Gary Horner Solutions for Chapter: Interaction, Exercise 14: Exercise 14

For following ionic reaction, ${\mathrm{Cu}}^{2+} + \mathrm{Mg} \to \mathrm{Cu} + {\mathrm{Mg}}^{2+}$, Balance the equation so the net charge is the same on each side of the equation.Construct the two half-equations from the ionic equation. Balance the charges for each half-equation by adding electrons. Identify the species that is being oxidized and the species being reduced.

For following ionic reaction, $\mathrm{Al} + {\mathrm{Fe}}^{3+} \to {\mathrm{Al}}^{3+} + \mathrm{Fe}$, Balance the equation so the net charge is the same on each side of the equation.Construct the two half-equations from the ionic equation. Balance the charges for each half-equation by adding electrons. Identify the species that is being oxidized and the species being reduced.

For following ionic reaction, ${\mathrm{Ag}}^{+} + \mathrm{Cd} \to {\mathrm{Cd}}^{2+} + \mathrm{Ag}$, Balance the equation so the net charge is the same on each side of the equation. Construct the two half-equations from the ionic equation. Balance the charges for each half-equation by adding electrons. Identify the species that is being oxidized and the species being reduced.

For following ionic reaction, $\mathrm{Sn} + {\mathrm{Pb}}^{2+} \to {\mathrm{Sn}}^{4+} + \mathrm{Pb}$, Balance the equation so the net charge is the same on each side of the equation. Construct the two half-equations from the ionic equation. Balance the charges for each half-equation by adding electrons. Identify the species that is being oxidized and the species being reduced.

Construct the half-equations for the rusting of iron.