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Related Concept Videos

Ionization Energy03:12

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy (IE1). The first ionization energy for an element, X, is the energy required to form a cation with 1+ charge:
The Energies of Atomic Orbitals03:21

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are also observed. The attractive and repulsive forces are dependent on the distance between the particles, as well as the sign and magnitude of the charges on the individual particles. When the charges on the particles are opposite, they attract each other. If both particles have the same charge, they repel each other.
Trends in Lattice Energy: Ion Size and Charge02:54

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure of the strength of this attraction. The lattice energy (ΔHlattice) of an ionic compound is defined as the energy required to separate one mole of the solid into its component gaseous ions. For the ionic solid sodium chloride, the lattice energy is the enthalpy change of the process:
Electron Affinity03:07

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).
Atomic Radii and Effective Nuclear Charge03:08

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number and distribution of electrons in their valence shells.
Chemical Ionization (CI) Mass Spectrometry01:21

Chemical Ionization (CI) Mass Spectrometry

The molecular ion peak of a molecule in the mass spectrum provides vital information for molecular identification. However, conventional electron impact ionization can lead to the rapid dissociation of some molecular ions before they reach the detector. A milder ionization method is required to increase the lifetime of such ionized analyte molecules. Chemical ionization (CI) is a gas-phase protonation reaction useful for mass-analyzing analyte molecules that are easily protonated to yield the...

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Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F&#8722;
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Published on: July 27, 2018

Average local ionization energy: A review.

Peter Politzer1, Jane S Murray, Felipe A Bulat

  • 1CleveTheoComp, 1951 W. 26th Street, Suite 409, Cleveland, OH 44113, USA. ppolitze@uno.edu

Journal of Molecular Modeling
|April 23, 2010
PubMed
Summary
This summary is machine-generated.

The average local ionization energy I(r) identifies electron locations for chemical reactions. This fundamental property also impacts atomic structure, electronegativity, and local polarizability.

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Area of Science:

  • Quantum Chemistry
  • Chemical Physics

Background:

  • The average local ionization energy, I(r), quantifies the energy to remove an electron from a specific point in a system.
  • Understanding I(r) is crucial for predicting chemical reactivity and electronic properties.

Purpose of the Study:

  • To review the definition and properties of the average local ionization energy, I(r).
  • To discuss the significance of I(r) in various fundamental chemical and physical concepts.

Main Methods:

  • Conceptual review of the definition and properties of I(r).
  • Discussion of I(r)'s role in atomic shell structure, electronegativity, and local polarizability/hardness.

Main Results:

  • I(r) directly indicates sites of least tightly-held electrons.
  • Lowest I(r) values pinpoint favored locations for electrophilic and radical reactions.

Conclusions:

  • The average local ionization energy, I(r), is a versatile descriptor of electronic structure and reactivity.
  • I(r) provides insights into fundamental chemical concepts beyond just reaction sites.