《普通化学(一）》课程教学大纲

《普通化学(一）》课程教学大纲（三号黑体）

一、课程基本信息

二、课程目标

（一）总体目标：

 General chemistry （1） is a basic course for non-chemical chemistry students, so that students understand the basic theory and framework of the 21st century chemistry, and can apply the chemical theory, viewpoint and method to deal with environmental pollution, material preparation and other scientific fields related to chemical problems.

（二）课程目标：

课程目标1：

1. Teaching students the viewpoints of chemistry, thinking methods and research methods of chemistry.

2. Stimulate students' innovative consciousness.

3. Cultivate students' ability to examine and solve problems from a chemical point of view in future engineering practice.

课程目标2：

2.1   Master the basic concepts, principles and skills of chemistry at the university level

（三）课程目标与毕业要求、课程内容的对应关系

表1：课程目标与课程内容、毕业要求的对应关系表

（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

第一章：MATTER, ENERGY, AND MEASUREMENT

1.教学目标:

This first chapter provides an overview of what chemistry is about and what chemists do.

2.教学重难点：

3.教学内容:

1.1.The Study of Chemistry:

Learn what chemistry is, what chemists do, and why it is useful to study chemistry.

1.2.Classifications of Matter:

 Examine fundamental ways to classify matter; distinguish between pure substances and mixtures and between elements and compounds.

1.3. Properties of Matter:

 Use properties to characterize, identify, and separate substances; distinguish between chemical and physical properties.

1.4.The Nature of Energy:

Explore the nature of energy and the forms it takes, notably kinetic energy and potential energy.

1.5.Units of Measurement:

Learn how numbers and units of the metric system are used in science to describe properties.

1.6.Uncertainty in Measurement:

Use significant figures to express the inherent uncertainty in measured quantities and in calculations.

1.7.Dimensional Analysis:

 Learn to carry numbers and units through calculations; use units to check if a calculation is correct.

4.教学方法:

Lecture method; case teaching method; practice method; independent learning method; discussion method

5.教学评价:

Classwork, matched problems, homework and discussions.

第二章：ATOMS, MOLECULES, AND IONS

1.教学目标:

In this chapter, we introduce the basic structure of atoms and discuss the formation of molecules and ions. This knowledge provides you with the foundation you need to understand the chapters that follow.

2.1   The Atomic Theory of Matter:

 Learn how scientists were able to postulate that atoms are the smallest building block of matter, long before they could be seen directly.

2.2   The Discovery of Atomic Structure:

 Examine key experiments that led to the discovery of electrons and to the nuclear model of the atom.

2.3   The Modern View of Atomic Structure:

 Learn how atomic number and mass number can be used to express the number of each subatomic particle— protons, neutrons, and electrons—in a given atom.

2.4   Atomic Weights:

 Learn about the concept of atomic weights and how they are derived from the masses and abundances of individual atoms.

2.5   The Periodic Table:

Examine the organization of the periodic table, in which elements are put in order of increasing atomic number and grouped by chemical similarity.

2.6   Molecules and Molecular Compounds:

 Explore the assemblies of atoms called molecules and learn how their compositions are represented by empirical and molecular formulas.

2.7   Ions and Ionic Compounds:

Realize that atoms can gain or lose electrons to form ions and learn how to use the periodic table to predict the charges on ions as well as the empirical formulas of ionic compounds.

2.8   Naming Inorganic Compounds:

Consider the systematic way in which substances are named, called nomenclature, and how this nomenclature is applied to inorganic compounds.

2.9   Some Simple Organic Compounds:

 Become familiar with simple families of organic compounds, compounds containing carbon and hydrogen, and the very basic nomenclature of these compounds.

第三章：CHEMICAL REACTIONS AND REACTION STOICHIOMETRY

1.教学目标:

In this chapter we begin exploring chemical reactions. Our focus will be on the use of chemical formulas to represent reactions and on the quantitative information we can obtain about the amounts of substances involved in those reactions.

3.1   Chemical Equations:

 Use chemical formulas to write equations representing chemical reactions.

3.2   Simple Patterns of Chemical Reactivity:

 Examine some simple chemical reactions: combination reactions, decomposition reactions, and combustion reactions.

3.3   Formula Weights:

 Learn to obtain quantitative information from chemical formulas by using formula weights.

3.4   Avogadro’s Number and the Mole:

Use chemical formulas to relate the masses of substances to the numbers of atoms, molecules, or ions contained in the substances, a relationship that leads to the crucially important concept of the mole, defined as 6.022 * 1023 objects (atoms, molecules, ions, and so on).

3.5   Empirical Formulas from Analyses:

Apply the mole concept to determine chemical formulas from the masses of each element in a given quantity of a compound.

3.6   Quantitative Information from Balanced Equations:

 Use the quantitative information inherent in chemical formulas and equations together with the mole concept to predict the amounts of substances consumed or produced in chemical reactions.

3.7   Limiting Reactants:

Recognize that one reactant may be used up before others in a chemical reaction. This is the limiting reactant. Once the limiting reactant is used up, the reaction stops, leaving some excess of the other starting materials.

(Chapters 4 and 5 will be thought at Gchem2)

第六章：ELECTRONIC STRUCTURE OF ATOMS

1.教学目标:

In this chapter, we explore quantum theory and its importance in chemistry. We begin by looking at the nature of light and how our description of light was changed by quantum theory. We will explore some of the tools used in quantum mechanics, the “new” physics that had to be developed to describe atoms correctly. We will then use quantum theory to describe the arrangements of electrons in atoms—what we call the electronic structure of atoms.

6.1   The Wave Nature of Light:

 Learn that light (radiant energy, or electromagnetic radiation) has wave-like properties and is characterized by wavelength, frequency, and speed.

6.2   Quantized Energy and Photons:

Recognize that electromagnetic radiation also has particle-like properties and can be described as “particles” of light called photons.

6.3   Line Spectra and the Bohr Model:

Examine the light emitted by electrically excited atoms (line spectra) and infer from those spectra that only certain energy levels are allowed for electrons in atoms. These observations lead to the Bohr model of the atom, which pictures the electrons moving around the nucleus only in certain allowed orbits.

6.4   The Wave Behavior of Matter:

Recognize that matter also has wave-like properties. As a result, it is impossible to determine simultaneously the exact position and the exact momentum of an electron in an atom (Heisenberg’s uncertainty principle).

6.5   Quantum Mechanics and Atomic Orbitals:

 Describe how the electron exists in the hydrogen atom by treating it as if it were a wave. The wave functions that mathematically describe the electron’s position and energy in an atom are called atomic orbitals. Each orbital is characterized by a set of quantum numbers.

6.6   Representations of Orbitals:

 Consider the three-dimensional shapes of orbitals and how they can be represented by graphs of electron density.

6.7   Many-Electron Atoms:

 Learn that the energy levels of an atom having more than one electron are different from those of the hydrogen atom, and that each electron has an additional quantum-mechanical property called spin. The Pauli exclusion principle states that no two electrons in an atom can have the same four quantum numbers. Therefore, each orbital can hold a maximum of two electrons.

6.8   Electron Configurations:

 Learn how the orbitals of the hydrogen atom can be used to describe the arrangements of electrons in many-electron atoms. Using patterns in orbital energies as well as some fundamental characteristics of electrons described by Hund’s rule, we determine how electrons are distributed among the orbitals (electron configurations).

6.9   Electron Configurations and the Periodic Table:

 Recognize that the electron configuration of an atom is related to the location of the element in the periodic table.

第七章：PERIODIC PROPERTIES OF THE ELEMENTS

1.教学目标:

In this chapter, we explore several fundamental characteristics of elements. We see how these characteristics change as we move across a row or down a column of the periodic table, which in turn helps us rationalize and predict the physical and chemical properties of the elements.

7.1   Development of the Periodic Table:

Learn about the discovery and key moments in the development of the periodic table.

7.2   Effective Nuclear Charge:

Understand the concept of effective nuclear charge, the force between the outer or valence electrons and the nucleus, and how it varies throughout the periodic table.

7.3   Sizes of Atoms and Ions:

Explore the relative sizes of atoms and ions, both of which follow trends that are related to their placement in the periodic table and the trends in effective nuclear charge.

7.4   Ionization Energy:

Learn that ionization energy is the energy required to remove one or more electrons from an atom. The periodic trends in ionization energy depend on variations in effective nuclear charge and atomic radii.

7.5   Electron Affinity:

 Learn that electron affinity is the energy released when an electron is added to an atom and understand its periodic trends.

7.6   Metals, Nonmetals, and Metalloids:

Differentiate the physical and chemical properties of metals from those of nonmetals. The differences in properties arise from the fundamental characteristics of atoms, particularly ionization energy. Metalloids display properties that are intermediate between those of metals and those of nonmetals.

7.7   Trends for Group 1 and Group 2 Metals:

 Examine some periodic trends in the chemical and physical properties of metals belonging to groups 1 and 2.

7.8   Trends for Selected Nonmetals:

Investigate some of the periodic trends in the chemical and physical properties of hydrogen and the elements in groups 16, 17, and 18.

第八章：BASIC CONCEPTS OF CHEMICAL BONDING

1.教学目标:

In this chapter and the next, we examine the relationship between the electronic structure of atoms and the ionic and covalent chemical bonds they form.

8.1   Lewis Symbols and the Octet:

Rule Learn about the three main types of chemical bonds: ionic, covalent, and metallic. In evaluating bonding, Lewis symbols provide a useful shorthand for keeping track of valence electrons. We learn that atoms usually follow the octet rule.

8.2   Ionic Bonding:

 Explore ionic substances, substances in which atoms are held together by the electrostatic attractions between ions of opposite charge. Analyze the energetics of forming ionic substances and describe the lattice energy of these substances.

8.3   Covalent Bonding:

 Examine the bonding in molecular substances, in which atoms bond by sharing one or more electron pairs. In general, the electrons are shared in such a way that each atom attains an octet of electrons.

8.4   Bond Polarity and Electronegativity:

 Learn that electronegativity is the ability of an atom in a compound to attract electrons to itself. In general, electron pairs are shared unequally between atoms with different electronegativities, leading to polar covalent bonds.

8.5   Drawing Lewis Structures:

 Learn that Lewis structures are a simple yet powerful way of predicting covalent bonding patterns in molecules. In addition to the octet rule, see how the concept of formal charge can be used to identify the dominant Lewis structure.

8.6   Resonance Structures:

 Learn that in some cases, more than one equivalent Lewis structure can be drawn for a molecule or polyatomic ion. The bonding description in such cases is a blend of two or more resonance structures.

8.7   Exceptions to the Octet Rule:

Recognize that the octet rule is more of a guideline than an absolute rule. Exceptions to the rule include molecules with an odd number of electrons, molecules where large differences in electronegativity prevent an atom from completing its octet, and molecules where an element from period 3 or below in the periodic table attains more than an octet of electrons.

8.8   Strengths and Lengths of Covalent Bonds:

 Observe that bond strengths and lengths vary with the number of shared electron pairs as well as other factors.

第九章：MOLECULAR GEOMETRY AND BONDING THEORIES

1.教学目标:

In this chapter, we examine the relationship between the electronic structure of atoms and the ionic and covalent chemical bonds they form.

9.1  Molecular Shapes：

Draw three-dimensional structures of molecules.

9.2  The VSEPR Model：

Predict molecular geometries using the valence-shell electron-pair

repulsion, or VSEPR, model, which is based on Lewis structures and the repulsions between regions of high electron density.

9.3  Molecular Shape and Molecular Polarity：

Determine whether a molecule is polar or nonpolar by analyzing its geometry and the types of bonds it contains.9.4  Covalent Bonding and Orbital Overlap： Explore how electrons are shared between atoms in a covalent bond. In valencebond theory, the bonding electrons are visualized as originating in atomic orbitals on two atoms. A covalent bond is formed when these orbitals overlap.

9.5  Hybrid Orbitals：

Examine how the orbitals of one atom mix with one another, or hybridize, to create hybrid orbitals.

9.6  Multiple Bonds：

Learn how atomic orbitals overlap in multiple ways to produce sigma and pi bonds between atoms. Single bonds consist of one sigma bond; multiple bonds involve one sigma and one or more pi bonds. Examine the geometric arrangements of these bonds and how they are exemplified in organic compounds.

9.7  Molecular Orbitals：

Examine a more sophisticated treatment of bonding called molecular orbital theory, which introduces the concepts of bonding and antibonding molecular orbitals.

9.8  Bonding in Period 2 Diatomic Molecules：

Extend the concepts of molecular orbital theory to construct energy-level diagrams for second-row diatomic molecules

四、学时分配（四号黑体）

表2：各章节的具体内容和学时分配表（五号宋体）

五、教学进度（四号黑体）

表3：教学进度表（五号宋体）

六、教材及参考书目

 1．14-Bruce E. Bursten, Catherine Murphy, H. Eugene LeMay, Matthew E. Stoltzfus, Patrick Woodward, Theodore E. Brown - Chemistry. The Central Science in SI Units, global edition   14th ed. (2018, Pearson)    

七、教学方法

 In the teaching process of this course, the teaching method highlights the heuristic teaching method. Through the introduction of the teaching content, combined with the example explanation and case analysis, the students are guided to think more, ask more questions and discuss more.

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）（五号宋体）

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（五号宋体）

（三）评分标准