# High Cycling Performance Cathode Material: Interconnected LiFePO4/Carbon Nanoparticles Fabricated by Sol-Gel Method

Authors: Zhigao Yang; Shengping Wang
Journal: Journal of Nanomaterials
 (2014)

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## Abstract

Interconnected LiFePO4/carbon nanoparticles for Li-ion battery cathode have been fabricated by sol-gel method followed by a carbon coating process involving redox reactions. The carbon layers coated on the LiFePO4 nanoparticles not only served as a protection layer but also supplied fast electrons by building a 3D conductive network. As  a cooperation, LiFePO4 nanoparticles encapsulated in interconnected conductive carbon layers provided the electrode reactions with fast lithium ions by offering the lithium ions shortening and unobstructed pathways. Field emission scanning electron microscopy (FESEM) and X-ray diffraction (XRD) tests showed optimized morphology. Electrochemical characterizations including galvanostatic charge/discharge, cyclic voltammetry (CV), and electrochemical impedance spectroscopy (EIS) tests, together with impedance parameters calculated, all indicated better electrochemical performance and excellent cycling performance at high rate (with less than 9.5% discharge capacity loss over 2000 cycles, the coulombic efficiency maintained about 100%).


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## Body

## 1. Introduction

Reported by Goodenough and coworkers for the first time in 1997, the phosphate polyanionic compound of LiFePO4 shows superior performance including a high theoretical capacity (170 mAh g−1) and an acceptable operating voltage (3.45 V versus Li+/Li) [1, 2]. However, the slow diffusivity of Li+ in LiFePO4 (ca. 10−14 cm2 s−1) and the low electronic conductivity (ca. 10−9 S cm−1) [3] restrict the high rate performance of LiFePO4. Generally, carbon coating, nanocrystallization, and doping are main techniques to modify LiFePO4. Although doping improved the performance of LiFePO4 in some researches, the mechanism had not been clearly explained yet. Furthermore, there are some problems about the balance of charge and energy raising after doping to be taken into further consideration [4, 5]. Carbon coating can significantly improve the electrical conductivity [6–8] and reduce particle size as well as avoiding particle aggregation [9], nanocrystallization shortening the pathway of Li+ [10], and mitigating the problem of slow Li+ transport in the solid state. Thus, aiming at improving the low conductivity and slow diffusivity of Li+ at the same time, many modification researches are conducted based on the combination of carbon coating (or carbon-decorating) and nanocrystallization [6, 11, 12]. However, the high surface energy of nanosized materials causes the problem of agglomeration, making the efforts of fabricating nanomaterials in vain [13]. This warns us that the carbon coating process should better take place accompanying the formation of nanoparticles or their precursors. Heterogeneous distribution of carbon and LiFePO4 results in limited utilization of the LiFePO4 active material [14], which emphasizes the importance of the quality of carbon layer (including the integrity, uniformity, and thickness). In order to make full use of the synergistic effect of carbon coating and nanocrystallization, structure of complete and uniform carbon layer coated on every single LiFePO4 nanoparticle is highly desirable [15, 16]. For us, that means only a carbon coating process which happens during the formation of LiFePO4 (or LiFePO4 precursor) nanoparticles and resulting uniform, compact, and intact carbon layers can notably enhance the electrochemical performance of LiFePO4 nanoparticles (especially the cycling and rate performances).The interconnected LiFePO4/carbon nanoparticles reported here possess the target structure (structure of complete and uniform carbon layer coated on every single LiFePO4 nanoparticle) and exhibit commendable cycling performance at high rate.


## 2. Experimental

### 2.1. Fabrication of Bare LiFePO4

The raw materials (all the chemical reagents used were obtained from Sinopharm Chemical Reagent Co., Ltd, China) for synthesizing the LiFePO4 are P2O5, LiCl, and FeSO4·7H2O. With continuous stirring, 7.0970 g (0.05 mol) of P2O5 was dissolved into 50 mL absolute ethyl alcohol to form solution A, and 4.4621 g (0.1 mol) of LiCl was dissolved into 100 mL absolute ethyl alcohol to form solution B. After 27.8020 g (0.1 mol) of FeSO4·7H2O was added into 100 mL absolute ethyl alcohol, solution A and solution B were added into it with the volume ratio of 1 : 2 while stirring. Then the solution was covered with plastic film and stirred for 3 hours to form a uniform sol. After stirring in the 65°C water bath without plastic film for several hours, the gel was formed. Finally, sucrose (A reducing atmosphere was created by thermal decomposition of the sucrose at the upstream) and as-prepared gel were put in a magnetic boat with the mass ratio of 1 : 10 to undergo the calcining process at 700°C in argon atmosphere for 8 hours. The heat rate was 10°C min−1 before 400°C and then 2°C min−1 to 700°C.


### 2.2. Fabrication of LiFePO4/Carbon Composite (LiFePO4/C)

All the experimental procedures did not change until the formation of a uniform sol. After forming the sol, 4.4 mL of aniline was added into the sol, followed by another stirring and reaction process for 3 hours. During this process, the redox reaction for coating polyaniline took place. The parameters of the solvent evaporation and heat treatment processes did not change either.


### 2.3. Characterizations

The phase structure of the products was determined by powder X-ray diffraction on a Bruker AXS D8-FOCUS diffractometer with Cu Kα radiation. The morphology and particle sizes were observed by field emission scanning electron microcopy (FDAC SU8010). Thermogravimetry/differential scanning calorimetry curves were obtained using STA 449F3 analyzer (NETZSCH) in the temperature range of 30~1000°C, using alumina crucible under nitrogen atmosphere and heating rate of 10°C min−1.


### 2.4. Electrochemical Measurements

Test cells were fabricated utilizing active materials (LiFePO4 and LiFePO4/C) with acetylene black and polyvinylidene difluoride (PVDF) as the working electrode. Active material (85 wt.%), acetylene black (10 wt.%), and PVDF binder (5 wt.%) were dispersed in N-methyl-2-pyrrolidinone (NMP) solvent and ground thoroughly to form a slurry. Then the slurry was spread onto aluminum foil and maintained at 65°C in oven overnight. Metallic lithium plate was used as the counter electrode. The long-term galvanostatic charge/discharge was evaluated with an Arbin BT2000 multichannel galvanostat in the potential range of 2.5~4.2 V (versus Li/Li+) at current densities of 34 mA g−1 and 850 mA g−1 (0.2 C and 5 C). CV and EIS were conducted on a Vmp3 (Biologic) electrochemical workstation. CV tests were done between 2.5 and 4.2 V (versus Li/Li+) at the scan rate of 0.5 mV s−1. EIS measurements were carried out over a frequency range of 105~10−2 Hz using a sine wave of 5 mV.


## 2.1. Fabrication of Bare LiFePO4

The raw materials (all the chemical reagents used were obtained from Sinopharm Chemical Reagent Co., Ltd, China) for synthesizing the LiFePO4 are P2O5, LiCl, and FeSO4·7H2O. With continuous stirring, 7.0970 g (0.05 mol) of P2O5 was dissolved into 50 mL absolute ethyl alcohol to form solution A, and 4.4621 g (0.1 mol) of LiCl was dissolved into 100 mL absolute ethyl alcohol to form solution B. After 27.8020 g (0.1 mol) of FeSO4·7H2O was added into 100 mL absolute ethyl alcohol, solution A and solution B were added into it with the volume ratio of 1 : 2 while stirring. Then the solution was covered with plastic film and stirred for 3 hours to form a uniform sol. After stirring in the 65°C water bath without plastic film for several hours, the gel was formed. Finally, sucrose (A reducing atmosphere was created by thermal decomposition of the sucrose at the upstream) and as-prepared gel were put in a magnetic boat with the mass ratio of 1 : 10 to undergo the calcining process at 700°C in argon atmosphere for 8 hours. The heat rate was 10°C min−1 before 400°C and then 2°C min−1 to 700°C.


## 2.2. Fabrication of LiFePO4/Carbon Composite (LiFePO4/C)

All the experimental procedures did not change until the formation of a uniform sol. After forming the sol, 4.4 mL of aniline was added into the sol, followed by another stirring and reaction process for 3 hours. During this process, the redox reaction for coating polyaniline took place. The parameters of the solvent evaporation and heat treatment processes did not change either.


## 2.3. Characterizations

The phase structure of the products was determined by powder X-ray diffraction on a Bruker AXS D8-FOCUS diffractometer with Cu Kα radiation. The morphology and particle sizes were observed by field emission scanning electron microcopy (FDAC SU8010). Thermogravimetry/differential scanning calorimetry curves were obtained using STA 449F3 analyzer (NETZSCH) in the temperature range of 30~1000°C, using alumina crucible under nitrogen atmosphere and heating rate of 10°C min−1.


## 2.4. Electrochemical Measurements

Test cells were fabricated utilizing active materials (LiFePO4 and LiFePO4/C) with acetylene black and polyvinylidene difluoride (PVDF) as the working electrode. Active material (85 wt.%), acetylene black (10 wt.%), and PVDF binder (5 wt.%) were dispersed in N-methyl-2-pyrrolidinone (NMP) solvent and ground thoroughly to form a slurry. Then the slurry was spread onto aluminum foil and maintained at 65°C in oven overnight. Metallic lithium plate was used as the counter electrode. The long-term galvanostatic charge/discharge was evaluated with an Arbin BT2000 multichannel galvanostat in the potential range of 2.5~4.2 V (versus Li/Li+) at current densities of 34 mA g−1 and 850 mA g−1 (0.2 C and 5 C). CV and EIS were conducted on a Vmp3 (Biologic) electrochemical workstation. CV tests were done between 2.5 and 4.2 V (versus Li/Li+) at the scan rate of 0.5 mV s−1. EIS measurements were carried out over a frequency range of 105~10−2 Hz using a sine wave of 5 mV.


## 3. Results and Discussion

Figure1(a) shows the 2nd cycle of galvanostatic charge/discharge curves of LiFePO4 and LiFePO4/C at 0.2 C. The LiFePO4 delivered a capacity of 102.2 mAh g−1, while the LiFePO4/C delivered a capacity as high as 117.1 mAh g−1 with a coulombic efficiency of 99.2%. The relative low specific capacity was calculated based on the composite of LiFePO4 and carbon and could be explained by the high carbon content (~18.6%) of LiFePO4/C obtained from the comparison of TG/DSC curves of LiFePO4 and LiFePO4/C shown in Figure 2 (the carbon content of our LiFePO4/C was calculated from weight loss of the composite and this method was also reported by Lee et al. [17]). It is obviously showed that, comparing to LiFePO4, the longer platforms of charge/discharge curves of LiFePO4/C are almost parallel to each other from the beginning to the end, and the difference between the voltages of platforms is also much smaller, which represented better reversible performance, indicating decreased polarization. Electrochemical polarization was decreased because of fast electrons provided by carbon layers of high quality. Controlled particle size offered short diffusion distance for Li+ in the solid state and large specific surface areas with abundant active sites for Li+ to intercalate or deintercalate and concentration polarization was decreased in this way. With better reversible performance, the cycling performance of LiFePO4/C is also notable even at high rate (5 C). As shown in Figure 1(b), with less than 9.5% discharge capacity loss over 2000 cycles, the coulombic efficiency maintained about 100%. The excellent cycling performance of our LiFePO4/C is comparable with many other reports [15, 18, 19] and is closely associated with the structure produced by the carbon coating step involving redox reactions during the sol-gel process. The carbon coating process took place when the sol formed, as shown in Figure 3. After all the raw materials except aniline were mixed together and stirred for several hours, a uniform sol was formed. As there is O2 in the air, amounts of ferrous ions were oxidized to ferric ions inevitably. The ferric ions were adsorbed to the surface of sol molecules due to the adsorption nature (the adsorption of charge particles) of sol. As a result of electrostatic interaction, all the ferric ions adsorbed distributed on the surface of the sol molecules uniformly and densely (state A). The polymerization of aniline is an oxidation process and ferric ions on the surface of sol molecules act as active sites for this oxidation reaction because the reduction process of ferric ions can coordinate with the oxidation process. That is to say the active sites for polymerization of aniline distributed on the surface of the sol molecules uniformly and densely. Aniline molecules have equal possibility to polymerize at anywhere on the surface of the sol molecules (state B). Thus, uniform, compact and intact polyaniline layers can be obtained by the cooperation between the polymerization of aniline (the oxidation process) and the reduction of ferric ions (state C). Finally, the same uniform, compact, and intact carbon layers coated on every single LiFePO4 particle can be obtained after the calcining process (state D), instead of carbon layer with several agglomerated LiFePO4 particles inside (state E) due to agglomeration caused by the high surface energy of the nanosized particles [13] or LiFePO4 particles partially coated by carbon.(a) Discharge/charge voltage profiles cycled at the 2nd cycle of LiFePO4 and LiFePO4/C at a current density of 34 mA g−1 (0.2 C). (b) Cycling performance of interconnected LiFePO4/C nanoparticles at a current density of 850 mA g−1 (5 C).
(a)
(b)Figure 2
TG/DSC curves of LiFePO4 and LiFePO4/C.Figure 3
Scheme of formation process of interconnected LiFePO4/C particles.The FESEM picture shows irregular morphology of LiFePO4 particles (Figure 4(a)). Although there are some particles with the size of ~50 nm, these particles are not independent, but parts of much larger clusters and truly independent particles are not smaller than 500 nm. Comparing with LiFePO4, the particles of LiFePO4/C composite become much smaller and this huge change of morphology is mainly caused by the obtained carbon layers of high quality, which restrict the growth of LiFePO4 and avoid the agglomeration of bare LiFePO4 nanoparticles. As shown in Figure 4(b), with the size of ~50 nm, LiFePO4/C nanoparticles interconnect with each other compactly, forming 3D continuous conductive structure. This is the very structure desired, which is shown as state D in Figure 3. In this optimized structure, electrons from multidimension can reach the LiFePO4 particles immediately. The sluggish diffusion of Li+ in the solid state accelerated as a result of the shortened diffusion distance in smaller particles.FESEM micrographs of samples: (a) SEM micrographs of LiFePO4 and (b) SEM micrographs of LiFePO4/C.
(a)
(b)The crystallographic structure determined by XRD further confirmed the smaller particle size after carbon coating. As shown in Figure5, the widths of the major diffraction peaks turn to be bigger after carbon coating, indicating smaller particle size of LiFePO4/C (according to Scherrer’s formula). This phenomenon which is consistent with FESEM observations affirmed the main functions of the carbon layers, namely, the function of controlling particle size and avoiding agglomeration. From XRD patterns of the obtained LiFePO4 and LiFePO4/C, we can also see that all dominant diffraction peaks of LiFePO4 and LiFePO4/C samples can be indexed to orthorhombic LiFePO4 (JCPDS card number 40-1499), indicating a perfect crystallinity of the as-synthesized samples. Besides, there is no evidence for the formation of amorphous carbons for the LiFePO4/C.Figure 5
XRD patterns of LiFePO4 and interconnected LiFePO4/C particles.As shown in Figure6(a), a couple of redox peaks were observed for both LiFePO4 and LiFePO4/C in the CV curves obtained at a scan rate of 0.5 mV s−1. Compared to LiFePO4, the smaller peak potential difference of LiFePO4/C indicates better reversibility, which is brought about by the decreased polarizations just mentioned (Figure 1(a)). Much higher peak currents are also shown, indicating faster reaction rate of LiFePO4/C, and further confirmed the advantage of the interconnected structure, which provided electrode reactions of fast electrons and Li+. Figure 6(b) presents the typical EIS responses of LiFePO4 and LiFePO4/C. Both of the Nyquist plots are composed of a depressed semicircle in the high-frequency region followed by a slanted line in the low-frequency region.Electrochemical measurements of prepared samples: (a) CV curves of LiFePO4 and the interconnected LiFePO4/C nanoparticles in a voltage range of 2.5~4.2 V at a scanning rate of 0.5 mV s−1. (b) Comparison of impedance spectra of LiFePO4 and LiFePO4/C.
(a)
(b)Referring to reported methods [20] and based on our EIS measurements, impedance parameters were calculated and listed in Table 1. The equivalent circuit diagram is shown in Figure 7.Table 1
Impedance parameters of the samples.
Samples
R
e/Ω
R
ct/Ω
C
d
/F
σ
ω/Ω cm2 s−0.5
D/cm2 s−1
σ/S cm−1
i
0/mA cm−2
LiFePO4/C
9.3
41.3
2.2
×
10
-
4
23.2
1.4
×
10
-
11
3.0
×
10
-
4
6.2
×
10
-
4
LiFePO4
10.5
488.2
3.7
×
10
-
7
946.2
8.3
×
10
-
15
2.5
×
10
-
5
5.3
×
10
-
5Figure 7
Equivalent circuit diagram used in the calculation of impedance parameters.The Warburg coefficientσ
ω can be obtained by
(1)
Z
r
e
=
R
e
+
R
ct
+
σ
ω
ω
-
0.5
,
where R
e is the resistance of the electrolyte, R
ct is the charge transfer resistance, and ω is the angular frequency in the low-frequency region. Both R
e and R
ct are kinetic parameters independent of frequency. So σ
ω is the slope for the plot of Z
r
e versus the reciprocal root square of the lower angular frequencies (ω
-
0.5); as shown in Figure 8, the slope of the fitted line is the Warburg coefficient σ
ω.Figure 8
The relationship betweenZ
r
e and ω
-
0.5 at low frequencies for LiFePO4 and LiFePO4/C samples.The diffusion coefficient values of the lithium ions (D) can be obtained from
(2)
D
=
R
2
T
2
2
A
2
n
4
F
4
C
2
σ
2
,
where R is the gas constant (8.314 J mol−1 K−1), T is the temperature (298.5 K), A is the area of the electrode surface (2.0106 cm2), F is Faraday’s constant (96,500 C mol−1), C is the molar concentration of Li+ (1.09 mol L−1), and n is the number of electrons transferred in the electrode reactions (for LiFePO4, n
=
1).The conductivity values (σ) are calculated from
(3)
σ
=
1
R
ct
·
t
A
,
where t is the thickness of the cathode (250 μm).The values of the exchange current density (i
0) are calculated from
(4)
i
0
=
R
T
n
F
R
ct
.The double layer capacitanceC
d is determined by
(5)
C
d
=
1
ω
R
ct
.Comparing all the impedance parameters of LiFePO4/C and LiFePO4, we can see there is no big difference of R
e between the two samples, because the whole system and operation conditions were kept the same. While the values of R
ct and σ
ω changed dramatically, several orders of magnitude increases of D, σ, and i
0 were observed for LiFePO4/C. All the changes reflected from the parameters listed in Table 1 can be explained from the aspect of structure. With uniform carbon layers on every single nanoparticle, all the nanoparticles interconnected with each other, forming 3D conductive network. The value of conductivity increases because electrons can diffuse from all directions. Diffusion of Li+ in the solid state becomes much faster in nanoparticles with controlled size, leading to the increase of the diffusion coefficient value of Li+ and reduction of Warburg impedance. Both electrons and Li+ can respond to the electrode reactions immediately, minimizing the electrochemical polarization and concentration polarization. What is more, according to some research, polyaniline contains element N, which can also affect the electrochemical performance [21]. That is why the values of exchange current density increased and the charge transfer resistance decreased and our LiFePO4/C sample exhibited notable cycling performance even at high rate.Analysis based on all the parameters confirmed the results of CV and galvanostatic charge/discharge tests, which suggests that our carbon coating method is ingenious, efficient, and preferred and can result in ideal structure with carbon layers of high quality.In addition to shortening the diffusion distance of Li+, the controlled particle size can also improve the utilization of active materials. In the lattice of LiFePO4, Li+ migrates through one-dimensional channels [5, 22–24]. Cross-channel diffusion of Li-ion happens with the help of antisite defects [25, 26], but, with several immobile point defects (such as F
e
Li
•, a kind of defects: one ferrous ion occupies the lattice position of lithium ion) in a single channel, Li+ sites situated between immobile point defects cannot be reached, which causes “blocked” capacity. In very large particles most sites will be blocked by defects in this way, while the total channel length between surfaces in nanoparticles is small, resulting in channels containing very few or even zero defects. For instance, for particles smaller than 60 nm, 1% F
e
Li
• population leads to on average fewer than two defects residing in each channel and therefore no “blocked” Li+ sites [26]. For our interconnected LiFePO4/C nanoparticles with an average diameter around 50 nm, there are less immobile point defects, which minimized the “blocked” capacity and improved the utilization of active materials.Our carbon coating process is based on a couple of redox reactions following the formation of LiFePO4 sol. Owing to the redox reactions, the position of carbon layer was fixed, the thickness of the carbon layer was limited, and the uniformity of the carbon layer was guaranteed. Finally, the target structure formed. With high quality carbon layers and controlled particle size, the electronic conductivity (σ), the diffusion coefficient of Li+ (D), and the exchange current density (i
0) all increased. Obviously, for the same purpose of ensuring the homogeneous distribution of carbon, our method turns to be more convenient, more efficient, and more ingenious. Because no surfactant is used, no complex experiments operations are needed and high cycling performance mentioned above is presented.


## 4. Conclusions

In conclusion, interconnected LiFePO4/carbon nanoparticles were synthesized successfully in our work. By an ingenious, efficient, and convenient method involving a couple of redox reactions, the structure of uniform, compact, and intact carbon layer on every single LiFePO4 nanoparticle was obtained. The high quality carbon layers coated on every LiFePO4 particle not only acted as protection layers but also provided fast electrons for electrode reactions by forming 3D conductive network. The proper particle size controlled offered Li+ shorter diffusion distance, accelerating the diffusion of Li+ in the solid state. And the large specific surface area ensured the sufficient contact between the electrode material and electrolyte. Considering the existence of immobile point defects, the utilization of active materials was also improved. The synergistic effect of high quality carbon layers and controlled particle size decreased the electrochemical polarization and concentration polarization, making the reaction rate fast enough to exhibit dramatically improved electrochemical performance including remarkable cycling performance at high rate.



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*Source: 801562-2014-06-12.xml*