The second in a three-quarter series examining the principles of General Chemistry with the primary emphasis on inorganic chemistry. Topics include: Chemical equilibrium, gas laws, molecular geometry, introduction to solution chemistry (acids and bases, precipitation reactions, redox chemistry), reaction rates and states of matter. Relevance of course material to current practices in chemistry is a fundamental focus.
Prerequisites
Successful completion of CHEM& 161 or instructors permission
Quarters Offered
Winter
Course Outcomes
Upon successful completion of the course, students should be able to demonstrate the following knowledge or skills:
- Apply the Ideal Gas Law to gaseous systems.
- Understand the Kinetic Theory of an ideal gas.
- Generate Lewis Dot Structures for most molecules.
- Describe covalent and ionic bonds.
- Predict the geometry of a simple molecule by application of the Valance Shell Electron Pair Repulsion Model (VSEPR).
- Apply Molecular Orbital Theory to predict energy levels of electrons in diatomic molecules.
- Identify and describe the characteristics of the three states of matter.
- Calculate and express solution concentrations in terms of molarity, molality, mole fraction and mass percent.
- Predict the effect of concentration on the colligative properties of a solution.
- Determine reaction rates from experimental data.
- Determine equilibrium constants and use equilibrium constants in calculations.
- Recognize acid and base character of molecules and predict reactions.
- Distinguish between strong and weak common acids and bases.
- Describe the mathematical basis of the pH concept.
Institutional Outcomes
IO2 Quantitative Reasoning: Students will be able to reason mathematically.
Course Content Outline
- Molecular Geometry
VSEPR model
Valance bond theory
Molecular orbital theory - The Gaseous State
Empirical gas laws
Ideal gas laws
Kinetic Molecular Theory of Gases - Liquids and solids
Phase transitions
Properties of liquids
Types of solids - Solutions
Solution concentration and units
Solubility
Colligative properties - Rates of reaction
Experimental determination of reaction rate
Determination of rate constants
Determination of rate law
Effect of catalysis - Equilibrium
Dynamic equilibrium
Determination of the equilibrium constant
Qualitative interpretation of equilibrium
Le Chatelier’s Principle
Catalysis - Acids and bases
Arrhenius, Lewis and Bronsted-Lowry concept of acids and bases
Molecular structure and acid strength
pH of water