CHEM 211 1st Edition Lecture 4Outline of Last 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 momentOutline of Current Lecture I. The Hydrogen BondII. Polarizability and Induced DipolesIII. Dispersion (London) ForcesIV. Molecular shape, Intermolecular Contact, and Boiling PointCurrent LectureI. The Hydrogen BondA. Hydrogen bonding is possible for molecules that have a hydrogen atom covalently bonded to a small, highly electronegative atom with lone electron pairs, specifically N, O,or F.B. An intermolecular hydrogen bond is the attraction between the H atom of one molecule and a lone pair of the N, O, or F atom of another molecule.II. Polarizability and Induced DipolesA. A nearby electric field can induce a distortion in the electron cloud of an atom, ion, or molecule.a) For a nonpolar molecule, this induces a temporary dipole moment.b) For a polar molecule, the field enhances the existing dipole moment.B. The polarizability of a particle is the ease with which its electron cloud is distorted.C. Smaller particles are less polarizable than larger ones because their electrons are held more tightly.D. Polarizability increases down a group because atomic size increases and larger electron clouds distort more easily.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.E. Polarizability decreases across a period because of increasing Zef (efective nuclear charge).F. Cations are smaller than their parent atoms and less polarizable; anions show the opposite trend.G. Polarizability correlates closely with molar mass for similar particles.III. Dispersion (London) ForcesA. Dispersion forces or London forces arises when an instantaneous dipole in one particle induces a dipole in another, resulting in an attraction between them.B. Dispersion forces exist between all particles, increasing the energy of attraction in all matter.C. Dispersion forces are stronger for more polarizable particles. D. In general, larger particles experience stronger dispersion forces than smaller ones.E. When atoms are far apart they do not influence one other.F. When atoms are close together, the instantaneous dipole in one atom induces a dipole in the other.a) The process occurs throughout the sample.IV. Molecular shape, Intermolecular Contact, and Boiling PointA. In a more rectangular molecule there are more points at which dispersion forces act.B. In a rounder molecule there are fewer points at which dispersion forces