Field of the Invention This invention relates to a synthetic poorly-crystalline hydroxyapatite useful as human or animal bone substitution material and for other purposes. The invention further relates to synthesis of amorphous phosphate compounds useful in the formation of poorly-crystalline hydroxyapatite at low temperatures.

Background of the Invention Calcium phosphates are the principal constituent of hard tissues (bone, cartilage, tooth enamel and dentine). Naturally-occurring bone mineral is made of nanometer-sized, poorly-crystalline calcium phosphate with hydroxyapatite structure. However, unlike the ideal stoichiometric crystalline hydroxyapatite, Ca ₁₀ (PO ₄ ) ₆ (OH) ₂ , with atomic Ca/P ratio of 1.67, the composition of bone mineral is significantly different and may be represented by the following formulae,

Ca _8.3 (PO ₄ ) ₄₃ (HPO ₄ ,CO ₃ ) _{1 7} (OH, CO ₃ ) ₀₃ . Bone mineral non-stoichiometry is primarily due to the presence of divalent ions, such as CO ₃ ^2" and HPO ₄ ^3" , which are substituted for the trivalent PO ₄ ^3" ions. Substitution by HPO ₄ ³ ' and CO ₃ ^2" ions produces a change of the Ca/P ratio, resulting in Ca/P ratio which may vary between 1.50 to 1.70, depending on the age and bony site. Generally, the Ca/P ratio increases during aging of bone, suggesting that the amount of carbonate species typically increases for older bones. It is the Ca/P ratio in conjunction with nanocrystalline size and the poorly- crystalline nature that yields specific solubility property of the bone minerals. And because bone tissues undergo constant tissue repair regulated by the mineral- resorbing cells (Osteoclasts) and mineral-producing cells (Osteoblasts), solubility behavior of minerals is important in maintaining a delicate metabolic balance between these cell activities.

Synthetic bone graft material made to closely resemble natural bone minerals can be a useful replacement for natural bone. Acceptable synthetic bone can avoid the problem of availability and harvesting of autogenous bone (patient's own bone) and the risks and complications associated with allograft bone (bone from a cadaver), such as risks of viral transmission. Consequently, there has been

considerable attempts to synthesize a ceramic material which closely resembles natural bone for use as implants. Hydroxyapatite is the preferred choice because, although it is a stoichiometric, crystalline form with generally larger crystal sizes, is chemically closest to the naturally occurring mineral in bone. An ideal synthetic bone graft should possess a minimum of the following four properties: (1) it should be chemically biocompatible like hydroxyapatite; (2) it should provide some degree of structural integrity in order to keep the graft in place and intact until the patient's own bone heals around it; (3) it should be a soluble form to permit resorption so that the patient's own bone replace the foreign hydroxyapatite; and, (4) because it may be necessary to incorporate biomolecules, such as bone growth proteins that can stimulate bone-forming osteoblast cells, into the synthetic bone material, it is desirable that the process used to form the material be carried out at low temperatures. Most bone growth proteins (such as Bone Morphogenetic Proteins) are heat sensitive and lose their bioactivity at temperatures exceeding body temperatures.

Fulfillment of these requirements may be accomplished by a material in which parameters, such as Ca/P ratios, crystal size, crystallinity, porosity, density, thermal stability and material purity are controlled.

The prior art (LeGeros R.Z., in Calcium Phosphates in Oral Biology and Medicine. Karger Pub. Co., New York, 1991) teaches that highly crystalline form of hydroxyapatite is produced by solution precipitation followed by sintering at high temperatures (800-1200 ^* C). High temperature treatment yields highly stoichiometric hydroxyapatite with crystal sizes on the order of several microns with Ca/P of 1.67. Such highly crystalline hydroxyapatite has an extremely low solubility rendering it essentially insoluble in the host tissue. Therefore, it is not replaced by living bone tissue and it remains intact in the patient for an undesirably extended period.

The prior art further teaches that hydroxyapatite is produced by a solid- state acid-base reaction of primarily crystalline calcium phosphate reactants. Such an approach results in materials that are sometimes poorly reacted, inhomogeneous and which have a significant crystalline hydroxyapatite content.

Constantz in U.S. Patent No. 4,880,610 reports on the preparation of

calcium phosphate minerals by the reaction of a highly concentrated phosphoric acid with a calcium source in the presence of a base and hydroxyapatite crystals. The resultant product is a polycrystalline material containing a crystalline form of hydroxyapatite minerals. Likewise, U.S. Patent No. 5,053,212 to Constantz et al. discloses the use of a powdered acid source to improve the workability and mixability of the acid/base mixture; however, a mixed-phase calcium phosphate material similar to that of US 4,880,610 is reported. Recently, Constantz et al. reported in Science (Vol. 267, pp. 1796-9 (24 March, 1995)) the formation of a carbonated apatite from the reaction of monocalcium phosphate monohydrate, Beta-tricalcium phosphate, Alpha-tricalcium phosphate, and calcium carbonate in a sodium phosphate solution, to provide a calcium phosphate material which is still substantially more crystalline in character than naturally occurring bone minerals. Similarly, Brown et al. in U.S. Reissue No. 33,221 report on the reaction of crystalline tetracalcium phosphate (Ca/P of 2.0) with acidic calcium phosphates. Liu et al. in U.S. Patent No. 5,149,368 discloses the reaction of crystalline calcium phosphate salts with an acidic citrate.

All of these prior art references disclose a chemical reaction resulting in crystalline form of hydroxyapatite solids that has been obtained by reacting crystalline solids of calcium phosphate. There has been little reported on the use of amorphous calcium phosphates (Ca/P of approximately 1.5) as one of the reactants because the amorphous calcium phosphates are the least understood solids among the calcium phosphates and the conventional amorphous calcium phosphate is largely considered to be inert and non-reactive solid.

The only mention of the amorphous calcium phosphate material in prior art has focused on the use of the amorphous calcium phosphate as a direct precursor to the formation of a highly crystalline hydroxyapatite compounds under generally high temperature treatments. Such a highly crystalline material is inappropriate for synthetic bone because it is highly insoluble under physiological conditions. For example, Palmer et al. in U.S. Patent No. 4,849,193 report the formation of crystalline hydroxyapatite powder by reacting an acidic calcium phosphate solution with a calcium hydroxide solution, with both solutions near saturation, so as to form an amorphous hydroxyapatite precipitate powder. The

amorphous powder is then immediately dried and sintered at high temperature of 700-1100°C to obtain a very high crystalline hydroxyapatite. Brown et al. in U.S. Reissue No. 33,221 report on the formation of crystalline hydroxyapatite for dental cement by reacting an amoφhous phase specifically restricted to tetracalcium phosphate (Ca/P of 2.0) with at least one of the more acidic calcium phosphates. Further, Brown et al , does not disclose the preparation or the properties of such a tetracalcium phosphate in amorphous state. Tung in U.S. Patent No. 5,037,639 discloses the use and application of standard amorphous calcium phosphate paste for the remineralization of teeth. Tung proposes the use of standard inert amorphous calcium phosphate mixed with and delivered through as a chewing gum, mouth rinse or toothpaste, which upon entering oral fluids converts to crystalline fluoride containing hydroxyapatite which is useful to remineralize tooth enamel. Simkiss in PCT/GB93/01519 describes the use of inhibitors, such as Mg ions or pyrophosphate, mixed with amorphous calcium phosphate and implanted into living tissues. Upon leaching of, for example Mg ions, into surrounding bodily fluids, the amoφhous calcium-magnesium phosphate converts into crystalline hydroxyapatite.

There remains a need to develop new synthetic bone material that more closely mimics the properties of naturally-occurring minerals in bone. In particular, there remains a need to provide synthetic bone materials which are completely bioresorbable, poorly-crystalline, nanometer-sized crystals which can be formed at low temperatures.

Summary of the Invention It is an object of the present invention to provide a bone substitute material that is bioresorbable.

It is yet another object of the present invention to provide a bone substitute material which can be formed at low temperatures and which is readily formable and injectable. It is a further object of the present invention to form a nano-size, poorly- crystalline hydroxyapatite solids with Ca/P ratios comparable to naturally occurring bone minerals.

It is an object of the present invention to provide a process for converting a standard inert amoφhous calcium phosphate into a reactive amoφhous calcium phosphate.

It is an object of the present invention to provide a reactive amoφhous calcium phosphate with surfaces properties that mimic the surface reactivity of naturally-occurring bone mineral.

It is yet another object of the present invention to provide a reactive amoφhous calcium phosphate which is capable of forming poorly-crystalline hydroxyapatite at low temperatures (at body temperature of 37°C). It is yet a further object of the present invention to provide an injectable calcium phosphate mixture.

In one aspect of the present invention, a method for obtaining a reactive amoφhous calcium phosphate is provided. A reactive amoφhous calcium phosphate may be prepared by reacting calcium ions, phosphate ions and a third ion, so as to obtain an amoφhous calcium phosphate and then removing at least a portion of the third ion, so as to obtain a reactive amoφhous calcium phosphate.

By "amoφhous" as that term is used here, it is meant a material with significant amoφhous character. Significant amoφhous character contemplates greater than 75% amoφhous content and preferably greater than 90% amoφhous content and is characterized by a broad, featureless X-ray diffraction pattern. It is recognized that a small degree of crystallinity may exist in the material, however, it is anticipated, in the case of the amoφhous components of the invention, that such crystallinity will not be greater than the degree of crystallinity desired in the product poorly crystalline hydroxyapatitic calcium phosphate. "Reactive" is used herein to refer to the reactivity of the amoφhous calcium phosphate of the present invention with other calcium phosphates. The reactivity is characterized by the ability of the amoφhous calcium phosphate to harden at 37 ^* C in less than five hours and substantially harden in about one to five hours in the presence of a calcium phosphate or crystallization promoter. Completeness of reaction, the rate of reaction, homogeneity of the resultant product and ability to react with otherwise inert compounds are characteristic of the reactive ACP of the invention.

In another aspect of the invention includes a reactive amoφhous calcium phosphate material having at least 90% percent amoφhous character and characterized in that, when prepared 1:1 as a mixture with dicalcium diphosphate in water at 37 'C, the mixture hardens within about 10 to about 60 minutes. The invention also includes a reactive amoφhous calcium phosphate, obtained by removal of a carbonate pre-component of an amoφhous calcium phosphate by thermal decomposition of the pre-component into gaseous or vaporous by¬ products. The invention still further includes a reactive amoφhous calcium phosphate, obtained by removal of a labile component of an amoφhous calcium phosphate by thermal decomposition of the component into gaseous or vaporous by-products. The invention yet further still includes a reactive amoφhous calcium phosphate material having at least 90% percent amoφhous character and characterized in that, when prepared 1:1 as a mixture with dicalcium diphosphate in water at 37 ^* C, the reaction is substantially complete mixture within about 75 minutes, and preferably 40 min.

In another aspect of the invention, a method of preparing a poorly crystalline hydroxyapatite is provided in which the reactive amoφhous calcium phosphate of the invention is reacted with a second calcium phosphate. The second calcium phosphate and the reactive amoφhous calcium phosphate are mixed in a proportion to form a hydroxyapatitic calcium phosphate.

In another aspect of the invention, a method of preparing a poorly crystalline hydroxyapatite is provided in which the reactive amoφhous calcium phosphate of the invention is reacted with a promoter. The promoter selected to convert the reactive amoφhous calcium phosphate into a hydroxyapatitic calcium phosphate.

Another aspect of the invention includes a resorbable bone substitute material comprising a poorly crystalline hydroxyapatite having an X-ray diffraction pattern substantially as shown in Fig. 7d. The invention also includes a resorbable bone substitute material comprising a poorly crystalline hydroxyapatite having an X-ray diffraction pattern comprising broad peaks at 20 values of 26" , 28.5" , 32 ^* and 33' . The invention further includes a resorbable bone substitute material comprising a poorly crystalline hydroxyapatite, characterized in that, when placed

in a rat intramuscular site, resoφtion of at least 100 mg, and preferably 300 mg, of the bone substitute material is complete within one month.

The resorbable bone substitute material is further characterized in that, when prepared from a reaction of amoφhous calcium phosphate and a second phosphate in a fluid, the reaction mixture hardens after a time greater than 60 minutes at about 22 ^* C, and the reaction mixture hardens within about 10 to 60 minutes at 37 ^* C. In preferred embodiments, the mixture is injectable for a time greater than about 60 minutes at about 22 ^* C. In other preferred embodiments, the mixture is formable for a time greater than about 60 minutes at about 22 "C. Another aspect of the invention, includes a formable paste, suitable for use as a resorbable bone substitution material. The paste includes a mixture of the reactive amoφhous calcium phosphate of the invention, and a second calcium phosphate powder; and an amount of a fluid sufficient to provide the desired consistency, said mixture capable of hardening at about 22 "C. The paste of the invention may also include a mixture of the reactive amoφhous calcium phosphate of the invention, and a promoter, the promoter selected to convert the reactive amoφhous calcium phosphate into a hydroxyapatitic calcium phosphate; and an amount of a fluid sufficient to provide the desired consistency, said mixture capable of hardening at about 22 ^* C. In preferred embodiments, the mixture hardens after a time greater than 60 minutes at about 22 ^* C, and wherein the mixture hardens within about 10 to 60 minutes at about 37 ^* C.

Brief Description of the Drawings A description of the invention is made with reference to the figures in which:

Figure 1 is a high-resolution transmission electron micrograph of the reactive amoφhous calcium phosphate illustrating the nanometer-sized grains in clusters with relatively unclear boundaries and partially immersed in shapeless form (arrows);

Figure 2 is an infrared spectrum of the reactive amoφhous calcium phosphate of the present invention (a) prior to and (b) after heating step. Note the

disappearance of H-O-H group (- 3,550 cm ^'1 and 1,640 cm ¹ ) and CO ₃ ^2" group (1420-1450 cm ¹ ) after heat treatment;

Figure 3 is an x-ray diffraction pattern of the reactive amoφhous calcium phosphate of the present invention (a) prior to and (b) after the vacuum heating step. The material is showing the preservation of the amoφhous state after the vacuum heat treatment. It is characterized by absence of shaφ peaks and broad maxima between 20° and 35° diffraction angle. The amoφhous state of the solids is maintained throughout the entire process of the present invention;

Figure 4 is an energy-dispersive electron microprobe spectrum of the reactive amoφhous calcium phosphate of the present invention after the vacuum heating procedure which yielded Ca/P to be 1.58;

Figure 5 is a solubility curve of a poorly crystalline hydroxyapatite product derived from amoφhous calcium phosphate of the present invention when compared with a crystalline hydroxyapatite. Note the relative higher solubility of the material of the present invention versus a more crystalline form of hydroxyapatite, as measured by the amount of calcium ions released into solution at 37°C;

Figure 6 are X-ray diffraction patterns of (a) reactive amoφhous calcium phosphate; and (b) dicalcium diphosphate used in a reaction to form a bone substitute material of the invention;

Figure 7a-d are X-ray diffraction patterns tracking the progress of the reaction of a mixture of reactive amoφhous calcium phosphate and dicalcium diphosphate to form a bone substitute material of the present invention;

Figure 8 is infrared spectra of (a) dicalcium phosphate dihydrate, (b) the activated ACP of the invention, and (c) the poorly crystalline HA of the present invention; and

Figure 9 is an X-ray diffraction pattern of naturally occurring bone.

Detailed Description of the Invention The current invention provides a fully resorbable and reossifying poorly crystalline hydroxyapatite (HA) useful as a bone substitute material (BSM) for the treatment of bone disorders and injuries and other biological applications requiring

resorbable calcium phosphate. The poorly crystalline HA of the invention is characterized by its biological resorbability and its minimal crystallinity. It may be highly porous and rapidly resorbable or of decreased porosity and slowly resorbable. Its crystalline character is substantially the same as natural bone, without the higher degree of crystallinity seen in the bone substitute materials known to the art. The inventive poorly crystalline HA also is biocompatible and not detrimental to the host.

In an important aspect of the invention, the ease of use of the poorly crystalline HA in a surgical setting is significantly improved over other bone substitute materials known in the art. Specifically, the reaction is initiated outside the body and proceeds slowly at room temperature thereby minimizing any possibility that the material will "set up" prior to application to the surgical site and become unusable. The reaction accelerates significantly at body temperature and the material hardens in place. Furthermore, the consistency and formability of the poorly crystalline HA as well as the reaction speed may be varied according to the therapeutic need, by modifying a few simple parameters.

The resorbability of the bone substitute material of the instant invention is attributable to the combination of its porosity and significant amoφhous character. The bone substitute material of the invention comprises a poorly crystalline hydroxyapatitic calcium phosphate, substantially similar to that found in natural bone. Lack of crystallinity in apatites is associated with somewhat increased solubility in aqueous systems compared to other more crystalline species, thus the low crystallinity and/or presence of stably amoφhous apatitic domains is believed to promote resorbability in biological systems. Porosity facilitates both the penetration of cells and cell processes into the bone substitute material matrix and the diffusion of substances to and from the matrix interior. Accordingly, bone substitute materials of lower porosity resorb more slowly in vivo than those of high porosity.

In preferred embodiments, the reactants are mixed outside of the body, yielding a formable bone substitute material suitable for application to a surgical site. The reaction generally is completed after application to the surgical site. Bone substitute materials of the invention generally harden in less than five hours

and substantially harden in about one to five hours under physiological conditions, and preferably in about 10-30 minutes. In a preferred embodiment, the reaction is initiated by adding distilled water to a mixmre of two dry components to form a thick paste which hardens in about a half an hour. Other aqueous agents such as serum or tissue culture medium may be used in place of distilled water. Most often the resulting resorbable poorly crystalline hydroxyapatite will be calcium deficient with a calcium to phosphate ratio of less than 1.5 as compared to the ideal stoichiometric value of approximately 1.67 for hydroxyapatite.

The invention also provides a test for identifying suitable reactive bone substitute materials and reactive precursors. The test comprises combining the components, producing a formable substance and demonstrating its ability to harden in a suitable amount of time at or around body temperature. Components which harden in this way may then be placed intramuscularly in a test animal and checked for biological resorbability. One hundred milligrams (100 mg), and preferably three hundred milligrams (300 mg), of a bone substitute material of the present invention will resorb in less than 1 month in a rat muscle. Some more slowly resorbable bone substitute materials may require more than a year for complete resorbtion in rodents.

The bone substitute material formation reaction employs at least one amoφhous calcium phosphate (ACP) precursor, and preferably employs an activated ACP. In some instances, the reaction may employ only one precursor ACP which is converted in a controlled fashion in part or whole to the poorly crystalline HA (bone substitute material) of the invention. Alternatively, the reaction may employ one or more additional precursors preferably a calcium and/or a phosphate source, which combine with the ACP to yield the poorly crystalline hydroxyapatite of the invention. In any event, reactions which can be initiated outside of the body, carried on in a paste-like configuration and which significantly accelerate at 37 " C leading to a hardened calcium phosphate product are greatly preferred. ACP precursors only: When amoφhous calcium phosphate is used as the sole precursor to produce a resorbable bone substitute material, it is important to control the natural tendency of the ACP to convert to highly crystalline

hydroxyapatite. On the other hand, the time course of conversion should be fast enough to have surgical utility. One approach is to combine a precursor ACP containing an inhibitor of crystal formation (e.g. the ACP of example 1) with an ACP that does not contain an inhibitor of crystal formation (e.g., a promoter). The reactants may be mixed in a dry state, with the appropriate particulate size and an excess of the inhibitor-containing ACP. The reactants can then be exposed to crystal-forming conditions such as the addition of water, followed by an elevation in temperature, such as that which occurs following introduction into the body, to convert the reactants to the poorly crystalline HA of the invention. ACP precursor plus additional calcium phosphate sources: ACP may be reacted with a second calcium source (including a second ACP) using any reaction promoting technique. The reaction being promoted is the conversion of an amoφhous calcium phosphate into a nanocrystalline or poorly crystalline hydroxyapatite. Such reactions include acid/base, displacement, substitution, and hydrolysis reactions as well as purely physical and mechanical reactions (e.g., grinding, mixing). Under any reaction scheme it is important that the ACP retains significant amoφhous character throughout the reaction. Specifically, the overall crystallinity within the starting product cannot exceed that desired in the end product. Thus certain reaction schemes may require stabilization of the amoφhous nature of the ACP throughout the reaction period. Examples of suitable such inhibitors of crystal formation known to the art include carbonate, fluoride, and magnesium.

In many forms of the current invention, at least one of the precursors must be activated so as to react with the other components at physiological conditions. In some preferred embodiments the ACP component is activated under heat in order to facilitate the reaction with the second calcium containing reactant. Examples of suitable such second reactants include DCPD, other crystalline or poorly crystalline calcium phosphates, calcium sources or phosphate sources, or a second ACP. Other methods of activation known to the art such catalysis or the use of ionic solvents may also be used to promote reaction between substituents. The second calcium phosphate reactant may be of any crystalline structure and should be chosen so as to be reactive with the first ACP either directly or through

the use of a reaction promoting vehicles such as ionic solvents. Appropriate reaction conditions will be determined by demonstration of rapid hardening at 37 ^* C, following mixing of the reactants and the addition of water.

The bone substitute material forming reaction may also be designed to produce an end product that is porous. In one embodiment, the principles of acid/base chemistry plus the use of a dry mixmre of controlled particle size reactants leads to a porous bone substitute material. Other methods of promoting porosity such as chemical or physical etching and leaching may be employed. The present invention provides a novel process for converting a standard inert amoφhous calcium phosphate precipitate into highly reactive amoφhous solids. The amoφhous solids can be used in the reactions described above to form a poorly- or nano-crystalline synthetic hydroxyapatite that provides bioactivity, bioresorbability and structural integrity. This novel amoφhous material can be reacted with other calcium phosphates at or below 37°C to form a bone-like material consisting of poorly crystalline hydroxyapatite.

The amoφhous calcium phosphate of the present invention is highly reactive towards other acidic or basic calcium phosphates. Also, the amoφhous calcium phosphate of the present invention is considered reactive in that it is capable of reacting at room temperature with a variety of calcium- or phosphorus- bearing compounds which are conventionally considered "inert" to ACP, for example CaO, CaCO ₃ and calcium acetate. Prior art acid-base reactions of conventional crystalline calcium phosphate results in poorly reacted solids, having reaction product that are too crystalline to be sufficiently soluble in a living tissues. The reactions from the prior art are generally incomplete and the reaction products are inhomogeneous. In contrast, the amoφhous calcium phosphate of the present invention reacts quickly and completely with a wide variety of calcium phosphates and other calcium- or phosphorus-bearing materials to provide a homogeneous product.

The source of the enhanced reactivity is not completely understood; however, it is believed to be associated with the amoφhicity (lack of crystallinity) and, in some embodiments, site vacancies in the material, as created by the process of the present invention. The vacancies may provide reactive sites for

subsequent reaction. These observations will be discussed more fully, below.

The method of the present invention permits initial formation of amoφhous calcium phosphate particles of less than 1000 A, preferably 200-500 A, and most preferably 300 A, the further growth of which are curtailed by rapid precipitation of the product from solution. During reaction of calcium and phosphate ion sources to form an amoφhous calcium phosphate, a third ion is introduced in the solution so that these ions are incoφorated in the amoφhous precipitate structure instead of trivalent PO ₄ ^3" group(s). Because some PO ₄ ^3" is replaced by the third ion, the overall PO ₄ ^3* decreases, thus increasing the Ca/P ratio of the amoφhous precipitate (as compared to standard amoφhous calcium phosphate) and modifying the valence or charge state of the calcium phosphate. The amoφhous solids then may be rapidly freeze-dried to preserve the chemical and physical properties of the material. The amoφhous solids then may be treated under specific conditions selected to promote removal of at least some of the third ion. In the case of carbonate, specific temperature and pressure conditions lead to the reduction of total carbon, presumably as gaseous carbon dioxide and oxygen from the amoφhous solid, while maintaining the amoφhicity.

The resultant material is an amoφhous solid with a higher Ca/P ratio than is typically found in amoφhous calcium phosphates, which is generally reported in the past to be 1.50. Further, removing carbon from the material results in a vacancies in the interstitial structure within the amoφhous solids, rendering it a highly reactive solid. The may be several possible vacancies sources. The material possesses a porosity which promotes reactivity by various means, such as increase surface area. The material may also undergo a change in the stoichiometry balance upon removal of the third ion. This stoichiometry change may result a charge imbalance which is responsible for the increased reactivity of the amoφhous calcium phosphate.

It is desirable to maintain the amoφhous property of the material throughout the entire process. If crystallinity in its entirety (single crystalline regions) or even in local domains (microcrystalline regions) is introduced during the process or in the final product, the solid has been found to lose its reactivity. The resultant highly reactive calcium phosphate is amoφhous in nature and has a

calcium to phosphorous ratio in the range of 1.55 to 1.65. In a preferred embodiment, the amoφhous calcium phosphate has a Ca/P ratio of about 1.58.

The amoφhous state is induced by controlling the rate and duration of the precipitation process. The amoφhous hydroxyapatite of the present invention is precipitated from solution under conditions where initial precipitation is rapid. Rapid precipitation results in the formation of many extremely small calcium phosphate nuclei. Additionally, rapid crystal or grain growth leads to the production of more defects within each grain, thereby also increasing solubility. At the extreme end of the spectrum, crystal or grain growth is so rapid and defect density is so significant that an amoφhous calcium phosphate results. Amoφhous calcium phosphate is gel-like and includes solid solutions with variable compositions. These gels have no long range structure, but are homogeneous when measured on an Angstrom scale. Under physiological conditions, these amoφhous compounds have high solubilities, high formation rates and high rates of conversion to poorly crystalline hydroxyapatite.

The amoφhous calcium phosphate solids acquired by this method retain their amoφhous nature sufficiently long enough to be introduced into the final reaction as substantially amoφhous solids. They can also be mixed and reacted with other solids or solutions containing phosphates, to obtain solids containing a homogeneous distribution of nanometer-sized crystals. Further in preferred embodiments, because the amoφhous calcium phosphate reacts completely with the other solids, the Ca/P of the resultant solid will constitute the total calcium and phosphorous from such reaction, i.e. , there will be an essentially complete reaction. When a proper molar concentration of phosphate from the solution or solids is reacted with the novel amoφhous calcium phosphate material, a poorly crystalline hydroxyapatite material (Ca/P 1.1-1.9) is obtained. Thus, the present invention permits one to design and modify the chemical composition of the resultant product, thereby providing a further mode of controlling bioactivity of the final product used as bone graft material. In one embodiment of the present invention, a solution is prepared which contains calcium and phosphate ions and a third ion in a concentration, at a pH and at a temperature which will promote the rapid nucleation and precipitation of

calcium phosphate. When precipitation is sufficiently rapid, an amoφhous gel-like calcium phosphate is formed. Because the thermodynamically favored crystalline form of hydroxyapatite is enhanced by reducing the rate of reaction, certain processing steps of increasing the rate of reaction may be taken to ensure that an amoφhous compound is obtained. The following factors, among others, are to be considered when designing a solution for the rapid precipitation of the amoφhous calcium phosphate of the present invention.

Preferred conditions: Rapid mixture of calcium and phosphate sources to increase the rate of reaction. The rate of reaction is increased to favor non-stable phases as a product. Allowing more reaction time for each of the ions to juxtapose correctly to form a solid will result in a more thermodynamically favorable crystalline and stable structure.

Preferred calcium and phosphate sources: The use of highly concentrated or near supersaturation solutions ensures that a more rapid reaction will occur. Preferred temperature: Although the reaction can be carried out at room temperature, temperatures of near boiling point to increase the concentration of one reactant is a possible means of increasing the rate of reaction.

In one embodiment, an aqueous solution of calcium ions, phosphate ions and carbonate ions are mixed together rapidly to obtain a carbonate containing amoφhous calcium phosphate solid. The relative concentrations of the ions are selected to give a precipitate having the desired Ca/P ratio. The carbonate ion substitutes for a phosphate ion in the amoφhous calcium phosphate. The carbonated amoφhous calcium phosphate may be obtained by precipitation from an aqueous carbonate solution. Suitable aqueous carbonate solutions include, by way of example only, bicarbonate solution, sodium carbonate solution, potassium carbonate solution. It is further contemplated as within the scope of the invention to use non-aqueous solutions.

Use of a carbonated material is desirable because it permits manipulation of the Ca/P ratio by substitution of PO ₄ ^3" by CO ₃ ^2" . Additionally, the presence of CO ₃ ² " is known to retard the development of crystallinity in amoφhous calcium phosphate. Is recognized, however, that other ions or a mixture of ions may be suitable in place of or in addition to carbonate ion in modifying the Ca/P ratio and

in introduction of reactive site vacancies into the amoφhous calcium phosphate, such as by way of example only, nitrate, nitrite, acetate, Mg ⁺² and P ₂ O ₇ ^4" ions.

The amoφhous calcium phosphate precipitate may be collected and filtered prior to activation. It is preferred to perform this step in a cold room or at sub- ambient temperamres so as to preserve the amoφhous state of the precipitate collected. Collection may typically may be carried out by any conventional means, including, but in no way limited to gravity filtration, vacuum filtration or centrifugation. The collected precipitate is gelatinous and is washed more than once with distilled water. The washed precipitate is then dried under any conditions which maintain the amoφhous character of the material. Lyophilization is a suitable, but not exclusive, technique. Upon' freezing, the precipitate while kept frozen, is dried to remove the bulk of the entrained liquid. This procedure may be accomplished by placing the frozen precipitate into a vacuum chamber for a given period of time. Freeze-drying typically occurs at liquid nitrogen temperatures for a time in the range of 12-78 hrs, preferably about 24 hours, and under a vacuum in the range of lO '-lO ^"4 , preferably 10 ^"2 , torr. A preferred method includes lyophilization because the cryogenic temperamres typically used in lyophilization inhibit further crystallization of the material. As a result, the amoφhous calcium phosphate obtained thereby is an extremely fine free flowing powder.

The dried ACP may then be activated. In a preferred embodiment, where carbonate is present in the ACP, the ACP powder is heated to drive off remaining free water, water of hydration and to remove carbon, presumably through the decomposition of CO ₃ ^2" into CO ₂ and oxygen. The heating step is carried out at a temperamre of less than 500°C but more than 425°C, so as to prevent conversion of the amoφhous calcium phosphate into crystalline hydroxyapatite. Heating is preferably carried out at a temperamre in the range of 450-460°C. In a preferred embodiment, the freeze-dried amoφhous calcium phosphate powder is heated under vacuum. In a vacuum environment, the temperamre may be considerably less, i.e., in the range of about 175-225°C, to obtain the same result. The lower temperamres may be desirable because they reduce the risk of crystallization of the amoφhous powder.

Low crystallinity and site vacancies (porosity and/or stoichiometric changes) may account for the observed higher reactivity of the amoφhous calcium phosphate of the present invention. This is exemplified by the following observations. A carbonate-containing amoφhous calcium phosphate which has been heated to 525 'C is observed to have an increase in formation of crystalline hydroxyapatite and to have a corresponding decrease in reactivity. Amoφhous calcium phosphate that is heated to only 400 ^* C retains its amoφhous characteristic, but exhibits a decreased reactivity. Presumably this decrease in reactivity is related to the higher carbonate levels (and less site vacancies) observed by IR in samples treated at this lower temperature. This suggests that both amoφhicity and decreased carbon content (vacant reactive sites) are a factor in reactivity. This is not intended to be in any way an exclusive basis for reactivity. Other basis for the observed reactivity are considered to be within the scope of the invention. The resulting amoφhous calcium phosphate powder is a highly reactive amoφhous calcium phosphate material with a Ca/P ratio of between 1.1-1.9, preferably about 1.55 to 1.65, and most preferably about 1.58. The powder has been characterized by a variety of analytical techniques.

In Figure 1 , a high-resolution transmission electron micrograph is shown to illustrate the moφhological characteristics and the angstrom-sized nature of the preferred reactive amoφhous calcium phosphate of the present invention.

Preferred particle sizes are less than 1,000 A, preferably in the range of 300-400 A. Note the unclear boundaries separating the globule-like clusters, lacking clear edges and surfaces, in contrast to crystalline materials. Figure 2a and 2b illustrate infrared spectra of the amoφhous calcium phosphate after lyophilization process (a) and after the subsequent heat treatment at 450°C for 1 hr (b). Infrared peaks illustrating presence of local chemical groups in the material show that the presence of H-O-H (at approximately 3,400 cm ^"1 and 1640 cm ^"1 ) and CO ₃ ^2" group (at 1420-1450 cm ^"1 ) are significantly reduced after heat treatment. However, the x-ray diffraction patterns in Figure 3 of similar materials show that the amoφhous state after the lyophilization (a) is substantially unchanged after the heat treatment (b). The amoφhous nature of the present invention material is characterized by broad peaks and undefined background with absence of shaφ peaks at any position

of the diffracting angles that correspond to known crystalline calcium phosphates. The Ca/P measurement performed using wave length-dispersive X-ray analysis on an electron micro-probe of the same material after heat treatment yields Ca/P to be 1.58 (Figure 4). These characterizations demonstrate that although there is a change in the local moiety of certain groups in the amoφhous calcium phosphate solids, the overall amoφhicity is maintained throughout the process. Thus allowing an inteφretation of the material to contain local vacancies or "holes" in the amoφhous structure which may activate the ACP. In another preferred embodiment, the highly reactive amoφhous calcium phosphate is reacted with an acidic or basic calcium phosphate to obtain a poorly crystalline hydroxyapatite. As discussed above, hydroxyapatite is the thermodynamically preferred reaction product which readily crystallizes to give a product that is not biocompatible due to its insolubility under physiological conditions. The use of an amoφhous calcium phosphate, which can react quickly and completely to a product hydroxyapatite without significant crystallization, provides a novel route to a poorly-crystalline hydroxyapatite which is resorbable under physiological conditions.

The amoφhous calcium phosphate powder of the present invention may be mixed with a variety second component to thereby react to form a poorly crystalline form of hydroxyapatite. This reaction occurs at room temperamre upon mixing of the powder with a variety of both acidic and basic calcium phosphates in the presence of a fluid, such as but not limited to, water, saline, buffer solution, serum or tissue culture medium. Depending upon the amount of fluid added the mixmre of amoφhous calcium phosphate of the present invention and acidic calcium phosphate results in a highly formable and/or highly injectable paste with varying degrees of paste consistency.

Appropriate calcium phosphates include both basic and acidic calcium phosphates which provide the appropriate stoichiometry for reaction to obtain a hydroxyapatitic calcium phosphate. In a preferred embodiment, an acidic (pH 5-7) calcium phosphate is used. Suitable acidic calcium phosphates include, but are in no way limited to, calcium metaphosphate, dicalcium phosphate dihydrate,

heptacalcium phosphate, tricalcium phosphates, calcium pyrophosphate dihydrate, poorly crystalline HA, calcium pyrophosphate, and octacalcium phosphate. Suitable basic calcium phosphates include additional ACPs. Other solids which would provide a source of phosphate or calcium, such as by way of example only, CaO, CaCO ₃ , calcium acetate, and H ₃ PO ₄ , may be mixed to form a final product to yield a desired Ca/P ratio close to natural bone. It may be desirable to provide the second component in the amoφhous or poorly crystalline state, as well.

Hydroxyapatite is a thermodynamically favored form of calcium phosphate. It is therefore within the scope of the invention to merely promote the conversion of the reactive ACP into a poorly crystalline HA, by addition of components which promote conversion of ACP into HA, without chemical reaction. Suitable promoters include, but are not limited to, water and heat.

The second calcium phosphate is often crystalline, as is evidenced by the presence of shaφ diffraction peaks typical to the calcium phosphate of interest in the X-ray diffraction pattern (Fig 6a). In contrast, the reactive ACP is amoφhous and shows no identifiable peaks by X-ray diffraction (Fig 6b). Despite its higher crystallinity, however, dicalcium diphosphate is consumed in the reaction with reactive ACP and the product HA is of much reduced crystallinity.

Because at least one of the reactants is amoφhous and highly reactive, the reaction proceeds at room temperamre to provide an apatitic material having a poorly-crystalline or microcrystalline microstructure. The reaction also is substantially complete, thereby insuring that all calcium and phosphate of the mixmre are consumed by the resultant hydroxyapatite product. This permits reliable manufacture of hydroxyapatite products simply by selection of the relative proportions of the starting amoφhous and secondary calcium phosphates. It is desirable to maintain a calcium to phosphate ratio of about 1.2-1.68, preferably less than 1.5, and most preferably about 1.38.

The product hydroxyapatite material contains labile environments characteristic of naturally-occurring bone. In naturally occurring bone, minerals are characterized by nanometer-sized structure, providing high surface areas to interact with the surrounding tissue environment, resulting in resoφtion and remodelling of tissues. The present invention, with its nanometer-sized crystals as

the product, closely mimics the naturally occurring bone minerals. Further, properties such as crystallinity and Ca/P ratios are closely designed in the present invention to simulate the mineral properties found in living tissues of bone. In another preferred embodiment, an injectable paste may be prepared, which can be introduced into the bone repair site. The paste is generally prepared by mixmre of the amoφhous calcium phosphate of the present invention with a second component in an amount of water or buffer sufficient to produce the desired consistency for injection. Most often this will be as thick as possible while still being able to be passed through a 16-18 gauge syringe. Because of the amoφhous nature of the component solids in the paste, the material has markedly improved flow characteristics over prior art compositions. Flow characteristics of the resultant paste are toothpaste-like while prior art materials inherit a granular or oat meal-like consistency. The paste may be prepared before use, up to a period of several hours if held at room temperamre and vaporization is minimized. The storage time may be extended by maintaining the paste at reduced temperamres in the range of 1-10 °C in the refrigerator provided steps are taken to minimize vaporization.

By selecting the appropriate amount of liquid to be added to the reactants, the viscosity of the bone substitution material paste may be adjusted according to need. The paste may be prepared either with an injectable or a formable consistency. Injectable consistency means as thick as possible while still capable of passing through a 16 to 18 gauge needle. Most often this will be a "toothpaste "-like consistency. Formable refers to consistency which allow the material to retain its shape. In the extreme case of a formable consistency, the paste will have the consistency of glazing putty or caulking compounds. The paste also may be prepared with just enough liquid to be both injectable and formable.

In some preferred embodiments (e.g., Examples 9-14, below), the reaction occurs slowly at room temperamre, but is accelerated significantly at body temperamre. This is particularly useful in a surgical situation, since the paste formed by mixing reactants with water remains injectable for a considerable period of time (up to several hours) while held at room temperamre. Thus, at room temperamre (ca. 22 ^* C) the paste hardens after a time greater than one hour and

remains formable and/or injectable for longer than 10 minutes, and preferably longer than one hour and most preferably longer than three hours. Following injection at the implant site (ca. 37 ^* C), the paste hardens in less than about an hour, preferably in about 10-30 minutes. In another embodiment of the invention, it is contemplated to incoφorate bone regenerative proteins (BRP) into the amoφhous calcium phosphate and acidic calcium phosphate mixmre. BRPs have been demonstrated to increase the rate of bone growth and accelerate bone healing. A bone graft including nanocrystalline or poorly crystalline hydroxyapatite and BRP is expected to promote bone healing even more rapidly than a bone graft using the hydroxyapatite of the present invention alone. The efficacy of BRP is further enhanced by controlling the solubility of the nanocrystalline or poorly crystalline hydroxyapatite such that it dissolves at a rate that delivers BRP, calcium, and phosphorus at the optimum dosage for bone growth. Such a method of incoφorating BRP would include, but not limited to, mixing a buffer solution containing BRP with its optimum pH that would maintain protein activity, instead of distilled water. Exemplary BRPs include, but are in no way limited to, Transforming Growth Factor-Beta, Cell- Attachment Factors, Endothelial Growth Factors, and Bone Moφhogenetic Proteins. Such BRPs are currently being developed by Genetics Institute, Cambridge, MA; Genentech, Palo Alto, CA; and Creative Biomolecules, Hopkinton, MA.

In another embodiment of the invention, it is contemplated to incoφorate antibiotics or its agents into the amoφhous calcium phosphate and its mixmre. From a clinical sense, one of the major implication arising from a bone-graft surgery is a need to control the post-operative inflammation or infection. A bone graft including poorly crystalline hydroxyapatite and antibiotic(s) is expected to reduce the chances of local infection at the surgery site, contributing to infection- free, thus faster bone healing process. The efficacy of antibiotics is further enhanced by controlling the release of the poorly crystalline hydroxyapatite such that it dissolves at a rate that delivers antibiotic peptides or its active component at the most effective dosage to the tissue repair site. Exemplary antibiotics include, but are in no way limited to, Penicillin, Chlortetracycline hydrochloride

96/36562 PC17US96/07273

(Aureomycine), Chloramphenicol and Oxytetracycline (Terramycine). Both antibiotics, mostly polypeptides, and bone regenerating proteins may be intermixed with the poorly crystalline hydroxyapatite material of the present invention, to locally deliver all or most of the necessary components in facilitating optimum condition for bone tissue repair.

Examples The invention is further exemplified with reference to the following examples, which are presented for the puφose of illustration only and are not to be considered as limiting of the invention. Example 1. This example describes the step-by-step preparation and methods to render relatively inert amoφhous calcium phosphate solids into a highly reactive amoφhous calcium phosphate of the present invention.

Solution A was prepared at room temperamre by the rapid dissolution of 55g Na ₂ HP0 ₄ .7H ₂ O (sodium phosphate), 50g NaOH (sodium hydroxide), 30g NaHCO ₃ , (sodium bicarbonate) in 1.3 1 of distilled water. H ₂ O volumes in the range of 0.7 to 1.3 ml. have also been used. Solution B was prepared at room temperamre by rapid dissolution of 43g Ca(NO ₃ ) ₂ .4H ₂ 0 (calcium nitrate tetrahydrate) in 0.5 1 of distilled water.

The inert carbonated amoφhous calcium phosphate was then prepared at room temperamre by the rapid addition of solution B to rapidly stirring solution A. The precipitate of gel-like amoφhous calcium phosphate thus formed was immediately filtered using filter paper (0.05 sq. m) with medium filter speed and a vacuum pressure of about 10 ^"2 torr. The material formed a thin cake and was washed with approximately 4 liters of distilled water by adding water into the filtrating funnel. The washed material was then collected using spatula and immersed into a liquid nitrogen in a 2.5 L container. Following the formation of hard frozen pieces, the container was transferred into a vacuum chamber for 24 rs (10 ¹ - 10 ^"2 torr), until a fine and dry powder was obtained.

Although the procedure described above may be performed at room temperamre, the entire process preferably takes place below ambient temperamre (4-5°C), so as to further prevent the amoφhous state from converting into more stable crystalline form. Further, such elements or ions known to act as inhibitors

of crystalline hydroxyapatite formation may be added into the solution in trace amounts. These may be, for example, Mg ions in the form of less than 1.0 g MgCl ₂ .6H ₂ 0 (magnesium chloride), pyrophosphate ions in the form of less than 2 g Na ₄ P ₂ 0 ₇ .10H ₂ 0 (sodium pyrophosphate). An infrared spectrum of the inert amoφhous material at this point in process is shown in Fig. 2a. This spectrum contains peaks characteristic of P-O groups (600 and 1000 cm ^"1 ), C0 ₃ ^2" group (1,420-1,450 cm ^'1 ) with relatively large peak of O-H group (~ 3,550 cm ^'1 ). X-ray diffraction pattern of the same material (Figure 3a) show amoφhous nature of the material as demonstrated by absence of any shaφ peaks when me measurement of crystallinity is determined by taking ratio of coherent peaks to background.

The inert amoφhous material described above was then made into a reactive form by heating for 60 minutes at 450 'C (±3'C). The IR of the heated material is shown in Fig. 2b. This spectrum showed reduction of particular O-H and C0 ₃ ^2" groups, indicating significant reduction of H ₂ O and C0 ₃ ^2" as CO ₂ and O ₂ . In similarly prepared samples the carbon content was observed to drop approximately 60% with a total carbonate ratio decreasing from 1.56% to 0.5%. Note, however, that the amoφhous nature of the material was not lost during this process, as demonstrated by the x-ray diffraction pattern shown in Figure 3(b). The Ca/P ratio measurement of this material after the heat treatment was determined to be 1.575, using a method of quantitative electron microprobe analysis (Figure 4). The overall moφhological and ultrastructural properties of amoφhous material is shown in Figure 1 , as seen under a transmission electron microscope. Note the "amoφhous" appearance of the material with absence of shaφ edges separating each granules with certain portion of the material to exhibit shapeless form (arrows). An extremely high specific surface area of 120 m ² /g, with an average pore size of approximately 130 A was observed in this material.

Example 2: The preparation was conducted as described in Example 1 above, with the exception that the preparation of Solutions A and B was replaced by the following reactions. Solution A was prepared at room temperamre by the rapid dissolution of 90.68g of Ca(NO ₃ ) ₂ .4H ₂ 0 in 1.2 liter of carbonated distilled H ₂ O. Solution B was prepared by dissolving 40.57 g of K ₂ HPO ₄ in 1.53 liters of

distilled H ₂ O, containing 24 ml of 45 vol. % KOH solution. Chemical and physical properties of the product amoφhous calcium phosphate resulting from this procedure were similar to those of the material prepared accordingly for Example 1. Example 3: The preparation was conducted as described in Example 1 above, with the exception that the preparation of Solutions A and B were replaced by the following reactions. Solution A was prepared at room temperature by the rapid dissolution of 10.58 g of Ca(NO ₃ ) ₂ .6H ₂ 0 in 0.15 liters of carbonated distilled H ₂ 0 at pH greater than 9.0, as adjusted by NaOH. Solution B was prepared by dissolving 7.8 g of (NH ₄ ) ₂ HPO ₄ in 0.35 liters of distilled H ₂ 0. Chemical and physical properties of the product amoφhous calcium phosphate resulting from this procedure were similar to those of the material prepared according to Examples 1 and 2.

Example 4: This example describes the preparation of bone substitute material of the invention.

The dicalcium phosphate dihydrate (DCPD) used in this example was prepared in the following manner. Solution A was prepared at room temperamre by rapid dissolution of lOg HoN ₂ 0 ₄ P (diammonium hydrogen phosphate) in 500 ml distilled water at a pH of 4.6-4.8. Solution B was prepared at room temperamre by the rapid dissolution of 17. Ig Ca(NO ₃ ) ₂ .4H ₂ 0 (calcium nitrate tetrahydrate) in 250 ml distilled water. The dicalcium phosphate dihydrate was prepared at room temperamre by the rapid addition of solution B to the stirring solution A. Immediately thereafter, the sample was filtered using filter paper (0.05 sq. m) with medium filter speed and a vacuum pressure of about 10 ^"2 torr. The material formed a thin cake which was washed with about 2 liters of distilled water and then dried at room temperamre for 24-72 hrs.

The reactive amoφhous calcium phosphate material prepared from Examples 1, 2, or 3 was physically dry-mixed with dicalcium phosphate dihydrate (CaHPO ₄ .2H ₂ O) at 50:50 wt% using a mortar and pestle for 3-5 min. Water (lml/g of mixed material) was then added to the powder mixmre to yield a paste¬ like consistency. The amount of H ₂ 0 added varied, depending on whether a thick or thin paste was desired. The paste material was then placed in a moist tissue

environment where upon reaching body temperamre (37 °C), hardened into a solid mass without exothermic behavior. The hardening process could be delayed for several hours by placing it into a refrigerating temperature of 4°C. The hardened material was composed of nanometer-sized, poorly crystalline hydroxyapatite with an inherent solubility property that exceeded reported solubilities for a synthetic hydroxyapatite material. This is demonstrated in Figure 5, where the concentration of calcium ions released into a controlled pH buffer solution over 24 hrs at 37 °C, was significantly higher for the poorly crystalline HA material of the present invention (curve 50) than the standard crystalline hydroxyapatite material (curve 52).

Example 5: This example demonstrates the preparation of bone substitute material using materials having a selected particle size.

The reactive amoφhous calcium phosphate material prepared from Examples 1, 2, or 3 was physically dry-mixed with dicalcium phosphate dihydrate (CaHPO ₄ .2H ₂ O) with a particle size of less than 100 μm at 50:50 wt. % using a SPEX 8510 laboratory mill for 2 min with a 8505 alumina ceramic grinding chamber, followed by sieving to a size of less than 100 μm. Water (lml/g of mixed material) was then added to the powder mixmre to yield a paste-like consistency. Example 6: Reactive amoφhous calcium phosphate material as prepared in

Examples 1, 2, or 3 was dry-mixed with other calcium phosphate compounds, according to the method described in Example 4. These compounds included, but were not limited to: Ca(PO ₃ ) ₂ (calcium metaphosphates), Ca ₇ (P ₅ 0ι ₆ ) ₂ (heptacalcium phosphate), Ca ₂ P ₂ O ₇ (calcium pyrophosphate), Ca ₃ (PO ₄ ) ₂ (tricalcium phosphates). The dry-mixmre ratio was properly calculated to be between Ca/P ratios of 1.5- 1.70, depending on the molar Ca/P ratio of the compound mixed with the reactive amoφhous calcium. The resulting material was poorly crystalline hydroxyapatite solids with solubility properties same as shown in Figure 5.

Example 7: This example describes the preparation of an injectable paste for the formation of poorly crystalline hydroxyapatite solid.

The dried mixed materials prepared according to Examples 4 or 6 were mixed with distilled H ₂ O (2.3 ml/g). A paste was formed that could be easily

shaped by hand or injected through a nozzle as small as 0.5mm ID. The flowability increased after refrigerating the paste at 4'C for 2-3 hrs.

The material could be stored in a paste form for about 12 hours at 4 ^* C in an air tight container without hardening. Example 8. The crystalline content of the product bone substitute material was monitored by X-ray diffraction and I-R spectrometry.

Fig. 7a-d are the X-ray diffraction spectra of the reaction product between DCPD and the reactive amoφhous calcium phosphate as described in Example 4. The reaction mixture was placed in a moist environment at 37 "C and examined by X-ray diffraction spectrometry at different times. X-ray scan conditions are (a) copper anode, (b) λ = 1.4540598 A, and (c) a scan range 20-35 ^* at a step of 0.02 ^* and step interval of 2 seconds. Figure 8 shows the infrared spectra of dicalcium phosphate dihydrate (a), the activated ACP of the invention (b), and the poorly crystalline HA of the present invention (c). Samples of Figs. 7a-7d were incubated for 0, 20 min, 75 min and 5 hours, respectively. The samples were removed at the noted time and lyophilized to preserve chemical characteristics. Fig. 7a, taken at the start of the reaction, represents a combination of peaks attributable to the starting ACP and dicalcium diphosphate (see, Fig. 6 for component XRD patterns). The shaφ peaks at ca. 20.25 ^* , 23.5 ^* , 29.5 ^* , 30.75 ^* and 34.2 ^* for crystalline dicalcium diphosphate are readily observed. With increase in reaction time, the shaφ crystalline peaks subside and wide (amoφhous) peaks appear centered at 26 ^* , 28.5' , 32.0' and 33.0" . It is interesting to note that there is no change in the spectra after 75 minutes of reaction, indicating that the reaction essentially complete in little more than one hour. The X-ray diffraction pattern of the bone substitute material of the invention (Fig. 7d) can be compared to that of naturally occurring bone, shown in Fig. 9. The two spectra are nearly identical, indicating the close biomimetry of the bone substitution material of the invention.

Examples 9-14: These examples demonstrate the effect of fluid volume on the consistency and reactivity of injectable paste to be used in the formation of bone substitute material. Each of the pastes were prepared as described in Example 7, above, and the consistency and rate of reaction at room temperamre

and 37 ^* C were determined. Observations are reported in Table 2.

Table 2. Formability, injectability and reactivity of one gram bone substitute material prepared with variable water volume.

Example No. water volume formability injectability hardening (mL) time (min)

(4 'CIRT VQ

9 0.7 - -/-/- crumbles

10 0.8 ^* + + + + > 60/ > 60/30 easily formed paste

11 0.9 ^* + + + + > 60/ > 60/30 toothpaste

12 1.0 + + + + > 60/ > 60/30 liquid toothpaste ^v Under some circumstances (e.g., evaporation) these samples may dry out somewhat over a period of one hour at room temperamre. In such cases, additional water may be added to restore the original consistency.

Example 13: The puφose of this study was to evaluate the model as an analysis of efficacy of the implanted poorly crystalline hydroxyapatite calcium bone substitute material phosphate ceramic material of the invention when it was implanted into tibial bone surgically created defects of New Zealand White

Rabbits.

I. Test Article and Animals Test Article: The test article used was prepared as described in Example 7 with the exception that a buffer solution with optimum pH (saline) range for the protein or peptide bioactivity was used.

Animals: Seven adult male and female NZW rabbits (2.5-3.0 kg) were used in this study. Animals were obtained from Pine Acres Rabbitry/Farm. Animals were held in quarantine and acclimatization for a minimum of 10 days prior to the initiation of the study. They were evaluated by a veterinarian for general health prior to release from quarantine. Animals were individually housed in suspended stainless steel cages. Wood shavings were used in dropping pans

under the cages. Animals were identified by a numbered ear tag or tattoo and by a corresponding cage card. All animals received the same treatment- one defect was placed in one tibia. Timepoints for evaluations were 0, 2, 4, and 8 weeks. Surgical Procedure: After obtaining adequate anesthesia, using aseptic technique, an incision was made over the proximal tibia. The soft tissue was deflected away and the bone was exposed. Using a 5 mm trephine in a low speed dental handpiece drill with irrigation (0.9% physiologic saline) as needed, the bony disk was dissected free and the site was prepared for implantation. The bone substitute material paste form mixed α-BSM with saline, was placed into the defect. One sample per animal was administered using this method. The soft tissues were then closed in layers with 3-0 suture material. The animals were monitored and were given buprenoφhine (0.02-0.05 mg/kg, s.c.) and cephalothin (20 mg./kg, s.c.) upon awakening. The analgesic and antibiotic were administered 2 times per day for five to seven days after surgery. II. Experimental Observations

Clinical Observations and Radiographs: Clinical observations of the animals' general health and well-being with special regard to ambulation were performed at least weekly. Radiographs of the tibia were made at scheduled intervals including after surgery and at the time of necropsy. The animals were allowed to heal for scheduled periods of time. The animals were anesthetized for tibial radiographs, which were taken every 2 weeks throughout the smdy. The radiographs were used to determine the duration of the smdy. Approximately every 2 weeks, 2 animals were sacrificed and the test sites were removed for histology. The animals were monitored daily to see if any changes in diet or behavior occurred. At the end of the smdy the animals were euthanized by an overdose of prescribed euthanasia solution, (ketamine HC1 and Xylazine followed by saturated KC1)

Microscopic Pathology: The implantation sites were prepared as undecalcified and decalcified sections. Decalcified slides were prepared as plastic embedded light green basic fucsin 90 micron slides; undecalcified slides were stained with hematoxylin and eosin and Masson's trichrome. Slides were microscopically evaluated by a board certified veterinary pathologist (ACVP) with

experience in laboratory animal pathology. III. Results

Clinical Observations and Radiographs: Radiographs of the tibial defects showed increasing radiodensity with time. Necropsy: The tibial defect sites appeared to be smaller with time. No excessive inflammation, other than that anticipated with any surgery, was observed grossly.

Microscopic Pathology: At 2 weeks, the bone substitute material calcium phosphate was still observed in the defect site as crystals both in the site and in local macrophages. Small spicules of trabecular bone were seen at the defect edges and in the defect site. By 4 weeks, few if any crystals of the device were visible; thicker trabecular bone was seen throughout the defect site. Specimens at 6 and 8 weeks had no evidence of the device; bone seen in the defect site was very thick trabecular to cortical type bone. Example 16. This example compares the infrared spectra of crystalline and amoφhous precursors produced according to the examples and the final poorly crystalline HA produced by reacting similar precursors. Fig. 8a presents the IR spectrum of brushite (DCPD) prepared as described in Example 4; Fig. 8b presents the spectrum of ACP after heat treatment, prepared as described in Example 1; and Fig. 8c is the IR spectrum of poorly crystalline HA prepared as described in Example 4.

It will be understood that the objects set forth above, among those made apparent from the preceding description, are efficiently attained and, since certain changes may be made in carrying out the above process and in the composition set form without departing from the spirit and scope of the invention, it is intended that all matter contained in the above description and shown in the accompanying drawing(s) shall be inteφreted as illustrative and not in a limiting sense.

It will be further understood that the following claims are intended to cover all of the generic and specific features of the invention herein described, and all statements of the scope of the invention which might be said to fall there between.

What is claimed is: