Matter is anything that has mass and takes up space.
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Elements and Compounds are PURE SUBSTANCES
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A mixture is when two or more substances are mixed together but
not combined chemically
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A mixture retains properties of all original ingredients.
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MIXTURE OR PURE SUBSTANCE?
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NaHCO3 - Sodium Bicarbonate
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MIXTURE OR PURE SUBSTANCE? Soil
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MIXTURE OR PURE SUBSTANCE? Milk
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MIXTURE OR PURE SUBSTANCE? Sugar: C 12 H 22 O 11
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MIXTURE OR PURE SUBSTANCE? Air
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MIXTURE OR PURE SUBSTANCE? Oxygen
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Homogeneous Mixtures are the same throughout.
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Warm-Up: 1. Is H 2 O a _____________. a. Element b. Compound c.
Mixture d. All of the Above 2. Why is tap water considered a
mixture?
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Steel is a homogeneous mixture.
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Heterogeneous Mixtures are not the same throughout.
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4 States of Matter: -Solid -Liquid -Gas -Plasma
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In a gas, molecules are very far apart
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In a liquid, molecules are closer together but still move
around
Slide 22
In a solid, molecules vibrate in place and do not move
around
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Plasmas are gases that are so energized that some of their
electrons have been stripped away
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Gasses and liquids take the shape of their containers, solids
do not.
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Energy must be added to change a solid to a liquid;
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More energy must be added to change a liquid to a gas
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Slide 30
Warm-Up: 1. In which state of matter are the molecules moving
the fastest? 2. In which state of matter are the molecules not
moving around, just vibrating in place? 3. Matter in which two
states takes the shape of its container? 4. To make matter change
from a solid to a liquid, what must happen to the molecules?
Slide 31
WARM-UP: 1. Matter in which two states takes the shape of its
container? 2. To make matter change from a solid to a liquid, what
must happen to the molecules?
Slide 32
WARM-UP: 1. Which state of matter is the most dense? 2. When a
substance changes from a solid to a liquid what is this called? 3.
When a substance changes from a liquid to a gas what is this
called? 4. When a substance changes from a gas to a liquid, what is
this called?
Slide 33
WARM-UP: 1. What is volume? Give two examples of two things
that have different volumes. 2. What makes each element different
from one another? 3. What is atomic number?
Slide 34
1. What are the types of pure substances? 2. What are the types
of mixtures? 3. What is density? Describe two things that have
different densities. 4. What combination of substances retains the
properties of its components?
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5. Give an example of a homogeneous mixture. 6. Give an example
of a heterogeneous mixture. 7. List the phases of matter in
ascending order of density. 8. What must be done to change a gas to
a liquid?
Slide 36
9. What is the phase change called when a solid changes
directly to a gas? 10. Is density a physical or chemical property
of matter? 11. Nitrogen boils at -196 o C. Is this a physical or
chemical property? 12. List these items in order of ascending
density: -a bowling ball a beach ball a penny a hot air balloon in
the air
Slide 37
Physical Properties of matter describe the matters physical
characteristics
Slide 38
Boiling/Melting Points H 2 O = 100 0 C (212 0 F) CO 2 = -57 0 C
(-70 0 F)
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Density is a physical property
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Density = Mass Volume Practice: A material has a mass of 100g
and a volume of 10 cm 3. Calculate the density.
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Others include: -Thermal Conductivity
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-Malleability (ability to be pounded into thin sheets)
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-Ductility (ability to be drawn into a thin wire)
Slide 44
Chemical Properties describe how a substance reacts chemically
with another substance
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In a chemical reaction, you always get a new substance.
Slide 46
Law of Conservation of Matter/Mass: Matter can never be created
or destroyed
Slide 47
Warm-Up: 1. Find the density of an object with a mass of 40g
and a volume of 5 cubic cm. 2. Find the mass of a sample of a
substance with a density of 5 g/ml and a volume of 2 ml 3. List
three physical properties of H 2 O
Slide 48
Solutions: S o l u t i o n s - A homogeneous mixture composed
of only one phase
Slide 49
Solutions: S o l v e n t - the most abundant substance in a
solution. The solvent dissolves the solute. S o l u t e - the least
abundant substance in a solution. The solute dissolves into the
solvent. In a sugar water solution, water is the solvent &
sugar is the solute. In steel (a solution which becomes a solid)
iron is the solvent and carbon is the solute Air is a solution
Slide 50
Solutions Homogeneous mixture Homogeneous mixture Mixed
molecule by molecule Mixed molecule by molecule Can occur between
any state of matter. Can occur between any state of matter. Solid
in liquid- Kool-aid Liquid in liquid- antifreeze Gas in gas- air
Solid in solid - brass Liquid in gas- water vapor
Slide 51
Concentration of Solution Shows level of solute in the solvent
Can be Expressed in several ways Relative Concentrations Dilute
small amounts of solute compared to solvent Concentrated large
amounts of solute compared to solvent Levels of Concentration
Unsaturated solution is able to dissolve more solute Saturated
solution has dissolved the maximum amount of solute Supersaturated
solution has dissolved excess solute (at a higher temperature).
Solid crystals generally form when this solution is cooled.
Slide 52
Percent Composition (by mass) We can consider percent by mass
(or weight percent, as it is sometimes called) in two ways: The
parts of solute per 100 parts of solution. The fraction of a solute
in a solution multiplied by 100. We need two pieces of information
to calculate the percent by mass of a solute in a solution: The
mass of the solute in the solution. The mass of the solution. Use
the following equation to calculate percent by mass: (Write the
equation)
Slide 53
Rate of Dissolving
Slide 54
Factors Affecting How Fast a Solute Dissolves
Slide 55
1. Temperature If we heat particles they will move faster The
solvent will carry the solute particles away faster Hotter =
Dissolve Faster
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2. Agitating Stirring or shaking a solution moves the solute
particles around so that they are closer to the solvent. The
solvent particles can then attract them easily and carry them away!
Stir or Shake = Dissolve Faster
Slide 57
3. Crushing (More Surface Area) When a solute is broken into
small pieces, the individual particles can get closer to solvent
particles so they can be easily dissolved So smaller pieces=
dissolves faster
Slide 58
Dissolving happens on the surface of particles When solute is
broken up, there is more surface area where dissolving can occur
broken up
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4. Pressure Pressure forces solute particles into the spaces
between the solvent particles More pressure = Dissolve Faster
gas
Slide 60
Warm-Up 1.Find the density of a bowling ball with a mass of
6,000 g and a volume of 300 ml. 2. Find the mass of an object with
a density of 20 g/ml and a volume of 100 ml.
Slide 61
Types of Chemical Reactions Synthesis reactions occur when two
elements combine and form a compound. (Sometimes these are called
combination or addition reactions.) reactant + reactant 1 product
Basically: A + B AB Example: 2H 2 + O 2 2H 2 O Example: C + O 2 CO
2
Slide 62
Practice Predict the products. Write and balance the following
synthesis reaction equations. Sodium metal reacts with chlorine gas
Na + Cl 2 Solid Magnesium reacts with fluorine gas Mg + F 2
Aluminum metal reacts with fluorine gas Al + F 2
Slide 63
Decomposition reactions occur when a compound breaks up into
the elements or in simpler compounds 1 Reactant Product + Product
In general: AB A + B Example: 2 H 2 O 2H 2 + O 2 Example: 2 HgO 2Hg
+ O 2
Slide 64
Practice Predict the products. Then, write and balance the
following decomposition reaction equations: Solid Lead (IV) oxide
decomposes PbO 2( Aluminum nitride decomposes AlN
Slide 65
Practice Identify the type of reaction for each of the
following synthesis or decomposition reactions, and write the
balanced equation: N 2 + O 2 BaCO 3 Co + S NH 3 + H 2 CO 3 NI
3
Slide 66
Single Replacement Reactions occur when one element replaces
another in a compound. element + compound element + compound A + BC
AC + B (if A is a metal) OR A + BC BA + C (if A is a nonmetal)
Slide 67
Double Replacement Reactions occur when a metal replaces a
metal in a compound and a nonmetal replaces a nonmetal in a
compound Compound + compound compound + compound AB + CD AD +
CB
Slide 68
Combustion reactions occur when a hydrocarbon reacts with
oxygen gas. This is also called burning!!! In order to burn
something you need the 3 things in the fire triangle : 1) A Fuel
(hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the
reaction (spark)
Slide 69
Combustion Reactions In general: C x H y + O 2 CO 2 + H 2 O
Products in combustion are ALWAYS carbon dioxide and water.
(although incomplete burning does cause some by-products like
carbon monoxide) Combustion is used to heat homes and run
automobiles (octane, as in gasoline, is C 8 H 18 )
Slide 70
Combustion Reactions Edgar Allen Poes drooping eyes and mouth
are potential signs of CO poisoning.
Slide 71
Combustion Example C 5 H 12 + O 2 CO 2 + H 2 O Write the
products and balance the following combustion reaction: C 10 H 22 +
O 2 5 6 8
Slide 72
Practice Identify the type of reaction for each of the
following synthesis or decomposition reactions, and write the
balanced equation: N 2 + O 2 BaCO 3 Co + S NH 3 + H 2 CO 3 NI
3
Slide 73
Warm-Up: State the type of reaction and predict the products:
1.BaCl 2 + H 2 SO 4 2.C 6 H 12 + O 2 3.Zn + CuSO 4 4.Cs + Br 2
5.FeCO 3
Slide 74
Warm-Up: In one paragraph, explain why a glass of ice water
forms droplets of water on the outside of the glass. Use the
following terms: -temperature -molecules -decrease
Slide 75
Warm-Up: 1. What does CO 2 (dry ice) do at room temperature? 2.
Name a physical property of charcoal. 3. Name a chemical property
of charcoal.
Slide 76
Warm-Up: 1. What is the change of state called when matter goes
from a solid directly to a gas? 2. What are some ways to make a
substance dissolve faster? 3. If a solvent cannot dissolve any more
of the solute, what is this called?
Slide 77
Warm-Up: As you sit by the fireplace, your little brother says
we need to add more wood to the fire because these logs have almost
disappeared the fire has destroyed them. How would you respond to
your brother? Explain.
Slide 78
1. Find the area of a section of carpet that is 10 m wide and
12 m long. 2. Find the area of a roof that is 15 m wide and 20 m
long. 3. Find the area of a county that is shaped like a square
with boundaries that are 30 km by 30 km.
Slide 79
Warm-Up: 1. What is the difference between a physical change
and a chemical change? 2. What are some clues that a chemical
change/reaction has taken place?
Slide 80
Warm-Up: 1. List three physical properties of matter. 2.
Describe a chemical change.
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2 11 12 14 16 33 34 36 43 44
Slide 82
Warm-Up: 1. What is volume? 2. What is density?
Slide 83
Warm-Up: 1. What is volume? 2. What is density? 3. What is the
difference between a physical change and a chemical change? 4. What
are some clues that a chemical change/reaction has taken
place?
Slide 84
Warm-up Understanding Density In class today, we are going to
make a density column. Predict what order these liquids will settle
into if they are poured into the same cylinder: Water Alcohol Dawn
dish soap Vegetable oil Syrup Milk (whole)
Slide 85
SubstanceMass (g)Volume (mL)Density g/mL water alcohol Syrup
Vegetable oil Milk (whole) Fill out this chart on page 39 of your
notebook. You have 4 minutes.
Slide 86
Pure Substances Elements Compounds Homogeneous MATTER
Heterogeneous Mixtures Solute Solution SolventExamples:
Slide 87
Pure Substances Made of one type of matter Elements Made of one
type of atom Compounds Made of 2 or More atoms bonded together
Homogeneous Smooth; consistent MATTER Made of Atoms Has Mass &
takes up Space Heterogeneous Chunky; inconsistent Mixtures Made of
more than one type of matter Solute The stuff that is dissolved In
the liquid Ex: Kool-Aid mix Atom + Atom = Element Atom + Atom =
Molecule Solution Homogeneous; All one phase Ex: Kool-Aid Solvent
The liquid that forms the solution Ex: Water Examples: Trail Mix
Salad
Slide 88
Characteristics Physical Properties Chemical Properties Changes
of State Signs of Change Chemical Reactions Examples States
Properties of Matter
Slide 89
Characteristics Color Shape Size Texture Mass Volume Density
Physical Properties Describe a Substance Changes of State Melting
Freezing Boiling Condensation Ionization Relaxation States Solid
Liquid Gas Plasma Properties of Matter Chemical Properties Describe
how it can form a new substance Signs of Change Odor Change in Temp
Change in Color Bubbles form Solids form Chemical Reactions Atoms
in two substances combine to form new substances Examples Burning
Rusting Rotting Tarnishing Examples 2Na+Cl 2 2NaCl 2H 2 +O 2 2H 2
O
Slide 90
Solid _____Energy Atoms ______stuck together Liquid
____________Energy Atoms __________stuck together Gas ______Energy
Atoms _____stuck together Plasma ________Energy Atoms ____stuck
together _____________ _________ __________ ____________ __________
____________ _________Point _______Point ______Point _________Point
States of Matter Temperature
Slide 91
Solid Low Energy Atoms tightly stuck together Liquid Medium
Energy Atoms loosely stuck together Gas High Energy Atoms not stuck
together Plasma Highest Energy Atoms not stuck together Freezing
Melting Relaxation Condensation Ionization Evaporation _Melting
Point Boiling Point Dew Point Freezing Point States of Matter
Temperature
Slide 92
Match the Columns 1.Molecule____ 2.Element ____ 3.Compound ____
4.Volume ____ 5.Mixture ____ 6.Atom ____ 7.Mass ____ 8.Matter ____
A.Amount of matter in an object B.The smallest building block of
matter C.2 or more atoms combined together D.The amount of space an
object occupies E.Is made of atoms F.A substance with only 1 type
of atom G.A substance with 2 or more atoms bound together H.A
combination of different substances which retain their individual
properties
Slide 93
Match the Columns_Answers 1.Molecule__C__ 2.Element __F__
3.Compound _G__ 4.Volume _D___ 5.Mixture __H__ 6.Atom __B__ 7.Mass
__A__ 8.Matter __E__ A.Amount of matter in an object B.The smallest
building block of matter C.2 or more atoms combined together D.The
amount of space an object occupies E.Is made of atoms F.A substance
with only 1 type of atom G.A substance with 2 or more atoms bound
together H.A combination of different substances which retain their
individual properties