Hydrogen bonding is a special case of bonding which involves hydrogen atom and a strong electronegative atom (such as oxygen, fluorine, nitrogen, etc.). Since hydrogen acquires a relatively strong partial positive charge when it bonds with an electronegative atom, such a bond represents a special case of dipole-dipole interactions. Another way to think about the reason behind the dipole-dipole interactions is the strong pull on the covalently bonded electron pair that is exerted by the electronegative atom.
If the hydrogen bonding takes place between the atoms of the same molecule (that is hydrogen bonding within a molecule), such a hydrogen bonding is known as intramolecular hydrogen bonding. An example is the hydrogen bonding between the hydroxyl groups of ethylene glycol.
If the hydrogen bonding takes place between two different molecules, it is known as intermolecular hydrogen bonding. An example is the hydrogen bonding between ammonia and water (between a hydrogen from water and nitrogen from ammonia).
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