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Chemical Bonds02:40

Chemical Bonds

16.3K

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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Bond Energies and Bond Lengths02:49

Bond Energies and Bond Lengths

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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

Valence Bond Theory

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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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Bond Dissociation Energy and Activation Energy02:13

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Bond energy is the energy required to break a bond homolytically. These values are usually expressed in units of kcal/mol or kJ/mol and are referred to as bond dissociation energies when given for specific bonds or average bond energies when indicated for a given type of bond over many compounds. Firstly, the bond dissociation energy for a single bond is weaker than that of a double bond, which in turn is weaker than that of a triple bond. Secondly, hydrogen forms relatively strong bonds with...
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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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Quantitative bond energetics in atomic-scale junctions.

Sriharsha V Aradhya1, Aileen Nielsen, Mark S Hybertsen

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Summary
This summary is machine-generated.

Researchers developed a method to measure the potential energy of chemical bonds in materials using atomic force microscopy. This technique provides quantitative bond energy data, revealing universal properties of single-atom contacts and molecular junctions.

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Area of Science:

  • Materials Science
  • Surface Science
  • Nanotechnology

Background:

  • Direct measurement of potential energy surfaces for chemical bonds is crucial for understanding materials.
  • Previous studies under ambient conditions primarily focused on rupture force trends.

Purpose of the Study:

  • To demonstrate a method for directly measuring the potential energy surface of individual chemical bonds in metallic single-atom contacts and single-molecule junctions.
  • To extract quantitative bond energy information from atomic force microscope (AFM) measurements.

Main Methods:

  • Utilizing ambient atomic force microscope (AFM) measurements in the near-equilibrium regime.
  • Fitting AFM data to a simple, physical functional form to map the energy profile.
  • Comparing extracted bond energies with density functional theory (DFT) calculations.

Main Results:

  • Successfully mapped the energy profiles for metallic single-atom contacts and single-molecule junctions.
  • Extracted quantitative bond energies for metallic bonds and metal-molecule link bonds.
  • Demonstrated excellent quantitative agreement between experimental AFM data and DFT calculations.
  • Showed that measurements from numerous junctions collapse to a universal force-extension curve, indicating similar potential energy surface shapes.

Conclusions:

  • The developed AFM-based method significantly expands quantitative information obtainable from junction measurements beyond rupture force.
  • The approach allows direct analysis of trends in bond energy, offering deeper insights into chemical bonding in complex materials.
  • A surprising universality in the potential energy surface shape governing these chemical bonds was revealed.