CHEM 211 1st Edition Lecture 3Outline of Last Lecture I. Liquid-Gas Equilibrium.II. Factors affecting Vapor PressureIII. The Clausius-Clapeyron EquationIV. Vapor Pressure and Boiling PointOutline of Current Lecture I. Phase diagram for CO2 and H2OII. The Nature of Intermolecular ForcesIII. Covalent and Van der Waals radiiIV. Comparison of Bonding and Nonbonding (Intermolecular) ForcesV. Polar molecules, dipole-dipole forces, dipole momentCurrent LectureI. Phase diagram for CO2 and H2OA. At the critical point, the densities of the liquid and gas phasesbecome equal. >>B. At the triple point, all three phases are in equilibrium.C. The solid-liquid line slants to the left for H2O, because thesolid is less dense than the liquid. Water expands on freezing.>>II. The Nature of Intermolecular ForcesA. Intermolecular forces arise from the attraction betweenmolecules with partial charges, or between ions andmolecules.B. Intermolecular forces are relatively weak compared tobonding forces because they involve smaller charges that arefarther apart.III. Covalent and Van der Waals radiiA. The van der Waals distance is the distance between two non-bonded atoms in adjacent molecules.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 van der Waals radius is one-half the closest distance between the nuclei of two non-bonded atoms. The VDW radius is always larger than the covalent radius.C. Increases down a group and increases right to leftIV. Comparison of Bonding and Nonbonding (Intermolecular) ForcesV. Polar molecules, dipole-dipole forces, dipole momentA. The positive pole of one polar molecule attracts the negative pole of another.B. Solid is in a pattern while liquid is more randomly
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