Molecular Complexes of Fullerenes C60 and C70 with Saturated Amines

Synthesis, Crystal Structures, Magnetic Properties and Photoconductivity of C60 and C70 Complexes with Metal Dialkyldithiocarbamates M(R2dtc)x, where M = CuII, CuI, AgI, ZnII, CdII, HgII, MnII, NiII, and PtII; R = Me, Et, and nPr

“…[59] A condition necessary for the observation of this band in the solid-state spectra of the complexes is close packing of fullerene molecules in the crystal. [7,60] Since C 60 molecules are closely packed in 1, 7, and 6, this band can manifest itself in their spectra. However, in the spectrum Table 3.…”

“…Fullerenes form a wide variety of donor-acceptor complexes ranging from molecular to ionic ones [1][2][3] with different classes of organic and organometallic donors: aromatic hydrocarbons, [4] amines, [5][6][7] tetrathiafulvalenes, and a flattening of the central (NCS 2 ) 2 Cu fragments. Complex 10 shows a spectrum exhibiting features from 50 to 600 mT and manifests strong antiferromagnetic coupling of spins with a Weiss temperature of -96 K and the maximum of magnetic susceptibility at 46 K. Such magnetic behavior can be explained by the formation of [Mn(Et 2 dtc) 2 ] 2 dimers in 10.…”

Crystal Structures, EPR Spectra, and Magnetic Properties of a Series of Ionic Multi‐Component Complexes [(TBPDA)2·(C60·–)·(D+)] (D = Cp*2Cr, Cp*2Co, TDAE)

“…The absorption bands of TBPDA in the IR spectrum are shifted by up to 10 cm -1 in 1 and 2 relative to those in the spectrum of neutral TBPDA·(C 60 ) 2 . [27] This is probably associated with the different geometry of TBPDA in 1, 2, and TBPDA·(C 60 ) 2 . The absence of additional absorption bands in the IR and UV/ Visible/NIR spectra of 1 and 2, which must accompany the dimerization or polymerization of C 60 ·-, [28] indicates their monomeric nature at room temperature (room temp.).…”

Synthesis and Crystal Structure of a Cocrystalline Compound of a Rare Earth Metalloporphyrin with Fullerene {[TPPYb(μ‐OH)2Yb(THF)TPP]·C60}n

“…[9g,10a] The N···C(C 60 ) distances in 1 are in the range of 3.08-3.09 Å and lie at the lower end of the range of van der Waals contacts, and well below the "standard" contact distance (3.2-3.3 Å), and are similar to the corresponding distances in metal-free porphyrin fullerene complexes. [13] However, these distances are significantly longer than the corresponding distances in transition metalloporphyrin fullerene cocrystals. [9][10][11] This may be attributed to the electron-deficient character of rare earth metal ions, and the electronacceptor nature of fullerene, resulting in weaker interactions between the metalated porphyrin units and the fullerenes.…”