无机化学课程双语教学大纲.doc

The outline of bilingual teaching for Inorganic Chemistry无机化学课程双语教学大纲（For undergraduate education of pharmacy）1. The character, goal and task of the courseInorganic chemistry is the first basal course for related specialty, such as pharmacy, clinical medicine, etc. The inorganic chemists face the problem of ascertaining the structures, properties, and reactivity of and extraordinary range of materials, with widely differing properties and with exceedingly complicated patterns of structure and reactivity. We must hence be concerned with a number of different methods of synthesis, manipulation, and characterization of inorganic compounds. In accounting for the existence and in describing the behavior of inorganic materials, more will also be depicted, including thermodynamics, electronic structures of atoms, molecular bonding theories, reaction kinetics and the periodic relationships that exist among the types of substances, their structures and their reactivity. This course emphasizes three most important aspects of inorganic chemistry that include the structures, properties, and reactivity of the various inorganic substances, which we believe is the heart of chemistry. In doing so, one of the central themes to be found throughout the course is the periodic relationship that exists among the types of substances, their structures and their reactivity. 2. Elementary demands of the courseThere are three kinds of learning level for this course: master, familiarity and understand. You should deeply learn the content for mastering, and can skillfully use the elementary theories and concepts. As for the content to be familiar with, you should know very well the relative concepts and theories. You can just know the relative concepts and theories for the content to be understood. Through the study of inorganic chemistry, learners can master the elementary concepts, theories and knowledge of inorganic chemistry in a whole, including the thermochemistry, reaction rate, chemical equilibrium, acid-base equilibrium, precipitation-dissolution equilibrium, redox equilibrium, coordination equilibrium, periodic law of elements and substance structure. Furthermore, the major properties, structure, synthesis and application of important elements and their compounds will be mastered. Learners can also train their experimental skills by the experiment courses. All these can be helpful for their consequent courses, work and scientific research.The period of the bilingual teaching for Inorganic Chemistry is 90 including 54 for academic teaching and 36 for experimental course. The academic course is divided into 5 parts: (1) the elementary theories of chemistry; (2) the properties of solutions; (3) the structure of atoms and molecules; (4) coordination compounds; (5) part of elemental inorganic chemistry. The content of examination including the part for mastering (70%), the part for familiarity and understand (25%) and the part beyond this outline (5%).The teaching material for this outline is General Chemistry (1st edition ZHANG Yingshan, Beijing, Chemical Industry Press，2005).Recommendable teaching materials：1. Chemistry: The Central Science，8th, Theodore L. Brown et.al, 北京，机械工业出版社，2003年。2. General Chemistry, Jean B. Umland, Jon M. Bellama, 北京，机械工业出版社，2004 年。3.无机化学，李惠芝主编，北京，中国医药科技出版社，2002年。4无机化学第四版，大连理工大学无机教研室编，北京，高等教育出版社， 20015现代基础化学，朱裕贞, 顾达, 黑恩成编，北京，化学工业出版社，1998年。6化学(Chemistry, Schaums)，David E. Goldberg编，北京，高等教育出版社，2000年。7无机化学第三版，武汉大学等校编，北京，高等教育出版社，1999年。8无机化学丛书，张青莲主编，北京，科学出版社，陆续出版。9化学元素周期系，车云霞，申泮文主编，天津，南开大学出版社，1999年。3. The course content and distributing of period Chapter 1 Gases, Gas Phase Equilibria (5 period)Master:1. Chemical equilibrium in gaseous state: description and characteristics of chemical equilibrium, equilibrium expression and equilibrium constant, equilibrium position, relationship between Kp and Kc, characteristics and uses of equilibrium constant.2. The shift of chemical equilibrium: the effect of changes in concentration, pressure and temperature on equilibrium, Le Chteliers principle, the temperature dependence of equilibrium constant.Be familiar with:1. The partial pressures of components of a gas mixture: Daltons Law of partial pressures, mole fractions.2. The Perfect-Gas Law: the idea gas law.Understand:1. Diffusion and effusion.2. Real gases.3. Heterogeneous equilibria. Chapter 2 Chemical Thermodynamics (5 period)Master:1. Proper nouns and preliminaries of thermodynamics: system, surrounding, state, state function, process, pathway, phase, extend of reaction.2. First Law of Thermodynamics: the definition and signs of heat, work and thermodynamic energy, First Law of Thermodynamics.Be familiar with:1. Enthalpy, enthalpy change, calculation and characteristics of enthalpy changes, enthalpies of formation, standard enthalpy of formation, the application of Hesss Law.2. Spontaneous processes and entropy: the definition and characteristics of spontaneous processes, entropy, third law of thermodynamics, absolute entropy, the calculation of entropy changes in chemical reactions.3. Gibbs free energy: the definition of Gibbs free energy, standard free energies of formation, G calculation, Gibbs equation, G as a criterion for spontaneity, Gibbs free energy and equilibrium constant.Understand: The isothermal expansion of an ideal gas.Chapter 3 Chemical Kinetics (5 period)Master:1. Reaction rates: the definition, the average rate, the instantaneous rate.2. Rate laws and reaction order: rate law, rate constant, reaction order.Be familiar with:Determining the rate law: initial-rate method, integrated rate law method, half-life.Understand:1. Temperature and rate (a model for chemical kinetics): collision model, energy of activation, orientation effect, temperature, and reaction rate. (the Arrehenius equation).2. Reaction mechanisms: elementary reactions, reaction mechanisms, elementary step.3. Catalysis: catalyst, the characteristics of catalysis.Chapter 4 Atomic Structure and the Periodic Table of the Elements (8 period)Master:1. Electron configurations of atoms: building-up principle, Pauli exclusion principle, electron configurations, the periodic table, exceptions to the building-up principle.2. Electron diagrams of atoms: Hunds Law, magnetic properties of atoms.Be familiar with:1. The quantum mechanical description of atoms: de Broglie Waves, uncertainty principle, Schrdingers equation, wave functions, quantum numbers, electron spin quantum number, atomic orbital shapes and energies.2. Polyelectronic atoms: effective nuclear charge, penetration effect, energy level overlap.3. The periodic table: the relationship between the electron configuration and the periodic table. Be capable of ascertaining the location of any element in period table.4. Periodic trends in atomic properties: ionization energy, electron affinity, atomic radius.Understand:1. The development of the theories of atomic structure: Daltons atomic theory, basic composition of atoms.2. The birth of the quantum theory: the wave nature of light, the emission spectrum of light, Plancks constant.3. The structure of hydrogen atom: the atomic spectrum of hydrogen, Bohrs model, ground state, excited state, duality principle.Chapter 5 The Chemical Bond (7 period)Master:1. Some preliminaries: chemical bond, ionic bond, covalent bond, metallic bond.2. Covalent bond: definition, the localized electron bonding model. 3. Predicting the molecular structure with the VSEPR model. 4. Molecular orbital theory: the basic ideas, bonding and antibonding orbitals, bond order, bonding in homonuclear diatomic molecules, molecular orbital energy-level diagram for homonuclear diatomic molecules Be familiar with:1. Description of ionic bonds: formation of ionic bond, ion configurations of main-group elements and transition elements, ionic radii.2. Describing the valence electron arrangement: Lewis formula, octet rule, skeleton structure of a molecule.3. Valence bond theory-hybrid orbitals: basic ideas of valence bond theory, formation and types of hybrid orbitals, multiple bonding.4. Polar covalent bond: electronegativity, polar covalent bond and dipole moment.Understand:Bone energy: definition.Chapter 6 Liquid and Solid (3 period)Master:1. Intermolecular forces: definition, dipole-dipole forces, London forces, Hydrogen bond.2. The cause of hydrogen bond and its effect on some physical properties of substances.Be familiar with:Some properties of solids: vapor pressure, melting point, boiling point.Understand: Solid state, lattices, metallic crystals, ionic crystals, covalent network solids and phase transitions.Chapter 7 Acid-Base Equilibria (5 period)Master:1. Acid-Base concept: Arrhenius concept, Bronsted-Lowry concept of acids and bases, Lewis concept of acids and bases.2. The amphiprotic characteristics of water: base dissociation constant, acid dissociation constant, ion-product constant for water.3. Calculating the pH of weak acid solutions: calculating the pH of weak monoacid solutions, common ion effect.4. Buffered solutions: definition and components of buffered solutions, buffering capacity.Be familiar with:Relative strengths of acids and bases: acid-base conjugate pair, percent dissociation. Know how to compare the relative strength of acids and bases.Understand:1. The pH scale.2. Calculating the pH of polyprotic acid solutions.3. The calculation of the pH of a buffered solution (Henderson-Hasselbalch equation).Chapter 8 Solutions (5 period)Master:1. Solubility equilibria of slightly soluble solids in water: the solubility-product principle, solubility product constant, the relationship between solubility and solubility product, common ion effect.2. The precipitation and separating of ions: criterion for the formation of precipitates, ion product, pH and solubility, selective precipitation and its application. 3. Complex ion equilibria: definition, ligand, coordinate covalent bond, coordination number, complex-ion formation, complex ions and solubility. Be familiar with:Colligative properties: the vapor pressure lowering, boiling-point elevation, freezing-point depression, osmotic pressure, calculating colligative properties.Understand:Solubility: definition of solvent, solutes and solubility, the concentration of solutions, dependence of solubility on temperature and pressure.Chapter 9 Electrochemistry (5 period)Master:1. Preliminaries of redox reactions: oxidation, reduction, reducing agent, oxidizing agent.2. Electrochemical cells: half-reactions, the structure of electrochemical cells, cell potential and its measurement.3. Standard reduction potentials: definition and measurement, strength of and oxidizing or reducing agent.4. Uses of standard reduction potentials: spontaneous direction of redox reaction, calculation of cell potentials, standard-potential diagram.5. The standard-potential diagram and its application. Be familiar with:1. Dependence of the cell potential on concentration: Nernst equation and its application, concentration cells.Understand:Electrochemistry and thermodynamics: cell potential and free energy, equilibrium constants for oxidation-reduction reaction.Chapter 10 The Main-Group Elements (7 period)Be familiar with:1. The properties of the main-group elements: oxidation states, etc.2. The properties of group I A elements, the chemistry of hydrogen (preparation, hydrides, etc).3. The properties of group II A elements, group III A elements, group IV A elements, group V A elements, group VI A elements, group VII A elements and group VIII A elements.4. The chemistry of some typical elements: nitrogen, phosphorus and sulfur.2. Key exercises:1. Identify each of the following substances from the description.(1) A white, waxy solid, normally stored under water because it spontaneously bursts into flames when exposed to air.(2) A viscous liquid that reacts with table sugar, giving a charred mass.(3) An acid that etches glass.(4) A pale green gas that dissolves in aqueous sodium hydroxide to give a solution used as a bleach agent.2. Give two reasons why F2 is the most reactive of the halogens.Chapter 11 Transition Metals and Coordination Chemistry (8 period)Master:1. Complex ions and coordination compounds: formation, definition, coordination compound, types of ligands, naming.2. Structure and isomerism: definition, classification, stereoisomerism and optical isomerism.Be familiar with:1. Properties of the transition elements: ionization energies, electron configurations, oxidation states, atomic radii, melting points, boiling points and hardness.2. The chemistry of first-row transition metals: important chemical properties of scandium, titanium, vanadium, chromium, manganese, iron, cobalt, nickel, copper and zinc.3. Valence bond theory of complex ions: the formation of coordinate covalent bond, the steric conformation of complex, high-spin and low-spin complex ion, octahedral complexes, tetrahedral and square planar complexes, linear complex.Understand: The crystal field model: the ideas, effect of an octahedral field on the d orbitals, the distribution of electrons, spectrochemical series.The recommended period distributionchapter No.Content/chapter No.Experiment periodTheory period1chapter 1. Gases, Gas Phase Equilibria452chapter2.Chemical hermodynamics/53chapter 3. Chemical Kinetics/54chapter 4. Atomic Structure and the Periodic Table of the Elements/85chapter 5. The Chemical Bond/76chapter 6. Liquid and Solid837chapter 7. Acid-Base Equilibria458chapter 8. Solutions859chapter 9. Electrochemistry4510chapter 10. The main-group elements4711chapter 11.Transition metals and coordination chemistry48Total993663The outline of bilingual teaching for Inorganic Chemistry Experiments无机化学实验课程双语教学大纲（For undergraduate education of pharmacy）1. The guidance and purpose of experimental courseInorganic chemistry is the first basal course for related specialty, such as pharmacy, clinical medicine, etc. and it is a kind of subject based on experiments. “Inorganic chemical experiments” is a self-governed experimental course and is helpful for studying the “inorganic chemistry ” course. This experimental course is to investigate the important theories of inorganic chemistry, the behavior of typical elements and their compounds and the corresponding instrument, apparatus, operation, etc. Through the laboratory training, students will obtain lots of chemical information that is helpful for their learning of inorganic chemistry. They also gain experience of practical laboratory techniques and carry out chemical experiments, largely in connection with quantitative analysis and important chemical principles. In one hand, the learners will further understand the elementary theories and concepts of inorganic chemistry. On the other hand, the learners can train the primary skills for chemical experiments and be proficient in them, which can be helpful for their following study and investigation. 2. Elementary demands for experimental course2.1 An experiment course composed of experiments and lecture For the part of experiments, students should do 9 elementary and synthesis experiments to master the elementary operation, further understand the theoretic knowledge, master the general preparation and separation methods for inorganic compounds and obtain the ability to do overall experiments independently. At the same time, the lecture can make students attach importance to the safety. They will be familiar with the experimental methods and skills of inorganic chemistry.2.2 The course content The content of this experimental course includes basic knowledge and operation, elementary principles, elemental chemistry, the preparation of compounds and overall experiments. Through these trai