Download Additional Review

Science 10
Unit A:
A1.1
Unit A: Energy and Matter in Chemical Change
Energy and Matter in Chemical Change
Introduction
Read pages: 6-11
WHMIS
o Workplace Hazardous Materials Information System
o There are three components to the WHMIS system:
 ___________________________________________________________________
 ___________________________________________________________________
 ___________________________________________________________________
WHMIS Symbols:
1
Science 10
A1.2
Unit A: Energy and Matter in Chemical Change
Properties and classification of matter
Read pages: 12-17
Physical Properties
Describe the physical appearance and composition of a substance:
They include:
Chemical Properties
Describe how a substance will react chemically with another substance.
They include:
Pure Substance
Are only made up of one type of particle, all particles are identical.
Elements
____________________________________________________________________________
Are listed on the periodic table.
Eg. _________________________________________________________
Compounds
____________________________________________________________________________
Eg.
CO2 – carbon dioxide
___________________________
_______________________________
2
Science 10
Unit A: Energy and Matter in Chemical Change
Mixtures
_______________________________________________________________________________________
_______________________________________________________________________________________
Solution
Is uniform throughout, cannot see the different particles.
Eg. ____________________________________________________________________
Mechanical Mixture
You can see the different particles.
Eg. ____________________________________________________________________
Suspension
Is a mixture when the particles have different states.
Eg. ____________________________________________________________________
Colloid
Is like a suspension but it is not easy to separate the parts.
Eg. ____________________________________________________________________
3
Science 10
Unit A: Energy and Matter in Chemical Change
Chemical Reactions
The following are signs that a chemical reaction has occurred:
1.
2.
3.
4.
5.
Assignment:
Check and Reflect Page 17: Questions 1 - 9
4
Science 10
Unit A: Energy and Matter in Chemical Change
Student Worksheet: Classification of Matter
5
Science 10
A1.3
Unit A: Energy and Matter in Chemical Change
6
Atomic Models
Read pages: 18-25
Aristotle [400 BC – 1500 AD]
Thought that all matter is made up of only four
elements:
o ___________________________________________________
o all of matter is some combination of these four elements
Alchemy [1500 AD]
In the 1500’s many scientists were________________________________________________
________________________________________________________________________________________
While they were not able to create
gold they did discover many useful
properties of matter such as:
o density
o boiling point
o melting point
o separation techniques
Dalton [1766-1844]
Developed the _____________________________________________________________
o All matter is made up of tiny particles called atoms.
o The atom is the smallest particle of matter and cannot be divided.
o The atoms of an element are all identical in size and mass.
o Atoms of different elements have
different properties.
o Different atoms combine together in
specific ratios to form new
substances.
Eg
H2O
Science 10
Unit A: Energy and Matter in Chemical Change
7
JJ Thomson [1890s]
Developed the
____________________________________________
o Studied the properties of cathode rays.
o Discovered the electron.
o Within the atom there exists tiny negative
particles called electrons, the rest of the
atom is a positive fluid sphere.
Ernest Rutherford [1908]
Rutherford did the gold foil
scattering experiment.
_________________________________________________
o The atom has a small
positive, dense nucleus.
o Most of the matter is found in
the nucleus.
o The negative electrons orbit
the nucleus like planets orbit
the sun.
Neils Bohr
Bohr studied the bright lines in the visible spectrum of hydrogen.
Bohr created a theory where ___________________________________________________
__________________________________________________________
o Electrons can occupy only specific orbits.
o Each orbital can only hold a certain number of electrons.
o For an electron to occupy an orbital it must has a specific amount of
energy (energy level).
Quantum Mechanical
In today’s model of the atom ___________________________________________________
___________________________________
o We have the greatest probability of locating electrons in certain
regions around the atom.
o Depending on how many electrons an atom has and which energy
level the electron is in then that electron can be found in a certain
cloud formation.
o The electron can exist as a particle and as a wave at the same time.
Check and Reflect: 4 – 8
A1.R
Section 1 Review
page 25
page 27
Science 10
A2.1
Unit A: Energy and Matter in Chemical Change
Atomic Structure
Read pages 28-38
Elements
Are made up of only one type of atom.
Metals
Properties include:
Non-metals
Properties include:
Metalloids
Properties include:
8
Science 10
Unit A: Energy and Matter in Chemical Change
9
The Period Table
All of the elements have been organized onto the periodic table of elements.
The elements are organized into rows and columns _____________________________
_________________________________________________________________________________________
Groups
Elements are placed into _________________________________________.
Elements in the same group/family have the same physical and chemical
properties.
i. ____________________________________
- Group IA
- Very reactive metals
- Li, Na, K, Rb, Cs, Fr
ii. _____________________________________
- Group IIA
- Reactive metals
- Be, Mg, Ca, Sr, Ba, Ra
iii. _____________________________________
- Group VIIA
- Very reactive non-metals
- F, Cl, Br, I, At
iv. _____________________________________
- Group VIIIA
- These elements are non-reactive
- They do not form ions or compounds
- He, Ne, Ar, Kr, Xe, Rn
Periods
Elements are placed into rows.
Elements in the same row all have the same number of orbits and energy
levels.
Eg. Li, Be, B, C, N, O, F, Ne
Science 10
Unit A: Energy and Matter in Chemical Change
10
Subatomic Particles
The atom is made up of three types of subatomic particles:
Particle
Proton
Neutron
electron
Symbol
Charge
Mass
1.67 x 10-27 kg
1.67 x 10-27 kg
9.11 x 10-31 kg
Location
atomic mass number
atomic number
52.00
24
Cr
Atomic Mass Number
____________________________________________________________.
Is the mass of 1 mole of atoms.
Atomic Number
____________________________________________________________.
The number of electrons is equal to the number of protons in one
atom.
Example:
Chromium
Protons:
Electrons:
Neutrons:
___________
___________
____________________
Ru
_______________
_______________
_______________________
Science 10
Unit A: Energy and Matter in Chemical Change
11
Formation of Ions
Atoms of the same element will always have the same number of protons.
When an atom _________________________________________ it will become an ion.
Metals
Will form _________________________________
They _____________________________________ electrons from the outer orbit
Non-metals
Will form _____________________________
They _______________________________ to gain extra electrons
Science 10
Unit A: Energy and Matter in Chemical Change
12
Octet Rule
o Atoms strive to have _______________________ in their outermost orbit.
o Atoms will give away or steal electrons until it has a complete and
stable outer orbital.
o The number of electrons in the outer orbital is called ___________________
_________________________________
o The number of electrons an atom will gain or lose to reach a stable
orbit is called the _______________________________.
o Example:
o Sodium
 Valance electrons: _________
 valance number: ___________________________
 ion: _______________
o Chlorine
 Valance electrons: _________
 Valance number: ___________________________
 Ion: _________________
Lewis Dot Structures
o A Lewis diagram is a model where the valance electrons are drawn as
dots around the atom.
o This model shows ___________________________________________________________
________________________________________________________________________________
o Examples:
o
Science 10
Unit A: Energy and Matter in Chemical Change
13
How Ions Form Compounds
o When atoms combine to form an ionic compound the _______________________
_____________________________________________________________________________________
o One ion will become positive and the other ion will become negative.
o Each atom ends up with a
complete outer orbit with 8
electrons each.
Examples:
1.
Complete the following for each atom
Atom
Atomic
Number
1st orbit
2nd orbit
3rd orbit
Valance #
Ion
Na
N
Cl
2.
For each of the following draw the Lewis dot structure and write the
atom as an ion:
a.
Li
b.
S
Check and Reflect: 1 – 12
page 39
Science 10
A2.2
Unit A: Energy and Matter in Chemical Change
14
Naming Ionic and Molecular Compounds
Read pages: 40-49
Ionic Compounds
o An ionic compound is formed when ___________________________________________
_____________________________________________________________________________________
o An ionic compound is formed because the metal ion becomes positive and
the non-metal ion becomes negative so they _________________________________
____________________________.
Ionic Compound Formulas
o For two atoms to form an ionic compound there must be __________________
_____________________________ between the negative ions and the positive ions.
1. Write the correct formula for the ionic compound.
a.
Li   F  
b.
Ca 2  Cl  
c.
K   O2 
d.
Al 3  S 2 
Science 10
Unit A: Energy and Matter in Chemical Change
Naming Ionic Compounds
o {metal} {non-metal} + “ide”
o Example:
o Sodium + chlorine  ______________________________
2.
Name each compound above in #1.
3.
Write the formula given the name
a. lithium oxide
b. strontium chloride
Assignment: Worksheet A2.2: Ionic Compounds Worksheet #1
- simple ionic compounds
Multivalent Elements
o Some metals have the ability to form __________________________________________
________________________________.
o These elements are usually the transitional-earth metals.
o Examples:
o Iron (II): Fe2+, iron (III): Fe3+
o Copper (I): Cu+, Copper (II): Cu2+
4. Write the equation for each of the following
a. Iron (III) oxide
b. Copper (II) bromide
5. Given the formula write the correct chemical name:
a. CrO
b. Co2S3
15
Science 10
Unit A: Energy and Matter in Chemical Change
16
Polyatomic Ions
o A polyatomic ion is made up of ______________________________________.
o Polyatomic ions can combine in ______________________________.
o Suffixes
 “ite” has fewer atoms of an atom
 “ate” has more atoms of an element
 Sulfite: ___________
 Sulfate: ___________
o Compounds containing polyatomic ions follow the same balancing rules as all
other ionic compounds.
o Naming polyatomic compounds:
 {metal} + {polyatomic ion}
 the name of the polyatomic ion does not change (it has been married
once already)
Example:
 Calcium carbonate
1.
Write the correct chemical formula for the following:
a. sodium sulfite
b. magnesium nitrate
c. ammonium sulfide
Assignment: Ionic Compounds Worksheet #2
Science 10
Unit A: Energy and Matter in Chemical Change
17
Molecular Compounds
o A molecular compound is created when _________________________________________
__________________________________.
o When non-metal atoms form molecules they must ______________________________,
they form _________________________________. By sharing electrons the outer orbits
still have _______________________________.
o
Science 10
Unit A: Energy and Matter in Chemical Change
18
o Because non-metals atoms ______________________________ the same two elements
they ________________________________________
(we cannot predict the ratio in a molecular compound)
o To name molecular compounds we use a prefix system for naming.
o Examples:
a. SO,
______________________________
b. SO2, ______________________________
c. SO3, ____________________________________________________________
d. SO4, ____________________________________________________________
e. P3O5, ____________________________________________________________
o A number of molecular compounds have common names:
Name
Formula
H2O(l)
CO2(g)
C6H12O6(s)
C12H22O11(s)
CH4(g)
NH3(g)
H2O2(l)
C3H8(g)
Molecular elements
o Many of the non-metal elements exist in molecular form:
Element
Formula
Hydrogen
Nitrogen
Oxygen
Fluorine
Chloride
Bromine
Iodine
Phosphorus
Sulfur
Ozone
Assignment: Molecular Compounds Worksheet #2
Check and Reflect: 1 – 11
page 50
Science 10
A2.3
Unit A: Energy and Matter in Chemical Change
19
Properties of Ionic and Molecular Compounds
Read pages 51-60
Properties of ionic compounds
o
o
o
o
o
o
o
o
o an ionic compound is also referred to as “a salt”
Solubility of Ionic Compounds
o some ionic compounds are more soluble than others
o a substance that dissolves well is considered very soluble
o an ionic compound that is soluble in a solution is written as ___________________,
a an ionic compound that is not soluble will be written as ______________________
Solubility Table
Ion
Very
Soluble
Group
1
NH4+
H3O+
(H+)
All
Slightly None
Soluble
ClO3- CH3COONO3ClO4-
ClBrI-
SO42-
S2-
OH-
PO43SO32CO32-
All
Most
Most
Most
Only
with:
Group
1
Group
2
NH4+
Only
with:
Group
1
NH4+
None Only
with:
Ag+
Hg+
Only
with:
Ag+
Pb2+
Hg+
Cu+
Tl+
Only
with:
Ca2+
Sr2+
Ba2+
Ra2+
Pb2+
Ag+
Most
Only
with:
Group
1
NH4+
Sr2+
Ba2+
Tl+
Most
Most
Science 10
Unit A: Energy and Matter in Chemical Change
20
Examples:
1. Which of the following compounds will most likely dissolve in water?
a. NaNH4
b. LiCl
c. CaS
d. KOH
e. AgCl
f. CaSO4
g. Cu(OH)2
Properties of Molecular Compounds
o Molecular compounds are compounds made up of ___________________________
_____________________________________________
o The non-metal atoms are held together by ________________________________, the
atoms share electrons which make a _____________________________________.
o The attraction between neighboring molecules is weak so ___________________
__________________________________________
o Molecular compounds can also make crystalline structures that crumble
easily.
o Molecular compounds _______________________________________________ because they
are made up of non-metal atoms.
Special Properties of Water
o ______________________________________, one side is slightly positive and the other
side is slightly negative.
o The molecules form an electrostatic attraction to each other.
o Water has the following properties:
 _________________________, water molecules are attracted to other water
molecules
 _________________________, water molecules are attracted to other
molecules
 _________________________________, because of cohesion water makes a
strong surface force
 _________________________________, water can crawl up a straw or edge of a
container because of adhesion
 Conducts heat
 __________________________________
 Specific heat capacity
Science 10
Unit A: Energy and Matter in Chemical Change
21
Phases of Water (Ice)
o Ice (solid) is less dense than the liquid form of water because of the
molecular formation of water, ordered molecular structure
o _________________________________________________________________________________
__________________________________________
o Water (lakes) freezes from the top down.
Assignment: Check and Reflect: 1 – 9
Page 61
Science 10
A2.4
Unit A: Energy and Matter in Chemical Change
22
Acids and Bases
Read pages 62-68
Properties of Acids
o
o
o
o
o
o
Properties of Bases
o
o
o
o
o
o
ph Scale
o pH is an indication of the ________________________________________ in a solution
o the higher the concentration of H+ ions the stronger the acid, the higher the
pH
 acids:
_________________
 neutral
_________________
 bases:
_________________
Science 10
Unit A: Energy and Matter in Chemical Change
23
Indicators
o an acid-base indicator is a chemical that is used to determine if a solution is
________________________________________
o an indicator ________________________________________________________________________
o different indicators will change colour for different pH ranges:
o universal indicator is a mixture of several indicators that change colour as
the pH changes to different ranges
Naming Acids
o acids are named based on the non-metal anion in the compound
Anion
“ide”
“ite”
“ate”
Compound name
Hydrogen (anion)-ide
Hydrogen (anion)-ite
Hydrogen (anion)-ate
Acid name
Hydro (anion)-ic acid
(anion)-ic acid
(anion)-ous acid
Examples:
Formula
HS(aq)
H2SO3(aq)
H2SO4(aq)
Compound
Common Acid name
Hydrogen sulfide
Hydrogen sulfite
Hydrogen sulfate
IUPAC naming system for acids:
[International Union of Pure and Applied Chemistry]
Formula
HS(aq)
H2SO3(aq)
H2SO4(aq)
Compound
IUPAC name
Hydrogen sulfide
Hydrogen sulfite
Hydrogen sulfate
1. Name the following acids:
a. H3N(aq)
b. HNO2(aq)
c. HNO3(aq)
d. H3PO4(aq)
Assignment: Worksheet – A2.4 Naming acids
Science 10
Unit A: Energy and Matter in Chemical Change
24
Bases
o Most bases contain an __________________________________
o Bases _____________________________________ because they react with oils and
grease
o Some common bases:
Base
NaOH(aq)
NH4OH(aq)
Mg(OH)2(aq)
Name
Common name
Sodium hydroxide
Ammonium hydroxide
Magnesium hydroxide
Use
Acids and Bases in Your Body
o Our bodies contain a variety of substances each substance has a specific pH:
 Saliva – 6.4
 Blood – 7.35
 Stomach – (1-2)
 Small intestine – 8.5
 Large intestine – (5.5-7.0)
 Urine – 6.4
o It is important that our bodies maintain this pH balance
o ______________________________, is a substance that helps to maintain a pH level in
a solution, it resists change in pH
Acids and Bases in the Home
o acids and bases serve a variety of functions in our homes
o some typical acids are:
o _________________________________________________________________________
o some typical bases are:
o _________________________________________________________________________
Science 10
Unit A: Energy and Matter in Chemical Change
Neutralization
o a type of chemical reaction where ______________________________________________
_____________________________________________________is called a neutralization
o the products of a neutralization reaction are always:
_____________+_______________--> ____________________+______________________
HClaq  NaOH aq  H 2Ol  NaClaq
o carbon dioxide is produced only when one of the compounds contain the
carbonate molecule
o eg vinegar + baking soda
Assignment: Check & Reflect
25
Science 10
A2.5
Unit A: Energy and Matter in Chemical Change
26
Our Chemical Society
Read pages: 70-75
Issues Related to Chemicals
o some chemicals are hazardous because of:
 ____________________________________________________________
 how they are produced
 ________________________________________________________________________________
 their effect on the ecosystem
Environmental Effects
o some chemicals are harmful because of how they effect components within
the environment
o some harmful chemicals ____________________________________________________________
____________________________________________
o CFC’s chlorofluorocarbons
 come from Freon used in __________________________________________________
 can stay in the atmosphere for up to 50 years
 _________________________________________, the ozone helps to protect the
Earth from harmful UV, and X-Rays from the sun
o Greenhouse gases (________________________)
 most of the greenhouse gases come from the _____________________________
______________________________
 levels of greenhouse gases in our atmosphere are increasing
 the greenhouse gases are trapping in heat and the temperatures
around the Earth are increasing
o Acid Precipitation
 other products of the combustion of fossil fuels are ____________________
________________________________________________________
 particulates enter the Earth’s atmosphere and return in the form of
_____________________________________________
 ______________________________________________________________________________
_________________________________
Science 10
Unit A: Energy and Matter in Chemical Change
27
Health Concerns
o Many people use chemical substances for recreational purposes
o Some of these chemicals are ____________________________________________
o Some of these chemicals _____________________________________
o Alcohol (CH3CH2OH(l))
 alcohol is considered a drug because of its effects on the body
 excessive amounts can
 __________________________________________________
 ______________________________________________________________________
 repeated use can lead to physical and psychological dependence,
______________________________________________
o Nicotine and tobacco products
 __________________________________________________________________________
 The use of tobacco products have been related to high incidences of
cancer
Benzene
o Benzene is a hazardous chemical that is both toxic and flammable
o Many products are made using benzene
 ________________________________________________________________
o Benzene is a regulated chemical so there are strict regulations about its
transportation and storage
o Because of its toxic effects any ____________________________________________________
is hazardous
 Workers must take specific steps for protection, WHMIS
Chemistry Related Careers
o Because we use so many different chemicals there are many careers that
involve chemistry:
 Chemical engineers
 Chemistry teachers
 ___________________________________________
 ___________________________________________________________
 Cosmetics
 Household product design
o Almost each person works or interacts with chemicals everyday
 Food and cooking
 _____________________________________________
 Gas and transportation
 _____________________________________________
 Manufactured products
A2.R Section 2 Review
AQ.2
Quiz 2
pages 76-77
Science 10
A3.1
Unit A: Energy and Matter in Chemical Change
Examples of Chemical Change
Read pages: 79-85
During a chemical reaction a ___________________________________________________________
_____________________________________________________________
Example:
Methane + oxygen  water + carbon dioxide + (energy)
____________________
_______________________________
Showing States in a Chemical Formula
o In some chemical reactions the products may be in the form of a
_______________ or in the form of a ____________________________
o The symbol (aq) means that in solution the compound will
________________________________________.
o In any chemical equation it is important that you show the state of each
element or compound in the reaction
o Examples
CH 4(g)  O2(g)  H 2O(g)  CO2(g)  energy
CaC2(s)  H 2O(l )  Ca OH 2(s)  C2 H 2(g)
Which compounds are gases?
Which compounds are solid?
Which compounds are liquid?
Which of these was an element?
28
Science 10
Unit A: Energy and Matter in Chemical Change
29
Energy Changes
o ____________________________________________________________________________________
_________________________________________.
Phase Change
o When a substance changes state there is a characteristic change in
energy that occurs.
o In a pure substance the phase changes
(_____________________________________________________________)
o In a mixture there are a variety of phase changes.
Exothermic Reaction
o Release energy usually in the form of __________________________________
o The energy of the products is ____________________ than the energy of the
reactants. (______________________________________________________________)
o Example:
CH 4(g)  O2(g)  H 2O(g)  CO2(g)  energy
Endothermic Reaction
o
Energy is absorbed from the surrounding environment, usually
__________________________________________________________________
o The energy of the products is________________________ than the energy of
the reactants. (___________________________________________________)
o Example:
Ba OH 2(s)  NH 4 SCN  Ba SCN 2(aq)  NH 4OH(aq)
Biochemical Reactions
o Two important biochemical reactions are:
o Cellular Respiration
 This is how living organisms (cells) get energy from glucose.
 Is an __________________________________________.
o Photosynthesis
 This is how plants get energy from the sun.
 Is an ___________________________________________.
Science 10
Unit A: Energy and Matter in Chemical Change
30
Evidence of a Chemical Reaction
o In all chemical reactions a new substance is produced that has its own
characteristic properties.
o Indicators of a chemical change:
Conservation of Mass
o Mass is conserved in all chemical reactions.
o In all chemical reactions ______________________________________________________ the
mass of the reactants.
o Example:
o
2AgNO3(aq)  Cu(s)  Cu NO3 2(aq)  2Ag(s )
(33.98g)
Assignment
(6.36g)
(______________)
Check and Reflect: 1 – 11
(21.57g)
P. 85
Science 10
A3.2
Unit A: Energy and Matter in Chemical Change
31
Writing Chemical Equations
Read pages: 86-89
Chemical Equations
o a word equation describes the reactants and products of a chemical reaction
____________________________
o a chemical equation _______________________________________________________________
to identify the reactants and products in a chemical reaction
o a chemical equation is more useful because:
o _____________________________________________________________________________
o _____________________________________________________________
Example:
Word equation
Silver nitrate + copper  copper nitrate + silver
Chemical equation
Practice:
Write the following as a chemical equation:
1.
potassium + oxygen  potassium oxide
2.
scandium + nitrite  scandium nitrite
3.
sulfur + oxygen  sulfate
Worksheet:
A3.2
Writing chemical equations
Science 10
Unit A: Energy and Matter in Chemical Change
32
Balancing Chemical Equations
o in all chemical reactions mass is conserved so we ______________________________
_____________________________________ for each element in the reactants and in the
products
o it is important that we balance any chemical equation that we write
Examples:
Balance each of the following chemical equations
a.
Na(s) +
b.
H2(g) +
O2(g) 
c.
N2(g) +
H2(g) 
d.
Na(s) +
H2O(l) 
NaOH(aq) +
e.
CH4(g) +
O2(g) 
H2O(g) +
f. Pb(s) +
NaCl(s)
H2O(l)
NH3(g)
H3PO4(aq)  H2(g) +
g. AgNO3(aq) +
Worksheet
Cl2(g) 
H2(g)
CO2(g)
Pb3(PO4)2(s)
CuSO4(aq)  Ag2SO4(s) +
Cu(NO3)2(aq)
A 3.2 Balancing Chemical Equations
Check & reflect
6–9
p. 90
Science 10
A3.3
Unit A: Energy and Matter in Chemical Change
33
Five Common Chemical Reactions
Read pages: 91-105
There are five common types of Chemical Reactions:
I. Formation Reaction (Synthesis)
o During a formation reaction two or more elements __________________________
_____________________________________________________
o A formation reaction is also referred to as a __________________________________.
o Many formation reactions are ____________________________, that is heat is
given off during the reaction.
A + B  AB
Example:
magnesium + oxygen  magnesium oxide
Practice:
Complete the reaction by writing the product, write the chemical equation, then
balance.
1.
aluminum + chlorine 
2.
carbon + hydrogen  methane
Text: Practice problems:
Skill Practice:
2, 3, 4
1, 2, 3
p. 92, 93
p. 93
Science 10
II.
Unit A: Energy and Matter in Chemical Change
34
Decomposition
o During a decomposition reaction __________________________________________
into its component elements.
o Many decomposition reactions are ____________________________, that means
that energy must be added to the reaction to break apart the existing
chemical bonds.
AB  A + B
Example:
Water + energy (electricity)  hydrogen + oxygen
Practice:
1.
calcium oxide 
2.
aluminum sulfide 
Text
Practice problems: 5
p. 94
Science 10
III.
Unit A: Energy and Matter in Chemical Change
Hydrocarbon Combustion
o During a combustion reaction a __________________________________________
_______________________________________________________________________________
_________________________________________________
o Combustion reactions are _________________________________.
o The potential energy of the reactants is higher than the energy of the
products so during the reaction heat energy was released.
Example
Methane + oxygen  carbon dioxide + water + (energy)
Practice:
1. propane C3H8(g) + oxygen 
2. glucose + oxygen 
Text:
Practice Problem:
6
p. 95
35
Science 10
Unit A: Energy and Matter in Chemical Change
36
Solubility of Ionic Compounds
o some ionic compounds are more soluble than others
o a ionic compound that ___________________________________________________________
_____________________________________________________________________________________
o an ionic compound that is soluble in a solution is written as __________________,
a an ionic compound that is not soluble will be written as _____________________,
it will form a ____________________________
Solubility Table
Ion
Very
Soluble
Slightly
Soluble
Group 1
NH4+
H 3O +
(H+)
All
ClO3NO3ClO4-
CH3COO-
ClBrI-
SO42-
S2-
OH-
PO43SO32CO32-
All
Most
Most
Most
Only
with:
Group 1
Group 2
NH4+
Only
with:
Group 1
NH4+
None
None
Only
with:
Ag+
Hg+
Only
with:
Ag+
Pb2+
Hg+
Cu+
Tl+
Only
with:
Ca2+
Sr2+
Ba2+
Ra2+
Pb2+
Ag+
Most
Only
with:
Group 1
NH4+
Sr2+
Ba2+
Tl+
Most
Most
Examples:
Which of the following compounds are very soluble and which are
slightly soluble?
a. NaNH4
b. LiCl
c. CaS
d. KOH
e. AgCl
f. CaSO4
g. Cu(OH)2
Science 10
IV.
Unit A: Energy and Matter in Chemical Change
37
Single Replacement
o During a single replacement reaction an ionic compound reacts with
another element, the chemical bond in the compound breaks apart and
then ______________________________________________
_______________________________________________________________
o The other two ions will have a ____________________________________ (bond) this
is why they combine to form a different compound.
A + BC  B + AC
D + BC  C + BD
Example:
Sodium chloride + silver  silver chloride + sodium
Practice:
Complete the word equation and predict the products.
Write the appropriate chemical equation, indicate if a precipitate is formed.
Balance the equation.
1.
Lithium sulfate + calcium 
2.
Chlorine + copper I bromide 
Text:
Skill practice: 1 – 4
p. 97
Science 10
V.
Unit A: Energy and Matter in Chemical Change
38
Double Replacement
o During a double replacement reaction two ionic compounds in a solution
will combine and then _________________________________________________________
___________________________________________________________________________________
o One pair of ions will have a _______________________________________ (bond) this
is why a different compound is formed.
o Quite often a _________________________________________ as a result of a double
replacement reaction.
AB(aq) + CD(aq)  AD(s) + CB(aq)
Example:
sodium chloride + silver nitrate  sodium nitrate + silver chloride
Practice:
Complete the word equation and predict the products.
Write the appropriate chemical equation, indicate if a precipitate is formed.
Balance the equation.
1.
Text:
Assignment:
Potassium iodide + silver nitrate 
Practice problem:
9, 10, 11, 12 p. 100 – 105
Worksheet A 3.3 Reaction Types
Check and Reflect: 1 – 8
p. 106
Science 10
A3.4
Unit A: Energy and Matter in Chemical Change
The Mole
39
Read pages: 107-111
Avogadro’s Number
o The quantity that chemists use to measure _______________________________________
is present in a sample is called the _______________________________
o The number of atoms or particles in one mole is Avogadro’s Number
o 1 mole = ____________________________________
Atomic Mass
o the atomic mass of an element is the mass of 1 mole of atoms of that element
that is the mass of 6.02 x 1023 atoms.
o For example:
o 6.02 x 1023 atoms of Carbon weigh: __________________
o 6.02 x 1023 atoms of Oxygen weigh: __________________
Where did the atomic masses of all of the elements come from?
o By looking at how atoms combine to form compounds scientists were able to
find the atomic masses of all of the elements as they were _____________________
__________________________________________________.
o Today’s periodic table is based on _____________________________________________
o After finding the atomic numbers and the atomic masses ____________________
then created the _______________________________________.
Finding the Atomic Mass of a Compound
o The atomic mass of 1 mole of a compound will be the sum of the atomic
masses of each of the elements in the compound.
o ________________________________________________________________________________________
o Example:
what is the atomic mass of one mole of
a.
H2O(l): 2 H + 1 O = 2(1.01) + 1 (16.00) = 18.02 g/mol
b.
CO2(g) :
c.
Na3PO4(s):
d.
Ca(NO3)2(s):
1C+2O=
Science 10
Unit A: Energy and Matter in Chemical Change
Converting Moles to Grams (mass)
mn M
m
n
M
Examples:
m
n
M
mass (g)
moles
molar mass
Find the mass of
a. 3 moles of NaCl(s)
b. 2 Fe2SO4(s)
c. 4.5 Zn(NO2)2(s)
Converting Grams (mass) to Moles
Examples:
a.
How many moles are there for each compound given
the mass.
65.0 g of: NaOH(s)
1 mole: NaOH(s) = 40.00 g
n
Text:
A3.R
AR
b.
348.75 g of: CoSO4(s)
c.
880.10 g of: Cr(NO3)2(s)
Practice Problems: 13 – 20
Check & Reflect: 1 – 11
Section Three Review
Unit A Review
m
60.0g

 1.5 mol
M 40.00g
p . 108, 109
p. 112
p. 113
p. 117-121
40