The title is video link (where available). PDF file is below the description.
- Balancing a Redox Equation – MnO4-NO2 – Reduce pink MnO4– with NO2– in aqueous solution to produce colorless Mn2+.
- Chemical Traffic Light – Add NaOH, glucose, and indigo carmine to water in an Erlenmeyer flask. The solution starts green, and when the flask is open to the air, the solution gradually changes to red and then to yellow. Seal the flask and give it a light shake to turn the solution red, and give it a hard shake to turn it green. Repeatable! Shows how a reaction’s spontaneity and color change are driven by Gibbs Free Energy and oxidation-reduction cycling.
- Combustion of Candy – Contrast the oxidation of sucrose in the body (by eating some candy) with the oxidation of sucrose by KClO3 (as shown by dropping some candy into molten KClO3, producing steam and a lavender flame. Body temperature is ~37°C, and the melting point of KClO3 is 368°C.
- Copper Zinc voltaic cell – Demonstrate a copper/zinc voltaic cell turning a motor to show that a spontaneous reaction can be harnessed to do work.
- Electrolysis of Water – Electrolyze water (dilute Na2SO4 solution with indicator) in the Hoffman apparatus to decompose it into its component elements, hydrogen and oxygen. If desired, you can test the H2 (g) and/or O2 (g) produced with a flame and a glowing splint, respectively.
- Luminol – Pour solutions of luminol and H2O2 into a tall glass spiral to produce a beautiful chemiluminescent reaction. The light-emitting species is the dicarboxylate ion, aminophthalate, the product of the oxidation of luminol with H2O2
- Metal Redox Reactions – Choose from one of the following metal redox combinations:
- Fe in CuSO4 vs. Cu in FeSO4
- Zn in CuSO4 vs. Cu in ZnSO4
- Zn in Pb(NO3)2
- Copper Star Oxidation – Immerse copper wire in AgNO3 (aq). This is best done on the document camera over a lengthy period of time so students can observe the continuing reaction.
- Metal Redox Reactions.pdf
- Multiple Oxidation States of Manganese – Starting with KMnO4 (aq) in four beakers, carry out reactions to display manganese in the +7, +4, +3, and +2 oxidation states.
- Multiple Oxidation States of Vanadium – Shake a solution of ammonium meta-vanadate with a Zn-Hg amalgam to reduce the vanadium from +5 to +4 to +3 to +2 with different colors at each stage.
- Oxidation of Alcohols – Demonstrate the oxidation of ethanol with K2Cr2O7 on the overhead projector; the alcohol solution changes from orange to green to blue as the Cr(VI) is reduced; this reaction is the basis for the Breathalyzer test.
- Thionine Reaction – Hold a solution of thionine and FeSO4 in front of a bright light to show the reduction of thionine from a violet form to a colorless form; this is an endothermic reaction that absorbs light energy.
- Tollen’s Test– Create a silver coating inside a small Erlenmeyer flask using Tollen’s reagent and an aldehyde solution.
- Zinc and HCl – Immerse mossy zinc in HCl (aq) and use a lighted splint to ignite the hydrogen gas produced.