DEPARTMENT  OF CHEMISTRY AND BIOCHEMISTRY
COLLEGE OF CHARLESTON
CHEMISTRY 112 SYLLABUS

 I. 	Chemical Thermodynamics
	A.	First Law of Thermodynamics
		1.	Work in Chemical Reactions
		2.	Internal Energy
	B.	Second Law of Thermodynamics
		1.	Definition of Entropy
	C.	Free Energy
		1.	Definition
		2.	Spontaneity
II.	Chemical Equilibrium
	A.	Law of Chemical Equilibrium
		1.	Kp and Kc
		2.	Determination of Kc from Concentrations
		3.	Determination  of Concentration  from Kc
		4.	Heterogeneous  Equilibrium   (Activity) 
	B.	Effect on Equilibrium by
		1.	Pressure
		2.	Concentration Changes
		3.	Temperature
III.	Solubility Equilibria
	A.	Sparingly Soluble Compounds
		1.	Net Ionic Equations
		2.	Ksp Concept
	B.	Calculations
		1.	Ksp from Solubility
		2.	Solubility from Ksp 
		3.	Common Ion Effect
	C.	Applications
		1.	Gravimetric Analysis
		2.	Precipitation Titrations
		3.	Selective Precipitations
IV.	Acid-Base
	A.	Definitions of Acids, Bases, and Neutralization
		1.	Arrhenius Theory
		2.	Brønsted-Lowry Theory
			a.	Acid-Base Conjugates
		3.	Lewis Theory
	B.	Autoionization of Water
		1.	Kw
		2.	pH and pOH
	C.	Calculation of pH and Concentrations of All Species Solutions
		1.	Strong Acids
		2.	Strong Bases
		3.	Weak Monoprotic Acids
			a.	Degree of Ionization
		4.	Weak Monohydroxo Bases
		5.	Polyprotic Acids
		6.	Polyhydroxo Bases
		7.	Dissolving Precipitates
	D.	Buffer Solutions
		1.	Concept
		2.	Preparation	
		3.	Applications
	E.	Hydrolysis of Ionic and Salts
		1.	Concept
		2.	Calculations of pH
	F.	Titrations
		1.	Selection of Indicator
		2.	Calculations
			a.	pKa from Half-Equivalence Point
			b.	pH of Equivalence Point
			c.	Stoichiometry
		3.	Titration Curves
			a.	Strong Acid-Strong Base
			b.	Weak Acid-Strong Base
			c.	Strong Acid-Weak Base
			d.	Polyprotic Acid-Strong Base
V.	Coordination Compounds
	A.	Definitions
		1.	Complex Ions
		2.	Coordinate Covalent Bond
		3.	Ligands
		4.	Coordination Number
		5.	Chelates
	B.	Nomenclature
	C.	Bonding and Geometry
		1.	Valence-Bond Theory
		2.	Crystal-Field Theory
	D.	Equilibria Involving Kd
	E.	Applications in Analytical Chemistry
		1.	Dissolving Precipitates
VI.	Chemical Kinetics
	A.	Concepts
		1.	Rate Equations
			a.	First Order
			b.	Second Order
		2.	Half-Life
		3.	Rate Constants
	B.	Energy Profile Diagrams
		1.	Catalysis
		2.	Activation Energy
			a.	Arrhenius Equation
	C.	 Mechanisms
VII.	Oxidation-Reduction and Electrochemistry
	A.	Reactions
		1.	Concepts
		2.	Oxidizing and Reducing Agents
		3.	Balancing
		4.	Prediction of Products
		5.	Faraday’s Law
	B.	Galvanic Cells
		1.	Concepts
		2.	Cell Diagrams
		3.	Anode and Cathode
		4.	Half-Cell Reactions and emfs
		5.	Overall Cell Reactions and emfs
		6.	Cell Spontaneity and  G
		7.	Nernst Equations
		8.	Extent of Reaction and K
	C.	Electrolytic Cells
		1.	Concept
		2.	Molten Salts
		3.	Aqueous Solution
	D.	Commercial Cells
VIII.	Inorganic Reactions
	A.	Classification
		1.	Redox
			a.	Combination
			b.	Decomposition
			c.	Displacement
			d.	 Disproportionation 
		2.	 Nonredox 
			a.	Combination
			b.	Decomposition
			c.	Single Displacement
			d.	Double Displacement
	B.	Prediction of Products
		1.	Driving Forces
	C.	Brief Descriptive Chemistry
		1.	Metals and their Compounds
			a.	Properties of Metals
			b.	Metallic Bond
			c.	Chemical Properties of Groups I and II
		2.	Nonmetals and Their Compounds
			a.	Properties of Nonmetals
			b.	allotropes
			c.	Hydrocarbon Compounds
			d.	Oxygen Compounds
			e.	Halogen Compounds
IX.	Organic Chemistry (Optional)
			a.	Functional Groups
			b.	Polymers
			c.	Biochemistry
X.	Final Examination
	All sections will use the Standardized ACS final examination.  CHEM 112 Lab is a  corequisite  for CHEM 112.