Hollow α-LiVOPO4 sphere cathodes for high energy Li-ion battery application
Transcript of Hollow α-LiVOPO4 sphere cathodes for high energy Li-ion battery application
Dynamic Article LinksC<Journal ofMaterials Chemistry
Cite this: J. Mater. Chem., 2011, 21, 10042
www.rsc.org/materials PAPER
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online / Journal Homepage / Table of Contents for this issue
Hollow a-LiVOPO4 sphere cathodes for high energy Li-ion batteryapplication
Kuppan Saravanan,a Hwang Sheng Lee,b Mirjana Kuezma,b Jagadese J Vittal*a and Palani Balaya*b
Received 17th December 2010, Accepted 18th February 2011
DOI: 10.1039/c0jm04428h
Hollow spheres of electroactive a-LiVOPO4 were synthesized via a simple one step solvothermal
method. A powder X-ray diffraction study revealed that the obtained product crystallized in the
triclinic a-LiVOPO4 phase. The morphology of the product was largely influenced by reaction
conditions such as reaction time, temperature, etc., and the product morphology was easily fine tuned
from hollow spheres to hard spheres upon changing the reaction time. Without any post-heat treatment
or milling with conductive additives, these hollow spheres exhibited comparatively large reversible Li
storage of 130 and 61 mA h g�1 at 0.1 and 1.7 C respectively. Excellent capacity retention and long term
cycling stability were demonstrated by the hollow spheres of a-LiVOPO4. We believe that a-LiVOPO4
is likely to be a prospective cathode material for high-voltage Li ion batteries application.
Introduction
Ever growing population, industrialisation, concurrent CO2
emission associated with global warming and limited availability
of fossil-fuel together have forced the way for the evolution of
green/alternative technologies of energy production, such as
wind, solar, tidal and wave. However, superior energy storage
systems are mandatory to back up these intermittent energy
sources for a reliable energy supply. Among the existing storage
systems, lithium ion batteries (LIBs) are the most promising
storage device, which has dominated the portable/mobile elec-
tronics industry until now. LIB technology is one of the serious
contenders for powering the automotive electric vehicles and
hybrid electric vehicles.1,2 Ever since LIBs were introduced in the
marketplace, more attention has been paid to focus on improving
the energy/power density. Further efforts have been made to
replace the current layered toxic heavy metal oxide cathodes with
safer, cheaper and less environmental impact electrode mate-
rials.3 Phosphate-based polyanionic transition metal complexes
LiMPO4,3–5 Li3M2(PO4)3,6–12 LiVOPO4F13,14 and LiVOPO415–18
are the best alternatives for the transition metal oxides. Phospho-
olivines possess a robust three dimensional framework, due to
the PO43� polyanion, as strong P–O covalent bonds hinder the
liberation of oxygen. These features provide exceptional stability
for the battery under abnormal conditions. Even though these
phospho-olivines are cheaper, environmentally benign and
exhibit good energy density, they suffer from poor electronic and
aNational University of Singapore (NUS), 3 Science Drive 3, Singapore117543. E-mail: [email protected] of Mechanical Engineering, NUS, Singapore 119260. E-mail:[email protected]; Fax: +65-6775-4710
10042 | J. Mater. Chem., 2011, 21, 10042–10050
ionic conductivity.19–23 Extensive work has been carried out to
improve the above cited major setbacks.24
In the hunt for perfect polyanion intercalation hosts, lithium
vanadyl phosphate (LiVOPO4) is also considered as a potential
contender. It has a theoretical capacity of �166 mA h g�1 which
is quite closer to LiFePO4 (170 mA h g�1) in addition to this, it
shows higher lithium intercalation potential of nearly 4 V. The
high theoretical energy density (166 mA h g�1 � 3.9 V ¼ 647 Wh
kg�1) with appropriately high operating voltage makes it to be
a fascinating alternate for high volt cathode material in LIBs.
Based on the spatial arrangement of VO6 octahedra and PO4
tetrahedra units which host the Li ions in the interstitial sites of
the framework, LiVOPO4 exists mainly in two different crystal-
lographic phases, namely orthorhombic b-LiVOPO4 and triclinic
a-LiVOPO4.17 Between these phases, b-LiVOPO4 is studied
extensively in the view of lithium ion intercalation, and it shows
better storage performance in comparison with the triclinic a-
LiVOPO4 phase.25 However, single crystal studies by Lii et al.26
show that the structure of a-LiVOPO4 is a close-packed column
of VO octahedra with all interstitial holes alternately filled with
Li and P atoms. Whereas in the b-LiVOPO4 the interstitial hole is
filled with a P atom and a Li atom is located in between the VO
and PO4 coordination polyhedrons surrounded by six oxygen
atoms leading to a distorted octahedron. As a result, b-LiVOPO4
structure does not accomplish the steric condition required
for facile Li ion transport. Besides this, the high temperature
a-LiVOPO4 phase has more open framework with large Li sites in
which Li atoms are loosely bound as compared to the metastable
b-LiVOPO4.26 Till now LiVOPO4 has been synthesised by high
temperature ceramic routes,16,27–29 hydrothermal methods18,26
or combination of these methods to synthesize VOPO4 fol-
lowed by lithiation to produce LiVOPO4.16,17 However, these
methods suffer from the unavoidable high-energy utilization
This journal is ª The Royal Society of Chemistry 2011
Fig. 1 PXRD patterns of the triclinic a-LiVOPO4, s unidentified
impurity.
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online
and polydispersed growth of the grains due to the high processing
temperatures (generally at 600–900 �C) which also increase the
material cost. Most of the LiVOPO4 synthesised by these methods
resulted in the particle size of around 2–6 or above 6 mm and they
exhibit the poor material utilization during cycling.15,30 From an
energy economy point of view, there is a growing concern to
synthesize the electrode materials via eco-friendly processes, such
as low temperature solvothermal processes.31,32 Here we present
a simple solvothermal approach to synthesize the high tempera-
ture phase of LiVOPO4, namely, triclinic a-LiVOPO4. The judi-
cious choice of experimental parameters helps to control the
morphology of triclinic LiVOPO4 from hollow to hard spheres.
These hollow a-LiVOPO4 spheres display superior electro-
chemical properties compared to the micron sized particles
reported earlier.
Experimental section
All the solvents and chemicals are commercially available and
used as received unless otherwise stated.
Synthesis of a-LiVOPO4
a-LiVOPO4 was synthesized in a single step by the solvothermal
method. A mixture of vanadium(III) acetylacetonate (V(acac)3,
Aldrich), lithium hydroxide (LiOH, Aldrich), ammonium dihy-
drogen phosphate (NH4H2PO4, Aldrich) and ascorbic acid
(C6H8O6, Aldrich) in a 1 : 3 : 1.5 : 2 millimolar ratio was placed
in a Teflon-lined stainless steel reaction vessel. Ethylene glycol
(25 mL) was added as solvent and the vessel was sealed tightly.
The mixture was autoclaved at 300 �C for 10 h in an oven and
then it was allowed to cool naturally to ambient temperature.
The green precipitate obtained was washed copiously with
ethanol and then dried. The synthesized a-LiVOPO4 powders
were directly used to evaluate their electrochemical performance,
without any post-heat treatment.
Physicochemical and electrochemical characterization
Powder X-Ray diffraction (PXRD) patterns were recorded using
a D5005 Bruker X-ray diffractometer equipped with Cu Ka
radiation. The accelerating voltage and current were 40 kV and
40 mA, respectively. A scan speed of 0.015� s�1 was used to
record the PXRD patterns. The morphology of the product was
examined using a field emission scanning electron microscope
(FESEM) model Jeol JSM-6700F operated at 5 kV and 10 mA
and a high resolution transmission electron microscope (JEOL
JEM-2010). For SEM examination, the sample surface was
sputtered with platinum. For TEM studies, the sample was
dispersed in ethanol by sonication, a drop was loaded on a Cu-
grid and dried. For electrochemical studies, composite electrodes
were fabricated with the active material, super P carbon black
and binder (Kynar 2801) in the weight ratio 70 : 15 : 15 using
N-methyl pyrrolidone (NMP) as solvent. Electrodes with
a thickness of 10 mm were prepared using an etched aluminium
foil (20 mm thick) as a current collector using the doctor-blade
technique. Lithium metal foil, 1 M LiPF6 in ethylene carbonate
(EC), diethyl carbonate (DEC) and dimethyl carbonate (DMC)
(1 : 1 : 1, v/v) (Merck) and Celgard 2502 membrane were used as
counter electrode, electrolyte and separator respectively to
This journal is ª The Royal Society of Chemistry 2011
assemble coin-type cells (size 2016) in an Ar-filled glove box
(MBraun, Germany). The geometrical area of the electrode was
2.0 cm2. The active material content in the electrode was around
�1.5 to 2 mg. Further details of cell fabrication have been
described previously.33 The cells were aged for 12 h before
measurement. Charge–discharge cycling at a constant current
mode was carried out using a computer controlled Arbin battery
tester (Model, BT2000, USA) and cyclic voltammetry studies
were carried out at room temperature using a computer
controlled VMP3 (Bio-logic, France). Raman spectra were
recorded with a Raman spectrometer JYT64000.
Results and discussion
PXRD was used to characterize the crystalline phase formation of
a-LiVOPO4 synthesized by the solvothermal method. It is clear
from the PXRD pattern (Fig. 1) that the triclinic a-LiVOPO4
phase was formed. All the peaks in the PXRD pattern were indexed
to a triclinic phase. The structural refinement of the PXRD pattern
was done based on a triclinic structure using P�1 space group.
Obtained lattice parameters for the a-LiVOPO4 spheres are
a ¼ 6.9089 A, b ¼ 7.3009 A and c ¼ 7.8492 A much closer to the
previous report (JCPDS Card No: 72-2253). It can be seen that
very minor unidentified impurities denoted by the symbol s were
present at an angle of 42.9� and 52.2�. No other common impu-
rities such as Li3PO4, Li2VPO6 and V2O5 have been observed.18,29
Several control try-outs have been conducted to establish the
factors that govern the formation of hollow a-LiVOPO4 micro-
spheres including effects of (1) temperature, (2) time, (3)
precursor and (4) solvent.
(1) Effect of temperature
The pure phase was observed only when the temperature was
above 300 �C. Li3PO4 was formed when the temperature is below
300 �C. Fig. 2 shows the PXRD pattern of the Li3PO4 powder
formed during synthesis at 260 �C and 280 �C.
(2) Effect of time
Fig. 3 presents the FESEM images of a-LiVOPO4 synthesised at
various time durations. Pure phase microspheres were observed
J. Mater. Chem., 2011, 21, 10042–10050 | 10043
Fig. 2 PXRD patterns of the products at various temperatures and time.
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online
when the reaction duration has reached at 20 h (Fig. 3a–c). The
low magnification FESEM image shows the sphere-like archi-
tectures of a-LiVOPO4 ranging from 1–1.5 mm in diameters
(Fig. 3a). The higher magnification FESEM image reveals that
a-LiVOPO4 microspheres are built from small 2D nanoplates
with thickness ranging from 80–120 nm (Fig. 3c). These nano-
plates are aligned interpenetrative to the spherical surface,
directed towards the core of the sphere. Most of the spheres are
broken at the center (Fig. 3b and c). When the reaction
temperature is increased to 30 h microspheres started to elongate
and became irregular in shape and size. (Fig. 3d–f) With further
time progression to 40 h nanoplates fused together to form the
rice ball shaped more dense spheres (Fig. 3g–i).
(3) Effect of precursor
While H3PO4 was used as a phosphate source, nanoplates were
formed. However, they were densely aggregated in the core and
irregular in shape and size, which were also confirmed from the
TEM analysis (see Fig. 4).
(4) Effect of solvent
The solvent has a vital role to play on the morphology of
a-LiVOPO4. We found that only micron sized diamond shaped
particles (Fig. 5a–c) were formed, instead of hollow spheres,
when tetra ethylene glycol was used as solvent instead of ethylene
glycol (EG). This clearly shows the significance of EG in the
formation of LVOP nanoplates and their hierarchical assembly.
Special physical and chemical properties of ethylene glycol, such
as viscosity, vapor pressure, and chelation resulted in the LVOP
crystal growth. Besides, the hydrogen bonding in EG molecules
helps them to exist in long chains which traps the cations (Li and
V4+) in the reaction mixture and may assist in nucleation and
10044 | J. Mater. Chem., 2011, 21, 10042–10050
growth of LVOP in plate shape. The unique chelating ability of
the EG makes it not only a solvent but also a soft template for
assembling the nanoplates into microstructures.34
The TEM, HRTEM and SAED (selected area electron
diffraction pattern) images of hollow a-LiVOPO4 spheres are
shown in Fig. 6. TEM images (Fig. 6a–d) show the hollow nature
of the a-LiVOPO4 synthesised at 20 h. The HRTEM image
(Fig. 6e) of hollow a-LiVOPO4 spheres exhibits clear lattice
fringes demonstrating single crystallinity of the individual plates.
The observed width, 3.271 A, of neighbouring lattice fringes
corresponds to the (�121)/(1–12) plane of a-LiVOPO4. Various
electron diffraction spots shown in Fig. 6f were indexed to
(�121)/(1�12), (402), (2�12) and (�140) plane of a-LiVOPO4. These
SAED spots are consistent with the PXRD pattern shown in
Fig. 1. This confirms that these hollow a-LiVOPO4 spheres are
indeed a pure crystalline phase.
(5) Carbon coating
Diffuse reflectance spectra analysis and DFT calculation by
Yang et al.30 demonstrated that triclinic a-LiVOPO4 is a wide
band gap semiconductor (2.78 eV) which is confirmed using the
AC impedance technique.30 Highly aggregated and dense nature
of the large a-LiVOPO4 particles synthesised commonly by
ceramic methods15,30 exhibit extremely poor electronic conduc-
tivity. Ball milling with acetylene black and adding electronic
binder found to boost the electrochemical and kinetics
process.35,36 In the case of b-LiVOPO4, RuO2 has also been
employed to enhance the electrical conductivity problems,
however, which is expensive for practical applications.25
We have shown that optimising the carbonising precursor will
have strong influence on the storage behaviour of LiFePO4.31,37
Here, we have used ascorbic acid as a carbonising agent. Fig. 7
shows a characteristic Raman spectrum of a-LiVOPO4 hollow
spheres synthesised by the solvothermal method. A small band
appears at 939 cm�1 is attributed to the symmetric stretching
mode of PO43� anion in a-LiVOPO4. Two broad and strong
bands situated at 1357 and 1601 cm�1 are designated to the D
(disordered) and G (graphene) bands of the residual carbon
coated on the hollow spheres respectively. The relative intensity
ratio between the D and G bands can be used to assess the
content of sp3 and sp2 carbon in the a-LiVOPO4. In general,
decreased D/G ratio or increased amounts of sp2 type carbon
greatly enhances the electronic conductivity leading to the good
discharge capacities and superior rate capabilities.38,39 The ID/IG
ratios of the LFP nanoplates were found to be 0.660, this shows
the larger amount of graphene clusters than the disordered
carbon structure, which in turn expected facilitates a far better
cell performance of a-LiVOPO4 when compared with the bulk
sample prepared from ceramic routes.30 Currently systematic
work is in progress on optimising the carbon coating for
a-LiVOPO4.
Electrochemical characterisation
The electrodes made of hollow spheres of a-LiVOPO4 were
subjected to galvanostatic charge–discharge cycles between 3 and
4.5 V vs. Li/Li+ at various current rates. Few charge–discharge
cycles at 0.1 C are shown in Fig. 8. Cycle life of the hollow sphere
This journal is ª The Royal Society of Chemistry 2011
Fig. 3 FESEM images of a-LiVOPO4 synthesized at 300 �C in different time intervals: (a–c) 20 h, (d–e) 30 h and (g–i) 40 h.
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online
electrode at 0.1 C is shown as inset in Fig. 8. Lithium ion inter-
calation process in the a-LiVOPO4 is expressed in eqn (1).
Reversible lithium extraction and insertion of a-LiVOPO4 are
based on the V4+/V5+ redox couple.17
LiVOPO4 # VOPO4 + Li+ + e� (1)
During the first Li-deintercalation (oxidation) process, the
voltage increased sharply to 4.06 V from the open circuit voltage
(OCV z 3.0 V) followed by a flat long plateau (Fig. 8) and then
gradually increased to the cut-off voltage (4.5 V). The first charge
process resulting in a storage capacity of 145 mA h g�1 which is
equivalent to 87.3% of the theoretical capacity. (Theoretical
capacity 166 mA h g�1 assuming complete extraction of Li.) The
discharge curve shows a similar bi-phasic plateau region at 4.00
V and leading to the storage capacity of 129.5 mA h g�1. In the
first cycle, there is an irreversible capacity loss of about 15 mA h
This journal is ª The Royal Society of Chemistry 2011
g�1 with coulombic efficiency of 90%. Subsequent cycles show the
similar plateau behaviour, however, there is a decline of revers-
ible capacity values for the initial cycles resulting in the invariable
capacity of 101 mA h g�1 at 50th cycle. The small polarisation
(DV) of 0.06 V (DV ¼ voltage difference between the charge and
discharge curves) is indicative of the energetic reversibility of the
V4+/V5+ system under the low rate conditions. Under similar rate
conditions of a-LiVOPO4 prepared by Ren et al.18 exhibited
a huge irreversible capacity loss (ICL) with a coulombic effi-
ciency of 52% and a polarisation of nearly 200 mV. While
comparing with the previously reported triclinic a-LiVOPO4
samples obtained by the sol–gel method,30 hollow a-LiVOPO4
spheres synthesized here exhibit excellent cyclability and very
good rate performance.
To further explain the influence of current rate on the redox
behavior, several replicate cells were tested at different C rates.
The galvanostatic charge–discharge profiles of a-LiVOPO4
hollow spheres at various rates are displayed in Fig. 9a–e.
J. Mater. Chem., 2011, 21, 10042–10050 | 10045
Fig. 4 FESEM and TEM images of a-LiVOPO4 synthesized using H3PO4.
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online
Polarisation between the charge–discharge plateaus increased
upon increasing the rate. It is found to be 0.08, 0.15, 0.22, 0.35
and 0.45 V for 0.36 C (60 mA g�1), 0.72 C (120 mA g�1), 1.08 C
(180 mA g�1), 2.53 C (420 mA g�1) and 4.22 C (700 mA g�1)
respectively. Columbic efficiency is greatly enhanced to 98%
beyond 0.36 C. The capacity retention of the a-LiVOPO4 elec-
trodes versus cycling number is shown in Fig. 9f which reveals
good and consistent cycling stabilities found at all the rates. The
overall reversible storage capacity is found to be 85, 77, 71, 48
and 40 mA h g�1 for 0.36 C (60 mA g�1), 0.72 C (120 mA g�1),
1.08 C (180 mA g�1), 2.53 C (420 mA g�1) and 4.22 C (700 mA
g�1) respectively. As compared to the chemically lithiated and
mechanically ground a-LiVOPO4 by Kerr et al.17 at 1 C rate,
Fig. 5 FESEM images of the a-LiVOPO4 synthesised in te
10046 | J. Mater. Chem., 2011, 21, 10042–10050
these a-LiVOPO4 hollow spheres display a better performance. It
is believed that the hollow nature favours efficient wetting of the
active materials by electrolytes thereby providing more active
sites for the electrochemical reactions.40 Thus the morphology of
the product appears to be one of the important factors in
improving the kinetic properties of the a-LiVOPO4.
Galvanostatic cycling of the a-LiVOPO4 sample at 1.7 C rate is
shown in Fig. 10. Under this rate (280 mA g�1) 500 cycles were
carried out to elucidate the long term cycling stability. Reversible
capacities of 58 mA h g�1 and 51 mA h g�1 were observed at the
end of 1st and 500th cycle respectively. This shows an average
capacity degradation of just 0.01 mA h g�1 per cycle. In addition
to this, the observed columbic efficiency was found to be more
traethylene glycol as solvent at different magnifications.
This journal is ª The Royal Society of Chemistry 2011
Fig. 6 TEM, HRTEM and SAED images of hollow spheres of a-LiVOPO4.
Fig. 7 Raman spectrum of the a-LiVOPO4 hollow spheres.
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online
than 99% during these long term cycles. The long term stability of
the lithium insertion/extraction reactions in a-LiVOPO4 hollow
spheres is evidenced by negligible capacity fade over the 500
charge–discharge cycles. Plate type architecture offers the
advantages of fast transport of Li+ ions. Besides this, the hollow
nature of the spheres offers sufficient active sites and short
diffusion path for lithium ions to intercalate. These features lead
to good electrochemical activity of hollow a-LiVOPO4 spheres
compared with the bulk (>6 mm) LiVOPO4 synthesised from
ceramic routes.18,30,35
This journal is ª The Royal Society of Chemistry 2011
The high rate capability is one of the mandatory electro-
chemical features of LIBs to power the high energy applications
(HEV and EV). The rate performance of a-LiVOPO4 electrodes
was evaluated for 9 different (Fig. 11) charge–discharge current
rates corresponding to 0.18, 0.6, 1.7, 3.4, 5.1, 6, 8.5, 13 and 0.36 C
(here 1 C ¼ 166 mA g�1), in the voltage range 3–4.5 V (Fig. 11).
On average, minimum 50 cycles were carried out for a given rate.
As expected, the capacity decreases from 98 mA h g�1 to 22 mA h
g�1 with increasing C-rate from a value of 0.18 C (16 mA g�1) to
13 C (2158 mA g�1), showing a diffusion-limited mass transfer of
Li+ between the surface and core of the a-LiVOPO4 particles.
Upon decreasing the current from 13 C to 0.36 C, 85 mA h g�1
was observed. At each C-rate, the storage capacity is found to be
stable except at a low rate of 0.18 C. Fig. 11 shows charge–
discharge voltage profiles of hollow a-LiVOPO4 spheres at
various C rates. Upon increasing the C rate, it is seen that the
polarization of the electrode material increases, which imitates
the variation of DV, this is possibly due to increase in the elec-
trode resistance, thereby declining the storage performance of the
electrodes.
The cyclic voltammograms (CV) of hollow a-LiVOPO4
spheres are shown in Fig. 12. The CV was recorded with Li metal
as the counter and reference electrodes in the voltage range of
3–4.5 V at the scan rate of 0.058 mV s�1 up to 10 cycles at room
temperature. A single pair of anodic/cathodic peaks found in the
CV which corresponds to the V4+/V5+ redox couple trans-
formations. During the first cycle (i.e., Li-deintercalation), the
anodic peak is at 4.06 V and the corresponding cathodic peak is
J. Mater. Chem., 2011, 21, 10042–10050 | 10047
Fig. 8 Galvanostatic charge–discharge cycle curves of a-LiVOPO4 hollow spheres at 0.1 C. Current density of 16 mA g�1, 1 C refers to a capacity of 166
mA g�1 in one h, potential window 3–4.5 V and the data were recorded at room temperature (inset: capacity vs. cycle number plots).
Fig. 9 Galvanostatic charge–discharge profiles of a-LiVOPO4 hollow spheres at various rates (selected cycles are given): (a) 0.36 C (60 mA g�1); (b) 0.72 C
(120 mA g�1); (c) 1.08 C (180 mA g�1); (d) 2.53 C (420 mA g�1); (e) 4.22 C (700 mA g�1) and (f) reversible capacity vs. cycle number plots, here open symbols refer
to the charge capacity and closed symbols refer to the discharge capacity. The potential window is 3–4.5 V and the data were recorded at room temperature.
10048 | J. Mater. Chem., 2011, 21, 10042–10050 This journal is ª The Royal Society of Chemistry 2011
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online
Fig. 10 (a) Long term galvanostatic charge–discharge voltage profiles of
a-LiVOPO4 at 1.7 C. (b) Reversible capacity vs. cycle number plots
(selected cycles are given) over the potential window 3–4.5 V.
Fig. 12 Cyclic voltammograms of a-LiVOPO4 hollow spheres. Scan
rate: 0.058 mV s�1.
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online
at 3.85 V (i.e., Li-intercalation) in good agreement with the
charge/discharge curves (Fig. 8.). The symmetrical nature of
the redox peaks in the CV is suggestive of the good movement of
the interfacial boundary.17 In the subsequent cycles, the oxida-
tion peak and the corresponding reduction peak are unaltered
upto 10 cycles; this infers good reversibility of a-LiVOPO4. This
also suggests that the unidentified impurities observed in the
PXRD (Fig. 1) were electrochemically inactive in the potential
window used. In comparison, the results of solvothermally
Fig. 11 a-LiVOPO4 hollow spheres: (a) the rate capability and (b)
charge–discharge voltage profiles at various C rates.
This journal is ª The Royal Society of Chemistry 2011
prepared a-LiVOPO4 hollow spheres indicate that this synthetic
approach offers significant improvement in producing an elec-
trode material with favorable electrochemical properties over the
existing methods.18,30,35
Conclusions
In summary, triclinic a-LiVOPO4 hollow spheres were syn-
thesised by the solvothermal method at 300 �C for 10 h and they
were characterized using PXRD, SEM, HRTEM and SAED.
Reaction parameters have a strong influence on the morphology
of the final product. The as-synthesized a-LiVOPO4 was tested as
a 4 V cathode material for LIB and it exhibited reversible
capacities of 130 and 61 mA h g�1 at 0.1 C and 1.7 C respectively.
The remarkable long term cycling stability and good high rate
performance were found upto 13 C. The hollow nature and
nanosized plates forming the spheres favour the absolute wetting
of the a-LiVOPO4 by the liquid electrolyte so that Li+ interca-
lation/deintercalation can be achieved easily leading to the
superior Li storage when compared with the a-LiVOPO4 syn-
thesised by other methods. Therefore, hollow a-LiVOPO4
spheres synthesised by the solvothermal method is a very good
alternative for the cathode materials in certain LIB applications.
Acknowledgements
We thank the Ministry of Education Singapore for financial
support through NUS FRC Grant No. R-143-000-371-112 and
US DARPA grant R-265-000-320-597. K.S. thanks NUSNNI
for research scholarship. H.S.L thanks Andrew A. O. Tay for
fruitful discussions.
References
1 M. Armand and J. M. Tarascon, Nature, 2008, 451, 652–657.2 J. Hassoun, S. Panero, P. Reale and B. Scrosati, Adv. Mater., 2009,
21, 4807–4810.3 A. K. Padhi, K. S. Nanjundaswamy and J. B. Goodenough, J.
Electrochem. Soc., 1997, 144, 1188–1194.4 S. Y. Chung, J. T. Bloking and Y. M. Chiang, Nat. Mater., 2002, 1,
123–128.5 H. Huang, S. C. Yin and L. F. Nazar, Electrochem. Solid-State Lett.,
2001, 4, A170–A172.
J. Mater. Chem., 2011, 21, 10042–10050 | 10049
Publ
ishe
d on
24
Mar
ch 2
011.
Dow
nloa
ded
by T
he U
nive
rsity
of
Auc
klan
d L
ibra
ry o
n 29
/10/
2014
00:
11:0
7.
View Article Online
6 A. S. Andersson, B. Kalska, P. Jonsson, L. Haggstrom, P. Nordblad,R. Tellgren and J. O. Thomas, J. Mater. Chem., 2000, 10, 2542–2547.
7 Y. Z. Li, Z. Zhou, M. M. Ren, X. P. Gao and J. Yan, Electrochim.Acta, 2006, 51, 6498–6502.
8 C. Masquelier, C. Wurm, J. Rodriguez-Carvajal, J. Gaubicher andL. Nazar, Chem. Mater., 2000, 12, 525–532.
9 S. Patoux, C. Wurm, M. Morcrette, G. Rousse and C. Masquelier, J.Power Sources, 2003, 119, 278–284.
10 M. M. Ren, Z. Zhou, Y. Z. Li, X. P. Gao and J. Yan, J. PowerSources, 2006, 162, 1357–1362.
11 H. Huang, S. C. Yin, T. Kerr, N. Taylor and L. F. Nazar, Adv.Mater., 2002, 14, 1525–1528.
12 M. Y. Saidi, J. Barker, H. Huang, J. L. Swoyer and G. Adamson,Electrochem. Solid-State Lett., 2002, 5, A149–A151.
13 J. Barker, R. K. B. Gover, P. Burns and A. Bryan, Electrochem. Solid-State Lett., 2005, 8, A285–A287.
14 J. Barker, R. K. B. Gover, P. Burns, A. Bryan, M. Y. Saidi andJ. L. Swoyer, J. Power Sources, 2005, 146, 516–520.
15 B. M. Azmi, T. Ishihara, H. Nishiguchi and Y. Takita,Electrochemistry, 2003, 71, 1108–1110.
16 J. Barker, M. Y. Saidi and J. L. Swoyer, J. Electrochem. Soc., 2004,151, A796–A800.
17 T. A. Kerr, J. Gaubicher and L. F. Nazar, Electrochem. Solid-StateLett., 2000, 3, 460–462.
18 M. M. Ren, Z. Zhou, X. P. Gao, L. Liu and W. X. Peng, J. Phys.Chem. C, 2008, 112, 13043–13046.
19 C. Delacourt, L. Laffont, R. Bouchet, C. Wurm, J. B. Leriche,M. Morcrette, J. M. Tarascon and C. Masquelier, J. Electrochem.Soc., 2005, 152, A913–A921.
20 P. P. Prosini, M. Lisi, D. Zane and M. Pasquali, Solid State Ionics,2002, 148, 45–51.
21 R. Amin, J. Maier, P. Balaya, D. P. Chen and C. T. Lin, Solid StateIonics, 2008, 179, 1683–1687.
22 M. S. Islam, D. J. Driscoll, C. A. J. Fisher and P. R. Slater, Chem.Mater., 2005, 17, 5085–5092.
10050 | J. Mater. Chem., 2011, 21, 10042–10050
23 C. A. J. Fisher and M. S. Islam, J. Mater. Chem., 2008, 18, 1209–1215.24 A. Yamada, S. C. Chung and K. Hinokuma, J. Electrochem. Soc.,
2001, 148, A224–A229.25 M. M. Ren, Z. Zhou, L. W. Su and X. P. Gao, J. Power Sources, 2009,
189, 786–789.26 K. H. Lii, C. H. Li, C. Y. Cheng and S. L. Wang, J. Solid State Chem.,
1991, 95, 352–359.27 H. T. Kuo, N. C. Bagkar, R. S. Liu, C. H. Shen, D. S. Shy,
X. K. Xing, J. F. Lee and J. M. Chen, J. Phys. Chem. B, 2008, 112,11250–11257.
28 M. M. Ren, Z. Zhou and X. P. Gao, J. Appl. Electrochem., 2010, 40,209–213.
29 K. Nagamine, T. Honma and T. Komatsu, J. Am. Ceram. Soc., 2008,91, 3920–3925.
30 Y. Yang, H. S. Fang, J. Zheng, L. P. Li, G. S. Li and G. F. Yan, SolidState Sci., 2008, 10, 1292–1298.
31 K. Saravanan, P. Balaya, M. V. Reddy, B. V. R. Chowdari andJ. J. Vittal, Energy Environ. Sci., 2010, 3, 457–464.
32 K. Saravanan, M. V. Reddy, P. Balaya, H. Gong, B. V. R. Chowdariand J. J. Vittal, J. Mater. Chem., 2009, 19, 605–610.
33 K. Saravanan, K. Ananthanarayanan and P. Balaya, Energy Environ.Sci., 2010, 3, 939–948.
34 Y. Wang, X. Jiang and Y. Xia, J. Am. Chem. Soc., 2003, 125, 16176–16177.
35 B. M. Azmi, T. Ishihara, H. Nishiguchi and Y. Takita, J. PowerSources, 2005, 146, 525–528.
36 B. M. Azmi, H. S. Munirah, T. Ishihara and Y. Takita, Ionics, 2005,11, 402–405.
37 K. Saravanan, J. J. Vittal, M. V. Reddy, B. V. R. Chowdari andP. Balaya, J. Solid State Electrochem., 2010, 14, 1755–1760.
38 M. M. Doeff, J. D. Wilcox, R. Kostecki and G. Lau, J. PowerSources, 2006, 163, 180–184.
39 M. Doeff, J. Wilcox, R. Yu, A. Aumentado, M. Marcinek andR. Kostecki, J. Solid State Electrochem., 2008, 12, 995–1001.
40 M. Nagarathinam, K. Saravanan, W. L. Leong, P. Balaya andJ. J. Vittal, Cryst. Growth Des., 2009, 9, 4461–4470.
This journal is ª The Royal Society of Chemistry 2011