Chapter 11 Intermolecular Forces, Liquids, and Solids liquids... · 28/04/2015 · INTERMOLECULAR...
Transcript of Chapter 11 Intermolecular Forces, Liquids, and Solids liquids... · 28/04/2015 · INTERMOLECULAR...
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Intermolecular Forces
Chapter 11 Intermolecular Forces,
Liquids, and Solids John D. Bookstaver
St. Charles Community College St. Peters, MO
© 2006, Prentice Hall, Inc.
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.;
and Bruce E. Bursten
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Intermolecular Forces
Intermolecular Forces Affect Many Physical Properties
The strength of the attractions between particles can greatly affect the properties of a substance or solution.
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Intermolecular Forces
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Intermolecular Forces
Viscosity • Resistance of a
liquid to flow Ø related to the ease
with which molecules can move past each other.
Ø increases with stronger intermolecular forces and decreases with higher temperature.
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Intermolecular Forces
Surface Tension
• results from the net inward force experienced by the molecules on the surface of a liquid.
• Stronger IM forces = more surface tension
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Intermolecular Forces
Vapor Pressure • At any temperature, some molecules in a
liquid have enough energy to escape. • As the temperature rises, the fraction of
molecules that have enough energy to escape increases.
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Intermolecular Forces
Vapor Pressure
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Intermolecular Forces
Vapor Pressure • When a liquid is first
placed in an empty closed container none of the substance exists as a gas
• As more molecules escape the liquid, the pressure they exert increases.
• liquid and vapor reach a state of dynamic equilibrium: liquid molecules evaporate and vapor molecules condense at the same rate.
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Intermolecular Forces
Vapor Pressure • The boiling point of a
liquid is the temp. at where its vapor pressure equals atmospheric pressure.
• The normal boiling point is the temperature at which its vapor pressure is 760 torr which is air pressure at sea level.
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Intermolecular Forces
The States of Matter The state a substance is in at a particular
temp and pressure depends on the kinetic energy of the particles.
What determines the KE? 1. The temperature (higher temp = more KE
= less condensed phase), 2. The strength of the attractions between
the particles (more attraction = less KE = more condensed phase) THINK INTERMOLECULAR FORCES!!!!
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Intermolecular Forces
The States of Matter The state a substance is in at a particular
temp and pressure depends on the kinetic energy of the particles.
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Intermolecular Forces
States of Matter • Differ in terms distance between particles
Ø causes the differences in properties we observe
• solid and liquid states are condensed phases Table 11.1
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Intermolecular Forces
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Intermolecular Forces
Phase Changes
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Intermolecular Forces
Energy in Phase Changes
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Intermolecular Forces
Energy in Phase Changes • The heat added to the system at the melting and boiling
points goes into pulling the molecules farther apart from each other (= heat of fusion ΔHfus for melting and heat of vaporization ΔHvap for boiling.
• The temperature of the substance does not rise during the phase change.
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Intermolecular Forces
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Intermolecular Forces
Energy Changes Associated with Changes of State
• Heat of Fusion: Energy required to change a solid at its melting point to a liquid.
• Heat of Vaporization: Energy required to change a liquid at its boiling point to a gas.
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Intermolecular Forces
Types of Bonding in Crystalline Solids
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Intermolecular Forces
Solids
• We can think of solids as falling into two groups:
Ø Crystalline—particles are in highly ordered arrangement.
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Intermolecular Forces
Solids
Ø Amorphous—no particular order in the arrangement of particles.
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Intermolecular Forces
Attractions in Ionic Crystals In ionic crystals, ions pack themselves so as to maximize the attractions and minimize repulsions between the ions.
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Intermolecular Forces
Crystalline Solids
There are several types of basic arrangements in crystals, such as the ones shown above.
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Intermolecular Forces
Covalent-Network and Molecular Solids
• Diamonds are an example of a covalent-network solid in which atoms are covalently bonded to each other. Ø They tend to be hard and have high melting
points.
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Intermolecular Forces
Covalent-Network and Molecular Solids
• Graphite is an example of a molecular solid in which atoms are held together with van der Waals forces. Ø They tend to be softer and have lower melting
points.
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Intermolecular Forces
Metallic Solids • Metals are not
covalently bonded, but the attractions between atoms are too strong to be van der Waals forces.
• In metals, valence electrons are delocalized throughout the solid.