For a given atom, if the oxidation state decreases, that means the atom has gained electrons, or has been reduced; likewise, if the oxidation state increases, that means the atom lost electrons, or has been oxidized.
So, let's take the equations one by one and try to see if the oxidation state of any of the atoms changes
Notice that the oxidation states of all the atoms involved in the reaction do not change. This means that this reaction is not a redox reaction.
Once again, the oxidation state of the oxygen atoms was not changed by the reaction, so you're not dealing with a redox reaction.
Notice that the oxidation state of zinc went from 0 on the reactants' side, to +2 on the products' side, which means that it has been oxidized.
At the same time, the oxidation state of copper went from +2 on the reactants' side, to 0 on the products' side, which means that it has been reduced.
Zinc metal lost two electrons to become
One species was oxidized and another was reduced, so this qualifies as a redox reaction.
The oxidation states of all the atoms remain unchanged by the reaction, so this cannot be considered a redox reaction.