Divided: Chemistry
The use of electronic data in the process significantly facilitates the implementation of the lesson, allows for an individual, differentiated approach to the time of communication between the student and the teacher, which is of great help The teacher has an hour of preparation before the lesson.
Just as during the hour of computer science lessons the computer stands as a meta-lighting process, then in other lessons, during the hour of chemistry lessons, the computer is used to achieve initial goals.
A traditional tool for writing and studying in the classroom: a board, a pencil, a pen, a sewing board, and the same tools are available for the new student, for example, like an electronic SMART board.
Interactive lessons allow you to increase the intensity of the lesson:
Lesson objectives:
Lighting: consolidate the knowledge of students about nitrogen oxides, repeat the classification and main powers of oxides, repeat the main powers of nitric acid and consolidate the specifics of their interactions with metals, learn about stagnation m nitric acid.
Developing: be able to independently systematize developments and analyze theoretical and experimental information, see the headaches in the process of demonstrating follow-ups, carry out independent work on innovations, and make analogies.
Vikhova: the formation of a scientific outlook, the development of communicative skills in the course of group, pair and collective work, the need for new information technologies to obtain chemistry before understanding and description of cesіv, which are in the middle of nowhere, taking care of your health and well-being 'I'm a dovkilla.
Lesson form– seminar
Methods to use in class – verbal (conversation, opinion), basic (presentation), practical (virtual chemical laboratory), novelty (virtual interactive board), control (learning experience, writing notes) chemical reactions).
Possession and materials:
Disc "Virtual chemical laboratory", 9th grade
1. Organizational stage. The teacher’s word comes: Greetings, checking readiness for the lesson.
2. Motivational stage
The topic of the lesson is logical extension of the use of nitrogen.
Stage of expansion, formalization, consolidation of theoretical and practical knowledge of learning on the topic of the lesson
What kind of nitrogen oxides do you know? Name the skin oxide
Indicate the valency and stage of oxidation of nitrogen in skin oxide
What type of oxides are introduced into the skin?
Learn to go through the school and write on the electronic SMART - school the chemical formulas of nitrogen oxides, indicate the valence and oxidation stage of nitrogen in the skin, give the name of the oxides, indicate the type of skin.
What are the physical and chemical effects of nitric oxide (I)? (Slide 5)
What are the physical and chemical effects of nitric oxide (II)? (Slide 6)
Complete the chemical reactions characteristic of this oxide
What are the physical and chemical effects of nitric oxide (III)? (Slide 7)
Complete the chemical reactions characteristic of this oxide
N 2 O 3 + H 2 O =
What are the physical and chemical effects of nitric oxide (IV)? (Slide 8)
Complete the chemical reactions characteristic of this oxide
There is a large amount of nitrogen (IV) oxide that enters the storage of exhaust gases from cars and gas fluids from industrial enterprises, causing acid rain.
What are the physical and chemical effects of nitric oxide (V)? (Slide 9)
Complete the chemical reactions characteristic of this oxide
N 2 O 5 + H 2 O =
In what ways can you remove all nitrogen oxides? Write a comparison of chemical reactions. Learn to go to the interactive board and write an equal reaction. (Slide 10)
What acids do you know about nitrogen? Carry out the purification of these acids.
| Leveling parameters | Nitrous acid | Nitric acid |
| Chemical formula | HNO2 | HNO3 |
| Nitrogen oxidation stage | + 3 | +5 |
| Valency of nitrogen | 3 | 4 |
| Boiling temperature | - | 82.6 0 С |
| Durability | It only sleeps at low temperatures and in diluted areas; at elevated temperatures it easily decomposes: 3 HNO 2 = HNO 3 + 2NO + H 2 O |
Lays out on the light 4HNO 3 =4 NO 2 + O2+2H2O |
| Chemical power | Reveals oxidative and regenerative powers. | Reveals less oxide power |
In the eyes of the ancient descendants, nitric acid is a substance that has great power in the hands of people. (Slide 12)
Finish the comparison of chemical reactions: (Slide 13)
HNO3 + Mg(OH)2 =
HNO 3 + Na 2 CO 3 =
HNO 3 + K 2 SiO 3 =
Turn over the equation of chemical reactions: (Slide 14)
2HNO 3 + Mg(OH) 2 -> Mg(NO 3) 2 +2H 2 O
2HNO 3 + MgO -> Mg(NO 3) 2 +2H 2 O
2HNO 3 + Na 2 CO 3 -> 2NaNO 3 +CO 2 +H 2 O
2HNO 3 + K 2 SiO 3 -> 2KNO 3 + H 2 SiO 3?
Features of the interaction of nitric acid with metals. (Slide 15)
The teachings confirm the supply:
When nitric acid reacts with metals, the following is formed: salt (Me nitrate) + H 2 Pro + A, where “A” is the product of renewal N +5: NO 2, N 2 O 3, NO, N 2 O, N 2, NH 3 (NH 4 NO 3);
Metals interact with nitric acid, which stand before and after water in the activity series, where the active metal and the diluted acid, thereby replacing the nitrogen atom in nitric acid.
Nitric acid (concentrated) does not interact (passively): Al, Fe, Cr, Ni, Pb etc.
The interactions of nitric acid with metals and non-metals are confirmed by demonstration traces, as scientists have concluded using a virtual chemical laboratory disk. The various reactions of the interaction of nitric acid with metals and non-metals are recorded in the SMART electronic dossier. (Slide 16,17)
Nitric acid has a wide range of properties. Stagnation of nitric acid affects two individuals: creative and destructive. Nitric acid is used for the removal of nitrogen fibers, vibukhovyh rayons, barnacles, plastics, piece fibers, etc. (Slide 18-21)
After the seminar, you can conduct a ten-week control section, which will be included in the presentation.
4. Pouch fitment. Reflection.
You and I were effectively dealt with. Do you think we have reached the goal we set? What was important to you? What was the easiest thing for you?
Write down the chemical reactions of nitric acid in atmospheric nitrogen.
Summary of a 9th grade chemistry lesson on the topic “Turkish reactions to nitrogen” based on the elementary methodological complex of O.S. Gabrielyan. It is important to take a closer look at the oxidative power of nitrogen ions on the butt of tarnished resin. Summary of illuminating, developing, spiritual and health-preserving tasks.
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Kisnevy with nitrogen.
Nitrogen oxides. Nitrogen dissolves six tarnished compounds. oxidation stage + 1 N 2 O + 2 NO + 3 N 2 O 3 + 4 NO 2, N 2 O 4 + 5 N 2 O 5
Removal: NH 4 NO = N 2 O +2H 2 O Chemical power: 1. expansion when heated 2 N 2 +1 O = 2 N 2 0 + O 2 2. with water N 2 +1 O + H 2 = N 2 0 + H 2 O non-saline +1 N 2 O nitrous oxide (I), nitrous oxide or “laughing gas”, which causes nervous system people who use medicine as an anesthetic agent. Physical power: gas, no color or smell. Reveals oxides of power and is easy to decompose.
NO +2 Extraction: 1. In nature: N 2 + O 2 = 2NO 2. In industry: 4 NH 3 + 5O 2 = 4NO +6H 2 O Chemical power: 1. easily oxidized: 2 N +2 O + O 2 = 2N +4 O 2 2. oxidizing agent: 2 N +2 O + 2SO 2 = 2SO 3 +N 2 0 non-saline, barbaric-free gas, thermally stable, poorly resistant to water, practically mitite interaction with acid (at room temperature).
N 2 O 3 +3 Chemical power: NO 2 + NO N 2 O 3 Removal: ALL power of acid oxides. acidic acid oxide, dark blue color, thermally unstable, boiling point. = 3.5 0C, then it starts in a rare state only when cooled, in the case of normal minds, go to a gas-like state. When interacting with water, nitrous acid is dissolved.
NO 2 + 4 Removal: 1. 2 NO + O 2 = 2NO 2 2. Cu + 4HNO 3(k) = Cu(NO 3) 2 + 2NO 2 + 2H 2 O Chemical power: 1. with water 2 NO 2 + H 2 O = HNO 3 + HNO 2 2. from the meadows 2NO 2 + 2NaOH = NaNO 3 + NaNO 2 + H 2 O 3. dimerization 2NO 2 N 2 O 4 toxic nitrogen oxide (IV) or nitrogen dioxide, brown gas, good responsible for water, which completely reacts with it. Є strong oxidation.
N 2 O 5 + 5 Removal: 1. 2NO 2 + O 3 = N 2 O 5 + O 2 2. 2HNO 3 + P 2 O 5 = 2HPO 3 + N 2 O 5 Chemical power: 1. easy to decompose 2N 2 O 5 = 4NO 2 + O 2 2. strong oxidizing acid oxide nitrogen oxide (V), nitric anhydride, white solid resin (melt. = 41 0 C). It reveals acidic power and is a very strong oxidizer.
HNO 3 Warehouse. Budova. Authority. H O N O O - - stage of nitrogen oxidation, nitrogen valence +5 IV chemical bond covalent polar Nitric acid is a barless, hygroscopic liquid, with a pungent odor, smokes on the surface, and is indispensable near water. Melting point −41.59 °C, boiling point +82.6 °C from partial distribution. When stored on light, it decomposes into nitric oxide (IV), acidity and water, swelling the yellowish color: 4HNO 3 = 4NO 2 + O 2 + 2H 2 O Nitric acid is removed.
Nitric acid (HNO 3) Classification by: presence of acidity: basicity: toxicity in water: volatility: stage of electrolytic dissociation: acidic monobasic volatile volatile strong
Removal of nitric acid in industry NH 3 NO NO 2 HNO 3 4NH 3 + 5O 2 = 4NO + 6H 2 O 2NO+O 2 = 2NO 2 4 NO 2 + 2 H 2 O + O 2 = 4 HNO 3 Contact oxidation of ammonia to oxide nitrogen (II): 2. Oxidation of nitrogen oxide (II) to nitrogen oxide (IV): 3. Adsorption (claying) of nitrogen (IV) oxide with water when there is too much sourness
In the laboratory nitric acid keep concentrated sulfuric acid on nitrates under low heat. NaNO 3 + H 2 SO 4 = NaHSO 4 + HNO 3
Chemical properties of nitric acid Nitric acid exhibits all types of acid properties. 1 . Power of HNO 3 as an electrolyte: 1 3 2 3 2) with basic and amphoteric oxides 3) with bases 1) Dissociation: HNO 3 = H + + NO 3 – 2HNO 3 + CuO = Cu(NO 3) 2 + H 2 O 6HNO 3 + Al 2 O 3 = 2Al(NO 3) 3 + 3H 2 O HNO 3 + NaOH = NaNO 3 + H 2 O 2HNO 3 + Zn(OH) 2 = Zn(NO 3) 2 + 2H 2 O 4) s salts 2HNO 3 + Na 2 SiO 3 = H 2 SiO 3 ↓ + 2NaNO 3
2. Oxidative power: particular interactions with metals: (nitric acid does not see water at all!) Me + HNO 3 = Me(NO 3) 2 + H 2 ￪ Metal concentrated (> 60%) Diluted (5-60%) More diluted (
With metals that stand near the voltage to the left of the water: With metals that stand near the voltage to the right of the water: Concentrated HNO 3 Diluted HNO 3 Chemical power of nitric acid
2. Oxidative power 2) Features of interaction with non-metals (S, P, C): 3) Interaction with organic speeches(turpentine is consumed): Chemical power of nitric acid 3P + 5HNO 3 + H 2 O = 3H 3 PO 4 + 5NO C + 4HNO 3 = CO 2 + H 2 O + 4NO 2 5 HNO 3 + 3 P + 2 H 2 O → 3 H 3 PO 4 + 5 NO
Stagnation of nitric acid 1 5 4 6 2 3 Virobination of nitrogen and complex additives. Virobination of barnacles Virobination of barnberries Virobination of liks Virobination of fluffs, nitrovarnishes, nitroemals Virobination of piece fibers 7
Nitrates are salts of nitric acid that are present in the presence of acids on metals, their oxides and hydroxides. Saltpeter – salts of nitric acid meadow metals. NaNO 3 – sodium nitrate KNO 3 – potassium nitrate NH 4 NO 3 – ammonium nitrate Ca (NO 3) 2 – calcium nitrate Power: ALL important things in water.
When heated, the waste is decomposed higher, which is right in the electrochemical series of voltage, which is the metal that is created by the salt. Li K Ba Ca Na Mg Al Mn Zn Cr Fe Co Sn Pb Cu Ag Hg Au nitrite + O 2 metal oxide + NO 2 + O 2 Me + NO 2 + O 2 2NaNO 3 = 2NaNO 2 + O 2 2Pb(NO 3) 2 = 2PbO + 4NO 2 + O 2 2AgNO 3 = 2Ag + 2NO 2 + O 2
Saltpeter is praised as being kind. KNO 3 is used for preparing black powder.
Home management: § 26, ex. 2.4 side 121.
Slide 1
addition of NITROGEN Material for repetition and preparation before DPA Chemistry teacher Municipal Educational Institution “Gymnasium No. 1” p. Saratova Shishkina I.Yu.Slide 2
Nitrogen is removed from water by a small amount of honey, including ammonia, which is the most important. The electronic formula of the ammonia molecule is: Ottrimanya ammonia. In the laboratory: 2NH4Cl + Ca (OH)2 = CaCl2 + 2NH3 + 2H2O In the industry: N2 + 3H2 2NH3 + 92 kJ
Slide 3
Chemical characteristics 1. Ammonia is a strong agent. 3Cu+2O + 2N-3H3 = 3Cu0 + N20 + 3H2O 2N-3 – 6e = N 2 Cu2+ + 2e = Cu 3 4NH3 + 3O2 = 2N2 + 6H2O In the presence of a catalyst, chromium (III) oxide, reaction (II) and water : Cr2O3 4NH3 + 5O2 = 4NO + 6H2O Renewal of metals from their oxides:
Slide 4
Ammonia reacts with potassium permanganate: NH3 + KMnO4 = N2 + H2O + MnO2 +KOH Reacts with halogens: 2NH3 + 3Br2 = 6HBr + N2 2NH3 + 3Cl2 = 6HCl + N2 Adding ammonia changes the amount ir rozchina
Slide 5
2. dilution of salts with ammonium. Reactions from the formation of a donor-acceptor bond. NH3 + H2O NH3. H2O NH4+ + OH- NH4OH NH4+ + OH- H NH3 + H+Cl- [ H N H ]+ Cl- H
Slide 6
Ammonium salts Ammonium salts are released by the interaction of ammonia or water with acids. NH3 + HNO3 = NH4NO3 NH3H2O + HNO3 = NH4NO3 + H2O Ammonium salts interact with acids and other salts: (NH4)Cl + NaOH = NaCl + H2O + NH3 CONC. 2NH4Cl + H2SO4 = (NH4)2SO4 + 2HCl (NH4)2SO4 + BaCl2 = 2NH4Cl + BaSO4
Slide 7
All ammonium salts disintegrate when heated. (NH4)2CO3 = 2NH3 + H2O CO2 NH4NO2 = 2H2O + N2 NH4Cl NH3 + HCl (NH4)2Cr2O7 = Cr2O3 + 4H2O + N2 salts of lethal acids salts of oxidizing acids
Slide 8
A clear reaction to ion amonia. NH4+ + OH- H2O + NH3 Even more important is the power of ammonium salts and their interactions with plant species
Slide 9
Nitrogen oxides. Nitrogen dissolves six tarnished compounds. oxidation stage +1 N2O +2 NO +3 N2O3 +4 NO2, N2O4 +5 N2O5
Slide 10
N2O Removal: NH4NO = N2O +2H2O Chemical power: 1. expansion when heated 2N2+1O = 2N20+O2 2. with water N2+1O +H2 = N20 +H2O non-solidifying +1
Slide 11
NO +2 Extraction: 1. In nature: N2 + O2 = 2NO 2. In industry: 4NH3 + 5O2 = 4NO +6H2O Chemical properties: 1. easily oxidized: 2N+2O + O2 = 2N+4O2 2. oxidizing agent: 2N+ 2O + 2SO2 = 2SO3 + N20 non-solitary
Slide 12
N2O3 +3 Chemical power: NO2 + NO N2O3 Removal: ALL power of acid oxides. acid oxide
Slide 13
NO2 +4 Removal: 1. 2NO + O2 = 2NO2 2. Cu + 4HNO3(k) = Cu(NO3)2 + 2NO2 + 2H2O Chemical power: 1. with water 2NO2 + H2O = HNO3 + HNO2 2. with meadows 2NO2 + 2NaOH = NaNO3 + NaNO2 + H2O 3. dimerization 2NO2 N2O4 toxic
Slide 14
N2O5 +5 Removal: 1. 2NO2 + O3 = N2O5 + O2 2. 2HNO3 + P2O5 = 2HPO3 + N2O5 Chemical properties: 1. easily decomposed 2N2O5 = 4NO2 + O2 2. strong oxidizing acid oxide
Slide 15
Nitric acid. Trimming of nitric acid: KNO3 + H2SO4 = HNO3 + KHSO4 In the laboratory, with low heating: In industry, the process of stripping nitric acid can be divided into three stages: 1. Oxidation of ammonia on a platinum catalyst to NO: 4NH3 + 5O2 = 4NO +6H2O2. acidify NO to NO2: 2NO + O2 = 2NO2 3. Eliminate NO2 with water in the presence of excess acidity: 4NO2 + 2H2O + O2 = 4HNO3
Slide 16
HNO3 dilute concentrated meadows and meadows Fe, Su important metals NH4NO NH3 NO meadows and meadows important metals N2O NO2 Fe Cr Au Al Pt passive not mutually
Slide 17
Nitric acid is diluted. Concentrated nitric acid. Ag + 2HNO3 = AgNO3 + NO2 H2O 3Ag + 4HNO3 = 3AgNO3 + NO + 2H2O 4Zn + 10HNO3 (even dissolved) = 4Zn(NO3)2 + NH4NO3 + 3H2O
Slide 18
Nitric acid interacts with a lot of non-metals, oxidizing them to derivative acids: 3P + 5HNO3 + H2O = 3H3PO4 + 5NO C + 4HNO3 = CO2 + H2O + 4NO2
Slide 19
Nitrates are salts of nitric acid that are present in the presence of acids on metals, their oxides and hydroxides. Saltpeter is a salt of nitric acid and potassium metals. NaNO3 – sodium nitrate KNO3 – potassium nitrate NH4NO3 – ammonium nitrate Ca(NO3)2 – calcium nitrate Power: ALL the details of water.
Slide 20
When heated, nitrates decompose into visible acid (O2) t MeNO3 MeNO2 + O2 t MeNO3 MeO + NO2 + O2 t MeNO3 Me + NO2 + O2 before Mg before Mg before Pb after Cu
Slide 21
Saltpeter is praised as being kind. KNO3 is used for preparing black powder.
Slide 22
1 Ammonia for normal minds - this is... 1) barb-free, odorless gas 2) brown gas, which smells hot 3) bark-free, hot-smelling gas 4) bark-free liquid Tests: 2 No interaction with concentrated nitric acid... 1) Hg 2) Al 3 ) Cu 4) Zn 3 In industry, nitric acid is involved in the reaction: 1) NaNO3(K) + H2SO4(K) = NaHSO4 + HNO3 2) Ba(NO3)2 + H2SO4 = BaSO4 + 2HNO3 3) 4NO2 + O2 + 2H2O = 4HNO3 4) N2O5 + H2O = 2HNO3 4 Ammonium salts react with the meadows, so as with this ... 1) a weak base is created with ammonium hydroxide 2) ammonia gas is seen 3) a new salt is created 4) a weak base is created and the appearance gas flows 5 Level coefficient reactions Mg + HNO3 NO + … + H2O more advanced... 1)3 2)4 3)6 4)8 6 When the nitrate was added to the grinding, a white precipitate formed. This is good... 1) calcium nitrate 2) potassium nitrate 3) ammonium nitrate 4) sylvinite 7 weakest acids, formula HNO3 2) H2SiO3 3) H2SO3 4) H3PO4 8 nitric acid oxide... 1) N 2O 2) NO 3) NO2 4)N2O5 9 with overinsurance chemical elements The greatest electrical negativity among the connections is: 1) Be 2)B 3) S 4)N 10 add the phrase “saltpetre is …” I option
Slide 23
II option 1 nitric acid is a strong acid, as it is ... 1) completely dissociated in water 2) destroys the water 3) strong oxide 4) good in water 6 Possibly dissociated and water is mineral good ... 1) ammonium chloride 2) glue nitrate 3) sylvinite 4) superphosphate 4 ammonium salts mixed with water... 1) good, 2) bad, 3) non-essential 4) both, and non-substantial 3 ammonia is essential in industry t... 1) N2 + 3H2 2 O2 + 2H2O = 4hno3 3) n2o5 + h2o = 2hno3 4) nano3 (k) + h2SO4 (k) = nahso4 + HNO3 8 nitrogen acid oxide ... 1) n2o 2) no 3) no2 4) n2o 5 coefice in front of the vidnovnik formula equal reactions Zn + HNO3 N2O +… + H2O more advanced 1) 1 2) 2 3) 3 4) 4 2 minimum level of nitrogen oxidation connected… 1) N2 2) NO 3) NO2 4) HNO3 7 weakest h acids, formula any HNO3 2) H2SO4 3) H2CO3 4) H3SiO3 9 from over-contained chemical elements the greatest electronegativity in the compounds may be: 1) B 2)P 3) N 4)F 10 add the phrase “nitrates - tse...”
Slide 24
1. Liquidize the mixture with ammonia, which is required for extracting 200 kg of nitric acid with a mass fraction of HNO3 60%. When unraveling, swirl until the yield of the final product during synthesis reaches 80%. Instructions: 2. When heated sodium nitrate, 280 ml of sour water is created (normal washing). Yakka salt knew the layout. 3. Dissolve the mixture with calcium(II) hydroxide, which can be neutralized with 630 g of nitric acid, in which the mass fraction of HNO3 is 20%. weight 300 g. Calculate the mass fraction of ammonium nitrate. 5. At the sum of 75 g of copper and copper (II) oxide, excess HNO3 (concentrated) was added. In this case, gas was released with a volume of 26.88 liters (normal volume). Determine the mass fraction of copper(II) oxide from the output mixture. 6. Ammonia with a volume of 7.84 liters (normal concentrations) was subject to catalytic oxidation and subsequent conversion to nitric acid. As a result, they won a massacre of 200g. If the yield of HNO3 is equal to 40%, calculate the mass fraction in the extracted mixture.
"Oxide of carbon dioxide IV" - Nezabar water will become calamut. Physical power of CO2. Dry ice, separated from water ice, thick. Non-toxic, do not carry out electric shock. Zastosuvannya to carbon oxide (IV). Dry ice is also CO2. Gas necessary for photosynthesis. In nature. The amount of carbon dioxide in the atmosphere is quite small, 0.04 - 0.03.
“Nitrogen oxide” - 2. The cylinder containing nitrogen (II) oxide is closed with a plate. Oxidation: 2NO + 2SO2 = 2SO3 + N2 Nitrogenous method of containing sulfuric acid. 1. Three closed cylinders: with nitrogen (IV) oxide, with nitrogen, with ammonia. No-nitrogen oxide (II). It’s good to break up near the water. N2O5. All nitrogen oxides, including N2O, are pure substances.
“Classification of oxides” - Classification of oxides. Basic oxides. Oxide. Amphoteric oxides. Acid oxides. Glossary. Indifferent oxides (non-salt-soluble). Classif. Zmіst. Zavdannya. Help for students.
“Oxide” – from nature. Metal ores. CHROME OXIDE cr2o3. The amount of carbon dioxide in the atmosphere is very small, only 0.04-0.03%. Bilila. For example: red, magnetic and brown weeds, bauxite (aluminum oxide), gas needed by plants for photosynthesis. Carbon dioxide (II) CO. Titanium (IV) oxide – TiO2 – has the same valuable properties.
"Carbon Oxide" - Carbon oxide (II) is characterized by strong power. Or carbon dioxide is a gas without color or odor. H. Carbon dioxide (II). Carbon oxide (IV). Obsession with carbon oxide (IV). Vikoristani TsOR: Demonstration planning. Oxide carbon.
“Chemical oxides” are words that are in storage. Quartz sand. H2O. Carbon oxide (IV). Oxides are complex words. Boxing. Olive-green Farby pigment. Quicklime is important. Metal oxides. Oxide. Carbon dioxide (II).
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