liquids & solids i. intermolecular forces. a. definition of imf attractive forces between...
TRANSCRIPT
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Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
I. Intermolecular Forces
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A. Definition of IMFA. Definition of IMF
Attractive forces between molecules.
Much weaker than chemical bonds within molecules.
a.k.a. van der Waals forces
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B. Types of IMFB. Types of IMF
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B. Types of IMFB. Types of IMF
London Dispersion Forces
View animation online.
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B. Types of IMFB. Types of IMF
Dipole-Dipole Forces
+ -
View animation online.
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B. Types of IMFB. Types of IMF
Hydrogen Bonding
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C. Determining IMFC. Determining IMF
NCl3• polar = dispersion, dipole-dipole
CH4
• nonpolar = dispersionHF
• H-F bond = dispersion, dipole-dipole, hydrogen bonding
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II. Physical Properties
Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
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A. Liquids vs. SolidsA. Liquids 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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B. Liquid PropertiesB. Liquid Properties
Surface Tension• attractive force between particles in a
liquid that minimizes surface area
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B. Liquid PropertiesB. Liquid Properties
Capillary Action• attractive force between the surface of
a liquid and the surface of a solid
water mercury
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C. Types of SolidsC. Types of Solids
Crystalline - repeating geometric pattern• covalent network• metallic• ionic• covalent molecular
Amorphous - no geometric pattern
decreasingm.p.
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C. Types of SolidsC. Types of Solids
Ionic(NaCl)
Metallic
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C. Types of SolidsC. Types of Solids
CovalentMolecular
(H2O)
CovalentNetwork
(SiO2 - quartz)
Amorphous(SiO2 - glass)
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Ch. 12 - Liquids & SolidsCh. 12 - Liquids & SolidsCh. 12 - Liquids & SolidsCh. 12 - Liquids & Solids
III. Changes of State
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A. Phase ChangesA. Phase Changes
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A. Phase ChangesA. Phase 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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A. Phase ChangesA. Phase Changes
Kinetic Energy
# o
f P
art
icle
s
p. 477
Boltzmann Distribution
temp
volatility
IMF
volatility
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A. Phase ChangesA. Phase Changes
EquilibriumEquilibrium• trapped molecules reach a balance
between evaporation & condensation
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A. Phase ChangesA. Phase 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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A. Phase ChangesA. Phase 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?
A. Phase ChangesA. Phase Changes
Melting Point• equal to freezing point
polar
ionic
IMF m.p.
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A. Phase ChangesA. Phase Changes
Sublimation
• solid gas
• v.p. of solid equals external pressure
EX: dry ice, mothballs, solid air fresheners
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Heating Curves
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A. Heating CurvesA. Heating Curves
Melting - PE
Solid - KE
Liquid - KE
Boiling - PE
Gas - KE
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A. Heating CurvesA. Heating 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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A. Heating CurvesA. Heating 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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A. Heating CurvesA. Heating 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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B. Phase DiagramsB. Phase Diagrams
Show the phases of a substance at different temps and pressures.