CH 222 General Chemistry 2

Lecture Hours: 3
Lab Hours: 3
Credits: 5

Covers solutions and solids; rates and mechanisms of reactions; kinetic molecular theory of gases; thermodynamics; chemical kinetics; properties of solutions and nuclear chemistry. Second of a three-term sequence designed for students majoring in scientific, engineering, and medical fields.

Prerequisite: Placement into WR 115 (or higher), or completion of WR 090 (or higher); and completion of CH 221; or consent of instructor. (All prerequisite courses must be completed with a grade of C or better.)
Student Learning Outcomes:

Generate and test models in a logical and objective manner and use them to identify key trends and relationships.
Perform experiments safely, make clear observations, summarize data in tables, interface computers to chemical sensors, maintain laboratory notebooks and write concise laboratory reports.
Construct Lewis structures and computer-generated molecular models of substances and relate their predicted shapes and polarities to observed chemical properties.
Think critically about the role that intermolecular forces play in determining the macroscopic (observable) properties of the chemical around us.
Illustrate the solution process, interpret phase diagrams, calculate a variety of solution concentrations and distinguish between solution and colloids.
Use free energy to determine the direction of chemical changes and how temperature affects their spontaneity.
Use Internet, oral and written communication skills to analyze and discuss the properties of advanced modern materials

Statewide General Education Outcomes:

Gather, comprehend, and communicate scientific and technical information in order to explore ideas, models, and solutions and generate further questions.
Apply scientific and technical modes of inquiry, individually, and collaboratively, to critically evaluate existing or alternative explanations, solve problems, and make evidence-based decisions in an ethical manner.
Assess the strengths and weaknesses of scientific studies and critically examine the influence of scientific and technical knowledge on human society and the environment.

Content Outline

The Properties of Mixtures: Solutions and Colloids
- Energy Changes in the Solution Process
- Solubility as an Equilibrium Process
- Expressing Concentrations Quantitatively
- Fundamentals of Solution Stoichiometry
- Writing and Balancing Net Ionic Equations for Precipitation, Acid-Base and Redox Reactions
- The Structure and Properties of Colloids
Gases and the Kinetic-Molecular Theory
- Gas pressure and its measurement
- Empirical and ideal gas laws
- Kinetic-Molecular Theory as a model of gas behavior
- Real gases
Thermochemistry: Energy Flow and Chemical Change
- Forms of energy and their interconversion
- Enthalpy, bond strengths and heats of reaction
- Calorimetry: Laboratory measurement of heats of reaction
- Stoichiometry of Thermochemical Equations
- Hess’s Law of Heat Summation and Standard Heats of Reaction
Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Change
- Second law of thermodynamics: Predicting spontaneous change
- Calculating the change in entropy of a reaction
- Entropy, free energy, and work
- Free energy, equilibrium, and reaction direction
Kinetics: Rates and Mechanisms of Chemical Reactions
- Factors influencing reaction rate
- Rate Law and its components
- Integrated Rate Laws: concentration changes over time
- Explaining the effects of temperature and concentration on reaction rate
- Reaction mechanisms and the roles of catalysts and inhibitors on reaction rate
- Kinetics of ozone depletion and the functioning of biological catalysts
Nuclear Chemistry
- Radioactivity
- Kinetics of Decay
- Transmutation, Fusion
- Fission and Applications
Laboratory Experiments
- Analysis of Double Displacement Reactions
- Titration of an Acid
- Enthaply of a Reaction
- Molar Volume of a Gas
- Molar Mass of a Volatile Liquid
- Thermodynamic Values of Reactions
- Factors Affecting Rates of Reactions
- Determining a Rate Law
- Nuclear Decay