TIGER

Journal Articles: 102 results
Oven versus Bunsen Burner When Heating Copper(II) Chloride Dihydrate  Michael C. Wirtz
In "greening up" the classical stoichiometry experiment where students determine the formula of copper(II) chloride dihydrate, it is critical that teachers and instructors use a 110°C oven rather than a Bunsen burner. Copper(II) chloride dihydrate decomposes at temperatures above 300°C, releasing chlorine gas.
Wirtz, Michael C. J. Chem. Educ. 2008, 85, 1345.
Laboratory Management |
Stoichiometry
Lewis Structure Representation of Free Radicals Similar to ClO  Warren Hirsch and Mark Kobrak
An unconventional Lewis structure is proposed to explain the properties of the free radical ClO and a series of its isoelectronic analogues, particularly trends in the spin density of these species.
Hirsch, Warren; Kobrak, Mark. J. Chem. Educ. 2007, 84, 1360.
Atmospheric Chemistry |
Computational Chemistry |
Covalent Bonding |
Free Radicals |
Lewis Structures |
Molecular Modeling |
MO Theory |
Valence Bond Theory
The Chemistry of Swimming Pool Maintenance  Carl Salter and David L. Langhus
This paper examines the key ideas behind swimming pool chemistry -- the central importance of pH and its effect on chlorine sanitation and calcium carbonate solubility. The paper also reviews the analytical procedures and common practices used to monitor and control pool chemistry or correct problems.
Salter, Carl; Langhus, David L. J. Chem. Educ. 2007, 84, 1124.
Acids / Bases |
Applications of Chemistry |
Aqueous Solution Chemistry |
Dyes / Pigments |
pH |
Photochemistry |
Precipitation / Solubility |
Water / Water Chemistry
Potassium Iodide  Jay A. Young
The hazards of potassium iodide are discussed.
Young, Jay A. J. Chem. Educ. 2006, 83, 1286.
Laboratory Management
Iodine  Jay A. Young
The hazards of iodine are discussed.
Young, Jay A. J. Chem. Educ. 2006, 83, 1285.
Laboratory Management |
Nonmetals
Methyl Iodide  Jay A. Young
The hazards of methyl iodide are discussed.
Young, Jay A. J. Chem. Educ. 2006, 83, 1284.
Laboratory Management
Ethyl Bromide  Jay A. Young
The hazards of ethyl bromide are discussed.
Young, Jay A. J. Chem. Educ. 2006, 83, 841.
Laboratory Management
Mass Relationships in a Chemical Reaction: Incorporating Additional Graphing Exercises into the Introductory Chemistry Laboratory  Stephen DeMeo
The purpose of this article is to increase student involvement with graph construction specifically in the context of introductory laboratory activities that involve mass relationships between reacting substances and products. In this regard, five massmass plots derived from a synthesis of a binary compound from its elements are presented as well as a set of questions to focus learners on the significance of each plot. The benefit of providing learners with these types of graphing activities include the use of higher-order cognitive processes as well as the elucidation of fundamental chemical knowledge such as the law of the conservation of mass, the law of constant composition, limiting and excess reactants, and empirical formula.
DeMeo, Stephen. J. Chem. Educ. 2005, 82, 1219.
Stoichiometry |
Oxidation / Reduction |
Reactions |
Quantitative Analysis
A Substitute for “Bromine in Carbon Tetrachloride”  Joshua M. Daley and Robert G. Landolt
Benzotrifluoride (BTF) is a suitable solvent substitute for carbon tetrachloride in experiments requiring application of bromine (Br2) in free radical or addition reactions with organic substrates. A 1 M solution of Br2 in BTF may be used to distinguish hydrocarbons based on the ease of abstraction of hydrogen atoms in thermally or light-induced free radical substitutions. Efficacy of minimization of solvent use, by aliquot addition to neat samples, has been established.
Daley, Joshua M.; Landolt, Robert G. J. Chem. Educ. 2005, 82, 120.
Alkenes |
Free Radicals |
Green Chemistry |
Qualitative Analysis |
Reactions
Carbon Tetrachloride  Jay A. Young
The hazards of carbon tetrachloride are discussed.
Young, Jay A. J. Chem. Educ. 2004, 81, 1416.
Laboratory Management |
Laboratory Equipment / Apparatus
Dichloromethane  Jay A. Young
The hazards of dichloromethane are discussed.
Young, Jay A. J. Chem. Educ. 2004, 81, 1415.
Laboratory Management |
Laboratory Equipment / Apparatus
Boiling Point versus Mass  Michael Laing
I am very pleased that Ronald Rich has written making these comments, because he is pre-eminent in this field, beginning with his early book, Periodic Correlations.
Laing, Michael. J. Chem. Educ. 2004, 81, 642.
Atomic Properties / Structure |
Molecular Properties / Structure |
Noncovalent Interactions |
Liquids |
Phases / Phase Transitions / Diagrams
Boiling Point versus Mass   Ronald L. Rich
Laing gave a useful examination of the boiling points of small molecules versus molecular mass. However, a molecule escaping from a liquid is not closely analogous to a satellite breaking free from the earths gravitational field with the requirement of a minimum escape velocity, such that the required kinetic energy is proportional to the mass of the satellite at that escape velocity.
Rich, Ronald L. J. Chem. Educ. 2004, 81, 642.
Molecular Properties / Structure |
Atomic Properties / Structure |
Liquids |
Noncovalent Interactions |
Phases / Phase Transitions / Diagrams
A Reaction That Takes Place in Beakers but Not in Conical Flasks: A Catalysis-Related Demonstration  Colin White
A striking demonstration emphasizing that substances which promote reactions are not catalysts if they are consumed in the process. The demonstration is based on the iron(II) induced oxidation of iodide by chromium(VI).
White, Colin. J. Chem. Educ. 2004, 81, 364.
Catalysis |
Oxidation / Reduction |
Reactions
Chlorine  Jay A. Young
Properties, hazards, and storage requirements for chlorine.
Young, Jay A. J. Chem. Educ. 2004, 81, 186.
Laboratory Equipment / Apparatus |
Laboratory Management |
Physical Properties
Colorful Iodine  Richard W. Ramette
Design for an iodine thermometer, demonstrating sublimation of iodine.
Ramette, Richard W. J. Chem. Educ. 2003, 80, 878.
Main-Group Elements |
Phases / Phase Transitions / Diagrams |
Applications of Chemistry
Uncle Tungsten  Martin E. Fuller
Design for an iodine thermometer, demonstrating sublimation of iodine.
Fuller, Martin E. J. Chem. Educ. 2003, 80, 878.
Main-Group Elements |
Phases / Phase Transitions / Diagrams |
Applications of Chemistry
Use of Chloroisocyanuarates for Disinfection of Water: Application of Miscellaneous General Chemistry Topics  Gabriel Pinto and Brian Rohrig
Using the chlorination of water (using sodium dichloroisocyanurate and trichloroisocyanuric acid) to develop general chemistry concepts; includes question for students and answers.
Pinto, Gabriel; Rohrig, Brian. J. Chem. Educ. 2003, 80, 41.
Stoichiometry |
Water / Water Chemistry |
Applications of Chemistry |
Photochemistry
Sodium Fluoride  Jay A. Young
Properties, hazards, and storage requirements for sodium fluoride.
Young, Jay A. J. Chem. Educ. 2002, 79, 1197.
Laboratory Management |
Physical Properties
Tick Tock, a Vitamin C Clock  Stephen W. Wright
Uses supermarket chemicals to perform a clock reaction; students vary the concentration of reactants and observe the effect on the time required for the reaction to reach its endpoint.
Wright, Stephen W. J. Chem. Educ. 2002, 79, 40A.
Consumer Chemistry |
Oxidation / Reduction |
Vitamins |
Equilibrium |
Mechanisms of Reactions
Chemical Demonstrations with Consumer Chemicals: The Black and White Reaction  Stephen W. Wright
Color change demonstration using supermarket materials (white vinegar, bleach, tincture of iodine, vitamin C, Epsom salt, ammonia, and liquid laundry starch).
Wright, Stephen W. J. Chem. Educ. 2002, 79, 44.
Consumer Chemistry |
Vitamins
The Vitamin C Clock Reaction  Stephen W. Wright
Clock reaction using supermarket materials (vitamin C, hydrogen peroxide, tincture of iodine, and starch).
Wright, Stephen W. J. Chem. Educ. 2002, 79, 41.
Consumer Chemistry |
Oxidation / Reduction |
Vitamins |
Carboxylic Acids
Boiling Points of the Family of Small Molecules CHwFxClyBrz: How Are They Related to Molecular Mass?  Michael Laing
Investigating the role of molecular mass in determining boiling points of small molecules.
Laing, Michael. J. Chem. Educ. 2001, 78, 1544.
Atomic Properties / Structure |
Noncovalent Interactions |
Liquids |
Molecular Properties / Structure |
Physical Properties
The Synthesis and Analysis of Copper(I) Iodide. A First-Year Laboratory Project  Lara A. Margolis, Richard W. Schaeffer, and Claude H. Yoder
This project provides a convenient preparation of a compound whose identity will not be obvious to students. The analytical procedures illustrate the fundamentals of gravimetric analysis and some basic chemical and physical characteristics of the elements. The analytical data allow students to find the identity of the product by determining its empirical formula.
Margolis, Lara A.; Schaeffer, Richard W.; Yoder, Claude H. J. Chem. Educ. 2001, 78, 235.
Synthesis |
Oxidation / Reduction |
Stoichiometry |
Gravimetric Analysis |
Qualitative Analysis |
Stoichiometry
Teaching about Flame Retardants. A Joint Israeli-Dutch Project  Miri Kesner and Wobbe de Vos
Flame retardants make interesting chemistry and moreover, the chemistry is highly relevant from an everyday life point of view. This article reports on a joint Israeli-Dutch project aimed at teaching the production, properties, and applications of some bromine-containing flame retardants, including their environmental aspects, in secondary education.
Kesner, Miri; de Vos, Wobbe. J. Chem. Educ. 2001, 78, 41.
Industrial Chemistry |
Oxidation / Reduction |
Reactions |
Applications of Chemistry
No, the Molecular Mass of Bromobenzene Is Not 157 amu: An Exercise in Mass Spectrometry and Isotopes for Early General Chemistry  Steven M. Schildcrout
Even with no background in bonding and structure, students can successfully interpret the output of a modern research instrument. They learn to identify an isotope pattern, assign chemical formulas to ions giving mass spectral peaks, calculate an average atomic weight (for bromine) from measured isotopic abundances, and write balanced equations for ion fragmentation reactions.
Schildcrout, Steven M. J. Chem. Educ. 2000, 77, 1433.
Isotopes |
Mass Spectrometry |
Atomic Properties / Structure |
Molecular Properties / Structure
Ionic Crystals: A Simple and Safe Lecture Demonstration of the Preparation of NaI from Its Elements  Zelek S. Herman
A simple and safe classroom demonstration showing the production of sodium iodide (NaI) crystals from elemental sodium and elemental (molecular) iodine is presented. The demonstration, which is quite impressive, naturally fits into the discussion of ionic bonding and the alkali halide crystals.
Herman, Zelek S. J. Chem. Educ. 2000, 77, 619.
Crystals / Crystallography |
Thermodynamics |
Ionic Bonding |
Crystals / Crystallography
Dioxin, Not Doomsday  Jeffrey M. Zimpleman
On the basis of findings from epidemiologic cohort studies, dioxin appears not to be as potent a carcinogen or teratogen as popularly thought. In fact, through its antiestrogenic properties, dioxin may provide a weapon against breast cancer.
Zimpleman, Jeffrey M. J. Chem. Educ. 1999, 76, 1662.
Toxicology
A Simple, Safe Way To Prepare Halogens and Study Their Visual Properties at a Technical Secondary School  Domingo A. Liprandi, Orlando R. Reinheimer, José F. Paredes, and Pablo C. L'Argentière
In this paper we propose an easy-to-build apparatus to obtain chlorine, bromine, and iodine. The experiment was developed considering not only theoretical and safety conditions but simplicity and clarity as well.
Liprandi, Domingo A.; Reinheimer, Orlando R.; Paredes, José F.; L'Argentière, Pablo C. J. Chem. Educ. 1999, 76, 532.
Oxidation / Reduction |
Aqueous Solution Chemistry
An Easy Way To Make Chlorine Water  L. H. Holmes Jr.
Chlorine water can be made easily by mixing hypochlorite and hydrochloric acid. The equilibrium lies toward Cl2 in the reaction HOCl + HCl -> Cl2 + H2O and this can be used to make chlorine water from sodium hypochlorite and hydrochloric acid if the presence of NaCl in the chlorine water does not interfere with its use.
Holmes Jr; L. H. J. Chem. Educ. 1997, 74, 1326.
Synthesis
Iodine Clock Reaction  Richard S. Mitchell
The study of kinetics using the iodine clock reaction has provided an interesting experience for students for many years.
Mitchell, Richard S. J. Chem. Educ. 1996, 73, 783.
Kinetics |
Laboratory Management
The Iodide-Catalyzed Decomposition of Hydrogen Peroxide: A Simple Computer-Interfaced Kinetics Experiment for General Chemistry  John C. Hansen
188. The reaction studied is the iodide-catalyzed decomposition of hydrogen peroxide. The rate of oxygen production is measured as a function of time using a computer-interfaced pressure transducer.
Hansen, John C. J. Chem. Educ. 1996, 73, 728.
Rate Law |
Kinetics |
Catalysis |
Oxidation / Reduction
The Helium-Neon Laser-Induced Fluorescence Spectrum of Molecular Iodine: An Undergraduate Laboratory Experiment  John S. Muenter
The wavelength analyzed fluorescence spectrum provides accurate values of spectroscopic properties for the ground state electronic configuration of I2. From these spectroscopic properties students calculate the bond length, harmonic oscillator force constant, and a Birge-Sponer estimate of the bond dissociation energy.
Muenter, John S. J. Chem. Educ. 1996, 73, 576.
Fluorescence Spectroscopy |
Molecular Properties / Structure |
Lasers
Sodium Chloride Revisited  Robert V. Stick and Mauro Mocerino
This "Tested Demonstration" describes the preparation of sodium chloride from its elements, sodium and chlorine. Along the way, tests for chlorine, iodine, and the chloride ion are included.
Stick, Robert V.; Mocerino, Mauro. J. Chem. Educ. 1996, 73, 539.
Precipitation / Solubility |
Oxidation / Reduction
Binding-Energy Curve for Iodine Using Laser Spectroscopy   L. C. O'Brien and R. L. Kubicek
The laser induced fluorescence spectrum of iodine is recorded using the 514.5 nm line of an Ar+ laser to excite the molecule. The molecular constants obtained by the analysis are used as input to an RKR program, which calculates the classical turning points for the binding-energy curve for iodine.
O'Brien, L. C.; Kubicek, R. L. J. Chem. Educ. 1996, 73, 86.
Laboratory Computing / Interfacing |
Lasers |
Spectroscopy
A Convenient Way to Generate Hydrogen Chloride: In the Freshman Lab  Francisco J. Arnáiz
A convenient way to generate hydrogen chloride.
Arnáiz, Francisco J. J. Chem. Educ. 1995, 72, 1139.
Laboratory Management |
Laboratory Equipment / Apparatus
Iodine Demonstration of Sublimation  Robert H. Goldsmith
Simple sublimation demonstration using iodine and an overhead projector.
Goldsmith, Robert H. J. Chem. Educ. 1995, 72, 1132.
Main-Group Elements |
Phases / Phase Transitions / Diagrams
The Chemical Adventures of Sherlock Holmes: The Problem of Woolthshrap Prison  Thomas R. Rybolt and Thomas G. Waddell
A chemical mystery with an emphasis on scientific observation and the criminal use of a classic reaction of chemistry (iodine and starch).
Rybolt, Thomas R.; Waddell, Thomas G. J. Chem. Educ. 1995, 72, 1090.
Enrichment / Review Materials |
Carbohydrates
Demonstrating a Lack of Reactivity Using a Teflon-Coated Pan  Thomas G. Richmond
Demonstration to illustrate a lack of chemical activity using a Teflon-coated pan.
Richmond, Thomas G.; Krause, Paul F. J. Chem. Educ. 1995, 72, 731.
Reactions |
Covalent Bonding
A Melting Point Depression Activity Using Two Inorganic Substances  DeMeo, Stephen
Measuring melting point depression using iodine and sulfur.
DeMeo, Stephen J. Chem. Educ. 1994, 71, 796.
Physical Properties |
Phases / Phase Transitions / Diagrams
Pyrotechnic Reactions Without Oxygen  Wright, Stephen W.
Reaction of K3FeF6 with Al and poly(tetrafluoroethylene) with Mg.
Wright, Stephen W. J. Chem. Educ. 1994, 71, 251.
Oxidation / Reduction |
Reactions
Bleaching with Chlorine: Another Tomato Juice Demonstration   Nemetz, Thomas M.; Ball, David W.
Bubbling chlorine gas through tomato juice produces dramatic color changes. This paper provides safe instructions for the demonstration.
Nemetz, Thomas M.; Ball, David W. J. Chem. Educ. 1993, 70, 154.
Periodicity / Periodic Table |
Reactions
Sulfur Hexafluoride: Classroom Uses for an Unusual Compound  Sullivan, Dan M.
A profile of one of the heaviest known gases and its possible safe uses in the classroom.
Sullivan, Dan M. J. Chem. Educ. 1993, 70, 100.
Gases |
Enrichment / Review Materials
A simple and colorful demonstration of light-catalyzed bromination of an alkane  Stevens, Malcolm P.
Light-catalyzed bromination of an alkane.
Stevens, Malcolm P. J. Chem. Educ. 1992, 69, 1028.
Catalysis |
Alkanes / Cycloalkanes |
Photochemistry |
Reactions
New source for starch solutions: Biodegradable pellets  de Moura, John M.
Convenient way to prepare starch indicator for use in iodine titrations or in "clock" reactions.
de Moura, John M. J. Chem. Educ. 1992, 69, 860.
Carbohydrates |
Titration / Volumetric Analysis
Microscale experiments: Dissolved oxygen and chloride determination in water  Crosson, Mary; Gibb, Reen
Determining the dissolved oxygen and chloride content of water samples through titrations.
Crosson, Mary; Gibb, Reen J. Chem. Educ. 1992, 69, 830.
Microscale Lab |
Water / Water Chemistry |
Aqueous Solution Chemistry |
Titration / Volumetric Analysis
Three methods for studying the kinetics of the halogenation of acetone.  Birk, James P.; Walters, David L.
Three methods for carrying out a kinetic study of the reaction between propanone and elemental iodine.
Birk, James P.; Walters, David L. J. Chem. Educ. 1992, 69, 585.
Aldehydes / Ketones |
Kinetics |
Spectroscopy |
Rate Law
Fast molecular motion  Knox, Kerro
A demonstration that shows that molecules do indeed move very fast and over long distances in a short time when nothing is in the way.
Knox, Kerro J. Chem. Educ. 1992, 69, 574.
Gases |
Kinetic-Molecular Theory
The pH range of the Mohr titration for chloride ion can be usefully extended to 4-10.5  Finlayson, A. C.
The pH ranges found in textbooks for this titration are misleading because of inadequate explanations for their basis.
Finlayson, A. C. J. Chem. Educ. 1992, 69, 559.
pH |
Titration / Volumetric Analysis |
Quantitative Analysis
The preparation of halogen waters   Diemente, Damon
Aqueous solutions of halogens can provide important demonstrations regarding periodicity, however many instructors are understandably hesitant to handle halogens. This author discusses the safe handling of halogens.
Diemente, Damon J. Chem. Educ. 1991, 68, 932.
Periodicity / Periodic Table |
Aqueous Solution Chemistry
Chloride in natural waters: An environmental application of a potentiometric titration  Lisensky, George; Reynolds, Kelly.
An environmental application of a potentiometric titration to determine chloride found in fresh water.
Lisensky, George; Reynolds, Kelly. J. Chem. Educ. 1991, 68, 334.
Potentiometry |
Titration / Volumetric Analysis |
Green Chemistry |
Geochemistry |
Quantitative Analysis
Reaction of bromine with hydrocarbons on the overhead, real or simulated  Solomon, Sally; Gregory, Michael; Padmanabhan, Sandeep; Smith, Kurt
A simulation that looks like the addition of bromine to hydrocarbons but is not (the bromine is simulated using a mixture of food colorings).
Solomon, Sally; Gregory, Michael; Padmanabhan, Sandeep; Smith, Kurt J. Chem. Educ. 1990, 67, 961.
Alkanes / Cycloalkanes |
Aromatic Compounds |
Addition Reactions
The H2 + Cl2 explosion as a chemical analogue of the photoelectric effect: A true quantum mechanical demonstration  Knox, Kerro
The photochemical hydrogen-chlorine reaction affords a good example of the quantum aspect of light and its interaction with matter.
Knox, Kerro J. Chem. Educ. 1990, 67, 897.
Reactions |
Quantum Chemistry |
Photochemistry
A visual demonstration of Raoult's law  Wilson, Archie S.
Reducing the vapor pressure of bromine by adding chloroform.
Wilson, Archie S. J. Chem. Educ. 1990, 67, 598.
Gases |
Equilibrium
Consumer chemistry demonstrations  Carberry, Edward; Gonnella, Thomas; Eliason, Robert
Demonstrating the hazards of mixing an acidic cleaner with bleach and the light-absorbing ability of sunscreens.
Carberry, Edward; Gonnella, Thomas; Eliason, Robert J. Chem. Educ. 1989, 66, 1041.
Consumer Chemistry |
Nonmajor Courses |
Photochemistry |
Toxicology
The iodine clock reaction: A surprising variant  Autuori, Marcos Alberto; Brolo, Alexandre Guimaraes; Mateus, Alfredo Luis M. L.
Substituting malonic acid for sulfuric acid.
Autuori, Marcos Alberto; Brolo, Alexandre Guimaraes; Mateus, Alfredo Luis M. L. J. Chem. Educ. 1989, 66, 852.
Reactions |
Kinetics |
Mechanisms of Reactions
Fluoropolymers: Part 1  Waller, F. J.
A brief account of fluoropolymers as an important part of polymer chemistry.
Waller, F. J. J. Chem. Educ. 1989, 66, 487.
The study of a simple redox reaction as an experimental approach to chemical kinetics  Elias, Horst; Zipp, Arden P.
The authors present a kinetics experiment based on the oxidation of iodide ions that, like the iodine clock, is quick and easy to perform but has the advantage of being followed directly rather than indirectly.
Elias, Horst; Zipp, Arden P. J. Chem. Educ. 1988, 65, 737.
Kinetics |
Reactions |
Rate Law
An overhead demonstration of some descriptive chemistry of the halogens and LeChtelier's principle  Hansen, Robert C.
Colorful demonstrations that illustrate Le Chtelier's principle, solubility rules, and periodic trends.
Hansen, Robert C. J. Chem. Educ. 1988, 65, 264.
Equilibrium |
Descriptive Chemistry |
Periodicity / Periodic Table
Redox demonstrations and descriptive chemistry: Part 2. Halogens  Ophardt, Charles E.
Oxidation states of bromine and iodine.
Ophardt, Charles E. J. Chem. Educ. 1987, 64, 807.
Oxidation / Reduction |
Descriptive Chemistry |
Oxidation State
The effect of pH and chloride ion concentration on the mobilities of various cations in soil  Brown, Melody; Sutherland, Mary; Leharne, Stephen
Measuring the mobilities of cations (particularly of toxic metals) in soils using soil thin layer chromatography.
Brown, Melody; Sutherland, Mary; Leharne, Stephen J. Chem. Educ. 1987, 64, 448.
pH |
Agricultural Chemistry |
Metals |
Thin Layer Chromatography
Methods for preparing aqueous solutions of chlorine and bromine for halogen displacement reactions  Hiegel, Gene A.; Abdala, Miguel H.; Burke, S. Vincent; Beard, Donald P.
Alternatives to handling and storing cylinders of chlorine gas and containers of liquid bromine.
Hiegel, Gene A.; Abdala, Miguel H.; Burke, S. Vincent; Beard, Donald P. J. Chem. Educ. 1987, 64, 156.
Aqueous Solution Chemistry |
Laboratory Management
Iodine clock reaction mechanisms  Lambert, Jack L.; Fina, Gary T.
Outlines the mechanism for the simple iodine clock reaction and the "Old Nassau" modification.
Lambert, Jack L.; Fina, Gary T. J. Chem. Educ. 1984, 61, 1037.
Mechanisms of Reactions |
Reactions |
Kinetics |
Oxidation / Reduction
Treat 'em to Tchaikovsky  Whitman, Mark
The author shares a demonstration that attracts great student attention. Students are highly successful when answering questions about the phenomenon in this demonstration on ensuing exams.
Whitman, Mark J. Chem. Educ. 1983, 60, 229.
Reactions |
Rate Law
Simplest formula of copper iodide: a stoichiometry experiment  MacDonald, D. J.
It is difficult to find a chemistry experiment that convincingly demonstrates stoichiometric relationships. The experiment in this article is elegant and pedagogically effective.
MacDonald, D. J. J. Chem. Educ. 1983, 60, 147.
Stoichiometry
Spontaneous combustion of familiar substances in chlorine  Briggs, Thomas S.
Reacting chlorine generated from liquid bleach with red phosphorus (from a match book) and iron from steel wool.
Briggs, Thomas S. J. Chem. Educ. 1982, 59, 788.
Reactions |
Oxidation / Reduction
More "quickies"  Rosenberg, Milton H.
Some quick, challenging questions that cover various areas of chemistry.
Rosenberg, Milton H. J. Chem. Educ. 1981, 58, 994.
X-ray Crystallography |
Aqueous Solution Chemistry |
Solutions / Solvents
Recycling silver chloride  Thall, Edwin
A simple way to reduce lab cost by recycling silver in the academic lab.
Thall, Edwin J. Chem. Educ. 1981, 58, 561.
Laboratory Management
Rossini, William Tell and the iodine clock reaction: A lecture demonstration  Brice, L. K.
The iodine clock reaction is timed to coincide with three portions of the William Tell Overture.
Brice, L. K. J. Chem. Educ. 1980, 57, 152.
Reactions |
Kinetics |
Rate Law
Determination of the equilibrium constant for triiodide formation. Use of a less toxic solvent  Ackermann, Martin N.
A typical equilibrium laboratory may be hazardous for inexperienced students to perform.
Ackermann, Martin N. J. Chem. Educ. 1978, 55, 795.
Equilibrium
The Landolt, "Old Nassau", and variant reactions   Moss, Arthur
Instructions for a modification to the classic "iodine clock" reaction.
Moss, Arthur J. Chem. Educ. 1978, 55, 244.
Kinetics |
Reactions
Different experiment on chemical composition  Wells, Norman; Boschmann, Erwin
The synthesis of antimony iodide.
Wells, Norman; Boschmann, Erwin J. Chem. Educ. 1977, 54, 586.
Stoichiometry
Determination of iodide in seaweed. A general chemistry research experience  Senyk, Joan I.
Students determine the best procedure for the analysis of iodide in locally gathered seaweed.
Senyk, Joan I. J. Chem. Educ. 1977, 54, 511.
Quantitative Analysis |
Separation Science |
Titration / Volumetric Analysis
Singlet oxygen in aqueous solution: A lecture demonstration   Shakhashiri, Bassam Z.; Williams, Lloyd G.
Lecture demonstrations involving chemiluminescence are useful for the purpose both of displaying chemical phenomena and of illustrating specific principles.
Shakhashiri, Bassam Z.; Williams, Lloyd G. J. Chem. Educ. 1976, 53, 358.
Photochemistry |
Reactions |
Oxidation / Reduction |
Spectroscopy
Chlorine in your water  Smith, J. G.
The use, chemistry, and alternatives to chlorine and chlorine compounds in water supplies.
Smith, J. G. J. Chem. Educ. 1975, 52, 656.
Water / Water Chemistry |
Consumer Chemistry
A spectrophotometric determination of fluoride adapted for the freshman laboratory  Daines, Terri L.; Morse, Karen W.
In this experiment the student determines the fluoride ion concentration of a sodium fluoride solution, which they can do with high precision and accuracy.
Daines, Terri L.; Morse, Karen W. J. Chem. Educ. 1974, 51, 680.
Quantitative Analysis |
Solutions / Solvents |
Spectroscopy
Questions [and] Answers  Campbell, J. A.
Six questions requiring the application of basic principles of chemistry.
Campbell, J. A. J. Chem. Educ. 1972, 49, 538.
Enrichment / Review Materials |
Applications of Chemistry |
Electrochemistry |
Astrochemistry |
Stoichiometry |
Metals
A classroom demonstration of exothermicity  Boschmann, Erwin
The heat generated by dissolving NaOH in water causes iodine crystals to sublime.
Boschmann, Erwin J. Chem. Educ. 1970, 47, A206.
Calorimetry / Thermochemistry |
Reactions |
Aqueous Solution Chemistry |
Phases / Phase Transitions / Diagrams
Detection of chloride, bromide, and iodide following sodium fusion  McCullough, Thomas; Allaire, Pierre N.; Boettcher, Brian R.
Presents the use of paper chromatography in conjunction with the sodium fusion detection of chloride, bromide, and iodide.
McCullough, Thomas; Allaire, Pierre N.; Boettcher, Brian R. J. Chem. Educ. 1970, 47, 217.
Qualitative Analysis |
Chromatography
Group VII. The Halogens. E. Iodine   Alyea, Hubert N.; Gorman, Raymond P.
Five overhead demonstrations involving iodine.
Alyea, Hubert N.; Gorman, Raymond P. J. Chem. Educ. 1969, 46, A451.
Instantaneous precipitation from homogeneous solution  Hiskey, C. F.; Cantwell, F. F.
Procedure for the iodine clock reaction.
Hiskey, C. F.; Cantwell, F. F. J. Chem. Educ. 1967, 44, A727.
Precipitation / Solubility |
Aqueous Solution Chemistry |
Kinetics
Letter to the editor (the author replies)  Holloway, John L.
Warns readers about the dangers associated with the preparation of xenon fluoride.
Holloway, John L. J. Chem. Educ. 1966, 43, 619.
Photochemistry
Letter to the editor  Chernick, Cedrick L.
Warns readers about the dangers associated with the preparation of xenon fluoride.
Chernick, Cedrick L. J. Chem. Educ. 1966, 43, 619.
Photochemistry
The dissolution of tin in solutions of iodine  Davies, J. F.; Trotman-Dickenson, A. F.
The progress of this reaction can be followed by the loss of weight of a tin disc.
Davies, J. F.; Trotman-Dickenson, A. F. J. Chem. Educ. 1966, 43, 483.
Solutions / Solvents |
Precipitation / Solubility |
Kinetics |
Gravimetric Analysis
Stoichiometry of the reaction of bromine with phenols  Lockwood, Karl L.
The purpose of this investigation is to establish the stoichiometry for the reaction of a number of phenols with bromine, and to demonstrate the rapid and quantitative nature of the reaction of bromine with enols.
Lockwood, Karl L. J. Chem. Educ. 1965, 42, 482.
Stoichiometry |
Phenols
Detection of chloride ion in the presence of bromide, iodide, and thiocyanate ions  Paul, Armine D.; Gibson, John A., Jr.
Summarizes and evaluates several published methods for detecting chloride ions in the presence of bromide, iodide, and thiocyanate ions.
Paul, Armine D.; Gibson, John A., Jr. J. Chem. Educ. 1965, 42, 440.
Aqueous Solution Chemistry |
Qualitative Analysis |
Solutions / Solvents |
Precipitation / Solubility
Teaching principles of quantitative analysis with "qual" reactions  O'Donnell, T. A.
A series of test-tube reactions using semi-micro techniques has been devised to precede each section of the course in quantitative analysis designed to illustrate qualitatively or semi-qualitatively the chemical reactions or principles that are the basis of each quantitative exercise.
O'Donnell, T. A. J. Chem. Educ. 1965, 42, 434.
Quantitative Analysis |
Reactions
Polar properties and solubility  Summerlin, Lee R.
Compares the solubility of iodine in layers of CCl4, water, and ether, all in the same container.
Summerlin, Lee R. J. Chem. Educ. 1964, 41, A883.
Aqueous Solution Chemistry |
Precipitation / Solubility
Concerning equilibrium, free energy changes, Le Chtelier's principle  Eberhardt, William H.
Aqueous KI is added to a solution of CuSO4 in a separatory funnel; adding more CuSO4 demonstrates an equilibrium sift.
Eberhardt, William H. J. Chem. Educ. 1964, 41, A477.
Equilibrium |
Thermodynamics |
Reactions
A kinetics experiment for first year chemistry  Shaefer, William P.
The exchange of iodine atoms between organic and inorganic iodides serves as a kinetics experiment for first year chemistry.
Shaefer, William P. J. Chem. Educ. 1964, 41, 558.
Kinetics |
Isotopes |
Rate Law
The oxidation of iodide ion by persulfate ion  Moews, P. C., Jr.; Petrucci, R. H.
Presents the oxidation of iodide ion by persulfate ion as an ideal reaction to study as part of an experiment on kinetics.
Moews, P. C., Jr.; Petrucci, R. H. J. Chem. Educ. 1964, 41, 549.
Oxidation / Reduction |
Reactions |
Kinetics |
Rate Law
Effect of chloride ion on precipitation of cadmium sulfide  O'Donnell, T. A.
Adding NaCl or KCl to suspended CdS causes the suspension to disappear.
O'Donnell, T. A. J. Chem. Educ. 1963, 40, A313.
Precipitation / Solubility |
pH |
Equilibrium
Oxidation of bromide and iodide ions  Dutton, Frederic B.
Color changes are indicative of oxidation reactions of bromide and iodide ions.
Dutton, Frederic B. J. Chem. Educ. 1963, 40, A241.
Oxidation / Reduction |
Reactions |
Electrochemistry
Oxidation of bromide and iodide ions  Dutton, Frederic B.
Color changes are indicative of oxidation reactions of bromide and iodide ions.
Dutton, Frederic B. J. Chem. Educ. 1963, 40, A241.
Oxidation / Reduction |
Reactions |
Electrochemistry
A reaction tube for sodium and chlorine  Barnard, W. Robert
Describes reacting sodium and chlorine in Pyrex tubing.
Barnard, W. Robert J. Chem. Educ. 1963, 40, A49.
Reactions |
Laboratory Equipment / Apparatus
Would Mendeleev have predicted the existence of XeF4?  Ward, Roland
The author suggests that a contemporary Mendeleev might have used the concept of molecular orbitals to predict the existence of XeF4.
Ward, Roland J. Chem. Educ. 1963, 40, 277.
Nonmetals |
Molecular Properties / Structure
Iodomercurates  Young, Jay A.; Taylor, John K.
Suggests some research activities based on an article published previously in the Journal.
Young, Jay A.; Taylor, John K. J. Chem. Educ. 1962, 39, A960.
Undergraduate Research
The discovery of bromine. The chemistry of fixed air (Klopfer, Leo E.)  Benfey, O. T.

Benfey, O. T. J. Chem. Educ. 1962, 39, A142.
Letters to the editor  Kapp, George
Presents a demonstration of chlorine's ability to bleach wet or moist but not dry materials.
Kapp, George J. Chem. Educ. 1956, 33, 414.
Demonstration of dynamic nature of ions using I131  Blake, Richard F.
This demonstration presents visual evidence of the ionic nature of solid salts and the dynamic equilibrium existing between dissolved and undissolved ions.
Blake, Richard F. J. Chem. Educ. 1956, 33, 354.
Isotopes |
Aqueous Solution Chemistry |
Solids |
Precipitation / Solubility |
Equilibrium
Effect of water on the interaction of aluminum and iodine  Azmatullah, Syed; Viswanathan, Argot
A drop of water added to powdered aluminum and iodine initiates a vigorous reaction.
Azmatullah, Syed; Viswanathan, Argot J. Chem. Educ. 1955, 32, 447.
Water / Water Chemistry |
Reactions
Letters to the editor  Wolf, Milton G.
The results of collecting chlorine through the displacement of saturated aqueous solutions of calcium chloride and sodium chloride.
Wolf, Milton G. J. Chem. Educ. 1954, 31, 48.
Aqueous Solution Chemistry |
Gases