Chapter 9 honors

Chemical Reactions
• The process by which one or more
substances are rearranged to form different
substances is called a chemical reaction.
And rummy tummmy

Chemical Reactions (cont.)
• Evidence of a chemical reaction
– Change in temperature
– Change in color
– Odor, gas, or bubbles may form.

Representing Chemical Reactions
• Chemists use statements called equations
to represent chemical reactions.
• Reactants are the
starting substances.
• Products are the
substances formed in
the reaction.
• This table summarizes
the symbols used in
chemical equations.

Diatomic elements
• There are 8 elements that never want to
be alone.
• They form diatomic molecules.
• H2 , N2 , O2 , F2 , Cl2 , Br2 , I2 , and At2
• The –ogens and the –ines
• 1 + 7 pattern on the periodic table

Representing Chemical Reactions (cont.)
• In word equations, aluminum(s) +
bromine(l) → aluminum bromide(s) reads
as “aluminum and bromine react to
produce aluminum bromide”.
• Skeleton equations use symbols and
formulas to represent the reactants and
products.
Al(s) + Br2(l) → AlBr3(s)
• Skeleton equations lack information about
how many atoms are involved in the reaction.

Convert these to equations
• Solid iron (III) sulfide reacts with gaseous
hydrogen chloride to form iron (II) chloride
and hydrosulfuric acid gas.
• Nitric acid dissolved in water reacts with
solid sodium carbonate to form liquid
water and carbon dioxide gas and sodium
nitrate dissolved in water.

The other way
• Fe(s) + O2(g) → Fe2O3(s)
• Cu(s) + AgNO3(aq) →
Ag(s) + Cu(NO3)2(aq)

Representing Chemical Reactions (cont.)
• A chemical equation is a statement that
uses chemical formulas to show the
identities and relative amounts of the
substances involved in a chemical reaction.

Balancing Chemical Equations
• The most fundamental law in chemistry is
the law of conservation of mass.
• Balanced equations show this law.

• Atoms can’t be created or destroyed
• All the atoms we start with we must end
up with
• A balanced equation has the same
number of each element on both sides of
the equation.

Balancing Chemical Equations
• This figure shows the balanced equation
for the reaction between aluminum and
bromine.

Balancing Chemical Equations (cont.)
• A coefficient in a chemical equation is the
number written in front of a reactant or
product, describing the lowest whole-number
ratio of the amounts of all the reactants and
products.

Rules for balancing
• 1 Write the correct formulas for all the
reactants and products
• 2 & 3 Count the number of atoms of each
type appearing on both sides
• 4 Balance the elements one at a time by
adding coefficients (the numbers in front)
• 5 Reduce if necessary
• 6 Check to make sure it is balanced.

Never
• Never change a subscript to balance an
equation.
• If you change the formula you are
describing a different reaction.
• H2O is a different compound than H 2O2
• Never put a coefficient in the middle of a
formula
• 2 NaCl is okay, Na2Cl is not.

Example
H2 + O2 → H2O

Make a table to keep track of the elements

Example
H2 + O2 → H2O

R P
2 H 2
2 O 1

Need twice as much O in the product

Example
H2 + O 2 → 2H O
2

R P
2 H 2
2 O 1

Changes the O

Example
H2 + O 2 → 2H O
2

R P
2 H 2
2 O 1 2

Also changes the H

Example
H2 + O 2 → 2H O
2

R P
2 H 2 4
2 O 1 2

Need twice as much H in the reactant

Example
2H +O → 2H O
2 2 2

R P
2 H 2 4
2 O 1 2

Recount

Example
2H +O → 2H O
2 2 2

R P
4 2 H 2 4
2 O 1 2

The equation is balanced, has the same
number of each kind of atom on both sides

Example
2H +O → 2H O
2 2 2

R P
4 2 H 2 4
2 O 1 2
This is the answer
Not this

Balancing Chemical Equations (cont.)

Practice

• CH4 + O2 → CO2 + H2O
• AgNO3 + Cu → Cu(NO3)2 + Ag

• Mg + N2 → Mg3N2

• P + O2 → P4O10
• Na + H2O → H2 + NaOH

Section 9.1 Assessment

Which of the following is NOT a chemical
reaction?
A. a piece of wood burning
B. a car rusting
C. an ice cube melting into water A. A
D. red litmus paper turning blue B. B
C. C
0% 0% 0% 0%

D. D
A

B

D
C


What is the coefficient of bromine in the
equation 2Al(s) + 3Br2(l) → 2AlBr3(s)?

A. 1
B. 2
C. 3 A. A
D. 6 B. B
C. C
0% 0% 0% 0%

D. D
A

B

D
C

Types of Chemical Reactions

• Chemists classify reactions in order to
organize the many types
• We will learn 5 types.
• Will be able to predict the products.
• For some we will be able to predict
whether they will happen at all.
• Will recognize them by the reactants

Types of Chemical Reactions (cont.)
• A synthesis reaction is a reaction in which
two or more substances combine to produce
a single product.
• When two elements react, the reaction is
always a synthesis reaction.


• Predicting products of a synthesis
reaction:
• Element + Element  compound
• Fe + O2  Fe2O3 (you would be told iron (III))
– Rules of forming compounds must be
followed
• Predict the products
– Calcium reacts with chlorine
– Aluminum reacts with oxygen

• In a combustion reaction, oxygen
combines with a substance and releases
energy in the form of heat and light.
• Heated hydrogen reacts with oxygen to
produce heat and water in a combustion
reaction. This is also a synthesis reaction.

Two specific types of combustion
•If compound composed of only C, H and
maybe O is reacted with oxygen, there are
two possible outcomes
•Complete combustion will produce CO 2 and
H2O.
•Incomplete combustion will produce CO
and H2O.

Predict Products of combustion reactions:
•C4H10 + O2 → (complete)
•C4H10 + O2 → (incomplete)
•C6H12O6 + O2 → (complete)
•C8H8 + O2 → (incomplete)
•Mg + O2 

Decomposition Reactions
• A decomposition reaction is one in which
a single compound breaks down into two or
more elements or new compounds.
• Decomposition reactions often require an
energy source, such as heat, light, or
electricity, to occur.
• Compound  Element or compound +
Element or compound

• Predicting Products of Decomposition
• Easily predict the products if it is a binary
compound
• Made up of only two elements
• Compound will fall apart into its elements
• H2O   → 
electricity
electricity
  →
• HgO
→ heat

Replacement Reactions
• A reaction in which the atoms of one
element replace the atoms of another
element in a compound is called a single
replacement reaction.
A + BX → AX + B

• We can tell whether a reaction will
happen
• Some elements are more reactive than
others
• Use Activity Series List
• More reactive replaces less reactive
– Higher on the list replaces lower.
– If the element by itself is higher, reaction
occurs, if lower it doesn’t

• Fe + CuSO4 →
• Pb + KCl →
• Al + HCl →

• What does it mean that Ag, Pt and Au are
on the bottom of the Activity Series List?

Replacement Reactions (cont.)
• Halogens frequently replace other
halogens in replacement reactions.
• Halogens also have different reactivities and
do not always replace each other.

• The order of activity is on the periodic
table.
• Higher replaces lower.
• F2 + HCl →
• Br2 + KCl →

• Double replacement reactions occur
when ions exchange between two
compounds.
• This figure shows a generic double
replacement equation.

• A solid product produced during a chemical
reaction in a solution is called a
precipitate.
• All double replacement reactions produce
either water, a precipitate, or a gas.

Complete and Balance
•assume all of the reactions take place.
•CaCl2 + NaOH →
•CuCl2 + K2S →
•KOH + Fe(NO3)3 →
•(NH4)2SO4 + BaF2 →

• This table summarizes different ways to
predict the products of a chemical reaction.

Examples

• H2 + O2 →
• H2O →
• Zn + H2SO4 →
• HgO →
• KBr +Cl2 →
• AgNO3 + NaCl →
• Mg(OH)2 + H2SO3 →


Which of the following is NOT one of the
four types of reactions?
A. deconstructive
B. synthesis
C. single replacement A. A
D. double replacement B. B
C. C
0% 0% 0% 0%

D. D
A

B

D
C


The following equation is what type of
reaction?
KCN(aq) + HBr(aq) → KBr(aq) + HCN(g)
A. deconstructive
B. synthesis A. A
C. single replacement B. B
D. double replacement C. C
0% 0% 0% 0%

D. D
A

B

D
C

Aqueous Solutions
• An aqueous solution contains one or
more dissolved substances (called
solutes) in water.
• The solvent is the most plentiful substance in
a solution.

Aqueous Solutions (cont.)
• Water is always the solvent in an aqueous
solution.
• There are many possible solutes—sugar and
alcohol are molecular compounds that exist
as molecules in aqueous solutions.
• Compounds that produce hydrogen ions in
aqueous solutions are acids.

Aqueous Solutions (cont.)
• Ionic compounds can also be solutes in
aqueous solutions.
• When ionic compounds dissolve in water,
their ions separate in a process called
dissociation.

Types of Reactions in Aqueous Solutions
• When two solutions that contain ions as
solutes are combined, the ions might react.
• If they react, it is always a double
replacement reaction.
• Three products can form: precipitates, water,
or gases.

Types of Reactions in Aqueous Solutions (cont.)
• Aqueous solutions of sodium hydroxide and
copper(II) chloride react to form the
precipitate copper(II) hydroxide.
2NaOH(aq) + CuCl2(aq) → 2NaCl(aq) + Cu(OH)2(s)

• Ionic equations that show all of the particles
in a solution as they actually exist are called
complete ionic equations.
2Na+(aq) + 2OH–(aq) + Cu2+ (aq)+ 2Cl–(aq) → 2Na+
(aq) + 2Cl–(aq) + Cu(OH)2(s)

• Ions that do not participate in a reaction are
called spectator ions and are not usually
written in ionic equations.
• Formulas that include only the particles that
participate in reactions are called net ionic
equations.
2OH–(aq) + Cu2+(aq) → Cu(OH)2(s)

• Some reactions produce more water
molecules.
• No evidence of a chemical reaction is
observable.
HBr(aq) + NaOH(aq) → H2O(l) + NaBr(aq)
• Without spectator ions
H+(aq) + OH–(aq) → H2O(l).

• Gases that are commonly produced are
carbon dioxide, hydrogen cyanide, and
hydrogen sulfide.
2HI(aq) + Li2S(aq) → H2S(g) + 2LiI(aq)


What is the solvent in an aqueous
solution?
A. hydrogen
B. sodium ions
C. water A. A
D. alcohol B. B
C. C
0% 0% 0% 0%

D. D
A

B

D
C


An equation that includes only the
particles that participate in a reaction is
called:
A. net ionic equation
B. spectator ions
A. A
C. complete ionic equation B. B
D. reduced ionic equation C. C
0% 0% 0% 0%

D. D
A

B

D
C

Section 9.1 Reactions and Equations
Key Concepts
• Some physical changes are evidence that indicate a
chemical reaction has occurred.
• Word equations and skeleton equations provide
important information about a chemical reaction.

• A chemical equation gives the identities and relative
amounts of the reactants and products that are
involved in a chemical reaction.

• Balancing an equation involves adjusting the
coefficients until the number of atoms of each element
is equal on both sides of the equation.

Section 9.2 Classifying Chemical
Reactions
Key Concepts
• Classifying chemical reactions makes them easier to
understand, remember, and recognize.

• Activity series of metals and halogens can be used to
predict if single-replacement reactions will occur.

Section 9.3 Reactions in
Aqueous Solutions
Key Concepts
• In aqueous solutions, the solvent is always water.
There are many possible solutes.
• Many molecular compounds form ions when they
dissolve in water. When some ionic compounds
dissolve in water, their ions separate.

• When two aqueous solutions that contain ions as
solutes are combined, the ions might react with one
another. The solvent molecules do not usually react.

• Reactions that occur in aqueous solutions are double-
replacement reactions.

The law of conservation of mass requires what in
a chemical reaction equation?
A. both sides of the equation to contain
the same substances
B. the reactants to have the same
amount of molecules as the products
A. A
C. both sides to have the same amount
of atoms of each element B. B
D. the products to have fewer molecules C. C
than the reactants 0% 0% 0% 0%
D. D
A

B

C

D

A reaction that gives off heat is what type
of reaction?
A. single replacement reaction
B. double replacement reaction
C. synthesis reaction A. A
D. combustion reaction B. B
C. C
0% 0% 0% 0%

D. D
A

B

D
C

Ions that are present in a solution and do
not participate in a chemical reaction
when another substance is added are
called ____.
A. spectator ions
B. reactants A. A
B. B
C. products
C. C
D. net ions 0% 0% 0% 0%

D. D
A

B

D
C

A double replacement reaction produces
all of the following except ____.
A. gases
B. solids
C. light A. A
D. water B. B
C. C
0% 0% 0% 0%

D. D
A

B

D
C

What type of reaction is the following?
2H2O(l) + energy → H2(g) + O2(g)

A. synthesis reaction
B. decomposition reaction
A. A
C. combustion reaction
B. B
D. replacement reaction C. C
0% 0% 0% 0%

D. D
A

B

D
C

What type of reaction is the following?
2H2(g) + O2(g) → 2H2O(l)

A. replacement reaction
B. synthesis
A. A
C. combustion reaction
B. B
D. double replacement reaction C. C
0% 0% 0% 0%

D. D
A

B

D
C

A precipitate forms in a double
replacement reaction only if:
A. the reactivities of the compounds
differ
B. the new compound is denser
than water A. A
B. B
C. the new compound is soluble
in water C. C
0% 0% 0% 0%

D. the new compound is not D. D
A

B

D
C
soluble in water

A ____ is a statement that uses chemical
formulas to show the identities and
relative amounts of the substances
involved in a chemical reaction.
A. word equation
B. skeleton equation A. A
B. B
C. chemical equation
C. C
D. balanced equation 0% 0% 0% 0%

D. D
A

B

D
C

Predict the type of reaction.
LiBr2 (aq) + 2NaOH (aq) → ____

A. synthesis reaction
B. combustion reaction
A. A
C. single replacement reaction
B. B
D. double replacement reaction C. C
0% 0% 0% 0%

D. D
A

B

D
C

Which reactions are essentially the
opposite of synthesis reactions?
A. single-replacement
B. decomposition
C. combustion A. A
D. double-replacement B. B
C. C
0% 0% 0% 0%

D. D
A

B

D
C

Chapter 9 honors

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