It has C 2v structure (planar).ĭisulfur monoxide (S 2O) is an analogue of sulfur dioxide. Disulfur dioxide (S 2O 2) is a dimer of sulfur monoxide. Sulfur monoxide (SO) and its dimer (S 2O 2) have been trapped at low temperature. At a few millibars pressure, the relative stabilities are S 2O > S 2O 2 > SO. Instead, when condensed, they undergo dimerization and oligomerization, usually yielding sulfur dioxide and elemental sulfur. These species are well characterized in the gas phase, but they cannot be isolated as solids or liquids. Sulfur monoxide, disulfur dioxide, disulfur monoxide Some compounds reported by early workers such as the blue "sesquioxide", S 2O 3, formed by dissolving sulfur in liquid SO 3 appears to be a mixture of polysulfate salts of the S 4 2+ and S 8 2+ ions. Interest in the lower sulfur oxides has increased because of the need to understand terrestrial atmospheric sulfur pollution and the finding that the extraterrestrial atmospheres of Io, one of Jupiter's moons, and Venus contain significant amounts of sulfur oxides. Some well characterized examples include sulfur monoxide (SO), its dimer S 2O 2, and a series of cyclic sulfur oxides, S nO x (x = 1, 2), based on cyclic S n rings. They are significant intermediates in the combustion of elemental sulfur. These species are often unstable and thus rarely encountered in everyday life. The lower sulfur oxides are a group of inorganic compounds with the formula S mO n, where 2m > n. Structure of S 2O Space-filling model of S 2O
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