Page 11
S8P1a.
Matter
Describe matter and what is it composed of?
Matter is anything that has mass and takes
up space.
Examples: book, toy, car, paper
Non-examples: heat, light
Matter is made of tiny indivisible particles
called atoms. They are the basic building
blocks of all matter.
For many years, people have wondered
what matter is made of including
Democritus, Lavoisier, Dalton, Thompson,
Rutherford and Bohr.
On page 10, create a t-chart and identify each of the following as
an example of matter or not an example of matter.
Water, juice, plant, lightning, electricity, magnetism, force, heat,
air, helium, oxygen, time, sound, clothes, sunlight, energy, inertia
Matter
Not Matter
Page 13
The nucleus is the small dense, positively
charged center of an atom. It contains the
most of the atom’s mass. It contains
protons and neutrons.
Protons are positively charged particles
located inside the nucleus.
Neutrons are neutrally charged particles
located inside the nucleus.
Electrons are negatively charged particles
found in electron clouds outside the
nucleus.
On page 12
+
-
+ +
+ +
+
-
-
Page 61
There are two kinds of pure substances:
elements and compounds.
An element is matter made up of only one kind
of atom. There are over 100 known elements.
About 90 of them are found naturally on Earth
and the other 20+ are synthetic (man-made).
All known elements are arranged in a chart
called the periodic table of elements. Each
element on the chart has a chemical symbol
with one to three letters.
The periodic table is arranged in rows called
periods and columns called groups or families.
There are 7 periods and 18 groups.
Elements in the same group share similar
properties.
Page 63
Each element has an atomic number and an
atomic mass.
The atomic mass is the average of all of the
isotopes of an element.
The atomic number is ALWAYS the number of
protons. It is also the number of electrons in a
neutral atom.
To determine the number of neutrons, you
must subtract the atomic number from the
atomic mass.
For example, Copper has an atomic number of
29 and an atomic mass of 63. It has 29
protons , 29 electrons and 34 neutrons.
On page 60
Identify the group/family number of the following elements:
1. Lithium
4. Beryllium
2. Xenon
5. Hydrogen
3. Gold
Identify the period number of the following elements:
6. Arsenic
9. Xenon
7. Palladium
10. Mercury
8. Argon
Identify the group/family name of the following elements:
11. Lithium
14. Beryllium
12. Xenon
15. Aluminum
13. Gold
On page 62, draw and complete the table below.
Element Name # of protons
# of electrons
# of neutrons
Aluminum
Barium
Neon
Tin
Platinum
Titanium
Zirconium
Describe how the periodic table is arranged/organized.
Page 65
About 75% of all the elements are metals.
They generally have a shiny or metallic luster
and are good conductors of heat and
electricity. All metals except mercury are
solid at room temperature. Metals are
located on the left side of the Periodic Table.
Nonmetals are elements that are usually dull
in appearance. Most are gases and poor
conductors of heat and electricity. Nonmetals
are located on the right side of the Periodic
Table.
Metalloids are elements that have
characteristics of metals and nonmetals.
They are found between the metals and the
nonmetals along a zig-zag line.
On page 64, identify whether the following elements are metals,
nonmetals or metalloids.
Hydrogen, Helium, Lithium, Beryllium, Boron, Argon, Potassium,
Mercury, Calcium, Oxygen, Sulfur, Zinc, Gold, Xenon, Neon
Metal
Nonmetal
Metalloid
Page 67
Each element has a unique # of protons
which is the atomic number. Every single
atom of that element must have the same
number of protons.
Atoms of one element must have the same
# of protons, but can have a different # of
neutrons.
Isotopes are atoms with the same # of
protons and a different number of
neutrons. This gives an isotope a different
atomic mass.
For example Hydrogen sometimes has an
atomic number of 1, 2 or 3. This is because
the number of neutrons may vary.
Page 69
When referring to an isotope, you state the
element name followed by its atomic mass.
For example:
Hydrogen-1 or Hydrogen-2 or Hydrogen-3
1
1
1
H
H
H
Hydrogen
Hydrogen
Hydrogen
1.001
2.001
3.004
protons = 1
electrons = 1
neutrons = 0
protons = 1
electrons = 1
neutrons = 1
protons = 1
electrons = 1
neutrons = 2
Note: Mass numbers are decimals because some
isotopes are more common than others. The one
listed in the periodic table is the most common
isotope.
On page 66, determine the number of protons, electrons and
neutrons for the following isotopes.
Carbon -12
Carbon-13
Chlorine 35
Chlorine 37
Carbon-14
Protons
Electrons
Neutrons
Protons
Electrons
Neutrons
Iron-54
Protons
Electrons
Neutrons
Iron-56
Iron-57
Iron-58
On page 66, determine the number of protons, electrons and
neutrons for the following isotopes.
Carbon -12
Carbon-13
Carbon-14
Protons
6
6
6
Electrons
6
6
6
Neutrons
6
7
8
Chlorine 35
Chlorine 37
Protons
17
17
Electrons
17
17
Neutrons
18
20
Iron-54
Iron-56
Iron-57
Iron-58
Protons
26
26
26
26
Electrons
26
26
26
26
Neutrons
28
30
31
32
Page 71
Ions are atoms that have a charge. They
may be positively or negatively charged.
Ions that have a positive charge are called
cations. They form when an atom loses
electrons.
Number of Electrons < Number of Protons
Ions that have a negative charge are called
anions. They form when an atom gains
electrons.
Number of Electrons > Number of Protons
Only the electrons change. The protons and
neutrons stay the same.
Ions with opposite charges attract
therefore cations and anions attract each
other. Moving ions conduct electricity
On page 70, determine the number of protons, electrons and neutrons for the
following.
Remember: Only the electrons change. The protons and neutrons stay the same.
P
P -3
Protons
Protons
Electrons
Electrons
Neutrons
Neutrons
Ca
Ca +2
Protons
Protons
Electrons
Electrons
Neutrons
Neutrons
K
K +1
Protons
Protons
Electrons
Electrons
Neutrons
Neutrons
Cl
Cl -1
Mg
Mg +2
Sc
Sc +3
On page 70, determine the number of protons, electrons and neutrons for the
following.
Remember: Only the electrons change. The protons and neutrons stay the same.
Cl
Cl -1
Protons
17
17
18
Electrons
17
18
16
Neutrons
18
18
Mg
Mg +2
P
P -3
Protons
15
15
Electrons
15
Neutrons
16
Ca
Ca +2
Protons
20
20
Protons
12
12
Electrons
20
18
Electrons
12
10
Neutrons
20
20
Neutrons
12
12
K
K +1
Sc
Sc +3
Protons
19
19
Protons
21
21
Electrons
19
18
Electrons
21
18
Neutrons
20
20
Neutrons
24
24
Electron Levels
Page 15
Electrons surrounding an atom are located in
regions around the nucleus call “energy levels”.
They represent 3-D spaces surrounding the
nucleus.
The first energy level is closest to the nucleus
with each level moving a little farther away.
Each energy level can accommodate or “hold” a
different number of electrons before additional
electrons go into the next level.
Page 15
1st Level = 2 electrons max.
2nd Level = 8 electrons max.
3rd Level = 8 electrons max.
4th Level = 18 electrons max.
5th Level = 18 electrons max.
6th Level = 32 electrons max.
7th Level = 32 electrons max.
The electrons in the farthest (outer) level are
called valence electrons. Elements in the same
group have the same number of valence
electrons.
On page 72
Draw the electron arrangement of the following.
Lithium
Chlorine
Sodium
Sulfur
Page 77
S8P1a., S8P1f.,
S8P1d
States of Matter
11/ /13
Compare and contrast the particle movement in the different states of
matter?
A state of matter is the physical form in which
matter exists. There are four states (phases) of
matter : solid, liquid, gas and plasma. Matter often
changes state when heat is added or taken away.
A solid is a substance with a definite shape and a
definite volume. The particles in a solid are packed
closely together and maintain a rigid form without
a container. They vibrate slowly against one
another.
A liquid is a substance with a definite volume, but
not a definite shape. The particles in a liquid move
faster and freely past one another, but are still
close to one another. Liquids take the shape of the
container they are in.
Page 79
A gas is a substance that does not have a
definite shape or a definite volume. Gas
particles move very fast and bounce off of one
another. Gases fill the container they are in.
Summary: Describe the particle movement in the states of matter.
On page 76
Identify whether each of the following are solids, liquids or
gases in the table below.
Milk toy car
helium
hydrogen
steam
sugar
salt
pepsi
Solid
Liquid
water
ice
oxygen
Gas
On page 78
Compare and contrast the characteristics and the particle
position and movement in the 3 common states of matter
Solid
Shape
Volume
Particle Position
Particle Movement
Miscellaneous
Liquid
Gas
Page 83
S8P1d.
Properties of Matter
11/ /13
What are the various properties of matter and how can I distinguish
between physical and chemical properties of matter?
A property is a characteristic of matter.
A physical property is a characteristic that can be
observed or measured without changing the
identity of a substance.
Examples: density (mass/volume), electrical
conductivity, hardness, pH, state of matter and
luster
A chemical property is a characteristic that
describes how a substance will interact with other
substances during a chemical reaction.
Examples: reactivity, the ability to burn and rust
Summary: What are the various properties of matter and how can I distinguish
between physical and chemical properties of matter?
Common Physical Properties
Density is the amount of mass in a given
volume.
Density = mass
or D=m
volume
V
The density of water is 1.0 g/cm3
Page 85
pH is a measure of how acidic or basic a
solution is ranging in a scale from 0 to 14. The
values are the concentration of hydrogen ions
in a solution.
acidic (acid)
0
Most acidic
High concentration
of hydrogen ions
neutral
7
basic (base)
14
Most basic
Low concentration
of hydrogen ions
Page 87
Common Chemical Properties
Tarnishing – the reaction between sulfur in
the air and metals.
Rusting – the reaction between oxygen and
metals.
Combustibility – the reaction between
oxygen and fuel that results in fire.
Flammability – the ability to burn
Reactivity – the ease and speed with which
an element combines, or reacts (bonds), with
other elements and compounds
Page 82
Draw the pH scale and illustrate each item on it in its
appropriate place on the scale and classify each of the
following materials as an acid or base.
pH
Baking soda
Lemon
8.5
2
Ammonia
11.5
Milk
6.5
Soap
10
Drain cleaner
14
Water
7
Banana
5.2
Vinegar
2.8
Acid or Base
Page 82
Draw the pH scale and illustrate each item on it in its
appropriate place on the scale and classify each of the
following materials as an acid or base.
pH
Acid or Base
8.5
base
2
acid
Ammonia
11.5
base
Milk
6.5
acid
Soap
10
base
Drain cleaner
14
base
Water
7
neutral
Banana
5.2
acid
Vinegar
2.8
acid
Baking soda
Lemon
Page 84
Create a two-column table and classify each of the terms
below as either a physical property or a chemical property.
reacts with base to form water
Boiling point
density
Taste
reacts with an acid
color
flammability
melting point
luster reacts to oxygen
solubility hardness odor reacts with water to form gas
Physical Property
Chemical Property
Page 89
S8P1.d & S8P1.e
Changes in Matter
11/ /13
What types of changes can matter undergo? What happens to
matter when it undergoes changes?
Matter can change. The types of changes matter
undergoes are classified into two groups: physical
changes and chemical changes.
A physical change alters the physical properties of
a substance without changing the identity of the
substance. Physical changes cause a change in
properties such as volume, mass, or state of
matter. Many physical changes can be reversed.
Examples: melting, evaporating, freezing, cutting
A chemical change occurs when a substance is
changed into a new substance with different
properties. During a chemical change, the identity
of a substance is changed.
Examples: burning, rusting, baking, combusting
Page 91
A chemical reaction is the process by which new
substances are formed during a chemical
change. Some signs that indicate a chemical
reaction has occurred include the forming of
gases, a change in color, the release of heat, or
the emission of light.
Another sign of a chemical reaction is the
formation of a precipitate. A precipitate is a
solid that forms from a chemical reaction that
takes place in a solution.
It is very difficult or impossible to reverse the
effects of a chemical change.
Summary: EQ - What types of changes can matter undergo? What
happens to matter when it undergoes changes?
page 88
Create a two-column table and classify each of the descriptions below as
either a physical change or a chemical change.
Iron rusts
sodium hydroxide dissolves in water
milk goes sour
a match ignites and burns
an ice cube melts to form a puddle of water
icicles form at the edge of a roof
chocolate bar melts in the sun
water is heated and changed into steam
vinegar and baking soda react
acid on limestone produces carbon dioxide gas
wood and leaves rot
a tea kettle begins to whistle
Physical Change
Chemical Change
Page 90
PHYSICAL OR
YES
PHYSICAL
CHANGE
CHEMICAL CHANGE?
QUESTION: AFTER THE CHANGE
IS IT THE SAME SUBSTANCE?
EVIDENCE OF A CHEMICAL CHANGE
BUBBLING
TURNS CLOUDY
TEMPERATURE CHANGES
EXOTHERMIC – ENERGY IS EXITING - GETS HOTTER
ENDOTHERMIC – ENERGY IS ENTERING – GETS COOLER
COLOR CHANGE
CHANGE IN SMELL OR TASTE
NO
CHEMICAL
CHANGE
Page 93
EQ-Water can be found in solid, liquid and gas forms. How
does that happen?
The transformation of matter from one state to
another is called a phase transition. Phase
transitions occur at precise points when the
energy of motion in the atom is too much or too
little for the atom to remain at that state.
Phase Transition
Description
Melting (add heat)
Solid to Liquid
Evaporation (heat added)
Liquid to Gas
Sublimation (heat added)
Solid to Gas (skipping Liquid)
Condensation (heat removed)
Gas to Liquid
Freezing (heat removed)
Liquid to Solid
Deposition (heat removed)
Gas to Solid (skipping Liquid)
Summary: EQ-Water can be found in solid, liquid and gas forms. How does that
happen?
On page 92
The freezing point and melting point are the same temperature.
On page 92
The following processes are phase transitions. Identify the
type of transition.
Phase Transition
Water droplets coat your cold
soda can on a hot day.
A cloud releases rain.
Solid dry ice steams in air.
Glaciers floating in the ocean
are shrinking.
Morning dew disappears from
the grass by midday.
A cloud releases snow.
Substances and Mixtures
Distinguish between pure substances and mixtures?
Page 17
All forms of matter can be classified into two groups: pure
substances and mixtures.
A pure substance is one having a homogeneous
composition. There are two types of pure substances:
elements and compounds.
An element is matter that is made of only one kind of
atom. An atom is the smallest unit of an element.
A compound is matter that is formed when two or more
elements join (bond) chemically (a chemical reaction).
They cannot be broken apart. A molecule is the smallest
unit of a compound that has all the properties of the
compound.
On page 16
Identify whether each of the following are
elements or compounds in the table below.
H
CO2
Fe2S
CO
H20
Co
OH
SiO2
Element
Ca
Na
CH4
NaCl
NaOH
Compounds
Page
A molecule is the smallest unit of a
compound that has all the properties of the
compound. The makeup of a molecule is
shown in a chemical formula. A chemical
formula uses chemical symbols and
subscripts to identify the number and types
of atoms of each element that make up a
compound.
A subscript is a small number written to the
right and slightly below a chemical symbol
to tell the number of atoms of that element
is in the substance.
The chemical formula for water is H20.
This means one molecule of water has 2
Hydrogen atoms and 1 Oxygen atom.
On page 96
Determine the number of atoms of each element present in
each of the following compounds.
1. CO
2. CO2
3. H2O2
4. NaCl
5. NaOH
6. C12H22O11
7. FeS2
8. Fe2O3
9. C2O
10.Na2O
11.CH4
Page 99
Elements can combine in different ways to
form either compounds or mixtures. A mixture
forms when two or more substances combine
without joining chemically. They are not
bonded together.
Because they are not bonded chemically, the
parts of a mixture retain their own individual
identities and properties and can be separated.
A mixture that is unevenly mixed is called a
heterogeneous mixture. Ex. Trailmix. A mixture
that is mixed evenly is called a homogeneous
mixture. Ex. Kool-Aid
Summary: EQ- How can matter be classified?
On page 98
Identify whether each of the following are heterogeneous or
homogeneous mixtures in the table below.
Vegetable soup
Chex Mix
coffee
cake batter
chocolate chip cookie
milk
salt water
pizza
spaghetti & meatballs
cereal in milk
taco salad
Heterogeneous Mixture
Homogeneous Mixture
Page 101
S8P1g.
Conservation of Matter
During a change in matter, how does the amount of matter
compare before and after it changes?
The law of conservation of matter states that,
during a chemical reaction, matter cannot be
created or destroyed.
Even though the matter may change from one form
to another, the same number of atoms exist before
and after the changes take place.
Reactant – the substances there before a reaction
occurs.
Product – the substances there after the reaction
takes place.
MASS OF REACTANT = MASS OF PRODUCT
UNDERSTANDING CHEMICAL REACTIONS &
THE LAW OF CONSERVATION OF MATTER
If 25g of Potassium
is reacted with 5g of
Oxygen, how much
Potassium Oxide is
produced?
4K + O2
25g
+
5g
Reactants
2H2 + O2
A coefficient shows the
number of molecules.
2H2 means 2 hydrogen
molecules for a total of 4
hydrogen atoms.
Page 103
2K20
30g
Products
2H20
A subscript shows how
many atoms are in a
formula. In O2, the 2
means 2 atoms of
oxygen.
Page 100 – Write the questions and answer each.
How many different elements are present?
N2
CaF2
CO2
NaSO3
CaCO3
SiO2
How many molecules are present?
2H2O
5Be2Br
8CO2
3NaCl
O2
MgS
How many total atoms are present?
2H2O
2Be2Br
7CO2
6NaCl
4O2
2MgS
Using this reaction, answer the following questions.
Li2O + MgCl2  2LiCl + MgO
Name the first reactant.
Circle the second reactant.
Underline the first product.
Name the second product.
How many Mg atoms are on the reactant side? the product side?
How many Chlorine atoms are on the reactant side? the product side?
page 102 – Write each chemical reaction (and question) and
determine the missing value?
If 23g of Magnesium is reacted with
Oxygen to produce 38 g of Magnesium
Oxide, how much Oxygen was used in
the reaction?
2Mg + O2  2Mg0
23g
+ ?g
2KCl + Li2O
21g
+
4g
38g
 K2O + 2LiCl
?g
+
12g
Using the numbers provided,
determine how much K2O is
produced in the reaction.