THINK
What is matter?
Matter
Think – Pair - Share
SHARE
What do you think?
What do you think?
PAIR
Individually, think of what you know about “matter”. This was part of your 6th
grade science class. Write down what comes to mind when you think of
“matter”. 5 - 7 minutes
Now pair up with a partner (or team) and share your thoughts and ideas. One
person serve are the recorder and put these on the construction paper.
5 – 7 minutes
Each team will then share their information with the class. Tape the
construction paper up for other students to see.
Matter: Properties and Change
http://www.youtube.com/watch?v=FSyAehMdpyI “The Nucleus: Crash Course Introduction To Chemistry” #1” 10:12
Matter, is a substance that has mass and also volume. The volume is determined by the space it
occupies, while the mass is defined as a measure of how much matter is in an object.
http://micro.magnet.fsu.edu/primer/java/scienceopticsu/powersof10/ size comparisons from milky way galaxy to quarks
What is matter? Explain your reasoning.
http://commons.wikimedia.org
Sunlight
Water
Electricity
Heat
Smoke
Earth’s Atmosphere
Early alchemists thought that everything was made of either earth, air, water or fire.
Why can you never trust an
atom?
“The Elements” VHS
http://youtu.be/zUDDiWtFtEM “The New Periodic Table Song 3:00 min.
http://www.ncpublicschools.org/docs/accountability/testing/releasedforms/2009grade8periodic.pdf DPI periodic table
Element Information
Chemistry Spoons Game
The first letter is always capitalized.
In symbols with two or more letters,
only the first letter is capitalized.
73
An atom will have the same number of electrons as protons.
Coach Lesson #1
Atoms:
most basic unit of matter; atoms make up everything
Lithium atom (atomic #3 = protons)
Atomic Mass = 7 (protons and neutrons)
Protons = positively charged
Neutrons = neutral (no) charge
Electrons = negatively charged
What particles are in the
nucleus?
- An atom containing an equal
number of protons (+) and
electrons (-) is electrically neutral,
otherwise it is positively or
negatively charged and is known
as an ion.
An atom is classified according to the
number of protons (atomic #):
- the number of protons (atomic #)
determines the chemical element,
- and the number of neutrons
determines the isotope of the
element. ( i.e. carbon 12 and 14)
How do sizes of atomic particles differ?
- Electrons are extremely
small compared to all of
the other parts of the
atom.
- The mass of an electron
is almost 1,000 times
smaller than the mass of
a proton.
(Quarks make up protons and neutrons.)
How is the size of atomic particles measured?
The nanometer is often used to express dimensions
on an atomic scale:
- The diameter of a helium atom, for example, is
about 0.1 nm, and that of a ribosome is about
20 nm.
Where are the protons and neutrons located?
2
(protons and neutrons)
Electron Orbitals/ Cloud/Energy Level/Shell Configurations
How many valence electrons are shown
in this atom?
Valence electrons are those located in the outer most shell/level.
Valence Electrons
The valence is the number of outer shell/orbital electrons. These are the electrons available to take part in chemical reactions.
The periodic trend for valence works well for the representative elements, which are in groups 1, 2, 13, 14, 15, 16, 17, and 18
(the ‘tall’ parts of the table). Reading left to right, the valence for each of the main groups increases from one to 8. The noble
gas elements, with 8 valence electrons, are especially stable.
Helium only has 2 valence electrons. Why is it in group 18?
Why are the noble gasses the “happiest” elements?
Atomic Structure of Helium
1.
2.
3.
4.
How many protons(+) are in helium?
How many neutrons (neutral) are in helium?
How many electrons (-) are in helium?
How many valence (outer level) electrons are
shown?
Name That Element 
N
Lithium
- Protons = 3 (atomic number)
N
- Neutrons = 4
- Mass Number/Weight = 7
(protons and neutrons)
Lithium (Li): One neutron is not shown.
1. What period is lithium in?
- Electrons = 3
2. What group/family is lithium
in?
* The number of protons (+) and
3. How many valence (outer)
electrons (-) will be the same.
electrons does lithium have?
Elements above 92
are synthetic
meaning they are
“manmade” and
not found in nature.
Name That Element
Atomic Structure of Carbon
1. How many protons (+) are
shown?
2. What is the atomic mass?
3. How many neutrons
(neutral) are shown?
4. How many electrons (-) are
shown?
5. How many valence (outer
level) electrons are shown?
Classifications of elements
Some sources have astatine as a metalloid while others do not.
Atom Diagram Practice
Name That Element
Atomic Structure of Boron
“Build That Atom” Activity
http://phet.colorado.edu/en/simulation/build-an-atom build an atom activity
A. What is the atomic
number of boron?
B. What is the mass
number of boron?
C. What family is boron in?
D. What group is boron in?
1. How many protons (+) are
shown?
2. How many neutrons
(neutral) are shown?
3. How many electrons (-) are
shown?
4. How many valence (outer
level) electrons are shown?
“The Elements” VHS 50:52
Valence electrons can be determined by looking at the group/family.
Group 1 = 1 valence (outer) electron
Periodic Table Color Coding Activity
Group 2 = 2 valence (outer) electrons
Group 13 = 3 valence (outer) electrons, etc. (transition elements 3-12 will vary)
A group/family on the periodic table means the elements have similar chemical properties.
Elements of the same period have the same number of electron orbitals/shells.
Valence electrons are what determine the bonding ability of an atom.
Essential mineral elements : (elements required by living organisms, other than the four
elements carbon, hydrogen, nitrogen, and oxygen present in common organic molecules)
nitrogen, phosphorus, potassium, calcium, magnesium, sulfur, boron, chlorine, iron, manganese,
zinc, copper, molybdenum, and nickel.
Beneficial elements: elements which promote plant growth in many plant species but are not
absolutely necessary for completion of the plant life cycle : Silicon, sodium, cobalt, and
selenium
Essential nonmineral elements; (elements taken up as gas or water): hydrogen, oxygen, and
carbon
Metals, Nonmetals and Metalloids
Some sources show astatine as a metalloid while other do not.
along zigzag line
Classifications of Elements
Why is hydrogen not connected to group 1?
Classifications of elements
34
Se
Seleniu
m
77
84
Po
Polonium
209
Some periodic tables include astatine as a metalloid. Based on the site
http://www.chemicalelements.com/groups/metalloids.html astatine is
not a metalloid.
http://www.chemtopics.com/elements.htm interactive periodic table
Metalloids
Metalloids are a chemical element with properties that are in-between or a mixture of those of
metals and nonmetals. The seven elements commonly recognized as metalloids are boron,
silicon, germanium, arsenic, antimony, astatine and tellurium. They or their compounds find
uses in glasses, alloys or semiconductors. These are located along the zigzag line.
Metals
Notice that the metalloids and nonmetals are not included. Compare this
section of the periodic table to the complete periodic table of elements.
Metalloids & Nonmetals
Metalloids
Some sources show astatine
as a metalloid while other do not.
Nonmetals
Physical Properties: can be observed and measured without changing
the kind of matter being studied; can be used to identify substances
Melting Point:
- The temperature at which a solid can change to a liquid.
- The temperature at which a pure substance melts is unchanging
under constant conditions.
Boiling Point:
- The temperature at which a liquid boils.
- A substance changes from a liquid to a gas.
- Boiling temperature is unchanging under constant conditions for a
given substance.
Assessment Probe: “Floating Logs”
Example:
Man
from
Zambia
Demo: Density Blocks
Density:
- a property that describes the relationship between the mass of a
material and its volume
- Substances that have higher densities contain more matter in a
given volume.
- The density of a substance will stay constant/the same.
Color: may be used to identify substances but not always
Physical Properties of Metals and Nonmetals
STC: “Finding the Conductor” 1.1
Physical Properties of Noble Gasses (Group/Family #18)
How are properties used to identify substances?
H
How are properties used to determine how elements and substances are used?
1. Why is aluminum used in airplanes?
2. Why is helium used in balloons instead of oxygen or hydrogen?
Chemical Property: any of a material's properties that becomes evident
during a chemical reaction; that is, any quality that can be established
only by changing a substance's chemical identity
1.
Can be used to help identify a substance
Example: Man from Zambia
2.
Usually involves the substance’s ability to react or not react with another
specific
substance
Examples
Reacting with Oxygen (oxidation): The ability of a substance to burn is a chemical
property that involves a substance reacting quickly with oxygen to produce light and
heat. (i.e. iron rusts or apples turn brown).
http://www.youtube.com/watch?v=mjkuSm__G7s phosphorus reacting with oxygen
Reacting with Acids: The ability of a substance to react with an acid is a chemical
property. Some metals react with various acids to form compounds. All metals do not
react with all acids. Bases react with acids to form water and neutralize the acid.
Reactivity: the tendency of a substance to undergo chemical reaction, either by itself or with
other materials.; reactivity is a chemical property of an element
http://www.youtube.com/watch?v=Jy1DC6Euqj4
potassium reaction in water 20 sec.
http://www.youtube.com/watch?v=MTcgo46nxNE
sodium reaction in water 48 sec.
These soft, silvery sodium chunks were cut
with a knife and stored under oil. In air they
turn white in seconds; exposed to water
they generate hydrogen gas and explode in
flaming balls of molten sodium.
http://www.youtube.com/watch?v=1bJBueGSC9M
calcium reactivity with oxygen 27 sec.
(silver oxide (Ag2O) demonstration)
Less
Reactive
Physical & Chemical Properties
Substance
Physical Property
Chemical Property
Helium
Less dense than air
Nonflammable
Wood
Grainy texture
Flammable/combustible
Baking Soda
White powder
Reacts with vinegar to form
bubbles (CO2)
Powdered Sugar
White powder
Does not react with vinegar
Rubbing Alcohol
Clear liquid
Flammable/Combustible
Red Food Coloring
Red color
Reacts with bleach and loses
color
Iron
Malleable
Reacts with oxygen (oxidation)
to form iron oxide (rust) Ag2O
Tin
Malleable
Reacts with oxygen to form tin
dioxide
(demonstration)
Physical or Chemical Property… What do you think?
1. Shape
2. Density
3. Acidity (below 7 pH)
4. Solubility
5. Basicity (above 7 pH)
6. Combustibility
7. Odor
8. Melting point
9. Reactivity
10. Boiling point
11. Color
Points to Consider
If the property changes, is a new substance
formed? If not, it is a physical property. 
If you still have the same substance after
changing the property, it is a physical
property.
http://www.glencoe.com/sites/common_assets/science/vir
tual_labs/E21/E21.html
Is the change a physical or chemical change?
http://www.youtube.com/watch?v=vW9of4JYHY0 Chemical and Physical Changes 1:26
Physical Changes
Physical Change:
- The physical properties change but the type of substance stays the
same.
- Matter changes is size, shape or form.
- There is no change in the chemical makeup of the substance(s) that
are changed.
- Physical changes can be reversed.
- Examples: cutting, changes in states of matter (melting, boiling,
freezing), etc.
http://glencoe.mcgraw-hill.com/sites/dl/free/0078617650/160350/00044680.html Brain Pop Chemical and Physical Changes program w/quiz (note: Cooking an egg
is a chemical change.)
Phase Change
(mixing two or more substances)
(dissolving a substance)
Chemical vs Physical Changes (laptop review)
Chemical Change:
- properties change and a different substance is produced.
- Chemical changes cannot be reversed.
- Examples: iron reacts with oxygen and water to form iron oxide (rust);
silver reacts with oxygen to form silver oxide (tarnish)
Evidence of a chemical change:
1.
Change in energy: temperature increase = exothermic chemical reaction
temperature decrease = endothermic chemical reaction
Color change:
This is not when a color has been covered, for example dying, painting,
etc.
Formation of a gas: if in a solution, bubbles will often times been seen when the gas is
formed
2.
3.
4.
Formation of a precipitate: when two or more solutions are combined and a solid is
formed
STC: “The Burning Candle” 1.3 “Mixing the Solutions” 1.8
“Adding the Acid” 1.5
What evidence is there of a chemical change in these two pictures of the Statue of Liberty?
Sublimation: when a substance changes directly from a
gas to a solid
Examples:
- The forming of frost from water vapor
-
When dry ice forms: Dry ice is frozen carbon dioxide.
As it breaks down, it turns directly into carbon
dioxide gas rather than a liquid
http://www.youtube.com/watch?v=8tHOVVgGkpk
dry ice bubbles 2:20; also shows properties of polar
molecules water and detergent (surface tension)
-
Solid air fresheners
Apples brown (react with oxygen)
Physical change rearranges molecules but doesn't affect their internal
structures. Some examples of physical change are:
- whipping egg whites (air is forced into the fluid, but no new substance is produced)
- magnetizing a compass needle (there is realignment of groups ("domains") of iron atoms,
but no real change within the iron atoms themselves).
- boiling water (water molecules are forced away from each other when the liquid changes
to vapor, but the molecules are still H2O.)
- dissolving sugar in water (sugar molecules are dispersed within the water, but the
individual sugar molecules are unchanged.)
- dicing potatoes (cutting usually separates molecules without changing them.)
Chemical change is any change that results in the formation of new
chemical substances. At the molecular level, chemical change involves
making or breaking of bonds between atoms. These changes are
chemical:
-
iron rusting (iron oxide forms)
gasoline burning (water vapor and carbon dioxide form)
eggs cooking (fluid protein molecules uncoil and crosslink to form a network)
bread rising (yeast converts carbohydrates into carbon dioxide gas)
milk souring (sour-tasting lactic acid is produced)
suntanning (vitamin D and melanin is produced)
Mini-Poster Analysis
1. Is a phase change a physical or chemical change? Explain.
2. What is the relationship between phase change and temperature?
3. What effect does phase change have on the volume of the
substance/molecules? Density? Mass? Explain.
http://www.youtube.com/watch?v=czmQ2_ymaOo formation of ice crystals 37 sec.
Is the change a physical or chemical change?
1
4
2
5
3
6
Is the change a physical or chemical change?
1. Chemical
4. Physical
2. Chemical
5. Chemical
3. Physical
6. Chemical
Is the change a chemical or physical change?
1
4
3
2
5
6
Is the change a chemical or physical change?
1. Physical
4. Physical
2. Physical
5. Chemical
3. Chemical
6. Chemical
Chemical Changes Require Chemical Reactions
Chemical Reaction: when substances chemically combine to
form new substances.
STC: “Reacting A Tablet” 1.7
MRE Lab
Endothermic Reactions = temperature decrease; Exothermic Reactions = Temperature increase
A chemical change involves a physical change, and can include but is not limited to the following:
Chemical changes do not change the mass, because according to the Law of Conservation of Mass/Matter,
during a chemical reaction the mass of the reactants of the formula will always equal the mass of the
products.
Chemical Reactions = Chemical Changes = New Substance(s) Formed
Chemical reactions are shown in the form of chemical equations.
Word equation:
Sodium + Chlorine yields sodium chloride
Chemical equation:
2Na + Cl2
reactants
Coefficient = # of molecules in the compound
2NaCl
products
Subscript = # of atoms of the element
1.
What is the mass of the reactants? (Use your periodic table.)
2. What is the mass of the products? (Use your periodic table.)
3. Does this reaction meet the “Law of Conservation of Mass/Matter”?
Explain.
Law of Conservation of Mass/Matter: “Nuts & Bolts of Law of Conservation of Mass” or Simulation
- In a chemical equation, matter cannot be created or destroyed
- The mass of the reactants will equal the mass of the products.
STC: “Mixing the Solutions” 1.8
“Balancing Chemical Equations” practice
Chemical Reactions = Chemical Changes = New Substance(s) Formed
Chemical reactions are shown in the form of chemical equations.
Word equation:
Sodium + Chlorine yields sodium chloride
Chemical equation:
1.
2Na + Cl2
reactants
2NaCl
products
What is the mass of the reactants? 116
- 2 Na atoms = 23 x 2 = 46
- 2 Cl atoms = 35 x 2 = 70
2.
What is the mass of the products? 116
- 2 Na atoms = 23 x 2 = 46
- 2 Cl atoms = 35 x 2 = 70
3.
Does this reaction meet the “Law of Conservation of Mass/Matter”?
Explain. Yes, because the mass of the reactants equals the mass of
the
products
Law of Conservation of Mass/Matter:
- In a chemical equation, matter cannot be created or destroyed
- The mass of the reactants will equal the mass of the products.
STC: “Mixing the Solutions” 1.8
“Balancing Chemical Equations” practice
Balanced Chemical Equations
The coefficient shows how many total molecules are present. Multiply this by the subscript.
No subscript indicates that 1 atom is present.
Hydrogen = 4
Oxygen = 2
Hydrogen = 4
Oxygen = 2
Does this equation meet the “Law of Conservation of Mass/Matter”? Explain.
http://www.sciencespot.net/Media/blncact.pdf Balancing Act WS
Balance the following chemical equations.
1.
2.
3.
4.
5.
Reactants
Products
Na + Cl2
H2 + Cl2
CO2 + H2
2NO + O2
4Fe + 3O2
NaCl
HCl
CO + H2O
2NO2
2Fe2O3
Note: You may only add coefficients when balancing equations, not subscripts.
One of the equations is balanced. 
Check your equations.
Reactants
1.
2.
3.
4.
5.
2Na + Cl2
H2 + Cl2
CO2 + H2
2NO + O2
4Fe + 3O2
Products
2NaCl
2HCl
CO + H2O
2NO2
2Fe2O3
Balanced chemical equations support the law of conservation of
mass/matter. Explain why.
The chemical reaction for photosynthesis
Reactants
Reactants
6 carbon
24 oxygen
24 hydrogen
yield
Products
Products
6 carbon
24 oxygen
24 hydrogen
Chemical Equation for Cellular Respiration
Reactants
Reactants
6 carbon
24 oxygen
24 hydrogen
yield
Products
Products
6 carbon
24 oxygen
24 hydrogen
Compounds and Mixtures
Substances combine but NOT chemically; they keep
their original properties
Have the same consistency throughout
- Elements combine to form compounds.
- Compounds have a chemical formula.
- Elements that combine DO NOT keep their
original properties.
- May be natural or synthetic (manmade)
Heterogeneous
Do not have the same consistency throughout
What is the difference between a compound and a molecule?
1.
2.
A molecule is formed when two or more atoms join together chemically.
A compound is a molecule that contains at least two different elements.
- All compounds are molecules but not all molecules are compounds.
Example:
- Molecular hydrogen (H2), molecular oxygen (O2) and molecular nitrogen
(N2) are not compounds because each is composed of a single element.
They are diatomic molecules because in nature they do not exist as
individual atoms.
- Water (H2O), carbon dioxide (CO2) and methane (CH4) are compounds
because each is made from more than one element.
- The smallest bit of each of these substances would be referred to as a
molecule.
STC: “Our Ideas About Pure Substances and Mixtures”
Cannot be changed into a simpler substance
Pure substances composed of two or
more types of elements that are
chemically combined
Compounds
- A compound is a type of matter that forms when two or more different elements combine
chemically. Two or more atoms bonded together is a molecule of the substance that is formed.
- When atoms combine chemically, they do not retain their original properties. How do the following
compounds provide evidence of this?
In the compounds below, compare the properties of elements before and after chemical bonding has
occurred.
Examples: Chemical formulas for common substances
H2O chemical formula for 1 water molecule
Subscript: #of atoms present of the element to the left
no # as with oxygen means there is 1 atom present
C12H22O11
NaCl
O2
NaClO
HCl
NaCl
sucrose
table salt
oxygen (diatomic element)
household bleach
hydrochloric acid
sodium chloride (table salt)
NaHCO3
HC2H3O2
H2O
NH3
CO2
H2O2
Activity: Identification of Element & Compounds in Products
“Analyzing Formulas” practice
baking soda
vinegar
water
ammonia
carbon dioxide
hydrogen peroxide
Water (H 0)
2
• Water is a compound formed
from two atoms of hydrogen
and one atom of oxygen; H20
_ and + indicates the charged area of the molecule
_
+
+
• In their form as elements,
hydrogen and oxygen are
gasses. They both are also
highly flammable.
• When combined in this 2
to 1 ratio, they form a
liquid that is not
flammable.
“Biological Molecules: “You Are What You Eat”
complete study guide
http://www.youtube.com/watch?v=H8WJ2KENlK0 (14:09)
Sodium Chloride: Table Salt (NaCl)
Sodium Chloride (table salt) is
a combination of 1 sodium
atom and 1 chlorine atom;
NaCl.
• In their form as elements,
sodium is a highly explosive
solid that explodes in water
and chlorine is a toxic gas.
http://www.youtube.com/watch?v=9bAhCHedVB4&safe=active
• When combined in a 1 to 1
ration, they form table salt
which is a white solid that
dissolves in water.
Sugar (C6H O )
12
6
• What elements are in a molecule of sugar?
“A Compound Problem” Practice
What elements are in the compounds below and in
what ratio? What are the properties of the elements?
Glucose and Fructose (sugar) Molecules
What elements are common is both of these compounds?
How are they different?
Carbohydrate Compounds – the main source of energy for our bodies
What elements are in these molecules? What is a better source of carbohydrates,
simple or complex carbohydrates?
What elements are in a molecule of protein?
In nature, matter is continually recycled.
What elements are in the essential nutrient protein?
Lipids/Fats
What elements are in lipid molecules?
Common Chemicals
Common Name
Chemical Name
Chemical Formula
white vinegar
acetic acid
CH3COOH + H2O
nail polish remover
acetone
CH3COCH3
ammonia
ammonium hydroxide
CH3 + H2O
boric acid
boric acid
H3BO3
marble,limestone,chalk
calcium carbonate
CaCO3
road salt
calcium chloride
CaCl2
garden lime
calcium hydroxide
Ca(OH)2
corn syrup
glucose
C6H12O6 + H2O
epsom salt
magnesium sulfate
MgSO4 + 7H2O
moth balls
naphthalene
C10H8
baking soda
sodium bicarbonate
NaHCO3
table salt
sodium chloride
NaCl
cane sugar
sucrose
C12H22O11
sulfuric acid
sulfuric acid
H2SO4
Review: Molecules & Compounds
1.
2.
2.
A molecule is what you get when any atoms join together.
A
A compound
compound is
is what
what you
you get
get when
when atoms
atoms of
of two
two or
or more
more different
different elements
elements
join together.
join together.
3. All compounds are molecules, but not all molecules are compounds.
3. All compounds are molecules, but not all molecules are compounds.
- Water is a molecule because it is made from atoms that have been
-chemically
Water is acombined.
molecule Itbecause
is made from
atomsthe
thatatoms
have that
been
is also aitcompound
because
chemically
combined.
It issame
also -asome
compound
because
atoms
make
water are
not all the
are oxygen
andthe
some
are that
make
water are not all the same - some are oxygen and some are
hydrogen.
hydrogen.
- Oxygen in the atmosphere is a molecule because it is made from two
atoms of oxygen. It is not a compound because it is made from atoms of
only -one
element
- oxygen.
This type
molecule
is called
a diatomic
Oxygen
in the
atmosphere
is a of
molecule
because
it is
made from two
molecule,
molecule
made
two atoms
of theitsame
type.
atoms ofaoxygen.
It is
not afrom
compound
because
is made
from atoms of
only one element - oxygen. This type of molecule is called a diatomic
molecule, a molecule made from two atoms of the same type.
The Difference Between Compounds and Mixtures
Mixture - A physical blend of two or more substances that are
NOT chemically combined.
Compound - A substance that contains two or more elements
CHEMICALLY combined in a fixed proportion. The elements do
not retain their original properties.
Compound is chemically combined, mixture is not chemically combined.
*Cake would be a compound because all of the ingredients are together to make batter you
cannot see the individual components (eggs, flour, sugar, etc.)
*Trail mix would be a mixture because you can see every individual item (M&M, peanuts,
raisins, pizza, etc.)
“Introduction to Matter”
Mini-poster examples
STC lab activities: “Comparing the Two Mixtures” 1.6
“Separating a Mixture” 1.4
“Filtering a Mixture” 1.2
Mixture
Ways to separate mixtures:
- Filtration (separates large particles from small)
- Evaporation (use boiling point)
- Centrifuge (use density)
- tin + copper = pewter
(more)
-
(less)
- Magnet
- Sifting
- copper + tin = bronze
(more)
(less)
Steel is an alloy of iron, with carbon being the primary alloying element.
The air you breathe is made up of about 21% oxygen, 78% nitrogen, and small
amounts of other gases like argon, carbon dioxide and methane.
Homogenous or Heterogeneous Mixtures… Do you know? 
#1 M & M
#2 Salad
#3 Kool Aid drink
#4 Fruit Loops
#8 Hot Chocolate
#5 Milk
#6 Cake Batter
#7 Chocolate Chip Cookie
#9 Trail Mix
#10 Tap Water
#11 Smoke
#12 Clear Seawater