CH 122 College Chemistry 2

Lecture Hours: 3
Lab Hours: 2
Credits: 5

Provides basic understanding of molecular compound formations, changes of state, solutions and reaction rates. Covers quantitative composition; stoichiometry; the gaseous state; thermodynamics, Kinetics, solutions, colligative properties. Second of a three-term sequence.

Prerequisite: Placement into WR 115 (or higher), or completion of WR 090 (or higher); and completion of CH 121; or consent of instructor. (All prerequisite courses must be completed with a grade of C or better.)
Student Learning Outcomes:

Explain gas pressure-volume relationship.
Explain gas temperature-volume relationships.
Utilize the Combined Gas Law.
Utilize the Ideal Gas Law.
Explain the Law of Effusion.
Explain the kinetic theory and gas laws.
Explain changes of state and dynamic equilibrium.
Predict energy changes during changes of state.
Describe intermolecular attractions.
Differentiate between crystalline and non-crystalline solids.
State the difference between physical and chemical properties.
State the general properties of liquids and solids.
Calculate molarity.
Prepare dilute solution from concentrated solutions.
Define dynamic equilibrium and LeChatelier’s principle.
Describe electrolytes.
Explain acids and bases as electrolytes.
Balance ionic equations.
Predict metathesis reaction.
Perform acid-base titrations.
Calculate equivalent weights and normalities.
State the Bronsted-Lowry acid-base concept.
State the Lewis concept of acids and bases.
Apply the acid/base concept.
Apply the concept of equilibrium and list the factors that affect it.
Describe oxidation-reduction reactions.
Discuss the concept of nuclear chemistry.

Additional 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

Lecture

The Gaseous State of Matter
- Gas properties and the kinetic-molecular theory
- Boyle’s, Charles’, Dalton’s Laws
- Avogadro’s hypothesis
- Density and specific gravity of gases
- Calculations and the ideal gas equation
Water and the Properties of Liquids
- Properties, structure, and occurrence of water
- Hydrogen bonding
- Hygroscopic substances
- Natural waters
- Physical properties of water
Solutions
- Types, components, and properties of solutions
- Solubilities and related factors
- Concentrations and colligative properties
- Osmosis
Ionization: Acids, Bases, Salts
- Acids, bases, salts
- Electrolytes
- Ionization and dissociation
- Neutralization
- Ionic equations
- Colloids
Acids, Bases and Salts
- Continuation of the overall concept from CH122
- Ionization of water
- Introduction to pH and H+ concentration
- Writing ionic equations
Chemical Equations
- Chemical equilibrium and reaction rates
- Reversible reactions and LeChatelier’s Principle
- Effects on equilibrium and reaction rates
- Equilibrium and ionization constants
- Solubility product constant
- Buffers
- Reaction mechanisms
Oxidation-Reduction
- Oxidation number
- Balancing redox equations
- Balancing ionic redox equations
- Activity series of metals
- Electrolytic and voltaic cells
Radioactivity and nuclear chemistry
- Natural radioactivity and particle properties
- Disintegration series
- Measurement of radioactivity
- Fission and fusion
- Mass-energy relationships
- Biological effects and applications

Laboratory Outline and Objectives:

Charles’ Law lab
- Volume and temperature relationships
- Volume and pressure relationships
Gases in the Atmosphere lab
- Gaseous Diffusion
  - The kinetic molecular theory
  - Graham’s law of diffusion
  - Rates of diffusion
  - Calculations with Graham’s Law
Gas Constant lab
- Ideal Gas Law
  - Production of a gas
  - Collection of a gas over water
  - Measurement of gas volume at constant pressure
  - Calculation of the Universal Gas Constant, R
Mole Weight of a Solute by Freezing Pint Depression lab
- Calculation of the number of moles from the change of temperature
- Lowering of the vapor pressure of a solution
- Determination of the molality
- Finding the mole weight of an unknown non-volatile solute
Properties of Solutions lab
- Solvent and solute relationships
- Solubilities
- Miscibility
- Particle size and temperature effects
- Ionic reactions
Acids and Bases lab
- Ionization - Acids, Bases, and Salts
  - Ionization
  - Properties of acids
  - Properties of bases
  - Neutralization
  - Indicators
- Electrolytes
- Acids, bases
- Buffers
- Solvent properties of water
- Standardizations
Equivalent Weight lab
- Titration of unknown acids with standardized bases
- Use of burets in acid-base analysis
- Use of the pH scale to find Molarity of solutions
- Differences of the point of neutrality for complex indicators
pH with Indicators lab
- pH as a measurement of hydrogen ion concentration
- Color changes of acid-base indicators
- Use of the pH scale to find Molarity of solutions
- Differences of the point of neutrality for complex indicators
Chemical Equilibrium lab
- Reversible reactions
- Saturated salts
- LeChatelier’s principle
Activity of Metals lab
- Oxidation-Reduction reactions
- Balancing Redox reactions
- Oxidatizing and Reducing agents
- Single replacement reactions of metals
- Activity series of metals
Conductivity lab
- Electric current introduction
- Definitions of cathodes and anode
- Primary and secondary conductors
- Electrolytic cells and production of gases at electrodes
- Conduction of electric current through ionic and polar aqueous solutions

Required textbook for college credit: Open Stax Chemistry 2e. ISBN 978-1-947172-62-3