Starter S-139

1
Starter S-139

• List and describe the four states of matter.

2
States of Matter

• Chapter 13

3
13.1 The Nature of Gases

• Chapter 13

4
13.1 The Nature of Gases

• Kinetic Theory all matter consists of tiny
  particles that are in constant motion
• The particles of a gas are considered to be small
  hard spheres with an insignificant volume
• The motion of the
• particles in a gas is
• rapid, constant, and
• random

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13.1 The Nature of Gases

• Collisions between particles in a gas are
  perfectly elastic.
• -no energy is lost in
• collisions

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13.1 The Nature of Gases

• Gas pressure is caused by the collision of
  particles with the container
• Atmospheric Pressure caused by the collision of
  atoms and molecules in air with objects

PhET Gas
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13.1 The Nature of Gases

• Barometer a device to measure atmospheric
  pressure
• The pressure depends on
• Temperature
• Altitude
• Measured in pascal (Pa)
• very small unit

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13.1 The Nature of Gases

• Units must be converted for problems to work out
• These are equalities, so they can be used to
  create conversion factors

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Starter S-137

• Convert each of the following to kilopascals
• 450 mmHg
• 1045 torr
• 1.29 atm
• 95,000 pa

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13.1 The Nature of Gases

• The Kelvin temperature of a substance is directly
  proportional to the average kinetic energy of the
  particles of the substance

PhET Gas
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13.1 The Nature of Gases

• Notice
• - the average shifts, but there are particles
  with very different temperatures
• - the hotter one has particles with almost no
  energy, just like the colder one
• - this is a
• change in
• kinetic
• energy,
• not speed

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13.2 The Nature of Liquids

• Chapter 13

13
13.2 The Nature of Liquids

• Fluids substances that
• can flow
• gases
• liquids
• Unlike gases, liquids particles
• attracted to
• each other

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13.2 The Nature of Liquids

• Physical properties of a liquid are determined by
• Motion of the particles (due to temperature)
• Attraction among the particles
• The particles are
• closer together
• due to these
• forces

Phase Change
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13.2 The Nature of Liquids

• Vaporization conversion of a liquid to a gas or
  vapor
• Evaporation vaporization on
• the surface of a liquid that is
• not boiling

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13.2 The Nature of Liquids

• During evaporation only molecules with a
  certain minimum kinetic energy escape from the
  liquid
• Evaporation takes
• away the hot (faster) particles and is a
• cooling process

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13.2 The Nature of Liquids

• Vapor Pressure the force exerted by a gas above
  a liquid
• Because of the gas
• produced by evaporation
• Eventually particles leaving the liquid equal the
  particles reentering the liquid

Vapor Pressure
Equilibrium
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13.2 The Nature of Liquids

• The container only reaches equilibrium if it is
  sealed
• Vapor pressure depends on temperature
• at higher temperature the average kinetic energy
  is higher

Vapor Pressure (kPa) Vapor Pressure (kPa) Vapor Pressure (kPa) Vapor Pressure (kPa) Vapor Pressure (kPa) Vapor Pressure (kPa) Vapor Pressure (kPa)
0oC 20oC 40oC 60oC 80oC 100oC
Water 0.61 2.33 7.37 19.92 47.34 101.3
Ethanol 1.63 5.85 18.04 47.02 108.3 225.8
Diethyl ether 24.70 58.96 122.8 230.6 399.1 647.9
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Starter S-139

• 1. What is
• Vaporization
• Boiling
• Evaporation
• Vapor Pressure
• 2. What is the relationship between vapor
  pressure and boiling?

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13.2 The Nature of Liquids

• The vapor pressure shows of volatile a liquid is
• How easily it evaporates

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13.2 The Nature of Liquids

• Boiling when the temperature is high enough,
  that particles throughout the liquid have the
  kinetic energy to vaporize
• Bubbles of vapor form
• throughout the liquid
• Boiling point the point
• where the vapor pressure
• of the liquid is equal to
• the external pressure on the liquid

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13.3 The Nature of Solids

• Chapter 13

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13.3 The Nature of Solids

• Properties of solids are determined by
• Orderly arrangement of their particles
• Fixed locations of their particles
• Melting point temperature at
• which a
• solid
• changes
• into a
• liquid

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13.3 The Nature of Solids

• The melting point and freezing point are the same
  temperature
• The states are at
• equilibrium
• Crystalline Solids the
• particles are arranged
• in crystals
• Crystal orderly 3D
• pattern

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13.3 The Nature of Solids

• Crystal Systems
• Defined by
• 6 Values

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13.3 The Nature of Solids

• Seven Basic Shapes
• Unit Cell the
• smallest group
• of particles that
• has the
• geometric shape
• of the crystal

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13.3 The Nature of Solids

• Allotropes two or more different molecular
  forms of the same element in the same physical
  state
• Carbon
• Diamond
• Graphite
• Soot (buckminsterfullerene)

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13.3 The Nature of Solids

• Amorphous Solid lacks an internal structure
• Rubber
• Plastics
• Glass
• Do not have a
• specific
• melting point
• Shatter into
• random
• shapes

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13.4 Changes of State

• Chapter 13

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13.4 Change of State

• Solid molecules vibrate in place
• Melting Particles increase speed start to move
• Liquid molecules move, but still attracted to
  each other
• Evaporation particles move fast enough to that
  intermolecular forces do not matter

Melting
Phase Change
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13.4 Change of State

• Sublimation solid goes directly to a gas
• Vapor pressure of the solid is greater than
  atmospheric pressure
• Carbon Dioxide (Dry Ice)
• Iodine

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13.4 Change of State

• Phase Diagram shows states (solid, liquid, gas)
  in relation to pressure and temperature

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13.4 Change of State

• Triple Point the point where a solid, liquid,
  and gas state can all exist
• For water that would be 0.61 kPa and 0.016 oC
• Notice An increase in pressure drives most
  substances toward a solid
• An increase in temperature drives substances
  toward a gas

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Starter S-140

• 1. Define
• Crystalline Solid
• Amorphous Solid
• 2. What are the three allotropes
  of carbon?

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Starter S-141

• 1. Define
• Melting
• Boiling
• Freezing
• Evaporation
• Condensation
• Sublimation

36
Starter S-142

• Happy Test Day

37
Starter S-143

• What makes a bottle rocket fly? Be specific and
  discuss the force, the cause of the force, and
  what is doing the pushing or pulling.
• Also discuss why there is a need to put water
  into the bottle.