Write net ionic equations for these reactions :
Cu^2+ + Fe ->
Hg^2+ + Fe->
Fe^3+ +Fe->
Pb^2+ +Fe->
Ag^+ + Fe->
and then the same but instead of Fe, addition of Cu to the six solution that I wrote before.. What ions are reacting in each case? please help me with this..
Look at the activity series of metals. A metal will displace any ION below it.
http://en.wikipedia.org/wiki/Reactivity_series
Along with what DrBob said, keep in mind that a more reactive metal will lose electrons (and thus become ions) when in the presence of a less reactive metal. These less reactive metals (the chart on wikipedia shows them as at the bottom) will thus steal any electrons needed in order to maintain a net charge of 0.
This is why gold never seems to diminish or lose its luster in comparison to other metals. It will steal ions from any metal nearby in order to keep from oxidizing, whereas other metals will oxidize (lose electrons -> increase charge #), or as we tend to know it, rust.
To write the net ionic equations, we need to first determine the chemical formulas of the reactants and products involved in each reaction. We will then balance the equations and remove any spectator ions to obtain the net ionic equations.
1. Cu^2+ + Fe -> (potential products: Cu + Fe^2+)
The ions reacting are Cu^2+ and Fe. Balancing the equation, we have:
Cu^2+ + Fe -> Cu + Fe^2+
The net ionic equation is:
Cu^2+ + Fe -> Cu + Fe^2+
2. Hg^2+ + Fe -> (potential products: Hg + Fe^2+)
The ions reacting are Hg^2+ and Fe. Balancing the equation, we have:
Hg^2+ + Fe -> Hg + Fe^2+
The net ionic equation is:
Hg^2+ + Fe -> Hg + Fe^2+
3. Fe^3+ + Fe -> (potential product: Fe^2+)
The ions reacting are Fe^3+ and Fe. Balancing the equation, we have:
Fe^3+ + Fe -> Fe^2+
The net ionic equation is:
Fe^3+ + Fe -> Fe^2+
4. Pb^2+ + Fe -> (potential products: Pb + Fe^2+)
The ions reacting are Pb^2+ and Fe. Balancing the equation, we have:
Pb^2+ + Fe -> Pb + Fe^2+
The net ionic equation is:
Pb^2+ + Fe -> Pb + Fe^2+
5. Ag^+ + Fe -> (potential products: Ag + Fe^2+)
The ions reacting are Ag^+ and Fe. Balancing the equation, we have:
Ag^+ + Fe -> Ag + Fe^2+
The net ionic equation is:
Ag^+ + Fe -> Ag + Fe^2+
Now, let's consider the reactions involving the addition of Cu to each of the solutions:
1. Cu^2+ + Cu -> (potential product: Cu^+)
The ions reacting are Cu^2+ and Cu. Balancing the equation, we have:
Cu^2+ + Cu -> Cu^+
The net ionic equation is:
Cu^2+ + Cu -> Cu^+
2. Hg^2+ + Cu -> (potential products: Hg + Cu^+)
The ions reacting are Hg^2+ and Cu. Balancing the equation, we have:
Hg^2+ + Cu -> Hg + Cu^+
The net ionic equation is:
Hg^2+ + Cu -> Hg + Cu^+
3. Fe^3+ + Cu -> (potential product: Fe^2+)
The ions reacting are Fe^3+ and Cu. Balancing the equation, we have:
Fe^3+ + Cu -> Fe^2+
The net ionic equation is:
Fe^3+ + Cu -> Fe^2+
4. Pb^2+ + Cu -> (potential products: Pb + Cu^+)
The ions reacting are Pb^2+ and Cu. Balancing the equation, we have:
Pb^2+ + Cu -> Pb + Cu^+
The net ionic equation is:
Pb^2+ + Cu -> Pb + Cu^+
5. Ag^+ + Cu -> (potential products: Ag + Cu^+)
The ions reacting are Ag^+ and Cu. Balancing the equation, we have:
Ag^+ + Cu -> Ag + Cu^+
The net ionic equation is:
Ag^+ + Cu -> Ag + Cu^+
In each case, the ions that are reacting are indicated in the chemical equations.