1. The Activity Series

2. Energy States of Valence Electrons
Each electron in each orbital of atoms has a specific energy
Valence electrons always have the highest energy;
In metals, valence electrons have very high energy, non-metals, less so.
The metals have low ionization energy because their valence electrons are in high energy states.

3. Active Metals
The most active metals will spontaneously give electrons to the ions of less active metals
The valence electrons are “looking” for an orbital of lower energy; they will give off a photon and “drop” into an orbital around the less active metal.

4. The Activity Series The most active metals are on top
The least active metals are on bottom
The metal above will donate electron(s) spontaneously to the ion of the metal below.
The metal below will not sponateously give up its valence electrons to the ion of the metal above.

5. Using the Activity Series
For example,
Li + Ba2+ 
Barium is below lithium, the reaction happens spontaneously.
Mg + K+ 
Potassium ion is above Mg, and will not receive electrons; the reaction is non-spontaneous

6. Non-Metals and Table J
The most active non-metals are found at the top right corner of the periodic table..
The most active non-metals gain electrons – they don’t lose them!

7. Halogens and Table J
The more active non-metal will take electrons from the ion of the less active metal:
F2 + 2Cl- 
For the opposite reaction, nothing happens:
Cl2 + 2F- 

8. Mg + H+ 
Ag + H+ 
Zn + Ca2+ 
F2 + Br- 
Br2 + F- 
Sr + Cu2+ 
Pb + Au3+ 
Cs + Fe3+ 
Au + Ag+ 
Cu + Au3+ 

9. Lab 19: Activity Series of Metals
In the first set of reactions you will add acid to a series of metals.
You will see some differences in the ability of metals to reduce hydrogen ions to hydrogen gas.

10. Find Fe, Cu, Mg, and Zn Where is acid (H+) on the table?
Why is hydrogen on a list of metals???
Remember, one of the properties of acids is that they are corrosive – they oxidize most metals.

11. What is your prediction?
Zn + HCl (aq) 
Cu + HCl (aq) 
Fe + HCl (aq) 
Mg + HCl (aq) 

12. Part 1 The effect of adding acid to metals
Materials
Well plate, dropper bottles of HCl, Mg(NO3)2 , FeCl3, Zn(NO3)2, CuSO4, magnesium, copper, iron, and zinc filings
Procedure
Add 1 “squirt” of HCl into a well plate.
Add a small scoop of Zn filings to the well and observe any reaction that occurs. Record your observations in Table 1 on your answer sheet.
Repeat step 2 with each of the other metals.

13. Reaction of metals with acid
Write the oxidation half reaction for each reaction.
If there is no reaction, you leave the box empty.
Note that for the polyvalent metals, Fe and Cu, the highest oxidation number is more common and is assumed to have occurred here.

14. Oxidation half-reaction
Metal
Reaction (y/n)
Oxidation half-reaction Fe Cu Zn Mg

15. Questions: Acids and Metals
What metals react with the acid and which did not? How could you tell?
Write the reduction half reaction that is common for all of the metals that reacted in the box below.

16. Write balanced chemical equations for each of the three reactions that occurred.

17. Which metals react most vigorously with the acid
Which metals react most vigorously with the acid? What happened to the metals that seemed to disappear?
What do you think will happen to the pH of the solution as the reaction proceeds? How could you test your prediction?
For any metal that does not react with the acid, explain why using Table J to justify your answer.

18. Part 2: Metals and Metal Ions
In the second set of reactions, you will study combinations of metals and ions, seeing which ones react spontaneously and which ones do not.
For both sets of experiments, you can use Table J to predict the results beforehand or explain your experimental results.

19. Part 2 Single Replacement Reactions of Various Metals
You have been supplied with solutions of metal compounds and small grains of the metals as a pure element.
For example, you have a solution of a copper salt that will supply you with Cu2+(aq) in one test tube and 1 ml of Zn2+(aq) in another.
Put a piece of zinc in the Cu2+(aq) and a piece of copper in the Zn2+(aq).
Note that the Zn begins to discolor. This is because metallic copper is being deposited on the zinc. What you cannot see is the zinc going into solution.

20. As the copper is deposited:Cu2+(aq) + 2e-  Cuo(s)
The zinc is dissolved: Zno(s)  Zn2+(aq) + 2e-

21. The other tube
Look at the other test tube. There doesn’t seem to be anything happening. There isn’t.
This is because reactions that are spontaneous in one direction are never spontaneous in the reverse direction.
In this case, the spontaneous reaction was:

22. Part 2. Single Replacement Reactions with Two Metals
Table 2. Metal-Ion Redox reactions  R = reaction NR = no reaction
Mg2+
Cu2+
Fe3+
Zn2+
Mgo *
Cuo NR
Feo
Zno R

23. Oxidation half reaction
Reduction half-reaction
Balanced net ionic equation
Zn  Zn2+ + 2e-
Cu2+ + 2e-  Cu
Zn + Cu2+  Zn2+ + Cu

24. Which metal seemed to be the least reactive
Which metal seemed to be the least reactive? Explain each of your “No Reactions” using Table J.
What happens when you add a metal to a solution containing its ion?
Each of the solutions used in this lab are electrolytes. Using your knowledge of atomic structure and properties, explain why this is so.

25. Assign oxidation numbers to the solutes of the solutions used and name the compounds they contain:
Compound Name
HCl(aq)
FeCl3
Mg(NO3)2
Zn(NO3)2
CuSO4

26. Several of these compounds have to be named using roman numerals, while others do not. Explain why, using specific examples.

27. Using Table J, predict whether or not oxidation-reduction will happen spontaneously, or not (S or NS).
a) Zn and Li ______ b) Ag and H+ _________
c) Mg and Al3+ ______ d) Co and Fe3+ _________
e) Pb and Cu2+ _______ f) Na and Ca2+ _________
g) Ba and Mn2+ _______ h) Sr and K+ _________

28. According to Reference Table J, which atom-ion pair will react spontaneously?
Ag + Au3+
Pb + Co2+
Ni + Al3+
Zn + Ca2+

29. According to Reference Table J, which metal will react spontaneously with Ag+ ions, but not with Zn2+ ions? Cu Au Al Mg

30. Which metal will react with hydrochloric acid and produce H2(g)?Au Cu Mg Hg