Outline of Inorganic Chemistry 一、 Basic information of the course Course Code CHM21700T English name of the Inorganic Chemistry course Type of the course Fundamental course Adapted specialty Chemistry science Term of giving classes 1ssemester of the 1st grade in university Total period 72 Total score 4.5 Parallel courses(code) Chemical experiments for university students Inorganic chemistry-a sub-branch of chemistry-is an important course for chemical engineering specialty and an important part for training engineers with complete knowledge structure and ability.The course is a bridge between knowledge of middle school and further deep theories,and also a base for further study. Brief introduction of the Through the course,students can master the basic principles of course chemical reactions,basic theories of structures of materials, theories of elements,new merging fields of inorganic chemistry, the inherent relationship of chemistry and practical industries, lives,as well as improve their preliminary ability in view of analyzing and solving chemistry relating problems,and ability to self-study chemistry. Recommended text [1]Dalian Institute of Technology,Inorganic Chemistry, books 5thEd.Beijing.Higher Education Press,2004;[2]
Outline of Inorganic Chemistry 一、 Basic information of the course Course Code CHM21700T English name of the course Inorganic Chemistry Type of the course Fundamental course Adapted specialty Chemistry science Term of giving classes 1 st semester of the 1st grade in university Total period 72 Total score 4.5 Parallel courses(code) Chemical experiments for university students Brief introduction of the course Inorganic chemistry - a sub-branch of chemistry - is an important course for chemical engineering specialty and an important part for training engineers with complete knowledge structure and ability. The course is a bridge between knowledge of middle school and further deep theories, and also a base for further study. Through the course, students can master the basic principles of chemical reactions, basic theories of structures of materials, theories of elements, new merging fields of inorganic chemistry, the inherent relationship of chemistry and practical industries, lives, as well as improve their preliminary ability in view of analyzing and solving chemistry relating problems, and ability to self-study chemistry. Recommended text books [1] Dalian Institute of Technology, Inorganic Chemistry, 5 th Ed.,．Beijing, Higher Education Press，2004; [2]
Raymond Chang.Chemistry,9h edition,McGraw Hill Education,1999 [1]Oxtoby,Gillis,Nachtrieb.Principhes of Modern Chemistry (Fifth).U.S.A.Thomson.2002 [2]C.E.Housecroft and A.G.Sharpe,Inorganic Chemistry,3rd edition,Pearson Education/Prentice Hall [3]F.A.Cotton,G.Wilkinson,C.A.Murillo,and M. Bochmann,Advanced Inorganic Chemistry,Six Edition, Willey Interscience,1999 [4]M.S.Silberberg,Chemistry-The Molecular Nature of Matter and Change,hed,,McGraw Hill,Boston,2006 [5]G.Rayner-Canham,T.Overton,Descriptive Inorganic References Chemistry,4h ed,Freeman&Co.New York,2006. 扩充性无机化学中文优秀教材 [山傅献彩主编大学化学（上、下册）.北京：高等教育出版 社，1999. [2]吉林大学，武汉大学，南开大学等校编，宋天佑等，无 机化学，（上、下册），高等教育出版社，2005. [3]唐有祺主编.当代无机化学前沿.北京：中国致公出版 社，1997. [4唐有祺，王夔主编化学与社会.北京：高等教育出版 社，1997. 二、Targets of the course education 1.Aims of the course in view of moral character
Raymond Chang, Chemistry, 9th edition，McGraw Hill Education, 1999. References [1] Oxtoby, Gillis, Nachtrieb. Principhes of Modern Chemistry. (Fifth).U.S.A. Thomson,2002 [2] C. E. Housecroft and A. G. Sharpe, Inorganic Chemistry, 3rd edition, Pearson Education/ Prentice Hall [3] F. A. Cotton, G. Wilkinson, C. A. Murillo, and M. Bochmann, Advanced Inorganic Chemistry, Six Edition, Willey Interscience, 1999 [4] M. S. Silberberg，Chemistry – The Molecular Nature of Matter and Change, 4th ed, , McGraw Hill, Boston, 2006 [5] G. Rayner-Canham, T. Overton, Descriptive Inorganic Chemistry, 4th ed, Freeman & Co., New York, 2006. 扩充性无机化学中文优秀教材 [1] 傅献彩主编. 大学化学(上、下册). 北京：高等教育出版 社，1999. [2] 吉林大学，武汉大学，南开大学等校编，宋天佑等，无 机化学，（上、下册），高等教育出版社，2005. [3] 唐有祺主编. 当代无机化学前沿. 北京：中国致公出版 社，1997. [4] 唐有祺，王 夔主编. 化学与社会. 北京：高等教育出版 社，1997. 二、 Targets of the course education 1．Aims of the course in view of moral character
Dialectic materialism theories will be utilized during the course to explain chemical basic principles and rules of elements and chemical reactions,in order to promote formation of Weltanschauung of dialectic materialism. Try to help students to understand some questions of wide interest in order to enrich their social responsibilities,strengthen their understanding about that science and technology is the first fertility,let them get to know the current status of the chemistry and chemical industries in the world,inspire their proper attitude towards study,love and get them to devote to chemistry and chemical technology relating career. 2.Aims in view of specialty knowledge and ability Teach student scientific thinking way,help them adapt study in university and improve their ability for self-study and self-solving chemistry questions. Combine new development of the chemical industries,reflect the developing trends of inorganic chemistry and its practical applications in high technologies, stimulate students'enthusiasm and consciousness,incubate their independence,activity and creativity The contents of the course is set up at three different levels,namely,(1)to master(learn),(2)to be familiar with (understand),and (3)to know. Contents and requirements on theory teaching(including time distribution) Chapter 1.Preface and introduction (1.5 hrs) $1.1 Chemistry---the central science full of practicability and creativity $1.2 Features of chemical changes $1.3 History,revival and development of inorganic chemistry $1.4 How to study easily but efficiently inorganic chemistry $1.5 Styles and forms of examination for the course This chapter mainly consists of brief introduction about the status of chemistry,features of chemical changes,the history,revival and development of inorganic chemistry,how to study effectively and efficiently inorganic chemistry,clarifying requirements,and course plan and styles of examinations Chapter 2 Thermochemistry(2.0 hrs) $2.1 Basic terms in thermodynamics $2.2 the First law of thermodynamics $2.3 Heat of a chemical reaction $2.4 the Hess's law aims of teaching:
Dialectic materialism theories will be utilized during the course to explain chemical basic principles and rules of elements and chemical reactions, in order to promote formation of Weltanschauung of dialectic materialism. Try to help students to understand some questions of wide interest in order to enrich their social responsibilities, strengthen their understanding about that science and technology is the first fertility, let them get to know the current status of the chemistry and chemical industries in the world, inspire their proper attitude towards study, love and get them to devote to chemistry and chemical technology relating career. 2．Aims in view of specialty knowledge and ability Teach student scientific thinking way, help them adapt study in university and improve their ability for self-study and self-solving chemistry questions. Combine new development of the chemical industries, reflect the developing trends of inorganic chemistry and its practical applications in high technologies, stimulate students’ enthusiasm and consciousness, incubate their independence, activity and creativity The contents of the course is set up at three different levels, namely, (1) to master (learn)，(2) to be familiar with (understand), and (3) to know. 三、 Contents and requirements on theory teaching (including time distribution) Chapter 1. Preface and introduction （1.5 hrs） §1.1 Chemistry---the central science full of practicability and creativity §1.2 Features of chemical changes §1.3 History, revival and development of inorganic chemistry §1.4 How to study easily but efficiently inorganic chemistry §1.5 Styles and forms of examination for the course This chapter mainly consists of brief introduction about the status of chemistry, features of chemical changes, the history, revival and development of inorganic chemistry, how to study effectively and efficiently inorganic chemistry, clarifying requirements, and course plan and styles of examinations Chapter 2 Thermochemistry (2.0 hrs） §2.1 Basic terms in thermodynamics §2.2 the First law of thermodynamics §2.3 Heat of a chemical reaction §2.4 the Hess’s law aims of teaching：
To know the concepts of system,surrounding,phase etc,and to be familiar with the Law of conservation and conversion of energy in chemical reactions.To understand the concepts of state function,enthalpy,molar enthalpy change,standard molar enthalpy of formation and so on.To master thermochemical equation, enthalpy change of a reaction,Hess'law and related calculation. important and difficult points Law of conservation and conversion of energy in chemical reactions.Heat and work are two forms of energy transfer between systems and surroundings. Reaction enthalpy is dependent on composition,state and condition of the chemical reaction. Paying attention on how to write thermochemical equation.Calculation of standard molar enthalpy change of a reaction Afrom standard molar enthalpy of formation of substancesA The essential of Hess'law:enthalpy is a state function,the enthalpy change of a reaction is constant,whether the reaction is carried out directly in one step or indirectly through a number of steps Chapter 3 Chemical kinetics(self-study) $3.1 Brief introduction of chemical reaction rates $3.2 Brief introduction of effect of concentration of reactants on reaction rate-the rate expression $3.3 Brief introduction of effect of temperature on reaction rate-Arrhenius equation $3.4 Brief introduction of theory of reaction rate and reaction mechanisms $3.5 Brief introduction of catalyst and catalysis aims of study To understand the concepts of reaction rate,order of a reaction and reaction rate expression.To master the concepts of activity energy,activated molecule,and to explain essential of the influence of concentration,catalyst on rate of a particular chemical reaction.To master reaction rate expression. important and difficult points Concept of reaction rate under constant pressure and temperature.Reaction rate expression in the case of complex reaction has to be determined by experiments.Rate constant k,and the order of a reaction a.B.Collision theory,activated complex.The concepts of activation energy,activated molecule,the influence of concentration,temperature,catalyst on a particular chemical reaction. Chapter 4 Chemical equalibria,entropy,and Gibbs function (5.0 hrs)
To know the concepts of system, surrounding, phase etc, and to be familiar with the Law of conservation and conversion of energy in chemical reactions. To understand the concepts of state function, enthalpy, molar enthalpy change, standard molar enthalpy of formation and so on. To master thermochemical equation, enthalpy change of a reaction, Hess’ law and related calculation. important and difficult points Law of conservation and conversion of energy in chemical reactions. Heat and work are two forms of energy transfer between systems and surroundings. Reaction enthalpy is dependent on composition, state and condition of the chemical reaction. Paying attention on how to write thermochemical equation. Calculation of standard molar enthalpy change of a reaction ΔfHm Q from standard molar enthalpy of formation of substances ΔfHm Q. The essential of Hess’ law: enthalpy is a state function, the enthalpy change of a reaction is constant, whether the reaction is carried out directly in one step or indirectly through a number of steps. Chapter 3 Chemical kinetics (self-study) §3.1 Brief introduction of chemical reaction rates §3.2 Brief introduction of effect of concentration of reactants on reaction rate —the rate expression §3.3 Brief introduction of effect of temperature on reaction rate—Arrhenius equation §3.4 Brief introduction of theory of reaction rate and reaction mechanisms §3.5 Brief introduction of catalyst and catalysis aims of study To understand the concepts of reaction rate, order of a reaction and reaction rate expression. To master the concepts of activity energy, activated molecule, and to explain essential of the influence of concentration, catalyst on rate of a particular chemical reaction. To master reaction rate expression. important and difficult points Concept of reaction rate under constant pressure and temperature. Reaction rate expression in the case of complex reaction has to be determined by experiments. Rate constant k, and the order of a reaction α、β. Collision theory, activated complex. The concepts of activation energy, activated molecule, the influence of concentration, temperature, catalyst on a particular chemical reaction. Chapter 4 Chemical equalibria, entropy, and Gibbs function（5.0 hrs）
$4.1 The standard equilibrium constant $4.2 The application of the standard equilibrium constant $4.3 The shift of a chemical equilibrium $4.4 Spontaneous reactions and entropy $4.5 Gibbs function aims of teaching: To be familiar with the concept of shift of a chemical equilibrium,calculation of stand equilibrium constant and compositions of a reaction from thermodynamic functions or Van't Hoff equation equilibrium.To be familiar with reaction quotient criterion,Le Chatelier principle,to master how concentration,pressure, temperature influence a shift of chemical equilibrium and related calculation.To know the concepts of standard molar entropy Sstandard molar Gibbs function of formation AGm,simple calculation of standard molar entropy change ASand standard molar Gibbs function change of a reaction ArGm,the relationship amongandStojudge in principle the direction and extent of a chemical reaction based onandA important and difficult points: Calculation of stand equilibrium constant of a reaction from thermodynamic functions or Van't Hoff equation.Summarizing the parameters influencing chemical equilibrium shift and rules of chemical equilibrium shift,understanding on the Le Chatelier principle. Chapter 5 Acid-base equilibria (8.0 hrs) 5.1 The Brensted theory of acids and bases $5.2 Ionization equilibrium of water and the pH scale 5.3 Equilibria in solutions of weak acids and weak bases 5.4 Buffer solutions 5.5 Acid-bases indicators 5.6 Lewis acids and bases and coordination compounds 5.7 Complexation reaction and coordination equilibria aims of teaching:
§4.1 The standard equilibrium constant §4.2 The application of the standard equilibrium constant §4.3 The shift of a chemical equilibrium §4.4 Spontaneous reactions and entropy §4.5 Gibbs function aims of teaching: To be familiar with the concept of shift of a chemical equilibrium, calculation of stand equilibrium constant and compositions of a reaction from thermodynamic functions or Van’t Hoff equation equilibrium. To be familiar with reaction quotient criterion, Le Châtelier principle, to master how concentration, pressure, temperature influence a shift of chemical equilibrium and related calculation. To know the concepts of standard molar entropy Sm Q, standard molar Gibbs function of formation DfGm Q , simple calculation of standard molar entropy change DSm Q and standard molar Gibbs function change of a reaction DrGm Q, the relationship among DrGm Q , DrHm Q and DrSm Q , to judge in principle the direction and extent of a chemical reaction based on DrGm and DrGm Q. important and difficult points: Calculation of stand equilibrium constant of a reaction from thermodynamic functions or Van’t Hoff equation. Summarizing the parameters influencing chemical equilibrium shift and rules of chemical equilibrium shift, understanding on the Le Châtelier principle. Chapter 5 Acid-base equilibria（8.0 hrs） § 5.1 The Brønsted theory of acids and bases § 5.2 Ionization equilibrium of water and the pH scale § 5.3 Equilibria in solutions of weak acids and weak bases § 5.4 Buffer solutions § 5.5 Acid-bases indicators § 5.6 Lewis acids and bases and coordination compounds § 5.7 Complexation reaction and coordination equilibria aims of teaching:
To know essential points of the Bronsted theory of acids and bases and basic concepts on the theory about Lewis acids and bases.To master ionization of water. standard ion-product constant of water,and calculation of pH of strong acid and strong base.To master the ionization equilibria of monoprotic weak acid and weak base,the calculation of equilibrium composition;to be familiar with equilibrium of stepwise process of polyprotic weak acid and calculation of equilibrium composition. To master the ionization equilibrium in solutions of salt of monoprotic weak acid and strong base,and salt of monoprotic weak bases and strong acid,calculation of equilibrium composition,to be familiar with multi-step hydrolysis of salt of polyprotic weak acid and calculation of equilibrium composition.To master the concepts of common ion effect and buffer solution,and calculation of pH of a buffer solution.To master the basic concepts on complex,to know how to name a complex,To master complex formation reaction and its equilibrium,to know calculation of equilibrium composition,to know calculation of equilibrium composition under the condition of coexistence of equilibrium of acid and base reaction and dissociation equilibrium of complex. important and difficult points: Essential points of the Bronsted theory of acids and bases:concepts of acid,base,amphiprotic substance;conjugate acid-base pair.The essential of acid-base reaction is transfer of protons.The essential of ionization of water,ionization of acid and base,as well as that hydrolysis of salt are transfer of protons.The major content on Lewis acids and bases:the concept of Lewis acids and bases.The ligand in a complex is Lewis base.lonization equilibrium of water:ion- product constant of water,influence of temperature on ion-product constant of water,T=298K.Kw(298K)=1.0x1014 PH=-Igc(H+))POH=- lg'c(OH-)1,298K,PH+POH=14.00.Of importance is to master the ionization equilibrium in solutions of monoprotic weak acids and weak bases,ionization equilibrium constant,percent ionizaton(),calculation of equilibrium composition and pH of a reaction,the conditions for approximate calculation and methods of calculation.To master the ionization equilibrium in solutions of salt of monoprotic weak acid and strong base,and salt of monoprotic weak bases and strong acid,the relationship between constant of ionization of water and constant of ionization of acid and base.Features of salt of polyprotic weak acids:multi-steps hydrolysis;relationship between ionization constant and hydrolysis constant,simple calculation of hydrolysis equilibrium of salt of polyprotic weak aicd and strong base(treat it as an equilibrium of hydrolysis of polyprotic base). To be familiar with concepts of ligand,coordination atom,coordination number etc about coordination compound,naming normal compounds,distinguish simple and chelating complexes,ie,normal ligands.The dissociation equilibrium of complex(stepwise process),dissociation equilibrium constant,stability constant(stepwise process).relationship of dissociation equilibrium constant and stability constant,calculation of equilibrium composition. Chapter 6 Precipitation-solubility equilibria (4.0 hrs) 6.1 Solubility and solubility product 6.2 Forming and dissolving of precipitates $6.3 Equilibrium between two precipitates
To know essential points of the Brønsted theory of acids and bases and basic concepts on the theory about Lewis acids and bases. To master ionization of water, standard ion-product constant of water, and calculation of pH of strong acid and strong base. To master the ionization equilibria of monoprotic weak acid and weak base, the calculation of equilibrium composition; to be familiar with equilibrium of stepwise process of polyprotic weak acid and calculation of equilibrium composition. To master the ionization equilibrium in solutions of salt of monoprotic weak acid and strong base, and salt of monoprotic weak bases and strong acid, calculation of equilibrium composition, to be familiar with multi-step hydrolysis of salt of polyprotic weak acid and calculation of equilibrium composition. To master the concepts of common ion effect and buffer solution,and calculation of pH of a buffer solution. To master the basic concepts on complex, to know how to name a complex, To master complex formation reaction and its equilibrium, to know calculation of equilibrium composition, to know calculation of equilibrium composition under the condition of coexistence of equilibrium of acid and base reaction and dissociation equilibrium of complex. important and difficult points： Essential points of the Brønsted theory of acids and bases: concepts of acid, base, amphiprotic substance; conjugate acid-base pair. The essential of acid-base reaction is transfer of protons. The essential of ionization of water, ionization of acid and base, as well as that hydrolysis of salt are transfer of protons. The major content on Lewis acids and bases: the concept of Lewis acids and bases. The ligand in a complex is Lewis base. Ionization equilibrium of water: ionproduct constant of water , influence of temperature on ion-product constant of water, T = 298K, KW Q(298K)=1.0×10-14 , PH=-lg{c(H+)},POH=- lg{c(OH-)},298K时，PH+POH=14.00. Of importance is to master the ionization equilibrium in solutions of monoprotic weak acids and weak bases, ionization equilibrium constant, percent ionizaton (a), calculation of equilibrium composition and pH of a reaction, the conditions for approximate calculation and methods of calculation. To master the ionization equilibrium in solutions of salt of monoprotic weak acid and strong base, and salt of monoprotic weak bases and strong acid, the relationship between constant of ionization of water and constant of ionization of acid and base. Features of salt of polyprotic weak acids: multi-steps hydrolysis; relationship between ionization constant and hydrolysis constant; simple calculation of hydrolysis equilibrium of salt of polyprotic weak aicd and strong base (treat it as an equilibrium of hydrolysis of polyprotic base). To be familiar with concepts of ligand, coordination atom, coordination number etc about coordination compound, naming normal compounds, distinguish simple and chelating complexes, i.e., normal ligands. The dissociation equilibrium of complex (stepwise process), dissociation equilibrium constant , stability constant (stepwise process), relationship of dissociation equilibrium constant and stability constant, calculation of equilibrium composition. Chapter 6 Precipitation-solubility equilibria （4.0 hrs） § 6.1 Solubility and solubility product § 6.2 Forming and dissolving of precipitates § 6.3 Equilibrium between two precipitates
aims of teaching: To be familiar with equilibrium of dissolving and forming of a sparingly soluble electrolyte,to master standard solubility product constant,the relationship with solubility,and related calculation.To master solubility product rule,to know how to judge forming or dissolving of a precipitate based on solubility product rule. To master the effect of pH on solubility of sparingly soluble metal sulfides and metal hydroxides and related calculation;to be familiar with simple calculation of equilibrium of complexing-dissolving of precipitate.To know Equilibria between two precipitates and related calculation. important and difficult points: Definition of solubility product.Forming and dissolving of precipitates comes to an equilibrium.solubility product.Relationship between solubility and solubityroduct,andthe readcalcuo The sotproduct rue Thetino precipitationsouqba forming precipitate:p forming saturated solution;dissolving precipitate.Shift of an equilibrium between forming and dissolving of precipitate.Shift of an quilibrium can occur through either changing pH of solution,formation of complex,or transformation between two precipitate.The key point to be familiar with dissolving-forming equilibria is to understand the relationship between precipitation reaction and muti-equilibria.To deeply understand a few examples. Chapter 7 Redox Reactions and Electrochemistry (7.0 hrs) $7.1 The fundamental concepts of redox reactions $7.2 Electrochemical cells $7.3 Electrode potentials $7.4 Application of electrode potentials aims of teaching: To be familiar with basic concepts on redox reaction,and balancing redox equations using ion-electron method.To know the concepts about galvanic(voltaic) cell and electromotive force.To master the concept of electrode potential and affecting parameters,the Nernst equation and related simple calculation, application of electrode potentials.To master elemental potential diagram and its application. important and difficult points:
aims of teaching: To be familiar with equilibrium of dissolving and forming of a sparingly soluble electrolyte, to master standard solubility product constant, the relationship with solubility, and related calculation. To master solubility product rule, to know how to judge forming or dissolving of a precipitate based on solubility product rule. To master the effect of pH on solubility of sparingly soluble metal sulfides and metal hydroxides and related calculation; to be familiar with simple calculation of equilibrium of complexing-dissolving of precipitate. To know Equilibria between two precipitates and related calculation. important and difficult points: Definition of solubility product. Forming and dissolving of precipitates comes to an equilibrium. solubility product. Relationship between solubility and solubility product, and the related calculation. The solubility product rule: The reaction quotient criterion for precipitation—solubility equilibria: J > Ksp Q, forming precipitate; J = Ksp Q, forming saturated solution; J > Ksp Q, dissolving precipitate. Shift of an equilibrium between forming and dissolving of precipitate. Shift of an quilibrium can occur through either changing pH of solution, formation of complex, or transformation between two precipitate. The key point to be familiar with dissolving-forming equilibria is to understand the relationship between precipitation reaction and muti-equilibria. To deeply understand a few examples. Chapter 7 Redox Reactions and Electrochemistry（7.0 hrs） §7.1 The fundamental concepts of redox reactions §7.2 Electrochemical cells §7.3 Electrode potentials §7.4 Application of electrode potentials aims of teaching: To be familiar with basic concepts on redox reaction, and balancing redox equations using ion-electron method. To know the concepts about galvanic(voltaic) cell and electromotive force. To master the concept of electrode potential and affecting parameters, the Nernst equation and related simple calculation, application of electrode potentials. To master elemental potential diagram and its application. important and difficult points:
How to balance redox equations using ion-electron method,electromotive force of a cell and electrode potentials.The Nernst equation and related simple calculation,analysis on the influence of concentration on electrode potential.Principle of concentration-differing cell.Element potential diagram and its application,Predicting the relative strength of an oxidizing agent and a reducing agent,Predicting the direction of a redox reaction,calculation of standard equilibrium constant. Chapter 8 atomic structure (6.0 hrs) 8.1 The atomic structure of hydrogen 8.2 The atomic structure of many-electron atoms 8.3 Periodic law of elements aims of teaching: To understand the hydrogen spectrum and the concept of energy level.To understand the concepts of atomic orbital function y2-the distribution of electron density in three-dimensional space around the nucleus,electron cloud and etc..to be familiar with the names,symbols,values and meanings of the four quantum numbers;to be familiar with the shapes and spatial configuration of s,p,d atomic orbits and electron clouds.To master the approximate energy level plot of multi-electron atoms and electron configuration,and identifying the position in the periodic table. To master the periodic table,the rules of periodic trends of atomic radii,ionization energy,affinity energy and atom electro negativity. important and difficult points: The hydrogen spectrum and orbital energy levels.State of electron movement,Schrodinger equation,wave function and electron cloud.Wave function using quantum numbers to describe state of electron movement is called atomic orbit. Atom electron configurations and atomic orbital energy levels,the three rules of electron configuration,the shielding effect and penetrating effect Periodic table,the rules of periodic trends of atomic radii,ionization energy,affinity energy and atom electronegativity. Chapter 9 molecular structure (6.0 hrs) $9.1 Valence Bond Theory $9.2 Valence Shell Electron Pair Repulsion(VSEPR)Theory $9.3 Molecular Orbital Theory $9.4 Bond Parameters
How to balance redox equations using ion-electron method, electromotive force of a cell and electrode potentials. The Nernst equation and related simple calculation, analysis on the influence of concentration on electrode potential. Principle of concentration-differing cell. Element potential diagram and its application, Predicting the relative strength of an oxidizing agent and a reducing agent, Predicting the direction of a redox reaction, calculation of standard equilibrium constant. Chapter 8 atomic structure （6.0 hrs） 8.1 The atomic structure of hydrogen 8.2 The atomic structure of many-electron atoms 8.3 Periodic law of elements aims of teaching: To understand the hydrogen spectrum and the concept of energy level. To understand the concepts of atomic orbital function Ψ 2 - the distribution of electron density in three-dimensional space around the nucleus, electron cloud and etc.. to be familiar with the names, symbols, values and meanings of the four quantum numbers ; to be familiar with the shapes and spatial configuration of s, p, d atomic orbits and electron clouds. To master the approximate energy level plot of multi-electron atoms and electron configuration, and identifying the position in the periodic table. To master the periodic table, the rules of periodic trends of atomic radii, ionization energy, affinity energy and atom electro negativity. important and difficult points: The hydrogen spectrum and orbital energy levels. State of electron movement, Schrödinger equation, wave function and electron cloud. Wave function using quantum numbers to describe state of electron movement is called atomic orbit. Atom electron configurations and atomic orbital energy levels, the three rules of electron configuration, the shielding effect and penetrating effect. Periodic table, the rules of periodic trends of atomic radii, ionization energy, affinity energy and atom electronegativity. Chapter 9 molecular structure （6.0 hrs） §9.1 Valence Bond Theory §9.2 Valence Shell Electron Pair Repulsion (VSEPR) Theory §9.3 Molecular Orbital Theory §9.4 Bond Parameters
aims of teaching: To be familiar with basic essentials,features and classificationof covalent bond.To be familiar with concept and classification of hybrid orbitals,to acquire the ability to explain the geometries of simple molecules or multi-atom ions.To understand the essentials of valence shell electron pair repulsion theory and the way to guess the geometries of simple molecules or multi-atom ions.To know the concept of molecular orbital,the energy level plot of the 2ed row in the periodic table and the configuration of configuration of electrons in molecular orbital,predicting their magnetic property and stability.To know the concepts on bond energy,bond length,bond angle,bond moment,bond order,polarity of bond and molecule. important and difficult points: Valence bond theory,hybrid orbital theory,Valence Shell Electron Pair Repulsion Theory.Symmetry of atomic and molecular orbits.Parameters describing characteristics of chemical bonds are comprised of bond energy,bond length,bond angle,bond moment,bond order etc,together with related bond dissociation energy,atomization energy,covalent bond radii and so on.Intermolecular force and hydrogen bond,dipole moment and polarizability of molecules. Chapter 10 solid structure (4.0 hrs) $10.1 The Structures and Types of Crystals $10.2 Metallic Crystals $10.3 Ionic Crystals $10.4 Molecular Crystals $10.5 Network Crystals Aims of teaching: To be familiar with crystal types,features and the interaction force among the particles in a crystal.To know the structures and characteristics of the three types of close packing;to understand the formation and characteristics of a metal bond.To be familiar with the structural features of the three typical types of ionic crystal;to understand the concept of crystal lattice energy and influence of ion charge and radii on crystal lattice energy;to be familiar with influence of crystal lattice energy on melting point,hardness of ionic crystal;to understand the calculation method of crystal lattice energy using thermchemistry.To know ionic radii and the rule of transform of ionic radii,ionic polarization and influence of ionic polarization on bond type,crystal lattice type,solubility,melting point,and color.To know dipolar moment and polarizability of molecules and the rule of transform of them;to know the origin of intermolecular force and influence of intermolecular on physical properties;to know the condition of formation of hydrogen bonds and influence of hydrogen bonds on some physical properties. important and difficult points:
aims of teaching: To be familiar with basic essentials, features and classificationof covalent bond. To be familiar with concept and classification of hybrid orbitals, to acquire the ability to explain the geometries of simple molecules or multi-atom ions. To understand the essentials of valence shell electron pair repulsion theory and the way to guess the geometries of simple molecules or multi-atom ions. To know the concept of molecular orbital, the energy level plot of the 2ed row in the periodic table and the configuration of configuration of electrons in molecular orbital, predicting their magnetic property and stability. To know the concepts on bond energy, bond length, bond angle, bond moment, bond order, polarity of bond and molecule. important and difficult points: Valence bond theory, hybrid orbital theory, Valence Shell Electron Pair Repulsion Theory. Symmetry of atomic and molecular orbits. Parameters describing characteristics of chemical bonds are comprised of bond energy, bond length, bond angle, bond moment, bond order etc, together with related bond dissociation energy, atomization energy , covalent bond radii and so on. Intermolecular force and hydrogen bond, dipole moment and polarizability of molecules. Chapter 10 solid structure （4.0 hrs） §10.1 The Structures and Types of Crystals §10.2 Metallic Crystals §10.3 Ionic Crystals §10.4 Molecular Crystals §10.5 Network Crystals Aims of teaching: To be familiar with crystal types, features and the interaction force among the particles in a crystal. To know the structures and characteristics of the three types of close packing; to understand the formation and characteristics of a metal bond. To be familiar with the structural features of the three typical types of ionic crystal; to understand the concept of crystal lattice energy and influence of ion charge and radii on crystal lattice energy; to be familiar with influence of crystal lattice energy on melting point, hardness of ionic crystal; to understand the calculation method of crystal lattice energy using thermchemistry. To know ionic radii and the rule of transform of ionic radii, ionic polarization and influence of ionic polarization on bond type, crystal lattice type, solubility, melting point, and color. To know dipolar moment and polarizability of molecules and the rule of transform of them; to know the origin of intermolecular force and influence of intermolecular on physical properties; to know the condition of formation of hydrogen bonds and influence of hydrogen bonds on some physical properties. important and difficult points:
Packing arrangement of ions and voids in a crystal;the closed packed arrangements:hexagonal closed packing,face-centered cubic close packing,body- centered cubic close packing.Crystals are divided into metallic crystals,ionic crystals,atomic crystals,molecular crystals according to the difference of the types of particle and the forced among them;crystals of different types have different physical properties.Ionic radii and types of ionic crystals.The strength of the forces among ions in an ionic crystal can be measured in view of crystal lattice energy.The extent of polarization effect of an ion is dependent on polarizing force and polarizability of the ion.In an ionic crystal,polarization of ion results in transformation chemical bond types and crystal types,the corresponding physical properties such as melting point,solubility,decomposition temperature,extent of hydrolysis of a salt,color will change. Chapter 11 structures of coordination compounds (4.5 hrs) $11.1 Configurations and Magnetism of Coordination Compounds $11.2 Chemical Bonding Theory in Complexes Aims of teaching: To be familiar with the essentials of valence bond theory,the relationship between geometry of a complex with the hybridization type of its central ion.To know the concepts of outer-orbital and inner-orbital type complexes,the relationship between electron configuration of the central ion and stability and magnetism of the complex ion.To know the essentials of crystal filed theory on complex;to know the electron configuration in a octahedral field and the concept of high spin and low spin,to predict stability and magnetism of a complex;to know the relationship of color of complex with d-d transfer. important and difficult points: valence bond theory,crystal field theory,molecular orbital theory.Explaining some properties of complexes based on these theories.Calculating the number of un-paired electrons from experimental magnetic moment,predicting the configuration of valence electrons of the central cation and the adopted hybridization types of the central cation;determining whether the complex is outer-orbital type or iner-orbital type,and explaining the relative stabilities of complexes.On the basis of relative difference in value of the crystal field splitting energy and electron pairing energy,judge the electron configuration in various atomic orbitals of an atom in a crystal filed,predict the type of a complex,determine the magnetic property,estimate the magnetic moment of the complex,and further on calculate crystal field stabilization energy,explain the relative stabilities of complexes. Chapter 12 the s block elements (2.0 hrs) $12.1 The general properties of the s-block elements $12.2 The elementary substances $12.3 The properties of the alkali and alkaline earth compounds
Packing arrangement of ions and voids in a crystal; the closed packed arrangements: hexagonal closed packing, face-centered cubic close packing, bodycentered cubic close packing. Crystals are divided into metallic crystals, ionic crystals, atomic crystals, molecular crystals according to the difference of the types of particle and the forced among them; crystals of different types have different physical properties. Ionic radii and types of ionic crystals. The strength of the forces among ions in an ionic crystal can be measured in view of crystal lattice energy. The extent of polarization effect of an ion is dependent on polarizing force and polarizability of the ion. In an ionic crystal, polarization of ion results in transformation chemical bond types and crystal types, the corresponding physical properties such as melting point, solubility, decomposition temperature, extent of hydrolysis of a salt, color will change. Chapter 11 structures of coordination compounds （4.5 hrs） §11.1 Configurations and Magnetism of Coordination Compounds §11.2 Chemical Bonding Theory in Complexes Aims of teaching: To be familiar with the essentials of valence bond theory, the relationship between geometry of a complex with the hybridization type of its central ion. To know the concepts of outer-orbital and inner-orbital type complexes, the relationship between electron configuration of the central ion and stability and magnetism of the complex ion. To know the essentials of crystal filed theory on complex; to know the electron configuration in a octahedral field and the concept of high spin and low spin, to predict stability and magnetism of a complex; to know the relationship of color of complex with d-d transfer. important and difficult points: valence bond theory, crystal field theory, molecular orbital theory. Explaining some properties of complexes based on these theories. Calculating the number of un-paired electrons from experimental magnetic moment; predicting the configuration of valence electrons of the central cation and the adopted hybridization types of the central cation; determining whether the complex is outer-orbital type or iner-orbital type, and explaining the relative stabilities of complexes. On the basis of relative difference in value of the crystal field splitting energy and electron pairing energy, judge the electron configuration in various atomic orbitals of an atom in a crystal filed, predict the type of a complex, determine the magnetic property, estimate the magnetic moment of the complex, and further on calculate crystal field stabilization energy, explain the relative stabilities of complexes. Chapter 12 the s block elements （2.0 hrs） §12.1 The general properties of the s-block elements §12.2 The elementary substances §12.3 The properties of the alkali and alkaline earth compounds
