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
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.
- 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
Evaluation will be accomplished by a combination of graded homework, examination, quizzes and laboratory performance and write up.
The final grade will be based on a percentage of the total points possible:
A typical breakdown of the points is: Three unit exams comprise approximately 40% of the total score, the final exam approximately 20%, laboratories approximately 24%, quizzes and homework provide the balance of the points.
PO5 should be assessed: Students will be able to solve problems by gathering, interpreting, combining and/or applying information from multiple sources.