For metals

(and Acids- Use H₂)

Remember metals are losers...this is a loser table.

If the metal is above the other metal it will be oxidized into the ION of that metal.  (Also would be the Anode)

Ex

Zn(s)-->  Zn²⁺ + 2e-

If the metal is lower on the table  the ION of the metal will be reduced to a smaller positive ion or the solid metal. (That metal would be the Cathode)

Ex.

Cu²⁺ --> Cu⁺ + e-

or

Cu²⁺ --> Cu(s) + 2e-

So in order for a metal to oxidize it needs to be above the other metal (ion) on the table. In order for a metal (ION) to be reduced, it need to be below the other metal on the table.

To be spontaneous (to eventually react without a time limit)

the solid metal is on top of the ion of the other metal.

For Nonmetals everything is reversed

Nonmetals are gainers.

The nonmetal element on top the is reduced to ions, the bottom would be an ion and is is oxidized into the element.

All this is single replacement rules using redox.

Reality Check....

If all else fails, 3 choices are above and 1 is below on the table....choose the 1. That is how multiple choice works.