Magnesium battery

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Magnesium batteries are batteries that utilize magnesium cations as the active charge transporting agent in solution and as the elemental anode of an electrochemical cell. Both non-rechargeable primary cell and rechargeable secondary cell chemistries have been investigated. Magnesium primary cell batteries have been commercialised and have found use as reserve and general use batteries.

Magnesium secondary cell batteries are an active topic of research, specifically as a possible replacement or improvement over lithium-ion–based battery chemistries in certain applications. A significant advantage of magnesium cells is their use of a solid magnesium anode, allowing a higher energy density cell design than that made with lithium, which in many instances requires an intercalated lithium anode. Insertion type anodes ('magnesium ion') have also been researched.

Primary cells[edit]

Primary magnesium cells have been developed since the early 20th century. A number of chemistries for reserve battery types have been researched, with cathode materials including silver chloride, copper(I) chloride, palladium(II) chloride, copper(I) iodide, copper(I) thiocyanate, manganese dioxide and air (oxygen).[1] For example, a water activated silver chloride/magnesium reserve battery became commercially available by 1943.[2]

The magnesium dry battery type BA-4386 was fully commercialised, with costs per unit approaching that of zinc batteries – in comparison to equivalent zinc-carbon cells the batteries had greater capacity by volume, and longer shelf life. The BA-4386 was widely used by the US military from 1968 until c.1984 when it was replaced by a lithium thionyl chloride battery.[3][4]

A magnesium–air fuel cell has theoretical operating voltages of 3.1 V and energy densities of 6.8 kWh/kg. General Electric produced a magnesium air fuel cell operating in neutral NaCl solution as early as the 1960s. The magnesium air battery is a primary cell, but has the potential to be 'refuelable' by replacement of the anode and electrolyte. Magnesium air batteries have been commercialised and find use as land based backup systems as well as undersea power sources, using seawater as the electrolyte.[5] The Mark 44 torpedo uses a water-activated magnesium battery.

Secondary cells[edit]


Magnesium is under research as a possible replacement or improvement on lithium-ion battery in certain applications: In comparison to lithium as an anode material magnesium has a (theoretical) energy density per unit mass under half that of lithium (18.8 MJ/kg vs. 42.3 MJ/kg), but a volumetric energy density around 50% higher (32.731 GJ/m3 vs. 22.569 GJ/m3).[note 1][note 2][6] In comparison to metallic lithium anodes, magnesium anodes do not exhibit dendrite formation,[7] which may allow magnesium metal to be used without an intercalation compound at the anode;[note 3] the ability to use a magnesium anode without an intercalation layer raises the theoretical maximum relative volumetric energy density to around 5 times that of a lithium ion cell.[9] Additionally, modeling and cell analysis have indicated that magnesium based batteries may have a cost advantage over lithium due to the abundance of magnesium on earth and the relative scarcity of lithium deposits.[6][7]

Potential use of a Mg-based battery had been recognised as early as the 1990s based on a V2O5, TiS2, or Ti2S4 cathode materials and magnesium metal anodes. However observation of instabilities in the discharge state and uncertainties on the role of water in the electrolyte limited progress was reported.[10][11] The first successful rechargeable cell was reported in 2000, based on Chevrel-type Mo6S8 cathode with a magnesium organohaloaluminate / THF based electrolyte.[12]

As of 2018 secondary magnesium battery research had not produced a commercialisable battery, with specific challenges being the electrolytes and cathode materials.[6][13] As of 2015 the barriers to producing a commercially useful magnesium battery were the lack of demonstrated practical electrolytes and high energy density cathode materials for magnesium ions.[6]


Anodes and electrolytes[edit]

A key drawback to using a metallic magnesium anode is the tendency to form a passivating (non conducting) layer when recharging, blocking further charging (in contrast to lithium's behaviour);[14] The passivating layers were thought to originate from decomposition of the electrolyte during magnesium ion reduction. Common counter ions such as perchlorate and tetrafluoroborate were found to contribute to passivation, as were some common polar aprotic solvents such as carbonates and nitriles.[15]

Early attempts to develop magnesium batteries explored the use of 'magnesium insertion electrodes', based on reversible insertion of magnesium metal into metal alloy anode (such as Bismuth/Antinomy or Tin).[16] These have been shown to be able to prevent anode surface passivation, but suffered from anode destruction due to volumetric changes on insertion, as well as slow kinetics of insertion.

Examples of insertion anode types researched include Sn, Mg2Sn.[17][18][19]

Grignard based ethereal electrolytes have been shown not to passivate;[20] Magnesium organoborates also showed electroplating without passivation. The compound Mg(BPh2Bu2)2 was used in the first demonstrated rechargeable magnesium battery, its usefulness was limited by electrochemical oxidation (i.e. a low anodic limit of the voltage window).[21] Other electrolytes researched include borohydrides, phenolates, alkoxides, amido based complexes (e.g. based on hexamethyldisilazane), carborane salts, fluorinated alkoxyborates, a Mg(BH4)(NH2) solid state electrolyte, and gel polymers containing Mg(AlCl2EtBu)2 in tetraglyme/PVDF.[22][23]

The current wave of interest in magnesium-metal batteries started in 2000, when an Israeli group reported reversible magnesium plating from mixed solutions of magnesium chloride and aluminium chloride in ethers, such as THF.[24][25] The primary advantage of this electrolyte is a significantly larger positive limit of the voltage window (and, thus, a higher battery voltage) than of the previously reported Mg plating electrolytes. Since then, several other Mg salts, less corrosive than chloride, have been reported.[26]

One drawback compared to lithium is magnesium's higher charge (+2) in solution, which tends to result in increased viscosity and reduced mobility in the electrolyte.[27] In solution a number of species may exist depending on counter ions/complexing agents – these often include singly charged species (e.g. MgCl+ in the presence of chloride) – though dimers are often formed (e.g. Mg2Cl3+ ).[28] The movement of the magnesium ion into cathode host lattices is also (as of 2014) problematically slow.[29]

In 2018 a chloride free electrolyte together with a quinone based polymer cathode demonstrated promising performance, with up to 243 Wh (870 kJ) per kg energy density, up to 3.4 kW/kg power density, and up to 87% retention at 2,500 cycles. The absence of chloride in the electrolyte was claimed to improve ion kinetics, and so reduce the amount of electrolyte used, increasing performance density figures.[30]

A promising approach could be the combination of a Mg anode with a sulfur/carbon cathode.[31] Therefore, a non-nucleophilic electrolyte is necessary which does not convert the sulfur into sulfide just by its reducing properties. Such electrolytes have been developed on the basis of chlorine containing [32][33][34] and chlorine-free complex salts.[23] The electrolyte in [23] is a Mg salt containing Mg cation and two boron-hexafluoroisoproplylate groups as anions. This system is easy to synthesize, it shows an ionic conductivity similar to that of Li ion cells, its electrochemical stability window is up to 4.5 V, it is stable in air and versatile towards different solvents.[35]

Cathode materials[edit]

For cathode materials a number of different compounds have been researched for suitability, including those used in magnesium primary batteries. New cathode materials investigated or proposed include zirconium disulfide, cobalt(II,III) oxide, tungsten diselenide, vanadium pentoxide and vanadate based cathodes. Cobalt based spinels showed inferior kinetics to insertion compared to their behaviour with lithium.[6][1] In 2000 the chevrel phase form of Mo6S8 was shown to have good suitability as a cathode, enduring 2000 cycles at 100% discharge with a 15% loss; drawbacks were poor low temperature performance (reduced Mg mobility, compensated by substituting Selenium), as well as a low voltage, c. 1.2V, and low energy density (110mAh/g).[6] A molybdenum disulfide cathode showed improved voltage and energy density, 1.8V and 170mAh/g. Transition metal sulfides are considered promising candidates for magnesium ion battery cathodes.[36] A hybrid magnesium cell using a mixed magnesium/sodium electrolyte with sodium insertion into a nanocrystalline iron(II) disulfide cathode was reported in 2015.[37]

Manganese dioxide based cathodes have shown good properties, but deteriorated on cycling.[38] Modified manganese-based spinels ("post spinels") are an active topic of research (2014) for magnesium-ion insertion cathodes.[39]

In 2014 a rechargeable magnesium battery was reported utilising an ion exchanged, olivine type MgFeSiO4 cathode with a bis(trifluoromethylsulfonyl)imide/triglyme electrolyte – the cell showed a capacity of 300mAh/g with a voltage of 2.4V.[40] MgMnSiO4 has also been investigated as a potential Mg2+ insertion cathode.[41]

Cathodic materials other than non-inorganic metal oxide/sulfide types have also been investigated : in 2015 a cathode based on a polymer incorporating anthraquinone was reported;[42] and other organic, and organo-polymer cathode materials capable of undergoing redox reactions have also been investigated, such as poly-2,2'-dithiodianiline.[43] Quinone based cathodes also formed the cathode a high energy density magnesium battery reported by researchers in 2019.[30]

In 2016 a porous carbon/iodine combination cathode was reported as a potential alternative to Mg2+ insertion cathodes - the chemistry was reported as being potentially suitable for a rechargeable flow battery.[44]


In Oct 2016, Honda and Saitec (Saitama Industrial Technology Center) claimed to have a commercialisable Mg battery, based on a xerogel cathode of vanadium pentoxide/sulfur.[45][46] A commercialisation date of 2018 was also claimed.[45][needs update]

See also[edit]


  1. ^ Li: Standard electrode potential −3.04; cationic charge +1; Faraday constant 96485.33289 C/mol; Energy per mole 293315.411986 J/mol; Atomic mass 6.94 g/mol; Energy density (mass) 42264.4685858 J/g; density 0.534 g/cm3; energy density (volumetric) 22569.2262248 J/cm3
  2. ^ Mg: Standard electrode potential −2.372; cationic charge +2; Faraday constant 96485.33289 C/mol; Energy per mole 457726.41923 J/mol; Atomic mass 24.305 g/mol; Energy density (mass) 18832.6031364 J/g; density 1.738 g/cm3; energy density (volumetric) 32731.0642511 J/cm3
  3. ^ The requirement to intercalate the 'metallic' lithium greatly reduces the energy density of a lithium-ion battery compared to a metallic lithium battery i.e. 372 mAh/g vs. 3862 mAh/g (or 837 mAh/cm3 vs. 2061 mAh/cm3) for lithium/graphite (as LiC6) vs. Li metal.[6][8]


  1. ^ a b Mohtadi & Mizuno 2014, §3.
  2. ^ Blake, Ivan C. (August 1952), "Silver Chloride-Magnesium Reserve Battery", Journal of the Electrochemical Society, 99 (8): 202C, doi:10.1149/1.2779735
  3. ^ Crompton, Thomas Roy (2000), Battery Reference Book, §39
  4. ^ Office, U. S. Government Accountability (26 Sep 1985), Army's Procurement of Batteries: Magnesium vs. Lithium, US Government Accountability Office
  5. ^ Zhang, Tianran; Tao, Zhanliang; Chen, Jun (Mar 2014), "Magnesium–air batteries: From principle to application", Materials Horizons, 1 (2): 196–206, doi:10.1039/c3mh00059a
  6. ^ a b c d e f g Gerbrand Ceder, Pieremanuele Canepa (February 2017), "Odyssey of Multivalent Cathode Materials: Open Questions and Future Challenges" (PDF), Chemical Reviews, 117 (5): 4287–4341, doi:10.1021/acs.chemrev.6b00614, PMID 28269988
  7. ^ a b Mohtadi & Mizuno 2014, p.1292, col.2.
  8. ^ Mohtadi & Mizuno 2014, p.1292, col.1.
  9. ^ Orikasa et al 2014, Introduction.
  10. ^ Novak, Petr; Shklover, V.; Nesper, R. (1994). "Magnesium Insertion in Vanadium Oxides: A Structural Study". Zeitschrift für Physikalische Chemie. 185: 51–68. doi:10.1524/zpch.1994.185.part_1.051. S2CID 101615877.
  11. ^ Bruce, Peter; Krok, F.; Nowinski, Jan; Gibson, Vernon; Tavvakoli, K (1991). "Chemical intercalation of magnesium into solid hosts". Journal of Materials Chemistry. 1 (4): 705–706. doi:10.1039/JM9910100705.
  12. ^ Aurbach, Doron; Lu, Z.; Schecter, A.; Gizbar, H; Turgeman, R.; Cohen, Y.; Moskovich, M.; Levi, E. (2000). "Prototype systems for rechargeable magnesium batteries". Nature. 407 (6805): 724–727. Bibcode:2000Natur.407..724A. doi:10.1038/35037553. PMID 11048714. S2CID 4394214.
  13. ^ Mohtadi & Mizuno 2014, Conclusion, p.1309.
  14. ^ Bucur, Claudiu B.; Gregory, Thomas; Oliver, Allen G.; Muldoon, John (2015), "Confession of a Magnesium Battery", J. Phys. Chem. Lett., 6 (18): 3578–3591, doi:10.1021/acs.jpclett.5b01219, PMID 26722727
  15. ^ Mohtadi & Mizuno 2014, § 1.1.
  16. ^ Mohtadi & Mizuno 2014, §1.2.
  17. ^ Singh, N; Arthur, Timothy S.; Ling, C.; Matsui, M.; Mizuno, F. (2013). "A high energy-density tin anode for rechargeable magnesium-ion batteries". Chemical Communications. 49 (2): 149–151. doi:10.1039/c2cc34673g. PMID 23168386. S2CID 13471874.
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  19. ^ Nguyen, D.-T.; Song, S.-W. (2017). "Magnesium stannide as a high-capacity anode material for magnesium-ion batteries". Journal of Power Sources. 368: 11–17. doi:10.1016/j.jpowsour.2017.09.054.
  20. ^ Mohtadi & Mizuno 2014, §2; Fig.1, p.1293.
  21. ^ Mohtadi & Mizuno 2014, §2.
  22. ^ Mohtadi & Mizuno 2014, Table 1, p.1298.
  23. ^ a b c Zhao-Karger, Zhirong; Bardaji, Maria Elisa Gil; Fuhr, Olaf; Fichtner, Maximilian (2017). "A new class of non-corrosive, highly efficient electrolytes for rechargeable magnesium batteries". Journal of Materials Chemistry A. 5 (22): 10815–10820. doi:10.1039/C7TA02237A. ISSN 2050-7496. S2CID 99093669.
  24. ^ Aurbach, D.; Lu, Z.; Schechter, A.; Gofer, Y.; Gizbar, H.; Turgeman, R.; Cohen, Y.; Moshkovich, M.; Levi, E. (2000). "Prototype systems for rechargeable magnesium batteries". Nature. 407 (6805): 724–727. Bibcode:2000Natur.407..724A. doi:10.1038/35037553. PMID 11048714. S2CID 4394214.
  25. ^ Mohtadi & Mizuno 2014, §2 "In the early 2000, Aurbach et al. reported a breakthrough which constituted preparing an electrolyte with higher oxidative stability (2.5 V vs Mg) than the organoborates (1.9 V vs Mg for Mg(BPh2Bu2)2) by combining a Grignard reagent with aluminum-based Lewis acids ". p.1296, col.2.
  26. ^ Mohtadi & Mizuno 2014, §2.1.
  27. ^ Van Noorden, Richard (5 Mar 2014), "The rechargeable revolution: A better battery",, 507 (7490), pp. 26–28, Bibcode:2014Natur.507...26V, doi:10.1038/507026a, PMID 24598624
  28. ^ Mohtadi & Mizuno 2014, §2.1.5.
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  31. ^ Zhao-Karger, Zhirong; Fichtner, Maximilian (2019). "Beyond Intercalation Chemistry for Rechargeable Mg Batteries: A Short Review and Perspective". Frontiers in Chemistry. 6: 656. doi:10.3389/fchem.2018.00656. ISSN 2296-2646. PMC 6341060. PMID 30697538.
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  36. ^ Mohtadi & Mizuno 2014, §3.3.
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  38. ^ Mohtadi & Mizuno 2014, §3.4.
  39. ^ Example sources:
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  • Mohtadi, Rana; Mizuno, Fuminori (2014), "Magnesium batteries: Current state of the art, issues and future perspectives", Beilstein J. Nanotechnol., 5: 1291–1311, doi:10.3762/bjnano.5.143, PMC 4168907, PMID 25247113
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