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

1 Answer
May 14, 2017

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.