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Bond Energies and Bond Lengths

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.

Hydrogen Bonds

Hydrogen Bonds

A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...

Hydrogen Bonds

Hydrogen Bonds

Hydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.
Hydrogen Bonds Control the World!
Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared....

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

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Hylleraas hydride binding energy: diatomic electron affinities.

Edward S Chen¹, Herman Keith, Tristan Lim

¹Baylor College of Medicine, One Baylor Plaza, Houston, TX, 77030, USA, eschen@bcm.edu.

Journal of Molecular Modeling

|March 12, 2015

Summary

This study revisits experimental electron affinities, assigning new values for diatomic molecules like Cl2 and Br2. It also calculates anion Morse potentials for H2 and N2, advancing our understanding of molecular stability.

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Published on: January 25, 2020

Area of Science:

Physical Chemistry
Quantum Chemistry
Spectroscopy

Background:

Theoretical electron affinities often lack accuracy due to single-value referencing.
Recent work established ground state electron affinities for main group elements and diatomics using normalized hydrogen atom binding energy.

Purpose of the Study:

To re-evaluate experimental electron affinity values.
To extend electron affinity identifications to diatomics within the G2-1 molecular set.
To calculate anion Morse potentials and explore hyperfine superoxide states.

Main Methods:

Revisiting and analyzing experimental data for electron affinities.
Assigning new ground state electron affinities for various diatomic molecules.
Calculating anion Morse potentials using established positive electron affinity data.

Main Results:

New ground state electron affinities were assigned: Cl2 (3.2(2) eV), Br2 (2.87(14) eV), CH (2.1(2) eV), H2 (0.6 eV), NH (1.1 eV), and SiH (1.90 eV).
Anion Morse potentials were computed for H2 and N2.
Hyperfine superoxide states were analyzed for the first time.

Conclusions:

The study provides refined experimental electron affinities for several diatomic molecules.
The calculation of anion Morse potentials and exploration of superoxide states offer new insights into molecular behavior and stability.