oxide or oxides known as linking the different elements with oxygen.Almost all of these elements form compounds.Chloro, as well as other halogens, characterized in compounds positive oxidation state.All chlorine oxides are highly volatile substances, which is typical of oxides of halogens.Four known substance whose molecules contain chlorine and oxygen.
- gaseous compounds from yellow to reddish color with a characteristic smell (reminiscent of the smell of gas Cl2) - Chlorine oxide (I).Chemical Formula Cl2O.Melting point minus 116 ° C, the boiling point of + 2 ° C.Under normal conditions, its density is equal to 3.22 kg / m³.
- yellow or orange-yellow gas with a characteristic odor - chlorine oxide (IV).Chemical formula ClO2.Melting point minus 59 ° C, the boiling point plus 11 ° C.
- red-brown liquid - chlorine oxide (VI).Chemical Formula Cl2O6.Melting point plus 3,5 ° C, the boiling point plus 203 ° C.
- colorless, oily liquid - chlorine oxide (VII).Chemical Formula Cl2O7.Melting point minus 91,5 ° C, the boiling point plus 80 ° C.
chlorine monoxide oxidation state is one anhydride monobasic weak hypochlorous acid (HClO).Get him on the method of interaction Peluso mercuric oxide with chlorine gas in one of reaction equations: 2Cl2 + 2HgO → Cl2O + Hg2OCl2 or 2Cl2 + HgO → Cl2O + HgCl2.Conditions of these reactions are different.Chlorine oxide (I) is condensed at a temperature of minus 60 ° C because at higher temperatures it decomposes explosively, and in concentrated form explosive.Cl2O aqueous solution obtained by chlorination in water or alkaline earth carbonates of alkali metals.Oxide is highly soluble in water, forming hypochlorous acid: Cl2O + H2O ↔ 2HClO.Furthermore, it is also dissolved in carbon tetrachloride.
chlorine monoxide oxidation state 4 otherwise known dioxide.This material was dissolved in water, sulfuric acid and acetic acid, acetonitrile, carbon tetrachloride, and other organic solvents with increasing polarity which increases its solubility.In the laboratory, it is prepared by reacting potassium chlorate with oxalic acid: 2KClO3 + H2C2O4 → K2CO3 + 2ClO2 + CO2 + H2O.Since chlorine oxide (IV) is a volatile substance, it can not be stored in solution.For this purpose, silica is used, on whose surface in adsorbed form ClO2 can be stored for a long time, while unable to get rid of its impurities contaminating chlorine since it is not absorbed by the silica gel.In industrial conditions ClO2 produced by reduction of sulfur dioxide in the presence of sulfuric acid, sodium chlorate: 2NaClO3 + SO2 + H2SO4 → 2NaHSO4 + 2ClO2.Used as a bleach, e.g., paper or cellulose, etc., and for sterilization and disinfection of the various materials.
chlorine monoxide oxidation state +6 decomposes upon melting of the reaction equation: Cl2O6 → 2ClO3.Get chlorine oxide (VI) oxidizing ozone dioxide: 2O3 + 2ClO2 → 2O2 + Cl2O6.This oxide is capable of reacting with alkaline solutions and water.Thus reactions of disproportionation.For example, by reaction with potassium hydroxide: 2KOH + Cl2O6 KClO3 + → H2O + KClO4, obtained as a result of chlorate and potassium perchlorate.
higher oxides of chlorine is also called chlorine dioxide or dihlorogeptaoksid is a strong oxidant.It is capable of a stroke or explode when heated.However, this material is more stable, than oxides in the oxidation state of +1 and -4.Disintegration it to chlorine and oxygen is accelerated by the presence of lower oxides and the temperature rises from 60 to 70 ° C.Chlorine oxide (VII) capable of slowly soluble in cold water, is formed by the reaction of perchloric acid: H2O + Cl2O7 → 2HClO4.Get dihlorogeptaoksid gently heating perchloric acid with phosphorus pentoxide: P4O10 + 2HClO4 → Cl2O7 + H2P4O11.Cl2O7 also be obtained by using, instead of phosphoric anhydride oleum.
Section inorganic chemistry, which studies the halogen oxides, including oxides of chlorine, in recent years began to develop actively, since these compounds are energy intensive.They are capable of in the combustion chambers of jet engines give instant energy and in chemical power sources its rate of return can be adjusted.Another reason for the interest - it is possible to synthesize new groups of inorganic compounds, such as chlorine oxide (VII) is the founder of perchlorates.
