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Related Concept Videos

Valence Bond Theory02:45

Valence Bond Theory

Overview of Valence Bond Theory
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...
Hydrogen Bonds01:04

Hydrogen Bonds

A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...
Hydrogen Bonds00:26

Hydrogen Bonds

Hydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.
Hydrogen Bonds Control the World!
Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared.
Molecular Orbital Theory II03:51

Molecular Orbital Theory II

Molecular Orbital Energy Diagrams
Valence Bond Theory and Hybridized Orbitals02:38

Valence Bond Theory and Hybridized Orbitals

According to valence bond theory, a covalent bond results when: (1) an orbital on one atom overlaps an orbital on a second atom, and (2) the single electrons in each orbital combine to form an electron pair. The strength of a covalent bond depends on the extent of overlap of the orbitals involved. Maximum overlap is possible when the orbitals overlap on a direct line between the two nuclei.
A σ bond (single bond in a Lewis structure) is a covalent bond in which the electron density is...

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Related Experiment Video

Updated: May 13, 2026

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
06:44

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

Published on: March 24, 2018

Halogen bonding and other σ-hole interactions: a perspective.

Peter Politzer1, Jane S Murray, Timothy Clark

  • 1Department of Chemistry, University of New Orleans, New Orleans, LA 70148, USA. ppolitze@uno.edu

Physical Chemistry Chemical Physics : PCCP
|March 2, 2013
PubMed
Summary

Sigma-hole bonds are noncovalent interactions involving a positive electrostatic potential region (σ-hole) on an atom. These interactions, including halogen bonding, are explained by electrostatics and polarization, with strength correlating to electrostatic potentials.

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Spatial Separation of Molecular Conformers and Clusters
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Last Updated: May 13, 2026

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
06:44

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

Published on: March 24, 2018

Construction and Systematical Symmetric Studies of a Series of Supramolecular Clusters with Binary or Ternary Ammonium Triphenylacetates
06:35

Construction and Systematical Symmetric Studies of a Series of Supramolecular Clusters with Binary or Ternary Ammonium Triphenylacetates

Published on: February 15, 2016

Spatial Separation of Molecular Conformers and Clusters
10:37

Spatial Separation of Molecular Conformers and Clusters

Published on: January 9, 2014

Area of Science:

  • Chemical Physics
  • Supramolecular Chemistry
  • Computational Chemistry

Background:

  • A σ-hole bond is a noncovalent interaction formed between a Group IV-VII atom and a negative site.
  • This interaction arises from a region of positive electrostatic potential, the σ-hole, on the atom's bond extension.
  • Halogen bonding is a well-known subset of these σ-hole interactions.

Purpose of the Study:

  • To elucidate the fundamental nature and driving forces of σ-hole bonds.
  • To explain the characteristics and properties of σ-hole interactions, including halogen bonding.
  • To investigate the factors influencing the strength and favorability of these noncovalent interactions.

Main Methods:

  • Analysis of electrostatic potentials and charge distribution anisotropy.
  • Application of electrostatics, polarization, and dispersion principles.
  • Consideration of polarizabilities and dative sharing in specific cases.

Main Results:

  • The features of σ-hole bonds are comprehensively explained by electrostatics, polarization, and dispersion.
  • Interaction strengths generally correlate with the magnitudes of the positive σ-hole potential and the negative site's potential.
  • In some cases, significant polarization leads to a degree of coordinate covalence.

Conclusions:

  • σ-hole interactions are primarily governed by electrostatic and polarization effects.
  • The strength of these bonds is predictable based on electrostatic potential magnitudes.
  • Gas-phase interactions with neutral bases can be thermodynamically unfavorable due to entropy loss.