This article includes a list of references, related reading or external links, but its sources remain unclear because it lacks inline citations. (April 2018) (Learn how and when to remove this template message)
Electron deficiency is a term describing atoms or molecules having fewer than the number of electrons required for maximum stability. At the atomic level, main group atoms having less than 8 electrons or transition metal atoms having less than 18 electrons are described as electron-deficient. At the molecular level, molecules which have an incompletely filled set of bonding molecular orbitals are considered to be electron-deficient. Thus, CH3 and BH3 are electron-deficient, while methane (CH4) and diborane (B2H6) are not. Not surprisingly, electron-deficient molecules are typically strongly electron-attracting (electrophilic). As the most extreme form of electron deficiency one can consider the metallic bond.
Boranes and carboranesEdit
For many years, "electron-deficiency" was often used as a general descriptor for boron hydrides and other molecules featuring multicenter bonding (in which a pair of bonding electrons extends over more than two atoms, as in three-center two-electron bonds), as a way of distinguishing such molecules from conventionally bonded compounds such as hydrocarbons. However, this usage was incorrect, as many (indeed most) of the molecules formerly labeled "electron-deficient", such as boranes, are actually electron-precise. An example is the extremely stable icosahedral B12H122- dianion, whose 26 cluster valence electrons exactly fill the 13 bonding molecular orbitals and is in no actual sense deficient in electrons; indeed it is thermodynamically far more stable than benzene. The same is true of its isoelectronic C2B10H12 carborane analogues. More generally, nearly all carboranes, boranes, and other known and characterized polyboron clusters are similarly electron-precise. Some molecules that have no overall electron deficiency can nevertheless function as electron-acceptors at specific locations on the cluster, e.g., 1,2-C2B10H12 (o-carborane), whose C-H bonds are slightly acidic owing to the local positive charge at the carbon vertices, which increases the polarity of these bonds. In contrast, the B-H groups in this molecule have a relatively high electron density and exhibit no electrophilic behavior.
The term electron-deficient has traditionally been used in organic chemistry to indicate a pi-system such as an alkene or arene that has electron-withdrawing groups attached, as found in nitrobenzene or acrylonitrile. Instead of showing the nucleated character common with simple C=C bonds, electron-deficient pi-systems may be electrophilic and susceptible to nucleophilic attack, as is seen in the Michael addition or in nucleophilic aromatic substitution.
- R. N. Grimes (2016) Carboranes 3rd Edition, Elsevier, New York and Amsterdam, pp. 16-17.
- H. C. Longuet-Higgins (1957) "The structures of electron-deficient molecules", Quarterly Reviews, Chemical Society, Volume 11, issue 2, pp. 121–133.
|This chemistry-related article is a stub. You can help Wikipedia by expanding it.|