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Related Concept Videos

Ionic Association01:28

Ionic Association

The ionic association is the association of oppositely charged ions in an electrolyte solution to form ion pairs. Bjerrum defined ion pairs as two oppositely charged ions whose electrostatic attraction exceeds the thermal energy of the system, typically expressed as 2kT. Electrostatic attraction depends on ionic charge, separation distance, and the dielectric constant of the medium. Thermal energy, represented by kT, reflects the tendency of ions to move independently due to molecular motion.
Intermolecular Forces03:13

Intermolecular Forces

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 bonds, and dispersion...
Solvating Effects02:12

Solvating Effects

An understanding of the solvating effect helps rationalize the relation between solvation and acidity of the compound. In addition, this also explains the relative stability of conjugate bases for compounds with different pKa values. This lesson details, in-depth, the principle of solvating effects. The strength of an acid and the stability of its corresponding conjugate base are determined using pKa values. This observed relationship is a consequence of solvation, which is the interaction...
Aqueous Solutions and Heats of Hydration02:42

Aqueous Solutions and Heats of Hydration

Water and other polar molecules are attracted to ions. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. These attractions play an important role in the dissolution of ionic compounds in water.
When ionic compounds dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution because water molecules surround and solvate the ions, reducing the strong electrostatic forces between them. This process...
Theory of Strong Electrolytes01:23

Theory of Strong Electrolytes

The interionic forces of the strong electrolytes depend on the solvent's dielectric constant, which is the ability of a solvent to store electrical energy, based on its polarizability. and the solution's concentration. In high-dielectric solvents and in dilute solutions, weak electrostatic forces keep ions apart. However, in low-dielectric solvents or concentrated solutions, stronger interionic forces may cause ions to pair up as ionic doublets despite being fully ionized. The theory of strong...
Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

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.

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Synthesis of Ionic Liquid Based Electrolytes, Assembly of Li-ion Batteries, and Measurements of Performance at High Temperature
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Published on: December 20, 2016

Ionicity and proton transfer in protic ionic liquids.

Jelena Stoimenovski1, Ekaterina I Izgorodina, Douglas R MacFarlane

  • 1School of Chemistry, Monash University, Clayton, Victoria 3800, Australia. Jelena.Stoimenovski@sci.monash.edu.au

Physical Chemistry Chemical Physics : PCCP
|July 6, 2010
PubMed
Summary

Proton transfer in protic ionic liquids differs between primary and tertiary amines. Primary amines show more complete proton transfer due to better ion solvation via hydrogen bonding.

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Area of Science:

  • Chemistry
  • Physical Chemistry
  • Ionic Liquids

Background:

  • Proton transfer in protic ionic liquids (PILs) is not fully understood.
  • Observed proton transfer extents deviate from predictions based on aqueous pKa data.
  • Investigating factors influencing proton transfer completeness in PILs is crucial.

Purpose of the Study:

  • To investigate proton transfer completeness in PILs formed from acetic acid and various amine bases.
  • To differentiate the behavior of primary versus tertiary amines in these systems.
  • To elucidate the role of ion solvation and hydrogen bonding in proton transfer.

Main Methods:

  • Synthesis of protic ionic liquids from acetic acid and diverse amine bases.
  • Utilizing probe indicator observations to assess proton transfer.
  • Analyzing transport properties and constructing Walden plots.
  • Performing computational studies to understand molecular interactions.

Main Results:

  • A clear distinction in proton transfer behavior was observed between primary and tertiary amines.
  • Proton transfer was found to be more complete in PILs derived from primary amines.
  • Tertiary amine-derived PILs exhibited less complete proton transfer.
  • Evidence suggests differences in ion solvation environments based on amine structure.

Conclusions:

  • The hydrogen bonding ability of ammonium ions significantly influences proton transfer completeness.
  • Primary amines facilitate more complete proton transfer due to superior solvation of resulting ions.
  • Amine structure (primary vs. tertiary) is a key determinant of proton transfer extent in PILs.
  • Understanding these factors is vital for designing PILs with specific properties.