1. Chapter 13 States of Matter Gases, Liquids and Solids
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2. Figure 10.1 Schematic Representations of the Three States of Matter
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GASES
INDIVIDUAL MOLECULES FAR APART
PARTICLES INTERACTING VERY LITTLE
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SOLIDS
MOLECULES ARE VIRTUALLY LOCKED IN PLACE
CAN VIBRATE ABOUT THEIR POSITIONS
VERY ORGANIZED
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LIQUIDS
MOTION OF MOLECULES IS INCREASE
GREATER MOVEMENT
GREATER DISORDER
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6. Kinetic Molecular Theory
Postulates
A gas consists of a collection of small particles traveling in straight-line motion and obeying Newton's Laws.
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Postulates
The molecules in a gas occupy no volume (that is, they are points).
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Postulates
Collisions between molecules are perfectly elastic (that is, no energy is gained or lost during the collision).
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Postulates
There are no attractive or repulsive forces between the molecules.
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Postulates
The average kinetic energy of a molecule is
3/2 kT
T is the absolute temperature.
k is a constant
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Liquids
Particles in a liquid are attracted to each other.
More dense than gases
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13. Some Properties of a Liquid
Surface Tension: The resistance to an increase in its surface area (polar molecules).
Capillary Action: Spontaneous rising of a liquid in a narrow tube.
Viscosity: Resistance to flow (molecules with large intermolecular forces).
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Liquids
Conversion of a liquid to a gas is called vaporization.
Evaporation versus Boiling?
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Surface Tension
UNEVEN PULL OF MOLECULES AT THE SURFACE
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16. Figure 10.6 Molecules in a Liquid
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Liquids
Vapor Pressure:
Measure of the force exerted by a gas above a liquid.
Increasing Temperature increases vapor pressure.
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Solids
Generally described as
an orderly arrangement of particles
in fixed positions.
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Types of Solids
Crystalline Solids: highly regular arrangement of their components
Amorphous solids: considerable disorder in their structures (glass).
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Crystalline Solid
Lattice: A 3-D system of points designating the centers of components that make up the substance.
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Unit Cell
Smallest repeating unit of the lattice.
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Crystalline Solid
Unit Cell: The smallest repeating unit of the lattice.
Three common types:
simple cubic
body-centered cubic
face-centered cubic
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23. Figure 10.9 Three Cubic Unit Cells and the Corresponding Lattices
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24. Figure 10.12 Examples of Three Types of Crystalline Solids
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Allotropes
Two or more different forms of the same element in the same physical state.
Allotropes of carbon: diamond, graphite and buckminsterfullerene
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Diamond
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Graphite
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28. Buckminsterfullerene
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To answer that
we need to know more
about
Gas Pressure.
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Pressure
Pressure
Force per unit area
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32. The gas molecules are in constant motion, and so
Gases.
The gas molecules are in constant motion, and so
they regularly hit the walls of the container.
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33. The force of the gas molecules hitting the walls
Gases.
The force of the gas molecules hitting the walls
of the container is called the Gas Pressure.
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34. The more gas molecules there are, the more often the
Gases.
The more gas molecules there are, the more often the
walls of the container are hit,
therefore the Gas Pressure is higher.
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35. If the temperature (energy) of the gas is increased
Gases.
If the temperature (energy) of the gas is increased
the molecules move faster and so hit the walls harder
causing the Gas Pressure to rise also.
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Measuring Pressure.
Vacuum.
Vacuum.
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Measuring Pressure.
Vacuum.
Gas Pressure.
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Measuring Pressure.
Vacuum.
Gas Pressure.
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Measuring Pressure.
Vacuum.
Gas Pressure.
Manometer.
Pressure is enough to push 20 cm/H2O………or 10 mm/Hg……..
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Atmosphere is
a gas (Air).
Air molecules
hit the surface of
the earth.
Space
is a vacuum.
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Atmospheric Pressure
Pressure of the Air
molecules hitting
the earth.
(or any other surface
in the atmosphere).
14 lbs. per square inch
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Atmospheric Pressure.
Patm = 760 mm/Hg (compared to a vacuum).
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44. We are so accustomed to Atmospheric Pressure that we forget its there.
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Atmospheric Pressure =
Weight of the Air
Results from the mass of the air being
pulled toward the center of the
earth by GRAVITY.
Measures using a barometer.
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46. Figure 5.2 A Torricellian Barometer
At sea level =
760 mm Hg
At elevation of
9600 feet =
520 mm Hg
Figure 5.2 A Torricellian Barometer
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Pressure
is equal to force/unit area
SI units = Newton/meter2 = 1 Pascal (Pa)
1 standard atmosphere = 101,325 Pa
1 standard atmosphere = 1 atm =
760 mm Hg = 760 torr
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Pressure Units
1 atmosphere (atm)
= 760 mm Hg
= 760 torr
= 101,325 Pa
= inch Hg
= lb/ in2 (psi)
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CHANGES OF STATE
(PHASE TRANSISTIONS)
1) MELTING: s  l
2) FREEZING: l  s
3) VAPORIZATION: l  g
4) SUBLIMATION: s  g
CONDENSATION:
LIQUEFACTION: g  l
DEPOSITION: g  s
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PHASE DIAGRAMS
GRAPHICAL WAY TO SUMMARIZE THE PHASES OF A SUBSTANCE AS A FUNCTION OF TEMPERATURE ANE PRESSURE
DIAGRAMS NOT DRAWN TO SCALE
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51. The Phase Diagram for Water
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52. Figure 10.52 The Phase Diagram for Carbon Dioxide
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TRIPLE POINT
REPRESENTS TEMPERATURE AND PRESSURE AT WHICH 3 PHASES OF A SUBSTANCE COEXIST IN EQUILIBRIUM
FOR WATER,
0.016 °C, atm (0.61 kPa).
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CRITICAL POINT
CRITCAL TEMPERATURE: TEMPERATURE ABOVE WHICH THE VAPOR CANNOT BE LIQUEFIED NO MATTER WHAT PRESSURE IS APPLIED
CRITICAL PRESSURE: VAPOR PRESSURE AT THE CRITICAL TEMPERATURE
WATER: 374°C, 218 atm.
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