Bismuth subhalides

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Bismuth-containing solid-state compounds pose an interest to both the physical inorganic chemists as well as condensed matter physicists due to the element's massive spin-orbit coupling, stabilization of lower oxidation states, and the inert pair effect. [1] Additionally, the stabilization of the Bi in the +1 oxidation state gives rise to a plethora of subhalide compounds with interesting electronics and 3D structures. [2] [3] [4]

Contents

Overview of subhalide bismuth solid-state chemistry

Topological insulators and the relationship to bismuth solid-state chemistry

Bismuth subhalides, such as Bi4Br4 and β-Bi4I4, have been recently reported as topological insulators. [2] [3] Topological insulators have caught attention of physical inorganic chemists as well as condensed matter physicists due to the unique physicochemical properties emerging upon transition from bulk to surface states. [5] Exhibiting an energy band gap of classic insulator, the edge/surface states of the material acquire dissipationless electric transport. The subject has been investigated by condensed matter physicists as well as mathematicians to provide a link between the experimental emerging properties and the modeled topology. Broadly, the material's physics pertains to the Quantum Hall effect relying upon two pillars: time-reversal symmetry and spin orbit coupling, the latter dependent on the elemental material composition. [5] Bismuth's heavy pnictogen nature yields a large spin-orbit coupling. [1] Additionally, when bound to heavy halogens, bismuth subhalides give rise to a low-dimensional van der Waals bonded structure, exfoliatable into nanowires. [3]

Structure of β-Bi4I4

Low dimensional van der Waals bonded materials display a fundamental material unit, usually depicted as the simplest molecular formula obeying stoichiometry. A series of such fundamental units align in the bulk material phase due to weak van der Waals interactions. Overall, key advantages conferred by the chemical structure are the ease to scale the materials down to nanostructures under simultaneous conservation of the bulk structure and the reduction in defects amount. [6]

b-Bi4I4 solid-state material structure (Bi - purple, I - red). Beta-Bi4I4.png
β-Bi4I4 solid-state material structure (Bi - purple, I - red).
a-Bi4I4 solid-state material structure (Bi - green, I - orange). Alpha-Bi4I4 1.png
α-Bi4I4 solid-state material structure (Bi - green, I - orange).

Belonging to the larger class of quasi 1-dimensional van der Waals bonded materials, β-Bi4I4 has been recently reported as a novel topological insulator. [2] The binary bismuth-iodine family class includes the known bismuth(III) iodide along with additional representatives such as α-Bi4I4, Bi14I4, Bi16I4, and Bi18I4. [2] Having the same stoichiometric chemical formula, α-Bi4I4 and β-Bi4I4 show similar solid-state structures yet critically different physicochemical properties. [8] Specifically, α-Bi4I4 represents the trivial insulator phase, while stacking of the bismuth atoms along the b crystallographic axis in the β-Bi4I4 phase yield a different topological insulator phase. Both isoforms crystallyse in the C2/m space group, with α-Bi4I4 having a unit cell volume almost double of its topological insulator counterpart. [7] The β crytallographic angle is higher in the β-Bi4I4: 107.87 vs 92.96, making the β-Bi4I4 more tilted (see images above). [7]

Synthesis

b-Bi4I4 solid-state synthesis Bi4I4 synthesis.png
β-Bi4I4 solid-state synthesis

Crystal growth of β-Bi4I4 was achieved through a solid-state reaction between Bi and HgI2 in a ratio of 1:2. The mixture of solid-state precursors was sealed under dynamic vacuum in a quartz ampoule and subjected to a temperature gradient of 250°C - 210°C in a two-zone furnace for 20 days. [2] [8] Needle-like blue crystals were obtained with sizes varying from a couple of mm in length and tenths of mm in diameter. [2]

DFT Calculations

Key to modeling the topology of a material are the special points along k-vector of the Brillouin zone, accounting for the accurate depiction of the density of states emerging from the electronics of the material. Density functional theory (DFT) analyses predicted an indirect band gap of 0.158 eV in the β-Bi4I4 phase with the valence and conduction band maxima localized at the Γ and M k-space points, respectively. [2] Interestingly enough, the major contributors to the band structure around the Fermi level are bismuth's p orbitals of even and odd parity, thus giving the gerade and ungerade points of symmetry.

ARPES measurements

The allowed electron energies in the topological insulator were probed with the well-employed angle-resolved photoemission spectroscopy (ARPES). [2] Γ and M space points were found to exhibit binding energies of 0.3 eV and 0.8 eV, respectively. [2] ARPES also probed the Fermi electron velocities along the x and y axes to be 0.1(1)×106 m*s-1 and 0.60(4)×106 m*s-1. [2] The emerging non-trivial states of the topological insulator are expected to show at the space point where the conductive and valence bands almost cross or, in other words, display the smallest band gap. This point indeed showed a binding energy of 0.06 eV as measured by ARPES. [2] ARPES measurements on a different β-Bi4Br4 topological insulator phase show similarity to its iodine counterpart. [9]

Subhalide complexes

Structure of RhBi7Br8 subhalide complex RhBi7Br8.jpg
Structure of RhBi7Br8 subhalide complex

A ternary rhodium-centered bipyramidal dibismuth complex is an example of subhalide complexes with interesting geometry and unusual electronic properties, particularly what has been reported as an example of Möbius aromaticity. [4] [10] The complex exhibits a 4-electron-5-centered bond in the central plane occupied by a Bi5 equatorial pentagon with the rhodium center in the middle. [10] Based on the electronic analysis carried out by Ruck (2003), the bismuth bonding consists of 2-centered-2-electron bonds, namely, Bi-Rh and Bi-Br one (see structure on the right).

The electronic analysis was carried out starting with counting the available skeletal electrons. Each of the 7 bismuth atoms contribute a total of 3x7=21 electrons (3 per each atom), while Rh gives all of its 9 electrons and the 8 bridging bromide atoms yield 3 electrons each. The total skeletal electron count is thus 54. The total skeletal electron count gets distributed as follows: 2 electrons per each of the 16 2c-2e- Bi-Br bond, 2 electrons per each of the 7 2c-2e- Rh-Bi metallic bond, 2 rhodium lone pairs remaining on the Rh centre (total of 4e-), and 4 electrons for 5c-4e- bond pertaining to the central pentagon. The sum of electrons used in bonding is therefore 54. Hence, the subhalide complex is electron-precise, i.e., with all of its skeletal electrons involved in chemical bonding. [10]

Orbital bonding in RhBi7Br8 subhalide complex compared to C5H5 cyclopentadienyl unit Orbital overlap in aromatic systems.jpg
Orbital bonding in RhBi7Br8 subhalide complex compared to C5H5 cyclopentadienyl unit

The bonding in such a system was compared to the aromatic cyclopentadienyl aromatic anion. Contrary to the π-type all in-phase orbital overlap exhibited by the organic cyclopentadienyl anion, σ-type bonding of the RhBi5 unit yields a phase change for an orbital pair (see figure). [10]

Mobius- and Huckel-type aromaticity of the Rh-Bi subhalide complex and cyclopentadienyl anion, respectively Aromaticity.png
Möbius- and Hückel-type aromaticity of the Rh-Bi subhalide complex and cyclopentadienyl anion, respectively

The relative orbital energy diagram is rationalized for each of the systems relying on the Frost-Musulin mnemonic. [11] The two lone pairs stemming from the rhodium metallic center are localized on the lowest-lying twicely degenerate set of molecular orbitals, consistent with the Möbius-type aromaticity. For reference, the electronics of the aromatic organice cyclopentadienyl unit is shown to the right of the rhodium-centered pentagonal Bi5 unit. As can be seen, Hückel rules dictate the molecular orbital splitting is inverted compared to its metallic counterpart, the highest-occupied molecular orbitals this time being twicely degenerate.

See also

Related Research Articles

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<span class="mw-page-title-main">Bismuth(III) oxide</span> Chemical compound

Bismuth(III) oxide is a compound of bismuth, and a common starting point for bismuth chemistry. It is found naturally as the mineral bismite (monoclinic) and sphaerobismoite, but it is usually obtained as a by-product of the smelting of copper and lead ores. Dibismuth trioxide is commonly used to produce the "Dragon's eggs" effect in fireworks, as a replacement of red lead.

<span class="mw-page-title-main">SIESTA (computer program)</span>

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The Hückel method or Hückel molecular orbital theory, proposed by Erich Hückel in 1930, is a simple method for calculating molecular orbitals as linear combinations of atomic orbitals. The theory predicts the molecular orbitals for π-electrons in π-delocalized molecules, such as ethylene, benzene, butadiene, and pyridine. It provides the theoretical basis for Hückel's rule that cyclic, planar molecules or ions with π-electrons are aromatic. It was later extended to conjugated molecules such as pyridine, pyrrole and furan that contain atoms other than carbon and hydrogen (heteroatoms). A more dramatic extension of the method to include σ-electrons, known as the extended Hückel method (EHM), was developed by Roald Hoffmann. The extended Hückel method gives some degree of quantitative accuracy for organic molecules in general and was used to provide computational justification for the Woodward–Hoffmann rules. To distinguish the original approach from Hoffmann's extension, the Hückel method is also known as the simple Hückel method (SHM).

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<span class="mw-page-title-main">Möbius aromaticity</span>

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x. They were originally observed in solutions of bismuth metal in molten bismuth chloride. It has since been found that these clusters are present in the solid state, particularly in salts where germanium tetrachloride or tetrachloroaluminate serve as the counteranions, but also in amorphous phases such as glasses and gels. Bismuth endows materials with a variety of interesting optical properties that can be tuned by changing the supporting material. Commonly-reported structures include the trigonal bipyramidal Bi3+
5 cluster, the octahedral Bi2+
6 cluster, the square antiprismatic Bi2+
8 cluster, and the tricapped trigonal prismatic Bi5+
9 cluster.

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The stabilization of bismuth's +3 oxidation state due to the inert pair effect yields a plethora of organometallic bismuth-transition metal compounds and clusters with interesting electronics and 3D structures.

References

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  6. ↑ Ma, Yuhang; Yi, Huaxin; Liang, Huanrong; Wang, Wan; Zheng, Zhaoqiang; Yao, Jiandong; Yang, Guowei (2023-09-14). "Low-dimensional van der Waals materials for linear-polarization-sensitive photodetection: materials, polarizing strategies and applications". Materials Futures. 3: 012301. doi: 10.1088/2752-5724/acf9ba . ISSN   2752-5724.
  7. 1 2 3 4 "Wismutmonojodid Bi J, eine Verbindung mit Bi(0) und Bi(II)". 1978.
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  9. ↑ Noguchi, Ryo; Kobayashi, Masaru; Jiang, Zhanzhi; Kuroda, Kenta; Takahashi, Takanari; Xu, Zifan; Lee, Daehun; Hirayama, Motoaki; Ochi, Masayuki; Shirasawa, Tetsuroh; Zhang, Peng; Lin, Chun; Bareille, Cédric; Sakuragi, Shunsuke; Tanaka, Hiroaki (2021-02-11). "Evidence for a higher-order topological insulator in a three-dimensional material built from van der Waals stacking of bismuth-halide chains". Nature Materials. 20 (4): 473–479. arXiv: 2002.01134 . Bibcode:2021NatMa..20..473N. doi:10.1038/s41563-020-00871-7. ISSN   1476-4660. PMID   33398124. S2CID   230660660.
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