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

1 Answer
May 14, 2017

Answer:

#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.