Classification and properties of complex inorganic substances. Relationship

The philosophical truth: everything in our world is relative, is also true for the classification of substances and their properties. The great variety of substances in the Universe and on our planet consists of only 90 chemical elements. In nature, there are substances composed of elements with serial numbers from 1 to 91 inclusive. Element 43 – technetium, is currently not found in nature on Earth, because this element has no stable isotopes. It was produced artificially as a result of a nuclear reaction. Hence the name of the element - from the Greek. téhnos – artificial.
All earthly natural chemical substances, built from 90 elements, can be divided into two large types - inorganic and organic.
Organic substances are carbon compounds with the exception of the simplest: carbon oxides, metal carbides, carbonic acid and its salts. All other substances are classified as inorganic.
There are more than 27 million organic substances - much more than inorganic substances, the number of which, according to the most optimistic estimates, does not exceed 400 thousand. We will talk about the reasons for the diversity of organic compounds a little later, but for now we note that there is no sharp boundary between these two groups of substances. For example, ammonium isocyanate salt NH4NCO is considered an inorganic compound, and urea (NH2)2CO, which has exactly the same elemental composition N2H4CO, is an organic substance.
Substances that have the same molecular formula but different chemical structures are called isomers.
Inorganic substances are usually divided into two subtypes - simple and complex (Scheme 1). As you already know, simple substances are substances consisting of atoms of one chemical element, and complex substances are called substances consisting of two or more chemical elements.
Scheme 1

Classification of inorganic substances

It would seem that the number of simple substances should coincide with the number of chemical elements. However, it is not. The fact is that atoms of the same chemical element can form not one, but several different simple substances. This phenomenon, as you know, is called allotropy. The reasons for allotropy can be a different number of atoms in a molecule (for example, allotropic modifications of the oxygen element - oxygen O2 and ozone O3), as well as a different structure of the crystal lattice of a solid substance (for example, the already familiar allotropic modifications of carbon - diamond and graphite).
The subtype of simple substances includes metals, nonmetals and noble gases, the latter often being classified as nonmetals. This classification is based on the properties of simple substances, determined by the structure of the atoms of the chemical elements from which these substances are formed, and the type of crystal lattice. Everyone knows that metals conduct electric current, are thermally conductive, ductile, and have a metallic luster. Nonmetals, as a rule, do not have such properties. Our clause “as a rule” is not accidental, and it once again emphasizes the relativity of the classification of simple substances. Some metals resemble non-metals in properties (for example, the allotropic modification of tin - gray tin - is a gray powder, does not conduct electricity, lacks luster and ductility, while white tin, another allotropic modification, is a typical metal). In contrast, the nonmetal graphite, an allotrope of carbon, is highly electrically conductive and has a characteristic metallic luster.
The most general classification of complex inorganic substances is familiar to you from the basic school chemistry course. There are four classes of compounds: oxides, bases, acids and salts.
The division of inorganic substances into classes is carried out on the basis of their composition, which, in turn, is reflected in the properties of the compounds. Let us recall the definitions of representatives of each class.
Oxides – complex substances consisting of two elements, one of which is oxygen in the –2 oxidation state (for example, H2O, CO2, CuO).
Grounds – these are complex substances consisting of a metal atom and one or more hydroxy groups (for example, NaOH, Ca(OH)2).
Acids – these are complex substances consisting of hydrogen atoms and an acid residue (for example, HCl, HNO3, H2SO4, H3PO4).
Salts – these are complex substances consisting of metal atoms and acidic residues (for example, NaNO3, K2SO4, AlCl3).
Such classification and definitions are also very relative. Firstly, the role of a metal in bases and salts can be played by complex particles like the familiar ammonium cation NH4+, consisting only of non-metal elements. Secondly, there is a fairly large group of substances that are formally (in composition) bases, but in properties belong to amphoteric hydroxides, i.e. combine the properties of bases and acids. For example, aluminum hydroxide Al(OH)3 behaves like a base when interacting with an acid:
Al(OH)3 + 3HCl = AlCl3 + 3H2O,
and when fused with alkalis it exhibits the properties of an acid:
H3AlO3 + NaOH = NaAlO2 + H2O.
Thirdly, the above classification of complex inorganic substances does not include a large number of compounds that cannot be classified into any of the listed classes. These are, for example, compounds formed by two or more non-metal elements (phosphorus(V) chloride PCl5, carbon sulfide CS2, phosgene COCl2).
? 1. Which substances are called inorganic and which are called organic? Give examples. Prove the relativity of this classification of substances.
2. Which substances are called simple and which are called complex? Why does the number of simple substances exceed the number of chemical elements?
3. What is the classification of simple substances? Give examples of each type of substance. Are noble gases substances of atomic or molecular structure? Give arguments in favor of both points of view.
4. What inorganic substances are called oxides, bases, acids, salts? Give examples of substances of each class, illustrate their properties with two or three equations of chemical reactions.
5. Using equations of chemical reactions, prove that amphoteric hydroxides exhibit the properties of both acids and bases.
6. Calcium carbonate (chalk, marble, limestone) inspired sculptors, artists, and poets. For example:

To date, more than five hundred thousand inorganic compounds have been identified. The classification and nomenclature of inorganic substances is an important issue that allows us to understand the variety of compounds.

Historical reference

In the 18th-19th centuries, Antoine Lavoisier, Mikhail Lomonosov, and John Dalton proposed the first classification and nomenclature of inorganic substances. Simple ones were distinguished and the first group was divided into metals and non-metals. A group of compounds that had intermediate properties, called metalloids, was also isolated. This division formed the basis of the modern classification.

Currently there are four classes. Let's take a closer look at each of these classes.

Oxides

They are polyatomic compounds that consist of two elements, the second in them is always an oxygen ion in the oxidation state -2. The classification and nomenclature of inorganic substances involves dividing the class of oxides into three groups:

• basic;
• amphoteric;
• acidic

Classification

The first group consists of compounds of metals (with minimal oxidation states) with oxygen. For example, MgO is magnesium oxide. Among the main chemical properties of this compound, one can note their interaction with acidic oxides, acids, and more active metals.

Oxygen compounds of nonmetals, as well as metallic elements with oxidation states from +4 to +7. For example, this group includes MnO 2, CO 2. Among the typical ones, we highlight the interaction with water (weak carbonic acid is formed), basic oxides, and soluble bases (alkalis).

Amphoteric (transition) oxides are metal compounds with an oxidation state of +3 (as well as beryllium and zinc oxide), which are capable of reacting with both acids and alkalis.

Oxides are divided into salt-forming and non-salt-forming. The first group corresponds to acids or bases in which the main element retains its oxidation state. The non-salt-forming group is small in number; its representatives are not capable of forming salts. For example, among non-salt-forming oxides there are: N 2 O, NO, SiO, CO.

Hydroxides

The classification and nomenclature of inorganic substances involves the identification of a class of hydroxides. They are called complex substances that contain atoms of some element, as well as hydroxyl groups OH. This class is divided into two large groups:

• grounds;
• acids

Acids contain several hydrogen atoms that can be replaced by metal atoms subject to the rules of stoichiometric valency. Many are in meta form, and their hydrogen atoms are located at the beginning of the formula. They have the general form HxEOy, where the second part is called the acid residue. Classification and their nomenclature are discussed as part of a school chemistry course. To sulfuric acid - sulfates, nitric acid - nitrates, carbonic acid - carbonates.

Depending on the number of hydrogen atoms, the following groups are distinguished:

• monobasic;
• dibasic;
• tribasic acids

Bases contain metal and OH cations that can be replaced in chemical reactions by acid residues, subject to the rules of stoichiometric valence.

The bases are in ortho form and have the general formula M(OH)n, with n = 1 or 2. When naming compounds of this group, the corresponding metal is added to the hydroxide.

Among the main chemical properties that representatives of this class of inorganic substances possess, it is necessary to note their reaction with acids; the reaction products are water and salt.

For example, in the reaction of sodium hydroxide with hydrochloric acid, the products will be water and sodium chloride.

Depending on their solubility in water, soluble bases (alkalis) and insoluble hydroxides are distinguished. The first group includes hydroxyl compounds of metals of the first and second groups of the main subgroups (alkali and alkaline earth metals).

For example, NaOH is alkali (sodium hydroxide); Fe(OH) 2 - iron II hydroxide (insoluble compound).

Salts

What else does the classification and nomenclature of inorganic substances include? Assignments for students in grades 8-9 involve dividing the proposed list of compounds into separate classes: oxides, bases, acids, salts.

Salts are complex substances that contain metal cations and anions of an acid residue. Medium salts have the general formula Mx(EOy) n. An example of this group is Ca 3 (PO 4) 2 - calcium phosphate.

If hydrogen cations also appear in the composition, the salts are called acidic, and the presence of hydroxyl groups is characteristic of basic salts. For example, NaHCO 3 is sodium bicarbonate, and CaOHCl is calcium hydroxychloride.

Those salts that contain cations of two different metals are called double salts.

Complex salts are complex compounds that contain a complexing agent and ligands. In high school, the classification and nomenclature of inorganic substances is considered. The theory of complex compounds is studied as part of a specialized course in general chemistry. Questions concerning the nomenclature and chemical properties of complex salts are not included in the test questions of the unified state exam in chemistry for the high school course.

Conclusion

How is the classification and nomenclature of inorganic substances used in the school curriculum? Groups of substances are briefly discussed as part of the eighth and ninth grade curriculum, and they are studied in more detail in the 11th grade general chemistry course. Tasks related to the classification of inorganic compounds and comparison of the chemical properties of compounds with the proposed products are included in the final certification tests in chemistry (USE) for eleventh grade graduates. In order to successfully cope with them, students must have basic knowledge of the classification of inorganic compounds and the skills of comparing the proposed substances with the chemical properties of the entire class.

And their derivatives. All other substances are inorganic.

Classification of inorganic substances
Inorganic substances are divided into simple and complex according to their composition.

Simple substances consist of atoms of one chemical element and are divided into metals, nonmetals, and noble gases. Complex substances consist of atoms of different elements chemically bonded to each other.

Complex inorganic substances, according to their composition and properties, are divided into the following important classes: oxides, bases, acids, amphoteric hydroxides, salts.

In the school course, four main classes of complex substances are studied: oxides, bases, acids, salts.

Oxides

- these are complex substances consisting of two elements, one of which is oxygen.

Oxides are divided into:

non-salt-forming - do not interact with acids or alkalis and do not form salts. These are nitrogen oxide (I) N 2 O, nitrogen oxide (II) NO, carbon monoxide (II) CO and some others.

salt-forming - when interacting with acids or bases, they form salt and water.

In turn, they are divided into:

basic - the grounds correspond to them. These include metal oxides with low oxidation states (+1, +2). They are all solids)

acidic - they correspond to acids. These include non-metal oxides and metal oxides with high oxidation states. For example, chromium (VI) oxide CrO 3, manganese (VII) oxide Mn 2 O 7.

amphoteric - depending on the conditions, they exhibit basic or acidic properties, i.e. have dual properties. These are zinc oxide ZnO, aluminum oxide Al 2 O 3, iron (III) oxide Fe 2 O 3, chromium (III) oxide Cr 2 O 3.

Typical reactions of basic oxides

1. Basic oxide + water = alkali (! The reaction proceeds if a soluble base is formed!)

K2O + H2O = 2KOH

CaO + H 2 O = Ca(OH) 2

2. Basic oxide + acidic oxide = salt

CaO + N 2 O 5 = Ca(NO 3) 2

MgO + SiO 2 = MgSiO 3

3. Basic oxide + acid = salt + water

FeO + H 2 SO 4 = FeSO 4 + H 2 O

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

Typical acid oxide reactions

1. Acidic oxide + water = acid (except silicon oxide SiO 2)

SO 2 + H 2 O = H 2 SO 3

CrO 3 + H 2 O = H 2 CrO 4

2. Acidic oxide + basic oxide = salt

SO 3 + K 2 O = K 2 SO 4

CO 2 + CaO = CaCO 3

3. Acid oxide + base = salt + water

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

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

Typical reactions of amphoteric oxides

1. Amphoteric oxide + acid = salt + water

ZnO + 2HCl = ZnCl 2 + H 2 O

Al 2 O 3 + 6HCl = 2AlCl 3 + 3H 2 O

2. Amphoteric oxide + alkali = salt + water

ZnO + 2NaOH + H 2 O = Na 2

Al 2 O 3 + 2NaOH + 3H 2 O = 2Na

Cr 2 O 3 + 2NaOH + 7H 2 O = 2Na

When fusion

ZnO + 2KOH = K 2 ZnO 2 + H 2 O

Al 2 O 3 + 2NaOH = 2NaAlO 2 + H 2 O

Cr 2 O 3 + 2NaOH = 2NaCrO 2 + H 2 O

Grounds

- these are complex substances that contain metal atoms connected to one or more hydroxo groups.

The grounds are divided into:

soluble in water (alkalis) - formed by elements of group I of the main subgroup LiOH, NaOH, KOH, RbOH, CsOH and elements of group II of the main subgroup (except magnesium and beryllium) Ca(OH) 2, Sr(OH)2, Ba(OH)2.

insoluble in water - other.

Reactions characteristic of all bases

1. Base + acid = salt + water

2KOH + H 2 SO 4 = K 2 SO 4 + 2H 2 O

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

Typical reactions of alkalis

1. Aqueous solutions change the color of indicators (litmus - blue, methyl orange - yellow, phenolphthalein - crimson)

KOH = K+ + OH - (OH ions - cause an alkaline reaction of the environment)

Ca(OH) 2 = Ca 2 + + 2OH -

2. Alkali + acid oxide = salt + water

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

2KOH + CO 2 = K 2 CO 3 + H 2 O

3. Alkali + salt = salt + base (if the reaction product is an insoluble compound or a slightly dissociating substance NH 4 OH)

2NaOH + CuSO 4 = Na 2 SO 4 + Cu(OH) 2 (insoluble)

Ca(OH) 2 + Na 2 SiO 3 = CaSiO 3 (insoluble) + 2NaOH

NaOH + NH 4 Cl = NaCl + NH 4 OH

4. React with fats to form soap

Typical reactions of insoluble bases

1. Decomposes when heated

Fe(OH) 2 = FeO + H 2 O

2Fe(OH) 3 = Fe 2 O 3 + 3H 2 O

Among the insoluble bases there are amphoteric ones. For example, Be(OH) 2, Zn(OH) 2, Ge(OH) 2, Pb(OH) 2, Al(OH) 3, Cr(OH) 3, Sn(OH) 4, etc.

They react with alkalis in aqueous solution

Zn(OH) 2 + 2NaOH = Na 2

Fe(OH)3 + NaOH = Na

or by fusion

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

Fe(OH) 3 + NaOH = NaFeO 2 + 2H 2 O

Acids

- these are complex substances consisting of hydrogen atoms that can be replaced by metal atoms and acidic residues.

Reactions characteristic of all acids

1. Acid + base = salt + water

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

2HCl + Ca(OH) 2 = CaCl 2 + 2H 2 O

2. Acid + basic oxide = salt + water

CuO + H 2 SO 4 = CuSO 4 + 2H 2 O

3CaO + 2H 3 PO 4 = Ca 3 (PO 4) 2 + 3H 2 O

Salts

- these are complex substances that contain metal atoms and an acid residue.

Salts are divided into:

average - contain only metal atoms as cations and only an acid residue as anions. They can be considered as products of complete replacement of hydrogen atoms in the acid with metal atoms or products of complete replacement of hydroxyl groups in the basic hydroxide molecule with acidic residues.

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

3H 2 SO 4 + 2Fe(OH) 3 = Fe 2 (SO 4) 3 + 6H 2 O

sour - contain not only metal atoms, but also hydrogen atoms as cations. They can be considered as products of incomplete replacement of hydrogen atoms in the acid. Formed only by polybasic acids. They are obtained when there is insufficient amount of base to form a medium salt.

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

basic - as anions they contain not only an acid residue, but also a hydroxo group. They can be considered as products of incomplete replacement of hydroxo groups in the composition of a polyacid base with an acid residue. Formed only by polyacid bases. They are obtained when there is not enough acid to form a medium salt.

H 2 SO 4 + Fe(OH) 3 = FeOHSO 4 + 2H 2 O

Typical reactions of medium salts

1. Salt + acid = another salt + another acid (The reaction occurs if an insoluble compound is formed, a gas is released - carbon dioxide CO 2, sulfur dioxide SO 2, hydrogen sulfide H 2 S - or a slightly dissociating substance is formed, for example, acetic acid CH 3 COOH!)

BaCl 2 + H 2 SO 4 = BaSO 4 ↓ + 2HCl

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

(CH 3 COO) 2 Ca + 2HNO 3 = Ca(NO 3) 2 + 2CH 3 COOH

As a result of this reaction, volatile acids can be obtained: nitric and hydrochloric, if you take a solid salt and a strong concentrated acid (preferably sulfuric)

2NaCl + H 2 SO 4 = Na 2 SO 4 + 2HCl

2KNO3 + H2SO4 = K2SO4 + 2HNO3

2. Salt + alkali = another salt + another base (The reaction occurs if an insoluble compound is formed or a slightly dissociating substance is formed, for example, ammonium hydroxide NH 4 OH!)

Cu(NO 3) 2 + 2NaOH = 2NaNO 3 + Cu(OH) 2 ↓

NH 4 Cl + NaOH = NaCl + NH 4 OH

3. Salt(1) + salt(2) = salt(3) + salt(4) (The reaction proceeds if an insoluble compound is formed!)

NaCl + AgNO 3 = NaNO 3 + AgCl↓

CaCl 2 + Na 2 CO 3 = CaCO 3 ↓ + 2NaCl

4. Salt + metal = another salt + another metal (A metal displaces from salt solutions all other metals that are to the right of it in the series of metal stresses. The reaction occurs if both salts are soluble and the metal itself does not interact with water!)

CuCl 2 + Fe = FeCl 2 + Cu

2AgNO3 + Cu = Cu(NO3)2 + 2Ag

5. Decomposition reactions:

a) carbonates. Insoluble carbonates of divalent metals decompose mainly when heated into oxide and carbon dioxide. Of the alkali metals, the reaction is typical for lithium carbonate in an inert environment.

b) bicarbonates decompose into carbonates, carbon dioxide and water.

c) nitrates: according to the scheme - up to magnesium inclusive, according to a number of voltages, metals decompose into nitrite and oxygen; from magnesium to copper inclusive to metal oxide (often the metal changes its oxidation state to a higher one), nitric oxide (IV) and oxygen; after copper into metal, nitric oxide (IV) and oxygen.

Typical reactions of acid salts

1. Acid salt + alkali = medium salt + water

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

Typical reactions of basic salts

1. Basic salt + alkali = medium salt + water

(CuOH) 2 CO 3 + H 2 CO 3 = CuCO 3 ↓ + 2H 2 O

Every day a person interacts with a large number of objects. They are made from different materials and have their own structure and composition. Everything that surrounds a person can be divided into organic and inorganic. In the article we will look at what such substances are and give examples. We will also determine what inorganic substances are found in biology.

Description

Inorganic substances are those substances that do not contain carbon. They are the opposite of organic. This group also includes several carbon-containing compounds, for example:

• cyanides;
• carbon oxides;
• carbonates;
• carbides and others.

• water;
• various acids (hydrochloric, nitric, sulfuric);
• salt;
• ammonia;
• carbon dioxide;
• metals and non-metals.

The inorganic group is distinguished by the absence of a carbon skeleton, which is characteristic of organic substances. According to their composition, they are usually divided into simple and complex. Simple substances make up a small group. There are approximately 400 of them in total.

Simple inorganic compounds: metals

Metals are simple atoms which are based on a metallic bond. These elements have characteristic metallic properties: thermal conductivity, electrical conductivity, ductility, luster and others. In total, there are 96 elements in this group. These include:

• alkali metals: lithium, sodium, potassium;
• alkaline earth metals: magnesium, strontium, calcium;
• copper, silver, gold;
• light metals: aluminum, tin, lead;
• semimetals: polonium, moscovium, nihonium;
• lanthanides and lanthanum: scandium, yttrium;
• actinides and actinium: uranium, neptunium, plutonium.

Metals are mainly found in nature in the form of ores and compounds. To obtain pure metal without impurities, it is purified. If necessary, it is possible to carry out alloying or other processing. This is done by a special science - metallurgy. It is divided into black and colored.

Simple inorganic compounds: nonmetals

Nonmetals are chemical elements that do not have metallic properties. Examples of inorganic substances:

• water;
• nitrogen;
• sulfur;
• oxygen and others.

Nonmetals are characterized by a large number of electrons per their atom. This determines some properties: the ability to attach additional electrons increases, and higher oxidative activity appears.

In nature you can find non-metals in a free state: oxygen, chlorine, as well as solid forms: iodine, phosphorus, silicon, selenium.

Some nonmetals have a distinctive property - allotropy. That is, they can exist in various modifications and forms. For example:

• gaseous oxygen has modifications: oxygen and ozone;
• solid carbon can exist in the following forms: diamond, graphite, glassy carbon and others.

Complex inorganic compounds

This group of substances is more numerous. Complex compounds are distinguished by the presence of several chemical elements in the substance.

Let's take a closer look at complex inorganic substances. Examples and their classification are presented below in the article.

1. Oxides are compounds in which oxygen is one of the elements. The group includes:

• non-salt-forming (for example, nitrogen);
• salt-forming oxides (for example, sodium oxide, zinc oxide).

2. Acids are substances that contain hydrogen ions and acidic residues. For example, nitrogen hydrogen sulfide.

3. Hydroxides are compounds that contain the -OH group. Classification:

• bases - soluble and insoluble alkalis - copper hydroxide, sodium hydroxide;
• oxygen-containing acids - dihydrogen trioxocarbonate, hydrogen trioxonitrate;
• amphoteric - chromium hydroxide, copper hydroxide.

4. Salts are substances that contain metal ions and acidic residues. Classification:

• medium: sodium chloride, iron sulfide;
• acidic: sodium bicarbonate, hydrosulfates;
• main: dihydroxochrome nitrate, hydroxochrome nitrate;
• complex: sodium tetrahydroxyzincate, potassium tetrachloroplatinate;
• double: potassium alum;
• mixed: potassium aluminum sulfate, potassium copper chloride.

5. Binary compounds are substances consisting of two chemical elements:

• oxygen-free acids;
• oxygen-free salts and others.

Inorganic compounds containing carbon

Such substances traditionally belong to the group of inorganic ones. Examples of substances:

• Carbonates - esters and salts of carbonic acid - calcite, dolomite.
• Carbides are compounds of non-metals and metals with carbon - beryllium carbide, calcium carbide.
• Cyanides - salts of hydrocyanic acid - sodium cyanide.
• Carbon oxides are a binary compound of carbon and oxygen - carbon monoxide and carbon dioxide.
• Cyanates are derivatives of cyanic acid - fulmic acid, isocyanic acid.
• Carbonyl metals - a complex of metal and carbon monoxide - nickel carbonyl.

All the substances considered differ in their individual chemical and physical properties. In general terms, the distinctive features of each class of inorganic substances can be identified:

1. Simple metals:

• high thermal and electrical conductivity;
• metallic shine;
• lack of transparency;
• strength and ductility;
• at room temperature they retain their hardness and shape (except for mercury).

2. Simple non-metals:

• simple non-metals can be in a gaseous state: hydrogen, oxygen, chlorine;
• bromine occurs in the liquid state;
• solid non-metals have a non-molecular state and can form crystals: diamond, silicon, graphite.

3. Complex substances:

• oxides: react with water, acids and acid oxides;
• acids: react with water and alkalis;
• amphoteric oxides: may react with acidic oxides and bases;
• hydroxides: soluble in water, have a wide range of melting points, and can change color when interacting with alkalis.

The cell of any living organism consists of many components. Some of them are inorganic compounds:

• Water. For example, the amount of water in a cell ranges from 65 to 95%. It is necessary for the implementation of chemical reactions, the movement of components, and the process of thermoregulation. It is also water that determines the volume of the cell and the degree of its elasticity.
• Mineral salts. They can be present in the body both in dissolved and undissolved form. An important role in cellular processes is played by cations: potassium, sodium, calcium, magnesium - and anions: chlorine, bicarbonates, superphosphate. Minerals are necessary to maintain osmotic balance, regulate biochemical and physical processes, form nerve impulses, maintain blood clotting levels and many other reactions.

Not only the inorganic substances of the cell are important for maintaining life. Organic components occupy 20-30% of its volume.

Classification:

• simple organic substances: glucose, amino acids, fatty acids;
• complex organic substances: proteins, nucleic acids, lipids, polysaccharides.

Organic components are necessary to perform the protective, energetic function of the cell; they serve as a source of energy for cellular activity and store nutrients, carry out protein synthesis, and transmit hereditary information.

The article examined the essence and examples of inorganic substances, their role in the composition of the cell. We can say that the existence of living organisms would be impossible without groups of organic and inorganic compounds. They are important in every area of ​​human life, as well as in the existence of every organism.