The next section of the module deals with redox chemistry of the elements of Groups 1, 2 and 13.
The common oxidation states for these elements are given below.
| Group 1 | Li | Na | K | Rb | Cs | | Group 2 | Be | Mg | Ca | Sr | Ba | | Group 13 | B | Al | Ga | In | Tl |
| ns1 | +1 | +1 | +1 | +1 | +1 | | ns2 | +2 | +2 | +2 | +2 | +2 | | ns2 np1 | +3 | +3 | +3 | +3 | +3 |
| | 0 | 0 | 0 | 0 | 0 | | | 0 | 0 | 0 | 0 | 0 | | B and Al have ill-defined
negative oxidation states | +1 | +1 |
| | | | | | | | | | | 0 | 0 | 0 | 0 | 0 |
Consider the oxidation states in light of the definitions of oxidants and reductants.
- Oxidants are electron acceptors.
Thus an element in its maximum oxidation state can only act as an oxidant.
M+ for Group 1, M+2 for Group 2 and M+3 for Group 13 can act as oxidants.
- Reductants are electron donors.
Thus an element in its minimum oxidation state can only act as a reductant.
Thus all of the elements (0 oxidation state) for Groups 1 through 13 can act as reductants.
Therefore
intermediate oxidation states can act as
oxidants or reductants.
Thus In+ and Tl+ can either act as an oxidant or a reductant.