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Electrolyte and Nonelectrolyte Solutions02:21

Electrolyte and Nonelectrolyte Solutions

Substances that undergo either a physical or a chemical change in solution to yield ions that can conduct electricity are called electrolytes. If a substance yields ions in solution, that is, if the compound undergoes 100% dissociation, then the substance is a strong electrolyte. Complete dissociation is indicated by a single forward arrow. For example, water-soluble ionic compounds like sodium chloride dissociate into sodium cations and chloride anions in aqueous solution.
Electrolytes: van't Hoff Factor03:08

Electrolytes: van't Hoff Factor

Colligative Properties of ElectrolytesThe colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one dissolved...
Factors Affecting Solubility04:01

Factors Affecting Solubility

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 Chȃtelier’s principle. Consider the dissolution of silver iodide:
Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

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 cation—the calcium...
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...
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Electrochemical Systems

Electrochemical systems provide a fascinating insight into the dynamic interplay of charged species within various phases. One notable example is the interaction between a membrane permeable to K⁺ ions but not to Cl⁻ ions, separating an aqueous KCl solution from pure water. As K⁺ ions diffuse through the membrane, they generate net charges on each phase, leading to a potential difference between them.Similarly, when a piece of Zn is immersed in an aqueous ZnSO₄ solution, the Zn metal, composed...

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Solid-state Graft Copolymer Electrolytes for Lithium Battery Applications
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Los efectos del disolvente en la electrofilicidad.

P Pérez1, A Toro-Labbé, R Contreras

  • 1Departamento de Química Física, Pontificia Universidad Católica de Chile, Casilla 306, Correo 22, Santiago, Chile.

Journal of the American Chemical Society
|June 8, 2001
PubMed
Resumen
Este resumen es generado por máquina.

Los efectos del disolvente en la electrofilicidad se estudiaron utilizando el modelo de continuo polarizado de isodensidad autoconsistente (SCI-PCM). La disolución aumenta la electrofilicidad para las moléculas neutras, pero la reduce para las cargadas.

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Área de la Ciencia:

  • Química computacional es la química computacional.
  • Química teórica es la química teórica.
  • La química cuántica es una química cuántica.

Sus antecedentes:

  • El índice de electrofilicidad cuantifica la resistencia de una molécula al ataque nucleófilo.
  • Comprender los efectos del disolvente es crucial para predecir la reactividad química en la solución.
  • El modelo de continuo polarizado de isodensidad autoconsistente (SCI-PCM) es un método para simular los efectos del disolvente.

Objetivo del estudio:

  • Para investigar el impacto de los efectos del disolvente continuo en el índice de electrofilicidad.
  • Para analizar la relación entre la energía de solvatación y los cambios en la electrofilicidad.
  • Examinar cómo los entornos polarizables influyen en la electrofilicidad de diversas moléculas.

Principales métodos:

  • Utilizó el modelo de continuo polarizado de isodensidad autoconsistente (SCI-PCM) para modelar los efectos del disolvente.
  • Calculó el índice de electrofilicidad para 18 electrofiles diferentes en diversos entornos de disolventes.
  • Teoría de campo de reacción aplicada para relacionar la energía de solvación y los cambios en el índice de electrophilicidad.

Principales resultados:

  • Se observó una correlación lineal entre el cambio en el índice de electrofilicidad y la energía de disolución.
  • Se encontró que la disolución aumentaba la electrofilicidad de los ligandos electrofílicos neutros.
  • Se descubrió que la solvación disminuye la electrofilicidad de los electrofiles cargados y iónicos.

Conclusiones:

  • Los modelos de disolvente continuo como el SCI-PCM capturan con precisión la influencia del entorno en la electrofilicidad.
  • El efecto de la solvación sobre la electrophilicidad depende de la carga de las especies electrófilas.
  • Este estudio proporciona información sobre la predicción de la reactividad en solución para una gama de electrófilos.