Fluorine water

Fluorine, Water Hydrogen chloride. Hydrogen peroxide Hydrogen peroxide. 

Several chapters dealing with the interaction of fluorine and fluorides with plants, animals and men can be also found in the series Advances in Fluorine Science Elsevier, Amsterdam (2006), Effects of fluorine emissions on plants and organisms by A.W. Davison and L.H. Weinstein (Vol. 1) Physiological effects of highly fluorinated waters by M. Pontie et al. (Vol. 2.). See also in the present book interaction between fluorinated biomaterials and the human body by C. Rey et al. and fluoride in dentistry by J. W. Nicholson and B. Czarnecka. 

Chemically, chlorine is extremely reactive, though less so than fluorine. Water absorbs about twice its volume of the gas at 25°. It is present in the solution partly... 

Oxidative fluorination Water only HF Very high temperatures Special reactors Energy HF handling One step with recycling of fluoride 80%... 

The results for the n-butane cracking test expressed in terms of pseudo-first-order rate constants are tabulated in Table VI. Fluorinated water-washed and fluorinated calcined samples were also tested. Water washing promotes removal of entrapped soluble fluoride compounds. The calcination was carried out on LZ-105 and erionite samples treated under relatively severe conditions. 

Less regularly used reagents are tert-hu y hydroperoxide, tf/Y-butyllithium, ozone. dioxiranes, fluorine/water/acetonitrile, or A, A -diethylhydroxylamine. Alkenes carrying a donor substituent can also be epoxidized with pcracids. Fluorinated allylic alcohols give, under Sharpless conditions, epoxides in good yield and enantiosclcclivity. ... 

In a study of the adverse effects of fluorinated drinking water (3), a few patients had non-specific ailments of varying duration, involving different systems. Severe headache, loss of strength, and abdominal cramps were noted, sometimes with polydipsia and polyuria. The symptoms disappeared promptly when fluorinated water was withdrawn, and reappeared immediately after rechallenge. 

Tooth enamel is composed of hydroxyapatite, whose simplest formula is Ca5(P04)30H, and whose corresponding ATjp = 6.8 X 10 . As discussed in the Chemistry and Life box on page 730, fluoride in fluorinated water or in toothpaste reacts with hydroxyapatite to form fluoroapatite, Ca5(P04)3F, whose = 1.0 X 10 . (a) Write the expression for the solubihty-constant for hydroxyapatite and for fluoroapatite. (b) Calculate the molar solubihty of each of these compounds. 

Ammonia, sodium, calcium sulfides and sulfates, chlorine, phenols, fluorine, water treatment chemicals, trace elements... 

Siher I) fluoride, AgF, is prepared by evaporation of a solution of excess Ag20 in HF after filtration or by heating anhydrous AgBF. The anhydrous salt is yellow hydrates are known, It is very soluble in water and in many organic solvents. Used as a mild fluorinating agent. On treatment of a solution with Ag a sub-fluoride, Ag2F, is formed. 

Antimony Ill) fluoride is a readily hydrolysable solid which finds use as a fluorinaling agent. Antimony(lll) chloride is a soft solid, m.p. 347 K. It dissolves in water, but on dilution partial hydrolysis occurs and antimony chloride oxide SbOCl is precipitated ... 

Ozone is formed in certain chemical reactions, including the action of fluorine on water (p. 323) and the thermal decomposition ofiodic(VII) (periodic) acid. It is also formed when dilute (about 1 M) sulphuric acid is electrolysed at high current density at low temperatures the oxygen evolved at the anode can contain as much as 30% ozone. 

Evidence for the solvated electron e (aq) can be obtained reaction of sodium vapour with ice in the complete absence of air at 273 K gives a blue colour (cf. the reaction of sodium with liquid ammonia, p. 126). Magnesium, zinc and iron react with steam at elevated temperatures to yield hydrogen, and a few metals, in the presence of air, form a surface layer of oxide or hydroxide, for example iron, lead and aluminium. These reactions are more fully considered under the respective metals. Water is not easily oxidised but fluorine and chlorine are both capable of liberating oxygen ... 

Both selenium hexafluoride and tellurium hexafluoride are more reactive than sulphur hexafluoride. Tellurium hexafluoride is slowly hydrolysed by water to telluric) VI) acid and on heating it decomposes to fluorine and the tetrafluoride. 

The tetrafluorides of the elements can be prepared. They are all less stable than the corresponding hexafluorides and are hydrolysed readily by water. They can all be used as fluorinating agents and sulphur tetrafluoride is extensively used for this purpose, for example the fluorination of organic carbonyl groups ... 

Fluorine occurs widely in nature as insoluble fluorides. Calcium fluoride occurs as jluospar or fluorite, for example in Derbyshire where it is coloured blue and called bluejohn . Other important minerals are cryolite NajAlFg (p. 141) and Jluorapatite CaFjSCaj (P04)2. Bones and teeth contain fluorides and some natural water contains traces. 

Chlorine reacts with most elements, both metals and non-metals except carbon, oxygen and nitrogen, forming chlorides. Sometimes the reaction is catalysed by a trace of water (such as in the case of copper and zinc). If the element attacked exhibits several oxidation states, chlorine, like fluorine, forms compounds of high oxidation state, for example iron forms iron(III) chloride and tin forms tin(IV) chloride. Phosphorus, however, forms first the trichloride, PCI3, and (if excess chlorine is present) the pentachloride PCI5. 

The oxidising power of fluorine is seen in its reaction with water in the liquid phase, water reacts to give hydrogen peroxide and some... 

Recent work indicates the existence offluoric I) acid. HFO, formed by the reaction of fluorine and water at 273 K. The acid forms colourless crystals, m.p. 156 K. is very unstable, and has, as expected, very strong oxidising properties. 

Halogens can act as ligands and are commonly found in complex ions the ability of fluorine to form stable complex ions with elements in high oxidation states has already been discussed (p. 316). However, the chlorides of silver, lead(Il) and mercury(l) are worthy of note. These chlorides are insoluble in water and used as a test for the metal, but all dissolve in concentrated hydrochloric acid when the complex chlorides are produced, i.e. [AgCl2] , [PbC ] and [Hg Clj]", in the latter case the mercury(I) chloride having also disproportionated. 

---