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Electron Behavior00:54

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Overview
Electrons are negatively charged subatomic particles that are attracted to an orbit around the positively-charged nucleus of an atom. They reside in locations that are associated with energy levels called shells and are further organized into sub-shells and orbitals within each shell.
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Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions. 
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Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F&#8722;
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Odd-Electron Bonds.

Timothy Clark1

  • 1Computer-Chemie-Centrum, Department of Chemistry and Pharmacy, Friedrich-Alexander-University of Erlangen-Nuernberg, Nägelsbachstr. 25, 91052, Erlangen, Germany.

Chemphyschem : a European Journal of Chemical Physics and Physical Chemistry
|May 26, 2017
PubMed
Summary
This summary is machine-generated.

The study discusses one- and three-electron bonds, revealing that odd-electron bond energy calculations need to incorporate ion-pairing energy for neutral complexes. This refines our understanding of chemical bonding. Keywords: odd-electron bonds, ion-pairing energy, chemical bonding theory.

Keywords:
ab initio calculationsbond theoryodd-electron bondsradical reactionsreactive intermediates

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Area of Science:

  • Chemistry
  • Chemical Physics
  • Quantum Chemistry

Background:

  • Theories of chemical bonding, particularly those involving an odd number of electrons, are fundamental to understanding molecular stability and reactivity.
  • One- and three-electron bonds represent unique bonding scenarios with distinct energetic properties.

Purpose of the Study:

  • To present a comprehensive historical and theoretical overview of one- and three-electron bonds.
  • To identify and correct a key factor influencing the energy calculations of neutral odd-electron bonded complexes.

Main Methods:

  • Review of historical and theoretical literature on electron bonding.
  • Theoretical analysis of the energetic contributions to odd-electron bonds.

Main Results:

  • The dependence of odd-electron bond energy on ionization potential differences requires adjustment.
  • Inclusion of ion-pairing energy is essential for accurate calculations of neutral odd-electron bonded complexes.

Conclusions:

  • The established models for odd-electron bond energy require refinement.
  • Accurate prediction of stability for neutral odd-electron complexes necessitates considering ion-pairing effects.