Catalyst
 Fill in the table with your scores on the standards.
End
72.00
71.73
71.50
Total Score (%)
71.00
70.87
70.50
70.00
69.50
69.00
Period 5
Period 2
3.62
3.6
3.6
Average Scaled Score
3.58
3.56
3.54
3.52
3.5
3.48
3.48
3.46
3.44
3.42
Period 5
Period 2
Lead Nitrate and Sodium Chloride
Lecture 3.2 – Types of Chemical
Reactions
Today’s Learning Targets
 LT 3.2 – I can translate a chemical reaction into a net ionic
equation that contains only the ions/molecules that participate in
the chemical reaction.
 LT 3.3 – I can identify a reaction as being an acid-base,
precipitation, oxidation/reduction, decomposition, combustion,
combination, single replacement, or double replacement.
 LT 3.4 – I can hypothesize about the product(s) that would form
from the reaction between two or more reactants and write the
net ionic equation for the reaction. Furthermore, I can
hypothesize when a reaction will not occur.
Organization of Reactions
Chemical Reactions
5 Types of
Chemical
Reactions
3 Types of
Reaction
Properties
Single Replacement Reactions
 In a single replacement reaction one molecule substitutes
itself for another in a different compound.
 Example: NaNO3 + Cu  Na + CuNO3
Cu replaces Na in
the compound!
Double Replacement Reactions
 In a double replacement reaction, the two compounds in the
reaction switch the molecule that they are bonded to.
 Example: NaNO3 + KBr  NaBr + KNO3
Both compounds switch
the ion they are bonded to!
Combination Reactions
 Combination reactions are reactions whereby two or more
substances react to produce one final product.
 Example: 2Mg + O2  2MgO
Both compounds
combine to make one!
Decomposition Reaction
 In a decomposition reaction, one substance breaks apart into two
or more new substances
 Example: 2NaN3  2Na + 3N2
Compound breaks down to
two elements
Combustion Reaction
 Combustion reactions are produced from burning
hydrocarbons (compounds of hydrogen and carbon) in air
(O2). When this is done, only water and carbon dioxide are
produced.
Class Example
 Identify the types of chemical reaction shown below:
Li + F2  2LiF
Table Talk
 Identify the types of chemical reaction shown below:
C6H12O6 + 6 O2  6H2O + 6 CO2
Al + HCl  AlCl3 + H2
N2 + 3H2  2 NH3
Classifying Reactions by Elements
 We can also classify reactions based on the types of
elements/compounds and/or the reaction that proceeds.
Chemical Reactions
5 Types of
Reactions
3 Types of
Reaction
Properties
Acid/Base Reactions
 Recall that acids are substances that donate a hydrogen ions when
they are placed in water.
 Bases are substances that accept H+ when in solution. They
usually, but not always, contain an OH- ion.
 Acids react with bases in a neutralization reaction whereby a
salt and water are produced
Strong/Weak Acids and Bases
 An acid or base that completely dissociates, is a strong
acid/base.
 An acid or base that partially dissociates, is a weak acid/base.
Strong Acids/Bases
 These must be memorized!
Strong Acids
HCl
HBr
HI
HClO3
HClO4
HNO3
H2SO4
Strong Bases
Group 1A hydroxides:
LiOH
NaOH
KOH
RbOH
CsOH
Select Group 2A hydroxides:
Ca(OH)2
Sr(OH)2
Ba(OH)2
Oxidation-Reduction Reaction
 Oxidation-Reduction reactions (or redox reactions) are
reactions that involve the transfer of electrons from one
element to another element
 More to come on these types next week!
Precipitation Reaction
 Many reactions results in the production of a solid compound
know as a precipitate. These reactions are known as
precipitation reactions.
 We can determine whether or not
a solid will form based on a few
set rules.
PbNO3 reaction
Solubility Rules
 The solubility of a compound is determined by the identity of the ions in the
compound
 Whether or not a compound will dissolve in solution or form a solid depends
on the following rules:
1. All group I and ammonium ions are soluble
2. All nitrate, acetate, and chlorate compounds are soluble
3. All binary compounds of halogens (other than F) with metals are soluble,
except those of Ag, Hg (I) and Pb.
4. All sulfate containing compounds are soluble, except those of barium,
strontium, calcium, lead, silver, and mercury
5. Except for rule 1, all carbonate, hydroxide, oxide, silicate, and phosphate
containing compounds are insoluble
6. Sulfide containing compounds are insoluble, except for those with calcium,
barium, strontium, magnesium, sodium, potassium, and NH4+
Soluble Ionic Compounds
Compounds Containing
Exceptions
NO3-
None
CH3COO-
None
Cl-
Compounds of Ag+, Hg2+, Pb2+
Br-
Compounds of Ag+, Hg2+, Pb2+
I-
Compounds of Ag+, Hg2+, Pb2+
SO42-
Compounds of Sr2+, Ag+, Hg2+, Pb2+
Insoluble Ionic Compounds
Compounds Containing
Exceptions
S2-
Compounds of NH4+, the alkali metal
cations, Ca2+, Sr2+, Ba2+
CO32-
Compounds of NH4+ and the alkali metal
cations.
PO42-
Compounds of NH4+ and the alkali metal
cations.
OH-
Compounds of NH4+, the alkali metal
cations, Ca2+, Sr2+, Ba2+
Class Example
 Identify the compounds that soluble and the ones that are
insoluble:
 Na2CO3
 PbSO4
Table Talk
 Identify the compounds that soluble and the ones that are
insoluble:
 Co(OH)2
 Ba(NO3)2
Around the World
 All the reactions around the room are double displacement
reactions.
 For each reaction, write the net ionic equation that results and
determine if a precipitate forms.
 Answers are on the back side of the sheets of paper
Net Ionic Equations Lab
 Take notes from the board and make sure that they get
transferred to your lab notebook.
Lab Work Time
Closing Time
 Read sections 3.2, 4.2 and 4.3 in textbook
 Formal Lab Report due Monday/Tuesday!
 No book problems so that you can complete your lab report, but
you should memorize the solubility rules.
 Lab write up for Lab 5 due next Thursday/Friday