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—
Classifying
Reactions:
Chemicals
in
Balance
Picture
a
starry
night
and
tired
hikers
sitting
around
a
campfire.
Everywhere
in
this
peaceful
setting,
chemical
reactions
are
taking
place.
The
cellulose
in
the
firewood
reacts
with
the
oxygen
in
the
air,
producing
carbon
dioxide
and
water.
The
light
and
heat
of
the
campfire
are
evidence
of
the
chemical
reaction.
If
someone
roasts
a
marshmallow
its
sugars
react
with
oxygen.
The
soft,
white
marshmallow
forms
a
brown
and
brittle
crust.
When
someone
eats
a
marshmallow,
the
chemicals
in
the
stomach
react
with
the
sugar
molecules
to
digest
them.
A
person
telling
a
story
exhales
carbon
dioxide
with
every
breath.
Carbon
dioxide
is
the
product
of
respiration,
another
chemical
reaction.
In
each
star
in
the
night
sky
above,
another
type
of
reaction
is
taking
place.
This
type
of
reaction
is
called
a
nuclear
reaction,
because
it
involves
changes
within
the
nucleus
of
the
atom.
Nuclear
reactions
are
responsible
for
the
enormous
amounts
of
heat
and
light
generated
by
all
the
stars,
including
our
Sun.
Back
on
Earth,
however,
chemical
reactions
are
everywhere
in
our
daily
lives.
We
rely
on
chemical
reactions
for
everything
from
powering
a
car
to
making
toast.
In
this
chapter,
you
will
learn
how
to
write
balanced
chemical
equations
for
these
reactions.
You
will
look
for
patterns
and
similarities
between
the
chemical
equations,
and
you
will
classify
the
reactions
they
represent.
As
well,
you
will
learn
how
to
balance
and
classify
equations
for
nuclear
reactions.
.
o
o
-
i
;:‘
:
)
Y
.
&
]
N
o
e
)
cellulose
v
hapt
T
XVZ]En
to-?t')fic
arbon
dioxide
anw
er.
How
cz
|Eche
cal
re
tl,
Yt'lat
cau
esa
!
hu
ko
-harcoal?
Wi
B
’
N
‘e
.
-
=
ce
of-
flrgwp
happeni
-
|
Chapter
Preview
4.1
Chemical
Equations
4.2
Synthesis
and
Decomposition
Reactions
4.3
Single
Displacement
and
Double
Displacement
Reactions
l
4.4
Simple
Nuclear
Reactions
Concepts
and
Skills
You
Will
Need
Before
you
begin
this
chapter,
review
the
following
concepts
and
skills:
m
defining
and
describing
the
relationships
among
atomic
number,
mass
number,
atomic
mass,
isotope,
and
radioisotope
(Chapter
2,
section
2.1)
[
m
naming
chemical
I
compounds
(Chapter
3,
section
3.4)
m
writing
chemical
formulas
(Chapter
3,
section
3.4)
m
explaining
how
different
elements
combine
to
form
covalent
and
ionic
bonds
using
the
octet
rule
(Chapter
3,
sections
3.2
and
3.3)
e
N
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
111
I
|
Section
Preview/
Specific
Expectations
In
this
section,
you
will
m
use
word
equations
and
skeleton
equations
to
describe
chemical
reactions
m
balance
chemical
equations
m
communicate
your
under-
standing
of
the
following
terms:
chemical
reactions,
reactant,
product,
chemical
equations,
word
equation,
skeleton
equation,
law
of
conservation
of
mass,
balanced
chemical
equation
CHECKP
INT
Write
the
chemical
formulas
of
the
products
in
the
reactions
described
in
Practice
Problem
1.
\.J
CHEM
FACT
Caffeine
is
an
ingredient
in
coffee,
tea,
chocolate,
and
cola
drinks.
lts
chemical
name
is
1,3,7-trimethylxanthene.
You
can
see
how
long
names
like
this
would
become
unwieldy
in
word
equations.
Chemical
Equations
In
Chapter
3,
you learned
how
and
why
elements
combine
to
form
different
compounds.
In
this
section,
you
will
learn
how
to
describe
what
happens
when
elements
and
compounds
interact
with
one
another
to
form
new
substances.
These
interactions
are
called
chemical
reactions.
A
substance
that
undergoes
a
chemical
reaction
is
called
a
reactant.
A
substance
that
is
formed
in
a
chemical
reaction
is
called
a
product.
For
example,
when
the
glucose
in
a
marshmallow
reacts
with
oxygen
in
the
air
to
form
water
and
carbon
dioxide,
the
glucose
and
oxygen
are
the
reactants.
The
carbon
dioxide
and
water
are
the
products.
Chemists
use
chemical
equations
to
communicate
what
is
occurring
in
a
chemical
reaction.
Chemical
equations
come
in
several
forms.
All
of
these
forms
condense
a
great
deal
of
chemical
information
into
a
short
statement.
Word
Equations
A
word
equation
identifies
the
reactants
and
products
of
a
chemical
reaction
by
name.
In
Chapter
3,
you
learned
that
chlorine
and
sodium
combine
to
form
the
ionic
compound
sodium
chloride.
This
reaction
can
be
represented
by
the
following
word
equation:
sodium
+
chlorine
—
sodium
chloride
In
this
equation,
“+”
means
“reacts
with”
and
“—”
means
“to
form.”
Try
writing
some
word
equations
in
the
following
Practice
Problems.
Practice
Problems
1.
Describe
each
reaction
using
a
word
equation.
Label
the
reactant(s)
and
product(s).
~
(a)
Calcium
and
fluorine
react
to
form
calcium
fluoride.
(b)
Barium
chloride
and
hydrogen
sulfate
react
to
form
hydrogen
chloride
and
barium
sulfate.
(e)
Calcium
carbonate,
carbon
dioxide,
and
water
react
to
form
calcium
hydrogen
carbonate.
(d)
Hydrogen
peroxide
reacts
to
form
water
and
oxygen.
(e)
Sulfur
dioxide
and
oxygen
react
to
form
sulfur
trioxide.
2.
Yeast
can
facilitate
a
reaction
in
which
the
sugar
in
grapes
reacts
to
form
ethanol
and
carbon
dioxide.
Write
a
word
equation
to
describe
this
reaction.
J
Word
equations
are
useful
because
they
identify
the
products
and
reactants
in
a
chemical
reaction.
They
do
not,
however,
provide
any
chemical
information
about
the
compounds
and
elements
themselves.
If
you
did
not
know
the
formula
for
sodium
chloride,
for
example,
this
equation
would
not
help
you
understand
the
reaction
very
well.
Another
shortcoming
of
a
word
equation
is
that
the
names
for
chemicals
are
often
very
long
and
cumbersome.
Chemists
have
therefore
devised
a
more
convenient
way
of
representing
reactants
and
products.
112
MHR
-
Unit
1
Matter
and
Chemical
Bonding
Skeleton
Equations
Table
4.1
Symbols
Using
a
chemical
formula
instead
of
a
chemical
name
simplifies
a
Used
in
Chemical
Equations
chemical
equation.
It
allows
you
to
see
at
a
glance
what
elements
and
Symbol
|
Meaning
compounds
are
involved
in
the
reaction.
A
skeleton
equation
lists
the
+
reacts
with
chemical
formula
of
each
reactant
on
the
left,
separated
by
a
+
sign
(reactant
side)
if
more
than
one
reactant
is
involved,
followed
by
an
arrow
—.
The
+
and
(product
side)
chemical
formula
of
each
product
is
listed
on
the
right,
again
separated
=
|
to
form
by
a
+
sign
if
more
than
one
product
is
produced.
A
skeleton
equation
,
—
.
.
.
(s)
solid
or
precipitate
also
shows
the
state
of
each
reactant
by
using
the
appropriate
subscript,
as
shown
in
Table
4.1.
(€)
|
liquid
The
reaction
of
sodium
metal
with
chlorine
gas
to
form
sodium
(8)
|egas
chloride
can
be
represented
by
the
following
skeleton
equation:
(ag)
|
in
aqueous
(water)
Nag)
+
Clz(g)
—
NaCly)
solution
A
skeleton
equation
is
more
useful
to
a
chemist
than
a
word
equation,
because
it
shows
the
formulas
of
the
compounds
involved.
It
also
shows
the
state
of
each
substance.Try
writing
some
skeleton
equations
in
the
following
Practice
Problems.
Practice
Problems
3.
Write
a
skeleton
equation
for
each
reaction.
(a)
Solid
zinc
reacts
with
chlorine
gas
to
form
solid
zinc
chloride.
(b)
Solid
calcium
and
liquid
water
react
to
form
solid
calcium
hydroxide
and
hydrogen
gas.
(¢)
Solid
barium
reacts
with
solid
sulfur
to
produce
solid
barium
sulfide.
(d)
Aqueous
lead(II)
nitrate
and
solid
magnesium
react
to
form
aqueous
magnesium
nitrate
and
solid
lead.
4.
In
each
reaction
below,
a
solid
reacts
with
a
gas
to
form
a
solid.
Write
a
skeleton
equation
for
each
reaction.
(a)
carbon
dioxide
+
calcium
oxide
—
calcium
carbonate
(b)
aluminum
+
oxygen
—
aluminum
oxide
(c)
magnesium
+
oxygen
—
magnesium
oxide
Why
Skeleton
Equations
Are
Incomplete
Although
skeleton
equations
are
useful,
they
do
not
fully
describe
chemi-
cal
reactions.
To
understand
why,
consider
the
skeleton
equation
showing
the
formation
of
sodium
chloride
(above).
According
to
this
equation,
one
sodium
atom
reacts
with
one
chlorine
molecule
containing
two
chlorine
\J
CHEM
atoms.
The
product
is
one
formula
unit
of
sodium
chloride,
containing
one
atom
of
sodium
and
one
atom
of
chlorine.
Where
has
the
extra
chlorine
atom
gone?
Many
chemical
reactions
can
go
in
either
direction,
so
an
.
arrow
pointing
in
the
opposite
The
Law
of
Conservation
of
Mass
direction
is
often
added
to
the
All
atoms
must
be
accounted
for,
according
to
an
important
law.
The
law
e_guatlo_\n.Thl_s
can
look
like
of
conservation
of
mass
states
that
in
any
chemical
reaction,
the
mass
<
ors.
To
|nd|c§te
which
of
the
products
is
always
equal
to
the
mass
of
the
reactants.
In
other
reaction
is
more
likely
to
:
;
_
occur,
one
arrow
can
be
words,
according
to
this
law,
matter
can
be
neither created
nor
destroyed.
drawn
longer
than
the
other:
Chemical
reactions
proceed
according
to
the
law
of
conservation
of
mass,
for
example:
=~
or
2—,
which
is
based
on
experimental
evidence.
\
/
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
113
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-1
in
Chemistry
Food
Chemist
alginate
forms,
which
causes
the
stream
of
pimento
mixture
to
form
a
gel
instantly.
The
R
7
A
gelled
strip
is
then
sliced
thinly
and
stuffed
into
1
r
g
the
olives.
.
B
Food
chemists
work
in
universities,
govern-
f\
ment
laboratories,
and
major
food
companies.
To
u
,
become
a
food
chemist,
most
undergraduates
'
>
|
take
a
food
science
degree
with
courses
in
chem-
.
‘
istry.
It
is
also
possible
to
become
a
food
chemist
with
an
undergraduate
chemistry
degree
plus
N
-
I
J
experience
in
the
food
industry.
Students
can
How
do
you
make
a
better
tasting
sports
drink?
specialize
in
food
chemistry
at
the
graduate
level.
How
can
you
make
a
gravy
mix
that
can
be
ready
to
serve
in
5
min,
yet
maintain
its
consistency
Make
Career
Connections
under
a
heat
lamp
for
8
h?
Food
chemists
use
their
knowledge
of
chemical
reactions
to
improve
food
quality
and
develop
new
products.
A
good
example
of
food
chemistry
in
action
is
the
red
pimento
stuffing
in
olives.
Chopped
pimentos
(sweet
red
peppers)
and
sodium
algi-
nate
are
mixed.
This
mixture
is
then
added
to
a
solution
of
calcium
chloride.
The
sodium
alginate
reacts
with
the
calcium
chloride.
Solid
calcium
w
Balanced
Chemical
Equations
h
A
balanced
chemical
equation
reflects
the
law
of
conservation
of
mass.
Jan
Baptista
van
Helmqnt
This
type
of
equation
shows
that
there
is
the
same
number
of
each
kind
(1577-1644)
was
a
Flemish
of
atom
on
both
sides
of
the
equation.
Some
skeleton
equations
are,
by
physician
who
left
medical
.
,
.
coincidence,
already
balanced.
For
example,
examine
the
reaction
of
ractice
to
devote
himself
’?o
the
study
of
chemistry.
He
carbon
with
oxygen
to
form
carbon
dioxide,
shown
in
Figure
4.1.
In
the
1.
If
you
are
interested
in
becoming
a
food
chemist,
you
can
look
for
a
summer
or
part-
time
job
in
the
food
industry.
2.
To
find
out
more
about
food
science,
search
for
Agriculture
and
Agri-Food
Canada's
web
site
and
the
Food
Web
web
site.
You
can
also
contact
the
Food
Science
department
of
a
university.
used
the
mass
balance
in
an
skeleton
equation,
one
carbon
atom
and
two
oxygen
atoms
are
on
the
left
important
experiment
that
laid
side
of
the
equation,
and
one
carbon
atom
and
two
oxygen
atoms
are
on
the
foundations
for
the
law
the
right
side
of
the
equation.
of
conservation
of
mass.
He
showed
that
a
definite
quantity
of
sand
could
be
fused
with
excess
alkali
to
form
a
kind
of
glass.
He
also
showed
:
that
when
this
product
was
Q
+
¥
treated
with
acid,
it
regenerat-
'
ed
the
original
amount
of
sand
(silica).
As
well,
Van
Helmont
is
famous
for
demonstrating
the
existence
of
gases,
which
he
described
as
“aerial
fluids.”
C
+
O,
—
co,
Investigate
on
the
Internet
or
in
the
library
to
find
out
how
he
did
this.
EEMZXXD
This
skeleton
equation
is
already
balanced.
114
MHR
-
Unit
1
Matter
and
Chemical
Bonding
Most
skeleton
equations,
however,
are
not
balanced,
such
as
the
one
showing
the
formation
of
sodium
chloride.
Examine
Figure
4.2
to
see
why.
There
is
one
sodium
atom
on
each
side
of
the
equation,
but
there
are
two
chlorine
atoms
on
the
left
side
and
only one
chlorine
atom
on
the
right
side.
To
begin
to
balance
an
equation,
you
can
add
numbers
in
front
of
the
appropriate
formulas.
The
numbers
that
are
placed
in
front
of
chemical
formulas
are
called coefficients.
They
represent
how
many
of
each
atom,
molecule,
or
formula
unit
take
part
in
each
reaction.
For
example,
if
you
add
a
coefficient
of
2
to
NaCl
in
the
equation
in
Figure
4.2,
you
indicate
that
two
formula
units
of
NaCl
are
produced
in
the
reaction.
Is
the
equa-
tion
balanced
now?
As
you
can
see
by
examining
Figure
4.3,
it
is
not.
The
chlorine
atoms
are
balanced,
but
now
there
is
one
sodium
atom
on
the
left
side
of
the
equation
and
two
sodium
atoms
on
the
right
side.
-l
B-din
A
lYy
=
Na
+
C
NaCl
Na
+
Cl,
2NaCl
[EETIEXE]
This
skeleton
equation
is
unbalanced.
The
mass
[GFTIZXE]
The
equation
is
still
unbalanced.
The
mass
of
of
the
reactants
is
greater
than
the
mass
of
the
product.
the
product
is
now
greater
than
the
mass
of
the
reactants.
Add
a
coefficient
of
2
to
the
sodium
on
the
reactant
side.
As
you
can
see
in
Figure
4.4,
the
equation
is
now
balanced.
The
mass
of
the
products
is
equal
to
the
mass
of
the
reactants.
This
balanced chemical
equation
satisfies
the
law
of
conservation
of
mass.
mind
STRETCH
Why
is
it
not
acceptable
to
w
.
I.’.
I
balance
the
equation
Na
+
Cl,
—
NaCl
by
changing
the
formula
of
é_b
NaCl
to
NaCl,?
Would
this
not
=
satisfy
the
law
of
conservation
2Na
+
Cl»
==
2NaCl
of
mass?
Write
an
explanation
in
your
notebook.
The
equation
is
now
balanced
according
to
the
law
of
conservation
of
mass.
-
J
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
115
%
Electronic
Learning
Partner
Go
to
the
Chemistry
11
Electronic
Learning
Partner
for
some
extra
practice
balancing
chemical
equations.
You
cannot
balance
an
equation
by
changing
any
of
the
chemical
formulas.
The
only
way
to
balance
a
chemical
equation
is
to
put
the
appropriate
numerical
coefficient
in
front
of
each
compound
or
element
in
the
equation.
Many
skeleton
equations
are
simple
enough
to
balance
by
a
back-and-
forth
process
of
reasoning,
as
you
just
saw
with
the
sodium
chloride
reaction.
Try
balancing
the
equations
in
the
Practice
Problems
that
follow.
Practice
Problems
5.
Copy
each
skeleton
equation
into
your
notebook,
and
balance
it.
)
(a)
S(s)
+
Oz
—
SOz
(e)
Hy(g)
+
Clyg)
—
HClg
(b)
Pags)
+
Og(g)
=
PsO1g()
(d)
SOz
+
H20(¢)
—
H2SO03(q)
6.
Indicate
whether
these
equations
are
balanced.
If
they
are
not,
balance
them.
(a)
4Fe(s)
+
302
—
2Fe203(5
(b)
HgOs)
—
Hge)
+
Ogg)
(6)
HyOzaq)
=
2H,0()
+
Oz
(d)
2HCl(aq)
+
NazSO3(aq)
=
2NaCl(ag)
+
HyO(g)
+
SOy
\_
J
Steps
for
Balancing
Chemical
Equations
More
complex
chemical
equations
than
the
ones
you
have
already
tried
can
be
balanced
by
using
a
combination
of
inspection
and
trial
and
error.
Here,
however,
are
some
steps
to
follow.
Step1
Write
out
the
skeleton
equation.
Ensure
that
you
have
copied
all
the
chemical
formulas
correctly.
Step2
Begin
by
balancing
the
atoms
that
occur
in
the
largest
number
on
either
side
of
the
equation.
Leave
hydrogen,
oxygen,
and
other
elements
until
later.
Step3
Balance
any
polyatomic
ions,
such
as
sulfate,
SO,%",
that
occur
on
both
sides
of
the
chemical
equation
as
an
ion
unit.
That
is,
do
not
split
a
sulfate
ion
into
1
sulfur
atom
and
4
oxygen
atoms.
Balance
this
ion
as
one
unit.
Step
4
Next,
balance
any
hydrogen
or
oxygen
atoms
that
occur
in
a
combined
and
uncombined
state.
For
example,
combined
oxygen
might
be
in
the
form
of
CO,,
while
uncombined
oxygen
occurs
as
O;.
Step5
Finally,
balance
any
other
element
that
occurs
in
its
uncombined
state:
for
example,
Na
or
Cl,.
Step6
Check
your
answer.
Count
the
number
of
each
type
of
atom
on
each
side
of
the
equation.
Make
sure
that
the
coefficients
used
are
whole
numbers
in
their
lowest
terms.
Examine
the
following
Sample
Problem
to
see
how
these
steps
work.
116
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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’Sample
Problem
Balancing
Chemical
Equations
Problem
Balance
the
equation.
What
Is
Required?
Plan
Your
Strategy
Act
on
Your
Strategy
Check
Your
Solution
Left
Side
Cu
1
NOs~
2
K
2
OH~
2
Practice
Problems
Copper(II)
nitrate
reacts
with
potassium
hydroxide
to
form
potassium
nitrate
and
solid
copper(lI)
hydroxide.
CU(NO3)2(aq)
+
KOH(aq)
—
Cu(OH)z(S)
+
KNOg(aq]
The
atoms
of
each
element
on
the
left
side
of
the
equation
should
equal
the
atoms
of
each
element
on
the
right
side
of
the
equation.
Balance
the
polyatomic
ions
first
(NO5~,
then
OH~).
Check
to
see
whether
the
equation
is
balanced.
If
not,
balance
the
potassium
and
copper
ions.
Check
your
equation
again.
There
are
two
NO;™
ions
on
the
left,
so
put
a
2
in
front
of
KNO3.
Cu(NO3)2(aq)
+
KOH(aq)
—
Cu(OH)Z(S)
+
ZKNO;;(aq]
To
balance
the
two
OH™
ions
on
the
right,
put
a
2
in
front
of
the
KOH.
CU(N03)2(aq)
+
ZKOH(aq)
—
Cu(OH)z(S)
+
ZKN03(aq)
Check
to
see
that
the
copper
and
potassium
ions
are
balanced.
They
are,
so
the
equation
above
is
balanced.
Tally
the
number
of
each
type
of
atom
on
each
side
of
the
equation.
CU[NO3)2(aq)
+
ZKOH(aq)
—
Cu(OH)z(s)
+
ZKN03(aq)
Right
Side
1
2
2
2
(@)
SOz(g)
+
Oz(g)
=
SOs()
sent
these
reactions.
\—
7.
Copy
each
chemical
equation
into
your
notebook,
and
balance
it.
(h)
BaClz(aq)
+
NaySOy(aq)
—
NaCl(aq)
+
BaSOy()
8.
When
solid
white
phosphorus,
P,,
is
burned
in
air,
it
reacts
with
oxygen
to
produce
solid
tetraphosphorus
decoxide,
P,0;0.
When
water
is
added
to
the
P,O,y,
it
reacts
to
form
aqueous
phosphoric
acid,
H3PO,4.
Write and
balance
the
chemical
equations
that
repre-
Math
o
LiNK
9
What
does
it
mean
when
a
fraction
is
expressed
in
lowest
terms?
The
fraction
%,
expressed
in
lowest
terms,
is
%
Similarly,
the
equation
4Hyq)
+
205
—
4H0y
is
balanced,
but
it
can
be
simplified
by
dividing
all
the
coefficients
by
two.
2Hz(g)
+
Oz(g)
—>
2H20(g)
Write
the
balanced
equation
6KC|03(S)
—
6KC|(9)
+
902(5)
SO
that
the
coefficients
are the
lowest
possible
whole
num-
bers.
Check
that
the
equation
is
still
balanced.
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
117
Continued
...
2
—
FROM
PAGE
117
:
!
9.
Copy
each
chemical
equation
into
your
notebook,
and
balance
it.
(a)
AsySg(s)
+
Ozg)
=
AS40g(s)
+
SOy
(b)
Sc;03(5)
+
Hz0()
—
Sc(OH),)
{e)
C.H50Hg)
+
Og(g)
=
COsg)
+
H20(y)
(d)
CaHiggg)
+
Ozig)
=
COgq)
+
H2Og)
—
_J
Section
Wrap-up
In
this
section,
you
learned
how
to
represent
chemical
reactions
using
balanced chemical
equations.
Because
there
are
so
many
different
chemical
reactions,
chemists
have
devised
different
classifications
for
these
reactions.
In
section
4.2,
you
will
learn
about
five
different
types
of
chemical
reactions.
Section
Review
©
D
In
your
own
words,
explain
what
a
chemical
reaction
is.
Write
descriptions
of
four
chemical
reactions
that
you
encounter
every
day.
O
O
Write
a
word
equation,
skeleton
equation,
and
balanced
equation
for
each
reaction.
(a)
Sulfur
dioxide
gas
reacts
with
oxygen
gas
to
produce
gaseous
sulfur
trioxide.
(b)
Metallic
sodium
reacts
with
liquid
water
to
produce
hydrogen
gas
and
aqueous
sodium
hydroxide.
(c)
Copper
metal
reacts
with
an
aqueous
hydrogen
nitrate
solution
to
produce
aqueous
copper(Il)
nitrate,
nitrogen
dioxide
gas,
and
liquid
water.
©
The
equation
for
the
decomposition
of
hydrogen
peroxide,
H,O,
is
H2O2(aq)
=
H20()
+
Oz(g).
Explain
why
you
cannot
balance
it
by
writing
it
as
HyOz(aq)
=
H20(g)
+
O(g)
(4]
Balance
the
following
chemical
equations.
(a)
Alg)
+
Oz)
>
AlOj5
(b)
NElezO3(aq)
+
IZ[aq)
—
N&I[aq)
+
NazS406(aq)
(c)
Al(s)
+
FeyO3(5
—
A1203(S)
+
Fey)
(d)
NH3(g)
+
Oz
—
NOg)
+
H2O(y)
(e)
NaZO(s)
+
(NH4)ZSO4(aq)
—>
NaZSO4(aq)
+
HZO(g)
+
NHg(aq]
(f)
CsHaz(e)
+
Oz(g)
=
COyg)
+
HyO(g)
©
©
A
student
places
0.58
g
of
iron
and
1.600
g
of
copper(Il)
sulfate
in
a
reaction
vessel.
The
reaction
vessel
has
a
mass
of
40.32
g,
and
it
contains
100.00
g
of
water.
The
aqueous
copper
sulfate
and
solid
iron
react
to
form
solid
copper
and
aqueous
iron(II)
sulfate.
After
the
reaction,
the
reaction
vessel
plus
the
products
have
a
mass
of
142.5
g.
Explain
the
results.
Then
write
a
balanced
chemical
equation
to
describe
the
reaction.
118
MHR
-
Unit
1
Matter
and
Chemical
Bonding
Synthesis
and
Decomposition
Reactions
How
are
different
kinds
of
compounds
formed?
In
section
4.1,
you
Section
Preview/
learned
that
they
are
formed
by
chemical
reactions
that
you
can
describe
-
Specific
Expectations
using
balanced chemical
equations.
Just
as
there
are
different
types
of
In
this
section,
you
will
compounds,
there
are
different
types
of
chemical
reactions.
In
this
a
distinguish
between
section,
you
will
learn
about
five
major
classifications
for
chemical
synthesis,
decomposition,
reactions.
You
will
use
your
understanding
of
chemical
formulas
and
and
combustion
reactions
chemical
equations
to
predict
products
for
each
class
of
reaction.
=
write
balanced
chemical
equations
to
represent
Why
Classify?
synthesis,
decomposition,
e
s
.
.
ti
ti
People
use
classifications
all
the
time.
For
example,
many
types
of
wild
and
combustion
reactions
mushrooms
are
edible,
but
many
others
are
poisonous—even
deadly!
How
can
you
tell
which
is
which?
Poisonous
and
deadly
mushrooms
have
characteristics
that
distinguish
them
from
edible
ones,
such
as
odour,
=
demonstrate
an
under-
colour,
habitat,
and
shape
of
roots.
It
is
not
always
easy
to
distinguish
standing
of
the
relationship
one
type
of
mushroom
from
another;
the
only
visible
difference
may
be
2fizvr\ln?sgltrr]eea2?oen0;n
d
the
the
colour
of
the
mushroom’s
spores.
Therefore,
you
should
never
try
to
nature
of
the
reactants
eat
any
wild
mushrooms
without
an
expert’s
advice.
Examine
Figure
4.5.
Which
mushroom
looks
more
appetizing
to
you?
An
expert
will
always
be
able
to
distinguish
an
edible
mushroom
from
a
m
predict
the
products
of
chemical
reactions
m
communicate
your
under-
standing
of
the
following
terms:
synthesis
reaction,
poisonous
mushroom
based
on
the
characteristics
that
have
been
used
to
decomposition
reaction,
classify
each
type.
By
classifying,
they
can
predict
the
effects
of
eating
any
combustion
reaction,
wild
mushroom.
incomplete
combustion
W“!
>
43
d
,
3
-
°‘
"‘.:
f__‘
‘“
MY
The
mushroom
on
the
left,
called
a
chanterelle,
is
edible
and
very
tasty.
The
mushroom
on
the
right
is
called
a
death
cap.
It
is
extremely
poisonous.
——
-
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
119
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The
iron
in
this
car
undergoes
a
synthesis
reaction
with
the
oxygen
in
the
air.
Iron(lll)
oxide,
also
known
as
rust,
is
formed.
In
the
same
way,
you
can
recognize
similarities
between
chemical
reactions
and
the
types
of
reactants
that
tend
to
undergo
different
types
of
reactions.
With
this
knowledge,
you
can
predict
what
will
happen
when
one,
two,
or
more
substances
react.
In
this
section,
you
will
often
see
chemical
reactions
without
the
subscripts
showing
the
states
of
matter.
They
are
omitted
deliberately
because,
in
most
cases,
you
are
not
yet
in
a
position
to
predict
the
states
of
the
products.
Synthesis
Reactions
In
a
synthesis
reaction,
two
or
more
elements
or
compounds
combine
to
form
a
new
substance.
Synthesis
reactions
are
also
known
as
combination
or
formation
reactions.
A
general
equation
for
a
synthesis
reaction
is
A+B—>C
In
a
simple
synthesis
reaction, one
element
reacts
with
one
or
more
other
elements
to
form
a
compound.
Two,
three,
four,
or
more
elements
may
react
to
form
a
single
product,
although
synthesis
reactions
involving
four
or
more
reactants
are
extremely
rare.
Why
do
you
think
this
is
so?
When
two
elements
react
together,
the
reaction
is
almost
always
a
synthesis
reaction
because
the
product
is
almost
always
a
single
compound.
There
are
several
types
of
synthesis
reactions.
Recognizing
the
patterns
of
the
various
types
of
reactions
will
help
you
to
predict
whether
substances
will
take
part
in
a
synthesis
reaction.
When
a
metal
or
a
non-metal
element
reacts
with
oxygen,
the
product
is
an
oxide.
Figure
4.6
shows
a
familiar
example,
in
which
iron
reacts
with
oxygen
according
to
the
following
equation:
3Fe(s)
+
Oz
=
Fe
03
Two
other
examples
of
this
type
of
reaction
are:
2Hy(g)
+
Oag)
—
2H20(g)
ZMg(S)
+
Oz(g]
—
ZMgO(S]
A
second
type
of
synthesis
reaction
involves
the
reaction
of
a
metal
and
a
non-metal
to
form
a
binary
compound.
One
example
is
the
reaction
of
potassium
with
chlorine.
2K
+
Clz(g)
—
2KCl)
120
MHR
-
Unit
1
Matter
and
Chemical
Bonding
Synthesis
Reactions
Involving
Compounds
In
the
previous
two
types
of
synthesis
reactions,
two
elements
reacted
to
form
one
product.
There
are
many
synthesis
reactions
in
which
one
or
more
compounds
are
the
reactants.
For
the
purpose
of
this
course,
howev-
er,
we
will
deal
only
with
the
two
specific
types
of
synthesis
reactions
involving
compounds
that
you
should
recognize:
oxides and
water.
When
a
non-metallic
oxide
reacts
with
water,
the
product
is
an
acid.
You
will
learn
more
about
acids
and
the
rules
for
naming
them
in
Chapter
10.
The
acids
that
form
when
non-metallic
oxides
and
water
react
are
composed
of
hydrogen
cations
and
polyatomic
anions
containing
oxygen
and
a
non-metal.
For
example,
one
contributor
to
acid
rain
is
hydrogen
sulfate
(sulfuric
acid),
H,SO,4,
which
forms
when
sulfur
trioxide
reacts
with
water.
The
sulfur
trioxide
comes
from
sources
such
as
industrial
plants
that
emit
the
gas
as
a
byproduct
of
burning
fossil
fuels,
as
shown
in
Figure
4.7.
SO3(g)
+
HzO(g]
—
HzSO4(aq]
~
'L‘
-
Sulfur
trioxide,
emitted
by
this
factory,
reacts
with
the
water
in
the
air.
Sulfuric
acid
is
formed
in
a
synthesis
reaction.
Conversely,
when
a
metallic
oxide
reacts
with
water,
the
product
is
a
metal
hydroxide.
Metal
hydroxides
belong
to
a
group
of
compounds
called
bases.
You
will
learn
more
about
bases
in
Chapter
10.
For
example,
when
calcium
oxide
reacts
with
water,
it
forms
calcium
hydroxide,
Ca(OH),.
Calcium
oxide
is
also
called
lime.
It
can
be
added
to
lakes
to
counteract
the
effects
of
acid
precipitation.
CaO(S)
+
HZO(g)
—
Ca(OH)Z(aq)
Sometimes
it
is
difficult
to
predict
the
product
of
a
synthesis
reaction.
The
only
way
to
really
know
the
product
of
a
reaction
is
to
carry
out
the
reaction
and
then
isolate
and
identify
the
product.
For
example,
carbon
can
react
with
oxygen
to
form
either
carbon
monoxide
or
carbon
dioxide.
Therefore,
if
all
you
know
is
that
your
reactants
are
carbon
and
oxygen,
you
cannot
predict
with
certainty
which
compound
will
form.
You
can
only
give
options.
Cig)
+
Ozg)
=
CO2g)
2C)
+
Oz(g)
—
ZCO(g)
You
would
need
to
analyze
the
products
of
the
reaction
by
experiment
to
determine
which
compound
was formed.
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
"
History
&
LiNK
|
D
Today we
have
sophisticated
lab
equipment
to
help
us
ana-
lyze
the
products
of
reactions.
In
the
past,
when
such
equip-
ment
was
not
available,
chemists
sometimes
jeopard-
ized
their
safety
and
health
to
determine
the
products
of
the
reactions
they
studied.
Sir
Humphry
Davy
(1778-1829),
a
contributor
to
many
areas
of
chemistry,
thought
nothing
of
inhaling
the
gaseous
prod-
ucts
of
the
chemical
reactions
that
he
carried
out.
He
tried
to
breathe
pure
CO,,
then
known
as
fixed
air.
He
nearly
suffocated
himself
by
breath-
ing
hydrogen.
In
1800,
Davy
inhaled
dinitrogen
monoxide,
N,0,
otherwise
known
as
nitrous
oxide,
and
discovered
its
anaesthetic
properties.
What
is
nitrous
oxide
used
for
today?
CHECKP@INT
As
you
begin
learning
about
different
types
of
chemical
reactions,
keep
a
separate
list
of
each
type
of
reaction.
Add
to
the
list
as
you
encounter
new
reactions.
121
As
electricity
passes
through
the
water,
it
decomposes
to
hydrogen
and
oxygen
gas.
Try
predicting
the
products
of
synthesis
reactions
in
the
following
Practice
Problems.
Practice
Problems
10.
Copy
the
following
synthesis
reactions
into
your
notebook.
Predict
the
product
of
each
reaction.
Then
balance
each
chemical
equation.
(a)
K+
Br,
—
(¢)
Ca+Cl,
—»
(b)
Hy
+
Clz
—
(d)
Li+
Oz
—
~
11.
Copy
the
following
synthesis
reactions
into
your
notebook.
For
each
set
of
reactants,
write
the
equations
that
represent
the
possible
products.
(a)
Fe
+
Oz
—
(suggest
two
different
synthesis
reactions)
(b)
V+
0O,
—»
(suggest
four
different
synthesis
reactions)
(¢)
Co+Cl,
—
(suggest
two
different
synthesis
reactions)
(d)
Ti+O;
—
(suggest
three
different
synthesis
reactions)
12.
Copy
the
following
equations
into
your
notebook.
Write
the
product
of
each
reaction.
Then
balance
each
chemical
equation.
(a)
K,O
+
H,0 —
(¢)
SO,
+
H,0
—
(b)
MgO
+
H,0
—
13.
Ammonia
gas
and
hydrogen
chloride
gas
react
to
form
a
solid
compound.
Predict
what
the
solid
compound
is.
Then
write
a
balanced chemical
equation.
\.
J
Decomposition
Reactions
In
a
decomposition
reaction,
a
compound
breaks
down
into
elements
or
other
compounds.
Therefore,
a
decomposition
reaction
is
the
opposite
of
a
synthesis
reaction.
A
general
formula
for
a
decomposition
reaction
is:
C—A+B
The
substances
that
are
produced
in
a
decomposition
reaction
can
be
elements
or
compounds.
In
the
simplest
type
of
decomposition
reaction,
a
compound
breaks
down
into
its
component
elements.
One
example
is
the
decomposition
of
water
into
hydrogen
and
oxygen.
This
reaction
occurs
when
electricity
is
passed
through
water.
Figure
4.8
shows
an
apparatus
set
up
for
the
decomposition
of
water.
ZHzO
—
2H,
+
Oz
More
complex
decomposition
reactions
occur
when
compounds
break
down
into
other
compounds.
An
example
of
this
type
of
reaction
is
shown
in
Figure
4.9.
The
photograph
shows
the
explosive
decomposition
of
ammonium
nitrate.
122
NMHR
-
Unit
1
Matter
and
Chemical
Bonding
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When
ammonium
nitrate
is
heated
to
a
high
temperature,
it
forms
dinitrogen
monoxide
and
water
according
to
the
following
balanced
equation:
NH/NO;3)
—
NZO(g)
+
ZHZO(g)
Try
predicting
the
products
of
the
decomposition
reactions
in
the
following
Practice
Problems.
Practice
Problems
14.
Mercury(II)
oxide,
or
mercuric
oxide,
is
a
bright
red
powder.
It
decomposes
on
heating.
What
are
the
products
of
the
decomposition
of
HgO?
15.
What
are
the
products
of
the
following
decomposition
reactions?
Predict
the
products.
Then
write
a
balanced
equation
for
each
reaction.
(a)
HI
—
(e)
AICl;
—
(b)
Ag20O
—
(d)
MgO
—
16.
Calcium
carbonate
decomposes
into
calcium
oxide and
carbon
dioxide
when
it
is
heated.
Based
on
this
information,
predict
the
products
of
the
following
decomposition
reactions.
(a)
MgCO3
—
(b)
CuCO;
—
~
\-
J
Combustion
Reactions
Combustion
reactions
form
an
important
class
of
chemical
reactions.
The
combustion
of
fuel
—wood,
fossil
fuel,
peat,
or
dung—has,
throughout
history,
heated
and
lit
our
homes
and
cooked
our
food.
The
energy
produced
by
combustion
reactions
moves
our
airplanes,
trains,
trucks,
and
cars.
A
complete
combustion
reaction
is
the
reaction
of
a
compound
or
element
with
O,
to
form
the
most
common
oxides
of
the
elements
that
make
up
the
compound.
For
example,
a
carbon-containing
compound
undergoes
combustion
to
form
carbon
dioxide,
CO,.
A
sulfur-contain-
ing
compound
reacts
with
oxygen
to
form
sulfur
dioxide,
SO,.
Combustion
reactions
are
usually
accompanied
by
the
production
of
light
and
heat.
In
the
case
of
carbon-containing
compounds,
complete
combustion
results
in
the
formation
of,
among
other
things,
carbon
dioxide.
For
example,
methane,
CH,,
the
primary
constituent
of
natural
gas,
undergoes
complete
combustion
to
form
carbon
dioxide,
(the
most
common
oxide
of
carbon),
as
well
as
water.
This
combustion
reaction
is
represented
by
the
following
equation:
CH4(g)
+
202(8)
—
COZ(g)
+
ZHZO(g)
The
combustion
of
methane,
shown
in
Figure
4.10,
leads
to
the
formation
of
carbon
dioxide
and
water.
The
complete
combustion
of
any
compound
that
contains
carbon,
hydrogen,
and
oxygen
(such
as
ethanol,
C;H;OH)
produces
carbon
dioxide
and
water.
At
high
temperatures,
ammonium
nitrate
explodes,
decomposing
into
dinitrogen
monoxide
and
water.
This
photo
shows
the
combustion
of
methane
in
a
laboratory
burner.
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
123
CHECKP@INT
Copy
the
following
skeleton
equation
for
the
combustion
of
pentane,
CsHy3,
into
your
notebook
and
balance
it.
C5H12
+
02
—
COZ
+
H20
If
it
took you
a
long
time
to
balance
this
equation,
chances
are
that
you
did
not
use
the
quickest
method.
Try
balancing
carbon
first,
hydrogen
second,
and
finally
oxygen.
What
is
the
advantage
of
leaving
O,
until
the
end?
Would
this
method
work
for
incomplete
combus-
tion
reactions?
Would
this
method
work
if
the
“fuel”
contained
oxygen
in
addition
to
C
and
H?
Now
try
balancing
the
chemical
equation
for
the
combustion
of
heptane
(C7H1¢)
and
the
combustion
of
rubbing
alcohol,
isopropanol
(C3HgO).
-
Compounds
that
contain
elements
other
than
carbon
also
undergo
complete
combustion
to
form
stable
oxides.
For
instance,
sulfur-contain-
ing
compounds
undergo
combustion
to
form
sulfur
dioxide,
SO,
a
precursor
to
acid
rain.
Complete
combustion
reactions
are
often
also
synthesis
reactions.
Metals,
such
as
magnesium,
undergo
combustion
to
form
their
most
stable
oxide,
as
shown
in
Figure
4.11.
2Mg(s)
+
Ozg)
=
2MgOy)
MY
XE]
Magnesium
metal
burns
in
oxygen.
The
smoke
and
ash
that
are
produced
in
this
combustion
reaction
are
magnesium
oxide.
In
the
absence
of
sufficient
oxygen,
carbon-containing
compounds
under-
go
incomplete
combustion,
leading
to
the
formation
of
carbon
monoxide,
CO, and
water.
Carbon
monoxide
is
a
deadly
gas.
You
should
always
make
sure
that
sufficient
oxygen
is
present
in
your
indoor
environment
for
your
gas
furnace,
gas
stove,
or
fireplace.
Try
the
following
problems
to
practise
balancing
combustion
reactions.
Practice
Problems
17.
The
alcohol
lamps
that
are
used
in
some
science
labs
are
often
fuelled
with
methanol,
CH30H.
Write
the
balanced
chemical
equation
for
the
complete
combustion
of
methanol.
18.
Gasoline
is
a
mixture
of
compounds
containing
hydrogen
and
carbon,
such
as
octane,
CgH,5.
Write
the
balanced chemical
equation
for
the
complete
combustion
of
CgHs.
19.
Acetone,
C3HgO,
is
often
contained
in
nail
polish
remover.
Write
the
balanced chemical
equation
for
the
complete
combustion
of
acetone.
20.
Kerosene
consists
of
a
mixture
of
hydrocarbons.
It
has
many
uses
including
jet
fuel
and
rocket
fuel.
It
is
also
used
as
a
fuel
for
hurri-
cane
lamps.
If
we
represent
kerosene
as
C;6Hs4,
write
a
balanced
chemical
equation
for
the
complete
combustion
of
kerosene.
124
MHR
-
Unit
1
Matter
and
Chemical
Bonding
Section
Wrap-up
In
this
section,
you learned
about
three
major
types
of
reactions:
synthe-
sis,
decomposition,
and
combustion
reactions.
Using
your
knowledge
about
these
types
of
reactions,
you
learned
how
to
predict
the
products
of
various
reactants.
In
section
5.3,
you
will
increase
your
understanding
of
chemical
reactions
even
further,
learning
about
two
major
types
of
chemical
reactions.
As
well,
you
will
observe
various
chemical
reactions
in
three
investigations.
Section
Review
(1]
Write
the
product
for
each
synthesis
reaction.
Balance
the
chemical
equation.
(a)
Be
+
Oy
—
(b)
Li
+
Cl,
—
()
Mg
+
Ny
—
(d)
Al
+
Br,
—
(e)
K+
O;
—
(2]
Write
the
products
for
each
decomposition
reaction.
Balance
the
chemical
equation.
(a)
K20
—
(b)
CuO
—
(c)
H,O
—
(d)
Ni,O3
—
(e)
Ag,O
—
©
©
Write
a
balanced
chemical
equation
for
each
of
the
following
word
equations.
Classify
each
reaction.
(a)
With
heating,
solid
tin(IV)
hydroxide
produces
solid
tin(IV)
oxide
and
water
vapour.
(b)
Chlorine
gas
reacts
with
crystals
of
iodine
to
form
iodine
trichloride.
(4]
Write
a
balanced chemical
equation
for
the
combustion
of
butanol,
C4HgOH.
O
O
Ared
compound
was
heated,
and
the
two
products
were
collected.
The
gaseous
product
caused
a
glowing
splint
to
burn
brightly.
The
other
product
was
a
shiny
pure
metal,
which
was
a
liquid
at
room
temperature.
Write
the
most
likely
reaction
that
would
explain
these
results.
Classify
the
reaction.
Hint:
Remember
that
the
periodic
table
identifies
the
most
common
valences.
O
D
Explain
why
gaseous
nitrogen
oxides
emitted
by
automobiles
and
industries
contribute
to
acid
rain.
Write
balanced chemical
reactions
to
back
up
your
ideas.
You
may
need
to
look
up
chemical
formulas
for
your
products.
}
Unit
Project
Prep
Before
you
design
your
Chemistry
Newsletter
at
the
end
of
Unit
1,
consider
that
fuels
are
composed
of
com-
pounds
containing
hydrogen
and
carbon
(hydrocarbons).
What
kind
of
reaction
have
you
seen
in
this
section
that
involves
those
kinds
of
com-
pounds?
What
type
of
warning
would
you
expect
to
see
on
a
container
of
lawnmower
fuel?
How
is
the
warning
related
to
the
types
of
reaction
that
involve
hydrocarbons?
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
125
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Section
Preview/
Specific
Expectations
In
this
section,
you
will
126
distinguish
between
synthesis,
decomposition,
combustion,
single
displacement,
and
double
displacement
reactions
write
balanced
chemical
equations
to
represent
single
displacement
and
double
displacement
reactions
predict
the
products
of
chemical
reactions
and
test
your
predictions
through
experimentation
demonstrate
an
understand-
ing
of
the
relationship
between
the
type
of
chemical
reaction
and
the
nature
of
the
reactants
investigate,
through
experi-
mentation,
the
reactivity
of
different
metals
to
produce
an
activity
series
communicate
your
under-
standing
of
the
following
terms:
single
displacement
reaction,
activity
series,
double
displacement
reaction,
precipitate,
neutralization
reactions
Single
Displacement
and
Double
Displacement
Reactions
In
section
4.2,
you
learned
about
three
different
types
of
chemical
reactions.
In
section
4.3,
you
will
learn
about
two
more
types
of
reactions.
You
will
learn
how
performing
these
reactions
can
help
you
make
inferences
about
the
properties
of
the
elements
and
compounds
involved.
Single
Displacement
Reactions
In
a
single
displacement
reaction,
one
element
in
a
compound
is
displaced
(or
replaced)
by
another
element.
Two
general
reactions
represent
two
different
types
of
single
displacement
reactions.
One
type
involves
a
metal
replacing
a
metal
cation
in
a
compound,
as
follows:
A+BC
-
AC+8B
For
example,
Zn(s)
+
Fe(NO3)2(aq)
—>
ZH(N03)z(aq)
+
Fez(s)
The
second
type
of
single
displacement
reaction
involves
a
non-metal
(usually
a
halogen)
replacing
an
anion
in
a
compound,
as
follows:
DE+F
—
DF
+E
For
example,
Cly(g)
+
CaBra@g
—
CaClyg)
+
Bray
Single
Displacement
Reactions
and
the
Metal
Activity
Series
Most
single
displacement
reactions
involve
one
metal
displacing
another
metal
from
a
compound.
In
the
following
equation,
magnesium
metal
replaces
the
zinc
in
ZnCl,,
thereby
liberating
zinc
as
the
free
metal.
Mgs)
+
ZnClyaq)
=
MgClaag)
+
Zng)
The
following
three
reactions
illustrate
the
various
types
of
single
displacement
reactions
involving
metals:
1.
Cug)
+
2AgNO3(3aq)
—
Cu(NO3)2(aq)
+
2Ag(s)
In
this
reaction,
one
metal
replaces
another
metal
in
an
ionic
compound.
That
is,
copper
replaces
silver
in
AgNO;.
Because
of
the
+2
charge
on
the
copper
ion,
it
requires
two
nitrate
ions
to
balance
its
charge.
2.
Mg
+
2HC1(aq)
—
MgClz(aq)
+
Ha(g)
In
this
reaction,
magnesium
metal
replaces
hydrogen
from
hydrochloric
acid,
HClg).
Since
hydrogen
is
diatomic,
it
is
“liberated”
in
the
form
of
H,.
This
reaction
is
similar
to
reaction
1
if
e
you
treat
hydrochloric
acid
as
an
ionic
compound
(which
it
techni-
cally
is
not),
and
if
e
you
treat
hydrogen
as
a
metal
(also,
technically,
not
the
case).
3.
2Nag,)
+
2H,0()
—
2NaOH(yq)
+
Hy(g)
Sodium
metal
displaces
hydrogen
from
water
in
this
reaction.
Again,
since
hydrogen
is
diatomic,
it
is
produced
as
H,.
As
above,
you
can
understand
this
reaction
better
if
e
you
treat
hydrogen
as
a
metal,
and
if
e
you
treat
water
as
an
ionic
compound,
H*(OH").
MHR
«
Unit
1
Matter
and
Chemical
Bonding
All
of
the
reactions
just
described
follow
the
original
general
example
of
a
single
displacement
reaction:
=~
A+BC—>
AC+B
e
Figures
4.12
and
4.13
show
two
examples
of
single
displacement
reactions.
When
analyzing
single
displacement
reactions,
use
the
following
guidelines:
e
Treat
hydrogen
as
a
metal.
e
Treat
acids,
such
as
HCI,
as
ionic
compounds
of
the
form
H*Cl".
(Treat
sulfuric
acid,
HySO,,
as
HH*SO,%*7).
¢
Treat
water
as
ionic,
with
the
formula
H*(OH").
-
Lithium
metal
reacts
violently
with
waterin
a
single
displacement
reaction.
Lithium
must
be
stored
under
)
W
kerosene
or
oil
to
avoid
reaction
with
atmospheric
moisture,
»
\
or
oxygen.
v.‘
B
|
MY
XE]
When
an
iron
nail
is
placed
in
a
solution
of
copper{ll)
sulfate,
a
single
displacement
reaction
takes
place.
Fes)
+
cu304(aq)
—
FeSO4(aq)
+
Cuig
Notice
the
formation
of
copper
metal
on
the
nail.
Practice
Problems
21.
Each
of
the
following
incomplete
equations
represents
a
single
A
displacement
reaction.
Copy
each
equation
into
your
notebook,
and
write
the
products.
Balance
each
chemical
equation.
When
in
doubt,
use
the
most
common
valence.
(a)
Ca
+
H,0
—
(e)
Pb
+
H,SO,
—
(b)
Zn
+
Pb(NQO3),
—
(h
Mg
+
Pt(OH),
—
(c)
Al
+
HCI
—
(g)
Ba
+
FeCl;
—
(d)
Cu
+
AgNO;
—
(h)
Fe
+
Co(ClO3);
—
\_
J
Through
experimentation,
chemists
have
ranked
the
relative
reactivity
of
the
metals,
including
hydrogen
(in
acids
and
in
water),
in
an
activity
series.
The
reactive
metals,
such
as
potassium,
are
at
the
top
of
the
activity
series.
The
unreactive
metals,
such
as
gold,
are
at
the
bottom.
In
Investigation
4-A,
you
will
develop
an
activity
series
using
single
displacement
reactions.
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
127
;
2
-
stigation
&
-
fA
Creating
an
Activity
Series
of
Metals
Certain
metals,
such
as
silver
and
gold,
are
extremely
unreactive,
while
sodium
is
so
reactive
that
it
will
react
with
water.
Zinc
is
unreactive
with
water.
It
will,
however,
react
with
acid.
Why
will
magnesium
metal
react
with
copper
sulfate
solution,
while
copper
metal
will
not react
with
aqueous
magnesium
sulfate?
In
Chapter
3,
you
learned
that
an
alloy
is
a
solution
of
two
or
more
metals.
Steel
is
an
alloy
that
contains
mostly
iron.
Is
its
reactivity
different
from
iron’s
reactivity?
Question
How
can
you
rank
the
metals,
including
hydro-
gen,
in
terms
of
their
reactivity?
Is
the
reactivity
of
an
alloy
very
different
from
the
reactivity
of
its
major
component?
Predictions
Based
on
what
you
learned
in
Chapter
3
about
periodic
trends,
make
predictions
about
the
Cation
or
solutia
Cu
MICROSCALE
/;
-'
o
-
erforming
and
recordin
‘Analyzing
and
interpreting
relative
reactivity
of
copper,
iron,
magnesium,
zinc,
and
tin.
Explain
your
reasons
for
these
predictions.
What
do
you
know
about
alloys
such
as
bronze,
brass,
and
steel?
Based
on
what
you
know,
make
a
prediction
about
whether
steel
will
be
more
or
less
reactive
than
iron,
its
main
component.
Materials
well
plate(s):
at
least
a
6
X
8
matrix
wash
bottle
with
distilled
water
5
test
tubes
test
tube
rack
dilute
HCl(aq)
6
small
pieces
each
of
copper,
iron,
magnesium,
zinc,
tin,
steel,
galvanized
steel,
stainless
steel
dropper
bottles
of
dilute
solutions
of
CuSO,,
FeSO,4,
MgSQO,,
ZnSO,,
SnCl,
Sn
Zn
Fe
steel
galvanized
steel
stainless
steel
128
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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Safety
Precautions
3.
Look
at
Figure
4.12.
Lithium
reacts
violently
with
water
to
form
aqueous
lithium
hydroxide
e
and
hydrogen
gas.
Do
you
expect
lithium
to
Handle
the
hydrochloric
acid
solution
with
care.
react
with
hydrochloric
acid?
It
is
corrosive.
Wipe
up
any
spills
with
copious
:
(a)
Write
the
balanced
chemical
equation
for
amounts
of
water,
and
inform
your
teacher.
this
reaction.
Procedure
(b)
Is
lithium
more
or
less
reactive
than
magnesium?
1.
Place
your
well
plate(s)
on
a
white
sheet
of
paper.
Label
them
according
to
the
matrix
on
the
previous
page.
4.
What
evidence
do
you
have
that
hydrogen
in
hydrochloric
acid
is
different
from
hydrogen
in
water?
2.
Place
a
rice-grain-sized
piece
of
each
metal
in
the
appropriate
well.
Record
the
appearance
Conclusion
of
each
metal.
_
o
_
_
5.
(a)
Write
the
activity
series
corresponding
to
3.
Put
enough
drops
of
the
appropriate
solution
your
observations.
Include
hydrogen
in
the
to
completely
cover
the
piece
of
metal.
form
of
water
and
also
as
an
ion
(H").
Do
4.
Record
any
changes
in
appearance
due
to
a
not
include
the
alloys.
chemical
reaction.
In
reactions
of
metal
with
(b)
How
did
the
reactivity
of
the
iron
compare
acid,
look
carefully
for
the
formation
of
bub-
with
the
reactivity
of
the
various
types
bles.
If
you
are
unsure
about
any
observation,
of
steel?
repeat
the
experiment
in
a
small
test
tube.
This
will
allow
you
to
better
observe
the
reaction.
6.
How
do
you
think
an
activity
series
for
metal
would
help
you
predict
whether
or
not
a
single
displacement
reaction
will
occur?
Use
5.
If
you
believe
that
a
reaction
has
occurred,
examples
to
help
you explain
your
answer.
write
“r”
on
the
matrix.
If
you
believe
)
e
7.
You
have
learned
that
an
alloy
is
a
homoge-
that
no
reaction
has
occurred,
write
“nr”
on
neous
mixture
(solution)
of
two
or
more
the
matrix.
metals.
Steel
consists
of
mostly
iron.
6.
Dispose
of
the
solutions
in
the
waste
(a)
Which
type
of
steel
appeared
to
be
the
most
beaker
supplied
by
your
teacher.
Do
not
reactive?
Which
type
was
the
least
reactive?
pour
anything
down
the
drain.
Did
you
notice
any
differences?
]
(b)
What
other
components
make
up
steel,
Analysis
galvanized
steel,
and
stainless
steel?
1.
For
any
reactions
that
occurred,
write
the
corresponding
single
displacement
reaction.
Application
2.
(a)
What
was
the
most
reactive
metal
that
you
8.
For
what
applications
are
the
various
types
of
tested?
steel
used?
Why
would
you
not use
iron
for
(b)
What
was
the
least
reactive
metal
that
you
these
applications?
tested?
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
129
A
single
displacement
reaction
always
favours
the
production
of
the
less
reactive
metal.
In
other
words,
the
“free”
metal
that
is
formed
from
the
com-
pound
must
always
be
less
reactive
than
the
metal
that
displaced
it.
For
example,
2AgN03(aq)
ot
CU(S)
—>
CU(N03)2(aq)
+
2Ag(s)
Silver
metal
is
more
stable
than
copper
metal.
In
other
words,
silver
is
below
copper
in
the
activity
series.
\_
PROBLEM
TIP
\l
CHEM
FACT
Most
metals
that
we
use
in
everyday
life
are
actually
alloys.
An
alloy
is
a
solid
solution
of
one metal
(or
non-
metal)
in
another
metal.
For
example,
steel
is
an
alloy
of
iron.
Steel
has
many
uses,
from
construction
to
the
automobile
industry.
If
the
iron
were
not
alloyed
with
other
elements,
it
would
not
have
the
physical
and
chemical
properties
required,
such
as
hardness
and
corrosion
resistance.
The
Metal
Activity
Series
As
you
can
see
in
Table
4.2,
the
more
reactive
metals
are
at
the
top
of
the
activity
series.
The
less
reactive
metals
are
at
the
bottom.
A
reactive
metal
will
displace
or
replace
any
metal
in
a
compound
that
is
below
it
in
the
activity
series.
Metals
from
lithium
to
sodium
will
displace
hydrogen
as
a
gas
from
water.
Metals
from
magnesium
to
lead
will
displace
hydrogen
as
a
gas
only
from
acids.
Copper,
mercury,
silver,
and
gold
will
not
displace
hydrogen
from
acids.
Table
4.2
Activity
Series
of
Metals
CEHERTH
(]
[
ELEER
T
T
e
(T
E
from
cold
water
lithium
Most
Reactive
potassium
o
barium
calcium
sodium
magnesium
aluminum
zinc
chromium
iron
cadmium
cobalt
nickel
I
tin
lead
hydrogen
copper
Imercury
silver
platinum
gold
Least
Reactive
You
can
use
the
activity
series
to
help
you
predict
the
products
of
the
reaction
of
a
metal
and
a
metal-containing
compound.
For
example,
consider
the
following
incomplete
equation.
Fe(s)
+
CUSO4(aq)
—
You
can
see
from
the
activity
series
that
iron
is
above
copper.
This
means
that
iron
is
more
reactive
than
copper.
This
reaction
will
proceed.
Feg)
+
CuSOyaq
—
FeSOyuq)
+
Cug)
The
copper
metal
produced
is
less
reactive
than
iron
metal.
What
about
the
following
incomplete
reaction
between
silver
and
calcium
chloride?
Ag(s)
+
CaClz(aq)
—
Silver
is
below
calcium
in
the
activity
series,
meaning
that
it
is
less
reactive.
There
would
be
no
reaction
between
these
two
substances.
Predict
whether
the
substances
in
the
following
Practice
Problem
will
react.
130
MHR
-
Unit
1
Matter
and
Chemical
Bonding
Practice
Problems
22.
Using
the
activity
series,
write
a
balanced
chemical
equation
for
A
each
single
displacement
reaction.
If
you
predict
that
there
will
be
no
reaction,
write
“NR.”
(a)
Cu
+
MgSQ,
—
(e)
Fe
+
Aly(SOy4);
—
(b)
Zn
+
FeCl,
—
(i
Ni
+
NiCl,
—
(¢)
K+
H,O
—
(g)
Zn
+
H,SO,
—
(d)
Al
+
H,SO,
—
(h)
Mg
+
SnCl,
—
\_
J
Single
Displacement
Reactions
Involving
Halogens
Non-metals,
typically
halogens,
can
also
take
part
in
single
displacement
reactions.
For
example,
molecular
chlorine
can
replace
bromine
from
KBr,
an
ionic
compound,
producing
bromine
and
potassium
chloride.
Clz(g)
+
2KBr(aq)
—
ZKCl(aq)
+
Bry(e)
The
activity
series
for
halogens
directly
mirrors
the
position
of
halogens
in
the
periodic
table.
It
can
be
shown
simply
in
the
following
way.
Fluorine
is
the
most
reactive,
and
iodine
is
the
least
reactive.
F>Cl>Br>I
In
the
same
way
as
you
used
the
activity
series
for
metals,
you
can
use
the
activity
series
for
halogens
to
predict
whether
substances
will
undergo
a
single
displacement
reaction.
For
example,
fluorine
is
above
chlorine
in
the
activity
series.
So,
given
the
reactants
fluorine
and
sodium
chloride,
you
can
predict
that
the
following
reaction
will
occur:
Fz(g)
+
2NaC1(aq)
—
2NaF(aq)
+
Clz(aq)
On
the
other
hand,
iodine
is
below
bromine
in
the
activity
series.
So,
given
the
reactants
iodine
and
calcium
bromide,
you
can
predict
that
no
reaction
will
occur.
Iz(aq]
+
CaBrz(aq)
—
NR
Try
the
following
problems
to
practise
using
the
metal
and
halogen
activity
series
to
predict
whether
reactions
will
occur.
Practice
Problems
~
23.
Using
the
activity
series
for
halogens,
write
a
balanced chemical
equation
for
each
single
displacement
reaction.
If
you
predict
that
there
will
be
no
reaction,
write
“NR”.
(a)
Bry
+
KCl
—
(b)
Cl,
+
Nal
—
24.
Using
the
appropriate
activity
series,
write
a
balanced chemical
equation
for
each
single
displacement
reaction.
If
you
predict
that
there
will
be
no
reaction,
write
“NR”.
(a)
Pb
+
HCl
—
(d)
Ca
+
H,O
—
(b)
KI
+
Bry,
—
(e)
MgSO4
+
Zn
—
(e)
KF
+Cl,
—»
()
Ni+
H,SO,
—
.
J
CHECKP@INT
Based
on
what
you
know
about
the
electronegativity
and
electron
affinity
for
the
halo-
gens,
explain
the
organization
of
the
halogen
activity
series.
J
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
131
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When
a
few
drops
of
silver
nitrate,
AgNO3,
are
added
to
a
sample
of
salt
water,
NaCl,,q),
a
white
precipitate
of
silver
chloride,
AgCl,
is
formed.
Double
Displacement
Reactions
A
double
displacement
reaction
involves
the
exchange
of
cations
between
two
ionic
compounds,
usually
in
aqueous
(water)
solution.
A
double
displacement
reaction
is
also
known
as
a
double
replacement
reaction.
A
general
equation
for
a
double
displacement
reaction
is:
AB+CD
—
CB
+
AD
In
this
equation,
A
and
C
are
cations
and
B
and
D
are
anions.
Consider
the
following
situation.
You
have
two
unlabelled
beakers.
One
contains
distilled
water,
and
the
other
contains
salt
water.
The
two
samples
look virtually
identical.
How
can
you quickly
determine
which
is
the
salt
water
without
tasting
them?
(You
should
never
taste
anything
in
a
chemistry
laboratory.)
A
common
test
for
the
presence
of
chloride
ions
in
water
is
the
addition
of
a
few
drops
of
silver
nitrate
solution.
The
formation
of
a
white
solid
indicates
the
presence
of
chloride
ions,
as
you
can
see
in
Figure
4.14.
A
double
displacement
reaction
has
occurred.
That
is,
the
cations
in
the
reactants
have
essentially
changed
places.
This
switch
is
modelled
in
Figure
4.15.
/N
NaClg)
+
AgNO3@aq
—
AgCl)
+
NaNOj(qq)
EETMZXYRE]
Sodium
chloride
and
silver
nitrate
form
ions
in
solution.
When
silver
ions
and
chloride
ions
come
into
contact,
they
form
a
solid.
Since
silver
chloride
is
virtually
insoluble
in
water,
it
forms
a
solid
compound,
or
precipitate.
Double
displacement
reactions
tend
to
occur
in
aqueous
solution.
Not
all
ionic
compounds,
however,
will
react
with
one
another
in
this
way.
You
can
tell
that
a
double
displacement
reaction
has
taken
place
in
the
following
cases:
e
a
solid
(precipitate)
forms
®
a
gas
is
produced
e
some
double
displacement
reactions
also
form
a
molecular
compound,
such
as
water.
It
is
hard
to
tell
when
water
is
formed,
because
often
the
reaction
takes
place
in
water.
Double
Displacement
Reactions
that
Form
a
Precipitate
A
precipitate
is
a
solid
that
separates
from
a
solution
as
the
result
of
a
chemical
reaction.
You
will
learn
more
about
precipitates
in
Chapter
9.
Many
double
displacement
reactions
involve
the
formation
of
a
precipitate.
Examine
the
double
displacement
reaction
that
occurs
when
aqueous
solutions
of
barium
chloride
and
potassium
sulfate
are
mixed.
A
white
precipitate
is
immediately
formed.
The
equation
for
the
reaction
is
BaClz(aq)
+
K3504(aq)
—
BaSOy)
+
2KC1(aq)
132
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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You
should
think
about
two
questions
when
analyzing
a
double
displacement
reaction.
1.
How
do
we
determine
the
products?
2.
Which
of
the
products—if
any—will
precipitate
out
of
solution?
Barium
chloride
solution
contains
Ba?*
ions
and
Cl~
ions.
Potassium
sulfate
solution
contains
K*
and
SO,*
ions.
When
they
are
mixed,
the
Ba?*
ions
come
in
contact
with
SO,*"
ions.
Because
barium
sulfate
is
insoluble,
the
product
comes
out
of
solution
as
a
solid.
The
K*
ions
and
Cl™
ions
also
come
into
contact
with
each
other,
but
potassium
chloride
is
soluble,
so
these
ions
stay
in
solution.
How
do
you
know
that
the
precipitate
is
BaSO4
and
not
KC1?
More
generally,
how
can
you
predict
whether
a
precipitate
will
be
formed
in
a
double
displacement
reaction?
In
this
chapter,
you
will
be
given
informa-
tion
on
solubility
as
you
need
it.
You
will
learn
more
about
how
to
predict
whether
a
compound
is
soluble
or
not
in
Chapter
9.
Barium
sulfate,
BaSO,
is
not
soluble
in
water,
while
potassium
chloride,
KCl,
is.
Therefore,
a
reaction
will
take
place
and
barium
sulfate
will
be
the
precipitate.
In
summary,
to
determine
the
products
and
their
physical
states
in
a
double
displacement
reaction,
you
must
first
“deconstruct”
the
reactants.
Then
switch
the
cations,
and
“reconstruct”
the
products
using
proper
chemical
formulas.
You
should
then
balance
the
chemical
equation.
You
will
be
given
information
to
determine
which
of
the
products,
if
any,
will
form
a
precipitate.
Finally,
you
can
write
the
physical
state—(s)
or
(aq)—
of
each
product
and
balance
the
equation.
Given
the
following
reactants,
how
would
you
predict
the
products
of
the
reaction
and
their
state?
Note
that
many
hydroxide
compounds,
including
magnesium
hydroxide,
are
insoluble.
Potassium
cations
form
soluble
substances
with
all
anions.
MgClz(aq)
+
KOH(aq)
—
Examine
figure
4.16
to
see
how
to
separate
the
compounds
into
ions,
Mg?*
and
Cl7;
K*
and
OH™.
Then
switch
the
anions
and
write
chemical
formu-
las
for
the
new
compounds.
Check
to
ensure
your
equation
is
balanced.
@
MgClL
+
2KOH
—
Mg(OH)yy
+
2KClag)
—
|
]
2
L,
Mg
OH-
K
-
Predicting
a
double
displacement
reaction.
What
happens
if
both
products
are
soluble
ionic
compounds?
Both
ionic
compounds
will
be
ions
dissolved
in
the
water.
If
neither
product
precipitates
out,
no
reaction
occurs.
Try
the
following
problem
to
practise
writing
the
products
of
double
displacement
reactions
and
predicting
their
states.
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
133
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When
aqueous
solutions
of
barium
chloride
and
sodium
chromate
are
mixed,
a
precipi-
tate
is
formed.
The
balanced
equation
for
this
double
replacement
reaction
is
BaClyjaq)
+
NazCrOs(aq)
—
BaCr04(7)
+
2NaCI(?)
What
is
the
precipitate?
From
experience,
you
know
that
NaCl
is
water
soluble.
So,
by
process
of
elimination,
the
precipitate
must
be
barium
\chromate,
BaCrOyg).
PROBLEM
TIP
MY
XEA
The
reaction
of
hydrochloric
acid
and
sodium
carbonate,
Na,CO;
(washing
soda),
is
a
double
displacement
reaction.
This
reaction
initially
forms
sodium
chloride
and
car-
bonic
acid,
H,C0;.
The
carbonic
acid
spontaneously
decomposes
to
water
and
carbon
dioxide
gas.
Practice
Problems
25.
Write
a
balanced
chemical
equation
for
each
double
displacement
reaction.
Write
“NR”
if
you
predict
that
no
reaction
will
occur.
Note
that
K*,
Na*,
and
Li*
ions
form
soluble
compounds
with
all
anions.
All
nitrate
compounds
are
soluble.
Sulfate
compounds
with
Ca?*,
Sr?*,
Ba?*,
Ra?*,
and
Pb?*
are
insoluble,
but
most
other
sulfate
compounds
are
soluble.
Lead(II)
iodide
is
insoluble.
(a)
Pb(Noa)z(aq)
+
KI(aq)
-
(d)
Ba(NOs)z(aq)
+
MgSOy(aq)
—
\
J
\
Double
Displacement
Reactions
That
Produce
a
Gas
In
certain
cases,
you
know
that
a
double
displacement
reaction
has
occurred
because
a
gas
is
produced.
The
gas
is
formed
when
one
of
the
products
of
the
double
displacement
reaction
decomposes
to
give
water
and
a
gas.
Consider
the
reaction
of
aqueous
sodium
carbonate
(washing
soda)
and
hydrochloric
acid,
shown
in
Figure
4.17.
Hydrochloric
acid
is
sold
at
the
hardware
store
under
the
common
name
“muriatic
acid.”
If
you
carry
out
this
reaction,
you
immediately
see
the
formation
of
carbon
dioxide
gas.
The
first
reaction
that
takes
place
is
a
double
displacement
reaction.
Determine
the
products
in
the
following
way.
Separate
the
reactions
into
ions,
and
switch
the
anions.
Write
chemical
formulas
for
the
products
and
balance
the
equation.
N82C03(aq)
+
ZHCl(aq)
-
2NaCl(aq)
+
H2C03(aq)
But
this
isn’t
all
that
is
happening!
The
carbonic
acid,
H,CO3,
is
unstable
and
subsequently
decomposes
to
carbon
dioxide
and
water.
H2C03(aq)
—
H30(g)
+
COxg
Overall,
we
can
write
this
two-step
reaction
as
follows:
NazCOs(aq)
+
2HCl(ag)
=
2NaClaq)
+
H20(¢)
+
CO2(g)
Another
double
displacement
reaction
results
in
the
formation
of
gaseous
ammonia,
NH;.
Ammonia,
a
pungent-smelling
gas,
is
an
impor-
tant
industrial
chemical.
It
is
used
as
a
fertilizer
and,
when
dissolved
in
water,
as
a
household
cleaner.
Ammonium
hydroxide
is
formed
in
the
reaction
below
NH4C1(aq)
+
NaOH(aq)
-
NH4OH(aq)
+
NaCl(aq)
The
ammonium
hydroxide,
NH,OH,
immediately
decomposes
to
give
ammonia
and
water,
according
to
the
equation
NH4OH(aq)
—>
NH3(g)
+
HZO(g]
Combining
these
equations
gives
NH4C1(aq)
+
NaOH(aq)
—
NaCl(aq)
+
NHg(g]
+
HZO(g]
This
example
illustrates
the
formation
of
a
gas
by
an
initial
double
displacement
reaction,
followed
by
the
decomposition
of
one
of
the
products
to
a
gas
and
water.
134
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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Practice
Problems
N
26.
(a)
When
sodium
sulfite,
Na;SOj3(,q),
is
mixed
with
hydrogen
chloride,
HCl(aq)
(hydrochloric
acid),
the
odour
of
sulfur
dioxide
gas,
SOy,
is
detected.
Write
the
balanced chemical
equation
for
this
reaction.
(b)
Hydrogen
sulfide,
H,S,
is
a
poisonous
gas
that
has
the
odour
of
rotten
eggs.
When
aqueous
calcium
sulfide,
CaS,
is
reacted
with
sulfuric
acid,
a
rotten
egg
smell
is
detected.
Write
the
balanced
chemical
equation
for
this
reaction.
The
Formation
of
Water
in
a
Neutralization
Reaction
Neutralization
reactions
are
a
special
type
of
double
displacement
reaction
that
produces
water.
Neutralization
involves
the
reaction
of
an
acid
with
a
base
to
form
water
and
an
ionic
compound.
You
will
learn
more
about
neutralization
reactions
in
Chapter
10.
For
example,
the
neutralization
of
hydrogen
nitrate
(nitric
acid)
with
sodium
hydroxide
(a
base)
is
a
double
displacement
reaction.
HNOg(aq)
+
NaOH(aq)
-
NaNO3(aq)
+
HZO(Z)
Often
neutralization
reactions
produce
no
precipitate
or
gas.
In
Chapter
10,
you
will
learn
how
chemists
recognize
when
neutralization
reactions
take
place.
Practice
Problems
2].
Write
the
balanced chemical
equation
for
each
neutralization
reaction.
(a)
HCl(aq)
+
LiOH(aq)
—
(b)
HCIO4(aq)
+
Ca(OH);(aq)
—
(c)
HZSO4(aq]
+
NaOH(aq]
—
28.
Write
the
balanced chemical
equation
for
each
double
replacement
reaction.
Be
sure
to
indicate
the
physical
state
of
all
products.
(a)
BaCly(aq)
+
NazCrOyaq)
—
(A
precipitate
is
produced.)
(b)
H3POy(aq)
+
NaOHyq)
—
(Water
is
produced.)
\J
CHEM
FACT
To
non-chemists,
the
term
“salt”
refers solely
to
sodium
chloride.
To
chemists,
“salt”
is
a
generic
term
that
describes
an
ionic
compound
with
an
anion
that
is
not
OH~
or
0%~
and
with
a
cation
that
is
not
H*.
Sodium
chloride,
NaCl,
and
potassium
fluoride,
KF,
are
two
examples.
(c)
K3CO3(aq)
+
HNOg(aq)
—
(A
gas
is
produced.)
J
You
have
learned
about
a
variety
of
double
displacement
reactions.
In
Investigation
4-B,
you
will
make
predictions
about
whether
double
displacement
reactions
will
take
place.
Then
you
will
make
observations
to
test
your
predictions.
In
Investigation
4-C,
you
will
perform
reactions
that
involve
copper
compounds
to
reinforce
what
you
have
learned
about
the
different
types
of
reactions.
You
will
identify
the
series
of
reactions
that
begin
by
reacting
copper
and
finish
by
producing
copper.
mind
ST
RETCH
Consider
the
reaction
The
products
are
both
water
soluble.
Has
a
chemical
reac-
tion
occurred?
If
the
water
is
allowed
to
evaporate,
what
compounds
will
remain?
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
135
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Observing
Double
Displacement
Reactions
A
double
displacement
reaction
involves
the
exchange
of
cations
between
two
ionic
compounds,
usually
in
aqueous
solution.
It
can
be
represented
with
the
general
equation
AB+CD
—
AD+
CB
Most
often,
double
displacement
reactions
result
in
the
formation
of
a
precipitate.
However,
some
double
displacement
reactions
result
in
the
formation
of
an
unstable
compound
which
then
decomposes
to
water
and
a
gas.
The
reaction
of
an
acid
and
a
base—a
neutralization
reaction—is
also
a
type
of
double
displacement
reaction.
It
results
in
the
formation
of
a
salt
and
water.
Question
How
can
you
tell
if
a
double
displacement
reaction
has
occurred?
How
can
you
predict
the
products
of
a
double
displacement
reaction?
Prediction
For
each
reaction
in
Tables
A
and
B,
write
a
balanced
chemical
equation.
Use
the
following
guidelines
to
predict
precipitate
formation
in
Table
A.
¢
Hydrogen,
ammonium,
and
Group
I
ions
form
soluble
compounds
with
all
negative
ions.
¢
Chloride
ions
form
compounds
that
are
not
very
soluble
when
they
bond
to
silver,
lead(Il),
mercury(I),
and
copper(I)
positive
ions.
e
All
compounds
that
are
formed
from
a
nitrate
and
a
positive
ion
are
soluble.
e
With
the
exception
of
the
ions
in
the
first
bulleted
point,
as
well
as
strontium,
barium,
radium,
and
thallium
positive
ions,
hydroxide
ions
form
compounds
that
do
not
dissolve.
¢
Jodide
ions
that
are
combined
with
silver,
lead(II),
mercury(I),
and
copper(I)
are
not
very
soluble.
e
Chromate
compounds
are
insoluble,
except
when
they
contain
ions
from
the
first
bulleted
point.
MHR
«
Unit
1
Matter
and
Chemical
Bonding
T
MICROSCALE
'
o
-
erforming
and
recordin
‘Analyzing
and
interpreting
Materials
well
plate
sheet
of
white
paper
several
test
tubes
test
tube
rack
test
tube
holder
2
beakers
(50
mL)
tongs
scoopula
laboratory
burner
flint
igniter
red
litmus
paper
wooden
splint
wash
bottle
with
distilled
water
HCI
solution
the
following
aqueous
solutions
in
dropper
bottles:
BaCl,,
CaCl,,
MgCl;,
Na,SO,4,
NaOH,
AgNQj;,
Pb(NO3),,
KI,
FeCls,
solid
Na,CO3
and
NH,CI
Safety
Precautions
e
Hydrochloric
acid
is
corrosive.
Use
care
when
handling
it.
e
Before
lighting
the
laboratory
burner,
check
that
there
are
no
flammable
liquids
nearby.
¢
If
you
accidentally
spill
a
solution
on
your
skin,
immediately
wash
the
area
with
copious
amounts
of
water.
e
Wash
your
hands
thoroughly
after
the
experiment.
Procedure
1.
Copy
Tables
A
and
B
into
your
notebook.
Do
not
write
in
this
textbook.
2.
Place
the
well
plate
on
top
of
the
sheet
of
white
paper.
3.
Carry
out
each
of
the
reactions
in
Table
A
by
adding
several
drops
of
each
solution
to
a
well.
Record
your
observations
in
Table
A.
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If
you
are
unsure
about
the
formation
of
a
Analysis
precipitate,
repeat
the
reaction
in
a
small
1.
Write
the
balanced
chemical
equation
test
tube
for
improved
visibility.
for
each
reaction
in
Table
A.
4.
Place
a
scoopula
tipful
of
Na,CO3
in
a
50
mL
9
beaker.
Add
5
mL
of
HCI.
Use
a
burning
wooden
splint
to
test
the gas
produced.
Record
your
observations
in
Table
B.
.
For
each
reaction
in
Table
B,
write
the
appropriate
balanced
chemical
equation
for
the
double
displacement
reaction.
Then
write
a
balanced chemical
equation
for
the
5.
Place
a
scoopula
tipful
of
NH,CI
in
a
test
decomposition
reaction
that
leads
to
the
tube.
Add
2
mL
NaOH.
To
detect
any
odour,
formation
of
a
gas
and
water.
gently
waft
your
hand
over
the
mouth
of
the
test
tube
towards
your
nose.
Warm
the
tube
Conclusion
gently
(do
not
boil)
over
a
flame.
Record
your
3.
How
did
you
know
when
a
double
displace-
observations
in
Table
B.
ment
reaction
had
occurred?
How
did
your
6.
Dispose
of
all
chemicals
in
the
waste
beaker
results
compare
with
your
predictions?
supplied
by
your
teacher.
Do
not
pour
any-
thing
down
the
drain.
Application
Table
A
Double
Displacement
4.
Suppose
that
you
did not
have
any
informa-
Reactions
That
May
Form
a
Precipitate
tion
about
the
solubility
of
various
com-
pounds,
but
you
did
have
access
to
a
large
variety
of
ionic
compounds.
What would
you
need
to
do
before
predicting
the
products
of
FeCl;
+
NaOH
the
displacement
reactions
above?
Outline
a
BaCl,
+
Na,SO,
brief
procedure.
CaC].z
+
AgN03
Pb(NOg)z
+
KI
A
G
GGG
TR
|
Observations
MgCl,
+
NaOH
Table
B
Double
Displacement
Reactions
That
May
Form
a
Gas
Reaction
|
Observations
N82C03
+
HCl
NH,CI
+
NaOH
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
137
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From
Copper
to
Copper
This
experiment
allows
you
to
carry
out
the
sequential
conversion
of
copper
metal
to
copper(Il)
nitrate
to
copper(Il)
hydroxide
to
copper(Il)
oxide
to
copper(Il)
sulfate
and
back
to
copper
metal.
This
conversion
is
carried
out
using
synthesis,
decomposition,
single
displace-
ment,
and
double
displacement
reactions.
Question
What
type
of
chemical
reaction
is
involved
in
each
step
of
this
investigation?
Prediction
Examine
the
five
reactions
outlined
in
the
proce-
dure.
Predict
what
reactions
will
occur,
and
write
equations
to
describe
them.
Materials
hot plate
glass
rod
wash
bottle
with
distilled
water
50
mL
Erlenmeyer
flask
beaker
tongs
250
mL
beaker
containing
ice
and
liquid
water
red
litmus
paper
Cu(NOs3),
solution
*6
mol/L
NaOH
solution
in
dropping
bottle
*3
mol/L
H,SO,
solution
in
dropping
bottle
0.8
g
of
flaked
zinc
Safety
Precautions
Constantly
stir,
or
sw1r1
any
prempltate-
containing
solution
that
is
being
heated
to
avoid
a
sudden
boiling
over,
or
bumping.
e
Unplug
any
hot
plate
not
in
use.
MICROSCALE
/4
=
-
.
A
.
’q"s
erforming
and
Recording
‘Analyzing
and
Interpreting
e
Do
not
allow
electrical
cords
to
hang
over
the
edge
of
the
bench.
e
NaOH
and
H,SO,
solutions
are
corrosive.
Handle
them
with
care.
If
you
accidentally
spill
a
solution
on
your
skin,
wash
the
area
immediately
with
copious
amounts
of
cool
water.
Inform
your
teacher.
Procedure
Reaction
A:
Reaction
of
Copper
Metal
to
form
Copper(ll)
Nitrate
Cugg)
+
4HNO3(aq]
—
Cu(NO3]2(aq)
+
2NO;3(g
+
2H20(y)
Your
teacher
will
carry
out
steps
1
to
4
in
the
fumehood
before
class.
Concentrated
nitric
acid
is
required,
and
the
NOy)
produced
is
poisonous.
Furthermore,
this
reaction
is
quite
slow.
Your
teacher
will
perform
a
brief
demon-
stration
of
this
reaction
so
that
you
may
record
observations.
1.
Place
0.100
g
(100
mg)
of
Cu
in
a
50
mL
Erlenmeyer
flask.
2.
Add
2
mL
of
6
mol/L
HNOj,q)
to
the
flask
in
the
fumehood.
3.
Warm
the
flask
on
a
hot plate
in
the
fumehood.
The
heating
will
continue
until
all
the
Cu
dissolves
and
the
evolution
of
brown
NOy
ceases.
4.
Cool
the
flask
in
a
cool
water
bath.
5.
Add
about
2
mL
of
distilled
water
to
the
flask
containing
the
Cu(NOs);
solution.
*The
unit
mol/L
refers
to
concentration.
You
will
learn
more
about
this
in
Unit
3.
For
now,
you
should
know
that
6
mol/L.
NaOH
and
3
mol/L
H,SO,
are
highly
corrosive
solutions,
and
you
should
treat
them
with
respect.
138
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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Reaction
B:
Preparation
of
Copper(ll)
Hydroxide
11.
When
the
reaction
is
complete,
add
5
mL
of
3
mol/L
sulfuric
acid
while
stirring
or
swirling
6.
At
room
temperature,
while
stirring
with
a
the
solution.
This
removes
any
unreacted
zinc
glass
rod,
add
6
mol/L.
NaOH,
drop
by
drop,
until
the
solution
is
basic
to
red
litmus
paper.
(Red
litmus
paper
turns
blue
in
basic
but
does
not
affect
the
copper
metal.
Carefully
decant
the
liquid
into
a
clean
waste
container.
Wash
the
copper
metal
carefully
several
times
with
water.
Return
the
copper
metal
to
your
teacher.
Wash
your
hands.
This
sulfuric
acid
is
highly
corrosive.
If
any
comes
in
contact
with your
skin,
rinse
the
area
thoroughly
and
immediately
with
water.
solution.)
Do
not
put
the
red
litmus
paper
in
the
solution.
Dip
the
glass
rod
into
the
solution and
touch
it
to
the
red
litmus
paper.
Record
your
observations.
Reaction
C:
Preparation
of
Copper(ll)
Oxide
7.
While
constantly
stirring
the
solution
with
a
Analysis
glass
rod,
heat
the
mixture
from
step
6
on
a
1
hot
plate
until
a
black
precipitate
is
formed.
If
necessary,
use
the
wash
bottle
to
wash
loose
any
unreacted
light
blue
precipitate
that
is
2.
Write
a
balanced chemical
equation
for
adhering
to
the
side
of
the
flask.
reactions
B
through
E.
.
What
type
of
reaction
is
occurring
in
reactions
A
through
E?
3.
Explain
why
H,SO,
reacts
with
Zn
but
not
with
Cu.
(See
step
11
in
the
procedure.)
8.
When
all
of
the
light
blue
precipitate
has
reacted
to
form
the
black
precipitate,
cool
the
flask
in
an
ice
bath
or
a
cool
water
bath
for
4
.
Could
another
metal
have
been
used
in
place
several
minutes.
of
Zn
in
step
10?7
Explain.
Reaction
D:
Preparation
5.
Why
was
powdered
Zn
used
in
step
10,
rather
of
Copper(ll)
Sulfate
Solution
than
a
single
piece
of
Zn?
9.
Carefully
add
about
6
mL
of
3
mol/L
sulfuric
6.
You
used
0.100
g
of
Cu
metal
in
reaction
A.
acid
to
the
flask.
Stir
it
until
all
the
black
precipitate
has
dissolved.
Record
your
observations.
The
sulfuric
acid
is
highly
corrosive.
If
any
comes
in
contact
with
your
skin,
rinse
the
area
thoroughly
and
immediately
with
water.
How
much
copper should
theoretically
be
recovered
at
the
end
of
reaction
E?
Conclusion
1.
Create
a
flowchart
that
shows
each
step
of
the
reaction
series.
Include
the
balanced chemical
Reaction
E:
Regeneration
of
Copper
Metal
equations.
10.
In
the
fumehood
or in
a
well
ventilated
area,
carefully
add
about
0.8
g
of
powdered
zinc
to
the
solution
of
copper(Il)
sulfate.
Stir
or
swirl
the
solution
until
the
blue
colour
disappears.
Record
your
observations.
You
should
wear
a
mask
for
this
step
to
avoid
breathing
in
the
powdered
zinc.
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
139
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(oo
T
T
O
F-
1
[P{-1
gl
Predicting
Chemical
Reactions
Y
Y
Chemical
Reactions
Y
Reaction
Type
General
Equation
Concepts
Synthesis
>
A+B=C
1
Decomposition
-
C>A+B
.|
knowledge
of
bonding
and
periodic
table
_|
A+
oxygen
—oxides
of
A
+
T
Combustion
other
compound(s)
¢
activity
series
of
metals
Y
and
halogens
"|
«knowledge
of
bonding
Y
A+BC—AC+B
Single
Displacement
and
periodic
table
¢
understanding
of
Y
|
solubility
"
|
*knowledge
of
bonding
AC
+
BD—AD
+BC
Y
Double
Displacement
and
periodic
table
Section
Wrap-up
In
sections
4.2
and
4.3,
you
have
examined
five
different
types
of
chemi-
cal
reactions:
synthesis,
decomposition,
combustion,
single
displacement,
and
double
displacement.
Equipped
with
this
knowledge,
you
can
exam-
ine
a
set
of
reactants
and
predict
what
type
of
reaction
will
occur
and
what
products
will
be
formed. The
Concept
Organizer
above
provides
a
summary
of
the
types
of
chemical
reactions.
}
Unit
Project
Prep
Before
you
design
your
Chemistry
Newsletter
at
the
end
of
Unit
1,
take
a
look
at
some
of
the
labels
of
chemical
products
in
your
home.
Are
there
any
warnings
about
mix-
ing
different
products
together?
Use
what
you
know
about
chemical
reactions
to
explain
why
mixing
some
chemical
products
might
be
dangerous.
Section
Review
O
Write
the
product(s)
of
each
single
displacement
reaction.
If
you
predict
that
there
will
be
no
reaction,
write
“NR.”
Balance
each
chemical
equation.
(a)
Li+
H,O
—
(d)
Al
+
MgSO,;
—
(b)
Sn
+
FeCl,
—
(e)
Zn
+
CuSO,;
—
(c)
Fy
+
KI
—
)
K+
H,0O
—
(2]
Complete
each
double
displacement
reaction.
Be
sure
to
indicate
the
physical
state
of
each
product.
Then
balance
the
equation.
Hint:
Compounds
containing
alkali
metal
ions
are
soluble.
Calcium
chloride
is
soluble.
Iron(III)
hydroxide
is
insoluble.
(a)
NaOH
+
Fe(NQOj);
—
(e)
K,CrO4
+
NaCl
—
(b)
Ca{OH),
+
HC]
—
(d)
K,CO3;
+
H;SO,
—
140
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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©
(a)
©
Explain
why
the
following
chemical
equation
represents
a
double
displacement
reaction
followed
by
a
decomposition
reaction.
(NH4)ZSO4(aq)
+
KOH(aq)
—>
NH3(g)
+
HZO(E)
+
KZSO4(aq)
(b)
Balance
the
chemical
equation
in
part
(a).
(4]
Identify
each
reaction
as
synthesis,
combustion
(complete
or
incomplete),
decomposition,
single
displacement,
or
double
displacement.
Balance
the
equations,
if
necessary.
(a)
CgHig(e)
+
Ozg)
=
COyg)
+
H2O(g)
(b)
Pbys)
+
HySO4aq)
—
PbSOye)
+
Hag
(e)
Al2(SO4)saq)
+
KaCrOy(aq)
=
K2SOs(aq)
+
Al2(CrOa)s)
(d)
C3H,OHp)
+
Oy
—
COsg
+
HyOpg
(e)
(NH4)2Cr207()
=
Ny
+
H;O(g)
+
Crz03()
(f)
Mg(s)
+
Na(g)
—
MgaNy(s
(@)
N2Og(g)
>
2NOg
©
D
Biosphere
II
was
created
in
1991
to
test
the
idea
that
scientists
could
build
a
sealed,
self-sustaining
ecosystem.
The
carbon
dioxide
levels
in
Biosphere
II
were
lower
than
scientists
had
predicted.
Scientists
discovered
that
the
carbon
dioxide
was
reacting
with
calcium
hydroxide,
a
basic
compound
in
the
concrete.
(a)
Write
two
balanced
equations
to
show
the
reactions.
Then
classify
the
reactions.
Hint:
In
the
first
reaction,
carbon
dioxide
reacts
with
water
in
the
concrete
to
form
hydrogen
carbonate.
Hydrogen
carbon-
ate,
an acid,
reacts
with
calcium
hydroxide,
a
base.
(b)
Why
do
you
think
scientists
failed
to
predict
that
this
would
happen?
(¢)
Suggest
ways
that
scientists
could
have
combatted
the
problem.
0O
What
reaction
is
shown
in
the
figure
below?
Write
a
balanced
chemical
equation
to
describe
the
reaction,
then
classify
it.
Copper
wire
coated
with
silver
Copper
nitrate
solution
Silver
nitrate
solution
Ag
atoms
coating
wire
Cu
atoms
in
wire
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
141
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4.4
Section
Preview/
Specific
Expectations
In
this
section,
you
will
m
balance
simple
nuclear
equations
m
communicate
your
under-
standing
of
the
following
terms:
nuclear
reactions,
nuclear
equation,
alpha
(o)
particle
emission,
beta
()
decay,
beta
particle,
gamma
fy)
radiation,
nuclear
fission,
nuclear
fusion
|
ol
.
%
.
"
This
patient
is
about
to
undergo
radiation
therapy.
Media
o
LinK
9
The
media
are
full
of
references
to
radioactivity.
For
example,
the
comic
book
hero
Spiderman
gained
the
abilities
of
a
spider
after
being
bitten
by
a
radioactive
spider.
Bart
Simpson
reads
Radioactive
Man
comics.
Can
you
think
of
any
other
references
to
radioactivity
in
popular
culture?
What
kind
of
reputation
do
radioactivity
and
nuclear
reactions
have?
Do
you
think
this
reputation
is
deserved?
Simple
Nuclear
Reactions
You
have
seen
some
chemical
reactions
that
involve
the
formation
and
decomposition
of
different
compounds.
These
reactions
involve
the
rearrangement
of
atoms
due
to
the
breaking
and
formation
of
chemical
bonds.
Chemical
bonds
involve
the
interactions
between
the
electrons
of
various
atoms.
There
is
another
class
of
reactions,
however,
that
are
not
chemical.
These
reactions
involve
changes
that
occur
within
the
nucleus
of
atoms.
These
reactions
are
called
nuclear
reactions.
We
know
that
nuclear
weapons
are
capable
of
mass
destruction,
yet
radiation
therapy,
shown
in
Figure
4.18,
is
a
proven
cancer
fighter.
Smoke
detectors,
required
by
law
in
all
homes,
rely
on
the
radioactive
decay
of
americium-241.
The
human
body
itself
is
radioactive,
due
to
the
presence
of
radioactive
isotopes
including
carbon-14,
phosphorus-32,
and
potassi-
um-40.
Most
people
view
radioactivity and
nuclear
reactions
with
a
mixture
of
fascination,
awe,
and
fear.
Since
radioactivity
is
all
around
us,
it
is
important
to
understand
what
it
is,
how
it
arises,
and
how
we
can
deal
with
it
safely.
Types
of
Radioactive
Decay
and
Balancing
Nuclear
Equations
There
are
three
main
types
of
radioactive
decay:
alpha
particle
emission,
beta
particle
emission,
and
the
emission
of
gamma
radiation.
When
an
unstable
isotope
undergoes
radioactive
decay,
it
produces
one
or
more
dif-
ferent
isotopes.
We
represent
radioactive
decay
using
a
nuclear
equation.
Two
rules
for
balancing
nuclear
equations
are
given
below.
Rules
for
Balancing
Nuclear
Equations
1.
The
sum
of
the
mass
numbers
(written
as
superscripts)
on
each
side
of
the
equation
must
balance.
2.
The
sum
of
the
atomic
numbers
(written
as
subscripts)
on
each
side
of
the
equation
must
balance.
Alpha
Decay
Alpha
(o)
particle
emission,
or
alpha
decay,
involves
the
loss
of
one
alpha
particle.
An
o
particle
is
a
helium
nucleus,
§He,
composed
of
two
protons
and
two
neutrons.
Since
it
has
no
electrons,
an
alpha
particle
carries
a
charge
of
+2.
One
example
of
alpha
particle
emission
is
the
decay
of
radium.
This
decay
is
shown
in
the
following
equation:
225Ra
—
222Rn
+
%He
Notice
that
the
sum
of
the
mass
numbers
on
the
right
(222
+
4)
equals
the
mass
on
the
left
(226).
As
well,
the
atomic
numbers
balance
(88
=
86
+
2).
Thus,
this
nuclear
equation
is
balanced.
142
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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In
another
example
of
alpha
particle
emission,
Berkelium-248
is
formed
by
the
decay
of
a
certain
radioisotope
according
to
the
balanced
nuclear
equation:
9X
—
28Bk
+
3He
Given
this
information,
what
is
$X?
You
can
use
your
knowledge
of
how
to
balance
a
nuclear
equation
to
determine
the
identity
of
a
radioisotope
undergoing
alpha
particle
decay.
The
total
of
the
atomic
masses
on
the
right
side
is
(248
+ 4)
=
252.
The
total
of
the
atomic
numbers
on
the
right
is
(97
+
2)
=
99.
Therefore,
a
=
252
and
b
=
99.
From
the
periodic
table,
you
see
that
element
number
99
is
Es,
einsteinium.
The
missing
atom
is
%32Es,
so
the
balanced
nuclear
equation
is:
232Es
—
238Bk
+
3He
Try
the
following
problems
to
practise
balancing
alpha
emission
nuclear
reactions.
Practice
Problems
29,
Uranium
was
the
first
element
shown
to
be
radioactive.
Complete
the
following
reaction
representing
the
alpha
decay
of
uranium-238.
238
4
goU
—
+
5He
~
30.
Radon-222,
?22Rn,
is
known
to
decay
by
alpha
particle
emission.
Write
a
balanced
nuclear
equation
and
name
the
element
produced
in
this
decay
process.
31.
Plutonium-242
decays
by
emitting
an
alpha
particle.
Write
the
balanced
nuclear
equation
for
this
reaction.
32.
Neodymium-144,
'33Nd,
decays
by
alpha
particle
emission.
Write
the
balanced
nuclear
equation
for
this
nuclear
decay.
Beta
Decay
Beta
(f)
decay
occurs
when
an
isotope
emits
an
electron,
called
a
beta
particle.
Because
of
its
tiny
mass
and
—1
charge,
a
beta
particle,
is
repre-
sented
as
_Ye.
For
example,
hydrogen-3,
or
tritium,
emits
a
beta
particle
to
form
helium-3
as
illustrated
by
the
equation:
SH
-
3He+
%
Notice
that
the
total
of
the
atomic
masses
and
the
total
of
the
atomic
numbers
on
each
side
of
the
nuclear
equation
balance.
What
is
happen-
ing,
however
to
the
hydrogen-3
nucleus
as
this
change
occurs?
In
effect,
the
emission
of
a
beta
particle
is
accompanied
by
the
conversion,
inside
the
nucleus,
of
a
neutron
into
a
proton:
1
1
0
oll
—
.H
+
_1e
neutron
proton
electron
(B
particle)
\J
CHEM
iistory
e
LINK
9
Marie
Curie
discovered
the
element
polonium,
Po,
in
1898.
She
named
polonium
after
Poland,
her
homeland.
Curie
won
two
Nobel
Prizes,
one
in
Physics
(1903)
for
sharing
in
the
discovery
of
radioactivity,
and
one
in
Chemistry
(1911)
for
the
discovery
of
radium,
which
has
been
used
to
treat
cancer.
Radium-226
undergoes
alpha
decay
to
yield
radon-222.
FACT
One
of
the
most
harmful
potential
sources
of
radiation
in
the
home
is
radon
gas.
Radon-222
is
a
product
of
the
decay
of
uranium-containing
rocks
beneath
Earth’s
surface.
Since
radon
is
denser
than
air,
it
can
build
up
to
dangerous
levels
in
basements when
it
seeps
through
cracks
in
walls
and
floors.
Simple
radon
detectors
can
be
purchased
at
hardware
stores.
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
-
MHR
143
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\J
CHEM
FACT
The
nucleus
of
the
most
com-
mon
isotope
of
hydrogen
con-
sists
of
one
proton.
Therefore,
a
proton
can
be
represented
by
H*
or
IH.
-
J
\.J
CHEM
FACT
The
terms
radiation
and
radioactivity
are
often
con-
fused.
Radiation
refers
to
electromagnetic
radiation—
everything
from
gamma
rays,
to
X-rays,
to
visible
light,
to
microwaves,
to
radio
and
television
signals.
Radioactivity,
on
the
other
hand,
involves
the
emission
of
particles
or
energy
from
an
unstable
nucleus.
Carbon-14
is
a
radioactive
isotope
of
carbon.
Its
nucleus
emits
a
beta,
particle
to
form
a
nitrogen-14
nucleus,
according
to
the
balanced
nuclear
equation
shown
below
in
Figure
4.19.
14
14
0
C
—
YN+
_Je
proton
neutron
E
g
+
14
6C
B
particle
(electron)
o
14
0
-N
+
1€
Carbon-14
decays
by
emitting
a
beta
particle
and
converting
to
nitrogen-14.
Notice
that
a
neutron
in
the
nucleus
of
carbon
is
converted
to
a
protron
as
the
P
particle
is
emitted.
Radioactive
waste
from
certain
nuclear
power
plants
and
from
weapons
testing
can
lead
to
health
problems.
For
example,
ions
of
the
radioactive
isotope
strontium-90,
an
alkali
metal, exhibit
chemical
behav-
iour
similar
to
calcium
ions.
This
leads
to
incorporation
of
the
ions
in
bone
tissue,
sending
ionizing radiation
into
bone
marrow,
and
possibly
causing
leukemia.
Given
the
following
equation
for
the
decay
of
stron-
tium-90,
how
would
you
complete
it?
99Sr
—
+
%
Since
both
atomic
numbers
and
mass
numbers
must
balance,
you
can
find
the
other
product.
The
mass
number
of
the
unknown
element
is
equal
to
90
+
0
=
90.
The
atomic
number
of
the
unknown
element
is
equal
to
38
—
(—1)
=
39.
From
the
periodic
table,
you
can
see
that
element
39
is
yttrium,
Y.
The
balanced
nuclear
equation
is
therefore
39Sr
—
20Y
+
e
You
can
check
your
answer
by
ensuring
that
the
total
mass
number
and
the
total
atomic
number
on
each
side
of
the
equation
are
the
same.
Mass
numbers
balance:
90
=
90
+
0
Atomic
numbers
balance:
38
=
39
+
(—1)
Try
the
following
problems
to
practise
balancing
beta
emission
equations.
Practice
Problems
33.
Write
the
balanced
nuclear
equation
for
the
radioactive
decay
of
)
potassium-40
by
emission
of
a
B
particle.
34.
What
radioisotope
decays
by
B
particle
emission
to
form
%7Sc?
35.
Complete
the
following
nuclear
equation:
L
BGa
—>
e+
)
144
NMHR
-
Unit
1
Matter
and
Chemical
Bonding
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Harriet
Brooks
It
was
the
Nobel
that
just
missed
being
Canadian.
In
1907,
Ernest
Rutherford
left
Montréal’s
McGill
University
for
a
position
in
England.
The
following
year,
he
received
the
Nobel
Prize
for
Chemistry
for
his
investigations
of
the
chemistry
of
radioactive
substances.
Most
of
the
work,
however,
had
been
done
in
Montréal.
Moreover,
one
young
Canadian
woman
had
played
an
important
role
in
putting
it
on
the
right
track.
Gamma
Radiation
Harriet
Brooks
is
nearly
forgotten
today,
even
though
she
helped
to
show
that
elements
could
be
transformed.
For
over
a
century,
chemists
had
rejected
the
dream
of
the
ancient
alchemists
who
thought
that
they
might
turn
lead
into
gold
with
the
help
of
the
philosopher's
stone.
They
believed
that
elements
were
forever
fixed
and
unchangeable.
Then
Harriet
Brooks
arrived
on
the
scene.
When
she
joined
Rutherford’s
team,
she
was
asked
to
measure
the
atomic
mass
of
the
isotopes
that
make
up
the
mysterious
vapour
given
off
by
radium.
She
determined
that
its
atomic
mass
was
between
40
and
100,
whereas
radium
was
known
to
have
an
atomic
mass
of
over
140.
Surely
this
was
not
just
a
gaseous
form
of
radium.
Somehow
radium
was
turning
into
another
element!
It
turned
out
that
Brooks’
result
was
a
mis-
take.
Radon—as
the
mystery
gas
is
now
known—
has
almost
the
same
atomic
mass
as
radium.
Brooks'
result
was
a
fruitful
mistake,
however.
Her
experiment
led
to
a
basic
understanding
of
radioactivity
and
isotopes.
Why
did
Rutherford
win
a
Nobel
Prize
for
Chemistry?
Both
he
and
Brooks
worked
as
physicists.
By
proving
that
elements
transformed,
Rutherford,
Brooks,
and
their
co-workers
revolu-
tionized
traditional
chemistry.
Gamma
(y)
radiation
is
high
energy
electromagnetic
radiation.
It
often
accompanies
either
alpha
or
beta
particle
emission.
Since
gamma
radiation
has
neither
mass
nor
charge,
it
is
represented
as
Jv,
or
simply
.
For
example,
cesium-137
is
a
radioactive
isotope
that
is
found
in
nuclear
fall-out.
It
decays
with
the
emission
of
a
beta
particle
and
gamma
radiation,
according
to
the
equation
137
137
0
0
::Cs
—
“g¢Ba
+
_je
+
oY
How
is
gamma
radiation
produced
in
a
radioactive
decay?
When
a
radioactive
nucleus
emits
an
alpha
or
beta
particle,
the
nucleus
is
often
left
in
an
unstable,
high-energy
state.
The
“relaxation”
of
the
nucleus
to
a
more
stable
state
is
accompanied
by
the
emission
of
gamma
radiation.
Nuclear
Fission
and
Fusion
All
cases
of
radioactive
decay
involve
the
atom’s
nucleus.
Since
these
processes
do
not
involve
the
atom’s
electrons, they
occur
regardless
of
the
chemical
environment
of
the
nucleus.
For
example,
radioactive
hydrogen-
3,
or
tritium,
will
decay
by
B
particle
emission
whether
it
is
contained
in
a
water
molecule
or
hydrogen
gas,
or in
a
complex
protein.
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
145
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Mode
Emission
Decay
Change
in
...
Mass
Atomic
Number
of
numbers
numbers
neutrons
o
Decay
o
(3He)
+
d
4
_2
_2
reactant
product
o
expelled
B
Decay
B
nig
-
>
o
+
B
0
+1
-1
in
nucleus
in
nucleus
B
expelled
O
+
Oy
0
0
0
vEmission
2y
excited
stable
vy
photon
nucleus
nucleus
radiated
A
summary
of
alpha
decay,
beta
decay,
and
gamma
emission
Many
chemical
reactions,
once
begun,
can
be
stopped.
For
example,
a
combustion
reaction,
such
as
a
fire,
can
be
extinguished
before
it
burns
itself
out.
Nuclear
decay
processes,
on
the
other
hand,
cannot
be
stopped.
The
principles
of
balancing
nuclear
equations
apply
to
all
nuclear
reactions.
Nuclear
fission
occurs
when
a
highly
unstable
isotope
splits
into
smaller
particles.
Nuclear
fission
usually
has
to
be
induced
in
a
particle
accelerator.
Here,
an
atom
can
absorb
a
stream
of
high-energy
particles
such
as
neutrons,
jn.
This
will
cause
the
atom
to
split
into
smaller
fragments.
For
example,
when
uranium-235
absorbs
a
high
energy
neutron,
jn,
it
breaks
up,
or
undergoes
fission
as
follows:
23%U
+
jn
—
87Br+
+3in
How
would
you
identify
the
missing
particle?
Notice
that
three
neutrons,
ont,
have
a
mass
number
of
3
and
a
total
atomic
number
of
0.
The
total
atomic
mass
on
the
left
side
is
(235
+
1)
=
236.
On
the
right
we
have
(87
+
3(1))
=
90,
and
so
(236
—
90}
=
146
remains.
The
missing
particle
must
have
a
mass
number
of
146.
The
total
atomic
number
on
the
left
is
92.
The
total
atomic
number
on
the
right,
not
including
the
missing
particle,
is
35.
This
means
that
(92
—
35)
=
57
is
the
atomic
number
of
the
missing
particle.
From
the
periodic
table,
atomic
number
57
corresponds
to
La,
lanthanum.
The
balanced
nuclear
equation
is
235U
+
¢n
—
87Br+
%La
+
3}n
Check
your
answer
by
noting
that
the
total
mass
number
and
the
total
atomic
number
are
the
same
on
both
sides.
146
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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Nuclear
fusion
occurs
when
a
target
nucleus
absorbs
an
accelerated
particle.
The
reaction
that
takes
place
in
a
hydrogen
bomb
is
a
fusion
reaction,
as
are
the
reactions
that
take
place
within
the
Sun,
shown
in
Figure
4.21.
Fusion
reactions
require
very
high
temperatures
to
proceed
but
produce
enormous
amounts
of
energy.
The
fusion
reaction
that
takes
place
in
a
hydrogen
bomb
is
represented
by
the
following
equation:
Li+
jn
—
SH+
%He
Notice
that
the
total
mass
numbers
and
the
total
atomic
numbers
are
the
same
on
both
sides.
GETIEY®X]
The
Sun's
interior
.
has
a
temperature
of
about
Practice
Problems
15
000 000
°C,
due
to
the
energy
N\
provided
by
nuclear
fusion
36.
Astatine
can
be
produced
by
the
bombardment
of
a
certain
atom
reactions.
with
alpha
particles,
as
follows:
+3He
—
211At+2ln
Identify
the
atom.
37.
Balance
the
following
equation
by
adding
a
coefficient.
232CE+
2B
—
22'Md
+
on
38.
How
many
neutrons
are
produced
when
U-238
is
bombarded
with
C-12
nuclei
in
a
particle
accelerator?
Balance
the
following
equation.
238U
+
12C
—
238Cf
+
in
39.
Aluminum-27,
when
it
collides
with
a
certain
nucleus,
transforms
into
phosphorus-30
along
with
a
neutron.
Write
a
balanced
nuclear
equation
for
this
reaction.
\-
J
Section
Wrap-Up
In
this
chapter,
you learned
how
atoms
can
interact
with
each
other
and
how
unstable
isotopes
behave.
In
the
first
three
sections,
you
learned
about
chemical
reactions.
In
section
4.4,
you
learned
about
different
types
of
nuclear
reactions:
reactions
in
which
atoms
of
one
element
change
into
atoms
of
another
element.
In
Unit
2,
you
will
learn
how
stable
isotopes
contribute
to
an
indirect
counting
method
for
atoms
and
molecules.
Section
Review
(1]
Draw
a
chart
in
your
notebook
to
show
alpha
decay,
beta
decay,
gamma
decay,
nuclear
fusion,
and
nuclear
fission.
Write
a
description
and
give
an
example
of
each
type
of
reaction.
Illustrate
each
example
with
a
drawing.
(2]
Complete
each
nuclear
equation.
Then
state
the
type
of
nuclear
reaction
that
each
equation
represents.
(a)
232Th
+
—23Th
(b)
23Pa
23U+
(c)
228Ra
—
+
3He
(d)
219Bi
—205T1
+
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
147
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(e)
219Bi
—
+298
T1
+
(f)
+on
—>30Sr
+
133Xe
+
35n
(g)
8Li
+
2H
—
2
۩
D
Nuclear
reactors
have
complex
cooling
systems
that
absorb
the
heat
given
off
by
the
fission
reaction.
The
absorbed
heat
is
used
to
produce
steam
to
drive
a
generator,
thus
producing
electrical
energy.
Cooling
the
steam
for
re-use
requires
a
large
amount
of
cool
water,
which
is
usually
obtained
from
a
nearby
river
or
lake.
A
large
amount
of
hot
water
is
then
released
into
the
river
or
lake.
Do
you
think
this
is
a
form
of
pollution?
What
kinds
of
problems
might
warm
water
cause?
(4]
Alpha
or
beta
particle
emission
from
a
radioactive
nucleus
is
often,
but not
always,
accompanied
by
gamma
rays.
Why
does
the
presence
of
gamma
rays
not
affect
how
a
nuclear
equation
of
this
type
is
balanced?
O
Write
a
balanced
nuclear
equation
to
describe
each
of
the
following
statements.
Classify
the
reactions.
(a)
Radon-222
undergoes
alpha
decay,
forming
polonium-218.
(b)
When
hydrogen-2
(deuterium)
and
hydrogen-3
(tritium)
react,
they
form
an
alpha
particle
and
a
subatomic
particle.
(c)
Bismuth-214
undergoes
beta
decay,
emitting
one
electron
and
forming
a
different
nucleus.
(d)
When
a
neutron
collides
with
uranium-235,
it
forms
krypton-92
and
one
other
nucleus.
(e)
Polonium-218
decays
to
lead-214,
emitting
one
other
particle.
(i
Strontium-90
emits
a
subatomic
particle,
forming
yttrium-90.
148
MHR
-
Unit
1
Matter
and
Chemical
Bonding
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Review
Reflecting
on
Chapter
4
Summarize
this
chapter
in
the
format
of
your
choice.
Here
are
a
few
ideas
to
use
as
guidelines.
¢
Distinguish
between
chemical
reactions
and
nuclear
reactions.
e
Summarize
guidelines
for
balancing
chemical
equations.
e
Summarize
the
different
types
of
chemical
reactions.
¢
Summarize
the
types
of
nuclear
decay.
e
Explain
why
knowing
the
solubility
of
compounds
is
important
to
predicting
double
displacement
reactions.
e
Summarize
guidelines
for
balancing
nuclear
equations
e
Describe
how
to
use
the
activity
series
of
metals
and
the
activity
series
of
halogens.
Reviewing
Key
Terms
For
each
of
the
following
terms,
write
a
sentence
that
shows
your
understanding
of
its
meaning.
activity
series
neutralization
reactions
alpha
(o)
particle
emission
nuclear
equation
balanced
chemical
equation
nuclear
fission
beta
particle
nuclear
fusion
beta
()
decay
chemical
equations
chemical
reactions
combustion
reaction
decomposition
reaction
double
displacement
reaction
gamma
(y)
radiation
incomplete
combustion
law
of
conservation
of
mass
nuclear
reactions
precipitate
product
reactant
single
displacement
reactions
skeleton
equation
synthesis
reaction
word
equation
Knowledge/Understanding
1.
How
can
you
tell
if
a
chemic.al
reaction
has
occurred?
2.
Explain
why
the
mixing
of
red
paint
with
white
paint
does
not
constitute
a
chemical
reaction,
even
though
the
“product”
has
a
different
appearance.
3.
Explain
how
balancing
a
chemical
equation
satisfies
the
law
of
conservation
of
mass.
4.
Copy
each
chemical
equation
into
your
notebook,
and
balance
it.
(a)
PdClz(aq)
+
HNO;;(aq)
—>
Pd(NOg)z(aq]
+
HCl(aq)
(b)
CI‘(S)
+
HCl(aq)
—>
CI‘Clz(aq)
+
Hz(g)
(e)
FeOg)
+
Oz
—
Fea0s3
5.
What
type
of
chemical
reaction
is
illustrated
in
each
diagram
below?
x&/
o
g
-
&
PO
D
d
>
P
|-
f)
6.
Classify
each
reaction
as
synthesis,
decomposi-
tion,
single
displacement,
double
displacement,
or
combustion.
Also,
balance
each
chemical
equation.
(a)
Hz(g)
+
CuO(S]
-
Cu(s)
+
HZO(g)
(b)
Ag(s)
+
Sa(s)
=
AB2S(s)
(e}
C4Hg(g)
+
Oarg)
=
COzg)
+
HaOfg)
(d)
NHjg)
+
HCI(g)
—
NH,Cl(y
(e)
Mg()
+
Ozg)
=
MgOy)
(fl
RbCl)
+
O
—>
RbCl1O0,
(g)
Clle(s]
+
Oz(g)
—>
CuZO(g)
+
SOZ(g)
.
Why
is
the
solubility
chart
useful
for
analyzing
double
displacement
reactions?
.
Nitrogen
dioxide
is
a
component
of
smog.
It
is
produced
in
an
automobile
engine’s
combus-
tion
chamber.
When
exposed
to
sunlight,
nitrogen
dioxide
forms
nitrogen
monoxide
and
oxygen.
What
type
of
reaction
is
this?
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
149
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9.
Write
a
balanced
chemical
equation
corresponding
to
each
word
equation.
(a)
The
reaction
between
aqueous
sodium
hydroxide
and
iron(III)
nitrate
produces
a
precipitate.
(b)
Powdered
antimony
reacts
with
chlorine
gas
to
produce
antimony
trichloride.
(c)
Mercury(II)
oxide
is
prepared
from
its
elements.
(d)
Ammonium
nitrite
decomposes
into
nitrogen
gas
and
water.
(e)
Aluminum
metal
reacts
with
a
solution
of
zinc
sulfate
to
produce
aluminum
sulfate
and
metallic
zinc.
10.
Consider
the
unbalanced
chemical
equation
corresponding
to
the
formation
of
solid
lead(II)
chromate,
PbCrQOy:
Pb(NOs)Z(aq)
+
K2C1‘04(aq)
—
PbCI‘O4(S)
+
KNO3(aq)
(a)
What
type
of
chemical
reaction
is
this?
(b)
Balance
the
equation.
11.
In
general,
what
is
formed
when
an
oxide
of
a
non-metal
reacts
with
water?
Give
an
example.
12.
In
general,
what
is
formed
when
an
oxide
of
a
metal
reacts
with
water?
Give
an
example.
13.
Complete
and
balance
each
nuclear
equation.
Then
classify
the
reaction.
(a)
2H
+
3H
—
4He+
(b)
gggU
—
+
91.3
(c)
22°Np
—
23%Pu
+
(d)
238U
—
234Th
+
+
207
14.
Write
the
product(s)
for
each
reaction.
If
you
predict
that
there
will
be
no
reaction,
write
“NR.”
Balance
each
chemical
equation.
(a)
BaClz(aq)
+
NayCO3z(aq)
—
(b)
Fe(s)
+
CuSOyaq)
—
()
CzHag)
+
Oag)
—
(d)
PCls()
—
(e)
Mg
+
Fe0O3
—
(f)
Cag)
+
Clz(g)
—
+
Clz(g)
15.
Iron
often
occurs
as
an
oxide,
such
as
Fe;03.
In
the
steel
industry,
Fe,Oj
is
reacted
with
carbon
monoxide
to
produce
iron
metal
and
carbon
dioxide.
Write
the
balanced chemical
equation
for
this
reaction,
and
classify
it.
16.
Calcium
chloride
is
often
used
to
melt
ice
on
roads
and
sidewalks,
or
to
prevent
it
from
forming.
Calcium
chloride
can
be
made
by
150
MHR
-
Unit
1
Matter
and
Chemical
Bonding
reacting
hydrochloric
acid
with
calcium
car-
bonate.
Write
the
balanced chemical
equation
corresponding
to
this
reaction,
and
classify
it.
Inquiry
172.
18.
An
American
penny
is
composed
of
a
zinc
core
clad
in
copper.
Some
of
the
copper
is
filed
away,
exposing
the
zinc,
and
placed
in
a
solution
of
hydrochloric
acid.
Describe
what
will
occur.
What
will
happen
to
a
silver
earring
that
is
accidentally
dropped
into
toilet
bowl
cleaner
that
contains
hydrochloric
acid?
Communication
19.
20.
21.
22.
Explain
why
it
is
advisable
to
store
chemicals
in
tightly
sealed
bottles
out
of
direct
sunlight.
Why
is
smoking
not
allowed
near
an
oxygen
source?
What would happen
if
a
match
were
struck
in
an
oxygen-rich
atmosphere?
Even
if
a
smoker
is
very
careful
not
to
let
a
lighted
cigarette
come
in
contact
with
liquid
gasoline,
why
is
it
very
dangerous
to
smoke
when
refuelling
an
automobile?
Solutions
that
have
been
used
to
process
film
contain
silver
ions,
Ag{aq).
(a)
Explain
how
you could
recover
the
silver,
in
the
form
of
an
ionic
compound.
(b)
How
could you
recover
the
silver
as
silver
metal?
Making
Connections
23.
Calcium
oxide,
CaO
(lime),
is
used
to
make
mortar
and
cement.
(a)
State
two
reactions
that
could
be
used
to
make
lime.
Classify
each
reaction,
based
on
the
types
of
reactions
studied
in
this
chapter.
(b)
In
construction,
cement
is
prepared
by
mixing
the
powdered
cement
with
water.
Write
the
chemical
equation
that
represents
the
reaction
of
calcium
oxide
with
water.
Why
are
we
cautioned
not
to
expose
skin
to
dry
cement
mix and
wet
cement?
It
may
help
you
to
know
that
bases
are
often
corrosive.
They
can
burn
exposed
skin.
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Answers
to
Practice
Problems
and
Short
Answers
to
Section
Review
Questions
Practice
Problems:
1.(a)
calcium
+
fluorine
(reactants)
—
calcium
fluoride
(product)
(b)
barium
chloride
+
hydro-
gen
sulfate
—
hydrogen
chloride
+
barium
sulfate
{¢)
calcium
carbonate
+
carbon
dioxide
+
water
—
calcium
hydrogen
carbonate
(d)
hydrogen
peroxide
—
water
+
oxygen
(e)
sulfur
dioxide
+
oxygen
—
sulfur
trioxide
2.
Sugar
—
ethanol
+
carbon
dioxide
3.(a)
Zn(s)
+
Clz(g)
—
ZnClz(s)
(b)
Ca(s)
+
HzO(l)
-
Ca(OH)z(aq)
+
Hz(g)
()
Bag)
+
S(S)
-
BaS(S)
(d)
Pb(NOg)z(aq)
+
Mg(s)
—
Mg(N()g)z(aq)
+
Pb(s)
4.(a)
COZ(g)
+
CaO(s)
—
CaCOg(g)
(b)
Al(s)
+
Oz(g)
—
A1203(s)
(c)
Mg
+
Oz(g)
—
MgO(s)
B.(a)
S(s)
+
Oz(g)
—
Soz(g)
(b)
P4(s)
+
502(g)
—
P4010(s)
(c)
Hz(g)
+
Clz(g)
-
ZHCI(g)
(d)
Soz(g)
+
HZO(l)
-
H2503(aq)
6.(a)
balanced
(b)
ZHgO(s)
—
ZHg(l)
+
Oz(g)
(c)
HzOz(aq)
—
ZHZO(l)
+
Oz(g)
(d)
balanced
17.a)
ZSOZ(g)
+
Oz(g)
—
2503(g)
(b)
BaClz(aq)
+
NaZSO4(aq)
—
NaCl(aq)
+
BaSO0y()
8
Py
+
502(g)
—
P4O1¢(s);
P4O1g(s)
+
6H20()
—
4H3PO4(aq)
9.(a)
ASsSe(s)
+
QOZ(g)
—
As4Og(5)
+
GSOZ(g)
(b)
Sc203)
+
3H0p)
—
ZSC(OH]g(S)
(e)
CoHsOHgy
+
302(g)
—
2C0;3(g
+
3H20q)
(d)
2C4H1gg)
+
902
—
8CO0,
+
10H20(g)
10.{(a)
2K
+
Br,
—
2KBr
(b)
H;
+
Clz
—
2HCI
()
Ca
+
Cl;
—
CaCl;
(d)
Li
+
O,
—
LiO,
11.a)
products
are
Fe;O3,
FeO
(b)
possible
products:
V05,
VO,
V,03,
VO;
(e)
possible
products:
TiO,,
TiO,
Ti,O3
12(a)
K,O
+
H,0
—
2KOH
(b)
MgO
+
H,0
—
Mg(OH),
{c)
SO,
+
H,O —
H,SO3;
13.
NHg(g)
+
HCl(g)
—
NH4C1(S)
14.
Hg,
Oz
15.(a)
2HI
—
H,
+
I,
(b)
2Ag20
—>
4Ag
+
02
{c)
2A1C13
—
2Al
+
3C12
{d)
MgO
—>
Mg
+
Oz
16.(a)
MgCO3
—
MgO
+
CO;
(b)
CuCO3
—
CuO
+
CO,
17.
2CH;0H
+
30,
—
2C0,
+
4H,0
18.
2C8H18
+
250,
— 16C0,
+
18H,O
19.
C3H60
+
0y
—
CO,
+
H,O
20.
2C16H34
+
490,
—
32C0,
+
34H,0
21.(a)
Ca
+
2H,0O
—
Ca(OH);
+
H,
(b)
Zn
+
Pb(NQO3);
—
ZD(N03)2
+
Pb
(¢)
2Al
+
6HCl
—
2A1C13
+
3H,
(d)
Li+
AgN03
—>
Ag
+
L1N03
(e)
Pb
+
stO4
—>
PbSO4
+
H,
h
2Mg
+
Pt(OH),
—
2Mg(OH),
+
Pt
(g)
Ba
+
FeCl,
—
BaClz
+
Fe
(h)
Fe
+
CO(C103)2
—>
FB(C103]3
+
Co
22.(a)
NR
(b)
Zn
+
FeCl,
—
ZnCl;
+
Fe
(¢)
K
+
H,O
—
KOH
+
H,
(d)
2Al
+
3H,SO,
—
Al»(SO,)3
+
3H,
(e)
NR
H
NR
(g)
Zn
+
H,SO,
—
ZnSO,
+
H;
(h)
Mg
+
SnCl;
—
MgCl;
+
Sn
23a)
NR
(b)
Cl;
+
2Nal
—
2NaCl
+
I,
24.(a)
2Pb
+
2HCI
—
2PbCl
+
H,
(b)
KI
+
Br,
—
KBr
+1,
(c)
NR
(d)
Ca
+
Hzo
—>
C&(OH)Z
+
Hz
(e)
NR
(f)
Ni+
H,SO,;
—
NiSQO,;
+
H,
25(a)
Pb(NO3)2(aq)
+
ZKI(aq)
—
ZKN03(aq)
+
PbIZ(S)
(b)
NR
{c)
NR
(d)
Ba(N03)2(aq)+
Mg(SO4)(aq)
—
BaSOy
+
Mg(NO;g)z(aq)
26.(a)
NaZSO3(aq)
+
ZHCI(aq)
—
Soz(g)
+
2NaC1(aq)
+
H20q
(b)
CaS(aq)+
HZSO4(aq)
—
HZS(g)
+
CaSO4(1)
21.(a)
HCl(aq)
+
LiOH(aq)
—
HZO(I)
+
LiCl(aq)
(b)
HClO4(aq)
+
Ca(OH)Z(aq)
—
HZO(I)
+
Ca(ClO4)2(aq)
(c)
HzSO4(aq)
+
NaOH(aq)
—
Nast4(aq)
+
H,Oq)
284a)
BaClz(aq)
+
NazCrO4(aq)
—
BaCrQOy)
+
2NaC1(aq)
(b)
HNOg(aq)
+
NaOH(aq)
—
H,0q)
+
NaN03(aq)
{c)
K2C03(aq)
+
ZHN03(aq)
—
H,Oq)
+
ZKN03(aq)
+
COz(g)
29.
[234/90]Th
30.[222/86]Rn
—
[4/2]He
+
[218/82]Pb
31.
[242/94]Pu
—
[4/2]He
+
[238/92]U
32.
[144/60]Nd
—
[4/2]He
+
[140/58]Ce
33.[40/19]K
—
[0/
—1]e
+
[40/20]Ca
34.[47/20]Ca
35.[73/31]Ga
—
[0/
—1]e
+[73/32]Ge
36.[208/83]Bi
37.5
38.4
39.
[27/13]Al+
[4/2]He
—
[30/15]P
+
[1/0]n
Section
Review:
4.1:
2(a)
250,
+
Oz
—
2503
(b)
Nag)
+
H2Oq)
—
Hz(g)
+
NaOH(aq)
(c)
Cugg
+
HNOg(aq)
—
CU(N03)z(aq)
+
Noz(g)
+H;0q)
4.(a)
4A1(s)
+
302(g)
—
42A1203(s)
(b)
2N328203(aq)
+
Iz(aq)
-
2NaI(aq)
+
NaZS4OG(aq)
(c)
ZAI(S)
+
Fezo;;(s)
—
A1203(s)
+
2Fey,
(d)
4NH3(g)
+
502(g)
-
4NO(g)
+
6H20q)
(e)
NaOg)+
(NH4)2504¢aq)
+
H2Oq)
+
NHaag)
)
CsHazqy
+
802
—
5C02(g)
+
BHZO(g)
5.
Fe()
+
CUSO4(aq)
—
Cu
+
FGSO4(aq)
4.2:
1(a)
Be
+
O,
— BeO
()
2Li
+
Cl,
—
2LiCl
{c)
Mg
+
Ny
—
MgsN;
(d)
Ca
+
Br,
—
CaBr;
2.a)
2K;0
—
Oz
+
4K
(b)
2Cu0O
—
2Cu
+
Oz
(c)
ZHzo
—>
ZHZ
+
02
(d)
2NizO3
—
4Ni
+
30,
(e)
2Ag,0
—
4Ag
+
O,
3.(a)
Sn(OH)45)
—
SnOjy()
+
2H;0(g),
decomposition
(b)
3Cl2(g)
+
Iy
—
2ICl;
synthesis
(¢)
C;HgOH
+
60,
—
5H,0
+
4CO,
b&.
ZHgO(s)
—
Oz(g)
+
2Hg()
decomposition
4.3:
1.a)
Li
+
H;O
—
Li;O
+
H;
(b))
NR
(¢)
Fo
+
2KI
—
2KF
+
I,
(d)
NR
(e)
Zn
+
CuSO,
—
Cu
+7ZnS0,
HK
+
H,O —
K,0
+
H,
2(a)
NaOHgq)+
FG(N03)3(aq)
—
NaNO;;(aq)
+
FG(OH)g(S)
(b)
Ca(OH)Z(aq)+
HCl(aq)
-
CaClz(aq)
+
HZO)(l)
{¢)
NR
(d)
K2C03(s)+
HZSO4(aq)
-
KZSO4(aq)
+
COz(g)
+
H20(1)
3.(b)
(NH4]ZSO4(aq)
+
ZKOH(aq)
—
2NHjg)
+
2H,0q,
+
K3S04(aq)
4{a)
incomplete
combustion
(b)
single
displacement
(c¢)
double
displacement
(d)
complete
combustion
(e)
decomposition
(f)
synthesis
{g)
decomposition
5.4:
2(a)
[1/0]n
(b)
[0/ —
1]e
{e)
[222/2]Rn
(d)
[4/2]He
(e)
[236/92]U
f)
[4/2]He
Chapter
4
Classifying
Reactions:
Chemicals
in
Balance
«
MHR
151
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Project
Developing
a
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Background
Many
of
the
chemicals
in
your
school laboratory
are
hazardous.
Some
are
corrosive,
some
are
flammable,
and
some
are
poisonous.
Many
exhibit
these
proper-
ties
when
they
are
combined.
You
can
work
safely
with
these
chemicals,
as
long
as
you
treat
them
with
care
and
respect,
observe
proper
safety
precautions,
and
follow
the
directions
that
are
given
by
your
teacher and
this
textbook.
Did
you
know
that
many
of
the
chemical
products
in
your
home
are
hazardous,
too?
For
example,
com-
mon
household
bleach,
when
used
as
directed,
is
safe
for
disinfecting
and
whitening
clothing.
Hazard
labels
on
bleaching
products,
however,
warn
against
mixing
bleach
with
acids,
household
ammonia,
or
products
that
contain
these
chemicals.
Bleach,
when
combined
with
acids,
produces
toxic
chlorine
gas.
The
products
of
combining
bleach
with
ammonia
are
explosive.
Most
homes
contain
numerous
chemical
products,
ranging
from
cleaners
and
disinfectants,
to
fertilizers
and
fuels.
All
potentially
hazardous
products
have
a
warning
on
their
containers
or
on
paper
inserts
in
their
packaging.
Many,
but
not
all,
have
a
list
of
the
chemicals
they
contain.
Some
hazardous
products
advise
users
only
to
keep
them
away
from
children
and
pets.
How
much
do
you
know
about
the
safe
use
of
chemical
products?
Would
you
know
what
to
do
if
an
accidental
spill
occurred?
Would
the
members
of
your
family,
or
people
in
your
community,
know
what
to
do?
Challenge
Design,
produce,
and
distribute
a
newsletter
to
inform
your
community
about
the
safe
use
of
common
chemical
products.
Include
the
potential
hazards
of
these
products
to
living
things
and
the
environment.
Also
include
emergency
procedures
to
follow
if
an
accident
occurred.
Materials
Select
a
medium
for
your
newsletter,
such
as
a
traditional
paper
newsletter
or
an
electronic
version
for
the
Internet.
For
a
traditional
newsletter,
you
will
need
to
decide
on
methods
of
production
and
distribution.
For
an
electronic
version,
you
will
need
to
use
computer
hardware
and
software.
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After
you
complete
this
project:
m
Assess
the
success
of
your
project
based
on
how
similar
the
final
project
is
to
your
action
plan.
Desi
Criteri
I
m
Assess
your
project
based
on
how
clearly
the
esign
Criteria
chemistry
concepts
and
safety
recommendations
(A
As
a
class,
develop
a
rubic
listing
criteria
for
7
are
conveyed.
assessing
the
newsletters.
For
example,
one
|
criterion
may
involve
a
newsletter’s
effectiveness
in
altering
the
behaviour
of
its
readers.
You
may
want
to
develop
different
criteria
for
traditional
and
elec-
tronic
newsletters.
.
Your
newsletter
must
be
factual,
easy
to
read
for
a
wide
variety
of
audiences,
and
educational.
m
Assess
your
project
using
the
rubric
designed
in
class.
Action
Plan
@
The
following
items
must
be
part
of
your
newsletter:
e
examples
of
household
chemical
products
and
their
uses
»
hazards
associated
with
each
chemical
product
*
suggestions
to
encourage
safe
and
responsible
use
e
environmental
considerations
for
the
disposal
of
the
chemical
products
e
alternative
products
(if
any),
and
hazards
(if
any)
associated
with
these
alternatives
e
an
interview
with
a
professional
who
researches,
develops,
or
works
with
household
chemical
products
ODevelop
detailed
steps
to
research,
plan,
and
produce
your
newsletter.
Include
deadlines
for
completion
and
specific
roles
for
the
members
of
your
group
(for
example,
editor,
writers,
artists,
and
designers).
Evaluate
Present
your
completed
newsletter
to
your
class.
Hold
a
focus
group
session
to
evaluate
the
content
and
impact
of
your
newsletter.
The
focus
group
could
include
students
from
other
classes,
parents and
relatives,
and
members
of
the
community.
:
'
‘:;.‘.".':
E;
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Review
Knowledge/Understanding
Multiple
Choice
In
your
notebook,
write
the
letter
for
the
best
answer
to
each question.
1.
Which
statement
is
the
best
scientific
description
(based
on
observations)
of
a
car?
(a)
It
is
red,
and
it
goes
fast.
(b)
It
was
made
in
Detroit
by
unionized
workers,
using
metal and
fibreglass.
(c)
It
has
chrome
bumpers,
a
red
fibreglass
body,
and
wheels
made
of
a
magnesium
alloy.
It
has
been
tested
on
a
straight
road
and
found
to
be
able
to
accelerate
from
0
to
60
km/h
in
4.9
s.
(d)
It
is
owned
by
my
cousin.
(e)
My
cousin
bought
it
at
the
car
dealership
down
the
street.
She
got
a
good
deal
on
it.
2.
An
ocean
is
not
a
solution
because
(a)
solutions
cannot
contain
salt
(b)
solutions
cannot
be
blue
(c)
solutions
should
not
have
particles
that
can
be
seen
(d)
solutions
should
not
be
clear
enough
to
see
through
them
(e)
a
whale
could
not
breathe
through
a
solution
3.
Which
mass
is
expressed
to
four
significant
dig-
its?
(a)
0.0027
g
(¢)
0.270
g
(e)
2.700
g
(b)
0.027
g
(d)
2.70
g
4.
Suppose
that
you
multiply
a
density
of
13.6
g/cm?®
by
a
volume
of
2.0
cm?®.
How
many
significant
digits
does
the
resulting
mass
have?
(a)
five,
because
you
add
the
total
number
of
significant
digits
in
the
question
(b)
three,
because
you
use
the
greatest
number
of
significant
digits
in
the
numbers
in
the
question
(c)
six,
because
you
multiply
the
significant
digits
in
the
question
when
you
multiply
the
numbers
(d)
two,
because
you
use
the
least
number
of
significant
digits
in
the
numbers
in
the
question
(e)
as
many
as
you
like,
because
both
of
the
given
quantities
are
exact
numbers
154
MHR
-
Unit
1
Matter
and
Chemical
Bonding
.
Now
suppose
that
you
measure
the
mass
of
a
chemical
on
a
filter
paper.
The
mass
of
the
filter
paper
is
1.6
g.
The
mass
of
the
chemical
and
the
filter
paper,
together,
is
14.168
g.
How
many
significant
digits
should
the
final
mass
of
the
chemical
have?
(a)
three,
because
you
subtract
to
determine
the
number
of
significant
digits
(b)
three,
because
you
use
the
least
number
of
significant
digits
after
the
decimal
place
(the
tenths place
in
this
question)
(c)
five,
because
you
measured
the
chemical
and
filter
paper
very
accurately
and
you
want
your
answer
to
be
as
precise
as
possible
(d)
two,
because
you
should
use
the
least
number
of
significant
digits
in
the
numbers
in
the
question
(e)
as
many
as
you
like,
because
both
of
the
given
quantities
are
exact
numbers
.
Rust
is
an
example
of
(a)
a
compound
(b)
an
element
(c)
a
homogeneous
mixture
(d)
a
heterogeneous
mixture
(e)
a
solution
.
Which
statement
contains
only
qualitative
observations
about
a
copper
sulfate
solution?
(a)
The
solution
fills
a
250
mL
beaker,
and
the
solution
is
clear.
(b)
The
solution
has
not
evaporated
more
than
0.5
mL
overnight,
and
the
temperature
is
23°C.
(c)
The
solution
is
clear
and
is
a
pale
blue
colour.
(d)
4.6
g
of
copper
sulfate
was
added
to
249
mL
of
water
to
produce
the
solution.
(e)
The
solution
easily
conducts
about
3
V
of
electricity
between
two
probes.
8.
Which
of
the
following
chemical
groups
are
least
likely
to
react
with
other
elements?
(a)
the
halogen
gases
(b)
the
noble
gases
(c)
the
transition
metals
(d)
the
alkaline
earth
metals
(e)
the
alkali
metals
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9.
Periodic
trends
are
linked
to
(a)
the
number
of
electrons
in
an
atom
and
the
way
they
are
arranged
(b)
the
atomic
mass
of
the
atoms
(c)
the
number
of
neutrons
that
an
atom
has
(d)
the
temperature
of
the
elements
(e)
the
arrangement
of
the
protons
10.
Blake
measured
a
piece
of
steel
three
times
using
Vernier
calipers.
He
recorded
values
of
13.62
mm,
13.53
mm,
and
13.55
mm.
His
lab
partner
Ayako
measured
the
same
piece
of
steel.
She
recorded
values
of
13.45
mm,
13.33
mm,
and
13.56
mm.
Which
of
the
following
statements
are
true?
(a)
Blake’s
results
were
more
precise
than
14.
15.
16.
17.
18.
19.
20.
L
Sie
RS
e
e
e
The
measurement
4.90
m
has
three
significant
figures.
Matter
is
anything
that
has
a
weight
and
a
density.
The
three
standard
states
of
matter
that
exist
at
room
temperature
are
liquid,
solid,
and
plasma.
When
iron
rusts,
a
compound
becomes
an
ele-
ment.
This
is
a
physical
change.
Acid
rain
is
a
pure
liquid.
When
water
melts,
a
quantitative
chemical
change
occurs.
To
change
water
from
ice
to
liquid,
energy
must
be
removed
from
the
water.
o’
21.
A
gold
ring
is
an
example
of
a
heterogeneous
i
.
mixture.
(b)
Ayako’s
results
were
more
precise
_
than
Blake’s
22.
Water
is
an
example
of
an
element.
(c)
Blake’s
results
were
more
accurate
23.
When
the
atoms
of
two
elements
are
not
than
Ayako’s.
significantly
different
in
size,
the
element
(d)
Ayako’s
results
were
more
accurate
than
with
the
larger
atomic
radius
has
a
smaller
Blake’s.
electronegativity.
(e)
Blake’s
results
and
Ayako’s
results
were
equally
accurate
and
precise.
11.
Which
of
the
following
represent
polar
covalent
bonds?
(i)
Na—Cl;
(ii)
N-O;
(iii)
Hg—O;
(iv)
Ag-S
(a)
(i),
(iii),
and
(iv)
only
(b)
(i)
and
(iii)
only
(c)
(iii)
and
(iv)
only
(d)
(iii)
only
(e)
(i)
only
12.
Which
equation
most
accurately
represents
the
following
reaction:
iron
metal
+
copper(Il)
sulfate
solution
—
copper
metal
+
iron(II)
sulfate
solution
(a)
Fe(s)
+
Cu(SO4)z(aq)
—>
CU(S)
+
Fe(SO4)2(aq)
24.
25.
Nitric
oxide,
NO,
is
a
non-polar
molecule.
In
a
balanced chemical
equation,
the
number
of
particles
of
products
is
always
equal
to
the
number
of
particles
of
reactants.
Short
Answer
26.
2].
28.
Name
four
chemical
processes
that
occur
in
everyday
life.
How
many
different
types
of
atoms
would
you
expect
to
find
in
a
cylinder
of
pure
nitrogen
gas?
Using
only
a
periodic
table,
rank
the
atoms
in
each
set
in
order
of
decreasing
size.
Explain
your
ranking.
(a)
Na,
K,
H
(b)
Fe(aq)
+
Cu(SO4)(aq)
-
CU(aq)
+
FG(SO4)(aq)
(b)
Mg,
S,
Si
(e)
2Fe()
+
Cuz(SOy4)ag)
=
2Cu(s)
+
Fea(SO4)ag)
(¢
Cl
,K
’
Ar
(d)
Fe()
+
CU(SO4)(aq)
-
CU(S)
+
Fe(SO4)(aq)
_
T
o
29.
Using
only
a
periodic
table,
rank
the
elements
(e)
Fe(s)
+
CuS(aq)
—
CU.(S]
+
FBS(aq)
in
each
set
in
order
of
increasing
ionization
True/False
energy.
Explain
your
ranking.
In
your
notebook,
indicate
whether
each
statement
(a)
B,
1\{’
¥
is
true
or
false.
If
a
statement
is
false,
rewrite
it
to
(b)
¥,
CL,
Br
(e)
Na,
Cs,
K
make
it
true.
13.
Masses
of
3.9
g,
4.1
g,
and
4.0
g
were
obtained
30.
Using
only
a
periodic
table,
rank
the
elements
on
a
scale
for
a
brass
5
g
weight.
This
scale
is
in
each
set
in
order
of
increasing
electron
accurate
but
not
precise.
affinity.
Explain
your
ranking.
Unit
1
Review
*
MHR
155
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(a)
Be,
Ca,
Mg
(b)
Kr,
Se,
Br
(e)
Na,
Cs,
K
31.
Write
the
chemical
name
for
each
compound.
(a)
NH,NO;
(d)
Ba(NO);
(b)
Pb(C2H302)4
(e)
P,Oq9
(C)
SzClz
(f)
Mn203
32.
Write
the
chemical
formula
of
each
compound.
(a)
strontium
chloride
(b)
lead(II)
sulfite
(c)
chromium(III)
acetate
(d)
hydrogen
sulfide
(e)
iodine
heptafluoride
33.
Explain
why
it
is
useful
to
classify
reactions.
34.
Balance
each
chemical
equation,
if
necessary.
State
which
class
it
belongs
to.
(a)
Zn(s)
+
AgNO3(aq)
—>
ZD(N03)2(aq)
+
Ag(s)
(b)
Fe()
+
S5
=
FeSyg
(c)
KClO3)
—
2KClg)
+
302(g)
(d)
NaCOj3(aq)
+
MgSO4aq)
—
MgCO3s)
+
NazSOy(aq)
(e)
CZHBO(@
+
Oz(g)
—>
COz(g)
+
HZO(g)
35.
Predict
the
products
of
each
reaction.
Then
write
a
balanced
chemical
equation,
and
state
which
class
the
reaction
belongs
to.
(a)
Mg
+
HCl(aq)
—
(b)
HgO(S)
—
(c)
Al(s)
+
Oz(g)
—
(d)
CeH1206(s)
+
Oz
—
(e)
BaClz(aq)
+
Na3SOyaq)
—
Inquiry
36.
Describe
an
experimental
procedure
to
test
three
qualitative
properties
and
two
quantitative
properties
of
lead.
37.
Design
an
experiment
that
uses
acids
to
test
the
reactivities
of
one
metal
from
each
of
the
following
groups:
alkali
metals,
alkaline
earth
metals,
and
transition
metals.
38.
Raja
weighed
calcium
sulfate
on
filter
papers
for
an
experiment
that
he
performed
three
times.
His
data
are
shown
below.
156
MHR
-
Unit
1
Matter
and
Chemical
Bonding
ss
of
filte
Mass
of
Mass
of
paper
paper
+
powder
|
calcium
sulfate
Trial
#
1
4.13¢g
13.6
g
9.47
g
Trial
#
2
4.2¢g
12.81¢g
8.51g
Trial
#
3
4.12¢g
10.96
g
6.88
What
errors
did
Raja
make
in
his
reporting
and
calculations?
39.
What
kinds
of
tests
could
be
used
to
differenti-
ate
between
unknown
metal
and
non-metal
samples
in
a
laboratory?
Design
an
experiment
that
includes
these
tests.
40.
You
are
given
a
substance.
You
must
decide
whether
it
is
an
ionic
compound
or
a
covalent
compound.
The
substance
has
roughly
cube-
shaped
granules,
which
are
translucent
and
colourless.
(a)
Predict
whether
the
compound
is
ionic
or
covalent.
(b)
Explain
your
prediction.
(c)
Design
an
experiment
to
collect
data
that
will
support
your
prediction.
#1.
A
student
drops
a
coil
of
metal
wire,
X,
into
a
water
solution
of
a
metal
sulfate,
ZSOy(sq).
The
student
observes
that
the
colour
of
the
solution
changes,
and
that
a
metallic-looking
substance
appears
to
be
forming
on
the
metal
wire.
Based
on
these
observations,
answer
the
following
questions.
(a)
Has
a
reaction
taken
place?
If
so,
what
kind
of
reaction
has
taken
place?
Explain
your
answer.
(b)
Which
metal
is
more
reactive,
metal
X
or
metal
Z
in
compound
ZS0,?
Explain
your
answer.
(c)
Write
the
names
of
a
real
metal
and
a
metal
sulfate
that
you
predict
would
behave
this
way
in
a
laboratory.
Communication
42.
Perform
each
calculation.
Express
the
answer
to
the
correct
number
of
significant
digits.
(a)
19.3g+2.22¢g
(b)
14.2
cm
X
1.1
cm
X
3.69
cm
(c)
57.9
kg
+
3.000
dm?
(d)
18.76
g—
1.3
g
(e)
25.2
+
273°C
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43.
Name
four
groups
in
the
periodic
table.
Give
characteristics
of
each
group,
and
list
three
members
of
each
group.
44.
Copy
the
following
table
into
your
notebook,
and
fill
in
the
missing
information.
If
isotopic
data
are
not
given,
use
the
atomic
mass
from
the
periodic
table
to
find
the
number
of
neutrons.
mass
numDbe
16
18
2
2
7Li+
3
20
16
45.
Draw
a
Lewis
structure
for
each
element.
(a)
argon,
Ar
(b)
sodium,
Na
(c)
aluminum,
Al
(d)
boron,
B
46.
Draw
a
Lewis
structure
for
each
element.
Explain
the
two
patterns
that
appear.
(a)
carbon,
C
(b)
neon,
N
(c)
oxygen,
O
(d)
fluorine,
F
(e)
chlorine,
Cl
(f)
bromine,
Br
47.
Describe
three
periodic
trends.
Explain
how
these
trends
change
across
and
down
the
periodic
table.
48.
Arrange
the
following
quantities
in
a
table
to
show
which
are
physical
and
chemical
properties,
which
are
qualitative,
and
which
are
quantitative:
melting
point,
colour,
density,
reactivity
with
acids,
flammability,
malleability,
electrical
conductivity,
boiling
point,
reactivity
with
air,
hardness,
toxicity,
brittleness.
49.
Draw
a
Lewis
structure
for
each
compound.
(a)
CrBr,
(b)
H,S
(e}
CCl,
(d)
AsHj
(e)
CS,
50.
Draw
diagrams
to
represent
each
class
of
reaction
below.
Use
symbols
or
drawings
to
represent
different
kinds
of
atoms.
(a)
synthesis
(b)
decomposition
(e)
combustion
(d)
single
displacement
(e)
double
displacement
51.
Compare
the
boiling
points
of
ammonia,
NHj,
phosphorus
trihydride,
PHj,
and
arsenic
trihydride,
AsHj.
Use
the
periodic
table
and
the
concept
of
molecular
shape
and
polarity.
52.
The
molecule
BF;
contains
polar
covalent
bonds,
yet the
molecule
is
not
polar.
Explain
why.
Include
a
diagram
with your
explanation.
Making
Connections
53.
What
effects
do
accuracy,
precision,
and
margin
of
error
have
in
courts
of
law?
Consider
court
cases
that
involve
forensic
analysis.
What
are
the
implications
of
inaccurate
science
in
the
courts?
54.
Some
metals
(such
as
gold,
lead,
and
silver)
were
known
and
widely
used
in
ancient
times.
Other
metals
have
only
been
discovered
relatively
recently.
For
example,
both
sodium
and
potassium
were
discovered
in
the
early
nineteenth
century
by
Sir
Humphrey
Davy.
Explain
why
ancient
cultures
knew
about
some
metals,
while
other
metals
remained
unknown
for
thousands
of
years.
LS
~
CHALLENG
—
Consider
the
following
as
you
continue
to
plan
for
your
Chemistry
Course
Challenge:
Planet
Unknown
e
How
did
chemists
use
trends
of
physical
and
chemical
properties
to
arrange
elements
in
a
periodic
table?
e
What
are
several
ways
of
comparing
the
reactivity
of
metals?
e
How
can you
use
the
physical
and
chemical
properties
of
elements
to
help
identify
them?
Unit
1
Review
«
MHR
157
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duction to MasteringChemistry - Attempt 1
duction to Vocabulary Questions
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maple
1. Hardwoods reproduce using flowers and have broad leaves; hardwoods include trees such as
pine
cedar
elm
and pine
mango
2. Conifer leaves are generally thin and needle-like, while seeds are contained in cones. Conifers
cedar
include pine and elm
elm
3. Deciduous trees lose their leaves seasonally and include trees such as mango and maple
4. Evergreens are plants that maintain their leaves in all seasons and include trees such as elm
pine
and cedar
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Introduction to Ma.
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10
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Write the balanced chemical reaction showing the neutralization of aqueous solutions of strontium
hydroxide and sulfuric acid (H2SO4). The salt produced in this reaction is insoluble. You must use the
proper subscripts, superscripts, and states
HTML Editor
B
I E
三星x x。
Vx
T T 12pt
Paragraph
O words
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Scientists can learn a great deal about a community's drug use (both legal and illegal) by analyzing the contaminants in
wastewater. In a recent study in New York State, chemists measured the concentration of cotinine, a derivative of nicotine that i
produced in the liver and excreted in the urine of tobacco users. The chemists found the average cotinine concentrations in the
wastewater stream was 1.43 µg/L.
a
Ι
Ι
H-
b
HH
H
H-C
C-N:
C=0:
TH
HH
Jonutis/Shutterstock
Revell, Introductory Chemistry, 2e, © 2021
W. H. Freeman and Company
Cotinine is slightly soluble in water. Using the structure of cotinine, identify any polar covalent bonds that are present in
this substance.
C-O
C-C
C-H
C-N
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Students react zinc with hydrochloric
acid to produce zinc chloride and
hydrogen gas in a test tube. They
weighed the reactants, the flask, and the
balloon that captured the hydrogen gas.
The zinc was added to the acid and the
balloon attached across the mouth of
the flask. The table shows the data each
group collected.
Zinc
Zinc &
Chloride
Hydrochloric &
|Group acid
Hydrogen
gas
155.67 g
155.65 g
2
157.80 g
157.78 g
3
148.22 g
146.54 g
4
155.93 g
155.92 g
169.42 g
169.43 g
Explain how the data supports the Law
of Conservation of Mass is followed.
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Give 5 examples of any organic compound which changes in the same way as sugar and benzoic acid when heated.
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-1
A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 9.0 g·L
The geochemist also
measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 5.3 g·L *.
Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated
lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated.
Be sure your answer has the correct number of significant digits.
x10
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F1
!
What kind of symbols are used to represent the reactants and products?
Q
O
A
element symbols from the periodic table
multiplying scale
F2
letters of their name
the alphabet
2
W
S
F3
-0+
#
3
E
F4
D
$
णी व
4
F5
R
%
5
F
F6
T
F7
< 6
G
Y
F8
&
7
P
H
F9
U
00 X
8
F10
J
N
a
9
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[References]
Copper metal can be prepared by roasting copper ore, which can contain cuprite (Cu₂ S) and copper(II) sulfide.
Cu₂ S (s) + O2(g) → 2 Cu(s) + SO2(g)
CuS(s) + O₂(g) → Cu(s) + SO2(g)
Suppose an ore sample contains 12.0% impurity in addition to a mixture of CuS and Cu₂ S. Heating 100.0 g of the mixture produces 75.7 g of copper metal with a
purity of 88.2%. What is the weight percent of CuS in the ore? The weight percent of Cu₂S?
Weight percent of CuS =
2
Weight percent of Cu₂S:
Submit Answer
=
%
%
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Once you have completed your chemistry experiments, either by producing products or
leaving reagents behind, you must put these substances into the appropriate chemical
waste container. The list of items below includes those that will be used in your labs and
are thus considered "waste." From this list, select the correct location to deposit each
substance once it has been deemed Waste: (match the number on the right with the
waste on the left, there will be one number that is not used in the matching)
Bromoacetone(1)
1. Inorganic acids and salts
2. Inorganic bases
>
NaCl(aq)
HCl(aq)
Acetone(1)
Cu(s)
NaOH(aq)
3. Solid waste
4. Organics
5. Halogenated Organics
6. Pour down the sink
7. Garbage pail
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Fill in the Blanks
Chemical
Price/kg (in dollars)
NaOH
21.17
CaCl2
41.28
КОН
31.38
CUSO4
93.32
NH4NO3
59.64
NH4CI
25.04
NaCl
21.15
NaNO3
72.35
Type your answers in all of the blanks and submit
Another requirement is that the cost of the salt needs to be evaluated to determine if it is economical to use. To do this, you should
consider the price per degree of dropping the temperature of the solution. The table of prices per kg for each salt is shown above.
Let's determine the cost for the NaOH solid as an example. We want to determine how much it costs to change the temperature by
1 deg C so we start with the cost given in the table and end with $/deg C.
For NaOH:
21.17
$/
1
kg)
X (
1
kg/
1000
X (
Type your answer here
g/ Type your answer here
deg C)
Please type your answer to submit
Please type your answer to submit
Type your answer here
$/deg C
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The organic lab program generates around 200 liters of non-halogenated organic waste every week. A student accidentally added some halogenated organic waste to a waste container that entered the non-halogenated waste stream.
The cost to dispose of 1.000 liter of non-halogenated organic waste is $20.27
The cost to dispose of 1.000 liter of halogenated organic waste is $89.71
Due to the error, how much extra money will it cost to dispose of 210.9 liters of the waste that week?
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Please answer question 5 part A
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When Kay added 30g of Hydrochloric acid (HCI) to 65g of Zn, bubbles appeared and a white precipitate, zinc chloride (ZnCl2) was produced. She found that the mass of the zinc chloride was 93g. Since the law of conservation of matter stated that matter can’t be created or destroyed, she was puzzled about the difference in mass. What is the best explanation for the missing 2g?
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Using the table provided, what is the enthalpy for the reaction shown below:
6H₂(g) + 4NO(g) + CH₂(g) → CO₂(g) + 2H₂O(l) + 4NH3 (9)
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Related Questions
- duction to MasteringChemistry - Attempt 1 duction to Vocabulary Questions Reset Help maple 1. Hardwoods reproduce using flowers and have broad leaves; hardwoods include trees such as pine cedar elm and pine mango 2. Conifer leaves are generally thin and needle-like, while seeds are contained in cones. Conifers cedar include pine and elm elm 3. Deciduous trees lose their leaves seasonally and include trees such as mango and maple 4. Evergreens are plants that maintain their leaves in all seasons and include trees such as elm pine and cedar Submit Previous Answers Request Answer Introduction to Ma. fa トト」 トI fo fo ins prt sc 8% 8 9 10arrow_forwardWrite the balanced chemical reaction showing the neutralization of aqueous solutions of strontium hydroxide and sulfuric acid (H2SO4). The salt produced in this reaction is insoluble. You must use the proper subscripts, superscripts, and states HTML Editor B I E 三星x x。 Vx T T 12pt Paragraph O wordsarrow_forwardScientists can learn a great deal about a community's drug use (both legal and illegal) by analyzing the contaminants in wastewater. In a recent study in New York State, chemists measured the concentration of cotinine, a derivative of nicotine that i produced in the liver and excreted in the urine of tobacco users. The chemists found the average cotinine concentrations in the wastewater stream was 1.43 µg/L. a Ι Ι H- b HH H H-C C-N: C=0: TH HH Jonutis/Shutterstock Revell, Introductory Chemistry, 2e, © 2021 W. H. Freeman and Company Cotinine is slightly soluble in water. Using the structure of cotinine, identify any polar covalent bonds that are present in this substance. C-O C-C C-H C-Narrow_forward
- Students react zinc with hydrochloric acid to produce zinc chloride and hydrogen gas in a test tube. They weighed the reactants, the flask, and the balloon that captured the hydrogen gas. The zinc was added to the acid and the balloon attached across the mouth of the flask. The table shows the data each group collected. Zinc Zinc & Chloride Hydrochloric & |Group acid Hydrogen gas 155.67 g 155.65 g 2 157.80 g 157.78 g 3 148.22 g 146.54 g 4 155.93 g 155.92 g 169.42 g 169.43 g Explain how the data supports the Law of Conservation of Mass is followed.arrow_forwardGive 5 examples of any organic compound which changes in the same way as sugar and benzoic acid when heated.arrow_forward-1 A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 9.0 g·L The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 5.3 g·L *. Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Be sure your answer has the correct number of significant digits. x10arrow_forward
- F1 ! What kind of symbols are used to represent the reactants and products? Q O A element symbols from the periodic table multiplying scale F2 letters of their name the alphabet 2 W S F3 -0+ # 3 E F4 D $ णी व 4 F5 R % 5 F F6 T F7 < 6 G Y F8 & 7 P H F9 U 00 X 8 F10 J N a 9arrow_forward[References] Copper metal can be prepared by roasting copper ore, which can contain cuprite (Cu₂ S) and copper(II) sulfide. Cu₂ S (s) + O2(g) → 2 Cu(s) + SO2(g) CuS(s) + O₂(g) → Cu(s) + SO2(g) Suppose an ore sample contains 12.0% impurity in addition to a mixture of CuS and Cu₂ S. Heating 100.0 g of the mixture produces 75.7 g of copper metal with a purity of 88.2%. What is the weight percent of CuS in the ore? The weight percent of Cu₂S? Weight percent of CuS = 2 Weight percent of Cu₂S: Submit Answer = % % Try Another Version 9 item attempts remaining Cengage Learning Cengage Technical Support Previous Next Save and Exitarrow_forwardOnce you have completed your chemistry experiments, either by producing products or leaving reagents behind, you must put these substances into the appropriate chemical waste container. The list of items below includes those that will be used in your labs and are thus considered "waste." From this list, select the correct location to deposit each substance once it has been deemed Waste: (match the number on the right with the waste on the left, there will be one number that is not used in the matching) Bromoacetone(1) 1. Inorganic acids and salts 2. Inorganic bases > NaCl(aq) HCl(aq) Acetone(1) Cu(s) NaOH(aq) 3. Solid waste 4. Organics 5. Halogenated Organics 6. Pour down the sink 7. Garbage pailarrow_forward
- Fill in the Blanks Chemical Price/kg (in dollars) NaOH 21.17 CaCl2 41.28 КОН 31.38 CUSO4 93.32 NH4NO3 59.64 NH4CI 25.04 NaCl 21.15 NaNO3 72.35 Type your answers in all of the blanks and submit Another requirement is that the cost of the salt needs to be evaluated to determine if it is economical to use. To do this, you should consider the price per degree of dropping the temperature of the solution. The table of prices per kg for each salt is shown above. Let's determine the cost for the NaOH solid as an example. We want to determine how much it costs to change the temperature by 1 deg C so we start with the cost given in the table and end with $/deg C. For NaOH: 21.17 $/ 1 kg) X ( 1 kg/ 1000 X ( Type your answer here g/ Type your answer here deg C) Please type your answer to submit Please type your answer to submit Type your answer here $/deg Carrow_forwardThe organic lab program generates around 200 liters of non-halogenated organic waste every week. A student accidentally added some halogenated organic waste to a waste container that entered the non-halogenated waste stream. The cost to dispose of 1.000 liter of non-halogenated organic waste is $20.27 The cost to dispose of 1.000 liter of halogenated organic waste is $89.71 Due to the error, how much extra money will it cost to dispose of 210.9 liters of the waste that week?arrow_forwardPlease answer question 5 part Aarrow_forward
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