intermolecular forces and physical...
TRANSCRIPT
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Intermolecular Forcesand
Physical Properties
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Attractive Forces
Particles are attracted to each other by electrostatic forces
The strength of the attractive forces depends on the kind(s) of particles
The stronger the attractive forces between the particles, the more they resist moving
The strength of the attractions between particles of a substance determines its physical state.
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Kinds of Attractive Forces
Hydrogen Bonds An especially strong dipole–dipole attraction
resulting from the attachment of H to an extremely electronegative atom
Dispersion Forces Polarity in molecules due to temporary
unequal electron distribution
Dipole–Dipole Attractions Permanent polarity in molecules due to
their structure
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Some molecules are considered nonpolar because of the atoms which they contain and the
arrangement of these atoms in space.
CH4 BH3 C2H2 CO2
Nonpolarizedelectronclouds
But these molecules can all be “condensed.”
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Origin of Instantaneous Dipoles
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Size of the Induced Dipole
The magnitude of the induced dipole depends on several factors:
Polarizability of the electrons
Volume of the electron cloud
larger molecules have more electrons, leading to
increased polarizability
+ + + + + +
+ + +
+ + + +
+
− − − − − − − − − − −
− −
+ +
+ + + +
+
- -
- - - -
-
larger molar mass ⇒ more electrons ⇒ larger electron cloud ⇒ increased polarizability ⇒ stronger attractions
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Size of the Induced DipoleShape of the molecule
more surface-to-surface contact ⇒ larger induced dipole
⇒ stronger attraction
+ +
+ + + +
+
- -
- - - -
-
molecules that are flat have more
surface interaction than spherical
ones
+
+ + +
+
-
- - -
-
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Effect of Molecular Sizeon Magnitude of Dispersion Force
As the molar mass increases,
the number of electrons increases. Therefore the
strength of the dispersion forces increases.
The stronger the
attractive forces
between the molecules, the higher
the boiling point will be.
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Boiling Points of Straight Chain AlkanesNonPolar Molecules
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Effect of Molecular Shapeon Size of Dispersion Force
the larger surface-to-surface
contact between molecules in n-pentane
results in stronger dispersion force
attractions
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Some molecules are inherently polar because of the atoms which they contain and the
arrangement of these atoms in space.
H2O NH3 CH2O HCl
δ− δ+ A crude representation of a polar molecule
Dipole–Dipole Attractions
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Dipole–Dipole Attractions
Polar molecules have a permanent dipole because of bond polarity and shape
1) dipole moment 2) as well as the always present induced dipole
The permanent dipole adds to the attractive forces between the molecules
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Effect of Dipole–Dipole Attraction on Boiling and Melting Points
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Hydrogen Bonding
When a very electronegative atom is bonded to hydrogen, it strongly pulls the bonding electrons toward it:
O─H, N─H, F─H
Because hydrogen has no other electrons, when its electron is pulled away, the nucleus becomes deshielded, exposing the H proton.
The exposed proton acts as a very strong center of positive charge.
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H-Bonding in Water
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Hydrogen bonding and boiling point.
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Effect of H-Bonding on Boiling Point
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One of these compounds is a liquid at room temperature (the others are gases). Which one and why?
MM = 30.03PolarNo H-Bonds
MM = 34.03PolarNo H-Bonds
MM = 34.02PolarH-Bonds
Because only hydrogen peroxide has the additional very strong H-bond additional attractions, its intermolecular attractions will be the strongest. We therefore expect hydrogen peroxide to be the liquid.
-19ºC -78ºC +150ºC
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All Molecules
Polar Molecules
Molecules containing O-H, N-H, or F-H
Bonds
Dispersion forces
Dipole forces
H-bonding
Hierarchy of Intermolecular Forces
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Boiling Points of Other Organic “Families”
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Solubility
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SolubilityWhen one substance (solute) dissolves in another (solvent) it is said to be soluble.
When one substance does not dissolve in another it is said to be insoluble.
The solubility of one substance in another depends on two factors - nature’s tendency toward mixing, and the potential intermolecular attractive forces between solute and solvent.
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Attractive Forces Acting Between Ions & Molecules
δ−δ+ δ−δ+ δ−δ+
δ−δ+ δ−δ+ δ−δ+ δ−δ+
δ−δ+
Dispersion Forces Very weak, due to a temporary shift in electron distributiondependent on the size of the molecule
Dipole-dipole attractions - chiefly between molecules
Pure Electrostatic Attractions - chiefly ionic compounds
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What happens when you dissolve an ionic compound in water??
What happens when you dissolve a polar molecule in water??
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What Happens When an Ionic Compound Dissolves in Water?
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dipole-dipole attractions
What Happens When a Polar Covalent Compound Dissolves in Water?
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What happens when you try to dissolve a nonpolar molecule in water??
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What happens when you try to dissolve a nonpolar molecule in water??
Non polar solvents, such as ethanol, carbon tetrachloride, ether, and hexane, are also commonly used to dissolve nonpolar solutes, such as grease and oils.
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General Solubility Rule: “Like Dissolves Like”
Polar solutes form solutions with polar solvents.
Nonpolar solutes form solutions with nonpolar solvents.
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Selected Polar and Nonpolar Solvents
! ! POLAR SOLVENTS NONPOLAR SOLVENTS water, H2O hexane, C6H14
methanol, CH3OH heptane, C7H16
ethanol, C2H5OH toluene, C7H8
acetone, C3H6O carbon tetrachloride, CCl4
methyl ethyl ketone, CH3CH2C(O)CH3 chloroform, CHCl3
formic acid, HCOOH methylene chloride, CH2Cl2
acetic acid, CH3COOH ethyl ether, CH3CH2OCH2CH3
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Solubility* of a Series of Alcohols in Water and Hexane