Inorganic chemistry in the reactions of deryabin. Inorganic chemistry in exercises and tasks. Books that shaped my inner world

You are the masterpiece of your own life, you are the Michelangelo of your life. The David you are sculpting is yourself. All that is required of you is to take a step forward and move in the direction in which the inner force pushes you.

Dr. Joe Vitale

Promise yourself

Be very strong so that nothing can disturb your peace of mind.

Wish health, happiness and prosperity to every person you meet on your way.

Make each of your friends feel that there is something special about them.

Look for the bright side in any event and make your optimism a reality.

Think only of the best, work only for the best, and expect only the best.

To perceive the success of others with no less joy than your own.

Forget about the mistakes of the past and focus on great achievements in the future.

Always keep a happy expression on your face and give a smile to everyone and everyone.

Devote so much time to your own improvement that it is not left for criticism of others.

To be too free to worry, too generous to be angry, too strong to be afraid, and too happy to be in trouble.

It is good to think about yourself and demonstrate this fact to the world, but not with loud words, impressive deeds.

Believe that the whole world is on your side as long as you are true to your best self.

About myself

Pedagogical experience 33 years, teacher of chemistry of the highest category. My family is a husband and two daughters, a grandson.

Books that shaped my inner world

Eleanor Porter "Pollyanna", Joe Vitale "Secret of attraction. How to get what you really want", "Key. Turn it and reveal the secret of attraction", Daily Carnegie How to stop worrying and start living, Anatoly Nekrasov "Mother's love", " 1000 and one way to be yourself", "Learning to love".

My view of the world

LIFE is an opportunity - use it.
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LIFE, this is grief - overcome it.
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LIFE is happiness - create it.
LIFE is too beautiful - don't ruin it.
LIFE is life - fight for it.

My achievements

Diploma of the Ministry of Education of the Moscow Region for many years of fruitful work, successful work in teaching and educating students, the victories of my students at olympiads, scientific and practical conferences, the orientation of my students to healthy lifestyle life.

My portfolio

Anyone who has taken seriously scientific activity, understands that the words "You must believe" are written above the entrance to the temple of science.

Our faith and our beliefs are conditioned by our personal experience rather than external causes.

You can achieve absolutely everything - even what seems impossible to you.

It is in your power to change your thoughts.

You are not the master of the Earth, but you have much more power than you can imagine.

transcript

1 DERYABINA N.E. INORGANIC CHEMISTRY IN EXERCISES AND TASKS Tutorial class pupils high school IPO "At the Nikitsky Gate" Moscow 2012

2 UDC 546 LBC 24.1 D36 D36 Deryabina N.E. Inorganic chemistry in exercises and tasks. - M.: IPO "At the Nikitsky Gates", 2012, - 32 p. ISBN The manual is a collection of exercises and tasks on the most important section of inorganic chemistry, the main classes inorganic compounds. Included with the Inorganic Chemistry in Reactions mini-guidebook to help students complete the suggested exercises. Recommended for secondary school students (basic level). ISBN Deryabina N.E., 2012

3 1. CLASSIFICATION OF INORGANIC SUBSTANCES 1.1. METALS AND NON-METALS 1. In the periodic table shown on the cover, fill in yellow the cells with non-metal elements. 2. Underline the symbols of non-metals: N, Na, Ne, H, Hf, He, B, Ba, Br, S, Sr, Si, Se, Os, O, C, Cs, Cd, Cl, Cu, Fr, F, Al, At, Ar, As, Ag. Write down the symbols: a) alkali metals; b) alkaline earth metals (see the list of group names of chemical elements on page 9 of the mini-reference book "Inorganic chemistry in reactions"). 3. Write down one symbol of a metal element and a non-metal element that are in the periodic table: a) side by side; b) in one group; c) in one subgroup; d) in one period. 4. The symbols of which metal element and non-metal element consist of the same letters? 5. Write down the symbols: a) non-metals with constant s.d. ; b) metals with constant s.d. 6. Which metal forms a simple substance: a) red; b) yellow; c) liquid at n.o.s.? What non-metal forms at n.s.: a) a gaseous toxic simple substance of a yellow-green color; b) a simple substance in the form of purple crystals with a metallic sheen; c) a simple substance in the form of solid transparent crystals capable of cutting glass? 7. Two students played chemical tic-tac-toe. The first wrote down the symbols of metals in the cells, the second non-metals (according to the rules of the game, the elements do not repeat). Which of them won? N Na Zn Cl Hg Ge O He Al Si S Sr Pb Ca F Te Br Te N Fe Co Br Se Rb As Ar Cs Ba Sn Ag Au C 3

4 1.2. OXIDES, HYDROXIDES, SALTS 8. Find errors in the definition: "Oxides are complex substances consisting of two elements, one of which is oxygen." What essential features of the concept of "oxides" are not indicated in the definition? What features can be removed from the definition? Write the correct definition. Oxides - 9. Underline the formulas of oxides: H 2 O, CO, O 2, H-O-H, As +3 2O 3, H-O-O-H, P 2 O 5, P 2 O 3, O 3, SO 2, OF 2, I 2 O 7, HClO, SO 3, KO 2, KO 3, P 4 O 6, P 4 O 10, H 2 CO, XO 2, XO 2-2, XO -1 2, XO , X 2 O. 10. Complete the scheme for the classification of oxides (see the mini-reference book "Inorganic chemistry in reactions", p. 1). Non-metal oxide Metal oxide in the oxidation state +2 others non-salt-forming oxide acidic amphoteric basic salt-forming oxide Can metal atoms form oxides: a) non-salt-forming; b) acid; amphoteric? 2. Can atoms of non-metals form oxides: a) amphoteric; b) basic; c) non-salt-forming? 3. Can XO 2 oxide be: a) acidic; b) amphoteric; c) main; non-salt-forming? 4. Can the oxide X 2 O 3 be: a) acidic; b) amphoteric; c) main; non-salt-forming? Check yourself the number of positive answers in the whole exercise should be equal Make formulas and sign the nature of oxides: a) nitrogen (s.o. +1, +2, +3, +5); b) chlorine (s.d. +1, +3, +5, +7); 4

5 2. CHEMICAL PROPERTIES OF SOME CLASSES OF INORGANIC SUBSTANCES 2.1. PROPERTIES OF BASIC AND ACID OXIDES 25. Look in the mini-handbook "Inorganic chemistry in reactions" how oxides interact with water. Cross out the formulas of oxides that do not react with water: Na 2 O, SO 2, MgO, SiO 2, CuO, P 2 O 5, Ag 2 O, H 2 O, BaO, Fe 2 O 3, CO, SeO 3. Which oxides metals interact with water? 26. Get acquainted with PD and figure out how to write reaction equations using a mini-guide. ACTIVITY PROGRAM 3 “Compilation of reaction equations using the mini-handbook“ Inorganic chemistry in reactions ” Activity program Example of execution: 1. Rewrite the task in a notebook. Na 2 O + H 2 O 2. Under the formulas of substances, sign the names of the classes to which they belong to basic water Na 2 O + H 2 O. oxide 3. In the mini-reference find the corresponding scheme of transformation - basic + water alkali "Basic oxides" scheme 1: oxide. 4. Check if the proposed substances can react in this way (see the description of the reaction under the diagram) 5. Identify the other participants in the reaction, write them in the diagram. 6. Arrange the stoichiometric coefficients. Only oxides of alkali and alkaline earth metals react in this way. Na 2 O alkali metal oxide, interacts with water. The oxide Na 2 O corresponds to the base NaOH Na 2 O + H 2 O NaOH Na 2 O + H 2 O 2NaOH 27. Complete the equations of possible reactions. 1. (see the mini-reference book, schemes 1 of the sections "Basic oxides", "Acid oxides") CaO + H 2 OP 2 O 5 + H 2 O MgO + H 2 OH 2 O + Na 2 OH 2 O + CrO N 2 O 3 + H 2 O Cs 2 O + H 2 OH 2 O + SO 3 11

6 SeO 2 + H 2 OH 2 O + K 2 O FeO + H 2 O BaO + H 2 OH 2 O + SiO 2 H 2 O + CO 2 2. Acid oxides") Na 2 O + HCl CsOH + N 2 O 5 CrO + HNO 3 BaO + H 2 SO 4 CO 2 + NaOH SO 3 + KOH CaO + H 3 PO 4 HBr + CuO Ca (OH) 2 + P 2 O 5 CoO + H 2 SO 4 H 2 SO 4 + MgO CO 2 + NH 4 OH HCl + BaO CO + NaOH 3. (see mini-reference book, schemes 3 of the sections "Basic oxides", "Acid oxides") CaO + SO 2 CO 2 + SO 2 MgO + SiO 2 MgO + SO 3 BaO + P 2 O 5 Al 2 O 3 + SiO 2 Na 2 O + N 2 O 5 BeO + Na 2 OK 2 O + Al 2 O 3 Na 2 O + Li 2 OP 2 O 5 + SrO N 2 O 3 + K 2 O Al 2 O 3 + CaO CaO + CO 2 CO 2 + BaO CaO + NO 4. (see mini-reference book, scheme 4, section "Basic oxides") CaO + H 3 PO 4 Be(OH) 2 + CuO CaO + Al(OH) 3 K 2 O + Zn(OH) 2 CO + KOH Sn(OH) 2 + Na 2 O Al 2 O 3 + Pb(OH) 2 FeO + Al(OH) 3 Cs 2 O + Al(OH) 3 Li 2 O + Zn(OH) 2 5. (see mini-reference book, Scheme 4 of the Acid Oxides section) Na 2 CO 3 + SiO 2 SiO 2 + MgSO 3 CO 2 + CaSiO 3 K 2 CO 3 + SO 2 Na 3 PO 4 + SiO 2 Na 2 CO 3 + P 2 O 5 12

7 28. Complete the reaction equations involving oxides: a) CaO + CaSO 4 ; d) Na 2 CO 3; b) CaO + ... CaSO 4 + H 2 O; e) ... + KOH ... + K 2 SO 3; c) + Ba(OH) 2 ; e) MgCl How many acids can be obtained by adding to water: a) nitric oxide (V); b) phosphorus (V) oxide; c) zinc oxide; d) nitric oxide (II); e) hydrogen chloride; e) sodium oxide; g) carbon monoxide? Check yourself, the total number of acids must be equal Make up the reaction equations corresponding to the schemes (each reaction involves one or more oxides). a) SO 3 H 2 SO 4 BaSO 4; b) Na 2 O NaOH Na 2 CO 3 Na 2 SiO 3; c) SO 2 H 2 SO 3 K 2 SO 3 SO 2 K 2 SO 3; d) HCl H 2 O H 2 SO 4 CaSO 4; e) CaCO 3 CO 2 K 2 CO 3 K 2 SiO 3; f) CO 2 Na 2 CO 3 CO 2 CaCO 3. ; g) acid oxide acid water; h) basic oxide salt acidic oxide; i) acid oxide water alkali. 31. Suggest a method: a) extraction of magnesium oxide from its mixture with potassium oxide; b) isolation of silicon oxide from its mixture with phosphorus (V) oxide. 32. Underline the names of hydroxides that can be obtained by reacting oxides with water: sulfuric acid, ammonium hydroxide, aluminum hydroxide, silicic acid, iron (II) hydroxide, phosphoric acid, hydrofluoric acid, copper (II) hydroxide, sodium tetrahydroxoaluminate, hydroxochloride magnesium, potassium hydroxide. Check yourself the number of underlined names should be equal to 3. 13

8 SeO 2 + H 2 OH 2 O + K 2 O FeO + H 2 O BaO + H 2 OH 2 O + SiO 2 H 2 O + CO 2 2. Acid oxides") Na 2 O + HCl CsOH + N 2 O 5 CrO + HNO 3 BaO + H 2 SO 4 CO 2 + NaOH SO 3 + KOH CaO + H 3 PO 4 HBr + CuO Ca (OH) 2 + P 2 O 5 CoO + H 2 SO 4 H 2 SO 4 + MgO CO 2 + NH 4 OH HCl + BaO CO + NaOH 3. (see mini-reference book, schemes 3 of the sections "Basic oxides", "Acid oxides") CaO + SO 2 CO 2 + SO 2 MgO + SiO 2 MgO + SO 3 BaO + P 2 O 5 Al 2 O 3 + SiO 2 Na 2 O + N 2 O 5 BeO + Na 2 OK 2 O + Al 2 O 3 Na 2 O + Li 2 OP 2 O 5 + SrO N 2 O 3 + K 2 O Al 2 O 3 + CaO CaO + CO 2 CO 2 + BaO CaO + NO 4. (see mini-reference book, scheme 4, section "Basic oxides") CaO + H 3 PO 4 Be(OH) 2 + CuO CaO + Al(OH) 3 K 2 O + Zn(OH) 2 CO + KOH Sn(OH) 2 + Na 2 O Al 2 O 3 + Pb(OH) 2 FeO + Al(OH) 3 Cs 2 O + Al(OH) 3 Li 2 O + Zn(OH) 2 5. (see mini-reference book, Scheme 4 of the Acid Oxides section) Na 2 CO 3 + SiO 2 SiO 2 + MgSO 3 CO 2 + CaSiO 3 K 2 CO 3 + SO 2 Na 3 PO 4 + SiO 2 Na 2 CO 3 + P 2 O 5 12

9 28. Complete the reaction equations involving oxides: a) CaO + CaSO 4 ; d) Na 2 CO 3; b) CaO + ... CaSO 4 + H 2 O; e) ... + KOH ... + K 2 SO 3; c) + Ba(OH) 2 ; e) MgCl How many acids can be obtained by adding to water: a) nitric oxide (V); b) phosphorus (V) oxide; c) zinc oxide; d) nitric oxide (II); e) hydrogen chloride; e) sodium oxide; g) carbon monoxide? Check yourself, the total number of acids must be equal Make up the reaction equations corresponding to the schemes (each reaction involves one or more oxides). a) SO 3 H 2 SO 4 BaSO 4; b) Na 2 O NaOH Na 2 CO 3 Na 2 SiO 3; c) SO 2 H 2 SO 3 K 2 SO 3 SO 2 K 2 SO 3; d) HCl H 2 O H 2 SO 4 CaSO 4; e) CaCO 3 CO 2 K 2 CO 3 K 2 SiO 3; f) CO 2 Na 2 CO 3 CO 2 CaCO 3. ; g) acid oxide acid water; h) basic oxide salt acidic oxide; i) acid oxide water alkali. 31. Suggest a method: a) extraction of magnesium oxide from its mixture with potassium oxide; b) isolation of silicon oxide from its mixture with phosphorus (V) oxide. 32. Underline the names of hydroxides that can be obtained by reacting oxides with water: sulfuric acid, ammonium hydroxide, aluminum hydroxide, silicic acid, iron (II) hydroxide, phosphoric acid, hydrofluoric acid, copper (II) hydroxide, sodium tetrahydroxoaluminate, hydroxochloride magnesium, potassium hydroxide. Check yourself the number of underlined names should be equal to 3. 13

10 33. Underline the formulas of substances with which it reacts: a) carbon monoxide (IV): HCl, Mg (OH) 2, CaO, H 3 PO 4, SiO 2; b) calcium oxide: NaOH, H 2 O, SO 2, S 2 O, CO 2, MgO; c) phosphorus oxide (V): HCl, Ca (OH) 2, H 2 O, H 3 PO 4, Na 2 CO 3? Write the equations of the corresponding reactions. 34. Which of the following substances can react in pairs with each other: a) SO 2, P 2 O 5, HCl, CaO; b) Na 2 O, CuO, HCl, N 2 O; c) K 2 O, CO, BaO, P 2 O 5? Write reaction equations. Check yourself in total, you should get 7 reaction equations. 35. Using the mini-reference book (sections "Basic oxides" and "Acid oxides"), determine which substances are encrypted in letters (if several options are possible, offer one). 1. A + B H 2 SO 4; A + B NaOH; B + C D. 3. A + B BaSiO 3 ; B + C BaSiO 3 + D; D + A C. 2. A + H 2 O B; B + SO 2 C + H 2 O (C contains atoms of three elements, one of which is potassium). 4. A + B C; B + D D + A; A + E B + H 2 O; B + H 2 O E (substance C is called soda ash, substance D is insoluble in water). 5. H 2 O A (contains 6 atoms) H 2 O B (3 atoms) H 2 O C (8 atoms) D (13 atoms). 36. In the proposed series, exclude (cross out) one extra formula - one that does not form a homogeneous group with the rest: a) N 2 O, NO 2, N 2 O 3; b) CO 2, SO 2, SiO 2; c) SrO, SnO, CrO; d) Mn 2 O 7, P 2 O 5, CrO 3. Explain your choice. 37. Using only reactions involving oxides, get in the maximum possible number of ways: a) sodium sulfate; b) water; c) potassium sulfite; d) calcium carbonate. 14

11 89. Salt A is a white, water-soluble compound. When silver nitrate is added to an aqueous solution A, a white precipitate is formed. When a NaOH solution is added dropwise to the same solution, a white gelatinous precipitate B is formed. When B is calcined, a white refractory substance C is formed, approaching diamond in hardness. Write the reaction equations. Why is NaOH added dropwise to form B? 90. A simple gaseous substance A of yellow-green color with a pungent odor reacts with red metal B to form salt C. When alkali acts on an aqueous solution of C, a blue gelatinous precipitate is released. Write the reaction equations. 91. A simple substance containing element X, which is part of the thyroid gland, when interacting with a gaseous substance Y, forms a strong acid Z. Z enters an exchange reaction with precious metal nitrate to form a yellow precipitate. Write the equations of the described reactions. 92. When an HCl solution acts on an aqueous solution of salt A, a colorless gas B with an unpleasant odor is released, which, when passed through a solution of lead nitrate, forms a black precipitate C. Give the reaction equations. 93. Volatile acid A, when neutralized with KOH, gives salt B, which, when ignited, releases a gas that supports combustion, and another salt C. Write the reaction equations. CONTENTS 1. CLASSIFICATION OF INORGANIC SUBSTANCES Metals and non-metals Oxides, hydroxides, salts 4 2. CHEMICAL PROPERTIES OF SOME CLASSES OF INORGANIC SUBSTANCES 2.1. Properties of basic and acidic oxides Ion exchange reactions (RIR) in electrolyte solutions Properties of bases and acids Properties of salts Interactions of acids with metals Additional tasks 31 32

The structure of the atom and the periodic law of D.I. Mendeleev 1. The charge of the nucleus of an atom of a chemical element located in the 3rd period, group IIA is 1) +12 2) +2 3) +10 4) +8 2. What is the charge of the nucleus atom (+Z),

TO SCHOOLCHILDREN AND APPLICANT DERYABIN N.E. CHEMISTRY MAIN CLASSES OF INORGANIC SUBSTANCES Theoretical basis Questions Exercises Assignments Reference material Moscow 2010 7.6. Acid oxides Acid oxides

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1 SCHOOLCHILDREN AND APPLICANT DERYABINA N.E. CHEMISTRY MAIN CLASSES OF INORGANIC SUBSTANCES Theoretical foundations Questions Exercises Tasks Reference material Moscow 2010

2 7.6. Acid oxides Acid oxides are oxides to which acid hydroxides correspond. Acid oxides are oxides of non-metals (excluding non-salt-forming CO, NO, N 2 O, SiO, S 2 O) and metal oxides in SO. +5, +6, +7, +8. In oxides of non-metals, the bond between atoms is covalent polar. Among the oxides of the molecular structure there are gaseous (CO 2, SO 2, N 2 O, NO 2), liquid (volatile SO 3, N 2 O 3), solid (volatile P 2 O 5, N 2 O 5, SeO 2, TeO 2). Solid, very refractory oxide SiO 2 (sand) substance with an atomic crystal lattice. For acidic oxides, the name "anhydride" is often used, the product of the elimination of water from the corresponding acid. So, SO 2 - sulfurous anhydride H 2 SO 3, SO 3 sulfuric anhydride H 2 SO 4, P 2 O 5 anhydride of three acids metaphosphoric HPO 3, pyrophosphoric H 4 P 2 O 7 and orthophosphoric H 3 PO Chemical properties of acid oxides 1. ACID OXIDE + WATER \u003d ACID When acid oxides are dissolved in water, hydroxides are formed - acids in which the oxidation state of the non-metal SO 3 + H 2 O \u003d H 2 SO 4 is preserved (excl.: SiO 2 is insoluble in water). SiO 2 + H 2 O Oxides NO 2 and ClO 2 do not have corresponding acid hydroxides; when they are dissolved in water, a disproportionation reaction occurs, as a result of which a change in S.O. acid-forming element. 2NO 2 + H 2 O = HNO 3 + HNO 2 3NO 2 + H 2 O = 2HNO 3 + NO 2ClO 2 + H 2 O = HClO 3 + HClO 2 6ClO 2 + 3H 2 O = 5HClO 3 + HCl When dissolved in water P 2 O 5, depending on the number of attached water molecules, three acids can be formed: metaphosphoric HPO 3, pyrophosphoric H 4 P 2 O 7 or ortho- P 2 O 5 + 2H 2 O \u003d H 4 P 2 O 7 P 2 O 5 + H 2 O \u003d 2HPO 3 phosphoric H 3 PO 4. P 2 O 5 + 3H 2 O \u003d 2H 3 PO 4 CrO 3 oxide corresponds to two acids - chromic H 2 CrO 4 and dichromic H 2 Cr 2 O 7. CrO 3 + H 2 O \u003d H 2 CrO 4 2CrO 3 + H 2 O \u003d H 2 Cr 2 O 7 Oxides CO 2 and SO 2 react with water reversibly, the equilibrium is strongly shifted to the left. 2. ACID OXIDE + BASE \u003d SALT + WATER Soluble acid oxides interact with bases when normal conditions, insoluble upon fusion. SiO 2 + 2NaOH \u003d Na 2 SiO 3 + H 2 O With an excess of acid oxide, which is an anhydride of a polybasic acid, an acid salt is formed. With an excess of a polyacid base - the main one. CO 2 (ex) + NaOH \u003d NaHCO 3 P 2 O 5 (ex) + 2Ca (OH) 2 \u003d 2CaHPO 4 + H 2 OP 2 O 5 (ex) + Ca (OH) 2 + H 2 O \u003d Ca (H 2 PO 4) 2 CO 2 + 2Mg (OH) 2 (ex) \u003d (MgOH) 2 CO 3 + H 2 O Oxides NO 2 and ClO 2 do not have the corresponding acid hydroxides, when they interact with alkalis, a disproportionation reaction occurs, as a result which pro- 2NO 2 + 2NaOH \u003d NaNO 3 + NaNO 2 + H 2 O changes CO. acid-forming 2ClO 2 + 2NaOH = NaClO 3 + NaClO 2 + H 2 O element and two salts are formed. 8ClO 2 + 8NaOH \u003d 5NaClO 4 + 3NaCl + 4H 2 O Acid CO 2 oxide also reacts with some amphoteric hydroxides (Be (OH) 2, Zn (OH) 2, Pb (OH) 2 and Cu (OH) 2, which also exhibits partially amphoteric properties) with the formation of precipitation of basic salts and CO 2 + 2Be (OH) 2 \u003d (BeOH) 2 CO 3 + H 2 O of water. CO 2 + 2Cu(OH) 2 = (CuOH) 2 CO 3 + H 2 O 26

3 1. Test Yourself Exercise 1. Complete the reaction equations. SeO 2 + H 2 OH 2 O + NO 2 (cold) P 2 O 5 + H 2 O Cl 2 O 7 + H 2 OH 2 O + Na 2 OH 2 O + CO 2 N 2 O 3 + H 2 O ClO 2 + H 2 O (gor.) P 2 O 5 + H 2 O (ex.) P 2 O 5 (ex.) + H 2 OH 2 O + SO 3 NO 2 + H 2 O (gor.) 2 .Co (OH) 3 + P 2 O 5 (ex) Al (OH) 3 + SO 2 CO 2 (ex) + NaOH H 2 SO 4 + MgO (ex) CaO + H 3 PO 4 (ex) BaO + H 2 SO 4 CO 2 + NaOH K 2 O + Zn (OH) 2 KOH (gor.) + ClO 2 NO 2 + NaOH Ca (OH) 2 (ex) + P 2 O 5 SO 3 + KOH KOH + SiO 2 Cu (OH) 2 + CO 2 CsOH + N 2 O 5 ClO 2 + NaOH (cold) Exercise 2. Fill in the table. Oxides dissolved in The reaction equation for the interaction of an oxide with water in water Ions found in a solution of SO 4 2-, H + NO 2 -, H + Ca 2+, OH - Exercise 3. Write the reaction equations involving oxides, as a result of which in solution the following ions appeared: a) CO 3 2-, K + ; b) NO 3 -, H +; c) H +, PO 3 -, d) Rb +, OH - ; e) NO 3 -, NO 2 -, H + ; e) Na +, Cl -? Exercise 4. Make up the reaction equations corresponding to the schemes: 1) S H 2 S Na 2 S CuS; 2) Fe FeO Fe 2 O 3 Fe 2 (SO 4) 3 BaSO 4; + H 2 + H 2 O + CO 2 3) Na Ca (OH) Na 2 O 4) Ag 2 O) basic oxide alkali salt 6) acid oxide H 2 O base 7) acid oxide acid water 8) ClO 2 acid NaClO 2 Exercise 5. In the proposed rows, exclude (cross out) one extra formula - one that does not form a homogeneous group with the rest. Explain your choice. a) N 2 O, NO 2, N 2 O 3; b) NO 2, N 2 O 3, N 2 O 5; c) SrO, SnO, CrO; d) CO 2, SO 2, SiO 2; e) SO 2, NO 2, ClO 2; e) Mn 2 O 7, P 2 O 5, XeO 4; g) HPO 3, H 3 PO 3, H 3 PO 4, H 4 P 2 O 7; h) NaClO 2, NaClO 3, NaClO 4. 27

4 7.7. Chemical properties of acid oxides (continued) 3. ACID OXIDE + BASIC / AMPHOTERIC OXIDE = SALT In these reactions, an element from a basic / amphoteric oxide forms a cation, and an element from an acid anion of a salt, amphoteric oxides in this case exhibit the properties of basic ones. Reactions between solid oxides occur during fusion. Basic oxides that are amphoteric and insoluble in water interact only with solid and liquid acid oxides. 3SO 3 + Al 2 O 3 \u003d Al 2 (SO 4) 3 4. NON-VOLATILE ACID OXIDE + SALT \u003d SALT + Non-volatile acid oxides displace volatile acid oxides from their salts during fusion. VOLATILE ACID OXIDE SiO 2 + CaCO 3 \u003d CaSiO 3 + CO 2 P 2 O 5 + Na 2 CO 3 \u003d 2Na 3 PO 4 + 3CO 2 3SiO 2 + Ca 3 (PO 4) 2 \u003d 3CaSiO 3 + P 2 O 5 5 Acidic oxides extremely rarely interact with each other or with acids. Thus, for example, phosphoric anhydride P 2 O 5, the strongest dehydrating agent, reacts with anhydrous oxygen-containing acids to form HPO 3 and the anhydride of the corresponding acid. P 2 O 5 + 2HClO 4 (anhydrous) \u003d Cl 2 O 7 + 2HPO 3 P 2 O 5 + 2HNO 3 (anhydrous) \u003d N 2 O 5 + 2HPO 3 Some redox reactions of acid oxides A. Recovery. At high temperatures, some non-metals (C, H 2) reduce oxides (partially or completely). Magnesium is also often used to reduce nonmetals from their oxides. CO 2 + 2Mg \u003d C + 2MgO SiO 2 + 2Mg \u003d Si + 2MgO N 2 O + Mg \u003d N 2 + MgO 2CO 2 + 5Ca \u003d CaC 2 + 4CaO B. Oxidation. Under the action of oxygen (ozone), when heated or in the presence of a catalyst, lower oxides are converted into higher ones. NO + O 3 \u003d NO 2 + O 2 SO 2 + O 3 \u003d SO 3 + O 2 2NO 2 + O 3 \u003d N 2 O 5 + O 2 CO 2 + C \u003d 2CO SiO 2 + C \u003d SiO + CO SO 3 + C \u003d SO 2 + CO SO 2 + C \u003d S + CO 2 2N 2 O + C \u003d 2N 2 + CO 2 2NO + C \u003d N 2 + CO 2 2NO 2 + 2C \u003d N 2 + 2CO 2 P 2 O 5 + 5C \u003d 2P + 5CO H 2 O + C \u003d H 2 + CO N 2 O + H 2 \u003d N 2 + H 2 O 2NO + 2H 2 \u003d N 2 + 2H 2 O,ka CO 2 + 4H 2 \u003d CH 4 + 2H 2 O 2CO + O 2 = 2CO 2,ka 2SO 2 + O 2 = 2SO 3 P 2 O 3 + O 2 = P 2 O 5 2NO + O 2 = 2NO 2 2N 2 O 3 + O 2 = 2N 2 O 4 In addition to those listed, oxides also enter into other redox reactions, for example: SO 2 + NO 2 \u003d NO + SO 3 4NO 2 + O 2 + 2H 2 O \u003d 4HNO 3 N 2 O + 2Cu \u003d N 2 + Cu 2 O 2SO 2 + 2NO \u003d N 2 + 2SO 3 2N 2 O 5 \u003d 4NO 2 + O 2 2NO + 4Cu \u003d N 2 + 2Cu 2 O SO 2 + 2H 2 S \u003d 3S + 2H 2 O 2NO 2 \u003d 2NO + O 2 N 2 O 3 + 3Cu \u003d N 2 + 3CuO 2SO 2 + O 2 + 2H 2 O \u003d 2H 2 SO 4 2CO 2 + 2Na 2 O 2 \u003d 2Na 2 CO 3 + O 2 3N 2 O + 2NH 3 \u003d 4N 2 + 3H 2 O 10NO 2 + 8P = 5N 2 + 4P 2 O 5 2NO 2 + 4Cu = N 2 + 4CuO N 2 O 5 + 5Cu = N 2 + 5CuO 28

5 3. Check Yourself Exercise 1. Complete the reaction equations. CaO + SO 2 CO 2 + BaO N 2 O 3 + Na 2 O MgO + SO 3 SrO + P 2 O 5 CO 2 + CuO Li 2 O + Al 2 O 3 Al 2 O 3 + SiO 2 SiO 2 + ZnO BeO + Na 2 ON 2 O 5 + Na 2 O CO 2 + SO 2 4. Na 2 CO 3 + SiO 2 SiO 2 + MgSO 3 CO 2 + CaSiO 3 K 2 CO 3 + SO 2 Na 3 PO 4 + SiO 2 Na 2 CO 3 + P 2 O 5 5. CO 2 + Mg Mg + SiO 2 P 2 O 5 + H 2 SO 4 HNO 3 + P 2 O 5 SO 3 + CH 2 O + C NO 2 + O 2 + H 2 O SO 2 + O 3 HCl + P 2 O 5 NO + O 2 Na 2 O + O 2 K 2 CO 3 + SiO 2 H 2 O + C NO 2 + H 2 O (horizontal) CO 2 + NaOH K 2 O + Zn(OH) 2 SrO + P 2 O 5 CO 2 + C Cu 2 O + O 2 Na 2 O + O 2 H 2 + CO 2 H 2 O + CO Al 2 O 3 + C Na 2 O + C CO 2 + Na 2 O 2 CO 2 + H 2 O Na 2 O + H 2 O ZnO + Cu Exercise 2. Write the reaction equations corresponding to the schemes: 1) SO 2 SO 3 H 2 SO 4 BaSO 4; 2) SO 3 SO 2 Na 2 SO 3; 3) N 2 NO NO 2 NaNO 3; 4) P P 2 O 3 P 2 O 5 X H 3 PO 4; 5) HNO 3 N 2 O 5 NaNO 3; 6) C CO 2 Na 2 CO 3 CO 2 Ca (HCO 3) 2; + O 2 + O 2 + H 2 O + H 2 O + Ca (OH) 2 7) Ca 3 (PO 4) 2; + O 2 + H 2 S + O 2 + O 3 + Al 2 O 3 + Ba (OH) 2 + HCl 8) S; +O 2 +O 2 +KOH +KOH +HCl +Mg +CO 2 9) C

6 Building 1. Classification of inorganic substances Degree of oxidation in inorganic chemistry Nomenclature of inorganic substances Names of simple substances names of binary compounds of bases of bases, amphoteric hydroxides, acids and salts Classes of inorganic compounds from the point of view of electrolytic dissociation of acid, base and amphoteric hydroxides as an average, acidic and basic salts as electrolytes CLASSIFICATION OF CHEMICAL REACTIONS. CONDITIONS FOR ION EXCHANGE REACTIONS SIMPLE SUBSTANCES METALS AND NON-METALS Some physical properties simple substances Some chemical properties of simple substances OXIDE Classification of oxides Oxides and their corresponding hydroxides Non-salt-forming oxides Basic oxides Chemical properties of basic oxides Acidic oxides Chemical properties of acid oxides Amphoteric oxides Chemical properties of amphoteric oxides BASEs Classification of bases Chemical properties of bases ACIDS Classification of acids Chemical properties of acids AMPHOTERIC HYDROXIDES Amphotericity . Amphoteric hydroxides Chemical properties of amphoteric hydroxides SALT Classification of salts Chemical properties of salts ways to obtain salts Application

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