As an inexpensive and high capacity oxidant, electrolytic manganese dioxide (γ-MnO 2 ) is of interest as a cathode for secondary aqueous batteries. Electrochemical behavior of γ-MnO 2 was characterized in aqueous 5.0 M KOH and LiOH solutions, and found to depend strongly upon cation identity. In LiOH and mixed LiOH / KOH solutions, Li-ion intercalation appeared to operate in competition with proton intercalation, being favored at higher [Li + ] and, for mixed electrolytes, lower sweep rates. Electrochemical and in situ X-ray diffraction data indicated that γ-MnO 2 underwent a chemically irreversible transformation upon the first reduction in LiOH solution, while in KOH solution, structure was largely unchanged after the first cycle. These experiments with γ-MnO 2 as well as with a closely-related, ramsdellite-like sample, suggest that depending on sample morphology/rate capability, the irreversible process proceeds either through a solid-solution reaction or a two-phase reaction followed by a solid-solution reaction. While discharge capacity and capacity retention during galvanostatic cycling of γ-MnO 2 were worse in LiOH than in KOH solution, some improvement was noted in a mixed LiOH/KOH solution. Electrolytic manganese dioxide (EMD or ε/γ-MnO 2 ) is the material most commonly employed as the cathode in primary alkaline batteries and primary non-aqueous lithium cells owing to its relatively low cost, low toxicity, high reduction potential, and high gravimetric capacity. Unfortunately, MnO 2 -based secondary cells tend to have limited cycle life, due to the conversion of active material into electrochemically inactive or electronically resistive phases, such as hausmannite (Mn 3 O 4 ) or hetaerolyte (ZnMn 2 O 4 ) in aqueous cells, 1,2 and to pulverization associated with large changes in volume with state of charge.3 Under certain conditions, however, γ-MnO 2 can be cycled with relatively good capacity retention. Major criteria for reversible cycling are to limit the depth of discharge to minimize the solubility of manganese in lower oxidation states, and to avoid the formation of soluble high oxidation state species during charging (i.e. MnO 4 2− ). 4,5,6,7 It has also been reported that the use of LiOH instead of KOH as the electrolyte can improve the cycle life of γ-MnO 2 . 8 The structure of γ-MnO 2 is highly defective both in terms of type and concentration of defects. According to the De Wolff model, the structure is thought to be an intergrowth of ramsdellite and pyrolusite layers (Fig. 1).9,10 Both phases have tunnel-structures, as is apparent from the viewpoint in Fig. 1. γ-MnO 2 also contains microtwinning defects, which introduce kinks to the tunnel structure.10 Manganese vacancies can also be present and necessitate the incorporation of protons (Ruetschi protons) in the structure to maintain charge balance.
12In aqueous KOH or NH 4 Cl media (in the case of a Leclanché cell), the reduction of the Mn 4+ to Mn 3+ is accompanied by the incorporation of protons into the tunnels in the structure (along th...