- About this Journal ·
- Abstracting and Indexing ·
- Aims and Scope ·
- Article Processing Charges ·
- Articles in Press ·
- Author Guidelines ·
- Bibliographic Information ·
- Citations to this Journal ·
- Contact Information ·
- Editorial Board ·
- Editorial Workflow ·
- Free eTOC Alerts ·
- Publication Ethics ·
- Reviewers Acknowledgment ·
- Submit a Manuscript ·
- Subscription Information ·
- Table of Contents
Advances in Materials Science and Engineering
Volume 2013 (2013), Article ID 747383, 9 pages
Characterization and Neutron Shielding Behavior of Dehydrated Magnesium Borate Minerals Synthesized via Solid-State Method
1Chemical Engineering Department, Faculty of Chemical and Metallurgical Engineering, Yildiz Technical University, Davutpasa Street, No. 127, Esenler, 34210 Istanbul, Turkey
2Environmental Engineering Department, Faculty of Civil Engineering, Yildiz Technical University, Davutpasa Street No. 127, Esenler, 34210 Istanbul, Turkey
Received 14 February 2013; Revised 2 October 2013; Accepted 2 October 2013
Academic Editor: Kunpeng Wang
Copyright © 2013 Azmi Seyhun Kipcak et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
Magnesium borates are one of the major groups of boron minerals that have good neutron shielding performance. In this study, dehydrated magnesium borates were synthesized by solid-state method using magnesium oxide (MgO) and boron oxide (B2O3), in order to test their ability of neutron shielding. After synthesizing the dehydrated magnesium borates, characterizations were done by X-ray Diffraction (XRD), fourier transform infrared (FT-IR), Raman spectroscopy, and scanning electron microscopy (SEM). Also boron oxide (B2O3) contents and reaction yields (%) were calculated. XRD results showed that seven different types of dehydrated magnesium borates were synthesized. 1000°C reaction temperature, 240 minutes of reaction time, and 3 : 2, 1 : 1 mole ratios of products were selected and tested for neutron transmission. Also reaction yields were calculated between 84 and 88% for the 3 : 2 mole ratio products. The neutron transmission experiments revealed that the 3 : 2 mole ratio of MgO to B2O3 neutron transmission results (0.618–0.655) was better than the ratio of 1 : 1 (0.772–0.843).
Dehydrated magnesium borates are well-known metal borates that have many chemical formulas such as, Mg2B2O5 (suanite), MgB3B2O6 (kotoite), and MgB4O7 . They owe very important properties like high heat-resisting, antiwear and anticorrosion materials, super mechanical strength, super insulation, lightweight, high strength, and high coefficient of elasticity . Magnesium borates have many potential applications involving catalysts for the conversion of hydrocarbons , the thermoluminescence phosphor , and as fused cast refractory that possesses corrosion-erosion resistance in basic oxygen steel making environments and high degree of thermal shock resistance .
The synthesis of magnesium borates can be divided into two according to their structures, such as; hydrated or dehydrated. For the production of hydrated magnesium borates, hydrothermal method can be used. Thermal or solid-state (solid-solid reaction type) method  or chemical deposition method  can be applied for the production of dehydrated magnesium borates. Various synthesis methods for preparation of dehydrated magnesium borates have been proposed up to now. In recent years, several nanostructure forms of dehydrated magnesium borates, such as nanorods [1, 2, 7] and nanowhiskers , have been synthesized through high temperature solid-state synthesis method, respectively. Došler et al., Qasrawi et al., and Elssfah et al. synthesized Mg2B2O5 type magnesium borate where Došler et al. used MgO and B2O3 and Qasrawi et al. and Elssfah et al. used magnesium hydroxide (Mg(OH)2) and boric acid (H3BO3) [2, 9, 10]. Li et al., also synthesized Mg2B2O5 type magnesium borate but they used magnesium chloride hexahydrate (MgCl2·6H2O) and sodium borohydrate (NaBH4) as starting materials . Zhang et al. synthesized Mg3B2O6 with a particle size of 100–300 nm . Zeng et al. synthesized Mg2B2O5 from hydrated magnesium borate minerals .
Many countries around the world, especially USA and France, use boron compounds as a shielding material in nuclear reactor technologies. A number of studies have been conducted in the area of nuclear shielding, both in Turkey and in the world . Some materials  were constructed and investigated at the area of nuclear shielding namely polyboron , neutron filter , thermal neutron radiation shield , ceramic shield material containing boron carbide (B4C) , and biological shielding material . In these studies the materials like B4C, B2O3, iron (Fe), lead (Pb), and bismuth (Bi) were investigated. Kipcak investigated the usability of boron minerals as a neutron shielding material and conducted a study including the shielding behavior of boron minerals against neutron radiation and twelve year performance of neutron transmission, he used only boron minerals as a shield material [13, 19–21].
The aim of the article can be divided into two parts, where in part one high crystalline dehydrated magnesium borate synthesis via solid-state method was studied. In the literature, the studies involving dehydrated magnesium borate formation were lacking reaction yields and crystalline scores. So, it is necessary to develop a cost friendly with a high reaction yield and effective method for the production of high crystalline dehydrated magnesium borates. After the successful synthesis of dehydrated magnesium borates the techniques of XRD, FT-IR, Raman Spectroscopy, and SEM were used to characterize the obtained minerals. Also B2O3 contents were determined by titration and reaction yields were calculated. In the second phase the neutron shielding behavior of dehydrated magnesium borates against neutron radiation were tested, where neutron radiation experiments were conducted with 241Am-Be source moderated in howitzer. In this analysis high crystalline type of minerals is important for the neutron shielding studies since crystal structures show the homogeneous radiation shielding performance and repeatability of the experiments.
2. Materials and Methods
2.1. Preparation of the Reactants
B2O3 was supplied from Kırka Boron Management Plant (EtiMine Kırka Boron Works) in Eskisehir, Turkey, and MgO was supplied from Merck Chemicals. B2O3 was crushed, grinded, and sieved to +200 meshes with agate mortar. MgO was used without being subjected to any physical process. Then these reactants were taken for identification analysis, which was made by Philips PANanalytical XRD, where X-rays were produced from Cu-Kα tube at the parameters of 45 kV and 40 mA.
2.2. Solid-State Synthesis of Dehydrated Magnesium Borates
Different mole ratios of MgO : B2O3 were selected as 2 : 1, 3 : 2, 1 : 1, 1 : 2, and 1 : 4. These mole ratios were determined after some preliminary experiments. Prepared mixtures were pressed (10 tones) with Manfredi OL57 hydraulic press. After the pelletization process the minerals were subjected to 600°C through 1000°C temperatures with Protherm MOS 180/4 model high temperature furnace. The temperature increment was selected as 10°C/min and the experimental time is set as 240 minutes for the temperatures of 600°C and 700°C. For 800°C, 900°C, and 1000°C, the experiment times were set as 30, 60, and 240 minutes. All reactions were conducted in a ceramic crucible whose inside was coated with Al2O3. The reaction atmosphere was used as air. After the reaction, the obtained solid particles were crashed and grinded.
2.3. Characterizations of the Synthesized Products
The identification and characterization of the synthesized products were done with the parameters that are the same as the one conducted at Section 2.1 by XRD technique. Perkin Elmer brand FT-IR technique with Universal ATR sampling accessory-diamond/ZnSe was used with 1800–650 cm−1 measurement range and 4 cm−1 resolution. Scan number was set to 4. To support the FT-IR results, Raman spectroscopy of Perkin Elmer Brand, Raman Station 400 F, was used with the exposure time of 4 seconds, number of exposures of 4, 1800–250 cm−1 measurement range, and 2 cm−1 data interval. Full (100%) laser power was used and “auto baseline” option was also selected during the experiments.
In order to investigate and analyze the surface morphology SEM analysis was conducted. CamScan Apollo brand 300 Field-Emission SEM was used at 20 kV with back scattering electron (BEI) detector. Magnifications were set to 1000 and 5000.
Since boron is the well-known neutron absorber, it was important to determine the B2O3 content of the synthesized minerals. B2O3 analyses were made and calculated by using the procedure given in Moroydor Derun et al.  in this procedure, 1 g of synthesized mineral was dissolved in 3 mL of 37% HCl and then diluted to 100 mL. Pure H3BO3 obtained from Merck Chemicals was prepared in the same manner and was used as the reference material. Then, B2O3 amounts were determined through acid-base titration with a Mettler DL-25 titrator.
Reaction yields were also calculated with the method given in Moroydor Derun et al.  and Fogler . Reaction yields are based on molar flow rates, the overall yield, , is defined as the ratio of moles of product formed at the end of the reaction, is the number of moles of the key reactant (MgO), that have been consumed, and and are the initial and final moles of consumed reactant, respectively. For a batch system the overall yield is given in the following [22, 23]:
2.4. Neutron Shielding Study
Neutron transmission experiments were conducted in Cekmece Nuclear Research and Training Center (CNAEM). For the experimental system 241Am-Be source moderated in howitzer that has 74 GBq activity was used. The neutrons in this source had an average and maximum energy of 4.5 MeV and 12 MeV, respectively. Neutron counts were measured by BF3 neutron detector (diameter: 2.54 cm, length: 28 cm) and counter.
With the experimental setup mentioned, the minerals which were synthesized using MgO and B2O3 with 1000°C reaction temperature, 240 minutes of reaction time, and 3 : 2 and 1 : 1 mole ratios were tested for neutron radiation. For the neutron radiation experiments 10, 15, and 25 g of minerals were taken and mixed with wax (C3H8O7N7) (10% by weight). Wax was used as an adhesive. The mixtures were mixed five minutes in the agate mortar. Then the mixtures were pelleted with (25 MPa) hydraulic press, using the 40 mm molding set.
For each sample, the neutrons passing through the pelleted minerals were counted () by neutron detector. Then the same procedure was conducted without using the pelleted minerals in order to measure the collimated neutrons (). The experiments were conducted with 4 parallels in order to minimize the experimental errors. Total neutron transmission (2) values and total macroscopic cross-sections (3) were calculated with the Beer-Lambert law, for the energy value of 4.5 MeV, where “” is the thickness of the minerals
3. Results and Discussion
3.1. X-Ray Diffraction Results
The raw materials used in the solid-state experiments were analyzed by XRD and MgO was found as “periclase [MgO]” with a reference code of “01-077-2179”. B2O3 was found as the mixture of “boron oxide [B2O3]” and “boron oxide [BO2]” with the reference codes of “00-006-0297” and “01-088-2485,” respectively.
In Table 1, XRD results of the synthesized dehydrated magnesium borates were shown. From the results it is seen that seven different types of dehydrated magnesium borates were formed. The crystallographic data obtained from XRD are given in Table 2. “K” code represents “kotoite” and S1 and S2 represent “suanite” minerals that have different lattice structures. And four different types of magnesium borates coded “MB1” through “MB4” were synthesized during the experiments. “MB1” and “MB3” coded minerals formula is the same as “S1” and “S2” but their lattice structures are different.
At the reaction temperature of 600°C, the formation of dehydrated magnesium borates was started. At the ratio of 2 : 1 MgO was seen at the products as “periclase” which means that it reacts very little at that ratio; the same situation was seen at 700°C reaction temperature also. At the other ratios the formation of S1, S2 and MB4 was seen but their crystal scores were too low, where perfect crystal structure of an element, mineral, or compound XRD score is equal to 100. XRD crystal scores were increased and a new mineral coded MB3 was synthesized at the reaction temperature of 700°C but their crystal scores were still low, which means that the crystallization was not enough at that temperature. At 800°C reaction time, major magnesium borate phase was seen as kotoite, “K.” At this temperature and 30 minutes of reaction time the ratio of 1 : 1 had the greatest score among the other ratios. This score was increased to “66” at the reaction time of 60 minutes and finally became “86” at the reaction time of 240 minutes. The major phase of “K” which was seen on 800°C was turned up a little to MB1 and MB2 at the reaction temperature 900°C, because it was seen from the results that kotoite’s crystal scores were decreased and the minor phase crystal scores were increased. At the highest reaction temperature of 1000°C minor phase scores of “MB1”s were coming close to the “K” scores. The “K” scores did not change much with the increasing reaction time at 1000°C but “MB1” scores were increased. The highest crystal scores were obtained at the mole ratios of 3 : 2 and 1 : 1. For the comparison, XRD patterns of the dehydrated magnesium borates synthesized at 1000°C with the reaction times of 30, 60, and 240 minutes are shown in Figure 1. It can be seen in Figure 1 that the ratios of 2 : 1, 3 : 2, and 1 : 1 patterns are smother than 1 : 2 and 1 : 4 ratios, meaning that better crystal structures were obtained at the first three ratios.
A three dimensional model graph of K and MB1 formations which were obtained from the score data by XRD was given in Figure 2. In this figure the MgO : B2O3 mole ratios of “3 : 2” and “1 : 1” were used. At this graph -, - and -axes represents the XRD score, reaction temperature as °C and the reaction time as minutes, respectively. From this figure K and MB1 scores were the highest in 800°C, and 1000°C, respectively. According to the obtained graphs, there was no score of MB1 at the temperature of 800°C.
3.2. FT-IR, Raman, SEM, B2O3 Results, and Reaction Yields
Obtained FT-IR and Raman spectra from the synthesized dehydrated magnesium borates were approximately the same, so only 1000°C reaction time and 240 minutes of reaction time results were given in Figures 3 and 4, respectively.
From the FT-IR spectrum, the peak value at around 1411 cm−1 represents the asymmetric stretching of three coordinate boron . The peaks between 1283–1285 cm−1 represent also . Bending of B–O–H [δ(B–O–H)] was formed at the peaks between 1123 and 1125 cm−1. The peak at around 883 cm−1 is the symmetric stretching of three coordinate boron . Last peaks between 709 and 711 cm−1 represents the asymmetric stretching of four coordinate boron .
According to the Raman spectrum, is formed between the peaks of 1392–1396 and 1286 cm−1. The peaks between 881–979 cm−1 represents the . is seen at the peak values between 807–848 cm−1. The characteristic peaks of magnesium borates, [B4O5(OH)4]2− and [B5O6(OH)4]− are seen at 543 and 499 cm−1, respectively. The other peaks (<417 cm−1) are the bending of four coordinate boron [δ].
SEM morphologies of the minerals are given in Figure 5. According to the results, mineral thicknesses of the 1 : 1 and 3 : 2 mole ratio minerals were changed between the 3.74–23.47 μm and 5.05–16.82 μm, respectively, in 800°C reaction temperature. These particle thicknesses were decreased to 3.23–10.73 μm at the mole ratio of 3 : 2 and increased to 4.69–29.53 μm at the mole ratio of 1 : 1 in 900°C reaction temperature. In 1000°C compared to 800°C reaction temperature the 1 : 1 mole ratio of minerals was decreased to 4.70–17.86 μm and 3 : 2 mole ratio of minerals was decreased to 3.45–14.76 μm. The lowest particle sizes were seen on 1 : 1 mole ratio at the reaction temperature of 1000°C and 3 : 2 mole ratio at the reaction temperature of 900°C.
The B2O3 results of the dehydrated magnesium borates were given in Table 3. Since the XRD crystal scores of the minerals at 240 minutes are higher than the other reaction times, only these minerals B2O3 percentages were calculated. And it is seen from the experimental results the B2O3 contents were similar to the theoretical contents of the kotoite and suanite B2O3 contents which are 36.54 and 46.34%, respectively. For example theoretically ((4) and (5)), at the mole ratio of 1 : 1 suanite formation was higher and at the mole ratio of 3 : 2 kotoite formation was higher than the other minerals. At the mole ratio of 3 : 2 and temperatures of 800°C, 900°C and 1000°C, the B2O3 ratios were seen as 30.12, 36.25 and 37.51% respectively which are nearly equal to the theoretical kotoite B2O3 ratio of 36.54%. Similarly at the mole ratio of 1 : 1 and temperatures of 800°C, 900°C, and 1000°C, the B2O3 ratios were seen as 44.99, 40.62, and 42.56%, respectively, which are nearly equal to the theoretical suanite B2O3 ratio of 46.34%. Since the obtained minerals have at least two phases, the B2O3 contents can be varied from each other
Reaction yields were calculated for the mole ratios of 3 : 2 and 1 : 1. The minerals obtained at those ratios were Mg2B2O5 and Mg3B2O6, so the minimum reaction yields were calculated using the Mg3B2O6 molecular weight of 190.53 g/mol. The results are given in Table 4. According to the reaction yields obtained 3 : 2 mole ratio (82–88%) is greater than the 1 : 1 mole ratio (46–53%). Reaction yields of dehydrated magnesium borates were changed with little amounts according to the temperature increase and reaction temperature. So reaction temperature and reaction time only changed the crystal structures and scores. The highest reaction yield was seen at 800°C, 240 minutes of reaction time, and 3 : 2 mole ratio product with a value of 88%.
3.3. Neutron Transmission Results
The neutron transmission values and total macroscopic cross-sections of the dehydrated magnesium borate minerals synthesized by solid–state method using the MgO and B2O3 with 1000°C reaction temperature, 240 minutes of reaction time and 1 : 1 and 3 : 2 mole ratios were shown in Table 5.
From the results obtained it was seen that the 3 : 2 mole ratio synthesized minerals neutron transmission values were lower than the 1 : 1 mole ratio synthesized minerals. The difference between the minerals neutron transmission values can be explained by the crystal score differences obtained from XRD results. “K” crystal scores of synthesized minerals were 61 and 58 for the 3 : 2 and 1 : 1 mole ratios, respectively. By the same manner “MB3” crystal scores of synthesized minerals were 38 and 55 for the 3 : 2 and 1 : 1 mole ratios, respectively. Closed formula of the “K” is “Mg3(BO3)2” and that for “MB3” is “Mg2(B2O5).” So at the mole ratio of 3 : 2 Mg3(BO3)2 score was higher than that Mg2(B2O5), which means that the “K” is the major phase in this synthesis. Different formation was seen on 1 : 1 mole ratio where the Mg3(BO3)2 crystal score was nearly equal to the Mg2(B2O5) score, which means that both the “K” and “MB3” phases were obtained equally. “K” phase has an additional structure of “MgO” than the “MB3” phase as seen on
The 3 : 2 mole ratio neutron transmission value (0.618–0.655) is lower than the 1 : 1 mole ratio neutron transmission value (0.772–0.843). So better results were obtained where “K” was the major phase and has high crystal score (61) than 1 : 1 ratio (58). Also neutron transmission values and total macroscopic sections were decreased with increasing pellet thicknesses.
In this study, using the raw materials of MgO and B2O3, the synthesis of dehydrated magnesium borates was studied. The solid-state method was used with varying both of reaction temperatures at 600°C to 1000°C and reaction times of 30 minutes to 240 minutes. XRD results showed that the formation of dehydrated magnesium borates was started at a temperature of 600°C, and the “K” formation was started at a temperature of 800°C, and the highest crystal scores are obtained at the reaction time of 240 minutes and 800°C reaction temperature and higher. From the experiments, the formation of kotoite [Mg3(BO3)2], two types of suanite [Mg2(B2O5)], and four different formulated dehydrated magnesium borates [Mg2(B2O5), MgB4O7, Mg2B2O5, MgO(B2O3)2] were seen.
FT-IR and Raman spectrum of the synthesized minerals showed the characteristic peaks of the magnesium borates both in infrared and visible regions. The lowest particle size on 1 : 1 mole ratio determined by the SEM analysis was seen between 4.70 and 17.86 μm at the reaction temperature of 1000°C. At the 3 : 2 mole ratio the lowest particle size was seen between 3.45 and 14.76 μm at the reaction temperature of 900°C. Obtained B2O3 contents were calculated and seen with a mutual agreement with the theoretical kotoite and suanite contents. Reaction yields were changed between 82 and 88% in 3 : 2 mole ratio and 46 and 53% in 1 : 1 mole ratio.
From the neutron transmission experiments, it was seen that where “K” was the major phase less neutron transmission values were obtained. So it can be said that the “K” type dehydrated magnesium borates are better than the “MB1” type dehydrated magnesium borates against neutron radiation.
This study was supported by the “Office of Scientific Research Project Coordination” in Yildiz Technical University with the Project no. of “2012-07-01-KAP03.”
- S. Li, X. Fang, J. Leng, H. Shen, Y. Fan, and D. Xu, “A new route for the synthesis of Mg2B2O5 nanorods by mechano-chemical and sintering process,” Materials Letters, vol. 64, no. 2, pp. 151–153, 2010.
- E. M. Elssfah, A. Elsanousi, J. Zhang, H. S. Song, and C. Tang, “Synthesis of magnesium borate nanorods,” Materials Letters, vol. 61, no. 22, pp. 4358–4361, 2007.
- E. G. Baker, “Boron zinc oxide and boron magnesium oxide catalysts for conversion of hydrocarbons,” US Patent no: 2,889,266, 1959.
- C. Furetta, G. Kitis, P. S. Weng, and T. C. Chu, “Thermoluminescence characteristics of MgB4O7: Dy,Na,” Nuclear Instruments and Methods in Physics Research, Section A, vol. 420, no. 3, pp. 441–445, 1999.
- A. M. Alper and R. N. Corning, “MgO-B2O3 fused cast refractory,” 1967, US Patent no: 3,337,353.
- S. H. Kim, K. H. Lee, B. S. Seong, G.-H. Kim, J. S. Kim, and Y. S. Yoon, “Synthesis and structural properties of lithium titanium oxide powder,” Korean Journal of Chemical Engineering, vol. 23, no. 6, pp. 961–964, 2006.
- Y. Li, Z. Fan, J. G. Lu, and R. P. H. Chang, “Synthesis of magnesium borate (Mg2B2O5) nanowires by chemical vapor deposition method,” Chemistry of Materials, vol. 16, no. 13, pp. 2512–2514, 2004.
- W. Zhu, G. Li, Q. Zhang, L. Xiang, and S. Zhu, “Hydrothermal mass production of MgBO2(OH) nanowhiskers and subsequent thermal conversion to Mg2B2O5 nanorods for biaxially oriented polypropylene resins reinforcement,” Powder Technology, vol. 203, no. 2, pp. 265–271, 2010.
- U. Došler, M. M. Kržmanc, and D. Suvorov, “The synthesis and microwave dielectric properties of Mg3B2O6 and Mg2B2O5 ceramics,” Journal of the European Ceramic Society, vol. 30, no. 2, pp. 413–418, 2010.
- A. F. Qasrawi, T. S. Kayed, A. Mergen, and M. Gürü, “Synthesis and characterization of Mg2B2O5,” Materials Research Bulletin, vol. 40, no. 4, pp. 583–589, 2005.
- J. Zhang, Z. Li, and B. Zhang, “Formation and structure of single crystalline magnesium borate (Mg3B2O6) nanobelts,” Materials Chemistry and Physics, vol. 98, no. 2-3, pp. 195–197, 2006.
- Y. Zeng, H. Yang, W. Fu et al., “Synthesis of magnesium borate (Mg2B2O5) nanowires, growth mechanism and their lubricating properties,” Materials Research Bulletin, vol. 43, no. 8-9, pp. 2239–2247, 2008.
- E. M. Derun and A. S. Kipcak, “Characterization of some boron minerals against neutron shielding and 12 year performance of neutron permeability,” Journal of Radioanalytical and Nuclear Chemistry, vol. 292, no. 2, pp. 871–878, 2012.
- S. I. Bhuiyan, F. U. Ahmed, A. S. Mollah, and M. A. Rahman, “Studies of the neutron transport and shielding properties of locally developed shielding material: poly-boron,” Health Physics, vol. 57, no. 5, pp. 819–824, 1989.
- M. Adib and M. Kilany, “On the use of bismuth as a neutron filter,” Radiation Physics and Chemistry, vol. 66, no. 2, pp. 81–88, 2003.
- S. E. Gwaily, M. M. Badawy, H. H. Hassan, and M. Madani, “Natural rubber composites as thermal neutron radiation shields-I. B4C/NR composites,” Polymer Testing, vol. 21, no. 2, pp. 129–133, 2002.
- M. Celli, F. Grazzi, and M. Zoppi, “A new ceramic material for shielding pulsed neutron scattering instruments,” Nuclear Instruments and Methods in Physics Research, Section A, vol. 565, no. 2, pp. 861–863, 2006.
- D. L. Chichester and B. W. Blackburn, “Radiation fields from neutron generators shielded with different materials,” Nuclear Instruments and Methods in Physics Research, Section B, vol. 261, no. 1-2, pp. 845–849, 2007.
- A. S. Kipcak, The Investigation of the Usability of Boron Minerals As a Neutron Shielding Material Yildiz Technical University [Ph.D. thesis], 2009, (Turkish).
- A. S. Kipcak, D. Yilmaz Baysoy, E. Moroydor Derun, and S. Piskin, The Evaluation of the Neutron Radiation Absorption Capacities of Inderite Minerals, vol. 1 of 2011 Research Bulletin of the Australian Institute of High Energetic Materials, 2011.
- A. S. Kipcak, D. Yilmaz Baysoy, E. Moroydor Derun, and S. Piskin, Characterization of the Kurnacovite Mineral and Its Absorption Behavior due to Neutron Radiation, vol. 1 of 2011 Research Bulletin of the Australian Institute of High Energetic Materials, 2011.
- E. Moroydor Derun, A. S. Kipcak, F. T. Senberber, and M. Sari Yilmaz, “Characterization and thermal dehydration kinetics of admontite mineral hydrothermally synthesized from magnesium oxide and boric acid precursor,” Research on Chemical Intermediates.
- H. S. Fogler, Element of Chemical Reaction Engineering, Prentice-Hall, Englewood Cliffs, NJ, USA, 3rd edition, 1999.