The number of flies that crawl through a small hole from one chamber to another is used to demonstrate principles of chemical kinetics. (CP)

Describes an approach for making chemistry relevant to everyday life. Involves the study of kinetics using the decomposition of hydrogen peroxide by vegetable juices. Allows students to design and carry out experiments and then draw conclusions from their results. (JRH)

Three chemistry demonstrations are described: (1) partition coefficients; (2) Rutherford simulation experiment; and (3) demonstration of the powerful oxidizing property of dimanganeseheptoxide. Background information, materials needed, and procedures are provided for each demonstration. (JN)

Discusses an attempt to have students learn chemistry by conducting and discussing laboratory experiments in small groups largely independent of the teacher. The project results and the 30 experiments that student groups conducted are described. (WB)

Changes, reactions, deductions. Five simple experiments add new skills and excitement to science. (Editor)

Describes an approach that challenges students to construct illustrations of chemical reactions by using colorful Bingo card paint markers. Enables them to visually demonstrate their understanding of chemical notations and the law of conservation of mass. Also discusses teaching chemical formulas, a modeling lab, illustrating chemical reactions,…

Modifies a laboratory activity to ensure that consistencies exist between the laboratory objectives and the teacher's instructional goals (the constructivist learning theory). The changes are included in the article as well as a rationale for each change. (ZWH)

Describes an Introduction to Chemical Engineering course with particular reference to the development, use, and evaluation of four simple experiments centered around the fundamental principles of heat transfer, mass transfer, reaction kinetics, and momentum transfer. (WRM)

Discusses the formation of lipid peroxides as important degradative biomolecules. (SL)

Presents a laboratory exercise that illustrates stoichiometry, limiting reagents, and proportionality. Highlights the safety and low cost factors of this exercise. Outlines procedures for the students. (ML)

Describes fluorescence demonstrations related to several aspects of molecular theory and quantitized energy levels. Demonstrations use fluorescent chemical solutions having luminescence properties spanning the visible spectrum. Also describes a demonstration of spontaneous combustion of familiar substances in chlorine. (JN)

Reports a method of preparation for tris(ethylenediamine)cobalt(III) and tris(2,2'-bipyridine)cobalt(III) that will shorten the preparation time by approximately 3 hours. Notes the time for synthesis and isolation of compound one was 1 hour (yield 38 percent) while compound two took 50 minutes (yield 71%). (MVL)

Describes an experiment where the gram-equivalent mass of an unknown metal is determined by reacting the metal with dilute hydrochloric acid and collecting the evolved gas over water. This simple, reliable experiment routinely gives results within 1% of the accepted value. (PR)

Background information, laboratory procedures, and a discussion of the results of an experiment designed to investigate the difference in energy gained from the aerobic and anaerobic oxidation of glucose are presented. Sample experimental and calculated data are included. (CW)

Suggests ways to avoid some of the problems students have learning the principles of organometallic chemistry. Provides a description of an experiment used in a third-year college chemistry laboratory on molybdenum. (TW)