CHEM 1312 1st Edition Lecture 2Outline of Last Lecture I. Understanding physical properties of solutionsII. Recognizing the seven different types of solutionsIII. Classifying solutions according to solubilityIV. Brief introduction to solution concentration units (Molarity and Molality)Outline of Current LectureI. Review intermolecular forcesII. Understanding enthalpy changes in solvationIII. EntropyCurrent LectureUnderstanding three specific types of intermolecular forces is critical in developing an understanding of solutions:- Ion-dipole – Charged ion experiences attraction towards the partial charge on a polar molecule- Dipole-induced dipole – The partial charge on a polar molecule causes a temporary partial charge on a nonpolar molecule when in close proximity- Ion-induced dipole – The charge on an ion causes a temporary partial charge on a nonpolar molecule when in close proximityEnthalpy changes in the solvation process:1) Solute molecules break apart from one anothera. dH> 0: Endothermic2) Solvent molecules separate from one anothera. dH> 0: Endothermic3) Solute and solvent molecules mix with one anothera. dH< 0: ExothermicThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.The overall heat of solution can be determine by combining the separate enthalpy changes. If dHsolution is less than 0 than the overall heat of solution is exothermic, and endothermic when dHsolution is greater than 0.Entropy is a measure of disorder in a system. According to the 2nd Law of Thermodynamics, the total entropy of the universe is constantly increasing.- Endothermic solutions cause an increase in the overall