Chlorine monoxide

Chlorine monoxide, CI2O. M.p. — 116°C, b.p. 4 C, yellow-red gas (CI2 plus HgO), dissolves in water to give some HOCl. Dissociates to CI2 plus O2. 

Chlorine heptoxide is more stable than either chlorine monoxide or chlorine dioxide however, the CX C) detonates when heated or subjected to shock. It melts at —91.5°C, bods at 80°C, has a molecular weight of 182.914, a heat of vapori2ation of 34.7 kj/mol (8.29 kcal/mol), and, at 0°C, a vapor pressure of 3.2 kPa (23.7 mm Hg) and a density of 1.86 g/mL (14,15). The infrared spectmm is consistent with the stmcture O CIOCIO (16). Cl O decomposes to chlorine and oxygen at low (0.2—10.7 kPa (1.5—80 mm Hg)) pressures and in a temperature range of 100—120°C (17). It is soluble in ben2ene, slowly attacking the solvent with water to form perchloric acid it also reacts with iodine to form iodine pentoxide and explodes on contact with a flame or by percussion. Reaction with olefins yields the impact-sensitive alkyl perchlorates (18). 

Titanium oxide dichloride [13780-39-8] TiOCl2, is a yellow hygroscopic soHd that may be prepared by bubbling ozone or chlorine monoxide through titanium tetrachloride. It is insoluble in nonpolar solvents but forms a large number of adducts with oxygen donors, eg, ether. It decomposes to titanium tetrachloride and titanium dioxide at temperatures of ca 180°C (136). 

Hypochlorous Acid. Hypochlorous acid [7790-92-3] solutions are made for immediate use as chemical intermediates from chlorine monoxide or in bleaching and water disinfection by adjusting the pH of hypochlorite solutions. Salt-free hypochlorous acid solutions have been economically made... 

Anhydride of chloric acid, Cl20, is unknown. Oxides with even number of oxygen atoms are mixed anhydrides. Other chlorine oxides such as the radicals CIO, CIO, and CIO are known. Chlorine monoxide [14989-30-17, CIO, plays a key role in depletion of the o2one layer. 

Dichlorine monoxide is an intermediate in the manufacture of calcium hypochlorite. It has been used in sterilization for space appHcations (70) (see Sterilization techniques). Its use in the preparation of chlorinated solvents (71) and chloroisocyanurates has been described. Chlorine monoxide has been shown to be effective in bleaching of pulp (qv) and textiles (72—74). 

Hypochlorous acid and chlorine monoxide coexist in the vapor phase (78—81). Vapor pressure measurements of aqueous HOCl solutions show that HOCl is the main chlorine species in the vapor phase over <1% solutions (82), whereas at higher concentrations, CI2O becomes dominant (83). The equihbtium constant at 25°C for the gas-phase reaction, determined by ir and uv spectrophotometry and mass spectrometry, is ca 0.08 (9,66,67,69). The forward reaction is much slower than the reverse reaction. 

Carbon tetrachloride extracts chlorine monoxide but not HOCl from concentrated HOCl solutions. For the equilibrium, Cl2 0(aq) Cl2 0(CCl4), the partition coefficient at 0°C is 2.22 (55,84). 

TCCA can also be prepared by reaction of performed or in situ generated HOCl with CA slurry (23). Chlorine monoxide can also be used to prepare TCCA from finely powdered CA (24). 

The Montreal Protocol of July 1987 resulted in an international treaty in which the industrialized nations agreed to halt the production of most ozone-destroying chlorofluorocarbons by the year 2000. This deadline was hastily changed to 1996, in February 1992, after a U.S. National Aeronautics and Space Administration (NASA) satellite and high-altitude sampling aircraft found levels of chlorine monoxide over North America that were 5i % greater than that measured over Antarctica. 

P pentachloride causes ignition on contact with Al powder (Ref 2), while contact with a mixt of chlorine and chlorine dioxide usually results in expln, possibly due to formation of the more sensitive chlorine monoxide (Ref 5). Interaction with diphosphorus trioxide is rather violent at ambient temp (Ref 3) treatment with fluorine causes the entire mass to become incandescent (Ref 1). Ignition occurs when hydroxylamine is mixed with P pentachloride (Ref 6), while mixts with Mg oxide react with brilliant incandescence (Ref 7). The residue from interaction of P pentachloride and anilide in benz and removal of solvent and phosphoryl chloride in vacuo expld violently on admission of air (Ref 12). A soln of P pentachloride in nitrobenzene is stable at 110°, but begins to de-... 

Write the Lewis structure of each of the following reactive species, all of which are found to contribute to the destruction of the ozone layer, and indicate which are radicals (a) chlorine monoxide, CIO (b) dichloroperoxide, Cl—O—O—Cl ... 

Chlorine Monoxide, Dimethyl Ether, Chlorine Dioxide and Sulfur Dioxide.—The radial distribution curves for C120, (CH3)20, C102 and S02 (Fig. 8) show two peaks, the positions of the... 

Fig. 8.—Radial distribution curves for chlorine monoxide, dimethyl ether, chlorine dioxide.and sulfur dioxide.

The presence of PSCs also leads to the removal of nitrogen oxides (NO and NO2) from the gas phase. As long as there are significant amounts of NO2 it will react with chlorine monoxide (CIO) to produce chlorine nitrate (reaction 11). This species subsequently reacts with HQ on PSC surfaces to produce nitric acid (reaction 13), which remains in the condensed phase. Also, nitric acid directly condenses with water to form nitric acid trihydrate particles, hence it is not available to regenerate NO2 by photochemical processes, as it does when it is in the gas phase. 

In 1986 we proposed a cycle that involves the self reaction of chlorine monoxide radicals, without requiring free oxygen atoms to regenerate the chlorine atoms (14) ... 

Figure 5. Measurements of chlorine monoxide by Anderson et al (19) and of ozone by Proffitt et al (21) carried out in 1987 during the Airborne Antarctic Ozone Experiment.

Chlorine atoms react with O3 molecules to produce O2 and CIO, as shown by the molecular pictures in Figure 15-19. This is a catalytic process because chlorine monoxide reacts with an oxygen atom to produce a second O2... 

It also detonates in the presence of phosphorus, sulphur and carbon monoxide. With a chlorine/phosphorus pentachloride mixture the resulting detonation was explained by the hypothetical formation of chlorine monoxide. 

Chlorine monoxide reacts violently [1], and sulfur trioxide very violently [2], with dipheny lmercury. 

Contact between phosphorus pentachloride and a mixture of chlorine and chlorine dioxide (previously considered to be dichlorine trioxide) usually causes explosion, possibly owing to formation of the more sensitive chlorine monoxide. 

PPG [Pittsburgh Plate Glass Company] A process for making calcium hypochlorite. Hypochlorous acid and chlorine monoxide, generated by reacting chlorine and carbon dioxide with sodium carbonate monohydrate, are passed into lime slury. Invented in 1938 by I. E. Muskatt and G. H. Cady at the Pittsburgh Plate Glass Company. 

Chlorine-hydrogen hazards, 9 646 Chlorine Institute, 21 831 25 343 Chlorine market, in vinyl chloride manufacture, 25 646 Chlorine monofluoride, 13 123-124 Chlorine monoxide, 8 545t Chlorine oxygen acids/salts, 17 389t Chlorine pentafluoride, 13 125 Chlorine peroxide, oxidation state and stability, 8 545t... 

Butyl h3q)Ochlorite has been prepared by treatment of an alkaline solution of /-butyl alcohol with chlorine, - and a recent warning cautions against allowing the temperature to rise above 20° during this reaction. /-Butyl hypochlorite has been prepared in solution by shaking a solution of the alcohol in carbon tetrachloride, fluorotrichloromethane (Freon 11), and other solvents with aqueous hypochlorous acid. It has also been prepared by the action of chlorine on an aqueous /-butyl alcohol suspension of calcium carbonate, and by the action of chlorine monoxide on a carbon tetrachloride solution of the alcohol. ... 

Through the natural processes of the UV rays of the sun passing through this layer, the absorbs the rays and is broken down to molecules and O atoms. This process is reversible, and ozone (O ) is constantly being reformed from UV effects on However, the separation can be accelerated faster than the reformation of new by induction of other chemical gases into the ozone layer. Of particular concern is that chlorine from CFCs and from other sources, such as the ocean and volcanic eruptions, combines with atomic oxygen that is broken down from Oj by UV radiation. It then forms chlorine monoxide (CIO), which means the atomic oxygen is not available for reformation into O by UV radiation. Herein lie the potential problem and the controversy. 

Chlorine monoxide and CIF3O reacted slowly at room temperature (246) ... 

Chlorine monoxide is used as a selective chlorinating agent. 

Chlorine monoxide is prepared by passing chlorine gas over yellow mercuric oxide. It is stored below -80°C as a liquid or solid. 

Reaction with chlorine yields chlorine monoxide, CIO, and in aqueous solution or with chlorine water, the product is hypochlorous acid, HOCl ... 

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