![]() Hydrogen bonding is the strongest type of intermolecular bond. This type of intermolecular bond is stronger than London dispersion forces with the same number of electrons. Polar molecules display attractions between the oppositely charged ends of the molecules. Molecules with a permanent dipole are polar. Permanent dipole-permanent dipole interactions London dispersion forces increase the larger the atomic size. This leads to larger dipoles being established. Larger atoms and molecules have more electrons. The strength of London dispersion forces depends on the size of the molecule or atom. The opposite charges then attract each other. London dispersion forces are the electrostatic attractions set up between the slightly positive end of one atom/molecule and the slightly negative end of one atom/molecule. This temporary dipole can induce a temporary dipole on a neighbouring atom/molecule. This results in a slightly negative ( \(\delta-\) ) and slightly positive \((\delta )\) charge on either side of the atom. London dispersion forces are caused by an uneven distribution of electrons within an atom. This shows that there must be an attraction between the individual molecules (or atoms in the case of monatomic substances) that is being overcome. ![]() Molecular elements (oxygen, nitrogen etc) and monatomic elements (the noble gases) will condense (move closer together) forming solids if cooled to sufficiently low temperatures. They exist between all atoms and molecules. London dispersion forces are the weakest type of intermolecular bond. They are also known as Van der Waals forces, and there are several types to consider. Intermolecular bonds are found between molecules.
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