CP Chapter 11 Notes
Reactions and Equations
Evidence of Chemical Reactions
 How can you tell a _________________ reaction has taken place?
– Temperature change
– Color change
– _________________
– Gas/bubbles
– Appearance of a _________________ (precipitate)
Chemical Reaction
 A chemical reaction is the process by which atoms of one or more substances are
_________________ to form _________________ substances.
Question Time
 What are the signs that a chemical reaction has taken place?
 What is a chemical reaction?
Reactant(s) and Product(s)
 Reactant(s) are the _________________ substance(s) of a reaction
 Product(s) are the substance(s) formed _________________ the reaction
  means “react to produce” or “yield”
 Reactant(s) are on the left
 Product(s) are on the _________________
Representing Chemical Reactions
 reactant A+ reactant B  product C + product D
 The plus sign _________________ each reactant or product
 (s) Identifies solid state
 (l) Identifies _________________ state
 (g) Identifies gaseous state
 (aq) Identifies _________________ solution
  - ________________is applied to the reaction
 Example

 NH4NO3(s)
 N2O(g) + 2H2O(g)
Question Time
 What are reactants?
 What are products?
 What does “” mean in a chemical reaction?
 Where are the reactants located in a written chemical reaction?
 Where are the products located in a written chemical reaction?
Word Equation
 Uses _________________ not chemical symbols to indicate the _________________ (s) and
product(s) of a chemical reaction.
– Example iron(s) + chlorine(g) iron(III) _________________ (s)
Skeleton Equation
 Skeleton equation uses _________________rather than words to identify the reactant(s) and
product(s)
– Example _________________ (s) + Cl2(g)  FeCl3(s)
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Balanced Chemical Equation
 The equation that shows the _________________ of atoms of each reactant and each product
is _________________ on both sides of the arrow is a _________________ chemical equation
– Example 2Fe(s) + 3Cl2(g)  2FeCl3(s)
Question Time
 What is a word equation?
 What is a skeleton equation?
 What is a balanced chemical equation?
Balancing Equations
Step 1

Step 2


Step 3


Step 4



Step 5


Write the _________________ equation.
Balance each element by placing _________________in front of the chemical formulas.
Balance in this order:
– metals
– non-metals
– hydrogen
– oxygen _________________
Select coefficients that will give the _________________number of atoms on each side of the
equation.
If you have an _________________number of oxygen atoms, multiply the coefficient by
______ first to make it an even number. Then try to balance the equation.
Check all other elements to see whether the equation is _________________.
Other elements may have become unbalanced.
Make _________________to balance all the elements.
If it becomes difficult to balance an equation, use a _________________ as a coefficient then
_________________to get rid of the fraction.
Balance these equations.
1.
HgO

Hg
+
O2
2.
Mg
+
O2

MgO
3.
KClO3

KCl
+
O2
4.
AgNO3
+
H2S

Ag2S
5.
Al(OH)3
+
H2SO4 
Al2(SO4)3
+
H2O
6.
Zn(OH)2
+
H3PO4 
Zn3(PO4)2
+
H2O
7.
FeCl3
+
NaOH 
Fe(OH)3
+
NaCl
2
+
HNO3
Types of Reactions
Five Types of Reactions
 There are _________________different types of reactions
– Synthesis/Combination Reaction
– _________________Reaction
– Decomposition Reaction
– Single-replacement Reaction
– Double-_________________Reaction
Synthesis/Combination Reaction
 A+B __________
 2Fe(s) + 3Cl2(g)  2FeCl3(s)
 CaO(s) + H2O(l)  Ca(OH)2(s)
 Two or more substances react to produce a _________________product
 To tell if it is a synthesis/combination reaction, one product is formed from two or more
____________
Combustion Reaction
 In a combustion reaction _________________combines with a substance and
_________________ energy.
 Oxygen (O2) is a _________________in a combustion reaction
Example: 2H2(g) + O2(g)  2H2O(g)
 In the combustion of a hydrocarbon (molecule with just hydrogen and carbon)
_________________and carbon dioxide are produced
 Ex: CH4(g) + O2(g)  CO2(g) + H2O(g)
Question Time
 How can you tell if there is a synthesis/combination reaction?
 How can you tell if there is a combustion reaction?
 Determine if the reaction is synthesis/combination or combustion
– 2Na + Cl2  2NaCl
– C(s) + O2(g)  CO2(g)
Decomposition Reaction
 In a decomposition reaction a _________________compound breaks down into two or more
________ elements or compounds
 AB  A + B
 2NaN3(s)  2Na(s) + 3N2(g)
 One reactant breaks up into two or more _________________.
 To tell if it is a decomposition reaction, there is only one reactant forming two or more products
Single Replacement Reactions
 Single replacement reactions are when atoms of one element _________________the atoms
of another element in a compound.
 A + BX  AX + B
 2Li(s) + 2H2O(l)  2LiOH(aq) + H2(g)
 To tell if it is a single replacement reaction, a _________________, H2 or a halogen is by itself.
Like a “boyfriend thief”
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Double Replacement Reactions
 A double replacement reaction is when there is an _________________of ions between
________ compounds.
 AX + BY  AY + BX
 Ca(OH)2(aq) +2HCl(aq)  CaCl2(aq) + 2H2O(l)
 To tell if it is a double replacement reaction, there are two compounds reacting with each other
forming two _________________compounds
Question Time
 How can you tell if there is a decomposition reaction?
 What is a single replacement reaction and how can you tell if there is one?
 What is a double replacement reaction and how can you tell if there is one?
Single Replacement Reactions
Single Replacement Reaction: A + BX 
Metals will replace _______________ or ________________
Halogens will replace ______________
If an ion can take on two different charges, we will use the _____ charge for this worksheet.
Metals + H2O 
H2 + __________OH
You must use the Activity Series Chart to find out if the reaction takes place.
For each reaction use the activity series to complete the reaction. If no reaction will occur, write “no
reaction. Make sure to balance your final answer.
Most reactive
AgNO3 ___________________________________
1.
Zn
+
2.
Cl2
+
KI ___________________________________
3.
Ag
+
KNO3 ___________________________________
4.
Mg
+
HCl ___________________________________
5.
Fe
+
CuSO4 ___________________________________
6.
Al
+
CuSO4 ___________________________________
7.
Br2
+
CaI2 ___________________________________
8.
Mg
+
H2SO4 ___________________________________
9.
Cu
+
H2O
___________________________________
Least reactive
10.
Fe
+
AgC2H3O2 ___________________________________
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Activity Series
Metals
Non-metals
Li
F2
Rb
Cl2
K
Br2
Cs
I2
Ba
Sr
Ca
Na
Mg
Al
Ti
Mn
Zn
Cr
Fe
Cd
Co
Ni
Sn
Pb
H
Sb
Bi
Cu
Hg
Ag
Pt
Au
Double Replacement Reactions
AY + BX  AX + BY
DR Reactions Equation: _____________________________________
One of Three things happens in a DR Reaction:
1. ___________________ (s)
2. ___________________(l)
Or __________________(aq)
3. ___________________(g)
________
________
________
If both products are ___________________ then there will be no __________________.
Use the Solubility Chart to predict if a substance is soluble or insoluble.
1. Na3PO4____________________ 4. Fe(OH)3__________________
2. PbBr2______________________ 5. AlCl3_____________________
3. CaCl2______________________ 6. NaCl______________________
Complete and balance the equations for the following double-replacement reactions. Write “(s)” next to
the product that is insoluble, “(aq)” next to the product that is soluble, or “(l)” next to water. If no reaction
takes place write “NR.”
1.
AgNO3(aq)
+
NaCl(aq)  _______________________________________
2.
Mg(NO3)2(aq)
+
KOH(aq) _______________________________________
3.
NaNO3(aq)
+
K3PO4(aq) _______________________________________
4.
HI(aq)
+
Li2S(aq) _______________________________________
5.
AgNO3(aq)
+
KCl(aq) _______________________________________
6.
HCl(aq)
+ Na2CO3(aq) _______________________________________
7.
H2SO4 (aq)
+
Mg(OH)2(aq) _______________________________________
8.
KCN(aq)
+
HBr(aq) _______________________________________
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Activity Series
Metals
Li
Rb
K
Cs
Ba
Sr
Ca
Na
Mg
Al
Ti
Zn
Cr
Fe
Ni
Sn
Pb
*H
Cu
Ag
Pd
Hg
Pt
Au
Nonmetals
F2
Cl2
Br2
I2
Most Reactive
Least Reactive
SOLUBILITY CHART
NEGATIVE ION
(ANION)
PLUS
POSITIVE ION
(CATION)
any negative ion
any negative ion
nitrate (NO3-)
acetate (C2H3O2-)
+
+
+
+
chloride (Cl-),
bromide (Br-), or
iodide (I-)
sulfate (SO4-2)
+
alkali metal ions
ammonium (NH4+)
any positive ion
any positive ion except Ag+ or
Hg+
Ag+, Pb+2, Hg+, or Cu+
+
+
any other positive ion
Ca+2, Sr+2, Ba+2, Ra+2, Ag+, or Pb+2
soluble
not soluble
sulfide (S-2)
+
+
any other positive ion
alkali metal ions, NH4+, Be+2, Mg+2,
Ca+2, Sr+2, Ba+2, or Ra+2
soluble
soluble
hydroxide (OH-)
+
+
any other positive ion
alkali metal ions or NH4+
not soluble
soluble
+
+
any other positive ion
alkali metal ions or NH4+
not soluble
soluble
+
any other positive ion
not soluble
phosphate (PO4-3),
carbonate (CO3-2),
or sulfite (SO3-2)
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FORMS A
COMPOUND
WHICH IS:
soluble
soluble
soluble
soluble
not soluble