Human education version of the new curriculum standard senior high school chemistry compulsory first unit 1 knowledge points summary

High School Chemistry Compulsory Study I Senior High School Knowledge Combination Senior High School Chemistry Knowledge Points Summary Senior High School Chemistry Review Materials

Topic I The World of Matter in the Eyes of a Chemist

Unit I The Colorful World of Chemistry

I. Classification and Transformation of Substances

Classification of Substances (can be classified according to their composition, state, properties, etc.)

Substances Mixtures Non-homogeneous mixtures

Homogeneous mixtures

Pure substances Monomers Non-metallic monomers

Metallic monomers

Compounds Organic compounds

Inorganic compounds Oxides Metallic oxides

Non-metallic oxides

...

Acids

Bases

Salt

...

Types of Transformations (Reactions) of Substances

The four basic reaction types: chemosynthesis, decomposition, replacement, and complex decomposition

Chemical Reactions Essentials Redox Reactions Chemical Reactions Ionic Reactions

Non-Redox Reactions Nonionic Reactions

Redox reactions

1. Redox reactions: reactions with electron transfer

2. Redox reactions Substance: transfer of electrons

Judgment basis: change in the valence of the element

3.

Methods of representation of the transfer of electrons in redox reactions

1. The two-wire bridge method shows the direction and number of electron transfer

1. direction and number of transfer

Note: a. "e-" indicates electron.

b. The two-wire bridge method indicates that the arrows point from the reactants to the products, and the arrows start and end at the same element.

The "gain" and "loss" and the total number of electrons gained and lost should be indicated.

c. The reactant that loses electrons is the reducing agent, and the reactant that gains electrons is the oxidizing agent

d. The product that is oxidized is the oxidized product, and the product that is reduced is the reduced product

2. One-Wire Bridge Method (From Loss→Gain)

Reducing agent Oxidizing agent

Relationships between Redox Reactions and the Four Basic Types of Reactions

Redox reactions: total number of increases in valence = total number of decreases in valence

Total number of electrons lost by an element = total number of electrons gained by an element

Ionic reactions (chemical reactions involving ions)

The writing of ionic equations:

1. Write

2. Split: (can be thought of as simply as a strong acid, a strong base, or a soluble salt split)

3. delete

4. check (follow: conservation of charge, conservation of mass)

Two, the amount of matter

1, the amount of matter is a physical quantity, the symbol is n, the unit is moles (mol)

2, the number of particles of a mol is the number of carbon atoms contained in the 0.012 kg of 12C, which is about 6.02 × 1023 .

3. The number of particles in 1 mol is also known as Avogadro's constant, symbolized as NA, in mol-1.

4. When using moles, the type of particle must be specified, which can be molecules, atoms, ions, electrons, and so on.

5.,

Three, molar mass

1. Definition: the mass of 1 mol of any substance, called the molar mass of the substance. Expressed by the symbol: M, commonly used units of g?mol-1

2, mathematical expression:

Four, the state of aggregation of substances

1, the state of aggregation of substances: gaseous, liquid and solid

2, the molar volume of gases

Volume occupied by a gas per unit of volume of matter. Symbol: Vm expression: Vm= ; unit: L?mol-1

In standard conditions, the volume of 1 mol of any gas is about 22.4 L.

V. Dispersion of substances

1. Dispersion: the particles of a substance (or substances) are dispersed into another substance to form a mixture.

Classification (according to the size of the diameter of the particles of dispersed matter): solution (less than 10-9m 〉, colloid (10-9 ~ 10-7m)

Turbid liquid (greater than 10-7m)

2. colloid:

(1) concept: dispersed matter particles in the diameter of the size of the dispersed matter of the dispersion of the system between the size of 10-9 ~ 10-7m.

(2) Properties: ① Tyndall phenomenon (with a spotlight flashlight on the colloid, you can see in the colloid a bright "pathway", which is the colloid Tyndall phenomenon.)

② coagulation (adsorption of suspended particles in water)

3. solution: electrolyte solution, non-electrolyte solution

4. compounds

electrolyte: in aqueous solution or molten state can conduct electricity compounds

non-electrolyte: in aqueous solution or molten state can not conduct electricity compounds

5. Ionization (the process by which an electrolyte produces free-moving ions in an aqueous solution or in the molten state) Equation

NaCl == Na+ + Cl- H2SO4 == 2H+ + SO42- NaOH == Na+ + OH-

Unit II Experimental Methods for Studying Substances

I. Separation and Purification of Substances

Methods for Separating and Methods of purification Substances to be separated Matters to be noted Examples of applications

Filtration Used in the separation of solid-liquid mixtures A paste, two low, three rely on such as the purification of crude salt

Distillation Purification or separation of mixtures of liquids with different boiling points Preventing liquids from boiling violently, the position of the thermometer's mercury bulb, such as the flow of water in the condenser tube of the petroleum distillation Such as the distillation of petroleum

Extraction The solubility of a solute in a solvent that is not soluble in each other is utilized. solute in immiscible solvent solubility, a solvent to extract the solute from the solution composed of it and another solvent method The selection of the extractant should meet the following requirements: and the original solution of the solvent is immiscible with each other; solubility of the solute should be much greater than the original solvent with carbon tetrachloride extraction of bromine in bromine, iodine

Separation separation of immiscible liquids to open the upper end of the piston or so that the piston on the groove with the water hole on the funnel, the water hole on the piston, and the water hole on the piston, and the water hole on the funnel. Open the upper piston or make the groove on the piston with the water hole on the funnel so that the air inside and outside the funnel is connected. Open the piston, so that the lower liquid slowly flow out, close the piston in time, the upper liquid from the upper end of the pouring such as carbon tetrachloride extraction of bromine, iodine in the bromine water and then liquid separation

Evaporation and crystallization used to separate and purify the mixture of several soluble solids Heating evaporation dish to make the solution evaporate, the solution should be constantly stirred with a glass rod; when more solids in the evaporation dish, that is, to stop the heating Separation of NaCl and KNO3 mixture

Separation of the liquid from a mixture of immiscible liquids. KNO3 mixture

Two, the test of common substances

Three, the preparation and analysis of solutions

1. The concentration of the amount of substances C (B) = n (B)/V (solution)

2. The concentration of the amount of substances in the preparation of the amount of substances: calculating, weighing (or measuring), dissolving, transferring, washing, constant volume, shaking, bottling labeling

Specific steps:

(1) calculation: solid substances to calculate the required mass, liquid substances to calculate the required volume;

(2) weighing (measure): solid with a balance, liquid with a measuring cylinder;

(3) dissolve (dilute): transfer the solid (solution) to a beaker, dissolve (dilute) with the appropriate amount of distilled water, cool to room temperature;

(4) Transfer: the solution in the beaker has a glass rod carefully drained into a volumetric flask (of appropriate size):

(5) Wash: have distilled water to wash the inner wall of the beaker for 2~3 times, and each time the solution was washed was injected into the volumetric flask;

(6) Volumizing: slowly inject distilled water into a volumetric flask until the liquid level of the flask is close to the graduated line of the flask at a point of 1~2 cm. Switch to a rubber-tipped burette and add distilled water until the concave surface of the solution is just tangent to the scale line;

(7) Shaking: cap the volumetric flask and repeatedly turn it up and down and shake it well;

(8) Bottling.

Unit III Human Understanding of Atomic Structure

I. Evolution of Atomic Structure Models

Evolution of Modern Atomic Structure Models

Model Dalton Thomson Rutherford Bohr Quantum Mechanics

Era 1803 1904 1911 1913 1926

Based on the ratio of the masses of elements at the time of their compounds Relationships Discovery of electrons ɑ particle scattering Hydrogen atom spectroscopy Modern science experiments

Main content Atoms are indivisible solid spheres Raisin Bread Nucleus Model Planetary Orbital Atom Model Quantum Mechanics

1. Extranuclear electrons are always arranged in the lower-energy electron layers first, and then in the higher-energy electron layers from the inside out

(1) The electrons are always arranged in the lower-energy electron layers first, and then in the higher-energy electron layers from the inside out

(2) The electrons are arranged in the higher-energy electron layers from the inside out.

(2) Each electron layer outside the nucleus of an atom holds at most 2n2 electrons (indicating the number of electron layers).

(3) The number of electrons in the outermost field of an atom cannot exceed 8 (not more than 2 in the first layer)

(4) The number of electrons in the second outer layer cannot exceed 18 (not more than 2 when the first layer is the second outer layer), and the number of electrons in the penultimate layer cannot exceed 32.

II. Composition of Atoms

Indicates a specific X atom with mass number A and proton number Z.

Mass number (A) = number of protons (Z) + number of neutrons (N)

(1) Atom: nuclear charge (number of protons) = number of electrons outside the nucleus,

(2) Cation: nuclear charge (number of protons) > number of electrons outside the nucleus,

(3) Anion: nuclear charge (number of protons) < number of electrons outside the nucleus,

Nuclide: an atom with a certain number of protons and a certain number of neutrons.

Isotope: atoms (nuclides) with the same number of protons and different mass numbers (number of neutrons) are isotopes of each other

Topic II Chemical Substances Obtained from Seawater

Unit I Chlorine, Bromine, Iodine and their Compounds

I. Principle of Production of Chlorine Gas

2NaCl + 2H2O ==== 2NaOH + H2↑ + Cl2↑

Negative pole Positive pole

II. Properties of Chlorine Gas

Physical Properties

1. color: yellowish-green 2. odor: irritating odor 3. state: gaseous 4. toxicity: poisonous 5. density: greater than air

6. solubility: soluble in water (1 : 2)

Chemical Properties

1. Cl2 reacts with metals (generally oxidizes metals to higher valence states)

2. Cl2 reacts with non-metals

3. Cl2 reacts with bases

Chlorine + base → hypochlorite + metal chloride + water

Chlorine water

Components Molecules: H2O, Cl2, HClO Ions: H+, Cl- (and ClO-, OH-)

Properties of chlorine water

1. acidity 2. oxidizing 3. bleaching 4. instability

Test for Cl-: reagents: AgNO3 solution and dilute nitric acid Phenomenon: a white precipitate is produced (insoluble in dilute nitric acid)

Conclusion: there is Cl- in the solution

Properties of hypochlorous acid

1. acidity 2. Oxidizing property 3.Bleaching property

4.Instability:

Uses of chlorine: Disinfection of water, production of pesticides, synthesis of drugs, etc.

II. Extraction of bromine and iodine

Chemical properties of bromine and iodine: Order of the strength of non-metallicity of elements (oxidizing): Cl > Br > I

Experiment Experimental phenomenon Chemical equation

Chlorine water and potassium bromide are mixed with potassium bromide. p>Reaction of chlorine water with potassium bromide solution Solution changes from colorless to orange 2KBr+Cl2=2KCl+Br2

Reaction of chlorine water with potassium iodide solution Solution changes from colorless to yellow-brown 2KI+Cl2=2KCl+I2

Reaction of bromine water with potassium iodide solution Solution changes from colorless to yellow-brown 2KI+Br2=2KBr+I2

Reaction of bromine water with potassium iodide Solution changes from colorless to yellow-brown 2KI+Br2=2KBr+I2

Reaction of bromine water with potassium iodide solution I2

Physical properties of monomers

1. state: gas (Cl2) → liquid (Br2) → solid (I2)

2. color: yellowish-green (Cl2) → dark reddish-brown (Br2) → purplish-black (I2), the color ranges from light to dark

3. melting and boiling points: liquid bromine is volatile, iodine is easily sublimated by heat

4. .Solubility: Cl2 is soluble in water, Br2 and I2 are insoluble in water; Br2 and I2 are soluble in organic solvents such as gasoline, alcohol, benzene and CCl4.

I2 test: reagents: starch solution Phenomenon: the solution turns blue

Br-, I- test:

Reagents: AgNO3 solution and dilute nitric acid

Phenomenon: light yellow precipitate (containing Br-); yellow precipitate (containing I-)

Example: NaBr + AgNO3 = AgBr↓ + NaNO3

NaI + AgNO3 = AgI↓ + NaNO3

Unit II Sodium, Magnesium and their compounds

I. Properties and Applications of Sodium Metal

Properties of Sodium

Physical Properties

Silver-white solid, with a metallic sheen, density is greater than kerosene than water is smaller, soft, low melting point, conductive of electricity and heat.

Chemical properties

1, and O2, Cl2, S and other non-metals react

4Na + O2 === 2Na2O (white)

2Na + O2 === Na2O2 (yellowish solid)

2Na + Cl2 === 2NaCl (white smoke)

2Na + S == Na2S (sparks)

2Na + S == Na2S (sparks). == Na2S (sparks, and even an explosion)

2, the reaction with water

2Na + 2H2O === 2NaOH + H2↑ ( floating, soluble, swimming, red )

Two, sodium carbonate's properties and applications

Na2CO3's properties (aqueous solution is alkaline)

(1) Reaction with alkali Na2CO3 + Ca(OH)2 === CaCO3↓ + 2NaOH

(2) reaction with salt Na2CO3 + BaCl2 === BaCO3↓ + 2NaCl

(3) reaction with CO2: Na2CO3 + CO2 + H2O === 2NaHCO3

Na2CO3 vs. Comparison of the properties of NaHCO3

III. Extraction and application of magnesium

Extraction of magnesium

Sea water mother liquor MgCl2

a solution

Shells Milk of Lime

CaCO3 === CaO + CO2↑

CaO + H2O ===Ca(OH)2 (Milk of lime)

Ca(OH)2 (Milk of lime)

Ca(OH)2 (Milk of lime)

Ca(OH)2 (Milk of lime)

Ca(OH)2 (milk of lime)

Ca(OH)2 + MgCl2 === Mg (OH)2↓+ CaCl2

Mg(OH)2 + 2HCl === MgCl2 + 2H2O

MgCl2 === Mg + Cl2↑

Physical Properties

Magnesium is a silvery-white metal, with a metallic sheen, a small density, a large hardness , soft texture, low melting point, and is a good conductor of heat and electricity.

Chemical Properties

1.Reaction with Air

2Mg + O2 === 2MgO

3Mg + N2 === 2Mg2N3

2Mg + CO2 === 2MgO + C

2.Reaction with Water

Mg+2H2O === Mg(OH)2+ H2↑

Mg+2H2O === Mg(OH)2+ Mg(OH)2+ H2↑

2. H2↑

3, reaction with acid

Mg + H2SO4 === MgSO4 + H2↑

Use

1) Magnesium alloys have less density but more hardness and strength, so they are used in the manufacture of rockets. Missiles and aircraft parts

2) magnesium burning emits a dazzling white light, so it is often used to make communication missiles and fireworks;

3) magnesium oxide has a very high melting point, is a high quality high-temperature materials

Topic 3 from minerals to basic materials

Unit 1 from bauxite to aluminum alloys

A. Extraction of Aluminum from bauxite

①Dissolving: Al2O3+2NaOH === 2NaAlO2+H2O

②Filtering: removing impurities

③Acidifying: NaAlO2+CO2+2H2O === Al(OH)3↓+NaHCO3

④Filtering: retaining aluminum hydroxide

⑤Scorching: 2Al(OH)3 ===== == 4Al+3O2↑

Aluminum alloy features: 1, low density 2, high strength 3, good plasticity 4, simple manufacturing process 5, low cost 6, strong corrosion resistance

Four, the chemical properties of aluminum

(1) reaction with acid: 2Al + 6HCl = 2AlCl3 + 3H2↑

(2) reaction with alkali: 2Al + 2NaOH + 2H2O

(2) reaction with alkali: 2Al + 2NaOH + 2H2O 4H2O +3H2↑

(3) passivation: at room temperature, aluminum and concentrated nitric acid, concentrated sulfuric acid will be generated on the surface of the dense oxide film and passivation occurs, not with concentrated nitric acid, concentrated sulfuric acid further reaction.

(4) Aluminum thermal reaction:

2Al + Fe2O3 === 2Fe + Al2O3

Aluminum thermite: aluminum powder and some metal oxides (Fe2O3, FeO, Fe3O4, V2O5, Cr2O3, MnO2) composed of a mixture.

III. Aluminum hydroxides (amphoteric)

(1) Reaction with acids: Al(OH)3 + 3HCl = AlCl3 + 3H2O

(2) Reaction with bases: Al(OH)3 + NaOH = NaAlO2 + 2H2O

Preparation of Al(OH)3:

H2O

Aluminum salt ( AlCl3 ) Al(OH)3↓ meta-aluminate ( NaAlO2 )

To AlCl3 solution drop NaOH solution: first there is a white precipitate produced, and then disappeared;

To NaOH solution drop AlCl3 solution: first no obvious phenomenon, and then there is a precipitate produced.

Unit II Applications of Iron, Copper and Their Compounds

I. Obtaining Iron and Copper from Nature

Blast Furnace Ironmaking (1) Production of CO: C + O2 === CO2, CO2 + C === CO

(2) Reduction (Principle of Ironmaking): Fe2O3 + 3CO === 2Fe + 3CO2

(3) In addition to SiO2: CaCO3 === CaO + CO2↑, CaO + SiO2 === CaSiO3

Copper refining: 1. High-temperature smelting of chalcopyrite → Electrolytic refining; 2. Wet refining of copper: Fe + CuSO4 = FeSO4 + Cu; 3. Biorefining of copper

The second, the application of iron, copper and their compounds

Chemical properties of iron: Iron is the more active metal (or moderately active metal) exhibits reducing properties.

Iron Copper

(1) and non-metallic reactions

①Iron rusts (iron corrodes in moist air to produce Fe2O3)

②2Fe + 3Cl2 === 2FeCl3

③2Fe + 3Br2 === 2FeBr3 Reductive: Fe2+>Br

④3Fe +2O2 === Fe3O4 (2-valent Fe accounts for 2/3 of the 2-valent Fe)

Cu + O2 === 2CuO

Cu + Cl2 === CuCl2

2Cu + S === Cu2S

(2) Reactions with Acids ①Non-strongly aerobic acids: Fe + 2H+ == Fe2+ + H2↑

< p>② Strongly oxygenated acids (concentrated H2SO4, HNO3):

a. Passivation at room temperature (concentrated H2SO4, concentrated HNO3 in iron containers)

b. Reaction to form Fe(Ⅲ) under certain conditions ①Non-strongly oxygenated acids: no reaction

② Strongly oxygenated acids (concentrated H2SO4, HNO3): generation of Cu(Ⅱ) under certain conditions )

(3) Reaction with salt solution (1) Fe + Cu2+ == Fe2+ + Cu

(2) Fe + 2Fe3+ == 3Fe2+

Cu + 2Ag+=2Ag + Cu2+

Cu + 2Fe3+ == 2Fe2+ + Cu2+ (Experimental phenomenon: copper powder dissolves and the color of solution changes. )

Mutual transformation of Fe2+ and Fe3+:

Test of Fe3+: (yellowish brown)

Experiment ①: add a few drops of KSCN solution to FeCl3 solution, the solution shows blood red color,

Fe3+ + 3SCN- Fe(SCN)3

Experiment ②: add NSCN solution to FeCl3 solution. FeCl3 solution add NaOH solution, there is reddish brown precipitate.

Fe3+ +2OH- Fe(OH)3↓

Test for Fe2+: (light green)

Experiment: add NaOH solution to FeCl2 solution.

Fe2+ +2OH- Fe(OH)2↓ (white/light green) 4Fe(OH)2 +O2 + 2H2O 4Fe(OH)3 (reddish brown)

III. Corrosion of Steel

Unit III Silicon Containing Minerals and Information Materials

I. Silicate Minerals, Silicate Products (Traditional materials) and information materials

1. Silicon in nature: the earth's crust in the second place after oxygen. (About one-fourth of the mass of the earth's crust); no free state, the main form of existence of the chemosynthesis state is silicate and silicon dioxide,

2. The structure of silicates:

(1) the structure of silicates is complex, commonly used in the form of oxides to express the more convenient. Silicate structure is stable, stable in nature.

(2) The law of writing the form of oxides:

① Each element is written as the corresponding oxide, and the valence state of the element remains unchanged.

② order according to the first metal and then non-metal, metal elements according to the order of metal activity table in order, in the middle with "?" in the center with a "?" interval.

3 Note that after rewriting the original chemical formula should be unchanged in the ratio of the number of atoms.

3. Properties of Na2SiO3: Na2SiO3 is soluble in water, aqueous solution is commonly known as "water glass", is the construction industry's adhesive, but also for wood preservation and fire prevention.

Chemical properties are mainly manifested as follows:

(1) the aqueous solution is alkaline (measured with PH paper), through CO2 has a white precipitate: Na2SiO3 + CO2 + H2O == Na2CO3 + H2SiO3 ↓ (white gelatinous precipitate), ionic equation: SiO32- ＋ CO2 + H2O = = = CO32- + H2SiO3 CO32- + H2SiO3↓.

Silicic acid decomposition by heat: H2SiO3 H2O + SiO2,

proto-silicic acid and silicic acid are insoluble in water, weak acid, acidity: H2CO3 stronger than H4SiO4 or H2SiO3.

(2) sodium silicate solution with dilute hydrochloric acid droplets with a white precipitate:

Na2SiO3 + 2HCl == 2NaCl + H2SiO3↓, ionic equation: SiO32- + 2H+ == H2SiO3↓.

(3) Silicic acid and sodium hydroxide reaction: H2SiO3 + 2NaOH == Na2SiO3 + 2H2O.

Ionic equation: H2SiO3 ＋ 2OH- == SiO32- + 2H2O.

4. Silicate products (traditional materials)

Main raw materials Main components of the products

Ordinary glass Quartz, soda ash, limestone Na2SiO3, CaSiO3, SiO2 (the ratio of the amount of substances is 1:1:4)

Ordinary cement Clay, limestone, a small amount of gypsum 2CaO?SiO2, 3CaO?SiO2 3CaO?Al2O3

Ceramics Clay, quartz sand Complex composition mainly silicates

Main reactions in glass making: SiO2 + Na2CO3 Na2SiO3 + CO2↑,SiO2 + CaCO3 CaSiO3 + CO2↑.

Two, silicon monomers

1. Properties: (1) Physical Properties: crystalline silicon is gray-black metallic luster, hard and brittle solid; conductivity between conductors and insulators, is a good semiconductor material, high melting and boiling point, hardness, insoluble in solvents.

(2) chemical properties: room temperature, only with a single fluorine, hydrofluoric acid and strong alkali solution reaction. Stable nature.

Si +2F2 == SiF4 (gaseous), Si + 4HF == SiF4 +2 H2,

Si +2NaOH + H2O == Na2SiO3 +2H2↑, (Si +2NaOH + 4H2O == Na2SiO3 +2H2↑+ 3H2O.)

3. Manufacture of silicon chips, integrated circuits, transistors, silicon rectifiers and other semiconductor devices; (2) the manufacture of solar energy; (3) the manufacture of alloys, such as containing silicon 4% (mass fraction) of the steel conductivity is good for the manufacture of transformer cores; containing silicon 15% (mass fraction) of the steel has a good resistance to acidity and so on.

4. Industrial production of silicon:

Crude silicon: SiO2 + 2C Si + 2CO

Pure silicon: Si + 2Cl2 SiCl4 (liquid)

SiCl4 + 2H2 Si + 4HCl

Three, silicon dioxide, the structure and nature of the:

1. SiO2 has a more pure crystal, containing a small amount of impurities in nature. crystals, quartz with a few impurities, and prevalent sand. Silicon dioxide in nature is also known as silica.

2. SiO2 physical properties: hardness, high melting point, insoluble in solvent (water) solid.

3. SiO2 Chemical Properties: room temperature, stable nature, only with a single fluorine, hydrofluoric acid and strong alkali solution reaction.

SiO2 + 2F2 == SiF4 + O2 , SiO2 + 4HF == SiF4 + 2H2O (carving glass reaction),

SiO2 + 2NaOH == Na2SiO3 + H2O (laboratory alkali reagent bottles can not be used for the reason of glass stopper).

Heating high temperature: SiO2 + 2C Si +2 CO, SiO2 + Na2CO3 Na2SiO3 + CO2↑

SiO2 + CaCO3 CaSiO3 + CO2↑, SiO2 + CaO CaSiO3 .

4. SiO2 use: the production of quartz glass, is the main raw material of optical fiber; the production of clock parts; can be made wear-resistant materials; used in the production of glass; in the optical instruments, electronic industry and other widely used.

Topic IV Sulfur, Nitrogen and Sustainable Development

Unit I Properties and Applications of Sulfur-Containing Compounds

I. Causes and Prevention of Sulfuric Acid Rain:

1. Massive Combustion of Sulfur-Containing Fuels (Fossil Fuels)

Reactions Involved:

2SO2 + O2 2SO3 SO3 + H2O = H2SO4

SO2 + H2O H2SO3 2H2SO3 + O2 = 2H2SO4

2. Preventive and curative measures:

①To prevent and control acid rain at the root of the problem - the development of the use of green energy instead of fossil fuels (hydrogen, nuclear energy, solar energy)

②To the sulfur fuels for the desulfurization treatment (such as coal liquefaction and coal gasification)

③ improve environmental awareness, strengthen international cooperation

Second, the nature of SO2 and its application

1. Physical Properties: colorless, irritating odor, poisonous gases, easily soluble in water

* atmospheric pollutants usually include: SO2, CO, oxides of nitrogen, hydrocarbons, solid particulate matter (dust)

3, the use of sulfur-containing fuels to desulfurize the fuel. /p>

2. The chemical properties of SO2 and its application

1) SO2 is an acidic oxide

SO2 + H2O H2SO3

SO2 + Ca(OH)2 = CaSO3↓ + H2O; CaSO3 + SO2 + H2O = Ca(HSO3)2

SO2 + 2NaOH = Na2SO3 + H2O (HSO3)2

SO2 + 2NaOH = Na2SO3 = H2O (HSO3)2

SO2 + 2NaOH = Na2SO3 + H2O (Na2SO3 + H2O) Na2SO3 + H2O (NaOH solution is used in the laboratory to absorb SO2 exhaust)

* Reduction of SO2 emissions during coal combustion (calcium-based sulfur fixation)

CaCO3 CaO + CO2↑; CaO + SO2 = CaSO3

SO2 + Ca(OH)2 = CaSO3 + H2O

2CaSO3 + O2 = 2CaSO4

(2) SO2 has bleaching properties: commonly used in the laboratory for the test of SO2 gas

Types of bleaching principles

①Adsorption type: activated charcoal bleaching - activated charcoal adsorption of pigments (including colloidal)

②Strong oxidation type: HClO, O3, H2, Na2O2 and other strong oxidizing agents bleaching - oxidation of colored substances, irreversible

③ chemotaxis: SO2 bleaching - and the combination of colored substances, reversible

③ SO2 has a reducing <

2SO2 + O2 2SO3

SO2 + X2 + 2H2O = 2HX + H2SO4

Third, the contact method of sulfuric acid

Process Equipment Reactions

Generation of sulfur dioxide Boiling furnace S + O2 SO2 or 4FeS2 + 11O2 2Fe2O3 + 8SO2

SO2 contact Oxidation contact chamber 2SO2 + O2 2SO3

SO3 absorption Absorption tower SO3 + H2O = H2SO4

* In order to prevent the formation of acid fog, improve the absorption rate of SO3, commonly used in concentrated sulfuric acid to absorb SO3 to get fuming sulfuric acid

Four, the nature of sulfuric acid and its application

1. acidic sulfuric acid: Sulfuric acid is a binary strong acid H2SO4 = 2H+ + SO42- (with the 5-point generality of the acid)

such as: Fe2O3 + 3H2SO4 = Fe2(SO4)3 + 3H2O Sulfuric acid is used for pickling and descaling

2. Concentrated sulfuric acid's absorbent properties: Concentrated sulfuric acid has absorbent properties, and it can be used as a drying agent

3. Concentrated sulfuric acid's dehydration Concentrated sulfuric acid is used as dehydrating agent and catalyst for many organic reactions.

4. Strong oxidizing property of concentrated sulfuric acid:

Cu + 2H2SO4(Concentrated) CuS O4 + SO2↑+ 2H2O

Concentrated sulfuric acid can oxidize many metals:

The oxidizing property of concentrated sulfuric acid is stronger than that of dilute sulfuric acid:

The oxidizing property of concentrated sulfuric acid is caused by the S of the +6 valence. Dilute sulfuric acid's oxidizing property is caused by H+ (it can only oxidize metals that are in front of H in the order of metal activity table).

C + 2H2SO4(Concentrated) CO2↑+ 2SO2↑+ 2H2O

The interconversion of sulfur and its compounds

1. Sulfur compounds with different valence states

-2-valent: H2S, Na2S, FeS; +4-valent: SO2, H2SO3, Na2SO3

+6-valent: SO3, H2SO4, Na2SO4, Na2SO3

+6-valent: SO3, H2SO4, H2SO4, Na2SO4, Na2SO3

Sulphuric acid is strong. H2SO4, Na2SO4, BaSO4, CaSO4 , FeSO4

2. Transformation between substances containing sulfur elements in different valence states through redox reactions

-2 0 +4 +6

S S S S S S S S S S S S S S S S S

SO42- ions Test: SO42- + Ba2+ = BaSO4↓

Take a small amount of the liquid to be measured No obvious phenomenon Produces a white precipitate

Unit II, nitrogen-containing compounds in production and life

I. Production and transformation of nitrogen oxides

Pathway I: thunderstorms hair crops

N2 + O2=== 2NO

N2 + O2=== 2NO

N2 + O2 ==== 2NO

N2 + O2 ==== 2NO 2NO

2NO+O2===2NO2

3NO2+H2O===2HNO3+NO

Pathway II: Biological Nitrogen Fixation

Pathway III: Synthesis of Ammonia N2+3H2=======2NH3

(1) How do the environmental problems appear? (1), the result of the improper use of science and technology by mankind

(2), what is the root cause of environmental problems? (2), Extreme pursuit of commercial profits

(3), What are the ways to overcome environmental problems? (3), Governance, use of new technology, change of lifestyle, education on environmental awareness

II. Production and use of nitrogen fertilizers

1. Synthesis of ammonia in industry

N2+3H2=======2NH3

2. Laboratory production of ammonia gas

2NH4Cl+Ca(OH)2====CaCl2+ 2NH3↑+2H2O

3. Properties of ammonia gas

: ammonia is soluble in water, dissolved in water shows alkaline, can make the wet red litmus paper turn blue. Ammonia is volatile and not easy to transport, but low cost. Ammonia should be kept in a cool place. Ammonia nitrogen fertilizer should not be applied in rain or hot sun.

Reaction with acids NH3 +HCl==NH4Cl (produces white smoke) 2NH3+H2SO4==(NH4)2SO4

Salt: solid, decomposes easily, soluble in water, reacts with alkali, produces and volatilizes. Cannot be used in alkaline soil or on rainy days. NH4Cl===NH3↑+HCl↑(decompose NH4Cl crystals by heating)

Fountain experiment:(1). How does the experimental setup work? (2). Reasons for the solution turning red? (3). What conditions should be present for a fountain to occur?

Three, the properties of nitric acid

1. Physical properties: colorless, volatile liquid

2. Chemical properties:

(1) instability will decompose and release gas in the presence of light or heat

4HNO3 == 4NO2↑ + O2↑ + 2H2O

(2) strong oxidizing

is a strong oxidizing acid. a strongly oxidizing acid, the vast majority of metals and many non-metallic monomers can react with nitric acid ....

Concentrated :

C+4HNO3==CO2↑+ 4NO2↑+2H2O Generally produces gas.

Dilute : Generally produces gas.

Also,

(1)

Applicable : Solid + Liquid Gas. The method is the easiest. The latter reaction is more violent, the drip of concentrated nitric acid should be controlled.

(2) C + 4HNO3 == CO2 ↑ + 4NO2 ↑ + 2H2O 4HNO3 == 4NO2 ↑ + O2 ↑ + 2H2O

Applicable: solid + liquid Gas. The method is more cumbersome and there are impurity gases in the product.