If sulfur is directly below oxygen on the periodic table, why isn't SO the most common sulfur oxide? Instead of third, behind SO2 and SO3? [closed]








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Chalcogen like oxygen and sulfur want to 'grab' (or share) two electrons to get to eight, if possible, or maybe 'give up' (or share) six, if necessary, to again get to eight... Right?


So, why is sulfur dioxide, where the sulfur shares four electrons (usually), more common than sulfur monoxide or sulfur trioxide?


Isn't sulfur dioxide a higher energy, less stable molecule?




Nobody really knows why $\ce{SO}$ is such a rare and unstable substance. It is an orange gas at room temperature. The only way to synthesize $\ce{SO}$ is to reduce thionyl chloride $\ce{SOCl2}$ with some reagent eager to react with the chlorine atom, like sodium, silver or tin : $$\ce{SOCl2 + 2 Na -> SO + 2 NaCl}$$ The strangest property of this gas is its reaction with water. It is decomposed with the smallest amount of water vapor according to the disproportion equation : $$\ce{3SO + H2O -> H2S + 2 SO2}$$ It is an extraordinary reaction, as it requires $3$ molecules $\ce{SO}$. Another oxide is known to disproportionate with water : $\ce{NO2}$. But there is a good reason for this behavior : $\ce{NO2}$ has an uneven number of electrons. It is not the case for $\ce{SO}$.


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