In lesson one of this program, experiments are conducted on five white "mystery" powders to determine chemical content and reaction. Salt is fused into a solid block. By feeding gaseous oxygen into a plastic bag of liquid nitrogen, we observe the resulting changes in gases; argon condenses into liquid, then turns to gas upon being removed from liquid nitrogen. Lesson two shows the three states of bromine. Mercury is evaporated and a match is lit using only steam. In lesson three, the density of solids and liquids is examined. Gas densities of copper sulfate solutions, liquid paraffin, carbon tetrachloride, and dyed propanol are illustrated by layering each substance in a graduated cylinder. The gas density of a soap bubble is tested with and without hydrogen; various gas densities are tested to float a hot air balloon.
In lesson one, heat is used to distill ethanol. Iodine distilled from seaweed demonstrates the chemical phenomenon of sublimation. The principle of chromatography is explored by studying color pigments in water-base pens. Lesson two studies salt dissolution. Degrees of solubility are measured by dissolving quantities of boric acid at different temperatures. Recrystallization is achieved. In lesson three, bleach and pig’s liver are combined to produce oxygen; carbon dioxide, ammonia, and hydrogen are produced and their properties are studied.
Lesson one looks at copper atoms using a Scanning Tunnelling Microscope connected to a computer. Several demonstrations of combustion include burning firecrackers under water. Lesson two shows combustion of an industrial diamond. Thermite reaction produces iron metal from iron oxide. Tatara, the traditional Japanese steelmaking process, is described. Lesson three studies chemical reactions between iron powder and sulfur, zinc and sulfur, and copper and sulfur. Chemical combination and decomposition, dry distillation, and pyrolysis are discussed.
Lesson one demonstrates the circumstances under which common materials, such as sugar and table salt, conduct electricity. The process of electrolysis is demonstrated in the making of metallic leaves. In investigating the movement of ions, permanganate ions spread toward the anode side of a liquid chamber when electricity is applied. Lesson two demonstrates the formation of a metallic copper crystal tree, and silver crystals are formed when copper wire is immersed in aqueous sulfur nitrate. Lead iodide is formed by heating a mixture of potassium iodide and lead nitrate solutions. In lesson three, chemical batteries are made of copper, zinc, a grapefruit, and an eggplant. Fuel cells generate pollution-free electricity.
The first lesson provides examples of the Law of Conservation and Mass and the Law of Definite Proportions. Recycling of elements is examined. In lesson two, exothermic and endothermic reactions are demonstrated by an experiment that uses the chemical contents of a pocket warmer and dry ice. The third lesson includes demonstrations of oscillating reactions and clock reactions, as well as interesting though hazardous experiments such as a hydrogen explosion, acetone peroxide explosion, surface polymerization, and silver mirror reaction.
In the first lesson, five aqueous solutions are tested for degrees of acidity and alkalinity. The nature of acids and bases is examined. In lesson two, table salt is produced by mixing small pieces of aluminum with solutions of hydrochloric acid and sodium hydroxide. Current flow in acid, neutral, and alkaline solutions is demonstrated. An experiment using ammonia water and dry ice tests varying degrees of acidity. An on-site visit to a neutralization plant in Japan shows how acid levels are reduced by putting quantities of limestone into the Yukawa River. A third lesson demonstrates precautions that should be taken when performing experiments involving heat. Investigations that use chemicals such as chlorine bleach, ether, and metallic sodium, which should not be attempted in a school lab, are also demonstrated.