Who reacts with what table. Types of chemical reactions. Double substitution reactions

The material world in which we live and of which we are a tiny particle is one and at the same time infinitely diverse. Unity and diversity chemical substances of this world is most clearly manifested in the genetic connection of substances, which is reflected in the so-called genetic series. Let's highlight the most characteristic features of such series.

1. All substances of this series must be formed by one chemical element. For example, a series written using the following formulas:

2. Substances formed by the same element must belong to different classes, ie, reflect different forms of its existence.

3. Substances that form the genetic line of one element must be linked by interconversions. On this basis, complete and incomplete genetic series can be distinguished.

For example, the above genetic lineup of bromine will be incomplete, incomplete. And here is the next row:

can already be regarded as complete: it began with a simple substance with bromine and ended with it.

Summarizing the above, we can give the following definition of the genetic series.

Genetic series is a number of substances - representatives different classes, which are compounds of one chemical element, interconverted and reflecting the common origin of these substances or their genesis.

Genetic link- the concept is more general than the genetic series, which is, albeit a bright, but a particular manifestation of this connection, which is realized in any mutual transformations of substances. Then, obviously, the first given series of substances also fits this definition.

There are three types of genetic series:

The richest range of metals exhibits different oxidation states. As an example, consider the genetic line of iron with oxidation states +2 and +3:

Recall that to oxidize iron to iron (II) chloride, you need to take a weaker oxidizing agent than to obtain iron (III) chloride:

Similarly to the metal series, a number of nonmetals with different oxidation states are richer in bonds, for example, the genetic series of sulfur with oxidation states +4 and +6:

Only the last transition can cause difficulty. Follow the rule: in order to obtain a simple substance from an oxidized compound of an element, you need to take for this purpose its most reduced compound, for example, a volatile hydrogen compound of a non-metal. In our case:

According to this reaction, sulfur is formed in nature from volcanic gases.

Similarly for chlorine:

3. The genetic series of the metal, which corresponds to the amphoteric oxide and hydroxide,very rich in bonds, since, depending on the conditions, they exhibit either acidic or basic properties.

For example, consider the genetic makeup of zinc:

Genetic relationship between classes of inorganic substances

Reactions between representatives of different genetic lines are characteristic. Substances from the same genetic series, as a rule, do not interact.

For example:
1.metal + non-metal = salt

Hg + S = HgS

2Al + 3I 2 = 2AlI 3

2.basic oxide + acid oxide= salt

Li 2 O + CO 2 = Li 2 CO 3

CaO + SiO 2 = CaSiO 3

3.base + acid = salt

Cu (OH) 2 + 2HCl = CuCl 2 + 2H 2 O

FeCl 3 + 3HNO 3 = Fe (NO 3) 3 + 3HCl

salt acid salt acid

4.metal - basic oxide

2Ca + O 2 = 2CaO

4Li + O 2 = 2Li 2 O

5.non-metal - acidic oxide

S + O 2 = SO 2

4As + 5O 2 = 2As 2 O 5

6.basic oxide - base

BaO + H 2 O = Ba (OH) 2

Li 2 O + H 2 O = 2LiOH

7.acid oxide - acid

P 2 O 5 + 3H 2 O = 2H 3 PO 4

SO 3 + H 2 O = H 2 SO 4

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

The elements are conventionally divided into elements with metallic and non-metallic properties. The first of them are always included in the composition cations multielement substances (metal properties), the second - in the composition anions (non-metallic properties). In accordance with By the Periodic Law in periods and groups between these elements there are amphoteric elements, exhibiting simultaneously to one degree or another metallic and non-metallic (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 the classes of inorganic substances, their most important chemical properties and methods of preparation.

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

Simple substances formed by atoms of one element. Divided by chemical properties:

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

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

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.

Nonmetals- 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.

Non-metals are highly oxidizing compared to typical metals.

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

Amphigens have lower reducibility than typical metals. In the electrochemical series of voltages, they are adjacent to the left of hydrogen or stand behind it on the right.

Aerogens- noble gases, monatomic simple substances of the elements of the 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), and Kr, Xe, and Rn exhibit some properties of non-metals with high electronegativity.

Complex substances formed by 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 (-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. Mixed binary compounds, for example S + IV Cl 2 -I O-II, do not belong to oxides.

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 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 referred to as basic.

Acidic oxides- products of complete dehydration (real or conditional) of acidic 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: oxides NO 2 and ClO 2 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 = 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 amphigens (except Ga), when burned in air, form 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 formed either by atoms of one amphoteric element in different degrees oxidation, or by atoms of two different (metallic, amphoteric) elements, which determines their chemical properties. Examples:

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

Iron oxide is formed when iron is burned in air, lead oxide is formed when lead is weakly heated in oxygen; oxides of two different metals are obtained in other ways.

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

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 the element is always positive (from + I to + VIII). The number of hydroxyl groups is from 1 to 6. They are divided according to their 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 = 2MON (M = Li, Na, K, Rb, Cs)

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

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

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

2LiOH = Li 2 O + H 2 O

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

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

Basic hydroxides well 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:

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

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

Cl 2 O + H 2 O = 2HClO

E 2 O 3 + H 2 O = 2HEO 2 (E = N, As)

As 2 O 3 + 3H 2 O = 2H 3 AsO 3

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

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

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

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

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

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

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

2HAsO 2 = As 2 O 3 + H 2 O

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

2HIO 3 = I 2 O 5 + H 2 O

2H 3 AsO 4 = As 2 O 5 + H 2 O

H 2 SeO 4 = SeO 3 + H 2 O

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

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

2M + 3H 2 SO 4 (par.) = M 2 (SO 4) 3 + 3H 2 ^ (M = Al, Ga)

3M + 2H 3 PO 4 (dil.) = M 3 (PO 4) 2 v + 3H 2 ^ (M = Mg, Fe, Zn)

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

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 is formed from amphoteric oxides and water, but undergoes 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 a 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 corresponding oxides).

Salt- connections consisting of cations basic or amphoteric (in the role of basic) hydroxides and anions(residues) acidic or amphoteric (in the role of acidic) hydroxides. Unlike 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-, etc .; for example: K 2 CO 3, Mg (NO 3) 2, Cr 2 (SO 4) 3, Zn 3 (PO 4) 2.

If average salts are obtained by reactions involving hydroxides, then the reagents are taken in equivalent amounts. For example, the 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 of the formation of medium salts:

Base + Acid> Salt + Water

1а) basic hydroxide + acidic hydroxide> ...

2NaOH + H 2 SO 4 = 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 = Al 2 (SO 4) 3 + 6H 2 O

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

1c) basic hydroxide + amphoteric hydroxide> ...

NaOH + Al (OH) 3 = NaAlO 2 + 2H 2 O (in the melt)

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

Basic Oxide + Acid = Salt + Water

2а) basic oxide + acidic hydroxide> ...

Na 2 O + H 2 SO 4 = Na 2 SO 4 + H 2 O

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

2b) amphoteric oxide + acidic hydroxide> ...

Al 2 O 3 + 3H 2 SO 4 = Al 2 (SO 4) 3 + 3H 2 O

ZnO + 2HNO 3 = Zn (NO 3) 2 + H 2 O

2c) basic oxide + amphoteric hydroxide> ...

Na 2 O + 2Al (OH) 3 = 2NaAlO 2 + ЗН 2 O (in the melt)

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

Base + Acid Oxide> Salt + Water

For) basic hydroxide + acidic oxide> ...

2NaOH + SO 3 = Na 2 SO 4 + H 2 O

Ba (OH) 2 + CO 2 = BaCO 3 + H 2 O

3b) amphoteric hydroxide + acidic oxide> ...

2Al (OH) 3 + 3SO 3 = Al 2 (SO 4) 3 + 3H 2 O

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

Sv) basic hydroxide + amphoteric oxide> ...

2NaOH + Al 2 O 3 = 2NaAlO 2 + H 2 O (in the melt)

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

Basic oxide + Acidic oxide> Salt

4а) basic oxide + acidic oxide> ...

Na 2 O + SO 3 = Na 2 SO 4, BaO + CO 2 = BaCO 3

4b) amphoteric oxide + acidic oxide> ...

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

4c) basic oxide + amphoteric oxide> ...

Na 2 O + Al 2 O 3 = 2NaAlO 2, Na 2 O + ZnO = 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 = K 3

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

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

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

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

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

Ba (OH) 2 + 2H 3 PO 4 (conc.) = Ba (H 2 PO 4) 2 + 2H 2 O

Zn (OH) 2 + H 3 PO 4 (conc.) = 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.) = 2KN 2 PO 4

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

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

By adding the corresponding metal hydroxide or amphigenes acidic salts translated into averages:

NaHSO 4 + NaOH = Na 2 SO 4 + H 2 O

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

Almost all acidic salts are readily soluble in water, dissociate completely (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 upon action on acid hydroxides excess basic hydroxide containing at least two hydroxo groups in the formula unit:

Co (OH) 2 + HNO 3 = 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, with the addition of the corresponding acidic hydroxide, they change to the average:

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

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

Most of the basic salts are poorly soluble in water; they precipitate during joint hydrolysis if they are formed by weak acids:

2MgCl 2 + H 2 O + 2Na 2 CO 3 = 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) upon co-crystallization of the corresponding middle salts from a saturated solution:

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

Double salts are often less soluble in water than individual medium salts.

Binary compounds 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 conventional).

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

Examples of:

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

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

v) 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

g) 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 distinguish between:

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 hydroxocomplex) 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 external sphere, for example and [No. (CO) 4].

By analogy with the relationship between hydroxides and salts, anoxic acids and salts are isolated from all binary compounds (the rest of the compounds are classified as others).

Anoxic acids contain (like oxoacids) mobile hydrogen H + and therefore exhibit some chemical properties of acidic 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 of salt formation reactions:

2HBr + ZnO = ZnBr 2 + H 2 O

2H 2 S + Ba (OH) 2 = Ba (HS) 2 + 2H 2 O

2HI + Pb (OH) 2 = Pbl 2 v + 2H 2 O

Metals and amphigens, standing in a 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 (the actual reactions are shown):

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

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

Oxygen-free salts formed by cations of metals and amphigens (as well as ammonium cation NH 4 +) and anions (residues) of anoxic acids; examples: AgF, NaCl, KBr, PbI 2, Na 2 S, Ba (HS) 2, NaCN, NH 4 Cl. Show some chemical properties of oxosalts.

The general method for the preparation of 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 general form G 2) and sulfur S (actual reactions are shown):

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

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

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

2M + S = M 2 S (M = 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 МCl 2, МBr 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 (a mixture of FeBr 3 and FeBr 2), with I 2 (product FeI 2)

d) Cu upon reaction with S forms a mixture of products Cu 2 S and CuS

Other binary compounds- all substances of this class, except for those isolated in separate subclasses of anoxic acids and salts.

Methods for obtaining binary compounds of this subclass are varied, the simplest is the interaction of simple substances (the actual reactions are shown):

a) halides:

S + 3F 2 = SF 6, N 2 + 3F 2 = 2NF 3

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

C + 2F 2 = CF 4

Si + 2G 2 = Sir 4 (G = F, CI, Br, I)

b) chalcogenides:

2As + 3S = As 2 S 3

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 = 2M 3 N (M = Li, Na, K)

3M + N 2 = M 3 N 2 (M = Be, Mg, Ca)

2Al + N 2 = 2AlN

3Si + 2N 2 = Si 3 N 4

d) carbides:

2M + 2C = M 2 C 2 (M = Li, Na)

2Be + C = Be 2 C

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

4Al + 3C = Al 4 C 3

e) silicides:

4Li + Si = Li 4 Si

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

f) hydrides:

2M + H 2 = 2MH (M = Li, Na, K)

M + H 2 = MH 2 (M = Mg, Ca)

g) peroxides, superoxides:

2Na + O 2 = Na 2 O 2 (combustion in air)

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

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

РCl 5 + 4Н 2 O = Н 3 РO 4 + 5НCl

SiBr 4 + 2Н 2 O = SiO 2 v + 4НBr

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

SiS 2 + 2H 2 O = SiO 2 v + 2H 2 S

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

Na 3 N + 4H 2 O = 3NaOH + NH 3 H 2 O

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

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

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

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

MgH 2 + 2H 2 O = Mg (OH) 2 v + H 2 ^

CaH 2 + 2H 2 O = Ca (OH) 2 + H 2 ^

Na 2 O 2 + 2H 2 O = 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.

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)> ...

the total sum of the number of atoms of all elements is

4. Calcium oxide can react (separately) with all substances in 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 by 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 the molecular equation of the reaction

ZnO + HNO 3> Zn (NO 3) 2 + ...

the sum of the coefficients is

8. The reaction products 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. The 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. Residue corresponding to the acid with the name

11. Sulfur

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 medium salt is displayed

1) PL 3 (PO 4) 2

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

18. Probable 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 a 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 the equations of possible reactions according to the scheme

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

24. Make the equations of four possible reactions between substances:

1) nitric acid (conc.)

2) carbon (graphite or coke)

3) calcium oxide

During chemical reactions some substances produce others (not to be confused with nuclear reactions, in which one chemical element turns into another).

Any chemical reaction is described chemical equation :

Reagents → Reaction Products

The arrow indicates the direction of the reaction.

For example:

In this reaction, methane (CH 4) reacts with oxygen (O 2), resulting in the formation of carbon dioxide (CO 2) and water (H 2 O), or rather, water vapor. This is exactly the reaction that happens in your kitchen when you light the gas burner. The equation should be read like this: one molecule of methane gas reacts with two molecules of oxygen gas, resulting in one molecule of carbon dioxide and two molecules of water (water vapor).

The numbers in front of the components of a chemical reaction are called reaction coefficients.

Chemical reactions are endothermic(with energy absorption) and exothermic(with the release of energy). Combustion of methane is a typical example of an exothermic reaction.

There are several types of chemical reactions. The most common:

• compound reactions;
• decomposition reactions;
• single substitution reactions;
• double substitution reactions;
• oxidation reactions;
• redox reactions.

Compound reactions

In compound reactions, at least two elements form one product:

2Na (t) + Cl 2 (g) → 2NaCl (t)- the formation of table salt.

Attention should be paid to the essential nuance of the reactions of the compound: depending on the conditions of the reaction or the proportions of the reactants entering into the reaction, different products may result. For example, under normal conditions of combustion of coal, carbon dioxide is obtained:
C (t) + O 2 (g) → CO 2 (g)

If the amount of oxygen is not enough, then deadly carbon monoxide is formed:
2C (t) + O 2 (g) → 2CO (g)

Decomposition reactions

These reactions are, as it were, essentially opposite to the reactions of the compound. As a result of the decomposition reaction, the substance decomposes into two (3, 4 ...) simpler elements (compounds):

• 2H 2 O (l) → 2H 2 (g) + O 2 (g)- decomposition of water
• 2H 2 O 2 (l) → 2H 2 (g) O + O 2 (g)- decomposition of hydrogen peroxide

Single substitution reactions

As a result of single substitution reactions, the more active element replaces the less active one in the compound:

Zn (t) + CuSO 4 (p-p) → ZnSO 4 (p-p) + Cu (t)

The zinc in the copper sulfate solution displaces the less active copper, resulting in a zinc sulfate solution.

The degree of activity of metals by increasing activity:

• The most active are alkali and alkaline earth metals.

The ionic equation of the above reaction will be:

Zn (t) + Cu 2+ + SO 4 2- → Zn 2+ + SO 4 2- + Cu (t)

The ionic bond CuSO 4, when dissolved in water, decomposes into a copper cation (charge 2+) and a sulfate anion (charge 2-). As a result of the substitution reaction, a zinc cation is formed (which has the same charge as the copper cation: 2-). Note that the sulfate anion is present in both sides of the equation, so it can be abbreviated by all the rules of mathematics. As a result, you get the ion-molecular equation:

Zn (t) + Cu 2+ → Zn 2+ + Cu (t)

Double substitution reactions

In double substitution reactions, two electrons are already substituted. Such reactions are also called exchange reactions... Such reactions take place in solution with the formation of:

• insoluble solid (precipitation reaction);
• water (neutralization reaction).

Precipitation reactions

When mixing a solution of silver nitrate (salt) with a solution of sodium chloride, silver chloride is formed:

Molecular Equation: KCl (p-p) + AgNO 3 (p-p) → AgCl (t) + KNO 3 (p-p)

Ionic equation: K + + Cl - + Ag + + NO 3 - → AgCl (t) + K + + NO 3 -

Molecular ion equation: Cl - + Ag + → AgCl (s)

If the compound is soluble, it will be ionic in solution. If the compound is insoluble, it will precipitate forming a solid.

Neutralization reactions

These are the reactions of interaction of acids and bases, as a result of which water molecules are formed.

For example, the reaction of mixing a solution of sulfuric acid and a solution of sodium hydroxide (lye):

Molecular Equation: H 2 SO 4 (p-p) + 2NaOH (p-p) → Na 2 SO 4 (p-p) + 2H 2 O (g)

Ionic equation: 2H + + SO 4 2- + 2Na + + 2OH - → 2Na + + SO 4 2- + 2H 2 O (g)

Molecular ion equation: 2H + + 2OH - → 2H 2 O (l) or H + + OH - → H 2 O (l)

Oxidation reactions

These are reactions of interaction of substances with gaseous oxygen in the air, in which, as a rule, a large amount of energy is released in the form of heat and light. A typical oxidation reaction is combustion. At the very beginning of this page, the reaction of the interaction of methane with oxygen is given:

CH 4 (g) + 2O 2 (g) → CO 2 (g) + 2H 2 O (g)

Methane refers to hydrocarbons (compounds of carbon and hydrogen). When a hydrocarbon reacts with oxygen, a lot of thermal energy is released.

Redox reactions

These are reactions in which there is an exchange of electrons between the atoms of the reactants. The reactions discussed above are also redox reactions:

• 2Na + Cl 2 → 2NaCl - compound reaction
• CH 4 + 2O 2 → CO 2 + 2H 2 O - oxidation reaction
• Zn + CuSO 4 → ZnSO 4 + Cu - single substitution reaction

The most detailed redox reactions with a large number of examples of solving equations by the electronic balance method and the half-reaction method are described in the section