Inorganic chemistry covers a wide variety of disciplines, dealing with all elements in the periodic table. The aim of this class is to understand properties of elements and their compounds (e.g., chemical bonds, physical property, and reactivity) by focusing on electronic structures of atoms and molecules. The lecture starts with behaviors of electrons in atoms, which determine properties of elements, then moving on atomic parameters, changeable periodically, such as ionization energy, electron affinity, and electronegativity. In the molecular bonding theory section, the instructor tells you how to describe covalent molecules based on valence bond theory and VSEPR rule. Besides the basics of molecular orbital theory is introduced as a means of describing covalent molecules by referencing a simple diatomic molecule. The inorganic solids’ section includes the structures of ionic solids and metals, band theory, and the related thermodynamics. In the section of acid and base, the lecture begins with the definition of acid and base, and deals with factors governing acid strength by focusing on electronic configuration and molecular orbitals.
This class requests you to acquire fundamental knowledge on inorganic chemistry, thereby establishing a strong backbone toward upcoming more advanced classes. By repeating to ask yourself “why it is so?” and “why something happens?” and striving to gain essence of inorganic chemistry, you will be able to have a strong general foundation that may help you to understand a wide range of chemistry.
At the end of this course, students will be able to:
(1) explain/understand properties of elements and ions, based on the periodic table of the elements.
(2) explain reactivity of chemical species and stability of compounds.
(3) explain chemical bonds that consist of various materials.
Materials science, chemical bonding theory, physical property theory, solid state chemistry, acid and base
|Intercultural skills||Communication skills||Specialist skills||Critical thinking skills||Practical and/or problem-solving skills|
Topics change every 2-3 lessons. In each class, students are given exercise and homework related to what is taught on that day.
|Course schedule||Required learning|
|Class 1||Introductory lecture on inorganic chemistry, and the objectives of this class||Explain the course objectives.|
|Class 2||Atomic structure - Quantum number - Atomic orbital - Radial distribution||Explain the atomic structure and the correlation between each quantum number and atomic orbital.|
|Class 3||Atomic structure - The periodic table of the elements - Electronic configuration - Hund’s rule and Pauli’s exclusion law||Explain the correlation between atomic orbital and potential energy based on shielding and penetration, and draw electronic configuration of atoms up to the 4th period.|
|Class 4||The periodic table and atomic properties - The periodic table of the elements - Ionization energy - Electron affinity||Explain changes in ionization energy and electron affinity on the periodic table of the elements, based on the correlation between atomic orbital and potential energy.|
|Class 5||The periodic table and atomic properties - Electronegativity - Atomic (ionic) radius||Explain changes in electronegativity and atomic (ionic) radius on the periodic table of the elements, based on the correlation between atomic orbital and potential energy.|
|Class 6||Covalent bondings and molecular structure - Lewis structures - The octet rule - Resonance - Oxidation number and valence||Draw Lewis structure of covalent molecules based on the octet rule, and decide the oxidation number.|
|Class 7||Covalent bondings and molecular structure - Structures and bonding characters||Explain bonding properties of p-block elements, based on electronic configuration and electronegativity.|
|Class 8||Covalent bondings and molecular structure - Valence bond theory - VSEPR rule||Draw the structure of covalent molecules based on valence bond theory and VSEPR rule.|
|Class 9||Basics of molecular orbital theory - Bonding orbitals and untibonding orbitals||Draw the basic concept of molecular orbital theory by referencing a typical diatomic molecule.|
|Class 10||Basics of molecular orbital theory - Molecular orbital of diatomic molecules - Bond order||Draw a diagram of molecular orbitals of diatomic molecules. Explain the corrections among bond order, bond length, and bond enthalpy.|
|Class 11||Inorganic solids and their bondings - Classification of solids - Band theory - The structures of metals and their bondings - Ionic solids||Classify solids in terms of electron conductivity and draw band structures. Explain factors that govern the crystal structure of ionic solids.|
|Class 12||Inorganic solids and their bondings - Lattice defects - Lattice enthalpy - Born-Harber cycle||Explain why lattice defects are generated in crystalline solids in terms of thermodynamics. Explain what lattice enthalpy is, and calculate it based on the Born-Harber cycle.|
|Class 13||Acid and base - Definition of acid and base - Brønsted acidity||Explain the three definitions of acid and base. Explain factors that govern Brønsted acidity by referencing polybasic acid and hydrogen halides.|
|Class 14||Acid and base - Superacids - Leveling effect - Acidic/basic oxides||Explain what superacids are and how their acidity is quantitatively evaluated. Explain periodical change in acidity and basicity of oxides, based on their bonding character.|
|Class 15||Acid and base - Lewis acidity - HSAB theory - Solid acids||Explain what hard and soft in Lewis acids/bases mean, and the reactivity of them.|
Shriver-Atkins, Mukikagaku(Jo) The 6th edition, Tokyo Kagakudojin
Katsuhiko Miyoshi, "Hajimetemanabudaigakunomukikagaku" Kagakudojin
Additional documents may be distributed via OCW-i by the instructor if necessary.
Students' course scores are based on the final exam (80%) and exercise problems (20%).
No prerequisites, but enrollment in the related courses (Basic Inorganic Chemistry, Basic Quantum Chemistry, Basic Organic Chemistry, and Basic Chemical Thermodynamics) is desirable.