Flat, symmetrical molecules can be modeled by folding a sheet of paper, cutting patterns into the folded structure, and unfolding to produce the flat paper models. The finished models resemble paper snowflakes, but have a variety of rotational symmetries. Template patterns for several molecules are available for download in the Supporting Information.
Beautiful, metallic mirrors of copper or silver can easily be formed in test tubes. Simply add the appropriate metal salt to a test tube, and heat! These reactions should be performed in a fume hood.
Learn how to form a blue-green copper compound on a penny, and then use that compound to make green flames. This is a great summer time activity for your next campfire!
Solutions of copper (II) dissolved in acetone are easy to prepare, and can display orange, yellow, green, and blue color depending upon conditions. Such solutions allow for a variety of demonstrations and experiments that illustrate principles of chemical equilibrium.
Erica Jacobsen shares highlights from the September 2019 issue of the Journal of Chemical Education of special interest to our ChemEd X community.
Simple chemical tests are described that can indicate the presence of certain metals in coins. A wide variety of chemical concepts are involved. The experiments described are a natural fit for the 2019 National Chemistry Week theme of "Marvelous Metals!"
A description of a quick and easy lesson that is sure to add some spark into your next lesson on stoichiometry.
The June 2015 issue of the Journal of Chemical Education is now available online to subscribers at http://pubs.acs.org/toc/jceda8/92/6. This issue includes articles on curriculum; assessment; inorganic chemistry; investigating galvanic cells & exploring LEDs; atomic structure; nanochemistry laboratories; physical chemistry in the lab; synthesis.
A good inquiry activity is an engaging way to begin a new semester.
In this Activity, students first prepare a gel using the superabsorbent polymer sodium polyacrylate (found in certain diapers) and water. The gel is split into piles and samples of different compounds are sprinkled on the piles. Students determine that ionic compounds break down the gel, while covalent compounds have no effect on the gel.