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Advances in Materials Science and Engineering
Volume 2013 (2013), Article ID 763838, 11 pages
Characterisation and Properties of Lithium Disilicate Glass Ceramics in the SiO2-Li2O-K2O-Al2O3 System for Dental Applications
National Metal and Materials Technology Center, 114 Thailand Science Park, Pathumthani 12120, Thailand
Received 29 April 2013; Revised 25 June 2013; Accepted 28 June 2013
Academic Editor: Delia Brauer
Copyright © 2013 Naruporn Monmaturapoj 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.
This work proposes four different glass formulas derived from the SiO2-Li2O-K2O-Al2O3 system to investigate the effect of glass composition on their crystal formations and properties. Glass LD1 was SiO2-Li2O-K2O-Al2O3 system with the addition of P2O5 and CaF2 as nucleating agents. In Glass LD2, a slight amount of MgO was mixed in order to increase the viscosity of the melting glass. Finally, the important factor of Si : Li ratio was increased in Glasses LD3 and LD4 with compositions otherwise the same as LD1 and LD2. The results found that P2O5 and CaF2 served as a nucleating site for lithium phosphate and fluorapatite to encourage heterogenous nucleation and produce a fine-grained interlocking microstructure of lithium disilicate glass ceramics. MgO content in this system seemed to increase the viscosity of the melting glass and thermal expansion coefficient including the chemical solubility. Increasing the Si : Li ratio in glass compositions resulted in the change of the microstructure of Li2Si2O5 crystals.
All-ceramic systems for dental restoration have been extensively used over recent years due to substantial developments meeting dental requirements, particularly in terms of their mechanical properties and the opaque, presently accessible appearance of all-ceramic materials . Lithium disilicate glass ceramic (Li2Si2O5) is one such all-ceramic system, currently used in the fabrication of single and multiunit dental restorations mainly for dental crowns, bridges, and veneers because of its color being similar to natural teeth and its excellent mechanical properties .
In general, glass ceramics can be produced by melting glass and converting the substance into a uniform nucleation and growth of fine-grained ceramics by controlled crystallization process, in which the crystalline phases are nucleated and grown in glass via heat treatment [3–5]. Lithium disilicate glass ceramic, in particular the Li2O-SiO2 system, is the first material classified as glass ceramic discovered by Stookey as having better mechanical properties over base glass . Since then, many comprehensive studies have paid attention to the binary Li2O-SiO2 system [7–13]. However, this binary system lacks chemical durability for use as a restorative material in dentistry. Therefore, nonstoichiometric compositions or multicomponent glass ceramics were carried out to improve the chemical durability, especially the addition of Al2O3 and K2O to the stoichiometric composition reported to enhance the chemical durability of this glass ceramic [14–16]. Several constituents, for example, ZnO, ZrO2, CaO, and P2O5, were introduced to improve the properties of the final material [4, 17–20]. Also, it is noted that P2O5 as a nucleating agent plays an important role in phase formation and crystallization for lithium disilicate glass ceramic [16, 21, 22]. For that reason, a slight P2O5 content in glass composition could produce a fine-grained interlocking microstructure resulting in high mechanical strength .
Fluorine in glass affect its crystallization mechanism and the phases formation due to the fact that fluorine is a network modifier which could rearrange the glass network by forming nonbridging fluorine to replace nonbridging oxygens . Fluorine in calcium phosphate glasses produces a fluorapatite phase which has less solubility characteristics; therefore, it could improve the chemical solubility of the glass ceramic . In addition, Beall  and Echeverria and Beall  suggested that the SiO2 : Li2O ratio is also a key success factor in the formation of the main crystal phase in a new lithium disilicate glass ceramic system. In order to optimize the viscous properties of lithium disilicate glass to have better pressing ability, components such as La2O3 and MgO were added to the main composition [25, 26].
In fact, studies of lithium disilicate glass ceramics have focused mainly on the phase formation and crystallization of Li2Si2O5, as affected by variations of temperature during the heat treatment cycle and of minor compositional changes in the main glass composition. These factors influence the microstructure of the glass ceramic and consequently affect the properties of the final products.
In this study, four different glass formulas derived from the SiO2-Li2O-K2O-Al2O3 system were prepared to investigate the effect of glass compositions on their crystal formations, microstructures, and properties through the conventional glass melting process. P2O5 and CaF2 as nucleating agents were introduced to induce heterogeneous nucleation and then produce a fine-grained interlocking microstructure after heat treatment. MgO was added in the glass system to increase the viscous properties, and, finally, the SiO2 : Li2O ratio in the glass composition was increased. The experimental results and their discussion are addressed as concerns the crystallization behavior of the glasses, the microstructures, and properties of the glass ceramics with the potential to be used as dental restorations.
2. Materials and Methods
2.1. Glass Preparation
Glass batches were prepared by mixing appropriate amounts of SiO2, Li2CO3, MgCO3 (Sigma-Aldrich Company, Belgium), Al2O3 (Fluka Analytical, Germany), P2O5 (Acros organics, USA), K2CO3 (Fluka chemika, France), and CaF2 (Merck chemicals, Germany). All starting materials were reagent grade. Glass batches according to glass compositions as shown in Table 1 were melted in a covered Pt-10%Rh crucible at 1500°C for 2 hrs and then quenched in cold water to make frit. To achieve homogeneity, glass frit was milled before being remelted at the same temperature for 2 hrs. The melting glass was cast into warm graphite molds to obtain glass rods with a dimension of 14 mm in diameter × 100 mm long. Graphite molds were annealed in a muffle furnace at 400–500°C for 2 hrs to reduce the internal stress in the glasses followed by cooling to room temperature at 1°C/min.
2.2. Heat Treatment
Samples were cut into several disks of 14 mm × 5 mm long and then heat-treated in a Lenton furnace (Lenton Ltd., Hope Valley, UK). A two-stage heat-treatment schedule was performed in which the glasses were heated to a nucleating temperature of 500°C with a heating rate of 5°C/min, held for 2 hrs, and then ramped up to various crystal growth temperatures (e.g., 700°C). The heating rate was 5°C/min, and samples were held for 2 hrs followed by furnace cooling with 5°C/min to room temperature. Following heat treatment, samples were referred to as glass ceramics LD1–LD4.
2.3. Thermal Analysis
2.3.1. Differential Thermal Analysis
A Netzsch thermal analysis (NETZSCH STA 449 F3, Germany) was used to determine and by heating to 1000°C with a heating rate of 10°C/min. Fine glass samples (6–10 μm) were analyzed under flowing nitrogen with a Pt crucible filled with alumina as reference and then heated together at the set up heating rate. The results were used as a guide for determining the heat treatment temperatures applied to induce crystallization.
2.3.2. Thermal Expansion Measurement
The coefficient of thermal expansion using a Netzsch thermal analysis (NETZSCH DIL 402 PC, Germany) dilatometer with a heating rate of 5°C/min was applied on the glass ceramic bars (5 mm × 5 mm × 25 mm) measuring from room temperature up to 600°C. The linear thermal expansion coefficient () was calculated using the general equation: , where () is the increase in length, () is the temperature interval over which the sample is heated, and () is the original length of the specimen.
2.4. X-Ray Diffraction Analysis
Phase analyses of the glasses and glass ceramics were performed by X-ray diffraction (XRD, Rigaku TTRAX III) operating from 10° to 70° 2θ at a scan speed of 2° 2θ/min and a step size of 0.02° 2θ with Cu radiation ( nm) at 300 mA and 50 kV. Identification of phases was achieved by comparing the result diffraction patterns with the ICDD (JCPDS) standard.
2.5. Scanning Electron Microscopy
Microstructure of the glass ceramics was investigated by scanning electron microscope (SEM: Hitachi S-3400N). After heat treatment, the samples were polished with SiC paper (nos. 400, 800, 1000, 1200, and 2500) and finally with diamond paste (sizes 6, 3, and 1 μm). Then, the samples were edged by chemical etching process with hydrofluoric acid (4% vol) for 1 minute and cleaned afterwards with a high-frequency vibration. The samples were coated with gold by ion sputtering device (JEOL JFC-1200) at a current generation of 15 mA for 200 seconds.
2.6. Mechanical Properties Testing
2.6.1. Indentation Fracture Toughness (IFT)
Glass specimens (∅14 mm × 5 mm) were initially cut from the glass rod with a diamond saw blade machine (IsoMet 4000, Buehler, Ltd., USA) to create parallel faces. After heat treatment, they were polished down using SiC paper and finally with diamond paste. Indentations were obtained using Vickers hardness testing machine (Vickers-Armstrong, Ltd., Crayford, UK) for loads of 1 kg, 2 kg, 3 kg, 5 kg, and 7.5 kg. The used loads were restricted to a range over which the indentation patterns remained well defined, at the lower end by the minimum requirement , where is the radial crack length and is the indentation half-diagonal length, and at the upper end by chipping or by the limitation of specimen thickness. For each load, at least 15–20 indentations were made, and at least ten to fifteen readings were taken using an optical microscopy (ZEISS Model Axiotech) equipped with a digital camera and computer. Fracture toughness was calculated using the formula P/C3/2, where is indentation fracture toughness (IFT), is the indentation load, and is the radial crack size.
2.6.2. Biaxial Flexural Strength
Glass specimens (∅14 mm × 4 mm) were cut from the glass rods to obtain at least six disks. After two-stage heat treatment, they were ground and polished using SiC paper and diamond paste. Test geometry of three-ball supported test-jig equipped with a universal testing machine (Model 8872, Instron Instruments, Ltd., Fareham, Hampshire, UK) with a ring support of 10 mm at a cross-head speed of 1 mm/min was performed on the samples (Figure 1). A sheet of paper was placed between the samples and support ring to eliminate any additional flatness and reduce friction . The center of each disk was marked as the correct place for the loading ball before testing. The maximum stress, at the center was calculated applying the following equation : where is load, is disk thickness, is the radius of the circle of the support ring, is the radius of the region of uniform loading at the center , is the radius of the disk sample, and is Poisson’s ratio, .
2.7. Chemical Solubility Testing
After two-stage heat treatment, the glass specimens (∅14 mm × 2 mm) were polished to create parallel faces. Glass ceramic specimens were washed and dried at 150°C for 4 hrs followed by being weighed to the nearest 0.1 mg (). The total surface area of the specimens was determined to the nearest 0.1 cm2. Specimens were then individually immersed in a 250 mL glass bottle with 100 mL acetic acid, 4% solution in water. The bottles were closed with their caps and then placed in an oven at 80°C for 16 hrs. Next, the specimens were washed and dried at 150°C for 4 hrs to achieve a constant mass. Finally, the specimens were reweighed to obtain the mass after immersion (). The chemical solubility was determined by the following equation: The chemical solubility test method in this study was referred to the ISO 6872 .
3. Results and Discussion
3.1. Differential Thermal Analysis
The DTA traces for glasses LD1–LD4 in Figure 2 and the summary of the exothermic and endothermic peaks in Table 2 show the exothermic and endothermic anomalies for all glasses attributed to either the glass transition () or crystallization temperatures ().
The DTA traces of Glass LD1 exhibited triple exothermic peaks at 650°C, 860°C, and 910°C. A similar trend of three crystallization peaks at 650°C, 860°C, and 910°C was observed in Glass LD2. The study by Schweiger et al.  reported that the first crystallization of SiO2-Li2O system founds at 589°C corresponding to Li2SiO3 and the second crystallization peak at 770°C associated to Li2Si2O5. The first and second crystallization temperatures of Li2O-Al2O3-SiO2 system in this study were at a higher temperature than the stoichiometric composition. This might be because of the addition of P2O5 and CaF2 into glass compositions. Then, the third exothermic peak was observed. The addition of the MgO may not result in any significant changes in the and of the Glasses LD1 and LD2.
In Glass LD3, s were observed at 650°C and 910°C. Two exothermic peaks associated with the crystallization temperatures were observed by increasing the Si : Li ratio in LD3. Differently, in Glass LD4, three exothermic peaks were observed: firstly, a small peak at about 650°C and two broadening peaks at 770°C and 885°C. It seems that the second crystallization temperature decreased to 770°C in this composition. The addition of MgO in LD4 was behind the decrease of the second crystallization down to a lower temperature than that of LD1 and LD2 which had lower SiO2 : Li2O ratios. Moreover, the crystallization of fluorapatite, Li3PO4, and aluminosilicate is the minor crystallization in the system, so that it is difficult to identify the exothermic peaks related to these minor phases.
3.2. The Coefficient of Thermal Expansion
Figure 3 presents the changes in thermal expansion coefficients of glass ceramics as a function of heat treatment temperatures. The coefficients of thermal expansion for LD1–LD4 decreased with increasing heat treatment temperature in all glass ceramic samples except LD2, of which the thermal expansion coefficient rose following heat treatment at 850°C.
The increasing in thermal expansion coefficient value of LD2 after heat treatment at 850°C was possibly due to the addition of MgO. It is well known that MgO is not a glass former; therefore, the addition of MgO causes a weakening of the glass network structure and, consequently, a higher coefficient of thermal expansion . Even though MgO was also added in LD4, the thermal expansion coefficient of LD4 after heat treatment at 850°C was decreased. The possible reason to explain this phenomenon is the different in SiO2 : Li2O ratio. The SiO2 : Li2O ratio of LD4 was 2.21, which was higher than that of LD2 (1.90).
In general, the thermal expansion coefficients of the glass ceramics mainly depend on the crystalline phases present at different temperatures and volume content in the matrix glass. Not only crystal types affect the thermal expansion coefficient but also the glass composition which is related to the structure of the glass . The different crystal types have different thermal expansion coefficients . The explanation behind the high thermal expansion coefficient of all glass ceramics in this study is the presence of several crystalline phases such as fluorapatite (10.0 × 10−6/°C ), lithium phosphate, lithium metasilicate (13.0 × 10−6/°C ) and lithium disilicate (11.4 × 10−6/°C ), which have a high thermal expansion coefficient in the glass composition. The decrease of the thermal expansion coefficient as the temperature rise can be explained by the -quartz solid solution changes into lithium aluminium silicate: virgilite (a stuffed -quartz), having a low or negative thermal expansion coefficient with the temperature increasing .
3.3. Summary of the Phase Evolution
Figure 4 shows XRD patterns of all glass ceramics heat treated at 700–850°C for 2 hrs, and the crystalline phases are summarized in Table 3. The crystal structures found in LD1 heat treated at 700°C were lithium disilicate (LD, Li2Si2O5: ICDD no. 40-0376), lithium metasilicate (LS, Li2SiO3: ICDD no. 29-0829), lithium aluminium silicate (virgilite, Li0.6Al0.6Si2.4O6: ICDD no. 21-0503 and spodumene (LiAlSi2O6: ICDD no. 033-0786), fluorapatite (Ca5(PO4)3F: ICDD no. 15-0876), lithium phosphate (Li3PO4: 015-0760), and SiO2: high quartz (2θ = 20.26°, ICDD no. 11-0252). At higher temperatures, the intensity of LS and virgilite peaks decreased while the intensity of lithium disilicate peaks increased. This exhibited higher in lithium disilicate crystallization. In addition, the peaks of -quartz decreased until disappeared when heat treated at 850°C.
A similar phase formation was also observed in LD2 with the addition of MgO. The small discrepancy was the crystal peaks associated to -quartz solid solution (2 = 26.26°) when heat treatment at 700°C transformed into virgilite (2 = 25.88°) after heat treatment at 750°C. And this phase remained when heat treatment was at 800°C and 850°C.
Generally, the -quartz could be stabilized by Li+ or Mg2+, Zn+, and Al3+ called quartz-solid-solution which normally does not transform into the low-quartz-solid-solution while cooling down to room temperature resulting of a small thermal expansion coefficient . Meanwhile, virgilite is the naturally occurring representative of the solid-solution series between -quartz and LiAlSi2O6 with a stuffed -quartz structure . However, the possible explanation of the virgilite formation in laboratory experiment was that the sluggish reaction rates in the system Li2O-Al2O3-SiO2 require high pressure and temperature. Then reaction rate could be increased by the presence of Fe, alkalis, and volatiles, thus promoting the formation of virgilite at lower pressure within its stability field .
Figure 4(c) presents XRD pattern of LD3 heat treatment at different temperatures. By increasing the SiO2 : Li2O ratio, in the glass composition, phase separation occurred due to the white and semiopaque appearance observed in LD3. Therefore, the crystal structures found in the as-cast glass were Li3PO4. At 700°C, XRD patterns showed the phase formation of Li2SiO3, lithium aluminium silicate, Li2Si2O5, Ca5(PO4)3F, and SiO2: high quartz. The small peaks of Li3PO4 decreased when heat treated at higher temperatures. With increasing temperature, the intensity of Li2Si2O5 increased as well as the retention of Li2SiO3, lithium aluminium silicate (virgilite), and Ca5(PO4)3F. By increasing the SiO2 : Li2O ratio, the more lithium aluminium silicate crystal peaks were observed compared to LD1 which has low SiO2 : Li2O ratio.
The phase formation of LD4 is presented in Figure 4(d). The as-cast glass appearance looks clearer than that of LD3, implying that no phase separation occurred in this glass. At 700°C, the peaks corresponded to Li2SiO3, Li3PO4, Li2Si2O5, Ca5(PO4)3F, lithium aluminium silicate, and SiO2 in the form of the high quartz observed. Then after heat treatment at higher temperature, the crystal peaks associated to -quartz solid solution (2 = 26.26°) when heat-treated at 700°C transformed into virgilite (2 = 25.88°) after heat treatment at 750°C; this is similar to LD2. The difference from LD2 was the number of Li2SiO3 peaks observed in LD4 wich was less than that in LD2.
The growth of lithium disilicate could be initiated by the primary crystallization of the precursor lithium metasilicate, in particular, lithium disilicate glass ceramic containing Al2O3 . Glass ceramic containing P2O5 may be nucleated by the initiation of the phase separation process, such as Li3PO4 nuclei [4, 37, 38]. P2O5 can react with Li2O in Li2O-rich regions to form the Li3PO4 crystal nuclei which act as nucleating sites shown in reaction(3). Some Li2O was consumed in the Li2O-rich regions to form Li3PO4 phase (reaction (3)) which can induce the precipitation of Li2SiO3 crystal (reaction(4)). It is reasonable to assume that Li2SiO3 precipitated on the Li3PO4 crystal nuclei in Li-rich regions, and the growth of Li2Si2O5 was at the expense of consuming Li2SiO3 as shown in reaction (5)
Therefore, the sequence of the primary crystal phase formation as Li3PO4, Li2SiO3, and Li2Si2O5 was proposed . On the other hand, the investigation on complex simultaneous and sequential solid-state reactions in an Al2O3-free lithium disilicate glass ceramic found that Li3PO4 crystals were formed after the crystallization of Li2SiO3 and Li2Si2O5 . Hence, they  concluded that Li3PO4 does not nucleate lithium disilicate crystals, as previously studied for the glasses of similar composition .
However, in this case a different early phase formation was observed. Due to CaF2 added in this system, the peaks were associated with the crystal of fluorapatite indexed in the XRD pattern in parallel with Li3PO4. Subsequently, at an early stage, the incorporation of fluorine in phosphate glasses leads to P-F bonds at the expense of P-O-P bonds to possibly form fluorapatite: Ca5(PO4)3F crystals . Therefore, it is reasonable to conclude that the formation of Li2Si2O5 crystals in this case occurred from the heterogeneous nucleation of Li3PO4 and Ca5(PO4)3F caused from the addition of CaF2 and P2O5 in glass compositions. Hence, P2O5 also act as a nucleating agent in this system.
Furthermore, the investigation on spodumene, Li2O·Al2O3·4SiO2 glass ceramics adding ZrO2 suggested that Al2O3 content should not exceed 30% wt to achieve a low coefficient of thermal expansion and highly thermal shock resistant , as a result of detritions of mechanical strength . In this study only 2% wt of Al2O3 was added in the glass compositions, in the range to produce a low thermal expansion coefficient glass ceramic.
The morphology of the system was studied, and SEM micrographs of the sample surfaces are shown in Figure 5. At 700°C, SEM images of glass ceramic LD1 illustrate the spherical-like crystals of both Li2SiO3 and Li3PO4. Normally, Li2SiO3 and Li3PO4 crystals could dissolve in HF solution if one-stage treatment applied due to the precipitate crystals was not stable . In this study, two-stage treatment was applied, thus, Li2SiO3 and Li3PO4 crystals could be seen by SEM consistent with XRD pattern which indicated the formation of both crystals. XRD patterns also indicated the formation of the lithium aluminium silicate: virgilite and fluorapatite crystals. Both crystals have a rounded or spherical-like shape similar to Li2SiO3 and Li3PO4 but smaller in size, which is hardly to find by either SEM technique or energy dispersive spectroscopy (EDS) . Transmission electron microscopy could be a better technique to show these spherical shapes of the virgilite and fluorapatite crystals [42, 43].
After heat treatment at 800°C, several lath-like crystals of lithium disilicate were observed. With increasing heat treatment temperature, the more and the coarser the lath-like crystals occurred, in close consistency with XRD results. A similar microstructure was also observed in LD2. A small discrepancy appeared at 750°C for LD2 in which no lath-like crystal of Li2Si2O5 was noticed but the lath-like crystals can be observed in samples after heat treatment at 800°C and 850°C.
SEM images of LD3 and LD4 shown in Figures 5(c) and 5(d) reveal that the spherical-shaped crystals of both Li2SiO3 and Li3PO4 occurred at 700°C and 750°C followed by the appearance of needle-like crystals or plate-like crystals of Li2Si2O5 in a glassy matrix at 800°C and 850°C. This needle-like crystal looked very long with a narrow diameter. The higher the temperature of heat treatment, the larger the aspect ratio and greater interlocking of the needle-like crystal was observed. The increase in the Si : Li ratio in LD3 and LD4 compositions seems to have induced the change in the microstructure of the Li2Si2O5 crystal from the fine lath-like crystal to the needle-like or plate-like crystal. The addition of a slight amount of MgO content in glass composition showed no significant changes in the microstructure of the glass ceramics. This phenomenon was also observed in LD1 and LD2.
3.5. Mechanical Properties
3.5.1. Indentation Fracture Toughness (IFT)
The IFT values of the glass ceramics LD1–LD4 at different temperatures are shown in Figure 6. The highest IFT for all samples was obtained at 800°C with glass ceramics LD1, LD2, and LD4, , , and MPa m1/2, respectively, which suggests that this heat-treatment temperature is close to the optimum, probably caused by the finer and more highly interlocked crystals. Of exceptional note was that the highest IFT value of LD3, MPa m1/2 was found in samples at a heat treatment of 850°C at which a finer microstructure with a high aspect ratio might be occurring. It was reported that the finer the microstructure, the more twisted the path for fracture and, therefore, the higher the fracture toughness . Consequently, LD1, LD2, and LD4 at 850°C and LD3 at 800°C, which illustrated a coarser microstructure, obtained lower IFT values. As shown in (Figure 4(c)), XRD pattern of LD3 indicated the more numbers of lithium aluminium silicate: virgilite crystals with a high intensity compared to that of other glasses, particularly at 800°C and 850°C. Therefore, the thermal expansion mismatch between Li2Si2O5 and virgilite resulted in residual stresses or microcracks on cooling, which create crack tip shielding and enhanced toughness of LD3 at 800C° and 850°C.
3.5.2. Biaxial Flexural Strength (BFS)
Figure 7 presents the BFS values of the glass ceramics LD1-LD4 at different temperatures. For LD1, the BFS was at its maximum ( MPa) at 750°C which didnot significantly decrease after heat treatment at 800°C ( MPa) followed by drastical change to MPa at 850°C. In LD2, the maximum BFS was MPa at 800°C which increased from MPa at 750°C followed by a decrease to MPa at 850°C. In LD3, an increase in BFS was observed from MPa in samples heat-treated at 750°C to MPa at 800°C followed by a decrease to MPa at 850°C. For LD4, the maximum BFS was MPa at 800°C which sharply increased from MPa at 750°C followed by a decrease to MPa at 850°C. Overall, the highest BFS of the studied glass ceramics was found at 800°C in which a finer microstructure was noted. Another reason is that the thermal expansion mismatch between lithium disilicate and other phases, including glass matrix, probably caused tangential compressive stresses around the crystals, which was responsible for crack deflection and enhanced strength .
Irwin, as with Griffith approach, introduced stress intensity factors as a quantitative indicator on the effect of dimension and shape  on the magnitude of the stresses near a crack tip . This is expressed in a general formula for an infinite plate with crack length = at its center, where is the nominal stress or biaxial flexural strength, is the fracture toughness, and is the flaw size.
With this formula, it is possible to find the correlation between strength and the stress field (fracture toughness) in the terms of a critical flaw size, as shown in Table 4 since both strength and fracture toughness are known. It is worth noting that Mencik  and Green  suggested that if the crack length or flaw size is smaller than the pore or crystal size, a high but low strength value may occur. This could explain the situation of the high fracture toughness but low in strength of LD3 at 800°C and 850°C due to the largest critical flaw size (~102 μm for 800°C and ~197 μm for 850°C) which was found in these samples.
3.6. Chemical Solubility
Chemical solubility is an important property for dental restoration since a high solubility or low resistance to erosion will strictly limit the effective lifetime of the restoration. Moreover, the chemical solubility property also directly affects the strength of the glass ceramic material. Figure 8 shows the chemical solubility value of all glass ceramics at different temperatures. It was found that the chemical solubility of all glass ceramics slightly decreased with increasing temperature, except that of LD2 which had MgO content. The addition of alkaline earth such as CaO and MgO in glass composition could increase chemical solubility in glass ceramics owing to the increased volume of crystalline phase . Considerably, the microstructure of LD2 at 850°C (Figure 5(d)) shows a high aspect ratio of needle-like crystals which are loosely interlocking compared to other glasses. This kind of microstructure might be easy for the acid to attack on the surface of the sample. Therefore, the microstructure could also be responsible for high chemical solubility of LD2.
In fact, the chemical solubility of the core ceramic materials must be less than 2000 μg/cm2, and that of the body ceramic materials directly in contact with the oral environment should be less than 100 μg/cm2 according to ISO 6872 . Generally, the chemical solubility of the glass ceramic in this study was in the acceptable range according to ISO 6872 for core ceramic material. The lowest chemical durability was LD4, at ~28 μg/cm2, heat-treated at 800°C.
All glass ceramics were identified by X–ray diffraction method, and it was found that P2O5 and CaF2 served as a nucleating site for lithium phosphate, Li3PO4, and fluorapatite, Ca5(PO4)3F, to induce heterogeneous nucleation and then produce a fine-grained interlocking microstructure of lithium disilicate glass ceramics. MgO content in this system seems to have played less of a role in changing the phase formation and microstructure of the glasses but enhanced the viscosity of the melting glass and thermal expansion coefficient including the chemical solubility. The increase in the Si : Li ratio in glass compositions resulted from the change in the microstructure of Li2Si2O5 crystal from fine lath-like crystals to needle-like or plate-like crystals. In this study, LD3 heat-treated at 850°C exhibited the best fracture toughness of ~8 MPa m1/2. In addition, LD4 heat-treated at 800°C had the best biaxial flexural strength and chemical solubility of ~490 MPa and ~28 μg/cm2, respectively. These glass compositions are promising for potential use as dental crowns.
Conflict of Interests
There is no financial or other relationship that might be perceived as leading to a conflict of interests. The authors declare that there is no conflict of interests.
This work was performed with support from the National Metal and Materials Technology Center, Ministry of Science and Technology of Thailand, under Project no. 1100057.
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