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Related Concept Videos

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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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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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.
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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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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.
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Valence Bond Theory02:45

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Overview of Valence Bond Theory
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Electron-Pair Distribution in Chemical Bond Formation.

M Rodríguez-Mayorga1,2, M Via-Nadal1, M Solà2

  • 1Kimika Fakultatea, Euskal Herriko Unibertsitatea, UPV/EHU, and Donostia International Physics Center (DIPC). P.K. 1072 , 20080 Donostia, Euskadi, Spain.

The Journal of Physical Chemistry. A
|January 31, 2018
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Summary
This summary is machine-generated.

This study introduces relaxation holes (Δh(u)) to analyze chemical bond formation by examining electron pair reorganization. The shape and magnitude of Δh(u) reveal details about chemical bonds and electron distributions in larger systems.

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Area of Science:

  • Quantum Chemistry
  • Computational Chemistry
  • Chemical Physics

Background:

  • Understanding chemical bond formation is fundamental in chemistry.
  • Electron pair behavior significantly influences molecular structure and reactivity.
  • Analyzing electron density distributions provides insights into bonding.

Purpose of the Study:

  • To investigate chemical formation processes using relaxation holes (Δh(u)).
  • To demonstrate that Δh(u) can visualize electron reorganization and covalent bond formation.
  • To explore the utility of Δh(u) characteristics in defining chemical bond nature.

Main Methods:

  • Calculation of radial intracule density and its nonrelaxed counterpart.
  • Analysis of the difference, Δh(u), between these densities.
  • Development of a computationally affordable method for calculating radial intracule density from approximate pair densities.

Main Results:

  • The shape of Δh(u) clearly distinguishes internal electron reorganization and covalent bond formation.
  • Magnitude, shape, and key distances within Δh(u) correlate with chemical bond properties.
  • A new method allows for the study of electron-pair distributions in larger molecular systems.

Conclusions:

  • Relaxation holes (Δh(u)) are effective indicators of chemical bond formation dynamics.
  • Δh(u) analysis offers a detailed view of electron behavior during chemical reactions.
  • The proposed computational approach broadens the scope for studying electron distributions in complex systems.