Problem

In order to determine the position of three metals in a reactivity series, the metals were placed in different aqueous solutions of metal ions. The table summarizes whether or not a reaction occurred.

	$\text{Ag}^+\text{(aq)}$	$\text{Pb}^{2+}\text{(aq)}$	$\text{Ni}^{2+}\text{(aq)}$
Ag(s)	—	no reaction	no reaction
Pb(s)	reaction	—	no reaction
Ni(s)	reaction	reaction	—

Deduce the ionic equations for the three reactions that take place. Use this information to place the metals silver, lead and nickel in a reactivity series, with the strongest reducing agent first. Explain your reasoning.

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