CHEM 213: Physical Chemistry I

Atomic structure: A qualitative treatment of the Quantum Mechanical Model of the atom; quantum numbers; shape of orbitals. Electronic configuration of atoms; chemical periodicity;Models of chemical bonding: Review of ionic and covalent (including dative) bonds; polar bonds; van der Waals forces, hydrogen bonding; Valence Bond concepts – orbital overlaps; electron-pair sharing; sigma- and pi-bonds; Hybridization (as mathematical combination of atomic orbitals LCAO); sp, sp2, sp3, dsp2, sp3d2 hybridized orbitals and the resulting molecular shapes; Resonance and canonical structures; Valence bond description of simple molecules;
VSEPR: Qualitative Molecular Orbital model (homogeneous and heterogeneous diatomic molecules only).;Chemical Reactions and equilibrium: Enthalphy, exothermic and endothermic reactions; heat capacities Cp, Cv. Born-Haber cycle (Hess’ law); Bond energies, standard enthalpies of formation; effect of temperature on enthalpy changes; Simple ideas on Entropy; entropy as a driving force; (No calculations on entropy). Gibbs Free Energy and spontaneity, standard free energies. Relationship between free energy, enthalpy and entropy. Kinetics: differential rate law, rate constants, order of reactions, effects of concentration, temperature (Arrhenius equation); mechanical slope method (No integrated rate laws); concept of reaction mechanism.