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Chem 370: P-Chem 1 for Biophysical and Traditional Students (Gutow)
This text/resource was developed for use in a first semester physical chemistry course meant to accommodate both students needing a one semester biophysical course and traditional chemistry majors who will go on to take a second semester of physical chemistry. Because of this more topics are covered in less depth than a traditional first semester physical chemistry course.
- Author
- Jonathan Gutow
- Publisher
- University of Wisconsin Oshkosh
- Source
- LibreTexts
- License
- CC BY-NC-SA
- Language
- EN
- Category
- Basic Sciences
Contents· 92 sections
- 01: Thermodynamics
- 1.01: Thermodynamic Variables and Equations of State
- 1.02: The First Law of Thermodynamics
- 1.03: Thermochemistry
- 1.04: The Second Law of Thermodynamics
- 1.05: The Boltzmann Distribution and the Statistical Definition of Entropy
- 1.06: The Gibbs and Helmholtz Energy
- 1.07: Phase Equilibria and Mixtures
- 1.08: Colligative Properties
- 1.09: Henry's Law
- 02: Chemical Equilibria
- 2.01: Chemical Equilibria
- 2.02: Composition Dependence of Free Energy (G)
- 2.03: Equilibrium Calculations (ICE) Review
- 2.04: Fractional Composition at Equilibrium
- 2.05: Coupled Equilibria
- 2.06: Equilibrium Dependence on Conditions
- 2.07: Coupled Equilibria Driving Nonspontaneous Reactions
- 2.08: Brnsted-Lowry Acids and Bases
- 2.09: pH and pOH
- 2.10: Acid-Base Equilibria
- 2.11: Hydrolysis of Salts
- 2.12: Polyprotic Acids
- 2.13: Buffers
- 03: Ions and Electrochemistry
- 3.01: Mean Ionic Activity Coefficients and the Debye-Huckel Model
- 3.02: Extending Debye-Huckel Theory to Higher Concentrations
- 3.03: Ion Transport
- 3.04: Review of Redox Chemistry
- 3.05: Half Cells and Standard Reduction Potentials
- 3.06: Cell potentials under non-standard conditions (Nernst equation)
- 3.07: Thermodynamics from Electrochemistry
- 3.08: Redox Examples
- 04: Reaction Kinetics
- 4.01: Reaction Rates and Rate Laws
- 4.02: Measuring Reaction Rates
- 4.03: Determining Rate Laws
- 4.04: Integrated Rate Laws
- 4.05: Examples of Using Graphs to Determine Reaction Order
- 4.06: Temperature Dependence of Rate Constants
- 05: Kinetic Mechanisms 1
- 5.01: Reaction Mechanisms
- 5.02: Relaxation Methods
- 5.03: Representative Reaction Mechanisms
- 5.04: The Rate Determining Step Approximation
- 5.05: The Equilibrium Approximation
- 5.06: The Steady-State Approximation
- 06: Molecular Level Models of Kinetics
- 6.01: Kinetics of Reactions in Solution
- 6.02: Kinetic vs. Thermodynamic Control of Reactions
- 6.03: Collision Theory
- 6.04: Transition State Theory
- 6.05: Reactions Involving Ions
- 07: Kinetic Mechanisms 2
- 7.01: Numerical Modeling of Mechanisms
- 7.02: The Michaelis-Menten Mechanism
- 7.03: The Lindemann Mechanism
- 7.04: Chain Reactions
- 7.05: Catalysis (ozone example)
- 7.06: Oscillating Reactions
- 7.07: Diffusion
- 7.08: Membrane Diffusion
- 7.09: Ion Mobilities
- 7.10: Transport Across Cell Membranes
- 7.11: Kinetics of Electron Transfer Reactions
- 08: Quantum Chemistry Fundamentals
- 8.01: Failures of Classical Physics
- 8.02: The Schrodinger Wave Equation
- 8.03: Particle in a One-Dimensional Box
- 8.04: Tunneling
- 8.05: Particle in a 2-Dimensional Box
- 8.06: Particle on a Ring
- 8.07: The Schrodinger Wave Equation for the Hydrogen Atom
- 8.08: Many-Electron Atoms and the Periodic Table
- 8.09: Harmonic Oscillator
- 09: Molecular Quantum Mechanics
- 9.01: The Born-Oppenheimer Approximation Simplifies the Schrodinger Equation for Molecules
- 9.02: Valence Bond Theory
- 9.03: Hybridization of Atomic Orbitals
- 9.04: Molecular Orbital Theory
- 9.05: Diatomic Molecules With More Than s Orbitals
- 9.06: Huckel MO Model of Conjugation
- 9.07: Benzene and Aromaticity
- 9.08: Numerical QM Methods
- 10: Aggregates and Macromolecules
- 10.01: Mass Spectrometry
- 10.02: X-Ray Crystallography
- 10.03: Cryo-Electron Microscopy
- 10.04: Intermolecular Forces
- 10.05: Structure of Gases Liquids and Glasses
- 10.06: Macromolecules
- 10.07: Simulations