[Summary of the course] This course covers fundamental concepts in inorganic chemistry such as the atomic structure and the nature of chemical bonds.
[Aim of the course] The atomic structure and the nature of chemical bonds are essential topics to understand general chemistry. This course covers the atomic structure based on quantum theory as well as atomic parameters including atomic radius and ionization energy. Among the chemical bonds, covalent bonds are focused and taught with the Lewis structure, valence bond theory, and molecular orbital theory. The knowledge would be the basics for further learning of the related courses.
At the end of this course, students will be able to:
1) Explain the scheme of the periodic table and the nature of elements such as atomic radius and electronegativity.
2) Explain the structure and bonding of simple molecules and ions on the basis of the Lewis structure, valence bond theory, and molecular orbital theory.
atomic orbital, ionization energy, electron affinity, electronegativity, Lewis structure, octet rule, formal oxidation number, mean bond enthalpy, valence bond theory, VSEPR model, molecular orbital theory, bonding orbital, antibonding orbital
|✔ Specialist skills||Intercultural skills||Communication skills||Critical thinking skills||Practical and/or problem-solving skills|
This course first covers fundamentals in quantum physics and chemistry. In the second half of the course, applications to problems in organic chemistry and inorganic chemistry are introduced. In the last day, final examination is set to assess the level of understanding.
|Course schedule||Required learning|
|Class 1||Introduction to inorganic chemistry. Atomic structure||Explain the atomic structure based on the atomic orbitals.|
|Class 2||Electronic configurations and periodic table||Explain the scheme of the periodic table on the basis of the electronic configuration.|
|Class 3||Ionization energy, electron affinity, and electronegativity||Explain the definition and trend of ionization energy, electron affinity, and electronegativity.|
|Class 4||Molecular structure and bonding: Lewis structure and VSEPR model||Explain the molecular structure based on the Lewis structure and VSEPR model.|
|Class 5||Valence bond theory and molecular orbital theory||Explain the valence bond theory and molecular orbital theory.|
|Class 6||Molecular orbital of diatomic molecules||Explain the molecular orbitals of diatomic molecules.|
|Class 7||Practice problems to assess the level of understanding and explanation of the answers||Understand the course contents and solve practice problems.|
To enhance effective learning, students are encouraged to spend approximately 100 minutes preparing for class and another 100 minutes reviewing class content afterwards (including assignments) for each class.
They should do so by referring to textbooks and other course material.
P. Atkins, T. Overton, J. Rourke, M. Weller, F. Armstrong, "Inorganic Chemistry", 6th Ed., Oxford University Press; ISBN: 978-0199641826.
Final examination (60%), level of class participation (40%) which is assessed by small quizzes and so on.
Students require the knowledge of physical chemistry and organic chemistry taught in the freshman year.
Toshiro Takao: takao.t.aa[at]m.titech.ac.jp
Shigeki Kuwata: skuwata[at]apc.titech.ac.jp
Contact by e-mail in advance to schedule an appointment.
Classes A and B are for the students with an odd and even student ID numbers, respectively.