Reactivity of halogens. See what "fluorine" is in other dictionaries Fluorine interacts with water
Halogens are the most reactive group of elements in the periodic table. They are composed of molecules with very low bond dissociation energies (see Table 16.1), and their atoms have seven electrons in the outer shell and are therefore very electronegative. Fluorine is the most electronegative and most reactive non-metallic element in the periodic table. The reactivity of the halogens gradually decreases when moving towards the bottom of the group. The next section will examine the ability of halogens to oxidize metals and non-metals and show how this ability decreases from fluorine to iodine.
Halogens as oxidants
When gaseous hydrogen sulfide is passed through chlorine water, sulfur is precipitated. This reaction proceeds according to the equation
In this reaction, chlorine oxidizes hydrogen sulfide, taking away hydrogen from it. Chlorine also oxidizes to For example, if chlorine is stirred by shaking with an aqueous solution of sulfate, sulfate is formed
The oxidative half-reaction occurring in this case is described by the equation
As another example of the oxidative effect of chlorine, let us give the synthesis of sodium chloride by burning sodium in chlorine:
In this reaction, sodium is oxidized as each sodium atom loses an electron to form a sodium ion:
Chlorine attaches these electrons to form chloride ions:
Table 16.3. Standard electrode potentials for halogens
Table 16.4. Standard enthalpies of formation of sodium halides
All halogens are oxidizing agents, of which fluorine is the strongest oxidizing agent. Table 16.3 shows the standard electrode potentials for halogens. From this table it can be seen that the oxidative capacity of halogens gradually decreases towards the lower part of the group. This pattern can be demonstrated by adding a potassium bromide solution to a container of chlorine gas. Chlorine oxidizes bromide ions, resulting in the formation of bromine; this leads to the appearance of a color in a previously colorless solution:
Thus, one can make sure that chlorine is a stronger oxidizing agent than bromine. Likewise, if a solution of potassium iodide is mixed with bromine, a black precipitate is formed from solid iodine. This means that bromine oxidizes iodide ions:
Both reactions described are examples of displacement (displacement) reactions. In each case, the more reactive, that is, the more powerful oxidizing agent, the halogen displaces the less reactive halogen from the solution.
Oxidation of metals. Halogens oxidize metals easily. Fluorine easily oxidizes all metals except gold and silver. We have already mentioned that chlorine oxidizes sodium, forming sodium chloride with it. To give another example, when a stream of chlorine gas is passed over the surface of heated iron filings, a brown solid chloride is formed:
Even iodine is capable, albeit slowly, of oxidizing metals located in the electrochemical series below it. The ease of oxidation of metals by various halogens decreases when moving to the lower part of the VII group. This can be verified by comparing the energies of formation of halides from the initial elements. Table 16.4 shows the standard enthalpies of formation of sodium halides in order of displacement to the bottom of the group.
Oxidation of non-metals. With the exception of nitrogen and most noble gases, fluorine oxidizes all other non-metals. Chlorine reacts with phosphorus and sulfur. Carbon, nitrogen and oxygen do not react directly with chlorine, bromine or iodine. The relative reactivity of halogens to non-metals can be judged by comparing their reactions with hydrogen (Table 16.5).
Oxidation of hydrocarbons. Under certain conditions, halogens oxidize hydrocarbons.
Table 16.5. Reactions of halogens with hydrogen
childbirth. For example, chlorine completely removes hydrogen from the turpentine molecule:
The oxidation of acetylene can proceed with an explosion:
Reactions with water and alkalis
Fluorine reacts with cold water forming hydrogen fluoride and oxygen:
Chlorine dissolves slowly in water to form chlorine water. Chlorine water has a slight acidity due to the fact that disproportionation (see Section 10.2) of chlorine occurs in it to form of hydrochloric acid and hypochlorous acid:
Bromine and iodine disproportionate in water in a similar way, but the degree of disproportionation in water decreases from chlorine to iodine.
Chlorine, bromine and iodine also disproportionate in alkalis. For example, in cold dilute alkali, bromine disproportionates into bromide ions and hypobromite ions (bromate ions):
When bromine interacts with hot concentrated alkalis, disproportionation proceeds further:
Iodate (I), or hypoiodite ion, is unstable even in cold dilute alkalis. It spontaneously disproportionates with the formation of iodide ion and iodate (I) ion.
The reaction of fluorine with alkalis, like its reaction with water, is not similar to the analogous reactions of other halogens. In cold dilute alkali, the following reaction takes place:
In hot concentrated alkali, the reaction with fluorine proceeds as follows:
Analysis for halogens and with the participation of halogens
Qualitative and quantitative analysis for halogens is usually performed using a silver nitrate solution. For example
For the qualitative and quantitative determination of iodine, a starch solution can be used. Since iodine is very slightly soluble in water, it is usually analyzed in the presence of potassium iodide. This is done for the reason that iodine forms a soluble triiodide ion with the iodide ion
Solutions of iodine with iodides are used for the analytical determination of various reducing agents, for example, as well as some oxidizing agents, for example Oxidants shift the above equilibrium to the left, releasing iodine. Iodine is then titrated with thiosulfate (VI).
So let's do it again!
1. Atoms of all halogens have seven electrons in the outer shell.
2. To obtain halogens under laboratory conditions, oxidation of the corresponding hydrohalic acids can be used.
3. Halogens oxidize metals, non-metals and hydrocarbons.
4. Halogens disproportionate in water and alkalis, forming halide ions, hypohalogenic and halogenate (-ions.
5. Regularities of changes in the physical and chemical properties of halogens when moving to the bottom of the group are shown in table. 16.6.
Table 16.6. Regularities of changes in the properties of halogens with increasing atomic number
6. Fluorine has anomalous properties among other halogens for the following reasons:
a) it has a low bond dissociation energy;
b) in fluorine compounds, it exists only in one oxidation state;
c) fluorine is the most electronegative and most reactive of all non-metallic elements;
d) its reactions with water and alkalis differ from similar reactions of other halogens.
The hydrogen atom has the electronic formula of the outer (and only) electronic level 1 s 1 . On the one hand, by the presence of one electron at the outer electronic level, the hydrogen atom is similar to the atoms of alkali metals. However, he, like halogens, lacks only one electron to fill the external electronic level, since no more than 2 electrons can be located at the first electronic level. It turns out that hydrogen can be placed simultaneously in both the first and the penultimate (seventh) groups of the periodic table, which is sometimes done in different versions of the periodic system:
In terms of the properties of hydrogen as a simple substance, it still has more in common with halogens. Hydrogen, like halogens, is a non-metal and forms, like them, diatomic molecules (H 2).
Under normal conditions, hydrogen is a gaseous, low-activity substance. The low activity of hydrogen is explained by the high strength of the bond between the hydrogen atoms in the molecule, which requires either strong heating, or the use of catalysts, or both at the same time to break it.
Interaction of hydrogen with simple substances
with metals
Of the metals, hydrogen reacts only with alkaline and alkaline earth metals! Alkali metals include metals of the main subgroup Group I(Li, Na, K, Rb, Cs, Fr), and to alkaline earth metals - metals of the main subgroup of group II, except for beryllium and magnesium (Ca, Sr, Ba, Ra)
When interacting with active metals, hydrogen exhibits oxidizing properties, i.e. lowers its oxidation state. In this case, hydrides of alkali and alkaline earth metals are formed, which have an ionic structure. This reaction takes place by heating:
It should be noted that the interaction with active metals is the only case when molecular hydrogen H 2 is an oxidizing agent.
with non-metals
Of non-metals, hydrogen reacts only with carbon, nitrogen, oxygen, sulfur, selenium and halogens!
Carbon should be understood as graphite or amorphous carbon, since diamond is an extremely inert allotropic modification of carbon.
When interacting with non-metals, hydrogen can only perform the function of a reducing agent, that is, only increase its oxidation state:
Interaction of hydrogen with complex substances
with metal oxides
Hydrogen does not react with metal oxides that are in the range of metal activity up to aluminum (inclusive), however, it is able to reduce many metal oxides to the right of aluminum when heated:
with oxides of non-metals
Of the oxides of non-metals, hydrogen reacts when heated with oxides of nitrogen, halogens and carbon. Of all the interactions of hydrogen with oxides of non-metals, its reaction with carbon monoxide CO should be especially noted.
A mixture of CO and H 2 even has its own name - "synthesis gas", since, depending on the conditions, such popular industrial products as methanol, formaldehyde and even synthetic hydrocarbons can be obtained from it:
with acids
Hydrogen does not react with inorganic acids!
Of organic acids, hydrogen reacts only with unsaturated ones, as well as with acids containing functional groups capable of being reduced by hydrogen, in particular aldehyde, keto or nitro groups.
with salts
In the case of aqueous solutions of salts, their interaction with hydrogen does not occur. However, when hydrogen is passed over solid salts of some metals of medium and low activity, their partial or complete reduction is possible, for example:
Chemical properties of halogens
Chemical elements of group VIIA (F, Cl, Br, I, At), as well as the simple substances formed by them, are called halogens. Here and further in the text, unless otherwise stated, under halogens we mean just simple substances.
All halogens have a molecular structure, which leads to low melting and boiling points of these substances. Halogen molecules are diatomic, i.e. their formula can be written in general form as Hal 2.
It should be noted such a specific physical property iodine, as its ability to sublimation or, in other words, sublimation. Sublimation, is called the phenomenon in which a substance in a solid state does not melt when heated, but, bypassing the liquid phase, immediately passes into a gaseous state.
The electronic structure of the external energy level of an atom of any halogen has the form ns 2 np 5, where n is the number of the period of the periodic table in which the halogen is located. As you can see, up to the eight-electron outer shell, halogen atoms lack only one electron. From this, it is logical to assume the predominantly oxidizing properties of free halogens, which is also confirmed in practice. As you know, the electronegativity of non-metals decreases when moving down the subgroup, and therefore the activity of halogens decreases in the following order:
F 2> Cl 2> Br 2> I 2
Interaction of halogens with simple substances
All halogens are high active substances and react with most simple substances. However, it should be noted that fluorine, due to its extremely high reactivity, can react even with those simple substances with which other halogens cannot react. These simple substances include oxygen, carbon (diamond), nitrogen, platinum, gold, and some noble gases (xenon and krypton). Those. actually, fluorine does not react only with some noble gases.
The rest of the halogens, i.e. chlorine, bromine and iodine are also active substances, but less active than fluorine. They react with almost all simple substances except oxygen, nitrogen, carbon in the form of diamond, platinum, gold and noble gases.
Interaction of halogens with non-metals
hydrogen
When all halogens react with hydrogen, hydrogen halides with the general formula HHal. At the same time, the reaction of fluorine with hydrogen begins spontaneously even in the dark and proceeds with an explosion in accordance with the equation:
The reaction of chlorine with hydrogen can be initiated by intense ultraviolet irradiation or heating. Also proceeds with an explosion:
Bromine and iodine react with hydrogen only when heated, and at the same time, the reaction with iodine is reversible:
phosphorus
The interaction of fluorine with phosphorus leads to the oxidation of phosphorus to the highest oxidation state (+5). In this case, the formation of phosphorus pentafluoride occurs:
When chlorine and bromine interacts with phosphorus, it is possible to obtain phosphorus halides both in the + 3 oxidation state and in the +5 oxidation state, which depends on the proportions of the reactants:
In this case, in the case of white phosphorus in an atmosphere of fluorine, chlorine or liquid bromine, the reaction starts spontaneously.
The interaction of phosphorus with iodine can lead to the formation of only phosphorus triodide due to the significantly lower oxidizing ability than that of other halogens:
gray
Fluorine oxidizes sulfur to the highest oxidation state +6, forming sulfur hexafluoride:
Chlorine and bromine react with sulfur, forming compounds containing sulfur in the extremely unusual oxidation states of +1 and +2. These interactions are very specific, and the ability to write down the equations of these interactions is not necessary to pass the exam in chemistry. Therefore, the following three equations are given rather for informational purposes:
Interaction of halogens with metals
As mentioned above, fluorine is capable of reacting with all metals, even such inactive ones as platinum and gold:
The rest of the halogens react with all metals except platinum and gold:
Reactions of halogens with complex substances
Substitution reactions with halogens
More active halogens, i.e. the chemical elements of which are located higher in the periodic table are able to displace less active halogens from the hydrohalic acids and metal halides they form:
Similarly, bromine and iodine displace sulfur from sulfide and or hydrogen sulfide solutions:
Chlorine is a stronger oxidizing agent and oxidizes hydrogen sulfide in its aqueous solution not to sulfur, but to sulfuric acid:
Interaction of halogens with water
Water burns in fluorine with a blue flame in accordance with the reaction equation:
Bromine and chlorine react with water differently than fluorine. If fluorine acted as an oxidizing agent, then chlorine and bromine disproportionate in water, forming a mixture of acids. In this case, the reactions are reversible:
The interaction of iodine with water occurs to such an insignificant extent that it can be neglected and it can be assumed that the reaction does not proceed at all.
Interaction of halogens with alkali solutions
Fluorine, when interacting with an aqueous solution of alkali, again acts as an oxidizing agent:
The ability to write this equation is not required to pass the exam. It is enough to know the fact about the possibility of such interaction and the oxidative role of fluorine in this reaction.
Unlike fluorine, other halogens in alkali solutions disproportionate, that is, they simultaneously increase and decrease their oxidation state. In this case, in the case of chlorine and bromine, depending on the temperature, the flow through two different directions... In particular, in the cold, reactions proceed as follows:
and when heated:
Iodine reacts with alkalis exclusively according to the second option, i.e. with the formation of iodate, because hypoioditis is not stable not only when heated, but also at normal temperatures and even in the cold.
Fluorine
FLUORINE-a; m.[from the Greek. phthoros - death, destruction] Chemical element (F), light yellow gas with a pungent odor. Add to drinking water f.
fluorine(lat. Fluorum), a chemical element of the VII group of the periodic system, refers to halogens. Free fluorine consists of diatomic molecules (F 2); pale yellow gas with a pungent odor, t pl –219.699 ° C, t bale –188,200 ° C, density 1.7 g / l. Most reactive non-metal: reacts with all elements except helium, neon and argon. The interaction of fluorine with many substances easily turns into combustion and explosion. Fluorine destroys many materials (hence the name: Greek phthóros - destruction). The main minerals are fluorite, cryolite, fluorapatite. Fluorine is used to obtain organofluorine compounds and fluorides; fluoride is part of the tissues of living organisms (bones, tooth enamel).
FLUORINEFLUORINE (Latin Fluorum), F (read "fluorine"), chemical element with atomic number 9, atomic mass 18.998403. Natural fluorine consists of one stable nuclide (cm. NUCLID) 19 F. Configuration of outer electron layer 2 s 2
p 5
... In compounds, it exhibits only the oxidation state –1 (valence I). Fluorine is located in the second period in group VIIA of the periodic table of elements of Mendeleev, belongs to halogens (cm. HALOGENS).
The radius of the neutral fluorine atom is 0.064 nm, the radius of the F ion is 0.115 (2), 0.116 (3), 0.117 (4), and 0.119 (6) nm (the coordination number is indicated in parentheses). The sequential ionization energies of a neutral fluorine atom are 17.422, 34.987, 62.66, 87.2, and 114.2 eV, respectively. The electron affinity is 3.448 eV (the highest among the atoms of all elements). On the Pauling scale, the electronegativity of fluorine is 4 (the highest value among all elements). Fluorine is the most active non-metal.
Free fluorine is a colorless gas with a pungent suffocating odor.
Discovery history
The history of the discovery of fluorine is associated with the mineral fluorite (cm. FLUORITE), or fluorspar. The composition of this mineral is now known to correspond to the formula CaF 2, and it is the first substance containing fluorine to be used by humans. In ancient times, it was noted that if fluorite is added to the ore during metal smelting, the melting point of the ore and slags decreases, which greatly facilitates the process (hence the name of the mineral - from the Latin fluo - teku).
In 1771, Swedish chemist K. Scheele treated fluorite with sulfuric acid (cm. SCHEEELE Karl Wilhelm) prepared an acid, which he called "hydrofluoric". French scientist A. Lavoisier (cm. LAVOISIER Antoine Laurent) suggested that this acid contains a new chemical element, which he proposed to call "fluorem" (Lavoisier believed that hydrofluoric acid is a combination of fluorium with oxygen, because, according to Lavoisier, all acids must contain oxygen). However, he could not highlight the new element.
Behind the new element, the name "fluor" was consolidated, which is reflected in its Latin name. But long-term attempts to isolate this element in a free form were unsuccessful. Many scientists who tried to obtain it in free form died during such experiments or became disabled. These are the English chemists brothers T. and G. Knox, and the French J.-L. Gay lussac (cm. GAY-LUSSAC Joseph Louis) and L. J. Thénard (cm. TENAR Louis Jacques), and many others. G. Davy himself (cm. DEVI Humphrey), who was the first to receive free sodium, potassium, calcium and other elements, was poisoned as a result of experiments on obtaining fluorine by electrolysis and became seriously ill. Probably, under the impression of all these failures, in 1816 for the new element, although similar in sounding, but completely different in meaning, the name was proposed - fluorine (from the Greek phtoros - destruction, death). This name of the element is accepted only in Russian, the French and Germans continue to call fluorine "fluor", the British - "fluorine".
Even such an outstanding scientist as M. Faraday could not get fluorine in free form. (cm. FARADAY Michael)... Only in 1886 the French chemist A. Moissant (cm. Moissant Henri) Using the electrolysis of liquid hydrogen fluoride HF, cooled to –23 ° C (the liquid must contain a little potassium fluoride KF, which ensures its electrical conductivity), I was able to obtain the first portion of a new, highly reactive gas at the anode. In the first experiments to obtain fluorine, Moissan used a very expensive electrolyzer made of platinum and iridium. Moreover, each gram of the obtained fluorine "ate" up to 6 g of platinum. Later, Moissan began to use a much cheaper copper electrolyzer. Fluorine reacts with copper, but the reaction forms a thin film of fluoride, which prevents further destruction of the metal.
Being in nature
The fluorine content in the earth's crust is quite high and amounts to 0.095% by mass (much more than the closest analogue of fluorine in the group - chlorine (cm. CHLORINE)). Of course, due to its high chemical activity, free fluorine is not found. The most important minerals of fluorine are fluorite (fluorspar), as well as fluorapatite 3Ca 3 (PO 4) 2 CaF 2 and cryolite (cm. CRYOLITE) Na 3 AlF 6. Fluorine as an impurity is part of many minerals and is found in groundwater; v sea water 1.3 · 10 -4% fluorine.
Receiving
At the first stage of obtaining fluorine, hydrogen fluoride HF is isolated. Preparation of hydrogen fluoride and hydrofluoride (cm. HYDROFLUORIC ACID)(hydrofluoric) acid occurs, as a rule, along the way with the processing of fluorapatite into phosphoric fertilizers. The gaseous hydrogen fluoride formed during the sulfuric acid treatment of fluorapatite is then collected, liquefied and used for electrolysis. Electrolysis can be applied to both a liquid mixture of HF and KF (the process is carried out at a temperature of 15-20 ° C), and a KH 2 F 3 melt (at a temperature of 70-120 ° C) or a KHF 2 melt (at a temperature of 245-310 ° C) ...
In the laboratory, for the preparation of small amounts of free fluorine, one can use either heating MnF 4, in which fluorine is eliminated, or heating a mixture of K 2 MnF 6 and SbF 5:
2K 2 MnF 6 + 4SbF 5 = 4KSbF 6 + 2MnF 3 + F 2.
Physical and chemical properties
Under normal conditions, fluorine is a gas (density 1.693 kg / m 3) with a pungent odor. Boiling point –188.14 ° C, melting point –219.62 ° C. In the solid state, it forms two modifications: the a-form, which exists from the melting point to –227.60 ° C, and the b-form, which is stable at temperatures lower than –227.60 ° C.
Like other halogens, fluorine exists as diatomic F 2 molecules. The internuclear distance in a molecule is 0.14165 nm. The F 2 molecule is characterized by an abnormally low dissociation energy into atoms (158 kJ / mol), which, in particular, determines the high reactivity of fluorine.
The chemical activity of fluorine is extremely high. Of all the elements with fluorine, only three light inert gases do not form fluorides - helium, neon and argon. In all compounds, fluorine exhibits only one oxidation state, –1.
Fluorine reacts directly with many simple and complex substances. So, upon contact with water, fluorine reacts with it (it is often said that "water burns in fluorine"):
2F 2 + 2H 2 O = 4HF + O 2.
Fluorine reacts explosively on simple contact with hydrogen:
H 2 + F 2 = 2HF.
In this case, hydrogen fluoride gas HF is formed, which is infinitely soluble in water with the formation of a relatively weak hydrofluoric acid.
Fluorine interacts with most non-metals. So, when fluorine reacts with graphite, compounds of the general formula CF x are formed, when fluorine reacts with silicon, fluoride SiF 4, with boron, trifluoride BF 3. When fluorine interacts with sulfur, SF 6 and SF 4 compounds are formed, etc. (see Fluorides (cm. FLUORIDE)).
It is known big number fluorine compounds with other halogens, for example, BrF 3, IF 7, ClF, ClF 3 and others, bromine and iodine ignite in a fluorine atmosphere at ordinary temperatures, and chlorine interacts with fluorine when heated to 200-250 ° C.
Do not react with fluorine directly, except for the indicated inert gases, also nitrogen, oxygen, diamond, carbon dioxide and carbon monoxide.
Indirectly obtained nitrogen trifluoride NF 3 and oxygen fluorides O 2 F 2 and OF 2, in which oxygen has unusual oxidation states +1 and +2.
When fluorine interacts with hydrocarbons, their destruction occurs, accompanied by the production of hydrofluorocarbons of various compositions.
When heated slightly (100-250 ° C), fluorine reacts with silver, vanadium, rhenium and osmium. With gold, titanium, niobium, chromium and some other metals, the reaction with the participation of fluorine begins to proceed at temperatures above 300-350 ° C. With those metals, the fluorides of which are non-volatile (aluminum, iron, copper, etc.), fluorine reacts with noticeable speed at temperatures above 400-500 ° C.
Some higher metal fluorides, for example, uranium hexafluoride UF 6, are obtained by acting with fluorine or a fluorinating agent such as BrF 3 on lower halides, for example:
UF 4 + F 2 = UF 6
It should be noted that the already mentioned hydrofluoric acid HF corresponds not only to average fluorides such as NaF or CaF 2, but also acid fluorides - hydrofluorides such as NaHF 2 and KHF 2.
A large number of different organofluorine compounds have also been synthesized. (cm. Organofluorine Compounds), including the famous Teflon (cm. TEFLON)- material that is a polymer of tetrafluoroethylene (cm. TETRAFLUOROETHYLENE) .
Application
Fluorine is widely used as a fluorinating agent in the preparation of various fluorides (SF 6, BF 3, WF 6 and others), including compounds of inert gases (cm. NOBLE GASES) xenon and krypton (see. Fluorination (cm. FLUORINATION)). Uranium hexafluoride UF 6 is used to separate uranium isotopes. Fluorine is used in the production of Teflon and other fluoroplastics. (cm. Fluoroplastics), fluoroelastomers (cm. FLUOROSAUCHUKI), fluorine-containing organic substances and materials that are widely used in technology, especially in cases where resistance to aggressive environments, high temperatures, etc. is required.
Biological role
As a trace element (cm. MICROELEMENTS) fluorine is found in all organisms. In animals and humans, fluoride is present in bone tissue (in humans - 0.2-1.2%) and, especially, in dentin and tooth enamel. The body of an average person (body weight 70 kg) contains 2.6 g of fluorine; the daily requirement is 2-3 mg and is met mainly with drinking water. Lack of fluoride leads to dental caries. Therefore, fluoride compounds are added to toothpastes, sometimes they are added to drinking water. Excess fluoride in water, however, is also unhealthy. It leads to fluorosis (cm. FLUOROSIS)- changes in the structure of enamel and bone tissue, bone deformation. The maximum permissible concentration for the content of fluoride ions in water is 0.7 mg / l. Maximum concentration limit of gaseous fluorine in air is 0.03 mg / m 3. The role of fluoride in plants is unclear.
encyclopedic Dictionary. 2009 .
Synonyms:See what "fluorine" is in other dictionaries:
fluorine- fluorine, and ... Russian spelling dictionary
fluorine- fluorine / ... Morphemic-spelling dictionary
- (lat.Fluorum) F, a chemical element of the VII group of the periodic system of Mendeleev, atomic number 9, atomic mass 18.998403, refers to halogens. Pale yellow gas with a pungent odor, m.p.? 219.699 .C, b.p.? 188.200 .C, density 1.70 g / cm & sup3. ... ... Big Encyclopedic Dictionary
F (from the Greek phthoros death, destruction, Latin Fluorum * a. Fluorine; N. Fluor; F. fluor; and. Fluor), chem. element of group VII periodic. Mendeleev system, refers to halogens, at. n. 9, at. m. 18.998403. In nature, 1 stable isotope 19F ... Geological encyclopedia
- (Fluorum), F, chemical element of group VII of the periodic system, atomic number 9, atomic mass 18.9984; refers to halogens; gas, bp 188.2 ° C. Fluorine is used in the production of uranium, freons, medicines and others, as well as in ... ... Modern encyclopedia
19. Mechanism chemical reaction fluorine and water compounds
The equation for the reaction of the interaction of fluorine with water.
F 2 + H 2 O = 2 FH + O
Hydrogen in water removes "energy" (free photons) from the surface of fluorine. This "energy" appears on the hydrogen surface of the water. Those photons that fall into the region where hydrogen and oxygen are bonded to each other cause the bond between them to break. The water molecule disintegrates.
Simultaneously with this process, a gravitational bond is established between the hydrogen of water and fluorine. In those areas of the element fluorine, where hydrogen has removed free photons by its attraction, exposure occurs, and the Fluorine Attraction Field is manifested outside to a greater extent. This is the formation of a new chemical bond and new chemical compound- hydrogen fluoride. Water breaks down, fluorine combines with hydrogen, and oxygen is released.
It should be mentioned here that the fluorine elements are not at all combined with each other in pairs to form molecules. In gaseous fluorine, fluorine elements can be held against each other by very weak forces of attraction. In addition, each chemical element acts on the others with very weak Repulsive Forces. This situation occurs in any gaseous body.
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