Chemistry in a nutshell: The major concepts and ideas of chemical science, and a look at some of the major currents of modern Chemistry. We hope this will motivate you get through the less-fun stuff in the first-year course!
condensed states, liquids, types of solids, intermolecular forces, types of molecular units; hydrogen bonding and water; introduction to crystals, ionic solids, cubic and close-packed lattices. Liquids and interfacial effects. Changes of state: vapor pressure, boiling, and phase maps. Polymers and plastics.
Ten-part tutorial set on covalent bonding and polar covalence, shapes of molecules (VSEPR theory), hybrid orbitals, molecular orbitals applied to simple diatomics, introduction to transition metal d-orbital splitting and band theory of metals and semiconductors.
Covers the fundamental concepts of acids and bases. Except for some stoichiometry and a discussion on pH, this section is largely qualitative. Acid-base equilibrium calculations are covered in Unit 21.
This thorough treatment sets out the underlying concepts without invoking thermodynamics or complicated calculations; considerable emphasis is placed on the distinction between Q and K. The section on equilibrium calculations contains problem examples illustrating techniques such as iterative and graphical solutions of polynomials, all of which employ the "systematic" method of organizing information.
Acid-base chemistry can be extremely confusing, particularly when dealing with weak acids and bases. This set of lessons presents an updated view of the Brønsted-Lowry theory that makes it easy to understand answers to common questions: What's the fundamental difference between a strong acid and a weak acid? Can acid A neutralize base B? Why are some salts acidic and others alkaline? How do buffers work? What governs the shapes of titration curves?
This complete rewrite of the previous 1996 pdf document is now organized into seven lessons covering all aspects of the subject. Considerable effort has been expended to make most of this material accessible to those whose knowledge of thermodynamics is minimal, while still incorporating the proton-free energy concept that makes it easy to answer the questions posed in the preceding paragraph.
Much emphasis is placed on the practical aspects of calculations, including how to deal with quadratic equations and how to judge when approximations are appropriate. The commonly-taught algebraic method of solving acid-base problems hides the underlying principles and is able to deal with only the simplest systems. The use of log-C vs pH plots avoids the math, provides a bird's-eye view of what's going on in the solution, and yield useful results without algebra. Finally, there are separate lessons on practical applications (physiology, acid rain, and the geochemical carbonate system) and, for more advanced students, on exact numerical solutions.
All about entropy, free energy, and why chemical reactions do or don't take place. Energy spreading and spontaneous change • What is entropy? • The Second Law • Gibbs free energy • free energy and equilibrium • some applications of entropy and free energy
Chemistry and electricity • galvanic cells and electrodes • potential differences at interfaces • cell potentials and thermodynamics • Nernst equation and its applications • batteries and fuel cells • electrochemical corrosion • electrolytic cells and electrolysis
Rate of a reaction, rate laws • integrated rate laws, half-life• collision theory, activation energy and the Arrhenius equation • elementary processes, reaction mechanisms and chain reactions • kinetics of reactions in solution • catalysts and catalysis • experimental methods
The first three sections of this unit cover units and dimensions, measurement error and significant figures and are duplicated in an early first-semester unit. The last two sections, reliability of a measurement and drawing conclusions from data introduce simple statistics that are needed in analytical chemistry courses.
How to predict the directions of oxidation-reduction reactions while avoiding formal electrochemistry. Similar to Fall of the Proton unit 21c. Coverage of biological redox reactions makes this a useful supplement for biochemistry courses.
Provides an overview of "environmental chemistry" in its broadest context: the chemical evolution and constitution of the lithosphere, hydrosphere, atmosphere, and biosphere. This formed the background reading for the first two weeks of a third-year Environmental Chemistry course. Much of it is suitable for lower-level courses.
In contrast to the common but misleading "entropy is disorganization" line, this tutorial describes entropy as a measure of the spreading and sharing of thermal energy. This concept provides rational, non-mathematical explanations of the effects of temperature change on reaction equilibria and on the colligative properties of solutions.
Below: engraving by Bernard Picart (1673-1733) for an illustration to Fontenelle's Oevres Diverses (1729) depicting an alchemy laboratory with alembic at centre, and, at right, four putti gathered around a crucible; at left, putto carrying coal in a basket