Open Access

Porous NASICON-Type Li3Fe2(PO4)3 Thin Film Deposited by RF Sputtering as Cathode Material for Li-Ion Microbatteries

Nanoscale Research Letters201611:365

https://doi.org/10.1186/s11671-016-1574-7

Received: 3 May 2016

Published: 17 August 2016

Abstract

We report the electrochemical performance of porous NASICON-type Li3Fe2(PO4)3 thin films to be used as a cathode for Li-ion microbatteries. Crystalline porous NASICON-type Li3Fe2(PO4)3 layers were obtained by radio frequency sputtering with an annealing treatment. The thin films were characterized by XRD, SEM, and electrochemical techniques. The chronoamperometry experiments showed that a discharge capacity of 88 mAhg−1 (23 μAhcm−2) is attained for the first cycle at C/10 to reach 65 mAhg−1 (17 μAhcm−2) after 10 cycles with a good stability over 40 cycles.

Keywords

Radio frequency sputtering Li-ion microbatteries NASICON-type Li3Fe2(PO4)3 Cathode thin film

Background

Due to remarkable properties such as excellent cycle life, high thermal resistance, no memory effect, and low self-discharge, Li-ion batteries have attracted great attention in electrochemical energy storage [13]. More recently, the miniaturization of these power sources has been investigated to meet many applications in microelectronics such as real-time clocking (RTC), radio frequency identification (RFID), sensors, medical implants, memory backup power, solar cell, and smartcards [46]. One of the major challenges in the microbattery field is related to the manufacturing process and its compatibility with the integrated circuit technology. Particularly, metallic Li which is currently used as a negative electrode is not compatible with the reflow soldering process because of its low melting point (180.5 °C). Therefore, the rocking chair technology involving stable materials must be explored. Many researches focused on the development of new components with nanostructured materials and 3D designs [711].

As potential cathode materials, the NASICON-type compounds A3Fe2(XO4)3 (A = Li, Na; X = P, As, S) with 3D frameworks like Li3Fe2(PO4)3 have attracted considerable attention [12]. NASICON-type Li3Fe2(PO4)3 can generate 2.8 V vs. Li with an excellent capacity retention, and up to 2 mol of Li+ can be reversibly intercalated into Li3Fe2(PO4)3, delivering a capacity of 128 mAhg−1. NASICON has also a relatively high ionic conductivity resulting from the disorder of lithium ions in the structure, favorable redox properties, low cost, structural stability, and simple fabrication procedures [5, 6, 12]. Many methods have been reported to synthesize Li3Fe2(PO4)3 nanostructures such as hydrothermal [13, 14], gel combustion [15], solid state [1619], solution with the use of citric acid [20], sol-gel [21], ultrasonic spray combustion [22], and ion exchange with molten salt [23, 24].

In this work, we report the fabrication of porous NASICON-type Li3Fe2(PO4)3 thin film electrodes by radio frequency sputtering. Sputtering techniques are widely employed in microelectronics for the successive deposition of thin films; they are the main process used to fabricate planar all-solid-state Li-ion microbatteries [25, 26]. To the best of our knowledge, this approach has never been applied to deposit Li3Fe2(PO4)3. We show that this material tested as a cathode reveals a good electrochemical behavior for all-solid-state Li-ion microbatteries.

Methods

Preparation of Li3Fe2(PO4)3 Thin Films

Firstly, thin films of LiFePO4 were deposited on titanium foil as substrate by radio frequency (RF) sputtering (PLASSYS). The target was LiFePO4 (purity 99.9 %, Neyco). The process was carried out in a vacuum chamber with a base pressure before deposition of 10−6 Torr. The sputtering gas was pure argon, and the working pressure was 10 mTorr with a gas flow of 21.5 sccm. A sputtering power of 150 W was applied to the target. The deposition time was 3 h. Secondly, the as-deposited thin films were annealed in air at 700 °C for 3 h with a heating rate of 10 °C min−1 (furnace: NABERTHERM Controller B 180).

Structural Characterization

Phases and crystallinity of thin films were examined by X-ray diffraction (XRD) with Cu Kα radiation (wavelength = 1.5405 Å) using a D5000 BRUKER-SIEMENS diffractometer. The morphology of the Li3Fe2(PO4)3 was investigated by scanning electron microscopy (SEM, Hitachi, S-570). Thickness measurement was performed by profilometry analysis using a DEKTAT XT (BRUKER) equipment. A portion of the sample is masked during deposition, and the thickness is given by the height of the step.

Electrochemical Measurements

The electrochemical tests of the half-cell were performed using Swagelok cell assembled in a glove box filled with purified argon in which moisture and oxygen content were less than 0.5 ppm. The half-cells consisted of metallic Li as counter electrode. Two circular sheets of Whatman glass microfiber soaked with lithium hexafluorophosphate in ethylene carbonate and diethylene carbonate (1 M LiPF6 in (EC:DEC) 1:1 w/w) were used as separator. Cyclic voltammetry measurements were performed using a Versastat potentiostat (AMETEK) in the range of 1.25–5 V vs. Li/Li+ with a scan rate of 1 mVs−1. Galvanostatic cycles were performed with a VMP3 (Bio Logic) at 25 °C between 2 and 4 V vs. Li/Li+. The different cycles of the charge/discharge rate were investigated at a kinetic rate of C/10 and C/5 considering that the theoretical capacity of Li3Fe2(PO4)3 is 128.25 mAhg−1. Hence, the applied currents were 3.3 and 6.6 μA cm−2, respectively. No additives or binder was used for all electrochemical tests.

Results and Discussion

Prior to battery assembly, the crystallinity of the thin films were examined by XRD. The XRD patterns of initial target and as-deposited sample are shown in Fig. 1. It can be seen that the target is well-crystallized and corresponds to the Olivine-type LiFePO4 phase (JCPDS file no. 040-1499). Various deposition parameters (such as target power, substrate temperature, or argon pressure) were previously investigated, and in all cases, the as-deposited thin films were amorphous. As it can be seen in Fig. 1, the annealing treatment leads to the crystallization of NASICON-type Li3Fe2(PO4)2 phases (JCPDS file no. 047-0107), which is known to have better electrochemical properties [27]. Three small peaks are attributable to the Fe2O3 phase. The oxidation state of Fe in LiFePO4 and Li3Fe2(PO4) are +II and +III, respectively. It can be noted that the annealing in air of amorphous LiFePO4 not only leads to crystallization but also to the iron oxidation according to (Eq. 1) [28, 29]:
Fig. 1

XRD patterns of samples a LiFePO4 target, b as-deposited Li3Fe2(PO4)3, and c annealed Li3Fe2(PO4)3 at 700 °C for 3 h

$$ 12{\mathrm{Li}\mathrm{FePO}}_4+3{\mathrm{O}}_2=4{\mathrm{Li}}_3{\mathrm{Fe}}_2{\left({\mathrm{PO}}_4\right)}_3 + 2{\mathrm{Fe}}_2{\mathrm{O}}_3 $$
(1)

However, the conversion reaction of Fe2O3 with Li+ occurs at low potential which is not interesting for its use as a cathode [30, 31].

The morphology of the Li3Fe2(PO4)3 thin films before and after annealing was observed by SEM. From Fig. 2a, it is apparent that the as-deposited Li3Fe2(PO4)3 layer is homogeneous with a thickness of 850 nm according to the surface profilometry analysis given in Fig. 2b. After annealing, the film became rough and a sponge-like texture clearly appeared (Fig. 2c, d). Hence, the thermal treatment promoted the formation of a mesoporous material with a larger surface area than the as-deposited layer.
Fig. 2

a as-deposited Li3Fe2(PO4)3 with b profilometry analysis, low (c) and high magnification (d) SEM images of porous Li3Fe2(PO4)3 deposited by RF sputtering after annealing treatment

The electrochemical characterization of the porous Li3Fe2(PO4)3 thin film was carried out by cyclic voltammetry (CV). Figure 3 shows the cyclic voltammogram (CV) is obtained. In agreement with literature, the electrochemical reactivity of crystalline Li3Fe2(PO4)3 is confirmed by the presence of anodic and cathodic peaks [3, 32]. These two peak pairs can be attributed to the reversible insertion reactions of two Li+ according to Eqs. (2) and (3):
  • First reduction (R1 2.68 V/Li) and oxidation peaks (O1 2.58 V/Li)

$$ {\mathrm{Li}}_4{\mathrm{Fe}}_2{\left({\mathrm{PO}}_4\right)}_3={\mathrm{Li}}^{+}+{\mathrm{Li}}_3{\mathrm{Fe}}_2{\left({\mathrm{PO}}_4\right)}_3+{\mathrm{e}}^{-} $$
(2)
  • Second reduction (R2 2.72 V/Li) and oxidation peaks (O2 2.85 V/Li)

$$ {\mathrm{Li}}_5{\mathrm{Fe}}_2{\left({\mathrm{PO}}_4\right)}_3={\mathrm{Li}}^{+}+{\mathrm{Li}}_4{\mathrm{Fe}}_2{\left({\mathrm{PO}}_4\right)}_3+{\mathrm{e}}^{-} $$
(3)
Fig. 3

CV curve of the annealed Li3Fe2(PO4)3 thin film deposited on Ti substrate recorded at a scan rate of 1 mVs−1

The presence of an additional reversible peak (O3 and R3 peaks) at around 2.4 V reveals that Li+ can also react with another phase. This active material is supposed to be LiFePO4(OH) into which lithium intercalation occurs through the reduction of Fe3+ to Fe2+ [3335]. Compared with literature, it can be noticed that the peaks are quite broad. This phenomenon can be explained by the presence of pores. Indeed, the large surface area offered by the porous texture promotes the storage of charge at the surface according to a non-faradaic process. Hence, the contribution of the capacitive effect leads to the broadening of the peaks.

The galvanostatic charge/discharge profiles obtained at C/10 of the half-cell battery are shown in Fig. 4a. In agreement with the CV curve, the presence of three pseudo-plateaus confirms that Li+ ions react with Li3Fe2(PO4)3 and LiFePO4(OH).
Fig. 4

Battery cycling tests at the kinetic rate of C/10 in the potential window of 2–4 V (a). Discharge capacity of cathode at multi-C-rate (b)

The capacity values obtained for the as-deposited sample (Fig. 4b) are very low in the range of 1–2 μAhcm−2. But, a first discharge capacity of 88 mAhg−1 (23 μAhcm−2) is achieved at C/10 for the annealed sample. An average value of about 65 mAhg−1 (17 μAhcm−2) is delivered after 20 cycles. This capacity corresponds to more than 50 % of the theoretical capacity of Li3Fe2(PO4)3 (33 μAhcm−2). We can observe that capacity is slightly fading during the first cycles. The capacity lost may be caused by the different effects which are associated with side reactions due to the phase changes in the insertion electrode, dissolution of the active material, or the decomposition of the electrolyte. The capacity loss has been also discussed by Song et al. [36] who reported that capacity fading can be attributed to surface impurities (such as lithiated iron oxide which is also involved in the lithium insertion/extraction) leading to the irreversible reaction of Li+ with iron oxide and the formation of a solid electrolyte interface (SEI) at the surface of the electrode.

In order to study the operational stability of the NASICON-type Li3Fe2(PO4)3, the cycling life performance has been also studied at two different C-rates (Fig. 4b). From this graph, it can be seen that the capacity becomes stable after 10 cycles. At C/5, the battery capacity is about 50 mAhg−1 (13 μAhcm−2) and remains constant over 40 cycles. These results also show that the porous geometry of the mesoporous electrode is beneficial for tolerating the volume expansion that generally occur during alloying/de-alloying reactions.

Conclusions

In this work, we report the fabrication of mesoporous NASICON-type Li3Fe2(PO4)3 thin film by radio frequency sputtering. The electrochemical studies suggest that after annealing, the crystallized layer is also composed of LiFePO4(OH), which is able to react reversibly with Li+. In the first cycle, the discharge capacity reaches about 88 mAhg−1 (23 μAhcm−2) at C/10 and attains 65 mAhg−1 (17 μAhcm−2) after 10 cycles. The electrochemical characterizations also reveal a good stability suggesting that this material can be used as a cathode for Li-ion microbatteries.

Declarations

Acknowledgements

This work has been carried out thanks to the support of the A*MIDEX project (no. ANR-11-IDEX-0001-02) funded by the “Investissements d’Avenir” French government program, managed by the French National Research Agency (ANR).

Authors’ contributions

VAS did experimental works. ME and PK participated to the discussion. FV and TD supervised the research work.

Competing Interests

The authors declare that they have no competing interests.

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors’ Affiliations

(1)
Aix-Marseille University, CNRS, MADIRELLaboratory, UMR 7246
(2)
Department of Flexible Electronics, Ecole National Supérieure des Mines de Saint-Etienne

References

  1. Padhi AK, Nanjundaswamy KS, Goodenough JB (1997) Phospho-olivines as positive-electrode materials for rechargeable lithium batteries. J Electrochem Soc 144:1188–1194View ArticleGoogle Scholar
  2. Li D, Zhou H (2014) Two-phase transition of Li-intercalation compounds in Li-ion batteries. Mater Today 17:451–463View ArticleGoogle Scholar
  3. Xu J, Deshpande RD, Pan J et al (2015) Electrode side reactions, capacity loss and mechanical degradation in lithium-ion batteries. J Electrochem Soc 162:A2026–A2035View ArticleGoogle Scholar
  4. Porthault H, Decaux C (2016) Electrodeposition of lithium metal thin films and its application in all-solid-state microbatteries. Electrochim Acta 194:330–337View ArticleGoogle Scholar
  5. Luais E, Ghamouss F, Wolfman J et al (2015) Mesoporous silicon negative electrode for thin film lithium-ion microbatteries. J Power Sources 274:693–700View ArticleGoogle Scholar
  6. Lafont U, Anastasopol A, Garcia-Tamayo E, Kelder E (2012) Electrostatic spray pyrolysis of LiNi0.5Mn1.5O4 films for 3D Li-ion microbatteries. Thin Solid Films 520:3464–3471View ArticleGoogle Scholar
  7. Ferrari S, Loveridge M, Beattie SD et al (2015) Latest advances in the manufacturing of 3D rechargeable lithium microbatteries. J Power Sources 286:25–46View ArticleGoogle Scholar
  8. Meng X, Yang X-Q, Sun X (2012) Emerging applications of atomic layer deposition for lithium-ion battery studies. Adv Mater 24:3589–3615View ArticleGoogle Scholar
  9. Plylahan N, Kyeremateng N, Eyraud M et al (2012) Highly conformal electrodeposition of copolymer electrolytes into titania nanotubes for 3D Li-ion batteries. Nanoscale Res Lett 7:349View ArticleGoogle Scholar
  10. Plylahan N, Maria S, Phan TN et al (2014) Enhanced electrochemical performance of lithium-ion batteries by conformal coating of polymer electrolyte. Nanoscale Res Lett 9:544View ArticleGoogle Scholar
  11. Ellis BL, Knauth P, Djenizian T (2014) Three-dimensional self-supported metal oxides for advanced energy storage. Adv Mater 26:3368–3397View ArticleGoogle Scholar
  12. Masquelier C, Padhi AK, Nanjundaswamy KS, Goodenough JB (1998) New cathode materials for rechargeable lithium batteries: the 3-D framework structures Li3Fe2(XO4)3(X = P, As). J Solid State Chem 135:228–234View ArticleGoogle Scholar
  13. Sato M (2002) Preparation of iron phosphate cathode material of Li3Fe2(PO4)3 by hydrothermal reaction and thermal decomposition processes. Solid State Ionics 152–153:247–251View ArticleGoogle Scholar
  14. Yang S, Zavalij PY, Stanley Whittingham M (2001) Hydrothermal synthesis of lithium iron phosphate cathodes. Electrochem Commun 3:505–508View ArticleGoogle Scholar
  15. Karami H, Taala F (2011) Synthesis, characterization and application of Li3Fe2(PO4)3 nanoparticles as cathode of lithium-ion rechargeable batteries. J Power Sources 196:6400–6411View ArticleGoogle Scholar
  16. Morcrette M, Wurm C, Masquelier C (2002) On the way to the optimization of Li3Fe2(PO4)3 positive electrode materials. Solid State Sci 4:239–246View ArticleGoogle Scholar
  17. Pylinina AI, Mikhalenko II, Ivanov-Shits AK et al (2006) The influence of plasma chemical treatments on the activity of the Li3Fe2(PO4)3 catalyst in butanol-2 transformations. Russ J Phys Chem 80:882–885View ArticleGoogle Scholar
  18. Smiley DL, Davis LJM, Goward GR (2013) An improved understanding of Li+ hopping pathways and rates in Li3Fe2(PO4)3 using selective inversion 6Li NMR spectroscopy. J Phys Chem C 117:24181–24188View ArticleGoogle Scholar
  19. Kim HS, Kim CS (2013) Spin ordering between sub-lattices in nasicon Li3Fe2(PO4)3 measured by Mössbauer spectroscopy. J Appl Phys 113:17E117Google Scholar
  20. Shirakawa J, Nakayama M, Wakihara M, Uchimoto Y (2006) Changes in electronic structure upon Li insertion reaction of monoclinic Li3Fe2(PO4)3. J Phys Chem B 110:17743–17750View ArticleGoogle Scholar
  21. Salah AA, Jozwiak P, Garbarczyk J et al (2005) Local structure and redox energies of lithium phosphates with olivine- and nasicon-like structures. J Power Sources 140:370–375View ArticleGoogle Scholar
  22. Ivanov-Schitz A (2001) Li3Fe2(PO4)3 solid electrolyte prepared by ultrasonic spray pyrolysis. Solid State Ionics 139:153–157View ArticleGoogle Scholar
  23. Andersson A (2001) Lithium insertion into rhombohedral Li3Fe2(PO4)3. Solid State Ionics 140:63–70View ArticleGoogle Scholar
  24. Becht G, Hwu S-J (2006) Hydrothermal ion exchange on submillimeter-size single crystals of a new iron(III) phosphate. Chem Mater 18:4221–4223View ArticleGoogle Scholar
  25. Yoon Y, Park C, Kim J, Shin D (2012) Characterization of lithium borophosphate glass thin film electrolytes deposited by RF-magnetron sputtering for micro-batteries. Solid State Ionics 225:636–640View ArticleGoogle Scholar
  26. Nakazawa H, Sano K, Baba M, Kumagai N (2014) Stability of thin-film lithium-ion rechargeable batteries fabricated by sputtering method without heating. J Electrochem Soc 162:A392–A397View ArticleGoogle Scholar
  27. Bajars G, Kucinskis G, Smits J, Kleperis J (2011) Physical and electrochemical properties of LiFePO4/C thin films deposited by direct current and radiofrequency magnetron sputtering. Solid State Ionics 188:156–159View ArticleGoogle Scholar
  28. Hamelet S, Gibot P, Casas-Cabanas M et al (2009) The effects of moderate thermal treatments under air on LiFePO4-based nano powders. J Mater Chem 19:3979–3991View ArticleGoogle Scholar
  29. Yu F, Zhang L, Li Y et al (2014) Mechanism studies of LiFePO 4 cathode material: lithiation/delithiation process, electrochemical modification and synthetic reaction. RSC Adv 4:54576–54602View ArticleGoogle Scholar
  30. Larcher D, Masquelier C, Bonnin D et al (2003) Effect of particle size on lithium intercalation into α-Fe2O3. J Electrochem Soc 150:A133–A139View ArticleGoogle Scholar
  31. Ortiz GF, Hanzu I, Lavela P et al (2010) A novel architectured negative electrode based on titania nanotube and iron oxide nanowire composites for Li-ion microbatteries. J Mater Chem 20:4041–4046View ArticleGoogle Scholar
  32. Antolini E (2004) LiCoO2: formation, structure, lithium and oxygen nonstoichiometry, electrochemical behaviour and transport properties. Solid State Ionics 170:159–171View ArticleGoogle Scholar
  33. Yaghoobnejad Asl H, Choudhury A (2014) Phosphorous acid route synthesis of iron tavorite phases, LiFePO4(OH)x F1−x [0 ≤ × ≤ 1] and comparative study of their electrochemical activities. RSC Adv 4:37691–37700View ArticleGoogle Scholar
  34. Ellis BL, Ramesh TN, Rowan-Weetaluktuk WN et al (2012) Solvothermal synthesis of electroactive lithium iron tavorites and structure of Li2FePO4F. J Mater Chem 22:4759–4766View ArticleGoogle Scholar
  35. Marx N, Croguennec L, Carlier D et al (2010) The structure of tavorite LiFePO4(OH) from diffraction and GGA + U studies and its preliminary electrochemical characterization. Dalton Trans 39:5108–5116View ArticleGoogle Scholar
  36. Song J, Cai M-Z, Dong Q-F et al (2009) Structural and electrochemical characterization of SnOx thin films for Li-ion microbattery. Electrochim Acta 54:2748–2753View ArticleGoogle Scholar

Copyright

© The Author(s). 2016