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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

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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...
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Hydrogen Bonds00:26

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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.
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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....
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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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Valence Bond Theory02:45

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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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Covalent Bonds01:29

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From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
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Covalent Bonding in the Hydrogen Molecule.

George B Bacskay1, Sture Nordholm2

  • 1School of Chemistry, The University of Sydney , Sydney, NSW 2006, Australia.

The Journal of Physical Chemistry. A
|November 18, 2017
PubMed
Summary

Covalent bonding is explained by a decrease in kinetic energy due to electron delocalization, not just electrostatic forces. This quantum mechanical phenomenon is crucial for understanding molecular stability.

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Area of Science:

  • Quantum Chemistry
  • Theoretical Chemistry
  • Chemical Bonding

Background:

  • Ongoing debate exists regarding the primary mechanism of covalent bonding: kinetic energy reduction via electron delocalization versus electrostatic potential energy reduction.
  • Previous studies on H2+ laid the groundwork for investigating electron pair bonding in H2.

Purpose of the Study:

  • To resolve the debate on covalent bonding mechanisms by studying the hydrogen molecule (H2).
  • To analyze the contributions of electron density, kinetic energy, and potential energy to the stability of H2.

Main Methods:

  • Employed various computational approaches to analyze electron density and energy distributions.
  • Examined the electronic structure and energetics of the H2 molecule in detail.

Main Results:

  • The study's findings for H2 align with the Ruedenberg analysis, indicating kinetic energy decrease is key.
  • Electronic delocalization leads to a reduction in interatomic kinetic energy, stabilizing the covalent bond.

Conclusions:

  • Covalent bonding is fundamentally a quantum dynamical phenomenon driven by a decrease in kinetic energy.
  • The description of covalent bonding necessitates the inclusion of quantized kinetic energy principles.