Characterization of CBD-CdS Doped with Some Rare Earths III ( Eu 3 + , Ce 3 + ) as Function of Synthesis Time

Rare earths (Europium, cerium)-doped CdS nanofilms are prepared using the growth technique chemical bath deposition (CBD) at the reservoir temperature of 70±2°C varying the synthesis time in a wide range. For the rare earths doped CdS nanofilms the synthesis time was ranged from 80 to 135 min. The rare earths molar concentration was in the range 0.0≤x≤3.47, which was determined by energy dispersive X-ray spectroscopy (EDS). The X-ray diffraction (XRD) analysis reveals that CdS nanofilms showed the zinc blende (ZB) crystalline phase. The nanocrystal size was ranged from 2.67 to 2.35 nm for the CdS and 1.84-2.33 nm for rare earth-doped CdS that were determined by the Debye-Scherrer equation from ZB (111) direction and it was confirmed by transmission electron microscopy (TEM). The doped CdS exhibits a direct band gap that diminishes with the increase of the synthesis time, from 2.50 to 2.42 eV, which was obtained by transmittance. The room-temperature photoluminescence of CdS presents the band-to-band transition at 431 nm, which is associated with quantum confinement because the grain size is less than its Bohr exciton radius and a dominant band at 523 nm, which is called the optical signature of interstitial oxygen. Eu3+-doped CdS photoluminescence shows the dominant radiative peak at 576 nm that is associated to the intra-4f radiative transition of Eu3+ ions, which corresponds to the magnetic dipole transition, (D0→ 7F1). For the Ce3+-doped CdS the dominant radiative transitions are clearly redshifted. Additionally, other radiative peaks associated at structural defects are observed. The passivation of the CdS by rare earths was approximately of two orders of magnitude obtaining better results with cerium.


Introduction
Semiconductor nanostructures have attracted a lot of attention due to their unique optical, electronic mechanical and properties.Inorganic compounds doped with lanthanide ions are widely used as the luminescent materials in lighting 1 and displays 2 , optical amplifiers 3 and lasers 4 .Recently, the optical properties of nanocrystals doped with lanthanide impurities have attracted much attention because of they are expected to modify both electronic states and electromagnetic fields.Therefore, a possible influence of quantum size effect on the luminescence properties is expected for II-VI semiconductor nanocrystals due to the inclusion of rare earth (RE) metal ions 5 .The effects of the quantum-confinement size of the semiconductor nanoparticles not only create photogenerated carriers, which may have an interaction with f-electrons but also significantly influence the optical properties 6 .Excitonic transition in the host material and an improvement in the luminescence intensity are also expected for the semiconductor nanostructures after the rare earths (RE) doping.The effects of the reduced dimensionality on the electronic relaxation and the phonon density-of-states of semiconductor compounds and insulating nanocrystals have been extensively investigated by both theoretical and experimental approaches 7,8 .Doping of II-VI compounds with lanthanides ions like cerium, terbium and europium, etc., has been extensively studied 9 .Doping of rare earth element like cerium reduces the particle size of nanomaterials and increases surface area 10 .Vij et al. reported the luminescence studies on Ce doped SrS nanostructures and Ce doped CaS nanoparticles synthesized by solid state diffusion method 11 .Other authors have reported luminescence investigations on Ce 3+ -doped CaS synthesized using the chemical co-precipitation method 12 .
The Chemical bath deposition (CBD) method is one of the cheapest methods to deposit thin films and nanomaterials, as it does not depend on expensive equipment and is a scalable technique that can be employed for large area batch processing or continuous deposition.The major advantages of CBD is that it requires only solution containers and substrate mounting devices and it is friendly to the environment because of the deposition of the films is carried out at low temperatures.The one drawback of this method is the wastage of solution after every deposition.Among various deposition techniques, chemical bath deposition yields stable, adherent, uniform and hard films with good reproducibility by a relatively simple process.The chemical bath deposition method is one of the suitable methods for preparing highly efficient thin films in a simple manner.The growth of thin films strongly depends on growth conditions, such as duration of deposition, composition and temperature of the solution, and topographical and chemical nature of the substrate.Deposition by chemical bath technique of thin films consists of moderate release of metal ions into alkaline solution 13 .This technique has become important for the development of thin film solar cells, since the synthesis of CdS by this method offers a better efficiency than traditional evaporation method [14][15][16] .In the deposition of the thin film by CBD technique exhibits two different mechanisms: The first mechanism is that involving the reaction of atomic species on the surface, this mechanism is called ion-to-ion [17][18][19] and the second mechanism is associated with the agglomeration of colloids formed in the solution, which can be regarded as an increase in grouping or cluster-by-cluster.For practical purposes, the formation of the core, which leads to the formation of the film, it can occur by a process of heterogeneous nucleation on the substrate or through a process of homogeneous nucleation in the volume of the solution.
In this work reports the synthesis and structural and optical characterization of CdS and CdS:(Ce 3+ , Eu 3+ ) nanofilms obtained by chemical bath deposition on glass substrates at low temperature and at different synthesis times.The effects of the chemical composition on structural and optical properties of the CdS and CdS:(Ce 3+ ,Eu 3+ ) alloys were studied by EDS, X-ray diffraction, HRTEM, transmittance and room-temperature photoluminescence.

Experimental details
The chemical bath deposition is a technique to deposit films on a solid substrate from a reaction that occurs in solution.It starts from an aqueous solution of salts of the elements of the compound to be obtained.It requires that the compound to deposit is relatively insoluble and chemically stable in the solution to give a simple precipitation in an ionic reaction 20 .The method of obtaining of CdS doped with rare earth was the chemical bath deposition in its modality of immersion, in which a cryo-thermostat of circulation Polyscience with temperature controller of -40 to 200°C was used.Being graded it to the temperature of 20°C to avoid the release of harmful gases into the environment and using ammonium nitrate as complexing agent.The solutions mixture is carried out using the following precursors: cadmium chloride dehydrate (CdCl 2 +2H 2 O) (Productos Químicos Monterrey S. A.), potassium hydroxide (KOH) (JT Baker, 98.6% purity), Ammonia Nitrate (NH 4 (NO 3 )) (Sigma-Aldrich, 99.5% purity) and thiourea thiocarbamide (Fermet, 99.9% purity).The nitrifying reagents are Europium (III) nitrate pentahydrate (Eu(NO 3 ) 3 +5H 2 O) (Sigma-Aldrich, 99.999% purity) and Cerium (III) nitrate (Ce(NO 3 ) 3 +6H 2 O) (Sigma-Aldrich, 99.999% purity) working with the following concentrations 0.05 M CdCl 2 , 0.05 M KOH, 0.1 M NH 4 (NO 3 ), 0.05 M NH 2 SCNH 2 .The used precursors concentrations are Eu(NO 3 ) 3 0.001 M and Ce(NO 3 ) 3 0.001 M with the appropriate volumes, the doping is achieved when the solutions mixture has a slightly basic pH.The synthesis time was ranged from 60-75 min for single CdS, 80-135 min for doping by lanthanide impurities, achieving yellowish-opaque surfaces.The number that accompanies the name of the sample corresponds to the time of synthesis, for example the sample C60 indicates that it was synthesized during 60 min.The CdS:(0,Eu 3+ ,Ce 3+ ) nanofilms chemical stoichiometry was obtained by Energy Dispersive Spectrometry (EDS), which was carried out in a System LEO 438VP, with W.D. of 26 mm using a pressure of 20 Pa.The crystalline phase and structure of the films were determined with a Bruker D8 Discover diffractometer using the copper Kα radiation (λ=1.5406Å) at 40 kV and 40 mA with parallel beam geometry.High resolution transmission electron microscopy (HRTEM) studies were carried out in a JEOL JEM200 of 80-200 kV, the obtained image is recorded with a CCD camera in real time.The Gatan Digital Micrograph software was used for the analysis of HRTEM images.The transmittance measurement was performed using a Bruker Infrared Spectrometer Vertex 70 at room temperature.The photoluminescence was measured using a He-Cd (Omnichrome-Series 56) laser emitting at 325 nm with an optical excitation power of ~15 mW at room temperature.The radiative emission from the sample was focalized to the entrance slit of a HRD-100 Jobin-Yvon double monochromator with a resolution better than 0.05nm, and detected with an Ag-Cs-O Hamamatsu photomultiplier with a spectral response in the range 350-1000 nm.

Experimental Results and Discussion
The chemical stoichiometry of the CdS (or CdS:RE 3+ ) nanofilms was estimated by EDS measurements that besides allowed to know the presence of the residual impurities in the samples along with cadmium and sulphur.EDS spectra indicate that samples in addition to silicon, potassium, calcium, sodium and oxygen contain a significant amount of other residual impurities and besides the doped samples contain rare earths.In the subsequent to the samples CdS:(Ce, Eu) will be denominated like CdS:RE to simplify the notation.Consequently, the most of residual impurities detected in the nanolayers come from of the substrate.It has found that oxygen ions are present in synthesised samples in the form of O 2-ions that may produce CdO 21 .Oxidation of CdS to CdO occurs at high temperatures as has been reported 22 , in this case the temperature is low during synthesis and air drying, the conversion may have happened only at a very low percentage so that its presence could not be detected by X-Ray diffraction.However, these oxygen ions can form trap levels in the band gap, resulting in several transitions contributing or affecting to luminescence.Therefore, it appears that oxygen ions have replaced sulphurs at some random points of the CdS (CdS:RE 3+ ) lattice.The results of EDS measurements are presented in Table 1, in which are included the atomic and mass percentages of the elements.The number that accompanies the sample name corresponds to the synthesis time.From the table can be seen that the nanolayers are not stoichiometric for the investigated synthesis time interval.From these results is observed that sample C60 is not a stoichiometric compound and that starting from it a higher synthesis time (higher thiourea concentration in the solution) gives a higher presence of cadmium and an absence of sulphur.Considering that each CdS unit cell contains two cadmium atoms and two sulphur atoms, since the crystalline phase of the synthesised CdS is zinc blende, as was obtained by X-ray diffraction, which will be discussed extensively later.The atomic weight of the ideal unit cell is ~288.95 that corresponds to 22.19% sulphur atoms and 77.81% cadmium atoms.Therefore, when it occurs a deviation of the stoichiometric composition of the ideal unit cell could establish a relationship between vacancies or interstices of the elements of the crystalline lattice (V S , V Cd , Cd i , S i ).In the case of C65, which has excess of Cd and absence of S that is indicative that cadmium is interstitial and there are sulphur vacancies.The average errors with that were calculated percentage masses of different elements were for cadmium 1.25%, sulphur 0.35%, europium 0.25% and for cerium 0.30%.As can be seen in Table 1, these errors do not significantly alter the found results.Table 2 shows that the samples contain a lower concentration of sulphur, indicating that have a high concentration of sulphur vacancies.Also.It can induce that there is a high concentration of cadmium and RE interstices.Therefore, in the synthesised samples; there is excess elements II and lack element VI.
Figure 1 shows X-ray diffraction patterns of CdS:RE nanofilms synthesised at different times at a temperature of 70±2°C.It is observed from diffraction patterns that CdS and CdS:RE 3+ nanofilms are in polycrystalline nature.It can be observed that each peak corresponds fairly well with data of CdS marked in the software DICVOL04 data.The structural parameters obtained with the software DICVOL04 data are in good agreement with the published ones elsewhere 23 .From this close agreement, it is confirmed that as-deposited CdS:RE 3+ nanofilms for all the used synthesis times and precursor concentrations belong to face-centered cubic system (fcc).The X-ray diffraction patterns of CdS and CdS:RE 3+ nanofilms are described in the Fm-3m( 225), whose lattice parameters were calculated using the software DICVOL04, obtaining the lattice parameter value for C60: a = 5.76 Å, which is in agreement with the reported values [23][24][25] .As has been reported Cadmium sulphide exists in two crystalline phase modifications: the wurtzite (WZ) 26 and zinc blende (ZB) phase 25 .As can be seen in Fig. 1, the obtained X-ray diffraction patterns of the samples show clearly a predominant peak at 2θ = 26.8°,which can be assigned to (111) plane of CdS ZB crystalline phase.Additionally, the intensity weak of peak at 2θ = 28.3° is due to the diffraction from the (101) plane WZ phase whereas at 2θ = 26.4°position can be co-occupied by the (111) plane of ZB phase as well as the (002) plane WZ.However, the maximum peak intensity for both crystalline phases are different, ZB maximizes at 2θ = 26.8°corresponding to the (111) plane, whereas WZ crystalline phase has its maximum intensity peak at 2θ = 28.2°corresponding to (101) plane 27 .The diffraction peaks observed in the 15-17° range are the peaks associated with the rare earths incorporated at the sub-lattices sites of Cd 2+ , as can be seen from the diffractograms.It has been reported in the literature that the probability that CdS dissolves in the RE 2 S 3 (III) lattice at room temperature is very low 28 but when increases the synthesis time also is increased the probability.From XRD patterns can be assured that the RE 3+ forms RE 2 S 3 according to the peak located at 2θ~15-17°.From the XRD study can infer that the formation of the CdS:RE 3+ occurs in the early stage, following by the formation of RE 2 S 3 nanocrystallites in the stage of the film growth 29 .Additionally, it is observed a widening at the peak of the preferential ZB (111) direction that could be caused by a) undergoing stress and b) size of small crystalline domain or fluctuations in chemical composition.As the used substrates are amorphous, they do not produce a mismatch in the lattice parameters of layers, so the first case does not happen.Therefore, this can occur due to the small size of the crystals and by presence of strains that possess multiple facet diffraction peaks, which is the result of multidirectional growth of the synthetized nanocrystals.The peaks do not match exactly with the reported plane spacing for ZB and WZ phases that can be explained by the broadening of peaks, see Fig. 2. In the case of extremely small particles, where the contribution of surface free energy is very important, some deviations cannot be excluded.Fig. 2 shows the deconvolution of X-ray diffractograms of three typical samples C60, Ce130 and Eu115, to find all the diffraction peaks that make up the X-ray diffraction diffractograms.The crystallite sizes (D( hkl )) were calculated from the line broadening of the X-ray diffraction peaks at 2θ using the Debye-Scherrer equation.The lattice parameters of CdS and the mean grain sizes are presented in Table 2. Fig. 3 shows the variation of the size of the average crystalline domain with the incorporated REs as function of synthesis time obtained by the Debye-Scherer equation through the measurement of the width at half-maximum (FWHM) of the peak of the preferential ZB (111) direction of each deposited layer.In fact, to apply the Debye-Scherrer equation 30 finds that the crystalline domain presents clearly two behaviours: a) as the synthesis time increases for single CdS the average grain size diminishes slightly from 2.67 to 2.35 nm.b) For RE 3+ -doped CdS there is a noticeable decrease in grain size, although for RE 3+ -doped samples there is a light increased from 1.85 to 2.03 nm for Ce and 1.84 to 1.87 for Eu by increasing the synthesis time, where clearly is observed the RE 3+ ions effect to replace Cd 3+ ions of the CdS lattice.Similar behaviour is observed for the lattice constant, as is shown in the inset of Fig. 3, for single CdS lattice constant increases lightly as synthesis time is increased, from 5.76 to 5.88 nm, and for the samples doped with cerium (europium) increases (decreases) lightly.For the interplanar distance (ID) (111) of the ZB phase is presented in Table 2, which increases lightly and was calculated from the 2θ peak position versus synthesis time.This ID, in practice, coincides with (111) ID of the ZB crystalline phase.It is worth-noting the values of electronegativity for Ce (1.12), Eu(1.2) and Cd (1.69), which are favourable to form a solid solution 31 .The TEM measurements of the obtained samples corroborate the presence and the nanometric size of particles.In Fig. 4 is shown some TEM micrographs of typical samples, it is evident the presence of particles with almost completely spherical shape at nanometric scale.Based on more than 100 measurements taken from the TEM micrographs of the typical samples a size distribution histogram was obtained, which are shown in the inset of Fig. 4, and it can be detected a Gaussian adjustment with a narrow distribution of size and a maximum value of 5.44 and 3.55 nm, for single CdS and CdS:Eu 3+ .Absence of bimodal size distribution in the size distribution histograms suggests that the nanoparticles obtained by the synthesis process at different times correspond to the formation of an CdS:RE 3+ system and not the physical mixture of nanoparticles sizes.A comparable analysis was performed for some of the samples and the results are listed on Table 2. Bigger semiconductor particles are obtained single CdS.Therefore, the reaction time can be used to control the formation and size of the CdS nanoparticles.As can be observed in Table 2, the particle size values obtained from the X-ray diffraction using Debye-Scherrer equation and those measured from the TEM micrographs have small discrepancy.These small discrepancies in particle size is due to some approximations involved in the calculations using the Debye-Scherrer equation or coalescence of nanocrystals during preparation for TEM analysis.With the purpose of verifying the structure's quality and crystalline phase of the obtained semiconductor nanoparticles, HRTEM images were taken and the results are included in the inset of Fig. 4, which are the result of the processing of the HRTEM image using filters in Fourier space.From the HRTEM micrograph of typical samples, it is clearly observed the formation of nanoparticles with a defined crystalline structure, zinc blende.Amplifying and analysing the selected area of the micrograph (it is shown as insets in Fig. 4), it was possible to calculate the interplanar distances of ~0.33 nm corresponding to plane (111) of particles of crystallized CdS in blende zinc type crystalline phase.As can be seen, the results obtained by HRTEM are in good agreement with the results calculated from X-ray diffraction.
It can be seen in Fig. 3 the single CdS grain size decreases as synthesis time increases, suggesting the formation of a solid solution as has been reported 10 , having a region of discontinuity when is added RE 3+ molar concentration (V[RE 3+ ]), the grain size decreases markedly as is observed in figure.It remains almost constant for higher synthesis times, that is similar to a higher V[RE 3+ ].Moreover, the lattice constant increases lightly with increasing synthesis time and happens a discontinuity when is added V(RE 3+ ) in the film, which is an effect of RE 3+ substituting Cd 2+ in CdS lattice.A possible explication to this experimental fact can be due to difference of the ionic radii of Cd 2+ (0.97 Å) and Ce 3+ (1.15 Å) and Eu 3+ (1.09 Å).The (111) ID of ZB cubic phase in bulk is 0.3367 nm, this value is light lower than the ID values found for the CdS-CdS:RE films in this work.It is probable that ID values in CdS:RE 3+ films are owing to the existence of Cd 2+ vacancies.For a relative low concentration of RE 3+ ions, this can be, in a large majority, be situated in: (a) Cd 2+ vacancies sites that otherwise would be empty 32 , (b) in Cd 2+ sites provoking the appearing of Cd 2+ interstitial, and (c) in interstitial positions.For higher synthesis times, that is higher V(RE 3+ ), the material behaves like a solid solution, the generation of Cd 2+ vacancies, whose creation is needed to charge balance, starts to be important in number and given the relative ionic radius of S 2-.There is a tendency of the Full Width at Half Maximum (FWHM) of (111) peak of the growth films probably due to all of the possible RE 3+ species present in Cd 2+ sites and interstitials positions 33 , and also to the existence of RE 2 S 3 , which distort the crystalline lattice and provoke disorder.The distortion produces a strong strain that affects the interatomic distances; this similar fact has been reported 23,34 .In this work, the strain and distortion of the lattice can be smaller.The appearing of S 2-ions into the material favours the relaxing of the lattice.
The effect of doping by rare earths on the optical properties of CdS nanolayers was investigated by room temperature transmittance measurements as a function of the synthesis time.The transmittance spectra in the visible and infrared ranges are recorded for the CdS:RE 3+ nanofilms in the wavelength range 350-900 nm at room temperature, see Fig. 5.The effect of V(RE 3+ ) added in the nanofilms on the optical properties including percentage of transmittance (% of T) and fundamental band gap (E g ) were studied in detail.The C60 sample transmittance measured in the visible range varies from zero to almost 86.5% (without considering the substrate contribution) and is the largest of all measured transmittance spectra.The sharp reduction in the transmittance spectra at the wavelengths lower than 500 nm is due to the fundamental absorption edges of the different films.The CdS:RE 3+ nanofilms were transparent, with no observable blue colouration under our experimental conditions.The intrinsic absorption edge of the CdS nanofilms can be evaluated and discusses in terms of the indirect interband transition.As is well-known the optical band gap (E g ) of a semiconductor material is related to the optical absorption coefficient (α) and the incident photon energy (E).The α for a film of thickness d and reflectance R is determined near the absorption edge using the simple relation: α = ln{(1-R) 2 /T+[((1-R 2 )/2T) 2 +R 2 ] 1/2 }/d, where multiple reflections are taken into, but interference neglected, and d is the film thickness.The band gap energy (E g ) for the different synthesis times and doping was calculated from optical transmittance data.Fig. 6a shows the first derivative of the optical density [d(OD)/dE] as a function of the incident photon energy (E) of typical samples.The relative minima in the transmittance spectra of the first derivative d(OD)/ dE versus E graph define the critical points of the band structure 35,36 , which are associated absorption bands due impurities and vacancies 23 , as is observed in Fig. 6a.Fig. 6b illustrates the second derivative of OD plotted against E of typical samples.A more precise position of the critical point E g in the E-axis is defined by the maximum of the second derivative curve.The estimated optical band gap of the CdS nanofilm is of 2.50 eV that corresponds to pure CdS and is 82 meV higher that band gap in CdS bulk, which indicates that there is quantum confinement.This discrepancy is associated to the average grain size 37,38 .As is observed in Fig. 6b band gap energy redshifts slightly with the V[RE 3+ ] increase or that is the same with the increase of the synthesis time, these results are shown in Fig. 7.The transmittance spectrum of RE 3+ -doped CdS is fundamentally similar to that of single CdS as can see in Fig. 5, with some slight shifts in the absorption band, which are caused by the incorporation of RE in Cd sub-lattice.The main absorption band slightly redshifts as V[RE 3+ ] increases.The slight reduction of the main absorption edge is indicative of the compensation of broken bonds, but also it indicates that the RE atoms are being incorporated into interstitials of the unit cell, see Table 1.In order to the Ce135 sample the optical band gap decreased slightly by about 84.22 meV compared with the band gap energy of the C60 sample, which can be related to RE 3+ incorporation to the molecule and the average grain size.This band gap decrease can be explained due to the substitution in the sub-lattice of cadmium atoms (ionic radii ~0.95 Å) by cerium (ionic radii 1.15 Å) and europium (ionic radii 1.09 Å) atoms that are larger.Figure 8 shows the photoluminescence spectra of the single CdS for the four different synthesis times.The energy of the radiative transitions and the linewidth at half-maximum (FWHM) of each band have been determined by a quantitative fit to the experimental PL spectra using a sum of Gaussian line distributions, the dominant peaks were first fit and the additional peaks were added as were necessary.For sample C65, which presents best luminescence, the radiative bands are observed at 434 nm (2.86 eV) (violet), 523 nm (2.37 eV) (green), 565 nm (2.19 eV) (orange), 659 nm (1.88 eV) (red) and 898.21 nm (1.38 eV) (infrared) eV that are labelled by A, B, C, D and E in the PL spectrum of the C65 sample.The band A is associated a radiative transition band-to-band, which is higher than the single CdS band gap for 358 meV.This is due to the quantum confinement associated with grain size since it is less than the exciton Bohr radius.The band B is clearly identified on as-grown CBD-CdS at 523 nm (2.37 eV), which is called the optical signature of interstitial oxygen 39 .Its relative intensity increases with the synthesis time until it reaches a maximum at 65 min and then decreases for longer synthesis times, as is observed in the inset of Fig. 8.It has reported that in samples grown by close-spaced sublimation (CSS) technique the effect of oxygen is different since the use of oxygen during the growth leads to the appearance of Materials Research eV), this band named the "orange band" has been observed between 610 to 596 nm (2.03-2.08 eV) 41,42 , it is possibly associated to a donor-acceptor pair (DAP) radiative transition between a donor level related to interstitial cadmium (I cd 2+ ) and an unidentified acceptor level.The ionization energy of this donor has estimated to be between 120 and 206 meV, which corresponds to I Cd 2+ 39 .Finally, the broad and weak peak observed in 892 nm (1.39 eV), which disappears when synthesis time increases, it is in the infrared region and is associated with unidentified deep impurities.In the inset of Fig. 8 shows the behaviour of the intensities the four main bands, clearly is observed that the band C is dominant for 65 min and very weak for other times.In Fig. 9 the photoluminescence spectra of the Eu 3+doped CdS samples are shown.It is clearly observed that in the PL spectra the band called the optical signature of interstitial oxygen at ~523 nm (2.37 eV) is not present, which is indicative that the incorporation of rare earths in CdS lattice decreases the concentration of interstitial oxygen.The luminescence spectrum of the Eu115 sample, which presents the best luminescence, exhibits four main radiative transitions at 431 nm (2.88 eV), 576 nm (2.15 eV), 683 (1.81 eV) and 840 (1.48) nm (eV).The violet emission peak a at 431 nm is clearly observed, which is associated to radiative transition band-to-band.This band has been related to the radiative transition of CdS nanostructures into bandedge and surface defects due to the quantum confinement effect because of grain size is lower than the exciton Bohr radius, which is greater by 409 meV than its band gap.The dominant radiative peak b at 576 nm (2.15 eV), which has been associated to the intra-4f radiative transitions of Eu 3+ ions that corresponds to the magnetic dipole transition ( 5 D 0 → 7 F 1 ), which was blue shifted compared to previous  39 .In addition, the band C could be attributed to the CdO complexes that would be formed during the growth due to the presence of oxygen during the nucleation of the layer, since the CdO band gap is about 574 nm (2.16 eV) 40 .For three studied CBD-CdS samples, another broad band, band D, is observed around 659 nm (1.88 results 39,43 .In Eu 3+ -doped CdS, the 5 D 0 → 7 F 1 transition is mainly magnetically allowed (magnetic-dipole transition).The surface-defect radiative transitions are caused by surface states, such as sulphur vacancies and/or sulphur dangling bonds created by doping are in the wavelength range from 700-500 nm (1.77-2.48eV) 32 .Therefore, the peak c at 683 nm (1.81 eV) is associated with surface defects of the CdS nanocrystals.Additionally, the peak d at 840 nm (1.48 eV) is region of low energies, for which is associated at deep residual impurities.These observations indicate that a part of Eu 3+ ions, contained in CdS nanocrystals and the energy can be significantly transferred from the host CdS to Eu 3+ ions 44,45 .Upon excitation, the energy from non-radiative recombination of electron-hole pairs can be transferred to the high energy levels of the Eu ions 46,47 .The mechanism of the intensification of (rare earth emission) REE has already been reported 47 , which also supports the observed results of the present study.These results indicate that the adsorbed CdS particles significantly influence the excitation of 4f electrons in rare-earth ion.A significant change in the intensity of the emission bands was observed for the samples prepared using different synthesis time, which are due to the variation in the structures.As is seen in the inset of Fig. 9, peak b is the one that increases its intensity with the synthesis time, reaching a maximum of 115 min and then decreasing.It may also be attributed to the change in the energy transfer rate with particle size variation and the shape of the nanocrystals.432 nm corresponds to the band-band transition.The band β at 602 nm is the dominant band of PL spectrum, which is associated to Ce 3+ incorporated to the sub-lattice of Cd.Therefore, it is considered that the radiative transitions present in the luminescence of the Ce 3+ -doped CdS have the same origin as those present in the PL of the Eu 3+ -doped CdS and their redshift is due to the ionic radius of the Ce 3+ is higher than the Cd, which strains the lattice.

Conclusions
(Eu,Ce)-doped CdS nanostructures were synthesised by chemical bath deposition technique.Synthesised samples showed cubic zinc-blende crystalline phase of CdS, which was obtained by powder XRD and HRTEM analyses.The incorporation of rare earths in the CdS lattice was confirmed by X-ray diffraction.Transmittance spectra reveal the blueshift of absorption edge by incorporation of rare earths, which allowed estimate the band gaps of RE 3+ -doped CdS, which confirms the quantisation effect by grain size in the synthesized samples.It was observed that the structure, crystallite size and the band gap of the europium and cerium doped CdS nanocrystals can be finely controlled by simply varying the synthesis time.The room temperature photoluminescence of the undoped CdS presents the bandband transition associated to CdS nanocrystals and the transitions associated with residual impurities and structural defects, mainly the optical signature of interstitial oxygen.The samples doped with rare earths present the band-band transition, in addition the radiative band associated to the intra-4f radiative transitions of Eu 3+ ions that corresponds to the magnetic dipole transition ( 5 D 0 → 7 F 1 ).For the case of cerium-doped samples, the results obtained were similar to those for europium.The results confirm that at least a part of the Eu 3+ ions is effectively doped into CdS nanocrystals and the energy transfer occurs from CdS nanocrystals to Eu 3+ ions.

Figure 3 .
Figure 3.It illustrates the grain size as function of synthesis time for single CdS and RE-doped CdS.The inset shows the lattice parameters for undoped and doped CdS.The dash lines are some figures-of-merit for following the behaviour of experimental points

Figure 4 .
Figure 4. HRTEM micrographs of the typical CdS samples: a) C60, b) Eu100 and c) Ce130.Additionally, in the insets the histograms are shown to estimate the grain size of the nanoparticles

Figure 5 .
Figure 5. Transmittance spectra of CdS samples synthesized at different synthesis time

Figure 7 .Figure 8 .
Figure 7.It shows band gap energy as a function of synthesis time for three sample series

Figure 6 .
Figure 6.a) It is shown the first derivative of the optical absorption (OD) as a function of the photon energy (hν), for three different synthesis time values.b) Figure displays the second derivative of OD versus E, which allows calculate the band gap energy.The arrows indicate the position of band gap energy, E g

Figure 9 .
Figure 9.It presents the photoluminescence spectra of Eu-doped CdS.In addition, it is shown the deconvolution of dominant PL spectrum, Eu115 sample.In the inset is illustrated the radiative transition bands of the PL spectra as function of the synthesis time

Figure 10 .Figure 11 .
Figure 10.It illustrates the photoluminescence spectra Ce-doped CdS for three synthesis times, in which is presented the PL deconvolution of the Ce100 sample.In inset is shown the intensity of four the main radiative transition as function of synthesis time

Figure 10
Figure10shows the photoluminescence spectra of the Ce 3+ -doped CdS, which are very similar to those obtained with the Eu 3+ -doped CdS.The photoluminescence spectrum of the sample Ce100, which presents the best luminescence, shows radiative bands at 432 nm (2.87 eV), 602 nm (2.06 eV), 726 nm (1.71 eV) and 875 (1.42 eV).The band α at

Table 1 .
It presents the CdS:RE 3+ films grown and the doping volume added to each one.The Cd, S and RE concentrations in the samples were estimated by EDS.The average errors with that were calculated percentage masses of different elements were for cadmium 1.25%, sulphur 0.35%, europium 0.25% and for cerium 0.30%.For a stoichiometric compound (CdS), the percentage atomic masses are cadmium 77.81% and 22.19% sulphur.The number that accompanies the sample name corresponds to the synthesis time.

Table 2 .
Mean grain size of the nanofilms obtained by the Debye-Scherrer equation for the ZB (111) preferred direction showing their dependence on the synthesis time.In addition, it presents the grain sizes obtained by TEM.Additionally, the interplanar distance estimated by X-ray diffraction and by HRTEM are shown.