Overview of chemical organics 1. Physical properties methane: colorless, odorless, insoluble ethylene: colorless, slightly odorless, insoluble acetylene: colorless, odorless, slightly soluble (calcium carbide formation: containing H2S and a particularly unpleasant smell of PH3) benzene: colorless, odorless, insoluble in liquid, toxic ethanol: colorless, odorless, miscible, volatile acetic acid: colorless, irritating, soluble. Laboratory preparation method ①: methane: CH3COONa+NaOH →(CaO, heating )→ CH4 ↑+Na2CO3 Note: anhydrous sodium acetate: alkaline lime = 1: 3 solid-solid heating (the same as O2 and NH3) anhydrous (NaAc crystal is not allowed) CaO: water absorption, NaOH dilution, Not catalyst ②: ethylene: C2H5OH →170 )→ CH2 = CH2 = ↑+H2O Note: V ethanol: V concentrated sulfuric acid = 65438 Use soda lime to remove SO2 and CO2, and break ceramic tiles to prevent boiling ③: acetylene: CaC2+2H2O → C2H2 =+Ca (OH). 2 Note: Drainage and collection without impurities can not saturate NaCl with Kipp generator: reduce the reaction rate, put cotton at the catheter mouth: prevent slightly soluble Ca(OH)2 foam from blocking the catheter ④: ethanol: CH2=CH2+H2O → (catalyst, heating, pressurizing )→→→ CH3C2OH (I don't know if this is an industrial laboratory). . . Note: anhydrous CuSO4 test water (white → blue) to increase the concentration: add CaO, and then heat and distill. 3. Combustion phenomenon: alkanes: the flame is light blue and not bright. Olefin: Bright flame with black smoke. Acetylene: bright flame with strong black smoke (pure oxygen: oxyacetylene flame above 3000℃). Benzene: The flame is bright and there is a lot of black smoke. Alcohol: The flame is light blue and gives off a lot of heat. 4. Brominated alkanes: all-colorfast alkynes: all-colorfast (the former is oxidized and the latter is added) Benzene: KMnO4 colorfast extraction discolors bromine water V. Important reaction equation ①: alkanes: substituted CH4+Cl2 → (illumination) → CH3Cl(g)+HCl CH3Cl+Cl2 → (illumination) → CH2Cl2 (L). → CHCl3(l)+HCl CHCl3+Cl2 → (illumination) → CCl4(l)+HCl phenomenon: there is oily liquid on the device wall. Note: among the four products, only chloroform is gaseous chloroform = chloroform carbon tetrachloride as fire extinguishing agent ②: olefin: 1, addition CH2 = CH2+br2 → CH2 brch2 = CH2+HCl → (catalyst) → CH3CH2OH Cl2 = CH2+H2 → (catalyst, heating) → CH3CH3 ethane CH2 = CH2+H2O. . ④: benzene: 1. 1, instead of (bromine) ▽+Br2→(Fe or febr 3)→▽-Br+HBr Note: V benzene: V bromine = 4: 1 long duct: condensation reflux gas guide to prevent NaOH reflux for impurity removal. CCl4: brown water-insoluble liquid (bromobenzene) 1.2, substitution-nitration (nitric acid) ◎+HNO3 → (concentrated H2SO4, 60℃)→◎-NO2+H2O Note: first add concentrated nitric acid, then add concentrated sulfuric acid to cool to room temperature, and then add benzene. 50℃-60℃ water bath thermometer is inserted into a beaker to react under the liquid surface to remove mixed acids: NaOH nitrobenzene: colorless oily liquid, insoluble bitter almond poison 1.3, substitution-sulfonation (concentrated sulfuric acid) ◎+H2SO4 (concentrated) → (70- addition ◎+3H2 →(Ni, Heating) →→ (cyclohexane) →: alcohol: 1, substituted (active metal) 2ch 3 ch 2 oh+2Na→2ch 3 ch 2 ona+H2↓ eliminated (intramolecular dehydration) c2h5oh →170℃) → CH2 = CH2 ↑+H2O2, substituted (H2O) 140℃) → ch3ch2ch2ch3 (ether) +H2O (ether: colorless, nontoxic and volatile liquid anesthetic) 4. Catalytic oxidation of 2CH3CH2OH+O2 →(Cu heating )→ 2ch3cho (acetaldehyde) +2H2O phenomenon: the surface of copper wire turns black and red after being immersed in ethanol. This liquid has a special pungent smell. 6. Acid: Substitute (esterify) CH3COOH+C2H5OH → (concentrated H2SO4, heated) → CH3COOC2H5+H2O (ethyl acetate: odorless oily liquid, Note: acid dehydrogenated hydroxyl alcohol (isotope tracing method) broken porcelain: prevent concentrated sulfuric acid from boiling: Na2CO3 catalyzed dehydration and saturated water absorption: halogenated hydrocarbon is easy to separate and purify: 1, naoH aqueous solution replaces (hydrolyzes) CH3CH2X+NaOH →(H2O, heating) → CH3CH2OH+NaX Note: NaO eliminates NaOH alcoholic solution CH3CH2Cl+NaOH → Dehydrogenation in alcohol solution containing less H (Markov Law): inhibition of hydrolysis (inhibition of NaOH ionization) VI. Alkane CnH2n+2 alkane CnH2n olefin/cycloalkane CnH2n-2 alkyne/diene CnH2n-6 benzene and its homologue CnH2n+2O monoalcohol/alkyl ether CnH2nO saturated monoaldehyde/ketone CnH2n-6O aromatic alcohol/phenol CnH2nO2 carboxylic acid/ester VII. Other knowledge points 1. Tiangan name: methyl, propyl, pentyl, heptyl, octyl and non-decyl 2. Combustion formula: CxHy+(x+y/4)O2 → (ignition) → xc2+y/2h2o cxhyoz+(x+y/4-z/2) O2 → (ignition) → xco2+y/2h2o3, with constant pressure/volume before and after the reaction: y = 4 and decreased: y. Oxygen consumption: the amount of equal substances (equal to V): The more C, the more oxygen consumption. Equal mass: The higher C%, the less oxygen consumption. 5. Unsaturation = (number of C atoms × 2+2–number of H atoms) /2 Double bond/ring = 1, triple bond = 2. You can add 6. Industrial olefin production: cracking (non-cracking) 7. Medical alcohol: 75% industrial alcohol: 95% (methanol is toxic) anhydrous alcohol: 99% 8. Glycerol: Glycerol 9. Acetic acid is between HCl and H2CO3. Vinegar: 3%~5% glacial acetic acid: pure acetic acid 10. Alkyl is not a functional group. Summary 1, sulfate ion: bacl2+Na2SO4 = baso4 ↓+2nac2, carbonate ion: CaCl2+Na2CO3 = CaCO3 ↓+2nac3, reaction of sodium carbonate with hydrochloric acid: Na2CO3+2hcl = 2ncl+H2O+CO2 ↑ 4, reduction of copper oxide with charcoal: 2cuo+C. The reaction of 2Cu+CO2↑ 5 with copper sulfate solution at high temperature: Fe+cuso 4 = feso 4+ sodium peroxide with water: 2Na2O2+2H2O = 4NaOH+O2↑ 9, sodium peroxide with carbon dioxide: 2na2CO3+O2 10, and sodium with water: 2na+2h2o = 2n. Reaction of iron with steam: 3fe+4h2o (g) = f3o4+4h2 =12; Reaction of aluminum with sodium hydroxide solution: 2al+2nNaOH+2h2o = 2nalo2+3. Reaction of calcium oxide with water: CaO+H2O = Ca(OH)2 14, reaction of iron oxide with hydrochloric acid: Fe2O3+6HCl = 2fecl3+3H2O15, reaction of alumina with hydrochloric acid: Al2O3+6HCl = 2AlCl3+3H2O16. Reaction of ferric chloride with sodium hydroxide solution: FeCl 3+3 NaOH = Fe (OH) 3 ↓+3 NaCl18; The reaction between ferrous sulfate and sodium hydroxide solution: FeSO4+2NaOH = Fe(OH). 2↓+ Na2SO4 19, ferrous hydroxide oxidized to ferric hydroxide: 4Fe(OH)2+2H2O+O2 = 4Fe(OH)3 20, ferric hydroxide decomposed by heating: 2Fe(OH)3 △ Fe2O3+3H2O↑ 2 1, aluminum hydroxide prepared in laboratory: Al2. H2O = 2Al(OH)3←+3(NH3)2so 4 22, the reaction between aluminum hydroxide and hydrochloric acid: Al(OH)3+3HCl = AlCl3+3H2O 23, the reaction between aluminum hydroxide and sodium hydroxide solution: Al (OH) 3+NaOH = NaO2+2H2O24, and the thermal decomposition of aluminum hydroxide:. 3 △ Al2O3+3H2O 25, the reaction between ferric chloride solution and iron powder: 2FeCl3+Fe = 3FeCl2 26, and the introduction of ferrous chloride into chlorine gas: 2FeCl2+Cl2 = 2FeCl3 27. Silicon dioxide reacts with hydrofluoric acid: SiO2+4HF = SiF4+2H2O silicon reacts with hydrofluoric acid: Si+4HF = SiF4+2H2↑ 28; SiO2 reacts with calcium oxide at high temperature: SiO2+CaO at high temperature: CaSiO3 29; SiO2 reacts with sodium hydroxide solution: SiO2+2noh = Na2SiO3+H2O 30; Introducing carbon dioxide into sodium silicate solution: Na2SiO3+CO2+H2O = Na2CO3+H2SiO3 ↓ 31; Sodium silicate reacts with hydrochloric acid: Na2SiO3+2HCl = 2NaCl+H2SiO3↓ 32, chlorine reacts with metallic iron: 2Fe+3Cl2 ignites 2FeCl3 33, chlorine reacts with metallic copper: Cu+Cl2 ignites CuCl2 34, chlorine reacts with metallic sodium: 2Na+Cl2 ignites 2NaCl 35, and chlorine reacts with water: Cl2+H2O = HCl+. Photolysis of hypochlorous acid: 2HClO photolysis: 2HCl+O2↑ 37, reaction of chlorine with 2 = CaCl2+Ca(ClO)2+2H2O 39, reaction of hydrochloric acid with silver nitrate solution: HCl+AgNO3 = AgCl↓+HNO3 40, reaction of long-term exposure to air bleaching * * * *: Ca (clo) 2+. Kloc-0/, reaction of sulfur dioxide with water: SO2+H2O ≈ H2SO3 42, discharge of nitrogen with oxygen: N2+O2 discharge of 2NO 43, reaction of nitric oxide with oxygen: reaction of sulfur dioxide with oxygen under the action of catalyst: 2SO2+O2 catalyst 2SO3 46, reaction of sulfur trioxide with water: SO3+H2O = H2SO4 47, reaction of concentrated sulfuric acid with copper: △ CO2 =+2SO2 =+2H2O49, the reaction between concentrated nitric acid and copper: Cu+4NO3 (concentrated) = Cu (NO3) 2+2H2O+2NO2 = 50, and the reaction between dilute nitric acid and copper: 3Cu+8HNO3 (dilute) △ 3cu (NO3) 2+4h2o+2no = 560. H2O △ NH3↑+H2O 52, reaction between ammonia and hydrogen chloride: NH3+HCl = NH4Cl 53, thermal decomposition of ammonium chloride: NH4Cl △ NH3 ↑+HCl 54, thermal decomposition of ammonium bicarbonate: NH4CO3 △ NH3 ↑+H2O ↑+CO2 ↑ 55, The reaction between ammonium nitrate and sodium hydroxide: NH4NO3+NaOH △ NH3↑+NaNO3+H2O 56, SO2+2NaOH = Na2SO3+H2O 6 1, SO2+Ca (OH) 2 = caso362, recovered SO2+Cl2+2H2O = 2HCl+H2SO4 63, SO2+2H2S = 3S+2H2O 64, NO and NO2: NO2+NO+2NaOH = 2NaNO2+H2O 65, Si+2F 2 = SiF4 66, Si+2NaOH+H2O = Na2SiO3 +2H2↑ 67. The laboratory manufacturing method of simple silicon: prepare the melting point of crude silicon 1. Hydrocarbons. hydrocarbons. For homologues, the intermolecular force increases with the increase of relative molecular mass, so the melting boiling point of homologues increases with the increase of relative molecular mass. The melting points of homologues, halogenated hydrocarbons and aldehydes of various hydrocarbons increase with the increase of the number of carbon atoms in the molecule. For example, they are all alkanes, and the order of melting points is: they are all olefins, and the order of melting points is: and so on. Between isomers of the same type, the more carbon atoms in the main chain, the higher the melting point of hydrocarbons; The more branches, the more symmetrical the spatial position and the lower the melting point. For example. 2. Because the molecule of alcohol contains -OH, there are hydrogen bonds between alcohol molecules, and the intermolecular force is stronger than the general intermolecular force, so the melting point of alcohol is much higher than that of hydrocarbons with similar relative molecular mass, such as 78℃, -42℃ and -48℃. The factors that affect the boiling point of alcohol are: (1) the number of -OH in the molecule: the more OH number, the higher the boiling point. For example, the boiling point of ethanol is 78℃, and that of ethylene glycol is 179℃. (2) Number of carbon atoms in the molecule: The more carbon atoms, the higher the boiling point. For example, the boiling point of methanol is 65℃ and the boiling point of ethanol is 78℃. 3. Carboxylic acid molecules contain -—COOH, and there are hydrogen bonds between molecules, not only between hydroxyl oxygen and hydroxyl hydrogen between carboxylic acid molecules, but also between carbonyl oxygen and hydroxyl hydrogen between carboxylic acid molecules. Therefore, there are more opportunities to form hydrogen bonds between carboxylic acid molecules than alcohols with similar molecular weight, so the boiling point of carboxylic acid is higher than that of alcohols with similar molecular weight, for example, the boiling point of 1- propanol is 97.4℃, and the boiling point of acetic acid is 65438. The factors affecting the boiling point of carboxylic acid are: (1) the number of carboxyl groups in the molecule: the more carboxyl groups, the higher the boiling point of carboxylic acid; (2) Number of carbon atoms in the molecule: The more carbon atoms, the higher the boiling point of carboxylic acid. Second, the state of a substance is closely related to its melting point, which is determined by intermolecular forces. Because most organic compounds are macromolecules (relative to inorganic substances), the intermolecular attraction of organic compounds is large, so they are generally liquid and solid, and only a few small molecules are gaseous. 1. With the increase of the number of carbon atoms in the molecule, hydrocarbons change from gas to liquid and then to solid. Hydrocarbons with 1~4 carbon atoms in the molecule are generally gaseous, hydrocarbons with 5~ 16 carbon atoms are generally liquid, and hydrocarbons with more than 17 carbon atoms are solid. For example, under normal circumstances, benzene and its homologues are gaseous, generally liquid and mostly solid. 2. Alcohols and carboxylic acids contain-OH, and there are hydrogen bonds between molecules, so liquids usually have fewer carbon atoms in their molecules, while solids have more carbon atoms in their molecules, such as methanol, ethanol, formic acid and acetic acid. 3. Aldehydes: Generally, aldehydes with relative molecular weight greater than 100 are solid, except that formaldehyde with fewer carbon atoms is gaseous and acetaldehyde is liquid. 4. Esters: Generally, esters with fewer carbon atoms in the molecule are liquids, and the rest are solids. 5. Phenol and its homologues: Because it contains -OH, the benzene ring has a large molecular weight, so it is usually solid. Third, the density of hydrocarbons generally increases with the increase of carbon atoms; The relative density of monochloroalkanes decreases with the increase of carbon atoms. Note: 1. The density of gaseous organic matter is generally higher than that of air, and its relative molecular mass is greater than 29. 2. Generally, compared with water, the density of liquid organic matter: (1) hydrocarbons, esters, monochlorohydrocarbons, monohydric alcohols, aldehydes, ketones and higher fatty acids is lower than that of water; (2) Brominated hydrocarbons, nitrobenzene, carbon tetrachloride, chloroform, ethylene glycol, glycerol, etc. Dense than water. Four. Solubility when studying the solubility of organic compounds, the groups of organic molecules are often divided into hydrophobic groups and hydrophilic groups: groups with water-insoluble properties or unattractive to water are called hydrophobic groups; Groups that are soluble in or attractive to water are called hydrophilic groups. The solubility of organic matter is determined by the solubility of hydrophilic groups and hydrophobic groups in the molecule. Solubility of 1. functional groups: (1) water-soluble groups (i.e. hydrophilic groups) include —OH, —CHO, —COOH and —NH2. (2) Water-insoluble groups (i.e. hydrophobic groups) include all hydrocarbon groups (such as-,-—CH=CH2,-—C6H5, etc.). ), halogen atom (-x), nitro group (-—NO2), etc. 2. The ratio of hydrophilic groups to hydrophobic groups in the molecule affects the solubility of substances: (1) When the number of functional groups is the same, with the increase of the number of carbon atoms in hydrocarbon groups (hydrophobic groups), the solubility gradually decreases, such as solubility: >: (Generally, alcohols with more than 5 carbon atoms are almost insoluble in water); For another example, carboxylic acids with less than 4 carbon atoms in the molecule are miscible with water. With the increase of carbon chain in the molecule, the solubility in water decreases rapidly until it is close to alkanes with similar molecular weight. (2) When the number of carbon atoms in the hydrocarbon group is the same, the more hydrophilic groups, the stronger the solubility of the substance. Such as solubility:. (3) When hydrophilic groups and hydrophobic groups have almost the same influence on solubility, the substance is slightly soluble in water. For example, common substances that are slightly soluble in water are phenol, aniline, benzoic acid and n-amyl alcohol (the "-"on the left is a hydrophobic group, and the "-"on the right is a hydrophilic group). (4) A substance consisting of two hydrophobic groups must be insoluble in water. For example, halogenated hydrocarbon R-X and nitro compound R- are hydrophobic groups, so they are almost insoluble in water. 3. The solubility of organic matter in gasoline, benzene, carbon tetrachloride and other organic solvents is opposite to that in water. For example, ethanol is composed of a small hydrophobic group and a hydrophilic group -OH, so ethanol is easily soluble in water, and because it contains hydrophobic groups, it must also be soluble in organic solvents such as carbon tetrachloride. Other alcohols are soluble in water because they all contain hydrophilic groups -OH, but with the increase of hydrophobic groups, their solubility in water gradually decreases, and they are soluble in organic solvents such as carbon tetrachloride.