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Related Concept Videos

Molecular and Ionic Solids02:54

Molecular and Ionic Solids

20.1K
Crystalline solids are divided into four types: molecular, ionic, metallic, and covalent network based on the type of constituent units and their interparticle interactions.
Molecular Solids
Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...
20.1K
Ionic Radii03:10

Ionic Radii

33.6K
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...
33.6K
Ionic Crystal Structures02:42

Ionic Crystal Structures

17.1K
Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
17.1K
Ionic Bonds00:42

Ionic Bonds

131.0K
Overview
When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.
Opposing Charges Hold Ions Together in Ionic Compounds
Ionic bonds are reversible electrostatic interactions between ions...
131.0K
Oxidation Numbers03:14

Oxidation Numbers

42.8K
In redox reactions, the transfer of electrons occurs between reacting species. Electron transfer is described by a hypothetical number called the oxidation number (or oxidation state). It represents the effective charge of an atom or element, which is assigned using a set of rules.
42.8K
Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

68.2K
Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water.
68.2K

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Oxidation states and ionicity.

Aron Walsh1,2, Alexey A Sokol3, John Buckeridge3

  • 1Department of Materials, Imperial College London, London, UK. a.walsh@imperial.ac.uk.

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This summary is machine-generated.

Oxidation states and atomic charges are distinct concepts crucial for materials science. Understanding their differences and applications is key to interpreting material properties and electronic behaviors.

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Area of Science:

  • Materials Science
  • Quantum Chemistry

Background:

  • Oxidation state and atomic charge concepts are often intertwined in materials science.
  • Distinguishing these quantities is essential for accurate material property analysis.

Purpose of the Study:

  • To differentiate between oxidation state and atomic charge.
  • To explore their limitations and utility in understanding material properties.
  • To review the evolution and significance of these concepts.

Main Methods:

  • Discussion of atomic bonding and electron density partitioning techniques.
  • Analysis of the application of oxidation states and atomic charges in physical processes.
  • Review of recent advancements and current understanding.

Main Results:

  • Formal oxidation states aid in electron counting, while partial atomic charges describe physical phenomena like dielectric response.
  • Partial charges, though useful in models, may lack transferability.
  • Oxidation states aim for universality, with deviations highlighting complex systems.

Conclusions:

  • Clarifying the distinct roles of oxidation states and atomic charges enhances the understanding of materials.
  • These concepts are fundamental to interpreting electronic spectroscopies and dielectric responses.
  • Continued research into deviations from universal oxidation states drives innovation in materials science.