電気化学的エネルギー貯蔵のための固有微孔性の溶液処理可能なリドックス活性ポリマー
Anqi Wang1, Rui Tan1, Charlotte Breakwell2
1Department of Chemical Engineering, Imperial College London, London SW7 2AZ, U.K.
Journal of the American Chemical Society
|September 8, 2022
まとめ
リチウムイオン電池の新型リドックス活性ポリマー (PIM) は,リチウムイオン電池のソリューションを提供します. これらの材料は溶解性や加工問題を克服し 安定して効率的なエネルギー貯蔵を可能にします
科学分野:
- 材料科学
- 電気化学
- ポリマー化学
背景:
- エネルギー貯蔵のための無機電極の代替品として,レドックス活性有機物質が調査されています.
- 難題には,溶解性,遅い充電/質量輸送,有機物質の複雑な処理が含まれています.
研究 の 目的:
- リチウムイオン電池の性能を改善するために,内在微孔性のリドックス活性ポリマー (PIM) を開発する.
- 分子工学による従来の有機電極材料の限界に対処する.
主な方法:
- カルボニル基のリドックスサイトを持つ内在微孔性の合成されたリドックス活性ポリマー (PIMs).
- 薄膜とポリマー-炭素複合材料を作るための溶液処理技術を使用した.
- リチウムイオン輸送と貯蔵を研究した PIM の多孔構造.
主要な成果:
- 開発されたPIMは,高速イオン輸送を容易にするオープンで微細なネットワークを示しています.
- レドックス活性PIMは,電解質溶剤に溶けず,溶液処理が可能である.
- 溶液処理されたPIMから作られた電極は,容量低下のないリチウムイオン電池のサイクル性能を向上させました.
結論:
- レドックス活性型PIMは,先進的なエネルギー貯蔵ソリューションのための有望な材料プラットフォームを提供します.
- 固有の微小孔性,酸化還元活性,および溶液処理性の組み合わせが鍵となる.
- これらの材料は 電池やセンサーや電子機器に 応用できる可能性があります
さらに関連する動画
05:47Preparation of Polyoxometalate-based Photo-responsive Membranes for the Photo-activation of Manganese Oxide Catalysts
Published on: August 7, 2018
7.8K
06:53Author Spotlight: Magnetometric Characterization of Intermediates in the Solid-State Electrochemistry of Redox-Active Metal-Organic Frameworks
Published on: June 9, 2023
2.1K
関連する概念動画
Batteries and Fuel Cells
24.1K
A battery is a galvanic cell that is used as a source of electrical power for specific applications. Modern batteries exist in a multitude of forms to accommodate various applications, from tiny button batteries such as those that power wristwatches to the very large batteries used to supply backup energy to municipal power grids. Some batteries are designed for single-use applications and cannot be recharged (primary cells), while others are based on conveniently reversible cell reactions that...
24.1K
Electrolysis
22.8K
In a galvanic cell, the electrical work is done by a redox system on its surroundings as electrons produced by the spontaneous redox reactions are transferred through an external circuit. Alternatively, an external circuit does work on a redox system by imposing a voltage sufficient to drive an otherwise nonspontaneous reaction in a process known as electrolysis. For instance, recharging a battery involves the use of an external power source to drive the spontaneous (discharge) cell reaction in...
22.8K
Electrochemical Systems
179
Electrochemical systems provide a fascinating insight into the dynamic interplay of charged species within various phases. One notable example is the interaction between a membrane permeable to K⁺ ions but not to Cl⁻ ions, separating an aqueous KCl solution from pure water. As K⁺ ions diffuse through the membrane, they generate net charges on each phase, leading to a potential difference between them.Similarly, when a piece of Zn is immersed in an aqueous ZnSO₄ solution,...
179
Electrochemical Cells
405
Electrochemical cells are systems that convert chemical energy into electrical energy or use electrical energy to drive chemical reactions. They consist of two electrodes in contact with an electrolyte, where redox reactions enable electron transfer. Most electrochemical cells include two half-cells connected by an external wire for electron flow and a salt bridge for ion flow. The salt bridge contains an electrolyte solution and maintains charge neutrality by allowing ions—not...
405
The Electrical Double Layer
241
In the region where two bulk phases meet, an intricate electric charge distribution arises due to charge transfer, ion adsorption, molecular orientation, and charge distortion. This complex distribution is commonly referred to as the electrical double layer.When a solid electrode interfaces with ions in an electrolyte solution, the speed of electron transfer dictates the rates of oxidation and reduction. The electrode acquires a charge through the escape of atoms into the solution as cations or...
241
Processes at Electrodes
98
The electrode interacts with ions in the electrolyte solution at its interface. The rate of oxidation and reduction depends on the speed at which electrons can transfer through this interface. As ions attach to or leave the electrode surface, the electrode acquires a charge, and an electrical potential forms across the interface, making the process more difficult to reach equilibrium. The charge on the electrode affects the local ion concentrations in the solution, though thermal motion...
98
