Schoolboy and entrant N.E.Deryabin chemistry are the main classes of inorganic substances. Inorganic chemistry in Deryabin's exercises and problems, not organic chemistry in reactions

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1 SCHOOLBOY AND ENTRANCE DERYABIN N.E. CHEMISTRY BASIC 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. Acidic oxides are oxides of non-metals (excluding non-salt-forming CO, NO, N 2 O, SiO, S 2 O) and metal oxides in S.O. +5, +6, +7, +8. In oxides of non-metals, the bond between atoms is covalent polar. Among the oxides of 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) is a 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 is anhydride of sulfurous acid H 2 SO 3, SO 3 anhydride of sulfuric acid 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 = 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 = H 2 SO 4 is preserved (excl .: SiO 2 is insoluble in water). SiO 2 + H 2 O The oxides NO 2 and ClO 2 do not have the corresponding acidic hydroxides; when they are dissolved in water, a disproportionation reaction occurs, as a result of which the CO changes. 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 = H 4 P 2 O 7 P 2 O 5 + H 2 O = 2HPO 3 phosphoric H 3 PO 4. P 2 O 5 + 3H 2 O = 2H 3 PO 4 Oxide CrO 3 corresponds to two acids - chromic H 2 CrO 4 and dichromic H 2 Cr 2 O 7. CrO 3 + H 2 O = H 2 CrO 4 2CrO 3 + H 2 O = H 2 Cr 2 O 7 Oxides CO 2 and SO 2 react reversibly with water, the equilibrium is strongly shifted to the left. 2. ACID OXIDE + BASE = SALT + WATER Soluble acid oxides react with bases at normal conditions, insoluble on fusion. SiO 2 + 2NaOH = 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, it is basic. CO 2 (g) + NaOH = NaHCO 3 P 2 O 5 (g) + 2Ca (OH) 2 = 2CaHPO 4 + H 2 OP 2 O 5 (g) + Ca (OH) 2 + H 2 O = Ca (H 2 PO 4) 2 CO 2 + 2Mg (OH) 2 (g) = (MgOH) 2 CO 3 + H 2 O Oxides NO 2 and ClO 2 do not have corresponding acidic hydroxides, when they interact with alkalis, a disproportionation reaction occurs, as a result which pro 2NO 2 + 2NaOH = NaNO 3 + NaNO 2 + H 2 O changes in C.O. acid-forming 2ClO 2 + 2NaOH = NaClO 3 + NaClO 2 + H 2 O element and two salts are formed. 8ClO 2 + 8NaOH = 5NaClO 4 + 3NaCl + 4H 2 O Acidic oxide CO 2 also reacts with some amphoteric hydroxides (Be (OH) 2, Zn (OH) 2, Pb (OH) 2 and Cu (OH) 2, also exhibiting partially amphoteric properties) with the formation of precipitation of basic salts and CO 2 + 2Be (OH) 2 = (BeOH) 2 CO 3 + H 2 O 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 (hot) P 2 O 5 + H 2 O (hot) P 2 O 5 (hot) + H 2 OH 2 O + SO 3 NO 2 + H 2 O (hot) 2 . Co (OH) 3 + P 2 O 5 (g) Al (OH) 3 + SO 2 CO 2 (g) + NaOH H 2 SO 4 + MgO (g) CaO + H 3 PO 4 (g) BaO + H 2 SO 4 CO 2 + NaOH K 2 O + Zn (OH) 2 KOH (hot) + ClO 2 NO 2 + NaOH Ca (OH) 2 (g) + 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 equation of the reaction of the interaction of oxide with water water Ions found in a solution SO 4 2-, H + NO 2 -, H + Ca 2+, OH - Exercise 3. Write the equations of reactions 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 +; f) 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) СlO 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; f) 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 acidic anion of a salt, amphoteric oxides in this case exhibit basic properties. Reactions between solid oxides take place during fusion. Amphoteric and water-insoluble basic oxides interact only with solid and liquid ki - P 2 O 5 + 3CuO = Cu 3 (PO 4) 2 SiO2 + BaO = BaSiO 3 slot oxides. 3SO 3 + Al 2 O 3 = Al 2 (SO 4) 3 4. NON-VOLATILE ACID OXIDE + SALT = SALT + Non-volatile acid oxides displace volatile acid oxides from their salts during fusion. VOLATILE ACID OXIDE SiO 2 + CaCO 3 = CaSiO 3 + CO 2 P 2 O 5 + Na 2 CO 3 = 2Na 3 PO 4 + 3CO 2 3SiO 2 + Ca 3 (PO 4) 2 = 3CaSiO 3 + P 2 O 5 5 Acidic oxides very rarely interact with each other or with acids. For example, phosphoric anhydride P 2 O 5, the strongest dehydrating agent, reacts with anhydrous oxygen-containing acids to form HPO 3 and the corresponding acid anhydride. P 2 O 5 + 2HClO 4 (anhydrous) = Cl 2 O 7 + 2HPO 3 P 2 O 5 + 2HNO 3 (anhydrous) = N 2 O 5 + 2HPO 3 Some redox reactions of acid oxides A. Reduction. At high temperature some non-metals (C, H 2) reduce oxides (partially or completely). For the reduction of non-metals from their oxides, magnesium heat is also often used. CO 2 + 2Mg = C + 2MgO SiO 2 + 2Mg = Si + 2MgO N 2 O + Mg = N 2 + MgO 2CO 2 + 5Ca = CaC 2 + 4CaO B. Oxidation. Under the influence of oxygen (ozone), when heated or in the presence of a catalyst, lower oxides are transformed into higher ones. NO + O 3 = NO 2 + O 2 SO 2 + O 3 = SO 3 + O 2 2NO 2 + O 3 = N 2 O 5 + O 2 CO 2 + C = 2CO SiO 2 + C = SiO + CO SO 3 + C = SO 2 + CO SO 2 + C = S + CO 2 2N 2 O + C = 2N 2 + CO 2 2NO + C = N 2 + CO 2 2NO 2 + 2C = N 2 + 2CO 2 P 2 O 5 + 5C = 2P + 5CO H 2 O + C = H 2 + CO N 2 O + H 2 = N 2 + H 2 O 2NO + 2H 2 = N 2 + 2H 2 O, ka CO 2 + 4H 2 = 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 the above, oxides also enter into other redox reactions, for example: SO 2 + NO 2 = NO + SO 3 4NO 2 + O 2 + 2H 2 O = 4HNO 3 N 2 O + 2Cu = N 2 + Cu 2 O 2SO 2 + 2NO = N 2 + 2SO 3 2N 2 O 5 = 4NO 2 + O 2 2NO + 4Cu = N 2 + 2Cu 2 O SO 2 + 2H 2 S = 3S + 2H 2 O 2NO 2 = 2NO + O 2 N 2 O 3 + 3Cu = N 2 + 3CuO 2SO 2 + O 2 + 2H 2 O = 2H 2 SO 4 2CO 2 + 2Na 2 O 2 = 2Na 2 CO 3 + O 2 3N 2 O + 2NH 3 = 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. Test 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 (hot) 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. Make 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 CONTENTS 1. CLASSIFICATION OF INORGANIC SUBSTANCES The degree of oxidation INORGANIC CHEMISTRY NOMENCLATURE OF INORGANIC SUBSTANCES simple substances Names Names Names bases binary compounds, amphoteric hydroxides, acids and salts classes of inorganic compounds in terms of electrolytically DISSOCIATION Acids, bases and amphoteric hydroxides as electrolytes Medium, acidic and basic salts as electrolytes. CLASSIFICATIONS OF CHEMICAL REACTIONS. PROCESS CONDITIONS OF ION EXCHANGE REACTIONS SIMPLE SUBSTANCES METALS AND NON-METALS Some physical properties of simple substances Some Chemical properties simple substances OXIDES Classification of oxides Oxides and their corresponding hydroxides Non-salt-forming oxides Basic oxides Chemical properties of basic oxides Acid 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. Amphoteric hydroxides Chemical properties of amphoteric hydroxides SALTS Classification of salts Chemical properties of salts GENETIC RELATIONSHIP BETWEEN CLASSES OF INORGANIC COMPOUNDS METHODS OF OBTAINING OXIDES, BASES, AMPHOTERIC HYDROXIDES, BASIC HYDROXIDES AND BASES OF AMPHOTERIC HYDROXIDES AND BASES OF ACIDS methods of obtaining salts Appendix

Repetition of A9 and A10 (properties of oxides and hydroxides); А11 Characteristic chemical properties of salts: medium, acidic, basic; complex (for example, aluminum and zinc compounds) А12 Relationship of inorganic

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1 Deryabina N.E. INORGANIC CHEMISTRY IN EXERCISES AND TASKS Textbook for secondary school students in the IPO "At Nikitskiye Vorota" Moscow 2012

2 UDC 546 BBK 24.1 D36 D36 Deryabina N.Ye. Inorganic chemistry in exercises and tasks. - M .: IPO "At Nikitskiye Vorota", 2012, - 32 p. ISBN The manual is a collection of exercises and problems on the most important section of inorganic chemistry, the main classes of inorganic compounds. Included in the set with the mini-reference book "Inorganic chemistry in reactions", the material from which will help students to perform the proposed exercises. Recommended for middle school students (basic). ISBN Deryabina N.E., 2012

3 1. CLASSIFICATION OF INORGANIC SUBSTANCES 1.1. METALS AND NON-METALS 1. On the periodic table shown on the cover, paint over yellow cells with non-metallic 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 the metal element and the metal element, which are in the periodic table: a) next to each other; 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 d.o. ; b) metals with constant c.o .. 6. What metal forms a simple substance: a) red; b) yellow color; c) liquid at n.u.? What kind of non-metal forms under normal conditions: a) gaseous poisonous simple substance of yellow-green color; b) a simple substance in the form of violet crystals with a metallic luster; c) a simple substance in the form of solid transparent crystals capable of cutting glass? 7. Two students played chemistry tic-tac-toe. The first one wrote down the symbols of metals in the cells, the second of non-metals (according to the rules of the game, the elements are not repeated). Which one 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 kind essential features are "oxides" not specified in the definition? What features can be removed from the definition? Write down 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. Finish the classification scheme for oxides (see the mini-reference book "Inorganic chemistry in reactions", page 1). Non-metal oxide Metal oxide in the oxidation state +2 other non-salt-forming oxide acidic amphoteric basic salt-forming oxide Can metal atoms form oxides: a) non-salt-forming; b) acidic; 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 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 up the formulas and sign the nature of the 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 ACIDIC OXIDES 25. Look in the mini-guide "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. What oxides metals interact with water? 26. Get to know the PD and figure out how to compose the reaction equations with the help of the mini-reference book. ACTIVITY PROGRAM 3 "Compilation of reaction equations using the mini-reference book" Inorganic chemistry in reactions "Activity program Example of implementation: 1. Rewrite the task in the notebook. Na 2 O + H 2 O 2. Under the formulas of substances, sign the names of the classes to which they belong to the main water Na 2 O + H 2 O. oxide 3. In the mini-reference book, find the appropriate scheme for converting basic + water to alkali "Basic oxides" Scheme 1: oxidation. 4. Check if the proposed substances can react in this way (see the description of the reaction under the scheme) 5. Identify the rest of the participants in the reaction, enter them into the scheme. 6. Place the stoichiometric coefficients. Only oxides of alkali and alkaline earth metals react 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. Finish 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 + К 2 O FeO + H 2 O BaO + H 2 OH 2 O + SiO 2 H 2 O + CO 2 2. (see the mini-reference book, diagrams of 2 sections "Basic oxides", " 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 the mini-reference book, schemes of 3 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 the mini-reference book, scheme 4 of the 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 the mini-guide, scheme 4 of the section "Acid oxides") 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 equations of reactions with the participation of 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; f) 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; f) sodium oxide; g) carbon monoxide? Check yourself the total number of acids should 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) acidic oxide acid water; h) basic oxide salt acidic oxide; i) acidic oxide water alkali. 31. Propose a method: a) separation of magnesium oxide from its mixture with potassium oxide; b) separation of silicon oxide from its mixture with phosphorus (V) oxide. 32. Underline the names of hydroxides that can be obtained by the interaction of oxides with water: sulfuric acid, ammonium hydroxide, aluminum hydroxide, silicic acid, iron (II) hydroxide, phosphoric acid, hydrofluoric acid, copper (II) hydroxide, sodium tetrahydroxoaluminate, hydroxychloride magnesium, potassium hydroxide. Check yourself the number of underlined names should be 3. 13

8 SeO 2 + H 2 OH 2 O + К 2 O FeO + H 2 O BaO + H 2 OH 2 O + SiO 2 H 2 O + CO 2 2. (see the mini-reference book, schemes 2 of sections "Basic oxides", " 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 the mini-reference book, schemes of 3 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 the mini-reference book, scheme 4 of the 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 the mini-guide, 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. Finish the equations of reactions with the participation of 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; f) 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; f) sodium oxide; g) carbon monoxide? Check yourself the total number of acids should 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) acidic oxide acid water; h) basic oxide salt acidic oxide; i) acidic oxide water alkali. 31. Propose a method: a) separation of magnesium oxide from its mixture with potassium oxide; b) separation of silicon oxide from its mixture with phosphorus (V) oxide. 32. Underline the names of hydroxides that can be obtained by the interaction of oxides with water: sulfuric acid, ammonium hydroxide, aluminum hydroxide, silicic acid, iron (II) hydroxide, phosphoric acid, hydrofluoric acid, copper (II) hydroxide, sodium tetrahydroxoaluminate, hydroxychloride magnesium, potassium hydroxide. Check yourself the number of underlined names should be 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 (V) oxide: HCl, Ca (OH) 2, H 2 O, H 3 PO 4, Na 2 CO 3? Write down the equations of the corresponding reactions. 34. Which of the listed 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? Make up the reaction equations. Check yourself there should be 7 reaction equations. 35. Using the mini-reference book (sections "Basic oxides" and "Acid oxides"), determine which substances are encoded in letters (if several options are possible, suggest 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 B + 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 B (8 atoms) G (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 the reactions proceeding with the participation of oxides, get the maximum possible number of ways: a) sodium sulfate; b) water; c) potassium sulfite; d) calcium carbonate. fourteen

11 89. Salt A is a white compound, readily soluble in water. When silver nitrate is added to 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 heated, a white refractory substance C is formed, which is close to diamond in hardness. Write down the reaction equations. Why is NaOH added dropwise to form B? 90. Simple gaseous substance A, yellow-green in color with a pungent odor, reacts with red metal B to form salt C. Under the action of alkali on an aqueous solution of C, a blue gelatinous precipitate is released. Write down the reaction equations. 91. A simple substance containing the element X, which is part of the thyroid gland, when interacting with a gaseous substance Y forms a strong acid Z. Z reacts with the precious metal nitrate to form a yellow precipitate. Write down the equations of the described reactions. 92. When the HCl solution acts on an aqueous solution of salt A, colorless gas B is released with unpleasant odor, when passing through a solution of lead nitrate, a black precipitate C is formed. Give the reaction equations. 93. Volatile acid A, when neutralized with KOH, gives salt B, which, when ignited, gives off a gas supporting combustion and another salt C. Write down 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 (RIO) in electrolyte solutions Properties of bases and acids Properties of salts Interactions of acids with metals Additional tasks 31 32

FOR SCHOOLBOY AND ENTRANCE DERYABIN N.E. CHEMISTRY BASIC CLASSES OF INORGANIC SUBSTANCES Theoretical foundations Questions Exercises Tasks Reference material Moscow 2010 7.6. Acid oxides Acid oxides

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Schoolboy and entrant N.E.Deryabin chemistry are the main classes of inorganic substances. Inorganic chemistry in Deryabin's exercises and problems, not organic chemistry in reactions

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Schoolboy and entrant N.E.Deryabin chemistry are the main classes of inorganic substances. Inorganic chemistry in Deryabin's exercises and problems, not organic chemistry in reactions

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