![]() ![]() It will dissolve other polar molecules easily due to the dipole-dipole interactions.ĭipole-Dipole interactions are not as strong as hydrogen bonds due to the lower electronegativity of the atoms involved, but stronger than London dispersion forces.ĭon’t be fooled by molecules however that are not polar. ![]() ![]() It also allows water to act as a polar solvent. The dipole-dipole attractions between water molecules give water many of its properties, including its high surface tension. Water is another example of a polar molecule (oxygen is more electronegative than hydrogen). The interaction between the two dipoles is an attraction rather than full bond because no electrons are shared between the two molecules. When two of these molecules align (see below), the opposite partial charges attract to one another in a weak intermolecular attraction, known as an electrostatic interaction. This created an uneven distribution of electrons, giving chlorine a slightly negative charge (δ-) and hydrogen a slightly positive charge (δ+). This is because there is a difference in electronegativity between H and Cl: Chlorine is more electronegative than hydrogen and pulls the electrons in the covalent bond towards itself. For example, a molecule of hydrogen chloride, HCl has a large permanent dipole. Molecules that contain dipoles are called polar molecules. Dipole–dipole interactions are a type of intermolecular force that exists when molecules with permanent dipoles align forming an electrostatic interaction. ![]()
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