Summary of senior high school chemistry knowledge (very comprehensive)
Inorganic part of chemical formula:
Soda soda, soda, natural alkali, oral alkali: Na2CO3.
Baking soda: sodium bicarbonate
Soda: Na2S2O3
Gypsum (raw gypsum): CaSO4.2H2O
Gypsum: 2CaSO4 .H2O
Fluorite: CaF2
Barite: barium sulfate (nontoxic)
Ammonium bicarbonate: NH4HCO3
Limestone and marble: CaCO3
Quicklime: CaO
Hydrated lime and hydrated lime: Ca(OH)2
Salt: sodium chloride
Glauber's salt: Na2SO4 7H2O (laxative)
Caustic soda, caustic soda and caustic soda: NaOH
Chlorite: FaSO4 7H2O
Dry ice: carbon dioxide
Alum: potassium sulfate
Bleaching powder: Ca (ClO)2, CaCl2 (mixture)
Diarrhea salt: magnesium sulfate 7H2O
Bile alum and blue alum: CuSO4 5H2O
Hydrogen peroxide: H2O2
Alumni: Zinc Sulfate 7H2O
Silica, when applicable: silica
Corundum: Al2O3
Sodium silicate, sodium silicate, mineral glue: Na2SiO3.
Iron red and iron ore: Fe2O3
Magnetite: Fe3O4
Pyrite and pyrite: FeS2
Chlorophyll and malachite: Cu2(OH)2CO3
Siderite: FeCO3
Chalcopyrite: Cu2O
Bordeaux mixture: calcium hydroxide and copper sulfate
Sulfur mixture: calcium hydroxide and sulfur.
Main components of glass: sodium siloxane, siloxane and silica.
Calcium superphosphate (main components): Ca (H2PO4)2 and CaSO4.
Calcium superphosphate (main component): Ca (H2PO4)2
Natural gas, biogas and biogas (main components): CH4.
Water gas: carbon monoxide and H2
Ammonium ferrous sulfate (light blue-green): Fe (NH4)2(SO4)2 turns light green after being dissolved in water.
Photochemical smog: NO2 is a toxic gas produced by light.
Aqua regia: concentrated nitric acid and concentrated hydrochloric acid are mixed according to the volume ratio of 1: 3.
Thermite: Al+Fe2O3 or other oxides.
Urea: carbon dioxide
Organic part:
Chloroform: chloroform
Calcium carbide: CaC2
Carbide gas: C2H2 (acetylene)
TNT: trinitrotoluene
Alcohol, ethanol: C2H5OH
HCFCs: It is a good refrigerant and toxic, but it will destroy the ozone layer.
Acetic acid: glacial acetic acid, vinegar CH3COOH.
Cracking gas components (petroleum cracking): olefins, alkanes, alkynes, H2S, CO2, CO, etc.
Glycerol, glycerol: C3H8O3
Composition of coke oven gas (coal dry distillation): H2, CH4, ethylene, CO, etc.
Carbonic acid: phenol
Formaldehyde: formaldehyde formaldehyde
Formalin: 35%-40% formaldehyde aqueous solution.
Formic acid: formic acid HCOOH
Glucose: C6H 12O6
Fructose: C6H 12O6
Sucrose: C 12H22O 1 1.
Maltose: C 12H22O 1 1.
Starch: (C6H 10O5)n
Stearic acid: C 17H35COOH
Oleic acid: C 17H33COOH
Palmitic acid: C 15H3 1COOH.
Oxalic acid: HOOC—COOH oxalate discolors blue ink, which is strongly acidic and decomposes into CO2 and water when heated, thus discoloring KMnO4 acidic solution.
chemical phenomenon
1. The reaction between aluminum flake and hydrochloric acid is exothermic, while the reaction between Ba(OH)2 and NH4Cl is endothermic.
2. Sodium reacts with H2O (with phenolphthalein), melts, floats on the water surface, rotates and releases gas (melts, floats, swims, hisses and is red).
3. Flame reaction: Na yellow, K purple (through blue cobalt glass), Cu green, Ca brick red, Na+ (yellow), K+ (purple).
4. Copper wire burns in chlorine to produce brown smoke.
5. The combustion of 5.H2 in Cl2 is a pale flame.
6. The combustion of 6.Na in Cl _ 2 produces a lot of white smoke.
7. The combustion of P in Cl _ 2 produces a lot of white smoke.
8. Introduce SO2 into magenta solution to fade first, and then restore the original color after heating.
9, NH3 and HCl meet to produce a lot of white smoke.
10, aluminum foil burns violently in oxygen to produce dazzling white light.
1 1. Magnesium bars produce dazzling white light when burned in air, and white powder (MgO) and black smoke when burned in carbon dioxide.
12, iron wire burns in Cl2, producing brown smoke.
13, HF corrodes glass: 4HF+SiO2 =SiF4+2H2O.
14 and Fe(OH)2 are oxidized in the air: from white to grayish green, and finally to reddish brown.
15. At room temperature: iron and aluminum are passivated in concentrated H2SO4 and concentrated HNO3.
16, dropping FeCl3 solution into a test tube containing phenol solution, and the solution is purple; Phenol turns pink when exposed to air.
17, protein will turn yellow when it encounters strong HNO3, and it will smell like burnt feathers when it burns.
18, burning in air:
A faint light blue flame
H2- light blue flame
H2S- light blue flame
Cobalt blue flame
CH4- bright blue flame.
S burns in O2- bright blue-purple flame.
19. Characteristic reaction phenomenon:
20. Pale yellow solid: sulfur or Na2O2 or AgBr.
2 1. Gases that change the color of magenta solution: SO2 (red after heating) and Cl2 (red after heating).
22. Colored solution:
Fe2+ (light green)
Fe3+ (yellow)
Cu2+ (blue)
MnO4- (purple)
Colored solids:
Red (copper, cuprous oxide, iron oxide)
Reddish brown [iron hydroxide]
Black (CuO, FeO, FeS, CuS, Ag2S, PbS)
Blue [copper hydroxide]
Yellow (AgI, Ag3PO4)
White [Fe(0H)2, CaCO3, BaSO4, AgCl, BaSO3]
Colored gas:
Cl2 (yellow-green)
NO2 (reddish brown)
Some special properties of elements
1. Elements in special positions in the periodic table
Elements of (1) group whose ordinal number is equal to the number of periods: H, Be, al and Ge.
② Elements with group ordinal number equal to twice the period number: C and S. ..
(3) Elements with groups equal to three times the number of periods: O.
(4) Elements whose period is twice the number of families: Li and Ca.
⑤ Elements whose period number is three times that of the family: Na and Ba.
⑥ Short-period element whose algebraic sum of the highest positive price and the lowest negative price is zero: C.
⑦ A short-period element whose highest positive price is three times the absolute value of the lowest negative price: S.
8 the element with the smallest atomic radius except h: f.
The element with the largest ion radius in a short period: P.
2. Characteristics of common elements and their compounds
① The element that forms the most kinds of compounds, the simple substance is the hardest substance in nature or the element with the largest mass fraction of hydrogen in gaseous hydride: C.
② The most abundant element in the air or the element whose gaseous hydride aqueous solution is alkaline: N.
③ The most abundant element in the earth's crust, the element with the highest boiling point of gaseous hydride or the element with hydride in liquid state under normal conditions: O.
④ Lightest element: H; The lightest element of metal: Li.
⑤ Non-metallic element whose simple substance is liquid at room temperature: br; Metal element: mercury.
⑥ The highest valence oxides and their corresponding hydrates can react with both strong acids and strong bases: Be, Al and Zn.
⑦ The gaseous hydride of this element and its highest valence oxide can react with the corresponding hydrate: n; Element capable of redox reaction: S.
⑧ The gaseous hydride of this element can react with its oxide at room temperature to generate a simple element: S.
⑨ Short-period elements that can react with water at room temperature to release gas: Li, Na and F.
⑩ Common elements that can form allotropes: C, P, O, S.
General rules of chemistry examination
1, solubility law-see solubility table;
2, on the inert electrode, the discharge order of various ions:
Cathode (ability to extract electrons): Au3+>; ag+& gt； Hg2+>； Cu2+>； Pb2+>； fa2+& gt； Zn2+>； h+& gt； Al3+>； Mg2+>； na+& gt； Ca2+>； K+
Anode (ability to lose electrons): S2->; I-> br–& gt； cl->； Oh-> Oxyacid radical
Note: If metal is used as anode, the anode itself will undergo redox reaction during electrolysis (except pt and Au).
3, double hydrolysis ionic equation's writing:
(1) Write hydrolyzed ions on the left and hydrolyzed products on the right;
(2) Balance: first balance the charge on the left, and then balance other atoms on the right;
(3) If H and O are uneven, add water there.
Example: when Na2CO3 is mixed with AlCl3 solution: 3co32-+2al3++3H2O = 2al (OH) 3↓+3co2 ↑.
4, write the electrolytic total reaction equation method:
(1) Analysis: What are the reactants and products;
(2) balance.
5. Divide the chemical reaction equation into two electrode reactions:
(1) Write two and a half reactions according to electron gain and loss;
(2) Considering the reaction environment (acidic or alkaline);
(3) Make the number of atoms and charges on both sides equal.
Example: The reaction in the battery is: Pb+PbO2+ 2H2SO4 = 2PbSO4+2H2O. Try to write the electrode reaction when it is used as a primary battery (discharge).
Write two and a half reactions: Pb -2e- → PbSO4.
PbO2+2e- → PbSO4
Analysis: In acidic environment, filling other atoms should be:
Negative electrode: Pb+SO42-2e- = PbSO4
Positive electrode: PBO 2+4h+SO4 2-+2e-= pbso4+2h2o.
Note: When charging, it is electrolysis, and the electrode reaction is the reverse reaction of the above electrode reaction:
Cathode: PbSO4+2e-= Pb+SO42-
Anode: pbso4+2h2o-2e-= PBO2+4h+so42-
6. Identities commonly used in solving calculation problems: atomic identities, ionic identities, electronic identities, charge identities, electric identities, etc. The methods used are: mass conservation method, difference method, normalization method, limit method, relationship method and crossover method.
And estimation method.
(Non-redox reaction: atomic conservation, charge balance and material balance are much used, while redox reaction: electron conservation is much used)
7. For ions with the same electron shell structure, the more nuclear charges, the smaller the ion radius;
8. Melting point of crystal: atomic crystal >; Ionic crystals > atomic crystals What we have learned in molecular crystals are: Si, SiC, SiO _ 2 = and diamond.
The comparison of melting points of atomic crystals is based on atomic radius: diamond >; SiC & gtSi (because atomic radius: Si >；; C & gto)。
9. Melting point and boiling point of molecular crystals: The higher the molecular weight, the higher the melting point and boiling point of substances with similar composition and structure.
10. Colloidal electrification: Generally speaking, colloidal particles of metal hydroxide and metal oxide are positively charged, while colloidal particles of non-metal oxide and metal sulfide are negatively charged.
1 1, oxidizability: MnO 4->; Cl2 & gtBr2 & gtFe3+>； I2 & gtS=4(+4 valence S)
For example: I2+SO2+H2O = H2SO4+ 2HI
12. The solution containing Fe3+ is usually acidic.
13. Substances that can form hydrogen bonds: H2O, NH3, HF, CH3CH2OH.
14, and the density of ammonia (like ethanol solution) is less than 1. The higher the concentration, the smaller the density. The density of sulfuric acid is greater than 1. The density of 98% concentrated sulfuric acid is 1.84g/cm3.
15, whether there are ions in * * *:
(1) Whether precipitation or gas release occurs;
(2) Whether there is weak electrolyte;
(3) Whether redox reaction occurs;
(4) Whether complex ions [Fe(SCN)2, Fe(SCN)3, Ag(NH3)+, [Cu (NH3) 4] 2+] are generated;
(5) Whether double hydrolysis occurs.
16, in the crust:
The most abundant metal element is aluminum.
The nonmetallic element with the most content is-o.
HClO4 (perchloric acid)-is the strongest acid.
17 The metal with the lowest melting point is Hg (-38.9C). ),;
The highest melting point is W (W 3410C);
The lowest density (normal) is k;
The highest density (common) is Pt.
18, when the PH value of rainwater is less than 5.6, it becomes acid rain.
19. Acidity of organic acids: oxalic acid >: formic acid >; Benzoic acid > acetic acid > carbonic acid > phenol >; Bicarbonate-
20, organic matter identification, pay attention to the use of water and bromine water these two substances. Example: Identification: Ethyl acetate (insoluble in water, floating), bromobenzene (insoluble in water, sinking) and acetaldehyde (miscible with water) can be used.
2 1. substitution reactions include halogenation, nitration, sulfonation, halogenated hydrocarbon hydrolysis, ester hydrolysis, esterification and so on.
22, the simplest type of the same kind of organic matter, no matter in what proportion, as long as the total mass of the mixture is certain, the amount of CO2, H2O and O2 produced by complete combustion remains unchanged. The amount of CO2, H2O and O2 consumed when the mass of a single component remains unchanged.
23. There are several kinds of substances that can make bromine water fade, but the reasons for fading are different: unsaturated hydrocarbons such as olefins and alkynes (addition fading), phenol (substitution fading), ethanol, aldehyde, formic acid, oxalic acid, glucose (oxidation fading), organic solvents [CCl4, chloroform, bromobenzene, CS2 (density greater than water), hydrocarbons, benzene, benzene.
24. Aldehydes, formic acid, formate, ammonium formate (HCNH2O), grape samarium, fructose and maltose can all react with silver mirror. (It can also react with Cu(OH)2)
The relationship in the calculation is generally: —CHO—2Ag.
Note: When the silver ammonia solution is sufficient, the oxidation of formaldehyde is special: HCHO-4ag↓+H2CO3.
The reaction formula is: hcho+4 [ag (NH3) 2] oh = (NH4) 2co3+4ag6h3 ↑+2h2o.
25, colloidal aggregation method:
(1) Add electrolyte;
(2) adding colloid with opposite electrical properties;
(3) heating.
Common colloids: liquid sol: Fe(OH)3, AgI, milk, soybean milk, porridge, etc. Aerosol: fog, clouds, smoke, etc. Solid sol: colored glass, smoke crystal, etc.
26. Gases that pollute the atmosphere: SO2, CO, NO2 and NO, in which SO2 and NO2 form acid rain.
27. Environmental pollution: air pollution, water pollution, soil pollution, food pollution, solid waste pollution and noise pollution. Industrial three wastes: waste residue, waste water and waste gas.
28. At room temperature (20C. ) when the solubility is above 10g-soluble; /kloc-above 0/g-soluble; Less than1g-slightly soluble; Less than 0.0 1 g-insoluble.
29. The water content in human body accounts for about 2/3 of human body mass. The total surface fresh water is less than 1% of the total water. The three major fossil fuels in the world today are coal, oil and natural gas. Petroleum mainly contains C and H elements. ..
30. The carbon content of pig iron is 2%-4.3%, and that of steel is 0.03%-2%. Raw salt: NaCl contains MgCl2 and.
CaCl2, because MgCl2 absorbs water, the original salt is easy to deliquesce. Concentrated nitric acid forms a white mist in the air. Solid NaOH easily absorbs water in the air to form a solution.
3 1, gas solubility: at a certain pressure and temperature, the volume of gas in 1 volume of water reaches saturation.
Common important oxidants and reductants
1. redox reaction
Deoxyoxygen is raised to reduce Deoxyoxygen (oxidant/reductant, oxidation product/reduction product, oxidation reaction/reduction reaction).
Oxidation: oxidant >; oxidation products
Reducibility: reducing agent >; Reduced sediment
The oxidant and reductant are organic compounds containing S, SO32-, HSO3-, H2SO4-3, SO2, NO2-, Fe2+ and -CHO.
2. Salt hydrolysis
Salts are hydrolyzed and water is weakly decomposed; Hydrolyzes only when it is weak, and does not hydrolyze without weakness; The weaker the hydrolysis, the weaker the double hydrolysis; Whoever is strong is human, and the same power is neutral.
Conservation relation in electrolyte solution;
Charge conservation: the number of positive charges of all cations in electrolyte solution is equal to the number of negative charges of all anions. For example, in NaHCO3 solution: n (Na+)+n (H+) = n (HCO3-)+2n (CO32-)+n (OH-): [Na+]+[H+] = [HCO3-]+2 [CO32-]+[OH-]
Conservation of materials: due to ionization or hydrolysis, ions in electrolyte solution will become other ions or molecules, but the total number of atoms of a specific element in ions or molecules will not change. For example, in the solution of nahco3: n (na+): n (c) =1:1,c (na+) = c (hco3-)+c (co32-)+c (h2co3) is deduced.
Proton conservation: The amount of substances that molecules or ions gain or lose protons (H+) in electrolyte solution should be equal. For example, in NH4HCO3 solution, H3O+ and H2CO3 are the products after obtaining protons; NH3, OH- and CO32- are products after losing protons, so they have the following relationship: C (H3o+)+C (H2CO3) = C (NH3)+C (OH-)+C (CO32-).
Ion * * * has a problem.
Whether ions can exist in a large number in the solution involves comprehensive knowledge such as the properties of ions and the acidity and alkalinity of the solution. Anything that will significantly change the concentration of related ions in the solution due to the reaction cannot be stored in large quantities. If insoluble and hard-to-ionize gaseous substances are formed or can be converted into other kinds of ions (including redox reactions), the following aspects can generally be considered:
1. Weak base cations only exist in strongly acidic solutions, such as Fe3+, Al3+, Zn2+, Cu2+, NH4+, Ag+, etc. And OH- cannot exist in large quantities.
2. Weak acid anion only exists in alkaline solution. For example:
CH3COO-, F-, CO32-, SO32-, S2-, PO43- and AlO2- cannot exist in large quantities with H+.
3. The acid anion of weak acid can't exist in large quantities in strong acid or strong alkaline solution. When they encounter strong acid (H+), they will generate weak acid molecules; When it meets strong alkali (OH-), it generates normal salt and water.
Such as: HSO3-, HCO3-, HS-, H2PO4-, HPO42-, etc.
4. If anions and cations can combine with each other to form insoluble or slightly soluble salts, they cannot be stored in large quantities.
For example: Ba2+, Ca2+ and CO32-, SO32-, PO43-, SO42- and so on. Ag+ and Cl-, Br-, I-, etc. Ca2+ and F-, C2O42- etc.
5. If the anion and cation have double hydrolysis reaction, they can't be stored in large quantities. For example, Fe3+ such as Al3+ and HCO3-, CO32-, HS-, S2-, AlO2-, ClO-, SiO2-and Fe3+ such as HCO3-, CO32-, AlO2-, ClO-, SiO2-,C6H5O-; NH4+ and AlO2-, SiO32-, ClO-, CO32- and so on.
6. If anions and cations can undergo redox reaction, they cannot be stored in large quantities. Such as: Fe3+ and I-, S2-; MnO4-(H+) and I-, Br-, Cl-, S2-, SO32-, Fe2+, etc. NO3-(H+) and the above anions. S2-、SO32-、H+
7. Due to complexation reaction or other reactions, such as Fe3+ and F-, CN-, SCN-, etc., a large amount of * * * cannot be stored. H2PO4- and PO43- will generate HPO42-, so they do not exist.
10 storage and access of special reagents
1. Sodium and potassium: isolated from air; Anti-oxidation, stored in kerosene (or liquid paraffin), (plum sealed with paraffin). Take it off with tweezers, cut the glass slide, suck the kerosene with filter paper, and then put the rest in the kerosene.
2. White phosphorus: stored in water, protected from oxidation and light. Take tweezers, immediately put them into water, cut them open with a long-handled knife, and suck up the water with filter paper.
3. Liquid Br2: toxic, volatile, put in a ground-mouth flask and sealed with water. The bottle cap is tight.
4.I2: It is easy to sublimate and has a strong pungent smell. It should be kept in a bottle sealed with wax and kept at low temperature.
5. Concentrated HNO3 _ 3 and AgNO3 _ 3: They are easy to decompose when exposed to light, and should be stored in a brown bottle at low temperature and protected from light.
6. Solid alkali: it is easy to deliquesce and should be stored in a dry flask that is easy to seal. The bottle mouth is plugged with a rubber stopper or covered with a plastic cover.
7. NH3 H2O: volatile and should be sealed at low temperature.
8.C6H6, C6H5-CH3, CH3CH2OH, CH3CH2OCH2CH3: volatile, flammable, sealed at low temperature, away from fire sources.
9.Fe2+ salt solution, H2SO4 33 and its salt solution, hydrogen sulfate and its salt solution: It is not suitable for long-term storage because it is easy to be oxidized by air, so it should be prepared now.
10. Salt water, lime water, silver ammonia solution, copper hydroxide suspension, etc. You should take it with you, not leave it for a long time.
Expanding reading: the learning method of chemistry in senior high school
First, understand double bases and master chemical terms.
The so-called "double basis" refers to the basic concepts and theories of chemistry, which is an important part of the basic knowledge of chemistry and the basis for learning chemistry well. They are generally expressed in concise and clear words, which are scientific, rigorous and logical. When learning, don't just memorize, be good at grasping key words and phrases and understanding them accurately. For example, the key words of the catalyst concept are "variable", "before and after the reaction", "quality and chemical properties" and "unchanged"; The law of conservation of mass focuses on understanding "participation in reaction", "total mass" and "equality" and grasping "three conservation" (elements, atoms and mass). We should not only correctly understand double bases, but also use them. The so-called "chemical terms" refer to some chemical terms commonly used in the process of communication, description and expression of material changes in chemical science, such as element symbols, chemical formulas, chemical equations and so on. , to master, flexible use.
Second, according to the structure, understand the material properties.
The object of chemical research is matter. The composition and structure of matter determine the nature of matter, which restricts the way of existence, preparation and use of matter. Therefore, when studying the properties of elemental compounds, we should master their structures to understand the properties of substances. For example, when learning oxygen, we must think that oxygen is composed of many oxygen molecules, and one oxygen molecule is composed of two oxygen atoms. There are six electrons in the outermost layer of oxygen atom, which is easy to obtain, so the chemical properties of oxygen are more active. Many substances can change chemically with oxygen at room temperature, and when ignited or heated, a lot of heat will be released. After learning a lot of materials, we should be good at building related materials into a knowledge network, so that knowledge can be organized and grasped firmly.