- Course name: General chemistry
- Code course: 2104039
- Course credit: 3(3,0,6)
- Degree: First year student
- Course hours
- Class 45 hours
- Laboratory 0 hour
- Home study 90 hours
- Prerequisite: No
- Course Objectives
Course prove chemical bonding and molecular structure and chemical process knowledge
- Course Description
This course is the first of a three-quarter sequence in Chemistry intended for students majoring in the sciences or engineering. Covers atomic nature of matter, stoichiometry, periodic table, acids and bases, and gas laws, thermochemistry, electrochemistry. Group work in class includes active learning exercises.
- Student duty:
Class attandance, assay, examine acording to the regulation No. 43/2007-QĐ-BGD&ĐT date 15/08/2007 of MOET, regulation No 235/QĐ-ĐHCN-ĐT date 30/08/2007 of IUH.
- Course material:
Textbook:
Principle of general chemistry, Martin S. Silberberg, McGraw-Hill Higher Education, 2007.
Reference:
General Chemistry, Raymond Chang, Jason Overby, College of Charlesto 2011.
- Grades:
- Class Participation
- Assay
- Short quizzes
- Mid term
- Final term
- Other
- Grade Rule: Follow the credit regulation
- Contents:
| No. |
Content | Hours | Hours | Note | ||
| Class | Lab | Home study | ||||
| 1 | Chapter 1: Fundamental Definitions and laws of chemistry | 3 | 3 | 6 | ||
| 2 | Chapter 2: Quantum Theory and Atomic Structure | 6 | 6 | 12 | ||
| 3 | Chapter 3: Chemical Periodicity and Chemical Table |
3 |
3 |
6 |
||
| 4 | Chapter 4: Chemical bonding and molecular structure | 8 | 8 | 16 | ||
| 5 | Chapter 5 Sate of matter | 1 | 1 | 2 | ||
| 6 | Chương 6: Thermochemistry and Thermodynamics | 5 | 5 | 10 | ||
| 7 | Chapter 7: Chemical Equilibrium | 3 | 3 | 6 | ||
| 8 | Chapter 8: Kinetics: Rates and Mechanisms of Chemical Reaction | 3 | 3 | 6 | ||
| 9 | Chapter 9: Solution | 8 | 8 | 16 | ||
| 10 | Chapter 10: Electrochemistry: Chemical Change and Electrical Work | 5 | 5 | 10 | ||
| Total | 45 | 45 | 90 | |||
Chapter 1: Fundamental Definitions and laws of chemistry
1.1. Fundamental Definitions
1.1.1. Atome and molecules
1.1.2. Atomic nucleus
1.1.3. Elements, Isotopes
1.1.4. Atomic Symbol, Chemical Formula and chemical equation
1.1.5. Compounds and
1.1.6. Atomic Masses, Atomic Number, Mass Number, Molar Mass
1.2. Basic laws
1.2.1 Law of Mass Conservation
1.2.2. Law of Definite Composition Law
1.2.3 Law of Multiple Proportions
1.2.4. Law of Volumetric Ratio
1.2.5. Avogadro’s Law and Avogadro number
1,2,6 Boy- Mariotte’s Law and Charler-Gay-Lussac’s Law and Dalton’s Law
1.2.7. The Ideal Gas Equation
1.2.8. Law of Equivalent
1.3 Their Experimental Foundations of atom, molecules and compounds
Chapter 2: Quantum Theory and Atomic Structure
2.1. The Nature of Light and Atomic Spectra
2.1.1 The Wave and particle Nature of Light
2.1.2 Atomic Spectra
2.2. The Classical Atomic Theory
2.2.1. Thompson Theory
2.2.2 Rutherford Theory
2.2.3 Bohr’s atomic theory and Bohr-Somerfeld
2.3. The Atomic Theory Today
2.3.1. The Wave-Particle Duality of Matter and Energy
2.3.2. The de Broglie Wavelengths
2.3.3. The Heisenberg Uncertainty Principle
2.3.4. Schrodinger’s Wavelengths Equation
2.4. Characteristics of Signle-Electron Atoms and the Quantum-Mechanical Model of the Atom
2.5 Characteristics of Many-Electron Atoms and Electron Configurations
2.5.1 The Electron-Spin Quantum Number
2.5.2 The Exclusion Principle
2.5.3 Electrostatic Effects and Energy-Level Splitting
2.5.4. Electron Configurations
Chapter 3: Chemical Periodicity and Chemical Table
3.1. Chemical Periodicity
3.2. Development of the Periodic Table Electron Configurations
3.2.1 Period
3.2.2 Group
3.2.3 Sub-group
3.3. Trends in Atomic Properties
3.4.1. Trends in Atomic Size
3.4.2. Trends in Ionization Energy
3.4.3. Trends in Electron Affinity
3.4.4. Trends in Metallic Behavior
3.4.5. Oxidation number
Chapter 4: Chemical bonding and molecular structure
4.1. An Overview of Chemical Bonding
4.2. Ionic bonds
4.2.1. Energy Considerations in Ionic Bonding
4.2.2. Periodic Trends in Lattice Energy
4.2.3. How the Model Explains the Properties of Ionic Compounds
4.3. The Covalent Bonding Model
4.3.1 Valence Bond (VB) Theory and Orbital Hybridization
The Central Themes of VB Theory
Types of Hybrid Orbitals
The Mode of Orbital Overlap and the Types of Covalent Bonds
4.3.2 Molecular Orbital (MO) Theory and Electron Delocalization
The Central Themes of MO Theory
Homonuclear Diatomic Molecules of the Period 1 and 2 Elements
4.4. Metal bonds
4.5 Weak bonds
4.5.1 Hydrogen bond
4.5.2 Van Der Waals Bond
Chapter 5 Sate of matter
5.1 An Overview of Physical States and phase Changes of Matter
5.2 Gas State
5.3 Liquid State
5.4 Solid State
Chương 6: Thermochemistry and Thermodynamics
6.1 An Overview (Thermochemistry, thermodynamic, system, state, work, energy and heat)
6.2 The First Law of Thermodynamics:
6.2.1 Internal Energy
6.2.2 Equation
6.2.3 Apllication (Specific Heat Capacity,….)
6.2.4 Heat of chemical reaction
6.2.5 Hess’s Law
6.3. The Second Law of Thermodynamics
6.3.1 Reaction direction (Reaction Spontaneity, Reaction Nonspontaneity… )
6.3.2 The Second Law of Thermodynamics: – Entropi
6.3.3 Entropy Changes
6.3.4 Entropy, Free Energy, and Reaction Direction
Chapter 7: Chemical Equilibrium
7.1 Fundermental (Reversible Reactions, …)
7.2 The Reaction Quotient and the Equilibrium Constant
7.2.1 Van’t Hoff’s Equation
7.2.2 Expressing Equilibria with Pressure and Concentration Terms
7.3 Reaction Conditions and the Equilibrium State
7.3.1 Le Chotelier’s Principle
7.3.2 The Effect of a Change in Concentration
7.3.3 The Effect of a Change in Pressure (Volume)
7.3.4 The Effect of a Change in Temperature
Chapter 8: Kinetics Rates and Mechanisms of Chemical Reaction
8.1 An Overview of Kinetic
8.1.1 Object of study
8.1.2 Expressing the Reaction Rate
8.1.3 Single Reaction and Multiple Reaction
8.1.4 Reaction Mechanisms
8.1.5 Reaction Orders
8.2 The Effect of Concentration on Reaction Rate
8.2.1 Mass Law
8.2.2 First-Order Reactions
8.2.3. Second-Order Reactions
8.2.3 Zero-Order Reactions
8.3 The Effect of Temperature on Reaction Rate
8.3.1 Van’t Hoff Law
8.3.2 Arrhenius’s Equation
8.4 The Effect of a Catalyst on Reaction Rate
8.4.1 Overview of Catalyst
8.4.2 Classification
8.4.3 Properties of Catalyst
Chapter 9: Solution
9.1. Types of Solutions
9.1.1 Solid Phase Solution
9.1.2 Concentration Term
9.1.3 Formation of Solution (
9.1.4 Solubility and Effect of Factors on Solubility
9.1.5 Why Substances Dissolve: Understanding the Solution Process (Heats of Solution and Solution Cycles; Heats of Hydration: Ionic Solids in Water; The Solution Process and the Change in Entropy)
9.2. Properties of Nonvolatile Nonelectrolyte Solutions
9.2.1 Vapor Pressure – Raoult’s Law I
9.2.2 Boiling Point Elevation Freezing Point Depression – Raoult’s Law II
9.2.3 Osmotic Pressure-Van’t Hoff’s Law
9.3 Properties of Electrolyte Solutions
9.3.1 Electrolytic Theory (The Van’t Hoft factor, Arrhenius Theory)
9.3.2 Dissocication, Dissocication Constant and Factors effect on Dissocication
9.3.3 Ionic Equilibria in Aqueous Systems (Equilibria of Strong Electrolyte Compounds, Equilibria of Slightly Soluble Ionic Compounds; The lon-Product Expression (Qsp) and the Solubility-Product Constant (Ksp); The Effect on Solubility)
9.3.4 Acid-Base Theory and Acids and Bases in Water (The Acid-Dissociation Constan, Arrhenius’s Acid-Base Theory, Bronsted Acid-Base, Lewis Acid-Base)
Chapter 10: Electrochemistry
10.1 Redox Reactions
10.1.1 Oxidation-Reduction Concepts
10.1.2 Half-Reaction Method for Balancing Redox Reactions
10.2 Ganvanic Cell
10.2.1 Gavanic Cells
10.2.2 Construction and Operation of Ganvanic Cells
10.2.3 Electrical Energy l of Ganvanic Cell
10.3 Cell Potential and Equilibrium Constant of Redox Reactions
10.3.1 Standard Cell Potential
10.3.2 Electrodes
10.3.3 Nernst Equation
10.3.4 Direction of Redox Reactions
10.4 Electrolysis
10.4.1 Electrolysis Concept
10.4.2 Laws (Faraday 1 and 2)
10.4.3 Electrolysis of Electrolyte Ionic Compounds: (NaCl, NaOH, H2SO4)
10.5 Industrial Electrochemistry
10.5.1 Batteries
10.5.2 Fuel Cells
