Xenon fluoride products

Unless a deficiency of xenon fluoride was used in the preparation at 0°C or below, the title product exploded violently on warming to ambient temperature. 

Xenon fluorides are also excellent fiuorinaiors. though not so reactive as KiF2 (see below). They are often dean." the only by-product being xenon gas ... 

Direct fluorination of aromatic rings is so exothermic that a tarry mixture of products is obtained. Reaction of benzene with the xenon fluorides, XeF2 or XeF4, does give fluorobenzene, but the mechanism is probably free radical rather than polar.137... 

In 1962, Neil Bartlett produced a reaction of xenon, the first reported reaction of any noble gas. Later it was found that fluorine reacts directly with xenon to give one of three xenon fluorides, depending on temperature and pressure. Because all the products and the reactants are colorless, the easiest way to tell that a reaction is occurring is the drop in the total pressure of the system as the number of moles of gas decreases. For example,... 

Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400°C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25°C. The reaction vessel is heated to 400°C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container where the pressure of F2 at 25°C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product ... 

Xenon difluoride is easy to make, and relative to other xenon fluorides, safe to handle. It is therefore attractive as a reagent. Because of its low average bond energy ( 30 kcal. mole- ) and the "inertness of its reduction product (Xe) it has considerable potential in oxidative fluorinations. However, others have shown that the compound has considerable kinetic stability, e.g. it may be retrieved from aqueous solution in which it is thermodynamically unstable towards hydrolysis. 

Boldface type is used to indicate individual preparations described in detail, whether for numbered syntheses or for intermediate products (in the latter case, usually without stating the purpose of the preparation). Group headings, as Xenon fluorides, are in lightface type unless all the formulas under them are boldfaced. 

The three xenon fluorides, XeF2, XeF4, and XeFe, can all be prepared by direct reaction of xenon and fluorine gases under pressure, but conditions must be carefully controlled to obtain the desired product. Xenon tetrafluo-ride is produced in nearly quantitative amounts when a 1 5 mixture of Xe and F2 is heated to 400°C under 6 atm pressure. Xenon difluoride is formed by the same procedure if xenon is in excess. The preparation of XeFe requires 1 20 volume mixtures of xenon and fluorine at 250-300°C and 50-60 atm pressure. 

Three stable oxyfluorides have been characterized XeOF4 and Xe02F2 with Xe in the -1-6 oxidation state, and Xe03F2 with Xe in the - -8 oxidation state. These are obtained by controlled hydrolysis of xenon fluorides or by fluorination of xenon trioxide. The oxyfluoro anions, [XeOgF] and [(XeOF4)3F] result when the hydrolysis products of XeOs and XeOF4 are treated with F. ... 

Xenon difluoride, XeF2, is hydrolyzed (broken up by water) in basic solution to give xenon, fluoride ion, and O2 as products. Write a balanced equation for the reaction. 

Xenon reacts directly only with F2. Three different xenon fluorides can be produced by heating xenon and fluorine in nickel reaction vessels, but the product obtained depends on the experimental conditions, as summarized below ... 

All the xenon fluorides react with water to form various products. For example, in aqueous solution, xenon hexafluoride is first hydrolyzed to xenon oxide tetrafluoride, XeOp4, which is further hydrolyzed to xenon trioxide. The reactions are as follows ... 

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