solid, liquids, and gases their properties and changes
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Solid, Liquids, and Gases
Their properties and changes
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Properties of Solids, Liquids, and Gases
• What are some of the characteristics that distinguish solids, liquids, and gases?
• What is the evidence for each of these properties?
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Property Solid Liquid Gas
Shape
Volume
Compressibility
Space between particles
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Property Solid Liquid Gas
Relative Density
Fluid?
Diffusion rate
Motion of particles(amount and type)
Forces between particles?
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The three states of matter.
Silberberg, Principles of Chemistry
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Gases
• Because gases have so much space between the particles they have properties that are dependent on one another.
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Gas Variables
• Volume (V) - mL, L, kL…• Temperature (T) – oC measured in lab but K
(kelvin) for calculations• Number of particles (n) – moles • Pressure (P) – mmHg, psi…(more to come)
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Pressure
• Force per unit area
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Figure 5.3A mercury barometer
Silberberg, Principles of Chemistry
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Table 5.1 Common Units of Pressure
Atmospheric PressureUnit Scientific Field
chemistryatmosphere(atm) 1 atm*
pascal(Pa); kilopascal(kPa)
1.01325x105Pa; 101.325 kPa
SI unit; physics, chemistry
millimeters of mercury(Hg)
760 mm Hg* chemistry, medicine, biology
torr 760 torr* chemistry
pounds per square inch (psi or lb/in2)
14.7lb/in2 engineering
bar 1.01325 bar meteorology, chemistry, physics
*This is an exact quantity; in calculations, we use as many significant figures as necessary.Silberberg, Principles of Chemistry
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Gas Variable Relationships
• To investigate the relationship between 2 gas variables we need to hold the other 2 constant.
• Constant P - same # of collisions/unit area• Constant V - rigid container• Constant T – thermostat control• Constant n – keep container sealed
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The Relationship Between Pressure and Volume
Silberberg, Principles of Chemistry
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The relationship between the volume and pressure of a gas.
Boyle’s Law
1 1 2 2PV = PV
Silberberg, Principles of Chemistry
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A molecular description the relationship between temperature and volume.
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The relationship between the volume and temperature of a gas.
Charles’s Law
2 2
1 1
V T =
V T
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The relationship between pressure and temperature
•As temperature increases, gas particles move faster and make more collisions. As a result the pressure in the container increases.
•For an aerosol can the pressure may be so great that the seam on the can may give way in an explosion.
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An experiment to study the relationship between the volume and amount of a gas.
V n or V = constant x nThe more gas particles you have the more collisions occur. To keep the pressure the same, the volume has to increase so there is more room for the particles. This is why balloons expand when you blow air into them.
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Solids and Liquids
• Because the particles are so much closer in liquids and solids, there are chances for particles to attract (or repel). This and the mass of the particles are main factors in determining the properties of solids and liquids.
• Some properties are boiling and melting points, surface tension, vapor pressure, and crystalline structure.
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Surface Tension
• Surface tension is the tendency for liquid surface to contract.
• Depends on attractive forces
• Compounds that interfere with the forces and reduce surface tension are called surfactants.
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The molecular basis of surface tension.
hydrogen bondingoccurs in three
dimensions
hydrogen bondingoccurs across the surface
and below the surfacethe net vectorfor attractive
forces is downward
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Shape of water or mercury meniscus in glass.
adhesive forcesstronger
cohesive forces
H2O
capillarity
Hg
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Solids• Solids may have a definite structure and are
called crystalline.
• Solids that have no regular shape are called amorphous.
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The hexagonal structure of ice.
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The striking beauty of crystalline solids.
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portion of a 3-D lattice
The crystal lattice and the unit cell.
lattice point
unit cell
portion of a 2-D lattice
unit cell
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Phase Changes
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Phase Changes
solid liquid gas
melting
freezing
vaporizing
condensing
sublimination
Energy absorbed
Energy released