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Room-Temperature Chemical Synthesis of C2

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Room-Temperature Chemical Synthesis of C2 ARTICLE https://doi.org/10.1038/s41467-020-16025-x OPEN Room-temperature chemical synthesis of C2 ✉ Kazunori Miyamoto 1,6 , Shodai Narita1,6, Yui Masumoto1, Takahiro Hashishin1, Taisei Osawa1, ✉ Mutsumi Kimura 2,3, Masahito Ochiai4 & Masanobu Uchiyama 1,3,5 Diatomic carbon (C2) is historically an elusive chemical species. It has long been believed that the generation of C2 requires extremely high physical energy, such as an electric carbon arc or multiple photon excitation, and so it has been the general consensus that the inherent nature of C2 in the ground state is experimentally inaccessible. Here, we present the chemical 1234567890():,; 3 synthesis of C2 from a hypervalent alkynyl-λ -iodane in a flask at room temperature or below, providing experimental evidence to support theoretical predictions that C2 has a singlet biradical character with a quadruple bond, thus settling a long-standing controversy between experimental and theoretical chemists, and that C2 serves as a molecular element in the bottom-up chemical synthesis of nanocarbons such as graphite, carbon nanotubes, and C60. 1 Graduate School of Pharmaceutical Sciences, The University of Tokyo, 7-3-1 Hongo, Bunkyo-ku, Tokyo 113-0033, Japan. 2 Division of Chemistry and Materials, Faculty of Textile Science and Technology, Shinshu University, Ueda 386-8567, Japan. 3 Research Initiative for Supra-Materials (RISM), Shinshu University, Ueda 386-8567, Japan. 4 Graduate School of Pharmaceutical Sciences, University of Tokushima, 1-78 Shomachi, Tokushima 770-8505, Japan. 5 Cluster of Pioneering Research (CPR), Advanced Elements Chemistry Laboratory, RIKEN, 2-1 Hirosawa, Wako-shi, Saitama 351-0198, Japan. 6These authors ✉ contributed equally: Kazunori Miyamoto, Shodai Narita. email: [email protected]; [email protected] NATURE COMMUNICATIONS | (2020) 11:2134 | https://doi.org/10.1038/s41467-020-16025-x | www.nature.com/naturecommunications 1 ARTICLE NATURE COMMUNICATIONS | https://doi.org/10.1038/s41467-020-16025-x → ← iatomic carbon (C2) exists in carbon vapor, comets, the means of dative interactions (L: C2 :L), but such stabilized com- 9–12 stellar atmosphere, and interstellar matter, but although it plexes no longer retain the original character of C2 (Fig. 1b) . D 1 was discovered in 1857 , it has proven frustratingly dif- Instead, theoretical/computational simulation has been applied fi cult to characterize, since C2 gas occurs only at extremely high recently, and the results indicated that C2 has a quadruple bond with temperatures (above 3500 °C)2. Considerable efforts have been a singlet biradical character in the ground state13,14. fi made to generate/capture C2 experimentally and to measure its These various theoretical and experimental ndings have physicochemical properties. The first successful example of arti- sparked extensive debate on the molecular bond order and elec- fi fi fi cial generation of C2, which was con rmed spectroscopically, tronic state of C2 in the scienti c literature, probably because of involved the use of an electric carbon arc under high vacuum the lack of a method for the synthesis of ground-state C2. Here, conditions3. Subsequent chemical trapping studies pioneered by we present a straightforward room-temperature/pressure synth- Skell indicated that C2 behaves as a mixture of singlet dicarbene esis of C2 in a flask. We show that C2 generated under these and triplet biradical states in a ratio of 7:3 to 8:2 (Fig. 1a)4–7. conditions behaves exclusively as a singlet biradical with quad- Multiple photon dissociation of two-carbon small molecules ruple bonding, as predicted by theory. We also show that spon- (acetylene, ethylene, tetrabromoethylene, etc.) by infrared or UV taneous, solvent-free reaction of in situ generated C2 under an irradiation in the gas phase was also developed to generate C2, but argon atmosphere results in the formation of graphite, carbon 8 this photo-generated C2 also exhibited several electronic states . nanotubes (CNTs), and fullerene (C60) at room temperature. This Recently, other approaches for the isolation of C2 have been not only represents a bottom-up chemical synthesis of nano- reported, using potent electron-donating ligands to stabilize C2 by carbons at ordinary temperature and pressure, but it also provides a Chemical trapping reactions of C2 singlet O carbene path Me Me O 3 Me C CC + H singlet triplet carbene path biradical path 2 4 C Graphite + 16V-arc C C C in vacuo (10 Torr) 5 6 (ca. 7 : 3) 7 6 (singlet carbene path) b Isolation of C2 by stabilization with electron-donating ligands Mes iPr Et Et Me N C C N Me Me iPr Me N 9 + + CC Mes Ph3P C C PPh3 N Me i Me 10 Et Et Pr Me i Pr Mes = Me 8 Me c This work F Me3Si CC I FBF3 2 Room Bottom-up Ph temperature Singlet chemical 1a biradical synthesis Fig. 1 Previous experimental work on C2 and our synthesis of C2 at low temperature in a flask. a Chemical trapping of C2 generated by a carbon arc. b Isolation of C2 stabilized by potent electron-donating ligands. c Our chemical synthesis of C2 at ambient temperature under normal pressure by utilizing hypervalent alkynyl-λ3-iodane 1a. 2 NATURE COMMUNICATIONS | (2020) 11:2134 | https://doi.org/10.1038/s41467-020-16025-x | www.nature.com/naturecommunications NATURE COMMUNICATIONS | https://doi.org/10.1038/s41467-020-16025-x ARTICLE λ2 experimental evidence that C2 may serve as a key intermediate in as those via ethynyl(phenyl)- -iodanyl radical (Supplementary the formation of various carbon allotropes (Fig. 1c). Fig. 4)27. In order to obtain more direct information about the “ ” fl Results generation of C2 gas, we designed a connected- ask, solvent- free experiment (Fig. 2c): a solvent-free chemical synthesis of C2 Chemical synthesis of C2. The key strategy underlying the pre- – using 1a with three equivalents of CsF was carried out in one of a sent achievement is the use of hypervalent iodane chemistry15 17, pair of connected flasks (Flask A), and three equivalents of 14 was aiming to utilize the phenyl-λ3-iodanyl moiety as a hyper-leaving placed in the other flask (Flask B). The reaction mixture in Flask group (ca. 106 times greater leaving ability than triflate A was vigorously stirred at room temperature for 72 h under (–OSO CF ), a so-called super-leaving group)18. We designed [β- 2 3 argon. As the reaction proceeds in Flask A, generated C gas (trimethylsilyl)ethynyl](phenyl)-λ3-iodane 1a19, in the expecta- 2 should pass from Flask A to Flask B. Indeed, the color of 14 in tion that it would generate C upon desilylation of 1a with 2 Flask B gradually changed from deep purple to deep brown as the fluoride ion to form anionic ethynyl-λ3-iodane 11, followed by reaction progressed. After 72 h, the formation of 15 and 16 was facile reductive elimination of iodobenzene. Gratifyingly, expo- confirmed by APCI–MS analysis of the residue in Flask B. We sure of 1a to 1.2 equivalents of tetra-n-butylammonium fluoride then performed a 13C-labeling experiment using 1b-13Cβ, which (Bu4NF) in dichloromethane resulted in smooth decomposition 13 – 28,29 − was synthesized from H3 C I in eight steps . Treatment of at 30 °C with the formation of acetylene and iodobenzene, 13 13 1b- Cβ (99% C) with Bu4NF in the presence of 14 in CH2Cl2 indicating the generation of C2! However, all attempts to capture gave a mixture of 15-13Cα and 15-13Cβ, suggesting that C is C with a range of ketones and olefins, such as acetone (3), 2 2 generated before the O-ethynyl bond-forming reaction with 14 1,3,5,7-cyclooctatetraene (4), styrene (7), and 1,3,5-cyclohepta- (Fig. 2d). The observed O–13C/12C selectivity (71:29) may be triene, failed, though they smoothly reacted with arc-generated C – 2 related to very fast radical pairing between C and 14 prior to on an argon matrix at −196 °C3 5,20. These findings immediately 2 ejection of iodobenzene from the solvent cage30. We also carried suggested that the putative C2 synthesized here at −30 °C has a out 13C-labeling experiments using 1b-13Cβ in solvents of significantly different character from C generated under high- 2 different viscosities (η). The observed O–13C/12C selectivity energy conditions (Supplementary Fig. 1). decreased as the viscosity decreased, and the regioselectivity was almost lost (52:48) under solvent-free conditions. Similarly, the Experimental evidence for singlet biradical character. Taking O–13C/12C selectivity was 51:49 in the connected-flask experi- account of the fact that quantum chemical calculations suggest a ment. All these findings rule out stepwise addition/elimination relatively stable singlet biradical C2 with quadruple bonding in the mechanisms (Supplementary Fig. 5). ground state, we next examined an excellent hydrogen donor. 9,10- Dihydroanthracene has very weak C–H bonds (bond dissociation −1 −1 21,22 energy of 12:76.3kcalmol vs CH2Cl2:97.3kcalmol ) that Role as molecular element of nanocarbons. Given that C2 might effectively trap the putative singlet biradical C2.When12 was generated at room temperature or below behaves exclusively as a added to the reaction mixture, anthracene (13) was obtained singlet biradical, as theoretically predicted for the ground state, accompanied with the formation of acetylene (Fig. 2a), which we examined whether this ground-state C2 would serve as a clearly suggests that the generation of C2 and subsequent molecular element for the formation of various carbon allotropes. hydrogen abstraction from 12 gave acetylene. The formation of Today, nanocarbons such as graphene, CNTs, and fullerenes, in 2 acetylene was confirmed by Raman spectroscopy after AgNO3 which sp carbon takes the form of a planar sheet, tube, ellipsoid, trapping, and the amount of acetylene was estimated by the or hollow sphere, are at the heart of nanotechnology31.
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