徐杉　盧琳　劉戀　駱義文　王石泉＊,　劉建文　李國(guó)華　馮傳啟(湖北大學(xué)湖北先進(jìn)有機(jī)化學(xué)材料協(xié)同創(chuàng)新中心，武漢4006)(湖北大學(xué)有機(jī)功能分子的合成與應(yīng)用教育部重點(diǎn)實(shí)驗(yàn)室，武漢4006)(浙江工業(yè)大學(xué)綠色化學(xué)合成技術(shù)國(guó)家重點(diǎn)實(shí)驗(yàn)室，杭州00)

鋰離子電池正極材料線團(tuán)狀α-M nO2的合成及電化學(xué)性能

徐杉1,2盧琳1,2劉戀1,2駱義文1,2王石泉＊,1,2劉建文1,2李國(guó)華3馮傳啟1,2
(1湖北大學(xué)湖北先進(jìn)有機(jī)化學(xué)材料協(xié)同創(chuàng)新中心，武漢430062)
(2湖北大學(xué)有機(jī)功能分子的合成與應(yīng)用教育部重點(diǎn)實(shí)驗(yàn)室，武漢430062)
(3浙江工業(yè)大學(xué)綠色化學(xué)合成技術(shù)國(guó)家重點(diǎn)實(shí)驗(yàn)室，杭州310032)

以MnSO4,(NH4)2S2O8為反應(yīng)物，Ag+作為催化劑的溶液相方法合成了線團(tuán)狀的α-MnO2。采用XRD、SEM和TEM等手段對(duì)合成產(chǎn)物進(jìn)行了表征。發(fā)現(xiàn)反應(yīng)溫度和反應(yīng)時(shí)間對(duì)產(chǎn)物的結(jié)晶度和形貌有很大的影響。通過(guò)恒電流充電/放電測(cè)試和循環(huán)伏安法(CV)對(duì)最終產(chǎn)物的電化學(xué)性能進(jìn)行了表征。結(jié)果表明，由于其獨(dú)特的形態(tài)，25℃下反應(yīng)2 d的產(chǎn)物作為鋰離子電池正極材料，表現(xiàn)出良好的循環(huán)穩(wěn)定性(100次循環(huán)后放電比容量為124 mAh·g-1)。線團(tuán)狀α-MnO2在鋰離子電池應(yīng)用中可能是一個(gè)潛在的正極材料。

線團(tuán)狀α-MnO2；溶液相合成方法；鋰離子電池

The cost efficiency and environmental friendliness of cathode materials is currently a major focus in battery research[1-2].In this regard,manganese oxides can meet all requirements and offer other desirable features,such as convenient preparation and abundant availability[3].Manganese dioxide is a widely-used material in electrochemical cells for its abundance and benignity.Due to the different interlink of the octahedral MnO6moiety,α,β,γ,δ and λ forms of MnO2are classified into three groups according to the tunnel structures in one,two or three dimensions[4-5],of which the α,β and γ forms are 1D tunnels.The δ and λ forms are 2D layered compound and 3D spinel structure,respectively[4,6].The properties of MnO2largely depend on it crystal structure[4,7-8].In recent years,1D nanostructures have been demonstrated to exhibit superior electrical,optical,mechanical,and thermal properties,showing their potential applications as building blocks in microscale devices[9-13].For example,α-MnO2has been widely used as magnetic materials[14-15],electrode materials in batteries[16-19]and supercapacitors[20-21].For Li/MnO2battery,among the polymorphs of MnO2,α-MnO2has large(2×2)tunnels existing in the crystalline lattice which can facilitate the Li+intercalation and de-intercalation within these systems thereby enhancing the capacity performance[18,23-24].Utilization of 1D α-MnO2could be advantageous in batteries as they not only provide large tunnels but also facilitate shorter diffusion path lengths and stress relaxation during intercalation/deintercalation process leading to a higher rate capability and cyclic stability[18,22,25-26].So far,many methods for synthesis of MnO2have been developed,mainly including hydrothermal method and solution phase synthesis method.Li et al.[9]have reported that a novel α-MnO2core-shell structure could be obtained by introducing a homogeneous catalyst of an Ag+solution[27]to prepare α-MnO2with a specific urchin-like structure. The diameters of these urchin-like structures are 1.6～2.0 μm,which densely aligned with nanorods with uniform diameters of 30～40 nm.In view of the special morphology of the product,it is likely to have high discharge specific capacity and stable cycling performance as cathode material in lithium ion batteries(LIBs).

In this work,we synthesizedα-MnO2via solution-phase method,using MnSO4and(NH4)2S2O8as reactants and Ag+ions as catalyst.The effects of reaction temperature and time on the crystal structure, the morphology and the electrochemical performance of the products were investigated.

1　Experimental

1.1Synthesis and characterization of the samples

The synthesis process is shown in Scheme 1, modified by the previous literature[9].The solutions were prepared by mixing 0.507 g MnSO4·H2O(3 mmol)and 0.684 6 g(NH4)2S2O8(3 mmol)in 50 mL distilled water,1 mL AgNO3(0.059 mol·L-1)solution was added in the above solution.After the homogeneous solution reacted for 2 days at 0℃(25,45,65℃),or reacted at 25℃for 1 day(3,5 days),the products were washed with distilled water and ethanol with centrifugal filtration for several times,respectively, and then dried in a vacuum at 60℃for 5 h.Then α-MnO2products were obtained(designated as α-MnO2-0℃-2 d,α-MnO2-25℃-2 d,α-MnO2-45℃-2 d,α-MnO2-65℃-2d,α-MnO2-25℃-1 d,α-MnO2-25℃-3 d,α-MnO2-25℃-5 d,respectively).

Scheme 1 Illustration of synthesis for α-MnO2

1.2General characterization of the sam p les

The structure and crystallinity of the samples were characterized using an X-ray diffractometer(XRD; Rigaku X-ray diffractometer)with Cu Kα radiation source(λ=0.150 6 nm)under a voltage of 40 kV and a current of 30 mA.The particle sizes of the samples were observed by scanning electron microscopy(SEM; JEOL JSM,6510 V)and transmission electron microscopy(TEM;FEI Tecnai G20).

1.3Electrochem ical characterization of the samples

The electrochemical characterizations were performed using coin cells(CR2016).The anode wasprepared by dispersing 70%as-prepared powders and 20%carbon black in 10%polyvinylidene fluoride (PVDF)solution.The mixture was rolled into a film and was dried at 120℃for 24 h in vacuum.The film was cut to size(1 cm2)and pressed onto a nickel mesh substrate(1 cm2).Coin test cells were assembled in an argon-filled glove box,with a metallic Li counter electrode,Celgard 2400 microporous membrane separator, and the electrolyte was a solution of l mol·L-1solution of LiPF6in ethylene carbonate(EC)and diethyl carbonate(DEC)(1∶1,V/V).The cyclic voltammetry (CV)was measured by an electrochemical workstation (CHI660E)between 1.5 and 4.2 V at a scan rate of 0.1 mV·s-1.The electrochemical impedance spectroscopy(EIS)measurements were performed with CHI660E over the frequency range of 0.01～100 kHz with an amplitude of 3 mV.These cells were galvanostatically charged and discharged in the voltage range of 1.5～4.2 V at the current density of 50 mA·g-1to measure the electrochemical response.The current densities used were from 50 to 500 mA·g-1.

2　Results and discussion

The chemical reaction in the homogeneous catalytic route to synthesize various α-MnO2structures could be described as follows[9]:

Without the existence of an Ag+ions solution or Ag foil,no product was formed at room temperature.It was known that the role of catalyst Ag+could reduce the potential energy of this chemical reaction so that the reaction could proceed with the existence of catalyst Ag+even at room temperature[9].

The XRD patterns of the as-prepared α-MnO2are shown in Fig.1(a,b),which indicates that the products can be indexed as α-MnO2(a=0.280 0 nm,b=0.280 0 nm,c=0.445 0 nm;Space group P63/mmc(194),PDF #300820).The crystallinity of the samples is not very good because the reaction temperature is very low(0～65℃).It can be seen with the increase of temperature and time,the crystallinity of the samples are getting better,which gives the fact that reaction temperature and reaction time have influenced on the crystallinity of materials.The structure of α-MnO2is hollandite structure,which is based on rhombic manganese ore structure.It is generally believed to adopt an octahedron structure in which Mn2+occupies the center of octahedron and O2-is distributed over octahedral sites, shown in Fig.1(c).[MnO6]octahedron forms doublestranded along the axis direction,the octahedron with double-chain shares apex angle with adjacent chains to form the T(2×2)tunnel structure[18,22-23].Tunnel sectional area becomes bigger because of its doublechain structure,which makes it accommodate ions such as Li+ions.It indicates that α-MnO2maybe a potential cathode material for LIBs.

Fig.1 XRD patterns of the samples prepared at various temperatures(a)and for various times at 25℃(b); (c)Crystal structure of as-prepared α-MnO2

The SEM images of the samples are shown in Fig.2(a～g).The insets of the SEM images are the higher magnification SEM images.It can be observed that nanowire with different thickness is the smallest unit of the microstructure.The sample α-MnO2-0℃-2 d(Fig.2(a))presents the inchoate mircrospherescomposed of nanowires with the size of 20～25 nm because of the low reaction temperature.With the increase of the temperature,microspheres were formed gradually,shown in Fig.2(b,c).The microspheres fell apart into nanowires with the size of 30～40 nm when the reaction temperature rose to 65℃(Fig.2(d)).With the increase of the reaction time,the morphology of the samples gradually became microspheres winded with nanowires instead of microspheres with diameter of 1 μm.And the longer the time is,the thicker the nanowires are,shown in Fig.2(b,e,f,g).Thus it can be seen that reaction time is the key factor for the formation of nanowires.The sample α-MnO2-25℃-2 d exhibits a mess of clews composed of the thinnest nanowires with the size of 15～20 nm,which can be observed at higher magnifications images(Fig.2(b)). The TEM images of α-MnO2-25℃-2 d are shown in Fig.2(h),present a clearer morphology with the aggregation of many nanowires.The average diameter of clews is about 1μm.There are many interspaces among nanowires,which are in favor for embedding of Li+ions.The nanometered structure of α-MnO2means that the Li+ions diffusion path is shortened and the electrochemical properties are enhanced for LIBs.

Fig.2 SEM images of the samples:(a)α-MnO2-0℃-2 d, (b)α-MnO2-25℃-2 d,(c)α-MnO2-45℃-2 d, (d)α-MnO2-65℃-2 d,(e)α-MnO2-25℃-1 d, (f)α-MnO2-25℃-3 d,(g)α-MnO2-25℃-5 d; TEM images:(h)α-MnO2-25℃-2 d

Fig.3 shows the typical charge/discharge curves of the as-prepared electrodes between 1.5 and 4.2 V with a current density of 50 mA·g-1,respectively.In the discharge curves,a voltage plateaus near at 2.8 V are clearly observed in Fig.3(a～g).It can be found that the initial discharge capacities ofα-MnO2prepared at 0,25,45,65℃for 2 days increase from 102 to 135 mAh·g-1gradually shown in Fig.3(a～d). However,the capacities of the samples(α-MnO2-0℃-2 d,α-MnO2-45℃-2 d,α-MnO2-65℃-2 d)fade sharply except for α-MnO2-25℃-2 d,which delivers an initial discharge capacity of 124 mAh·g-1(Fig.3(b)).The discharge capacity increases to 134 mAh·g-1after 20 cycles,136 mAh·g-1after 50 cycles,and stabilizes at 124 mAh·g-1after 100 cycles.Obviously,too short/ long reaction time also has great influence on electrochemical performance of the products shown in Fig.3(b,e,f,g).The samples(α-MnO2-25℃-1 d,α-MnO2-25℃-3 d,α-MnO2-25℃-5 d)exhibit a incremental initial discharge capacity(93～134 mAh·g-1), however,they all fade obviously.These phenomena can be explained by their crystallinities and morphologies.The microspheres were formed gradually with the rising reaction temperature.The shapes of the microspheres are imperfect and the crystallinity is worse when the temperature was too low,which leads to the low capacity of the product.When the reaction temperature was too high,the as-obtained samples such as α-MnO2-65℃-2 d,have thicker nanowires and better crystallinity,resulting in a lower capacity of the product.From the point in reaction time,for α-MnO2-25℃-1 d,a worse electrochemical performance may be due to the lack of nanowires.For α-MnO2-25℃-3d/5 d electrodes,they exhibit low capacities and unstable electrochemical performance,which can be attributed to their thicker nanowires aggregation.The sample α-MnO2-25℃-2 d exhibits a highest discharge capacity and best cycling stability due to its smaller size of nanowires,appropriate crystallinity.And the existence of the interspace can increase the electrode/ electrolyte contact,shorten the diffusion length of both Li+ions and electrons,and effectively buffer the volume expansion during the lithiation/delithiation process.

Fig.3 Charge/discharge curves of as-prepared samples(a～g)and CV curves of α-MnO2-25℃-2 d(h)

Based on the good electrochemical property of the as-prepared α-MnO2-25℃-2 d,it was further studied as cathode material for LIBs.Fig.3(h)shows the cyclic voltammograms(CVs)of α-MnO2-25℃-2 d at a scan rate of 0.1 mV·s-1between 1.5 and 4.2 V.The reactions associated with the redox processes are given below[28]:

In the first charging process,a reductive peak appears at 2.61 V and an oxidative peak appears at 3.12 V,which can be indexed to the formation of Mn, shown in Eq.(4,5).Then Eq.6 occurs in the subsequent four cycles,all the redox peaks repeat well except for the slight shift to higher potential,indicating good redox reversibility and structural stability(Fig.3(h)).

Fig.4(a)Cycling performances of the samples;(b)Coulombic efficiency of the samples;(c)Rate capacity and coulombic efficiency of α-MnO2-25℃-2 d at different current densities(50,100,500 mA·g-1)

The cycling performances of the samples are shown in Fig.4(a).The specific capacity of the samples of α-MnO2-0℃-2 d,α-MnO2-45℃-2 d,α-MnO2-65℃-2 d,α-MnO2-25℃-1 d,α-MnO2-25℃-3 d,α-MnO2-25℃-5 d electrodes show obvious decrease with cycling, from 101,126,132,92,132,133 mAh·g-1for the first cycle to 33,60,61,39,46,42 mAh·g-1for the 50th cycle.It is obvious that the α-MnO2-25℃-2 d electrode shows much stable cycling performance with higher specific capacities at the same cycle with the same current density,as compared with the other samples,which further indicates that the reaction temperature and reaction time have much influence on the electrochemical properties of the products.The coulombic efficiency of the samples is shown in Fig.4 (b).The values of the coulombic efficiency are at around 100%,which indicates discharge/charge process has well conducted in these electrodes.Fig.4(c)shows the rate capacities and coulombic efficiency of the α-MnO2-25℃-2 d electrode of various current densities. The discharge capacity is 123 mAh·g-1at 50 mA·g-1after 20 cycles,and this value is slowly reduced to 76 and 31 mAh·g-1when the current rate is consecutively set at 100 and 500 mA·g-1,respectively.At last,when the current rate returns to initial 50 mA·g-1, the final discharge capacity is 95 mAh·g-1,recovering 78%of the initial capacity.The discharge/charge process has well conducted when the current densities are 50,100 and 500 mA·g-1.

The electrochemical impedance spectra(EIS)of different electrodes,which are collected before the electrochemical properties testing under open voltage conditions,shown in Fig.5(a).For the α-MnO2-2 d(0～65℃)electrodes,the diameters of the semicircle of the curves are 156.83,61.89,77.82 and 70.61 Ω and for the α-MnO2-25℃(1～5 d)electrodes,the diameters of the semicircle of the curves are 226.38,61.89, 87.29 and 108.30 Ω at the frequency of 12.1 Hz, respectively.Among all the samples,the α-MnO2-25℃-2 d has the smallest charge transfer resistance,the highest conductivity and Li+is apt to deintercalate and intercalate,indicating it has the best electrochemical performance.The convective change of Li+from high frequency to low frequency is the migration of Li+in the electrolyte,the conversion of Li+in the interface and the diffusion of Li+in the solid phase. The diffusion process of Li+in the solid phase is a slow process,which becomes a control step.The larger the diffusion coefficient is,the better the highrate discharge performance is.The remaining inclined lines in the low frequency range in the EIS spectra are attributed to the Warburg impedance(Zw).As revealed in Fig.5(b),the Warburg coefficient(Aw)is equal to the slope of the Z′vs ω-1/2line at lowfrequency,where ω is the angular frequency of the alternating current.The numerical value of the Li+diffusion coefficient in the electrode can be estimated from the following equation[29-30]:

Fig.5(a)Electrochemical impedance spectra of the samples;(b)Linear fitting of Warburg impedance of the samples

where Vmis the molar volume of the material,S is the apparent surface area of the electrode,and d E/d x is the slope of the open-circuit potential vs the mobile ion concentration x at each x value.Hence,the numerical values of Vm,S,and d E/d x are constant for the model test cells,and the Li+diffusion coefficient is in direct proportion to(1/Aw)2[30].The Warburg coefficients(Aw)of the above cells are 71.69,32.03, 41.99,38.13,85.38,44.57 and 49.47 Ω·s-1/2,respectively,confirming that the ionic conductivity of α-MnO2-25℃-2 d is better than that of other materials according to the Eq.7.These results are consistent with the electrochemical properties of the above electrodes.

3　Conclusions

Clew-like α-MnO2was synthesized by a facile solution phase method using MnSO4and(NH4)2S2O8as reactants and Ag+ions as catalyst.The results reveal that the reaction time and temperature play crucial roles to synthesize products with different morphologies,which consequently influence the electrochemical properties of the products.The results show that the product α-MnO2prepared at 25℃for 2 days as cathode material for LIBs,exhibits a highest reversible capacity and excellent cycling stability(124 mAh·g-1after 100 cycles)due to its uniform microspheres composed of many thinner nanowires and appropriate crystallinity.The clew-likeα-MnO2could be a potential cathode material for the application of LIBs.

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Synthesis and Electrochem ical Characteristics of Clew-like α-M nO2as Cathode M aterial for Lithium Ion Battery

XU Shan1,2LU Lin1,2LIU Lian1,2LUO Yi-Wen1,2WANG Shi-Quan＊,1,2LIU Jian-Wen1,2LI Guo-Hua3FENG Chuan-Qi1,2
(1Hubei Collaborative Innovation Center for Advanced Organic Chemical Materials,Hubei University,Wuhan 430062,China)
(2Ministry-of-Education Key Laboratory for the Synthesis and Application of Organic Functional Molecules,Hubei University,Wuhan 430062,China)
(3State Key Laboratory Breeding Base of Green Chemistry-Synthesis Technology,Zhejiang University of Technology,Hangzhou 310032,China)

Clew-like α-MnO2was synthesized by a solution phase synthesis method using MnSO4and(NH4)2S2O8as reactants and Ag+ions as catalyst.The synthetic materials were characterized by XRD,SEM and TEM.It was found that the reaction temperature and reaction time have much influence on the crystallinity and morphology of the products.The electrochemical properties of the final products were tested by galvanostatic charge/discharge profile measurement and cyclic voltammetry(CV).The results show that the product prepared at 25℃for 2 days as cathode material for lithium ion battery,exhibits excellent cycling stability(124 mAh·g-1after 100 cycles)due to its unique morphology.The clew-structure α-MnO2could be a potential cathode material for the application of lithium ion batteries(LIBs).

clew-like α-MnO2;solution phase synthesis method;lithium ion battery

TM912.9

A

1001-4861(2016)01-0124-07

10.11862/CJIC.2016.013

2015-09-07。收修改稿日期：2015-10-19。

浙江工業(yè)大學(xué)綠色化學(xué)合成技術(shù)國(guó)家重點(diǎn)實(shí)驗(yàn)室培育基地開(kāi)放基金(No.GCTKF2014013)、貴州省教育廳安順學(xué)院功能材料與資源化學(xué)特色重點(diǎn)實(shí)驗(yàn)室開(kāi)放基金(No.GAFMRC201305)和武漢市青年科技晨光計(jì)劃項(xiàng)目(No.2014070404010213)資助。

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