TIGER

Journal Articles: 66 results
Probing the Orbital Energy of an Electron in an Atom  James L. Bills
This article answers an appeal for simple theoretical interpretations of atomic properties. A theoretical snapshot of an atom, showing the screened nuclear charge and the electron to be ionized at its radius of zero kinetic energy, enables anyone to approximate its ionization energy.
Bills, James L. J. Chem. Educ. 2006, 83, 473.
Atomic Properties / Structure |
Main-Group Elements |
Periodicity / Periodic Table |
Physical Properties |
Quantum Chemistry |
Theoretical Chemistry
The Place of Zinc, Cadmium, and Mercury in the Periodic Table  William B. Jensen
Explanation for why the zinc group belongs with the main group elements; includes several versions of periodic tables.
Jensen, William B. J. Chem. Educ. 2003, 80, 952.
Periodicity / Periodic Table |
Main-Group Elements |
Transition Elements |
Descriptive Chemistry |
Atomic Properties / Structure
Ionization Energies of Atoms and Atomic Ions  Peter F. Lang and Barry C. Smith
Explanations for the apparently irregular first and second ionization energies of transition and inner transition elements.
Lang, Peter F.; Smith, Barry C. J. Chem. Educ. 2003, 80, 938.
Atomic Properties / Structure |
Main-Group Elements |
Periodicity / Periodic Table |
Transition Elements |
Inner Transition Elements
The Noble Gas Configuration—Not the Driving Force but the Rule of the Game in Chemistry  Roland Schmid
Explains the covalent and ionic bonding behavior of main-group elements in terms of electromagnetic forces rather than the supposed "stability" of noble-gas configurations.
Schmid, Roland. J. Chem. Educ. 2003, 80, 931.
Molecular Modeling |
Periodicity / Periodic Table |
Main-Group Elements |
Atomic Properties / Structure |
Reactions |
Covalent Bonding |
Ionic Bonding
Understanding and Interpreting Molecular Electron Density Distributions  C. F. Matta and R. J. Gillespie
A simple introduction to the electron densities of molecules and how they can be analyzed to obtain information on bonding and geometry.
Matta, C. F.; Gillespie, R. J. J. Chem. Educ. 2002, 79, 1141.
Covalent Bonding |
Molecular Properties / Structure |
Quantum Chemistry |
Theoretical Chemistry |
Atomic Properties / Structure |
Molecular Modeling |
VSEPR Theory
Response to Lowe's Potential-Energy-Only Models  Lowe, John P.
Discussion of the suitability of a potential-only model for the successive ionization energies of sulfur for an introductory chemistry course.
Lowe, John P. J. Chem. Educ. 2002, 79, 430.
Atomic Properties / Structure |
Quantum Chemistry |
Theoretical Chemistry
Response to Lowe's Potential-Energy-Only Models (re J. Chem. Educ. 2000, 77, 155-156)  Frank Rioux and Roger L. DeKock
Discussion of the suitability of a potential-only model for the successive ionization energies of sulfur for an introductory chemistry course.
Rioux, Frank; DeKock, Roger L. J. Chem. Educ. 2002, 79, 429.
Atomic Properties / Structure |
Quantum Chemistry |
Theoretical Chemistry
The Mendeleev-Seaborg Periodic Table: Through Z = 1138 and Beyond  Paul J. Karol
Extending the periodic table to very large atomic numbers and its implications for the organization of the periodic table, consideration of relativistic effects, and the relative stability of massive and supermassive atomic nuclei.
Karol, Paul J. J. Chem. Educ. 2002, 79, 60.
Atomic Properties / Structure |
Nuclear / Radiochemistry |
Periodicity / Periodic Table |
Astrochemistry
Response to Potential-Energy-Only Models (re J. Chem. Educ. 2000, 77, 155-156)  Frank Rioux and Roger L. DeKock
Example of buffering power in deviations of the pH of sodium acetate from calculated values.
Rioux, Frank; DeKock, Roger L. J. Chem. Educ. 2002, 79, 29.
Acids / Bases |
Carboxylic Acids |
pH |
Atomic Properties / Structure |
Quantum Chemistry |
Theoretical Chemistry
Screening Percentages Based on Slater Effective Nuclear Charge as a Versatile Tool for Teaching Periodic Trends  Kimberley A. Waldron, Erin M. Fehringer, Amy E. Streeb, Jennifer E. Trosky, and Joshua J. Pearson
Using charge shielding to identify and explain trends within the periodic table.
Waldron, Kimberley A.; Fehringer, Erin M.; Streeb, Amy E.; Trosky, Jennifer E.; Pearson, Joshua J. J. Chem. Educ. 2001, 78, 635.
Periodicity / Periodic Table |
Theoretical Chemistry |
Atomic Properties / Structure
Comments on Kinetic, Potential, and Ionization Energies  John P. Lowe
Despite the importance of kinetic energy changes in ionization processes, it is not necessary to explicitly include them when modeling ionization energies: the virial theorem allows one to use potential-energy-only models. A simple potential-energy-only model calculation of the ionization energies of sulfur illustrates the shell structure of this atom.
Lowe, John P. J. Chem. Educ. 2000, 77, 155.
Atomic Properties / Structure |
Quantum Chemistry |
Theoretical Chemistry
The Genius of Slater's Rules  James L. Reed
With only a few modifications a procedure has been developed that yields the one-electron energies for atoms and ions with a level of detail very well suited for instruction in the structure and properties of atoms. It provides for the computation of very reasonable values for such properties as ionization energies, electron affinities, promotion energies, electronic transitions, and even XPS and ESCA spectra.
Reed, James L. J. Chem. Educ. 1999, 76, 802.
Atomic Properties / Structure |
Quantum Chemistry |
Theoretical Chemistry |
Spectroscopy
Letters  
Consideration of kinetic energy in interpreting atomic ionization energies is redundant.
Richman, Robert M. J. Chem. Educ. 1999, 76, 605.
Atomic Properties / Structure |
Quantum Chemistry
Chemistry of the Heaviest Elements-One Atom at a Time  Darleane C. Hoffman and Diana M. Lee
A 75-year perspective of the chemistry of the heaviest elements, including a 50-year retrospective view of past developments, a summary of current research achievements and applications, and some predictions about exciting, new developments that might be envisioned within the next 25 years.
Hoffman, Darleane C.; Lee, Diana M. J. Chem. Educ. 1999, 76, 331.
Chromatography |
Instrumental Methods |
Isotopes |
Nuclear / Radiochemistry |
Separation Science |
Descriptive Chemistry |
Enrichment / Review Materials |
Atomic Properties / Structure
Experimental 4s and 3d Energies in Atomic Ground States  James L. Bills
A new definition is given for the effective charge Zf. HF orbital energies e4s and e3d are used in concert with I4s and I3d to answer four questions: Why does the 4s sublevel fill before 3d? Why is ionization easier for 4s than 3d? When 4s23dn has e3d < e4s, why doesn't 4s23dn -> 4s13dn+1? Why are Cr and Cu each 4s13dn+1 instead of 4s23dn?
Bills, James L. J. Chem. Educ. 1998, 75, 589.
Atomic Properties / Structure
Deducing the Shell Model from Ionization Energies and the Use of Models in Introductory Chemistry  Ronald J. Gillespie, Richard S. Moog, and James N. Spencer
A major objection of Rioux and DeKock is the statement in the authors' earlier paper that electron repulsion is responsible for the relative ionization energies of H and He. The commentators work clearly shows that a quantum mechanical treatment of this problem reveals that kinetic energy considerations play a crucial role in these values. However, although their criticism is appropriate in the context of this more sophisticated QM treatment, it does not in any way invalidate the authors original paper, the goal of which was to provide a model, namely the shell model, for the electronic structure of atoms that is consistent with experimental ionization energies.
Gillespie, Ronald J.; Moog, Richard S.; Spencer, James N. J. Chem. Educ. 1998, 75, 539.
Atomic Properties / Structure |
Quantum Chemistry |
Theoretical Chemistry
The Crucial Role of Kinetic Energy in Interpreting Ionization Energies  Frank Rioux and Roger L. DeKock
The experimental ratio of the ionization energies of H and He is 1.81. The authors show that it is not correct to interpret this ratio using a classical Coulombic potential energy model. Rather a quantum mechanical model is required in which both kinetic and potential energy play a role.
Rioux, Frank; DeKock, Roger L. J. Chem. Educ. 1998, 75, 537.
Atomic Properties / Structure |
Quantum Chemistry |
Theoretical Chemistry
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
Dymystification at What Cost? (re J. Chem. Educ. 1996, 73, 617 and 627)  R. J. Gillespie, J. N. Spencer, R. S. Moog
Rationale for using Allen's scale of electronegativities.
Gillespie, R. J.; Spencer, J. N.; Moog, R. S. . J. Chem. Educ. 1997, 74, 480.
Atomic Properties / Structure
Dymystification at What Cost? (re J. Chem. Educ. 1996, 73, 617 and 627)  Eric Scerri
Errors and questionable rationale for using Allen's scale of electronegativities.
Scerri, Eric. J. Chem. Educ. 1997, 74, 480.
Atomic Properties / Structure
Wiley Series in Ion Chemistry and Physics: Low Energy Ion-Surface Interactions (Rabalais, J. Wayne; Baer, Tomas; Ng, Cheuk-Yiu; Powis, Ivan)  
Monograph.
J. Chem. Educ. 1995, 72, A42.
Atomic Properties / Structure |
Surface Science
Examining the Shapes of Atomic Orbitals Using Mathcad  Ramachandran, B.
180. Bits and pieces, 55. Describes how three-dimensional contour plots of spherical harmonics may be generated using MathCad.
Ramachandran, B. J. Chem. Educ. 1995, 72, 1082.
Atomic Properties / Structure |
Quantum Chemistry |
Mathematics / Symbolic Mathematics
The Periodic Table of Atoms: Arranging the Elements by a Different Set of Rules  Treptow, Richard S.
The periodic table found in this paper is based on the properties of free gaseous atoms rather than atoms in a chemical environment.
Treptow, Richard S. J. Chem. Educ. 1994, 71, 1007.
Periodicity / Periodic Table |
Atomic Properties / Structure
Simulations and Interactive Resources  Martin, John S.
12 Simulations and Interactive Resources (SIRs) including Periodic Table Displays, Electron Orbits and Orbitals, Electron Configurations, Barometers and Manometers, Vapor Pressure, Ideal Gas Behavior, Heat Capacity and Heat of Reaction, Approach to Equilibrium, The Law of Chemical Equilibrium, Titration Curves, Electrochemical Cells, and Rate of Reaction.
Martin, John S. J. Chem. Educ. 1994, 71, 667.
Periodicity / Periodic Table |
Atomic Properties / Structure |
Gases |
Calorimetry / Thermochemistry |
Equilibrium |
Titration / Volumetric Analysis |
Electrolytic / Galvanic Cells / Potentials |
Rate Law
Transition Metals and the Aufbau Principle  Vanquickenborne, L. G.; Pierloot, K.; Devoghel, D.
Explanation of why the ground state configuration of the neutral transition metals is in most cases 3dn4s2, and why the ground state configuration of the corresponding ions is obtained by preferentially removing the 4s electrons.
Vanquickenborne, L. G.; Pierloot, K.; Devoghel, D. J. Chem. Educ. 1994, 71, 469.
Transition Elements |
Metals |
Atomic Properties / Structure
Experiment in quantization: Atomic line spectra  Shields, George C.; Kash, Michael M.
This experiment offers a simple and visual method for determining the wavelength of spectral lines.
Shields, George C.; Kash, Michael M. J. Chem. Educ. 1992, 69, 329.
Atomic Properties / Structure |
Quantum Chemistry |
Spectroscopy
More about the particle-in-a-box system: The confinement of matter and the wave-particle dualism  Volkamer, Klaus; Lerom, Michael W.
Since the particle-in-a-box system (PIB model) is mathematically so simple, it can be used to provide illustrations of many important quantum mechanical concepts without obscuring the principles with mathematical details.
Volkamer, Klaus; Lerom, Michael W. J. Chem. Educ. 1992, 69, 100.
Quantum Chemistry |
Atomic Properties / Structure
Developmental instruction: Part II. Application of the Perry model to general chemistry  Finster, David C.
The Perry scheme offers a framework in which teachers can understand how students make meaning of their world, and specific examples on how instructors need to teach these students so that the students can advance as learners.
Finster, David C. J. Chem. Educ. 1991, 68, 752.
Learning Theories |
Atomic Properties / Structure |
Chemometrics |
Descriptive Chemistry
There are no such things as orbitals-Act two!  Simons, Jack
What is the role of molecular orbital theory in chemistry instruction?
Simons, Jack J. Chem. Educ. 1991, 68, 131.
MO Theory |
Atomic Properties / Structure |
Quantum Chemistry
The nature of the chemical bond--1990: There are no such things as orbitals!  Ogilivie, J. F.
The author discusses the fundamental principles of quantum mechanics, the laws and theories, and the relationship of quantum-mechanics to atomic and molecular structure, as well as their relevance to chemical education.
Ogilivie, J. F. J. Chem. Educ. 1990, 67, 280.
Quantum Chemistry |
Atomic Properties / Structure |
Molecular Properties / Structure
A formula for calculating atomic radii of metals  Ping, Mei; Xiubin, Lei; Yuankai, Wen
In this paper, the authors present a theoretical formula for calculating metallic radii.
Ping, Mei; Xiubin, Lei; Yuankai, Wen J. Chem. Educ. 1990, 67, 218.
Atomic Properties / Structure |
Metals
The Heisenberg uncertainty principle: An application to the shell structure of atoms and orbit descriptions of molecules  Hartcourt, Richard D.
A further novel use of the uncertainty principle to deduce the 2n2 shell occupancy rule for atoms.
Hartcourt, Richard D. J. Chem. Educ. 1987, 64, 1070.
Atomic Properties / Structure
Electron spectroscopic methods in teaching  Allan, Michael
Presents several spectra in a format suitable for teaching applications with the intention of promoting the use of electron energy-loss spectroscopy in teaching the electronic structure of atoms and molecules at an elementary level.
Allan, Michael J. Chem. Educ. 1987, 64, 418.
Spectroscopy |
Quantum Chemistry |
Photochemistry |
Atomic Properties / Structure |
Molecular Properties / Structure |
MO Theory
An upward view of the periodic table: Getting to the bottom of it  Guenther, William B.
Develops the 18-group basis of the periodic table; shows that, while the 1-18 designations can give unambiguous information to students, no printed designations are needed for teaching; and shows how to obtain unique, physical group definitions that avoid the problems of conflicting and changeable chemical interpretations.
Guenther, William B. J. Chem. Educ. 1987, 64, 9.
Periodicity / Periodic Table |
Atomic Properties / Structure
Revised atomic form periodic table  Strong, Frederick C., III
A circular periodic table.
Strong, Frederick C., III J. Chem. Educ. 1985, 62, 456.
Atomic Properties / Structure |
Periodicity / Periodic Table
Orbital shape representations  Kikuchi, Osamu; Suzuki, Keizo
The use of two-dimensional polar plots and three-dimensional contour surfaces to represent atomic orbitals.
Kikuchi, Osamu; Suzuki, Keizo J. Chem. Educ. 1985, 62, 206.
Atomic Properties / Structure
Electronic structure prediction for transition metal ions  Nance, Lewis E.
A useful mnemonic for the electronic structure for M (II) elements.
Nance, Lewis E. J. Chem. Educ. 1984, 61, 339.
Transition Elements |
Metals |
Oxidation State |
Atomic Properties / Structure
Presenting the Bohr atom  Haendler, Blanca L.
A more significant consideration of the role of the Bohr theory in the development of quantum mechanics would have many benefits for introductory and advanced chemistry classes.
Haendler, Blanca L. J. Chem. Educ. 1982, 59, 372.
Atomic Properties / Structure |
Quantum Chemistry
Illustrating the problem described by Heisenberg's uncertainty principle  Cosser, Ronald C.
A simple overhead projector demonstration illustrating Heisenberg's Uncertainty Principle.
Cosser, Ronald C. J. Chem. Educ. 1982, 59, 300.
Atomic Properties / Structure
Groups and subgroups in the periodic table of the elements: A proposal of modification in the nomenclature  Araneo, Antonio
A proposal to eliminate the "A" and "B" designations of subgroups and replace them with letters referring directly to the electronic structures of atoms.
Araneo, Antonio J. Chem. Educ. 1980, 57, 784.
Periodicity / Periodic Table |
Nomenclature / Units / Symbols |
Atomic Properties / Structure
Electrons, bonding, orbitals, and light: A unified approach to the teaching of structure and bonding in organic chemistry courses  Lenox, Ronald S.
A suggested list of topics and methods for teaching introductory organic students bonding concepts.
Lenox, Ronald S. J. Chem. Educ. 1979, 56, 298.
Atomic Properties / Structure |
Lewis Structures |
Spectroscopy |
Covalent Bonding
Questions [and] Answers  Campbell, J. A.
303-308. Six practical, environmental chemistry application questions and their answers. Q303 submitted by Jerry Ray Dias.
Campbell, J. A. J. Chem. Educ. 1977, 54, 369.
Enrichment / Review Materials |
Metals |
Toxicology |
Coordination Compounds |
Membranes |
Aqueous Solution Chemistry |
Atomic Properties / Structure
Chemical aspects of Bohr's 1913 theory  Kragh, Helge
The chemical content of Bohr's 1913 theory has generally been neglected in the treatises on the history of chemistry; this paper regards Bohr as a theoretical chemist and discusses the chemical aspects of his atomic theory.
Kragh, Helge J. Chem. Educ. 1977, 54, 208.
Periodicity / Periodic Table |
Atomic Properties / Structure |
Molecular Properties / Structure |
Covalent Bonding |
Theoretical Chemistry
Simple models for tough concepts  Cavagnol, Richard M.; Barnett, Thomas
One of the most challenging aspects of instructional interaction is the presentation of dynamic chemical concepts interaction is the presentation of dynamic chemical concepts in a way that is both believable and understandable. The authors have devised a series of models that are simple, inexpensive, and require very little time or skill to construct. They allow students to visualize a whole spectrum of phenomena from atomic structure to enzyme-substrate interactions.
Cavagnol, Richard M.; Barnett, Thomas J. Chem. Educ. 1976, 53, 643.
Enzymes |
Molecular Modeling |
Molecular Mechanics / Dynamics |
Atomic Properties / Structure |
Transport Properties
d orbitals in main group elements  Brill, T. B.
An exposition on some of the reasons there are questions regarding the involvement of d orbitals in bonding among the main group elements and several alternative explanations for using d orbitals in this respect.
Brill, T. B. J. Chem. Educ. 1973, 50, 392.
Main-Group Elements |
Atomic Properties / Structure
Transparent 3-D models of electron probability distributions  McClellan, A. L.
The authors describe transparent, three-dimensional models in which regions of high electron probability seem to float in space, without definite boundaries and with the "internal" variations of probability density clearly visible.
McClellan, A. L. J. Chem. Educ. 1970, 47, 761.
Atomic Properties / Structure |
Molecular Modeling
On the discovery of the electron  Morrow, B. A.
Thomson's experiment resolved the controversy concerning the corpuscular or wave nature of cathode rays, while Millikan's experiment resolved the controversy concerning the continuous or discrete nature of electrical phenomena.
Morrow, B. A. J. Chem. Educ. 1969, 46, 584.
Atomic Properties / Structure
Increased-valence theory of valence  Harcourt, R. D.
Describes several "increased valence" formulas for molecular systems with one or more sets of pour electrons distributed among three atomic orbitals of three atoms.
Harcourt, R. D. J. Chem. Educ. 1968, 45, 779.
Atomic Properties / Structure |
Valence Bond Theory
The electron repulsion theory of the chemical bond. I. New models of atomic structure  Luder, W. F.
Describes the electron repulsion theory of electron configuration and applies it to representative elements.
Luder, W. F. J. Chem. Educ. 1967, 44, 206.
Atomic Properties / Structure |
Covalent Bonding |
Metals
V - Atomic orbitals  Berry, R. Stephen
Examines atomic orders of magnitude and the Bohr atom, matter waves, one- and many-electron systems, and the correlation problem.
Berry, R. Stephen J. Chem. Educ. 1966, 43, 283.
Atomic Properties / Structure |
Quantum Chemistry
Atomic orbitals: Limitations and variations  Cohen, Irwin; Bustard, Thomas
The three most widely used methods of arriving at a set of atomic orbitals afford respective hydrogen-like orbitals, self-consistent field orbitals, and various analytical approximations such as the Slater or Morse orbitals, all of which may differ greatly in shape and size from each other.
Cohen, Irwin; Bustard, Thomas J. Chem. Educ. 1966, 43, 187.
Atomic Properties / Structure |
Quantum Chemistry
Tangent-sphere models of molecules. III. Chemical implications of inner-shell electrons  Bent, Henry A.
While a study of atomic core sizes might seem to hold little promise of offering interesting insights into the main body of chemical theory, it is demonstrated here that from such a study emerges a picture of chemical bonding that encompasses as particular cases covalent, ionic, and metallic bonds.
Bent, Henry A. J. Chem. Educ. 1965, 42, 302.
Atomic Properties / Structure |
Molecular Properties / Structure |
Molecular Modeling |
Covalent Bonding |
Ionic Bonding |
Metallic Bonding
Behavior of electrons in atoms: Structure, spectra, and photochemistry of atoms (Hochstrasser, Robin M.)  Gregory, N. W.

Gregory, N. W. J. Chem. Educ. 1965, 42, 62.
Atomic Properties / Structure |
Photochemistry |
Spectroscopy |
Quantum Chemistry
Atomic structure and chemical bonding (Seel, F.; Greenwood, N. N.; Stadler, H. P.)  Murmann, R. Kent

Murmann, R. Kent J. Chem. Educ. 1964, 41, 518.
Atomic Properties / Structure |
Covalent Bonding |
Metallic Bonding |
Ionic Bonding |
Noncovalent Interactions
Electronic structure, properties, and the periodic law (Sisler, Harry H.)  Eblin, Lawrence P.

Eblin, Lawrence P. J. Chem. Educ. 1964, 41, 172.
Periodicity / Periodic Table |
Atomic Properties / Structure
Contour surfaces for atomic and molecular orbitals  Ogryzlo, E. A.; Porter, Gerald B.
Describes the determination of and illustrates contour surfaces for atomic and molecular orbitals.
Ogryzlo, E. A.; Porter, Gerald B. J. Chem. Educ. 1963, 40, 256.
Atomic Properties / Structure |
Molecular Properties / Structure |
Molecular Modeling
Atomic spectra (Kuhn, H. G.)  Strickler, S. J.

Strickler, S. J. J. Chem. Educ. 1962, 39, A918.
Spectroscopy |
Atomic Properties / Structure
Paddle-wheel Crookes tube  Campbell, J. A.
The effect in the Crookes paddle-wheel tube is the same as in the light radiometer and should be interpreted in the same way.
Campbell, J. A. J. Chem. Educ. 1961, 38, 480.
Atomic Properties / Structure
Electronic configuration of metal oxides  O'Reilly, D. E.
Examines the properties of metal oxides in light of crystal field theory, covalency, catalysis, and energy bands.
O'Reilly, D. E. J. Chem. Educ. 1961, 38, 312.
Atomic Properties / Structure |
Metals |
Transition Elements |
Crystal Field / Ligand Field Theory |
Catalysis
The structure of the nucleus  Flowers, B. H.
Describes the liquid drop, shell, and optical models of the atomic nucleus.
Flowers, B. H. J. Chem. Educ. 1960, 37, 610.
Atomic Properties / Structure
The coordinate bond and the nature of complex inorganic compounds. I. The formation of single covalent bonds  Busch, Daryle H.
The factors determining the stabilities of complex inorganic compounds are considered in terms of thermochemical cycle; it is pointed out that the stabilities of complexes increase as the percent covalent character in their bonds increases, and weak covalent bonds will occur in any given instance.
Busch, Daryle H. J. Chem. Educ. 1956, 33, 376.
Coordination Compounds |
Covalent Bonding |
Metals |
Atomic Properties / Structure
Atomic structure and the photoelectric effect  Brockett, Clyde P.
The ubiquitous and inexpensive 110-volt, 2-watt neon glow lamp appears to have been overlooked as a device well suited to a brief but telling demonstration of a few key principles of atomic structure that underlie the study of electrovalence and comparative chemistry.
Brockett, Clyde P. J. Chem. Educ. 1953, 30, 498.
Atomic Properties / Structure
Electronegativities in inorganic chemistry  Sanderson, R. T.
This is the first of a series of short papers intended to demonstrate the application of a broadened concept of electronegativity toward explaining chemistry.
Sanderson, R. T. J. Chem. Educ. 1952, 29, 539.
Atomic Properties / Structure
A space model of the periodic system of elements  Clauson, Jennie E.
Illustrates a three-dimensional model of the periodic system of elements.
Clauson, Jennie E. J. Chem. Educ. 1952, 29, 250.
Periodicity / Periodic Table |
Atomic Properties / Structure
The periodic table: The 6d-5f mixed transition group  Coryell, Charles D.
With relatively few modifications, the Bohr-type periodic table presented by Glocker and Popov can be made to reflect more instructively the rather complex relationships obtained in the neighborhood of the 4f or gadolinium transition group and, more importantly, in the 6d-5f sequence extending from actinium through the region of uranium and the synthetic earths to element 103.
Coryell, Charles D. J. Chem. Educ. 1952, 29, 62.
Periodicity / Periodic Table |
Transition Elements |
Atomic Properties / Structure
Atomic structure models for clay minerals  Perkins, Alfred T.
Describes the use of ceramic clay to produce atomic structure models for clay minerals.
Perkins, Alfred T. J. Chem. Educ. 1951, 28, 388.
Atomic Properties / Structure