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Related Concept Videos

Intermolecular Forces03:13

Intermolecular Forces

62.1K
Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen...
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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:
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Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

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The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary...
1.9K
Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

43.1K
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. 
43.1K
Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

64.7K
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.
64.7K
Ionic Bonds00:42

Ionic Bonds

122.6K
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...
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Interactions and stabilisation of acetone, sulfur dioxide and water with 1-octyl-3-methylimidazolium tetrafluoroborate [OMIM][BF<sub>4</sub>] at low temperatures.

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A Method to Manipulate Surface Tension of a Liquid Metal via Surface Oxidation and Reduction
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Ionic liquids on oxide surfaces.

Jordan Cole1, Karen L Syres1

  • 1Jeremiah Horrocks Institute for Mathematics, Physics and Astronomy, University of Central Lancashire, Preston, PR1 2HE, United Kingdom.

Journal of Physics. Condensed Matter : an Institute of Physics Journal
|March 2, 2022
PubMed
Summary

Ionic liquids (ILs) on oxide surfaces show complex interactions, influenced by surface defects and ion choice. Understanding these interfacial behaviors is key for applications in catalysis, energy storage, and nanoparticle synthesis.

Keywords:
TiO2ZnOinterfacesionic liquidsnanoparticle synthesisoxidessurfaces

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Writing and Low-Temperature Characterization of Oxide Nanostructures
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Area of Science:

  • Materials Science
  • Surface Chemistry
  • Electrochemistry

Background:

  • Ionic liquids (ILs) are versatile materials with applications spanning catalysis, energy storage, and nanotechnology.
  • The interface between ILs and oxide surfaces is complex, with defects and ion choice significantly impacting properties.
  • Oxide surfaces like TiO2, ZnO, and Al2O3 are crucial components in many IL-based systems.

Purpose of the Study:

  • To review recent experimental and theoretical studies on the interaction of ILs with oxide surfaces.
  • To highlight the role of surface defects and IL composition in adsorption and electronic properties.
  • To consolidate knowledge on IL/oxide systems for diverse technological applications.

Main Methods:

  • Review of experimental investigations on ILs interacting with model single crystal oxide surfaces.
  • Analysis of theoretical/computational studies on IL adsorption and electronic properties at oxide interfaces.
  • Examination of IL/oxide performance in prototype devices, including catalysis and energy storage.

Main Results:

  • Defects on oxide surfaces play a critical role in IL adsorption and electronic properties.
  • The cation/anion selection of ILs influences molecular ordering and interfacial electronic behavior.
  • Controllable interfacial properties of IL/oxide systems are demonstrated for various applications.

Conclusions:

  • The interaction of ILs with oxide surfaces is a complex phenomenon crucial for advanced material design.
  • Further research into IL/oxide interfaces will drive innovation in catalysis, energy, and nanotechnology.
  • Understanding these interactions enables the development of novel materials for diverse technological applications.