important constituent of the atmosphere of stars, such as the Sun. In chemistry, this ion is called hydride. The ion has two electrons bound by the electromagnetic force to a nucleus containing one proton. The binding energy of H− equals the binding energy of an extra electron to a hydrogen atom, called electron affinity of hydrogen. It is measured to be {{val|0.754195|(19)|ul=eV}} or {{val|0.0277161|(62)|ul=hartree}} (see Electron affinity (data page)). The total ground state energy thus becomes {{val|-14.359888|u=eV}}. OccurrenceThe hydrogen anion is the dominant bound-free opacity source at visible and near-infrared wavelengths in the atmospheres of stars like the Sun and cooler (Mihalas 1978); its importance was first noted in the 1930s (Wildt 1939). The ion absorbs photons with energies in the range 0.75–4.0 eV, which ranges from the infrared into the visible spectrum (Rau 1996, Srinivasan 1999). Most of the electrons in these negative ions come from the ionization of metals with low first ionization potentials, including the alkali metals and alkali earths. The process which ejects the electron from the ion is properly called photodetachment rather than photoionization because the result is a neutral atom (rather than an ion) and a free electron. H− also occurs in the Earth's ionosphere (Rau 1999), and can be produced in particle accelerators. Its existence was first proven theoretically by Hans Bethe in 1929 ({{harvnb|Bethe|1929}}). H− is unusual because, in its free form, it has no bound excited states, as was finally proven in 1977 ({{harvnb|Hill|1977}}). It has been studied experimentally using particle accelerators ({{harvnb|Bryant|1977}}). In chemistry, the hydride anion is hydrogen that has the formal oxidation state −1. The term hydride is probably most often used to describe compounds of hydrogen with other elements in which the hydrogen is in the formal −1 oxidation state. In most such compounds the bonding between the hydrogen and its nearest neighbor is covalent. An example of a hydride is the borohydride anion ({{chem|BH|4|-}}). See also
References1. ^{{Cite web|url = https://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=166653|title = Hydride - PubChem Public Chemical Database|work = The PubChem Project|location = USA|publisher = National Center for Biotechnology Information}} Sources{{refbegin}}
3 : Hydrogen physics|Astrophysics|Anions |
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