[{"language":[{"iso":"eng"}],"month":"08","oa_version":"Submitted Version","has_accepted_license":"1","publication":"Nature Chemistry","status":"public","user_id":"2DF688A6-F248-11E8-B48F-1D18A9856A87","file":[{"content_type":"application/pdf","file_name":"Freunberger on Eichhorn.pdf","date_updated":"2020-07-14T12:47:55Z","file_size":286805,"checksum":"76806cff3d5b62f846499a8617cee7ef","date_created":"2020-06-29T15:38:21Z","creator":"sfreunbe","file_id":"8054","access_level":"open_access","relation":"main_file"}],"oa":1,"publication_identifier":{"issn":["1755-4330","1755-4349"]},"type":"journal_article","date_published":"2019-08-19T00:00:00Z","article_type":"letter_note","publisher":"Springer Nature","file_date_updated":"2020-07-14T12:47:55Z","quality_controlled":"1","page":"761-763","intvolume":"        11","title":"Interphase identity crisis","article_processing_charge":"No","date_created":"2020-01-15T12:12:53Z","publication_status":"published","issue":"9","author":[{"id":"A8CA28E6-CE23-11E9-AD2D-EC27E6697425","orcid":"0000-0003-2902-5319","full_name":"Freunberger, Stefan Alexander","first_name":"Stefan Alexander","last_name":"Freunberger"}],"_id":"7282","ddc":["540","547"],"extern":"1","volume":11,"abstract":[{"text":"Interphases that form on the anode surface of lithium-ion batteries are critical for performance and lifetime, but are poorly understood. Now, a decade-old misconception regarding a main component of the interphase has been revealed, which could potentially lead to improved devices.","lang":"eng"}],"day":"19","doi":"10.1038/s41557-019-0311-0","citation":{"ama":"Freunberger SA. Interphase identity crisis. <i>Nature Chemistry</i>. 2019;11(9):761-763. doi:<a href=\"https://doi.org/10.1038/s41557-019-0311-0\">10.1038/s41557-019-0311-0</a>","apa":"Freunberger, S. A. (2019). Interphase identity crisis. <i>Nature Chemistry</i>. Springer Nature. <a href=\"https://doi.org/10.1038/s41557-019-0311-0\">https://doi.org/10.1038/s41557-019-0311-0</a>","chicago":"Freunberger, Stefan Alexander. “Interphase Identity Crisis.” <i>Nature Chemistry</i>. Springer Nature, 2019. <a href=\"https://doi.org/10.1038/s41557-019-0311-0\">https://doi.org/10.1038/s41557-019-0311-0</a>.","ieee":"S. A. Freunberger, “Interphase identity crisis,” <i>Nature Chemistry</i>, vol. 11, no. 9. Springer Nature, pp. 761–763, 2019.","short":"S.A. Freunberger, Nature Chemistry 11 (2019) 761–763.","mla":"Freunberger, Stefan Alexander. “Interphase Identity Crisis.” <i>Nature Chemistry</i>, vol. 11, no. 9, Springer Nature, 2019, pp. 761–63, doi:<a href=\"https://doi.org/10.1038/s41557-019-0311-0\">10.1038/s41557-019-0311-0</a>.","ista":"Freunberger SA. 2019. Interphase identity crisis. Nature Chemistry. 11(9), 761–763."},"year":"2019","date_updated":"2021-01-12T08:12:44Z"},{"quality_controlled":"1","page":"1091-1099","language":[{"iso":"eng"}],"publisher":"Springer Nature","article_type":"original","_id":"7305","publication":"Nature Chemistry","issue":"12","author":[{"first_name":"Lee","last_name":"Johnson","full_name":"Johnson, Lee"},{"first_name":"Chunmei","last_name":"Li","full_name":"Li, Chunmei"},{"full_name":"Liu, Zheng","last_name":"Liu","first_name":"Zheng"},{"full_name":"Chen, Yuhui","last_name":"Chen","first_name":"Yuhui"},{"orcid":"0000-0003-2902-5319","full_name":"Freunberger, Stefan Alexander","first_name":"Stefan Alexander","last_name":"Freunberger","id":"A8CA28E6-CE23-11E9-AD2D-EC27E6697425"},{"last_name":"Ashok","first_name":"Praveen C.","full_name":"Ashok, Praveen C."},{"first_name":"Bavishna B.","last_name":"Praveen","full_name":"Praveen, Bavishna B."},{"full_name":"Dholakia, Kishan","first_name":"Kishan","last_name":"Dholakia"},{"full_name":"Tarascon, Jean-Marie","last_name":"Tarascon","first_name":"Jean-Marie"},{"first_name":"Peter G.","last_name":"Bruce","full_name":"Bruce, Peter G."}],"date_created":"2020-01-15T12:18:18Z","article_processing_charge":"No","publication_status":"published","oa_version":"None","intvolume":"         6","month":"11","title":"The role of LiO2 solubility in O2 reduction in aprotic solvents and its consequences for Li–O2 batteries","volume":6,"status":"public","related_material":{"link":[{"relation":"erratum","url":"https://doi.org/10.1038/nchem.2138"}]},"user_id":"2DF688A6-F248-11E8-B48F-1D18A9856A87","extern":"1","year":"2014","citation":{"chicago":"Johnson, Lee, Chunmei Li, Zheng Liu, Yuhui Chen, Stefan Alexander Freunberger, Praveen C. Ashok, Bavishna B. Praveen, Kishan Dholakia, Jean-Marie Tarascon, and Peter G. Bruce. “The Role of LiO2 Solubility in O2 Reduction in Aprotic Solvents and Its Consequences for Li–O2 Batteries.” <i>Nature Chemistry</i>. Springer Nature, 2014. <a href=\"https://doi.org/10.1038/nchem.2101\">https://doi.org/10.1038/nchem.2101</a>.","ieee":"L. Johnson <i>et al.</i>, “The role of LiO2 solubility in O2 reduction in aprotic solvents and its consequences for Li–O2 batteries,” <i>Nature Chemistry</i>, vol. 6, no. 12. Springer Nature, pp. 1091–1099, 2014.","ama":"Johnson L, Li C, Liu Z, et al. The role of LiO2 solubility in O2 reduction in aprotic solvents and its consequences for Li–O2 batteries. <i>Nature Chemistry</i>. 2014;6(12):1091-1099. doi:<a href=\"https://doi.org/10.1038/nchem.2101\">10.1038/nchem.2101</a>","apa":"Johnson, L., Li, C., Liu, Z., Chen, Y., Freunberger, S. A., Ashok, P. C., … Bruce, P. G. (2014). The role of LiO2 solubility in O2 reduction in aprotic solvents and its consequences for Li–O2 batteries. <i>Nature Chemistry</i>. Springer Nature. <a href=\"https://doi.org/10.1038/nchem.2101\">https://doi.org/10.1038/nchem.2101</a>","ista":"Johnson L, Li C, Liu Z, Chen Y, Freunberger SA, Ashok PC, Praveen BB, Dholakia K, Tarascon J-M, Bruce PG. 2014. The role of LiO2 solubility in O2 reduction in aprotic solvents and its consequences for Li–O2 batteries. Nature Chemistry. 6(12), 1091–1099.","short":"L. Johnson, C. Li, Z. Liu, Y. Chen, S.A. Freunberger, P.C. Ashok, B.B. Praveen, K. Dholakia, J.-M. Tarascon, P.G. Bruce, Nature Chemistry 6 (2014) 1091–1099.","mla":"Johnson, Lee, et al. “The Role of LiO2 Solubility in O2 Reduction in Aprotic Solvents and Its Consequences for Li–O2 Batteries.” <i>Nature Chemistry</i>, vol. 6, no. 12, Springer Nature, 2014, pp. 1091–99, doi:<a href=\"https://doi.org/10.1038/nchem.2101\">10.1038/nchem.2101</a>."},"date_updated":"2021-01-12T08:12:55Z","type":"journal_article","date_published":"2014-11-10T00:00:00Z","day":"10","publication_identifier":{"issn":["1755-4330","1755-4349"]},"doi":"10.1038/nchem.2101","abstract":[{"text":"When lithium–oxygen batteries discharge, O2 is reduced at the cathode to form solid Li2O2. Understanding the fundamental mechanism of O2 reduction in aprotic solvents is therefore essential to realizing their technological potential. Two different models have been proposed for Li2O2 formation, involving either solution or electrode surface routes. Here, we describe a single unified mechanism, which, unlike previous models, can explain O2 reduction across the whole range of solvents and for which the two previous models are limiting cases. We observe that the solvent influences O2 reduction through its effect on the solubility of LiO2, or, more precisely, the free energy of the reaction LiO2* ⇌ Li(sol)+ + O2−(sol) + ion pairs + higher aggregates (clusters). The unified mechanism shows that low-donor-number solvents are likely to lead to premature cell death, and that the future direction of research for lithium–oxygen batteries should focus on the search for new, stable, high-donor-number electrolytes, because they can support higher capacities and can better sustain discharge.","lang":"eng"}]},{"extern":"1","user_id":"2DF688A6-F248-11E8-B48F-1D18A9856A87","status":"public","volume":5,"date_published":"2013-05-12T00:00:00Z","type":"journal_article","date_updated":"2021-01-12T08:12:56Z","year":"2013","citation":{"apa":"Chen, Y., Freunberger, S. A., Peng, Z., Fontaine, O., &#38; Bruce, P. G. (2013). Charging a Li–O2 battery using a redox mediator. <i>Nature Chemistry</i>. Springer Nature. <a href=\"https://doi.org/10.1038/nchem.1646\">https://doi.org/10.1038/nchem.1646</a>","ama":"Chen Y, Freunberger SA, Peng Z, Fontaine O, Bruce PG. Charging a Li–O2 battery using a redox mediator. <i>Nature Chemistry</i>. 2013;5(6):489-494. doi:<a href=\"https://doi.org/10.1038/nchem.1646\">10.1038/nchem.1646</a>","ieee":"Y. Chen, S. A. Freunberger, Z. Peng, O. Fontaine, and P. G. Bruce, “Charging a Li–O2 battery using a redox mediator,” <i>Nature Chemistry</i>, vol. 5, no. 6. Springer Nature, pp. 489–494, 2013.","chicago":"Chen, Yuhui, Stefan Alexander Freunberger, Zhangquan Peng, Olivier Fontaine, and Peter G. Bruce. “Charging a Li–O2 Battery Using a Redox Mediator.” <i>Nature Chemistry</i>. Springer Nature, 2013. <a href=\"https://doi.org/10.1038/nchem.1646\">https://doi.org/10.1038/nchem.1646</a>.","short":"Y. Chen, S.A. Freunberger, Z. Peng, O. Fontaine, P.G. Bruce, Nature Chemistry 5 (2013) 489–494.","mla":"Chen, Yuhui, et al. “Charging a Li–O2 Battery Using a Redox Mediator.” <i>Nature Chemistry</i>, vol. 5, no. 6, Springer Nature, 2013, pp. 489–94, doi:<a href=\"https://doi.org/10.1038/nchem.1646\">10.1038/nchem.1646</a>.","ista":"Chen Y, Freunberger SA, Peng Z, Fontaine O, Bruce PG. 2013. Charging a Li–O2 battery using a redox mediator. Nature Chemistry. 5(6), 489–494."},"abstract":[{"text":"The non-aqueous Li–air (O2) battery is receiving intense interest because its theoretical specific energy exceeds that of Li-ion batteries. Recharging the Li–O2 battery depends on oxidizing solid lithium peroxide (Li2O2), which is formed on discharge within the porous cathode. However, transporting charge between Li2O2 particles and the solid electrode surface is at best very difficult and leads to voltage polarization on charging, even at modest rates. This is a significant problem facing the non-aqueous Li–O2 battery. Here we show that incorporation of a redox mediator, tetrathiafulvalene (TTF), enables recharging at rates that are impossible for the cell in the absence of the mediator. On charging, TTF is oxidized to TTF+ at the cathode surface; TTF+ in turn oxidizes the solid Li2O2, which results in the regeneration of TTF. The mediator acts as an electron–hole transfer agent that permits efficient oxidation of solid Li2O2. The cell with the mediator demonstrated 100 charge/discharge cycles.","lang":"eng"}],"doi":"10.1038/nchem.1646","publication_identifier":{"issn":["1755-4330","1755-4349"]},"day":"12","language":[{"iso":"eng"}],"page":"489-494","quality_controlled":"1","article_type":"original","publisher":"Springer Nature","author":[{"last_name":"Chen","first_name":"Yuhui","full_name":"Chen, Yuhui"},{"id":"A8CA28E6-CE23-11E9-AD2D-EC27E6697425","first_name":"Stefan Alexander","last_name":"Freunberger","orcid":"0000-0003-2902-5319","full_name":"Freunberger, Stefan Alexander"},{"last_name":"Peng","first_name":"Zhangquan","full_name":"Peng, Zhangquan"},{"first_name":"Olivier","last_name":"Fontaine","full_name":"Fontaine, Olivier"},{"last_name":"Bruce","first_name":"Peter G.","full_name":"Bruce, Peter G."}],"issue":"6","_id":"7307","publication":"Nature Chemistry","title":"Charging a Li–O2 battery using a redox mediator","month":"05","intvolume":"         5","oa_version":"None","publication_status":"published","article_processing_charge":"No","date_created":"2020-01-15T12:18:43Z"}]