Chapter 10
Liquids and Solids
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10.1 Intermolecular Forces
• Intermolecular forces – attractive
forces between two molecules
• Intramolecular – within a
molecule
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Dipole-Dipole Forces
• Attractive forces between two
polar molecules
• Opposite charges will pull towards
each other
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Hydrogen Bonding
• NOT an actual bond
• An extreme form of dipole-dipole
• H must be bonded to an F, O, or N
• H is attracted to another F, O, or N
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London Dispersion
• An instantaneous polarization that
creates a very weak dipole moment
• Can induce a “domino effect” in
surrounding
molecules
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Dipole-Induced Dipole
• A polar molecule induces a dipole
moment in a non-polar molecule
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IMF strengths
IMF
H bonding
Dipole-dipole
Dipole-induced
London Dispersion
Energy (kJ/mol)
10-40
5-25
2-10
0.05-40
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IMF affects…
• State of matter
• Boiling points/Melting points
• Solubility
• Reactions Rates
• Surface tension/Capillary action
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10.2 Liquid State
• Surface tension – resistance of a
liquid to an increase in its surface
area
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10.2 Liquid State
• Capillary action – spontaneous rising
of a liquid in a narrow tube
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10.2 Liquid State
• Viscosity – a measure of a liquid’s
resistance to flow
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10.3 An Introduction to
Structures and Types of
Solids
• Crystalline – highly regular
arrangement
• Amorphous – considerable
disorder
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Crystal Structures
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Types of Crystalline Solids
• Ionic solids – made of ionic compounds
• Molecular solids – made of molecules
• Atomic solids – made of atoms
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10.4 Structure & Bonding in
Metals
• Alloy – contains mix of elements &
has metallic properties
• Substitutional alloy – some metal
atoms replaced by other metal
atoms
• Interstitial alloy – atoms go in holes
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10.5 Carbon & Silicon:
Network Atomic Solids
• Network solids – contain strong
directional covalent bonds
• Carbon
• Graphite
• Diamond
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Network Solids
• Silicon
• Silica – SiO2
• Silicates – compounds closely related
to silica, found in most rocks, soils,
and clay
• Glass – amorphous solid formed when
silica is heated & cooled rapidly
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Semiconductors
• Electrons can jump from the
empty molecular orbitals in silicon
but not in carbon
• Carbon is an insulator
• Silicon is a semiconductor
• Can increase conductivity by
“doping”
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Doping Semiconductors
• Doping – adding alternate
atoms
• n-type semiconductor –
adding another element
with more valence
electrons
• p-type semiconductor –
adding another element
with less valence electrons
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10.6 Molecular Solids
• Ice, CO2, I2, P4, S8
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10.7 Ionic Solids
• They form 3D crystalline lattice
structures
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10.8 Vapor Pressure & Changes
of State
• Vapor pressure
• Clausius-Clapeyron Equation
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Lab Calculations
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10.8 Vapor Pressure & Changes
of State
• Phase changes
• Vaporization/evaporization
• Condensation
• Sublimation
• Melting (fusion)
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Heating Curve
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10.9 Phase Diagrams
Review
on your
own
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