The ionic equation for the displacement reaction that occurs when zinc metal is added to a solution of silver nitrate is shown below:
Zn (s)+2Ag+(aq)→Zn2+(aq)+2Ag (s) \text{Zn (s)} + 2\text{Ag}^{+}\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + 2\text{Ag (s)} Zn (s)+2Ag+(aq)→Zn2+(aq)+2Ag (s)This displacement reaction is classified as a redox reaction.
Explain, in terms of electron transfer, which species is oxidised and which species is reduced in this reaction.
110 exam-style questions on Edexcel GCSE Chemistry 5.1 Obtaining and using metals, covering 5.1.1 The reactivity series of metals, 5.1.2 Displacement reactions as redox reactions, 5.1.3 Extracting metals from ores by reduction, 5.1.4 Biological methods of metal extraction, 5.1.5 Resistance to oxidation and recycling metals, and 5.1.6 Life cycle assessment. Each one has a worked solution and a mark scheme showing where the marks go.