# Synthesis and Characterisation of  Calcium Carbonate Aragonite Nanocrystals from Cockle Shell Powder (Anadara granosa)

Authors: Abdullahi Shafiu Kamba; Maznah Ismail; Tengku Azmi Tengku Ibrahim; Zuki Abu Bakar Zakaria
Journal: Journal of Nanomaterials
 (2013)

---

## Abstract

The synthesis of pure calcium carbonate nanocrystals using a high pressure homogeniser (HPH) via a microemulsion system produced uniform nanosized particles, which were characterised using transmission electron microscopy (TEM), field-emission scanning electron microscopy (FESEM), X-ray diffraction (XRD), Fourier transform infrared spectroscopy (FTIR), and thermogravimetric analysis (TGA). The identified particles were aragonite polymorphs with a rod shape and were approximately 50 nm in size. The aragonite polymorph of calcium carbonate was prepared from biogenic materials, cockle shells, and exhibited unique characteristics (i.e., a higher density than that of calcite), which makes it biocompatible and potentially suitable for applications in the medical, pharmaceutical, cosmetic, and paint industries. The methods adopted and the nonionic surfactant used in the synthesis of calcium carbonate nanocrystalline aragonite polymorphs were environmentally friendly and can be scaled up for industrial production. The sources are naturally available materials that are by-products of the seafood industry, which offers an opportunity for exploitation in numerous industrial applications.


---

## Body

## 1. Introduction

Calcium carbonate nanoparticles are abundant inorganic biomaterials with different morphological structures that have attracted the interest of researchers in different fields. This interest is due to the wider application of these nanoparticles in many industries, such as the paint, rubber, and plastics industries. With the present focus of interest in nanotechnology, calcium carbonate nanoparticles have been observed to be biocompatible for use in medicine, pharmaceutical industries, and drug delivery systems [1, 2]. The most important aspect with respect to the synthesis of nanoparticles is control of the particle size, polymorphism, and morphology of the desired material. Control of this parameter has led to the development of new materials with unique properties that differ from those in the bulk material [3]. Many studies have been conducted to mimic nature in the synthesis of nanomaterial with the aim of analysing the biogenic materials and identifying how nature controls the morphology, size, and polymorphism in organisms.Biomineralization is the process by which a living organism secretes inorganic material in the form of a skeleton, a shell, teeth, or bone [1]. These processes are natural, are often performed with a high level of spatial control, and usually occur in a confined reaction environment. The organic matter or biopolymers observed in the hard tissue, such as the bones, teeth, and shells of living organisms, have the unique capacity to control the morphology, crystal size, polymorphism, and structure of the inorganic material. These biopolymers are usually soluble and are referred to as a functional matrix [1–3]. Biomaterials are highly optimised materials with remarkable properties, and they serve as natural archetypes for future materials [1]. These unusual properties have recently attracted the attention of numerous researchers, including both materials chemists and researchers in the medical and pharmaceutical sciences because of the biogenic origin and potential biocompatibilities of these materials [3]. Biomaterials with an optimised structure exhibit better performance, durability, and appearance, which offers valuable opportunities for the development of new techniques for the synthesis and control of nanostructures materials with potential applications in pharmaceuticals, cosmetics, drug delivery, medicine, microelectronics, and energy technology [3].Biological systems are capable of producing inorganic materials such as calcium carbonate with different structures, morphologies, and polymorphs. Such biological systems are observed in numerous marine organisms such as oyster shells, coral, ivory sea urchin, and mollusc shell bivalve nacre, whereby the main components of the shells are calcium carbonate and other organic components, such as anionic protein and glycoprotein [4].Currently, research with respect to cockle shells, in which the primary component is approximately 98-99% calcium carbonate, is in its infancy [5, 6]. Calcium carbonate has three anhydrous crystalline phases: calcite, which is thermodynamically stable under ambient conditions; aragonite, which is a high-pressure polymorph that is less stable than calcite; and vaterite, which is the least stable among the three polymorphs and has the ability to transform into one of the other two polymorphs [7]. Different techniques for the preparation of calcium carbonate nanoparticles have been reported, including the precipitation of homogeneous solutions [8], water-in-oil-in-water emulsions [9], mechanochemical and sonochemical syntheses [10] and water-in-oil (W/O) microemulsions [11]. Other preparation methods include the high-pressure homogeniser (HPH) technique and high-gravity precipitation. For precipitation methods, two different routes have been reported with the only difference being the chemicals used. The first method is based on the carbonation process, whereby carbon dioxide gas is bubbled through aqueous slurry of calcium hydroxide at specific temperature in present of organic additive such as surfactant thereby inducing precipitation of calcium carbonate. The second method is known as double decomposition and involves the combination of salt of calcium ions with salt of carbonate ions, such as the reaction of calcium chloride or calcium nitrate with sodium carbonate or ammonium carbonate [12].Most researchers are now diverting their attention to the microemulsion route for the synthesis of different types of nanoparticles. Microemulsions are a thermodynamically stable, optically transparent, isotropic dispersion of two immiscible liquids, such as water and oil, stabilised by an interfacial film of a surfactant molecule [13]. The system is a single optical dispersion of thermodynamically stable liquids that typically consists of small particle droplets with diameters in the range of less than from 10 nm to 100 nm [14]. A microemulsion serves as a special microreactor that inhibits the growth of nanosized particles [15]. The advantage of this method is that it increases the homogeneity of the chemical decomposition at the nanolevel and allows the easy preparation of nanocrystals of comparatively equal sizes [16].The research in this paper was focused on the synthesis of calcium carbonate nanocrystals from cockle shells by the microemulsion route using a HPH. The process is a top-down technique that occurs in a special homogenising valve at the heart of homogenising equipment. The fluid passes through a minute gap in the homogenising valve [17], which creates conditions of high turbulence and shear, combined with compression, acceleration, and a pressure drop. The impact causes disintegration of particles and dispersion throughout the sample [17]. After homogenisation, the particles are uniform in size, and their sizes depend on the number of cycles, the processing, and the operating pressure. The homogeniser is the most efficient device for the reduction of particle and droplet sizes.To the best of our knowledge, no research related to the synthesis of calcium carbonate nanocrystals from biogenic origins or its reservoir using calcium carbonate as the main source of calcium and carbonate ions has been reported. Most research has focused on the use of chemical reactions, whereby the salts of calcium and carbonate ions act as the precursors for the synthesis of calcium carbonate nanocrystals.


## 2. Experimental

### 2.1. Synthesis of Calcium Carbonate Powder

Cockle shells were obtained from market. The calcium carbonate powders were prepared from the cockle shells according to the procedure described by Islam et al. [18]. Samples of the cockle shells were dried in an oven at 50°C for 7 days, and the shells were then crushed and blended into a fine powder, which was sieved through a 90-μm laboratory stainless steel sieve (Endecott, London, England). The calcium carbonate powders were finally packed into a polyethylene plastic bag for further analyses.


### 2.2. Synthesis of Calcium Carbonate Nanocrystals

The synthesis of calcium carbonate nanocrystals was performed through oil-in-water (O/W) microemulsions using a HPH. In this technique, the particles sizes are reduced after leaving the homogenising gap by cavitations, particle collisions, and shear forces [19, 20].The calcium carbonate nanocrystals were prepared by the dissolution of 2 g of dry cockle shell powder in a formulated oil-in-water (O/W) microemulsion, which was moderately stirred by a magnetic stirrer for 5 min at 100 rpm to form a calcium carbonate suspension. The formulated suspension was passed through the liquid inlet of a HPH for premilling at a moderate pressure of 300 and 500 bars for three cycles each. The premilled suspension was collected at the HPH outlet and was again passed through the HPH liquid inlet at a high pressure of 1500 bars for 25 homogenising cycles to obtain the desired product. The product of the crystal suspension was filtered and dried in an oven at 105°C for 24 hours.


### 2.3. Characterisation of Calcium Carbonate Nanocrystals

The following instruments were employed for the observation and characterisation of the calcium carbonate nanocrystals. The morphology and particle size of the nanocrystals were analysed using a transmission electron microscope (TEM, Hitachi H-7100) and a field-emission scanning electron microscope (FESEM, JOEL 7600F) operated at a voltage of 5 kV and equipped with an energy-dispersive X-ray spectroscopy (EDX) unit. The crystal powder was characterised by X-ray powder diffraction (XRD) using a Rigaku X-ray diffractometer equipped with a Cu Kα (λ = 0.15406 nm) radiation source; samples were scanned at a rate of 40/min. Pellets of the calcium carbonate nanocrystals were calibrated in a weight proportion of 1 wt% in Ker, and analyses were performed with a Fourier-transform infrared spectrometer (FTIR, model 100, Perkin Elmer, 710 Bridgeport Avenue, Shelton, CT, USA) in the range of 400–4000 cm−1. Thermogravimetric analysis of the calcium carbonate nanocrystals was performed using a TG-DTA instrument (Netzsch STA449C) with an air flow of 100 mL/min and a heating rate of 10 K/min from room temperature to 1000°C.


## 2.1. Synthesis of Calcium Carbonate Powder

Cockle shells were obtained from market. The calcium carbonate powders were prepared from the cockle shells according to the procedure described by Islam et al. [18]. Samples of the cockle shells were dried in an oven at 50°C for 7 days, and the shells were then crushed and blended into a fine powder, which was sieved through a 90-μm laboratory stainless steel sieve (Endecott, London, England). The calcium carbonate powders were finally packed into a polyethylene plastic bag for further analyses.


## 2.2. Synthesis of Calcium Carbonate Nanocrystals

The synthesis of calcium carbonate nanocrystals was performed through oil-in-water (O/W) microemulsions using a HPH. In this technique, the particles sizes are reduced after leaving the homogenising gap by cavitations, particle collisions, and shear forces [19, 20].The calcium carbonate nanocrystals were prepared by the dissolution of 2 g of dry cockle shell powder in a formulated oil-in-water (O/W) microemulsion, which was moderately stirred by a magnetic stirrer for 5 min at 100 rpm to form a calcium carbonate suspension. The formulated suspension was passed through the liquid inlet of a HPH for premilling at a moderate pressure of 300 and 500 bars for three cycles each. The premilled suspension was collected at the HPH outlet and was again passed through the HPH liquid inlet at a high pressure of 1500 bars for 25 homogenising cycles to obtain the desired product. The product of the crystal suspension was filtered and dried in an oven at 105°C for 24 hours.


## 2.3. Characterisation of Calcium Carbonate Nanocrystals

The following instruments were employed for the observation and characterisation of the calcium carbonate nanocrystals. The morphology and particle size of the nanocrystals were analysed using a transmission electron microscope (TEM, Hitachi H-7100) and a field-emission scanning electron microscope (FESEM, JOEL 7600F) operated at a voltage of 5 kV and equipped with an energy-dispersive X-ray spectroscopy (EDX) unit. The crystal powder was characterised by X-ray powder diffraction (XRD) using a Rigaku X-ray diffractometer equipped with a Cu Kα (λ = 0.15406 nm) radiation source; samples were scanned at a rate of 40/min. Pellets of the calcium carbonate nanocrystals were calibrated in a weight proportion of 1 wt% in Ker, and analyses were performed with a Fourier-transform infrared spectrometer (FTIR, model 100, Perkin Elmer, 710 Bridgeport Avenue, Shelton, CT, USA) in the range of 400–4000 cm−1. Thermogravimetric analysis of the calcium carbonate nanocrystals was performed using a TG-DTA instrument (Netzsch STA449C) with an air flow of 100 mL/min and a heating rate of 10 K/min from room temperature to 1000°C.


## 3. Results and Discussion

### 3.1. FESEM and TEM Characterisation of Calcium Carbonate Nanocrystals

The morphological characteristics of the calcium carbonate nanocrystals presented in Figures1(a) and 1(b) are typical FESEM micrographs of the samples under study. The nanometre-sized and rod-shaped particles in Figure 1(a) were synthesised in the confined microemulsion system, whereas Figure 1(b) shows micrographs of a cockle shell powder without any organic additives. These results indicate a natural ability of the biological system to control specific size and morphology, which is very difficult to achieve using classical methods or colloid-chemistry routes [21]. A living organism has the ability to secrete macromolecules, such as in oyster shells, coral, mollusc shells and bivalve nacre. Living organisms achieve this natural phenomenon by utilising the secreted macromolecules (proteins, polysaccharides, and acidic macromolecules) as the nucleators (usually in the form of phospholipid membranes) to modulate the formation of a unique inorganic-organic material with a special morphology and function [21].FESEM micrographs of (a) cockle shell calcium carbonate nanocrystals and (b) cockle shell powder.
(a)
(b)TEM was also used to study the calcium carbonate crystal particles. The images of the crystal presented in both Figures2(a) and 2(b) reveal a rod shape of calcium carbonate aragonite polymorphs. The particles in Figure 2(a) are uniformly distributed at the nanometre scale and were formed in the microemulsion system; this system is considered an ideal medium for the preparation of inorganic nanoparticles [22]. The nanocrystal particles synthesised in the microemulsion system presented in Figure 2(a) differ in size, being approximately 50 nm with individual particles measuring 12–30 nm; in addition, the shape of the particles is clear, and the difference in the particle size may result from the presence of Tween 80 used in the prepared microemulsion. In contrast, the particles shown in Figure 2(b) agglomerated, and the rod shape was not clear compared with the shape in Figure 2(a), which may be due to the differences in the preparation conditions and the additional surfactant (Tween 80) used. Surfactants, both ionic and nonionic, have been reported to strongly affect the size and morphology of calcium carbonate nanoparticles during synthesis [23]. However, nonionic surfactants have a weaker effect on the morphology than do ionic surfactants [23]. This result is most likely due to the weak interactions between a nonionic surfactant and Ca2+ and CO32- ions [24]; in addition, the microemulsion route, when used for the synthesis of nanoparticles, enables control of the size and morphology of the obtained materials [23].TEM images of (a) rod-shaped nanocrystals synthesised via microemulsion routes and (b) cockle shell powder without organic additive added.
(a)
(b)


### 3.2. FTIR Spectra of Calcium Carbonate Nanocrystals

FTIR spectra of the calcium carbonate nanocrystals are presented in Figures3(a) and 3(b). FTIR spectroscopy is an important instrument used to identity different phases of organic and inorganic compounds and, specifically, calcium carbonate phases due to the differences in their carbonate ions, CO32-. Carbonate ions and similar molecules have four normal modes of vibration peaks: v1, symmetric stretching; v2, out-of-plane bending; v3, doubly degenerate planar asymmetric stretching; and v4, doubly degenerate planar bending [25]. The spectral data obtained for the samples reveal a broad absorption peak of CO32- at ~1455 cm−1, ~1082 cm−1, ~1786 cm−1, ~855 cm−1, and ~709 cm−1, which have been reported to be the common characteristic features of the carbonate ions in calcium carbonate and are the fundamental modes of vibration for this molecule [26]. However, the observed bands at ~1082 cm−1 and ~855 cm−1 were carefully assigned as v1 symmetric stretching and v2 out-of-plane bending modes of CO32-, respectively. The peak at ~1082 cm−1 was only observed in the spectrum of aragonite-phase calcium carbonate, whose CO32- ions are inactive in the infrared region. This observation was verified by other reports in the literature on characteristic infrared bands, which are experimentally not observed in the spectrum of calcite [26]. In contrast, the doubly degenerate peak that appears at ~709 cm−1 can be attributed to the v4 in-plane bending mode of CO32- ions, which indicates a structural change in the calcium ions from the symmetry of the calcite phase. This degeneracy can only be removed by splitting the band into two; thus, the band is attributed to the aragonite phase only, which has been confirmed in the literature [26]. This assertion was also supported by a very broad doubly degenerate band v3 at ~1452 cm−1, which confirms the structural changes in the symmetry of the CO32- molecular ions that correspond to the asymmetric stretching mode of CO32-. A similar result was also reported by Cheng et al. [27]. The fundamental changes in the positions of the vibration mode of a molecule are caused by a modification of the electrostatic valence of the Ca–O bond due to changes in the coordination; the Ca–O bond alteration occurs because the displacement of the carbonate vibration mode changes in the environment of oxygen atoms [26–28]. This evidence further demonstrates that the synthesis involves a single phase of calcium carbonate aragonite crystals. The observed IR frequencies at ~1786 cm−1 and ~252 cm−1 are due to the combination of the fundamental vibration frequencies of the carbonate molecular ions assigned between (v1 and v4) and (v1 and v3), respectively, as reported in the literature [26–28].FTIR spectra of calcium carbonate nanocrystals (a) and cockle shell powder (b).
(a)
(b)Both the cockle shell powder and the synthesised calcium carbonate nanocrystals possess the same vibration frequencies as observed in the FTIR data obtained in Figure3(a). The results demonstrate that the nonionic surfactant (Tween 80) used in the preparation of the microemulsion does not affect the vibration frequencies because no additional peaks were observed when the spectrum of the calcium carbonate nanocrystals was compared with that of the cockle shell powder in Figure 3(b). The cockle shell powder was prepared in distilled water only and without the use of additional organic additives or surfactants. This result may be due to the presence of a natural or organic matrix composed of an elastic biopolymer, such as the silk-like protein chitin; this organic matrix secreted by marine shell plays an important role in controlling the inorganic structure, morphology, size, and polymorphism [28, 29].


### 3.3. Elemental Compositions of Synthesised Nanocrystals and Cockle Shell Powder

The chemical compositions of the samples were analysed using EDX, which revealed the presence of individual elements in the samples. As indicated in Tables1(a) and 1(b), the samples contained almost identical elements, with no significant differences observed between the elements detected in the two samples analysed. Both samples contained negligible traces of elemental sodium, and a minute percentage of aluminium was recorded only in the cockle shell powder (Figure 4(b)). This analysis proves that the composition of the calcium carbonate in the cockle shell powder is not 100% pure due to the presence of other elements such as aluminium and sodium.Table 1
(a) Elemental compositions of calcium carbonate nanocrystals and (b) elemental compositions of cockle shell powder.
(a)
Spectrum
Carbon
Oxygen
Sodium
Calcium
Total (%)
Spectrum 1
20.18
59.51
0.53
19.78
100.00
Spectrum 2
14.44
46.73
0.30
38.53
100.00
Spectrum 3
13.57
28.14
0.18
58.11
100.00
Mean
16.06
44.79
0.34
38.81
100.00
Standard deviation
3.59
15.78
0.17
19.17
Max.
20.18
59.51
0.53
58.11
Min.
12.65
28.14
0.18
19.78
(b)
Spectrum
Carbon
Oxygen
Sodium
Calcium
Aluminium
Total (%)
Spectrum 1
22.18
50.51
0.53
27.60
0.17
100.00
Spectrum 2
12.44
46.32
0.30
30.53
0.41
100.00
Spectrum 3
13.57
37.14
0.18
58.11
100.00
Mean
16.06
44.79
0.34
38.81
100.00
Standard deviation
3.59
15.78
0.17
19.17
Max.
19.82
69.52
0.36
58.11
Min.
13.57
26.42
0.16
23.87EDX spectral data for calcium carbonate nanocrystals and cockle shell powder.
(a)
(b)


### 3.4. X-Ray Diffraction Pattern of Calcium Carbonate Nanocrystals

X-ray diffraction is a sensitive instrument used for the identification of crystalline phases of inorganic compounds. The data obtained from the X-ray diffraction patterns in Figures5(a) and 5(b) demonstrate the crystalline nature and phase composition of both samples under analysis. The X-ray diffraction pattern of the synthesised calcium carbonate nanocrystals and cockle shell powder in Figures 3(a) and of 3(b) exhibits characteristics peaks of aragonite at 2θ values of 26.34°, 33.24°, 45.98° and 26.31°, 33.24°, 45.98°, and respectively, which correlate with (hkl) indices of (111), (012), (221), and (021), (0.12), and (221), respectively. These are the strongest peaks observed in the X-ray diffraction patterns of the analysed samples. However, peaks are also observed at 26.71°, 26.87°, 27.02°, 27.38°, 27.57°, 27.72°, 41.28°, 45.62°, 46.54°, 48.84°, and 52.53°. These values also correspond with calcium carbonate aragonite polymorphs reported in the PDF-4+ data bank of the International Centre for Diffraction Data [30]. All the reflections can be attributed to the pure aragonite phase of calcium carbonate, which validates the FTIR results of the aragonite polymorph of calcium carbonate.X-ray diffraction patterns of calcium carbonate nanocrystals (a) and cockle shell powder (b).
(a)
(b)


### 3.5. Thermal Decomposition of Calcium Carbonate Nanocrystals

Thermogravimetric analyses of the cockle shell powder and the nanocrystals synthesised from the powder were performed using the shrinking core model (SCM), whereby the reaction usually begins from the outer layer of the particles and moves toward the solid, which yields an ash solid as the converted material [5]. Therefore, Figures 6(a) and 6(b) illustrate the weight losses of the samples analysed during the process. Both samples were stable until 300°C and then decomposed in two steps. The first step was the initial process, which started with a very small weight loss of 4.0% due to the moisture content in the samples [31]; a similar result has been reported by Yu et al. [32] for bulk or microcalcium carbonate, and this value would also be the loss for nanoparticles of the same material, as reported as by Mohamed et al. [5]. Endothermic behaviour was also observed in the temperature range from 304 to 373°C, which may be due to the removal of water molecules from the carbonate lattice and the phase transformation of aragonite to calcite due to its unstable nature, as described previously. The phase transition of aragonite to calcite in coral and other marine shells occurs at a lower temperature than that of the phase transition in aragonite of mineral origin [26]. Second, a rapid weight loss of 41.88% and endothermic behaviour from 600 to 800°C were observed in both samples; in this temperature range, volatile minerals in the sample began to decompose, thereby releasing CO2. For the cockle shell powder, the rate of decomposition was slower compared with that of the nanocrystals, as shown in Figure 6(a); this result has been reported in the literature, whereby particles of smaller size decompose faster than larger particles [5] because smaller-sized particles have a greater surface area than larger particles. However, both samples remained unchanged when the temperature reached 900°C. This result indicates the total decomposition of calcium carbonate to CaO and signifies the release of CO2 from calcium carbonate, leaving only the product, that is, “ash” [5]. This assumption derived from the TGA analysis is also supported by the XRD data shown in Figure 5.(a) Graphical representation of nanocrystal TGA results. (b) Graphical representation of cockle shells powder TGA data.
(a)
(b)


## 3.1. FESEM and TEM Characterisation of Calcium Carbonate Nanocrystals

The morphological characteristics of the calcium carbonate nanocrystals presented in Figures1(a) and 1(b) are typical FESEM micrographs of the samples under study. The nanometre-sized and rod-shaped particles in Figure 1(a) were synthesised in the confined microemulsion system, whereas Figure 1(b) shows micrographs of a cockle shell powder without any organic additives. These results indicate a natural ability of the biological system to control specific size and morphology, which is very difficult to achieve using classical methods or colloid-chemistry routes [21]. A living organism has the ability to secrete macromolecules, such as in oyster shells, coral, mollusc shells and bivalve nacre. Living organisms achieve this natural phenomenon by utilising the secreted macromolecules (proteins, polysaccharides, and acidic macromolecules) as the nucleators (usually in the form of phospholipid membranes) to modulate the formation of a unique inorganic-organic material with a special morphology and function [21].FESEM micrographs of (a) cockle shell calcium carbonate nanocrystals and (b) cockle shell powder.
(a)
(b)TEM was also used to study the calcium carbonate crystal particles. The images of the crystal presented in both Figures2(a) and 2(b) reveal a rod shape of calcium carbonate aragonite polymorphs. The particles in Figure 2(a) are uniformly distributed at the nanometre scale and were formed in the microemulsion system; this system is considered an ideal medium for the preparation of inorganic nanoparticles [22]. The nanocrystal particles synthesised in the microemulsion system presented in Figure 2(a) differ in size, being approximately 50 nm with individual particles measuring 12–30 nm; in addition, the shape of the particles is clear, and the difference in the particle size may result from the presence of Tween 80 used in the prepared microemulsion. In contrast, the particles shown in Figure 2(b) agglomerated, and the rod shape was not clear compared with the shape in Figure 2(a), which may be due to the differences in the preparation conditions and the additional surfactant (Tween 80) used. Surfactants, both ionic and nonionic, have been reported to strongly affect the size and morphology of calcium carbonate nanoparticles during synthesis [23]. However, nonionic surfactants have a weaker effect on the morphology than do ionic surfactants [23]. This result is most likely due to the weak interactions between a nonionic surfactant and Ca2+ and CO32- ions [24]; in addition, the microemulsion route, when used for the synthesis of nanoparticles, enables control of the size and morphology of the obtained materials [23].TEM images of (a) rod-shaped nanocrystals synthesised via microemulsion routes and (b) cockle shell powder without organic additive added.
(a)
(b)


## 3.2. FTIR Spectra of Calcium Carbonate Nanocrystals

FTIR spectra of the calcium carbonate nanocrystals are presented in Figures3(a) and 3(b). FTIR spectroscopy is an important instrument used to identity different phases of organic and inorganic compounds and, specifically, calcium carbonate phases due to the differences in their carbonate ions, CO32-. Carbonate ions and similar molecules have four normal modes of vibration peaks: v1, symmetric stretching; v2, out-of-plane bending; v3, doubly degenerate planar asymmetric stretching; and v4, doubly degenerate planar bending [25]. The spectral data obtained for the samples reveal a broad absorption peak of CO32- at ~1455 cm−1, ~1082 cm−1, ~1786 cm−1, ~855 cm−1, and ~709 cm−1, which have been reported to be the common characteristic features of the carbonate ions in calcium carbonate and are the fundamental modes of vibration for this molecule [26]. However, the observed bands at ~1082 cm−1 and ~855 cm−1 were carefully assigned as v1 symmetric stretching and v2 out-of-plane bending modes of CO32-, respectively. The peak at ~1082 cm−1 was only observed in the spectrum of aragonite-phase calcium carbonate, whose CO32- ions are inactive in the infrared region. This observation was verified by other reports in the literature on characteristic infrared bands, which are experimentally not observed in the spectrum of calcite [26]. In contrast, the doubly degenerate peak that appears at ~709 cm−1 can be attributed to the v4 in-plane bending mode of CO32- ions, which indicates a structural change in the calcium ions from the symmetry of the calcite phase. This degeneracy can only be removed by splitting the band into two; thus, the band is attributed to the aragonite phase only, which has been confirmed in the literature [26]. This assertion was also supported by a very broad doubly degenerate band v3 at ~1452 cm−1, which confirms the structural changes in the symmetry of the CO32- molecular ions that correspond to the asymmetric stretching mode of CO32-. A similar result was also reported by Cheng et al. [27]. The fundamental changes in the positions of the vibration mode of a molecule are caused by a modification of the electrostatic valence of the Ca–O bond due to changes in the coordination; the Ca–O bond alteration occurs because the displacement of the carbonate vibration mode changes in the environment of oxygen atoms [26–28]. This evidence further demonstrates that the synthesis involves a single phase of calcium carbonate aragonite crystals. The observed IR frequencies at ~1786 cm−1 and ~252 cm−1 are due to the combination of the fundamental vibration frequencies of the carbonate molecular ions assigned between (v1 and v4) and (v1 and v3), respectively, as reported in the literature [26–28].FTIR spectra of calcium carbonate nanocrystals (a) and cockle shell powder (b).
(a)
(b)Both the cockle shell powder and the synthesised calcium carbonate nanocrystals possess the same vibration frequencies as observed in the FTIR data obtained in Figure3(a). The results demonstrate that the nonionic surfactant (Tween 80) used in the preparation of the microemulsion does not affect the vibration frequencies because no additional peaks were observed when the spectrum of the calcium carbonate nanocrystals was compared with that of the cockle shell powder in Figure 3(b). The cockle shell powder was prepared in distilled water only and without the use of additional organic additives or surfactants. This result may be due to the presence of a natural or organic matrix composed of an elastic biopolymer, such as the silk-like protein chitin; this organic matrix secreted by marine shell plays an important role in controlling the inorganic structure, morphology, size, and polymorphism [28, 29].


## 3.3. Elemental Compositions of Synthesised Nanocrystals and Cockle Shell Powder

The chemical compositions of the samples were analysed using EDX, which revealed the presence of individual elements in the samples. As indicated in Tables1(a) and 1(b), the samples contained almost identical elements, with no significant differences observed between the elements detected in the two samples analysed. Both samples contained negligible traces of elemental sodium, and a minute percentage of aluminium was recorded only in the cockle shell powder (Figure 4(b)). This analysis proves that the composition of the calcium carbonate in the cockle shell powder is not 100% pure due to the presence of other elements such as aluminium and sodium.Table 1
(a) Elemental compositions of calcium carbonate nanocrystals and (b) elemental compositions of cockle shell powder.
(a)
Spectrum
Carbon
Oxygen
Sodium
Calcium
Total (%)
Spectrum 1
20.18
59.51
0.53
19.78
100.00
Spectrum 2
14.44
46.73
0.30
38.53
100.00
Spectrum 3
13.57
28.14
0.18
58.11
100.00
Mean
16.06
44.79
0.34
38.81
100.00
Standard deviation
3.59
15.78
0.17
19.17
Max.
20.18
59.51
0.53
58.11
Min.
12.65
28.14
0.18
19.78
(b)
Spectrum
Carbon
Oxygen
Sodium
Calcium
Aluminium
Total (%)
Spectrum 1
22.18
50.51
0.53
27.60
0.17
100.00
Spectrum 2
12.44
46.32
0.30
30.53
0.41
100.00
Spectrum 3
13.57
37.14
0.18
58.11
100.00
Mean
16.06
44.79
0.34
38.81
100.00
Standard deviation
3.59
15.78
0.17
19.17
Max.
19.82
69.52
0.36
58.11
Min.
13.57
26.42
0.16
23.87EDX spectral data for calcium carbonate nanocrystals and cockle shell powder.
(a)
(b)


## 3.4. X-Ray Diffraction Pattern of Calcium Carbonate Nanocrystals

X-ray diffraction is a sensitive instrument used for the identification of crystalline phases of inorganic compounds. The data obtained from the X-ray diffraction patterns in Figures5(a) and 5(b) demonstrate the crystalline nature and phase composition of both samples under analysis. The X-ray diffraction pattern of the synthesised calcium carbonate nanocrystals and cockle shell powder in Figures 3(a) and of 3(b) exhibits characteristics peaks of aragonite at 2θ values of 26.34°, 33.24°, 45.98° and 26.31°, 33.24°, 45.98°, and respectively, which correlate with (hkl) indices of (111), (012), (221), and (021), (0.12), and (221), respectively. These are the strongest peaks observed in the X-ray diffraction patterns of the analysed samples. However, peaks are also observed at 26.71°, 26.87°, 27.02°, 27.38°, 27.57°, 27.72°, 41.28°, 45.62°, 46.54°, 48.84°, and 52.53°. These values also correspond with calcium carbonate aragonite polymorphs reported in the PDF-4+ data bank of the International Centre for Diffraction Data [30]. All the reflections can be attributed to the pure aragonite phase of calcium carbonate, which validates the FTIR results of the aragonite polymorph of calcium carbonate.X-ray diffraction patterns of calcium carbonate nanocrystals (a) and cockle shell powder (b).
(a)
(b)


## 3.5. Thermal Decomposition of Calcium Carbonate Nanocrystals

Thermogravimetric analyses of the cockle shell powder and the nanocrystals synthesised from the powder were performed using the shrinking core model (SCM), whereby the reaction usually begins from the outer layer of the particles and moves toward the solid, which yields an ash solid as the converted material [5]. Therefore, Figures 6(a) and 6(b) illustrate the weight losses of the samples analysed during the process. Both samples were stable until 300°C and then decomposed in two steps. The first step was the initial process, which started with a very small weight loss of 4.0% due to the moisture content in the samples [31]; a similar result has been reported by Yu et al. [32] for bulk or microcalcium carbonate, and this value would also be the loss for nanoparticles of the same material, as reported as by Mohamed et al. [5]. Endothermic behaviour was also observed in the temperature range from 304 to 373°C, which may be due to the removal of water molecules from the carbonate lattice and the phase transformation of aragonite to calcite due to its unstable nature, as described previously. The phase transition of aragonite to calcite in coral and other marine shells occurs at a lower temperature than that of the phase transition in aragonite of mineral origin [26]. Second, a rapid weight loss of 41.88% and endothermic behaviour from 600 to 800°C were observed in both samples; in this temperature range, volatile minerals in the sample began to decompose, thereby releasing CO2. For the cockle shell powder, the rate of decomposition was slower compared with that of the nanocrystals, as shown in Figure 6(a); this result has been reported in the literature, whereby particles of smaller size decompose faster than larger particles [5] because smaller-sized particles have a greater surface area than larger particles. However, both samples remained unchanged when the temperature reached 900°C. This result indicates the total decomposition of calcium carbonate to CaO and signifies the release of CO2 from calcium carbonate, leaving only the product, that is, “ash” [5]. This assumption derived from the TGA analysis is also supported by the XRD data shown in Figure 5.(a) Graphical representation of nanocrystal TGA results. (b) Graphical representation of cockle shells powder TGA data.
(a)
(b)


## 4. Conclusions

Cockle shells consist of a higher percentage of calcium carbonate aragonite polymorphs, as described in the introduction of this paper. On the basis of the analysis of calcium carbonate nanocrystals from the cockle shell powder and that of the powder itself, the shells are composed of the aragonite form of calcium carbonate, which is less stable and denser than calcite. These properties make it a potential biomaterial for medical applications. The thermogravimetric analyses of the two samples revealed the solid-state phase transformation of aragonite to calcite. The transformation of aragonite began at approximately at 300–373°C and at 600–700°C; the complete removal of volatile substances occurred, and the phase transformation of aragonite to calcite was completed with a loss of 41% of the initial weight of the sample. These results also demonstrate that smaller particles decompose faster than larger particles within a short time at low temperatures.The methods adopted and the nonionic surfactant used in the synthesis of aragonite nanocrystals are environmentally friendly and could be scaled up for industrial production, thereby permitting a greener synthesis from naturally available materials and utilising the waste shells that are a by-product of the seafood industry. This method thus offers a great opportunity for exploitation in numerous industrial applications.



---

*Source: 398357-2013-04-15.xml*