1.
Weakest intermolecular force, caused by temporary fluctuations in electron density. Present in all molecules, regardless of polarity.
2.
Attractive forces between polar molecules. The positive end of one molecule is attracted to the negative end of another.
3.
A special type of dipole-dipole force that occurs when a hydrogen atom bonded to a highly electronegative1 atom (N, O, or F) is attracted to a2 lone pair of electrons on another electronegative atom.
4.
A measure of the separation of charge within a molecule.
5.
The ease with which an electron cloud can be distorted, influencing the strength of dispersion forces.
6.
When a molecule has a net dipole moment, meaning it has a positive and negative end.
7.
When a molecule has no net dipole moment, meaning it has no significant charge separation.
8.
A measure of the polarity of a bond or molecule, calculated by multiplying the charge separation by the bond length.
9.
Force of attraction between oppositely charged particles. The amount of force between two charges is directly proportional to the product of the charges and inversely proportional to the square of the distance between them.
10.
A type of bonding that involves the transfer of electrons from one atom to another, resulting in the formation of ions and an electrostatic attraction between them.
11.
A type of bonding that involves the sharing of electron pairs between atoms.
12.
A type of bonding found in metals, where valence electrons are delocalized and shared among many atoms.
13.
A type of bonding where atoms are connected in a continuous pattern, resulting in giant molecules like diamond and silicon dioxide.
