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Salts of nitric acid, application The motto of the lesson "Au, Na, Ar, Ne, It, Eu - Os, Ra, U, Db, In, Er, As Ni, Es C, Eu La b" L. N. Tolstoy
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know and be able to name salts of nitric acid, determine what oxidizing or reducing properties are characteristic of them; determine: the degree of oxidation of chemical elements in the formulas of salts; types of chemical reactions in which they can participate; characterize: general chemical properties of nitric acid salts;
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tic-tac-toe game A solution of nitric acid reacts with each of the substances. MgO Al P2O5 KCl CO2 CaCO3 Al2O3 K2SiO3 Zn
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What class of inorganic substances do these substances belong to? 1. Name the salts - the products of these reactions 2. Make in your notebook the molecular equations for the reactions of obtaining nitrates. MgO Al P2O5 KCl CO2 CaCO3 Al2O3 K2SiO3 Zn
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Complete the reaction equations and explain which classes of compounds can give nitrates when interacting. BaO + HNO3 → BaO + N2O5 → Ba(NO3)2 + Na2SO4 →
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Pairs of substances are given, make possible reaction equations a) sodium hydroxide and Nitric acid, b) potassium hydroxide and nitric oxide (V), c) calcium oxide and nitric acid, d) ammonia and nitric acid, e) barium sulfate and calcium nitrate, f) sodium chloride and barium nitrate Which of the reactions are impossible and why?
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List the salts obtained as a result of possible reactions. Potassium, sodium, calcium and ammonium nitrates are called saltpeters KNO3 - potassium nitrate (Indian saltpeter), NaNO3 - sodium nitrate (Chilean saltpeter), Ca (NO3) 2 - calcium nitrate (Norwegian saltpeter) NH4NO3 - ammonium nitrate (ammonium or ammonium nitrate, there are no deposits of it in nature). The German industry is considered the first in the world to obtain the salt NH4NO3 from nitrogen N2 in the air and hydrogen in water, suitable for plant nutrition.
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Nitrates are solid crystalline substances, refractory, determine from the solubility table which electrolytes they belong to - strong or weak?
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Physical properties of nitrates What substances are called salts? It is necessary to build a logical chain: the type of chemical bond - the type of crystal lattice - the forces of interaction between particles at the lattice nodes - physical properties substances.
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Chemical properties of nitrates Interaction of nitrates with metals, acids, alkalis, salts Cu(NO3)2 + Zn … , AgNO3 + HCl … , Cu(NO3)2 + NaOH … , AgNO3 + BaCl2 … .
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An interesting story An inquisitive chemist studied the types of chemical reactions and noticed that insoluble carbonates (CaCO3), sulfites (CaSO3), silicates (CaSiO3), some sulfates (FeSO4) decompose when heated. He set himself the task of determining whether nitrates would decompose. For the experiment, he took a laboratory tripod, a test tube with sodium nitrate, and an alcohol lamp. Knowing that gas is formed during the decomposition of many salts, an inquisitive chemist prepared a torch, litmus test and lime water (Ca (OH) 2). When the salt heated up and melted, he lowered a smoldering splinter into the test tube, it suddenly flared up. What conclusions did the young chemist come to?
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Salts of nitric acid. What are the salts of nitric acid called? Nitrates. Nitrates K, Na, NH4+ are called saltpeters. KNO3. NaNO3. NH4NO3. Nitrates are white crystalline substances. Strong electrolytes, in solutions completely dissociate into ions. They enter into exchange reactions. How can you determine the nitrate ion in solution? Sulfuric acid and copper are added to the salt (containing the nitrate ion). The mixture is slightly heated. Emission of brown gas (NO2) indicates the presence of the nitrate ion. Write the formulas for the listed salts.
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“Carbonic acid and its salts” - Correct answers: 1st option - 1, 2, 3, 4, 8, 10 Option 2 - 3, 5, 6, 7, 9, 10. What carbon oxides are mentioned in the following statements? Enter in the diagram. What phenomenon are we talking about? Very toxic Does not burn and does not support combustion Used in metallurgy for iron smelting Formed by complete combustion of fuel Magnesium burns in it Typical acidic oxide.
"Fatty acids" - Lipid extracts. n-6. 2. Arachidonic acid and other polyenes fatty acid as signaling molecules. Polyunsaturated fatty acids as signal molecules. Since 1978 S.D. Varfolomeev, A.T. Mevkh, G.F. Sud'ina, P.V. Vrzheshch et al. 1. PGE2. A. TxA2 PGI2 PGE2 PGF2a PGD2. Platelets: [AA]o = 5 mM 1% - 50 mM (w) Leukocytes: 0.1-1 mM (w) Islets of Langerhans: 15 mM (w) [AA]excl = 1-10 mM DHA~50% cells brain.
"Physical and chemical properties of acids" - 1. According to the oxygen content. 2. By the number of hydrogen atoms. You kept a test tube over your trousers With acid? Нn+1 (KO)-n. Hydrochloric acid. Sulfuric acid. Single-basic hcl HNO3. Acids. Phosphoric acid. HCI H2SO4 H3PO4 HNO3 H2S HNO2 H2SO3 H2CO3 H2sio4. Nitrous acid. Carbonic acid. The harm of acids.
"Sulfuric acid lesson" - How diluted acid interacts sulphuric acid with metals? Negative impact on the environment. "What are the special properties of concentrated sulfuric acid? Lesson motto: What indicators can detect acids? Acid rain. What are the general properties of acids characteristic of sulfuric acid? Lesson goal:
"Production of sulfuric acid" - Cleaning from coarse dust. Production technology. III stage. Cleaning of fine dust Grid positively charged Wire negatively. 2 SO2(g) + O2(g) ? 2 SO3(g) + Q Compounds Exothermic Homogeneous Catalytic Reversible Redox. II stage. In the contact apparatus, shelves with V2O5 catalyst.
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n and one vessel does not contain more than its volume, except for the vessel of knowledge; it is constantly expanding. Arabic proverb
This substance is called "Chinese snow" in Europe; in 808, the Chinese alchemist Qin invented black powder based on it. Determine the molecular formula of a substance if it contains 38.61% potassium, 13.86% nitrogen and oxygen.
Salts of nitric acid
Salt nomenclature Nitrates: Ba (NO₃)₂ , AgNO ₃ , Zn(NO₃)₂ , NaNO ₃ Saltpeters: NaNO ₃ , KNO₃ , Ca(NO₃)₂ , NH₄NO₃
The structure and physical properties of nitrates Type of chemical bond - ionic Type of crystal lattice - ionic Aggregate state - solid crystalline substances Solubility in water - most soluble
Chemical properties common with other salts Electrolytes Reactions with acids Ba (NO₃)₂ + H₂SO₄ with alkalis Fe(NO₃)₃ + NaOH with salts AgNO ₃ + BaCl ₂ with metals Cu(NO₃)₂ + Fe
Special properties of nitrates Thermal decomposition Without wasting time, Let's figure out how nitrates decompose in the stove. What happens? The alkali metal is so active, He says in a commanding tone: “Being a nitrate is so disgusting. I’d better turn into nitrite!” And metals from the company from magnesium to copper, Zinc, iron and their other neighbors Carefully and calmly, without offense, Extract their oxide from nitrate. But what about silver and mercury? Metals that consider themselves noble, Desire to become very, very free.
Special properties of nitrates Qualitative reaction to NO₃⁻ NaNO ₃ + Cu + H₂SO₄
Nitrates: pros and cons
Plant name Recommendations for use Patisson It is better to cut off the upper part adjacent to the stalk Cucumber Peel the cucumber from the skin and cut off the tail Cabbage Remove the upper covering leaves and discard the stalk Zucchini Cut off the skin Beetroot Cut off the upper and lower parts of the root Potato Peeled potatoes pour 1% for a day table salt or ascorbic acid Carrots Cut off the top and bottom of the root vegetable Table. Accumulation of nitrates in various parts of the productive organs of plants.
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Kirillov
Margarita Alekseevna
chemistry teacher of lyceum № 369
Krasnoselsky district
The nitrogen atom has three unpaired p-electrons on the outer layer, due to which it forms three σ-bonds with oxygen atoms. Due to the lone electron pair, a fourth covalent bond is formed. electronic cloud
delocalized between
two oxygen atoms.
Valence - IV
Oxidation state -5
Colorless liquid, fuming
on air.
Acrid smell.
yellow color concentrated
acids (decomposition to form
NO2). 4HNO3 = 4NO2 + 2H2O + O2
Density 1.52 g/cm3.
Boiling point - 860C.
Solidification temperature - -41.60C.
Hygroscopic.
Miscible with water in any
ratios.
Dilute nitric acid exhibits properties common to all acids:
Dissociation in aqueous solution:
HNO3 → H++NO3-
Reaction with bases:
NaOH + HNO3 = NaNO3 + H2O
Cu(OH)2 + 2HNO3 = Cu(NO3)2 + 2H2O
Reaction with basic oxides:
CaO + 2HNO3 = Ca(NO3)2 + H2O
Reaction with salts:
Na2CO3 + 2HNO3 = 2NaNO3 + H2O + CO2
Metal oxidation:
Recovery Products
activity dependent
metal and dilution
nitric acid.
HNO3 (conc) + v-l
II. Nitric acid is a strong oxidizing agent
Al, Fe, Co, Ni, Cr do not interact without heating
HNO3 (conc) + v-l
K, Ca, Na, Mg, Zn…
K, Ca, Na, Mg, Zn…
4HNO3(conc) + Hg = Hg(NO3)2 + 2NO2 + 2H2O
4Zn + 10HNO3(razb)= 4Zn(NO3)2 + NH4NO3 + 3H2O
3Cu + 8HNO3(razb) = 3Cu(NO3)2 + 2NO + 4H2O
Cu + 4HNO3(conc) = Cu(NO3)2 + 2NO2 + 2H2O
Zn + 4HNO3(conc) = Zn(NO3)2 + 2NO2 + 2H2O
Al + HNO3(conc) =
Fe+ HNO3(conc) =
Р + 5HNO3 (conc) = H3PO4 + 5NO2 + H2O
Oxidation of non-metals and organic
C + 4HNO3(conc) = 4NO2 + CO2 + 2H2O
Organic matter is oxidized
and ignite in nitric acid.
In industry - oxidation
4NH3 + 5O2 = 4NO + 6H2O
4NO2 + O2 + 2H2O = 4HNO3
In the laboratory - interaction
potassium or sodium nitrate with
concentrated sulfuric acid
when heated:
KNO3 + H2SO4 = HNO3 + KHSO4
Obtained by the interaction of nitric acid with metals, metal oxides, bases,
ammonia and some salts.
physical properties. These are solid crystalline substances, highly soluble in water.
Chemical properties. strong electrolytes,
exhibit all the properties of salts.
NaNO3 Na+ + NO3-
Cu(NO3)2 + 2KOH = Cu(OH)2↓ + 2KNO3
AgNO3 + NaCl = AgCl↓ + NaNO3
Pb(NO3)2 + Zn = Pb + Zn(NO3)2
Ba(NO3)2 + H2SO4 = BaSO4↓ + 2HNO3
MexOy + NO2 + O2
2KNO3 = 2KNO2 + O2
2Cu(NO3)2 = 2CuO + 4NO2 + O2
2AgNO3 = 2Ag + 2NO2 + O2
Decomposition of ammonium nitrate:
NH4NO3 = N2O + 2H2O
NaNO3 + H2SO4 = NaHSO4 + HNO3
4HNO3 + Cu = Cu(NO3)2 + 2NO2 + 2H2O
brown gas
solid nitrates. a pinch of salt
throw burners into the fire.
There is a bright flash.
dyes
medicines
fertilizer
plastic
pyrotechnics
explosive
substances
HNO3 and nitrates
On the topic: methodological developments, presentations and notes
The lesson has a pronounced practical orientation. Students conduct a chemical experiment, study the properties of nitrates and discover them practical value for plants and humans....