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Related Concept Videos

Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

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.
Ionic Bonds00:42

Ionic Bonds

When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.Opposing Charges Hold Ions Together in Ionic CompoundsIonic bonds are reversible electrostatic interactions between ions with...
Ionic Bonds00:42

Ionic Bonds

When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.Opposing Charges Hold Ions Together in Ionic CompoundsIonic bonds are reversible electrostatic interactions between ions with...
Bond Polarity, Dipole Moment, and Percent Ionic Character02:48

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Valence Bond Theory02:42

Valence Bond Theory

Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
Valence Bond Theory02:45

Valence Bond Theory

Overview of Valence Bond Theory

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Updated: Jun 2, 2026

Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides
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Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides

Published on: September 7, 2019

A one-electron perspective on dative and ionic bonding.

D Barrena-Espés1, E Francisco1, Á Martín Pendás1

  • 1Dpto. Química Física y Analítica, Universidad de Oviedo C/ Julián Clavería 8 33006 Oviedo Spain ampendas@uniovi.es.

Chemical Science
|June 1, 2026
PubMed
Summary
This summary is machine-generated.

This study re-examines chemical bonding, suggesting single-electron interactions are key. It proposes a new framework for understanding dative and ionic bonds, challenging the electron pair model.

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Area of Science:

  • Quantum Chemistry
  • Theoretical Chemistry
  • Chemical Bonding Theory

Background:

  • The traditional distinction between electron-sharing and dative bonding, established by Lewis, is debated.
  • Overemphasis on electron pairs as the fundamental units of bonding may obscure alternative interpretations.
  • Existing models struggle to consistently explain diverse bonding scenarios.

Purpose of the Study:

  • To investigate the role of single-electron interactions in chemical bonding.
  • To propose a unified framework for interpreting dative, ionic, and polar covalent bonds.
  • To challenge the exclusive focus on electron pairs in bonding theories.

Main Methods:

  • Generalized Valence Bond (GVB) theory.
  • Real-space descriptors: Laplacian of electron density, delocalization indices, IQA energy decomposition.
  • Electron distribution functions and variational quantum Monte Carlo Born maxima.

Main Results:

  • Many bonds traditionally classified as dative or ionic can be explained by a single-electron bonding framework.
  • In this framework, one electron remains localized, while its spin-paired partner delocalizes, contributing significantly to bonding.
  • This motif is observed in ionic, polar covalent, and donor-acceptor systems.

Conclusions:

  • A single-electron bonding perspective offers a coherent interpretation across various bonding regimes.
  • This viewpoint challenges the traditional electron pair model and suggests a more nuanced understanding of chemical bonds.
  • Single-electron bonding is likely a common and chemically relevant phenomenon.