Why does reduction always accompany oxidation and vice versa? We've all learnt that the reduction always accompanies oxidation and vice versa Why is this so? Why is it not possible that a species releases an electron and the electron just "floats around"? Is this related to the stability of a free electron?
If something is to be reduced then there must be a reducing agent present. Also if something is oxidized then there must be an oxidizing agent present. 

You must have a reducing agent or oxidizing agent present in order for a redox reaction to take place. An element can't just dislocate it's electrons. There must be an outside force present in order to do that.