Mechanism and Theory in Organic Chemistry |
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Page 2
... atoms to share pairs of elec- trons . Ordinarily , a shared pair is designated by a line : H - H All valence electrons of all atoms in the structure must be shown explicitly . Those electrons not in shared covalent bonds are indicated ...
... atoms to share pairs of elec- trons . Ordinarily , a shared pair is designated by a line : H - H All valence electrons of all atoms in the structure must be shown explicitly . Those electrons not in shared covalent bonds are indicated ...
Page 13
... atoms were radically different , since in that case different pictures would be required for each atom . But the feature of the hydrogen atom problem that determines the most important characteristics of the hydrogen atom orbitals is ...
... atoms were radically different , since in that case different pictures would be required for each atom . But the feature of the hydrogen atom problem that determines the most important characteristics of the hydrogen atom orbitals is ...
Page 130
... atomic number of the directly bonded atom , the higher is the priority . If two atoms are isotopes , the one with higher atomic mass has higher priority . An unshared pair of electrons is treated as a ligand atom of atomic number zero ...
... atomic number of the directly bonded atom , the higher is the priority . If two atoms are isotopes , the one with higher atomic mass has higher priority . An unshared pair of electrons is treated as a ligand atom of atomic number zero ...
Contents
THE COVALENT BOND | 1 |
Molecular Orbital Theory | 87 |
SOME FUNDAMENTALS OF PHYSICAL | 127 |
Copyright | |
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acetic acid-base acidity function addition alkene alkyl American Chemical Society anion Arnett aromatic atomic orbitals atoms base Brønsted C-X bond carbanion carbon carbonyl catalysis cation CH₂ CH3 CH3 charge Chem coefficients compounds configuration conjugate conjugate acid Copyright correlation delocalized diagram dissociation double bond electron electrophilic equilibrium constant example Figure free energy gas-phase H H H H₂O HOMO hydrogen interaction intermediate ion pair ionization isotope effect Jencks k₁ kcal kcal mol¹ kinetic kJ mol¯¹ leaving group LUMO mechanism methyl mol-¹ molecular orbitals molecule nucleophile occur Olah Organic Chemistry oxygen parameters phenyl Phys potential energy proton proton transfer racemic rate constant rate-determining ratio reactants reaction coordinate reactive rearrangement relative resonance ring Scheme Schleyer shown in Equation solution solvation solvent solvolysis stabilization steric Streitwieser structure substituents substitution substrate symmetry Table tion tosylate transition values vibrational Wiley Winstein York