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Related Concept Videos

Formation of Complex Ions03:45

Formation of Complex Ions

25.7K
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...
25.7K
Complexation Equilibria: Overview01:23

Complexation Equilibria: Overview

1.3K
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...
1.3K
Complexation Equilibria: The Chelate Effect01:19

Complexation Equilibria: The Chelate Effect

1.2K
In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
1.2K
Factors Affecting Solubility04:01

Factors Affecting Solubility

36.6K
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:
36.6K
Common Ion Effect03:24

Common Ion Effect

45.8K
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:
45.8K
Complexometric Titration: Ligands00:43

Complexometric Titration: Ligands

2.2K
Different monodentate and polydentate ligands are used as complexing agents in complexometric titration reactions. The formation of complexes by mono- and bidentate ligands involves two or more intermediate steps, limiting their use as complexing agents. In comparison, polydentate ligands can form complexes with metal ions in a single-step process, facilitating sharper end points. This means polydentate ligands, such as amino carboxylic acid derivatives, are most commonly employed in...
2.2K

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Updated: Jan 15, 2026

A Study of the Complexation of MercuryII with Dicysteinyl Tetrapeptides by Electrospray Ionization Mass Spectrometry
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A Study of the Complexation of MercuryII with Dicysteinyl Tetrapeptides by Electrospray Ionization Mass Spectrometry

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Mineral dissolution by dimeric complexes.

Xiaoxu Li1, Qing Guo2, Yatong Zhao1,3

  • 1Physical & Computational Science Directorate, Pacific Northwest National Laboratory, Richland, WA 99354.

Proceedings of the National Academy of Sciences of the United States of America
|October 6, 2025
PubMed
Summary
This summary is machine-generated.

Mineral dissolution, specifically gibbsite, occurs via dimer release, not just monomers. This finding, observed with atomic force microscopy, clarifies mineral dissolution mechanisms in nature and industry.

Keywords:
atomic force microscopydensity functional tight-binding simulationsmachine learningmineral dissolution

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Thermochemical Studies of NiII and ZnII Ternary Complexes Using Ion Mobility-Mass Spectrometry
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Controlling the Size, Shape and Stability of Supramolecular Polymers in Water
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Controlling the Size, Shape and Stability of Supramolecular Polymers in Water

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Thermochemical Studies of NiII and ZnII Ternary Complexes Using Ion Mobility-Mass Spectrometry
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Controlling the Size, Shape and Stability of Supramolecular Polymers in Water
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Area of Science:

  • Geochemistry
  • Materials Science
  • Surface Chemistry

Background:

  • Mineral dissolution is crucial for geochemical cycles and industrial processes.
  • Current models often assume dissolution occurs through monomeric unit detachment.
  • Direct evidence for dissolution mechanisms at the molecular level is scarce.

Purpose of the Study:

  • To investigate the molecular mechanisms of gibbsite dissolution in alkaline solutions.
  • To provide direct experimental evidence for mineral dissolution pathways.
  • To understand the role of polynuclear species in mineral dissolution.

Main Methods:

  • In situ high-speed atomic force microscopy (HS-AFM) for high-resolution imaging of step-edge retreat.
  • Alkaline solution experiments with gibbsite.
  • Density functional tight-binding (DFTB) simulations to calculate detachment activation energies.

Main Results:

  • Gibbsite dissolution in alkaline solutions primarily occurs through the release of aluminate dimers.
  • These dimers subsequently dissociate into monomeric species in solution.
  • Observed dissolution anisotropy is explained by the dimer release mechanism.
  • DFTB simulations support the proposed mechanism by analyzing detachment energies.

Conclusions:

  • Mineral dissolution can occur via polynuclear species, not solely monomers.
  • This discovery refines our understanding of mineral dissolution kinetics.
  • The findings have implications for natural processes and industrial applications involving mineral dissolution.