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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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EDTA titrations are usually carried out in highly basic conditions, where the fully deprotonated form of EDTA, Y4−, actively complexes with the free metal ions in the solution. Several metal ions precipitate as hydrous oxide (hydroxides, oxides, or oxyhydroxides) under these conditions, lowering the concentration of free metal ions in the solution. For this reason, auxiliary complexing agents or ligands such as ammonia, tartrate, citrate, or triethanolamine are used in EDTA titrations to...
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Metal ions can be separated from one another by complexation with organic ligands–the chelating agent– to form uncharged chelates. Here, the chelating agent must contain hydrophobic groups and behave as a weak acid, losing a proton to bind with the metal. Since most organic ligands used in this process are insoluble or undergo oxidation in the aqueous phase, the chelating agent is initially added to the organic phase and extracted into the aqueous phase. The metal-ligand complex is...
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On comparing the reactivity of silver and lead, it is observed that the two ionic species, Ag+ (aq) and Pb2+ (aq), show a difference in their redox reactivity towards copper: the silver ion undergoes spontaneous reduction, while the lead ion does not. This relative redox activity can be easily quantified in electrochemical cells by a property called cell potential. This property is commonly known as cell voltage in electrochemistry, and it is a measure of the energy which accompanies the charge...
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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.
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Critical Solvation Structures Arrested Active Molecules for Reversible Zn Electrochemistry.

Junjie Zheng1,2, Bao Zhang3, Xin Chen1,2

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Researchers developed a new strategy for aqueous zinc-ion batteries (AZIBs) using acetonitrile to prevent side reactions and dendrites. This method stabilizes the zinc anode, enabling long-lasting and efficient energy storage.

Keywords:
Arrest active moleculeCritical solvationHelmholtz layerReversible zinc anodeZinc-ion battery

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Area of Science:

  • Electrochemistry
  • Materials Science
  • Energy Storage

Background:

  • Aqueous zinc-ion batteries (AZIBs) offer safe and economical energy storage.
  • Zinc anode instability, including side reactions and dendrites, limits AZIB performance.

Purpose of the Study:

  • To develop a critical solvation strategy for reversible zinc electrochemistry in AZIBs.
  • To enhance the stability and cycle life of zinc anodes in aqueous electrolytes.

Main Methods:

  • Introducing acetonitrile as a polar molecule to form a "catcher" for active molecules.
  • Stabilizing the [Zn(H2O)6]2+ solvation structure to inhibit free water molecules.
  • Investigating the desolvation process at the zinc anode interface.

Main Results:

  • Achieved stable cycling for 2250 hours in Zn||Zn symmetric batteries at 1 mAh cm-2.
  • Demonstrated 99.2% capacity retention over 10,000 cycles in Zn||V6O13 full batteries at 10 A g-1.
  • Successfully inhibited dendrite formation and side reactions at the zinc anode.

Conclusions:

  • The critical solvation strategy effectively stabilizes zinc electrochemistry in AZIBs.
  • Acetonitrile acts as a "catcher" to ensure stable Zn2+ desolvation and prevent detrimental side reactions.
  • This approach provides a pathway for developing high-performance and durable AZIBs.