Related Experiment Video
Updated: May 26, 2025

06:58
Zinc-Sponge Battery Electrodes that Suppress Dendrites
Published on: September 29, 2020
4.3K
Enabling Solid-Electrolyte Interphase Formation Prior to Water Reduction in Aqueous Zinc Batteries by Mild Protic
Taiqiang Chen1, Yunfei Wang1, Xin Li1
1School of Materials and Chemistry, University of Shanghai for Science and Technology, Shanghai, 200093, China.
Angewandte Chemie (International Ed. in English)
|February 22, 2025
Summary
This study introduces 2-mercapto-1-methylimidazole (MMI) to form a protective solid-electrolyte interphase (SEI) on zinc anodes in aqueous zinc batteries (AZBs). The MMI-derived SEI effectively prevents water decomposition and dendrite formation, enhancing battery performance.
Area of Science:
- Electrochemistry
- Materials Science
- Energy Storage
Background:
- Aqueous zinc batteries (AZBs) face challenges like hydrogen evolution reaction (HER) and zinc anode dendrite formation, hindering practical application.
- These issues stem from the lack of an effective passivating solid-electrolyte interphase (SEI) that can prevent water decomposition.
- In situ SEI construction prior to water reduction is crucial for stable AZB operation.
Purpose of the Study:
- To investigate the potential of protic solid-electrolyte interphase (SEI) chemistry for aqueous zinc batteries.
- To introduce 2-mercapto-1-methylimidazole (MMI) as a precursor for forming a protective SEI on zinc anodes.
- To evaluate the effectiveness of the MMI-derived SEI in suppressing side reactions and improving zinc anode stability.
Main Methods:
- Thermodynamic prediction of reduction potentials for mild protic compounds.
- Electrochemical evaluation of 2-mercapto-1-methylimidazole (MMI) reduction prior to water.
- Analysis of the SEI composition (organic compounds and Zn(OH)2) formed from MMI reduction on zinc anodes.
- Corrosion current measurements to assess the passivating effect of the MMI-derived SEI.
Main Results:
- 2-mercapto-1-methylimidazole (MMI) was found to reduce before water due to its higher proton activity, forming an SEI via a ring cleavage mechanism.
- The MMI-derived SEI significantly reduced the corrosion current of zinc anodes by two orders of magnitude (from 1170 to 13.6 μA cm⁻²).
- The SEI effectively suppressed hydrogen evolution reaction (HER) and ensured dendrite-free zinc deposition.
Conclusions:
- The MMI-derived SEI provides a superior passivating effect, crucial for stable zinc anodes in AZBs.
- This protic SEI strategy effectively suppresses detrimental side reactions like HER and dendrite formation.
- The study demonstrates a promising approach for developing high-performance and reversible zinc anodes for AZBs.
Related Concept Videos
Standard Electrode Potentials
43.2K
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...
43.2K
Formation of Complex Ions
23.2K
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...
23.2K
Electrolysis
25.9K
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...
25.9K
Voltaic/Galvanic Cells
56.5K
Spontaneous Chemical Reactions
Spontaneous redox reactions occur abundantly in nature. The chemical reaction occurring in a disposable AA battery powering our remote controls is one such example of a spontaneous redox reaction. Another example is the immersion of coiled copper wire into an aqueous silver nitrate solution. The reaction shows a gradual, visually impressive color change from colorless to bright blue and the formation of a grey precipitate on the copper wire. In this experiment,...
Spontaneous redox reactions occur abundantly in nature. The chemical reaction occurring in a disposable AA battery powering our remote controls is one such example of a spontaneous redox reaction. Another example is the immersion of coiled copper wire into an aqueous silver nitrate solution. The reaction shows a gradual, visually impressive color change from colorless to bright blue and the formation of a grey precipitate on the copper wire. In this experiment,...
56.5K
Electrodeposition
567
Electrodeposition is a technique used to separate an analyte from interferents by electrochemical processes. Here, the analyte is a metal ion that can be deposited on an electrode immersed in the sample solution. The electrochemical setup consists of an anode and a cathode. When an electric current is applied to the setup, oxidation occurs at the anode. At the cathode, which consists of a large metal surface, metal ions undergo reduction and deposit onto the surface.
Electrodeposition can...
Electrodeposition can...
567
Concentration Cells
22.2K
A concentration cell is a type of a voltaic cell constructed by connecting two almost identical half-cells, both based on the same half-reaction and using the same electrode, differing only in the concentration of one redox species. A concentration cell's potential, therefore, is determined only by the concentration difference of the particular redox species.
Consider the following voltaic cell:
Consider the following voltaic cell:
22.2K

