Electron deficiency
Template:Short description In chemistry, electron deficiency (and electron-deficient) is jargon that is used in two contexts: chemical species that violate the octet rule because they have too few valence electrons and species that happen to follow the octet rule but have electron-acceptor properties, forming donor-acceptor charge-transfer salts.
Octet rule violationsEdit
{{#invoke:Labelled list hatnote|labelledList|Main article|Main articles|Main page|Main pages}} Traditionally, "electron-deficiency" is used as a general descriptor for boron hydrides and other molecules which do not have enough valence electrons to form localized (2-centre 2-electron) bonds joining all atoms.<ref>Template:Cite book</ref> For example, diborane (B2H6) would require a minimum of 7 localized bonds with 14 electrons to join all 8 atoms, but there are only 12 valence electrons.<ref>Template:Cite journal</ref> A similar situation exists in trimethylaluminium. The electron deficiency in such compounds is similar to metallic bonding.Template:Cn
Electron-acceptor moleculesEdit
Alternatively, electron-deficiency describes molecules or ions that function as electron acceptors. Such electron-deficient species obey the octet rule, but they have (usually mild) oxidizing properties.<ref>Template:Cite journal</ref> 1,3,5-Trinitrobenzene and related polynitrated aromatic compounds are often described as electron-deficient.<ref name=Goetz>Template:Cite journal</ref> Electron deficiency can be measured by linear free-energy relationships: "a strongly negative ρ value indicates a large electron demand at the reaction center, from which it may be concluded that a highly electron-deficient center, perhaps an incipient carbocation, is involved."<ref>Template:March6th</ref>