[Description of the course] In this course, the instructor will explain acid-base reactions, redox reactions, and structures of crystalline solids to students who studied Inorganic Chemistry I (Chemical Bonding).
[Aim of the course] A chemical reaction involves formations and dissociations of chemical bonds that are initiated by transfers of valence electrons between the constituent atoms. Understanding the mechanisms of basic reactions as well as basic structures of crystalline solids is essential for comprehending the chemical nature of individual elements. Students gain an understanding of methods for describing the reactivity of acid-base and redox reactions, by using the Brønsted and Lewis acids and bases, HSAB rule, and electrochemical series. Also, they learn how a different atomic nature leads to different types of crystal structures and electronic structures in crystalline solids. Finally, students acquire the ability to discuss the reactivity of molecules and compounds and the chemical states of closely packed atoms based on the periodic table.
At the end of this course, students will be able to:
1) acquire basic knowledge about and approaches to acids, bases, and redox.
2) explain crystal structures of simple solids based on knowledge of the chemical nature of elements
3) discuss the reactivity of molecules and compounds and the chemical states of closely packed atoms based on the periodic table.
acid-base reaction, Brønsted acid and base, Lewis acid and base, redox reaction, electrochemical series, disproportionation, comproportionation, crystal structure, ionic bond, lattice enthalpy
|✔ Specialist skills||Intercultural skills||Communication skills||Critical thinking skills||Practical and/or problem-solving skills|
This lecture will proceed in the following order: (1) acid and base, (2) redox, (3) crystal structure of solids. In the last day, exercise problems and interpretation of the answers will be given to assess the students’ level of understanding.
|Course schedule||Required learning|
|Class 1||Acid and base||Understand how to represent the equilibrium of proton transfer quantitatively, using the acidity constant, and explain the features of the Brønsted acid-base.|
|Class 2||Acid-base reactions||Understand the characteristics of the Lewis acid-base, generalized for acceptor and donor of an electron-pair, and explain the principle of various acid-base reactions with no proton transfer.|
|Class 3||Redox pairs and electrochemical series||Understand how to represent the redox equilibrium quantitatively, using the standard potential of the redox couple, and derive the stability of the chemical species from the electrochemical series.|
|Class 4||Redox reactions||Using Latimer, Frost, Pourbaix, and Ellingham diagrams, explain the features of the redox reaction in the various environments.|
|Class 5||Crystal structures of solids||Understand the type and description methods of crystal structure, and represent a variety of crystal structure.|
|Class 6||Crystal structures of ionic solids||Understand the classification of some ionic solids and determine the bonding scheme and coordination number of them.|
|Class 7||Ionic bonding||Explain the thermodynamic properties of solids based on the theory of ion model.|
|Class 8||Practice problems and remarks for confirming the level of understanding||Use the exercise problems to better understand the topics covered, and evaluate one’s own progress.|
P. Atkins, T. Overton, J. Rourke, M. Weller, F. Armstrong, "Inorganic Chemistry", 6th Ed., Oxford University Press; ISBN: 978-0199641826.
Course materials are provided during class and uploaded on OCW-i.
Students will be assessed on their achievements of learning outcomes based on the final exam (60%) and exercise problems (40%).
No prerequisites are necessary, but enrollment in the related courses (Inorganic Chemistry I (Chemical Bonding) (CAP.B221.R)) is desirable.
Akira Ohtomo: aohtomo[at]apc.titech.ac.jp
Hajime Arai: arai.h.af[at]m.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.