Honors Chemistry
Unit 9
(2016-2017)
 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
Unit 9A
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.
5
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)
5)
6)
Write the formula for the given polyatomic ion name.
Add the charges to any ion that doesn’t already have a charge.
Along the top and side, highlight all the halogens and put a box around the Group I metal ions.
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.
calcium
sodium
lead (II)
silver
ammonium
Iron (II)
strontium
mercury (II)
carbonate
phosphate
sulfate
bromine
sulfur
chlorate
acetate
chlorine
nitrate
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Predicting Products and Solubility Rules Practice:
Write the formula for each compound underneath its name. Next, write both product formulas 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) , insoluble
(s), or liquid [(l), only when water forms ].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.
Calcium chloride
CaCl2
Sodium carbonate
Na2CO3
Lead (II) nitrate
Silver acetate
Sodium hydroxide
Iron (II) fluoride
NaCl(aq)
CaCO3(s)
Rubidium phosphate
Potassium sulfate
Ammonium bromide
Lithium sulfide
Sulfuric acid
Barium chlorate
14
Name __________________________________________
Double Replacement/Displacement Reactions
 Predict the products and balance the reaction
 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)
 Identify if the reaction is a precipitation reaction, neutralization reaction, or a reaction that will
not occur.
 Name the product that makes the reaction occur.
 Draw the results (products) in a test tube.
1. ___ NaOH(aq) + ___ CaBr2(aq) 
precipitation, neutralization, or no reaction?
2. ___ Pb(NO3)2(aq) + ___ HCl(aq) 
precipitation, neutralization, or no reaction?
3. ___ Na2CO3(aq) + ___ KF(aq) 
precipitation, neutralization, or no reaction?
4. ___ AgNO3(aq) + ___ CuSO4(aq) 
precipitation, neutralization, or no reaction?
5. ___ AgClO3(aq) + ___ NiCl2(aq) 
precipitation, neutralization, or no reaction?
6.
Write out a reaction for producing solid silver chromate, given any two other ionic compounds
(remember, the reactants must be aqueous). Write the reaction here:
15
Double Replacement & Ionic Equations Practice
Complete the following on a separate sheet of paper. For each problem below,




write the full balanced reaction
name the product that will make the reaction occur.
write the net ionic equation.
draw the results in the test tube.
1. Al(NO3)3(aq) +
Na2SO4(aq) 
2.
KCl(aq) +
Hg(NO3)2(aq) 
3.
HCl(aq) +
NaOH(aq) 
4.
(NH4)2SO4(aq) +
5.
NiCl2(aq) +
6.
H2SO4(aq) +
LiOH(aq)

Na3PO4(aq) 
KOH(aq) 
7.
NaOH(aq) + HNO3(aq) 
8.
HCl(aq) + AgNO3(aq) 
9.
NH4C2H3O2(aq) +
10.
aqueous iron (II) acetate +
11.
aqueous chloric acid +
12.
aqueous lead (II) nitrate +
13.
aqueous magnesium iodide +
14.
aqueous francium carbonate +
15.
aqueous lithium sulfate + aqueous rubidium hydroxide
KCl(aq)

aqueous cesium hydroxide 
aqueous ammonium hydroxide 
aqueous aluminum bromide 
aqueous lead (II) nitrate 
aqueous calcium iodide 

16
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. Write the balanced molecular equation.
2. Add 10-15 drops of the each reactant to a test tube.
3. Observe the results when the two solutions are combined in the test tube.
4. Record your observations for when the two solutions are mixed together and draw and
label the contents of the test tube.
5. If no precipitate (ppt) is detected or water is not formed, write NR or no reaction.
6. 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.
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Reaction #1:
aqueous barium chloride + aqueous sodium sulfate
Observations:
Balanced molecular equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #2:
aqueous sodium carbonate + aqueous silver nitrate
Observations:
Balanced molecular equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #3:
aqueous barium chloride + aqueous lead (II) nitrate
Observations:
Balanced molecular equation:
Net ionic equation:
Name of product that makes the reaction occur:
18
Reaction #4:
aqueous cadmium chloride + aqueous sodium sulfide
Observations:
Balanced molecular equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #5:
aqueous barium chloride + aqueous silver nitrate
Observations:
Balanced molecular 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:
Net ionic equation:
Name of product that makes the reaction occur:
19
Reaction #7:
aqueous iron (III) chloride + aqueous sodium hydroxide
Observations:
Balanced molecular equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #8:
aqueous ammonium chloride + aqueous sodium hydroxide
Observations:
Balanced molecular equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #9:
aqueous barium chloride + aqueous sulfuric acid
Observations:
Balanced molecular equation:
Net ionic equation:
Name of product that makes the reaction occur:
20
Reaction #10:
aqueous barium nitrate + aqueous sodium sulfate
Observations:
Balanced molecular equation:
Net ionic equation:
Name of product that makes the reaction occur:
Reaction #11:
aqueous barium chloride + aqueous sodium hydroxide
Observations:
Balanced molecular 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:
Net ionic equation:
Name of product that makes the reaction occur:
21
Reaction #13: Pick the 2 chemicals from this lab that will create a neutralization
reaction. Feel the test tube bottom to note any temp. change when the
chemicals are combined.
Observations:
Balanced molecular 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:
Net ionic equation:
Name of product that makes the reaction occur:
22
Unit 9B
Chemical
Reactions
23
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
??? WHAT KIND OF REACTION ???
1. Ca + O2  CaO
__________________________________
2. HgO  Hg + O2
__________________________________
3. Cd + HCl  CdCl2 + 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
__________________________________
24
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,
D = Decomposition,
C = Combustion
DR = Double replacement, NA = None of these
**If DR, also determine if the reaction is a neutralization reaction,
precipitation reaction (you will need to determine the solubility of the
products) or a no reaction.**
_____ 1.
_____ Na
_____ 2.
____ HgO 
___ O2
+
____ Hg
_____ 3.
_____ Li
+
___ H2O

___ LiOH
+
___ H2
_____ 4.
____ SnCl2
+ ___Cr(NO3)6

___ CrCl6
+
___ Sn(NO3)2
+ ___ H3PO4

___ Na3PO4
+
___ H2O
_____ 5. ____ NaOH
_____ 6. _____ C4H10
+
+ ___ O2
______ 7. _____ (NH4)3PO4
______ 8.
_____ BrF3
___ O2



___ Na2O
___ CO2
___ H2O
+ ___ Fe(NO3)2  ___ Fe3(PO4)2
___ Br2
+
_____ 9. _____ C3H8 + ___ O2  ____ CO2
______ 10. _____ BaO
+
+ ____HCl
+
___ NH4NO3
___ F2
+ _____ H2O
 ____ BaCl2
+ _____ H2O
Continued on the next page
25
______ 11. _____P4O10
+ ____HNO3  ____H3PO4
______ 12. ____Rb2Cr2O7 + ___ CuNO3
+ ____ N2O5
 ___ Cu2Cr2O7 +
______ 13. ____K2Cr2O7 + ___HCl  ___ KCl
___ RbNO3
+ ____CrCl3 + ____ H2O + ____ Cl2
______ 14. _____PbS + ____HNO3  ____ Pb(NO3)2 + ____ NO + ____ S + ____ H2O
______ 15. ____ FeCl3
______ 16.
+ ____ H2S
_____ NH3 + ____ O2  ____ NO2
_____ 17. _____ C8H18 + ____ O2
______ 18.
 ____ FeCl2

+ ____ S
+ ____ HCl
+ ____H2O
____ CO2 + ____ H2O
_____ Sb + ____ I2  ____ SbI3
______ 19. _____ AlCl3 + ____ Pb(NO2)2  ____ PbCl2
+ ____ Al(NO2)3
______ 20. _____ Mg + ____ CrCl3
_____ Cr

____ MgCl2 +
26
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 (______________ agent)
Gain electrons, reduced (______________ agent)
Redox reactions are: single replacement, synthesis, combustion and
decomposition.
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Steps to Redox Reactions:
1. Write down complete reaction.
2. Assign an oxidation number to each element.
**The oxidation #’s you learned are for ionic compounds. They are not
necessarily the same when applied to covalent compounds.**
 Any element by itself (including diatomics) have an oxidation number
of zero.
 Group I metals always 1+ and Group II metals always 2+, fluorine 1-.
 Oxygen is 2- in most compounds.
 Chlorine is 1- in most compounds.
 Hydrogen is 1+ in most compounds (if it is with a metal, it will be 1-)
 The sum of all the oxidation numbers of the atoms in a compound must
equal zero; the sum of the oxidation numbers of all atoms in a
polyatomic ion will equal the charge of the ion.
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.
Examples:
Oxidation #’s for one atom of the element below the #
0
2 K
4+ 2-
CO2
4- 1+
CH4
0
+
H2
0
+
F2
2+ 2-
→
0
+ O2 →
CO
→
2 KF
1+ 2-
+ H2 O
4+ 2-
CO2
1+ 1-
1+ 2-
+
H2O
28
1)
Type of reaction =
Al
+ O2
Al2O3

Aluminum is being _________________ (ox. # went _____) and is the ___________agent.
Oxygen is being _________________ (ox. # went ______) and is the_____________ agent.
2)
Type of reaction =
FeO 
Fe +
O2
Iron is being ________________(ox. # went ______) and is the_____________ agent.
Oxygen is being _______________(ox. # went ______) and is the_____________ agent.
3)
Type of Reaction =
Mg
+ PbCl4

Pb +
MgCl2
_____ is being oxidized and it ________ electrons. (ox. # went _______)
_____ is being reduced and it ________ electrons. (ox. # went _______)
4)
Type of reaction =
Ba(NO3)2 + Na3PO4 
Ba3(PO4)2 + NaNO3
_____ is being oxidized and it ________ electrons. (ox. # went _______)
_____ is being reduced and it ________ electrons. (ox. # went _______)
29
Types of Reactions and Oxidation/Reduction Worksheet
For each reaction: balance, predict reaction type and determine if anything is oxidized/reduced and if it gained/lost
electrons.
1. ___NaBr + ___H3PO4 → ___Na3PO4 + ___HBr
Type of Reaction: __________________________
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
2.
___Mg + ___Cr2O3 → ___Cr + ___MgO
Type of Reaction: __________________________
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
3.
___Fe + ___Cl2 → ___FeCl3
Type of Reaction: __________________________
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
4.
___CaS → ___Ca + ___S8
Type of Reaction: __________________________
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
5.
___Pb + ___HCl → ___PbCl2 + ___H2
Type of Reaction: __________________________
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
6.
___H2SO4 + ___NH4OH → ___H2O + ___(NH4)2SO4
Type of Reaction: __________________________
_____ is being oxidized (_____________ electrons).
_____ is being reduced (_____________ electrons).
7.
___HgO → ___Hg + ___O2
Type of Reaction: __________________________
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
8.
___Rb + ___P4 → ___Rb3P
Type of Reaction: __________________________
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
9.
___C8H16 + ___O2 → ___CO2 + ___H2O
Type of Reaction: __________________________
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons
30
Name:_______________________________
Class:_______
Oxidation and Reduction Practice
In each of the following equations, indicate the element that has been oxidized and the one that has
been reduced and if it gained or lost electrons. You should also label the oxidation state of each
before and after the process:
1)
2 Na + FeCl2  2 NaCl + Fe
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
2)
2 C2H2 + 5 O2  4 CO2 + 2 H2O
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
3)
2 PbS + 3 O2  2 SO2 + 2 PbO
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
4)
2 H2 + O2  2 H2O
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
5) Ca(NO3)2 + CuSO4  Cu(NO3)2 + CaSO4
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
6)
Cu + HNO3  CuNO3 + H2
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
7)
AgNO3 + Cu  CuNO3 + Ag
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
8)
2 C3H6 + 9 O2  6 CO2 + 6 H2O
_____ is being oxidized (______________ electrons).
_____ is being reduced (______________ electrons).
31
32
33
34
Single Replacement Reactions
** Single Displacement**
+

+
A __________________ “A” displaces or switches places with a
___________________ “B” (or a halogen will replace a halogen)
Example:
1.
Fe(s) + CuCl2(aq)  FeCl2(aq) + Cu(s)
2.
AgNO3(aq) + Cu(s)  Ag(s) + Cu(NO3)2(aq)
3.
Na(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(s) + KCl(aq)  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) + NaF(aq) 
35
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.
Clean Up:




Let all reactions finish.
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.
36
Data:
Zn(NO3)2
Pb(NO3)2
MgSO4
CuSO4
Fe(NO3)3
CaCl2
Zn
Pb
Mg
Cu
Fe
Ca
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
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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(s) +
_____
2.
Pb(s) +
Fe(NO3)3(aq) 
MgSO4(aq) 
(if the reaction occurs, Pb will lose 2 electrons)
_____
3.
Br2(l) +
FeCl3(aq) 
_____
4.
Fe(s) +
CuCl2(aq) 
(if the reaction occurs, Fe will lose 3 electrons)
Ag(s) 
_____
5.
CuSO4(aq) +
_____
6.
Cl2(g) +
CaBr2(aq) 
_____
7.
Cr(s) +
NiI2(aq) 
(if the reaction occurs, Cr will lose 2 electrons)
_____
8.
K(s) +
_____
9.
MgCl2(aq) +
_____
10.
H2O(l) 
Ca(NO3)2(aq)
I2(s)
+

Na(s) 
38
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
39
Decomposition of Water:
___H2O
Gas = ____
Proof:
→ ___H2 + ___O2
Gas =_____
Proof:
40
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
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.
41
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
6. ____(NH4)2Cr2O7 → ___ NH3 + ___H2O + ___Cr2O3 + ___O2
Translate to chemical equations and balance:
7. Silver Oxide decomposes into Silver and Oxygen
8. Iron (III) Oxide decomposes into Iron and Oxygen
9. Calcium Carbonate decomposes into Calcium Oxide and Carbon Dioxide
42
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:
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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) Bunsen 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 Empty
Crucible (g)
Mass of reactant, Mg
(g)
Mass of Crucible
after Heating (g)
Mass of Product (g)
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.
3) Compare the mass of the reactant (Mg) with the mass of the product. Why is there a
difference?
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Synthesis Reactions:
!!write the product formula from the name given and then balance!!
1) ___H2 + ___ O2  ___
dihydrogen monoxide
2) ___S8 + ___ O2  ___
sulfur trioxide
3) ___Si + ___S8  ___
disilicon tetrasulfide
4) ___P4 + ___ O2  ___
diphosphrous pentoxide
5) ___N2 + ___ H2  ___
nitrogen trihydride
6) ___Na2O + ___ CO2  ___
sodium carbonate
7) ___P4O10 + ___H2O  ___
phosphoric acid
8) ___P4 + ___Cl2  ___
phosphorus trichloride
9)___NH3 + ___H2SO4  ___
ammonium sulfate
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Synthesis Reactions
Predict the products of these reactions and then balance the equations.
(use what you know about oxidation numbers and ionic compounds to determine the products)
1) ___Mg + ___O2 → ___
2) ___Fe
(Hint: the iron will lose 3 electrons)
+ ___ I2 → ___
3) ___H2 + ___Cl2 → ___
4) Zinc + Sulfur →
5) Lead (Hint: the lead will lose 4 electrons) + Oxygen →
6) Potassium + Fluorine →
7) Hydrogen + Oxygen →
46
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
47
Combustion Reactions
Write the balanced chemical equation for the combustion of the following
hydrocarbons:
1) Methane (CH4)
2) Propane (C3H8)
3) Octane (C8H18)
4) Ethane (C2H4)
5) Methanol (CH3OH)
6) _____C6H12O6
7) _____C6H6
8) _____C3H7OH
9) _____C8H17OH
10) ____C6H5OH
48
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) (Hint: iron will lose 3 electrons) +
___was oxidized, ____ was reduced
Br2(l) 
___was oxidized, ____ was reduced
Decomposition
AB  A + B
1.
MgO(s) 
___was oxidized, ____ was reduced
2.
SiCl4(s) 
___was oxidized, ____ was reduced
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.
MgCl2(aq) +
3. Au(s) +
MgCl2(aq) 
F2(g) 
MgCl2(aq) 
___was oxidized, ____ was reduced
___was oxidized, ____ was reduced
___was oxidized, ____ was reduced
49
Double Replacement/Displacement
(net ionic equation and test tube results drawing
also)
AB + CD  AD + CB
1.
AgNO3(aq) +
NaBr(aq) 
Net ionic equation:
Name of product that made reaction occur:_________________
2.
MgSO4(aq) +
KCl(aq) 
Net ionic equation:
Name of product that made reaction occur:_________________
3.
KOH(aq) +
H2SO4(aq) 
Net ionic equation:
Name of product that made reaction occur:_________________
Combustion (write the full balanced reaction for each)
CxHy + O2  CO2 + H2O
1.
C2H2 +
___was oxidized, ____ was reduced
2.
C10H20 +
___was oxidized, ____ was reduced
3.
hexane (C6H14) +
___was oxidized, ____ was reduced
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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)
____ Sr(NO3)2 (aq) + ____ Na2SO4 (aq) 
2)
____ NaI(aq) + ____ Pb(NO3)2 (aq) 
3)
____ HNO3(aq) + ____ LiOH(aq) 
4)
_____Cs3N(s) 
5)
____ AlCl3 (aq) + ____ (NH4)3PO4 (aq) 
6)
____ Pb(s) + ____ Fe(NO3)3(aq) 
(Hint: lead will lose 2 electrons)
7)
____ C3H6(g) + ____ O2(g) 
8)
____ Na(s) + ____ MgSO4(aq) 
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9)
____ Na(s) + ____ O2(g) 
10)
____ C4H10(g) + ____ O2(g) 
11)
_____BrF3 
12)
______NaI(aq)
13)
_____ C8H18(l) + ____O2(g) 
14)
_____ Rb(s) + ____I2(s) 
15)
____ Al2O3 
+ _______ Br2(l)

52
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) + ____Cu2SO4(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(s) 
11. ____________ ____ H3PO4(aq)
+
LiOH(aq) 
53
Convert these word equations to formulas with the states of matter (remember, if it is D.R., the
reactants must be aqueous), predict the products, and balance. Put the reaction type in the
margin to the left of the number.
12. sodium carbonate + barium chloride 
13. potassium phosphate + magnesium
14. barium + oxygen  (the product will be solid)
15. potassium chloride + bromine 
16. ammonium sulfate + sodium chloride 
17. zinc + nickel (II) iodide 
18. solid iron (III) bromide 
19. liquid benzene (C6H6) + oxygen 
20. aluminum chloride + ammonium phosphate 
21. Calcium carbonate powder breaks down into solid calcium oxide and carbon dioxide gas.
54
22. Write the name or the chemical formula for the following compounds and indicate if it would
be soluble in water or not (aq or s).
a)
Potassium sulfate
________________
f) SnF2 ________________________
b) calcium phosphate
________________
g) Li3PO4 _______________________
c)
Lead (IV) carbonate ________________
h) BaS
_________________________
d) Sodium bromide __________________
i) Cu(OH)2
_______________________
e)
Zinc hydroxide
__________________
j) NH4Cl
_________________________
23. Write a reaction in which one of the products is solid mercury (I) chloride. Keep in mind that
the 2 reactants you chose must be aqueous.
____________
+ _____________ 
_____________
+
HgCl
(s)
Name the two reactants: ______________________________ and ____________________________
Name the two products: ______________________________ and _____________________________
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