Inert gases properties. Inert or noble gases. How are inert gases used?
Probably, even those people who do not often encounter questions in chemistry have repeatedly heard that some gases are called noble. However, few people wonder why gases were called noble. And today, in this article, we will try to understand this issue in detail.
What are “noble” gases
The group of noble gases includes a whole list of different chemical elements that can be ordered or combined according to their properties. Naturally, gases do not have a completely identical composition, and what they have in common is that under the simplest conditions, which in chemistry are called normal conditions, these gases have no color, taste or smell. In addition, they also have in common the fact that they have extremely low chemical reactivity.
List of "noble" gases
The list of noble gases known to mankind includes only 6 names. Among them are the following chemical elements:
- Radon;
- Helium;
- Xenon;
- Argon;
- Krypton;
- Neon.
Why are gases called “noble”?
As for the direct origin of the name that scientists assigned to the chemical elements described above, it was given to them because of the behavior of the atoms of the elements with other elements.
As is known, chemical elements can influence each other and exchange atoms with each other. This condition also applies to many gases. However, if we talk about the elements from the list presented above, they do not react with any other elements present in the periodic table known to us all. This led to the fact that scientists very quickly conditionally classified the gases into one group, calling it noble in honor of their “behavior.”
Other names for noble gases
It is important to note that noble gases also have other names by which scientists call them and which can also be called official
“Noble” gases are also called “Inert” or “Rare” gases
As for the second option, its origin is quite obvious, because from the entire periodic table of elements, only 6 atoms can be noted that belong to the list of noble gases. If we talk about the origin of the name “Inert,” then here you can use synonyms of this word, among which there are such concepts as “inactive” or “lacking initiative.”
Thus, all three names used for such gases are relevant and rationally selected.
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Noble (inert) gases.
|
2 He |
10 Ne |
18 Ar |
36 Kr |
54 Xe |
86 Rn |
|
|
Atomic mass |
4,0026 |
20,984 |
39,948 |
83,80 |
131,30 |
|
|
Valence electrons |
1s 2 |
(2)2s 2 2p 6 |
(8)3s 2 3p 6 |
(18)4s 2 4p 6 |
(18)5s 2 5p 6 |
(18)6s 2 6p |
|
Atomic radius |
0,122 |
0,160 |
0,192 |
0,198 |
0,218 |
0,22 |
|
Ionization energy E - → E + |
24,59 |
21,57 |
15,76 |
14,00 |
12,13 |
10,75 |
|
Content in the earth's atmosphere, % |
5*10 -4 |
1,8*10 -3 |
9,3*10 -1 |
1,1*10 -4 |
8,6*10 -6 |
6*10 -20 |
Noble (inert) gases are the elements of the main subgroup of group VIII: helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe) and radon (Rn) (a radioactive element). Each noble gas completes the corresponding period in the Periodic Table and has a stable, fully completed external electronic level - ns 2 n.p. 6 . – this explains the unique properties of the elements of the subgroup. The noble gases are considered to be completely inert. This is where their second name comes from – inert.
All noble gases are part of the atmosphere, their content in the atmosphere by volume (%) is: helium - 4.6 * 10 -4; argon – 0.93; krypton – 1.1* 10 -4; xenon – 0.8 * 10 -6 and radon – 6 * 10 -8. Under normal conditions, all of them are odorless and colorless gases, poorly soluble in water. Their boiling and melting points increase with increasing atomic sizes. The molecules are monatomic.
|
Properties |
He |
Ne |
Ar |
Kr |
Xe |
Rn |
|
Atomic radius, nm |
0,122 |
0,160 |
0,191 |
0,201 |
0,220 |
0,231 |
|
Ionization energy of atoms, eV |
24,58 |
21,56 |
15,76 |
14,00 |
12,13 |
10,75 |
|
Boiling point, o C |
-268,9 |
-245,9 |
-185,9 |
-153,2 |
-181,2 |
Near |
|
Melting point, o C |
-272.6(under pressure) |
-248,6 |
-189,3 |
-157,1 |
-111,8 |
Near |
|
Solubility in 1 liter of water at 0 o C, ml |
10 |
- |
60 |
- |
50 |
- |
§1. Helium
Helium was discovered in 1868. Using the method of spectral analysis of solar radiation (Lockyer and Frankland, England; Jansen, France). Helium was discovered on Earth in 1894. In the mineral kleveite (Ramsay, England).
From Greek
ἥλιος - "Sun" (see Helios). It is curious that the name of the element used the ending “-i”, characteristic of metals (in Latin “-um” - “Helium”), since Lockyer assumed that the element he discovered was a metal. By analogy with other noble gases, it would be logical to give it the name “Helion”. In modern science, the name “helion” is assigned to the nucleus of a light isotope of helium - helium-3.
The special stability of the electronic structure of the atom distinguishes helium from all other chemical elements of the periodic table.
Helium is less soluble than other gases in water and other solvents. Under normal conditions, helium is chemically inert, but with strong excitation of atoms it can form molecular ions. Under normal conditions these ions are unstable; I capture the missing electron, they split into two neutral atoms. The formation of ionized molecules is also possible. Helium is the most difficult to compress of all gases.
Helium can be converted into a liquid state only at a temperature approaching absolute zero, i.e. -273.15. Liquid helium at a temperature of about 2K has a unique property - superfluidity, which in 1938. P.L. was opened. Kapitsa and theoretically substantiated by L.D. Landau, who created the quantum theory of convolution. Liquid helium exists in two modifications: helium I, which behaves like an ordinary liquid, and helium II, a superthermal conductive and supervolatile liquid. Helium II conducts heat 10 7 times better than helium I (and 1000 times better than silver). It has virtually no viscosity, instantly passes through narrow capillaries, and spontaneously overflows through the walls of blood vessels in the form of a thin film. He atoms in the superfluid state behave in much the same way as electrons in superconductors.
In the earth's crust, helium accumulates due to the decay of particles of radioactive elements, and is found dissolved in minerals and native metals.
Helium nuclei are extremely stable and are widely used to carry out various nuclear reactions.
In industry, helium is mainly isolated from natural gases by deep cooling. At the same time, it, as the lowest boiling substance, remains in the form of a gas, while all other gases condense.
Helium gas is used to create an inert atmosphere when welding metals, preserving food products, etc. Liquid helium is used in the laboratory as a coolant in low-temperature physics.
§2. Neon
Neon was discovered in June 1898 by Scottish chemist William Ramsay and English chemist Maurice Travers. They isolated this inert gas by “exclusion,” after oxygen, nitrogen, and all the heavier components of the air were liquefied. The element was given the simple name “neon,” which translated from Greek means “new.” In December 1910, French inventor Georges Claude made a gas-discharge lamp filled with neon.
The name comes from the Greek. νέος - new.
There is a legend according to which the name of the element was given by Ramsay's thirteen-year-old son, Willie, who asked his father what he was going to call the new gas, noting that he would like to give it a name novum(Latin - new). His father liked the idea, but felt that the title neon, derived from a Greek synonym, will sound better.
Neon, like helium, has a very high ionization potential (21.57 eV), so it does not form valence-type compounds. Its main difference from helium is due to the relatively greater polarizability of the atom, i.e. a slightly greater tendency to form intermolecular bonds.
Neon has very low boiling points (-245.9 o C) and melting points (-248.6 o C), second only to helium and hydrogen. Compared to helium, neon has a slightly higher solubility and ability to be adsorbed.
Like helium, neon, when strongly excited by atoms, forms molecular ions of the Ne 2 + type.
Neon is produced together with helium as a by-product during the process of liquefying and separating air. The separation of helium and neon is carried out by adsorption or condensation. The adsorbed method is based on the ability of neon, unlike helium, to be adsorbed by activated carbon cooled with liquid nitrogen. The condensation method is based on freezing out neon while cooling the mixture with liquid hydrogen.
Neon is used in electric vacuum technology to fill voltage stabilizers, photocells and other devices. Various types of neon lamps with a characteristic red glow are used in lighthouses and other lighting devices, in illuminated advertising, etc.
Natural neon consists of three stable isotopes: 21 Ne and 22 Ne.
In world matter neon It is distributed unevenly, but in general it ranks fifth in abundance in the Universe among all elements - about 0.13% by mass. The highest concentration of neon is observed on the Sun and other hot stars, in gaseous nebulae, in the atmosphere of outer planets of the solar system- Jupiter, Saturn, Uranus, Neptune. In the atmosphere of many stars, neon ranks third after hydrogen and helium. Of all the elements of the second period neon- the smallest population on Earth. Within the eighth group neon It ranks third in terms of content in the earth's crust - after argon and helium. Gas nebulae and some stars contain many times more neon than is found on Earth.
On Earth, the highest concentration of neon is observed in the atmosphere - 1.82 10 −3% by volume, and its total reserves are estimated at 7.8 10 14 m³. 1 m³ of air contains about 18.2 cm³ of neon (for comparison: the same volume of air contains only 5.2 cm³ of helium). The average neon content in the earth's crust is low - 7·10−9% by mass. In total, there are about 6.6 10 10 tons of neon on our planet. Igneous rocks contain about 10 9 tons of this element. As rocks break down, gas escapes into the atmosphere. To a lesser extent, the atmosphere is supplied with neon and natural waters.
Scientists see the reason for the neon poverty of our planet in the fact that the Earth once lost its primary atmosphere, which took with it the bulk of inert gases that could not, like oxygen and other gases, chemically bond with other elements into minerals and thereby gain a foothold on planet.
In 1892, the British scientist John Strett, better known to us as Lord Rayleigh ( cm. Rayleigh criterion), was engaged in one of those monotonous and not very exciting works, without which experimental science nevertheless cannot exist. He studied the optical and chemical properties of the atmosphere, setting himself the goal of measuring the mass of a liter of nitrogen with an accuracy that no one before him had been able to achieve.
However, the results of these measurements seemed paradoxical. The mass of a liter of nitrogen obtained by removing all other then known substances (such as oxygen) from the air and the mass of a liter of nitrogen obtained through a chemical reaction (by passing ammonia over copper heated to red heat) turned out to be different. It turned out that nitrogen from the air is 0.5% heavier than nitrogen obtained chemically. This discrepancy haunted Rayleigh. Having made sure that no errors were made in the experiment, Rayleigh published in the journal Nature letter asking if anyone could explain the reason for these discrepancies.
Sir William Ramsay (1852–1916), then working at University College London, responded to Rayleigh's letter. Ramsay suggested that there may be an undiscovered gas in the atmosphere, and he proposed using the latest equipment to isolate this gas. In the experiment, oxygen-enriched air mixed with water was exposed to an electrical discharge, which caused atmospheric nitrogen to combine with oxygen and dissolve the resulting nitrogen oxides in water. At the end of the experiment, after all the nitrogen and oxygen from the air had been exhausted, there was still a small bubble of gas left in the vessel. When an electric spark was passed through this gas and subjected to spectroscopy, scientists saw previously unknown spectral lines ( cm. Spectroscopy). This meant that a new element had been discovered. Rayleigh and Ramsay published their results in 1894, naming the new gas argon, from the Greek “lazy”, “indifferent”. And in 1904, both of them received the Nobel Prize for this work. However, it was not divided between scientists, as is customary in our time, but each received a prize in their field - Rayleigh in physics, and Ramsay in chemistry.
There was even some kind of conflict. At the time, many scientists believed that they "mastered" certain areas of research, and it was not entirely clear whether Rayleigh gave Ramsay permission to work on this problem. Fortunately, both scientists were wise enough to realize the benefits of working together, and by publishing their results together, they eliminated the possibility of an unpleasant battle for primacy.
Argon is a monatomic gas. Having a relatively larger atomic size, argon is more prone to forming intermolecular bonds than helium and neon. Therefore, argon in the form of a millet substance is characterized by slightly higher boiling points (at normal pressure) -185.9 °C (slightly lower than oxygen, but slightly higher than nitrogen) and melting points (-184.3 °C). 3.3 ml of argon dissolves in 100 ml of water at 20 °C; argon dissolves in some organic solvents much better than in water.
Argon forms intermolecular inclusion compounds - clathrates of the approximate composition Ar*6H 2 0 is a crystalline substance that decomposes at atmospheric pressure and a temperature of -42.8 °C. It can be obtained directly by the interaction of argon with water at 0°C and a pressure of the order of 1.5 * 10 7 Pa. With compounds H 2 S, SO 2, CO 2, HCl, argon gives double hydrates, i.e. mixed clathrates.
Argon is obtained by separating liquid air, as well as from waste gases of ammonia synthesis. Argon is used in metallurgical and chemical processes that require an inert atmosphere, in lighting engineering, electrical engineering, nuclear energy, etc.
Argon (along with neon) is observed on some stars and in planetary nebulae. In general, there is more of it in space than calcium, phosphorus, and chlorine, while on Earth the opposite relationships exist.
Argon is the third most abundant component of air after nitrogen and oxygen, its average content in the Earth's atmosphere is 0.934% by volume and 1.288% by mass, its reserves in the atmosphere are estimated at 4 10 14 tons. Argon is the most common inert gas in the Earth's atmosphere , 1 m³ of air contains 9.34 liters of argon (for comparison: the same volume of air contains 18.2 cm³ of neon, 5.2 cm³ of helium, 1.1 cm³ of krypton, 0.09 cm³ of xenon).
§4. Krypton
In 1898, the English scientist W. Ramsay isolated from liquid air (having previously removed oxygen, nitrogen and argon) a mixture in which two gases were discovered by the spectral method: krypton (“hidden”, “secret”) and xenon (“alien”, “ unusual").
From Greek
κρυπτός - hidden. Located in atmospheric air. It is formed during nuclear fission, including as a result of natural processes occurring in ores of radioactive metals. Krypton is obtained as a by-product from.
Gaseous oxygen containing Kr and Xe from the condenser of the installation for producing O 2 is supplied for rectification in the so-called. a krypton column, in which Kr and Xe are extracted from gaseous O 2 when it is washed with reflux formed at the top of the condenser of the krypton column. The bottom liquid is enriched in Kr and Xe; it is then almost completely evaporated, the non-evaporated part is the so-called. called lean iron-xenon concentrate (less than 0.2% Kr and Xe) - continuously flows through the evaporator into the gas tank. With an optimal reflux ratio of 0.13, the degree of extraction of Kr and Xe is 0.90. The separated concentrate is compressed to 0.5-0.6 MPa and fed through a heat exchanger into a contact apparatus with CuO heated to ~1000 K to burn off the hydrocarbons contained in it. After cooling in a water refrigerator, the gas mixture is purified from impurities of CO 2 and water using KOH, first in scrubbers and then in cylinders. Burning and cleaning are repeated several times. once. The purified concentrate is cooled and continuously fed into the rectifier. column under pressure 0.2-0.25 MPa. In this case, Kr and Xe accumulate in the bottom liquid to a content of 95-98%. This so-called The raw krypton-xenon mixture is sent through a gasifier, an apparatus for burning hydrocarbons and a purification system into gas tanks. From the gas holder, the gas mixture enters the gasifier, where it is condensed at 77 K. Part of this mixture is subjected to fractional evaporation. As a result, the last purification from O 2 in a contact apparatus with CuO produces pure krypton. The remaining gas mixture is subjected to adsorption in devices with activator. coal at 200-210 K; in this case, pure krypton is released, and Xe and part of the krypton are absorbed by coal. Adsorbed Kr and Xe are separated by fractionated desorption. With a capacity of 20,000 m 3 /h of processed air (273 K, 0.1 MPa), 105 m 3 of krypton are obtained per year. It is also extracted from the methane fraction of purge gases in NH 3 production. They produce pure krypton (more than 98.9% by volume of krypton), technical. (more than 99.5% mixture of Kr and Xe) and krypton-xenon mixture (less than 94.5% krypton). Krypton is used to fill incandescent lamps, gas-discharge and X-ray tubes. The radioactive isotope 85 Kr is used as a source of b-radiation in medicine, to detect leaks in vacuum installations, as isotope tracer during corrosion studies, to monitor wear of parts. Krypton and its mixtures with Xe are stored and transported under a pressure of 5-10 MPa at 20°C in sealed steel cylinders black resp. with one yellow stripe and the inscription "Krypton" and two yellow stripes and the inscription "Krypton-xenon". Krypton was discovered in 1898 by W. Ramsay and M. Travers. Lit.
§5. Xenon
Discovered in 1898 by English scientists W. Ramsay and W. Rayleigh as a small admixture of krypton.
From Greek
ξένος - stranger.
Melting point −112 °C, boiling point −108 °C, violet glow in the discharge. The first inert gas for which true chemical compounds were prepared. Examples of connections could be, xenon difluoride, xenon tetrafluoride, xenon hexafluoride.
xenon trioxide Located in atmospheric air. It is formed during nuclear fission, including as a result of natural processes occurring in ores of radioactive metals. Krypton is obtained as a by-product from Xenon is produced as a by-product when
. It is isolated from krypton-xenon concentrate (see Krypton). They produce pure (99.4% by volume) and high purity (99.9%) xenon. Xenon is obtained as a by-product of the production of liquid oxygen at metallurgical enterprises. In industry, xenon is produced as a by-product of the separation of air into oxygen and nitrogen. After this separation, which is usually carried out by rectification, the resulting liquid oxygen contains small amounts of krypton and xenon. Further rectification enriches liquid oxygen to a content of 0.1-0.2% krypton-xenon mixture, which is separated adsorption
on silica gel or by distillation. Finally, the xenon-krypton concentrate can be separated by distillation into krypton and xenon.
Due to its low prevalence, xenon is much more expensive than lighter inert gases.
Despite its high cost, xenon is indispensable in a number of cases:
Xenon is used to fill incandescent lamps, powerful gas-discharge and pulsed light sources (the high atomic mass of the gas in lamp bulbs prevents the evaporation of tungsten from the surface of the filament).
Radioactive isotopes (127 Xe, 133 Xe, 137 Xe, etc.) are used as radiation sources in radiography and for diagnostics in medicine, for detecting leaks in vacuum installations.
Xenon fluorides are used for passivation of metals.
Since the end of the 20th century, xenon began to be used as a means for general anesthesia (quite expensive, but absolutely non-toxic, or rather, like an inert gas, it does not cause chemical consequences). The first dissertations on the technique of xenon anesthesia in Russia - 1993, as a therapeutic anesthesia, it is effectively used to relieve acute withdrawal states and treat drug addiction, as well as mental and somatic disorders.
Liquid xenon is sometimes used as a working medium for lasers.
Xenon fluorides and oxides are proposed as powerful oxidizers of rocket fuel, as well as components of gas mixtures for lasers.
In the 129 Xe isotope, it is possible to polarize a significant portion of the nuclear spins to create a state with co-directed spins - a state called hyperpolarization.
Xenon is used in the design of the Golay cell.
As chemical catalysts.
For transportation of fluorine, which exhibits strong oxidizing properties.
Xenon is in earth's atmosphere in extremely small quantities, 0.087±0.001 parts per million (μL/L), and is also found in gases emitted by some mineral springs. Some radioactive isotopes of xenon, such as 133 Xe and 135 Xe, are produced by neutron irradiation of nuclear fuel in reactors.
The English scientist E. Rutherford noted in 1899 that thorium preparations emit, in addition to α-particles, some previously unknown substance, so that the air around the thorium preparations gradually becomes radioactive. He proposed to call this substance an emanation (from the Latin emanatio - outflow) of thorium and give it the symbol Em. Subsequent observations showed that radium preparations also emit a certain emanation, which has radioactive properties and behaves like an inert gas.
Initially, the emanation of thorium was called thoron, and the emanation of radium was called radon. It was proven that all emanations are actually radionuclides of a new element - an inert gas, which corresponds to atomic number 86. It was first isolated in its pure form by Ramsay and Gray in 1908, they also proposed to call the gas niton (from the Latin nitens, luminous ). In 1923, the gas was finally named radon and the symbol Em was changed to Rn.
Radon is a radioactive monatomic gas, colorless and odorless. Solubility in water 460 ml/l; in organic solvents and in human adipose tissue, the solubility of radon is tens of times higher than in water. Gas penetrates well through polymer films. Easily adsorbed by activated carbon and silica gel.
Radon's own radioactivity causes it to fluoresce. Gaseous and liquid radon fluoresces with blue light, while solid radon when cooled to nitrogen temperatures The fluorescence color becomes first yellow, then red-orange.
Radon forms clathrates, which, although they have a constant composition, do not contain chemical bonds involving radon atoms. With fluorine, radon at high temperatures forms compounds of the composition RnF n, where n = 4, 6, 2. Thus, radon difluoride RnF 2 is a white non-volatile crystalline substance. Radon fluorides can also be produced by the action of fluorinating agents (for example, halogen fluorides). At hydrolysis of tetrafluoride RnF 4 and hexafluoride RnF 6 form radon oxide RnO 3 . Compounds with the RnF + cation were also obtained.
To obtain radon, air is blown through an aqueous solution of any radium salt, which carries with it the radon formed during the radioactive decay of radium. Next, the air is carefully filtered to separate microdroplets of the solution containing the radium salt, which can be captured by the air current. To obtain radon itself, chemically active substances (oxygen, hydrogen, water vapor, etc.) are removed from a mixture of gases, the residue is condensed with liquid nitrogen, then nitrogen and other inert gases (argon, neon, etc.) are distilled from the condensate.
Radon is used in medicine to prepare radon baths. Radon is used in agriculture to activate animal feed [ source not specified 272 days ] , in metallurgy as an indicator when determining the speed of gas flows in blast furnaces and gas pipelines. In geology, measuring radon content in air and water is used to search for deposits of uranium and thorium, in hydrology - to study the interaction of groundwater and river waters. The dynamics of radon concentration in groundwater can be used to predict earthquakes.
It is part of the radioactive series 238 U, 235 U and 232 Th. Radon nuclei constantly arise in nature during the radioactive decay of parent nuclei. The equilibrium content in the earth's crust is 7·10−16% by mass. Due to its chemical inertness, radon relatively easily leaves the crystal lattice of the “parent” mineral and enters groundwater, natural gases and air. Since the longest-lived of the four natural isotopes of radon is 222 Rn, it is its content in these environments that is maximum.
The concentration of radon in the air depends primarily on the geological situation (for example, granites, which contain a lot of uranium, are active sources of radon, while at the same time there is little radon above the surface of the seas), as well as on the weather (during rain, microcracks through which radon comes from the soil and is filled with water; snow cover also prevents radon from entering the air). Before the earthquakes, an increase in radon concentration in the air was observed, probably due to a more active exchange of air in the ground due to an increase in microseismic activity.
(Galina Afanasyevna – HELP with krypton, xenon, argon! can I add something else? And what should I write next?)
Page 1
In this article we will focus on VIIIA-group.
These are the elements: helium(He), neon(Ne), argon(Ar), krypton(Kr), xenon(Xe) (these are basic), as well as radioactive radon(Rn).
And formally, artificially obtained ununoctium (Uuo) can also be included here.
This group of elements also has its own name - aerogens, but more often they are called noble, or inert gases.
Noble gases
These gases are united by low reactivity. The word inertia precisely means inactivity. Therefore, for a long time they were not even aware of their existence. They cannot be determined using reactions. They were discovered in the air (hence the name aerogens), removing oxygen and other “by-product gases” from it to obtain nitrogen, and experimentally established that the nitrogen thus obtained has impurities. These impurities turned out to be inert gases.
To understand the reason for the low reactivity of these gases, you need to construct their electronic diagrams:
We can see that no unpaired electrons, orbitals are filled. This is a very favorable state of the electron shell. Therefore, all other elements, forming compounds, tend to acquire the electronic configuration of noble gases (remember the octet rule), because it is energetically favorable, and atoms, like people, love benefits.
Due to their low activity, noble gas atoms do not even combine into diatomic molecules (as they do: O 2, Cl 2, N 2, etc.).
Noble gases exist as monatomic molecules.
It is impossible to say that noble gases are absolutely inert. Some aerogens have empty orbitals within the same energy level, which means that the process of excitation of electrons is possible. Currently, some compounds of these “lazy” elements from the point of view of chemical activity have been obtained under extremely extreme conditions. But in the school curriculum, and especially in the school, this is not considered.
Physical properties
- helium and neon are lighter than air, the rest of the noble gases, which are lower, are heavier, which is due to the increase in atomic mass.
- Due to chemical inertness, taste and olfactory receptors cannot detect the presence of noble gases in the air, so they have neither taste nor smell.
Practical significance noble gases.
Helium is a well-known gas for filling balloons, which makes the voice funny. Airships are filled with helium (this gas, unlike hydrogen, is not explosive).
Noble gases are used to create an inert (chemically inactive) atmosphere. Some aerogens are part of breathing mixtures, diluting oxygen (oxygen is a strong oxidizing agent and cannot be breathed in its pure form).
When a current discharge is passed through noble gases, they tend to glow brightly. Which provides aerogens with applications for lighting equipment. It looks quite spectacular.
- (a. inert gasses; n. Inertgase, Tragergase; f. gaz inertes; i. gases inertes) noble, rare gases, monatomic gases without color and odor: helium (He), neon (Ne) ... Geological encyclopedia
- (noble gases, rare gases) elements Ch. subgroups of group VIII periodic. systems of elements. Irradiation includes helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radioactivity. radon (Rn). In nature, i.g. are present in the atmosphere, Not... ... Physical encyclopedia
Big Encyclopedic Dictionary
Noble gases- the same as noble gases... Russian encyclopedia of labor protection
Noble gases- INERT GASES, the same as noble gases. ... Illustrated Encyclopedic Dictionary
INERT [ne], aya, oh; ten, tna. Ozhegov's explanatory dictionary. S.I. Ozhegov, N.Yu. Shvedova. 1949 1992 … Ozhegov's Explanatory Dictionary
inert gases- Elements of group VIII Periodic. systems: He, Ne, Ar, Kr, Xe, Rn. I. g. differ chemically. inertia, which is explained by the stable external an electronic shell, on which Ne has 2 electronics, the rest have 8 electronics. I. g. have a high potential... Technical Translator's Guide
Group → 18 ↓ Period 1 2 Helium ... Wikipedia
inert gases- elements of Group VIII of the Periodic Table: He, Ne, Ar, Kr, Xe, Rn. Noble gases are characterized by chemical inertness, which is explained by a stable outer electron shell, on which He has 2 electrons, the rest have 8... ... Encyclopedic Dictionary of Metallurgy
Noble gases, rare gases, chemical elements forming the main subgroup of the 8th group of the periodic system of Mendeleev: Helium He (atomic number 2), Neon Ne (10), Argon Ar (18), Krypton Kr (36), Xenon Xe (54) and Radon Rn (86). From… … Great Soviet Encyclopedia
Books
- Set of tables. Chemistry. Nonmetals (18 tables), . Educational album of 18 sheets. Art. 5-8688-018 Halogens. Chemistry of halogens. Sulfur. Allotropy. Chemistry of sulfur. Sulfuric acid. Chemistry of nitrogen. Nitrogen oxides. Nitric acid is an oxidizing agent. Phosphorus.…
- Inert gases, Fastovsky V.G.. The book discusses the basic physical and physico-chemical properties of the inert gases helium, neon, argon, krypton and xenon, as well as their areas of application in chemical, metallurgical,…
- (inert gas), a group of colorless and odorless gases that make up group 0 in the periodic table. These include (in order of increasing atomic number) HELIUM, NEON, ARGON, KRYPTON, XENON and RADON. Low chemical activity... ... Scientific and technical encyclopedic dictionary
NOBLE GASES- NOBLE GASES, chemical. elements: helium, neon, argon, krypton, xenon and emanation. They got their name from their inability to react with other elements. In 1894 the English. Scientists Rayleigh and Ramsay found that N obtained from air... ... Great Medical Encyclopedia
- (inert gases), chemical elements of group VIII of the periodic system: helium He, neon Ne, argon Ar, krypton Kr, xenon Xe, radon Rn. Chemically inert; all elements except He form inclusion compounds, for example Ar?5.75H2O, Xe oxides,... ... Modern encyclopedia
Noble gases- (inert gases), chemical elements of group VIII of the periodic system: helium He, neon Ne, argon Ar, krypton Kr, xenon Xe, radon Rn. Chemically inert; all elements except He form inclusion compounds, for example Ar´5.75H2O, Xe oxides,... ... Illustrated Encyclopedic Dictionary
- (inert gases) chemical elements: helium He, neon Ne, argon Ar, krypton Kr, xenon Xe, radon Rn; belong to group VIII of the periodic table. Monatomic gases are colorless and odorless. Present in small quantities in the air, found in... ... Big Encyclopedic Dictionary
Noble gases- (inert gases) elements of group VIII of the periodic table of D.I. Mendeleev: helium He, neon Ne, argon Ar, krypton Kr, xenon Xe, radon Rn. Present in small quantities in the atmosphere, found in some minerals, natural gases,... ... Russian encyclopedia of labor protection
NOBLE GASES- (see) simple substances formed by atoms of elements of the main subgroup of group VIII (see): helium, neon, argon, krypton, xenon and radon. In nature, they are formed during various nuclear processes. In most cases, they are obtained fractionally... ... Big Polytechnic Encyclopedia
- (inert gases), chemical elements: helium He, neon Ne, argon Ar, krypton Kr, xenon Xe, radon Rn; belong to group VIII of the periodic table. Monatomic gases are colorless and odorless. Present in small quantities in the air, found in... ... encyclopedic Dictionary
- (inert gases, rare gases), chemical. elements VIII gr. periodic systems: helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), radon (Rn). In nature they are formed as a result of decomposition. nuclear processes. Air contains 5.24 * 10 4% by volume He, ... ... Chemical encyclopedia
- (inert gases), chemical elements: helium He, neon Ne, argon Ar, krypton Kr, xenon Xe, radon Rn; belong to the VIII periodic group. systems. Monatomic gases are colorless and odorless. They are present in small quantities in the air, contained in certain... ... Natural history. encyclopedic Dictionary
Books
- , D. N. Putintsev, N. M. Putintsev. The book examines the structural, thermodynamic and dielectric properties of noble gases, their relationship with each other and with intermolecular interaction. Part of the text of the manual serves...
- Structure and properties of simple substances. Noble gases. Tutorial. Grif MO RF, Putintsev D.N. The book examines the structural, thermodynamic and dielectric properties of noble gases, their relationship with each other and with intermolecular interaction. Part of the text of the manual serves...