phases of matter liquids, solids (crystals) & solutions colligative properties
DESCRIPTION
Intermolecular Forces I. Phases of Matter Liquids, Solids (Crystals) & Solutions Colligative Properties. Dr. Ron Rusay. Intermolecular Forces: Phases of Matter & Colligative Properties. Changes of State Phase transitions Phase Diagrams Liquid State - PowerPoint PPT PresentationTRANSCRIPT
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Phases of Matter Liquids, Solids (Crystals) & Solutions
Colligative Properties
Dr. Ron Rusay
Intermolecular Forces I
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• Changes of State– Phase transitions– Phase Diagrams
• Liquid State– Pure substances and colligative properties of solutions,
which depend upon the ratio of the number of solute particles to the number of solvent molecules in a solution. They are independent of the nature of the solute particles.
Intermolecular Forces: Phases of Matter & Colligative Properties
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Solid StateClassification of Solids by Type of Attraction between UnitsCrystalline solids; crystal lattices and unit cellsStructures of some crystalline solidsDetermining the Crystal Structure by X-ray Diffraction
Intermolecular Forces: Phases of Matter
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Phase Transitions• Melting: change of a solid to a
liquid.
• Freezing: change a liquid to a solid.
• Vaporization: change of a solid or liquid to a gas. Change of solid to vapor often called Sublimation.
• Condensation: change of a gas to a liquid or solid. Change of a gas to a solid often called Deposition.
H2O(s) H2O(l)
H2O(l) H2O(s)
H2O(l) H2O(g)
H2O(s) H2O(g)
H2O(g) H2O(l)
H2O(g) H2O(s)
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Phases of Matter / Intermolecular Forces
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Phase Changes
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QUESTION
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Bonds vs. Intermolecular Forces
16 kJ/mol
431 kJ/mol
(150 - 1000 kJ/mol) (Ionic bond 700-4,000 kJ/mol)
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Ion-Dipole Forces (40-600 kJ/mol)• Interaction between an ion and a dipole (e.g. NaOH and
water = 44 kJ/mol)• Strongest of all intermolecular forces.
Intermolecular Forces
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Dipole-Dipole Forces
(permanent dipoles)
Intermolecular Forces
5-25 kJ/mol
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Dipole-Dipole Forces
Intermolecular Forces
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London or Dispersion Forces• An instantaneous dipole can induce another dipole in an
adjacent molecule (or atom).• The forces between instantaneous dipoles are called
London or Dispersion forces ( 0.05-40 kJ/mol).
Intermolecular Forces
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London Dispersion Forces
Intermolecular Forces
Which has the higherattractive force?
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London Dispersion Forces
Intermolecular Forces
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Gecko: toe, setae, spatulae6000x Magnification
http://micro.magnet.fsu.edu/primer/java/electronmicroscopy/magnify1/index.html
Geim, Nature Materials (2003) Glue-free Adhesive100 x 10 6 hairs/cm2
Full et. al., Nature (2000)5,000 setae / mm2
600x frictional force; 10-7 Newtons per seta
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Boiling Points &
Hydrogen Bonding
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Boiling Points &
Hydrogen Bonding
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Hydrogen Bonding
• Hydrogen bonds, a unique dipole-dipole (10-40 kJ/mol).
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Fig. 1 STM and AFM measurements
J Zhang et al. Science 2013;342:611-614
Published by AAAS
Visualizing IntermolecularHydrogen Bonds
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(Left) Fig. 2 AFM measurements of 8-hq assembled clusters on Cu(111)(Right) Fig. 4 AFM measurements of coordination complexes
J Zhang et al. Science 2013;342:611-614
Visualizing IntermolecularHydrogen Bonds
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Which pure substances will not form hydrogen bonds?
I) CH3CH2OH II) CH3OCH3
III) H3C−NH−CH3 IV) CH3F
A) I and II B) I and III C) II and III D) II and IV
QUESTION
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Hydrogen Bonding
Intermolecular Forces
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DNA: Size, Shape & Self Assemblyhttp://www.umass.edu/microbio/chime/beta/pe_alpha/atlas/atlas.htm
Views & Algorithms
10.85 Å10.85 Å
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Intermolecular Forces
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Protein Shape: Forces, Bonds, Self Assembly,Folding
10-40kJ/mol
700-4,000kJ/mol
150-1000kJ/mol
0.05-40kJ/mol
Ion-dipole(Dissolving)40-600kJ/mol
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Predict which liquid will have the strongest intermolecular forces of attraction (neglect the small differences in molar masses).
A) CH3COCH2CH2CH3 (molar mass = 86 g/mol)
B) CH3CH2CH2CH2CH2OH (molar mass = 88 g/mol)
C) CH3CH2CH2CH2CH2CH3 (molar mass = 86 g/mol)
D) HOH2C−CH=CH−CH2OH (molar mass = 88 g/mol)
QUESTION
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Vapor Pressure on the Molecular Level
Vapor Pressure
Would water have a higher or lower vapor pressure @ the same temperature? (bp H2O > CH3CH2OH;
bp = oC when Vapor Pressure = Atmospheric Pressure)
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Explaining Vapor Pressure on a Molecular Level
Vapor Pressure
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Volatility, Vapor Pressure, and Temperature
Vapor Pressure
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QUESTION
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Temperature & Vapor Pressure• The boiling point (b.p.) of
a pure liquid is the temperature at which the vapor pressure above the liquid equals the external pressure.
• Could water boil @ 0oC?
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Temperature Dependence of Vapor Pressures
• The vapor pressure above the liquid varies exponentially with changes in the temperature.
• The Clausius-Clapeyron equation shows how the vapor pressure and temperature are related.
€
lnP = −ΔHvap
R×
1
T+ C (R = 8.314 J K−1 mol−1)
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Clausius – Clapeyron Equation
• A straight line plot results when ln P vs. 1/T is plotted and has a slope of Hvap/R.
• Clausius – Clapeyron equation is true for any two pairs of points.
€
lnP2
P1
=ΔHvap
R×
1
T1
−1
T2
⎛
⎝ ⎜
⎞
⎠ ⎟
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QUESTION
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Heating Curve
http://chemconnections.org/general/movies/HeatingCurves.swf
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Energy (Heat) and Phase Changes
• Heat of vaporization: heat needed for the vaporization of a liquid.
H2O(l) H2O(g) DH = 40.7 kJ/mol
• Heat of fusion: heat needed for the melting of a solid.
H2O(s) H2O(l) DH = 6.01 kJ/mol
• Temperature does not change during the change from one phase to another.
50.0 g of H2O(s) and 50.0 g of H2O(l) were mixed together at 0°C. Determine the heat required to heat this mixture to 100.0°C and evaporate half of the water.