sonochemical synthesis of metal oxides - připravované...
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Sonochemical Synthesis of Metal
Oxide Nanoparticles
Jiri Pinkas
Department of Chemistry
Masaryk University
Brno
Czech Republic
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OutlineIntroduction
Ultrasound and Sonochemistry
Sonochemical Synthesis of Nanoparticles
Iron Oxides - Fe2O3 - maghemite and hematite
- Fe3O4 - magnetite
Mixed Y/Fe oxides - YFeO3 and Y3Fe5O12
Ferrites CoFe2O4
Conclusions
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UltrasoundUtrasound frequencies from 20 kHz to 50 MHz
frequency, Hz
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Ultrasound in Chemistry
Sound = pressure waves = periodic compression/expansion
cycles traveling through a medium possessing elastic
properties (gas, liqud, solid)
frequency 20 kHz
Acoustic Cavitation = creation, growth, and implosive collapse of bubbles in a liquid
Bubble size
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Acoustic Pressure
cIPA 2
PA = driving pressure amplitude [Pa]
I = irradiation intensity [W m2]
(500 W system - 1.3 105 W m2)
ρ = liquid density [kg m3]
c = sound velocity in liquid [m s1]
(Water 1482 m s1)
Compression and rarefaction
(expansion) regions
PA = 620 700 Pa = 6.2 bar
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Bubble formation = breakage of liquid during expansion,
overcoming tensile strength (pure water 1500 bar, only 6.2 bar
available)
Weak spots needed = dissolved gas molecules, solid particles,
trapped gases
Bubble growth (300 µs), energy absorption, size oscillations
critical size (170-300 µm) = most efficient energy absorption, rapid
growth, inefficient energy absorption, collapse
Acoustic Cavitation
Cavitation effects = creation, growth, and implosive collapse of
bubbles in a liquid
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Bubbles collapse = spherically symmetrical implosion,
shear forces, adiabatic compression, life time 1-2 µs
Hot spot = end of the collapse
temperature of the gas inside bubble
5 000 – 20 000 C (for 1 ns)
surrounding liquid layer 2000 C
pressure 500 – 1500 bar
Extreme cooling rates 1010 K s1
red hot steel poured into water 2500 K s1
Acoustic Cavitation
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Cavitation effects = creation, growth, and implosive collapse of
bubbles (1-2 µs) in a liquid = implosion HOT SPOT (1 ns)
Acoustic Cavitation
stable cavitation - bubbles
oscillate for many cycles
transient cavitation -
transient cavities expand
rapidly
collapse violently
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Sonochemical Reactions
• Chemical changes/reactions induced by ultrasound
• No direct interaction of ultrasound field with molecules (in
contrast to photons, heat, electro-magmetic field,…)
• Liquid phase reactions – chemical reactions driven by cavitation
effects – radical generation, excited species formation,
mechanochemical bond scission, …
• Solid state reactions – introduction of defects = speeding up
diffusion
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Homogeneous Sonochemistry
Two-Site MechanismCavity interiorFilled with gases and vapors
temperatures 5 000 – 20 000 C
pressure 500 – 1500 bar
Surrounding liquid layertemperatures 2000 C
Bulk liquidShock waves, shear forces
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• Apparent blackbody temperature
• Ar emission
• SO and O2+ emission
How to Measure the Temperature
inside a Bubble ?Sonoluminescence - Light generated during the implosive
collapse of bubbles in liquids irradiated with ultrasound
95% H2SO4(aq.)
under Ar
20 kHz (14 W/cm2)
Ti horn directly immersed
T = 298 K
Kenneth S. Suslick
University of Illinois
8 000 – 15 000 K
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Sonochemical Reactor
Piezoelectric Ultrasound Generator
Ultrasound Processor VCX 500 W
Piezoelectric
transducer
PZT ceramics
Titanium horn
Reaction
vessel
Argon
inlet
AC generator
Frequency 20 kHz
Cooling
Piezoelectric
transducer
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Project Goals
Sonochemical synthesis of metal oxide nanoparticles
for magnetic, catalytic, biomedical applications
Metal acac complexes as precursors, organic solvents
Influence of reaction parameters, added water
Control of phase composition, particle size,
distribution, shape, crystallinity, metal stoichiometry in
mixed-metal oxides
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Product Control in Sonochemical
Synthesis of Metal Oxides
• Polymorphic modification control
Iron Oxides Fe2O3 - maghemite and hematite
• Oxidation state control
Reduction to Fe3O4 magnetite and Fe
• Phase control
Y-Fe oxides – YFeO3 and Y3Fe5O12
• Composition control - CoxFe2xO4 ferrite
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Iron Oxide-Based Materials
Magnetic nanoparticles
• Hyperthermia
• Magnetic drug delivery
• MRI contrast agents
Iron Gate
Samaria Gorge, Crete, Greece
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OO
M
H
CH3H3C
OO
M
CH3
- C3H4
200 °C
- CH3COCH3
300 °CMCO3 MxOy
765 °C
- CO2
M(acac)n Precursors
M = Fe, Y, Co, Mn
MO
O
O
O
O
O
Me
Me
Me
Me
Me
Me
Ismail, H. M. J. Anal. Appl. Pyrolysis 1991, 21, 315326.
Thermal decompositon pathway
• Volatile
• Organics soluble
• Nontoxic
• Well studied class of compounds
• Precursors in CVD
• Easily chemically modified
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• Solution of M(acac)3 (0.03 M)
• 50 cm3 of tetraglyme (b.p. 549.0 K)
• Water addition (0, 1, 3 cm3)
• Ar flow rate 60 cm3 min1
• Sonication 8 hrs
• Frequency 20 kHz
• Pulsed 2s / 2s
• Power 22 W cm2
• Colloidal soln. precipitated by hexane
• Centrifugation, washing with iPrOH
• Drying in air
Reaction Setup
VCX 500 W
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Iron Oxide-Based Materials
Fe2O3
amorphous
Fe2O3
maghemite
Fe2O3
hematite
300 oC
340 oC
He, Nitrogen
bulk
dynam/isothermal, air
Fe(acac)3
)))))
tetraglyme
TGLsolution
thin layer
Fe3O4
magnetite
200 oC
Fe3O4
magnetite
linear, air
340 oC
Fe
-iron
MO
O
O
O
O
O
Me
Me
Me
Me
Me
MeDefect spinel
Corundum
Spinel
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Sonochemical Synthesis
Amorphous Iron Oxides
Fe2O3
amorphous
)))))Fe(acac)3
Colloidal solution of iron oxide
Particle size by Dynamic Light Scattering
(Zetasizer)
Mean D = 9.2 nm (by volume)
Pinkas, J.; Reichlova, V.; Zboril, R.; Moravec, Z.; Bezdicka, P.; Matejkova, J. Ultrasonics Sonochem. 2008, 15, 257–264.
Particle size 20 - 30 nm
Spherical shape
Uniform size distribution
Specific surface area
BET 188 m2/g
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TEMproves amorphous character
of sono-Fe2O3
Electron diffraction
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Time under TEM beam
Maghemite or Magnetite
Crystallization of Amorphous Fe2O3
under TEM Beam
Electron diffraction
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Amorphous
Fe2O3
Crystallization induced
by heating (300 C)
HR-TEM
Fe2O3 calcined at 300 C
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Low blocking
temperature
25 K
Amorphous
Fe2O3
High-spin Fe3+ octahedral
superparamagnetic nanoparticles
size less than 10 nm
57Fe Mössbauer Spectra
of Sono-Fe2O3
Zero-Field
5T-Field
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Decomposition of Acac Ligands
OO
C
HC
C
H3C CH3
Fe
H2O
O
C
CH3H3C
OO
Fe
C
CH3
OO
Fe
C
CH3
OO
Fe
C
CH3
Fe
OO
C
HC
C
H3C CH3
FeH3C C C H
Speculation about the nature of residual organic groups
WET
DRYBinding modes of acetate groups
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3 5 0 0 3 0 0 0 2 5 0 0 2 0 0 0 1 5 0 0 1 0 0 0 5 0 0
0
0 . 2 5
0 . 5
0 . 7 5
F e J P 6
IR and MS Evidence for Acetate
in Sono-Fe2O3
as(COO)
1566 cm-1
s(COO)
1432 cm-1
Acetate stretchingDiketonate vibrations absent
Mass Spectrometry
Direct insertion probe, 70 eV
T = 50 – 300 C
m/z 60 / 45 / 43 = CH3COOH+
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Synthesis of Fe2O3 from
Fe(acac)3Water
%vol.
SA
m2 g1
H Pore vol.
cm3 g1
Fe
%
C
%
H
%
Mass loss %
at 500 ºC
dry 48 H3 0.304 22.0 30.5 4.52 63.1
2 105 H1 0.611 35.6 22.6 3.48 46.0
6 147 H3 0.455 43.6 15.3 2.75 35.2
2 + wet Arc 260 H2 0.291 42.0 15.5 2.73 37.3
Increasing water concentration
= larger surface area
= lower organics content
= higher metal content
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Nitrogen Adsorption-Desorption
Isotherms
0
0
0 11
)1(p
p
CV
C
CV
p
pV
p
p
mm
BET
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Specific Surface Area
BET surface area
of the Fe2O3 heated
to different
temperatures
during 12h
outgassing periods
120
140
160
180
200
220
0 50 100 150 200 250 300 350 400
Temperature, ºC
SA
, m
2/g
The oxide surface area increases as the acetate groups are
removed, then the particle size increases because of sintering
Surface area 48 to
260 m2 g-1 (BET)
depending on H2O
content
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BET Constant C
RT
qqC L1exp
q1 is the adsorption heat of the first layer
qL is the liquefaction heat
C is an indication of the affinity of the adsorbed molecule for the solid :
if this affinity is high, q1 >> qL and C is high (for example 100)
if the affinity is low, q1 ≥ qL and C may be as low as a few units.
For BET validity C = 20 – 200
0
0
0 11
)1(p
p
CV
C
CV
p
pV
p
p
mm
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BET Constant C
C constant (BET)
10,00
30,00
50,00
70,00
90,00
0 50 100 150 200 250 300 350 400
Temperature, oC
C
The strenght of interaction of nitrogen with oxide surface increases
as the acetate groups are removed
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Composite Particles of Sono-Fe2O3
HR-TEM (5 nm bar)
TEM (20 nm bar)
after heating to 250 °C
Iron oxide particle size 2 - 3 nm
Embedded in organic matrix
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Thermal Transformations of
Amorphous Iron Oxides
Fe2O3
amorphous Fe2O3
hematite
dynam/isothermal, air
Fe(acac)3
)))))
tetraglyme
340 oC
thin layer
Heating in on a hot-stage of an XRD diffractometer
Sample in a thin layer on a Pt holder
Ramp 2.5 °C min-1, 2 min data collection, 25 °C steps
Polymorphic modification control
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HT-PXRD of Sono-Fe2O3
Amorphous Hematite
Crystallization
325 - 350 C
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Hematite Particle Size
30
40
50
60
70
80
350 400 450 500 550 600
Temperature, °C
D,
nm
D/nm, 104
Coherence length
D (nm)
By Scherrer
equation
Dependence of the coherence length, D (nm) of -Fe2O3 on
the crystallization temperature under dynamic-isothermal
conditions of the HT-XRD measurement
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Crystallization to hematite induced by heating (above 300 C)
BET Surface area decreased from 188 to 120 m2/g
HR-TEM
Fe2O3 calcined at 300 CFe2O3 calcined at 600 C
TEM
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Thermal Transformations of
Amorphous Iron Oxides
Fe2O3
amorphous Fe2O3
maghemite
linear, air
Fe(acac)3
)))))
tetraglyme
300 oC
thick layer
Heating in a DSC crucible
Sample in a thick layer
Ramp 2.5 °C min1
360 °C250 °C
300 °C
Polymorphic modification control
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20 40 60 80 100
2[deg]
2000
3000
4000
cou
nts
2000
4000
6000
8000
16000
24000
maghemite
250 oC
300 oC
360 oC
PXRD
of amorphous Fe2O3
heated dynamically in air
up to 250, 300, and 360 °C
250 °C
300 °C
360 °C
Maghemite
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In-field 57Fe Mössbauer Spectrum of
Amorphous Fe2O3 Heated to 300 °C
subspectra for the tetrahedral and octahedral positions of
Fe3+ in the defect-spinel structure of maghemite resolved
some content (cca 21%) of amorphous phase is still present
20 K / 6 T
Maghemite
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Solution Thermolysis Amorphous Iron Oxide
Red-brown colloidal solution after sonolysis
Particle size by DLS (Zetasizer)
Mean D = 9.2 nm (by volume)
Black suspension, magneticParticle size by DLS (Zetasizer)
Mean D = 11.3 nm (by volume)
Surface area 103 m2 g1 BET
Heating to 250 C
3 hrs in air
Fe2O3
amorphous Fe3O4
magnetite
TGL solution
Fe(acac)3
)))))
tetraglyme
250 oC
Oxidation state control
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HR-TEM
Fe2O3 thermolysed at 250 C
TEM
SAED
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XRD of Fe2O3 Thermolysed at 250 C
Coherence domain size
by Scherrer equation
8 - 9 nm
Magnetite Fe3O4
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57Fe Mössbauer Spectrum of Fe2O3
Thermolysed at 250 C
T
(K) 0.01
(mm/s)
ΔEQ 0.01
(mm/s)
Bhf 0.03
(mm/s)
0.01
(mm/s)
A
()
Sextet 293 K 0.42 -0.03 26.89 0.61 84.3
Dublet 0.35 0.81 ---- 0.47 11.3
Singlet 0.34 --- --- 0.47 4.5
high-spin Fe3+ octahedral
superparamagnetic nanoparticles
size less than 10 nm
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Thermal Transformations of
Amorphous Iron Oxides
Fe2O3
amorphous Fe3O4
magnetite
Helium, Nitrogen
Fe(acac)3
)))))
tetraglyme
250 oC
Fe
-iron
Heating in on a hot-stage of an XRD diffractometer
Flowing He gas
Sample in a thin layer on a Pt holder
Ramp 5 °C min-1, 20 min data collection, 50 °C steps
TG/DSC under flowing nitrogen
Sample in a thick layer in a Pt crucible
Ramp 5 °C min-1
Oxidation state control
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100 200 300 400 500 600 700 800 900Temperature /°C
40
50
60
70
80
90
100
TG /%
Mass Change: -43.90 %
Mass Change: -15.48 %
[1]
300 °C
250 °C
700 °C
**
* = Pt holder
Magnetite Fe3O4PXRDof amorphous Fe2O3
heated dynamically in He
Magnetite Fe3O4
Wustite FeO
Iron Fe
TG/DSC in N2
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Sonochemical Synthesis
of Ternary Y/Fe Oxides
amorphous
)))))
)))))
Y(acac)3
YxFeyOz
Fe(acac)3
crystalline
Y3Fe5O12
YFeO3
crystalline
Y/Fe = 3/5
Y/Fe = 1/1
TetraglymeCalcination
One-step synthesis
Perovskite (YIP)
Garnet (YIG)SEM
Phase Control
Pinkas, J.; Reichlova, V.; Serafimidisova, A.; Moravec, Z.; Zboril, R.; Jancik, D.; Bezdicka, P.
J. Phys. Chem. C 2010, 114, 13557-13564
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SEM and TEM of Sono-YFeO3
As-prepared sono-YFeO3 is amorphous
Particle size 30-50 nm
Uniform particle size distribution
BET surface area 85 m2 g1
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57Fe Mössbauer Spectra
of Sono-Y-Fe-Oxide
Temperature
KComponent
IS
mm s-1
EQ
mm s-1
Q
mm s-1B / T A / % Assignment
RT D 0.34 0.79 – – 100.0Fe3+ HS
octahedral
25 D 0.46 0.84 – – 100.0
Fe3+ HS
octahedral
amorphous
Quadrupole doublet
High-spin Fe3+
Octahedral coordination
Superparamagnetic nanoparticles
Size less than 10 nm
Amorphous
YFeO3
Same parameters for amorphous Fe2O3, YFeO3, Y3Fe5O12
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4000 3500 3000 2500 2000 1500 1000 500
Absorbance
-1
-0.8
-0.6
-0.4
-0.2
Acac to Acetate Transformation
as(COO)
1587 cm-1
s(COO)
1386 cm-1
Acetate stretchingDiketonate vibr. absent
OO
C
HC
C
H3C CH3
Fe
H2O
O
C
CH3H3C
OO
Fe
C
CH3
OO
Fe
C
CH3
OO
Fe
C
CH3
Fe
OO
C
HC
C
H3C CH3
FeH3C C C H
Mass spectrometry
Direct insertion probe, 70 eV
T = 50 – 300 C
m/z 60 / 45 / 43 = CH3COOH+
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Crystallization of Sono-YFeO3
Perovskite YFeO3
700 °C
800 °C
780 °C
760 °C
740 °C
720 °C
Ramp 1 °C min-1, 1 min equilb.,
30 min data collect., 20 °C steps
HT-XRD25-1000 °C
Size 60 nm
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Growth of Particle Size in YFeO3
Dependence of the coherence length, D (nm) of YFeO3 on
the crystallization temperature under dynamic-isothermal
conditions of the HT-XRD measurement under air
coherence
length
D (nm)750 °C
70 nm
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Calcination of Sono-YFeO3 in Air
200 400 600 800 1000Temperature /°C
-3
-2
-1
0
1
2
3
DSC /(mW/mg)
40
50
60
70
80
90
100
TG /%
[1] FeY88air_1.dsu TG
DSC
Mass Change: -43.44 %
Mass Change: -19.39 %
Mass Change: -1.65 %
End: 347.0 °C
End: 723.6 °C
[1]
[1]
exo
Removal of weakly bound groups
Oxidation of tightly bound groups
OH removal
Crystallization
TG
DSC
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Calcination of Sono-YFeO3 in N2
sono-YFeO3YFeO3 + Y2O3 + Fe
Reduction of Fe(III) to Fe(0) by organic residuals
Removal of weakly bound groups
Removal of tightly bound groups
Reduction
Crystallization XRD
TG
DSC886 C
Metal-Oxide Composite
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Sonochemical Synthesis of
CoFe2O4
amorphous
)))))
)))))
Co(acac)3
CoFe2O4
Co(acac)2
)))))
Fe(acac)3
CoFe2O4
crystalline Spinel
Composition control
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SEM/TEM of Amorphous Co-Fe Oxide
TEM of CoFe Oxide Calcined at 300 C
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CoFe2O4 - Metal Stoichiometry
Single phase CoFe2O4
obtained for the final product stoichiometry
Co : Fe from 1 : 1.3 to 1 : 2.0
Excess Co resulted in CoO separation
Excess Fe resulted in Fe2O3 separation
Composition control
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HT-XRD of CoFe Oxide
Direct
crystallization to
CoFe2O4
300 oC
400 oC
500 oC
600 oC
700 oC
800 oC
900 oC
1000 oC
Ramp 1 °C min-1, 1 min equilb., 30 min data collect., 20 °C steps
No hematite
Size 15 nm
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TG-DSC of Sono-CoFe2O4 in Air
Removal of weakly bound groups
Removal of tightly bound groups
Complete removal of organics
below 300 oC
TG
DSC
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HT-XRD of CoFe Oxide300 - 1000 C
8,3
8,32
8,34
8,36
8,38
8,4
8,42
8,44
8,46
8,48
8,5
0 200 400 600 800 1000
Temperature, oC
0
10
20
30
40
50
60
70
80
90
100
a sp
D sp
Particle Size
of CoFe2O4
Lattice parametr
of CoFe2O4
Particle size
under 20 nm
up to 600 C
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TEM of CoFe Oxide Calcined at 300 C
CoFe2O4
nanoparticles
covered with an
amorphous layer
preventing their
growth
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TEM of CoFe Oxide Calcined
at 400 C
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Calcination of Sono-CoFe2O4 in N2
200 400 600 800 1000Temperature /°C
-1.5
-1.0
-0.5
0.0
DSC /(mW/mg)
40
50
60
70
80
90
100
TG /%
[1] CoFe13-1_1.dsu TG
DSC
DSC: 936.0 °C
[1]
[1]
exo
TG
DSCMp. 936 C
Complete
removal of
organics
below 600 oC
XRD Co-Fe alloy
Complete reduction of CoFe2O4 nanoparticles by carbon-containing
residues in the absence of oxygen
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ConclusionsPolymorphic modification control
Iron Oxides Fe2O3 - maghemite and hematite
Oxidation state control
Reduction to Fe3O4 magnetite and Fe
Phase control
Y-Fe oxides – YFeO3 and Y3Fe5O12
Composition control
CoxFe2xO4 ferrite, Co : Fe ratio from 1 : 1.3 to 1 : 2.0
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AcknowledgmentFinancial support:
Ministry of Education
MSM0021622410 and 6198959218
Grant Agency of the Czech Republic (203/08/1111,
106/09/0700)
Ph.D. students:
Zdenek Moravec
Jan Chyba
Petr Ostrizek
M.S. students:
Iva Kolhammerova
Martin Janicek
David Skoda
Ales Styskalik
B.C.
Martin Kejik
Prof. Radek Zboril, Mössbauer sp.
Prof. Zdenek Travnicek, CHN
Dr. Petr Bezdicka, HT-XRD
Dr. Mariana Klementova, TEM
Dr. Nataliya Murafa, TEM
Dr. Dalibor Jancik, TEM
Dr. Eva Vecernikova, TG-MS
Dr. Oldrich Schneewiess, Magnetic
Dr. Petr Pikal, TG-MS
Dr. Jirina Matejkova, SEM
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Department of Chemistry
Masaryk University
Brno
Czech Republic