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For example, in uranium(VI) fluoride the oxidation number of uranium is 6. Another example is the iron oxides. FeO is iron(II) oxide and Fe 2 O 3 is iron(III) oxide. An older system used prefixes and suffixes to indicate the oxidation number, according to the following scheme:
An atom (or ion) whose oxidation number increases in a redox reaction is said to be oxidized ... the inorganic prefixes (e.g. pent = 5, hept = 7) are used. Meth Eth
The number indicates the degree of oxidation of each element caused by molecular bonding. In ionic compounds, the oxidation numbers are the same as the element's ionic charge. Thus for KCl, potassium is assigned +1 and chlorine is assigned -1. [4] The complete set of rules for assigning oxidation numbers are discussed in the following sections.
Since this oxidation state is lower than the other possibility (Fe 3+), this compound is sometimes called ferrous oxide. For the compound, SnO 2 , the tin ion is Sn 4+ (balancing out the 4− charge on the two O 2− anions), and because this is a higher oxidation state than the alternative ( Sn 2+ ), this compound is termed stannic oxide .
The number of ligands coordinating is indicated by the prefixes di-, tri-, tetra- penta- etc. for simple ligands or bis-, tris-, tetrakis-, etc. for complex ligands. For example: For example: [CoCl(NH 3 ) 5 ]Cl 2 pentaamminechloridocobalt(3+) chloride where ammine (NH 3 )precedes chloride.
Element Negative states Positive states Group Notes −5 −4 −3 −2 −1 0 +1 +2 +3 +4 +5 +6 +7 +8 +9 Z; 1 hydrogen: H −1 +1: 1 2 helium: He 0 18
In the "Stock system", the oxidation states of some or all of the elements in a compound are indicated in parentheses by Roman numerals. [1] [2] Style
Only the cationic element (i.e. the element whose name appears unchanged in the compound name) is assigned its oxidation number. Except in rare cases (none at present), we do not assign the oxidation number in the anion : hence potassium permanganate not potassium manganate(VII) , sodium hypochlorite not sodium chlorate(I) .