Predicting redox properties using the oxidation state hierarchy

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
ns¹	+1*	+1*	+1*	+1*	+1*
	0	0	0	0	0

Group 2	Be	Mg	Ca	Sr	Ba
ns²	+2*	+2*	+2*	+2*	+2*
	0	0	0	0	0

Group 13	B	Al	Ga	In	Tl
ns² np¹	+3*	+3*	+3*	+3*	+3
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.