| Home | E-Submission | Sitemap | Login | Contact Us |  
J. Korean Ceram. Soc. > Volume 54(1); 2017 > Article
Kim, Shin, Ko, Lee, Woo, Kim, and Yoon: Functional Li-M (Ti, Al, Co, Ni, Mn, Fe)-O Energy Materials


Many new functional materials have been studied for efficient production and storage of energy. Many new materials such as sodium-based and sulfide-based materials have been proposed for energy storage, but research on Li batteries is still dominant. Due to the influence of environmental concerns regarding nuclear energy, interest in and research on fusion power are steadily increasing. For the commercialization of nuclear fusion, a design standard based on a considerable level of physical analysis and modeling is proposed. Nevertheless, limitations of existing materials in nuclear fusion environments limit practical applications. Tritium propagation material for continuous fusion reaction is one of the core materials, and therefore research on this material is being carried out intermittently. The key material for Li-based energy storage and tritium generation is the functional material Li-M-O. In this review, a structural description of functional Li-M-O system materials and technical trends for its applications are introduced.

Part 1. Li-M-O Materials for Lithium Secondary Batteries

1. Cathode Materials for Lithium Secondary Batteries

1.1. Introduction

Cathode materials are significant, accounting for about 35% of the lithium secondary battery material cost; these materials are classified according to the crystal structure and the constituents of the metallic salt. Crystalline structures under consideration are divided into layered rock salt, spinel, and olivine type structures. In addition, Co, Ni, Mn, Al, Fe, and others are studied mainly as constituents of metal salts. Fig. 1 shows the three main types of crystal structure under consideration as cathode materials for lithium secondary batteries.
The requirements for the cathode materials of the lithium secondary battery are as follows:
  1. High Energy Density

  2. High Life Cycle

  3. Superb Charge/Discharge Rate

  4. Affordable Price

  5. Environmentally Friendly

CoO2, which has a layered rock salt type structure, is the most widely used cathode material for lithium secondary batteries, and is still the mainstay in the industry today. However, cobalt (Co), which is used in the production of LiCoO2, is a rare metal with a small amount of reserves; also, areas that can produce this material are limited. Therefore, it is disadvantageous in that the unit price is expensive and in that the material is unstable in terms of supply. For this reason, many studies have been carried out in the direction of not using cobalt or in minimizing its usage. As prime examples, there is LiMn2O4, which has a spinel type structure that uses Mn, and the LiNiO2 layered rock salt structure, which uses Ni. Both Ni and Mn are easily available compared to cobalt. In addition, research on ternary alloy materials using combinations of Ni, Co, and Mn, or Ni, Co, and Al have been actively conducted.2) However, the structure of LiNiO2 is unstable in the charged state, and the performance of LiMn2O4 deteriorates at high temperature. For these reasons, the tritium alloys of Li[Ni, Co, Mn]O2 are the most actively used materials in industry, and not LiCoO2. The general characteristics of the afore-mentioned materials are listed below in Table 1.

1.2. LiCoO2

LiCoO2 has a layered rock salt structure called “α-NaFeO2”, in which oxide ions constitute a (111) plane, and lithium ions and cobalt ions are alternately present between the layers. An attempt to apply such a layered oxide containing lithium ion as a cathode material was made when the Mizushima Corporation discovered in 1980 that LiCoO2 in a solution of 1 M LiBF4/PC exhibited a potential of 4 V to lithium metal and that reversible insertion and desorption of lithium ions was possible.3,4)
Insertion/desorption proceeds as lithium ions migrate into a two-dimensional plane with a CoO6 octahedral structure. Since lithium ions are intercalated/deintercalated in a state in which the crystal structure, composed of an oxide and a cobalt ion, is maintained, good characteristics are exhibited in a normal charge/discharge cycle. The fact that expansion/contraction only occurs during the charging/discharging cycle can be advantageous when the battery is built because the use of graphite as an anode leads to the opposite effect. In addition, since the diffusion path of lithium ions is a single layer of a two-dimensional plane, it is advantageous in terms of the characteristics of the battery, which has a larger diffusion coefficient than those of other crystal structures. From the manufacturability aspect, LiCoO2 also has a great advantage as a cathode material for a lithium secondary battery because a good quality product can be obtained by a relatively simple process.
Although, due to ly used as a cathode material for lithium secondary batteries in the early days, the continuous use of LiCoO2 has been greatly limited by the increase in unit price due to the scarcity of the source material. Fig. 2 shows charge/discharge curves at C/24 rate in the range of 3.6-4.85 V. The curves show that LiCoOx has several phases during the range of electrochemical cycling.5) In addition, there is a problem of phase change when this material is charged excessively during the charging/discharging process. That is, when the amount of lithium ions desorbed exceeds 0.5, the phase changes from hexagonal to monoclinic, and the structure of LiCoO2 becomes unstable. In order to prevent such a phenomenon, the charging voltage is limited to about 4.2 V when LiCoO2 is used as the cathode material of a lithium secondary battery. For this reason, the theoretical capacity of LiCoO2 is 274 mAh g−1, but the capacity that can actually be used is limited to 130-150 mAh g−1.
The charge/discharge reaction is as follows:
Many studies are being conducted to develop a cathode material for a lithium secondary battery with excellent properties that can compensate for the shortcomings of LiCoO2. The research is divided into two major categories:
  1. Developing a method that can compensate for the flaws of LiCoO2

  2. Finding a new material that can replace LiCoO2

In order to compensate for the disadvantages of LiCoO2, many studies on surface coating using metal oxide were conducted. Studies on the surface coating of LiCoO2 using ZrO2, Al2O3, MgO, SiO, etc., have been carried out and the life cycle of LiCoO2 during charging/discharging cycles at potentials of 4.2 V or higher has improved significantly compared to that of LiCoO2 without metal oxide. This improvement has been due to the suppression of physical phase change, inhibition of elution of cobalt ions, and suppression of increased interfacial resistance.6)

1.3. LiNiO2

LiNiO2, which has the same crystal structure (α-NaFeO2) as LiCoO2, has been studied for a long time as a replacement cathode material for LiCoO2. Because it has a crystal structure identical to that of LiCoO2, it exhibits characteristics equivalent to those of LiCoO2 in various aspects. In fact, LiNiO2 is 1.2 times larger than LiCoO2 in terms of capacity because the amount of lithium that can be extracted is 0.7 for LiNiO2, which is higher than the 0.5 extraction value for LiCoO2. Also, it is easier to supply nickel, due to its low cost, than it is to supply cobalt.
The price of nickel is also cheaper than cobalt, which is superior in terms of supply.
The charge/discharge reaction is as follows:
However, LiNiO2 has some problems when materials are synthesized. In order for LiNiO2 to be activated electrochemically, it must stay as Ni3+ for the lithium to exist, but it is easy for Ni3+ to be reduced to Ni2+ during material synthesis. If Ni2+ is present instead of Ni3+, it is easy for lithium to become Li1−xNi1+xO2. This phenomenon leads to the diffusion of lithium ions and to a deterioration in the cycle of charge and discharge. Many synthetic methods have been studied as alternatives, but there is no clear solution yet. Also, when Li is removed from LiNiO2, the Ni moves to the position of Li. When the number of Li is large, Li occupies the location of Ni; this deteriorates the charge and discharge rate. Such inversion of Li and Ni, and the low thermal stability, prevent LiNiO2 from being commercialized.

1.4. LiMn2O4

The spinel structure generally has the form of AB2X4. LiMn2O4 generally has this spinel structure and Mn ion occupies the 16d octahedral site, while Li ion occupies the 8a tetrahedral site. The 16c octahedral site, which is near the 8a tetrahedral site (occupied by Li ion), is empty; this path is necessary for Li ion to diffuse inside LiMn2O4. Fig. 3 provides the voltage profile of an Li//LiMn2O4 cell discharged at C/24 rate with LMO material synthesized at 700°C.5) During the process of charging and discharging, a flat section appears in the region of 3 V and 4 V. However, in the 3 V region, Li ions are further inserted into the 16c site; this generates Li2Mn2O4, which results in degradation in the cycles due to volumetric expansion.7)
Compared to other cathode materials, LiMn2O4 has a small capacity. It also has problems during charge and discharge cycles in the 4 V region. The leading causes for these problems include dissolution of Mn in the organic electrolytes, 8,9) structural instability,10,11) and the Jahn-Teller Effect.12) For these reasons, studies are underway to improve the cycle of charging and discharging by replacing a part of the Mn with another metal.
The charge/discharge reaction is as follows:

1.5. LiFePO4

LiFePO4, an olivine-type compound, is an excellent cathode material due to its high capacity and the low cost of its raw material. In particular, due to its excellent cycle of charging/discharging, and its thermal stability, it is attracting attention from many researchers in the industry as a cathode material for batteries of large-sized electric vehicles. LiFePO4 has been studied continuously since the Goodenough Corp. used a polyanion in the form of XO4y− (X = S, P, As, Mo, W, y=2, 3) to develop an Fe compound with an operating voltage of 3.4 V.13,14) LiFePO4 is a cheap material with outstanding life cycle and thermal stability; it is also environmentally friendly. Despite these advantages, the use of this material is still limited. This is because this material is difficult to charge and discharge rapidly due to its low electrical conductivity (10−10 S cm−1). In order to solve these problems, two approaches are under study. The first is to increase the surface area of the sample that will be used in the reaction by inserting particles with large specific surface area into the nanostructure. The second method is to coat a conductive material such as carbon onto the surface of the particles. A variety of studies have been conducted using these two methods, and a lot of progress has been made until now.15-19)
The charge/discharge reaction is as follows:

1.6. LiNixCoyMnzO2

LiNixCoyMnzO2 is a ternary cathode material with a crystal structure identical to that of LiCoO2; its capacity and operating voltage are similar to those of LiCoO2. According to the research, it is possible to charge and discharge this material with a high capacity of 200 mAh g−1 when the voltage is raised to 4.6 V.20) LiNixCoyMnzO2 has a high thermal stability compared to that of LiNiO2, and it uses a 3 times lower amount of Co compared to LiCoO2. Many studies have been done on the possibility that a solid solution compound of the transition metal can be used to take advantage of existing materials and mitigate the mentioned disadvantages. Among potential materials, LiNixCoyMnzO2 is one of the few solid solution compounds that is actually being used in the industry, and it is the closest to becoming commercialized.

2. Solid Electrolyte Materials for Lithium Secondary Batteries

2.1. Introduction

Secondary batteries provide high energy for various electronic devices, but they are subject to flame hazard because they use volatile and highly reactive liquid electrolytes. Next generation secondary batteries will use solid electrolytes instead of liquid electrolytes, and research is underway to fabricate batteries with low flame hazard.21,22) Advantages of batteries manufactured using solid electrolytes (also known as “all solid-state batteries”) are that they do not use liquid electrolytes, so there is little risk of fire, and that there is no leakage of liquid. In addition, such batteries are safe for use at high temperature and pressure, and their low self-discharge rate enables long-term storage. Unlike liquid electrolytes, solid electrolytes do not leak, so there is no restriction on packing, and this means the battery can be miniaturized. In order to manufacture all solid-state batteries with these advantages, it is important to develop a new solid electrolyte with excellent electrolyte performance. The performance of the battery is affected by the internal movement of Li ions. Therefore, the higher the ionic conductivity of the solid electrolyte is, the better the performance of the battery is.23-25)
The following are additional requirements for solid-state batteries:
  1. Interfacial stability between anode and cathode

  2. High chemical structural stability

  3. Large working windows of voltage and current

  4. Stability over a wide temperature range

  5. Low corrosion and high thermal mechanical strength (for demanding environments)

  6. Economically and environmentally friendly

The solid electrolytes that are being studied recently are LiSiCON, NASiCON, the Garnet type, the Perovskite type, the anti-perovskite type, and more. A lot of the research that has been conducted has mainly focused on the wide range of chemical compositions and crystal structures. Fig. 4 shows serval types of solid electrolytes with good ion conductivity for use in lithium secondary batteries.
In order to understand Li-M-O solid electrolytes, this chapter mainly focuses on their structure and material properties. Also, this chapter will discuss the pros and cons of these electrolytes, and how we will overcome their flaws.

2.2. NASICON type solid electrolyte

The general structure of the NASICON (Na super ionic conductor) solid electrolyte is expressed as AM1M2P3O12/AM1M2(PO4)3. One AO6 octahedron and the PO4 tetrahedrons share six oxygen atoms at the edges to form a three dimensional skeleton. Three-dimensional channels (M1, M1/2, M2) are formed in the crystal lattice and the conduction of ions become possible. B-alumina, Na3Zr2Si2PO12, and NaZr2 (PO4)3 are materials representative of the NASICON structure (Fig. 5).28) Many studies have been conducted on Li1+xAlxTi2−x(PO4)3 (LATP) (0 ≤ × ≤ 0.4, LATP), in which Na and Zn are replaced by Li and Ti ions and some Al.29) NaZr2 (PO4)3 shows a low ionic conductivity of about 10−5 S cm−1 at 300 °C, but it has been reported that this ionic conductivity increases tenfold when Na is replaced with Li.30) When Zr4+ ions are replaced by Ti4+ions, which are small in size, the ionic conductivity improves due to the formation of a channel that is more suitable for ions to move in, while the skeletal structure of NASICON is maintained. Many studies have been conducted on Li1+xAlxTi2-x(PO4)3 (LATP) (0 ≤ × ≤ 0.4, LATP), in which Na and Zn are replaced by Li and Ti ions and some Al.31,32) The structure of LATP depends on the amount of lithium inserted; the ionic conductivity of Li1.3Ti1.7Al0.3(PO4)3 was at its highest (10−2-10−3 S cm−1) when the x value was 0.3. Research on the synthesis of LATP is continuously being performed using various methods such as solid state reaction, sol-gel reaction, hydrothermal reaction, and more. Studies have reported that the ionic conductivity increased with the replacement of Ti4+ and P5+ ions with trivalent cations (Al, Ga, Sc, In, Y) in the LATP structure. 33,34) However, when LATP comes in contact with Li metal, which is used as a cathode, Ti4+ is reduced to Ti3+ and it becomes difficult to apply these methods to all solid-state batteries. LAGP substitutes Ge4+ for Ti4+; therefore, LAGP is attracting more attention than LATP as a solid electrolyte because LAGP makes Li more stable by replacing Ti4+ with Ge4+.35)

2.3. Garnet type solid electrolyte

The general structure of a garnet type solid electrolyte is expressed as A3B3C2O12, which forms as a tetrahedron (site A), a dodecahedron (site B), and an octahedron (site C), and coordinating oxygen atoms.36,37) Fig. 6 shows the crystal structure of Li5La3M2O12 (M=Nb/Ta). Among the garnet type solid electrolytes, Lithium Lanthanum Zirconia Oxide (LLZO), which was studied by Weppner’s group in 2007, has been the most studied compound. LLZO has cubic and tetragonal structures, with ionic conductivity values of ~ 5 × 10−4 S cm−1 in the cubic structure and 1.6 × 10−6 S cm−1 in the tetragonal structure.38,39) In previous research, a method of synthesizing LLZO by adding Al+ to form a stable cubic structure has been studied.40,41) Ever since then, many synthesis studies were performed by adding a variety of cations. 40,42) Other garnet compound includes lithium lanthanum metal oxide (Metal = Nb, Ta); Li6ALa2M2O12 with Ca, Sr, and Ba (position A) has ionic conductivity of 4 × 10−5 S cm−1.43) In order to synthesize a solid electrolyte with a garnet structure, the material must be made to remain at a high temperature of 1100°C for a long period. During this process, Li+ ions become volatile and either the garnet structure collapses or a solid electrolyte with low ionic conductivity is synthesized. Experiments are underway to synthesize solid electrolytes with excellent properties.

2.4. LISICON-type solid electrolyte

LISICON, which was introduced by Bruce and West, is an abbreviation of “Lithium Super Ionic Conductor”; its structural formula is Li2+2xZn1−xGeO4.44) Due to its structure, lithium ions are distributed between two different octahedron sites (Li1 and Li2 sites inside the lattice) and move between them. Li3.5Zn0.25GeO4 has a high ionic conductivity of 1.2 × 10−1 S cm−1 at 300°C, but a low ionic conductivity of 10−7 S cm−1 at room temperature.45) The Li-rich Li3.5Zn0.25GeO4 structure octahedron sites are shown in Fig. 7. The use of Li3.5Zn0.25GeO4 for batteries is limited at room temperature. On the other hand, thio-LISICON (e.g. Li4GeS4, Li3PS4, Li5AlS4), in which oxygen is replaced by sulfur, has an ion conductivity value that is 100 times higher than that of oxide type LISICON.46,47) In particular, Li3.25Ge0.25P0.75S4 has a high ionic conductivity of 2.2 × 10−3 S cm−1 at room temperature. Therefore, in the case of LISICON-type solid electrolytes, researchers are developing methods to replace the oxygen in thio-LISICON with sulfur.

2.5. Perovskite type solid electrolyte

Perovskite is also known to have a formula of ABO3; the BO3 surrounding the A-site ions becomes the frame of the crystal structure.48,49) The perovskite structure (ex. tetragonal Li3xLa3/2−xTiO3) is shown in Fig. 8. The first research into the Li-M-O type perovskite material was conducted after a study on the A-site deficiency structure was undertaken by Latie and Belous; in this study, La2/3TiO3 was replaced with Li+ instead of replacing it with La3+.50,51) After that study, a variety of materials have been studied. As of now, the most widely studied material is Li0.34La0.51TiO2.94 (LLTO); its ionic conductivity is 2 × 10−5 S cm−1, which is relatively high compared to the values of other materials.52) LLTO has high ionic conductivity because its structure deforms when there are not a sufficient number of A-site ions. However, the ionic conductivity of LLTO differs between its total ion conductivity (2 × 10−5 S cm−1) and bulk ion conductivity (1 × 10−3 S cm−1). This shows that the movement of Li+ ions is restricted by contact resistance generated at the grain boundaries.53) In order to solve this issue, many studies have examined the effect of the heat treatment temperature in order to determine an optimum temperature. It was also necessary to reduce the activation energy and, for that reason, a variety of ions were studied as substitutions (La3+=Pr, Nb, Sm).54) LLTO has excellent ionic conductivity, but the intercalation of lithium causes Ti4+ to be substituted with Ti3+, resulting in a deterioration in the performance, which limits the use of this material as a solid electrolyte. Various studies have been carried out to improve the ionic conductivity of perovskite structure materials. For example, Martin et al. obtained an ion conductivity of 4.3 × 10−5 S cm−1 by replacing TiO3 with NbO3.49)

2.6. Anti-perovskite type solid electrolyte

The anti-perovskite structure is a typical ABO3 perovskite structure, in which A is a monovalent metal cation, B is a divalent metal cation, and O is a negative monovalent anion. This structure is created when an anion element in the conventional perovskite structure is replaced with a cation metal. Zhao et al. were the first to study Li3OA (A = halogen) anti-perovskites.23,24,55,56) The most basic material of this structure is Li3OCl, which has a high ionic conductivity (0.85 × 10−3 S cm−1) and low activation energy. Fig. 9 shows the structure of Li3ClO. This material has a structure of Li+ ion at the octahedral corner, O2 anion at the center, and Cl at the center of the Li6O octahedron. Recently, in Braga et al., a material with a glass-liquid transition of Li3−2xMxAO (M = Mg2+, Ca2+, Ba2+, A = halogen) was synthesized in order to increase the ionic conductivity and obtain a high ionic conductivity of 2.5 × 10−2 S cm−1.57) However, despite the good performance of this anti-perovskite, it is necessary to study the mechanism of ion conduction up to date. In addition, studies conducted so far have mainly focused on the stability of the phase. Further, studies on defects and movements of ions in Li3OCl have been carried out through simulation. 56) It is necessary to study the applicability of anti-perovskite materials as solid electrolytes using various types of experiments and by subjecting results to verification.

3. Anode Materials for Lithium Secondary Batteries

3.1. Introduction

A battery’s energy density increases as the charging voltage of the cathode increases (e.g. 4.1 V → 4.3 V), as the result the performance of the anode improves. When amorphous carbon was replaced with graphite, the voltage flatness improved and the anode capacity increased from 260 mA h g−1 to 360 mA h g−1. This value (360 mA h g−1) is very close to the theoretical capacity of graphite (C6Li) of 372 mA h g−1. However, it is still necessary to improve the performance of this anode active material. In order to improve the performance of lithium ion secondary batteries, the following tasks must be accomplished:
  1. The anode material must be replaced.

  2. Electrode coating technology must be improved.

  3. Electrode packing technology needs to be improved.

  4. The Li ion absorption rate of the anode must be higher.

The ideas in three (2 ~ 4) of the four statements listed above have reached their limit through space optimization within cell design and packaging. Therefore, it is necessary to increase the capacity of the anodic active material by developing a new an anode material and changing the structure itself.
The most noteworthy candidates for replacement of anode materials in the research so far are the following, including metal (M: Si, Sn, Sb, Al), M-O (M: Sn, Fe, Co, Ti, Ni), Li-M-O (M: Sn, Ti, V), LixMyN2 (M: Co). 59-61) These materials have higher capacity than that of commercialized graphite. Compared to graphite, which is a commercial cathode material, high-capacity metal-based materials go through rapid volume expansion during the alloying/dealloying process with Li ions. For example, Si has a theoretical capacity (4,010 mA h g−1) that is 10 or more times higher than that of the theoretical capacity of graphite (372 mA h g−1). However, the volume of Si increases by 300 ~ 400 % (theoretically), while the volume of graphite only increases by 12 %. The following phenomenon also occurs in MO type anodic active materials; it is a problem that must be solved before it will be possible to replace graphite. On the other hand, Li4Ti5O12 (titanium based Li oxide) only goes through a slight change in crystal lattice of about 0.1 to 0.2 % during the reaction with Li ions; it also has excellent power and high cycle life, and is safe. However, the disadvantage of Si is that its capacity is low because its reaction potential is high (higher than that of commercialized graphite).

3.2. Li-Ti-O (LTO)

Li4Ti5O12 (LTO), which has a cubic spinel structure, has been intensively studied by a number of researchers over the last 20 years. The performance of LTO has been improved through approaches such as changing the size (micro and nano) of the crystalline particles, changing the shapes, creating different composites with other cathode materials, and carbon coating. LTO, which has a spinel structure (a type of crystal structure), has high electrochemical output due to its three-dimensional diffusion of Li ions. Jung et al. prepared carbon coated LTO anodes with high electrochemical performance. Because of its spherical shape and good electronic conductivity, a C coated LTO (5.2 wt %) exhibited outstanding cyclability up to 100 cycles under 1, 5, and 10 C-rates with voltage windows in the range of 1 - 3 V (Li vs. Li+), as shown in Fig. 10.62)
The advantage of LTO is that it does not form an SEI (Solid-Electrolyte Interphase) because it reacts at a relatively high reaction potential (~1.5 V).63) LTO, because it is thermally stable during the charging/discharging process, is receiving a lot of attention from researchers as an anode material for high output medium-to large-sized batteries. It is thermally stable because there is no exothermic reaction while the SEI on the electrode surface is being decomposed. However, the low energy density that results from the high reaction voltage, and the high cost, make it difficult to commercialize this material.64)

3.3. Li-Co-N

NTT and Panasonic discovered Li2.6Co0.4N is a nitride anode synthesized using a general ceramic method. A full cell test was carried out with various cathode materials having a high capacity of 900 mA h g−1 as well as low reaction potentials ranging from 0.1 to 1.4 V.65) However, this material has limitations for use as a commercial cathode material due to its low life cycle.

3.4. Li-V-O

Vanadium-based Oxide (Li1.1V0.9O2) is an anodic active material that has a theoretical volume energy density of ~1000 mA h cc−1; this is because it reacts with Li ion at a low potential of 0.3 V. For this reason, it is expected to be applicable to batteries with high energy density. However, in order to commercialize this material, it will be necessary to develop a way to increase the low initial reversible capacity and prevent the volume from changing (~30 %) during electrochemical reactions. 66)

3.5. Li-Ti-Nb-O

LiTiNbO5 (layered structure) was synthesized by Collin through the ion exchange method.67) An electrode containing 0.8 mol of Li was found to have a charge/discharge cutoff range of 1.67 (Li vs. Li+) and a capacitance value of ~115 mA h g−1 in the first cycle. When the charge/discharge test was performed at a C-rate of 0.1, LiTiNbO5 became a low cycle material due a capacity decrease to ~90 mA h g−1 after 40 cycles.

3.6. Li-Ti-P-O

Cathode materials that are composed of LiTi2P3O12, which has a framework structure of NASICON (sodium superionic conductor) type have recently been studied using various synthesis methods.68) As a result of electrochemical analysis, the main reduction and oxidation have been found to take place between 2.38 and 2.6 V, and the material has been found to have a reversible capacity of ~120 mA h g−1 at 0.1 C. These traits are similar to those of TiP2O7, and further research is necessary in order to lower the reaction potential by alloying and compounding this material with other materials.

Part 2. Li-M-O Materials for Nuclear Fusion

1. Introduction

Nuclear fusion is a phenomenon in which two light nuclei gather to form a single heavy nucleus. In order for nuclear fusion to take place, it is necessary to have a very high temperature and a large amount of energy that can separate the electrons from the atom.69) Plasma is a hot ionized gas consisting of atoms with separate electrons and nuclei (ions); plasma is considered a fourth state of matter after solid, liquid, and gas. All plasmas are ionized, but that does not mean that all ionized gases are plasmas. In order to create a plasma, it is necessary to ionize deuterium and tritium (These isotopes are capable of nuclear fusion).70-72)
The following conditions are required for nuclear fusion:
  1. Plasma at 100 million degrees Celsius

  2. A device that can safely operate the plasma at 100 million degrees Celsius

  3. Seawater, which is rich in deuterium (1 L of seawater contains about 0.03 g of deuterium)

As mentioned above, nuclear fusion involves using a magnetic field to confine a high-temperature (about 100 million degrees Celsius) plasma in a device called a “tokamak” to generate stable helium molecules, neutrons, and thermal energy after collisions between deuterium and tritium at high energy.73,74) This device is expected to be a next-generation energy source that can generate electric energy. As a representative sample, there is the International Thermonuclear Experimental Reactor (ITER), which obtains energy from the D-T (Deuterium-Tritium) fusion reaction. 75-77) Fig. 11 shows the inner and outer fuel cycle of a fusion reactor.
D+TH4e (3.5MeV)+n (14.1MeV)
In this case, “D” represents deuterium, “T” represents tritium, and “n” represents neutrons. In Korea, KSTAR (Korea Superconducting Tokamak Advanced Research) is a nuclear fusion research institute that has developed its own tokamak. 78) In addition, there are various nuclear fusion research institutes such as the Jet program of the European Union, JT-60U in Japan, EAST in China, W-7X in Germany, the US TFTR, the TOCE-SUPRA of France, and the SST-1 of India.
In a fusion reactor that uses a tokamak, there is a blanket that absorbs the generated neutrons. Inside the blanket, there is a tritium breeder, a ceramic material containing lithium, which produces tritium through a nuclear reaction of tritium breeders and neutrons.80,81) This process is shown in the schematic diagram of the lithium transfer step of the solid breeder material, in Fig. 12.
Thus, the breeder of a nuclear fusion reactor is the key component in producing tritium; the role of lithium in the fusion reaction is to generate tritium via a nuclear reaction. Furthermore, the breeder must simultaneously convert nuclear energy to thermal energy while shielding the neutrons. 83) The tritium breeder should have the following conditions. 84,85)
  1. It must contain a lot of lithium.

  2. It must have high thermal conductivity and a low thermal expansion coefficient.

  3. It must be mechanically and chemically stable.

  4. The emission rate of tritium must be high

  5. The structure must be stable under irradiation

Materials those satisfy the conditions above include oxide ceramic materials such as Li2O, Li2TiO3, Li2ZrO3, LiAlO2, and Li4SiO4, which are lithium-based compounds capable of generating tritium.86)

2. Characteristics of Nuclear Fusion Materials

Li2O has a high lithium atom density, high thermal conductivity, low tritium solubility, and high tritium growth rate, but has disadvantages such as high water reactivity and high lithium vapor pressure.87) LiAlO2 has a high melting point and low reactivity with water; it has a wide temperature range for use, and has excellent radiation properties, but has a poor tritium emission rate.88) Li4SiO4 has good tritium diffusivity and excellent chemical stability, but it is easily fragmented by radiation due to the anisotropy of its thermal expansion coefficient.89) Li2ZrO3 is chemically and mechanically stable and has a high tritium emission rate, but there is an issue of zirconium becoming excited when heat is radiated after irradiation.90) Among researchers, Li2TiO3 became a popular material as a breeder due to its excellent maneuverability of tritium, its chemical stability, and its low activation energy.91,92) The physical properties of these lithium-based oxides are closely related to their physical properties such as their porosity, particle size, particle shape, and microstructure. Therefore, optimization of the manufacturing process of breeders plays an important role in controlling the physical properties. Since the characteristics of the initial powder in the preparation of an oxide sintered body have great influence on the physical properties of the sintered body, optimization of the initial powder plays a very important role in the manufacturing process.93) In addition, the breeder is present in the form of pebbles; these pebbles can easily relax the thermoadaptive force morphologically, and reduce the possibility of cracking and swelling due to irradiation.94,95) In terms of TBR (Tritium breeding ratio), pebbles should have spherical shapes of about 1 mm diameter or more, and should have enough strength to maintain a certain density. Fig. 13 shows TiO2 Pebbles (Used to make Li2TiO3 Pebbles) before rolling process, after 6 h of rolling process, and after 20 h of rolling process. With the increased rolling time, the pebbles became spherical.
Since the porosity has an important influence on the heat conductivity of the pebbles, it is important for the breeder to have an appropriate porosity.97,98) In order to synthesize various tritium breeders, a variety of methods are being used to produce powders.99) Generally, a high-temperature solid phase method and a high-energy ball mill method in which calcination and sintering proceed through a mixing process among ceramic manufacturing methods are used. Recently, liquid phase methods such as hydrothermal synthesis, the sol-gel process, the precipitation method, the hydrolysis method, the precipitation method, and the micro-emulsion method have also been used. When the liquid phase method is used, a fine powder with high purity can be obtained, and the composition and particle size of the product can be controlled. NFRI Korea ITER and the Material Development Department of KAERI are pursuing world trends by focusing the research direction of the nuclear fusion tritium breeder on the ITER DEMO. In Korea, research and development is mainly focused on Li2TiO3 through the ITER project at NFRI. However, KSTAR’s research has been mainly focused on tritium breeders composed of lithium oxide, and there has not been much progress. In order to develop domestic technology such as KSTAR in the future, it will be necessary to conduct research on breeders through various synthesis methods and optimization. It will be possible for Korea to join the ranks of the advanced countries once Korea acquires essential nuclear fusion technology.


This research was supported by the National R&D Program through the National Research Foundation of Korea (NRF), funded by the Ministry of Science, ICT and Future Planning (NRF-2015M1A7A1A02002288).

Fig. 1
Representative crystal structures of cathode materials for lithium secondary batteries: (a) layered LiCoO2, LiNiO2, LiMnxCoyMnzO2; (b) cubic LiMn2O4 spinel; (c) olivine structured LiFePO4.1)
Fig. 2
Charge-discharge curves of LixCoO2 at C/24 rate in the range of 3.6 - 4.85 V vs. Li0/Li+. The sequence of the several phases is indicated as x varies from 1.0 - 0.05.5)
Fig. 3
Voltage profile of an Li//LiMn2O4 cell discharged at C/24 rate with LMO material synthesized at 700 °C (left). Variation of the lattice parameters as a function of the Li content x during charge/discharge in the LMO cathode (right).5)
Fig. 4
Reported total lithium ion conductivity as function of temperature. 26)
Fig. 5
Crystal structure of NaZr2(PO4)3. The solid box indicates the unit cell.27)
Fig. 6
Crystal structure of Li5La3M2O12 (M = Nb/Ta) (a). Details of 3D lithium ion migration pathway in Li5La3M2O12 (M=Nb/T a) (b).27)
Fig. 7
Crystal structures of Li2ZnGeO4 (a) and Li3.5Zn0.25GeO4 (LISICON) (b). The remaining lithium occupies the interstitial sites within the rigid network of LISICON. 27)
Fig. 8
Crystal structure of tetragonal Li3xLa3/2-xTiO3 (a). Lithium, lanthanum, and vacancies are distributed at the A-sites. Schematic representation of 3D mobility of lithium ions in the perovskite structure (b).27)
Fig. 9
Unit cell of cubic anti-perovskite.58)
Fig. 10
(a) Rate capacity ability of 5.2 wt % C-coated Li4− Ti5O12 and (b) cycle performances of 5.2 wt % Ccoated Li4Ti5O12 from 1C rate (0.17 A g−1) to 10C rate (1.7 A g−1) compared with performance of carbon free Li4Ti5O12 at 1C rate (0.15 A g−1) between 1.0 and 3 V(Li vs. Li+).62)
Fig. 11
Schematic diagram of fuel cycle system of nuclear fusion reactor.79)
Fig. 12
Schematic diagram of the lithium transfer step in the solid breeder material.82)
Fig. 13
(a) TiO2 Pebbles (Used to make Li2TiO3 Pebbles) before rolling process, (b) after 6 h of rolling process, (c) after 20 hours of rolling process.96)
Table 1
Types and Characteristics of Cathode Materials for Lithium Secondary Batteries
Material LiCoO2 LiNiO2 LiMn2O4 LiFePO4 LiNi1/3Co1/3Mn1/3O2
Crystal Structure Layered Layered Spinel Olivine Layered
Operating Voltage 3.7 V 3.5 V 4.0 V 3.2 V 3.6 V
Practical Capacity 145 mAh g−1 175 mAh g−1 100 mAh g−1 150 mAh g−1 140 mAh g−1
Stability high low middle very high high
Cycle Performance high low low high high
Cost high middle middle low middle


1. MS. Islam, and CAJ. Fisher,, “Lithium and Sodium Battery Cathode Materials: Computatianal Insights into Voltage, Diffusion and Nanostructural Properties,” Chem Soc Rev, 43 [1] 185-204 (2014).
2. HJ. Kim, UC. Chung, YU. Jeong, JH. Lee,, and JJ. Kim, “Crystal Structures, Electrical Conductivities and Electrochemical Properties of LiCo1−XMgxO2(x=0.03) for Secondary Lithium Ion Batteries,” J Korean Ceram Soc, 42 [9] 602-6 (2005).
3. K. Mizushima, PC. Jones, PJ. Wiseman,, and JB. Goodenough, “LixCoO2 (0<x<1): A New Cathode Materials for Batteries of High Energy Density,” Mat Res Bull, 15 [6] 783-89 (1980).
4. SH. Kim, KB. Shim, JP. Ahn,, and CS. Kim,, “Structural Stability during Charge-Discharge Cycles in Zr-Doped LiCoO2 Powders,” J Korean Ceram Soc, 45 [3] 167-171 (2008).
5. CM. Julien, A. Mauger, K. Zaghib,, and H. Groult,, “Comparative Issues of Cathode Materials for Li-Ion Batteries,” Inorganics, 2 [1] 132-54 (2014).
6. MS. Whittingham,, “Lithium Batteries and Cathode Materials,” Chem Rev, 104 [10] 4271-301 (2004).
7. T. Ohzuku, M. Kitakawa,, and T. Hirai,, “Electrochemistry of Manganese Dioxide in Lithium Nonaqueous Cell III. X-Ray Diffractional Study on the Reduction of Spinel-Related Manganese Dioxide,” J Electrochem Soc, 137 [3] 769-75 (1990).
8. DH. Jang, YJ. Shin,, and SM. Oh,, “Dissolution of Spinel Oxides and Capacity Losses in 4 V Li/LixMn2O4 Cells,” J Electrochem Soc, 143 [7] 2204-11 (1996).
9. T. Inoue, and M. Sano,, “An Investigation of Capacity Fading of Manganese Spinels Stored at Elevated Temperature,” J Electrochem Soc, 145 [11] 3704-7 (1998).
10. Y. Xia, and M. Yoshio,, “An Investigation of Lithium Ion Insertion into Spinel Structure Li-Mn-O Compound,” J Electrochem Soc, 143 [3] 825-33 (1996).
11. Y. Xia, T. Sakai, T. Fujieda, X. Yang, X. Sun, Z. Ma, J. McBreen,, and M. Yoshio, “Correlating Capacity Fading and Structural Changes in Li1+xMn2−yO4− Spinel Cathode Material: A Systematic Study on the Effects of Li/Mn Ratio and Oxygen Deficiency,” J Electrochem Soc, 148 [7] 723-29 (2001).
12. MM. Thackeray, YS. Horn, AJ. Kahian, KD. Kepler, E. Skinner, JT. Vaughey,, and SA. Hackney,, “Structural Fatigue in Spinel Electrodes in High Voltage (4 V) Li/LixMn2O4 Cells,” Electrochem Soc Solid-State Lett, 1 [1] 7-9 (1998).
13. AK. Padhi, KS. Nanjundaswamy,, and JB. Goodenough,, “Phospho-Olivines as Positive-Electrode Materials for Rechargeable Lithium Batteries,” J Electrochem Soc, 144 [4] 1188-94 (1997).
14. SY. Chung, JT. Bloking,, and YM. Chiang,, “Electronically Conductive Phospho-olivines as Lithium Storage Electrodes,” Nat Mater, 1 [2] 123-28 (2002).
15. W. Ojczyk, J. Marzec, K. Swierczek, W. Zajac, M. Molenda, R. Dziembaj,, and J. Molenda,, “Studies of Selected Synthesis Procedures of the Conducting LiFePO4-Based Composite Cathode Materials for Li-Ion Batteries,” J Power Sources, 173 [2] 700-6 (2007).
16. H. Liu, J. Xie,, and K. Wang, “Synthesis and Characterization of LiFePO4/(C+Fe2P) Composite Cathodes,” Solid State Ionics, 179 [27] 1768-71 (2008).
17. Y. Lin, MX. Gao, D. Zhu, YF. Liu,, and HG. Pan,, “Effects of Carbon Coating and Iron Phosphides on the Electrochemical Properties of LiFePO4/C,” J Power Sources, 184 [2] 444-48 (2008).
18. H. Liu, and D. Tang,, “The Low Cost Synthesis of Nanoparticles LiFePO4/C Composite for Lithium Rechargeable Batteries,” Solid State Ionics, 179 [33] 1897-901 (2008).
19. BW. Kang, and G. Ceder,, “Battery Materials for Ultrafast Charging and Discharging,” Nature, 458 [7235] 190-93 (2009).
20. N. Yabuuchi, and T. Ohzuku,, “Novel Lithium Insertion Material of LiCo1/3Ni1/3Mn1/3O2 for Advanced Lithium-ion Batteries,” J Power Sources, 119-121 171-74 (2003).
21. RH. Shin, SI. Son, SM. Lee, YS. Han, YD. Kim,, and SS. Ryu,, “Effect of Li3BO3 Additive on Densification and Ion Conductivity of Garnet-Type Li7La3ZrO12 Solid Electrolytes of All-Solid-State Lithium-Ion Batteries,” J Korean Ceram Soc, 53 [1] 712-718 (2016).
crossref pdf
22. IY. Kim, SH. Jee,, and YS. Yoon, “High-Speed Deposited Amorphous Li-B-W-O Thin Film Electrolytes for All-Solid-State Batteries,” Sci Adv Mater, 8 [1] 96-102 (2016).
23. Y. Zhao, and LL. Daemen,, “Superionic Conductivity in Lithium-Rich Anti-Perovskites,” J Am Chem Soc, 134 [36] 15042-47 (2012).
24. A. Emly, E. Kioupakis,, and AV. Ven, “Phase Stability and Transport Mechanisms in Antiperovskite Li3OCl and Li3OBr Superionic Conductors,” Chem Mater, 25 [23] 4663-70 (2013).
25. F. Lalère, JB. Lerichea, M. Courty, S. Boulineau, V. Viallet, C. Masquelier,, and V. Seznec,, “An All-Solid State NASICON Sodium Battery Operating at 200°C,” J Power Sources, 247 975-80 (2014).
26. JC. Bachman, S. Muy, A. Grimaud, HS. Chang, N. Pour, SF. Lux, O. Paschos, F. Maglia, S. Lupart, P. Lamp, L. Giordano,, and YS. Horn,, “Inorganic Solid-State Electrolytes for Lithium Batteries: Mechanisms and Properties Governing Ion Conduction,” Chem Rev, 116 [1] 140-62 (2016).
27. I. Kokal, “Solid State Electrolytes for All Solid State 3D Lithium ion Batteries,” 9-34 PhD Thesis, Eindhoven University of Technology, Eindhoven2012.

28. HB. Kang, NH. Cho,, and YH. Kim,, “Effects of Heat-Treatment Condition on the Characteristics of Sintering and Electrical Behaviors of Two NASICON Compounds,” J Korean Ceram Soc, 34 [7] 685-92 (1997).

29. H. El-Shinawi, C. Greaves,, and J. Janek,, “Sol-Gel Synthesis and Room-Temperature Properties of α-LiZr2(PO4)3,” RSC Adv, 5 [22] 17054-59 (2015).
30. KM. Kim, DO. Shin,, and YG. Lee,, “Effects of Preparation Conditions on the Ionic Conductivity of Hydrothermally Synthesized Li1+xAlxTi2−x(PO4)3 Solid Electrolytes,” Electrochim Acta, 176 1364-73 (2015).
31. K. Arbi, W. Bucheli, R. Jiménez,, and J. Sanz, “High Lithium ion Conducting Solid Electrolytes based on NASICON Li1+xAlxM2−x(PO4)3 Materials (M = Ti, Ge and 0 ≤ x ≤ 0.5),” J Eur Ceram Soc, 35 [5] 1477-84 (2015).
32. K. Arbi, S. Mandal, JM. Rojo,, and J. Sanz, “Dependence of Ionic Conductivity on Composition of Fast Ionic Conductors Li1+xTi2−xAlx(PO4)3, 0 ≤ × ≤ 0.7. A Parallel NMR and Electric Impedance Study,” Chem Mater, 14 [3] 1091-97 (2002).
33. DH. Kothari, and DK. Kanchan, “Effect of Doping of Trivalent Cations Ga3+, Sc3+, Y3+ in Li1.3Al0.3Ti1.7(PO4)3 (LATP) System on Li+ Ion Conductivity,” Phys B, 501 90-4 (2016).
34. H. Aono, E. Sugimoto, Y. Sadaoka, N. Imanaka,, and GY. Adachi,, “Ionic Conductivity of Solid Electrolytes Based on Lithium Titanium Phosphate,” J Electrochem Soc, 137 [4] 1023-27 (1990).
35. XL. Wu, J. Zong, H. Xu, W. Wang,, and XJ. Liu,, “Effects of LAGP Electrolyte on Suppressing Polysulfide Shuttling in Li-S Cells,” RSC Adv, 6 [62] 57346-56 (2016).
36. D. Rettenwander, CA. Geiger, M. Tribus, P. Tropper,, and G. Amthauer, “A Synthesis and Crystal Chemical Study of the Fast Ion Conductor Li7−3xGaxLa3Zr2O12 with x = 0.08 to 0.84,” Inorg Chem, 53 [12] 6264-69 (2014).
37. NC. R-Navarro, T. Yamashita, A. Miura, M. Higuchi,, and K. Tadanaga,, “Effect of Sintering Additives on Relative Density and Li-Ion Conductivity of Nb-Doped Li7La3ZrO12 Solid Electrolyte,” J Am Ceram Soc, 100 [1] 276-85 (2017).
38. R. Murugan, V. Thangadurai,, and W. Weppner,, “Fast Lithium Ion Conduction in Garnet-Type Li7La3Zr2O12,” Angewandte Chemie, 46 [41] 7778-81 (2007).
39. J. Awaka, N. Kijima, H. Hayakawa,, and J. Akimoto,, “Synthesis and Structure Analysis of Tetragonal Li7La3Zr2O12 with the Garnet-Related Type Structure,” J Solid State Chem, 182 [8] 2046-52 (2009).
40. Y. Jin, and PJ. McGinn,, “Al-Doped Li7La3Zr2O12 Synthesized by a Polymerized Complex Method,” J Power Sources, 196 [20] 8683-87 (2011).
41. H. El-Shinawi, GW. Paterson, DA. MacLaren, EJ. Cussen,, and SA. Corr,, “Low-Temperature Densification of Aldoped Li7La3Zr2O12: a Reliable and Controllable Synthesis of Fast-ion Conducting Garnets,” J Mater Chem A, 5 [1] 319-29 (2017).
42. Y. Jiang, X. Zhu, S. Qin, M. Ling,, and J. Zhu, “Investigation of Mg2+, Sc3+ and Zn2+ Doping Effects on Densification and Ionic Conductivity of Low-Temperature Sintered Li7− La3Zr2O12 Garnets,” Solid State Ionics, 300 73-7 (2017).
43. S. Song, D. Sheptyakov, AM. Korsunsky, HM. Duong,, and L. Lua,, “High Li Ion Conductivity in a Garnet-Type Solid Electrolyte via Unusual Site Occupation of the Doping Ca Ions,” Mater Des, 93 232-37 (2016).
44. PG. Bruce, and AR. West,, “Ionic Conductivity of LISICON Solid Solutions, Li2+2xZn1−xGeO4,” J Solid State Chem, 44 [3] 354-65 (1982).
45. S. Hori, M. Kato, K. Suzuki, M. Hirayama, Y. Kato,, and R. Kanno,, “Phase Diagram of the Li4GeS4-Li3PS4 Quasi-Binary System Containing the Superionic Conductor Li10GeP2S12,” J Am Ceram Soc, 98 [10] 3352-60 (2015).
46. P. Zhou, J. Wang, F. Cheng, F. Li,, and J. Chen,, “A Solid Lithium Superionic Conductor Li11AlP2S12 with a Thio-LISICON Analogous Structure,” Chem Commun, 52 [36] 6091-94 (2016).
47. R. Kanno, and M. Murayama,, “Lithium Ionic Conductor Thio-LISICON: The Li2S GeS2 P2S5 System,” J Electrochem Soc, 148 [7] A742-46 (2001).
48. Y. Inaguma, L. Chen, M. Itoh,, and T. Nakamura,, “Candidate Compounds with Perovskite Structure for High Lithium Ionic Conductivity,” Solid State Ionics, 70 196-202 (1994).
49. S. García-Martína, JM. Rojob, H. Tsukamotoc, E. Morána,, and MA. Alario-Francoa,, “Lithium-Ion Conductivity in the Novel La1/3− x Li3xNbO3 Solid Solution with Perovskite-Related Structure,” Solid State Ionics, 116 [1] 11-8 (1999).
50. L. Latie, G. Villeneuve, D. Conte,, and G. Le Flem, “Ionic Conductivity of Oxides with General Formula LixLn1/3Nb1− xTixO3 (Ln= La, Nd),” J Solid State Chem, 51 [3] 293-99 (1984).
51. AG. Belous, GN. Novitskaya, SV. Polyanetskaya, and YI. Gornikon, “Investigation into Complex Oxides of La2/3− xLi3xTiO3 Composition,” Izv Akad Nauk SSSR, Neorg Mater, 23 [3] 470-72 (1987).

52. X. Lu, “Effect of Microstructure on the Mechanical, Thermal, and Electronic Property Measurement of Ceramic Coatings,” Int J Miner Metall Mater, 21 [11] 1127-31 (2014).
53. CW. Ban, and GM. Choi, “The Effect of Sintering on the Grain Boundary Conductivity of Lithium Lanthanum Titanates,” Solid State Ionics, 140 [3] 285-92 (2001).
54. M. Itoh, Y. Inaguma, WH. Jung, L. Chen, and T. Nakamura, “High Lithium Ion Conductivity in the Perovskite-type Compounds Ln1/2Li1/2TiO3 (Ln = La,Pr,Nd, Sm),” Solid State Ionics, 70 203-7 (1994).
55. G. Schwering, A. Honerscheid, L. Wullen, and M. Jansen, “High Lithium Ionic Conductivity in the Lithium Halide Hydrates Li3−n(OHn)Cl (0.83 ≤ n ≤ 2) and Li3−n(OHn)Br (1 ≤ n ≤ 2) at Ambient Temperatures,” Chem Phys Chem, 4 [4] 343-48 (2003).

56. MH. Braga, JA. Ferreira, V. Stockhausen, JE. Oliveira, and A. El-Azab, “Novel Li3ClO based Glasses with Superionic Properties for Lithium Batteries,” Mater Chem A, 2 [15] 5470-80 (2014).
57. Z. Lu, C. Chen, ZM. Baiyee, X. Chen, C. Niu, and F. Ciucci, “Defect Chemistry and Lithium Transport in Li3OCl Antiperovskite Superionic Conductors,” Phys Chem Chem Phys, 17 [48] 32547-55 (2015).
58. M. Bilal, SJ. Asadabadi, R. Ahmad, and I. Ahmad, “Electronic Properties of Antiperovskite Materials from State-of-the-Art Density Functional Theory,” J Chem, 2015 1-11 (2015).
crossref pdf
59. KS. Lee, SY. Shin, and YS. Yoon, “Fe3O4 Nanoparticles on MWCNTs Backbone for Lithium Ion Batteries,” J Korean Ceram Soc, 53 [3] 376-80 (2016).
crossref pdf
60. MV. Reddy, GV. Subba Rao, and BVR. Chowdari, “Metal Oxides and Oxysalts as Anode Materials for Li Ion Batteries,” Chem Rev, 113 [7] 5364-457 (2013).
61. WJ. Zhang, “A Review of the Electrochemical Performance of Alloy Anodes for Lthium-Ion Batteries,” J Power Sources, 196 [1] 13-24 (2011).
62. HG. Jung, ST. Myung, CS. Yoon, SB. Son, KH. Oh, K. Amine, B. Scrosati, and YK. Sun, “Microscale Sherical Crbon-Cated Li4Ti5O12 as Urahigh Power Anode Material for Lithium Batteries,” Energy Environ Sci, 4 1345-51 (2011).
63. M. Wakihara, Y. Kadoma, N. Kumagai, H. Mita, R. Araki, K. Ozawa, and Y. Ozawa, “Development of Nonflammable Lithium Ion Battery using a New All-Solid Polymer Electrolyte,” J Solid State Electrochem, 16 [3] 847-55 (2012).
64. B. Tian, H. Xiang, L. Zhang, Z. Li, and H. Wang, “Niobium Doped Lithium Titanate as a High Rate Anode Material for Li-ion Batteries,” Electrochim Acta, 55 [19] 5453-58 (2010).
65. Y. Takeda, M. Nishijima, M. Yamahata, K. Takeda, N. Imanishi, and O. Yamamoto, “Lithium Secondary Batteries Using a Lithium Cobalt Nitride, Li2.6Co0.4N, as the Anode,” Solid State Ionics, 130 61-9 (2000).
66. NS. Choi, JS. Yin, RZ. Kim, and SS. Kim, “Electrochemical Properties of Lithium Vanadium Oxide as an Anode Material for Lithium-ion Battery,” Mater Chem Phys, 116 [2] 603-6 (2009).
67. JF. Colin, VPV. Caignaert, M. Hervieu, and B. Raveau, “A Novel Layered Titanoniobate LiTiNbO5: Topotactic Synthesis and Electrochemistry Versus Lithium,” Inorg Chem, 45 [18] 7217-23 (2006).
68. ZX. Lin, HJ. Yu, SC. Li, and SB. Tian, “Lithium ion Conductors based on LiTi2P3O12 Compound,” Solid State Ionics, 31 [2] 91-4 (1988).
69. REH. Clark, and DH. Reiter, Nuclear Fusion Research: Understanding Plasma-Surface Interactions; 78 pp. 3-26 Springer, Berlin, 2005.

70. R. Kodama, H. Shiraga, K. Shigemori, Y. Toyama, S. Fujioka, H. Azechi, H. Fujita, H. Habara, T. Hall, Y. Izawa, T. Jitsuni, Y. Kitagawa, KM. Krushelnick, KL. Lancaster, K. Mima, K. Nagai, M. Nakai, H. Nishimura, T. Norimatsu, PA. Norreys, S. Sakabe, KA. Tanaka, A. Youssef, M. Zepf, and T. Yamanaka, “Nuclear Fusion: Fast Heating Scalable to Laser Sufion Ignition,” Nature, 418 [6901] 933-34 (2002).
71. PC. Stangeby, and GM. McCracken, “Plasma Boundary Phenomena Ion Tokamaks,” Nucl Fusion, 30 [7] 1225(1990).
72. B. LaBombard, JE. Rice, AE. Hubbard, JW. Hughes, M. Greenwald, J. Irby, Y. Lin, B. Lipschultz, ES. Marmar, and CS. Pitcher, “Transport-Driven Scrape-Off-Layer Flows and the Boundary Conditions Imposed at the Magnetic Separatrix in a Tokamak Plasma,” Nucl Fusion, 44 [10] 1047(2004).
73. PN. Yushmanov, T. Takizuka, KS. Riedel, OJWF. Kardaun, JG. Cordey, SM. Kaye, and DE. Post, “Scalings for Tokamak Energy Confinement,” Nucl Fusion, 30 [10] 1999(1990).
74. MN. Rosenbluth, and SV. Putvinski, “Theory for Avalanche of Runaway Electrons in Tokamaks,” Nucl Fusion, 37 [10] 1355(1997).
75. N. Taylor, and P. Cortes, “Lessons Learnt from ITER Safety & Licensing for DEMO and Future Nuclear Fusion Facilities,” Fusion Eng Des, 89 [9-10] 1995-2000 (2014).
76. FJ. Casson, E. Poli, C. Angioni, R. Buchholz, and AG. Peeters, “Effect of Turbulence on Electron Cyclotron Current Drive and Heating in ITER,” Nucl Fusion, 55 [1] 012002(2015).
77. DW. Lee, BG. Hong, YH. Kim, WK. In, and KH. Yoon, “Preliminary Design of a Helium Cooled Molten Lithium test Blanket Module for the ITER Test in Korea,” Fusion Eng Des, 82 [4] 381-88 (2007).
78. GS. Lee, J. Kim, SM. Hwang, CS. Chang, HY. Chang, MH. Cho, BH. Choi, K. Kim, KW. Cho, and S. Cho, “The KSTAR Project: An Advanced Steady State Superconducting Tokamak Experiment,” Nucl Fusion, 40 [3Y] 575(2000).
79. M. Glugla, D. Babineau, L. Bo, S. Maruyama, R. Pearce, G. Piazza, B. Rogers, S. Willms, T. Yamanishi, and SH. Yun, “Review of the ITER D-T Fuel Cycle Systems and Recent Progress,” pp. 24-9 In: 9th International Conference on Tritium Science and Technology; Tritium, Japan. 2010.

80. H. Kawamura, E. Ishitsuka, K. Tsuchiya, M. Nakamichi, M. Uchida, H. Yamada, K. Nakamura, H. Ito, T. Nakazawa, and H. Takahashi, “Development of Advanced Blanket Materials for a Solid Breeder Blanket of a Fusion Reactor,” Nucl Fusion, 43 [8] 675(2003).
81. M. Enoeda, Y. Kosaku, T. Hatano, T. Kuroda, N. Miki, T. Honma, M. Akiba, S. Konishi, H. Nakamura, and T. Kawamura, “Design and Technology Development of Solid Breeder Blanket Cooled by Supercritical Water in Japan,” Nucl Fusion, 43 [12] 1837(2003).
82. M. Nishikawa, T. Kinjyo, T. Ishizaka, S. Beloglazov, T. Takeishi, M. Enodeda, and T. Tanifuji, “Release Behavior of Bred Tritium from LiAlO2,” J Nucl Mater, 335 [1] 70-6 (2004).
83. AR. Raffray, M. Akiba, V. Chuyanov, L. Giancarli, and S. Malang, “Breeding Blanket Concepts for Fusion and Materials Requirements,” J Nucl Mater, 307 21-30 (2002).
84. JG. van der Laan, H. Kawamura, N. Roux, and D. Yamaki, “Ceramic Breeder Research and Development: Progress and Focus,” J Nucl Mater, 283 99-109 (2000).
85. CE. Johnson, “Ceramic Breeder Materials,” Ceram Int, 17 [4] 253-58 (1991).
86. GW. Hollenberg, “Fast Neutron Irradiation Results on Li2O, Li4SiO4, Li2ZrO3 and LiAlO2,” J Nucl Mater, 123 [1-3] 896-900 (1984).
87. JL. Ethridge, and DE. Baker, “Effects of Fast Neutron Irradiation on Thermal Conductivity of Li2O and LiAlO2,” J Am Ceram Soc, 71 [6] C294-96 (1988).
88. J. Kin, Z. Wen, X. Xu, N. Li, and S. Song, “Characterization and Improvement of Water Compatibility of γ-LiAlO2 Ceramic Breeders,” Fusion Eng Des, 85 [7-9] 1162-66 (2010).
89. J. Han, X. Gao, Y. Gong, X. Chen, and CT. Yang, “Fabrication of a Li4SiO4-Pbtritium Breeding Material,” Fusion Eng Des, 89 [12] 3046-53 (2014).
90. L. Guo, X. Wang, S. Zhang, C. Zhong, and L. Li, “Effect of Alkalinity on the Hydrothermal Synthesis of Li2ZrO3 Nano Tube Arrays,” J Mater Sci, 46 6960-63 (2011).
91. YH. Park, SY. Cho, and MY. Ahn, “Fabrication of Li2− TiO3 Pebbles Using PVA-Boric Acid Reaction for Solid Breeding Materials,” J Nucl Mater, 455 [1-3] 106-10 (2014).
92. KM. Min, YH. Park, and SY. Cho, “Synthesis of Li2TiO3 Powder with High Crystalline Structure for Tritium Breeding Material by Ion-Exchange Process,” Fusion Eng Des, 109 326-29 (2016).
93. CE. Johnson, “Tritium Behavior in Lithium Ceramics,” J Nucl Mater, 270 [1-2] 212-20 (1999).
94. P. Gierszewski, M. Dalle Donne, H. Kawamura, and M. Tillack, “Ceramic Pebble Bed Development for Dusion Blankets,” Fusion Eng Des, 27 167-78 (1995).
95. G. Piazza, J. Reimann, E. Gunther, R. Knitter, N. Roux, and JD. Lulewicz, “Characterization of Ceramic Breeder Materials for the Helium Cooled Pebble Bed Blanket,” J Nucl Mater, 307 811-16 (2002).
96. MW. Yu, YH. Park, and SJ. Lee, “Fabrication of Li2TiO3 Pebbles by Lithium Solution Penetration Method,” J Korean Ceram Soc, 50 [5] 333-40 (2013).
97. G. Dell’Orco, A. Ancona, A. Dimaio, M. Simoncini, and G. Vella, “Thermo-Mechanical Testing of Li-Ceramic for the Helium Cooled Pebble Bed (HCPB) Breeding Blanket,” J Nucl Mater, 329 1305-8 (2004).
98. A. Abou-Sena, A. Ying, and M. Abdou, “Effective Thermal Conductivity of Lithium Ceramic Pebble Beds for Fusion Blankets: A Review,” Fusion Sci Technol, 47 [4] 1094-100 (2005).
99. J. Ongena, and Y. Ohawa, “Nuclear Fusion: Status Report and Future Prospects,” Energ Policy, 96 770-78 (2016).
PDF Links  PDF Links
PubReader  PubReader
ePub Link  ePub Link
Full text via DOI  Full text via DOI
Download Citation  Download Citation
Related article
Editorial Office
Meorijae Bldg., Suite # 403, 76, Bangbae-ro, Seocho-gu, Seoul 06704, Korea
TEL: +82-2-584-0185   FAX: +82-2-586-4582   E-mail: ceramic@kcers.or.kr
About |  Browse Articles |  Current Issue |  For Authors and Reviewers
Copyright © The Korean Ceramic Society.                      Developed in M2PI