Crystallization and quantification of crystalline and non-crystalline phases in kaolin-based cordierites

materials Article Crystallization and Quantification of Crystalline and Non-Crystalline Phases in Kaolin-Based Cordierites Marta Valášková1,* , Zdenˇek Klika 2, Boris Novosad 3,4 and Bedˇrich Smetana 5 1Institute of Environmental Technology, VŠB-Technical University of Ostrava, 17. listopadu 15, 708 00 Ostrava-Poruba, Czech Republic 2Department of Chemistry, VŠB-Technical University of Ostrava, 17. listopadu 15, 708 00 Ostrava-Poruba, Czech Republic; [email protected] 3Nanotechnology Centre, VŠB-Technical University of Ostrava, 17. listopadu 15, 708 00 Ostrava-Poruba, Czech Republic; [email protected] 4Faculty of Electrical Engineering and Computer Science, VŠB-Technical University of Ostrava, 17. listopadu 15, 708 00 Ostrava-Poruba, Czech Republic 5Faculty of Materials Science and Technology, VŠB-Technical University of Ostrava, 17. listopadu 15, 708 00 Ostrava-Poruba, Czech Republic; [email protected] *Correspondence: [email protected]; Tel.: +420-597-327-308 Received: 1 August 2019; Accepted: 19 September 2019; Published: 23 September 2019   Abstract: Kaolin is most often used as traditional raw material in ceramic industry. The purpose of the study was to obtain understanding of the structural and chemical variability of cordierite ceramics influenced by chemical and mineralogical properties of six raw kaolins taken from different localities when they are applied in ceramics mixtures with vermiculite and sintered up to 1300 ◦ C. The X-ray diffraction and simultaneous thermogravimetric and differential thermal analysis were used to identify and characterize crystalline mineral phases and the course of reactions during the heating. The percentages of the crystalline and non-crystalline phases were newly determined by recalculation of the bulk chemical analyses of kaolins and cordierite ceramics using Chemical Quantitative Mineral Analysis (CQMA) method. Varying amounts of minerals in kaolins: kaolinite from 73.3 to 85.0, muscovite from 4.2 to 9.9, and quartz from 6.0 to 19.5 (mass %) affected amount of cordierite/indialite from 75.2 to 85.1, enstatite from 5.8 to 8.9 (when are calculated as their maximal possible percentages), and non-crystalline phases from 8.8 to 15.1 (mass %) in cordierite ceramics. Regression analysis predicted high relationship between quantity of: (a) kaolinite in kaolins and crystalline cordierite and (b) quartz in kaolins and non-crystalline phases in the ceramics. The migration of potassium from muscovite into the cordierite structure, melting point and crystallization of cordierite/indialite phases and pore size variability in relation to impurity of kaolins are documented and discussed. Keywords: rawkaolins; cordierite/indialite; thermalconversions; X-raydiffraction; chemicalquantitative mineral analysis 1. Introduction Cordierite (Mg 2 Al 4 Si 5 O 18 ) has the oxide ratio composition 2:2:5 of 2MgO · 2Al 2 O 3· 5SiO 2 , and is one of the phases, which are present in the ternary glass–ceramic system MgO–Al 2 O 3 –SiO 2 [ 1 ]. Cordierite-like crystals synthesized below 830 ◦ C were termed β form [ 2 ]. The µ -cordierite was considered as a metastable product crystallizing from glass at temperatures below 950 ◦ C which transforms irreversibly upon heating to the α form. The low temperature orthorhombic form is cordierite stable below 1450 ◦ C. The high temperature hexagonal form is disordered indialite stable above 1450 ◦ C [ 3 ], which below 1450 ◦ C transforms slowly to β phase [ 4 ]. The conventional methods for the synthesis of cordierite ceramics include solid-state sintering of magnesium, aluminum, Materials 2019,12, 3104; doi:10.3390/ma12193104 www.mdpi.com/journal/materials Materials 2019,12, 3104 2 of 13 and silicon oxides in the mixtures corresponding to chemical composition of cordierite. Addition of nucleating agents (e.g., TiO 2 , ZrO 2 , Fe 2 O 3 ) effectively increases the softening and decreases glass transition temperatures. The oxide ratio in composition of cordierite is economically produced from the raw kaolin containing kaolinite (Al 2 O 3· 2SiO 2· 2H 2 O), talc (3MgO · 4SiO 2· H 2 O) and a correcting component alumina (Al 2 O 3 ). The fact that the properties of clay minerals used in the mixture and the conditions of preparation influence sintering and properties of ceramic body is widely known. Structural properties of cordierites prepared by the solid-state reaction from the mixtures of talc, kaolin, and alumina as well as from kaolin and vermiculite without further correcting additives at 1300 ◦ C were characterized in the previous works [ 5 , 6 ]. Raw kaolins contain kaolinite, muscovite (white mica), quartz, and an admixture of silicates, mostly feldspars, biotite, and accessory minerals [ 7 ]. Transformation of kaolin containing kaolinite, quartz, and muscovite in the temperature range of 980–1121 ◦ C produced primary mullite with a Si-Al spinel [ 8 , 9 ]. Impurities in kaolins such as muscovite and K-feldspar, containing potassium in their structure, act as flux that facilitated easy melting upon firing and formation of non-crystalline glassy phase [ 10 – 12 ]. Similarly, Fe-impurities supported crystallization of mullite [ 13 ]. Interaction between kaolinite and muscovite in the temperature range of dehydroxylation of muscovite between 800–900 ◦ C was not declared [ 14 ]. The minerals of the mica groups transformed at 950 ◦ C to mullite, K-feldspar and plagioclase [ 15 ]. At temperatures below 1000 ◦ C, muscovite was replaced by alkali feldspars and quartz was preserved even at 1100 ◦ C, while cristobalite was identified only in quartz-rich clays [11]. The main aim of this work was to obtain an understanding of the structural and chemical variability of cordierite ceramics influenced by chemical and mineralogical properties of kaolins taken from different localities. Therefore, the simple two-phase ceramic mixtures of kaolin and vermiculite without correcting additives were prepared in the mass ratio 1:1, close to the oxide ratio composition 2:2:5 of cordierite 2MgO · 2Al 2 O 3· 5SiO 2 for the solid state reaction up to 1300 ◦ C. X-ray diffraction and simultaneous thermogravimetric and differential thermal analysis were used to characterize crystalline mineral phases and decomposition and crystallization of phases from the melt. Quantification of crystalline and non-crystalline phases is newly performed based on the elemental bulk chemical analysis using the Chemical Quantitative Mineral Analysis (CQMA) method [16]. 2. Material and Methods 2.1. Kaolin Samples The granite-derived kaolins of the Karlovy Vary region and kaolins from K-feldspar-rich sedimentary rocks of the Pilsen region represent two main Czech kaolin deposits [ 17 , 18 ]. The three kaolin samples originating from the Karlovy Vary region are from personal collection and are labeled as Bo (locality Božiˇcany), Se (locality Sedlec) and Po (locality Podboˇrany). Kaolin samples originating from the Pilsen Basin were obtained from LB Minerals, Ltd., Czech Republic, and are labelled as Ka (KKN from locality Kaznˇejov), Br (locality Horn í Bˇr í za) and Ch (DSF from locality Chlumˇcany). All kaolin samples were subjected to sieving through 0.04 mm sieve. 2.2. Kaolin–Vermiculite Ceramic Mixtures Vermiculite from the Paraiba region of Brazil (Ver) [ 19 ] was supplied by Grena, Ltd., Vesel í nad Lužnic í , Czech Republic. Sample (30 g) was milled using agate planetary mill Fritsch Pulverisette 5 and then sieved to the fraction <40 µm. The ceramic kaolin–vermiculite mixtures marked as C-Bo, C-Se, C-Po, C-Ka, C-Br, and C-Ch were prepared in their mass ratio of 1:1, homogenized for 1 h (Heidolph Reax overhead shaker, REAX 20/4, Merck, Darmstadt, Germany), and then milled for 15 min at 550 rpm in agate planetary mill Fritsch Pulverisette 5. Samples were prepared in a porcelain combustion boat and then sintered in an electrical laboratory furnace LH15/13 at the heating rates 10 ◦ C min −1 up to 1000 ◦ C and 2 ◦ C min −1 to Materials 2019,12, 3104 3 of 13 1300 ◦ C. The samples were then left at this temperature for 1 h and after that slowly cooled to the room temperature. The ceramic samples were marked identically as their parent ceramic mixtures. 2.3. Methods Elemental analysis was performed using the SPECTRO XEPOS energy dispersive X-ray fluorescence (ED-XRF) spectrometer (Spectro Analytical Instruments, Kleve, Germany). The results from the XRF analysis were calculated to the stoichiometric metal oxides concentrations. Simultaneous thermogravimetric (TG) and differential thermal analysis (DTA) of samples was performed in platinum crucibles using the experimental system SETARAM SETSYS 18 TM TG/DTA/TMA (Lyon, France) with an “S”-type measuring rod (tricouple) in argon atmosphere (6N) at a heating rate of 10 ◦ C min −1 from 25 to 1300 ◦ C. The transition temperatures determined according DTA with an estimated error of ±5◦C. The X-ray diffraction (XRD) analysis of crystalline mineral phases was carried out on the X-ray diffractometer Ultima IV (RIGAKU, Tokyo, Japan). The XRD patterns were recorded in the 8–60 ◦ 2 θ range (CuK α radiation λ =0.15418 nm, a scintillation detector and a scanning rate of 2 ◦ /min at 40 kV and 40 mA). The porosity of the dried ceramic samples was measured using a mercury intrusion porosimeter AutoPore IV 9500 (Micromeritics Instrument Corporation, Norcross, GA, USA). All methods listed here are more fully described in the previous work [6,20]. The Chemical Quantitative Mineral Analysis (CQMA) method recalculates the elemental bulk chemical analysis (analytes SiO 2 , Al 2 O 3 , etc.) to the identified minerals in XRD analysis and their crystallochemical formulas of the analyzed sample. The calculation of mineral amounts is performed by optimization procedures(e.g., the leastsquare and/ornon-negative least squaremethod). Theadditional more detailed information as well as recalculation of the quantitative content of minerals determined by other methods to their elemental bulk chemical analysis has recently been published [16]. 3. Results 3.1. Kaolin Samples The chemical compositions of kaolin samples indicate not pure kaolinites (Al 2 O 3· 2SiO 2· 2H 2 O) (Table 1). The XRD patterns of kaolins (Figure 1) showed kaolinite (PDF card no. 00-058-2005), muscovite (PDF card no. 01-076-0668), quartz (PDF card no. 01-086-2237), and orthoclase (PDF card no. 01-075-1592) in the kaolin sample Ch. Table 1. ED-XRF analysis of kaolin samples. Samples Hi 1Bo 0.93 Se 1.08 Po 1.22 Ka 1.57 Br 1.59 Ch 1.30 Oxides (mass %) SiO249.97 49.65 56.25 49.71 50.83 50.45 TiO20.16 0.07 0.38 0.66 0.93 0.72 Al2O334.62 35.17 30.07 34.80 33.61 33.94 Fe2O31.10 0.86 0.72 0.72 0.67 0.72 CaO 0.15 0.12 0.25 0.09 0.01 0.06 MgO 0.22 0.21 0.24 0.21 0.17 0.27 Na2O 0.03 0.03 0.03 0.06 0.08 0.07 K2O 1.18 0.93 0.84 1.21 1.41 1.88 L.O.I. 212.21 12.26 11.15 12.26 12.01 11.63 Sum 99.66 99.30 99.94 99.72 99.72 99.75 1Hinckley index [21]; 2Loss on ignition after heating at 1000 ◦C for 2 h =H2O+. Materials 2019,12, 3104 4 of 13 Materials 2019, 12, x FOR PEER REVIEW 4 of 13 Figure 1. XRD patterns of kaolin samples from 5 to 40° 2θ. Peaks of kaolinite (K) are unlabeled; M— muscovite, Q—quartz, and O—orthoclase. The DTA/TG analysis (DTA curves in Figure 2) of kaolins heated to 1100 °C displayed thermal events occurring within the temperature intervals characteristic for transformation of kaolinite and micas (Table 2). Table 2. TG/DTA of kaolin samples Ranges: 1 2 3 4 Total Mass Loss Kaolin Sample Mass (mg) ΔT1 (°C) Δm1 (mg) ΔT2 (°C) Δm2 (mg) T2min (°C) ΔT3 (°C) Δm3 (mg) ΔT4 (mg) T4max (°C) ΔmTML (mg) (%) Bo 20.20 20–175 0.04 410–730 2.36 526 730–946 0.18 963–1031 988 2.58 12.8 Se 21.40 20–160 0.05 403–720 2.41 528 720–946 0.13 959–1041 990 2.59 12.1 Po 18.60 20–185 0.11 440–730 2.04 535 730–932 0.13 955–1041 993 2.28 12.3 Ka 20.90 20–200 0.06 450–725 2.32 535 750–946 0.16 961–1041 997 2.54 12.2 Br 19.90 20–170 0.01 430–720 2.19 533 730–931 0.13 972–1051 999 2.33 11.7 Ch 27.90 20–160 0.12 410–715 2.88 534 720–939 0.11 976–1047 997 3.11 11.1 Figure 1. XRD patterns of kaolin samples from 5 to 40 ◦ 2 θ . Peaks of kaolinite (K) are unlabeled; M—muscovite, Q—quartz, and O—orthoclase. The DTA/TG analysis (DTA curves in Figure 2) of kaolins heated to 1100 ◦ C displayed thermal events occurring within the temperature intervals characteristic for transformation of kaolinite and micas (Table 2). Table 2. TG/DTA of kaolin samples. Ranges: 1 2 3 4 Total Mass Loss Kaolin Sample Mass (mg) ∆T1 (◦C) ∆m1 (mg) ∆T2 (◦C) ∆m2 (mg) T2min (◦C) ∆T3 (◦C) ∆m3 (mg) ∆T4 (mg) T4max (◦C) ∆mTML (mg) (%) Bo 20.20 20–175 0.04 410–730 2.36 526 730–946 0.18 963–1031 988 2.58 12.8 Se 21.40 20–160 0.05 403–720 2.41 528 720–946 0.13 959–1041 990 2.59 12.1 Po 18.60 20–185 0.11 440–730 2.04 535 730–932 0.13 955–1041 993 2.28 12.3 Ka 20.90 20–200 0.06 450–725 2.32 535 750–946 0.16 961–1041 997 2.54 12.2 Br 19.90 20–170 0.01 430–720 2.19 533 730–931 0.13 972–1051 999 2.33 11.7 Ch 27.90 20–160 0.12 410–715 2.88 534 720–939 0.11 976–1047 997 3.11 11.1 Materials 2019,12, 3104 5 of 13 1 Figure 2 Figure 4 Figure 2. DTA curves of kaolin samples. The temperature conversions of kaolins containing admixture of muscovite and quartz produce new phases that will be involved in the sintering and crystallization process of cordierite-indialite. The temperature range ∆ T 1 =20–200 ◦ C correspond to the loss of adsorbed water [ 22 , 23 ]. The temperature range ∆ T 2 =400–730 ◦ C was assigned to dehydroxylation of kaolinite and conversion to metakaolinite (e.g., [11,22,24]), according to the reaction (Equation (1)) Al2Si2O5(OH)4 Kaolinite 400–730 ◦C −−−−−−−−→ Al2Si2O7+2H2O Metakaolinite (1) The position of the endothermic minimum T 2min moving from 526 ◦ C to 535 ◦ C was consistent with structural ordering, expressed by Hinckley index [20,25,26] (Table 1). The temperature range ∆ T 3 =720–946 ◦ C of an endothermal process accompanied by the mass loss ∆ m 3 about 0.67 ± 0.17% was assigned to dehydroxylation of muscovite [ 11 , 27 ]. The transformation temperature from muscovite into dehydroxylated muscovite were reported in the various ranges (e.g., 300–1000 ◦C [27], 650–750 ◦C [28], 850–1000 ◦C [29]), according to the reaction (Equation (2)) KAl2(AlSi3)O10(OH)2 Muscovite 900 ◦C −−−−−→ KAl2(AlSi3)O11 Dehydroxylated muscovite +H2O (2) The temperature range ∆ T 4 =955 ◦ C–1051 ◦ C and the exothermic maximum from 988–999 ◦ C (marked as T 4max in Table 2) was assigned to the transformation of metakaolinite to primary mullite. Other small diffuse exothermic effects above 1050 ◦ C were attributed to the secondary mullite [ 29 ]. The processes of the formation of primary and secondary mullites from the kaolin refractory clays were mostly described by the reactions (Equations (3)–(5)) [12,29,30] Al2Si2O7 Metakaolinite 550–1200 ◦C −−−−−−−−−→ (3Al2O3·2SiO2) Primary mullite +SiO2(amorphous)(3) Depending on the structural defects of kaolinites, metakaolinite structure decomposes at about 900 ◦C with segregation of alumina and silica according to the reaction (Equation (4)) [31] Al2Si2O7 Metakaolinite 900 ◦C −−−−−→ γ−Al2O3 Alumina +2SiO2(4) A very diffuse DTA exothermic peaks observed in the region of 1100–1200 ◦ C was attributed to a recombination reaction of the segregated phases (Equation (4)) and then to the formation of secondary mullite (Equation (5)) 4SiO2+6γ−Al2O3 >1050 ◦C −−−−−−−→ 2(3Al2O3·2SiO2) Secondary mullite (5) Materials 2019,12, 3104 6 of 13 Structure of dehydroxylated muscovite is unstable and easily melts in the temperature of the formation stage of mullite (Equation (6)). The initial stage of mullite crystals in SiO 2 —melt can be supported by the presence of K 2 O released upon melting from the dehydroxylated muscovite [ 32 ] according to the reaction (Equation (6)) 2KAl2(AlSi3)O11 Dehydroxylated muscovite 1125–1150 ◦C −−−−−−−−−−→ (3Al2O3·2SiO2) Mullite +K2O+4SiO2(6) 3.2. Cordierite Samples The elemental composition of the ceramic samples prepared at 1300 ◦ C was recalculated to the stoichiometric oxides. Fe was recalculated to Fe2O3(Table 3). Table 3. The ED-XRF analysis of ceramic samples. Oxides Samples (mass %) C-Bo C-Se C-Po C-Ka C-Br C-Ch SiO252.88 52.82 56.01 52.71 53.29 52.95 TiO20.57 0.52 0.62 0.87 0.89 0.81 Al2O325.76 26.13 23.00 25.77 25.15 25.27 Fe2O34.68 4.53 4.48 4.45 3.99 4.44 MnO 0.06 0.06 0.05 0.05 0.05 0.05 CaO 0.81 0.75 0.86 0.73 0.70 0.70 MgO 13.25 13.24 13.19 13.28 13.22 13.26 Na2O 0.21 0.21 0.19 0.20 0.22 0.21 K2O 1.69 1.51 1.50 1.71 1.83 2.09 Sum 99.91 99.77 99.90 99.77 99.34 99.78 The XRD patterns of ceramic samples were very similar and two ceramic samples C-Se and C-Po are given as examples (Figure 3). The crystalline indialite (PDF card No. 01-082-1884), enstatite (PDF card no. 00-019-0768) and a broad area of non-crystalline phases were identified at all ceramic samples. The TG/DTA results of kaolin–vermiculite mixtures (Table 4) and DTA curves (Figure 4) were evaluated as follows: dehydration of vermiculite and kaolinite have occurred in the temperature range ∆ T 1 =20–265 ◦ C. The temperature range of ∆ T 2 =407–437 ◦ C, accompanied by a mass loss of approximately 6.58 ± 0.30%, was assigned to dehydroxylation of kaolinite and a continuing dehydration and dehydroxylation of vermiculite. Vermiculite dehydroxylated and crystallized to enstatite at about 835 ◦ C at the temperature range ∆ T 3 =745–848 ◦ C (marked E in Figure 4) [ 33 , 34 ]. The exothermal reactions in the range ∆ T 4 =905–1017 ◦ C and maximum peaks at T 4max =960–972 ◦ C have been attributed to the formation of MgAl 2 O 4 spinel and µ -cordierite [ 35 , 36 ]. The temperature range ∆ T 5 corresponds to the melting and crystallization of indialite and enstatite. Table 4. TG/DTA of kaolin–vermiculite ceramic mixtures. Ranges: 1 2 3 4 5 Total Mass Loss Sample Mass m (mg) ∆T1 (◦C) ∆m1 (mg) ∆T2 (◦C) ∆m2 (mg) ∆T5 (◦C) ∆T3 (◦C) ∆m3 (mg) ∆T4 (◦C) T4max (◦C) ∆T5 (◦C) ∆mTML (mg) (%) C-Bo 15.12 20–256 0.19 409–597 1.01 1084–1254 757–836 0.18 913–999 964 1084–1254 1.38 9.1 C-Se 15.00 20–226 0.18 416–610 1.01 1086–1255 755–843 0.19 906–1000 960 1086–1255 1.38 9.2 C-Po 15.11 20–233 0.19 407–631 0.93 1075–1252 753–838 0.18 905–1002 964 1075–1252 1.30 8.6 C-Ka 14.97 20–251 0.16 424–609 1.02 1080–1246 745–848 0.16 906–1017 960 1080–1246 1.34 8.9 C-Br 15.14 20–239 0.17 434–603 0.95 1102–1258 745–835 0.16 905–999 970 1102–1258 1.28 8.5 C-Ch 15.15 20–265 0.17 437–650 1.04 1104–1243 748–848 0.12 907–999 972 1104–1243 1.33 8.8 Materials 2019,12, 3104 7 of 13 Materials 2019, 12, x FOR PEER REVIEW 6 of 13 Structure of dehydroxylated muscovite is unstable and easily melts in the temperature of the formation stage of mullite (Equation (6)). The initial stage of mullite crystals in SiO 2 —melt can be supported by the presence of K 2 O released upon melting from the dehydroxylated muscovite [32] according to the reaction (Equation (6)) 2KAl 2 (AlSi 3 )O 11  ° 󰇒 ⎯ ⎯ ⎯ ⎯ ⎯ ⎯ ⎯ ⎯ 󰇏 (3Al 2 O 3 ·2SiO 2 ) + K 2 O + 4SiO 2 Dehydroxylated muscovite Mullite (6) 3.2. Cordierite Samples The elemental composition of the ceramic samples prepared at 1300 °C was recalculated to the stoichiometric oxides. Fe was recalculated to Fe 2 O 3 (Table 3). Table 3. The ED-XRF analysis of ceramic samples Oxides Samples (mass %) C-Bo C-Se C-Po C-Ka C-Br C-Ch SiO 2 52.88 52.82 56.01 52.71 53.29 52.95 TiO 2 0.57 0.52 0.62 0.87 0.89 0.81 Al 2 O 3 25.76 26.13 23.00 25.77 25.15 25.27 Fe 2 O 3 4.68 4.53 4.48 4.45 3.99 4.44 MnO 0.06 0.06 0.05 0.05 0.05 0.05 CaO 0.81 0.75 0.86 0.73 0.70 0.70 MgO 13.25 13.24 13.19 13.28 13.22 13.26 Na 2 O 0.21 0.21 0.19 0.20 0.22 0.21 K 2 O 1.69 1.51 1.50 1.71 1.83 2.09 Sum 99.91 99.77 99.90 99.77 99.34 99.78 The XRD patterns of ceramic samples were very similar and two ceramic samples C-Se and CPo are given as examples (Figure 3). The crystalline indialite (PDF card No. 01-082-1884), enstatite (PDF card no. 00-019-0768) and a broad area of non-crystalline phases were identified at all ceramic samples. The TG/DTA results of kaolin–vermiculite mixtures (Table 4) and DTA curves (Figure 4) were evaluated as follows: dehydration of vermiculite and kaolinite have occurred in the temperature range ΔT 1 = 20–265 °C. The temperature range of ΔT 2 = 407–437 °C, accompanied by a mass loss of approximately 6.58 ± 0.30%, was assigned to dehydroxylation of kaolinite and a continuing dehydration and dehydroxylation of vermiculite. Vermiculite dehydroxylated and crystallized to enstatite at about 835 °C at the temperature range ΔT 3 = 745–848 °C (marked E in Figure 4) [33,34]. The exothermal reactions in the range ΔT 4 = 905–1017 °C and maximum peaks at T 4max = 960–972 °C have been attributed to the formation of MgAl 2 O 4 spinel and µ-cordierite [35,36]. The temperature range ΔT 5 corresponds to the melting and crystallization of indialite and enstatite. Figure 3. XRD patterns of ceramic samples C-Se and C-Po. The peaks of indialite are unmarked and enstatite is marked with arrow. A non-crystalline phase area is separated from the background by a dashed line. 1 Figure 2 Figure 4 Figure 4. DTA curves of kaolin–vermiculite mixtures. E—enstatite. The transformation temperatures of the mineral phases and the temperatures prior to the crystallization process during the sintering of the kaolin–vermiculite ceramic mixtures on the TG-DTA curves (Figure 4) were determined at the five ranges (Table 4). 4. Discussion The process of the formation of cordierite/indialite from kaolin–vermiculite mixtures can be generally described by the reactions including transformation of vermiculite to enstatite (Equation (7)) 2 Mg3(Si3Al1)O10(OH)2 Vermiculite 700–900 ◦C −−−−−−−−→ 6MgSiO3 Enstatite +Al2O3+H2O (7) and then, the reaction between enstatite, mullite and SiO 2 into cordierite/indialite formation (Equation (8)) 6MgSiO3 Enstatite +2(3Al2O3·2SiO2) Mullite +5SiO21250 ◦C −−−−−−→ 3Mg2Al4Si5O18 Cordierite/Indialite (8) The previous literature has confirmed the facts, that the impurity products react with the liquid phase influencing crystallization. Therefore, the position of the exothermic peak shifts to the lower temperatures, e.g., the presence of 1.5 mass % K2O lowered temperature about 25 ◦C [37]. The CQMA procedure [ 16 ] calculated from the bulk chemical analyses crystallochemical formulas and quantity of minerals, which were identified using the XRD patterns (Figure 1). In the case of Materials 2019,12, 3104 8 of 13 kaolin samples, the CQMA recalculated all elements (Table 1) to the kaolinite Al 2 Si 2 O 5 (OH) 4, quartz SiO 2 , orthoclase KAlSi 3 O 8 and muscovite, whose crystallochemical formula has been refined to K 0.87 Na 0.07 (Al 1.43 Fe 3+0.07 Mg 0.50 Ti 0.02 )(Si 3.39 Al 0.61 )O 10 (OH) 2 , and residual elements Fe and Ti to the commonly occurring minor phases in kaolins as limonite Fe2O3·H2O and rutile TiO2(Table 5). Table 5. Quantitative amounts of minerals in kaolin samples determined using CQMA method. Mineral (mass %) Samples Bo Se Po Ka Br Ch Kaolinite 81.9 85.0 73.3 82.4 79.0 79.7 Muscovite 9.0 6.6 5.2 9.1 9.9 4.2 Quartz 7.2 6.7 19.5 6.7 9.0 6.0 Limonite 1.2 0.9 0.8 0.7 0.7 0.8 Rutile 0.1 0.1 0.3 0.6 0.9 0.7 Orthoclase 0.0 0.0 0.0 0.0 0.0 8.0 Sum 99.4 99.3 99.1 99.5 99.5 99.4 The results in the Table 5revealed similar amounts of kaolinites in kaolin samples Bo, Se, and Po from the Karlovy Vary region (80.1 ± 6.1 mass %) and kaolin samples Ka, Br, and Ch from the Pilsen area (80.4 ± 1.8 mass %), except the kaolin sample Po, which is poor in kaolinite (73.3 mass %) at the expense of quartz (19.5 mass %). All kaolins contain K-bearing muscovite in amounts lower than 10 mass % and orthoclase (8 mass % in kaolin sample Ch). In the case of ceramic samples, the CQMA recalculated all elements of the bulk chemical analyses (Table 3) to the quantitative amounts of crystalline minerals indialite/cordierite and enstatite (MgSiO 3 ), identified by XRD patterns (Figure 2). The refined crystallochemical formula Ca 0.1 Mg 1.90 Fe 3+0.40 Al 3.60 Si 5.00 O 18 of cordierite/indialite includes all content of Fe and Ca determined at the six ED-XRF analyses of ceramic samples (Table 3). It should be noted that a similar crystallochemical formula of indialite was reported by Balassone et al. [ 38 ]. The excess Si and all percentages of Ti, Na, and K were calculated as the oxidic non-crystalline phases based on 10SiO 2 (Table 6), while considering all elements—Al, Fe, Mg, andCa (Table 3)—already included in crystallochemical formulas of crystalline cordierite/indialite and enstatite. Table 6. Quantitative amounts of minerals in ceramic samples determined using CQMA method. Mineral (mass %) Samples C-Bo C-Se C-Po C-Ka C-Br C-Ch Cordierite 84.0 85.1 75.2 84.1 81.7 82.3 Enstatite 6.2 5.8 8.9 6.5 6.8 6.7 Others (1) 9.4 8.8 15.1 9.3 11.1 10.6 Sum 99.6 99.7 99.2 99.9 99.6 99.6 (1) The calculated oxidic formulas of residual—non-crystalline phases based on 10SiO 2 : C-Bo: 0.29Na 2 O · 1.52K 2 O · 0.61TiO 2· 10SiO 2 ; C-Se: 0.31Na 2 O · 1.45K 2 O · 0.60TiO 2· 10SiO 2 ; C-Po: 0.15Na 2 O · 0.65K 2 O · 0.36TiO 2·10SiO2; C-Ka: 0.28Na 2 O · 1.72K 2 O · 0.96TiO 2· 10SiO 2 ; C-Br: 0.26Na 2 O · 1.41K 2 O · 0.82TiO 2· 10SiO 2 ; C-Ch: 0.27Na 2 O · 1.72K 2 O · 0.81TiO2·10SiO2. The quantitative amounts of minerals in ceramic samples determined using CQMA method (Table 6) can then be considered as the calculated percentages of the highest possible crystalline phases and the lowest possible non-crystalline phases. In six cordierite samples, the amount of cordierite/indialite varied from 75.2 to 85.1 mass %, enstatite from 5.8 to 8.9 mass % and non-crystalline phases from 8.8 to 15.1 mass %, depending on the purity of kaolins, i.e., containing kaolinite from 73.3 to 85.0, muscovite from 4.2 to 9.9 and quartz from 6.0 to 19.5 (mass %). The temperature corresponding to the melting and crystallization of indialite at the stage ∆ T 5 varied from 177 to 139 ◦ C (Table 4) in the relation to the amount of K 2 O from 1.50 mass % to 2.09 mass % (Table 3). The relation in Figure 5a Materials 2019,12, 3104 9 of 13 between the temperature ∆ T 5 (Table 4) and the amount of K 2 O in the ceramic mixtures (Table 3) was described by the linear regression function (Equation (9)) ∆T5(◦C) =263.86 −58.68 ×K2O, the correlation coefficient R2=0.891 (9) The relationship makes it possible to determine the maximum K 2 O difference of 0.59% by mass between C-Po and C-Ch and corresponding to the ∆T5temperature reduced by 42 ◦C. A high cordierite, generally prepared by ceramic procedures at 1300 ◦ C, crystallizes in a pseudohexagonal symmetry (space group P6/mcc) (e.g., Benito et al. [ 39 ]). The earlier works have shown that alkalis can be incorporated into the structural channels of cordierite. In this case, a charge of the Al/Si ratio in the framework balances according to the equation (K, Na)++Al3+→Si4+ , causing distortion of the hexagonal symmetry (e.g., [ 40 – 43 ]). Diffusion of potassium ions was documented during the dehydroxylation processes of muscovite and kaolinite and detected in metakaolinite layers above 900 ◦ C [ 14 ]. The relation in Figure 5b shows a slightly larger lattice parameters aand cof indialites identified in ceramic samples in comparison with pure indialites designated as 1: Mg 2.00 Al 4.00 Si 5.00 O 18 [ 4 ] and 2: Mg 2.00 Al 4.00 Si 5.00 O 18 [ 44 ]. The similarly to the parameters of K-substituted indialites, designated as 3: (K 0.17 Mg 1.94 Fe 0.06 Ca 0.04 )Al 4.25 Si 4.75 O 18 [ 38 ] and 4: (K 0.25 Mg 1.75 )Al 4.25 Si 4.75 O 18 [ 43 ] can be considered as the result of a possible migration and substitution of potassium ions into their structure. Influence of kaolin on the quantity of crystallizing indialite/cordierite and quartz admixture in kaolin on the formulation of the non-crystalline phase is declared in Figure 6. The amounts of indialite/ cordierite in the ceramic samples (Table 6, Figure 6a) correlate with the amount of kaolinite in kaolins (Table 5), as it was described by the linear regression function (Equation (10)) Indialite/cordierite (mass %) =11.91 +0.87 ×kaolinite (mass %), R2=0.939 (10) Similarly, the good relation between the amounts of non-crystalline phases in the ceramic samples (Table 6) and the amounts of quartz in kaolins (Table 5, Figure 6b) was described by the linear regression function (Equation (11)) Non-crystalline phases (mass %) =6.39 +0.46 ×quartz (mass %), R2=0.942 (11) Materials 2019, 12, x FOR PEER REVIEW 9 of 13 The quantitative amounts of minerals in ceramic samples determined using CQMA method (Table 6) can then be considered as the calculated percentages of the highest possible crystalline phases and the lowest possible non-crystalline phases. In six cordierite samples, the amount of cordierite/indialite varied from 75.2 to 85.1 mass %, enstatite from 5.8 to 8.9 mass % and noncrystalline phases from 8.8 to 15.1 mass %, depending on the purity of kaolins, i.e., containing kaolinite from 73.3 to 85.0, muscovite from 4.2 to 9.9 and quartz from 6.0 to 19.5 (mass %). The temperature corresponding to the melting and crystallization of indialite at the stage ΔT5 varied from 177 to 139 °C (Table 4) in the relation to the amount of K2O from 1.50 mass % to 2.09 mass % (Table 3). The relation in Figure 5a between the temperature ΔT5 (Table 4) and the amount of K2O in the ceramic mixtures (Table 3) was described by the linear regression function (Equation (9)) ΔT5(°C) = 263.86 − 58.68 × K2O, the correlation coefficient R2 = 0.891 (9) The relationship makes it possible to determine the maximum K2O difference of 0.59% by mass between C-Po and C-Ch and corresponding to the ΔT5 temperature reduced by 42 °C. A high cordierite, generally prepared by ceramic procedures at 1300 °C, crystallizes in a pseudohexagonal symmetry (space group P6/mcc) (e.g., Benito et al. [39]). The earlier works have shown that alkalis can be incorporated into the structural channels of cordierite. In this case, a charge of the Al/Si ratio in the framework balances according to the equation (K, Na)+ + Al3+ → Si4+, causing distortion of the hexagonal symmetry (e.g., [40–43]). Diffusion of potassium ions was documented during the dehydroxylation processes of muscovite and kaolinite and detected in metakaolinite layers above 900 °C [14]. The relation in Figure 5b shows a slightly larger lattice parameters a and c of indialites identified in ceramic samples in comparison with pure indialites designated as 1: Mg2.00Al4.00Si5.00O18 [4] and 2: Mg2.00Al4.00Si5.00O18 [44]. The similarly to the parameters of K-substituted indialites, designated as 3: (K0.17Mg1.94Fe0.06 Ca0.04)Al4.25Si4.75O18 [38] and 4: (K0.25Mg1.75)Al4.25Si4.75O18 [43] can be considered as the result of a possible migration and substitution of potassium ions into their structure. Influence of kaolin on the quantity of crystallizing indialite/cordierite and quartz admixture in kaolin on the formulation of the non-crystalline phase is declared in Figure 6. The amounts of indialite /cordierite in the ceramic samples (Table 6, Figure 6a) correlate with the amount of kaolinite in kaolins (Table 5), as it was described by the linear regression function (Equation (10)) Indialite/cordierite (mass %) = 11.91 + 0.87 × kaolinite (mass %), R2 = 0.939 (10) Similarly, the good relation between the amounts of non-crystalline phases in the ceramic samples (Table 6) and the amounts of quartz in kaolins (Table 5, Figure 6b) was described by the linear regression function (Equation (11)) Non-crystalline phases (mass %) = 6.39 + 0.46 × quartz (mass %), R2 = 0.942 (11) Figure 5. Relationsships between: ( a ) temperature ∆ T 5 vs. amount of K 2 O in ceramic samples and ( b ) unit cell parameters cvs. aof indialites. The parameters labeled as: 1: Mg 2.00 Al 4.00 Si 5.00 O 18 [ 4 ]; 2: Mg 2.00 Al 4.00 Si 5.00 O 18 [ 44 ]; 3: (K 0.17 Mg 1.94 Fe 0.06 Ca 0.04 )Al 4.25 Si 4.75 O 18 [ 38 ]; and 4: (K 0.25 Mg 1.75 )Al 4.25 Si4.75O18 [43].