Probe the connections between biology and metals with this lecture on some compounds and reactions in the field of organometallic chemistry. As you'll quickly learn, organometallics have a range of practical applications; one example you'll encounter is Dotarem, an organometallic compound used to help detect tumors in cancer patients.

Starting with hydrogen, see how electrons organize themselves within the atom, depending on their energy state. Graduate from Niels Bohr's revolutionary model of the atom to Erwin Schrödinger's even more precise theory. Then, chart different electron configurations in heavier and heavier atoms.

Complete your study of acids and bases by searching out the fundamental causes of their disparate behavior. For example, why is there a difference in the ease with which various acids ionize? Your search draws on concepts from previous lectures, including electronegativity, molecular geometry, hybridization, and covalent bonding.

Transition to the other side of the visible spectrum and discover how infrared spectroscopy provides chemists with different information about structures. In doing so, you'll come to see molecular structures in a new light: not as rigid constructs but as dynamic, vibrating frameworks with bonds that can stretch and bend.

Although light has wave-like properties, it also behaves like a particle that comes in discrete units of energy, termed quanta. Learn how physicists Max Planck, Albert Einstein, and others built a revolutionary picture of light that recognizes both its wave- and particle-like nature.

Begin your study of chemical reactions by investigating how chemists write reactions using a highly systematized code. Next, Professor Davis introduces the "big four" types of chemical reactions: synthesis, decomposition, single displacement, and double displacement. He also shows how to translate between measurements in moles and grams.

Apply the physics of moving bodies to the countless particles comprising a gas. Observe how Graham's law links the mass of gas particles to the rate at which they escape through a small aperture, a process known as effusion. See how this technique was used to enrich uranium for the first atomic weapons.

Certain properties of solutions depend only on the concentration of the solute particles dissolved, not on the nature of the particles. Called colligative properties, these involve such behaviors as lowering the freezing point, raising the boiling point, and osmotic pressure. Study examples of each.

Meet one of the fathers of modern physical chemistry, Linus Pauling. Hear about his theory of orbital hybridization, which solves some of the shortcomings of VSEPR theory by averaging the charge of electrons in different orbitals, accounting for the peculiar geometry of certain molecules.

In this final lecture on spectroscopic techniques, discover the importance of modern NMR spectrometers, which use superconducting magnets and radio receivers to collect spectra with more speed and precision (and in different ways) than other techniques. Also, get an intriguing lesson in the human element - and limitations - involved in spectroscopy.