Sol-Gel Route for the Synthesis of CoFe2-x Er x O4 Nanocrystalline Ferrites and the Investigation of Structural and Magnetic Properties for Magnetic Device Applications.

This study reports the formation of Er-doped nanocrystalline cobalt ferrite with the formula CoFe2-x Er x O4 (0.0 ≤ x ≤ 0.10) from nontoxic metal precursors Co(NO3)2·6H2O, Fe(NO3)3·9H2O, and Er(NO3)3·5H2O through an easy and economical sol-gel route in which citric acid is served as the chelating agent. The as-prepared powder was annealed at 700 °C for 3 h in ambient air to get the required spinel structure. The annealed samples were subjected to structural and magnetic characterization. The X-ray diffraction (XRD) data of the samples confirmed the cubic spinel structure formation. The average crystallite size evaluated from XRD data increased from 21 to 34 nm with the substitution of Er due to the larger atomic size of Er3+ than Fe3+. Moreover, the crystallite size obtained from XRD data are well matched with the particle size measured from transmission electron microscopy images. The lattice parameters obtained from XRD data agree well with the values estimated from theoretical cation distribution and Rietveld refinement calculation. The hysteresis curve exhibits the particles are soft ferromagnetic and the coercivity increased from 54.7 to 76.6 kA/m with maximum saturation magnetization, M s = 61 emug-1 for 0.10 Er content. The squareness ratios were found to be less than 0.5, which indicates the single-domain nature of our particles. The blocking temperature measured from field cooled-zero field cooled curves is T B > 350 K for all the samples, which is much higher than the room temperature (300 K). The enhancement of saturation magnetization and coercivity has been explained based on the crystallite size, anisotropy constant, and cation distribution. Thus, the structural and magnetic properties of CoFe2O4 nanoparticles (NPs) can be tuned by Er incorporation and these NPs can be applied in different soft magnetic devices.

Introduction

There is a growing interest in magnetic materials and magnetic oxides owing to their variety of applications. Researchers have given special importance to nanosized soft ferromagnets because of their potential applications in power generation, data storage, magnetic diagnostics, magnetic shielding, and so on.[1,2] Among different magnetic materials, spinel cobalt (Co) ferrites have drawn continuous attention because of their soft ferromagnetic nature with high electromagnetic performance and exceptional physical properties.[3,4] The common form of the spinel ferrite structure is (A2+)[B23+]O42–, where the divalent A2+ and trivalent B23+ cations are occupied in the tetrahedral (A) and octahedral (B) sites. The face-centered structure of ferrite arises from the formulation of cations and oxygen anions. When the divalent cations occupy the tetrahedral sites, it forms the normal spinel structure. On the other hand, inverse spinel ferrite is formed when a divalent cation occupies both the tetrahedral and octahedral sites. The physical properties of CoFe2O4 strongly depend on substituting materials, annealing temperature, grain size, and also on the synthesis method. The replacement of trace amounts of rare earth ions on cobalt ferrites can alter their magnetic behaviors, which makes them suitable for hyperthermia applications.[5] The magnetic and dielectric properties of cobalt ferrite rely on the cation distribution, and the properties can be modified by wavering the location of cations in the interstitial sites. Among the rare earth ions, Er3+ is chosen as the doping material as it has a relatively higher magnetic moment (7 μB) than Fe3+ (5.92 μB). The magnetic properties of CoFe2O4 are strongly affected by the spin coupling of the 3d electrons (Fe3+–Fe3+ interactions). For example, the substitution of rare earth ions, such as Er3+ (4f electrons) to Fe3+ (3d electrons), yields spin coupling of 3d–4f electrons (Re3+–Fe3+ interactions), which may lead to changes in the magnetic properties of CoFe2O4.[6−8] The alteration of magnetization and coercivity were reported for Sn-doped cobalt ferrite and Er-doped nickel-zinc ferrite nanoparticles (NPs).[9,10] Moreover, the improved dielectric properties were reported for Ho-substituted nanocobalt ferrite.[11] Besides, doping of rare earth ions such as Ce–Dy, Dy3+–Y3+, Ce–Nd,[6−8] Y3+, Ho3+, Sm3+, Nd3+, and Er3+ into the ferrite has changed the structural and magnetic parameters.[12]

Different synthesis techniques such as sol–gel,[4,13,14] sol–gel-assisted auto combustion,[3] microemulsion,[15,16] sonochemical,[7] co-precipitation,[17,18] and hydrothermal[19] have been used to synthesize nanocrystalline Co spinel ferrites. Among them, the sol–gel route is convenient due to its easy preparation, cost effectiveness, and better control of size.[20] During the last 2 decades, a large number of research reports on nanosized CoFe2O4 have been reported using the sol–gel method. However, magnetic studies of Er-doped cobalt ferrites with cation distribution have been rarely reported.[3] Accordingly, in this work, we investigate the effect of Er3+ substitution on the microstructural and magnetic properties of nanosized CoFe2–ErO4 (x = 0, 0.05, and 0.10) powders synthesized through the sol–gel route.

Materials and Methods

The Er-doped spinel cobalt ferrite with the general formula CoFe2–ErO4, (x = 0, 0.05, and 0.10) was synthesized through the conventional sol–gel route. The stoichiometric amounts of 2.328 gm of (0.1 M) Co(NO3)2·6H2O (98%, Loba Chemie), 6.464 gm of (0.2 M) Fe(NO3)3·9H2O (98%, Merck), and 5.067 gm of (0.3 M) Er(NO3)3·5H2O (99.9%, Sigma-Aldrich) were mixed with 80 mL of ethanol. The citric acid was added as the chelating agent. The molar ratios of the raw materials are shown in Table .

Table 1

Characteristics of the Synthesizing Materials

sample	Er content, x	Co/Fe/citric acid molar ratio
1	0	1:2:3
2	0.05	1:1.95:3
3	0.10	1:1.90:3

Then, the mixture was homogenized by stirring magnetically for 2 h using a laboratory water bath at 80 °C for gel formation. Then, the sample was dried at 150 °C for 12 h in an electric microwave oven to completely swell the xerogel. The reticular substance was found after heating at 250 °C for 3 h. The substance was ground to powder in an agate mortar. Then, the powder was annealed at 700 °C for 3 h in ambient air using a high-temperature furnace to obtain the desired nanopowder sample. Figure shows the different steps of synthesis.

Figure 1

Different steps followed in sol–gel synthesis.

The thermogravimetric analysis (TGA) along with the differential thermal analysis (DTA) was performed using Pyris Series-STA-8000 on the ferrite powder to obtain its phase transition temperature. Structural analysis was performed by using a Philips X’Pert Pro X-ray diffractometer (operating at a temperature of 25 °C, at a voltage of 40 kV, and a current of 30 mA) with Cu-kα (λ = 1.54060 Å) radiation. Morphological analysis was performed by using scanning electron microscopy (SEM) (ZEISS EVO-18). The transmission electron microscopy (TEM) (Talos F200X, Thermo Fisher Scientific) images of the samples were taken to measure the size of the particles. The magnetic properties were investigated through a physical property measurement system (PPMS) with an applied magnetic field ±2T.

Results and Discussion

Thermal Analysis

Figure shows the TGA and DTA curves for the CoFe2O4 sample. The TGA curve shows about 70% weight loss at 530 °C. First, 8% weight loss of the sample was observed for moisture from 30 to 180 °C, and then it dropped about 20% weight at 250 °C. Similar weight loss for CoFe2O4 was reported by Rajput et al.[21] The major weight loss from 350 to 530 °C has been attributed to the fragmentation of organic compounds and nitrates. As expected, the decomposition reaction is strongly exothermic and conversions of hydroxides into metal oxides occur in the abovementioned temperature range.[22] The stable phase was observed beyond 550 °C in the TGA curve.

Figure 2

TGA and DTA curves for the as-synthesized CoFe2O4 sample.

In the DTA curve, crystal phase formation peaks were observed at 324 and 370 °C. The exothermic peak at 370 °C indicates the decomposition of organic compounds in the structure due to the crystallization of the spinel ferrite.[22] The area enclosed by the dashed line indicates the stable phase.

Structural Properties

Figure shows the X-ray diffraction (XRD) patterns of undoped and Er-doped CoFe2O4 powder samples (CoFe2–ErO4, x = 0, 0.05, and 0.10) annealed in ambient air at 700 °C for 3 h. Structural properties, for instance, the lattice constant, crystalline size, and other features, were obtained from XRD data. The major reflection peaks of all the planes for different compositions shown (Figure ) correspond to the cubic spinel phase having an Fd3̅m space group (JCPDS card no. 22-1086).[23,24] An insignificant amount of the orthoferrite (ErFeO3) phase is found for Er-doped ferrite (x = 0.05 and 0.10). The secondary phase formation was also reported for Er3+-, Eu3+-, and Ho3+-doped ferrites.[3,25,26] The heating of iron oxide is prone to forming a hematite phase.[27] Therefore, the formation of alpha ferrite is conceivable.

Figure 3

XRD patterns of the synthesized CoFe2–ErO4 (x = 0, 0.05, and 0.10) samples annealed at 700 °C in ambient air.

All the XRD patterns were fitted with the Rietveld refinement using the FullProf program, and the corresponding spectra are given in Figure . The Rietveld refined values of the lattice constant and crystallite size are also obtained and listed in Tables and 3. The results obtained from refinement are correlated with the values calculated from the XRD analysis as given below.

Figure 4

Rietveld refinement of XRD patterns for CoFe2–ErO4, x = 0 (a), 0.05 (b), and 0.10 (c) samples.

Table 2

Chemical Formula, Cation Distribution, Theoretical (ath), Experimental (aexpt), and Rietveld Refined (ariet) Lattice Parameters

chemical formula	A-site	B-site	rA (Å)	rB (Å)	ath (Å) (±0.006 Å)	aexpt (Å) (±0.006 Å)	ariet (Å) (±0.006 Å)
CoFe2O4 (for x = 0)	Co0.3Fe0.7	[Co0.7Fe1.3]O42–	0.651	0.645	8.275	8.353	8.362
CoFe1.95Er0.05O4 (for x = 0.05)	Co0.33Fe0.67	[Co0.67Er0.05Fe1.28]O42–	0.650	0.656	8.302	8.339	8.341
CoFe1.90Er0.10O4 (for x = 0.10)	Co0.36Fe0.64	[Co0.64Er0.1Fe1.26]O42–	0.649	0.661	8.314	8.358	8.369

Table 3

Crystallite Size (D), Rietveld Refined (Driet) Crystallite Size, Cell Volume (V), X-ray Density (ρ), Lattice Strain (ε), Dislocation Density (δ), and Packing Factor (p) of the Samples

	D (nm)
Er content, x	D–S method	W–H method	Driet	V (Å)3	ε	δ (×10–3) 1/(Å)2	ρx (gm/cc)	p
0.00	21	18	14	578.84	0.1583	13.54	5.385	108.46
0.05	24	22	17	579.89	0.1581	11.84	5.503	120.67
0.10	34	31	32	584.07	0.1574	8.28	5.590	167.27

The crystalline size, D, was estimated from XRD data using the Debye–Scherrer (D–S) formula[28]where λ is the wavelength of the radiation and β is the full width at half-maximum. The crystalline size, D, was also calculated from the Williamson–Hall (W–H) plot (Figure ) using the W–H method. The D values are listed in Table . Figure shows the increase in the crystalline size with Er content for both the D–S estimation and the W–H calculation.

Figure 5

W–H plot of CoFe2–ErO4 (x = 0.00, 0.05, and 0.10) samples’ XRD peaks for crystalline size calculation.

Figure 6

Variation of crystalline size with Er concentration.

Moreover, the value of the lattice constant from XRD data can be calculated as follows.[29]where d is the interplanar spacing of the crystal system. The variation of the lattice parameter with Er content is shown in Figure . It is seen that the lattice constant first decreases and then increases with the increase of Er content. Er3+ has a tendency to occupy in the octahedral sides due to the larger ionic radius (0.89 Å) than Fe3+ ions (0.66 Å). Subsequently, lattice distortion occurs in the grain boundary due to the diffusion of Er3+ ions.[25] The lattice constants can also be estimated theoretically from the following cationic distribution equation given aswhere R0 is the radius of the oxygen ion (1.32 Å) and rA and rB are the ionic radius for A- and B-sites’ spinel structure.[30] The values of rA and rB will depend critically on the cation distribution of the system. In order to compute rA and rB, the following cation distribution is proposed for the composition of CoFe2–ErO4: [Co2+ Fe1–3+]A [Co1–2+ Fe1+3+Erδ3+]B O42–, where A- and B-sites represent the tetrahedral and octahedral position, respectively. In the present case, CoFe2O4 is an inverse spinel structure in which half of the ferric ions preferentially occupy the tetrahedral (A-sites) and the other half occupy the octahedral sites (B-sites).[5,31] On the other hand, paramagnetic Er ions prefer to occupy the octahedral site for their larger ionic radius (0.89 Å) as compared to the ionic radius of Fe3+ (0.66 Å). Thus, the values of rA and rB can be calculated from the cation distribution of the cubic spinel system by the following equations[32]

Figure 7

Variation of experimental (aexpt) and theoretical (ath) lattice parameters.

The magnetic behavior of ferrites can be explained with the help of cation distribution.[33] The ionic radius for Co, Fe, and Er are 0.63, 0.66, and 0.89 Å, respectively. The chemical formula, cation distribution of A- and B-sites, and theoretical and experimental lattice parameters attained from XRD data are listed in Table .

Figure shows the theoretical lattice constant disagrees with the experimental lattice constant. This can be understood as follows. In theoretical calculation, cationic arrangements are regular and well distributed, but in the experimental case, defects and thermal effects along with synthesis conditions, fairly affect the lattice parameter.

Lattice strain gives information about the ordination of lattice constants, namely the lattice dislocations, which originate from crystal imperfections. To describe the variation in the strain and dislocation density, we calculated the packing factor (Table ). It is seen from Tables and 3 that the crystallite size, X-ray density, and packing factor increase with Er content but the lattice strain and dislocation density decrease with doping of Er. Similar results were reported by Kumar et al.[29]

Morphology

Figure shows the SEM images of Er-doped CoFe2O4 samples annealed at 700 °C for 3 h in ambient air. It is seen from the micrographs of all the samples that the micron-sized crystallites are dispersed and also reveal the polycrystalline nature.[24]

Figure 8

SEM images of the CoFe2–ErO4 for x = 0.00, 0.05, and 0.10 samples annealed at 700 °C.

Figure shows the TEM images, selected area electron diffraction (SAED) patterns and energy-dispersive X-ray spectroscopy (EDS) spectra of CoFe2–ErO4 (x = 0, 0.05, and 0.10). Te average particle sizes are estimated using ImageJ software and found to be 16, 24, and 29 nm, respectively, for x = 0, 0.05, and 0.10. Moreover, the particle sizes are well matched with the crystallite size measured from XRD data.

Figure 9

TEM images, SAED patterns, and EDS spectra of CoFe2–ErO4 (x = 0, 0.05, and 0.10) annealed at 700 °C for 3 h in ambient air.

The corresponding SAED patterns for all the samples are composed of (111), (220), (311), (222), (400), (422), (511), and (440) diffraction rings.[22] The ring pattern in SAED images shows the crystalline nature of the particles. The calculated values of lattice parameters from the SAED patterns by measuring d-spacing values using ImageJ software are 8.343, 8.337, and 8.351 Å for x = 0, 0.05, and 0.10, respectively, which correspond to the XRD calculation (Table ). The EDS spectra of CoFe2–ErO4 ferrite samples in Figure show the existence of Fe, Co, and O for x = 0 and the presence of Fe, Co, O, and Er for x = 0.05 and 0.10 samples. No magnetic impurity is detected in the samples, and the C and Cu peaks come from the copper microgrid. The molar ratios obtained from the EDS spectra are tabulated in Table . It is seen that there is a close proximity between nominal and experimental composition.

Table 4

Molar Values of the Elements Present in CoFe2–ErO4 (x = 0, 0.05, and 0.10) Samples

	x = 0.00		x = 0.05		x = 0.10
element	nominal	experimental	nominal	experimental	nominal	experimental
O	4.00	3.95	4.00	3.94	4.00	3.93
Fe	2.00	1.90	1.95	1.91	1.90	1.85
Co	1.00	1.13	1.00	1.10	1.00	1.07
Er	0.00	0.00	0.05	0.04	0.10	0.13

Magnetic Properties

The hysteresis loop of the Er-doped CoFe2O4 NPs measured at room temperature is shown in Figure . The saturation magnetization (Ms) increases for the increasing of Er content, and the maximum value is found to be 61 emug–1 for the 0.10 content of Er. Moreover, the magnetic coercivity (Hc) values increase with the increase of Er-substitution, and the values are 54.7, 60.2, and 76.6 kA/m (580, 730, and 1001 Oe) for 0.00, 0.05, and 0.10 compositions, respectively.

Figure 10

Ferromagnetic hysteresis loop of the CoFe2–ErO4 NPs for x = 0, 0.05, and 0.10 samples measured at room temperature using the PPMS.

The microstructure of the NPs influences their magnetic properties. More explicitly, the magnetic properties of ferrites truly depend on the particle size, cation distributions, A–B interactions, and doping elements.[5,34] The increase of saturation magnetization reported with nonmagnetic Zn doping in the CoFe2O4 matrix is due to the switching of Fe3+ ions to the octahedral B-sites from tetrahedral A-sites.[35] Besides, Abdallah et al.[36] reported that the modification of crystallite size and preference of Fe3+ ions at octahedral sites is responsible for the increase in saturation magnetization. In the present case, as the Er3+ ions have preference to hold the octahedral site because of their larger ionic radius as compared to the Fe3+; therefore, the Co2+ ions may partially transfer to the tetrahedral site by moving the same amount of Fe3+ ions from tetrahedral to octahedral sites.[3] Thus, the saturation magnetization, Ms is increased due to the increase of ionic population of Fe3+ to the octahedral sites.

Furthermore, the change of coercivity Hc and crystallite size D as a function of Er content are shown in Figure a. The increase in coercivity from 54.7 to 76.6 kA/m is observed for an increase in crystallite size from 21 to 34 nm. This increased value of Hc a result of the increased magnetocrystalline anisotropy with the enhancement of crystallite size.[37] Prathapani et al.[3] reported the enhancement of coercivity and found maximum coercivity, Hc = 65 kA/m for Er concentration, x = 0.02 and thereafter the coercivity decreases. They claimed that the orthoferrite phase pinning the domain wall causes it to suppress the coercivity. However, in the present study, even though the minute orthoferrite phase formation occurs in the doped sample, the increases in crystallite size overcome the domain wall pinning and, subsequently, the coercivity increases.

Figure 11

(a) Variation of crystallite size, coercivity, and (b) magnetic moment with Er content.

The magnetocrystalline anisotropy constant, K, was calculated by the law of approach method[38]Here, Ms, H, and M denotes the saturation magnetization, applied magnetic field, and magnetization, respectively. The variation of K for different concentrations of Er is tabulated in Table and the maximum K value was found to be 6.8 × 105 ergs/cm3 for Er concentration, x = 0.10. The magnetocrystalline anisotropy constant, K, largely depends on the saturation magnetization value.[5] Also, the anisotropy field Hk for a cubic crystal along with the easy direction [1 0 0] can be obtained using the relation[39,40]

Table 5

Magnetic Coercivity (HC), Saturation Magnetization (MS), Magnetic Moment (nB), Retentivity (Mr), Squareness Ratio (Mr/Ms), Anistropy Constant (K), and Anisotropy Field (Hk) Values

	HC
Er content, x	(kA/m)	(Oe)	MS (emug–1)	nB (μB/formula unit)	Mr (emug–1)	Mr/Ms	K × 105 (ergs/cm3)	Hk (kOe)
0.00	54.7	580	41	1.72	12.27	0.30	4.4	21.2
0.05	60.2	730	60	2.54	21.37	0.36	5.2	21.9
0.10	76.6	1001	61	2.68	23.95	0.39	6.8	22.5

The calculated Hk values are summarized in Table . It is seen that the Hk values increased for doped samples, which resulted in an increase in coercivity.[39,40]

The net magnetic moment of CoFe2O4 is attributed to the difference in magnetic moments of the cations from the octahedral site and the tetrahedral site.[19]Figure b shows the net magnetic moment of CoFe2O4 as a function of Er content. Because Er3+ has a higher magnetic moment than Fe3+,[3] thus the magnetic moment increases with increasing Er content. The squareness ratio (Mr/Ms) gives information about the reorientation of magnetization of the nearest easy axis in the absence of a magnetic field.[41] The values of saturation magnetization, retentivity, squareness ratio, and magnetic anisotropy constant of CoFe2–ErO4 are tabulated in Table . The calculated squareness ratio varies from 0.30 to 0.35, which reveals the anisotropic nature of CoFe2–ErO4 and also indicates that the CoFe2–ErO4 ferrites with the increase of Er concentration are more suitable for magnetic memory device applications. The fluctuation of the squareness ratio depends on the crystallite size, domain structure, and the anisotropy of the materials. According to previous investigation,[6] particles show a single-magnetic domain nature for the squareness ratio less than 0.5. On the other hand, the particles become multimagnetic domain in nature. The values of the squareness ratio in the present study are below 0.5. Hence, the particles manifest single-domain behavior.

The field cooled-zero field cooled (FC-ZFC) curves at 100 Oe for CoFe2–ErO4 (x = 0, 0.05, and 0.10) samples are shown in Figure . The blocking temperature, T > 350 K for all the samples, is much higher than room temperature (300 K). The bifurcation of FC and ZFC magnetization increases with decreasing temperature due to the large anisotropy contribution of CoFe2–ErO4 (x = 0, 0.05, and 0.10) powder samples.[42,43]

Figure 12

FC-ZFC curves for CoFe2–ErO4 (x = 0, 0.05, and 0.10) samples in a measuring field of 100 Oe.

Conclusions

The structural, morphological, and magnetic properties of the sol–gel-synthesized nanocrystalline CoFe2–ErO4 (x = 0, 0.05, and 0.10) ferrites were studied. The XRD analysis confirms the crystalline phase of the cubic spinel structure. The room temperature magnetic measurements show the soft ferromagnetic behavior of the samples. The noticeable change in magnetic properties is influenced by crystallite size and microstructure. The tuning of saturation magnetization, coercivity, squareness ratio, and anisotropy constant is observed due to the increase in crystallite size and the migration of Fe3+ ions to the octahedral sides. The FC-ZFC measurements show the blocking temperature is well above 350 K. The obtained NPs may offer potential applications in areas such as magnetic storage devices, magnetic heads and shields, hyperthermia-based therapy, biosensors, and so on.