1. Chemical Reactions 1. H2 + I2 HI S 2. Na +
H2O
NaOH + H2 SR 3. CO + O2
CO2 S 4.
KClO3
KCl + O2 D 5.
KNO3
KNO2 + O2 D 6.
NaOH +
H2SO4
Na2SO4 +
H2O DR 7. N2 + H2
NH3 S 8. Zn +
AgCl
ZnCl2 + Ag SR 9.
P4O10 +
H2O
H3PO4 S

2. Chemical Reactions
10.
H2O2
H2O + O2 D
11. Zn +
CuSO4
ZnSO4 + Cu SR
12.
KOH +
H3PO4
K3PO4 +
H2O DR
13. S8 + O2
SO2 S
14.
C6H12O6
C2H5OH +
CO2 D
15.
KCN +
HCl
KCl +
HCN DR
16. Al + O2
Al2O3 S
17. Cu +
HCl
CuCl2 + H2 SR
18.
Cl2 +
KBr
KCl +
Br2 SR

3. Chemical Reactions
19. Si +
Cl2
SiCl4 S
20.
HgO Hg + O2 D
21. H2 +
Cl2
HCl S
22. K +
FeI3 Fe + KI SR
23. C + O2
CO2 S
24.
HNO3 +
Ba(OH)2
Ba(NO3)2 +
H2O DR

4. Reaction Types -empirical formulas S = Synthesis = A + X AX D =
element or
simple
compound
element or
simple
compound
compound D =
Decomposition = AX A + X
compound
element or
simple
compound
element or
simple
compound SR =
Single Replacement = AX + B BX + A
compound
element
compound
element AX + Y AY + X DR =
Double Replacement = AX + BY BX + AY
compound
compound
compound
compound

5. -balancing an equation -the Law of Conservation of Matter states that
25.
C3H8 + O2
CO2 +
H2O
compound
element
compound
compound AX + Y AY + XY =
Combustion
Chemical Reactions
-balancing an equation
-the Law of Conservation of Matter states that
matter is neither created or destroyed by ordinary
chemical means, only changed in form
C3H8 + 5 O2 3
CO2 + 4
H2O
3 Carbon atoms 3
1 Carbon atom
8 Hydrogen atoms 8
2 Hydrogen atoms 10
2 Oxygen atoms 10 7
3 Oxygen atoms

6. 26. H3PO4 + Ca(OH)2 Ca3(PO4)2 + H2O 2 H3PO4 + 3 Ca(OH)2 Ca3(PO4)2 + 6
Hydrogen phosphate
Calcium hydroxide
Calcium phosphate
Hydrogen hydroxide 2
H3PO4 + 3
Ca(OH)2
Ca3(PO4)2 + 6
H2O 3
1 Calcium atoms
3 Calcium atoms 12 9
5 Hydrogen atoms 12
2 Hydrogen atoms 2
1 Phosphorus atoms
2 Phosphorus atoms 14 10
6 Oxygen atoms 14
9 Oxygen atoms
27.
C4H10 + O2
CO2 +
H2O
butane
Oxygen
Carbon dioxide
water 2
C4H10 + 13 O2 8
CO2 + 10
H2O 8
4 Carbon atoms 8
1 Carbon atoms 20
10 Hydrogen atoms 20
2 Hydrogen atoms 26
2 Oxygen atoms 26 12
3 Oxygen atoms

7. Reaction Types
I. Synthesis
-chemical reactions in which ____ or _____ simpler
substances react to form ____ ________
two
more
one
product
-Example #1: 2 Mg + O2 2
MgO 2 S + O2 2
SO2
-Example #2: 2 Na +
Cl2 2
NaCl 2 H2 + O2 2
H2O
-each of the four examples of chemical reactions are
also ____________, as _____ energy is _________ in
the formation of ____ ______ than is required to break
the bonds in the initial __________
exothermic
more
released
new
bonds
reactants

8. Reaction Types
II. Combustion
-chemical reactions in which _______ combines
with a substance to form ____ or _____ _______
and releases ______ in the forms of ____ and _____
oxygen
one
more
oxides
energy
heat
light
-Example #1: 1
CH4 + 2 O2 1
CO2 + 2
H2O
-Example #2: 2
CH3OH + 3 O2 2
CO2 + 4
H2O
-Example #3: 2
C2H5OH + 7 O2 4
CO2 + 6
H2O
-each of the four examples of chemical reactions are
also ____________, as _____ energy is _________ in
the formation of ____ ______ than is required to break
the bonds in the initial __________, and the ________
are _____ stable than the __________
exothermic
more
released
new
bonds
reactants
products
more
reactants

9. Predicting and Balancing Equations
Aluminum sulfate +
Lithium
Lithium sulfate +
Aluminum
compound
element
compound
element AX + B SR BX + A 1
Al2(SO4)3 + 6 2 Li 3
Li2SO4 + 2 Al
1. Identify the type of substances in the reactants or products
2. Identify the reaction type, using empirical formulas
3. Using empirical formulas, predict the names of the products
4. Write correct chemical formulas for reactants and products
5. Use coefficients to balance equation

10. -chemical reactions in which ____ __________
Reaction Types
III. Decomposition
-chemical reactions in which ____ __________
breaks down into ____ or _____ _________ or
_________ ___________
one
compound
two
more
elements
simpler
compounds
-Example #1: 2
H2O2 1 O2 + 2
H2O KI
-Example #2: 2
H2O 1 O2 + 2 H2
electricity
-Example #3:
C3H5N3O9 N2 +
CO2 +
H2O + O2
Nitroglycerine
IV. Single Replacement
-chemical reactions in which the atoms of a
more __________ ________ replace the
atoms of another ________ in a _________
reactive
element
element
compound
-Example #1: 1 Zn + 2
CuNO3 1
Zn(NO3)2 + 2 Cu
-Example #2: 1 Mg + 2
H2O 1
Mg(OH)2 + 1 H2 1 Ca + 2
H2O 1
Ca(OH)2 + 1 H2 2 Na + 2
H2O 2
NaOH + 1 H2 Na
> Ca
> Mg

11. Reaction Types IV. Single Replacement -reactivity series - + + + - - -
Mg(NO3)2
Cu(NO3)2
Fe(NO3)3
Zn(NO3)2 - + + + Mg - - - - Cu - - - Fe + - + + - Zn
1. Write a complete balanced equation for each reaction that took place: a. b. c. d. e. f.
2. List the four metals, in order, from most reactive to least reactive:

12. -chemical reaction in which both the
Reaction Types
V. Double Replacement
-chemical reaction in which both the
_________ _____ and the _________ _____
exchange between ____ __________
positive
ions
negative
ions
two
compounds
-Example #1: 2
NaOH + 1
CuCl2 2
NaCl + 1
Cu(OH)2
-Example #2: 1
NaOH + 1
HCl 1
NaCl + 1
HOH
-Example #3: 1
NaHCO3 + 1
HCl 1
NaCl + 1
H2CO3
VI. Reactions in Aqueous Solutions
-some ___________ compounds
such as ________ or ________
dissolve in water, because they
are ______, like water
molecular
sucrose
ethanol
polar
-some ___________ compounds
such as ________________
dissolve in water, but because
they are extremely ______, they
________ in water
molecular
Hydrogen chloride
polar
HCl H+ +
Cl-
(aq)
(aq)
ionize
Hydrogen chloride
Hydrochloric acid

13. VI. Reactions in Aqueous Solutions -when ______ compounds
Reaction Types
VI. Reactions in Aqueous Solutions
-when ______ compounds
dissolve in water, (being already
made up of _____), they
___________, or _______ from
each other
ionic
ions
NaOH
Na+ +
OH-
dissociate
separate
(aq)
(aq)
Sodium hydroxide
-______ ___________ reactions
often take place in ________
__________
double
replacement
aqueous
solutions
Writing an Ionic Equation – in a reaction that forms a precipitate
Balanced Chemical Equation 2
NaOH + 1
CuCl2 2
NaCl + 1
Cu(OH)2
Complete Ionic Equation 2
Na+ + 2
OH- + 1
Cu2+ + 2
Cl-
(aq)
(aq)
(aq)
(aq) 2
Na+ + 2
Cl- + 1
Cu(OH)2
(aq)
(aq)
(s)
Net Ionic Equation 2
OH- + 1
Cu2+ 1
Cu(OH)2
(aq)
(aq)
(s)

14. Writing an Ionic Equation – in a reaction that forms water
Balanced Chemical Equation 1
NaOH + 1
HCl 1
NaCl + 1
HOH
Complete Ionic Equation 1
Na+ + 1
OH- + 1 H+ + 1
Cl-
(aq)
(aq)
(aq)
(aq) 1
Na+ + 1
Cl- + 1
HOH
(aq)
(aq)
(l)
Net Ionic Equation 1
OH- + 1 H+ 1
HOH
(aq)
(aq)
(l)
Writing an Ionic Equation – in a reaction that forms a gas
Balanced Chemical Equation 1
NaHCO3 + 1
HCl 1
NaCl + 1
H2O + 1
CO2
Complete Ionic Equation 1
Na+ + 1
HCO3- + 1 H+ + 1
Cl-
(aq)
(aq)
(aq)
(aq) 1
Na+ + 1
Cl- + 1
HOH + 1
CO2
(aq)
(aq)
(l)
(g)
Net Ionic Equation 1
HCO3- + 1 H+ 1
HOH + 1
CO2
(aq)
(aq)
(l)
(g)