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A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
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Lewis Acids and Bases02:33

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In 1923, G. N. Lewis proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond.
A coordinate covalent bond (or dative bond) occurs when one of the atoms in the bond provides both bonding electrons. For example, a coordinate covalent bond occurs when a water molecule combines with a hydrogen ion to form a hydronium ion. A coordinate covalent bond also results when...
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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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Complexation Equilibria: Overview01:23

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Complexation reactions take place when dative or coordinate covalent bonds form between metal ions and ligands. The compounds formed in these reactions are called coordination compounds. The number of bonds formed between the metal ion and the ligands is called its coordination number. Generally, most metal ions in an aqueous solution are solvated by water molecules and thus exist as aqua complexes.
The equilibrium constant of the complexation reaction is represented as the formation constant...
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Common Ion Effect03:24

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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

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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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El efecto inductivo por sí solo no puede explicar la formación y disociación de los adductos de Lewis en las

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  • 1Department of Chemistry, University of Southern California, Los Angeles, California 90089, United States.

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Los investigadores crearon un adducto ácido-base de Lewis en una superficie de electrodo. El enlace nitrógeno-boro se desprende en potenciales negativos debido a los efectos iónicos, cruciales para comprender la electrocatálisis y la electroadsorción.

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Área de la Ciencia:

  • Química de las superficies
  • La electroquímica
  • Ciencias de los materiales

Sus antecedentes:

  • Comprender los enlaces de Lewis en las interfaces electrificadas es clave para la electrocatálisis y la electroadsorción.
  • Las complejidades interfaciales a menudo dificultan el estudio sistemático de estos enlaces.
  • Se necesita un sistema modelo para sondear las interacciones ácido-base de Lewis interfaciales.

Objetivo del estudio:

  • Para crear y estudiar un adducto ácido-base del grupo principal de Lewis en una superficie de electrodo.
  • Para investigar el comportamiento de este adducto bajo diferentes potenciales de electrodo.
  • Para aclarar los mecanismos que rigen la escisión de enlaces de Lewis en las interfaces electrificadas.

Principales métodos:

  • Formación de un adducto ácido-base de Lewis utilizando mercaptopiridina (base de Lewis) y trifluoruro de boro (BF3, ácido de Lewis) en un electrodo.
  • Mediciones electroquímicas para estudiar la estabilidad y la escisión del adducto a diferentes potenciales.
  • Investigación de la reversibilidad utilizando el electrolito Li+BF4.

Principales resultados:

  • Se formó un enlace de Lewis estable (N-B) entre la mercaptopiridina y BF3 en una superficie de electrodo.
  • El enlace N-B se escindía a potenciales negativos de aproximadamente -0,3 V frente a Ag/AgCl sin corriente.
  • La escisión fue totalmente reversible cuando se suministró BF3 a partir del electrolito Li+BF4.
  • Tanto la electroinducción como los efectos iónicos interfaciales influyen en el enlace N-B.

Conclusiones:

  • Las estructuras iónicas interfaciales y los equilibrios, no solo la electroinducción, impulsan la escisión del enlace de Lewis en potenciales negativos.
  • Este trabajo proporciona información fundamental sobre las interacciones ácido-base de Lewis interfaciales.
  • Los resultados son relevantes para el diseño de sistemas electrocatalíticos y de electroadsorción.