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Types of Chemical
Reactions
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Synthesis Reactions
A + B AB
The word “synthesize” means
to produce.
How to identify:
2 elements one product.
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Synthesis Reaction Ex.
• 4Fe + 3O2 2Fe
2O
3
• Iron + Oxygen Iron (III) Oxide
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Decomposition Reactions
AB A + B
How to identify: they
always have only one
reactant.
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Decomposition Rxn. Ex.
• H2CO
3 CO
2+ H
2O
• Carbonic acid Carbon dioxide + Water
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Single Replacement
A + BC AC + B
A single metal replaces
another one in a
compound.
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Double Replacement
AB + CD AD + CB
The metals in two
compounds switch places.
(2 compounds 2 new
compounds)
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Combustion
Organic cmpd. + O2
CO2
+ H2O
An organic compound
is any compound
containing C, H, and
sometimes O.
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Predicting
Products of
Reactions
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Synthesis
Two elements
Write the formula correctly
by balancing charges.
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Synthesis cont...
Nonmetal oxide + water
Acid
Combine atoms from both
reactants. Start acid
formula with H.
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Decomposition
Binary Compound
Break into elements.
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Decomposition cont...
Metal Carbonate Metal
oxide + CO2
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Single Replacement
Metal + Compound(aq)
Use “activity series”
If the lone metal is higher than
the one in the compound there
will be a reaction.
If not, write “N.R.” in the
products.
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Ex.
2Al(s)
+ 3Pb(NO3)2(aq)
3Pb(s)
+
2Al(NO3)3(aq)
Al is more reactive (“fun”) and
kicks Pb out of the “friendship”
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Double Replacement
Compound(aq)
+ Compound(aq)
Use the Solubility Table from
your book. If both products
are SOLUBLE, write “N.R.” in
the products.
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Combustion
Organic + O2
CO2
+ H2O
Completely perfect combustion,
but not reality.
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Reactions in
Aqueous Solution
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Ions in Solution
When ionic compounds dissolve in
water they break apart:
“NaCl(aq)
” means Na+
(aq) + Cl
-
(aq)
“CaCl2(aq)
” means Ca+2
(aq)+ 2Cl
-
(aq)
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Ionic Equations
In a “complete ionic equation” you split the
aqueous compounds into their ions:
NaCl(aq)
+ AgNO3(aq)
NaNO3(aq)
+ AgCl(s)
Becomes
Na+
(aq)+ Cl
-
(aq)+ Ag
+
(aq)+ NO
3
-
(aq) Na
+
(aq)+ NO
3
-
(aq)+
AgCl(s)
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Ionic Equations
Some of the ions don’t change
from one side to the other
(Na+ and NO
3
-). They are
“spectator ions”.
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Net Ionic Equations
“Net” means
“after adjustments and deductions”.
Writing the net ionic equation you
leave the spectator ions out.
Ag+
(aq)+ Cl
-
(aq) AgCl
(s)
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Examples
Balance these, then write the
complete ionic equation:
Pb(ClO4)2(aq)
+ NaI(aq) PbI
2(s)+
NaClO4(aq)
Zn(s)
+ HCl(aq)
ZnCl2(aq)
+ H2(g)
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Examples
Now give the net ionic equation
of the two reactions.
Pb+2
(aq)+ 2I
-
(aq) PbI
2(s)
Zn(s)
+ 2H+
(aq) Zn
+2
(aq)+ H
2(g)
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Keep in Mind
When you have the SAME
coefficient for ALL of the
reactants AND products, reduce
them to ONE.