PREREQUISITE: 

CHE 111 (General Chemistry I)

Students receiving credit for CHE111 and/or CHE112 cannot receive credit for CHE101. 

REQUIRED TEXTBOOK:

This course uses an Open Education Resource (OER) which is free. You can access the textbook at the following URL: https://www.openstaxcollege.org/textbooks/chemistry

Chemistry

ISBN-13: 978-1-938168-39-0

REQUIRED MATERIALS:  

A scientific or graphing calculator, a bound composition notebook with graph paper pages for lab, safety glasses, and a straight edge are all required for this course.

As the result of instructional activities, students will be able to:

1. use appropriate chemical terminology and nomenclature to effectively communicate their understanding of  concepts in chemistry
2. describe the phases of matter and their molecular and elemental properties
   1. define the Basic Gas Laws
      1. perform calculations using Boyle's, Charles, Gay-Lussac's and the Ideal Gas Laws
      2. define partial pressure and Dalton's Law
      3. define the Kinetic-Molecular Theory of Gases
      4. define the Real Gas Law behavior
   2. describe the difference between diffusion & effusion
   3. define the properties of liquids
      1. distinguish between the intermolecular forces involving polar molecules
      2. distinguish between the intermolecular forces involving non-polar molecules
      3. distinguish between different types of solids
   4. draw a phase diagram and label it completely
3. define the units of concentration
   1. calculate molarity, molality, mole fraction, weight percent, and ppm
   2. convert concentrations from one unit to another
4. explain solubility of solutions
   1. describe the process of liquids dissolving in liquids
   2. describe the process of solids dissolving in liquids
   3. define factors that affect solubility of gases dissolved in liquids in terms of Henry's Law
   4. calculate the enthalpy of solutions from thermodynamic data
5. describe colligative properties of solutions
   1. calculate Raoult's Law for changes in vapor pressure
   2. determine the boiling point elevation, freezing point depression and use colligative properties to calculate variables present in these relationships (molar mass and molality) 
6. distinguish between the different types of colloids
   1. identify and explain how a surfactant works
   2. define osmotic pressure
7. determine rates of chemical reactions
   1. determine order of reactions
      1. calculate and graph first-order reaction kinetic data
      2. calculate and graph second-order reaction kinetic data
      3. calculate and graph zero-order reaction kinetic data
      4. calculate and graph half-life for first, second & zero-order reactions
   2. write a rate equation
   3. determine the rate constant (k)
      1. calculate R (rate) using a rate law expression and k
   4. describe reaction conditions that determine reaction rates
8. explain Collision Theory
   1. distinguish between the effect concentration and temperature has on reaction rates
   2. calculate activation energy using the Arrhenius Equation
   3. define the function of a catalyst and the effect it has on reaction rates
9. describe reaction mechanisms
   1. describe molecularity and rate equations for elementary steps
   2. define molecularity and reaction order
   3. determine reaction mechanisms from kinetic data
10.  define chemical equilibrium
    1. write an equilibrium constant expression for a balanced equilibrium reaction
    2. define the meaning of the equilibrium constant K
    3. determine the reaction quotient Q for a reaction
    4. use equilibrium constants in calculations
11. explain Le Chateliers Principle
    1. explain the effects of the addition or removal of reactants or products
    2. explain the effects of volume changes on gas-phase equilibria
    3. explain the effects of temperature changes on equilibria
12. define acids and bases in terms of Arrhenius, Bronsted-Lowry and Lewis
    1. describe basic properties of acids & bases
    2. determine conjugate acid base pairs
    3. explain cationic & molecular Lewis acids and Lewis bases
13. describe the self ionization of water and K_w
    1. describe  and calculate K_a & K_b in acid base equilibria
       1. predict the direction of an acid base equation
14. define the pH scale and calculate pH using logarithms and K_w
    1. determine the relationship of acid-base reactions with respect to strength of each reactant
    2. perform an acid base titration
15. define pK_a and calculate using the Henderson-Hasselbach equation
16. determine the molecular structure, bonding and behavior of acids and bases
    1. determine the acid strength of metal halides
    2. compare strengths of oxoacids
    3. describe carboxylic acids and draw its functional group
17. define the common ion effect
    1. calculate concentration and pH of buffered solutions
       1. construct a pH titration curve
18. define solubility of slightly soluble salts and determine K_sp
    1. explain the effect of basic anions on salt solubility
19. define entropy & free energy
    1. calculate standard enthalpy values
    2. summarize spontaneous reactions
    3. calculate Gibbs free energy
       1. define standard free energies of formation
20. define oxidation-reduction reactions
    1. balance red-ox equations
21. describe simple and commercial voltaic cells
    1. draw a voltaic cell from electrochemical cell notation
    2. define dry cells and alkaline batteries
    3. describe  a fuel cell
22. determine standard electrochemical potentials
    1. use a table of standard reduction potentials
    2. describe relative strengths of oxidizing and reducing agents
    3. define the Nernst equation
23. define natural radioactivity
    1. determine rates of nuclear decay
    2. write balance nuclear equations
    3. describe the difference between nuclear fission and nuclear fusion
24. describe the kinetics of nuclear decay
    1. calculate half-life of a nuclear reaction
    2. describe carbon dating
    3. define nuclear medicine and explain its uses
25. define the processes, pros and cons of  nuclear energy

LAB OBJECTIVES:

The laboratory experience will reinforce the understanding that experimental work is the foundation of chemical knowledge and which requires fundamental laboratory skills. Students will: 

1. anticipate, recognize, and respond properly to potential hazards in laboratory procedures
   1. complete laboratory safety training as designed by the CCC science department
   2. review the contents of MSDS & location of MSDS sheets storage area
2. keep accurate and complete experimental records
   1. write all lab records in a bound lab notebook using Proper Lab Documentation (PLD) as required for Good Lab Practices (GLP)
   2. enter all data as it is generated in the lab
3. perform accurate quantitative measurements
   1. use properly calibrated instruments (i.e. spectrophotometers) and volumetric glassware
4. interpret experimental results and draw reasonable conclusions
   1. record in the lab notebook all information/data using tables, graphs, formulas and calculations
   2. write a conclusion of results in the lab notebook at the end of each lab to summarize what was discovered in the laboratory
5. communicate effectively through oral and written reports
   1. write 5 formal lab reports - Freezing Point Depression, Iodine Clock, Le Chatelier's Principle, Acid/Base Titration of an Unknown Acid, and pH Titration Curve
   2. write 2 Standard Operating Procedures (SOP's) - Calibration of a pH Meter and Calculations of Buffered Solutions
   3. perform 2 oral laboratory presentations/demonstrations - Solids, Liquids & Gases and Electrochemistry
   4. report required information such as tables, graphs, formulas, calculations background and summary in electronic format
   5. use Excel, Word and PowerPoint to present laboratory data and reports to the instructor and classmates as required
6. analyze data statistically, assess the reliability of experimental results, and discuss the sources of systematic and random error in experiments
   1. use statistical interpretation as needed in the summary of lab information and required lab reports
   2. include correlation of data on all graphs via electronically generate linear trend lines
7. plan & execute experiments through the use of appropriate chemical literature & electronic resources
   1. research background information required for labs and lab reports from reputable sources such as American Chemical Society (ACS) or .edu, .org, and .gov websites

 GENERAL TOPICS OUTLINE:

1. Gases & Their Properties  
2. Intermolecular Forces & Liquids
3. Chemistry of Solids
4. Solutions & Their Behavior
5. Chemical Kinetics
6. Chemical Equilibrium
7. Acids & Bases & Other Aspects of Aqueous Equilibria
8. Entropy & Free Energy
9. Electrochemistry

Feel free to contact a member of the Science Department or the Science Department Chair.