The basic concept of chemistry review materials: 1, chemical change: changes that produce other substances; 2. Physical changes: no changes in other substances; 3. Physical properties: properties (such as color, state, density, smell, melting point, boiling point, hardness, water solubility, etc. ) displayed without chemical changes; 4, chemical properties: the properties of substances in chemical changes (such as. Combustion-supporting, oxidizing, reducing, acid-base and stability, etc. 5. pure substance: composed of one substance; 6. Mixture: composed of two or more pure substances, all of which maintain their original properties; 7. Element: the general name of a kind of atoms with the same nuclear charge (i.e. proton number); 8. Atom: the smallest particle in chemical change, which can't be divided into 9. In chemical changes, it can be further divided into 10, simple substance: pure substance composed of the same element 1 1, compound: pure substance composed of different elements 12, and oxide: compound composed of two elements. One of the elements is oxygen element 13, and the chemical formula is 14, and the relative atomic mass:112 is the standard. The value obtained by comparing the mass of other atoms with it is the relative atomic mass of an atom = relative atomic mass ≈ proton number+neutron number (because the mass of atoms is mainly concentrated in the nucleus) 15, relative molecular mass: the sum of the relative atomic masses of atoms in the chemical formula 16, ion: charged atom or atomic group 17, and atomic structure:. Nuclear charge = number of protons ≠ number of electrons outside the nucleus 18, four basic types of chemical reactions: ① combination reaction: the reaction in which two or more substances generate a substance, such as A+B = AB ② decomposition reaction: the reaction in which one substance generates two or more other substances, such as AB = A+B ③ displacement reaction: the reaction in which simple materials reacts with a compound. Reactions to form another simple substance and another compound, such as: A+BC = AC+B4 double decomposition reaction: reactions to form another two compounds by exchanging components between the two compounds, such as AB+CD = AD+CB 19, reduction reaction: reactions in which the oxygen of oxygen-containing compounds is taken away (non-chemical basic reaction type) oxidation reaction: chemical reactions between substances and oxygen (non-chemical basic reaction type) Slow oxidation: an oxidation reaction that is very slow or even difficult to detect spontaneously: spontaneous combustion caused by slow oxidation 22 catalyst: can change the chemical reaction rate of other substances in chemical changes. Substances whose mass and chemistry have not changed before and after chemical change (note: 2h2o 2 = = 2h2o+O2 = MnO2 is the catalyst of this reaction) are 2 1, and the law of conservation of mass: the total mass of substances participating in chemical reaction is equal to the total mass of substances generated after the reaction. Before and after the reaction, the number, species and quality of atoms remain unchanged; The type of the element remains the same) 22. Solution: One or more substances are dispersed into another substance to form a uniform and stable mixture. Composition of solution: solvent and solute. (Solute can be solid, liquid or gas; When solids and gases are dissolved in liquids, they are solutes and liquids are solvents. When two liquids are mutually soluble, the solvent is one with more quantity and the solute is one with less quantity; When there is water in the solution, no matter how much water there is, we are used to using water as a solvent and others as solutes. ) 23, solid solubility: at a certain temperature, the mass of a solid substance dissolved when it reaches saturation in100g solvent is called the solubility of the substance in the solvent. 24, acid: a compound in which all cations generated during ionization are hydrogen ions. For example, HCl = = h++Cl-HNO3 = = h++NO3-H2SO4 = = 2h++SO4-base: Compounds in which all anions generated during ionization are hydroxide ions, such as KOH = = k++OH-NaOH = = Na++OH-. 2 = = Ba2 ++ 2OH- salt: compounds that generate metal ions and acid ions when ionized, such as: Kno3 = = k++NO3-Na2SO4 = = 2na++SO4-bacl2 = = Ba2++2cl-25, acid oxides (nonmetallic oxides): basic oxides that can react with alkali to generate salts and water (belonging to metal oxides) Crystal water: substances containing crystal water (such as Na2CO3. 10H2O, CuSO4). 5H2O) 27。 Thawing: the phenomenon that a substance can absorb moisture in the air and become moist is weathered: crystal hydrate is in dry air at room temperature. The phenomenon that crystal water can be gradually lost and turned into powder. 28. Combustion: A strong oxidation reaction that produces light and heat between combustible substances and oxygen. Combustion conditions: ① combustible substances; ② Oxygen (or air); (3) The temperature of combustible materials should reach the ignition point. Basic knowledge and theory: 1. Composition of air: nitrogen 78%, oxygen 2 1%, rare gas 0.94%, carbon dioxide 0.03%. Other gases and impurities account for 0.03%. 2. Main air pollutants: NO2, CO, SO2, H2S, NO, etc. 3. Chemical formulas of other common gases: NH3 (ammonia), CO (carbon monoxide), CO2 (carbon dioxide), CH4 (methane), SO2 (sulfur dioxide), SO3 (sulfur trioxide) and NO (nitric oxide). Hydrogen chloride. Common acids or ions: HSO4-2- (sulfate), NO3- (nitrate), HCO3-(carbonate), ClO3- (chlorate), MnO4- (permanganate), MnO42- (manganate), PO43- (phosphate) and Cl. H2PO4- (dihydrogen phosphate), OH- (hydroxide), HS- (sulfhydryl), S2- (sulfur ion), NH4+ (ammonium ion or ammonium ion), K+ (potassium ion), Ca2+ (calcium ion), Na+ (sodium ion), Mg2+ (magnesium ion) and so on. The valence of each element or atomic group of Ag+ (silver ion) and Ba2+ (barium ion) corresponds to the charge number of the above ions: textbook P80 univalent potassium, sodium, hydrogen and silver, bivalent calcium, magnesium, barium and zinc; One, two, copper, mercury, iron, trivalent aluminum and tetravalent silicon. (oxygen -2, chlorine in chloride is-1, fluorine-1, bromine is-1) (in simple substance, the valence of elements is 0; In the compound, the algebraic sum of the valence of each element is 0) 5. Chemical formula and valence: (1) Meaning of chemical formula: ① Macro meaning: a. Represents a substance; B, indicate the elemental composition of the substance; ② Microscopic significance: a. Molecules representing matter; B, indicating the molecular composition of the substance; ③ Meaning of quantity: a. Represents the number ratio of atoms in a substance molecule; B. indicates the mass ratio of the elements that make up the substance. (2) Reading and writing of chemical formula of simple substance ① Directly expressed by element symbols: a. Metal simple substance. Such as: potassium, potassium, copper, copper, silver, silver and so on. ; B. solid nonmetal. Such as: carbon, carbon, sulfur, phosphorus and other C rare gases. Such as: helium (gas) helium neon (gas) neon argon (gas) argon, etc. 2 polyatomic simple substance: if the molecule is composed of several atoms of the same kind, write a few in the lower right corner of the element symbol. For example, if each oxygen molecule consists of two oxygen atoms, the chemical formula of oxygen is O2 diatomic molecule simple chemical formula: O2 (oxygen), N2 (nitrogen), H2 (hydrogen), F2 (fluorine gas), Cl2 (chlorine gas), Br2 (liquid bromine) polyatomic molecule simple chemical formula: ozone O3, etc. (3) Read and write the chemical formula of the compound. After writing, read ① the compound composed of two elements: read "a chemical element", such as MgO (magnesium oxide) and NaCl (sodium chloride); read "an acid element", such as KMnO4 (potassium permanganate), K2MnO4 (potassium permanganate), MgSO4 (magnesium sulfate) and CaCO3 (calcium carbonate). (2) the step of writing chemical formula according to the valence of elements: a. writing element symbols and marking the valence according to the valence of elements; B. See if the valence of an element is a divisor and turn it into the simplest ratio; C. Cross-switch, and write the valence that has been reduced to the simplest ratio in the lower right corner of the element symbol. 6. Teaching material P73. Remember these 27 elements, symbols and names. Extranuclear electron configuration: element 1-20 (remember the name of the element and the schematic diagram of the atomic structure): ① The maximum number of electrons per layer is 2n2 (n stands for the number of layers); ② The number of electrons in the outermost layer shall not exceed 8 (the number of electrons in the outermost layer shall not exceed 2 in the first layer); ③ Fill the inner layer first, and then discharge the outer layer. Note: the chemical properties of elements depend on the number of electrons in the outermost layer 7. The solution is alkaline. (2) 2) The closer the pH value is to 0, the stronger the acidity is; The closer the PH value is to 14, the stronger the alkalinity is. The closer the PH value is to 7, the weaker the acidity and alkalinity of the solution is, and the closer it is to neutrality. 9. Metal activity sequence table: (potassium, calcium, sodium, magnesium, aluminum, zinc, iron, tin, lead, hydrogen, copper, mercury, silver, platinum, gold) Description: (1) The more metal remains, the stronger the metal activity, and the metal on the left can be replaced from the salt solution of the metal on the right (2). The one to the right of hydrogen can't. (3) Potassium, calcium and sodium are relatively active, and directly react with water in the solution to replace hydrogen 10, the structure of the substance: 1 1, the meaning and writing of the chemical symbol: (1) The meaning of the chemical symbol: a. Element symbol: ① represents an element; ② Represents an atom of an element. B. chemical formula: point 5 of this knowledge point, point (1) C. ion symbol: indicating the number of charges carried by ions and ions. D. Valence symbol: indicates the valence of an element or an atomic group. When there is a number in front of the symbol (valence symbol has no number), the meaning of the constituent symbol only indicates the number of particles. (2) Writing of chemical symbols: A. Representation of atoms: B. Representation of molecules: C. Representation of ions: D. Representation of valence: Note: When the number of atoms, molecules and ions is greater than "1", it can only be added before the symbol, but not elsewhere. 12, the relationship between atoms, molecules, ions, elements and substances (pure substances and mixtures): 13, 14, commonly used generating devices and collecting devices for gas preparation: generating devices, collecting devices [solid (+solid)] [solid+liquid] Simple devices [solid] Drainage method, upward ventilation method, downward ventilation method 15, laboratory preparation methods of three gases and their differences: gaseous oxygen (O2), hydrogen (H2), carbon dioxide (CO2), medicinal potassium permanganate (KMnO4) or hydrogen peroxide (H2O2), manganese dioxide (MnO 2)[ solid (+solid)] or Zinc particles (Zn) and hydrochloric acid (HCl) or dilute sulfuric acid (h2so 4)[ solid+liquid] limestone (marble) (CaCO3) and dilute hydrochloric acid (HCl)[ solid+liquid]. Reaction principle 2kmno4 = = k2mno4+MnO2+O2 = = 2h2o+O2 = Zn+H2SO4 = ZnSO4+H2 = Zn+2hcl = ZnCl2+H2 = CaCO3+2hcl = CaCl2+H2O+CO2 = Instrument P36 Figure 2-65438+ 08. 04 a) or P 1 1 1. Figure 6- 10( 14 b or c) p11. Fig. 6- 10 (Otherwise, it is not oxygen that ignites the batten into the bottle, the flame on the batten goes out, and the flame at the bottle mouth is light blue. Then the gas is hydrogen, and clear lime water is introduced to see if it becomes turbid. If it is turbid, it is CO2. Collection method ① Drainage method (insoluble in water) ② Upward discharge of air from the bottle mouth (density greater than air) ① Drainage method (insoluble in water) ② Downward discharge of air from the bottle mouth (density greater than air) ① Upward discharge of air from the bottle mouth (density greater than air) (drainage method cannot collect) Check the fullness (purity) with a wooden strip with Mars and put it flat on the mouth of the gas container. If the wood is rekindled, the oxygen will be full. 1 & gt； Block the test tube mouth filled with hydrogen with your thumb; & lt2> Get close to the flame, remove your thumb and light it. If there is a "poof", it means that hydrogen is pure; If there is a sharp popping sound, it means that the hydrogen is impure. Put a burning wooden stick flat on the mouth of the gas container. If the flame goes out, it is full; Otherwise, if it's not full, put it upside down, upside down. Precautions ① Check the air tightness of the device (the following items should be noted when using the first drug) ② The mouth of the test tube should be slightly inclined downward (to prevent the small water droplets condensed on the mouth of the test tube from flowing back to the bottom of the test tube and breaking the test tube) ③ When heating, the test tube should be heated evenly first, and then heated in the drug part. (4) After collecting oxygen by drainage method, first withdraw the catheter and alcohol lamp (to prevent the water in the sink from flowing backwards and breaking the test tube) (1) Check the air tightness of the device (2) The nozzle of the long-necked funnel should be inserted under the liquid surface; (3) Before igniting hydrogen, be sure to check the purity of hydrogen (in air, the volume of hydrogen reaches 4%-74.2% of the total volume, and it will explode when ignited. ① Check the air tightness of the device ② The nozzle of the long-necked funnel should be inserted under the liquid surface; ③ No drainage method can be used to collect 16, the properties (physical and chemical properties), physical properties (under normal circumstances) and chemical properties of some important common gases. Oxygen (O2) is a colorless and odorless gas, which is insoluble in water and has a slightly higher density than air. ①C+O2==CO2 (emitting white light and releasing heat) 1, used for breathing. 2. Steelmaking. 3.②S+O2 ==SO2 (light blue flame in the air; In oxygen-violet blue flame) ③4P+5O2 == 2P2O5 (white smoke and white solid P2O5) 43fe+2O3 = = Fe3O4 (burning violently, sparking everywhere, releasing a lot of heat and producing black solid) ⑤ The candle burns in oxygen, emitting white light and hot hydrogen (H2), which is colorless and odorless and insoluble in water. ① Flammability: 2h2+O2 = = 2h2oh2+Cl2 = = 2hcl1,gas filling, spacecraft (density less than air) 2, ammonia synthesis, hydrochloric acid production 3, gas welding and gas cutting (flammability) 4, refining metal (reducibility). ② Reducibility: H2+CuO = = Cu+H2O3H2+WO3 = = W+3H2O3H2+Fe2O3 = = 2Fe+3H2O Carbon dioxide (CO2) is a colorless and odorless gas with a density greater than that of air. Solid carbon dioxide is called "dry ice". CO2+H2O ==H2CO3 (acidic) (H2CO3 = = H2O+CO2 ↑) (unstable) 1, used for fire extinguishing (using its incombustibility, 2. CO2+Ca(OH) 2 ==CaCO3↓+H2O (CO2 identification) CO2+2 NaOH = = Na2CO3+H2O oxidation: CO2+C = = 2coCaCO3 = = Cao+CO2 = (industrial CO2) Carbon monoxide (CO) is a colorless and odorless gas. Toxic gas ① Flammability: 2CO+O2 == 2CO2 (the flame is blue and gives off a lot of heat, so it can be used as gas fuel) 1, which is used as fuel 2. Smelting metal ② Reducibility: Co+CuO = = Cu+Co2co+WO3 = = w+3co2co+Fe2O3 = = 2fe+3co2 (and blood red in blood) Destroy the ability of blood to transport oxygen) Problem solving skills and instructions: 1. Reasoning problem solving skills: Color of common substances: Most gases are colorless, most solid compounds are white, and most solutions are colorless. 2. Color of some special substances: black: MnO2, CuO, Fe3O4, C, FeS (ferrous sulfide) blue: CuSO4? 5H2O, Cu(OH)2, CuCO3, solution containing Cu2+, liquid solid O2 (light blue) red: Cu (bright red), Fe2O3 (reddish brown), red phosphorus (dark red) yellow: sulfur (element S), Fe3+ (brownish yellow) green: FeSO4? 7H2O, Fe2+-containing solution (light green), basic copper carbonate [Cu2(OH)2CO3] COlorless gas: N2, CO2, Co, O2, H2, CH4 Colored gas: Cl2 (yellow-green), NO2 (reddish-brown) irritant gas: NH3 (this gas can turn wet pH test paper blue), SO2 has the smell of rotten eggs. Judgments of common changes: ① white precipitate, insoluble in dilute nitric acid or acid: BaSO4 and AgCl (just these two substances); ② Blue precipitate: Cu(OH)2, CuCO3 ③ Red-brown precipitate: Fe(OH)3 Fe(OH)2 is a white flocculent precipitate, but it quickly turns into gray-green precipitate in the air. Then it becomes a reddish-brown precipitate of Fe(OH)3. ④ The precipitate can be dissolved in acid, releasing gas (CO2): insoluble carbonate. ⑤ The precipitate can be dissolved in acid without releasing gas: insoluble alkali. 4. Relationship between acid and corresponding acid oxide: ① Both acid oxide and acid can react with alkali to form salt and water: CO2+2NaOH = = Na2CO3+H2O (H2CO3+2NaOH = = Na2CO3+2H2O). SO2+2 KOH = = K2SO3+H2SO4 3+2 KOH = = K2SO3+2H2SO4+2NaOH = = Na2SO4+H2SO4+2NaOH = = Na2SO4+2H2O② Acid oxides react with water to generate corresponding acids: (valence of each element remains unchanged) CO2+H2O =. Relationship between alkali and corresponding alkaline oxides: ① Both alkaline oxides and alkali can react with acid to form salt and water: CuO+2HCl == CuCl2+H2O Cu(OH). 2+2HCl = = CuCl2+2H2ocao+2HCl = = CaCl2+H2oca (OH) 2+2HCl = = CaCl2+2H2O② Alkali metal oxides react with water to generate corresponding alkali: (The generated alkali must be soluble in water, otherwise, This reaction can't happen) K2O+H2O = = 2 KOH Na2O+H2O = = 2 NaOH Bao+H2O = = Ba (OH) 2 Cao+H2O = = Ca (OH) 2 ③ Insoluble alkali will decompose corresponding oxides and water when heated: Mg (OH) 2 = = MgO+H2O2 = = CuO+H2O2 Fe (OH Solution experiment: see clearly what the demand is, what to do and what the purpose is. (1) The gas used in the experiment is relatively pure, and the specific methods for removing common impurities are as follows: ① In addition to water vapor, concentrated acid, CaCl2 _ 2 solid, soda lime, anhydrous CuSO4 _ 4 (and whether there is water vapor in the impurities, the color changes from white to blue), quicklime, etc. ② CO2 removal is available: clarified limewater (which can detect whether there is CO2 in impurities), NaOH solution, KOH solution, alkali lime, etc. ③ In addition to HCl, there are AgNO3 solution (which can detect whether there is HCl in impurities), limewater, NaOH solution, KOH solution, etc. The principle of removing gas impurities: a substance absorbs or reacts with impurities, but does not absorb or react with effective components. (2) Precautions in the experiment: ① Explosion-proof: Before igniting combustible gases (such as H2, CO and CH4) or reducing CuO and Fe2O3 with CO and H2, the gas purity should be checked. ② Explosion-proof boiling: When diluting concentrated sulfuric acid, pour concentrated sulfuric acid into water instead of pouring water into concentrated sulfuric acid. (3) Poisoning prevention: experiments on the properties of toxic gases (such as CO, SO2 and NO2) should be carried out in a ventilated kitchen; And pay attention to the treatment of tail gas: CO is ignited and burned; SO2 and NO2 are absorbed by alkaline solution. ④ backflow prevention: gas is prepared by heating method and collected by drainage method. Pay attention to the order of turning off the lights. (3) Treatment of common accidents: ① Acid flows to the countertop and is washed with NaHCO3; Alkali flows to the table and is washed with dilute acetic acid. (2) Touching the skin or clothes: (1) Wash the acid with water first, and then wash it with 3-5% NaHCO3; Ii, washing alkali with water, and then coating boric acid; Ⅲ. Clean the concentrated sulfuric acid with a rag, and then do the first step. (4) Common impurities to be removed in the three main gases prepared in the laboratory:1; Impurities to be removed when preparing O2: water vapor (H2O) 2; Impurities to be removed when preparing H2 with hydrochloric acid and zinc particles: water vapor (H2O), hydrogen chloride gas (HCl, acid mist of hydrochloric acid) (this impurity is not removed with dilute sulfuric acid) 3. Impurities to be removed in carbon dioxide production: water vapor (H2O) and hydrogen chloride gas (HCl). Agents for removing water vapor: concentrated acid, CaCl2 solid, alkali lime (mainly composed of NaOH and CaO), quicklime, anhydrous CuSO4 (and can check whether there is water vapor in impurities, and the color changes from white to blue) and other agents for removing HCl gas: AgNO3 _ 3 solution (and can check whether there is HCl in impurities), clarified limewater, NaOH solution (or solid), KOH solution (or solid) [ Experimental methods are commonly used to verify that the mixed gas contains a certain gas 1. Verification method of CO: (first verify whether there is CO2 in the mixed gas, and then remove it) Introduce the mixed gas into hot CuO, and then introduce the mixed gas after hot CuO into clarified lime water. Phenomenon: Black CuO turns red, and clarified limewater becomes turbid. 2. Verification method of 2.H2: (first verify whether there is water in the mixed gas, and then remove it) Introduce the mixed gas into hot CuO, and then introduce the mixed gas after hot CuO into anhydrous CuSO4. Phenomenon: black CuO turns red and anhydrous CuSO4 turns blue. 3. Verification method of 3.CO2: Introduce the mixed gas into the clarified limewater. Phenomenon: Clear limewater becomes turbid. (6), self-designed experiment 1, try to design an experiment to prove that candles contain hydrocarbons of two elements. Experimental steps Experimental phenomena Conclusion ① Light the candle, cover a dry and clean beaker above the flame, and the inner wall of the beaker produces small water droplets, which proves that the candle has hydrogen; (2) Cover a beaker soaked in clarified limewater above the candle flame, and the clarified limewater becomes turbid, which proves that the candle has carbon; 2. Try to design an experiment to prove that CO2 does not support combustion, and its density is higher than that of air. Experimental Steps Experimental Phenomena Conclusion Figure Put two candles on a stepped shelf, put this shelf in a beaker (as shown in the figure), light the candles, and then pour CO2 along the wall of the beaker. The candle at the bottom of the ladder goes out first, and the candle at the top goes out later. It has been proved that CO2 does not support combustion, and its density is higher than air. 3. Solving calculation problems: The types of calculation problems are: ① Calculation of mass fraction (elements and solutes); ② Calculation according to chemical equation; ③ Mix ① and ② for calculation; (1) Calculation of solute mass fraction in solution = ╳ 100% (2), calculation of element mass fraction in compound (pure substance) = ╳ 100% (3), calculation of compound mass fraction in mixture = ╳/ Calculation of the mass fraction of an element in a mixture: the mass fraction of an element = ╳ 100% or: the mass fraction of an element = the mass fraction of a compound ╳ the mass fraction of the element in a compound (5), problem-solving skills 1, examination: Look at the requirements of the topic clearly, what do you know and what do you want? Find out the relevant formula to solve this problem. 2. According to the calculation of chemical equation, the steps to solve the problem are as follows: ① setting an unknown number; ② Write the correct chemical equation; ③ Write down the relative molecular mass, known quantity and unknown quantity of relevant substances; ④ List the proportional formula and solve the answer. 0 | Comments ask TA for help Respondents: Bing Meng 1 Rui | Three-level pass rate: 50% Good at areas: entertainment, leisure education/scientific research help to participate in activities: activities that have not been participated for the time being.