Download Types of Chemical Reactions

Types of Chemical Reactions
A + B  AB
Synthesis (Combination) reaction
AB  A + B
Decomposition reaction
ASingle-replacement
A + BC  AC + B
reaction
element
BDouble-replacement
reaction
Polymerization
Ause
activity series to predict
Bdriving
force…water, gas, or precipitate
element
compound
compound
compound
HX + BOH  BX + HOH
acid
Combustion reaction (of a hydrocarbon)
compound
AB + CD  AD + CB
compound
Neutralization reaction
compound
base
salt
water
CH + O2  CO2 + H2O
Polymer = monomer + monomer + …
Types of Chemical Reactions
Synthesis (Combination) reaction
Decomposition reaction
ASingle-replacement
reaction
BDouble-replacement
reaction
Neutralization reaction
Combustion reaction (of a hydrocarbon)
Polymerization
Ause
activity series to predict
Bdriving
force…water, gas, or precipitate
A + B  AB
AB  A + B
A + BC  AC + B
AB + CD  AD + CB
HX + BOH  BX + HOH
CH + O2  CO2 + H2O
Polymer = monomer + monomer + …
Chemical Equations
Synthesis Reaction
Direct combination reaction (Synthesis)
2 Na
+
Na
Cl2
Cl
Cl

2 NaCl

Na
General form: A
element or
compound
+
B
element or
compound

AB
compound
Synthesis Reaction
Direct combination reaction (Synthesis)
2 Na
+

Cl2
Na
2 NaCl
Cl
Na+ Cl -
Cl
Cl - Na+
Na
General form: A
element or
compound
+
B
element or
compound

AB
compound
Formation of a solid: AgCl
AgNO3(aq) + KCl(aq)  KNO3 (aq) + AgCl(s)
lead (II) chloride + potassium iodide
K1+
Pb2+ Cl1PbCl2
+
I1-
KI
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
potassium chloride + lead (II) iodide
Pb2+ Cl1KCl (aq)
K1+
+
I1-
PbI2 (ppt)
lead (II) chloride + potassium iodide
K1+
Pb2+ Cl1PbCl2
+
I1-
KI
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
potassium chloride + lead (II) iodide
Pb2+ Cl1KCl (aq)
K1+
+
I1-
PbI2 (ppt)
Decomposition Reaction
Decomposition reaction
2 H2 O
2 H2
+
O2
H
O
H
+
H
O
H
General form: AB
compound
A
+
B
two or more elements
or compounds
Single and Double Replacement
Reactions
Single-replacement reaction
Mg
+
CuSO4
General form:
A
+ BC

MgSO4

AC
+
+
Cu
B
Double-replacement reaction
CaCO3
+
General form:
AB
+
2 HCl

CaCl2
+
H2CO3
CD

AD
+
CB
Printable
Version
of
Activity
Series
Activity Series
Element Reactivity
Ca
Foiled again –
Aluminum loses to Calcium
Li
Rb
K
Ba
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Ni
Sn
Pb
H2
Cu
Hg
Ag
Pt
Au
Halogen Reactivity
F2
Cl2
Br2
I2
acetate
bromide
carbonate
chloride
chromate
hydroxide
iodide
nitrate
phosphate
sulfate
sulfide
TABLE OF SOLUBILITIES IN WATER
aluminum
ss
s
n
s
n
i
s
s
i
s
d
ammonium
s
s
s
s
s
s
s
s
s
s
s
barium
s
s
i
s
i
s
s
s
i
i
d
calcium
s
s
i
s
s
ss
s
s
i
ss
d
copper (II)
s
s
i
s
i
i
n
s
i
s
i
iron (II)
s
s
i
s
n
i
s
s
i
s
i
iron (III)
s
s
n
s
i
i
n
s
i
ss
d
lead
s
ss
i
ss
i
i
ss
s
i
i
i
magnesium
s
s
i
s
s
i
s
s
i
s
d
mercury (I)
ss
i
i
i
ss
n
i
s
i
ss
i
mercury (II)
s
ss
i
s
ss
i
i
s
i
d
i
potassium
s
s
s
s
s
s
s
s
s
s
s
silver
ss
i
i
i
ss
n
i
s
i
ss
i
sodium
s
s
s
s
s
s
s
s
s
s
s
zinc
s
s
i
s
s
i
s
s
i
s
i
Legend
SOLID
i = insoluble
SOLIDsoluble
ss = slightly
AQUEOUS
s = soluble
d = decomposes
n = not isolated
acetate
bromide
carbonate
chloride
chromate
hydroxide
iodide
nitrate
phosphate
sulfate
sulfide
TABLE OF SOLUBILITIES IN WATER
aluminum
s
aq
n
s
n
s
aq
aq
s
aq
d
ammonium
aq
aq
aq
aq
aq
aq
aq
aq
aq
aq
aq
barium
aq
aq
s
aq
s
aq
aq
aq
s
s
d
calcium
aq
aq
s
aq
aq
ss
aq
aq
s
s
d
copper (II)
aq
aq
s
aq
s
s
n
aq
s
aq
s
iron (II)
aq
aq
s
aq
n
s
s
aq
s
aq
s
iron (III)
aq
aq
n
aq
s
s
n
aq
s
s
d
lead
aq
s
s
ss
s
s
s
aq
s
s
s
magnesium
aq
aq
s
aq
aq
s
aq
aq
s
aq
d
mercury (I)
s
s
s
s
s
n
s
aq
s
s
si
mercury (II)
aq
s
s
aq
s
s
s
aq
s
d
si
potassium
aq
aq
aq
aq
aq
aq
aq
aq
aq
aq
aq
silver
s
s
s
s
s
n
s
s
s
s
s
sodium
aq
aq
aq
aq
aq
aq
aq
aq
aq
aq
aq
zinc
aq
aq
s
aq
aq
s
aq
aq
s
aq
s
Legend
s = solid
aq = aqueous
d = decomposes
n = not isolated
acetate
bromide
carbonate
chloride
chromate
hydroxide
iodide
nitrate
phosphate
sulfate
sulfide
TABLE OF SOLUBILITIES IN WATER
aluminum
ss
s
n
s
n
i
s
s
i
s
d
ammonium
s
s
s
s
s
s
s
s
s
s
s
barium
s
s
i
s
i
s
s
s
i
i
d
calcium
s
s
i
s
s
ss
s
s
i
ss
d
copper (II)
s
s
i
s
i
i
n
s
i
s
i
iron (II)
s
s
i
s
n
i
s
s
i
s
i
iron (III)
s
s
n
s
i
i
n
s
i
ss
d
lead
s
ss
i
ss
i
i
ss
s
i
i
i
magnesium
s
s
i
s
s
i
s
s
i
s
d
mercury (I)
ss
i
i
i
ss
n
i
s
i
ss
i
mercury (II)
s
ss
i
s
ss
i
i
s
i
d
i
potassium
s
s
s
s
s
s
s
s
s
s
s
silver
ss
i
i
i
ss
n
i
s
i
ss
i
sodium
s
s
s
s
s
s
s
s
s
s
s
zinc
s
s
i
s
s
i
s
s
i
s
i
Legend
s = solid
aq = aqueous
d = decomposes
n = not isolated
Solubility Rules
1.
Most nitrates are soluble.
2.
Most salts containing Group I ion and ammonium ion, NH4+, are soluble.
3.
Most chloride, bromide, and iodide salts are soluble, except Ag+, Pb2+
and Hg22+.
4.
Most sulfate salts are soluble, except BaSO4, PbSO4, Hg2SO4, and CaSO4.
5.
Most hydroxides except Group 1 and Ba(OH)2, Sr(OH)2, and Ca(OH)2 are
only slightly soluble.
6.
Most sulfides, carbonates, chromates, and phosphates are only slightly
soluble.
Ohn-Sabatello, Morlan, Knoespel, Fast Track to a 5 Preparing for the AP Chemistry Examination 2006, page 91
Potassium reacts with Water
POW!
Double Replacement Reaction
K2CO3 (aq)
Potassium carbonate
+
BaCl2 (aq)
Barium chloride
2 KCl (aq)
Potassium chloride
+
BaCO3 (s)
Barium carbonate
Synthesis Reactions
Photosynthesis
6 CO2 + 6 H2O
C6H12O6 +
Formation of water
2 H2 + O2
2 H2O
Formation of salt
2 Na + Cl2
2 NaCl
General Form
A + B
C
6 O2
Decomposition Reactions
Hydrogen Peroxide
2 H2O2
2 H2O
+
2 H2
+
O2
Electrolysis of water
2 H2O
electricity
O2
Nitrogen triiodide
2 NI3
N2
+ 3 I2
General Form
AB
A + B
Predict if these reactions will occur
3 Mg
+ 2 AlCl3
2 Al
+ 3 MgCl2
Can magnesium replace aluminum? YES, magnesium is more reactive than aluminum.
Activity Series
Al
+
MgCl2
No reaction
Can aluminum replace magnesium? NO, aluminum is less reactive than magnesium.
Activity Series
MgCl2
+
Al
Therefore, no reaction will occur.
No reaction
Order of reactants
DOES NOT
determine how
they react.
The question we must ask is can the single element replace its counterpart?
metal replaces metal or nonmetal replaces nonmetal.
Single-Replacement Reactions
Activity Series
“Magic blue-earth”
Fe + CuCl2
FeCl2
+
Cu
Can Fe replace Cu? Yes
Zinc in nitric acid
Zn
+ 2 HNO3
Can Zn replace H?
Zn(NO3)2
+ H2
Yes
NO REACTION
MgCl2
+
Can Br replace Cl?
Br2
MgBr2
+
No
General Form
A
+
BC
AC + B
Cl2
Li
Rb
K
Ba
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Ni
Sn
Pb
H2
Cu
Hg
Ag
Pt
Au
F2
Cl2
Br2
I2
How would you prepare potassium nitrate
(using a double replacement reaction)?
KKOH
NO33
HHNO
OH ++ _________
_________
Ca(NO3)2
2 KOH + Ca(NO3)2
formation of water
is a driving force.
KNO3 ++ _________
H2O
Both potassium nitrate and
calcium chloride are soluble
(no driving force – no reaction!)
2 KNO3 + Ca(OH)2
Combine a potassium hydroxide solution with nitric acid
to yield soluble potassium nitrate.
KOH(aq) + HNO3(aq)
KNO3(aq) + H?2O
The water could then be removed by distillation to recover solid potassium nitrate.
Predict if a reaction will occur when you combine aqueous solutions
of iron (II) chloride with aqueous sodium carbonate solution.
If the reaction does occur, write a Balanced
balanced chemical equation showing it.
(be sure to include phase notation)
iron (II) chloride + sodium carbonate
Fe2+ Cl1-
Na1+ CO32-
FeCl2
Na2CO3
sodium chloride + iron (II) carbonate
Na1+ CO32-
Fe2+ Cl1-
FeCO3 (ppt)
NaCl (aq)
Using a SOLUBILITY TABLE:
sodium chloride is soluble
iron (II) carbonate is insoluble
FeCl2 (aq)
+
Na2CO3 (aq)
Complete Ionic Equation
Fe2+(aq) + 2Cl1-(aq) + 2Na1+(aq) + CO32-(aq)
2 NaCl (aq)
+
FeCO3 (ppt)
2Na1+(aq) + 2Cl1-(aq) + FeCO3(s)