Been looking all across the internet but there doesn’t seem to be a straight answer (used a few chat bots too). CH3CN has the higher potential for making bonds with 2 addition dipole bonds on C and 3 possible H-bond on N but it has a smaller BP than CH3OCH3 even though it can only make an additional 2 H-bonds. Why though when the size of atoms and length of bonds are similar? Shouldn’t the more possible H-bond make it stronger?
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Dimethyl ether has a lower boiling point than CH3CN, no? It has to do with the polarity but mainly the intermolecular forces. The acetonitriles triple bond with the nitrogen makes it take a lot more energy than breaking up the dimethyl ether which has weak van der waals forces and can’t form hydrogen bonds with electronegative atoms like O, N , or F- oxygen in this case since the hydrogen is already bonded with the carbon
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