Course title
無機化学基礎   [Basic Inorganic Chemistry]
Course category	technology speciality courses,ets.	Requirement		Credit	2
Department		Year	1～4	Semester	Spring
Course type	Spring	Course code	021408
Instructor(s)
飯島 淳   [IJIMA Jun]
Facility affiliation	Graduate School of Engineering	Office		Email address

Course description

This course provides students with fundamentals of physical chemistry and inorganic chemistry. After getting the knowledge of atoms, the formation and mechanism of compound is lectured. To understand a variety of chemical reactions and phenomena, thermochemistry, kinetics, equilibrium, acids and bases, thermodynamics, electrochemistry are lectured. Finally, coordination chemistry is lectured.

Expected Learning

To acquire the basic chemical knowledge and to understand the phenomena from the view point of atomic and molecular level.

Course schedule

1. Guidance, structure of atom and stability 　　Law of mass conservation, Law of definite proportion, Law of multiple proportion Dalton’s atomic theory, atom, atomic number, Nuclear chemistry, Radioactivity 2. Periodicity of atoms and electronic structure 　　Electromagnetic wave, wave-particle duality, Uncertainty principle, wave function, orbital 　　Pauli exclusion principle, Electron configuration, Periodic table 3. Ionic bond and chemistry of main elements 　　Molecule, Ion, Ionic radius, Ionization energy, Electron affinity, Octet law, Ionic bond 　　Lattice energy 4. Covalent bond and molecular structure 　　Covalent bond, Electronegativity, Electron-dot structure, Formal charge, VSEPR 　　Valence bond theory, Hybrid orbital, Molecular orbital 5. Thermochemistry and chemical energy 　　State function, Hess’s law, Standard heats of formation, Dissociation energy, Enthalpy, Entropy 6. Properties and behaviors of gas 　　Gas laws, Ideal gas, Dalton’s law, Kinetic molecular theory of gases, Graham’s law, Real gas 7. Liquid, solid and phase transition 　　Polar covalent bond, Dipole moment, Intermolecular force, Phase transition X-ray crystallography, Ionic crystal, Covalent crystal 8. Properties of solution 　　Solubility, Solubility process, Colligative property, Raoult’s law, Elevation of boiling point 　　Depression of freezing point, osmotic pressure 9. Kinetics of chemical reaction 　　Reaction rate, Reaction order, First-order reaction, Second-order reaction, Half-life, Elementary reaction, Overall reaction, Arrhenius equation, Catalyst 10. Equilibrium of chemical reaction 　　Equilibrium constant, LeChatelier’s principle, Chemical equilibrium and kinetics 11. Acid and bases, and equilibrium in the aqueous solution 　　Definition of acids and bases, pH, Neutralization, Buffer solution, Henderson equation 12. Thermodynamics 　　Enthalpy, Entropy, Free energy, Second law of thermodynamics, chemical equilibrium 13. Electrochemistry 　　Galvanic cell, Standard potential, Nernst equation, Determination of pH, Standard potential of the cell, and equilibrium constant 14. Transition metals and coordination chemistry 　　Coordination compound, Ligand, Isomer, Chirality, Color of metal complex, Valence bond theory, 　　Crystal field theory 15. Final Examination

Prerequisites

Basic knowledge of chemistry learned in high school is required.

Required Text(s) and Materials

“McMurry General Chemistry” by John McMurry and Robert C. Fay

References

“Atkins General Chemistry” by P. Atkins, L. Jones, and L. Laverman “Spencer Basic Chemistry” by J. N. Spencer, G. M. Bodner, L. H. Rickard “Atkins Elements of Physical Chemistry” by P. Atkins, J. Paula

Assessment/Grading

Attendance and daily test (20%) Final examination (80%)

Message from instructor(s)

Based on the knowledge of chemistry in high school, basic chemistry is lectured.

Course keywords

Atom structure, Molecular structure, Bond formation, Thermochemistry, Kinetics, Equilibrium

Office hours

Remarks 1

Remarks 2

Related URL

Lecture Language

Language Subject

Last update

3/7/2018 9:52:50 AM