Unit #3: IMF's

dipole-dipole forces

The attractions between oppositely charged regions of polar molecules

London dispersion forces

The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

hydrogen bonding

A strong type of intermolecular dipole-dipole attraction; Occurs between a hydrogen atom and F, O or N of another atom

ion-dipole forces

The attractive forces between an ion and a polar molecule

induced dipole forces

A weak attraction that results when a polar molecule creates a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of electrons in the nonpolar substance

intermolecular forces

The forces of attraction between molecules

polarity

A lack of electrical symmetry in a molecule; An uneven distribution of charge (electrons) in a molecule

coordinate covalent bond

Forms when one atom donates both of the electrons to be shared with an atom or ion that needs two electrons to form a stable electron arrangement

network covalent bond

Atoms are held together in a lattice of covalent bonds; Composed of nonmetals and metalloids; hard solids; do not conduct electricity or dissolve; Examples: diamond, silicon

metalloid

An element that has physical and chemical properties of both metals and nonmetals; Examples: boron & silicon