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課程名稱 |
普通化學丙
General Chemistry (c) |
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開課學期 |
108-1 |
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授課對象 |
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授課教師 |
陳逸聰 |
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課號 |
Chem1009 |
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課程識別碼 |
203 101C0 |
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班次 |
05 |
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學分 |
3.0 |
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全/半年 |
半年 |
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必/選修 |
選修 |
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上課時間 |
星期三3,4(10:20~12:10)星期五3,4(10:20~12:10) |
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上課地點 |
普306普404 |
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備註 |
本課程中文授課,使用英文教科書。請依指定修習院系班次修習。詳閱化學系選課須知。初選期間不開放通識A7*課加選。。A7*:物質科學領域。可充抵通識
限學士班學生 且 限本系所學生(含輔系、雙修生)
總人數上限：60人 |
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Ceiba 課程網頁 |
http://ceiba.ntu.edu.tw/1081Chem1009_05 |
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課程簡介影片 |
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核心能力關聯 |
核心能力與課程規劃關聯圖 |
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課程大綱
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為確保您我的權利,請尊重智慧財產權及不得非法影印
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課程概述 |
本「普通化學」課程將以近代化學之發展為起點，首先講解在微觀觀點的論述下，構成原子與分子結構之量子概念。接著講述主導化學反應趨勢之熱力學定律，宰制化學反應快慢之動力學原理，其間並介紹電化學原理之應用。詳細授課內容所涵蓋之章節，條列於下列「課程大綱」中。 |
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課程目標 |
本「普通化學」之課程教學設計，旨在讓大一新鮮人理解化學之基本原理與定律。首先從學習量子力學之基本概念，得以了解原子與分子之結構。探究古典與統計熱力學之基本觀念與定律，以決定化學反應之趨勢與走向。理解動力學之原理，以解析化學反應速率之快慢及其反應機制。此外，探討分子內或分子間作用力之化學基本知識，對於後續之複雜生物分子結構、以及物質材料組態與構造將有助於全面性之理解。本課程亦強調化學基礎知識在生物科學上之應用，例如：學習電化學之基本原理，可藉以理解活細胞中因濃度梯度而造成電位變化等相關生理學現象之所據。 |
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課程要求 |
1. Chemical Foundations
1.1 Chemistry: An Atom First Approach
1.2 The Scientific Method
1.3 The Early History of Chemistry
1.4 Fundamental Chemical Laws
1.5 Dalton’s Atomic Theory
1.6 Early Experiments to Characterize the Atom
1.7 The Modern View of Atomic Structure: An Introduction
2. Atomic Structure and Periodicity
2.1 Electromagnetic Radiation
2.2 The Nature of Matter
2.3 The Atomic Spectrum of Hydrogen
2.4 The Bohr Model
2.5 The Quantum Mechanical Model of the Atom
2.6 Quantum Number
2.7 Orbital Shapes and Energies
2.8 Electron Spin and the Pauli Principle
2.9 Polyelectronic Atoms
2.10 The History of the Periodic Table
2.11 The Aufbau Principle and the Periodic Table
2.12 Periodic Trends in Atomic Properties
2.13 The Properties of a Group: The Alkali Metals
3. Bonding: General Concepts
3.1 Types of Chemical Bonds
3.2 Electronegativity
3.3 Ions: Electron Configurations and sizes
3.4 Energy Effects in Binary Ionic Compounds
3.5 Partial Ionic Character of Covalent Bonds
3.6 The Covalent Chemical Bonds: A Model
3.7 Covalent Bond Energies and Chemical Reactions
3.8 The Localized Electron Bonding Model
3.9 Lewis Structures
3.10 Exceptions to the Octet Rule
3.11 Resonance
3.12 Naming Simple Compounds
4. Molecular Structure and Orbitals
4.1 Molecular Structure: The VSEPR Model
4.2 Bond Polarity and Dipole Moment
4.3 Hybridization and the Localized Electron Model
4.4 The Molecular Orbital Model
4.5 Bonding in Homonuclear Diatomic Molecules
4.6 Bonding in Heteronuclear Diatomic Molecules
4.7 Combining the Localized Electron and Molecular Orbital Models
5. Stoichiometry
5.1 Counting by Weighing
5.2 Atomic Masses
5.3 Learning to Solve Problems
5.4 The Mole
5.5 Molar Mass
5.6 Percent Composition of Compounds
5.7 Determining the Formula of a Compound
5.8 Chemical Equations
5.9 Balancing Chemical Equations
5.10 Stoichiometric Calculations: Amounts of Reactants and Products
5.11 The Concept of Limiting Reactant
6. Types of Chemical Reactions and Solution Stoichiometry
6.1 Water, the Common Solvent
6.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes
6.3 The Composition of Solutions
6.4 Types of Chemical Reactions
6.5 Precipitation Reactions
6.6 Describing Reactions in solution
6.7 Stoichiometry of Precipitation Reactions
6.8 Acid-Base Reactions
6.9 Oxidation-Reduction Reactions
6.10 Balancing Oxidation-Reduction Reaction Equations
7. Chemical Energy
7.1 The Nature of Chemical Energy
7.2 Enthalpy
7.3 Calorimetry
7.4 Hess’s Law
7.5 Standard Enthalpies of Formation
7.6 Present Source of Energy
7.7 New Energy Sources
8. Gases
8.1 Pressure
8.2 The Gas Law of Boyle, Charles, and Avogadro
8.3 The Ideal Gas Law
8.4 Gas Stoichiometry
8.5 Dalton’s Law of Partial Pressures
8.6 The Kinetic Molecular Theory of Gases
8.7 Effusion and Diffusion
8.8 Real Gases
8.9 Characteristics of Several Real Gases
8.10 Chemistry in the Atmosphere
9. Liquids and Solids
9.1 Intermolecular Forces
9.2 The Liquid State
9.3 An Introduction to Structures and Types of Solids
9.4 Structure and Bonding in Metals
9.5 Carbon an Silicon: Network Atomic Solid
9.6 Molecular Solids
9.7 Ionic Solids
9.8 The Various Forces in Substances: Summary and Comparison
9.9 Vapor Pressure and Changes of State
9.10 Phase Diagrams
10. Properties of Solutions
10.1 Solution Composition
10.2 The Energies of solution Formation
10.3 Factors Affecting Solubility
10.4 The Vapor Pressures of Solutions
10.5 Boiling-Point Elevation and Freezing-Point Depression
10.6 Osmotic Pressure
10.7 Colligative Properties of Electrolyte Solutions
10.8 Colloids
11. Chemical Kinetics
11.1 Reaction Rates
11.2 Rate Laws: An Introduction
11.3 Determining the Form of the Rate Law
11.4 The Integrated Rate Law
11.5 Reaction Mechanisms
11.6 A Model for Chemical Kinetics
11.7 Catalysis
12. Chemical Equilibrium
12.1 The Equilibrium Condition
12.2 The Equilibrium Constant
12.3 Equilibrium Expressions Involving Pressures
12.4 Heterogeneous Equilibria
12.5 Applications of the Equilibrium Constant
12.6 Solving Equilibrium Problems
12.7 Le Châtelier's principle
13. Acid and Bases
13.1 The Nature of Acid and Bases
13.2 Acid Strength
13.3 The pH Scale
13.4 Calculating the pH of Strong Acid Solutions
13.5 Calculating the pH of Weak Acid Solutions
13.6 Bases
13.7 Polyprotic Acid
13.8 Acid-Base Properties of Salt
13.9 The Effect of Structure on Acid-Base Properties
13.10 Acid-Base Properties of oxides
13.11 The Lewis Acid-Base Model
13.12 Strategy for Solving Acid-Base Problems: A Summary
14. Acid-Base Equilibria
14.1 Solutions of Acids or Bases Containing a Common Ion
14.2 Buffered Solutions
14.3 Buffering Capacity
14.4 Titrations and pH Curves
14.5 Acid-Base Indicators
15. Solubility and Complex Ion Equilibria
15.1 Solubility Equilibria and the Solubility Product
15.2 Precipitation and Qualitative Analysis
15.3 Equilibria Involving Complex Ions
16. Spontaneity, Entropy, and Free Energy
16.1 Spontaneous Processes and Entropy
16.2 Entropy and the Second Law of Thermodynamics
16.3 The Effect of Temperature on Spontaneity
16.4 Free Energy
16.5 Entropy Changes in Chemical Reactions
16.6 Free Energy and Chemical Reactions
16.7 The Dependence of Free Energy on Pressure
16.8 Free Energy and Equilibrium
16.9 Free Energy and Work
17. Electrochemistry
17.1 Balancing Oxidation-Reduction Equations
17.2 Galvanic Cells
17.3 Standard Reduction Potentials
17.4 Cell Potential, Electrical Work, and Free Energy
17.5 Dependence of Cell Potential on Concentration
17.6 Batteries
17.7 Corrosion
17.8 Electrolysis
17.9 Commercial Electrolytic Processes
18. The Nucleus: A Chemist’s View
18.1 Nuclear Stability and Radioactive Decay
18.2 The Kinetics of Radioactive Decay
18.3 Nuclear Transformations
18.4 Detection and uses of Radioactivity
18.5 Thermodynamic Stability of the Nucleus
18.6 Nuclear Fission and Nuclear Fusion
18.7 Effect of Radiation
19. The Representative Elements
19.1 A Survey of the Representative Elements
19.2 The Group 1A(1) Elements
19.3 The Chemistry of Hydrogen
19.4 The Group 2A(2) Elements
19.5 The Group 3A(13) Elements
19.6 The Group 4A(14) Elements
19.7 The Group 5A(15) Elements
19.8 The Chemistry of Nitrogen
19.9 The Chemistry of Phosphorus
19.10 The Group 6A(16) Elements
19.11 The Chemistry of Oxygen
19.12 The Chemistry of Sulfur
19.13 The Group 7A(17) Elements
19.14 The Group 8A(18) Elements
20. Transition Metals and Coordination Chemistry
20.1 The Transition Metals: A Survey
20.2 The First-Row Transition Metals
20.3 Coordination Compounds
20.4 Isomerism
20.5 Bonding in Complex Ions: The Localized Electron Model
20.6 The Crystal Field Model
20.7 The Biological Importance of Coordination
20.8 Metallurgy and Iron and Steel Production
21. Organic and Biological Molecules
21.1 Alkanes: Saturated Hydrocarbons
21.2 Alkenes and Alkynes
21.3 Aromatic Hydrocarbons
21.4 Hydrocarbons Derivatives
21.5 Polymers
21.6 Natural Polymers
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預期每週課後學習時數 |
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Office Hours |
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指定閱讀 |
待補 |
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參考書目 |
Text Book：Chemistry: An Atoms First Approach (Second Edition)
Author： Steven S. Zumdahl, Susan A. Zumdahl
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評量方式
(僅供參考) |
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