Chemical Reactions
Single Replacement Reactions – Text Support, Ch 11
Introduction
The following lab activity will expose you to several single replacement reactions. Specifically,
you will examine what happens when metals are placed in solutions containing ions of other
ions. The metals you will use are copper, magnesium, zinc, and silver. The ionic solutions are
copper(II) nitrate, Cu(NO3)2; magnesium nitrate, Mg(NO3)2; zinc nitrate, Zn(NO3)2; silver
nitrate, AgNO3; hydrochloric acid, HCl.
Experimental Setup
The following is an overhead view of what your data will look like. Copy the template neatly
onto looseleaf paper.
Cu(NO3)2
Mg(NO3)2
Zn(NO3)2
AgNO3
HCl
Cu
Mg
Zn
Ag
Predictions
You will need to predict whether a reaction will happen when pieces of the metals on the left are
dropped into the solutions containing metal ions that are listed on top. The Activity
Series of Metals (Ch 11, pg 333) can be used for this. Using one colored pencil or marker,
indicate each well above where you predict that a reaction will occur by tracing around the
outside of the circle.
Testing the Predictions:
Be careful, silver nitrate stains skin and clothing. When you are using the bottle, be
sure not to spill… and when cleaning out the spot plate, be sure to tilt the plate and
rinse the contents away from your hands.
1) Dispense 5-8 drops of the first solution you are using into the bottom of its designated
well. Be sure you are reading labels carefully!
2) Obtain a small amount of each of the metals. Be conservative, a reaction will be more
visible if you use less solid… rather than more.
3) Place the metal pieces into their designated wells and watch for signs of a reaction.
4) Monitor each combination periodically. After a few minutes, make a final decision on
each combination. If a reaction occurred, write “Y” in the appropriate place on your data
table. If no reaction occurred, write “NR” (no reaction) in the appropriate place.
5) After finishing the analysis, dispose of any solid residues in a paper towel. Rinse liquids
with a large amount of water. Wash your hands. .
Analysis Questions – complete on loose-leaf. Be sure equations are legible.
10-9
8
7
All questions answered; answers
are clear, consistent, and
convincing; appropriate contentbased details are provided
All questions answered; some
functional details are provided
but many answers lack support;
or have minor errors
All questions answered; minimal
details provided; overall, answers
lacks depth or have avoidable
errors in content.
6-5
Incomplete, superficial, and/or
iIllegible.
1. Based on your lab results, rank the metals used in order of most reactive to least reactive.
Which metal is the most reactive? How do you know?
2. Explain what is happening to atoms of the more reactive metal, and what is happening to the
ions of the less reactive metal? Refer to electrons.
3. Write a word equation for each one of the combinations you tested. If no reaction occurred,
write “no reaction” on the product side. If a reaction did occur, write names for the expected
Products.
4. Write a balanced chemical equation for each of the reactions that occurred. Use symbols to
identify the state of matter for each formula you have written. (s) and (aq) will be appropriate
here. **Why is (l) not appropriate?**
5. Write both of the following equations. Identify which one will occur…Finish the products of
that one only, and then balance that equation. Indicate “NR” for the other one.
Cu (s) + Al(NO3)3 (aq) 
Al (s) + Cu(NO3)2 (aq) 
6. Single Replacement reactions are described on pgs 333-334 of your book. Complete CQ # 48
and 60 at the end of Ch 11. You need to refer to the Activity Series of Metals in order to
determine if the reaction can occur at all. Write “NR” fro the products if you determine a
reaction is not possible.
7. Honors only: Single Replacement reactions are Redox reactions. In each reaction that
occurred in lab, identify specific substance/particle was oxidized and what specific
substance/particle was reduced. You can utilize the equations you wrote in #4 above and
provide simple labels such as “O” and “R” above the formulas you are identifying.