3 edition of Electronic structure and chemical bonding found in the catalog.
Electronic structure and chemical bonding
Donald K. Sebera
Includes bibliographies and index.
|Statement||Donald K. Sebera.|
|The Physical Object|
|Pagination||ix, 298 p. :|
|Number of Pages||298|
This innovative text offers basic understanding of the electronic structure of covalent and ionic solids, simple metals, transition metals and their compounds. It also explains how to calculate dielectric, conducting, and bonding properties for each. Includes a . Boron-based heterocyclic clusters are intuitively even more electron-deficient and feature exotic chemical bonding, which make use of O 2p, S 3p, or N 2p lone-pairs for π delocalization over heterocyclic rings, facilitating new cluster structures and new types of bonding.
Chemical bonding, any of the interactions that account for the association of atoms into molecules, ions, crystals, and other stable species that make up the familiar substances of the everyday atoms approach one another, their nuclei and electrons interact and tend to distribute themselves in space in such a way that the total energy is lower than it would be in . This series presents critical reviews of the present position and future trends in modern chemical research concerned with chemical structure and bonding ; Short and concise reports, each written by the world's renowned experts ; Still valid and useful after 5 or 10 years.
CHAPTER 1 Electronic Structure and Covalent Bonding 1. The mass number =the number ofprotons +thenumber ofneutrons The atomic number =the number ofprotons. All isotopes ofaspecific element have thesame atomic number; theatomic number ofoxygen is8. Therefore: The isotope ofoxygen with amass number of 16has 8protons and 8neutrons. The book illuminates the relationships of the electronic structures of these materials and shows how to calculate dielectric, conducting, and bonding properties for each. Also described are various methods of approximating electronic structure, providing insight and even quantitative results from the comparisons.
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Classification of Chemical Bonds by Electronic Structure and Role of d and f Electrons in Coordination Bonding Qualitative Aspects and Electronic Configurations. Ligand Bonding. Energies, Geometries, and Charge Distributions. Relativistic Effects. Summary Notes. Exercises and Problems.
References. Crystal field theory was originally developed to describe the structure of metal ions in crystals. The energies of the d orbitals are split by electrostatic field. This was developed in the s, which ignored the covalent bonding since ionic crystals didn't describe it.
When the ligands come close to the metal, a big destabilization occurs. Publisher Summary. This chapter demonstrates how X-ray and electron spectroscopies can be used together with Density Functional Theory (DFT) calculations to obtain an understanding of the local electronic structure and chemical bonding of adsorbates on metal surfaces.
This book addresses the problem of teaching the Electronic Structure and Chemical Bonding of atoms and molecules to high school and university students. It presents the outcomes of thorough investigations of some teaching methods as well as an unconventional didactical approach which were developed.
Molecular orbital theory is used to explain the electronic structure of molecules, which is, of course, of fundamental importance to the chemist. Bonding theories for organic and inorganic models are developed and a brief treatment is given on the solid state at the end of the by: Chemical bonding - Chemical bonding - Atomic structure and bonding: To understand bond formation, it is necessary to know the general features of the electronic structure of atoms—that is, the arrangement of electrons around the central nucleus.
For background information about this subject and further details, see atom. The modern version of atomic structure begins with.
This book addresses the problem of teaching the Electronic Structure and Chemical Bonding of atoms and molecules to high school and university students. It presents the outcomes of thorough investigations of some teaching methods as well as an unconventional didactical approach which were developed during a seminar for further training.
The book illuminates the relationships of the electronic structures of these materials and shows how to calculate dielectric, conducting, and bonding properties for each. Also described are various methods of approximating electronic structure, providing insight and even quantitative results from the by: Chemical Binding and Structure describes the chemical binding and structure in terms of current chemical theory.
This book is composed of 13 chapters, and starts with a presentation of the principles of the old and modified quantum theory and its application. The next chapters cover some basic topics related to chemical binding and structure.
Electronic Structure of the Atom and Chemical Bonding Structure of the Atom In general chemistry, we focus on three subatomic particles that make up all atoms. These are the electron, proton, and neutron. We will not find it necessary to sort out the "particle zoo" that is the realm of particle physics.
Additional Physical Format: Online version: Sebera, Donald K. (Donald Keith), Electronic structure and chemical bonding. New York, Blaisdell Pub. For teachers and high-school and university students, this work addresses the problem of teaching the electronic structure and chemical bonding of atoms and molecules.
It presents the outcomes of thorough investigations of some teaching methods as well as an unconventional didactic approach. The Nature of Chemical Bonds- Molecular Orbital Theory Molecular Orbital theory (MO) is a more advanced bonding model than Valence Bond Theory, in which two atomic orbitals overlap to form two molecular orbitals – a bonding MO and an.
The LibreTexts libraries are Powered by MindTouch ® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot.
We also acknowledge previous National Science Foundation support under grant numbers. General Chemistry I. This book covers the following topics: Matter and Measurement, Atoms, Molecules and Ions, Aqueous Reactions and Solution Stoichiometry, Chemical Reactions and Reaction Stoichiometry, Thermochemistry, Chemical Bonding, Periodic Properties of the Elements, Electronic Structure of Atoms, Molecular Geometries and Bonding Theories, Gases.
Novel material is introduced in description of multi-orbital chemical bonding, spectroscopic and magnetic properties, methods of electronic structure calculation, and quantum-classical modeling for organometallic and metallobiochemical systems.
Greater the bond order, greater is the stability of the bond during chemical bonding i.e. greater is the bond enthalpy.
Greater the bond order, shorter is the bond length. Resonance in Chemical Bonding. There are molecules and ions for which drawing a single Lewis structure is not possible. For example, we can write two structures of O 3. Show no bonding pairs or lone pairs (lone pairs are an exception when they are needed to draw attention to some chemical property of the molecule) *IMPORTANT: Even though lone pairs are not shown in these Kekulé/Condensed Structures, you must remember that neutral nitrogen, oxygen, and halogen atoms ALWAYS have them - 1 pair for nitrogen, 2.
Structure and Bonding is a publication which uniquely bridges the journal and book format. Organized into topical volumes, the series publishes in depth and critical reviews on all topics concerning structure and bonding. and the electronic properties of metal ions involved in important biochemical enzymatic reactions.
The Molecular Orbital Theory of Electronic Structure. and Ions. Electronic Structures Photoelectron Spectroscopy. Other editions - View all. Chemical structure and bonding Roger L.
DeKock, Harry B. Gray Snippet view - Chemical structure and bonding All Book Search results » About the author () ROGER L 5/5(1). Ionic Bonding. Covalent Bonding. Chemical Nomenclature. Lewis Symbols and Structures.
Formal Charges and Resonance. Molecular Structure and Polarity. 5 Advanced Theories of Bonding. Valence Bond Theory. Hybrid Atomic Orbitals. Multiple Bonds. Molecular Orbital Theory. 6 Composition of Substances and.When drawing a Lewis structure, we used a pair of valence electrons from each nucleus in the molecule to form a chemical bond.
We also talked about formation of chemical bond in H 2 from two hydrogen atoms; two 1 s orbitals approach each other with overlapping tails, which gave rise to bonding and antibonding orbitals.This book covers the following topics: Matter and Measurement, Atoms, Molecules and Ions, Aqueous Reactions and Solution Stoichiometry, Chemical Reactions and Reaction Stoichiometry, Thermochemistry, Chemical Bonding, Periodic Properties of the Elements, Electronic Structure of Atoms, Molecular Geometries and Bonding Theories, Gases.