Patent Application
20140294720
1. Field of the Invention
The present invention relates to a precursor solution used to form a LiCoO2 film and a method of forming a LiCoO2 film using this solution.
Priority is claimed on Japanese Patent Application No. 2013-065839, filed on Mar. 27, 2013, the content of which is incorporated herein by reference.
2. Description of Related Art
Japanese Unexamined Patent Application, First Publication No. 2008-159399 discloses a lithium ion secondary battery. This lithium ion secondary battery is a thin film solid secondary battery in which a positive electrode collector layer including a positive electrode collector, a positive electrode active material layer including a positive electrode active material, a solid electrolyte layer including an electrolyte, a negative electrode active material layer including a negative electrode active material, and a negative electrode collector layer including a negative electrode collector are laminated on a substrate. The positive electrode active material layer contains one or two or more oxides selected from the group consisting of lithium-manganese oxides, lithium-cobalt oxides, lithium-nickel oxides, lithium-manganese-cobalt oxides, and lithium-titanium oxides (for example, refer to claims 5, 7, and 9 and paragraphs [0024], [0026], and [0041]). In this lithium ion secondary battery, the positive electrode collector layer, the positive electrode active material layer, the solid electrolyte layer, the negative electrode active material layer, and the negative electrode collector layer are formed by sputtering. In addition, as the lithium-manganese oxides, LiMn2O4, Li2Mn2O4, or the like can be used. As the lithium-cobalt oxides, LiCoO2, LiCo2O4, or the like can be used.
In the lithium ion secondary battery configured as above, a lithium-manganese oxide, a lithium-cobalt oxide, or the like from which or on which lithium ions can be desorbed or adsorbed is used as a positive electrode active material. As a result, many lithium ions can be stored in or released from the positive electrode active material, and charge-discharge characteristics of the lithium ion secondary battery are further improved. In addition, by forming the positive electrode active material layer and the like using sputtering, the time required to manufacture a lithium ion secondary battery, particularly, a thin film solid secondary battery can be reduced.
Meanwhile, Japanese Unexamined Patent Application, First Publication No. 2010-083700 discloses a laminate including: a substrate; and a cobalt oxide film formed of a plurality of single crystals of a cobalt oxide that are grown on a surface of the substrate, in which the cobalt oxide is formed of Co, O, and a doping metal element, and the doping metal element is Li, Na, or Ca (for example, refer to claims 1 to 3 and paragraphs [0022], [0077], and [0078]). In order to form the cobalt oxide film of the laminate, first, cobalt nitrate (Co source), lithium nitrate (Li source), and a mixed solution containing 80 mass % of water (solvent) and 20 mass % of acetyl acetone are prepared. Next, 0.1 mol/L of the cobalt nitrate and 0.05 mol/L of the lithium nitrate are dissolved in this mixed solution, thereby obtaining 100 mL of a cobalt oxide film-forming solution. Further, a substrate (slide glass) is heated to 400° C. using a hot plate, and 100 mL of the cobalt oxide film-forming solution is sprayed on the substrate using an ultrasonic nebulizer, thereby forming a cobalt oxide film on the substrate.
In the laminate configured as above, since the cobalt oxide film is formed of the single crystals of the cobalt oxide, typically, substantially no crystal defects or impurities are present, and the interface resistance between particles is lower than that of a cobalt oxide film obtained by allowing particles of a cobalt oxide to aggregate. Therefore, when a specific carrier is conducted in the cobalt oxide film, the conductivity of this carrier can be improved. Specifically, when the cobalt oxide film is formed of single crystals of LiCoO2, the laminate can be used as a positive electrode having superior lithium conductivity and electron conductivity.
Meanwhile, Y. H. Rho, K. Kanamura, T. Umegaki, J. Electrochem. Soc., 150[1] (2003), pp. A107 to A111 discloses a technique of forming a LiCoO2 or LiMn2O4 thin film electrode for a rechargeable Li battery with a sol-gel method using polyvinyl pyrrolidone (PVP) (for example, refer to Abstract,
As a result of investigating properties of the formed thin film by X-ray diffractionand an observation using a scanning electron microscope, it was found that the gel films formed using the Li—Co—O sol and the Li—Mn—O sol were LiCoO2 having a rock salt type structure and LiMn2O4 having a spinel structure, respectively. In addition, as a result of evaluating electrochemical properties of the thin films by a charge-discharge test and cyclic voltammetry in a mixed solution of ethylene carbonate and diethyl carbonate (volume ratio=1:1) containing 1.0 mol/dm3 of LiClO4, it was found that these thin films had superior electrochemical properties as electrodes.
Meanwhile, H. Porthault, F. Le Cras, S. Franger, J. Power Sources, 195[19] (2010), pp. 6262 to 6267 discloses a technique of synthesizing a LiCoO2 thin film with a sol-gel method in which acrylic acid (AA) is used as a chelating agent (for example, refer to Abstract, line 5 from the bottom of the lower right column of p. 6262 to line 10 from the top of the upper left column of p. 6263, and line 4 from the top of the right column of p. 6267 to line 7 from the top of the same column of the same page). In this technique of synthesizing a LiCoO2 thin film with a sol-gel method, in order to form a dense film as a positive electrode of a lithium battery, a method of forming a gel is optimized by controlling various solvents (ethylene glycol or water) and a molar ratio of precursors (Li, Co, and AA). Specifically, a LiCoO2 material is synthesized with a sol-gel method. First, salts such as lithium acetate (Li(CH3CO2).H2O) and cobalt acetate (CO(CH3CO2)2.4H2O) are dissolved in a solvent (distilled water (W) or ethylene glycol (EG)), followed by mixing with acrylic acid (AA). In this process, acrylic acid functions as a chelating agent to obtain a gel. In addition, the molar ratio Li:Co varies in a range from 1:0 to 1:1, and the molar ratio of the total metallic ions charges (M+) to acrylic acid (AA) varies in a range from 1:0 to 1:1. The obtained solution was stirred at a temperature of 75° C. for 24 hours. In the case of an aqueous solution, the solution is evaporated by being held at 75° C. for several hours until an ultraviolet gel having a desired viscosity is obtained. In the case of an ethylene glycol solution, a desired viscosity is directly obtained by changing the entire concentration of the initial composition of a reactant. Further, a SiO2 film, a SiN film, a TiO2 film, and an Au film are laminated on a Si substrate in this order, and the gel is formed by spin coating on the Au film, which is highest, as a gel film. The gel film formed on the Si substrate is baked at 800° C. for 5 hours, thereby forming a thin film. In order to increase the density of the thin film, this baking is performed to obtain an R-3m phase (HT-LiCoO2) after depositing the gel film through a process including one or plural steps.
The chemical properties of the gel prepared as above are investigated by Fourier-transform infrared (FTIR) spectroscopy, and the crystallinity of the thin film formed as above is analyzed by X-ray diffraction (XRD). As a result, it was able to be confirmed from infrared spectra of the gel obtained by FTIR spectroscopy that acrylic acid functioned as a chelating agent used to form a gel immediately after being present in the solution without the necessity of heating. In addition, it was found from a X-ray pattern of the thin film obtained by XRD that the R-3m phase of LiCoO2 was obtained by a heat treatment at 800° C.
However, in the lithium ion secondary battery disclosed in Japanese Unexamined Patent Application, First Publication No. 2008-159399 of the related art, since the positive electrode active material layer and the like are formed by sputtering, it is necessary for a large-sized sputtering device be used, and thus there is a problem in that the manufacturing costs are increased. In addition, in the laminate disclosed in Japanese Unexamined Patent Application. First Publication No. 2010-083700 of the related art, since cobalt acetate and lithium acetate are dissolved in a mixed solution of water and acetyl acetone, highly reactive nitrogen monoxide or nitrogen dioxide may be produced during film formation depending on film forming processes, and thus there is a problem in that stable film formation cannot be performed. Further in the technique of forming a thin film electrode of LiCoO2 or the like with a sol-gel method disclosed in Y. H. Rho, K. Kanamura, T. Umegaki, J. Electrochem. Soc., 150[1] (2003), pp. A107 to A111 of the related art and in the technique of synthesizing a LiCoO2 thin film with a sol-gel method disclosed in H. Porthault, F. Le Gras, S. Franger, J. Power Sources, 195[19] (2010), pp. 6262 to 6267 of the related art, since an acetate is used for preparing a gel solution, precipitates are likely to be formed, and thus there is a problem in that the storage stability is poor.
A first object of the invention is to provide a method of forming a LiCoO2 film using a LiCoO2 film-forming precursor solution, in which the LiCoO2 film-forming precursor solution can be coated on the substrate through a relatively simple process without using a large-sized sputtering device, and film formability is superior. A second object of the invention is to provide a LiCoO2 film-forming precursor solution having superior storage stability.
According to a first aspect of the invention, there is provided a LiCoO2 film-forming precursor solution used to form a LiCoO2 film which is used as a positive electrode material of a thin film lithium secondary battery, the LiCoO2 film-forming precursor solution including: an organic lithium compound; an organic cobalt compound; and an organic solvent, in which the organic lithium compound is a lithium salt of a carboxylic acid represented by a formula CnH2n+1COOH (wherein, 2≦n≦8).
According to a second aspect of the invention, in the LiCoO2 film-forming precursor solution according to the first aspect, the organic cobalt compound is preferably a cobalt salt of a carboxylic acid represented by a formula CnH2n+1COOH (wherein, 2≦n≦8):
According to a third aspect of the invention, in the LiCoO2 film-forming precursor solution according to the first or second aspect, the organic lithium compound is preferably a lithium salt of 2-ethylbutyric acid or 2-ethylhexanoic acid, and the organic cobalt compound is preferably a cobalt salt of 2-ethylbutyric acid or 2-ethylhexanoic acid.
According to a fourth aspect of the invention, in the LiCoO2 film-forming precursor solution according to any one of the first to third aspects, the organic solvent is preferably 1-butanol, 2-ethylbutrylic acid, 2-ethylhexanoic acid, or 3-methylbutyl acetate.
According to a filth aspect of the invention, there is provided a method of forming a LiCoO2 film, in which the LiCoO2 film-forming precursor solution according to any one of the first to fourth aspects is coated on a substrate to be used as a positive electrode material of a thin film lithium secondary battery.
According to a sixth aspect of the invention, there is provided a method of manufacturing a thin film lithium secondary battery which includes a LiCoO2 film formed using the method according to the fifth aspect.
The LiCoO2 film-forming precursor solution according to the first aspect contains: an organic lithium compound; an organic cobalt compound; and an organic solvent, in which the organic lithium compound is a lithium salt of a carboxylic acid represented by a formula CnH2n+1COOH (wherein, 2≦n≦8). As a result, a precursor solution having superior lipophilicity and superior storage stability can be obtained.
In the LiCoO2 film-forming precursor solution according to the second aspect, the organic cobalt compound is a cobalt salt of a carboxylic acid represented by a formula CnH2n+1COOH (wherein, 2≦n≦8). As a result, a precursor solution having superior lipophilicity and superior storage stability can be obtained.
In the method of forming a LiCoO2 film according to the fifth aspect, the LiCoO2 film-forming precursor solution according to any one of the first to fourth aspects is coated on a substrate. As a result, the LiCoO2 film-forming precursor solution can be uniformly coated on the substrate through a relatively simple process without using a large-sized sputtering device.
Next, embodiments of the invention will be described with reference to the drawings. A LiCoO2 film-forming precursor solution according to an embodiment of the invention is a precursor solution used to form a LiCoO2 film which is used as a positive electrode material of a thin film lithium secondary battery. This precursor solution contains an organic lithium compound, an organic cobalt compound, and an organic solvent. It is preferable that, in this precursor solution, the organic lithium compound and the organic compound be dissolved in the organic solvent.
The organic lithium compound is a lithium salt of a carboxylic acid represented by a formula CnH2n+1COOH (wherein, 2≦n≦8). The reason for limiting n to be in the range of 2≦n≦8 is as follows. When n is less than 2, the storage stability of the precursor solution is poor, and precipitates are likely to be formed. When n is more than 8, storage stability in a part of carboxylic acids is poor, and precipitates are likely to be formed.
Examples of the organic lithium compound include lithium salts of propionic acid (propanoic acid; n=2), n-butyric acid (butanoic acid; n=3), pentanoic acid (n-valeric acid; n=4), hexanoic acid (n-caproic acid; n=5), 2-ethylbutyic acid (2-ethylbutanoic acid; n=5), heptanoic acid (n-enanthic acid; n=6), octanoic acid (n-caprylic acid; n=7), 2-ethylhexanoic acid (2-ethylcaproic acid; n=7), and nonanoic acid (n-pelargonic acid; n=8). Among these lithium salts, a lithium salt of 2-ethylbutyric acid (n=5) or a lithium salt of 2-ethylhexanoic acid (n=7) is particularly preferably used.
As the organic cobalt compound, a cobalt salt of a carboxylic acid represented by a formula CnH2n+1COOH (wherein, 2≦n≦8) is preferably used.
Examples of the organic cobalt compound include cobalt salts of propionic acid (n=2), n-butyric acid (n=3), pentanoic acid (n=4), hexanoic acid (n=5), 2-ethylbutyic acid (n=5), heptanoic acid (n=6), octanoic acid (n=7), 2-ethylhexanoic acid (n=7), and nonanoic acid (n=8). Among these cobalt salts, a cobalt salt of 2-ethylbutyric acid (n=5) or a cobalt salt of 2-ethylhexanoic acid (n=7) is particularly preferably used.
As the organic solvent, for example, 1-butanol, 2-ethylbutrylic acid, 2-ethylhexanoic acid, or 3-methylbutyl acetate (isoamyl acetate) is preferably used. Among these organic solvents, 1-butanol is particularly preferably used.
A method of preparing the LiCoO2 film-forming precursor solution configured as above will be described. First, a Li source of the organic lithium compound, a Co source of the organic cobalt compound, and a carboxylic acid (represented by the formula CnH2n+1COOH (wherein 2≦n≦8)) are put into a reaction vessel with a predetermined ratio, followed by reflux in a nitrogen atmosphere, an argon gas atmosphere, or an inert gas atmosphere. As a result, the organic lithium compound and the organic cobalt compound are synthesized.
Examples of the Li source of the organic lithium compound include lithium carbonate or the like. Examples of the Co source of the organic cobalt compound include cobalt carbonate or the like.
Next, this synthesized solution is distillated under reduced pressure to remove by-products such as water or carbon dioxide from the solution. This solution is diluted with the organic solvent such as 1-butanol, 2-ethylbutrylic acid, 2-ethylhexanoic acid, or 3-methylbutyl acetate.
Further, the solution diluted with the organic solvent is filtered to remove particles of by-products from the solution. As a result, a LiCoO2 film-forming precursor solution, which contains metal compounds having a ratio of metals, that is, a mass ratio of Li to Co of 1:1 and a concentration of 1 mass % to 20 mass % in terms of oxides, is obtained.
In addition, the ratio in terms of oxides refers to a ratio of metal oxides to 100 mass % of the precursor solution used to form a LiCoO2 film which is calculated under the assumption that all of Li and Co in the precursor solution used to form a LiCoO2 film are converted into the metal oxides.
In the LiCoO2 film-forming precursor solution prepared as above, the organic lithium compound and the organic cobalt compound are dissolved in the organic solvent, and the organic lithium compound is a lithium salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, 2≦n≦8). As a result, a precursor solution having superior lipophilicity and superior storage stability can be obtained. In addition, the organic cobalt compound is a cobalt salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, 2≦n≦8). As a result, a precursor solution having superior lipophilicity and superior storage stability can be obtained.
A method of forming a LiCoO2 film on a substrate using the LiCoO2 film-forming precursor solution prepared as above to manufacture a positive electrode material will be described based on
Next, the coating films on the platinum layers 11d and 31c of the substrates 11 and 31 are dried by being held in the air at a temperature of 150° C. to 550° C. for 1 minute to 30 minutes. The thickness of a dried coating film formed per each coating process is preferably about 30 nm to 200 nm. Next, after the coating process and the drying process are repeated a predetermined number of times (for example, about 5 times to 50 times), the coating films on the platinum layers 11d and 31c of the substrates 11 and 31 are baked by rapid thermal annealing (RTA) by being held in an oxygen atmosphere at a temperature of 350° C. to 800° C. (a crystallization temperature or higher of the coating films) for 1 minute to 60 minutes. As a result, LiCoO2 films 12 and 32 having a thickness of about 1 μm to 10 μm can be formed on the platinum layers 11d and 31c of the substrates 11 and 31.
A method of confirming that the LiCoO2 films formed as above have properties as positive electrode materials 10 and 30 of a thin film lithium secondary battery will be described.
By supplying power such that the platinum layers below the LiCoO2 films are positive electrodes, the LiCoO2 films and the substrates are set as positive electrode materials, and metallic lithium which is a negative electrode is set as a negative electrode material. Next, 1 mol/dm3 of lithium hexafluorophosphate (LiPF6) is dissolved in a solvent, which is obtained by mixing ethylene carbonate and diethyl carbonate with a volume ratio of 1:1, to prepare an electrolyte solution. This electrolyte solution is put into a glass vessel, and the positive electrode material and the negative electrode material are dipped therein. In a state where the positive electrode and the negative electrode are exposed to the outside of the vessel, the vessel is filled with argon gas and is sealed in an argon gas atmosphere. As a result, a beaker cell type secondary battery structure is formed. In the beaker cell type secondary battery prepared as above, lithium ions contained in the LiCoO2 film can be adsorbed or desorbed, and battery characteristics can be exhibited.
Next, Examples of the invention and Comparative Examples will be described in detail.
First, lithium carbonate (Li source of the organic lithium compound), cobalt carbonate (Ca source of the organic cobalt compound), and 2-ethylbutyric acid (represented by the formula C5H11COOH) were put into a reaction vessel with a molar ratio Li:Co:C5H11COOH of 1:1:7, followed by reflux in a nitrogen atmosphere. As a result, a solution in which lithium 2-ethylbutyrate (a lithium salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=5)) and cobalt 2-ethylbutyrate (a cobalt salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=5)) were synthesized was obtained. Next, this solution was distillated under reduced pressure to remove by-products such as water or carbon dioxide from the solution. This solution was diluted with the addition of 1-butanol such that the concentration of the total amount of Li and Co was 5 mass % in terms of metal oxides. The diluted solution was filtered to removed particles of by-products from the solution. As a result, a LiCoO2 film-forming precursor solution, which contains metal compounds having a ratio of metals, that is, a mass ratio of Li to Co of 1:1 and a concentration of 5 mass % in terms of oxides, was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 1.
Lithium carbonate (Li source of the organic lithium compound), cobalt carbonate (Ca source of the organic cobalt compound), and 2-ethylhexanoic acid (represented by the formula C7H15COOH) were put into a reaction vessel with a molar ratio Li:Co:C7H15COOH of 1:1:7, followed by reflux in a nitrogen atmosphere. As a result, a solution in which lithium 2-ethylhexanoate (a lithium salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=7)) and cobalt 2-ethylhexanoate (a cobalt salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=7)) were synthesized was obtained. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 2.
Lithium carbonate (Li source of the organic lithium compound), cobalt carbonate (Ca source of the organic cobalt compound), and propionic acid (represented by the formula C2H5COOH) were put into a reaction vessel with a molar ratio Li:Co:C2H5COOH of 1:1:7, followed by reflux in a nitrogen atmosphere. As a result, a solution in which lithium propionate (a lithium salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=2)) and cobalt propionate (a cobalt salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=2)) were synthesized was obtained. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 3.
Lithium carbonate (Li source of the organic lithium compound), cobalt carbonate (Ca source of the organic cobalt compound), and pentanoic acid (represented by the formula C4H9COOH) were put into a reaction vessel with a molar ratio Li:Co:C4H9COOH of 1:1:7, followed by reflux in a nitrogen atmosphere. As a result, a solution in which lithium pentanoate (a lithium salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=4)) and cobalt pentanoate (a cobalt salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=4)) were synthesized was obtained. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 4.
Lithium carbonate (Li source of the organic lithium compound), cobalt carbonate (Ca source of the organic cobalt compound), and nonanoic acid (represented by the formula C8H17COOH) were put into a reaction vessel with a molar ratio Li:Co:C8H17COOH of 1:1:7, followed by reflux in a nitrogen atmosphere. As a result, a solution in which lithium nonanoate (a lithium salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=8)) and cobalt nonanoate (a cobalt salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=8)) were synthesized was obtained. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 5.
The solution, which was synthesized and distillated under reduced pressure to remove by-products from the solution with the same method as that of Example 1, was diluted with the addition of 2-ethylbutyric acid such that the concentration of the total amount of Li and Co was 5 mass % in terms of metal oxides. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 6.
The solution, which was synthesized and distillated under reduced pressure to remove by-products from the solution with the same method as that of Example 1, was diluted with the addition of 2-ethylhexanoic acid such that the concentration of the total amount of Li and Co was 5 mass % in terms of metal oxides. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 7.
The solution, which was synthesized and distillated under reduced pressure to remove by-products from the solution with the same method as that of Example 1, was diluted with the addition of 3-methylbutyl acetate such that the concentration of the total amount of Li and Co was 5 mass % in terms of metal oxides. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 8.
The solution, which was synthesized and distillated under reduced pressure to remove by-products from the solution with the same method as that of Example 1, was diluted with the addition of 1-propanol such that the concentration of the total amount of Li and Co was 5 mass % in terms of metal oxides. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Example 9.
Lithium carbonate (Li source of the organic lithium compound), cobalt carbonate (Ca source of the organic cobalt compound), and acetic acid (represented by the formula CH3COOH) were put into a reaction vessel with a molar ratio Li:Co:CH3COOH of 1:1:7, followed by reflux in a nitrogen atmosphere. As a result, a solution in which lithium acetate (a lithium salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=1)) and cobalt acetate (a cobalt salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=1)) were synthesized was obtained. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Comparative Example 1.
Lithium carbonate (Li source of the organic lithium compound), cobalt carbonate (Ca source of the organic cobalt compound), and decanoic acid (represented by the formula C9H19COOH) were put into a reaction vessel with a molar ratio Li:Co:C9H19COOH of 1:1:7, followed by reflux in a nitrogen atmosphere. As a result, a solution in which lithium decanoate (a lithium salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=9)) and cobalt decanoate (a cobalt salt of a carboxylic acid represented by the formula CnH2n+1COOH (wherein, n=9)) were synthesized was obtained. With the same method as that of Example 1 except for the above-described configurations, a LiCoO2 film-forming precursor solution was obtained. This LiCoO2 film-forming precursor solution was set as the solution of Comparative Example 2.
Each of the LiCoO2 film-forming precursor solutions of Examples 1 to 9 and Comparative Examples 1 and 2 was put into a vessel, an opening of this vessel was sealed with a cover, and the vessel is left to stand at room temperature for 1 day. Then, whether or not precipitates were formed in the precursor solution was investigated by visual inspection. The results are shown in Table 1.
As illustrated in
As illustrated in
As clearly seen from Table 1, the following results were obtained. In the precursor solution of Comparative Example 1, precipitates were formed after being left to stand at room temperature for 1 day. On the other hand, in the precursor solutions of Examples 1 to 9, precipitates were not formed even after being left to stand at room temperature for 1 day, and storage stability was superior. In addition, in the precursor solution of Comparative Example 2, the wettability was poor, and the solution was not absorbed. On the other hand, in the precursor solutions of Examples 1 to 9, the wettability was superior, and the precursor solution was uniformly coated on the substrate. In addition, in the LiCoO2 films of Examples 3 to 5, the peak intensity values of the crystal plane were low in a range from 484 counts to 725 counts, respectively. On the other hand, in the LiCoO2 films of Examples 1 to 2, the peak intensity values of the crystal plane were high at 1553 counts and 1624 counts, respectively. It can be seen from the above results that, when 2-ethylbutylate or 2-ethylhexanoate is used as the organic lithium compound and the organic cobalt compound dissolved in the precursor solution, a LiCoO2 film having higher crystallinity can be formed as compared to cases where propionate, pentanoate, or nonanoate is used as the organic lithium compound and the organic cobalt compound. Further, in the LiCoO2 film of Example 9, the peak intensity value of the crystal plane was low at 851 counts. On the other hand, in LiCoO2 films of Example 1 and 6 to 8, the peak intensity values of the crystal plane were high in a range from 1223 counts to 1624 counts, respectively. It can be seen from the above results that, 1-butanol, 2-ethylbutyric acid, 2-ethylhexanoic acid, or 3-methylbutyl acetate is used as the organic solvent for diluting the solution, a LiCoO2 film having higher crystallinity can be formed as compared to cases where 1-propnaol is used as the organic solvent.
While preferred embodiments of the invention have been described and illustrated above, it should be understood that these are exemplary of the invention and are not to be considered as limiting. Additions, omissions, substitutions, and other modifications can be made without departing from the spirit or scope of the present invention. Accordingly, the invention is not to be considered as being limited by the foregoing description, and is only limited by the scope of the appended claims.
| Number | Date | Country | Kind |
|---|---|---|---|
| 2013-065839 | Mar 2013 | JP | national |
