Chemical Reactions

1
Chemical Reactions
H2
HI
1.

I2
S
Na
NaOH
2.

H2O

H2
SR
CO
CO2
3.

O2
S
KClO3
KCl
4.

O2
D
KNO3
KNO2
5.

O2
D
NaOH
Na2SO4
6.

H2SO4

H2O
DR
N2
NH3
7.

H2
S
Zn
ZnCl2
8.

AgCl

Ag
SR
P4O10
H3PO4
9.

H2O
S
2
Chemical Reactions
H2O2
H2O
10.

O2
D
Zn
ZnSO4
11.

CuSO4

Cu
SR
KOH
K3PO4
12.

H3PO4

H2O
DR
S8
SO2
13.

O2
S
C6H12O6
C2H5OH
14.

CO2
D
KCN
KCl
15.

HCl

HCN
DR
Al
Al2O3
16.

O2
S
Cu
CuCl2
17.

HCl

H2
SR
Cl2
KCl
18.

KBr

Br2
SR
3
Chemical Reactions
Si
SiCl4
19.

Cl2
S
HgO
Hg
20.

O2
D
H2
HCl
21.

Cl2
S
K
Fe
22.

FeI3

KI
SR
C
CO2
23.

O2
S
HNO3
Ba(NO3)2
24.

Ba(OH)2

H2O
DR
4
Reaction Types
-empirical formulas
A
AX

X
S
Synthesis


element or simple compound
compound
element or simple compound
AX
A
D
Decomposition



X
compound
element or simple compound
element or simple compound
AX

B
SR
Single Replacement


BX

A
element
compound
element
compound
AX

Y
AY

X
AX

BY
DR
Double Replacement


BX

AY
compound
compound
compound
compound
5
C3H8
CO2
25.

O2

H2O
element
compound
compound
compound
Combustion
AX

Y
AY

XY

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
CO2

O2

H2O
3
4
5
3 Carbon atoms
1 Carbon atom
3
8 Hydrogen atoms
2 Hydrogen atoms
8
2 Oxygen atoms
3 Oxygen atoms
7
10
10
6
H3PO4
Ca3(PO4)2
26.

Ca(OH)2

H2O
Calcium hydroxide
Hydrogen phosphate
Hydrogen hydroxide
Calcium phosphate
Ca3(PO4)2

Ca(OH)2

H2O
3
H3PO4
2
6
1 Calcium atoms
3 Calcium atoms
3
5 Hydrogen atoms
2 Hydrogen atoms
9
12
12
1 Phosphorus atoms
2 Phosphorus atoms
2
6 Oxygen atoms
9 Oxygen atoms
10
14
14
C4H10
CO2
27.

O2

H2O
Oxygen
butane
water
Carbon dioxide
CO2

O2

H2O
C4H10
10
2
8
13
4 Carbon atoms
1 Carbon atoms
8
8
10 Hydrogen atoms
2 Hydrogen atoms
20
20
2 Oxygen atoms
3 Oxygen atoms
12
26
26
7
Reaction Types
I. Synthesis
-chemical reactions in which ____ or _____
simpler substances react to form ____ ________
two
more
one
product
Mg
MgO

O2
-Example 1
2
2
S
SO2

O2
2
2
Na
NaCl

Cl2
-Example 2
2
2
H2
H2O

O2
2
2
-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
CH4
CO2

O2
1
1
-Example 1

H2O
2
2
CH3OH
CO2

O2
-Example 2
2
2

H2O
4
3
C2H5OH
CO2

O2
-Example 3
4
2

H2O
6
7
-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
SR
AX

B
BX
A

Al2(SO4)3
Li

Li2SO4
Al

2
2
3
6
1
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
Reaction Types
III. Decomposition
-chemical reactions in which ____ __________
breaks down into ____ or _____ _________ or
_________ ___________
one
compound
two
more
elements
simpler
compounds
H2O2
O2
1
2
-Example 1

H2O
2
KI
H2O
O2
-Example 2
1
2

H2
2
electricity
C3H5N3O9
N2
-Example 3

H2O

O2

CO2
Nitroglycerine
IV. Single Replacement
-chemical reactions in which the atoms of a more
__________ ________ replace the atoms of another
________ in a _________
reactive
element
element
compound
Zn
Zn(NO3)2
1
2
-Example 1

Cu
2

CuNO3
1
Mg
Mg(OH)2
1
2
-Example 2

H2
1

H2O
1
Ca
Ca(OH)2
1
2

H2
1

H2O
1
Na
NaOH
2
2

H2
1

H2O
2
Na
gt
Ca
Mg
gt
11
Reaction Types
IV. Single Replacement
-reactivity series
Cu(NO3)2
Fe(NO3)3
Zn(NO3)2
Mg(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
Reaction Types
V. Double Replacement
-chemical reaction in which both the _________
_____ and the _________ _____ exchange between
____ __________
positive
ions
negative
ions
two
compounds
NaCl
NaOH
2
1
-Example 1

Cu(OH)2
1

CuCl2
2
NaCl
NaOH
1
1
-Example 2

HOH
1

HCl
1
NaCl
NaHCO3
1
1
-Example 3

H2CO3
1

HCl
1
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-
ionize
(aq)
(aq)
Hydrogen chloride
Hydrochloric acid
13
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
NaCl
NaOH
2
1

Cu(OH)2
1

CuCl2
2
Complete Ionic Equation
Na

OH-
Cu2

Cl-

2
2
2
1
(aq)
(aq)
(aq)
(aq)
Na

Cl-

2
2
1
Cu(OH)2
(aq)
(aq)
(s)
Net Ionic Equation
OH-
Cu2

2
1
1
Cu(OH)2
(aq)
(aq)
(s)
14
Writing an Ionic Equation in a reaction that
forms water
Balanced Chemical Equation
NaCl
NaOH
1
1

HOH
1

HCl
1
Complete Ionic Equation
Na

OH-
H

Cl-

1
1
1
1
(aq)
(aq)
(aq)
(aq)
Na

Cl-

1
1
1
HOH
(aq)
(aq)
(l)
Net Ionic Equation
OH-
H

1
1
1
HOH
(aq)
(aq)
(l)
Writing an Ionic Equation in a reaction that
forms a gas
Balanced Chemical Equation
NaCl
CO2

1
NaHCO3
1
1

H2O
1

HCl
1
Complete Ionic Equation
Na

HCO3-
H

Cl-

1
1
1
1
(aq)
(aq)
(aq)
(aq)
CO2

1
Na

Cl-

1
1
1
HOH
(aq)
(aq)
(g)
(l)
Net Ionic Equation
CO2

1
HCO3-
H

1
1
1
HOH
(aq)
(aq)
(g)
(l)