{"title":"Uptake of 131I, 134Cs and 137Cs in tulip (Tulipa gesneriana L.) after the Fukushima Daiichi nuclear accident and their translocation from its above ground parts to the bulb","authors":"K. Tagami, S. Uchida, Y. Uchihori, H. Kitamura","doi":"10.14494/jnrs.22.1","DOIUrl":"https://doi.org/10.14494/jnrs.22.1","url":null,"abstract":"","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"24 1","pages":""},"PeriodicalIF":0.0,"publicationDate":"2022-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"81197212","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
N. Kinoshita, Yuya Yoda, H. Nakashima, M. Asada, Shunsuke Kiyomura, Yuki Sasaki, K. Torii, K. Sueki
{"title":"Physical and adsorption characteristics of geopolymers prepared using 1–5 M NaOH solution for immobilization of radioactive wastes","authors":"N. Kinoshita, Yuya Yoda, H. Nakashima, M. Asada, Shunsuke Kiyomura, Yuki Sasaki, K. Torii, K. Sueki","doi":"10.14494/jnrs.22.7","DOIUrl":"https://doi.org/10.14494/jnrs.22.7","url":null,"abstract":"","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"7 1","pages":""},"PeriodicalIF":0.0,"publicationDate":"2022-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"82206988","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
{"title":"Isothermal gas chromatography study of Zr and Hf tetrachlorides using radiotracers of 88Zr and 175Hf","authors":"K. Shirai, S. Goto, K. Ooe, H. Kudo","doi":"10.14494/jnrs.21.7","DOIUrl":"https://doi.org/10.14494/jnrs.21.7","url":null,"abstract":"","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"467 1","pages":""},"PeriodicalIF":0.0,"publicationDate":"2021-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"77033706","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
{"title":"Phase transformation of mixed lanthanide oxides in an aqueous solution","authors":"M. Moniruzzaman, Taishi Kobayashi, T. Sasaki","doi":"10.14494/jnrs.21.15","DOIUrl":"https://doi.org/10.14494/jnrs.21.15","url":null,"abstract":"","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"62 1","pages":""},"PeriodicalIF":0.0,"publicationDate":"2021-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"89181822","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
Daisuke Akiyama, Tasuku Ishii, Yutaka Masaki, T. Narabayashi, A. Kirishima, N. Sato
{"title":"Sorption and desorption of radioactive organic iodine by silver doped zeolite and zeolite X","authors":"Daisuke Akiyama, Tasuku Ishii, Yutaka Masaki, T. Narabayashi, A. Kirishima, N. Sato","doi":"10.14494/jnrs.21.1","DOIUrl":"https://doi.org/10.14494/jnrs.21.1","url":null,"abstract":"","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"1 1","pages":""},"PeriodicalIF":0.0,"publicationDate":"2021-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"90748817","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
Plutonium (Pu), mainly derived from thermonuclear bomb testing, nuclear accidents, nuclear reprocessing facilities and nuclear power plants since the 1950s, entered the ocean by global fallout and by direct release and was then transported by ocean current, exchanged, transformed and eventually buried in the ocean. Pu in the marine environment consists mainly of four isotopes, namely,Pu (T1/2 = 87.7 a), Pu (T1/2 = 24100 a), Pu (T1/2 = 6561 a) and Pu (T1/2 = 14.3 a), in which a very small fraction of Pu originates from uranium mineral and most Pu comes f rom anth ropogenic act iv it y. Additionally, Pu has two isotopes with extremely low concentrations namely, Pu (T1/2 = 376000 a) and Pu (T1/2 = 8.7 ×10 a). The distribution of Pu concentration in the marine environment is influenced by ocean current distribution and biogeochemical cycles, and therefore, Pu isotopes are typically utilized to trace water mass exchange, particle scavenging and biogeochemical cycles. Compared to Sr (Kd: 10-10 L kg) and Cs (Kd: 10-10 L kg), Pu has a much stronger particle affinity in marine environments (Kd: 10-10 L kg) and thus can serve as a better tracer for indicating transport, scavenging and particle deposition. To use Pu as a tracer for environmental process, the geochemical behavior of Pu should be understood and the analytical method for Pu need to be improved. With the development of analytical methods for Pu, the detection limit of Pu in seawater and sediments has continuously decreased, which allows increasing numbers of researchers (Figure 1) to focus on the sources, geochemical behaviors, distribution and environmental implications. Pu fr om different sources or incidents has unique atom (or activity) ratios, e.g., Pu/Pu, Pu/Pu and Pu/Pu, and these ratios can be used to quantitatively evaluate the source of Pu and to study different marine processes along with Pu activity concentration. Therefore, this study aims to synthesize the application of Pu to marine processes based on a summary of its sources, geochemical behaviors, distribution and analytical methods.
{"title":"Plutonium Isotopes Research in the Marine Environment: A synthesis","authors":"Jinlong Wang, Jinzhou Du, Z. Jian","doi":"10.14494/JNRS.20.1","DOIUrl":"https://doi.org/10.14494/JNRS.20.1","url":null,"abstract":"Plutonium (Pu), mainly derived from thermonuclear bomb testing, nuclear accidents, nuclear reprocessing facilities and nuclear power plants since the 1950s, entered the ocean by global fallout and by direct release and was then transported by ocean current, exchanged, transformed and eventually buried in the ocean. Pu in the marine environment consists mainly of four isotopes, namely,Pu (T1/2 = 87.7 a), Pu (T1/2 = 24100 a), Pu (T1/2 = 6561 a) and Pu (T1/2 = 14.3 a), in which a very small fraction of Pu originates from uranium mineral and most Pu comes f rom anth ropogenic act iv it y. Additionally, Pu has two isotopes with extremely low concentrations namely, Pu (T1/2 = 376000 a) and Pu (T1/2 = 8.7 ×10 a). The distribution of Pu concentration in the marine environment is influenced by ocean current distribution and biogeochemical cycles, and therefore, Pu isotopes are typically utilized to trace water mass exchange, particle scavenging and biogeochemical cycles. Compared to Sr (Kd: 10-10 L kg) and Cs (Kd: 10-10 L kg), Pu has a much stronger particle affinity in marine environments (Kd: 10-10 L kg) and thus can serve as a better tracer for indicating transport, scavenging and particle deposition. To use Pu as a tracer for environmental process, the geochemical behavior of Pu should be understood and the analytical method for Pu need to be improved. With the development of analytical methods for Pu, the detection limit of Pu in seawater and sediments has continuously decreased, which allows increasing numbers of researchers (Figure 1) to focus on the sources, geochemical behaviors, distribution and environmental implications. Pu fr om different sources or incidents has unique atom (or activity) ratios, e.g., Pu/Pu, Pu/Pu and Pu/Pu, and these ratios can be used to quantitatively evaluate the source of Pu and to study different marine processes along with Pu activity concentration. Therefore, this study aims to synthesize the application of Pu to marine processes based on a summary of its sources, geochemical behaviors, distribution and analytical methods.","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"31 1","pages":"1-11"},"PeriodicalIF":0.0,"publicationDate":"2020-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"73244721","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
Liquid interfaces, such as gas/liquid, liquid/liquid, and solid/liquid interfaces, are ubiquitous and play important roles in chemistry. For chemical reactions at interfaces, the interfacial region at a ~1-nm depth is important because this thin interfacial region corresponds to the scale of the sizes of molecules. However, it is generally difficult to observe this very thin region of liquid interfaces by conventional methods. For example, photoelectron spectroscopy requires a vacuum to detect electrons ejected from sample surfaces; thus, it is not appropriate for liquid interfaces. X -ray scattering methods are generally used to study liquid interfaces. However, high brightness X-rays are prepared by synchrotrons, and experiments for radioactive species are difficult in such facilities. Vibrational sum frequency generation (VSFG) spectroscopy is one of the vibrational spectroscopic techniques besides FT-IR and Raman spectroscopy. VSFG spectroscopy is interface-specific and offers unique information on the molecular structure in the very thin interfacial region (~1 nm) of liquid interfaces. Although many interfacial studies by VSFG spectroscopy have been published thus far, application to lanthanides and actinides has been very limited because previous studies have paid considerable attention to interface chemistry relating to light elements, such as interface chemistry in the cell membrane. Some metal complexes have been observed at air/aqueous interfaces using VSFG spectroscopy; however, there have been no reports on actinides because special techniques and facilities for the management and treatment of actinides are required. Recently, we constructed an optical experimental setup for VSFG spectroscopy in a radiation management area in the Japan Atomic Energy Agency (JAEA), enabling us to study actinide chemistry by VSFG spectroscopy. In this paper, the focus is on liquid interfaces of solvent extraction of lanthanides and actinides studied using VSFG spectroscopy. In solvent extraction [Figure 1(a)], extractants are dissolved in an organic phase, and some extractant molecules come to the liquid/liquid interface and cover the interface because of the surface activity of the extractants. Metal ions in the aqueous phase come to the interface and form complexes with extractants (ligands) to subsequently transfer to the organic phase. However, it is unknown what occurs at the interface and how water and extractant molecules are bonded to metals at the interface to transfer into the organic phase. This is because of the experimental difficulty related to the organic/aqueous interface, and one reason for the difficulty is that metal complexes at the interface transfer into the organic phase after complex formation at the interface and are difficult to observe at the interface. Therefore, we trapped metal comLiquid interfaces related to lanthanide and actinide chemistry studied using vibrational sum frequency generation spectroscopy
{"title":"Liquid interfaces related to lanthanide and actinide chemistry studied using vibrational sum frequency generation spectroscopy","authors":"Ryoji Kusaka","doi":"10.14494/JNRS.20.28","DOIUrl":"https://doi.org/10.14494/JNRS.20.28","url":null,"abstract":"Liquid interfaces, such as gas/liquid, liquid/liquid, and solid/liquid interfaces, are ubiquitous and play important roles in chemistry. For chemical reactions at interfaces, the interfacial region at a ~1-nm depth is important because this thin interfacial region corresponds to the scale of the sizes of molecules. However, it is generally difficult to observe this very thin region of liquid interfaces by conventional methods. For example, photoelectron spectroscopy requires a vacuum to detect electrons ejected from sample surfaces; thus, it is not appropriate for liquid interfaces. X -ray scattering methods are generally used to study liquid interfaces. However, high brightness X-rays are prepared by synchrotrons, and experiments for radioactive species are difficult in such facilities. Vibrational sum frequency generation (VSFG) spectroscopy is one of the vibrational spectroscopic techniques besides FT-IR and Raman spectroscopy. VSFG spectroscopy is interface-specific and offers unique information on the molecular structure in the very thin interfacial region (~1 nm) of liquid interfaces. Although many interfacial studies by VSFG spectroscopy have been published thus far, application to lanthanides and actinides has been very limited because previous studies have paid considerable attention to interface chemistry relating to light elements, such as interface chemistry in the cell membrane. Some metal complexes have been observed at air/aqueous interfaces using VSFG spectroscopy; however, there have been no reports on actinides because special techniques and facilities for the management and treatment of actinides are required. Recently, we constructed an optical experimental setup for VSFG spectroscopy in a radiation management area in the Japan Atomic Energy Agency (JAEA), enabling us to study actinide chemistry by VSFG spectroscopy. In this paper, the focus is on liquid interfaces of solvent extraction of lanthanides and actinides studied using VSFG spectroscopy. In solvent extraction [Figure 1(a)], extractants are dissolved in an organic phase, and some extractant molecules come to the liquid/liquid interface and cover the interface because of the surface activity of the extractants. Metal ions in the aqueous phase come to the interface and form complexes with extractants (ligands) to subsequently transfer to the organic phase. However, it is unknown what occurs at the interface and how water and extractant molecules are bonded to metals at the interface to transfer into the organic phase. This is because of the experimental difficulty related to the organic/aqueous interface, and one reason for the difficulty is that metal complexes at the interface transfer into the organic phase after complex formation at the interface and are difficult to observe at the interface. Therefore, we trapped metal comLiquid interfaces related to lanthanide and actinide chemistry studied using vibrational sum frequency generation spectroscopy","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"22 1","pages":"28-31"},"PeriodicalIF":0.0,"publicationDate":"2020-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"89062042","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
For the safety assessment of radioactive waste disposal, it is necessary to predict the migration behavior of actinide elements under relevant geochemical conditions, as they are included in the waste as alpha-emitting radionuclides wit h long half-lives. Actinide elements of thorium, uranium, neptunium, and plutonium can exist in a tetravalent oxidation state under reducing geochemical conditions, deep underground and easily precipitate as a sparingly soluble amorphous hydroxide solid phase (An(IV)(OH)4(am)) under neutral to alkaline pH conditions of the waste repository systems [1-4]. The solubilities of An(IV)(OH)4(am), hence, play an important role in understanding their migration behavior. It is known that a crystalline oxide solid phase as An(IV)O2(cr) is thermodynamically more stable and it has been reported that the crystallization of An(IV)(OH)4(am) towards An(IV)O2(cr) proceeded under certain solution conditions such as strong alkaline pH or elevated temperatures [5-7]. The solubilities of An(IV)O2(cr) have been reported to several orders of magnitude lower than those of An(IV)(OH)4(am) [1-7]. Trivalent actinide elements of americium and curium also exhibit a strong hydrolysis reactions under neutral to alkaline pH conditions to precipitate the sparingly soluble amorphous hydroxide solid phase (An(III)(OH)3(am)) [8-11]. In contrast to the tetravalent actinide elements, no crystalline oxide solid phase (An(III)2O3(cr)) was observed in the solubility experiments [2,12]. A few literatures have observed crystalline hydroxide solid phase (An(III)(OH)3(cr)) from X-ray diffraction patterns instead of An(III)2O3(cr) and showed an order of magnitude lower solubility values than those of An(III) (OH)3(am) [13,14]. This can be explained by thermodynamic data of An(III)2O3(cr). For example, the standard enthalpy (∆fHm°) and entropy (Sm°) of Am2O3(cr) have been reported to be ∆fHm° = −1690.4±8.0 kJ/mol and Sm° = 133.6±6.0 J/K/mol resulted in the standard formation Gibbs energy of ∆fGm° = −1605.449±8.284 [2]. Combined with the thermodynamic data for Am and H2O [2], the standard reaction Gibbs energy (∆rGm°) for 1/2 Am2O3(cr) + 3H Am + 3/2 H2O was calculated to be ∆rGm° = −151.59 kJ/mol, leading to the solubility product (Ks°) of log Ks° = 26.56. This value is approximately 10 orders of magnitude h igher than those repor ted for Am(OH)3(am) and Am(OH)3(cr) [2,4], hinting the oxide solid phase is less stable in aqueous systems. However, due to experimental limitations for handling macro amounts of trivalent actinide elements, only few studies have investigated the An(III) solubility with a definite solid phase characterization [8,11,13] and the stability of An(III)2O3(cr) in aqueous systems has not been well experimentally clarified. Trivalent lanthanide elements are often used as analogues of trivalent actinide elements. A number of literatures have investigated the hydrolysis behavior, solubilities and solid phases of lighter to heavier lanthanide el
{"title":"Solubility and solid phase of trivalent lanthanide hydroxides and oxides","authors":"M. Moniruzzaman, Taishi Kobayashi, T. Sasaki","doi":"10.14494/JNRS.20.32","DOIUrl":"https://doi.org/10.14494/JNRS.20.32","url":null,"abstract":"For the safety assessment of radioactive waste disposal, it is necessary to predict the migration behavior of actinide elements under relevant geochemical conditions, as they are included in the waste as alpha-emitting radionuclides wit h long half-lives. Actinide elements of thorium, uranium, neptunium, and plutonium can exist in a tetravalent oxidation state under reducing geochemical conditions, deep underground and easily precipitate as a sparingly soluble amorphous hydroxide solid phase (An(IV)(OH)4(am)) under neutral to alkaline pH conditions of the waste repository systems [1-4]. The solubilities of An(IV)(OH)4(am), hence, play an important role in understanding their migration behavior. It is known that a crystalline oxide solid phase as An(IV)O2(cr) is thermodynamically more stable and it has been reported that the crystallization of An(IV)(OH)4(am) towards An(IV)O2(cr) proceeded under certain solution conditions such as strong alkaline pH or elevated temperatures [5-7]. The solubilities of An(IV)O2(cr) have been reported to several orders of magnitude lower than those of An(IV)(OH)4(am) [1-7]. Trivalent actinide elements of americium and curium also exhibit a strong hydrolysis reactions under neutral to alkaline pH conditions to precipitate the sparingly soluble amorphous hydroxide solid phase (An(III)(OH)3(am)) [8-11]. In contrast to the tetravalent actinide elements, no crystalline oxide solid phase (An(III)2O3(cr)) was observed in the solubility experiments [2,12]. A few literatures have observed crystalline hydroxide solid phase (An(III)(OH)3(cr)) from X-ray diffraction patterns instead of An(III)2O3(cr) and showed an order of magnitude lower solubility values than those of An(III) (OH)3(am) [13,14]. This can be explained by thermodynamic data of An(III)2O3(cr). For example, the standard enthalpy (∆fHm°) and entropy (Sm°) of Am2O3(cr) have been reported to be ∆fHm° = −1690.4±8.0 kJ/mol and Sm° = 133.6±6.0 J/K/mol resulted in the standard formation Gibbs energy of ∆fGm° = −1605.449±8.284 [2]. Combined with the thermodynamic data for Am and H2O [2], the standard reaction Gibbs energy (∆rGm°) for 1/2 Am2O3(cr) + 3H Am + 3/2 H2O was calculated to be ∆rGm° = −151.59 kJ/mol, leading to the solubility product (Ks°) of log Ks° = 26.56. This value is approximately 10 orders of magnitude h igher than those repor ted for Am(OH)3(am) and Am(OH)3(cr) [2,4], hinting the oxide solid phase is less stable in aqueous systems. However, due to experimental limitations for handling macro amounts of trivalent actinide elements, only few studies have investigated the An(III) solubility with a definite solid phase characterization [8,11,13] and the stability of An(III)2O3(cr) in aqueous systems has not been well experimentally clarified. Trivalent lanthanide elements are often used as analogues of trivalent actinide elements. A number of literatures have investigated the hydrolysis behavior, solubilities and solid phases of lighter to heavier lanthanide el","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"29 1","pages":"32-42"},"PeriodicalIF":0.0,"publicationDate":"2020-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"88341420","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
{"title":"Accurate determination of three halogen elements (Cl, Br, and I) in U.S. Geological Survey geochemical reference materials by radiochemical neutron activation analysis and an exhaustive comparison with literature data: a review","authors":"S. Sekimoto, M. Ebihara","doi":"10.14494/JNRS.20.12","DOIUrl":"https://doi.org/10.14494/JNRS.20.12","url":null,"abstract":",","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"7 1","pages":""},"PeriodicalIF":0.0,"publicationDate":"2020-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"74945427","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
is an activation product with a short half-life (2.06 years) that was released during the disaster. It is an important indicator of contamination from the disaster it has been more years since the last event when 134 Cs was released. The ratio of 137 Cs to 134 Cs was approximately the time of the and thus, it is possible to quantitatively evaluate the of
{"title":"Pretreatment conditions for detecting 134Cs -Eight years after the Fukushima Daiichi nuclear accident-","authors":"K. Shozugawa, Mayumi Hori","doi":"10.14494/JNRS.20.25","DOIUrl":"https://doi.org/10.14494/JNRS.20.25","url":null,"abstract":"is an activation product with a short half-life (2.06 years) that was released during the disaster. It is an important indicator of contamination from the disaster it has been more years since the last event when 134 Cs was released. The ratio of 137 Cs to 134 Cs was approximately the time of the and thus, it is possible to quantitatively evaluate the of","PeriodicalId":16569,"journal":{"name":"Journal of nuclear and radiochemical sciences","volume":"32 1","pages":""},"PeriodicalIF":0.0,"publicationDate":"2020-01-01","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"88436469","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":0,"RegionCategory":"","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}
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