Principles of Chemistry (CHM 3, 4) - Myweb @ CW Post - Long ...

LONG ISLAND UNIVERSITY
C.W. POST CAMPUS
Principles of Chemistry (CHM 3, 4) Syllabus 2009-2010
Prerequisite: Mathematics 3 Corequisites: Mathematics 7–8
Mandatory TEXT: CHEMISTRY, 10 th ed. By Raymond Chang (ISBN: 978-0-07-727431-6).
A discounted package includes Students Solutions Manual
and is available in Campus bookstore.
Chs.
LECTURE TOPICS – CHM 3
1. The scope of chemistry. Classification of matter and its properties. Measurement of
Matter. Uncertainties in Scientific Measurements.
2. The Atomic Theory. The Nuclear Atom. Chemical Elements. Introduction to Periodic
Table. The Concept of the Mole and The Avogadro Constant.
3. Atomic and Molar Masses. Chemical Compounds and Their Formulas. The Mole
Concept and Chemical Compounds. Composition of Chemical Compounds.
4. Chemical Reactions and Chemical Equations. Conservation Laws of Elements and
Mass. Stoichiometry. Chemical Reactions in Solutions.
5. The Nature of Aqueous Solutions. Classification of Reactions in Aqueous Solutions.
Solution Stoichiometry.
6. Gases. The Simple Gas Laws. The Ideal Gas Equation. Ideal Gases Opposed to Real
Gases. Kinetic–Molecular Theory of Gases.
7. Thermochemistry. The First Law of Thermodynamics. Energy Changes in Chemical
Reactions. Calorimetry. Standard Enthalpies. Hess's Law.
9. Quantum–Mechanical Preliminaries. Electron configuration. The Aufbau Principle.
10. Development of the Periodic Table. Periodic Classification of the Elements. Periodic
Variation of Physical and Chemical Properties.
11. Basic Concepts of Chemical Bonding. Lewis Octet Rule. Formal Charge. The Concept
of Resonance. The Shapes of Molecules.
12. Additional Aspects of Bonding. Molecular Geometry: VSEPR Model. Hybridization.
13. Intermolecular Forces and Types of Substances. Phase Diagrams. Liquid–Vapor
Equilibrium. Crystal Structure.
LABORATORY TOPICS – CHM 3L
Check–in: Introduction to Safety Rules and Safety Behavior in the Lab.
Exp.# 1: Measurements, Precision, Accuracy and Significant Figures.
Exp.# 2: What Is a Chemical Reaction? Chemical and Physical Change.

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Determination of an Empirical Formula.
Acid – Base Titration.
Oxidation – Reduction Titration.
Analysis of Some Commercial Bleaches.
The Empirical Gas Laws.
Determination of the Universal Gas Constant.
Molar Mass of a Volatile Liquid. Modified Dumas Bulb Method.
Thermochemistry I. The Heat of Reactions.
Thermochemistry II. The Heat of Reactions. The Hess' Law.
LECTURE TOPICS – CHM 4
Chs.
14. Colligative Properties of Solutions. Concentration Units. Solubility of Gases. Vapor
Pressure of Solutions. Osmotic Pressure. Freezing–Point Depression and Boiling–
Point Elevation.
15. Chemical Kinetics. The Rate Laws. Activation Energy and Temperature Dependence of
Rate Constants. Reaction Mechanisms.
16. Dynamic Equilibrium. The Equilibrium Constant Expression. Significance of
Equilibrium Constant Value. Predicting the Direction of a Reaction. Equilibrium
Calculations.
17. Acids and Bases. Br/o nsted–Lowry Theory. Acid–Base Properties of Water. The pH–
Scale. Acid–Base Properties of Salts.
18. Acid–Base Equilibria. The Common-Ion Effect and Buffers. Acid–Base Indicators.
19. Solubility Equilibria. Complex–Ion Equilibria. Principles of Qualitative Analysis.
20. Chemical Thermodynamics. Spontaneous Change. The Second Law of
Thermodynamics. Gibbs Free Energy and Chemical Equilibrium. Thermodynamics in
Living Systems.
21. Chemistry of Redox Reactions. Spontaneity of Redox Reactions. Batteries. Corrosion.
Industrial Applications of Electrochemistry: Electrolysis.
LABORATORY TOPICS – CHM 4L
Check–in:
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Introduction to Safety Rules and Safety Behavior in the Lab.
Spectrophotometric Analysis. Spectrophotometric Determination of
Copper in Brass.
Colligative Properties. Molar Mass by Freezing Point Depression.

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Qualitative Analysis of Inorganic Ions I. Analysis of Common Anions
and Their Salts.
Qualitative Analysis of Inorganic Ions II. Analysis of Group I and II
Cations and Their Salts.
Qualitative Analysis of Inorganic Ions III. Analysis of Group III and IV
Cations and Their Salts.
A Kinetic Study of an Iodine Clock Reaction.
Chemical Equilibrium I. Determination of Equilibrium Constant Using
Spectrophotometry.
Chemical Equilibrium II. Determination of Solubility Product Constant.
pH of Aqueous Solutions.
pH Titration Curves.
Electrochemistry. Investigation of Voltaic Cells.