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Uranocene
Names
IUPAC name
Bis(η8-cyclooctatetraene)uranium[1]
Other names
Uranium cyclooctatetraenide
U(COT)2
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/2C8H8.U/c2*1-2-4-6-8-7-5-3-1;/h2*1-8H;/q2*-2;/b2*2-1-,5-3-,8-6-; ☒N
    Key: RHDYKSUWBHNFEJ-GIKYMASMSA-N ☒N
  • InChI=1/2C8H8.U/c2*1-2-4-6-8-7-5-3-1;/h2*1-8H;/q2*-2;/b2*2-1-,5-3-,8-6-;
    Key: RHDYKSUWBHNFEJ-GIKYMASMBM
  • C1=CC=CC=CC=C1.C1=CC=CC=CC=C1.[U]
Properties
C16H16U
Molar mass 446.33 g/mol
Appearance green crystals[2]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 pyrophoric, radioactive, and toxic
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Uranocene, U(C8H8)2, is an organouranium compound composed of a uranium atom sandwiched between two cyclooctatetraenide rings. It was one of the first organoactinide compounds to be synthesized. It is a green air-sensitive solid that dissolves in organic solvents. Uranocene, a member of the "actinocenes," a group of metallocenes incorporating elements from the actinide series. It is the most studied bis[8]annulene-metal system, although it has no known practical applications.[3]

Synthesis, structure and bonding

[edit]

Uranocene was first described in 1968 by the group of Andrew Streitwieser, when it was prepared by the reaction of dipotassium cyclooctatetraenide and uranium tetrachloride in THF at 0°C:[2]

Synthesis of uranocene

Uranocene is highly reactive toward oxygen, being pyrophoric in air but stable to hydrolysis. The x-ray crystal structure of uranocene was first elucidated by the group of Ken Raymond.[4] Considering the molecule to be U4+(C8H82−)2, the η8-cyclooctatetraenide groups are planar, as expected for a ring containing 10 π-electrons, and are mutually parallel, forming a sandwich containing the uranium atom. In the solid state, the rings are eclipsed, conferring D8h symmetry on the molecule. In solution the rings rotate with a low activation energy.

The uranium-cyclooctatetraenyl bonding was shown by photoelectron spectroscopy to be primarily due to mixing of uranium 6d orbitals into ligand pi orbitals and therefore donation of electronic charge to the uranium, with a smaller such interaction involving the uranium (5f)2 orbitals.[5] Electronic theory calculations agree with this result[6][7] and point out that the weaker interaction of the open-shell 5f orbitals with the ligand orbitals determines |MJ|, the magnitude of the angular momentum quantum number along the 8-fold symmetry axis of the ground state.[7]

Spectroscopic properties

[edit]

Uranocene is paramagnetic. Its magnetic susceptibility is consistent with values of 3 or 4 for |MJ|, with the accompanying magnetic moment being affected by the spin-orbit coupling.[8] Its NMR spectrum is consistent with an |MJ| value of 3.[9] Electronic theory calculations from the simplest[10] to the most accurate[11] also give |MJ| values of 3 for the ground state and 2 for the first excited state, corresponding to double-group symmetry designations[12] of E3g and E2g for these states.

The green color of uranocene is due to three strong transitions in its visible spectrum.[2][13] In addition to finding vibrational frequencies, Raman spectra indicate the presence of a low-lying (E2g) excited electronic state.[13][14] On the basis of calculations,[7] the visible transitions are assigned to transitions primarily of 5f-to-6d nature, giving rise to E2u and E3u states.

Analogous compounds

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Analogous compounds of the form M(C8H8)2 exist for M = (Nd, Tb, Yb, Th, Pa, Np, and Pu). Extensions include the air-stable derivative U(C8H4Ph4)2 and the cycloheptatrienyl species [U(C7H7)2]−.[3] In contrast, bis(cyclooctatetraene)iron has a very different structure, with one each of a η6- and η4-C8H8 ligands.

References

[edit]

Further reading

[edit]
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Uranocene

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Uranocene, with the chemical formula (C₈H₈)₂U, is an organoactinide compound consisting of a uranium(IV) ion sandwiched between two parallel, planar cyclooctatetraene (COT) dianion ligands in an η⁸-coordination mode, forming a highly symmetric D₈ₕ structure.[1] First synthesized in 1968 by Andrew Streitwieser Jr. and Ulrich Mueller-Westerhoff through the reaction of uranium tetrachloride (UCl₄) with potassium cyclooctatetraenide (K₂C₈H₈) in tetrahydrofuran (THF), it represents the inaugural member of the actinocene family, analogous to metallocenes but featuring f-block elements.[2] This air-sensitive green solid sublimes at approximately 180 °C under reduced pressure (0.03 mmHg) and exhibits paramagnetic behavior due to two unpaired 5f electrons.[1] The discovery of uranocene built on earlier predictions of stable actinide-COT complexes and paralleled the 1950s breakthroughs in transition metal sandwich compounds like ferrocene, highlighting the potential for aromatic π-ligands with actinides.[1] Its crystal structure, determined in 1969 via X-ray diffraction, revealed average U–C bond lengths of 2.65 Å and C–C bond lengths of 1.39 Å within the planar COT rings, confirming a centrosymmetric geometry with the uranium atom at the molecular center.[3] Bonding in uranocene involves significant covalency, with contributions from uranium's 5f, 6d, and 7s/p orbitals interacting with the filled π-orbitals of the COT ligands, as evidenced by molecular orbital calculations and spectroscopic studies.[1] Uranocene's synthesis and characterization spurred advancements in f-element organometallic chemistry, including derivatives with substituted COT ligands and analogs for other actinides like thorocene and neptunocene.[1] Despite its thermal stability and solubility in organic solvents like benzene and THF, it reacts readily with air and moisture, limiting practical applications but enabling studies on actinide-ligand interactions relevant to nuclear chemistry and catalysis.[1] Its magnetic properties, including a room-temperature magnetic moment of 2.6–2.7 Bohr magnetons, further underscore the role of 5f electrons in these systems.[1]

History and Discovery

Discovery and Synthesis

Uranocene, with the chemical formula U(C₈H₈)₂, was first synthesized in 1968 by Andrew Streitwieser Jr. and Ulrich Müller-Westerhoff at the University of California, Berkeley.[4] This breakthrough marked the initial preparation of a stable organoactinide compound, achieved through the reaction of uranium tetrachloride (UCl₄) with the cyclooctatetraene dianion, generated in situ from potassium metal and cyclooctatetraene to form dipotassium cyclooctatetraenide (K₂C₈H₈), in tetrahydrofuran (THF) solvent.[5] The reaction proceeds as 2 K₂C₈H₈ + UCl₄ → U(C₈H₈)₂ + 4 KCl, yielding a green, crystalline solid after workup under inert conditions.[5] This compound was promptly recognized as the archetypal sandwich complex in actinide chemistry, featuring a uranium(IV) center η⁸-coordinated between two planar cyclooctatetraenide rings, analogous to ferrocene but utilizing f-orbital involvement.[4] The synthesis represented a pivotal advance, demonstrating the feasibility of delocalized π-bonding in f-block organometallics and opening the field of organoactinide chemistry.[5] Initial efforts to handle uranocene were complicated by its extreme air sensitivity and pyrophoric nature, necessitating rigorous inert-atmosphere techniques, as well as precautions against the inherent radioactivity of the uranium isotope used (typically ²³⁸U).[5] These properties limited early characterizations but underscored the compound's stability under anhydrous, anaerobic conditions.[4]

Historical Significance

Uranocene, synthesized in 1968, was recognized as the first stable actinide sandwich complex, featuring a uranium(IV) center coordinated between two cyclooctatetraenide dianion ligands in a parallel π-bonded arrangement.[5] This breakthrough challenged prevailing assumptions that f-orbitals in actinides contributed minimally to bonding, instead demonstrating significant involvement of uranium's 5f and 6d orbitals in covalent interactions with the carbon-based ligands.[5] By establishing a viable organometallic framework for an f-block element, uranocene shifted perceptions of actinides from predominantly ionic, inorganic species to elements capable of forming robust uranium-carbon bonds, thereby enabling broader exploration of organoactinide reactivity.[5] The compound's discovery had profound implications for electron-counting rules in f-block chemistry, extending the 18-electron rule—originally formulated for transition metals—to actinides by incorporating f-orbital contributions into the valence electron tally.[5] Uranocene's configuration, with its 20 valence electrons achieved through δ-bonding between the metal and ligands, provided a conceptual bridge between d- and f-block organometallics despite deviations from the strict 18-electron count. This paved the way for subsequent developments, including the synthesis of analogous lanthanide and actinide bent metallocenes, which further explored non-parallel ligand arrangements and enhanced understanding of f-orbital roles in molecular geometry and stability.[5] Uranocene represented a key milestone in the evolution of sandwich compound chemistry, building on the foundational work recognized by the 1973 Nobel Prize in Chemistry awarded to Ernst Otto Fischer for his pioneering studies on organometallic sandwich complexes like ferrocene. While Fischer's contributions focused on transition metal systems, uranocene exemplified the extension of these principles to the actinide series, inspiring a new era of research into f-element organometallics and their potential applications in catalysis and materials science. Despite its air sensitivity, which necessitated inert-atmosphere handling, the compound's stability in solution underscored the feasibility of actinide-based organometallics.[5]

Chemical Synthesis

Original Preparation

The original preparation of uranocene, reported in 1968, involves the reaction of uranium metal with potassium and cyclooctatetraene (C₈H₈) in refluxing tetrahydrofuran (THF) under an inert atmosphere.[4] A common modification, also from early work, generates the cyclooctatetraene dianion, K₂C₈H₈, by reducing C₈H₈ with excess potassium metal in THF at room temperature under nitrogen to prevent oxidation.[5] Uranocene is then formed by adding a slurry of UCl₄ in THF to a solution of the dianion (two equivalents) at 0°C, with the mixture stirred under nitrogen for several hours, following the stoichiometry:
2K2C8H8+UCl4→U(C8H8)2+4KCl 2 \mathrm{K_2C_8H_8} + \mathrm{UCl_4} \to \mathrm{U(C_8H_8)_2} + 4 \mathrm{KCl}
The reaction is highly sensitive to oxygen and moisture, requiring glovebox or Schlenk line techniques due to the pyrophoric nature of the reagents and product, which ignites in air.[5] Upon completion, the product precipitates as a deep green solid; hexane is added to complete precipitation, followed by filtration under inert conditions. The solid is washed with cold THF and hexane to remove KCl and excess reagents, then dried under vacuum. Further purification yields shiny green crystals via sublimation at approximately 180–200°C under reduced pressure (0.03–0.1 mmHg). Typical yields range from 50–70%, depending on the purity of the starting materials and handling precision.[5]

Alternative Synthetic Routes

Another approach utilizes the reduction of UCl₄ with magnesium in the presence of COT in THF to form the half-sandwich precursor (η⁸-C₈H₈)UCl₂, which can be further processed to uranocene. These metal reductions address solubility issues in the original protocol but often require optimization for complete bis-ligation. [6] Solvent-free methods have also been reported, such as the direct interaction of mercury-activated uranium metal with COT at room temperature, combining synthesis and extraction in a single apparatus without the need for a strictly oxygen-free environment. This variant enhances scalability for larger preparations and allows use of depleted uranium (low ²³⁵U content) to minimize radioactivity, facilitating safer handling for spectroscopic studies. Additionally, uranocene forms via reaction of COT with uranium hydride under similar conditions. [5][7]

Structure and Bonding

Molecular Geometry

Uranocene exhibits a classic sandwich molecular geometry, with a central uranium(IV) atom positioned equidistantly between two parallel cyclooctatetraenide (C₈H₈²⁻) ligands. Each ligand adopts an η⁸-coordination mode, binding all eight carbon atoms to the metal center. In the free cyclooctatetraene molecule, the ring assumes a non-planar tub conformation to minimize strain; however, upon deprotonation to the dianion and coordination, the rings flatten to become nearly perfectly planar, facilitating optimal π-overlap with the uranium orbitals.[5] The crystal structure of uranocene was determined by single-crystal X-ray diffraction in 1969, revealing an eight-coordinate uranium environment consistent with the predicted sandwich motif.[3] In the ideal gas-phase or solution structure, the molecule possesses D₈ₕ point group symmetry, characterized by eclipsed rings separated by approximately 3.80 Å and a linear U-centroid-U angle of 180°. The average uranium-carbon bond distance is 2.64 Å, while the perpendicular distance from the uranium atom to each ring centroid is 1.90 Å.[3] In the solid state, subtle deviations from ideal D₈ₕ symmetry are observed, including minor distortions in ring planarity and bond lengths, which have been attributed to Jahn-Teller-like effects arising from the electronic configuration of uranium(IV). These perturbations do not significantly alter the overall sandwich architecture but highlight the influence of crystal packing and low-symmetry electronic states on the molecular geometry.

Electronic Structure and Bonding Models

Uranocene, with the formula U(C₈H₈)₂, exhibits a 20-electron valence configuration, arising from the uranium(IV) center in a d⁰ f² electronic state and two cyclooctatetraenide (COT²⁻) ligands each donating 10 π electrons. This electron count deviates from the conventional 18-electron rule typical of d-block metallocenes, instead adhering to an 8-electron rule that emphasizes delta (δ) bonding interactions between the metal and ligands.[8][5] The primary bonding model for uranocene is a δ-bonding framework, in which the uranium 6d δ orbitals overlap with the π* orbitals of the COT²⁻ ligands to form eight U–C δ bonds. These interactions provide the dominant stabilization, with the planar, parallel arrangement of the COT rings facilitating symmetric δ overlap across the eight carbon atoms per ligand. Early theoretical treatments highlighted comparable contributions from 5f and 6d orbitals, but subsequent analyses refined this picture to underscore the primacy of 6d involvement.[8][5] The participation of 5f orbitals remains a point of debate, influenced by relativistic effects that contract and stabilize these orbitals in actinides. Density functional theory (DFT) calculations, incorporating relativistic corrections, reveal minimal direct 5f orbital involvement in the primary bonding, suggesting the f electrons are largely nonbonding and localized, while relativistic enhancements primarily affect the 6d orbital energies to promote covalency.[9] In contrast, an ionic bonding model posits uranocene as an electrostatic assembly of a U⁴⁺ cation electrostatically stabilized by two dianionic COT²⁻ ligands, akin to a "sandwich" of charged planes. Although this simple ionic description captures the overall charge balance and stability, computational studies confirm substantial covalent character, particularly through the δ interactions, rendering the pure ionic view incomplete.[5]

Properties

Physical Properties

Uranocene appears as a dark green to emerald green crystalline solid. It is highly air-sensitive and pyrophoric, igniting spontaneously upon exposure to air, and decomposes rapidly in air to form uranium dioxide and cyclooctatetraene.[10][5][11] Under inert conditions, uranocene exhibits limited thermal stability, subliming at 180–220 °C under high vacuum (ca. 0.03 mmHg). Above approximately 300 °C, it decomposes to uranium-containing residues and organic fragments. It is slowly hydrolyzed in neutral water but reacts rapidly with strong acids or bases.[10][5][11] Uranocene is soluble in coordinating and aromatic solvents such as tetrahydrofuran (THF), toluene, and benzene, but insoluble in nonpolar aliphatic hydrocarbons like hexane.[10]

Spectroscopic Properties

Uranocene has been characterized by several spectroscopic techniques that reveal its electronic and vibrational features, consistent with its D8h symmetric sandwich structure. In 1H NMR spectroscopy, uranocene exhibits a singlet at -41.9 ppm in THF-d8, reflecting the equivalence of all 16 protons on the two cyclooctatetraenide ligands and supporting the high D8h symmetry in solution.[12] Infrared (IR) spectroscopy shows characteristic C-H stretching vibrations for the aromatic protons at 3000–3100 cm−1, while the U-C bonding modes appear at 211 cm−1 (symmetric stretch) and 240 cm−1 (asymmetric stretch), as observed in the low-frequency region.[11] The UV-Vis spectrum of uranocene displays intense absorption bands at 627 nm, 655 nm, and 670 nm in the visible region, arising from 5f → 6d transitions.[13] Mass spectrometry confirms the molecular formula with a molecular ion peak at m/z 446 for [U(C8H8)2]+, accompanied by fragmentation to the [C8H8U]+ ion at m/z 342.[14]

Reactivity and Derivatives

Chemical Reactivity

Uranocene exhibits notable reactivity toward protic reagents, particularly water, where it undergoes hydrolysis to yield uranium oxides and a mixture of cyclooctatriene isomers (1,3,5-cyclooctatriene and 1,3,6-cyclooctatriene). This decomposition proceeds via a mechanism involving initial coordination of water to the uranium center, followed by protonation of the cyclooctatetraenide ligands. The reaction kinetics are pseudo-first-order under conditions of excess water (e.g., 1 M in THF), indicating a moderately facile process despite the compound's general stability in dry environments.[15][16] The compound is highly sensitive to oxidation by molecular oxygen, reacting in tetrahydrofuran (THF) solutions to quantitatively produce UO₂ and C₈H₈ upon exposure to air. This transformation reflects the susceptibility of the U(IV) center to aerial oxidation, forming uranyl-like species under prolonged contact, although ignition does not occur spontaneously at ambient temperatures. Instead, complete oxidation requires elevated conditions, such as heating at 120 °C in air for several days, underscoring the steric protection afforded by the bulky cyclooctatetraenide ligands that limits rapid reactivity compared to lighter metallocenes.[5] Coordination chemistry of uranocene involves the addition of neutral Lewis bases, which disrupt the parallel sandwich geometry to form bent adducts. For instance, reaction with bases like pyridine, 4,4'-bipyridine, or tert-butyl isocyanide yields complexes of the type [(η⁸-C₈H₈)₂U(L)], where the ligand L coordinates axially to the uranium, altering the U–centroid distances and introducing asymmetry in the structure. Similar behavior is observed with ethereal solvents such as THF, forming adducts like U(C₈H₈)₂(THF)₂ that maintain the core sandwich motif but exhibit modified electronic properties due to donor interactions. These adducts highlight the Lewis acidity of the U(IV) center, enabling reversible binding without ligand displacement. Efforts to reduce uranocene to lower oxidation states reveal its stability toward mild reductants, but strong reducing conditions or electrochemical methods successfully generate U(III) species. Cyclic voltammetry in THF shows two reversible one-electron reductions, the first at approximately -2.1 V vs. SCE, leading to the monoanion [U(C₈H₈)₂]⁻ representing a formal U(III) complex, and then the dianion [U(C₈H₈)₂]²⁻ representing U(II), with two dianionic cyclooctatetraene ligands. Chemical reduction with potent agents like potassium naphthalenide similarly affords these low-valent derivatives, which display enhanced reactivity due to the increased electron density at uranium.[5]

Key Derivatives

One prominent derivative of uranocene is bis(η⁸-1,3,5,7-tetraphenylcyclooctatetraenide)uranium(IV), formulated as $ \mathrm{U(C_8H_4Ph_4)_2} $, which was synthesized in 1975 by reacting uranium tetrachloride with the dilithium salt of 1,3,5,7-tetraphenylcyclooctatetraene in tetrahydrofuran. This compound forms as a black, air-stable solid, attributed to the steric bulk of the phenyl substituents that shield the uranium center from oxidative decomposition, in contrast to the air-sensitive parent uranocene. It sublimes unchanged at 400 °C under vacuum and exhibits a staggered sandwich geometry similar to the parent compound, with U–C distances averaging 2.72 Å. Alkyl-substituted uranocenes represent another class of derivatives designed to modulate stability and electronic properties through peripheral modification of the cyclooctatetraenide (COT) ligands. Examples include bis(η⁸-1,1',3,3',5,5',7,7'-octamethylcyclooctatetraenide)uranium(IV) and bis(η⁸-1,1',5,5'-tetra-tert-butylcyclooctatetraenide)uranium(IV), prepared via analogous metathesis reactions of UCl₄ with the corresponding dilithio-COT salts. These compounds display enhanced solubility in hydrocarbons and thermal stability compared to unsubstituted uranocene, with the tert-butyl variant showing particularly robust resistance to ligand displacement due to steric encumbrance. Crystal structures confirm retained parallel sandwich motifs, though subtle bending of the COT rings occurs in some cases, influencing the U–centroid distance to approximately 1.90 Å. Anionic derivatives arise from reduction of uranocene or its substituted analogs, yielding rare uranium(III) sandwich complexes. For instance, in 2024, bis(η⁸-dibenzocyclooctatetraenide)uranium(III) complexes were isolated as salts, accessed via salt metathesis of UI₃ precursors with the dilithio-dbCOT ligand followed by counterion exchange, featuring eclipsed or staggered geometries with U–centroid angles near 170–180° and exhibiting intense near-infrared absorptions diagnostic of f¹ electron configurations.[17] Such derivatives highlight the potential for accessing low-valent uranium chemistry while maintaining the core COT sandwich framework.[17]

Related Compounds

Actinide Analogues

Thorocene, Th(C₈H₈)₂, the actinide analogue featuring thorium, was synthesized in 1969 via the reaction of thorium tetrachloride with dipotassium cyclooctatetraenide in tetrahydrofuran, analogous to the preparation of uranocene. This bright yellow, air-sensitive solid exhibits greater thermal and chemical stability compared to uranocene, remaining intact under inert conditions up to higher temperatures.[18] Its bonding is predominantly ionic, with the Th⁴⁺ ion interacting electrostatically with the two η⁸-coordinated cyclooctatetraenide dianions, as evidenced by longer Th–C distances averaging 2.67 Å and minimal involvement of thorium 5f orbitals in metal–ligand overlap.[19] Neptunocene, Np(C₈H₈)₂, was prepared in 1970 by a similar metathesis reaction between neptunium tetrachloride and K₂C₈H₈ in a non-polar solvent, yielding an olive-green solid. It is less stable than thorocene or uranocene, decomposing more readily in solution and showing sensitivity to moisture and oxygen, though it can be handled under rigorous inert conditions.[18] The bonding displays intermediate character, with Np–C distances averaging 2.63 Å reflecting actinide contraction and slight enhancement in covalency through partial 5f orbital participation compared to thorium.[18] Plutonocene, Pu(C₈H₈)₂, the plutonium analogue, was first synthesized in 1970. A 2018 preparation involved oxidation of a plutonium(III) sandwich precursor derived from the reduction of PuCl₃ with potassium cyclooctatetraenide. As a highly radioactive compound, its handling is severely limited, but structural analysis reveals Pu–C distances of 2.63–2.64 Å, confirming further actinide contraction. The bonding exhibits increased covalency relative to lighter actinocenes, with stronger plutonium 5f–π* orbital interactions contributing to its reactivity.[18] Across the actinide series from thorium to plutonium, these sandwich compounds show decreasing stability and increasing reactivity with rising atomic number, attributed to progressive actinide contraction shortening metal–ligand bonds and enhanced 5f covalency that facilitates ligand displacement and redox processes.[18] Thorocene's ionic dominance gives way to more covalent interactions in neptunocene and plutonocene, influencing their spectroscopic and magnetic properties.

Non-Actinide Analogues

Lanthanide sandwich complexes with cyclooctatetraene (COT, C8H8) ligands serve as key non-actinide analogues to uranocene, featuring divalent metals in structures similar to U(C8H8)2 but with more ionic character due to the lanthanides' predominant electrostatic bonding. For example, the ytterbocene anion [Yb(C8H8)2]− exhibits a parallel sandwich geometry with D4h symmetry and has been synthesized as the potassium salt K[Yb(C8H8)2], displaying volatility suitable for applications in vapor deposition processes owing to its low molecular weight and weak intermolecular interactions.[20] These complexes, such as [Li(DME)3][Ln(COT″)2] where COT″ is the 1,4-bis(trimethylsilyl)COT ligand and Ln = Y, La, or Yb, demonstrate high solubility in nonpolar solvents and good crystallinity, facilitating their isolation and study.[21] In contrast to the parallel-ring arrangement in uranocene and lanthanocenes, Group 4 metallocene analogues with COT adopt bent structures to accommodate the smaller metal ions and achieve optimal orbital overlap. A representative example is the zirconocene complex [Zr(η⁴-C8H8)(η⁸-C8H8)], where one COT ring binds in a planar η⁸ mode parallel to the metal while the other coordinates in a non-planar η⁴ mode, resulting in a folded sandwich with a Zr–Ctr distance of approximately 2.1 Å for the η⁸ ring.[22] This geometry reflects the d-block metals' preference for localized bonding over the delocalized 10-electron donation seen in f-block analogues, leading to lower hapticity and reactivity differences, such as easier ring slippage.[23] Beryllocene, Be(C8H8), stands out as an early main-group analogue, marking the first reported sandwich compound utilizing an 8π-aromatic COT ligand with a non-f-block metal, though its high reactivity limits practical applications and structural characterization remains challenging due to instability.[24] Overall, non-actinide COT sandwiches, particularly lanthanide variants, exhibit greater air stability compared to actinide counterparts like uranocene, attributable to the lanthanides' larger ionic radii (e.g., Yb²⁺ ~1.02 Å vs. U⁴⁺ ~0.89 Å), lower charge, and more ionic bonding with minimal 4f orbital involvement.[21]
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