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Posiandon (x =
CobHepta
itron d Phot
nan= 0.0 –
Co++ O-
heating
balt Sulphateahydtrate (1.
Cobalt Oxi (1.0)
CHann
tocatnocry– 2.0)
+
O- C
C
+
C
e .0)
ide
Cobalt
pH
HAnihilaalyticystall) spin
O-
Cr+++ O-
Cr+++
+
CoCrxFe2-x
ChromHepx
t oxide (x)
H = 3.5
PTation c degine
nel fer
O-
O- Fe+++
Fe+++
O4 (Final p
mium Sulphaxahydtrate (x
Ferric oxi
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ate x)
de (2-x)
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ing and strin
Ferrous SuHeptahydtr
pH = 1OxidatOH- -
4 scopystudye2-xO4
ng at 60 °C
Na+ OH-
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y y 4
Chapter 4
4.1
4.1 X – ray powder diffractometry, Thermo Gravimetric (TG) and
Differential Scanning Calorimetric (DSC) analysis of
CoCrxFe2-xO4 spinel ferrite precursors
4.1(A) X – ray powder diffraction patterns analysis
Shown in Figure 4.1.1 are the room temperature (300 K) X – ray powder diffraction
patterns for the two end members, x = 0.0, CoFe2O4 and x = 2.0, CoCr2O4 precursors
of CoCrxFe2-xO4 spinel ferrite system.
Figure 4.1.1: X – ray powder diffractograms for Co – Cr ferrite precursors at
300 K.
Chapter 4
4.2
The spectra for the undigested particles have broad peaks without any
structure. The background noise and broadness of the peaks are characteristic of
particles with nano meter dimensions [1]. This happens because in nano size particles
there are insufficient diffraction centers that cause the line broadening [2].
4.1 (B) Thermo Gravimetric Analysis (TGA) and Differential Scanning
Calorimetric (DSC) study
The observed water content was determined from the weight difference measured at
30 – 700 °C from thermogravimetric data. The thermogravimetric analysis (TGA)
measurement will help to determine whether the change is physical or chemical in
nature. The reaction is chemical in nature if a mass change is associated with it and
physical if no mass change occurs.
The representative thermogravimetric (TG) traces for spinel ferrite precursor
with x = 0.0, 0.3, 1.1, 1.5 and 2.0 compositions of the system CoCrxFe2-xO4 are shown
in the Figure 4.1.2. DSC profiles, where the endothermic heat flow is measured versus
temperature are shown in Figure 4.1.3. The TGA traces exhibit three distinct weight
loss steps. The TG curves show total weight loss of 12 to 29% for x = 0.0 to 2.0
compositions in the temperature range 30 – 700 °C. In the temperature range
30 – 150 °C, 8 – 18 % of subsequent weight loss is observed, which is accompanied
by an endothermic broad hump around 95 ± 10 °C in the differential scanning
calorimetry (DSC) curves. This event is attributed to the dehydration process wherein
significant amount of adsorb water is released from the wet chemically synthesized
ferrite compounds.
Such peak is associated with nucleation of ferrite crystal from amorphous
precursor powder (Figure 4.1.1). The observed endothermic peak represents
decomposition of the metal hydroxides to oxides [4]. In the graphs it is mentioned that
sample started to degrade (decomposed) from 200 °C (Figure 4.1.3). The fact that
there are no such peaks above 105 °C shows that the formation of ferrite is almost
complete at this temperature and annealing above 200 °C is likely to give only grain
growth. This is consistent with the X-ray diffraction results described in the next
section. The further 2 – 8 % weight loss during 150 – 250 °C may be correlated with
Chapter 4
4.3
the removal of dispersant anion and hydroxyl group as reflected in EDAX spectra of
the samples heated at 200 °C.
The observed increase in total weight loss from 12 % for x = 0.0 composition
to 29 % for x = 2.0 composition, suggests that Cr3+ ions have tendency to adsorb
water in the lattice structure during chemical reaction of ferritization. The samples
heated at 300 °C had almost constant weight upon heating to higher temperature,
revealing the fact that Co – Cr ferrites are free from dispersant anions and hydroxyl
groups [3].
The powdered samples were dried at 473 K under vacuum for 8 h after
confirmation from TGA analysis, and the same samples were used for further
characterizations.
The various parameters determined from TGA and DSC measurements such
as total percentage weight loss, peak area, peak height and endothermic enthalpy are
given in Table 4.1.1.
Figure 4.1.2: TGA traces for cobalt – ferri – chromite precursors.
Chapter 4
4.5
Figure 4.1.3: Differential scaning calorimetry curves for x = 0.0, 1.1, 1.5 and 2.0
compositions of CoCrxFe2-xO4 system.
x= 1.5
x= 2.0
Chapter 4
4.6
Table 4.1.1: Paramters determined from TGA and DSC analysis.
Cr3+
content (x)
Weight loss
(in %) at 700 °C
Peak area
(mJ)
Peak
height
(mW)
Peak
temperature
(°C)
Enthalpy
(J/g)
0.0 12 221.06 0.93 85.38 86.52
0.3 20 − − − −
1.1 26 257.17 1.03 104.6 102.01
1.5 27 261.31 1.12 103.8 102.72
2.0 29 309.91 1.23 104.08 116.29
Conclusions
(i) The undigested particles of ferrite precursors shows amorphous like strucutre.
(ii) The weight loss increases with increase of Cr3+ - substitutuion in CoFe2O4,
suggest, Cr3+ ions have tendency to adsorb water during chemical reaction.
(iii) The ferritization or crystallization is taking place for temperature of 200 °C.
Chapter 4
4.7
References
1. J. P. Chen, C. M. Sorensen, K. J. Klabunde, G. C. Hadjipanayis, E. Devlin,
A. Kostikas, ‘Size-dependent magnetic properties of MnFe2O4 fine particles
synthesized by co-precipitation’, Phys. Rev. B, 54 (13) (1996) 9288 – 9296.
2. M. K. Rangolia, M. C. Chhantbar, A. R. Tanna, K. B. Modi, G. J. Baldha,
H. H. Joshi, ‘Magnetic behaviour of nano – sized and coarse powders of Cd –
Ni ferrites synthesized by wet – chemical route’, Ind. J. Pure Appl. Phys. 46
(2008) 60 – 64.
3. M. Rajendran, S. Deka, P. A. Joy, A. K. Bhattacharya, ‘Size-dependent
magnetic properties of nanocrystalline yttrium iron garnet powders’, J. Magn.
Magn.Mater. 301 (1) (2006) 212 – 219.
4. M. Javed Iqbal, M. Rukh Siddiquah,’Structural, electrical and magnetic
properties of Zr–Mg cobalt ferrite’, J. Magn. Magn. Mater., 320 (6) (2008)
845 – 850.
Chapter 4
4.8
4.2 Elemental analysis by Energy Dispersive Analysis of X-rays
(EDAX)
The wet-chemical methods or soft chemical routes like co-precipitation [1], sol-gel
[2], combustion [3], reverse micelle technique [4], hydrothermal route [5] for growing
nano-crystallites (bottom-up techniques) of ferrite materials are prone to
contamination and loss of compositional stoichiometry. Moreover, it is difficult to
obtain consistency in the physical properties of electro-ceramics synthesized by
chemical routes, particularly for the system containing more than three cations,
percentage substitution is very small or tetravalent – pentavalent cationic substituted
systems. The resultant off – stoichiometric composition shows unusual or unexpected
behaviour that is not possible to explain on the basis of normal stoichiometric
composition. Thus, to ratify the purity and surety of the chemical composition, energy
dispersive analysis of X-rays (EDAX) measurement was carried out at 300 K.
The EDAX spectra for the typical compositions of the system: CoCrxFe2-xO4,
with x = 0.0 (CoFe2O4), x = 1.1 (CoCr1.1Fe0.9O4) and x = 2.0 (CoCr2O4) are shown in
Figure 4.2.1.
The energy of the K, L and M series X-rays increase with increasing atomic
number (Z). For the normal energy range, typical of most spectrometers, 15 – 20 kV,
light elements will emit X-rays of the L series or K and L series. Intermediate
elements will emit X-rays of the L series or K and L series. On the other hand, heavy
elements will emit X-rays of the M series or L and M series [6]. Thus, it is possible to
record a wide range of elements simultaneously during a given scan.
In the spinel ferrite system under investigation, CoCrxFe2-xO4 light elements
like oxygen (O) (Z = 8), intermediate elements such as Cobalt (Co) (Z = 27),
Chromium (Cr) (Z = 24) and Iron (Fe) (Z = 26) are present while heavy elements are
not present.
The EDAX patterns shown in Figure 4.2.1, clearly show three characteristic
X-ray lines located between 5.3 keV to 7.7 keV energies for un-substituted cobalt
ferrite, CoFe2O4 (x = 0.0). For all the Cr3+ - substituted cobalt ferrite compositions
(x = 0.1 – 1.9), five peaks and for cobalt chromite, CoCr2O4 (x = 2.0), four peaks are
observed between said energy range.
Chapter 4
4.9
Figure 4.2.1: Room temperature (300 K) EDAX spectra for CoCrxFe2-xO4 spinel
ferrite system (x = 0.0, 1.1, 2.0).
x = 0.0
x= 1.1
x = 2.0
Chapter 4
4.10
The maximum observed at ~ 6.4 keV for all spectra is assign to FeKα line.
Here, it is important to note that CoKα (6.93 keV) line interferes (overlaps) with FeKβ
(7.06 keV) line in the spectra. The small peak at extreme right of the spectra centered
at ~ 7.65 keV clearly comes from CoKβ1. The intense peak located at 5.405 keV and
small peak appeared at ~ 5.95 keV are corresponding to CrKα1 and CrKβ1 respectively.
The maximum observed in the left part of the spectra at ~ 0.5 keV clearly comes from
O Kα while for peak that is located at ~ 0.75 keV comes from FeLα1 characteristic
line. It is important to note that if a Kα line is identified in a spectrum then a Kβ line
should exist having approximately a tenth of counts of the Kαline (Kα : Kβ= 10 : 1)
[6]. We have observed same relationship for CoKα and CoKβ1, CrKα1 and CrKβ1 lines
in the spectra. The low intensity peak at extreme left of the spectra centered at ~ 0.25
keV connected with carbon (CKα) characteristic line of impurity. The hardly visible
peaks at ~ 1.06 keV, ~ 2.4 keV and ~ 3.7 keV belong to impurity peak of sodium,
NaKα1/Naβ1, sulphur, SKα1/SKβ1 and calcium, CaKβ1 characteristic line respectively.
The origin of sulphur and sodium impurities is well understood from the chemical
used for the synthesis of spinel ferrite system, CoCrxFe2-xO4, i.e. CoSO4.7H2O,
FeSO4.7H2O and Cr2(SO4)3.6H2O as well as NaOH used as a precipitant. On the other
hand, impurity like carbon was likely to have been introduced from carbon-coated
shields to the pole pieces and special EDAX specimen holder made of carbon,
beryllium and aluminium used in the EDAX spectrometer [7]. The origin or source of
calcium impurity is not clearly understood. Further, the incorporation of Cr3+ in the
place of Fe3+ was indicated by the intensities of the respective peaks in the EDAX
patterns.
The atomic percentage (at %) and weight percentage (wt %) of constituent
elements, (Co, Cr, Fe and O) are calculated theoretically from the intermediate
chemical composition CoCr1.1Fe0.9O4 (x = 1.1) and that obtain from EDAX elemental
analysis are shown in Table 4.2.1. It can be seen that the stoichiometry is very close to
the anticipated values with small deficiencies of Cr3+ ions.
The EDAX results suggested that the precursors had fully undergone the
chemical reaction to form ferrite material of the expected composition.
Chapter 4
4.11
The peak to background (P/B) ratio for different elements is found to be large,
so background did not introduce much error. The (P/B) ratio for constituent elements
is also included in Table 4.2.1.
Table 4.2.1: Estimated stoichiometry for CoCr1.1Fe0.9O4 ferrite composition
from EDAX analysis.
Element
Weight percentage (wt %)
Atomic percentage (at %)
(P/B) ratio
Expected EDAX
analysis Expected
EDAX
analysis
O 27.78 27.56 57.14 56.90 197
Fe 21.82 21.36 12.86 12.66 78
Co 25.58 25.28 14.28 14.20 33
Cr 24.82 24.30 15.72 15.31 53
Total 100.00 − 100.00 − −
Conclusions
(i) The analysis of EDAX spectra have confirmed expected stoichiometry
without the loss of any ingredient.
(ii) All the peaks are well assigned in accordance with the standard positions.
(iii) The source of impurity peaks correspond to C, Na and S is well understood
but the origin Ca impurity in the spectra is not clear.
Chapter 4
4.12
Illustrative calculations for atomic percentage and weight percentage
Atomic percentage (at%) for CoCr1.1Fe0.9O4
(i) Molecular weight : (1) (58.93 amu) + (1.1) (52.0 amu) + (0.9)(55.85 amu)
+ (4) (16 amu)
= 58.93 + 57.2 + 50.265 + 64
= 230.395 amu
In the spinel ferrite material with general chemical formula, A+21B+3
2O-24, there are
total 7 atoms per formula unit.
(ii) Atomic contribution
Total no. of atoms is 7, corresponding molecular weight is 230.395 amu
∴ for 4 Oxygen atoms corresponding molecular weight is how much?
= 131.65 amu
(iii) Contribution in percentage
For the total molecular weight
of 230.395 amu, contributions from oxygen atoms is 131.65 amu
∴ for 100 amu contributions from oxygen atoms is how much ?
= 57.14 % (Expected)
= 56.90 % (Observed)
Wight percentage (wt %) for CoCr1.1Fe0.9O4
For the total molecular weight
of 230.395 amu, contribution from Fe ion is 50.265 amu
for 100 amu contribution from Fe ion is how much?
= 21.82 % (Expected)
= 21.16 % (Observed)
Chapter 4
4.13
References
1. K. B. Modi, N. H. Vasoya, V. K. Lakhani, T. K. Pathak, P. M. G. Nambissan,
‘Crystal defects and cation redistribution study on nanocrystalline cobalt –
ferri-chromites by positron annihilation spectroscopy’, Int. J. Spectro., 2013
(2013) 1 – 11.
2. I. Ahmad, T. Abbas, M. U. Islam, A. Maqsood, ‘Study of cation distribution
for Cu–Co nano ferrites synthesized by the sol–gel method’, Ceram. Int. 39 (6)
(2013) 6735 – 6741.
3. S. S. Manoharan, K. C. Patil, ‘Combustion Synthesis of Metal Chromite
Powders’, J. Am. Ceram. Soc., 75 (4) (1992) 1012 – 1015.
4. P. Pulisova, J. Covac, A. Voigt, P. Raschman, ‘Structure and magnetic
properties of Co and Ni nano-ferrites prepared by a two step direct
microemulsions synthesis’, J. Mag. Mag. Mater, 341 (2013) 93 – 99.
5. S. Phumying, S. Labuayai , E. Swatsitang, V. Amornkitbamrung, S. Maensiri,
‘Nanocrystalline spinel ferrite (MFe2O4, M = Ni, Co, Mn, Mg, Zn) powders
prepared by a simple aloevera plant-extracted solution hydrothermal route’,
Mater. Res. Bul., 48 (6) (2013) 2060 – 2065.
6. http://www.charfac.umm.edu.
7. http://nanoanalysis.materials.ox.ac.uk.
Chapter 4
4.14
4.3 Particle size distribution study
Size of particles influences many properties of particulate material. Furthermore, it is
a valuable indicator of quality and performance of material. In many applications,
particle size plays critical role, for example, it determines (a) appearance and gloss of
paint (b) flavor of coco powder (c) reflectivity of highway paint (d) absorption rate of
pharmaceuticals (e) appearance of cosmetics and (f) hydration rate and strength of
cement. Of course, this is more applicable to nano regime.
Particle size growth may be monitored during operations such as granulation
or crystallization. Determining the particle size of powders requiring mixing is
common since materials with similar and narrower distributions are less prone to
segregation [1].
Particle size distribution data can be presented in tabular format i.e.
numerically or graphically. In graphical form data are presented in differential and
cumulative distribution curves. Both the forms are interrelated, if one differentiated
the cumulative distribution curve, the differential distribution is obtained. On the
other hand, if one integrated the differential distribution curve, the cumulative
distribution is obtained [2]. The differential distribution shows the relative amount at
each particle size. From the different size distribution, measures of central tendency
such as the modal and mean diameters are determined. The diameter at the peak of
the differential distribution is the modal diameter while the mean diameter is the
average diameter.
The corresponding cumulative distribution curve demonstrates the relative
amount at or below a particular size. The median diameter is another measure of
central tendency. It is the diameter at the 50th percentile, designed d50. Quartile
diameters include d75, d50 and d25. There are several measures of absolute width one
can derive given the cumulative distribution. One common measure is the span, d90-
d10. A dimensionless measure of width is the relative span defined as span/d50. Other
relative measures of width include percentile ratios such as d90/d10 and d75/d25.
Chapter 4
4.15
Figure 4.3.1: Illustrative differential size distribution and cumulative
undersize distribution curves.
Figur
x= 2
x= 1
x =
re 4.3.2: Pa
com
2.0
1.1
0.0
article size d
mpositions
Chapter 4
4.16
distribution
of CoCrxFe
curves for x
e2-xO4 spinel
x = 0.0, 1.1 a
l ferrite syst
and 2.0
tem.
Chapter 4
4.17
Typical particle size distribution patterns, differential size distribution and
cumulative undersize distribution, for x = 0.0 and 1.1 and 2.0 compositions are shown
in Figure 4.3.2. The distribution is bimodal (double peaked) as well as not mono
disperse (all one size). Earlier, a bimodal size distribution was observed for the as
prepared sample and the sample annealed at 300 °C with an average particle sizes of
(∼ 2 nm and ∼ 8 nm) and (∼ 4 nm and ∼ 8 nm) respectively, for the two samples of
nickel ferrite synthesized using the sol-gel process [3]. On the other hand, the
existence of a broad (bimodal) distribution in the crystallite size has also been
reported for the high energy mechanically milled NiFe2O4, MgFe2O4, Fe3O4
nanoparticles and other ultrafine mechanically alloyed materials [4]. The origin of the
bimodality lies in the growth process by which the particles are formed. In a chemical
growth process such as co-precipitation which is used here, growth occurs by initial
nucleation and growth via a ‘seed and grow’ mechanism, followed by Ostwald
ripening. For smaller particle systems, where the growth has been restricted, some
original seeds remain in the colloid. For the larger particle systems a greater
percentage of the seeds have been observed in the ripening process leading to a more
uniform particle size distribution [5].
A careful examination of Figure 4.3.2 shows that for x = 0.0 composition two
well separated peaks are observed. The peak on the left hand side is with less
intensity and asymmetric one i.e. the curve tails to the left more than to the right, that
means the skew is negative. The peak on the right hand side with more intensity
having symmetric differential distribution i.e. has zero skew. The skew is positive if
curve tails to the right more than to the left. The reference point for tailing is with
respect to the modal diameter. On increasing Cr3+ - substitution (x) in the system,
CoCrxFe2-xO4, for x = 1.1 composition (CoCr1.1Fe1.9O4) both the peaks get merged and
also have same intensity. On the other hand, for cobalt chromite (x = 2.0), once again
two well resolved peaks are observed. The left hand side peak is with more intensity
and asymmetric in nature while the peak on the right hand side is with less intensity
but symmetric one.
There are several measures of width. One measure of width is FWHM, the full
width at half maximum. It is obtained by drawing a horizontal line at 50% of the
maximum and taking the difference between the two places it intersects the
Chapter 4
4.18
distribution. HWHM, the half width at half maximum, is another measure of width. It
is defined as FWHM/2. A relative fractional measure of width is obtained by dividing
HWHM by the measure of central tendency from which it was derived, the modal
diameter (HWHM/modal diameter).
The size of the particles shown in Figure 4.3.2 is in micrometer (μm) order.
These particles were agglomerates which were found to break further and further to
submicron level with more and more powerful ultrasonic de-agglomeration
techniques.
The important parameters such as: modal diameter, mean/average diameter,
full width half maximum (FWHM), span (d90-d10), relative span (span/d50), quartile
ratio (d75/d25) and median diameter (d50), for CoCr2O4 (x = 2.0) is determined and
tabulated in Table 4.3.1
Table 4.3.1: Measures of central tendency and width for CoCr2O4 (x = 2.0)
composition.
Parameter LHS Peak RHS Peak
Modal diameter 85 μm 300 μm
Average diameter 95 μm 350 μm
FWHM 177.5 μm 200 μm
Span 246.5 μm −
Relative span 4.93 −
Quartile ratio 8.12 −
Median diameter 55 μm −
Relative percent measure of width 104.4 % −
d10 = 4.5 μm, d25 = 15.4 μm, d50 = 55 μm, d75 = 125 μm and d90 = 250 μm.
Chapter 4
4.19
Conclusions
(i) Particle size distribution curves analysis suggests that the distribution is
bimodal as well as not mono disperse and having negative skew.
(ii) The size of the particles is in micrometer order and ultrasonic de-
agglomeration is required before further analysis.
(iii) Various important parameters can be determined from the differential size
distribution and cumulative undersize distribution curves.
(iv) The reason for bimodality lies in the growth mechanism and the relative
proportion of particles formed by nucleation and Ostwald ripening.
Chapter 4
4.20
References
1. http://www.Horiba.com.
2. http://www.Brookhaveninstruments.com.
3. R. Malik, S. Annapoorni, S. Lamba, V. R. Reddy, Ajay Gupta, P. Sharma,A.
Inoue. ‘Mossbauer and magnetic studies of nickel ferrite nanoparticles:
Effect of size distribution’, J. Magn. Magn. Mater., 322 (2010) 3742 – 3747.
4. V. Sepelak, D. Baabe, D. Mienert, D. Schultze, F. Krumeich, F. J. Litterst,
K. D. Becker, ‘Evolution of structure and magnetic properties with annealing
temperature in nanoscale high-energy-milled nickel ferrite’, J. Magn. Magn.
Mater., 257 (2003) 377 – 386.
5. M. Blanco – Mantecon, K. O’Grady, ‘Grain size and blocking distributions in
fine particle iron oxide nanoparticles’ J. Magn. Magn. Mater., 203 (1999)
50 – 53.
Chapter 4
4.21
4.4 Transmission Electron Microscopic (TEM) analysis
The morphology of Co – Cr ferrites nanoparticles prepared by the co-precipitation
route was examined by transmission electron microscopy (TEM). Figure 4.4.1(a – e)
shows bright field TEM pictures for x = 0.0, 0.3, 1.1, 1.5 and 2.0 compositions of
spinel ferrite system, CoCrxFe2-xO4. TEM micrographs show highly agglomerated
particles of nanoscale nature for all the compositions. This is because of the fact that
they experience permanent magnetic moment proportional to their volume. Hence,
each particle is permanently magnetized and gets agglomerated. The system under
investigation possesses cations which are highly magnetic in nature, Co2+ (3 µB),
Cr3+ (3 µB), Fe3+ (5 µB), such clustering of nanoparticles is expected. It can be seen
that for cobalt ferrite, CoFe2O4 (x = 0.0), clusters of irregularly shaped nanoparticles
with very few needle-shape nanoparticles, while for all other compositions no such
needle shaped particles are observed. In the present case, from TEM images it is not
possible to estimate particle size accurately, but in broad sense we can see that
particle size decreases with increasing Cr3+ - content (x) in the system. Earlier, we
have observe very systematic transformation of spherically shaped particles to
lamellar to thick needle shape particle morphology and decrease in particle size with
increase in Mg2+ - concentration (x) for Mn2+ in the system, MgxMn1-xFe2O4 (x = 0.0 –
1.0), [1]. The observed reduction in particle size and presence of needle shape
particles can be explain on the similar line of argument.
The growth of crystals in the solution is governed by different parameters.
Among all such parameters the most important being the molecular concentration of
the material approaching the tiny crystal surface during the growth process. Because
of the liberation of the latent heat at the surface, the local temperature is normally
higher than the solution temperature. The surface temperature affects the local
molecular concentration at the crystal surface and hence the crystal growth [2]. It
seems that the formation of cobalt chromite (x = 2.0) is more exothermic as compared
to the formation of cobalt ferrite, CoFe2O4 (x = 0.0). According to Jain et al [3], the
enthalpy of formation for CoFe2O4 is 11.28 eV/f.u. and 14.84 eV/ f.u. for CoCr2O4.
Thus, it is quite expected that when Cr3+ is substituted for Fe3+ in the system,
CoCrxFe2-xO4, more amount of heat will be liberated, which will increase the
temperature of the growing crystal surface, resulting in decrease of the molecular
Chapter 4
4.22
concentration approaching at the crystal surface and hence, hindering the crystal
growth. i.e. reduction in particle size.
The selected area electron diffraction (SAED) patterns for x = 0.0, 0.3, 1.1, 1.5
and 2.0 compositions are also shown in the Figure 4.4.1 (a) – (e). The patterns show
the Debye-Scherrer rings indicating the presence of structurally disordered regions in
the wet chemically synthesized Co-Cr ferrites. The rings are consistent with the cubic
spinel structure with an intense ring patterns form (hkl) planes. No secondary phases
are found. The diffused SAED patterns indicate nano crystalline nature of the
particles [4].
(a) (a)
(a) (a)
Chapter 4
4.24
Figure 4.4.1: TEM and SAED images for CoCrxFe2-xO4 system
(a) CoFe2O4 (x = 0.0) (b) CoCr0.3Fe1.7O4 (x = 0.3) (c) CoCr1.1Fe0.9O4 (x = 1.1)
(d) CoCr1.5Fe0.5O4 (x = 1.5) (e) CoCr2O4 (x = 2.0) compositions.
(d) (d)
(d) (d)
(e) (e)
(e) (e)
(2 2 0)
(3 1 1)
(4 0 0)
(5 1 1)
(4 4 0)
Chapter 4
4.25
Conclusions
(i) Highly agglomerated particles for all the compositions are due to the magnetic
nature of the constituent cations.
(ii) The reduction in particle size with Cr3+ - substitution is mainly due to the more
enthalpy of formation needed for CoCr2O4 as compared to that for CoFe2O4.
(iii) SAED patterns confirm nano crystalline nature of wet- chemically synthesized
ferrite particles.
Chapter 4
4.26
References
1. Kunal B. Modi, Nimish H. Vasoya, Vinay K. Lakhani, Tushar K. Pathak,
‘Spherical to Needle Shaped Particles Transformation Study on
Nanocrystalline Mg–Mn Ferrites’, J. Adv. Micro. Res., 7 (2012) 40 – 43.
2. R. F Strickland-Constable, ‘Kinetics and Mechanism of Crystallization’,
Academic Press, New York (1968).
3. A. Jain, G. Hautier, S. P. Ong, C. J. Moore, C. C. Fischer, K. A. Persson,
G. Ceder, ‘Formation of enthalpies by mixing GGA and GGA+U
calculations’, Phys. Rev. B, 84 (4) (2011) 045115 – 045124.
4. S. Verma, P. A. Joy, ‘Low temperature synthesis of nanocrystalline lithium
ferrite by a modified citrate gel precursor method’, Mater. Res. Bul., 43 (12)
(2008) 3447 – 3456.
Chapter 4
4.27
4.5 X-ray powder diffraction patterns analysis and structural
parameters determination
The polycrystalline samples of CoCrxFe2-xO4 spinel ferrite system were characterized
by X-ray powder diffractometry (XRD) to ascertain the mono-phase structure
formation, to deduce lattice parameter and cation distribution and particle size
verification. Typical XRD patterns of CoCrxFe2-xO4 samples with x = 0.0, 0.7, 1.1,
1.3, 1.7 and 2.0 are shown in Figure 4.5.1. The background noise and the broadness of
the peaks are characteristic of particles with nanometer dimensions since there is not
sufficient number of crystallographic planes to result in sharp diffraction lines. The
XRD patterns also showed that all the samples have the single phase spinel structure.
No extra lines corresponding to any other phase or non-reacted ingredients were
detected. The diffraction patterns could be indexed for a face centered cubic (fcc)
structure [1]. The cell edge parameter for each composition was determined by using
the ‘Powder-X’ software [2]. The concentration dependence of the lattice constant
(aexp) determined from the XRD pattern analysis is presented in Table 4.5.1.
The lattice constant remains more or less constant initially but rapidly decreases for
higher concentrations of Cr3+. Usually in a solid solution of ferrites within the
miscibility range, a linear change in lattice constant with concentration of the
components is observed. The observed change in lattice constant value with Cr3+-
content (x) is attributed to the small difference in the ionic radii of the constituent
cations, Fe3+ (0.640Å) and Cr3+ (0.630Å), and change in the distribution of cations
among the available A- and B-sites of the spinel lattice.
The various physical properties of ferrites are sensitive to the nature, the
valence state and distribution of cation over the tetrahedral (A-) and octahedral (B-)
sites of the spinel lattice. Therefore, the knowledge of cation distribution is essential
to understand the various physical properties of spinel ferrites.
Cation arrangements are not unique in spinel ferrites. Each spinel compound
possesses at least three degree of freedom, which it uses in its search for an
equilibrium structure: oxygen positional parameter (u), lattice constant (a) and cation
inversion parameter. The parameter ‘u’ varies, primarily, in accordance with the
radius ratio between the A – and B – sites cations, rA/rB (or rB/rA). This is to say, the
A – and B – sites bond lengths adjust themselves by variation in ‘u’ until the A- and
Chapter 4
4.28
B- sites volumes “best – fit” the cations. The parameter ‘a’ varies in accordance with
the average of the A – and B- sites cationic radii (i.e. with 0.33 rA + 0.67 rB). The
entire frame work of the unit cell swells or contracts to accommodate the size of the
cations. The cation inversion parameter varies based on a much more complex set of
factors. Some of the principal factors that influence cation inversion include [3]:
(i) temperature (ii) the electrostatic contribution to the lattice energy (iii) cationic radii
(iv) cationic charge and (v) crystal – field effects.
In order to determine the cation distribution, the XRD line intensity calculations
were made using the formula suggested by Buerger [4].
.LPFI m2
hklhkl = (1)
Here, Ihkl is the relative integrated intensity, Fhkl is the structure factor, Pm is the
multiplicity factor and L = (1+cos22θ)/(sin2θ cosθ) is the Lorentz polarization factor.
According to Ohnishi and Teranishi [5], the intensity ratios of planes I220/I440 and
I400/I422 are considered to be sensitive to the cation distribution. There exists distinct
contrast in the atomic scattering factors of Cr3+ or Fe3+ and Co2+ cations present in the
system. This makes the determination of the cation distribution quite reliable. Any
alteration in the distribution of cations causes a significant change in the XRD
intensity ratios. Therefore, in the process of arriving at the final cation distribution,
the site occupancy of all the cations was varied for many combinations and those that
agreed with the experimental intensity ratios are shown in Table 4.5.2. The final
cation distributions were deduced simultaneously by considering the Bragg plane
ratios, the fitting of the magnetization data at 80 K and the ion distribution parameters
of Fe3+among the A – and B – sites of spinel lattice derived from Mossbauer spectral
analysis [6].
F
S
T
an
(T
Figure 4.5.1:
tructural p
The X-ray de
nd Wijn [7]
Table 4.5.1)
: Room te
nanocryst
arameters d
ensity (ρx) o
, ρx = 8M/N
, NA the Av
emperature
talline CoCr
determinati
f the sample
NAa3, where
vogadro’s nu
Chapter 4
4.29
X-ray p
rxFe2-xO4 sp
on
es was deter
e, M is the m
umber (6.02
powder dif
pinel ferrite
rmined using
molecular w
2 x 1023 mol
ffraction p
system.
g relation gi
eight of the
le-1) and ‘a’
patterns fo
ven by Smit
composition
is the lattic
or
th
n,
ce
Chapter 4
4.30
constant. As there are 8 formula unit in the unit cell so 8 is included in the formula.
The ρx is inversely proportional to the lattice constant, which decreases with
increasing Cr3+- concentration; ρx is expected to increase with increasing (x). The
X-ray density (ρx) decreases with Cr3+- ion concentration, because the decrease in
molecular weight overtakes the decrease in volume of the unit cell. Bulk density (ρ)
of the samples was determined by employing the Archimedes principle using xylene
(ρ = 0.87 gcm-3) as the buoyant to obtain fairly good results. It is observed that ρx of
each sample is greater than the corresponding sintered density (ρ). This may be due to
the existence of pores in the samples. Pore fraction (f) was calculated using the
relation f = (1 – ρ/ρx) and percentage porosity was calculated using the relation
P = f * 100%. The variation of porosity (P) with Cr3+ content (x) is a result of the
interplay between ρ and ρx.
The average particle size (D) for the different compositions has been
calculated from the broadening of the respective high intensity (311) peak using the
Debye – Scherrer formula D = Kλ/B.cosθ, Here,λ is the wavelength of the CuKα
radiation (= 1.54059 Å), shape factor, K = 0.9, related both to the crystalline shape
and the way in which B and D are defined. B is the contribution to the XRD peak
width, full width at half maximum (FWHM) due to the small size of crystallites in
radians. The contribution must separate out from the measured line width, BM, which
includes instrumental broadening Bins., which is always present irrespective of the
particle size. For this, one can record X-ray powder diffraction pattern of a well
crystallized, bulk standard material such as silicon powder under identical geometrical
conditions and measure the peak width Bins. Usually, Bins. of a conventional X-ray
powder diffractometer is 0.1° (= 0.001744 radian), the broadening parameter B is
obtained from the relation: B = (BM2 – Bins.2)1/2. Here, the particle size is calculated
considering the B (FWHM) obtained by Gaussian fitting of most intense peak. The
particle size reduces from 72 nm for cobalt ferrite, CoFe2O4 (x = 0.0) to 17 nm for
cobalt chromite, CoCr2O4 (x = 2.0) (Table 4.5.1).
The particle size estimated from TEM analysis is found to be greater than the
particle size estimated from X-ray diffraction pattern analysis by Debye – Scherrer’s
formula. This is because of the fact that X-ray diffraction gives the information of
crystalline region only and the contribution from the amorphous grain surface does
Chapter 4
4.31
not considered. On the other hand, TEM gives the overall picture of the nanoparticles.
By analyzing TEM and XRD, one can have almost complete picture of the particle
size, their distribution and morphology.
An attempt has been made to calculate effective surface area (S) for the
selected ferrite compositions. Assuming spherically shaped particles, the specific
surface area (S, cm2/g) is given by [8]: S = 6000/D.ρ, where, D is the particle diameter
in nm and ρ is the bulk density of the particle is g/cm3. The specific surface area
(Table 4.5.1) of the particle increases as the particle size decreases as expected.
Table 4.5.1: Molecular weight, lattice constant (a), X-ray density (ρx), bulk
density (ρ), pore fraction (f), porosity (P), particle size (D) and
effective surface area (S) for CoCrxFe2-xO4 spinel ferrite system.
Besides using experimentally found value of lattice constant and oxygen
positional parameter (u), it is possible to calculate the value of the mean ionic radius
per molecule of the tetrahedral and octahedral sites, rA and rB, respectively, based on
the cation distribution for each composition using the relation [9]:
Cr3+ –
Content
(x)
Mw x 10-3
(kg/mole)
aexp(Å)
±0.002Å
ρx ρ
(g/cm3) f
P
(%)
D(nm)
±1 nm
S x 104
(cm2/g)
0.0 234.63 8.363 5.329 4.887 0.083 8.3 72 17.05
0.1 234.24 8.363 5.319 4.835 0.091 9.1 − −
0.3 233.48 8.362 5.303 4.762 0.102 10.2 65 19.38
0.7 231.94 8.358 5.276 4.690 0.111 11.1 60 21.32
1.1 230.40 8.352 5.253 4.560 0.132 13.2 39 33.74
1.3 229.63 8.348 5.243 4.383 0.164 16.4 33 41.48
1.5 228.85 8.344 5.232 4.264 0.185 18.5 28 50.25
1.7 228.08 8.342 5.219 4.154 0.204 20.4 21 68.78
1.8 227.69 8.340 5.213 4.123 0.209 20.9 − −
1.9 227.31 8.339 5.205 4.107 0.211 21.1 20 73.05
2.0 226.92 8.337 5.201 3.994 0.232 23.2 17 88.37
Chapter 4
4.32
[ ])r(Fe)(Fef)r(Cr)(Crf)r(Co)(Cofr 33c
33c
22cA
++++++ ⋅+⋅+⋅= (2)
[ ])r(Fe)(Fef)r(Cr)(Crf)r(Co)(Cof21r 33
c33
c22
cB++++++ ⋅+⋅+⋅=
(3)
where, fc and r, are the fractional concentration and ionic radius of respective cation
on the respective site. The ionic radius of Co2+ (0.720 Å), Cr3+ (0.630 Å) and Fe3+
(0.640 Å) ions are taken with reference to coordination 6. Using these formulae, the
mean ionic radius of the tetrahedral (A-) sites (rA) and of the octahedral (B-) sites (rB)
have been calculated and are listed in Table 4.5.2.
Table 4.5.2: The cationic distribution in the samples at different Cr3+
concentrations (x).
Cr3+ -
content
(x)
Cation distribution
A – Site B – Site
0.0 (Fe3+0.9Co2+
0.1)A [Co2+0.9Fe3+
1.1]B O42-
0.1 (Fe3+0.8Co2+
0.2)A [Co2+0.8Cr3+
0.1Fe3+1.1]B O4
2-
0.3 (Fe3+0.6Co2+
0.4)A [Co2+0.6Cr3+
0.3Fe3+1.1]B O4
2-
0.7 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
0.7Fe3+1.0]B O4
2-
1.1 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
1.1Fe3+0.6]B O4
2-
1.3 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
1.3Fe3+0.4]B O4
2-
1.5 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
1.5Fe3+0.2]B O4
2-
1.7 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
1.7]B O42-
1.8 (Co2+1.0)A [Cr3+
1.8Fe3+0.2]B O4
2-
1.9 (Co2+1.0)A [Cr3+
1.9Fe3+0.1]B O4
2-
2.0 (Co2+1.0)A [Cr3+
2.0]B O42-
It can be seen that rB decreases slowly while rA increases rapidly with
increasing Cr3+ - content (x) in the system, which in turn causes the lattice constant
‘a’, to decrease with Cr3+ substitution (x). It can be concluded that the octahedral sites
substitution plays a dominant role in influencing the variation of ‘a’ with
concentration (x).
Chapter 4
4.33
According to Steinfink et al [10,11] the tolerance factor, T, for the spinel
structured materials is defined as:
⎟⎟⎠
⎞⎜⎜⎝
⎛+
+⎟⎟⎠
⎞⎜⎜⎝
⎛++
=OB
O
OB
OA
RrR
21
RrRr
31T (4)
where, notations have their usual meaning. For an ideal spinel structure T value is
close to unity. It is found that for all the synthesized ferrites, value of T is close to
unity suggesting defect free formation of spinel structure and the value increases with
increase in Cr3+ - concentration (x) in the system (Table 4.5.3).
It is known that there is a correlation between the ionic radius and the lattice
constant. The radii of the tetrahedral and octahedral sites in a spinel ferrite can also be
calculated using the formulae given by [12]:
0A Ra41u3r −⎟⎠⎞
⎜⎝⎛ −= (5)
0B Rau85r −⎟
⎠⎞
⎜⎝⎛ −= (6)
where R0 represents the radius of the oxygen ion (taken as 1.32Å) and u is the oxygen
positional parameter. These relationships are further used to calculated the lattice
parameter theoretically ‘ath’ [13].
From equation (6), one can write,
aRr
85u 0B +−= (7)
By substituting the value of ‘u’ from equation (7) in to equation (5) and rearranging
the terms,
( )⎥⎦
⎤⎢⎣
⎡−⎟
⎠
⎞⎜⎝
⎛ +−
+=
41
aRr
853
Rra
0B
0A
( )2a8R8r5a3)R(r 8a
0B
0A
−−−
+=
)R8(r3aRr
8aa3
0B
0A
+−+
=
)Rr 8()R(r38a33 0A0B +=+−
[ ])R(r3)Rr (33
8a 0B0Ath +++= (8)
Chapter 4
4.34
It has been observed that the theoretically calculated values of lattice constant
follow the same trend as that obtained experimentally, although the values are
generally smaller than the experimental ones [13–15]. Theoretical calculations
presume an ideal close packed structure and valence state of the cations and thus
corresponding values of ionic radii have to be taken into consideration.
The oxygen positional parameter or anion parameter (u) for each composition was
calculated using the formulae available in the literature [3].
22R181R
4811
32R
41
u 2
21
22
m3
−
⎟⎠⎞
⎜⎝⎛ −+−
= (9)
22R181R
4811
1211R
21
u 2
21
22
3m4
−
⎟⎠⎞
⎜⎝⎛ −+−
= (10)
41
3aRr
u 0A3m4 ++
= (11)
0.07054
A
B3m4
rr
0.3876u−
⎟⎟⎠
⎞⎜⎜⎝
⎛=
(12)
where, R=(B-O) / (A-O). The bond lengths, B – 0 and A – O are average bond lengths
calculated based on the cation distribution listed in Table 4.5.2, where, 0BrO-B R+=
and 0A RrO-A += ,equation (9) gives ‘u’ assuming centre of symmetry at (1/4, 1/4,
1/4) for which uidea = 0.250 (origin at the B-site), while equations (10) – (12) give ‘u’
assuming centre of symmetry at (3/8, 3/8, 3/8) for which uidea = 0.375 (origin at the A-
site). The values of 3m4u determined from different formulae are in agreement with
each other (Table 4.5.3). To convert origin from A-site to B-site, 1/8uu m33m4 += [3],
relationship has been used. In an ideal fcc structure 0.250.u0.375;u m33m4 ==
Chapter 4
4.35
Table 4.5.3: Ionic radius (r), lattice constant (a), oxygen positional parameter
(u) and tolerance factor (T) for CoCrxFe2-xO4 spinel ferrite system.
Although, most ferrites generally have ‘u’ greater than this ideal value
[14,16], it is slightly larger in the present series (Table 4.5.3), implying that the
oxygen ions are displaced in such a way that in the A-B interaction, the distance
between A and O ions and between B - O ions decreased. This leads to an increase in
the A – A and B – B interactions. As ‘u’ increases from its ideal value, anions move
away from the tetrahedrally coordinated A - site cations along the ‹111› directions,
which increase the volume of each A - site interstice while the octahedral B –sites
become correspondingly smaller. The Fe2+ - ion (0.740 Å) is one of the largest
divalent ions found in spinels, whereas the Al3+ ion is the smallest of the trivalent
spinel cation: thus the r(Fe2+) / r(Cr3+) ratio is large, which favors large u values [3].
Using the experimental values of ‘a’ and anion parameter (u) of each
composition in equations [3, 14, 16, 17] interatomic distances has been calculated.
Cr3+ -
content(x)
rA
(Å)
rB
(Å)
ath
(Å)
m3u
(1/4,1/4,1/4)
3m4u (3/8, 3/8, 3/8)
Eq.(9) Eq.(10) Eq.(11) T
0.0 0.648 0.676 8.352 0.2609 0.3874 0.3858 0.3864 1.044
0.1 0.656 0.672 8.352 0.2604 0.3875 0.3864 0.3870 1.045
0.3 0.672 0.663 8.353 0.2632 0.3842 0.3876 0.3880 1.049
0.7 0.696 0.649 8.353 0.2645 0.3887 0.3892 0.3895 1.054
1.1 0.696 0.646 8.346 0.2643 0.3895 0.3893 0.3896 1.055
1.3 0.696 0.646 8.345 0.2671 0.3918 0.3894 0.3897 1.055
1.5 0.696 0.645 8.342 0.2649 0.3888 0.3895 0.3897 1.056
1.7 0.696 0.644 8.340 0.2646 0.3891 0.3895 0.3898 1.056
1.8 0.720 0.631 8.343 0.2664 0.3911 0.3912 0.3912 1.061
1.9 0.720 0.631 8.341 0.2663 0.3910 0.3912 0.3912 1.062
2.0 0.720 0.630 8.341 0.2671 0.3910 0.3913 0.3912 1.062
Chapter 4
4.36
( ) ⎟⎠⎞
⎜⎝⎛ −=
212u2ad 3m41/2
AE Shared tetrahedral edge
( ) ( )3m41/2BE 2u12ad −= Shared octahedral edge
( )1/2
3m423m4BEu 16
113uu4ad ⎥⎦⎤
⎢⎣⎡ +−= Unshared octahedral edge (13)
⎟⎠⎞
⎜⎝⎛ −=
41u3ad 3m4
AL Tetrahedral bond length
( )1/2
m3423m4BL 64
43u4
11u3ad ⎥⎦⎤
⎢⎣⎡ +−= Octahedral bond length
Table 4.5.4: Edge length and bond length for Co – Fe – Cr – O system.
The calculated values of edge lengths and bond lengths are given in
Table 4.5.4. It is found that with an increase in Cr3+ - concentration, shared octahedral
edge length and octahedral bond length decrease. These may be due to the
replacement of larger Fe3+ -ions by smaller Cr3+ ions on the octahedral site. On the
other hand, shared tetrahedral edge length and tetrahedral bond length increase while
unshared octahedral edge length remains uninfluenced by Cr3+ - substitution.
Cr3+-content (x) dAE (Å) dBE (Å) dBEu (Å) dAL (Å) dBL (Å)
0.0 3.2496 2.6631 2.9639 2.1481 1.9923
0.1 3.2520 2.6607 2.9639 2.1497 1.9931
0.3 3.1735 2.7384 2.9600 2.0978 2.0164
0.7 3.2784 2.6307 2.9644 2.1672 1.9826
1.1 3.2947 2.6098 2.9621 2.1779 1.9740
1.3 3.3477 2.5545 2.9645 2.2130 1.9560
1.5 3.2752 2.6240 2.9595 2.1651 1.9781
1.7 3.2813 2.6161 2.9586 2.1691 1.9757
1.8 3.3280 2.5685 2.9604 2.1999 1.9613
1.9 3.3254 2.5707 2.9603 2.1983 1.9594
2.0 3.3244 2.5700 2.9594 2.1976 1.9588
Chapter 4
4.37
Figure 4.5.2: Configuration of ion pairs in spinel ferrites with favorable
distances and angles for effective magnetic interactions.
The configuration of ion pairs in spinel ferrites with favorable distances and
angles for magnetic interactions are shown in Figure 4.5.2. The interionic distances
between the cations (Me-Me) (b, c, d, e, and f) and between the cation and anion
(Me-O) (p, q, r and s) were calculated using the experimental values of lattice
constant (aexp) and oxygen positional parameters (u3m) (Tables 4.5.1 and 4.5.3) by the
relations [18, 19]:
Me – O Me - Me
⎟⎠⎞
⎜⎝⎛ −= 3mu
21ap
1/22
4ab ⎟⎠⎞
⎜⎝⎛=
1/23m 381uaq ⎟⎠⎞
⎜⎝⎛ −=
1/211
8ac ⎟⎠⎞
⎜⎝⎛=
1/23m 1181uar ⎟⎠⎞
⎜⎝⎛ −=
1/23
4ad ⎟⎠⎞
⎜⎝⎛=
(14)
1/23m 321u
3as ⎟
⎠⎞
⎜⎝⎛ +=
1/23
83ae ⎟
⎠⎞
⎜⎝⎛=
1/264af ⎟⎠⎞
⎜⎝⎛=
The overall strength of the magnetic interactions (A−B, B−B and A−A)
depends upon the bond length and bond angles between the cations and cation - anion.
The strength is directly proportional to bond angle but inversely proportional to bond
length. It is seen from Table 4.5.5 that both interatomic distances between the cations
Chapter 4
4.38
(b, c, d, e and f) decrease with increasing Cr3+- concentration (x). These results are
accordance with decrease in unit cell volume. The bond angles (θ1, θ2, θ3, θ4 and θ5)
(Figure 4.5.2) were calculated by simple trigonometric principle using the interionic
distances with the help of following formulae:
⎥⎦
⎤⎢⎣
⎡ −+= −
2pqcqpcosθ
2221
1
⎥⎦
⎤⎢⎣
⎡ −+= −
2prerpcosθ
2221
2
(15)
⎥⎦
⎤⎢⎣
⎡ −+= −
2psfspcosθ
2221
4
⎥⎦
⎤⎢⎣
⎡ −+= −
2rqdqrcosθ
2221
5
It is found that angles θ1, θ2 and θ5 decrease while θ3 and θ4 increase with
increase in Cr3+- content (x). The observed decrease in θ1, θ2 and θ5 suggest
weakening of the A–B and A–A interactions while increase in θ3 and θ4 indicative of
strengthening of the B−B interaction on Cr3+-substitution in the system.
⎥⎦
⎤⎢⎣
⎡ −= −
2
221
3 2pb2pcosθ
Chapter 4
4.39
Table 4.5.5: Interionic distances (b, c, d, e, f and p, q, r, s) and bond angles (θ) for
Co – Fe – Cr – O system.
(Distances in Å and angles in degrees)
Cr3+-
content
(x)
0.0 0.1 0.3 0.7 1.1 1.3 1.5 1.7 1.8 1.9 2.0
b 2.9563 2.9568 2.9564 2.9550 2.9527 2.9515 2.9500 2.9492 2.9487 2.9485 2.9476
c 3.4671 3.4671 3.4667 3.4650 3.4623 3.4609 3.4592 3.4582 3.4576 3.4575 3.4564
d 3.6213 3.6213 3.6208 3.6191 3.6163 3.6149 3.6131 3.6120 3.6114 3.6112 3.6101
e 5.4319 5.4319 5.4313 5.4287 5.4245 5.4223 5.4196 5.4180 5.4171 5.4168 5.4152
f 5.1212 5.1212 5.1207 5.1182 5.1142 5.1122 5.1096 5.1081 5.1072 5.1070 5.1055
p 1.9995 2.0038 1.9801 1.9683 1.9684 1.9442 1.9617 1.9636 1.9483 1.9490 1.9417
q 1.9662 1.9590 1.9992 2.0170 2.0126 2.0522 2.0194 2.0145 2.0401 2.0386 2.0495
r 3.7687 3.7548 3.8321 3.8683 3.8577 3.9377 3.8709 3.8614 3.9106 3.9076 3.9285
s 3.6696 3.6672 3.6802 3.6847 3.6808 3.6929 3.6804 3.6779 3.6859 3.6853 3.6881
θ1 121.92 122.06 121.19 120.78 120.84 119.97 120.66 120.75 120.18 120.22 119.98
θ2 138.60 139.20 135.87 134.29 134.62 131.56 133.94 134.29 132.30 132.25 131.56
θ3 95.34 95.08 96.58 97.29 97.18 98.76 97.51 97.35 98.35 98.29 98.74
θ4 126.66 126.60 126.93 126.03 127.06 127.37 127.12 127.09 127.29 127.28 127.37
θ5 70.46 70.86 68.68 68.56 67.85 65.80 67.40 67.62 66.30 66.38 65.80
Chapter 4
4.40
Conclusions
(i) We have successfully synthesized single phase (fcc), defect free
nanocrystalline spinel structured ferrite materials of CoCrxFe2-xO4
(x = 0.0 – 2.0) system by the coprecipitation route.
(ii) It is found that Cr3+ - ions have strong preference for the octahedral B– site,
Fe3+ - ions distributed among the A – and B – sites almost equally, while
Co2+ - ions initially have preference for the B – site (x = 0.0 – 0.6) and for
higher concentration of x, (x ≥ 0.7), it preferably occupy the A– site. The
system gradually transfers from inverse spinel to mixed spinel to normal
spinel structure on increasing Cr3+ - concentration.
(iii) The particle size rapidly decreases while all other structural parameter slowly
decreases with increasing Cr3+ - substitution (x) in the system.
(iv) Various structural parameters can be determined from X-ray powder
diffraction pattern analysis and are found useful to explain other physical
properties.
(v) The strength of the B– B interaction increases while A–B interaction decreases
with Cr3+ - substitution for Fe3+ in the system.
Chapter 4
4.41
References 1. B. D. Cullity, ‘Elements of X-ray diffraction’, Addision Wesley, (1978).
2. C. Dong, ‘Powder X: Windows-95-based program for powder X-ray
diffraction data processing’, J. Appl. Cryst., 32 (4) (1999) 838 – 847.
3. K. E. Siokafus, J. M. Wills, N. W. Grimes, ‘Structure of Spinel’,
J. Am. Ceram. Soc., 82 (12) (1999) 3279-3291.
4. M. J. Buerger, ‘Crystal Structure Analysis’, Wiley, (1980).
5. H. Ohnish, T. Teranishi, ‘Crystal distortion in copper ferrite-chromite series’,
J. Phys. Soc. Jpn., 16 (1961) 35 – 43.
6. V. T. Thanki, ‘Study on magnetic properties of oxide materials’, Ph.D. Thesis,
Saurashtra University, Rajkot, (1996).
7. J. Smith, H. P. J. Wijn, ‘Ferrites’, Wiley, (1959).
8. C. G. Whinfrey, D. W. Eckart, A. Tauber, ‘Preparation and X-Ray Diffraction
Data1 for Some Rare Earth Stannates’, J. Am. Chem. Soc., 82 (1960) 2695 –
2699.
9. M. George, A. M. John, S. S. Nair, P. A. Joy, M. R. Anantharaman, ‘Finite
size effects on the structural and magnetic properties of sol–gel synthesized
NiFe2O4 powders’, J. Magn. Magn. Mater. 302 (1) (2006) 190 – 195.
10. K. Kugimiya, H. Steinfink, ‘Influence of crystal radii and electro negativities
on the crystallization of AB2X4 stoichiometries’, J. Inorg. Chem., 7 (9) (1968)
1762 – 1770.
11. R. Sharma, S. Singhal, ‘Structural, magnetic and electrical properties of zinc
doped nickel ferrite and their application in photocatalytic degradation of
methylene blue’, Physica B, 414 (2013) 83 – 90.
12. K. J. Standly, ‘Oxide Magnetic Materials’, Clarandom Press, (1972).
13. S. A. Mazen, M. H. Abdallah, B. A. Sabrah, H. A. M. Hasham, ‘The Effect of
Titanium on Some Physical Properties of CuFe2O4’, Phys. Status. Solidi
A, 134 (1992) 263-271.
Chapter 4
4.42
14. R. K. Sharma, Varkey Sebastain, N. Lakshmi, K. Venugopalan, V. R. Reddy,
Ajay Gupta, ‘Variation of structural and hyperfine parameters in nanoparticles
of Cr-substituted Co-Zn ferrites’, Phys. Rev. B, 75 (2007) 144419 – 144424.
15. H. Bhargava, N. Lakshmi, V. Sebastina, V. R. Reddy, K. Venugopalan, Ajay
Gupta, ‘Investigation of the large magnetic moment in nano-sized
Cu0.25Co0.25Zn0.5Fe2O4’, J. Phys D: Appl. Phys. 42(2009)245003-245010.
16. V. K. Lakhani, T. K. Pathak, N. H. Vasoya, K. B. Modi, ‘Structural
parameters and X-ray Debye temperature determination study on copper-
ferrite-aluminates’, Solid State Sci., 13 (2011) 539 – 547.
17. T. Abbas, Y. Khan, M. Ahmad, S. Anwar, ‘X-ray diffraction study of the
cation distribution in the Mn-Zn-ferrites’, Solid State Commun., 82 (9) (1992)
701-703.
18. J. B. Goodenough, ‘An interpretation of the magnetic properties of the
perovskite-type mixed crystals La1−xSrxCoO3−λ’, J. Phys. Chem. Solids,
6 (1958) 287-297.
19. J. Kanamori, ‘Super exchange interaction and symmetry properties of electron
orbitals’, J. Phys. Chem. Solids. 10 (2-3) (1959) 87-98.
Chapter 4
4.43
4.6 Crystal defects and cation redistribution study on
nanocrystalline cobalt – ferri – chromites by positron
annihilation spectroscopy
Crystalline materials with the characteristic spinel structure, comprising of well
designated tetrahedral (A-) and octahedral (B-) sites, constitute a very interesting class
of condensed matter systems evoking interest even from the very fundamental science
viewpoint [1, 2]. Cobalt ferrite (CoFe2O4), Cobalt chromite (CoCr2O4) and their solid
solutions with a typical crystalline structure AB2O4 are candidate materials in this
class where, A is normally a divalent and B a trivalent ion. These materials have
attracted a large number of chemists, physicists and metallurgists to study their
different aspects, including the structure and properties, using both theoretical
modeling and wide variety of experimental tools [3-5]. Ferrites composed of
nanometer-sized particles elevates this interest to new dimensions as the very large
network of interfaces will then play a decisive role in controlling the atomic transport
and spatial rearrangement of atoms within the structure. So far as the tools for
investigation into such details are concerned, conventional experimental methods such
as X-ray diffraction (XRD) and transmission electron microscopy (TEM) have helped
to obtain substantial information on a macroscopic scale. But, defect-specific probes
such as positron annihilation spectroscopy are needed to pinpoint their role in the
post-synthesis and characterization treatments such materials have to undergo. We
present in this section the results of our investigation carried out on CoFe2O4, both on
the nascent mother sample and samples in which the Fe3+ ions are replaced by Cr+3
ions, i.e. CoCrxFe2-xO4 , x = 0.0 – 2.0. The purpose of the work is double-sided. In this
section the emphasis is given to demonstrate the ability of positron annihilation
techniques to sense such changes. The latter is of importance since such works are
scarcely available in literature so far and secondly it offers a viable investigative
probe for such studies which are highly essential in the current scenario of novel
materials and arising challenges in their understanding.
In the previous sections (4.2 – 4.5) the changes occurring at the different
stages of Cr3+ - concentration (x) have been obtained from more conventional
experimental tools such as XRD, TEM, EDAX etc.
Chapter 4
4.44
According to the existing literature, cobalt ferrite (CoFe2O4) is an inverse
spinel and taken to be collinear ferrimagnet [6], while cobalt chromite, CoCr2O4, is a
normal spinel with a canted ferromagnetic structure and its Curie temperature is 97 K
[7]. Previous studies of magnetic properties and Mossbauer spectroscopy on mixed
cobalt-ferri-chromites,CoCrxFe2-xO4 of coarse-grain composition indicated that
canting of magnetic structure is observed when Co2+ is present at the tetrahedral (A-)
site [8,9]. While magnetization measurements on the same system could be explained
by Neel’s model as far as the series remained inverse spinel, they deviated
significantly when they began to have normal spinel structure [10]. Recently,
structural and magnetic properties of nanocrystalline CoCrxFe2-xO4 (0 ≤ x ≤ 1.0)
system prepared by the sol-gel auto combustion route have been studied by Jadhav et
al [11].
The redistribution of cations when one species is replaced by ions of
neighboring elements in the periodic table has been of tremendous significance in
modifying the properties as well as in giving rise to new phenomena and processes
[6,8,9]. The transformation of a nearly-complete inverse spinel ferrite, CoFe2O4, to a
normal spinel chromite, CoCr2O4, through successive replacement of the Fe3+ ions by
Cr3+ ions has been found to generate drastic changes in the cationic distribution in the
structure, owing to lattice contraction as well as the likely presence of vacancy-type
structural defects. Although substitution effects generally prompt such redistributions,
concomitant lattice contraction or expansion can also influence it and quite often it
will result in the generation of structural defects in the form of unoccupied lattice
sites. The latter are potential sites for investigation by positron annihilation
experiments. Such a defect-sensitive spectroscopic probe will be of immense benefit
as it can pinpoint the origin and evolution of such defects and their dominating role
over the redistribution of ions in the lattice. As is popularly known, the positron
lifetimes and Doppler broadening of the electron-positron annihilation gamma ray
spectrum are directly related to the electron density and momentum distribution in a
material and hence the information carried by the signals of annihilation can unravel
the material properties in the atomic scale [12]. The details regarding the positron
annihilation studies of the powdered samples and the methods of data analysis to
extract the relevant information can be found from [13, 14].
Chapter 4
4.45
4.6 (A) Positron lifetimes in the un-substituted sample, CoFe2O4 (x = 0.0)
The positron lifetime spectra were analyzed using the PALSfit computer program
developed by the Risoe group [15]. The spectra of all the samples were fitted to obtain
variances of fit within satisfactory limits (1.07±0.12). The fits yielded three distinct
lifetimes τ1, τ2 and τ3 in all the cases and their magnitudes, as discussed below, were
characteristic of positron trapping in specific sites within the spinel structure or
positronium formation within the grain boundaries. In the CoFe2O4 (x = 0.0) sample,
the intermediate lifetime τ2 was found as high as 356 ps with relative intensity I2 =
48.2 %. The normal interpretation for observation of such a well-resolved longer
lifetime with appreciable intensity is the presence of vacancy-type crystalline defects
within the material since positrons get trapped in such lower-than-average-electron-
density sites. This is a reasonable assumption since it is nearly impossible to
synthesize ferrites with fully occupied crystalline structure. Besides, those positrons
managing to diffuse out to the vacancies on the nanocrystalline grain interfaces may
also contribute to this component. The reason is that the thermal diffusion lengths of
positrons in oxide materials are typically about 50-60 nm [16, 17]. Hence, a small
fraction of positrons would inevitably diffuse and migrate to the surfaces of the
nanocrystals (which are of sizes about 60-65 nm) before their annihilation. Despite
prolonged heating, the grain dimensions could not be increased to more than the
above limit. On the other hand, the diffusion lengths in the present case could be
shortened due to the trapping of positrons by vacancy clusters if present within the
nanoparticles. The positron lifetime in the perfect crystalline sample (τf, for which no
theoretical value is available) can be calculated using the trapping model equation
[18]: ,τI
τI
τI
τ1
3
3
2
2
1
1
f
++= Substituting the experimental values of the positron lifetimes
and their intensities of the CoFe2O4 sample in the above equation, we obtain τf = 199
ps. The shorter lifetime component τ1 is obviously less than this value in all the cases
due to admixing with the Bloch state residence time of trapped positrons [12]. A small
contribution coming to τ1 from parapositronium atoms of lifetime 125 ps is ignored as
the intensity of this component, one-third that of the orthopositronium intensity I3, is
negligibly small.
Chapter 4
4.46
The annihilation characteristics of positrons diffusing out to the grain surfaces
are also reflected in the variation of the longest lifetime τ3 and its intensity I3. The
magnitude of this lifetime (1.8 – 2.1 ns) is typical of the “pick-off” annihilation of
orthopositronium atoms formed at the interfacial regions of the grains [12]. Although
positronium formation is not significant enough to alter the interpretations in metallic
oxides, it has been found still relevant enough to force a three-component analysis of
the positron lifetime spectra of nanocrystalline materials [19-21], and the intensity I3,
despite being relatively small (0.8 – 1.4 %), indicates the presence of large free
volume regions in the intergranular regions of materials when composed by
nanometer-sized particles or grains.
Figure 4.6.1: The lattice constant (a) and the radii of the tetrahedral (rA) and
octahedral (rB) sites versus Cr3+ - concentration (x).
4.6 (B) Results of Cr3+ substitution
Figures 4.6.2 (a) and (b) describe the changes occurring in the positron annihilation
parameters as a result of Cr3+ substitution for Fe3+ in CoFe2O4. A close look into the
trends of variation helps to identify three distinct stages of defects evolution and/or
structural variations. In the first stage spreading over the concentration x = 0.1 to 0.7,
the two positron lifetimes τ1 and τ2 show remarkable increase in the initial stage and
Chapter 4
4.47
attain saturation. The longer lifetime τ3 and its intensity I3 show characteristic
decrease that will be discussed later. The second stage of variation is marked for x>
0.7 till 1.7 during which the lifetimes decrease and the intensity sharply rises. All
these trends are just reversed once again in the last stage from x = 1.8 to 2.0.
The variation of the different positron annihilation parameters with Cr3+-
substitution is thus highly complex in nature, as the potential trapping centers might
have changed during the different stages of substitution, due to not only the arrival of
a new element but also the relative displacement they may cause in the positioning of
the other ions already present in the crystalline structure. Certain information in this
direction is available from the results of CDBS measurements shown in Figure
4.6.3(a).
Figure 4.6.2: (a): The positron lifetimes τ1 and τ2 and intensity I2 versus Cr3+
concentration (x) (b): The orthopositronium lifetime τ3 and intensity I3 versus
versus Cr3+ concentration (x).
Chapter 4
4.48
The data has been analyzed using the usual quotient spectral method in which
the projected one-dimensional spectra on the ((E1−E2)/2) axis of the counts in the
window ((E1+E2)/2) = 511 ± 1.2 keV are peak-normalized and divided by that of a
pure reference sample (Si single crystals) [14, 22]. The choice of Si to serve as a
reference is not unjustified since it is not a constituent of the material at any stage in
this investigation and the purpose is to magnify the differences in shapes of the
momentum distribution curves for easy understanding and interpretation. In Figure
4.6.3(a)(i),the ratio curves of the samples with the two extreme compositions,
CoFe2O4(x = 0.0) and CoCr2O4 (x = 2.0), are shown together with the identical curves
obtained for the constituent elemental samples. Figure 4.6.3(a) (ii) illustrates the
curves obtained similarly for the Cr3+- substituted samples of a few representative
concentrations. The ratio curves of the samples are found having a characteristic
peaks at pL= 10.3×10-3 m0c (where m0 is the electron mass and c is the velocity of
light). The peaks of the ratio curves of the three constituent metals, i.e., Co, Fe and
Cr, appear at 15.0×10-3 m0c, 12.2×10-3 m0c and 11.3×10-3 m0c respectively but with
decreasing amplitudes. This observation is consistent with the decreasing number of d
-electrons and decreasing radius of the 3d-shell. That the peak of the ratio curve of
either the pure or any of the Cr3+- substituted samples does not coincide with those of
the elemental curves is ample proof to suggest that positrons are not trapped in
oxygen vacancies, a fact even otherwise vindicated by their positive charge that will
repel positrons. On the other hand, trapping take place in the cationic vacancies and
the peak at pL = 10.3×10-3 m0c common to all the samples and irrespective of the Cr3+
- concentration (x) indicate the encirclement of the defects by oxygen ions. In several
of our recent studies on nanocrystalline oxide semiconductors, we have similarly
obtained the peak due to annihilation with oxygen electrons at pL = 10.3×10-3 m0c
[23-25].
The identical elemental environment around the positron trapping sites at all
concentrations of Cr3+ substitution is further verified from the S versus W plot shown
in Figure 4.6.3 (b) that is normally used to identify the changes in the predominant
type of positron trapping defects at different stages of variation of the experimental
parameters. The S and W parameters have been derived from the CDB spectra as the
counts falling under segments respectively from 0 to 3.75×10-3 m0c and from
Chapter 4
4.49
7.5×10-3 m0c to 12.25×10-3 m0c normalized by the total counts accumulated under 0 to
37.5×10-3 m0c. The S - W plot is linear and all the points lie essentially on a straight
line. This indicates that positrons essentially encounter similar elemental
environments irrespective of the cationic redistribution. This is further credence to the
argument that the defects which trap positrons are surrounded by oxygen ions and
therefore the traps are none other than the cationic vacancies. But there are variations
in the intensity of annihilation with the oxygen electrons, as indicated by the
individual variations of the S and W parameters with Cr3+- concentration (x), shown
in Figures 4.6.4(a) and (b). (For the sake of clarity, the curves of not all the samples
are shown in Figure 4.6.3(a) (i) or (ii) but the peak coordinates of all the curves are
shown in Figure 4.6.3 (b). From Figures 4.6.4(a) and (b) also, we can distinguish from
one another basically three regions, the demarcation being identical to that mentioned
in the case of the positron lifetime results. The first two regions (x = 0.0 – 0.7 and
x = 0.7 – 1.7) are characterized by a fall and rise of the peaks of the curves and the last
stage is marked by again a fall. It can be argued that, although the annihilation
environment of positrons essentially remain identical, they are trapped at different
stages of Cr3+ substitution by defects situated at different sites in the lattice structure.
These points are further discussed in detail afterwards.
The insensitivity of the CDB spectra to the oxygen vacancies can be explained
on the basis of the results of positron lifetime measurements as well. The difference
between the lifetime characteristic of defects (i.e., τ2) and the bulk lifetime τf is
normally considered as an indication of the size of the defect. The enhancement in
positron lifetime due to trapping in monovacancies is ~ 40-80 ps in typical metals and
alloys [26]. Assuming that τ2 = 356 ps is an upper limit of the positron lifetime in
vacancy clusters in the un-substituted sample, τ2 – τf = 356 – 199 = 157 ps will
correspond to defects much larger than monovacancies. Theoretical estimations in Fe,
which is normally bcc in structure but a constituent of the present samples, have
shown the enhancement of positron lifetime in a neutral vacancy cluster composed of
4-5 neighboring monovacancies as 152 ps [27]. Considering these facts, the positron
trapping site in the undoped alloy can be conceived to be a vacancy cluster composed
of the monovacancy created by the absence of a doubly ionized cation and four of its
coordinated oxygen ions.
Chapter 4
4.50
Figure 4.6.3: (a) The ratio curves generated from the coincidence Doppler
broadening spectra of the different samples - (i) elements Co, Fe and Cr besides
CoCrxFe2-xO4 of x = 0.0 and 2.0; (ii) CoCrxFe2-xO4 of x = 0.0, 0.3, 0.7, 1.7 and 1.9.
All the spectra had been peak-normalized and then divided by that of a pure
reference Si sample in order to generate the ratio curves. (b) The S – W plot of
the Cr3+- substituted samples.
Based on X-ray diffraction, magnetization and Mossbauer results, Mohan et al
[10] have shown that the CoFe2O4 (x = 0.0) is a nearly-complete inverse spinel and
the ionic distribution in it is of the form (Fe3+0.9Co2+
0.1)A [Co2+0.9Fe3+
1.1]B O42-. The
absence of a Co2+ ion with four oxygen neighbor ions will give rise to a neutral penta-
vacancy cluster in which positrons can be trapped and annihilated. The other
possibility of the absence of a trivalent cation with four neighboring oxygen ions
cannot be ruled out as it would have enhanced positron trapping due to surplus
negative charge and hence it is necessary to point out whether the said vacancy cluster
is centered at the A-site or at the B-site. This can be answered by looking at the
effects of Cr3+ substitution on the cationic redistribution. A schematic diagram
Chapter 4
4.51
showing the two neighboring octants of a normal spinel structure is shown in Figure
4.6.5. At the very onset of substitution, a drastic drop in the intensity of the peak in
the CDB spectra (represented by the W parameter) is observed (Figures 4.6.3(a)(ii)
and 4.6.4(b)) and it indicates the diminishing positron annihilation probability with
oxygen electrons. The ionic distributions obtained from the X-ray diffraction peak
intensity analysis for samples with the different concentrations of the Cr3+ ions are
given in Table 4.6.1. Thus, for example, the distribution is (Fe3+0.8Co2+
0.2)A
[Co2+0.8Cr3+
0.1Fe3+1.1]B O4
2- for x = 0.1. This implies that the substituted Cr3+ ions
initially replace equal number of Fe3+ ions from the B-sites but simultaneously equal
number of Fe3+ ions from the A-sites move over to the B-sites in exchange of Co2+
ions from the B-sites to the A-sites. In effect, an inversion of the spinel structure is
prompted as a result of the substitution process. Hence, as shown in Table 4.6.1, the
number of Fe3+ ions at the A-sites decrease whereas that at the B-sites remains
unaltered till x = 0.7 compositions. Since, CDB spectra indicate diminishing
annihilation with oxygen electrons and the positron lifetime τ2 increase from 356 ps to
374 ps, it is reasonable to argue that the defects in the sample with x = 0.1 is larger in
size and increasingly deficient in oxygen ions than those in the un-substituted(x = 0.0)
sample. In other words, the defects were centered at the A-sites in the un-substituted
sample and at the B-sites in the substituted samples. We attribute the second positron
lifetime component τ2 to such large vacancy clusters.
As already stated, the substitution or doping resulted in sharp rises in the two
lifetimes, τ1 and τ2. The intensity I2 however did not show any change. It is therefore a
local effect in which the vacancy cluster has undergone an increase in size. From
EDAX studies (section 4.2), we have estimated the actual concentration of the Cr3+
ions effectively substituted in the crystallites. It has been found that the B-sites
suffered from non-stoichiometric deficiencies of Cr3+ ions and hence the Co2+ ions
transferred to the A-sites is also less in number than that predicted by the
formula(Fe3+0.9-xCo2+
0.1+x)A [Co2+0.9-xCr3+
xFe3+1.1]BO4
2-. The result is that the vacancies
so created will add to the existing vacancy clusters, resulting in further increase in
their size and thereby enhancing the positron lifetimes. However, the deficiency
decreases on subsequent doping and therefore the lifetime τ2 and intensity I2 remain
rather unchanged in the range of concentration from 0.1 to 0.7.
Chapter 4
4.52
Table 4.6.1: The cationic distribution in the samples at different Cr3+-
concentration (x).
Figure 4.6.4: The S and W parameters versus Cr3+ - concentration (x).
Cr3+ -
content
(x)
Cation distribution
A – Site B – Site
0.0 (Fe3+0.9Co2+
0.1)A [Co2+0.9Fe3+
1.1]B O42-
0.1 (Fe3+0.8Co2+
0.2)A [Co2+0.8Cr3+
0.1Fe3+1.1]B O4
2-
0.3 (Fe3+0.6Co2+
0.4)A [Co2+0.6Cr3+
0.3Fe3+1.1]B O4
2-
0.7 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
0.7Fe3+1.0]B O4
2-
1.1 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
1.1Fe3+0.6]B O4
2-
1.3 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
1.3Fe3+0.4]B O4
2-
1.5 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
1.5Fe3+0.2]B O4
2-
1.7 (Fe3+0.3Co2+
0.7)A [Co2+0.3Cr3+
1.7]B O42-
1.8 (Co2+1.0)A [Cr3+
1.8Fe3+0.2]B O4
2-
1.9 (Co2+1.0)A [Cr3+
1.9Fe3+0.1]B O4
2-
2.0 (Co2+1.0)A [Cr3+
2.0]B O42-
F
ch
in
C
in
st
ap
co
in
ar
C
(F
io
ex
p
si
rB
ta
[1
ar
th
tr
Figure 4.6.5:
On th
hange despi
nversion pro
Cr3+ ions occ
ndicate furth
tarts decreas
ppears the
oncentration
ncreases (Fig
re smaller
CoCrxFe2-xO4
Figure 4.6.1
onic radius
xperimentall
arameter (u)
ites, rA and
B = (⅝ - u)a
aken as = 0.3
1,2]. The site
re also show
he vacancies
rapped in red
: Schematic
normal sp
The smal
tetrahedr
he other han
ite the subs
ocess in whic
cupy the B-
her inversion
sing (Table
sharpest a
n, indicating
gure 4.6.2 (a
in size can
4 samples st
). The contr
of Cr3+ (0
ly found va
) [1], it is po
rB respectiv
– R0, Here,
379 conside
e radii for th
wn in Figure
s at the octa
ducing num
c represent
pinel struct
ll solid and
al and octah
nd, the conc
titution by
ch the Co2+
-sites. The
n and hence
4.6.1). Whe
and the po
a reduction
a)). The fact
n be unders
teeply reduc
raction of th
.630 Å) co
alues of the
ossible to ca
vely, using t
R0 is the rad
ring that Co
he different c
e 4.6.1. Incre
ahedral sites
mber in the C
Chapter 4
4.53
tation of th
ture. The la
d open cir
hedral sites
centration o
Cr3+ ions ti
ions migrate
Cr3+ substit
the effectiv
ereas at x =
ositron lifet
n in size of t
that positron
stood as fo
es in sampl
he lattice can
ompared to
lattice con
alculate the r
the relations
dius of the o
oCrxFe2-xO4is
composition
easing conce
and, owing
Cr3+-vacancy
he two nei
arge circles
rcles repres
respectivel
of Fe3+ ions
ill x = 0.7
e to the A-si
tution (x) ab
ve number o
0.7, the pe
times start
the vacancy
ns are now a
ollows. The
es with incr
n be attribut
that of Fe3
nstant (a) an
radii of the t
s [1], rA =
oxygen ion (
s fully inver
ns estimated
entration of
to the posit
y complexes
ighboring o
represent
sent the ca
ly.
at the B-s
due to the
ites [10]. Th
bove this va
of Fe3+ ions
eak in the C
decreasing
clusters. Th
annihilating
lattice con
reased Cr3+
ted to the sli3+ (0.640 Å
nd the oxyg
tetrahedral a
(3)1/2(u - ¼
(taken as 1.3
rse at x = 0.0
from the abo
Cr3+ will re
tive charge,
so formed.
octants of
oxygen ion
ations at th
sites does no
simultaneou
his means, th
alue does no
at the B-site
CDB spectrum
g above th
he intensity
at sites whic
nstant of th
concentratio
ightly smalle
Å). Using th
gen position
and octahedr
¼)a – R0 an
32 Å) and u
0 compositio
ove equation
esult in fillin
positrons ar
On the othe
a
ns.
he
ot
us
he
ot
es
m
his
I2
ch
he
on
er
he
al
al
nd
is
on
ns
ng
re
er
Chapter 4
4.54
hand, while the octahedral sites were large enough to accommodate the Co2+ ions, the
radii of the tetrahedral sites are magnitude-wise smaller than its ionic radius (0.740 Å)
and hence it is likely that a fraction of the tetrahedral sites are unoccupied during the
inversion of the spinel structure at concentrations x< 0.7. As a result, positrons now
that they are no more trapped at the octahedral vacancies will move over to the
vacancies at the tetrahedral sites and get trapped there. The fast decreasing positron
lifetimes support this argument since the tetrahedral vacancy clusters are smaller than
the octahedral ones. The availability of additional trapping sites expectedly increases
the intensity I2 as well. Considering that positrons are now getting trapped in the
vacancy clusters present at the tetrahedral sites, the lattice contraction would directly
influence their lifetime and the observations in the range mentioned above are in
accordance with the same. A careful study of the ionic distribution shown in
Table 4.6.1 makes us realize that from x = 0.7 onwards till x = 1.7, the occupancies of
Fe3+ and Co2+ at the A-sites remain unchanged whereas the Cr3+ ions directly replace
the Fe3+ ions at the B-sites. At x = 1.7, all the Fe3+ ions at the B-sites are replaced by
Cr3+ ions (Table 4.6.1).
The last stage in the variation of the positron annihilation parameters versus
the Cr3+ concentration (x) is observed between x = 1.8 and 2.0. During x = 0.7 to 1.7,
the cation distribution at the A-sites remained unaltered as Fe3+0.3Co2+
0.7 while Cr3+
ions monotonically replaced the Fe3+ ions at the B-sites with the Co2+ concentration at
the B-sites remaining unaltered as 0.3. As the lattice contraction continues, the
transformation of the spinel structure from the inverse to the normal configuration that
had started during x = 0.1 - 0.7 and discontinued during x = 0.7 - 1.7 gets completed.
From octahedral site stabilization energy considerations, it is known that cobalt-
chromite (CoCr2O4) is a normal spinel [10]. In earlier positron annihilation studies of
nanocrystalline ZnFe2O4 [19] and NiFe2O4 [20,28], the positron lifetimes had been
observed to decrease when a normal spinel ferrite transforms to an inverse spinel and
conversely they increase when the transformation is just the opposite. These
observations had been verified through Mossbauer spectroscopic studies too [20,28].
Since, the two positron lifetimes, τ1 and τ2, drastically increase during x = 1.8 and 2.0
(Figure 4.6.2 (a)), this stage is attributed to the total transformation of the partly
inverse CoCrxFe2-xO4 to the fully normal CoCr2O4. Note further that, unlike during
Chapter 4
4.55
x = 0.1 – 0.7 when the intensity I2 did not show any change, it decreases in the final
stage of inversion indicating the full occupancy of the A-sites by Co2+ ions. The fact
remains that spinel structures normally suffer from non-stoichiometric disorders and
therefore vacancy clusters are inherently in-built in the structure. The large value of τ2
with still an appreciable intensity I2 supports this argument.
As has been already pointed out, the longest lifetime τ3 and its intensity I3 are
due to the nanocrystalline dimensions of the samples and they result from positronium
atoms annihilating at the intergranular region. Hence they need not necessarily reflect
the effects of any change in the vacancy cluster dynamics within the grains. Yet, τ3
shows a sudden decrease during the initial stage x = 0.1 to 0.7 and then remain
constant (Figure 4.6.2(b)). The intensity I3 gradually falls during this stage but shows
a characteristic rise during the second stage x = 0.7 to 1.7 and then remain constant
(Figure 4.6.2(b)). The initial fall can be attributed to small traces of Cr3+ ions,
unsuccessful in being incorporated into the spinel structure and hence left to remain in
trace amounts within the intergranular region. EDAX analysis also indicated
frustration even within the lattice due to the failure in complete substitution of Fe3+ by
the Cr3+ ions in the system. In the latter stage (i.e., x > 0.7), the lattice contraction has
expectedly resulted in a decrease by 0.3% in the grain size and thereby the number of
positrons reaching out on the grain surfaces has slightly increased.
Although it is known that the magnetic properties of the samples undergo
rapid and interesting changes during the Cr3+ - substitution, correlating such changes
to the behavior of positron annihilation parameters is never straightforward and is not
attempted here. The structural properties and their changes, as depicted by the
positron annihilation parameters and their variations, may influence the magnetic
properties, which need to be investigated by appropriate experimental methods.
Chapter 4
4.56
Conclusions
In understanding the effects of Cr3+-substitution in place of Fe3+ in CoFe2O4 studied
by positron annihilation spectroscopy, we have offered the physical interpretation of
results in terms of three distinct stages of defect evolution and interaction. First, the
un-substituted ferrite (CoFe2O4, x = 0.0) itself was found to contain large vacancy
clusters. These clusters are identified as being present at the A-sites with the divalent
Co2+ ion and four of its coordinated oxygen ions making way for such very strong
trapping centers for positrons. At the onset of Cr3+- substitution (x), the positron
lifetimes increased due to the transfer of positron trapping into defects to the B-sites.
In the second stage from x = 0.7 to x = 1.7, a concomitant lattice contraction
influenced the positron annihilation characteristics. This contraction is attributed to
the slightly smaller ionic radius of Cr3+ than that of Fe3+. There is also a change in the
positron trapping sites from the vacancy clusters at the B-sites back to those at the A-
sites. The last stage is marked by a full inversion of the structure to that of a normal
spinel chromite and the positron annihilation parameters depicted this stage with a
characteristic reversal of the trend of variation with the Cr3+-concentration.
Finally, we conclude that positron lifetime measurements complemented by
results from coincidence Doppler broadening spectroscopy can be a viable alternative
experimental tool to monitor the generation and evolution of structural disorders in
AB2O4 (where A and B are divalent and trivalent metals respectively) systems during
physical treatments like doping and grain size reduction. Positron annihilation
parameters are seen to sense, directly or indirectly, physical phenomena of different
kinds and implications like the redistribution of cations, lattice contraction or
expansion and structural transformations in certain cases [19-21].
Chapter 4
4.57
References
1. J. Smit, H. P. J. Wijn, ‘Ferrites—Physical Properties of Ferromagnetic
Oxides in Relation to Their Technical Applications’, N.V. Philips
Gloeilampenfabrieken, Eindhoven, The Netherlands, (1959).
2. F. Scordari, ‘Fundamentals of Crystallography’, edited by C. Giacovazzo,
Oxford University Press, New York, USA, (1992).
3. W. B. Cross, L. Affleck, M. V. Kuznetsov, I. P. Parkin, ‘Self propagating
high-temperature synthesis of ferrites MFe2O4 (M =Mg, Ba, Co, Ni, Cu, Zn);
reactions in an external magnetic field’, J. Mater. Chem., 9 (10) (1999)
2545 – 2552.
4. K. Tomiyasu, J. Fukunaga, H. Suzuki, ‘Magnetic short range order and
reentrant-spin-glass-like behavior in CoCr2O4and MnCr2O4by means of
neutron scattering and magnetization measurements’, Phys. Rev. B, 70 (21)
(2004) 214434 – 214445.
5. V. T. Thanki, N. N. Jani, U. V. Chhaya, H. H. Joshi, R. G. Kulkarni,
‘Magnetic properties of CoFe2− Cr O4 synthesized by co-precipitation
method’, Asian Jour. Phys., 6 (1-2) (1997) 222 – 226.
6. G. A. Sawatzky, F. van der Woude, A. H.Morrish, ‘Cation distributions in
octahedral and tetrahedral sites of the ferromagnetic spinel CoFe2O4’
J. Appl. Phys., 39, (2) (1968) 1204–1205.
7. G. Lawes, B. Melot, K. Page et al., ‘Dielectric anomalies and spiral magnetic
order in CoCr2O4’, Phys. Rev. B, 74 (2) (2006) 024413 – 024419.
8. N. Menyuk, K. Dwight, A. Wold, ‘Ferrimagnetic spiral configurations in
cobalt chromite’, Journal de Physique, 25 (1964) 528 –5 36.
9. A. Hauet, J. Teillet, B. Hannoyer, M. Lenglet, ‘Mossbauer study of Co and Ni
ferrichromites’, Phys. Stat. Solidi (A), 103 (1) (1987) 257 – 261.
10. H. Mohan, I. A. Shaikh, R. G. Kulkarni, ‘Magnetic properties of the mixed
spinel CoFe2− CrxO4’, Phys. B, 217 (3-4) (1996) 292 – 298.
11. B. G. Toksha, S. E. Shrisath, M. L. Mane, S. M. Patange, S. S. Jadhav,
K. M. Jadhav, ‘Autocombustion high-temperature synthesis, structural, and
magnetic properties of CoCr Fe2− O4 (0 ≤ ≤ 1.0)’, The Jour. Phys. Chem. C,
115 (43) (2011) 20905 – 20912.
Chapter 4
4.58
12. R. W. Siegel, ‘Positron annihilation spectroscopy’, Annual Review of
Materials Science, 10 (1980) 393 – 425.
13. S. Biswas, S. Kar, S. Chaudhuri, P. M. G. Nambissan, ‘Mn2+-induced
substitutional structural changes in ZnS nanoparticles as observed from
positron annihilation studies’, J. Phys.: Cond. Matter, 20 (23) (2008) 235226
– 1 – 10.
14. P. Asoka-Kumar, M. Alatalo, V. J. Ghosh, A. C. Kruseman, B. Nielsen,
K. G. Lynn, ‘Increased elemental specificity of positron annihilation spectra’,
Phys. Rev. Lett., 77 (10) (1996) 2097 – 2100.
15. J. V. Olsen, P. Kirkegaard, N. J. Pedersen, M. Eldrup, ‘PALSfit: a new
program for the evaluation of positron lifetime spectra’ Phys. Status Solidi
(C), 4, (10) (2007) 4004 – 4006.
16. T. Koida, S. F. Chichibu, A. Uedono et al., ‘Correlation between the
photoluminescence lifetime and defect density in bulk and epitaxial ZnO’,
Appl. Phys. Lett., 82 (4) (2003) 532 – 534.
17. A. Zubiaga, F. Tuomisto, F. Plazaola et al., ‘Zinc vacancies in the
heteroepitaxy of ZnO on sapphire: influence of the substrate orientation and
layer thickness’, Appl. Phys. Lett., 86 (4) (2005) 042103 – 042103 – 3.
18. P. Hautojarvi, C. Corbel, ‘For a detailed discussion ondifferent cases of
positron trapping in solids’, in Positron Spectroscopy of Solids, 491–532, IOS
Press, Amsterdam, The Netherlands, 1995.
19. P. M. G. Nambissan, C. Upadhyay, H. C. Verma, ‘Positron life time
spectroscopic studies of nanocrystalline ZnFe2O4’, J. Appl. Phys., 93 (10)
(2003) 6320 – 6326.
20. S. Chakraverty, S. Mitra, K. Mandal, P. M. G. Nambissan, S. Chattopadhyay,
‘Positron annihilation studies of some anomalous features of NiFe2O4
nanocrystals grown in SiO2’, Phys. Rev. B, 71 (2005) 024115 – 024121.
21. S. Chakrabarti, S. Chaudhuri, P. M. G. Nambissan, ‘Positron annihilation
lifetime changes across the structural phase transition in nanocrystalline
Fe2O3’, Phys. Rev. B, 71 (6) (2005) 064105 – 064110.
Chapter 4
4.59
22. Y. Nagai, T. Nonaka, M. Hasegawa et al.’ Direct evidence of positron trapping
at polar groups in a polymer-blend system’, Phys. Rev. B, 60 (17) (1999)
11863 – 11866.
23. T. Ghoshal, S. Biswas, S. Kar, S. Chaudhuri, P. M. G. Nambissan, ‘Positron
annihilation spectroscopic studies of solvothermally synthesized ZnO
nano bipyramids and nanoparticles’, J. Chem. Phys., 128 (7) (2008) Article ID
074702, Virtual Journal of Nanoscale Science and Technology, 17 (8) 2008.
24. T. Ghoshal, S. Kar, S. Biswas, S. K. De, P.M. G. Nambissan, ‘Vacancy-type
defects and their evolution under Mn substitution in single crystalline ZnO
nano cones studied by positron annihilation’, J. Phys. Chem. C, 113 (9) (2009)
3419–3425.
25. B. Roy, B. Karmakar, P. M. G. Nambissan, M. Pal, ‘Mn substitution effects
and associated defects in ZnO nano particles studied by positron annihilation’,
Nano, 6 (2) (2011) 173 – 183.
26. I. K. MacKenzie, ‘Positron Solid State Physics’, edited by W. Brandt and
A. Dupasquier, North Holland, Amsterdam, The Netherlands, (1983).
27. M. J. Puska, R. M. Nieminen, ‘Defect spectroscopy with positrons: a general
calculational method’, J. Phys. F, 13 (2) (1983) 333 – 346.
28. S. Mitra, K. Mandal, S. Sinha, P. M. G. Nambissan, S. Kumar,
‘Size and temperature dependent cationic redistribution in NiFe2O4 (SiO2)
nanocomposites: positron annihilation and Mossbauer studies’, J. Phys. D, 39
(19) (2006) 4228 – 4235.
Chapter 4
4.60
4.7 Photodegradation of 2, 4 – Dichlorophenoxyacetic Acid by Cr3+
substituted CoFe2O4 nanoparticulates During the last few decades, the use of pesticides and herbicides in agriculture
becomes worldwide. These herbicides and pesticides are now abundantly found in
water and food. Among all such agrochemicals, the herbicide,
2, 4–dichlorophenoxyacetic acid (2, 4-D) has been widely applied to control broad –
leaved weeds. 2, 4–dichlorophenoxyacetic acid, 2, 4−D, is a type of phenoxy acid
herbicide. The salts and esters of 2, 4–D are efficient, highly selective herbicides and
plant growth regulators [1]. This herbicide was registered for the first time in 1947
and till today it is one of the most used herbicide in the world [2]. It is the second
pesticide more used in Brazil and has the advantage of being non – volatile [3]. In
1982, the world health organization (WHO) considered 2, 4-D as moderately toxic
(class II) and recommended a maximum concentration of 0.1 part per million (ppm) in
drinking water. However, it may enter water bodies after usage in farmland [4], or for
improper disposal [5], resulting in its broad residues in environment [6,7]. The
herbicide 2, 4−D is also known to persist in the solid and contaminate surface and
ground water. For the health of not only human beings but also for animals, exposure
to this chemical has been proven to be harmful [8–10]. The intentional removal of this
chemical from water is necessary because the degradation of 2, 4–D is very slow in
water, with a half life of about 6 days to over 170 days in different situations [11–13].
Hence, the search and development of an effective process of degradation for such
herbicides has become a necessary task. Among the various removal methods
employed e.g. adsorption [14,15], biodegradation [16], photocatalytic degradation
[17] etc, photocatalytic degradation found most suitable [18]. This is due to the fact
that this technique is capable to distract entire chemical structure of 2, 4-D, further it
is cheap, simple in operating conditions and techniques. The molecular structure and
chemical properties of 2, 4-D have been summarized in Table 4.7.1.
Over the past few years’ studies on oxidic solid solutions as catalysts have
been steadily developed and today for commercial applications many industrial
establishments have shown interest in such compounds. Out of various models
explaining heterogeneous catalysis one which propose a relationship between
el
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Chapter 4
4.61
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as
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7,
Chapter 4
4.64
Figure 4.7.2: UV-visible spectra of 2, 4-D degradation in the presence of
nanocrystalline CoCrxFe2-xO4 photocatalysts.
Chapter 4
4.65
Figure 4.7.3 shows the percentage degradation of 2, 4–D herbicide on the
nanoparticles of CoCrxFe2-xO4 spinel ferrite system with different Cr3+ - content (x)
under ultraviolet light irradiation at different time interval. Blank experiments indicate
that the direct photolysis of 2, 4-D is negligible when illuminated with ultraviolet light
in the absence of ferrite catalysts. The adsorption-desorption equilibrium of 2, 4-D
herbicide and CoCrxFe2-xO4 were used as starting solutions (t = 0 min.). The variation
of percentage degradation as a function of Cr3+ - concentration (x) in the system for
different irradiation time is not systematic. In general percentage degradation of 2, 4-
D herbicide enhances with ultraviolet irradiation time. If we concentrate on
percentage degradation of 2, 4-D as a function of Cr3+ - content (x) for irradiation time
of 60 minutes duration, it can be seen that the variation can be divided into three
regions (Figure 4.7.4). During the initial stage, x = 0.0 – 0.7, percentage degradation
shows a sudden decrease from 36.8 % to 19.9 %, but shows characteristic rise during
the second stage, x = 0.7 – 1.7 (19.9% to 37.2%), and then gradually falls during the
last stage, x = 1.7 – 2.0 (37.2% to 21.2%).
Figure 4.7.3: Cr3+ - concentration (x) dependence of 2, 4-D photocatalytic
degradation with ultraviolet light irradiation time.
Chapter 4
4.66
The observed change in percentage degradation as a function of
Cr3+- concentration (x) may be explain by considering various structural and
microstructural parameters that affect photocatalytic activity of ferrite nanoparticles.
The governing factors are: (i) particle size, shape of particles, effective surface area
and surface to volume ratio (ii) optical energy band gap (iii) intensity of incident
radiation (iv) electronic configuration of transition metal ions (v) enthalpy of
formation (vi) crystal structure, degree of crystallinity, porosity etc. (vii) pH of the
solution [20] (viii) solvents micellar environments and interfering substances
(ix) other parameters such as glass made cuvetti as a reaction vessel, absence of
oxygen in the reaction medium, use of a UV light of same intensity but as a single
source, solar light as a substitution of UV light, the irradiation done at a stretch and
step by step etc [20].
The understanding of the role played by each of these parameters is rather
difficult and required more detailed work on each factor. Further, when the range of
the compositions under study is very wide, as in the present case, it is quite expected
that at different stages different factors play important or governing role. We have
attempted to explain the variation of percentage degradation of 2, 4–D as a function of
Cr3+ - concentration (x) in the system, CoCrxFe2-xO4, in best possible manner.
According to literature, the direct optical band gap for epitaxial thin film of
CoFe2O4 (x = 0.0) is 2.7 eV [21] on the other hand for CoCr2O4 (x = 2.0) thin film
band gap is reported to 3.1 eV [22]. Because of the higher band gap, the number of
electrons reaching the conduction band is relatively low, consequently, number of
holes in the valence band decrease with increase in Cr3+ - concentration (x) in the
system. Both these electrons and holes interact with surface bound H2O or OH⎯ to
produce ●OH radicals. According to Viswanath et al [23] these radicals are main
active species in the photocatalytic degradation process. Earlier, it has been reported
that some of the ternary semiconductors, InAsxP1-x and nanocomposites of Ni – Zn
ferrites with copolymer matrix of aniline and formaldehyde [24], disclosed that band
gap value varies inversely with change in the lattice constants value, as function of
concentration (x) in the system. Thus, the increase in optical band gap value from 2.7
eV for CoFe2O4to 3.1 eV for CoCr2O4 is consistent with the decrease in lattice
constant value with increasing Cr3+-concentration (x) in the system (Table 4.5.1).
Chapter 4
4.67
Based on the above facts, now it is possible to explain variation of percentage
degradation of 2, 4–D herbicide as a function of Cr3+ - concentration (x) for the
nanocrystalline spinel ferrite system, CoCrxFe2-xO4.
Figure 4.7.4: Percentage degradation of 2, 4-D as a function of Cr3+ - content (x)
in the system, CoCrxFe2-xO4 at ultraviolet light illumination time of
60 minutes.
The numbers of electrons in d – orbit of transition metal ions play an
important role in determining the catalytic behaviour. It is known that the cations with
a completely filled outermost orbit are more stable as compared to cations with a half
filled outer most orbit (e.g. Zn2+, Al3+, Fe3+, Mn2+). On the other hand, transition
metal ions with partially filled d – orbit (e.g. Cr3+, Ni2+ and Co2+) are more reactive.
In the spinel ferrite system under study, CoCrxFe2-xO4, highly magnetic Fe3+ (5 μB)
ions having a half filled (3d5) outer most orbit is replaced by less magnetic Cr3+ (3 μB)
ions with a partially filled outermost orbit (3d3), which actively contribute to the
reaction process.
As discussed, reduction in grain size results in increase in the effective surface
area and surface to volume ratio. These lead to higher catalytic activity as compared
with larger crystals of the same mass present on the active surface. In general, the
surface area is related to the mass and heat transfer between the particle and their
Chapter 4
4.68
surrounding (i.e. enthalpy of formation). Particles that are too small will not catalyze a
reaction (not enough electrons). In addition to size of particle, the shape of nano
particles can also provide a sensitive knob for tuning its catalytic activity and
selectivity.
On the other hand, higher porosity provides a larger amount of surface sites
for organic pollutant and the interface for reaction of the contaminant molecules and
oxygen species occur more easily and rapidly. In the case of nanocrystalline
photocatalysts high porosity is more favorable, because the organic contaminant can
penetrate or get absorbed on the catalyst structure more easily thereby providing a
larger reaction surface for catalytic activity. This leads to conclude that the
appropriate choice of substitution results in particle size reduction that in turn increase
porosity, which provides higher adsorption centers that lead to the enhancement of the
photocatalytic activity.
Spinel ferrite materials are shown to be effective photocatalysts by utilizing
light energy to create electron (e⎯)/hole (h+) pairs on the photocatalytic surface [25].
These e⎯/h+ pairs can be utilized for oxidation and reduction processes, which can
further involve in the formation of reactive oxygen species, such as O2⎯ and ●OH
respectively. The radicals thus formed were further aid in the decomposition of
contaminants. Further, to enhance the formation of reactive oxygen species, H2O2
oxidant is added to the reaction mixture, as in the present synthesis procedure.
According to the following reactions, iron cations, ferrous (Fe2+) and ferric (Fe3+)
ions, react with H2O2 results in formation of highly reactive ●OH radicals.
Fe2+ + H2O2 →Fe3+ + OH− + OH+
Fe3+ + H2O2 →Fe2+ + ●OOH + H+
H2O2 + OH→ H2O + ●OOH
H2O2 + e- → OH− + ●OH
H2O + h+ →H+ + ●OH
Based on the above facts, now it is possible to explain variation of percentage
degradation of 2, 4-D herbicide as a function of Cr3+ - concentration (x) for the
nanocrystalline spinel ferrite system, CoCrxFe2-xO4.
The initial decrease in percentage degradation of 2, 4 – D herbicide with Cr3+ -
concentration (x) from x = 0.0 – 0.7 is mainly due to the increase in optical energy
Chapter 4
4.69
band gap. The particle size is found to decrease and as a result effective surface area
is expected to increase (Table 4.5.1), leading to higher catalytic activity with Cr3+ -
substitution but this is not the case. Furthermore, porosity is found to increase from
11.9 % to 14.3 % for x = 0.0 – 0.7 compositions, as well as less effective Fe3+ ions are
replaced by effective Cr3+ ions in the system, thus, one can expect enhancement in
photocatalytic activity but this is also not the case. The observed sudden increase in
degradation of 2, 4-D, with Cr3+ - substitution for x = 0.7 to x = 1.7, may be correlated
with decrease in particle size, increase in porosity and replacement of Fe3+ ions by
Cr3+ ions in the system. On the other hand, observed decrease in photocatalytic
activity for x = 1.7 to 2.0 compositions is due to the almost no change in particle size
(19 ± 2 nm), and porosity (20 ± 1 %), that is dominated by increase in optical band
gap value. Here it is important to note that reduction in particle size in the substitution
range x = 0.7 to 1.7 is much larger than the x = 0.0 – 0.7 and x = 1.7 – 2.0 ranges
(Table 4.5.1). Small particle provide a tremendous driving force for diffusion
especially at elevated temperature [26]. Similarly relative change in porosity for x =
0.7 – 1.7 compositions is much higher than the x = 0.0 – 0.7 and x = 1.7 – 2.0
substitution ranges. The observed increase in porosity provides large surface area. The
larger the effective surface area available, the larger will be the number of surface
sites available for adsorption process of oxygen, giving higher catalytic response [27].
Very recently we have carried out crystal defects and cation redistribution
study on nanocrystalline cobalt – ferri – chromites, CoCrxFe2-xO4, (x = 0.0 – 2.0) by
positron annihilation spectroscopy [28]. Interestingly, the variation of the
orthopositronium life times and intensities is consistent with the compositional
dependence of percentage degradation of 2, 4-D (Figure 4.7.4) with three distinct
stages. This suggests that photocatalytic degradation is also influenced by crystal
defects like vacancy clusters and redistribution of cations as a function of Cr3+ -
substitution (x). Following the cation distribution formulae which indicated partial
inversion of the inverse spinel ferrite (x = 0.0 – 0.7), subsequent stabilization over a
range of substitution (x = 0.7 – 1.7) and finally the full inversion to the normal spinel
chromite (CoCr2O4, x = 2.0). According to this study, in the intermediate range of
substitution (x = 0.7 – 1.7), lattice contraction prevented a fraction of Co2+ ions
released from the B – sites from entering the tetrahedral sites and these vacancies at
Chapter 4
4.70
the A – sites trapped positrons. The observed increase in percentage photocatalytic
degradation for this range of the compositions may be responsible to those defects
evolutions or large vacancy clusters formation. Further, investigation is in progress.
Earlier, a correlation study has been carried out between bulk physical
properties and catalytic performance over decomposition of alcohols by ferrites, ferro
chromites and chromites [19]. The results on three spinel ferrite systems,
CuCrxFe2-xO4, MgCrxFe2-xO4 and CoCrxFe2-xO4 (x = 0.0, 1.0 and 2.0) have shown that
percentage degradation of alcohol decreases with decrease in lattice constant value
and increase in electronic activation energy.
For the system under investigation, lattice constant value is found to decrease
with increase in Cr3+ - concentration (x). Thus, decrease in percentage degradation for
x = 0.0 – 0.7 and x = 1.7 – 2.0 is consistent with previous results, but observed
increase in percentage degradation for the intermediate range, x = 0.7 – 1.7, is rather
unexpected. On the other hand, with replacement of highly magnetic Fe3+ - ions with
magnetic moment of 5 μB by less magnetic Cr3+ ions (3 μB), one can expect increase
in resistivity [29] and activation energy [30] values. As the catalysis involves transfer
of electrons/holes from the surface of the catalyst to substrate molecule and the
process is reversible, that is, greater the activation energy, the greater will be the
energy required for electronic transition resulting in decreased activity of
photocatalysts. Accordingly, percentage degradation of 2, 4–D herbicide is expected
to decrease as observed for initial (x = 0.0 – 0.7) and final (x = 1.7 – 2.0) stages.
The maximum photocatalytic activity observed for pure CoFe2O4 (x = 0.0)
(∼36.8%) among the whole range of the compositions, besides having many
unfavorable parameters (large value of lattice constant, low value of porosity, large
grain size etc) as compared to other nano ferrite compositions, may be due to the
presence of few nanoparticles with needle like shape as observed from TEM analysis
(Figure 4.4.1 (a)). According to Qu et al [31] needle shaped particles have greater
surface area than lamellar or rod shaped particles and thus enhanced photo catalytic
activity. Earlier, Darshane et al [32] have reported that percentage decomposition of
1 - Octanol by the spinel system Ga1-xFexCuMnO4 increased with increase in lattice
constant, Curie temperature and concentration of Fe(III) irons at the A – site. In the
present study based on the cation distribution formulae it is found that the
Chapter 4
4.71
concentration of ferric (Fe3+) ions at the tetrahedral (A-) site decreases with increase
in Cr3+ - concentration (x), for x = 0.0 – 0.7 compositions. For x = 0.7 – 1.7
compositions the concentration of Fe3+ remain constant i.e. 0.3, while for higher
concentration of x, 1.7 < x ≤ 2.0, Fe3+ ions at the A-site are completely absent. Thus,
the variation of percentage degradation of 2, 4–D as a function of Cr3+ - substitution
may be correlated with concentration of Fe3+ ions at the A – site as suggested in [32].
Chapter 4
4.72
Conclusions
(i) Ferrite nanoparticles of CoCrxFe2-xO4 system with variable compositions
synthesized by the co-precipitation technique can be used as an effective
photocatalytic material for the degradation of 2, 4−D herbicide under
irradiation of UV light.
(ii) The variation of percentage degradation of 2, 4−D with Cr3+-substitution is
divided into three distinct stages, each one dominated by one or more
structural and microstructural parameters.
Chapter 4
4.73
References
1. X. Bian, J. Chen, R. Ji, ‘Degradation of 2, 4-Dichlorophenoxyacetic Acid
(2, 4-D) by Novel Photocatalytic Material of Tourmaline-Coated TiO2
Nanoparticles: Kinetic Study and Model’, Materials, 6 (2013) 1530 – 1542.
2. M. Muñoz, B. K. Gullett, A. Touati, R. Font, ‘Effect of
2, 4-dichlorophenoxyacetic acid (2, 4-D) on PCDD/F emissions from open
burning of biomass’, Environ. Sci. Technol., 46 (2012) 9308 – 9314.
3. C. A. Gehring, H. R. Irving, R. W. Parish, ‘Effects of auxin and abscisic acid
on cytosolic calcium and pH in plant cells’, Proc. Natl. Acad. Sci. USA, 87
(1990) 9645 – 9649.
4. R. D. Wilson, J. Geronimo, J. A. Armbruster, ‘2, 4-D dissipation in field soils
after application of 2,4-D dimethylamine salt and 2, 4-D 2-ethylhexyl ester’,
Environ. Toxicol. Chem., 16 (1997) 1239 – 1246.
5. A. Lagana, A. Bacaloni, I. D. Leva, A. Faberi, G. Fago, A. Marino,
‘Occurrence and determination of herbicides and their major transformation
products in environmental waters’, Anal. Chim. Acta, 462 (2002) 187 – 198.
6. Y. Wang, C. Wu, X. Wang, S. Zhou, ‘The role of humic substances in the
anaerobic reductive dechlorination of 2,4-D by comamonas koreensis strain
CY01’, J. Hazard Mater., 164 (2009) 941 – 947.
7. M. G. Nishioka, H. M. Burlholer, M. C. Brinkman, C. H. Battelle, ‘Transport
of Lawn-Applied 2, 4-D from turf to home: Assessing the relative importance
of transport mechanisms and exposure pathways’, National Exposure
Research Laboratory, U.S. Environmental Protection Agency: Washington
D.C., USA, 1999.
8. C. Ang, K. Meleady, L. Wallace, ‘Pesticide residues in drinking water in the
North coast region of New South Wales, Australia, 1986-1987’, Arch.
Environ. Contam. Toxicol, 42 (1989) 595 – 602.
9. M. B. Fonseca, L. Glusczak, B. S. Moraes, C. C. Menezes, A. Pretto,
M. A. Tierno, R. Zanella, F. F. Goncalves, V. L. Loro, ‘The 2,4-D herbicide
effects on acetylcholinesterase activity and metabolic parameters of piava
freshwater fish (Leporinus. Obtusidens)’, Ecotoxicol. Environ. Saf., 69 (2008)
416 – 420.
Chapter 4
4.74
10. D. Kaioumova, C. Susal, G. Opelz, ‘Induction of apoptosis in human
lymphocytes by the herbicide 2, 4-D’, Hum. Immunol. 62 (2001) 64 – 74.
11. A. A. Pochettino, B. Bongiovanni, R. O. Duffrard, A. M. E. Duffard,
‘Oxidative stress in ventral prostate, ovary and breast by 2,4-D in pre and
postnatal exposed rats’, Environ. Toxicol., 28 (2013) 1 – 10.
12. O. M. Aly, S. D. Faust, ‘Herbicides in surface waters, studies on fate of 2, 4-D
and ester derivatives in natural surface waters’, J. Agric. Food Chem.,
12 (1964) 541 – 546.
13. K. Eme, ‘Detection and determination of chlorophenoxyacetic acid derivatives
in water’, Acta Chem. Scand., 17 (1963) 1663 – 1676.
14. T. O. Robson, ‘Some studies of the persistence of 2,4-D in natural surface
waters in Britain; British crop protection council: Survey, UK, 1966.
15. N. Ayar, B. Bilgin, G. Atun, ‘Kinetics and equilibrium studis of the herbicide
2,4-D absorption on bituminous shale’, Chem. Eng. J. 138 (2008) 239 – 248.
16. V. K. Gupta, I. Ali, Suhas, V. K. Saini, ‘Adsorption of 2,4-D and carbofuran
pesticides using fertilizer and steel industry wastes’, J. Colloid Interface Sci.,
299 (2006) 556 – 563.
17. A. M. Cupples, G. K. Sims, ‘Identification of in situ 2,4-D degrading soil
microorganisms using DNA-stable isotope probing’, Soil Biol. Biochem.,
39 (2007) 232 – 238.
18. A. C. Develosa, R. E. P. Nogueira, ‘2,4-D degradation promoted by nano
particul zerovalent iron (n ZVI) in aerobic suspensions’, J. Magn. Magn.
Mater, 121 (2013) 72 – 77.
19. V. S. Darshane, S. S. Lokegaonkar, S. G. Oak, ‘Catalysis by oxidic spinel
ferrites’, J. Phys. IV, France, 07 (1997) C1-683 – C1-684.
20. S. Kundu, A. Pal, A. K. Dixit, ‘UV induced degradation of herbicide 2, 4–D:
kinetics, mechanism and effect of various conditions on the degradation’, Sep.
Puri. Tech., 44 (2) (2005) 121 – 129.
21. B. S. Holinsworth, D. Mazumdar, H. Sims, Q. C. Sun, M. K. Yurtisigi, S.
Sarker, A. Gupta, W. H. Butler, J. L. Musfeldt, ‘Chemical tuning of the optical
band gap in spinel ferrites: CoFe2O4 vs NiFe2O4’, http:// web.utk.edu, 1 – 5.
Chapter 4
4.75
22. C. Shuchomski, C. Reitz, K. Brezesinki, C. T. de Sousa, M. Rohnke,
K. Iimura, J. P. E. de Araujo, T. Brezesinski, ‘Structural, Optical, and
Magnetic Properties of Highly Ordered Mesoporous MCr2O4 and
MCr2–xFexO4 (M = Co, Zn) Spinel Thin Films with Uniform 15 nm Diameter
Pores and Tunable Nanocrystalline Domain Sizes’, Chem. Mater., 24 (1)
(2012) 155 – 165.
23. K. N. Harish, H. S. B. Naik, P. N. P. Kumar, R. Viswanath, ‘Synthesis,
enhanced optical and photocatalytic study of Cd-Zn ferrites under sun light’,
Catal. Sci. Technol., 2 (2012) 1033 – 1039.
24. G. P. Joshi, N. S. Saxena, R. Mangal, A. Mishra, T. P. Sharma, ‘Band gap
determination of Ni-Zn ferrites’, Bull. Mater. Sci., 26 (4) (2003) 387 – 389.
25. T. S. Natrajan, K. Natrajan, H. C. Bajaj, R. J. Tayde, ‘Energy efficient UV-
LED source and TiO2 nanotube array-based reactor for photocatalytic
application’, Ind. Eng. Chem. Res., 50 (13) (2011) 7753 – 7762.
26. A. Z. Moshfegh, ‘Nanoparticle catalysts’, J. Phys. D: Appl. Phys., 42 (2009)
233001 – 233030.
27. L. K. Bagal, ‘Influence of metal oxide nanoclusters on Pt, Pd – doped SnO2
gas sensor’, Ph.D. Thesis, Solapur University, (2012).
28. K. B. Modi, N. H. Vasoya, V. K. Lakhani, T. K. Pathak, P. M. G. Nambissan,
‘Crystal defects and cation redistribution study on nanocrystalline cobalt –
ferri – chromites by positron annihilation spectroscopy’, Int. J. Spectroscopy,
2013 (2013) 11 pages.
29. M. Javed Iqbal, M. Rukh Siddiquah, ‘Electrical and magnetic properties of
chromium – substituted cobalt ferrite nanomaterials’, J. Alloy. Comp., 453
(1 -2) (2008) 513 – 518.
30. S. Singhal, S. Bhukal, ‘Effect of chromium substitution on the structural,
magnetic and electrical properties of nanocrystalline Co0.6Zn0.4Cu0.2CrxFe1.8 – x
O4 ferrite’, Solid State Phenomena, 202 (2013) 173 – 192.
31. J. Lx, L. Qiu, B. Qu, ‘Controlled synthesis of magnesium hydroxide
nanoparticles with different morphological structures and related properties in
flame retardant ethylene-vinyl acetate blends’, Nanotech., 15 (2004)
1576 –1581.