D. Raptisa,
G. Sfyrib,
L. Sygellouc,
V. Dracopoulosc,
E. Nouri†
a and
P. Lianos*a
aDepartment of Chemical Engineering, University of Patras, 26500 Patras, Greece. E-mail: lianos@upatras.gr
bPhysics Department, University of Patras, 26500 Patras, Greece
cFORTH/ICE-HT, P.O. Box 1414, 26504 Patras, Greece
First published on 13th May 2016
Antimony sulfide solar cells have been studied with the purpose to investigate an easy and efficient procedure of antimony sulfide deposition on mesoporous titania films. Two principal deposition methods have been studied based on different sulfur precursors (thiosulfate vs. thiourea) and chemical bath vs. spin-coating deposition. The two approaches led to the same practical effect thus highlighting spin-coating deposition using antimony chloride and thiourea as the simplest and most practical method of construction of antimony sulfide/titania photoanodes. Poly(3-hexylthiophene) was employed as a hole-transporter while PEDOT:PSS and Ag were used as the counter electrode. They were all deposited under ambient conditions. XPS measurements provided information about antimony sulfide stoichiometry while UPS measurements gave the ionization potential in each case. Both deposition methods led to sulfur-deficient antimony sulfide.
Fig. 1 Energy states corresponding to the components of a typical antimony sulfide solar cell.3,6 |
A major concern in the study of antimony sulfide solar cells is the quality of the Sb2S3 synthesis product. First, if such cells can hold the ambition of making it to the market, antimony sulfide should be deposited by an easy procedure under ambient conditions. The standard method of Sb2S3 formation in mesoporous titania is aqueous chemical bath deposition at low temperature (≤10 °C) using SbCl3 and sodium thiosulfate as precursors.3,12–14 Formation of Sb2S3 in an aqueous environment is described by the following reactions:7
2SbCl3 + 3Na2S2O3 → Sb2(S2O3)3 + 6NaCl |
Sb2(S2O3)3 + 6H2O → Sb2S3 + 3HSO4− + 3H3O+ |
Cooling is necessary in order to slow down these reactions, avoid precipitation and allow adsorption in the mesoporous oxide film. Other researchers have followed the opposite route by growing Sb2S3 in mixed water–alcohol environment at high temperature in an autoclave.4 A very interesting approach was recently adopted by Choi and Seok9 who deposited Sb2S3 on mesoporous titania films by a very simple room temperature method involving spin-coating of a concentrated solution of SbCl3 and thiourea in dimethylformamide (DMF) followed by annealing in inert atmosphere. The results were impressive since the efficiency of the obtained solar cells was comparable to champion reports9,15,16 at the same time offering simplicity and practicality of cell construction procedures. This room temperature synthesis of antimony sulfide proceeds through the formation of a complex with thiourea (TU)9
SbCl3 + 2TU → [Sb(TU)2]Cl3 |
In the present work, we have employed and compared the above two main procedures of Sb2S3 synthesis in mesoporous titania and have systematically characterized the obtained materials in order to appreciate under similar conditions the capacity of each procedure to produce efficient photoanodes.
Fig. 2 XRD analysis of Sb2S3/TiO2/FTO films. The small circles indicate the presence of stibnite, i.e. the chief crystalline form of antimony sulfide. |
The composition of the antimony sulfide films in each case was studied by XPS. The survey spectra (not shown) of the samples showed the presence of the following elements: Sb, S, Ti, O and C. Ti2p3/2, which was at a binding energy 459.0 eV was assigned to the Ti4+ chemical state. Fig. 3 shows the XP spectra of S2p for (1) spin coating and (2) chemical bath samples. The S2p spectra of both samples consist of one main peak at binding energy 161.8 eV assigned to sulphur in Sb2S3 bonds whereas a low intensity peak at ∼168 eV reveals the presence of small amount of S–O bonds. Fig. 4 shows the XP spectra of Sb3d3/2. The peak is analyzed into two equal width components differing by 0.8 eV and assigned to Sb2S3 and to Sb2O3 chemical states. The data extracted from Fig. 3 and 4 are listed in Table 1. The atomic ratio of Sb:S was calculated with 10% experimental error. It has to be mentioned that the Sb3d3/2 was chosen for analysis because of the overlapping of Sb3d5/2 with O1s peak.
Fig. 4 Deconvolution of XPS-Sb3d3/2 core level spectra of (1) spin-coated and (2) chemical-bath-deposited sample. |
Method of film deposition | Elements detected | Chemical state | Atomic ratio Sb:S | Ionization potential (eV) |
---|---|---|---|---|
Chemical bath | Ti, O, C, Sb, S | Ti4+(TiO2), Sb5+, S–Sb, S–O | 1:1.10 | 5.8 |
Spin-coating | Ti, O, C, Sb, S | Ti4+(TiO2), Sb5+, S–Sb, S–O | 1:0.78 | 5.6 |
From these results it is concluded that both processes have led to sulfur-deficient samples since the Sb2S3 stoichiometry would necessitate 1.5 atoms of sulfur for each atom of antimony. The quantity then of sulfur was lower than expected, in particular, in the case of the spin-coated sample. Table 1 also lists the calculated ionization potentials obtained by UPS measurements. The obtained values were a bit higher (4–7%) than those presented in previous publications3,6 and they are close to each other within experimental error. Therefore, the diagram of Fig. 1 is justified on the basis of these data.
The light harvesting capacity of the Sb2S3/TiO2/FTO photoanodes can be appreciated by the diffuse reflectance UV-vis spectra of Fig. 5. The absorbance in the two cases cannot be safely compared when the data are obtained by diffuse reflectance, however, it may be argued that the spin-coating deposition method demonstrated higher capacity of photon harvesting. The important conclusion to keep is that in both cases samples were deeply colored and they were strong light absorbers. Also both spectra had practically the same absorption threshold located around 740 nm.
Fig. 5 Diffuse reflectance absorption spectra Sb2S3/TiO2/FTO photoanodes made by (1) chemical bath and (2) spin-coating deposition. |
Action spectra have been recorded by using devices made by employing the two types of photoanodes. The obtained results are shown in Fig. 6. The two spectra were very similar. Absorption threshold perfectly matched action spectra threshold, indicating that in both cases Sb2S3 is the functional light harvesting species. The slightly higher maximum obtained with the spin-coated sample may be associated with the higher absorbance in that case. Fig. 6 suggests the greater importance of longer wavelength photons in current conversion. However, curve 3 of Fig. 6 gave a different form of IPCE spectrum. Curve 3 corresponds to a cell based on a photoanode made by the spin-coating method but annealing was carried out in air and not in an inert atmosphere as in the case of curves 1 and 2. This result came as a surprise and in order to verify its validity, 5 different cells were constructed and tested. It was then verified that photoanodes annealed in inert atmosphere led to greater contribution from longer wavelength absorbing antimony sulfide species. Annealing in air has been studied in our previous publication.3 In that case, antimony oxide formation was detected and further loss of sulfur was recorded, i.e. the samples were then even more sulfur deficient.
Fig. 6 Action spectra of solar cell devices made with Sb2S3/TiO2/FTO photoanodes based on (1) chemical bath and (2) spin-coating deposition. Curve (3) corresponds to a photoanode made by spin-coating but calcined in air. The maximum values of the action spectra are adapted to the corresponding values of current density given in Table 2. |
The above data support the fact that antimony sulfide deposited on titania films by the two methods may both be used as sensitizers of titania in HSCs. The current–voltage data obtained by characterization of the constructed devices are presented in Fig. 7 and Table 2. The two methods of antimony sulfide deposition produced the same practical effect. Spin-coating yielded a bit higher current and voltage but suffered of a lower fill factor. Over all, chemical bath deposition led to cells of slightly higher efficiency but the difference is judged as being within experimental error. Therefore, both methods are applicable and since spin coating is much simpler and handy, it is suggested as the method of choice. The results of Fig. 7 and Table 2 report improved data compared to data reported in our previous publication.3 In any case, differences are within experimental error.
Fig. 7 Current density–voltage curves recorded with solar cell devices comprising Sb2S3/TiO2/FTO photoanodes based on (1) chemical bath and (2) spin-coating deposition. |
Method of film deposition | Jsc (mA cm−2) | Voc (volts) | FF | η% |
---|---|---|---|---|
(1) Chemical bath | 18.9 | 0.50 | 0.40 | 3.8 |
(2) Spin coated | 19.8 | 0.53 | 0.33 | 3.5 |
We have also examined the possibility of hole transporting material substitution and its effect on the behavior of antimony sulfide solar cells. The results are shown in Fig. 8 and Table 3. It is obvious that the best combination is P3HT/PEDOT:PSS/Ag. Absence of PEDOT:PSS had a detrimental effect on cell efficiency while the employment of spiro-OMETAD, which has been very successful in the case of perovskite solar cells is of no use in the case of antimony sulfide solar cells. This of course, is not a particular problem since both P3HT and PEDOT:PSS are more easy and less expensive to synthesize and this is reflected on their commercial prices. The HOMO level of spiro-OMETAD is located at about −5.22 eV,17 i.e. very close to the presently used P3HT (−5.2 eV), therefore, there exist no potential constraints for its acting as hole scavenger. Apparently, the low efficiency obtained with spiro-OMETAD is a matter of poor interface forming between antimony sulfide and this small-molecule hole transporter. Obviously, this should be a subject of further research.
Hole-transporter/counter electrode | Jsc (mA cm−2) | Voc (volts) | FF | η% |
---|---|---|---|---|
(1) P3HT/PEDOT:PSS/Ag | 18.9 | 0.50 | 0.40 | 3.8 |
(2) P3HT/Au | 15.8 | 0.35 | 0.30 | 1.7 |
(3) Spiro-OMETAD/Au | 4.5 | 0.34 | 0.40 | 0.7 |
Sb2S3 was deposited on a freshly prepared titania film either by chemical bath deposition or by spin-coating a precursor solution. In the first case, the bath was prepared by dissolving 650 mg of SbCl3 in 2.5 ml of acetone and subsequently adding 25 ml of 1 M Na2S2O3 aqueous solution at 10 °C and sufficient water to make a final volume of 75 ml3. After many tests, we concluded that the optimum time of deposition is 2 h at 10 °C. The as-deposited orange films of amorphous Sb2S3 were annealed at 300 °C for 10 min in Ar atmosphere. After annealing, the color of the samples became dark-brown. In the second case, a precursor solution was prepared by dissolving 1 M of SbCl3 in DMF, stirring for 30 min and then adding 2 M of thiourea and stirring for an additional 30 min.9 This solution is stable if stored in the dark. The next step was to spin-coat the precursor solution on the titania film at 2000 rpm for 1 min followed by calcination in Ar atmosphere at 300 °C for 10 min.
XPS experiments were carried out in an ultra high vacuum system (UHV) which consists of a fast entry specimen assembly, a sample preparation and an analysis chamber. The base pressure in both chambers was 1 × 10−9 mbar. Unmonochromatized MgKα line at 1253.6 eV and an analyzer pass energy of 97 eV, giving a full width at half maximum (FWHM) of 1.6 eV for the Au4f7/2 peak, were used in all XPS measurements. The binding energy (BE) scale was calibrated by assigning the main C1s peak at 285.0 eV. UPS spectra were obtained using HeI irradiation with hν = 21.22 eV produced by a UV source (model UVS 10/35). During UPS measurements the analyzer was working at the Constant Retarding Ratio (CRR) mode, with CRR = 10. A bias of −12.29 V was applied to the sample in order to avoid interference of the spectrometer threshold in the UPS spectra. The high and low binding energy and highest occupied cutoff positions were assigned by fitting straight lines on the high and low energy cutoffs of the spectra and determining their intersections with the binding energy axis.
Footnote |
† Permanent address: Department of Materials Science and Engineering, Sharif University of Technology, Azadi Str., Tehran, Iran. |
This journal is © The Royal Society of Chemistry 2016 |