The same data as in Exercise E9B.3(a) may be used to calculate the molecular potential energy curve for the antibonding orbital, which is given by eqn 9B.7. Plot the curve.
Chemistry: August 22-September 2 Prerequisites to Review *Remember how to do Lewis Dot Structure *Review of Group Names on Period Table: 1A/1- Alkali Metals 2A/2- Alkali Earth Metals 6A/16- Chalcogens 7A/17- Halogens (Diatomic) 8A/18- Noble/Inert Gases *States at Room Temperature: Gas: Mg and Br Liquid: Fr, Cs, Gr, and Rb Solid- all others *Solubility: -Solute- what’s going into solvent; smaller number of moles -Solvent- dissolves solute; larger number of moles -Solubility- maximum amount of substance it can dissolve at a given volume -Miscible- liquids are mutually soluble in any proportion Chapter 6 Intermolecular Forces • Interactions between nonpolar molecules o Dispersion- momentary shift in electron density o Dispersion (London) forces- caused by presence of temporary dipoles in molecules (weakest bond) § Larger molecules usually solid, then liquid, then gas o Temporary (induced) dipole- separation of charge produced in atom or molecule by a temporary uneven distribution of electrons (middle strength) § May be caused by a reaction between a polar and nonpolar molecule o Polarizability- the ease that an electron cloud in a molecule, ion, or atom can be distorted, inducing a temporary dipole § Larger molecules/elements have higher polarizability because intermolecular forces are weaker Factors Affecting Strength of Dispersion: • Size of atom/molecule- larger are
