Download Syllabus: General Chemistry, CHEM 101 Section

Qatar University
College of Arts and Sciences
Department of Chemistry and Earth Sciences
Syllabus: General Chemistry, CHEM 101 Section Lxx
2009-2010 Spring Semester (3 Credit hours)
Textbook :
Chemistry,
Raymond Chang, McGraw Hill, 9th ed., 2007
Grading :
1st Exam :
2nd Exam:
Project/Term Paper
Quizzes
Final Exam:
25 %
25 %
5%
10 %
35 %
100%
Lecture Times and room:
Tutorials:
1 hr/wk according to posted schedule
Exam Dates:
1st Exam :
2nd Exam:
Project report:
Final :
Saturday March 27
Saturday May 8
due May 20
Sunday June 6
Chapters 1, 2, 3, 4 (in part)
Chapters 4 (in part) 5, 6, 7
Chapters 1-10
Professor:
Office and Office Hours:
Contact: Mahmoud Khader Tel. 2204
E-mail: [email protected]
Course Description
This course will provide students with a comprehensive overview of the major areas of
chemistry. Chemical principles for each topic under discussion are presented together with
their foundation in atomic and molecular structure. Topics covered range from atomic and
molecular theory to the descriptions of chemical reactivity and reactions, quantitative
methods in chemistry, reactions in aqueous media, thermochemistry and chemical energetics,
and chemical bonding. Applications of chemistry, “the central science” are discussed
throughout the lectures. Lecture sessions are complemented by weekly tutorials, giving
students the opportunity to practice their knowledge, and to gain extensive experience in
problem solving. Upon completion of the course the student will have gained a strong
foundation for the further study of chemistry, and for the application of chemical principles in
a variety of other fields.
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Course objectives
In this course, students will:
1)
develop an understanding of the basic principles of the major branches of
chemistry.
2)
obtain a thorough foundation in the various fields of chemistry.
3)
learn to solve chemical problems using basic mathematics.
4)
develop an understanding of chemical models and theories
5)
obtain an understanding of the role of chemistry in other disciplines, and its
importance in society.
6)
acquire positive attitudes towards further studies in chemistry and towards the
application of chemistry in other disciplines.
Learning outcomes
Following completion of the course, students will be able to:
1)
define the structure of the atom in terms of the nucleus with protons and
neutrons, and electrons.
2)
write and balance chemical equations, name inorganic compounds and ions
and describe the properties of the main group elements.
3)
carry out chemical calculations, including mass relations in chemical
reactions, limiting reagent and reaction yield calculations, and calculations
involving reactions taking place in solution..
4)
understand the concept of oxidation-reduction, calculate oxidation numbers,
and balance redox reactions.
5)
apply the ideal gas law in solving problems involving the gas phase.
6)
solve problems in chemical thermodynamics and calorimetry.
7)
predict the electronic structure of atoms and ions from quantum theory, and
relate the position of an element in the periodic table to its electronic structure
and to the physical and chemical properties of the elements.
8)
describe the principles of chemical bonding and write Lewis structures
9)
predict the geometry of the electron pairs and the shape of molecules using
VSEPR theory, predict bond polarity and molecular dipoles
10)
describe the valence bond theory, predict the hybridization of atoms in
molecules, and describe bonding in molecules with single, double and triple
bonds in terms of σ and π bonds, and delocalized molecular orbitals
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Course content
Chapter 1
Chemistry
1. 7
Measurements
1. 8
Handling Numbers
1. 9
Dimensional Analysis in Solving Problems
2 lectures
Chapter 2
Atoms, Molecules, and Ions
2. 3
Atomic Number, Mass Number, and Isotopes
2. 4
The Periodic Table
2. 5
Molecules and Ions
2. 6
Chemical Formulas
2. 7
Naming Compounds
3 lectures
Chapter 3
Mass Relationships in Chemical Reactions
3. 1
Atomic Mass
3. 2
Avogadro’s Number and Molar Mass of an Element
3. 3
Molecular Mass
3. 4 The Mass Spectrometer
3. 5
Percent Composition of Compounds
3. 6
Experimental Determination of Empirical Formulas
3. 7
Chemical Reactions and Chemical Equations
3. 8
Amounts of Reactants and Products
3. 9
Limiting Reagent Calculations
3. 10 Reaction Yield
5 lectures
Chapter 4
Reactions in Aqueous media
4. 1
General Properties of Aqueous Solutions
4. 2
Precipitation Reactions
4. 3
Acid-Base Reactions
4. 4
Oxidation-Reduction Reactions, Oxidation Numbers
4. 5
Concentration of Solutions, Solution Stoichiometry
4. 7
Acid-Base Titrations
5 lectures
Chapter 5
Gases
5.1
Gases
5.2
Pressure
5.4
The Ideal Gas Equation
5.5
Stoichiometry of Gas Phase Reactions
5.6
Partial Pressures
3 lectures
Chapter 6
Thermochemistry
6. 1
The Nature of Energy and Types of Energy
6. 2 Energy Changes in Chemical Reactions
6. 3 Introduction to Thermodynamics
6. 4
Enthalpy of Chemical Reactions
6. 5
Calorimetry
6. 6
Standard Enthalpy of Formation and Reaction
4 lectures
3
Quantum Theory and the Electronic Structure of Atoms
5 lectures
From Classical Physics to Quantum Theory
Bohr’s Theory of the Hydrogen Atom
Quantum Numbers
Atomic Orbitals
Electron Configurations
The Building-Up (Aufbau) Principle
Chapter 7
7. 1
7. 3
7. 6
7. 7
7. 8
7. 9
Chapter 8
Periodic Relationships Among the Elements
8. 1
Development of the Periodic Table
8. 2
Periodic Classification of the Elements
8. 3
Periodic Variation in Physical Properties
8. 4
Ionization Energy
8. 5
Electron Affinity
3 lectures
Chapter 9
Chemical Bonding I: Basic Concepts
9. 1
Lewis Dot Symbols
9. 2
The Ionic Bond
9. 4
The Covalent Bond
9. 5
Electronegativity
9. 6
Writing Lewis Structures
9. 7
Formal Charge and Lewis Structures
9. 8
The Concept of Resonance
9. 9
Exceptions to the Octet Rule
9. 10 Bond Energy
5 lectures
Chapter 10 Chemical Bonding II: Molecular Geometry and Hybridization of
Atomic Orbitals
4 lectures
10. 1 Molecular Geometry
10. 2 Dipole Moment
10. 3 Valence Bond Theory
10. 4 Hybridization of Atomic Orbitals
10. 5 Hybridization in Molecules Containing Double and Triple Bonds
10. 8 Delocalized Molecular Orbitals
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