Abstract:Just SO! The recently published synthesis of the SO dication is summarized along with the connection to the dications [C Me ] and [Cp* Fe ]. The molecular structure of the cation [C Me SO ] is shown in the figure (gray C, red O, yellow S).
“…The 1007.7, 755.3, 686.3, and 669.9 cm −1 absorptions exhibit identical behaviors upon sample annealing and UV−vis irradiation, indicating they should belong to different vibrational modes of the same product. The 1007.7 cm −1 band shifted to 958.9 cm −1 upon 18 O substitution with an 16 O/ 18 O frequency ratio of 1.0509, suggesting that it should be a terminal Mo−O stretch in comparison to the values of the same mode of OMoF 2 (1007.6 cm −1 and 1.0505). 40 This assignment is further confirmed by the zero shift when the 34 SO 2 F 2 sample was used.…”
Section: Methodsmentioning
confidence: 96%
“…14 The side-on (η 2 -SO) coordination fashion was corroborated for the group 4 and 5 metal complexes, 15,16 and the group 5 metal complexes can be considered as (OMF 2 ) + (SO) − based on the S−O stretching vibrational frequency and bond length. 16 The existence of SO − in the SO complexes of group 5 metals raises the question of whether SO can be further reduced upon coordination to transition metals with richer electrons, since O 2 , which is isoelectronic to SO, 6,17,18 undergoes stepwise activation to form superoxo and peroxo complexes upon coordination to metal centers. 19−21 There has been a comparison focusing on the Fe−SO 2− and Fe−O 2 2− intermediates from the theoretical point of view, 22 but experimental evidence that clearly demonstrates the existence of a peroxo-like sulfur monoxide (SO 2− ) complex of transition metal is limited.…”
Peroxo-like sulfur monoxide complexes of molybdenum and tungsten oxyfluorides [OMF 2 (η 2 -SO)] were prepared via the reactions of molybdenum and tungsten atoms and SO 2 F 2 in cryogenic matrixes. On the basis of the infrared spectra and density functional theory calculations, the SO ligand is bound to the metal center in a sideon fashion, and both complexes possess closed shell singlet ground states. The experimental S−O stretching frequencies of OMoF 2 (η 2 -SO) and OWF 2 (η 2 -SO) are much lower than those of SO − but close to that of singlet SO 2− , indicating that the SO ligand should be considered as SO 2− . This is consistent with the rather long S−O bond length in comparison to that of the ONbF 2 (η 2 -SO) and OTaF 2 (η 2 -SO) complexes with SO − ligand. Bonding analysis results reveal that the π* (3π) orbitals of the triplet SO molecule are both doubly occupied in OMoF 2 (η 2 -SO) and OWF 2 (η 2 -SO) due to the two-electron transfer from metal to SO. End-on isomers with M−OS or M−SO geometries were also predicted to be stable, but all of them are higher in energy than the side-on complexes, and the calculated frequencies are inconsistent with the experimental values. Comparisons in bond lengths, vibrational frequencies, and natural charges between the OMF 2 (η 2 -SO) and OMF 2 (η 2 -O 2 ) complexes (M = Mo, W, Nb, Ta) further confirm the peroxo-like character of the SO ligand in OMoF 2 (η 2 -SO) and OWF 2 (η 2 -SO).
“…The 1007.7, 755.3, 686.3, and 669.9 cm −1 absorptions exhibit identical behaviors upon sample annealing and UV−vis irradiation, indicating they should belong to different vibrational modes of the same product. The 1007.7 cm −1 band shifted to 958.9 cm −1 upon 18 O substitution with an 16 O/ 18 O frequency ratio of 1.0509, suggesting that it should be a terminal Mo−O stretch in comparison to the values of the same mode of OMoF 2 (1007.6 cm −1 and 1.0505). 40 This assignment is further confirmed by the zero shift when the 34 SO 2 F 2 sample was used.…”
Section: Methodsmentioning
confidence: 96%
“…14 The side-on (η 2 -SO) coordination fashion was corroborated for the group 4 and 5 metal complexes, 15,16 and the group 5 metal complexes can be considered as (OMF 2 ) + (SO) − based on the S−O stretching vibrational frequency and bond length. 16 The existence of SO − in the SO complexes of group 5 metals raises the question of whether SO can be further reduced upon coordination to transition metals with richer electrons, since O 2 , which is isoelectronic to SO, 6,17,18 undergoes stepwise activation to form superoxo and peroxo complexes upon coordination to metal centers. 19−21 There has been a comparison focusing on the Fe−SO 2− and Fe−O 2 2− intermediates from the theoretical point of view, 22 but experimental evidence that clearly demonstrates the existence of a peroxo-like sulfur monoxide (SO 2− ) complex of transition metal is limited.…”
Peroxo-like sulfur monoxide complexes of molybdenum and tungsten oxyfluorides [OMF 2 (η 2 -SO)] were prepared via the reactions of molybdenum and tungsten atoms and SO 2 F 2 in cryogenic matrixes. On the basis of the infrared spectra and density functional theory calculations, the SO ligand is bound to the metal center in a sideon fashion, and both complexes possess closed shell singlet ground states. The experimental S−O stretching frequencies of OMoF 2 (η 2 -SO) and OWF 2 (η 2 -SO) are much lower than those of SO − but close to that of singlet SO 2− , indicating that the SO ligand should be considered as SO 2− . This is consistent with the rather long S−O bond length in comparison to that of the ONbF 2 (η 2 -SO) and OTaF 2 (η 2 -SO) complexes with SO − ligand. Bonding analysis results reveal that the π* (3π) orbitals of the triplet SO molecule are both doubly occupied in OMoF 2 (η 2 -SO) and OWF 2 (η 2 -SO) due to the two-electron transfer from metal to SO. End-on isomers with M−OS or M−SO geometries were also predicted to be stable, but all of them are higher in energy than the side-on complexes, and the calculated frequencies are inconsistent with the experimental values. Comparisons in bond lengths, vibrational frequencies, and natural charges between the OMF 2 (η 2 -SO) and OMF 2 (η 2 -O 2 ) complexes (M = Mo, W, Nb, Ta) further confirm the peroxo-like character of the SO ligand in OMoF 2 (η 2 -SO) and OWF 2 (η 2 -SO).
“…Sulfur monoxide and its dimer S 2 O 2 are of great interest to astrophysics since they are abundant in the Venusian atmosphere [14]. SO is isovalence-electronic to O 2 with a triplet ground state and features a S-O bond length of 1.481 Å indicating double-bond character [80]. Sulfur monoxide is formed from SO 2 under microwave discharge and by oxidation of elemental sulfur [80,81].…”
Section: Sulfur Monoxidementioning
confidence: 99%
“…SO is isovalence-electronic to O 2 with a triplet ground state and features a S-O bond length of 1.481 Å indicating double-bond character [80]. Sulfur monoxide is formed from SO 2 under microwave discharge and by oxidation of elemental sulfur [80,81]. Both SO and S 2 O 2 are unstable—disproportionation of SO leads to the formation of S and SO 2 [80].…”
Section: Sulfur Monoxidementioning
confidence: 99%
“…Sulfur monoxide is formed from SO 2 under microwave discharge and by oxidation of elemental sulfur [80,81]. Both SO and S 2 O 2 are unstable—disproportionation of SO leads to the formation of S and SO 2 [80]. Two 3 SO produce two S 2 O 2 isomers OSSO or SOSO, which both have a cis and a trans conformers.…”
Oxidation of sulfide to sulfate is known to consist of several steps. Key intermediates in this process are the so-called small oxoacids of sulfur (SOS)—sulfenic HSOH (hydrogen thioperoxide, oxadisulfane, or sulfur hydride hydroxide) and sulfoxylic S(OH)2 acids. Sulfur monoxide can be considered as a dehydrated form of sulfoxylic acid. Although all of these species play an important role in atmospheric chemistry and in organic synthesis, and are also invoked in biochemical processes, they are quite unstable compounds so much so that their physical and chemical properties are still subject to intense studies. It is well-established that sulfoxylic acid has very strong reducing properties, while sulfenic acid is capable of both oxidizing and reducing various substrates. Here, in this review, the mechanisms of sulfide oxidation as well as data on the structure and reactivity of small sulfur-containing oxoacids, sulfur monoxide, and its precursors are discussed.
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