Journal of Power Sources 196 (2011) 4821–4825
Contents lists available at ScienceDirect
Journal of Power Sources
journa l homepage: www.e lsev ier .com
Short communication
Synthe th
Li[Li0.2M e c
J. Li, R. Kl S. P
Institute of Phy
a r t i c l
Article history:
Received 14 O
Received in re
17 December 2
Accepted 3 Jan
Available onlin
Keywords:
Lithium-ion ba
Cathode mate
Li[Li0.2Mn0.56N
NMC
Cycling perfor
Rate capability
Ni0.16
s bee
and
partic
bviou
capa
hiev
1. Introduction
Layered transition metal oxides have been investigated exten-
sively as ca
LiCoO2 is th
very good
hand, it als
and safety
pure electri
capacity an
point in the
regard, the
Co, Ni, etc.)
materials in
high capaci
bers of this
0.6Li2MnO3
(also indi
widely inv
an initial
tial range
Li[Li0.2Mn0.
because of
∗ Correspon
E-mail add
electrode polarization and improve the activation of the Li2MnO3
component, even if present in a small amount [13,14]. Neverthe-
less, the long-term cycling performance of this latter material is
0378-7753/$ –
doi:10.1016/j.
thode materials for lithium-ion batteries. There into,
e most important commercial material because of its
electrochemical performance. However, on the other
o suffers some drawbacks, such as high cost, toxicity,
problems, which inhibit its further use in hybrid and
c vehicles [1–3]. The identification of a cheaper, higher
d safer layered cathode materials has been the focusing
study of cathode materials in the last decade. In this
solid solutions of layered Li2MnO3 and LiMO2 (M=Mn,
have been shown as promising candidates for cathode
lithium ion batteries since they exhibit a relatively
ty, low cost and improved safety [2,4–11]. Two mem-
family, Li[Li0.2Mn0.6Ni0.2]O2, which can be indicated as
·0.4LiMn0.5Ni0.5O2, and Li[Li0.2Mn0.54Ni0.13Co0.13]O2
cated as 0.6Li2MnO3·0.4LiMn1/3Ni1/3Co1/3O2), are
estigated already. Usually, these materials deliver
capacity of about 250mAhg−1 within the poten-
extending from 2.0 to 4.8V [8–12]. Between them,
54Ni0.13Co0.13]O2 always shows better performance
the presence of cobalt that significantly reduce the
ding author. Tel.: +49 251 8336026; fax: +49 251 8336032.
ress: stefano.passerini@uni-muenster.de (S. Passerini).
still not very satisfactory. In addition, it still contains 13mol% of
Co, which certainly represents an issue with regard to cost. Finally,
most of the works on these materials report the electrochemical
performance at very low current rates (such as C/20), which is of no
help to ascertain their capability of matching with the requirement
of today’s lithium ion batteries.
In this work, we report on the synthesis and characterization
of a novel cathode material with a substantially lower Co content.
The material has a general formula of Li[Li0.2Mn0.56Ni0.16Co0.08]O2,
which can also be seen as the solid solution of Li2MnO3 and
LiMn0.4Ni0.4Co0.2O2 in 6:4 molar ratio. The structure, physical
properties and electrochemical performance are reported in the
following, with a special attention to the rate capabilities at high
current rates.
2. Experimental
Li[Li0.2Mn0.56Ni0.16Co0.08]O2 was synthesized by a solid-state
reaction method from lithium hydroxide hydrate (LiOH·H2O
Aldrich >98%) and manganese–nickel–cobalt hydroxide precursor
[15]. This precursor was prepared by co-precipitating the aqueous
solution of the three metal acetate salts (Mn, Ni, and Co; Aldrich
>98%) in a stoichiometric ratio of 56:16:8, with lithium hydrox-
ide. After extensive rinsing with distilled water, the precipitate
see front matter © 2011 Elsevier B.V. All rights reserved.
jpowsour.2011.01.006
sis and electrochemical performance of
n0.56Ni0.16Co0.08]O2 with improved rat
öpsch, M.C. Stan, S. Nowak, M. Kunze, M. Winter,
sical Chemistry, University of Muenster, Corrensstr. 28/30, 48149 Muenster, Germany
e i n f o
ctober 2010
vised form
010
uary 2011
e 14 January 2011
ttery
rial
i0.16Co0.08]O2
mance
a b s t r a c t
The high voltage layered Li[Li0.2Mn0.56
Li2MnO3 and LiMn0.4Ni0.4Co0.2O2, ha
temperature annealing at 900 ◦C. XRD
constitutedof small andhomogenous
capability. After the initial decay, no o
different rates. Steady-state reversible
at 5C and 110mAhg−1 at 20C were ac
2.5 and 4.8V at 20 ◦C.
/ locate / jpowsour
e high voltage cathode material
apability
asserini ∗
Co0.08]O2 cathode material, which is a solid solution between
n synthesized by co-precipitation method followed by high
SEM characterizations proved that the as prepared powder is
les (100–300nm),whichare seen toenhance thematerial rate
s capacity fading was observed when cycling the material at
cities of 220mAhg−1 at 0.2C, 190mAhg−1 at 1C, 155mAhg−1
ed in long-term cycle tests within the voltage cutoff limits of
© 2011 Elsevier B.V. All rights reserved.
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4822 J. Li et al. / Journal of Power Sources 196 (2011) 4821–4825
Fig. 1. Riet
Li[Li0.2Mn0.56N
was dried u
was then m
milling for5
was anneal
for 24h. The
liquidnitro
The com
tents in th
coupled pla
ARCOS, Am
terized by
the Bruker
90◦. Lattice
with GSAS
with the he
(SEM, EVO®
solid phase
the AccuPy
(USA).
Electrod
position of
(TIMCAL), a
onto Al foil
2mgcm−2
for 30 s) wa
reference e
swagelok c
electrolyte.
current rat
between 4.
tester (USA
couple.
All expe
reproducibi
3. Results
Fig. 1 sho
of Li[Li0.2M
(9.9%) demo
the low inte
the crystal l
ture with s
and (104) p
and (110) p
EM pictures of Li[Li0.2Mn0.56Ni0.16Co0.08]O2 material at different magnifica-
) ×5k; (b and c) ×50k.
xagonal latticeparameterswere refined tobea=2.8560(1) A˚,
83(2) A˚, and volume=100.65(2) A˚3, with a c/a ratio of 4.99.
veld refinement results for the XRD pattern of
i0.16Co0.08]O2 material by GSAS.
nder vacuum at 120 ◦C overnight. The dried material
ixed with a stoichiometric amount of LiOH·H2O by ball
h in thezirconia jar.After suitablegrinding, themixture
ed in air at 480 ◦C for 5h, and then, as a pellet, at 900 ◦C
final material was obtained by quenching the pellet in
gen in order to “freeze” the layered solid-solutionphase.
position in terms of lithium and transition metal con-
e active material was determined by the inductively
sma optical emission spectrometry (ICP-OES, SPECTRO
etek, Germany). The crystalline structure was charac-
X-ray diffraction (XRD) using the Cu K� radiation on
D8 Advance (Germany) in the 2� range from 10◦ to
parameters were determined by Rietveld refinement
software. The particle size distribution was evaluated
lp of a high resolution Scanning Electron Microscopy
MA 10 microscope, Zeiss). The BET surface area and
density were measured by using the ASAP 2020 and
c II 1340 from Micromeritics Instrument Corporation
es were prepared by casting the slurry, with the com-
80wt% active material (by weight), 10wt% Super P
nd 10wt% PVDF (Kynar® FLEX 2801, Arkema Group),
. The electrode active material mass loading was about
while the thickness (after pressing at 3–4 tons cm−2
s 10�m. With metal lithium foil as the counter and
lectrodes, the cathode electrodes were assembled into
ells with the 1M LiPF6 in 1:1 EC:DMC solution as the
Cellswere cycled galvanostatically at different constant
Fig. 2. S
tions. (a
Thehe
c=14.2
es (nominal capacity =200mAhg−1, 1C=200mAg−1)
8V and 2.5V at 20 ◦C using Maccor series 4000 battery
). All potential reported in this work refer to the Li/Li+
riments, including synthesis, were duplicated to check
lity.
and discussion
ws theXRDpattern and theRietveld refinement results
n0.56Ni0.16Co0.08]O2. The values of �2 (4.926) and Rwp
nstrate a satisfactory refinement.With the exclusion of
nsity reflections, in particular thosewithin 20◦ and 25◦,
attice was approximated as signed to the layered struc-
pace group of R3¯m [3], the intensity ratio of the (003)
eaks (equal to 1.11), and the clear splitting of the (108)
eaks suggest an ordering structure of R3¯m single phase.
The weak r
Li2MnO3-li
ordering of
[17].
The ICP
transition m
in good agr
The crystall
formula [1]
and (104).
of the pure
conditions
The mo
cles and p
microscopy
that the p
particles. T
eflections are known to originate from the monoclinic
ke (C2/m) super lattice [16], which correspond to the
the Li+, Ni2+, and Mn4+ ions in the transition metal layer
-OES analysis indicated the molar ratio of Li and the
etal ions to be Li:Mn:Ni:Co=1.21:0.53:0.17:0.09, i.e.,
eement with the composition of the starting reactants.
ite sizewas calculated fromXRDby using the Scherrer’s
for the three main reflection peaks, e.g. (0 03), (1 01)
The average result is 89nm which is smaller than that
LiMn0.4Ni0.4Co0.2O2 prepared with the same annealing
[18].
rphology of the Li[Li0.2Mn0.56Ni0.16Co0.08]O2 parti-
ressed electrode, investigated by scanning electron
, is shown in Fig. 2. The SEM image in Fig. 2a shows
owder contains aggregates of primary, round sharp
hese primary particles, which are better observed in
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J. Li et al. / Journal of Power Sources 196 (2011) 4821–4825 4823
Fig. 3. Com
Li[Li0.2Mn0.56N
Fig. 2b, are
300nm. Sin
Li ions, the
are expecte
electrode is
is compose
material an
the prepare
BET, is 7.3
mercial LiM
Europe Gm
from the so
(7.31m2 g−
100–300nm
is expected
enhancing t
cially the h
the compar
area materi
4.78m2 g−1
a worse hig
material in
larger parti
cycle and 61
87.2mAhg−
material. Th
better perfo
Fig. 4
Li[Li0.2Mn0.
sities. As e
exhibited tw
of two diffe
shifted to h
plateau, wh
almost the
on the curr
of the LiM
to the oxid
capability o
of the Li ion
ered in the
of 111.5mA
4.4/4.5V du
loss of oxyg
irst ch
at di
ycling performance of Li[Li0.2Mn0.56Ni0.16Co0.08]O2 electrodes charged at
discharged at different rates. The tests carried out in the voltage range
2.5V and 4.8V at 20 ◦C.
sformed in a MnO2-like phase. The capacity delivered in
cond plateau strongly decreases as the current increases
Ahg−1 at 0.1C against 105mAhg−1 at 20C) thus indicating
is process has rather slow kinetics.
capacity delivered during the first discharge is obvi-
resulting from the insertion of lithium in both the
4Ni0.4Co0.2O2-like regions and the MnO2-like regions.
parison of high rate (20C) cycling performance of
i0.16Co0.08]O2 electrodes with different particle sizes.
homogenous and have a small size between 100 and
ce small particles present shorter diffusion path for
insertion and de-insertion of the Li in this material
d to be faster [1,19,20]. The SEM image of pressed
shown in Fig. 2c. It can be seen that the electrode
d of a very homogenous mixture of primary active
d Super P. In addition, the specific surface area for
d Li[Li0.2Mn0.56Ni0.16Co0.08]O2 powder, as detected by
1m2 g−1, which is much higher than that of com-
n1/3Ni1/3Co1/3O2 material (0.61m2 g−1, TODA Kogyo
bH). In addition, the average particle size calculated
lid phase density of 4.30 g cm−2 and BET surface area
1), is 190nm, which is in very good agreement with the
particle size detected by SEM. Such a high surface area
to favor the charge transfer process of lithium ions thus
he electrochemical performance of this material, espe-
igh rate capability. This is well shown in Fig. 3 where
ison of the rate performance for different BET surface
als is shown. The material having a BET surface area of
(corresponding to 290nm average particle size) shows
h rate (20C) performance than the small particle size
terms of both capacity and cycling stability. In fact, the
cle size material delivered only 119mAhg−1 at the 1st
.6mAhg−1 after 300 cycles against 145.4mAhg−1 and
1, respectively, delivered by the smaller particle size
is result proved that the smaller particle will lead to
Fig. 4. F
as cycled
Fig. 5. C
0.1C and
between
be tran
this se
(220m
that th
The
ously
LiMn0.
rmance at high rate cycling.
compares the first charge–discharge profiles of
56Ni0.16Co0.08]O2 cathode at different current den-
xpected from the XRD characterization, the material
o plateaus during the first charge, due to the existence
rent lithium de-insertion processes [6]. Both plateaus
igher potential with the increase of current. In the first
ich is located at 3.8–4.4/4.5V, all electrodes delivered
same capacity (about 110–120mAg−1) independent
ent used. This plateau is associated to the delithiation
n0.4Ni0.4Co0.2O2-like regions [21] that corresponds
ation of Ni2+ →Ni4+ and Co3+ →Co4+. Since the rate
f these two processes is improved by the participation
s in the transition metal layer [22], the charge deliv-
first plateau is very close to the theoretical capacity
hg−1. The second plateau, which is located above
ring charging, is widely accepted to originate from the
en from the layered Li2MnO3 lattice [6], which might
Fig. 5
Li[Li0.2Mn0.
and discha
within the
capacities a
in Table 1.
able to de
at 0.2C and
Table 1
Capacity of Li
Charge rate w
Cycle
1st
30th
80th
100th
arge and discharge profiles of Li[Li0.2Mn0.56Ni0.16Co0.08]O2 electrodes
fferent rates in the voltage range between 2.5V and 4.8V at 20 ◦C.
compares the capacity retention of
56Ni0.16Co0.08]O2 electrodes when charged at 0.1C
rged at different current rates (0.2C, 1C, 5C and 20C)
cut-off voltages of 2.5V and 4.8V (20 ◦C). The delivered
t the 1st, 30th, 80th and 100th cycles are also listed
In the first discharge process, the electrodes were
liver capacities of 271.4mAhg−1 and 230.6mAhg−1
1C, respectively. Very interestingly, at 5C and 20C
[Li0.2Mn0.56Ni0.16Co0.08]O2 electrodes discharged at different rates.
as always 0.1C.
Discharge capacity (mAhg−1)
0.2C 1C 5C 20C
271.5 230.6 195.3 155.4
225.1 195.4 164.6 113.7
217.4 192.8 155.9 110.4
214.6 190.7 155.0 109.4
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4824 J. Li et al. / Journal of Power Sources 196 (2011) 4821–4825
rates, the electrodes were still able to deliver 195.3mAhg−1 and
155.4mAhg−1, respectively, which corresponded to 72% and 57%
of the 0.2C delivered capacity. This comparison clearly indicates
the promising high rate capability of the material. However, the
discharge capacities decreased in the next several cycles inde-
pendent on the current used in the test. At the 30th cycle, the
capacity dropped to 225.1mAhg−1 at 0.2C (i.e., 82.9% of the 1st
cycle capacity), and 113.4mAhg−1 at 20C (i.e., 73.1% of the 1st
cycle capacity). However, after the 30th cycle the capacity fade was
much less significant at all rates. It is proved that capacities as high
as 217.4mAhg−1 after 80 cycles at 0.2C rate, and 190.7mAhg−1,
155.5mAhg−1 and 109.4mAhg−1 after 100 cycles at 1C, 5C and
20C, respectively, were obtained. The comparison with the values
obtained at the 30th cycle indicates that only a minor capacity loss,
i.e., less than 8mAhg−1, took place. This proves that this material
is a good candidate for high discharge rate electrodes even though
the capacity retention in the initial 20 or 30 cycles still needs
to be improved. Nevertheless, it is important to notice that the
capacity delivered by our material during the 100th discharge
at 1C rate very well compare with that of the Li–Ni–PO4 coated
0.5Li2MnO3·0.5LiMn1/3Ni1/3Co1/3O2 which is reported to have
the better cycle stability at high rate [23]. Unfortunately, direct
comparison with long term high rate test of other materials from
the same family is not possible so far till now due to the lack of
literature data. In fact, most of the reports present results which
are limited in both the cycle number and rate capability. To the
best our knowledge, our material has shown the best cycle stability
during long-term test.
Because of the above mentioned high discharge rate perfor-
mance, the material was then tested at high charge current. Fig. 6
shows thedelivered capacities of Li[Li0.2Mn0.56Ni0.16Co0.08]O2 elec-
trodes char
cut-off volt
in the 1st, 3
From Fig. 6
charge capa
and 145.4m
values are o
ing process
Fig. 6. Cycling performance of Li[Li0.2Mn0.56Ni0.16Co0.08]O2 electrodes subjected to
continuous cycling at different rates (0.2C, 1C, 5C and 20C). Charged and discharged
at the same rate. The tests were carried out in the voltage range between 2.5V and
4.8V at 20 ◦C. The low rate test date (0.2C) is referred to the upper cycle number
scale. The charge efficiency during the cycle test at 0.2C is also reported.
Table 2
Capacity of Li[Li0.2Mn0.56Ni0.16Co0.08]O2 electrodes charged and discharged at dif-
ferent rates.
Cycle Discharge capacity (mAhg−1)
0.2C 1C 5C 20C
1st 266.8 233.6 191.3 145.4
30th 223.1 201.7 168.4 118.2
th
th
ot st
acity delivered by the electrode charged at 20C was 54.5%
delivered by the electrode tested at 0.2C. This latter value is
ally coincident with the result of Fig. 5. After 30 cycles, the
al maintained the similar capacity of 223.1mAhg−1 for the
Fig. 7. Cycling C and 20C. The test was carried out in the voltage range between 2.5V and
4.8V at 20 ◦C. due to a temperature increase (from 20 ◦C to 25 ◦C), which affected all cells
under test.
ged and discharged at the same current rate within the
age of 2.5V and 4.8V (20 ◦C). The delivered capacities
0th, 100th, and 300th cycles are also listed in Table 2.
, it is seen that the electrodes achieved first cycle dis-
cities of 266.8mAhg−1, 233.6mAhg−1, 191.3mAhg−1
Ahg−1 at 0.2C, 1C, 5C and 20C, respectively. These
nly slightly lower than those obtained with the charg-
at 0.1C (Table 1), thus indicating that the charge rate
100
300
does n
the cap
of that
practic
materi
performance of a Li[Li0.2Mn0.56Ni0.16Co0.08]O2 electrode cycled at, alternatively, 0.1
The anomalous capacity behavior recorded between the 60th and the 80th cycles is
209.4 181.5 148.9 100.3
161.0 132.5 87.2
rongly affect the material performance. Furthermore,
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J. Li et al. / Journal of Power Sources 196 (2011) 4821–4825 4825
low 0.2C rate, but got even a little more for the high C-rate like 1C,
5C and 20C. Then, it is expected that this material is not only useful
for high rate discharging, but also for high rate charging. As already
pointed out, the unsatisfying performance here is still the capacity
decrease during the initial cycles independent on the current rate.
The long-term fading phenomenon after the 30th cycle, espe-
cially seen in the high rate test appeared however, to be associated
with kinetics rather than degradation. Fig. 7 shows the capacity vs.
cycle number behavior of a Li[Li0.2Mn0.56Ni0.16Co0.08]O2 electrode
subjected to consecutive set of cycles at low (0.1C) and high (20C)
charge and discharge rates. This double rate test was performed by
charging anddischarging the electrode at 0.1C for 5 cycles, and then
at 20C (both charge and discharge) for the next ten cycles. The test
wasperformedwithin the voltage rangebetween2.5Vand4.8V, by
repeating the steps for several times. Considering only the low rate
cycles, it is seen that the electrode behaved very similarly to the one
reported in Fig. 6. It delivered 263.9mAhg−1 at the 5th cycle with
only a small decrease (261.7mAhg−1) at the 16th cycle, i.e., after
ten cycles at 20C. In practice, the high rate cycling did not affect
much the capacity fading of the material at low rate. As a matter of
fact, the electrode reached the steady-state conditions after 35 low
rate cycles with a stable delivered capacity of 225mAhg−1 (0.1C).
The delivered capacity during the high rate cycling also shows the
same behaviors as the electrode cycled at high rate only (see Fig. 6).
However, th
stable trend
cates that i
a degradati
composite e
cycling. It a
material can
ible current
4. Conclus
The laye
successful s
shows the
originating
are homoge
to be very h
rial.
The high
and good ra
at 0.2
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