Discussed and described are several types of chemical bonds: (1) ionic bonds; (2) covalent bonds; (3) hydrogen bonds; (4) bonds in the solid state; and (5) variation in bond strengths. (RH)

Discusses the vibrations of a linear triatomic chain and shows that the addition of the third atom gives rise to an extra optical branch. The nature of the normal modes in ionic crystals and molecular crystals is also discussed. (GA)

Describes the use of balloons to show the shape of atomic orbitals and their orientation in molecules. (MLH)

Describes the use of rubber hand-stamps to generate molecular pictures. These stamps (prepared with shapes of atoms and molecules at little cost by small, local print shops) can be used in creating pictures representing the microscopic state that can be linked to macroscopic descriptions for active conceptual exploration. (JN)

Surveyed are the etymology and the reason scientists coined a specific name for a newly discovered element. Approaches to naming from a historical viewpoint are considered. (CW)

Describes how the color of an object is related to its chemical structure. (CP)

Discusses evidence for the tetrahedral configuration of the carbon atom, indicating that three symmetrical configurations are theoretically possible for coordination number four. Includes table indicating that resolvability of compounds of type CR'R"R"'R"" is a necessary but not sufficient condition for proving tetrahedral…

Describes a 12 hour minicourse in Huckel molecular orbital (HMO) theory presented as part of a senior level chemical bonding course. (SL)

Discussed is the fundamental role that the favorable free energy of binding of the rate-determining transition state plays in catalysis. The principle that all of the catalytic factors discussed are realized by the use of this binding energy is reviewed. (CW)

Discussed are the molecular electronic terms which can arise from a given electronic configuration. Considered are simple cases, molecular states, direct products, closed shells, and open shells. Two examples are provided. (CW)

Discusses the energy levels of 3d and 4s electrons. (SL)

Discusses the use of orbital shapes for instructional purposes, emphasizing that differences between polar, contour, and three-dimensional plots must be made clear to students or misconceptions will occur. Also presents three-dimensional contour surfaces for the seven 4f atomic orbitals of hydrogen and discusses their computer generation. (JN)

Discusses major events leading to the development of the octet rule. Three conclusions based on the work of Mendeleev, Abegg, Thompson, Kossel, Lewis, and Langmuir are considered as is the debate over the rule's validity. (JN)

Discusses the measurement of electrons ejected from a system which is being irradiated with X-rays or ultraviolet photons, and a theoretical model for calculating core-electron ionization energies. (MLH)

Describes the use of magnets to simulate s, p, and d atomic orbitals from which a wide variety of molecular orbitals can be derived. The technique gives students an idea of molecular orbitals' shapes and stresses the importance of symmetry labels. (MLH)