Nanoscale structures, such as nanoparticles, nanorods, nanowires, nanocubes, and nanotubes, have attracted extensive synthetic attention as a result of their novel size-dependent properties (Xia et al., Adv. Mater., 2003, 15, 353; Patzke et al., Angew. Chem. Int. Ed., 2002, 41, 2446; Wu et al., Chem. Eur. J., 2002, 8, 1260; Tremel, W., Angew. Chem. Int. Ed., 1999, 38, 2175; Tenne, R., Chem. Eur. J., 2002, 8, 5296; Rao et al., J. Mater. Chem., 2001, 11, 2887; and Rao et al., J. Chem. Soc., Dalton Trans., 2003, (1), 1). In particular, one-dimensional (1-D) materials (e.g., nanorods) with their inherent anisotropy are the smallest dimension structures that can be used for efficient transport of electrons and optical excitations. As such, they are applicable as building blocks to assemble the next generation of molecular electronic and computational devices.
Part of the challenge of developing practical nanoscale devices for a variety of applications, including energy storage, fuel cells, and sensing, is the ability to conveniently synthesize well-characterizable, single-crystalline nanostructures in order to rationally exploit their nanoscale optical, electronic, thermal, and mechanical properties (Rao et al., J. Mater. Chem., 2001, 11, 2887; Duan et al., Nature, 2001, 409, 66; Rueckes et al., Science, 2000, 289, 94; and Gao et al., Nature, 2002, 415, 599).
Ideally, the net result of nanoscale synthesis is the production of structures that achieve monodispersity, stability, and crystallinity with a predictable morphology. Many of the synthetic methods used to attain these goals have been based on principles derived from semiconductor technology, solid state chemistry, and molecular inorganic cluster chemistry.
Strategies for the preparation of 1-D nanowires, for example, rely on the formation from a confined alloy droplet, as described by the vapor-liquid-solid (VLS) mechanism (Wu et al., Chem. Eur. J., 2002, 8, 1260 and Hu et al., Acc. Chem. Res., 1999, 32, 435), the kinetic control of growth through the use of capping reagents (Peng et al., J. Am. Chem. Soc., 2002, 124, 3343 and Puntes et al., Science, 2001, 291, 2115), the generation through a low temperature, chimie douce solution chemical methodology Limmer et al., Adv. Mater., 2001, 13, 1269 and Ginzburg-Margau et al., Chem. Commun., 2002, (24), 3022).
Metal oxides and metal fluorides, in particular, represent two of the most diverse classes of materials, with important structure-related properties, including superconductivity, ferroelectricity, magnetism, conductivity, and gas sensing capabilities (Smart et al. Solid State Chemistry; 2nd ed.; Chapman & Hall: New York, 1995 and West, A. R. Basic Solid State Chemistry; 2nd ed.; John Wiley & Sons: New York, 1999).
Prior art methods of synthesizing oxide nanostructures are by heating and calcination of precursors (Rao et al., J. Chem. Soc., Dalton Trans., 2003, (1), 1); reversed micelle templating techniques (Qi et al., J. Phys. Chem. B, 1997, 101, 3460 and Kwan et al., Chem. Commun., 2001, (5), 447); sol-gel processes (Krumeich et al., J. Am. Chem. Soc., 1999, 121, 8324); surfactant-mediated steps (Wang et al., Chem. Commun., 2001, (8), 727); and hydrothermal procedures (Liao et al., Chem. Mater., 2000, 12, 2819).
Prior art methods of synthesizing fluoride nanostructures are by hydrothermal/solvothermal method or reverse micelle method (Sun et al., Chem. Commun. 2003, 1768; Cao et al., J. Am. Chem. Soc. 2003, 125, 11196; Huang et al., Mater. Lett. 2005, 59, 430 and Agnoli et al., Adv. Mater. 2001, 13, 1697).
However, these prior art methods have substantial shortcomings. Most significantly, the prior art methods do not allow for the synthesis of pure, single-crystalline nanostructures with predictable size and morphology.
For example, although a few prior art methods allow for the synthesis of nanorods with a high aspect ratio, these methods do not yield pure nanostructures. In particular, these methods use organic surfactants in their processes for making nanostructures. (Shi et al., Adv. Mater., 2003, 15, 1647 and Shi et al., Chem. Commun., 2002, (16), 1704.) Thus, the resultant nanostructures have organic surfactant molecular groups, such as bis(2-ethylhexyl)sulphosuccinate, undecylic acid, decylamine, or double-hydrophilic block copolymers, present on their surfaces.
Additionally, the prior art methods do not enable the synthesis of single-crystalline nanostructures. For example, in spite of the variety of different deposition strategies used in the prior art, including electrochemical deposition, electroless deposition, polymerization, sol-gel deposition, and layer-by-layer deposition in nanoporous templates, the resultant nanostructures are polycrystalline. The reason for the observed polycrystallinity is that these prior methods require additional annealing steps at high temperature. (Lakshmi et al., Chem. Mater., 1997, 9, 857; Limmer et al., Adv. Funct. Mater., 2002, 12, 59; Schmid, G., J. Mater. Chem., 2002, 12, 1231; and Hulteen et al., J. Mater. Chem., 1997, 7, 1075.)
Moreover, the prior art methods do not enable the reproducible fabrication of ordered, monodisperse 3-D arrays of 1-D nanomaterials. Such fabrication is critical because assembly of nanoscale components is a key for building functional devices, important for applications including nanoscale electronics and molecular sensing (Colfen et al., Angew. Chem. Int. Ed., 2003, 42, 2350). Specifically, the fabrication of 3-D arrays of nanorods would be useful for optoelectronic applications, such as room-temperature ultraviolet lasing (Huang et al., Science, 2001, 292, 1897). Though a number of preparative methods have been reported for generating these types of nanoscale architectures, none of these techniques appears to work for metal oxides and fluorides (Yang, P., Nature, 2003, 425, 243; Feng et al., J. Am. Chem. Soc., 2004, 126, 62; Tian et al., Nat. Mater., 2003, 2, 821; and Tian et al., J. Am. Chem. Soc., 2003, 125, 12384).
Furthermore, the prior art methods require complex fabrication processes and high temperatures to yield nanostructures.
Accordingly, there remains a need for a low temperature and simplistic method of synthesizing pure single-crystalline nanostructures which allows for controlling the size, in particular the aspect ratio; the extent of monodispersity; and morphology of the resultant nanostructures.
The present invention includes pure single-crystalline metal oxide and metal fluoride nanostructures. These nanostructures include nanorods and nanoarrays. The nanostructures are at least about 80%, 90%, 95%, 99% or 100% free of defects and/or dislocations.
The nanorods have an aspect ratio of from about 2 up to about 1000. More typically, the aspect ratio is about 15. The diameter of the nanorod ranges from about 1 to about 10,000 nm, more typically from about 2 nm to about 2 μm. The length of the nanorod ranges from about 20 nm to about 20 μm, more typically about 10 μm.
In one embodiment, the present invention includes single crystalline nanorods with the chemical formula of ABO4. A is Ba, Sr, Pb, Ca, Fe, Mn, Co, Ni, Cu, Zn, Cd, Mg, and mixtures of thereof. B is W, Cr, Mo, S, I, Se, and mixtures thereof. The present invention includes nanostructures which consist essentially of the ABO4 compounds.
In another embodiment, the present invention includes single crystalline nanorods with the chemical formula of DEF3. D is Na, K, Li, Rb, Ce, and their mixtures. E is a transitional metal, Ca, Mg, Ba, Sr, Pb or mixtures of the aforementioned elements. Transitional metals include Mn, Zn, Cd, Fe, Co, and Ni. The present invention includes nanostructures which consist essentially of the DEF3 compounds.
In a further embodiment, the present invention includes single crystalline nanorods with the chemical formula of GF2. G is selected from the group consisting of Mg, Ca, Sr, Ba, Mn, Zn, Cd, Fe, Co, Ni, and their mixtures. The present invention includes nanostructures which consist essentially of the GF2 compounds.
In other embodiment of the present invention, the DEF3 and GF2 nanostructures are doped with trivalent rare earth ions.
In another aspect, the present invention includes nanoarray comprising a plurality of single crystalline nanorods wherein the chemical formula of the nanorods is ABO4, DEF3, or GF2, as described above. Preferably, the nanoarrays are at least 50%, 60%, 70%, 80%, 90%, 95%, 99% or virtually completely monodisperse.
In a further aspect, the present invention includes a method of producing single crystalline nanostructures (e.g., nanorods) with the chemical formula of ABO4, DEF3, or GF2. The method comprises providing a first reagent solution and providing a second reagent solution; placing a porous membrane between the first reagent solution and the second agent solution, thereby producing single crystalline nanostructures. Preferably, the production takes place at room temperature. In one embodiment, the first reagent solution comprises a salt of A; and the second reagent solution comprises a salt of B. In another embodiment, the first reagent solution comprises a fluoride of D; and the second reagent solution comprises a salt of E. In an additional embodiment, the first reagent solution comprise a salt of G; and the second reagent solution is ammonia fluoride or lithium fluoride.
Examples of porous membranes include “track-etch” polymeric membranes; copolymer templates; porous alumina or silica membranes; and TEFLON® membranes. Preferably, the method comprises a double-diffusion set-up.
In one aspect of the present invention, the method further comprises controlling the dimensions and morphology of the nanostructures (e.g., nanorods and nanoarrays).
In another aspect, the present invention provides devices comprising at least one single crystalline nanorod described above. Examples of the devices include sensors, a device used in molecular electronics, a device used in optoelectronics, and scanning probe microscopy tips.
The present invention overcomes many of the shortcomings of the prior art. For example, unlike the prior art methods, the present invention enables the synthesis of pure single-crystalline, monodisperse, stable (including thermally stable) nanostructures at room temperature. Another key advantage of the invention includes enabling the synthesis of nanostructures of a predictable size, shape, chemical composition, and morphology. The chemical and physical properties of template membranes (i.e., pore geometry and monodisperse diameters) enable a high degree of control over the dimensions of the resulting nanostructures.
A further advantage of the present method is that these nanostructures can be assembled into an architecture suitable for nanoscale electronics and molecular sensing. Specifically, the invention allows for the fabrication of nanoarrays in a predictable and reproducible manner. Such nanoarrays are useful for optoelectronic applications, such as room-temperature ultraviolet lasing.
The present invention relates to the field of nanotechnology, including nanostructures and their applications.
The present invention includes metal oxide and metal fluoride single crystalline nanostructures. These nanostructures include free-standing nanorods and include nanoarrays comprising a plurality of such nanorods. For the purposes of this specification, the term nanorod(s) is synonymous with nanowire(s). The invention also includes methods of making such nanostructures. In particlar, the methods enable the making of nanostructures with predictable size and morphology. The methods comprise the use of template membranes and proceed at room temperature.
Nanostructures with the Chemical Formula of ABO4
In one embodiment of the present invention, the nanostructures have the chemical formula of ABO4. A and B represent two different metallic elements with oxidation states of +2 and +6, respectively.
A can be an alkaline earth metal or a transitional metal. A can be, for example, barium (Ba), strontium (Sr), lead (Pb), calcium (Ca), iron (Fe), manganese (Mn), cobalt (Co), nickel (Ni), copper (Cu), zinc (Zn), cadmium (Cd), magnesium (Mg), or mixtures thereof. An example of a mixture is Ba1-xSrx, wherein x is 0≦x≦1.
B can be, for example, tungsten (W), chromium (Cr), molybdenum (Mo), sulfur (S), iodine (I), selenium (Se), and mixtures thereof. An example of a mixture is W1-xCrx, wherein x is 0≦x≦1.
In the methods of making nanostructures with the formula ABO4, any compound comprising A and any compound comprising B can be used as reagents, hereinafter termed “A-reagent” and “B-reagent,” repectively. These reagents are soluble in aqueous solvents.
Examples of A-reagents Include:
Ba(barium): acetate (Ba (CH3CO2)2); halides, such as bromide (BaBr2), chloride (BaCl2), and iodide (BaI2); hydroxide (Ba(OH)2); nitrate (Ba(NO3)2); oxalate (BaC2O4); perchlorate (Ba(ClO4)2); etc.
Sr(strontium): acetate (Sr(CH3CO2)2); halides, such as chloride (SrCl2), bromide (SrBr2)and iodide (SrI2); hydroxide (Sr(OH)2); nitrate (Sr(NO3)2); oxalate (SrC2O4); perchlorate (Sr(ClO4)2); etc.
Ca(calcium): acetate (Ca(CH3CO2)2); halides, such as chloride (CaCl2), bromide (CaBr2)and iodide (CaI2); hydroxide (Ca(OH)2); nitrate (Ca(NO3)2); oxalate (CaC2O4); perchlorate (Ca(ClO4)2); etc.
Fe(iron): acetate (Fe(CH3CO2)2); halides, such as bromide (FeBr2), chloride (FeCl2), and iodide (FeI2); nitrate (Fe(NO3)2), etc.
Mn(manganese): acetate (Mn(CH3CO2)2); halides, such as bromide (MnBr2), chloride (MnCl2), and iodide (MnI2); nitrate (Mn(NO3)2), etc.
Co(cobalt): acetate (Co(CH3CO2)2); halides, such as bromide (CoBr2), chloride (CoCl2), and iodide (CoI2); nitrate (Co(NO3)2), etc.
Ni(nickel): acetate (Ni(CH3CO2)2); halides, such as bromide (NiBr2), chloride (NiCl2), and iodide (NiI2); nitrate (Ni(NO3)2), etc.
Cu(copper): acetate (Cu(CH3CO2)2); halides, such as bromide (CuBr2), chloride (CuCl2), and iodide (CuI2); nitrate (Cu(NO3)2), etc.
Zn(zinc): acetate Zn(CH3CO2)2; halides, such as bromide (ZnBr2), chloride (ZnCl2), fluoride (ZnF2), and iodide (ZnI2); lactate Zn[CH3CH(OH)CO2]2; nitrate (Zn(NO3)2); oxalate (ZnC2O4); perchlorate (Zn(ClO4)2); sulfate (ZnSO4); etc.
Mg(magnesium): acetate (Mg(CH3CO2)2); halides, such as bromide (MgBr2), chloride (MgCl2), and iodide (MgI2); nitrate (Mg(NO3)2), etc.
Pb (lead): acetate; halides, such as, bromide, chloride, and iodide; nitrate , etc.
Cd (cadmium): acetate; halides, such as, bromide, chloride, and iodide; nitrate, etc.
Two or more A-reagents can be used to make a mixed A-reagent. For example, a mixed A-reagent can comprise barium chloride and strontium chloride, which can form nanostructures of the formula (Ba1-xSrx)BO4, wherein x is 0≦x≦1.
Examples of B-reagents include:
W(tungsten): Na2WO4; K2WO4; Li2WO4; (NH4)2WO4; oxychloride (WOCl4); rubidium tungstate; cesium tungstate; etc.
Cr(chromium): Na2(CrO4); K2CrO4; Li2CrO4; (NH4)2CrO4; oxychloride (CrOCl4); etc.
Mo(molybdenum): Na2MoO4; K2MoO4; Li2MoO4; (NH4)2MoO4; oxychloride (MoOCl4); etc.
S (sulfur): Na2SO4; K2SO4; Li2SO4; (NH4)2SO4; oxychloride (SOCl4); etc.
I (iodine): Na2IO4; K2IO4; Li2IO4; (NH4)2IO4; oxychloride (IOCl4); etc.
Se (selenium): Na2SeO4; K2SeO4; Li2SeO4; (NH4)2SeO4; oxychloride (SeOCl4); etc.
Two or more B-reagents can be used to make a mixed B-reagent. For example, a mixed B-reagent can comprise sodium tungstate and sodium chromate which can form nanostructures of A(W1-xCrx)O4 wherein x is 0≦x ≦1.
Specific examples of ABO4 compounds include, but are not limited to, BaWO4, BaCrO4, SrWO4, BaMoO4, ZnWO4, CaWO4, MgWO4, CaCrO4, MgCrO4, BaSO4, BaIO4, Ba1-xSrxWO4, etc.
Nanostructures with the Chemical Formula of DEF3.
In another embodiment of the present invention, the nanostructures have the chemical formula of DEF3.
D can be, for example, sodium (Na), potassium (K), lithium (Li), rubidium (Rb), cesium (Ce), and their mixtures. An example of a mixture is Na1-xKx, wherein x is 0≦x≦1.
E can be an alkaline earth metal or a transitional metal. E can be, for example, calcium (Ca), magnesium (Mg), barium (Ba), strontium (Sr), lead (Pb), manganese (Mn), zinc (Zn), cadmium (Cd), iron (Fe), cobalt (Co), nickel (Ni), copper (Cu) or mixtures thereof. An example of a mixture is Mn1-xZnx, wherein x is 0≦x≦1.
In the methods of making nanostructures with the formula DEF3, any compound comprising D and any compound comprising E can be used as reagents, hereinafter termed “D-reagent” and “E-reagent,” respectively. These reagents are soluble in aqueous solvents.
Examples of D-reagents include: sodium fluoride, potassium fluoride, lithium fluoride, rubidium fluoride, cesium fluoride, and their mixtures.
Two or more D-reagents can be used to make a mixed D-reagent. For example, a mixed D-reagent can comprise sodium fluoride and potassium fluoride, which can form nanostructures of the formula (Na1-xKx)EF3, wherein x is 0≦x≦1.
Examples of E-reagents include: acetates, hydroxides, percholates, oxalates, nitrates and halides, such as chloride and bromide, of Mn, Pb, Zn, Cd, Fe, Co, Ni, Ba, Sr, Ca, Mg, Cu and their mixtures.
Two or more E-reagents can be used to make a mixed E-reagent. For example, an mixed E-reagent can comprise manganese nitrate and zinc nitrate, which can form nanostructures of the formula D(Mn1-xZnx)F3, wherein x is 0≦x≦1.
Some specific examples of DEF3 compounds include KMnF3, NaMnF3, KZnF3, KCdF3, etc.
In an alternative embodiment, the nanostructures with the chemical formula of DEF3 are doped with trivalent rare earth ions to form nanostructures with the chemical formula of DE1−yF3−4: Rey, wherein y is 0≦y≦1 (when y is 1, then the formula is DReF4). Re is selected from the lanthanide or actinide series. The lanthanide series includes La, Ce, Pr, Nd, Pm, Sm, Eu, Gd, Tb, Dy, Ho, Er, Tm, Yb and Lu. The actinide series includes Ac, Th, Pa, U, Np, Pu, Am, Cm, Bk, Cf, Es, Fm, Md, No and Lr.
Any compound comprising Re can be used as a “Re-reagent.” Preferred examples of Re-reagents include nitrates and halides, such as chloride and bromide, of the lanthanides and actinides, and their mixtures, for example, Nd(NO3)3, Nd(OAc)3, Er(NO3)3, Ho(NO3)3, etc.
Two or more Re-reagents can be used to make a mixed Re-reagent. For example, a mixed Re-reagent can comprise erbium nitrate and holmium nitrate, which can form nanostructures of the formula DE1-yF3-4: (Er1-xHox)y, wherein x is 0≦x≦1 and y is 0≦y≦1 (when x is 1, and y is 1, then the formula is DHoF4).
Nanostructures with the Chemical Formula of GF2.
In a further embodiment of the present invention, the nanostructures have the chemical formula of GF2.
G can be an alkaline earth metal, a transitional metal or other metals. For example, G can be Mg, Ca, Sr, Ba, Mn, Zn, Cd, Fe, Co, Ni, Pb, Cu or mixtures thereof. An example of a mixture is Ba1-xCax, wherein x is 0≦x≦1.
In the methods of making nanostructures with the formula GF2, any compound comprising G can be used as a reagent, hereinafter termed “G-reagent.” A reagent comprising fluoride is ammonia fluoride or lithium fluoride. These reagents are soluble in aqueous solvents.
Examples of G-reagents include: acetates, hydroxides, percholates, oxalates, nitrates and halides, such as chloride and bromide, of Ba, Sr, Mn, Zn, Cd, Fe, Co, Ni, Ca, Mg, Pb, Cu and their mixtures.
Two or more G-reagents can be used to make a mixed G-reagent. For example, an mixed G-reagent can comprise barium nitrate and calcium nitrate, which can form nanostructures of the formula (Ba1-xCax)F2, wherein x is 0≦x≦1.
Some specific examples of GF2 compounds include BaF2, SrF2, CaF2, MgF2, etc.
In an alternative embodiment, the nanostructures with the chemical formula of GF2 are doped with trivalent rare earth ions to form nanostructures with the chemical formula of G1-yF2-3: Rey, wherein y is 0≦y≦1 (when y is 1, the formula is F3Re). Re is selected from the lanthanide or actinide series, as defined above. Any compound comprising Re can be used as a “Re-reagent,” as defined above.
Two or more Re-reagents can be used to make a mixed Re-reagent. For example, an mixed Re-reagent can comprise erbium nitrate and holmium nitrate, which can form nanostructures of the formula G1-yF2-3: (Er1-xHox)y, wherein x is 0≦x≦1 and y is 0≦y ≦1 (when x is 1 and y is 1, then the formula is HoF3).
Methods of Making the Nanostructures
An A-reagent and B-reagent, or a D-reagent and E-reagent, or a G-reagent and ammonia/lithium fluoride are each placed into separate aqueous solvents to form reagent solutions. Accordingly, different ions form in each of the different solutions, i.e., A2+; (BO4)2−; D+F−; E2+; G2+ or F− form in each of the solutions.
In the alternative embodiment wherein the E-reagent or G-reagent is doped with a Re-reagent, an Re-reagent is added to the E-reagent or to the G-reagent. In this embodiment, the ions formed in solution are DF− and E2+ along with Re3+; or F− and G2+ along with Re3+.
The concentrations of the two selected reagent solutions range from being equivalent (i.e., equimolar) to where one solution is twice or thrice as concentrated as the other.
Examples of suitable aqueous solvents include water; alkyl and alkylene glycols, such as, for example, ethylene glycol; mixtures of water and alcohols (methanol, ethanol, isopropanol, butanol, pentanol, hexanol); mixtures of water and acids, such as, for example, acetic acid, sulfuric acid, phosphoric acid, propionic acid, ethanoic acid, and/or nitric acid; and mixtures of ethylene glycol and acids, such as, for example, citric acid and/or tartaric acid. Solvents are selected according to the particular reagents used as would be known to a skilled artisan.
The two selected reagent solutions are then placed in contact with each other in a manner which allows production of single crystals. Reactions can be run at any temperature that is between the melting and boiling points of the solvents. Preferably, the reaction is run at room temperature. The reagent solutions are placed into contact with each other at a slow rate. Preferably, the reagent solutions are placed into two reservoirs separated from each other by a template membrane.
An example of a set-up which allows for such a slow rate of contact of reagent solutions is a double-diffusion set-up. See
A double diffusion crystallization set-up process is described in Park et al., Adv. Mater., 2002, 14, 1167; Park et al., J. Mater. Chem., 2004, 14, 2291; and Peters et al., M., J. Chem. Soc., Dalton Trans., 2001, 24, 358, all of which is incorporated herein by reference.
The reagent solutions flow into the membrane pores. The membrane slows down the rate of contact of the ions of the reagents. When the two ions meet, crystallization occurs thereby forming nanorods within the membrane pores. The nucleation and growth of crystalline nanorods occur essentially instantaneously through the direct chemical interaction between ions of the two different reagent solutions.
Although not wanting to be limited by a mechanism, it is believed that the formation mechanism of nanorods of the present invention is analogous to a biomimetic crystallization process (Dorozhkin et al., Cryst. Growth Des., 2004, 4, 389). That is, the growth of nanorods within the confinement of a template membrane is analogous to the precipitation of single crystals of calcium carbonate and calcium phosphate within the confinement offered by gels, micelles, chitin scaffolds, and collagen matrices. The interactions between the reagent molecules are likely stronger than those between the reagent molecules and the pore walls. The nucleation rate is primarily dictated by the supersaturation of the solution.
Single crystals of nanoscale materials derive from isolated, disparate nucleation sites (consisting of ABO4, DEF3 or GF2 (or their rare-earth doped species) nuclei generated via the reaction between their respective ions), which then grow by extension through the porous network. Continued growth then occurs at the crystal surface at a rate limited by ion availability, until the crystal impinges on the template surface, which ultimately limits further growth.
The reagents are in contact until the desired growth is achieved, e.g., from about 1 h to about 100 hrs, more typically from about 2 hrs to about 24 hrs. The membrane is then removed.
In the methods of making free-standing nanorods, the membranes can be removed from the resultant nanorods by immersion in a base solution as would be known by a skilled artisan. For example, the membranes can be removed by immersion in NaOH solution at room temperature. Thereafter, to retrieve free-standing nanostructures, the base solution is diluted in several steps with distilled water and an organic solvent. Free-standing nanostructures are then collected by centrifugation or filtration, as would be known by a skilled artisan.
In the methods of making nanoarrays, a membrane containing a nanoarray is attached to a substrate to form a composite, as would be known by a skilled artisan. The nanoarray can be attached, for example, by glue, or by vacuum or sputtering coating one side of the membrane containing nanorods with a thin film of substrates. An example of a glue is Epoxy resin. Examples of substrates include a paper towel, gold, polymeric thin films graphite, mica, silica, silicon, wood, glass, alumina, metal, and metal oxide.
The resulting composite is immersed into an aqueous base solution (e.g., NaOH aqueous solution) until the membrane is dissolved (e.g., for about 15 minutes to about 2 hrs). A nanoarray protruding out from the surface of the substrate is obtained. Preferably, the nanoarray is washed with distilled, deionized water and air-dried.
The methods of the present invention do not require that the resultant nanostructures be annealed.
Purity of Nanostructures
The nanostructures of the invention are crystalline and solid. Preferably, the nanostructures are at least 95%, more preferably at least 99%, and most preferably virtually completely free of defects and/or dislocations. As defined in this specification, defects are irregularities in the crystal lattice. Some examples of defects include a non-alignment of crystallites, an orientational disorder (e.g., of molecules or ions), vacant sites with the migrated atom at the surface (Schottky defect), vacant sites with an interstitial atom (Frenkel defects), and non-stoichiometry of the crystal. An example of a dislocation is a line defect in a crystal lattice.
Additionally, the nanostructures are free of organic surfactant molecular groups (including nonionic surfactants, cationic surfactants, and anionic surfactants), such as bis(2-ethylhexyl)sulphosuccinate, undecylic acid, sodium dodecyl sulfate (SDS), Triton X-100, decylamine, or double-hydrophilic block copolymers, which are present on the surfaces of prior art nanostructures.
Methods of Controlling the Dimensions and Morphology of Nanostructures
The dimensions and morphology of the resultant nanostructures are controlled by the structure of the template membranes within which the nanostructures are grown. The membranes act to spatially direct crystal growth.
The nanostructures grow within membrane pores. The pore sizes of the membranes are varied according to the desired diameters of the resultant nanostructures. For example, the diameters of the pores can range from about 1 nm to about 100 μm, preferably from about 3 nm to about 2 μm, more preferably from about 20 nm to several hundred nanometers. A resultant nanorod typically has approximately the same diameter as the size of the pore within which it was grown. For example, using a membrane with 200 nm pores produces nanorods having diameters in the range of 190 to 210 nm. Typically, the diameter is uniform throughout the length of a nanorod.
The thicknesses of the membranes are varied according to the desired lengths of the nanostructures. The thickness of a membrane corresponds with the length of a resultant nanorod. Accordingly, the maximum length of a nanorod is limited by the thickness of a membrane. Membranes typically range from approximately about 20 nm to about 20 μm, more typically from about one to about five microns, in thickness. Accordingly, nanostructures have the same range of lengths.
Aspect ratio, as defined in the present specification, is the ratio of length to width (i.e., diameter). The aspect ratio of a nanorod of the present invention can range from about 2 to about 1000, more typically from about 5 to about 50, and most typically from about 10 to about 25.
The width of an array corresponds with the width of the membrane on which the array was grown. The length of an array corresponds with the thickness of the membrane. The nanorods of an array can be monodisperse by using a membrane with uniform pores. Alternatively, the nanorods of an array can be polydisperse by using a membrane with a variety of different pore sizes.
Additionally, the distances between each individual nanorod within an array is controlled by varying the pore densities on the membranes. All other parameters being equal, the more dense the porosity of a membrane, the closer each individual nanorod is to each other. Alternatively, the pores on the membrane can be placed in such a fashion that they are not at a uniform distance from each other.
Although within a nanoarray the nanorods are individually separated from each other, they form a dense, continuous network. Preferably, the nanorods are roughly parallel to each other and vertically oriented on the substrates to form a packed array, stretching over micron-sized areas.
The shapes of the nanorods reflect the morphology and inner surface roughness of the pores within which they were grown. That is, the morphology of the nanorods can spatially map out the interior nanoscopic profile and localized contours of the internal pores of the membranes.
For example, if the inner surface of a pore within which a nanorod was grown is smooth, then the resultant nanorod is straight and smooth. Alternatively, if the inner surface of a pore is rough, then the resultant nanorod has protrusions or depressions on its surface.
Examples of membranes suitable for the present invention include porous alumina or silica membranes; “track-etch” polymeric membranes; copolymer templates; and TEFLON® membranes.
Alumina membranes have dimensions of the pores which are tunable in the range of 4 to several hundred nanometers. Pore densities as high as 1011 pores/cm2 can be obtained, and typical membrane thickness can range from 10 to 100 μm. Preferred membranes are porous anodic alumina (AAO) membranes. The AAO membranes have a porosity of 40 to 65%.
Silicon membranes are obtained by electrochemical etching of silicon wafers. The resulting porous structures has a thin nanoporous layer (with pore diameters of as small as 3 nm) on top of macroporous layer.
Track-etch membranes contain randomly distributed nanochannels (i.e., pores) of uniform diameter (as small as 10 nm). Pore densities approach 109 pores/cm2. These commercially available membranes are usually prepared from polycarbonate or polyester.
Preferably, porous anodic alumina membranes are used in the methods of the present invention because of their high pore density, parallel and straight channels, distribution of cylindrical pores of highly uniform diameter arranged in a hexagonal array, and size tunability of ca. 5 to 300 nm. Moreover, these membranes are thermally and mechanically stable, with pore densities as high as 1011 pores/cm2 readily achievable. (Schmid, G., J. Mater. Chem., 2002, 12, 1231; Mallouk, T. E., Science, 2001, 291, 443; and Hulteen et al., J. Mater. Chem., 1997, 7, 1075 are incorporated herein by reference.)
Uses of the Nanostructures
The nanostructures of the present invention have diverse applications including being building blocks of functional nanoscale devices.
For example, nanostructures with the formula of ABO4 have a wide range of uses. For instance, barium tungstate, BaWO4 (also called barite), nanostructures are suitable for use in the electro-optical industry due to their emission of blue luminescence, ascribed to the influence of the Jahn-Teller effect on the degenerated excited state of the (WO4)2− tetrahedral structure. In addition, their thermoluminescence and stimulated Raman scattering (SRS) properties allow BaWO4 nanostructures to be used in solid-state lasers that can emit radiation within a specific spectral region. As such, these nanostructures are suitable for medical laser treatment applications, up-conversion fiber lasers, and analogous spectroscopic functions.
Additionally, barium chromate, BaCrO4 (also called hashemite), nanostructures are suitable for use as oxidizing agents and as catalysts for enhancing vapor-phase oxidation reactions. Moreover, due to their excellent photophysical and photocatalytic properties, such nanostructures are highly efficient photocatalysts, with a particularly marked response to visible light irradiation (Yin et al., Chem. Phys. Lett., 2003, 378, 24).
Fluorides have wide applications in optics, as windows, biological labels, and lenses, as well as components of insulators, gate dielectrics, wide-gap insulating overlayers, and buffer layers in semiconductor-on-insulator structures. In addition, fluorides, doped with rare-earth ions such as Eu+3, Nd+3, and Ho+3, display unique luminescence properties with correspondingly useful applications in diagnostics, lasing, solid state light emitters, light amplification, optical telecommunication, and upconversion. Nanoscale fluorides can be used in technological applications including as high-density optical storage devices, nanosensors, and color displays.
Nanostructures with formula DEF3 have attractive physical properties, such as ferromagnetic, piezoelectric characteristics, and photoluminescence properties. They have wide applications as radiation detection and laser medium, etc. For example, KMnF3 nanostructures have antiferromagnetic properties. At room temperature, they are paramagnet with a cubic perovskite structure, while at 88.3 K they undergo a transition to an antiferromagnetic ordered state.
Nanostructures with formula GF2 have photoluminescence properties, a large optical transmission domain, high resistivity, electron acceptor behavior, or anionic conductivity. These properties are due to the specificity of fluorine as the most electronegative element. These nanostructures are suitable as host materials for optical applications, such as photochemical hole burning or X-ray storage phosphors. These nanostructures are also suitable for medical imaging and high-density optical data storage. For example, magnesium fluoride has been identified as a positive uniaxial crystal, which possesses the highest birefringence and a wide range of transparency in the spectrum region. These properties allow for the use of MgF2 for infrared transparent windows. (Cao et al., Solid State Chem. 2004, 177, 2205).
Materials Preparation. Alumina template membranes (Fisher Scientific) with pore sizes of 100 nm and 200 nm were prepared by a two-step aluminum anodic oxidation process. (See Schmid, G., J. Mater. Chem., 2002, 12, 1231 and Hulteen et al., J. Mater. Chem., 1997, 7, 1075, both incorporated herein by reference.) The membrane was initially hydrated by immersion and sonication in a small volume of distilled, deionized water for a few minutes, so as to avoid air bubble formation within its structure or on its surface. Subsequently, the membrane was mounted between the two halves of a U-tube cell. The half-cells were then filled with equimolar solutions of Ba(NO3)2 and either Na2WO4 or Na2CrO4 solutions to generate barium tungstate and chromate, respectively. After immersion times of up to 12 hours at room temperature, the alumina template, into which the precursors had presumably diffused resulting in product formation, was detached and thoroughly washed with deionized water. The alumina membrane was subsequently dissolved by immersion in 1 M NaOH for about 30 min.
The nanorods, which were characterized by means of X-ray diffraction (XRD), scanning electron microscopy (SEM), transmission electron microscopy (TEM), high resolution TEM (HRTEM), selected area electron diffraction (SAED), energy dispersive X-ray spectroscopy (EDS), Raman and FT-IR analyses, were collected by centrifugation. These were then washed with deionized water until the pH of the product suspensions attained approximately a value of 7. To prepare SEM samples of the corresponding BaWO4 and BaCrO4 nanorod arrays, a previously developed procedure was utilized. (See Lakshmi et al., Chem. Mater., 1997, 9, 857, incorporated herein by reference.) Briefly, alumina membranes containing BaWO4 and BaCrO4 nanorods were glued (using Epoxy resin) to a piece of paper towel. Resulting composites were immersed into a 1 M NaOH aqueous solution for ˜0.5 hour to dissolve the alumina. After washing steps with distilled, deionized water followed by air-drying, samples were subsequently mounted onto SEM stubs for imaging.
Materials Characterization. Products were characterized by a number of different methodologies, including XRD, SEM, TEM, HRTEM, SAED, and EDS as well as with Raman and FT-IR spectroscopies.
X-ray Diffraction. Crystallographic and purity information on the as-prepared barium tungstate and barium chromate nanostructure samples were obtained using powder XRD. To generate these samples, the as-prepared BaWO4 and BaCrO4 products, upon centrifugation, were subsequently sonicated for about 1 min, and later air-dried upon deposition onto glass slides. The diffraction patterns were collected using a Scintag diffractometer, operating in the Bragg configuration using Cu Kα radiation (λ=1.54 Å) from 10 to 80° at a scanning rate of 2° per minute.
Electron Microscopy. The size and morphology of the resulting BaWO4 and BaCrO4 products were initially characterized using a field emission SEM (FE-SEM Leo 1550) at accelerating voltages of 15 kV. Specifically, solid BaWO4 and BaCrO4 samples of isolated nanorods and their associated arrays immobilized onto Epoxy resin were mounted onto conductive carbon tapes, which were attached to the surfaces of SEM brass stubs. These samples were then conductively coated with gold by sputtering for 15 seconds to minimize charging effects under SEM imaging.
Low magnification TEM images were taken at an accelerating voltage of 120 kV on a Philip CM12 instrument, equipped with EDS capabilities. HRTEM images and SAED patterns as well as EDS data were obtained on a JEOL 2010F HRTEM (equipped with an Oxford INCA EDS system and subsequent potential of performing SAED) at an accelerating voltage of 200 kV to further characterize individual BaWO4 and BaCrO4 nanorods. Specimens for all of these TEM studies were prepared by depositing a drop of these aqueous suspension samples onto a 300 mesh Cu grid, coated with a lacey carbon film. Prior to deposition, solutions containing samples of BaWO4 and BaCrO4 nanorods, were sonicated for 2 min to ensure adequate dispersion of the nanorods.
Optical spectroscopy. Samples for Raman spectroscopy were analyzed on a Kaiser micro-Raman instrument, with a 200-micron confocal aperture, at a laser excitation of 752.5 nm using a power level of 5 mW. Infrared spectra were obtained, using a ThermoNicolet Nexus 670 using a ZnSe single reflectance ATR accessory.
Results
X-ray Diffraction
As-prepared BaWO4 and BaCrO4 nanorod samples were examined by powder XRD measurements on a Scintag diffractometer with Cu Kα radiation (
Electron Microscopy
The morphology of the as-synthesized BaWO4 and BaCrO4 nanorod samples was obtained using FE-SEM and low magnification TEM. Typical SEM and TEM images of BaWO4 nanorods are depicted in
To provide further insight into the structure of the as-prepared BaWO4 and BaCrO4 nanostructures, individual nanorods were analyzed by HRTEM as well as using SAED and EDS. An image of a randomly chosen single BaWO4 nanorod is shown in
Additional selected area electron diffraction patterns, associated with
To investigate the thermal stability of the as-prepared nanorods, samples of BaWO4 and BaCrO4 nanorods were further heated in air for 5 h at 650° C.
Optical Spectroscopy
Optical properties of the synthesized nanorods were also investigated.
In the FT-IR spectra (
Considering the imperfect correlation between the IR spectra of the bulk solid (
The results of Raman and IR data further corroborate the other data collected, confirming the identity of the as-prepared nanomaterials as indeed BaWO4 and BaCrO4, respectively. The generation of these materials provides the basis for a more thorough future investigation of their novel optical, optoelectronic, and catalytic properties for possible incorporation into nanoscale devices. The lasing and photocatalytic properties of these materials is particularly important.
Mao et al. “General, Room-Temperature Method for the Synthesis of Isolated as Well as Arrays of Single-Crystalline ABO4-Type Nanorods,” J. Am. Chem. Soc. 2004 126:15245-52 is incorporated herein by reference in its entirety.
Materials Preparation
Commercially available polycarbonate membranes (Whatman Co., UK) used in this study contain pore sizes of 50, 100, and 200 nm diameter, respectively, with a thickness of ˜6 μm. These polycarbonate filters contain track-etched channels. Pores were randomly distributed across the filter membranes, and pore densities were quoted as approaching 3×108 pores c−2. In order to avoid air bubble formation on their surface, the membranes were pre-hydrated by immersion and sonication in a small volume of distilled, deionized water for a few minutes. Subsequently, the membrane was placed between the two arms of a U-shaped tube (
In the typical synthesis, each half cell was filled with a solution of 0.25 M NH4F and either 0.125 mM CaCl2, SrCl2, or Ba(NO3)2 solutions to generate calcium fluoride, strontium fluoride and barium fluoride nanowires, respectively. After immersion times of up to 12 hours at room temperature, the polycarbonate membrane was detached and thoroughly washed with deionized water and subsequently dissolved in the presence of methylene chloride. Upon washing, alkaline earth metal fluoride nanowires were collected by centrifugation.
To limit unwanted particle formation and deposition onto the exterior of the polycarbonate templates, the nanowire products were selectively fabricated within the inner pores only. To this end, microcontact printed octadecyltetrachlorosilane (OTS) self-assembled monolayers as passivation layers on the external surfaces of polycarbonate membranes were used. (A. Kumar et al. Appl. Phys. Lett. 1993, 63, 2002.) Hence, prior to mounting of the polymeric membrane templates between the two halves of the U-shaped tube, both sides of the polycarbonate membranes were gently pressed with a homemade polydimethylsiloxane (PDMS) stamp, which had been initially inked with a 10 mM hexane solution of OTS and subsequently dried with nitrogen.
Materials Characterization
To prepare powder XRD samples, the resulting alkaline earth metal fluoride nanowires were rendered into slurries in ethanol, sonicated for about 1 min, and then air-dried with deposition onto glass slides. Diffraction patterns were collected using a Scintag diffractometer, operating in the Bragg configuration using Cu Ka radiation (λ=1.54 Å) from 10 to 80° at a scanning rate of 4° per minute.
The size and morphology of the resulting alkaline earth metal fluoride nanowires were initially characterized using a field emission SEM (FE-SEM Leo 1550), operating at accelerating voltages of 15 kV. Specifically, samples for SEM were prepared by dispersing as-prepared products in ethanol, sonicating for about 2 min, and ultimately deposited onto a conductive carbon tape, attached to the surface of a SEM brass stub. All samples were subsequently conductively coated with gold by sputtering for 15 s to minimize charging effects under SEM imaging conditions.
Both TEM and HRTEM images of fluoride nanowires were obtained on a JEOL 2010F instrument at accelerating voltages of 200 kV. It was equipped with an Oxford INCA EDS spectroscopy system with the potential of performing SAED. Specimens for all of these TEM experiments were prepared by dispersing a small quantity of as-prepared product in ethanol, sonicating for 2 min to ensure adequate dispersion of the nanowires, and ultimately evaporating one drop of the solution onto a 300 mesh Cu grid, coated with a lacey carbon film.
Alkaline metal earth nanowires, doped with Eu(III) and Tb(III), respectively, were prepared by adding either Eu or Tb salt (nitrate or chloride) at concentrations up to 8.0 atom percent into the appropriate U-tube half-cell, containing CaCl2/SrCl2/Ba(NO3)2 solution. Samples for photoluminescence (PL) spectra were dispersed in deionized water and sonicated for 1 min. A similar protocol was employed for the preparation of bulk samples by directly mixing all of the precursor solutions, with the exception that no U-tube apparatus was used. Fluorescence data were obtained at room temperature on a Jobin Yvon Spex Fluorolog 3 with a 10 s integration time. PL spectra for Eu3+ and Tb3+ were taken using excitation wavelengths of 365 and 350 nm, respectively.
Results and Discussion
The purity and crystallinity of as-prepared alkaline earth metal fluoride samples were characterized by powder X-ray diffraction (XRD).
The size and morphology of as-synthesized alkaline earth metal fluoride nanowires were initially examined by field-emission scanning electron microscopy (FE-SEM) and transmission electron microscopy (TEM). Typical SEM and TEM images, as shown in
It is noteworthy that SEM and TEM images were obtained from randomly selected areas of the sample, and as such, are representative of the overall sizes and shapes of the as-generated alkaline earth metal fluoride nanowires. Moreover, energy-dispersive X-ray spectroscopy (EDS) data, taken during SEM analysis, revealed signals associated with either Ca, Sr or Ba as well as F, e.g. elemental signatures (
All of the data presented suggest that as-prepared alkaline earth metal fluoride nanowires are monodisperse with controllable morphology. In other words, the ambient synthesis of straight, crystalline wire-like structures is possible using a modified template-directed method without the need for sophisticated experimental setups. Moreover, the shapes and sizes of these fluoride nanowires accurately replicated the interior pore structure as well as the pore lengths and diameters of the polycarbonate templates from whence they were generated. Whereas nanowires with expected lengths of several microns were routinely noted, shorter fluoride nanowires were also observed from TEM images; the latter could be attributed to localized fracturing, occurring during the sonication step employed prior to preparation of TEM samples.
To provide additional details about the crystallographic structure and chemical composition of as-prepared fluoride nanostructures, individual fluoride nanowires were investigated by high-resolution TEM (HRTEM), selected area electron diffraction (SAED), as well as energy dispersive X-ray spectroscopy (EDS).
The corresponding structural and chemical analyses from HRTEM data of as-prepared SrF2 and BaF2 nanowires are shown in
The key to the fabrication technique (
As previously mentioned, bulk alkaline earth metal fluoride crystals doped with rare earth metal ions display unique luminescence properties.(L. F. Johnson, et al. Appl. Phys. Lett. 1971, 19, 44; X. X. Zhang, et al. Phys. Rev. B 1995, 51, 9298; and P. Xie, et al. Opt. Lett. 1992, 17, 1198.) As a demonstration of principle, as-prepared alkaline earth metal fluoride nanowire samples, doped with either Eu3+ and Tb3+, displayed either pink or green luminescence, respectively, under UV lamp excitation (
The present invention enables the synthesis of a family of single-crystalline alkaline earth metal fluoride nanowires (in addition to their rare-earth ion-doped analogues) of varying controllable sizes using a modified template-directed methodology. It is noteworthy that single-crystalline, alkaline earth metal fluoride nanowires can be produced very readily using this modified, room-temperature, template-assisted method, without the use of either sophisticated experimental setups or high-temperature annealing. Moreover, the diameters of the as-fabricated nanowires could be controlled by choosing polycarbonate membranes with predictable pore sizes. Resulting nanowires have been extensively characterized by microscopy and spectroscopy data. The approach is quite general and can be applied to the synthesis of other important nanomaterials, including but not limited to SrWO4, BaMoO4, ZnWO4, BaSO4, and BaIO4 as well as Ba1−xSrxWO4. The luminescent properties of as-doped metal fluoride nanowires provide the basis for a more thorough investigation of their optical and optoelectronic properties for possible incorporation into nanoscale devices.
Although preferred embodiments of the present invention have been described herein with reference to the accompanying drawings, it is to be understood that the invention is not limited to those precise embodiments and that various other changes and modifications may be effected herein by one skilled in the art without departing from the scope or spirit of the invention, and that it is intended to claim all such changes and modifications that fall within the scope of the invention.
This application claims the benefit of U.S. Provisional Application No. 60/733,010, filed Nov. 2, 2005, which is incorporated herein by reference in its entirety.
This invention was made with support by the US Department of Energy under contract number DE-AC02-98CH10886 and the National Science Foundation under CAREER award DMR-0348239. The Government has certain rights in this invention.
Number | Date | Country | |
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20070113779 A1 | May 2007 | US |
Number | Date | Country | |
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60733010 | Nov 2005 | US |