Explain that oxidation can be modelled as the loss of electrons from a chemical species, and reduction can be modelled as the gain of electrons by a chemical species; these processes can be represented using balanced half-equations and redox equations (acidic conditions only).

Which balanced redox equation correctly represents the reaction between permanganate ions and iron(II) ions in acidic conditions?

A redox reaction occurs between zinc metal and acidified permanganate ions according to the unbalanced equation: \( \text{Zn}(s) + \text{MnO}_4^-(aq) + \text{H}^+(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Mn}^{2+}(aq) + \text{H}_2\text{O}(l) \) Explain which species is oxidised and which species is reduced in terms of electron transfer.

Which statement correctly describes the electron transfer in the redox reaction \(\text{Mg}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Mg}^{2+}(aq) + \text{Cu}(s)\)?