Fluorine hydride

An overview is presented of plutonium process chemistry at Rocky Flats and of research in progress to improve plutonium processing operations or to develop new processes. Both pyrochemical and aqueous methods are used to process plutonium metal scrap, oxide, and other residues. The pyrochemical processes currently in production include electrorefining, fluorination, hydriding, molten salt extraction, calcination, and reduction operations. Aqueous processing and waste treatment methods involve nitric acid dissolution, ion exchange, solvent extraction, and precipitation techniques. 

Bromine pentafluoride Hydrogen-containing materials Chlorine Nitrogen compounds Chlorine trifluoride Hydrogen-containing materials Fluorine Hydrides Iodine Ammonia... 

Fluorine hydride (FH). The FH ground state (J S+) PEC calculations have been performed in the range of the internuclear distances Re [0.64, 4.0] A. The correlation-consistent aug-cc-pVTZ basis set [65, 66] has been used in the calculations. 

The high chemical reactivity of radicals is due to their open shells. The similarity between the chemical properties of carbon, nitrogen, oxygen, fluorine hydrides, and those of atoms with the same number of electrons is characteristic. For instance, the CH radical is chemically similar to the N atom CH2 and NH radicals are similar to the 0 atom CH3, NH2, OH radicals resemble the F atom, and finally CH4, NH3, H2O and HF molecules resemble, in a certain sense (in their inertness), the Ne atom. As radicals are chemically unsaturated, the activation energy for processes they are involved in is of the same order as that for atomic reactions. For this reason, the rates of these reactions are, as a rule, approximately the same as those of atomic processes. 

Figure 2.5 shows the boiling points of the hydrides in elements of Groups IV. V, VI and VII. Clearly there is an attractive force between the molecules of the hydrides of fluorine, oxygen and nitrogen... 

The element before carbon in Period 2, boron, has one electron less than carbon, and forms many covalent compounds of type BX3 where X is a monovalent atom or group. In these, the boron uses three sp hybrid orbitals to form three trigonal planar bonds, like carbon in ethene, but the unhybridised 2p orbital is vacant, i.e. it contains no electrons. In the nitrogen atom (one more electron than carbon) one orbital must contain two electrons—the lone pair hence sp hybridisation will give four tetrahedral orbitals, one containing this lone pair. Oxygen similarly hybridised will have two orbitals occupied by lone pairs, and fluorine, three. Hence the hydrides of the elements from carbon to fluorine have the structures... 

Acetylene Bromine, chlorine, brass, copper and copper salts, fluorine, mercury and mercury salts, nitric acid, silver and silver salts, alkali hydrides, potassium metal... 

Chlorine Ammonia, acetylene, alcohols, alkanes, benzene, butadiene, carbon disulflde, dibutyl phthalate, ethers, fluorine, glycerol, hydrocarbons, hydrogen, sodium carbide, flnely divided metals, metal acetylides and carbides, nitrogen compounds, nonmetals, nonmetal hydrides, phosphorus compounds, polychlorobi-phenyl, silicones, steel, sulfldes, synthetic rubber, turpentine... 

Industrially, chlorine is obtained as a by-product in the electrolytic conversion of salt to sodium hydroxide. Hazardous reactions have occuned between chlorine and a variety of chemicals including acetylene, alcohols, aluminium, ammonia, benzene, carbon disulphide, diethyl ether, diethyl zinc, fluorine, hydrocarbons, hydrogen, ferric chloride, metal hydrides, non-metals such as boron and phosphorus, rubber, and steel. 

A fluorinated keto ester reacts as an electrophile with hydrides, giving a hydroxy ester in a highly stereoselective reduction [30] (equation 25). 

Although modern chemistry allows development of even more effective rocket propellants, energy efficiency is not the only consideration factor. For example, fluorine and its derivatives arc better oxidizers than oxygen, but their extreme toxicity make them environmentally dangerous. The same concerns prevent the use of beryllium hydride—an excellent fuel that combines high density with the energy efficiency comparable to liquid hydrogen. 

Uses. n-Pentane has found use as an anesthetic an expl suppressant when mixed with a halogen-ated hydrocarbon and included in aircraft fuel (Ref 13) a jet engine fuel (Ref 16a) as a base for synthetic rubbers and plastics a parent compd for the formation of nitropentanes and azido nitro pentanes used as expls and propints (Refs 15a, 15b 21a) also, as a parent compd for fluorine-contg resin binders which impart both thermal stability and, in conjunction with metal hydrides, high impulse to solid propints (Ref 15b)... 

Silicon, like carbon, is relatively inactive at ordinary temperatures. But, when heated, it reacts vigorously with the halogens (fluorine, chlorine, bromine, cmd iodine) to form halides and with certain metals to form silicides. It is unaffected by all acids except hydrofluoric. At red heat, silicon is attacked by water vapor or by oxygen, forming a surface layer of silicon dioxide. When silicon and carbon are combined at electric furnace temperatures of 2,000 to 2,600 °C (3,600 to 4700 °F), they form silicon carbide (Carborundum = SiC), which is an Importeint abrasive. When reacted with hydrogen, silicon forms a series of hydrides, the silanes. Silicon also forms a series of organic silicon compounds called silicones, when reacted with various organic compounds. 

Mellor, 1940, Vol. 2, 12, 483 1956, Vol. 2, Suppl. 1, 56 1941, Vol. 3, 73 Copper hydride, potassium hydride and sodium hydride all ignite on contact with fluorine at ambient temperature. 

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