Description:

1. This basic requirement aims to clarify the knowledge level of the national preliminary and final examination questions as the basis for the proposition of the examination questions. This basic requirement does not involve the selection of national team players.

2. The contents stipulated in the current middle school chemistry syllabus, the newly published standard experimental textbooks for ordinary high school chemistry courses (A 1-2, B 1-6) and the college entrance examination instructions are all preliminary requirements. Common sense of citizens with high school education and basic contents of mathematics, physics, biology, geography and environmental science in high school (including basic knowledge of China's national conditions, universe and earth related to chemistry, etc.). ) is also the content of the chemistry competition. The preliminary competition basically requires adding some chemical principles in quantitative relationship, material structure, stereochemistry and organic chemistry. Generally speaking, supplementary content is the natural growth point of middle school chemistry content.

3. The basic requirement of the final is to make an appropriate supplement on the basis of the basic requirements of the preliminary competition.

4. The national senior high school chemistry competition is a research study under the guidance of teachers and an extracurricular activity. The total class hours of extracurricular activities is an important restrictive factor in formulating the basic requirements of competitions. This basic requirement estimates that the preliminary round needs 40 units of extracurricular activities (3 hours per unit) (note: 40 units are calculated according to 40 weeks for senior one and senior two, one unit per week); At the end of the term, it is basically required to have 30 extracurricular activities (including at least 10 units of experiments) (note: 30 units are calculated according to 10,1,65438+February * * * for three months, about 14 weeks per week.

5. The test questions of the competition at the same level in the last three years involve knowledge that meets the requirements and automatically become the requirements of the next competition.

6. If it is necessary to adjust these basic requirements, notice should be given three months before the competition. After the new basic requirements are enabled, the original basic requirements will automatically become invalid.

Preliminaries:

1. A considerable number. Correct use of significant figures in chemical calculation and chemical experiment. Effective figures of measurement data of quantitative instruments (balance, measuring cylinder, pipette, burette, volumetric flask, etc.). ). The effective number of the operation result.

2. gas. Ideal gas standard state. Equation of state of ideal gas. Gas density. Law of partial pressure. Determination principle of relative molecular mass of gas. Gas solubility (Henry's law).

3. Solutions. Solution concentration. Solubility. Solution preparation (choose instruments according to the accuracy of concentration). Recrystallization and estimation of relative amount of solute/solvent. Filtering and washing (washing liquid selection, washing method selection). Solvents (including mixed solvents). Colloid.

4. Capacity analysis. Basic concepts such as measured substance, reference substance, standard solution, indicator and titration reaction. Titration curve of acid-base titration (qualitative relationship between the influence of acid-base strength, concentration and solvent polarity on titration jump). Selection of acid-base titration indicator. Alkaline titration reaction with potassium permanganate, potassium dichromate, sodium thiosulfate and EDTA as standard solutions. Calculation of analysis results. Accuracy and precision of analysis results.

5. Atomic structure. Motion state of extranuclear electrons: S, P and D are used to represent the extranuclear electron configurations of ground state configurations (including neutral atoms, positive ions and negative ions). Ionization energy, electron affinity, electronegativity.

6. Periodic law of elements and periodic system of elements. Main clan and auxiliary clan. Transition element. The general law of the change of the properties of the same family elements of the main and auxiliary families from top to bottom; The general law of the property change of the same periodic element from left to right. Atomic radius and ionic radius. Basic chemical properties of elements in S, P, D, ds and F regions and electron configuration of atoms. The relationship between the position of elements in the periodic table and the electronic structure outside the nucleus (number of electron layers, number of valence electrons, number of valence electrons). The relationship between the highest oxidation state and the number of families. Diagonal rule. Relationship between metallicity, nonmetal and position of periodic table of elements. The position of metals and nonmetals in the periodic table. The name, symbol, position in the periodic table, common oxidation states and main forms of important and common elements in the main group and sub-group of semimetals. The concept of platinum group elements.

7. Molecular structure. Lewis structural formula (electronic). Prediction of geometric configuration of simple molecules (including ions) by valence shell electron pair repulsion theory. Using hybrid orbital theory to explain the geometric configuration of simple molecules (including ions). * * * Price key. Bond length, bond angle, bond energy. σ bond and π bond. Delocalized π bond. * * * General concept of yoke (delocalization). General concept of isoelectronic body. Polarity of molecules. Law of similarity compatibility.

8. complicated. The concept of Lewis acid base. Coordination key center ions (atoms) of important common complexes and important common ligands (water, hydroxide ions, halide ions, pseudohalide ions, ammonia molecules, acid ions, unsaturated hydrocarbons, etc.). ). Chelates and their chelating effects. Important and common complexing agents and their important and common coordination reactions. The relationship between coordination reaction and acid-base reaction, precipitation reaction and redox reaction (qualitative explanation). Basic concepts of geometric configuration and isomerization of complexes. Hybrid orbital theory of complex. Crystal field theory of octahedral complexes. The color of titanium (H2O)63+.

9. Intermolecular forces. Other general concepts of van der Waals force hydrogen bonding intermolecular force.

10. Crystal structure. Cell atomic coordinates. Lattice energy. Calculation of atomic number or molecular number in cells and its relationship with chemical formula. Molecular crystals, atomic crystals, ionic crystals and metal crystals. Stacking and gap model of coordination crystal. Common crystal structure types, such as NaCl, CsCl, sphalerite (ZnS), fluorite (CaF2), diamond, graphite, selenium, ice, dry ice, urea, rutile, perovskite, potassium, magnesium, copper, etc.

1 1. chemical equilibrium. Equilibrium constant and conversion rate. Ionization constants of weak acids and bases. Solubility product. Using the calculation of equilibrium constant. The concept of entropy.

12. ionic equation's correct writing.

13. oxidation state. The basic concept of redox and the writing and balance of reaction. Electrode symbol of galvanic cell, electrode reaction, galvanic cell symbol, galvanic cell reaction. Standard electrode potential. Judging the reaction direction and the strength of oxidant and reductant by standard electrode potential. The electrode symbol of electrolytic cell reacts with the electrode. Electrolysis and electroplating. Electrochemical corrosion. General chemical power supply. Qualitative explanation of the influence of pH, complexing agent and precipitant on redox reaction.

Elemental chemistry Halogen, oxygen, sulfur, nitrogen, phosphorus, carbon, silicon, tin, lead, boron and aluminum. Alkaline earth metal, alkali metal, rare gas. Titanium, vanadium, chromium, manganese, iron, cobalt, nickel, copper, silver, gold, zinc, mercury, molybdenum and tungsten. Oxidation states of transition elements. Acidity, alkalinity and amphoteric of oxides and hydroxides. Common insoluble salts. Basic classification and main properties of hydrides. Morphology and basic properties of common inorganic acids and bases. Color, chemical properties, qualitative detection (without using special reagents) and separation of common ions in aqueous solution. General method for preparing simple substance.

Organic chemistry. The basic types of organic compounds-alkanes, alkenes, alkynes, cyclic hydrocarbons, aromatics, halogenated hydrocarbons, alcohols, phenols, ethers, aldehydes, ketones, acids, esters, amines, amides, nitro compounds and sulfonic acids-are systematically named, their basic properties and their mutual transformation. Heterogeneous phenomenon. C=C addition. Marconi's law. C=O addition. Substitution reaction. Aromatic substitution reaction and positioning rules. Substitution and oxidation of aromatic side chains. Basic reactions of carbon chain growth and shortening. Chirality of molecules and judgment of R and S configurations of asymmetric carbon atoms. Sugar, fat, protein.

16. Preliminary knowledge of the chemistry of natural polymers and synthetic polymers.

Final:

This basic requirement adds the following contents on the basis of the preliminary requirements, and does not involve calculus.

1. Atomic structure. The physical meaning and value of four quantum numbers. Calculation of orbital energy of single electron atom. Orbital images of sulfur, phosphorus and d atoms.

2. Molecular structure. Basic concepts of molecular orbitals. The key level of the localization key. Molecular orbital theory explains the structure and properties of oxygen molecules, nitrogen molecules, carbon monoxide molecules and nitric oxide molecules. Energy levels of particles in a one-dimensional box. Basic concepts of supramolecules.

3. Crystal structure. The basic concept of lattice. Crystal system. Macro symmetry element. Fourteen kinds of space lattice.

4. Fundamentals of chemical thermodynamics. Concepts of thermodynamic energy (internal energy), enthalpy, heat capacity, free energy and entropy. Enthalpy of formation, free energy of formation, standard entropy and related calculations. The change of free energy and the directionality of reaction. Gibbs-Helmholtz equation and its application. Van tehoff isothermal equation and its application. Standard free energy and standard equilibrium constant. Relationship between equilibrium constant and temperature. Thermochemical cycle. Thermodynamic decomposition temperature (standard configuration and non-standard configuration). Phase, phase law and phase diagram. Clara-Buron equation and its application (without calculus).

5. universality of dilute solution (chemical potential is not needed).

6. Fundamentals of chemical kinetics. The basic concept of reaction rate. Reaction series. Inferring reaction order from experimental data. First-order reaction integral formula and related calculations (rate constant, half-life, carbon-14 dating, etc.). Arrhenius formula and its calculation (concept and calculation of activation energy; Calculation of rate constant; Calculation of the influence of temperature on rate constant, etc. ). Relationship between activation energy and reaction heat. General concept of reaction mechanism. Derive the rate equation. The essence of the influence of catalyst on the reaction.

7. Acid-base proton theory. Buffer solution. Using the calculation of acid-base equilibrium constant. Principle of solubility product and related calculation.

8. Nernst equation and related calculations. Calculation of electromotive force of primary battery. Effect of pH on electromotive force, electrode potential and redox reaction direction of primary battery. Influence of precipitant and complexing agent on the direction of redox reaction.

9. Preliminary understanding of coordination field theory of complexes. Complex magnetism. Split energy and stable energy. Using the calculation of equilibrium constant of complex. Complexometric titration of soft and hard acids and bases.

10. The descriptive knowledge of elemental chemistry has reached the third level of the international competition outline.

1 1. The cycle of nitrogen, oxygen and carbon in nature. General concepts of environmental pollution and control, ecological balance and green chemistry.

12. The descriptive knowledge of organic chemistry has reached the third level of the international competition outline (asymmetric synthesis and racemic resolution are not required).

13. Basic concepts of amino acids, peptides and protein. DNA and RNA.

The basic concept of sugar. Glucose, fructose, mannose, galactose. Glycosides. Cellulose and starch.

15. Systematic nomenclature of simple organic compounds.

16. Basic concepts of organic stereochemistry. Configuration and conformation. Cis-trans isomerism (trans, cis and Z, E configurations). Chiral isomerization. Inner type and outer shape. D, l configuration.

17. Identification and structure inference of simple compounds through basic inorganic and organic reactions.

18. Basic operations of organic preparation and synthesis. Electronic balance. Preparing solution, heating, cooling, precipitating, crystallizing, recrystallizing, filtering (including suction filtration), washing, evaporation concentration, atmospheric distillation and reflux, decanting, liquid separation, stirring and drying. Experimental conditions are controlled by intermediate process detection (such as pH, temperature and color). Calculation of yield and conversion rate. Knowledge and operation of laboratory safety and accident emergency treatment. Waste disposal. Instrument cleaning and drying. Layout and arrangement of experimental working face. Records of raw data.

19. Basic operations, basic reactions and calculation of analysis results of common capability analysis. Error analysis of capacity analysis.

20. Spectrophotometry. colorimetric analysis