Texts: Chemistry for Engineers: An Applied Approach, by Mary Jane Shultz
Chem 154 Laboratory Manual, by Nussbaum et al.,
“Bridging to the Lab”, by Jones & Tasker.
The first half of this course is focussed on an introduction to chemical ideas which are needed to understand the basic properties of materials. The second half of the course is an introduction to basic thermodynamic ideas useful in working with chemical processes.
Note that the course is defined by the material covered in the lectures, which is not necessarily the same material as in the textbook.
Outline:
Introduction
Foundations (Ch 2) and Physical and Chemical Periodicity (Ch 3)
Electromagnetic Radiation; Line Spectra; Bohr Atom; Atomic Orbitals (s,p,d) and Energy Level Diagrams; Electronic Configurations of the Elements
Shape and Intermolecular Interactions (Ch 6)
Lewis Model of Covalent Bonding; Bond Polarity; Bond Lengths; Molecular Shapes by VSEPR; Molecular Polarity; Intermolecular Forces
Bulk Properties of Matter
Gases; Liquids; Phase Diagrams
Solid State Structures (Ch 4)
Ionic Structures: Common Cubic Crystal Structures NaCl, CsCl, ZnS, CaF2; Network Covalent Crystal Structures; Metals
Electronic Structure and Bonding (Ch 5)
Theories of Chemical Bonding; Valence Bond Theory; Molecular Orbital Theory First Row Diatomics); Band Structure of Solids: Conductivity, Semiconductors
Equilibrium: A Dynamic Steady State (Ch 8)
Solubility Equilibria; Acid-Base Theories; Acid-Base Equilibria
Thermochemistry and Thermodynamics (Ch 7)
First Law; Enthalpy; Standard State; Calorimetry; Hess's Law; Standard Enthalpy of Formation; Entropy; Spontaneity in Chemical Reactions; Second Law; Third Law; Gibbs Free Energy; Spontaneity and Approach to Equilibrium
Electrochemistry: Batteries, Corrosion, Fuel Cells and Membrane Potentials (Ch 9)
Redox processes; Electrochemical cells; Nernst Equation; Applications of Electrochemical cells