Default Header Image

Chemistry 205: Physical Chemistry

Course Level: 
Second Year
Academic Year: 

TEXTBOOKPhysical Chemistry for the Biosciences by Raymond Chang.

I. THERMODYNAMICS: (13-14 lecture hours)

1. Introduction

1.1 Ideal Gas Equation of State
1.2 Internal Energy and Temperature
1.3 Real Gas (Van der Waals)

2. Laws of Thermodynamics Revisited

2.1 First Law (Heat and Work)
2.2 Second Law (reversible and irreversible processes)
2.3 Entropy (Order and Chaos)
2.4 Equilibrium and Spontaneity
2.5 Free Energy (Gibbs)
2.6 Third Law (Absolute Zero concept)

3. Phase Equilibria

3.1 Pressure vs. Temperature Phase Diagrams (simple one component systems)

4. Gibbs Free Energy and Chemical Equilibrium

5. Thermodynamics of Electrochemical Cells

5.1 Electrical Work and Cell Thermodynamics
5.2 Conventions, Electrode Types and Applications

6. Colligative Properties and Donnan Membrane Equilibrium and Potential

II. KINETICS: (11-12 lecture hours)

1. Chemical Kinetics

1.1 Meaning of "Rate"
1.2 Steps to Studying Rate Processes
1.3 Integration of the Rate Equation

1.3.1 Zero Order Reaction
1.3.2 First Order Reaction
1.3.3 Second Order Reaction
1.3.4 General Reaction of Order n

2. Temperature Dependence of Reaction Rates

2.1 Arrhenius Equation
2.2 Collision Theory (brief discussion)
2.3 Transition State Theory (brief discussion)

3. More Complicated Rate Processes

3.1 Parallel and Consecutive Reactions
3.2 Reversible Reactions and Approach to Equilibrium

4. Reaction Mechanisms

4.1 Introduction and Steady State Approximations
4.2 Selected Examples

5. Enzyme Catalysis

5.1 General Introduction to Catalysis
5.2 The Michaelis-Menten Mechanism
5.3 Alternative forms of Michaelis-Menten Equation


1. Review

1.1 Atomic Spectroscopy (quantized energy concepts)
1.2 Atomic orbital functions and quantum numbers

2. Infrared Spectroscopy

2.1 Vibrational energy levels
2.2 Frequency vs. Wavenumber
2.3 Functional Group Analysis ( OH, NH, C=O etc)
2.4 FT-IR

3. Nuclear Magnetic Resonance Spectroscopy

3.1 Introduction to NMR Theory
3.2 Proton NMR and Chemical Shift
3.3 Proton NMR and Spin-Spin Coupling
3.4 13 C-NMR
3.5 Magnetic Resonance Imaging (MRI) ƒ brief introduction

4. UV/Visible Spectroscopy

4.1 Molecular orbitals (sigma and pi bonding/antibonding and non-bonding orbitals)
4.2 Beer's Law
4.3 Uses in High Pressure Liquid Chromatography (HPLC) as a detector

5. Mass Spectrometry

5.1 Brief review of the analytical capabilities of the technique

Marking Scheme

Final Examination 65%
Mid Term 20%
Quizzes 15%