1. Single Replacement Reactions (p. 6-7 in your notes)
There are three subgroups of single replacement reactions:
A. One metal replaces another metal in an ionic compound A + BX  AX + B
BX and AX are generally ionic compounds and A and B are metals
Mg (s) + CuSO4 (aq)  MgSO4 (aq) + Cu (s)
Fe (s) + CuSO4 (aq)  FeSO4 (aq) + Cu (s)

2. Single Replacement Reactions (p. 6-7 in your notes)
B. One halogen replaces another halogen in an ionic compound Y2 + AX  AY + X2
AX and AY are ionic compounds and X and Y are halogens
F2 (g) + 2NaCl (aq)  2NaF (aq) + Cl2 (g)
Cl2 (g) + CaBr2 (g)  CaCl2 (aq) + Br2 (l)

3. Single Replacement Reactions (p. 6-7 in your notes)
C. One metal replaces hydrogen in an acid A + HZ  H2 + AZ
A is a metal, H is hydrogen and Z is any anion.
Zn (s) + 2HCl (aq)  H2 (g)+ ZnCl2 (aq)
2Al (s) + 3H2SO4 (aq)  3H2 (g) + Al2(SO4)3 (aq)

4. A note about Diatomic Elements
Remember! There are seven (7) elements that come in pairs if they are not bonded to something else.
These elements are so reactive that you never find just one atom of them, if they aren’t attached to something else, they bond to another one of themselves.
Those 7 elements are:
H O N Cl Br I F
Or, better…
H2 O2 N2 Cl2 Br2 I2 F2
Which Diatomic elements are halogens?

5. Please find Table N in your data book
Table N can be used to determine if a single replacement reaction will happen or not.
Metals higher in the table will be replaced by metals lower in the table. (strong metals are on the bottom)
Halogens higher in the group will replace halogens lower in the group (F2 will replace all the other halogens.) (strong halogens are on the top)

6. What about Hydrogen?
In ionic compounds, hydrogen almost always makes a positive charge (these are called acids).
Thinking about this, does that mean it will behave more like a metal or a halogen in single replacement reactions?
Please find hydrogen on Table N.
What is one metal that can “kick out” hydrogen from an acid?

7. Try a few Pb (s) + CuSO4 (aq)  The final balanced equation is:
What are the two metals involved in this reaction?
Lead and copper (II) (remember how to figure out the charge on copper?)
Find both of those on Table N – which is closer to the bottom?
Pb (lead) – this means lead is stronger than copper and can “kick it out” of it’s compound.
This reaction will occur!
The final balanced equation is:
Pb (s) + CuSO4 (aq)  Cu (s) + PbSO4 (aq)

8. Try a few Mg (s) + HCl (aq)  What is the final balanced equation?
What are the two elements that could switch places in this reaction?
_____ and ______
Find both of those on Table N – which is closer to the bottom?
_______
Will this reaction occur?
What is the final balanced equation?

9. Try a few Al(s) + ZnCl2(aq)  What is the final balanced equation?
What are the two metals involved in this reaction?
_____ and ______
Find both of those on Table N – which is closer to the bottom?
_______
Will this reaction occur?
What is the final balanced equation?

10. Try a few F2 (g) + 2KI (aq)  What is the final balanced equation?
What are the two elements that could switch places in this reaction? (hint: metals or halogens?)
F and I
Since these are halogens, we look at the top of the table
Find both of those on Table N – which is closer to the top? F
Will this reaction occur?
Yes!
What is the final balanced equation?
F2 (g) + 2KI (aq)  2KF (aq) + I2 (s)