Trivial names of some inorganic compounds. Chemical nomenclature of inorganic compounds Cu hs 2 name

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Classification inorganic substances and their nomenclature is based on the simplest and most constant characteristic over time - chemical composition, which shows the atoms of the elements that form a given substance in their numerical ratio. If a substance is made up of atoms of one chemical element, i.e. is the form of existence of this element in free form, then it is called simple substance; if the substance is made up of atoms of two or more elements, then it is called complex substance. All simple substances (except monatomic ones) and all complex substances are usually called chemical compounds, since in them atoms of one or different elements are connected to each other by chemical bonds.

The nomenclature of inorganic substances consists of formulas and names. Chemical formula - depiction of the composition of a substance using symbols of chemical elements, numerical indices and some other signs. Chemical name - image of the composition of a substance using a word or group of words. The construction of chemical formulas and names is determined by the system nomenclature rules.

The symbols and names of chemical elements are given in the Periodic Table of Elements by D.I. Mendeleev. The elements are conventionally divided into metals And nonmetals . Non-metals include all elements of group VIIIA (noble gases) and group VIIA (halogens), elements of group VIA (except polonium), elements nitrogen, phosphorus, arsenic (VA group); carbon, silicon (IVA group); boron (IIIA group), as well as hydrogen. The remaining elements are classified as metals.

When compiling the names of substances, Russian names of elements are usually used, for example, dioxygen, xenon difluoride, potassium selenate. Traditionally, for some elements, the roots of their Latin names are introduced into derivative terms:

For example: carbonate, manganate, oxide, sulfide, silicate.

Titles simple substances consist of one word - the name of a chemical element with a numerical prefix, for example:

The following are used numerical prefixes:

An indefinite number is indicated by a numeric prefix n- poly.

For some simple substances they also use special names such as O 3 - ozone, P 4 - white phosphorus.

Chemical formulas complex substances made up of the designation electropositive(conditional and real cations) and electronegative(conditional and real anions) components, for example, CuSO 4 (here Cu 2+ is a real cation, SO 4 2 - is a real anion) and PCl 3 (here P +III is a conditional cation, Cl -I is a conditional anion).

Titles complex substances composed according to chemical formulas from right to left. They are made up of two words - the names of electronegative components (in the nominative case) and electropositive components (in the genitive case), for example:

CuSO 4 - copper(II) sulfate
PCl 3 - phosphorus trichloride
LaCl 3 - lanthanum(III) chloride
CO - carbon monoxide

The number of electropositive and electronegative components in the names is indicated by the numerical prefixes given above (universal method), or by oxidation states (if they can be determined by the formula) using Roman numerals in parentheses (the plus sign is omitted). In some cases, the charge of ions is given (for cations and anions of complex composition), using Arabic numerals with the appropriate sign.

The following special names are used for common multielement cations and anions:

H 2 F + - fluoronium	C 2 2 - - acetylenide
H 3 O + - oxonium	CN - - cyanide
H 3 S + - sulfonium	CNO - - fulminate
NH 4 + - ammonium	HF 2 - - hydrodifluoride
N 2 H 5 + - hydrazinium(1+)	HO 2 - - hydroperoxide
N 2 H 6 + - hydrazinium(2+)	HS - - hydrosulfide
NH 3 OH + - hydroxylamine	N 3 - - azide
NO+ - nitrosyl	NCS - - thiocyanate
NO 2 + - nitroyl	O 2 2 - - peroxide
O 2 + - dioxygenyl	O 2 - - superoxide
PH 4 + - phosphonium	O 3 - - ozonide
VO 2+ - vanadyl	OCN - - cyanate
UO 2+ - uranyl	OH - - hydroxide

For a small number of well-known substances it is also used special titles:

1. Acidic and basic hydroxides. Salts

Hydroxides are a type of complex substances that contain atoms of some element E (except fluorine and oxygen) and hydroxyl groups OH; general formula of hydroxides E(OH) n, Where n= 1÷6. Form of hydroxides E(OH) n called ortho-shape; at n> 2 hydroxide can also be found in meta-form, which includes, in addition to E atoms and OH groups, oxygen atoms O, for example E(OH) 3 and EO(OH), E(OH) 4 and E(OH) 6 and EO 2 (OH) 2.

Hydroxides are divided into two groups with opposite chemical properties: acidic and basic hydroxides.

Acidic hydroxides contain hydrogen atoms, which can be replaced by metal atoms subject to the rule of stoichiometric valence. Most acid hydroxides are found in meta-form, and hydrogen atoms in the formulas of acidic hydroxides are given first place, for example, H 2 SO 4, HNO 3 and H 2 CO 3, and not SO 2 (OH) 2, NO 2 (OH) and CO (OH) 2. The general formula of acid hydroxides is H X EO at, where the electronegative component EO y x - called an acid residue. If not all hydrogen atoms are replaced by a metal, then they remain as part of the acid residue.

The names of common acid hydroxides consist of two words: the proper name with the ending “aya” and the group word “acid”. Here are the formulas and proper names of common acid hydroxides and their acidic residues (a dash means that the hydroxide is not known in free form or in an acidic aqueous solution):

acid hydroxide	acid residue
HAsO 2 - metaarsenic	AsO 2 - - metaarsenite
H 3 AsO 3 - orthoarsenic	AsO 3 3 - - orthoarsenite
H 3 AsO 4 - arsenic	AsO 4 3 - - arsenate
	B 4 O 7 2 - - tetraborate
	ВiО 3 - - bismuthate
HBrO - bromide	BrO - - hypobromite
HBrO 3 - brominated	BrO 3 - - bromate
H 2 CO 3 - coal	CO 3 2 - - carbonate
HClO - hypochlorous	ClO- - hypochlorite
HClO 2 - chloride	ClO2 - - chlorite
HClO 3 - chloric	ClO3 - - chlorate
HClO 4 - chlorine	ClO4 - - perchlorate
H 2 CrO 4 - chrome	CrO 4 2 - - chromate
	НCrO 4 - - hydrochromate
H 2 Cr 2 O 7 - dichromic	Cr 2 O 7 2 - - dichromate
	FeO 4 2 - - ferrate
HIO 3 - iodine	IO 3 - - iodate
HIO 4 - metaiodine	IO 4 - - metaperiodate
H 5 IO 6 - orthoiodine	IO 6 5 - - orthoperiodate
HMnO 4 - manganese	MnO4- - permanganate
	MnO 4 2 - - manganate
	MoO 4 2 - - molybdate
HNO 2 - nitrogenous	NO 2 - - nitrite
HNO 3 - nitrogen	NO 3 - - nitrate
HPO 3 - metaphosphoric	PO 3 - - metaphosphate
H 3 PO 4 - orthophosphoric	PO 4 3 - - orthophosphate
	НPO 4 2 - - hydroorthophosphate
	H 2 PO 4 - - dihydroothophosphate
H 4 P 2 O 7 - diphosphoric	P 2 O 7 4 - - diphosphate
	ReO 4 - - perrhenate
	SO 3 2 - - sulfite
	HSO 3 - - hydrosulfite
H 2 SO 4 - sulfuric	SO 4 2 - - sulfate
	HSO 4 - - hydrogen sulfate
H 2 S 2 O 7 - disulfur	S 2 O 7 2 - - disulfate
H 2 S 2 O 6 (O 2) - peroxodisulfur	S 2 O 6 (O 2) 2 - - peroxodisulfate
H 2 SO 3 S - thiosulfur	SO 3 S 2 - - thiosulfate
H 2 SeO 3 - selenium	SeO 3 2 - - selenite
H 2 SeO 4 - selenium	SeO 4 2 - - selenate
H 2 SiO 3 - metasilicon	SiO 3 2 - - metasilicate
H 4 SiO 4 - orthosilicon	SiO 4 4 - - orthosilicate
H 2 TeO 3 - telluric	TeO 3 2 - - tellurite
H 2 TeO 4 - metatelluric	TeO 4 2 - - metatellurate
H 6 TeO 6 - orthotelluric	TeO 6 6 - - orthotellurate
	VO 3 - - metavanadate
	VO 4 3 - - orthovanadate
	WO 4 3 - - tungstate

Less common acid hydroxides are named according to nomenclature rules for complex compounds, for example:

The names of acid residues are used to construct the names of salts.

Basic hydroxides contain hydroxide ions, which can be replaced by acidic residues subject to the rule of stoichiometric valency. All basic hydroxides are found in ortho-shape; their general formula is M(OH) n, Where n= 1.2 (less often 3.4) and M n+ is a metal cation. Examples of formulas and names of basic hydroxides:

The most important chemical property of basic and acidic hydroxides is their interaction with each other to form salts ( salt formation reaction), For example:

Ca(OH) 2 + H 2 SO 4 = CaSO 4 + 2H 2 O

Ca(OH) 2 + 2H 2 SO 4 = Ca(HSO 4) 2 + 2H 2 O

2Ca(OH)2 + H2SO4 = Ca2SO4(OH)2 + 2H2O

Salts are a type of complex substances that contain M cations n+ and acidic residues*.

Salts with general formula M X(EO at)n called average salts, and salts with unsubstituted hydrogen atoms - sour salts. Sometimes salts also contain hydroxide and/or oxide ions; such salts are called main salts. Here are examples and names of salts:

	Calcium orthophosphate
	Calcium dihydrogen orthophosphate
	Calcium hydrogen phosphate
	Copper(II) carbonate
Cu 2 CO 3 (OH) 2	Dicopper dihydroxide carbonate
	Lanthanum(III) nitrate
	Titanium oxide dinitrate

Acid and basic salts can be converted to middle salts by reaction with the appropriate basic and acidic hydroxide, for example:

Ca(HSO 4) 2 + Ca(OH) = CaSO 4 + 2H 2 O

Ca 2 SO 4 (OH) 2 + H 2 SO 4 = Ca 2 SO 4 + 2H 2 O

There are also salts containing two different cations: they are often called double salts, For example:

2. Acidic and basic oxides

Oxides E X ABOUT at- products of complete dehydration of hydroxides:

Acid hydroxides (H 2 SO 4, H 2 CO 3) acid oxides answer(SO 3, CO 2), and basic hydroxides (NaOH, Ca(OH) 2) - basicoxides(Na 2 O, CaO), and the oxidation state of element E does not change when moving from hydroxide to oxide. Example of formulas and names of oxides:

Acidic and basic oxides retain the salt-forming properties of the corresponding hydroxides when interacting with hydroxides of opposite properties or with each other:

N 2 O 5 + 2NaOH = 2NaNO 3 + H 2 O

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

La 2 O 3 + 3SO 3 = La 2 (SO 4) 3

3. Amphoteric oxides and hydroxides

Amphotericity hydroxides and oxides - a chemical property consisting in the formation of two rows of salts by them, for example, for aluminum hydroxide and aluminum oxide:

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

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

(b) 2Al(OH) 3 + Na 2 O = 2NaAlO 2 + 3H 2 O

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

Thus, aluminum hydroxide and oxide in reactions (a) exhibit the properties main hydroxides and oxides, i.e. react with acidic hydroxides and oxide, forming the corresponding salt - aluminum sulfate Al 2 (SO 4) 3, while in reactions (b) they also exhibit the properties acidic hydroxides and oxides, i.e. react with basic hydroxide and oxide, forming a salt - sodium dioxoaluminate (III) NaAlO 2. In the first case, the element aluminum exhibits the property of a metal and is part of the electropositive component (Al 3+), in the second - the property of a non-metal and is part of the electronegative component of the salt formula (AlO 2 -).

If these reactions occur in an aqueous solution, then the composition of the resulting salts changes, but the presence of aluminum in the cation and anion remains:

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

Al(OH) 3 + NaOH = Na

Here, complex ions 3+ - hexaaqualuminium(III) cation, - - tetrahydroxoaluminate(III) ion are highlighted in square brackets.

Elements that exhibit metallic and non-metallic properties in compounds are called amphoteric, these include elements of the A-groups of the Periodic Table - Be, Al, Ga, Ge, Sn, Pb, Sb, Bi, Po, etc., as well as most elements of the B- groups - Cr, Mn, Fe, Zn, Cd, Au, etc. Amphoteric oxides are called the same as basic ones, for example:

Amphoteric hydroxides (if the oxidation state of the element exceeds + II) can be found in ortho- or (and) meta- form. Here are examples of amphoteric hydroxides:

Amphoteric oxides do not always correspond to amphoteric hydroxides, since when trying to obtain the latter, hydrated oxides are formed, for example:

If an amphoteric element in a compound has several oxidation states, then the amphotericity of the corresponding oxides and hydroxides (and, consequently, the amphotericity of the element itself) will be expressed differently. For low oxidation states, hydroxides and oxides have a predominance of basic properties, and the element itself has metallic properties, so it is almost always included in the composition of cations. For high oxidation states, on the contrary, hydroxides and oxides have a predominance acidic properties, and the element itself has non-metallic properties, so it is almost always included in the composition of anions. Thus, manganese(II) oxide and hydroxide have dominant basic properties, and manganese itself is part of cations of the 2+ type, while manganese(VII) oxide and hydroxide have dominant acidic properties, and manganese itself is part of the MnO 4 - type anion. . Amphoteric hydroxides with a high predominance of acidic properties are assigned formulas and names modeled after acidic hydroxides, for example HMn VII O 4 - manganese acid.

Thus, the division of elements into metals and non-metals is conditional; Between the elements (Na, K, Ca, Ba, etc.) with purely metallic properties and the elements (F, O, N, Cl, S, C, etc.) with purely non-metallic properties, there is a large group of elements with amphoteric properties.

4. Binary compounds

A broad type of inorganic complex substances are binary compounds. These include, first of all, all two-element compounds (except for basic, acidic and amphoteric oxides), for example H 2 O, KBr, H 2 S, Cs 2 (S 2), N 2 O, NH 3, HN 3, CaC 2 , SiH 4 . The electropositive and electronegative components of the formulas of these compounds include individual atoms or bonded groups of atoms of the same element.

Multielement substances, in the formulas of which one of the components contains unrelated atoms of several elements, as well as single-element or multi-element groups of atoms (except hydroxides and salts), are considered as binary compounds, for example CSO, IO 2 F 3, SBrO 2 F, CrO (O2)2, PSI3, (CaTi)O3, (FeCu)S2, Hg(CN)2, (PF3)2O, VCl2 (NH2). Thus, CSO can be represented as a CS 2 compound in which one sulfur atom is replaced by an oxygen atom.

The names of binary compounds are constructed according to the usual nomenclature rules, for example:

OF 2 - oxygen difluoride	K 2 O 2 - potassium peroxide
HgCl 2 - mercury(II) chloride	Na 2 S - sodium sulfide
Hg 2 Cl 2 - dimercury dichloride	Mg 3 N 2 - magnesium nitride
SBr 2 O - sulfur oxide-dibromide	NH 4 Br - ammonium bromide
N 2 O - dinitrogen oxide	Pb(N 3) 2 - lead(II) azide
NO 2 - nitrogen dioxide	CaC 2 - calcium acetylenide

For some binary compounds, special names are used, a list of which was given earlier.

The chemical properties of binary compounds are quite diverse, so they are often divided into groups by the name of anions, i.e. halides, chalcogenides, nitrides, carbides, hydrides, etc. are considered separately. Among binary compounds there are also those that have some characteristics of other types of inorganic substances. Thus, the compounds CO, NO, NO 2, and (Fe II Fe 2 III) O 4, the names of which are constructed using the word oxide, cannot be classified as oxides (acidic, basic, amphoteric). Carbon monoxide CO, nitrogen monoxide NO and nitrogen dioxide NO 2 do not have corresponding acid hydroxides (although these oxides are formed by non-metals C and N), nor do they form salts whose anions would include atoms C II, N II and N IV. Double oxide (Fe II Fe 2 III) O 4 - diiron(III)-iron(II) oxide, although it contains atoms of the amphoteric element - iron in the electropositive component, but in two different oxidation states, as a result of which, when interacting with acid hydroxides, it forms not one, but two different salts.

Binary compounds such as AgF, KBr, Na 2 S, Ba(HS) 2, NaCN, NH 4 Cl, and Pb(N 3) 2 are built, like salts, from real cations and anions, which is why they are called salt-like binary compounds (or simply salts). They can be considered as products of the substitution of hydrogen atoms in the compounds HF, HCl, HBr, H 2 S, HCN and HN 3. The latter in an aqueous solution have an acidic function, and therefore their solutions are called acids, for example HF (aqua) - hydrofluoric acid, H 2 S (aqua) - hydrosulfide acid. However, they do not belong to the type of acid hydroxides, and their derivatives do not belong to the salts within the classification of inorganic substances.

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 hydroxy 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 – id- 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 the 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 - dihydroorthophosphate 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 hemicoxide,

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 color of the solution 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)Preparation of 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) Receipt 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 obtain 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 interaction

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	Orthoarsenical	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

Currently, chemists know more than 20 million chemical compounds. Obviously, not a single person is able to remember the names of tens of millions of substances.

That is why the International Union of Pure and Applied Chemistry developed systematic nomenclature organic and inorganic compounds. A system of rules has been constructed that allows naming oxides, acids, salts, complex compounds, organic matter etc. Systematic names have a clear, unambiguous meaning. For example, magnesium oxide is MgO, potassium sulfate is CaSO 4, chloromethane is CH 3 Cl, etc.

The chemist who discovers a new compound does not choose its name himself, but is guided by clear IUPAC rules. Any of his colleagues working in any country in the world will be able to quickly construct a formula for a new substance based on its name.

The systematic nomenclature is convenient, rational and accepted throughout the world. There is, however, a small group of compounds for which the “correct” nomenclature is practically not used. The names of some substances have been used by chemists for decades and even centuries. These trivial names more convenient, more familiar, and so firmly ingrained in consciousness that practitioners do not want to change them to systematic ones. In fact, even IUPAC rules allow the use of trivial names.

Not a single chemist will name the substance CuSO 4 5H 2 O copper(II) sulfate pentahydrate. It is much easier to use the trivial name for this salt: copper sulfate. No one will ask a colleague: “Tell me, do you have any potassium hexacyanoferrate (III) left in your laboratory?” But you can even break your tongue! They will ask differently: “Is there any red blood salt left?”

Short, convenient and familiar. Unfortunately, trivial names of substances do not obey any modern rules. You just need to remember them. Yes, yes, the chemist must remember that FeS 2 is pyrite, and under the familiar term “chalk” lies calcium carbonate.

The table below lists some of the most common trivial names for salts, oxides, acids, bases, etc. Please note that one substance can have multiple trivial names. For example, sodium chloride (NaCl) can be called halite, Can i - rock salt.

Trivial name	Substance formula	Systematic name
diamond	WITH	carbon
potassium alum	KAl(SO 4) 2 12H 2 O	Aluminum Potassium Sulfate Dodecahydrate
anhydrite	CaSO4	calcium sulfate
barite	BaSO4	barium sulfate
Prussian blue	Fe 4 3	iron(III) hexacyanoferrate(II)
bischofite	MgCl 2 6H 2 O	magnesium chloride hexahydrate
borazon	BN	boron nitride
borax	Na 2 B 4 O 7 10H 2 O	sodium tetraborate decahydrate
water gas	CO+H2	hydrogen + carbon monoxide (II)
galena	PbS	lead(II) sulfide
halite	NaCl	sodium chloride
slaked lime	Ca(OH)2	calcium hydroxide
hematite	Fe2O3	iron(III) oxide
gypsum	CaSO 4 2H 2 O	calcium sulfate dihydrate
alumina	Al2O3	aluminium oxide
Glauber's salt	Na 2 SO 4 10H 2 O	sodium sulfate decahydrate
graphite	WITH	carbon
sodium hydroxide	NaOH	sodium hydroxide
caustic potassium	KOH	potassium hydroxide
iron pyrite	FeS 2	iron disulfide
inkstone	FeSO 4 7H 2 O	iron(II) sulfate heptahydrate
yellow blood salt	K 4	Potassium hexacyanoferrate(II)
liquid glass	Na 2 SiO 3	sodium silicate
lime water	solution of Ca(OH) 2 in water	calcium hydroxide solution in water
limestone	CaCO3	calcium carbonate
calomel	Hg2Cl2	Dimercury dichloride
rock salt	NaCl	sodium chloride
cinnabar	HgS	mercury(II) sulfide
corundum	Al2O3	aluminium oxide
red blood salt	K 3	Potassium hexacyanoferrate(III)
hematite	Fe2O3	iron(III) oxide
cryolite	Na 3	sodium hexafluoroaluminate
lapis	AgNO3	silver nitrate
magnesite	MgCO 3	magnesium carbonate
magnetite	Fe3O4
magnetic iron ore	Fe3O4	Diiron(III)-iron(II) oxide
malachite	Cu 2 (OH) 2 CO 3	hydroxycopper(II) carbonate
copper shine	Cu2S	copper(I) sulfide
copper sulfate	CuSO 4 5H 2 O	copper(II) sulfate pentahydrate
chalk	CaCO3	calcium carbonate
marble	CaCO3	calcium carbonate
ammonia	aqueous solution NH 3	ammonia solution in water
ammonia	NH4Cl	ammonium chloride
quicklime	CaO	calcium oxide
sodium nitroprusside	Na 2	sodium penatcyanonitrosylium ferrate(II)
oleum	solution of SO 3 in H 2 SO 4	solution of sulfur oxide (VI) in conc. sulfuric acid
hydrogen peroxide	H2O2	hydrogen peroxide
pyrite	FeS 2	iron disulfide
pyrolusite	MnO2	manganese dioxide
hydrofluoric acid	HF	hydrofluoric acid
potash	K 2 CO 3	potassium carbonate
Nessler's reagent	K2	alkaline solution of potassium tetraiodomercurate (II)
rhodochrosite	MnCO3	manganese(II) carbonate
rutile	TiO2	titanium dioxide
galena	PbS	lead(II) sulfide
red lead	Pb 3 O 4	dislead(III) oxide - lead(II)
ammonium nitrate	NH4NO3	ammonium nitrate
potassium nitrate	KNO 3	potassium nitrate
calcium nitrate	Ca(NO3)2	calcium nitrate
soda nitrate	NaNO3	sodium nitrate
Chilean saltpeter	NaNO3	sodium nitrate
sulfur pyrite	FeS 2	iron disulfide
sylvin	KCl	potassium chloride
siderite	FeCO3	iron(II) carbonate
smithsonite	ZnCO3	zinc carbonate
soda ash	Na 2 CO 3	sodium carbonate
caustic soda	NaOH	sodium hydroxide
baking soda	NaHCO3	sodium bicarbonate
Mohr's salt	(NH 4) 2 Fe(SO 4) 2 6H 2 O	ammonium iron(II) sulfate hexahydrate
corrosive sublimate	HgCl2	mercury(II) chloride
dry ice	CO 2 (solid)	carbon dioxide (solid)
sphalerite	ZnS	zinc sulfide
carbon monoxide	CO	carbon(II) monoxide
carbon dioxide	CO2	carbon(IV) monoxide
fluorite	CaF2	calcium fluoride
chalcocite	Cu2S	copper(I) sulfide
bleaching powder	mixture of CaCl 2, Ca(ClO) 2 and Ca(OH) 2	mixture of calcium chloride, calcium hypochlorite and calcium hydroxide
chromium-potassium alum	KCr(SO 4) 2 12H 2 O	chromium(III)-potassium sulfate dodecahydrate
aqua regia	mixture of HCl and HNO 3	a mixture of concentrated solutions of hydrochloric and nitric acids in a volume ratio of 3:1
zinc blende	ZnS	zinc sulfide
zinc sulfate	ZnSO 4 7H 2 O	zinc sulfate heptahydrate

Note: Natural minerals are composed of several substances. For example, silver compounds can be found in lead glitter. The table, of course, indicates only the main substance.

Substances of the form X n H 2 O are called crystalline hydrates. They include the so-called. "crystallization" water. For example, we can say that copper (II) sulfate crystallizes from aqueous solutions with 5 water molecules. We obtain copper (II) sulfate pentahydrate (the trivial name is copper sulfate).

If you are interested in systematic names, I recommend turning to the section "

TRIVIAL NAMES OF SUBSTANCES. For many centuries and millennia, people have used a wide variety of substances in their practical activities. Quite a few of them are mentioned in the Bible (these include precious stones, dyes, and various incense). Of course, each of them was given a name. Of course, it had nothing to do with the composition of the substance. Sometimes the name reflected an appearance or a special property, real or fictitious. A typical example is a diamond. In Greek damasma - subjugation, taming, damao - crushing; accordingly, adamas means indestructible (it’s interesting that in Arabic “al-mas” means the hardest, the hardest). In ancient times, miraculous properties were attributed to this stone, for example, this: if you put a diamond crystal between a hammer and an anvil, they would sooner shatter into pieces than the “king of stones” would be damaged. In fact, diamond is very fragile and cannot withstand impacts at all. But the word “diamond” actually reflects the property of a cut diamond: in French brilliant means brilliant.

Alchemists came up with many names for substances. Some of them have survived to this day. Thus, the name of the element zinc (it was introduced into the Russian language by M.V. Lomonosov) probably comes from the ancient German tinka - “white”; Indeed, the most common zinc preparation, ZnO oxide, is white. At the same time, alchemists came up with many of the most fantastic names - partly due to their philosophical views, partly - to classify the results of their experiments. For example, they called the same zinc oxide “philosophical wool” (alchemists obtained this substance in the form of a loose powder). Other names were based on how the substance was obtained. For example, methyl alcohol was called wood alcohol, and calcium acetate was called “burnt wood salt” (to obtain both substances, dry distillation of wood was used, which, of course, led to its charring - “burning”). Very often the same substance received several names. For example, even by the end of the 18th century. there were four names for copper sulfate, ten for copper carbonate, and twelve for carbon dioxide!

The description of chemical procedures was also ambiguous. Thus, in the works of M.V. Lomonosov one can find references to “dissolved scum,” which may confuse the modern reader (although cookbooks sometimes contain recipes that require “dissolving a kilogram of sugar in a liter of water,” and “scum” simply means "sediment")

Currently, the names of substances are regulated by the rules of chemical nomenclature (from the Latin nomenclatura - list of names). In chemistry, nomenclature is a system of rules, using which you can give each substance a “name” and, conversely, knowing the “name” of the substance, write down its chemical formula. Developing a unified, unambiguous, simple and convenient nomenclature is not an easy task: suffice it to say that even today there is no complete unity among chemists on this matter. Issues of nomenclature are dealt with by a special commission of the International Union of Pure and Applied Chemistry - IUPAC (according to the initial letters of the English name International Union of Pure and Applied Chemistry). And national commissions develop rules for applying IUPAC recommendations to the language of their country. Thus, in the Russian language, the ancient term “oxide” was replaced by the international “oxide”, which was also reflected in school textbooks.

Anecdotal stories are also associated with the development of a system of national names for chemical compounds. For example, in 1870, the commission on chemical nomenclature of the Russian Physicochemical Society discussed the proposal of one chemist to name compounds according to the same principle by which first names, patronymics and surnames are built in the Russian language. For example: Potassium Khlorovich (KCl), Potassium Khlorovich Trikislov (KClO 3), Chlorine Vodorodovich (HCl), Hydrogen Kislorodovich (H 2 O). After a long debate, the commission decided to postpone discussion of this issue until January, without specifying what year. Since then, the commission has not returned to this issue.

Modern chemical nomenclature is more than two centuries old. In 1787, the famous French chemist Antoine Laurent Lavoisier presented the results of the work of the commission he headed to create a new chemical nomenclature to the Academy of Sciences in Paris. In accordance with the proposals of the commission, new names were given chemical elements, as well as complex substances, taking into account their composition. The names of the elements were selected so that they reflected the features of their chemical properties. Thus, the element that Priestley previously called “dephlogisticated air”, Scheele - “fiery air”, and Lavoisier himself - “vital air”, according to the new nomenclature, received the name oxygen (at that time it was believed that acids necessarily included this element). Acids are named after their corresponding elements; as a result, “nitrate fumed acid” turned into nitric acid, and “oil of vitriol” into sulfuric acid. To designate salts, the names of acids and corresponding metals (or ammonium) began to be used.

The adoption of a new chemical nomenclature made it possible to systematize extensive factual material and greatly facilitated the study of chemistry. Despite all the changes, the basic principles laid down by Lavoisier have been preserved to this day. Nevertheless, among chemists, and especially among laymen, many so-called trivial (from Latin trivialis - ordinary) names have been preserved, which are sometimes used incorrectly. For example, a person who feels unwell is offered to “smell ammonia.” For a chemist, this is nonsense, since ammonia (ammonium chloride) is an odorless salt. In this case, ammonia is confused with ammonia, which really has a pungent odor and stimulates the respiratory center.

A lot of trivial names for chemical compounds are still used by artists, technologists, and builders (ochre, mummy, red lead, cinnabar, litharge, fluff, etc.). Even more trivial names among medicines. In reference books you can find up to a dozen or more different synonyms for the same drug, which is mainly associated with brand names adopted in different countries(for example, domestic piracetam and imported nootropil, Hungarian Seduxen and Polish Relanium, etc.).

Chemists also often use trivial names for substances, sometimes quite interesting ones. For example, 1,2,4,5-tetramethylbenzene has the trivial name "durol", and 1,2,3,5-tetramethylbenzene - "isodurol". A trivial name is much more convenient if it is obvious to everyone what we are talking about. For example, even a chemist will never call ordinary sugar “alpha-D-glucopyranosyl-beta-D-fructofuranoside”, but uses the trivial name for this substance - sucrose. And even in inorganic chemistry, the systematic, strictly nomenclature, name of many compounds can be cumbersome and inconvenient, for example: O 2 - dioxygen, O 3 - trioxygen, P 4 O 10 - tetraphosphorus decaoxide, H 3 PO 4 - tetraoxophosphate (V) of hydrogen , BaSO 3 – barium trioxosulfate, Cs 2 Fe(SO 4) 2 – iron(II)-dicesium tetraoxosulfate(VI), etc. And although the systematic name fully reflects the composition of the substance, in practice trivial names are used: ozone, phosphoric acid, etc.

Among chemists, the names of many compounds are also common, especially complex salts, such as Zeise's salt K.H 2 O - named after the Danish chemist William Zeise. Such short names are very convenient. For example, instead of “potassium nitrodisulfonate” the chemist will say “Fremy’s salt”, instead of “crystalline hydrate of double ammonium iron(II) sulfate” - Mohr’s salt, etc.

The table shows the most common trivial (everyday) names of some chemical compounds, with the exception of highly specialized, outdated, medical terms, and names of minerals, as well as their traditional chemical names.

Table 1. TRIVIAL (HOUSEHOLD) NAMES OF SOME CHEMICAL COMPOUNDS
Trivial name	Chemical name	Formula
Alabaster	Calcium sulfate hydrate (2/1)	2CaSO4 . H2O
Anhydrite	Calcium sulfate	CaSO4
Orpiment	Arsenic sulfide	As 2 S 3
White lead	Basic lead carbonate	2PbCO3 . Pb(OH)2
Titanium white	Titanium(IV) oxide	TiO2
Zinc whitewash	Zinc oxide	ZnO
Prussian blue	Iron(III)-potassium hexacyanoferrate(II)	KFe
Bertholet's salt	Potassium chlorate	KClO3
Marsh gas	Methane	CH 4
Borax	Sodium tetraborate tetrahydrate	Na2B4O7 . 10H2O
Laughing gas	Nitric oxide(I)	N2O
Hyposulfite (photo)	Sodium thiosulfate pentahydrate	Na2S2O3 . 5H 2 O
Glauber's salt	Sodium sulfate decahydrate	Na2SO4 . 10H2O
Lead litharge	Lead(II) oxide	PbO
Alumina	Aluminium oxide	Al2O3
Epsom salt	Magnesium sulfate heptahydrate	MgSO4 . 7H2O
Caustic soda (caustic)	Sodium hydroxide	NaOH
Caustic potassium	Potassium hydroxide	CON
Yellow blood salt	Potassium hexacyanoferrate(III) trihydrate	K4Fe(CN)6 . 3H2O
Cadmium yellow	Cadmium sulfide	CdS
Magnesia	Magnesium oxide	MgO
Slaked lime (fluff)	Calcium hydroxide	Ca(OH) 2
Burnt lime (quicklime, boiling water)	Calcium oxide	Sao
Calomel	Mercury(I) chloride	Hg2Cl2
Carborundum	Silicon carbide	SiC
Alum	Dodecahydrates of double sulfates of 3- and 1-valent metals or ammonium (for example, potassium alum)	M I M III (SO 4) 2 . 12H 2 O (M I – Na, K, Rb, Cs, Tl, NH 4 cations; M III – Al, Ga, In, Tl, Ti, V, Cr, Fe, Co, Mn, Rh, Ir cations)
Cinnabar	Mercury sulfide	HgS
Red blood salt	Potassium hexacyanoferrate(II)	K 3 Fe(CN) 6
Silica	Silicon oxide	SiO2
Vitriol oil (battery acid)	Sulfuric acid	H 2 SO4
Vitriol	Crystal hydrates of sulfates of a number of divalent metals	M II SO 4 . 7H 2 O (M II – Fe, Co, Ni, Zn, Mn cations)
Lapis	Silver nitrate	AgNO3
Urea	Urea	CO(NH 2) 2
Ammonia	Aqueous ammonia solution	NH 3 . x H2O
Ammonia	Ammonium chloride	NH4Cl
Oleum	A solution of sulfur(III) oxide in sulfuric acid	H2SO4 . x SO 3
Perhydrol	30% aqueous hydrogen peroxide solution	H 2 O 2
Hydrofluoric acid	Aqueous hydrogen fluoride solution	HF
Table (rock) salt	Sodium chloride	NaCl
Potash	Potassium carbonate	K 2 CO 3
Soluble glass	Sodium silicate nonahydrate	Na 2 SiO 3 . 9H2O
Lead sugar	Lead acetate trihydrate	Pb(CH3COO)2 . 3H2O
Seignet salt	Potassium sodium tartrate tetrahydrate	KNaC4H4O6 . 4H2O
Ammonium nitrate	Ammonium nitrate	NH4NO3
Potassium nitrate (Indian)	Potassium nitrate	KNO 3
Norwegian saltpeter	Calcium nitrate	Ca(NO3)2
Chilean saltpeter	Sodium nitrate	NaNO3
Sulfur liver	Sodium polysulfides	Na2S x
Sulphur dioxide	Sulfur(IV) oxide	SO 2
Sulfuric anhydride	Sulfur(VI) oxide	SO 3
Sulfur color	Fine sulfur powder	S
Silica gel	Dried silicic acid gel	SiO2 . x H2O
Hydrocyanic acid	Hydrogen cyanide	HCN
Soda ash	Sodium carbonate	Na 2 CO 3
Caustic soda (see Caustic soda)
Drinking soda	Sodium bicarbonate	NaHCO3
Foil	Tin foil	Sn
Corrosive sublimate	Mercury(II) chloride	HgCl2
Double superphosphate	Calcium Dihydrogen Phosphate Hydrate	Ca(H 2 PO 4) 2 . H 2 O
Simple superphosphate	The same mixed with CaSO 4
Gold leaf	Tin(IV) sulfide or gold foil	SnS2, Au
Lead minium	Lead(IV) oxide - dislead(II)	Pb 3 O 4 (Pb 2 II Pb IV O 4)
Iron minium	Diiron(III)-iron(II) oxide	Fe 3 O 4 (Fe II Fe 2 III) O 4
Dry ice	Solid carbon monoxide(IV)	CO2
Bleaching powder	Mixed chloride-calcium hypochlorite	Ca(OCl)Cl
Carbon monoxide	Carbon(II) monoxide	CO
Carbon dioxide	Carbon monoxide	CO 2
Phosgene	Carbonyl dichloride	COCl2
Chrome green	Chromium(III) oxide	Cr2O3
Chrompic (potassium)	Potassium dichromate	K2Cr2O7
verdigris	Basic copper acetate	Cu(OH)2 . x Cu(CH3COO)2

Ilya Leenson