Halide Perovskite Materials for Solar Cells

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This entry is adapted from the peer-reviewed paper 10.3390/nano13121886

The nomenclature “perovskite” was assigned to this structure in honor of Lev Perovski, the Russian mineralogist who initially unveiled it; since then, the name “perovskites” has been used to describe all materials that share calcium titanate’s crystal structure. The general formula for the perovskite light absorption layer is ABX₃, where A is an organic cation (CH₃NH₃⁺), B is a metal cation (Pb²⁺), and X is a halide anion (I⁻).

cell crystal solar fabrication perovskite tandem materials Physics photo-voltaic wide band

1. Halide Perovskite Materials for Solar Cells

Inorganic–organic halide solar cell researchers have become very interested in PSCs due to a striking rise in device efficiency from 3.8% ^[1] to 25.7% ^[2] since 2009. Considering an all-time high efficiency of around 26.7%, silicon PV systems hold most of the market share; perovskite has attracted much interest ^[3]. Given that certain materials have the potential to be employed in both photovoltaic PSCs and organic solar cells, this slight efficiency difference has recently caught the attention of researchers, particularly those with expertise in dye-sensitized solar cells (DSSCs) or organic solar cells. The DSSC device architecture is where PSCs display advantages over silicon-based devices, as seen in ^[4], which require labor-intensive and expensive high-vacuum deposition procedures. Based on the accounts of efficacious cell production on flexible substrates, further promise exists that the extensive roll-to-roll fabrication of PSCs could be implemented in various industrial sectors ^[5]^[6]. In 1839, German mineralogist Gustav Rose discovered a calcium titanate crystal structure. The nomenclature “perovskite” was assigned to this structure in honor of Lev Perovski, the Russian mineralogist who initially unveiled it; since then, the name “perovskites” has been used to describe all materials that share calcium titanate’s crystal structure. The general formula for the perovskite light absorption layer is ABX₃, where A is an organic cation (CH₃NH₃⁺), B is a metal cation (Pb²⁺), and X is a halide anion (I⁻).

2. Crystal Structure

In Figure 1a–c, researchers can observe that the molecular structure of the organic halide perovskite is of the ABX₃ type, where A and B are cations (with A being bigger than B), and X is the anion. The A cation (methylammonium, CH₃NH₃⁺, MA⁺, or formamidinium, CH₃ (NH₂)₂⁺, FA⁺) in a perovskite’s unit cell is surrounded by 12 X anions (Cl⁻, Br⁻, or I⁻, or a coexistence of multiple halogens) to form a cuboctahedron. The octahedral position of X is occupied by the B cation (Pb₂⁺, Sn₂⁺, etc.) The octahedra of the B cation and X anion are connected to create a stable three-dimensional network structure^[7]^[8]^[9]. For CH₃NH₃PbX₃, as the size of the halide grows from X = Cl to Br, the unit cell parameter grows from 5.68 to 5.92 and then to 6.27 Å. Mixing halides makes it easy to adjust the cubic phase’s lattice characteristics; for example, CH₃NH₃PbBr_2.3l_0.7, CH₃NH₃PbBr_2.07I_0.93, and CH₃NH₃PbBr_0.45I_2.55 all displayed a = 5.98 Å, 6.03 Å, and 6.25 Å, respectively. The cubic perovskite structure of CH₃NH₃SnBr_xl_3−x (x = 0–3) crystallized unit cell parameters are reported as follows: a = 5.89 Å (x = 3), a = 6.01 Å (x = 2), and a = 6.24 Å (x = 0). Some Sn-based perovskite compounds showed conducting capabilities in contrast to Pb-based perovskite materials ^[10]^[11].

Figure 1. (a) The standard crystal structure of perovskite. (b) B cation and X anion crystal structure. (c) The A cation occupies the octahedron location of the X anion in the crystal structure ^[9]. Copyright 2019, MDPI.

A dimensionless value termed the Goldschmidt tolerance factor (t), which measures the crystal’s stability and its structure’s deformability, is used to predict the formability of different kinds of perovskites.

t = \frac{r_{A} + r_{x}}{\sqrt{2} (r_{B} + r_{x})}

where the radius of cation A is r_A, the radius of cation B is r_B, and the radius of anion X is r_X. For perovskite composed of a transition metal cation and an oxide anion, t = 1 is projected to result in a cubic structure, while t < 1 is predicted to result in octahedral deformation. Additionally, at t < 1, symmetry is lost, which impacts the electrical characteristics. Perovskite formability for alkali metal halides is anticipated to be 0.813 < t < 1.107 ^[12]^[13]. Cubic structures have tolerance factors between 0.89 and 1, with values greater than 0.89; due to the instability of B–X bonding in 3D, a transition to a 2D layer structure may occur. In contrast, a tetragonal (β phase) or orthorhombic (γ phase) structure may form if the tolerance factor is less than 0.89 ^[14]. The octahedral factor (µ), provided by Equation (2), is another component for perovskite formation.

µ = \frac{r_{B}}{r_{x}}

Perovskite stability and distortion can be assessed through its utilization. The perovskite can have an octahedral factor between 0.45 and 0.89 without losing stability. Methylammonium lead trihalide (MAPbI₃, where X is the halide, could be Cl, Br, or I) is PSC's most widely utilized absorber substance. As the size of the halide atom grows from Cl to Br to I, the unit cell characteristics rise from 5.68 to 5.92 to 6.27 Å. However, the increased size and aspherical shape of methylammonium (MA) cause the network to distort, which causes a phase change and a drop in temperature. The orthorhombic structure is present for T < 160 K, the tetragonal structure for T > 162.2 K to T < 327.4 K, and the cubic structure for T > 327.4 K. The bandgap of methylammonium lead halide typically ranges from 1.5 to 2.3 eV; MAPbI₃ has a direct bandgap of roughly 1.55 eV, whereas MAPbBr₃ has a relative WB of 2.3 eV for 600 nm absorption started. FAPbI₃ (where FA is formamidinium) exhibits a NB of 1.48 eV as the absorber layer, indicating greater current extraction. However, this material has demonstrated lesser stability. The type of halogen atom employed also affects the structural characteristics of methylammonium lead halide. Lead halide perovskites have an octahedral crystal structure. The B cation (typically Pb but sometimes Sn) is octahedrally coupled to six halide ions. There is a shared corner between these octahedra, and the A cation lies between them ^[15]^[16]. The A cation of lead halide perovskites is either an organic molecule (methylammonium, MA, CH₃NH₃⁺) or an inorganic cation (usually Cs⁺), leading to the further categorization of lead halide perovskites as either organic–inorganic (hybrid) or all-inorganic. One can manipulate perovskites’ optical and electrical characteristics by changing the proportions of formed halide ions and, to a lesser extent, the cations ^[17]. Like traditional metal chalcogenide semiconductors, perovskites’ optical characteristics and object tuning can be achieved by adjusting their dimensions and size. Perovskites exhibit a pronounced inclination towards the creation of stratified two-dimensional (2D) and quasi-two-dimensional architectures, even though their dimensional range can be altered from three-dimensional to zero-dimensional by manipulating the synthetic parameters employed ^[18]^[18]^[19]^[19]^[20]. Numerous recent investigations have demonstrated the excellent photoluminescence quantum yields of colloidal perovskite nanocrystals. Furthermore, when their dimensional changes are reduced from 3D to 2D, they exhibit significant quantum confinement effects, allowing for the further customization of optical characteristics ^[21]^[22]. A good number of applications, such as solar cells and lasers, LEDs, and PV, have demonstrated the immense potential of perovskite.

3. Electronic Structure

Here, by considering the perovskite material’s electronic characteristics to understand its layered perovskite structure. Density functional theory (DFT) computer simulations were used in several theoretical investigations on the density of states (DOS) of perovskites, correlating the composition of the bands with the DOS. Researchers may learn more about where those remarkable optoelectronic capabilities of perovskite materials come from and how they can be optimized with the help of the DFT calculations performed on metal halide perovskites. The valence band results from the overlap between the M-site cation’s ns orbitals and the X-site anions’ np orbitals. In contrast, the conduction band is formed by combining the np orbitals of the M cation and the X anions ^[23]^[24]. It is well established that there is an antibonding feature between the valence band maximum (VBM) and the conduction band minimum (CBM) because of the orbital overlap among the filled ns of M and np of X ^[25]^[26]. The ionic nature of bonds expands, and E_g increases when the composition shifts from I to Cl because the energy difference between ns and np halogen atomic orbitals widens.

M metals have a less noticeable impact on the band structure. The final band structure is influenced by phenomena such as ns² lone pairs, the relativistic stabilization of the 6s² level in Pb²⁺, and the composition of M–X bonds (degree of covalence). Considering all these characteristics, the E_g of these materials can be precisely tuned by altering their compositions or making alloys. In addition, the absence of electron–phonon coupling in perovskites’ straight bandgap makes electronic transitions more likely. Since the electron’s quantized wave motion in a periodic crystalline lattice is connected to its crystal momentum (vector k), the VBM and CBM in direct bandgap materials are coplanar about this axis. Yin et al. computed the band structure and DOS of the cubic phase MAPbI₃ using DFT–PBE computation. The band structures of the tetragonal and orthorhombic phases of MAPbI₃ are very close to those of the cubic phase, according to a subsequent investigation by the same group. According to the experimental findings, the bandgaps are expected to be 1.55 and 1.57 eV in the tetragonal and cubic phases, respectively, and the UV-vis measurement of FASnI₃ is illustrated in Figure 2 ^[27]^[28]. Since the VBM and CBM coincide at the same point of the Brillouin zone, cubic MAPbI₃ is a direct bandgap semiconductor. The two MAPbI₃ phases, tetragonal and orthorhombic, are direct bandgap semiconductors exhibiting values that are nearly close to one another. The comparison between the experimental UV-vis spectrum of MAPbI₃ (red line) and the SOC–GW calculated spectrum (blue line) is depicted ^[27]^[29]. The Pb p orbital dominates the CBM, while I p states, through a minor addition from Pb s states, dominate the VBM. Given its position well below the VBM, the MA cation’s partial DOS does not make any direct electronic contributions to the CBM or VBM. MAPbI₃’s remarkable electrical properties can be traced back to a lone pair of s orbital electrons in the Pb cation. While the outer s orbitals of most metal cations are empty, Pb possesses an occupied 6s orbital just under the valence band ^[23]^[30].

4. Structure of Perovskite Solar Cells

Efficient PSCs could be the most fantastic solution for commercial solar technology manufacturing. PSC products are likewise separated into two categories for a good reason: normal and inverted ^[31]. The hole transport layer (HTL) or the electron transport layer (ETL) should be placed first; there are two distinct methods for fabricating PSCs. Semiconducting p-type polymers create an inverted structure, such as PEDOT: PSS, while the standard structure uses n-type semiconductors, such as TiO₂. The first ETL employing titanium oxide (TiO₂) was built in 2009, and it was the predecessor of the current structure. A PIN-type product based on the organic HTL poly(3,4-ethylene dioxythiophene)-co-polystyrene sulfate (PEDOT: PSS) was released four years later. These two architectures currently have the highest PCEs reported ^[4]^[32]^[33]^[34]^[35]. By employing growth methods, the fabrication temperature for n–i–p structured flexible PSCs could be kept to a minimum. However, an n–i–p structure device requires an excessive temperature method to develop a compact TiO₂ coating. Plastic is not a suitable surface for this ^[31]. The mesoporous TIO₂ film was initially employed as a scaffold for the initial PSCs fabricated from dye-sensitive solar cells (DSCs); as a result of sintering nanoparticles (NP), a porous TiO₂ layer developed, with the self-assembled perovskite absorber providing the filler.

It is easier to transfer electrons between the FTO electrode and the perovskite absorber, and a perovskite coating was formed on mesoporous TiO₂ ^[36]. Perovskite NPs work to progressively strip the photoexcited pigment of its electrons, enabling it to serve mainly as a light absorber in place of the molecular sensitizer it formerly was. However, the finding that organic–inorganic halide perovskite could independently conduct electrons and holes encouraged the creation of future devices. The mesoscopic variant’s perovskite capping layer extends well beyond the nanostructure thanks to the semiconductor oxide scaffold’s thoroughly infiltrated pores. The planar structure was researched to facilitate fabrication. Planar metal oxide ETL fabrication typically occurs below 200 °C without impairing the perovskite devices’ functionality. The standard structure is thus receiving much attention for further research ^[37]^[38]. Such a lower temperatures solution technique might result in the fabrication of the ETL, so the p–i–n-type arrangement has gained even greater notoriety.

Along with the electron-transporting material (ETM) layer, a hole-transporting material (HTM) layer was also applied; perovskites were suited for hole transport. This has been a major component in manufacturing p–i–n-structured solar cells. HTLs are well-suited for adaptable perovskite optoelectrical devices since their production often does not need a high-temperature annealing procedure ^[39]^[40]. HTM is also an air- and water-resistant alternative for PSCs. To prevent leakage, the objective of producing planar p–i–n on a uniform transparent conductive oxides (TCO) electrode is to manufacture a perovskite layer without pinholes by utilizing a one-step spin-coating procedure. Results from cells produced from a 1:1 molar PbI₂/CH₃NH₃I solution are inferior to those from the 1:3 molar PbCl₂/CH₃NH₃I solutions. The annealed perovskite film still exhibited pores and poor crystallinity since no scaffold had been used at 100 °C ^[41]^[42]. These findings prove that the perovskite layer’s appearance and crystallinity are critical to the device’s performance.

Utilizing the advantages of perovskite materials—known for their direct bandgap, high absorption coefficient, and superior charge transport properties—researchers have been designing and optimizing tandem solar cells. These perovskite tandem solar cells typically consist of a perovskite top cell paired with a bottom cell, often composed of silicon or another perovskite variant. This configuration broadens the solar spectrum coverage, thereby amplifying overall efficiency. Moreover, advancements have been made in improving the stability of these cells, with notable progress in encapsulation techniques and tweaks to perovskite composition that significantly reduce degradation over time. Despite these strides, challenges persist in areas such as large-scale manufacturing, consistency in the fabrication of thin films, and long-term stability, among others. However, the potential of perovskite tandem solar cells continues to drive substantial research and commercial interest. The Cell designs, structure, and applications of perovskite materials in tandem devices are depicted in Figure 3.

Figure 3. A sketch map of the solar cells fabrication for industrial application

Recent research has shown that greater PCEs can be obtained using organic–inorganic hybrid halide perovskite materials (CH₃NH₃PbI₃) instead of Si single-junction cells with advanced PV technology. For this reason, hybrid metallic halide perovskite materials, which are both organic and inorganic, share the benefits of both types of compounds. Because their performances increase higher than silicon-based PV technology, the newly developed perovskite solar cell (PSC) has been recognized as something that might drastically change the PV market. PSCs have captured significant interest in the solar world due to their bandgap's higher efficiency, minimal cost, process compatibility, and adjustability. With their widely-accepted bandgap of 1.1 eV, high open-circuit voltage (V_OC) of up to 750 mV, cheap manufacturing due to their supremacy in the industry, and exceptionally high efficiency, crystalline silicon solar cells are almost perfect for use in these tandem cells ^[43]^[44]. Nevertheless, the widespread use of III–V solar cells’ expensive manufacturing processes prevents them from being used for practical uses. The advancement of perovskite-based PV technology provided a viable solution to the need for inexpensive high-efficiency solar panels ^[45].

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