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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...
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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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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. 
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Ionic Compounds: Formulas and Nomenclature03:34

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An element composed of atoms that readily lose electrons (a metal) can react with an element composed of atoms that readily gain electrons (a nonmetal) to produce ions through complete electron transfer. The compound formed by this transfer is stabilized by the electrostatic attractions (ionic bonds) between the oppositely charged ions.
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Trends in Lattice Energy: Ion Size and Charge02:54

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24.0K
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:
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Solubility of Ionic Compounds02:55

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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.
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Characterization of Electrode Materials for Lithium Ion and Sodium Ion Batteries Using Synchrotron Radiation Techniques
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Order-disorder and ionic conductivity in calcium nitride-hydride.

G J Irvine1, Ronald I Smith2, M O Jones3,2

  • 1Chemistry, University of St Andrews, St Andrews, Scotland, KY16 9ST, UK. gji4@st-andrews.ac.uk.

Nature Communications
|July 20, 2023
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Summary

Calcium nitride hydride (Ca2NH) co-catalysts enable ammonia synthesis by acting as hydrogen sinks. This study reveals fast hydride ion conduction in one Ca2NH phase, crucial for understanding and improving these catalytic materials.

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Area of Science:

  • Materials Science
  • Catalysis
  • Solid-state Chemistry

Background:

  • Nitrogen-hydrogen compounds, like calcium nitride hydride (Ca2NH), are emerging co-catalysts for ammonia synthesis under mild conditions.
  • Ca2NH functions as a hydrogen (H2) sink, incorporating lattice hydrogen into ammonia (NH3) product.
  • Understanding ionic transport and diffusion in these co-catalysts is key to optimizing ammonia synthesis.

Purpose of the Study:

  • To investigate hydride ion conduction properties in distinct calcium nitride-hydride (Ca2NH) phases.
  • To correlate material structure and synthesis method with ionic conductivity.
  • To elucidate the mechanism of ion transport in conductive Ca2NH phases.

Main Methods:

  • Synthesis of two distinct Ca2NH phases using different routes.
  • Measurement of ionic conductivity at elevated temperatures (600°C).
  • In situ combined analysis techniques to probe ion transport mechanisms.

Main Results:

  • Two Ca2NH phases exhibited significantly different ionic properties.
  • The beta (β) phase demonstrated fast hydride ion conduction (0.08 S/cm at 600°C), surpassing CaH2 by tenfold.
  • The alpha (α) phase showed 100-fold lower conductivity compared to the β-phase.
  • The β-phase conducts ions via a vacancy-mediated mechanism, dependent on secondary site ion concentration and main site vacancy concentration.

Conclusions:

  • Hydride ion conduction is confirmed in calcium nitride-hydride materials.
  • The synthesis route critically influences the ionic transport properties of Ca2NH.
  • The β-phase exhibits promising ionic conductivity for potential applications in ammonia synthesis catalysis.