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3/8/2020
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CHAPTER 6
Intermolecular Forces Attractions between Particles
Scientists are interested in how matter behaves under unusual
circumstances. For example, before the space station could
be built, fundamental research into materials properties had to
be undertaken.
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Solids and Liquids
Intermolecular Forces
Ion-ion, Ion-dipole, dipole-dipole and H-
bonding, dipole-induced dipole, induced
dipole-induced dipole
Liquids
Vapor pressure and
temperature, Critical
T & P, Surface
tension and
viscosity
Phase Diagrams
Show relation of solid,
liquid, and gas phases
with change in T and
P
Solids
Unit cells, metal
structures, formulas
and structures of ionic
compounds,
Molecular, network,
and amorphous solids
Properties of Solids
Lattice energy, heat of
fusion, melting point
Summary of Intermolecular Forces
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Chapter Outline
▪ 6.1 London Dispersion Forces: They’re Everywhere▪ Nonpolar molecules – polarizability and temporary dipoles
▪ 6.2 Interactions Involving Polar Molecules▪ Polar molecules – ion-dipole, dipole-dipole, hydrogen bonds
▪ 6.3 Trends in Solubility
▪ 6.4 Phase Diagrams: Intermolecular Forces at Work
▪ 6.5 Some Remarkable Properties of Water
AlkanesWhy do increasing lengths increase the boiling point?
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London Dispersion Forces
“Temporary Dipoles”
▪ Even nonpolar molecules and
uncombined atoms have attractive
forces between them, otherwise
they would never condense or
solidify.
▪ Similar to a covalent bond, the
electron of an atom in one
molecule is attracted to the
nucleus of an atom in the adjacent
molecule and visa-versa
▪ This creates “temporary dipoles” or
London Dispersion Forces (named
after the physicist Fritz London)
Polarizability - a measure of the extent to which the
electron cloud of an atom or molecule can be
distorted by an external electric charge.
• In general, larger atoms
or molecules are more
easily polarizable than
smaller ones (more shells,
etc), and so experience
larger London forces
• Sometimes London forces
are called “induced dipole-
induced dipole”
London Dispersion Forces
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Effect of Increasing Polarizability and Increasing
Molecular Mass on Physical Properties
Combined together, these explain why boiling points of
nonpolar molecules like alkanes increase with size.
Explains the trends in boiling points for the
Noble Gases and the halogens.
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The Importance of Shape – Branched AlkanesWhich alkane has greater attractive intermolecular forces ?
• These molecules all have the same chemical formulas,
C5H12 ,but different shapes. These are known as “isomers”.
• The boiling points decrease as the isomers become more
branched.
The Importance of Shape – Branched AlkanesWhich alkane has greater attractive intermolecular forces ?
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Viscosity: the measure of a fluid’s
resistance to flow
http://www.reologie.ro/an-introduction-to-
rheology-and-viscosity/
Viscosities of some liquid alkanes
hexane
octane
decane
Molar
Mass
(g/mol)
Viscosity
@ 20oC
(cP)
86 0.29
114 0.54
142 0.92
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Chapter Outline
▪ 6.1 London Dispersion Forces: They’re Everywhere▪ Nonpolar molecules – polarizability and temporary dipoles
▪ 6.2 Interactions Involving Polar Molecules▪ Polar molecules – dipole-dipole and hydrogen bonds, ion-dipole
▪ 6.3 Trends in Solubility
▪ 6.4 Phase Diagrams: Intermolecular Forces at Work
▪ 6.5 Some Remarkable Properties of Water
Dipole-Dipole InteractionsAttractive forces between the dipoles of polar molecules.
Acetic acid
CH3COOH
-
+
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• Very strong type of dipole-dipole interactions
• Requires H atom covalently bonded to the very
electronegative atoms O, N, or F
Hydrogen Bonds
H2O NH3 HF
Boiling Points of Binary Hydrides
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adenine thymine
white = hydrogen
blue = nitrogen
black = carbon
red = oxygen
The Double Helix of DNA is held together
by hydrogen bonding
The polymer Nylon is also held together
by hydrogen bonding
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Interactions Involving Polar Molecules
▪ Ion-Dipole:
• Interaction between an ion and the partial
charge of a molecule with a permanent dipole.
▪ Sphere of Hydration:
• Cluster of water molecules surrounding an ion
as it dissolves in aqueous solution.
• Sphere of solvation if solvent other than H2O.
Ion-Dipole Interactions
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Ion-Dipole Interactions:
Sphere of Hydration
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