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Related Concept Videos

Formation of Complex Ions03:45

Formation of Complex Ions

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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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Ionization Energy03:12

Ionization Energy

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The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy (IE1). The first ionization energy for an element, X, is the energy required to form a cation with 1+ charge:
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Common Ion Effect03:24

Common Ion Effect

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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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Ions and Ionic Charges03:27

Ions and Ionic Charges

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In ordinary chemical reactions, the nucleus — which contains the protons and neutrons of each atom and thus identifies the element — remains unchanged. Electrons, however, can be added to atoms by transfer from other atoms, lost by transfer to other atoms, or shared with other atoms. The transfer and sharing of electrons among atoms govern the chemistry of the elements. During the formation of some compounds, atoms gain or lose electrons to form electrically charged particles called...
78.5K
Ions as Acids and Bases02:54

Ions as Acids and Bases

26.2K
Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt’s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:
26.2K
Precipitation of Ions03:11

Precipitation of Ions

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Predicting Precipitation
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
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Vibrational Spectra of a N719-Chromophore/Titania Interface from Empirical-Potential Molecular-Dynamics Simulation, Solvated by a Room Temperature Ionic Liquid
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Unusual Core-Ionization Pathways in Hydrated Na+: A Theoretical K-2V Study.

Stéphane Carniato1

  • 1Laboratoire de Chimie Physique Matière et Rayonnement (LCPMR), CNRS UMR 7614, Sorbonne Université (SU), 4 place Jussieu, Paris 75005, France.

Inorganic Chemistry
|September 9, 2025
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Summary

The study reveals how water molecules alter sodium ion (Na+) electronic structure using K-2V X-ray spectroscopy. Hydration significantly shifts electronic states, influencing charge distribution and orbital behavior in hydrated sodium clusters.

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Area of Science:

  • Atomic and Molecular Physics
  • Physical Chemistry
  • Spectroscopy

Background:

  • X-ray photoelectron spectroscopy (XPS) probes electronic structure.
  • K-2V spectroscopy, a variant of XPS, involves simultaneous core ionization and excitation.
  • Understanding hydrated ions is crucial for chemistry and biology.

Purpose of the Study:

  • Investigate the electronic structure of sodium ions (Na+) in hydrated clusters [Na(H2O)n]+.
  • Analyze the impact of hydration number (n=1-6) on electronic transitions.
  • Elucidate solvation-induced changes in core-level spectra.

Main Methods:

  • One-photon K-2V X-ray photoelectron spectroscopy.
  • Theoretical analysis of electronic structure and spectral features.
  • Correlation of spectral changes with hydration number and molecular arrangement.

Main Results:

  • Domination of spectra by the unusual 1s2 → 1s03s1 transition.
  • Pronounced redistribution of 1s2 → 1s03p1 transition cross sections with hydration.
  • Significant red shifts in K-2V binding energies due to initial and final-state effects.
  • Evidence of cooperative charge transfer from water to Na+ and electron back-donation.
  • Hydration-driven reordering of unoccupied electronic states around the Na+ center.

Conclusions:

  • K-2V spectroscopy effectively probes solvation effects on electronic structure.
  • Hydration significantly modifies Na+ electronic states, approaching neutrality at higher hydration levels.
  • Water molecules play a critical role in screening and electronic state reordering in hydrated ions.