Matter

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Matter
Chapter 2 Pages 58-81
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Matter

• Anything that has mass and takes up space

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States of matter

• The four states of matter are solids, liquids,
  gasses and plasma.

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Elements

• Cant be broken down into another substance.

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Compound

• Chemical Combination of elements.
• EX H2O?water
• CO2?Carbon Dioxide
• C12H11O22? Sugar
• C6H12O6? Glucose

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Atom

• The smallest particle of an element.

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• ATOMS

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Molecule

• A group of atoms joined together.

chocolate
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MOLECULES
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Chemical Bond

• The force that holds the atoms together.

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Formula

• Ratio of atoms of each element in a compound.

Theobromine, C7H8O4N2 or Chocolate
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Changes in Matter

• Physical Change When the state of matter
  changes.

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Physical Change

• 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.)

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PHYSICAL CHANGES
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Changes in Matter cont

• Chemical Change When a substance(s) combine or
  decompose into a new substance.

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Examples of a chemical change
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)
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Mixture

• When two or more substances are mixed together
  but have different properties.

EX Salt Water
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MIXTURE
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Solution or Homogenous mixture

• As well mixed as possible or when a substance has
  dissolved.

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• SOLUTION

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Pure Substance

• One kind of matter with no substances mixed in.
• EX. Sugar, gold, silver, salt.

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Law of Conservation of Matter

• Matter is neither created nor destroyed during a
  chemical change.
• It recombines to make a new type of chemical.

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• LAW OF CONSERVATION OF MASS

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Please select a Team.

1. Team 1
2. Team 2
3. Team 3
4. Team 4
5. Team 5
6. Team 6
7. Team 7
8. Team 8

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Gatorade would be considered a

1. Homogeneous mixture/ solution
2. Heterogeneous mixture
3. Pure substance

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When Ice melts its a

1. Chemical change only
2. Physical change only
3. Both physical and chemical change

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When you cook eggs its a

1. Chemical change only
2. Physical change only
3. Both physical and chemical change

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Team Scores
4.75 Team 4
4.75 Team 5
4.5 Team 1
4.5 Team 6
4.5 Team 7
4 Team 2
4 Team 3
3.25 Team 8


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H2O, NaCl and CO2 are all considered

1. Atoms
2. Elements
3. Compounds/molecules

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What are the different elements in these three
compounds? H2O, NaCl and CO2

1. H, O, Na, Cl and C
2. H2O, NaCl and CO2

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Which of the following processes involves a
chemical change?

1. Chopping wood
2. Melting plastic
3. Boiling alcohol
4. Digesting Food

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Team Scores
7.75 Team 4
7.75 Team 5
7.5 Team 1
7 Team 2
6.5 Team 7
6 Team 3
6 Team 6
4.75 Team 8


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What causes a liquid to turn into a gas or solid
to turn into a liquid?

1. Force
2. Energy
3. Chemical Bonds

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Stimpson J. Cat stirs a spoonful of Kool-Aid into
a glass of water.As he stirs, the solid powder
dissolves. What type of change is occurring?

1. Chemical Only
2. Physical Only
3. Both

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A chemical change results in

1. changes in state only
2. different substances with different properties
   and possibly a change in state.
3. no new substances

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Team Scores
10.75 Team 4
10.75 Team 5
10.5 Team 1
10 Team 2
9.5 Team 7
9 Team 3
7.75 Team 6
6 Team 8


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Characteristic/Chemical Properties

• Regardless of state of matter, a substance has a
  unique characteristic property.

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Types of characteristic properties

• Boiling Points/Vaporization/ Condensation The
  temperature at which a liquid boils.

Water's boiling point is 100 C
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Melting/Freezing Points

• Temperature at which a solid turns into a liquid
  or a liquid turns into a solid.

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Density

• Every substance has a particular density, no
  matter the amount.

Examples Gold 19.3 g/mL Silver 10.5 g/mL Oxygen
1.14 g/mL Helium 0.126 g/mL
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Intermolecular forces (IMFs)

• These are forces that hold one molecule to
  another.

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Energy and State Change

• When a substance changes state
• Solid? liquid? gas gaining energy
• Gas? liquid? solid loses energy

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Temperature affects state.

• Substances with weak IMFs become liquids and
  gasses at low temperatures.
• In contrast, substances with strong IMFs can
  stay in a solid state even at extreme
  temperatures.

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MATTER AND ENERGY
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http//172.26.64.6/?a3800ch5
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Changes in Matter

• Chapter 3 sections 1 and 3

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Solid

• Definite Shape and Definite Volume.

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Particles in a solid

• Molecules are packed closely together and
  slightly vibrate.

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Types of solids

• Crystalline solid Arranged in a crystal-like,
  repeating pattern.
• All have a distinct melting point.

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Types of solids cont.

• Amorphic Solid Particles are arranged in an
  irregular or random pattern.
• Dont have a distinct melting point.
• Example Glass, plastic, rubber

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Polymers

• Very large molecules made of a chain of smaller
  molecules
• Polymers form when chemical bonds link large
  numbers of monomers in a repeating pattern.

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Polymers and Composites

• The properties of synthetic polymers make them
  ideal starting materials for many common objects.

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Liquids

• Takes the shape of the container that its in.

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Particles in a Liquid

• Atoms and/or molecules are loosely packed
  together and move more freely.

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Suspension

• A mixture where particles can be seen and easily
  separated.
• Examples Milk, salad dressing and muddy water

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Viscosity
The resistance of a liquid to flow. The higher
the viscosity, the slower it will flow. Usually
amorphic solids.
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BILL NYE

• http//172.26.64.6/?a50060ch9
• TIME WARP

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• Surface tension Molecules on the surface are
  only affected by those below the surface, thus
  causing drops of liquid to be spheres.

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• Start video at 513

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Gases

• Have no definite shape and no definite volume.
• Very compressible.

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Particles in a gas

• Particles are not touching, therefore the
  Intermolecular forces are broken.
• Movement is random and independent of each other.

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Boyles Law

• At a constant temperature, if the volume
  decreases then the pressure of a gas increases.

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Graph of Boyles Law
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Pressure and Temperature of gases

• When the temperature of a gas increases its
  pressure increases and when temperature decreases
  pressure decreases.

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Charles' Law

• When temperature of a gas increases its volume
  increases.
• In other words, gases expand as they heat up and
  condense as they cool down.

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Measuring Gases

• Temperature the measure of the motion (kinetic
  energy) of the particles of a substance.

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Measuring Gases Cont

• Pressure of a gas The measure of the outward
  force divided by the surface area of the
  container.

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Please select a Team.

1. Team 1
2. Team 2
3. Team 3
4. Team 4
5. Team 5
6. Team 6
7. Team 7
8. Team 8

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Salad is an example of a

1. Homogeneous Mixture
2. Heterogeneous Mixture

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Pure water is

1. Mixture
2. Pure substance

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Salt water from the ocean is a

1. Pure substance
2. Mixture

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Team Scores
2 Team 1
2 Team 2
2 Team 3
2 Team 6
2 Team 7
2 Team 8
1.75 Team 4
1.5 Team 5


86
Otto stirs a spoon of sugar into a glass of
lemonade and the sugar disappears. What type of
change occurred?

1. Chemical change
2. Destroying matter
3. Physical change

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A chemical change results in..

1. A change in state
2. A different substance with different properties
3. No new substance

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When energy is continually added to a liquid till
the IMFs break in a substance such as water, it
undergoes..

1. Freezing
2. Melting
3. Vaporization (evaporation)

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Team Scores
5 Team 6
4.75 Team 3
4.25 Team 1
4 Team 2
4 Team 4
4 Team 7
4 Team 8
3 Team 5


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Snow melting is a

1. Chemical change
2. Physical change
3. Both a chemical and a physical change

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When molecules increase kinetic energy, the
intermolecular forces holding them together..

1. Increase
2. Decrease
3. Stay the same

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Team Scores
7 Team 6
6.5 Team 3
6 Team 1
6 Team 4
6 Team 8
5.75 Team 2
5.5 Team 7
4.25 Team 5


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Participant Scores
7 Participant 7 7 Participant 26
7 Participant 2 7 Participant 31
7 Participant 9 7 Participant 33
7 Participant 12 6 Participant 6
7 Participant 11 6 Participant 8
7 Participant 14 6 Participant 15
7 Participant 24 6 Participant 4
7 Participant 22 6 Participant 1
7 Participant 21 6 Participant 16
7 Participant 23 6 Participant 25
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Increased Temperature Increased average velocity
of gas particles
Increased Force per collision.
Increased number of collisions with walls of
container
Initial increase in pressure? force area of
container
Inside pressure is greater than external
pressure.
Container expands ? Increased Volume
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Take out your Hot Air Balloons Lab and write down
the Purpose
To Learn how the volume of a gas changes with
temperature.