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Intermolecular ForcesIntermolecular Forces
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Kinetic Molecular TheoryKinetic Molecular Theory
Describes the behavior of subatomic particles• Liquids, solids, and gases are composed of
small particles that have mass. • Particles are in constant, random, rapid motion.• Particles have collisions. • Particles have an avg. KE directly related to
temperature.• The state of a substance at room temperature
depends on the strength of the attractions between its particles.
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Definition of IMFDefinition of IMF
Attractive forces between molecules.
Much weaker than chemical bonds within molecules.
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Definition of IMFDefinition of IMF
Intramolecular forces:
Covalent Bonding
Much stronger than chemical bonds between atoms.
Examples : nonpolar, polar sharing
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Definition of IMFDefinition of IMF
Intermolecular ForcesAttractive forces between molecules.
Much weaker than chemical bonds within molecules.
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Intermolecular ForcesIntermolecular Forces
Attractive forces between molecules or particles (ions, metal atoms, etc…)
Examples:
dispersion, (London /Vander Waals); dipole-dipole, dipole-ion, hydrogen “bonding”, metallic bonding, ion-ion
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Intermolecular ForcesIntermolecular Forces
Relative Strength:
Examples:
dispersion, (London /Vander Waals); dipole-dipole, dipole-ion, hydrogen “bonding”, metallic bonding, ion-ion
Weakest
Strongest
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Types of IMFTypes of IMF
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Types of IMFTypes of IMF
London Dispersion Forces
View animation online.
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Types of IMFTypes of IMF
Dipole-Dipole Forces
+ -
View animation online.
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Types of IMFTypes of IMF
Hydrogen Bonding
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Determining IMFDetermining IMF
NCl3• polar = dispersion, dipole-dipole
CH4
• nonpolar = dispersionHF
• H-F bond = dispersion, dipole-dipole, hydrogen bonding
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Physical PropertiesPhysical Properties
Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
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Liquids vs. SolidsLiquids vs. Solids
LIQUIDS
Stronger than in gases
Y
high
N
slower than in gases
SOLIDS
Very strong
N
high
N
extremely slow
IMF Strength
Fluid
Density
Compressible
Diffusion
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Liquid PropertiesLiquid Properties
Surface Tension• attractive force between particles in a
liquid that minimizes surface area
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Liquid PropertiesLiquid Properties
Capillary Action• attractive force between the surface of
a liquid and the surface of a solid
water mercury
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Types of SolidsTypes of Solids
Crystalline - repeating geometric pattern• covalent network• metallic• ionic• covalent molecular
Amorphous - no geometric pattern
decreasingm.p.
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Types of SolidsTypes of Solids
Ionic(NaCl)
Metallic
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Types of SolidsTypes of Solids
CovalentMolecular
(H2O)
CovalentNetwork
(SiO2 - quartz)
Amorphous(SiO2 - glass)
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Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
Changes of StateChanges of State
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Phase ChangesPhase Changes
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Phase ChangesPhase Changes
EvaporationEvaporation• molecules at the surface gain enough
energy to overcome IMF
VolatilityVolatility• measure of evaporation rate• depends on temp & IMF
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Phase ChangesPhase Changes
Kinetic Energy
# o
f P
art
icle
s
p. 477
Boltzmann Distribution
temp
volatility
IMF
volatility
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Phase ChangesPhase Changes
EquilibriumEquilibrium• trapped molecules reach a balance
between evaporation & condensation
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Phase ChangesPhase Changes
Vapor PressureVapor Pressure• pressure of vapor above
a liquid at equilibrium
IMF v.p.temp v.p.
• depends on temp & IMF• directly related to volatility
p.478
temp
v.p
.
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Phase ChangesPhase Changes
Boiling Point• temp at which v.p. of liquid
equals external pressure
IMF b.p.Patm b.p.
• depends on Patm & IMF
• Normal B.P. - b.p. at 1 atm
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Which has a higher m.p.?• polar or nonpolar?• covalent or ionic?
Phase ChangesPhase Changes
Melting Point• equal to freezing point
polar
ionic
IMF m.p.
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Phase ChangesPhase Changes
Sublimation
• solid gas
• v.p. of solid equals external pressure
EX: dry ice, mothballs, solid air fresheners
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Heating CurvesHeating Curves
Melting - PE
Solid - KE
Liquid - KE
Boiling - PE
Gas - KE
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Heating CurvesHeating Curves
Temperature Change• change in KE (molecular motion) • depends on heat capacity
Heat Capacity• energy required to raise the temp of 1
gram of a substance by 1°C• “Volcano” clip - water has a very high
heat capacity
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Heating CurvesHeating Curves
Phase Change• change in PE (molecular arrangement)• temp remains constant
Heat of Fusion (Hfus)
• energy required to melt 1 gram of a substance at its m.p.
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Heating CurvesHeating Curves
Heat of Vaporization (Hvap)
• energy required to boil 1 gram of a substance at its b.p.
• usually larger than Hfus…why?
EX: sweating, steam burns, the drinking bird
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Phase DiagramsPhase Diagrams
Show the phases of a substance at different temps and pressures.