Principles of Chemistry

Course Code: B32001Y-01

Course Name:Principles of Chemistry

Credits: 3.0

Level: Undergraduate

Lecture Time: 60 hours

Course Description

This course is a basic course for undergraduates of chemistry andchemical engineering, and also can be an elective course for undergraduates whose majors are materials science, life science, environmental science, earth science, physics, medicine and pharmacy and other related majors.

This course focuses on the various basic principles of chemistry; the main contents include:basic law of gas and liquid, chemical thermodynamics and the direction of chemical reaction, chemical kinetics and reaction rate equation, atomic structure and deductions of quantum theory,molecular structure and molecular theory, crystal structure, complex compound and element chemistry etc. Through teaching, self-studying and classroom discussion, students should fully understand the basic concepts of chemistry, grasp the basic theories of chemistry and their application, establish a mode of thinking in chemistry, develop the ability to solve practical problems in chemical methods, and lay a solid foundation for the follow-up study of professional courses and related research work.

Topics and Schedule

Chapter 1   Gas, Liquid, Solid and Phase Change

  1.    Ideal gas equation;
  2.    Law of gas combining volumes and the Avogadro hypothesis;
  3.    Gas partial pressure law;
  4.    Gas diffusion law;
  5.    Gas molecular motion theory;
  6.    Velocity distribution and energy distribution of molecules;
  7.    Actual gas and Van Der Waals equation;
  8.    Liquefaction of gas · critical phenomenon;
  9.     Evaporation of liquid · vapor pressure;
  10. Solidification of liquids · melting of solids;
  11. Phase diagram of water;
  12. Liquid and liquid crystal.

Chapter 2   Solution

  1.    The concentration of solution;
  2.    Solubility;
  3.    The colligative properties of non-aqueous electrolyte dilute solution;
  4.    The colligative properties and conductivity of electrolyte solutions;
  5.    Colloidal solution.

Chapter 3   Chemical Thermodynamics

  1.    Measurement of heat of reaction;
  2.    Basic concepts of chemical thermodynamics:
  3.    Enthalpy and enthalpy change;
  4.    Thermochemistry equation and the law of thermochemistry;
  5.    Enthalpy of formation;
  6.    Bond enthalpy;
  7.    Entropy;
  8.    Gibbs free energy;
  9.    The application of Gibbs-Helmholtz equation

Chapter 4   Chemical Equilibrium and Chemical Kinetics

  1.    Equilibrium constant;
  2.    Equilibrium constant and Gibbs free energy change;
  3.    Multiple equilibrium;
  4.    Shift of chemical equilibrium;
  5.    The significance of reaction rate;
  6.    Concentration and reaction rate;
  7.    Order of reaction;
  8.    Temperature and reaction rate · activation energy;
  9.    Mechanism of reaction;
  10. Catalysis
  11. Acid-base balance theory;
  12. The equilibrium of self-coupling and ionization of water;
  13. The ionization equilibrium of weak acid-weak base;
  14. The shift of acid-base ionization equilibrium;
  15. Buffer solution;
  16. Neutralization reaction;
  17. Precipitation dissolution equilibrium:
  18. Solubility product;
  19. Formation of precipitation;
  20. Dissolution of precipitation;
  21. Transformation of precipitation;
  22. Fractional precipitation.

Chapter 5   Oxidation Reduction ·Electrochemistry

  1.    Oxidation number and balancing oxidation reduction equations;
  2.    Electromotive force of the battery and electrode potential;
  3.    Standard electrode potential and oxidation-reduction equilibrium;
  4.    Indirect calculation of electrode potential;
  5.    Effect of concentration on electrode potential -Nernst equation;
  6.    Calculating Ksp or pH by determination of electric potential;
  7.    Decomposition potential and over potential;
  8.    Electrochemical power source.

Chapter 6   Atomic Structure

  1.    The establishment of classical nuclear atomic model;
  2.    Atomic spectrum of hydrogen and Bohr hydrogen atom theory;
  3.    Microscopic particle characteristics and its law of motion;
  4.    Quantum mechanical model of hydrogen atom;
  5.    Polyelectron Atomic Structure and periodic law;
  6.    Periodic variation of basicproperties of elements.

Chapter 7   Chemical Bond and Molecular Structure

  1.    Ionic bond theory;
  2.    Classical Lewis theory;
  3.    Valence bond theory;
  4.    Molecular orbital theory;
  5.    Valence shell electron pair repulsion theory;
  6.    Polarity of molecules;
  7.    Metal bond theory;
  8.    Intermolecular force and hydrogen bond.

Chapter 8   Crystal and Crystal Structure

  1.    Characteristics of crystals;
  2.    Periodicity of crystal structure;
  3.    The packing of equal diametersphere;
  4.    Basic types and structures of crystals;
  5.    Chemical bond type and the variation of crystal structure;
  6.    Crystal imperfection ·amorphous.

Chapter 9   Complex Compound

  1.    Basic concept, composition, type and nomenclature of complex compounds;
  2.    The isomerism of complex compounds;
  3.    Valence bond theory of complex compound;
  4.    Crystal field theory;
  5.    Complex equilibrium and equilibrium constant;
  6.    The shift of complex equilibrium;
  7.    Application of complex compounds.

Chapter 10   Element Chemistry

  1. Elements of s-block and p-block;
  2. Elements of d-block and f-block;
  3. Abundance of elements in nature;
  4. Preparation of inorganic compounds.


[1]    Hua Tongwen, Wang Yingxia, Bian Jing, Chen Jingzu,General Principles of Chemistry (4th Edition),Peking University Press, 2013

[2]    Jin Ruoshui, Wang Yunhua, Rui Chengguo,Principles of Modern Chemistry (and),Higher Education Press,2003

[3]    Fu Xiancai, University Chemistry(and), Higher Education Press, 1999

[4]    Yin YongJia, Yao Tianyang, Principles of Chemistry (First Edition), Higher Education Press, 2006

[5]    General Chemistry Teaching and Research Group,Zhejiang University, General Chemistry (6th Edition), Higher Education Press2011