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By Milton Orchin, Roger S. Macomber, Allan R. Pinhas, R. Marshall Wilson
This ebook is a easy reference offering concise, exact definitions of the most important phrases and ideas of natural chemistry. now not easily an inventory of natural compounds, buildings, and nomenclatures, the publication is equipped into topical chapters during which similar phrases and ideas seem in shut proximity to each other, giving context to the data and supporting to make high-quality differences extra comprehensible. components coated contain: bonding, symmetry, stereochemistry, sorts of natural compounds, reactions, mechansims, spectroscopy, and photochemistry.
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Additional info for The Vocabulary and Concepts of Organic Chemistry
Sample text
Despite the merits of the VB approach with its emphasis on the electron pair bond, the theory has several drawbacks even for the description of the bonding in some simple molecules such as dioxygen, O2. qxd 5/17/2005 5:13 PM Page 27 CHEMICAL BOND 27 diamagnetic, which it is not. On the other hand, according to the MO description, the two highest occupied molecular orbitals of O2 are degenerate and antibonding and each contains one electron with identical spin, thus accounting for the observed paramagnetism, the most unusual property of dioxygen.
51 σ Bonding Molecular Orbital (σ Orbital); σ Bond σ Antibonding Molecular Orbital (σ* Orbital) pπ Atomic Orbital π Bonding Molecular Orbital (π Orbital) Localized π Bond π Antibonding Molecular Orbital (π* Orbital) σ Skeleton Molecular Orbital Energy Diagram (MOED) Electronic Configuration of Molecules MOED for 2nd Row Homodiatomic Molecules MOED for the 2nd Row Heteroatomic Molecule; Carbon Monoxide Coefficients of Atomic Orbitals cij Normalized Orbital Normalization Orthogonal Orbitals Orthonormal Orbitals Wave Functions in Valence Bond (VB) Theory 44 45 45 45 46 46 47 47 48 48 50 50 51 52 52 52 52 Electrons are the cement that binds together atoms in molecules.
A diatomic molecule in which the electrons are not shared equally gives rise to a dipole moment vector with a negative end and a positive end along the bond connecting the two atoms. Therefore, such a molecule acts as a dipole and tends to become aligned in an electrical field. The (electric) dipole moment µ (see also Sect. 31) is obtained by multiplying the charge at either atom (pole) q (in electrostatic units or esu) by the distance d (in centimeters) between the atoms (poles): q × d ϭ µ (in esu-cm).