1. Effective Numbers Correct use of effective numbers in chemical calculation and chemical experiments. Effective figures of measurement data of quantitative instruments (balance, measuring cylinder, pipette, burette, volumetric flask, etc.). ). Reduction rules of numerical operation and significant figures of operation results. Limitation of experimental methods on significant figures.
2. Ideal gas standard state of gas. Equation of state of ideal gas. Gas constant R. System standard pressure. Law of partial pressure. Determination principle of relative molecular mass of gas. Gas solubility (Henry's law).
3. Solution concentration. Solubility. Unit and conversion of concentration and solubility. Solution preparation (instrument selection). Recrystallization method and estimation of relative amount of solute/solvent. Filtering and washing (washing liquid selection, washing method selection). Selection of recrystallization and washing solvents (including mixed solvents). Colloid. Dispersed phase and continuous phase. Formation and destruction of colloid. Classification of colloids. Basic structure of colloidal particles.
4. Basic concepts of volumetric analysis, such as measured object, reference substance, standard solution, indicator and titration reaction. Acid-base titration curve (qualitative relationship between acid-base strength, concentration and solvent polarity during 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. The motion states of extranuclear electrons in atomic structure: S, P, D, etc. Are used to represent the extranuclear electron configuration of the ground state configuration (including neutral atoms, positive ions and negative ions). Ionization energy, electron affinity, electronegativity.
6. Periodic law of elements and periodic system of elements. 1~ 18 family. 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. The position of metals and nonmetals in the periodic table. Semi-metal (metalloid). Names, symbols, positions in the periodic table, common oxidation states and main forms of important and common elements of the main and auxiliary groups. The concept of platinum group elements.
7. Molecular structure Lewis structural formula. Valence 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 properties of yoke (delocalized) systems. General concept of isoelectronic body. Polarity of bonds and polarity of molecules. Law of similarity compatibility. Symmetry basis (finite rotation and rotation axis, reflection and mirror image, inversion and symmetry center).
8. Lewis acid-base complex. Coordination key center ions (atoms) of important common complexes and important common ligands (water, hydroxide ions, halide ions, pseudohalide ions, ammonia, acid ions, unsaturated hydrocarbons, etc.). ). Chelates and their chelating effects. Important and common coordination reactions. The relationship between coordination reaction and acid-base reaction, precipitation reaction and redox reaction (qualitative explanation). Basic concepts and facts of geometric configuration and isomerization of complexes. Hybrid orbital theory of complex. The magnetism and stability of the complexes are explained by hybrid orbital theory. The color of Ti(H2O)63+ is explained by the crystal field theory of octahedral complex. Basic concepts of soft and hard acids and bases and important soft acids, soft bases and hard bases.
9. The energy of intermolecular forces such as van der Waals force and hydrogen bond and their relationship with the properties of matter.
10. Crystal structure: molecular crystal, atomic crystal, ionic crystal and metal crystal. Cell (definition, cell parameters and atomic coordinates) and cell-based calculation. Lattice energy. Stacking and gap model of coordination crystal. Common crystal structure types: NaCl, CsCl, sphalerite (ZnS), fluorite (CaF2), diamond, graphite, selenium, ice, dry ice, rutile, silica, 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 initial concept of entropy and its relationship with the direction of spontaneous reaction.
12. ionic equation's correct writing.
13. Electrochemical oxidation. The basic concept of redox and the writing and balancing of reaction formula. 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. Explain the effects of pH, complexing agent and precipitant on redox reaction.
14. elemental chemistry halogen, oxygen, sulfur, nitrogen, phosphorus, carbon, silicon, tin, lead, boron and aluminum. Alkali metals, alkaline earth metals, rare gases. 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 substances. Basic classification and main properties of hydrides. Basic properties of common inorganic acids and bases. Color, chemical properties, qualitative detection (without special reagents) and general separation methods of common ions in aqueous solution. General method for preparing simple substance.
15. Nomenclature, basic properties and mutual transformation of basic types of organic compounds-alkanes, alkenes, alkynes, cyclic hydrocarbons, aromatic hydrocarbons, halogenated hydrocarbons, alcohols, phenols, ethers, aldehydes, ketones, acids, esters, amines, amides, nitro compounds and sulfonic acids. Heterogeneous phenomenon. Addition reaction. Marconi's law. Substitution reaction. Aromatic ring 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. The basic concepts, general formulas and typical substances, basic properties, structural characteristics and structural expressions of sugar, fat and protein.
16. Preliminary chemical knowledge of natural polymers and synthetic polymers (monomers, main synthetic reactions, main categories, basic properties and main applications).
The latest basic requirements of the national chemistry competition for senior high school students (08.4. 19) Basic requirements at the end of the term.
This basic requirement adds the following contents on the basis of the preliminary requirements, and the mathematical tools do not involve calculus.
The physical meaning and value of 1. atomic structure quadquantum number. Calculation of atomic orbital energy of hydrogen atom and hydrogen-like ion. Orbital profiles of sulfur, phosphorus and d atoms and their applications.
2. Basic concepts of molecular structure and molecular orbit. The key level of the localization key. Understand molecular orbital theory and apply it to the structure and properties of oxygen molecules, nitrogen molecules, carbon monoxide molecules and nitric oxide molecules. Explanation of electron absorption spectrum of yoke system by one-dimensional particle model in box. Basic concepts of supramolecules.
3. The basic concept of crystal structure lattice. Crystal system. Determine the crystal system according to the macroscopic symmetry element. Relationship between crystal system and cell shape. Fourteen kinds of space lattice. Discrimination of lattice structure with center (body center, face center and bottom center). Bragg equation of intrinsic unit cell.
4. Basic thermodynamic energy (internal energy), enthalpy, heat capacity, free energy and entropy of chemical thermodynamics. Enthalpy of formation, free energy of formation, standard entropy and related calculations. The change of reaction 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. Phase, phase law and single component phase diagram. Kra-Buron equation and its application.
5. Versatility of dilution solution (no chemical potential is needed).
6. Basic concepts of chemical kinetics and reaction rate. Rate equation. Reaction series. Calculation of reaction order with experimental data. The 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. ). Reaction process diagram. Relationship between activation energy and reaction heat. The general concept of reaction mechanism and the derivation of rate equation (speed control step, equilibrium hypothesis and steady-state hypothesis). Basic concepts and typical examples of ion reaction mechanism and free radical reaction mechanism. Catalyst and its influence on the reaction (reaction progress diagram). Number of molecules and number of transformations in heterogeneous reactions.
7. Basic concept of acid-base proton theory buffer solution, preparation of typical buffer system and calculation of pH value. 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. Calculate electrode potential and equilibrium constant by free energy, and vice versa.
9. Crystal field theoretical chemical spectral sequence of the complex. Complex magnetism. Splitting energy, electron pairing energy, stability energy. Using the calculation of equilibrium constant of complex. Complexometric titration of soft and hard acids and bases. Interpretation of octahedral complexes by coordination field theory.
10. The descriptive knowledge of elemental chemistry has reached the second 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 second 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. Basic concepts of organic stereochemistry. Configuration and conformation. Cis-trans isomerism (trans, cis and Z, E configurations). Enantiomers and diastereomers. Inner type and outer shape. D, l configuration.
16. Identification and structure inference of simple compounds by using basic reactions of organic compounds.
17. The basic operation of preparation and synthesis is weighed by electronic balance. Preparing solution, heating, cooling, precipitating, crystallizing, recrystallizing, filtering (including suction filtration), washing, concentrating and evaporating, distilling and refluxing at atmospheric pressure, decanting, separating liquid, 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 placement of experimental bench. Recording and processing of raw data.
18. Basic operations, basic reactions and calculation of analysis results of common capability analysis. Error analysis of capacity analysis.
19. Spectrophotometry. colorimetric analysis