全国高中学生化学竞赛基本内容（Basic content of chemistry competition for senior high school students in China）The national high school student chemistry competition basic content.Txt, the real good friend is not together has the topic which cannot say, but is together, even if does not speak, will not feel embarrassed. When you look at other people, you are also the scenery in other people's eyes. The road to tomorrow must remember the road that we walked yesterday and the road we are walking today. Basic content of chemistry competition for senior high school students in ChinaThe 1. national chemistry contest of senior high school students (preliminary division contest) and final (winter) two stages, plus the winter after the national team players qualifying in three stages. The basic contents of the preliminary and final examination reflects the national level, is the basis of the examination proposition. The selection of the national team's athletes shall be based on the preparation of the International Chemistry Olympiad in the year.2. the current middle school chemistry teaching requirements and contents are preliminary examination shows that the content of the provisions. A consistent level of content knowledge in preliminary principle to full-time high school chemistry textbook published by people's education press, but for some of the chemical principle of the quantitative relationship, material structure, solid chemistry and organic chemistry and other supplements, in general, supplementary content is the natural growth point in chemical content. The preliminary requirements of knowledge in order to achieve internationalchemical descriptive chemistry contest outline level as the standard, the outline of the two or three levels of knowledge are not required in the application of memory based on.The basic content of the final 3. is properly based on the basic contents of preliminaries, descriptive chemistry knowledge principle to reach the international level two level of knowledge of chemistry contest syllabus for the degree, the outline of the three levels of knowledge are not required in the application of memory based on.4., pay attention to the intersection and interpenetration of chemical knowledge and non chemical knowledge, but the requirements of mathematics and physics knowledge should not exceed the requirements of middle school syllabus.5. basic content, if necessary, will be adjusted and announced in mid August 2001.The basic content of the preliminaries1. the concept and application of effective numbers. Correct use of effective figures in chemical and chemical experiments. Quantitative instrument (analytical balance, cylinder, pipettes, burettes, flask etc.) the effective number of precision and measuring data. The valid number of the result of the operation.2. ideal gas standard condition. Ideal gas equation of state. Gas density. Determination of relative molecular mass of gases. Gas solubility. Law of partial pressure.3. solution concentration, solid solution and calculation. Solution preparation (selection of instruments based on the accuracy of concentration). Estimation of the amount of purification by recrystallization. Selection of washing liquid and selection of washing method in washing operation. The law of solvent (including mixed solvent) similarity with solutes.4. basic concepts of titrimetric analysis - analytes, standard solutions, indicators, titration reactions, etc.. Calculation of titration results. Qualitative relationship between the titration curve and the concept of sudden rise (acid base strength, concentration, and solvent polarity). Quantitative calculation of titration curve is not required. Basic principles of pH calculation and selection of common acid-base titration indicators. Calculated by Potassium Permanganate, potassium dichromate, sodium thiosulfate, EDTA titration analysis results as the standard solution.5. atomic structure the possible space state of an outer nuclear electron. S, P and D are used to indicate the ground state structure (including neutral atoms, positive ions and negative ions) (not requiring the interpretation of the energy level interleaving and distribution); quantum numbers, wave functions, images are not required. General concepts of ionization energy, electron affinity, and electronegativity.The 6. elements of the periodic law and the periodic system changes in general nature of the main group and subgroup, congeners from top to bottom; the concept of S, D, DS, P, f; positions of elements in the periodic table and the nuclearouter electronic structure (electron number, valence electron layer and valence electron number) the relationship between price and family; the highest number; diagonal rule; metal and non metal and the relation between the location of the periodic table. Metal and non metal in the periodic table position; half metal; primary and secondary group (first series) and important names, common elements, symbols and their positions in the periodic table and the main form of common valence.SevenMolecular structures: Lewis, structural (Electronic) and formal charges. Prediction of the three-dimensional structure of simple molecules (including ions) by valence electron pair repulsion model. The theory of hybrid orbitals explains the three-dimensional structure of simple molecules (including ions). Covalent bonds, [p-p, PI bonds, (S-S, S-P, P-P), sigma bonds and P-P large PI bonds] form conditions, bond energies, bond angles, saturation and directionality. The general concept of conjugate (or delocalization).8. complexes: the basic concepts of complexes (complexes) and complex ions (coordination ions). The center of important and common ion complex ions (atoms) and the important and common ions (water, hydroxyl, halogen ions, pseudo halide ions, ammonia molecules, ions, NO, CO etc.), the complexation reaction of complexing agent important and common and important and common. Qualitative description of the relation between complexation and acid base reactions, precipitation reactions, and redox reactions (not required by calculation). Basic concepts of space structure and geometric isomerism ofcomplexes. The basic concepts of the hybridization orbital theory of complexes. Memory magnetic moment calculation formula is not required. The basic concepts of crystal field and ligand field theory are not required.9. intermolecular force. The order of magnitude of the intermolecular interaction energy (does not require decomposition into orientational force, induced force, dispersive force). Hydrogen bond. Conditions for the formation of hydrogen bonds. Hydrogen bond energy. Relationship between hydrogen bond and physical properties.10. crystal structure: the basic concept of cell. Basic concepts of cell atomic coordinates. Calculation of the number of atoms or the number of molecules in a cell and its relation to the chemical formula. Basic concepts of elementary cell and complex cell (body, core, heart, and core). The basic concepts of molecular crystals, atomic crystals, ionic crystals and metallic crystals. Selection of crystal cell, crystal system concept and several typical two element ionic crystals.11. chemical equilibrium: the basic concept of equilibrium constant. Qualitative relationship between acid-base balance constant and acid base strength. The basic concept of solubility product. Simple calculations using equilibrium constants. Calculation of electrical neutrality, material balance, and no requirement for proton conditions.12. correct writing and balancing of ionic equations.13. electrochemistry: the basic concepts of oxidationreduction and the writing and trimming of reactions. Galvanic cell: electrode symbol and electrode reaction, galvanic cell sign, galvanic cell reaction. The basic concept of standard electrode potential is used to determine the direction of reaction and the strength of oxidant and reductant. Battery symbols and electrode reactions in an electrolytic bath. Basic concepts of electrolysis and electroplating. Common chemical power source. Qualitative description of the effects of pH, complexing agents, and precipitation agents (do not require Nernst equations, redox equilibrium constants, and related calculations).14. element chemistry knowledge to international competition level 1 knowledge level. Two or three levels of knowledge do not require memory.15. knowledge of organic chemistry, level 1 in international competition. Two or three levels of knowledge do not require memory.Basic content of finals1. atomic structure increases four quantum numbers and atomic orbital wave function in the preliminary basis (plus the angle distribution image and s, P, D image track name).The 2. increase in the basic concept of molecular structure in the preliminary content based on molecular orbital. Bond level concept. Explanation of the paramagnetic property of oxygen by molecular orbital theory. Memory molecular orbital energy level diagram is not required.3. crystal structures: basic concepts of structural primitives and lattices. The basic concepts of enthalpies of formation, formation free energies and lattices, 14 lattice types, dense deposits (A1, A2, A3 and A4) and a bulk interstitial model.4. fundamentals of chemical thermodynamics -- concepts of thermodynamics, energy, enthalpy, free energy, and entropy. Enthalpies of formation, free energies of formation, standard entropies, and related calculations. Free energy and direction of reaction. Gibbs Helmholtz equation and its application. Fant Huff isothermal equation and its application. Standard free energy and equilibrium constant. A function of the equilibrium constant to temperature. Thermochemical cycle. Thermodynamic decomposition of temperature (both standard and nonstandard States) the effect of pressure on decomposition temperature.5. fundamentals of chemical kinetics -- basic concepts of reaction rates. The concept of reaction series. Using the experimental data to derive the reaction order.Calculation of first-order reactions (integral formula) (rate constants, half-life, carbon, -14, age, etc.). Arrhenius equation and relevant calculation (calculation of the influence of temperature on the reaction rate constant of the concept and calculation; Arrhenius activation energy calculation; rate constants etc.). Relationship between activation energy and reaction heat. General concept of reaction mechanism. Using steady-state approximation to derive rate equations. The nature of the influence of the catalyst on the reaction. The expression for the reaction rate and thecalculation of the integral are not required.6. proton theory of acids and bases. Basic concept of buffer solution. Using the calculation of acid-base equilibrium constant. Solubility product principle and related calculation.Calculation of 7.Nernst equation. The calculation of electrode potential and electromotive force of galvanic cell. The influence of pH value on electromotive force, electrode potential and redox reaction direction of galvanic cell. Influence of precipitant and complexing agent on redox reaction direction.Hybrid orbital theory of chemical bonds of 8. complexes. The hybrid orbital model of the complex ion (plane, quadrilateral, tetrahedral, and eight body configurations). The relation between the magnetic moment of a single electron and the hybridization type. Hybrid orbital and solid structure. Isomerism of complexes (including CIS trans isomerism and optical isomerism). Calculation of equilibrium constants in complexation reactions. General concept of chelates.9. elements of chemical descriptive knowledge reached the international competition outline level one or two.10. natural cycles of nitrogen, oxygen and carbon. The general concept of environmental protection, ecological balance and sustainable development.11. organic chemistry descriptive knowledge, to theinternational competition outline level one or two. Organic synthesis reaches international competition outline one or two level knowledge level. Four spectrum is not required. Asymmetric synthesis is not required. Do not seek racemic resolution. Organic reactions are not required.The basic concept of 12. amino acids and peptides. No Biochemistry (such as the name, symbol, structure, classification of 20 amino acids), base structure, name, pairing, photosynthesis, metabolism, etc. of DNA and RNA.13. IUPAC nomenclature of simple organic compounds (do not require the number of atoms in the memory ring).14. basic concepts of organic stereochemistry. Basic concepts of conformation and conformation. CIS trans isomerism and chiral isomerism (R- and S-).15. the identification and structure inference of simple compounds (without special reagents and reactions) using the basic reactions of inorganic and organic compounds.The basic operation of electronic weighing scales, 16. Organic Preparation and organic synthesis solution, heating, cooling, precipitation, crystallization, recrystallization and filtration (including filtration), washing, evaporation, distillation and reflux, decantation, liquid, mixing and drying. The experimental conditions are controlled by intermediate process detection such as pH, temperature, color, etc.. Calculation of yield and conversion. Knowledge and operation of laboratory safety and emergency emergencyhandling. Waste disposal. Washing and drying of instruments. Arrangement and arrangement of experimental work surface. Record of raw data.17. basic operation of routine capacity analysis, basic reactions and calculation of titration results. Concept of titration curve and protrusion (relation between qualitative and quantitative), plotting titration curve.。