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Oxidation Rules
Rules for assigning oxidation states in Gen. Chem. 1
Term | Definition |
---|---|
Free elements in their atomic state have an oxidation state = 0 Ex. Na = 0 and Cl2 = 0 | Rule 1 |
The oxidation state of a single ion is its charge | Rule 2 |
Fluoride ion has an oxidation state of 1- | Rule 3 |
Hydrogen’s oxidation state is almost always 1+ (H^+), except when combined with a metal it behaves as the hydride ion 1- (H^-) | Rule 4 |
Oxygen’s oxidation state is almost always 2- (O^2- ion); however, it can have oxidations states of -1 (O2^2- or O^- peroxide ion) or -1/2 (O^1/2- superoxide ion) | Rule 5 |
Sum of the oxidation states of all the atoms in a compound is zero. Ex. Na = +1 and Cl = -1, NaCl = (+1) + (-1) = 0 | Rule 6 |
Sum of the oxidation states of all the atoms in a poly atomic ion = the charge of the ion Ex. N = +5 and O = -2, NO3^- = (+5 ) + 3(-2) = -1 | Rule 7 |