Oxidation Rules

This is a list of rules that we learned in class that we must use for classifying the oxidized and reduced substance, which are also the oxidizing agent and reducing agent.
1) Each atom in a pure element has an oxidation number of 0
2) Monatomic ions have an oxidation number equal to the charge on the ion
3) Fluorine always has an oxidation number of -1 in compounds with other elements
4) Cl, Br, and I always have an oxidation number of -1 in compounds, except when combined with oxygen or fluorine
5) The oxidation number of H is +1 and 0 is -2 in most compounds
There are exceptions:
in compounds with metals, H is -1
in peroxides, O has a charge of -1
6) The sum of the oxidation numbers for atoms in a neutral compound is 0
(no charge is shown at end)
In a polyatomic ion, the sum must be equal to the ion charge

http://www.drcruzan.com/Images/Chemistry/OxidationNumbers/OxidationNumbersTable.png

Here are some references to go through the process of figuring them out:
Video: https://www.youtube.com/watch?v=81WdyqvLlVA
Website http://www.occc.edu/kmbailey/chem1115tutorials/oxidation_numbers.htm