Layer-by-Layer Self-Assembled Ferrite Multilayer Nanofilms for Microwave Absorption

Heo, Jiwoong; Choi, Daheui; Hong, Jinkee

doi:https://doi.org/10.1155/2015/164619

Journal of Nanomaterials

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Abstract Introduction Methods Results and Discussion Conclusion Acknowledgments References Copyright Related Articles

Research Article | Open Access

Volume 2015 | Article ID 164619 | https://doi.org/10.1155/2015/164619

Layer-by-Layer Self-Assembled Ferrite Multilayer Nanofilms for Microwave Absorption

Jiwoong Heo,¹Daheui Choi,¹and Jinkee Hong¹

Academic Editor: Miguel A. Correa-Duarte

Received30 Aug 2015

Revised05 Oct 2015

Accepted15 Oct 2015

Published17 Nov 2015

Abstract

We demonstrate a simple method for fabricating multilayer thin films containing ferrite (Co_0.5Zn_0.5Fe₂O₄) nanoparticles, using layer-by-layer (LbL) self-assembly. These films have microwave absorbing properties for possible radar absorbing and stealth applications. To demonstrate incorporation of inorganic ferrite nanoparticles into an electrostatic-interaction-based LbL self-assembly, we fabricated two types of films: (1) a blended three-component LbL film consisting of a sequential poly(acrylic acid)/oleic acid-ferrite blend layer and a poly(allylamine hydrochloride) layer and (2) a tetralayer LbL film consisting of sequential poly(diallyldimethylammonium chloride), poly(sodium-4-sulfonate), bPEI-ferrite, and poly(sodium-4-sulfonate) layers. We compared surface morphologies, thicknesses, and packing density of the two types of ferrite multilayer film. Ferrite nanoparticles (Co_0.5Zn_0.5Fe₂O₄) were prepared via a coprecipitation method from an aqueous precursor solution. The structure and composition of the ferrite nanoparticles were characterized by X-ray diffraction, energy dispersive X-ray spectroscopy, transmission electron microscopy, and scanning electron microscopy. X-ray diffraction patterns of ferrite nanoparticles indicated a cubic spinel structure, and energy dispersive X-ray spectroscopy revealed their composition. Thickness growth and surface morphology were measured using a profilometer, atomic force microscope, and scanning electron microscope.

1. Introduction

Microwave absorbing materials, commonly known as radar absorbing materials, are in high demand for microwave absorption coatings on the surface of military stealth aircraft to avoid detection by enemy radar. A number of microwave absorbing materials have been explored for this application: conducting fibers [1, 2], ferromagnetic composites [3], carbon nanotubes [4], and ferrites [5–8] are frequently used. In particular, the unique microwave absorbing properties of ferrite nanoparticles, resulting from both magnetic and dielectric losses, have been explored by many groups [9–15]. Particularly, ferrite nanoparticles are widely used in the microwave absorbing technology. By controlling composition of ferrite, the performance of microwave absorbing can be tuned. Spinel ferrite has large resistivity and large magnetic loss; therefore, it has been used for microwave absorbing materials. Application of spinel ferrite is limited in 1–3 MHz region because of its low resonance frequency; however, by doping with metallic ions such as Co, Zn, and Mg the absorbing range can be controlled which leads to unlimited possibility of spinel ferrite. For examples, Zhao group doped cobalt and cupper ions with Ni-Zn spinel ferrite to tune the microwave absorbing properties. The microwave absorbing region, in which reflection loss values are lesser than −10 bB, of NiCoZnFe₂O₄ is achieved at 3.9–11.5 GHz. The control of microwave absorption of metallic ion doped Ni-Zn ferrites mainly results from magnetic loss change derive from metallic ions [16].

At present, however, 3-dimensional arrangements of microwave absorbing materials are not well developed. Microwave absorbing materials are usually prepared as a suspension of colloidal nanoparticles in a solvent, in which electrostatic or steric repulsive forces prevent aggregation of nanoparticles [17], and conventional 3-dimensional arrays of magnetic nanoparticles are fabricated as pressed or mixed pellets [18–20]. However, these methods are costly and require an excessive volume of material, as the ferrite nanoparticles are not densely packed in the pellets. Therefore, a more effective method such as film deposition is needed for industrial applications.

Layer-by-layer (LbL) self-assembly consists of sequential adsorption of oppositely charged polymers to build up a multilayer thin film at the molecular level [21–24]. It allows the fabrication of multilayered thin films having desired thickness, composition, and density [25, 26]. Moreover, various materials ranging from polyelectrolytes to nanoparticles [27], DNA [28], block copolymer micelles [29], and any kind of ferrite nanoparticles, such as cobalt ferrites [30], zin ferrites [31], and other mixed ferrites [32], can be incorporated into a LbL-deposited multilayer thin film through complementary interactions (e.g., electrostatic interactions, covalent bonding, hydrogen bonding, and hydrophobic interactions) [33–35].

There are previous studies about film deposition method that incorporates ferrite nanoparticles into multilayered film by LbL self-assembly [36–38].

In this study, we report a facile and simple method of preparing microwave absorbing nanofilm containing densely packed and well-organized ferrite nanoparticles. Since ferrite nanoparticles are inorganic, as-synthesized oleic-acid- (OA-) stabilized nanoparticles do not disperse in water and are unsuitable for electrostatic interaction-based LbL self-assembly. Therefore, additional ligand exchange treatment is needed to incorporate ferrite nanoparticles in an LbL-assembled film. During this study, we examined two different types of films and compared their surface morphologies, thicknesses, and the packing density of incorporated ferrite nanoparticles. The blended three-component LbL film consists of a weak-polyelectrolyte/ferrite-nanoparticle-blended layer and an oppositely charged weak polyelectrolyte layer. Poly(allylamine hydrochloride) (PAH) and poly(acrylic acid) (PAA) are typically used weak polyelectrolytes for electrostatic interaction-based LbL self-assembly and are used as building blocks for fabricating blended three-component LbL films. Tetralayer LbL films consist of two kinds of strong polyelectrolytes and ferrite nanoparticles. Poly(diallyldimethylammonium chloride) (PDADMAC) and poly(sodium 4-styrenesulfonate) (PSS) are used as strong polyelectrolytes for tetralayer LbL films. The main difference between a blended three-component LbL film and a tetralayer LbL film is that the blended three-component LbL film can be built using as-synthesized oleic-acid- (OA-) stabilized ferrite nanoparticles without functionalization of the nanoparticles, whereas the tetralayer film needs ligand exchange of the ferrite nanoparticles. The effect of ligand-exchanged nanoparticles and the composition of two types of LbL self-assembled films are examined in this study.

2. Material and Methods

2.1. Materials

Iron(III) chloride hexahydrate, zinc sulfate heptahydrate, cobalt(II) chloride hexahydrate, oleic acid (OA), and sodium hydroxide powder were purchased from DaeJung. Trioctylphosphine oxide (TOPO), poly(diallyldimethylammonium chloride) solution (PDADMAC, Mw 200,000–350,000, 20 wt. % in H₂O), poly(sodium 4-styrenesulfonate) (PSS, Mw 70,000), and branched polyethylenimine (bPEI, Mw 25,000) were obtained from Sigma Aldrich.

2.2. Synthesis of Ferrite Nanoparticles

2.2.1. Oleic-Acid- (OA-) Stabilized Ferrite Nanoparticles

Cobalt-doped zinc ferrite (Co_0.5Zn_0.5Fe₂O₄) nanoparticles were prepared following the procedure reported by López et al. [39]. Briefly, FeCl₃·6H₂O (15 mL; 0.4 M), CoCl₂·6H₂O (15 mL; 0.1 M), and ZnSO₄·7H₂O (15 mL; 0.1 M) solutions were mixed as the precursor solution. NaOH (15 mL; 3 M) was added as the coprecipitation agent to the precursor solution, dropwise with vigorous stirring. Precipitation occurred immediately, changing the solution’s color to brown. The precipitated solution was stirred at 80°C for 1 h for reaction. After reaction the pH of the solution changed from 12 to 10.5 by washing with DI water. To prevent aggregation of ferrite nanoparticles, 5 mL of OA was added to the solution as a coating agent and surfactant and then stirred for 2 h at 80°C. The precipitate was washed twice with DI water and then washed with ethanol and acetone to remove unnecessary compounds. The supernatant was separated by centrifugation for 15 min at 4000 rpm, and the precipitate dried overnight in an 80°C oven.

2.2.2. bPEI Ligand-Exchanged Ferrite Nanoparticles

Trioctylphosphine oxide (TOPO) was added as cosurfactant when the oleic acid was introduced to the ferrite solution (TOPO: 1 g, 2.5 mmol; OA: 1 mL, 3.2 mmol). The remainder of the process was as above for the OA-stabilized ferrite nanoparticles. Well-dried OA + TOPO stabilized ferrite nanoparticles were dispersed into chloroform in a bath sonicator to obtain the ferrite solution (5 mg/mL). Ferrite solution (2 mL; 5 mg/mL) was mixed with branched polyethylenimine (MW 25,000) in 100 mL of DMSO. After 48 h at room temperature for reaction, the bPEI-ferrite nanoparticles were collected by centrifugation for 1 h at 8000 rpm and redispersed into 10 mL of DI water.

2.3. Layer-by-Layer Assembly

2.3.1. Blended Three-Component LbL Film

LbL multilayer films were fabricated by hand-dipping. The silicon wafer was exposed to O₂ plasma to produce a negatively charged surface. The negatively charged wafer was dipped into cationic PAH solution (pH 7.5) for 15 s and then washed by dipping two times in DI water for 15 s to remove weakly attached polyelectrolytes. The PAA/ferrite blended layer, which follows in the sequence, was deposited on the PAH coated wafer surface by dipping the substrate into the blended solution of PAA and ferrite (pH 3.5). Washing was repeated as in the previous step. The pH of the solution was adjusted using NaOH (0.2 M).

2.3.2. Tetralayer LbL Film

Following O₂ plasma exposure, the negatively charged wafer was dipped into cationic PDADMAC solution for 10 min and washed three times by dipping in DI water for 2 min, 1 min, and 1 min to remove weakly attached PDADMAC. The PSS, bPEI-ferrite, and PSS layers were then deposited in sequence on the PDADMAC layer, using the same adsorption process. The PDADMAC and PSS solutions contained NaCl (0.3 M).

The processes for fabricating the two types of films are illustrated in Scheme 1.

2.4. Characterization of Ferrite Nanoparticles and Multilayer Films

Energy-filtering transmission electron microscopy (EF-TEM) images of ferrite nanoparticles were obtained using a LIBRA 120 microscope (Carl Zeiss). Energy-dispersive X-ray spectroscopy (EDX), in conjunction with field-emission scanning electron microscopy (FE-SEM), was used for analysis of the dried ferrite nanoparticle powders. Atomic force microscopy (AFM) images were obtained with NX-10 (Park Systems) in noncontact mode. The thickness of multilayer thin films on wafers was measured by Profilometer (Dektak 150, Veeco).

3. Results and Discussion

LbL self-assembly provides opportunities to control film thickness, composition, and morphology. Although intermolecular interactions such as hydrogen bonding, covalent bonding, and charge transfer can be adopted for LbL self-assembly, electrostatic interactions are most commonly used. During electrostatic interaction-based LbL assembly, the structure and morphology of fabricated multilayer thin film can be affected by parameters such as pH, adsorption time, and concentration of solute and salt. The charge density of weak polyelectrolytes is tunable through its sensitivity to the solution’s pH. In comparison, the ionic strength of strong polyelectrolytes can be controlled through NaCl concentration. NaCl screens the repulsive interaction of strong polyelectrolytes, leading to an increased film thickness [40].

As-synthesized oleic-acid-stabilized ferrite nanoparticles do not disperse in water and require additional processes such as blending with charged polyelectrolytes or ligand exchange if they are to be used as building blocks for LbL-deposited films. Figure 1(a) presents a TEM image showing the size and morphology of OA-stabilized Co_0.5Zn_0.5Fe₂O₄ ferrite nanoparticles, while Figure 1(b) shows ligand-exchanged bPEI-ferrite nanoparticles.

(a)

(b)

(c)

The average size of synthesized OA-stabilized ferrite nanoparticles was about 18.5 nm; in comparison, the ligand-exchanged bPEI-ferrite nanoparticles average size was about 7 nm. The size reduction of ferrite nanoparticles originated in the added TOPO, which was introduced as a cosurfactant and coating agent to increase stability and to provide sufficient binding sites for bPEI ligands. This ligand exchange enabled water dispersion of inorganic nanoparticles: the amine group of the bPEI ligand protonated in the water solvent and had a positive zeta potential value of +34.3 mV. The inset images of Figure 1 show ferrite nanoparticles in water: OA-stabilized ferrite nanoparticles did not disperse in water (Figure 1(a), left), while ligand-exchanged bPEI-ferrite nanoparticles were well dispersed (Figure 1(b), right). When magnetic nanoparticles are incorporated into film, a decreased magnetic dipole interaction between magnetic nanoparticles is important in creating a well-organized nanostructure.

X-ray diffraction patterns of the powdered OA-stabilized ferrite nanoparticles confirmed a cubic spinel structure of Co_0.5Zn_0.5Fe₂O₄ (Figure 1(c)). Peaks indexed (220), (311), (400), (422), (511), and (440) were observed; a strong (311) plane reflection indicates the ferrite cubic spinel structure. The synthesized ferrite nanoparticles were observed to have good crystallinity and high quality, as there were no peaks observed from other phases. Microwave energy can be absorbed and transformed into heat energy by dielectric and magnetic losses when the absorber’s characteristic impedance is matched to the characteristic impedance of free space [41]. Over the gigahertz (GHz) range, dielectric losses are negligible () and only magnetic loss affects microwave absorption. Spinel ferrites are familiar electromagnetic wave absorbers because of their resistivity and magnetic losses; however, at gigahertz frequencies, their permeability decreases according to Snoek’s limit [42]. To increase microwave absorption properties, metal ions such as cobalt and zinc can be doped into spinel-type ferrites. Doped metallic ions change the permeability of ferrite nanoparticles which result in enhancement of microwave absorption properties by magnetic losses. The composition of synthesized ferrite nanoparticles was determined by EDX-SEM analysis (Figure 2 and Table 1), showing a molar ratio of about 0.5 : 0.5 : 2 : 4 [Co/Zn/Fe/O].

Because the value of PAA is 4.5, the degree of ionization of PAA (pH 3.5) is about 30–40%, which offers sufficient binding sites for blended ferrite nanoparticles and sequential PAH (pH 7.5) layers [43]. Figure 3 shows the thickness growth curves of the two different types of LbL assembled film. The notation of LbL film listed as (PDADMAC/PSS/bPEI-ferrite/PSS)_0.5n represents multilayer film consisting of PDADMAC, PSS, bPEI ligand-exchanged ferrite, and PSS where means the number of layers. For examples, the notation of (PDADMAC/PSS/bPEI-ferrite/PSS)₁₀ where is 20 represents 10-tetralayer multilayer film consisting of repeated PDADMAC/PSS/bPEI-ferrite and PSS. Thickness of the blended three-component LbL film (red line) increased linearly with the number of bilayers, indicating that the PAA + ferrite nanoparticle layer and the PAH layer successfully developed an LbL film. Thickness of the tetralayer LbL film also increased with the number of the bilayers, once five tetralayers had been deposited (black line). The top-view FE-SEM image shows the surface of the three-component LbL film consisting of (PAH/PAA + ferrite)₁₀ (Figure 4(a)) and the tetralayer LbL film (PDADMAC/PSS/bPEI-ferrite/PSS)₁₀ (Figure 4(b)). The aggregation of ferrite nanoparticles in both films results from the nature of magnetic nanoparticles. Since ligand exchange of OA-stabilized ferrite nanoparticles with bPEI reduces the aggregation, the surface of the tetralayer LbL film shows much more densely packed ferrite nanoparticles than the blended three-component film. The key parameter for the phase distribution of ferrite nanoparticle is balance between attraction force of magnetic nanoparticles and repulsion force of positively charged bPEI ligand of ferrite particles [44]. Figures 5(a), 5(b), and 5(c) show top-view FE-SEM images of tetralayer LbL films. As the number of tetralayers increased, the surface density of ferrite nanoparticles gradually increased. The cross-sectional SEM image shows a homogeneously fabricated ferrite multilayer film that corresponds well to the thickness measured using a profilometer (Figure 3). The AFM height image (Figure 6) displays the surface morphology of tetralayer LbL film; ferrite nanoparticles did not fully cover the surface of the Si wafer until 10 tetralayers had been deposited. The root-mean-square () surface roughness was 66.726 nm for 10 tetralayers and 67.052 nm for 15 tetralayers. These rough surfaces resulted from aggregation of ferrite nanoparticles caused by strong polyelectrolytes. Since the size of ligand-exchanged bPEI-ferrite nanoparticles was about 7 nm as measured from the TEM image (Figure 1(b)), the spherical structures appearing in Figure 6(c) indicate aggregates of tens of bPEI-ferrite nanoparticles. Even though the positively charged bPEI ligand counteracted the magnetic attraction between nanoparticles, an aggregated ferrite structure was observed.

(a)

(b)

(a)

(b)

(c)

(d)

(a)

(b)

(c)

(d)

4. Conclusion

In this study, we focused on incorporating ferrite nanoparticles into a multilayer nanofilm. The inorganic ferrite nanoparticles were oleic-acid- (OA-) stabilized or ligand-exchanged using bPEI; the OA-stabilized nanoparticles had a diameter of about 18.5 nm, compared to 7 nm after ligand exchange. We successfully fabricated two types of nanofilms: (1) a blended three-component LbL film consisting of PAA/ferrite and PAH and (2) a tetralayer LbL film consisting of PDADMAC/PSS/bPEI-ferrite/PSS. In both methods, ferrite nanoparticles were deposited onto a Si wafer using an electrostatic-interaction-based LbL self-assembly method. Surface morphologies, thicknesses, and packing densities of the two types of film were investigated. Even though blended three-component LbL film is much simpler and faster than the tetralayer LbLfilm, the tetralayer LbL films had a better organized nanostructure of ferrite nanoparticles, in comparison to blended three-component LbL films. In conclusion, by employing LbL self-assembly, we can fabricate densely packed and well-organized multilayer ferrite films using either weak or strong polyelectrolytes. We believe that further research on this film deposition method for microwave absorbing ferrite nanoparticles will accelerate their industrial and military application in, for example, electronic devices, stealth aircraft, and other military technologies.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

Acknowledgments

This research was supported by the Bio & Medical Technology Development Program of the National Research Foundation of Korea (NRF), funded by the Korean government (no. 2012M3A9C6050104). Also, this work was supported by the National Research Foundation of Korea (NRF) grant funded by the Korea government Ministry of Science, ICT & Future Planning (no. 2013R1A1A1076126). Additionally, this work was carried out with the support of “Cooperative Research Program for Agriculture Science & Technology Development (Project no. PJ009986012015)” (Rural Development Administration, Republic of Korea), as well as the Korea Health Technology R&D Project through the Korea Health Industry Development Institute (KHIDI), funded by the Ministry of Health & Welfare (HI14C-3266-030014).

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Copyright © 2015 Jiwoong Heo et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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