全国高中学生化学竞赛基本要求(Basic requirements of chemistry competition for senior high school stu

全国高中学生化学竞赛基本要求（Basic requirements of chemistry competition for senior high school students in China）April 2007

Explain：

1. the basic requirements to clear the preliminary and final questions of the knowledge level, as the basis of the examination proposition. This basic

Does not involve national team selection requirements.

2. the current middle school chemistry teaching syllabus, the newly issued ordinary high school chemistry curriculum standard (experimental textbook of A1 - 2, B1 - 6) and college entrance examination showed that the provisions of the content are preliminary requirements. The basic content of common sense and high school mathematics, physics, biology, geography and environment science high school education of citizens (including the basic knowledge of the basic situation of our country, the universe, the earth and the related chemical etc.) is the content of chemistry contest. The basic requirements for some chemical principle of the quantitative relationship between material structure, solid chemistry and organic chemistry supplements, generally speaking, supplementary content is the natural growth point of middle school chemistry.

The final round of the 3. basic requirements are based on the basic requirements in the preliminary supplements.

4., the national senior high school students chemistry contest is a research study under the guidance of teachers. It is an extracurricular activity. The total number of hours after the competition is an important constraint on the basic requirements of the competition. The basic requirements of the basic requirements for the 40 preliminary estimation unit (3 per unit hour) extracurricular activities (Note: 40 unit is based on two years of high school for about 40 weeks, every Monday, the computation of the unit); the basic requirements of the final 30 additional units of extracurricular activities (including at least 10 units) (Note: 30 unit in 10, 11 and December, a total of three months for about 14 weeks, every week 2 ~ 3 unit calculation).

5. in the last three years, the same level of competition examination questions related to the requirements of the knowledge, automatically become the next competition requirements.

6. this basic requirement shall be adjusted if necessary and notified three months before the competition. After the new basic requirements are enabled, the basic

Automatic failure required.

The basic requirements for

1. significant figures. Correct use of effective figures in chemical and chemical experiments. Quantitative instrument (balance, cylinder, pipettes, burettes, flask and so on) effective digital measurement data. The reductive rules of

digital operations and the valid digits of the results of operations. The restriction of experimental methods on effective numbers.

2. gas. Standard state of ideal gas. Ideal gas equation of state. Gas constant R. Environmental standard pressure and system standard pressure. Gas density. Law of partial pressure. Determination principle of relative molecular mass of gas. Gas solubility (Henry's law).

3. solution. Solution concentration. Solubility. Unit and conversion of concentration and solubility. Preparation of solution (choice of instrument according to concentration accuracy). Recrystallization method and estimation of solute / solvent relative quantity. Filtration and washing (washing liquid selection, washing method selection). Selection of recrystallization and washing solvents (including mixed solvents). Colloid. Continuous phase of disperse system. Formation and destruction of colloids. Classification of colloids. The basic structure of colloids.

4. capacity analysis. The basic concepts of subject matter, reference substance, standard solution, indicator, titration reaction, etc.. Qualitative relationship between titration curve (acid base strength, concentration and solvent polarity) on titration jump of acid base titration. Selection of indicator for acid base titration. Potassium Permanganate, potassium dichromate, sodium thiosulfate, EDTA titration for standard solution reaction. Calculation of analytical results. The accuracy and precision of the analysis results are presented.

5. atom structure. The state of the motion of electrons outside the nucleus: s, P and D are used to indicate the configuration of the ground state configuration (including neutral, positive and negative ions). Ionization energy, electron affinity and electronegativity.

The periodic law of 6. elements and the periodic system of elements. Cycle. 1 - 18 ethnic groups. Principal and subordinate groups. Transition element. The general law of the nature change of the subordinate elements of the main and subordinate races from top to bottom; the general regularity of the change of the elements from left to right in the same cycle elements. Atomic radius and ionic radius. Basic chemical properties and electronic configurations of atoms in s, P, D, DS, and f- regions. The relation between the position of an element in the periodic table and the structure of an outer electron (the number of electrons, the valence electron layer and the number of valence electrons).

The relation between the highest oxidation state and the family number. Diagonal rule. The relation of metal and nonmetal to the position of periodic table. The position of metals and nonmetals in the periodic table. Half metallic (metalloid). The names and symbols of important and common elements of the main and minor groups, their location in the periodic table, common oxidation states and main forms. The concept of platinum elements.

7. molecular structure. Lewis structure (electronic). Prediction of the geometrical configurations of simple

molecules (including ions) by valence electron pair repulsion models. Hybrid orbital theory for the interpretation of geometries of simple molecules (including ions). Covalent bond. Valence bond (bond, bond). Bond length, bond angle, bond energy. Sigma bond and PI bond. Delocalized pi bond. General concept of conjugate (delocalization). The general concept of an electron body. Polarity of bonds and polarity of molecules. Law of similar dissolution.

8. complexes. Lewis's concept of acid and base. Coordination bond. The important and common complexes are the central ions (atoms) and important and common ligands (water, hydroxyl ions, halide ions, quasi halogen ions, ammonia molecules, acid ions, unsaturated hydrocarbons, etc.). Chelation and chelation effects. Important and common complexing agents and their important and common coordination reactions. The relation between coordination reaction and acid base reaction, precipitation reaction, redox reaction (qualitative description). The basic concepts and basic facts of the geometry and isomerism of complexes. Hybrid orbital theory of complexes. The magnetic properties and stability of the complexes are explained by the theory of hybridization orbitals. The crystal field theory of the eight body complex illustrates the color of Ti (H2O) 63+. The basic concept of acid-base and important soft hard acid and alkali and alkali.

9. intermolecular force. Fan Dehua force. Hydrogen bond. The general concept of intermolecular forces, energy, and the relation to the properties of matter.

10. crystal structure. Crystal cell. Atomic coordinates.

Lattice energy. Calculation of the number of atoms or molecules in a unit cell and its relation to the chemical formula. Molecular crystals, atomic crystals, ionic crystals and metal crystals. Coordination number. Crystal packing and

interstitial model. The common crystal structure types are NaCl, CsCl, CaF2, ZnS, diamond, graphite, selenium, ice, dry ice, urea, Jin Hongshi, perovskite, potassium, magnesium, copper and so on.

11. chemical equilibrium. Equilibrium constant and conversion rate. Ionization constant of weak acid and weak base. Solubility product. Using the calculation of equilibrium constant. The concept of entropy (confusion degree) and its relation with spontaneous reaction direction.

12. correct writing of ionic equations.

13. electrochemistry. Oxidation state. The basic concepts of oxidation reduction and the writing and trimming of reactions. Primary battery。 Electrode symbols, electrode reactions, galvanic cell symbols, galvanic cell reactions. Standard electrode potential. Determine the direction of the reaction and the strength of the oxidant and reductant with the standard electrode potential. Electrode symbols and electrode reactions in an electrolytic bath. Electrolysis and electroplating. Electrochemical corrosion. Common chemical power source. Qualitative description of the influence of pH, complexing agent and precipitant on redox reaction.

14. element chemistry. Halogen, oxygen, sulfur, nitrogen, phosphorus, carbon, silicon, tin, lead, boron and aluminium.

Alkaline earth metals, alkalis, and rare gases. Titanium, vanadium, chromium, manganese, iron, cobalt, nickel, copper, silver, gold, zinc, mercury, molybdenum, tungsten. Transition element oxidation state. Acidity and basicity of oxides and hydroxides. Common insoluble salts. Basic classification and main properties of hydrides. The morphology and basic properties of common inorganic acids and bases. The color, chemical properties, qualitative detection (without the use of special reagents) and general separation methods of common ions in aqueous solutions. General methods for preparing elemental substances.

15. organic chemistry. Organic compounds in the system of basic types - alkanes, alkenes and alkynes, cyclic hydrocarbons, aromatic hydrocarbons, halogenated hydrocarbons, alcohols, phenols, ethers, aldehydes, ketones, acids, esters, amines, amides, nitro compound, sulfonic acid name, basic properties and mutual transformation. Isomerism. C=C addition. Marconi's rule. C=O addition. Substitution reaction. Aromatic hydrocarbon substitution reaction and location rules. Substitution reactions and oxidation reactions of aromatic hydrocarbon side chains. The basic reaction of carbon chain growth and shortening.

Molecular chirality and the determination of R and S configurations of asymmetric carbon atoms. The basic concepts, general formulas and typical materials, basic properties, structural features and structural expressions of sugar, fat and protein are presented.

16. preliminary knowledge of natural polymer and synthetic

polymer chemistry. (monomers, main synthetic reactions, main categories, basic properties and main applications).

Basic requirements for finals

The basic requirements in the preliminary requirements increase the following basis, does not involve calculus.

1. atom structure. The physical meaning and value of four quantum numbers. Calculation of the energy of a single electron atom in hydrogen and hydrogen like atoms. S, P and D atomic orbital images.

2. molecular structure. Basic concepts of molecular orbital. Localized bond key stage. The molecular orbital theory explains the structure and properties of oxygen molecules, nitrogen molecules, carbon monoxide molecules, and nitric oxide molecules. Interpretation of the energy levels of the particle model in one dimensional box for the absorption spectra of conjugated systems. The basic concept of supramolecular.

3. crystal structure. The basic concept of lattice. Crystal system. Macroscopic symmetry elements determine the crystal system. The relation between the crystal system and the shape (lattice system) of a cell. Fourteen types of spatial lattice. Discrimination of the structure of the core (body, heart, heart, core) of a unit cell (lattice). The concept of unit cell. Prague equation.

4. fundamentals of chemical thermodynamics. The concepts of thermodynamic energy (internal energy), enthalpy, heat

capacity, free energy, and entropy. Enthalpies of formation, free energies of formation, standard entropies, and related calculations. The change of free energy of reaction and the direction of reaction. Gibbs Helmholtz equation and its applications. Fant Hoff isothermal equation and its application. Standard free energy and standard equilibrium constant. The relation between equilibrium constant and temperature. Thermochemical cycle. Thermodynamic decomposition of temperature (standard and nonstandard states). Phase, phase rule and single component phase diagram. The Cramer equation and its application (without calculus).

5. dilute solution (not for common chemical potential).

6. fundamentals of chemical kinetics. Basic concept of reaction rate. Rate equation. Reaction order. Using the experimental data to derive the reaction order. First order reaction integrals and related calculations (rate constants, half lives, carbon -14 methods, age, etc.). Arrhenius equation and calculation (activation concept and calculation; the calculation of the rate constant calculation; the effect of temperature on the rate constant etc.). Reaction process diagram. Relationship between activation energy and reaction heat. General concept of reaction mechanism and determination of rate equations (speed step, balance hypothesis and steady state hypothesis). Basic concepts and typical examples of ion reaction mechanism and radical reaction mechanism. The nature of the influence of the catalyst on the reaction (reaction process diagram). The number of reactive molecules and the number of transformations in heterogeneous reactions.

7. proton theory of acids and bases. The basic concept of buffer solution. Preparation of typical buffer system and calculation of pH value. Using the calculation of acid-base equilibrium constant. Solubility product principle and related calculation.

8. Nernst equations and related calculations. Calculation of electromotive force of galvanic cell. The influence of pH on electromotive force, electrode potential and redox reaction direction of galvanic cell. Influence of precipitant and complexing agent on redox reaction direction. The electrode potential and equilibrium constant are calculated by free energy, or vice versa.

9. elementary understanding of the crystal field theory and ligand field theory of complexes. Photochemical sequence. Magnetic properties of complexes. Fission energy, pair energy, and stabilization energy. The calculation of the equilibrium constants of complexes. Complexometric titration. Soft acid base. Preliminary theory of ligand field.

10. elements of chemical descriptive knowledge reached the international competition outline level three.

11. natural cycles of nitrogen, oxygen and carbon. General concepts of environmental pollution and governance, ecological balance and green chemistry.

12. organic chemistry descriptive knowledge, to the international competition outline level three (does not require asymmetric synthesis, do not seek racemic resolution).

13. basic concepts of amino acids, peptides and proteins. DNA and RNA.

14. basic concepts of sugar. Glucose, fructose, mannose, galactose. Glycoside. Cellulose and starch.

15. systematic nomenclature of simple organic compounds.

Sixteen

Basic concepts of organic stereochemistry. Conformation and conformation. CIS trans isomerism (trans-, cis- and Z-, E- configuration). Chiral isomerism. Endo- and exo-. D, L configuration.

17. identification and structure inference of simple compounds using basic reactions of inorganic and organic compounds.

18. basic operations of Organic Preparation and organic synthesis. Electronic balance。 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 (e.g., pH, temperature, color, etc.). Calculation of yield and conversion. Knowledge and operation of laboratory safety and emergency handling. Waste disposal. Instrument washing and drying. Arrangement and arrangement of the experimental work surface. Record of raw data.

19. the basic operation of common capacity analysis, the basic reaction and calculation of analysis results. Error analysis of volumetric analysis.

20. point spectrophotometry. Colorimetric analysis.