Crystal Structure Formation of CH₃NH₃PbI3-xClx Perovskite.

Inorganic-organic hydride perovskites bring the hope for fabricating low-cost and large-scale solar cells. At the beginning of the research, two open questions were raised: the hysteresis effect and the role of chloride. The presence of chloride significantly improves the crystallization and charge transfer property of the perovskite. However, though the long held debate over of the existence of chloride in the perovskite seems to have now come to a conclusion, no prior work has been carried out focusing on the role of chloride on the electronic performance and the crystallization of the perovskite. Furthermore, current reports on the crystal structure of the perovskite are rather confusing. This article analyzes the role of chloride in CH₃NH₃PbI3-xClx on the crystal orientation and provides a new explanation about the (110)-oriented growth of CH₃NH₃PbI₃ and CH₃NH₃PbI3-xClx.

1. Introduction

Since the first organic-inorganic halide perovskite solar cell was reported [1], perovskites have attracted growing interest and the power conversion efficiency (PCE) has reached 20.1% [2]. It is not very common that a photovoltaic device can experience such a rapid development. While the structure of the cells evolved from sensitized meso-structure to planar structure [3], both inorganic and organic materials can be applied as electron and hole transfer materials [4]. Furthermore, by tuning the composition of the perovskite, the band gap can be easily modified [5]. Given the numerous advantages of perovskite, a clear understanding of the crystal structure is crucial and the role of chloride in the formation of CH3NH3PbI3-xClx (hereafter, we use MA short for CH3NH3) is one of the most pressing topics.

It has been reported that the presence of chloride in the perovskite improves the uniformity of its layer [6] and results in an increase of the carriers’ diffusion length from ca. 100 nm to over 1 μm [7]. However, the long held debate over of the existence of chloride in the perovskite seems to have now come to a conclusion. First, when synthesizing the perovskite by the one step method with precursor solution of MACl and PbI2 (1:1 molar ratio) in anhydrous N,N-dimethylformamide (DMF), the resulting crystal is not MAPbI2Cl but a mixture of MAPbI3 and MAPbCl3 [8]. This provides direct evidence that chloride (Cl−) cannot substitute iodine (I−) in the perovskite to form a stable crystal. Then, two contradictory results were then reported. X-ray photoelectron spectroscopy (XPS) showed that the molar ratio C:N:Pb:I:Cl of the perovskite is ca. 1:1:1:2:1, when prepared from a precursor of MAI:PbCl2 (molar ratio 3:1) [9]. On the other hand, energy dispersive X-ray (EDX) analysis showed that no Cl− was present in the perovskite prepared from PbI2 + MAI + MACl [10]. Noting that the XPS was unable to determine the existence of MAPbI2Cl crystal and that EDX has its detecting limitation, more precise characterizations were needed. Later on, the simultaneous Fourier transform infrared spectroscopy analysis of the expelled gas during the decomposition of MAPbI3-xClx showed the presence of Cl−, angle-resolved XPS [11] and X-ray fluorescence spectroscopy (XFS) [12] not only confirmed the existence of Cl−, but also showed that Cl− was located at the interface between the perovskite and the electron transport TiO2 layer, and not in the perovskite structure [11,12]. Moreover, scanning transmission microscopy-energy dispersive spectroscopy (STEM-EDS) detected no trace of Cl− in the perovskite. Even though there is a strong Cl− signal, no N was observed indicting the presence of only PbCl2 [13]. Thus, Cl− only appears at the interface between MAPbI3 and the anode. Two more reports have further confirmed this conclusion. XPS analysis showed only weak Cl− signal after etching the surface of MAPbI3-xClx by a 50 nm thickness [14]. Hard X-ray photoelectron spectroscopy and fluorescence yield X-ray absorption spectroscopy showed no Cl− at the surface of MAPbI3-xClx with higher average concentration of Cl throughout the perovskite layer at the deep beneath [15]. Here, we refer to MAPbI3-xClx as MAPbI3 that is prepared using chloride-containing precursors. However, as the condition for depositing MAPbI3-xClx differs, Cl− may still remain in the resulting perovskite layer. For instance, X-ray absorption near edge structure (XANES) results showed that x = 0.05 ± 0.03 Cl atoms per formula unit remain in the films after annealing at 95 °C for 120 min [16]. The results from photothermal induced resonance (PTIR) showed that the MAPbI3-xClx film consists of a mixture of Cl-rich (xlocal < 0.3) and Cl-poor phases after a mild annealing (60 °C, 60 min) and homogeneous Cl-poorer (xlocal < 0.06) phase upon further annealing (110 °C) [17].

In addition, first-principles calculation results provide some good explanation. For the crystal structure, Cl− concentration was found below 3%–4% [8] and if the Cl− ions enter the crystal structure, they preferentially occupy the apical positions in the PbI4X2 octahedra [18]. For the electronic property, while the molecular orientations of CH3NH3+ result in three times larger photocurrent response than the ferroelectric photovoltaic BiFeO3, Cl− substitution at the equatorial site induces a larger response than does substitution at the apical site [19]. Results also showed that, using Cl− precursor can avoid forming the PbI defects [20]. Introducing Cl− would reduce the lattice constant which can inhibit the formation of interstitial defects [21]. As excitons may be screened by collective orientational motion of the organic cations, Cl− might hinder this motion and results in better transport properties [22]. Little difference of electronic properties was represent among orthorhombic, tetragonal and cubic phases of MAPbI3 [23], however, the valance-band-maximum and conduction-band-minimum states can be mainly derived from iodine ions at some unique positions, Cl− substitution can strengthen the unique position of the ions and result in more localized charge density [24]. Thus, lower carrier recombination rate and enhanced carrier transport ensued. For the interface, the (001) and (110) surfaces tend to favor hole injection to 2,2′,7,7′-tetrakis(N,N-di-p-methoxyphenylamine)-9,9′-spirobifluorene (Spiro-MeOTAD), while the (100) surface facilitates electron transfer to [6,6]-phenyl C61-butyric acid methyl ester (PCBM) [25]. A better structural matching between adjacent rows of perovskite surface halides and TiO2 under coordinated titanium may be the reason for the (110)-oriented growth of MAPbI3-xClx and MAPbI3 [26]. Interfacial Cl− may thus further stabilize the (110) surface and modify the interface electronic structure between MAPbI3 and TiO2 [26].

Despite the absence of Cl− in the perovskite, it still played an important role in the crystallization process. For instance, the morphology of MAPbI3-xClx was compared with MAPbI3 [27] and a model in which the Cl− rich phase modifies the morphologies of perovskite was proposed and fit well with the results from scanning electron microscopy (SEM) [27]. In addition, the transmission electron microscopy (TEM) of freeze-dried perovskite MAPbI3−xClx precursor solution showed the presence of PbCl2 nanoparticles [28] and this is in agreement with the dynamic light scattering (DLS) investigations of MAPbI3−xClx precursor solution [29]. Thus, references [28,29] further proved the model of the heterogeneous nucleation by PbCl2 nanoparticles proposed in reference [27]. However, the formation mechanism of the crystal structure remains undermined and this will be discussed in the following parts of this article.

2. Methods for Fabricating MAPbI3-xClx

In Section 3, we discuss the crystal structure of MAPbI3-xClx according to the deposition method. As the fabrication methods were discussed in detail in reference [30], here we add a brief introduction about the preparation methods of MAPbI3-xClx. For the one-step deposition method, MAI:PbI2/PbCl2 (molar ratio 1:1 or 3:1) [31,32] were dissolved in γ-butyrolactone (GBL) or DMF, spin-coated on the substrates and annealed to form perovskite. Different annealing conditions result in different morphology of the MAPbI3-xClx layer. While a rapid thermal annealing at 130 °C resulted in micron-sized perovskite grains [33], two-step annealing, such as 90 °C for 30 min then at 100 °C for 2 min [34] or 60 °C then ramping to 90 °C [35], resulted in optimal PCE on poly(3,4-ethylenedioxythiophene) poly(styrene-sulfonate) (PEDOT:PSS) substrates. A full coverage of perovskite can be achieved by rapid cooling after annealing [36]. To increase the solubility of Cl−, 1,8-diiodooctane [37] or other alkyl halide additives [38] or dimethyl sulfoxide [9] can be employed. Adding poly-(vinylpyrrolidone) (PVP) can also improve the surface coverage of perovskite [39]. It is interesting to note that, for MAPbI3−xClx, a simple annealing step is enough to form a good coverage [6,40], but for MAPbI3, a special step, such as multi-deposition [41], adding N-cyclohexyl-2-pyrrolidone (CHP) [42], fast deposition [43,44,45], or air flow during spin coating [46,47], is needed.

The sequential deposition method was mainly applied for MAPbI3 perovskite. In a typical synthesis, the solution of PbI2 in DMF was spun on a substrate as the first step then the substrate was dipped in a solution of MAI in 2-propanol (IPA) to form MAPbI3 crystals as the second step [48]. For the inclusion of chloride, in the first step the PbCl2 can be mixed with PbI2 in DMF or dimethyl sulfoxide (DMSO) [49,50,51,52], and/or the second step MACl can be added [53,54,55]. For vapor based deposition methods, the MAPbI3-xClx can be formed by co-evaporating MAI and PbCl2 onto the substrates [56,57] or by reacting PbCl2 on substrates with MAI vapor [58,59].

3. The Crystal Structure Form and Formation

3.1. Crystal Structure of MAPbI3 Layer

The parameters and transitions of phases of bulk MAPbI3 were included in references [60,61]. Here, we focus on the tetragonal and cubic phases [62]. In fact, there are no critical differences between the two phases, except a slight rotation of PbI6 octahedra along the c-axis. The atomic structures of MAPbI3 of the two phases are shown in Figure 1A,B. Thus, the tetragonal phase can be treated as a pseudocubic phase with a* = a/, c* = c/2 [63]. Below 54 °C, the cubic phase of MAPbI3 can be transformed into the tetragonal phase [60], and the opposite transition occurs by annealing at 100 °C for 15 min [41]. In Figure 1C, the X-ray diffraction (XRD) patterns of the two phases are shown. After transformation to the tetragonal phase, the (100) and (200) peaks of cubic MAPbI3 split, also new (211) and (213) peaks show up. Here, we use the peak splitting as indictor for phase transformation. Analysis of the MAPbI3-xClx usually shows the cubic phase of MAPbI3, however, with a much more preference along (100) and (200). This will be discussed in the Section 3.2 and Section 3.3.

Figure 1

(A) Atomic models of MAPbI3 with cubic phase; and (B) tetragonal phase; (C) the calculated XRD patterns for MAPbI3 in both phases. (A) and (B) are reprinted from reference [64], Copyright © IOP Publishing. Reproduced with permission. All rights reserved; (C) is reprinted from reference [65], Copyright © 2013, Royal Society of Chemistry.

Another phase which should be noted is the amorphous phase. Pair distribution function analysis of X-ray scattering showed that after annealing at 100 °C for 30 min, the MAPbI3 in meso-porous TiO2 has about 30 atom% in medium range crystalline order and the other 70 atom% in a disordered state with a coherence length of 1.4 nm [66]. The poor crystallization of the MAPbI3 in meso-porous TiO2 was studied by high-resolution TEM [67]. Quartz crystal microbalance measurements suggest that during the sequential method only half of PbI2 is converted to MAPbI3 instantly, while the other half is involved in reversible transformation with MAPbI3. Additionally, the amorphous character with a very small average crystallite size may be present after the transformation as previously discussed [68]. The amorphous phase may also present during the initially deposited MAPbI3-xClx, as indicated by the envelope in some XRD spectra. In reference [69], the amorphous phase MA5PbCl4I3 was also mentioned. Moreover, both XRD and photoluminescence studies of MAPbI2Cl (2MAPbI3+MAPbCl3) indicate the existence of the amorphous phase [70].

3.2. Converting Lead Halides to Perovskite

In the sequential deposition method, PbI2 or/and PbCl2 were first dissolved in a solvent. As PbI2 crystal has a layered structure, DMF can intercalate into the PbI2 interlayer space and screen PbI2 via Pb-O bonding [71,72,73]. When DMF is intercalated, the XRD peak of the PbI2 (001) plane red shifts from 14.8° to 7.94° [72,73]. The red-shift of this XRD peak to 9.17° also indicates the intercalation of DMSO [43]. While PbCl2 doesn’t possess a similar layered structure as PbI2, its solubility is poor where PbCl2 nanoparticles may only suspend in the solvent [28]. However, depositing a mixture of PbI2 and PbCl2 on the substrates result in a new PbICl phase [74], whose crystal structure is similar to PbCl2 [75].

At the beginning of the reaction of PbI2 and MAI, a predominant peak at (220) appeared (as shown in Figure 2B). In other words, the MAPbI3 preferentially grows along (220) plane at first. The annealing process increases the long range crystalline order and results in the predominant (110) peak instead. Noting the (220) is only a short range of (110), thus, another possible reason for the (110)-oriented growth of MAPbI3-xClx and MAPbI3 may be because layered crystal structure of PbI2 (growth along (001) planes of PbI2 like the liquid catalyst cluster model mentioned in reference [76]). The lattice planes of tetragonal MAPbI3 are showed in Figure 3.

Figure 2

XRD patterns of glass substrates with vapor deposition of (A) a layer of PbI2; and (B) a layer of PbI2 followed by a layer of MAI, repeating this step 7 times; XRD pattern of the (C) annealed 7-time deposited PbI2/MAI layer; (D) 1-time deposited PbI2 (50 nm thickness)/MAI (50 nm thickness) layer; and (E) 1-time deposited PbI2 (150 nm thickness)/MAI (150 nm thickness) layer. Reprinted from reference [77], Copyright © 2015, Royal Society of Chemistry.

Figure 3

Crystallographic (lattice) planes (in gray) of tetragonal MAPbI3. Reprinted from reference [78], Copyright © 2015, American Chemical Society.

For PbCl2, Cl− was detached from PbCl2 when the PbCl2 was evaporated on the MAI substrate [79] and all the atoms of lead halide were dissociated during the crystal formation of the perovskite [80]. Thus, except the speed and the way of breaking the lead halide, the following steps should be similar with the one step method (Section 3.3) for converting PbI2 or PbCl2 with MAI to the perovskite. However, the situation in the presence of MACl may be different. As less energy is needed for MACl than MAI to undergo phase transition from solid to gas [69], it may be easier for MACl than MAI to diffuse into the PbI2 and cause the crystallization of perovskite [81]. However, as Cl− cannot be incorporated into MAPbI3 crystal structure, the MAI and MACl may compete with each other to determine the result crystal, because only MAPbI3 or MAPbCl3 was formed when PbI2 was soaked in 80 mM MAI + 40 mM MACl or in 40 mM MAI + 80 mM MACl, respectively [80]. Thus, the incorporation of some amount of MACl managed to modify the morphology of the perovskite and resulted in better performance of the solar cells.

3.3. One Step Deposition of MAPbI3-xClx

The better crystallization of MAPbI3-xClx along (110) and (220) plane of the tetragonal phase or (100) and (200) planes of the cubic phase may be due to the lowered cubic-tetragonal phase transition temperature of MAPbI3−xClx after the incorporation of Cl− [82]. A clear cubic-tetragonal phase transition temperature of MAPbI3 was detected by differential scanning calorimeter (DSC) analysis [65], however no such phase transition was observed for MAPbI3−xClx [83]. To explain the absence of the phase transition for MAPbI3−xClx, we first study the crystallization process of MAPbI3-xClx by one step deposition method.

Detail information about crystal formation process of MAPbI3 is summarized in reference [85]. For MAPbI3-xClx, the transformation from the intermediate phase to the perovskite is determined as 80 °C by in situ grazing incidence wide-angle X-ray scattering (GIWAXS) [86]. Figure 4 presents a clearer picture of the crystal formation of MAPbI3-xClx. The 15.7° and 31.5° peaks are associated with the (100) and (200) diffraction peaks of MAPbCl3 [82]. These peaks were also observed in references [27,87,88]. In Figure 4, it is interesting to note that MAPbI3 was formed first for the as-spin coated film but converted to MAPbCl3 after annealing at 100 °C for 10 min, and then MAPbCl3 was converted back to MAPbI3 after 45 min of annealing [84]. Further annealing would result in the decomposition of MAPbI3 to PbI2, but this occurred after conversion to the intermediate phase to MAPbI3 [89]. Because MAPbCl3 is in a cubic phase, we suppose that MAPbCl3 may cause a template effect for the cubic MAPbI3 phase.

Figure 4

XRD patterns and optical images (insets) of MAPbI3-xClx film during annealing. Reprinted from reference [84], Copyright © 2015, American Chemical Society.

In addition, the MAI:PbI2 (molar ratio 3:1) precursor solution on compact TiO2 can also form MAPbI3 with a predominant (110) plane, but the annealing temperature need to be above 150 °C [84,88,90]. The different sublimation temperature of MAI and MACl and the evidence of residue MAI or MACl in the resulting perovskite may explain the higher annealing temperature needed for MAPbI3 [84,91].

The XRD patterns of the resulting MAPbI3-xClx prepared from different chloride-containing precursors are summarized in Figure 5. All the patterns showed predominant crystallization along the (110) and (220) planes. Interestingly, the (220) peak split at a high MACl (x = 2) concentration in Figure 5B [27]. This split was also observed in reference [29]. In the sequential deposition method, the (110) and (220) crystallization preference may be due to an in situ transformation process [92] of PbI2 to MAPbI3, as discussed in Section 3.2. However, the PbI6 octahedra are more likely to be fully dissociated in the one step precursor solution. [29,93,94,95] As MACl does not fit in the MAPbI3 structure, it could be possible that MACl may be expelled along the (110) planes of the MAPbI3 and that is why the MAPbI3-xClx always showed the (110) and (220) orientation preference. This assumption can be proved by (220) peak split in Figure 5B, as excess of MACl breaks down the crystal range along (110) planes resulting in peak split. However, MAI can fit in the MAPbI3 structure, (110)-oriented growth is just the result of cubic phase in high temperature (150 °C in refereneces [84,88,90]). Surprisingly, a main XRD peak of (310) was observed for the one step deposition prepared MAPbI3 [96]. The main peak of (310), which is distinct from the (110) peak, may have resulted from the fact that the MAI was added into the precursor solution after the PbI2 was completely dissolved instead of both MAI and PbI2 being present at the same time [96], or the fact that the (310) plane of MAPbI3 may match the crystal structure of the substrate better. Then the magnitude of the (110) peak of MAPbI3-xClx and the (310) peak of MAPbI3 further increases after 5 weeks [96]. Thus, we believe that the annealing process may only reinforce the crystallization preference as it is initially formed and the effects of substrate also contribute to the crystal structure formation of the perovskite in some cases. Returning to Figure 5, if excess of MACl breaks down the growth along the (110) plane, we believe MACl can also break down the crystalline order range. Since a large amount of MAPbI3 existed in the amorphous phase form, the cubic phase of MAPbI3 may be more favorable in short crystalline order range than the tetragonal phase.

Figure 5

XRD patterns of MAPbI3-xClx prepared from (A) precursor solution xPbCl2+yPbI2+zMAI (x = 0.25, 0.5, 0.75 and 1; y = 1 − x; z = 3 × x + y) in DMF; and (B) precursor solution 1PbI2+1MAI+xMACl (x = 0.5, 1, 1.5 and 2). Reprinted from reference [27], Copyright © 2014, American Chemical Society.

There are other influences associated with Cl−. Increasing the temperature during the soaking of the PbI2 substrate in MAI + MACl IPA solution can improve the (110) orientation of MAPbI3-xClx where the high temperature facilitates the expelling of MACl [97]. Annealing the MACl:PbI2 (3:1) precursor on compact TiO2 at 60 °C for 10 min followed by 100 °C for 20 min instead of gradually heating from 25 to 100 °C for 45 min resulted in the (200) crystal plane of MAPbI3-xClx being vertically aligned on the substrate [98]. The tetragonal phase MAPbI3−xClx was occasionally found on compact TiO2 substrate [53], while the cubic phase always occurred in meso-porous substrate, where the trapped MACl in meso-porous structure [8] helps the formation of cubic phase. While the size of MAPbI3 crystal grains are smaller but the degree of crystallinity improves in the presence of MACl [27,54], the sequential deposited MAPbI3-xClx results in (001) elongated crystals [13].

4. Conclusions

In this article, the location of Cl− and its influence on the crystal morphology of MAPbI3-xClx is summarized, where the deposition methods (one step deposition, sequential deposition and vapor based deposition) for MAPbI3-xClx are reviewed. Furthermore, the cubic and tetragonal phases of MAPbI3 are elucidated and the crystallization process of MAPbI3-xClx is also summarized. Detailed information about the crystal structure with variable deposition parameters is also discussed. Though a recent report showed that Cl− mainly improves the carrier transport at the perovskite/Spiro-MeOTAD and perovskite/TiO2 interfaces, rather than within the perovskite crystals, the authors of reference [99] more recently spatially resolved photoluminescence decay results showed less recombination in the high chlorine concentration region [100]. Thus, the effect of high concentration of Cl− on the morphologies and electronic properties of the perovskite can still not be ignored. Additionally, whether Cl− is predominantly present as a substituent for I−, as an interstitial, or at the surface of the crystal, remains unclear [101] and this is worth further investigation.