The study of the structure of atoms and molecules begins with a historic survey that highlights the experiments that have led to our nowadays insight in quantum mechanics. Subsequently, the electronic structure of the hydrogen atom is described in some detail, followed by an expansion of the insight to include many-electron atoms. The study of the chemical bond begins with a description of the electronic structure of the hydrogen molecular ion. The subseqent chapters describe molecular orbitals for homonuclear diatomics, valence bond theory for larger molecules, VSEPR theory of molecular structure, and a separate chapter describes intermolecular interactions.
The physical chemistry part of the course begins with a treatment of the equations of state for ideal and non-ideal gases, after which the First, Second and Third Laws of thermodynamics are discussed. Applications of the First Law are described in a separate chapter. Next, the concepts of Gibbs and Helmholtz energies and of chemical potentials are introduced for closed systems, followed by an extended chapter on open systems, in which mainly isobaric physical and chemical equilibria are treated using Gibbs energies and chemical potentials. That introduction of physical chemistry ends with a discussion of a number of phase equilibria of importance to general chemistry.