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Noncovalent Attractions in Biomolecules02:35

Noncovalent Attractions in Biomolecules

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Noncovalent attractions are associations within and between molecules that influence the shape and structural stability of complexes. These interactions differ from covalent bonding in that they do not involve sharing of electrons.
Four types of noncovalent interactions are hydrogen bonds, van der Waals forces, ionic bonds, and hydrophobic interactions.
Hydrogen bonding results from the electrostatic attraction of a hydrogen atom covalently bonded to a strong-electronegative atom like oxygen,...
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Noncovalent Attractions in Biomolecules02:35

Noncovalent Attractions in Biomolecules

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Covalent Bonding and Lewis Structures02:46

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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.
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Types of Chemical Bonds02:37

Types of Chemical Bonds

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Chemical bonding theories were pioneered by American chemist Gilbert N. Lewis. He developed a model called the Lewis model to explain the type and formation of different bonds. Chemical bonding is central to chemistry; it explains how atoms or ions bond together to form molecules. It explains why some bonds are strong and others are weak, or why one carbon bonds with two oxygens and not three; why water is H2O and not H4O. 
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Types of Chemical Bonds02:36

Types of Chemical Bonds

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Chemical Bonds02:40

Chemical Bonds

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Atoms participate in a chemical bond formation to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest to it in atomic number. Ionic, covalent, and metallic bonds are some of the important types of chemical bonds. Bond energy and bond length determine the strength of a chemical bond.
Types of Chemical Bonds
An ionic bond is formed due to electrostatic attraction between cations and anions. Often, the ions are formed by the transfer of electrons...
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Related Experiment Video

Updated: Dec 4, 2025

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

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Understanding noncovalent bonds and their controlling forces.

Steve Scheiner1

  • 1Department of Chemistry and Biochemistry, Utah State University, Logan, Utah 84322-0300, USA.

The Journal of Chemical Physics
|October 22, 2020
PubMed
Summary

This study explores noncovalent bonds, particularly σ-hole interactions, detailing their strength, influencing factors, and predictive methods for nucleophile interactions. It explains how anions bond and the role of first-row atoms.

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Area of Science:

  • Chemistry
  • Molecular Interactions
  • Computational Chemistry

Background:

  • Noncovalent bonds are crucial in molecular interactions.
  • Hydrogen bonds are well-studied, but related interactions like σ-hole bonds require further elucidation.
  • Understanding these interactions is key to predicting molecular behavior and designing new materials.

Purpose of the Study:

  • To present the fundamental principles of noncovalent bonds, with a focus on σ-hole interactions.
  • To discuss methods for assessing the strength of these bonds and the factors influencing them.
  • To explore the formation of noncovalent bonds and predict nucleophilic attack sites.

Main Methods:

  • Analysis of electrostatic and charge redistribution effects during bond formation.
  • Assessment of factors controlling noncovalent bond strength.
  • Methods for predicting nucleophile binding sites and coordination numbers.
  • Examination of anion-anion interactions and the role of first-row atoms.

Main Results:

  • Detailed presentation of σ-hole interactions, their relation to hydrogen bonds, and strength assessment.
  • Monitoring of bond establishment through subunit interaction, revealing electrostatic and charge redistribution effects.
  • Methods provided for predicting nucleophile attraction sites and maximum bonding around central atoms.
  • Explanation for anion pairing against Coulombic repulsion and discussion of first-row atom participation.

Conclusions:

  • Noncovalent bonds, especially σ-hole interactions, are fundamental and controllable.
  • Predictive methods for bond formation and strength are established.
  • The study expands the understanding of bonding, including anion interactions and first-row atom involvement.