CHM 152	General Chemistry II	(3/3/4)

Prerequisites:  CHM 151

Corequisites:  None

This course provides a continuation of the study of the fundamental principles and laws of chemistry.   Topics include kinetics, equilibrium, ionic and redox equations, acid-base theory, electrochemistry, thermodynamics, introduction to nuclear and organic chemistry, and complex ions.  Upon completion, students should be able to demonstrate an understanding of chemical concepts as needed to pursue further study in chemistry and related professional fields.  This course has been approved to satisfy the Comprehensive Articulation Agreement general education core requirement in natural sciences/mathematics.	

CHM 152 Outline

I.  Rates of Reactions
1.	Defining a rate
2.	Experimental determination of rate
3.	Dependence of rate on concentrations
rate law
rate constant
reaction order
determining the rate law using the initial rate method
4.	Change of concentration with time
 		first-order rate law
		second-order rate law
		half-life of a reaction
		graphing kinetic data
5.	Temperature and rate
collision theory
	activation energy
transition-state theory
	activated complex
	potential-energy diagrams
6.	Arrhenius equation
frequency factor
calculating activation energy
7.	Elementary reactions
reaction mechanisms
molecularity
reaction intermediates
rate equation for an elementary reaction
8.	The rate law and the mechanism
rate-determining step
mechanisms with initial fast steps
9.	Catalysts
Lowering of activation energy
homogeneous and heterogeneous catalysis
		enzymes

Operational Skills:
1.	Relating the different ways of expressing reaction rates
2.	Calculating the average rate of a reaction
3.	Determining the reaction order from a rate law
4.	Determining the rate law using the initial rate method
5.	Using the concentration-time equation for a first-order reaction
6.	Relating the rate-constant and the half-life
7.	Determining the activation energy using the Arrhenius equation
8.	Writing the overall chemical equation from the mechanism
9.	Determining the molecularity of an elementary step
10.	Determining the rate law from a reaction mechanism

II.  Chemical Equilibrium
1.	Defining a chemical equilibrium as a dynamic process
2.	Equilibrium constant
equilibrium-constant expression
law of mass action
calculating equilibrium constants
	using concentrations
	using partial pressures
	summation of reactions
3.	Heterogeneous equilibria
Definition of and understanding heterogeneous equilibria
4.	Qualitative interpretation of the equilibrium constant
5.	Predicting the direction of a reaction
reaction quotient
6.	Calculating equilibrium concentrations
7.	Removing products and adding reactants
Le Chatelier’s principle
8.	Changing the pressure and temperature
effect of pressure change
effect of temperature change
choosing optimum conditions for a reaction
9.	Effect of a catalyst

Operational Skills:
1.	Applying stoichiometry to an equilibrium mixture
2.	Writing an equilibrium-constant expression
3.	Obtaining an equilibrium constant from reaction composition
4.	Using the reaction quotient to predict the direction of a reaction
5.	Obtaining equilibrium concentrations from the equilibrium constant
6.	Applying le Chatelier’s principle to predict the change in equilibrium concentrations

III.  Acids and Bases
1.	Arrhenius concept of acids and bases
2.	Bronsted-Lowry concept of acids and bases
proton-transfer reactions
3.	Lewis concept of acids and bases
4.	Self-ionization of water
ion-product constant for water
5.	Solutions of a strong acid or base
6.	The pH of a solution
determination of hydrogen-ion concentration

Operational Skills:
1.	Identifying acids and bases
2.	Deciding whether reactants or products are favored in acid-base reactions
3.	Calculating the concentrations of hydrogen ion and hydroxide ion
4.	Using the pH to calculate the concentration of H+ and vice versa


IV.  Acid-Base Equilibria 
1.	Acid-ionization equilibria
acid-ionization constant
experimental determination of Ka
	degree of ionization
calculations using Ka
2.	Polyprotic acids
3.	Base-ionization equilibria
base-ionization constant
4.	Acid-base properties of salt solutions
hydrolysis
prediction of whether a salt solution is acidic, basic or neutral
pH of a salt solution
5.	Common-ion effect
6.	Buffers
pH of a buffer solution
Henderson-Hasselbalch equation
7.	Acid-base titration curves
equivalence point
titration of a strong acid with a weak base
titration of a strong base with a weak acid
titration of a strong base with a strong acid

Operational Skills:
1.	Determining the Ka and Kb of a solution from the pH
2.	Calculating concentrations of species in a weak acid solution using Ka
3.	Calculating concentrations of species in a weak base solution using Kb
4.	Predicting whether a salt solution is acidic, basic, or neutral
5.	Obtaining Ka from Kb and vice versa
6.	Calculating the concentrations of species in a salt solution
7.	Calculating the common-ion effect on acid ionization
8.	Calculating the pH of a buffer
9.	Calculating the equivalence point during a titration

V.  Solubility and Complex-Ion Formation
1. Solubility product constant
2.  Solubility and the common-ion effect
3.	Precipitation calculations
ion product
4.	 Effect of pH on solubility
5.	 Complex-ion formation
complex ions and ligands
stability constant
dissociation constant
			equilibrium calculations with Kf
6.	Complex ions and solubility
7.	Qualitative analysis of metal ions

Operational Skills:
1.	Writing solubility product expressions
2.	Calculating Ksp from the solubility, and vice versa
3.	Calculating the solubility of a slightly soluble salt in a solution of a common ion
4.	Predicting whether a precipitate will form
5.	Determining the qualitative effect of pH on solubility
6.	Calculating the concentration of a metal ion in equilibrium with a complex ion
7.	Predicting whether a precipitate will form in the presence of the complex ion
8.	Calculating the solubility of a slightly soluble ionic compound in a solution of the complex ion

VI.  Thermodynamics
1.	First law of thermodynamics
enthalpy and enthalpy change
spontaneous process
2.	Second law of thermodynamics
entropy
change in entropy
entropy and disorder

3.	Third law of thermodynamics
entropy change for a reaction
4.	Free energy and spontaneity
standard free-energy change
criterion for spontaneity
free-energy change during a reaction
5.	Relating free-energy change and the equilibrium constant
6.	Change of free energy with temperature

Operational Skills:
1.	Calculating the entropy change for a phase transition
2.	Predicting the sign of the entropy change for a reaction
3.	Calculating change of entropy for a reaction
4.	Calculating free-energy change from entropy change and enthalpy change
5.	Interpreting the sign of the change in free energy
6.	Calculating the equilibrium constant from the standard free-energy change

VII.  Oxidation-Reduction Reactions and Electrochemistry
1.	Oxidation-reductions
oxidation numbers
oxidation number rules
describing oxidation-reduction reactions
oxidizing and reducing reagents
2.	Balancing redox reactions
skeleton redox equations
half-reaction method
3.  Electrochemistry
	construction of a voltaic cell
salt bridge
		notation for voltaic cells

Operational Skills:
1.	Assigning oxidation numbers
2.	Balancing redox equations using the half-reaction method
3.	Sketching and labeling a voltaic cell
4.	Writing the cell reaction from the cell notation

VIII.  Nuclear chemistry
1. radioactivity
nuclear equations
nuclear force
types of radioactive decay
alpha emission
beta emission
electron capture
gamma emission
		radioactive decay series

2.  rate of radioactive decay
half-life
3.	radioactive dating
4.	applications of radioactive isotopes
5.	energy-mass calculations
6.	nuclear fission and fusion

Operational Skills:
1.	Writing a nuclear equation
2.	Deducing a product or reactant in a nuclear equation
3.	Predicting the type of radioactive decay
4.	Determining the fraction of nuclei remaining after a specified time
5.	Applying the carbon-14 dating method
6.	Calculating the energy change for a nuclear reaction


IX.  Organic Chemistry
1.  alkanes and cycloalkanes
nomenclature
2.  alkenes and alkynes
nomenclature
3.  organic compounds containing oxygen
functional groups
4.  organic compounds containing nitrogen
functional groups

Operational Skills:
1.	Writing the IUPAC name of a hydrocarbon
2.	Drawing a hydrocarbon from the IUPAC name
3.	Identifying and naming organic compounds containing various functional groups