electron pair


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Related to electron pair: Molecular geometry

electron pair

n.
1. Two electrons functioning or regarded as functioning in concert, especially two electrons that form a covalent bond between atoms.
2. The combination of an electron and a positron as produced by a high-energy photon.
References in periodicals archive ?
McMaster University professor emeritus Ronald Gillespie, HFCIC, (together with Australian Ronald Nyholm) developed valence shell electron pair repulsion theory.
From the simulation, it can be found that the inhibition efficiency afforded by DEAMB may be due to the its electron rich N atoms, imidazole and phenyl group, and the possible coordination points are unshared electron pair of heteroatoms and p-electrons of imidazole and phenyl group.
The VSEPR (valence shell electron pair repulsion) model (Gillespie, 1963) can predict the magnitudes of the various bond angles but offers no insights into why those angles have particular values.
To find the binding energy E < 0 of electron pair, we search the solution of the Schrodinger equation with introduction of wave function [psi]([?
Phosphine, PR3, is a three-coordinated organophosphorus compound comprising three covalent bonds and an unshared electron pair.
Lewis's electronic definition of acids and bases founded on electron pair sharing is valuable in its broadening of the field of acid/base reactions, it is problematic in that it does not allow for the establishment of a universal order of acid or base strength, unlike the competing Bronsted definition based on proton exchange.
Before the electron pair can jump back by emitting a red photon, they are redirected into QPF chute that captures the energy jump as a high-energy ATP bond instead.
These include explicit correlation methods that augment the conventional wavefunction expansion with terms that depend on the electron pair correlation factors.
The binding interactions between an electron pair donor (Lewis base) and an electron pair acceptor (Lewis acid) play an important role in many chemical processes.
The general saturable nature of this bond and the empirical fact that an electron pair cannot normally be used to form more than one covalent bond arise because the intensity of the magnetic field of the anti-parallel electron pair constituting the bond is significantly reduced due to the anti-parallel alignment.
The steric shielding of the free electron pair in the nitrogen atom of the amine and its reduced basicity enhance its effectiveness as a stabilizer.
The source of attraction is the acrylonitrile group specifically the triple bonded nitrogen via its unshared electron pair.

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