11.2
Types of Chemical Reactions
The heat and smoke of burning
charcoal are the products of a
combustion reaction.
Combustion is one of the five
general types of chemical
reactions. If you can recognize
a reaction as being a particular
type, you may be able to
predict the products of the
reaction.
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11.2
Classifying Reactions
Types of Chemical Reactions
>
Five general types of chemical reactions:
•
combination (synthesis)
•
decomposition
•
single-replacement
•
double-replacement
•
combustion
See websites for videos and animations
http://www.youtube.com/watch?v=i-HHvx1VC_8&NR=1
http://www.youtube.com/watch?v=tE4668aarck&feature=related
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11.2
Classifying Reactions
Combination Reactions
A combination reaction is a chemical change
in which two or more substances react to form a
single new substance.
for Conceptual Problem 11.4
11.2
Types of Chemical Reactions
>
Classifying Reactions
Decomposition Reactions
A decomposition reaction is a chemical
change in which a single compound breaks
down into two or more simpler products.
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for Conceptual Problem 11.5
11.2
Types of Chemical Reactions
>
Classifying Reactions
Single-Replacement Reactions
A single-replacement reaction is a chemical
change in which one element replaces a second
element in a compound.
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11.2
Types of Chemical Reactions
>
Classifying Reactions
The activity series of metals
lists metals in order of
decreasing reactivity.
For a single-replacement reaction to
occur, the element that is displaced
must be less active than the element
that is doing the displacing.
Metals above Hydrogen in the activity
series will replace H from acids.
Zn(s) + 2 HCl (aq) → H2 (g) + ZnCl2 (aq)
Metals below Hydrogen in the activity
series will not react with acids.
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for Conceptual Problem 11.6
11.2
Types of Chemical Reactions
>
Classifying Reactions
Double-Replacement Reactions
A double-replacement reaction is a chemical
change involving an exchange of positive ions
between two compounds.
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11.2
Types of Chemical Reactions
>
Classifying Reactions
Combustion Reactions (see regents ref tables)
A combustion reaction is a chemical change in
which an element or a compound reacts with
oxygen, often producing energy in the form of
heat and light.
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Note
your regents reference tables are helpful
for writing equations for combustion
reactions
Examples:
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11.2
Types of Chemical Reactions
>
Predicting the Products of a
Chemical Reaction
Predicting the Products of a Chemical
Reaction
How can you predict the products of the
five general types of reactions?
The number of elements and/or compounds
reacting is a good indicator of possible
reaction type and thus possible products.
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11.2
Types of Chemical Reactions
>
Predicting the Products of a
Chemical Reaction
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11.2
Types of Chemical Reactions
>
Predicting the Products of a
Chemical Reaction
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11.2
Types of Chemical Reactions
>
Predicting the Products of a
Chemical Reaction
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11.2
Types of Chemical Reactions
>
Predicting the Products of a
Chemical Reaction
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11.2
Types of Chemical Reactions
>
Predicting the Products of a
Chemical Reaction
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11.2 Section Quiz.
Assess students’ understanding
of the concepts in Section 11.2.
Continue to:
-or-
Launch:
Section Quiz
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11.2 Section Quiz.
1. What type of reaction is described by the
following equation?
6Li + N2  2Li3N
a. combination reaction
b. decomposition reaction
c. single-replacement reaction
d. combustion reaction
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11.2 Section Quiz.
2.
Balance the following equation and indicate whether it
represents a combustion, combination, or decomposition
reaction.
H2SO4  H2O2 + SO2
a. H2SO4  H2O2 + SO2, combination reaction
b. H2SO4  H2O2 + SO2, decomposition reaction
c. H2SO4  2H2O2 + SO2, combination reaction
d. H2SO4  2H2O2 + SO2, decomposition reaction
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11.3
Reactions in Aqueous Solution
Structures in limestone caverns
are formed when carbon
dioxide converts calcium
hydrogen carbonate into
calcium carbonate. The calcium
carbonate precipitates and
forms dramatic stalactites and
stalagmites. You will learn to
predict the formation of
precipitates and write
equations to describe the
reactions that produce them.
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11.3
When AgNO3 (aq) and NaCl (aq) are mixed, a white
precipitate of AgCl (s) is formed. We can write a balanced
equation to describe this double-replacement reaction:
AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)
Two other types of equations can be written for this reaction
(complete ionic equation and a net-ionic equation)
A complete ionic equation is an equation that shows
dissolved ionic compounds as dissociated free ions.
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11.3
Net Ionic Equations
An ion that appears on both sides of an
equation and is not directly involved in the
reaction is called a spectator ion.
The net ionic equation is an equation for a
reaction in solution that shows only those
particles that are directly involved in the
chemical change.
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11.3
Net Ionic Equations
Complete ionic equation:
Sodium ions and nitrate ions are not changed
during the chemical reaction of silver
nitrate and sodium chloride so the net
ionic equation is
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11.3
Predicting the Formation of a Precipitate
Predicting the Formation of a Precipitate
How can you predict the formation of a precipitate
in a double-replacement reaction?
You can predict the formation of a precipitate by
using the general rules for solubility of ionic
compounds and by using the regents reference
tables.
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11.3
Predicting the Formation of a Precipitate
Will a precipitate form when a sodium
carbonate solution is mixed with a barium
nitrate solution?
Hints: what are the products? and are those
products soluble? (Use your reference
tables).
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11.3
Predicting the Formation of a Precipitate
Balanced equation:
Ba(NO3)2 + Na2CO3 (aq)→ BaCO3 (s) + 2 NaNO3 (aq)
Complete ionic equation:
Ba2+(aq) + 2 NO3 - (aq) + 2 Na+(aq) + CO3 2- (aq)
→
BaCO3(s) + 2 Na+(aq)+ 2 NO3 - (aq)
Net Ionic equation:
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11.3 Section Quiz.
2. Which one of the following products of
double-replacement reactions would NOT
form a precipitate?
a. AgCl
b. PbSO4
c. Mg(OH)2
d. Mo(NO3)2
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11.3 Section Quiz
3. Which reaction will NOT produce a precipitate
from aqueous solution?
a. Hg2(NO3)2 + KCl
b. FeSO4 + Ba(OH)2
c. Pb(NO3)2 + Na2CO3
d. NaBr + Al2(SO4)2
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