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Related Concept Videos

Ionic Radii03:10

Ionic Radii

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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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Atomic Radii and Effective Nuclear Charge03:08

Atomic Radii and Effective Nuclear Charge

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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.
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Common Ion Effect03:24

Common Ion Effect

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Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Châtelier’s principle. Consider the dissolution of silver iodide:
47.8K
Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

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Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions. 
53.2K
Basicity of Aliphatic Amines01:21

Basicity of Aliphatic Amines

7.1K
Amines can behave as Brønsted–Lowry bases by accepting a proton from the acid to form corresponding conjugate acids. Due to a lone pair of nonbonding electrons, aliphatic amines can also act as Lewis bases by forming a covalent bond with an electrophile.
To measure the basicity of amines, two conventions are generally used. The first defines Kb as the basicity constant for the deprotonation reaction of water by the amine, as presented in Figure 1. Conventionally, lower Kb indicates higher...
7.1K
Ionic Crystal Structures02:42

Ionic Crystal Structures

19.9K
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...
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Updated: Mar 16, 2026

Vibrational Spectra of a N719-Chromophore/Titania Interface from Empirical-Potential Molecular-Dynamics Simulation, Solvated by a Room Temperature Ionic Liquid
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Vibrational Spectra of a N719-Chromophore/Titania Interface from Empirical-Potential Molecular-Dynamics Simulation, Solvated by a Room Temperature Ionic Liquid

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On the effective ionic radii for ammonium.

Vasyl Sidey1

  • 1Department of Chemistry and Research Institute for Physics and Chemistry of Solids, Uzhgorod National University, Pidgirna Street 46, Uzhgorod 88000, Ukraine.

Acta Crystallographica Section B, Structural Science, Crystal Engineering and Materials
|August 4, 2016
PubMed
Summary
This summary is machine-generated.

New ionic radii for ammonium (NH4+) have been determined for various coordination numbers (CNs). These values are compatible with Shannon

Keywords:
ammoniumbond valence modelionic radii

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

  • Crystallography
  • Inorganic Chemistry
  • Materials Science

Background:

  • Accurate ionic radii are crucial for understanding crystal structures and chemical bonding.
  • Existing radii systems may not fully encompass the diverse coordination environments of polyatomic ions like ammonium.
  • The ammonium ion (NH4+) presents unique challenges due to its size and charge distribution.

Purpose of the Study:

  • To derive a comprehensive set of effective ionic radii for the ammonium ion (NH4+) across various coordination numbers (CNs).
  • To ensure compatibility of the derived radii with the established Shannon ionic radii system.
  • To determine bond-valence parameters for ammonium-fluorine bonds.

Main Methods:

  • Utilizing crystallographic data and established methodologies for radius determination.
  • Applying the bond-valence model to analyze ammonium-containing compounds.
  • Comparing derived radii with existing data to ensure consistency and accuracy.

Main Results:

  • Effective ionic radii for ammonium (NH4+) were determined for coordination numbers IV, VI, VIII, and XII: 1.40 Å, 1.48 Å, 1.54 Å, and 1.67 Å, respectively.
  • The derived radii are consistent with Shannon's ionic radii system.
  • Bond-valence parameters (r0 = 2.3433 Å, B = 0.262 Å) were established for ammonium-fluorine bonds.

Conclusions:

  • The newly derived ionic radii for ammonium provide a more accurate representation of its size in various coordination environments.
  • These radii enhance the predictive power of crystallographic and chemical bonding models involving ammonium.
  • The determined bond-valence parameters facilitate precise analysis of ammonium-fluorine interactions in diverse chemical systems.