Honors Chemistry
Unit 10
 Non-redox reactions
o Double replacement/displacement/precipitate reactions
 Solubility rules
o Neutralization reactions
o Complete and net ionic equations
 Redox reactions
o Oxidized vs reduced
o Combustion reactions
o Synthesis reactions
o Decomposition reactions
o Single replacement/displacement reactions
 Activity series
1
Honors Chemistry Learning Targets
“Non-Redox and Redox Reactions, Reaction Types”
At the conclusion of this unit, the student will be able to”
1.
Demonstrate an understanding of non-redox reactions (double displacement/ppt-precipitate and neutralization).
We are learning to:
1. Demonstrate an understanding of non-redox reactions (double displacement/ppt-precipitate and neutralization).
We are looking for:
1a. Identify non-redox reactions (double displacement/ppt and neutralization).
1b. Use solubility rules to determine if a compound is aqueous (soluble) or solid (insoluble).
1c. Illustrate the dissociation of aqueous (soluble) compounds.
1d. Illustrate the precipitation of solid (insoluble) compounds.
1e. Recognize that a non-redox/double displacement neutralization reaction will occur when
an acid and a base react to form water and a salt.
1f. Determine if a non-redox/double displacement ppt reaction will occur using solubility rules.
1g. Complete and balance any non-redox reaction that will occur.
1h. Write complete and net ionic equations for any non-redox reaction that will occur.
1i. Using solubility rules determine aqueous reactants to produce a given ppt.
At the conclusion of this unit, the student will be able to:
2. Demonstrate an understanding of redox reactions
We are learning to:
1.
2.
3.
4.
5.
Demonstrate an understanding of oxidation and reduction.
Demonstrate an understanding of combustion reactions.
Demonstrate an understanding of synthesis reactions.
Demonstrate an understanding of decomposition reactions.
Demonstrate an understanding of single replacement reactions.
We are looking for:
1a. Assign oxidation numbers to any element/ion in a compound.
1b. Determine which element/ion is oxidized and which one is reduced (Leo the Lion says Ger or Oil Rig).
2a. Identify and complete a combustion reaction (hydrocarbon reacting with oxygen to produce carbon dioxide and
water).
3a. Identify, complete, and balance a synthesis reaction.
4a. Identify, complete, and balance a decomposition reaction.
5a. Identify a single replacement reaction.
5b. Using activity series of metals or halogens, determine if a single replacement reaction will occur.
5c. Complete and balance any single replacement reaction that will occur.
2
To react or not to react?
THAT is the question!
Chemical changes are a result of chemical reactions. All chemical reactions involve a change in substances and
a change in energy. Neither matter or energy is created or destroyed in a chemical reaction---only changed.
There are so many chemical reactions that it is helpful to classify them into 5 general types which include the
following:
SYNTHESIS REACTION
In a synthesis reaction two or more simple substances combine to form a more complex substance.
Two or more reactants yielding one product is another way to identify a synthesis reaction.
For example, simple hydrogen gas combined with simple oxygen gas can produce a more complex
substance-----water!
The chemical equation for this synthesis reaction looks like:
reactant + reactant -------> product
To visualize a synthesis reaction look at the following cartoon:
In the cartoon, the skinny bird (reactant) and the worm (reactant) combine to make one product, a fat
bird.
DECOMPOSITION REACTION
In a decomposition reaction a more complex substance breaks down into its more simple parts. One
reactant yields 2 or more products. Basically, synthesis and decomposition reactions are opposites.
For example, water can be broken down into hydrogen gas and oxygen gas. The chemical equation for
this decomposition reaction looks like:
reactant -------> product + product
3
To visualize a decomposition reaction look at the following cartoon:
In this cartoon the egg (the reactant), which contained the turtle at one time, now has opened and the
turtle (product) and egg shell (product) are now two separate substances.
SINGLE REPLACEMENT REACTION
In a single replacement reaction a single uncombined element replaces another in a compound. Two
reactants yield two products. For example when zinc combines with hydrochloric acid, the zinc
replaces hydrogen. The chemical equation for this single replacement reaction looks like:
reactant + reactant ---------> product + product
To visualize a single replacement reaction look at the following cartoon:
Notice, the guy in the gray shirt steals the date of the other guy. So, a part of one of the reactants trades
places and is in a different place among the products.
4
DOUBLE REPLACEMENT REACTION
In a double replacement reaction parts of two compounds switch places to form two new compounds.
Two reactants yield two products. For example when silver nitrate combines with sodium chloride, two
new compounds--silver chloride and sodium nitrate are formed because the sodium and silver switched
places. The chemical equation for this double replacement reaction looks like:
reactant + reactant ---------> product + product
To visualize a double replacement reaction look at the following cartoon:
COMBUSTION REACTION
A combustion reaction occurs when a compound containing carbon combines with the oxygen gas in
the air. This process is commonly called burning. The products are always carbon dioxide and water.
Here’s the equation that represents the burning of propane:
C3H8 + O2
CO2 + H2O
ENERGY OF CHEMICAL REACTIONS
Chemical reactions always involve a change in energy. Energy is neither created or destroyed. Energy
is absorbed or released in chemical reactions. Chemical reactions can be described as endothermic or
exothermic reactions.
Endothermic Reactions
Chemical reactions in which energy is absorbed are endothermic. Energy is required for the reaction to
occur. The energy absorbed is often heat energy or electrical energy. Adding electrical energy to metal
oxides can separate them into the pure metal and oxygen. Adding electrical energy to sodium chloride
can cause the table salt to break into its original sodium and chlorine parts.
Exothermic Reactions
Chemical reactions in which energy is released are exothermic. The energy that is released was
originally stored in the chemical bonds of the reactants. Often the heat given off causes the product(s)
to feel hot. Any reaction that involves combustion (burning) is an exothermic chemical reaction.
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6
7
8
Non-Redox Reactions
Do NOT involve a transfer of electrons.
Oxidation state of each element/species remains the same before and after the
reaction.
Na SO
2
4(aq)
+ CaCl
2(aq)
 CaSO
4(s)
+ 2NaCl
(aq)
The following are redox reactions: (the oxidation #’s are changing; any element
not in a compound has an oxidation # that is 0)
2 Fe + 3 Cl  2 FeCl
2
2K
(s)
+ FeCl
2(aq)
3
 Fe
(s)
+ 2 KCl
(aq)
Types of non-redox reactions:
1) Double replacement/displacement reactions
2) Neutralization reactions
Double Replacement
(or Double Displacement or Precipitation)
AB + CD → AD + CB
Both pairs change partners –

Always write positive ion (cation) first



Formulas can and will change
Look up charges for each ion
Do 1 to 1 or criss cross
For Products:
Once formulas are adjusted:
 Take inventory of reactants and products
 Balance equation
9
Example:
Potassium Iodide + Lead (II) Nitrate →
KI
+
Pb(NO3)2
→
AB
+
CD
→
AD
+
CB
Not all combinations of reactants will result in a chemical reaction.
A double replacement reaction will occur IF:

Water forms, H2O(l)

A gas forms
o H2CO3 immediately breaks down


It forms CO2 + H2O
CO2 is a gas
o Other gases: H2, O2, N2, Cl2, F2

A precipitate forms (Use solubility table)
o If a compound is soluble (aqueous)– it is not a sign that the reaction will go.
o A precipitate is insoluble (not aqueous; it is a solid ppt)– it is evidence that the
reaction will go.
Neutralization Reaction
(a special type of double replacement)
Acid + Base  a salt + H2O
Acid = formula starts with H
Base = formula ends with OH
Salt = doesn’t start with H or end in OH
H2O = H (OH)
Ex)
H2SO4(aq) +
2 NH4OH(aq) 
(NH4)2SO4(aq) + 2 HOH(l)
~2 H2O
10
Ion Solubility Rules
*For Double Replacement/Displacement Reactions*
*Soluble means it does dissolve= aqueous (aq)
*Insoluble means it does NOT dissolve = solid, ppt (s).
1. **All compounds containing alkali metals (Li+, Na+, K+, Rb+, Cs+)
or ammonium (NH4+) are soluble =(aq)**
2. All compounds with nitrates (NO3-), acetates (C2H3O2-), and
chlorates (ClO3-) are soluble =(aq)
3. All metal ions combined with the halogens (F- , Cl-, Br-, I-) are
soluble = (aq), except for when combined with Hg, Ag, and
Pb, these are insoluble =(s).
4. All compounds with sulfates (SO42-) are soluble =(aq) , except
for when combined with Ca, Ba, Sr, and Hg, Ag, and Pb,
these are insoluble =(s).
5. Except for rule #1, all carbonate (CO32-), chromates
(CrO42-), hydroxides (OH-), oxides (O2-), phosphates (PO43-)
and sulfides (S2-) are insoluble = (s). If these are with an
alkali metal or ammonium, then they are soluble (aq).
See back side for a memory aid to these rules!!
11

C A S H N GiAm
Read it as "Cashin’ GiAm"







C is chlorates
A is acetates
S is sulfates *
H is halogens *
N is nitrates
Gi is Group I metals (the alkali metals)
Am is Ammonium
These are all soluble (aq),
EXCEPT: the following are insoluble = (s)
o
o
for sulfates of: Ca, Ba, Sr, Hg, Ag, Pb

just remember the tv network CBS and
Happy…whats happy? Hg Ag Pb
for halogens of: Hg, Ag, Pb (Happy); remember
this as the happy halogens are NOT soluble =(s).
If its not part of CASHN GiAm it's insoluble,(s).
12
Predicting Products and Solubility Rules Practice:
1)
2)
3)
4)
Add the charges to any ion that doesn’t already have a charge.
Write formula of the compound that will form from the 2 ions that meet at each square.
Indicate for the compound if it will be soluble (aq) or insoluble (s).
If the compound is insoluble (s), circle it.
Ca
Na
Pb2+
Ag
NH4
Fe2+
Sr
Hg2+
CO3
PO4
SO4
Br
S
ClO3
C2H3O2
Cl
NO3
13
Predicting Products and Solubility Rules Practice:
Write both products that will form from the combination of the 2 reactants that meet at each square. Indicate
for each product if it will be soluble (aq) or insoluble (s). If a reaction will occur, circle the product that makes
the reaction occur. If no reaction will occur, write N.R. next to the products.
CaCl2
Na2CO3
Pb(NO3)2
AgC2H3O2
FeF2
NaCl(aq)
CaCO3(s)
Rb3PO4
K2SO4
NH4Br
Li2S
14
Name __________________________________________
Double Replacement Reactions
 Predict the products.
 Predict if these reactions will go to completion using the
solubility rules. Indicate whether each product is soluble (aq) or
insoluble/ppt (s); or if water forms, H2O(l)
 If the reaction occurs, you must then balance the reaction.
1. ___ NaOH(aq) + ___ CaBr2(aq) 
Will this reaction occur? _____
2. ___ Pb(NO3)2(aq) + ___ HCl(aq) 
Will this reaction occur? _____
3. ___ Na2CO3(aq) + ___ KF(aq) 
Will this reaction occur? _____
4. ___ AgNO3(aq) + ___ CuSO4(aq) 
Will this reaction occur? _____
5. ___ AgClO3(aq) + ___ NiCl2(aq) 
Will this reaction occur? _____
6. Devise a method (reaction) for producing silver chromate, given any two
other ionic compounds. Write the equation here:
15
Double Replacement & Ionic Equations Practice
1.
Al(NO3)3(aq) +
Na2SO4(aq) 
Complete ionic equation:
Net ionic equation:
2.
KCl(aq) +
Hg(NO3)2(aq) 
Complete ionic equation:
Net ionic equation:
3.
HCl(aq) +
NaOH(aq) 
Complete ionic equation:
Net ionic equation:
4.
(NH4)2SO4(aq) +
LiOH(aq)

Complete ionic equation:
Net ionic equation:
16
5.
NiCl2(aq) +
Na3PO4(aq) 
Complete ionic equation:
Net ionic equation:
6.
H2SO4(aq) +
KOH(aq) 
Complete ionic equation:
Net ionic equation:
7.
2KOH(aq) + H2SO4(aq) 
Complete ionic equation:
Net ionic equation:
8.
HCl(aq) + AgNO3(aq) 
Complete ionic equation:
Net ionic equation:
17
9.
NH4C2H3O2(aq) +
KCl(aq)

Complete ionic equation:
Net ionic equation:
10.
Fe(C2H3O2)3(aq) +
Ca(OH)2(aq) 
Complete ionic equation:
Net ionic equation:
11.
HClO3(aq) +
Ba(OH)2(aq) 
Complete ionic equation:
Net ionic equation:
12.
Pb(NO3)2(aq) +
AlBr3(aq) 
Complete ionic equation:
Net ionic equation:
18
13.
MgI2(aq) +
Pb(NO3)2(aq) 
Complete ionic equation:
Net ionic equation:
14.
Fr2CO3(aq) +
CaI2(aq) 
Complete ionic equation:
Net ionic equation:
15.
Li2SO4(aq) +
RbOH(aq) 
Complete ionic equation:
Net ionic equation:
19
Double Replacement Lab
Precipitation & Neutralization Reactions
Purpose:
1. Identify the ions present in various aqueous solutions.
2. Combine solutions and identify the reactions that form
precipitates or water.
3. Write balanced molecular equation, complete ionic equation, and a net ionic
equation for each precipitation reaction.
4. Identify/name the product that makes the reaction occur.
5. Draw & label the contents of the test tube once the reactants are mixed
together.
Materials:

Small test tubes

Various solutions
Procedure:
For each reaction #1-12
1. Add 10-15 drops of the each reactant to a test tube.
2. Observe the results when the two solutions are combined in the test tube.
3. Record your observations for when the two solutions are mixed together and
draw and label the contents of the test tube.
4. If no precipitate (ppt) is detected or water is not formed, write NR or no
reaction.
5. Thoroughly clean your test tube before conducting another reaction in the same
test tube.
For each reaction #13-14
You decide which 2 reactants to combine that have not been tested in this
lab, then follow steps 1-5 from above.
20
Reaction #1:
aqueous barium chloride + aqueous sodium sulfate 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #2:
aqueous sodium carbonate + aqueous silver nitrate 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
21
Reaction #3:
aqueous barium chloride + aqueous lead (II) nitrate 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #4:
aqueous cadmium chloride + aqueous sodium sulfide 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
22
Reaction #5:
aqueous barium chloride + aqueous silver nitrate 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #6:
aqueous copper (II) chloride + aqueous sodium carbonate 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
23
Reaction #7:
aqueous iron (III) chloride + aqueous sodium hydroxide 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #8:
aqueous ammonium chloride + aqueous sodium hydroxide 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
24
Reaction #9:
aqueous barium chloride + aqueous sulfuric acid 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #10:
aqueous barium nitrate + aqueous sodium sulfate 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
25
Reaction #11:
aqueous barium chloride + aqueous sodium hydroxide 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #12:
aqueous lead (II) nitrate + aqueous potassium iodide 
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
26
Reaction #13: Pick any 2 that you have not combined in this lab
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #14: Pick any 2 that you have not combined in this lab
Observations:
Balanced molecular equation:
Complete ionic equation:
Net ionic equation:
Name of product that makes the reaction occur:
27
28
Chemical
Reactions
29
Classification of Chemical Reactions
A
+
B
AB 
A + BC

AB
A + B

Synthesis
Decomposition
B + AC
Single Replacement
AB + CD  AD + CB
Double Replacement
CxHy + O2  CO2 + H2O
Combustion
30
??? WHAT KIND OF REACTION ???
1. Ca + O2  CaO
2. HgO  Hg + O2
3. Cd + HCl  CdCl3 + H2
4. MnSO4  MnO + SO3
5. Na + Cl2  NaCl
6. FeCl2 + Na3PO4  NaCl + Fe3(PO4)2
7. Mg + CuSO4
 MgSO4 + Cu
8. NaNO3  NaNO2 + O2
9. Mg + N2  Mg3N2
31
Chemical reactions
A. Balance the following equations:
B. Identify the type of reaction: (write the correct letters to the left of
the number.)
S = combination, synthesis SR = Single replacement,
C = Combustion
D = Decomposition,
DR = Double replacement, NA = None of these
_____ 1.
_____ Na
+
_____ 2.
____ HgO 
___ O2
+
____ Hg
_____ 3.
_____ Cl2
+
___ H2O

___ HCl
+
___ O2
_____ 4.
____ SnCl2
+ ___Cr(NO3)6

___ CrCl6
+
___ Sn(NO3)2
+ ___ H3PO4

___ Ca3(PO4)2 +
_____ 5. ____ Ca(OH)2
_____ 6. _____ C4H10
___ O2
+ ___ O2
______ 7. _____ (NH4)3PO4
______ 8.
_____ BrF3



___ Na2O
___ CO2
+
___ H2O
___ H2O
+ ___ Fe(NO3)2  ___ Fe3(PO4)2
___ Br2
+
___ NH4NO3
___ F2
_____ 9. _____ C3H8 + ___ O2  ____ CO2
+ _____ H2O
______ 10. _____ BaO
+ ____HCl
 ____ BaCl2
______ 11. _____P4O10
+ ____HNO3  ____H3PO4
+ _____ H2O
+ ____ N2O5
______ 12. ____Fe2(Cr2O7) 3 + ___ CuNO3  ___ Cu2Cr2O7 +
______ 13. ____K2Cr2O7 + ___HCl  ___ KCl
+
___ Fe(NO3) 3
+ ____CrCl3 + ____ H2O + ____ Cl2
______ 14. _____PbS + ____HNO3  ____ Pb(NO3)2 + ____ NO + ____ S + ____ H2O
______ 15. ____ FeCl3
______ 16.
+ ____ H2S
 ____ FeCl2
_____ NH3 + ____ O2  ____ NO2
+ ____ S
+ ____ HCl
+ ____H2O
32
_____ 17. _____ C8H18 + ____ O2
______ 18.

____ CO2 + ____ H2O
_____ Sb + ____ I2  ____ SbI3
______ 19. _____ AlCl3 + ____ Pb(NO2)2  ____ PbCl2
+ ____ Al(NO2)3
______ 20. _____ Mg + ____ CrCl3
_____ Cr

____ MgCl2 +
Write the name or the chemical formula for the following compounds
a)
Potassium sulfate
______________
f) SnF2
______________________
b) calcium phosphate
______________
g) Li3PO4
______________________
h) BaS
______________________
c)
Lead (IV) carbonate ______________
d) Sodium bromide
______________
i) Cu(OH)2 ______________________
e)
_______________
j) NH4Cl ______________________
Zinc hydroxide
33
Redox Reactions
 Involve a transfer of electrons.
 Redox reactions have a change in charge (oxidation state) between
the reactants and products.
 The element that loses the electrons (oxidation state increases) is
"oxidized"
 The element that gains the electrons (oxidation state decreases) is
"reduced"
If an element loses electrons, it is oxidized and if an element
gains electrons, it is reduced (LEO the lion says GER!!)
Lose electrons, oxidized.
Gain electrons, reduced.
Redox reactions are: single replacement, synthesis, combustion
and decomposition.
Example:
K + F2 → KF
CO2 + H2 →
CO + H2O
34
Steps to Redox Reactions:
1. Write down complete reaction
2. Assign an oxidation number to each element.
 Diatomics and metals (as elements) have an oxidation number of
zero.
 For ions, it is equal to its charge (Na+1, Cl-1, Ca+2).
 Oxygen is 2- in most compounds.
 Hydrogen is 1+ in most compounds.
3. Determine which element is being reduced (gaining electrons,
decrease in oxidation #). Connect them and mark the number of
electrons gained.
4. Determine which element is being oxidized (losing electrons,
increasing in oxidation #). Connect them and mark the number of
electrons lost.
Example:
Al + O2  Al2O3
Type of reaction =
Al
+ O2

Al2O3
35
Al
+ O2

Al2O3
Aluminum is being __________________
Oxygen is being _________________
Another example:
FeO  Fe + O2
Type of reaction =
FeO 
Fe +
O2
Iron is ______________
Oxygen is _______________
36
Mg + PbCl4 
Mg
Pb + MgCl2
+ PbCl4
Ba(NO3)2 + Na3PO4 
Type of Reaction =

Pb +
MgCl2
Ba3(PO4)2 + NaNO3
Type of reaction =
Ba(NO3)2 + Na3PO4 
Ba3(PO4)2 + NaNO3
37
Types of Reactions Worksheet
For each reaction: balance, predict reaction type and show oxidation and reduction if
appropriate.
1. ___NaBr + ___H3PO4 → ___Na3PO4 + ___HBr
Type of Reaction: __________________________
2. ___Mg + ___Cr2O3 → ___Cr + ___MgO
Type of Reaction: __________________________
3. ___Fe + ___Cl2 → ___FeCl3
Type of Reaction: __________________________
4. ___CaS → ___Ca + ___S8
Type of Reaction: __________________________
5. ___Pb + ___HCl → ___PbCl2 + ___H2
Type of Reaction: __________________________
38
6. ___H2SO4 + ___NH4OH → ___H2O + ___(NH4)2SO4
Type of Reaction: __________________________
7. ___HgO → ___Hg + ___O2
Type of Reaction: __________________________
8. ___Rb + ___P4 → ___Rb3P
Type of Reaction: __________________________
9. ___C6H14 + ___O2 → ___CO2 + ___H2O
Type of Reaction: __________________________
39
Oxidation and Reduction Practice
In each of the following equations, indicate the element that has been oxidized and the one that
has been reduced. You should also label the oxidation state of each before and after the
process:
1)
2 Na + FeCl2  2 NaCl + Fe
2)
2 C2H2 + 5 O2  4 CO2 + 2 H2O
3)
2 PbS + 3 O2  2 SO2 + 2 PbO
4)
2 H2 + O2  2 H2O
5)
Cu + HNO3  CuNO3 + H2
6)
AgNO3 + Cu  CuNO3 + Ag
40
41
42
Single Replacement Reactions
** Single Displacement**
+

+
A __________________ “A” displaces or switches places with a
___________________ “B”
Example:
1.
Fe(s) + CuCl2(aq)  FeCl2(aq) + Cu
2.
Cu(s) + AgNO3(aq)  Ag(s) + Cu(NO3)2(aq)
3.
Ca(s) + H2O(l) 
**Refer to the activity series list.** - you will get this after the
experiment.
If A is ___________ than B, the reaction takes place!
If A is _____________ than B, nothing happens!!
Ex) Mg + KCl  N.R. (no reaction)
Can also occur with halogens. In this case the halogens are A and C
in the reaction. The most reactive halogen is F and the reactivity
decrease as you move down the group.
Ex)
Cl2(g) + KBr(aq) 
Br2(L) + KCl(aq) 
43
Single Replacement/Displacement Lab
Introduction:
A single replacement reaction is the type of chemical change that occurs when
you react an element with a compound. The element will attempt to take a
place in the compound (becoming an ion) kicking another element out of the
compound. The major issue with single replacement reactions is that they will
only occur if a more active substance is attempting to replace a less active
substance.
The object of this lab is to determine the activities of various metals in
relation to each other. These include Zn, Pb, Mg, Cu, Fe, Ca, and Ag. The
activity of hydrogen will also be determined. Though hydrogen is not
considered to be a metal, it does form a cation and will replace certain metals
of ionic compounds.
Materials:




2 microplates (24 wells each)
forceps
spatula
pipets






Zn(s)
Pb(s)
Mg(s)
Cu(s)
Fe(s)
Ca(s)






Zn(NO3)2
Pb(NO3)2
MgSO4
CuSO4
Fe(NO3)3
CaCl2
Procedure:
1) Obtain 2 dry microplates, place them on a white sheet of paper, and put them together
to form an 6 x 6 grid.
2) Place a small amount of metal in the appropriate well according to the data table.
3) Add 10-15 drops (enough to cover the metal) of the appropriate solution to each metal.
4) Make note of any indicators of a chemical reaction in the space in the data table.
Note: Some reactions may take a few minutes to occur. Continue on, but refer back to
them before making your final observations.
5) In the data table, identify that a reaction occurred with a check mark and no visible
reaction with an X.
6) Make certain you have all observations before clean up.
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Clean Up:




Let all reactions come to completion.
Use forceps to remove any unreacted metal and place it in a paper towel to throw
away.
Rinse and scrub each well with a test tube brush. Shake the microplate to remove as
much water as possible.
Clean your lab bench and make certain that all solutions and containers are sealed.
Data:
Zn(NO3)2
Pb(NO3)2
MgSO4
CuSO4
Fe(NO3)3
CaCl2
Zn
Pb
Mg
Cu
Fe
Ca
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One last test,
take a piece of copper (Cu) and test it with AgNO3 solution.
 Do you see a reaction? ________________
 What does this result mean? _____________________
Conclusion:
Below – Rank the metals from this activity based on their reactivity.
Include silver (Ag) in the rankings!
Most reactive metal







Least reactive metal
46
Using the activity chart provided, predict whether or not the following
reactions will take place. For the reactions that will occur, predict the
products and then balance the reaction.
= Go
= No Go
_____
1. Al + Fe2O3 
_____
2. Pb + MgSO4 
(Pb charge = +2)
_____
3. Zn + FeCl3 
(Zn charge = +2)
_____
4. Fe + CuCl2 
(Fe charge = +3)
_____
5. Ag + CuSO4 
(Ag charge = +1)
_____
6. Au + AgBr 
(Au charge = +1)
_____
7. Cr + NiI2 
(Cr charge = +2)
_____
8. K + MgSO4 
_____
9. Zn + MgCl2 
(Zn charge = +2)
_____
10. Na + CaSO4 
47
Decomposition Reactions
_________ → _______
+ _______
1 reactant
(compound)
forms
2 or more products
(simpler compounds or elements)
For decomposition reactions to occur –
need energy:




Some compounds decompose readily, if formed in a reaction:
H2CO3 = Carbonic Acid
H2CO3(aq) → H2O(l) + CO2(g)
H2SO3 = Sulfurous Acid
H2SO3(aq) → H2O(l) + SO2(g)
Verifying your products:
 If product is H2
o Use burning splint
o Will hear a “POP”
 If product is O2
o Use glowing splint
o Will re-light
48
Decomposition of Water:
___H2O
Gas = ____
Proof:
→ ___H2 + ___O2
Gas =_____
Proof:
49
Decomposition of Hydrogen Peroxide
In this activity, you will be determining the products of the decomposition of hydrogen
peroxide.
Materials:
1) glass jar
2) pie plate
3) 125 ml Hydrogen peroxide
4) 100 ml graduated cylinder
5) Food coloring
6) 100 ml warm water
11) wood splints
7) 250 ml beaker
12) Mg ribbon
8) 7g yeast
9) weigh boat
10) stirring rod
Procedure:
Group 1:
1. Place glass jar in center of pie plate.
2. Add 125 ml of hydrogen peroxide to the glass jar.
3. Add 4 drops of food coloring to glass jar – your choice!
4. Place pie plate with glass jar in center of lab station
5. Wait for further instructions
Group 2:
1. Put 100 ml of warm water into 250 ml beaker
2. Add 7 grams of yeast to same 250 ml beaker
3. Using stirring rod, stir yeast and warm water for 3-5 minutes
4. Wait for further instructions
Analysis:
Write the balanced equation for the reaction that occurred. Be sure to include any
inputs and outputs such as heat, chemical catalysts, energy, light, etc. Hint: The yeast
remains unchanged and one of the products is water.
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Decomposition Reactions
Complete the product side (where missing) and balance all reactions!
→
1.
____Na2CO3
____ Na2O + ____ CO2
2.
____ HgO →
3.
____ NaCl →
4.
____ NH4NO3 → ____ N2O + ____ H2O
5. ____ KClO3 → ____ KCl + ____ O2
Translate to chemical equations and balance:
6. Silver (I) Oxide decomposes into Silver and Oxygen
7. Iron (III) Oxide decomposes into Iron and Oxygen
8. Calcium Carbonate decomposes into Calcium Oxide and Carbon Dioxide
Tough One (OMG!!):
____(NH4)2Cr2O7 → ___ NH3 + ___H2O + ___Cr2O3 + ___O2
51
Synthesis Reactions
+

__ elements or small compounds reacted together to make
_________________
Examples:
Joining elements:
__ Fe
+ ___S8

__FeS
What is the oxidation number of Iron
if sulfur has a -2 charge? ____
__Na + __Cl2  __NaCl
*** Synthesis reactions have one main purpose:
52
Synthesis:
In this activity, you will be determining the mass of the reactants before a chemical reaction
and the mass of the products after the reaction.
Materials:
1) crucible
2) crucible tongs
3) ring stand with
clay triangle
4) Balance
5) Tirrill burner
6) Mg ribbon
Procedure:
1) Determine the mass of the empty crucible with lid and record in table 1.
2) Obtain a 6 in strip of Mg ribbon. Cut it into about 12 pieces and put the pieces into the
crucible and determine the mass. Record in table 1.
3) Place the crucible on the clay triangle and slowly heat it with a “soft” blue flame for a
minute.
4) Increase the heat gradually by adjusting the burner’s flame until the crucible is at the
tip of the inner cone.
5) Once the Mg begins to react, turn off the burner. REMEMBER: DO NOT LOOK
DIRECTLY AT THE LIGHT!!!
6) Allow the crucible to cool on the ring stand for 15-20 min. Then determine the mass of
the product by weighing the crucible + product and subtracting the mass of the crucible.
Record in table 1.
7) After cooling, discard the ashes in the trash.
Mass of Crucible
Mass of reactant (Mg)
Mass of product (?)
Analysis:
1) Compare the mass of the reactant to the mass of the product by determining the %
recovery:
a. % recovery = (mass of product/mass of reactant) x 100
2) Write the balanced equation for the reaction that occurred. Be sure to include any inputs
and outputs such as heat, chemical catalysts, energy, light, etc. Hint: Mg combined with
oxygen.
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Synthesis Reactions:
!!Balance!!
1) ___H2 + ___ O2  ___H2O
2) ___S8 + ___ O2  ___SO3
3) ___Si + ___S8  ___Si2S4
4) ___P + ___ O2  ___P2O5
5) ___N2 + ___ H2  ___NH3
6) ___Na2O + ___ CO2  ___Na2CO3
7) ___P4O10 + ___H2O  ___H3PO4
8) ___P + ___Cl2  ___PCl3
9) ___C5H5 + ___Fe  ___Fe(C5H5)2
10)___NH3 + ___H2SO4  ___(NH4)2SO4
54
Synthesis Reactions
Predict the products of these reactions and then balance the equations.
1) ___Mg + ___O2 → ___
2) ___Fe (III)
+ ___ I2 → ___
3) ___H2 + ___Cl2 → ___
4) Zinc + Sulfur →
5) Lead (IV) + Oxygen →
6) Potassium + Fluorine →
7) Hydrogen + Oxygen →
55
Combustion Reactions
+

+
**One reactant needs ___________________________ **
**The other _______________________________**
The products are always __________+ ___________.
_____________________________ are always exothermic
(They give off ________________________!)
Examples:

___CH4 + ___ O2  ___CO2 + ___H2O
 ___C4H10 + O2  ___CO2 + ___H2O
The CxHy reactant can also contain _________:
(CxHyOz)
 ______CH3OH + ____O2  _____CO2 + ____H2O
56
Combustion Reactions
Write the balanced chemical equation for the combustion of the following
hydrocarbons:
1. methane
1) propane
2) octane
3) ethene
4) methanol
5) _____C6H12O6
6) _____C6H6
7) _____C3H7OH
8) _____C8H17OH
10) ____C6H5OH + ___O2 
57
When making products – go back to the charges of each element,
then do criss cross. Do not take subscripts to the product side!
Each letter represents one element or one polyatomic
Synthesis
A + B  AB
1.
Mg(s) +
O2(g) 
2.
Fe(s) (Charge +3) +
Br2(l) 
Decomposition
AB  A + B
1.
MgO(s) 
2.
SiCl4(s) 
Single Replacement/Displacement (need activity chart)
A + BC  AC + B if A is stronger (more active) than B
If B is stronger (more active) – no reaction will take place (N.R.)
1.
K(s) +
2.
Au(s) +
MgCl2(aq) 
MgCl2(aq) 
58
Double Replacement/Displacement
(complete & net ionic equations also)
AB + CD  AD + CB
1.
AgNO3(aq) +
NaBr(aq) 
2.
MgSO4(aq) +
KCl(aq) 
Combustion
CxHy + O2  CO2 + H2O
1.
CH4(g) +
2.
C8H18(l) +
59
Fun With Predicting Reaction Products
Predict the products of each of the following chemical reactions. If a reaction will not occur,
explain why not:
1)
____ Ag2SO4(aq) + ____ NaNO3 (aq) 
2)
____ NaI(aq) + ____ CaSO4(aq) 
3)
____ HNO3(aq) + ____ Ca(OH)2(aq) 
4)
_____CaCO3(s)  CaO(s) + CO2(g)
5)
____ AlCl3 (aq) + ____ (NH4)3PO4 (aq) 
6)
____ Pb(s) + ____ Fe(NO3)3(aq) 
(+2)
7)
____ C3H6(g) + ____ O2(g) 
8)
____ Na(s) + ____ CaSO4(aq) 
60
9)
____ Na(s) + ____ O2(g) 
10)
____ C4H10(g) + ____ O2(g) 
11)
_____BrF3 
12)
_____ C8H18(l) + ____O2(g) 
13)
_____ Rb(s) + ____I2(s) 
14)
____ Al2O3 
61
Practice Completing & Balancing Equations
For each problem, indicate the type of reaction shown, predict the product(s), and balance the
equation.
Type of Reaction
1.____________
____Ag(s) + ____Cl2(g) 
2. ____________
____Mg(s) + ____Cu3SO4(aq) 
3.____________
____AlBr3(aq) + ____K2SO4(aq) 
4. ____________
____KCl(s) 
5. ____________
____C5H12(l) + ____O2(g) 
6. ____________
____Pb(C2H3O2)2(aq) + ____HCl(aq) 
7. ____________
____Al(s) + ____CuCl2(aq) 
8. ____________
____C3H8(g) + ____ O2(g) 
9. ____________
____Na(s) + ____Br2(l) 
10. ____________ ____ HgO 
62
Convert these word equations to formulas, predict the products, and balance. Put the reaction
type in the margin to the left of the number.
11. sodium carbonate + barium chloride 
12. potassium phosphate + magnesium
13. barium + oxygen 
14. ammonium sulfate + sodium chloride 
15. zinc + nickel (II) iodide 
16. iron (III) bromide 
17. benzene + oxygen 
18. aluminum chloride + ammonium phosphate 
19. Calcium carbonate powder breaks down into solid calcium oxide and carbon dioxide gas.
63