Physical Chemistry (LibreText)
- Page ID
- 589936
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)This Physical Chemistry textbook addressed the study of macroscopic, and particulate phenomena in chemical systems in terms of the principles, practices, and concepts of physics such as motion, energy, force, time, thermodynamics, quantum chemistry, statistical mechanics, analytical dynamics and chemical equilibria. In contrast to chemical physics, physical chemistry is predominantly (but not always) a macroscopic or supra-molecular science, as the majority of the principles on which it was founded relate to the bulk rather than the molecular/atomic structure alone.
- 1: The Dawn of the Quantum Theory
- 1.1: Blackbody Radiation Cannot Be Explained Classically
- 1.2: Quantum Hypothesis Used for Blackbody Radiation Law
- 1.3: Photoelectric Effect Explained with Quantum Hypothesis
- 1.4: The Hydrogen Atomic Spectrum
- 1.5: The Rydberg Formula and the Hydrogen Atomic Spectrum
- 1.6: Matter Has Wavelike Properties
- 1.7: de Broglie Waves can be Experimentally Observed
- 1.8: The Bohr Theory of the Hydrogen Atom
- 1.9: The Heisenberg Uncertainty Principle
- 1.E: The Dawn of the Quantum Theory (Exercises)
- 3: The Schrödinger Equation and a Particle in a Box
- 3.1: The Schrödinger Equation
- 3.2: Linear Operators in Quantum Mechanics
- 3.3: The Schrödinger Equation is an Eigenvalue Problem
- 3.4: Wavefunctions Have a Probabilistic Interpretation
- 3.5: The Energy of a Particle in a Box is Quantized
- 3.6: Wavefunctions Must Be Normalized
- 3.7: The Average Momentum of a Particle in a Box is Zero
- 3.8: The Uncertainty Principle - Estimating Uncertainties from Wavefunctions
- 3.9: A Particle in a Three-Dimensional Box
- 3.E: The Schrödinger Equation and a Particle in a Box (Exercises)
- 3.S: The Schrödinger Equation and a Particle in a Box (Summary)
- 4: Postulates and Principles of Quantum Mechanics
- 4.1: The Wavefunction Specifies the State of a System
- 4.2: Quantum Operators Represent Classical Variables
- 4.3: Observable Quantities Must Be Eigenvalues of Quantum Mechanical Operators
- 4.4: The Time-Dependent Schrödinger Equation
- 4.5: Eigenfunctions of Operators are Orthogonal
- 4.6: Commuting Operators Allow Infinite Precision
- 4.E: Postulates and Principles of Quantum Mechanics (Exercises)
- 4.S: Postulates and Principles of Quantum Mechanics (Summary)
- 5: The Harmonic Oscillator and the Rigid Rotor
- 5.1: A Harmonic Oscillator Obeys Hooke's Law
- 5.2: The Equation for a Harmonic-Oscillator Model of a Diatomic Molecule Contains the Reduced Mass of the Molecule
- 5.3: The Harmonic Oscillator Approximates Molecular Vibrations
- 5.4: The Harmonic Oscillator Energy Levels
- 5.5: The Harmonic Oscillator and Infrared Spectra
- 5.6: The Harmonic Oscillator Wavefunctions involve Hermite Polynomials
- 5.7: Hermite Polynomials are either Even or Odd Functions
- 5.8: The Energy Levels of a Rigid Rotor
- 5.9: The Rigid Rotator is a Model for a Rotating Diatomic Molecule
- 5.E: The Harmonic Oscillator and the Rigid Rotor (Exercises)
- 5.S: The Harmonic Oscillator and the Rigid Rotor (Summary)
Thumbnail: Space-filling model of the LUMO of pyridine. Structure calculated and image produced using HF/6-31G*. (Public Domain; Ben Mills via Wikipedia)