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Dipole forces occur between polar molecules due to positive and negative charges on different sides. London dispersion forces are temporary and occur due to the probability of electron arrangements. Permanent dipole forces are dipole-dipole interactions and hydrogen bonds, which are stronger. Hydrogen bonds are important for water’s properties.
Dipole forces describe a form of interaction that can occur between molecules. Like magnets, molecules are often polar; they have positive and negative charges on different sides based on their molecular structure. The positive part of one molecule can attract the negative part of another, bringing them closer together. There are two different types of dipole forces; some are permanent and some last only for an instant. Both types have a significant impact on the interactions between molecules.
The momentary and instantaneous dipole forces are known as the London dispersion forces. The electrons in atoms are highly mobile and can line up in such a way that a temporary dipole or separation of positive and negative charges occurs. When this happens to multiple molecules at the same time, brief attractive or repulsive forces can occur. This process is based on the probability that the arrangement of electrons in a given atom or molecule exists in a specific way at a specific time. London dispersion forces, despite their relative rarity in individual atoms and molecules, are significant because the massive number of atoms or molecules typically present in any given substance almost guarantees that at least some of them will interact via instantaneous dipoles.
Permanent dipole forces are known as dipole-dipole interactions or Keesom interactions and exist between polar molecules. A molecule tends to have a permanent dipole when it is composed of atoms that have different electronegativity values. Electronegativity is a property of atoms or molecules that describes their ability to attract electrons to themselves and form bonds with other atoms or molecules. When atoms with different electronegativity values bond and form molecules, they tend to have different permanent charges on different parts of their structures. When molecules with permanent dipoles are close to other molecules with permanent dipoles, there are many strong attractive and repulsive interactions between the polar parts of the molecules.
Hydrogen bonds are a third type of intermolecular interaction caused by dipole forces and are another form of permanent dipole interaction. They can only occur between hydrogen and another atom, hence the name. The other atom can be oxygen, fluorine or nitrogen. Hydrogen bonds are essentially a stronger form of dipole-dipole interactions.
Hydrogen bonds are probably the most important of the different types of dipole forces due to their effects on water. Water molecules are very polar due to their arrangement of electrons and tend to exhibit a large amount of hydrogen bonding. Hydrogen atoms on a water molecule can interact with oxygen atoms on other water molecules. This degree of attraction gives water many of the properties necessary for its vital role in the earth’s environment, such as cohesion and a high boiling point. It takes a significant amount of energy to break through hydrogen bonds, which lends great stability in an environment consisting primarily of water.
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