# Mechanochemical Preparation of Cobalt Nanoparticles through a Novel Intramolecular Reaction in Cobalt(II) Complexes

Authors: Seyed Abolghasem Kahani; Massumeh Khedmati
Journal: Journal of Nanomaterials
 (2015)

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## Abstract

A novel solid state reaction involving a series of cobalt(II) hydrazine-azides has been used to prepare metallic cobalt nanoparticles. The reactions of [Co(N2H4)(N3)2], [Co(N2H4)2(N3)2], and [Co(N2H4)(N3)Cl]·H2O via NaOH, KOH as reactants were carried out in the solid state. These complexes undergo an intramolecular two-electron oxidation-reduction reaction at room temperature, producing metallic cobalt nanoparticles (Co1–Co6). The aforementioned complexes contain cobalt(II) that is an oxidizing agent and also hydrazine ligand as a reducing agent. Other products produced include sodium azide and ammonia gas. The cobalt metal nanoparticles were characterized using X-ray powder diffraction (XRD), scanning electron microscopy (SEM), and vibrating sample magnetometer (VSM). The synthesized cobalt nanoparticles have similar morphologies; however, their particle size distributions are different.


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## Body

## 1. Introduction

Among the ferromagnetic elements, Co nanoparticles have a wide range of applications in catalysis, optoelectronics, magnetic recording media, and rechargeable batteries [1–3]. Many interesting properties were observed when magnetic metal particles were being prepared in nanoscale. For example, as particle size decreases, the surface-to-volume ratio increases, and properties which depend on this ratio change. Thus, nanoparticles show many unusual chemical and physical properties compared to bulk particles [4]. In an elaboration of this kind of approach, various methods have been developed for the synthesis of metal nanoparticles including vapor, liquid, and solid state processing routes [5, 6]. In the literature, the top-down and the bottom-up approaches are used to synthesize nanoparticles [7]. The mechanochemical synthesis is an interdisciplinary new approach between the top-down and bottom-up approaches [8]. The idea of performing reactions directly between solids, excluding the dissolving stage, is attractive to chemists because reactions in aqueous solution undergo side reactions [9]. Mechanochemistry refers to reactions that are induced by mechanical processes, milling, or grinding. The synthesis of nanocrystalline materials by mechanical milling, mechanical alloying, and mechanochemical processing has been studied [10]. On the other hand, the study of coordination mechanochemical redox reactions is still in its infancy [11, 12]. The chemistry of coordination compounds is a wide area of inorganic chemistry and an enormous number of reactions are known to occur in these compounds [13]. The numerous types of reactions including ligand exchange reactions, isomerization reactions, redox reactions, and reactions of coordinated ligands have been reported in the solid state [14]. The electronic interactions between metal and ligands play a prominent role in the intramolecular reactions [15]. Consequently, intramolecular electron transfer involving metal and ligands takes place between coupled redox centers. In many cases, ligand to metal charge transfer excitation is associated with the reduction of the metal and oxidation of the ligand but in some cases the ligand serves as the source of the reducing agent [16]. Hydrazine is such a compound, and the preparation of many complexes is based on it [17]. The extensive coordination chemistry of hydrazine is evidence for this type of reaction [18]. Transition metal complexes have several unique features in reactions. The most important one is the pattern of electron transfer [19]. So far, there are no reports in the field of mechanochemical reduction of cobalt(II) complexes to metallic cobalt nanoparticles in any literature. In undertaking this project, [Co(N2H4)(N3)2], [Co(N2H4)2(N3)2], and [Co(N2H4)(N3)Cl]·H2O complexes are used for the preparation of cobalt nanoparticles in the solid state. Results show that an electron is transferred from ligand to metal, and an intramolecular oxidation reduction reaction has occurred. A new preparation method of nickel nanoparticles in the solid state at room temperature has been reported [20]. Here this new method is extended to cobalt(II) complexes. These researches join the topics of the intramolecular reaction, metals, mechanochemistry, nanoscience, and coordination chemistry. Using coordination compounds as reactants in the preparation of metallic nanoparticles creates a new area of research in coordination chemistry.


## 2. Experimental

### 2.1. Starting Materials

All chemical reagents used in this experiment were pure grade and used without further purification. Cobalt sulfate heptahydrate, cobalt chloride hexahydrate, sodium azide, hydrazine monohydrate solution, sodium hydroxide, and potassium hydroxide were purchased from Merck. The water used throughout this work was doubly distilled water.


### 2.2. Synthesis of [Co(N2H4)(N3)2] Complex

Using hydrazine (N2H4) as a cobridge with azide, a honeycomb layered cobalt(II) coordination polymer [Co(N2H4)(N3)2] is obtained as follows.An aqueous solution (10 mL) of hydrazine sulfate (0.13 g, 1.0 mmol) and CoSO4
·7H2O (0.28 g, 1.0 mmol) was heated at 93°C for 10 min and then quickly mixed with a hot aqueous solution (15 mL) of excessive NaN3 (1.3 g, 20 mmol). The mixed purple solution was kept at 93°C for 10 min without disturbance. After slow cooling down to room temperature at 5°C/h, dark-red column crystals were obtained. The crystals were filtered and washed with distilled water and ethanol, respectively, and then dried in vacuo [21].


### 2.3. Synthesis of [Co(N2H4)2(N3)2] Complex

Co(N3)2 in solution was obtained by reacting the cobalt(II) chloride with sodium azide solution 1 : 2. Cobalt(II) azide molar ratios CoCl2
·6H2O (4.80 g, 20 mmol) reacted with NaN3 (2.60 g, 40 mmol) in 50 mL water. Stoichiometry amounts of hydrazine hydrate (2.40 g, 40 mmol) were added to the Co(N3)2 solution. The solutions were continuously stirred in an ice bath for 0.5 h. The solid complex, thus obtained, was filtered and washed with dilute ethanol and dried over anhydrous calcium chloride [22].


### 2.4. Synthesis of [Co(N2H4)(N3)Cl]·H2O Complex

Co(N3)Cl in solution was obtained by reacting the cobalt(II) chloride with sodium azide solution 1 : 1 molar ratios in 50 mL water. Stoichiometry amounts of hydrazine hydrate (1.20 g, 20 mmol) were added to the Co(N3)Cl solution. The solutions were continuously stirred in an ice bath for 0.5 h. The solid complex, thus obtained, was filtered and washed with dilute ethanol and dried over anhydrous calcium chloride [22].


### 2.5. The Mechanochemical Synthesis of Cobalt Nanoparticles

A mixture 0.175 g (0.1 mmole) of [Co(N2H4)(N3)2] complex and 0.5 g (12.5 mmole) sodium hydroxide in excess was loaded into a mortar pestle of 50 mL capacity. The stoichiometry of reactions between cobalt(II) hydrazine complex and alkali bases (NaOH, KOH) was 1 : 2.5, and grinding was carried out for 1 h. For the purification process, the product was transferred to a beaker and washed. The product (Co1) was washed with methanol, filtered, and dried in a vacuum oven at room temperature for a period of at least 24 h. A similar procedure for the preparation of Co2 from [Co(N2H4)2(N3)2] (0.207 g, 0.1 mmole) and NaOH (0.5 g, 12.5 mmole) is carried out. In the reaction between [Co(N2H4)(N3)Cl]·H2O complex (0.203 g, 0.1 mmole) and NaOH (0.5 g, 12.5 mmole), Co3 nanoparticles were produced. In the preparation of Co4, Co5, and Co6 the mole ratio is similar to Co1, Co2, and Co3, respectively. However, in the preparation of Co4, Co5, and Co6, the alkaline reactant is KOH. In the solid phase, an intramolecular redox chemical reaction between ligand and central atom occurred, and cobalt metal generated ((1), (2), and (3)). The following reactions take place at room temperature in the solid phase:
(1)
[
Co
N
2
H
4
N
3
2
]
+
5
2
NaOH
⟶
1
2
NH
3
+
5
2
NaN
3
+
Co
+
5
2
H
2
O
(2)
[
Co
N
2
H
4
2
N
3
2
]
+
5
2
NaOH
⟶
1
2
NH
3
+
5
2
NaN
3
+
Co
+
5
2
H
2
O
+
N
2
H
4
(3)
Co
N
2
H
4
N
3
Cl
·
H
2
O
+
5
2
NaOH
⟶
1
2
NH
3
+
3
2
NaN
3
+
Co
+
7
2
H
2
O
+
NaClSimilar reactions occurred in the presence of KOH as alkaline in solid state reaction. During the milling of reactants in the redox reactions ammonia gas is released, and NaN3 was produced. Ammonia combines with hydrochloric acid and forms ammonium chloride. Colorimetric testing can be used to detect NaN3 [23]. A drop of the filtered solution is placed in the depression of a spot plate and treated with 1 or 2 drops of dilute hydrochloric acid. A drop of ferric chloride solution is added and the spot plate gently heated. A red color indicates hydrazoic acid and thus the presence of sodium azide in the solution.


### 2.6. Characterization of Materials

The cobalt complex and cobalt powders were characterized by X-ray powder diffraction (XRD). XRD measurements were performed using a Philips X’pert pro MPD diffractometer with Cu Kα radiation in the range 2θ from 10 to 80 at room temperature. IR spectra were obtained as KBr pellets in the range 4000 to 400 cm−1 using a Shimadzu FTIR spectrometer. Scanning electron microscopy (Philips XL30ESEM) was used to characterize cobalt nanoparticles. A vibrating sample magnetometer (VSM, Meghnatis Daghigh Kavir Co.) was used to evaluate the magnetic parameters of cobalt nanoparticles.


## 2.1. Starting Materials

All chemical reagents used in this experiment were pure grade and used without further purification. Cobalt sulfate heptahydrate, cobalt chloride hexahydrate, sodium azide, hydrazine monohydrate solution, sodium hydroxide, and potassium hydroxide were purchased from Merck. The water used throughout this work was doubly distilled water.


## 2.2. Synthesis of [Co(N2H4)(N3)2] Complex

Using hydrazine (N2H4) as a cobridge with azide, a honeycomb layered cobalt(II) coordination polymer [Co(N2H4)(N3)2] is obtained as follows.An aqueous solution (10 mL) of hydrazine sulfate (0.13 g, 1.0 mmol) and CoSO4
·7H2O (0.28 g, 1.0 mmol) was heated at 93°C for 10 min and then quickly mixed with a hot aqueous solution (15 mL) of excessive NaN3 (1.3 g, 20 mmol). The mixed purple solution was kept at 93°C for 10 min without disturbance. After slow cooling down to room temperature at 5°C/h, dark-red column crystals were obtained. The crystals were filtered and washed with distilled water and ethanol, respectively, and then dried in vacuo [21].


## 2.3. Synthesis of [Co(N2H4)2(N3)2] Complex

Co(N3)2 in solution was obtained by reacting the cobalt(II) chloride with sodium azide solution 1 : 2. Cobalt(II) azide molar ratios CoCl2
·6H2O (4.80 g, 20 mmol) reacted with NaN3 (2.60 g, 40 mmol) in 50 mL water. Stoichiometry amounts of hydrazine hydrate (2.40 g, 40 mmol) were added to the Co(N3)2 solution. The solutions were continuously stirred in an ice bath for 0.5 h. The solid complex, thus obtained, was filtered and washed with dilute ethanol and dried over anhydrous calcium chloride [22].


## 2.4. Synthesis of [Co(N2H4)(N3)Cl]·H2O Complex

Co(N3)Cl in solution was obtained by reacting the cobalt(II) chloride with sodium azide solution 1 : 1 molar ratios in 50 mL water. Stoichiometry amounts of hydrazine hydrate (1.20 g, 20 mmol) were added to the Co(N3)Cl solution. The solutions were continuously stirred in an ice bath for 0.5 h. The solid complex, thus obtained, was filtered and washed with dilute ethanol and dried over anhydrous calcium chloride [22].


## 2.5. The Mechanochemical Synthesis of Cobalt Nanoparticles

A mixture 0.175 g (0.1 mmole) of [Co(N2H4)(N3)2] complex and 0.5 g (12.5 mmole) sodium hydroxide in excess was loaded into a mortar pestle of 50 mL capacity. The stoichiometry of reactions between cobalt(II) hydrazine complex and alkali bases (NaOH, KOH) was 1 : 2.5, and grinding was carried out for 1 h. For the purification process, the product was transferred to a beaker and washed. The product (Co1) was washed with methanol, filtered, and dried in a vacuum oven at room temperature for a period of at least 24 h. A similar procedure for the preparation of Co2 from [Co(N2H4)2(N3)2] (0.207 g, 0.1 mmole) and NaOH (0.5 g, 12.5 mmole) is carried out. In the reaction between [Co(N2H4)(N3)Cl]·H2O complex (0.203 g, 0.1 mmole) and NaOH (0.5 g, 12.5 mmole), Co3 nanoparticles were produced. In the preparation of Co4, Co5, and Co6 the mole ratio is similar to Co1, Co2, and Co3, respectively. However, in the preparation of Co4, Co5, and Co6, the alkaline reactant is KOH. In the solid phase, an intramolecular redox chemical reaction between ligand and central atom occurred, and cobalt metal generated ((1), (2), and (3)). The following reactions take place at room temperature in the solid phase:
(1)
[
Co
N
2
H
4
N
3
2
]
+
5
2
NaOH
⟶
1
2
NH
3
+
5
2
NaN
3
+
Co
+
5
2
H
2
O
(2)
[
Co
N
2
H
4
2
N
3
2
]
+
5
2
NaOH
⟶
1
2
NH
3
+
5
2
NaN
3
+
Co
+
5
2
H
2
O
+
N
2
H
4
(3)
Co
N
2
H
4
N
3
Cl
·
H
2
O
+
5
2
NaOH
⟶
1
2
NH
3
+
3
2
NaN
3
+
Co
+
7
2
H
2
O
+
NaClSimilar reactions occurred in the presence of KOH as alkaline in solid state reaction. During the milling of reactants in the redox reactions ammonia gas is released, and NaN3 was produced. Ammonia combines with hydrochloric acid and forms ammonium chloride. Colorimetric testing can be used to detect NaN3 [23]. A drop of the filtered solution is placed in the depression of a spot plate and treated with 1 or 2 drops of dilute hydrochloric acid. A drop of ferric chloride solution is added and the spot plate gently heated. A red color indicates hydrazoic acid and thus the presence of sodium azide in the solution.


## 2.6. Characterization of Materials

The cobalt complex and cobalt powders were characterized by X-ray powder diffraction (XRD). XRD measurements were performed using a Philips X’pert pro MPD diffractometer with Cu Kα radiation in the range 2θ from 10 to 80 at room temperature. IR spectra were obtained as KBr pellets in the range 4000 to 400 cm−1 using a Shimadzu FTIR spectrometer. Scanning electron microscopy (Philips XL30ESEM) was used to characterize cobalt nanoparticles. A vibrating sample magnetometer (VSM, Meghnatis Daghigh Kavir Co.) was used to evaluate the magnetic parameters of cobalt nanoparticles.


## 3. Results and Discussion

In the solid state [Co(N2H4)(N3)2], [Co(N2H4)2(N3)2], and [Co(N2H4)(N3)Cl]·H2O undergo an intramolecular two-electron oxidation reduction reaction. These reactions under alkaline condition (NaOH, KOH) lead to formation of cobalt metal, azide, and ammonia. Depending on the oxidizing agent, pH, and temperature, hydrazine reacts in different pathways. In aqueous solution, hydrazine reacts as one, two, or four electron oxidation paths and is converted to a mixture of dinitrogen and ammonia, azide, and ammonia and/or only dinitrogen, respectively. The redox reactions of hydrazine cobalt(II) complexes have several unique features, the most important of them being the patterns of electron transfer from ligand to metal. On the other hand, these mechanochemical reactions occurred at room temperature, and the final main product is metallic cobalt nanoparticles. In this work, the cobalt nanoparticles are prepared with different shapes by using a mechanochemical route. However, when the cobalt complex as a reactant was used in aqueous solution, cobalt nanoparticles with different morphologies were formed [24]. The metallic cobalt nanoparticles were characterized using XRD, IR, VSM, and SEM analysis.


### 3.1. Analysis of Metallic Cobalt Nanoparticles Crystalline Phase

According to the XRD pattern in the literature, [Co(N2H4)(N3)2] crystallizes in the orthorhombic system and space groupC2221. This complex is showed as a cobridge with azide and hydrazine and honeycomb layered cobalt(II) coordination polymer [21]. However, XRD patterns and crystal structure of [Co(N2H4)2(N3)2] and [Co(N2H4)(N3)Cl]·H2O have not been reported. During solid state reactions, all complexes are converted to metallic cobalt; thus, all diffraction peaks related to complex patterns disappeared. In accordance with the diffraction pattern analyses, it could be concluded that the nanoparticles prepared in this work were pure hcp cobalt. The cobalt nanoparticles have JCPDS card no. 05-0727 and P63/mmc space group. The mechanochemical reaction of cobalt(II) complex to metallic cobalt is accompanied by a change in the crystal structure. All the diffraction peaks can be well indexed to hcp phase cobalt, with lattice constants of a
0
=
2.5031 Å c
0
=
4.0605 Å. The fundamental difference between crystalline and amorphous solids is due to their X-ray diffraction patterns. However, poor crystallinity of the powder results in broad peaks in the X-ray pattern. There are different lines broadening sources, such as crystallite size, lattice strain, anisotropic sample broadening, and faulting, tending to produce different effects on the line profiles. Here in the metallic cobalt pattern the background noise from fluoresced X-rays is increased, which is most problematic in powder diffraction (Figure 1). The choice of X-ray source in X-ray powder diffraction is dependent on the material that must be analyzed. Some atoms absorb incident X-rays and fluoresce by the absorption of X-rays, which decreases the diffracted signal, and also the fluoresced X-rays increase the background noise. When copper radiation is employed, the X-ray powder pattern of cobalt nanoparticles demonstrates the effect of fluorescence on the diffraction pattern [25]. Therefore there is an uncertainty in the estimation of crystallite size from the full width at half maximum (FWHM) of the diffraction peaks by the Scherrer formula. The pattern of X-ray diffraction shows the crystalline structure of final products. All the diffraction peaks can be well indexed to the hexagonal phase of cobalt.Figure 1
X-ray diffraction patterns of the Co(N2H4)(N3)2, Co(N2H4)2(N3)2, and Co(N2H4)(N3)Cl and their products, cobalt metal nanoparticles (Co1–Co6), in hcp lattice.


### 3.2. Infrared Spectra of Complexes and Cobalt Nanoparticles

Vibration spectra of [Co(N2H4)(N3)2], [Co(N2H4)2(N3)2], and [Co(N2H4)(N3)Cl]·H2O show N2H4 and azido vibrations frequencies (Figure 2). Hydrazine coordinates to a Co(II) as a bridging bidentate ligand showing bands (N-N) near 970 cm−1 [26]. Here the azido vibrations appear at 2010–2050, 1260–1350, and 610–670 cm−1. The antisymmetric and symmetric N
3
- stretching absorption bands occur at 2010–2050 cm−1 and 1260–1350, respectively; the deformation stretching also was observed at 610–670 cm−1 [27]. In the chemical reaction, the cobalt complexes are converted to cobalt metal nanoparticles (Co1–Co6); thus, the absorption bands due to ligands group in complexes disappeared and the metallic cobalt nanoparticles have no absorption bands in medium IR.Figure 2
IR spectra of Co(N2H4)(N3)2, Co(N2H4)2(N3)2, and Co(N2H4)(N3)Cl in the region 400–4000 cm−1, and cobalt nanoparticles (Co1–Co6) are produced, and all the absorption bands disappear.


### 3.3. Magnetic Properties of Metallic Cobalt Nanoparticles

Cobalt nanoparticles were prepared from [Co(N2H4)(N3)2], [Co(N2H4)2(N3)2], and [Co(N2H4)(N3)Cl]·H2O by chemical redox reaction in solid state. The magnetic susceptibility reveals paramagnetic and a week interaction between cobalt(II) ions in the polynuclear complex [21]. The conversion of cobalt(II) complexes to metallic cobalt can be accompanied by a change in magnetization. These molecular paramagnetic complexes are changed into ferromagnetic cobalt metal nanoparticles (Figure 3). The saturation magnetization (M
S) values of Co1, Co2, Co3, Co4, Co5, and Co6 at 298 K were 135.45, 99.62, 88.33, 68.68, 113.92, and 119.18 emu/g, respectively (Table 1). Here the cobalt nanoparticles have a saturation magnetization less than that of the bulk cobalt. The M
S value of the bulk cobalt was about 162.5 emu/g at 300 K. It is known that the magnetization behavior of a magnetic material is highly size dependent. Despite the endless number of reports on magnetic studies of magnetic nanoparticles the influence of particle size on the magnetic properties has not been systematically studied [28]. The metallic cobalt nanoparticles show magnetic parameters such as saturation magnetization and coercivity that vary with particle size, usually in a nonlinear fashion [29, 30]. It is envisaged that the application of Co nanoparticles can be expanded once the intrigue relationship between magnetic properties and particle size of Co can be delineated. The large magnetic particle contains mobile walls when the size of the particle decreases below a critical size, the domain walls disappear, and the particles become single domain. Magnetic particles in the nanometer-size range are necessarily single-magnetic-domain structures. The critical size depends on the saturated magnetization, anisotropy energy, and exchange interaction between individual spins [31].Table 1
Magnetic parameters in cobalt metal nanoparticles that have been measured at 298 K.
Sample
H
c (Oe)
M
r (emu/g)
M
S (emu/g)
Co1
398.05
20.19
135.45
Co2
341.18
15.49
99.62
Co3
389.92
15.33
88.33
Co4
471.16
11.72
68.68
Co5
398.05
19.48
113.92
Co6
235.58
15.48
119.18Figure 3
Hysteresis loop and the saturation magnetizations of cobalt nanoparticles have been measured at 298 K (Co1 = 135.45, Co2 = 99.62, Co3 = 88.33, Co4 = 68.68, Co5 = 113.92, and Co6 = 119.18 emu/g), respectively.


### 3.4. Analysis of Cobalt Particles Morphologies

Figure4 shows an SEM image of a typical cobalt particle prepared via intramolecular chemical reduction. Morphology of the cobalt nanoparticles was dependent on the complex structure as reactant. The SEM of Co1 and Co2 show aggregated pore structure containing the nanosheets and nanosheet thickness ranging from 35 nm to 60 nm. An aggregated spherical particle without pore is observed in Co3 and Co4, and their particle sizes are ranging from 50 nm to 80 nm. The Co5 and Co6 nanoparticles have pore structure containing the nanosheets and nanosheet thickness ranging from 25 nm to 35 nm. The statistical analysis shows that Co1, Co2, Co5, and Co6 nanoparticles have similar morphology, whereas Co3 and Co4 nanoparticles have a different morphology. The results show that when polynuclear complex [Co(N2H4)(N3)2] is used in the reaction, the product changes to aggregated without pore and nanosheet cobalt nanoparticles. However when mononuclear complexes [Co(N2H4)2(N3)2] and [Co(N2H4)(N3)Cl]·H2O are used, the complex is converted to an aggregated powder of Co1, Co2, Co5, and Co6, respectively. On the other hand the results show that when alkaline media are changed from NaOH to KOH, respectively, the morphology of metallic cobalt nanoparticles has significantly changed. In the new solid state method an intramolecular chemical reduction of the cobalt complex causes the formation of particles in the nanoscale range. Besides XRD patterns and SEM micrographs of metallic cobalt phase formation are confirmed by using the energy-dispersive X-ray (EDX) data. The EDX spectra acquired at low magnification of the powders are shown in Figure 5. Energy-dispersive X-ray analysis of these prepared cobalt nanoparticles, show that they are all pure.Figure 4
SEM show morphologies and particle size distributions in metallic cobalt nanoparticles (Co1 and Co2) aggregated nanosheet with thickness 35–60 nm; (Co3 and Co4) aggregated spherical particles with size 50–80 nm; (Co5 and Co6) aggregated nanosheet with thickness 25–35 nm.Figure 5
Energy-dispersive X-ray spectrum of metallic cobalt nanoparticle that is prepared from Co(N2H4)(N3)2 complex.


## 3.1. Analysis of Metallic Cobalt Nanoparticles Crystalline Phase

According to the XRD pattern in the literature, [Co(N2H4)(N3)2] crystallizes in the orthorhombic system and space groupC2221. This complex is showed as a cobridge with azide and hydrazine and honeycomb layered cobalt(II) coordination polymer [21]. However, XRD patterns and crystal structure of [Co(N2H4)2(N3)2] and [Co(N2H4)(N3)Cl]·H2O have not been reported. During solid state reactions, all complexes are converted to metallic cobalt; thus, all diffraction peaks related to complex patterns disappeared. In accordance with the diffraction pattern analyses, it could be concluded that the nanoparticles prepared in this work were pure hcp cobalt. The cobalt nanoparticles have JCPDS card no. 05-0727 and P63/mmc space group. The mechanochemical reaction of cobalt(II) complex to metallic cobalt is accompanied by a change in the crystal structure. All the diffraction peaks can be well indexed to hcp phase cobalt, with lattice constants of a
0
=
2.5031 Å c
0
=
4.0605 Å. The fundamental difference between crystalline and amorphous solids is due to their X-ray diffraction patterns. However, poor crystallinity of the powder results in broad peaks in the X-ray pattern. There are different lines broadening sources, such as crystallite size, lattice strain, anisotropic sample broadening, and faulting, tending to produce different effects on the line profiles. Here in the metallic cobalt pattern the background noise from fluoresced X-rays is increased, which is most problematic in powder diffraction (Figure 1). The choice of X-ray source in X-ray powder diffraction is dependent on the material that must be analyzed. Some atoms absorb incident X-rays and fluoresce by the absorption of X-rays, which decreases the diffracted signal, and also the fluoresced X-rays increase the background noise. When copper radiation is employed, the X-ray powder pattern of cobalt nanoparticles demonstrates the effect of fluorescence on the diffraction pattern [25]. Therefore there is an uncertainty in the estimation of crystallite size from the full width at half maximum (FWHM) of the diffraction peaks by the Scherrer formula. The pattern of X-ray diffraction shows the crystalline structure of final products. All the diffraction peaks can be well indexed to the hexagonal phase of cobalt.Figure 1
X-ray diffraction patterns of the Co(N2H4)(N3)2, Co(N2H4)2(N3)2, and Co(N2H4)(N3)Cl and their products, cobalt metal nanoparticles (Co1–Co6), in hcp lattice.


## 3.2. Infrared Spectra of Complexes and Cobalt Nanoparticles

Vibration spectra of [Co(N2H4)(N3)2], [Co(N2H4)2(N3)2], and [Co(N2H4)(N3)Cl]·H2O show N2H4 and azido vibrations frequencies (Figure 2). Hydrazine coordinates to a Co(II) as a bridging bidentate ligand showing bands (N-N) near 970 cm−1 [26]. Here the azido vibrations appear at 2010–2050, 1260–1350, and 610–670 cm−1. The antisymmetric and symmetric N
3
- stretching absorption bands occur at 2010–2050 cm−1 and 1260–1350, respectively; the deformation stretching also was observed at 610–670 cm−1 [27]. In the chemical reaction, the cobalt complexes are converted to cobalt metal nanoparticles (Co1–Co6); thus, the absorption bands due to ligands group in complexes disappeared and the metallic cobalt nanoparticles have no absorption bands in medium IR.Figure 2
IR spectra of Co(N2H4)(N3)2, Co(N2H4)2(N3)2, and Co(N2H4)(N3)Cl in the region 400–4000 cm−1, and cobalt nanoparticles (Co1–Co6) are produced, and all the absorption bands disappear.


## 3.3. Magnetic Properties of Metallic Cobalt Nanoparticles

Cobalt nanoparticles were prepared from [Co(N2H4)(N3)2], [Co(N2H4)2(N3)2], and [Co(N2H4)(N3)Cl]·H2O by chemical redox reaction in solid state. The magnetic susceptibility reveals paramagnetic and a week interaction between cobalt(II) ions in the polynuclear complex [21]. The conversion of cobalt(II) complexes to metallic cobalt can be accompanied by a change in magnetization. These molecular paramagnetic complexes are changed into ferromagnetic cobalt metal nanoparticles (Figure 3). The saturation magnetization (M
S) values of Co1, Co2, Co3, Co4, Co5, and Co6 at 298 K were 135.45, 99.62, 88.33, 68.68, 113.92, and 119.18 emu/g, respectively (Table 1). Here the cobalt nanoparticles have a saturation magnetization less than that of the bulk cobalt. The M
S value of the bulk cobalt was about 162.5 emu/g at 300 K. It is known that the magnetization behavior of a magnetic material is highly size dependent. Despite the endless number of reports on magnetic studies of magnetic nanoparticles the influence of particle size on the magnetic properties has not been systematically studied [28]. The metallic cobalt nanoparticles show magnetic parameters such as saturation magnetization and coercivity that vary with particle size, usually in a nonlinear fashion [29, 30]. It is envisaged that the application of Co nanoparticles can be expanded once the intrigue relationship between magnetic properties and particle size of Co can be delineated. The large magnetic particle contains mobile walls when the size of the particle decreases below a critical size, the domain walls disappear, and the particles become single domain. Magnetic particles in the nanometer-size range are necessarily single-magnetic-domain structures. The critical size depends on the saturated magnetization, anisotropy energy, and exchange interaction between individual spins [31].Table 1
Magnetic parameters in cobalt metal nanoparticles that have been measured at 298 K.
Sample
H
c (Oe)
M
r (emu/g)
M
S (emu/g)
Co1
398.05
20.19
135.45
Co2
341.18
15.49
99.62
Co3
389.92
15.33
88.33
Co4
471.16
11.72
68.68
Co5
398.05
19.48
113.92
Co6
235.58
15.48
119.18Figure 3
Hysteresis loop and the saturation magnetizations of cobalt nanoparticles have been measured at 298 K (Co1 = 135.45, Co2 = 99.62, Co3 = 88.33, Co4 = 68.68, Co5 = 113.92, and Co6 = 119.18 emu/g), respectively.


## 3.4. Analysis of Cobalt Particles Morphologies

Figure4 shows an SEM image of a typical cobalt particle prepared via intramolecular chemical reduction. Morphology of the cobalt nanoparticles was dependent on the complex structure as reactant. The SEM of Co1 and Co2 show aggregated pore structure containing the nanosheets and nanosheet thickness ranging from 35 nm to 60 nm. An aggregated spherical particle without pore is observed in Co3 and Co4, and their particle sizes are ranging from 50 nm to 80 nm. The Co5 and Co6 nanoparticles have pore structure containing the nanosheets and nanosheet thickness ranging from 25 nm to 35 nm. The statistical analysis shows that Co1, Co2, Co5, and Co6 nanoparticles have similar morphology, whereas Co3 and Co4 nanoparticles have a different morphology. The results show that when polynuclear complex [Co(N2H4)(N3)2] is used in the reaction, the product changes to aggregated without pore and nanosheet cobalt nanoparticles. However when mononuclear complexes [Co(N2H4)2(N3)2] and [Co(N2H4)(N3)Cl]·H2O are used, the complex is converted to an aggregated powder of Co1, Co2, Co5, and Co6, respectively. On the other hand the results show that when alkaline media are changed from NaOH to KOH, respectively, the morphology of metallic cobalt nanoparticles has significantly changed. In the new solid state method an intramolecular chemical reduction of the cobalt complex causes the formation of particles in the nanoscale range. Besides XRD patterns and SEM micrographs of metallic cobalt phase formation are confirmed by using the energy-dispersive X-ray (EDX) data. The EDX spectra acquired at low magnification of the powders are shown in Figure 5. Energy-dispersive X-ray analysis of these prepared cobalt nanoparticles, show that they are all pure.Figure 4
SEM show morphologies and particle size distributions in metallic cobalt nanoparticles (Co1 and Co2) aggregated nanosheet with thickness 35–60 nm; (Co3 and Co4) aggregated spherical particles with size 50–80 nm; (Co5 and Co6) aggregated nanosheet with thickness 25–35 nm.Figure 5
Energy-dispersive X-ray spectrum of metallic cobalt nanoparticle that is prepared from Co(N2H4)(N3)2 complex.


## 4. Conclusions

The common method is used in the preparation of metallic cobalt nanoparticles which is the chemical reduction of cobalt(II) salts by hydrazine in alcoholic solution at 60–70°C. There are many substances that contributed in the reactions and the high temperature causes many side reactions on metallic nanoparticle. Here we proposed a new method for the preparation of cobalt nanoparticles in the solid state at room temperature. Besides being able to react at room temperature conditions, the complex has both oxidizing and reducing properties. In all aqueous preparation of metallic cobalt by hydrazine a 4e− oxidation reduction pathway has been reported but here we observed a new 2e− oxidation reduction pathway in the solid state reaction. This is a new methodology in the intramolecular reaction at room temperature. Fine cobalt powders with a different morphology were prepared from cobalt(II) hydrazine complexes by intramolecular redox reaction in solid state. Here depending on the interaction between the metal ion and ligands a special cobalt(II) complex for intramolecular redox reaction is designed. Therefore, the coordination sphere of complex has a profound effect on the intramolecular redox reaction. The results show that when complexes and alkaline media are changed the morphology of metallic cobalt nanoparticles has significantly changed. However, the cobalt metal is produced from [Co(N2H4)(N3)2] complex and has completely different morphology than ones prepared from [Co(N2H4)2(N3)2] and [Co(N2H4)(N3)Cl]·H2O. The advantages of this work for preparing the metallic powders lie in variation on morphology, the high yield, and solid state reaction conditions. In comparison with the method of preparing cobalt powders from cobalt(II) salts in aqueous solution, the intramolecular redox reaction of cobalt(II) hydrazine complexes show a high purity of metal cobalt. Therefore, mechanochemical intramolecular redox reaction is attractive and offers a new method in preparation of metallic cobalt nanoparticle.



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