Calculating the entropy change associated with a phase transition

Since phase transitions are reversible processes, the entropy change associated with them is the enthalpy of transition divided by the temperature of transition in Kelvin. This should fit into the idea that every bit of energy is being used to change the average intermolecular forces they experience at a fixed temperature. This means that phase transitions that are endothermic (melting, vaporization, and sublimation) will always have an increase in entropy, because the molecules are more able to move and spread out this new energy after the transition has taken place. Exothermic phase transitions (freezing, condensation, and sublimation) will always have a decrease in entropy because intermolecular forces start to "lock molecules" into place and there is less freedom of motion and ability to spread out energy.