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Chemistry Oxidation Reaction?
hey we are doing oxidation reactions in chemistry so in the reaction 2 H2O2(aq)--->2 H2O(L) + O2(g) what is oxidized and what is reduced, for me the numbers for electronegativity dont make any sense
1 Answer
- 1 decade agoFavorite Answer
***********memorize these rules*************
oxidation number rules
1. Elemental state= 0.
2. Monatomic ion equals the charge of the ion. (ex Na+ is +1 N3- is -3.)
3. Group IA +1 all compounds.
4. Group 2A +2 all compounds
5. Group 3A +3 all compounds few exceptions.
6. Hydrogen is +1 non-metal and metals -1.
7. Oxygen -1 in peroxides and -2 all other compounds.
8. Halogens group 7A elements. Fluorine -1 all compounds. Other Halogens in a compound is -1, except when that element is combined with O or a lighter halogen.
9. The sum of the O.N. of all of the atoms in a neutral compound is 0.
If an element has a -2 oxidation number this means it has got 2 more electrons than a element that is 0 and 3 more electrons then an element with a +1 oxidation number.
***********memorize these definitions*************
* Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom or ion.
* Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom or ion.
For your question:
The oxidation state of oxygen in hydrogen peroxide is -1. It can therefore be oxidized to O2 (zero oxidation state) or reduced to H2O or OH- (-2 oxidation state for oxygen). On the whole, hydrogen peroxide is a very powerful oxidizing agent and a poor reducing agent.
