Course code: 20 12 1 1

English name of the course: Organic and Analytical Chemistry

Course category: basic subject courses

Credits: 5 credits

Total class hours: 144

Theoretical class hours: 80

Class object: chemical engineering, pharmacy, high-quality materials, food, environmental engineering, sanitary engineering and other majors in the whole school.

First semester: the first and second semesters.

Textbook: Inorganic and Analytical Chemistry, Zhejiang University, Higher Education Press.

Main reference books:

1. Inorganic and Analytical Chemistry, Research Group of Inorganic and Analytical Chemistry, Nanjing University, Higher Education Press (3rd edition).

2. Inorganic Chemistry (Volume I and Volume II), written by Dalian University of Technology, Higher Education Press (Third Edition)

3. Analytical Chemistry, edited by Wuhan University, Higher Education Press (Third Edition)

First, the nature, purpose and task of the course.

This course is a compulsory basic chemistry course for engineering majors in the first academic year. It is a combination of inorganic chemistry and analytical chemistry. This course attempts to combine inorganic chemistry and analytical chemistry closely, so that the two basic courses can be integrated, and the theory and knowledge in inorganic chemistry can be directly combined with analytical chemistry and applied to experiments and measurements, so that theory and practice can be more closely combined and learning efficiency can be improved. It is an important link to cultivate the overall knowledge structure and ability of engineering students, and it is also the basis of subsequent courses.

The task of this course is to enable students to independently analyze and deal with inorganic chemistry problems and basic analytical problems while acquiring basic theories and knowledge of inorganic chemistry and analytical chemistry (to master the basic operation skills of experiments and be competent for general basic analytical work).

Second, the course content, basic requirements and class allocation

Introduction (1 class)

1. solution and colloid (4 hours)

(1) dispersion system;

(2) the expression method of solution concentration;

(3) The universality of dilute solution: the law of gas partial pressure, the decrease of vapor pressure, the increase of boiling point, the decrease of freezing point and osmotic pressure;

(4) Colloidal solution: the properties of colloidal solution, the structure of micelle, the stability and cohesiveness of sol.

This chapter focuses on the dependence of dilute solution.

2. General principles of chemical reactions (12 class hours)

(1) Basic concepts and the first law of thermodynamics;

(2) Thermochemistry: heat, work, isovolumetric reaction heat, isobaric reaction heat, enthalpy and thermochemical equations.

(3) Gass theorem, calculation of chemical reaction heat;

(4) chemical reaction direction: chaos and entropy, the criterion of chemical reaction direction, the relationship between Gibbs free energy change and temperature;

(5) Chemical equilibrium and its movement: reversible reaction and chemical equilibrium, equilibrium constant, principle of chemical equilibrium movement;

(6) Chemical reaction rate: the concept of chemical reaction rate, chemical reaction rate equation, reaction rate theory, activation energy, temperature and the influence of catalyst on reaction rate;

(7) Optimization of chemical reaction conditions

This chapter focuses on: the properties, calculation and application of enthalpy, entropy and Gibbs function; The relationship between standard equilibrium constant and Gibbs function and related calculation: Understand the concepts of reaction rate, elementary reaction, reaction order and the factors affecting reaction rate.

Difficulties in this chapter: understanding the nature of state function, the relationship between enthalpy, entropy, Gibbs function and equilibrium constant, and the calculation of elementary reaction rate.

3. Basis of quantitative analysis (4 hours)

(1) Tasks and functions of analytical chemistry;

(2) Classification of quantitative analysis methods: chemical analysis and instrumental analysis;

(3) the general process of quantitative analysis and the expression of results;

(4) Errors in quantitative analysis: accuracy and precision, causes of errors and methods to reduce errors;

(5) Data processing of analysis results: average deviation and standard deviation, confidence interval of average value, selection of suspicious values, processing and reporting of analysis results;

(6) Effective numbers and their operation rules

(7) Overview of titration analysis: classification of titration analysis and requirements for chemical reactions, calculation of standard substances and standard solutions, and calculation rules of titration analysis;

The focus of this chapter: error, significant figures

Difficulties in this chapter: data processing of analysis results, meaning of significant figures and operation rules.

Mid-term exam (2 hours)

4. Acid-base balance and acid-base titration (10 class hour)

Ionization of (1) electrolyte: strong electrolyte and weak electrolyte, activity and activity coefficient;

(2) Acid-base proton theory;

(3) Acid-base balance: the pH value of solution and its calculation, the movement of acid-base balance;

(4) Buffer solution: composition and properties of buffer solution, calculation of acidity and buffer capacity of buffer solution;

(5) Distribution of species in weak alkaline solution;

(6) Alkaline titration: acid-base titration curve and indicator, preparation and calibration of acid-base standard solution, and application of acid-base titration;

This chapter focuses on: acid-base proton theory, calculation of pH value in weak electrolyte solution, calculation of pH value in buffer solution, acid-base titration and its application.

Difficulties in this chapter: the definition of acid and alkali, the calculation formula of pH value of different types of weak electrolyte solutions, the calculation of pH value in acid-base titration and the selection of indicator.

5. Precipitation-dissolution equilibrium and its application in analytical chemistry (5 hours)

(1) Precipitation-dissolution equilibrium: solubility product, solubility product, solubility;

(2) Application of solubility product principle: solubility product principle, precipitation generation, precipitation dissolution, step-by-step precipitation and precipitation transformation;

(3) Precipitation titration: the summary of precipitation titration, the determination of titration curve and the end point of silver titration-the application of Mohr method, Forhad method and Fayens method;

This chapter focuses on: solubility product constant, solubility product principle and application, and several common precipitation titration methods.

Difficulties in this chapter: the application of solubility product principle in practice

6. Redox Balance and Redox Titration (12 class hours)

(1) redox reaction, oxidation number, redox;

(2) Balance of redox equation: Balance by ion electron method;

(3) Electrode potential: the definition of galvanic cell, standard electrode potential, and Nernst equation, which is a factor affecting electrode potential;

(4) Application of electrode potential: calculation of electromotive force of primary battery, equilibrium constant of redox reaction;

(5) Elemental electrode potential diagram and its application;

(6) The rate of redox reaction and its influencing factors;

(7) Redox titration: Redox titration curve, indicator and common redox titration methods;

This chapter focuses on the definition, application and redox titration of electrode potential.

Difficulties in this chapter: calculation of electrode potential and application of Nernst equation.

7. Material Structure Foundation (10 class hour)

(1) The motion state of extranuclear electrons: the motion characteristics of microscopic particles, atomic orbits and electron cloud images;

(2) Multi-electron atomic structure: extranuclear electron configuration rule, electron shell structure and periodic law of elements;

(3) Chemical bond theory: ionic bond theory, valence bond theory and molecular orbital theory; * * * valence bond theory; * * * Price keyword type;

(4) Spatial configuration of polyatomic molecules: valence shell electron pair repulsion theory; Mixed orbit theory;

(5) Valuable substance crystals: molecular crystals;

(6) ionic crystal: ionic polarization;

This chapter focuses on: the rules of extranuclear electron configuration, the theory of chemical bonds, the judgment of the spatial configuration of polyatomic molecules, and ionic polarization.

Difficulties in this chapter: explain the formation of chemical bonds and the judgment of molecular space configuration with different theories.

8. Coordination Compounds and Coordination Titration (10 class hour)

Basic concepts of (1) coordination compounds: composition and nomenclature of coordination compounds;

(2) Chemical bond theory of coordination compounds: valence bond theory and crystal field theory;

(3) Dissociation equilibrium of coordination ions in solution: coordination equilibrium constant, coordination equilibrium shift;

(4) Chelates

(5) coordination titration: coordination titration curve, metal indicator

(6) Application of coordination titration

This chapter focuses on: naming of coordination compounds, chemical bond theory of coordination compounds, movement of coordination equilibrium and coordination titration.

Difficulties in this chapter: valence bond theory, coordination equilibrium movement

9. Ultraviolet-visible spectrophotometry (4 hours)

(1) Overview

(2) Light absorption law: Lambert-Beer law and the reasons for its deviation.

(3) Ultraviolet-visible spectrophotometer and determination method.

(4) Color reaction and its influencing factors.

(5) Error of UV-Vis Spectrophotometry and Selection of Measurement Conditions (6) Application Example of UV-Vis Spectrophotometry

10. Introduction to Modern Instrumental Analysis (2 hours)

(1) potential analysis method

(2) Atomic absorption spectrophotometry

(3) chromatographic analysis

1 1. Elemental chemistry (4 hours)

Elements in (1)d region

(2) 2) Elements in the DS region

Third, exercises and extracurricular teaching requirements

Each chapter is required to read several reference books at the same time.

The requirements for students' homework are: each student should prepare two exercise books, hand them in on time after class every time, finish them independently, and do not copy them.

The requirement for teachers to correct homework is that every homework should be carefully reviewed, corrected in time and sent to students. When correcting, we should point out the mistakes and let the students correct them. After each correction, students should be explained the typical mistakes in their homework and their correction methods. Homework should be graded, and a certain proportion should be recorded in the total grade of the semester.

Fourth, assessment methods and performance evaluation.

Exam: In the first semester, there will be a mid-term exam and a final exam. Mid-term and final exams are generally conducted in the form of closed-book exams.