Identify the element oxidized and the element reduced, in this chemical equation:
H3AsO4+H2S ---> H3AsO3+S+H2O
The Attempt at a Solution
So I have learned the rules for oxidation numbers:
1. The oxidation number of an element is always 0 regardless of its subscript. This is true as long as they are not part of compound.
2. The oxidation number of a simple ion is the charge of the ion.
3.The oxidation number of oxygen in compounds is -2.
4. The oxidation number of hydrogen in compounds is +1.
5.Group 1 and group 2 metals always have a +1, and +2 value, respectively, in compounds.
6. All other oxidation numbers are assigned so that the net sum of the oxidation numbers equals the net charge of the molecule or complex ion.
So with what I know I can figure out the oxidation numbers for the oxygens and hydrogens in the chemical equation but how do I figure out the numbers for arsenic and sulfur?