In the liquid and solid states, molecules are held together by attractions called intermolecular forces. there are several types
of intermolecular forces. london dispersion forces, found in all substances, result from the motion of electrons. these work to attract both polar and nonpolar molecules to one another via instantaneous dipole moments. dipole-dipole forces arise from molecular dipole moments. ion-dipole forces result from the interaction of an ion and a molecular dipole. hydrogen-bond forces result from the attraction of a hydrogen atom bonded to a small highly electronegative atom (n, o, and f) and the unshared electron pairs of another electronegative atom physical properties such as boiling point, melting point, vapor pressure, viscosity, and surface tension are all affected by the strength of the intermolecular forces within a substance. part a what happens to these physical properties as the strength of intermolecular forces increases?
<span>Since these molecules are all non-polar, the only intermolecular force of attraction will be London dispersion forces. Since these increase by the size of the molecule, the boiling points will decrease in the same order:
Parafin > Heptadecane > hexane > 2,2-dimethylbutane > propane
For these two, hexane > 2,2-dimethylbutane, dispersion forces are greater in a molecule which is longer and unbranched compared to one which is branched and more compact.</span>
I think that different liquids have different freezing points because every liquid consists of different atoms and different things that make up the atom causing them to have different freezing points.
