What substances can react with inert gases

Chemists have forced the relatively large noble gases of krypton, xenon, and radon to combine with atoms like fluorine and oxygen, which are particularly fond of accepting electrons from other atoms. Noble gases with smaller atoms – helium, neon, argon – have so far not been able by any chemist to involve them in chemical reactions.

Some production departments often use them as shielding gases, and can be made into a variety of mixed gas lasers. With the development of industrial production and science and technology, noble gases are becoming more and more widely used in industry, medicine, cutting-edge science and technology, and even daily life.

For example, argon is often used as a shielding gas in the welding of precision parts or reactive metals such as magnesium and aluminum, as well as in the manufacture of semiconductor transistors. Plutonium, the nuclear fuel of an atomic reactor, also oxidizes rapidly in the air and also needs to be mechanically processed under the protection of argon. Filling the bulb with argon gas can reduce the vaporization of the tungsten filament and prevent the oxidation of the tungsten filament, so as to prolong the life of the bulb.

The compound is in the atom of a noble gas element, and the arrangement of electrons in each electron shell just reaches a stable number. Therefore, atoms are not easy to lose or gain electrons, and it is difficult for them to chemically react with other substances, so these elements are called "noble gas elements".

Among noble gas atoms with a larger atomic weight and a higher number of electrons, the outermost electrons are farther away from the nucleus and are relatively weakly bound. If you encounter other atoms that attract strong electrons, these outermost electrons are lost, resulting in a chemical reaction.

In 1933, the famous American chemist Pauling (through the calculation of ionic radius, once predicted that xenon hexafluoride (XEF6), krypton hexafluoride (KRF6), xenon acid and its salts could be prepared. Inspired by Aintopov's first report and Pauling's prophecy, D.M. Younst tried unsuccessfully to synthesize xenon fluoride and xenon chloride by ultraviolet irradiation and discharge.

Uses of noble gases:

Depending on the nature of noble gases, they are used in production and scientific research. Helium is non-combustible, light in weight, and can replace flammable hydrogen to fill high-altitude balloons and airships. Due to the chemical properties of noble gases, they are often used as protective gases in industrial production.

For example, when welding stainless steel and aluminum alloy materials used in rockets, aircraft, missiles, ships, etc., with arc welding, high-purity argon can be used as a shielding gas to prevent the reaction of metals and oxygen in the air at high temperatures. The commonly used incandescent bulb is filled with a mixture of argon and nitrogen as a protective gas to protect the filament and prolong the service life of the bulb. Noble gases emit a variety of colors of light when discharged at low voltage, such as neon will emit a red glow, argon will emit a violet-blue glow, and helium will emit a pink glow, so the rare gas can be used to make colorful neon lights, and the night of the modern city will be dressed up with flowers.

The red light emitted by neon lamps can transmit through dense fog and is often used as an indicator light for aviation, navigation and railway traffic. Noble gases are playing a role in high-tech fields, helium has the lowest boiling point of any known substance, liquid helium is often used as a refrigerant in ultra-low temperature research, and helium can also be used as a refrigerant in atomic reactors. Neon, krypton, and xenon are also used to make lasers, etc.

Noble gases, also known as noble gases, include six gases: helium, neon, argon, krypton, xenon, and radon. Their volumes in the air are: argon, neon, helium, krypton, xenon, and radon is a radioactive gas.

Because their amounts in the air are very tiny, they are called noble gases. In general, the chemical properties of noble gases are very good.

Due to the inert gas nature is very inactive, it is often used as a shielding gas, such as using noble gas to isolate the air when welding metal, and filling the bulb with noble gas to make the bulb durable. Because the noble gas can emit different colors of light when it is energized, it can be made into a variety of electric light sources, such as navigation lights, strong lights, flashing lights, neon lights, etc., and can also be used in laser technology.

The role of inert gas can be played. The role of safety protection in isolating hazardous substances.

Some noble gases have a low density, such as helium, which can also be used to fill large probe balloons or airships.

Noble gases refer to the gas elementals corresponding to all group 0 elements on the periodic table.

At room temperature and pressure, they are all colorless and odorless monoatomic gases, which are difficult to carry out chemical reactions. There are 7 types of noble gases, which are helium (HE), neon (Ne), argon (AR), krypton (KR), xenon (XE), radon (RN, radioactive), (OG, radioactive, man-made element).

History of the discovery of noble gases:

In 1868, astronomers discovered a special yellow line d3 in the sun's spectrum, which was different from the two yellow lines d1 and d2 of sodium that had been known for a long time, thus predicting that there might be an unknown element in the sun. Later, this element was named "helium", which means "solar element".

More than 20 years later, Ramsey confirmed that helium is also present on Earth. In 1895, the American geologist Hillbrand observed that yttrium-uranium ore heated in sulfuric acid produced a gas that could not spontaneously ignite or support combustion. He thought the gas could be nitrogen or argon.

But no further research was carried out. Knowing of this experiment, Ramsey repeated it with yttrium-uranium ore to obtain a small amount of gas.

The above content reference:

Gases such as helium (He), neon (Ne), argon (Ar), krypton (Kr), and xenon (XE) are known as "lazy" and are called inert gases.

On August 13, British chemist Ramsay and physicist Rayleigh reported at a conference that they had discovered a new element with strange properties. This element exists in a gaseous state, and it is indifferent to any of the most reactive and powerful substances, hence the name argon, which means "lazy". Later, several elements were discovered, which also had similar properties, and they were like "hermits" of the elements, never chemically reacting with other elements.

What is the reason for this? It turns out that except for helium atoms, which have a stable structure of 2 electrons, the atoms of other gases have a stable structure of 8 electrons in the outermost shell. At that time, chemical theory believed that elements with such a structure could not undergo chemical reactions.

So, chemists conclude that it is impossible for noble gas elements to form compounds.

In the year, the young British chemist Bartlett accidentally obtained a dark red solid when he was conducting experiments on the reaction of platinum group metals and fluorine, and after analysis, he knew that it was a compound of hexafluoroplatinate oxygen (02ptf6), and saw from this compound the fact that the oxygen molecule that has reached the stable structure of 8 electrons can actually lose one electron and form a cation. Oxygen, on the other hand, is very difficult to lose electrons, and its first ionization energy (i.e., how difficult it is for an atom to lose electrons) is greater than the first ionization energy of xenon.

So, can the noble element xenon also form cations? Besides, platinum hexafluoride is a strong oxidizing agent, if platinum hexafluoride is combined with xenon, what will happen Batalet imitates the conditions and methods for synthesizing oxygen hexafluoroplatinate, and mixes platinum hexafluoride vapor with excess xenon at room temperature, and the result is an orange-yellow solid of xenon hexafluoroplatinate. This is the world's first noble gas compound.

Since then, xenon fluoride, chloride, and oxide have also been introduced, and now, there are hundreds of inert gas compounds such as hydrogen fluoride and argon difluoride.

The synthesis of noble gas compounds has given scientists another revelation: science is endless, and what is true today is likely to become a fallacy tomorrow. Only by having the courage to explore can we always stand on the side of truth.

There are seven types of noble gases (noble gases), which are helium (He), neon (Ne), argon (Ar), krypton (KR), xenon (Xe), radon (RN, radioactive), and gas (OG, radioactive, man-made element). The roles are:

1. Helium is usually a colorless and odorless gas, and it is the only substance that cannot be solidified at standard atmospheric pressure. Helium is the least reactive element. The main applications of helium are as shielding gases, working fluids in gas-cooled nuclear reactors, and ultra-low temperature refrigerants.

In addition, due to its smaller density than air and stable properties, helium can also be used as a buoyancy gas.

2. Neon is an inert gas that does not react with other substances under normal circumstances. Neon emits an orange-red glow when discharged, and is widely used in urban neon signs. In addition, the electric tester used in daily life is also filled with neon gas, which is the use of neon discharge, light and high resistance.

3. Argon is a colorless, odorless and tasteless gas. Argon cannot be burned and cannot be combusted. The earliest use of argon was to inflate light bulbs.

Large amounts of argon are also used for welding and cutting metals. It is used as a shielding gas for arc welding of stainless steel, magnesium, aluminum and other alloys, i.e. argon arc welding.

4. Krypton is a chemical element, a colorless, odorless, and tasteless inert gas, which is orange-red when it is discharged, and is often used to make fluorescent lamps.

5. Xenon, chemical properties are extremely inactive. Xenon has a very high luminous intensity, and is used in lighting technology to fill photocells, flash lamps and xenon high-profile pressure lamps. In addition, xenon is also used in deep anesthetics, medical ultraviolet light, lasers, welding, refractory metal cutting, standard gases, specialty gas mixtures, etc.

6. Radon, also known as 氭, symbol rn. The usual elemental form of radon is radon gas, which is a colorless, odorless, tasteless, inert gas that is radioactive. It can be used as a neutron source in the laboratory. Radon can also be used as a gas tracer to study pipeline leaks and gas movements, among other things.

7. OG is element No. 118, known as gas ao in Chinese, which is a synthetic rare gas element. As of September 14, 2019, there is no relevant application of the air element.

The old name for a noble gas.

Noble gases, also known as noble gases (less used) or noble gases (less used), refer to group 0 elements on the periodic table (IUPAC new regulations: group 18), which are all single-atom gases with molecules at room temperature.

Inert gases include: helium, neon, argon, krypton, xenon, radon.

Noble gases, also known as noble gases, noble gases, noble gases, noble gases, noble gases or blunt gases, refer to group 18 (8a) elements on the periodic table (IUPAC new regulations, that is, the original group 0), at room temperature and pressure, they are all odorless, colorless, monoatomic gases, and their reactivity is very low. There are six naturally occurring noble gases: helium (He), neon (Ne), argon (Ar), krypton (KR), xenon (Xe), and radioactive radon (RN).

UUO, on the other hand, is a synthetic noble gas, which is very unstable and has a very short half-life.

The characteristics of noble gases can be explained by modern theories of atomic structure: their outermost electron shell is "full" (i.e., it has reached the octagram state), so they are very stable, rarely undergo chemical reactions, and only a few hundred noble gas compounds have been successfully prepared so far. The melting and boiling points of each noble gas are very close, with a temperature difference of less than 10 °C (18 °F), so they exist in a liquid state only in a small temperature range.

Neon, argon, krypton and xenon can be obtained from air by gas liquefaction and fractionation methods; Helium is usually extracted from natural gas; Radon gas is usually separated by radioactive decay of radium compounds. In the industrial aspect, precious gases are mainly used in lighting equipment, welding and space exploration. Helium is also used in deep-sea diving.

If the diving depth is greater than 180 feet (55 meters), the nitrogen in the compressed air cylinder used by the diver should be replaced with helium to avoid oxygen poisoning and nitrogen anesthesia. On the other hand, because hydrogen is very unstable and flammable, helium is used instead of hydrogen in today's airships and balloons.

Refers to a gas that is stable in nature, does not combine with other elements, and exists only in the form of a single atom. There are six types of noble gases, which are arranged in order of increasing atomic weight, in order of helium, neon, argon, krypton, xenon, and radon.

Inert gases are: helium, neon, argon, krypton, xenon, radon.

Inert gases are: helium, neon, argon, krypton, xenon, radon.

Inert gases are: helium, neon, argon, krypton, xenon, radon.

Gases that do not react with other gases.

Generally refers to noble gases, such as helium, neon, argon, krypton, xenon, which are all noble gases.

OK. For example.

Xenon fluoride. fuhuaxian)

There are 3 binary compounds of fluorine and xenon, namely xenon difluoride XEF2, xenon tetrafluoride XEF4, xenon hexafluoride XEF6, which can be directly synthesized from fluorine and xenon under different conditions. These three fluorides are colorless solids with strong oxidizing properties, and the oxidation capacity increases with the increase of the oxidation number of xenon. They react with hydrogen as follows:

xef2+h2-xe+2hf

xef4+2h2-xe+4hf

xef6+3h2-xe+6hf

Xenon hexafluoride can also react with silica:

2xef6+3sio2→2xeo3+3sif4

The product xenon trioxide has the highest properties, therefore, xenon hexafluoride should not be stored in glass or quartz containers. Xenon trifluoride and xenon tetrafluoride cannot react with silica. All 3 xenon fluorides are covalent compounds.

Xenon fluoride is a strong oxidizing agent. The first compound of br( ) was obtained by oxidizing bro-3 with xenon difluoride in the following reaction:

xef2+bro-3+h2o→xe+bro-4+2hf

Xenon fluoride can not only oxidize many substances that are difficult to be oxidized, but also reduce itself to xenon gas to escape, without adding impurities to the system, for quantitative determination. For example, I-, Cr+3 are directly oxidized to IO-4 and CRO2-4 in a slightly acidic solutionXenon difluoride has good fluorinating properties for many organic and inorganic substances, and is a promising fluorinating agent in chemical production.

Xenon fluoride is also an initiator for the polymerization of alkene unsaturated compounds. Tungsten incandescent bulbs filled with xenon fluoride can prolong the life of the filament. When refining metals, xenon fluoride is added to the melt to help remove gaseous and non-metallic impurities.

Go to "krypton fluoride" and "argon fluoride", "neon fluoride" and "helium fluoride" only dry up.

Fluorine is the strongest non-metallic element, and the ability to capture electrons is super strong, and some noble gases with a large number of electron layers, the nucleus is far away from the outermost electron, and the absorption of bright can not attract the outermost electron, so it is attracted by fluorine to produce compounds.