What would you expect to see if a piece of copper metal is placed in a solution that contains nickel(II) ions? A. copper atoms become copper(II) ions
b. nickel ions become solid nickel
c. no reaction happens
d. a precipitate forms that contains copper and nickel ions

c. no reaction happens

Explanation:

Let me take your mind back to the idea of electrode potentials of metals. Remember that the more negative the electrode potential of a metal, the more reducing the metal is. Metals with more negative electrode potentials displace metals with less negative electrode potentials from their aqueous solutions.

The electrode potential of nickel is -0.25 V while that of copper is +0.34 V. Hence, copper is lower than nickel in the activity series and can not displace it from aqueous solution.

This implies that, if a piece of copper metal is placed in a solution that contains nickel(II) ions, no reaction happens .

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