Inorganic Chemistry

Hong Jin, Dramou Pierre, Wang Yue, Guo Qi, and Li Jiabin

目录

  • 1 Introduction
    • 1.1 What is chemistry?
    • 1.2 What are banches of chemistry?
    • 1.3 What is inorganic chemistry?
    • 1.4 How is the course organized and graded?
    • 1.5 How to learn this course effectively?
    • 1.6 Pre-test
  • 2 Gases and Solutions
    • 2.1 Introduction
    • 2.2 Gases
    • 2.3 Solutions
    • 2.4 Learning outcomes and exercises
  • 3 Thermochemistry
    • 3.1 Energy
    • 3.2 The First Law of Thermodynamics
    • 3.3 Enthalpy
    • 3.4 Enthalpies of Reaction
    • 3.5 Hess's Law
    • 3.6 Enthalpies of Formation
    • 3.7 Learning outcomes and exercises
  • 4 Chemical Thermodynamics
    • 4.1 Spontaneous Processes
    • 4.2 Entropy and the Second Law of Thermodynamics
    • 4.3 The Molecular Interpretation of Entropy and the Third Law of Thermodynamics
    • 4.4 Entropy Changes in Chemical Reactions
    • 4.5 Gibbs Free Energy
    • 4.6 Free Energy and Temperature
    • 4.7 Learning outcomes and exercises
  • 5 Chemical Kinetics
    • 5.1 Factors that Affect Reaction Rates
    • 5.2 Reaction Rates
    • 5.3 Concentration and Rate Laws
    • 5.4 Temperature and Rate
    • 5.5 Catalysis
    • 5.6 Learning outcomes and exercises
  • 6 Chemical Equilibrium
    • 6.1 The Concept of Equilibrium
    • 6.2 The Equilibrium Constant
    • 6.3 Understanding and Working with Equilibrium Constants
    • 6.4 Calculating Equilibrium Constants
    • 6.5 Applications of Equilibrium Constants
    • 6.6 Le Châtelier's Principle
    • 6.7 Free Energy and the Equilibrium Constants
    • 6.8 Learning outcomes and exercises
  • 7 Acid-Base Equilibria
    • 7.1 The Concepts of Acids and Bases
    • 7.2 The Autoionization of Water
    • 7.3 The pH Scale
    • 7.4 Strong Acids and Bases
    • 7.5 Weak Acids and Bases
    • 7.6 Relationship between Ka and Kb
    • 7.7 Acid-Base Properties of Salt Solutions
    • 7.8 Lewis Acids and Bases
    • 7.9 Learning Outcomes and Exercises
    • 7.10 Lecture Notes Handout
  • 8 Solubility Equilibria
    • 8.1 Precipitation Reactions
    • 8.2 Saturated Solutions and Solubility
    • 8.3 Solubility Equilibria
    • 8.4 Factors Affecting Solubility
    • 8.5 Precipitation and Separation of Ions
    • 8.6 Learning Outcomes
    • 8.7 Lecture Notes Handout
  • 9 Electronic Structure of Atoms & Periodic Table
    • 9.1 The Discovery of Atomic Structure
    • 9.2 The Wave Nature of Light
    • 9.3 Quantized Energy and Photons
    • 9.4 Line Spectra and the Bohr Model
    • 9.5 The Wave Behavior of Matter
    • 9.6 Quantum Mechanics and Atomic Orbitals
    • 9.7 Many-Electron Atoms and Electron Configuration
    • 9.8 The Periodic Table and Periodic Properties of the Elements
    • 9.9 Learning Outcomes and Exercises
  • 10 Chemical Bonding, Molecular Geometry and Intermolecular Forces
    • 10.1 Ionic Bonding
    • 10.2 Covalent Bonding and Orbital Overlap
    • 10.3 The VSEPR Model
    • 10.4 Hybrid Orbital Theory
    • 10.5 Molecular Orbital Theory
    • 10.6 Intermolecular Forces
    • 10.7 Learning Outcomes and Exercises
  • 11 Redox Reactions & Electrochemistry
    • 11.1 Redox Reactions and Oxidation Numbers
    • 11.2 Balancing Redox Equations
    • 11.3 Voltaic Cells
    • 11.4 Cell Potentials under Standard Conditions
    • 11.5 Free Energy and Equilibrium Constant*
    • 11.6 Free Energy and Redox Reactions
    • 11.7 Cell Potentials under Nonstandard Conditions
    • 11.8 Some Applications of Electrochemistry
    • 11.9 Learning Outcomes and Exercises
  • 12 Transition Metals & Coordination Chemistry
    • 12.1 The Transition Metals
    • 12.2 Transition-Metal Complexes
    • 12.3 Common Ligands in Coordination Chemistry
    • 12.4 Nomenclature and isomerism in Coordination Chemistry
    • 12.5 Color and Magnetism in Coordination Chemistry
    • 12.6 Crystal-Field Theory
    • 12.7 Learning Outcomes and Exercises
  • 13 Supplymentary Materials
    • 13.1 Note
    • 13.2 Gases and Solutions
    • 13.3 Thermodynamics
    • 13.4 Kinetics and Equilibrium
      • 13.4.1 Application of Equilibrium Concentration
      • 13.4.2 Le Chatelier's Principle
    • 13.5 Acid-Base and Precipitation
    • 13.6 Matter Structures
    • 13.7 Electrochemistry and Coordination
Pre-test

The Pre-test will be allowed to take after 10:20 am of Feb-18-2020, some explanations to this test are listed below,

1. Pre-test is designed to collect enough information of the background and level of chemistry you have before this course. The exact results will help us to make an effective teaching plan and adjustment for you. Every student has to take the pre-test although your score of pre-test will NOT be counted into your course grade.

2. Prerequisites: You have to finish more than 80% of the tasks in chapter 1 before starting the pre-test.

3. Time limitation: 60 minutes, only once, please arrange your time and finish the pre-test as early as possible. 

4. Content: There are 25 multiple-choices-with-one-answer questions and 3 short-answer question in pre-test.

5. Preparation: Good network connection and a computer are required for taking this test, smart phone is less convenient to finish the short-answer questions than laptop.

6.     You can not see the results and score until all of your classmates finish the test and the teachers complete the analysis of that.  The teaching group will inform you when it is ready.

7.     For the computer user, the entrance of pre-test was showed in the picture below, while smart phone user can download the tutorial file (at the bottom of this page) to learn how to open pre-test in your mobile phone.  

Don't worry about the pre-test, arrange your time and make a good preparation before taking it. You are able to finish the test smoothly! Good luck!