(a) Define oxidation in terms of… | Chemistry

Question 1 Report

(a) Define oxidation in terms of electron transfer.

(b) Consider the following: Cu\(_{(s)}\) + 2Ag\(^{+}_{(Ag)}\) \(\to\) Cu\(^{2+}_{(aq)}\) + 2Ag\(_{(s)}\)

(i) State the species that is reduced

(ii) Write half-cell equation for each of the species.

Answer

Answer Details

(a) Oxidation (in terms of electron transfer)

Oxidation is the loss of electrons by an atom, ion or molecule.

(b) \( Cu_{(s)} + 2Ag^+_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)} \)

(i) The species that is reduced is Ag⁺, because it gains electrons (its oxidation state falls from +1 to 0).

(ii) Half-cell equations:

Oxidation: \[ Cu \to Cu^{2+} + 2e^- \]

Reduction: \[ 2Ag^+ + 2e^- \to 2Ag \]

(a) Define oxidation in terms of electron transfer. (b) Consider the following: Cu\(_{(s)}\) + 2Ag\(^{+}_{(Ag)}\) \(\to\) Cu\(^{2+}_{(aq)}\) + 2Ag\(_{(s)}\)...