Genetic relationship between classes of inorganic substances. Genetic relationship between classes of inorganic substances Exe Chemistry relationship of inorganic substances

The relationship and relationship of chemical transformations is confirmed by the genetic relationship between classes not organic matter. One simple substance, depending on the class and chemical properties, forms a chain of transformations complex substances- genetic series.

inorganic substances

Compounds that do not have a carbon skeleton characteristic of organic substances are called inorganic or mineral substances. All mineral compounds are classified into two broad groups:

simple, consisting of atoms of one element;
complex, including atoms of two or more elements.

Rice. one. General classification substances.

Simple connections include:

metals (K, Mg, Ca);
non-metals (O 2 , S, P);
inert gases (Kr, Xe, Rn).

Complex substances have a more branched classification given in the table.

Rice. 2. Classification of complex substances.

Amphoteric metals form the corresponding oxides and hydroxides. Amphoteric compounds exhibit the properties of acids and bases.

genetic series

Simple substances - metals and non-metals - form chains of transformations that reflect the genetic relationship of inorganic substances. Through chemical reactions additions, substitutions and decompositions, new simpler or more complex compounds are formed.

Each link in the chain is associated with the previous presence of a simple substance. The difference between the two types of genetic series lies in the reaction with water: metals form soluble and insoluble bases, non-metals form acids.

The main chains of transformations are described in the table.

*Substance*	*genetic series*	*Examples*
	Active metal → basic oxide → alkali → salt	2Ca + O 2 → 2CaO; CaO + H 2 O → Ca (OH) 2; Ca (OH) 2 + 2HCl → CaCl 2 + 2H 2 O
	Inactive metal → basic oxide → salt → insoluble base → basic oxide → metal	2Cu + O 2 → 2CuO; CuO + 2HCl → CuCl 2 + H 2 O; CuCl 2 + 2KOH → Cu(OH) 2 + 2KCl; Cu(OH) 2 → CuO + H 2 O; CuO + H 2 → Cu + H 2 O
Non-metal	→ acid oxide → soluble (strong) acid → salt	4P + 5O 2 → 2P 2 O 5; P 2 O 5 + 3H 2 O → 2H 3 PO 4; H 3 PO 4 + 3NaOH → Na 3 PO 4 + 3H 2 O
Non-metal	→ acid oxide → salt → insoluble (weak) acid → acid oxide → non-metal	Si + O 2 → SiO 2; SiO 2 + 2NaOH → Na 2 SiO 3 + H 2 O; Na 2 SiO 3 + 2HCl → H 2 SiO 3 + 2NaCl; H 2 SiO 3 → SiO 2 + H 2 O; SiO 2 + 2Zn → 2ZnO + Si

Rice. 3. Diagram of the genetic relationship between classes.

With the help of a transformation chain, medium (normal) or acid salts can be obtained. Complex salts can include several metal and non-metal atoms.

What have we learned?

genetic connection shows the relationship between classes of inorganic substances. It is characterized by a genetic series - a series of transformations simple substances. Simple substances include metals and non-metals. Metals form soluble and insoluble bases depending on activity. Non-metals are transformed into strong or weak acids. New complex substances of the series are formed by addition, substitution and decomposition reactions.

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The classification of inorganic substances is based on chemical composition- the simplest and most constant characteristic in time. The chemical composition of a substance shows which elements are present in it and in what numerical ratio for their atoms.

Elements conventionally divided into elements with metallic and non-metallic properties. The first of these is always included in cations multielement substances (metal properties), the second - in the composition anions (non-metallic properties). In accordance with Periodic law in periods and groups between these elements are amphoteric elements that simultaneously exhibit metallic and non-metallic to one degree or another (amphoteric, dual) properties. Elements of the VIIIA-group continue to be considered separately (noble gases), although for Kr, Xe and Rn clearly non-metallic properties were found (the elements He, Ne, Ar are chemically inert).

The classification of simple and complex inorganic substances is given in Table. 6.

Below are the definitions (definitions) of classes of inorganic substances, their most important Chemical properties and methods of obtaining.

inorganic substances- connections formed by all chemical elements(except for most organic compounds carbon). Divided by chemical composition:

Simple substances made up of atoms of the same element. They are divided according to their chemical properties:

Metals- simple substances of elements with metallic properties (low electronegativity). Typical metals:

Metals have a high reduction ability compared to typical non-metals. In the electrochemical series of voltages, they are much to the left of hydrogen, they displace hydrogen from water (magnesium - during boiling):

The simple substances of the elements Cu, Ag and Ni are also referred to as metals, since their oxides CuO, Ag 2 O, NiO and hydroxides Cu (OH) 2, Ni (OH) 2 are dominated by basic properties.

non-metals- simple substances of elements with non-metallic properties (high electronegativity). Typical non-metals: F 2, Cl 2, Br 2, I 2, O 2, S, N 2, P, C, Si.

Nonmetals have a high oxidizing power compared to typical metals.

Amphigenes- amphoteric simple substances formed by elements with amphoteric (dual) properties (electronegativity is intermediate between metals and non-metals). Typical amphigenes: Be, Cr, Zn, Al, Sn, Pb.

Amphigenes have a lower reducing power compared to typical metals. In the electrochemical series of voltages, they adjoin hydrogen on the left or stand behind it on the right.

Aerogens- noble gases, monatomic simple substances of elements of group VIIIA: He, Ne, Ar, Kr, Xe, Rn. Of these, He, Ne, and Ar are chemically passive (compounds with other elements have not been obtained), while Kr, Xe, and Rn exhibit some of the properties of non-metals with high electronegativity.

Complex Substances made up of atoms of different elements. Divided by composition and chemical properties:

oxides- compounds of elements with oxygen, the oxidation state of oxygen in oxides is always equal to (-II). Divided by composition and chemical properties:

The elements He, Ne and Ar do not form compounds with oxygen. Compounds of elements with oxygen in other oxidation states are not oxides, but binary compounds, for example O + II F 2 -I and H 2 + I O 2 -I. Do not apply to oxides and mixed binary compounds, for example S + IV Cl 2 -I O -II.

Basic oxides- products of complete dehydration (real or conditional) of basic hydroxides retain the chemical properties of the latter.

Of the typical metals, only Li, Mg, Ca, and Sr form the oxides Li 2 O, MgO, CaO, and SrO when burned in air; oxides of Na 2 O, K 2 O, Rb 2 O, Cs 2 O and BaO are obtained by other methods.

Oxides CuO, Ag 2 O and NiO are also classified as basic.

Acid oxides- products of complete dehydration (real or conditional) of acid hydroxides, retain the chemical properties of the latter.

Of the typical non-metals, only S, Se, P, As, C and Si form oxides SO 2, SeO 2, P 2 O 5, As 2 O 3, CO 2 and SiO 2 when burned in air; oxides Cl 2 O, Cl 2 O 7 , I 2 O 5 , SO 3 , SeO 3 , N 2 O 3 , N 2 O 5 and As 2 O 5 are obtained by other methods.

Exception: NO 2 and ClO 2 oxides do not have corresponding acidic hydroxides, but they are considered acidic, since NO 2 and ClO 2 react with alkalis, forming salts of two acids, and ClO 2 with water, forming two acids:

a) 2NO 2 + 2NaOH \u003d NaNO 2 + NaNO 3 + H 2 O

b) 2ClO 2 + H 2 O (cold) = HClO 2 + HClO 3

2ClO 2 + 2NaOH (cold) = NaClO 2 + NaClO 3 + H 2 O

Oxides CrO 3 and Mn 2 O 7 (chromium and manganese in the highest degree oxidation) are also acidic.

Amphoteric oxides- products of complete dehydration (real or conditional) of amphoteric hydroxides retain the chemical properties of amphoteric hydroxides.

Typical amphigenes (except Ga) when burned in air form the oxides BeO, Cr 2 O 3 , ZnO, Al 2 O 3 , GeO 2 , SnO 2 and PbO; amphoteric oxides Ga 2 O 3 , SnO and PbO 2 are obtained by other methods.

double oxides are formed either by atoms of one amphoteric element in different oxidation states, or by atoms of two different (metal, amphoteric) elements, which determines their chemical properties. Examples:

(Fe II Fe 2 III) O 4 , (Рb 2 II Pb IV) O 4 , (MgAl 2) O 4 , (CaTi) O 3 .

Iron oxide is formed by the combustion of iron in air, lead oxide - by weak heating of lead in oxygen; oxides of two different metals are obtained by other methods.

Non-salt-forming oxides- non-metal oxides that do not have acid hydroxides and do not enter into salt formation reactions (difference from basic, acidic and amphoteric oxides), for example: CO, NO, N 2 O, SiO, S 2 O.

Hydroxides- compounds of elements (except fluorine and oxygen) with hydroxo groups O -II H, may also contain oxygen O -II. In hydroxides, the oxidation state of an element is always positive (from +I to +VIII). The number of hydroxo groups is from 1 to 6. They are divided by chemical properties:

Basic hydroxides (bases) formed by elements with metallic properties.

Obtained by the reactions of the corresponding basic oxides with water:

M 2 O + H 2 O \u003d 2MON (M \u003d Li, Na, K, Rb, Cs)

MO + H 2 O \u003d M (OH) 2 (M \u003d Ca, Sr, Ba)

Exception: Mg(OH) 2, Cu(OH) 2 and Ni(OH) 2 hydroxides are obtained by other methods.

When heated, real dehydration (loss of water) occurs for the following hydroxides:

2LiOH \u003d Li 2 O + H 2 O

M (OH) 2 \u003d MO + H 2 O (M \u003d Mg, Ca, Sr, Ba, Cu, Ni)

Basic hydroxides replace their hydroxo groups with acidic residues to form salts; metallic elements retain their oxidation state in salt cations.

Basic hydroxides that are readily soluble in water (NaOH, KOH, Ca (OH) 2, Ba (OH) 2, etc.) are called alkalis, since it is with their help that an alkaline environment is created in the solution.

Acid hydroxides (acids) formed by elements with non-metallic properties. Examples:

Upon dissociation in dilute aqueous solution cations H + are formed (more precisely, H 3 O +) and the following anions, or acid residues:

Acids can be obtained by reactions of the corresponding acid oxides with water (the following are the actual reactions taking place):

Cl 2 O + H 2 O \u003d 2HClO

E 2 O 3 + H 2 O \u003d 2NEO 2 (E \u003d N, As)

As 2 O 3 + 3H 2 O \u003d 2H 3 AsO 3

EO 2 + H 2 O \u003d H 2 EO 3 (E \u003d C, Se)

E 2 O 5 + H 2 O \u003d 2HEO 3 (E \u003d N, P, I)

E 2 O 5 + 3H 2 O \u003d 2H 3 EO 4 (E \u003d P, As)

EO 3 + H 2 O = H 2 EO 4 (E = S, Se, Cr)

E 2 O 7 + H 2 O \u003d 2HEO 4 (E \u003d Cl, Mn)

Exception: SO 2 oxide as acidic hydroxide corresponds to SO 2 polyhydrate n H 2 O (“sulphurous acid H 2 SO 3” does not exist, but acid residues HSO 3 - and SO 3 2- are present in salts).

When some acids are heated, real dehydration occurs and the corresponding acid oxides are formed:

2HAsO 2 \u003d As 2 O 3 + H 2 O

H 2 EO 3 \u003d EO 2 + H 2 O (E \u003d C, Si, Ge, Se)

2HIO 3 \u003d I 2 O 5 + H 2 O

2H 3 AsO 4 \u003d As 2 O 5 + H 2 O

H 2 SeO 4 \u003d SeO 3 + H 2 O

When the (real and formal) hydrogen of acids is replaced by metals and amphigenes, salts are formed, acid residues retain their composition and charge in salts. The acids H 2 SO 4 and H 3 RO 4 in a dilute aqueous solution react with metals and amphigens that are in the series of voltages to the left of hydrogen, while the corresponding salts are formed and hydrogen is released (HNO 3 acid does not enter into such reactions; below are typical metals, except Mg are not listed as they react with water under similar conditions):

M + H 2 SO 4 (pasb.) \u003d MSO 4 + H 2 ^ (M \u003d Be, Mg, Cr, Mn, Zn, Fe, Ni)

2M + 3H 2 SO 4 (razb.) \u003d M 2 (SO 4) 3 + 3H 2 ^ (M \u003d Al, Ga)

3M + 2H 3 PO 4 (diff.) \u003d M 3 (PO 4) 2 v + 3H 2 ^ (M \u003d Mg, Fe, Zn)

Unlike anoxic acids, acidic hydroxides are called oxygenated acids or oxoacids.

Amphoteric hydroxides formed by elements with amphoteric properties. Typical amphoteric hydroxides:

Be(OH) 2 Sn(OH) 2 Al(OH) 3 AlO(OH)

Zn(OH) 2 Pb(OH) 2 Cr(OH) 3 CrO(OH)

He are formed from amphoteric oxides and water, but undergo real dehydration and form amphoteric oxides:

Exception: for iron(III) only metahydroxide FeO(OH) is known, "iron(III) hydroxide Fe(OH) 3" does not exist (not obtained).

Amphoteric hydroxides exhibit the properties of basic and acidic hydroxides; form two types of salts, in which the amphoteric element is part of either salt cations or their anions.

For elements with several oxidation states, the rule applies: the higher the oxidation state, the more pronounced acid properties hydroxides (and/or corresponding oxides).

salt- connections made up of cations basic or amphoteric (in the role of basic) hydroxides and anions(residues) of acid or amphoteric (in the role of acid) hydroxides. In contrast to the anoxic salts, the salts considered here are called oxygenated salts or oxosalts. They are divided according to the composition of cations and anions:

Medium salts contain medium acid residues CO 3 2- , NO 3 - , PO 4 3- , SO 4 2- and others; for example: K 2 CO 3, Mg (NO 3) 2, Cr 2 (SO 4) 3, Zn 3 (PO 4) 2.

If medium salts are obtained by reactions involving hydroxides, then the reagents are taken in equivalent quantities. For example, salt K 2 CO 3 can be obtained by taking the reagents in the ratios:

2KOH and 1H 2 CO 3, 1K 2 O and 1H 2 CO 3, 2KOH and 1CO 2.

Reactions for the formation of medium salts:

Base + Acid > Salt + Water

1a) basic hydroxide + acid hydroxide >…

2NaOH + H 2 SO 4 \u003d Na 2 SO 4 + 2H 2 O

Cu(OH) 2 + 2HNO 3 = Cu(NO 3) 2 + 2H 2 O

1b) amphoteric hydroxide + acidic hydroxide >…

2Al (OH) 3 + 3H 2 SO 4 \u003d Al 2 (SO 4) 3 + 6H 2 O

Zn (OH) 2 + 2HNO 3 \u003d Zn (NO 3) 2 + 2H 2 O

1c) basic hydroxide + amphoteric hydroxide >…

NaOH + Al (OH) 3 \u003d NaAlO 2 + 2H 2 O (in melt)

2NaOH + Zn(OH) 2 = Na 2 ZnO 2 + 2H 2 O (in melt)

Basic Oxide + Acid = Salt + Water

2a) basic oxide + acidic hydroxide >…

Na 2 O + H 2 SO 4 \u003d Na 2 SO 4 + H 2 O

CuO + 2HNO 3 \u003d Cu (NO 3) 2 + H 2 O

2b) amphoteric oxide+ acid hydroxide >…

Al 2 O 3 + 3H 2 SO 4 \u003d Al 2 (SO 4) 3 + 3H 2 O

ZnO + 2HNO 3 \u003d Zn (NO 3) 2 + H 2 O

2c) basic oxide + amphoteric hydroxide >…

Na 2 O + 2Al (OH) 3 \u003d 2NaAlO 2 + ZN 2 O (in melt)

Na 2 O + Zn(OH) 2 = Na 2 ZnO 2 + H 2 O (in melt)

Base + Acid oxide > Salt + Water

For) basic hydroxide + acid oxide > ...

2NaOH + SO 3 \u003d Na 2 SO 4 + H 2 O

Ba (OH) 2 + CO 2 \u003d BaCO 3 + H 2 O

3b) amphoteric hydroxide + acid oxide >…

2Al (OH) 3 + 3SO 3 \u003d Al 2 (SO 4) 3 + 3H 2 O

Zn (OH) 2 + N 2 O 5 \u003d Zn (NO 3) 2 + H 2 O

Sv) basic hydroxide + amphoteric oxide >…

2NaOH + Al 2 O 3 \u003d 2NaAlO 2 + H 2 O (in melt)

2NaOH + ZnO = Na 2 ZnO 2 + H 2 O (in melt)

Basic oxide + Acid oxide > Salt

4a) basic oxide + acid oxide >…

Na 2 O + SO 3 \u003d Na 2 SO 4, BaO + CO 2 \u003d BaCO 3

4b) amphoteric oxide + acidic oxide >…

Al 2 O 3 + 3SO 3 \u003d Al 2 (SO 4) 3, ZnO + N 2 O 5 \u003d Zn (NO 3) 2

4c) basic oxide + amphoteric oxide >…

Na 2 O + Al 2 O 3 \u003d 2NaAlO 2, Na 2 O + ZnO \u003d Na 2 ZnO 2

Reactions 1c, if they proceed in solution, accompanied by the formation of other products - complex salts:

NaOH (conc.) + Al(OH) 3 = Na

KOH (conc.) + Cr (OH) 3 \u003d K 3

2NaOH (conc.) + M (OH) 2 \u003d Na 2 (M \u003d Be, Zn)

KOH (conc.) + M (OH) 2 \u003d K (M \u003d Sn, Pb)

All medium salts in solution are strong electrolytes (dissociate completely).

Acid salts contain acidic acid residues (with hydrogen) HCO 3 -, H 2 PO 4 2-, HPO 4 2-, etc., are formed by the action of basic and amphoteric hydroxides or medium salts of an excess of acid hydroxides containing at least two hydrogen atoms in the molecule ; the corresponding acid oxides act similarly:

NaOH + H 2 SO 4 (conc.) = NaHSO 4 + H 2 O

Ba (OH) 2 + 2H 3 RO 4 (conc.) \u003d Ba (H 2 RO 4) 2 + 2H 2 O

Zn (OH) 2 + H 3 PO 4 (conc.) \u003d ZnHPO 4 v + 2H 2 O

PbSO 4 + H 2 SO 4 (conc.) = Pb (HSO 4) 2

K 2 HPO 4 + H 3 PO 4 (conc.) \u003d 2KN 2 PO 4

Ca (OH) 2 + 2EO 2 \u003d Ca (HEO 3) 2 (E \u003d C, S)

Na 2 EO 3 + EO 2 + H 2 O \u003d 2NaHEO 3 (E \u003d C, S)

When the hydroxide of the corresponding metal or amphigen is added, the acid salts are converted into medium ones:

NaHSO 4 + NaOH \u003d Na 2 SO 4 + H 2 O

Pb (HSO 4) 2 + Pb (OH) 2 \u003d 2PbSO 4 v + 2H 2 O

Almost all acid salts are highly soluble in water, completely dissociate (KHCO 3 = K + + HCO 3 -).

Basic salts contain OH hydroxo groups, considered as separate anions, for example FeNO 3 (OH), Ca 2 SO 4 (OH) 2, Cu 2 CO 3 (OH) 2, are formed by the action of acid hydroxides excess basic hydroxide containing at least two hydroxo groups in a formula unit:

Co (OH) 2 + HNO 3 \u003d CoNO 3 (OH) v + H 2 O

2Ni(OH) 2 + H 2 SO 4 = Ni 2 SO 4 (OH) 2 v + 2H 2 O

2Cu(OH) 2 + H 2 CO 3 = Cu 2 CO 3 (OH) 2 v + 2H 2 O

Basic salts formed strong acids, when the corresponding acid hydroxide is added, they go into the average:

CoNO 3 (OH) + HNO 3 \u003d Co (NO 3) 2 + H 2 O

Ni 2 SO 4 (OH) 2 + H 2 SO 4 \u003d 2NiSO 4 + 2H 2 O

Most basic salts are sparingly soluble in water; they are precipitated by co-hydrolysis if formed by weak acids:

2MgCl 2 + H 2 O + 2Na 2 CO 3 \u003d Mg 2 CO 3 (OH) 2 v + CO 2 ^ + 4NaCl

double salts contain two chemically different cations; for example: CaMg (CO 3) 2, KAl (SO 4) 2, Fe (NH 4) 2 (SO 4) 2, LiAl (SiO 3) 2. Many double salts are formed (in the form of crystalline hydrates) during the co-crystallization of the corresponding medium salts from a saturated solution:

K 2 SO 4 + MgSO 4 + 6H 2 O \u003d K 2 Mg (SO 4) 2 6H 2 Ov

Often double salts are less soluble in water compared to individual medium salts.

Binary connections- these are complex substances that do not belong to the classes of oxides, hydroxides and salts and consist of cations and oxygen-free anions (real or conditional).

Their chemical properties are varied and are considered in inorganic chemistry separately for non-metals of different groups Periodic system; in this case, the classification is carried out according to the type of anion.

Examples:

a) halides: OF 2, HF, KBr, PbI 2, NH 4 Cl, BrF 3, IF 7

b) chalcogenides: H 2 S, Na 2 S, ZnS, As 2 S 3, NH 4 HS, K 2 Se, NiSe

in) nitrides: NH 3, NH 3 H 2 O, Li 3 N, Mg 3 N 2, AlN, Si 3 N 4

G) carbides: CH 4 , Be 2 C, Al 4 C 3 , Na 2 C 2 , CaC 2 , Fe 3 C, SiC

e) silicides: Li 4 Si, Mg 2 Si, ThSi 2

e) hydrides: LiH, CaH 2 , AlH 3 , SiH 4

and) peroxide H 2 O 2, Na 2 O 2, CaO 2

h) superoxides: HO 2, KO 2, Ba (O 2) 2

Type chemical bond among these binary compounds are distinguished:

covalent: OF 2, IF 7, H 2 S, P 2 S 5, NH 3, H 2 O 2

ionic: Nal, K 2 Se, Mg 3 N 2, CaC 2, Na 2 O 2, KO 2

Meet double(with two different cations) and mixed(with two different anions) binary compounds, for example: KMgCl 3 , (FeCu)S 2 and Pb(Cl)F, Bi(Cl)O, SCl 2 O 2 , As(O)F 3 .

All ionic complex salts (except hydroxo complex salts) also belong to this class of complex substances (although they are usually considered separately), for example:

SO 4 K 4 Na 3

Cl K 3 K 2

Binary compounds include covalent complex compounds without an outer sphere, for example, and [Na(CO) 4].

By analogy with the relationship of hydroxides and salts, oxygen-free acids and salts are isolated from all binary compounds (other compounds are classified as others).

Anoxic acids contain (like oxo acids) mobile hydrogen H + and therefore exhibit some chemical properties of acid hydroxides (dissociation in water, participation in salt formation reactions as an acid). Common anoxic acids are HF, HCl, HBr, HI, HCN and H 2 S, of which HF, HCN and H 2 S are weak acids, and the rest are strong.

Examples salt formation reactions:

2HBr + ZnO = ZnBr 2 + H 2 O

2H 2 S + Ba (OH) 2 \u003d Ba (HS) 2 + 2H 2 O

2HI + Pb (OH) 2 \u003d Pbl 2 v + 2H 2 O

Metals and amphigenes, standing in the series of voltages to the left of hydrogen and not reacting with water, interact with strong acids HCl, HBr and HI (in general view NG) in a dilute solution and displace hydrogen from them (actual reactions are given):

M + 2NG = MG 2 + H 2 ^ (M = Be, Mg, Zn, Cr, Mn, Fe, Co, Ni)

2M + 6NG = 2MG 3 + H 2 ^ (M = Al, Ga)

Anoxic salts formed by metal and amphigen cations (as well as ammonium NH 4 + cation) and anions (residues) of oxygen-free acids; examples: AgF, NaCl, KBr, PbI 2 , Na 2 S, Ba(HS) 2 , NaCN, NH 4 Cl. They show some chemical properties of oxosalts.

General way obtaining oxygen-free salts with single-element anions - the interaction of metals and amphigens with non-metals F 2, Cl 2, Br 2 and I 2 (in the general form G 2) and sulfur S (actual reactions are given):

2M + G 2 = 2MG (M = Li, Na, K, Rb, Cs, Ag)

M + G 2 \u003d MG 2 (M \u003d Be, Mg, Ca, Sr, Ba, Zn, Mn, Co)

2M + ZG 2 = 2MG 3 (M = Al, Ga, Cr)

2M + S \u003d M 2 S (M \u003d Li, Na, K, Rb, Cs, Ag)

M + S = MS (M = Be, Mg, Ca, Sr, Ba, Zn, Mn, Fe, Co, Ni)

2M + 3S = M 2 S 3 (M = Al, Ga, Cr)

Exceptions:

a) Cu and Ni react only with halogens Cl 2 and Br 2 (products MCl 2, MBr 2)

b) Cr and Mn react with Cl 2, Br 2 and I 2 (products CrCl 3, CrBr 3, CrI 3 and MnCl 2, MnBr 2, MnI 2)

c) Fe reacts with F 2 and Cl 2 (products FeF 3, FeCl 3), with Br 2 (mixture of FeBr 3 and FeBr 2), with I 2 (product FeI 2)

d) Cu reacts with S to form a mixture of products Cu 2 S and CuS

Other binary compounds- all substances of this class, except for oxygen-free acids and salts allocated to separate subclasses.

The methods for obtaining binary compounds of this subclass are diverse, the simplest is the interaction of simple substances (actual reactions are given):

a) halides:

S + 3F 2 \u003d SF 6, N 2 + 3F 2 \u003d 2NF 3

2P + 5G 2 = 2RG 5 (G = F, CI, Br)

C + 2F 2 = CF 4

Si + 2Г 2 = Sir 4 (Г = F, CI, Br, I)

b) chalcogenides:

2As + 3S = As2S3

2E + 5S = E 2 S 5 (E = P, As)

E + 2S = ES 2 (E = C, Si)

c) nitrides:

3H 2 + N 2 2NH 3

6M + N 2 \u003d 2M 3 N (M \u003d Li, Na, K)

3M + N 2 \u003d M 3 N 2 (M \u003d Be, Mg, Ca)

2Al + N 2 = 2AlN

3Si + 2N 2 \u003d Si 3 N 4

d) carbides:

2M + 2C \u003d M 2 C 2 (M \u003d Li, Na)

2Be + C \u003d Be 2 C

M + 2C = MC 2 (M = Ca, Sr, Ba)

4Al + 3C \u003d Al 4 C 3

e) silicides:

4Li + Si = Li 4 Si

2M + Si = M 2 Si (M = Mg, Ca)

f) hydrides:

2M + H 2 \u003d 2MH (M \u003d Li, Na, K)

M + H 2 \u003d MH 2 (M \u003d Mg, Ca)

g) peroxides, superoxides:

2Na + O 2 \u003d Na 2 O 2 (combustion in air)

M + O 2 \u003d MO 2 (M \u003d K, Rb, Cs; combustion in air)

Many of these substances completely react with water (more often they are hydrolyzed without changing the oxidation states of the elements, but hydrides act as reducing agents, and superoxides enter into dismutation reactions):

PCl 5 + 4H 2 O \u003d H 3 PO 4 + 5HCl

SiBr 4 + 2H 2 O \u003d SiO 2 v + 4HBr

P 2 S 5 + 8H 2 O \u003d 2H 3 PO 4 + 5H 2 S ^

SiS 2 + 2H 2 O \u003d SiO 2 v + 2H 2 S

Mg 3 N 2 + 8H 2 O \u003d 3Mg (OH) 2 v + 2 (NH 3 H 2 O)

Na 3 N + 4H 2 O \u003d 3NaOH + NH 3 H 2 O

Be 2 C + 4H 2 O \u003d 2Be (OH) 2 v + CH 4 ^

MC 2 + 2H 2 O \u003d M (OH) 2 + C 2 H 2 ^ (M \u003d Ca, Sr, Ba)

Al 4 C 3 + 12H 2 O \u003d 4Al (OH) 3 v + 3CH 4 ^

MH + H 2 O \u003d MOH + H 2 ^ (M \u003d Li, Na, K)

MgH 2 + 2H 2 O \u003d Mg (OH) 2 v + H 2 ^

CaH 2 + 2H 2 O \u003d Ca (OH) 2 + H 2 ^

Na 2 O 2 + 2H 2 O \u003d 2NaOH + H 2 O 2

2MO 2 + 2H 2 O = 2MOH + H 2 O 2 + O 2 ^ (M = K, Rb, Cs)

Other substances, on the contrary, are resistant to water, among them SF 6, NF 3, CF 4, CS 2, AlN, Si 3 N 4, SiC, Li 4 Si, Mg 2 Si and Ca 2 Si.

Examples of tasks for parts A, B, C

1. Simple substances are

1) fullerene

2. In formula units of reaction products

Si + CF1 2 >…, Si + O 2 >…, Si + Mg >…

3. In metal-containing reaction products

Na + H 2 O >…, Ca + H 2 O >…, Al + HCl (solution) >…

total amount the number of atoms of all elements is

4. Calcium oxide can react (individually) with all substances of the set

1) CO 2, NaOH, NO

2) HBr, SO 3, NH 4 Cl

3) BaO, SO 3 , KMgCl 3

4) O 2, Al 2 O 3, NH 3

5. There will be a reaction between sulfur oxide (IV) and

6. Salt МAlO 2 is formed during fusion

2) Al 2 O 3 and KOH

3) Al and Ca (OH) 2

4) Al 2 O 3 and Fe 2 O 3

7. In molecular equation reactions

ZnO + HNO 3 > Zn(NO 3) 2 +…

the sum of the coefficients is

8. The products of the reaction N 2 O 5 + NaOH > ... are

1) Na 2 O, HNO 3

3) NaNO 3 , H 2 O

4) NaNO 2, N 2, H 2 O

9. A set of bases is

1) NaOH, LiOH, ClOH

2) NaOH, Ba (OH) 2, Cu (OH) 2

3) Ca (OH) 2, KOH, BrOH

4) Mg (OH) 2, Be (OH) 2, NO (OH)

10. Potassium hydroxide reacts in solution (separately) with the substances of the set

4) SO 3, FeCl 3

11–12. The residue corresponding to the acid named

11. sulfuric

12. Nitrogen

has the formula

13. From hydrochloric and dilute sulfuric acids does not highlight gas only metal

14. Amphoteric hydroxide is

15-16. According to the given formulas of hydroxides

15. H 3 PO 4 , Pb(OH) 2

16. Cr(OH) 3 , HNO 3

the formula for average salt is derived

1) Pb 3 (PO 4) 2

17. After passing excess H 2 S through a solution of barium hydroxide, the final solution will contain salt

18. Possible reactions:

1) CaSO 3 + H 2 SO 4 >…

2) Ca(NO 3) 2 + HNO 3 >…

3) NaHCOg + K 2 SO 4 >…

4) Al(HSO 4) 3 + NaOH >…

19. In the reaction equation (CaOH) 2 CO 3 (t) + H 3 PO 4 > CaHPO 4 v + ...

the sum of the coefficients is

20. Establish a correspondence between the formula of the substance and the group to which it belongs.

21. Establish a correspondence between the starting materials and reaction products.

22. In the scheme of transformations

substances A and B are indicated in the set

1) NaNO 3, H 2 O

4) HNO 3, H 2 O

23. Make equations of possible reactions according to the scheme

FeS > H 2 S + PbS > PbSO 4 > Pb(HSO 4) 2

24. Make equations for four possible reactions between substances:

1) Nitric acid(conc.)

2) carbon (graphite or coke)

3) calcium oxide

Elements conventionally divided into elements with metallic and non-metallic properties. The first of these is always included in cations multielement substances (metal properties), the second - in the composition anions (non-metallic properties). In accordance with the Periodic Law, in periods and groups between these elements there are amphoteric elements that simultaneously exhibit metallic and non-metallic to one degree or another. (amphoteric, dual) properties. Group VIIIA elements continue to be considered separately (noble gases), although for Kr, Xe and Rn clearly non-metallic properties were found (the elements He, Ne, Ar are chemically inert).

The classification of simple and complex inorganic substances is given in Table. 6.

Below are the definitions (definitions) of classes of inorganic substances, their most important chemical properties and methods of obtaining.

inorganic substances- compounds formed by all chemical elements (except for most organic carbon compounds). They are divided according to their chemical composition:

Simple substances made up of atoms of the same element. They are divided according to their chemical properties:

Metals- simple substances of elements with metallic properties (low electronegativity). Typical metals:

The simple substances of the elements Cu, Ag and Ni are also referred to as metals, since their oxides CuO, Ag 2 O, NiO and hydroxides Cu (OH) 2, Ni (OH) 2 are dominated by basic properties.

non-metals- simple substances of elements with non-metallic properties (high electronegativity). Typical non-metals: F 2, Cl 2, Br 2, I 2, O 2, S, N 2, P, C, Si.

Nonmetals have a high oxidizing power compared to typical metals.

Amphigenes have a lower reducing power compared to typical metals. In the electrochemical series of voltages, they adjoin hydrogen on the left or stand behind it on the right.

Aerogens- noble gases, monatomic simple substances of elements of group VIIIA‑group: He, Ne, Ar, Kr, Xe, Rn. Of these, He, Ne, and Ar are chemically passive (compounds with other elements have not been obtained), while Kr, Xe, and Rn exhibit some of the properties of non-metals with high electronegativity.

Complex Substances made up of atoms of different elements. Divided by composition and chemical properties:

oxides- compounds of elements with oxygen, the oxidation state of oxygen in oxides is always equal to (-II). Divided by composition and chemical properties:

Basic oxides- products of complete dehydration (real or conditional) of basic hydroxides retain the chemical properties of the latter.

Of the typical metals, only Li, Mg, Ca, and Sr form the oxides Li 2 O, MgO, CaO, and SrO when burned in air; oxides of Na 2 O, K 2 O, Rb 2 O, Cs 2 O and BaO are obtained by other methods.

Oxides CuO, Ag 2 O and NiO are also classified as basic.

Acid oxides- products of complete dehydration (real or conditional) of acid hydroxides, retain the chemical properties of the latter.

a) 2NO 2 + 2NaOH \u003d NaNO 2 + NaNO 3 + H 2 O

b) 2ClO 2 + H 2 O (cold) = HClO 2 + HClO 3

2ClO 2 + 2NaOH (cold) = NaClO 2 + NaClO 3 + H 2 O

Oxides CrO 3 and Mn 2 O 7 (chromium and manganese in the highest oxidation state) are also acidic.

Amphoteric oxides- products of complete dehydration (real or conditional) of amphoteric hydroxides retain the chemical properties of amphoteric hydroxides.

Typical amphigenes (except Ga) when burned in air form the oxides BeO, Cr 2 O 3 , ZnO, Al 2 O 3 , GeO 2 , SnO 2 and PbO; amphoteric oxides Ga 2 O 3 , SnO and PbO 2 are obtained by other methods.

(Fe II Fe 2 III) O 4 , (Рb 2 II Pb IV) O 4 , (MgAl 2) O 4 , (CaTi) O 3 .

Iron oxide is formed by the combustion of iron in air, lead oxide - by weak heating of lead in oxygen; oxides of two different metals are obtained by other methods.

Hydroxides- compounds of elements (except for fluorine and oxygen) with hydroxo groups O ‑II H, may also contain oxygen O ‑II. In hydroxides, the oxidation state of an element is always positive (from +I to +VIII). The number of hydroxo groups is from 1 to 6. They are divided by chemical properties:

Basic hydroxides (bases) formed by elements with metallic properties.

Obtained by the reactions of the corresponding basic oxides with water:

M 2 O + H 2 O \u003d 2MON (M \u003d Li, Na, K, Rb, Cs)

MO + H 2 O \u003d M (OH) 2 (M \u003d Ca, Sr, Ba)

Exception: Mg(OH) 2, Cu(OH) 2 and Ni(OH) 2 hydroxides are obtained by other methods.

When heated, real dehydration (loss of water) occurs for the following hydroxides:

2LiOH \u003d Li 2 O + H 2 O

M (OH) 2 \u003d MO + H 2 O (M \u003d Mg, Ca, Sr, Ba, Cu, Ni)

Basic hydroxides replace their hydroxo groups with acidic residues to form salts; metallic elements retain their oxidation state in salt cations.

Basic hydroxides that are readily soluble in water (NaOH, KOH, Ca (OH) 2, Ba (OH) 2, etc.) are called alkalis, since it is with their help that an alkaline environment is created in the solution.

Acid hydroxides (acids) formed by elements with non-metallic properties. Examples:

Dissociation in a dilute aqueous solution produces H + cations (more precisely, H 3 O +) and the following anions, or acid residues:

Acids can be obtained by reactions of the corresponding acid oxides with water (the following are the actual reactions taking place):

Cl 2 O + H 2 O \u003d 2HClO

E 2 O 3 + H 2 O \u003d 2NEO 2 (E \u003d N, As)

As 2 O 3 + 3H 2 O \u003d 2H 3 AsO 3

EO 2 + H 2 O \u003d H 2 EO 3 (E \u003d C, Se)

E 2 O 5 + H 2 O \u003d 2HEO 3 (E \u003d N, P, I)

E 2 O 5 + 3H 2 O \u003d 2H 3 EO 4 (E \u003d P, As)

EO 3 + H 2 O = H 2 EO 4 (E = S, Se, Cr)

E 2 O 7 + H 2 O \u003d 2HEO 4 (E \u003d Cl, Mn)

Exception: SO 2 oxide as acidic hydroxide corresponds to SO 2 polyhydrate n H 2 O (“sulphurous acid H 2 SO 3” does not exist, but acid residues HSO 3 - and SO 3 2 - are present in salts).

When some acids are heated, real dehydration occurs and the corresponding acid oxides are formed:

2HAsO 2 \u003d As 2 O 3 + H 2 O

H 2 EO 3 \u003d EO 2 + H 2 O (E \u003d C, Si, Ge, Se)

2HIO 3 \u003d I 2 O 5 + H 2 O

2H 3 AsO 4 \u003d As 2 O 5 + H 2 O

H 2 SeO 4 \u003d SeO 3 + H 2 O

M + H 2 SO 4 (pasb.) \u003d MSO 4 + H 2 (M \u003d Be, Mg, Cr, Mn, Zn, Fe, Ni)

2M + 3H 2 SO 4 (razb.) \u003d M 2 (SO 4) 3 + 3H 2 (M \u003d Al, Ga)

3M + 2H 3 PO 4 (razb.) \u003d M 3 (PO 4) 2 ↓ + 3H 2 (M \u003d Mg, Fe, Zn)

Unlike anoxic acids, acidic hydroxides are called oxygenated acids or oxoacids.

Amphoteric hydroxides formed by elements with amphoteric properties. Typical amphoteric hydroxides:

Be(OH) 2 Sn(OH) 2 Al(OH) 3 AlO(OH)

Zn(OH) 2 Pb(OH) 2 Cr(OH) 3 CrO(OH)

He are formed from amphoteric oxides and water, but undergo real dehydration and form amphoteric oxides:

Exception: for iron(III) only metahydroxide FeO(OH) is known, "iron(III) hydroxide Fe(OH) 3" does not exist (not obtained).

Amphoteric hydroxides exhibit the properties of basic and acidic hydroxides; form two types of salts, in which the amphoteric element is part of either salt cations or their anions.

For elements with several oxidation states, the rule applies: the higher the oxidation state, the more pronounced the acidic properties of hydroxides (and/or the corresponding oxides).

Medium salts contain medium acid residues CO 3 2-, NO 3 -, PO 4 3-, SO 4 2-, etc.; for example: K 2 CO 3, Mg (NO 3) 2, Cr 2 (SO 4) 3, Zn 3 (PO 4) 2.

If medium salts are obtained by reactions involving hydroxides, then the reagents are taken in equivalent quantities. For example, salt K 2 CO 3 can be obtained by taking the reagents in the ratios:

2KOH and 1H 2 CO 3, 1K 2 O and 1H 2 CO 3, 2KOH and 1CO 2.

Reactions for the formation of medium salts:

Base + Acid → Salt + Water

1a) basic hydroxide + acidic hydroxide →…

2NaOH + H 2 SO 4 \u003d Na 2 SO 4 + 2H 2 O

Cu(OH) 2 + 2HNO 3 = Cu(NO 3) 2 + 2H 2 O

1b) amphoteric hydroxide + acidic hydroxide →…

2Al (OH) 3 + 3H 2 SO 4 \u003d Al 2 (SO 4) 3 + 6H 2 O

Zn (OH) 2 + 2HNO 3 \u003d Zn (NO 3) 2 + 2H 2 O

1c) basic hydroxide + amphoteric hydroxide →…

NaOH + Al (OH) 3 \u003d NaAlO 2 + 2H 2 O (in melt)

2NaOH + Zn(OH) 2 = Na 2 ZnO 2 + 2H 2 O (in melt)

Basic Oxide + Acid = Salt + Water

2a) basic oxide + acidic hydroxide →…

Na 2 O + H 2 SO 4 \u003d Na 2 SO 4 + H 2 O

CuO + 2HNO 3 \u003d Cu (NO 3) 2 + H 2 O

2b) amphoteric oxide + acidic hydroxide →…

Al 2 O 3 + 3H 2 SO 4 \u003d Al 2 (SO 4) 3 + 3H 2 O

ZnO + 2HNO 3 \u003d Zn (NO 3) 2 + H 2 O

2c) basic oxide + amphoteric hydroxide →…

Na 2 O + 2Al (OH) 3 \u003d 2NaAlO 2 + ZN 2 O (in melt)

Na 2 O + Zn(OH) 2 = Na 2 ZnO 2 + H 2 O (in melt)

Base + Acid oxide → Salt + Water

For) basic hydroxide + acid oxide → ...

2NaOH + SO 3 \u003d Na 2 SO 4 + H 2 O

Ba (OH) 2 + CO 2 \u003d BaCO 3 + H 2 O

3b) amphoteric hydroxide + acid oxide →…

2Al (OH) 3 + 3SO 3 \u003d Al 2 (SO 4) 3 + 3H 2 O

Zn (OH) 2 + N 2 O 5 \u003d Zn (NO 3) 2 + H 2 O

Sv) basic hydroxide + amphoteric oxide →…

2NaOH + Al 2 O 3 \u003d 2NaAlO 2 + H 2 O (in melt)

2NaOH + ZnO = Na 2 ZnO 2 + H 2 O (in melt)

Basic oxide + Acid oxide → Salt

4a) basic oxide + acidic oxide →…

Na 2 O + SO 3 \u003d Na 2 SO 4, BaO + CO 2 \u003d BaCO 3

4b) amphoteric oxide + acidic oxide →…

Al 2 O 3 + 3SO 3 \u003d Al 2 (SO 4) 3, ZnO + N 2 O 5 \u003d Zn (NO 3) 2

4c) basic oxide + amphoteric oxide →…

Na 2 O + Al 2 O 3 \u003d 2NaAlO 2, Na 2 O + ZnO \u003d Na 2 ZnO 2

Reactions 1c, if they proceed in solution, accompanied by the formation of other products - complex salts:

NaOH (conc.) + Al(OH) 3 = Na

KOH (conc.) + Cr (OH) 3 \u003d K 3

2NaOH (conc.) + M (OH) 2 \u003d Na 2 (M \u003d Be, Zn)

KOH (conc.) + M (OH) 2 \u003d K (M \u003d Sn, Pb)

All medium salts in solution are strong electrolytes (dissociate completely).

NaOH + H 2 SO 4 (conc.) = NaHSO 4 + H 2 O

Ba (OH) 2 + 2H 3 RO 4 (conc.) \u003d Ba (H 2 RO 4) 2 + 2H 2 O

Zn (OH) 2 + H 3 PO 4 (conc.) \u003d ZnHPO 4 ↓ + 2H 2 O

PbSO 4 + H 2 SO 4 (conc.) = Pb (HSO 4) 2

K 2 HPO 4 + H 3 PO 4 (conc.) \u003d 2KN 2 PO 4

Ca (OH) 2 + 2EO 2 \u003d Ca (HEO 3) 2 (E \u003d C, S)

Na 2 EO 3 + EO 2 + H 2 O \u003d 2NaHEO 3 (E \u003d C, S)

When the hydroxide of the corresponding metal or amphigen is added, the acid salts are converted into medium ones:

NaHSO 4 + NaOH \u003d Na 2 SO 4 + H 2 O

Pb (HSO 4) 2 + Pb (OH) 2 \u003d 2PbSO 4 ↓ + 2H 2 O

Almost all acid salts are highly soluble in water, completely dissociate (KHCO 3 = K + + HCO 3 -).

Co (OH) 2 + HNO 3 \u003d CoNO 3 (OH) ↓ + H 2 O

2Ni(OH) 2 + H 2 SO 4 = Ni 2 SO 4 (OH) 2 ↓ + 2H 2 O

2Cu(OH) 2 + H 2 CO 3 = Cu 2 CO 3 (OH) 2 ↓ + 2H 2 O

Basic salts formed by strong acids, when the corresponding acid hydroxide is added, turn into medium ones:

CoNO 3 (OH) + HNO 3 \u003d Co (NO 3) 2 + H 2 O

Ni 2 SO 4 (OH) 2 + H 2 SO 4 \u003d 2NiSO 4 + 2H 2 O

Most basic salts are sparingly soluble in water; they are precipitated by co-hydrolysis if formed by weak acids:

2MgCl 2 + H 2 O + 2Na 2 CO 3 \u003d Mg 2 CO 3 (OH) 2 ↓ + CO 2 + 4NaCl

K 2 SO 4 + MgSO 4 + 6H 2 O \u003d K 2 Mg (SO 4) 2 6H 2 O ↓

Often double salts are less soluble in water compared to individual medium salts.

Binary connections- these are complex substances that do not belong to the classes of oxides, hydroxides and salts and consist of cations and oxygen-free anions (real or conditional).

Their chemical properties are diverse and are considered in inorganic chemistry separately for non-metals of different groups of the Periodic system; in this case, the classification is carried out according to the type of anion.

Examples:

a) halides: OF 2, HF, KBr, PbI 2, NH 4 Cl, BrF 3, IF 7

b) chalcogenides: H 2 S, Na 2 S, ZnS, As 2 S 3, NH 4 HS, K 2 Se, NiSe

in) nitrides: NH 3, NH 3 H 2 O, Li 3 N, Mg 3 N 2, AlN, Si 3 N 4

G) carbides: CH 4 , Be 2 C, Al 4 C 3 , Na 2 C 2 , CaC 2 , Fe 3 C, SiC

e) silicides: Li 4 Si, Mg 2 Si, ThSi 2

e) hydrides: LiH, CaH 2 , AlH 3 , SiH 4

and) peroxide H 2 O 2, Na 2 O 2, CaO 2

h) superoxides: HO 2, KO 2, Ba (O 2) 2

By the type of chemical bond among these binary compounds are distinguished:

covalent: OF 2, IF 7, H 2 S, P 2 S 5, NH 3, H 2 O 2

ionic: Nal, K 2 Se, Mg 3 N 2, CaC 2, Na 2 O 2, KO 2

Meet double(with two different cations) and mixed(with two different anions) binary compounds, for example: KMgCl 3 , (FeCu)S 2 and Pb(Cl)F, Bi(Cl)O, SCl 2 O 2 , As(O)F 3 .

All ionic complex salts (except hydroxo complex salts) also belong to this class of complex substances (although they are usually considered separately), for example:

SO 4 K 4 Na 3

Cl K 3 K 2

Binary compounds include covalent complex compounds without an outer sphere, for example, and [Na(CO) 4].

By analogy with the relationship of hydroxides and salts, oxygen-free acids and salts are isolated from all binary compounds (other compounds are classified as others).

Examples salt formation reactions:

2HBr + ZnO = ZnBr 2 + H 2 O

2H 2 S + Ba (OH) 2 \u003d Ba (HS) 2 + 2H 2 O

2HI + Pb (OH) 2 \u003d Pbl 2 ↓ + 2H 2 O

Metals and amphigenes, standing in the series of voltages to the left of hydrogen and not reacting with water, interact with strong acids HCl, HBr and HI (in the general form NH) in a dilute solution and displace hydrogen from them (actual reactions are given):

M + 2NG = MG 2 + H 2 (M = Be, Mg, Zn, Cr, Mn, Fe, Co, Ni)

2M + 6NG = 2MG 3 + H 2 (M = Al, Ga)

The general method for obtaining oxygen-free salts with single-element anions is the interaction of metals and amphigens with non-metals F 2, Cl 2, Br 2 and I 2 (in the general form G 2) and sulfur S (real reactions are shown):

2M + G 2 = 2MG (M = Li, Na, K, Rb, Cs, Ag)

M + G 2 \u003d MG 2 (M \u003d Be, Mg, Ca, Sr, Ba, Zn, Mn, Co)

2M + ZG 2 = 2MG 3 (M = Al, Ga, Cr)

2M + S \u003d M 2 S (M \u003d Li, Na, K, Rb, Cs, Ag)

M + S = MS (M = Be, Mg, Ca, Sr, Ba, Zn, Mn, Fe, Co, Ni)

2M + 3S = M 2 S 3 (M = Al, Ga, Cr)

Exceptions:

a) Cu and Ni react only with halogens Cl 2 and Br 2 (products MCl 2, MBr 2)

b) Cr and Mn react with Cl 2, Br 2 and I 2 (products CrCl 3, CrBr 3, CrI 3 and MnCl 2, MnBr 2, MnI 2)

c) Fe reacts with F 2 and Cl 2 (products FeF 3, FeCl 3), with Br 2 (mixture of FeBr 3 and FeBr 2), with I 2 (product FeI 2)

d) Cu reacts with S to form a mixture of products Cu 2 S and CuS

Other binary compounds- all substances of this class, except for oxygen-free acids and salts allocated to separate subclasses.

The methods for obtaining binary compounds of this subclass are diverse, the simplest is the interaction of simple substances (actual reactions are given):

a) halides:

S + 3F 2 \u003d SF 6, N 2 + 3F 2 \u003d 2NF 3

2P + 5G 2 = 2RG 5 (G = F, CI, Br)

C + 2F 2 = CF 4

Si + 2Г 2 = Sir 4 (Г = F, CI, Br, I)

b) chalcogenides:

2As + 3S = As2S3

2E + 5S = E 2 S 5 (E = P, As)

E + 2S = ES 2 (E = C, Si)

c) nitrides:

6M + N 2 \u003d 2M 3 N (M \u003d Li, Na, K)

3M + N 2 \u003d M 3 N 2 (M \u003d Be, Mg, Ca)

2Al + N 2 = 2AlN

3Si + 2N 2 \u003d Si 3 N 4

d) carbides:

2M + 2C \u003d M 2 C 2 (M \u003d Li, Na)

2Be + C \u003d Be 2 C

M + 2C = MC 2 (M = Ca, Sr, Ba)

4Al + 3C \u003d Al 4 C 3

e) silicides:

4Li + Si = Li 4 Si

2M + Si = M 2 Si (M = Mg, Ca)

f) hydrides:

2M + H 2 \u003d 2MH (M \u003d Li, Na, K)

M + H 2 \u003d MH 2 (M \u003d Mg, Ca)

g) peroxides, superoxides:

2Na + O 2 \u003d Na 2 O 2 (combustion in air)

M + O 2 \u003d MO 2 (M \u003d K, Rb, Cs; combustion in air)

PCl 5 + 4H 2 O \u003d H 3 PO 4 + 5HCl

SiBr 4 + 2H 2 O \u003d SiO 2 ↓ + 4HBr

P 2 S 5 + 8H 2 O \u003d 2H 3 PO 4 + 5H 2 S

SiS 2 + 2H 2 O \u003d SiO 2 ↓ + 2H 2 S

Mg 3 N 2 + 8H 2 O \u003d 3Mg (OH) 2 ↓ + 2 (NH 3 H 2 O)

Na 3 N + 4H 2 O \u003d 3NaOH + NH 3 H 2 O

Be 2 C + 4H 2 O \u003d 2Be (OH) 2 ↓ + CH 4

MC 2 + 2H 2 O \u003d M (OH) 2 + C 2 H 2 (M \u003d Ca, Sr, Ba)

Al 4 C 3 + 12H 2 O \u003d 4Al (OH) 3 ↓ + 3CH 4

MH + H 2 O \u003d MOH + H 2 (M \u003d Li, Na, K)

MgH 2 + 2H 2 O \u003d Mg (OH) 2 ↓ + H 2

CaH 2 + 2H 2 O \u003d Ca (OH) 2 + H 2

Na 2 O 2 + 2H 2 O \u003d 2NaOH + H 2 O 2

2MO 2 + 2H 2 O = 2MOH + H 2 O 2 + O 2 (M = K, Rb, Cs)

Other substances, on the contrary, are resistant to water, among them SF 6, NF 3, CF 4, CS 2, AlN, Si 3 N 4, SiC, Li 4 Si, Mg 2 Si and Ca 2 Si.

inorganic substances

genetic series

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