Presentation of nitric acid salt. Presentation on the topic "nitric acid and its salts." Effect on the body

To use presentation previews, create an account for yourself ( account) Google and log in: https://accounts.google.com

Slide captions:

Lesson on the topic “Nitric acid” 9th grade Chemistry teacher: Matyushkina T.S.

In the lesson we will: -continue to study nitrogen compounds -look in detail at the properties of HNO 3 -we will improve our skills in writing reaction equations -learn about the areas practical application HNO 3 and its salts

Chemical warm-up: 1. Formula of ammonia: a) NH 2 b) NH 4 c) NH 3 d) N 2 2. Ammonia: a) lighter than air, b) heavier than air, c) neither lighter nor heavier 3. Ammonia is: a) an oxidizing agent, b) a reducing agent, c) both. 4. Ammonium ion a) NH 2 + b) NH 4 + c) NH 3 – d) NH 3 5. The electron donor during the formation of the ammonium ion is a) nitrogen atom, b) hydrogen ion, c) ammonium ion 6. Oxidation state nitrogen in ammonia: a)0, b)-3, 4)+3, 5)8

Chemical warm-up Determine the oxidation state of nitrogen in each oxide

Nitric acid HNO 3 is one of the most powerful acids. Physical properties: - colorless liquid - “smoke” in air, t boil = 84 o C, t pl = -42 o C -in the light turns yellow due to the release of NO 2: 4HNO 3 = 2H 2 O +4NO 2 + O 2

Obtaining HNO 3

Chemical properties Typical properties of acids

Chemical properties Reacts particularly with metals:

Chemical properties: Interaction with non-metals

For the curious:

Application of HNO 3 -c salts agriculture-for dyeing fabrics -in medicine -in pyrotechnics

Check yourself: The degree of oxidation of nitrogen in HNO 3 a) -3 b)0 c)+5 d)+4 When stored in the light, HNO 3 a) turns red b) turns yellow c) remains colorless Nitric acid is: a) an oxidizing agent, b) reducing agent, c) both. Does HNO 3 exhibit properties common to other acids? a) yes b) no c) depends on the weather Aqua regia is a) concentrated alcohol b) 3 volumes of HCl and 1 volume of HNO 3 c) concentrated nitric acid

Complete the sentences: -today in class I learned... -I practiced... -I saw...

Homework: Learn the theory: pp. 118-121 Exercises 2, 3,4 p. 121

On the topic: methodological developments, presentations and notes

Klochkova Violetta Mikhailovna, chemistry teacher, Secondary School No. 2 named after I. I. Tarasenko senior Settlements of the Krasnodar Territory....

Summary of a combined lesson on the topic "Nitric acid". This lesson discusses the physical, general and specific properties, laboratory and industrial methods for producing nitric acid...

Kirillova

Margarita Alekseevna

Chemistry teacher at Lyceum No. 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.

Mixes 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

depend on activity

metal and dilution

nitric acid.

HNO3(conc)+ content

II. Nitric acid is a strong oxidizing agent

Al, Fe, Co, Ni, Cr do not interact without heating

HNO3(conc)+ content

K, Ca, Na, Mg, Zn…

4HNO3(conc) + Hg = Hg(NO3)2 + 2NO2 + 2H2O

4Zn + 10HNO3(dil)= 4Zn(NO3)2 + NH4NO3 + 3H2O

3Cu + 8HNO3(dil) = 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) =

P + 5HNO3(conc) = H3PO4 + 5NO2 + H2O

Oxidation of non-metals and organic

C + 4HNO3(conc) = 4NO2 + CO2 + 2H2O

Organic substances are 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

Ammonium nitrate decomposition:

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

fertilizers

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 reveal their practical significance for plants and humans....

1 slide

Salts of nitric acid, application Lesson motto “Au, Na, Ar, Ne, It, Eu – Os, Ra, U, Db, In, Er, As Ni, Es C, Eu La b” L. N. Tolstoy

2 slide

know and be able to name salts of nitric acid, determine what oxidative or reducing properties are characteristic of them; determine: the degree of oxidation of chemical elements in salt formulas; the types of chemical reactions in which they can participate; characterize: general chemical properties of nitric acid salts;

3 slide

Game “Tic-Tac-Toe” A solution of nitric acid reacts with each of the substances. MgO Al P2O5 KCl CO2 CaCO3 Al2O3 K2SiO3 Zn

4 slide

What classes of inorganic substances do these substances belong to? 1. Name the salts - the products of these reactions. 2. Write down the molecular equations for the reactions producing nitrates in your notebook. MgO Al P2O5 KCl CO2 CaCO3 Al2O3 K2SiO3 Zn

5 slide

Complete the reaction equations and explain which classes of compounds can produce nitrates when interacting. BaO + HNO3 → BaO + N2O5 → Ba(NO3)2 + Na2SO4 →

6 slide

Given pairs of substances, create 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 reactions are impossible and why?

7 slide

List the salts obtained as a result of possible reactions. Potassium, sodium, calcium and ammonium nitrates are called nitrates KNO3 - potassium nitrate (Indian nitrate), NaNO3 - sodium nitrate (Chilean nitrate), Ca(NO3)2 - calcium nitrate (Norwegian nitrate) NH4NO3 - ammonium nitrate (ammonium or ammonium nitrate, there are no deposits of it in nature). German industry is considered the first in the world to produce NH4NO3 salt from nitrogen N2 in air and hydrogen in water, suitable for plant nutrition.

8 slide

Nitrates are solid crystalline substances, refractory, determine from the solubility table which electrolytes they belong to - strong or weak?

Slide 9

Physical properties of nitrates What substances are called salts? It is necessary to build a logical chain: type of chemical bond - type of crystal lattice - interaction forces between particles at lattice nodes - physical properties of substances.

10 slide

Chemical properties of nitrates Interaction of nitrates with metals, acids, alkalis, salts Cu(NO3)2 + Zn..., AgNO3 + HCl..., Cu(NO3)2 + NaOH..., AgNO3 + BaCl2....

11 slide

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 stand, a test tube with sodium nitrate, and an alcohol lamp. Knowing that the decomposition of many salts produces gas, the inquisitive chemist prepared a torch, litmus paper 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?

12 slide

To use presentation previews, create a Google account and log in to it: https://accounts.google.com

Slide captions:

and not one vessel can hold more than its capacity, except 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 gunpowder based on it. Determine the molecular formula of a substance if it contains 38.61% potassium, 13.86% nitrogen and oxygen.

Nitric acid salts

Nomenclature of salts Nitrates: Ba (NO₃)₂ , AgNO ₃ , Zn(NO₃)₂ , NaNO ₃ Nitrates: NaNO ₃ , KNO₃ , Ca(NO₃)₂ , NH₄NO₃

Structure and physical properties of nitrates Type of chemical bond - ionic Type of crystal lattice - ionic State of aggregation - crystalline solids Solubility in water - most soluble

Chemical properties common to 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 rather turn into nitrite!” And metals from the company from magnesium to copper, Zinc, iron and their other neighbors Carefully and calmly, without offense, their oxide is extracted from nitrate. Well, what about silver and mercury? Metals that consider themselves noble wish to become completely, completely free.

Special properties of nitrates Qualitative reaction to NO₃⁻ NaNO ₃ + Cu + H₂SO₄

Nitrates: pros and cons

Name of plant Recommendations for use Patisson It is better to cut off the upper part adjacent to the stalk Cucumber Peel the cucumber and cut off the tail Cabbage Remove the upper covering leaves and throw away the stalk Zucchini Cut off the skin Beets Cut off the upper and lower parts of the root vegetable Potatoes Pour 1% water over the peeled potatoes 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 plant productive organs.

On the topic: methodological developments, presentations and notes

This lesson is considered first in the section “ Computer presentations" In this lesson, students become familiar with POWERPOINT program, learn to change the design and layout of slides....

Presentation "Use of multimedia presentations as a universal means of cognition"

In the presentation "Using multimedia presentations as a universal means of cognition" provides advice on the design and content of presentations....

Development of a lesson and presentation "The Sightseeng Tours" London and Saint-Petersburg with presentation

Goals: development of speech skills (monologue statement); improving grammatical reading and speaking skills (past indefinite tense, definite article) Objectives: teach...

Presentation "Recommendations for creating multimedia presentations"

Slide 2

This substance was described by the Arab chemist in the 8th century Jabir ibn Hayyan (Geber) in his work “The Coachman of Wisdom”, and since the 15th century this substance has been extracted for industrial purposes - Thanks to this substance, the Russian scientist V.F. Petrushevsky first received dynamite in 1866. This substance is a component of rocket fuel, it was used for the engine of the world's first Soviet jet aircraft, BI-1. This substance is the progenitor of most explosives (for example, TNT, or tola) - This substance, mixed with hydrochloric acid, dissolves platinum and gold, recognized “ king of metals. The mixture itself, consisting of 1 volume of this substance and 3 volumes of hydrochloric acid, is called “aqua regia”.

Slide 3

Her Majesty Nitric acid Yakonyuk Vera Sergeevna chemistry teacher Znamenskaya Secondary School Chemistry lesson 9th grade

Slide 4

Slide 5

Alchemists were the first to obtain nitric acid by heating a mixture of saltpeter and ferrous sulfate: 4KNO3 + 2(FeSO4 7H2O) (t°) → Fe2O3 + 2K2SO4 + 2HNO3 + NO2 + 13H2O Pure nitric acid was first obtained by Johann Rudolf Glauber by acting on saltpeter with concentrated sulfuric acid : KNO3 + H2SO4 (conc.) (t°) → KHSO4 + HNO3 By further distillation the so-called “fuming nitric acid”, practically free of water Historical background

Slide 6

It has been experimentally proven that the double bond is evenly distributed between two oxygen atoms. The oxidation state of nitrogen in nitric acid is +5, and the valency (note) is four, because there are only four common electron pairs. The bond is covalent polar. Crystal lattice - molecular structure

Slide 7

Obtaining HNO 3 Laboratory method of obtaining: NaNO3 + H2SO4 t NaHSO4 + HNO3 this produces fuming nitric acid

Slide 8

Industrial method 1. Oxidation of ammonia to NO in the presence of a platinum-rhodium catalyst: 4NH3 + 5O2 = 4NO + 6H2O 3. Absorption of NO2 by water in the presence of oxygen: 4NO2 + 2H2O + O2 = 4HNO3 The mass fraction of HNO3 is about 60% 2. Oxidation of NO in NO2 in the cold under pressure (10 atm): 2NO + O2 = 2NO2

Slide 9

Physical properties Physical properties colorless liquid tmp=-41.60C tbp=82.60C indefinitely miscible with water volatile - “smoke” in air Conc. nitric acid is usually yellow in color

Slide 10

Research (tasks in groups): (Repetition of PTB!). Group 1: carry out the reaction of a solution of nitric acid and copper (II) oxide, write down the reaction equation, determine its type; Group 2: obtain the insoluble base Cu(OH)2; carry out the reaction of a solution of nitric acid and copper (II) hydroxide; write down the reaction equation, determine its type Group 3: carry out the reaction of solutions of nitric acid and sodium carbonate, write down the reaction equation, determine its type For everyone: carry out the reaction of solutions of nitric acid and potassium hydroxide in the presence of phenolphthalein, write down the reaction equation, determine its type

Slide 11

Group No. 1 CuO + 2 HNO3 = Cu(NO3)2 + H2O - ion exchange reaction, irreversible CuO + 2H+ + 2 NO3- = Cu2+ + 2 NO3- + H2O CuO + 2H+ = Cu2+ + H2O Group No. 2 CuCl2 + 2 NaOH = Cu(OH)2↓ + 2 NaCl (obtaining an insoluble base) Cu(OH)2 ↓+ 2 HNO3 = Cu(NO3)2 + 2 H2O - ion exchange reaction, irreversible Cu(OH)2 ↓ + 2H+ + 2 NO3 - = Cu2+ + 2 NO3- + 2 H2O Cu(OH)2↓ + 2H+ = Cu2+ + 2 H2O Sign of the reaction – dissolution of the blue precipitate Cu(OH)2 Group No. 3 2 HNO3 + Na2CO3 = 2 NaNO3 + H2O + CO2 - reaction ion exchange, irreversible 2 H+ + 2NO3- + 2 Na+ + CO32- = 2 Na+ +NO3- + H2O + CO2 2 H+ + CO32- = H2O + CO2 A sign of the reaction is a characteristic “boiling.”

Slide 12

Common with other acids: 1. Strong electrolyte, dissociate well into ions HNO3 -> H+ +NO3- Changes the color of the indicator. 2. Reacts with basic oxides CuO+2 HNO3 -> Cu(NO3)2 +H2O 3. Reacts with bases HNO3 + KOH -> KNO3 + H2O 4. Reacts with salts of more volatile acids Na2CO3 + 2HNO3 -> 2NaNO3 +H2CO3 dry / \H2OCO2

Slide 13

Specific: When heated and exposed to light, it decomposes 4HNO3 = 2H2O + 4NO2 + O2 Reacts with non-metals C + 4HNO3(conc.) = CO2 + 4NO2 + 2H2O S+6HNO3(60%) =H2SO4+6NO2+2H2O S+2HNO3(40 %) =H2SO4+2NO P+5HNO3(60%) =H3PO4+5NO2+ H2O P+5HNO3(30%)+2H2O =3H3PO4+5NO NOHeMe + HNO3NO2. Nitric acid oxidizes nonmetals

Slide 14

The interaction of nitric acid with metals has been studied quite well, because conc. HNO3 is used as a rocket fuel oxidizer. The point is that the reaction products depend on two factors: 1) the concentration of nitric acid; 2) the activity of the metal. The composition of the reaction products is determined by the combination of these two parameters. What could it be? a) the metal may or may not react ( do not react at all, passivate); b) the composition of gases is mixed (as a rule, not one gaseous product is released, but a mixture of gases, sometimes one gas predominates over others); c) usually hydrogen is not released in these processes (there is an exception when practice has proven that Mn + diluted HNO3 actually releases hydrogen gas) The main rule: The more active the metal and the more dilute the nitric acid, the deeper the reduction of nitric acid goes (the extreme option is reduction to ammonia NH3, more precisely to NH4NO3; here the process of reduction of N( +5) + 8e ----> N(-3)). Intermediate options for reduction to NO2, NO, N2O, N2 are possible. General process scheme: HNO3 + Me ---> nitric acid salt (nitrate) + nitric acid reduction product + H2O

Slide 15

Interaction with metals: When interacting with metals, nitrate, water and a third product are formed according to the scheme: HNO3 (s.) + Me (before H2) → nitrate + H2O + NH3 (NH4NO3) HNO3 (s.) + Me (after H2) → nitrate+H2O+NO HNO3(c.)+Me(before H2)→nitrate+H2O+N2O(N2) HNO3(c.)+Me(after H2)→nitrate+H2O+NO2 Concentrated HNO3 on Al, Cr, Fe, Au, Pt has no effect.

Slide 16

P.S concentrated HNO3 >60% dilute HNO3 = 30-60% very dilute HNO3

Slide 17

Application of Nitric Acid:

Production of nitrogen and combined fertilizers, -explosives (trinitrotoluene, etc.), -organic dyes. -as a rocket fuel oxidizer. - In metallurgy, nitric acid is used for etching and dissolving metals, as well as for separating gold and silver.

Slide 18

Effect on the body

Inhalation of nitric acid vapors leads to poisoning; contact of nitric acid (especially concentrated) on the skin causes burns. The maximum permissible content of Nitric acid in the air of industrial premises is 50 mg/m3 in terms of N2O5 Concentrated Nitric acid in contact with organic substances causes fires and explosions

Slide 19

Check yourself:

Oxidation degree of nitrogen in HNO3 a) -3 b)0 c)+5 d)+4 When stored in the light, HNO3 a) turns red b) turns yellow c) remains colorless When interacting with metals, nitric acid is: a) an oxidizing agent, b) a reducing agent , c) both. Nitric acid in solution does not react with a substance whose formula is: a) CO2; b) NaOH; c) Al(OH)3; d) NH3. Aqua regia is a) concentrated alcohol b) 3 volumes of HCl and 1 volume of HNO3 c) concentrated nitric acid

Slide 20

key

1 - c 2 - b 3 - a 4 - a 5 - b

Slide 21

conclusion:

1. Nitric acid is characterized general properties acids: reaction to an indicator, interaction with metal oxides, hydroxides, salts of weaker acids due to the presence of H+ ion in the molecules; 2. The strong oxidizing properties of nitric acid are due to the structure of its molecule; When it interacts with metals, hydrogen is never formed, but nitrates, nitrogen oxides or other nitrogen compounds (nitrogen, ammonium nitrate) and water are formed, depending on the concentration of the acid and the activity of the metal; 3. The strong oxidizing ability of HNO3 is widely used to produce various important products of the national economy (fertilizers, medicines, plastics, etc.)

Slide 22

Homework:

§26 exercise 4.5 Creative task – presentation of the history of the discovery of nitric acid. Application of nitric acid

Slide 23

Thank you for the lesson

Slide 24

literature

O.S. Gabrielyan, I.G. Ostroumov Desk book 9th grade chemistry teacher. Bustard 2003 Lidin R.A., Molochko V.A., Andreeva L.L. Chemical properties of inorganic substances Khimiya2000 http://ru.wikipedia.org/wiki/HNO3http://centralnyj.fis.ru/Petrochemicalshttp://dic.academic.ru/dic.nsf/bse/61981/%D0%90% D0%B7%D0%BE%D1

View all slides

It might be useful to read: