Manifestation of site energy landscapes for ion transport in borate glasses

  • 0Philipps-Universität Marburg, Chemistry Department, Hans-Meerwein Str. 4, 35043 Marburg, Germany. weitzel@chemie.uni-marburg.de.

Summary

This summary is machine-generated.

Investigating lithium borate glass, researchers found that replacing lithium ions with larger alkali ions significantly slows down native ion diffusion. This reveals insights into the material's energy landscape and ion transport mechanisms.

Area Of Science

  • Materials Science
  • Solid-State Chemistry
  • Ion Transport Phenomena

Background

  • Lithium borate glasses are crucial in various applications, including solid electrolytes.
  • Understanding ion transport is key to optimizing glass properties for technological use.
  • The potential energy landscape governs ion mobility within these materials.

Purpose Of The Study

  • To investigate the potential energy landscape of Li3B7O12 glass.
  • To determine the effect of substituting native lithium ions with foreign alkali ions (K+, Rb+, Cs+) on ion diffusion.
  • To model the energy landscape using a site energy distribution.

Main Methods

  • Charge Attachment Induced Transport (CAIT) technique was employed.
  • Macroscopic ion replacement experiments were conducted.
  • Nernst-Planck-Poisson modeling was used with secondary ion mass spectrometry (SIMS) data.

Main Results

  • A significant decrease in native ion diffusion coefficients (over 4 orders of magnitude) was observed as the local population of Li+ decreased.
  • The energy landscape was successfully modeled by a site energy distribution (SED).
  • The populated part of the SED exhibited a width of 250 meV (FWHM).

Conclusions

  • The study elucidates the relationship between alkali ion substitution and ion diffusion in lithium borate glass.
  • The findings provide a quantitative model for the energy landscape governing ion transport.
  • The research offers insights into generalizing macroscopic transport theories.

Related Concept Videos

Trends in Lattice Energy: Ion Size and Charge 02:54

23.9K

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:



Conventions

Here, the convention is used where the ionic...

Crystal Field Theory - Octahedral Complexes 02:58

26.4K

Crystal Field Theory
To explain the observed behavior of transition metal complexes (such as colors), a model involving electrostatic interactions between the electrons from the ligands and the electrons in the unhybridized d orbitals of the central metal atom has been developed. This electrostatic model is crystal field theory (CFT). It helps to understand, interpret, and predict the colors, magnetic behavior, and some structures of coordination compounds of transition metals.
CFT focuses on...

The Born-Haber Cycle 02:44

21.8K

Lattice Energy 

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. 

Here, the convention is used where the ionic solid is separated into ions, meaning the lattice energies will be...

Crystal Field Theory - Tetrahedral and Square Planar Complexes 02:46

42.4K

Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...

Ionic Strength: Effects on Chemical Equilibria 01:19

1.4K

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...

Intermolecular Forces 03:13

58.2K

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...