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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.
Intermolecular Forces03:13

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...
Polyprotic Acids03:38

Polyprotic Acids

Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
Basicity of Aliphatic Amines01:21

Basicity of Aliphatic Amines

Amines can behave as Brønsted–Lowry bases by accepting a proton from the acid to form corresponding conjugate acids. Due to a lone pair of nonbonding electrons, aliphatic amines can also act as Lewis bases by forming a covalent bond with an electrophile.
To measure the basicity of amines, two conventions are generally used. The first defines Kb as the basicity constant for the deprotonation reaction of water by the amine, as presented in Figure 1. Conventionally, lower Kb indicates higher...
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...
Ionic Association01:28

Ionic Association

The ionic association is the association of oppositely charged ions in an electrolyte solution to form ion pairs. Bjerrum defined ion pairs as two oppositely charged ions whose electrostatic attraction exceeds the thermal energy of the system, typically expressed as 2kT. Electrostatic attraction depends on ionic charge, separation distance, and the dielectric constant of the medium. Thermal energy, represented by kT, reflects the tendency of ions to move independently due to molecular motion.

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Related Experiment Video

Updated: May 24, 2026

Analyzing Protein Dynamics Using Hydrogen Exchange Mass Spectrometry
11:37

Analyzing Protein Dynamics Using Hydrogen Exchange Mass Spectrometry

Published on: November 29, 2013

Interplay between anion-pi and hydrogen bonding interactions.

Daniel Escudero1, Antonio Frontera, David Quiñonero

  • 1Departament de Química, Universitat de les Illes Balears, 07122 Palma de Mallorca, Spain.

Journal of Computational Chemistry
|May 30, 2008
PubMed
Summary

Synergistic effects occur when anion-pi and hydrogen bonding interactions coexist in aromatic systems. High-level calculations reveal these interactions mutually influence each other, enhancing molecular complex stability.

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Area of Science:

  • Computational chemistry
  • Supramolecular chemistry
  • Chemical physics

Background:

  • Noncovalent interactions are crucial in molecular recognition and self-assembly.
  • Aromatic rings participate in various noncovalent interactions, including hydrogen bonding and anion-pi interactions.
  • Understanding the interplay of these forces is essential for designing functional molecular systems.

Purpose of the Study:

  • To investigate the synergistic effects between anion-pi and hydrogen bonding interactions.
  • To elucidate the mutual influence of these two noncovalent interactions in complexes involving aromatic rings.
  • To quantify the impact of combined interactions on molecular complex stability.

Main Methods:

  • High-level ab initio calculations were employed to model the molecular complexes.
  • The "atoms-in-molecules" (AIM) theory was used to analyze electron distribution and bonding characteristics.
  • The Molecular Interaction Potential with polarization (MIP) partition scheme was applied to quantify interaction energies.

Main Results:

  • Synergistic effects were confirmed in complexes featuring coexisting anion-pi and hydrogen bonding interactions.
  • The mutual influence between anion-pi and hydrogen bonding was demonstrated to enhance binding.
  • Quantitative analysis revealed the contribution of each interaction to the overall complex stability.

Conclusions:

  • Anion-pi and hydrogen bonding interactions exhibit significant synergy when present together in aromatic systems.
  • These findings provide valuable insights into the cooperative nature of noncovalent interactions.
  • The study contributes to a deeper understanding of molecular complex formation and stability.