Learning objectives

The common oxidation states of the Group 1, 2 and

elements are given below with the most stable oxidation state marked with an asterisk (*). The most stable state is usually the naturally-ocurring one. These can be used to predict the redox reactivity of the elemental form and of ions/molecules containing these elements in combination with other elements.

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

Group 1

Group 2

Group 13

ns¹

+1*

ns²

+2*

ns² np¹

+3*

B and Al have ill-defined
negative oxidation states

+1*

On completion of the module, for Group 1, 2 and

elements, you should be able, on the basis of the given information

to identify whether a given oxidation state can act as a reductant, an oxidant or both
to identify the relative strengths of the various oxidation states as reductants or oxidants
to identify whether an element in a particular oxidation state will react with a common reductant (iodide ion) or a common oxidation (permanganate ion)