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Page 61
Science 10/Kennedy/2016
1
Introduction
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Millions of different chemical compounds exist as a result of different
combination of elements. A systematic way of naming these
compounds has been developed by the International Union of Pure
and Applied Chemistry (IUPAC).
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International
International
Union
Union
ofof
Pure
Pure
and
and
Applied
Applied
Chemistry
Chemistry
IUPAC
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3
Introduction
Page 61
Millions of different chemical compounds exist as a result of different
combination of elements. A systematic way of naming these
compounds has been developed by the International Union of Pure
and Applied Chemistry (IUPAC).
Compounds contain more than one kind of element chemically
bonded together.
• Alloys: metal-metal
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Alloys
Alloys are combinations of metals: e.g., steel
Alloys have properties such as higher melting point, hardness.
Gold is a very soft metal; too soft to use as jewelry in its pure form. It
is combined with copper and silver to make it harder.
The purity of gold is given in units of karats:
Pure gold
24 k
25% copper
18 k
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Introduction
Page 61
Millions of different chemical compounds exist as a result of different
combination of elements. A systematic way of naming these
compounds has been developed by the International Union of Pure
and Applied Chemistry (IUPAC).
Compounds contain more than one kind of element chemically
bonded together.
• Alloys: metal-metal
• Ionic: metal-nonmetal
• Molecular: nonmetal-nonmetal
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Atoms are bonded together using valence electrons.
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Compounds form when two or more atoms bond together.
Bonds occur when valence electrons between two atoms form
a pair. Electrons can form a pair by
• transferring Ionic compounds
• sharing
Molecular compounds
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3.1 Binary Ionic Compounds
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 Notes:
Ionic compounds combine a metal with a
nonmetal. Binary ionic compounds contain one
type of metal ion and one type of non-metal
ion.
Properties:
metal-nonmetal
empirical
Solids at SATP
Conduct electricity if dissolves in water
Theoretical:
A metal atom losses an electron to a nonmetal atom.
Thus positive and negative ion are produced. This
forms a network of ions where the overall charge is
balanced.
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Theoretical:
A metal atom losses an electron to a nonmetal atom. Thus positive and
negative ion are produced. This forms a network of ions where the overall
charge is balanced.
+
_
+
_
+
_
+
_
+
_
+
_
+
_
+
All the ions are interconnected with each other
Single units of ionic compounds do not exist by themselves
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Nomenclature
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Nomenclature
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An analogy between words and compounds:
The elements of the periodic table are like letters of the
alphabet. The elements are put together to form compounds
like letters are put together to form words.
There are scientific rules for putting elements together just as
there are spelling rules for putting letters together.
There are rules for how compounds may react just as there
are grammatical rules for how words interact
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Nomenclature
 Notes:
Cation name/space/anion name
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e.g.,
sodium chloride
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Cation name/space/anion name
2.
Name the following binary ionic substances.
IUPAC Name
Formula
a.
sodium chloride
NaCl
b.
magnesium chloride
MgCl2
c.
strontium bromide
SrBr2
p. 63 #1, 2
Do
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Ionic substances
All the atoms are interconnected with each other
+
_
+
_
+
_
+
_
+
_
+
_
+
_
+
2:1 Ratio
1:1 Ratio
e.g., NaCl
Na2Cl2
Always use the lowest
possible numbers
Na4Cl4
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Ca2+
Cl-
CaCl2
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Ca2+
+
Cl-
CaCl2
Cl-
Two to one ratio for neutral compound
Needed to balance charge
3. Determine the formula for each of the following binary ionic
substances.
Name
Formula
a.
sodium bromide
b.
sodium oxide
c.
potassium nitride
f.
magnesium phosphide
Na+
Na+ Na+
BrO2-
NaBr
Na2O
K+ K+ K+
N3-
K3N
P3-
Mg3P2
Mg2+
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Superscripts are different than subscripts
Superscripts – the
charge on each ion
Mg2+ +
3P
Mg3P2
Subscripts – how
many ions are in the
compound
p. 63 #3
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Multivalent Ions
 Notes:
metals
Multivalent ions: Some atoms have the
possibility of forming more than one
type of ion charge. This will affect the
properties and therefore the name of
the substance.
Only positive ions
Fe2+
Iron(II)
Fe3+
Iron(III)
Metal name(roman numeral)
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The total charge must = zero
4. Determine the formula for each of the following binary ionic
substances.
Name
Formula
FeBr2
a.
iron(II) bromide Fe2+
Br-
b.
iron(III) bromide Fe3+
Br-
h.
gold(I) oxide
i.
gold(III) oxide Au3+ Au3+ O2- O2- O2-
Au+
Au+
BrBr-
Br-
O2-
FeBr3
Au2O
Au2O3
p. 63 #4
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Stock Nomenclature for multivalent ions
Metal name(roman numeral) nonmetal name
Space
No space
5. Determine the name for each of the following binary ionic substances.
Formula
c.
d.
Name
niobium(III) oxide
niobium(V) oxide
Nb2O3
Nb2O5
First consider negative charge on nonmetal ion
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Stock Nomenclature for Multivalent Ions
Some elements may form differently charged ions.
This will affect their formula and properties.
• Consider negative charge on nonmetal ion
• Determine the total negative charge
• The total positive charge is equal to the total negative charge
• Determine the charge on each positive ion
p. 63 #5
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Classical Nomenclature
Latin: Ferric and Ferrous
Fe3+
Fe2+
Latin: cupric and cuprous
Cu2+
Cu+
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 Notes:
Polyatomic ions
Groups of atoms may form an ion and
form ionic bonds with other ions.
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sulfate
SO42-
ammonium
NH4+
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Memorize Common Polyatomic Ions
hydroxide
OH-
sulfate
SO42-
acetate
CH3COO-
nitrate
NO3-
phosphate
PO43-
ammonium
NH4+
No Quiz
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Metal name(roman numeral) nonmetal name
6. Determine the name for each of the following polyatomic substances.
Name
Formula
a.
sodium carbonate
Na2CO3
b.
sodium nitrite
NaNO2
g.
aluminium hydroxide
Al(OH)3
i.
iron(III) sulfate
Fe2(SO4)3
p. 64 #6
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7. Determine the formula for each of the following polyatomic
substances.
Name
Formula
a.
sodium cyanide
c.
calcium hydroxide
e.
iron(II) carbonate
f.
iron(III) carbonate
h.
aluminium persulfide
NaCN
Ca(OH)2
FeCO3
Fe2(CO3)3
Al2(S2)3
There are many
more polyatomic
ions than what
are in our chart
e.g., persulfide
S22-
p. 64 #7
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Solubility
aqueous
Solubility is if a substance dissolves in water
 Notes:
dissolves
A substance may be highly soluble or
low soluble when placed into water
Does not dissolve
(or very little)
ionic
NaCl(s)
molecular
C12H22O11(s)
Dissociates when it
dissolves
Separates into ions
Does not dissociates
when it dissolves
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Soluble – dissolves in water
aqueous
Breaks apart into ions as it dissolves
dissociates
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Ionic substances
All the ions are interconnected
with each other
+
_
_
+
_
+
+
_
+
_
+
_
+
_
+
Molecular substances
The atoms join to form molecules
that are not connected with other
molecules
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Ionic substances
+
-
+
-
-
+
-
+
+
-
+
-
Salt
Dissociate – individual ions areScience
formed
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Molecular substances
Sugar
31
Ionic substances
Molecular substances
Both dissolve
Salt solution
-
Sugar solution
-
+
+
-
+
+
+
-
+
Dissociate – individual ions are
formed
Science
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Compounds that include group I ions or NH4+ are generally soluble
Using Solubility Table
Only works for ionic substances
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aq
s
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Use solubility table
Page 64
8. Use your solubility table to determine the solubility for each of the
following.
Formula
Solubility (s or aq)
a.
Na2CO3
c
FeSO4
aq
aq
f.
Al(OH)3
s
aq
s
Not all substances are in the solubility table
p. 64 #8
Compounds that include group I ions are always soluble
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Use solubility table
Page 65
10. Use your solubility table to determine the solubility for each of the
following.
Name
Solubility (s or aq)
a. sodium carbonate
b. ammonium carbonate
f.
Sodium hypochlorite
aq
aq
aq
p. 64 #8, 9
Do
p. 65 #10 - 13
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Ionic Nomenclature Quiz: Provide the name
or formula for the following. (1 mark each)
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Ionic Nomenclature Quiz: Provide the name or formula for the
following. (1 mark each) 0.5 marks off for each minor mistake
Name
Formula
1.
magnesium bromide
MgBr2
2.
nickel(II) hydroxide
Ni(OH)2
3.
sodium carbonate
4.
gold(III) borate
Na2CO3
Au2(B03)3
5.
ZnCl2
6.
zinc chloride
ammonium sulfate
7.
iron(III) hydroxide
Fe(OH)3
8.
vanadium(IV) dichromate
V(Cr2O7)2
Use your solubility
table to determine
the solubility for each
of the following.
Name
9.
Lithium carbonate
10.
10
(NH4)2SO4
calcium hydroxide
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Solubility (s or aq)
aq
s
37
3.2 Molecular Compounds
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 Notes:
Molecular compounds are combinations
of nonmetals
Properties: Empricial
• They may be solid, liquid, or gas
• They do not conduct electricity if they
dissolve in water
Theoretical:
• Nonmetals may combine by sharing
electrons
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Ionic substances
All the ions are interconnected with
each other
+
_
_
+
_
+
+
_
+
_
+
_
+
_
+
Molecular substances
The atoms join to form molecules
that are not connected with other
molecules
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Molecular Compounds
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Atoms join to form individual molecules that are not connected with
other molecules
O
H
H
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Ionic Substances
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All the atoms are interconnected with each other
Molecular Substances
The atoms join to form molecules that are not connected with other
molecules
H
O
H
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H
H
O
HC
H
O
C
H
H
C
H
H
O
H
H
O
C
H
C
C
O
O
H
H
C
H
C
O
H
O
H
H
H
C
C
O
O
C
H
C
H
OH
H
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Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
42
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Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
43
Nomenclature
Ionic Compounds
• Metal, nonmetal
• Balance charges
Molecular Compounds
Page 66
• Nonmetal, nonmetal
• Use prefix system
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3.2 Molecular Compounds
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 Notes:
Molecular compounds are combinations
of nonmetals
• Molecular elements contain only one type of
atom:
• Monoatomic atoms can exist on their own
e.g., Ar, Ni, Cr
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Ozone
O3(g)
Sulfur
S8(s)
Phosphorus
P4(s)
Diatomic elements:
O2(g)
H2(g)
Cl2(g)
Br2(l)
I2(g)
F2(g)
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Some elements tend to come together as groups.
Ozone
Sulfur
Phosphorus
O3(g)
S8(s)
P4(s)
Diatomic elements
O2(g) H2(g) Cl2(g)
Br2(l) I2(g)
F2(g)
N2(g)
Memorize
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Compounds at Home
Common Name
Chemical Name
Use
muriatic acid
hydrochloric acid
Cleaning cement
nail polish remover acetone
Nail polish remover
Wood alcohol
methanol
Paint solvent, gas line antifreeze,
lantern fuel
lighter fluid
butane
lighters
propane
propane
BBQ fuel
hydrogen peroxide
Hydrogen peroxide
H2O2
•
•
•
Baking soda
Sodium bicarbonate Cleaning, baking, putting out
fires, absorbing odours
vinegar
Acetic acid
disinfectant for wounds (3 %)
Hair bleach (6 %)
Rocket fuel (> 70 %)
Cooking, cleaning
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Memorized Compounds
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Memorized Compounds
Water
H2O(l) or HOH(l)
Hydrogen peroxide
H2O2(l)
Methane (natural gas)
CH4(g)
Propane
C3H8(g)
Ethanol
C2H5OH(l) or CH3CH2OH(l)
Methanol
CH3OH(l)
Ammonia
NH3(g)
Hydrogen sulfide
H2S(g)
Sucrose
C12H22O11(s)
Glucose
C6H12O6(s)
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Compound Quiz: Provide the name or symbol
for the following elements. (1 mark each)
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Compound Quiz: Provide the name or symbol for the following compounds.
(1 mark each)
CH4(g)
Methane
C12H22O11(s)
Sucrose
NH3(g)
Ammonia
O3(g)
Ozone
CH3OH(l)
Methanol
Propane
C3H8(g)
Ethanol
C2H5OH(l)
HOH
water
Glucose
C6H12O6(s)
H2O2(l)
Hydrogen peroxide
or
CH3CH2OH(l)
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3.2 Molecular Compounds
Page 66
 Notes:
Molecular compounds are combinations
of nonmetals
Nomenclature:
• The number of atoms present must be
indicated using a prefix
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Nomenclature:
The number of atoms in a molecule must be indicated using a
prefix:
1 – mono
2 – di
3 – tri
4 – tetra
5 – penta
6 – hexa
7 – hepta
8 – octa
9 – nona
10 – deca
The first element is usually the one more to the left on the periodic
table.
The second element gets an “ide” ending to its name
The prefix “mono” only gets used on the second atom
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If there are two vowels in a row that sound the same
once the prefix is added (they "conflict"), the extra
vowel on the end of the prefix is removed.
3. Name each compound.
IUPAC Name
Formula
c.
dinitrogen monoxide
d. diphosophorus pentoxide
N2 O
P2O5
Double vowels
that sound the
same - drop the
first one
The “a” is dropped
2. Provide the formula for each molecular compound
Name
formula
a. nitrogen dioxide
NO2
b. dinitrogen dioxide
N2O2
p. 67 #1 - 3
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3.3 Acids & Bases
 Notes:
Acids
Properties (empirical)
• Turns blue litmus paper red
• Acids are s, l or g as pure compounds at
SATP but act as an acid only when dissolved
in water
• Conducts electricity as an aqueous solution
• Sour tasting
Theoretically, acids release a hydrogen H+
ion while in solution
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3.3 Acids & Bases
 Notes:
Bases
Empirically
• Tastes bitter
• Feels slippery
• Turns red litmus paper blue
• Conducts electricity as an aqueous solution
Theoretically
Bases release a hydroxide ion (OH-) while in solution
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3.3 Acids & Bases
The strength of an acid or base is measured on the pH scale. pH
means power of the hydrogen
H+
OH-
Neutral
Basic (alkaline)
Acidic
0
1
2
3
4
5
6
7
8
9
10
11
12
13
14
pH may be measured using a pH meter or dyes that change colour
such as as indicators of pH paper
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Acid Nomenclature:
There are three ways of determining the name of an acid:
i.
Memorization
ii. IUPAC System
iii. Classical System
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i. Memorize Common Acids:
HCl(aq)
H2SO4(aq)
HNO3(aq)
HF(aq)
H3PO4(aq)
Hydrogen ion
combined with a
non-metal
CH3COOH(aq)
HCl(g)

Organic acids contain carbon and a
COOH
HCl(aq)
Acids will always be aqueous
p. 70 #1, 2
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ii. IUPAC System for Acids
Give ionic name
Place “aqueous” in front
3. Name the hydrogen compound using the ionic system and then
modify the name using the IUPAC system for acids.
a.
Ionic Name
IUPAC Acid name
Formula
hydrogen nitrite
aqueous hydrogen nitrite
HNO2
p. 70 #3
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iii. Classical Acid Nomenclature
Name the hydrogen compound using the ionic system and then modify the
name as shown in the chart below.
Rule
Ionic Name
Acid Name
1.
hydrogen ________ ide
hydro ______ ic acid
2.
hydrogen ________ ite
______ ous acid
3.
hydrogen ________ ate
______ ic acid
Acid names containing
• sulfur must add “ur” to the acid name.
• phosphorus must add “or” to the acid name.
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Rule
Ionic Name
Acid Name
1.
hydrogen ________ ide
hydro ______ ic acid
2.
hydrogen ________ ite
______ ous acid
3.
hydrogen ________ ate
______ ic acid
Acid names containing
• sulfur must add “ur” to the acid name.
• phosphorus must add “or” to the acid name.
4. Complete the chart.
Ionic Name
hydrogen thiosulfate
b. hydrogen sulfide
c. hydrogen chlorate
a.
Classical Acid Name
Formula
thiosulfuric acid
hydrosulfuric acid
H2S2O3(aq)
chloric acid
HClO3
H2S(aq)
p. 71 #4
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The strength of an acid or base is measured using the pH scale
pH = power of the hydrogen
H+
acidic
0
1
2
3
OHbasic
neutral
4
5
6
7
8
9
10
11
12
13
14
pH may be measured using:
• a pH meter
• dyes that change colour such as indicators or pH paper
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Nomenclature Quiz: Provide the name or formula for the
following. (1 mark each)
Name
Formula
1.
diphosophorus pentoxide
P2O5
2.
nickel(II) hydroxide
Ni(OH)2
3.
glucose
4.
5.
gold(III) tetraborate
dinitrogen heptaoxide
C6H12O6
Au2(B4O7)3
N2O7
6.
sulfurous acid
H2SO3(aq)
aqueous hydrogen sulfite
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65
Nomenclature Quiz: Provide the name or formula for the
following. (1 mark each)
Name
Formula
1.
triphosophorus heptoxide
P3O7
2.
nickel(II) nitrite
Ni(NO2)2
3.
sucrose
4.
5.
gold(III) thiosulfate
dinitrogen heptachloride
C12H22O11
Au2(S2O3)3
N2Cl7
6.
sulfurous acid
H2SO3(aq)
6
aqueous hydrogen sulfite
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Empirical Classification of Compounds
ionic
molecular
s, l, or g at SATP
Solids at SATP
Conducts electricity when
dissolved in water
Do not conduct electricity when
dissolved in water
p. 71 #5, 6
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Water
Hydrogen peroxide
Methane (natural gas)
Propane
Ethanol
Methanol
Ammonia
Hydrogen sulfide
Sucrose
Glucose
Hydrochloric acid
Sulfuric acid
Acetic acid
Nitric acid
Phosphoric acid
Ozone
Sulfur
Phosphorus
Diatomic elements
H2O(l) or HOH(l)
H2O2(l)
CH4(g)
C3H8(g)
C2H5OH(l) or CH3CH2OH(l)
CH3OH(l)
NH3(g)
H2S(g)
C12H22O11(s)
C6H12O6(s)
HCl(aq)
H2SO4(aq)
CH3COOH(aq)
HNO3(aq)
H3PO4(aq)
O3(g)
S8(s)
P4(s)
O2(g) H2(g) Cl2(g) Br2(l) I2(g)
N2 (g)
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F2(g)
69
4 Chemical Change
Page 77
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70
Introduction
Page 77
Chemistry is the study of change. The change may be physical or
chemical.
 Notes:
4.1 Chemical Reactions
Chemical reactions may be defined
theoretically or empirically:
Theoretical:
A chemical reaction occurs when atoms
rearrange themselves into new molecules
Particles must collide with a minimum
speed/energy and orientation.
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KMT
Kinetic molecular theory
Particles are in
constant and random
motion
71
4.1 Chemical Reactions
Page 77
Chemical reactions are changes that may be defined theoretically
or empirically:
Reactants
Chemicals
you start with
Products
Chemicals you
end up with
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Physics
Phun
Useful Reactions
Laundry detergent:
The oxygen in hydrogen peroxide and sodium hypochlorite
takes the colour away from stains
Baking:
The yeast produces carbon dioxide to make the bread rise
Swimming pool:
Chlorine in the water kills bacteria and micro-organisms
Swimming pool:
Chlorine in the water kills bacteria and micro-organisms
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4.1 Chemical Reactions
Page 77
 Notes:
Empirical:
reaction
Evidence of a chemical change:
• colour change
• odor change
• gas produced
• state change
• energy change (the substance changes
temperature)
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Exothermic: heat is
given off
(surrounding temp
increases)
Endothermic: heat
is absorbed
(surrounding temp
decreases)
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Chemical changes always involve energy changes
An energy change may show up as a temperature change or
light given off.
Exothermic: heat is given off (surrounding temp goes up)
Endothermic: heat is absorbed (surrounding temp goes down)
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 Notes:
Mass is conserved in all chemical reactions
Theoretical
A chemical reaction occurs when atoms
rearrange themselves into new molecules.
Particles must collide with a minimum
speed/energy and orientation to react.
KMT
A reaction is written as follows:
Reactants
Products
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Chemical Reactions
Page 77
Reactants
Chemicals
you start with
Reactant 1 + Reactant 2
Products
Chemicals you
end up with
Product 1 +
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Product 2
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Methane and oxygen react to form water and carbon dioxide
CH4
+
O2
H
H C H
H
+
O O
---->
H 2O
H
O
+
H
CO2
+
O C O
2H
1C
3O
4H
1C
2O
The number of atoms on each side do not add up!!!???
They must add up!!
Science 10/Kennedy/2016
78
Page 75
CH4
+
O2
10 g of reactants
---->
H 2O
+
CO2
10 g of products
Mass is conserved
Science 10/Kennedy/2016
79
Page 78
Law of Conservation of Mass
For mass to be conserved the number of atoms in the reactants must
be the same as the number of each type of atoms in the products
The number of atoms don’t add properly. It must be balanced.
CH4
H
H C H
H
+
+
2 O2
O O
---->
2 H2 O
H
O O
H
O
O
H
+
+
CO2
O C O
H
Science 10/Kennedy/2016
80
One water molecule
H
O
H2O
H
Two hydrogen atoms
One oxygen atom
Two water molecules
H
O
H
H
O
H
2H2O
Four hydrogen atoms
Two oxygen atoms
Coefficient
subscript
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81
Page 78
Law of Conservation of Mass
It must be balanced.
CH4
+
2 O2
---->
2 H2 O
+
CO2
One molecule of methane reacts with 2 molecules of oxygen to
produce 2 molecules of water and 1 molecule of carbon dioxide
Science 10/Kennedy/2016
82
Page 75
Balancing Chemical Equations
•
Make a list of each element on each side of the reaction
•
Count how many of each element is present before and
after
•
Use coefficients to balance the reaction
• Only use coefficients to balance the reaction
• Don’t change the subscripts when balancing a
reaction
• Keep polyatomic ions together
Science 10/Kennedy/2016
83
Page 78
Balancing chemical equations
Only use coefficients to balance – don’t change the subscripts!
Science 10/Kennedy/2016
84
Page 79
•
Balancing chemical equations
Write the correct formulae for the products and the reactants
• Use coefficients to ensure you have the same amount of
each type of atom on both sides of the equation
9. Balance the following equations using whole number coefficients.
2 Mg
+
2
O2
1 Mg
2O
---->
2 MgO
2 1 Mg
1O
List and
count atoms
Only use coefficients to balance – don’t change the subscripts!
Science 10/Kennedy/2016
85
Page 38
Products
Reactants
Only use coefficients to balance – don’t change the subscripts!
Science 10/Kennedy/2016
86
Balancing Chemical Equations
•
Make a list of each element on each side of the reaction
•
Count how many of each element is present before and
after
•
Use coefficients to balance the reaction
• Only use coefficients to balance the reaction
• Don’t change the subscripts when balancing a reaction
• Keep polyatomic ions together
Science 10/Kennedy/2016
87
•
Write the correct formulae for the products and the reactants
• Use coefficients to ensure you have the same amount of
each type of atom on both sides of the equation
Page 79
4.
Balance the following chemical reaction using the lowest possible
whole number coefficients.
Mercury(II) oxide decomposes to produce mercury and oxygen gas.
2 HgO
2 Hg +
O2
Only use coefficients to balance – don’t change the subscripts!
Science 10/Kennedy/2016
88
One carbon dioxide molecule
CO2
One carbon atom
Two oxygen atoms
Three carbon dioxide molecules
Coefficient
3CO2
Three carbon atom
Six oxygen atoms
subscript
Science 10/Kennedy/2016
p. 78 #1 - 3
Do
89
Page 79
8.
Balance the following chemical reaction using the lowest possible
whole number coefficients.
Reactants
3 Li +
AlCl3
Products
Al
+
3 LiCl
Only use coefficients to balance – don’t change the subscripts!
Science 10/Kennedy/2016
90
Page 78
3. Identify the reaction below that is properly balanced.
a.
b.
c.
d.
N2
N2
2N2
N2
+
+
+
+
H2
H2
6H2
3H2
⟶
⟶
⟶
⟶
NH3
2NH3
4NH3
2NH3
The lowest possible whole number coefficients must be used.
Science 10/Kennedy/2016
91
Balancing Chemical Equations
•
Make a list of each element on each side of the reaction
•
Count how many of each element is present before and
after
•
Use coefficients to balance the reaction
• Only use coefficients to balance the reaction
• Don’t change the subscripts when balancing a reaction
• Keep polyatomic ions together
p. 79 #1 - 11
Science 10/Kennedy/2016
Do
92
Page 80
14.
The following reactions contain polyatomic ions. Balance the following
equations using the lowest possible whole number coefficients.
Keep the polyatomic ions together
2 NaOH +
H2SO4
2 HOH
H 2O +
1
2
Na
2
Na
1
2
OH
2
1
OH
2
H
2
1
H
1
SO4
1
SO4
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Na2SO4
93
Page 80
Same question as a multiple choice
NaOH
+
H2SO4
H 2O +
Na2SO4
The coefficients for the balanced chemical equation are:
a.
b.
c.
d.
2, 0, 2, 0
1, 2, 1, 2
2, 1, 2, 2
2, 1, 2, 1
p. 80 #12 – 17
Science 10/Kennedy/2016
Do
94
Remember!!
Water
Hydrogen peroxide
Methane (natural gas)
Propane
Ethanol
Methanol
Ammonia
Hydrogen sulfide
Sucrose
Glucose
Hydrochloric acid
Sulfuric acid
Acetic acid
Nitric acid
Phosphoric acid
Ozone
Sulfur
Phosphorus
Diatomic elements
H2O(l) or HOH(l)
H2O2(l)
CH4(g)
C3H8(g)
C2H5OH(l) or CH3CH2OH(l)
CH3OH(l)
NH3(g)
H2S(g)
C12H22O11(s)
C6H12O6(s)
HCl(aq)
H2SO4(aq)
CH3COOH(aq)
HNO3(aq)
H3PO4(aq)
O3(g)
S8(s)
P4(s)
O2(g) H2(g) Cl2(g) Br2(l) I2(g)
Science 10/Kennedy/2016
N2 (g)
F2(g)
95
Page 66
Remember!!
Ozone
Sulfur
Phosphorus
Diatomic elements
O3(g)
S8(s)
P4(s)
O2(g) H2(g) Cl2(g)
F2(g) N2 (g)
Science 10/Kennedy/2016
Br2(l) I2(g)
96
Page 81
A chemical reaction may be expressed using words rather than symbols. Write
the balanced chemical equation, including states of matter, for each of the
following:
21. Sodium metal reacts with water to produce hydrogen gas and sodium
hydroxide.
2 Na(s) + 2 HOH(l)
H2(g) + 2 NaOH(aq)
1 Na
1
Na
2
1
H
2
2
H
2
1
OH
2
1
OH
Science 10/Kennedy/2016
97
Same question as a numeric response
Page 81
21. Sodium metal reacts with water to produce hydrogen gas and sodium
hydroxide.
2 Na(s) + 2 HOH(l)
H2(g) + 2 NaOH(aq)
The coefficients for the balanced chemical reaction, in order from left
to right are _____, ______, ______, and _______,
2 21 2
p. 81 #18 – 26
Do
Science 10/Kennedy/2016
0
0
0
0
1
1
1
1
2
2
2
2
3
3
3
3
4
4
4
4
5
5
5
5
6
6
6
6
7
7
7
7
8
8
8
8
9
9
9
9
98
Balancing Quiz
Balance the following reactions. (2 marks each)
1.
8 HgS
2.
2 NaF
3.
8 Hg +
+
Ba(OH)2
S8
6
2 NaOH
+
BaF2
Aluminium reacts with sodium hydroxide to produce
sodium metal and aluminium hydroxide
Al + 3 NaOH
3 Na
+ Al(OH)3
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99
4.2 The Mole Concept
Page 82
Dealing with individual atoms is not typically
practical in chemical reactions. A larger amount
called the mole is used. The number of particles
called Avogadro’s number is equal to one mole:
 Notes:
1 mole = 6.02 x 1023 particles
Science 10/Kennedy/2016
100
Amount
Science 10/Kennedy/2016
101
The amount of a substance can be expressed in numerous ways:
couple
2
few
3
dozen
12
score
20
ream
500
mole
6.02 x 1023
A mole is an amount:
Science 10/Kennedy/2016
102
Page 82
1 mole = 6.02 x 1023 particles
atoms
molecules
ions
Science 10/Kennedy/2016
103
Page 82
1 mole = 6.02 x 1023
Is a very large number!
Dealing with individual atoms is not typically practical in
chemical reactions.
Science 10/Kennedy/2016
104
6.02 x 1023
Avogadro’s number
1 mol of watermelon Seeds: Would fit inside a hollow sphere
the size of the moon
1 mol of Timbits: Would cover the Earth and be 8 km deep
1 mol of dimes: Would make at least 7 stacks that would
reach the moon
1 mol of grains of sand: Would be more than all of the sand
on Miami Beach
Science 10/Kennedy/2016
105
4.2 The Mole Concept Page 82
Dealing with individual atoms is not typically
practical in chemical reactions. A larger amount
called the mole is used. The number of particles
called Avogadro’s number is equal to one mole:
 Notes:
1 mole = 6.02 x 1023 particles
A mole is defined as the number of atoms in 12
g of carbon.
Science 10/Kennedy/2016
106
Page 82
The Mole
A mole is defined as the number of atoms in 12 g of carbon.
Unit
mole
Symbol
mol
Science 10/Kennedy/2016
107
Page 83
4.
One mole of carbon has a mass of 12 g but one mole of sulfur
is measured as 36 g. The mass of one sulfur atom must be
______
times larger than the mass of one carbon atom
3
36 g sulfur
12 g carbon
=
3
Sulfur atoms are 3 times heavier than carbon atoms.
Science 10/Kennedy/2016
108
Page 84
The amount of a substance in a balanced chemical reaction may
be communicated as moles.
7.
Note the balanced chemical equation below. Four mol of FeCl3
6 mol of BaCl2.
will produce _____
2FeCl3 +
3BaBr2
2FeBr3 +
3BaCl2
Two moles of iron(III) chloride react with 3 moles of barium
bromide to produce 2 moles of iron(III) bromide plus 3 moles
of barium chloride
p. 83 #1 – 7
Science 10/Kennedy/2016
Do
109
Molar Mass (pg 95)
• To calculate the molar mass of the
substance.
1. Determine the chemical formula (if
necessary)
2. Count the number of each atom.
3. Look up molar mass of each atom
and multiply by number of atoms
4. Add
Science 10/Kennedy/2016
110
Mass to moles and Moles to
Mass (pg 95)
• Determine the conversion
• Identify the conversion factor
• Set up conversion line and set up
conversion to cancel units
Ex) 5.00g of sodium in moles ?
_5.00g__1 mol____0.217 mol
22.99g
Science 10/Kennedy/2016
p. 95 #1 – 3
Do
111
4.3 Reaction Types
Page 85
Chemical reactions can be classified according to
type. Knowledge of reaction type may make it
possible to predict the products of a chemical
reaction.
 Notes:
Reaction types:
•
•
•
•
•
Formation
Decomposition
Single Replacement
Double replacement
Combustion
•
Other (any reaction that does not match the
above types)
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112
Page 85
Formation:
element +
element
Decomposition:
compound ---->
---->
compound
element + element
Single replacement:
element + compound
----> compound + element
Double replacement:
compound + compound
----> compound
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+
compound
113
Page 85
Formation:
element +
element
Decomposition:
compound ---->
---->
element
compound
+
element
p. 86 #1 – 12
Science 10/Kennedy/2016
Do
114
Predicting Reactions requires:
• Ionic Nomenclature
• Solubility
• Multivalent charges
• Polyatomic ions
• Molecular Nomenclature
• Acid/base Nomenclature
• Memorized compounds
• Balancing Reactions
Science 10/Kennedy/2016
115
Page 87
Predictions of Formation & Decomposition Reactions
• Predict the missing substances
• Identify the reaction as either formation (f) or decomposition (d)
• Balance using whole number coefficients
Formation:
element + element
Decomposition:
compound ---->
---->
element
Science 10/Kennedy/2016
compound
+
element
116
Page 87
Predicting Reactions:
Formation:
element + element
Decomposition:
compound ---->
13.
2 Mg(s)
+
---->
compound
element + element
O2(g)

2 MgO(s)
p. 87 #13 – 20
Science 10/Kennedy/2016
Do
117
Page 85
Single replacement:
element + compound
----> compound
+
element
Double replacement:
compound + compound
----> compound
+
compound
Page 88
23. NaOH(aq) +
dr
HCl(aq)
HOH(l) +
NaCl(aq)
May also be called a neutralization reaction
Neutralization reaction: Acid plus base
Science 10/Kennedy/2016
118
Single replacement:
element + compound ----> compound
Double replacement:
compound + compound
+
element
----> compound
+
compound
Page 88
25. Aqueous iron(II) hydroxide reacts with aqueous aluminium chloride to
produce a solution of aluminium hydroxide and iron(II) chloride.
3 Fe(OH)2(aq)
+ 2 AlCl3(aq)
2 Al(OH)3(s)
Need to check solubility table
Science 10/Kennedy/2016
+ 3 FeCl2(aq)
p. 88 #21 – 27
Do
119
Page 89
Predictions of Single & Double Replacement Reactions
• Predict the missing substances
• Identify the reaction as either single replacement (sr) or double
replacement (dr)
• Balance using whole number coefficients
Single replacement:
element + compound ----> compound + element
29. Br2(aq) + 2 NaI(aq)
Science 10/Kennedy/2016
2NaBr(aq) +
l2(s)
120
Page 89
Predictions of Single & Double Replacement Reactions
• Predict the missing substances
• Identify the reaction as either single replacement (sr) or double
replacement (dr)
• Balance using whole number coefficients
Page 89
32 Iron reacts with copper(II) chloride (use the most common ion
charge for iron).
2 Fe(s)
+ 3 CuCl2(aq)
3 Cu(s)
+ 2 FeCl3(aq)
p. 89 #28 – 34
Science 10/Kennedy/2016
Do
121
Page 90
Combustion (oxidation):
burns
rusts
tarnish
compound + oxygen
Add oxygen
----> most common oxides
Science 10/Kennedy/2016
122
Page 90
Combustion (oxidation):
Science 10/Kennedy/2016
123
Page 90
Combustion (oxidation):
burns
rusts
tarnish
Science 10/Kennedy/2016
124
Page 90
Fossil Fuel Combustion
The combustion of fossil fuels is exothermic producing carbon
dioxide and water
Usually the combustion is incomplete resulting in carbon
monoxide – very poisonous
Science 10/Kennedy/2016
125
Page 90
41. Liquid pentane (C5H12) reacts with oxygen gas in the air to
undergo complete combustion to produce carbon dioxide and
water vapour.
C5H12(l)
+
8 O2(g)
5 CO2(g)
+ 6 H2O(g)
42. Liquid pentane (C5H12) reacts with oxygen gas in the air to
undergo incomplete combustion to produce carbon monoxide
and water vapour.
2 C5H12(l)
+ 11 O2(g)
10 CO(g)
+ 12 H2O(g)
p. 90 #35 – 42
Science 10/Kennedy/2016
Do
126
Page 91
Burns, tarnish
Rusts, oxidation, explodes
Add oxygen
Predictions of Combustion Reactions
• Predict the missing substances
• Balance using whole number coefficients
compound + oxygen
----> most common oxides
H
N
C
S
H2O(g)
NO2(g)
CO2(g)
SO2(g)
Metals form their metal oxides
p. 91 #43 – 47
Science 10/Kennedy/2016
Do
127
Page 94
Chemical Tests
Evidence
Hydrogen
Explode (pop)
Burning splint
Carbon dioxide
Burning splint
Lime water
Ca(OH)2 + CO2  CaCO3(s)
Extinguishes fire
Precipitate (cloudy)
Oxygen
Splint catches fire
Glowing splint
Water
Cobalt(II) chloride paper
Blue paper turns pink
Acidity
Acid: Blue turns red
pH paper
Science 10/Kennedy/2016
Base: Red turns blue128
Writing Chemical Equations
Predict the missing chemicals based on reaction type
• Know the most common oxides
• Know your memorized substances
Use coefficients to balance the reaction:
• Only use coefficients to balance the reaction
• Don’t change the subscripts when balancing a reaction
• Keep polyatomic ions together
• Check solubility of products
• Balance oxygen last in combustion reactions
p. 92 #48 - 69
Science 10/Kennedy/2016
Do
129
Balancing Quiz
Balance the following equations.
8 HgS
Cl2 + 2 Na
8 Hg +
S8
2 marks
2NaCl
2 marks
8
Barium reacts with aluminium hydroxide to produce
aluminium metal and barium hydroxide
4 marks
3 Ba + 2 Al(OH)3
2 Al
Science 10/Kennedy/2016
+
3 Ba(OH)2
130
The End
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131