MULTIVALENCE CERIUM OXIDE NANOPARTICLES IN SOLUBLE BORATE GLASS MATRICES FOR TARGETED RELEASE

Abstract

A composition comprising glass containing both trivalent cerium oxide and tetravalent cerium oxide states nano particles. A soluble sodium borate glass comprising cerium oxide that is stable against crystallizations, the cerium oxide comprising both trivalent Ce.sup.3+ (Ce.sub.2O.sub.3) and tetravalent Ce.sup.4+ (CeO.sub.2) states, wherein the cerium oxide nano particles are configured to be released when the glass is dissolved.

Claims

1.-20. (canceled)

21. A method of forming a composition comprising glass containing both trivalent cerium oxide and tetravalent cerium oxide states nanoparticles, the method comprising: heating a raw material comprising CeO.sub.2 to a temperature above the melting point of the raw material, wherein the temperature is between 1100° C. and 1300° C., including the end points; maintaining the temperature for a specified amount of time; and cooling the melted raw material to form the glass, wherein the glass contains a ratio of the trivalent cerium oxide and tetravalent cerium oxide states nanoparticles that is controlled and sealed within the glass.

22. The method of claim 21, wherein the raw material comprises 0.01 to 0.09 mol % CeO.sub.2.

23. The method of claim 21, wherein the glass comprises a sodium borate glass.

24. The method of claim 21, wherein the nanoparticles each have a size between 2 and 5 nm.

25. The method claim 21, wherein the raw material comprises CePO.sub.4 or Ce(NO.sub.3).sub.3, or a combination thereof.

26. The method of claim 21, wherein the temperature is between 1200° C. and 1300° C., including the end points.

27. The method of claim 21, wherein the temperature is maintained for between 1 and 24 hours, including the end points.

28. The method of claim 21, wherein the temperature is 400-600° C. above the melting point of the raw material.

29. The method of claim 21, further comprising adding reducing agents to increase Ce.sup.3+ or adding oxidizing chemicals to reduce Ce.sup.3+.

30. The method of claim 21, wherein cerium oxide nanoparticles are configured to be released when the glass is dissolved.

31. A method of forming a soluble sodium borate glass comprising cerium oxide nanoparticles that is stable against crystallizations, the cerium oxide comprising both trivalent Ce.sup.3+ (Ce.sub.2O.sub.3) nanoparticles and tetravalent Ce.sup.4+ (CeO.sub.2) nanoparticles, the method comprising: modulating one or more synthesis parameters of the soluble sodium borate glass to achieve a controlled ratio of the trivalent Ce.sup.3+ (Ce.sub.2O.sub.3) and the tetravalent Ce.sup.4+ (CeO.sub.2) nanoparticles by: melting a raw material at a temperature; maintaining the temperature for a specified amount of time; and cooling the melted raw material to form the soluble sodium borate glass.

32. The method of claim 31, wherein cerium oxide nanoparticles are configured to be released when the glass is dissolved.

33. The method of claim 31, further comprising doping the sodium borate glass with Ce.sub.2O to produce the trivalent Ce.sup.3+ (Ce.sub.2O.sub.3) nanoparticles and tetravalent Ce.sup.4+ (CeO.sub.2) nanoparticles.

34. The method of claim 31, wherein the nanoparticles each have a size between 2 and 5 nm.

35. The method of claim 31, wherein the glass is formed from a raw material comprising 0.01 to 0.09 mol % CeO.sub.2.

36. The method of claim 31, wherein the raw material comprises 0.01 to 0.09 mol % CeO.sub.2.

37. The method of claim 31, wherein the temperature is between 1000° C. and 1300° C. including the end points.

38. The method of claim 31, wherein the temperature is maintained between 1 and 24 hours including the end points.

39. The method of claim 31, wherein the temperature is 400-600° C. above the melting point of the raw material.

40. The method of claim 31, further comprising adding reducing agents to increase Ce.sup.3+ or adding oxidizing chemicals to reduce Ce.sup.3+.

Description

BRIEF DESCRIPTION OF THE DRAWINGS

[0012] The Appendices attached hereto are hereby incorporated by reference in their entirety and form a part of the specification.

[0013] The following drawings show generally, by way of example, but not by way of limitation, various examples discussed in the present disclosure. In the drawings:

[0014] FIG. 1 shows an example plot of DSC thermographs of (a) glass transition (b) crystallization and (c) melting temperature for S1 to S 6 glass with increasing CeO.sub.2 content.

[0015] FIGS. 2A-C show example images (a) Low resolutions (b) Higher resolution TEM image of cerium oxide nanoparticles from S6 glass that was dissolved in DI water at 37° C. (c) size of the cerium oxide nanoparticles that was created within the S6 glass that was dispersed in DI.

[0016] FIGS. 3A-B show (A) Atomic distance of CeO.sub.2 nanoparticles recovered from S6 glass after it was dissolved in DI water for 7 hrs. (B) size of CeO.sub.2 nanoparticles from S6 glass after dissolved in DI water 2 hrs.

[0017] FIG. 4 shows an example Ce L3 edge XANES spectrum for the reference crystalline compounds CeF.sub.3(Ce.sup.3+) (---) and CeO.sub.2(Ce.sup.4+) (---) with (a) trivalent (Ce.sup.3+) due to 5d.fwdarw.4f emission, and tetravalent reference (Ce.sup.4+) due to 2p.fwdarw.5d with final state (b) 2p4f15d1 (c) with 2p5d.

[0018] FIG. 5 shows an example XANES spectrum for the glasses containing from 0.01 to 0.05 mols of CeO.sub.2 compared to the spectrum for pure CeF.sub.3 (Ce.sup.3+) and pure CeO.sub.2(Ce.sup.4+)

[0019] FIGS. 6A-B show an example XANES spectra for S6 glass with 0.05 mols of (a) cerium with different melting temperature and melting time (b) melted with different raw materials

[0020] FIGS. 7A-B show an example FTIR spectra (a) S1 with increased cerium content (b) S6 glass with different melting time and temperature

[0021] FIG. 8 shows example Ce.sup.3+ and Ce.sup.4+ amounts in the glasses containing from 0.01 to 0.05 mol % analyzed from XANES spectrums.

[0022] FIG. 9 shows example Ce.sup.3+ and Ce.sup.4+ amounts in the glass containing 0.05 mol % for different melting temperatures, melting time, and raw materials analyzed from XANES spectrums.

DETAILED DESCRIPTION

[0023] A borate glass containing varying amounts of cerium (IV) oxide was successfully prepared with both trivalent Ce.sup.3+ (Ce.sub.2O.sub.3) and tetravalent Ce.sup.4+ (CeO.sub.2) states nano particles in 2-5 nm in size. X-ray absorption near edge spectroscopy measurement was used to investigate coexistence of the multivalence in the borate glass. Significant changes in the Ce.sup.+3 and Ce.sup.+4 were observed when the glass was melted with different melting parameters as well as different raw materials. Glass made with borax that contained 0.05 mols of CeO.sub.2 melted at 1100° C. for 3 hrs yields the highest Ce.sup.3+ while the glass containing 0.03 mols of CeO.sub.2 melted for 1100° C. for 1 hr. yields a higher amount of Ce.sup.4+. TEM micrographs confirm the coexistence of Ce.sub.2O.sub.3 and tetravalent CeO.sub.2 nano particles in the glassy matrix. FTIR measurements suggest that the CeO.sub.2 in the glass acts as both a glass-former and a glass modifier.

[0024] In the present disclosure a novel glass that is stable and soluble was synthesized by doping with Ce.sub.2O to produce both trivalent Ce.sup.3+ (Ce.sub.2O.sub.3) and tetravalent Ce.sup.4+ (CeO.sub.2) nanoparticles. These mixed-valence-state nanoparticles are hermetically sealed within the glass with a specific amounts of Ce.sup.3+ and Ce.sup.4+ using a solid-state reaction and further these nano particles are releases when dissolved in aqueous solution.

[0025] The glass of the present disclosure may be changed by adding reducing agents such as carbonates and sulfates to increase Ce.sup.3+ or adding oxidizing chemicals (e.g., nitrates) to reduce Ce.sup.3+. As shown herein, CeO.sub.2 may be used. Alternatively or additionally the glass may comprise CePO.sub.4, Ce(NO3).sub.3 to achieve different amount of Ce.sup.3+ and Ce.sup.4+.

[0026] Potential Applications of Borate glass with multivalent cerium oxide nanoparticle (CeONP) Ce atom can exist in both trivalent Ce.sup.3+ (Ce.sub.2O.sub.3 reduced) and tetravalent Ce4.sup.+ (CeO.sub.2 oxidized) states as it has two partially filled subs-shells, 4f and 5d, allowing several excited states. When combine with oxygen in a nanoparticle formulation, cerium oxide emerges as a fascinating material. In the experiment, relative amount of cerium ions, Ce3.sup.+ and Ce4.sup.+ is controlled and made available within a soluble glass with sealed Ce.sup.3+ and Ce.sup.4+ ratios indefinitely. Further, these cerium oxide nanoparticles (CeONP) is released when dissolved. The TEM microscopy images of nanoparticles extracted when the glass is dissolved provide direct evidence of the coexistence of Ce.sub.2O.sub.3 and CeO.sub.2 nanoparticles.

[0027] As an example, this cerium oxide nanoparticle (CeONP) has been used prolifically in various engineering and biological applications, and by combining the attributes of glass and CeONP at least the following applications may make use of borate glass doped with nanoceria: [0028] 1. Three-Way-Catalysts (TWC)—During automobile emission, three pollutants, HC, CO and NO are simultaneously removed by three-way-catalysts to Co.sub.2 and water by oxidation. It has been understood that ceria nanoparticles have much better performance when used in catalytic converters. For example, mixing ceria particles with diesel is known to dramatically reduce soot in diesel exhausts. In this process typically CeO.sub.2 is used but the glass of the present disclosure can be optimized to provide the necessary oxidation ratio Ce.sup.3+ Ce.sup.4+ to provide the thermal stability that enhances the catalytic reaction. This could lead to more-efficient catalytic converters and cleaner air. [0029] 2. Fuel cells—Solid oxide fuel cells have been widely investigated for energy and environmental pollution problems by directly transforming chemical energy into electric power. Ceria has been studied as a possible electrolyte due to its high ionic conductivity. Still, transformation between Ce.sup.3+ and Ce.sup.4+ ions is a major problem. With nanoparticles embedded in the glass sealed with amounts of Ce.sup.3+ and Ce.sup.4+, the glass of the present disclosure will be able to overcome these drawbacks and can be used as an interface to provide the necessary ion diffusion. [0030] 3. Ionic Solvent—Hydroxylammonium nitrate (HONH2) is an Ionic fluid that has been identified as an environmentally friendly, high performing substance used for space and rocket propulsion. It has been identified that a specific form of an in situ Ce.sup.3+/Ce.sup.4+ ion couple in ceria is critical in deciding the reactivity of HONH2 decomposition generating free radicals ONH2, which are rapidly oxidized to nitrate by the presence of ceria nanoparticles. The synthesized glass can be used to provide this optimized Ce.sup.3+/Ce.sup.4+ to create a further higher-performing monopropellant. [0031] 4. New scintillators—Scintillators convert high-energy particles such as X-ray photons into visible light where the visible light is detected by photomultipliers and translated into an electrical/digital signal. With the effect of the controlled photocatalyst via covalent nanoceria, the synthesized glass will be a promising candidate for potential applications in both high-energy physics and X-ray Computerized Tomography (CT) for industrial and medical imaging. [0032] 5. Solar-cells—With the ozone layer thinning out considerable attention has been given to developing materials that block or reduce ultraviolet (UV) transmission. A varied ratio of Ce.sup.3+ and Ce.sup.4+ in the borate glass of the present disclosure could be used to block (UV) transmission when combined with aluminosilicate. The aluminosilicate will produce a different variation of the borate glass with advanced network structure preventing dissolution. Further, this version of the borate glass series can be used as a novel coating/covers for solar cells that enhances the UV absorption and radiation stability [0033] 6. Commercial development of nanoceria—the glass of the present disclosure can create multivalent CeONP powder in 2-5 nm particles size that are commercially not available

[0034] The present disclosure describes the creation of a soluble glass containing mixed valence cerium oxide nanoparticles. When dissolved, the glass releases multivalent Ce.sup.3+ (Ce.sub.2O.sub.3) and Ce.sup.4+ (CeO.sub.2) nanoparticles and the presence of Ce.sup.3+ and Ce.sup.4+ in the nanoparticle gives it the unique property to neutralize free radicals and function as an antioxidant. The resulting product is a novel glass that has sealed within it specific ratios of Ce.sup.3+ and Ce.sup.4+ and can function as a ready to use biocompatible, antioxidant material.

[0035] As an example, nanoceria containing glass can neutralize free radicals by mimicking the activity of catalase, an important anti-oxidant enzyme in living systems. Catalase mimetic activity of the nanoceria containing glass was tested using a amplex red, a reagent that is able to detect hydrogen peroxide, a common free radical generating compound in living cells. Glass without nanoceria does not have catalase activity, however, glass containing nanoceria has catalase activity. The concentration of cerium (IV) oxide in the glass is 250 PM. These results clearly show that the glass containing nanoceria is able to degrade hydrogen peroxide into water and oxygen, just like catalase does in living cells.

[0036] As an example, nanoceria containing glass can kill bacteria such as Staphylococcus Aureus and Escherichia Coli. The antimicrobial activity of the nanoceria containing glass was tested on two different clinically relevant strains of bacteria—Escherichia Coli and Staphylococcus Aureus. Increasing amounts of glass containing nanoceria (concentration of CeO.sub.2 in micromolar—μM is indicated) inhibit the growth of both strains of bacteria.

[0037] As an example, nanoceria containing glass is biocompatible with mammalian cells. The effect of nanoceria containing glass was determined on mammalian cells using the MTS assay. Epithelial cells were treated with nanoceria containing glass with different concentrations of cerium (IV) oxide. As seen in FIG. 3, after 16 hours of treatment, cells treated with 290-871 μM CeO.sub.2 were still metabolically active at around 80-90% compared to the control (no treatment), while cells treated with the base glass with no ceria showed a significant decrease in cell activity.

[0038] The bioactive glass of the present disclosure that contains mixed valence cerium oxide nanoparticles may dissolve and release nanoparticles has antioxidant activity has anti-microbial activity against the bacteria tested is biocompatible with tested mammalian cells. These properties may be implemented for: [0039] a. Implant coatings—Glass can be used to coat tissue implants. Glass containing antioxidant and antimicrobial nanoceria could be potentially used to [0040] i. Improve biocompatibility of implants [0041] ii. Reduce inflammation at tissue sites because of antioxidant activity [0042] iii. Reduce microbial contamination at tissue sites [0043] iv. Accelerate tissue healing [0044] b. Bandages for wounds—Glass can be processed into fibers that can be used as dressing for wounds. Antioxidant and antimicrobial activities would accelerate wound healing as well as prevent microbial infections. [0045] c. Synthesis of anti-microbial glass equipment for hospitals—antibiotic resistance is a growing concern in the healthcare industry and using glass that has anti-bacterial activity to create glassware for hospitals as well as other equipment would be highly beneficial. [0046] d. Biocompatible material for tissue engineering—bioactive glass is extensively used as scaffolds in both hard and soft tissue regeneration. Glass with antioxidant properties would provide a biocompatible material with additional properties that would enhance the effect of the glass at tissue sites.

[0047] As an example, in order to study the cerium valence states in the novel glass, in-situ valence states of Ce.sup.3+ and Ce.sup.4+ was measured using X-ray Absorption Near Edge Spectroscopy (XANES) obtained at the Ce LIII-edge for all the glass samples using 81D ISS beam line at the National Synchrotron Light Source NSLS II at Brookhaven National Lab. XANES spectroscopy can measure in-situ valence states of redox-sensitive elements such as cerium with much higher accuracy when compared to X-ray photoelectron spectroscopy which can reduce additional Ce.sup.4+ to Ce.sup.3+ under high-vacuum, thus overestimating the Ce.sup.3+ concentration. XANES can circumvent this limitation and therefore is a more appropriate technique to study the in-situ valence states of Ce.sup.+3 and Ce.sup.+4. Synchrotron based determinations of Ce.sup.3+/Ce.sup.4+ in materials have traditionally used Ce L.sub.3-edge XANES which involves a 2p.fwdarw.5d transition located around 5.7 keV. In this experiment the 8-ID ISS beam line with an energy range of 4.9 keV-36 keV was used to measure Ce L.sub.3 edge XANES. This method was also used to compare the Ce.sup.+3 and Ce.sup.+4 amounts in the novel glass when different amounts of cerium oxide are used as well as different raw materials. Further, the glass was physiochemically characterized and the released nanoparticles were investigated via transmission electron microscopy.

Experimental Method:

[0048] A sodium borate glass with molar composition of Na.sub.2O.Math.2B.sub.2O.sub.3 was used as a parent glass (S1 Glass in Table 1) to create a series of borate glass doped with varying concentrations of CeO.sub.2 (Na.sub.2O.Math.2B.sub.2O.sub.3.Math.xCeO.sub.2). Each glass was melted in a platinum crucible in a different atmosphere such as air, argon and nitrogen. The raw materials, boron trioxide and sodium carbonate were obtained from Alfa Aesar with 99.99 purity. Another group of glasses S6-1 to S6-5 with 0.05 mol % of cerium (IV) oxide, melted at 1100° C., 1200° C. and 1300° C. for 1, 2, and 3 hrs contained borax (sodium tetraborate decahydrate) as raw materials (Table 2). Additionally, borate glass-using with different raw materials such as sodium tetraborate (S13) and boric acid (S14) were produced with different amounts of Ce.sup.+3 and Ce.sup.+4. Further, instead of cerium (IV) oxide, cerium (III) fluoride was also used as a source of cerium. Glass S-12 was melted with CeF.sub.3, rich in Ce.sup.3+ instead of CeO.sub.2 along with boron trioxide and sodium carbonate. Each glass was melted in at temperatures 1000° C., 1100° C. 1200° C., and 1300° C. and times 1, 2, 3, 5, 8, 10, 18, and 24 hours. Some compositions were re-melted and some were annealed to obtain different reduced states. Each melt was given a quick stir and was poured and quenched between two steel plates. The quenched glass was then ground in to powder where the particle sizes ranged from 30 μm to 500 μm. Each poured glass was investigated via optical microscopy to observe possible undissolved CeO.sub.2 particles in the glass.

TABLE-US-00001 TABLE 1 Compositional Changes in Glass Samples Sample Amount Melted Melted Time Labeled of Cerium Temperature(° C.) (hrs) Glass S1 0 1100 1 Glass S 3 0.02 mol % CeO.sub.2 1100 1 Glass S 4 0.03 mol % CeO.sub.2 1100 1 Glass S 5 0.04 mol % CeO.sub.2 1100 1 Glass S 6 0.05 mol % CeO.sub.2 1100 1 Glass S 7 0.06 mol % CeO.sub.2 1100 1 Glass S 8 0.07 mol % CeO.sub.2 1100 1 Glass S 9 0.08 mol % CeO.sub.2 1100 1 Glass S 10 0.09 mol % CeO.sub.2 1100 1

TABLE-US-00002 TABLE 2 Example Glass Composition/Identification with change in melting temperature and meting time for glass melted in the air atmosphere that contained borax. Melting Temperature Melting Time Glass ID (° C.) (hrs.) Glass S 6-1 1100 1 Glass S 6-2 1100 2 Glass S 6-3 1100 3 Glass S 6-4 1200 1 Glass S 6-5 1300 1

TABLE-US-00003 TABLE 3 Glass Composition/Identification with change in raw materials, melted at 1100° C., for 1 hr. in the air atmosphere Glass ID Raw Materials Glass S6-1 0.05 mol CeO.sub.2 with Borax Glass S13 0.05 mol CeO.sub.2 with Tetraborate Glass S14 0.05 mol CeO.sub.2 with Boric Acid Glass S12 0.05 mol CeF.sub.3 with Borax

Extracting Nano Particles and Observing Via TEM

[0049] A 625 mg of glass powder with a particle size 150 μm was dissolved in 25 ml distilled water (DI) overnight at 37° C. The solution was then centrifuge and the nanoparticle suspension was separated and sonicated for 5 minutes with fresh DI water. Then the solution was centrifuged and the process was repeated several times to completely remove the glassy substrate. The final sonicated solutions that included the cleaned nano particles were used to examine the microstructure using Transmission electron Microscope (FEI Tecnai 30 TEM). A small drop of the nano particle solution is then placed on the TEM copper grid followed by overnight drying. The sizes of the nanoparticles as well as the inter atomic distances of these ceria nano particles was observed and measured.

Thermal Analysis

[0050] A DSC Q600 differential Thermal analyzer was used to measure the glass transition temperature (Tg), crystallization peaks (Tc), and melting point (Tm) of each glass A 30 mg sample of glass powder (400-450 μm) was measured and tested by heating the sample to 900° C. at 20° C./min. The entire set of borate glass was tested, and the thermographs were obtained for comparing the Tg, Tc, and Tm with the parent S1 glass and to measure the Hurby parameter of glass stability against crystallization.

XANES Spectroscopy

[0051] XANES measurements were performed at Ce L3 edge XAS, at NSLS-II, using the 8-ID ISS beamline with an energy range of 4.9 keV-36 keV. The glasses were prepared by a pellet press to create a smooth flat dense sample of 2-3 mm thickness. The data was collected and analyzed using Athena software to calculate Ce.sup.3+ and Ce.sup.4+ concentrations.

FTIR Absorption Spectroscopy

[0052] To determine the effects of Cerium Oxide on glass structure, FTIR absorption spectra were recorded at room temperature for all the samples between 600-4000 cm.sup.−1 using a Perkin Elmer ATR-IR Spectrum Two Spectrometer. Instrument was manipulated, and the data was collected using “Spectrum 10” software.

Results:

Thermal Analysis:

[0053] Each glass was analyzed using Differential Scanning Calorimetry (DSC) to observe any changes in glass transition, (Tg), crystallization (Tc), and melting point (Tm), as the doping concentration of cerium (IV) oxide changes. All thermographs showed a similar glass transition temperature region while some glass samples showed a dual exothermic crystal peak for some concentrations. The DSC thermographs for all the cerium concentrations are shown in FIG. 1, where thermograms have been normalized with respect to 1 mg of mass for all the glasses for better comparison. The glass transition temperature, Tg falls within the same temperature range for all the glasses except S5. The crystallization temperature (Tc) changes as the cerium content in the glass increases. All the glasses have a higher crystallization temperature Tc than the parent (S1) glass without cerium. There are two crystallization peak temperatures; TPk for S1 glass at 575° C. and 592° C. The second TPk of the parent glass was significantly smaller and the dominant peak temperature increases with increasing cerium content. All glass samples have dual crystallization peaks and the peak temperatures are labeled in Table 4 with the exception the S2 glass which was melted with 0.01 mols of CeO.sub.2. The melting temperature Tm is similar in all the glass compositions.

TABLE-US-00004 TABLE 4 Glass transition, (T.sub.g), Crystallization on-set (T.sub.c), Crystallization Peaks (T.sub.Pk1) and (T.sub.Pk2) and melting (T.sub.m) temperatures (±0.5° C.), as the concentration of CeO.sub.2 increases in the glass along with the calculated Hruby parameter, KH: Glass ID T.sub.G(° C.) T.sub.C(° C.) T.sub.Pk1(° C.) T.sub.Pk2(° C.) T.sub.m(° C.) K.sub.H S1 471 553 575 592 724 0.48 ± 0.003 S2 469 364 586 — 711 0.65 ± 0.004 S3 467 570 589 610 710 0.74 ± 0.004 S4 468 572 605 637 718 0.71 ± 0.004 S5 459 553 575 645 670 0.80 ± 0.006 S6 474 607 562 655 712 1.27 ± 0.008

[0054] Coexistence of the mixed-valence-state Ce.sup.3+ (Ce.sub.2O.sub.3) and Ce.sup.4+ (CeO.sub.2) nanoparticles were observed. S6 glass was dissolving in DI water for different hours to determine the presence of ceria nanoparticles and TEM images for 2 hrs and 7 hrs are shown in FIGS. 3 (a) and (b) respectively with (a) shows a fairly low magnification image with agglomerated ceria nano particles while figure (b) shows a high resolution image with ceria nano particles with the size of 2-5 nm. Results demonstrate that the particle-size didn't change considerably with hours of dissolution. FIG. 6 displays two enhanced images of nanoparticles after the glass S6 was dissolved for (a) 7 hrs and (b) 2 hrs. Both micrographs show evidence of nano particles with atomic distances of (0.388±0.02) nm, (0.245±0.02) nm, and (0.422±0.02) nm confirming the presence Ce.sub.2O.sub.3 nano crystals and the measured inter atomic distances of (0.311±0.02) nm and (0.386±0.02) nm are in complete agreement to the lattice parameter of CeO.sub.2. Results demonstrate that the ceria nanoparticle size didn't change considerably with hours of dissolution while the particles recovered after dissolved in DI water are in sizes ranged from (2.02±0.005) nm to (4.75±0.05) nm as shown in the high-resolution image in FIGS. 2(c) and 3(c).

XANES Spectral Analysis

[0055] Glass compositions were studied with XANES via Ce L.sub.3 edge and compared to compounds CeF.sub.3 and CeO.sub.2. Results shows trivalent (CeF.sub.3—Ce.sup.3+) with a strong narrow single peak at 5727 eV while tetravalent reference (CeO.sub.2—Ce.sup.4+) shows a multi-peak at 5731 eV and 5738 eV as shown in FIG. 4. FIG. 5 shows the XANES spectrum as the amount of CeO.sub.2 in the glass increases for glass melted at 1100° C. for 1 hr. Glass S2 shows a higher Ce.sup.3+ peak while glass S5 shows a higher Ce.sup.4+ peak. The temperature and time effects on the redox states were observed and measured using the XANES spectra as shown in FIG. 6(a) for glass with 0.05 mol % of CeO.sub.2 with borax used in the raw material. The Ce.sup.3+ peak height increased with increasing melting time when melted at 1100° C. When the glass was melted at different temperatures for 1 hr, the glasses meted at 1000° C. and 1300° C. had similar Ce.sup.3+ peak heights. The data, as indicated that the glass melted at 1100° C. 3 hr had the highest Ce.sup.3+ peak height out if all the melts. In order to further understand the different mechanisms of oxygen reduction of the glass, the glass sample with 0.05 mol % of CeO.sub.2 was melted with different raw materials, such as borax, tetraborate, boric acid, and cerium fluoride. FIG. 6(b) shows the XANES spectra for the glass melted with different raw materials to obtain 0.05 mol % Ce. According to these results, the glass doped with CeF.sub.3 had the higher Ce.sup.3+ concentration compared to the glass melted with CeO.sub.2.

FTIR Spectral Analysis

[0056] The FTIR spectra of S1 parent glass along with the glass sample of varying CeO.sub.2 are shown in FIG. 7(a). Significant changes in the peaks were observed as the cerium content of the glass increases. IR spectra of the parent S1 glass shows a peaks between 600 cm.sup.−1 to 850 cm.sup.−1 are due to bending vibrations of various borate segments while the bending vibrations of the B—O—B linkage is shown by the small peak around 710 cm.sup.−1. The spectral lines between 850 cm.sup.−1 to 1200 cm.sup.−1 attributes to B—O stretching vibrations of BO.sub.4, while region of 1200 cm.sup.−1-1500 cm.sup.−1 B—O attributes to stretching vibrations of BO.sub.3 units. Peaks around 775, 880, 1034, 1220, 1345 and 1432 cm.sup.−1 seems to decrease in height as the cerium content in the glass increased and completely disappear in S6 glass, then starts to appear and increase in height when the cerium in the glass is further increased. Peaks 823, 936, 997, 1133, and 1226 cm.sup.−1 increased in overall height with increasing the amount of cerium but rapidly decreased in height with 0.05 and 0.06 mols of CeO.sub.2 and again increased in height with further increment of Ce. These results show that the glass containing 0.05 and 0.06 mols of CeO.sub.2 of cerium is notably different from the rest of the glasses containing cerium and that of the parent glass.

DISCUSSION

[0057] The glass containing Na.sub.2O and B.sub.2O.sub.3 was mixed in with several different amounts CeO.sub.2 to study the development of multivalent CeO.sub.2 and Ce.sub.2O.sub.3 nano particles created within the glass due to different oxygen reduction conditions. The first set of data was obtained from changing the number of CeO.sub.2 mols in small quantities, as 0-0.05 mols of CeO.sub.2. The second set was obtained by changing the melting time and temperature while keeping doped amount of CeO.sub.2 constant; 0.02 and 0.05 mols. The third set was obtained by introducing different raw materials to achieve different reduction status. The DSC micrographs shows that the melting temperature of these glasses are around 700° C. and the glass was melted at 400-600° C. above the melting point to achieve the full dissolution of CeO.sub.2 and CeF.sub.3 and a higher homogeneity. The optical micrographs conducted for all the glasses shows no evidence of undissolved CeO.sub.2 particles. The DSC micrographs shows that the glass transition region is similar in all compositions even though T.sub.g changes with the added CeO.sub.2 amount. These samples had pronounced but different crystallization temperatures with a similar trend like T.sub.g exhibiting an increase with added CeO.sub.2 amount. The Glass-forming ability, which relates to the ease by which melts can be cooled to form glasses with the avoidance of crystal formation, remains similar to the parent glass as CeO.sub.2 content increases since the glass transformation region and the glass melting temperature regions remains similar to each another. On the other hand, the glass stability, which was calculated using Hruby parameter, KH, differ as the amount of CeO.sub.2 content increases as shown in Table 2. Glasses with higher K.sub.H are stable against crystallization upon reheating, indicating changes in the glass network as the cerium content changes, which is confirmed by FTIR Spectroscopy. Glass composition with 0.05 mols of CeO.sub.2 (S6, S13 and S14) have the highest stability against crystallization.

[0058] Strong evidence of the coexistence of multivalence CeO.sub.2 and Ce.sub.2O.sub.3 nanoparticles was observed when the nanoparticles were recovered from these glasses by dissolving the powdered glass in DI water. As discussed earlier, the CeO.sub.2 easily interchange to more reduced Ce.sub.2O.sub.3 by exchanging oxygen, creating a hexagonal structure from a more fluoride structure. High resolution FEI Tecnai 30 TEM measurements are in a very good agreement with the known atomic distances of CeO.sub.2 and Ce.sub.2O.sub.3 structures. As shown in FIG. 3, the measured inter atomic distances of (0.311±0.02) nm are in complete agreement to the ideal lattice parameters of the cubic structure of CeO.sub.2. Additionally, inter atomic distances of (0.388±0.02) nm and (0.386±0.02) nm are in complete agreement to the lattice parameter of A-type hexagonal structure of Ce.sub.2O.sub.3 (0001) plane interatomic distance of 0.3888 nm. The atomic distances (0.242±0.03) and (0.422±0.03) nm refers to (200) of and (101) planes of the hexagonal Ce.sub.2O.sub.3 nano particles. Both TEM micrographs shown in FIGS. 2(c) and 3(c) provide evidence of the coexistence of both types of cubic structure of CeO.sub.2 and hexagonal Ce.sub.2O.sub.3 nano particle in the range of 2 to 5 nm in size. The shapes and the sizes of these particles are in very good agreement with the nano particles obtained by Day et al.

[0059] The results obtained from the XANES measurements using Ce L.sub.3 edge confirms the coexistence of the two valences Ce.sup.3+ and Ce.sup.4+ in the glass when doped with CeO.sub.2 (Ce.sup.4+). All the glasses measured via XANES were compared to compounds CeF.sub.3 (Ce.sup.3+) and CeO.sub.2. Results shows trivalent (Ce.sup.3+) with a strong narrow single peak as shown in FIG. 3 (a) due to 5d.fwdarw.4f emission while the tetravalent reference (Ce.sup.4+) shows a multi-peak. Peak (c) in FIG. 3, due to the transition where electron is exited from Ce 2p to 5d with no electron in the Ce 4f shell, while peak FIG. 3 (b) which is also a Ce.sup.4+ peak where final state is 2p4f15d1. In addition to an electron exited from the valence 2p to 5d, another electron is excited from the valence band of Oxygen 2p shell to Cerium 4f shell leaving a hole. None of the glass compositions exhibited this forbidden peak (b) which denotes that an electron is excited only from the Ce 2p shell to its 5d shell. These results were comparable to the results of Cicconi et. al. thus providing strong evidence of the coexistence of the both trivalent (Ce.sup.3+) and tetravalent (Ce.sup.4+) with in the glass. Out of all the glasses melted with B.sub.2O.sub.3, S2 glass melted with 0.01 mols of CeO.sub.2 for 1100° C. for 1 hr had the highest amount of Ce.sup.4+ ions, while glass S6-2 melted with borax and 0.05 mols of CeO.sub.2 for 1100° C. for 3 hr had the highest amount of Ce.sup.3+ ions out of all meted glass samples, reaching higher oxidization to reduced status. When the same composition of S 6 glass with 0.05 mol of CeO.sub.2 is melted at different melting times, the Ce.sup.3+ concentration increases as the melting time increases as shown in FIG. 6(a). Glass melted at 1200° C. had the highest Ce.sup.4+ concentration. The Ce.sup.3+ concentration of S12 glass melted with CeF.sub.3 (rich in Ce.sup.3+) is similar to S2 glass melted with different melting times using 0.01 mol of CeO.sub.2—. Significant changes in the Ce.sup.3+ peak height was not observed when the same S6 glass composition was made with borax (S6-1), tetra borate (S13) and boric acid (S14) instead of using raw materials of B.sub.2O.sub.3 and Na.sub.2CO.sub.3 and melted for 1100° C. for 1 hr. Out of all the glasses made with borax, the S6-3 glass made with borax for 3 hrs had the highest amount of Ce.sup.3+ concentration.

[0060] Each of the glass samples except the glasses labeled S12-S14 were processed using B.sub.2O.sub.3 as part of the composition. Vitreous B.sub.2O.sub.3 consist of BO.sub.3 unit associated to form Boroxol rings which produces a spectral band at 806 cm.sup.−1 in the glassy matrix. The Na.sub.2O present in the glass convert BO.sub.3 units to BO.sub.4 units. The peak at 1034 cm.sup.−1 in the parent glass S1 is due to the bond stretching vibrations of BO.sub.4 while 775 cm.sup.−1 peak is comparable to the bind bending vibrations of BO.sub.4. Spectral lines at 1345 and 1432 cm.sup.−1 in the FTIR absorption spectra are comparable to B—O stretching of trigonal BO.sub.3 units. The lack of a peak at 806 cm.sup.−1 in the absorption spectra in any of the glass tested indicate that the glass network mainly consists of BO.sub.3 units to BO.sub.4 units at the expense of boroxol rings. However, adding CeO.sub.2 to the glass network works much differently than adding alkali as discussed in Damwari et al. CeO.sub.2 act as a glass modifier as well as a glass network former. Both BO.sub.3 units to BO.sub.4 units in the IR spectra of the S6 glass disappeared indicating a formation where BO.sub.3 units would be used to form Ce—O—B units rather than BO.sub.4 units. It has been investigated that the asymmetric stretching vibrations of Ce—O—B lies in the 400 and 1370 cm.sup.−1. All the glasses formed from 0.05 mol of cerium oxide, S6-1 to S6-5 show the same significant difference that the S6 glass shown in the IR spectra with a peak broadening from 1200 to 1600 cm.sup.−1 as shown in FIG. 7(b). This could be due to the existence of both active bands of Ce—O—B and B—O—B links overlapping in this series of glass. The formation of Ce—O—B link as a glass former is supported by the XANES data where glass with 0.05 mol (specially S6-2) showed the highest amount of oxygen reduction providing larger amount of non-bridging oxygen (NBO) in the glass, forming much stable Ce—O—B link.

CONCLUSION

[0061] A soluble sodium borate glass containing varying amounts of cerium oxide that is stable against crystallizations was successfully prepared with both trivalent Ce.sup.3+ (Ce.sub.2O.sub.3) and tetravalent Ce.sup.4+ (CeO.sub.2) states. Cerium oxide nano particles were released when these glasses were dissolved in DI water. The TEM data provides strong evidence of coexistence of both types of cubic structure of CeO.sub.2 (tetravalent Ce.sup.4+) and hexagonal Ce.sub.2O.sub.3 (trivalent Ce.sup.3+) nano particles. The concentrations of Ce.sup.3+ and Ce.sup.4+ in these glasses were determined using XANES Ce L.sub.3 edge x-ray absorption spectroscopy. The XANES results also confirmed the coexistence of Ce.sup.3+ and Ce.sup.4+ valences in a series glasses with different concentrations of CeO.sub.2 (Ce.sup.4+) melted with different temperatures, times, and raw materials. The Ce.sup.3+ and Ce.sup.4+ amounts significantly differed as the amounts of CeO.sub.2 changed as well as with changes in melting time, temperature and raw materials. Glass S6-2 with 0.05 mol % CeO.sub.2 had the maximum amount of Ce.sub.2O.sub.3(Ce.sup.3+) while glass S5 with 0.04 mol % CeO.sub.2 had the maximum amount of CeO.sub.2 (Ce.sup.4+). The results of this work also confirmed that the cerium oxide in the glass acts as both network modifier and network former. Cerium in the glass contained higher order Ce.sup.3+ act as a glass network former by creating a Ce—O—B link instead of BO.sub.4 units while the glass with higher concentration of Ce.sup.4+ use cerium as a network modifier by creating BO.sub.4 units from BO.sub.3 units with increasing addition of CeO.sub.2.

[0062] Borate glass containing varying amounts of cerium oxide was successfully prepared with both trivalent Ce.sup.3+ (Ce.sub.2O.sub.3) and tetravalent Ce.sup.4+ (CeO.sub.2) states nano particles with 2-5 nm in size and the Ce.sup.+3 and Ce.sup.+4 concentrations of these glass compositions was determined using XANES CeL.sub.3 edge x-ray absorption spectroscopy. The results confirmed the coexistence of Ce.sup.+3 and Ce.sup.+4 valances in a series glass with different compositions. The Ce.sup.+3 and Ce.sup.+4 amounts significantly differed as the amounts of CeO.sub.2 changed as well as with changes in melting time, temperature and raw materials. The glass S6-2 with 0.05 mol % CeO.sub.2 had the maximum amount of Ce.sub.2O.sub.3(Ce.sup.3+) while the glass S5 with 0.04 mol % CeO.sub.2 had the maximum amount of CeO.sub.2 (Ce.sup.4+). The results of this experiment also confirmed that the cerium oxide in the glass acts as both network modifier and network former. Cerium in the glass contained higher order Ce.sup.+3 act as a glass network former by creating a Ce—O—B link instead of BO.sub.4 units while the glass with higher concentration of Ce.sup.+4 use cerium as a network modifier by creating BO.sub.4 units from BO.sub.3 units with increasing addition of CeO.sub.2.