Question

Which species undergoes a loss of electrons in this equation: `Mg(s) + 2Ag^+(aq) -> Mg^(2+)(aq) + 2Ag(s)`?

Answer 1

`Mg (s)`

Explanation:

This is an oxidation-reduction reaction, so one substance is oxidized (higher oxidation state, loss of electrons) and another is reduced (lower oxidation state, gains electrons).

In this reaction, `Mg (s)` with a net charge of `0` (oxidation state of `0`) reacts with a solution containing `Ag^+` ions. The products are `Mg^(2+) (aq)` and solid `Ag`. We can see that `Mg (s)` has been oxidized, since it's oxidation state raised from `0` to `+2`. Therefore, `Mg (s)` has lost electrons to become a cationic species.