LECTURE TOPIC: amines and amino alcohols
Questions:
general characteristics Keywords: structure, classification, nomenclature.
Acquisition Methods
Chemical properties
individual representatives. Identification methods.
General characteristics: structure, classification, nomenclature
Amines are called derivatives of ammonia, the molecule of which hydrogen atoms are replaced by hydrocarbon radicals.
Classification
1– Depending on the number of substituted hydrogen atoms of ammonia, amines are distinguished:
– primary contain an amino group an amino group (–NH 2), general formula: R–NH 2,
– secondary contain an imino group (–NH),
general formula: R 1 -NH - R 2
– tertiary contain a nitrogen atom, the general formula: R 3 -N
There are also known compounds with a quaternary nitrogen atom: quaternary ammonium hydroxide and its salts.
2– Depending on the structure of the radical, amines are distinguished:
– aliphatic (limiting and unsaturated)
– alicyclic
- aromatic (containing an amino group or side chain in the core)
- heterocyclic.
Nomenclature, amine isomerism
1. The names of amines according to rational nomenclature are usually derived from the names of their constituent hydrocarbon radicals with the addition of the ending -amine : methylamine CH 3 -NH 2, dimethylamine CH 3 -NH-CH 3, trimethylamine (CH 3) 3 N, propylamine CH 3 CH 2 CH 2 -NH 2, phenylamine C 6 H 5 - NH 2, etc.
2. According to the IUPAC nomenclature, the amino group is considered as a functional group and its name amino put before the name of the main chain:
The isomerism of amines depends on the isomerism of radicals.
Methods for obtaining amines
Amines can be obtained in various ways.
A) Action on ammonia by haloalkyls
2NH 3 + CH 3 I -–® CH 3 - NH 2 + NH 4 I
B) Catalytic hydrogenation of nitrobenzene with molecular hydrogen:
C 6 H 5 NO 2 -–® C 6 H 5 NH 2 + H 2 O
nitrobenzene cat aniline
C) Obtaining lower amines (С 1 -С 4) by alkylation with alcohols:
350 0 C, Al 2 O 3
R–OH + NH 3 –––––––––––® R–NH 2 +H 2 O
350 0 C, Al 2 O 3
2R–OH + NH 3 –––––––––––® R 2 –NH +2H 2 O
350 0 C, Al 2 O 3
3R–OH + NH 3 –––––––––––® R 3 –N + 3H 2 O
Physical properties of amines
Methylamine, dimethylamine and trimethylamine are gases, the middle members of the amine series are liquids, the higher ones are solid bodies. With the increase molecular weight amines, their density increases, the boiling point rises and the solubility in water decreases. Higher amines are insoluble in water. Lower amines have an unpleasant odor, somewhat reminiscent of the smell of spoiled fish. Higher amines are either odorless or have a very low odor. Aromatic amines are colorless liquids or solids, which have an unpleasant odor and are poisonous.
Chemical properties of amines
The chemical behavior of amines is determined by the presence of an amino group in the molecule. On the outside electron shell The nitrogen atom has 5 electrons. In the amine molecule, as well as in the ammonia molecule, the nitrogen atom spends three electrons on the formation of three covalent bonds, and two remain free.
The presence of a free electron pair at the nitrogen atom makes it possible for it to attach a proton, therefore amines are similar to ammonia, exhibit basic properties, form hydroxides, salts.
Salt formation. Amines with acids give salts, which, under the action of a strong base, again give free amines:
Amines give salts even with weak carbonic acid:
Like ammonia, amines have basic properties due to the binding of protons into a weakly dissociating substituted ammonium cation:
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When an amine is dissolved in water, part of the water protons is spent on the formation of a cation; thus, an excess of hydroxide ions appears in the solution, and it has alkaline properties sufficient to color litmus solutions in blue color and phenolphthalein to raspberry. The basicity of amines of the limiting series varies within very small limits and is close to the basicity of ammonia.
The effect of methyl groups slightly increases the basicity of methyl- and dimethylamine. In the case of trimethylamine, the methyl groups already impede the solvation of the resulting cation and reduce its stabilization and, consequently, its basicity.
Amine salts should be considered as complex compounds. The central atom in them is a nitrogen atom, the coordination number of which is four. Hydrogen atoms or alkyls are bonded to the nitrogen atom and are located in the inner sphere; the acid residue is located in the outer sphere.
Acylation of amines. Under the action of some derivatives of organic acids (acid halides, anhydrides, etc.) on primary and secondary amines, amides are formed:
Secondary amines with nitrous acid give nitrosamines- yellowish liquids, slightly soluble in water:
Tertiary amines are resistant to the action of dilute nitrous acid in the cold (they form salts of nitrous acid), under more severe conditions one of the radicals is cleaved off and nitrosoamine is formed.
Diamines
Diamines play an important role in biological processes. As a rule, they are easily soluble in water, have a characteristic odor, have a strong alkaline reaction, interact with CO 2 air. Diamines form stable salts with two equivalents of acid.
Ethylenediamine (1,2-ethanediamine) H 2 NCH 2 CH 2 NH 2 . It is the simplest diamine; can be obtained by the action of ammonia on ethylene bromide:
Tetramethylenediamine (1,4-butanediamine), or putrescine, NH 2 CH 2 CH 2 CH 2 CH 2 NH 2 and pentamethylenediamine (1,5-pentanediamine) NH 2 CH 2 CH 2 CH 2 CH 2 CH 2 NH 2, or cadaverine. They were discovered in the decomposition products of protein substances; are formed during the decarboxylation of diamino acids and are named ptomains(from Greek - corpse), they were previously considered "cadaveric poisons." It has now been found that the toxicity of rotting proteins is not caused by ptomaines, but by the presence of other substances.
Putrescine and cadaverine are formed as a result of the vital activity of many microorganisms (for example, causative agents of tetanus and cholera) and fungi; they are found in cheese, ergot, fly agaric, brewer's yeast.
Some diamines are used as raw materials for the production of polyamide fibers and plastics. So, from hexamethylenediamine NH 2 CH 2 CH 2 CH 2 CH 2 CH 2 CH 2 NH 2, a very valuable synthetic fiber was obtained - nylon(US) or anid(Russia).
Amino alcohols
Amino alcohols- compounds with mixed functions, the molecule of which contains amino and hydroxy groups.
Aminoethanol(ethanolamine) HO-CH 2 CH 2 -NH 2, or colamine.
Ethanolamine is a thick oily liquid, miscible with water in all respects, and has strong alkaline properties. Along with monoethanolamine, diethanolamine and triethanolamine are also obtained:
Choline is part of lecithins- fat-like substances, very common in animal and plant organisms, and can be isolated from them. Choline is a crystalline, highly hygroscopic mass that easily deflates in air. It has strong alkaline properties and readily forms salts with acids.
When choline is acylated with acetic anhydride, choline acetate, also called acetylcholine:
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Acetylcholine plays an extremely important biochemical role, as it is a mediator (intermediary) that transmits excitation from nerve receptors to muscles.
N, e.g. CH 3 NH 2 -methylamine, CH 3 NHC 3 H 7 - methylpropylamine, (C 2 H 5) 3 N -. Names formed by adding the prefix "", "", etc. are also used. to the generic designation, for example, a compound of the type C 2 H 5 CH (NH 2) CH 2 CH 3 - 3-aminopentane. Many aromatic have trivial names, eg. C 6 H 5 NH 2 -, CH 3 C 6 H 4 NH 2 - and CH 3 OS 6 H 4 NH 2 - (respectively from "" and from ""). Higher aliphatic normal structure sometimes called. by the names of the radicals fatty to-t, from which were synthesized, for example. , trilaurylamine.
In the IR spectra, the characteristic stretching vibrations of NH bonds in p-re are observed for primary alkylamines in the regions of 3380-3400 cm -1 and 3320-3340 cm -1; for primary aromatics. - two absorption bands in the region of 3500-3300 cm -1 (due to symmetric and asymmetric stretching vibrations N-H bonds); for aliphatic and aromatic. secondary amiov-one band resp. in the region of 3360-3310 cm -1 and in the region of 3500-3300 cm -1 ; tertiaries do not absorb in this region. In the spectra of chem. the shift is 1-5 ppm. Aliphatic in the UV and visible regions do not absorb, aromatic. in the UV spectra they have two absorption bands due to -transitions.
When loading with carboxylic acids, their, anhydride chlorides or primary and secondary are acylated to form N-substituted amides, for example: RNH 2 + CH 3 COOH -> RNHCOCH 3 + H 2 O. react under mild conditions, even easier -, to-rymi spend in the presence. , binding formed in the district of HC1. When with dicarboxylic acids, their esters or are formed. Acylated ones have weak basic sv-you.
Under the action of HNO 2 aliphatic. the primary ones are converted into with the release of N 2 and H 2 O, the secondary ones are converted into N-nitrosamines R 2 NNO. Tertiary at normal t-re with HNO 2 do not react. R-tion with HNO 2 is used for aliphatic. . When interacting primary aromatics. with HNO 2 in an acidic environment are formed: ArNH 2 + HNO 2 + HC1 -> ArCl - + 2H 2 O. Under the same conditions, secondary aromatic. turn into N-nitrosamines, tertiary - into para-nitroso derivatives. Primary alicyclic. with HNO 2 they form, which is often accompanied by a narrowing or expansion of the cycle (see).
Aliphatic primary and secondary interactions. with C1 2 or Br 2, forming N-halogenated. Primary with COC1 2 form RNCO or disubstituted (RNH) 2 CO, secondary - tetrasubstituted R 2 NCONR 2 . Primary easy interaction. with , giving azomethines (), e.g.:
When interacting with primary and secondary, hydroxyethyl derivatives are formed, for example: C 6 H 5 NH 2 + C1CH 2 CH 2 OH -> C 6 H 5 NHCH 2 CH 2 OH + HCl. More often for the synthesis of the same Comm. apply, lesko reacting with in the presence. small quantities of H 2 O: 
When used instead of NH 3 primary or secondary, secondary and (or) tertiary are obtained. This method () is common for the production of N-alkyl- and N, N-dialkylanilines. A similar method for obtaining interaction has been developed. with NH3. They react very easily with NH 3, forming (see).
5. R-tion of amides aliphatic. and aromatic. carbon kit with alkaline solutions of C1 2, Br 2 or I 2 with the formation of primary. In this case, the carbon chain is shortened by one ().
6. R-tion with the participation of alkyl- and aryl halides. K with alkyl halides with last. (see) get pure primary aliphatic: 
Aryl halides react with NH 3 and with difficulty, so in the industry they use Comm., in which it is activated by strong electron-withdrawing substituents, most often nitro or sulfo groups. In this way, dec.
The classification of amines is diverse and is determined by what feature of the structure is taken as the basis.
Depending on the number organic groups associated with the nitrogen atom, there are:
primary amines - one organic group at the nitrogen RNH 2
secondary amines - two organic groups at the nitrogen R 2 NH, organic groups can be different R "R" NH
tertiary amines - three organic groups at nitrogen R 3 N or R "R" R "" N
According to the type of organic group associated with nitrogen, aliphatic CH 3 - N6H 5 - N are distinguished
According to the number of amino groups in the molecule, amines are divided into monoamines CH 3 - NH 2, diamines H 2 N (CH 2) 2 NH 2, triamines, etc.
Amine nomenclature.
the word “amine” is added to the name of the organic groups associated with nitrogen, while the groups are mentioned in alphabetical order, for example, CH 3 NHC 3 H 7 - methylpropylamine, CH 3 N (C 6 H 5) 2 - methyldiphenylamine. The rules also allow the name to be composed based on a hydrocarbon in which the amino group is considered as a substituent. In this case, its position is indicated using a numerical index: C 5 H 3 C 4 H 2 C 3 H (NH 2) C 2 H 2 C 1 H 3 - 3-aminopentane (the blue upper numerical indices indicate the numbering order of C atoms) . For some amines, trivial (simplified) names have been preserved: C 6 H 5 NH 2 - aniline (the name according to the rules of nomenclature is phenylamine).
In some cases, established names are used, which are distorted correct names: H 2 NCH 2 CH 2 OH - monoethanolamine (correctly - 2-aminoethanol); (OHCH 2 CH 2) 2 NH - diethanolamine, the correct name is bis (2-hydroxyethyl) amine. Trivial, distorted and systematic (composed according to the rules of nomenclature) names quite often coexist in chemistry.
Physical properties of amines.
The first representatives of the amine series - methylamine CH 3 NH 2, dimethylamine (CH 3) 2 NH, trimethylamine (CH 3) 3 N and ethylamine C 2 H 5 NH 2 - are gaseous at room temperature, then with an increase in the number of atoms in R, amines become liquids , and as the chain length R increases to 10 C atoms, crystalline substances. The solubility of amines in water decreases as the chain length R increases and as the number of organic groups associated with nitrogen increases (transition to secondary and tertiary amines). The smell of amines resembles the smell of ammonia, higher (with large R) amines are practically odorless.
Chemical properties of amines.
The distinctive ability of amines is to add neutral molecules (for example, hydrogen halides HHal, with the formation of organoammonium salts, similar to ammonium salts in inorganic chemistry. For the formation of a new bond, nitrogen provides an unshared electron pair, acting as a donor. The H + proton involved in the formation of the bond (from hydrogen halide) plays the role of an acceptor (receiver), such a bond is called a donor-acceptor bond (Fig. 1). Emerging covalent bond N–H is completely equivalent to the N–H bonds present in the amine.
Tertiary amines also add HCl, but when the resulting salt is heated in an acid solution, it decomposes, while R is split off from the N atom:
(C 2 H 5) 3 N+ HCl ® [(C 2 H 5) 3 N H]Cl
[(C 2 H 5) 3 N H]Cl ® (C 2 H 5) 2 N H + C 2 H 5 Cl
When comparing these two reactions, it can be seen that the C 2 H 5 group and H, as it were, change places, as a result, a secondary is formed from the tertiary amine.
Dissolving in water, amines capture a proton in the same way, as a result, OH ions appear in the solution, which corresponds to the formation of an alkaline environment, which can be detected using conventional indicators.
C 2 H 5 N H 2 + H 2 O ® + + OH -
With the formation of a donor-acceptor bond, amines can add not only HCl, but also haloalkyls RCl, and a new N–R bond is formed, which is also equivalent to the existing ones. If we take a tertiary amine as the initial one, then we get a tetraalkylammonium salt (four R groups on one N atom):
(C 2 H 5) 3 N+ C 2 H 5 I ® [(C 2 H 5) 4 N]I
These salts, dissolving in water and some organic solvents, dissociate (decompose), forming ions:
[(C 2 H 5) 4 N]I ® [(C 2 H 5) 4 N] + + I –
Such solutions, like all solutions containing ions, conduct electricity. In tetraalkylammonium salts, the halogen can be replaced by an HO group:
[(CH 3) 4 N]Cl + AgOH ® [(CH 3) 4 N]OH + AgCl
The resulting tetramethylammonium hydroxide is a strong base, similar in properties to alkalis.
Primary and secondary amines interact with nitrous acid HON=O, but they react differently. Primary alcohols are formed from primary amines:
C 2 H 5 N H 2 + H N O 2 ® C 2 H 5 OH + N 2+H2O
Unlike primary amines, secondary amines form yellow, sparingly soluble nitrosamines with nitrous acid, compounds containing the >N–N = O moiety:
(C 2 H 5) 2 N H+H N O 2 ® (C 2 H 5) 2 N N\u003d O + H 2 O
Tertiary amines do not react with nitrous acid at ordinary temperatures, so nitrous acid is a reagent that makes it possible to distinguish between primary, secondary and tertiary amines.
When amines condense with carboxylic acids acid amides are formed - compounds with a -C (O) N fragment
The condensation of amines with aldehydes and ketones leads to the formation of the so-called Schiff bases, compounds containing the -N=C2 moiety.
The interaction of primary amines with phosgene Cl 2 C=O gives compounds with the –N=C=O group, called isocyanates (Fig. 2D, obtaining a compound with two isocyanate groups).
Among aromatic amines, aniline (phenylamine) C 6 H 5 NH 2 is the most famous. In terms of properties, it is close to aliphatic amines, but its basicity is less pronounced - in aqueous solutions it does not form an alkaline environment. Like aliphatic amines, it can form ammonium salts with strong mineral acids [C 6 H 5 NH 3] + Cl -. When aniline reacts with nitrous acid (in the presence of HCl), a diazo compound containing the R–N=N moiety is formed; it is obtained in the form of an ionic salt called the diazonium salt (Fig. 3A). Thus, the interaction with nitrous acid is not the same as in the case of aliphatic amines. The benzene nucleus in aniline has a reactivity characteristic of aromatic compounds (cm. AROMATICITY), upon halogenation, hydrogen atoms in ortho- And pair-positions to the amino group are substituted, resulting in chloranilines with various degrees of substitution (Fig. 3B). The action of sulfuric acid leads to sulfonation in pair-position to the amino group, the so-called sulfanilic acid is formed (Fig. 3B).
Getting amines.
When ammonia reacts with haloalkyls, such as RCl, a mixture of primary, secondary and tertiary amines is formed. The resulting by-product HCl adds to the amines to form an ammonium salt, but with an excess of ammonia, the salt decomposes, which allows the process to be carried out up to the formation of quaternary ammonium salts (Fig. 4A). Unlike aliphatic haloalkyls, aryl halides, for example, C 6 H 5 Cl, react with ammonia with great difficulty; synthesis is possible only with catalysts containing copper. In industry, aliphatic amines are obtained by the catalytic interaction of alcohols with NH3 at 300–500°C and a pressure of 1–20 MPa, resulting in a mixture of primary, secondary, and tertiary amines (Fig. 4B).
The interaction of aldehydes and ketones with the ammonium salt of formic acid HCOONH4 gives primary amines (Fig. 4C), while the reaction of aldehydes and ketones with primary amines (in the presence of formic acid HCOOH) leads to secondary amines (Fig. 4D).
Nitro compounds (containing the -NO 2 group) form primary amines upon reduction. This method, proposed by N.N. Zinin, is little used for aliphatic compounds, but is important for obtaining aromatic amines and formed the basis for the industrial production of aniline (Fig. 4E).
As separate compounds, amines are used little, for example, polyethylenepolyamine [-C 2 H 4 NH-] is used in everyday life n(trade name PEPA) as a hardener for epoxy resins. The main use of amines is as intermediates in the preparation of various organic matter. The leading role belongs to aniline, on the basis of which a wide range of aniline dyes is produced, and the color "specialization" is laid already at the stage of obtaining the aniline itself. Ultrapure aniline without homologues is called in the industry "aniline for blue" (meaning the color of the future dye). "Aniline for red" must contain, in addition to aniline, a mixture ortho- And pair-toluidine (CH 3 C 6 H 4 NH 2).
Aliphatic diamines are the initial compounds for the production of polyamides, for example, nylon (Fig. 2), which is widely used for the manufacture of fibers, polymer films, as well as components and parts in mechanical engineering (polyamide gears).
Polyurethanes are obtained from aliphatic diisocyanates (Fig. 2), which have a complex technically important properties: high strength combined with elasticity and very high abrasion resistance (polyurethane shoe soles) as well as good adhesion to a wide range of materials (polyurethane adhesives). They are widely used in foamed form (polyurethane foams).
Based on sulfanilic acid (Fig. 3), anti-inflammatory drugs sulfonamides are synthesized.
Diazonium salts (Fig. 2) are used in photosensitive materials for blueprinting, which makes it possible to obtain an image bypassing the usual silver halide photograph ( cm. LIGHT COPYING).
Mikhail Levitsky
I. According to the number of hydrocarbon radicals in the amine molecule:
Primary amines R-NH 2
(derivatives of hydrocarbons in which the hydrogen atom is replaced by an amino group -NH 2),
Secondary amines R-NH-R"
II. According to the structure of the hydrocarbon radical:
Aliphatic, for example: C 2 H 5 -NH 2 ethylamine
Limit primary amines
General formula C n H 2n+1 NH 2 (n ≥ 1); or C n H 2n+3 N (n ≥ 1)
Nomenclature
The names of amines (especially secondary and tertiary) are usually given according to the radical-functional nomenclature, listing the radicals in alphabetical order and adding the class name - amine. The names of primary amines according to the substitution nomenclature are made up of the name of the parent hydrocarbon and the suffix - amine.
CH 3 -NH 2 methanamine (methylamine)
CH 3 -CH 2 -NH 2 ethanamine (ethylamine)
Primary amines are often referred to as derivatives of hydrocarbons, in the molecules of which one or more hydrogen atoms are replaced by NH 2 amino groups. The amino group is considered as a substituent, and its location is indicated by a number at the beginning of the name. For example:
H 2 N-CH 2 -CH 2 -CH 2 -CH 2 -NH 2 1,4-diaminobutane.
Aniline (phenylamine) C 6 H 5 NH 2 in accordance with this method is called aminobenzene.
Homologous series of saturated amines
CH 3 NH 2 - methylamine (primary amine), (CH 3) 2 NH - dimethylamine (secondary amine), (CH 3) 3 N - trimethylamine (tertiary amine), etc.
isomerism
Structural isomerism
Carbon skeleton, starting with C 4 H 9 NH 2:
Positions of the amino group, starting with C 3 H 7 NH 2:
Isomerism of the amino group associated with a change in the degree of substitution of hydrogen atoms at nitrogen:
Spatial isomerism
Optical isomerism is possible, starting with C 4 H 9 NH 2:
Optical (mirror) isomers - spatial isomers, the molecules of which relate to each other as an object and an incompatible mirror image (like left and right hands).
Physical Properties
Lower limiting amines - gaseous substances; middle members homologous series- liquids; higher amines are solids. Methylamine has an ammonia smell, other lower amines have a sharp unpleasant smell, reminiscent of the smell of herring brine.
Lower amines are highly soluble in water, with an increase in the hydrocarbon radical, the solubility of amines decreases. Amines are formed during the decay of organic residues containing proteins. A number of amines are formed in human and animal organisms from amino acids (biogenic amines).
Chemical properties
Amines, like ammonia, exhibit pronounced properties of bases, which is due to the presence of a nitrogen atom in the amine molecules, which has an unshared pair of electrons.
1. Interaction with water
Solutions of amines in water are alkaline.
2. Interaction with acids (formation of salts)
Amines are released from their salts under the action of alkalis:
Cl + NaOH → CH 3 CH 2 NH 2 + NaCl + H 2 O
3. Combustion of amines
4CH 3 NH 2 + 9O 2 → 4CO 2 + 10H 2 O + 2N 2
4. Reaction with nitrous acid (the difference between primary amines and secondary and tertiary ones)
Under the action of HNO 2, primary amines are converted into alcohols with the release of nitrogen:
C 2 H 5 NH 2 + HNO 2 → C 2 H 5 OH + N 2 + H 2 O
How to get
1. Reaction of haloalkanes with ammonia
CH 3 Br + 2NH 3 → CH 3 NH 2 + NH 4 Br
2. Interaction of alcohols with ammonia
(In practice, these reactions produce a mixture of primary, secondary, tertiary amines and a quaternary ammonium salt.)
Amines entered our lives quite unexpectedly. Until recently, these were toxic substances, collision with which could lead to death. And now, after a century and a half, we are actively using synthetic fibers, fabrics, building materials, dyes, which are based on amines. No, they did not become safer, people were simply able to "tame" them and subdue them, deriving certain benefits for themselves. About which one, and we'll talk further.
Definition
For the qualitative and quantitative determination of aniline in solutions or compounds, a reaction with is used at the end of which a white precipitate in the form of 2,4,6-tribromaniline falls on the bottom of the test tube.
Amines in nature
Amines are found in nature everywhere in the form of vitamins, hormones, metabolic intermediates, they are also found in animals and plants. In addition, when living organisms rot, medium amines are also obtained, which, in a liquid state, spread an unpleasant smell of herring brine. The "cadaveric poison" widely described in the literature appeared precisely due to the specific ambergris of amines.
For a long time, the substances we are considering were confused with ammonia due to a similar smell. But in the mid-nineteenth century, the French chemist Wurtz was able to synthesize methylamine and ethylamine and prove that they release hydrocarbons when burned. This was the fundamental difference between the mentioned compounds and ammonia.
Obtaining amines in industrial conditions
Since the nitrogen atom in amines is in the lowest oxidation state, the reduction of nitrogen-containing compounds is the simplest and most affordable way to obtain them. It is he who is widely used in industrial practice because of its cheapness.
The first method is the reduction of nitro compounds. The reaction during which aniline is formed is named by the scientist Zinin and was carried out for the first time in the middle of the nineteenth century. The second method is to reduce amides with lithium aluminum hydride. Primary amines can also be reduced from nitriles. The third option is alkylation reactions, that is, the introduction of alkyl groups into ammonia molecules.
Application of amines
By themselves, as pure substances, amines are used little. One rare example is polyethylenepolyamine (PEPA), which makes epoxy resin easier to cure in the home. Basically a primary, tertiary or secondary amine is an intermediate in the production of various organics. The most popular is aniline. It is the basis of a large palette of aniline dyes. The color that will turn out at the end depends directly on the selected raw material. Pure aniline gives a blue color, while a mixture of aniline, ortho- and para-toluidine will be red.
Aliphatic amines are needed to obtain polyamides such as nylon and others. They are used in mechanical engineering, as well as in the production of ropes, fabrics and films. In addition, aliphatic diisocyanates are used in the manufacture of polyurethanes. Due to their exceptional properties (lightness, strength, elasticity and the ability to attach to any surface), they are in demand in construction (mounting foam, glue) and in the shoe industry (anti-slip soles).
Medicine is another area where amines are used. Chemistry helps to synthesize antibiotics of the sulfonamide group from them, which are successfully used as second-line drugs, that is, reserve ones. In case bacteria develop resistance to essential drugs.
Harmful effects on the human body
It is known that amines are very toxic substances. Any interaction with them can cause harm to health: inhalation of vapors, contact with open skin or ingestion of compounds into the body. Death occurs from a lack of oxygen, since amines (in particular, aniline) bind to blood hemoglobin and prevent it from capturing oxygen molecules. Alarming symptoms are shortness of breath, blue nasolabial triangle and fingertips, tachypnea (rapid breathing), tachycardia, loss of consciousness.
In case of contact with these substances on bare areas of the body, it is necessary to quickly remove them with cotton wool previously moistened with alcohol. This must be done as carefully as possible so as not to increase the area of \u200b\u200bcontamination. If symptoms of poisoning appear, you should definitely consult a doctor.
Aliphatic amines are a poison for the nervous and cardiovascular systems. They can cause depression of liver function, its degeneration and even oncological diseases of the bladder.
