Classification of Matter

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Classification of Matter

• Unit 2

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Which of the following are examples of matter?

1. Rock
2. Water
3. Carbon dioxide
4. 1 2 only
5. All of the above

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What criteria must be met in order to be matter?

• Is Gas Matter?
• What about Helium ?

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Investigation

• Without bumping the table, add 1 drop of food
  coloring to your hot water and 1 drop to your
  cold water. Observe carefully for 1 minute.
• Write down your observations, then look again at
  your beakers and make any further observations
• What do you think is different about the hot and
  cold water that caused this difference?

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How many phases of matter exist?

1. One
2. Two
3. Three
4. Four

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• PHASES OF MATTER
• Matter exists in four States (or Phases)
• Solid
• Liquid
• Gas
• Plasma

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Solids.

• are packed tightly together in an organized
  pattern
• have a definite shape and volume
• Particles do not move much, but vibrate in place

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Liquids.

• Particles move freely over one another in an
  unorganized pattern
• Do NOT have definite shape - take shape of
  container
• DO have a definite volume
• Particles stay in close contact with each other,
  but usually less dense than solid

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What do you think will happen when the solid is
dropped in to the liquid?
Solid Methanol

1. It will Float
2. It will Sink
3. It will hang midway

Liquid Methanol
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We would expect the solid to sink because the
particles are more closely packed in a solid than
liquid
Solid Methanol


Can you think of an exception to this trend?
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Water Exception to the Rule
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Liquids.

• Do NOT have definite shape - take shape of
  container
• DO have a definite volume (can not be compressed)
• Particles stay in close contact with each other,
  but usually less dense than solid
• Particles freely move over one another in an
  unorganized pattern

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Gases.

• Gas does have mass
• Particles are very spread out and move a lot
• Do NOT have definite shape - take shape of
  container
• Do NOT have a definite volume - fill volume of
  container. Can be compressed (volume can be made
  smaller)
• Collisions of particles with wall causes Pressure

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Animation of Phase Changes
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Factors affecting Volume of Gas

• Change in temperature will change volume.
• An increase in temperature will cause an _______
  in volume of a gas
• Charles Law V1/T1 V2/T2
• Change in pressure will change volume
• An increase in the outside pressure will cause
  a(n) _________ in the volume of a gas.
• Boyles Law P1V1 P2V2

increase
Is this a direct or inverse relationship?
decrease
Is this a direct or inverse relationship?
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What are two ways to increase the pressure in a
basketball?

• Increase the Amount of Gas
• more gas particles means more collisions
• Increase the Temperature
• Particles move faster, means more collisions
• Faster moving particles mean collisions have more
  force

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Pressure vs Temperature

• At a fixed volume, changing temperature will
  affect the pressure

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Pressure vs Temperature

• At a fixed volume, changing temperature will
  affect the pressure
• An increase in temperature will cause a(n)
  _________ in pressure
• P1/T1P2/T2
• Finish this sentence Increasing the temperature
  of a gas at fixed volume will cause an increase
  in pressure because.

increase
Is this a direct or inverse relationship?
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Back to our colored water investigation

• Lets share our observations
• Write a new explanation to explain why the
  coloring behaved differently
• What was different about your original
  explanation and your new explanation?

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Units of Temperature Air Pressure

• When using gas law formulas, all Temperatures
  must be in Kelvin
• Kelvin C 273
• Example Room Temp of 25C 273 298K
• Units of Standard Air Pressure
• 1.00 Atmosphere (atm)
• 760 millimeters of mercury (mm Hg)
• 101,325 Pascals (Pa)
• 29.92 inches of mercury (in Hg)
• 14.70 psi

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If the air pressure today is 29.32in Hg what is
the pressure in mm Hg?

1. 22,280 mmHg
2. 25.92 mmHg
3. 744.8 mmHg
4. 755.3 mmHg
5. 775.6 mmHg
6. 1.15 mmHg

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Which of the following is not true of gases?

1. They have mass
2. They exert pressure
3. They have a definite volume
4. They have large distance between particles.

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Which of the following will not cause an increase
in pressure?

1. Adding more gas
2. Lowering the temperature
3. Reducing the volume the gas occupies

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A gas initially at 2.0 atm is in an adjustable
volume container of 10. L in volume. If the
outside pressure is increased to 4.0 atm, what is
the new volume?

1. 40.L
2. 20.L
3. 10.L
4. 5.0L

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Assuming pressure is held constant, to what
volume will a balloon initially at 1.0 L change
if its temperature is decreased from 300 K to 75
K?

1. 1.0 L
2. 2.0 L
3. 4.0 L
4. 0.25 L
5. 0.50 L

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• Almost all substances can exist as solids,
  liquids, or gases
• The phase will depend on the temperature,
  pressure, and attractive forces of particles
• As substance gains kinetic energy (Temperature),
  it will change phases
• Solid --gt Liquid --gt Gas --gt Plasma

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Phase Changes
MELTING

• Solid Liquid
• Liquid Gas
• Solid Gas

FREEZING
EVAPORATION
CONDENSATION
SUBLIMATION
DEPOSITION
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• SUBLIMATION A phase change that skips the
  liquid state.

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Learning Check True or False
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All substances can exist in all 3 states

1. True
2. False

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The faster gas particles are moving, the more
pressure they will exert.

1. True
2. False

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Water always boils at 100 degrees C

1. True
2. False

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Liquids and solids both have a definite volume

1. True
2. False

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All three phases expand or contract with changes
in temperature

1. True
2. False

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Warm-Up
Gas Law Info V1P1V2P2 V1/T1 V2/T2 P1/T1
P2/T2

• A basketball is inflated to a pressure of 465.4
  mm Hg at a temperature of 298K. If the
  basketball can withstand a pressure 195.3 kPa
  before it bursts, what temperature would we need
  to heat it up to before it blows up? (Assume the
  volume of the basketball does not change after it
  was inflated). Put your answer in ?C.

Standard Air Pressures 760.0 mm Hg 1.000
atm 101,325 Pa
Temperature TK TC 273
Answer on next slide
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Warm-Up
Gas Law Info V1P1V2P2 V1/T1 V2/T2 P1/T1
P2/T2

• Answer 938 K or 665 ? C

Standard Air Pressures 760.0 mm Hg 1.000
atm 101,325 Pa
Temperature TK TC 273
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Time to Investigate Properties of Gases

• Gas Stations Lab
• Boyles Law Graphing POGIL

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Element, Compounds, Mix

• Warm-Up
• Read Page 77 in text and complete Sections 1,2,
  4 on page 3 of Unit 2 Packet.

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Elements
Silver Oxygen Carbon

• Homogeneous
• Made of only 1 type of atom
• Simplest form of matter
• Cant be broken down
• Pure Substance

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Compounds
Water Salt Sugar

• H2O
• NaCl
• C12H22O11

• Homogeneous
• 2 or more types of atoms Chemically Bonded

• Made of only 1 type of Molecule
• Pure Substance
• Can be separated chemically, not physically
• Each substance gains new identity (ex NaCl)
• Has a definite ratio

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Mixtures
Chex Mix Chili Kool Aid

• Can appear heterogeneous or homogeneous
  (solutions are homogeneous mixtures)
• 2 or more types of atoms/molec. Physically
  Blended -- see pic of all three.
• Impure substance
• Can be separated physically
• Ratio of components not exact
• Each Substance maintains its identity

No Magic
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Your Turn Which of the following pictures
represent

1. Pure Elements
2. Elements made of single atoms
3. Elements made of molecules
4. Mixtures
5. Pure Compounds
6. Mixture of 2 compounds
7. Mixture of 2 elements

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Types of Homogeneous MixturesSolutions

• A True Homogeneous mixture
• All particles are broken down into individual
  molecules or ions
• A beam will light will pass straight through,
  with no dispersion.
• Examples Saltwater, Kool-Aid

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Types of Homogeneous MixturesColloidal
Suspensions (Colloid)

• Appear Homogeneous
• Breaks down into small clumps of molecules, but
  not into individual molecules
• Examples mayonnaise, Jell-O, fog, butter and
  whipped cream
• Tyndall Effect will scatter a beam of light
  passed through it. (Ex. Light reflecting off dust
  in the air)

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Distinguishing Colloids from Solutions The
Tyndall Effect
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Types of Colloids
Dispersing Medium Dispersed Phase Name Examples
Gas Liquid Aerosol
Gas Solid Solid Aerosol
Liquid Gas Foam
Liquid Liquid Emulsion
Liquid Solid Sol
Solid Gas Solid Foam
Solid Liquid Gel
Solid Solid Solid Sol
Fog, mist
Smoke
Whipped Cream
Mayonnaise
Latex paint
Styrofoam
Jelly, butter
Alloys (steel)
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Classification of Matter
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• Example putting iron and sulfur together.

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• SECTION 15-4
• PHYSICAL AND CHEMICAL CHANGES

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• In a physical change, substances change form but
  not their identities. In a chemical change,
  substances change into other substances.
• CHANGES OF STATE and DISSOLVING are examples of
  PHYSICAL changes. In both cases, the substances
  retain identity.

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Signs of a Chemical Reaction

• Observing any one of the following is an
  indication that a Chemical Rxn is occurring
• Change in Color
• Bubbling (a gas is being produced)
• Formation of a Precipitate
• Change in Temperature

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METALS vs NONMETALS

• Shiny Luster
• Malleable
• Ductile
• Conduct Electricity
• On left side of staircase of Pd Table

• Dull, glassy luster
• Brittle
• Do not conduct electricity
• On right side of staircase of Pd Table

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Return to Comparison of Metals and NonMetals
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Common Methods of Separation

• Filtration
• Distillation
• Crystallization
• Chromatography
• Extraction by Separatory Funnel
• Centrifugation
• Electrolysis

Physical
Chemical
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Household Centrifuge
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Centrifuge
Useful for quickly separating substances with
different densities
Examples Pulp out of OJ Fats out of Milk
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Extraction by Separatory Funnel
Can be used to separate liquids that do not mix
together
Liquid A
Liquid B
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Distillation
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Atom

• The smallest piece of an element that still
  retains the properties of that element.

Return to Elements
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Molecule

• The smallest part of a compound that still
  retains the properties of the compound.
• Made of two or more atoms bonded chemically

Return to Compounds
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Classification of Matter
Impure Substance
Pure Substances
Back to Mixtures