| Course title | |||||
| 無機化学Ⅰ [Inorganic Chemistry Ⅰ] | |||||
| Course category | technology speciality courses,ets. | Requirement | Credit | 2 | |
| Department | Year | 1～4 | Semester | Fall | |
| Course type | Fall | Course code | 021315 | ||
| Instructor(s) | |||||
| 尾﨑 弘行 [OZAKI Hiroyuki] | |||||
| Facility affiliation | Faculty of Engineering | Office | Email address | ||
| Course description |
| Chemistry aims to reveal the natures and changes of substances. The natures depend on those of the constituent atoms while the changes stem from the arrangement and rearrangement of atoms. The combination of atoms affords various chemical bonds with the specific structures and properties of the substance. This course discusses such fundamentals of chemistry, taking various examples of inorganic simple substances and compounds. |
| Expected Learning |
| Learners who successfully complete this course will be able to understand the meaning of “orbital” and the necessity of the periodic law (Part 1), two ways of approaching covalent bonds (localized bonds approximation and delocalized molecular orbitals approximation) (Part 2), and several items proper to inorganic chemistry such as ionic solids, coordination compounds, and acids and bases (Part 3). |
| Course schedule |
|
Part 0 (Chapter 1, Section 2 in the text) Week 1 Characteristics of inorganic chemistry when compared with other fields of chemistry; Minimum knowledge on thermochemistry necessary for this course. Part 1 (Chapter 2) Week 2 Atomic orbitals (AOs) (1). Quantum numbers; Energy and degeneracy; Mathematical expressions; Real linear combinations. Week 3 AOs (2). Several ways depicting AOs; Born interpretation for the meaning of an orbital; Radial distribution function. Week 4 Periodic law (1). Pauli exclusion principle; Orbital penetration through inner shells; Aufbau principle; Electron configuration of atoms (period 1 - 4 elements); Irregularity in the order of orbital occupation. Week 5 Periodic law (2). Electron configuration of atoms (period 5 - 7 elements); Hund’s rule distributing electrons to degenerated orbitals; Ionization energies of atoms dependent on the atomic number; Definitions of electron negativity; Magnetism of chemical species. Part 2 (Chapter 3) Week 6 Localized bond approximation (1). Lewis structure; Resonance; Bonding pair and lone pair; Covalent bonds in beryllium hydride; sp hybrid orbitals. Week 7 Localized bond approximation (2). Covalent bonds in boron trifluoride, methane, and carbon dioxide; sp2 and sp3 hybrid orbitals; π and σ bond; Valence shell electron pair repulsion model; Shapes and bond angles of ABn molecules. Week 8 Midterm Examination (50 minutes) Molecular orbital (MO) approximation. Bonding and antibonding interactions in hydrogen molecular ion. Week 9 MO approximation for homonuclear diatomic molecules (1). Combinations of AOs affording σ, π, and δ MOs; Energy diagram; MO drawing and naming; Electron configuration. Week 10 MO approximation for homonuclear diatomic molecules (2). Electronic structures; Bond order and length; Binding energy; Magnetism. Part 3 Week 11 (Chapter 4) Ionic solids. Structural types and cation-anion radius ratio; Lattice energy; Madelung constant peculiar to the structural type; Born-Haber cycle. Week 12 (Chapter 5) Chemistry of selected anions. Oxide, hydroxide, and alkoxide ions; Oxoanions of C, N, P, S, halogens, and transition metals; Borates; Silicates; Aluminosilicates; Halogeno complex anions; Pseudohalogenide ions. Week 13 (Chapter 6, Sections 1 - 3) Structural aspects of coordination compounds. Coordination numbers and geometries; Ligand types; Isomerism; Nomenclature. Week 14 (Chapter 7) Solvents, solutions, acids, and bases. Characteristics of useful solvents; Protic and aprotic solvents; Definitions of acids and bases; Electronic and steric effects in acidity or basicity; Properties of common protic acids. Week 15 (Chapter 8, Sections 4 & 5) Structures and properties of some simple substances. Polyatomic molecules; Extended structures (chains, planes, and 3D-networks). |
| Prerequisites |
| Required Text(s) and Materials |
| F. A. Cotton, G. Wilkinson, and P. L. Gauss, “Basic Inorganic Chemistry”, 3rd Ed., Wiley, 1995. |
| References |
| Handouts will be distributed. Chapters 8 - 11 in Atkins’ “Physical Chemistry” 8th (or 9th) Ed., Oxford, 2006 (2009), will be of some help. |
| Assessment/Grading |
| Final examination (60 %); Midterm examination (30 %); Quizzes, Reports, and Attendance (10 %). |
| Message from instructor(s) |
|
Modern chemistry cannot be mastered by a memorization-only study; it has been constructed and systematized on the background of quantum theory. With this understanding, learners are expected to understand the fundamental concepts and principles indispensable not only for this course but for other courses in which the natures of individual chemical species are discussed. Depending on learners’ comprehension, explanation for certain items may be repeated; in that case the above mentioned schedule will be changed and some items will have to be omitted. |
| Course keywords |
| Atoms and molecules, Periodic law, Covalent bond, Ionic solids, Acids and bases |
| Office hours |
| Monday 12:00 - 13:00 (after the lecture) |
| Remarks 1 |
| Remarks 2 |
| Related URL |
| Lecture Language |
| Japanese |
| Language Subject |
| Last update |
| 3/22/2017 9:01:31 PM |