Ion Dranca/Chem.J. Mold. 2008, 3 (1), 31-43are inherently unstable because <strong>of</strong> a strong thermodynamic drive toward crystallization. A great deal <strong>of</strong> studies hasbeen concerned with evaluating the physical stability <strong>of</strong> amorphous drugs. Most <strong>of</strong> these studies have been focusedon the dynamics <strong>of</strong> the glass transition (-relaxation), because this is the process that on its heating transforms anamorphous system from a low- to high-mobility state, in which crystallization occurs very quickly. It is known thatthe molecular mobility associated with the -relaxation fades away rapidly as the temperature drops below the glasstransition temperature, T g . Nevertheless, slow crystallization <strong>of</strong> indomethacin has been reported by several workers[39, 40] at temperature as low as 20 o C, which is about 25 o C below the respective T g value. On the other hand,relaxation in amorphous indomethacin is still detectable as much as 47 o C below T g [41]. It seems to be generallythought that at temperature 50 o C below T g , the molecular mobility should be too negligible to cause any significantrelaxation and, therefore, crystallization. This is certainly true for the -relaxation that requires a cooperative motion<strong>of</strong> multiple molecules and therefore has a huge energy to it. However, local noncooperative motion has a significantlysmaller energy barrier and continues to occur at lower temperatures, giving rise to the -process [46]. Although the-relaxations (Fig. 1) had been well known for polymers, Johari and Goldstein [42] discovered similar processes insimple inorganic glasses, and suggested these to be universal feature <strong>of</strong> the glassy state.1.3 Glucose (Gl) and Maltitol (Mt). Sugar and sugar alcohols find a wide application in various pharmaceuticalsystems as sweeteners and/or binding matrices for drug components. As such they are frequently used in the glassy state,which is thermodynamically unstable and unavoidably tends to relax toward the liquid state [43]. Understanding thedynamics <strong>of</strong> this process is <strong>of</strong> a great practical importance for designing physically stable formulations <strong>of</strong> amorphousdrugs.In this work, we apply DSC to measure the -relaxation in a PS-clay system, in virgin PS, in amorphousindomethacin, and also in amorphous glucose and maltitol. The objective <strong>of</strong> this study is to obtain comparative informationon the relaxation dynamics <strong>of</strong> these systems by estimating the effective activation energies <strong>of</strong> the relaxation as well asthe sizes <strong>of</strong> cooperatively rearranging regions at the glass transition. This paper is intended to initiate systematic kineticstudies <strong>of</strong> polymer nanocomposites and pharmaceutic materials, therefore, to fill the presently existing void in theunderstanding <strong>of</strong> the thermal behavior <strong>of</strong> these exciting materials.Experimental SectionA sample <strong>of</strong> the PS-clay composite was provided by Dr. Xiaowu Fan (Northwestern University). The compositewas prepared by intercalating a monocationic free radical initiator into montmorillonite clay and the subsequentsolution surface-initiated polymerization (SIP), where the chain growth was initiated in situ from clay surfaces. Themontmorillonite clay was Cloisite ® Na + (Southern Clay Product Inc.) with the cation exchange capacity 92 mequiv per100g and the specific surface area 750 m 2 g -1 . The initiator was an azobisisobutyronitrile (AIBN)-analogue moleculewith a quaternized amine group at one end. The intercalation process was realized by cation exchange reaction in whichthe cationic end <strong>of</strong> the initiator was ionically attached to the negatively charged clay surfaces. The details regarding thepreparation and characterization <strong>of</strong> the intercalated clay can be found elsewhere [44]. The subsequent SIP was performedin THF solvent with styrene as the monomer, resulting in a PS-clay nanocomposite by the in situ polymerization. Details<strong>of</strong> the initiator synthesis, the SIP process and product analysis can be found in previous publication, which shows thatthis free radical SIP strategy can achieve exfoliated PS-clay nanocomposites <strong>of</strong> high clay loading. According to ourpervious TGA [45] measurements the resulting composite contains about 1% <strong>of</strong> clay by weight. The molecular weight(~90,000) and polydispersity (~2.3) <strong>of</strong> the product were measured by size exclusion chromatography (SEC) usingPS standards. The obtained material will be referred to as nPS90. For comparison purposes, we have used radicallypolymerized PS that was purchased from Alfa Aesar and used as received. Its Mw value is 100,000 (polydispersity isaround 2.1) and it will be referred to as PS100.The -relaxation measurements were performed on ~10 mg samples placed in 40L Al pans. The glass transitionwas measured by heating a sample ~40°C above its glass transition temperature and holding it at this temperature for 10min to erase thermal history. The samples were then cooled down to ~40°C below the glass transition temperature at therates form 5, 7.5, 10, 12.5, 15, 17.5, 20, 22.5 and 25 °C min -1 . Immediately after completion <strong>of</strong> the cooling segment, thesamples were heated at a rate whose absolute value was equal to the rate <strong>of</strong> preceding cooling. TGA data [45] indicatethat no detectable degradation <strong>of</strong> PS100 and nPS90 occurs in air below 240°C.Indomethacin(1-(p-chlorobenzoil)-5-methoxy-2-methylindole-3-acetic acid) was obtained from MP Biomedicals,LLC (catalogue number 190217, lot number 9331E), with a melting point at 160oC obtained by DSC, and it was usedwithout further purification.The -relaxation measurements were performed on ~10.0 mg samples placed in 40L Al sealed pans withoutholes. TGA data [46] indicate that no detectable degradation <strong>of</strong> Indomethacin occurs in air atmosphere below 180°C.The glass transition was measured by heating a sample ~40°C above its glass transition temperature (90 o C) and holdingit at this temperature for 10 min to erase thermal history. The samples were then cooled down to ~40°C below the glasstransition temperature (-10 o C) at the rates form (10, 15, 20, 25 and 30°C min -1 ). Immediately after completion <strong>of</strong> the33
Ion Dranca/Chem.J. Mold. 2008, 3 (1), 31-43cooling segment, the samples were heated at a rate whose absolute value was equal to the rate <strong>of</strong> preceding cooling. Theheat capacity was measured on ~27 mg sample by using a standard procedure that is precise to 1%. A sapphire sample<strong>of</strong> 41.48 mg was used as the calibrant. The temperature program used for the heat capacity measurement involved 5min isothermal hold at 0C followed by heating at 10C min -1 to 90C and another 5 min isothermal hold at the finaltemperature.Anhydrous glucose (Dextrose) and maltitol were, respectively, purchased from Fisher and MP Biomedicals andused without purification. In order to produce amorphous (glassy) samples, ~15 mg <strong>of</strong> samples was placed in 40 lclosed Al pans and heated to ~10 o C above their respective melting points, 161 o C (glucose) and 149 o C (maltitol). Shortlyafter heating the samples were quenched into liquid nitrogen. The glass transition temperatures <strong>of</strong> amorphous sampleswere estimated as midpoint temperatures <strong>of</strong> the DSC glass transition steps measured at 10 o C min -1 .Sub-T gmeasurements, freshly quenched samples were quickly placed into the DSC cell that was maintained at-40 o C . From -40 o C the samples were heated to an annealing temperature, T a, and held at it for 30 min. After completion<strong>of</strong> the annealing segment, the samples were cooled down to -40 o C and immediately heated above T g. The heating rateswere 15, 20, 25, and 30 o C min -1 .All the aforementioned measurements we conducted by using a Mettler-Toledo heat flux DSC 822e in theatmosphere <strong>of</strong> nitrogen flow (80 ml min -1 ) at University <strong>of</strong> Alabama, USA. The temperature and heat flow calibrationwere performed by using an Indium standard.Results and DiscussionGlass transition or -relaxation in PS100 and nPS90. DSC data for both materials demonstrate (Fig. 1) typicalglass transition steps, the midpoint <strong>of</strong> which has been used as an estimate <strong>of</strong> the T gvalue. It is seen that in nPS90 theglass transition occurs at about 10 o C greater temperature than PS100.-2.0PS100nPS90Heat flow / mW-2.5-3.0Exo-40 60 80 100 120 140Fig. 2. DSC curves for the glass transition (-relaxation) in PS100 and nPS90 measured at 10 o C min -1The values <strong>of</strong> T ghave been determined at nine heating rates (two times at each heating rate). The heating ratedependence <strong>of</strong> Tg can be used to evaluate the effective activation energy <strong>of</strong> the glass transition from eq 1.T / o Cd ln E R(2)dT gln( / o C min -1 )3.53.02.52.0305 kJ mol -1PS100nPS90201 kJ mol -11.50.0026 0.0027T -1 /K -1Fig. 3. Evaluating activation energies (eq 2) for -relaxation in PS100 and nPS90 as proposed byMoynihan et al. [6, 47]34
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