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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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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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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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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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From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
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Strumming a Single Chemical Bond.

Alfred J Weymouth1, Elisabeth Riegel1, Oliver Gretz1

  • 1University of Regensburg, 93053 Regensburg, Germany.

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|May 30, 2020
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Summary
This summary is machine-generated.

Lateral force microscopy with a CO-terminated tip measures molecular interactions and energy dissipation. This technique reveals unique insights into surface dynamics with unprecedented vertical resolution.

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Area of Science:

  • Surface Science
  • Nanotechnology
  • Molecular Imaging

Background:

  • Atomic force microscopy (AFM) and scanning tunneling microscopy (STM) image molecular structures on surfaces.
  • A common method involves using a carbon monoxide (CO) molecule at the tip for Pauli repulsion imaging.

Purpose of the Study:

  • To investigate energy dissipation during molecular manipulation using lateral force microscopy (LFM).
  • To characterize the vertical decay length of energy dissipation in LFM.

Main Methods:

  • Utilizing lateral force microscopy (LFM) with a CO-terminated tip.
  • Oscillating the tip laterally to probe interactions and measure energy dissipation.

Main Results:

  • LFM demonstrated the ability to pull and release a CO molecule over chemical bonds.
  • Measurable energy dissipation was observed during the CO molecule's motion.
  • A characteristic vertical decay length of 4 pm was determined for energy dissipation.

Conclusions:

  • LFM offers a unique method for probing molecular interactions and energy dissipation at the nanoscale.
  • The observed decay length is significantly smaller than in conventional STM/AFM, indicating high sensitivity.