Definition of oxidation

1. Oxidation is gain of

2. Definition of Reduction Reduction is loss of

3. ExAmPle Ammonium Sulfate Ammonium SULFATE IS AN IONIC COMPOUND; 2 AMMONIUM ION AND 1 SULFATE ION

4. Hard tO Remember? LEO L ose E lectrons in O xidation G ain E lectrons in R eduction GER

5. VIDEO!! http://www.youtube.com/watch?v=dxlWtsFinTM ENJOY!

6. FUN F@CTS! - My name is BOND … Convalent Bond!:D - When an atom or molecule combines with oxygen, it tends to give up electrons to the oxygen in forming a chemical bond .

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8. Calculating oxidation states For example, in the reaction (unbalanced), MnO4- + H+ -> Mn2+ + H2O the oxidation of Mn goes from +7 to +2. Thus, Mn is reduced. In the following reaction (unbalanced), H2C2O4 + O2 -> CO2 + H2O the element C is oxidized , because its oxidation state changes from +3 to +4 in the reaction.

9. The sum of the oxidation states of all the in an ion is equal to the charge on the ion.  The oxidation state of an uncombined element is .That's obviously so, because it hasn't been either oxidised or reduced yet!  The sum of the oxidation states of all the atoms or ions in a neutral compound is zero .

10. First determine what the oxidation numbers of your known atoms are. we know the oxidation number for H is +1 . Then set this value equal to the overall net charge of the ion. In this case, it is +1. Our equation now looks like this: 1(4) = 1 , You use the multiplier of 4 to indicate that the ammonium ion has 4 hydrogen. Next substitute a variable in the equation for the missing oxidation number: +1(4) + N = +1 Solve for N. +1(4) + N = +1 N + 4 = +1 N = +1 - 4 N = -3 Thus, the oxidation number for Nitrogen is -3. 

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