1. Introduction

OJAppS

Open Journal of Applied Sciences

2165-3917

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10.4236/ojapps.2019.99059

OJAppS-95251

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Biomedical&Life Sciences Chemistry&Materials Science Computer Science&Communications Engineering Physics&Mathematics

Growth of a Pure and Single Phase Iron Sulfide (Pyrite) Thin Film by Electrochemical Deposition for Photovoltaic Applications

Emmanuel

A. Botchway

¹Francis

K. Ampong

¹Isaac

Nkrumah

¹^*Francis

K. Boakye

¹Robert

K. Nkum

Department of Physics, Kwame Nkrumah University of Science and Technology, Kumasi, Ghana

19092019

09097257359, August 201921, September 2019 24, September 2019

2014

This work is licensed under the Creative Commons Attribution International License (CC BY). http://creativecommons.org/licenses/by/4.0/

Single phase iron pyrite (FeS₂) films have been successfully deposited on ITO-coated glass substrates using a 3-electrode electrochemical system with graphite as the counter electrode and Ag/AgCl as the reference electrode. In this single-step electrodeposition, the FeS precursor thin film was directly electrodeposited on the conductive substrate from the electrolytic bath solution which contained FeSO₄.7H₂O as an iron source, and Na₂S₂O₃.5H₂O as a sulfur source. The deposition was carried out potentiostatically at a constant potential of -0.9 V vs . Ag/AgCl at room temperature. The growth of the iron pyrite phase was achieved by annealing the as-deposited at 500°C for an hour in an ambient of sulfur to form the pyrite phase . For sulfurization, two different techniques, one using the Kipp’s apparatus and a second, which involved heating elemental sulfur at 200°C, were used for the production of the sulfur gas. X-ray diffraction analyses of the sulfurized films showed that both sulfurization techniques appeared to form the pyrite phase , however, the second method yielded films with maximum crystalline order and stoichiometry with no discernable impurity peaks. Optical absorption measurements revealed the existence of a direct transition with an estimated band gap of 1.75 eV. SEM micrograph showed a compact morphology with a rough surface made up of crystallites of irregular shapes and sizes with well-defined edges, covering the entire substrate. EDAX analysis of the film was consistent with the formation of FeS₂ pyrite thin films.

Iron Pyrite Films Electrodeposition Sulfurization Solar Cell Materials

1. Introduction

Iron sulfide (FeS₂) pyrite phase, is a semiconductor material with remarkable properties suitable for solar cell applications. It is non-toxic and its constituents iron and sulfur are considered as elements which are highly abundant with low cost of extraction and processing [1] . This makes the large scale production of these materials quite feasible and cost-effective.

Pyrite is an absorber material that can be either an n or p type semiconductor depending on the type of dopant impurities [2] . Pyrite has electrical conductivity value which varies between 0.05 and 3.5 (Ω∙cm)⁻¹ and carrier concentration which varies between 6.9 × 10¹⁵ and 5.4 × 10¹⁷ cm⁻³ [3] . As a result of its moderate band gap of 0.95 eV and high optical absorption coefficient in the mid-infra-red range, Iron pyrite is considered as one of the most promising semiconductor materials to meet the pressing demand for low cost energy solutions. It has superior electrical properties with long minority carrier diffusion length of ~0.1 to 1.0 μm and carrier mobility of about 360 cm²∙V⁻¹∙s⁻¹ [4] . The advantage of having a high absorption coefficient is of particular importance since only about 40 nm of pyrite is required to absorb 90% of the incident light [5] .

Pyrite devices demonstrate elevated quantum efficiencies (often >90%) and photo-currents (>40 mA∙cm⁻²) but small photo-voltages (typically <200 mV, ~20% of the band gap) [6] . The low photo-voltage value is liable for the restricted solar cell efficiency. Although theoretical investigation envisaged that greater than 18% efficiency should be achievable, in reality, pyrite based solar cells fabricated so far show evidence of less than 3% conversion efficiency [7] . The low photo-voltage is ascribed to bulk and surface vacancies that produce electronic states within the band gap [6] . The low efficiency is additionally thought to be caused by phase impurities like marcasite which is formed alongside pyrite when grown from aqueous solutions [8] . This mixed phase of FeS₂ also deteriorates its photovoltaic performance.

Several techniques are available for the deposition of FeS₂ thin films. Among these techniques, electrochemical deposition offers several advantages such as; the ability to control film thickness, composition, morphology, etc. by mainly controlling electrical parameters such as electrode voltage and current density, which are easily adjustable. The technique is simple and economical because of its use of low cost apparatus, low operating temperature, and negligible waste materials.

Electrochemical deposition of iron sulfide is usually carried out by a two-stage process using direct compound electrodeposition followed by sulfurization to obtain the pyrite phase.

Sulfurization plays a significant role in achieving single phase pyrite films, it involves thermal treatment of the thin film in a sulfur rich atmosphere. The main purpose of this is to increase the sulfur concentration of the films and in this case fill the sulfur vacancies usually found in FeS systems. The choice of sulfurization technique is crucial in determining the level of purity of the iron pyrite thin film. Different sulfurization techniques would produce iron pyrite films with different levels of purity. A few authors have studied and reported on various aspects of electrochemical deposition of iron sulfide thin films. Arico et al. [9] Studied some structural properties of electrodeposited iron sulfide thin films on Platinum substrates. Dong et al. [10] studied the effect of sulfurization temperature on the structure of Ferrous sulfide (FeS) thin films deposited on indium-tin oxide (ITO) substrates by electrochemical deposition, whilst Wang et al. [11] studied the effect of sulfurization time on the structure of electrodeposited iron sulfide thin films. Finally, Kawai et al. [12] studied the optimal conditions for the electrodeposition of iron sulfide thin films. Each of these authors used their own unique electrochemical factors such as pH, electrolyte concentration, deposition potential, and temperature and deposition time. In this work, the use of graphite as the counter electrode, the deposition potential vs. Ag/AgCl, the pH of the electrolyte and concentrations FeSO₄∙7H₂O and Na₂S₂O₃∙5H₂O used in preparing the electrolyte are unique to this work. We also devised our own technique for post deposition treatment of the as-deposited samples before sulfurization.

2. Materials and Methods

A conventional three-electrode setup consisting of an Ag/AgCl reference electrode, a graphite plate as a counter electrode, and an ITO-coated glass substrateas a working electrode which was employed for electrodeposition.

The electrolyte solution contained FeSO₄∙7H₂O as an iron source, Na₂S₂O₃∙5H₂O was used as a sulfur source, H₂SO₄ was used to adjust the pH during the electrodeposition process.

In preparation of the electrolyte, equal volumes (~40 mL) of 0.24 M FeSO₄∙7H₂O and 0.45 M Na₂S₂O₃∙5H₂O were mixed together in a 100 ml beaker. The resulting solution had a pH = 3.73 at room temperature. This pH was adjusted from 3.73 to 1.96 by adding a few drops of 2M H₂SO₄, this was done to improve the adherence of the electrodeposits. The solution turned cloudy on adding the acid due to the formation of elemental sulfur. After about 20 to 30 minutes the electrolyte in the bath suddenly started to turn from cloudy to colorless as the sulfur precipitate had settled at the bottom of the beaker. Electrodeposition was carried out potentiostatically using an Echem ER466 potentiostat-galvanostat, at constant potential of −0.9 V vs. Ag/AgCl at room temperature (30˚C ± 2˚C). A growth time of ~30 minutes was ensured during electrodeposition. Beyond this time the films become too thick. A diagram of the experimental set-up is shown in Figure 1.

Most reports on the deposition of iron sulfide by a 3-electrode deposition, involve the use of saturated calomel electrode (SCE) as the reference electrode and platinum or gold as the counter electrode. However, in this work silver/silver chloride is used as the reference electrode and graphite plate as the counter electrode. The choice of the reference electrode affects the deposition potential. To the best of our knowledge not much work has been cited using this combination for a 3-electrode deposition of Iron sulfide thin films. In order to prevent the as-deposited films from oxidation, whilst being dried, the following technique

was devised. A desiccator with freshly prepared drying agent was initially purged with Argon gas. The as-deposited sample was introduced into the desiccator which was connected to a vacuum pump to extract the argon and create a tight seal around the edge of the desiccator. After drying, the as-deposited films were annealed in a sulfur atmosphere at 500˚C to form the pyrite phase. Two different techniques, described in the next section, were used to produce the sulfur gas for the sulfurization process. Emphasis is on comparing the quality of iron pyrite films produced by using the Kipp’s apparatus to generate hydrogen sulfide gas for the sulfurization process and when elemental sulfur is heated at 200˚C to form sulfur vapor for sulfurization.

2.1. Sulfurization

Procedure 1: Production of H₂S Using Kipps Apparatus (Figure 2)

In this procedure, sufficient amounts of iron sulfide lumps are placed in the central bulb of a Kipp’s apparatus. 2M dilute sulfuric acid is added to the upper bulb with the tap open until the lower bulb is completely filled and the Iron Sulfide lumps covered with acid. The tap is then closed. The acid will react with iron Sulfide to produce hydrogen sulfide gas which fills up the middle bulb. The reaction equation is shown below

FeS + H 2 SO 4 → FeSO 4 + H 2 S

The hydrogen sulfide gas can be delivered for sulfurizing by opening the tap, as shown in Figure 1.

Procedure 2: Using sulfur powder (Figure 3)

In the procedure illustrated in Figure 3, elemental sulfur powder is used to produce the sulfur vapor. 0.5 g of sulfur powder was poured into a ceramic boat and together with the FeS₂ sample, placed inside an enclosed borosilicate glass tube. Prior to this, the tube was flushed with Argon for 10 minutes to get rid of

any oxygen. The temperature of the sample heating zone was raised and held at 500˚C for 30 minutes. The Sulfur zone was heated and maintained at 200˚C. Having sulfur vapor in the tube throughout the process is very important to ensure the supplement and incorporation of sulfur into the film during the annealing process. An Argon flux was used to carry the sulfur vapor inside the tube. After the sulfurization process, the furnace was allowed to cool down naturally by turning down the heat whilst under the flow of argon.

2.2. Characterization

Structural analysis was first carried out to determine which sulfurization technique was suitable for achieving single phase pyrite films. The pyrite film with the highest purity score was then characterized further by optical absorbance measurements, scanning electron microscopy (SEM) and energy dispersive X-ray (EDX) analysis.

3. Results and Discussions3.1. XRD Analysis

The XRD data was obtained by a PANalytical Empyrean Series 2 powder X-ray diffractometer with Cu-kα radiation (1.5406 Å) in the range of 2θ = (10˚ - 90˚). The machine was operated at 40 mA and 45 kV for phase analysis using the Bragg-Brentano geometry. Total analysis time per samples was around 35 minutes for a 2θ scan step of 0.06˚. The X-ray data was analyzed using the HighScore Plus software.

The X-ray diffractogram shown in Figures 4(a)-(c) compares the composition of the as-deposited FeS precursor thin film and films sulfurized by the two different procedures described.

Figure 4(a) shows the diffraction pattern obtained after the direct compound electrodeposition of FeS₂. The pattern of prominent peaks in the diffractogram was matched to FeS (JCPDS Card No. 65- 9124) and Fe_1-xS (JCPDS Card No. 29-0726) compounds. There were no peaks corresponding to the FeS₂ pyrite phase.

Figure 4(b) had a significant number of peaks indexed to the FeS₂ pyrite phase (JCPDS No. 65-3321). A few peaks labelled as ‘x’ were matched to impurity phases such as FeS (JCPDS Card No.65- 9124) and Fe_1−xS (JCPDS Card No. 29-0726). The score for the pyrite phase is 70 as shown in the pattern list in Table 1.

The different assigned peaks shown in Figure 4(c) were made by comparing with JCPDS standards and they were a perfect match to FeS₂ pyrite phase (JCPDS No. 65-3321). These crystalline peaks occurring at 2θ = 28.4956˚, 33.0393˚, 37.07443˚, 40.7648˚, 47.4354˚, 56.2717˚, 59.0751˚, 61.6613˚, 64.2344˚ and 79.0545˚ correspond to reflections from the (111), (200), (210), (211), (220),

Table 1 Pattern List for procedure 1

Visible	Ref.Code	Score	Compound Name	Scale Fac.	Chem. Formula
*	01-071-4918	37	Iron Oxide	0.829	Fe₃O₄
*	01-083-0078	22	Iron Sulfate Hydrate	0.691	Fe(SO₄)(H₂O)
*	00-042-1340	70	Iron Sulfide	1.012	Fe S₂

(311), (222), (023), (321) and (420) planes, respectively. The absence of any impurity peaks is a clear indication of the high purity of the sample. The score for the pyrite phase is 94 as shown in the pattern list in Table 2.

It is clear from the diffractograms and the pattern list in Table 1 and Table 2 that the sulfurization technique described in procedure 2, that is, by using sulfur vapor is preferable for achieving single phase pyrite films.

Table 1 and Table 2 are the qualitative information on the relative amounts of different phases detected in the thin films and their corresponding structure, produced by the High Score Plus software.

The crystal structure of pyrite is cubic [13] . The lattice parameter “a” was estimated from the equation below

1 d 2 = h 2 + k 2 + l 2 a 2

where d and h, k and l are inter-planar spacing and Millar indices respectively.

The value obtained for the lattice parameters was 5.42256 Å. This result is close to the reported value for pyrite.

The average grain size determined by Scherrer’s formula was 31.9861 nm which is close to values reported by [14] [15] .

3.2. Scanning Electron Microscopy (SEM)

Scanning electron microscopy (SEM) images and energy dispersive X-ray (EDX) analyses were obtained using a Phenom instrument with nominal electron beam voltages of 15 kV respectively.

The SEM micrograph of FeS₂ (pyrite phase) thin film is shown in Figure 5. The micrograph shows a compact morphology with a rough surface made up of crystallites of irregular shapes and sizes with well-defined edges, covering the entire substrate.

3.3. Compositional Analysis by Energy Dispersive X-Ray Spectroscopy (EDX)

Figure 6 shows the EDAX spectrum and elemental composition of the films. The EDAX analysis of the film is consistent with the formation of FeS₂. From the table (inset), it can be observed that the films have good stoichiometry.

3.4. Determination of the Optical Band Gap

A Cecil CE7500 series double beam UV-Visible spectrometer operating in the

Table 2 Pattern List for procedure 2

Visible	Ref.Code	Score	Compound Name	Displ. [˚2Th]	Scale Fac.	Chem. Formula
*	01-071-2219	94	Iron Sulfide	0.000	0.800	Fe S₂

wavelength range of 190 nm to 1100 nm, was used for optical absorbance measurements. Alternatively, the energy band gap and type of electronic transition can be estimated with the Stern (1963) equation [16] .

A = [ k ( h υ − E g ) ] n / 2 h υ

where v is the frequency, h is the Planck’s constant, k equals a constant while the value of n is either 1 for direct transitions and 4 for indirect transitions, respectively. The band gap energy is obtained by plotting a line of best fit on the ( A h υ ) 2 / n versus h υ graph and extrapolating the line to intersect the energy axis at ( A h υ ) 2 / n = 0 .

Figure 7 shows the band gap of the FeS₂ thin film. The linear nature of the plot confirms the presence of a direct transition. The estimated band gap for the FeS₂thin film is 1.75 eV. This significant blue shift (0.85 eV) of the band gap from the bulk value of 0.95 eV, could be attributed to quantum size effect induced by the Nano crystallites in the film [17] [18] .

4. Conclusion

Single phase iron pyrite (FeS₂) films have been successfully deposited on ITO-coated glass substrates using a 3-stage electrochemical system followed by sulfurization. X-ray diffraction analyses confirmed that the sulfurization technique which involved heating elemental sulfur at 200˚C to generate sulfur gas, yielded films with maximum crystalline order and stoichiometry. There were no discernable peaks corresponding to impurity phases. EDAX analysis of the film was consistent with the formation of FeS₂. SEM micrograph of the FeS₂ pyrite films showed a compact morphology with a rough surface made up of crystallites of irregular shapes and sizes with well-defined edges, covering the entire substrate. Optical absorption measurements revealed the existence of a direct transition with an estimated band gap of 1.75 eV. All the results from the characterization techniques indicate that the synthesis process used in this work, produced single phase iron pyrite (FeS₂) thin films, which can be used as absorber materials in solar cells. Future work would include further characterization by techniques such as Photoluminescence, and I-V measurements, and also measuring the variation of the concentration of FeSO₄∙7H₂O with electrical conductivity.

Acknowledgements

The authors wish to acknowledge the Department of Physics, and the Department of Earth science, both in the University of Ghana, Legon, for the use of the X-ray diffraction equipment, scanning electron microscope and the energy dispersive x-ray machine.

Conflicts of Interest

The authors declare no conflicts of interest regarding the publication of this paper.

Cite this paper

Botchway, E.A., Ampong, F.K., Nkrumah, I., Boakye, F.K. and Nkum, R.K. (2019) Growth of a Pure and Single Phase Iron Sulfide (Pyrite) Thin Film by Electrochemical Deposition for Photovoltaic Applications. Open Journal of Applied Sciences, 9, 725-735. https://doi.org/10.4236/ojapps.2019.99059

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