Hydrogen bonding occurs when hydrogen is bonded to a very small, highly electronegative atom (nitrogen, oxygen or fluorine). The δ+ hydrogen atom is attracted to a lone pair on an N, O or F atom of a neighbouring molecule.Hydrogen bonding is only significant when hydrogen is bonded to nitrogen, oxygen or fluorine.Hydrogen bonds are not always the strongest of all intermolecular attractions. This is true for water but not true for the majority of molecules.E.g. methanol vs pentanol - as the chain length increases the hydrogen bonding becomes less significant.The strength of hydrogen bonds: H-F > H-O > H-N
The most important example is hydrogen bonding in water. There is some partial bond formation utilising the lone pair on the oxygen. Like covalent bonds hydrogen bonds are directional. The bond angle is close to 180 °.
The most important example is hydrogen bonding in water. There is some partial bond formation utilising the lone pair on the oxygen. Like covalent bonds hydrogen bonds are directional. The bond angle is close to 180 °.