Intercalation materials for lithium rechargeable batteries

Intercalation materials for lithium rechargeable batteries

SOLID STATE ELSEYIER Solid State Ionics 86-88 Intercalation materials for lithium rechargeable D. Rahner”, Dresden University IONICS (1996) 891...

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SOLID STATE ELSEYIER

Solid State Ionics 86-88

Intercalation

materials for lithium rechargeable

D. Rahner”, Dresden

University

IONICS

(1996) 891-896

S. Machill, H. Schlijrb, K. Sky,

of Technology,

Institute of Physical Chemistry

batteries

M. Klo13, W. Plieth

and Electrochemistry,

D-01062

Dresden,

Gemany

Abstract In this contribution an overview will be given about the intercalation materials both for the negative and positive electrode of lithium batteries in comparison with results of our own research. Besides lithium metal as a negative electrode, interest is focused on insertion materials based on aluminium alloys. In the case of the positive electrode metal-oxides, those based on manganese, nickel and cobalt are discussed. Keywords:

Intercalation

materials;

Lithium battery;

Electrode

1. Introduction

oxides, lithium ommended.

The realization of rechargeable lithium batteries with sufficient capacity requires an improvement in the cycleability of the negative and the positive electrode. However, using lithium in secondary batteries is not without problems. High energy densities could only be observed in secondary batteries with pure lithium as the anode material. During charging, lithium is often deposited in a dendritic form. A possibility for improving the cycleability of lithium batteries is the “swing” concept or the “lithium ion battery” concept, which accords with the following reaction scheme Li(Me,C)tiLi’(oxide)

+ e-

This type of intercalation battery demands excellent host materials concerning the insertion/reinsertion of lithium and lithium ions. For the negative electrode, intercalation materials based on carbon or lithium alloys are used and for the positive electrode metal *Corresponding

author.

0167-2738/96/$15.00 Copyright PII SO167-2738(96)00202-O

01996

spinels

in particular

have been rec-

2. Anode materials The cycleability of the lithium electrode can be improved by the use of lithium-inserting substrates. The most common materials are lithium-carbon and lithium-aluminium. Other suitable alloying substrates are Sn, Pb, Bi, Sb, As and others. The anodes based on LiAl alloys can be cycled up to 1000 times, depending on the cycling conditions. One should emphasize that the depth of discharge (DOD) reaches only 1 to 10% of the value of the comparable primary lithium batteries. Using substrate forming alloys or intercalation compounds with lithium, the reactivity against the electrolyte or the solvent can be decreased. Therefore, the lithium in the host material will be “shielded” and the formation of dendrites will be reduced or avoided if the diffusion velocity inside the host material is high enough. However, a po-

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892

D. Ruhner et al. / Solid Stute Ionics 86-88

tential shift occurs and leads to a decrease in the energy and power density. For some purposes, the increase in cycleability compensates for these disadvantages. The diffusion of lithium in the alloy matrix determines the charge/discharge rate of the battery and limits its use as a low or high rate cell. The diffusion process itself is determined by the nature of the host material and its morphology. The main problems of lithium alloy electrodes are connected with the significant differences in volume between the pure basic material and the formed lithium alloy. Therefore, during cycling, mechanical stress and cracks are induced by these volume differences (LiAl 96.8% [l] in relation to the host lattice). In the case of carbon, the volume difference during the formation of LiC, is only 9.4% [2]. Carbon has therefore been the most favoured host material in recent years.

2.1. Insertion

into carbon

Carbon is a low cost material for the battery industry. Many different kinds of carbonaceous materials have been developed, such as graphite, coke or carbon fibre materials [3]. Due to its layered structure, it can insert lithium according to the following scheme: xLi + 6CeLi,C, with O
(1996) 891-896

properties that have been based on lithium metal. 2.2. Insertion

into aluminium

displayed

by batteries

alloys

Alloys have been under investigation since Dey in 1971 [6] demonstrated the possibility of electrochemical alloying with lithium in organic electrolytes. The use of alloys as the negative electrode is based on the reversible insertion of lithium into the host material in accordance with the reaction xLi+ + Al + xe-ttLi,Al. Anodes of this alloy can be cycled many times, without side reactions such as the rapid decomposition of the organic electrolyte or dendrite formation. However, the anode is covered by a fairly stable, thin, passivating layer [7]. As in the case of lithium, the structure of the thin passivating surface layer is also strongly influenced by the composition of the electrolyte solution. Many researchers described the positive effect obtained by adding small amounts of organic or inorganic compounds. Recently, we studied the effect of dilithiumphthalocyanine on cycling efficiency, cycle life and corrosion behaviour of different anodes in 1 M LiClO,-propylene carbonate solution [8]. It was shown by electrochemical impedance spectroscopy and current-potential measurements that the addition of dilithium-phthalocyanine reduces the thickness of the surface layer. Probably, the freshly deposited lithium is either not as reactive or a modified film with enhanced migration properties for lithium ions is growing. In the case of lithium-aluminium alloy anodes, the addition of dilithium-phthalocyanine has a positive influence on long term cycling (Fig. lb). In the electrolyte without additive, “normal” behaviour of the aluminium electrode is observed (Fig. la). In the absence of an additive, the overvoltage increases during cycling due to a hindered lithium transport through the formed surface film. After about 80 cycles the lithium transfer is blocked and the aluminium electrode stops working as an insertion material. In the electrolyte with an additive, a

D. Rahner et al. I Solid State Ionics 86-88

0

5M

Iwo

1500

2m

25w

Time [sl

Fig. 1. (a) Galvanostatic cycling behaviour of an aluminium substrate in proplylene carbonate-l M LiClO, solution without additive. (b) Galvanostatic cycling behaviour of an aluminium substrate in propylene carbonate-l M LiC10,-10-2 M dilithiumphthalocyanine solution.

modified surface film is obviously growing on top of the aluminium surface. This film shows no changes in its properties, however, a small overvoltage is observed during subsequent cycling. The layer is not a hindrance for the transfer of lithium in the aluminium host material. It seems that the combination of lithium alloys and dilithium-phthalocyanine gives a synergetic improvement in the lithium cycleability. The change in volume due to changes in the morphology of LiAl and other Li,Me alloys (Me=

(1996) 891-896

893

metal) is the central problem in the development of rechargeable negative electrodes for lithium cycling. Attempts have been made to avoid this problem by creating “dimension-stable” alloying electrodes in such a way that (i) small particles of the active phase of LilMe are embedded in a stabilizing matrix [9,10] or (ii) the aluminium host previously formed an alloy with other metals that are soluble in aluminium or form intermetallic compounds with it, but do not form alloys with lithium, e.g., nickel. In this way one creates an alloy matrix of modified grain size with stabilizing properties towards “mechanical stressing” during charge/discharge processes of lithium [11,12]. Therefore, the suitability of different binary AlNi, Al-Mn and Al-Be alloys as anode substrates in rechargeable lithium batteries have been tested, compared with pure aluminium. The changed composition by alloying of aluminium with a second metal does dramatically influence the mechanical properties and the electrochemical behaviour. On the other hand, the electrochemical properties of these substrates are also determined by the macro- and microstructure. In particular, the eutectic mixture of Al-N1 (Al/Al,Ni) seems to be an interesting substrate material in rechargeable lithium batteries. The Al,Ni phase does not form an alloy with lithium and acts only in the improvement of the mechanical stability. The second phase of pure aluminium can receive the incorporated lithium. We investigated some different qualities of this eutectic mixture. By fast quenching one gets very finely spread segregations of the Al,Ni phase. A direct heat flow (vertical Bridgeman method) leads to a directionally solidified rodlike Al-Al,Ni eutectic. This directionally solidified eutectic consists of an Al matrix of faceted Al,Ni rods grown into it nearly parallel to each other and in the direction of heat flow. The usefulness of a new anode material can be examined only under real conditions. The consumer is interested in a maximum number of charge/discharge cycles with highest power density, if possible. Fig. 2 presents a set of typical cycling curves of an aluminium substrate. The cycling efficiency was estimated to be 88% under the conditions used (DOD: 10%). The reversible behaviour is lost for

894

D. Raker

et d.

/ Solid State Innics 86-X8

(1996) 891-896

formed by an alternating arrangement of two double chains and one single chain of MnO, octahedrons. The reversibility of the lithium intercalation into MnO, depends on the degree of discharge. xLi+ + MnO, + xe-wLi,MnO,

-I 0

5co

Km

1500

2crQ

25RJ

3001, 3m

4m

4500

mx

Time [s] Fig. 2. Galvanostatic

Fig. 3. Average

cylcling

cycling

of an aluminium

efficiency

substrate.

of various substrates.

cycle numbers much larger than 100. Comparable curves were obtained with the other substrates. With an increasing content of manganese or nickel, the cycling efficiency decreases dramatically (Fig. 3).

3. Cathode materials 3. I. Lithium-manganese

oxides

Manganese dioxide is an interesting material for battery applications. In principle it is suitable for the intercalation of small ions (H+, Li+) and it is also non-polluting and readily available. It inexpensive, occurs in various modifications, among them the most used for industrial purposes is y-MnO,, which can be synthezised either chemically (CMD-MnO,) or electrochemically (EMD-MnO,). This oxide is characterised by a tunnel-structure

(0
In y-MnO,/Li cells the lithium insertion during discharge occurs mainly into the (2 X 1) tunnels. The intercalation of Li + into the (1 X 1) tunnels leads only to a ratio of 0.2 Li’/Mn in these domains. A higher lithium intercalation causes a change of the (1 X 1) domains into a [Mn,]O,-spinel-type lattice [13]. The original lattice is destroyed and cannot be renewed during recharge. However, the spinel-type lattice shows a more or less reversible Li + intercalation. For practical purposes this is insufficient, however, the properties of manganese dioxide described above have lead to concerted efforts to synthezise MnO,-forms that could be suitable in secondary lithium batteries. That the spine1 form is a lithium insertion compound was lirst shown by Hunter [14], who has reported the extraction of lithium from LiMn,O, by acid treatment. The resulting material was identified as A-MnO,, where the [Mn,O,] framework remains as a spine1 structure and allows the intercalation and deintercalation of Li+ ions. Therefore, the lithium spine1 Li[Mn,O,] is of great interest in the system Li-0-Mn. The transport places in the of Li+ is achieved at interstitial [Mn,]O, sublattice. The spine1 itself is stable over a wide range of stoichiometry Li,TIMn,O,] (0~x12). Starting from the LiMn,O, phase, one has two possibilities: (i) intercalation of a second Li+ gives the composition 1
D. Rahner et al. I Solid State Ionics 86-88

crystal symmetry from cubic to tetragonal. The width of this two-phase domain (characterized by a flat discharge curve) allows cycling in the composition range 1.1 x>OS and in the second step between os>x>o. Fig. 4 shows the cycling behaviour of Li,Mn,O,. The two intercalation processes of lithium are clearly visible. Investigations in the area of 3.5-4.5 V show the good reversibility of the spine1 in this potential region and the electrolyte stability up to 4.5 V (Fig.

895

(1996) 891-896

I

08 0.6 t

34

3.6

3.8

4.0 Potential

42

44

46

48

vs. Li IV]

Fig. 5. Cycling behaviour of the Li-Mn spine1 described in the high voltage area, sweep rate 10 pV/s.

in Fig. 4

5). Although the spinel-type manganese oxide is very promising, there are a lot of investigations being undertaken in order to improve the stability of the structure by doping with metal-ions like Ni, Co, Fe, Mg or Zn [ 171. The complete exchange of manganese by nickel or cobalt leads to a layered structure of the Li-metal oxides. 3.2. Layered lithium-metal

oxides

alternating layers of octahedral sites in a cubic, close-packed, lattice of oxygen ions. The compounds Li,_,NiO, (0~~50.5) and Li, _CoO, (0~~~0.5) are suitable cathode materials for 4 V rechargeable lithium cells using a carbon anode (“lithium ion” battery). The cell reaction in the C/LiMeO, systems can be summarized by the following electrochemical process: LiMeO,

Lithiated nickel and cobalt oxides of the general formula LiMeO, (where Me=Ni, Co or Ni/Co) are insertion compounds for high-voltage lithium batteries. These materials possess a layer structure where lithium and the transition metal ions fill

+ 6CwLi,

2.0

2.5

30

3.5

4.0

45

50

U vs. Li [VI

Fig. 4. Cyclic voltammogram of Li,Mn,O, (low temperature synthesis) in propylene carbonate-l M LiClO,, sweep rate 50 PVIS.

+ Li,C,

.

Broussely et al. [ 181 investigated the mechanism of Li insertion/reinsertion by cyclic voltammetry. This mechanism is quite different for nickel and for cobalt oxide. The first charge and discharge curve of a LiNiO, cathode is totally different from subsequent cycles. The Li from LiNiO, cannot be fully inserted during the subsequent reduction step due to a structural transformation to Li,_.NiO,. After a few cycles, the reversible reaction (shown in Fig. 6) can be described as follows: Li,,,SNiO,t+Li

-2.0’ 1.5

_.MeO,

oXsNiO, + O.SLi+ + 0.5e

The practical specific capacity of Li-Ni oxides is about 125-150 mAh/g [l&19]. Contrary to these observations, in the case of LiCoO,, the lithium after the first charging process is completely inserted during the following discharge process [18]. The overall reaction of the LiCoO, charge/discharge is LiCoO,&i,

,CoO,

+ 0.5Li+ + 0.5e-

896

D. Rahner et al. I Solid State lonics 86-88

2.0 1

1 -6th

cycle

(1996) 891-896

den, for the preparation of the directionally rodlike Al-Al,Ni eutectic mixtures.

solidified

-----7thcycle 1.0

t

..... 8thcycle

References

I

I

30

35

Potential

Fig. 6. Cyclic voltammogram of synthesis) in propylene carbonate-l mV/s.

40

I

45

vs. Li [VI

LiNiO, (high temperature M LiCIO,, sweep rate 0.1

Practical specific capacities of LiXCoO, cathodes correspond to the capacity range of the Li-Ni materials. Both compounds show a very pronounced plateau in the charge and discharge curve. The Li-Ni and Li-Co oxides possess a high structural stability in the voltage range investigated (4.1-3.0 V). This is the reason for the good reversibility of the charging/ discharging process. However, it seems that the price (6 $/kg for LiNiO, and 48 $/kg for LiCoO, [20]) and the resources of nickel and cobalt could limit its worldwide use in secondary batteries. From these considerations, one believes the Li-Mn spinels, in combination with carbon, may be the most promising systems for rechargeable lithium batteries.

Acknowledgments Financial support from the “Deutsche Forschungsgemeinschaft” and the “Bundesministerium fur Bildung und Forschung” is gratefully acknowledged. The authors would like to thank Dr. W. Loser, Institut fur Festkiirper- und Werkstofforschung Dres-

[l] D. Billaud, E. MacRae and A. Herold, Mat. Res. Bull. 14 (1979) 857. [2] D. Fauteux and R. Koksbang, J. Appl. Electrochem. 23 (1993) 1. [3] C. Liebenow, M.W. Wagner, K. Liihder, P. Lobitz and J.O. Besenhard, J. Power Sources 54 (1995)369. [4] B. Scrosati, in: The Electrochemistry of Novel Materials, eds. J. Lipkowski and P.N. Ross (VCH Publishers, New York, 1994) pp. 111-140. [S] M. Inaba, H. Yoshida, Z. Ogumi, T. Abe, Y. Mizutani and M. Asano, J. Electrochem. Sot. 142 (1995) 20. [6] A.N. Dey, J. Electrochem. Sot. 118(1971) 1547. [7] A. Cisak and L. Werblan, High-Energy Non-Aqueous Batteries (Polish Scientific Publishers PWN, Warszawa, 1993). [8] S. Machill and D. Rahner, in: Power Sources, Vol. 15, International Power Sources Symposium Committee, eds. A. Attewell and T. Keily (Brighton, 1995) p. 471. [9] J.O. Besenhard, M. Hess and P. Komenda, Solid State Ionics 40-41 (1990) 525. [lo] B.A. Boukamp, G.C. Lesh and R.A. Huggins, J. Electrothem. Sot. 128 (1981) 725. [I I] I. Hauke, S. Machill, D. Rahner and K. Wiesener, J. Power Sources 43-44 ( 1993) 42 I. [12] R.V Moshtev, P. Zlatilova, B. Puresheva, V. Manev and A. Kozawa, J. Power Sources 51 (1994) 99. [13] W.I.F. David, M.M. Thackeray, P.G. Bruce and J.B. Goodenough, Mat. Res. Bull. 19 (1984) 99. [14] J.C. Hunter, J. Solid State Chem. 39 (1981) 142. [15] M.M. Thackeray, W.I.F. David, P.G. Bruce and J.B. Goodenough, Mat. Res. Bull. 18 (1983) 461. [ 161 J.M. Tarascon, E. Wang, F.K. Shokoohi, W.R. McKinnon and S.J. Colson, J. Electrochem. Sot. 138 (1991) 2859. [17] R.J. Gummow, A. de Kock and M.M. Thackeray, Solid State Ionics 69 (1994) 59. [18] M. Broussely, F. Perton, J. Labat, R.J. Staniewicz and A. Romero, J. Power Sources, 43-44 (1993) 209. [19] RV. Moshtev, P. Zlatilova, V. Manev and A. Sato, J. Power Sources 54 (1995) 329. [20] K. Brandt, J. Power Sources 54 (1995) 151.