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Related Concept Videos

Solvating Effects02:12

Solvating Effects

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An understanding of the solvating effect helps rationalize the relation between solvation and acidity of the compound. In addition, this also explains the relative stability of conjugate bases for compounds with different pKa values. This lesson details, in-depth, the principle of solvating effects. The strength of an acid and the stability of its corresponding conjugate base are determined using pKa values. This observed relationship is a consequence of solvation, which is the interaction...
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Phosphate Buffer01:22

Phosphate Buffer

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The phosphate buffer system is a critical biological mechanism for maintaining pH stability in the body. This system operates primarily through two components: sodium dihydrogen phosphate (NaH2PO4), which acts as a weak acid, and sodium hydrogen phosphate (Na2HPO4), which serves as a weak base.
Sodium dihydrogen phosphate does not fully dissociate in neutral or acidic solutions. When a strong base, such as sodium hydroxide (NaOH), is introduced into the solution, sodium dihydrogen phosphate...
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Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

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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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Aqueous Solutions and Heats of Hydration02:42

Aqueous Solutions and Heats of Hydration

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Water and other polar molecules are attracted to ions. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. These attractions play an important role in the dissolution of ionic compounds in water.
When ionic compounds dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution because water molecules surround and solvate the ions, reducing the strong electrostatic forces between them. This process...
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Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

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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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Complexation Equilibria: Factors Influencing Stability of Complexes01:09

Complexation Equilibria: Factors Influencing Stability of Complexes

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In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
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Constructing Quasi-Localized High-Concentration Solvation Structures to Stabilize Battery Interfaces in Nonflammable

Chenyang Shi1, Mengran Wang1,2,3,4, Zari Tehrani5

  • 1School of Metallurgy and Environment, Central South University, Changsha, Hunan, 410083, China.

Advanced Science (Weinheim, Baden-Wurttemberg, Germany)
|December 16, 2024
PubMed
Summary
This summary is machine-generated.

Introducing polar carbonate solvents to lithium-ion batteries prevents flame-retardant tris(2,2,2-trifluoroethyl) phosphate (TFEP) from degrading graphite anodes. This strategy enhances battery safety and cycling performance.

Keywords:
battery safetyflame‐retardant electrolytesfluorinated phosphatesmolecular designsolvation shell tuning

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Area of Science:

  • Materials Science
  • Electrochemistry
  • Chemical Engineering

Background:

  • Phosphate-based electrolytes enhance lithium-ion battery safety but face compatibility issues with graphite anodes and high-voltage cathodes.
  • Fluorinated phosphates, commonly used, increase interfacial resistance, leading to performance degradation.

Purpose of the Study:

  • To develop a flame-retardant electrolyte with improved compatibility for graphite anodes and high-voltage cathodes.
  • To enhance the cycling stability and overall performance of lithium-ion batteries using phosphate-based electrolytes.

Main Methods:

  • Incorporation of polar carbonate solvents to modify the solvation structure of lithium ions.
  • Formation of a quasi-localized high-concentration solvation structure to restrict electrolyte reduction.
  • Electrochemical testing of LiNi0.8Mn0.1Co0.1O2 (NCM811) | Graphite (Gr) pouch cells with optimized electrolytes.

Main Results:

  • The optimized electrolyte prevented tris(2,2,2-trifluoroethyl) phosphate (TFEP) from participating in the lithium-ion solvation shell, restricting its reduction.
  • NCM811|Gr pouch cells with the optimized electrolyte showed 80.1% capacity retention after 370 cycles at 0.5C, significantly better than controls (47.1% after 300 cycles).
  • Cells operated at a 4.5V cut-off voltage maintained 82.8% capacity after 125 cycles, outperforming commercial carbonate electrolytes (56.9% after 125 cycles).

Conclusions:

  • The developed quasi-localized high-concentration solvation structure effectively stabilizes the electrode interface.
  • This strategy significantly enhances the cycling performance of phosphate-based flame-retardant electrolytes for safer and more durable lithium-ion batteries.