Are there hydrogen bonds in methanol

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Hydrogen bonding occurs when there is a significant amount of positive charge building up on a hydrogen atom. That happens because the hydrogen is attached to an atom that is much more electronegative than the hydrogen. As a result of that positive charge, a lone pair on another molecule strongly interacts with the hydrogen. Hydrogen bonds occur only when a hydrogen is attached to one of the few most electronegative elements in the periodic table: fluorine, oxygen or nitrogen.

It is these strong hydrogen bonds that are responsible for the relatively high boiling point of methanol; there is so much positive charge on the hydrogen of the OH group that it can essentially form a real bond with the lone pair on another methanol molecule. Water is an even better example of a hydrogen bonding compound; in fact, water molecules are so tightly bound to each other that this very small molecule freezes at 0 o C and does not boil until o C way, way hotter than an August day in Las Vegas.

Water molecules are much less able to move around freely than are ethane molecules, even though ethane molecules weigh almost twice as much. For practical purposes, hydrogen bonding usually involves compounds that contain N-H and O-H bonds. That's because oxygen and nitrogen are the second- and third-most electronegative elements in the periodic table, respectively.

Therefore, the hydrogen of the -OH group on the ethanol may hydrogen bond to an oxygen of a water molecule shown or to an oxygen of an alcohol not shown. Hydrogen Bonding.

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