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Related Concept Videos

Types of Chemical Bonds02:37

Types of Chemical Bonds

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.
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.
Chemical Bonds02:40

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.
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 from...
Radical Formation: Homolysis00:54

Radical Formation: Homolysis

A bond is formed between two atoms by sharing two electrons. When this bond is broken by supplying sufficient energy, either two electrons can be taken up by one atom forming ions by the cleavage called heterolysis, or the two electrons are shared by two atoms, with one each creating radicals by the cleavage called homolysis.
Types of Chemical Bonds02:37

Types of Chemical Bonds

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.
Introduction to Chemical Bonds01:01

Introduction to Chemical Bonds

Chemical Bonds
The electrons of the outermost energy level determine the energetic stability of the atom and its tendency to form chemical bonds with other atoms. The innermost electron shell has a maximum capacity of two electrons, but the next two electron shells can each have a maximum of eight electrons. This is known as the octet rule, which states that, with the exception of the innermost shell, atoms are most stable energetically when they have eight electrons in their valence shell, the...

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Related Experiment Video

Updated: Jul 7, 2026

The Preparation of Electrohydrodynamic Bridges from Polar Dielectric Liquids
10:03

The Preparation of Electrohydrodynamic Bridges from Polar Dielectric Liquids

Published on: September 30, 2014

Chemical bond-making, bond-breaking, and electron transfer in solution.

E M Arnett, K Amarnath, N G Harvey

    Science (New York, N.Y.)
    |January 26, 1990
    PubMed
    Summary

    This study introduces a method to calculate heats of heterolysis and homolysis for organic compounds using reaction heats and redox potentials. This provides new data on bond energies and ion properties.

    Area of Science:

    • Physical Organic Chemistry
    • Thermochemistry
    • Computational Chemistry

    Background:

    • Understanding bond dissociation energies is crucial in organic chemistry.
    • Existing methods for determining these energies can be complex or limited in scope.

    Purpose of the Study:

    • To develop a novel method for calculating heats of heterolysis (DeltaH(het)) and homolysis (DeltaH(homo)).
    • To compile a comprehensive dataset of these thermochemical values for various organic compounds.

    Main Methods:

    • Determining heats of reaction for resonance-stabilized carbenium ions and carbanions in solution.
    • Calculating electron transfer energies (deltaG(ET)) from redox potentials.
    • Correlating DeltaH(het), DeltaH(homo), and deltaG(ET) values.

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    From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

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    Last Updated: Jul 7, 2026

    The Preparation of Electrohydrodynamic Bridges from Polar Dielectric Liquids
    10:03

    The Preparation of Electrohydrodynamic Bridges from Polar Dielectric Liquids

    Published on: September 30, 2014

    Solvent Bonding for Fabrication of PMMA and COP Microfluidic Devices
    04:54

    Solvent Bonding for Fabrication of PMMA and COP Microfluidic Devices

    Published on: January 17, 2017

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    Main Results:

    • A reliable method for calculating DeltaH(het) from reaction heats was established.
    • Conversion of DeltaH(het) to DeltaH(homo) using electron transfer energies was achieved.
    • A comprehensive tabulation of DeltaH(het), DeltaH(homo), and deltaG(ET) for an extended series of organic compounds was generated.

    Conclusions:

    • The developed method provides accurate thermochemical data for organic compounds.
    • The interrelationships between DeltaH(het), DeltaH(homo), and deltaG(ET) offer insights into ion and radical properties.
    • This work expands the understanding of chemical bonding and reactivity in organic systems.