Alkali-Activated Metakaolins: Mineral Chemistry and Quantitative Mineral Composition

: The reaction products resulting from the alkali-activation of metakaolin are impacted by the composition of the initial kaolin, and amount of alkali-activated kaolinite and water. The present study focused on analyzing these parameters on the metakaolins calcined at 800 ◦ C from three kaolins, and the metakaolins’ alkali activation for 2, 3 and 28 days. The ﬁrst objective was to evaluate the mineral chemistry and quantitative mineral phase composition from the bulk chemical analysis using the chemical quantitative mineral analysis (CQMA) procedure and conduct a comparison of the chemistry of the metakaolins after alkali activation for 28 days according to the elements Al, Si, Na and K, using the leaching test in distilled water. The second task was to search for possible relationships between the quantitative number of phases in alkali-activated metakaolins and compressive strength. The main methods used for the characterization of material were X-ray ﬂuorescence, X-ray diffraction, thermal TG/DTA and infrared spectroscopy. Metakaolins alkali activated for 28 days contained crystalline quartz, muscovite, orthoclase, and unreacted metakaolinite contained zeolite A (Z-A), hydrosodalite (HS) and thermonatrite (TN) in the amorphous/weakly crystalline phase. The compressive strengths (CS) from 6.42 ± 0.33 to 9.97 ± 0.50 MPa are related positively to H 2 O+ and H 2 O bound in HS and TN.


Introduction
Kaolin minerals are safe and abundant natural materials that are excellent candidates for green technologies in the industry.Recent developments in the use of kaolin clay include the production of metakaolin as an artificial pozzolanic additive to cement-based systems.Over the last years, the research focus has been on the feasibility of using this "green" binder instead of, or as a supplement to, conventional cement applications [1].In the literature, the terms alkali-activated material and geopolymers occur interchangeably and even as synonyms [2].Alkali-activated materials are binders which can develop high compressive strength, chemical resistance, and thermal stability after preparation.The precursor of the alkali-activated materials is a mixture of a solid aluminosilicate and a solid alkali source, and their admixtures with water.The alkali-activation procedure is comparable to the preparation of ordinary Portland cement.In theory, the whole aluminosilicate precursor could potentially be dissolved and polymerized [3].The process produces metastable amorphous and or "proto-zeolitic nuclei" in semi-crystalline alkali aluminosilicate hydrates, which are often termed zeolite precursor gels or geopolymer gels [4][5][6][7].
The common process, where metakaolin from high-quality kaolin is formed by calcination at 650-850 • C, is one of the conventional production methods [8][9][10][11].The reaction products of the metakaolin alkali-activation process confirmed the presence of remaining kaolinite, not fully reacted with the alkali activator in metakaolin [12,13].The alkaline activation of metakaolin with NaOH solution involves reactions that produce amorphous hydrated sodium aluminosilicates of the general formula Na 2 O•3SiO 2 •Al 2 O 3 •3H 2 O with a predominant three-dimensional structure [14].
To explain and refine the phase composition of the activated products of kaolinite, analytical methods should be employed.X-ray diffraction (XRD) qualitative and quantitative phase analysis have limited capabilities for studying amorphous phases.Traditionally, powder XRD deals with the characterization of polycrystalline materials that contain amorphous or weakly crystalline phases.The contributions of the intensities of the amorphous phases to the diffraction pattern are not always obvious, especially at low concentrations.The available method for quantitative phase analysis of these materials is quantitative XRD coupled with Rietveld analysis.However, their accuracy is highly dependent on the 'degree of crystallinity' of the solids present.The X-ray amorphous phase cannot be directly measured, and the crystalline phases in the presence of amorphous/unidentified crystalline phases may be significantly overestimated [15].
Considering the quantity of the phases in the activated system, where a certain amount of amorphous matter is expected, the quantitative estimation can be performed using several approaches.Currently, the quantitative phase analysis of amorphous components in the mixture was performed using the direct-derivation method, including a backgroundsubtracted halo pattern together with profile models for crystalline components [16].
In another study the combination of analytical methods, two XRD methods and point counting using SEM, was able to assess the fraction of reacted metakaolin quantitatively for four geopolymer samples [17].One more study integrated the XRD data of identified minerals with relevant chemical analysis using the chemical quantitative mineral analysis (CQMA) procedure [18,19].The CQMA procedure performs recalculation of the bulk chemical analyses (XRF) to the quantitative number of phases occurring in all crystallization stages and refines the mineral composition.
The present study focused on the experimental dehydroxylation of kaolins and the formation of metakaolins at 800 • C. The alkali activation of metakaolins to geopolymer precursors was characterized for 2, 3 and 28 days.The first objective was to evaluate the mineral chemistry and quantitative mineral phase composition from the bulk chemical analysis using the CQMA procedure and the comparison of the chemistry of metakaolins after alkali activation for 28 days according to the elements Al, Si, Na and K using the leaching test in distilled water.The second task was solving the relation between the quantitative mineral composition of metakaolins alkali activated for 28 days and compressive strengths.The study aims to be guide for further application of activated metakaolins in cements regarding composition.

Materials and Samples Preparation
The three kaolins denoted as samples 1-3 originated from the Sedlec, Kaznějov and Chlumčany kaolin deposits in the Czech Republic, respectively, was purchased from LB Minerals, Ltd. (Horní Bříza, Czech Republic).Sodium hydroxide (NaOH) was purchased from Lach-Ner Co. (Neratovice, Czech Republic).

Characterization Techniques
The elemental analysis was obtained using an ED-XRF spectrometer (Spectro Analytical Instruments, Kleve, Germany).Each sample (2 × 4 g) was mixed with wax (0.9 g) and pressed at 10 tons for 30 s using a manual hydraulic press BSL-2 (BrioHranice, Hranice, Czech Republic) to a cylindrical pellet.The concentration of elements Si, Al, K, Na in water leachates was determined using high-resolution continuum source AAS, contrAA ® 700 (Analytik Jena AG, Jena, Germany).
The conversion of hydrocarbons to carbon dioxide and water vapor was determined at 1000 • C using a RC612 Multiphase Carbon and Hydrogen/Moisture Analyzer (LECO Instruments, St. Joseph, MI, USA) at oxygen of 99.95% purity and flow 3 L/min.
The specific surface area (S) was measured using the 3Flex physisorption set-up (Micromeritics Instrument Corporation, Norcross, GA, USA) and was quantified according to the classical Brunauer-Emmett-Teller (BET) theory for the p/p 0 = 0.05-0.25 [20].
Simultaneous (TG/DTA) thermal analyzer STA 504 (BÄHR-Thermoanalyse GmbH, Hüllhorst, Germany) was used to measure changes in the kaolin mass and temperature at a heating rate of 10 • C/min between 25 and 1200 • C in an air flow of 5 L/h.The X-ray diffraction (XRD) analyses were performed with a Rigaku SmartLab diffractometer (RIGAKU Corporation, Tokyo, Japan), which was equipped by detector D/teX Ultra 250 and operated at 40 kV and 40 mA in the symmetrical Bragg-Brentano geometry.The XRD measurements were performed in the 2θ range with the CoKα radiation at the speed of 0.5 • /min and a step size of 0.01 • .The samples were measured in the Si sample holder rotated with a speed of 15 rpm.The XRD patterns were evaluated using PDXL2 software No. 2.4.2.0 (Rigaku Corporation, Tokyo, Japan) and database PDF-2, 2015 (ICDD, Newton Square, PA, USA).
The infrared spectra of the samples were recorded using a Fourier transform infrared (FTIR) spectrometer Nicolet 6700 (Thermo Scientific, Waltham, MA, USA), equipped with the Thermo Scientific OMNIC™ software package.For each sample, 64 scans were recorded over the mid-IR (MIR, 4000-400 cm −1 ) or near-IR (NIR, 8000-4000 cm −1 ) range with a resolution of 4 cm −1 .To obtain spectra in the MIR region, the KBr pressed disk technique (1 mg of sample and 200 mg of KBr) was used, while for NIR spectra, a diffuse reflectance accessory (DRIFT) was utilized.

Test of Metakaolins and Alkali-Activated Metakaolins in Water
The stability of Si, Na, Al, and K elements in the metakaolin M1, M2 and M3 samples and M1-28, M2-28 and M3-28 samples, alkali-activated for 28 days, was evaluated by the stirring of 1 g of a powder sample and 100 mL of distilled water for 24 h.The concentration of elements released into the water was determined after centrifugation of the solid sample using atomic absorption spectrometry (AAS).

Test of Alkali-Activated Metakaolins in Compressive Strength
The compressive strength values of 7 pieces of each sample were measured on the press machine (BRIO, Hranice, Czech Republic) at a loading rate of 500 N•s −1 .Two values (highest and lowest) were excluded, and the remaining five measurements were averaged [21].

CQMA Calculation
Chemical quantitative mineral analysis (CQMA procedure) was used for the recalculation of the bulk chemical analyses (XRF) to the quantitative mineral analyses of crystalline and semi-crystalline alkali aluminosilicate hydrate phases.
For this calculation, the identified (XRD) phases and their crystallochemical formulas were used.The CQMA procedure is based on two principial equations.
The oxides of elements in minerals (c i,calc ) were calculated according to Equation (1): where: c i,calc -the calculated ith element oxide (wt.%) of the sample; c i,j -the percentage (wt.%) of the ith element oxide in the jth mineral phase; w j -the wt.fraction of the jth mineral in the sample; m-the number of calculated minerals.
The wt. fraction of the ith element oxide in the jth mineral c i,j is calculated from the crystallochemical formula of the jth mineral.
The wt. fractions of the jth mineral (w j ) were calculated according to Equation (2): where: c i,exp -the ith element oxide in the sample (wt.%) from bulk chemical analysis; min-minimum calculated value of the sum of quadrates; n-the number of element oxides in the bulk chemical analysis used for the calculation; n ≥ m-calculation condition.The calculation of the % wt.fraction (w j ) of the jth mineral in the sample according to Equation (2) was performed using the least squares CQMA method [18].

TG/DTA Analysis
The thermal transformation of kaolin samples 1-3 was characterized according to TG and DTA curves (Figure 1).The shape of the endothermic peaks supports the concept of a different course of dehydroxylation of kaolinite [22].
The dehydration of adsorbed water can be observed on the small wt.loss to 400 • C. The dehydroxylation process in kaolin samples 1 and 2 forms a broad asymmetric DTA curve from about 400 • C to a maximum at about 518 • C and 537 • C, respectively, while from 400 • C to a maximum at 664 • C in kaolin 3, like in disordered kaolinites [23].
The weight losses on the TG thermograms were between 10 and 13.9% (13.9% correspond to the ideal kaolinite).The difference in the water loss is associated with a defect in the kaolinite structure.
At higher temperatures, an exothermic effect at a maximum of 991.0 • C in 1 and 999.9 • C in 2 and 3 was assigned to the recrystallization of metakaolin to primary mullite [24].
The DTA endotherm peak between 440 and 530 • C formed from the removal of hydroxyls from kaolinite in certain sequences resulted in a metakaolinite structure with the persistence of about 10% residual hydroxyls [25].In the upper temperature regions, dehydration and dehydroxylation may overlap as well as dehydroxylation and recrystallization [26].
Muscovite in kaolins dehydroxylated in the temperature range from 300 to 1000 • C [27], according to the reaction in Equation (3): The different shape of the DTA curve in the kaolin 3 can be formed due to the presence of the hydroxyl populations in this dehydroxylation temperature range [28] and/or the additional effects of the particle size, thickness of platelet and stacking [29].
The different shape of the DTA curve in the kaolin 3 can be formed due to the presence of the hydroxyl populations in this dehydroxylation temperature range [28] and/or the additional effects of the particle size, thickness of platelet and stacking [29].

XRD Analysis
The XRD patterns of kaolin samples (Figure 2a   It was found that low NaOH concentrations promote the crystallization of zeolite A (Z-A), while very high concentrations favor the crystallization of hydrosodalite (HS) [31].Another work [12] documented the formation of Z-A and sodalite in activated metakaolin, and only HS and no other intermediate phases in kaolinite.
In this work, XRD patterns of metakaolins (M1, M2 and M3) and their alkali-activated products are compared in Figure 3.All alkali-activated metakaolin samples contained HS, ( It was found that low NaOH concentrations promote the crystallization of zeolite A (Z-A), while very high concentrations favor the crystallization of hydrosodalite (HS) [31].Another work [12] documented the formation of Z-A and sodalite in activated metakaolin, and only HS and no other intermediate phases in kaolinite.
In addition to the zeolites, thermonatrite (TN) (Na2CO3•H2O, PDF card No. 00-008-0448) was formed by the atmospheric carbonation of the excess NaOH [32].Quartz, muscovite, and orthoclase, which were identified in the metakaolin samples, were retained after alkaline activation.The peaks halo was shifted to the higher 2θ angle position from 20-40°, which was ascribed to the alkali-activated products of metakaolin (geopolymers) [33].

FTIR Spectroscopy Analysis
In addition to the XRD, the FTIR spectroscopy was used to investigate the structural changes of kaolins upon heating at 800 °C and alkali activation.In Figure 4, the MIR

FTIR Spectroscopy Analysis
In addition to the XRD, the FTIR spectroscopy was used to investigate the structural changes of kaolins upon heating at 800 °C and alkali activation.In Figure 4, the MIR spectra of studied kaolins are remarkably similar either in the OH stretching (3700-3600 cm −1 ) or in the lattice (1200-400 cm −1 ) regions (Figure 4).Four resolved intensive bands at 3696, 3670, 3653 and 3620 cm −1 (not shown), related to the OH stretching vibrations of inner--hydrosodalite, +-thermonatrite.The area of halo under the amorphous scattering hump is separated from the background by a dotted line.In addition to the zeolites, thermonatrite (TN) (Na 2 CO 3 •H 2 O, PDF card No. 00-008- 0448) was formed by the atmospheric carbonation of the excess NaOH [32].Quartz, muscovite, and orthoclase, which were identified in the metakaolin samples, were retained after alkaline activation.The peaks halo was shifted to the higher 2θ angle position from 20-40 • , which was ascribed to the alkali-activated products of metakaolin (geopolymers) [33].

FTIR Spectroscopy Analysis
In addition to the XRD, the FTIR spectroscopy was used to investigate the structural changes of kaolins upon heating at 800 • C and alkali activation.In Figure 4, the MIR spectra of studied kaolins are remarkably similar either in the OH stretching (3700-3600 cm −1 ) or in the lattice (1200-400 cm −1 ) regions (Figure 4a).Four resolved intensive bands at 3696, 3670, 3653 and 3620 cm −1 (not shown), related to the OH stretching vibrations of inner-surface and inner groups, indicate well-ordered kaolinite as the dominant phase in all studied kaolins [34,35] Heating of the kaolins at 800 °C induced significant changes in their structure reflected also in the MIR spectra.As The high intensity of the kaolinite bands, overlapping the bands of the minerals' admixture, hinders the identification of the impurities in the kaolins.The only exception is kaolin 2, where an increase in intensity and a slight shift of the Si-O band to higher wavenumbers (796 cm −1 ) compared to kaolins 1 and 2 reflects a higher content of quartz in this sample.For quartz, a doublet near 800 and 780 cm −1 is diagnostic [36].
Minerals 2022, 12, 1342 9 of 18 Heating of the kaolins at 800 • C induced significant changes in their structure reflected also in the MIR spectra.As a result of the dehydroxylation, the OH stretching and bending bands of kaolinite completely disappeared (not shown), while the range 1400-400 cm −1 did not show any features typical for unheated kaolinite (Figure 4b).The number of IR bands was reduced, and only several broad bands remained.The spectrum of M1 shows an exceptionally large band at 1080 cm −1 containing multiple overlapping components of the stretching vibrations of the Si-O and Al-O tetrahedra.The origin of a less intensive but still extremely broad band at 805 cm −1 is unclear; most likely, both the symmetric Si-O and Al-O stretching vibrations absorb in this region [34,37].However, the assignment of the band near 800 cm −1 in metakaolinites to the Al-O bending mode of AlO 6 octahedra was reported as well [9].The absorption peak at 562 cm −1 corresponds to AlO 6 stretching motions and the band at 464 cm −1 to deformation vibrations of the SiO 4 tetrahedra [38].The IR pattern of the M2 strongly resembles that of M1 (Figure 4b).The difference is in the 800-650 cm −1 region, where the characteristic bands of quartz at 798, 782 and 693 cm −1 appeared.Their presence confirms the highest content of this mineral in M2 within the studied samples, as indicated also by the XRD (Figure 1).Compared to M1 and M2, the IR spectrum of M3 shows a shift of the most intensive band to a lower wavenumber, i.e., to 1060 cm −1 (Figure 4b).Such a shift may result from the higher contribution of the tetrahedra-coordinated Al-O groups.Another possible explanation for this shift is the higher content of orthoclase in M3.The main Si-O stretching band of this mineral, appearing at 1035-1015 cm −1 [36], can lower the position of the complex Si-O-Al stretching band.
The alkali activation of metakaolins for 28 days induces significant changes in the IR spectra.A shift of the broad Si-O-Si(Al) asymmetric stretching band of metakaolinite from about 1080 cm −1 (Figure 4b) down to ~1000 cm −1 (Figure 4c) is usually considered to be the result of the formation of geopolymers, although it is also observed during the creation of zeolites from disordered aluminosilicate precursors [39].The band near 720 cm −1 is supposed to indicate the formation of Al IV as the main Al environment in the geopolymers [36], while the peaks in the 460-440 cm −1 region can be assigned to the bending vibrations of the bridging O-Si-O and O-Al-O bonds [40].The presence of alkaline carbonates was confirmed by a band near 1650 cm −1 and less intensive sharp peak at 881 cm −1 related to the asymmetric stretching and out-of-plane bending vibrations, respectively, of the CO 3 2− ion of thermonatrite as confirmed by the XRD results.The bands present in the NIR spectra (8000-4000 cm −1 ) of kaolins (Figure 5) are related to the first overtones of the kaolinites OH stretching vibrations (2νOH) of the structural OH groups, or to the combinations involving stretching and bending modes of the adsorbed water molecules, (ν+δ)OH, and structural OH groups (ν+δ)OH) [35].The NIR spectra of all kaolins, metakaolins as well as their alkali-activated metakaolins are remarkably similar; therefore, only the results for 1, M1 and AM1-28 are discussed.
Untreated kaolinite shows a strong band at 7066 assigned to the 2νOH overtones of the OH stretching modes of inner hydroxyl groups, while a complex band with several more or less resolved peaks in the 7400-7100 cm −1 region corresponds to the first overtones of the coupled inner-surface OH groups [41].The weak band at 5236 cm −1 is due to the combination band of water molecules (ν+δ)H 2 O; the intensive band at 4527 cm −1 is associated with the (ν+δ) OH of inner OH groups, and the band at 4624 cm −1 corresponds to the combination mode of the inner surface hydroxyls.The bands observed below 4500 cm −1 are probably combinations of the OH stretching bands with lattice deformation vibrations involving octahedral atoms [42].
The heating of kaolins at 800 • C resulted in the removal of the structural OH groups of kaolinites evidenced by the almost complete disappearance of the OH bands from the NIR spectra of M1.The very weak band at 7319 cm −1 can be assigned to the first overtone of the isolated (free) surface silanol groups, while that at 7139 cm −1 , to the silanol groups hydrogen bonded to the adsorbed water molecules.The presence of a small amount of water confirms also a weak (ν+δ)H 2 O band at 5235 cm −1 .The slightly more intensive band at 4593 cm −1 may possibly be due to the combination of the OH stretching vibration of free silanol groups and siloxane (Si-O-Si) bending vibrations [43].
the CO3 2− ion of thermonatrite as confirmed by the XRD results.
The bands present in the NIR spectra (8000-4000 cm −1 ) of kaolins (Figu lated to the first overtones of the kaolinites OH stretching vibrations (2νOH) tural OH groups, or to the combinations involving stretching and bending m adsorbed water molecules, (ν+δ)OH, and structural OH groups (ν+δ)OH) [3 spectra of all kaolins, metakaolins as well as their alkali-activated metakaolins ably similar; therefore, only the results for 1, M1 and AM1-28 are discussed.Untreated kaolinite shows a strong band at 7066 assigned to the 2νOH the OH stretching modes of inner hydroxyl groups, while a complex band more or less resolved peaks in the 7400-7100 cm −1 region corresponds to the fi of the coupled inner-surface OH groups [41].The weak band at 5236 cm −1 combination band of water molecules (ν+δ)H2O; the intensive band at Creation of new phases because of the kaolins' dissolution in NaOH also affects the shape of the NIR spectrum of AM1-28.Broad bands at 6965 cm −1 corresponding to the 2νH 2 O overtone and at 5176 cm −1 due to the (ν+δ)H 2 O combination mode reflect the presence of water molecules in hydrosodalite and thermonatrite.The weaker band at 4445 cm −1 possibly arises from the combination mode of the Si-OH and Al-OH groups.

Test of Metakaolins and Alkali-Activated Metakaolins (M-28) in Water
Leaching tests are a very powerful tool to determine the degree of elements immobilization within an alkali-activated system to distilled water [44].The chemical compositions of metal elements obtained from XRF analysis were calculated to the stoichiometric metal oxides concentration in the kaolin and metakaolin samples (Table 1) and in the alkaliactivated AM-28 samples (Table 2).Figure 6 illustrates the Si, Na, Al, and K releasing from metakaolins M1, M2 and M3 (Figure 6a) and their alkali-activated products AM1-28, AM2-28, and AM3-28 (Figure 6b). Figure 6 illustrates the Si, Na, Al, and K releasing from metakaolins M1, M2 and M3 (Figure 6a) and their alkali-activated products AM1-28, AM2-28, and AM3-28 (Figure 6b) The stability of metakaolins M1 and M2 in water at higher pH 9.39 and pH 9.83, respectively, was manifested by the Si/Al ratio of 2.068 (Table 3).The slightly higher release of elements Si and Al from M3 was observed at pH 8.9 (Figure 6a) at the Si/Al ratio of 3.782 (Table 3), probably due to the bonding properties of Si-Al-O in the tetrahedra (Figure 4B).Metakaolin samples alkali-activated for 28 days exhibited good stability in water which can be documented on the leached Si/Al ratio = 0.39 of AM1-28 at pH 10.17, in comparison with the slightly higher Si/Al ratio = 0.65 of AM2-28 and AM3-28 at higher pH 10.76 and 10.95, respectively (Table 3, Figure 6b).The highest release of Na 4.98 wt.% during leaching of AM3-28 in distilled water relates to the highest Na2O content in this sample (15.28 wt.% in Table 2).Similarly, the lowest release of Na2O 2.68 wt.% from AM1-28 corresponds to the lowest content of Na2O in this sample (14.21 wt.% in Table 2).The stability of metakaolins M1 and M2 in water at higher pH 9.39 and pH 9.83, respectively, was manifested by the Si/Al ratio of 2.068 (Table 3).The slightly higher release of elements Si and Al from M3 was observed at pH 8.9 (Figure 6a) at the Si/Al ratio of 3.782 (Table 3), probably due to the bonding properties of Si-Al-O in the tetrahedra (Figure 4b).Metakaolin samples alkali-activated for 28 days exhibited good stability in water, which can be documented on the leached Si/Al ratio = 0.39 of AM1-28 at pH 10.17, in comparison with the slightly higher Si/Al ratio = 0.65 of AM2-28 and AM3-28 at higher pH 10.76 and 10.95, respectively (Table 3, Figure 6b).The highest release of Na 4.98 wt.% during leaching of AM3-28 in distilled water relates to the highest Na 2 O content in this sample (15.28 wt.% in Table 2).Similarly, the lowest release of Na 2 O 2.68 wt.% from AM1-28 corresponds to the lowest content of Na 2 O in this sample (14.21 wt.% in Table 2).

CQMA Calculations
The crystalline phases identified in XRD patterns of the kaolin samples (Figure 2a) and in the metakaolin samples (Figure 2b) were recalculated using the CQMA procedure from the elemental oxides (Table 1) using their crystallochemical formulas.The percentages of minerals in kaolin samples 1, 2 and 3 and in metakaolin samples M1, M2 and M3 (Table 4) were calculated according to Equation (2).Different amounts of metakaolinite 85.4, 70.5 and 75.0 (wt.%) produce a proportionally intensive XRD halo (Figure 2b) as well as the specific surface areas, S(BET), of 16.7, 5.2 and 11.3 (m 2 /g), respectively (Table 1).
Similarly, the bulk chemical analyses of metakaolin samples alkali-activated for 28 days (AM-28 in Table 2), mineral phases identified in XRD patterns (Figure 3) and their crystallochemical formulas were used for the calculation of a quantitative number of phases (Equation (2), Table 5).The chemistry of crystalline and metastable fragments (amorphous) of proto-zeolitic phases of zeolites Z-A (Na  NaOH reacts also with gaseous CO 2 in laboratory ambient environment to the crystalline thermonatrite, TN, (Na 2 CO 3 •H 2 O), according to Equation ( 7): The bar graph in Figure 7 proves that MK in M1, M2, M3 (left bar in Figure 7a) did not react completely with NaOH in AM1-28, AM2-28, AM3-28 and transformed to the products containing different amounts of HS, Z-A and MK Un -28 (right bar).Nevertheless, the wt.% of MK in metakaolin samples (left bar) and the sums of wt.% of MK Un -28 + Z-A + HS + TN (right bar) were in good agreement and confirmed the accuracy of the chemical reaction (Equation ( 6)).The bar graph in Figure 7 proves that MK in M1, M2, M3 (left bar in Figure 7a) did not react completely with NaOH in AM1-28, AM2-28, AM3-28 and transformed to the products containing different amounts of HS, Z-A and MKUn-28 (right bar).Nevertheless, the wt.% of MK in metakaolin samples (left bar) and the sums of wt.% of MKUn-28 + Z-A + HS + TN (right bar) were in good agreement and confirmed the accuracy of the chemical reaction (Equation ( 6)).
Regarding the quantity of accompanying minerals M, Q, and F (Figure 7b), the wt.% in MK (left bar) and in alkali-activated metakaolins AM-28 (right bar) are in good agreement, which confirms their-non-reactivity during alkaline activation.

Test of Alkali-Activated Metakaolins in Compressive Strength
In the literature, several works demonstrated the effect of alkali-activated kaolins and metakaolins on compressive strength.As an example, the fraction of reacted metakaolin varied from 2.6 to 38% for geopolymers with compressive strengths varying from 3.1 to 67 MPa [17]; kaolin-based geopolymers produced low compressive strength assigned to the unreacted material and CS increase linearly with more than 50% of metakaolinite [10]; kaolin activated with 8M NaOH for 28 days showed the highest CS value of 3.38 MPa at optimized SiO2/Na2O molar ratio of 3.58 [44]; and metakaolin calcined at 700 °C and acti- Regarding the quantity of accompanying minerals M, Q, and F (Figure 7b), the wt.% in MK (left bar) and in alkali-activated metakaolins AM-28 (right bar) are in good agreement, which confirms their-non-reactivity during alkaline activation.

Test of Alkali-Activated Metakaolins in Compressive Strength
In the literature, several works demonstrated the effect of alkali-activated kaolins and metakaolins on compressive strength.As an example, the fraction of reacted metakaolin varied from 2.6 to 38% for geopolymers with compressive strengths varying from 3.1 to 67 MPa [17]; kaolin-based geopolymers produced low compressive strength assigned to the unreacted material and CS increase linearly with more than 50% of metakaolinite [10]; kaolin activated with 8M NaOH for 28 days showed the highest CS value of 3.38 MPa at optimized SiO 2 /Na 2 O molar ratio of 3.58 [44]; and metakaolin calcined at 700 • C and activated with 8M NaOH for 28 days expressed a CS value of 5.56 MPa [45].
In alkali-activated metakaolins, metakaolinite alkali activated (MKA) to the zeolites according to Equation ( 6) can be calculated to MKA wt.% as the difference between MK wt.% in metakaolins (Table 2) and unreacted MKUn-28 wt.% in alkali-activated AM-28 (Table 4), according to Equation ( 8  The different CS MPa values of the metakaolins alkali activated for 28 days will be related to the phase composition calculated using CQMA (Figure 9).

Figure 6 .
Figure 6.Relation between the elements in distilled water leached from (a) metakaolins (M) and (b alkali activated AM-28.

Figure 6 .
Figure 6.Relation between the elements in distilled water leached from (a) metakaolins (M) and (b) alkali activated AM-28.

Table 1 .
The oxides composition of kaolin and metakaolin samples and the specific surface area, S(BET).

Table 2 .
The oxides composition of alkali-activated AM-28 samples.

Table 4 .
CQMA of minerals in kaolin and metakaolin samples.