CH 8 Chemical Equations and Reactions
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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