Fluorine oxidation number

Xenon difluoride has been used to oxidize a number of antimony compounds [102, 109] in yields ranging from 73 to 98%. Elemental fluorine oxidized tris(pen-tafluorophenyl)stibine to tris(pentafluorophenyl)stibine difluoride in 98% yield [706]. Oxidative fluonnation of stibines has also been accomplished with iodine pentafluoride [707]. 

Certain elements have the same oxidation number in all or almost all their compounds. The Group 1 metals always exist as +1 ions in their compounds and hence are assigned an oxidation number of +1. By the same token, Group 2 elements always have oxidation numbers of +2 in their compounds. Fluorine always has an oxidation number of — 1. 

Oxidation A half-reaction in which there is an increase in oxidation number, 88 chromium, 548 electrolysis and, 498 fluorine, 557 halogens, 557-558 oxoacids, 568-570 oxoanions, 568-570 species strength, 506-507q transition metals, 546t zinc, 86-87... 

The oxidation number of all the halogens is - 1 unless the halogen is in combination with oxygen or another halogen higher in the group. The oxidation number of fluorine is —1 in all its compounds. 

The oxidation number of oxygen is —2 in most of its compounds. Exceptions are its compounds with fluorine (in which case, the previous statement takes precedence) and its occurrence as peroxides (022-), superoxides (02 ), and ozonides (03 ). 

Fluorine has a number of peculiarities that stem from its high electronegativity, small size, and lack of available d-orbitals. It is the most electronegative element of all and has an oxidation number of — 1 in all its compounds. Its high electronegativity and small size allow it to oxidize other elements to their highest oxidation numbers. The small size helps in this, because it allows several F atoms to pack around a central atom, as in IF7. 

CIF3 Fluorine is the more electronegative atom, so each fluorine atom has an oxidation number of-1 (Guideline 4). For the sum of the oxidation numbers to be zero (Guideline 2), chlorine must be +3. 

The more electronegative element will take the negative oxidation state, (a) The maximum oxidation state of sulfur is +6 the most common negative oxidation number of oxygen is -2. Therefore, it takes three oxygen atoms to balance one sulfur atom, and the formula is SO v (b) The maximum oxidation state of carbon is +4 the only oxidation number of fluorine in its compounds is - 1. Therefore, it takes four fluorine atoms to balance one carbon atom, and the formula is CF4,... 

Oxidation inhibitors, for lubricating oil and grease, 75 219-221 Oxidation number system, 7 7 392 Oxidation potential, of fluorine, 77 828 Oxidation process(es), 9 275. See also Dye oxidation advanced, 77 803... 

A nonmetal may adopt any oxidation number between the values predicted in the preceding two paragraphs. The only exceptions are fluorine, which is only -1 in compounds, and helium, neon, and argon, which have no known compounds. When there is a choice of oxidation states, there must be additional information available in order to allow you to choose the correct state. 

Problem 2.39 Give a True or False answer to each question and justify your answer, (a) Since in polyatomic anions XY[, (such as SO and BF, ), the central atom X is usually less electronegative than the peripheral atom Y, it tends to acquire a positive oxidation number, (ft) Oxidation numbers tend to be smaller values than formal charges, (c) A bond between dissimilar atoms always leads to nonzero oxidation numbers, (d) Fluorine never has a positive oxidation number. ... 

The tetrafluoroammonium cation (NF/) has high electronegativity (the oxidation number of nitrogen is + 5) and high kinetic stability (NF4+ is isoelectronic with CF4).15 -17 It has been shown that in anhydrous hydrogen fluoride, benzene and its derivatives are fluorinated by tetrafluoroammonium tetrafluoroborate with substitution of hydrogen by fluorine.15-17... 

Silver differs markedly from copper in forming few 0x3 compounds. One of these is silver oxynitratc or silvcrdl, III) nitrate which has the empirical formula AgO 145(1 03)3453, in which the average oxidation number of silver is 2.448, It is prepared by action of fluorine upon aqueous silver nitrate or is obtained as an anodic deposit by electrolysis of silver nitrate in dilute HNO3. 

Give the most common oxidation number for the following elements (a) fluorine (b) the alkaline earth metals (c) aluminum, as found in nature. 

For group VIIA atoms, the oxidation numbers of chlorine (Cl), bromine (Br), and iodine (I) are -1 except when they combine with oxygen (O) or Fluorine (F). 

Of all the elements, fluorine is the most reactive and the most electronegative (a measure of tendency to acquire electrons). In its chemically combined form, it always has an oxidation number of -1. Fluorine has numerous industrial uses, such as the manufacture of UF6, a gas used to enrich uranium in its fissionable isotope, uranium-235. Fluorine is used to manufacture uranium hexafluoride, SF6, a dielectric material contained in some electrical and electronic apparatus. A number of organic compounds contain fluorine, particularly the chlorofluorocarbons used as refrigerants and organofluorine polymers, such as DuPont s Teflon. 

Solutions Oxygen will be 2- as it is quite often. Potassium is located in group 1 and will have an oxidation number of 1+. Calcium is in group 2 and will have a charge of 2+. Hydrogen is bonded with a metal in a metal hydride and will have an oxidation number of 1-. Fluorine will have an oxidation number of 1-. Iron is a lone element and will have an oxidation state of zero. 

B When it has reacted, fluorine will have an oxidation number of 1-. 

The nitrogen atom, when uncombined, has 5 valence electrons. In the compound, the shared electrons are controlled by the fluorine atoms, so the nitrogen atom retains control of only the unshared pair of electrons. It controls only 2 electrons. Its oxidation state is 5 - 2 = -1-3. The uncombined fluorine atom has 7 valence electrons but in the compound, each fluorine atom controls 8, so its oxidation number is 7 - 8 = -1. 

Note that an oxidation number, like the charge on an ion, is assigned to each atom in a compound. Thus, each fluorine atom in NF3 has an oxidation number of 1. 

The oxidation number of oxygen in its compounds is generally -2 (except in peroxides, -1, superoxides, and its two compounds with fluorine). 

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