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Related Concept Videos

Ionic Radii03:10

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it is smaller than the atom from which it is derived. For example, the covalent radius of an aluminum atom (1s22s22p63s23p1) is 118 pm, whereas the ionic radius of an Al3+ (1s22s22p6) is 68 pm. As electrons are removed from the outer valence shell, the remaining core electrons occupying smaller shells experience a greater effective nuclear...
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Chemical Bonds


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 from...
Bond Energies and Bond Lengths02:49

Bond Energies and Bond Lengths

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.
Covalent Bonding and Lewis Structures02:46

Covalent Bonding and Lewis Structures

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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Dependence of Laser-induced Breakdown Spectroscopy Results on Pulse Energies and Timing Parameters Using Soil Simulants
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Molecular double-bond covalent radii for elements Li-E112.

Pekka Pyykkö1, Michiko Atsumi

  • 1Department of Chemistry, University of Helsinki, P.O.B. 55 (A.I. Virtasen aukio 1), 00014 Helsinki, Finland. pekka.pyykko@helsinki.fi

Chemistry (Weinheim an Der Bergstrasse, Germany)
|October 27, 2009
PubMed
Summary

This study extends covalent radii calculations to include double-bonds, providing a comprehensive model for predicting bond lengths. The new system accurately fits experimental and theoretical data for various chemical bonds.

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Area of Science:

  • Chemical bonding theory
  • Quantum chemistry
  • Atomic radii

Background:

  • Existing models for covalent radii primarily address single and triple bonds.
  • Accurate prediction of bond lengths is crucial in chemistry and materials science.

Purpose of the Study:

  • To develop and validate a self-consistent model for additive covalent radii that incorporates double-bonds.
  • To expand the predictive capabilities of covalent radii calculations.

Main Methods:

  • Utilized a self-consistent fitting procedure for covalent radii (r(E)).
  • Incorporated experimental and theoretical primary bond lengths (R) for diverse chemical species.
  • Employed models such as E=CH(2) and H-E=CH(2) for data generation.

Main Results:

  • Successfully extended the additive covalent radii model to include sigma(2)pi(2) double-bonds.
  • Achieved a standard deviation of 3 pm across 316 data points, indicating high accuracy.
  • Included data from homonuclear dimers, formaldehyde-type molecules, and Group 16 dimers.

Conclusions:

  • The developed model provides a unified and accurate system for calculating covalent radii across single, double, and triple bonds.
  • This work enhances the ability to predict and understand chemical bond lengths in various molecular systems.