Hydrogen-bond chemistry in rechargeable batteries

Building a Long-Lifespan Aqueous K-Ion Battery Operating at −35 °C

“…This represents a higher H-bond breakage degree in 10 m KCF 3 COO electrolyte than the 10 m KCF 3 SO 3 electrolyte, resulting in the H 2 O molecule in 10 m KCF 3 COO electrolyte becoming an ice crystal with rich H-bonds more difficult. This result demonstrates that the larger the H-bond breakage degree, the lower the freezing point, which is consistent with previous literature. − In addition to the H-bond breakage degree, we propose that the average ice formation energy can also be used to understand the antifreezing mechanism. The average ice formation energy is defined as the average energy required while moving an H 2 O molecule in aqueous electrolyte into the ice crystal lattice (see the Supporting Information).…”

Fast Reaction Kinetics and Commendable Low‐Temperature Adaptability of Zinc Batteries Enabled by Aprotic Water‐Acetamide Symbiotic Solvation Sheath

“…The thermogravimetric analysis (TGA) confirms the molar ratio of water to Zn(BF 4 ) 2 in Zn(BF 4 ) 2 • 4H 2 O is � 4.4 (Figure S1). Herein, Zn(BF 4 ) The unique amide group (À C=O, -NH 2 ) provides enough sites to interact with water molecules to form hydrogen bond receptors and hydrogen bond donors, [19] which effectively destroys the original hydrogen bond network between water molecules and significantly reduces the freezing point of the electrolytes. In essence, these results demonstrate that the 1ace-1H 2 O electrolyte can operate at extremely wide temperature without the risk of combustion.…”

“…Furthermore, the digital photographs of our five electrolytes shown in Figure S5 after cooling to −40 °C for 4 h show that the 1ace‐0H 2 O, 1ace‐2H 2 O and 0ace‐1H 2 O electrolytes have solidified, whereas the 2ace‐1H 2 O and 1ace‐1H 2 O electrolytes remained liquid, which is consistent with the DSC results. The unique amide group (−C=O, ‐NH 2 ) provides enough sites to interact with water molecules to form hydrogen bond receptors and hydrogen bond donors, [19] which effectively destroys the original hydrogen bond network between water molecules and significantly reduces the freezing point of the electrolytes. In essence, these results demonstrate that the 1ace‐1H 2 O electrolyte can operate at extremely wide temperature without the risk of combustion.…”

An Energetic Aqueous Mn Metal Anode

“…For rechargeable batteries, an expectation generally exists for the cycling CE of the electrode to be 100% to ensure the utmost cycling stability of the full cell. , However, even the most advanced deposition/​dissolution-type metal electrodes currently cannot guarantee a CE of 100%. , The aqueous Mn metal anode, due to a series of severe side reactions, particularly fails to meet these criteria. In the study of aqueous Mn anodes, it is crucial to employ objective and impartial electrochemical protocols for performance evaluation.…”

“…10 Another approach involves the addition of hydrogen bond acceptor-or donor-based organic molecules to break the conventional hydrogen bond network of the aqueous Mn electrolyte, effectively inhibiting HER due to the strong binding energy between organic molecules and water molecules. 49,52 Furthermore, the design of chemically crosslinked hydrogel electrolytes emerges as an essential direction to maximize the suppression of side reactions induced by active water molecules, 34 theoretically providing better stability at the Mn metal electrode−electrolyte interface. Additionally, hydrogels also confer mechanical flexibility to the aqueous Mn anode, expanding its application range.…”