Related Experiment Video
Updated: Jan 29, 2026

05:33
Solid-state Graft Copolymer Electrolytes for Lithium Battery Applications
Published on: August 12, 2013
22.3K
Direct Observation of a Li-Ionic Space-Charge Layer Formed at an Electrode/Solid-Electrolyte Interface
Yuki Nomura1,2,3, Kazuo Yamamoto2, Tsukasa Hirayama2
1Technology Innovation Division, Panasonic Corporation, 3-1-1 Yagumo-naka-machi, Moriguchi, 570-8501, Japan.
Angewandte Chemie (International Ed. in English)
|February 8, 2019
Summary
Researchers visualized ionic and potential profiles in the space-charge layer (SCL) at electrode-solid electrolyte interfaces. This visualization is key for improving ion conduction in next-generation electrochemical devices.
Area of Science:
- Materials Science
- Electrochemistry
- Solid-State Physics
Background:
- Mobile charge carriers redistribute at interfaces between different materials due to potential differences.
- This charge redistribution significantly impacts ion conduction across interfaces, particularly between electrodes and solid electrolytes.
- Understanding ionic carrier distribution and potential is crucial for enhancing interfacial ion transport.
Purpose of the Study:
- To visualize the ionic and potential profiles within the space-charge layer (SCL) at the interface between a copper electrode and a lithium-conductive solid electrolyte.
- To investigate the role of charge redistribution in interfacial phenomena relevant to electrochemical devices.
Main Methods:
- Utilized phase-shifting electron holography for visualization.
- Employed spatially resolved electron energy-loss spectroscopy for detailed analysis.
- Focused on electron microscopy techniques to probe the nanoscale interface.
Main Results:
- Successfully visualized the Li-ionic space-charge layer (SCL) at the Cu/solid electrolyte interface.
- Observed a significant potential drop of 1.3 V within 10 nm of the interface.
- Demonstrated the capability of the applied electron microscopy techniques to map ionic and potential distributions.
Conclusions:
- The study provides direct visualization of the ionic and potential profiles in the SCL.
- These findings offer critical insights into interfacial charge transport mechanisms.
- The applied techniques hold potential for advancing the development of next-generation electrochemical devices, such as solid-state batteries.
Related Concept Videos
Molecular and Ionic Solids
20.0K
Crystalline solids are divided into four types: molecular, ionic, metallic, and covalent network based on the type of constituent units and their interparticle interactions.
Molecular Solids
Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...
Molecular Solids
Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...
20.0K
Ions and Ionic Charges
79.0K
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...
79.0K
Electrolyte and Nonelectrolyte Solutions
71.8K
Substances that undergo either a physical or a chemical change in solution to yield ions that can conduct electricity are called electrolytes. If a substance yields ions in solution, that is, if the compound undergoes 100% dissociation, then the substance is a strong electrolyte. Complete dissociation is indicated by a single forward arrow. For example, water-soluble ionic compounds like sodium chloride dissociate into sodium cations and chloride anions in aqueous solution.
71.8K
Ionic Radii
33.5K
Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it is smaller than the atom from which it is derived. For example, the covalent radius of an aluminum atom (1s22s22p63s23p1) is 118 pm, whereas the ionic radius of an Al3+ (1s22s22p6) is 68 pm. As electrons are removed from the outer valence shell, the remaining core electrons occupying smaller shells experience a greater effective nuclear...
33.5K
Electrolytes: van't Hoff Factor
36.5K
Colligative Properties of Electrolytes
The colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one...
The colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one...
36.5K
Ionic Crystal Structures
17.0K
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.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
17.0K

