《Inorganic Chemistry》课程教学大纲

一、课程基本信息

二、课程目标

（一）总体目标：

This course is a full-semester general course for pharmacy students. The content covers general principles in chemistry, including basic concepts in matters, measurements, stoichiometry, chemical reactions, gases, atomic structure, electron configuration and the periodic table, chemical bonds, chemical compounds, intermolecular forces, chemical kinetics, chemical equilibriums, acids and bases, chemical thermodynamics, and chemical spontaneity. The course aims to promote the scientific ability of students and offers a good basis for studying the pharmacy courses. Students should become familiar with the basic chemistry concepts needed to understand important life processes and pharmacy.

（二）课程目标：

课程目标1：

 1.1 To understand the basic concepts in matters, measurements, stoichiometry, and chemical reactions.

 1.2 To understand the concepts in gases, atomic structure, electron configuration and the periodic table, chemical bonds, chemical compounds, and intermolecular forces.

 1.3 To understand the concepts in chemical kinetics, chemical equilibriums, acids and bases, chemical thermodynamics, and chemical spontaneity.

课程目标2：

2.1 To learn course materials in English.

2.2 To improve the skill in listening, speaking, reading, and writing English.

2.3 To grasp basic English terms in chemistry.

（要求参照《普通高等学校本科专业类教学质量国家标准》，对应各类专业认证标准，注意对毕业要求支撑程度强弱的描述，与“课程目标对毕业要求的支撑关系表一致）（五号宋体）

（三）课程目标与毕业要求、课程内容的对应关系（小四号黑体）

表1：课程目标与课程内容、毕业要求的对应关系表 （五号宋体）

（大类基础课程、专业教学课程及开放选修课程按照本科教学手册中各专业拟定的毕业要求填写“对应毕业要求”栏。通识教育课程含通识选修课程、新生研讨课程及公共基础课程，面向专业为工科、师范、医学等有专业认证标准的专业，按照专业认证通用标准填写“对应毕业要求”栏；面向其他尚未有专业认证标准的专业，按照本科教学手册中各专业拟定的毕业要求填写“对应毕业要求”栏。）

三、教学内容

Chapter 1.  Matter: Its Properties and Measurement

1. 教学目标

• Learn how to use the scientific methods to study a subject

• Be able to classify matters

• Understand the general properties of different matters

• Know how to make measurements properly

2. 教学重难点

教学重点:

• Definition, properties and classification of matters

• Measurement of matters

教学难点:

• Classification of matters

• Unit conversion

• Uncertainties in scientific measurements

• Significant figures in calculations

3. 教学内容

1. The Scientific Method

 How to study chemistry

 The definition of hypothesis, law and theory

2. Properties of Matter

 Physical properties and physical changes

 Chemical properties and chemical changes

 Extensive and intensive properties

3. Classification of Matter

 Identification of matter

 Matter at the atomic level

4. Measurement of Matter: SI (Metric) Units

 Measurements are quantitative observations

 SI base units and their definition

 Derived SI units

 Rules of using SI units

 Converting units

5. Density and Percent Composition: Their Use in Problem Solving

 Measuring and calculating density

 Calculating percent composition

6. Uncertainties in Scientific Measurements

 Definition of uncertainty

 Precision and accuracy

1-7 Significant Figures

   Definition of significant figures

   Significant figures in calculations

4. 教学方法

多媒体教学：

• Illustration of scientific methods

• Illustration of classification of matters

• Illustration of matter at microscopic level

• Illustration of different types of measurements

• Illustration of significant figure in calculations

互动教学：

• What kind of matter is … (air, oxygen, tap water, distilled water, soda, woods)?

• Why need to standardize units?

• How to achieve precision and accuracy?

• How to determine uncertainty in measurement?

• How to maintain the precision of measurement during calculation?

5. 教学评价

课后问题：

• Textbook, Chapter 1: 7, 10, 12, 23, 31, 32, 54, 61, 69, 89

Chapter 2.  Atoms and the Atomic Theory

1. 教学目标

• Understand the structure of atoms

• Understand the general properties of atoms

• Get a genera idea about the periodic table

• Understand the meaning of molar mass

2. 教学重难点

教学重点:

• The historical path leading to identification of atomic structure

• Mass number, atomic number, neutron number, and atomic mass of an atom

• Trends in periods and groups

• Definition of mole and Avogadro’s number

教学难点:

• Experiments leading to discovery of electrons and nucleus

• Converting between mass, number of moles, and number of atoms

3. 教学内容

2-1 Early Chemical Discoveries and the Atomic Theory

   Law of conservation of matter

   Law of constant composition

   John Dalton’s atomic theory

   Law of multiple proportions

2-2 Electrons and Other Discoveries in Atomic Physics

   Thomson’s cathode-ray experiment and Thomson’s model of the atom

   Millikan’s oil drop experiment and determination of the charge and mass of the electron

2-3 The Nuclear Atom

   Rutherford’s gold foil experiment and Rutherford’s model of the atom

   Discovery of protons

   Discovery of neutrons

   Atomic structure

   Mass number, atomic number (proton number), and neutron number

2-4 Chemical Elements

   Chemical symbols

   Isotopes and the percent natural abundances

   Mass spectrometer   

2-5 Atomic Mass

   Definition of atomic mass

   Atomic mass units

   Average atomic masses

2-6 Introduction to the Periodic Table

   Types of elements

   Trends in periods and groups

   Introduction of main group elements

2-7 The Concept of the Mole and the Avogadro Constant

   Definition of mole and Avogadro’s number

   Definition of molar mass

2-8 Using the Mole Concept in Calculations

   Converting between mass, number of moles, and number of atoms

4. 教学方法

多媒体教学：

• Illustration of law of conservation of matter and law of multiple proportions

• Illustration of key experiments leading to discoveries in atomic physics

• Illustration of isotopes and mass spectra

• Illustration of periodic table

互动教学：

• How can cathod-ray experiment prove the existence of electrons

• What is the identity of each of the radiation rays?

• How can the gold-foil experiment tell us the structure of an atom?

• There are 118 elements listed in the periodic table. Are there only 118 unique atoms in the world?

• Why is the relative atomic mass number never a whole number?

5. 教学评价

课后问题：

• Textbook, Chapter 2: 5, 12, 23, 25, 42, 44, 50, 59, 71

Chapter 3.  Chemical Compounds

1. 教学目标 （五号宋体）

• Understand the properties of different chemical compounds and their formulas

• Know how to name common inorganic compounds

2. 教学重难点

教学重点:

• Properties of different chemical compounds and their formulas

• The mole concept and chemical compounds

• Naming inorganic compounds

教学难点:

• Distinguish between molecular and ionic compounds

• Naming different types of inorganic compounds

3. 教学内容

3-1 Types of Chemical Compounds and Their Formulas

   Molecular compounds

 Molecular formula and empirical formula

   Structure of molecules

   Ions and ionic compound

3-2 The Mole Concept and Chemical Compounds

   Relating molar mass, the Avogadro constant, and formula units of a compound

   Combining several factors in a calculation involving molar mass

3-3 Composition of Chemical Compounds

   Percent composition from formulas

   Combustion analysis of C and H in compounds

   Empirical formulas from percent composition

3-5 Naming Compounds: Organic and Inorganic Compounds

   Definition of inorganic and organic compounds

3-6 Names and Formulas of Inorganic Compounds

   Naming molecular compounds

    Naming ionic compounds (binary ionic compounds: type I and type II; compounds containing polyatomic ions)

   Naming acids (Binary acids; oxyacids)

   Naming hydrates

3-7 Names and Formulas of Organic Compounds

Root names for the parent hydrocarbon chains

Root names for organic compounds of different classes

4. 教学方法

多媒体教学：

• Illustration of molecular compounds and ionic compounds

• Illustration of predicting ions forming

• Illustration of rules for naming different types of inorganic compounds

互动教学：

• Do ionic compounds have molecular formulas?

• Can you see the patterns of names of polyatomic ions?

• How to name N₂O₅, LiCl, CuSO₄,HCl, and HNO₃?

5. 教学评价

课后问题：

• Textbook, Chapter 3: 11, 12, 16, 19, 37, 43, 57, 58, 61, 62

Chapter 4.  Chemical Reactions

1. 教学目标 （五号宋体）

• Know how to balance an equation

• Know different ways to present solution concentration

• Understand the molar relationship in chemical reactions

• Be able to solve stoichiometry related questions

2. 教学重难点

教学重点:

• Molar relationship in chemical reactions

• Solve different types of stoichiometry questions

教学难点:

• Additional conversion factors (volume, density, and percent composition) in reaction stoichiometry

• Solve limiting-reactant problems

• Theoretical, actual, and percent yield

3. 教学内容

4-1 Chemical Reactions and Chemical Equations

   Definition of chemical reactions

   How to write chemical equations

4-2 Chemical Equations and Stoichiometry

   Molar relationship in chemical reactions

   Mass relationship in chemical reactions

   Additional conversion factors: volume, density, and percent composition

4-3 Chemical Reactions in Solution

   Solvent and solute

   Saturated solution and solubility

   Concentration of a solution (expressed as percent and molarity)

4-4 Determining the Limiting Reactant

   Identify the limiting reactant

   Solve limiting-reactant problems

4-5 Other Practical Matters in Reaction Stoichiometry

   Theoretical, actual, and percent yield

   Main reaction and side reactions

   Consecutive reactions, overall reaction, and simultaneous reactions

4. 教学方法

多媒体教学：

• Illustration of molar relationship in chemical reactions

• Illustration of step-by-step solution for different types of stoichiometry questions

互动教学：

• How to balance the shown chemical reactions?

• How to solve the example questions?

5. 教学评价

课后问题：

• Textbook, Chapter 4: 5, 9, 17, 26, 33, 41, 49, 65, 73, 84

Chapter 5. Reactions in Aqueous Solutions

1. 教学目标 （五号宋体）

• Understand the properties of different electrolytes

• Be able to predict reactions between electrolyte solutions

• Be able to balance redox reactions by half-reaction method in acidic solution

2. 教学重难点

教学重点:

• Types of electrolytes (acid, base, salt) and their properties

• General principles of oxidation-reduction reactions

教学难点:

• Prediction of reactions between electrolyte solutions

• Oxidation numbers and chemical properties

• Balance redox reactions by half-reaction method in acidic or basic solution

3. 教学内容

5-1 The Nature of Aqueous Solutions

   Types of electrolytes (acid, base, salt)

   Strong and weak electrolytes

5-2 Precipitation Reactions

   Water solubility of common compounds

5-3 Acid Base Reactions

   Neutralization reactions

   Ionic equations

5-4 Oxidation Reduction Reactions: Some General Principles

   Definition of oxidation state/oxidation number

   Rules for assigning oxidation numbers

   Oxidation numbers and chemical properties

   Properties of an oxidation-reduction reaction

5-5 Balancing Oxidation Reduction Equations

   Balance redox reactions by inspection

   Balance redox reactions by half-reaction method in acidic or basic solution

5-6 Oxidizing and Reducing Agents

   Properties of oxidants and reductants

   Identify oxidants and reductants

5-7 Stoichiometry of Reactions in Aqueous Solutions: Titrations

   How to do a titration experiment for neutralization

   Calculations in titrations reactions

4. 教学方法

多媒体教学：

• Illustration of reactions between ions in solution

• Illustration of oxidation numbers and the periodic table

• Illustration of general properties of oxidation-reduction reactions

互动教学：

• How to determine if a given electrolyte is strong or weak?

• How to predict if an aqueous reaction with given reactants can happen or not?

• How to balance an ionic equation that is too complicated to balance by inspection?

5. 教学评价

课后问题：

• Textbook, Chapter 5: 5, 14, 21, 23, 58, 67, 73

Chapter 6.  Gases

1. 教学目标

• Understand the general properties of the ideal gas

• Understand the ideal gas laws

• Be able to solve questions related to ideal gases

• Understand the difference between ideal gas and the real gas

2. 教学重难点

教学重点:

• Ideal gas laws

• Applications of the ideal gas equation

教学难点:

• Stoichiometry problems involving gases

• Effusion rates of gases and Graham’s law of effusion

3. 教学内容

6-1 Properties of Gases: Gas Pressure

   Definitions of gas pressure

   Measurement of gas pressure

   Units of gas pressure

6-2 The Simple Gas Laws

   Boyle’s Law: relation between pressure and volume of a gas

   Charles’s Law: relation between volume and temperature of a gas

   Gay-Lussac’s Law: relation between pressure and temperature of a gas

   Avogadro’s Law: relation between volume and the number of gas molecules

6-3 Combining the Gas Laws: The Ideal Gas Equation and the General Gas Equation

   Ideal gas law

   Properties of ideal gas

6-4 Applications of the Ideal Gas Equation

   Using the ideal gas equation to solve problems

   Standard temperature and pressure

6-5 Gases in Chemical Reactions

   Stoichiometry problems involving gases

6-6 Mixtures of Gases

   Dalton’s law of partial pressures

   Collecting gases over water

6-7 Kinetic-Molecular Theory of Gases

   Main points of the kinetic-molecular theory

   Distribution of molecular speeds at various temperature

6-8 Gas Properties Relating to the Kinetic-Molecular Theory

   Effusion rates of gases and Graham’s law of effusion

   Diffusion rates of gases

6-9 Nonideal (Real) Gases

   Properties of real gases

The van der Waals equation

4. 教学方法

多媒体教学：

• Illustration of gas behaviors in a container

• Illustration of deduction of ideal gas laws

• Illustration of step-by-step solution for stoichiometry problems involving gases

互动教学：

• Is atmospheric pressure an extensive or intensive property?

• What is the essential of gas pressure?

• How to solve the example questions?

5. 教学评价

课后问题：

• Textbook, Chapter 6: 1, 15, 19, 29, 35, 45, 53, 55, 72, 81

Chapter 7 Thermochemistry

1. 教学目标

• Understand the key terms related to thermochemistry

• Understand the first law of thermodynamics

• Understand the concept of enthalpy of chemical reactions

• Be able to solve stoichiometry problems involving enthalpy

2. 教学重难点

教学重点:

• Key terms related to thermochemistry

• Measurement of calculation of heat and work of a chemical reaction

• Calculation of enthalpy of a chemical reaction

教学难点:

• Important characteristics of enthalpy

• Application of Hess’s law

3. 教学内容

7-1 Getting Started: Some Terminology

   Systems, surroundings, and universe

   Isolated, closed and open systems

   Energy forms

   Energy units

7-2 Heat

   Heat, thermal energy and temperature

   Quantifying heat

7-3 Heats of Reaction and Calorimetry

   Measure heat of reaction at constant volume: bomb calorimeter

   Measure heat of reaction at constant pressure: coffee-cup calorimeter

7-4 Work

   Pressure-volume work

7-5 The First Law of Thermodynamics

   Law of conservation of energy

7-6 Heats of Reaction: U and H

   Internal energy change of reaction: U

 U is a state function

 Enthalpy is the heat evolved in a chemical reaction at constant pressure

 Thermochemical equation

 Important characteristics of enthalpy

7-7 Indirect Determination of H: Hess s Law

   Calculation of enthalpies of reaction by combination of thermochemical equations

   Rule for combining equations

7-8 Standard Enthalpies of Formation

   Definition of formation reaction

   Definition of enthalpies of formation

   Standard state and standard enthalpies of formation

   Calculation of enthalpies of reaction from enthalpies of formation

7-9 Fuels as Sources of Energy

   Standard enthalpy of combustion

   Calculation of enthalpies of formation from enthalpy of combustion

4. 教学方法

多媒体教学：

• Illustration of the key terms related to thermochemistry

• Illustration of different energy forms and their conversion

• Illustration of the law of conservation of energy

• Illustration of enthalpy calculations

• Illustration of Hess’s law

• Illustration of step-by-step solution for stoichiometry problems involving enthalpy

互动教学：

• What is the relationship between system, surroundings and the universe?

• Internal energy is a state function, is heat or work a state function?

• What are the corollaries of Hess’s law?

5. 教学评价

课后问题：

• Textbook, Chapter 7: 10, 15, 29, 37, 39, 55, 63, 65, 69, 79, 105

Chapter 8.  Electrons in Atoms

1. 教学目标 （五号宋体）

• Understand the properties of electrons

• Understand the quantum mechanics and electron configuration

• Understand different models for atomic structure

• Understand the relationship between electron configurations and the periodic table

2. 教学重难

教学重点:

• Wave properties and particle properties of electrons

• Quantum mechanics and electron configuration

• Electron configurations and the periodic table

教学难点:

• Quantum numbers and electron orbitals

• Electron configurations of multi-electron atoms

3. 教学内容

8-1 Electromagnetic Radiation

   General properties of waves

   Diffraction and interference are wave properties

   The electromagnetic spectrum

   The photoelectric effect

   Wave-particle duality of electromagnetic radiation

8-2 Atomic Spectra

   Generation of atomic spectra

   Emission and absorption spectra

   Explanation of atomic spectra

8-3 Quantum Theory

   The energy of electrons in atoms is quantized

8-4 The Bohr Atom

   The Bohr Model   

8-5 Two Ideas Leading to a New Quantum Mechanics

   Wave-particle duality of electrons

   The Heisenberg uncertainty principle

8-6 Wave Mechanics

   Standing waves

   Schrödinger’s quantum mechanics and wave function

8-7 Quantum Numbers and Electron Orbitals

   The principal quantum number

   The angular momentum quantum number

   The magnetic quantum number

8-8 Interpreting and Representing the Orbitals of the Hydrogen Atom

   Orbital s, p, d

   Shapes and properties

8-9 Electron Spin: A Fourth Quantum Number

   Electron spin

   Pauli exclusion principle

8-10 Multielectron Atoms

   Orbital energies in a single-electron atom

   Effective nuclear charges: shielding and penetration

   Orbital energies in a multi-electron atom

8-11 Electron Configurations

   Aufbau principle

   Hund’s rule

   Electron configurations of multi-electron atoms

   Electron configuration anomalies

8-12 Electron Configurations and the Periodic Table

   Periodic table showing orbitals being filled

   The construction of the periodic table

4. 教学方法

多媒体教学：

• Illustration of wave properties and particle properties of electrons

• Illustration of atomic spectra

• Illustration of quantum numbers and electron orbitals

• Illustration of orbital energies in single-electron and multi-electron atoms

• Illustration of electron configuration

互动教学：

• What’s the possible explanation for the photoelectric effect?

• How to interpret the wave-particle duality of electromagnetic radiation?

5. 教学评价

课后问题：

• Textbook, Chapter 8: 5, 11, 21, 25, 39, 57, 59, 61, 79, 81, 83

Chapter 9.  The Periodic Table and Some Atomic Properties

1. 教学目标 （五号宋体）

• Understand the way of element arrangement in the periodic table

• Understand the trend of atomic size, ionization energy, and electron affinity of elements in the periodic table

• Be able to predict the properties of a given element based on its position in the periodic table

2. 教学重难点

教学重点:

• The definition of atomic size, ionization energy, and electron affinity of elements

• The trend of atomic size, ionization energy, and electron affinity of elements in the periodic table

• Periodic properties of the elements

教学难点:

• Periodic trends in atomic radii and ionic radii

• First ionization energy and successive ionization energies

• Irregularities of atomic size, ionization energy, and electron affinity

3. 教学内容

9-1 Classifying the Elements: The Periodic Law and the Periodic Table

   The periodic law

   Atomic number as the basis for the periodic law

9-2 Metals and Nonmetals and Their Ions

   Main group metal ions

   Main group nonmetal ions

   Transition metal ions

9-3 Sizes of Atoms and Ions

   Atomic radius

   Periodic trends in atomic radii

   Ionic radius

   Periodic trends in ionic radii

9-4 Ionization Energy

   Definition of first ionization energy

   First ionization energy irregularities

   First ionization energy of transition metals

   Definition of successive ionization energies

9-5 Electron Affinity

   Definition of electron affinity

   Electron affinity irregularities

   Electron affinity of ions

9-6 Magnetic Properties

   Diamagnetic atom

   Paramagnetic atom

9-7 Periodic Properties of the Elements

   Variation of physical properties within a group

   Variation of physical properties across a period

4. 教学方法

多媒体教学：

• Illustration of arrangement of periodic table

• Illustration of trend of atomic size, ionization energy, and electron affinity of elements in the periodic table

• Illustration of diagonal relationship in the periodic table

互动教学：

• How can the arrangement of periodic table be related to electron configuration of atoms?

• How to explain the irregularities of atomic size, ionization energy, and electron affinity?

5. 教学评价

课后问题：

• Textbook, Chapter 9: 9, 17, 21, 31, 42

Chapter 10.  Chemical Bonding I: Basic Concepts

1. 教学目标 （五号宋体）

• Understand Lewis theory

• Understand the properties of covalent bond

• Know how to write Lewis structures for covalent compounds

• Understand the polarity of covalent bond

• Know how to use valence shell electron pair repulsion (VSEPR) theory to predict the shape of molecules

2. 教学重难点

教学重点:

• Lewis theory and Lewis electron dot symbols

• Properties of covalent bond

• Lewis structures for covalent compounds

• Bond polarity and dipole moment

• Valence shell electron pair repulsion (VSEPR) theory

教学难点:

• Resonance structures

• Exceptions to the octet rule

3. 教学内容

10-1 Lewis Theory: An Overview

   Lewis theory

   Lewis electron dot symbols and Lewis structure

   Lewis structures for ionic compounds

10-2 Covalent Bonding: An Introduction

   Covalent bonds

   Lewis structures for covalent compounds

10-3 Polar Covalent Bonds and Electrostatic Potential Maps

   Electronegativity

   Nonpolar and polar covalent bonds

   Bond polarity

   Dipole moment

10-4 Writing Lewis Structures

   Steps of writing Lewis structure

   Definition, calculation and application of formal charges

10-5 Resonance

   Resonance structures

   Steps in writing resonance structures

   Resonance structures and chemical properties

10-6 Exceptions to the Octet Rule

   Species with more than eight electrons around the atom

 Species with fewer than eight electrons around the atom

 Species with an odd total number of electrons

10-7 Shapes of Molecules

   Valence shell electron pair repulsion (VSEPR) theory

   The electron geometry

   The molecular geometry

   Molecular shapes and dipole moments

10-8 Bond Order and Bond Lengths

   Bond order

   Bond length

   Bond number and valence electrons

10-9 Bond Energies

   Bond-dissociation energy

   Average bond energies

4. 教学方法

多媒体教学：

• Illustration of bond formation

• Illustration of comparison between covalent bond and ionic bond

• Illustration of electronegativity trend in periodic table

• Illustration of step-to-step writing of Lewis structure

• Illustration of valence shell electron pair repulsion (VSEPR) theory

互动教学：

• What are the Lewis structures of these compounds?

• What are the shapes of these compounds?

• What are the dipole moments of these compounds?

5. 教学评价

课后问题：

• Textbook, Chapter 10: 3, 6, 11, 13, 17, 25, 27, 37, 44, 49, 51, 59, 60

Chapter 12. Intermolecular Forces: Liquids and Solids

1. 教学目标

• Understand the properties of different intermolecular forces

• Understand the properties of liquids and solids

2. 教学重难点

教学重点:

• Intermolecular forces

• Properties of liquids and solids

• Phase diagrams

教学难点:

• Judge the type of intermolecular force in a given substance

• Interpretation of a phase diagram

3. 教学内容

12-1 Intermolecular Forces

dispersion force (London force)

dipole-dipole force

hydrogen bonding

ion–dipole force

12-2 Some Properties of Liquids

Surface tension

Viscosity

Vaporization and vapor pressure

Boiling and the Boiling Point

The critical point

12-3 Some Properties of Solids

Melting, Melting Point, and Heat of Fusion

Sublimation

12-4 Phase Diagrams

The major features of a phase diagram

Phase diagram for water

Phase diagram for iodine

Phase diagram for carbon dioxide

12-5 Network Covalent Solids and Ionic Solids

Molecular solids

Ionic solids

Atomic solids

4. 教学方法

多媒体教学：

• Illustration of different intermolecular forces

• Illustration of properties of liquids and solids

• Illustration of phase diagram of different substances

互动教学：

• What are the types of intermolecular interactions in these substances?

• What is special about water based on its phase diagram?

5. 教学评价

课后问题：

• Textbook, Chapter 12: 3, 4, 15, 23, 33, 51, 60

Chapter 13.  Solutions and their physical properties

1. 教学目标 （五号宋体）

• Understand the basic properties of solutions

• Be able to solve the solution-related problems

2. 教学重难点

教学重点:

• Intermolecular forces and the solution process

• Solution formation and equilibrium

• Colligative properties

教学难点:

• Vapor pressure lowering

• Freezing point depression

• Boiling point elevation

• Osmotic pressure

3. 教学内容

13-1 Intermolecular forces and the solution process

 Enthalpy of solution

 Intermolecular forces in mixtures

 Formation of ionic solutions

13-2 Solution formation and equilibrium

 Solubility as a function of temperature

 Fractional crystallization

13-3 Solubilities of gases

 Effect of temperature

 Effect of pressure

13-4 Vapor pressures of solutions

 Liquid vapor equilibrium: ideal solutions

 Fractional distillation

 Liquid vapor equilibrium: nonideal solutions

13-5 Osmotic pressure

    Definition of osmotic pressure

 Practical applications

13-6 Freezing-point depression and boiling-point elevation of nonelectrolyte solutions

 Practical applications

13-7 Colloidal mixtures

 Definition of colloids

4. 教学方法

多媒体教学：

• Illustration of physical properties of solutions

• Illustration of how to solve the solution-related problems

互动教学：

• What is the difference between the ideal solution and non-ideal solution?

• What is the nature of the intermolecular forces in a given solution?

• How to determine the colligative properties of a given solution?

5. 教学评价

课后问题：

• Textbook, Chapter 13: 3, 4, 15, 23, 33, 51, 60

Chapter 14.  Chemical Kinetics

1. 教学目标 （五号宋体）

• Understand the definition of rate of the chemical reaction

• Understand the rate law and the expression

• Understand the reaction mechanisms

2. 教学重难点

教学重点:

• The expression of the rate law and rate constant

• Determine the reaction rate

• Reaction mechanisms

教学难点:

• Method of initial rates

• The integrated rate laws

• Mechanisms with a fast initial step

3. 教学内容

14-1 The Rate of a Chemical Reaction

   The average rate of the reaction

   The instantaneous rate of the reaction

   Expression of the rate of a chemical reaction

14-2 Measuring Reaction Rates

   Initial rate of reaction

 Method of initial rates

14-3 Effect of Concentration on Reaction Rates: The Rate Law

   The expression of the rate law

   Rate constant

   Reaction order

14-4 Zero-Order Reactions

   Rate = k[A]⁰=k = constant

   Zero-order integrated rate law: [A]_t= - kt + [A]₀

   Zero-order reaction half-life

14-5 First-Order Reactions

   Rate = k[A]¹

 First-order integrated rate law

 First-order half-life

14-6 Second-Order Reactions

   Rate = k[A]²

 Second-order integrated rate law

 Second-order reaction half-life

14-7 Reaction Kinetics: A Summary

14-8 Theoretical Models for Chemical Kinetics

   Collision theory

   Transition state theory

14-9 The Effect of Temperature on Reaction Rates

   Activation energy

   Arrhenius equation

14-10 Reaction Mechanisms

   Elementary step

   Rate laws for elementary steps

   Rate-determining step

   Overall reaction rate laws

   Mechanisms with a fast initial step

14-11 Catalysis

   The effect of catalyst on reaction rates

4. 教学方法

多媒体教学：

• Illustration of different types of rates of a chemical reaction

• Illustration of how to determine the rate law based on initial rates

• Illustration of integrated rate laws of different orders of reactions

• Illustration of how to determine the reaction mechanism

互动教学：

• How to evaluate the effect of concentration on reaction rates?

• How to determine the rate law of a given reaction?

• How to determine the reaction mechanism of a given reaction?

5. 教学评价

课后问题：

• Textbook, Chapter 14: 1, 9, 11, 15, 17, 21, 39, 43, 49, 51, 59, 67

Chapter 15.  Principles of Chemical Equilibrium

1. 教学目标 （五号宋体）

• Understand the significance of chemical equilibrium

• Be able to solve chemical equilibrium problems

• Understand how chemical equilibrium can be altered

2. 教学重难点

教学重点:

• The definition and expression of equilibrium constant

• Definition and expression of reaction quotient

• Le Châtelier s Principle

教学难点:

• Combining equilibrium constants

• Relationship between K_c and K_p

• Position of equilibrium and rate of reacting equilibrium

3. 教学内容

15-1 Dynamic Equilibrium

   All chemical reactions are reversible

   Chemical equilibria

15-2 The Equilibrium Constant Expression

   Homogeneous equilibria

   Heterogeneous equilibria

 Concentration equilibrium constant and its expressions

 Partial pressure equilibrium constants

 Units of the equilibrium constants

15-3 Relationships Involving Equilibrium Constants

   The relationship between balanced equation and the value of the equilibrium constant

   Combining equilibrium constants

   Relationship between K_c and K_p

15-4 The Magnitude of an Equilibrium Constant

   Position of equilibrium and rate of reacting equilibrium

15-5 The Reaction Quotient, Q: Predicting the Direction of Net Change

   Definition and expression of reaction quotient

 How to predict the direction of reaction

15-6 Altering Equilibrium Conditions: Le Châtelier s Principle

   Effect of changes in concentration

   Effect of changes in pressure

   Effect of changes in temperature

   Effect of a catalyst

15-7 Equilibrium Calculations: Some Illustrative Examples

 Determine the values of concentration equilibrium constants when the concentration of all reactants and products at equilibrium are known

 Determine the equilibrium concentrations from the initial concentrations

 Calculating equilibrium concentration from equilibrium constant

4. 教学方法

多媒体教学：

• Illustration of chemical equilibrium

• Illustration of step-by-step solution to equilibrium problems

• Illustration of how to predict the direction of reaction

• Illustration of how to manipulate the outcomes of reversible reactions

互动教学：

• How to distinguish the homogeneous and heterogeneous equilibrium?

• How to write equilibrium expressions of given reactions?

• How to solve these equilibrium problems?

• How to predict the effects of certain alteration to a given equilibtrium?

5. 教学评价

课后问题：

• Textbook, Chapter 15: 8, 13, 19, 20, 38, 44, 51, 66, 81, 82

Chapter 16.  Acids and Bases

1. 教学目标 （五号宋体）

• Understand the definition and properties of acid and base

• Understand how calculate the pH of a given acid or base solution

• Understand the acid-base properties of salts

2. 教学重难点

教学重点:

• Brønsted-Lowry theory of acids and bases

• Calculating the pH for strong/weak acids and strong/weak bases

• Definition of Lewis acids and bases

教学难点:

• Calculating the pH for weak acids and weak bases

• Ionization of polyprotic acids

• Strengths of acids and bases

3. 教学内容

16-1 Arrhenius Theory: A Brief Review

   Arrhenius definition of acids and bases

16-2 Brønsted Lowry Theory of Acids and Bases

   Brønsted-Lowry definition of acids and bases

   Brønsted-Lowry definition of acid-base reactions

   Properties of Brønsted-Lowry acids and bases

   Conjugate acid-base pairs

16-3 Self-Ionization of Water and the pH Scale

   Brønsted-Lowry acid and base in water

   Brønsted-Lowry definition of water

   The ion product for water, K_w

   Definitions of neutral, acidic and basic solutions

   The pH scales

16-4 Strong Acids and Strong Bases

   Calculating the pH for strong acids and strong bases

16-5 Weak Acids and Weak Bases

   Acid ionization/dissociation constant

   Percent ionization of a weak acid

   Base ionization constant

   Calculating the pH for weak acids and weak bases

16-6 Polyprotic Acids

   Ionization of polyprotic acids

   Calculating ion concentrations in sulfuric acid solutions

16-7 Ions as Acids and Bases

   Anions as weak bases

   Cations as weak acids

   Hydrolysis of salt

   The acid-base properties of salts

16-8 Molecular Structure and Acid Base Behavior

   Strengths of binary acids

   Strengths of oxyacids

   Strengths of amines as bases

16-9 Lewis Acids and Bases

   Definition of Lewis acids and bases

   Properties of Lewis acids and bases

4. 教学方法

多媒体教学：

• Illustration of acid-base reactions

• Illustration of pH and pOH scales

• Illustration of step-to-step calculation of the pH for strong/weak acids and strong/weak bases

• Illustration of strengths of acids and bases

互动教学：

• How to determine the pH for strong/weak acids and strong/weak bases?

• How to determine the strengths of acids and bases?

5. 教学评价

课后问题：

• Textbook, Chapter 16: 3, 5, 23, 25, 39, 47, 53, 55, 65, 71

Chapter 17. Additional Aspects of Acid Base Equilibria

1. 教学目标 （五号宋体）

• Understand the properties of buffer solutions

• Know how to make a buffer solution

• Know how to calculate the pH or pH change of a buffer solution

• Understand the titration curve

2. 教学重难点

教学重点:

• Calculating the pH of a buffer solution

• Preparing buffer solutions

• Calculating pH changes in buffer solutions

• Properties of buffer solutions

教学难点:

• Calculating pH changes in buffer solutions

• Buffer effectiveness, range and capacity

3. 教学内容

17-1 Common-Ion Effect in Acid Base Equilibria

Solutions of weak acids and strong acids

Solutions of weak acids and their Salts

17-2 Buffer Solutions

Calculating the pH of a buffer solution

The Henderson-Hasselbalch equation

Preparing buffer solutions

Calculating pH changes in buffer solutions

Buffer effectiveness

Buffer range

Buffer capacity

17-3 Acid Base Indicators

17-4 Neutralization Reactions and Titration Curves

Titration curve of acid and base

Titration curve of buffers

4. 教学方法

多媒体教学：

• Illustration of how buffer solution works

• Illustration of how to calculate pH of a buffer solution

• Illustration of how to prepare buffer solution

• Illustration of how to calculate pH change of a buffer solution

• Illustration of the titration curve

互动教学：

• Why a buffer solution has much more tolerance to acid or base?

• How to calculate pH of a buffer solution?

• At what circumstances can you use the Henderson-Hasselbalch equation?

• How to determine the buffer range and capapcity?

5. 教学评价

课后问题：

• Textbook, Chapter 17: 7, 11, 15, 24

Chapter 19.  Spontaneous Change: Entropy and Gibbs Energy

1. 教学目标

• Understand the meaning of spontaneous change

• Understand the meaning of entropy and its application

• Understand the second and third law of thermodynamics

• Understand the meaning of Gibbs free energy and its application

2. 教学重难点

教学重点:

• Definition of spontaneous process and nonspontaneous process

• Calculation of standard entropy changes

• Calculation of Gibbs free energy change

• Gibbs free energy change and equilibrium

教学难点:

• The statistical view of entropy

• The difference between G and ΔG

• The temperature dependence of the equilibrium constant

3. 教学内容

19-1 Spontaneity: The Meaning of Spontaneous Change

   Definition of spontaneous process and nonspontaneous process

   Spontaneous process can be endothermic

19-2 The Concept of Entropy

   Definition of entropy

   The Boltzmann equation for entropy

   The statistical view of entropy

   The kinetic-molecular view of entropy   

 The second law of thermodynamics

19-3 Evaluating Entropy and Entropy Changes

   The third law of thermodynamics

   Standard molar entropy

   Calculation of standard entropy changes

19-4 Criteria for Spontaneous Change: The Second Law of Thermodynamics

   The second law of thermodynamics

   Gibbs free energy, G = H – TS

   Temperature and direction of spontaneous change

19-5 Standard Gibbs Energy Change, G°

   Standard free-energy change (ΔG)

   Calculation of ΔG from ΔH and ΔS

   Standard free energy of formation (ΔG_f)

   Calculation of GfromG_f

19-6 Gibbs Energy Change and Equilibrium

   Gibbs energy change and equilibrium constant

 19-7 G° and K as Functions of Temperature

   The temperature dependence of the equilibrium constant

   The van’t Hoff equation

19-8 Coupled Reactions

4. 教学方法

多媒体教学：

• Illustration of spontaneous process and nonspontaneous process

• Illustration of the concept of entropy

• Illustration of how to calculate standard entropy changes

• Illustration of how to calculate Gibbs free energy change

互动教学：

• How to predict if a reaction will happen spontaneously at the given conditions?

• Why can spilled water evaporate spontaneously even though ΔG for the vaporization of water is positive?

5. 教学评价

课后问题：

• Textbook, Chapter 19: 2, 5, 7, 15, 23, 31, 33, 43, 57, 63

Chapter 20.  Electrochemistry

1. 教学目标

• Understand the basic concept of electrochemistry

• Understand the mechanisms of batteries

• Understand the application of electrochemistry in industry

2. 教学重难点

教学重点:

• Electrode Potentials and Their Measurement

• E_cell, G, and K

• E_cell as a Function of Concentrations

• Different types of batteries

教学难点:

• Nernst equation

• Battery mechanism

3. 教学内容

20-1 Electrode Potentials and Their Measurement

    Definition of electrode potential

    Cell diagrams and terminology

20-2 Standard Electrode Potentials

 The standard hydrogen electrode

 The standard cell potential

20-3 E_cell, G, and K

    Combining Reduction Half-Equations

    Spontaneous Change in Oxidation Reduction Reactions

    The Relationship Between E_cell and K

20-4 E_cell as a Function of Concentrations

 Concentration Cells

 Alternative Standard Electrodes

20-5 Batteries: Producing Electricity Through Chemical Reactions

    Different types of batteries

20-6 Corrosion: Unwanted Voltaic Cells

20-7 Electrolysis: Causing Nonspontaneous Reactions to Occur

 Predicting Electrolysis Reactions

 Quantitative Aspects of Electrolysis

20-8 Industrial Electrolysis Processes

 Electrorefining

 Electroplating

 Electrosynthesis

4. 教学方法

多媒体教学：

• Illustration of electrochemical cells

• Illustration of different types of batteries

• Illustration of how to solve electrochemistry-related problems

互动教学：

• How to predict the electron flow in an electrochemical cell?

• How to solve electrochemistry-related problems?

5. 教学评价

课后问题：

Textbook, Chapter 20: 2, 6, 7, 15, 20, 31, 33, 40, 58, 62

四、学时分配

表2：各章节的具体内容和学时分配表

五、教学进度

表3：教学进度表

六、教材及参考书目

（电子学术资源、纸质学术资源等，按规范方式列举）

1. Nivaldo J. Tro, Chemistry: A Molecular Approach, Prentice Hall, Pearson Education Inc., 2010

2. Jean B. Umland and Jon M. Bellama, General Chemistry, Thomson Learning, 2001

3. Bruce Averill, General Chemistry: Principles, Patterns, and Applications, Saylor Academy, 2012

4. Linus Pauling, General Chemistry, BN Publishing, 2011

5. Satyajit D. Sarker and Lutfun Nahar, Chemistry for Pharmacy Students, John Wiley & Sons, 2007

七、教学方法

（讲授法、讨论法、案例教学法等，按规范方式列举，并进行简要说明）（五号宋体）

 1．多媒体教学法：在授课同时，利用多媒体展示图片或录像，让学生对复杂的生物现象或科学技术有更直观的认识，帮助学生刚好地理解及掌握复杂概念。

 2. 互动教学：学生回答老师提出的问题或参与课堂讨论，提高学生课堂参与度，开阔思维，并锻炼表达能力。

八、考核方式及评定方法

（一）课程考核与课程目标的对应关系

表4：课程考核与课程目标的对应关系表

（二）评定方法

1．评定方法

（例：平时成绩：10%，期中考试：30%，期末考试60%，按课程考核实际情况描述）

2．课程目标的考核占比与达成度分析

表5：课程目标的考核占比与达成度分析表

（三）评分标准