Trivial names of some inorganic compounds. Chemical names and formulas of substances 2 name of the substance
Oxides– compounds of elements with oxygen, the oxidation state of oxygen in oxides is always -2.
Basic oxides form typical metals with C.O. +1,+2 (Li 2 O, MgO, CaO, CuO, etc.).
Acidic oxides form nonmetals with S.O. more than +2 and metals with S.O. from +5 to +7 (SO 2, SeO 2, P 2 O 5, As 2 O 3, CO 2, SiO 2, CrO 3 and Mn 2 O 7). Exception: the oxides NO 2 and ClO 2 do not have corresponding acidic hydroxides, but they are considered acidic.
Amphoteric oxides formed by amphoteric metals with C.O. +2,+3,+4 (BeO, Cr 2 O 3, ZnO, Al 2 O 3, GeO 2, SnO 2 and PbO).
Non-salt-forming oxides– non-metal oxides with CO+1,+2 (CO, NO, N 2 O, SiO).
Grounds (main hydroxides ) - complex substances that consist of a metal ion (or ammonium ion) and a hydroxyl group (-OH).
Acidic hydroxides (acids)- complex substances that consist of hydrogen atoms and an acid residue.
Amphoteric hydroxides formed by elements with amphoteric properties.
Salts- complex substances formed by metal atoms combined with acidic residues.
Medium (normal) salts- all hydrogen atoms in acid molecules are replaced by metal atoms.
Acid salts- hydrogen atoms in the acid are partially replaced by metal atoms. They are obtained by neutralizing a base with an excess of acid. To correctly name sour salt, It is necessary to add the prefix hydro- or dihydro- to the name of a normal salt, depending on the number of hydrogen atoms included in the acid salt.
For example, KHCO 3 - potassium bicarbonate, KH 2 PO 4 - potassium dihydrogen orthophosphate
It must be remembered that acid salts can only form two or more basic acids.
Basic salts- hydroxo groups of the base (OH −) are partially replaced by acidic residues. To name basic salt, it is necessary to add the prefix hydroxo- or dihydroxo- to the name of a normal salt, depending on the number of OH groups included in the salt.
For example, (CuOH) 2 CO 3 is copper (II) hydroxycarbonate.
It must be remembered that basic salts can only form bases containing two or more hydroxo groups.
Double salts- they contain two different cations; they are obtained by crystallization from a mixed solution of salts with different cations, but the same anions. For example, KAl(SO 4) 2, KNaSO 4.
Mixed salts- they contain two different anions. For example, Ca(OCl)Cl.
Hydrate salts (crystal hydrates) - they contain molecules of water of crystallization. Example: Na 2 SO 4 10H 2 O.
Trivial names of commonly used inorganic substances:
| Formula | Trivial name |
| NaCl | halite, rock salt, table salt |
| Na 2 SO 4 *10H 2 O | Glauber's salt |
| NaNO3 | Sodium, Chilean nitrate |
| NaOH | caustic soda, caustic soda, caustic soda |
| Na 2 CO 3 *10H 2 O | crystal soda |
| Na 2 CO 3 | Soda Ash |
| NaHCO3 | baking (drinking) soda |
| K2CO3 | potash |
| CON | caustic potassium |
| KCl | potassium salt, sylvite |
| KClO3 | Berthollet's salt |
| KNO 3 | Potassium, Indian saltpeter |
| K 3 | red blood salt |
| K 4 | yellow blood salt |
| KFe 3+ | Prussian blue |
| KFe 2+ | Turnbull blue |
| NH4Cl | Ammonia |
| NH 3 *H 2 O | ammonia, ammonia water |
| (NH 4) 2 Fe(SO 4) 2 | Mohr's salt |
| CaO | quicklime (burnt) lime |
| Ca(OH) 2 | slaked lime, lime water, milk of lime, lime dough |
| СaSO 4 *2H 2 O | Gypsum |
| CaCO3 | marble, limestone, chalk, calcite |
| CaHPO 4 × 2H2O | Precipitate |
| Ca(H 2 PO 4) 2 | double superphosphate |
| Ca(H 2 PO 4) 2 +2CaSO 4 | simple superphosphate |
| CaOCl 2 (Ca(OCl) 2 + CaCl 2) | bleaching powder |
| MgO | magnesia |
| MgSO 4 *7H 2 O | Epsom (bitter) salt |
| Al2O3 | corundum, bauxite, alumina, ruby, sapphire |
| C | diamond, graphite, soot, coal, coke |
| AgNO3 | lapis |
| (CuOH) 2 CO 3 | malachite |
| Cu2S | copper luster, chalcocite |
| CuSO 4 *5H 2 O | copper sulfate |
| FeSO 4 *7H 2 O | inkstone |
| FeS 2 | pyrite, iron pyrite, sulfur pyrite |
| FeCO 3 | siderite |
| Fe 2 O 3 | red iron ore, hematite |
| Fe 3 O 4 | magnetic iron ore, magnetite |
| FeO × nH 2 O | brown iron ore, limonite |
| H2SO4 × nSO 3 | oleum solution of SO 3 in H 2 SO 4 |
| N2O | laughing gas |
| NO 2 | brown gas, foxtail |
| SO 3 | sulfuric gas, sulfuric anhydride |
| SO 2 | sulfur dioxide, sulfur dioxide |
| CO | carbon monoxide |
| CO2 | carbon dioxide, dry ice, carbon dioxide |
| SiO2 | silica, quartz, river sand |
| CO+H2 | water gas, synthesis gas |
| Pb(CH3COO)2 | lead sugar |
| PbS | lead luster, galena |
| ZnS | zinc blende, sphalerite |
| HgCl2 | corrosive sublimate |
| HgS | cinnabar |
8.1. What is chemical nomenclature
Chemical nomenclature developed gradually over several centuries. As chemical knowledge accumulated, it changed several times. It is being refined and developed even now, which is connected not only with the imperfection of some nomenclature rules, but also with the fact that scientists are constantly discovering new and new compounds, which sometimes turn out to be named (and sometimes even put together formulas), using existing rules. impossible. The nomenclature rules currently accepted by the scientific community around the world are contained in a multi-volume publication: “IUPAC Nomenclature Rules for Chemistry”, the number of volumes in which is continuously increasing.
You are already familiar with the types of chemical formulas, as well as some of the rules for their composition. What are the names of chemical substances?
Using nomenclature rules, you can create systematic Name substances.
For many substances, in addition to systematic ones, traditional, so-called trivial titles. When they appeared, these names reflected certain properties of substances, methods of preparation, or contained the name of what the substance was isolated from. Compare the systematic and trivial names of the substances given in Table 25.
All names of minerals (natural substances that make up rocks) are also trivial, for example: quartz (SiO 2); rock salt, or halite (NaCl); zinc blende, or sphalerite (ZnS); magnetic iron ore, or magnetite (Fe 3 O 4); pyrolusite (MnO 2); fluorspar, or fluorite (CaF 2) and many others.
Table 25. Systematic and trivial names of some substances
Systematic name |
Trivial name |
|
| NaCl | Sodium chloride | Salt |
| Na 2 CO 3 | Sodium carbonate | Soda, soda ash |
| NaHCO3 | Sodium bicarbonate | Baking soda |
| CaO | Calcium oxide | Quicklime |
| Ca(OH)2 | Calcium hydroxide | Slaked lime |
| NaOH | Sodium hydroxide | Caustic soda, caustic soda, caustic |
| KOH | Potassium hydroxide | Caustic potassium |
| K2CO3 | Potassium carbonate | Potash |
| CO2 | Carbon dioxide | Carbon dioxide, carbon dioxide |
| CO | Carbon monoxide | Carbon monoxide |
| NH4NO3 | Ammonium nitrate | Ammonium nitrate |
| KNO 3 | Potassium nitrate | Potassium nitrate |
| KClO3 | Potassium chlorate | Bertholet's salt |
| MgO | Magnesium oxide | Magnesia |
For some of the most well-known or widespread substances, only trivial names are used, for example: water, ammonia, methane, diamond, graphite and others. In this case, such trivial names are sometimes called special.
You will learn how the names of substances belonging to different classes are composed in the following paragraphs.
| Sodium carbonate Na 2 CO 3 . The technical (trivial) name is soda ash (that is, calcined), or simply “soda.” The white substance, thermally very stable (melts without decomposition), dissolves well in water, partially reacting with it, and an alkaline environment is created in the solution. Sodium carbonate is an ionic compound with a complex anion, the atoms of which are linked together by covalent bonds. Soda was previously widely used in everyday life for washing clothes, but has now been completely replaced by modern washing powders. Sodium carbonate is obtained using a rather complex technology from sodium chloride, and is used mainly in the production of glass. Potassium carbonate K 2 CO 3. The technical (trivial) name is potash. In structure, properties and use, potassium carbonate is very similar to sodium carbonate. Previously, it was obtained from plant ash, and the ash itself was used in washing. Currently, most potassium carbonate is obtained as a by-product of the production of alumina (Al 2 O 3), used to make aluminum. Due to its hygroscopicity, potash is used as a drying agent. It is also used in the production of glass, pigments, and liquid soap. In addition, potassium carbonate is a convenient reagent for the production of other potassium compounds. |
CHEMICAL NOMENCLATURE, SYSTEMATIC NAME, TRIVIAL NAME, SPECIAL NAME.
1. Write down ten trivial names of any compounds (not in the table) from the previous chapters of the textbook, write down the formulas of these substances and give their systematic names.
2. What do the trivial names “table salt”, “soda ash”, “carbon monoxide”, “burnt magnesia” mean?
8.2. Names and formulas of simple substances
The names of most simple substances coincide with the names of the corresponding elements. Only all allotropic modifications of carbon have their own special names: diamond, graphite, carbyne and others. In addition, one of the allotropic modifications of oxygen has its own special name - ozone.
The simplest formula of a simple non-molecular substance consists only of the symbol of the corresponding element, for example: Na - sodium, Fe - iron, Si - silicon.
Allotropic modifications are designated using alphabetic indices or letters of the Greek alphabet:
C (a) – diamond; -
Sn – gray tin;
C (gr) – graphite; -
Sn – white tin.
In the molecular formulas of molecular simple substances, the index, as you know, shows the number of atoms in the molecule of the substance:
H 2 – hydrogen; O 2 – oxygen; Cl 2 – chlorine; O 3 – ozone.
In accordance with nomenclature rules, the systematic name of such a substance must contain a prefix indicating the number of atoms in the molecule:
H 2 – dihydrogen;
O 3 – trioxygen;
P 4 – tetraphosphorus;
S 8 - octasulfur, etc., but at present this rule has not yet become generally accepted.
Table 26.Numeric prefixes
| Factor | Console | Factor | Console | Factor | Console |
| mono | penta | nona | |||
| di | hexa | soundboard | |||
| three | hepta | undeka | |||
| tetra | Octa | dodeca |
| Ozone O3– a light blue gas with a characteristic odor, in a liquid state it is dark blue, in a solid state it is dark purple. This is the second allotropic modification of oxygen. Ozone is much more soluble in water than oxygen. O 3 is unstable and even at room temperature slowly turns into oxygen. Very reactive, destroys organic substances, reacts with many metals, including gold and platinum. You can smell ozone during a thunderstorm, since in nature ozone is formed as a result of the action of lightning and ultraviolet radiation on atmospheric oxygen. Above the Earth there is an ozone layer located at an altitude of about 40 km, which traps the bulk of the ultraviolet radiation of the Sun, which is destructive for all living things. Ozone has bleaching and disinfecting properties. In some countries it is used to disinfect water. In medical institutions, ozone produced in special devices - ozonizers - is used to disinfect premises. |
8.3. Formulas and names of binary substances
In accordance with the general rule, in the formula of a binary substance, the symbol of an element with a lower electronegativity of atoms is placed in the first place, and in the second place - with a higher one, for example: NaF, BaCl 2, CO 2, OF 2 (and not FNa, Cl 2 Ba, O 2 C or F 2 O!).
Since electronegativity values for atoms of different elements are constantly being refined, two rules of thumb are usually used:
1. If a binary compound is a compound of a metal-forming element with
element forming a non-metal, then the symbol of the element forming the metal is always placed in first place (on the left).
2. If both elements included in the compound are elements that form non-metals, then their symbols are arranged in the following sequence:
B, Si, C, Sb, As, P, N, H, Te, Se, S, At, I, Br, Cl, O, F.
Note: It should be remembered that nitrogen's place in this practical series does not correspond to its electronegativity; as a general rule it should be placed between chlorine and oxygen.
Examples: Al 2 O 3, FeO, Na 3 P, PbCl 2, Cr 2 S 3, UO 2 (according to the first rule);
BF 3, CCl 4, As 2 S 3, NH 3, SO 3, I 2 O 5, OF 2 (according to the second rule).
The systematic name of a binary compound can be given in two ways. For example, CO 2 can be called carbon dioxide - you already know this name - and carbon monoxide (IV). In the second name, the Stock number (oxidation state) of carbon is indicated in parentheses. This is done in order to distinguish this compound from CO - carbon monoxide (II).
You can use either type of name, depending on which one is more convenient in this case.
Examples (more convenient names are highlighted):
| MnO | manganese monoxide | manganese(II) oxide |
| Mn2O3 | dimanganese trioxide | manganese oxide(III) |
| MnO2 | manganese dioxide | manganese(IV) oxide |
| Mn2O7 | dimanganese heptoxide | manganese oxide(VII) |
Other examples:
If the atoms of the element that comes first in the formula of a substance exhibit only one positive oxidation state, then neither numerical prefixes nor the designation of this oxidation state in the name of the substance are usually used, for example:
Na 2 O – sodium oxide; KCl – potassium chloride;
Cs 2 S – cesium sulfide; BaCl 2 – barium chloride;
BCl 3 – boron chloride; HCl – hydrogen chloride (hydrogen chloride);
Al 2 O 3 – aluminum oxide; H 2 S – hydrogen sulfide (hydrogen sulfide).
1. Make up systematic names of substances (for binary substances - in two ways):
a) O 2, FeBr 2, BF 3, CuO, HI;
b) N 2, FeCl 2, Al 2 S 3, CuI, H 2 Te;
c) I 2, PCl 5, MnBr 2, BeH 2, Cu 2 O.
2.Name each of the nitrogen oxides in two ways: N 2 O, NO, N 2 O 3, NO 2, N 2 O 4, N 2 O 5. Emphasize more user-friendly names.
3. Write down the formulas of the following substances:
a) sodium fluoride, barium sulfide, strontium hydride, lithium oxide;
b) carbon(IV) fluoride, copper(II) sulfide, phosphorus(III) oxide, phosphorus(V) oxide;
c) silicon dioxide, diiodine pentoxide, diphosphorus trioxide, carbon disulfide;
d) hydrogen selenide, hydrogen bromide, hydrogen iodide, hydrogen telluride;
e) methane, silane, ammonia, phosphine.
4. Formulate the rules for composing formulas for binary substances according to the position of the elements that make up this substance in the system of elements.
8.4. Formulas and names of more complex substances
As you have already noticed, in the formula of a binary compound, the first place is the symbol of a cation or an atom with a partial positive charge, and the second is the symbol of an anion or an atom with a partial negative charge. Formulas for more complex substances are compiled in the same way, but the places of atoms or simple ions in them are taken by groups of atoms or complex ions.
As an example, consider the compound (NH 4) 2 CO 3. In it, the formula of the complex cation (NH 4) is in first place, and the formula of the complex anion (CO 3 2) is in second place.
In the formula of the most complex ion, the symbol of the central atom, that is, the atom to which the remaining atoms (or groups of atoms) of this ion are associated, is placed first, and the oxidation state of the central atom is indicated in the name.
Examples of systematic names:
Na 2 SO 4 sodium tetraoxosulfate(VI),
K 2 SO 3 potassium(II) trioxosulfate(IV),
CaCO 3 calcium(II) trioxocarbonate(IV),
(NH 4) 3 PO 4 ammonium tetraoxophosphate(V),
PH 4 Cl phosphonium chloride,
Mg(OH) 2 magnesium(II) hydroxide.
Such names accurately reflect the composition of the compound, but are very cumbersome. Therefore, abbreviated ones ( semi-systematic) names of these compounds:
Na 2 SO 4 sodium sulfate,
K 2 SO 3 potassium sulfite,
CaCO 3 calcium carbonate,
(NH 4) 3 PO 4 ammonium phosphate,
Mg(OH) 2 magnesium hydroxide.
The systematic names of acids are composed as if the acid is a hydrogen salt:
H 2 SO 4 hydrogen tetraoxosulfate(VI),
H 2 CO 3 hydrogen trioxocarbonate (IV),
H 2 hydrogen hexafluorosilicate (IV). (You will learn about the reasons for using square brackets in the formula of this compound later)
But for the most well-known acids, nomenclature rules allow the use of their trivial names, which, together with the names of the corresponding anions, are given in Table 27.
Table 27.Names of some acids and their anions
Name |
Formula
SEMI-SYSTEMATIC NAMES OF ACIDS AND SALTS. | |||
Chemical formula is an image using symbols.
Chemical element signs
Chemical sign or chemical element symbol– this is the first or two first letters of the Latin name of this element.
For example: FerrumFe , Cuprum –Cu , OxygeniumO etc.
Table 1: Information provided by a chemical sign
| Intelligence | Using the example of Cl |
| Item name | Chlorine |
| Non-metal, halogen | |
| One element | 1 chlorine atom |
| (Ar) of this element | Ar(Cl) = 35.5 |
| Absolute atomic mass of a chemical element
m = Ar 1.66 10 -24 g = Ar 1.66 10 -27 kg |
M (Cl) = 35.5 1.66 10 -24 = 58.9 10 -24 g |
The name of a chemical symbol in most cases is read as the name of a chemical element. For example, K – potassium, Ca – calcium, Mg – magnesium, Mn – manganese.
Cases when the name of a chemical symbol is read differently are given in Table 2:
| Chemical element name | Chemical sign | Chemical symbol name
(pronunciation) |
| Nitrogen | N | En |
| Hydrogen | H | Ash |
| Iron | Fe | Ferrum |
| Gold | Au | Aurum |
| Oxygen | O | ABOUT |
| Silicon | Si | Silicium |
| Copper | Cu | Cuprum |
| Tin | Sn | Stanum |
| Mercury | Hg | Hydrargium |
| Lead | Pb | Plumbum |
| Sulfur | S | Es |
| Silver | Ag | Argentum |
| Carbon | C | Tse |
| Phosphorus | P | Pe |
Chemical formulas of simple substances
The chemical formulas of most simple substances (all metals and many non-metals) are the signs of the corresponding chemical elements.
So iron substance And chemical element iron are designated the same - Fe .
If it has a molecular structure (exists in the form , then its formula is the chemical symbol of the element with index bottom right indicating number of atoms in a molecule: H 2, O2, O 3, N 2, F 2, Cl2, BR 2, P 4, S 8.
Table 3: Information provided by a chemical symbol
| Intelligence | Using C as an example |
| Substance name | Carbon (diamond, graphite, graphene, carbyne) |
| Belonging of an element to a given class of chemical elements | Non-metal |
| One atom of an element | 1 carbon atom |
| Relative atomic mass (Ar) element that forms a substance | Ar(C) = 12 |
| Absolute atomic mass | M(C) = 12 1.66 10-24 = 19.93 10 -24 g |
| One substance | 1 mole of carbon, i.e. 6.02 10 23 carbon atoms |
| M (C) = Ar (C) = 12 g/mol |
Chemical formulas of complex substances
The formula of a complex substance is prepared by writing down the signs of the chemical elements of which the substance is composed, indicating the number of atoms of each element in the molecule. In this case, as a rule, chemical elements are written in order of increasing electronegativity in accordance with the following practical series:
Me, Si, B, Te, H, P, As, I, Se, C, S, Br, Cl, N, O, F
For example, H2O , CaSO4 , Al2O3 , CS 2 , OF 2 , NaH.
The exceptions are:
- some compounds of nitrogen with hydrogen (for example, ammonia NH 3 , hydrazine N 2H 4 );
- salts of organic acids (for example, sodium formate HCOONa , calcium acetate (CH 3COO) 2Ca) ;
- hydrocarbons ( CH 4 , C2H4 , C2H2 ).
Chemical formulas of substances existing in the form dimers (NO 2 , P2O 3 , P2O5, salts of monovalent mercury, for example: HgCl , HgNO3 etc.), written in the form N 2 O4,P 4 O6,P 4 O 10Hg 2 Cl2,Hg 2 ( NO 3) 2 .
The number of atoms of a chemical element in a molecule and a complex ion is determined based on the concept valency or oxidation states and is recorded index lower right from the sign of each element (index 1 is omitted). In this case, they proceed from the rule:
the algebraic sum of the oxidation states of all atoms in a molecule must be equal to zero (the molecules are electrically neutral), and in a complex ion - the charge of the ion.
For example:
2Al 3 + +3SO 4 2- =Al 2 (SO 4) 3
The same rule is used when determining the oxidation state of a chemical element using the formula of a substance or complex. It is usually an element that has several oxidation states. The oxidation states of the remaining elements forming the molecule or ion must be known.
The charge of a complex ion is the algebraic sum of the oxidation states of all the atoms that form the ion. Therefore, when determining the oxidation state of a chemical element in a complex ion, the ion itself is placed in brackets, and its charge is taken out of brackets.
When compiling formulas for valence a substance is represented as a compound consisting of two particles of different types, the valencies of which are known. Next they use rule:
in a molecule, the product of valence by the number of particles of one type must be equal to the product of valence by the number of particles of another type.
For example:
The number preceding the formula in a reaction equation is called coefficient. She indicates either number of molecules, or number of moles of substance.
The coefficient before the chemical symbol, indicates number of atoms of a given chemical element, and in the case when the sign is the formula of a simple substance, the coefficient indicates either number of atoms, or the number of moles of this substance.
For example:
- 3 Fe– three iron atoms, 3 moles of iron atoms,
- 2 H– two hydrogen atoms, 2 moles of hydrogen atoms,
- H 2– one molecule of hydrogen, 1 mole of hydrogen.
The chemical formulas of many substances have been determined experimentally, which is why they are called "empirical".
Table 4: Information provided by the chemical formula of a complex substance
| Intelligence | For example C aCO3 |
| Substance name | Calcium carbonate |
| Belonging of an element to a certain class of substances | Medium (normal) salt |
| One molecule of substance | 1 molecule calcium carbonate |
| One mole of substance | 6.02 10 23 molecules CaCO3 |
| Relative molecular mass of the substance (Mr) | Мr (CaCO3) = Ar (Ca) + Ar (C) + 3Ar (O) = 100 |
| Molar mass of the substance (M) | M (CaCO3) = 100 g/mol |
| Absolute molecular mass of the substance (m) | M (CaCO3) = Mr (CaCO3) 1.66 10 -24 g = 1.66 10 -22 g |
| Qualitative composition (what chemical elements form the substance) | calcium, carbon, oxygen |
| Quantitative composition of the substance: | |
| The number of atoms of each element in one molecule of a substance: | a calcium carbonate molecule is made up of 1 atom calcium, 1 atom carbon and 3 atoms oxygen. |
| Number of moles of each element in 1 mole of substance: | In 1 mole CaCO 3(6.02 · 10 23 molecules) contained 1 mole(6.02 · 10 23 atoms) calcium, 1 mole(6.02 10 23 atoms) carbon and 3 mol(3 6.02 10 23 atoms) of the chemical element oxygen) |
| Mass composition of the substance: | |
| Mass of each element in 1 mole of substance: | 1 mole of calcium carbonate (100g) contains the following chemical elements: 40g calcium, 12g carbon, 48g oxygen. |
| Mass fractions of chemical elements in the substance (composition of the substance as a percentage by weight):
|
Composition of calcium carbonate by weight:
W (Ca) = (n (Ca) Ar (Ca))/Mr (CaCO3) = (1·40)/100= 0.4 (40%) W (C) = (n (Ca) Ar (Ca))/Mr (CaCO3) = (1 12)/100 = 0.12 (12%) W (O) = (n (Ca) Ar (Ca))/Mr (CaCO3) = (3 16)/100 = 0.48 (48%) |
| For a substance with an ionic structure (salt, acid, base), the formula of the substance provides information about the number of ions of each type in the molecule, their quantity and the mass of ions per 1 mole of the substance:
|
Molecule CaCO 3 consists of an ion Ca 2+ and ion CO 3 2-
1 mol ( 6.02 10 23 molecules) CaCO 3 contains 1 mol Ca 2+ ions And 1 mole ions CO 3 2-; 1 mole (100g) of calcium carbonate contains 40g ions Ca 2+ And 60g ions CO 3 2- |
| Molar volume of a substance at standard conditions (for gases only) | |
Graphic formulas
To obtain more complete information about a substance, use graphic formulas , which indicate order of connection of atoms in a molecule And valence of each element.
Graphic formulas of substances consisting of molecules sometimes, to one degree or another, reflect the structure (structure) of these molecules, in these cases they can be called structural .
To compile a graphical (structural) formula of a substance, you must:
- Determine the valence of all chemical elements that form the substance.
- Write down the signs of all chemical elements that form the substance, each in an amount equal to the number of atoms of a given element in the molecule.
- Connect the signs of chemical elements with dashes. Each dash denotes a pair that communicates between chemical elements and therefore belongs equally to both elements.
- The number of lines surrounding the sign of a chemical element must correspond to the valency of this chemical element.
- When formulating oxygen-containing acids and their salts, hydrogen atoms and metal atoms are bonded to the acid-forming element through an oxygen atom.
- Oxygen atoms are combined with each other only when formulating peroxides.
Examples of graphic formulas:
Classes and nomenclature of chemical inorganic compounds
PART II
Guidelines for laboratory work in the course "CHEMISTRY"
COMPILERS:
BELOVA S.B
GRISHINA N.D.
GORLACHEVA T.K.
MAMONOV I.M.
MOSCOW 2001
1. COMPLEX CONNECTIONS
Complex connections are certain chemical compounds formed by a combination of individual components and representing complex ions or molecules capable of existing in both crystalline and dissolved states.
In the molecule of a complex compound, one of the atoms, usually positively charged, occupies a central position and is called complexing agent, or central atom. In close proximity to it are located (coordinated) oppositely charged ions or neutral molecules, called ligands. The complexing agent and ligands constitute the inner sphere of the complex compound.
Outside the inner sphere of the complex compound is its outer sphere, containing positively charged ions (if the inner sphere of the complex compound is negatively charged) or negatively charged ions (if the complex ion is positively charged); in the case of an uncharged inner sphere, there is no outer sphere.
The formula of a multi-element complex particle (charged or neutral) includes a central atom M and a certain number n of ligands L: . The name of such a particle is constructed according to the following scheme:
Number of identical _ Name _ Name of central
ligands ligands atom
In this case, the names of the ligands receive a connecting vowel – O, For example:
F - - fluoro,OH - - hydroxo,
Cl - - chloro , CN - - cyano,
O -2 – oxo , NCS -2 – thiocyano,
S -2 - thio.H - - hydrido.
The names of neutral ligands do not change (N 2 - dinitrogen, N 2 H 4 - hydrazine, C 6 H 6 - benzene, etc.), except for the names of the following common ligands:
H 2 O – aqua, CO – carbonyl,
NH 3 – amine, NO – nitrosyl.
Ion H + called a hydroligand.
The names of neutral complexes are constructed without any additions, the names of cationic complexes indicate the oxidation state of the neutral atom, and the names of anionic complexes have the ending - at and the same indication of the degree of oxidation (for some elements, the roots of the Latin names of the elements are used as the central atoms, i.e. instead of copper - cupr, instead of iron - ferr, etc.).
[Co(NH 3) 3 Cl 3 ] - trichlorotriammine cobalt,
[Сu(NH 3) 4 ]SO 4 – tetraammine copper (II) sulfate,
Cl 3 – hexaaqua aluminum (III) chloride,
K 4 – potassium hexacyanoferrate (II),
K 3 – potassium hexacyanoferrate (III).
2. NAME OF IONS
2.1.NAMES OF CATIONS
Monatomic cations are indicated by the words " and he" and the Russian name of the corresponding elements in the genitive case.
Li +1 – lithium ion,
Th +4 – thorium ion.
If an element forms cations with different valence states, then it is indicated by a Roman numeral in parentheses after the name of the element.
Ce +3 – cerium (III) ion,
Ce +4 – cerium ion (IY).
When complex cations a prefix is added to the name of the main element forming the ion, indicating the number of electronegative atoms or groups connected to it.
Al(OH) +2 – hydroxo aluminum ion,
Al(OH) 2 +1 – dihydroxo aluminum ion.
The different valence states of cation-forming elements are indicated by a Roman numeral after the name of the element.
FeOH +1 – iron hydroxyl II-and he,
FeOH +2 – iron hydroxyl III-and he.
If the basic salts are dehydrated (lost water), then the name of the cation containing an oxygen atom is prefixed oxo-.
TiO +2 – oxo titanium ion
UO 2 +2 – dioxo uranium ion.
2.2. NAME OF ANIONS
Titles elementary anions are formed from the roots of the Latin names of the corresponding elements with the suffix – go- and the words " and he", connected by a hyphen.
F -1 – fluoride ion,
H -1 –hydride ion,
S -2 – sulfide ion,
O -2 is an oxide ion.
If the anion contains hydrogen atom, then the prefix is added to the name of the elementary ion hydro-.
HS -1 –hydrosulfide ion,
OH -1 –hydroxide ion.
Titles oxygen acid anions are composed from the root of the Latin name of the acid-forming element and have the endings - at(for the highest degree of oxidation of the element) and - it(for the lowest oxidation state of the element).
SO 4 -2 -sulf at-and he,
SO 3 -2 -sulf it-and he.
If an element forms an acid in more than two oxidation states, then:
For the highest degree of oxidation, acid anions have the suffix – at- and prefix per-;
For the lowest oxidation state, the suffix is – it- and prefix hypo-.
acid name of corresponding anion
chlorine HClO 4, lane chlorine at-and he,
hypochlorous HClO 3, chlorate ion,
chloride HClO 2, chlorite ion,
hypochlorous HClO, hypo chlorine it- and he.
For meta- and ortho-acid anions, the corresponding prefixes are added to the name of the ion.
PO 4 -3 -orthophosphate ion,
PO 3 -1 -metaphosphate ion.
The names of anions of acid salts use the prefix hydro-, indicating the number of hydrogen atoms contained in the ion.
HPO 4 -2 is a hydroorthophosphate ion.
H 2 PO 4 -1 - dihydrogen orthophosphate ion
IN complex ion before the root of the Latin name of the complex-forming atom, a prefix from Greek numerals is placed, indicating the number of ligands and the name of the ligand, and after - the ending - at. In the case when the ligand is an anion, its name is supplemented with a vowel - O.
3 – hexacyan O III ferr at-and he,
4 – hexacyan O II ferr at-and he.
3. INDIVIDUAL TASK
OPTION I
| Exercise 1 | Exercise 2 | Exercise 3 |
| Cu2O | HNO3 | V +3 |
| CuO | HNO2 | Bi(OH) 2 +1 |
| BaO2 | HNbO3 | HSO 3 -1 |
| LaF 3 | H2CrO4 | CrPO 4 |
| H2S | H2Cr2O7 | KHCO 3 |
| Al 2 S 3 | Ce(OH)3 | Fe(OH)2Cl |
| OF 2 | U(OH)2 | KFe(SO 4) 2 |
Exercise 4
1. Lithium hemioxide,
2. Tantalum hemipentaoxide,
3. Zirconium tetrafluoride,
4. Selenic acid,
5. Oxygen difluoride,
6. Europium trihydride,
7. Tin tetrahydroxide,
8. Neodymium orthophosphate,
9. Rubidium bicarbonate,
10. Potassium hexacyanoferrate (II).
OPTION II
Write the names of chemical compounds and ions
| Exercise 1 | Exercise 2 | Exercise 3 |
| V2O5 | H2SO4 | La +3 |
| Na2O2 | H2SO3 | Ir(OH) 2 +2 |
| NdF 3 | HIO | HSO 4 -1 |
| H2Se | HIO 3 | LaPO 4 |
| CS 2 | HVO 3 | NaHSO3 |
| Al 4 C 3 | La(OH)3 | Cr(OH)2Br |
| Mg 3 As 2 | Ir(OH) 4 | NaCr(SO 4) 2 |
Exercise 4
Write their formulas based on the names of chemical compounds.
1. Cerium tetrahydroxide,
2. Chromium hemitrioxide,
3. Yttrium trifluoride,
4. Metavanadic acid,
5. Carbon disulfide,
6. Calcium dihydride,
7. Zirconium monocarbide,
8. Lanthanum orthophosphate,
9. Dihydroxoaluminum chloride,
10. Potassium hexacyanoferrate (III).
OPTION III
Write the names of chemical compounds and ions
| Exercise 1 | Exercise 2 | Exercise 3 |
| UO 2 | H2SiO3 | U+3 |
| UO 3 | H4SiO4 | As(OH) 2 +1 |
| Hg2O | HClO | HCO 3 -1 |
| H2Te | HClO2 | VPO 4 |
| B 2 C | H2B4O7 | KHSO 4 |
| Ba 3 Sb 2 | Nd(OH)3 | Al(OH)2Cl |
| CH 4 | Th(OH) 4 | K2NaPO3 |
Exercise 4
Write their formulas based on the names of chemical compounds.
1. Chromium trihydroxide,
2. Manganese dioxide,
3. Uranium tetrafluoride,
4. Molybdic acid,
5. Yttrium trihydride,
6. Potassium dichromate,
7. Dihydroxoaluminum bromide,
8. Sodium bicarbonate,
9. Potassium chromate,
10. Sodium hexacyanoferrate (II).
OPTION IY
Write the names of chemical compounds and ions
| Exercise 1 | Exercise 2 | Exercise 3 |
| WO 2 | H2MnO4 | Th +4 |
| WO 3 | HMnO4 | Al(OH) 2 +1 |
| K2O2 | HClO4 | HCrO 4 -1 |
| LuF 3 | HClO3 | NdPO4 |
| HI | H4P2O7 | KHCrO4 |
| ZnSe | V(OH)3 | BiOHCl2 |
| SiF 4 | Hf(OH) 4 | LiAl(SO 4) 2 |
Exercise 4
Write their formulas based on the names of chemical compounds.
1. Sulfur dioxide,
2. Thorium tetrahydroxide,
3. Uranium hexafluoride,
4. Zirconium tetrahydride,
5. Sodium hydrosulfite,
6. Dihydroxoiron(III) chloride,
7. Ammonium molybdate,
8. Tetraboric acid,
9. Potassium chromium sulfate,
10. Sodium hexacyanoferrate (III).
4. METHODS OF OBTAINING CHEMICAL COMPOUNDS
4.1.WAYS TO OBTAIN BASES
1)Preparation of alkalis:
1) Metal + water 2Na+2H 2 O=2NaOH+H 2.
Ba+2H 2 O=2Ba(OH) 2 +H 2.
2) Oxide + water Li 2 O+H 2 O=2LiOH.
CaO + 2H 2 O=2Ca(OH) 2.
3) Electrolysis of aqueous NaCl Û Na + + Cl - .
alkaline salt solutions
metals
2)Preparation of water-insoluble bases:
Salt + alkali CuSO 4 +2NaOH=Cu(OH) 2 ¯+Na 2 SO 4,
Cu 2+ + 2OH - =Cu(OH) 2.
FeCl 2 +2KOH=Fe(OH) 2 ¯+2KCl,
Fe 2+ + 2OH - =Fe(OH) 2.
________________________________________________
Exception: Na 2 CO 3 +Ca(OH) 2 =2NaOH+Ca(CO) 3¯.
OBTAINING THE GROUND
Experience 1. Interaction of magnesium with water.
Mg+2H 2 O = Mg(OH) 2 ¯+H 2
raspberry color
Conclusion: the coloring of the solution crimson in the presence of phenolphthalein (pf) at the Mg - H 2 O phase interface occurs due to the formation of Mg(OH) 2.
Experience 2. Reaction of magnesium oxide with water
MgO+H 2 O = Mg(OH) 2 ¯
raspberry color
Conclusion: the solution turns crimson in the presence of phenolphthalein (pf) indicates the formation of Mg(OH) 2. We observe a more intense coloring of the solution than in the first experiment, because MgO has a large surface area.
Experience 3. Preparation of weak and poorly soluble bases
1.1. NH 4 Cl + NaOH = NH 4 OH (NH 3 + H 2 O) + NaCl.
1.2. FeCl 3 +3NaOH = Fe(OH) 3 ¯+3NaCl,
Fe 3+ + 3OH - =Fe(OH) 3.
1.3. CuSO 4 +2NaOH=Cu(OH) 2 ¯+Na 2 SO 4,
k. blue
Cu 2+ + 2OH - =Cu(OH) 2.
Conclusion: Weak and poorly soluble bases are formed by the interaction of salts with alkalis.
METHODS OF OBTAINING ACIDS
1)Obtaining oxygen-containing acids:
interaction of the corresponding SO 3 + H 2 O = H 2 SO 4
anhydrides with water N 2 O 5 + H 2 O = 2HNO 3.
2)Preparation of some oxygen-containing acids:
effect on non-metals of strong 2P + 5HNO 3 + 2H 2 O = 3H 3 PO 4 +5NO
oxidizing agents 3I 2 +10HNO 3 = 6HIO 3 +10NO+2H 2 O.
3) Obtaining oxygen-free acids:
direct interaction of elements H 2 +Cl 2 =2HCl.
4)General method:
exchange reaction between salt NaCl + H 2 SO 4 = HCl + NaHSO 4
and less volatile acid NaNO 3 +H 2 SO 4 =HNO 3 +NaHSO 4.
4.4. OBTAINING ACIDS
Experience 1. Reaction of anhydride with water
1.1. S+O 2 =SO 2,
1.2.SO 2 +H 2 O +H 2 SO 3.
Experience 2. Exchange reaction between a salt and a more volatile acid
2.1. 2NaCH 3 COO+H 2 SO 4 =Na 2 SO 4 +2CH 3 COOH,
k. characteristic odor
CH 3 COO - +H + = CH 3 COOH.
2.2. 2NaCl+H 2 SO 4 =Na 2 SO 4 +2HCl.
gas evolution
Conclusion. Some of the ways to produce acids are:
Interaction of anhydride with water;
Interaction of salt with non-volatile acid.
4.5. METHODS OF OBTAINING SALT
1) From metals:
Metals with non-metals Mg+Cl 2 =MgCl 2,
Metals with acids Zn+H 2 SO 4 =ZnSO 4 +H 2,
Metals with salts Cu+HgCl 2 =CuCl 2 +Hg.
2) From oxides:
Basic oxides with acids CaO+2HCl= CaCl 2 +H 2 O,
Acidic oxides with bases CO 2 +Ca(OH) 2 = CaCO 3 +H 2 O,
Acidic oxides with basic CaO+CO 2 =CaCO 3.
3)Neutralization reaction:
Acid with base H 2 SO 4 +2NaOH=Na 2 SO 4 +2H 2 O.
4)From salts:
Salts with salts AgNO 3 +NaCl=AgCl¯+NaNO 3,
Salts with bases CuSO 4 +2NaOH=Cu(OH) 2 ¯+Na 2 SO 4,
Salts with acids Na 2 CO 3 +2HCl=2NaCl+H 2 O+CO 2.
4.6. OBTAINING SALT
Experience 1. Interaction of salt with base
Al 2 (SO 4) 3 +8NaOH= 3Na 2 SO 4 +2NaAlO 2 +4H 2 O.
Experience 2. Salt-salt interactions
Pb(NO 3) 2 +KI=PbI 2 ¯+2KNO 3,
Pb 2+ + 2I - =PbI 2 ¯.
4.7.PREPARATION AND PROPERTIES OF AMPHOTERIC HYDROXIDES
Experience 1.
ZnSO 4 +2NaOH= Zn(OH) 2 ¯+ Na 2 SO 4,
Zn +2 + 2OH - =Zn(OH) 2 ¯.
2H + + ZnO 2 -2 ÛZn(OH)2 ÛZn +2 + 2OH -.
Experience 1.1 .
Zn(OH) 2 +2HCl=ZnCl 2 +2H 2 O,
Zn(OH) 2 +2H + =Zn +2 +2H 2 O.
Experience 1.2 .
Zn(OH) 2 +2NaOH=Na 2 ZnO 2 +2H 2 O,
Zn(OH) 2 +2OH - =ZnO 2 -2 +2H 2 O.
Conclusion: zinc hydroxide has amphoteric properties, i.e. reacts both with acids, exhibiting basic properties, and with bases, exhibiting acidic properties.
APPLICATION
Names of the most important acids and their salts
| Acid | Name | |
| acids | Salts | |
| HAlO2 | Meta-aluminum | Metaaluminate |
| HASO 3 | Metaarsenic | Metaarsenate |
| H3AsO4 | Orthoarsenic | Orthoarsenate |
| HАsO 2 | Metaarsenic | Metaarsenite |
| H3AsO3 | Orthoarsenic | Orthoarsenite |
| HBO 2 | Metaborn | Metaborate |
| H3BO3 | Orthoboric | Orthoborate |
| H2B4O7 | Quadruple | Tetraborate |
| HBr | Hydrogen bromide | Bromide |
| HOBr | brominated | Hypobromite |
| HBrO3 | Bromonic | Bromate |
| HCOOH | Ant | Formate |
| CH3COOH | Vinegar | Acetate |
| HCN | Hydrogen cyanide | Cyanide |
| H 2 CO 3 | Coal | Carbonate |
| H 2 C 2 O 4 | Sorrel | Oxalate |
| HCl | Hydrogen chloride | Chloride |
| HClO | Hypochlorous | Hypochlorite |
| HClO 2 | Chloride | Chlorite |
| HClO 3 | Chlorous | Chlorate |
| HClO 4 | Chlorine | Perchlorate |
| HCrO2 | Metachromic | Metachromite |
| H 2 СrO 4 | Chrome | Chromate |
| H 2 Cr 2 O 7 | Two-chrome | Dichromate |
| HI | Hydrogen iodide | Iodide |
| HOI | Iodineous | Hypoioditis |
| HIO 3 | Iodine | Iodate |
| HIO 4 | Iodine | Periodat |
| HMnO4 | Manganese | Permanganate |
| H2MnO4 | Manganese | Manganat |
| H2MoO4 | Molybdenum | Molybdate |
| HN 3 | Hydrogen azide (hydrogen nitrous) | Azid |
| HNO2 | Nitrogenous | Nitrite |
| HNO3 | Nitrogen | Nitrate |
| HPO 3 | Metaphosphoric | Metaphosphate |
| H3PO4 | Orthophosphoric | Orthophosphate |
| H4P2O7 | Diphosphoric (pyrophosphoric) | Diphosphate (pyrophosphate) |
| H3PO3 | Phosphorous | Phosphite |
| H3PO2 | Phosphorous | Hypophosphite |
| H2S | Hydrogen sulfide | Sulfide |
| HSCN | Rhodane hydrogen | Radonite |
| H2SO3 | Sulphurous | Sulfite |
| H2SO4 | Sulfuric | Sulfate |
| H2S2O3 | Thiosulfur | Thiosulfate |
| H2S2O7 | Two-sulphur (pyrosulfur) | Disulfate (pyrosulfate) |
| H2S2O8 | Peroxodusulfur (supersulfur) | Peroxodisulfate (persulfate) |
| H2Se | Hydrogen selenide | Selenide |
| H2SeO3 | Selenistaya | Selenite |
| H2SeO4 | Selenium | Selenat |
| H2SiO3 | Silicon | Silicate |
| HVO 3 | Vanadium | Vanadat |
| H2WO4 | Tungsten | Tungstate |
Check information. It is necessary to check the accuracy of the facts and reliability of the information presented in this article. On the talk page there is a discussion on the topic: Doubts regarding terminology. Chemical formula ... Wikipedia
A chemical formula reflects information about the composition and structure of substances using chemical symbols, numbers and dividing symbols of brackets. Currently, the following types of chemical formulas are distinguished: The simplest formula. Can be obtained by experienced... ... Wikipedia
A chemical formula reflects information about the composition and structure of substances using chemical symbols, numbers and dividing symbols of brackets. Currently, the following types of chemical formulas are distinguished: The simplest formula. Can be obtained by experienced... ... Wikipedia
A chemical formula reflects information about the composition and structure of substances using chemical symbols, numbers and dividing symbols of brackets. Currently, the following types of chemical formulas are distinguished: The simplest formula. Can be obtained by experienced... ... Wikipedia
A chemical formula reflects information about the composition and structure of substances using chemical symbols, numbers and dividing symbols of brackets. Currently, the following types of chemical formulas are distinguished: The simplest formula. Can be obtained by experienced... ... Wikipedia
Main article: Inorganic compounds List of inorganic compounds by element informational list of inorganic compounds presented in alphabetical order (by formula) for each substance, hydrogen acids of the elements (if ... ... Wikipedia
This article or section needs revision. Please improve the article in accordance with the rules for writing articles... Wikipedia
A chemical equation (equation of a chemical reaction) is a conventional representation of a chemical reaction using chemical formulas, numerical coefficients and mathematical symbols. The equation of a chemical reaction gives qualitative and quantitative... ... Wikipedia
Chemical software are computer programs used in the field of chemistry. Contents 1 Chemical editors 2 Platforms 3 Literature ... Wikipedia
Books
- A brief dictionary of biochemical terms, Kunizhev S.M. , The dictionary is intended for students of chemical and biological specialties at universities studying general biochemistry, ecology and fundamentals of biotechnology, and can also be used in ... Category: Biology Publisher: VUZOVSKAYA KNIGA, Manufacturer: UNIVERSITY BOOK,
- Emissions of harmful substances and their dangers to living organisms, V.I. Romanov, The book aims to combine and convey to the reader in a popular form a large amount of information of a medical-biological, environmental and emergency nature. It examines emissions... Category:
