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Related Concept Videos

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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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. 
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Overview of Valence Bond Theory
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Valence Bond Theory02:42

Valence Bond Theory

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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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In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
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Bonding in Metals02:32

Bonding in Metals

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Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”. 
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From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
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The Origin of Chalcogen-Bonding Interactions.

Dominic J Pascoe1, Kenneth B Ling2, Scott L Cockroft1

  • 1EaStCHEM School of Chemistry, University of Edinburgh , Joseph Black Building, David Brewster Road, Edinburgh EH9 3FJ, U.K.

Journal of the American Chemical Society
|October 7, 2017
PubMed
Summary

Chalcogen bonds, interactions between group 16 elements, are as strong as hydrogen bonds but solvent-independent. These molecular interactions are driven by orbital delocalization, not electrostatic forces, impacting molecular recognition.

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Area of Science:

  • Chemistry
  • Molecular Interactions
  • Computational Chemistry

Background:

  • Chalcogen bonds, analogous to hydrogen and halogen bonds, involve group 16 elements and are crucial in various chemical fields.
  • The energetic significance and origins of chalcogen bonds remain debated, particularly their dependence on solvent effects.

Purpose of the Study:

  • To quantitatively investigate the energetics of chalcogen-bonding interactions experimentally.
  • To examine the influence of substituents and solvents on chalcogen bond strength and characteristics.
  • To elucidate the underlying physicochemical origins of chalcogen bonds.

Main Methods:

  • Utilized synthetic molecular balances to measure over 160 experimental conformational free energies.
  • Investigated various chalcogen contacts (O···S, O···Se, S···S) and related C-H contacts (O···HC, S···HC).
  • Analyzed substituent and solvent effects across 13 different solvents.

Main Results:

  • The strongest chalcogen bonds were experimentally found to be comparable in strength to conventional hydrogen bonds.
  • Unlike hydrogen bonds, chalcogen bond strength showed surprising independence from solvent polarity, polarizability, and hydrogen-bonding capacity.
  • Orbital delocalization (n → σ*) between donor lone pairs and acceptor antibonding orbitals was identified as the dominant stabilizing interaction, irrespective of contact type.

Conclusions:

  • Chalcogen bonds are primarily governed by orbital delocalization, explaining their strength and solvent independence.
  • Electrostatic, solvophobic, and van der Waals forces do not adequately explain the observed experimental trends in chalcogen bonding.
  • Orbital delocalization plays a critical role in conformational control and molecular recognition, highlighting its importance in chemical systems.