Monodisperse MFe2O4 (M ) Fe, Co, Mn) Nanoparticles
Shouheng Sun,*,† Hao Zeng,† David B. Robinson,† Simone Raoux,‡ Philip M. Rice,‡
Shan X. Wang,§ and Guanxiong Li§
Contribution from the IBM T. J. Watson Research Center, Yorktown Heights, New York 10598,
IBM Almaden Research Center, 650 Harry Road, San Jose, California 95120, and Department
of Materials Science and Engineering, Stanford UniVersity, Stanford, California 94305
Received August 22, 2003; E-mail: ssun@us.ibm.com
Abstract: High-temperature solution phase reaction of iron(III) acetylacetonate, Fe(acac)3, with 1,2-
hexadecanediol in the presence of oleic acid and oleylamine leads to monodisperse magnetite (Fe3O4)
nanoparticles. Similarly, reaction of Fe(acac)3 and Co(acac)2 or Mn(acac)2 with the same diol results in
monodisperse CoFe2O4 or MnFe2O4 nanoparticles. Particle diameter can be tuned from 3 to 20 nm by
varying reaction conditions or by seed-mediated growth. The as-synthesized iron oxide nanoparticles have
a cubic spinel structure as characterized by HRTEM, SAED, and XRD. Further, Fe3O4 can be oxidized to
Fe2O3, as evidenced by XRD, NEXAFS spectroscopy, and SQUID magnetometry. The hydrophobic
nanoparticles can be transformed into hydrophilic ones by adding bipolar surfactants, and aqueous
nanoparticle dispersion is readily made. These iron oxide nanoparticles and their dispersions in various
media have great potential in magnetic nanodevice and biomagnetic applications.
Introduction
Magnetic iron oxide nanoparticles and their dispersions in
various media have long been of scientific and technological
interest. The cubic spinel structured MFe2O4, or MOâFe2O3,
represents a well-known and important class of iron oxide
materials where oxygen forms an fcc close packing, and M2+
and Fe3+ occupy either tetrahedral or octahedral interstitial sites.1
By adjusting the chemical identity of M2+, the magnetic
configurations of MFe2O4 can be molecularly engineered to
provide a wide range of magnetic properties. Due in part to
this versatility, nanometer-scale MFe2O4 materials have been
among the most frequently chosen systems for studies of
nanomagnetism and have shown great potential for many
important technological applications, ranging from information
storage and electronic devices to medical diagnostics and drug
delivery. Dispersions of magnetic MFe2O4 nanoparticles, es-
pecially magnetite (Fe3O4) nanoparticles, have been used widely
not only as ferrofluids in sealing, oscillation damping, and
position sensing2 but also as promising candidates for biomol-
ecule tagging, imaging, sensing, and separation.3 Depending on
the chemical identity of M2+, the densely packed solid state
form of nanocrystalline MFe2O4-based materials, on the other
hand, can have either high magnetic permeability and electrical
resistivity (for M representing one or the mixed components
from Co, Li, Ni, Zn, etc.) or half-metallicity (for M ) Fe), and
may be a potential candidate for future high-performance
electromagnetic4 and spintronic devices.5
To use MFe2O4 nanoparticles for future highly sensitive
magnetic nanodevice and biomedical applications, a practical
route to monodisperse MFe2O4 nanoparticles with diameters
smaller than 20 nm and a tight size distribution (less than 10%
standard deviation) is needed. A commonly used solution phase
procedure for making such particles has been the coprecipitation
of M2+ and Fe3+ ions by a base, usually NaOH or NH3âH2O in
an aqueous solution6 or in a reverse micelle template.7 Although
this precipitation method is suitable for mass production of
† IBM T. J. Watson Research Center.
‡ IBM Almaden Research Center.
§ Stanford University.
(1) (a) West, A. R. Basic Solid State Chemistry; John Wiley & Sons: New
York, 1988; pp 356-359. (b) O’Handley, R. C. Modern Magnetic
Materials-Principles and Applications; John Wiley & Sons: New York,
2000; pp 126-132.
(2) Raj, K.; Moskowitz, R. J. Magn. Magn. Mater. 1990, 85, 233.
(3) (a) Ha¨feli, U.; Schu¨tt, W.; Teller, J.; Zborowski, M. Scientific and Clinical
Applications of Magnetic Carriers; Plenum Press: New York, 1997. (b)
Oswald, P.; Clement, O.; Chambon, C.; Schouman-Claeys, E.; Frija, G.
Magn. Reson. Imaging 1997, 15, 1025. (c) Hergt, R.; Andra, W.; d’Ambly,
C. G.; Hilger, I.; Kaiser, W. A.; Richter, U.; Schmidt, H.-G. IEEE Trans.
Mag. 1998, 34, 3745. (d) Jordan, A.; Scholz, R.; Wust, P.; Fa¨hling, H.;
Felix, R. J. Magn. Magn. Mater. 1999, 201, 413. (e) Kim, D. K.; Zhang,
Y.; Kehr, J.; Klason, T.; Bjelke, B.; Muhammed. M. J. Magn. Magn. Mater.
2001, 225, 256. (f) Pankhurst, Q. A.; Connolly, J.; Dobson, J. J. Phys. D:
Appl. Phys. 2003, 36, R167. (g) Tartaj, P.; Morales, M. P.; Veintemillas-
Verdaguer, S.; Gonza´lez-Carren˜o, T.; Serna, C. J. J. Phys. D: Appl. Phys.
2003, 36, R182. (h) Berry, C. C.; Curtis, A. S. G. J. Phys. D: Appl. Phys.
2003, 36, R198.
(4) (a) Fannin, P. C.; Charles, S. W.; Vincent, D.; Giannitsis, A. T. J. Magn.
Magn. Mater. 2002, 252, 80. (b) Matsushita, N.; Nakamura, T.; Abe, M.
IEEE Trans. Magn. 2002, 38, 3111. (c) Matsuchita, Chong, C. P.; Mizutani,
T.; Abe, M. J. Appl. Phys. 2002, 91, 7376. (d) Nakamura, T.; Miyamoto,
T.; Yamada, Y. J. Magn. Magn. Mater. 2003, 256, 340.
(5) (a) Verwey, E. J. W. Nature 1939, 144, 327. (b) Zhang, Z.; Satpathy, S.
Phys. ReV. B 1991, 44, 13319. (c) Anisimov, V. I.; Elfimov, I. S.; Hamada,
N.; Terakura, K. Phys. ReV. B 1996, 54, 4387. (d) Gong, G. Q.; Gupta, A.;
Xiao, G.; Qian, W.; Dravid, D. P. Phys. ReV. B 1997, 56, 5096. (e) Coey,
J. M. D.; Berkowitz, A. E.; Balcells, L. I.; Putris, F. F.; Parker, F. T. Appl.
Phys. Lett. 1998, 72, 734. (f) Li, X. W.; Gupta, A.; Xiao, G.; Gong, G. Q.
J. Appl. Phys. 1998, 83, 7049. (g) Kiyomura, T.; Maruo, Y.; Gomi M. J.
Appl. Phys. 2000, 88, 4768. (h) Moore, R. G. C.; Evans, S. D.; Shen, T.;
Hodson, C. E. C. Physica E 2001, 9, 253. (i) Versluijs, J. J.; Bari, M. A.;
Coey, J. M. D. Phys. ReV. Lett. 2001, 87, 26601. (j) Soeya, S.; Hayakawa,
J.; Takahashi, H.; Ito, K.; Yamamoto, C.; Kida, A.; Asano, H.; Matsui, M.
Appl. Phys. Lett. 2002, 80, 823. (k) Sorenson, T. A.; Morton, S. A.; Dan
Waddill, G.; Switzer, J. A. J. Am. Chem. Soc. 2002, 124, 7604.
Published on Web 12/10/2003
10.1021/ja0380852 CCC: $27.50 © 2004 American Chemical Society J. AM. CHEM. SOC. 2004, 126, 273-279 9 273
magnetic MFe2O4 ferrofluids, it does require careful adjustment
of the pH value of the solution for particle formation and
stabilization, and it is difficult to control sizes and size
distributions, particularly for particles smaller than 20 nm. An
alternative approach to monodisperse iron oxide nanoparticles
is via high-temperature organic phase decomposition of an iron
precursor, for example, decomposition of FeCup3 (Cup: N-
nitrosophenylhydroxylamine, C6H5N(NO)O-)8 or decomposition
of Fe(CO)5 followed by oxidation to Fe2O3.9 The latter process
has recently been extended to the synthesis of monodisperse
cobalt ferrite (CoFe2O4) nanoparticles.10 Although significant
progress in making monodisperse Fe2O3 and CoFe2O4 nano-
particles has been made in organic phase reactions, there is still
no general process for producing MFe2O4, especially Fe3O4
nanoparticles with the desired size and acceptable size distribu-
tion.
Recently, we reported a convenient organic phase process
for making monodisperse Fe3O4 nanoparticles through the
reaction of Fe(acac)3 and a long-chain alcohol.11 Our further
experiments indicated that this reaction could be readily
extended to the synthesis of MFe2O4 nanoparticles (with M )
Co, Ni, Mn, Mg, etc.) by simply adding a different metal
acetylacetonate precursor to the mixture of Fe(acac)3 and 1,2-
hexadecanediol. Here we present detailed syntheses and char-
acterization of Fe3O4 and related MFe2O4 nanoparticles (with
M ) Co and Mn as two examples) with sizes tunable from 3 to
20 nm in diameter. The process involves high-temperature (up
to 305 °C) reaction of metal acetylacetonate with 1,2-hexade-
canediol, oleic acid, and oleylamine. The size of the oxide
nanoparticles can be controlled by varying the reaction tem-
perature or changing metal precursors. Alternatively, with the
smaller nanoparticles as seeds, larger monodisperse nanopar-
ticles up to 20 nm in diameter can be synthesized by seed-
mediated growth. The process does not require a low-yield
fractionation procedure to achieve the desired size distribution
and is readily scaled up for mass production. The nanoparticles
can be dispersed into nonpolar or weakly polar hydrocarbon
solvent, such as hexane or toluene. The hydrophobic nanopar-
ticles can be transformed into hydrophilic ones by mixing with
a bipolar surfactant, tetramethylammonium 11-aminounde-
canoate, allowing preparation of aqueous nanoparticle disper-
sions. These iron oxide nanoparticles and their dispersions in
various media have great potential in magnetic nanodevice and
biomagnetic applications.
Experimental Section
The synthesis was carried out using standard airless procedures and
commercially available reagents. Absolute ethanol, hexane, and dichlo-
romethane (99%) were used as received. Phenyl ether (99%), benzyl
ether (99%), 1,2-hexadecanediol (97%), oleic acid (90%), oleylamine
(>70%), cobalt(II) acetylacetonate, Mn(II) acetylacetonate, and poly-
ethylenimine (water-free, average Mw ca. 25 000) were purchased from
Aldrich Chemical Co. Iron(III) acetylacetonate was from Strem
Chemicals, Inc. Tetramethylammonium 11-aminoundecanoate was
prepared by titrating a methanolic suspension of 11-aminoundecanoic
acid with methanolic tetramethylammonium hydroxide (both from
Aldrich), evaporating the solvent under reduced pressure, and recrystal-
lizing in tetrahydrofuran.
Synthesis of 4 nm Fe3O4 Nanoparticle Seeds. Fe(acac)3 (2 mmol),
1,2-hexadecanediol (10 mmol), oleic acid (6 mmol), oleylamine (6
mmol), and phenyl ether (20 mL) were mixed and magnetically stirred
under a flow of nitrogen. The mixture was heated to 200 °C for 30
min and then, under a blanket of nitrogen, heated to reflux (265 °C)
for another 30 min. The black-brown mixture was cooled to room
temperature by removing the heat source. Under ambient conditions,
ethanol (40 mL) was added to the mixture, and a black material was
precipitated and separated via centrifugation. The black product was
dissolved in hexane in the presence of oleic acid (�0.05 mL) and
oleylamine (�0.05 mL). Centrifugation (6000 rpm, 10 min) was applied
to remove any undispersed residue. The product, 4 nm Fe3O4 nano-
particles, was then precipitated with ethanol, centrifuged (6000 rpm,
10 min) to remove the solvent, and redispersed into hexane.
Under identical conditions, reaction of Co(acac)2 (1 mmol) with Fe-
(acac)3 led to 3 nm CoFe2O4 nanoparticles that could be readily
dispersed into hexane, giving a dark red-brown hexane dispersion.
Synthesis of 6 nm Fe3O4 Nanoparticle Seeds. Fe(acac)3 (2 mmol),
1,2-hexadecanediol (10 mmol), oleic acid (6 mmol), oleylamine (6
mmol), and benzyl ether (20 mL) were mixed and magnetically stirred
under a flow of nitrogen. The mixture was heated to 200 °C for 2 h
and then, under a blanket of nitrogen, heated to reflux (�300 °C) for
1 h. The black-colored mixture was cooled to room temperature by
removing the heat source. Following the workup procedures described
in the synthesis of 4 nm particles, a black-brown hexane dispersion of
6 nm Fe3O4 nanoparticles was produced.
Similarly, by adding Co(acac)2 or Mn(acac)2, 10 nm CoFe2O4 or 7
nm MnFe2O4 nanoparticle seeds can be made.
Synthesis of 8 nm Fe3O4 Nanoparticles via 6 nm Fe3O4 Seeds.
Fe(acac)3 (2 mmol), 1,2-hexadecanediol (10 mmol), benzyl ether (20
mL), oleic acid (2 mmol), and oleylamine (2 mmol) were mixed and
magnetically stirred under a flow of N2. A 84 mg sample of 6 nm
Fe3O4 nanoparticles dispersed in hexane (4 mL) was added. The mixture
was first heated to 100 °C for 30 min to remove hexane, then to 200
°C for 1 h. Under a blanket of nitrogen, the mixture was further heated
to reflux (�300 °C) for 30 min. The black-colored mixture was cooled
to room temperature by removing the heat source. Following the workup
procedures described in the synthesis of 4 nm particles, a black-brown
hexane dispersion of 8 nm Fe3O4 nanoparticles was produced.
Similarly, 80 mg of 8 nm Fe3O4 seeds reacted with Fe(acac)3 (2
mmol) and the diol (10 mmol) led to 10 nm Fe3O4 nanoparticles. Using
this seed-mediated growth, bigger nanoparticles of Fe3O4 up to 20 nm,
CoFe2O4 up to 20 nm, or MnFe2O4 up to 18 nm have been made.
Synthesis of Hydrophilic Fe3O4 Nanoparticles. Under ambient
conditions, a hexane dispersion of hydrophobic Fe3O4 nanoparticles
(about 20 mg in 0.2 mL) was added to a suspension of tetramethy-
lammonium 11-aminoundecanoate (about 20 mg in 2 mL) in dichlo-
romethane. The mixture was shaken for about 20 min, during which
time the particles precipitated and separated using a magnet. The solvent
and nonmagnetic suspension were decanted, and the precipitate was
washed once with dichloromethane and separated again using a magnet
(6) See for example: (a) Kang, Y. S.; Risbud, S.; Rabolt, J. F.; Stroeve, P.
Chem. Mater. 1996, 8, 2209. (b) Hong, C.-Y.; Jang, I. J.; Horng, H. E.;
Hsu, C. J.; Yao, Y. D.; Yang, H. C. J. Appl. Phys. 1997, 81, 4275. (c)
Fried, T.; Shemer, G.; Markovich, G. AdV. Mater. 2001, 13, 1158. (d) Tang,
Z. X.; Sorensen, C. M.; Klabunde, K. J.; Hadjipanayis, G. C. J. Colloid
Interface Sci. 1991, 146, 38. (e) Zhang, Z. J.; Wang, Z. L.; Chakoumakos,
B. C.; Yin, J. S. J. Am. Chem. Soc. 1998, 120, 1800. (f) Neveu, S.; Bec,
A.; Robineau, M.; Talbol, D. J. Colloid Interface Sci. 2002, 255, 293.
(7) See for example: (a) Pileni, M. P.; Moumen, N. J. Phys. Chem. B 1996,
100, 1867. (b) Liu, C.; Zou, B.; Rondinone, A. J.; Zhang, Z. J. J. Phys.
Chem. B 2000, 104, 1141.
(8) Rockenberger, J.; Scher, E. C.; Alivisatos, P. A. J. Am. Chem. Soc. 1999,
121, 11595.
(9) (a) Bentzon, M. D.; van Wonterghem, J.; Mørup, S.; Tho¨le´n, A.; Koch, C.
J. Philos. Mag. B 1989, 60, 169. (b) Hyeon, T.; Lee, S. S.; Park, J.; Chung,
Y.; Na, H. B. J. Am. Chem. Soc. 2001, 123, 12798. (c) Guo, Q.; Teng, X.;
Rahman, S.; Yang, H. J. Am. Chem. Soc. 2003, 125, 630. (d) Redl, F. X.;
Cho, K.-S.; Murray, C. B.; O’Brien, S. Nature 2003, 423, 968.
(10) Hyeon, T.; Chung, Y.; Park, J.; Lee, S. S.; Kim, Y.-W.; Park, B. H. J.
Phys. Chem. B 2002, 106, 6831.
(11) Sun, S.; Zeng, H. J. Am. Chem. Soc. 2002, 124, 8204.
A R T I C L E S Sun et al.
274 J. AM. CHEM. SOC. 9 VOL. 126, NO. 1, 2004
Qingyu
Highlight
Qingyu
Highlight
Qingyu
Highlight
Qingyu
Highlight
MSE
Highlight
MSE
Highlight
MSE
Highlight
to remove excess surfactants before drying under N2. The product was
then dispersed in deionized water (18 M¿) or 1 mM phosphate buffer
at neutral pH.
Nanoparticle Characterization. Fe, Co, Mn, and S elemental
analyses of the as-synthesized nanoparticle powders were performed
on inductively coupled plasma-optic emission spectrometry (ICP-OES)
at Galbraith Laboratories (Knoxville, TN). To prepare samples for
elemental analysis, the particles were precipitated from their hexane
dispersion by ethanol, centrifuged, washed with ethanol, and dried.
Samples for transmission electron microscopy (TEM) analysis were
prepared by drying a dispersion of the particles on amorphous carbon-
coated copper grids. Particles were imaged using a Philips CM 12 TEM
(120 kV). The structure of the particles was characterized using HRTEM
and selected area electron diffraction (SAED) on a JEOL TEM
(400 kV). X-ray powder diffraction patterns of the particle assemblies
were collected on a Siemens D-500 diffractometer under Co KR
radiation (ì ) 1.788965 Å). Near-edge X-ray absorption fine structure
(NEXAFS) spectroscopy was performed at the Advanced Light Source
at beamline 7.3.1.1, which was equipped with a spherical grating
monochromator and had an energy resolution of E/¢E ) 1800.
Magnetic studies were carried out using a MPMS2 Quantum Design
SQUID magnetometer with fields up to 7 T and temperatures from 5
to 350 K. Infrared spectra of dried particles pressed into KBr pellets
were obtained on a Nicolet Nexus 670 FTIR spectrometer. A homemade
spin valve sensor12 was used to detect a single layer of 16 nm Fe3O4
nanoparticles.
Results and Discussion
Fe3O4 Synthesis. As illustrated in Scheme 1, reaction of Fe-
(acac)3 with surfactants at high temperature leads to monodis-
perse Fe3O4 nanoparticles, which can be easily isolated from
reaction byproducts and the high boiling point ether solvent. If
phenyl ether was used as solvent, 4 nm Fe3O4 nanoparticles
were separated, while the use of benzyl ether led to 6 nm Fe3O4.
As the boiling point of benzyl ether (298 °C) is higher than
that of phenyl ether (259 °C), the larger sized Fe3O4 particle
obtained from benzyl ether solution seems to indicate that high
reaction temperature will yield larger particles. However,
regardless of the size of the particles, the key to the success of
making monodisperse nanoparticles is to heat the mixture to
200 °C first and remain at that temperature for some time before
it is heated to reflux at 265 °C in phenyl ether or at �300 °C
in benzyl ether. Directly heating the mixture to reflux from room
temperature would result in Fe3O4 nanoparticles with wide size
distribution from 4 to 15 nm, indicating that the nucleation of
Fe3O4 and the growth of the nuclei under these reaction
conditions is not a fast process.
The low cost of Fe(acac)3 and the high yields it produces
makes it an ideal precursor for Fe3O4 nanoparticle synthesis.
The more expensive Fe(acac)2 or Fe(II) acetate can also be used
but yields no better result than Fe(acac)3. Fe(II) (D-gluconate)
is another good precursor for Fe3O4 synthesis. In benzyl ether,
the reaction of Fe(II) (D-gluconate) with a 3-fold excess of each
of oleic acid and oleylamine and a 5-fold excess of 1,2-
hexadecanediol led to nearly monodisperse 8 nm Fe3O4 nano-
particles.
Several different alcohols and polyalcohols have been tested
for their reactions with Fe(acac)3. It was found that 1,2-
hydrocarbon diols, including 1,2-hexadecanediol and 1,2-
dodecanediol, react well with Fe(acac)3 to yield Fe3O4 nano-
particles. Long-chain monoalcohols, such as stearyl alcohol and
oleyl alcohol, can also be used, but particle quality is worse
and product yield is poorer than those with diols in the synthesis
of Fe3O4 nanoparticle seeds. However, in the seed-mediated
growth process, these monoalcohols can be used to form larger
Fe3O4 nanoparticles.11
Oleic acid and oleylamine are necessary for the formation of
particles. Sole use of oleic acid during the reaction resulted in
a viscous red-brown product that was difficult to purify and
characterize. On the other hand, the use of oleylamine alone
produced iron oxide nanoparticles in a much lower yield than
the reaction in the presence of both oleic acid and oleylamine.
When the 4 nm particles were oxidized by bubbling oxygen
through the dispersion at room temperature, they precipitated
from hexane as a red-brown powder (the characterization of a
similar product is discussed below). Adding more oleic acid
did not cause re-dispersion of this powder into hexane. However,
adding oleylamine did, leading to an orange-brown hexane
dispersion. This is consistent with the previous observation that
ç-Fe2O3 nanoparticles can be stabilized by alkylamine surfac-
tants,13 suggesting that -NH2 coordinates with Fe(III) on the
surface of the particles.
The larger Fe3O4 nanoparticles can also be made by seed-
mediated growth. This method has been recently applied to
larger metallic nanoparticle and nanocomposite synthesis14 and
is believed to be an alternative way of making monodisperse
nanoparticles along with LaMer’s method through fast super-
saturated-burst nucleation15 and Finke’s method via slow,
continuous nucleation and fast, autocatalytic surface growth.16
In our synthesis, the small Fe3O4 nanoparticles, the seeds, are
mixed with more materials as shown in Scheme 1 and heated,