Oxides complex substances are called, the composition of the molecules of which includes oxygen atoms in the oxidation state - 2 and some other element.

can be obtained by direct interaction of oxygen with another element, or indirectly (for example, by the decomposition of salts, bases, acids). AT normal conditions oxides are in solid, liquid and gaseous state, this type of compounds is very common in nature. Oxides are found in the Earth's crust. Rust, sand, water, carbon dioxide are oxides.

They are salt-forming and non-salt-forming.

Salt-forming oxides are oxides that, as a result, chemical reactions form salts. These are oxides of metals and non-metals, which, when interacting with water, form the corresponding acids, and when interacting with bases, the corresponding acidic and normal salts. For example, copper oxide (CuO) is a salt-forming oxide, because, for example, when it reacts with hydrochloric acid (HCl), a salt is formed:

CuO + 2HCl → CuCl 2 + H 2 O.

As a result of chemical reactions, other salts can be obtained:

CuO + SO 3 → CuSO 4.

Non-salt-forming oxides called oxides that do not form salts. An example is CO, N 2 O, NO.

Salt-forming oxides, in turn, are of 3 types: basic (from the word « base » ), acidic and amphoteric.

Basic oxides such metal oxides are called, which correspond to hydroxides belonging to the class of bases. Basic oxides include, for example, Na 2 O, K 2 O, MgO, CaO, etc.

Chemical properties of basic oxides

1. Water-soluble basic oxides react with water to form bases:

Na 2 O + H 2 O → 2NaOH.

2. Interact with acid oxides, forming the corresponding salts

Na 2 O + SO 3 → Na 2 SO 4.

3. React with acids to form salt and water:

CuO + H 2 SO 4 → CuSO 4 + H 2 O.

4. React with amphoteric oxides:

Li 2 O + Al 2 O 3 → 2LiAlO 2 .

If the second element in the composition of oxides is a non-metal or a metal exhibiting a higher valency (usually exhibits from IV to VII), then such oxides will be acidic. Acid oxides (acid anhydrides) are oxides that correspond to hydroxides belonging to the class of acids. This is, for example, CO 2, SO 3, P 2 O 5, N 2 O 3, Cl 2 O 5, Mn 2 O 7, etc. Acid oxides dissolve in water and alkalis, forming salt and water.

Chemical properties of acid oxides

1. Interact with water, forming acid:

SO 3 + H 2 O → H 2 SO 4.

But not all acidic oxides directly react with water (SiO 2 and others).

2. React with based oxides to form a salt:

CO 2 + CaO → CaCO 3

3. Interact with alkalis, forming salt and water:

CO 2 + Ba (OH) 2 → BaCO 3 + H 2 O.

Part amphoteric oxide includes an element that has amphoteric properties. Amphotericity is understood as the ability of compounds to exhibit acidic and basic properties depending on the conditions. For example, zinc oxide ZnO can be both a base and an acid (Zn(OH) 2 and H 2 ZnO 2). Amphotericity is expressed in the fact that, depending on the conditions, amphoteric oxides exhibit either basic or acidic properties.

Chemical properties of amphoteric oxides

1. Interact with acids to form salt and water:

ZnO + 2HCl → ZnCl 2 + H 2 O.

2. React with solid alkalis (during fusion), forming as a result of the reaction salt - sodium zincate and water:

ZnO + 2NaOH → Na 2 ZnO 2 + H 2 O.

When zinc oxide interacts with an alkali solution (the same NaOH), another reaction occurs:

ZnO + 2 NaOH + H 2 O => Na 2.

Coordination number - a characteristic that determines the number of nearest particles: atoms or ions in a molecule or crystal. Each amphoteric metal has its own coordination number. For Be and Zn it is 4; For and Al is 4 or 6; For and Cr it is 6 or (very rarely) 4;

Amphoteric oxides usually do not dissolve in water and do not react with it.

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Chemical properties of acid oxides

1. Acid oxides interact with basic oxides and bases to form salts.

In this case, the rule is at least one of the oxides must correspond to a strong hydroxide (acid or alkali).

Acid oxides of strong and soluble acids interact with any basic oxides and bases:

SO 3 + CuO = CuSO 4

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

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

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

Acid oxides of water-insoluble and unstable or volatile acids interact only with strong bases (alkalis) and their oxides. In this case, the formation of acidic and basic salts is possible, depending on the ratio and composition of the reagents.

For example , sodium oxide interacts with carbon monoxide (IV), and copper oxide (II), to which the insoluble base Cu (OH) 2 corresponds, practically does not interact with carbon monoxide (IV):

Na 2 O + CO 2 \u003d Na 2 CO 3

CuO + CO 2 ≠

2. Acid oxides react with water to form acids.

Exception — silicon oxide, which corresponds to insoluble silicic acid. Oxides, which correspond to unstable acids, as a rule, react with water reversibly and to a very small extent.

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

3. Acidic oxides react with amphoteric oxides and hydroxides to form a salt or salt and water.

Please note that, as a rule, only oxides of strong or medium acids interact with amphoteric oxides and hydroxides!

For example , Sulfuric anhydride (sulfur oxide (VI)) reacts with aluminum oxide and aluminum hydroxide to form a salt - aluminum sulfate:

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

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

But carbon monoxide (IV), which corresponds to weak carbonic acid, no longer interacts with aluminum oxide and aluminum hydroxide:

CO 2 + Al 2 O 3 ≠

CO 2 + Al (OH) 3 ≠

4. Acid oxides interact with salts of volatile acids.

The following rule applies: in the melt, less volatile acids and their oxides displace more volatile acids and their oxides from their salts.

For example , solid silicon oxide SiO 2 will displace the more volatile carbon dioxide from calcium carbonate when fused:

CaCO 3 + SiO 2 \u003d CaSiO 3 + CO 2

5. Acid oxides are capable of exhibiting oxidizing properties.

Usually, element oxides in the highest degree oxidation - typical (SO 3, N 2 O 5, CrO 3, etc.). Strong oxidizing properties are also exhibited by some elements with an intermediate oxidation state (NO 2 and others).

6. Restorative properties.

Reducing properties, as a rule, are exhibited by oxides of elements in an intermediate oxidation state(CO, NO, SO 2, etc.). At the same time, they are oxidized to the highest or nearest stable oxidation state.

For example , sulfur oxide (IV) is oxidized by oxygen to sulfur oxide (VI):

2SO 2 + O 2 \u003d 2SO 3

Basic oxides are oxides, which correspond to bases as hydroxides.

Basic oxides form only metals and, as a rule, in the oxidation state +1 and +2 (exception: BeO, ZnO, SnO, PbO).

sodium hydroxide-

basic hydroxide

(base)

CaO ⇒ Ca(OH) 2

calcium hydroxide-

basic hydroxide

(base)

Basic oxides interact:

1. With acids, forming salt and water:

Basic Oxide + Acid = Salt + Water

For example:

MgO + 2HCl \u003d MgCl 2 + H 2 O.

In ion-molecular equations, the formulas of oxides are written in molecular form:

MgO + 2H + + 2 Cl - = Mg 2+ + 2 C l - + H 2 O

MgO + 2H + = Mg 2+ + H 2 O

2. With acidic oxides, forming salts:

Basic oxide + Acid oxide = Salt

For example:

CaO + N 2 O 5 \u003d Ca (NO 3) 2

In such equations, it is difficult to formulate the formula of the reaction product. To find out which acid corresponds to a given oxide, one must mentally add water to the acid oxide and then derive the formula of the desired acid:

N 2 O 5 + ( H2O ) → H 2 N 2 O 6

If in the resulting formula all indices are even, then they must be reduced by 2. In our case, it turns out: HNO 3 . The salt of this acid is the reaction product. So:

2+ 2+ 2+ 2+ 2+
CaO + N 2 O 5 \u003d CaO + N 2 O 5 + (H2O) \u003d CaO + H 2 N 2 O 6 \u003d CaO + HNO 3 \u003d Ca (NO 3) 2 -

3. With water. But only oxides formed by alkaline react with water (Li 2ONa 2OK2O, etc.) and alkaline earth metals (CaO,srO,BaO), since the products of these reactions are soluble bases (alkalis).

For example:

CaO + H 2 O \u003d Ca (OH) 2.

In order to derive the formula of the corresponding base from the oxide formula, water can be written as: H + - OH - and show how one hydrogen ion H + from a water molecule combines with an oxygen ion from CaO oxide and forms a hydroxide ion OH -. So:

CaO + H 2 O \u003d CaO + H + - OH - \u003d Ca (OH) 2.

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

CaO + H 2 O \u003d Ca (OH) 2;

with acidic compounds (acid oxides, acids) to form salts and water:

CaO + CO 2 \u003d CaCO 3;

CaO + 2HCl \u003d CaCl 2 + H 2 O;

3) with amphoteric compounds:

Li 2 O + Al 2 O 3 \u003d 2Li AlO 2;

3NaOH + Al(OH) 3 = Na 3 AlO 3 + 3H 2 O;

Acid oxides react:

1) with water to form acids:

SO 3 + H 2 O \u003d H 2 SO 4;

2) with basic compounds (basic oxides and bases) with the formation of salts and water:

SO 2 + Na 2 O \u003d Na 2 SO 3;

CO 2 + 2NaOH = Na 2 CO 3 + H 2 O;

with amphoteric compounds

CO 2 + ZnO \u003d ZnCO 3;

CO 2 + Zn(OH) 2 = ZnCO 3 + H 2 O;

Amphoteric oxides exhibit properties of both basic and acidic oxides. They are answered by amphoteric hydroxides:

acidic medium alkaline medium Be (OH) 2 BeO H 2 BeO 2

Zn(OH) 2 ZnO H 2 ZnO 2

Al (OH) 3 Al 2 O 3 H 3 AlO 3, HAlO 2

Cr(OH) 3 Cr 2 O 3 HCrO 2

Pb (OH) 2 PbO H 2 PbO 2

Sn(OH) 2 SnO H 2 SnO 2

Amphoteric oxides interact with acidic and basic compounds:

ZnO + SiO 2 \u003d ZnSiO 3; ZnO + H 2 SiO 3 \u003d ZnSiO 3 + H 2 O;

Al 2 O 3 + 3Na 2 O \u003d 2Na 3 AlO 3; Al 2 O 3 + 2NaOH \u003d 2NaAlO 2 + H 2 O.

Variable valence metals can form oxides of all three types. For example:

CrO basic Cr(OH) 2 ;

Cr 2 O 3 amphoteric Cr(OH) 3 ;

Cr 2 O 7 acidic H 2 Cr 2 O 7 ;

MnO, Mn 2 O 3 basic;

MnO 2 amphoteric;

Mn 2 O 7 acidic HMnO 4 .

Foundations

Bases are complex substances, which include metal atoms and one or more hydroxide groups (OH ‾). The general formula of bases is Me (OH) y, where y is the number of hydroxide groups equal to the valency of the metal.

Nomenclature

The name of the base consists of the word "hydroxide" + the name of the metal.

If the metal has a variable valency, then it is indicated at the end in brackets. For example: CuOH - copper (I) hydroxide, Cu (OH) 2 - copper (II) hydroxide, NaOH - sodium hydroxide.

Bases (hydroxides) are electrolytes. Electrolytes are substances that, in melts or solutions of polar liquids, decompose into ions: positively charged cations and negatively charged anions. The breakdown of a substance into ions is called electrolytic dissociation.

All electrolytes can be divided into two groups: strong and weak. Strong electrolytes in aqueous solutions are almost completely dissociated. Weak electrolytes dissociate only partially and in solutions a dynamic equilibrium is established between undissociated molecules and ions: NH 4 OH NH 4 + + OH - .

2.2. Classification

a) by the number of hydroxide groups in the molecule. The number of hydroxide groups in the base molecule depends on the valency of the metal and determines the acidity of the base.

The bases are divided into:

Single acid, the molecules of which contain one hydroxide group: NaOH, KOH, LiOH, etc.;

Biacid, the molecules of which contain two hydroxide groups: Ca (OH) 2, Fe (OH) 2, etc.;

Triacid, the molecules of which contain three hydroxide groups: Ni (OH) 3, Bi (OH) 3, etc.

Two- and three-acid bases are called polyacid.

b) according to the strength of the base are divided into:

Strong (alkalis): LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH) 2 , Sr(OH) 2 , Ba(OH) 2 ;

Weak: Cu (OH) 2, Fe (OH) 2, Fe (OH) 3, etc.

Strong bases are soluble in water, while weak bases are insoluble.

Base dissociation

Strong bases dissociate almost completely:

Ca (OH) 2 \u003d Ca 2+ + 2OH -.

Weak bases dissociate in steps. With the successive elimination of the hydroxide ion from polyacid bases, basic hydroxocation residues are formed, for example:

Fe(OH) 3 OH - + Fe(OH) 2 + iron dihydroxocations;

Fe(OH) 2 + OH - + FeOH 2+ iron hydroxocations;

Fe (OH) 2+ OH - + Fe 3+ iron cations.

The number of basic residues is equal to the acidity of the base.

Modern chemical science is a wide variety of branches, and each of them, in addition to the theoretical base, is of great applied and practical importance. Whatever you touch, everything around is the products of chemical production. The main sections are inorganic and organic chemistry. Consider what main classes of substances are classified as inorganic and what properties they have.

Main categories of inorganic compounds

These include the following:

1. Oxides.
2. Salt.
3. Foundations.
4. Acids.

Each of the classes is represented by a wide variety of inorganic compounds and is important in almost any structure of human economic and industrial activity. All the main properties characteristic of these compounds, being in nature and obtaining are studied in the school chemistry course without fail, in grades 8-11.

There is a general table of oxides, salts, bases, acids, which presents examples of each of the substances and their state of aggregation, being in nature. It also shows interactions that describe chemical properties. However, we will consider each of the classes separately and in more detail.

Group of compounds - oxides

4. Reactions, as a result of which elements change CO

Me + n O + C = Me 0 + CO

1. Reagent water: acid formation (SiO 2 exception)

KO + water = acid

2. Reactions with bases:

CO 2 + 2CsOH \u003d Cs 2 CO 3 + H 2 O

3. Reactions with basic oxides: salt formation

P 2 O 5 + 3MnO \u003d Mn 3 (PO 3) 2

4. OVR reactions:

CO 2 + 2Ca \u003d C + 2CaO,

They show dual properties, interact according to the principle of the acid-base method (with acids, alkalis, basic oxides, acid oxides). They do not interact with water.

1. With acids: formation of salts and water

AO + acid \u003d salt + H 2 O

2. With bases (alkalis): formation of hydroxo complexes

Al 2 O 3 + LiOH + water \u003d Li

3. Reactions with acid oxides: preparation of salts

FeO + SO 2 \u003d FeSO 3

4. Reactions with RO: formation of salts, fusion

MnO + Rb 2 O = double salt Rb 2 MnO 2

5. Fusion reactions with alkalis and alkali metal carbonates: formation of salts

Al 2 O 3 + 2LiOH \u003d 2LiAlO 2 + H 2 O

They do not form acids or alkalis. They exhibit highly specific properties.

Each higher oxide, formed both by a metal and a non-metal, when dissolved in water, gives a strong acid or alkali.

Acids organic and inorganic

In the classical sound (based on the positions of ED - electrolytic dissociation - acids are compounds, in aquatic environment dissociating into cations H + and anions of acid residues An - . Today, however, acids have been carefully studied under anhydrous conditions, so there are many different theories for hydroxides.

Empirical formulas of oxides, bases, acids, salts are made up only of symbols, elements and indices indicating their amount in a substance. For example, inorganic acids are expressed by the formula H + acid residue n-. organic matter have a different theoretical representation. In addition to the empirical, for them, you can write the full and abbreviated structural formula, which will reflect not only the composition and amount of the molecule, but also the order of the atoms, their relationship to each other and the main functional group for carboxylic acids -COOH.

In the inorganic, all acids are divided into two groups:

• anoxic - HBr, HCN, HCL and others;
• oxygen-containing (oxo acids) - HClO 3 and everything where there is oxygen.

Also, inorganic acids are classified according to stability (stable or stable - everything except carbonic and sulphurous, unstable or unstable - carbonic and sulphurous). By strength, acids can be strong: sulfuric, hydrochloric, nitric, perchloric and others, as well as weak: hydrogen sulfide, hypochlorous and others.

Organic chemistry does not offer such diversity at all. Acids that are organic in nature are carboxylic acids. Them common feature- the presence of a functional group -COOH. For example, HCOOH (antic), CH 3 COOH (acetic), C 17 H 35 COOH (stearic) and others.

There are a number of acids, which are especially carefully emphasized when considering this topic in a school chemistry course.

1. Salt.
2. Nitrogen.
3. Orthophosphoric.
4. Hydrobromic.
5. Coal.
6. Iodine.
7. Sulfuric.
8. Acetic, or ethane.
9. Butane or oil.
10. Benzoic.

These 10 acids in chemistry are the fundamental substances of the corresponding class both in the school course and in general in industry and synthesis.

Properties of inorganic acids

The main physical properties should be attributed primarily to a different state of aggregation. After all, there are a number of acids that have the form of crystals or powders (boric, orthophosphoric) under normal conditions. The vast majority of well-known inorganic acids are different liquids. Boiling and melting points also vary.

Acids can cause severe burns, as they have the power to destroy organic tissues and skin. Indicators are used to detect acids:

• methyl orange (in normal environment - orange, in acids - red),
• litmus (in neutral - violet, in acids - red) or some others.

The most important chemical properties include the ability to interact with both simple and complex substances.

Chemical properties of inorganic acids

What do they interact with?	Reaction example
1. With simple substances-metals. A prerequisite: the metal must stand in the ECHRNM before hydrogen, since the metals standing after hydrogen are not able to displace it from the composition of acids. As a result of the reaction, hydrogen is always formed in the form of a gas and a salt.
2. With bases. The result of the reaction is salt and water. Such reactions of strong acids with alkalis are called neutralization reactions.	Any acid (strong) + soluble base = salt and water
3. With amphoteric hydroxides. Bottom line: salt and water.	2HNO 2 + beryllium hydroxide \u003d Be (NO 2) 2 (medium salt) + 2H 2 O
4. With basic oxides. Outcome: water, salt.	2HCL + FeO = iron (II) chloride + H 2 O
5. With amphoteric oxides. Final effect: salt and water.	2HI + ZnO = ZnI 2 + H 2 O
6. With salts formed by weaker acids. Final effect: salt and weak acid.	2HBr + MgCO 3 = magnesium bromide + H 2 O + CO 2

When interacting with metals, not all acids react in the same way. Chemistry (grade 9) at school involves a very shallow study of such reactions, however, even at this level, the specific properties of concentrated nitric and sulfuric acid are considered when interacting with metals.

Hydroxides: alkalis, amphoteric and insoluble bases

Oxides, salts, bases, acids - all these classes of substances have a common chemical nature, explained by the structure crystal lattice, as well as the mutual influence of atoms in the composition of molecules. However, if for oxides it was possible to give a very specific definition, then for acids and bases it is more difficult to do so.

Just like acids, bases, according to the ED theory, are substances capable of aqueous solution decompose into metal cations Me n + and anions of hydroxo groups OH - .

• Soluble or alkali (strong bases that change Formed by metals of groups I, II. Example: KOH, NaOH, LiOH (that is, elements of only the main subgroups are taken into account);
• Slightly soluble or insoluble (medium strength, do not change the color of the indicators). Example: magnesium hydroxide, iron (II), (III) and others.
• Molecular (weak bases, in an aqueous medium they reversibly dissociate into ions-molecules). Example: N 2 H 4, amines, ammonia.
• Amphoteric hydroxides (show dual basic-acid properties). Example: beryllium, zinc and so on.

Each group represented is studied in the school chemistry course in the "Foundations" section. Chemistry grades 8-9 involves a detailed study of alkalis and sparingly soluble compounds.

The main characteristic properties of the bases

All alkalis and sparingly soluble compounds are found in nature in a solid crystalline state. At the same time, their melting points are, as a rule, low, and poorly soluble hydroxides decompose when heated. The base color is different. If alkali white color, then the crystals of sparingly soluble and molecular bases can be of very different colors. The solubility of most compounds of this class can be viewed in the table, which presents the formulas of oxides, bases, acids, salts, shows their solubility.

Alkalis are able to change the color of indicators as follows: phenolphthalein - raspberry, methyl orange - yellow. This is ensured by the free presence of hydroxo groups in solution. That is why sparingly soluble bases do not give such a reaction.

The chemical properties of each group of bases are different.

Chemical properties
alkalis	sparingly soluble bases	Amphoteric hydroxides
I. Interact with KO (total - salt and water): 2LiOH + SO 3 \u003d Li 2 SO 4 + water II. Interact with acids (salt and water): conventional neutralization reactions (see acids) III. Interact with AO to form a hydroxocomplex of salt and water: 2NaOH + Me + n O \u003d Na 2 Me + n O 2 + H 2 O, or Na 2 IV. Interact with amphoteric hydroxides to form hydroxo complex salts: The same as with AO, only without water V. Interact with soluble salts to form insoluble hydroxides and salts: 3CsOH + iron (III) chloride = Fe(OH) 3 + 3CsCl VI. Interact with zinc and aluminum in an aqueous solution to form salts and hydrogen: 2RbOH + 2Al + water = complex with hydroxide ion 2Rb + 3H 2	I. When heated, they can decompose: insoluble hydroxide = oxide + water II. Reactions with acids (total: salt and water): Fe(OH) 2 + 2HBr = FeBr 2 + water III. Interact with KO: Me + n (OH) n + KO \u003d salt + H 2 O	I. React with acids to form salt and water: (II) + 2HBr = CuBr 2 + water II. React with alkalis: result - salt and water (condition: fusion) Zn(OH) 2 + 2CsOH \u003d salt + 2H 2 O III. They react with strong hydroxides: the result is salts, if the reaction takes place in an aqueous solution: Cr(OH) 3 + 3RbOH = Rb 3

These are the most chemical properties that bases exhibit. The chemistry of bases is quite simple and obeys general patterns all inorganic compounds.

Class of inorganic salts. Classification, physical properties

Based on the provisions of the ED, salts can be called inorganic compounds that dissociate in an aqueous solution into metal cations Me + n and anions of acid residues An n- . So you can imagine salt. Chemistry gives more than one definition, but this is the most accurate.

At the same time, according to their chemical nature, all salts are divided into:

• Acidic (containing a hydrogen cation). Example: NaHSO4.
• Basic (having a hydroxo group). Example: MgOHNO 3 , FeOHCL 2.
• Medium (consist only of a metal cation and an acid residue). Example: NaCL, CaSO 4.
• Double (include two different metal cations). Example: NaAl(SO 4) 3.
• Complex (hydroxocomplexes, aquacomplexes and others). Example: K 2 .

The formulas of salts reflect their chemical nature, and also speak of the qualitative and quantitative composition of the molecule.

Oxides, salts, bases, acids have different solubility, which can be seen in the corresponding table.

If we talk about the state of aggregation of salts, then you need to notice their uniformity. They exist only in a solid, crystalline or powdered state. The color scheme is quite varied. Solutions of complex salts, as a rule, have bright saturated colors.

Chemical interactions for the class of medium salts

They have similar chemical properties of bases, acids, salts. Oxides, as we have already considered, differ somewhat from them in this factor.

In total, 4 main types of interactions can be distinguished for medium salts.

I. Interaction with acids (only strong in terms of ED) with the formation of another salt and a weak acid:

KCNS + HCL = KCL + HCNS

II. Reactions with soluble hydroxides with the appearance of salts and insoluble bases:

CuSO 4 + 2LiOH = 2LiSO 4 soluble salt + Cu(OH) 2 insoluble base

III. Interaction with another soluble salt to form an insoluble salt and a soluble one:

PbCL 2 + Na 2 S = PbS + 2NaCL

IV. Reactions with metals to the left of the one that forms the salt in the EHRNM. In this case, the metal entering into the reaction should not, under normal conditions, interact with water:

Mg + 2AgCL = MgCL 2 + 2Ag

These are the main types of interactions that are characteristic of medium salts. The formulas of complex, basic, double and acidic salts speak for themselves about the specificity of the manifested chemical properties.

The formulas of oxides, bases, acids, salts reflect the chemical nature of all representatives of these classes of inorganic compounds, and in addition, give an idea of ​​the name of the substance and its physical properties. Therefore, their writing should be paid Special attention. A huge variety of connections offers us a whole amazing science- chemistry. Oxides, bases, acids, salts - this is only part of the vast variety.