Transcript CH 8 Chemical Equations and Reactions

CH 8 Chemical Equations
and Reactions
Section 3
Classifying Chemical Reactions
5 reaction types:
 Single
Replacement (displacement)
 Double Replacement (displacement)
Combustion
Synthesis
Decomposition
Single Replacement

Also called “displacement”
Generic form:
A
+ BC 
AC + B
A single element (A) reacts with a
compound (BC), and replaces an element
from the compound.
[A kicks out B]

Single Replacement cont.

A pure metal may replace a metal (or H)
in a compound.
Cu + AgNO3

identify the pure metal:
identify the metal (or H) in the compound:
Copper is a candidate to replace silver, and it will.
Cu + AgNO3  Ag + CuNO3
Single Replacement: Activity Series
Not all metals are active enough to
replace a metal (or H) in a compound.
 The activity series ranks the elements in
order of “strength”, those high on the list
will replace those below.

Single Replacement Reactions

Identify the element in the compound to
be replaced
A)
Li + CuCl2
B)
Fe + AgNO3
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
Li
K
Ba
Sr
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Co
Ni
Sn
Pb
H
Cu
Hg
Ag
Pt
Au
Activity Series of Metals
1.
2.
3.
4.
5.
6.
7.
8.
9.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
Li
K
Ba
Sr
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Co
Ni
Sn
Pb
Li
K
Ba
Sr
Ca
Na
Mg
Al
Mn
10.Zn
11.Cr
12.Fe
13.Co
14.Ni
15.Sn
16.Pb
17.H
18.Cu
19.Hg
20.Ag
21.Pt
22.Au
Practice:
Will
 Will
 Will
 Will
 Will
 Will

calcium replace Cobalt?
Sodium replace magnesium?
Lead replace Zinc?
Lithium replace…
gold replace…
sodium replace Potassium?
Practice equations

Aluminum is dipped into Zinc Nitrate solution.

Sodium is placed into cold water.

Gold is added to a solution of calcium chloride.

Magnesium is dipped into nickel (II) chloride
solution.

Lead is placed into an iron (III) nitrate solution.

Zinc is added to a solution of copper (II) sulfate.
Predict the products of the following
reactions:

Ca + CuSO4 

Al + KNO3 
Single replacement
the “other” activity series

A more active
halogen will replace a
less active halogen
1.
F
Cl
Br
I
At
2.
3.
4.
5.
Cl2 + KI 
Cl2 + KF 
Decomposition Reactions
Generic form:

Binary Compounds



AB  A + B
Break into the elements
2 HgO  2 Hg + O2
Ternary Compounds…escaping gas


Metal Carbonate breaks into metal oxide and CO2
CaCO3 
CaO + CO2
Determine the reaction category, Predict
the products and balance them.
Br2 + NaI 
CH4 + O2 
C6H14 + O2 
Combustion Reactions
Generic form: CxHy + O2  CO2 + H2O

A hydrocarbon uses oxygen from the air
to produce Carbon Dioxide and Water.
C2H6 + O2 
CO2 +
H2 O
Complete combustion always produces
carbon dioxide and water.
A “hydrocarbon” may also include an
oxygen
C3H7OH + O2  CO2 + H2O
Synthesis (Combination)
Generic Form: A + B  AB

2 elements combine to form an ionic
compound.
2 K + Cl2  2 KCl

A metal oxide and water combine to form a
base. (a base is a hydroxide compound)
MgO + HOH  Mg(OH)2
Li2O
+ HOH  2 LiOH
Synthesis (Combination)
A non-metal oxide and water combine to form
an acid. (an acid starts with “H”)
 CO2

 SO2

+ H2O
 H2CO3
+ H2O
 H2SO3
Carbon dioxide + water  Carbonic acid
Sulfur Dioxide + water  Sulfurous acid
Double Replacement Reactions
Generic form: AB + CD  AD + CB

2 ionic compounds “switch + partners”.


A solid precipitate, a gas, or water forms
Ba(NO3)2 +
Na2SO4 
BaSO4 + NaNO3
Make sure the new ionic
compounds have no net
charge.
Types of Chemical Reactions Lab
Pb(NO3)2 + KI
Mg + HCl
H2O2 
NaHCO3 
(+heat)
Electrolysis of H2O