Download Chemistry 228: Inorganic Chemistry

CHEM 228
Inorganic Chemistry
Syllabus: Fall 2009-2010
Instructor: Houssam El-Rassy, PhD, Assistant Professor
Office: Chemistry Bldg., Room 520
Office Hours: Tuesday and Friday 11:00 am – 1:00 pm, and by appointment
E-mail: [email protected], Tel: 4051
Course Objectives
The main objectives of this course are to:
1. Have an overview of the basic aspects related to the atomic structure and simple bonding theory.
2. Explain the symmetry properties of inorganic molecules and to classify them into point groups.
3. Apply the Molecular Orbital theory for the construction of MO diagrams.
4. Explain the various acid-base concepts and to compare the strength of acids and bases.
5. Describe the common structures of crystals and give the molecular orbital explanation of their bonding.
6. Introduce the chemistry of the main group elements.
Learning Outcomes
After completing this course, students should be able to:
1. Use the atomic structure arguments to explain the observed periodicity of the elements.
2. Explain the simple bonding theory and show how this applies to Lewis dot, resonance, formal charge,
and polarity.
3. Apply the Valence Shell Electron Pair Repulsion model to predict the geometry of inorganic molecules.
4. Identify the symmetry properties of molecules and classify molecules into point groups.
5. Apply the symmetry concepts to inorganic molecules and understand the concept of character tables.
6. Apply the basic principle of Molecular Orbital theory to describe bonding in inorganic molecules and
predict bond order, stability, relative bond lengths and magnetism.
7. Draw and label molecular orbital diagrams for homonuclear and heteronuclear polyatomic molecules.
8. Explain major inorganic concepts and essential ideas related to acids and bases.
9. Compare acids and bases strength based on interactions, thermodynamic measurements, proton affinity,
inductive and steric effects, and solvation.
10. Explain and compare the strength of oxyacids and superacids.
11. Explain the concepts of crystalline solid state chemistry, identify the seven crystal classes, and show how
the packing of spheres will lead to the formation of interstitial holes.
12. Describe the ionic crystals and their formation thermodynamics through the Born-Haber cycle and
calculate their lattice enthalpies.
13. Explain the bonding in metals, the electrical conductivity in ionic solids, the semiconductivity, and the
superconductivity.
14. Differentiate between and explain the advantages of different inorganic nanomaterials synthesis
techniques, and justify their use in nanoscience and nanotechnology.
15. Explain the most significant physical and chemical properties of the main group elements.
Resource Available to Students
Primary Textbook:
Miessler G.L. and Tarr D.A. Inorganic Chemistry, 3rd Edition, Pearson Education,
2004.
Supporting Textbooks:
1. Shriver D. and Atkins P. Inorganic Chemistry, 4th Edition, Oxford University
Press, 2006.
2. Housecroft C.E. and. Sharpe A.G. Inorganic Chemistry, 3rd Edition, Pearson
Education, 2008.
3. Douglas B.E.; McDaniel D.H.; Alexander J.J. Concepts and Models of Inorganic
Chemistry, 3rd Edition, John Wiley and Sons, 1994.
PowerPoint Slides
Lectures slides will be available to students through Moodle.
Course Policy, Exams and Grading
Students must be considerate of their classmates and abstain from disruptive behavior during the lecture period.
This includes talking and whispering, while the instructor is addressing the class.
Students are expected to attend all classes and participate in class discussion. Students who do not attend the
classes will be dropped out of the course. Students are expected to enter the classroom on time.
Students must sit for all exams. Unless a valid excuse is presented (AUB Infirmary or AUH medical report), the
student will take a zero on missed exams.
Two Exams:
20%+30% (30% for the better grade)
Cumulative Final Exam: 50%
If the student is granted permission to miss an exam, his/her grade distribution will become 35% for the other
exam and 65% for the final.
Non-graphing non-programmable calculators are indispensable during the exams. Programmable calculators are
not allowed in the exam room. The student must take a quiz without calculator if he/she doesn’t bring an
appropriate calculator. Students are not allowed to use their mobile phones or any other alternative as calculators
during the exams.
Mobile phones are not allowed in classrooms and exam rooms.
Students must respect the Student Code of Conduct. Any violation of this Student Code of Conduct, either
academic or non-academic misconduct, will be reported to the appropriate level where the student risks being
subject to disciplinary action in accordance with the Student Code of Conduct.
CHEM 228: Tentative Course Outline
1. Atomic Structure
Historical development of atomic theory; The Schrödinger equation; Periodic
properties of atoms.
2 lectures
2. Simple Bonding Theory
Lewis electron-dot diagrams; Valence Shell Electron Pair Repulsion (VSEPR)
theory; Polar molecules; Hydrogen bonding.
3 lectures
3. Symmetry and Group Theory
Symmetry elements and operations; Points groups; Properties and representations of
groups; Examples and applications of symmetry to determine chirality and molecular
vibrations.
5 lectures
4. Molecular Orbitals
Formation of molecular orbitals from atomic orbitals; Homonuclear diatomic
molecules; Heteronuclear diatomic molecules; Molecular orbitals for larger
molecules; Expanded shells and molecular orbitals
6 lectures
5. Acids and Bases
Acid-Base concepts as organizing concepts; Major acid-base concepts; Hard and soft
acids and bases; Acid and base strength
5 lectures
6. Oxidation and Reduction
Redox reactions and oxidation states; Reduction potentials; Redox stability;
Potential diagrams; Chemical extraction of the elements.
4 lectures
7. Solid State and Materials Chemistry
Nonstoichiometric compounds and solid solutions; Formulas and structures;
Polymorphism; Alloys and intermetallic compounds; Thermodynamics of ionic
crystal formation; Molecular orbitals and band structure; Imperfections and defects
in solids; Metal oxides, nitrides and fluorides; Electrical conductivity;
Superconductivity.
5 lectures
8. Nanoscience, Nanomaterials, and Nanotechnology
Optical properties of nanomaterials; Characterization and synthesis; Layered
materials; Self-assembled nanostructures; Bioinorganic nanomaterials; Hybrid
nanocomposites.
3 lectures
9. Physical Techniques in Inorganic Chemistry
X-Ray and neutron diffraction; UV-Vis, Infrared and Raman absorption
spectroscopy; NMR; EPR; Mossbauer spectroscopy; Photoelectron spectroscopy;
Mass spectrometry; Atomic absorption spectroscopy; Elementals analysis; Thermal
analysis; Magnetometry; Electrochemical techniques.
2 lectures