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Related Concept Videos

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.
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...
Bond Energies and Bond Lengths02:49

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, that is, the energy necessary to separate the bonded atoms. Separating any pair of bonded atoms requires energy — the stronger a bond, the greater the energy required to break it.
Covalent Bonding and Lewis Structures02:46

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual attraction of atoms for a “shared” pair of electrons.
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...

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Related Experiment Video

Updated: May 16, 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

Is the decrease of the total electron energy density a covalence indicator in hydrogen and halogen bonds?

Emilio L Angelina1, Darío J R Duarte, Nélida M Peruchena

  • 1Laboratorio de Estructura Molecular y Propiedades, Área de Química Física, Departamento de Química, Facultad de Ciencias Exactas y Naturales y Agrimensura, Universidad Nacional del Nordeste, Avda. Libertad 5460, Corrientes, Argentina.

Journal of Molecular Modeling
|November 29, 2012
PubMed
Summary
This summary is machine-generated.

This study reveals that decreasing electronic energy density in halogen and hydrogen bonds stems primarily from electrostatic attraction, not solely covalent character. Understanding these interactions is key for molecular design.

More Related Videos

Spatial Separation of Molecular Conformers and Clusters
10:37

Spatial Separation of Molecular Conformers and Clusters

Published on: January 9, 2014

Related Experiment Videos

Last Updated: May 16, 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

Spatial Separation of Molecular Conformers and Clusters
10:37

Spatial Separation of Molecular Conformers and Clusters

Published on: January 9, 2014

Area of Science:

  • Quantum Chemistry
  • Supramolecular Chemistry
  • Computational Chemistry

Background:

  • Halogen bonding (XB) and hydrogen bonding (HB) are crucial non-covalent interactions.
  • Understanding the energetic contributions to these interactions is vital for predicting molecular behavior.

Purpose of the Study:

  • To analyze the variation of total electronic energy density H(r b) with interaction strengthening in XB and HB complexes.
  • To elucidate the energetic origins of interaction strengthening in these complexes.

Main Methods:

  • High-level ab initio calculations using MP2/6-311++G(2d,2p) approximation.
  • Atoms in Molecules (AIM) theory and Reduced Variational Space Self-Consistent Field (RVS) energy decomposition analysis.
  • Derivation of an equation to decompose H(r b) based on the local virial theorem.

Main Results:

  • A relationship was established between H(r b) energy densities and RVS interaction energy components.
  • A decrease in H(r b) was observed with increasing interaction strength in both HB and XB complexes.
  • This decrease is predominantly driven by enhanced electrostatic attraction, with a lesser contribution from covalent character.

Conclusions:

  • The energetic basis for interaction strengthening in XB and HB complexes is primarily electrostatic.
  • The study refines the understanding of non-covalent interactions beyond traditional covalent character emphasis.
  • Findings provide insights into molecular interactions relevant to various chemical and biological systems.