CHEM 211 1st Edition Lecture 6Outline of Last Lecture I. Surface TensionII. CapillarityIII. ViscosityIV. Properties of WaterV. The Unusual Density of Solid WaterVI. Structural Features of SolidsVII. Packing Efficiency and the Creation of Unit CellsVIII. Types and Properties of Crystalline SolidsIX. Bonding in Solids II: Band TheoryX. Conductivity of Solids and the Size of the Energy GapOutline of Current Lecture I. Solutions and ColloidsII. Solutions and SolubilityIII. Solutions and Intermolecular ForcesIV. Dual Polarity and Effects on SolubilityV. Heats of Solution and Solution CyclesVI. Heat of SolutionVII. Solvation and HydrationCurrent LectureI. Solutions and ColloidsA. A solution is a homogeneous mixture and exists as a single phase.a) The particles in a solution are individual atoms, ions, or small molecules.B. A colloid is a heterogeneous mixture and exists as two or more phases, which may be visibly distinct.These 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.b) The particles in a colloid are typically macromolecules or aggregations of small molecules.C. Colloidal suspension= light as haze, scatters light;Solution= no haze.II. Solutions and SolubilityD. A solute dissolves in a solvent to form a solution.E. Usually, the solvent is the most abundant component.F. The solubility (S) of a solute is the maximum amount that dissolves in a fixed quantity of solvent at a given temperature.G. Substances that exhibit similar types of intermolecular force dissolve in each other.c) This is often expressed by saying “like dissolves in like.”III. Solutions and Intermolecular ForcesA. When a solution forms, solute-solute attractions and solvent-solvent attractions are replaced by solute-solvent attractions.B. LIKE DISSOLVES LIKE:Substances with similar types of intermolecular forces dissolve in each other.C. This can only occur if the forces within the solute and solvent are similar to the forces that replace them.IV. Dual Polarity and Effects on SolubilityA. Alcohols are organic compounds that have dual polarity.d) The general formula for an alcohol is CH3(CH2)nOH.B. The –OH group of an alcohol is polar.e) It interacts with water through H bonds and with hexane through weak dipole-induced dipole forces.C. The hydrocarbon portion is nonpolar.f) It interacts through weak dipole-induced dipole forces with water and by dispersion forces with hexane.V. Heats of Solution and Solution CyclesD. Solute particles separate from each other – endothermic.g) solute (aggregated) + heat -------solute (separated) ∆Hsolute> 0E. Solvent particles separate from each other – endothermic.h) solvent (aggregated) + heat--------solvent (separated) ∆Hsolvent> 0F. Solute and solvent particles mix – exothermic.i) solute (separated) + solvent (separated)---------solution + heat ∆Hmix< 0∆Hsoln = ∆Hsolute + ∆Hsolvent + ∆HmixVI. Heat of Solution∆Hsoln = ∆Hsolute + ∆Hsolvent + ∆HmixG. Exothermic process: ∆Hsoln< 0 because the sum of the endothermic processes (∆Hsolute + ∆Hsolvent) is smaller than the exothermic term (∆Hmix).H. Endothermic process: ∆Hsoln> 0 because the sum of the endothermic processes (∆Hsolute + ∆Hsolvent) is larger than the exothermic term (∆Hmix).I. The overall solution process may be either exothermic or endothermic.VII. Solvation and HydrationA. Solvation is the process of surrounding a particle with solvent particles. In water, solvation is called hydration.∆Hsolvation = ∆Hsolvent + ∆Hmix; In water, ∆Hsoln = ∆Hsolute + ∆HhydrB. The hydration of an ion is always exothermic because ion-dipole forces are very strong.j) M+(g) [or X-(g)] → M+(aq) [or X-(aq)] ∆Hhydr of the ion (always <