In the following reactions first Identify the substance that is oxidized and the one that is reduced. Then identify the oxidizing and reducing agents.

A. 2Li (s) + F2 (g) - - > 2LiF (s)

B. Fe (s) + CuSO4 (aq) - - > FeSO4 (aq) + Cu (s)

A) In a, both the Li and the F start out with a neutral charge. When they react, the Li becomes positive and the F becomes negative. Becoming positive means losing electrons. Becoming negative means gaining electrons.

So the Li is oxidized and the F is reduced.

when you become negative you gain electrons=reduction

The atom that causes the reduction is the reducing agent, so since the Li caused the F to be reduced it is the reducing agent. And vice versa. The F is the oxidizing agent.

B) Fe is oxidized, but the element that is reduced is Cu. The charge must change for it to be oxidized or reduced. The SO4 is - 2 the whole time. Fe is the reducing agent and Cu is the oxidizing agent.

Whatever is oxidized is the reducing agent, and whatever is reduced is the oxidizing agent.