A. Irkhina*a,
S. Levcenkoa,
V. Hinrichsb,
P. Plateb and
T. Unold*a
aDepartment Structure and Dynamics of Energy Materials, Helmholtz-Zentrum Berlin für Materialien und Energie GmbH, Berlin 14109, Germany. E-mail: unold@helmholtz-berlin.de; anastasia.irkhina@helmholtz-berlin.de
bInstitute for Solar Fuels, Helmholtz-Zentrum Berlin für Materialien und Energie, Berlin 14109, Germany
First published on 16th February 2017
We report the colloidal synthesis of small-sized Cu2ZnSnS4 (CZTS) nanocrystals (NCs) via a hot-injection method using zinc and tin acetates in combination with copper acetylacetonate as metal precursors. A systematic investigation of the influence of the injection temperature in the range from 190 °C to 300 °C on the size distribution, composition and phase purity of CZTS nanocrystals has been performed. It has been found that temperature plays the key role in changing of the metal sources reactivity and influences the final composition of the nanocrystals. The mechanism of nanocrystal formation has been investigated by Raman spectroscopy of aliquots of their solutions. It starts from the formation of a Cu2−xS phase as a core followed by the incorporation of Zn2+ and Sn4+ atoms into its structure regardless of injection temperature.
Colloidal synthesis routes allow tuning of the composition, phase and size distribution for the wide range of elemental and binaries nanocrystals.3–6 The application of this method to ternary and quaternary systems such as CuInS(Se)2, CuInxGa1−xS2 and CZTSSe gives the opportunity to obtain NCs with a specifically tuned energy band gap and optoelectronic properties.7–9
Due to the various degrees of freedom of the quaternary CZTS compound, secondary phases are easily formed and composition control is an important aspect in the synthesis of this material.10,11 The nature of precursors and growth temperature value play an important role for the nucleation and growing processes.
CZTS nanocrystals with narrow size distribution have been obtained by hot-injection synthesis, by the ‘heat up’ approach or by thermal decomposition of single-source precursors such as metal dithiocarbamate complexes.12–14 Despite the fact that the tetragonal kesterite phase is the most thermodynamically stable phase for the CZTS compound, nanocrystals with metastable wurtzite structure have been also synthesized utilizing thiols as sulfur source which has a strong coordination between thiol group and metal cations (Cu+, Zn2+).15,16 It has been noted that for the formation of the kesterite phase it is necessary to use low reactivity precursors, solvents and surfactants with weak coordination toward metal cations such as oleylamine (OAm).17
In terms of the nucleation rate of the nanocrystals it is very important to control the reactivity of the elemental sources. For instance, using such chemicals as thiourea (TU) or thioacetamide (TAA) leads to a lower rate of H2S release in comparison to an elemental sulfur source.18 On the other hand, differences in and a deliberate tuning of the reactivity of the metal precursors should considered.
The hot injection method has several advantages over other wet chemical methods such as the potential high quality of the obtained nanocrystals, narrow size distributions and the control of the mean particle size. Although there are many reports of CZTS nanocrystals synthesized by the hot-injection method, the influence of the injection temperature on the nanocrystal nucleation and growth has not been extensively investigated so far.19 Besides that, it is still unclear which size of the NCs is better suited for solar cells fabrication. Previously reported recipes based on this technique usually result in nanocrystals with an average size of 7–20 nm.1,18,20,21 In this paper we report a recipe for the synthesis of small-sized CZTS nanocrystals (∼4–5 nm), where zinc acetate, tin acetate and copper acetylacetonate as metal precursors in combination with OAm have been used. The effect of the injection temperature on the morphology, chemical composition and secondary phase formation has been systematically investigated. Based on the detailed Raman scattering analysis of the aliquots taken at different growth time, the formation mechanism of CZTS nanocrystals has been proposed.
Separately the sulfur precursor solution (1 M) was prepared by dissolving of elemental sulfur in oleylamine in a 25 ml two-neck flask. The solution was placed under vacuum at 60 °C in an ultrasonic bath for 1 hour. The flask was connected to the nitrogen line with permanent heating until total dissolution of the sulfur powder.
4 ml of sulfur solution at 60 °C was injected to the metal precursor solution via a rubber septum at varied temperatures. After the injection the reaction mixture immediately changed the color to dark-brown. Injection temperatures between 190 °C and 300 °C were used. The system was kept at the injection temperature for 40 min and then cooled down and disconnected from the heating source. The experimental details are summarized in Table S1 (ESI†).
Size control of NPs can be obtained via thermodynamic and/or kinetic means. According to the theory of homogeneous nucleation a decrease of the nanocrystal size can be achieved by a decrease of the critical radius rcr, which represents the most stable particle size for the system due to the lowest Gibbs free energy. This value can be decreased by increasing the supersaturation or by reduction of the surface energy of the nanocrystals, which is influenced by the ligands, solvents and additives in the solution.24 Thus, the reported preferential formation of small particles may have different origins, which will be discussed in the following.
As has been previously reported, an increasing amount of oleylamine reduces the size of the nanocrystals by lowering the surface energy of the particles.23,25,26 However, we found that the reduction of the amount of OAm does not lead to any significant increase of the average nanocrystal size (Fig. S1 in ESI†).
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Fig. 2 Scheme of the experimentally observed decreasing of the nanocrystal size of Cu2−xS, CTS and CZTS with the increasing amount of acetates in the reaction system. |
In order to understand the process of nanocrystal formation the composition of the various synthesized NCs was characterized by LA-ICP-MS (Table 1). For this purpose, two syntheses for each injection temperature have been performed.
Temperature | Sample series | Cu/Sn | Zn/Sn |
---|---|---|---|
190 °C | a | 1.97 ± 0.25 | 1.10 ± 0.13 |
200 °C | a | 2.06 ± 0.26 | 1.13 ± 0.13 |
b | 2.30 ± 0.27 | 1.29 ± 0.14 | |
225 °C | a | 1.60 ± 0.24 | 0.87 ± 0.11 |
b | 1.7 ± 0.2 | 0.75 ± 0.09 | |
250 °C | a | 1.78 ± 0.20 | 1.03 ± 0.12 |
b | 1.66 ± 0.27 | 0.93 ± 0.14 | |
275 °C | a | 1.86 ± 0.24 | 1.04 ± 0.13 |
b | 1.82 ± 0.25 | 0.88 ± 0.12 | |
300 °C | a | 1.87 ± 0.26 | 0.91 ± 0.12 |
b | 2.13 ± 0.35 | 0.74 ± 0.10 |
Although the as-prepared metal precursor solution was Cu-poor and Zn-rich, the quantitative elemental analysis shows that depending on the injection temperature, the Cu/Sn and Zn/Sn ratios of the nanocrystals deviate from the precursor values (Fig. 3).
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Fig. 3 Temperature dependence of the Cu/Sn and Zn/Sn ratios of the obtained nanocrystals according to the LA-ICP-MS analysis (2 series of samples). |
We observe that an injection temperature below 200 °C results in a significant Cu- and Zn-richness of the NCs, which means that Sn is poorly incorporated in nanocrystals at low temperature. Further increasing of the injection temperature leads to decreasing of Cu/Sn and Zn/Sn ratios with the lowest value at 225 °C and thereafter increasing slightly again. The weight-in ratios can be achieved in the range of temperatures between 225 °C and 275 °C injection temperature.
The change in cation ratios can be partially explained according to the principle of hard and soft Lewis acids and bases (HSAB).28 Lewis bases donate pairs of electrons and Lewis acids accept pairs of electrons.29 The Cu+ ion behaves as a soft Lewis acid after the Cu(acac)2 decomposition and will have the fastest reactivity with S2− which is a soft Lewis base.30 It has been previously reported that the formation of Cu2−xS phase is the first step of wurtzite and kesterite CZTS nanocrystals formation.31,32 The lowest reactivity can be expected from Sn4+ because of the low affinity of this hard acid for a soft base. Because Zn2+ is a borderline acid, its reactivity to sulfur will be lower than of Cu+, but faster than of Sn4+. At the same time due to basicity of oleylamine, high coordinating power between Sn4+ ion and OAm can lead to Sn-rich nuclei at higher temperatures which influence the Zn/Sn ratio. Thus, in order to achieve Cu-poor composition as desired for CZTS solar cells, the synthesis of nanocrystals by hot injection should utilize reaction temperatures between 225 °C and 275 °C. It can be assumed that at these synthesis temperatures the reactivity difference of metal ions is eliminated and thus it leads to a more homogeneous growth of particles.
In order to investigate the possibility of increasing the Zn content in the NCs additional experiments have been performed with higher weight-in value of Zn/Sn = 1.2 (Fig. S3 in ESI†). However, we found that at Tinj = 225 °C increasing of the zinc content leads to the formation of strongly Cu-rich nanocrystals which is undesirable for solar cells application. At the same time at Tinj = 250 °C there is no significant change in metal composition in comparison with the previous experiments with initial metal ratio Zn/Sn = 1.05. This indicates that the Zn amount which can be incorporated in Cu-poor CZTS nanocrystals is limited.
It was experimentally and theoretically shown that the ternary phase diagram of the Cu2S–ZnS–SnS2 system exhibits a very narrow region of stability for single-phase kesterite.33–35 From a thermodynamic equilibrium point of view high excess of copper, zinc or tin is expected to lead to the formation of secondary phases such as Cu2−xS and ZnS, SnxSy, which should be identifiable by XRD or Raman.36 On the other hand, it is conceivable that comparatively more metal atoms might be segregated at the surface of nanocrystals, which could result in an essentially enlarged single phase existence region for nanocrystals.37
Fig. 4 shows XRD patterns of the obtained nanocrystals which exhibit three prominent peaks attributed to the kesterite CZTS (112), (220) and (312) crystal planes (JCPDS 00-026-0575).
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Fig. 4 XRD patterns of as-synthesized nanocrystals with different injection temperatures compared to the reference patterns of cubic ZnS, cubic and tetragonal CTS, kesterite CZTS orthorhombic SnS. |
Due to the similar lattice parameters of tetragonal CTS (JCPDC 01-089-4714), cubic CTS (JCPDC 01-089-2877) and sphalerite ZnS (JCPDC 01-071-5975) the presence of these secondary phases cannot be excluded. No reflexes of the Cu2−xS phase have been observed. It can be seen that for the samples obtained at 250 °C and 275 °C injection temperatures two additional small peaks are present near the most intense (112) peak. This is a possible indication of the presence of stacking faults in the structure.38,39 For the sample synthesized at 300 °C, the secondary phase SnS with orthorhombic herzenbergite structure (JCPDS 01-071-3679) has been found. The line broadening observed in the XRD patterns is common for nanocrystal XRD patterns because of the finite crystallite size. The full width at half maximum (FWHM) of the diffraction peaks increases with decreasing crystallite size. The average coherence volume associated with the crystallite size can be estimated from FWHM of the most intensive diffraction peak (112) using the Scherrer formula under the assumption of spherical nanocrystals: D = Kλ/(βcos
θ). The resulting estimates for average crystallite sizes are given in Table 2. The values for low temperature synthesis (190–225 °C) are in very good agreement with the TEM-derived nanocrystal sizes. Samples giving larger average particle sizes from XRD probably contain a fraction of NCs having diameter larger than the size determined from TEM which indicates the increasing polydispersity with temperature.
Temperature | TEM average particle size, nm | XRD crystallite size (112), nm |
---|---|---|
200 °C | 5.1 ± 0.9 | 5 |
225 °C | 3.9 ± 0.6 | 3.6 |
250 °C | 4.6 ± 0.7 | 2.9, 17 (15%) |
275 °C | 3.6 ± 0.7 (22 ± 5) | 3.1, 19.2 (30%) |
300 °C | — | 21.2 |
To gain further information on the kesterite as well as phase purity, Raman spectroscopy was employed. The Raman spectra of a CZTS nanocrystals obtained with different injection temperatures are presented in Fig. 5a (λexc = 632.8 nm).
The Raman spectra obtained for nanocrystals synthesized at different injection temperatures (190–300 °C) is characterized by the main broad peak located at 337 cm−1 and a shoulder at 375 cm−1, corresponding to the reported characteristic peaks for kesterite polycrystalline films.40
Also the shoulder at ∼300 cm−1 can be observed, which can be explained by CZTS modes at 289 and 302 cm−1.41 Despite of the very small size of nanocrystals no evidence of phonon confinement is observed probably because of the strain effect.42 As can be seen in Fig. 5a the increase of the injection temperature leads to a decrease of the FWHM of the main A mode at 337 cm−1. To evaluate the changes in FWHM with an increasing of Tinj we deconvolute Raman spectra with 4 Lorentzians located at about 250, 294, 338 and 373 cm−1. A representative example of this procedure is shown on Fig. 5b for Tinj = 250 °C. We determine that the FWHM of A mode varies from 45 to 25–30 cm−1 when Tinj increases from 190 to 300 °C (Fig. 5c).
Due to the broadening of peaks it is not possible to conclude about the presence of the CTS phase (peaks at 297 and 337 cm−1 for tetragonal CTS, 303 cm−1 and 355 cm−1 for cubic CTS, 318 cm−1 for orthorhombic CTS).40,43 To study CTS nanocrystals the identical synthesis with no Zn precursor at 225 °C was performed and Raman measurements were carried out to indicate the growth process (Fig. S4 in ESI†). For as-synthesized nanocrystals two main characteristic peaks at 291 cm−1 and 350 cm−1 of monoclinic CTS phase and 318 cm−1 of orthorhombic CTS phase were found.44 Therefore we exclude a CTS phase contribution to the shoulder at 300 cm−1 in Raman of CZTS NP.
At the highest injection temperature (300 °C) a peak45,46 at 191 cm−1 indicative of SnS nanocrystals has been observed (Fig. 5a), supporting our XRD results. To determine the presence of the ZnS phase, UV Raman scattering measurements (λexc = 325 nm) corresponding to near-resonant excitation for the ZnS phase were performed (Fig. S5 in ESI†). Only a very weak peak at 347 cm−1 is present for Tinj = 190, 200, 225 and 300 °C, with the highest intensity corresponding to Tinj = 200 °C. Thus the presence of the ZnS phase in some samples could be identified.
Optical transmission measurements were performed for all synthesized nanocrystals. In Fig. 6 the derived absorption is shown for different hot injection temperatures. Analysing the data further it is found that for the NCs synthesized between 225–275 °C a band gap of approximately 1.5 eV can be derived by modeling the absorption coefficient, however with the presence of very substantial subband gap absorption (Fig. S6 in ESI†).
For the samples synthesized at injection temperatures of 190 °C and 200 °C a broad absorption peak in the near-infrared region can be observed. This can be a result of the localized surface plasmonic resonance (LSPR) possibly corresponding to a Cu2−xS phase.47 Since there is no evidence of the presence of Cu2−xS phase in XRD and Raman for this sample, formation of Cu2−xS–CZTS heterostructure due to the insufficient metals interdiffusion at this temperatures can be an explanation.48 The estimated band gap energy of 1.5 eV corresponds well to the value found for CZTS-bulk crystalline and polycrystalline material.49,50 The presence of strong bandtails can indicate the presence of defects at the surface and in the interior of the nanocrystals, which has previously been shown by high resolution transmission electron microscopy.51
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Fig. 7 Evolution of Raman signal with increasing growth time at (a) 200 °C, (b) 250 °C and (c) 300 °C. |
The first aliquot was always taken immediately after injection (<2 s) of the sulfur precursor and indicated as 0 min time. For all injection temperatures a pronounced peak at 474 cm−1 and a weak mode at 263 cm−1 originating from Cu2−xS phase can be observed.52,53 The aliquots for this synthesis time have green color which is typical attributed in literature to formation of covellite CuS nanocrystals.54–56 With the exception of the sample synthesized at Tinj = 200 °C (Fig. 7a), Cu2−xS phases were not detected in other samples after 5 min of the reaction time (Fig. 7b and c) which is also characterized by changing of color of the aliquots from green to dark brown. We also observe that the Cu2−xS peak decreases faster with increasing injection temperature.
With the decrease of the Cu2−xS mode intensity, a broad peak centered at 337 cm−1 corresponding to the main kesterite A-mode emerges and becomes more pronounced during the growth time. The transition from the Cu2−xS phase to CZTS occurs at an earlier time for the higher injection temperatures (Fig. 7). We assume that this is due to a faster incorporation of Zn2+ and Sn4+ ions into the Cu2−xS crystal structure. However, at about 5–20 min after injection at 300 °C a new mode at 318 cm−1 (Fig. 7c) appears, which could be due to formation of the orthorhombic Cu3SnS4 phase.44 For the growth time >20 min we do not observe this Cu3SnS4 phase probably due to complete transformation to the CZTS phase. Note that at Tinj = 275 °C the Cu3SnS4 phase can be observed during the first minute of the synthesis (Fig. S7 in ESI†). The appearance of Cu3SnS4 at higher temperature is an indication that the competing ternary phase formation process delays complete formation of CZTS. Remarkably the Cu3SnS4 phase growth is influenced by both factors: Zn2+ ions presence and the growth temperature as the CTS formation can already start at Tinj = 225 °C without Zn precursor (Fig. S4 in ESI†). Overall, Fig. 8 shows NP formation path dependence on time and reaction temperature. Our data suggest that the growth time of about 40 min leads to complete CZTS NP formation in the temperature range of 190–300 °C.
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Fig. 8 Scheme showing nanocrystals evolution with time and temperature obtained from Raman spectroscopy measurements on aliquots from reaction solution. |
The CZTS nanocrystal formation mechanism at different temperatures has been studied by using Raman characterization of aliquots, taken during nanocrystal growth. We observed that Cu2−xS seeds form first, while the further incorporation of Zn2+ and Sn4+ ions into the structure strongly depends on the injection temperature. The time of complete transformation from the Cu2−xS phase into the CZTS phase decreases from about 40 to 1 min, when the growth temperature increases from 200 to 300 °C. The growth at high injection temperatures (∼275–300 °C) is characterised by the formation of a competing orthorhombic CTS phase during the first 20 min of the nanocrystal synthesis.
Footnote |
† Electronic supplementary information (ESI) available: TEM image for the sample obtained with lower amount of oleylamine; TEM images of Cu2−xS, CTS, ZnS and SnxSy nanocrystals obtained with same reaction conditions as CZTS nanocrystals; temperature dependence of Cu/Sn and Zn/Sn ratios of NCs synthesized with weight-in ratio of Zn/Sn = 1.2; evolution of Raman signal of CTS nanocrystals with increasing of the growth time at 225 °C; Raman spectrum of nanocrystals synthesized at different injection temperatures measured with UV excitation laser; absorption coefficient of CZTS nanocrystals in conjunction with model. See DOI: 10.1039/c6ra28588k |
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