To determine the reaction that can take place in the anode we have to follow the relationship below.
anode → oxidation → oxidation number increases
The rules for oxidation states are as follows:
A. General Rules:
1. For an atom in its elemental form (Zn, Cl2, C(graphite), etc.) O.S. = 0
2. For an ion (Li+, Al3+, etc.) O.S. = charge
B. Specific Rules:
1. Group 1A O.S. = +1
2. Group 2A O.S. = +2
3. Hydrogen O.S. = +1, with nonmetals
O.S. = –1 with metals and boron
4. Fluorine O.S. = –1
5. Oxygen O.S. = –1 in peroxides (X2O2, X = Group 1A)
O.S. = –1/2 in superoxides (XO2, X = Group 1A)
O.S. = –2 in other compounds
6. Group 7A O.S. = –1 (except when bonded to O)
Which transformation could take place at the anode of an electrochemical cell?
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