Which species undergoes a loss of electrons in this equation: $M g (s) + 2 A g^{+} (a q) \to M g^{2 +} (a q) + 2 A g (s)$ $Mg(s) + 2Ag^+(aq) -> Mg^(2+)(aq) + 2Ag(s)$ ?

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Which species undergoes a loss of electrons in this equation: $M g (s) + 2 A g^{+} (a q) \to M g^{2 +} (a q) + 2 A g (s)$ $Mg(s) + 2Ag^+(aq) -> Mg^(2+)(aq) + 2Ag(s)$ ?

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Answer 1 · 2017-05-14T01:17:45

$M g (s)$ $Mg (s)$

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

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Which species undergoes a loss of electrons in this equation: $M g (s) + 2 A g^{+} (a q) \to M g^{2 +} (a q) + 2 A g (s)$ $Mg(s) + 2Ag^+(aq) -> Mg^(2+)(aq) + 2Ag(s)$ ?

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Explanation:

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Which species undergoes a loss of electrons in this equation: Mg(s)+2Ag+(aq)→Mg2+(aq)+2Ag(s)Mg(s) + 2Ag^+(aq) -> Mg^(2+)(aq) + 2Ag(s)?

1 Answer

Explanation:

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Which species undergoes a loss of electrons in this equation: $M g (s) + 2 A g^{+} (a q) \to M g^{2 +} (a q) + 2 A g (s)$ $Mg(s) + 2Ag^+(aq) -> Mg^(2+)(aq) + 2Ag(s)$ ?