2.6. How Are the Electrons in an Atom Arranged?, 49
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Paramagnetism: Compounds Vials of a number of compounds (NaCl, MnSO4, FeSO4, CoCl2, NiSO4, ZnSO4, K4Fe(CN)6, [Co(NH3)6]Cl3, [Ni(NH3)6]Cl2, and H2O) are hung from a thread. When a magnet is brought near, some of the vials are attracted.
Magnetic Properties |
Atomic Properties / Structure
Paramagnetism: Oxidation States of Manganese Manganese(III) oxide, with 4 unpaired electrons per Mn atom, is more strongly attracted to a magnet than is manganese(IV) oxide, with only 3 unpaired electrons per Mn atom. Potassium permanganate, a compound of Mn(VII), has no unpaired electrons and is not attracted to a magnet.
An incomplete concept map is shown below, which set of terms for A, B, C and D would result in a correct map based on the concept of wave mechanics applied to a hydrogen atom?
Trends in Ionization Energy of Transition-Metal ElementsPaul S. Matsumoto Examines why, as the number of protons increase along a row in the periodic table, the first ionization energies of the transition-metal elements are relatively steady, but that for the main-group elements increases. Matsumoto, Paul S. J. Chem. Educ.2005, 82, 1660.
Atomic Properties / Structure |
Periodicity / Periodic Table |
Transition Elements
A Program of Computational Chemistry Exercises for the First-Semester General Chemistry CourseScott E. Feller, Richard F. Dallinger, and Paul Caylor McKinney A series of 13 molecular modeling exercises designed for the first-semester general chemistry course is described. The modeling exercises, which are used as both prelecture explorations and postlecture problems, increase in difficulty and in student independence. Feller, Scott E.; Dallinger, Richard F.; McKinney, Paul Caylor. J. Chem. Educ.2004, 81, 283.
Atomic Properties / Structure |
Computational Chemistry |
Molecular Modeling |
Molecular Properties / Structure
Ionization Energies, Parallel Spins, and the Stability of Half-Filled ShellsPeter Cann Three methods for explaining the decrease in first ionization energies between group V and group VI elements are described and commented upon. The quantum mechanical origin of the unhelpful concept of half-shell stability is explained in terms of exchange energy, for which the alternative term parallel spin avoidance factor is suggested. It is recommended that for pre-university students the simplest explanation, in terms of Coulombic repulsion between two electrons occupying the same orbital, is adopted: it involves fewer difficult concepts than the other explanations and its predictions are no less accurate. Cann, Peter. J. Chem. Educ.2000, 77, 1056.
The Amount of Substance: MolesEd Vitz, John W. Moore A section of ChemPrime, the Chemical Educations Digital Library's free General Chemistry textbook.
