Common Oxidation States
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11 Terms
Oxidation State
The hypothetical electrical charge an atom would have if all the bonds in a compound were completely ionic
Pure Elements
Any uncombined element by itself has an oxidation state of 0 (O₂, Na, Cl₂, S₈)
Monatomic Ions
The oxidation state is equal to the net charge of the ion (NA⁺ is +1, and Cl⁻ is -1)
Fluorine
Always -1 in compounds
Group 1 metals
Always +1 in compounds
Group 2 metals
Always +2 in compounds
Hydrogen
+1 when bonded to nonmetals, and -1 when bonded to metals
Oxygen
Usually -2 in compounds, except in peroxides (where it is -1) or when bonded to fluorine (where it is positive)
Neutral Compounds
The sum of all oxidation states for all atoms in a neutral molecule must equal 0
Polyatomic Ions
The sum of all oxidation states for all atoms in a polyatomic ion must equal the overall charge of that ion
Halogens (Group 17)
Usually -1 when not bonded to oxygen or a lighter halogen