Chemical Reactions
Chap. 10
I. Evidence of a Reaction
I. Evidence of a Reaction
A. Color change
I. Evidence of a Reaction
A. Color change
B. Gas produced
I. Evidence of a Reaction
A. Color change
B. Gas produced
C. Solid formed
I. Evidence of a Reaction
A.
B.
C.
D.
Color change
Gas produced
Solid formed
Heat released
II. Writing Equations
II. Writing Equations
A. + takes the place of
the word ____
II. Writing Equations
A. + takes the place of
the word ____
B.
takes the place of
the word ____
II. Writing Equations
A. + takes the place of
the word ____
B.
takes the place of
the word ____
C. Reactants
Written on the left side of the equation
Reactant
chemical that enters a
reaction. Starting
material.
II. Writing Equations
A. + takes the place of
the word ____
B.
takes the place of
the word ____
C. Reactants
D. Products
Written on the right side of the equation
Product
chemical that is formed
in a reaction.
II. Writing Equations
E. Phases
II. Writing Equations
E. Phases
1. Solid (s)
II. Writing Equations
E. Phases
1. Solid (s)
2. Liquid (l)
II. Writing Equations
E. Phases
1. Solid (s)
2. Liquid (l)
3. Gas (g)
II. Writing Equations
E. Phases
1.
2.
3.
4.
Solid (s)
Liquid (l)
Gas (g)
Aqueous (aq)
II. Writing Equations
E. Phases
F. Word Equations
Names of reactants and products written
Self Check – Ex. 1
Write the word equation
for:
K + H 2O
KOH + H2
II. Writing Equations
E. Phases
F. Word Equations
G. Chemical Equations
Symbols used in place of names
Self Check – Ex. 2
Write the chemical
equation for the reaction
that produces sulfur
dioxide and oxygen gas
when sulfur trioxide is
decomposed.
III. Balancing Equations
III. Balancing Equations
A. Law of conservation of
mass
The number and types of atoms in the
reactants must be the same in the products
III. Balancing Equations
A. Law of conservation of
mass
B. Coefficients
Numbers written before each atom or
molecule in an equation
III. Balancing Equations
A. Law of conservation of
mass
B. Coefficients
C. Significance of a
coefficient
A coefficient in front of a formula alters
the number of each atom in the formula
III. Balancing Equations
A. Law of conservation of
mass
B. Coefficients
C. Significance of a
coefficient
D. Examples
Self Check – Ex. 3
Balance this equation:
__CH4 + __O2
__CO2 + __H2O
Self Check – Ex. 4
Balance this equation:
__N2 + __H2
__NH3
Self Check – Ex. 5
Balance this equation:
__Na2CO3 + __ HCl
__NaCl + __H2O + ___CO2
IV. Types of Reactions
IV. Types of Reactions
A. Synthesis
IV. Types of Reactions
A. Synthesis
1. Two or more reactants,
and one product
IV. Types of Reactions
A. Synthesis
1. Two or more reactants,
and one product
2. A + B
AB
Self Check – Ex. 6
Aluminum reacts with
chlorine in a synthesis
reaction. Write the
equation.
IV. Types of Reactions
A. Synthesis
B. Decomposition
IV. Types of Reactions
A. Synthesis
B. Decomposition
1. Two or more products,
and one reactant
IV. Types of Reactions
A. Synthesis
B. Decomposition
1. Two or more products,
and one reactant
2. AB
A + B
Self Check – Ex. 7
When potassium chlorate is
heated it decomposes into
potassium chloride and
oxygen gas. Write the
equation.
IV. Types of Reactions
A. Synthesis
B. Decomposition
C. Single Replacement
IV. Types of Reactions
A. Synthesis
B. Decomposition
C. Single Replacement
1. An element reacts with a
compound.
IV. Types of Reactions
A. Synthesis
B. Decomposition
C. Single Replacement
1. An element reacts with a
compound.
2. A + BX
AX + B
IV. Types of Reactions
A. Synthesis
B. Decomposition
C. Single Replacement
1. An element reacts with a
compound.
2. A + BX
AX + B
3. An element must be more
active in order to replace
another.
Activity series for metals
Li
K
Ca
Na
Mg
Al
Zn
Fe
Ni
Pb
Ag, Pt, Au
Activity series for metals
Most active
Least active
Li
K
Ca
Na
Mg
Al
Zn
Fe
Ni
Pb
Ag, Pt, Au
IV. Types of Reactions
D. Double Replacement
IV. Types of Reactions
D. Double Replacement
1. A compound reacts with
another compound and
the positive ions switch.
IV. Types of Reactions
D. Double Replacement
1. A compound reacts with
another compound and
the positive ions switch.
2. AX + BY
AY + BX
IV. Types of Reactions
D. Double Replacement
1. A compound reacts with
another compound and
the positive ions switch.
2. AX + BY
AY + BX
3. Produce an insoluble
solid, a gas, or water.
IV. Types of Reactions
A.
B.
C.
D.
E.
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
Burning a fuel in the presence of oxygen
Self Check – Ex. 10
Write the equation for the
combustion of ethane, C2H6
Self Check – Ex. 11
Write the equation for the
combustion of methanol,
CH3OH.