Cobalt titanatecobalt oxide composite thinfilms deposited from heterobimetallicprecursorMuhammad Ali Ehsana, Muhammad Adil Mansoora, Muhammad Mazhara*,Asif Ali Tahirb, Mazhar Hamidc and K. G. Upul Wijayanthab

A single molecular heterobimetallic complex, [Co2Ti(m3-O)(TFA)6(THF)3] (1) [TFA= trifluoroacetate, THF= tetrahydrofuran], wassynthesized, structurally and spectroscopically characterized and implemented as a single-source precursor for the prepara-tion of CoTiO3CoO composite thin films by aerosol-assisted chemical vapour deposition (AACVD). The precursor complexwas prepared by interaction of Co(OAc)2.4H2O [OAc= (CH3COO

)] with Ti(iso-propoxide)4 in the presence of trifluoroacetic acidin THF, and was analysed by melting point, CHN, FT-IR, single-crystal X-ray diffraction and thermogravimetric analysis. Theprecursor complex thermally decomposed at 480 C to give a residual mass corresponding to a CoTiO3CoO composite material.Good-quality crystalline CoTiO3CoO composite thin films deposited at 500 C by AACVD and characterized through powderX-ray diffraction and scanning electron microscopy/energy-dispersive X-ray spectroscopy shows that the crystallites have arose-flower-like morphology with an average petal size in the range of 26mm. Copyright 2012 John Wiley & Sons, Ltd.

Keywords: cobalt titanatecobalt oxide; polynuclear bimetallic complex; composite; thin films

Introduction

Q1 High-purity titanates are sought for dye-sensitized solar cells[1,2]

as photocatalysts for water splitting to hydrogen and oxygen,degradation of air pollutants,[3] for self-cleaning and energy effi-cient windows,[4] gas sensors[5] and photoluminescent materi-als.[6] Ferromagnetic cobalt titanium oxide systems[7,8] have beeninvestigated as materials for dynamic random access memory,[9]

as dilute magnetic semiconductors and dilute magnetic dielec-trics[10] and for metal oxide semiconductor field-effect transistors.Cobalt titanium-based oxides systems are also employed ascatalysts, e.g. in hydrogenation processes, FisherTropsch reac-tions[11] and the oxidative dehydrogenation of ethane.[12] Cobalttitanate (CoTiO3) is used in the preparation of magnetic, ferroelec-tric nano-composite materials and nano-particulate gas sensors.Particularly, cobalt titanate plays an important role in the produc-tion of semiconductor devices, since with this oxide it is possibleto manufacture thin films with a very high k-constant.[13,14] Thegrowing interest of researchers in CoTiO3 materials is also due toa series of its physiochemical properties permitting its applicationas pigments, magnetic recording media[15] and gas sensors foralcohol, as humidity sensors and as catalysts.[16]

Cobalt titanium oxide powders have been prepared via differ-ent synthetic routes, such as conventional solid-state reactionsbetween fine powders,[17] solgel processes,[18] stearic acid gelmethods,[19] aerogel approaches,[20] the Pechini process,[21] co-precipitation of mixed metal oxalates[22] and micelle solutionmethods.[23] These methods generally involve mechanical mixingof oxides and/or carbonates followed by heating cycles, calcina-tion and ball milling for extended periods. This often yieldsinhomogeneous mixtures with only low control over the stoichi-ometry, appearance of undesirable phases, abnormal graingrowth and poor reproducibility. Fabrication of thin films from

these powders is often a formidable task, usually requiring hightemperatures and some kind of sophisticated equipment. Whenusing low-melting materials as the substrate the high processingtemperatures affect not only the quality of the thin films, but thethermal stability of the substrate also becomes a problem. Toovercome these challenges associated with the fabrication ofceramic thin films we focused our work on the design andsynthesis of soluble single-phase precursor materials that arecapable of delivering all the components of the target materialto a substrate in the required ratio, where they then can bedecomposed under mild conditions to form the desired thinfilms. Aerosol-assisted chemical vapour deposition (AACVD) is aversatile technique ideally suited for this purpose. Its only requi-site is for the precursor to be soluble in a suitable solvent,and the resulting solution can then be used to fabricate multi-component material layers while at the same time ensuring bothreproducibility and stoichiometry in the deposited layer(s). More-over, high-quality thin films can be obtained by AACVD as thehomogeneity of the aerosol depends on the size of the aerosoldroplets, which can be controlled through the frequency of theultrasonic generator. In continuation of our previous work[24,25]

and taking advantage of carboxylate ligand which coordinates

* Correspondence to: Muhammad Mazhar, Department of Chemistry, Faculty ofScience, University of Malaya, Lembah Pantai, 50603 Kuala Lumpur, Malaysia.E-mail: mazhar42pk@yahoo.com

a Department of Chemistry, Faculty of Science, University of Malaya, LembahPantai, 50603 Kuala Lumpur, Malaysia

b Department of Chemistry, Loughborough University, Loughborough LE11 3TU, UK

c Department of Chemistry, Quaid-I-Azam University, Islamabad 45320, Pakistan

Appl. Organometal. Chem. (2012) Copyright 2012 John Wiley & Sons, Ltd.

Full Paper

Received: 19 April 2012 Revised: 7 May 2012 Accepted: 21 May 2012 Published online in Wiley Online Library

(wileyonlinelibrary.com) DOI 10.1002/aoc.2893

1Journal Code Article ID Dispatch: 16.06.12 CE:

A O C 2 8 9 3 No. of Pages: 6 ME:

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to metal atoms in a variable way with potential to gain highnuclearity species, we investigated the design of soluble cobalt ti-tanium bimetallic molecular complex [Co2Ti(m3-O)(TFA)6(THF)3](1) (TFA= trifluoroacetate, THF = tetrahydrofuran) and fabricatedof CoTiO3CoO composite thin films by AACVD. The thin filmswere characterized by powder X-ray diffraction (PXRD), scanningelectron microscopy (SEM) and energy-dispersive X-ray spectros-copy (EDX) for crystallinity morphology and composition.

Experimental

General Considerations

All manipulations were carried out under an inert atmosphere of dryargon gas using Schlenk tube and glove box techniques. Solventswere carefully dried and distilled over sodiummetal/benzophenone.Cobalt(II) acetate tetrahydrate and titanium(IV) iso-propoxide werepurchased from Aldrich. Melting points were recorded on a Mita-mura Riken Kogyo (MT-D) apparatus and are uncorrected. Elementalanalysis was performed using a CHN analyser LECO model CHNS-932. FT-IR spectra were recorded with a Bio-Rad Excalibur FT-IRmodel FTs 300MX spectrometer from KBr discs. Controlled thermalanalysis was carried out using a PerkinElmer thermogravimetricanalyser TGA-7 with computer interface. Thermal measurementwas carried out in an alumina crucible under an atmosphere offlowing nitrogen gas (25mlmin1) at a heating rate of 12 Cmin1.

Synthesis

Synthesis of [Co2Ti(m3-O)(TFA)6(THF)3] (1)

0.200g (0.803mmol) cobalt(II) acetate tetrahydrate was suspendedin 10ml dry THF in a 50ml Schlenk tube fitted with an inert gas/vacuum line adapter and magnetic stirrer. 0.238ml titanium(IV)iso-propoxide (0.809mmol) was added drop by drop via syringeto the suspension. The contents were stirred for 1 h to obtain a cleardeep-blue solution. 0.2ml (2.00mmol) of trifluoroacetic acid (TFAH)was added to the blue solution, which turned deep red. The reac-tion mixture was evaporated to dryness under vacuum and the

solid was redissolved in 5ml of dry THF. The red solution was fil-tered through a cannula to remove any solid residue and wasplaced in a freezer at 10 C to obtain red-coloured crystals after2weeks with yield 82%. m.p. 115 C. Anal. Calcd for C24H24Co2F18O16Ti: C, 26.76; H, 2.23. Found: C, 26.96; H, 2.47%. IR (cm

1):1713 s, 1672 s, 1584m, 1468 s, 1426m, 1198 s, 1146 s, 1026m,897w, 793 s, 721 s, 618 s, 522 s, 461w. TGA: 129246C (28.58% wtloss); 259363 C (46.16% wt loss); 363480 C (residue of 21.76%).

X-ray Crystallography

Data were collected on a Bruker AXS SMART APEX CCD diffractom-eter at 100(2)K using Mo Ka radiation (0.71073) with the scantechnique. The unit cell was determined using SMART[26] andSAINT[27] and the data were corrected for absorption using SADABSin SAINT. The structure was solved by direct methods and refinedby full matrix least squares against F2 with all reflections usingSHELXTL.[28] All non-hydrogen atoms were refined anisotropically.The molecule is situated on a crystallographic mirror plane cuttingthrough the Ti atom, the central oxo atom, one of the THFmolecules and two of the TFA molecules. One of these TFA anionsshows rotational disorder of the CF3 group with an occupancy ratioof 0.672(19) to 0.328(19). The THF molecule on the mirror plane isdisordered over two symmetry-equivalent positions. Crystal dataand refinement parameters are given in Table T11.

Deposition of Thin Films by AACVD

Thin films were deposited by AACVD on commercially availablesoda glass slides from precursor (1) using a self-designed ultrasonicaerosol assisted chemical vapour deposition (AACVD) assembly asdescribed elsewhere.[29] Substrate was ultrasonically cleaned withdistilled water, acetone, isopropanol and ethanol and placed insidethe reactor tube. It was then heated to 500 C for 20min beforecarrying out the deposition. In a typical deposition, a 0.1 M solutionof precursor (1) was used to generate the aerosol at room temper-ature using a PIFCO air humidifier. Air was passed through theaerosol mist at a flow rate of 150mlmin1, thus forcing the aerosoldroplets into the reactor chamber. Depositions were conducted for

Table 1. Crystal data and structure refinement for precursor 1

Empirical formula C24H24Co2F18O16Ti range for data collection 1.65 to 28.28

Formula weight 1076.19 Reflections collected 15 004

Solvent THF Independent reflections 4795

Crystal habit, colour Rod, red Absorption correction Multi-scan

Temperature 100(2) K Max. and min. transmission 0.6182 and 0.7462

Crystal system Monoclinic Data/restraints/ parameters 5 538 / 0 / 314

Space group P21/m Goodness-of-fit on F2 1.054

Unit cell dimensions a=8.6429(6) , Final R indices [I> 2s (I)] R1= 0.0341,b=17.7715(13) wR2= 0.0826

c=12.5427(9)

b = 99.4220(10)

Volume 1900.5(2) 3 R indices (all data) R1= 0.0432,

wR2= 0.0882

Z 2 Largest diff. peak and hole 1.01 and 0.43 e 3Density (calculated) 1.881mgm3 Crystal size (mm) 0.55 0.20 0.20Absorption coefficient 1.223mm1 range for data collection 1.7 to 28.3

F(000) 1068 Index ranges 11 h 1121 k 2316 l 16

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45min. The exhaust from the reactor was vented directly into theextraction system of a fume cupboard. Towards the end of theexperiment the aerosol line was closed, and air was allowed to flowover the substrate to cool the films to about 40 C before they wereremoved from the reaction chamber for structural studies.

The surface morphology of deposited thin film was analysedusing a high-resolution scanning electron microscope (NNL 200)and composition was investigated with an energy-dispersiveX-ray spectrometer (EDX, GENESIS). The identity of the phasesand the degree of crystallinity of the deposited films weredetermined using a PAN analytical X-ray diffractometer modelXPert HighScore with primary monochromatic high-intensityCu-Ka (l=1.54184 ) radiation in the 2 range 5.0090.00 withstep size 0.026 operated at 40 kV and 40mA.

Results and Discussion

Synthesis and Characterization

The synthesis of oligomeric homo- or hetero-bi-trimetalic molecu-lar complexes is usually carried out by solution mixing of readilyavailable reactants such asmetal carboxylates, b-diketonates, metalalkoxides and aminoalkoxides that have bridging or bridgingchelating coordination capabilities. The trifluoroacetate ligand isalso known to be able to easily change its coordination from biden-tate tomonodentate, according to the electronic and steric require-ments of the central metal atom, thus improving the chances ofobtaining a stable, well-defined, bimetallic precursor complex.[30]

The precursor [Co2Ti(m3-O)(TFA)6(THF)3] (1) was prepared bystoichiometric reaction of Co(OAc)2.4H2O with Ti(

iPrO)4 andtrifluoroacetic acid (TFAH) in THF at room temperature undermild conditions as shown in equation (1):

The reaction seems to proceed through the hydrated startingmaterial accompanied by the loss of acetate and isopropanolresulting in the formation of oxo-bridged complex. The precursor(1) as crystallized from THF has a cobalt:titanium ratio of 2:1, isstable in air and soluble in organic solvents such as toluene andTHF. Melting point, elemental analysis, FT-IR, TGA and single-crystalX-ray analysis were conducted to characterize precursor 1. The IRabsorption bands of 1 are consistent with those reported in theliterature for its acetate analogue.[31] Two characteristic bands thatappear at 1679 and 1468 cm1 in the IR spectrum can be attributedto COO nasym and COO nsym vibrations, respectively. The differ-ence between n(COO)asym and n(COO)sym is approximately200 cm1 and suggests the presence of bridging TFA ligands.Strong absorptions due to CF and CO stretching vibrationsobserved at 1198 and 1146 cm1, respectively, correspond to theTFA group.[32] Low-intensity absorptions at 522 and 461 cm1 canbe assigned to nMO vibrations.[33]

Structural Analysis

The crystal structure of precursor 1 is depicted in Fig. F11 and crys-tal data and refinement parameters are given in Table 1. Selectedbond distances and angles are given in Table T22.

The geometry of 1 is based on an isosceles triangular Co2Tifragment, made up from two Co(II) atoms and one Ti(IV) atom

Figure 1. ORTEP diagram of precursor [Co2Ti(m3-O)(TFA)6(THF)3] (1) with atom labels for metal, oxygen and fluorine atoms. Symmetry operator (i):x, y+1/2, z. Disorder of one of the TFA anions and the THF molecule located on a mirror plane are omitted for clarity

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Cobalt titanatecobalt oxide composite thin films

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with one oxygen (m3-O7) at the centre of the triangle. Thisstructure is analogous to those of similar compounds reportedin the literature.[34] Six bridging trifluoroacetate anions arrangedalong the rim join the metal atoms through carboxylate oxygenatoms, reinforcing the triangular framework: the carboxylategroups display a bridging O, Oi coordination (symmetry operator(i): x, y+ 1/2, z). The oxygen donor atoms of the THF moleculescomplete the coordination of each 3d-metal to six, so that eachCo2+ and Ti4+ ion exhibits a distorted octahedral environmentof oxygen atoms. The co-planarity of the m3-O7 atom with themetal triangle shows that it is an sp2-hybridized oxide ion,removing the ambiguity associated with a possible m3-OH

bridge (no electron density indicating the presence of a hydro-gen atom was found in difference density maps). The m3-OCodistance [2.1069(11) ] is greater than the m3-O Ti value [1.755(2) ] due to the larger ionic radius of Co2+.[35] The TiO7Cobond angles [123.31(5) and 123.32(5)] are slightly larger thanthe CoO7Co angle [113.35(9)]. For the Ti4+ ion, three sets ofvalues of the TiO bond lengths are found: short m3-O7 Tidistances (1.755(2) ), two intermediate TiO distances (one2.0027(16) for TiO6 and TiO6i and a second for TiO4and TiO4i(2.0185(16) ), where O4 and O6 are oxygenatoms of the carboxylate bridges), and longer TiOTHF bonds(2.180(2) ). The bond distances TiO7 and CoO7 arecomparable to previously reported bond lengths.[37]Q2 For the Co2+ ions, the CoOCOO bond lengths [2.0402(15) , 2.0618(15) ,2.0965(15) and 2.0791(14) ] are in good agreement with thebond lengths in analogous trinuclear acetate complexes.[37]

The CoOTHF bond length (2.0611(15) ) is shorter than theTiOTHF bond length (2.180(2) ) and similar to such bondlengths in Co4(THF)4(TFA)8(m-OH)2Cu2(dmae)2.

[36,37]Q3

Thermal Decomposition and Thin Film Characterization

The thermal characteristics of precursor 1 have been examinedby thermogravimetric analysis, performed under an inert atmo-sphere of flowing nitrogen gas (25mlmin1) and a heating rate

of 12 Cmin1. The TGA curve (Fig. F33) shows a rapid mass lossat temperatures above 129 C and there appear to be threestages of weight loss. The first stage begins at 129 C and iscompleted at 246 C with a weight loss of 28.58%. The secondstep starts at 259 C and is completed at 363 C with a maximumweight loss of 46.16%. Directly following is the third and laststage, ranging from 363 to 480 C, resulting in a stable residualamount of 21.76% of the initial weight of precursor 1. Furtherheating above 480 C to up to 900 C did not cause anyadditional change in weight, indicating thermal stability of thedecomposition product. The residual mass is in good agreementwith the expected composition for CoTiO3CoO (21.76%), indicat-ing that the precursor has decomposed quantitatively into acomposite oxide phase. DTG curves confirm the occurrence ofthree major steps of decomposition of the precursor and indicatetemperatures of maximum heat flow at 233, 337 and 415C ineach degradation step, respectively.

An X-ray diffractogram of the thin films deposited from precur-sor 1 at 500 C indicates the formation of a composite of twodifferent types of crystalline oxide phases: CoTiO3 and CoO(Fig. F44). Peaks indexed by X at 2= 24.10, 33.17, 35.68, 40.93,

Table 2. Selected bond lengths () and angles () for precursor 1,[Co2Ti(m3-O)(TFA)6(THF)3]. Symmetry operator (i) as in Figure 1

Bond distances ()Co1O1 2.0402(15) Ti2O6 2.0028(16)

Co1O2 2.0618(15) Ti2O7 1.755(2)

Co1O3 2.0965(15) Ti2O8 2.180(2)

Co1O5 2.0791(14) Ti2O6i 2.0027(16)

Co1O7 2.1069(11) Ti2O4 i 2.0185(16)

Bond angles ()O9Co1O7 176.75(7) O5Co1O3 87.64(6)

O2Co1O7 93.15(7) O1Co1O7 96.89(7)

O5Co1O7 91.19(7) Co1O7Co i 113.35(9)

O3Co1O7 89.48(7) O7Ti2O6 98.09(6)

Ti2O7Co1 123.32(5) O6iTi2O6 93.62(10)

O1Co1O9 86.34(6) O7Ti2O4 95.83(6)

O9Co1O2 87.15(6) O6i Ti2O4 165.58(7)

O1Co1O5 171.23(6) O6Ti2O4 88.13(7)

O9Co1O5 85.56(6) O4i Ti2O4 86.71(9)

O2Co1O5 93.33(6) O7Ti2O8 177.71(9)

O1Co1O3 89.04(7) O6Ti2O8 83.46(6)

O9Co1O3 90.27(6) O4i Ti2O4 86.71(9)

O2Co1O3 177.17(6) Co1O7Co1 123.32(5)

Figure 3. Thermogravimetric plot showing loss in weight with increasein temperature for precursor 1

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Figure 2. Oxygen-coordinated octahedral spheres of Co1, and Ti2 in thecore unit of complex 1. Symmetry operator (i) as in Fig. 1

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49.39, 53.56, 57.02, 57.14, 63.91, 65.53, 71.11, 78.99 and 87.70correspond to reflections (012), (104), 210 , 213 , (024), (116),(018), (122), (030), (125) (1010), 431 and 426 , respectively,are in good agreement with reported crystallographic values

for hexagonal CoTiO3[36] with the space group R3 and lattice

dimensions of a= b= 5.065 and c= 13.920 [intensifiedcharge-coupled device (ICCD)Q4 : 980016548]. The reflections(111) and (113) produced at 2=37.29 and 73.99 marked byY relate to CoO phase,[37] which has a cubic structure with

the space group Fm3m, and cubic axis length of 4.263 [ICCD:980009865]. The lines at 2= 43.34, 62.58, 73.99 correspondsto both hexagonal CoTiO3 (202), (214), (420)Q5 planes and cubicCoO (002), (022) (113) planes.

The XRD peak patterns of the thin films deposited from precur-sor (1) at 500 C indicate its clean decomposition as it did notshow any impurities such as TiO2, Co2O3, Co3O4, Co2TiO4 orCoTi2O4 which were frequently observed in earlier studied

[1925]

cobalt titanium oxide preparative methods involving heating to600 C and above.[21]Q6

It is inferred that impurity-free CoTiO3CoO composite thin filmscan be deposited directly on soda glass substrate from precursor 1

at 500 C, as indicated in equation (1). The resulting greenish-coloured thin films reflect light in multicoloured fringes whenobserved at different angles. Good adhesion properties wereconfirmed when the films were subjected to the scotch tape test.

Co2Ti m3 O TFA 6 THF 3

1 !500C

AACVDCoTiO3 CoO Volatiles 2

Generally, fabrication of thin films of titanium-based compositesfrom pre-synthesized powders for industrial applications requirestemperatures of 1300 C or higher. It has been reported[15,38,39] thatduring fabrication of such films part of the Ti4+ ions are reduced toTi3+ and other low-valent titanium species, which negatively affectsthe dielectric properties and quality of these films. Since precursor 1cleanly decomposes at a relatively low temperature (~500 C),reduction of Ti4+ is avoided, resulting in thin films containingstoichiometric composite oxides while preserving the dielectricproperties of the targeted Ti(IV) materials. Precursor 1 also has thepotential to be used for the growth of high-melting ceramiccomposite films on low-melting substrates such as soda glass withsome control over particle size andmorphology in the film, therebymeeting the substrate requirements as well as microstructuralrequirements in certain applications.[42,43] Q7

The SEM image of the CoTiO3CoO composite thin filmfabricated at 500 C indicates the formation flower petal-likemorphology with well-defined grain boundaries and with featuresizes ranging between 2 and 6mm as shown in Fig. F66.

EDX spectra (Fig. 6) determined the stoichiometric composi-tion of the CoTiO3CoO composite thin films, indicating thatthe molar ratio of Co/Ti obtained from the peak areas of theEDX spectra is 15.61/7.51 and thus agrees well to the expected2:1 ratio of CoTiO3CoO composite thin films. Q9

We believe that the development of suitable precursors,selection of an appropriate CVD technique to grow thin filmsand mastering of deposition conditions are of crucial importancefor further advancements of new technologies and applications.A recent example emphasizing this is the report by Wijayanthaand co-workers who used the AACVD route to deposit SnO2/ZnO composite films for novel photovoltaic cells and optoelec-tronic devices.[40,41]

Figure 5. Comparison of CoTiO3CoO composite with standard CoTiO3and CoO patterns

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Figure 4. X-ray diffractogram of the composite oxide obtained fromprecursor 1. X indicates peaks corresponding to CoTiO3 and Y indicatespeaks corresponding to CoO

Figure 6. Q8High-resolution SEM image of CoTiO3CoO composite thinfilms deposited on soda glass substrate at 500 C from precursor 1

Cobalt titanatecobalt oxide composite thin films

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Conclusions

The single molecular complex [Co2Ti(m3-O)(TFA)6(THF)3] (1) hasbeen synthesized and characterized by physicochemical methods.Owing to its readily availability, stability and solubility in organicsolvents, complex 1 is a suitable precursor for the deposition ofcobalt titanatecobalt oxide composite thin films at 500 C by theAACVDmethod. X-ray diffraction and SEM/EDX analysis of thin filmsdeposited on a glass substrate indicate the formation of flower-likemorphology composed of crystalline phases of a CoTiO3CoOcomposite in which the atomic ratio of Co/Ti is almost equal tothe expected ratio of 2:1 of the precursor. Surface morphology,structure and composition observed in the CoTiO3CoO compositethin films imply that further customization of such systems could bevaluable for technological applications.

Acknowledgements

The authors acknowledge the High-Impact Research Grant No. UM.C/625/1/035, the UMRG scheme (Grant No. RG097/10AET) PakistanScience Foundation (PSF) Project No. PSF/Res/C-QU/CHEM. (408),Higher Education Commission (HEC) Project No. 1-308/ andILPUFU/HEC/2009 for funding this research. The X-ray diffractometerwas funded by NSF Grant No. 0087210, Ohio Board of Regents GrantCAP-491, and by Youngstown State University. AAT and KGUWacknowledge the support from UK EPSRC.

SUPPORTING INFORMATIONQ10

Complete structural data were deposited with the CambridgeCrystallographic Data Base. CCDC 808929 contains the supple-mentary crystallographic data for Precursor (1). The data can beobtained free of charge from the Cambridge CrystallographicData Centre via www.ccdc.cam.ac.uk/data_request.cif.

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Figure 7. EDX spectra of CoTiO3CoO composite thin films depositedfrom precursor 1

M. A. Ehsan et. al.

wileyonlinelibrary.com/journal/aoc Copyright 2012 John Wiley & Sons, Ltd. Appl. Organometal. Chem. (2012)

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Full Paper

Cobalt titanatecobalt oxide composite thin films deposited from heterobimetallic precursor

Muhammad Ali Ehsan, Muhammad Adil Mansoor, Muhammad Mazhar, Asif Ali Tahir, Mazhar Hamid and K. G. UpulWijayantha

Synthesis and characterization of heterobimetallic complex [Co2Ti(m3-O)(TFA)6(THF)3] (1) is reported for implementationfor deposition of CoTiO3-CoO composite thin films at 500 C by AACVD technique. The films are characterized by PXRD,SEM and EDX indicate their possible application in technology.

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