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When it was realized that some metals form two different binary compounds with the same nonmetal, the two compounds were often distinguished by using the ending -ic for the higher metal oxidation state and the ending -ous for the lower. For example, FeCl 3 is ferric chloride and FeCl 2 is ferrous chloride. This system is not very satisfactory ...
The oxidation states are also maintained in articles of the elements (of course), and systematically in the table {{Infobox element/symbol-to-oxidation-state}} See also [ edit ]
The "common" oxidation states of these elements typically differ by two instead of one. For example, compounds of gallium in oxidation states +1 and +3 exist in which there is a single gallium atom. Compounds of Ga(II) would have an unpaired electron and would behave as a free radical and generally be destroyed rapidly, but some stable radicals ...
Several elements show their highest oxidation state only in a few compounds, one of which is the fluoride; and some elements' highest known oxidation state is seen exclusively in a fluoride. For groups 1–5, 13–16 (except nitrogen), the highest oxidation states of oxides and fluorides are always equal. Differences are only seen in chromium ...
The oxidation states are also maintained in articles of the elements (of course), and systematically in the table {{Infobox element/symbol-to-oxidation-state}} See also [ edit ]
All of the Group 14 elements form compounds in which they are in the +4, predominantly covalent, oxidation state; even in the +2 oxidation state tin generally forms covalent bonds. [131] The oxides of tin in its preferred oxidation state of +2, namely SnO and Sn(OH) 2, are amphoteric; [132] it forms stannites in strongly basic solutions. [58]
Nickel can enter into metal oxygen clusters with other high oxidation state elements to form polyoxometalates. These may stabilize higher oxidation states of nickel, or show catalytic properties. Nonamolybdonickelate(IV), [NiMo 9 O 32] 6− can oxidize aromatic hydrocarbons to alcohols. [46]
The chemical formulas of the oxides of the chemical elements in their highest oxidation state are predictable and are derived from the number of valence electrons for that element. Even the chemical formula of O 4 , tetraoxygen , is predictable as a group 16 element .