Standard

R State Standard £Institutionally Developed College: N/A

CHM 1112 – Chemistry II
Continues the exploration of basic chemical principles and concepts. Topics include: equilibrium theory; kinetics; thermodynamics; solution chemistry; acid-base theory; and nuclear chemistry.
Competency Areas	Hours
Equilibrium Theory	Class	4
Kinetics	D. Lab	0
Thermodynamics	P. Lab	3
Solution Chemistry	Credit	5
Acid-Base Theory
Nuclear Chemistry

Prerequisite:	CHM 1111
Corequisite:

Course Guide

Competency	After completing this section, the student will be able to:	Hours
		Class	D.Lab	P.Lab/ O.B.I.
Equilibrium Theory		8	0	6
Thermodynamics	Explain what is occurring in a chemical reaction, including bonding and energy changes.
	Define the reversibility of reactions.
	Discuss the underlying concepts of endothermic and exothermic reactions.
	Define the role of enthalpy and entropy in these reaction types.
Kinetics		4	0	3
Kinetics	Describe the concept of reaction kinetics. Summarize the primary factors that alter reaction rates.
	Explain forward and reverse reaction rates.
	Describe activation energy and catalysts.
Thermodynamics		12	0	6
Equilibrium	Describe the concept of chemical equilibrium as a dynamic equilibrium.
	Use equilibrium constants Keq, Ka, and Ksp in chemical calculations.
	Explain the Law of Mass Action and Le Chatelier’s Principle.
Solution Chemistry		6	0	6
Interactive forces	Explain the interactive forces between solvent and solute particles in solution chemistry and the significance of these forces.
	Describe the properties of electrolytes and non-electrolytes in solutions.
Solutions	Specify and be able to calculate concentrations of solutions, including: percent w/w, percent w/v, molarity, and molality.
	Explain the concept of colligative properties and calculate changes in their values based on solute concentrations, including the effects of ionic solutes and van't Hoff factors where appropriate.
Osmosis	Describe osmosis and reverse osmosis.
	Illustrate osmosis and reverse osmosis.
Acid-Base Theory		6	0	9
Theories	Define acid, base, and neutralization in terms of the Arrhenius theory and Bronsted-Lowry acid-base theory.
	Apply thermodynamic equilibrium theory to acid-base dissociation.
	Apply the Bronsted-Lowry acid-base theory to identify conjugate acid-base pairs in neutralization reactions.
Equations	Write balanced molecular equations, total ionic equations, and net ionic equations for neutralization reactions of acids and bases to form salts.
Calculations	Perform calculations for titrations and neutralizations.
	Perform calculations involving pH and pOH.
Buffers	Define an acid-base buffer system. Relate to Le Chatelier’s Principle.
	Use the Henderson-Hasselbach equation to calculate the pH of a buffer.
Nuclear Chemistry		4	0	0
Radioactive decay	Describe the processes involved in radioactive decay.
	Define the major radioactive decay products: alpha particles, beta particles, gamma radiation, x-rays.
	Discuss neutron/proton ratios (magic numbers) and how these relate to decay.
	Define half-life and calculate remaining activity in a radioactive sample.

Suggested Resources

Media (print/audio/ visual/www/ other)	Author	Year	Title: Subtitle	Edition	Location	Publisher/ Publication	pp.
Print	Adamson, A. W	1986	A textbook of physical chemistry.	3^rd ed,	New York	Elsevier	971
	Bettelheim, B., et.al.	2006	Introduction to general, organic, and biochemistry.	8^th ed.	Belmont, CA	Brooks/Cole	928
	Bettelheim, B., et.al.	2006	Introduction to general, organic, and biochemistry: Student solutions manual.	8^th ed.	Clifton Park, NY	Centage Delmar	192
	Block and McKelvy	2006	Lab experiments for general chemistry.	5^th ed.	Clifton Park, NY	Centage Delmar
	Brady and Senese	2007	Chemistry: The study of matter and Its change.	5^th ed.	New York	John Wiley & Sons
	Bretherick, L.	1986	Hazards in the chemical laboratory.	4^th ed.	London	Royal Society of Chemistry	618
	Brown, LeMay and Bursten	2005	Chemistry: The central science.	10th ed.	New York	Prentice Hall
	Burns, Ralph	2004	Fundamentals of Chemistry.	4^th ed.	New York	Prentice Hall
	Chang, R. 5	2005	Chemistry.	8^th ed.	New York	Mc-Graw HIll
	Cotton, F. A., & Wilkinson, G	1999	Advanced inorganic chemistry.	6^th ed.	New York	John Wiley & Sons	1376
	CRC edition		Handbook of C\chemistry and Physics, any	Any edition		CRC Press.
	Davis, R. E	1988	Study guide to accompany general chemistry with qualitative analysis	3^rd ed.	Philadelphia	Saunders
	Hein, M., et al.	1988	College chemistry: An introduction to general, organic, and biochemistry	4^th ed.	Pacific Grove	Brooks/Cole	903
	Kanare, H. M.	1985	Writing the laboratory notebook.		Washington, DC	Oxford University Press	145
	Kotz Treichel & Wege	2005	Chemistry and chemistry reactivity.	6^th ed.	Belmont, CA	Brooks/Cole
	Lefèvre, M. J.	1990	First aid manual for chemical accidents.	2^nd ed.	New York	John Wiley & Son	272
	Loebel, A. B.	1987	Chemical problem solving by dimensional analysis.	3^rd. ed.	Boston	Centage Delmar	417
	Masterton and Hurley	2008	Chemistry: Principles and reactions.	6^th ed.	Belmont, CA	Brooks/Cole
	Moore, Stanitski and Jurs	2007	Chemistry: The Molecular science.	3^rd ed.	Boston	Centage Delmar
	Olmsted and Williams	2004	Chemistry.	4^th ed.	New York	John Wiley & Son

Posted: 10/01/08