Physical Chemistry

TRAMA

Every chemist should own a copy of this uniquely thorough yet incisive treatment of the basic principles of physical chemistry. Written by three eminent physical chemists, the second edition of this exceptional work is the most lucid and comprehensive physical chemistry reference available.<BR>The authors present the fundamentals of the three major areas of physical chemistry--the microscopic structure of matter, the equilibrium properties of systems, and the physical and chemical kinetics of transformations of systems--in a logical sequence, from the simple to the complex. Beginning with<BR>atomic and molecular structure, they progress to properties of condensed matter, to statistical and thermodynamic properties of systems in equilibrium, and then to transport phenomena and chemical reaction processes. The book's mathematical level begins with elementary calculus and rises to the use<BR>of simple properties of partial differential equations and the special functions that enter into their solutions. The conceptual structure of physical chemistry is emphasized throughout and appendices develop the details of the mathematical tools as they are needed. <BR>This new edition features: <BR>DT In-depth and illuminating presentation of conceptual arguments <BR>DT No shortcuts--derives whole formulas <BR>DT 100 new problems <BR>DT New material on nuclear magnetic resonance <BR>DT Expanded treatment of linear and nonlinear irreversible processes and thermodynamics <BR>DT A completely revised treatment of electrode kinetics <BR>DT Many updates throughout <BR>DT Several vignettes--written by leaders in the field--that cover topics at the cutting edge of physical chemistry research

NOTE EDITORE

The authors' goal is the presentation of the three major areas of physical chemistry: molecular structure, the equilibrium properties of systems, and the kinetics of transformations of systems. The theoretical foundations of these subjects are, respectively, quantum mechanics, thermodynamics and equilibrium statistical mechanics, and chemical kinetics and kinetic theory. These theories, firmly based on experimental findings, constitute the structure required for the understanding of past accomplishments and the basis for recognition and development of significant new areas in physical chemistry. The presentation of the theories of physical chemistry requires careful discussions at several levels of exposition. The authors' approach aims toward depth of understanding of fundamentals more than toward breadth of recognition of the multitude of activities that go on under the name of physical chemistry. The organization of the book, with its three principal sections, should make this clear. The mathematical level begins with elementary calculus, and rises to the use of simple properties of partial differential equations and the special functions that enter into their solutions. The authors' intention is to keep the reader's mind on the scienc rather than on the mathematics, especially at the beginning. This procedure also corresponds to the pattern, followed by many students, of taking physical chemistry and advanced calculus concurrently. Appendices develop the details of the mathematical tools as they are needed. The text discussion contains more material than can be covered in the traditional one-year physical chemistry sequence; it is designed to fulfill the dual purpose of providing a clear and incisive treatment of fundamental principles at a level accessible to all students while broadening the perspectives and challenging the minds of the best students. Individual instructors will wish to make their own selections of material for inclusion and exclusion, respectively.

SOMMARIO

1.1 - Development of the Atomic Theory: Relative Atomic Weights1.2 - Atomic Magnitudes1.3 - The Charge-to-Mass Ratio of the Electron: Thomson's Method1.4 - The Charge of the Electron: Millikan's Method1.5 - Mass Spectrometry1.6 - The Atomic Mass Scale and the Mole1.7 - The Periodic Table2.1 - The Franck-Hertz Experiment2.2 - The Photoelectric Effect2.3 - x Rays and Matter2.4 - The Emission Spectra of Atoms2.5 - The Nuclear Atom2.6 - The Problem of Black-Body Radiation2.7 - The Concept of Action2.8 - The Harmonic Oscillator2.9 - Action Quantized: The Heat Capacity of Solids2.10 - Some Orders of Magnitude2.11 - Bohr's Model of the Atom3.1 - The de Broglie Hypothesis3.2 - The Nature of Waves3.3 - Dispersion Relations and Wave Equations: The Free Particle3.4 - Operators3.5 - Eigenfunctions and Eigenvalues3.6 - The Particle in a One-Dimensional Box3.7 - The Interdeterminacy or Uncertainty Principle3.8 - Expectation Values; Summary of Postulates3.9 - Particles in Two- and Three-Dimensional Boxes3.10 - Particles in Circular Boxes3.11 - Particles in Spherical Boxes3.12 - The Rigid Rotor4.1 - Finite Potential Barriers4.2 - The Quantum Mechanical Harmonic Oscillator4.3 - The Hydrogen Atom4.4 - The Shapes of Orbitals4.5 - Transitions Between Energy Levels5.1 - Electron Spin; Magnetic Phenomena5.2 - The Pauli Exclusion Principle; the Aufbau Principle5.3 - Electronic Configuration of Atoms5.4 - Calculation of Atomic Structures5.5 - Atomic Structure and Periodic Behavior5.6 - Term Splitting and the Vector Model5.7 - Fine Structure and Spin--Orbit Interactions6.1 - Bonding Forces Between Atoms6.2 - The Simplest Molecule: The Hydrogen Molecule-Ion, H2+6.3 - H2+: Molecular Orbitals and the LCAO Approximation6.4 - H2+: Obtaining the Energy Curve6.5 - H2+: Correlation of Orbitals; Excited States6.6 - The H2 Molecule: Simple MO Description6.7 - Symmetry Properties of Identical Particles6.8 - H2: The Valence BOnd Representation6.9 - H2: Beyond the Simple MO and VB Approximations6.10 - H2: Excited Electronic States7.1 - Vibrations of Diatomic Molecules7.2 - Rotations of Diatomic Molecules7.3 - Spectra of Diatomic Molecules7.4 - The Ionic Bond7.5 - Homonuclear Diatomic Molecules: Molecular Orbitals and Orbital Correlation7.6 - Homonuclear Diatomic Molecules: Aufbau Principle and the Structure of First-Row Molecules7.7 - Introduction to Heteronuclear Diatomic Molecules: Electronegativity7.8 - Bonding in LiH: Crossing and Noncrossing Potential Curves7.9 - Other First-Row Diatomic Hydrides7.10 - Isoelectronic and Other Series8.1 - Electronic Structure and Geometry in the Simplest Cases: H3 and H3+8.2 - Dihydrides: Introduction to the Water Molecule8.3 - Hybrid Orbitals8.4 - Delocalized Orbitals in H2O: The General MO Method8.5 - Bonding in More Complex Triatomic Molecules8.6 - Normal Coordinates and Modes of Vibration8.7 - A Solvable Example: The Vibrational Modes of CO28.8 - Transition and Spectra of Polyatomic Molecules9.1 - Small Molecules9.2 - Catenated Carbon Compounds; Transferability9.3 - Other Extended Structures9.4 - Some Steric Effects9.5 - Complex Ions and Other Coordination Compounds: Simple Polyhedra9.6 - Chirality and Optical Rotation9.7 - Chiral and Other Complex Ions9.8 - Magnetic Properties of Complexes9.9 - Electronic Structure of Complexes10.1 - Long-Range Forces: Interactions Between Charge Distributions10.2 - Empirical Intermolecular Potentials10.3 - Weakly Associated Molecules11.1 - Some General Properties of Solids11.2 - Space Lattices and Crystal Symmetry11.3 - x Ray Diffraction from Crystals: The Bragg Model11.4 - The Laue Model11.5 - Determination of Crystal Structures11.6 - Techniques of Diffraction11.7 - Molecular Crystals11.8 - Structures of Ionic Crystals11.9 - Binding Energy of Ionic Crystals11.10 - Covalent Solids11.11 - The Free-Electron Theory of Metals11.12 - The Band Theory of Solids11.13 - Conductors, Insulators, and Semicondutors11.14 - Other Forms of Condensed Matter12.1 - The Perfect Gas: Definition and Elementary Model12.2 - The Perfect Gas: A General Relation Between Pressure and Energy12.3 - Some Comments About Thermodynamics12.4 - Temperature and the Zeroth Law of Thermodynamics12.5 - Empirical Temperature: The Perfect Gas Temperature Scale12.6 - Comparison of the Microscopic and Macroscopic Approaches13.1 - Microscopic and Macroscopic Energy in a Perfect Gas13.2 - Description of Thermodynamic States13.3 - The Concept of Work in Thermodynamics13.4 - Intensive and Extensive Variables13.5 - Quasi-static and Reversible Processes13.6 - The First Law: Energy and Heat13.7 - Some Historical Notes13.8 - Microscopic Interpretation of Internal Heat and Energy13.9 - Constraints, Work, and Equilibrium14.1 - Heat Capacity and Enthalpy14.2 - Energy and Enthalpy Changes in Chemical Reactions14.3 - Thermochemistry of Physical Processes14.4 - Introduction to Phase Changes14.5 - Standard States14.6 - Thermochemistry of Solutions14.7 - Molecular Interpretation of Physical Processes14.8 - Bond Energies14.9 - Some Energy Effects in Molecular Structures14.10 - Lattice Energies of Ionic Crystals15.1 - The Relationship Between Average Propertis and Molecular Motion in an N-Molecule System: Time Averages and Ensemble Averages15.2 - Ensembles and Probability Distributions15.3 - Some Properties of a System with Many Degrees of Freedom: Elements of the Statistical Theory of Matter at Equilibrium15.4 - The Influences of Constraints on the Density of States15.5 - The Entropy: A Potential Function for the Equilibrium State16.1 - The Second Law of Thermodynamics16.2 - The Existence of an Engropy Function for Reversible Processes16.3 - Irreversible Processes: The Second Law Interpretation16.4 - The Clausius and Kelvin Statements Revisited16.5 - The Second Law as an Inequality16.6 - Some Relationships Between the Microscopic and Macroscopic Theories17.1 - Choice of Independent Variables17.2 - The Available Work Concept17.3 - Entropy Changes in Reversible Processes17.4 - Entropy Changes in Irreversible Processes17.5 - Entropy Changes in Phase Transitions18.1 - The Magnitude of the Entropy at T=018,2 - The Unattainability of Absolute Zero18.3 - Experimental Verification of the Third Law19.1 - Properties of the Equilibrium State of a Pure Substance19.2 - Alternative Descriptions of the Equilibrium State for Different External Constraints19.3 - The Stability of the Equilibrium State of a One-Component System19,4 - The Equilibrium State in a Multicomponent System19.5 - Chemical Equilibrium19.6 - Thermodynamic Weight: Further Connections Between Thermodynamics and Microscopic Structure19.7 - An Application of the Canonical Ensemble: The Distribution of Molecular Speeds in a Perfect Gas20.1 - General Form of the Equation of Continuity20.2 - Conservation of Mass and the Diffusion Equation20.3 - Conservation of Momentum and the Navier-Stokes Equation20.4 - Conservation of Energy and the Second Law of Thermodynamics20.5 - Linear Transport Processes20.6 - Negative Temperature20.7 - Thermodynamics of Systems at Negative Absolute Temperature21.1 - Thermodynamic Descripti

ALTRE INFORMAZIONI

• Condizione: Nuovo
• ISBN: 9780195105896
• Collana: Topics in Physical Chemistry
• Dimensioni: 218 x 55.9 x 279 mm Ø 2517 gr
• Formato: Copertina rigida
• Illustration Notes: 7 halftones, numerous line illustrations
• Pagine Arabe: 1080