TIGER

Journal Articles: 22 results
A New "Bottom-Up" Framework for Teaching Chemical Bonding  Tami Levy Nahum, Rachel Mamlok-Naaman, Avi Hofstein, and Leeor Kronik
This article presents a general framework for bonding that can be presented at different levels of sophistication depending on the student's level and needs. The pedagogical strategy for teaching this model is a "bottom-up" one, starting with basic principles and ending with specific properties.
Levy Nahum, Tami; Mamlok-Naaman, Rachel; Hofstein, Avi; Kronik, Leeor. J. Chem. Educ. 2008, 85, 1680.
Atomic Properties / Structure |
Covalent Bonding |
Ionic Bonding |
Lewis Structures |
Materials Science |
MO Theory |
Noncovalent Interactions
Six Pillars of Organic Chemistry  Joseph J. Mullins
This article focuses on a core set of conceptselectronegativity, polar covalent bonding, inductive and steric effects, resonance, and aromaticitythe proper application of which can explain and predict a wide variety of chemical, physical, and biological properties of molecules and conceptually unite important features of general, organic, and biochemistry.
Mullins, Joseph J. J. Chem. Educ. 2008, 85, 83.
Bioorganic Chemistry |
Covalent Bonding |
Hydrogen Bonding |
Mechanisms of Reactions |
Periodicity / Periodic Table |
Reactive Intermediates |
Resonance Theory
More on the Nature of Resonance  Robert C. Kerber
The author continues to find the use of delocalization preferable to resonance.
Kerber, Robert C. . J. Chem. Educ. 2006, 83, 1291.
Aromatic Compounds |
Covalent Bonding |
Molecular Properties / Structure |
Resonance Theory |
Nomenclature / Units / Symbols
More on the Nature of Resonance  William B. Jensen
Supplements a recent article on the interpretation of resonance theory with three additional observationsone historical and two conceptual.
Jensen, William B. J. Chem. Educ. 2006, 83, 1290.
Aromatic Compounds |
Covalent Bonding |
Molecular Properties / Structure |
Nomenclature / Units / Symbols |
Resonance Theory
Rules of Thumb for Assessing Equilibrium Partitioning of Organic Compounds: Successes and Pitfalls  Kai-Uwe Goss and René P. Schwarzenbach
Factors to consider when predicting equilibrium partitioning of organic compounds between two phases, including volatility, polarity, and hydrophobicity; and a simple model for the evaluation of bulk phase partitioning.
Goss, Kai-Uwe; Schwarzenbach, René P. J. Chem. Educ. 2003, 80, 450.
Equilibrium |
Noncovalent Interactions |
Separation Science |
Thermodynamics
Chemical Bonding and Molecular Geometry: From Lewis to Electron Densities (Gillespie and Popelier)  Daniel Rabinovich
Overview of the classical and modern concepts used to explain and predict molecular geometries of the nonmetallic elements and their compounds.
Rabinovich, Daniel. J. Chem. Educ. 2003, 80, 31.
Covalent Bonding |
Molecular Properties / Structure |
VSEPR Theory |
Valence Bond Theory |
Lewis Structures |
Nonmetals
How Do Organic Chemistry Students Understand and Apply Hydrogen Bonding?  J. Henderleiter, R. Smart, J. Anderson, and O. Elian
Examination of how students completing a two-semester organic sequence understand, explain, and apply hydrogen bonding to determine the physical attributes of molecules.
Henderleiter, J.; Smart, R.; Anderson, J.; Elian, O. J. Chem. Educ. 2001, 78, 1126.
Noncovalent Interactions |
Learning Theories |
Hydrogen Bonding |
Molecular Properties / Structure
Electronegativity and Bond Type: Predicting Bond Type  Gordon Sproul
Important limitations with using electronegativity differences to determine bond type and recommendations for using electronegativities in general chemistry.
Sproul, Gordon. J. Chem. Educ. 2001, 78, 387.
Covalent Bonding |
Materials Science |
Periodicity / Periodic Table |
Ionic Bonding |
Atomic Properties / Structure |
Metallic Bonding
Chemical Bonding as a Superposition Phenomenon  Frank Weinhold
The characteristic phenomena of chemistry-covalent and coordinate bonding, resonance delocalization, aromaticity, H-bonding, hyperconjugation-can also be seen as special cases of a central superposition paradigm: the "donor-acceptor" interaction between filled and unfilled orbitals.
Weinhold, Frank. J. Chem. Educ. 1999, 76, 1141.
Covalent Bonding |
Quantum Chemistry |
Aromatic Compounds |
Noncovalent Interactions |
Quantum Chemistry |
MO Theory
The Use of Molecular Modeling and VSEPR Theory in the Undergraduate Curriculum to Predict the Three-Dimensional Structure of Molecules  Brian W. Pfennig and Richard L. Frock
Despite the simplicity and elegance of the VSEPR model, however, students often have difficulty visualizing the three-dimensional shapes of molecules and learning the more subtle features of the model, such as the bond length and bond angle deviations from ideal geometry that accompany the presence of lone pair or multiple bond domains or that result from differences in the electronegativity of the bonded atoms, partial charges and molecular dipole moments, and site preferences in the trigonal bipyramidal electron geometry.
Pfennig, Brian W.; Frock, Richard L. J. Chem. Educ. 1999, 76, 1018.
Molecular Modeling |
Molecular Properties / Structure |
Covalent Bonding |
VSEPR Theory
Teaching Chemistry with Electron Density Models  Gwendolyn P. Shusterman and Alan J. Shusterman
This article describes a powerful new method for teaching students about electronic structure and its relevance to chemical phenomena. This method, developed and used for several years in general chemistry and organic chemistry courses, relies on computer-generated three-dimensional models of electron density distributions.
Shusterman, Gwendolyn P.; Shusterman, Alan J. J. Chem. Educ. 1997, 74, 771.
Learning Theories |
Computational Chemistry |
Molecular Modeling |
Quantum Chemistry |
Atomic Properties / Structure |
Covalent Bonding |
Ionic Bonding |
Noncovalent Interactions
Grade-12 students' misconceptions of covalent bonding and structure  Peterson, Raymond F.; Treagust, David F.
A multiple-choice pencil-and-paper diagnostic instrument used to measure student understanding of covalent bonding and structure concepts, its results, and implications for instruction.
Peterson, Raymond F.; Treagust, David F. J. Chem. Educ. 1989, 66, 459.
Covalent Bonding |
Molecular Properties / Structure
Principles of electronegativity Part I. General nature  Sanderson, R. T.
The concept of electronegativity has been modified, expanded, and debated. The concept can be used to help students gain valuable insights and understanding of the cause-and-effect relationship between atomic structure and compound properties. This is the first in a series of articles that explores the important concept of electronegativity.
Sanderson, R. T. J. Chem. Educ. 1988, 65, 112.
Electrochemistry |
Periodicity / Periodic Table |
Noncovalent Interactions |
Atomic Properties / Structure |
Physical Properties |
Enrichment / Review Materials
Methane pistol  Skinner, James F.
This simple demonstration leaves a lasting impression of the importance of intermolecular forces and hydrogen bonding.
Skinner, James F. J. Chem. Educ. 1987, 64, 171.
Noncovalent Interactions |
Hydrogen Bonding |
Molecular Properties / Structure
Coulombic models in chemical bonding. II. Dipole moments of binary hydrides  Sacks, Lawrence J.
A discussion of Coulumbic models and their aid in understanding chemical bonding.
Sacks, Lawrence J. J. Chem. Educ. 1986, 63, 373.
Electrochemistry |
Molecular Properties / Structure |
Covalent Bonding |
Noncovalent Interactions
Competition analogy  Felty, Wayne L.
Using football competition as an analogy for bond polarity.
Felty, Wayne L. J. Chem. Educ. 1985, 62, 869.
Covalent Bonding |
Atomic Properties / Structure
Understanding chemistry: Current and possible  Sanderson, R. T.
This paper attempts to present a traditional teaching approach in a concise form, and to allow evaluation of the approach as a whole, in contrast to the piecemeal treatment available up to now.
Sanderson, R. T. J. Chem. Educ. 1976, 53, 675.
Atomic Properties / Structure |
Quantum Chemistry |
Covalent Bonding
Why does methane burn?  Sanderson, R. T.
A thermodynamic explanation for why methane burns.
Sanderson, R. T. J. Chem. Educ. 1968, 45, 423.
Thermodynamics |
Reactions |
Oxidation / Reduction |
Calorimetry / Thermochemistry |
Covalent Bonding |
Ionic Bonding
Principles of chemical reaction  Sanderson, R. T.
The purpose of this paper is to examine the nature of chemical change in the hope of recognizing and setting forth the basic principles that help us to understand why they occur.
Sanderson, R. T. J. Chem. Educ. 1964, 41, 13.
Reactions |
Thermodynamics |
Mechanisms of Reactions |
Kinetics |
Synthesis |
Covalent Bonding |
Ionic Bonding |
Metallic Bonding
Ionic character, polarity, and electronegativity  Wilmshurst, J. K.
This article attempts to clearly define ionic character and polarity in both the valence bond and molecular orbital approximations; the electronegativity concept is also discussed.
Wilmshurst, J. K. J. Chem. Educ. 1962, 39, 132.
Covalent Bonding |
MO Theory
Principles of chemical bonding  Sanderson, R. T.
Develops, through 25 statements, the basic principles of chemical bonding.
Sanderson, R. T. J. Chem. Educ. 1961, 38, 382.
Covalent Bonding |
Metallic Bonding |
Ionic Bonding |
Atomic Properties / Structure |
Molecular Properties / Structure
Bonding in boron compounds and in inorganic polymers  Burg, Anton B.
The element boron is such a close neighbor to carbon in the periodic table that one might expect it to offer an equally extensive and varied chemistry of covalent compounds.
Burg, Anton B. J. Chem. Educ. 1960, 37, 482.
Covalent Bonding