The present invention is directed to a synthetic biomaterial compound based on stabilized calcium phosphates and more particularly to the molecular, structural and physical characterization of this compound. The compound comprises calcium, oxygen and phosphorous, wherein at least one of the elements is substituted with an element having an ionic radius of approximately 0.1 to 1.1 Å. The knowledge of the specific molecular and chemical properties of the compound allows for the development of several uses of the compound in various bone-related clinical conditions.
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1. An isolated bioresorbable biomaterial compound comprising calcium, oxygen and phosphorous, wherein a portion of at least one of said elements is substituted with an element having an ionic radius of approximately 0.1 to 0.6 Å Si4+, wherein said compound has a microporous structure.
15. A biomaterial compound comprising calcium, oxygen and phosphorous, wherein at least one of said elements is substituted with an element having an ionic radius of approximately 0.1 to 1.1 Å and wherein said compound is selected from the group consisting of Ca3(P0.750Si0.25O3.875)2 and Ca3(P0.9375Si0.0625O3.96875)2.
18. A biomaterial compound having the formula:
(Ca)i{(P1-x-y-zBxCyDz)Oj}2 wherein B, C and D are selected from those elements having an ionic radius of approximately 0.1 to 0.4 Å and selected from the group consisting of silicon and boron;
x is greater than or equal to zero but less than 1;
y is greater than or equal to zero but less than 1;
z is greater than or equal to zero but less than 1;
x+y+z is greater than zero but less than 1;
i is greater than or equal to 2 but less than or equal to 4; and
j is equal to 4-δ, where δ is greater than or equal to zero but less than or equal to 1.
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6. The biomaterial compound as claimed in claim 5 1 wherein said compound is formed as a macroporous structure comprising an open cell construction with interconnected voids having a pore size of approximately 50 to 1000 microns.
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8. The biomaterial compound as claimed in
9. The biomaterial compound as claimed in claims 1, wherein said compound exhibits monoclinic pseudo-rhombic symmetry and is in the monoclinic space group P21/a.
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This application is a continuation-in-part of copending U.S. patent application Ser. No. 09/029,872, filed
Since the conversion of HA into TCP results in the simultaneous formation of CaO and release of H2O, changes in the activity of both CaO and H2O should modify the location of the phase boundaries. The upper diagonal lines show the phase boundary when the activity of CaO is made progressively smaller. This effect can be practically accomplished by chemical combination of CaO with other compounds such as Sio2. In the presence of silica (SiO2), the resultant compound could be one or more of several calcium silicates. The calculations show that the decomposition boundaries in the temperature range of 800-1100° C. are in approximate agreement if CaO has the activity expected when the CaO is combined with SiO2 as follows in equation (3):
CaO+SiO2⇄CaSiO2 (3)
The most stable phosphorous-containing conversion product is, however, β-TCP. This is consistent with the widespread observation of the magnesium doped HA-based mineral whitlockite as the natural form of β-Ca3(PO4)2 (Schroeder, L., B. Dickens and W. Brown. J Solid State Chem 22 1977; pp. 253-62). On the basis of the information available within the FACT database it is not possible to explain the observation of a phase similar to α-TCP as a conversion product below 1000° C. other than to assume that β-TCP is not nucleated when CaSiO3 forms and that Si-TCP develops as a metastable allotropic form.
It may be noted that on the basis of chemical thermodynamics, any reaction which changes the activity of CaO should modify the phase diagram. Oxides such as TiO2 have only one product with CaO as in equation (4):
CaO+TiO2⇄CaTiO3 (4)
and may therefore be more predictable in their action. Similar calculations to those for Si showed that for a similar partial pressure of water, the phase boundary for Ti was located at a slightly lower temperature.
The XRD pattern for powders prepared using Ti as the additive also showed that conversion occurs upon addition of the Ti. However, the results were more complex as the predominant phase of TCP formed was β-TCP (
The simplest interpretation of the differences between the effects of Si and Ti additives is based on the observation of the effects of additive precipitation and the changes observed in degree of conversion following powder grinding and pellet formation. In the case of Si-based additions, the degree of precipitation was essentially independent of the carrier and relatively minor changes in the degree of conversion occurred on formation into ceramic pellets. In contrast, Ti additions were ineffective when precipitation occurred when the additive was introduced into the Ca—P colloidal suspension (for no carrier and 2Me). Ti additions were effective when precipitation did not occur (for ACAC) and conversion became stronger upon grinding of the powder to form pellets and subsequent resintering. This suggests that the conversion from HA to TCP requires intimate contact between the additive and HA, possibly through surface functionalization of the precipitated mHA particles within the colloid suspension by the additive species or adsorption of the additive species on the surface of the mHA particle. When the additive and the mHA precipitate as separate species, the conversion occurs only upon strong physical inter-mixing and thermal treatment.
For comparative purposes, reference materials were prepared by equivalent thermal processing of commercially available powders (see Table 1) in an attempt to produce ceramics with a similar phase composition and surface morphology. Commercial powders were processed as pure compounds and in combination with selective additives introduced either as inorganic powders or as metallorganic species in a carrier. XRD results indicate that conversion of commercial HA (cHA) does take place, but that the primary resultant phase is β-TCP. The typical phase distribution is 73% β-TCP, 20% α-TCP and 7% HA. These results are consistent with the phase composition predicted by thermodynamics as noted in equations (2) and (3) and illustrated in FIG. 8. Of equal significance is that the surface morphology of the ceramics prepared from these powders exhibits a jagged or fractured morphology (
The solid state chemistry of the cHA powders with introduced additives suggest that the conversion behaviour as a function of temperature, humidity and additive is consistent with equations (2)-(4). In particular, if physical mixing of the additive into the cHA powders takes place the β-TCP phase predicted by chemical thermodynamics is observed. In comparison, if intimate mixing of an unprecipitated silicon additive and a Ca—P colloid occurs the resultant phase is Si-TCP. This phase is not consistent with the predictions of equilibrium thermodynamics, but it is closely linked with the presence of Si in the Ca—P lattice. In order to use the FACT database to predict the phase boundaries for transitions to this Skelite™ compound, new values for the Gibbs free energy will be required.
The origin of the Skelite™ compound and confirmation of the mechanism of formation was investigated using techniques which assess the location of the additive within the HA or TCP strictures, in an attempt to observe the presence of the reaction products predicted by equations (3) and (4).
Significantly, no calcium silicate peaks were identifiable in XRD spectra taken on either colloidal-based or mixed powder compositions where Si was the selected additive. This suggests that Si forms a dispersed or substituted phase within the phosphate lattice. Previous workers (Dickens, B. and W. Brown. Acta Cryst B28 1972; pp. 3056-65 and Nurse, R., J. Welch and W. Gutt. J Chem Soc 1959; pp. 1077-83 have suggested that calcium silicate and β-TCP form a miscible solid solution at high temperatures (>1350° C.) over the composition range of interest. The XRD spectra reported in these earlier experiments did not match that of α-TCP or the Skelite™ presently described, thus demonstrating the uniqueness of this compound. In this work, when commercially available CaSiO3 was physically mixed with cHA or β-TCP powders (Table 1) and then sintered for 8 hr in alumina crucibles in air at 1250° C., the results showed that CaSiO3 nucleates a crystallographic phase consistent with the Skelite™ compound (Si-TCP) (FIG. 15). The degree of conversion to Skelite™ increases as the temperature of the reaction is increased. At 1250° C. and above, depending on the amount of Si present, the powder mixtures show an increasing tendency to form a melt thus eliminating the microporous structure.
Comparison of three major peaks in the XRD spectrum of Skelite™ and α-TCP between 2θCu=30 and 2θCu=31°, assuming a Gaussian theoretical peak shape with a width of 0.225°, shows that there is a shift of approximately 0.1° to lower 2θ in Si-TCP (
Nuclear Magnetic Resonance Studies
Magic-angle NMR studies were carried out on Si-mHA powders. Comparisons were made with simple physical mixtures of cHA, α- and β-TCP, CaSiO3 and SiO2 in proportions similar to the phases present in the Si-mHA powders. For Si-mHA, no Si signals could be observed under any conditions of measurement. Careful comparison with signals measured on CaSiO3 and amorphous SiO2 was used to set the lowest level of sensitivity at which the compounds or local structures could be measured.
Infrared Spectroscopy Studies
In order to assess these changes, IR spectra of CaSiO3, CaO, SiO2 and commercial β-TCP were examined. The CaSiO3 spectrum shows a series of distinctive peaks at 717, 563 and 434 cm−1 that are not apparent anywhere in the spectra for Si-mHA powders. The CaO spectrum has a strong sequence of bands below 463 cm−1 which are also not observed in the Si-mHA spectrum. The SiO2 spectrum shows a very strong, well-resolved peak at 1104 cm−1 characteristic of the Si—O bond. An interpretation of the Si-mHA spectra is that the Si—O bond absorption occurs at lower wave numbers than in the pure SiO2. The apparent shift in the P—O stretch can be explained by the growth of a Si—O peak. It is logical that the Si—O and P—O peaks would occur at similar positions since silicon and phosphorus are located beside each other in the periodic table and have similar ionic radii. The fact that the P—O peak appears to shift further indicates the formation of a new silicon compound, Skelite™.
A structural model for silicon substitution based on the IR analysis is a crystal lattice of TCP-like and HA-like material with molecular dispersion of silicon throughout the lattice. This is consistent with the NMR and XRD results. The narrowing of the P—O peak suggests the existence of a less broad distribution of types of P—O bonds within the structure or an increase in crystallinity compared to the mHA with no introduced additives.
In Vitro Bone Cell Activity Studies
The Skelite™ compound on a substrate may be used to assess the resorptive activity of osteoclasts and monitor the change in this level of resorptive activity either as a result of a disease process or the inclusion, in the culture medium, of an agent such as a drug which would influence, either directly or indirectly, osteoclastic resorptive activity. As provided as a film on a substrate, the compound is also suitable for the culture of active osteoblasts in order to observe and assess the secretion of mineralized matrix thereon. As shown in
The thin film devices may be used as a means of quantifying the resorptive activity of osteoclasts or the formation of mineralized matrix by the activity of osteoblasts. Such activity analysis may occur under continuous real-time monitoring, time-lapse intervals or end-point determination. The steps in establishing bone cell activity are common to each of the above monitoring schedules in that bone cells (either animal or human) are cultured, in specific conditions, on one or more of the thin film devices. The culture period is from several hours to many days and preferably from approximately 2 to 10 days (the optimum time is cell species and protocol dependent), during which time the extent of osteoclast activity may be continuously monitored, periodically monitored, or simply not monitored on an on-going basis in favour of final-end-point determination. FIGS. 11(B) and 22 illustrate osteoclast resorption pits on ceramic pellet and thin film formats of the Si-TCP compound.
Similarly, osteoblast activity may be quantified by measuring the amount of mineralized matrix deposition. As is shown in FIG. 21(a), a quartz disc coated with a stabilized film of the present invention and simultaneously cultured with osteoblasts in the presence of culture medium containing tetracycline, a natural fluorescent material, displays fluorescence indicating the presence of mineralized matrix. In contrast, a stabilized film coated on a quartz substrate in the presence of medium containing tetracycline but no osteoblasts (FIG. 21(b)) shows no fluorescence. As the cells take up tetracycline, it is metabolized and incorporated into the newly formed mineralized matrix. The amount of mineralized matrix is proportional to the measurable fluorescence emitted. This demonstrates that osteoblasts actively secrete mineralized matrix on the stabilized composition.
The Skelite™ Compound
The significant correlations with cell-based bioactivity and resistance to dissolution at normal physiological pH 6.4 to 7.3 are the presence of the additive stabilized compound and the microporous morphology. The morphology is accounted for by the sintering of particles of average size 0.2 to 1.0 μm. The presence of a Si-TCP phase that is essentially insoluble in biological media at low temperature using silicon as the introduced additive is unexpected and is induced by the distribution of Si substituted throughout the structure. Considering that the underlying structure of the particles is the agglomeration of granules of size range of approximately 1 to 20 nm, uniform dispersion of the silicon additive and functionalization of the surface of an individual granule is assured by permeation of the silicon sol throughout the agglomerate. The key aspect of this investigation was the determination that silicon does not induce an α-TCP phase resulting from the decomposition of HA, but rather it creates a Si-TCP phase, a new biomaterial compound, by substitution of silicon at phosphorus sites. The fact that silicon induces a Si-TCP compound can now be explained through the crystallography of the calcium-phosphate system and the defect chemistry associated with silicon substitution into the Ca—P lattice. One skilled in the art would understand that other additives having an ionic radius which is different to that of silicon as described herein, but may still substitute into the Ca—P lattice is also embodied for the compound of the present invention. Therefore the compound is not restricted only to silicon as the additive.
It is important to note that “effective ionic radius” has been selected as the term of reference in these studies (Shannon, R. D., Acta Cryst. A32., 751, (1976). The ionic radius specifications provided herein reflect the effective ionic radius for coordination numbers of 4, 6 or 8. It is apparent to those skilled in the art that “ionic crystal radius” may also be used in the practice of the present invention and thus may be used to define equivalent specifications for the compound and the formula of the compound as described herein. A summary of the effective ionic radius and the ionic crystal radius for various elements is provided in Table 2.
When substituting Si in the HA lattice, the ionic radius of Si4+ (IR=0.26 Å for CN=4) suggests that Si4+ can enter at P5+ (IR=0.17 Å for CN=4) sites within the PO43− tetrahedra although it could also be included at Ca2+ (IR=1.0 Å for CN=6) sites. The lattice strain and compensating defect will be significantly different in the two cases and the effects of covalency will substantially modify the result. A low temperature substitution of Si4+ into P5+ sites creates less strain and accommodates the covalency well. The radius ratio for silicon and oxygen is consistent with that required for the tetrahedral coordination of silicon in an oxygen lattice. Such a substitution requires the formation of a single positively charged defect for charge compensation. An obvious defect is one oxygen vacancy for every two silicon ions, although the energy required to displace oxygen-phosphorous bonds within an already formed PO43− tetrahedron may be substantial. Theoretically, substitution of an ion with an appropriate ionic radius and a valence of ≧3 at Ca2+ sites could also provide charge compensation. Such elements may include Ce, La, Sc, Y and Zr. Restrictions on the use of particular elements may be present due to the particular applications for use as a biomaterial.
In the formation of the Si-TCP compound, compositional analysis suggests that the Ca:P ratio decreases from approximately 1.67 (HA) to 1.5 (TCP). This could be induced by (1) the removal of calcium from the lattice, or (2) the introduction of additional phosphorous or an element that substitutes for phosphorous. A reduction in the calcium content of the lattice could theoretically occur by the formation of calcium silicate distributed within the structure. However, no evidence of calcium silicates as a well defined compound can be found in either the NMR or the IR results. Thus extensive silicon substitution must occur forming a multitude of Si-substituted P—O sites in the lattice.
In the case of Ti4+, the ionic radius of (IR=0.42 Å for CN=4) likely precludes its substitution at P5+ sites and it must therefore enter the crystal at more general interstitial sites within the lattice. Since titanium has been demonstrated to be less effective in modifying the crystal structure to create a stabilized TCP, this suggests that the nucleation of the Si-TCP phase is intimately connected with the substitution of silicon at phosphorous sites. In particular, the observed phase being in fact a Ca—P—Si compound with a crystallographic structure similar but different from α-TCP rather than pure α-TCP, resolves conflicts with respect to the new compound's decreased solubility and the predicted decomposition phase diagram.
The crystallography of the Ca—P phase diagram has been extensively studied and compared (Elliott J. Structure and Chemistry of the Apatites and Other Calcium Orthophosphates New York: Elsevier (1994) in apatites (Elliott, J. Nature Physical Science 230 1971; p. 72), β-TCP (Dickens, B., L. Schroeder and W. Brown. J Solid State Chem 10 1974; pp. 232-48 and Labarther, J., G. Bonel and G. Montel. Ann Chim (Paris) 14th Series 8 1973; pp. 289-301) and α-TCP (Calvo, C. and R. Gopal. Am Miner 60 1975; pp. 120-33). Significant differences have been noted between the structures of α and β-TCP (Elliott J. Structure and Chemistry of the Apatites and Other Calcium Orthophosphates New York: Elsevier (1994) and Calvo, C. and R. Gopal. Am Miner 60 1975; pp. 120-33) and equally significant similarities have been seen between α-TCP, apatites and calcium silico-phosphate compounds via the glaserite structure (Mathew, M., W. Schroeder, B. Dickens and W. Brown. Acta Cryst B33 1977; pp. 1325-33). A primary component of the phosphate lattice is the presence of PO43− tetrahedra, although these structures can vary considerably throughout a complex lattice. For example, in α-TCP the P—O distances vary from 1.516 to 1.568 Å and the O—P—O angles vary from 104.1 to 115.2° (Calvo, C. and R. Gopal. Am Miner 60 1975; pp. 120-33). Substitution of a Si at such sites implies a range of environments for such an additive.
Following Elliott (Keller, L., P. Rey-Fessler. Characterization and Performance of Calcium Phosphate Coatings for Implants edited by E. Horowitz and J. Parr. Philadelphia: ASTM, pp. 54-62 (1994) the space group of HA has three kinds of vertical or columnar symmetry. There are columns of Ca2+ ions spaced by one half of the c-axis parameter along three-fold axes which account for two-fifths of the Ca2+ ions in the structure. These ions are given the designation Ca(1). The Ca2+ ions are linked together by PO4 tetrahedra in which three oxygen atoms come from one column and the fourth comes from an adjacent column. The result is a three-dimensional network of PO4 tetrahedra with enmeshed Ca2+ ions, and channels that contain the residual calcium, Ca(2), and ions such as OH− which make up the HA structure.
The α-TCP structure also comprises columns of Ca2+ and PO43− ions parallel to the c-axis (Elliott, J. Nature Physical Science 230 1971; p. 72). The columns are actually anion-anion columns . . . Ca Ca Ca Ca . . . and cation-anion columns . . . PO4 Ca PO4 □ PO4 Ca PO4 □ PO4 Ca PO4 . . . where □ is a vacancy (Elliott J. Structure and Chemistry of the Apatites and Other Calcium Orthophosphates New York: Elsevier (1994)). The presence of this vacancy may facilitate the creation of O2− vacancies in neighboring PO43− tetrahedra required to accommodate the substitution of Si4+ at P5+ sites. Analogous cation-anion columns occur in glaserite, K3Na(SO4)2, except that the vacancy is occupied by a K+ ion. Strong similarities exist between the glaserite and apatite structures (Dickens, B. and W. Brown. Acta Cryst B28 1972; pp. 3056-65). The apatite structure can be derived from that of α-TCP by replacing cation-cation columns at the corner of the apatite unit cell by anion columns (OH− or F−). The remaining cation columns in α-TCP become the columnar Ca(1) ions in apatite, whilst the PO43− and Ca2+ ions that form the cation-anion columns in α-TCP have approximately the same positions as the PO43− and Ca(2) ions in apatite. Of significance to this analysis is that the glaserite structure is related to silico-camotite Ca5(PO4)2SiO4 (Labarther, J., G. Bonel and G. Montel. Ann Chim (Paris) 14th Series 8 1973; pp. 289-301) and α-Ca2SiO4 (Calvo, C. and R. Gopal. Am Miner 60 1975; pp. 120-33). This is consistent with the report that the system Ca2SiO4—Ca3(PO4)2 forms a continuous series of solid solutions at higher temperatures based on the glaserite structure (Nurse, R., J. Welch and W. Gutt. J Chem Soc 1959; pp. 1077-83).
In contrast, there are no such similarities between the structure of HA and β-TCP. The β-TCP structure is a distortion of the parent lattice, Ba3(VO4)2, with layers perpendicular to the c-axis. There is no columnar relationship between cations in the structure. Because of the size of the Ca2+ ion, there is a reduction in the number of PO4 tetrahedra in the structure compared to that for the parent lattice and a reduction in the number of formula units within the hexagonal unit cell. Two types of Ca sites exist within the β-TCP unit cell: those known as Ca(5) are fully occupied, while a particular set of cation sites known as Ca(4) are only half occupied (Elliott J. Structure and Chemistry of the Apatites and Other Calcium Orthophosphates New York: Elsevier (1994)). Upon doping TCP with Mg2+ (IR=0.72 Å for CN=6) the Mg distributes itself first randomly on the Ca(4) and Ca(5) sites, but subsequently only substitutes at the Ca(5) sites. Because Mg2+ is smaller than Ca2+ (IR=1.0 Å for CN=6) and the original distortion of the Ba3(VO4)2 structure occurred because Ca2+ is smaller than Ba2+ (IR=1.35 Å for CN=6), the β-TCP structure is stabilized with the addition of Mg2+ to form the naturally occurring mineral, whitlockite (Calvo, C. and R. Gopal. Am Miner 60 1975; pp. 120-33). Indeed the addition of Mg to β-TCP at high temperatures tends to stabilize the structure well into the α-TCP range. In the case of the addition of an ion such as Ti4+, the slightly larger ionic radius (IR=0.6 1 Å for CN=6) would suggest that it would also be accommodated by substitution at Ca(5) cation sites with results that are less defined than for Mg2+. Since charge compensating defects are necessary, the stabilization or creation of Ca2+ vacancies on Ca(4) sites would serve this purpose. Therefore substitutional Ti should stabilize the β-phase once TCP has been formed.
A feature of the presently characterized compound is that the Skelite™ structure is only achieved when intimate contact occurs between the precipitate and the additive. When silicon is introduced into already formed and fired powders at relatively low temperatures, the resulting post-sintered phase is predominantly β-TCP. In this case the silicon plays a role similar to that described for titanium above and simply acts to reduce the activity of CaO in the decomposition of HA under the terms of equation (3). In the case of colloidal powders precipitated in close association with an additive such as silicon, both the surface activity will be high and strongly functionalized complexes will be formed in the solution and at the interfaces of the precipitated granules. Through sintering, a range of PO43− and Sio44− tetrahedra will be established along with the necessary oxygen vacancies. In this case, nucleation of the glaserite-based Si/P phase will take place. While previously this was interpreted as a form of α-TCP it is, in fact, an entirely different compound with its own values for solubility and bioactivity (Si-TCP). Thus the crystal phase composition, surface morphology and bulk morphology originates from the chemically active and agglomerated state in which the starting material is precipitated, and the degree to which this state controls the location at which the Si4+ cation is substituted.
Again, although silicon has been the most extensively studied and appears to be the preferred substituted element of the invention, it is apparent to one skilled in the art, that any additive that can enter and distribute throughout the crystal structure of the calcium phosphate lattice and result in the compound of the present invention can be substituted for silicon. Therefore, the present compound is not restricted to only silicon as the substituted element but may also include other suitable elements having a suitable ionic radius of approximately 0.1-0.4 Å such as for example boron. It is also understood that other additives in addition to the silicon or boron may also be present in the compound of the present invention. Such elements may also form part of the Ca—P lattice where such elements and/or the amount of oxygen may act to balance charge compensation for additives incorporated into the compound. Such additives may be selected from the group consisting of Ce, La, Sc, Y, and Zr.
It is also understood by those skilled in the art that the novel compound of the present invention can be combined with a calcium phosphate material such as calcium hydroxyapatite, α-TCP, β-TCP, octocalcium phosphate, tetracalcium phosphate, dicalcium phosphate, calcium oxide and other like materials. The resultant combination can be as a physical mixture or as a solid solution. In addition, other additives such as polymers or microfibers may additionally be added to the compound of the present invention to increase mechanical strength and toughness. The particle size of these additives may be selected such that the additive may be removed through phagocytosis by the action of macrophages. Metals may also be present in combination with the present compound to form composite structures. Such structures are also intended to be embodied in the present invention.
The Skelite™ Morphology
The morphology of the synthetic stabilized calcium phosphate compound (Skelite™) is unique and has not been previously reported or demonstrated. We have now demonstrated a morphology presenting an interconnected globular structure of rounded particles having an interconnected microporosity. In accordance with a preferred aspect of this invention, the morphology successfully supports cultures of functional osteoclasts and osteoblasts.
The surface morphology of the coating has a characteristic form involving a interconnected globular structure (FIG. 6a). The size of the particles varies from approximately 0.2-1 μm in lateral dimension. This morphology may allow for the percolation of liquid media and other physiological fluids within the coating. In contrast, the surface morphology of hydroxyapatite prepared from other methods, does not result in a structure as provided by the present invention. In addition, is has been reported that synthetic polycrystalline hydroxyapatite is not resorbed by osteoclasts (Shimizu, Bone and Minerology, Vol. 6, 1989).
The globular morphology is made up of rounded particles comparable in size to the aggregated deposits initially made by an osteoblast cell in the process which leads to bone formation. The present composition provides a morphology compatible with the type of morphology bone cells encounter in vivo. Particularly, the size and shape of the cell/compound interface facilitates bone cell attachment. Such attachment is a necessary precursor to normal bone cell activity.
The bulk microporosity of the synthetic stabilized calcium phosphate compound may ensure that the calcium or phosphate ion concentrations near the surface of the artificial material are within the limits expected by the cell as encountered in vivo with natural bone which is made up of hydroxyapatite, collagen and other fibrous tissues. During osteoclast mediated extracellular dissolution processes which lead to resorption, this complex material leads to a particular local concentration of dissolution products.
The bioactive synthetic biomaterial compound of the present invention provides a unique chemical composition together with a unique morphology and internal microporous structure that has never previously been demonstrated. Compositions have not been previously reported which demonstrate consistent bone cell bioactivity in vivo and in vitro in which bioactivity in vitro can be readily, accurately and repetitively quantified. The nature of the stabilized biomaterial compound is versatile in that it can be provided in a fine or coarse powder, pellets, three-dimensional shaped pieces, macroporous structures, thin films and coatings. In each case, the unique morphology and internal microporosity is maintained as well as the stabilized calcium phosphate composition.
In summary, a new calcium phosphate-based biomaterial compound has been created and specifically characterized. This new biomaterial exhibits two prominent features:
It is now revealed via numerous difficult analytical tests and complex data interpretation that this stabilized calcium phosphate compound is a novel additive stabilized structure referred to as Skelite™ that may exist in combination with HA, α-TCP, β-TCP or other suitable calcium phosphate phases. This new compound has been characterized to have the formula, (Ca1-wAw)i[(P1-x-y-zBxCyDzOj)]2, wherein A is selected from those elements having an ionic radius of approximately 0.4 to 1.1 Å; B, C and D are selected from those elements having an ionic radius of approximately 0.1 to 0.4 Å; w is greater than or equal to zero but less than 1; x is greater than or equal to zero but less than 1; y is greater than or equal to zero but less than 1; z is greater than or equal to zero but less than 1; x+y+z is greater than zero but less than 1; i is greater than or equal to 2 but less than or equal to 4; and j equals 4-δ, where δ is greater than or equal to zero but less than or equal to 1. The terms w and δ may be selected to provide charge compensation of the elements present in the compound.
An important processing step involves the intimate mixing of silicon as a candidate additive with the particles of the colloidal suspension to ensure the local availability of reactants. This in combination with the similarity of the silicon and phosphorous ionic radii, creates an environment favorable for silicon substitution at phosphorous sites within the Ca—P lattice and the development of the silicon-stabilized TCP structure.
The unique composition does not occur in the absence of intimate mixing as the effect of added silicon in these circumstances is only to influence the activity of CaO as an HA decomposition product. Similarly, the use of additives comprised of larger ions, such as titanium, cannot be accommodated in the lattice at phosphorous sites thereby precluding the important phosphate substitution phenomenon. In both of these cases, the resulting product is predictably β-TCP.
In view of the ability of Skelite™ to participate in the natural bone remodeling process, significant opportunities exist for the development of synthetic bone grafts and bone repair products that are indeed bioactive.
Synthetic Bone Graft Applications
A synthetic bone graft that comprises in whole or in part the novel compound of the present invention has numerous applications in the orthopedic industry. In particular, there are applications in the fields of trauma repair, spinal fusion, reconstructive surgery, maxillo-facial surgery and dental surgery.
The gold standard in the industry for treating traumatized bone is an autologous bone graft, commonly referred to as an autograft. Autograft transplants involve a surgical procedure in which healthy bone is taken from an alternate part of the patient's skeleton to repair areas of skeletal trauma. Autografts however, require double surgical procedures; one for graft removal and a second for re-implantation at the damaged site. This makes the procedure very expensive and time consuming. Additionally, it is not uncommon for patients to subsequently suffer chronic pain at the autograft harvest site.
Another widely used bone graft technique is the use of allograft, a term referring to a tissue graft from another individual or animal. In this situation, bone is removed from the donor and implanted in the patient. Allografts are susceptible to various negative consequences. For example, the use of allograft from an animal other than a human carries the possibilities of cross species infection and immunological rejection. Even human sourced allograft, which is used more often than animal tissue, exposes the implant recipient to the possibilities of rejection and disease.
The use of Skelite™ eliminates the pain and costs associated with the bone harvest procedure required in autograft transplants. Furthermore, since Skelite™ is generated in a laboratory and is completely synthetic, it removes the possibility of transmission of infection and disease, as well as eliminates sources of immunological rejection by the patient.
Skelite™ fulfils the need for a versatile bone reconstruction material. Its ability to immediately stimulate local natural bone growth provides stability and rapid integration, while the body's normal cell-based bone remodeling process slowly resorbs and replaces the implant with natural bone. This removes the concerns of long term compatibility and durability associated with current artificial implant technologies.
Products formed from Skelite™ will involve different configurations in order to address the requirements of particular applications. For example, Skelite™-based products can be manufactured as a fine or coarse powder, pellets, shaped three dimensional pieces, macroporous structures, thin films and coatings. In addition, these products could potentially carry an integrated bone growth factor to speed short term recovery.
The use of Skelite™ in a macroporous configuration allows the open porous structure to serve as a scaffold for the integration of new bone tissue. The macroporous structure is formed by the coating of the compound onto a reticulated polymer and subsequently removing the polymer through pyrolysis. The macroporous structure comprises an open cell construction with interconnected voids having a pore size of approximately 50 to 1000 micron. Due to this design, Skelite™ is the ideal bone substitute for implantation at defect sites where special measures are required to encourage new bone growth to bridge areas of major tissue loss due to trauma or surgical intervention. The Applicant has identified two primary approaches for the clinical use of such a product: direct implantation and tissue engineering.
Direct Implantation
The simplest approach is to directly implant the Skelite™ scaffold at the location of skeletal trauma where the bioactive properties of the biomaterial compound stimulate the body's natural bone repair mechanism. Once the initial healing process is complete, the Skelite™ scaffold is progressively replaced with natural bone as part of the body's orderly remodeling process.
Hybrid versions of Skelite™-based products are possible where bone growth factors are incorporated into the scaffold as a post-manufacturing process or at the time of surgery. The availability of the growth factor at the repair site increases the rate of new bone formation thereby improving patient recovery time and lowering overall health care costs.
Tissue Engineering
The concept that underlies the tissue engineering application is to remove bone cells from the patient's skeleton using an established bone marrow aspiration technique, and then carefully introduce the collected cells (cell seeding) into the open cell structure of the Skelite™ scaffold in a sterile biotechnology facility. The cells and scaffold are then incubated so that the cells have an opportunity to multiply and begin to fill the scaffold with new mineralized matrix. After several weeks, the biological implant is ready for implantation back into the patient. This biotechnology bone growth process is termed “tissue engineering”, and the procedure serves to enhance the ability of surgeons to reconstruct severely compromised areas of the skeleton. Once successfully integrated at the repair site, the Skelite™ implant is subsequently remodeled into natural bone by the ongoing activity of bone cells.
A refinement of this approach is to selectively extract and multiply in cell culture only special precursor cells termed Mesenchymal Stem Cells (MSCs). In order for these cells to remain healthy during biological processing, they need to be attached to a suitable physical carrier. In addition, the performance of the cells can benefit from the addition of organic bone growth factors. Skelite™ is a suitable carrier since it allows for both the integration of bone growth factors and the attachment of specialized MSCs. In addition, following implantation and patient recovery, the Skelite™ scaffold is subsequently remodeled into natural bone.
The use of Skelite™ in direct implantation or tissue engineering applications has important advantages over the use of naturally sourced bone graft material, and consequently Skelite™ products have the potential to replace the autograft procedure as the orthopedic surgeon's preferred treatment strategy.
The key advantages of implantable products formed from the Skelite™ material are:
The Skelite™ biomaterial may also be used for the incorporation of selected pharmaceuticals into the compound for the further enhancement of the bone healing and remodeling processes. In this respect, pharmaceuticals that have been incorporated into the Skelite™-based products can be predictably released at the site of implantation and hence become available to assist in the bone regeneration process. The Skelite™ biomaterial may also be designed as a slow release vehicle for appropriate pharmaceutical compounds.
Primary candidates for incorporation into Skelite™-based products are selected bone growth factors. These proteins have been identified as being critically important in growing and maintaining healthy bone tissue. In particular, when applied at the site of traumatized bone, natural bone growth is enhanced with a corresponding improvement in overall therapeutic response. However, a compatible carrier system is required to deliver such therapeutic biologicals to the site and ensure local release of appropriate concentrations of the drug. Implant studies have shown that products formed from the Skelite™ biomaterial are suitable for use as drug carriers. One skilled in the art would understand that other pharmaceuticals such as antibiotics for example which may aid in the bone healing process may also be incorporated into the Skelite™ compound.
Coating Applications
Through a liquid application process, the Skelite™ material can be coated on to orthopedic and dental implants to improve and promote natural bone fixation and to improve long term implant stability. Such a coating of approximately 0.1 to 10 μm acts at the interface with the patient's own tissue to promote natural bone growth during the weeks immediately following surgery, and is then progressively replaced by the ongoing activity of bone cells once the initial healing process is complete. The result is a strong union between the implant and the host bone. This is not the case with conventional calcium phosphate implant coatings where the biologically inert coating is subject to mechanical detachment (delamination) from the metal substrate, causing potentially catastrophic implant failure.
The key advantages of an implant coating formed from the Skelite™ material are:
As a thin film as provided on a suitable substrate, the Skelite™ compound significantly advances the study and understanding of bone cell functional properties. The composition and morphology of the stabilized film, as provided in accordance with this invention, permits the culture of various types of bone cells thereon. The properties of the film may be adjusted to encourage a significant degree of resorption of the Si-TCP compound of the film material through to a negligible degree of resorption of the Si-TCP compound in the study of osteoclast activity. Similarly, osteoblast activity may be studied by detecting the deposition of mineralized matrix. The ability to provide the material in a film format which is sufficiently thin that resorption of the Si-TCP compound by osteoclasts can be detected provides a simple inexpensive format for analysis compared to the prior art techniques. The film as made in accordance with this invention, supports the biological function of bone cells. The benefit in providing the film on a transparent supporting substrate, such as quartz or glass, lends to easy evaluation techniques of the diagnostic process including automated machine reading.
Ideally the film thickness is greater than 0.1 micron because it has been found that at film thicknesses less than 0.1 microns it is difficult to obtain uniform film coverage, free from discrete voids. As to the upper thickness limit for the film, it can be of any desired thickness depending upon its end use. The degree of resorption may be detected by light transmittance, which preferably requires a film less than 10 microns in thickness. The substrate is of quartz which readily withstands the required sintering temperatures and has the desired degree of transparency to permit light transmittance tests to determine the extent of resorption of the film material.
The developed thin films may be used in kits and analytical products to provide for assessment of bone cell activity. The film may be embodied in the form of a kit or device comprising quartz substrates, pre-coated with the stabilized calcium phosphate (Si-TCP) compound, which may be used in a cell culture vessel (possibly a 24-well optionally sterilized multi-well plate i.e. of approximately 15 mm diameter) as a system suitable for the culture of mixed bone cell populations. The device is simple and relies on only routine laboratory equipment and techniques for use, is suitable for quantitative analysis, and is inexpensive to fabricate but strong enough to withstand normal levels of handling and may be packaged in lots, of (for example) 24 samples in a plastic multiwell plate. The thin film surfaces have a defined and reproducible chemistry and are mechanically strong enough to withstand transport when used with an appropriate packing material.
In each case the culture conditions may be such that osteoclasts, in either mononuclear or multinucleate form could be expected to survive in a functional state and resorb the synthetic stabilized calcium phosphate compound. Similarly, osteoblasts are also capable of actively secreting mineralized matrix under such culture conditions.
Once the colloidal suspension (sol-gel) is prepared, it may be applied as a thin film to the desired substrate in a variety of techniques. For example, the dip-coating method (C. J. Brinker et al., Fundamentals of Sol-Gel Dip Coating, Thin Solid Films, Vol. 201, No. 1, 97-108, 1991) consists of a series of processes: withdrawal of the substrate from a sol-gel or solution at a constant speed, drying the coated liquid film at a suitable temperature, and firing the film to a final ceramic.
In spin-coating the sol-gel is dropped on a plate which is rotating at a speed sufficient to distribute the solution uniformly by centrifugal action. Subsequent treatments are the same as those of dip coating.
It is appreciated that there are a variety of other techniques which may be used to apply a thin film of the sol-gel to the substrate. Other techniques include a spraying of the sol-gel, roller application of the sol-gel, spreading of the sol-gel and painting of the sol-gel.
An alternative to coating discrete discs of a singular size is to coat an enlarged substrate with a film of the sol-gel. The entire film on the substrate is then sintered. A device, such as a grid, may then be applied over the film to divide it into a plurality of discrete test zones.
In these various techniques of the sol-gel substance application, the thickness and quality (porosity, microstructure, crystalline state and uniformity) of formed films are affected by many factors. These include the physical properties, composition and concentration of the starting sol, the cleanliness of the substrate surface, withdrawal speed of the substrate and the firing temperature. In general the thickness depends mainly on the withdrawal rate and sol viscosity for a dip coating process. Since heterogeneity in the sol-gel is responsible for the formation of voids, the coating operation should be undertaken in a clean room to avoid particulate contamination of the sol. At the heat-treatment stage, high temperatures are required to develop the required microstructure and desired conversion of hydroxyapatite into the biomaterial (Skelite™) compound.
The purpose of applying the dip coating method to fabricate calcium phosphate films is twofold: (a) to make films with required qualities (uniformity, thickness, porosity, etc.); and (b) to make translucent Si-TCP films on transparent substrates for biological experiments.
Macroporous Structures
A particular aspect of ceramic preparation for use in biological applications is the fabrication of ceramic pieces with a globular morphology and internal microporosity which leads to bioactivity, and a larger internal macrostructure of pores of dimensions 50-1000 μm. This encourages bone growth and subsequent remodeling in a system more closely resembling physiological iii vivo bone (FIG. 23). Such macroporosity at the low end of the range being particularly suited to in vivo applications desiring rapid ingrowth of bone matrix, while macroporosity at the high end of the range allows cells in culture to access the interior for uses such as for ex vivo tissue engineering production of bone grafts.
Using powders with the prefered additive, silicon, and sintered prior to use, porous ceramics can be made as described herein in the Examples. The procedures described in the accompanying examples result in the formation of a bulk ceramic having a globular microporous structure, an underlying internal microporous structure and an internal macroporous structure allowing cells to migrate and function throughout the entire bulk ceramic unit.
It is to be understood by those skilled in the art that several different materials and procedures may be used to develop macroporosity within the ceramic structure. Other materials which are capable of pyrolysis at temperatures below the normal sintering temperatures are also useful to form the macroporous structure. The materials used should also not leave any toxic residues. It is also understood that other methods can also be used to form the macrostructure such as mechanical drilling of holes, the use of lasers or use of foaming agents.
All of the applications in which the present synthetic biomaterial compound can be used have the advantage that both osteoclasts and osteoblasts function actively with the compound in any form thus providing natural cell-mediated remodeling much like that found in vivo. The synthetic biomaterial compound of the present invention promotes both osteogenesis and resorption so that normal tissue healing can occur while simultaneously allowing the synthetic material to be resorbed in the process of normal bone tissue remodeling.
The examples are described for the purposes of illustration and are not intended to limit the scope of the invention. The examples exemplify aspects of the invention for providing a Skelite™ compound which is an additive stabilized structure having unique physical characteristics and is fully biocompatible with natural bone tissue.
Methods of synthetic chemistry and organic chemistry referred to but not explicitly described in this disclosure and examples are reported in the scientific literature and are well known to those skilled in the art.
Preparation of Ca—P Colloidal Suspension (Sol-Gel)
The following procedure is based on preparing sufficient sol-gel hydroxyapatite for manufacturing purposes. Solution A comprises a calcium nitrate tetrahydrate and Solution B comprises an ammonium dihydrogen orthophosphate (mono basic). Solution A is mixed with Solution B to produce the desired colloidal suspension. Solution A is prepared by adding 40 mls of doubly distilled water to 4.722 grams of calcium nitrate, Ca(NO3)2. The solution is stirred at moderate speed for sufficient time to dissolve all of the calcium nitrate which is normally in the range of 3 minutes. To this solution, 3 mls of ammonia hydroxide (NH4OH) is added and stirred for approximately another 3 minutes. To this solution is added 37 mls of double distilled water to provide a total solution volume of approximately 80 mls. The solution is stirred for another 7 minutes and covered. The pH of the solution is tested where a pH of about 11 is desired.
Solution B is prepared by adding 60 mls of double distilled water to a 250 ml beaker containing 1.382 grams of NH4H2PO4. The beaker is covered and stirred at moderate speed for 3 to 4 minutes until all NH4H2PO4 is dissolved. To this solution is added 71 mls of NH4OH and the beaker then covered and stirring continued for approximately another 7 minutes. To this is added another 61 mls of double distilled water and the beaker covered to provide a total solution volume of approximately 192 mls. The solution is then stirred for a further 7 minutes and covered. The pH of the solution is tested where a pH of about 11 is desired.
The desired sol-gel is then prepared by combining Solution B with Solution A. All of Solution A is introduced to a 500 ml reagent bottle. Stirring is commenced at a moderate speed and Solution B introduced to the reagent bottle at a rate of approximately 256 mls per hour until all 192 ml of Solution B is delivered into Solution A. An excess of Solution B may be prepared to compensate for any solution losses which may occur in the transfer process. After completion of this addition and combination of Solution A with Solution B, the resultant product is continued to be stirred at moderate speed for approximately 24 hours. The resultant colloidal suspension (sol-gel) is inspected for any abnormal precipitation or agglomeration. If any abnormal precipitation or agglomeration has occurred, the solution must be discarded and preparation commenced again. Approximately 240 mls of the colloidal suspension, that is the resultant sol-gel, is delivered to a centrifuge bottle and centrifuged for 20 minutes at about 500 rpm at room temperature. Following centrifugation, 180 mls of supernatant is discarded without disturbing the sediments. The sediments are gently resuspended by mixing in a smooth rotating manner for about 30 minutes.
The resulting Ca—P colloidal suspension may be used in a variety of further preparations.
Sintering of Ca—P Products
The following sintering process may be carried out in standard laboratory furnaces of various sizes, capable of operating at temperatures from ambient up to at least 1100° C., and designed to maintain accurate and stable internal temperatures, particularly between 800° C. and 1100° C., such as Lindberg models 51744 or 894-Blue M. The components prepared by any of the procedures described herein are carefully transferred onto a standard ceramic plate (as is common practice in the Lindberg oven). The ceramic plate is used as a carrier during the sintering process to facilitate easy loading and withdrawal of multiple substrates from the furnace. The furnace temperature is set to the temperature required to achieve the desired ratios of HA:SiTCP. Utilizing a programmable furnace such as the Lindberg model 894-Blue M, the furnace may be programmed to hold the desired temperature, which will normally be selected from the range 800° C. to 1100° C., for a maximum of one hour to ensure desired diffusion of the selected stabilizing additives. The ceramic plate carrying the sintered substrates is removed at any time after the internal furnace temperature has cooled to an acceptable and safe touch-temperature of approximately 60° C. Individual substrates may then be stored or packaged for final use.
In accordance with this process a fine or coarse powder, pellets, three-dimensional shaped pieces, macroporous structures, thin films and coatings of the biomaterial compound can be produced on a consistent basis having the desired composition where variability in the various processing parameters have been minimized to ensure such consistency.
Preparation of Thin Films
To create a thin film on a transparent substrate, quartz (amorphous silica) substrates were cleaned using water and chromic acid and subsequently dip coated in the colloidal suspension of Example 1. The substrate needs to be thoroughly cleaned to ensure satisfactory film coverage. In the case of quartz substrates, cleaning is achieved by placing the discs in a glass beaker and supplying chromic acid cleaning solution to the glass beaker to cover all discs. The beaker is then covered. The discs are then sonicated in a water bath for 1 hour. The acid is washed away using tap water for 20 minutes. The residual tap water is removed by three changes of doubly distilled water. After the final change of double distilled water, every single disc is dried with lint-free towel and inspected for flaws in the quartz surface. Any residual particulate on the surface is removed as needed with compressed nitrogen or air. The discs are stored in covered trays in an aseptic environment. This method can be used to clean any type of quartz substrate.
Dip coating was achieved by suction mounting the substrates on a computer controlled linear slide. The mounted substrates were lowered into the colloidal suspension and immediately withdrawn at a programmed speed of 2 mm/s. Following dip coating, the substrates were allowed to dry in ambient conditions and were subsequently sintered in a programmable furnace for a period of 1 hour at temperatures ranging from 800° C. to 1100° C. The sintered thin films had a uniform translucent appearance characteristic of a polycrystalline thin film. The thin film had an approximate thickness of 0.5 to 1.0 μm with a particle size on the order of 0.2 to 1.0 μm.
Preparation of Ca—P Powder with No Introduced Additives
Following the procedures for the formation and aging of the colloidal suspension of Example 1, the colloid was processed to the stage of reducing the volume by centrifugation. The precipitate was dried for approximately 5 hours at 100° C. and sintered for one hour in an open alumina crucible in air at a temperature of 1000° C. A fine powder was formed through mechanical grinding of the sintered material in a motorized mortar and pestle (Retsch Model RM 100 USA).
Preparation of Ca—P Powder with Silicon as the Introduced Additive
Following the procedures for the formation and aging of the colloidal suspension of Example 1, the colloid was processed to the stage of reducing the volume by centrifugation. In order to retain the colloidal sol characteristics, the silicon additive was introduced as a sol-gel metal-organic precursor in an organic carrier. The precursor was either tetrapropyl orthosilicate (Si(OC3H7)4 or TPOS) or tetraethyl orthosilicate (Si(OC2H5)4 or TEOS). Addition was accomplished by creating a sol using a precursor carrier such as 2-methoxyethanol (CH3OCH2CH2OH or 2Me) or 2-4 pentanedione (CH3COCH2COCH3 or ACAC). The action of the carrier was to ensure that the additive did not precipitate upon addition to an aqueous solution having a pH similar to that of the Ca—P colloidal suspension. This ensured that the additive was uniformly mixed within the colloid to create a single precipitate rather than two distinct precipitates. Precipitation of the additive was examined in a separate experiment with aqueous solutions. For the silicon compounds, precipitation was minimal for 2Me, ACAC and even if no carrier was employed. The precipitate with introduced silicon was dried for approximately 5 hours at 100° C. and sintered for one hour in an open alumina crucible in air at a temperature of 1000° C. A fine powder was formed through mechanical grinding of the sintered material in a motorized mortar and pestle (Retsch Model RM100 USA). The presence of the additive within the sintered ceramics was checked by wet chemical analysis.
Preparation of Ca—P Powder with Titanium as the Introduced Additive
Following the procedures for the formation and aging of the colloidal suspension of Example 1, the colloid was processed to the stage of reducing the volume by centrifugation. In order to retain the colloidal sol characteristics, the titanium additive was introduced as a sol-gel metal-organic precursor in an organic carrier. The precursor was titanium n-propoxide (Ti(OC3H7)4). Addition was accomplished by creating a sol using a precursor carrier such as 2-methoxyethanol (CH3OCH2CH2OH or 2Me) or 2-4 pentanedione (CH3COCH2COCH3 or ACAC). ACAC was used in particular for its strong chelating action. Precipitation of the additive was examined in a separate experiment with aqueous solutions. For titanium n-propoxide, precipitation of the additive occurred for both no carrier and 2Me, but not for ACAC. The precipitate with introduced titanium was dried for approximately 5 hours at 100° C. and sintered for one hour in an open alumina crucible in air at a temperature of 1000° C. A fine powder was formed through mechanical grinding of the sintered material in a motorized mortar and pestle (Retsch Model RM 100 USA). The presence of the additive within the sintered ceramics was checked by wet chemical analysis.
Preparation of Ceramic Pellets
Ceramic pellets were formed from previously sintered powder that had been prepared according to Examples 4, 5, or 6, using a small amount of the concentrated colloid suspension mixed into the sintered powder as a binding agent. The powders were uniaxially pressed into pellets with a pressure of 1×108 N/M2 [15,000 psi]. The final pellets were sintered for one hour in air at a temperature of 1000° C. to create ceramic components with the desired characteristics. Following thermal processing, the pellet density was approximately 1.5 g/cm3, and the pellet exhibited a uniform microporosity throughout the structure.
Preparation of Macroporous Structures
Sintered powder that had been prepared according to Examples 4, 5, or 6, was sieved using a motorized sieve shaker (Retsch Model AS200 BASIC USA). Powder having a particle size of −325 Mesh was collected and subsequently suspended in water to form a slurry. The interior and exterior surfaces of a preformed piece of open cell (reticulated) polyurethane foam were completely coated by immersing the foam in the slurry. The slurry-coated component was then allowed to dry and was subsequently sintered at 1000° C. for 1 hour. During thermal processing, the foam was removed from the structure through pyrolysis. Importantly, the shape of the final ceramic component replicates the original shape of the foam, including the open-cell structure.
In the preparation of these components, the pore density of the foam was selected to produce the required pore size in the ceramic. Typical pore sizes prepared were in the range of 45 to 80 pores per inch. The coating of the foam was managed to ensure complete coverage of the foam without clogging of the cells. The duration and temperature of the thermal processing were selected to ensure pyrolysis of the foam and to obtain the desired physical properties of the resulting macroporous structure.
An alternate method for the formation of a macroporous structure is to introduce styrene balls of a desired size into the powder being prepared according to Examples 4, 5 or 6. The mixture is combined with a binder, such as a PVA (polyvinyl alcohol) solution, and uniaxially pressed into pellets. A pressing pressure of 1×108 N/m2 [15,000 psi] was selected so as to not extrude the styrene during compression. The pellets were subsequently sintered at 1000° C. for one hour during which the styrene was removed through pyrolysis.
Preparation of Drug Carrier with Associated Pharmaceutical Agent
Depending on application requirements, either the powder of Example 5 or the macroporous structure of Example 8 was sterilized using ethylene oxide or similar approved medical device sterilization technique. In a laminar flow hood, a liquid drug volume was made up according to dosing requirements. In the case of the agent BCSF™ (Bone Cell Stimulating Factor), this required addition of sterile normal saline (0.9% NaCl) to previously lyophilized stored aliquots of the drug, at room temperature. Following reconstitution, the drug was either mixed by gentle agitation with the powder, or slowly dispensed over the surface of the macroporous structure.
Recognizing the natural protein avidity of the bioceramic material, a period of 5 minutes was allowed for the drug to percolate and bind to either the powder or the macroporous structure. Following this period, the preparation was ready for direct patient administration as a therapeutic device or for use as a tissue-engineering scaffold.
In the case of therapeutic administration of the powder-based preparation, a predetermined volume of the suspension (powder plus attached pharmaceutical agent) was injected percutaneously at the desired skeletal site.
In the case of therapeutic administration of macroporous structures, surgical intervention was required to implant the device at skeletal sites in order to effect subsequent bone repair.
Commercial Reference Materials
The commercially available HA (cHA), α-TCP, β-TCP, calcium silicate and silica materials listed in Table 1 (below) were used as reference standards for the analytical techniques performed in the evaluation of the internally prepared mHA and Si-mHA materials described in this study.
TABLE 1
List of Materials Used For Experimental Samples and Reference Standards
Commercial
Materials
Source
Commercial HA
CHA
Aldrich #28,939-6 Lot#04302TQ
α-TCP
αTCP
Supelco Inc #3-3910 Lot#200792
β-TCP
β-TCP
Fluka #21238 Analysis#357352/1 14996
Calcium silicate
CaSiO3
Aldrich #37,266-8 Lot#00714LN
Silica
SiO2
PPG Industries Inc. #63231674 Lot#9-134
Internally Prepared
Materials
Preparation Technique
Microporous HA
MHA
Powder prepared from the thermal
processing of the colloid in
equation (1)
Si-TCP + mHA
Si-mHA
Powder prepared from the thermal
processing of the colloid in
equation (1) where Si is the
introduced additive
Analytical Techniques
X-ray diffraction (XRD) spectra of thin films were acquired using a glancing angle (GA-XRD) technique with an angle of incidence θ=2°, whereas powders were examined using conventional θ-2θ geometry. The source was a 12 kW Rigaku rotating anode XRD generator fitted with a Cr target for improved peak resolution. The glancing angle geometry significantly reduced the contribution from the substrate. For convenience of comparison to other literature, all spectra were converted to that expected for a Cu anode using the following relationship: sin(θCu)=(λCu/λCr)sin (θCr), where λCu=1.54056 Å and λCr32 2.28970 Å. The phase composition was determined by comparing acquired spectra with peaks identified in the Joint Committee on Powder Diffraction Standards (JCPDS) database of standards (JCPDS-International Centre for Diffraction Data and American Society for Testing and Materials. Powder Diffraction File (Inorganic and Organic). Swarthmore, Pa. JCPDS-International Centre for Diffraction Data. 1999). Of particular relevance to this study are the XRD spectra of HA (JCPDS #9-432), α-TCP (JCPDS #9-348) and β-TCP (JCPDS #9-169). Following the collection of XRD data, the background noise was subtracted and the integrated intensities of peaks distinguishable as HA, α-TCP or β-TCP were calculated. These values were then used to determine the percentage phase composition (plus or minus 5%).
Optical microscopy, scanning electron microscopy (SEM, using a JEOL JSM 840) and transmission electron microscopy (TEM, using a Philips CM20) were performed to assess the surface and bulk morphology. Chemical analysis of the samples was carried out by wet chemical methods and neutron activation analysis. Wide-line nuclear magnetic resonance (NMR) experiments on 29Si were accomplished using a Bruker NMR CXP 200 MHz spectrometer with magic angle spinning using a pulse width of 5 ms and a pulse delay of 20 s. Infrared spectroscopy (IR) of powders using a KBr pellet technique utilized a BOMEM MB-120 spectrometer. Approximately 2 mg of sample and approximately 200 mg of KBr were ground and pressed in a 6 mm diameter die at 10 tonnes for 1 minute to produce uniform discs for analysis.
A particle size analysis of the Ca—P colloid at various stages of processing was made by observation of 633 nm He—Ne laser light scattered at various angles. Samples were prepared by adding 10 drops of the precipitated solution to 4 mL ammoniated water (one part 30% NH4OH mixed with five parts water) having a pH greater than 10. Results from these suspensions were reproducible for equivalent samples and stable over time. The power spectrum of the scattered light at a known angle was fitted to a Lorentzian distribution and analyzed by standard methods using a solution viscosity of 8.9×104 kg m−1s−1 and refractive index of 1.3312 (Clark, N., H. Lunacek and G. Benedek. Am J Phys 38(5) 1970; pp. 575-85 and Schumacher, R. Am J Phys 54(2) 1986; pp. 137-41).
Although preferred embodiments have been described herein in detail, it is understood by those skilled in the art that variations may be made thereto without departing from the scope of the invention as defined by the appended claims.
TABLE 2
Summary of Effective Ionic Radius and Ionic Crystal
Radius for Various Elements
Coordination
Ionic Crystal
Effective Ionic
Ion
Number (CN)
Radius (CR)
Radius (IR)
B3+
4
0.25
0.11
6
0.41
0.27
Ba2+
6
1.49
1.35
8
1.56
1.42
Ca2+
6
1.14
1.00
8
1.26
1.12
Co3+
6
1.15
1.01
8
1.28
1.14
La3+
6
1.17
1.03
8
1.30
1.16
Mg2+
4
0.71
0.57
6
0.85
0.72
8
1.03
0.89
p5+
4
0.31
0.17
6
0.52
0.38
Sc3+
6
0.89
0.75
8
1.01
0.87
4
0.40
0.26
Si4+
6
0.54
0.40
Ti4+
4
0.56
0.42
6
0.75
0.61
8
0.88
0.74
Y5+
6
1.04
0.90
8
1.16
1.02
Zr4+
4
0.73
0.59
6
0.86
0.72
8
0.98
0.84
Data from: Shannon, R. D., Acta Cryst. (1976) A32,751
Pugh, Sydney M., Smith, Timothy J. N., Sayer, Michael, Langstaff, Sarah D.
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